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href="#Isotopes"> <div class="vector-toc-text"> 2.1 Isotopes </div> </a> <ul id="toc-Isotopes-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Chemistry_and_compounds" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Chemistry_and_compounds"> <div class="vector-toc-text"> 3 Chemistry and compounds </div> </a> <button aria-controls="toc-Chemistry_and_compounds-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Chemistry and compounds subsection </button> <ul id="toc-Chemistry_and_compounds-sublist" class="vector-toc-list"> <li id="toc-Hydrogen_chloride" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Hydrogen_chloride"> <div class="vector-toc-text"> 3.1 Hydrogen chloride </div> </a> <ul id="toc-Hydrogen_chloride-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Other_binary_chlorides" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Other_binary_chlorides"> <div class="vector-toc-text"> 3.2 Other binary chlorides </div> </a> <ul id="toc-Other_binary_chlorides-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Polychlorine_compounds" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Polychlorine_compounds"> <div class="vector-toc-text"> 3.3 Polychlorine compounds </div> </a> <ul id="toc-Polychlorine_compounds-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Chlorine_fluorides" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Chlorine_fluorides"> <div class="vector-toc-text"> 3.4 Chlorine fluorides </div> </a> <ul id="toc-Chlorine_fluorides-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Chlorine_oxides" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Chlorine_oxides"> <div class="vector-toc-text"> 3.5 Chlorine oxides </div> </a> <ul id="toc-Chlorine_oxides-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Chlorine_oxoacids_and_oxyanions" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Chlorine_oxoacids_and_oxyanions"> <div class="vector-toc-text"> 3.6 Chlorine oxoacids and oxyanions </div> </a> <ul id="toc-Chlorine_oxoacids_and_oxyanions-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Organochlorine_compounds" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Organochlorine_compounds"> <div class="vector-toc-text"> 3.7 Organochlorine compounds </div> </a> <ul id="toc-Organochlorine_compounds-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Occurrence" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Occurrence"> <div class="vector-toc-text"> 4 Occurrence </div> </a> <ul id="toc-Occurrence-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Production" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Production"> <div class="vector-toc-text"> 5 Production </div> </a> <button aria-controls="toc-Production-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Production subsection </button> <ul id="toc-Production-sublist" class="vector-toc-list"> <li id="toc-Chloralkali_processes" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Chloralkali_processes"> <div class="vector-toc-text"> 5.1 Chloralkali processes </div> </a> <ul id="toc-Chloralkali_processes-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Non-chloralkali_processes" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Non-chloralkali_processes"> <div class="vector-toc-text"> 5.2 Non-chloralkali processes </div> </a> <ul id="toc-Non-chloralkali_processes-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Applications" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Applications"> <div class="vector-toc-text"> 6 Applications </div> </a> <button aria-controls="toc-Applications-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Applications subsection </button> <ul id="toc-Applications-sublist" class="vector-toc-list"> <li id="toc-Sanitation,_disinfection,_and_antisepsis" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Sanitation,_disinfection,_and_antisepsis"> <div class="vector-toc-text"> 6.1 Sanitation, disinfection, and antisepsis </div> </a> <ul id="toc-Sanitation,_disinfection,_and_antisepsis-sublist" class="vector-toc-list"> <li id="toc-Combating_putrefaction" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Combating_putrefaction"> <div class="vector-toc-text"> 6.1.1 Combating putrefaction </div> </a> <ul id="toc-Combating_putrefaction-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Disinfection" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Disinfection"> <div class="vector-toc-text"> 6.1.2 Disinfection </div> </a> <ul id="toc-Disinfection-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Semmelweis_and_experiments_with_antisepsis" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Semmelweis_and_experiments_with_antisepsis"> <div class="vector-toc-text"> 6.1.3 Semmelweis and experiments with antisepsis </div> </a> <ul id="toc-Semmelweis_and_experiments_with_antisepsis-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Public_sanitation" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Public_sanitation"> <div class="vector-toc-text"> 6.1.4 Public sanitation </div> </a> <ul id="toc-Public_sanitation-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Use_as_a_weapon" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Use_as_a_weapon"> <div class="vector-toc-text"> 6.2 Use as a weapon </div> </a> <ul id="toc-Use_as_a_weapon-sublist" class="vector-toc-list"> <li id="toc-World_War_I" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#World_War_I"> <div class="vector-toc-text"> 6.2.1 World War I </div> </a> <ul id="toc-World_War_I-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Middle_east" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Middle_east"> <div class="vector-toc-text"> 6.2.2 Middle east </div> </a> <ul id="toc-Middle_east-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> </ul> </li> <li id="toc-Biological_role" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Biological_role"> <div class="vector-toc-text"> 7 Biological role </div> </a> <ul id="toc-Biological_role-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Hazards" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Hazards"> <div class="vector-toc-text"> 8 Hazards </div> </a> <button aria-controls="toc-Hazards-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Hazards subsection </button> <ul id="toc-Hazards-sublist" class="vector-toc-list"> <li id="toc-Chlorine-induced_cracking_in_structural_materials" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Chlorine-induced_cracking_in_structural_materials"> <div class="vector-toc-text"> 8.1 Chlorine-induced cracking in structural materials </div> </a> <ul id="toc-Chlorine-induced_cracking_in_structural_materials-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Chlorine-iron_fire" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Chlorine-iron_fire"> <div class="vector-toc-text"> 8.2 Chlorine-iron fire </div> </a> <ul id="toc-Chlorine-iron_fire-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-See_also" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#See_also"> <div class="vector-toc-text"> 9 See also </div> </a> <ul id="toc-See_also-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Notes" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Notes"> <div class="vector-toc-text"> 10 Notes </div> </a> <ul id="toc-Notes-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-References" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#References"> <div class="vector-toc-text"> 11 References </div> </a> <button aria-controls="toc-References-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle References subsection </button> <ul id="toc-References-sublist" class="vector-toc-list"> <li id="toc-Bibliography" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Bibliography"> <div class="vector-toc-text"> 11.1 Bibliography </div> </a> <ul id="toc-Bibliography-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-External_links" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#External_links"> <div class="vector-toc-text"> 12 External links </div> </a> <ul id="toc-External_links-sublist" class="vector-toc-list"> </ul> </li> </ul> </div> </div> </nav> </div> </div> <div class="mw-content-container"> <main id="content" class="mw-body"> <header class="mw-body-header vector-page-titlebar"> <nav aria-label="Contents" class="vector-toc-landmark"> <div id="vector-page-titlebar-toc" class="vector-dropdown vector-page-titlebar-toc vector-button-flush-left" title="Table of Contents" > <input type="checkbox" id="vector-page-titlebar-toc-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-vector-page-titlebar-toc" class="vector-dropdown-checkbox " aria-label="Toggle the table of contents" > <label id="vector-page-titlebar-toc-label" for="vector-page-titlebar-toc-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--icon-only " aria-hidden="true" > Toggle the table of contents </label> <div class="vector-dropdown-content"> <div id="vector-page-titlebar-toc-unpinned-container" class="vector-unpinned-container"> </div> </div> </div> </nav> <h1 id="firstHeading" class="firstHeading mw-first-heading">Chlorine</h1> <div id="p-lang-btn" class="vector-dropdown mw-portlet mw-portlet-lang" > <input type="checkbox" id="p-lang-btn-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-p-lang-btn" class="vector-dropdown-checkbox mw-interlanguage-selector" aria-label="Go to an article in another language. Available in 165 languages" > <label id="p-lang-btn-label" for="p-lang-btn-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--action-progressive mw-portlet-lang-heading-165" aria-hidden="true" > 165 languages </label> <div class="vector-dropdown-content"> <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li class="interlanguage-link interwiki-af mw-list-item"><a href="https://af.wikipedia.org/wiki/Chloor" title="Chloor – Afrikaans" lang="af" hreflang="af" data-title="Chloor" data-language-autonym="Afrikaans" data-language-local-name="Afrikaans" class="interlanguage-link-target">Afrikaans</a></li><li class="interlanguage-link interwiki-am mw-list-item"><a href="https://am.wikipedia.org/wiki/%E1%8A%AD%E1%88%8E%E1%88%AA%E1%8A%95" title="ክሎሪን – Amharic" lang="am" hreflang="am" data-title="ክሎሪን" data-language-autonym="አማርኛ" data-language-local-name="Amharic" class="interlanguage-link-target">አማርኛ</a></li><li class="interlanguage-link interwiki-anp mw-list-item"><a href="https://anp.wikipedia.org/wiki/%E0%A4%95%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A5%80%E0%A4%A8" title="क्लोरीन – Angika" lang="anp" hreflang="anp" data-title="क्लोरीन" data-language-autonym="अंगिका" data-language-local-name="Angika" class="interlanguage-link-target">अंगिका</a></li><li class="interlanguage-link interwiki-ar badge-Q17437798 badge-goodarticle mw-list-item" title="good article badge"><a href="https://ar.wikipedia.org/wiki/%D9%83%D9%84%D9%88%D8%B1" title="كلور – Arabic" lang="ar" hreflang="ar" data-title="كلور" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target">العربية</a></li><li class="interlanguage-link interwiki-an mw-list-item"><a href="https://an.wikipedia.org/wiki/Cloro" title="Cloro – Aragonese" lang="an" hreflang="an" data-title="Cloro" data-language-autonym="Aragonés" data-language-local-name="Aragonese" class="interlanguage-link-target">Aragonés</a></li><li class="interlanguage-link interwiki-hyw mw-list-item"><a href="https://hyw.wikipedia.org/wiki/%D5%94%D5%AC%D5%B8%D6%80" title="Քլոր – Western Armenian" lang="hyw" hreflang="hyw" data-title="Քլոր" data-language-autonym="Արեւմտահայերէն" data-language-local-name="Western Armenian" class="interlanguage-link-target">Արեւմտահայերէն</a></li><li class="interlanguage-link interwiki-roa-rup mw-list-item"><a href="https://roa-rup.wikipedia.org/wiki/Cloru" title="Cloru – Aromanian" lang="rup" hreflang="rup" data-title="Cloru" data-language-autonym="Armãneashti" data-language-local-name="Aromanian" class="interlanguage-link-target">Armãneashti</a></li><li class="interlanguage-link interwiki-ast mw-list-item"><a href="https://ast.wikipedia.org/wiki/Cloru" title="Cloru – Asturian" lang="ast" hreflang="ast" data-title="Cloru" data-language-autonym="Asturianu" data-language-local-name="Asturian" class="interlanguage-link-target">Asturianu</a></li><li class="interlanguage-link interwiki-az mw-list-item"><a href="https://az.wikipedia.org/wiki/Xlor" title="Xlor – Azerbaijani" lang="az" hreflang="az" data-title="Xlor" data-language-autonym="Azərbaycanca" data-language-local-name="Azerbaijani" class="interlanguage-link-target">Azərbaycanca</a></li><li class="interlanguage-link interwiki-azb mw-list-item"><a href="https://azb.wikipedia.org/wiki/%DA%A9%D9%88%D9%84%D9%88%D8%B1" title="کولور – South Azerbaijani" lang="azb" hreflang="azb" data-title="کولور" data-language-autonym="تۆرکجه" data-language-local-name="South Azerbaijani" class="interlanguage-link-target">تۆرکجه</a></li><li class="interlanguage-link interwiki-ban mw-list-item"><a href="https://ban.wikipedia.org/wiki/Klorin" title="Klorin – Balinese" lang="ban" hreflang="ban" data-title="Klorin" data-language-autonym="Basa Bali" data-language-local-name="Balinese" class="interlanguage-link-target">Basa Bali</a></li><li class="interlanguage-link interwiki-bn mw-list-item"><a href="https://bn.wikipedia.org/wiki/%E0%A6%95%E0%A7%8D%E0%A6%B2%E0%A7%8B%E0%A6%B0%E0%A6%BF%E0%A6%A8" title="ক্লোরিন – Bangla" lang="bn" hreflang="bn" data-title="ক্লোরিন" data-language-autonym="বাংলা" data-language-local-name="Bangla" class="interlanguage-link-target">বাংলা</a></li><li class="interlanguage-link interwiki-zh-min-nan mw-list-item"><a href="https://zh-min-nan.wikipedia.org/wiki/I%C3%A2m-s%C3%B2%CD%98" title="Iâm-sò͘ – Minnan" lang="nan" hreflang="nan" data-title="Iâm-sò͘" data-language-autonym="閩南語 / Bân-lâm-gú" data-language-local-name="Minnan" class="interlanguage-link-target">閩南語 / Bân-lâm-gú</a></li><li class="interlanguage-link interwiki-ba mw-list-item"><a href="https://ba.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Bashkir" lang="ba" hreflang="ba" data-title="Хлор" data-language-autonym="Башҡортса" data-language-local-name="Bashkir" class="interlanguage-link-target">Башҡортса</a></li><li class="interlanguage-link interwiki-be mw-list-item"><a href="https://be.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Belarusian" lang="be" hreflang="be" data-title="Хлор" data-language-autonym="Беларуская" data-language-local-name="Belarusian" class="interlanguage-link-target">Беларуская</a></li><li class="interlanguage-link interwiki-be-x-old mw-list-item"><a href="https://be-tarask.wikipedia.org/wiki/%D0%A5%D0%BB%D1%91%D1%80" title="Хлёр – Belarusian (Taraškievica orthography)" lang="be-tarask" hreflang="be-tarask" data-title="Хлёр" data-language-autonym="Беларуская (тарашкевіца)" data-language-local-name="Belarusian (Taraškievica orthography)" class="interlanguage-link-target">Беларуская (тарашкевіца)</a></li><li class="interlanguage-link interwiki-bh mw-list-item"><a href="https://bh.wikipedia.org/wiki/%E0%A4%95%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A5%80%E0%A4%A8" title="क्लोरीन – Bhojpuri" lang="bh" hreflang="bh" data-title="क्लोरीन" data-language-autonym="भोजपुरी" data-language-local-name="Bhojpuri" class="interlanguage-link-target">भोजपुरी</a></li><li class="interlanguage-link interwiki-bcl mw-list-item"><a href="https://bcl.wikipedia.org/wiki/Klorina" title="Klorina – Central Bikol" lang="bcl" hreflang="bcl" data-title="Klorina" data-language-autonym="Bikol Central" data-language-local-name="Central Bikol" class="interlanguage-link-target">Bikol Central</a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Bulgarian" lang="bg" hreflang="bg" data-title="Хлор" data-language-autonym="Български" data-language-local-name="Bulgarian" class="interlanguage-link-target">Български</a></li><li class="interlanguage-link interwiki-bo mw-list-item"><a href="https://bo.wikipedia.org/wiki/%E0%BD%9A%E0%BE%AD%E0%BC%8B%E0%BD%A2%E0%BE%B3%E0%BD%B4%E0%BD%84%E0%BC%8B%E0%BC%8D" title="ཚྭ་རླུང་། – Tibetan" lang="bo" hreflang="bo" data-title="ཚྭ་རླུང་།" data-language-autonym="བོད་ཡིག" data-language-local-name="Tibetan" class="interlanguage-link-target">བོད་ཡིག</a></li><li class="interlanguage-link interwiki-bs mw-list-item"><a href="https://bs.wikipedia.org/wiki/Hlor" title="Hlor – Bosnian" lang="bs" hreflang="bs" data-title="Hlor" data-language-autonym="Bosanski" data-language-local-name="Bosnian" class="interlanguage-link-target">Bosanski</a></li><li class="interlanguage-link interwiki-br mw-list-item"><a href="https://br.wikipedia.org/wiki/Klor" title="Klor – Breton" lang="br" hreflang="br" data-title="Klor" data-language-autonym="Brezhoneg" data-language-local-name="Breton" class="interlanguage-link-target">Brezhoneg</a></li><li class="interlanguage-link interwiki-ca mw-list-item"><a href="https://ca.wikipedia.org/wiki/Clor" title="Clor – Catalan" lang="ca" hreflang="ca" data-title="Clor" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target">Català</a></li><li class="interlanguage-link interwiki-cv mw-list-item"><a href="https://cv.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Chuvash" lang="cv" hreflang="cv" data-title="Хлор" data-language-autonym="Чӑвашла" data-language-local-name="Chuvash" class="interlanguage-link-target">Чӑвашла</a></li><li class="interlanguage-link interwiki-ceb mw-list-item"><a href="https://ceb.wikipedia.org/wiki/Klorin" title="Klorin – Cebuano" lang="ceb" hreflang="ceb" data-title="Klorin" data-language-autonym="Cebuano" data-language-local-name="Cebuano" class="interlanguage-link-target">Cebuano</a></li><li class="interlanguage-link interwiki-cs mw-list-item"><a href="https://cs.wikipedia.org/wiki/Chlor" title="Chlor – Czech" lang="cs" hreflang="cs" data-title="Chlor" data-language-autonym="Čeština" data-language-local-name="Czech" class="interlanguage-link-target">Čeština</a></li><li class="interlanguage-link interwiki-co mw-list-item"><a href="https://co.wikipedia.org/wiki/Cloru" title="Cloru – Corsican" lang="co" hreflang="co" data-title="Cloru" data-language-autonym="Corsu" data-language-local-name="Corsican" class="interlanguage-link-target">Corsu</a></li><li class="interlanguage-link interwiki-cy mw-list-item"><a href="https://cy.wikipedia.org/wiki/Clorin" title="Clorin – Welsh" lang="cy" hreflang="cy" data-title="Clorin" data-language-autonym="Cymraeg" data-language-local-name="Welsh" class="interlanguage-link-target">Cymraeg</a></li><li class="interlanguage-link interwiki-da mw-list-item"><a href="https://da.wikipedia.org/wiki/Klor" title="Klor – Danish" lang="da" hreflang="da" data-title="Klor" data-language-autonym="Dansk" data-language-local-name="Danish" class="interlanguage-link-target">Dansk</a></li><li class="interlanguage-link interwiki-ary mw-list-item"><a href="https://ary.wikipedia.org/wiki/%D9%83%D9%84%D9%88%D8%B1" title="كلور – Moroccan Arabic" lang="ary" hreflang="ary" data-title="كلور" data-language-autonym="الدارجة" data-language-local-name="Moroccan Arabic" class="interlanguage-link-target">الدارجة</a></li><li class="interlanguage-link interwiki-de badge-Q17437798 badge-goodarticle mw-list-item" title="good article badge"><a href="https://de.wikipedia.org/wiki/Chlor" title="Chlor – German" lang="de" hreflang="de" data-title="Chlor" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target">Deutsch</a></li><li class="interlanguage-link interwiki-dv mw-list-item"><a href="https://dv.wikipedia.org/wiki/%DE%86%DE%B0%DE%8D%DE%AE%DE%83%DE%A8%DE%82%DE%B0" title="ކްލޮރިން – Divehi" lang="dv" hreflang="dv" data-title="ކްލޮރިން" data-language-autonym="ދިވެހިބަސް" data-language-local-name="Divehi" class="interlanguage-link-target">ދިވެހިބަސް</a></li><li class="interlanguage-link interwiki-et mw-list-item"><a href="https://et.wikipedia.org/wiki/Kloor" title="Kloor – Estonian" lang="et" hreflang="et" data-title="Kloor" data-language-autonym="Eesti" data-language-local-name="Estonian" class="interlanguage-link-target">Eesti</a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%A7%CE%BB%CF%8E%CF%81%CE%B9%CE%BF" title="Χλώριο – Greek" lang="el" hreflang="el" data-title="Χλώριο" data-language-autonym="Ελληνικά" data-language-local-name="Greek" class="interlanguage-link-target">Ελληνικά</a></li><li class="interlanguage-link interwiki-myv mw-list-item"><a href="https://myv.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Erzya" lang="myv" hreflang="myv" data-title="Хлор" data-language-autonym="Эрзянь" data-language-local-name="Erzya" class="interlanguage-link-target">Эрзянь</a></li><li class="interlanguage-link interwiki-es mw-list-item"><a href="https://es.wikipedia.org/wiki/Cloro" title="Cloro – Spanish" lang="es" hreflang="es" data-title="Cloro" data-language-autonym="Español" data-language-local-name="Spanish" class="interlanguage-link-target">Español</a></li><li class="interlanguage-link interwiki-eo mw-list-item"><a href="https://eo.wikipedia.org/wiki/Kloro" title="Kloro – Esperanto" lang="eo" hreflang="eo" data-title="Kloro" data-language-autonym="Esperanto" data-language-local-name="Esperanto" class="interlanguage-link-target">Esperanto</a></li><li class="interlanguage-link interwiki-ext mw-list-item"><a href="https://ext.wikipedia.org/wiki/Cloru" title="Cloru – Extremaduran" lang="ext" hreflang="ext" data-title="Cloru" data-language-autonym="Estremeñu" data-language-local-name="Extremaduran" class="interlanguage-link-target">Estremeñu</a></li><li class="interlanguage-link interwiki-eu mw-list-item"><a href="https://eu.wikipedia.org/wiki/Kloro" title="Kloro – Basque" lang="eu" hreflang="eu" data-title="Kloro" data-language-autonym="Euskara" data-language-local-name="Basque" class="interlanguage-link-target">Euskara</a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%DA%A9%D9%84%D8%B1" title="کلر – Persian" lang="fa" hreflang="fa" data-title="کلر" data-language-autonym="فارسی" data-language-local-name="Persian" class="interlanguage-link-target">فارسی</a></li><li class="interlanguage-link interwiki-hif mw-list-item"><a href="https://hif.wikipedia.org/wiki/Chlorine" title="Chlorine – Fiji Hindi" lang="hif" hreflang="hif" data-title="Chlorine" data-language-autonym="Fiji Hindi" data-language-local-name="Fiji Hindi" class="interlanguage-link-target">Fiji Hindi</a></li><li class="interlanguage-link interwiki-fo mw-list-item"><a href="https://fo.wikipedia.org/wiki/Klor" title="Klor – Faroese" lang="fo" hreflang="fo" data-title="Klor" data-language-autonym="Føroyskt" data-language-local-name="Faroese" class="interlanguage-link-target">Føroyskt</a></li><li class="interlanguage-link interwiki-fr mw-list-item"><a href="https://fr.wikipedia.org/wiki/Chlore" title="Chlore – French" lang="fr" hreflang="fr" data-title="Chlore" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target">Français</a></li><li class="interlanguage-link interwiki-fur mw-list-item"><a href="https://fur.wikipedia.org/wiki/Cl%C3%B4r" title="Clôr – Friulian" lang="fur" hreflang="fur" data-title="Clôr" data-language-autonym="Furlan" data-language-local-name="Friulian" class="interlanguage-link-target">Furlan</a></li><li class="interlanguage-link interwiki-ga mw-list-item"><a href="https://ga.wikipedia.org/wiki/Cl%C3%B3ir%C3%ADn" title="Clóirín – Irish" lang="ga" hreflang="ga" data-title="Clóirín" data-language-autonym="Gaeilge" data-language-local-name="Irish" class="interlanguage-link-target">Gaeilge</a></li><li class="interlanguage-link interwiki-gv mw-list-item"><a href="https://gv.wikipedia.org/wiki/Cloreen" title="Cloreen – Manx" lang="gv" hreflang="gv" data-title="Cloreen" data-language-autonym="Gaelg" data-language-local-name="Manx" class="interlanguage-link-target">Gaelg</a></li><li class="interlanguage-link interwiki-gd mw-list-item"><a href="https://gd.wikipedia.org/wiki/Cl%C3%B2rain" title="Clòrain – Scottish Gaelic" lang="gd" hreflang="gd" data-title="Clòrain" data-language-autonym="Gàidhlig" data-language-local-name="Scottish Gaelic" class="interlanguage-link-target">Gàidhlig</a></li><li class="interlanguage-link interwiki-gl mw-list-item"><a href="https://gl.wikipedia.org/wiki/Cloro" title="Cloro – Galician" lang="gl" hreflang="gl" data-title="Cloro" data-language-autonym="Galego" data-language-local-name="Galician" class="interlanguage-link-target">Galego</a></li><li class="interlanguage-link interwiki-gan mw-list-item"><a href="https://gan.wikipedia.org/wiki/%E6%B0%AF" title="氯 – Gan" lang="gan" hreflang="gan" data-title="氯" data-language-autonym="贛語" data-language-local-name="Gan" class="interlanguage-link-target">贛語</a></li><li class="interlanguage-link interwiki-gu mw-list-item"><a href="https://gu.wikipedia.org/wiki/%E0%AA%95%E0%AB%8D%E0%AA%B2%E0%AB%8B%E0%AA%B0%E0%AA%BF%E0%AA%A8" title="ક્લોરિન – Gujarati" lang="gu" hreflang="gu" data-title="ક્લોરિન" data-language-autonym="ગુજરાતી" data-language-local-name="Gujarati" class="interlanguage-link-target">ગુજરાતી</a></li><li class="interlanguage-link interwiki-hak mw-list-item"><a href="https://hak.wikipedia.org/wiki/Liu%CC%8Dk" title="Liu̍k – Hakka Chinese" lang="hak" hreflang="hak" data-title="Liu̍k" data-language-autonym="客家語 / Hak-kâ-ngî" data-language-local-name="Hakka Chinese" class="interlanguage-link-target">客家語 / Hak-kâ-ngî</a></li><li class="interlanguage-link interwiki-xal mw-list-item"><a href="https://xal.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Kalmyk" lang="xal" hreflang="xal" data-title="Хлор" data-language-autonym="Хальмг" data-language-local-name="Kalmyk" class="interlanguage-link-target">Хальмг</a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%EC%97%BC%EC%86%8C_(%EC%9B%90%EC%86%8C)" title="염소 (원소) – Korean" lang="ko" hreflang="ko" data-title="염소 (원소)" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target">한국어</a></li><li class="interlanguage-link interwiki-haw mw-list-item"><a href="https://haw.wikipedia.org/wiki/Kolorine" title="Kolorine – Hawaiian" lang="haw" hreflang="haw" data-title="Kolorine" data-language-autonym="Hawaiʻi" data-language-local-name="Hawaiian" class="interlanguage-link-target">Hawaiʻi</a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D5%94%D5%AC%D5%B8%D6%80" title="Քլոր – Armenian" lang="hy" hreflang="hy" data-title="Քլոր" data-language-autonym="Հայերեն" data-language-local-name="Armenian" class="interlanguage-link-target">Հայերեն</a></li><li class="interlanguage-link interwiki-hi mw-list-item"><a href="https://hi.wikipedia.org/wiki/%E0%A4%95%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A5%80%E0%A4%A8" title="क्लोरीन – Hindi" lang="hi" hreflang="hi" data-title="क्लोरीन" data-language-autonym="हिन्दी" data-language-local-name="Hindi" class="interlanguage-link-target">हिन्दी</a></li><li class="interlanguage-link interwiki-hr mw-list-item"><a href="https://hr.wikipedia.org/wiki/Klor" title="Klor – Croatian" lang="hr" hreflang="hr" data-title="Klor" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target">Hrvatski</a></li><li class="interlanguage-link interwiki-io mw-list-item"><a href="https://io.wikipedia.org/wiki/Kloro" title="Kloro – Ido" lang="io" hreflang="io" data-title="Kloro" data-language-autonym="Ido" data-language-local-name="Ido" class="interlanguage-link-target">Ido</a></li><li class="interlanguage-link interwiki-id mw-list-item"><a href="https://id.wikipedia.org/wiki/Klorin" title="Klorin – Indonesian" lang="id" hreflang="id" data-title="Klorin" data-language-autonym="Bahasa Indonesia" data-language-local-name="Indonesian" class="interlanguage-link-target">Bahasa Indonesia</a></li><li class="interlanguage-link interwiki-ia mw-list-item"><a href="https://ia.wikipedia.org/wiki/Chloro" title="Chloro – Interlingua" lang="ia" hreflang="ia" data-title="Chloro" data-language-autonym="Interlingua" data-language-local-name="Interlingua" class="interlanguage-link-target">Interlingua</a></li><li class="interlanguage-link interwiki-os mw-list-item"><a href="https://os.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Ossetic" lang="os" hreflang="os" data-title="Хлор" data-language-autonym="Ирон" data-language-local-name="Ossetic" class="interlanguage-link-target">Ирон</a></li><li class="interlanguage-link interwiki-zu mw-list-item"><a href="https://zu.wikipedia.org/wiki/IChwenzi" title="IChwenzi – Zulu" lang="zu" hreflang="zu" data-title="IChwenzi" data-language-autonym="IsiZulu" data-language-local-name="Zulu" class="interlanguage-link-target">IsiZulu</a></li><li class="interlanguage-link interwiki-is mw-list-item"><a href="https://is.wikipedia.org/wiki/Kl%C3%B3r" title="Klór – Icelandic" lang="is" hreflang="is" data-title="Klór" data-language-autonym="Íslenska" data-language-local-name="Icelandic" class="interlanguage-link-target">Íslenska</a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Cloro" title="Cloro – Italian" lang="it" hreflang="it" data-title="Cloro" data-language-autonym="Italiano" data-language-local-name="Italian" class="interlanguage-link-target">Italiano</a></li><li class="interlanguage-link interwiki-he mw-list-item"><a href="https://he.wikipedia.org/wiki/%D7%9B%D7%9C%D7%95%D7%A8" title="כלור – Hebrew" lang="he" hreflang="he" data-title="כלור" data-language-autonym="עברית" data-language-local-name="Hebrew" class="interlanguage-link-target">עברית</a></li><li class="interlanguage-link interwiki-jv mw-list-item"><a href="https://jv.wikipedia.org/wiki/Klor" title="Klor – Javanese" lang="jv" hreflang="jv" data-title="Klor" data-language-autonym="Jawa" data-language-local-name="Javanese" class="interlanguage-link-target">Jawa</a></li><li class="interlanguage-link interwiki-kbp mw-list-item"><a href="https://kbp.wikipedia.org/wiki/Kl%C9%94r%C9%A9" title="Klɔrɩ – Kabiye" lang="kbp" hreflang="kbp" data-title="Klɔrɩ" data-language-autonym="Kabɩyɛ" data-language-local-name="Kabiye" class="interlanguage-link-target">Kabɩyɛ</a></li><li class="interlanguage-link interwiki-kn mw-list-item"><a href="https://kn.wikipedia.org/wiki/%E0%B2%95%E0%B3%8D%E0%B2%B2%E0%B3%8B%E0%B2%B0%E0%B2%BF%E0%B2%A8%E0%B3%8D" title="ಕ್ಲೋರಿನ್ – Kannada" lang="kn" hreflang="kn" data-title="ಕ್ಲೋರಿನ್" data-language-autonym="ಕನ್ನಡ" data-language-local-name="Kannada" class="interlanguage-link-target">ಕನ್ನಡ</a></li><li class="interlanguage-link interwiki-ka mw-list-item"><a href="https://ka.wikipedia.org/wiki/%E1%83%A5%E1%83%9A%E1%83%9D%E1%83%A0%E1%83%98" title="ქლორი – Georgian" lang="ka" hreflang="ka" data-title="ქლორი" data-language-autonym="ქართული" data-language-local-name="Georgian" class="interlanguage-link-target">ქართული</a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Kazakh" lang="kk" hreflang="kk" data-title="Хлор" data-language-autonym="Қазақша" data-language-local-name="Kazakh" class="interlanguage-link-target">Қазақша</a></li><li class="interlanguage-link interwiki-kw mw-list-item"><a href="https://kw.wikipedia.org/wiki/Klorin" title="Klorin – Cornish" lang="kw" hreflang="kw" data-title="Klorin" data-language-autonym="Kernowek" data-language-local-name="Cornish" class="interlanguage-link-target">Kernowek</a></li><li class="interlanguage-link interwiki-sw mw-list-item"><a href="https://sw.wikipedia.org/wiki/Klorini" title="Klorini – Swahili" lang="sw" hreflang="sw" data-title="Klorini" data-language-autonym="Kiswahili" data-language-local-name="Swahili" class="interlanguage-link-target">Kiswahili</a></li><li class="interlanguage-link interwiki-kv mw-list-item"><a href="https://kv.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Komi" lang="kv" hreflang="kv" data-title="Хлор" data-language-autonym="Коми" data-language-local-name="Komi" class="interlanguage-link-target">Коми</a></li><li class="interlanguage-link interwiki-ht mw-list-item"><a href="https://ht.wikipedia.org/wiki/Kl%C3%B2" title="Klò – Haitian Creole" lang="ht" hreflang="ht" data-title="Klò" data-language-autonym="Kreyòl ayisyen" data-language-local-name="Haitian Creole" class="interlanguage-link-target">Kreyòl ayisyen</a></li><li class="interlanguage-link interwiki-ku mw-list-item"><a href="https://ku.wikipedia.org/wiki/Klor%C3%AEn" title="Klorîn – Kurdish" lang="ku" hreflang="ku" data-title="Klorîn" data-language-autonym="Kurdî" data-language-local-name="Kurdish" class="interlanguage-link-target">Kurdî</a></li><li class="interlanguage-link interwiki-ky mw-list-item"><a href="https://ky.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Kyrgyz" lang="ky" hreflang="ky" data-title="Хлор" data-language-autonym="Кыргызча" data-language-local-name="Kyrgyz" class="interlanguage-link-target">Кыргызча</a></li><li class="interlanguage-link interwiki-mrj mw-list-item"><a href="https://mrj.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Western Mari" lang="mrj" hreflang="mrj" data-title="Хлор" data-language-autonym="Кырык мары" data-language-local-name="Western Mari" class="interlanguage-link-target">Кырык мары</a></li><li class="interlanguage-link interwiki-la mw-list-item"><a href="https://la.wikipedia.org/wiki/Chlorum" title="Chlorum – Latin" lang="la" hreflang="la" data-title="Chlorum" data-language-autonym="Latina" data-language-local-name="Latin" class="interlanguage-link-target">Latina</a></li><li class="interlanguage-link interwiki-lv mw-list-item"><a href="https://lv.wikipedia.org/wiki/Hlors" title="Hlors – Latvian" lang="lv" hreflang="lv" data-title="Hlors" data-language-autonym="Latviešu" data-language-local-name="Latvian" class="interlanguage-link-target">Latviešu</a></li><li class="interlanguage-link interwiki-lb mw-list-item"><a href="https://lb.wikipedia.org/wiki/Chlor" title="Chlor – Luxembourgish" lang="lb" hreflang="lb" data-title="Chlor" data-language-autonym="Lëtzebuergesch" data-language-local-name="Luxembourgish" class="interlanguage-link-target">Lëtzebuergesch</a></li><li class="interlanguage-link interwiki-lt mw-list-item"><a href="https://lt.wikipedia.org/wiki/Chloras" title="Chloras – Lithuanian" lang="lt" hreflang="lt" data-title="Chloras" data-language-autonym="Lietuvių" data-language-local-name="Lithuanian" class="interlanguage-link-target">Lietuvių</a></li><li class="interlanguage-link interwiki-lij mw-list-item"><a href="https://lij.wikipedia.org/wiki/Cloro" title="Cloro – Ligurian" lang="lij" hreflang="lij" data-title="Cloro" data-language-autonym="Ligure" data-language-local-name="Ligurian" class="interlanguage-link-target">Ligure</a></li><li class="interlanguage-link interwiki-li mw-list-item"><a href="https://li.wikipedia.org/wiki/Chloear" title="Chloear – Limburgish" lang="li" hreflang="li" data-title="Chloear" data-language-autonym="Limburgs" data-language-local-name="Limburgish" class="interlanguage-link-target">Limburgs</a></li><li class="interlanguage-link interwiki-ln mw-list-item"><a href="https://ln.wikipedia.org/wiki/Koloki" title="Koloki – Lingala" lang="ln" hreflang="ln" data-title="Koloki" data-language-autonym="Lingála" data-language-local-name="Lingala" class="interlanguage-link-target">Lingála</a></li><li class="interlanguage-link interwiki-olo mw-list-item"><a href="https://olo.wikipedia.org/wiki/Hlor" title="Hlor – Livvi-Karelian" lang="olo" hreflang="olo" data-title="Hlor" data-language-autonym="Livvinkarjala" data-language-local-name="Livvi-Karelian" class="interlanguage-link-target">Livvinkarjala</a></li><li class="interlanguage-link interwiki-jbo mw-list-item"><a href="https://jbo.wikipedia.org/wiki/kliru" title="kliru – Lojban" lang="jbo" hreflang="jbo" data-title="kliru" data-language-autonym="La .lojban." data-language-local-name="Lojban" class="interlanguage-link-target">La .lojban.</a></li><li class="interlanguage-link interwiki-lg mw-list-item"><a href="https://lg.wikipedia.org/wiki/Kololiini" title="Kololiini – Ganda" lang="lg" hreflang="lg" data-title="Kololiini" data-language-autonym="Luganda" data-language-local-name="Ganda" class="interlanguage-link-target">Luganda</a></li><li class="interlanguage-link interwiki-lmo mw-list-item"><a href="https://lmo.wikipedia.org/wiki/Cloro" title="Cloro – Lombard" lang="lmo" hreflang="lmo" data-title="Cloro" data-language-autonym="Lombard" data-language-local-name="Lombard" class="interlanguage-link-target">Lombard</a></li><li class="interlanguage-link interwiki-hu mw-list-item"><a href="https://hu.wikipedia.org/wiki/Kl%C3%B3r" title="Klór – Hungarian" lang="hu" hreflang="hu" data-title="Klór" data-language-autonym="Magyar" data-language-local-name="Hungarian" class="interlanguage-link-target">Magyar</a></li><li class="interlanguage-link interwiki-mk mw-list-item"><a href="https://mk.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Macedonian" lang="mk" hreflang="mk" data-title="Хлор" data-language-autonym="Македонски" data-language-local-name="Macedonian" class="interlanguage-link-target">Македонски</a></li><li class="interlanguage-link interwiki-ml mw-list-item"><a href="https://ml.wikipedia.org/wiki/%E0%B4%95%E0%B5%8D%E0%B4%B2%E0%B5%8B%E0%B4%B1%E0%B4%BF%E0%B5%BB" title="ക്ലോറിൻ – Malayalam" lang="ml" hreflang="ml" data-title="ക്ലോറിൻ" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target">മലയാളം</a></li><li class="interlanguage-link interwiki-mi mw-list-item"><a href="https://mi.wikipedia.org/wiki/Haum%C4%81ota" title="Haumāota – Māori" lang="mi" hreflang="mi" data-title="Haumāota" data-language-autonym="Māori" data-language-local-name="Māori" class="interlanguage-link-target">Māori</a></li><li class="interlanguage-link interwiki-mr mw-list-item"><a href="https://mr.wikipedia.org/wiki/%E0%A4%A8%E0%A5%80%E0%A4%B0%E0%A4%9C%E0%A5%80" title="नीरजी – Marathi" lang="mr" hreflang="mr" data-title="नीरजी" data-language-autonym="मराठी" data-language-local-name="Marathi" class="interlanguage-link-target">मराठी</a></li><li class="interlanguage-link interwiki-arz mw-list-item"><a href="https://arz.wikipedia.org/wiki/%D9%83%D9%84%D9%88%D8%B1" title="كلور – Egyptian Arabic" lang="arz" hreflang="arz" data-title="كلور" data-language-autonym="مصرى" data-language-local-name="Egyptian Arabic" class="interlanguage-link-target">مصرى</a></li><li class="interlanguage-link interwiki-ms mw-list-item"><a href="https://ms.wikipedia.org/wiki/Klorin" title="Klorin – Malay" lang="ms" hreflang="ms" data-title="Klorin" data-language-autonym="Bahasa Melayu" data-language-local-name="Malay" class="interlanguage-link-target">Bahasa Melayu</a></li><li class="interlanguage-link interwiki-mni mw-list-item"><a href="https://mni.wikipedia.org/wiki/%EA%AF%80%EA%AF%AD%EA%AF%82%EA%AF%A3%EA%AF%94%EA%AF%A4%EA%AF%9F" title="ꯀ꯭ꯂꯣꯔꯤꯟ – Manipuri" lang="mni" hreflang="mni" data-title="ꯀ꯭ꯂꯣꯔꯤꯟ" data-language-autonym="ꯃꯤꯇꯩ ꯂꯣꯟ" data-language-local-name="Manipuri" class="interlanguage-link-target">ꯃꯤꯇꯩ ꯂꯣꯟ</a></li><li class="interlanguage-link interwiki-cdo mw-list-item"><a href="https://cdo.wikipedia.org/wiki/L%E1%B9%B3%CC%86k_(ngu%C3%B2ng-s%C3%B3)" title="Lṳ̆k (nguòng-só) – Mindong" lang="cdo" hreflang="cdo" data-title="Lṳ̆k (nguòng-só)" data-language-autonym="閩東語 / Mìng-dĕ̤ng-ngṳ̄" data-language-local-name="Mindong" class="interlanguage-link-target">閩東語 / Mìng-dĕ̤ng-ngṳ̄</a></li><li class="interlanguage-link interwiki-mn mw-list-item"><a href="https://mn.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Mongolian" lang="mn" hreflang="mn" data-title="Хлор" data-language-autonym="Монгол" data-language-local-name="Mongolian" class="interlanguage-link-target">Монгол</a></li><li class="interlanguage-link interwiki-my mw-list-item"><a href="https://my.wikipedia.org/wiki/%E1%80%80%E1%80%9C%E1%80%AD%E1%80%AF%E1%80%9B%E1%80%84%E1%80%BA%E1%80%B8" title="ကလိုရင်း – Burmese" lang="my" hreflang="my" data-title="ကလိုရင်း" data-language-autonym="မြန်မာဘာသာ" data-language-local-name="Burmese" class="interlanguage-link-target">မြန်မာဘာသာ</a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Chloor_(element)" title="Chloor (element) – Dutch" lang="nl" hreflang="nl" data-title="Chloor (element)" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target">Nederlands</a></li><li class="interlanguage-link interwiki-ne mw-list-item"><a href="https://ne.wikipedia.org/wiki/%E0%A4%95%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="क्लोरिन – Nepali" lang="ne" hreflang="ne" data-title="क्लोरिन" data-language-autonym="नेपाली" data-language-local-name="Nepali" class="interlanguage-link-target">नेपाली</a></li><li class="interlanguage-link interwiki-new mw-list-item"><a href="https://new.wikipedia.org/wiki/%E0%A4%95%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="क्लोरिन – Newari" lang="new" hreflang="new" data-title="क्लोरिन" data-language-autonym="नेपाल भाषा" data-language-local-name="Newari" class="interlanguage-link-target">नेपाल भाषा</a></li><li class="interlanguage-link interwiki-ja mw-list-item"><a href="https://ja.wikipedia.org/wiki/%E5%A1%A9%E7%B4%A0" title="塩素 – Japanese" lang="ja" hreflang="ja" data-title="塩素" data-language-autonym="日本語" data-language-local-name="Japanese" class="interlanguage-link-target">日本語</a></li><li class="interlanguage-link interwiki-frr mw-list-item"><a href="https://frr.wikipedia.org/wiki/Kloor" title="Kloor – Northern Frisian" lang="frr" hreflang="frr" data-title="Kloor" data-language-autonym="Nordfriisk" data-language-local-name="Northern Frisian" class="interlanguage-link-target">Nordfriisk</a></li><li class="interlanguage-link interwiki-no mw-list-item"><a href="https://no.wikipedia.org/wiki/Klor" title="Klor – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Klor" data-language-autonym="Norsk bokmål" data-language-local-name="Norwegian Bokmål" class="interlanguage-link-target">Norsk bokmål</a></li><li class="interlanguage-link interwiki-nn mw-list-item"><a href="https://nn.wikipedia.org/wiki/Klor" title="Klor – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Klor" data-language-autonym="Norsk nynorsk" data-language-local-name="Norwegian Nynorsk" class="interlanguage-link-target">Norsk nynorsk</a></li><li class="interlanguage-link interwiki-nov mw-list-item"><a href="https://nov.wikipedia.org/wiki/Klore" title="Klore – Novial" lang="nov" hreflang="nov" data-title="Klore" data-language-autonym="Novial" data-language-local-name="Novial" class="interlanguage-link-target">Novial</a></li><li class="interlanguage-link interwiki-oc mw-list-item"><a href="https://oc.wikipedia.org/wiki/Cl%C3%B2r" title="Clòr – Occitan" lang="oc" hreflang="oc" data-title="Clòr" data-language-autonym="Occitan" data-language-local-name="Occitan" class="interlanguage-link-target">Occitan</a></li><li class="interlanguage-link interwiki-or mw-list-item"><a href="https://or.wikipedia.org/wiki/%E0%AC%95%E0%AD%8D%E0%AC%B2%E0%AD%8B%E0%AC%B0%E0%AC%BF%E0%AC%A8" title="କ୍ଲୋରିନ – Odia" lang="or" hreflang="or" data-title="କ୍ଲୋରିନ" data-language-autonym="ଓଡ଼ିଆ" data-language-local-name="Odia" class="interlanguage-link-target">ଓଡ଼ିଆ</a></li><li class="interlanguage-link interwiki-uz mw-list-item"><a href="https://uz.wikipedia.org/wiki/Xlor" title="Xlor – Uzbek" lang="uz" hreflang="uz" data-title="Xlor" data-language-autonym="Oʻzbekcha / ўзбекча" data-language-local-name="Uzbek" class="interlanguage-link-target">Oʻzbekcha / ўзбекча</a></li><li class="interlanguage-link interwiki-pa mw-list-item"><a href="https://pa.wikipedia.org/wiki/%E0%A8%95%E0%A8%B2%E0%A9%8B%E0%A8%B0%E0%A9%80%E0%A8%A8" title="ਕਲੋਰੀਨ – Punjabi" lang="pa" hreflang="pa" data-title="ਕਲੋਰੀਨ" data-language-autonym="ਪੰਜਾਬੀ" data-language-local-name="Punjabi" class="interlanguage-link-target">ਪੰਜਾਬੀ</a></li><li class="interlanguage-link interwiki-pi mw-list-item"><a href="https://pi.wikipedia.org/wiki/%E0%A4%95%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="क्लोरिन – Pali" lang="pi" hreflang="pi" data-title="क्लोरिन" data-language-autonym="पालि" data-language-local-name="Pali" class="interlanguage-link-target">पालि</a></li><li class="interlanguage-link interwiki-pnb mw-list-item"><a href="https://pnb.wikipedia.org/wiki/%DA%A9%D9%84%D9%88%D8%B1%DB%8C%D9%86" title="کلورین – Western Punjabi" lang="pnb" hreflang="pnb" data-title="کلورین" data-language-autonym="پنجابی" data-language-local-name="Western Punjabi" class="interlanguage-link-target">پنجابی</a></li><li class="interlanguage-link interwiki-blk mw-list-item"><a href="https://blk.wikipedia.org/wiki/%E1%80%80%E1%80%9C%E1%80%AD%E1%80%AF%E1%80%9B%E1%80%89%E1%80%BA%E1%80%B8" title="ကလိုရဉ်း – Pa'O" lang="blk" hreflang="blk" data-title="ကလိုရဉ်း" data-language-autonym="ပအိုဝ်ႏဘာႏသာႏ" data-language-local-name="Pa'O" class="interlanguage-link-target">ပအိုဝ်ႏဘာႏသာႏ</a></li><li class="interlanguage-link interwiki-ps mw-list-item"><a href="https://ps.wikipedia.org/wiki/%DA%A9%D9%84%D9%88%D8%B1%D9%8A%D9%86" title="کلورين – Pashto" lang="ps" hreflang="ps" data-title="کلورين" data-language-autonym="پښتو" data-language-local-name="Pashto" class="interlanguage-link-target">پښتو</a></li><li class="interlanguage-link interwiki-pms mw-list-item"><a href="https://pms.wikipedia.org/wiki/Cl%C3%B2r" title="Clòr – Piedmontese" lang="pms" hreflang="pms" data-title="Clòr" data-language-autonym="Piemontèis" data-language-local-name="Piedmontese" class="interlanguage-link-target">Piemontèis</a></li><li class="interlanguage-link interwiki-nds mw-list-item"><a href="https://nds.wikipedia.org/wiki/Chlor" title="Chlor – Low German" lang="nds" hreflang="nds" data-title="Chlor" data-language-autonym="Plattdüütsch" data-language-local-name="Low German" class="interlanguage-link-target">Plattdüütsch</a></li><li class="interlanguage-link interwiki-pl mw-list-item"><a href="https://pl.wikipedia.org/wiki/Chlor" title="Chlor – Polish" lang="pl" hreflang="pl" data-title="Chlor" data-language-autonym="Polski" data-language-local-name="Polish" class="interlanguage-link-target">Polski</a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/Cloro" title="Cloro – Portuguese" lang="pt" hreflang="pt" data-title="Cloro" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target">Português</a></li><li class="interlanguage-link interwiki-ro mw-list-item"><a href="https://ro.wikipedia.org/wiki/Clor" title="Clor – Romanian" lang="ro" hreflang="ro" data-title="Clor" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target">Română</a></li><li class="interlanguage-link interwiki-qu mw-list-item"><a href="https://qu.wikipedia.org/wiki/Kuluru" title="Kuluru – Quechua" lang="qu" hreflang="qu" data-title="Kuluru" data-language-autonym="Runa Simi" data-language-local-name="Quechua" class="interlanguage-link-target">Runa Simi</a></li><li class="interlanguage-link interwiki-rue mw-list-item"><a href="https://rue.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Rusyn" lang="rue" hreflang="rue" data-title="Хлор" data-language-autonym="Русиньскый" data-language-local-name="Rusyn" class="interlanguage-link-target">Русиньскый</a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Russian" lang="ru" hreflang="ru" data-title="Хлор" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target">Русский</a></li><li class="interlanguage-link interwiki-sa mw-list-item"><a href="https://sa.wikipedia.org/wiki/%E0%A4%95%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="क्लोरिन – Sanskrit" lang="sa" hreflang="sa" data-title="क्लोरिन" data-language-autonym="संस्कृतम्" data-language-local-name="Sanskrit" class="interlanguage-link-target">संस्कृतम्</a></li><li class="interlanguage-link interwiki-sc mw-list-item"><a href="https://sc.wikipedia.org/wiki/Cloro" title="Cloro – Sardinian" lang="sc" hreflang="sc" data-title="Cloro" data-language-autonym="Sardu" data-language-local-name="Sardinian" class="interlanguage-link-target">Sardu</a></li><li class="interlanguage-link interwiki-sco mw-list-item"><a href="https://sco.wikipedia.org/wiki/Chlorine" title="Chlorine – Scots" lang="sco" hreflang="sco" data-title="Chlorine" data-language-autonym="Scots" data-language-local-name="Scots" class="interlanguage-link-target">Scots</a></li><li class="interlanguage-link interwiki-stq mw-list-item"><a href="https://stq.wikipedia.org/wiki/Chlor" title="Chlor – Saterland Frisian" lang="stq" hreflang="stq" data-title="Chlor" data-language-autonym="Seeltersk" data-language-local-name="Saterland Frisian" class="interlanguage-link-target">Seeltersk</a></li><li class="interlanguage-link interwiki-sq mw-list-item"><a href="https://sq.wikipedia.org/wiki/Klori" title="Klori – Albanian" lang="sq" hreflang="sq" data-title="Klori" data-language-autonym="Shqip" data-language-local-name="Albanian" class="interlanguage-link-target">Shqip</a></li><li class="interlanguage-link interwiki-scn mw-list-item"><a href="https://scn.wikipedia.org/wiki/Cloru" title="Cloru – Sicilian" lang="scn" hreflang="scn" data-title="Cloru" data-language-autonym="Sicilianu" data-language-local-name="Sicilian" class="interlanguage-link-target">Sicilianu</a></li><li class="interlanguage-link interwiki-si mw-list-item"><a href="https://si.wikipedia.org/wiki/%E0%B6%9A%E0%B7%8A%E0%B6%BD%E0%B7%9D%E0%B6%BB%E0%B7%93%E0%B6%B1%E0%B7%8A" title="ක්ලෝරීන් – Sinhala" lang="si" hreflang="si" data-title="ක්ලෝරීන්" data-language-autonym="සිංහල" data-language-local-name="Sinhala" class="interlanguage-link-target">සිංහල</a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Chlorine" title="Chlorine – Simple English" lang="en-simple" hreflang="en-simple" data-title="Chlorine" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target">Simple English</a></li><li class="interlanguage-link interwiki-sd mw-list-item"><a href="https://sd.wikipedia.org/wiki/%DA%AA%D9%84%D9%88%D8%B1%D9%8A%D9%86" title="ڪلورين – Sindhi" lang="sd" hreflang="sd" data-title="ڪلورين" data-language-autonym="سنڌي" data-language-local-name="Sindhi" class="interlanguage-link-target">سنڌي</a></li><li class="interlanguage-link interwiki-sk badge-Q17437796 badge-featuredarticle mw-list-item" title="featured article badge"><a href="https://sk.wikipedia.org/wiki/Chl%C3%B3r" title="Chlór – Slovak" lang="sk" hreflang="sk" data-title="Chlór" data-language-autonym="Slovenčina" data-language-local-name="Slovak" class="interlanguage-link-target">Slovenčina</a></li><li class="interlanguage-link interwiki-sl mw-list-item"><a href="https://sl.wikipedia.org/wiki/Klor" title="Klor – Slovenian" lang="sl" hreflang="sl" data-title="Klor" data-language-autonym="Slovenščina" data-language-local-name="Slovenian" class="interlanguage-link-target">Slovenščina</a></li><li class="interlanguage-link interwiki-so mw-list-item"><a href="https://so.wikipedia.org/wiki/Koloriin" title="Koloriin – Somali" lang="so" hreflang="so" data-title="Koloriin" data-language-autonym="Soomaaliga" data-language-local-name="Somali" class="interlanguage-link-target">Soomaaliga</a></li><li class="interlanguage-link interwiki-ckb mw-list-item"><a href="https://ckb.wikipedia.org/wiki/%DA%A9%D9%84%DB%86%D8%B1" title="کلۆر – Central Kurdish" lang="ckb" hreflang="ckb" data-title="کلۆر" data-language-autonym="کوردی" data-language-local-name="Central Kurdish" class="interlanguage-link-target">کوردی</a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Serbian" lang="sr" hreflang="sr" data-title="Хлор" data-language-autonym="Српски / srpski" data-language-local-name="Serbian" class="interlanguage-link-target">Српски / srpski</a></li><li class="interlanguage-link interwiki-sh mw-list-item"><a href="https://sh.wikipedia.org/wiki/Hlor" title="Hlor – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Hlor" data-language-autonym="Srpskohrvatski / српскохрватски" data-language-local-name="Serbo-Croatian" class="interlanguage-link-target">Srpskohrvatski / српскохрватски</a></li><li class="interlanguage-link interwiki-su mw-list-item"><a href="https://su.wikipedia.org/wiki/Klor" title="Klor – Sundanese" lang="su" hreflang="su" data-title="Klor" data-language-autonym="Sunda" data-language-local-name="Sundanese" class="interlanguage-link-target">Sunda</a></li><li class="interlanguage-link interwiki-fi mw-list-item"><a href="https://fi.wikipedia.org/wiki/Kloori" title="Kloori – Finnish" lang="fi" hreflang="fi" data-title="Kloori" data-language-autonym="Suomi" data-language-local-name="Finnish" class="interlanguage-link-target">Suomi</a></li><li class="interlanguage-link interwiki-sv mw-list-item"><a href="https://sv.wikipedia.org/wiki/Klor" title="Klor – Swedish" lang="sv" hreflang="sv" data-title="Klor" data-language-autonym="Svenska" data-language-local-name="Swedish" class="interlanguage-link-target">Svenska</a></li><li class="interlanguage-link interwiki-tl badge-Q70894304 mw-list-item" title=""><a href="https://tl.wikipedia.org/wiki/Klorina" title="Klorina – Tagalog" lang="tl" hreflang="tl" data-title="Klorina" data-language-autonym="Tagalog" data-language-local-name="Tagalog" class="interlanguage-link-target">Tagalog</a></li><li class="interlanguage-link interwiki-ta mw-list-item"><a href="https://ta.wikipedia.org/wiki/%E0%AE%95%E0%AF%81%E0%AE%B3%E0%AF%8B%E0%AE%B0%E0%AE%BF%E0%AE%A9%E0%AF%8D" title="குளோரின் – Tamil" lang="ta" hreflang="ta" data-title="குளோரின்" data-language-autonym="தமிழ்" data-language-local-name="Tamil" class="interlanguage-link-target">தமிழ்</a></li><li class="interlanguage-link interwiki-tt mw-list-item"><a href="https://tt.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Tatar" lang="tt" hreflang="tt" data-title="Хлор" data-language-autonym="Татарча / tatarça" data-language-local-name="Tatar" class="interlanguage-link-target">Татарча / tatarça</a></li><li class="interlanguage-link interwiki-te mw-list-item"><a href="https://te.wikipedia.org/wiki/%E0%B0%95%E0%B1%8D%E0%B0%B2%E0%B1%8B%E0%B0%B0%E0%B0%BF%E0%B0%A8%E0%B1%8D" title="క్లోరిన్ – Telugu" lang="te" hreflang="te" data-title="క్లోరిన్" data-language-autonym="తెలుగు" data-language-local-name="Telugu" class="interlanguage-link-target">తెలుగు</a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B8%84%E0%B8%A5%E0%B8%AD%E0%B8%A3%E0%B8%B5%E0%B8%99" title="คลอรีน – Thai" lang="th" hreflang="th" data-title="คลอรีน" data-language-autonym="ไทย" data-language-local-name="Thai" class="interlanguage-link-target">ไทย</a></li><li class="interlanguage-link interwiki-tg mw-list-item"><a href="https://tg.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Tajik" lang="tg" hreflang="tg" data-title="Хлор" data-language-autonym="Тоҷикӣ" data-language-local-name="Tajik" class="interlanguage-link-target">Тоҷикӣ</a></li><li class="interlanguage-link interwiki-tr mw-list-item"><a href="https://tr.wikipedia.org/wiki/Klor" title="Klor – Turkish" lang="tr" hreflang="tr" data-title="Klor" data-language-autonym="Türkçe" data-language-local-name="Turkish" class="interlanguage-link-target">Türkçe</a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a href="https://uk.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80" title="Хлор – Ukrainian" lang="uk" hreflang="uk" data-title="Хлор" data-language-autonym="Українська" data-language-local-name="Ukrainian" class="interlanguage-link-target">Українська</a></li><li class="interlanguage-link interwiki-ur mw-list-item"><a href="https://ur.wikipedia.org/wiki/%DA%A9%D9%84%D9%88%D8%B1%DB%8C%D9%86" title="کلورین – Urdu" lang="ur" hreflang="ur" data-title="کلورین" data-language-autonym="اردو" data-language-local-name="Urdu" class="interlanguage-link-target">اردو</a></li><li class="interlanguage-link interwiki-ug mw-list-item"><a href="https://ug.wikipedia.org/wiki/%D8%AE%D9%84%D9%88%D8%B1_%DA%AF%D8%A7%D8%B2%D9%89" title="خلور گازى – Uyghur" lang="ug" hreflang="ug" data-title="خلور گازى" data-language-autonym="ئۇيغۇرچە / Uyghurche" data-language-local-name="Uyghur" class="interlanguage-link-target">ئۇيغۇرچە / Uyghurche</a></li><li class="interlanguage-link interwiki-za mw-list-item"><a href="https://za.wikipedia.org/wiki/Luz" title="Luz – Zhuang" lang="za" hreflang="za" data-title="Luz" data-language-autonym="Vahcuengh" data-language-local-name="Zhuang" class="interlanguage-link-target">Vahcuengh</a></li><li class="interlanguage-link interwiki-vep mw-list-item"><a href="https://vep.wikipedia.org/wiki/Hlor" title="Hlor – Veps" lang="vep" hreflang="vep" data-title="Hlor" data-language-autonym="Vepsän kel’" data-language-local-name="Veps" class="interlanguage-link-target">Vepsän kel’</a></li><li class="interlanguage-link interwiki-vi mw-list-item"><a href="https://vi.wikipedia.org/wiki/Chlor" title="Chlor – Vietnamese" lang="vi" hreflang="vi" data-title="Chlor" data-language-autonym="Tiếng Việt" data-language-local-name="Vietnamese" class="interlanguage-link-target">Tiếng Việt</a></li><li class="interlanguage-link interwiki-vo mw-list-item"><a href="https://vo.wikipedia.org/wiki/Klorin" title="Klorin – Volapük" lang="vo" hreflang="vo" data-title="Klorin" data-language-autonym="Volapük" data-language-local-name="Volapük" class="interlanguage-link-target">Volapük</a></li><li class="interlanguage-link interwiki-wa mw-list-item"><a href="https://wa.wikipedia.org/wiki/Cl%C3%B4re" title="Clôre – Walloon" lang="wa" hreflang="wa" data-title="Clôre" data-language-autonym="Walon" data-language-local-name="Walloon" class="interlanguage-link-target">Walon</a></li><li class="interlanguage-link interwiki-zh-classical mw-list-item"><a href="https://zh-classical.wikipedia.org/wiki/%E6%B0%AF" title="氯 – Literary Chinese" lang="lzh" hreflang="lzh" data-title="氯" data-language-autonym="文言" data-language-local-name="Literary Chinese" class="interlanguage-link-target">文言</a></li><li class="interlanguage-link interwiki-war mw-list-item"><a href="https://war.wikipedia.org/wiki/Cloro" title="Cloro – Waray" lang="war" 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href="https://zgh.wikipedia.org/wiki/%E2%B4%B0%E2%B4%BD%E2%B5%8D%E2%B5%93%E2%B5%94" title="ⴰⴽⵍⵓⵔ – Standard Moroccan Tamazight" lang="zgh" hreflang="zgh" data-title="ⴰⴽⵍⵓⵔ" data-language-autonym="ⵜⴰⵎⴰⵣⵉⵖⵜ ⵜⴰⵏⴰⵡⴰⵢⵜ" data-language-local-name="Standard Moroccan Tamazight" class="interlanguage-link-target">ⵜⴰⵎⴰⵣⵉⵖⵜ ⵜⴰⵏⴰⵡⴰⵢⵜ</a></li> </ul> <div class="after-portlet after-portlet-lang"><a href="https://www.wikidata.org/wiki/Special:EntityPage/Q688#sitelinks-wikipedia" title="Edit interlanguage links" class="wbc-editpage">Edit links</a></div> </div> </div> </div> </header> <div class="vector-page-toolbar"> <div class="vector-page-toolbar-container"> <div id="left-navigation"> <nav aria-label="Namespaces"> <div id="p-associated-pages" class="vector-menu vector-menu-tabs mw-portlet mw-portlet-associated-pages" > <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li id="ca-nstab-main" class="selected vector-tab-noicon mw-list-item"><a href="/wiki/Chlorine" title="View the 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Click here for more information." src="//upload.wikimedia.org/wikipedia/en/thumb/9/94/Symbol_support_vote.svg/19px-Symbol_support_vote.svg.png" decoding="async" width="19" height="20" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/94/Symbol_support_vote.svg/29px-Symbol_support_vote.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/94/Symbol_support_vote.svg/39px-Symbol_support_vote.svg.png 2x" data-file-width="180" data-file-height="185" /></a></div></div> <div id="mw-indicator-pp-default" class="mw-indicator"><div class="mw-parser-output"><a href="/wiki/Wikipedia:Protection_policy#semi" title="This article is semi-protected."><img alt="Page semi-protected" src="//upload.wikimedia.org/wikipedia/en/thumb/1/1b/Semi-protection-shackle.svg/20px-Semi-protection-shackle.svg.png" decoding="async" width="20" height="20" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/1/1b/Semi-protection-shackle.svg/30px-Semi-protection-shackle.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/1/1b/Semi-protection-shackle.svg/40px-Semi-protection-shackle.svg.png 2x" data-file-width="512" data-file-height="512" /></a></div></div> </div> <div id="siteSub" class="noprint">From Wikipedia, the free encyclopedia</div> </div> <div id="contentSub"><div id="mw-content-subtitle"></div></div> <div id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><style data-mw-deduplicate="TemplateStyles:r1236090951">.mw-parser-output .hatnote{font-style:italic}.mw-parser-output div.hatnote{padding-left:1.6em;margin-bottom:0.5em}.mw-parser-output .hatnote i{font-style:normal}.mw-parser-output .hatnote+link+.hatnote{margin-top:-0.5em}@media print{body.ns-0 .mw-parser-output .hatnote{display:none!important}}</style><div role="note" class="hatnote navigation-not-searchable">Not to be confused with <a href="/wiki/Chloride" title="Chloride">chloride</a>.</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">This article is about the chemical element. For other uses, see <a href="/wiki/Chlorine_(disambiguation)" class="mw-disambig" title="Chlorine (disambiguation)">Chlorine (disambiguation)</a>.</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">"Cl" and "Cl2" redirect here. For other uses, see <a href="/wiki/CL_(disambiguation)" class="mw-redirect mw-disambig" title="CL (disambiguation)">CL (disambiguation)</a> and <a href="/wiki/CL2_(disambiguation)" class="mw-redirect mw-disambig" title="CL2 (disambiguation)">CL2 (disambiguation)</a>.</div> <div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical element with atomic number 17 (Cl)</div><style data-mw-deduplicate="TemplateStyles:r1257001546">.mw-parser-output .infobox-subbox{padding:0;border:none;margin:-3px;width:auto;min-width:100%;font-size:100%;clear:none;float:none;background-color:transparent}.mw-parser-output .infobox-3cols-child{margin:auto}.mw-parser-output .infobox .navbar{font-size:100%}@media screen{html.skin-theme-clientpref-night .mw-parser-output .infobox-full-data:not(.notheme)>div:not(.notheme)[style]{background:#1f1f23!important;color:#f8f9fa}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .infobox-full-data:not(.notheme) div:not(.notheme){background:#1f1f23!important;color:#f8f9fa}}@media(min-width:640px){body.skin--responsive .mw-parser-output .infobox-table{display:table!important}body.skin--responsive .mw-parser-output .infobox-table>caption{display:table-caption!important}body.skin--responsive .mw-parser-output .infobox-table>tbody{display:table-row-group}body.skin--responsive .mw-parser-output .infobox-table tr{display:table-row!important}body.skin--responsive .mw-parser-output .infobox-table th,body.skin--responsive .mw-parser-output .infobox-table td{padding-left:inherit;padding-right:inherit}}</style><style data-mw-deduplicate="TemplateStyles:r1158442001">body.skin-minerva .mw-parser-output .infobox-full-data>.wikitable,body.skin-minerva .mw-parser-output .infobox .periodictable{display:table}body.skin-minerva .mw-parser-output .infobox-full-data{width:calc(100% - 20px)}body.skin-minerva .mw-parser-output .infobox-full-data>div{max-width:100%;overflow:auto}body.skin-minerva .mw-parser-output .infobox caption{display:table-caption}</style><table class="infobox"><caption class="infobox-title">Chlorine, 17Cl</caption><tbody><tr><td colspan="2" class="infobox-image"><a href="/wiki/File:Chlorine_in_bottle.jpg" class="mw-file-description"><img alt="A glass container filled with chlorine gas" src="//upload.wikimedia.org/wikipedia/commons/thumb/4/49/Chlorine_in_bottle.jpg/220px-Chlorine_in_bottle.jpg" decoding="async" width="220" height="293" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/49/Chlorine_in_bottle.jpg/330px-Chlorine_in_bottle.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/49/Chlorine_in_bottle.jpg/440px-Chlorine_in_bottle.jpg 2x" data-file-width="500" data-file-height="667" /></a></td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Chlorine</th></tr><tr><th scope="row" class="infobox-label">Pronunciation</th><td class="infobox-data"><a href="/wiki/Help:IPA/English" title="Help:IPA/English">/ˈklɔːriːn, -aɪn/</a> (<a href="/wiki/Help:Pronunciation_respelling_key" title="Help:Pronunciation respelling key">KLOR-een, -⁠eyen</a>)</td></tr><tr><th scope="row" class="infobox-label">Appearance</th><td class="infobox-data">pale yellow-green gas</td></tr><tr><td colspan="2" class="infobox-full-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1257001546"></td></tr><tr><th colspan="2" class="infobox-header" style="text-align: left; color:inherit; background: transparent;"><a href="/wiki/Standard_atomic_weight" title="Standard atomic weight">Standard atomic weight</a> <style data-mw-deduplicate="TemplateStyles:r886047488">.mw-parser-output .nobold{font-weight:normal}</style>Ar°(Cl)</th></tr><tr><th scope="row" class="infobox-label"></th><td class="infobox-data"><style data-mw-deduplicate="TemplateStyles:r1126788409">.mw-parser-output .plainlist ol,.mw-parser-output .plainlist ul{line-height:inherit;list-style:none;margin:0;padding:0}.mw-parser-output .plainlist ol li,.mw-parser-output .plainlist ul li{margin-bottom:0}</style><div class="plainlist"><ul><li>[35.446, 35.457]<a href="#cite_note-CIAAW-1">[1]</a></li><li>35.45±0.01 (<a href="/wiki/Standard_atomic_weight#Abridged_atomic_weight" title="Standard atomic weight">abridged</a>)<a href="#cite_note-CIAAW2021-2">[2]</a></li></ul></div></td></tr><tr style="display:none"><td colspan="2"> </td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Chlorine in the <a href="/wiki/Periodic_table" title="Periodic table">periodic table</a></th></tr><tr><td colspan="2" class="infobox-full-data"> <table class="wikitable" style="text-align:center; width:100%; margin:0;"> <tbody><tr> <td> <table class="periodictable" style="margin:0 auto"> <tbody><tr> <td style="border:none; width:5px"><div style="background-color:transparent; color:inherit; margin:0; padding:0; text-align:center; border:none;"> <table style="empty-cells:hidden; border:none; padding:0; border-spacing:1px; border-collapse:separate; margin:0;"> <tbody><tr> <td style="border:none;padding:0;"><a href="/wiki/Hydrogen" title="Hydrogen">Hydrogen</a> </td> <td colspan="30" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Helium" title="Helium">Helium</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Lithium" title="Lithium">Lithium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Beryllium" title="Beryllium">Beryllium</a> </td> <td colspan="24" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Boron" title="Boron">Boron</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Carbon" title="Carbon">Carbon</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nitrogen" title="Nitrogen">Nitrogen</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Oxygen" title="Oxygen">Oxygen</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Fluorine" title="Fluorine">Fluorine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Neon" title="Neon">Neon</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Sodium" title="Sodium">Sodium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Magnesium" title="Magnesium">Magnesium</a> </td> <td colspan="24" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Aluminium" title="Aluminium">Aluminium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Silicon" title="Silicon">Silicon</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Phosphorus" title="Phosphorus">Phosphorus</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Sulfur" title="Sulfur">Sulfur</a> </td> <td style="border:none;padding:0;"><a class="mw-selflink selflink">Chlorine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Argon" title="Argon">Argon</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Potassium" title="Potassium">Potassium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Calcium" title="Calcium">Calcium</a> </td> <td colspan="14" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Scandium" title="Scandium">Scandium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Titanium" title="Titanium">Titanium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Vanadium" title="Vanadium">Vanadium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Chromium" title="Chromium">Chromium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Manganese" title="Manganese">Manganese</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Iron" title="Iron">Iron</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Cobalt" title="Cobalt">Cobalt</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nickel" title="Nickel">Nickel</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Copper" title="Copper">Copper</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Zinc" title="Zinc">Zinc</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Gallium" title="Gallium">Gallium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Germanium" title="Germanium">Germanium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Arsenic" title="Arsenic">Arsenic</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Selenium" title="Selenium">Selenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Bromine" title="Bromine">Bromine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Krypton" title="Krypton">Krypton</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Rubidium" title="Rubidium">Rubidium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Strontium" title="Strontium">Strontium</a> </td> <td style="border:none;padding:0;; width:0;"> </td> <td colspan="13" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Yttrium" title="Yttrium">Yttrium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Zirconium" title="Zirconium">Zirconium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Niobium" title="Niobium">Niobium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Molybdenum" title="Molybdenum">Molybdenum</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Technetium" title="Technetium">Technetium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Ruthenium" title="Ruthenium">Ruthenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Rhodium" title="Rhodium">Rhodium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Palladium" title="Palladium">Palladium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Silver" title="Silver">Silver</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Cadmium" title="Cadmium">Cadmium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Indium" title="Indium">Indium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tin" title="Tin">Tin</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Antimony" title="Antimony">Antimony</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tellurium" title="Tellurium">Tellurium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Iodine" title="Iodine">Iodine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Xenon" title="Xenon">Xenon</a> </td></tr> <tr style="border:none;padding:0;"> <td style="border:none;padding:0;"><a href="/wiki/Caesium" title="Caesium">Caesium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Barium" title="Barium">Barium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lanthanum" title="Lanthanum">Lanthanum</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Cerium" title="Cerium">Cerium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Praseodymium" title="Praseodymium">Praseodymium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Neodymium" title="Neodymium">Neodymium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Promethium" title="Promethium">Promethium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Samarium" title="Samarium">Samarium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Europium" title="Europium">Europium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Gadolinium" title="Gadolinium">Gadolinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Terbium" title="Terbium">Terbium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Dysprosium" title="Dysprosium">Dysprosium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Holmium" title="Holmium">Holmium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Erbium" title="Erbium">Erbium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Thulium" title="Thulium">Thulium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Ytterbium" title="Ytterbium">Ytterbium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lutetium" title="Lutetium">Lutetium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Hafnium" title="Hafnium">Hafnium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tantalum" title="Tantalum">Tantalum</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tungsten" title="Tungsten">Tungsten</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Rhenium" title="Rhenium">Rhenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Osmium" title="Osmium">Osmium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Iridium" title="Iridium">Iridium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Platinum" title="Platinum">Platinum</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Gold" title="Gold">Gold</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Mercury_(element)" title="Mercury (element)">Mercury (element)</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Thallium" title="Thallium">Thallium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lead" title="Lead">Lead</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Bismuth" title="Bismuth">Bismuth</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Polonium" title="Polonium">Polonium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Astatine" title="Astatine">Astatine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Radon" title="Radon">Radon</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Francium" title="Francium">Francium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Radium" title="Radium">Radium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Actinium" title="Actinium">Actinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Thorium" title="Thorium">Thorium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Protactinium" title="Protactinium">Protactinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Uranium" title="Uranium">Uranium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Neptunium" title="Neptunium">Neptunium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Plutonium" title="Plutonium">Plutonium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Americium" title="Americium">Americium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Curium" title="Curium">Curium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Berkelium" title="Berkelium">Berkelium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Californium" title="Californium">Californium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Einsteinium" title="Einsteinium">Einsteinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Fermium" title="Fermium">Fermium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Mendelevium" title="Mendelevium">Mendelevium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nobelium" title="Nobelium">Nobelium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lawrencium" title="Lawrencium">Lawrencium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Rutherfordium" title="Rutherfordium">Rutherfordium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Dubnium" title="Dubnium">Dubnium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Seaborgium" title="Seaborgium">Seaborgium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Bohrium" title="Bohrium">Bohrium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Hassium" title="Hassium">Hassium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Meitnerium" title="Meitnerium">Meitnerium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Darmstadtium" title="Darmstadtium">Darmstadtium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Roentgenium" title="Roentgenium">Roentgenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Copernicium" title="Copernicium">Copernicium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nihonium" title="Nihonium">Nihonium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Flerovium" title="Flerovium">Flerovium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Moscovium" title="Moscovium">Moscovium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Livermorium" title="Livermorium">Livermorium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tennessine" title="Tennessine">Tennessine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Oganesson" title="Oganesson">Oganesson</a> </td></tr></tbody></table> </div> </td> <td style="vertical-align:middle; text-align:center; font-size:90%; line-height:100%; width:10px; border:none;"><a href="/wiki/Fluorine" title="Fluorine">F</a> ↑ Cl ↓ <a href="/wiki/Bromine" title="Bromine">Br</a> </td></tr> <tr> <td colspan="2" class="nowrap" style="text-align:center; font-size:90%; line-height:100%; padding-top:0; padding-bottom:1px; border:none;"><a href="/wiki/Sulfur" title="Sulfur">sulfur</a> ← chlorine → <a href="/wiki/Argon" title="Argon">argon</a> </td></tr></tbody></table> </td></tr></tbody></table></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Atomic_number" title="Atomic number">Atomic number</a> (Z)</th><td class="infobox-data">17</td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Group_(periodic_table)" title="Group (periodic table)">Group</a></th><td class="infobox-data"><a href="/wiki/Halogen" title="Halogen">group 17 (halogens)</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Period_(periodic_table)" title="Period (periodic table)">Period</a></th><td class="infobox-data"><a href="/wiki/Period_3_element" title="Period 3 element">period 3</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Block_(periodic_table)" title="Block (periodic table)">Block</a></th><td class="infobox-data">  <a href="/wiki/Block_(periodic_table)#p-block" title="Block (periodic table)">p-block</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Electron_configuration" title="Electron configuration">Electron configuration</a></th><td class="infobox-data">[<a href="/wiki/Neon" title="Neon">Ne</a>] 3s2 3p5</td></tr><tr><th scope="row" class="infobox-label">Electrons per shell</th><td class="infobox-data">2, 8, 7</td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Physical properties</th></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Phase_(matter)" title="Phase (matter)">Phase</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r886047488">at <a href="/wiki/Standard_temperature_and_pressure" title="Standard temperature and pressure">STP</a></th><td class="infobox-data"><a href="/wiki/Gas" title="Gas">gas</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Melting_point" title="Melting point">Melting point</a></th><td class="infobox-data">(Cl2) 171.6 <a href="/wiki/Kelvin" title="Kelvin">K</a> (−101.5 °C, −150.7 °F) </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Boiling_point" title="Boiling point">Boiling point</a></th><td class="infobox-data">(Cl2) 239.11 K (−34.04 °C, −29.27 °F) </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Density" title="Density">Density</a> (at STP)</th><td class="infobox-data">3.2 g/L</td></tr><tr><th scope="row" class="infobox-label">when liquid (at <a href="/wiki/Boiling_point" title="Boiling point">b.p.</a>)</th><td class="infobox-data">1.5625 g/cm3<a href="#cite_note-3">[3]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Triple_point" title="Triple point">Triple point</a></th><td class="infobox-data">172.22 K, 1.392 kPa<a href="#cite_note-4">[4]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Critical_point_(thermodynamics)" title="Critical point (thermodynamics)">Critical point</a></th><td class="infobox-data">416.9 K, 7.991 MPa </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Enthalpy_of_fusion" title="Enthalpy of fusion">Heat of fusion</a></th><td class="infobox-data">(Cl2) 6.406 <a href="/wiki/Kilojoule_per_mole" class="mw-redirect" title="Kilojoule per mole">kJ/mol</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Enthalpy_of_vaporization" title="Enthalpy of vaporization">Heat of vaporisation</a></th><td class="infobox-data">(Cl2) 20.41 kJ/mol </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Molar_heat_capacity" title="Molar heat capacity">Molar heat capacity</a></th><td class="infobox-data">(Cl2) 33.949 J/(mol·K) </td></tr><tr><td colspan="2" class="infobox-full-data"><a href="/wiki/Vapor_pressure" title="Vapor pressure">Vapour pressure</a><div style="position:relative; margin:0 auto; padding:0; text-align:initial; width:-moz-fit-content;width:-webkit-fit-content;width:fit-content;"> <table class="wikitable" style="text-align:center; font-size:90%; border-collapse:collapse; margin:0"> <tbody><tr> <th><abbr title="Pressure">P</abbr> (Pa) </th> <th>1 </th> <th>10 </th> <th>100 </th> <th>1 k </th> <th>10 k </th> <th>100 k </th></tr> <tr> <th>at <abbr title="Temperature">T</abbr> (K) </th> <td>128 </td> <td>139 </td> <td>153 </td> <td>170 </td> <td>197 </td> <td>239 </td></tr></tbody></table> </div></td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Atomic properties</th></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Oxidation_state" title="Oxidation state">Oxidation states</a></th><td class="infobox-data">common: −1, +1, +3, +5, +7 +2,<a href="#cite_note-GE28-5">[5]</a> +4,<a href="#cite_note-GE28-5">[5]</a> +6<a href="#cite_note-GE28-5">[5]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Electronegativity" title="Electronegativity">Electronegativity</a></th><td class="infobox-data">Pauling scale: 3.16 </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Ionization_energy" title="Ionization energy">Ionisation energies</a></th><td class="infobox-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>1st: 1251.2 kJ/mol </li><li>2nd: 2298 kJ/mol </li><li>3rd: 3822 kJ/mol </li><li>(<a href="/wiki/Molar_ionization_energies_of_the_elements#chlorine" title="Molar ionization energies of the elements">more</a>) </li></ul></div></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Covalent_radius" title="Covalent radius">Covalent radius</a></th><td class="infobox-data">102±4 <a href="/wiki/Picometre" title="Picometre">pm</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Van_der_Waals_radius" title="Van der Waals radius">Van der Waals radius</a></th><td class="infobox-data">175 pm </td></tr><tr><td colspan="2" class="infobox-full-data"><figure class="mw-default-size mw-halign-center" typeof="mw:File/Frameless"><a href="/wiki/File:17_(Cl_I)_NIST_ASD_emission_spectrum.png" class="mw-file-description"><img alt="Color lines in a spectral range" src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d1/17_%28Cl_I%29_NIST_ASD_emission_spectrum.png/240px-17_%28Cl_I%29_NIST_ASD_emission_spectrum.png" decoding="async" width="240" height="29" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d1/17_%28Cl_I%29_NIST_ASD_emission_spectrum.png/360px-17_%28Cl_I%29_NIST_ASD_emission_spectrum.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d1/17_%28Cl_I%29_NIST_ASD_emission_spectrum.png/480px-17_%28Cl_I%29_NIST_ASD_emission_spectrum.png 2x" data-file-width="4000" data-file-height="480" /></a><figcaption></figcaption></figure><a href="/wiki/Spectral_line" title="Spectral line">Spectral lines</a> of chlorine</td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Other properties</th></tr><tr><th scope="row" class="infobox-label">Natural occurrence</th><td class="infobox-data"><a href="/wiki/Primordial_nuclide" title="Primordial nuclide">primordial</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Crystal_structure" title="Crystal structure">Crystal structure</a></th><td class="infobox-data"> <a href="/wiki/Orthorhombic_crystal_system" title="Orthorhombic crystal system">orthorhombic</a> (<a href="/wiki/Pearson_symbol" title="Pearson symbol">oS8</a>)</td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Lattice_constant" title="Lattice constant">Lattice constants</a></th><td class="infobox-data"><div style="float:right;"><a href="/wiki/File:Orthorhombic.svg" class="mw-file-description"><img alt="Orthorhombic crystal structure for chlorine" src="//upload.wikimedia.org/wikipedia/commons/thumb/d/dd/Orthorhombic.svg/50px-Orthorhombic.svg.png" decoding="async" width="50" height="66" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/dd/Orthorhombic.svg/75px-Orthorhombic.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/dd/Orthorhombic.svg/100px-Orthorhombic.svg.png 2x" data-file-width="108" data-file-height="142" /></a></div>a = 630.80 pm b = 455.83 pm c = 815.49 pm (at triple point)<a href="#cite_note-Arblaster_2018-6">[6]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Thermal_conductivity" class="mw-redirect" title="Thermal conductivity">Thermal conductivity</a></th><td class="infobox-data">8.9×10−3 W/(m⋅K) </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Electrical_resistivity_and_conductivity" title="Electrical resistivity and conductivity">Electrical resistivity</a></th><td class="infobox-data">>10 Ω⋅m (at 20 °C) </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Magnetism" title="Magnetism">Magnetic ordering</a></th><td class="infobox-data"><a href="/wiki/Diamagnetic" class="mw-redirect" title="Diamagnetic">diamagnetic</a><a href="#cite_note-7">[7]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Magnetic_susceptibility" title="Magnetic susceptibility">Molar magnetic susceptibility</a></th><td class="infobox-data">−40.5×10−6 cm3/mol<a href="#cite_note-8">[8]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Speed_of_sound" title="Speed of sound">Speed of sound</a></th><td class="infobox-data">206 <a href="/wiki/Metre_per_second" title="Metre per second">m/s</a> (gas, at 0 °C)</td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/CAS_Registry_Number" title="CAS Registry Number">CAS Number</a></th><td class="infobox-data">Cl2: 7782-50-5 </td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">History</th></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Timeline_of_chemical_element_discoveries" class="mw-redirect" title="Timeline of chemical element discoveries">Discovery</a> and first isolation</th><td class="infobox-data"><a href="/wiki/Carl_Wilhelm_Scheele" title="Carl Wilhelm Scheele">Carl Wilhelm Scheele</a> (1774)</td></tr><tr><th scope="row" class="infobox-label">Recognized as an <a href="/wiki/Chemical_element" title="Chemical element">element</a> by</th><td class="infobox-data"><a href="/wiki/Humphry_Davy" title="Humphry Davy">Humphry Davy</a> (1808)</td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c"><a href="/wiki/Isotopes_of_chlorine" title="Isotopes of chlorine">Isotopes of chlorine</a><style data-mw-deduplicate="TemplateStyles:r1129693374">.mw-parser-output .hlist dl,.mw-parser-output .hlist ol,.mw-parser-output .hlist ul{margin:0;padding:0}.mw-parser-output .hlist dd,.mw-parser-output .hlist dt,.mw-parser-output .hlist li{margin:0;display:inline}.mw-parser-output .hlist.inline,.mw-parser-output .hlist.inline dl,.mw-parser-output .hlist.inline ol,.mw-parser-output .hlist.inline ul,.mw-parser-output .hlist dl dl,.mw-parser-output .hlist dl ol,.mw-parser-output .hlist dl ul,.mw-parser-output .hlist ol dl,.mw-parser-output .hlist ol ol,.mw-parser-output .hlist ol ul,.mw-parser-output .hlist ul dl,.mw-parser-output .hlist ul ol,.mw-parser-output .hlist ul ul{display:inline}.mw-parser-output .hlist .mw-empty-li{display:none}.mw-parser-output .hlist dt::after{content:": "}.mw-parser-output .hlist dd::after,.mw-parser-output .hlist li::after{content:" · ";font-weight:bold}.mw-parser-output .hlist dd:last-child::after,.mw-parser-output .hlist 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.navbar a>span,.mw-parser-output .navbar a>abbr{text-decoration:inherit}.mw-parser-output .navbar-mini abbr{font-variant:small-caps;border-bottom:none;text-decoration:none;cursor:inherit}.mw-parser-output .navbar-ct-full{font-size:114%;margin:0 7em}.mw-parser-output .navbar-ct-mini{font-size:114%;margin:0 4em}html.skin-theme-clientpref-night .mw-parser-output .navbar li a abbr{color:var(--color-base)!important}@media(prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .navbar li a abbr{color:var(--color-base)!important}}@media print{.mw-parser-output .navbar{display:none!important}}</style><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Infobox_chlorine_isotopes" title="Template:Infobox chlorine isotopes"><abbr title="View this template">v</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Infobox_chlorine_isotopes" title="Special:EditPage/Template:Infobox chlorine isotopes"><abbr title="Edit this template">e</abbr></a></li></ul></div></th></tr><tr><td colspan="2" class="infobox-full-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1257001546"></td></tr><tr><td colspan="2" class="infobox-full-data"> <table class="wikitable" style="text-align: center; vertical-align: middle; width: 100%; border-collapse: collapse; margin: 0; padding: 0;"> <tbody><tr> <th colspan="3">Main isotopes<a href="#cite_note-NUBASE2020-9">[9]</a> </th> <th colspan="2"><a href="/wiki/Radioactive_decay" title="Radioactive decay">Decay</a> </th></tr> <tr> <th> </th> <th style="padding: 0.1em;"><a href="/wiki/Natural_abundance" title="Natural abundance">abundance</a> </th> <th style="padding: 0.1em;"><a href="/wiki/Half-life" title="Half-life">half-life</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r886047488">(t1/2) </th> <th style="padding: 0.1em;"><a href="/wiki/Radioactive_decay#Types_of_decay" title="Radioactive decay">mode</a> </th> <th style="padding: 0.1em;"><a href="/wiki/Decay_product" title="Decay product">product</a> </th></tr> <tr> <th rowspan="1" style="vertical-align: top;">35Cl </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">76% </td> <td rowspan="1" colspan="3" style="vertical-align: top; text-align: left;"><a href="/wiki/Stable_isotope" class="mw-redirect" title="Stable isotope">stable</a> </td></tr> <tr> <th rowspan="2" style="vertical-align: top;"><a href="/wiki/Chlorine-36" title="Chlorine-36">36Cl</a> </th> <td rowspan="2" colspan="1" style="vertical-align: top; text-align: center;"><a href="/wiki/Trace_radioisotope" title="Trace radioisotope">trace</a> </td> <td rowspan="2" colspan="1" style="vertical-align: top; text-align: right;">3.01×105 y </td> <td style="text-align: left; vertical-align: top;"><a href="/wiki/Beta_minus_decay" class="mw-redirect" title="Beta minus decay">β−</a> </td> <td style="text-align: right; vertical-align: middle;"><a href="/wiki/Argon-36" class="mw-redirect" title="Argon-36">36Ar</a> </td></tr> <tr> <td style="text-align: left; vertical-align: top;"><a href="/wiki/Electron_capture" title="Electron capture">ε</a> </td> <td style="text-align: right; vertical-align: middle;"><a href="/wiki/Sulfur-36" class="mw-redirect" title="Sulfur-36">36S</a> </td></tr> <tr> <th rowspan="1" style="vertical-align: top;"><a href="/wiki/Chlorine-37" title="Chlorine-37">37Cl</a> </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">24% </td> <td rowspan="1" colspan="3" style="vertical-align: top; text-align: left;">stable </td></tr></tbody></table></td></tr><tr style="display:none"><td colspan="2"> </td></tr><tr><td colspan="2" class="infobox-below noprint" style="color:inherit; background:#fdff8c"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/9/96/Symbol_category_class.svg/16px-Symbol_category_class.svg.png" decoding="async" width="16" height="16" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/96/Symbol_category_class.svg/23px-Symbol_category_class.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/96/Symbol_category_class.svg/31px-Symbol_category_class.svg.png 2x" data-file-width="180" data-file-height="185" /> <a href="/wiki/Category:Chlorine" title="Category:Chlorine">Category: Chlorine</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist"><ul><li class="nv-view"><a href="/wiki/Template:Infobox_chlorine" title="Template:Infobox chlorine">view</a></li><li class="nv-talk"><a href="/wiki/Template_talk:Infobox_chlorine" title="Template talk:Infobox chlorine">talk</a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Infobox_chlorine" title="Special:EditPage/Template:Infobox chlorine">edit</a></li></ul></div> | <a href="/wiki/List_of_data_references_for_chemical_elements" title="List of data references for chemical elements">references</a></td></tr></tbody></table> Chlorine is a <a href="/wiki/Chemical_element" title="Chemical element">chemical element</a>; it has <a href="/wiki/Symbol_(chemistry)" class="mw-redirect" title="Symbol (chemistry)">symbol</a> Cl and <a href="/wiki/Atomic_number" title="Atomic number">atomic number</a> 17. The second-lightest of the <a href="/wiki/Halogen" title="Halogen">halogens</a>, it appears between <a href="/wiki/Fluorine" title="Fluorine">fluorine</a> and <a href="/wiki/Bromine" title="Bromine">bromine</a> in the periodic table and its properties are mostly intermediate between them. Chlorine is a yellow-green gas at room temperature. It is an extremely reactive element and a strong <a href="/wiki/Oxidizing_agent" title="Oxidizing agent">oxidising agent</a>: among the elements, it has the highest <a href="/wiki/Electron_affinity" title="Electron affinity">electron affinity</a> and the third-highest <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a> on the revised <a href="/wiki/Electronegativity#Pauling_electronegativity" title="Electronegativity">Pauling scale</a>, behind only <a href="/wiki/Oxygen" title="Oxygen">oxygen</a> and fluorine. Chlorine played an important role in the experiments conducted by medieval <a href="/wiki/Alchemy" title="Alchemy">alchemists</a>, which commonly involved the heating of chloride <a href="/wiki/Salt_(chemistry)" title="Salt (chemistry)">salts</a> like <a href="/wiki/Ammonium_chloride" title="Ammonium chloride">ammonium chloride</a> (<a href="/wiki/Sal_ammoniac" class="mw-redirect" title="Sal ammoniac">sal ammoniac</a>) and <a href="/wiki/Sodium_chloride" title="Sodium chloride">sodium chloride</a> (<a href="/wiki/Common_salt" class="mw-redirect" title="Common salt">common salt</a>), producing various chemical substances containing chlorine such as <a href="/wiki/Hydrogen_chloride" title="Hydrogen chloride">hydrogen chloride</a>, <a href="/wiki/Mercury(II)_chloride" title="Mercury(II) chloride">mercury(II) chloride</a> (corrosive sublimate), and <a href="/wiki/Aqua_regia" title="Aqua regia">aqua regia</a>. However, the nature of free chlorine gas as a separate substance was only recognised around 1630 by <a href="/wiki/Jan_Baptist_van_Helmont" title="Jan Baptist van Helmont">Jan Baptist van Helmont</a>. <a href="/wiki/Carl_Wilhelm_Scheele" title="Carl Wilhelm Scheele">Carl Wilhelm Scheele</a> wrote a description of chlorine gas in 1774, supposing it to be an <a href="/wiki/Oxide" title="Oxide">oxide</a> of a new element. In 1809, chemists suggested that the gas might be a pure element, and this was confirmed by <a href="/wiki/Sir_Humphry_Davy" class="mw-redirect" title="Sir Humphry Davy">Sir Humphry Davy</a> in 1810, who named it after the <a href="/wiki/Ancient_Greek_language" class="mw-redirect" title="Ancient Greek language">Ancient Greek</a> χλωρός (khlōrós, "pale green") because of its colour. Because of its great reactivity, all chlorine in the Earth's crust is in the form of <a href="/wiki/Ion" title="Ion">ionic</a> <a href="/wiki/Chloride" title="Chloride">chloride</a> compounds, which includes table salt. It is the <a href="/wiki/Abundance_of_elements_in_Earth%27s_crust" title="Abundance of elements in Earth's crust">second-most abundant</a> halogen (after fluorine) and 20th most abundant element in Earth's crust. These crystal deposits are nevertheless dwarfed by the huge reserves of chloride in seawater. Elemental chlorine is commercially produced from <a href="/wiki/Brine" title="Brine">brine</a> by <a href="/wiki/Electrolysis" title="Electrolysis">electrolysis</a>, predominantly in the <a href="/wiki/Chloralkali_process" title="Chloralkali process">chloralkali process</a>. The high oxidising potential of elemental chlorine led to the development of commercial <a href="/wiki/Bleach_(chemical)" class="mw-redirect" title="Bleach (chemical)">bleaches</a> and <a href="/wiki/Disinfectant" title="Disinfectant">disinfectants</a>, and a <a href="/wiki/Reagent" title="Reagent">reagent</a> for many processes in the chemical industry. Chlorine is used in the manufacture of a wide range of consumer products, about two-thirds of them organic chemicals such as <a href="/wiki/Polyvinyl_chloride" title="Polyvinyl chloride">polyvinyl chloride</a> (PVC), many intermediates for the production of <a href="/wiki/Plastics" class="mw-redirect" title="Plastics">plastics</a>, and other end products which do not contain the element. As a common disinfectant, elemental chlorine and chlorine-generating compounds are used more directly in <a href="/wiki/Swimming_pool" title="Swimming pool">swimming pools</a> to keep them <a href="/wiki/Swimming_pool_sanitation" title="Swimming pool sanitation">sanitary</a>. Elemental chlorine at high <a href="/wiki/Concentration" title="Concentration">concentration</a> is extremely dangerous, and <a href="/wiki/Poisonous" class="mw-redirect" title="Poisonous">poisonous</a> to most living organisms. As a <a href="/wiki/Chemical_warfare" title="Chemical warfare">chemical warfare</a> agent, chlorine was first used in <a href="/wiki/World_War_I" title="World War I">World War I</a> as a <a href="/wiki/Poison_gas" class="mw-redirect" title="Poison gas">poison gas</a> weapon. In the form of chloride <a href="/wiki/Ions" class="mw-redirect" title="Ions">ions</a>, chlorine is necessary to all known species of life. Other types of chlorine compounds are rare in living organisms, and artificially produced chlorinated organics range from inert to toxic. In the <a href="/wiki/Upper_atmosphere" title="Upper atmosphere">upper atmosphere</a>, chlorine-containing organic molecules such as <a href="/wiki/Chlorofluorocarbon" title="Chlorofluorocarbon">chlorofluorocarbons</a> have been implicated in <a href="/wiki/Ozone_depletion" title="Ozone depletion">ozone depletion</a>. Small quantities of elemental chlorine are generated by oxidation of chloride ions in <a href="/wiki/Neutrophil" title="Neutrophil">neutrophils</a> as part of an <a href="/wiki/Immune_system" title="Immune system">immune system</a> response against bacteria. <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="History">History</h2></div> The most common compound of chlorine, sodium chloride, has been known since ancient times; archaeologists have found evidence that <a href="/wiki/Rock_salt" class="mw-redirect" title="Rock salt">rock salt</a> was used as early as 3000 BC and <a href="/wiki/Brine" title="Brine">brine</a> as early as 6000 BC.<a href="#cite_note-10">[10]</a> <div class="mw-heading mw-heading3"><h3 id="Early_discoveries">Early discoveries</h3></div> Around 900, the authors of the Arabic writings attributed to <a href="/wiki/Jabir_ibn_Hayyan" title="Jabir ibn Hayyan">Jabir ibn Hayyan</a> (Latin: Geber) and the Persian physician and alchemist <a href="/wiki/Abu_Bakr_al-Razi" title="Abu Bakr al-Razi">Abu Bakr al-Razi</a> (<abbr title="circa">c.</abbr> 865–925, Latin: Rhazes) were experimenting with <a href="/wiki/Sal_ammoniac" class="mw-redirect" title="Sal ammoniac">sal ammoniac</a> (<a href="/wiki/Ammonium_chloride" title="Ammonium chloride">ammonium chloride</a>), which when it was distilled together with <a href="/wiki/Vitriol" title="Vitriol">vitriol</a> (hydrated <a href="/wiki/Sulfates" class="mw-redirect" title="Sulfates">sulfates</a> of various metals) produced <a href="/wiki/Hydrogen_chloride" title="Hydrogen chloride">hydrogen chloride</a>.<a href="#cite_note-11">[11]</a> However, it appears that in these early experiments with chloride <a href="/wiki/Salt_(chemistry)" title="Salt (chemistry)">salts</a>, the gaseous products were discarded, and hydrogen chloride may have been produced many times before it was discovered that it can be put to chemical use.<a href="#cite_note-12">[12]</a> One of the first such uses was the synthesis of <a href="/wiki/Mercury(II)_chloride" title="Mercury(II) chloride">mercury(II) chloride</a> (corrosive sublimate), whose production from the heating of <a href="/wiki/Mercury_(element)" title="Mercury (element)">mercury</a> either with <a href="/wiki/Alum" title="Alum">alum</a> and ammonium chloride or with vitriol and sodium chloride was first described in the De aluminibus et salibus ("On Alums and Salts", an eleventh- or twelfth century Arabic text falsely attributed to Abu Bakr al-Razi and <a href="/wiki/Latin_translations_of_the_12th_century" title="Latin translations of the 12th century">translated into Latin in the second half of the twelfth century</a> by <a href="/wiki/Gerard_of_Cremona" title="Gerard of Cremona">Gerard of Cremona</a>, 1144–1187).<a href="#cite_note-13">[13]</a> Another important development was the discovery by <a href="/wiki/Pseudo-Geber" title="Pseudo-Geber">pseudo-Geber</a> (in the De inventione veritatis, "On the Discovery of Truth", after c. 1300) that by adding ammonium chloride to <a href="/wiki/Nitric_acid" title="Nitric acid">nitric acid</a>, a strong solvent capable of dissolving gold (i.e., <a href="/wiki/Aqua_regia" title="Aqua regia">aqua regia</a>) could be produced.<a href="#cite_note-14">[14]</a> Although aqua regia is an unstable mixture that continually gives off fumes containing free chlorine gas, this chlorine gas appears to have been ignored until c. 1630, when its nature as a separate gaseous substance was recognised by the <a href="/wiki/Duchy_of_Brabant" title="Duchy of Brabant">Brabantian</a> chemist and physician <a href="/wiki/Jan_Baptist_van_Helmont" title="Jan Baptist van Helmont">Jan Baptist van Helmont</a>.<a href="#cite_note-Greenwood789-15">[15]</a><a href="#cite_note-16">[en 1]</a> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:PSM_V31_D740_Carl_Wilhelm_Scheele.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4d/PSM_V31_D740_Carl_Wilhelm_Scheele.jpg/140px-PSM_V31_D740_Carl_Wilhelm_Scheele.jpg" decoding="async" width="140" height="184" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4d/PSM_V31_D740_Carl_Wilhelm_Scheele.jpg/210px-PSM_V31_D740_Carl_Wilhelm_Scheele.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/4d/PSM_V31_D740_Carl_Wilhelm_Scheele.jpg/280px-PSM_V31_D740_Carl_Wilhelm_Scheele.jpg 2x" data-file-width="1665" data-file-height="2184" /></a><figcaption><a href="/wiki/Carl_Wilhelm_Scheele" title="Carl Wilhelm Scheele">Carl Wilhelm Scheele</a>, discoverer of chlorine</figcaption></figure> <div class="mw-heading mw-heading3"><h3 id="Isolation">Isolation</h3></div> The element was first studied in detail in 1774 by Swedish chemist <a href="/wiki/Carl_Wilhelm_Scheele" title="Carl Wilhelm Scheele">Carl Wilhelm Scheele</a>, and he is credited with the discovery.<a href="#cite_note-17">[16]</a><a href="#cite_note-krogt-18">[17]</a> Scheele produced chlorine by reacting <a href="/wiki/Manganese_dioxide" title="Manganese dioxide">MnO2</a> (as the mineral <a href="/wiki/Pyrolusite" title="Pyrolusite">pyrolusite</a>) with HCl:<a href="#cite_note-Greenwood789-15">[15]</a> <dl><dd>4 HCl + MnO2 → MnCl2 + 2 H2O + Cl2</dd></dl> Scheele observed several of the properties of chlorine: the bleaching effect on <a href="/wiki/Litmus_test_(chemistry)" class="mw-redirect" title="Litmus test (chemistry)">litmus</a>, the deadly effect on insects, the yellow-green colour, and the smell similar to <a href="/wiki/Aqua_regia" title="Aqua regia">aqua regia</a>.<a href="#cite_note-Greenwood792-19">[18]</a> He called it "dephlogisticated muriatic acid air" since it is a gas (then called "airs") and it came from <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">hydrochloric acid</a> (then known as "muriatic acid").<a href="#cite_note-krogt-18">[17]</a> He failed to establish chlorine as an element.<a href="#cite_note-krogt-18">[17]</a> Common chemical theory at that time held that an acid is a compound that contains oxygen (remnants of this survive in the German and Dutch names of <a href="/wiki/Oxygen" title="Oxygen">oxygen</a>: sauerstoff or zuurstof, both translating into English as acid substance), so a number of chemists, including <a href="/wiki/Claude_Berthollet" class="mw-redirect" title="Claude Berthollet">Claude Berthollet</a>, suggested that Scheele's dephlogisticated muriatic acid air must be a combination of oxygen and the yet undiscovered element, muriaticum.<a href="#cite_note-20">[19]</a><a href="#cite_note-Weeks-21">[20]</a> In 1809, <a href="/wiki/Joseph_Louis_Gay-Lussac" title="Joseph Louis Gay-Lussac">Joseph Louis Gay-Lussac</a> and <a href="/wiki/Louis-Jacques_Th%C3%A9nard" class="mw-redirect" title="Louis-Jacques Thénard">Louis-Jacques Thénard</a> tried to decompose dephlogisticated muriatic acid air by reacting it with charcoal to release the free element muriaticum (and carbon dioxide).<a href="#cite_note-krogt-18">[17]</a> They did not succeed and published a report in which they considered the possibility that dephlogisticated muriatic acid air is an element, but were not convinced.<a href="#cite_note-22">[21]</a> In 1810, <a href="/wiki/Sir_Humphry_Davy" class="mw-redirect" title="Sir Humphry Davy">Sir Humphry Davy</a> tried the same experiment again, and concluded that the substance was an element, and not a compound.<a href="#cite_note-krogt-18">[17]</a> He announced his results to the Royal Society on 15 November that year.<a href="#cite_note-Greenwood789-15">[15]</a> At that time, he named this new element "chlorine", from the Greek word χλωρος (chlōros, "green-yellow"), in reference to its colour.<a href="#cite_note-23">[22]</a> The name "<a href="/wiki/Halogen" title="Halogen">halogen</a>", meaning "salt producer", was originally used for chlorine in 1811 by <a href="/wiki/Johann_Salomo_Christoph_Schweigger" class="mw-redirect" title="Johann Salomo Christoph Schweigger">Johann Salomo Christoph Schweigger</a>.<a href="#cite_note-24">[23]</a> This term was later used as a generic term to describe all the elements in the chlorine family (fluorine, bromine, iodine), after a suggestion by <a href="/wiki/J%C3%B6ns_Jakob_Berzelius" class="mw-redirect" title="Jöns Jakob Berzelius">Jöns Jakob Berzelius</a> in 1826.<a href="#cite_note-25">[24]</a><a href="#cite_note-26">[25]</a> In 1823, <a href="/wiki/Michael_Faraday" title="Michael Faraday">Michael Faraday</a> liquefied chlorine for the first time,<a href="#cite_note-27">[26]</a><a href="#cite_note-28">[27]</a><a href="#cite_note-29">[28]</a> and demonstrated that what was then known as "solid chlorine" had a structure of <a href="/wiki/Clathrate_hydrate" title="Clathrate hydrate">chlorine hydrate</a> (Cl2·H2O).<a href="#cite_note-Greenwood789-15">[15]</a> <div class="mw-heading mw-heading3"><h3 id="Later_uses">Later uses</h3></div> Chlorine gas was first used by French chemist <a href="/wiki/Claude_Louis_Berthollet" title="Claude Louis Berthollet">Claude Berthollet</a> to bleach textiles in 1785.<a href="#cite_note-encyc-30">[29]</a><a href="#cite_note-Cotton-31">[30]</a> Modern bleaches resulted from further work by Berthollet, who first produced <a href="/wiki/Sodium_hypochlorite" title="Sodium hypochlorite">sodium hypochlorite</a> in 1789 in his laboratory in the town of <a href="/wiki/Javel_-_Andr%C3%A9_Citro%C3%ABn_(Paris_M%C3%A9tro)" class="mw-redirect" title="Javel - André Citroën (Paris Métro)">Javel</a> (now part of <a href="/wiki/Paris" title="Paris">Paris</a>, France), by passing chlorine gas through a solution of sodium carbonate. The resulting liquid, known as "Eau de Javel" ("<a href="/wiki/Javel_water" class="mw-redirect" title="Javel water">Javel water</a>"), was a weak solution of <a href="/wiki/Sodium_hypochlorite" title="Sodium hypochlorite">sodium hypochlorite</a>. This process was not very efficient, and alternative production methods were sought. Scottish chemist and industrialist <a href="/wiki/Charles_Tennant" title="Charles Tennant">Charles Tennant</a> first produced a solution of <a href="/wiki/Calcium_hypochlorite" title="Calcium hypochlorite">calcium hypochlorite</a> ("chlorinated lime"), then solid calcium hypochlorite (bleaching powder).<a href="#cite_note-encyc-30">[29]</a> These compounds produced low levels of elemental chlorine and could be more efficiently transported than sodium hypochlorite, which remained as dilute solutions because when purified to eliminate water, it became a dangerously powerful and unstable oxidizer. Near the end of the nineteenth century, E. S. Smith patented a method of sodium hypochlorite production involving electrolysis of <a href="/wiki/Brine" title="Brine">brine</a> to produce <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">sodium hydroxide</a> and chlorine gas, which then mixed to form sodium hypochlorite.<a href="#cite_note-32">[31]</a> This is known as the <a href="/wiki/Chloralkali_process" title="Chloralkali process">chloralkali process</a>, first introduced on an industrial scale in 1892, and now the source of most elemental chlorine and sodium hydroxide.<a href="#cite_note-Greenwood798-33">[32]</a> In 1884 Chemischen Fabrik Griesheim of Germany developed another <a href="/wiki/Chloralkali_process" title="Chloralkali process">chloralkali process</a> which entered commercial production in 1888.<a href="#cite_note-34">[33]</a> Elemental chlorine solutions dissolved in <a href="/wiki/Base_(chemistry)" title="Base (chemistry)">chemically basic</a> water (sodium and <a href="/wiki/Calcium_hypochlorite" title="Calcium hypochlorite">calcium hypochlorite</a>) were first used as anti-<a href="/wiki/Putrefaction" title="Putrefaction">putrefaction</a> agents and <a href="/wiki/Disinfectant" title="Disinfectant">disinfectants</a> in the 1820s, in France, long before the establishment of the <a href="/wiki/Germ_theory_of_disease" title="Germ theory of disease">germ theory of disease</a>. This practice was pioneered by <a href="/wiki/Antoine-Germain_Labarraque" class="mw-redirect" title="Antoine-Germain Labarraque">Antoine-Germain Labarraque</a>, who adapted Berthollet's "Javel water" bleach and other chlorine preparations.<a href="#cite_note-bouvet-35">[34]</a> Elemental chlorine has since served a continuous function in topical <a href="/wiki/Antiseptic" title="Antiseptic">antisepsis</a> (wound irrigation solutions and the like) and public sanitation, particularly in swimming and drinking water.<a href="#cite_note-Greenwood792-19">[18]</a> Chlorine gas was first used as a weapon on April 22, 1915, at the <a href="/wiki/Second_Battle_of_Ypres" title="Second Battle of Ypres">Second Battle of Ypres</a> by the <a href="/wiki/German_Army_(German_Empire)" class="mw-redirect" title="German Army (German Empire)">German Army</a>.<a href="#cite_note-36">[35]</a><a href="#cite_note-37">[36]</a> The effect on the allies was devastating because the existing <a href="/wiki/WWI_gas_mask" class="mw-redirect" title="WWI gas mask">gas masks</a> were difficult to deploy and had not been broadly distributed.<a href="#cite_note-38">[37]</a><a href="#cite_note-39">[38]</a> <div class="mw-heading mw-heading2"><h2 id="Properties">Properties</h2></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Chlorine_liquid_in_an_ampoule.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/78/Chlorine_liquid_in_an_ampoule.jpg/220px-Chlorine_liquid_in_an_ampoule.jpg" decoding="async" width="220" height="216" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/78/Chlorine_liquid_in_an_ampoule.jpg/330px-Chlorine_liquid_in_an_ampoule.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/78/Chlorine_liquid_in_an_ampoule.jpg/440px-Chlorine_liquid_in_an_ampoule.jpg 2x" data-file-width="3513" data-file-height="3442" /></a><figcaption>Chlorine, liquefied under a pressure of 7.4 bar at room temperature, displayed in a quartz ampule embedded in <a href="/wiki/Poly(methyl_methacrylate)" title="Poly(methyl methacrylate)">acrylic glass</a></figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Chlorine.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e6/Chlorine.jpg/220px-Chlorine.jpg" decoding="async" width="220" height="293" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/e6/Chlorine.jpg/330px-Chlorine.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/e6/Chlorine.jpg/440px-Chlorine.jpg 2x" data-file-width="2304" data-file-height="3072" /></a><figcaption>Gaseous chlorine stored inside a 500-mL water bottle. It is not recommended to store chlorine in this manner.</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Die_chemischen_elemente_cl.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/18/Die_chemischen_elemente_cl.jpg/220px-Die_chemischen_elemente_cl.jpg" decoding="async" width="220" height="156" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/18/Die_chemischen_elemente_cl.jpg/330px-Die_chemischen_elemente_cl.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/18/Die_chemischen_elemente_cl.jpg/440px-Die_chemischen_elemente_cl.jpg 2x" data-file-width="1081" data-file-height="765" /></a><figcaption>Solid chlorine at −150 °C</figcaption></figure> Chlorine is the second <a href="/wiki/Halogen" title="Halogen">halogen</a>, being a <a href="/wiki/Nonmetal_(chemistry)" class="mw-redirect" title="Nonmetal (chemistry)">nonmetal</a> in group 17 of the periodic table. Its properties are thus similar to <a href="/wiki/Fluorine" title="Fluorine">fluorine</a>, <a href="/wiki/Bromine" title="Bromine">bromine</a>, and <a href="/wiki/Iodine" title="Iodine">iodine</a>, and are largely intermediate between those of the first two. Chlorine has the electron configuration [Ne]3s23p5, with the seven electrons in the third and outermost shell acting as its <a href="/wiki/Valence_electron" title="Valence electron">valence electrons</a>. Like all halogens, it is thus one electron short of a full octet, and is hence a strong oxidising agent, reacting with many elements in order to complete its outer shell.<a href="#cite_note-Greenwood800-40">[39]</a> Corresponding to <a href="/wiki/Periodic_trend" class="mw-redirect" title="Periodic trend">periodic trends</a>, it is intermediate in <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a> between fluorine and bromine (F: 3.98, Cl: 3.16, Br: 2.96, I: 2.66), and is less reactive than fluorine and more reactive than bromine. It is also a weaker oxidising agent than fluorine, but a stronger one than bromine. Conversely, the <a href="/wiki/Chloride" title="Chloride">chloride</a> ion is a weaker reducing agent than bromide, but a stronger one than fluoride.<a href="#cite_note-Greenwood800-40">[39]</a> It is intermediate in <a href="/wiki/Atomic_radius" title="Atomic radius">atomic radius</a> between fluorine and bromine, and this leads to many of its atomic properties similarly continuing the trend from iodine to bromine upward, such as first <a href="/wiki/Ionisation_energy" class="mw-redirect" title="Ionisation energy">ionisation energy</a>, <a href="/wiki/Electron_affinity" title="Electron affinity">electron affinity</a>, enthalpy of dissociation of the X2 molecule (X = Cl, Br, I), ionic radius, and X–X bond length. (Fluorine is anomalous due to its small size.)<a href="#cite_note-Greenwood800-40">[39]</a> All four stable halogens experience intermolecular <a href="/wiki/Van_der_Waals_force" title="Van der Waals force">van der Waals forces</a> of attraction, and their strength increases together with the number of electrons among all homonuclear diatomic halogen molecules. Thus, the melting and boiling points of chlorine are intermediate between those of fluorine and bromine: chlorine melts at −101.0 °C and boils at −34.0 °C. As a result of the increasing molecular weight of the halogens down the group, the density and heats of fusion and vaporisation of chlorine are again intermediate between those of bromine and fluorine, although all their heats of vaporisation are fairly low (leading to high volatility) thanks to their diatomic molecular structure.<a href="#cite_note-Greenwood800-40">[39]</a> The halogens darken in colour as the group is descended: thus, while fluorine is a pale yellow gas, chlorine is distinctly yellow-green. This trend occurs because the wavelengths of visible light absorbed by the halogens increase down the group.<a href="#cite_note-Greenwood800-40">[39]</a> Specifically, the colour of a halogen, such as chlorine, results from the <a href="/wiki/Atomic_electron_transition" title="Atomic electron transition">electron transition</a> between the <a href="/wiki/HOMO/LUMO" class="mw-redirect" title="HOMO/LUMO">highest occupied</a> antibonding πg molecular orbital and the lowest vacant antibonding σu molecular orbital.<a href="#cite_note-Greenwood804-41">[40]</a> The colour fades at low temperatures, so that solid chlorine at −195 °C is almost colourless.<a href="#cite_note-Greenwood800-40">[39]</a> Like solid bromine and iodine, solid chlorine crystallises in the <a href="/wiki/Orthorhombic_crystal_system" title="Orthorhombic crystal system">orthorhombic crystal system</a>, in a layered lattice of Cl2 molecules. The Cl–Cl distance is 198 pm (close to the gaseous Cl–Cl distance of 199 pm) and the Cl···Cl distance between molecules is 332 pm within a layer and 382 pm between layers (compare the van der Waals radius of chlorine, 180 pm). This structure means that chlorine is a very poor conductor of electricity, and indeed its conductivity is so low as to be practically unmeasurable.<a href="#cite_note-Greenwood800-40">[39]</a> <div class="mw-heading mw-heading3"><h3 id="Isotopes">Isotopes</h3></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Isotopes_of_chlorine" title="Isotopes of chlorine">Isotopes of chlorine</a></div> Chlorine has two stable isotopes, 35Cl and 37Cl. These are its only two natural isotopes occurring in quantity, with 35Cl making up 76% of natural chlorine and 37Cl making up the remaining 24%. Both are synthesised in stars in the <a href="/wiki/Oxygen-burning_process" title="Oxygen-burning process">oxygen-burning</a> and <a href="/wiki/Silicon-burning_process" title="Silicon-burning process">silicon-burning processes</a>.<a href="#cite_note-Cameron-42">[41]</a> Both have nuclear spin 3/2+ and thus may be used for <a href="/wiki/Nuclear_magnetic_resonance" title="Nuclear magnetic resonance">nuclear magnetic resonance</a>, although the spin magnitude being greater than 1/2 results in non-spherical nuclear charge distribution and thus resonance broadening as a result of a nonzero <a href="/wiki/Nuclear_quadrupole_moment" class="mw-redirect" title="Nuclear quadrupole moment">nuclear quadrupole moment</a> and resultant quadrupolar relaxation. The other chlorine isotopes are all radioactive, with <a href="/wiki/Half-life" title="Half-life">half-lives</a> too short to occur in nature <a href="/wiki/Primordial_element" class="mw-redirect" title="Primordial element">primordially</a>. Of these, the most commonly used in the laboratory are 36Cl (t1/2 = 3.0×105 y) and 38Cl (t1/2 = 37.2 min), which may be produced from the <a href="/wiki/Neutron_activation" title="Neutron activation">neutron activation</a> of natural chlorine.<a href="#cite_note-Greenwood800-40">[39]</a> The most stable chlorine radioisotope is 36Cl. The primary decay mode of isotopes lighter than 35Cl is <a href="/wiki/Electron_capture" title="Electron capture">electron capture</a> to isotopes of <a href="/wiki/Sulfur" title="Sulfur">sulfur</a>; that of isotopes heavier than 37Cl is <a href="/wiki/Beta_decay" title="Beta decay">beta decay</a> to isotopes of <a href="/wiki/Argon" title="Argon">argon</a>; and 36Cl may decay by either mode to stable 36S or 36Ar.<a href="#cite_note-NUBASE-43">[42]</a> <a href="/wiki/Chlorine-36" title="Chlorine-36">36Cl</a> occurs in trace quantities in nature as a <a href="/wiki/Cosmogenic_nuclide" title="Cosmogenic nuclide">cosmogenic nuclide</a> in a ratio of about (7–10) × 10−13 to 1 with stable chlorine isotopes: it is produced in the atmosphere by <a href="/wiki/Spallation" title="Spallation">spallation</a> of 36<a href="/wiki/Argon" title="Argon">Ar</a> by interactions with <a href="/wiki/Cosmic_ray" title="Cosmic ray">cosmic ray</a> <a href="/wiki/Proton" title="Proton">protons</a>. In the top meter of the <a href="/wiki/Lithosphere" title="Lithosphere">lithosphere</a>, 36Cl is generated primarily by <a href="/wiki/Thermal_neutron" class="mw-redirect" title="Thermal neutron">thermal neutron</a> activation of 35Cl and spallation of 39<a href="/wiki/Potassium" title="Potassium">K</a> and 40<a href="/wiki/Calcium" title="Calcium">Ca</a>. In the subsurface environment, <a href="/wiki/Muon_capture" title="Muon capture">muon capture</a> by 40<a href="/wiki/Calcium" title="Calcium">Ca</a> becomes more important as a way to generate 36Cl.<a href="#cite_note-Zreda-44">[43]</a><a href="#cite_note-45">[44]</a> <div class="mw-heading mw-heading2"><h2 id="Chemistry_and_compounds">Chemistry and compounds</h2></div> <table class="wikitable" style="float:right; margin-top:0; margin-left:1em; text-align:center; font-size:10pt; line-height:11pt; width:25%;"> <caption style="margin-bottom: 5px;">Halogen bond energies (kJ/mol)<a href="#cite_note-Greenwood804-41">[40]</a> </caption> <tbody><tr> <th>X </th> <th>XX </th> <th>HX </th> <th>BX3 </th> <th>AlX3 </th> <th>CX4 </th></tr> <tr> <th>F </th> <td>159 </td> <td>574 </td> <td>645 </td> <td>582 </td> <td>456 </td></tr> <tr> <th>Cl </th> <td>243 </td> <td>428 </td> <td>444 </td> <td>427 </td> <td>327 </td></tr> <tr> <th>Br </th> <td>193 </td> <td>363 </td> <td>368 </td> <td>360 </td> <td>272 </td></tr> <tr> <th>I </th> <td>151 </td> <td>294 </td> <td>272 </td> <td>285 </td> <td>239 </td></tr></tbody></table> Chlorine is intermediate in reactivity between fluorine and bromine, and is one of the most reactive elements. Chlorine is a weaker oxidising agent than fluorine but a stronger one than bromine or iodine. This can be seen from the <a href="/wiki/Standard_electrode_potential" title="Standard electrode potential">standard electrode potentials</a> of the X2/X− couples (F, +2.866  V; Cl, +1.395 V; Br, +1.087  V; I, +0.615 V; <a href="/wiki/Astatine" title="Astatine">At</a>, approximately +0.3  V). However, this trend is not shown in the bond energies because fluorine is singular due to its small size, low polarisability, and inability to show <a href="/wiki/Hypervalence" class="mw-redirect" title="Hypervalence">hypervalence</a>. As another difference, chlorine has a significant chemistry in positive oxidation states while fluorine does not. Chlorination often leads to higher oxidation states than bromination or iodination but lower oxidation states than fluorination. Chlorine tends to react with compounds including M–M, M–H, or M–C bonds to form M–Cl bonds.<a href="#cite_note-Greenwood804-41">[40]</a> Given that E°(<style data-mw-deduplicate="TemplateStyles:r1214402035">.mw-parser-output .sfrac{white-space:nowrap}.mw-parser-output .sfrac.tion,.mw-parser-output .sfrac .tion{display:inline-block;vertical-align:-0.5em;font-size:85%;text-align:center}.mw-parser-output .sfrac .num{display:block;line-height:1em;margin:0.0em 0.1em;border-bottom:1px solid}.mw-parser-output .sfrac .den{display:block;line-height:1em;margin:0.1em 0.1em}.mw-parser-output .sr-only{border:0;clip:rect(0,0,0,0);clip-path:polygon(0px 0px,0px 0px,0px 0px);height:1px;margin:-1px;overflow:hidden;padding:0;position:absolute;width:1px}</style>⁠1/2⁠O2/H2O) = +1.229 V, which is less than +1.395 V, it would be expected that chlorine should be able to oxidise water to oxygen and hydrochloric acid. However, the kinetics of this reaction are unfavorable, and there is also a bubble <a href="/wiki/Overpotential" title="Overpotential">overpotential</a> effect to consider, so that electrolysis of aqueous chloride solutions evolves chlorine gas and not oxygen gas, a fact that is very useful for the industrial production of chlorine.<a href="#cite_note-Greenwood853-46">[45]</a> <div class="mw-heading mw-heading3"><h3 id="Hydrogen_chloride">Hydrogen chloride</h3></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:DCl_Neutron_powder.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/DCl_Neutron_powder.png/400px-DCl_Neutron_powder.png" decoding="async" width="400" height="381" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/DCl_Neutron_powder.png/600px-DCl_Neutron_powder.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fa/DCl_Neutron_powder.png/800px-DCl_Neutron_powder.png 2x" data-file-width="871" data-file-height="830" /></a><figcaption>Structure of solid deuterium chloride, with D···Cl hydrogen bonds</figcaption></figure> The simplest chlorine compound is <a href="/wiki/Hydrogen_chloride" title="Hydrogen chloride">hydrogen chloride</a>, HCl, a major chemical in industry as well as in the laboratory, both as a gas and dissolved in water as <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">hydrochloric acid</a>. It is often produced by burning hydrogen gas in chlorine gas, or as a byproduct of chlorinating <a href="/wiki/Hydrocarbon" title="Hydrocarbon">hydrocarbons</a>. Another approach is to treat <a href="/wiki/Sodium_chloride" title="Sodium chloride">sodium chloride</a> with concentrated <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> to produce hydrochloric acid, also known as the "salt-cake" process:<a href="#cite_note-Greenwood809-47">[46]</a> <dl><dd>NaCl + H2SO4 150 °C⟶  NaHSO4 + HCl</dd> <dd>NaCl + NaHSO4 540–600 °C⟶  Na2SO4 + HCl</dd></dl> In the laboratory, hydrogen chloride gas may be made by drying the acid with concentrated sulfuric acid. Deuterium chloride, DCl, may be produced by reacting <a href="/wiki/Benzoyl_chloride" title="Benzoyl chloride">benzoyl chloride</a> with <a href="/wiki/Heavy_water" title="Heavy water">heavy water</a> (D2O).<a href="#cite_note-Greenwood809-47">[46]</a> At room temperature, hydrogen chloride is a colourless gas, like all the hydrogen halides apart from <a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">hydrogen fluoride</a>, since hydrogen cannot form strong <a href="/wiki/Hydrogen_bond" title="Hydrogen bond">hydrogen bonds</a> to the larger electronegative chlorine atom; however, weak hydrogen bonding is present in solid crystalline hydrogen chloride at low temperatures, similar to the hydrogen fluoride structure, before disorder begins to prevail as the temperature is raised.<a href="#cite_note-Greenwood809-47">[46]</a> Hydrochloric acid is a strong acid (pKa = −7) because the hydrogen-chlorine bonds are too weak to inhibit dissociation. The HCl/H2O system has many hydrates HCl·nH2O for n = 1, 2, 3, 4, and 6. Beyond a 1:1 mixture of HCl and H2O, the system separates completely into two separate liquid phases. Hydrochloric acid forms an <a href="/wiki/Azeotrope" title="Azeotrope">azeotrope</a> with boiling point 108.58 °C at 20.22 g HCl per 100 g solution; thus hydrochloric acid cannot be concentrated beyond this point by distillation.<a href="#cite_note-Greenwood812-48">[47]</a> Unlike hydrogen fluoride, anhydrous liquid hydrogen chloride is difficult to work with as a solvent, because its boiling point is low, it has a small liquid range, its <a href="/wiki/Dielectric_constant" class="mw-redirect" title="Dielectric constant">dielectric constant</a> is low and it does not dissociate appreciably into H2Cl+ and HCl− 2 ions – the latter, in any case, are much less stable than the <a href="/wiki/Bifluoride" title="Bifluoride">bifluoride</a> ions (HF− 2) due to the very weak hydrogen bonding between hydrogen and chlorine, though its salts with very large and weakly polarising cations such as <a href="/wiki/Caesium" title="Caesium">Cs+</a> and <a href="/wiki/Quaternary_ammonium_cation" title="Quaternary ammonium cation">NR+ 4</a> (R = <a href="/wiki/Methyl_group" title="Methyl group">Me</a>, <a href="/wiki/Ethyl_group" title="Ethyl group">Et</a>, <a href="/wiki/Butyl_group" title="Butyl group">Bun</a>) may still be isolated. Anhydrous hydrogen chloride is a poor solvent, only able to dissolve small molecular compounds such as <a href="/wiki/Nitrosyl_chloride" title="Nitrosyl chloride">nitrosyl chloride</a> and <a href="/wiki/Phenol" title="Phenol">phenol</a>, or salts with very low <a href="/wiki/Lattice_energy" title="Lattice energy">lattice energies</a> such as tetraalkylammonium halides. It readily protonates <a href="/wiki/Nucleophile" title="Nucleophile">nucleophiles</a> containing lone-pairs or π bonds. <a href="/wiki/Solvolysis" title="Solvolysis">Solvolysis</a>, <a href="/wiki/Ligand" title="Ligand">ligand</a> replacement reactions, and oxidations are well-characterised in hydrogen chloride solution:<a href="#cite_note-Greenwood818-49">[48]</a> <dl><dd>Ph3SnCl + HCl ⟶ Ph2SnCl2 + PhH (solvolysis)</dd> <dd>Ph3COH + 3 HCl ⟶ Ph 3C+ HCl− 2 + H3O+Cl− (solvolysis)</dd> <dd>Me 4N+ HCl− 2 + BCl3 ⟶ Me 4N+ BCl− 4 + HCl (ligand replacement)</dd> <dd>PCl3 + Cl2 + HCl ⟶ PCl+ 4HCl− 2 (oxidation)</dd></dl> <div class="mw-heading mw-heading3"><h3 id="Other_binary_chlorides">Other binary chlorides</h3></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Nickel(II)-chloride-hexahydrate-sample.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/2/2a/Nickel%28II%29-chloride-hexahydrate-sample.jpg/220px-Nickel%28II%29-chloride-hexahydrate-sample.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/2a/Nickel%28II%29-chloride-hexahydrate-sample.jpg/330px-Nickel%28II%29-chloride-hexahydrate-sample.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/2a/Nickel%28II%29-chloride-hexahydrate-sample.jpg/440px-Nickel%28II%29-chloride-hexahydrate-sample.jpg 2x" data-file-width="1000" data-file-height="750" /></a><figcaption>Hydrated <a href="/wiki/Nickel(II)_chloride" title="Nickel(II) chloride">nickel(II) chloride</a>, NiCl2(H2O)6</figcaption></figure> Nearly all elements in the periodic table form binary chlorides. The exceptions are decidedly in the minority and stem in each case from one of three causes: extreme inertness and reluctance to participate in chemical reactions (the <a href="/wiki/Noble_gas" title="Noble gas">noble gases</a>, with the exception of <a href="/wiki/Xenon" title="Xenon">xenon</a> in the highly unstable <a href="/wiki/Xenon_dichloride" title="Xenon dichloride">XeCl2</a> and XeCl4); extreme nuclear instability hampering chemical investigation before decay and transmutation (many of the heaviest elements beyond <a href="/wiki/Bismuth" title="Bismuth">bismuth</a>); and having an electronegativity higher than chlorine's (<a href="/wiki/Oxygen" title="Oxygen">oxygen</a> and <a href="/wiki/Fluorine" title="Fluorine">fluorine</a>) so that the resultant binary compounds are formally not chlorides but rather oxides or fluorides of chlorine.<a href="#cite_note-Greenwood821-50">[49]</a> Even though <a href="/wiki/Nitrogen" title="Nitrogen">nitrogen</a> in NCl3 is bearing a negative charge, the compound is usually called <a href="/wiki/Nitrogen_trichloride" title="Nitrogen trichloride">nitrogen trichloride</a>. Chlorination of metals with Cl2 usually leads to a higher oxidation state than bromination with Br2 when multiple oxidation states are available, such as in <a href="/wiki/Molybdenum(V)_chloride" title="Molybdenum(V) chloride">MoCl5</a> and <a href="/wiki/Molybdenum(III)_bromide" title="Molybdenum(III) bromide">MoBr3</a>. Chlorides can be made by reaction of an element or its oxide, hydroxide, or carbonate with hydrochloric acid, and then dehydrated by mildly high temperatures combined with either low pressure or anhydrous hydrogen chloride gas. These methods work best when the chloride product is stable to hydrolysis; otherwise, the possibilities include high-temperature oxidative chlorination of the element with chlorine or hydrogen chloride, high-temperature chlorination of a metal oxide or other halide by chlorine, a volatile metal chloride, <a href="/wiki/Carbon_tetrachloride" title="Carbon tetrachloride">carbon tetrachloride</a>, or an organic chloride. For instance, <a href="/wiki/Zirconium_dioxide" title="Zirconium dioxide">zirconium dioxide</a> reacts with chlorine at standard conditions to produce <a href="/wiki/Zirconium_tetrachloride" class="mw-redirect" title="Zirconium tetrachloride">zirconium tetrachloride</a>, and <a href="/wiki/Uranium_trioxide" title="Uranium trioxide">uranium trioxide</a> reacts with <a href="/wiki/Hexachloropropene" title="Hexachloropropene">hexachloropropene</a> when heated under <a href="/wiki/Reflux" title="Reflux">reflux</a> to give <a href="/wiki/Uranium_tetrachloride" title="Uranium tetrachloride">uranium tetrachloride</a>. The second example also involves a reduction in <a href="/wiki/Oxidation_state" title="Oxidation state">oxidation state</a>, which can also be achieved by reducing a higher chloride using hydrogen or a metal as a reducing agent. This may also be achieved by thermal decomposition or disproportionation as follows:<a href="#cite_note-Greenwood821-50">[49]</a> <dl><dd>EuCl3 + <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035">⁠1/2⁠ H2 ⟶ EuCl2 + HCl</dd> <dd>ReCl5 at "bp"⟶  ReCl3 + Cl2</dd> <dd>AuCl3 160 °C⟶  AuCl + Cl2</dd></dl> Most metal chlorides with the metal in low oxidation states (+1 to +3) are ionic. Nonmetals tend to form covalent molecular chlorides, as do metals in high oxidation states from +3 and above. Both ionic and covalent chlorides are known for metals in oxidation state +3 (e.g. <a href="/wiki/Scandium_chloride" title="Scandium chloride">scandium chloride</a> is mostly ionic, but <a href="/wiki/Aluminium_chloride" title="Aluminium chloride">aluminium chloride</a> is not). <a href="/wiki/Silver_chloride" title="Silver chloride">Silver chloride</a> is very insoluble in water and is thus often used as a qualitative test for chlorine.<a href="#cite_note-Greenwood821-50">[49]</a> <div class="mw-heading mw-heading3"><h3 id="Polychlorine_compounds">Polychlorine compounds</h3></div> Although dichlorine is a strong oxidising agent with a high first ionisation energy, it may be oxidised under extreme conditions to form the <style data-mw-deduplicate="TemplateStyles:r1123817410">.mw-parser-output .template-chem2-su{display:inline-block;font-size:80%;line-height:1;vertical-align:-0.35em}.mw-parser-output .template-chem2-su>span{display:block;text-align:left}.mw-parser-output sub.template-chem2-sub{font-size:80%;vertical-align:-0.35em}.mw-parser-output sup.template-chem2-sup{font-size:80%;vertical-align:0.65em}</style>[Cl2]+ cation. This is very unstable and has only been characterised by its electronic band spectrum when produced in a low-pressure discharge tube. The yellow <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]+ cation is more stable and may be produced as follows:<a href="#cite_note-Greenwood842-51">[50]</a> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">Cl2 + ClF + AsF5 −78 °C⟶ <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]+[AsF6]−</dd></dl> This reaction is conducted in the oxidising solvent <a href="/wiki/Arsenic_pentafluoride" title="Arsenic pentafluoride">arsenic pentafluoride</a>. The trichloride anion, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410">[Cl3]−, has also been characterised; it is analogous to <a href="/wiki/Triiodide" title="Triiodide">triiodide</a>.<a href="#cite_note-Greenwood824-52">[51]</a> <div class="mw-heading mw-heading3"><h3 id="Chlorine_fluorides">Chlorine fluorides</h3></div> The three fluorides of chlorine form a subset of the <a href="/wiki/Interhalogen" title="Interhalogen">interhalogen</a> compounds, all of which are <a href="/wiki/Diamagnetic" class="mw-redirect" title="Diamagnetic">diamagnetic</a>.<a href="#cite_note-Greenwood824-52">[51]</a> Some cationic and anionic derivatives are known, such as ClF− 2, ClF− 4, ClF+ 2, and Cl2F+.<a href="#cite_note-Greenwood835-53">[52]</a> Some <a href="/wiki/Pseudohalogen" title="Pseudohalogen">pseudohalides</a> of chlorine are also known, such as <a href="/wiki/Cyanogen_chloride" title="Cyanogen chloride">cyanogen chloride</a> (ClCN, linear), chlorine <a href="/wiki/Cyanate" title="Cyanate">cyanate</a> (ClNCO), chlorine <a href="/wiki/Thiocyanate" title="Thiocyanate">thiocyanate</a> (ClSCN, unlike its oxygen counterpart), and chlorine <a href="/wiki/Azide" title="Azide">azide</a> (ClN3).<a href="#cite_note-Greenwood824-52">[51]</a> <a href="/wiki/Chlorine_monofluoride" title="Chlorine monofluoride">Chlorine monofluoride</a> (ClF) is extremely thermally stable, and is sold commercially in 500-gram steel lecture bottles. It is a colourless gas that melts at −155.6 °C and boils at −100.1 °C. It may be produced by the reaction of its elements at 225 °C, though it must then be separated and purified from <a href="/wiki/Chlorine_trifluoride" title="Chlorine trifluoride">chlorine trifluoride</a> and its reactants. Its properties are mostly intermediate between those of chlorine and fluorine. It will react with many metals and nonmetals from room temperature and above, fluorinating them and liberating chlorine. It will also act as a chlorofluorinating agent, adding chlorine and fluorine across a multiple bond or by oxidation: for example, it will attack <a href="/wiki/Carbon_monoxide" title="Carbon monoxide">carbon monoxide</a> to form carbonyl chlorofluoride, COFCl. It will react analogously with <a href="/wiki/Hexafluoroacetone" title="Hexafluoroacetone">hexafluoroacetone</a>, (CF3)2CO, with a <a href="/wiki/Potassium_fluoride" title="Potassium fluoride">potassium fluoride</a> catalyst to produce heptafluoroisopropyl hypochlorite, (CF3)2CFOCl; with <a href="/wiki/Nitrile" title="Nitrile">nitriles</a> RCN to produce RCF2NCl2; and with the sulfur oxides SO2 and SO3 to produce ClSO2F and ClOSO2F respectively. It will also react exothermically with compounds containing –OH and –NH groups, such as water:<a href="#cite_note-Greenwood824-52">[51]</a> <dl><dd>H2O + 2 ClF ⟶ 2 HF + Cl2O</dd></dl> <a href="/wiki/Chlorine_trifluoride" title="Chlorine trifluoride">Chlorine trifluoride</a> (ClF3) is a volatile colourless molecular liquid which melts at −76.3 °C and boils at 11.8  °C. It may be formed by directly fluorinating gaseous chlorine or chlorine monofluoride at 200–300 °C. One of the most reactive chemical compounds known, the list of elements it sets on fire is diverse, containing <a href="/wiki/Hydrogen" title="Hydrogen">hydrogen</a>, <a href="/wiki/Potassium" title="Potassium">potassium</a>, <a href="/wiki/Phosphorus" title="Phosphorus">phosphorus</a>, <a href="/wiki/Arsenic" title="Arsenic">arsenic</a>, <a href="/wiki/Antimony" title="Antimony">antimony</a>, <a href="/wiki/Sulfur" title="Sulfur">sulfur</a>, <a href="/wiki/Selenium" title="Selenium">selenium</a>, <a href="/wiki/Tellurium" title="Tellurium">tellurium</a>, <a href="/wiki/Bromine" title="Bromine">bromine</a>, <a href="/wiki/Iodine" title="Iodine">iodine</a>, and powdered <a href="/wiki/Molybdenum" title="Molybdenum">molybdenum</a>, <a href="/wiki/Tungsten" title="Tungsten">tungsten</a>, <a href="/wiki/Rhodium" title="Rhodium">rhodium</a>, <a href="/wiki/Iridium" title="Iridium">iridium</a>, and <a href="/wiki/Iron" title="Iron">iron</a>. It will also ignite water, along with many substances which in ordinary circumstances would be considered chemically inert such as <a href="/wiki/Asbestos" title="Asbestos">asbestos</a>, concrete, glass, and sand. When heated, it will even corrode <a href="/wiki/Noble_metal" title="Noble metal">noble metals</a> as <a href="/wiki/Palladium" title="Palladium">palladium</a>, <a href="/wiki/Platinum" title="Platinum">platinum</a>, and <a href="/wiki/Gold" title="Gold">gold</a>, and even the <a href="/wiki/Noble_gas" title="Noble gas">noble gases</a> <a href="/wiki/Xenon" title="Xenon">xenon</a> and <a href="/wiki/Radon" title="Radon">radon</a> do not escape fluorination. An impermeable fluoride layer is formed by <a href="/wiki/Sodium" title="Sodium">sodium</a>, <a href="/wiki/Magnesium" title="Magnesium">magnesium</a>, <a href="/wiki/Aluminium" title="Aluminium">aluminium</a>, <a href="/wiki/Zinc" title="Zinc">zinc</a>, <a href="/wiki/Tin" title="Tin">tin</a>, and <a href="/wiki/Silver" title="Silver">silver</a>, which may be removed by heating. <a href="/wiki/Nickel" title="Nickel">Nickel</a>, copper, and steel containers are usually used due to their great resistance to attack by chlorine trifluoride, stemming from the formation of an unreactive layer of metal fluoride. Its reaction with <a href="/wiki/Hydrazine" title="Hydrazine">hydrazine</a> to form hydrogen fluoride, nitrogen, and chlorine gases was used in experimental rocket engine, but has problems largely stemming from its extreme <a href="/wiki/Hypergolic_propellant" title="Hypergolic propellant">hypergolicity</a> resulting in ignition without any measurable delay. Today, it is mostly used in nuclear fuel processing, to oxidise <a href="/wiki/Uranium" title="Uranium">uranium</a> to <a href="/wiki/Uranium_hexafluoride" title="Uranium hexafluoride">uranium hexafluoride</a> for its enriching and to separate it from <a href="/wiki/Plutonium" title="Plutonium">plutonium</a>, as well as in the semiconductor industry, where it is used to clean <a href="/wiki/Chemical_vapor_deposition" title="Chemical vapor deposition">chemical vapor deposition</a> chambers.<a href="#cite_note-SIcvd-54">[53]</a> It can act as a fluoride ion donor or acceptor (Lewis base or acid), although it does not dissociate appreciably into ClF+ 2 and ClF− 4 ions.<a href="#cite_note-Greenwood828-55">[54]</a> <a href="/wiki/Chlorine_pentafluoride" title="Chlorine pentafluoride">Chlorine pentafluoride</a> (ClF5) is made on a large scale by direct fluorination of chlorine with excess <a href="/wiki/Fluorine" title="Fluorine">fluorine</a> gas at 350 °C and 250 atm, and on a small scale by reacting metal chlorides with fluorine gas at 100–300 °C. It melts at −103 °C and boils at −13.1 °C. It is a very strong fluorinating agent, although it is still not as effective as chlorine trifluoride. Only a few specific stoichiometric reactions have been characterised. <a href="/wiki/Arsenic_pentafluoride" title="Arsenic pentafluoride">Arsenic pentafluoride</a> and <a href="/wiki/Antimony_pentafluoride" title="Antimony pentafluoride">antimony pentafluoride</a> form ionic adducts of the form [ClF4]+[MF6]− (M = As, Sb) and water reacts vigorously as follows:<a href="#cite_note-Greenwood832-56">[55]</a> <dl><dd>2 H2O + ClF5 ⟶ 4 HF + FClO2</dd></dl> The product, <a href="/wiki/Chloryl_fluoride" title="Chloryl fluoride">chloryl fluoride</a>, is one of the five known chlorine oxide fluorides. These range from the thermally unstable FClO to the chemically unreactive <a href="/wiki/Perchloryl_fluoride" title="Perchloryl fluoride">perchloryl fluoride</a> (FClO3), the other three being FClO2, F3ClO, and F3ClO2. All five behave similarly to the chlorine fluorides, both structurally and chemically, and may act as Lewis acids or bases by gaining or losing fluoride ions respectively or as very strong oxidising and fluorinating agents.<a href="#cite_note-Greenwood875-57">[56]</a> <div class="mw-heading mw-heading3"><h3 id="Chlorine_oxides">Chlorine oxides</h3></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Chlorine_dioxide_gas_and_solution.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/Chlorine_dioxide_gas_and_solution.jpg/220px-Chlorine_dioxide_gas_and_solution.jpg" decoding="async" width="220" height="268" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/0/04/Chlorine_dioxide_gas_and_solution.jpg 1.5x" data-file-width="291" data-file-height="354" /></a><figcaption>Yellow <a href="/wiki/Chlorine_dioxide" title="Chlorine dioxide">chlorine dioxide</a> (ClO2) gas above a solution of hydrochloric acid and sodium chlorite in water, also containing dissolved chlorine dioxide</figcaption></figure> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Dichlorine-heptoxide-3D-balls.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/c/cd/Dichlorine-heptoxide-3D-balls.png/220px-Dichlorine-heptoxide-3D-balls.png" decoding="async" width="220" height="133" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/cd/Dichlorine-heptoxide-3D-balls.png/330px-Dichlorine-heptoxide-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/cd/Dichlorine-heptoxide-3D-balls.png/440px-Dichlorine-heptoxide-3D-balls.png 2x" data-file-width="1100" data-file-height="666" /></a><figcaption>Structure of <a href="/wiki/Dichlorine_heptoxide" title="Dichlorine heptoxide">dichlorine heptoxide</a>, Cl2O7, the most stable of the chlorine oxides</figcaption></figure> The <a href="/wiki/Chlorine_oxide" title="Chlorine oxide">chlorine oxides</a> are well-studied in spite of their instability (all of them are endothermic compounds). They are important because they are produced when <a href="/wiki/Chlorofluorocarbon" title="Chlorofluorocarbon">chlorofluorocarbons</a> undergo photolysis in the upper atmosphere and cause the destruction of the ozone layer. None of them can be made from directly reacting the elements.<a href="#cite_note-Greenwood844-58">[57]</a> <a href="/wiki/Dichlorine_monoxide" title="Dichlorine monoxide">Dichlorine monoxide</a> (Cl2O) is a brownish-yellow gas (red-brown when solid or liquid) which may be obtained by reacting chlorine gas with yellow <a href="/wiki/Mercury(II)_oxide" title="Mercury(II) oxide">mercury(II) oxide</a>. It is very soluble in water, in which it is in equilibrium with <a href="/wiki/Hypochlorous_acid" title="Hypochlorous acid">hypochlorous acid</a> (HOCl), of which it is the anhydride. It is thus an effective bleach and is mostly used to make <a href="/wiki/Hypochlorite" title="Hypochlorite">hypochlorites</a>. It explodes on heating or sparking or in the presence of ammonia gas.<a href="#cite_note-Greenwood844-58">[57]</a> <a href="/wiki/Chlorine_dioxide" title="Chlorine dioxide">Chlorine dioxide</a> (ClO2) was the first chlorine oxide to be discovered in 1811 by <a href="/wiki/Humphry_Davy" title="Humphry Davy">Humphry Davy</a>. It is a yellow paramagnetic gas (deep-red as a solid or liquid), as expected from its having an odd number of electrons: it is stable towards dimerisation due to the delocalisation of the unpaired electron. It explodes above −40 °C as a liquid and under pressure as a gas and therefore must be made at low concentrations for wood-pulp bleaching and water treatment. It is usually prepared by reducing a <a href="/wiki/Chlorate" title="Chlorate">chlorate</a> as follows:<a href="#cite_note-Greenwood844-58">[57]</a> <dl><dd>ClO− 3 + Cl− + 2 H+ ⟶ ClO2 + <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1214402035">⁠1/2⁠ Cl2 + H2O</dd></dl> Its production is thus intimately linked to the redox reactions of the chlorine oxoacids. It is a strong oxidising agent, reacting with <a href="/wiki/Sulfur" title="Sulfur">sulfur</a>, <a href="/wiki/Phosphorus" title="Phosphorus">phosphorus</a>, phosphorus halides, and <a href="/wiki/Potassium_borohydride" class="mw-redirect" title="Potassium borohydride">potassium borohydride</a>. It dissolves exothermically in water to form dark-green solutions that very slowly decompose in the dark. Crystalline clathrate hydrates ClO2·nH2O (n ≈ 6–10) separate out at low temperatures. However, in the presence of light, these solutions rapidly photodecompose to form a mixture of chloric and hydrochloric acids. Photolysis of individual ClO2 molecules result in the radicals ClO and ClOO, while at room temperature mostly chlorine, oxygen, and some ClO3 and Cl2O6 are produced. Cl2O3 is also produced when photolysing the solid at −78 °C: it is a dark brown solid that explodes below 0 °C. The ClO radical leads to the depletion of atmospheric ozone and is thus environmentally important as follows:<a href="#cite_note-Greenwood844-58">[57]</a> <dl><dd>Cl• + O3 ⟶ ClO• + O2</dd> <dd>ClO• + O• ⟶ Cl• + O2</dd></dl> <a href="/wiki/Chlorine_perchlorate" title="Chlorine perchlorate">Chlorine perchlorate</a> (ClOClO3) is a pale yellow liquid that is less stable than ClO2 and decomposes at room temperature to form chlorine, oxygen, and <a href="/wiki/Dichlorine_hexoxide" title="Dichlorine hexoxide">dichlorine hexoxide</a> (Cl2O6).<a href="#cite_note-Greenwood844-58">[57]</a> Chlorine perchlorate may also be considered a chlorine derivative of <a href="/wiki/Perchloric_acid" title="Perchloric acid">perchloric acid</a> (HOClO3), similar to the thermally unstable chlorine derivatives of other oxoacids: examples include <a href="/wiki/Chlorine_nitrate" title="Chlorine nitrate">chlorine nitrate</a> (ClONO2, vigorously reactive and explosive), and chlorine fluorosulfate (ClOSO2F, more stable but still moisture-sensitive and highly reactive).<a href="#cite_note-Greenwood883-59">[58]</a> Dichlorine hexoxide is a dark-red liquid that freezes to form a solid which turns yellow at −180 °C: it is usually made by reaction of chlorine dioxide with oxygen. Despite attempts to rationalise it as the dimer of ClO3, it reacts more as though it were chloryl perchlorate, [ClO2]+[ClO4]−, which has been confirmed to be the correct structure of the solid. It hydrolyses in water to give a mixture of chloric and perchloric acids: the analogous reaction with anhydrous <a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">hydrogen fluoride</a> does not proceed to completion.<a href="#cite_note-Greenwood844-58">[57]</a> <a href="/wiki/Dichlorine_heptoxide" title="Dichlorine heptoxide">Dichlorine heptoxide</a> (Cl2O7) is the anhydride of <a href="/wiki/Perchloric_acid" title="Perchloric acid">perchloric acid</a> (HClO4) and can readily be obtained from it by dehydrating it with <a href="/wiki/Phosphoric_acid" title="Phosphoric acid">phosphoric acid</a> at −10 °C and then distilling the product at −35 °C and 1 mmHg. It is a shock-sensitive, colourless oily liquid. It is the least reactive of the chlorine oxides, being the only one to not set organic materials on fire at room temperature. It may be dissolved in water to regenerate perchloric acid or in aqueous alkalis to regenerate perchlorates. However, it thermally decomposes explosively by breaking one of the central Cl–O bonds, producing the radicals ClO3 and ClO4 which immediately decompose to the elements through intermediate oxides.<a href="#cite_note-Greenwood844-58">[57]</a> <div class="mw-heading mw-heading3"><h3 id="Chlorine_oxoacids_and_oxyanions">Chlorine oxoacids and oxyanions</h3></div> <table class="wikitable" style="float:right; margin-top:0; margin-left:1em; text-align:center; font-size:10pt; line-height:11pt; width:25%;"> <caption>Standard reduction potentials for aqueous Cl species<a href="#cite_note-Greenwood853-46">[45]</a> </caption> <tbody><tr> <th>E°(couple)</th> <th>a(H+) = 1 (acid)</th> <th>E°(couple)</th> <th>a(OH−) = 1 (base) </th></tr> <tr> <td>Cl2/Cl−</td> <td>+1.358</td> <td>Cl2/Cl−</td> <td>+1.358 </td></tr> <tr> <td>HOCl/Cl−</td> <td>+1.484</td> <td>ClO−/Cl−</td> <td>+0.890 </td></tr> <tr> <td>ClO− 3/Cl−</td> <td>+1.459</td> <td> </td> <td>  </td></tr> <tr> <td>HOCl/Cl2</td> <td>+1.630</td> <td>ClO−/Cl2</td> <td>+0.421 </td></tr> <tr> <td>HClO2/Cl2</td> <td>+1.659</td> <td> </td> <td>  </td></tr> <tr> <td>ClO− 3/Cl2</td> <td>+1.468</td> <td> </td> <td>  </td></tr> <tr> <td>ClO− 4/Cl2</td> <td>+1.277</td> <td> </td> <td>  </td></tr> <tr> <td>HClO2/HOCl</td> <td>+1.701</td> <td>ClO− 2/ClO−</td> <td>+0.681 </td></tr> <tr> <td> </td> <td> </td> <td>ClO− 3/ClO−</td> <td>+0.488 </td></tr> <tr> <td>ClO− 3/HClO2</td> <td>+1.181</td> <td>ClO− 3/ClO− 2</td> <td>+0.295 </td></tr> <tr> <td>ClO− 4/ClO− 3</td> <td>+1.201</td> <td>ClO− 4/ClO− 3</td> <td>+0.374 </td></tr></tbody></table> Chlorine forms four oxoacids: <a href="/wiki/Hypochlorous_acid" title="Hypochlorous acid">hypochlorous acid</a> (HOCl), <a href="/wiki/Chlorous_acid" title="Chlorous acid">chlorous acid</a> (HOClO), <a href="/wiki/Chloric_acid" title="Chloric acid">chloric acid</a> (HOClO2), and <a href="/wiki/Perchloric_acid" title="Perchloric acid">perchloric acid</a> (HOClO3). As can be seen from the redox potentials given in the adjacent table, chlorine is much more stable towards disproportionation in acidic solutions than in alkaline solutions:<a href="#cite_note-Greenwood853-46">[45]</a> <dl><dd><table> <tbody><tr> <td>Cl2 + H2O</td> <td>⇌ HOCl + H+ + Cl−</td> <td>Kac = 4.2 × 10−4 mol2 l−2 </td></tr> <tr> <td>Cl2 + 2 OH−</td> <td>⇌ OCl− + H2O + Cl−</td> <td>Kalk = 7.5 × 1015 mol−1 l </td></tr></tbody></table></dd></dl> The hypochlorite ions also disproportionate further to produce chloride and chlorate (3 ClO− ⇌ 2 Cl− + ClO− 3) but this reaction is quite slow at temperatures below 70 °C in spite of the very favourable equilibrium constant of 1027. The chlorate ions may themselves disproportionate to form chloride and perchlorate (4 ClO− 3 ⇌ Cl− + 3 ClO− 4) but this is still very slow even at 100 °C despite the very favourable equilibrium constant of 1020. The rates of reaction for the chlorine oxyanions increases as the oxidation state of chlorine decreases. The strengths of the chlorine oxyacids increase very quickly as the oxidation state of chlorine increases due to the increasing delocalisation of charge over more and more oxygen atoms in their conjugate bases.<a href="#cite_note-Greenwood853-46">[45]</a> Most of the chlorine oxoacids may be produced by exploiting these disproportionation reactions. Hypochlorous acid (HOCl) is highly reactive and quite unstable; its salts are mostly used for their bleaching and sterilising abilities. They are very strong oxidising agents, transferring an oxygen atom to most inorganic species. Chlorous acid (HOClO) is even more unstable and cannot be isolated or concentrated without decomposition: it is known from the decomposition of aqueous chlorine dioxide. However, <a href="/wiki/Sodium_chlorite" title="Sodium chlorite">sodium chlorite</a> is a stable salt and is useful for bleaching and stripping textiles, as an oxidising agent, and as a source of chlorine dioxide. Chloric acid (HOClO2) is a strong acid that is quite stable in cold water up to 30% concentration, but on warming gives chlorine and chlorine dioxide. Evaporation under reduced pressure allows it to be concentrated further to about 40%, but then it decomposes to perchloric acid, chlorine, oxygen, water, and chlorine dioxide. Its most important salt is <a href="/wiki/Sodium_chlorate" title="Sodium chlorate">sodium chlorate</a>, mostly used to make chlorine dioxide to bleach paper pulp. The decomposition of chlorate to chloride and oxygen is a common way to produce oxygen in the laboratory on a small scale. Chloride and chlorate may comproportionate to form chlorine as follows:<a href="#cite_note-Greenwood856-60">[59]</a> <dl><dd>ClO− 3 + 5 Cl− + 6 H+ ⟶ 3 Cl2 + 3 H2O</dd></dl> Perchlorates and perchloric acid (HOClO3) are the most stable oxo-compounds of chlorine, in keeping with the fact that chlorine compounds are most stable when the chlorine atom is in its lowest (−1) or highest (+7) possible oxidation states. Perchloric acid and aqueous perchlorates are vigorous and sometimes violent oxidising agents when heated, in stark contrast to their mostly inactive nature at room temperature due to the high activation energies for these reactions for kinetic reasons. Perchlorates are made by electrolytically oxidising sodium chlorate, and perchloric acid is made by reacting anhydrous <a href="/wiki/Sodium_perchlorate" title="Sodium perchlorate">sodium perchlorate</a> or <a href="/wiki/Barium_perchlorate" title="Barium perchlorate">barium perchlorate</a> with concentrated hydrochloric acid, filtering away the chloride precipitated and distilling the filtrate to concentrate it. Anhydrous perchloric acid is a colourless mobile liquid that is sensitive to shock that explodes on contact with most organic compounds, sets <a href="/wiki/Hydrogen_iodide" title="Hydrogen iodide">hydrogen iodide</a> and <a href="/wiki/Thionyl_chloride" title="Thionyl chloride">thionyl chloride</a> on fire and even oxidises silver and gold. Although it is a weak ligand, weaker than water, a few compounds involving coordinated ClO− 4 are known.<a href="#cite_note-Greenwood856-60">[59]</a> The Table below presents typical oxidation states for chlorine element as given in the secondary schools or colleges. There are more complex chemical compounds, the structure of which can only be explained using modern quantum chemical methods, for example, cluster technetium chloride [(CH3)4N]3[Tc6Cl14], in which 6 of the 14 chlorine atoms are formally divalent, and oxidation states are fractional.<a href="#cite_note-61">[60]</a><a href="#cite_note-62">[61]</a> In addition, all the above chemical regularities are valid for "normal" or close to normal conditions, while at ultra-high pressures (for example, in the cores of large planets), chlorine can exhibit an oxidation state of -3, forming a Na3Cl compound with sodium, which does not fit into traditional concepts of chemistry.<a href="#cite_note-63">[62]</a> <table class="wikitable"> <tbody><tr> <th>Chlorine oxidation state </th> <td>−1 </td> <td>+1 </td> <td>+3 </td> <td>+5 </td> <td>+7 </td></tr> <tr> <th>Name </th> <td><a href="/wiki/Chloride" title="Chloride">chloride</a> </td> <td><a href="/wiki/Hypochlorite" title="Hypochlorite">hypochlorite</a> </td> <td><a href="/wiki/Chlorite" title="Chlorite">chlorite</a> </td> <td><a href="/wiki/Chlorate" title="Chlorate">chlorate</a> </td> <td><a href="/wiki/Perchlorate" title="Perchlorate">perchlorate</a> </td></tr> <tr> <th>Formula </th> <td>Cl− </td> <td>ClO− </td> <td>ClO− 2 </td> <td>ClO− 3 </td> <td>ClO− 4 </td></tr> <tr> <th>Structure </th> <td><a href="/wiki/File:Chloride-ion-3D-vdW.png" class="mw-file-description" title="The chloride ion"><img alt="The chloride ion" src="//upload.wikimedia.org/wikipedia/commons/thumb/8/8e/Chloride-ion-3D-vdW.png/50px-Chloride-ion-3D-vdW.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/8e/Chloride-ion-3D-vdW.png/75px-Chloride-ion-3D-vdW.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/8e/Chloride-ion-3D-vdW.png/100px-Chloride-ion-3D-vdW.png 2x" data-file-width="1100" data-file-height="1100" /></a> </td> <td><a href="/wiki/File:Hypochlorite-3D-vdW.png" class="mw-file-description" title="The hypochlorite ion"><img alt="The hypochlorite ion" src="//upload.wikimedia.org/wikipedia/commons/thumb/4/48/Hypochlorite-3D-vdW.png/50px-Hypochlorite-3D-vdW.png" decoding="async" width="50" height="38" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/48/Hypochlorite-3D-vdW.png/75px-Hypochlorite-3D-vdW.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/48/Hypochlorite-3D-vdW.png/100px-Hypochlorite-3D-vdW.png 2x" data-file-width="1100" data-file-height="840" /></a> </td> <td><a href="/wiki/File:Chlorite-3D-vdW.png" class="mw-file-description" title="The chlorite ion"><img alt="The chlorite ion" src="//upload.wikimedia.org/wikipedia/commons/thumb/4/42/Chlorite-3D-vdW.png/50px-Chlorite-3D-vdW.png" decoding="async" width="50" height="39" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/42/Chlorite-3D-vdW.png/75px-Chlorite-3D-vdW.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/42/Chlorite-3D-vdW.png/100px-Chlorite-3D-vdW.png 2x" data-file-width="1100" data-file-height="859" /></a> </td> <td><a href="/wiki/File:Chlorate-3D-vdW.png" class="mw-file-description" title="The chlorate ion"><img alt="The chlorate ion" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b2/Chlorate-3D-vdW.png/50px-Chlorate-3D-vdW.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/b2/Chlorate-3D-vdW.png/75px-Chlorate-3D-vdW.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/b2/Chlorate-3D-vdW.png/100px-Chlorate-3D-vdW.png 2x" data-file-width="1093" data-file-height="1100" /></a> </td> <td><a href="/wiki/File:Perchlorate-3D-vdW.png" class="mw-file-description" title="The perchlorate ion"><img alt="The perchlorate ion" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/bb/Perchlorate-3D-vdW.png/50px-Perchlorate-3D-vdW.png" decoding="async" width="50" height="51" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/bb/Perchlorate-3D-vdW.png/75px-Perchlorate-3D-vdW.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/bb/Perchlorate-3D-vdW.png/100px-Perchlorate-3D-vdW.png 2x" data-file-width="1089" data-file-height="1100" /></a> </td></tr></tbody></table> <div class="mw-heading mw-heading3"><h3 id="Organochlorine_compounds">Organochlorine compounds</h3></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Organochlorine_compound" class="mw-redirect" title="Organochlorine compound">Organochlorine compound</a></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Phosphorus_pentachloride_mechanism.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/71/Phosphorus_pentachloride_mechanism.png/500px-Phosphorus_pentachloride_mechanism.png" decoding="async" width="500" height="229" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/71/Phosphorus_pentachloride_mechanism.png/750px-Phosphorus_pentachloride_mechanism.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/71/Phosphorus_pentachloride_mechanism.png/1000px-Phosphorus_pentachloride_mechanism.png 2x" data-file-width="1961" data-file-height="899" /></a><figcaption>Suggested mechanism for the chlorination of a carboxylic acid by phosphorus pentachloride to form an <a href="/wiki/Acyl_chloride" title="Acyl chloride">acyl chloride</a></figcaption></figure> Like the other carbon–halogen bonds, the C–Cl bond is a common functional group that forms part of core <a href="/wiki/Organic_chemistry" title="Organic chemistry">organic chemistry</a>. Formally, compounds with this functional group may be considered organic derivatives of the chloride anion. Due to the difference of electronegativity between chlorine (3.16) and carbon (2.55), the carbon in a C–Cl bond is electron-deficient and thus <a href="/wiki/Electrophilic" class="mw-redirect" title="Electrophilic">electrophilic</a>. <a href="/wiki/Chlorination_reaction" class="mw-redirect" title="Chlorination reaction">Chlorination</a> modifies the physical properties of hydrocarbons in several ways: chlorocarbons are typically denser than <a href="/wiki/Water" title="Water">water</a> due to the higher atomic weight of chlorine versus hydrogen, and aliphatic organochlorides are <a href="/wiki/Alkylating_agent" class="mw-redirect" title="Alkylating agent">alkylating agents</a> because chloride is a <a href="/wiki/Leaving_group" title="Leaving group">leaving group</a>.<a href="#cite_note-Ullmann-64">[63]</a> <a href="/wiki/Alkanes" class="mw-redirect" title="Alkanes">Alkanes</a> and <a href="/wiki/Aryl" class="mw-redirect" title="Aryl">aryl</a> alkanes may be chlorinated under <a href="/wiki/Free-radical" class="mw-redirect" title="Free-radical">free-radical</a> conditions, with UV light. However, the extent of chlorination is difficult to control: the reaction is not <a href="/wiki/Regioselectivity" title="Regioselectivity">regioselective</a> and often results in a mixture of various isomers with different degrees of chlorination, though this may be permissible if the products are easily separated. Aryl chlorides may be prepared by the <a href="/wiki/Friedel-Crafts_halogenation" class="mw-redirect" title="Friedel-Crafts halogenation">Friedel-Crafts halogenation</a>, using chlorine and a <a href="/wiki/Lewis_acid" class="mw-redirect" title="Lewis acid">Lewis acid</a> catalyst.<a href="#cite_note-Ullmann-64">[63]</a> The <a href="/wiki/Haloform_reaction" title="Haloform reaction">haloform reaction</a>, using chlorine and <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">sodium hydroxide</a>, is also able to generate alkyl halides from methyl ketones, and related compounds. Chlorine adds to the multiple bonds on <a href="/wiki/Alkene" title="Alkene">alkenes</a> and <a href="/wiki/Alkyne" title="Alkyne">alkynes</a> as well, giving di- or tetrachloro compounds. However, due to the expense and reactivity of chlorine, organochlorine compounds are more commonly produced by using hydrogen chloride, or with chlorinating agents such as <a href="/wiki/Phosphorus_pentachloride" title="Phosphorus pentachloride">phosphorus pentachloride</a> (PCl5) or <a href="/wiki/Thionyl_chloride" title="Thionyl chloride">thionyl chloride</a> (SOCl2). The last is very convenient in the laboratory because all side products are gaseous and do not have to be distilled out.<a href="#cite_note-Ullmann-64">[63]</a> Many organochlorine compounds have been isolated from natural sources ranging from bacteria to humans.<a href="#cite_note-Gribble-65">[64]</a><a href="#cite_note-Gribble99-66">[65]</a> Chlorinated organic compounds are found in nearly every class of biomolecules including <a href="/wiki/Alkaloid" title="Alkaloid">alkaloids</a>, <a href="/wiki/Terpene" title="Terpene">terpenes</a>, <a href="/wiki/Amino_acid" title="Amino acid">amino acids</a>, <a href="/wiki/Flavonoid" title="Flavonoid">flavonoids</a>, <a href="/wiki/Steroid" title="Steroid">steroids</a>, and <a href="/wiki/Fatty_acid" title="Fatty acid">fatty acids</a>.<a href="#cite_note-Gribble-65">[64]</a><a href="#cite_note-67">[66]</a> Organochlorides, including <a href="/wiki/Polychlorinated_dibenzodioxins" title="Polychlorinated dibenzodioxins">dioxins</a>, are produced in the high temperature environment of forest fires, and dioxins have been found in the preserved ashes of lightning-ignited fires that predate synthetic dioxins.<a href="#cite_note-68">[67]</a> In addition, a variety of simple chlorinated hydrocarbons including dichloromethane, chloroform, and <a href="/wiki/Carbon_tetrachloride" title="Carbon tetrachloride">carbon tetrachloride</a> have been isolated from marine algae.<a href="#cite_note-69">[68]</a> A majority of the <a href="/wiki/Chloromethane" title="Chloromethane">chloromethane</a> in the environment is produced naturally by biological decomposition, forest fires, and volcanoes.<a href="#cite_note-70">[69]</a> Some types of organochlorides, though not all, have significant toxicity to plants or animals, including humans. Dioxins, produced when organic matter is burned in the presence of chlorine, and some insecticides, such as <a href="/wiki/DDT" title="DDT">DDT</a>, are <a href="/wiki/Persistent_organic_pollutant" title="Persistent organic pollutant">persistent organic pollutants</a> which pose dangers when they are released into the environment. For example, DDT, which was widely used to control insects in the mid 20th century, also accumulates in food chains, and causes reproductive problems (e.g., eggshell thinning) in certain bird species.<a href="#cite_note-71">[70]</a> Due to the ready homolytic fission of the C–Cl bond to create chlorine radicals in the upper atmosphere, <a href="/wiki/Chlorofluorocarbon" title="Chlorofluorocarbon">chlorofluorocarbons</a> have been phased out due to the harm they do to the ozone layer.<a href="#cite_note-Greenwood844-58">[57]</a> <div class="mw-heading mw-heading2"><h2 id="Occurrence">Occurrence</h2></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Liquid_chlorine_in_flask.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/45/Liquid_chlorine_in_flask.jpg/170px-Liquid_chlorine_in_flask.jpg" decoding="async" width="170" height="357" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/45/Liquid_chlorine_in_flask.jpg/255px-Liquid_chlorine_in_flask.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/45/Liquid_chlorine_in_flask.jpg/340px-Liquid_chlorine_in_flask.jpg 2x" data-file-width="787" data-file-height="1653" /></a><figcaption>Liquid chlorine analysis</figcaption></figure> Chlorine is too reactive to occur as the free element in nature but is very abundant in the form of its chloride salts. It is the 20th most abundant element<a href="#cite_note-72">[71]</a> in Earth's crust and makes up 126 <a href="/wiki/Parts_per_million" class="mw-redirect" title="Parts per million">parts per million</a> of it, through the large deposits of chloride minerals, especially <a href="/wiki/Sodium_chloride" title="Sodium chloride">sodium chloride</a>, that have been evaporated from water bodies. All of these pale in comparison to the reserves of chloride ions in seawater: smaller amounts at higher concentrations occur in some inland seas and underground <a href="/wiki/Brine" title="Brine">brine</a> wells, such as the <a href="/wiki/Great_Salt_Lake" title="Great Salt Lake">Great Salt Lake</a> in Utah and the <a href="/wiki/Dead_Sea" title="Dead Sea">Dead Sea</a> in Israel.<a href="#cite_note-Greenwood795-73">[72]</a> Small batches of chlorine gas are prepared in the laboratory by combining hydrochloric acid and <a href="/wiki/Manganese_dioxide" title="Manganese dioxide">manganese dioxide</a>, but the need rarely arises due to its ready availability. In industry, elemental chlorine is usually produced by the electrolysis of sodium chloride dissolved in water. This method, the <a href="/wiki/Chloralkali_process" title="Chloralkali process">chloralkali process</a> industrialized in 1892, now provides most industrial chlorine gas.<a href="#cite_note-Greenwood798-33">[32]</a> Along with chlorine, the method yields <a href="/wiki/Hydrogen" title="Hydrogen">hydrogen</a> gas and <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">sodium hydroxide</a>, which is the most valuable product. The process proceeds according to the following <a href="/wiki/Chemical_equation" title="Chemical equation">chemical equation</a>:<a href="#cite_note-74">[73]</a> <dl><dd>2 NaCl + 2 H2O → Cl2 + H2 + 2 NaOH</dd></dl> <div class="mw-heading mw-heading2"><h2 id="Production">Production</h2></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Chlorine_production" title="Chlorine production">Chlorine production</a></div> Chlorine is primarily produced by the <a href="/wiki/Chloralkali_process" title="Chloralkali process">chloralkali process</a>, although non-chloralkali processes exist. Global 2022 production was estimated to be 97 million tonnes.<a href="#cite_note-75">[74]</a> The most visible use of chlorine is in <a href="/wiki/Water_disinfection" class="mw-redirect" title="Water disinfection">water disinfection</a>. 35-40 % of chlorine produced is used to make <a href="/wiki/Poly(vinyl_chloride)" class="mw-redirect" title="Poly(vinyl chloride)">poly(vinyl chloride)</a> through <a href="/wiki/Ethylene_dichloride" class="mw-redirect" title="Ethylene dichloride">ethylene dichloride</a> and <a href="/wiki/Vinyl_chloride" title="Vinyl chloride">vinyl chloride</a>.<a href="#cite_note-76">[75]</a> The chlorine produced is available in cylinders from sizes ranging from 450 g to 70 kg, as well as drums (865 kg), tank wagons (15 tonnes on roads; 27–90 tonnes by rail), and barges (600–1200 tonnes).<a href="#cite_note-Greenwood796-77">[76]</a> Due to the difficulty and hazards in transporting elemental chlorine, production is typically located near where it is consumed. As examples, vinyl chloride producers such as <a href="/wiki/Westlake_Chemical" class="mw-redirect" title="Westlake Chemical">Westlake Chemical</a><a href="#cite_note-78">[77]</a> and <a href="/wiki/Formosa_Plastics" class="mw-redirect" title="Formosa Plastics">Formosa Plastics</a><a href="#cite_note-79">[78]</a> have integrated chloralkali assets. <div class="mw-heading mw-heading3"><h3 id="Chloralkali_processes">Chloralkali processes</h3></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Chloralkali_process" title="Chloralkali process">Chloralkali process</a></div> The electrolysis of chloride solutions all proceed according to the following equations: <dl><dd>Cathode: 2 H2O + 2 e− → H2 + 2 OH−</dd> <dd>Anode: 2 Cl− → Cl2 + 2 e−</dd></dl> In the conventional case where sodium chloride is electrolyzed, <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">sodium hydroxide</a> and chlorine are coproducts. Industrially, there are three chloralkali processes: <ul><li>The <a href="/wiki/Castner%E2%80%93Kellner_process" title="Castner–Kellner process">Castner–Kellner process</a> that utilizes a mercury electrode</li> <li>The diaphragm cell process that utilizes an asbestos diaphragm that separates the cathode and anode</li> <li>The membrane cell process that uses an <a href="/wiki/Ion_exchange" title="Ion exchange">ion exchange</a> membrane in place of the diaphragm</li></ul> The Castner–Kellner process was the first method used at the end of the nineteenth century to produce chlorine on an industrial scale.<a href="#cite_note-pauling-80">[79]</a><a href="#cite_note-lenn2-81">[80]</a> Mercury (that is toxic) was used as an electrode to <a href="/wiki/Sodium_amalgam" title="Sodium amalgam">amalgamate</a> the sodium product, preventing undesirable side reactions. In diaphragm cell electrolysis, an <a href="/wiki/Asbestos" title="Asbestos">asbestos</a> (or polymer-fiber) diaphragm separates a cathode and an <a href="/wiki/Anode" title="Anode">anode</a>, preventing the chlorine forming at the anode from re-mixing with the sodium hydroxide and the hydrogen formed at the cathode.<a href="#cite_note-Euro_Chlor3-82">[81]</a> The salt solution (brine) is continuously fed to the anode compartment and flows through the diaphragm to the cathode compartment, where the <a href="/wiki/Causticity" class="mw-redirect" title="Causticity">caustic</a> <a href="/wiki/Alkali" title="Alkali">alkali</a> is produced and the brine is partially depleted. Diaphragm methods produce dilute and slightly impure alkali, but they are not burdened with the problem of <a href="/wiki/Mercury_(element)" title="Mercury (element)">mercury</a> disposal and they are more energy efficient.<a href="#cite_note-Greenwood798-33">[32]</a> Membrane cell electrolysis employs <a href="/wiki/Semipermeable_membrane" title="Semipermeable membrane">permeable membrane</a> as an <a href="/wiki/Ion_exchange" title="Ion exchange">ion exchanger</a>. Saturated sodium (or potassium) chloride solution is passed through the anode compartment, leaving at a lower <a href="/wiki/Concentration" title="Concentration">concentration</a>. This method also produces very pure sodium (or potassium) hydroxide but has the disadvantage of requiring very pure brine at high concentrations.<a href="#cite_note-Euro_Chlor4-83">[82]</a> However, due to the lower energy requirements of the membrane process, new chlor-alkali installations are now almost exclusively employing the membrane process. Next to this, the use of large volumes of mercury is considered undesirable. Also, older plants are converted into the membrane process. <figure class="mw-default-size mw-halign-center" typeof="mw:File/Thumb"><a href="/wiki/File:Chloralkali_membrane.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/7a/Chloralkali_membrane.svg/610px-Chloralkali_membrane.svg.png" decoding="async" width="610" height="254" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/7a/Chloralkali_membrane.svg/915px-Chloralkali_membrane.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/7a/Chloralkali_membrane.svg/1220px-Chloralkali_membrane.svg.png 2x" data-file-width="1168" data-file-height="487" /></a><figcaption>Membrane cell process for chloralkali production</figcaption></figure> <div class="mw-heading mw-heading3"><h3 id="Non-chloralkali_processes">Non-chloralkali processes</h3></div> In the <a href="/wiki/Deacon_process" title="Deacon process">Deacon process</a>, hydrogen chloride recovered from the production of <a href="/wiki/Organochlorine_compound" class="mw-redirect" title="Organochlorine compound">organochlorine compounds</a> is recovered as chlorine. The process relies on oxidation using oxygen: <dl><dd>4 HCl + O2 → 2 Cl2 + 2 H2O</dd></dl> The reaction requires a catalyst. As introduced by Deacon, early catalysts were based on copper. Commercial processes, such as the Mitsui MT-Chlorine Process, have switched to chromium and ruthenium-based catalysts.<a href="#cite_note-chlorine-84">[83]</a> <div class="mw-heading mw-heading2"><h2 id="Applications">Applications</h2></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Tank_car_with_placard_1017_(chlorine).jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b6/Tank_car_with_placard_1017_%28chlorine%29.jpg/220px-Tank_car_with_placard_1017_%28chlorine%29.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/b6/Tank_car_with_placard_1017_%28chlorine%29.jpg/330px-Tank_car_with_placard_1017_%28chlorine%29.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/b6/Tank_car_with_placard_1017_%28chlorine%29.jpg/440px-Tank_car_with_placard_1017_%28chlorine%29.jpg 2x" data-file-width="4032" data-file-height="3024" /></a><figcaption>A railway <a href="/wiki/Tank_car" title="Tank car">tank car</a> carrying chlorine, displaying <a href="/wiki/Hazardous_materials" class="mw-redirect" title="Hazardous materials">hazardous materials</a> information including a diamond-shaped <a href="/wiki/Placard#United_States_Department_of_Transportation" title="Placard">U.S. DOT placard</a> showing a <a href="/wiki/UN_number" title="UN number">UN number</a><a href="#cite_note-:0-85">[84]</a></figcaption></figure> Sodium chloride is the most common chlorine compound, and is the main source of chlorine for the demand by the chemical industry. About 15000 chlorine-containing compounds are commercially traded, including such diverse compounds as chlorinated <a href="/wiki/Methane" title="Methane">methane</a>, <a href="/wiki/Ethane" title="Ethane">ethanes</a>, <a href="/wiki/Vinyl_chloride" title="Vinyl chloride">vinyl chloride</a>, <a href="/wiki/Polyvinyl_chloride" title="Polyvinyl chloride">polyvinyl chloride</a> (PVC), <a href="/wiki/Aluminium_trichloride" class="mw-redirect" title="Aluminium trichloride">aluminium trichloride</a> for <a href="/wiki/Catalysis" title="Catalysis">catalysis</a>, the chlorides of <a href="/wiki/Magnesium" title="Magnesium">magnesium</a>, <a href="/wiki/Titanium" title="Titanium">titanium</a>, <a href="/wiki/Zirconium" title="Zirconium">zirconium</a>, and <a href="/wiki/Hafnium" title="Hafnium">hafnium</a> which are the precursors for producing the pure form of those elements.<a href="#cite_note-Greenwood792-19">[18]</a> Quantitatively, of all elemental chlorine produced, about 63% is used in the manufacture of organic compounds, and 18% in the manufacture of inorganic chlorine compounds.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1997798-86">[85]</a> About 15,000 chlorine compounds are used commercially.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1997793-87">[86]</a> The remaining 19% of chlorine produced is used for bleaches and disinfection products.<a href="#cite_note-Greenwood796-77">[76]</a> The most significant of organic compounds in terms of production volume are <a href="/wiki/1,2-dichloroethane" class="mw-redirect" title="1,2-dichloroethane">1,2-dichloroethane</a> and <a href="/wiki/Vinyl_chloride" title="Vinyl chloride">vinyl chloride</a>, intermediates in the production of <a href="/wiki/Polyvinyl_chloride" title="Polyvinyl chloride">PVC</a>. Other particularly important organochlorines are <a href="/wiki/Methyl_chloride" class="mw-redirect" title="Methyl chloride">methyl chloride</a>, <a href="/wiki/Methylene_chloride" class="mw-redirect" title="Methylene chloride">methylene chloride</a>, <a href="/wiki/Chloroform" title="Chloroform">chloroform</a>, <a href="/wiki/Vinylidene_chloride" class="mw-redirect" title="Vinylidene chloride">vinylidene chloride</a>, <a href="/wiki/Trichloroethylene" title="Trichloroethylene">trichloroethylene</a>, <a href="/wiki/Perchloroethylene" class="mw-redirect" title="Perchloroethylene">perchloroethylene</a>, <a href="/wiki/Allyl_chloride" title="Allyl chloride">allyl chloride</a>, <a href="/wiki/Epichlorohydrin" title="Epichlorohydrin">epichlorohydrin</a>, <a href="/wiki/Chlorobenzene" title="Chlorobenzene">chlorobenzene</a>, <a href="/wiki/Dichlorobenzene" title="Dichlorobenzene">dichlorobenzenes</a>, and <a href="/wiki/Trichlorobenzene" title="Trichlorobenzene">trichlorobenzenes</a>. The major inorganic compounds include HCl, Cl2O, HOCl, NaClO3, <a href="/wiki/Aluminium_chloride" title="Aluminium chloride">AlCl3</a>, <a href="/wiki/Silicon_tetrachloride" title="Silicon tetrachloride">SiCl4</a>, <a href="/wiki/Tin(IV)_chloride" title="Tin(IV) chloride">SnCl4</a>, <a href="/wiki/Phosphorus_trichloride" title="Phosphorus trichloride">PCl3</a>, <a href="/wiki/Phosphorus_pentachloride" title="Phosphorus pentachloride">PCl5</a>, <a href="/wiki/Phosphoryl_chloride" title="Phosphoryl chloride">POCl3</a>, <a href="/wiki/Arsenic_trichloride" title="Arsenic trichloride">AsCl3</a>, <a href="/wiki/Antimony_trichloride" title="Antimony trichloride">SbCl3</a>, <a href="/wiki/Antimony_pentachloride" title="Antimony pentachloride">SbCl5</a>, <a href="/wiki/Bismuth_chloride" title="Bismuth chloride">BiCl3</a>, and <a href="/wiki/Zinc_chloride" title="Zinc chloride">ZnCl2</a>.<a href="#cite_note-Greenwood796-77">[76]</a> <div class="mw-heading mw-heading3"><h3 id="Sanitation,_disinfection,_and_antisepsis">Sanitation, disinfection, and antisepsis</h3></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main articles: <a href="/wiki/Water_chlorination" title="Water chlorination">Water chlorination</a> and <a href="/wiki/Bleach" title="Bleach">Bleach</a></div> <div class="mw-heading mw-heading4"><h4 id="Combating_putrefaction">Combating putrefaction</h4></div> In France (as elsewhere), <a href="/wiki/Catgut" title="Catgut">animal intestines</a> were processed to make musical instrument strings, <a href="/wiki/Goldbeater%27s_skin" title="Goldbeater's skin">Goldbeater's skin</a> and other products. This was done in "gut factories" (boyauderies), and it was an odiferous and unhealthy process. In or about 1820, the <a href="/wiki/Soci%C3%A9t%C3%A9_d%27encouragement_pour_l%27industrie_nationale" title="Société d'encouragement pour l'industrie nationale">Société d'encouragement pour l'industrie nationale</a> offered a prize for the discovery of a method, chemical or mechanical, for separating the <a href="/wiki/Peritoneum" title="Peritoneum">peritoneal</a> membrane of animal intestines without <a href="/wiki/Putrefaction" title="Putrefaction">putrefaction</a>.<a href="#cite_note-nbu-88">[87]</a><a href="#cite_note-knight-89">[88]</a> The prize was won by <a href="/wiki/Antoine-Germain_Labarraque" class="mw-redirect" title="Antoine-Germain Labarraque">Antoine-Germain Labarraque</a>, a 44-year-old French chemist and pharmacist who had discovered that Berthollet's chlorinated bleaching solutions ("<a href="/wiki/Javel_water" class="mw-redirect" title="Javel water">Eau de Javel</a>") not only destroyed the smell of putrefaction of animal tissue decomposition, but also actually retarded the decomposition.<a href="#cite_note-knight-89">[88]</a><a href="#cite_note-bouvet-35">[34]</a> Labarraque's research resulted in the use of chlorides and hypochlorites of lime (<a href="/wiki/Calcium_hypochlorite" title="Calcium hypochlorite">calcium hypochlorite</a>) and of sodium (<a href="/wiki/Sodium_hypochlorite" title="Sodium hypochlorite">sodium hypochlorite</a>) in the boyauderies. The same chemicals were found to be useful in the routine <a href="/wiki/Disinfectant" title="Disinfectant">disinfection</a> and deodorization of <a href="/wiki/Latrine" title="Latrine">latrines</a>, <a href="/wiki/Sewerage" title="Sewerage">sewers</a>, markets, <a href="/wiki/Abattoir" class="mw-redirect" title="Abattoir">abattoirs</a>, <a href="/wiki/Anatomical_theatre" title="Anatomical theatre">anatomical theatres</a>, and morgues.<a href="#cite_note-gedeon-90">[89]</a> They were successful in <a href="/wiki/Hospital" title="Hospital">hospitals</a>, <a href="/wiki/Lazaretto" title="Lazaretto">lazarets</a>, <a href="/wiki/Prison" title="Prison">prisons</a>, <a href="/wiki/Hospital" title="Hospital">infirmaries</a> (both on land and at sea), <a href="/wiki/Magnanery" title="Magnanery">magnaneries</a>, <a href="/wiki/Stable" title="Stable">stables</a>, cattle-sheds, etc.; and they were beneficial during <a href="/wiki/Exhumation" class="mw-redirect" title="Exhumation">exhumations</a>,<a href="#cite_note-91">[90]</a> <a href="/wiki/Embalming" title="Embalming">embalming</a>, outbreaks of epidemic disease, fever, and <a href="/wiki/Blackleg_(disease)" title="Blackleg (disease)">blackleg</a> in cattle.<a href="#cite_note-nbu-88">[87]</a> <div class="mw-heading mw-heading4"><h4 id="Disinfection">Disinfection</h4></div> Labarraque's chlorinated lime and soda solutions have been advocated since 1828 to prevent infection (called "contagious infection", presumed to be transmitted by "<a href="/wiki/Miasma_theory_of_disease" class="mw-redirect" title="Miasma theory of disease">miasmas</a>"), and to treat <a href="/wiki/Putrefaction" title="Putrefaction">putrefaction</a> of existing wounds, including septic wounds.<a href="#cite_note-92">[91]</a> In his 1828 work, Labarraque recommended that doctors breathe chlorine, wash their hands in chlorinated lime, and even sprinkle chlorinated lime about the patients' beds in cases of "contagious infection". In 1828, the contagion of infections was well known, even though the agency of the <a href="/wiki/Microorganism" title="Microorganism">microbe</a> was not discovered until more than half a century later. During the <a href="/wiki/1832_cholera_epidemic" class="mw-redirect" title="1832 cholera epidemic">Paris cholera outbreak</a> of 1832, large quantities of so-called chloride of lime were used to disinfect the capital. This was not simply modern <a href="/wiki/Calcium_chloride" title="Calcium chloride">calcium chloride</a>, but chlorine gas dissolved in lime-water (dilute <a href="/wiki/Calcium_hydroxide" title="Calcium hydroxide">calcium hydroxide</a>) to form <a href="/wiki/Calcium_hypochlorite" title="Calcium hypochlorite">calcium hypochlorite</a> (chlorinated lime). Labarraque's discovery helped to remove the terrible stench of decay from hospitals and dissecting rooms, and by doing so, effectively deodorised the <a href="/wiki/Latin_Quarter,_Paris" title="Latin Quarter, Paris">Latin Quarter</a> of Paris.<a href="#cite_note-corbin-93">[92]</a> These "putrid miasmas" were thought by many to cause the spread of "contagion" and "infection" – both words used before the germ theory of infection. Chloride of lime was used for destroying odors and "putrid matter". One source claims chloride of lime was used by Dr. John Snow to disinfect water from the cholera-contaminated well that was feeding the Broad Street pump in 1854 London,<a href="#cite_note-94">[93]</a> though three other reputable sources that describe that famous cholera epidemic do not mention the incident.<a href="#cite_note-Vinten-95">[94]</a><a href="#cite_note-96">[95]</a><a href="#cite_note-97">[96]</a> One reference makes it clear that chloride of lime was used to disinfect the <a href="/wiki/Offal" title="Offal">offal</a> and filth in the streets surrounding the Broad Street pump – a common practice in mid-nineteenth century England.<a href="#cite_note-Vinten-95">[94]</a>: 296  <div class="mw-heading mw-heading4"><h4 id="Semmelweis_and_experiments_with_antisepsis">Semmelweis and experiments with antisepsis</h4></div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Semmelweis_Ign%C3%A1c.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/Semmelweis_Ign%C3%A1c.jpg/130px-Semmelweis_Ign%C3%A1c.jpg" decoding="async" width="130" height="184" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/Semmelweis_Ign%C3%A1c.jpg/195px-Semmelweis_Ign%C3%A1c.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a2/Semmelweis_Ign%C3%A1c.jpg/260px-Semmelweis_Ign%C3%A1c.jpg 2x" data-file-width="1009" data-file-height="1428" /></a><figcaption><a href="/wiki/Ignaz_Semmelweis" title="Ignaz Semmelweis">Ignaz Semmelweis</a></figcaption></figure> Perhaps the most famous application of Labarraque's chlorine and <a href="/wiki/Base_(chemistry)" title="Base (chemistry)">chemical base</a> solutions was in 1847, when <a href="/wiki/Ignaz_Semmelweis" title="Ignaz Semmelweis">Ignaz Semmelweis</a> used chlorine-water (chlorine dissolved in pure water, which was cheaper than chlorinated lime solutions) to disinfect the hands of Austrian doctors, which Semmelweis noticed still carried the stench of decomposition from the dissection rooms to the patient examination rooms. Long before the germ theory of disease, Semmelweis theorized that "cadaveric particles" were transmitting decay from fresh medical cadavers to living patients, and he used the well-known "Labarraque's solutions" as the only known method to remove the smell of decay and tissue decomposition (which he found that soap did not). The solutions proved to be far more effective antiseptics than soap (Semmelweis was also aware of their greater efficacy, but not the reason), and this resulted in Semmelweis's celebrated success in stopping the transmission of <a href="/wiki/Childbed_fever" class="mw-redirect" title="Childbed fever">childbed fever</a> ("puerperal fever") in the maternity wards of <a href="/wiki/Vienna_General_Hospital" title="Vienna General Hospital">Vienna General Hospital</a> in <a href="/wiki/Austria" title="Austria">Austria</a> in 1847.<a href="#cite_note-98">[97]</a> Much later, during World War I in 1916, a standardized and diluted modification of Labarraque's solution containing hypochlorite (0.5%) and boric acid as an acidic stabilizer was developed by <a href="/wiki/Henry_Drysdale_Dakin" title="Henry Drysdale Dakin">Henry Drysdale Dakin</a> (who gave full credit to Labarraque's prior work in this area). Called <a href="/wiki/Dakin%27s_solution" title="Dakin's solution">Dakin's solution</a>, the method of wound irrigation with chlorinated solutions allowed antiseptic treatment of a wide variety of open wounds, long before the modern antibiotic era. A modified version of this solution continues to be employed in wound irrigation in modern times, where it remains effective against bacteria that are resistant to multiple antibiotics (see <a href="/wiki/Century_Pharmaceuticals" title="Century Pharmaceuticals">Century Pharmaceuticals</a>).<a href="#cite_note-99">[98]</a> <div style="clear:both;" class=""></div> <div class="mw-heading mw-heading4"><h4 id="Public_sanitation">Public sanitation</h4></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Mosul-swimming.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/7e/Mosul-swimming.jpg/220px-Mosul-swimming.jpg" decoding="async" width="220" height="241" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/7e/Mosul-swimming.jpg/330px-Mosul-swimming.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/7/7e/Mosul-swimming.jpg 2x" data-file-width="411" data-file-height="450" /></a><figcaption>Chlorinated water is used in <a href="/wiki/Swimming_pools" class="mw-redirect" title="Swimming pools">swimming pools</a> to disinfect water from microbial contaminants</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Liquid_Pool_Chlorine.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/62/Liquid_Pool_Chlorine.jpg/220px-Liquid_Pool_Chlorine.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/62/Liquid_Pool_Chlorine.jpg/330px-Liquid_Pool_Chlorine.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/62/Liquid_Pool_Chlorine.jpg/440px-Liquid_Pool_Chlorine.jpg 2x" data-file-width="4160" data-file-height="3120" /></a><figcaption>Liquid pool chlorine</figcaption></figure> The first continuous application of chlorination to drinking U.S. water was installed in <a href="/wiki/Jersey_City" class="mw-redirect" title="Jersey City">Jersey City</a>, New Jersey, in 1908.<a href="#cite_note-100">[99]</a> By 1918, the <a href="/wiki/US_Department_of_Treasury" class="mw-redirect" title="US Department of Treasury">US Department of Treasury</a> called for all drinking water to be disinfected with chlorine. Chlorine is presently an important chemical for <a href="/wiki/Water_purification" title="Water purification">water purification</a> (such as in water treatment plants), in <a href="/wiki/Disinfectant" title="Disinfectant">disinfectants</a>, and in <a href="/wiki/Bleach" title="Bleach">bleach</a>. Even small water supplies are now routinely chlorinated.<a href="#cite_note-CRC-101">[100]</a> Chlorine is usually used (in the form of <a href="/wiki/Hypochlorous_acid" title="Hypochlorous acid">hypochlorous acid</a>) to kill <a href="/wiki/Bacteria" title="Bacteria">bacteria</a> and other microbes in <a href="/wiki/Drinking_water" title="Drinking water">drinking water</a> supplies and public swimming pools. In most private swimming pools, chlorine itself is not used, but rather <a href="/wiki/Sodium_hypochlorite" title="Sodium hypochlorite">sodium hypochlorite</a>, formed from chlorine and <a href="/wiki/Sodium_hydroxide" title="Sodium hydroxide">sodium hydroxide</a>, or solid tablets of chlorinated isocyanurates. The drawback of using chlorine in swimming pools is that the chlorine reacts with the <a href="/wiki/Amino_acid" title="Amino acid">amino acids</a> in proteins in human hair and skin. Contrary to popular belief, the distinctive "chlorine aroma" associated with swimming pools is not the result of elemental chlorine itself, but of <a href="/wiki/Monochloramine" title="Monochloramine">chloramine</a>, a chemical compound produced by the reaction of free dissolved chlorine with amines in organic substances including those in urine and sweat.<a href="#cite_note-102">[101]</a> As a disinfectant in water, chlorine is more than three times as effective against <a href="/wiki/Escherichia_coli" title="Escherichia coli">Escherichia coli</a> as <a href="/wiki/Bromine" title="Bromine">bromine</a>, and more than six times as effective as <a href="/wiki/Iodine" title="Iodine">iodine</a>.<a href="#cite_note-103">[102]</a> Increasingly, <a href="/wiki/Monochloramine" title="Monochloramine">monochloramine</a> itself is being directly added to drinking water for purposes of disinfection, a process known as <a href="/wiki/Chloramination" title="Chloramination">chloramination</a>.<a href="#cite_note-CDC-Chloramination-104">[103]</a> It is often impractical to store and use poisonous chlorine gas for water treatment, so alternative methods of adding chlorine are used. These include <a href="/wiki/Hypochlorite" title="Hypochlorite">hypochlorite</a> solutions, which gradually release chlorine into the water, and compounds like <a href="/wiki/Sodium_dichloro-s-triazinetrione" class="mw-redirect" title="Sodium dichloro-s-triazinetrione">sodium dichloro-s-triazinetrione</a> (dihydrate or anhydrous), sometimes referred to as "dichlor", and <a href="/wiki/Trichloro-s-triazinetrione" class="mw-redirect" title="Trichloro-s-triazinetrione">trichloro-s-triazinetrione</a>, sometimes referred to as "trichlor". These compounds are stable while solid and may be used in powdered, granular, or tablet form. When added in small amounts to pool water or industrial water systems, the chlorine atoms hydrolyze from the rest of the molecule, forming hypochlorous acid (HOCl), which acts as a general <a href="/wiki/Biocide" title="Biocide">biocide</a>, killing germs, microorganisms, algae, and so on.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1997860-105">[104]</a><a href="#cite_note-106">[105]</a> <div class="mw-heading mw-heading3"><h3 id="Use_as_a_weapon">Use as a weapon</h3></div> <div class="mw-heading mw-heading4"><h4 id="World_War_I">World War I</h4></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Chemical_weapons_in_World_War_I" title="Chemical weapons in World War I">Chemical weapons in World War I</a></div> Chlorine gas, also known as bertholite, was first <a href="/wiki/Chemical_warfare" title="Chemical warfare">used as a weapon</a> in <a href="/wiki/World_War_I" title="World War I">World War I</a> by Germany on April 22, 1915, in the <a href="/wiki/Second_Battle_of_Ypres" title="Second Battle of Ypres">Second Battle of Ypres</a>.<a href="#cite_note-107">[106]</a><a href="#cite_note-CEN2015-108">[107]</a> As described by the soldiers, it had the distinctive smell of a mixture of pepper and pineapple.<a href="#cite_note-109">[108]</a> It also tasted metallic and stung the back of the throat and chest. Chlorine reacts with water in the <a href="/wiki/Mucous_membrane" title="Mucous membrane">mucosa</a> of the lungs to form <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">hydrochloric acid</a>, destructive to living tissue and potentially lethal. Human respiratory systems can be protected from chlorine gas by <a href="/wiki/Gas_mask" title="Gas mask">gas masks</a> with <a href="/wiki/Activated_charcoal" class="mw-redirect" title="Activated charcoal">activated charcoal</a> or other filters, which makes chlorine gas much less lethal than other chemical weapons. It was pioneered by a German scientist later to be a Nobel laureate, <a href="/wiki/Fritz_Haber" title="Fritz Haber">Fritz Haber</a> of the <a href="/wiki/Kaiser_Wilhelm_Institute_for_Chemistry" class="mw-redirect" title="Kaiser Wilhelm Institute for Chemistry">Kaiser Wilhelm Institute</a> in Berlin, in collaboration with the German chemical conglomerate <a href="/wiki/IG_Farben" title="IG Farben">IG Farben</a>, which developed methods for discharging chlorine gas against an <a href="/wiki/Trench" title="Trench">entrenched</a> enemy.<a href="#cite_note-110">[109]</a> After its first use, both sides in the conflict used chlorine as a chemical weapon, but it was soon replaced by the more deadly <a href="/wiki/Phosgene" title="Phosgene">phosgene</a> and <a href="/wiki/Mustard_gas" title="Mustard gas">mustard gas</a>.<a href="#cite_note-First_World_War-111">[110]</a> <div class="mw-heading mw-heading4"><h4 id="Middle_east">Middle east</h4></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main articles: <a href="/wiki/Chlorine_bombings_in_Iraq" title="Chlorine bombings in Iraq">Chlorine bombings in Iraq</a> and <a href="/wiki/Use_of_chemical_weapons_in_the_Syrian_Civil_War" class="mw-redirect" title="Use of chemical weapons in the Syrian Civil War">Use of chemical weapons in the Syrian Civil War</a></div> Chlorine gas was also used during the <a href="/wiki/Iraq_War_in_Anbar_Province" class="mw-redirect" title="Iraq War in Anbar Province">Iraq War in Anbar Province</a> in 2007, with insurgents packing <a href="/wiki/Truck_bomb" class="mw-redirect" title="Truck bomb">truck bombs</a> with <a href="/wiki/Mortar_(weapon)" title="Mortar (weapon)">mortar</a> shells and chlorine tanks. The attacks killed two people from the explosives and sickened more than 350. Most of the deaths were caused by the force of the explosions rather than the effects of chlorine since the toxic gas is readily dispersed and diluted in the atmosphere by the blast. In some bombings, over a hundred civilians were hospitalized due to breathing difficulties. The Iraqi authorities tightened security for elemental chlorine, which is essential for providing safe drinking water to the population.<a href="#cite_note-cnnchlorine-112">[111]</a><a href="#cite_note-Chlorine_bomb_BBC-113">[112]</a> On 23 October 2014, it was reported that the <a href="/wiki/Islamic_State_of_Iraq_and_the_Levant" class="mw-redirect" title="Islamic State of Iraq and the Levant">Islamic State of Iraq and the Levant</a> had used chlorine gas in the town of Duluiyah, <a href="/wiki/Iraq" title="Iraq">Iraq</a>.<a href="#cite_note-114">[113]</a> Laboratory analysis of clothing and soil samples confirmed the use of chlorine gas against Kurdish <a href="/wiki/Peshmerga" title="Peshmerga">Peshmerga</a> Forces in a vehicle-borne improvised explosive device attack on 23 January 2015 at the Highway 47 Kiske Junction near Mosul.<a href="#cite_note-115">[114]</a> Another country in the middle east, <a href="/wiki/Syria" title="Syria">Syria</a>, has used chlorine as a <a href="/wiki/Chemical_weapon" title="Chemical weapon">chemical weapon</a><a href="#cite_note-116">[115]</a> delivered from <a href="/wiki/Barrel_bomb" title="Barrel bomb">barrel bombs</a> and rockets.<a href="#cite_note-117">[116]</a><a href="#cite_note-118">[117]</a> In 2016, the <a href="/wiki/OPCW-UN_Joint_Investigative_Mechanism" title="OPCW-UN Joint Investigative Mechanism">OPCW-UN Joint Investigative Mechanism</a> concluded that the Syrian government used chlorine as a chemical weapon in three separate attacks.<a href="#cite_note-119">[118]</a> Later investigations from the OPCW's Investigation and Identification Team concluded that the <a href="/wiki/Syrian_Air_Force" title="Syrian Air Force">Syrian Air Force</a> was responsible for chlorine attacks in 2017 and 2018.<a href="#cite_note-120">[119]</a> <div class="mw-heading mw-heading2"><h2 id="Biological_role">Biological role</h2></div> The <a href="/wiki/Chloride" title="Chloride">chloride</a> anion is an <a href="/wiki/Mineral_(nutrient)" title="Mineral (nutrient)">essential nutrient</a> for metabolism. Chlorine is needed for the production of <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">hydrochloric acid</a> in the stomach and in cellular pump functions.<a href="#cite_note-121">[120]</a> The main dietary source is table salt, or sodium chloride. Overly low or high concentrations of chloride in the blood are examples of <a href="/wiki/Electrolyte_disturbance" class="mw-redirect" title="Electrolyte disturbance">electrolyte disturbances</a>. <a href="/wiki/Hypochloremia" title="Hypochloremia">Hypochloremia</a> (having too little chloride) rarely occurs in the absence of other abnormalities. It is sometimes associated with <a href="/wiki/Hypoventilation" title="Hypoventilation">hypoventilation</a>.<a href="#cite_note-pmid3764530-122">[121]</a> It can be associated with chronic <a href="/wiki/Respiratory_acidosis" title="Respiratory acidosis">respiratory acidosis</a>.<a href="#cite_note-pmid13611033-123">[122]</a> <a href="/wiki/Hyperchloremia" title="Hyperchloremia">Hyperchloremia</a> (having too much chloride) usually does not produce symptoms. When symptoms do occur, they tend to resemble those of <a href="/wiki/Hypernatremia" title="Hypernatremia">hypernatremia</a> (having too much <a href="/wiki/Sodium" title="Sodium">sodium</a>). Reduction in blood chloride leads to cerebral dehydration; symptoms are most often caused by rapid rehydration which results in <a href="/wiki/Cerebral_edema" title="Cerebral edema">cerebral edema</a>. Hyperchloremia can affect oxygen transport.<a href="#cite_note-pmid9760315-124">[123]</a> <div class="mw-heading mw-heading2"><h2 id="Hazards">Hazards</h2></div> <style data-mw-deduplicate="TemplateStyles:r1268415487">.mw-parser-output .ib-chembox{border-collapse:collapse;text-align:left}.mw-parser-output .ib-chembox td,.mw-parser-output .ib-chembox th{border:1px solid #a2a9b1;width:40%}.mw-parser-output .ib-chembox td+td{width:60%}@media screen{html.skin-theme-clientpref-night .mw-parser-output .ib-chembox figure:not(.skin-invert-image):not(.skin-invert):not(.bg-transparent){background:var(--background-color-inverted,#f8f9fa)}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .ib-chembox figure:not(.skin-invert-image):not(.skin-invert):not(.bg-transparent){background:var(--background-color-inverted,#f8f9fa)}}</style> <table class="infobox ib-chembox"> <caption>Chlorine </caption> <tbody><tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Hazards </th></tr> <tr> <td colspan="2" style="text-align:left; background-color:#eaeaea;color:inherit;"><a href="/wiki/Globally_Harmonized_System_of_Classification_and_Labelling_of_Chemicals" title="Globally Harmonized System of Classification and Labelling of Chemicals">GHS labelling</a>:<a href="#cite_note-125">[124]</a> </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/GHS_hazard_pictograms" title="GHS hazard pictograms">Pictograms</a></div> </td> <td><a href="/wiki/File:GHS-pictogram-rondflam.svg" class="mw-file-description" title="GHS03: Oxidizing"><img alt="GHS03: Oxidizing" src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e5/GHS-pictogram-rondflam.svg/50px-GHS-pictogram-rondflam.svg.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/e5/GHS-pictogram-rondflam.svg/75px-GHS-pictogram-rondflam.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/e5/GHS-pictogram-rondflam.svg/100px-GHS-pictogram-rondflam.svg.png 2x" data-file-width="724" data-file-height="724" /></a> <a href="/wiki/File:GHS-pictogram-skull.svg" class="mw-file-description" title="GHS06: Toxic"><img alt="GHS06: Toxic" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/58/GHS-pictogram-skull.svg/50px-GHS-pictogram-skull.svg.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/58/GHS-pictogram-skull.svg/75px-GHS-pictogram-skull.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/58/GHS-pictogram-skull.svg/100px-GHS-pictogram-skull.svg.png 2x" data-file-width="724" data-file-height="724" /></a> <a href="/wiki/File:GHS-pictogram-pollu.svg" class="mw-file-description" title="GHS09: Environmental hazard"><img alt="GHS09: Environmental hazard" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b9/GHS-pictogram-pollu.svg/50px-GHS-pictogram-pollu.svg.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/b9/GHS-pictogram-pollu.svg/75px-GHS-pictogram-pollu.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/b9/GHS-pictogram-pollu.svg/100px-GHS-pictogram-pollu.svg.png 2x" data-file-width="724" data-file-height="724" /></a> </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Globally_Harmonized_System_of_Classification_and_Labelling_of_Chemicals#Signal_word" title="Globally Harmonized System of Classification and Labelling of Chemicals">Signal word</a></div> </td> <td>Danger </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/GHS_hazard_statements" title="GHS hazard statements">Hazard statements</a></div> </td> <td><abbr class="abbr" title="H270: May cause or intensify fire: oxidizer">H270</abbr>, <abbr class="abbr" title="H315: Causes skin irritation">H315</abbr>, <abbr class="abbr" title="H319: Causes serious eye irritation">H319</abbr>, <abbr class="abbr" title="H330: Fatal if inhaled">H330</abbr>, <abbr class="abbr" title="H335: May cause respiratory irritation">H335</abbr>, <abbr class="abbr" title="H400: Very toxic to aquatic life">H400</abbr> </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/GHS_precautionary_statements" title="GHS precautionary statements">Precautionary statements</a></div> </td> <td><abbr class="abbr" title="P220: Keep/Store away from clothing/.../combustible materials.">P220</abbr>, <abbr class="abbr" title="P233: Keep container tightly closed.">P233</abbr>, <abbr class="abbr" title="P244: Keep valves and fittings free from grease and oil">P244</abbr>, <abbr class="abbr" title="P261: Avoid breathing dust/fume/gas/mist/vapours/spray.">P261</abbr>, <abbr class="abbr" title="P304: IF INHALED:">P304</abbr>, <abbr class="abbr" title="P312: Call a POISON CENTER or doctor/physician if you feel unwell.">P312</abbr>, <abbr class="abbr" title="P340: Remove victim to fresh air and keep at rest in a position comfortable for breathing.">P340</abbr>, <abbr class="abbr" title="P403: Store in a well ventilated place.">P403</abbr>, <abbr class="abbr" title="P410: Protect from sunlight.">P410</abbr> </td></tr> <tr> <td><a href="/wiki/NFPA_704" title="NFPA 704">NFPA 704</a> (fire diamond) </td> <td><style data-mw-deduplicate="TemplateStyles:r1170367383">.mw-parser-output .nfpa-704-diamond-ref{float:right;padding:1px;text-align:right}.mw-parser-output .nfpa-704-diamond-container{width:82px;font-family:sans-serif;margin:0 auto}.mw-parser-output .nfpa-704-diamond-container-ref{float:left;margin-left:1em}.mw-parser-output .nfpa-704-diamond-images{float:left;font-size:20px;text-align:center;position:relative;height:80px;width:80px;padding:1px}.mw-parser-output .nfpa-704-diamond-map{position:absolute;height:80px;width:80px}.mw-parser-output .nfpa-704-diamond .noresize{margin:0 auto}.mw-parser-output .nfpa-704-diamond-code{line-height:1em;text-align:center;position:absolute}.mw-parser-output .nfpa-704-diamond-code>a{color:black}.mw-parser-output .nfpa-704-diamond-blue{width:13px;top:31px;left:15px}.mw-parser-output .nfpa-704-diamond-red{width:12px;top:12px;left:35px}.mw-parser-output .nfpa-704-diamond-yellow{width:13px;top:31px;left:54px}.mw-parser-output .nfpa-704-diamond-white-image{position:relative;top:51px;left:0}.mw-parser-output .nfpa-704-diamond-white-text{vertical-align:middle;text-align:center;line-height:80%;position:absolute;top:52px}.mw-parser-output .nfpa-704-diamond-white-text a>span{position:absolute;color:black}.mw-parser-output .nfpa-704-diamond-white-wors{font-size:15px;width:23px;left:29px}.mw-parser-output .nfpa-704-diamond-white-wox{font-size:15px;font-stretch:condensed;width:21px;line-height:80%;top:-4px;left:29px}.mw-parser-output .nfpa-704-diamond-white-abcp{font-size:13.5px;font-stretch:condensed;width:28px;left:26px}.mw-parser-output .nfpa-704-diamond-white-ac{font-size:10px;width:30px;left:25px}.mw-parser-output .nfpa-704-diamond-white-strike{text-decoration:line-through}</style><div class="nfpa-704-diamond notheme"><div class="nfpa-74-diamond-refs"><a href="#cite_note-126">[125]</a></div><div class="nfpa-704-diamond-container nfpa-704-diamond-container-ref"><div class="nfpa-704-diamond-images nounderlines"> <div class="nfpa-704-diamond-map"><figure class="noresize" typeof="mw:File"><img alt="NFPA 704 four-colored diamond" src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/80px-NFPA_704.svg.png" decoding="async" width="80" height="80" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/120px-NFPA_704.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/6f/NFPA_704.svg/160px-NFPA_704.svg.png 2x" data-file-width="512" data-file-height="512" usemap="#ImageMap_96e46620850bc48d" /><map name="ImageMap_96e46620850bc48d"><area href="/wiki/NFPA_704#Blue" shape="poly" coords="23,23,47,47,23,70,0,47" alt="Health 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gas" title="Health 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gas" /><area href="/wiki/NFPA_704#Red" shape="poly" coords="47,0,70,23,47,47,23,23" alt="Flammability 0: Will not burn. E.g. water" title="Flammability 0: Will not burn. E.g. water" /><area href="/wiki/NFPA_704#Yellow" shape="poly" coords="70,23,94,47,70,70,47,47" alt="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" title="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" /><area href="/wiki/NFPA_704#White" shape="poly" coords="47,47,70,70,47,94,23,70" alt="Special hazard OX: Oxidizer. E.g. potassium perchlorate" title="Special hazard OX: Oxidizer. E.g. potassium perchlorate" /></map><figcaption></figcaption></figure></div><div class="nfpa-704-diamond-code nfpa-704-diamond-blue"> <a href="/wiki/NFPA_704#Blue" title="NFPA 704">3</a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-red"> <a href="/wiki/NFPA_704#Red" title="NFPA 704">0</a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-yellow"> <a href="/wiki/NFPA_704#Yellow" title="NFPA 704">0</a></div><div class="nfpa-704-diamond-white-text mw-no-invert"><a href="/wiki/NFPA_704#White" title="NFPA 704">OX</a></div></div></div></div> </td></tr> </tbody></table><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical compound</div> Chlorine is a toxic gas that attacks the respiratory system, eyes, and skin.<a href="#cite_note-127">[126]</a> Because it is denser than air, it tends to accumulate at the bottom of poorly ventilated spaces. Chlorine gas is a strong oxidizer, which may react with flammable materials.<a href="#cite_note-msds-cl-128">[127]</a><a href="#cite_note-129">[128]</a> Chlorine is detectable with measuring devices in concentrations as low as 0.2 parts per million (ppm), and by smell at 3 ppm. Coughing and vomiting may occur at 30 ppm and lung damage at 60 ppm. About 1000 ppm can be fatal after a few deep breaths of the gas.<a href="#cite_note-Greenwood792-19">[18]</a> The <a href="/wiki/IDLH" class="mw-redirect" title="IDLH">IDLH</a> (immediately dangerous to life and health) concentration is 10 ppm.<a href="#cite_note-NIOSH-130">[129]</a> Breathing lower concentrations can aggravate the respiratory system and exposure to the gas can irritate the eyes.<a href="#cite_note-tox-131">[130]</a> When chlorine is inhaled at concentrations greater than 30 ppm, it reacts with water within the lungs, producing <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">hydrochloric acid</a> (HCl) and <a href="/wiki/Hypochlorous_acid" title="Hypochlorous acid">hypochlorous acid</a> (HOCl). When used at specified levels for water disinfection, the reaction of chlorine with water is not a major concern for human health. Other materials present in the water may generate <a href="/wiki/Disinfection_by-products" class="mw-redirect" title="Disinfection by-products">disinfection by-products</a> that are associated with negative effects on human health.<a href="#cite_note-132">[131]</a><a href="#cite_note-133">[132]</a> In the United States, the <a href="/wiki/Occupational_Safety_and_Health_Administration" title="Occupational Safety and Health Administration">Occupational Safety and Health Administration</a> (OSHA) has set the <a href="/wiki/Permissible_exposure_limit" title="Permissible exposure limit">permissible exposure limit</a> for elemental chlorine at 1 ppm, or 3 mg/m3. The <a href="/wiki/National_Institute_for_Occupational_Safety_and_Health" title="National Institute for Occupational Safety and Health">National Institute for Occupational Safety and Health</a> has designated a <a href="/wiki/Recommended_exposure_limit" title="Recommended exposure limit">recommended exposure limit</a> of 0.5 ppm over 15 minutes.<a href="#cite_note-NIOSH-130">[129]</a> In the home, accidents occur when hypochlorite bleach solutions come into contact with certain acidic drain-cleaners to produce chlorine gas.<a href="#cite_note-134">[133]</a> Hypochlorite bleach (a popular <a href="/wiki/Laundry" title="Laundry">laundry</a> additive) combined with <a href="/wiki/Ammonia" title="Ammonia">ammonia</a> (another popular laundry additive) produces <a href="/wiki/Chloramines" title="Chloramines">chloramines</a>, another toxic group of chemicals.<a href="#cite_note-135">[134]</a> <div class="mw-heading mw-heading3"><h3 id="Chlorine-induced_cracking_in_structural_materials">Chlorine-induced cracking in structural materials</h3></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Chlorine_attack1.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/10/Chlorine_attack1.jpg/220px-Chlorine_attack1.jpg" decoding="async" width="220" height="153" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/10/Chlorine_attack1.jpg/330px-Chlorine_attack1.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/10/Chlorine_attack1.jpg/440px-Chlorine_attack1.jpg 2x" data-file-width="720" data-file-height="500" /></a><figcaption>Chlorine "attack" on an acetal resin plumbing joint resulting from a fractured acetal joint in a water supply system which started at an <a href="/wiki/Injection_molding" class="mw-redirect" title="Injection molding">injection molding</a> defect in the joint and slowly grew until the part failed. The fracture surface shows iron and calcium salts that were deposited in the leaking joint from the water supply before failure and are the indirect result of the chlorine attack.</figcaption></figure> Chlorine is widely used for purifying water, especially potable water supplies and water used in swimming pools. Several catastrophic collapses of swimming pool ceilings have occurred from chlorine-induced <a href="/wiki/Stress_corrosion_cracking" title="Stress corrosion cracking">stress corrosion cracking</a> of <a href="/wiki/Stainless_steel" title="Stainless steel">stainless steel</a> suspension rods.<a href="#cite_note-136">[135]</a> Some <a href="/wiki/Polymer" title="Polymer">polymers</a> are also sensitive to attack, including <a href="/wiki/Acetal_resin" class="mw-redirect" title="Acetal resin">acetal resin</a> and <a href="/wiki/Polybutene" title="Polybutene">polybutene</a>. Both materials were used in hot and cold water domestic plumbing, and <a href="/wiki/Stress_corrosion_cracking" title="Stress corrosion cracking">stress corrosion cracking</a> caused widespread failures in the US in the 1980s and 1990s.<a href="#cite_note-137">[136]</a> <div class="mw-heading mw-heading3"><h3 id="Chlorine-iron_fire">Chlorine-iron fire</h3></div> The element <a href="/wiki/Iron" title="Iron">iron</a> can combine with chlorine at high temperatures in a strong exothermic reaction, creating a chlorine-iron fire.<a href="#cite_note-bayerdatasheet2008-138">[137]</a><a href="#cite_note-sanders2004-139">[138]</a> Chlorine-iron fires are a risk in chemical process plants, where much of the pipework that carries chlorine gas is made of steel.<a href="#cite_note-bayerdatasheet2008-138">[137]</a><a href="#cite_note-sanders2004-139">[138]</a> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2></div> <ul><li><a href="/wiki/2022_Aqaba_toxic_gas_leak" title="2022 Aqaba toxic gas leak">2022 Aqaba toxic gas leak</a></li> <li><a href="/wiki/Chlorine_cycle" title="Chlorine cycle">Chlorine cycle</a></li> <li><a href="/wiki/Chlorine_gas_poisoning" title="Chlorine gas poisoning">Chlorine gas poisoning</a></li> <li><a href="/wiki/Industrial_gas" title="Industrial gas">Industrial gas</a></li> <li><a href="/wiki/Polymer_degradation" title="Polymer degradation">Polymer degradation</a></li> <li><a href="/wiki/Reductive_dechlorination" title="Reductive dechlorination">Reductive dechlorination</a></li></ul> <div class="mw-heading mw-heading2"><h2 id="Notes">Notes</h2></div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist"> <div class="mw-references-wrap"><ol class="references"> <li id="cite_note-16"><a href="#cite_ref-16">^</a> <style data-mw-deduplicate="TemplateStyles:r1238218222">.mw-parser-output cite.citation{font-style:inherit;word-wrap:break-word}.mw-parser-output .citation q{quotes:"\"""\"""'""'"}.mw-parser-output .citation:target{background-color:rgba(0,127,255,0.133)}.mw-parser-output .id-lock-free.id-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-subscription.id-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-free a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-limited a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-registration a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain;padding:0 1em 0 0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite id="CITEREFvan_Helmont1682" class="citation book cs1 cs1-prop-foreign-lang-source">van Helmont, Joannis Baptistae (1682). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=Qy5AAAAAcAAJ&pg=PP5">Opera omnia [All Works]</a> (in Latin). Frankfurt-am-Main, (Germany): Johann Just Erythropel.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Opera+omnia+%5BAll+Works%5D&rft.place=Frankfurt-am-Main%2C+%28Germany%29&rft.pub=Johann+Just+Erythropel&rft.date=1682&rft.aulast=van+Helmont&rft.aufirst=Joannis+Baptistae&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DQy5AAAAAcAAJ%26pg%3DPP5&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> From "Complexionum atque mistionum elementalium figmentum." (Formation of combinations and of mixtures of elements), §37, <a rel="nofollow" class="external text" href="https://books.google.com/books?id=Qy5AAAAAcAAJ&pg=PA105">p. 105:</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20231230133537/https://books.google.com/books?id=Qy5AAAAAcAAJ&pg=PA105#v=onepage&q&f=false">Archived</a> 2023-12-30 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a> "Accipe salis petrae, vitrioli, & alumnis partes aequas: exsiccato singula, & connexis simul, distilla aquam. Quae nil aliud est, quam merum sal volatile. Hujus accipe uncias quatuor, salis armeniaci unciam junge, in forti vitro, alembico, per caementum (ex cera, colophonia, & vitri pulverre) calidissime affusum, firmato; mox, etiam in frigore, Gas excitatur, & vas, utut forte, dissilit cum fragore." (Take equal parts of saltpeter [i.e., sodium nitrate], vitriol [i.e., concentrated sulfuric acid], and alum: dry each and combine simultaneously; distill off the water [i.e., liquid]. That [distillate] is nothing else than pure volatile salt [i.e., spirit of nitre, nitric acid]. Take four ounces of this [viz, nitric acid], add one ounce of Armenian salt [i.e., ammonium chloride], [place it] in a strong glass alembic sealed by cement ([made] from wax, rosin, and powdered glass) [that has been] poured very hot; soon, even in the cold, gas is stimulated, and the vessel, however strong, bursts into fragments.) From "De Flatibus" (On gases), <a rel="nofollow" class="external text" href="https://books.google.com/books?id=Qy5AAAAAcAAJ&pg=PA408">p. 408</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20231230133615/https://books.google.com/books?id=Qy5AAAAAcAAJ&pg=PA408#v=onepage&q&f=false">Archived</a> 2023-12-30 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a>: "Sal armeniacus enim, & aqua chrysulca, quae singula per se distillari, possunt, & pati calorem: sin autem jungantur, & intepescant, non possunt non, quin statim in Gas sylvestre, sive incoercibilem flatum transmutentur." (Truly Armenian salt [i.e., ammonium chloride] and nitric acid, each of which can be distilled by itself, and submitted to heat; but if, on the other hand, they be combined and become warm, they cannot but be changed immediately into carbon dioxide [note: van Helmont's identification of the gas is mistaken] or an incondensable gas.) See also: <ul><li><a rel="nofollow" class="external text" href="https://www.encyclopedia.com/people/science-and-technology/chemistry-biographies/johannes-joan-baptista-van-helmont">Helmont, Johannes (Joan) Baptista Van, Encyclopedia.Com</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20211218003254/https://www.encyclopedia.com/people/science-and-technology/chemistry-biographies/johannes-joan-baptista-van-helmont">Archived</a> 2021-12-18 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a>: "Others were chlorine gas from the reaction of nitric acid and sal ammoniac; ... "</li> <li>Wisniak, Jaime (2009) "Carl Wilhelm Scheele," Revista CENIC Ciencias Químicas, 40 (3): 165–73; see p. 168: "Early in the seventeenth century Johannes Baptiste van Helmont (1579–1644) mentioned that when sal marin (sodium chloride) or sal ammoniacus and aqua chrysulca (nitric acid) were mixed together, a flatus incoercible (non-condensable gas) was evolved."</li></ul> </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="References">References</h2></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239543626"><div class="reflist"> <div class="mw-references-wrap mw-references-columns"><ol class="references"> <li id="cite_note-CIAAW-1"><a href="#cite_ref-CIAAW_1-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://www.ciaaw.org/chlorine.htm">"Standard Atomic Weights: Chlorine"</a>. <a href="/wiki/Commission_on_Isotopic_Abundances_and_Atomic_Weights" title="Commission on Isotopic Abundances and Atomic Weights">CIAAW</a>. 2009.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Standard+Atomic+Weights%3A+Chlorine&rft.pub=CIAAW&rft.date=2009&rft_id=https%3A%2F%2Fwww.ciaaw.org%2Fchlorine.htm&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-CIAAW2021-2"><a href="#cite_ref-CIAAW2021_2-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFProhaskaIrrgeherBenefieldBöhlke2022" class="citation journal cs1">Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (2022-05-04). <a rel="nofollow" class="external text" href="https://www.degruyter.com/document/doi/10.1515/pac-2019-0603/html">"Standard atomic weights of the elements 2021 (IUPAC Technical Report)"</a>. Pure and Applied Chemistry. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1515%2Fpac-2019-0603">10.1515/pac-2019-0603</a>. <a href="/wiki/ISSN_(identifier)" class="mw-redirect" title="ISSN (identifier)">ISSN</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/issn/1365-3075">1365-3075</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Pure+and+Applied+Chemistry&rft.atitle=Standard+atomic+weights+of+the+elements+2021+%28IUPAC+Technical+Report%29&rft.date=2022-05-04&rft_id=info%3Adoi%2F10.1515%2Fpac-2019-0603&rft.issn=1365-3075&rft.aulast=Prohaska&rft.aufirst=Thomas&rft.au=Irrgeher%2C+Johanna&rft.au=Benefield%2C+Jacqueline&rft.au=B%C3%B6hlke%2C+John+K.&rft.au=Chesson%2C+Lesley+A.&rft.au=Coplen%2C+Tyler+B.&rft.au=Ding%2C+Tiping&rft.au=Dunn%2C+Philip+J.+H.&rft.au=Gr%C3%B6ning%2C+Manfred&rft.au=Holden%2C+Norman+E.&rft.au=Meijer%2C+Harro+A.+J.&rft_id=https%3A%2F%2Fwww.degruyter.com%2Fdocument%2Fdoi%2F10.1515%2Fpac-2019-0603%2Fhtml&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-3"><a href="#cite_ref-3">^</a> <a rel="nofollow" class="external text" href="http://encyclopedia.airliquide.com/Encyclopedia.asp?LanguageID=11&CountryID=19&Formula=&GasID=13&UNNumber=&EquivGasID=3&PressionBox=&VolLiquideBox=&MasseLiquideBox=&VolGasBox=&MasseGasBox=&RD20=29&RD9=8&RD6=64&RD4=2&RD3=22&RD8=27&RD2=20&RD18=41&RD7=18&RD13=71&RD16=35&RD12=31&RD19=34&RD24=62&RD25=77&RD26=78&RD28=81&RD29=82">Chlorine</a>, Gas Encyclopaedia, Air Liquide </li> <li id="cite_note-4"><a href="#cite_ref-4">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFAmbroseHallLeeLewis1979" class="citation journal cs1">Ambrose, D; Hall, D.J; Lee, D.A; Lewis, G.B; Mash, C.J (1979). "The vapour pressure of chlorine". The Journal of Chemical Thermodynamics. 11: 1089–1094. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1016%2F0021-9614%2879%2990139-3">10.1016/0021-9614(79)90139-3</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=The+Journal+of+Chemical+Thermodynamics&rft.atitle=The+vapour+pressure+of+chlorine&rft.volume=11&rft.pages=%3Cspan+class%3D%22nowrap%22%3E1089-%3C%2Fspan%3E1094&rft.date=1979&rft_id=info%3Adoi%2F10.1016%2F0021-9614%2879%2990139-3&rft.aulast=Ambrose&rft.aufirst=D&rft.au=Hall%2C+D.J&rft.au=Lee%2C+D.A&rft.au=Lewis%2C+G.B&rft.au=Mash%2C+C.J&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-GE28-5">^ <a href="#cite_ref-GE28_5-0">a</a> <a href="#cite_ref-GE28_5-1">b</a> <a href="#cite_ref-GE28_5-2">c</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGreenwoodEarnshaw1997" class="citation book cs1"><a href="/wiki/Norman_Greenwood" title="Norman Greenwood">Greenwood, Norman N.</a>; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). <a href="/wiki/Butterworth-Heinemann" title="Butterworth-Heinemann">Butterworth-Heinemann</a>. p. 28. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-08-037941-8" title="Special:BookSources/978-0-08-037941-8"><bdi>978-0-08-037941-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry+of+the+Elements&rft.pages=28&rft.edition=2nd&rft.pub=Butterworth-Heinemann&rft.date=1997&rft.isbn=978-0-08-037941-8&rft.aulast=Greenwood&rft.aufirst=Norman+N.&rft.au=Earnshaw%2C+Alan&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-Arblaster_2018-6"><a href="#cite_ref-Arblaster_2018_6-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFArblaster2018" class="citation book cs1">Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-1-62708-155-9" title="Special:BookSources/978-1-62708-155-9"><bdi>978-1-62708-155-9</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Selected+Values+of+the+Crystallographic+Properties+of+Elements&rft.place=Materials+Park%2C+Ohio&rft.pub=ASM+International&rft.date=2018&rft.isbn=978-1-62708-155-9&rft.aulast=Arblaster&rft.aufirst=John+W.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-7"><a href="#cite_ref-7">^</a> <a rel="nofollow" class="external text" href="http://www-d0.fnal.gov/hardware/cal/lvps_info/engineering/elementmagn.pdf">Magnetic susceptibility of the elements and inorganic compounds</a>, in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFLide2005" class="citation book cs1">Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton, Florida: CRC Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-8493-0486-5" title="Special:BookSources/0-8493-0486-5"><bdi>0-8493-0486-5</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=CRC+Handbook+of+Chemistry+and+Physics&rft.place=Boca+Raton%2C+Florida&rft.edition=86th&rft.pub=CRC+Press&rft.date=2005&rft.isbn=0-8493-0486-5&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-8"><a href="#cite_ref-8">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWeast1984" class="citation book cs1">Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-8493-0464-4" title="Special:BookSources/0-8493-0464-4"><bdi>0-8493-0464-4</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=CRC%2C+Handbook+of+Chemistry+and+Physics&rft.place=Boca+Raton%2C+Florida&rft.pages=E110&rft.pub=Chemical+Rubber+Company+Publishing&rft.date=1984&rft.isbn=0-8493-0464-4&rft.aulast=Weast&rft.aufirst=Robert&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-NUBASE2020-9"><a href="#cite_ref-NUBASE2020_9-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFKondevWangHuangNaimi2021" class="citation journal cs1">Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). <a rel="nofollow" class="external text" href="https://www-nds.iaea.org/amdc/ame2020/NUBASE2020.pdf">"The NUBASE2020 evaluation of nuclear properties"</a> (PDF). Chinese Physics C. 45 (3): 030001. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1088%2F1674-1137%2Fabddae">10.1088/1674-1137/abddae</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Chinese+Physics+C&rft.atitle=The+NUBASE2020+evaluation+of+nuclear+properties&rft.volume=45&rft.issue=3&rft.pages=030001&rft.date=2021&rft_id=info%3Adoi%2F10.1088%2F1674-1137%2Fabddae&rft.aulast=Kondev&rft.aufirst=F.+G.&rft.au=Wang%2C+M.&rft.au=Huang%2C+W.+J.&rft.au=Naimi%2C+S.&rft.au=Audi%2C+G.&rft_id=https%3A%2F%2Fwww-nds.iaea.org%2Famdc%2Fame2020%2FNUBASE2020.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-10"><a href="#cite_ref-10">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://web.archive.org/web/20110430145935/http://antiquity.ac.uk/ProjGall/weller/">"The earliest salt production in the world: an early Neolithic exploitation in Poiana Slatinei-Lunca, Romania"</a>. Archived from <a rel="nofollow" class="external text" href="https://antiquity.ac.uk/ProjGall/weller/">the original</a> on April 30, 2011. Retrieved 2008-07-10.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=The+earliest+salt+production+in+the+world%3A+an+early+Neolithic+exploitation+in+Poiana+Slatinei-Lunca%2C+Romania&rft_id=https%3A%2F%2Fantiquity.ac.uk%2FProjGall%2Fweller%2F&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-11"><a href="#cite_ref-11">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFKraus1942–1943" class="citation book cs1"><a href="/wiki/Paul_Kraus_(Arabist)" title="Paul Kraus (Arabist)">Kraus, Paul</a> (1942–1943). Jâbir ibn Hayyân: Contribution à l'histoire des idées scientifiques dans l'Islam. I. Le corpus des écrits jâbiriens. II. Jâbir et la science grecque. Cairo: <a href="/wiki/Institut_Fran%C3%A7ais_d%27Arch%C3%A9ologie_Orientale" title="Institut Français d'Archéologie Orientale">Institut Français d'Archéologie Orientale</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-3487091150" title="Special:BookSources/978-3487091150"><bdi>978-3487091150</bdi></a>. <a href="/wiki/OCLC_(identifier)" class="mw-redirect" title="OCLC (identifier)">OCLC</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/oclc/468740510">468740510</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=J%C3%A2bir+ibn+Hayy%C3%A2n%3A+Contribution+%C3%A0+l%27histoire+des+id%C3%A9es+scientifiques+dans+l%27Islam.+I.+Le+corpus+des+%C3%A9crits+j%C3%A2biriens.+II.+J%C3%A2bir+et+la+science+grecque&rft.place=Cairo&rft.pub=Institut+Fran%C3%A7ais+d%27Arch%C3%A9ologie+Orientale&rft.date=1942%2F1943&rft_id=info%3Aoclcnum%2F468740510&rft.isbn=978-3487091150&rft.aulast=Kraus&rft.aufirst=Paul&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> vol. II, pp. 41–42; <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFMulthauf1966" class="citation book cs1"><a href="/wiki/Robert_P._Multhauf" title="Robert P. Multhauf">Multhauf, Robert P.</a> (1966). The Origins of Chemistry. London: Oldbourne.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=The+Origins+of+Chemistry&rft.place=London&rft.pub=Oldbourne&rft.date=1966&rft.aulast=Multhauf&rft.aufirst=Robert+P.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> pp. 141–42. </li> <li id="cite_note-12"><a href="#cite_ref-12">^</a> <a href="#CITEREFMulthauf1966">Multhauf 1966</a>, p. 142, note 79. </li> <li id="cite_note-13"><a href="#cite_ref-13">^</a> <a href="#CITEREFMulthauf1966">Multhauf 1966</a>, pp. 160–163. </li> <li id="cite_note-14"><a href="#cite_ref-14">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFKarpenkoNorris2002" class="citation journal cs1">Karpenko, Vladimír; Norris, John A. (2002). <a rel="nofollow" class="external text" href="http://www.chemicke-listy.cz/ojs3/index.php/chemicke-listy/article/view/2266">"Vitriol in the History of Chemistry"</a>. Chemické listy. 96 (12): 997–1005. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20211218003227/http://www.chemicke-listy.cz/ojs3/index.php/chemicke-listy/article/view/2266">Archived</a> from the original on 2021-12-18. Retrieved 2021-02-09.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Chemick%C3%A9+listy&rft.atitle=Vitriol+in+the+History+of+Chemistry&rft.volume=96&rft.issue=12&rft.pages=%3Cspan+class%3D%22nowrap%22%3E997-%3C%2Fspan%3E1005&rft.date=2002&rft.aulast=Karpenko&rft.aufirst=Vladim%C3%ADr&rft.au=Norris%2C+John+A.&rft_id=http%3A%2F%2Fwww.chemicke-listy.cz%2Fojs3%2Findex.php%2Fchemicke-listy%2Farticle%2Fview%2F2266&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> p. 1002. </li> <li id="cite_note-Greenwood789-15">^ <a href="#cite_ref-Greenwood789_15-0">a</a> <a href="#cite_ref-Greenwood789_15-1">b</a> <a href="#cite_ref-Greenwood789_15-2">c</a> <a href="#cite_ref-Greenwood789_15-3">d</a> <a href="#CITEREFGreenwoodEarnshaw1997">Greenwood & Earnshaw 1997</a>, pp. 789–92 </li> <li id="cite_note-17"><a href="#cite_ref-17">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFScheele1774" class="citation journal cs1 cs1-prop-foreign-lang-source">Scheele, Carl Wilhelm (1774). <a rel="nofollow" class="external text" href="https://babel.hathitrust.org/cgi/pt?id=mdp.39015039452910;view=1up;seq=99">"Om Brunsten, eller Magnesia, och dess Egenskaper"</a> [On braunstein [i.e., pyrolusite, manganese dioxide], or magnesia, and its properties]. Kongliga Vetenskaps Academiens Handlingar [Proceedings of the Royal Scientific Academy] (in Swedish). 35: 89–116, 177–94. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20200423132126/https://babel.hathitrust.org/cgi/pt?id=mdp.39015039452910;view=1up;seq=99">Archived</a> from the original on 2020-04-23. Retrieved 2018-02-19.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Kongliga+Vetenskaps+Academiens+Handlingar+%5BProceedings+of+the+Royal+Scientific+Academy%5D&rft.atitle=Om+Brunsten%2C+eller+Magnesia%2C+och+dess+Egenskaper&rft.volume=35&rft.pages=%3Cspan+class%3D%22nowrap%22%3E89-%3C%2Fspan%3E116%2C+%3Cspan+class%3D%22nowrap%22%3E177-%3C%2Fspan%3E94&rft.date=1774&rft.aulast=Scheele&rft.aufirst=Carl+Wilhelm&rft_id=https%3A%2F%2Fbabel.hathitrust.org%2Fcgi%2Fpt%3Fid%3Dmdp.39015039452910%3Bview%3D1up%3Bseq%3D99&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> <a rel="nofollow" class="external text" href="https://babel.hathitrust.org/cgi/pt?id=mdp.39015039452910;view=1up;seq=103">In section 6 on pp. 93–94 of his paper</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20211218003341/https://babel.hathitrust.org/cgi/pt?id=mdp.39015039452910;view=1up;seq=103">Archived</a> 2021-12-18 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a>, Scheele described how chlorine was produced when a mixture of hydrochloric acid and manganese dioxide (Brunsten) was heated: "6) (a) På 1/2 uns fint rifven Brunsten slogs 1 uns ren Spiritus salis. ... samt lukten fo̊rsvunnen." ( 6) (a) On one half ounce of finely ground Braunstein [pyrolusite] was poured one ounce of pure spiritus salis [spirit of salt, hydrogen chloride]. After this mixture had been standing in the cold for one hour, the acid had assumed a dark brown colour. One part of this solution was poured into a glass, which was placed over the fire. The solution gave off an odour like warm aqua regia and after one quarter's hour duration, it was as clear and colourless as water, and the smell had disappeared.) For an English translation of the relevant passages of this article, see: The Early History of Chlorine : Papers by Carl Wilhelm Scheele (1774), C. L. Berthollet (1785), Guyton de Morveau (1787), J. L. Gay-Lussac and L. J. Thenard (1809) (Edinburgh, Scotland: Alembic Club, 1912), <a rel="nofollow" class="external text" href="https://babel.hathitrust.org/cgi/pt?id=coo.31924012394379;view=1up;seq=9">pp. 5–10.</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20211218003427/https://babel.hathitrust.org/cgi/pt?id=coo.31924012394379;view=1up;seq=9">Archived</a> 2021-12-18 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a> </li> <li id="cite_note-krogt-18">^ <a href="#cite_ref-krogt_18-0">a</a> <a href="#cite_ref-krogt_18-1">b</a> <a href="#cite_ref-krogt_18-2">c</a> <a href="#cite_ref-krogt_18-3">d</a> <a href="#cite_ref-krogt_18-4">e</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://web.archive.org/web/20100123003013/http://elements.vanderkrogt.net/element.php?sym=Cl">"17 Chlorine"</a>. Elements.vanderkrogt.net. Archived from <a rel="nofollow" class="external text" href="http://elements.vanderkrogt.net/element.php?sym=Cl">the original</a> on 2010-01-23. Retrieved 2008-09-12.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=17+Chlorine&rft.pub=Elements.vanderkrogt.net&rft_id=http%3A%2F%2Felements.vanderkrogt.net%2Felement.php%3Fsym%3DCl&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-Greenwood792-19">^ <a href="#cite_ref-Greenwood792_19-0">a</a> <a href="#cite_ref-Greenwood792_19-1">b</a> <a href="#cite_ref-Greenwood792_19-2">c</a> <a href="#cite_ref-Greenwood792_19-3">d</a> <a href="#CITEREFGreenwoodEarnshaw1997">Greenwood & Earnshaw 1997</a>, pp. 792–93 </li> <li id="cite_note-20"><a href="#cite_ref-20">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFIhde,_Aaron_John1984" class="citation book cs1">Ihde, Aaron John (1984). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=34KwmkU4LG0C&pg=PA158">The development of modern chemistry</a>. Courier Dover Publications. p. 158. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-486-64235-2" title="Special:BookSources/978-0-486-64235-2"><bdi>978-0-486-64235-2</bdi></a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20231230133555/https://books.google.com/books?id=34KwmkU4LG0C&pg=PA158">Archived</a> from the original on 2023-12-30. Retrieved 2020-05-06.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=The+development+of+modern+chemistry&rft.pages=158&rft.pub=Courier+Dover+Publications&rft.date=1984&rft.isbn=978-0-486-64235-2&rft.au=Ihde%2C+Aaron+John&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3D34KwmkU4LG0C%26pg%3DPA158&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-Weeks-21"><a href="#cite_ref-Weeks_21-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWeeks1932" class="citation journal cs1"><a href="/wiki/Mary_Elvira_Weeks" title="Mary Elvira Weeks">Weeks, Mary Elvira</a> (1932). "The discovery of the elements. XVII. The halogen family". Journal of Chemical Education. 9 (11): 1915. <a href="/wiki/Bibcode_(identifier)" class="mw-redirect" title="Bibcode (identifier)">Bibcode</a>:<a rel="nofollow" class="external text" href="https://ui.adsabs.harvard.edu/abs/1932JChEd...9.1915W">1932JChEd...9.1915W</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1021%2Fed009p1915">10.1021/ed009p1915</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Journal+of+Chemical+Education&rft.atitle=The+discovery+of+the+elements.+XVII.+The+halogen+family&rft.volume=9&rft.issue=11&rft.pages=1915&rft.date=1932&rft_id=info%3Adoi%2F10.1021%2Fed009p1915&rft_id=info%3Abibcode%2F1932JChEd...9.1915W&rft.aulast=Weeks&rft.aufirst=Mary+Elvira&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-22"><a href="#cite_ref-22">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGay-LussacThenard1809" class="citation journal cs1">Gay-Lussac; Thenard (1809). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=hnJKAAAAYAAJ&pg=PA295">"Extrait des mémoires lus à l'Institut national, depuis le 7 mars 1808 jusqu'au 27 février 1809"</a> [Extracts from memoirs read at the national Institute, from 7 March 1808 to 27 February 1809]. Mémoires de Physique et de Chimie de la Société d'Arcueil. 2: 295–358. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20231230133512/https://books.google.com/books?id=hnJKAAAAYAAJ&pg=PA295#v=onepage&q&f=false">Archived</a> from the original on 30 December 2023. Retrieved 24 February 2018.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=M%C3%A9moires+de+Physique+et+de+Chimie+de+la+Soci%C3%A9t%C3%A9+d%27Arcueil&rft.atitle=Extrait+des+m%C3%A9moires+lus+%C3%A0+l%27Institut+national%2C+depuis+le+7+mars+1808+jusqu%27au+27+f%C3%A9vrier+1809.&rft.volume=2&rft.pages=%3Cspan+class%3D%22nowrap%22%3E295-%3C%2Fspan%3E358&rft.date=1809&rft.au=Gay-Lussac&rft.au=Thenard&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DhnJKAAAAYAAJ%26pg%3DPA295&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> See: § De la nature et des propriétés de l'acide muriatique et de l'acide muriatique oxigéné (On the nature and properties of muriatic acid and of oxidized muriatic acid), pp. 339–58. From pp. 357–58: "Le gaz muriatique oxigéné n'est pas, en effect, décomposé ... comme un corps composé." ("In fact, oxygenated muriatic acid is not decomposed by charcoal, and it might be supposed, from this fact and those that are communicated in this Memoir, that this gas is a simple body. The phenomena that it presents can be explained well enough on this hypothesis; we shall not seek to defend it, however, as it appears to us that they are still better explained by regarding oxygenated muriatic acid as a compound body.") For a full English translation of this section, see: <a rel="nofollow" class="external text" href="http://web.lemoyne.edu/~giunta/thenard.html">Joseph Louis Gay-Lussac and Louis Jacques Thénard, "On the nature and the properties of muriatic acid and of oxygenated muriatic acid" (Lemoyne College, Syracuse, New York)</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20080725061430/http://web.lemoyne.edu/~giunta/thenard.html">Archived</a> 2008-07-25 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a> </li> <li id="cite_note-23"><a href="#cite_ref-23">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFDavy1811" class="citation journal cs1">Davy, Humphry (1811). <a rel="nofollow" class="external text" href="https://babel.hathitrust.org/cgi/pt?id=mdp.39015034564297;view=1up;seq=15">"The Bakerian Lecture. On some of the combinations of oxymuriatic gas and oxygene, and on the chemical relations of these principles, to inflammable bodies"</a>. Philosophical Transactions of the Royal Society of London. 101: 1–35. <a href="/wiki/Bibcode_(identifier)" class="mw-redirect" title="Bibcode (identifier)">Bibcode</a>:<a rel="nofollow" class="external text" href="https://ui.adsabs.harvard.edu/abs/1811RSPT..101....1D">1811RSPT..101....1D</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1098%2Frstl.1811.0001">10.1098/rstl.1811.0001</a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20200423032814/https://babel.hathitrust.org/cgi/pt?id=mdp.39015034564297;view=1up;seq=15">Archived</a> from the original on 2020-04-23. Retrieved 2018-02-19.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Philosophical+Transactions+of+the+Royal+Society+of+London&rft.atitle=The+Bakerian+Lecture.+On+some+of+the+combinations+of+oxymuriatic+gas+and+oxygene%2C+and+on+the+chemical+relations+of+these+principles%2C+to+inflammable+bodies&rft.volume=101&rft.pages=%3Cspan+class%3D%22nowrap%22%3E1-%3C%2Fspan%3E35&rft.date=1811&rft_id=info%3Adoi%2F10.1098%2Frstl.1811.0001&rft_id=info%3Abibcode%2F1811RSPT..101....1D&rft.aulast=Davy&rft.aufirst=Humphry&rft_id=https%3A%2F%2Fbabel.hathitrust.org%2Fcgi%2Fpt%3Fid%3Dmdp.39015034564297%3Bview%3D1up%3Bseq%3D15&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> Davy named chlorine on <a rel="nofollow" class="external text" href="https://babel.hathitrust.org/cgi/pt?id=mdp.39015034564297;view=1up;seq=46">p. 32:</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20211218003415/https://babel.hathitrust.org/cgi/pt?id=mdp.39015034564297;view=1up;seq=46">Archived</a> 2021-12-18 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a> "After consulting some of the most eminent chemical philosophers in this country, it has been judged most proper to suggest a name founded upon one of its obvious and characteristic properties – its colour, and to call it Chlorine, or Chloric gas.* *From χλωρος." </li> <li id="cite_note-24"><a href="#cite_ref-24">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSchweigger1811" class="citation journal cs1 cs1-prop-foreign-lang-source">Schweigger, J.S.C. (1811). <a rel="nofollow" class="external text" href="https://babel.hathitrust.org/cgi/pt?id=njp.32101076802287;view=1up;seq=295">"Nachschreiben des Herausgebers, die neue Nomenclatur betreffend"</a> [Postscript of the editor concerning the new nomenclature]. Journal für Chemie und Physik (in German). 3 (2): 249–55. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20200423132157/https://babel.hathitrust.org/cgi/pt?id=njp.32101076802287;view=1up;seq=295">Archived</a> from the original on 2020-04-23. Retrieved 2018-02-19.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Journal+f%C3%BCr+Chemie+und+Physik&rft.atitle=Nachschreiben+des+Herausgebers%2C+die+neue+Nomenclatur+betreffend&rft.volume=3&rft.issue=2&rft.pages=%3Cspan+class%3D%22nowrap%22%3E249-%3C%2Fspan%3E55&rft.date=1811&rft.aulast=Schweigger&rft.aufirst=J.S.C.&rft_id=https%3A%2F%2Fbabel.hathitrust.org%2Fcgi%2Fpt%3Fid%3Dnjp.32101076802287%3Bview%3D1up%3Bseq%3D295&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> On p. 251, Schweigger proposed the word "halogen": "Man sage dafür lieber mit richter Wortbildung Halogen (da schon in der Mineralogie durch Werner's Halit-Geschlecht dieses Wort nicht fremd ist) von αλς Salz und dem alten γενειν (dorisch γενεν) zeugen." (One should say instead, with proper morphology, "halogen" (this word is not strange since [it's] already in mineralogy via Werner's "halite" species) from αλς [als] "salt" and the old γενειν [genein] (Doric γενεν) "to beget".) </li> <li id="cite_note-25"><a href="#cite_ref-25">^</a> In 1826, Berzelius coined the terms Saltbildare (salt-formers) and Corpora Halogenia (salt-making substances) for the elements chlorine, iodine, and fluorine. See: <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFBerzelius1826" class="citation journal cs1 cs1-prop-foreign-lang-source">Berzelius, Jacob (1826). <a rel="nofollow" class="external text" href="https://babel.hathitrust.org/cgi/pt?id=hvd.32044092556919;view=1up;seq=195">"Årsberättelser om Framstegen i Physik och Chemie"</a> [Annual Report on Progress in Physics and Chemistry]. Arsb. Vetensk. Framsteg (in Swedish). 6. Stockholm, Sweden: P.A. Norstedt & Söner: 187. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20200423132254/https://babel.hathitrust.org/cgi/pt?id=hvd.32044092556919;view=1up;seq=195">Archived</a> from the original on 2020-04-23. Retrieved 2018-02-19.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Arsb.+Vetensk.+Framsteg&rft.atitle=%C3%85rsber%C3%A4ttelser+om+Framstegen+i+Physik+och+Chemie&rft.volume=6&rft.pages=187&rft.date=1826&rft.aulast=Berzelius&rft.aufirst=Jacob&rft_id=https%3A%2F%2Fbabel.hathitrust.org%2Fcgi%2Fpt%3Fid%3Dhvd.32044092556919%3Bview%3D1up%3Bseq%3D195&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> From p. 187: "De förre af dessa, d. ä. de electronegativa, dela sig i tre klasser: 1) den första innehåller kroppar, som förenade med de electropositiva, omedelbart frambringa salter, hvilka jag derför kallar Saltbildare (Corpora Halogenia). Desse utgöras af chlor, iod och fluor *)." (The first of them [i.e., elements], i.e., the electronegative [ones], are divided into three classes: 1) The first includes substances which, [when] united with electropositive [elements], immediately produce salts, and which I therefore name "salt-formers" (salt-producing substances). These are chlorine, iodine, and fluorine *).) </li> <li id="cite_note-26"><a href="#cite_ref-26">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSnelders,_H._A._M.1971" class="citation journal cs1">Snelders, H. A. M. (1971). "J. S. C. Schweigger: His Romanticism and His Crystal Electrical Theory of Matter". Isis. 62 (3): 328–38. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1086%2F350763">10.1086/350763</a>. <a href="/wiki/JSTOR_(identifier)" class="mw-redirect" title="JSTOR (identifier)">JSTOR</a> <a rel="nofollow" class="external text" href="https://www.jstor.org/stable/229946">229946</a>. <a href="/wiki/S2CID_(identifier)" class="mw-redirect" title="S2CID (identifier)">S2CID</a> <a rel="nofollow" class="external text" href="https://api.semanticscholar.org/CorpusID:170337569">170337569</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Isis&rft.atitle=J.+S.+C.+Schweigger%3A+His+Romanticism+and+His+Crystal+Electrical+Theory+of+Matter&rft.volume=62&rft.issue=3&rft.pages=%3Cspan+class%3D%22nowrap%22%3E328-%3C%2Fspan%3E38&rft.date=1971&rft_id=https%3A%2F%2Fapi.semanticscholar.org%2FCorpusID%3A170337569%23id-name%3DS2CID&rft_id=https%3A%2F%2Fwww.jstor.org%2Fstable%2F229946%23id-name%3DJSTOR&rft_id=info%3Adoi%2F10.1086%2F350763&rft.au=Snelders%2C+H.+A.+M.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-27"><a href="#cite_ref-27">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFFaraday1823" class="citation journal cs1">Faraday, M. (1823). <a rel="nofollow" class="external text" href="https://babel.hathitrust.org/cgi/pt?id=mdp.39015034564487;view=1up;seq=244">"On fluid chlorine"</a>. Philosophical Transactions of the Royal Society of London. 113: 160–64. <a href="/wiki/Bibcode_(identifier)" class="mw-redirect" title="Bibcode (identifier)">Bibcode</a>:<a rel="nofollow" class="external text" href="https://ui.adsabs.harvard.edu/abs/1823RSPT..113..160F">1823RSPT..113..160F</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1098%2Frstl.1823.0016">10.1098/rstl.1823.0016</a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20200423053126/https://babel.hathitrust.org/cgi/pt?id=mdp.39015034564487;view=1up;seq=244">Archived</a> from the original on 2020-04-23. Retrieved 2018-02-19.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Philosophical+Transactions+of+the+Royal+Society+of+London&rft.atitle=On+fluid+chlorine&rft.volume=113&rft.pages=%3Cspan+class%3D%22nowrap%22%3E160-%3C%2Fspan%3E64&rft.date=1823&rft_id=info%3Adoi%2F10.1098%2Frstl.1823.0016&rft_id=info%3Abibcode%2F1823RSPT..113..160F&rft.aulast=Faraday&rft.aufirst=M.&rft_id=https%3A%2F%2Fbabel.hathitrust.org%2Fcgi%2Fpt%3Fid%3Dmdp.39015034564487%3Bview%3D1up%3Bseq%3D244&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-28"><a href="#cite_ref-28">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFChodos,_Alan" class="citation web cs1">Chodos, Alan (ed.). <a rel="nofollow" class="external text" href="https://web.archive.org/web/20100615142343/http://aps.org/publications/apsnews/200108/history.cfm">"This Month in Physics History September 4, 1821 and August 29, 1831: Faraday and Electromagnetism"</a>. American Physical Society. Archived from <a rel="nofollow" class="external text" href="http://www.aps.org/publications/apsnews/200108/history.cfm">the original</a> on June 15, 2010. Retrieved 2010-05-08.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=This+Month+in+Physics+History+September+4%2C+1821+and+August+29%2C+1831%3A+Faraday+and+Electromagnetism&rft.pub=American+Physical+Society&rft_id=http%3A%2F%2Fwww.aps.org%2Fpublications%2Fapsnews%2F200108%2Fhistory.cfm&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-29"><a href="#cite_ref-29">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFO'Connor_J._J.Robertson_E._F." class="citation web cs1">O'Connor J. J.; Robertson E. F. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20100220051522/http://www-history.mcs.st-andrews.ac.uk/Biographies/Faraday.html">"Michael Faraday"</a>. School of Mathematics and Statistics, University of St Andrews, Scotland. Archived from <a rel="nofollow" class="external text" href="http://www-history.mcs.st-andrews.ac.uk/Biographies/Faraday.html">the original</a> on 2010-02-20. Retrieved 2010-05-08.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=School+of+Mathematics+and+Statistics%2C+University+of+St+Andrews%2C+Scotland&rft.atitle=Michael+Faraday&rft.au=O%27Connor+J.+J.&rft.au=Robertson+E.+F.&rft_id=http%3A%2F%2Fwww-history.mcs.st-andrews.ac.uk%2FBiographies%2FFaraday.html&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-encyc-30">^ <a href="#cite_ref-encyc_30-0">a</a> <a href="#cite_ref-encyc_30-1">b</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation encyclopaedia cs1"><a rel="nofollow" class="external text" href="https://web.archive.org/web/20120524111017/http://www.1902encyclopedia.com/B/BLE/bleaching.html">"Bleaching"</a>. Encyclopædia Britannica (9th Edition (1875) and 10th Edition (1902) ed.). Archived from <a rel="nofollow" class="external text" href="http://www.1902encyclopedia.com/B/BLE/bleaching.html">the original</a> on 2012-05-24. Retrieved 2012-05-02.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Bleaching&rft.btitle=Encyclop%C3%A6dia+Britannica&rft.edition=9th+Edition+%281875%29+and+10th+Edition+%281902%29&rft_id=http%3A%2F%2Fwww.1902encyclopedia.com%2FB%2FBLE%2Fbleaching.html&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-Cotton-31"><a href="#cite_ref-Cotton_31-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFAspin1981" class="citation book cs1">Aspin, Chris (1981). <a rel="nofollow" class="external text" href="https://archive.org/details/cottonindustry0000aspi/page/24">The Cotton Industry</a>. Shire Publications Ltd. p. <a rel="nofollow" class="external text" href="https://archive.org/details/cottonindustry0000aspi/page/24">24</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-85263-545-2" title="Special:BookSources/978-0-85263-545-2"><bdi>978-0-85263-545-2</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=The+Cotton+Industry&rft.pages=24&rft.pub=Shire+Publications+Ltd&rft.date=1981&rft.isbn=978-0-85263-545-2&rft.aulast=Aspin&rft.aufirst=Chris&rft_id=https%3A%2F%2Farchive.org%2Fdetails%2Fcottonindustry0000aspi%2Fpage%2F24&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-32"><a href="#cite_ref-32">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFPaul_May" class="citation web cs1">Paul May. <a rel="nofollow" class="external text" href="http://www.chm.bris.ac.uk/motm/bleach/bleachh.htm">"Bleach (Sodium Hypochlorite)"</a>. University of Bristol. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20161213230407/http://www.chm.bris.ac.uk/motm/bleach/bleachh.htm">Archived</a> from the original on 13 December 2016. Retrieved 13 December 2016.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Bleach+%28Sodium+Hypochlorite%29&rft.pub=University+of+Bristol&rft.au=Paul+May&rft_id=http%3A%2F%2Fwww.chm.bris.ac.uk%2Fmotm%2Fbleach%2Fbleachh.htm&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-Greenwood798-33">^ <a href="#cite_ref-Greenwood798_33-0">a</a> <a href="#cite_ref-Greenwood798_33-1">b</a> <a href="#cite_ref-Greenwood798_33-2">c</a> <a href="#CITEREFGreenwoodEarnshaw1997">Greenwood & Earnshaw 1997</a>, p. 798 </li> <li id="cite_note-34"><a href="#cite_ref-34">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFAlmqvist2003" class="citation book cs1">Almqvist, Ebbe (2003). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=OI0fTJhydh4C&q=Chlorine-Alkali+Griesheim+1884&pg=PA220">History of Industrial Gases</a>. Springer Science & Business Media. p. 220. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-306-47277-0" title="Special:BookSources/978-0-306-47277-0"><bdi>978-0-306-47277-0</bdi></a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20231230133537/https://books.google.com/books?id=OI0fTJhydh4C&q=Chlorine-Alkali+Griesheim+1884&pg=PA220#v=snippet&q=Chlorine-Alkali%20Griesheim%201884&f=false">Archived</a> from the original on 2023-12-30. Retrieved 2020-10-09.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=History+of+Industrial+Gases&rft.pages=220&rft.pub=Springer+Science+%26+Business+Media&rft.date=2003&rft.isbn=978-0-306-47277-0&rft.aulast=Almqvist&rft.aufirst=Ebbe&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DOI0fTJhydh4C%26q%3DChlorine-Alkali%2BGriesheim%2B1884%26pg%3DPA220&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-bouvet-35">^ <a href="#cite_ref-bouvet_35-0">a</a> <a href="#cite_ref-bouvet_35-1">b</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFBouvet,_Maurice1950" class="citation journal cs1 cs1-prop-foreign-lang-source">Bouvet, Maurice (1950). "Les grands pharmaciens: Labarraque (1777–1850)" [The great pharmacists: Labarraque (1777–1850)]. Revue d'Histoire de la Pharmacie (in French). 38 (128): 97–107. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.3406%2Fpharm.1950.8662">10.3406/pharm.1950.8662</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Revue+d%27Histoire+de+la+Pharmacie&rft.atitle=Les+grands+pharmaciens%3A+Labarraque+%281777%E2%80%931850%29&rft.volume=38&rft.issue=128&rft.pages=%3Cspan+class%3D%22nowrap%22%3E97-%3C%2Fspan%3E107&rft.date=1950&rft_id=info%3Adoi%2F10.3406%2Fpharm.1950.8662&rft.au=Bouvet%2C+Maurice&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-36"><a href="#cite_ref-36">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://web.archive.org/web/20070221140939/http://www.drcordas.com/education/weaponsmassd/Chlorine.pdf">"Chlorine – History"</a> (PDF). 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Retrieved 2016-04-12.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=www.doh.wa.gov&rft.atitle=Bleach+Mixing+Dangers+%3A+Washington+State+Dept.+of+Health&rft_id=http%3A%2F%2Fwww.doh.wa.gov%2FYouandYourFamily%2FHealthyHome%2FContaminants%2FBleachMixingDangers&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-136"><a href="#cite_ref-136">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFBertolini,_LucaElsener,_BernhardPedeferri,_PietroPolder,_Rob_B.2004" class="citation book cs1">Bertolini, Luca; Elsener, Bernhard; Pedeferri, Pietro; Polder, Rob B. (2004). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=cEmq232h1zcC&pg=PA148">Corrosion of steel in concrete: prevention, diagnosis, repair</a>. Wiley-VCH. p. 148. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-3-527-30800-2" title="Special:BookSources/978-3-527-30800-2"><bdi>978-3-527-30800-2</bdi></a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20231230134102/https://books.google.com/books?id=cEmq232h1zcC&pg=PA148#v=onepage&q&f=false">Archived</a> from the original on 2023-12-30. Retrieved 2020-05-06.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Corrosion+of+steel+in+concrete%3A+prevention%2C+diagnosis%2C+repair&rft.pages=148&rft.pub=Wiley-VCH&rft.date=2004&rft.isbn=978-3-527-30800-2&rft.au=Bertolini%2C+Luca&rft.au=Elsener%2C+Bernhard&rft.au=Pedeferri%2C+Pietro&rft.au=Polder%2C+Rob+B.&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DcEmq232h1zcC%26pg%3DPA148&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-137"><a href="#cite_ref-137">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFLewis,_P.R.2000" class="citation book cs1">Lewis, P.R. (1 January 2000). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=SFm8rKotSaUC&pg=PA19">Polymer Product Failure</a>. iSmithers Rapra Publishing. pp. 19–. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-1-85957-192-7" title="Special:BookSources/978-1-85957-192-7"><bdi>978-1-85957-192-7</bdi></a>. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20130510041524/http://books.google.com/books?id=SFm8rKotSaUC&pg=PA19">Archived</a> from the original on 10 May 2013. Retrieved 2011-04-30.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Polymer+Product+Failure&rft.pages=19-&rft.pub=iSmithers+Rapra+Publishing&rft.date=2000-01-01&rft.isbn=978-1-85957-192-7&rft.au=Lewis%2C+P.R.&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DSFm8rKotSaUC%26pg%3DPA19&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-bayerdatasheet2008-138">^ <a href="#cite_ref-bayerdatasheet2008_138-0">a</a> <a href="#cite_ref-bayerdatasheet2008_138-1">b</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://web.archive.org/web/20120915114003/https://tecci.bayer.de/io-tra-pro/emea/de/docId-2857612/Chlorine.pdf">"Chlorine: Product Datasheet"</a> (PDF). Bayer MaterialScience AG. 2008-04-21. Archived from <a rel="nofollow" class="external text" href="https://tecci.bayer.de/io-tra-pro/emea/de/docId-2857612/Chlorine.pdf">the original</a> (PDF) on September 15, 2012. Retrieved 2013-12-17.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Chlorine%3A+Product+Datasheet&rft.pub=Bayer+MaterialScience+AG&rft.date=2008-04-21&rft_id=https%3A%2F%2Ftecci.bayer.de%2Fio-tra-pro%2Femea%2Fde%2FdocId-2857612%2FChlorine.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> <li id="cite_note-sanders2004-139">^ <a href="#cite_ref-sanders2004_139-0">a</a> <a href="#cite_ref-sanders2004_139-1">b</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSanders2004" class="citation book cs1">Sanders, Roy E. (2004). Chemical Process Safety: Learning from Case Histories, 3rd Revised edition. Oxford: Elsevier Science & Technology. p. 92. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-7506-7749-3" title="Special:BookSources/978-0-7506-7749-3"><bdi>978-0-7506-7749-3</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemical+Process+Safety%3A+Learning+from+Case+Histories%2C+3rd+Revised+edition&rft.place=Oxford&rft.pages=92&rft.pub=Elsevier+Science+%26+Technology&rft.date=2004&rft.isbn=978-0-7506-7749-3&rft.aulast=Sanders&rft.aufirst=Roy+E.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"> </li> </ol></div></div> <div class="mw-heading mw-heading3"><h3 id="Bibliography">Bibliography</h3></div> <style data-mw-deduplicate="TemplateStyles:r1239549316">.mw-parser-output .refbegin{margin-bottom:0.5em}.mw-parser-output .refbegin-hanging-indents>ul{margin-left:0}.mw-parser-output .refbegin-hanging-indents>ul>li{margin-left:0;padding-left:3.2em;text-indent:-3.2em}.mw-parser-output .refbegin-hanging-indents ul,.mw-parser-output .refbegin-hanging-indents ul li{list-style:none}@media(max-width:720px){.mw-parser-output .refbegin-hanging-indents>ul>li{padding-left:1.6em;text-indent:-1.6em}}.mw-parser-output .refbegin-columns{margin-top:0.3em}.mw-parser-output .refbegin-columns ul{margin-top:0}.mw-parser-output .refbegin-columns li{page-break-inside:avoid;break-inside:avoid-column}@media screen{.mw-parser-output .refbegin{font-size:90%}}</style><div class="refbegin" style=""> <ul><li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGreenwoodEarnshaw1997" class="citation book cs1"><a href="/wiki/Norman_Greenwood" title="Norman Greenwood">Greenwood, Norman N.</a>; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). <a href="/wiki/Butterworth-Heinemann" title="Butterworth-Heinemann">Butterworth-Heinemann</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-08-037941-8" title="Special:BookSources/978-0-08-037941-8"><bdi>978-0-08-037941-8</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry+of+the+Elements&rft.edition=2nd&rft.pub=Butterworth-Heinemann&rft.date=1997&rft.isbn=978-0-08-037941-8&rft.aulast=Greenwood&rft.aufirst=Norman+N.&rft.au=Earnshaw%2C+Alan&rfr_id=info%3Asid%2Fen.wikipedia.org%3AChlorine" class="Z3988"></li></ul> </div> <div class="mw-heading mw-heading2"><h2 id="External_links">External links</h2></div> <ul><li><a rel="nofollow" class="external text" href="https://www.periodicvideos.com/videos/017.htm">Chlorine</a> at <a href="/wiki/The_Periodic_Table_of_Videos" class="mw-redirect" title="The Periodic Table of Videos">The Periodic Table of Videos</a> (University of Nottingham)</li> <li><a href="/wiki/Agency_for_Toxic_Substances_and_Disease_Registry" title="Agency for Toxic Substances and Disease Registry">Agency for Toxic Substances and Disease Registry</a>: <a rel="nofollow" class="external text" href="https://web.archive.org/web/20100607045216/http://www.atsdr.cdc.gov/substances/toxsubstance.asp?toxid=36">Chlorine</a></li> <li><a rel="nofollow" class="external text" href="https://web.archive.org/web/20090518141937/http://electrochem.cwru.edu/encycl/art-b01-brine.htm">Electrolytic production</a></li> <li><a rel="nofollow" class="external text" href="https://web.archive.org/web/20100429205421/http://www.amazingrust.com/Experiments/how_to/Liquid_Cl2.html">Production and liquefaction of chlorine</a></li> <li><a rel="nofollow" class="external text" href="https://web.archive.org/web/20080706020039/http://oceana.org/chlorine">Chlorine Production Using Mercury, Environmental Considerations and Alternatives</a></li> <li><a rel="nofollow" class="external text" href="https://web.archive.org/web/20091029202733/http://www.npi.gov.au/database/substance-info/profiles/20.html">National Pollutant Inventory – Chlorine</a></li> <li><a rel="nofollow" class="external text" href="https://www.cdc.gov/niosh/topics/chlorine/">National Institute for Occupational Safety and Health – Chlorine Page</a></li> <li><a rel="nofollow" class="external text" href="http://www.chlorineinstitute.org/">Chlorine Institute</a> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20120827050648/http://www.chlorineinstitute.org/">Archived</a> 2012-08-27 at the <a href="/wiki/Wayback_Machine" title="Wayback Machine">Wayback Machine</a> – Trade association representing the chlorine industry</li> <li><a rel="nofollow" class="external text" href="https://www.eurochlor.org/">Chlorine Online</a> – the web portal of Eurochlor – the business association of the European chlor-alkali industry</li></ul> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><style data-mw-deduplicate="TemplateStyles:r1236075235">.mw-parser-output .navbox{box-sizing:border-box;border:1px solid #a2a9b1;width:100%;clear:both;font-size:88%;text-align:center;padding:1px;margin:1em auto 0}.mw-parser-output .navbox .navbox{margin-top:0}.mw-parser-output .navbox+.navbox,.mw-parser-output .navbox+.navbox-styles+.navbox{margin-top:-1px}.mw-parser-output .navbox-inner,.mw-parser-output .navbox-subgroup{width:100%}.mw-parser-output .navbox-group,.mw-parser-output .navbox-title,.mw-parser-output .navbox-abovebelow{padding:0.25em 1em;line-height:1.5em;text-align:center}.mw-parser-output .navbox-group{white-space:nowrap;text-align:right}.mw-parser-output .navbox,.mw-parser-output .navbox-subgroup{background-color:#fdfdfd}.mw-parser-output .navbox-list{line-height:1.5em;border-color:#fdfdfd}.mw-parser-output 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.navbar{display:block;font-size:100%}.mw-parser-output .navbox-title .navbar{float:left;text-align:left;margin-right:0.5em}body.skin--responsive .mw-parser-output .navbox-image img{max-width:none!important}@media print{body.ns-0 .mw-parser-output .navbox{display:none!important}}</style><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"></div><div role="navigation" class="navbox" aria-labelledby="Chlorine_compounds138" style="padding:3px"><table class="nowraplinks mw-collapsible mw-collapsed navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Chlorine_compounds" title="Template:Chlorine compounds"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Chlorine_compounds" title="Template talk:Chlorine compounds"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Chlorine_compounds" title="Special:EditPage/Template:Chlorine compounds"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Chlorine_compounds138" style="font-size:114%;margin:0 4em"><a href="/wiki/Chlorine_compounds" class="mw-redirect" title="Chlorine compounds">Chlorine compounds</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Chloride" title="Chloride">Chlorides</a> and <a href="/wiki/Acid" title="Acid">acids</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Hydrogen_chloride" title="Hydrogen chloride">HCl</a></li> <li><a href="/wiki/Hypochlorous_acid" title="Hypochlorous acid">HClO</a></li> <li><a href="/wiki/Chlorous_acid" title="Chlorous acid">HClO2</a></li> <li><a href="/wiki/Chloric_acid" title="Chloric acid">HClO3</a></li> <li><a href="/wiki/Perchloric_acid" title="Perchloric acid">HClO4</a></li> <li><a href="/wiki/Chlorosulfuric_acid" title="Chlorosulfuric acid">HSO3Cl</a></li> <li><a href="/wiki/Barium_chloride_fluoride" title="Barium chloride fluoride">BaClF</a></li> <li><a href="/wiki/Boron_trichloride" title="Boron trichloride">BCl3</a></li> <li><a href="/wiki/Carbon_tetrachloride" title="Carbon tetrachloride">CCl4</a></li> <li><a href="/wiki/Silicon_tetrachloride" title="Silicon tetrachloride">SiCl4</a></li> <li><a href="/wiki/Titanium_tetrachloride" title="Titanium tetrachloride">TiCl4</a></li> <li><a href="/wiki/Chlorocyclopropane" title="Chlorocyclopropane">C3H5Cl</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Chlorine_fluoride" title="Chlorine fluoride">Chlorine fluorides</a></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Chlorine_monofluoride" title="Chlorine monofluoride">ClF</a></li> <li><a href="/wiki/Chlorine_trifluoride" title="Chlorine trifluoride">ClF3</a></li> <li><a href="/wiki/Chlorine_pentafluoride" title="Chlorine pentafluoride">ClF5</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Chlorine_oxide" title="Chlorine oxide">Chlorine oxides</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Chlorine_monoxide" title="Chlorine monoxide">ClO</a></li> <li><a href="/wiki/Chlorine_dioxide" title="Chlorine dioxide">ClO2</a></li> <li><a href="/wiki/Dichlorine_monoxide" title="Dichlorine monoxide">Cl2O</a></li> <li><a href="/wiki/Chlorine_peroxide" title="Chlorine peroxide">Cl2O2</a></li> <li><a href="/wiki/Dichlorine_trioxide" title="Dichlorine trioxide">Cl2O3</a></li> <li><a href="/wiki/Chlorine_perchlorate" title="Chlorine perchlorate">Cl2O4</a></li> <li><a href="/wiki/Dichlorine_pentoxide" title="Dichlorine pentoxide">Cl2O5</a></li> <li><a href="/wiki/Dichlorine_hexoxide" title="Dichlorine hexoxide">Cl2O6</a></li> <li><a href="/wiki/Dichlorine_heptoxide" title="Dichlorine heptoxide">Cl2O7</a></li> <li><a href="/wiki/Chlorine_tetroxide" title="Chlorine tetroxide">ClO4</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Chlorine <a href="/wiki/Oxyfluoride" class="mw-redirect" title="Oxyfluoride">oxyfluorides</a></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Chlorosyl_fluoride" title="Chlorosyl fluoride">ClOF</a></li> <li><a href="/wiki/Chlorine_trifluoride_oxide" title="Chlorine trifluoride oxide">ClOF3</a></li> <li><a href="/wiki/Chloryl_fluoride" title="Chloryl fluoride">ClO2F</a></li> <li>ClOF5 (predicted)</li> <li><a href="/wiki/Chlorine_trifluoride_dioxide" title="Chlorine trifluoride dioxide">ClO2F3</a></li> <li><a href="/wiki/Perchloryl_fluoride" title="Perchloryl fluoride">ClO3F</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Chlorine(I) derivatives</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Chlorine_nitrate" title="Chlorine nitrate">ClNO3</a></li> <li><a href="/w/index.php?title=Chlorine_fluorosulfate&action=edit&redlink=1" class="new" title="Chlorine fluorosulfate (page does not exist)">ClSO3F</a></li> <li><a href="/wiki/Chlorine_azide" title="Chlorine azide">ClN3</a></li> <li><a href="/wiki/Chlorine_nitride" class="mw-redirect" title="Chlorine nitride">Cl3N</a></li></ul> </div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"></div><div role="navigation" class="navbox" aria-labelledby="Periodic_table18" style="padding:3px"><table class="nowraplinks mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Periodic_table_(navbox)" title="Template:Periodic table (navbox)"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Periodic_table_(navbox)" title="Template talk:Periodic table (navbox)"><abbr title="Discuss 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element">3</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_4_element" title="Group 4 element">4</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_5_element" title="Group 5 element">5</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_6_element" title="Group 6 element">6</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_7_element" title="Group 7 element">7</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_8_element" title="Group 8 element">8</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_9_element" title="Group 9 element">9</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_10_element" title="Group 10 element">10</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_11_element" title="Group 11 element">11</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_12_element" title="Group 12 element">12</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Boron_group" title="Boron group">13</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Carbon_group" title="Carbon group">14</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Pnictogen" title="Pnictogen">15</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Chalcogen" title="Chalcogen">16</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Halogen" title="Halogen">17</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Noble_gas" title="Noble gas">18</a> </th></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_1_element" title="Period 1 element">1</a> </th> <td title="H, Hydrogen" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Hydrogen" title="Hydrogen">H</a> </td> <td colspan="30"> </td> <td title="He, Helium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Helium" title="Helium">He</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_2_element" title="Period 2 element">2</a> </th> <td title="Li, Lithium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Lithium" title="Lithium">Li</a> </td> <td title="Be, Beryllium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Beryllium" title="Beryllium">Be</a> </td> <td colspan="24"> </td> <td title="B, Boron" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Boron" title="Boron">B</a> </td> <td title="C, Carbon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Carbon" title="Carbon">C</a> </td> <td title="N, Nitrogen" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Nitrogen" title="Nitrogen">N</a> </td> <td title="O, Oxygen" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Oxygen" title="Oxygen">O</a> </td> <td title="F, Fluorine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Fluorine" title="Fluorine">F</a> </td> <td title="Ne, Neon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Neon" title="Neon">Ne</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_3_element" title="Period 3 element">3</a> </th> <td title="Na, Sodium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Sodium" title="Sodium">Na</a> </td> <td title="Mg, Magnesium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Magnesium" title="Magnesium">Mg</a> </td> <td colspan="24"> </td> <td title="Al, Aluminium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Aluminium" title="Aluminium">Al</a> </td> <td title="Si, Silicon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Silicon" title="Silicon">Si</a> </td> <td title="P, Phosphorus" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Phosphorus" title="Phosphorus">P</a> </td> <td title="S, Sulfur" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Sulfur" title="Sulfur">S</a> </td> <td title="Cl, Chlorine" style="text-align:center; background-color:#fdff8c; color:inherit; border:3px solid black; ;"><a class="mw-selflink selflink">Cl</a> </td> <td title="Ar, Argon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Argon" title="Argon">Ar</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_4_element" title="Period 4 element">4</a> </th> <td title="K, Potassium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Potassium" title="Potassium">K</a> </td> <td title="Ca, Calcium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Calcium" title="Calcium">Ca</a> </td> <td colspan="14"> </td> <td title="Sc, Scandium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Scandium" title="Scandium">Sc</a> </td> <td title="Ti, Titanium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Titanium" title="Titanium">Ti</a> </td> <td title="V, Vanadium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Vanadium" title="Vanadium">V</a> </td> <td title="Cr, Chromium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Chromium" title="Chromium">Cr</a> </td> <td title="Mn, Manganese" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Manganese" title="Manganese">Mn</a> </td> <td title="Fe, Iron" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Iron" title="Iron">Fe</a> </td> <td title="Co, Cobalt" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Cobalt" title="Cobalt">Co</a> </td> <td title="Ni, Nickel" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Nickel" title="Nickel">Ni</a> </td> <td title="Cu, Copper" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Copper" title="Copper">Cu</a> </td> <td title="Zn, Zinc" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Zinc" title="Zinc">Zn</a> </td> <td title="Ga, Gallium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Gallium" title="Gallium">Ga</a> </td> <td title="Ge, Germanium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Germanium" title="Germanium">Ge</a> </td> <td title="As, Arsenic" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Arsenic" title="Arsenic">As</a> </td> <td title="Se, Selenium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Selenium" title="Selenium">Se</a> </td> <td title="Br, Bromine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Bromine" title="Bromine">Br</a> </td> <td title="Kr, Krypton" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Krypton" title="Krypton">Kr</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_5_element" title="Period 5 element">5</a> </th> <td title="Rb, Rubidium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Rubidium" title="Rubidium">Rb</a> </td> <td title="Sr, Strontium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Strontium" title="Strontium">Sr</a> </td> <td colspan="14"> </td> <td title="Y, Yttrium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Yttrium" title="Yttrium">Y</a> </td> <td title="Zr, Zirconium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Zirconium" title="Zirconium">Zr</a> </td> <td title="Nb, Niobium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Niobium" title="Niobium">Nb</a> </td> <td title="Mo, Molybdenum" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Molybdenum" title="Molybdenum">Mo</a> </td> <td title="Tc, Technetium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Technetium" title="Technetium">Tc</a> </td> <td title="Ru, Ruthenium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Ruthenium" title="Ruthenium">Ru</a> </td> <td title="Rh, Rhodium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Rhodium" title="Rhodium">Rh</a> </td> <td title="Pd, Palladium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Palladium" title="Palladium">Pd</a> </td> <td title="Ag, Silver" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Silver" title="Silver">Ag</a> </td> <td title="Cd, Cadmium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Cadmium" title="Cadmium">Cd</a> </td> <td title="In, Indium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Indium" title="Indium">In</a> </td> <td title="Sn, Tin" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Tin" title="Tin">Sn</a> </td> <td title="Sb, Antimony" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Antimony" title="Antimony">Sb</a> </td> <td title="Te, Tellurium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Tellurium" title="Tellurium">Te</a> </td> <td title="I, Iodine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Iodine" title="Iodine">I</a> </td> <td title="Xe, Xenon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Xenon" title="Xenon">Xe</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_6_element" title="Period 6 element">6</a> </th> <td title="Cs, Caesium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Caesium" title="Caesium">Cs</a> </td> <td title="Ba, Barium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Barium" title="Barium">Ba</a> </td> <td title="La, Lanthanum" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Lanthanum" title="Lanthanum">La</a> </td> <td title="Ce, Cerium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Cerium" title="Cerium">Ce</a> </td> <td title="Pr, Praseodymium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Praseodymium" title="Praseodymium">Pr</a> </td> <td title="Nd, Neodymium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Neodymium" title="Neodymium">Nd</a> </td> <td title="Pm, Promethium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Promethium" title="Promethium">Pm</a> </td> <td title="Sm, Samarium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Samarium" title="Samarium">Sm</a> </td> <td title="Eu, Europium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Europium" title="Europium">Eu</a> </td> <td title="Gd, Gadolinium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Gadolinium" title="Gadolinium">Gd</a> </td> <td title="Tb, Terbium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Terbium" title="Terbium">Tb</a> </td> <td title="Dy, Dysprosium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Dysprosium" title="Dysprosium">Dy</a> </td> <td title="Ho, Holmium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Holmium" title="Holmium">Ho</a> </td> <td title="Er, Erbium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Erbium" title="Erbium">Er</a> </td> <td title="Tm, Thulium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Thulium" title="Thulium">Tm</a> </td> <td title="Yb, Ytterbium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Ytterbium" title="Ytterbium">Yb</a> </td> <td title="Lu, Lutetium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Lutetium" title="Lutetium">Lu</a> </td> <td title="Hf, Hafnium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Hafnium" title="Hafnium">Hf</a> </td> <td title="Ta, Tantalum" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Tantalum" title="Tantalum">Ta</a> </td> <td title="W, Tungsten" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Tungsten" title="Tungsten">W</a> </td> <td title="Re, Rhenium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Rhenium" title="Rhenium">Re</a> </td> <td title="Os, Osmium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Osmium" title="Osmium">Os</a> </td> <td title="Ir, Iridium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Iridium" title="Iridium">Ir</a> </td> <td title="Pt, Platinum" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Platinum" title="Platinum">Pt</a> </td> <td title="Au, Gold" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Gold" title="Gold">Au</a> </td> <td title="Hg, Mercury" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Mercury_(element)" title="Mercury (element)">Hg</a> </td> <td title="Tl, Thallium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Thallium" title="Thallium">Tl</a> </td> <td title="Pb, Lead" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Lead" title="Lead">Pb</a> </td> <td title="Bi, Bismuth" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Bismuth" title="Bismuth">Bi</a> </td> <td title="Po, Polonium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Polonium" title="Polonium">Po</a> </td> <td title="At, Astatine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Astatine" title="Astatine">At</a> </td> <td title="Rn, Radon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Radon" title="Radon">Rn</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_7_element" title="Period 7 element">7</a> </th> <td title="Fr, Francium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Francium" title="Francium">Fr</a> </td> <td title="Ra, Radium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Radium" title="Radium">Ra</a> </td> <td title="Ac, Actinium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Actinium" title="Actinium">Ac</a> </td> <td title="Th, Thorium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Thorium" title="Thorium">Th</a> </td> <td title="Pa, Protactinium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Protactinium" title="Protactinium">Pa</a> </td> <td title="U, Uranium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Uranium" title="Uranium">U</a> </td> <td title="Np, Neptunium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Neptunium" title="Neptunium">Np</a> </td> <td title="Pu, Plutonium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Plutonium" title="Plutonium">Pu</a> </td> <td title="Am, Americium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Americium" title="Americium">Am</a> </td> <td title="Cm, Curium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Curium" title="Curium">Cm</a> </td> <td title="Bk, Berkelium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Berkelium" title="Berkelium">Bk</a> </td> <td title="Cf, Californium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Californium" title="Californium">Cf</a> </td> <td title="Es, Einsteinium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Einsteinium" title="Einsteinium">Es</a> </td> <td title="Fm, Fermium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Fermium" title="Fermium">Fm</a> </td> <td title="Md, Mendelevium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Mendelevium" title="Mendelevium">Md</a> </td> <td title="No, Nobelium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Nobelium" title="Nobelium">No</a> </td> <td title="Lr, Lawrencium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Lawrencium" title="Lawrencium">Lr</a> </td> <td title="Rf, Rutherfordium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Rutherfordium" title="Rutherfordium">Rf</a> </td> <td title="Db, Dubnium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Dubnium" title="Dubnium">Db</a> </td> <td title="Sg, Seaborgium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Seaborgium" title="Seaborgium">Sg</a> </td> <td title="Bh, Bohrium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Bohrium" title="Bohrium">Bh</a> </td> <td title="Hs, Hassium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Hassium" title="Hassium">Hs</a> </td> <td title="Mt, Meitnerium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Meitnerium" title="Meitnerium">Mt</a> </td> <td title="Ds, Darmstadtium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Darmstadtium" title="Darmstadtium">Ds</a> </td> <td title="Rg, Roentgenium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Roentgenium" title="Roentgenium">Rg</a> </td> <td title="Cn, Copernicium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Copernicium" title="Copernicium">Cn</a> </td> <td title="Nh, Nihonium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Nihonium" title="Nihonium">Nh</a> </td> <td title="Fl, Flerovium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Flerovium" title="Flerovium">Fl</a> </td> <td title="Mc, Moscovium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Moscovium" title="Moscovium">Mc</a> </td> <td title="Lv, Livermorium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Livermorium" title="Livermorium">Lv</a> </td> <td title="Ts, Tennessine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Tennessine" title="Tennessine">Ts</a> </td> <td title="Og, Oganesson" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Oganesson" title="Oganesson">Og</a> </td></tr></tbody></table> </div></td></tr><tr><td colspan="2" class="navbox-list navbox-even wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"><div role="presentation" id="periodic-table-legend" style="border: 1px solid #a2a9b1; width:100%; line-height:120%; text-align:center; vertical-align:top; background:#f8f8f8;color:inherit; margin:0; margin:0;"><div style="padding:0.3em;"> <table style="width:100%; line-height:1.2em; table-layout:fixed; overflow:hidden; text-align:center;"> <tbody><tr> <td style="padding:0 1px; background:#ff9999;color:inherit;"><a href="/wiki/S-block" class="mw-redirect" title="S-block">s-block</a> </td> <td style="padding:0 1px; background:#9bff99;color:inherit;"><a href="/wiki/F-block" class="mw-redirect" title="F-block">f-block</a> </td> <td style="padding:0 1px; background:#99ccff;color:inherit;"><a href="/wiki/D-block" class="mw-redirect" title="D-block">d-block</a> </td> <td style="padding:0 1px; background:#fdff8c;color:inherit;"><a href="/wiki/P-block" class="mw-redirect" title="P-block">p-block</a> </td></tr></tbody></table> </div> </div></div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"></div><div role="navigation" class="navbox" aria-labelledby="Diatomic_chemical_elements63" style="padding:3px"><table class="nowraplinks mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Diatomic_elements" title="Template:Diatomic elements"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Diatomic_elements" title="Template talk:Diatomic elements"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Diatomic_elements" title="Special:EditPage/Template:Diatomic elements"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Diatomic_chemical_elements63" style="font-size:114%;margin:0 4em"><a href="/wiki/Diatomic_molecule" title="Diatomic molecule">Diatomic</a> <a href="/wiki/Chemical_element" title="Chemical element">chemical elements</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%">Common</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0;text-align:center;"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Hydrogen" title="Hydrogen">H2</a></li> <li><a href="/wiki/Nitrogen" title="Nitrogen">N2</a></li> <li><a href="/wiki/Oxygen" title="Oxygen">O2</a></li> <li><a href="/wiki/Fluorine" title="Fluorine">F2</a></li> <li><a class="mw-selflink selflink">Cl2</a></li> <li><a href="/wiki/Bromine" title="Bromine">Br2</a></li> <li><a href="/wiki/Iodine" title="Iodine">I2</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Other</th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0;text-align:center;"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Helium_dimer" title="Helium dimer">He2</a></li> <li><a href="/wiki/Diargon" title="Diargon">Ar2</a></li> <li><a href="/wiki/Diatomic_carbon" title="Diatomic carbon">C2</a></li> <li><a href="/wiki/Diphosphorus" title="Diphosphorus">P2</a></li> <li><a href="/wiki/Disulfur" title="Disulfur">S2</a></li> <li><a href="/wiki/Dilithium" title="Dilithium">Li2</a></li> <li><a href="/wiki/Dirubidium" title="Dirubidium">Rb2</a></li></ul> </div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"></div><div role="navigation" class="navbox" aria-labelledby="United_States_chemical_weapons_program3581" style=";wide;padding:3px"><table class="nowraplinks hlist mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2" style="background-color:#C3D6EF;color:inherit;"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:U.S._chemical_weapons" title="Template:U.S. chemical weapons"><abbr title="View this template" style="color:inherit">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:U.S._chemical_weapons" title="Template talk:U.S. chemical weapons"><abbr title="Discuss this template" style="color:inherit">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:U.S._chemical_weapons" title="Special:EditPage/Template:U.S. chemical weapons"><abbr title="Edit this template" style="color:inherit">e</abbr></a></li></ul></div><div id="United_States_chemical_weapons_program3581" style="font-size:114%;margin:0 4em"><a href="/wiki/United_States_chemical_weapons_program" title="United States chemical weapons program">United States chemical weapons program</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Units, formations, centers and institutes</th><td class="navbox-list-with-group navbox-list navbox-odd wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/2nd_Chemical_Battalion_(United_States)" title="2nd Chemical Battalion (United States)">2nd Chemical Battalion</a></li> <li><a href="/wiki/Chemical_Corps" title="Chemical Corps">U.S. Army Chemical Corps</a></li> <li><a href="/wiki/Edgewood_Chemical_Biological_Center" title="Edgewood Chemical Biological Center">U.S. Army Edgewood Chemical Biological Center</a></li> <li><a href="/wiki/United_States_Army_Medical_Research_Institute_of_Chemical_Defense" title="United States Army Medical Research Institute of Chemical Defense">U.S. Army Medical Research Institute of Chemical Defense</a> (USAMRICD)</li> <li><a href="/wiki/United_States_Army_Chemical_Materials_Activity" title="United States Army Chemical Materials Activity">U.S. Army Chemical Materials Activity</a></li> <li><a href="/wiki/Program_Executive_Office,_Assembled_Chemical_Weapons_Alternatives" title="Program Executive Office, Assembled Chemical Weapons Alternatives">Program Executive Office, Assembled Chemical Weapons Alternatives</a></li> <li><a href="/wiki/Chemical_mortar_battalion" title="Chemical mortar battalion">Chemical mortar battalion</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Industrial facilities</th><td class="navbox-list-with-group navbox-list navbox-even wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Anniston_Army_Depot" title="Anniston Army Depot">Anniston Army Depot</a></li> <li><a href="/wiki/Anniston_Chemical_Activity" title="Anniston Chemical Activity">Anniston Chemical Activity</a></li> <li><a href="/wiki/Blue_Grass_Army_Depot" title="Blue Grass Army Depot">Blue Grass Army Depot</a></li> <li><a href="/wiki/Deseret_Chemical_Depot" title="Deseret Chemical Depot">Deseret Chemical Depot</a></li> <li><a href="/wiki/Edgewood_Chemical_Activity" title="Edgewood Chemical Activity">Edgewood Chemical Activity</a></li> <li><a href="/wiki/Hawthorne_Army_Depot" title="Hawthorne Army Depot">Hawthorne Army Depot</a></li> <li><a href="/wiki/Johnston_Atoll_Chemical_Agent_Disposal_System" title="Johnston Atoll Chemical Agent Disposal System">Johnston Atoll Chemical Agent Disposal System</a></li> <li><a href="/wiki/Newport_Chemical_Depot" title="Newport Chemical Depot">Newport Chemical Depot</a></li> <li><a href="/wiki/Pine_Bluff_Chemical_Activity" title="Pine Bluff Chemical Activity">Pine Bluff Chemical Activity</a></li> <li><a href="/wiki/Pueblo_Chemical_Depot" title="Pueblo Chemical Depot">Pueblo Chemical Depot</a></li> <li><a href="/wiki/Tooele_Chemical_Agent_Disposal_Facility" title="Tooele Chemical Agent Disposal Facility">Tooele Chemical Agent Disposal Facility</a></li> <li><a href="/wiki/Umatilla_Chemical_Depot" title="Umatilla Chemical Depot">Umatilla Chemical Depot</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Operations and projects</th><td class="navbox-list-with-group navbox-list navbox-odd wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0;;wide"><tbody><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Research</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Edgewood_Arsenal_human_experiments" title="Edgewood Arsenal human experiments">Edgewood Arsenal human experiments</a></li> <li><a href="/wiki/Operation_Top_Hat" title="Operation Top Hat">Operation Top Hat</a></li> <li><a href="/wiki/Project_112" title="Project 112">Project 112</a></li> <li><a href="/wiki/Project_SHAD" title="Project SHAD">Project SHAD</a></li> <li><a href="/wiki/Operation_LAC" title="Operation LAC">Operation LAC</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Operational</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Operation_Ranch_Hand" title="Operation Ranch Hand">Operation Ranch Hand</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Disposal</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Operation_CHASE" title="Operation CHASE">Operation CHASE</a></li> <li><a href="/wiki/Operation_Davy_Jones%27_Locker" title="Operation Davy Jones' Locker">Operation Davy Jones' Locker</a></li> <li><a href="/wiki/Operation_Geranium" title="Operation Geranium">Operation Geranium</a></li> <li><a href="/wiki/Operation_Steel_Box" title="Operation Steel Box">Operation Steel Box</a></li> <li><a href="/wiki/Operation_Red_Hat" title="Operation Red Hat">Operation Red Hat</a></li></ul> </div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;"><a href="/wiki/CB_military_symbol" title="CB military symbol">Agents</a></th><td class="navbox-list-with-group navbox-list navbox-even wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/3-Quinuclidinyl_benzilate" title="3-Quinuclidinyl benzilate">3-Quinuclidinyl benzilate</a> (BZ)</li> <li><a class="mw-selflink selflink">Chlorine</a></li> <li><a href="/wiki/Methylphosphonyl_difluoride" title="Methylphosphonyl difluoride">Methylphosphonyl difluoride</a> (DF)</li> <li><a href="/wiki/Phosgene" title="Phosgene">Phosgene</a></li> <li><a href="/wiki/QL_(chemical)" title="QL (chemical)">QL</a></li> <li><a href="/wiki/Sarin" title="Sarin">Sarin</a> (GB)</li> <li><a href="/wiki/Mustard_gas" title="Mustard gas">Mustard gas</a> (HD)</li> <li><a href="/wiki/VX_(nerve_agent)" title="VX (nerve agent)">VX</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Munitions</th><td class="navbox-list-with-group navbox-list navbox-odd wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/BLU-80/B_Bigeye_bomb" title="BLU-80/B Bigeye bomb">BLU-80/B Bigeye bomb</a></li> <li><a href="/wiki/M1_chemical_mine" title="M1 chemical mine">M1 chemical mine</a></li> <li><a href="/wiki/M104_155_mm_projectile" title="M104 155 mm projectile">M104 155 mm projectile</a></li> <li><a href="/wiki/M110_155_mm_projectile" title="M110 155 mm projectile">M110 155 mm projectile</a></li> <li><a href="/wiki/M121_155_mm_projectile" title="M121 155 mm projectile">M121 155 mm projectile</a></li> <li><a href="/wiki/M125_bomblet" title="M125 bomblet">M125 bomblet</a></li> <li><a href="/wiki/M134_bomblet" title="M134 bomblet">M134 bomblet</a></li> <li><a href="/wiki/M138_bomblet" title="M138 bomblet">M138 bomblet</a></li> <li><a href="/wiki/M139_bomblet" title="M139 bomblet">M139 bomblet</a></li> <li><a href="/wiki/M2_mortar" title="M2 mortar">M2 mortar</a></li> <li><a href="/wiki/M23_chemical_mine" title="M23 chemical mine">M23 chemical mine</a></li> <li><a href="/wiki/M34_cluster_bomb" title="M34 cluster bomb">M34 cluster bomb</a></li> <li><a href="/wiki/M360_105_mm_projectile" title="M360 105 mm projectile">M360 105 mm projectile</a></li> <li><a href="/wiki/M426_8-inch_shell" title="M426 8-inch shell">M426 8-inch shell</a></li> <li><a href="/wiki/M43_BZ_cluster_bomb" title="M43 BZ cluster bomb">M43 BZ cluster bomb</a></li> <li><a href="/wiki/M44_generator_cluster" title="M44 generator cluster">M44 generator cluster</a></li> <li><a href="/wiki/M55_(rocket)" title="M55 (rocket)">M55 rocket</a></li> <li><a href="/wiki/M60_105_mm_projectile" title="M60 105 mm projectile">M60 105 mm projectile</a></li> <li><a href="/wiki/M687_155_mm_projectile" title="M687 155 mm projectile">M687 155 mm projectile</a></li> <li><a href="/wiki/XM736_8-inch_projectile" title="XM736 8-inch projectile">XM736 8-inch projectile</a></li> <li><a href="/wiki/MC-1_bomb" title="MC-1 bomb">MC-1 bomb</a></li> <li><a href="/wiki/M47_bomb" title="M47 bomb">M47 bomb</a></li> <li><a href="/wiki/Weteye_bomb" title="Weteye bomb">Weteye bomb</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Protective equipment</th><td class="navbox-list-with-group navbox-list navbox-even wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Chemical_Agent_Identification_Set" title="Chemical Agent Identification Set">CAIS</a></li> <li><a href="/wiki/TPz_Fuchs" title="TPz Fuchs">M93 Fox</a></li> <li><a href="/wiki/MOPP_(protective_gear)" title="MOPP (protective gear)">MOPP</a></li> <li><a href="/wiki/People_sniffer" title="People sniffer">People sniffer</a></li> <li><a href="/wiki/M1135_nuclear,_biological,_and_chemical_reconnaissance_vehicle" title="M1135 nuclear, biological, and chemical reconnaissance vehicle">M1135 NBCRV</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;background-color:#DCDCDC;color:inherit;">Related topics</th><td class="navbox-list-with-group navbox-list navbox-odd wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/CB_military_symbol" title="CB military symbol">CB military symbol</a></li> <li><a href="/wiki/Dugway_sheep_incident" title="Dugway sheep incident">Dugway sheep incident</a></li> <li><a href="/wiki/Unethical_human_experimentation_in_the_United_States" title="Unethical human experimentation in the United States">Unethical human experimentation in the United States</a></li> <li><a href="/wiki/MKULTRA" class="mw-redirect" title="MKULTRA">MKULTRA</a></li></ul> </div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"></div><div role="navigation" class="navbox" aria-labelledby="Agents_used_in_chemical_warfareincapacitationriot_control542" style="padding:3px"><table class="nowraplinks hlist mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:Chemical_agents" title="Template:Chemical agents"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Chemical_agents" title="Template talk:Chemical agents"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Chemical_agents" title="Special:EditPage/Template:Chemical agents"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Agents_used_in_chemical_warfareincapacitationriot_control542" style="font-size:114%;margin:0 4em"><div class="hlist"><ul><li>Agents used in <a href="/wiki/Chemical_warfare" title="Chemical warfare">chemical warfare</a></li><li><a href="/wiki/Incapacitating_agent" title="Incapacitating agent">incapacitation</a></li><li><a href="/wiki/Riot_control" title="Riot control">riot control</a></li></ul></div></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Blood_agent" title="Blood agent">Blood agents</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Cyanogen" title="Cyanogen">Cyanogen</a></li> <li><a href="/wiki/Cyanogen_bromide" title="Cyanogen bromide">Cyanogen bromide</a></li> <li><a href="/wiki/Cyanogen_chloride" title="Cyanogen chloride">Cyanogen chloride</a> (CK)</li> <li><a href="/wiki/Hydrogen_cyanide" title="Hydrogen cyanide">Hydrogen cyanide</a> (AC)</li> <li><a href="/wiki/Arsine" title="Arsine">Arsine</a></li> <li><a href="/wiki/Cacodyl_cyanide" title="Cacodyl cyanide">Cacodyl cyanide</a></li> <li><a href="/wiki/Cacodyl_oxide" title="Cacodyl oxide">Cacodyl oxide</a></li> <li><a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">Hydrogen sulfide</a></li> <li><a href="/wiki/Phosphine" title="Phosphine">Phosphine</a></li> <li><a href="/wiki/Carbon_monoxide" title="Carbon monoxide">Carbon monoxide</a></li> <li><a href="/wiki/Phosphorus_trifluoride" title="Phosphorus trifluoride">Phosphorus trifluoride</a></li> <li><a href="/wiki/Methyl_cyanoformate" title="Methyl cyanoformate">Methyl cyanoformate</a></li> <li><a href="/wiki/Iron_pentacarbonyl" title="Iron pentacarbonyl">Iron pentacarbonyl</a></li> <li><a href="/wiki/Nickel_tetracarbonyl" title="Nickel tetracarbonyl">Nickel tetracarbonyl</a></li> <li><a href="/wiki/2,3,7,8-Tetrachlorodibenzodioxin" title="2,3,7,8-Tetrachlorodibenzodioxin">2,3,7,8-Tetrachlorodibenzodioxin</a></li> <li><a href="/wiki/Glycolonitrile" title="Glycolonitrile">Glycolonitrile</a></li> <li><a href="/wiki/Lactonitrile" title="Lactonitrile">Lactonitrile</a></li> <li><a href="/wiki/Acetone_cyanohydrin" title="Acetone cyanohydrin">Acetone cyanohydrin</a></li> <li><a href="/wiki/Stibine" title="Stibine">Stibine</a></li> <li><a href="/wiki/Chloral_cyanohydrin" title="Chloral cyanohydrin">Chloral cyanohydrin</a></li></ul></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Blister_agent" title="Blister agent">Blister agents</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Arsenical" title="Arsenical">Arsenicals</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <li><a href="/wiki/Ethyldichloroarsine" title="Ethyldichloroarsine">Ethyldichloroarsine</a> (ED)</li> <li><a href="/wiki/Methyldichloroarsine" title="Methyldichloroarsine">Methyldichloroarsine</a> (MD)</li> <li><a href="/wiki/Phenyldichloroarsine" title="Phenyldichloroarsine">Phenyldichloroarsine</a> (PD)</li> <li><a href="/wiki/Lewisite" title="Lewisite">Lewisite</a> (L)</li> <li><a href="/wiki/Lewisite_2" title="Lewisite 2">Lewisite 2</a> (L2)</li> <li><a href="/wiki/Lewisite_3" title="Lewisite 3">Lewisite 3</a> (L3)</li> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Sulfur_mustard" class="mw-redirect" title="Sulfur mustard">Sulfur mustards</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Mustard_gas" title="Mustard gas">Levinstein mustard</a> (EA-229)</li> <li><a href="/wiki/O-Mustard" class="mw-redirect" title="O-Mustard">T</a></li> <li><a href="/wiki/Sesquimustard" title="Sesquimustard">Q</a></li> <li><a href="/wiki/2-Chloroethyl_ethyl_sulfide" title="2-Chloroethyl ethyl sulfide">CEES</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Nitrogen_mustard" title="Nitrogen mustard">Nitrogen mustards</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/HN1_(nitrogen_mustard)" title="HN1 (nitrogen mustard)">HN1</a></li> <li><a href="/wiki/Chlormethine" title="Chlormethine">HN2</a></li> <li><a href="/wiki/HN3_(nitrogen_mustard)" title="HN3 (nitrogen mustard)">HN3</a></li> <li><a href="/wiki/TL-301" title="TL-301">TL-301</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Nettle_agent" title="Nettle agent">Nettle agents</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Phosgene_oxime" title="Phosgene oxime">Phosgene oxime</a> (CX)</li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Other</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/KB-16" title="KB-16">KB-16</a></li> <li><a href="/wiki/Dibutylchloromethyltin_chloride" title="Dibutylchloromethyltin chloride">Dibutylchloromethyltin chloride</a></li> <li><a href="/wiki/Selenium_oxychloride" class="mw-redirect" title="Selenium oxychloride">Selenium oxychloride</a></li> <li><a href="/wiki/Phenacyl_bromide" title="Phenacyl bromide">Phenacyl bromide</a></li></ul> </div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Nerve_agent" title="Nerve agent">Nerve agents</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Nerve_agent#G-Series" title="Nerve agent">G-agents</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Tabun_(nerve_agent)" title="Tabun (nerve agent)">Tabun</a> (GA)</li> <li><a href="/wiki/Sarin" title="Sarin">Sarin (GB)</a></li> <li><a href="/wiki/Chlorosarin" title="Chlorosarin">Chlorosarin</a> (ClGB)</li> <li><a href="/wiki/Thiosarin" title="Thiosarin">Thiosarin</a> (SGB)</li> <li><a href="/wiki/Soman" title="Soman">Soman</a> (GD)</li> <li><a href="/wiki/Chlorosoman" title="Chlorosoman">Chlorosoman</a> (ClGD)</li> <li><a href="/wiki/Ethylsarin" title="Ethylsarin">Ethylsarin</a> (GE)</li> <li><a href="/wiki/GH_(nerve_agent)" title="GH (nerve agent)">GH</a></li> <li><a href="/wiki/Cyclosarin" title="Cyclosarin">Cyclosarin</a> (GF)</li> <li><a href="/wiki/GP_(nerve_agent)" title="GP (nerve agent)">GP</a></li> <li><a href="/wiki/Fluorotabun" title="Fluorotabun">Fluorotabun</a></li> <li><a href="/wiki/EA-1356" title="EA-1356">EA-1356</a></li> <li><a href="/wiki/EA-4352" title="EA-4352">EA-4352</a></li> <li><a href="/wiki/Crotylsarin" title="Crotylsarin">Crotylsarin</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Nerve_agent#V-Series" title="Nerve agent">V-agents</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/EA-2192" title="EA-2192">EA-2192</a></li> <li><a href="/wiki/EA-3148" title="EA-3148">EA-3148</a></li> <li><a href="/wiki/VE_(nerve_agent)" title="VE (nerve agent)">VE</a></li> <li><a href="/wiki/VG_(nerve_agent)" title="VG (nerve agent)">VG</a></li> <li><a href="/wiki/VM_(nerve_agent)" title="VM (nerve agent)">VM</a></li> <li><a href="/wiki/3,3,5-Trimethylcyclohexyl_3-pyridyl_methylphosphonate" title="3,3,5-Trimethylcyclohexyl 3-pyridyl methylphosphonate">VP</a></li> <li><a href="/wiki/VR_(nerve_agent)" title="VR (nerve agent)">VR</a></li> <li><a href="/wiki/VS_(nerve_agent)" title="VS (nerve agent)">VS</a></li> <li><a href="/wiki/VX_(nerve_agent)" title="VX (nerve agent)">VX</a></li> <li><a href="/wiki/EA-1763" title="EA-1763">EA-1763</a></li> <li><a href="/wiki/Chinese_VX" title="Chinese VX">Chinese VX</a></li> <li><a href="/wiki/V-sub_x" title="V-sub x">V-sub x (GD-7)</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">GV agents</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/GV_(nerve_agent)" title="GV (nerve agent)">GV (EA-5365)</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Novichok_agent" class="mw-redirect" title="Novichok agent">Novichok agents</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/VR_(nerve_agent)" title="VR (nerve agent)">A-208</a></li> <li><a href="/wiki/A-232" title="A-232">A-232</a></li> <li><a href="/wiki/A-234_(nerve_agent)" title="A-234 (nerve agent)">A-234</a></li> <li><a href="/wiki/A-242" title="A-242">A-242</a></li> <li><a href="/wiki/A-262" title="A-262">A-262</a></li> <li><a href="/wiki/C01-A035" title="C01-A035">C01-A035</a></li> <li><a href="/wiki/C01-A039" title="C01-A039">C01-A039</a></li> <li><a href="/wiki/C01-A042" title="C01-A042">C01-A042</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Carbamate" title="Carbamate">Carbamates</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Dimethylcarbamoyl_fluoride" title="Dimethylcarbamoyl fluoride">Dimethylcarbamoyl fluoride</a></li> <li><a href="/wiki/EA-3887" title="EA-3887">EA-3887</a></li> <li><a href="/wiki/EA-3887A" class="mw-redirect" title="EA-3887A">EA-3887A</a></li> <li><a href="/wiki/EA-3966" title="EA-3966">EA-3966</a></li> <li><a href="/wiki/EA-3990" title="EA-3990">EA-3990</a></li> <li><a href="/wiki/EA-4056" title="EA-4056">EA-4056</a></li> <li><a href="/wiki/T-1123" title="T-1123">T-1123</a></li> <li><a href="/wiki/T-1152" title="T-1152">T-1152</a></li> <li><a href="/wiki/T-1194" title="T-1194">T-1194</a></li> <li><a href="/wiki/Octamethylene-bis(5-dimethylcarbamoxyisoquinolinium_bromide)" title="Octamethylene-bis(5-dimethylcarbamoxyisoquinolinium bromide)">Octamethylene-bis(5-dimethylcarbamoxyisoquinolinium bromide)</a></li> <li><a href="/wiki/TL-599" title="TL-599">TL-599</a></li> <li><a href="/wiki/TL-1238" title="TL-1238">TL-1238</a></li> <li><a href="/wiki/TL-1299" class="mw-redirect" title="TL-1299">TL-1299</a></li> <li><a href="/wiki/TL-1317" class="mw-redirect" title="TL-1317">TL-1317</a></li> <li><a href="/wiki/Miotine" title="Miotine">Miotine (AR-28/T-1843)</a></li> <li><a href="/wiki/3152_CT" title="3152 CT">3152 CT</a></li> <li><a href="/wiki/4-686-293-01" title="4-686-293-01">4-686-293-01 (Agent 1-10)</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Other</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Diisopropyl_fluorophosphate" title="Diisopropyl fluorophosphate">Diisopropyl fluorophosphate</a></li> <li><a href="/wiki/Dicyclohexyl_phosphorofluoridate" title="Dicyclohexyl phosphorofluoridate">Dicyclohexyl phosphorofluoridate</a></li> <li><a href="/wiki/EA-2012" title="EA-2012">EA-2012</a></li> <li><a href="/wiki/EA-2054" title="EA-2054">EA-2054</a></li> <li><a href="/wiki/EA-2098" title="EA-2098">EA-2098</a></li> <li><a href="/wiki/EA-2613" title="EA-2613">EA-2613</a></li> <li><a href="/wiki/2-Ethoxycarbonyl-1-methylvinyl_cyclohexyl_methylphosphonate" title="2-Ethoxycarbonyl-1-methylvinyl cyclohexyl methylphosphonate">2-Ethoxycarbonyl-1-methylvinyl cyclohexyl methylphosphonate</a></li> <li><a href="/wiki/Neopentylene_fluorophosphate" title="Neopentylene fluorophosphate">Neopentylene fluorophosphate</a></li> <li><a href="/wiki/Selenophos" title="Selenophos">Selenophos</a></li> <li><a href="/wiki/Phospholine" class="mw-redirect" title="Phospholine">Phospholine</a></li> <li><a href="/wiki/R-16661" title="R-16661">R-16661</a></li> <li><a href="/wiki/Ro_3-0422" title="Ro 3-0422">Ro 3-0422</a></li> <li><a href="/wiki/Methanesulfonyl_fluoride" title="Methanesulfonyl fluoride">Methanesulfonyl fluoride</a></li> <li><a href="/wiki/Dimefox" title="Dimefox">Dimefox (TL-792)</a></li> <li><a href="/wiki/MSPI_(nerve_agent)" title="MSPI (nerve agent)">MSPI</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Precursors</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Acetonitrile" title="Acetonitrile">Acetonitrile</a></li> <li><a href="/wiki/Arsenic_trichloride" title="Arsenic trichloride">AT</a></li> <li><a href="/wiki/Arsenic_trioxide" title="Arsenic trioxide">ATO</a></li> <li><a href="/wiki/Aluminium_phosphide" title="Aluminium phosphide">AlP</a></li> <li><a href="/wiki/Kinnear%E2%80%93Perren_reaction" title="Kinnear–Perren reaction">A.P.C. complex</a></li> <li><a href="/wiki/Chlorosarin" title="Chlorosarin">Chlorosarin</a></li> <li><a href="/wiki/Chlorosoman" title="Chlorosoman">Chlorosoman</a></li> <li><a href="/wiki/Cyclohexanol" title="Cyclohexanol">Cyclohexanol</a></li> <li><a href="/wiki/1,8-Dibromooctane" title="1,8-Dibromooctane">1,8-Dibromooctane</a></li> <li><a href="/wiki/N,N-Diisopropylaminoethanol" title="N,N-Diisopropylaminoethanol">N,N-Diisopropylaminoethanol</a> (KB)</li> <li><a href="/wiki/Diisopropyl_methylphosphonate" title="Diisopropyl methylphosphonate">EA-1250</a></li> <li><a href="/wiki/Diisopropylphosphite" title="Diisopropylphosphite">DIHP</a></li> <li><a href="/wiki/Ethanol" title="Ethanol">ZS</a></li> <li><a href="/wiki/Diethylphosphite" title="Diethylphosphite">DEHP</a></li> <li><a href="/wiki/Dimethyl_methylphosphonate" title="Dimethyl methylphosphonate">EA-1224</a></li> <li><a href="/wiki/Dimethylamidophosphoric_dichloride" title="Dimethylamidophosphoric dichloride">Dimethylamidophosphoric dichloride</a></li> <li><a href="/wiki/Dimethylamidophosphoric_dicyanide" title="Dimethylamidophosphoric dicyanide">Dimethylamidophosphoric dicyanide</a></li> <li><a href="/wiki/Dimethylphosphite" title="Dimethylphosphite">DMHP</a></li> <li><a href="/wiki/Ethylphosphonoselenoic_dichloride" title="Ethylphosphonoselenoic dichloride">Ethylphosphonoselenoic dichloride</a></li> <li><a href="/wiki/Formaldoxime" title="Formaldoxime">Formaldoxime</a></li> <li><a href="/wiki/Fulminic_acid" title="Fulminic acid">Nital</a></li> <li><a href="/wiki/4-Hydroxycoumarin" title="4-Hydroxycoumarin">4-Hydroxycoumarin</a></li> <li><a href="/wiki/Isopropyl_alcohol" title="Isopropyl alcohol">Isopropyl alcohol</a> (TB)</li> <li><a href="/wiki/Methyldichlorophosphine" title="Methyldichlorophosphine">Methyldichlorophosphine</a> (SW)</li> <li><a href="/wiki/Methylphosphonyl_difluoride" title="Methylphosphonyl difluoride">Methylphosphonyl difluoride (difluoro)</a> (DF)</li> <li><a href="/wiki/Methylphosphonyl_dichloride" title="Methylphosphonyl dichloride">Methylphosphonyl dichloride (dichloro)</a></li> <li><a href="/wiki/Nitromethane" title="Nitromethane">Nitromethane</a></li> <li><a href="/wiki/OPA_mixture" title="OPA mixture">OPA mixture</a></li> <li><a href="/wiki/Phosphoryl_chloride" title="Phosphoryl chloride">Phosphoryl chloride</a></li> <li><a href="/wiki/Phosphorus_pentachloride" title="Phosphorus pentachloride">Phosphorus pentachloride</a></li> <li><a href="/wiki/Phosphorus_trichloride" title="Phosphorus trichloride">Phosphorus trichloride</a> (TH)</li> <li><a href="/wiki/Pinacolone" title="Pinacolone">Pinacolone</a></li> <li><a href="/wiki/Pinacolyl_alcohol" title="Pinacolyl alcohol">Pinacolyl alcohol</a></li> <li><a href="/wiki/Phenacyl_chloride" title="Phenacyl chloride">Phenacyl chloride</a></li> <li><a href="/wiki/QL_(chemical)" title="QL (chemical)">QL</a></li> <li><a href="/wiki/2,4,5-Trichlorophenol" title="2,4,5-Trichlorophenol">2,4,5-Trichlorophenol</a></li> <li><a href="/wiki/3,3,5-Trimethylcyclohexanol" title="3,3,5-Trimethylcyclohexanol">3,3,5-Trimethylcyclohexanol</a></li> <li><a href="/wiki/Triethyl_phosphite" title="Triethyl phosphite">Triethyl phosphite</a></li> <li><a href="/wiki/Trimethyl_phosphite" title="Trimethyl phosphite">Trimethyl phosphite</a></li> <li><a href="/wiki/Thionyl_chloride" title="Thionyl chloride">TC</a></li> <li><a href="/wiki/Thiodiglycol" title="Thiodiglycol">TG</a></li></ul> </div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Neurotoxin" title="Neurotoxin">Neurotoxins</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Anatoxin-a" title="Anatoxin-a">Anatoxin-a</a></li> <li><a href="/wiki/Saxitoxin" title="Saxitoxin">Saxitoxin</a> (TZ)</li> <li><a href="/wiki/Coniine" title="Coniine">Coniine</a></li> <li><a href="/wiki/Bungarotoxin" title="Bungarotoxin">Bungarotoxin</a></li> <li><a href="/wiki/Botulinum_toxin" title="Botulinum toxin">Botulinum toxin</a> (BTX)</li> <li><a href="/wiki/Tetanospasmin" class="mw-redirect" title="Tetanospasmin">Tetanospasmin</a> (TeNT)</li> <li><a href="/wiki/Ryanodine" title="Ryanodine">Ryanodine</a></li> <li><a href="/wiki/Ciguatoxin" title="Ciguatoxin">Ciguatoxin</a> (CTX)</li> <li><a href="/wiki/Guanitoxin" title="Guanitoxin">Guanitoxin</a> (GTX)</li> <li><a href="/wiki/Chlorophenylsilatrane" title="Chlorophenylsilatrane">Chlorophenylsilatrane</a></li> <li><a href="/wiki/Palytoxin" title="Palytoxin">Palytoxin</a> (PTX)</li> <li><a href="/wiki/Maitotoxin" title="Maitotoxin">Maitotoxin</a> (MTX)</li> <li><a href="/wiki/Tetrodotoxin" title="Tetrodotoxin">Tetrodotoxin</a></li> <li><a href="/wiki/Veratridine" title="Veratridine">Veratridine</a></li> <li><a href="/wiki/Aconitine" title="Aconitine">Aconitine</a></li> <li><a href="/wiki/Brevetoxin" title="Brevetoxin">Brevetoxin</a> (PbTX)</li> <li><a href="/wiki/Strychnine" title="Strychnine">Strychnine</a></li> <li><a href="/wiki/Antillatoxin" title="Antillatoxin">Antillatoxin</a> (ATX)</li> <li><a href="/wiki/Tetraethyllead" title="Tetraethyllead">Tetraethyllead</a></li> <li><a href="/wiki/Dimethylmercury" title="Dimethylmercury">Dimethylmercury</a></li> <li><a href="/wiki/HN1_(nitrogen_mustard)" title="HN1 (nitrogen mustard)">HN1 hydrochloride</a></li> <li><a href="/wiki/HN2" class="mw-redirect" title="HN2">HN2 hydrochloride</a></li> <li><a href="/wiki/Tris(2-chloroethyl)amine" class="mw-redirect" title="Tris(2-chloroethyl)amine">HN3 hydrochloride</a></li> <li><a href="/wiki/IDPN_(chemical)" title="IDPN (chemical)">A-8564</a></li> <li><a href="/wiki/Picrotoxin" title="Picrotoxin">Picrotoxin</a></li> <li><a href="/wiki/Gelsemine" title="Gelsemine">Gelsemine</a></li> <li><a href="/wiki/Sulfuryl_fluoride" title="Sulfuryl fluoride">Sulfuryl fluoride</a></li> <li><a href="/wiki/Tremorine" title="Tremorine">Tremorine</a></li> <li><a href="/wiki/Oxotremorine" title="Oxotremorine">Oxotremorine</a></li> <li><a href="/wiki/Batrachotoxin" title="Batrachotoxin">Batrachotoxin</a></li> <li><a href="/wiki/Tetramethylenedisulfotetramine" title="Tetramethylenedisulfotetramine">Tetramethylenedisulfotetramine (TETS)</a></li> <li><a href="/wiki/Bicyclic_phosphate" title="Bicyclic phosphate">Bicyclic phosphates</a> <ul><li><a href="/wiki/IPTBO" title="IPTBO">IPTBO</a></li> <li><a href="/wiki/TBPO" title="TBPO">TBPO</a></li> <li><a href="/wiki/TBPS" title="TBPS">TBPS</a></li></ul></li> <li><a href="/wiki/Cloflubicyne" title="Cloflubicyne">Cloflubicyne</a></li> <li><a href="/wiki/Trimethylolpropane_phosphite" title="Trimethylolpropane phosphite">Trimethylolpropane phosphite</a></li> <li><a href="/wiki/Domoic_acid" title="Domoic acid">Domoic acid</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Pulmonary_agent" title="Pulmonary agent">Pulmonary/ choking agents</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a class="mw-selflink selflink">Chlorine</a></li> <li><a href="/wiki/Bromine" title="Bromine">Bromine</a></li> <li><a href="/wiki/Phosgene" title="Phosgene">Phosgene</a> (CG)</li> <li><a href="/wiki/Fluorine" title="Fluorine">Fluorine</a></li> <li><a href="/wiki/Perfluoroisobutene" title="Perfluoroisobutene">Perfluoroisobutene</a></li> <li><a href="/wiki/Chloropicrin" title="Chloropicrin">Chloropicrin</a> (PS)</li> <li><a href="/wiki/Dimethyl(trifluoromethylthio)arsine" title="Dimethyl(trifluoromethylthio)arsine">Dimethyl(trifluoromethylthio)arsine</a></li> <li><a href="/wiki/Diphosgene" title="Diphosgene">Diphosgene</a> (DP)</li> <li><a href="/wiki/Disulfur_decafluoride" title="Disulfur decafluoride">Disulfur decafluoride</a> (Z)</li> <li><a href="/wiki/Acrolein" title="Acrolein">Acrolein</a></li> <li><a href="/wiki/Ethyl_bromoacetate" title="Ethyl bromoacetate">Ethyl bromoacetate</a></li> <li><a href="/wiki/Perchloromethyl_mercaptan" title="Perchloromethyl mercaptan">Perchloromethyl mercaptan</a></li> <li><a href="/wiki/Phenylcarbylamine_chloride" title="Phenylcarbylamine chloride">Phenylcarbylamine chloride</a></li> <li><a href="/wiki/Tetranitromethane" title="Tetranitromethane">Tetranitromethane</a></li> <li><a href="/wiki/Tetrachlorodinitroethane" title="Tetrachlorodinitroethane">Tetrachlorodinitroethane</a></li> <li><a href="/wiki/Chlorine_trifluoride" title="Chlorine trifluoride">Chlorine trifluoride</a></li> <li><a href="/wiki/Perchloryl_fluoride" title="Perchloryl fluoride">Perchloryl fluoride</a></li> <li><a href="/wiki/Cadmium_oxide" title="Cadmium oxide">Cadmium oxide</a></li> <li><a href="/wiki/Cadmium_chloride" title="Cadmium chloride">Cadmium chloride</a></li> <li><a href="/wiki/Mercury(II)_chloride" title="Mercury(II) chloride">Mercuric chloride</a></li> <li><a href="/wiki/Selenium_dioxide" title="Selenium dioxide">Selenium dioxide</a></li> <li><a href="/wiki/Selenoyl_fluoride" title="Selenoyl fluoride">Selenoyl fluoride</a></li> <li><a href="/wiki/Trifluoronitrosomethane" title="Trifluoronitrosomethane">Trifluoronitrosomethane</a></li> <li><a href="/wiki/Trichloronitrosomethane" title="Trichloronitrosomethane">Trichloronitrosomethane</a></li> <li><a href="/wiki/Nitric_oxide" title="Nitric oxide">Nitric oxide</a></li> <li><a href="/wiki/Nitrogen_dioxide" title="Nitrogen dioxide">Nitrogen dioxide</a></li> <li><a href="/wiki/Dinitrogen_tetroxide" title="Dinitrogen tetroxide">Dinitrogen tetroxide</a></li> <li><a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">Sulfur dioxide</a></li> <li><a href="/wiki/Phosphorus_trichloride" title="Phosphorus trichloride">Phosphorus trichloride</a></li> <li><a href="/wiki/Methyl_isocyanate" title="Methyl isocyanate">Methyl isocyanate</a></li> <li><a href="/wiki/Ethenone" title="Ethenone">Ethenone</a></li> <li><a href="/wiki/Methyl_vinyl_ketone" title="Methyl vinyl ketone">Methyl vinyl ketone</a></li> <li><a href="/wiki/Trifluoroacetyl_chloride" title="Trifluoroacetyl chloride">Trifluoroacetyl chloride</a></li> <li><a href="/wiki/Salcomine" title="Salcomine">Salcomine</a></li> <li><a href="/wiki/Fluomine" title="Fluomine">Fluomine</a></li> <li><a href="/wiki/Uranium_hexafluoride" title="Uranium hexafluoride">Uranium hexafluoride</a></li> <li><a href="/wiki/Diborane" title="Diborane">Diborane</a></li> <li><a href="/wiki/Green_Cross_(chemical_warfare)" title="Green Cross (chemical warfare)">Green Cross</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Vomiting_agent" title="Vomiting agent">Vomiting agents</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Adamsite" title="Adamsite">Adamsite</a> (DM)</li> <li><a href="/wiki/Chloropicrin" title="Chloropicrin">Chloropicrin</a></li> <li><a href="/wiki/Litharge" title="Litharge">Litharge</a>-<a href="/wiki/Glycerine" class="mw-redirect" title="Glycerine">glycerine</a></li> <li><a href="/wiki/Diphenylchlorarsine" title="Diphenylchlorarsine">Diphenylchlorarsine</a></li> <li><a href="/wiki/Diphenylcyanoarsine" title="Diphenylcyanoarsine">Diphenylcyanoarsine</a></li> <li><a href="/wiki/Cacodyl_cyanide" title="Cacodyl cyanide">Cacodyl cyanide</a></li> <li><a href="/wiki/O-Dianisidine" title="O-Dianisidine">o-Dianisidine</a></li> <li><a href="/wiki/Antimony_potassium_tartrate" title="Antimony potassium tartrate">Antimony potassium tartrate</a></li> <li><a href="/wiki/Lobeline" title="Lobeline">Lobeline</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Incapacitating_agent" title="Incapacitating agent">Incapacitating agents</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/3-Quinuclidinyl_benzilate" title="3-Quinuclidinyl benzilate">BZ</a> (CS-4030)</li> <li><a href="/wiki/Apomorphine" title="Apomorphine">Apomorphine</a></li> <li><a href="/wiki/Butyrophenone" title="Butyrophenone">Butyrophenone</a></li> <li><a href="/wiki/Etonitazene" title="Etonitazene">EA-4941</a> (CS-4640)</li> <li><a href="/wiki/Etorphine" title="Etorphine">Etorphine</a></li> <li><a href="/wiki/Benactyzine" title="Benactyzine">EA-2092</a></li> <li><a href="/wiki/Ditran" title="Ditran">CS-4297</a></li> <li><a href="/wiki/Etoxadrol" title="Etoxadrol">Etoxadrol</a></li> <li><a href="/wiki/Dimethylheptylpyran" title="Dimethylheptylpyran">Dimethylheptylpyran</a> (DMHP)</li> <li><a href="/wiki/Canbisol" title="Canbisol">Canbisol</a></li> <li><a href="/wiki/Phencyclidine" title="Phencyclidine">EA-2148</a></li> <li><a href="/wiki/EA-3167" title="EA-3167">EA-3167</a></li> <li><a href="/wiki/Nicotine" title="Nicotine">Nicotine</a></li> <li><a href="/wiki/EA-3443" title="EA-3443">EA-3443</a></li> <li><a href="/wiki/Methaqualone" title="Methaqualone">Methaqualone</a></li> <li><a href="/wiki/Pethidine" title="Pethidine">Pethidine</a></li> <li><a href="/wiki/EA-3580" title="EA-3580">EA-3580</a></li> <li><a href="/wiki/Ibogaine" title="Ibogaine">Ibogaine</a></li> <li><a href="/wiki/EA-3834" title="EA-3834">EA-3834</a></li> <li><a href="/wiki/Kolokol-1" title="Kolokol-1">Kolokol-1</a></li> <li><a href="/wiki/LSD" title="LSD">LSD-25</a></li> <li><a href="/wiki/PAVA_spray" title="PAVA spray">PAVA spray</a></li> <li><a href="/wiki/Psilocybin" title="Psilocybin">Psilocybin</a></li> <li><a href="/wiki/Incapacitating_agent#Sleeping_gas" title="Incapacitating agent">Sleeping gas</a></li> <li><a href="/wiki/Carfentanil" title="Carfentanil">Carfentanil</a></li> <li><a href="/wiki/N-Ethyl-3-piperidyl_benzilate" title="N-Ethyl-3-piperidyl benzilate">JB-318</a></li> <li><a href="/wiki/N-Methyl-3-piperidyl_benzilate" title="N-Methyl-3-piperidyl benzilate">JB-336</a></li> <li><a href="/wiki/CS-27349" title="CS-27349">CS-27349</a></li> <li><a href="/wiki/CAR-226,086" title="CAR-226,086">CAR-226,086</a></li> <li><a href="/wiki/CAR-301,060" title="CAR-301,060">CAR-301,060</a></li> <li><a href="/wiki/CAR-302,196" title="CAR-302,196">CAR-302,196</a></li> <li><a href="/wiki/CAR-302,282" title="CAR-302,282">CAR-302,282</a></li> <li><a href="/wiki/CAR-302,668" title="CAR-302,668">CAR-302,668</a></li> <li><a href="/wiki/Benperidol" title="Benperidol">Benperidol</a></li> <li><a href="/wiki/Desflurane" title="Desflurane">Desflurane</a></li> <li><a href="/wiki/Enflurane" title="Enflurane">Enflurane</a></li> <li><a href="/wiki/Bufotenin" title="Bufotenin">Bufotenin</a></li> <li><a href="/wiki/Isoflurane" title="Isoflurane">Isoflurane</a></li> <li><a href="/wiki/Halothane" title="Halothane">Halothane</a></li> <li><a href="/wiki/Sevoflurane" title="Sevoflurane">Sevoflurane</a></li> <li><a href="/wiki/Pentazocine" title="Pentazocine">Pentazocine</a></li> <li><a href="/wiki/Procarbazine" title="Procarbazine">Procarbazine</a></li> <li><a href="/wiki/Fluphenazine" title="Fluphenazine">Fluphenazine</a></li> <li><a href="/wiki/Chlorpromazine" title="Chlorpromazine">Chlorpromazine</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Tear_gas" title="Tear gas">Lachrymatory agents</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Xylyl_bromide" title="Xylyl bromide">Xylyl bromide</a></li> <li><a href="/wiki/Pepper_spray" title="Pepper spray">Pepper spray</a> (OC)</li> <li><a href="/wiki/Mace_(spray)" title="Mace (spray)">Mace (spray)</a></li> <li><a href="/wiki/Phenacyl_chloride" title="Phenacyl chloride">CN</a></li> <li><a href="/wiki/CS_gas" title="CS gas">CS</a></li> <li><a href="/wiki/CR_gas" title="CR gas">CR</a></li> <li><a href="/wiki/CNS_(chemical_weapon)" title="CNS (chemical weapon)">CNS</a></li> <li><a href="/wiki/Benzyl_chloride" title="Benzyl chloride">Benzyl chloride</a></li> <li><a href="/wiki/Benzyl_bromide" title="Benzyl bromide">Benzyl bromide</a></li> <li><a href="/wiki/Benzyl_iodide" title="Benzyl iodide">Benzyl iodide</a></li> <li><a href="/wiki/Bromobenzyl_cyanide" title="Bromobenzyl cyanide">Bromobenzyl cyanide</a></li> <li><a href="/wiki/Thiophosgene" title="Thiophosgene">Thiophosgene</a></li> <li><a href="/wiki/Chloroacetone" title="Chloroacetone">Chloroacetone</a></li> <li><a href="/wiki/Bromoacetone" title="Bromoacetone">Bromoacetone</a></li> <li><a href="/wiki/Bromomethyl_ethyl_ketone" title="Bromomethyl ethyl ketone">Bromomethyl ethyl ketone</a></li> <li><a href="/wiki/Acrolein" title="Acrolein">Acrolein</a></li> <li><a href="/wiki/Phenacyl_bromide" title="Phenacyl bromide">Phenacyl bromide</a></li> <li><a href="/wiki/Chloroacetophenone_oxime" title="Chloroacetophenone oxime">Chloroacetophenone oxime</a></li> <li><a href="/wiki/Ethyl_bromoacetate" title="Ethyl bromoacetate">Ethyl bromoacetate</a></li> <li><a href="/wiki/Ethyl_iodoacetate" title="Ethyl iodoacetate">Ethyl iodoacetate</a></li> <li><a href="/wiki/Iodoacetone" title="Iodoacetone">Iodoacetone</a></li> <li><a href="/wiki/Allyl_isothiocyanate" title="Allyl isothiocyanate">Allyl isothiocyanate</a></li> <li><a href="/wiki/Hexamethylene_diisocyanate" title="Hexamethylene diisocyanate">Hexamethylene diisocyanate</a></li> <li><a href="/wiki/Crotonaldehyde" title="Crotonaldehyde">Crotonaldehyde</a></li> <li><a href="/wiki/DRC-5593" title="DRC-5593">DRC-5593</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Malodorant" title="Malodorant">Malodorant</a> agents</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Thioacetone" title="Thioacetone">Thioacetone</a></li> <li><a href="/wiki/Allicin" title="Allicin">Allicin</a></li> <li><a href="/wiki/Skatole" title="Skatole">Skatole</a></li> <li><a href="/wiki/Cadaverine" title="Cadaverine">Cadaverine</a></li> <li><a href="/wiki/Putrescine" title="Putrescine">Putrescine</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Cornea-clouding agents</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Lewisite" title="Lewisite">Lewisite</a></li> <li><a href="/wiki/Phosgene_oxime" title="Phosgene oxime">CX</a></li> <li><a href="/wiki/KB-16" title="KB-16">KB-16</a></li> <li><a href="/wiki/Methyl_cyanoacrylate" title="Methyl cyanoacrylate">Methyl cyanoacrylate</a></li> <li><a href="/wiki/N-Methylmorpholine" title="N-Methylmorpholine">N-Methylmorpholine</a></li> <li><a href="/wiki/Allyl_alcohol" title="Allyl alcohol">Allyl alcohol</a></li> <li><a href="/wiki/Osmium_tetroxide" title="Osmium tetroxide">Osmium tetroxide</a></li> <li><a href="/wiki/Acrolein" title="Acrolein">Acrolein</a></li> <li><a href="/wiki/Cacodyl_cyanide" title="Cacodyl cyanide">Cacodyl cyanide</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Biological toxins</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Abrin" title="Abrin">Abrin</a></li> <li><a href="/wiki/Aconitine" title="Aconitine">Aconitine</a></li> <li><a href="/wiki/Cyclopiazonic_acid" title="Cyclopiazonic acid">Cyclopiazonic acid</a></li> <li><a href="/wiki/Histrionicotoxins" title="Histrionicotoxins">Histrionicotoxins</a></li> <li><a href="/wiki/Aflatoxins" class="mw-redirect" title="Aflatoxins">Aflatoxins</a></li> <li><a href="/wiki/Anatoxin-a" title="Anatoxin-a">Anatoxin-a</a></li> <li><a href="/wiki/Batrachotoxin" title="Batrachotoxin">Batrachotoxin</a></li> <li><a href="/wiki/Botulinum_toxin" title="Botulinum toxin">Botulinum toxin</a></li> <li><a href="/wiki/Brevetoxin" title="Brevetoxin">Brevetoxin</a></li> <li><a href="/wiki/Ciguatoxin" title="Ciguatoxin">Ciguatoxin</a></li> <li><a href="/wiki/Domoic_acid" title="Domoic acid">Domoic acid</a></li> <li><a href="/wiki/Enterotoxin_type_B" title="Enterotoxin type B">Enterotoxin type B</a></li> <li><a href="/wiki/Grayanotoxin" title="Grayanotoxin">Grayanotoxin</a></li> <li><a href="/wiki/Guanitoxin" title="Guanitoxin">Guanitoxin</a></li> <li><a href="/wiki/Maitotoxin" title="Maitotoxin">Maitotoxin</a></li> <li><a href="/wiki/Modeccin" title="Modeccin">Modeccin</a></li> <li><a href="/wiki/Palytoxin" title="Palytoxin">Palytoxin</a></li> <li><a href="/wiki/Ricin" title="Ricin">Ricin</a></li> <li><a href="/wiki/Saxitoxin" title="Saxitoxin">Saxitoxin</a></li> <li><a href="/wiki/Shiga_toxin" title="Shiga toxin">Shiga toxin</a></li> <li><a href="/wiki/T-2_mycotoxin" title="T-2 mycotoxin">T-2 mycotoxin</a></li> <li><a href="/wiki/Tetanospasmin" class="mw-redirect" title="Tetanospasmin">Tetanospasmin</a></li> <li><a href="/wiki/Tetrodotoxin" title="Tetrodotoxin">Tetrodotoxin</a></li> <li><a href="/wiki/Volkensin" title="Volkensin">Volkensin</a></li> <li><a href="/wiki/Veratridine" title="Veratridine">Veratridine</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Other</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Methyl_fluoroacetate" title="Methyl fluoroacetate">Methyl fluoroacetate</a></li> <li><a href="/wiki/Napalm" title="Napalm">Napalm</a> (variants and mixtures)</li> <li><a href="/wiki/Fluoroethyl_fluoroacetate" title="Fluoroethyl fluoroacetate">Fluoroethyl fluoroacetate</a></li> <li><a href="/wiki/Depleted_uranium" title="Depleted uranium">Depleted uranium</a> <ul><li>post-combustion <a href="/wiki/Uranium_oxide" title="Uranium oxide">uranium oxides</a></li></ul></li> <li><a href="/wiki/Plutonium" title="Plutonium">Plutonium</a> and <a href="/wiki/Plutonium_compounds" title="Plutonium compounds">its compounds</a></li> <li><a href="/wiki/Polonium" title="Polonium">Polonium</a></li> <li><a href="/wiki/White_phosphorus_munitions" class="mw-redirect" title="White phosphorus munitions">White phosphorus</a></li></ul> </div></td></tr><tr><td class="navbox-abovebelow" colspan="2"><div> <ul><li><a href="/wiki/List_of_chemical_warfare_agents" title="List of chemical warfare agents">List of chemical warfare agents</a></li> <li><a href="/wiki/CB_military_symbol" title="CB military symbol">CB military symbol</a></li></ul> </div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"></div><div role="navigation" class="navbox" aria-labelledby="E_numbers13" style="padding:3px"><table class="nowraplinks mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239400231"><div class="navbar plainlinks hlist navbar-mini"><ul><li class="nv-view"><a href="/wiki/Template:E_number_infobox_920-929" title="Template:E number infobox 920-929"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:E_number_infobox_920-929" title="Template talk:E number infobox 920-929"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:E_number_infobox_920-929" title="Special:EditPage/Template:E number infobox 920-929"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="E_numbers13" style="font-size:114%;margin:0 4em"><a href="/wiki/E_number" title="E number">E numbers</a></div></th></tr><tr><td colspan="2" class="navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Food_coloring" title="Food coloring">Colours</a> (E100–199)</li> <li><a href="/wiki/Preservative" title="Preservative">Preservatives</a> (E200–299)</li> <li><a href="/wiki/Antioxidant" title="Antioxidant">Antioxidants</a> & <a href="/wiki/Acidity_regulator" title="Acidity regulator">acidity regulators</a> (E300–399)</li> <li><a href="/wiki/Thickening_agent" title="Thickening agent">Thickeners</a>, <a href="/wiki/Food_additive#Categories" title="Food additive">stabilisers</a> & <a href="/wiki/Emulsifier" class="mw-redirect" title="Emulsifier">emulsifiers</a> (E400–499)</li> <li><a href="/wiki/PH" title="PH">pH</a> <a href="/wiki/Acidity_regulator" title="Acidity regulator">regulators</a> & <a href="/wiki/Anticaking_agent" title="Anticaking agent">anticaking agents</a> (E500–599)</li> <li><a href="/wiki/Flavoring" title="Flavoring">Flavour enhancers</a> (E600–699)</li> <li>Miscellaneous (E900–999)</li> <li>Additional chemicals (E1100–1599)</li></ul> <hr /> <ul><li><a href="/wiki/Wax" title="Wax">Waxes</a> (E900–909)</li> <li><a href="/wiki/Glazing_agent" title="Glazing agent">Synthetic glazes</a> (E910–919)</li> <li><a href="/wiki/Flour_treatment_agent" class="mw-redirect" title="Flour treatment agent">Improving agents</a> (E920–929)</li> <li><a href="/wiki/Packaging_gas" title="Packaging gas">Packaging gases</a> (E930–949)</li> <li><a href="/wiki/Sugar_substitute" title="Sugar substitute">Sweeteners</a> (E950–969)</li> <li><a href="/wiki/Foaming_agent" title="Foaming agent">Foaming agents</a> (E990–999)</li></ul> <hr /> <ul><li><a href="/wiki/Cysteine" title="Cysteine">L-cysteine</a> (E920)</li> <li><a href="/wiki/Cystine" title="Cystine">L-cystine</a> (E921)</li> <li><a href="/wiki/Potassium_persulfate" title="Potassium persulfate">Potassium persulfate</a> (E922)</li> <li><a href="/wiki/Ammonium_persulfate" title="Ammonium persulfate">Ammonium persulfate</a> (E923)</li> <li><a href="/wiki/Potassium_bromate" title="Potassium bromate">Potassium bromate</a> (E924)</li> <li><a class="mw-selflink selflink">Chlorine</a> (E925)</li> <li><a href="/wiki/Chlorine_dioxide" title="Chlorine dioxide">Chlorine dioxide</a> (E926)</li> <li><a href="/wiki/Azodicarbonamide" title="Azodicarbonamide">Azodicarbonamide</a> (E927)</li> <li><a href="/wiki/Urea" title="Urea">Carbamide</a> (E927b)</li> <li><a href="/wiki/Benzoyl_peroxide" title="Benzoyl peroxide">Benzoyl peroxide</a> (E928)</li></ul> </div></td></tr></tbody></table></div> <style data-mw-deduplicate="TemplateStyles:r1130092004">.mw-parser-output .portal-bar{font-size:88%;font-weight:bold;display:flex;justify-content:center;align-items:baseline}.mw-parser-output .portal-bar-bordered{padding:0 2em;background-color:#fdfdfd;border:1px solid #a2a9b1;clear:both;margin:1em auto 0}.mw-parser-output .portal-bar-related{font-size:100%;justify-content:flex-start}.mw-parser-output .portal-bar-unbordered{padding:0 1.7em;margin-left:0}.mw-parser-output .portal-bar-header{margin:0 1em 0 0.5em;flex:0 0 auto;min-height:24px}.mw-parser-output .portal-bar-content{display:flex;flex-flow:row wrap;flex:0 1 auto;padding:0.15em 0;column-gap:1em;align-items:baseline;margin:0;list-style:none}.mw-parser-output .portal-bar-content-related{margin:0;list-style:none}.mw-parser-output .portal-bar-item{display:inline-block;margin:0.15em 0.2em;min-height:24px;line-height:24px}@media screen and (max-width:768px){.mw-parser-output .portal-bar{font-size:88%;font-weight:bold;display:flex;flex-flow:column wrap;align-items:baseline}.mw-parser-output .portal-bar-header{text-align:center;flex:0;padding-left:0.5em;margin:0 auto}.mw-parser-output .portal-bar-related{font-size:100%;align-items:flex-start}.mw-parser-output .portal-bar-content{display:flex;flex-flow:row wrap;align-items:center;flex:0;column-gap:1em;border-top:1px solid #a2a9b1;margin:0 auto;list-style:none}.mw-parser-output .portal-bar-content-related{border-top:none;margin:0;list-style:none}}.mw-parser-output .navbox+link+.portal-bar,.mw-parser-output .navbox+style+.portal-bar,.mw-parser-output .navbox+link+.portal-bar-bordered,.mw-parser-output .navbox+style+.portal-bar-bordered,.mw-parser-output .sister-bar+link+.portal-bar,.mw-parser-output .sister-bar+style+.portal-bar,.mw-parser-output .portal-bar+.navbox-styles+.navbox,.mw-parser-output .portal-bar+.navbox-styles+.sister-bar{margin-top:-1px}</style><div class="portal-bar noprint metadata noviewer portal-bar-bordered" role="navigation" aria-label="Portals"><a href="/wiki/Wikipedia:Contents/Portals" title="Wikipedia:Contents/Portals">Portals</a>:<ul class="portal-bar-content"><li class="portal-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/19px-Papapishu-Lab-icon-6.svg.png" decoding="async" width="19" height="19" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/29px-Papapishu-Lab-icon-6.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/38px-Papapishu-Lab-icon-6.svg.png 2x" data-file-width="512" data-file-height="512" /> <a href="/wiki/Portal:Chemistry" title="Portal:Chemistry">Chemistry</a></li><li class="portal-bar-item"><a href="/wiki/File:Aegopodium_podagraria1_ies.jpg" class="mw-file-description"><img alt="icon" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/bf/Aegopodium_podagraria1_ies.jpg/21px-Aegopodium_podagraria1_ies.jpg" decoding="async" width="21" height="18" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/bf/Aegopodium_podagraria1_ies.jpg/32px-Aegopodium_podagraria1_ies.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/bf/Aegopodium_podagraria1_ies.jpg/42px-Aegopodium_podagraria1_ies.jpg 2x" data-file-width="800" data-file-height="700" /></a> <a href="/wiki/Portal:Environment" title="Portal:Environment">Environment</a></li><li class="portal-bar-item"><img alt="icon" src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/WHO_Rod.svg/8px-WHO_Rod.svg.png" decoding="async" width="8" height="19" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/WHO_Rod.svg/12px-WHO_Rod.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d6/WHO_Rod.svg/16px-WHO_Rod.svg.png 2x" data-file-width="107" data-file-height="250" /> <a href="/wiki/Portal:Medicine" title="Portal:Medicine">Medicine</a></li></ul></div><style data-mw-deduplicate="TemplateStyles:r1236088147">.mw-parser-output .sister-bar{display:flex;justify-content:center;align-items:baseline;font-size:88%;background-color:#fdfdfd;border:1px solid #a2a9b1;clear:both;margin:1em 0 0;padding:0 2em}.mw-parser-output .sister-bar-header{margin:0 1em 0 0.5em;padding:0.2em 0;flex:0 0 auto;min-height:24px;line-height:22px}.mw-parser-output .sister-bar-content{display:flex;flex-flow:row wrap;flex:0 1 auto;align-items:baseline;padding:0.2em 0;column-gap:1em;margin:0;list-style:none}.mw-parser-output .sister-bar-item{display:flex;align-items:baseline;margin:0.15em 0;min-height:24px;text-align:left}.mw-parser-output .sister-bar-logo{width:22px;line-height:22px;margin:0 0.2em;text-align:right}.mw-parser-output .sister-bar-link{margin:0 0.2em;text-align:left}@media screen and (max-width:960px){.mw-parser-output .sister-bar{flex-flow:column wrap;margin:1em auto 0}.mw-parser-output .sister-bar-header{flex:0 1}.mw-parser-output .sister-bar-content{flex:1;border-top:1px solid #a2a9b1;margin:0;list-style:none}.mw-parser-output .sister-bar-item{flex:0 0 20em;min-width:20em}}.mw-parser-output .navbox+link+.sister-bar,.mw-parser-output .navbox+style+.sister-bar,.mw-parser-output .portal-bar+link+.sister-bar,.mw-parser-output .portal-bar+style+.sister-bar,.mw-parser-output .sister-bar+.navbox-styles+.navbox,.mw-parser-output .sister-bar+.navbox-styles+.portal-bar{margin-top:-1px}@media print{body.ns-0 .mw-parser-output .sister-bar{display:none!important}}</style><div class="noprint metadata sister-bar" role="navigation" aria-label="sister-projects"><div class="sister-bar-header">Chlorine at Wikipedia's <a href="/wiki/Wikipedia:Wikimedia_sister_projects" title="Wikipedia:Wikimedia sister projects">sister projects</a>:</div><ul class="sister-bar-content"><li class="sister-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/0/06/Wiktionary-logo-v2.svg/19px-Wiktionary-logo-v2.svg.png" decoding="async" width="19" height="19" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/0/06/Wiktionary-logo-v2.svg/29px-Wiktionary-logo-v2.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/0/06/Wiktionary-logo-v2.svg/38px-Wiktionary-logo-v2.svg.png 2x" data-file-width="391" data-file-height="391" /><a href="https://en.wiktionary.org/wiki/chlorine" class="extiw" title="wikt:chlorine">Definitions</a> from Wiktionary</li><li class="sister-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/14px-Commons-logo.svg.png" decoding="async" width="14" height="19" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/21px-Commons-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/28px-Commons-logo.svg.png 2x" data-file-width="1024" data-file-height="1376" /><a href="https://commons.wikimedia.org/wiki/Chlorine" class="extiw" title="c:Chlorine">Media</a> from Commons</li><li class="sister-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/2/24/Wikinews-logo.svg/21px-Wikinews-logo.svg.png" decoding="async" width="21" height="11" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/24/Wikinews-logo.svg/32px-Wikinews-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/24/Wikinews-logo.svg/42px-Wikinews-logo.svg.png 2x" data-file-width="759" data-file-height="415" /><a href="https://en.wikinews.org/wiki/Chlorine_spill_in_China%27s_Jiangsu_province_kills_28,_injures_hundreds" class="extiw" title="n:Chlorine spill in China's Jiangsu province kills 28, injures hundreds">News</a> from Wikinews</li><li class="sister-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/18px-Wikisource-logo.svg.png" decoding="async" width="18" height="19" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/28px-Wikisource-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/36px-Wikisource-logo.svg.png 2x" data-file-width="410" data-file-height="430" /><a href="https://en.wikisource.org/wiki/1911_Encyclop%C3%A6dia_Britannica/Chlorine" class="extiw" title="s:1911 Encyclopædia Britannica/Chlorine">Texts</a> from Wikisource</li><li class="sister-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikibooks-logo.svg/19px-Wikibooks-logo.svg.png" decoding="async" width="19" height="19" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikibooks-logo.svg/29px-Wikibooks-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikibooks-logo.svg/38px-Wikibooks-logo.svg.png 2x" data-file-width="300" data-file-height="300" /><a href="https://en.wikibooks.org/wiki/Wikijunior:The_Elements/Chlorine" class="extiw" title="b:Wikijunior:The Elements/Chlorine">Textbooks</a> from Wikibooks</li><li class="sister-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0b/Wikiversity_logo_2017.svg/21px-Wikiversity_logo_2017.svg.png" decoding="async" width="21" height="17" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/0b/Wikiversity_logo_2017.svg/32px-Wikiversity_logo_2017.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/0b/Wikiversity_logo_2017.svg/42px-Wikiversity_logo_2017.svg.png 2x" data-file-width="626" data-file-height="512" /><a href="https://en.wikiversity.org/wiki/Chemicals/Chlorines" class="extiw" title="v:Chemicals/Chlorines">Resources</a> from Wikiversity</li><li class="sister-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/ff/Wikidata-logo.svg/21px-Wikidata-logo.svg.png" decoding="async" width="21" height="12" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/ff/Wikidata-logo.svg/32px-Wikidata-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/ff/Wikidata-logo.svg/42px-Wikidata-logo.svg.png 2x" data-file-width="1050" data-file-height="590" /><a href="https://www.wikidata.org/wiki/Q688" class="extiw" title="d:Q688">Data</a> from Wikidata</li></ul></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235"><style data-mw-deduplicate="TemplateStyles:r1038841319">.mw-parser-output .tooltip-dotted{border-bottom:1px dotted;cursor:help}</style><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1038841319"></div><div role="navigation" class="navbox authority-control" aria-labelledby="Authority_control_databases_frameless&#124;text-top&#124;10px&#124;alt=Edit_this_at_Wikidata&#124;link=https&#58;//www.wikidata.org/wiki/Q688#identifiers&#124;class=noprint&#124;Edit_this_at_Wikidata1493" style="padding:3px"><table class="nowraplinks hlist mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="col" class="navbox-title" colspan="2"><div id="Authority_control_databases_frameless&#124;text-top&#124;10px&#124;alt=Edit_this_at_Wikidata&#124;link=https&#58;//www.wikidata.org/wiki/Q688#identifiers&#124;class=noprint&#124;Edit_this_at_Wikidata1493" style="font-size:114%;margin:0 4em"><a href="/wiki/Help:Authority_control" title="Help:Authority control">Authority control databases</a> <a href="https://www.wikidata.org/wiki/Q688#identifiers" title="Edit this at Wikidata"><img alt="Edit this at Wikidata" src="//upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/10px-OOjs_UI_icon_edit-ltr-progressive.svg.png" decoding="async" width="10" height="10" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/15px-OOjs_UI_icon_edit-ltr-progressive.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/20px-OOjs_UI_icon_edit-ltr-progressive.svg.png 2x" data-file-width="20" data-file-height="20" /></a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%">International</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"><ul><li><a rel="nofollow" class="external text" href="http://id.worldcat.org/fast/858103/">FAST</a></li></ul></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">National</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"><ul><li><a rel="nofollow" class="external text" href="https://d-nb.info/gnd/4147748-0">Germany</a></li><li><a rel="nofollow" class="external text" href="https://id.loc.gov/authorities/sh85024541">United States</a></li><li><a rel="nofollow" class="external text" href="https://catalogue.bnf.fr/ark:/12148/cb119811094">France</a></li><li><a rel="nofollow" class="external text" href="https://data.bnf.fr/ark:/12148/cb119811094">BnF data</a></li><li><a rel="nofollow" class="external text" href="https://id.ndl.go.jp/auth/ndlna/00562008">Japan</a></li><li><a rel="nofollow" class="external text" href="https://aleph.nkp.cz/F/?func=find-c&local_base=aut&ccl_term=ica=ph163876&CON_LNG=ENG">Czech Republic</a></li><li><a rel="nofollow" class="external text" href="http://catalogo.bne.es/uhtbin/authoritybrowse.cgi?action=display&authority_id=XX533160">Spain</a></li><li><a rel="nofollow" class="external text" href="https://www.nli.org.il/en/authorities/987007285618505171">Israel</a></li></ul></div></td></tr></tbody></table></div>    </div><noscript><img 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