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class="vector-toc-list"> </ul> </li> <li id="toc-Hydrogen_iodide" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Hydrogen_iodide"> <div class="vector-toc-text"> 3.2 Hydrogen iodide </div> </a> <ul id="toc-Hydrogen_iodide-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Other_binary_iodine_compounds" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Other_binary_iodine_compounds"> <div class="vector-toc-text"> 3.3 Other binary iodine compounds </div> </a> <ul id="toc-Other_binary_iodine_compounds-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Iodine_halides" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Iodine_halides"> <div class="vector-toc-text"> 3.4 Iodine halides </div> </a> <ul id="toc-Iodine_halides-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Iodine_oxides_and_oxoacids" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Iodine_oxides_and_oxoacids"> <div class="vector-toc-text"> 3.5 Iodine oxides and oxoacids </div> </a> <ul id="toc-Iodine_oxides_and_oxoacids-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Polyiodine_compounds" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Polyiodine_compounds"> <div class="vector-toc-text"> 3.6 Polyiodine compounds </div> </a> <ul id="toc-Polyiodine_compounds-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Organoiodine_compounds" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Organoiodine_compounds"> <div class="vector-toc-text"> 3.7 Organoiodine compounds </div> </a> <ul id="toc-Organoiodine_compounds-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Occurrence_and_production" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Occurrence_and_production"> <div class="vector-toc-text"> 4 Occurrence and production </div> </a> <ul id="toc-Occurrence_and_production-sublist" class="vector-toc-list"> </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"> 5 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-X-ray_imaging" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#X-ray_imaging"> <div class="vector-toc-text"> 5.1 X-ray imaging </div> </a> <ul id="toc-X-ray_imaging-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Biocide" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Biocide"> <div class="vector-toc-text"> 5.2 Biocide </div> </a> <ul id="toc-Biocide-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Optical_polarizing_films" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Optical_polarizing_films"> <div class="vector-toc-text"> 5.3 Optical polarizing films </div> </a> <ul id="toc-Optical_polarizing_films-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Co-catalyst" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Co-catalyst"> <div class="vector-toc-text"> 5.4 Co-catalyst </div> </a> <ul id="toc-Co-catalyst-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Nutrition" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Nutrition"> <div class="vector-toc-text"> 5.5 Nutrition </div> </a> <ul id="toc-Nutrition-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Others" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Others"> <div class="vector-toc-text"> 5.6 Others </div> </a> <ul id="toc-Others-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Spectroscopy" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Spectroscopy"> <div class="vector-toc-text"> 6 Spectroscopy </div> </a> <ul id="toc-Spectroscopy-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Chemical_analysis" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Chemical_analysis"> <div class="vector-toc-text"> 7 Chemical analysis </div> </a> <ul id="toc-Chemical_analysis-sublist" class="vector-toc-list"> </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"> 8 Biological role </div> </a> <button aria-controls="toc-Biological_role-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Biological role subsection </button> <ul id="toc-Biological_role-sublist" class="vector-toc-list"> <li id="toc-Dietary_recommendations_and_intake" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Dietary_recommendations_and_intake"> <div class="vector-toc-text"> 8.1 Dietary recommendations and intake </div> </a> <ul id="toc-Dietary_recommendations_and_intake-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Deficiency" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Deficiency"> <div class="vector-toc-text"> 8.2 Deficiency </div> </a> <ul id="toc-Deficiency-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Precautions" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Precautions"> <div class="vector-toc-text"> 9 Precautions </div> </a> <button aria-controls="toc-Precautions-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Precautions subsection </button> <ul id="toc-Precautions-sublist" class="vector-toc-list"> <li id="toc-Toxicity" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Toxicity"> <div class="vector-toc-text"> 9.1 Toxicity </div> </a> <ul id="toc-Toxicity-sublist" class="vector-toc-list"> <li id="toc-Occupational_exposure" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Occupational_exposure"> <div class="vector-toc-text"> 9.1.1 Occupational exposure </div> </a> <ul id="toc-Occupational_exposure-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Allergic_reactions" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Allergic_reactions"> <div class="vector-toc-text"> 9.1.2 Allergic reactions </div> </a> <ul id="toc-Allergic_reactions-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-US_DEA_List_I_status" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#US_DEA_List_I_status"> <div class="vector-toc-text"> 9.2 US DEA List I status </div> </a> <ul id="toc-US_DEA_List_I_status-sublist" class="vector-toc-list"> </ul> </li> </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> <ul id="toc-References-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Bibliography" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Bibliography"> <div class="vector-toc-text"> 12 Bibliography </div> </a> <ul id="toc-Bibliography-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" > <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">Iodine</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 153 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-153" aria-hidden="true" > 153 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/Jodium" title="Jodium – Afrikaans" lang="af" hreflang="af" data-title="Jodium" 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%A0%E1%8B%AE%E1%8B%B2%E1%8A%95" title="አዮዲን – Amharic" lang="am" hreflang="am" data-title="አዮዲን" 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%86%E0%A4%AF%E0%A5%8B%E0%A4%A1%E0%A5%80%E0%A4%A8" title="आयोडीन – Angika" lang="anp" hreflang="anp" data-title="आयोडीन" data-language-autonym="अंगिका" data-language-local-name="Angika" class="interlanguage-link-target">अंगिका</a></li><li class="interlanguage-link interwiki-ar mw-list-item"><a href="https://ar.wikipedia.org/wiki/%D9%8A%D9%88%D8%AF" title="يود – Arabic" lang="ar" hreflang="ar" data-title="يود" 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/Yodo" title="Yodo – Aragonese" lang="an" hreflang="an" data-title="Yodo" data-language-autonym="Aragonés" data-language-local-name="Aragonese" class="interlanguage-link-target">Aragonés</a></li><li class="interlanguage-link interwiki-roa-rup mw-list-item"><a href="https://roa-rup.wikipedia.org/wiki/Iodu" title="Iodu – Aromanian" lang="rup" hreflang="rup" data-title="Iodu" 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/Yodu" title="Yodu – Asturian" lang="ast" hreflang="ast" data-title="Yodu" 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/Yod" title="Yod – Azerbaijani" lang="az" hreflang="az" data-title="Yod" 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/%DB%8C%D9%88%D8%AF" title="یود – South Azerbaijani" lang="azb" hreflang="azb" data-title="یود" 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/Yodium" title="Yodium – Balinese" lang="ban" hreflang="ban" data-title="Yodium" 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%86%E0%A6%AF%E0%A6%BC%E0%A7%8B%E0%A6%A1%E0%A6%BF%E0%A6%A8" title="আয়োডিন – Bangla" lang="bn" hreflang="bn" data-title="আয়োডিন" 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/Ak-s%C3%B2%CD%98" title="Ak-sò͘ – Minnan" lang="nan" hreflang="nan" data-title="Ak-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%98%D0%BE%D0%B4" title="Иод – Bashkir" lang="ba" hreflang="ba" data-title="Иод" 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%81%D0%B4" title="Ёд – Belarusian" lang="be" hreflang="be" data-title="Ёд" 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%81%D0%B4" title="Ёд – Belarusian (Taraškievica orthography)" lang="be-tarask" hreflang="be-tarask" data-title="Ёд" 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%86%E0%A4%AF%E0%A5%8B%E0%A4%A1%E0%A5%80%E0%A4%A8" title="आयोडीन – Bhojpuri" lang="bh" hreflang="bh" data-title="आयोडीन" 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/Iyodo" title="Iyodo – Central Bikol" lang="bcl" hreflang="bcl" data-title="Iyodo" data-language-autonym="Bikol Central" data-language-local-name="Central Bikol" class="interlanguage-link-target">Bikol Central</a></li><li class="interlanguage-link interwiki-bi mw-list-item"><a href="https://bi.wikipedia.org/wiki/Aiodin" title="Aiodin – Bislama" lang="bi" hreflang="bi" data-title="Aiodin" data-language-autonym="Bislama" data-language-local-name="Bislama" class="interlanguage-link-target">Bislama</a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%99%D0%BE%D0%B4" title="Йод – Bulgarian" lang="bg" hreflang="bg" data-title="Йод" 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%A3%E0%BE%A6%E0%BC%8B%E0%BD%9A%E0%BE%AD%E0%BC%8D" title="ལྦ་ཚྭ། – Tibetan" lang="bo" hreflang="bo" data-title="ལྦ་ཚྭ།" 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/Jod" title="Jod – Bosnian" lang="bs" hreflang="bs" data-title="Jod" 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/Iod" title="Iod – Breton" lang="br" hreflang="br" data-title="Iod" 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/Iode" title="Iode – Catalan" lang="ca" hreflang="ca" data-title="Iode" 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%98%D0%BE%D0%B4" title="Иод – Chuvash" lang="cv" hreflang="cv" data-title="Иод" 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/Yodo" title="Yodo – Cebuano" lang="ceb" hreflang="ceb" data-title="Yodo" 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/Jod" title="Jod – Czech" lang="cs" hreflang="cs" data-title="Jod" 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/Iodiu" title="Iodiu – Corsican" lang="co" hreflang="co" data-title="Iodiu" 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/%C3%8Fodin" title="Ïodin – Welsh" lang="cy" hreflang="cy" data-title="Ïodin" 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/Jod" title="Jod – Danish" lang="da" hreflang="da" data-title="Jod" 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%8A%D9%88%D8%AF" title="يود – Moroccan Arabic" lang="ary" hreflang="ary" data-title="يود" data-language-autonym="الدارجة" data-language-local-name="Moroccan Arabic" class="interlanguage-link-target">الدارجة</a></li><li class="interlanguage-link interwiki-de mw-list-item"><a href="https://de.wikipedia.org/wiki/Iod" title="Iod – German" lang="de" hreflang="de" data-title="Iod" 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%87%DE%A6%DE%94%DE%AE%DE%91%DE%A8%DE%82%DE%B0" title="އަޔޮޑިން – Divehi" lang="dv" hreflang="dv" data-title="އަޔޮޑިން" 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/Jood" title="Jood – Estonian" lang="et" hreflang="et" data-title="Jood" 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%99%CF%8E%CE%B4%CE%B9%CE%BF" title="Ιώδιο – Greek" lang="el" hreflang="el" data-title="Ιώδιο" 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%98%D0%BE%D0%B4" title="Иод – Erzya" lang="myv" hreflang="myv" data-title="Иод" 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/Yodo" title="Yodo – Spanish" lang="es" hreflang="es" data-title="Yodo" 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/Jodo" title="Jodo – Esperanto" lang="eo" hreflang="eo" data-title="Jodo" data-language-autonym="Esperanto" data-language-local-name="Esperanto" class="interlanguage-link-target">Esperanto</a></li><li class="interlanguage-link interwiki-eu mw-list-item"><a href="https://eu.wikipedia.org/wiki/Iodo" title="Iodo – Basque" lang="eu" hreflang="eu" data-title="Iodo" 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/%DB%8C%D8%AF" title="ید – Persian" lang="fa" hreflang="fa" data-title="ید" 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/Iodine" title="Iodine – Fiji Hindi" lang="hif" hreflang="hif" data-title="Iodine" 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/Jod" title="Jod – Faroese" lang="fo" hreflang="fo" data-title="Jod" 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/Iode" title="Iode – French" lang="fr" hreflang="fr" data-title="Iode" 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/Jodi" title="Jodi – Friulian" lang="fur" hreflang="fur" data-title="Jodi" 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/Iaid%C3%ADn" title="Iaidín – Irish" lang="ga" hreflang="ga" data-title="Iaidín" 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/Eeadeen" title="Eeadeen – Manx" lang="gv" hreflang="gv" data-title="Eeadeen" 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/Aidhodain" title="Aidhodain – Scottish Gaelic" lang="gd" hreflang="gd" data-title="Aidhodain" 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/Iodo" title="Iodo – Galician" lang="gl" hreflang="gl" data-title="Iodo" 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/%E7%A2%98" title="碘 – Gan" lang="gan" hreflang="gan" data-title="碘" 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%86%E0%AA%AF%E0%AB%8B%E0%AA%A1%E0%AA%BF%E0%AA%A8" title="આયોડિન – Gujarati" lang="gu" hreflang="gu" data-title="આયોડિન" 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/Ti%C3%A9n" title="Tién – Hakka Chinese" lang="hak" hreflang="hak" data-title="Tién" 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%99%D0%BE%D0%B4" title="Йод – Kalmyk" lang="xal" hreflang="xal" data-title="Йод" 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%95%84%EC%9D%B4%EC%98%A4%EB%94%98" title="아이오딘 – Korean" lang="ko" hreflang="ko" data-title="아이오딘" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target">한국어</a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D5%85%D5%B8%D5%A4" title="Յոդ – Armenian" lang="hy" hreflang="hy" data-title="Յոդ" 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%86%E0%A4%AF%E0%A5%8B%E0%A4%A1%E0%A4%BF%E0%A4%A8" title="आयोडिन – Hindi" lang="hi" hreflang="hi" data-title="आयोडिन" 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/Jod" title="Jod – Croatian" lang="hr" hreflang="hr" data-title="Jod" 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/Iodo" title="Iodo – Ido" lang="io" hreflang="io" data-title="Iodo" 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/Iodin" title="Iodin – Indonesian" lang="id" hreflang="id" data-title="Iodin" 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/Iodo" title="Iodo – Interlingua" lang="ia" hreflang="ia" data-title="Iodo" 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%99%D0%BE%D0%B4" title="Йод – Ossetic" lang="os" hreflang="os" data-title="Йод" 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/Inkwithi" title="Inkwithi – Zulu" lang="zu" hreflang="zu" data-title="Inkwithi" 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/Jo%C3%B0" title="Joð – Icelandic" lang="is" hreflang="is" data-title="Joð" 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/Iodio" title="Iodio – Italian" lang="it" hreflang="it" data-title="Iodio" 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%99%D7%95%D7%93" title="יוד – Hebrew" lang="he" hreflang="he" data-title="יוד" 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/Yodium" title="Yodium – Javanese" lang="jv" hreflang="jv" data-title="Yodium" 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/%C6%96y%C9%94d%C9%A9" title="Ɩyɔdɩ – Kabiye" lang="kbp" hreflang="kbp" data-title="Ɩyɔdɩ" 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%85%E0%B2%AF%E0%B3%8A%E0%B2%A1%E0%B2%BF%E0%B2%A8%E0%B3%8D" title="ಅಯೊಡಿನ್ – Kannada" lang="kn" hreflang="kn" data-title="ಅಯೊಡಿನ್" 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%98%E1%83%9D%E1%83%93%E1%83%98" title="იოდი – Georgian" lang="ka" hreflang="ka" data-title="იოდი" data-language-autonym="ქართული" data-language-local-name="Georgian" class="interlanguage-link-target">ქართული</a></li><li class="interlanguage-link interwiki-ks mw-list-item"><a href="https://ks.wikipedia.org/wiki/%D8%A2%DB%8C%D9%88%DA%88%DB%8C%D9%86" title="آیوڈین – Kashmiri" lang="ks" hreflang="ks" data-title="آیوڈین" data-language-autonym="कॉशुर / کٲشُر" data-language-local-name="Kashmiri" class="interlanguage-link-target">कॉशुर / کٲشُر</a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%99%D0%BE%D0%B4" title="Йод – Kazakh" lang="kk" hreflang="kk" data-title="Йод" 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/Iodin" title="Iodin – Cornish" lang="kw" hreflang="kw" data-title="Iodin" 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/Iodini" title="Iodini – Swahili" lang="sw" hreflang="sw" data-title="Iodini" 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%99%D0%BE%D0%B4" title="Йод – Komi" lang="kv" hreflang="kv" data-title="Йод" 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/Y%C3%B2d" title="Yòd – Haitian Creole" lang="ht" hreflang="ht" data-title="Yòd" data-language-autonym="Kreyòl ayisyen" data-language-local-name="Haitian Creole" class="interlanguage-link-target">Kreyòl ayisyen</a></li><li class="interlanguage-link interwiki-ky mw-list-item"><a href="https://ky.wikipedia.org/wiki/%D0%98%D0%BE%D0%B4" title="Иод – Kyrgyz" lang="ky" hreflang="ky" data-title="Иод" 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%98%D0%BE%D0%B4" title="Иод – Western Mari" lang="mrj" hreflang="mrj" data-title="Иод" data-language-autonym="Кырык мары" data-language-local-name="Western Mari" class="interlanguage-link-target">Кырык мары</a></li><li class="interlanguage-link interwiki-lld mw-list-item"><a href="https://lld.wikipedia.org/wiki/Iodie" title="Iodie – Ladin" lang="lld" hreflang="lld" data-title="Iodie" data-language-autonym="Ladin" data-language-local-name="Ladin" class="interlanguage-link-target">Ladin</a></li><li class="interlanguage-link interwiki-lo mw-list-item"><a href="https://lo.wikipedia.org/wiki/%E0%BB%84%E0%BA%AD%E0%BB%82%E0%BA%AD%E0%BA%94%E0%BA%B4%E0%BA%99" title="ໄອໂອດິນ – Lao" lang="lo" hreflang="lo" data-title="ໄອໂອດິນ" data-language-autonym="ລາວ" data-language-local-name="Lao" class="interlanguage-link-target">ລາວ</a></li><li class="interlanguage-link interwiki-la mw-list-item"><a href="https://la.wikipedia.org/wiki/Iodum" title="Iodum – Latin" lang="la" hreflang="la" data-title="Iodum" 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/Jods_(elements)" title="Jods (elements) – Latvian" lang="lv" hreflang="lv" data-title="Jods (elements)" 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/Iod" title="Iod – Luxembourgish" lang="lb" hreflang="lb" data-title="Iod" 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/Jodas" title="Jodas – Lithuanian" lang="lt" hreflang="lt" data-title="Jodas" 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/Iodio" title="Iodio – Ligurian" lang="lij" hreflang="lij" data-title="Iodio" 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/Jodium" title="Jodium – Limburgish" lang="li" hreflang="li" data-title="Jodium" data-language-autonym="Limburgs" data-language-local-name="Limburgish" class="interlanguage-link-target">Limburgs</a></li><li class="interlanguage-link interwiki-olo mw-list-item"><a href="https://olo.wikipedia.org/wiki/Joudu" title="Joudu – Livvi-Karelian" lang="olo" hreflang="olo" data-title="Joudu" 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/zirkliru" title="zirkliru – Lojban" lang="jbo" hreflang="jbo" data-title="zirkliru" 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/Ayodiini_(Iodine)" title="Ayodiini (Iodine) – Ganda" lang="lg" hreflang="lg" data-title="Ayodiini (Iodine)" 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/Iodio" title="Iodio – Lombard" lang="lmo" hreflang="lmo" data-title="Iodio" 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/J%C3%B3d" title="Jód – Hungarian" lang="hu" hreflang="hu" data-title="Jód" 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%88%D0%BE%D0%B4" title="Јод – Macedonian" lang="mk" hreflang="mk" data-title="Јод" 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%85%E0%B4%AF%E0%B5%8B%E0%B4%A1%E0%B4%BF%E0%B5%BB" title="അയോഡിൻ – Malayalam" lang="ml" hreflang="ml" data-title="അയോഡിൻ" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target">മലയാളം</a></li><li class="interlanguage-link interwiki-mr mw-list-item"><a href="https://mr.wikipedia.org/wiki/%E0%A4%86%E0%A4%AF%E0%A5%8B%E0%A4%A1%E0%A5%80%E0%A4%A8" title="आयोडीन – Marathi" lang="mr" hreflang="mr" data-title="आयोडीन" 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%8A%D9%88%D8%AF" title="يود – Egyptian Arabic" lang="arz" hreflang="arz" data-title="يود" 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/Iodin" title="Iodin – Malay" lang="ms" hreflang="ms" data-title="Iodin" data-language-autonym="Bahasa Melayu" data-language-local-name="Malay" class="interlanguage-link-target">Bahasa Melayu</a></li><li class="interlanguage-link interwiki-cdo mw-list-item"><a href="https://cdo.wikipedia.org/wiki/Di%C4%93ng" title="Diēng – Mindong" lang="cdo" hreflang="cdo" data-title="Diēng" 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%98%D0%BE%D0%B4" title="Иод – Mongolian" lang="mn" hreflang="mn" data-title="Иод" 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%A1%E1%80%AD%E1%80%AF%E1%80%84%E1%80%BA%E1%80%A1%E1%80%AD%E1%80%AF%E1%80%92%E1%80%84%E1%80%BA%E1%80%B8" title="အိုင်အိုဒင်း – Burmese" lang="my" hreflang="my" data-title="အိုင်အိုဒင်း" 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/Jodium_(element)" title="Jodium (element) – Dutch" lang="nl" hreflang="nl" data-title="Jodium (element)" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target">Nederlands</a></li><li class="interlanguage-link interwiki-new mw-list-item"><a href="https://new.wikipedia.org/wiki/%E0%A4%86%E0%A4%AF%E0%A5%8B%E0%A4%A1%E0%A4%BF%E0%A4%A8" title="आयोडिन – Newari" lang="new" hreflang="new" data-title="आयोडिन" 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/%E3%83%A8%E3%82%A6%E7%B4%A0" title="ヨウ素 – Japanese" lang="ja" hreflang="ja" data-title="ヨウ素" 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/Jood" title="Jood – Northern Frisian" lang="frr" hreflang="frr" data-title="Jood" 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/Jod" title="Jod – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Jod" 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/Jod" title="Jod – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Jod" data-language-autonym="Norsk nynorsk" data-language-local-name="Norwegian Nynorsk" class="interlanguage-link-target">Norsk nynorsk</a></li><li class="interlanguage-link interwiki-oc mw-list-item"><a href="https://oc.wikipedia.org/wiki/I%C3%B2de" title="Iòde – Occitan" lang="oc" hreflang="oc" data-title="Iòde" 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%86%E0%AD%9F%E0%AD%8B%E0%AC%A1%E0%AC%BC%E0%AC%BF%E0%AC%A8" title="ଆୟୋଡ଼ିନ – Odia" lang="or" hreflang="or" data-title="ଆୟୋଡ଼ିନ" 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/Yod" title="Yod – Uzbek" lang="uz" hreflang="uz" data-title="Yod" 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%86%E0%A8%87%E0%A8%93%E0%A8%A1%E0%A9%80%E0%A8%A8" title="ਆਇਓਡੀਨ – Punjabi" lang="pa" hreflang="pa" data-title="ਆਇਓਡੀਨ" 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%86%E0%A4%AF%E0%A5%8B%E0%A4%A1%E0%A4%BF%E0%A4%A8" title="आयोडिन – Pali" lang="pi" hreflang="pi" data-title="आयोडिन" 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/%D8%A2%D8%A6%DB%8C%D9%88%DA%88%DB%8C%D9%86" title="آئیوڈین – Western Punjabi" lang="pnb" hreflang="pnb" data-title="آئیوڈین" data-language-autonym="پنجابی" data-language-local-name="Western Punjabi" class="interlanguage-link-target">پنجابی</a></li><li class="interlanguage-link interwiki-ps mw-list-item"><a href="https://ps.wikipedia.org/wiki/%D8%A2%D9%8A%D9%88%DA%89%D9%8A%D9%86" title="آيوډين – Pashto" lang="ps" hreflang="ps" data-title="آيوډين" 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/J%C3%B2dio" title="Jòdio – Piedmontese" lang="pms" hreflang="pms" data-title="Jòdio" 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/Jod" title="Jod – Low German" lang="nds" hreflang="nds" data-title="Jod" 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/Jod" title="Jod – Polish" lang="pl" hreflang="pl" data-title="Jod" 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/Iodo" title="Iodo – Portuguese" lang="pt" hreflang="pt" data-title="Iodo" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target">Português</a></li><li class="interlanguage-link interwiki-ro badge-Q17437796 badge-featuredarticle mw-list-item" title="featured article badge"><a href="https://ro.wikipedia.org/wiki/Iod" title="Iod – Romanian" lang="ro" hreflang="ro" data-title="Iod" 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/Yutyu" title="Yutyu – Quechua" lang="qu" hreflang="qu" data-title="Yutyu" data-language-autonym="Runa Simi" data-language-local-name="Quechua" class="interlanguage-link-target">Runa Simi</a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%98%D0%BE%D0%B4" title="Иод – Russian" lang="ru" hreflang="ru" data-title="Иод" 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%85%E0%A4%AF%E0%A5%8B%E0%A4%A1%E0%A4%BF%E0%A4%A8%E0%A5%8D" title="अयोडिन् – Sanskrit" lang="sa" hreflang="sa" data-title="अयोडिन्" data-language-autonym="संस्कृतम्" data-language-local-name="Sanskrit" class="interlanguage-link-target">संस्कृतम्</a></li><li class="interlanguage-link interwiki-skr mw-list-item"><a href="https://skr.wikipedia.org/wiki/%D8%A2%D8%A6%DB%8C%D9%88%DA%88%DB%8C%D9%86" title="آئیوڈین – Saraiki" lang="skr" hreflang="skr" data-title="آئیوڈین" data-language-autonym="سرائیکی" data-language-local-name="Saraiki" class="interlanguage-link-target">سرائیکی</a></li><li class="interlanguage-link interwiki-sc mw-list-item"><a href="https://sc.wikipedia.org/wiki/J%C3%B2diu" title="Jòdiu – Sardinian" lang="sc" hreflang="sc" data-title="Jòdiu" data-language-autonym="Sardu" data-language-local-name="Sardinian" class="interlanguage-link-target">Sardu</a></li><li class="interlanguage-link interwiki-stq mw-list-item"><a href="https://stq.wikipedia.org/wiki/Iod" title="Iod – Saterland Frisian" lang="stq" hreflang="stq" data-title="Iod" 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/Jodi" title="Jodi – Albanian" lang="sq" hreflang="sq" data-title="Jodi" 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/Iodiu" title="Iodiu – Sicilian" lang="scn" hreflang="scn" data-title="Iodiu" data-language-autonym="Sicilianu" data-language-local-name="Sicilian" class="interlanguage-link-target">Sicilianu</a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Iodine" title="Iodine – Simple English" lang="en-simple" hreflang="en-simple" data-title="Iodine" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target">Simple English</a></li><li class="interlanguage-link interwiki-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/J%C3%B3d" title="Jód – Slovak" lang="sk" hreflang="sk" data-title="Jód" 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/Jod" title="Jod – Slovenian" lang="sl" hreflang="sl" data-title="Jod" 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/Aaydhiin" title="Aaydhiin – Somali" lang="so" hreflang="so" data-title="Aaydhiin" 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/%DB%8C%DB%86%D8%AF" title="یۆد – Central Kurdish" lang="ckb" hreflang="ckb" data-title="یۆد" 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%88%D0%BE%D0%B4" title="Јод – Serbian" lang="sr" hreflang="sr" data-title="Јод" 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/Jod" title="Jod – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Jod" 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/Yodium" title="Yodium – Sundanese" lang="su" hreflang="su" data-title="Yodium" 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/Jodi" title="Jodi – Finnish" lang="fi" hreflang="fi" data-title="Jodi" 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/Jod" title="Jod – Swedish" lang="sv" hreflang="sv" data-title="Jod" data-language-autonym="Svenska" data-language-local-name="Swedish" class="interlanguage-link-target">Svenska</a></li><li class="interlanguage-link interwiki-tl mw-list-item"><a href="https://tl.wikipedia.org/wiki/Yodo" title="Yodo – Tagalog" lang="tl" hreflang="tl" data-title="Yodo" 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%85%E0%AE%AF%E0%AF%8B%E0%AE%9F%E0%AE%BF%E0%AE%A9%E0%AF%8D" title="அயோடின் – Tamil" lang="ta" hreflang="ta" data-title="அயோடின்" 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%98%D0%BE%D0%B4" title="Иод – Tatar" lang="tt" hreflang="tt" data-title="Иод" 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%85%E0%B0%AF%E0%B1%8B%E0%B0%A1%E0%B0%BF%E0%B0%A8%E0%B1%8D" title="అయోడిన్ – Telugu" lang="te" hreflang="te" data-title="అయోడిన్" 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%B9%84%E0%B8%AD%E0%B9%82%E0%B8%AD%E0%B8%94%E0%B8%B5%E0%B8%99" title="ไอโอดีน – Thai" lang="th" hreflang="th" data-title="ไอโอดีน" 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%99%D0%BE%D0%B4" title="Йод – Tajik" lang="tg" hreflang="tg" data-title="Йод" 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/%C4%B0yot" title="İyot – Turkish" lang="tr" hreflang="tr" data-title="İyot" data-language-autonym="Türkçe" data-language-local-name="Turkish" class="interlanguage-link-target">Türkçe</a></li><li class="interlanguage-link interwiki-tyv mw-list-item"><a href="https://tyv.wikipedia.org/wiki/%D0%98%D0%BE%D0%B4" title="Иод – Tuvinian" lang="tyv" hreflang="tyv" data-title="Иод" data-language-autonym="Тыва дыл" data-language-local-name="Tuvinian" class="interlanguage-link-target">Тыва дыл</a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a href="https://uk.wikipedia.org/wiki/%D0%99%D0%BE%D0%B4" title="Йод – Ukrainian" lang="uk" hreflang="uk" data-title="Йод" 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/%D8%A2%DB%8C%D9%88%DA%88%DB%8C%D9%86" title="آیوڈین – Urdu" lang="ur" hreflang="ur" data-title="آیوڈین" 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/%D9%8A%D9%88%D8%AF" title="يود – Uyghur" lang="ug" hreflang="ug" data-title="يود" data-language-autonym="ئۇيغۇرچە / Uyghurche" data-language-local-name="Uyghur" class="interlanguage-link-target">ئۇيغۇرچە / Uyghurche</a></li><li class="interlanguage-link interwiki-vep mw-list-item"><a href="https://vep.wikipedia.org/wiki/Jod" title="Jod – Veps" lang="vep" hreflang="vep" data-title="Jod" 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/Iod" title="Iod – Vietnamese" lang="vi" hreflang="vi" data-title="Iod" data-language-autonym="Tiếng Việt" data-language-local-name="Vietnamese" class="interlanguage-link-target">Tiếng Việt</a></li><li class="interlanguage-link interwiki-zh-classical mw-list-item"><a href="https://zh-classical.wikipedia.org/wiki/%E7%A2%98" title="碘 – Literary Chinese" lang="lzh" hreflang="lzh" data-title="碘" 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/Iodo" title="Iodo – Waray" lang="war" hreflang="war" data-title="Iodo" data-language-autonym="Winaray" data-language-local-name="Waray" class="interlanguage-link-target">Winaray</a></li><li class="interlanguage-link interwiki-wuu mw-list-item"><a href="https://wuu.wikipedia.org/wiki/%E7%A2%98" title="碘 – Wu" lang="wuu" hreflang="wuu" data-title="碘" data-language-autonym="吴语" data-language-local-name="Wu" class="interlanguage-link-target">吴语</a></li><li class="interlanguage-link interwiki-yi mw-list-item"><a href="https://yi.wikipedia.org/wiki/%D7%99%D7%90%D7%93" title="יאד – Yiddish" lang="yi" hreflang="yi" data-title="יאד" data-language-autonym="ייִדיש" data-language-local-name="Yiddish" class="interlanguage-link-target">ייִדיש</a></li><li class="interlanguage-link interwiki-yo mw-list-item"><a href="https://yo.wikipedia.org/wiki/Iod%C3%ADn%C3%AC" title="Iodínì – Yoruba" lang="yo" hreflang="yo" data-title="Iodínì" data-language-autonym="Yorùbá" data-language-local-name="Yoruba" class="interlanguage-link-target">Yorùbá</a></li><li class="interlanguage-link interwiki-zh-yue mw-list-item"><a href="https://zh-yue.wikipedia.org/wiki/%E7%A2%98" title="碘 – Cantonese" lang="yue" hreflang="yue" data-title="碘" data-language-autonym="粵語" data-language-local-name="Cantonese" class="interlanguage-link-target">粵語</a></li><li class="interlanguage-link interwiki-diq mw-list-item"><a href="https://diq.wikipedia.org/wiki/%C4%B0yod" title="İyod – Zazaki" lang="diq" hreflang="diq" data-title="İyod" data-language-autonym="Zazaki" data-language-local-name="Zazaki" class="interlanguage-link-target">Zazaki</a></li><li class="interlanguage-link interwiki-zh badge-Q17437798 badge-goodarticle mw-list-item" title="good article badge"><a href="https://zh.wikipedia.org/wiki/%E7%A2%98" title="碘 – Chinese" lang="zh" hreflang="zh" data-title="碘" data-language-autonym="中文" data-language-local-name="Chinese" class="interlanguage-link-target">中文</a></li> </ul> <div class="after-portlet after-portlet-lang"><a 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For other uses, see <a href="/wiki/Iodine_(disambiguation)" class="mw-disambig" title="Iodine (disambiguation)">Iodine (disambiguation)</a>.</div> <div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical element with atomic number 53 (I)</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">Iodine, 53I</caption><tbody><tr><td colspan="2" class="infobox-image"><a href="/wiki/File:Sample_of_iodine.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0a/Sample_of_iodine.jpg/220px-Sample_of_iodine.jpg" decoding="async" width="220" height="114" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/0a/Sample_of_iodine.jpg/330px-Sample_of_iodine.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/0a/Sample_of_iodine.jpg/440px-Sample_of_iodine.jpg 2x" data-file-width="4069" data-file-height="2115" /></a></td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Iodine</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">/ˈaɪədaɪn, -dɪn, -diːn/</a> (<a href="/wiki/Help:Pronunciation_respelling_key" title="Help:Pronunciation respelling key">EYE-ə-dyne, -⁠din, -⁠deen</a>)</td></tr><tr><th scope="row" class="infobox-label">Appearance</th><td class="infobox-data">lustrous metallic gray solid, black/violet liquid, violet 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°(I)</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>126.90447±0.00003<a href="#cite_note-1">[1]</a></li><li>126.90±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">Iodine 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; background:#f8f8f8; color:black;"> <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 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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 class="mw-selflink selflink">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/Bromine" title="Bromine">Br</a> ↑ I ↓ <a href="/wiki/Astatine" title="Astatine">At</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/Tellurium" title="Tellurium">tellurium</a> ← iodine → <a href="/wiki/Xenon" title="Xenon">xenon</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">53</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_5_element" title="Period 5 element">period 5</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/Krypton" title="Krypton">Kr</a>] 4d10 5s2 5p5</td></tr><tr><th scope="row" class="infobox-label">Electrons per shell</th><td class="infobox-data">2, 8, 18, 18, 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/Solid" title="Solid">solid</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">(I2) 386.85 <a href="/wiki/Kelvin" title="Kelvin">K</a> (113.7 °C, 236.66 °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">(I2) 457.4 K (184.3 °C, 363.7 °F) </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Density" title="Density">Density</a> (at 20° C)</th><td class="infobox-data">4.944 g/cm3<a href="#cite_note-Arblaster_2018-3">[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">386.65 K, 12.1 kPa </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">819 K, 11.7 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">(I2) 15.52 <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">(I2) 41.57 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">(I2) 54.44 J/(mol·K) </td></tr><tr><td colspan="2" class="infobox-full-data"><a href="/wiki/Vapor_pressure" title="Vapor pressure">Vapour pressure</a> (rhombic)<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>260 </td> <td>282 </td> <td>309 </td> <td>342 </td> <td>381 </td> <td>457 </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-4">[4]</a> +4,<a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed">?</a> +6<a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed">?</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: 2.66 </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: 1008.4 kJ/mol </li><li>2nd: 1845.9 kJ/mol </li><li>3rd: 3180 kJ/mol </li><li> </li></ul></div></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Atomic_radius" title="Atomic radius">Atomic radius</a></th><td class="infobox-data">empirical: 140 <a href="/wiki/Picometre" title="Picometre">pm</a> </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">139±3 pm </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">198 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:Iodine_spectrum_visible.png" class="mw-file-description"><img alt="Color lines in a spectral range" src="//upload.wikimedia.org/wikipedia/commons/thumb/8/83/Iodine_spectrum_visible.png/240px-Iodine_spectrum_visible.png" decoding="async" width="240" height="41" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/83/Iodine_spectrum_visible.png/360px-Iodine_spectrum_visible.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/83/Iodine_spectrum_visible.png/480px-Iodine_spectrum_visible.png 2x" data-file-width="7430" data-file-height="1280" /></a><figcaption></figcaption></figure><a href="/wiki/Spectral_line" title="Spectral line">Spectral lines</a> of iodine</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">base-centered 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:Base-centered_orthorhombic.svg" class="mw-file-description"><img alt="Base-centered orthorhombic crystal structure for iodine" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b4/Base-centered_orthorhombic.svg/50px-Base-centered_orthorhombic.svg.png" decoding="async" width="50" height="66" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/b4/Base-centered_orthorhombic.svg/75px-Base-centered_orthorhombic.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/b4/Base-centered_orthorhombic.svg/100px-Base-centered_orthorhombic.svg.png 2x" data-file-width="108" data-file-height="142" /></a></div>a = 725.79 pm b = 478.28 pm c = 982.38 pm (at 20 °C)<a href="#cite_note-Arblaster_2018-3">[3]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Coefficient_of_thermal_expansion" class="mw-redirect" title="Coefficient of thermal expansion">Thermal expansion</a></th><td class="infobox-data">74.9×10−6/K (at 20 °C)<a href="#cite_note-5">[a]</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">0.449 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">1.3×107 Ω⋅m (at 0 °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-6">[5]</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">−88.7×10−6 cm3/mol (298 K)<a href="#cite_note-7">[6]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Bulk_modulus" title="Bulk modulus">Bulk modulus</a></th><td class="infobox-data">7.7 GPa </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">7553-56-2 </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/Bernard_Courtois" title="Bernard Courtois">Bernard Courtois</a> (1811)</td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c"><a href="/wiki/Isotopes_of_iodine" title="Isotopes of iodine">Isotopes of iodine</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_iodine_isotopes" title="Template:Infobox iodine isotopes"><abbr title="View this template">v</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Infobox_iodine_isotopes" title="Special:EditPage/Template:Infobox iodine 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 </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;"><a href="/wiki/Iodine-123" title="Iodine-123">123I</a> </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: center;"><a href="/wiki/Synthetic_radioisotope" title="Synthetic radioisotope">synth</a> </td> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">13.2232 h </td> <td style="text-align: left; vertical-align: top;"><a href="/wiki/Beta_plus_decay" class="mw-redirect" title="Beta plus decay">β+</a>100% </td> <td style="text-align: right; vertical-align: middle;"><a href="/wiki/Tellurium-123" class="mw-redirect" title="Tellurium-123">123Te</a> </td></tr> <tr> <th rowspan="1" style="vertical-align: top;">124I </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: center;">synth </td> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">4.1760 d </td> <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/Tellurium-124" class="mw-redirect" title="Tellurium-124">124Te</a> </td></tr> <tr> <th rowspan="1" style="vertical-align: top;"><a href="/wiki/Iodine-125" title="Iodine-125">125I</a> </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: center;">synth </td> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">59.392 d </td> <td style="text-align: left; vertical-align: top;">ε </td> <td style="text-align: right; vertical-align: middle;"><a href="/wiki/Tellurium-125" class="mw-redirect" title="Tellurium-125">125Te</a> </td></tr> <tr> <th rowspan="1" style="vertical-align: top;">127I </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">100% </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="1" style="vertical-align: top;"><a href="/wiki/Iodine-129" title="Iodine-129">129I</a> </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: center;"><a href="/wiki/Trace_radioisotope" title="Trace radioisotope">trace</a> </td> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">1.614×107 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/Xenon-129" class="mw-redirect" title="Xenon-129">129Xe</a> </td></tr> <tr> <th rowspan="1" style="vertical-align: top;"><a href="/wiki/Iodine-131" title="Iodine-131">131I</a> </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: center;">synth </td> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">8.0249 d </td> <td style="text-align: left; vertical-align: top;">β−100% </td> <td style="text-align: right; vertical-align: middle;"><a href="/wiki/Xenon-131" class="mw-redirect" title="Xenon-131">131Xe</a> </td></tr> <tr> <th rowspan="1" style="vertical-align: top;">135I </th> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: center;">synth </td> <td rowspan="1" colspan="1" style="vertical-align: top; text-align: right;">6.58 h </td> <td style="text-align: left; vertical-align: top;">β− </td> <td style="text-align: right; vertical-align: middle;"><a href="/wiki/Xenon-135" title="Xenon-135">135Xe</a> </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:Iodine" title="Category:Iodine">Category: Iodine</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_iodine" title="Template:Infobox iodine">view</a></li><li class="nv-talk"><a href="/wiki/Template_talk:Infobox_iodine" title="Template talk:Infobox iodine">talk</a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Infobox_iodine" title="Special:EditPage/Template:Infobox iodine">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> Iodine is a <a href="/wiki/Chemical_element" title="Chemical element">chemical element</a>; it has <a href="/wiki/Chemical_symbol" title="Chemical symbol">symbol</a> I and <a href="/wiki/Atomic_number" title="Atomic number">atomic number</a> 53. The heaviest of the stable <a href="/wiki/Halogen" title="Halogen">halogens</a>, it exists at <a href="/wiki/Standard_temperature_and_pressure" title="Standard temperature and pressure">standard conditions</a> as a semi-lustrous, non-metallic solid that melts to form a deep violet liquid at 114 °C (237 °F), and boils to a violet gas at 184 °C (363 °F). The element was discovered by the French chemist <a href="/wiki/Bernard_Courtois" title="Bernard Courtois">Bernard Courtois</a> in 1811 and was named two years later by <a href="/wiki/Joseph_Louis_Gay-Lussac" title="Joseph Louis Gay-Lussac">Joseph Louis Gay-Lussac</a>, after the <a href="/wiki/Ancient_Greek" title="Ancient Greek">Ancient Greek</a> Ιώδης, meaning 'violet'. Iodine occurs in many oxidation states, including <a href="/wiki/Iodide" title="Iodide">iodide</a> (I−), <a href="/wiki/Iodate" title="Iodate">iodate</a> (IO− 3), and the various <a href="/wiki/Periodate" title="Periodate">periodate</a> anions. As the heaviest essential <a href="/wiki/Mineral_(nutrient)" title="Mineral (nutrient)">mineral nutrient</a>, iodine is required for the synthesis of <a href="/wiki/Thyroid_hormones" title="Thyroid hormones">thyroid hormones</a>.<a href="#cite_note-lpi-8">[7]</a> <a href="/wiki/Iodine_deficiency" title="Iodine deficiency">Iodine deficiency</a> affects about two billion people and is the leading preventable cause of <a href="/wiki/Intellectual_disability" title="Intellectual disability">intellectual disabilities</a>.<a href="#cite_note-9">[8]</a> The dominant producers of iodine today are <a href="/wiki/Chile" title="Chile">Chile</a> and <a href="/wiki/Japan" title="Japan">Japan</a>. Due to its high atomic number and ease of attachment to <a href="/wiki/Organic_compound" title="Organic compound">organic compounds</a>, it has also found favour as a non-toxic <a href="/wiki/Radiocontrast_agent" title="Radiocontrast agent">radiocontrast</a> material. Because of the specificity of its uptake by the human body, radioactive isotopes of iodine can also be used to treat <a href="/wiki/Thyroid_cancer" title="Thyroid cancer">thyroid cancer</a>. Iodine is also used as a <a href="/wiki/Catalysis" title="Catalysis">catalyst</a> in the industrial production of <a href="/wiki/Acetic_acid" title="Acetic acid">acetic acid</a> and some <a href="/wiki/Polymer" title="Polymer">polymers</a>. It is on the <a href="/wiki/WHO_Model_List_of_Essential_Medicines" title="WHO Model List of Essential Medicines">World Health Organization's List of Essential Medicines</a>.<a href="#cite_note-WHO22nd-10">[9]</a> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="History">History</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=1" title="Edit section: History">edit</a>]</div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Iodine-evaporating.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/8/8a/Iodine-evaporating.jpg/220px-Iodine-evaporating.jpg" decoding="async" width="220" height="220" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/8a/Iodine-evaporating.jpg/330px-Iodine-evaporating.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/8a/Iodine-evaporating.jpg/440px-Iodine-evaporating.jpg 2x" data-file-width="1022" data-file-height="1022" /></a><figcaption>Iodine crystals <a href="/wiki/Sublimation_(phase_transition)" title="Sublimation (phase transition)">sublimating</a> into a purple gas</figcaption></figure> In 1811, iodine was discovered by French chemist <a href="/wiki/Bernard_Courtois" title="Bernard Courtois">Bernard Courtois</a>,<a href="#cite_note-court-11">[10]</a><a href="#cite_note-12">[11]</a> who was born to a family of manufacturers of <a href="/wiki/Potassium_nitrate" title="Potassium nitrate">saltpetre</a> (an essential component of <a href="/wiki/Gunpowder" title="Gunpowder">gunpowder</a>). At the time of the <a href="/wiki/Napoleonic_Wars" title="Napoleonic Wars">Napoleonic Wars</a>, saltpetre was in great demand in <a href="/wiki/France" title="France">France</a>. Saltpetre produced from French <a href="/wiki/Niter" title="Niter">nitre beds</a> required <a href="/wiki/Sodium_carbonate" title="Sodium carbonate">sodium carbonate</a>, which could be isolated from <a href="/wiki/Seaweed" title="Seaweed">seaweed</a> collected on the coasts of <a href="/wiki/Normandy" title="Normandy">Normandy</a> and <a href="/wiki/Brittany" title="Brittany">Brittany</a>. To isolate the sodium carbonate, seaweed was burned and the ash washed with water. The remaining waste was destroyed by adding <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a>. Courtois once added excessive sulfuric acid and a cloud of violet vapour rose. He noted that the vapour crystallised on cold surfaces, making dark black crystals.<a href="#cite_note-Greenwood794-13">[12]</a> Courtois suspected that this material was a new element but lacked funding to pursue it further.<a href="#cite_note-vdK-14">[13]</a> Courtois gave samples to his friends, <a href="/wiki/Charles_Bernard_Desormes" title="Charles Bernard Desormes">Charles Bernard Desormes</a> (1777–1838) and <a href="/wiki/Nicolas_Cl%C3%A9ment" title="Nicolas Clément">Nicolas Clément</a> (1779–1841), to continue research. He also gave some of the substance to chemist <a href="/wiki/Joseph_Louis_Gay-Lussac" title="Joseph Louis Gay-Lussac">Joseph Louis Gay-Lussac</a> (1778–1850), and to physicist <a href="/wiki/Andr%C3%A9-Marie_Amp%C3%A8re" title="André-Marie Ampère">André-Marie Ampère</a> (1775–1836). On 29 November 1813, Desormes and Clément made Courtois' discovery public by describing the substance to a meeting of the Imperial <a href="/wiki/Institut_de_France" title="Institut de France">Institute of France</a>.<a href="#cite_note-15">[14]</a> On 6 December 1813, Gay-Lussac found and announced that the new substance was either an element or a compound of <a href="/wiki/Oxygen" title="Oxygen">oxygen</a> and he found that it is an element.<a href="#cite_note-Gay-Lussac-16">[15]</a><a href="#cite_note-17">[16]</a><a href="#cite_note-18">[17]</a> Gay-Lussac suggested the name "iode" (<a href="/wiki/Anglicisation_(linguistics)" title="Anglicisation (linguistics)">anglicized</a> as "iodine"), from the <a href="/wiki/Ancient_Greek" title="Ancient Greek">Ancient Greek</a> Ιώδης (iodēs, "violet"), because of the colour of iodine vapor.<a href="#cite_note-court-11">[10]</a><a href="#cite_note-Gay-Lussac-16">[15]</a> Ampère had given some of his sample to British chemist <a href="/wiki/Humphry_Davy" title="Humphry Davy">Humphry Davy</a> (1778–1829), who experimented on the substance and noted its similarity to <a href="/wiki/Chlorine" title="Chlorine">chlorine</a> and also found it as an element.<a href="#cite_note-19">[18]</a> Davy sent a letter dated 10 December to the <a href="/wiki/Royal_Society" title="Royal Society">Royal Society of London</a> stating that he had identified a new element called iodine.<a href="#cite_note-20">[19]</a> Arguments erupted between Davy and Gay-Lussac over who identified iodine first, but both scientists found that both of them identified iodine first and also knew that Courtois is the first one to isolate the element.<a href="#cite_note-vdK-14">[13]</a> In 1873, the French medical researcher <a href="/wiki/Casimir_Davaine" title="Casimir Davaine">Casimir Davaine</a> (1812–1882) discovered the antiseptic action of iodine.<a href="#cite_note-21">[20]</a> <a href="/wiki/Antonio_Grossich" title="Antonio Grossich">Antonio Grossich</a> (1849–1926), an Istrian-born surgeon, was among the first to use <a href="/wiki/Sterilization_(microbiology)" title="Sterilization (microbiology)">sterilisation</a> of the operative field. In 1908, he introduced tincture of iodine as a way to rapidly sterilise the human skin in the surgical field.<a href="#cite_note-22">[21]</a> In early <a href="/wiki/Periodic_table" title="Periodic table">periodic tables</a>, iodine was often given the symbol J, for Jod, its name in <a href="/wiki/German_language" title="German language">German</a>; in German texts, J is still frequently used in place of I.<a href="#cite_note-23">[22]</a> <div class="mw-heading mw-heading2"><h2 id="Properties">Properties</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=2" title="Edit section: Properties">edit</a>]</div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:IodoAtomico.JPG" class="mw-file-description"><img alt="Round bottom flask filled with violet iodine vapour" src="//upload.wikimedia.org/wikipedia/commons/thumb/8/84/IodoAtomico.JPG/150px-IodoAtomico.JPG" decoding="async" width="150" height="177" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/84/IodoAtomico.JPG/225px-IodoAtomico.JPG 1.5x, //upload.wikimedia.org/wikipedia/commons/8/84/IodoAtomico.JPG 2x" data-file-width="252" data-file-height="297" /></a><figcaption>Iodine vapour in a flask, demonstrating its characteristic rich purple colour</figcaption></figure> Iodine is the fourth <a href="/wiki/Halogen" title="Halogen">halogen</a>, being a member of group 17 in the periodic table, below <a href="/wiki/Fluorine" title="Fluorine">fluorine</a>, <a href="/wiki/Chlorine" title="Chlorine">chlorine</a>, and <a href="/wiki/Bromine" title="Bromine">bromine</a>; since <a href="/wiki/Astatine" title="Astatine">astatine</a> and <a href="/wiki/Tennessine" title="Tennessine">tennessine</a> are radioactive, iodine is the heaviest stable halogen. Iodine has an electron configuration of [Kr]5s24d105p5, with the seven electrons in the fifth and outermost shell being its <a href="/wiki/Valence_electron" title="Valence electron">valence electrons</a>. Like the other halogens, it is one electron short of a full octet and is hence an oxidising agent, reacting with many elements in order to complete its outer shell, although in keeping with <a href="/wiki/Periodic_trends" title="Periodic trends">periodic trends</a>, it is the weakest oxidising agent among the stable halogens: it has the lowest <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a> among them, just 2.66 on the Pauling scale (compare fluorine, chlorine, and bromine at 3.98, 3.16, and 2.96 respectively; astatine continues the trend with an electronegativity of 2.2). Elemental iodine hence forms <a href="/wiki/Diatomic_molecule" title="Diatomic molecule">diatomic molecules</a> with chemical formula I2, where two iodine atoms share a pair of electrons in order to each achieve a stable octet for themselves; at high temperatures, these diatomic molecules reversibly dissociate a pair of iodine atoms. Similarly, the iodide anion, I−, is the strongest reducing agent among the stable halogens, being the most easily oxidised back to diatomic I2.<a href="#cite_note-Greenwood800-24">[23]</a> (Astatine goes further, being indeed unstable as At− and readily oxidised to At0 or At+.)<a href="#cite_note-25">[24]</a> The halogens darken in colour as the group is descended: fluorine is a very pale yellow, chlorine is greenish-yellow, bromine is reddish-brown, and iodine is violet. Elemental iodine is slightly soluble in water, with one gram dissolving in 3450 mL at 20 °C and 1280 mL at 50 °C; <a href="/wiki/Potassium_iodide" title="Potassium iodide">potassium iodide</a> may be added to increase solubility via formation of <a href="/wiki/Triiodide" title="Triiodide">triiodide</a> ions, among other polyiodides.<a href="#cite_note-Greenwood804-26">[25]</a> Nonpolar solvents such as <a href="/wiki/Hexane" title="Hexane">hexane</a> and <a href="/wiki/Carbon_tetrachloride" title="Carbon tetrachloride">carbon tetrachloride</a> provide a higher solubility.<a href="#cite_note-27">[26]</a> Polar solutions, such as aqueous solutions, are brown, reflecting the role of these solvents as <a href="/wiki/Lewis_acids_and_bases" title="Lewis acids and bases">Lewis bases</a>; on the other hand, nonpolar solutions are violet, the color of iodine vapour.<a href="#cite_note-Greenwood804-26">[25]</a> <a href="/wiki/Charge-transfer_complex" title="Charge-transfer complex">Charge-transfer complexes</a> form when iodine is dissolved in polar solvents, hence changing the colour. Iodine is violet when dissolved in carbon tetrachloride and saturated hydrocarbons but deep brown in <a href="/wiki/Alcohol_(chemistry)" title="Alcohol (chemistry)">alcohols</a> and <a href="/wiki/Amine" title="Amine">amines</a>, solvents that form charge-transfer adducts.<a href="#cite_note-King-28">[27]</a> The melting and boiling points of iodine are the highest among the halogens, conforming to the increasing trend down the group, since iodine has the largest electron cloud among them that is the most easily polarised, resulting in its molecules having the strongest <a href="/wiki/Van_der_Waals_force" title="Van der Waals force">Van der Waals interactions</a> among the halogens. Similarly, iodine is the least volatile of the halogens, though the solid still can be observed to give off purple vapor.<a href="#cite_note-Greenwood800-24">[23]</a> Due to this property iodine is commonly used to demonstrate <a href="/wiki/Sublimation_(phase_transition)" title="Sublimation (phase transition)">sublimation</a> directly from <a href="/wiki/Solid" title="Solid">solid</a> to <a href="/wiki/Gas" title="Gas">gas</a>, which gives rise to a misconception that it does not <a href="/wiki/Melting" title="Melting">melt</a> in <a href="/wiki/Atmospheric_pressure" title="Atmospheric pressure">atmospheric pressure</a>.<a href="#cite_note-29">[28]</a> Because it has the largest <a href="/wiki/Atomic_radius" title="Atomic radius">atomic radius</a> among the halogens, iodine has the lowest first <a href="/wiki/Ionization_energy" title="Ionization energy">ionisation energy</a>, lowest <a href="/wiki/Electron_affinity" title="Electron affinity">electron affinity</a>, lowest <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a> and lowest reactivity of the halogens.<a href="#cite_note-Greenwood800-24">[23]</a> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Iodine-unit-cell-3D-balls-B.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0c/Iodine-unit-cell-3D-balls-B.png/150px-Iodine-unit-cell-3D-balls-B.png" decoding="async" width="150" height="126" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/0c/Iodine-unit-cell-3D-balls-B.png/225px-Iodine-unit-cell-3D-balls-B.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/0c/Iodine-unit-cell-3D-balls-B.png/300px-Iodine-unit-cell-3D-balls-B.png 2x" data-file-width="1100" data-file-height="927" /></a><figcaption>Structure of solid iodine</figcaption></figure> The interhalogen bond in diiodine is the weakest of all the halogens. As such, 1% of a sample of gaseous iodine at atmospheric pressure is dissociated into iodine atoms at 575 °C. Temperatures greater than 750 °C are required for fluorine, chlorine, and bromine to dissociate to a similar extent. Most bonds to iodine are weaker than the analogous bonds to the lighter halogens.<a href="#cite_note-Greenwood800-24">[23]</a> Gaseous iodine is composed of I2 molecules with an I–I bond length of 266.6 pm. The I–I bond is one of the longest single bonds known. It is even longer (271.5 pm) in solid <a href="/wiki/Orthorhombic_crystal_system" title="Orthorhombic crystal system">orthorhombic</a> crystalline iodine, which has the same crystal structure as chlorine and bromine. (The record is held by iodine's neighbour <a href="/wiki/Xenon" title="Xenon">xenon</a>: the Xe–Xe bond length is 308.71 pm.)<a href="#cite_note-30">[29]</a> As such, within the iodine molecule, significant electronic interactions occur with the two next-nearest neighbours of each atom, and these interactions give rise, in bulk iodine, to a shiny appearance and <a href="/wiki/Semiconductor" title="Semiconductor">semiconducting</a> properties.<a href="#cite_note-Greenwood800-24">[23]</a> Iodine is a two-dimensional semiconductor with a <a href="/wiki/Band_gap" title="Band gap">band gap</a> of 1.3 eV (125 kJ/mol): it is a semiconductor in the plane of its crystalline layers and an insulator in the perpendicular direction.<a href="#cite_note-Greenwood800-24">[23]</a> <div class="mw-heading mw-heading3"><h3 id="Isotopes">Isotopes</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=3" title="Edit section: Isotopes">edit</a>]</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_iodine" title="Isotopes of iodine">Isotopes of iodine</a></div> Of the forty known <a href="/wiki/Isotopes_of_iodine" title="Isotopes of iodine">isotopes of iodine</a>, only one occurs in nature, <a href="/wiki/Isotopes_of_iodine" title="Isotopes of iodine">iodine-127</a>. The others are radioactive and have half-lives too short to be <a href="/wiki/Primordial_nuclide" title="Primordial nuclide">primordial</a>. As such, iodine is both <a href="/wiki/Monoisotopic_element" title="Monoisotopic element">monoisotopic</a> and <a href="/wiki/Mononuclidic_element" title="Mononuclidic element">mononuclidic</a> and its atomic weight is known to great precision, as it is a constant of nature.<a href="#cite_note-Greenwood800-24">[23]</a> The longest-lived of the radioactive isotopes of iodine is <a href="/wiki/Iodine-129" title="Iodine-129">iodine-129</a>, which has a half-life of 15.7 million years, decaying via <a href="/wiki/Beta_decay" title="Beta decay">beta decay</a> to stable <a href="/wiki/Xenon" title="Xenon">xenon</a>-129.<a href="#cite_note-NUBASE-31">[30]</a> Some iodine-129 was formed along with iodine-127 before the formation of the Solar System, but it has by now completely decayed away, making it an <a href="/wiki/Extinct_radionuclide" title="Extinct radionuclide">extinct radionuclide</a>. Its former presence may be determined from an excess of its <a href="/wiki/Decay_product" title="Decay product">daughter</a> xenon-129, but early attempts<a href="#cite_note-Reynolds1960a-32">[31]</a> to use this characteristic to date the supernova source for elements in the Solar System are made difficult by alternative nuclear processes giving iodine-129 and by iodine's volatility at higher temperatures.<a href="#cite_note-Manuel2002-33">[32]</a> Due to its mobility in the environment iodine-129 has been used to date very old groundwaters.<a href="#cite_note-34">[33]</a><a href="#cite_note-35">[34]</a> Traces of iodine-129 still exist today, as it is also a <a href="/wiki/Cosmogenic_nuclide" title="Cosmogenic nuclide">cosmogenic nuclide</a>, formed from <a href="/wiki/Cosmic_ray_spallation" title="Cosmic ray spallation">cosmic ray spallation</a> of atmospheric xenon: these traces make up 10−14 to 10−10 of all terrestrial iodine. It also occurs from open-air nuclear testing, and is not hazardous because of its very long half-life, the longest of all fission products. At the peak of thermonuclear testing in the 1960s and 1970s, iodine-129 still made up only about 10−7 of all terrestrial iodine.<a href="#cite_note-SCOPE50-36">[35]</a> Excited states of iodine-127 and iodine-129 are often used in <a href="/wiki/M%C3%B6ssbauer_spectroscopy" title="Mössbauer spectroscopy">Mössbauer spectroscopy</a>.<a href="#cite_note-Greenwood800-24">[23]</a> The other iodine radioisotopes have much shorter half-lives, no longer than days.<a href="#cite_note-NUBASE-31">[30]</a> Some of them have medical applications involving the <a href="/wiki/Thyroid" title="Thyroid">thyroid gland</a>, where the iodine that enters the body is stored and concentrated. <a href="/wiki/Iodine-123" title="Iodine-123">Iodine-123</a> has a half-life of thirteen hours and decays by <a href="/wiki/Electron_capture" title="Electron capture">electron capture</a> to <a href="/wiki/Isotopes_of_tellurium" title="Isotopes of tellurium">tellurium-123</a>, emitting <a href="/wiki/Gamma_radiation" class="mw-redirect" title="Gamma radiation">gamma radiation</a>; it is used in <a href="/wiki/Nuclear_medicine" title="Nuclear medicine">nuclear medicine imaging</a>, including <a href="/wiki/Single-photon_emission_computed_tomography" title="Single-photon emission computed tomography">single photon emission computed tomography</a> (SPECT) and <a href="/wiki/CT_scan" title="CT scan">X-ray computed tomography</a> (X-Ray CT) scans.<a href="#cite_note-37">[36]</a> <a href="/wiki/Iodine-125" title="Iodine-125">Iodine-125</a> has a half-life of fifty-nine days, decaying by electron capture to <a href="/wiki/Isotopes_of_tellurium" title="Isotopes of tellurium">tellurium-125</a> and emitting low-energy gamma radiation; the second-longest-lived iodine radioisotope, it has uses in <a href="/wiki/Assay" title="Assay">biological assays</a>, <a href="/wiki/Nuclear_medicine" title="Nuclear medicine">nuclear medicine imaging</a> and in <a href="/wiki/Radiation_therapy" title="Radiation therapy">radiation therapy</a> as <a href="/wiki/Brachytherapy" title="Brachytherapy">brachytherapy</a> to treat a number of conditions, including <a href="/wiki/Prostate_cancer" title="Prostate cancer">prostate cancer</a>, <a href="/wiki/Uveal_melanoma" title="Uveal melanoma">uveal melanomas</a>, and <a href="/wiki/Brain_tumor" title="Brain tumor">brain tumours</a>.<a href="#cite_note-38">[37]</a> Finally, <a href="/wiki/Iodine-131" title="Iodine-131">iodine-131</a>, with a half-life of eight days, beta decays to an excited state of stable <a href="/wiki/Isotopes_of_xenon" title="Isotopes of xenon">xenon-131</a> that then converts to the ground state by emitting gamma radiation. It is a common <a href="/wiki/Nuclear_fission_product" title="Nuclear fission product">fission product</a> and thus is present in high levels in radioactive <a href="/wiki/Nuclear_fallout" title="Nuclear fallout">fallout</a>. It may then be absorbed through contaminated food, and will also accumulate in the thyroid. As it decays, it may cause damage to the thyroid. The primary risk from exposure to high levels of iodine-131 is the chance occurrence of <a href="/wiki/Radiogenic_nuclide" title="Radiogenic nuclide">radiogenic</a> <a href="/wiki/Thyroid_cancer" title="Thyroid cancer">thyroid cancer</a> in later life. Other risks include the possibility of non-cancerous growths and <a href="/wiki/Thyroiditis" title="Thyroiditis">thyroiditis</a>.<a href="#cite_note-Rivkees-39">[38]</a> Protection usually used against the negative effects of iodine-131 is by saturating the thyroid gland with stable iodine-127 in the form of <a href="/wiki/Potassium_iodide" title="Potassium iodide">potassium iodide</a> tablets, taken daily for optimal prophylaxis.<a href="#cite_note-40">[39]</a> However, iodine-131 may also be used for medicinal purposes in <a href="/wiki/Radiation_therapy" title="Radiation therapy">radiation therapy</a> for this very reason, when tissue destruction is desired after iodine uptake by the tissue.<a href="#cite_note-41">[40]</a> Iodine-131 is also used as a <a href="/wiki/Radioactive_tracer" title="Radioactive tracer">radioactive tracer</a>.<a href="#cite_note-42">[41]</a><a href="#cite_note-43">[42]</a><a href="#cite_note-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>[<a href="/w/index.php?title=Iodine&action=edit&section=4" title="Edit section: Chemistry and compounds">edit</a>]</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/Iodine_compounds" title="Iodine compounds">Iodine compounds</a></div> <table class="wikitable" style="float:right; width:25%;"> <caption style="margin-bottom: 5px;">Halogen bond energies (kJ/mol)<a href="#cite_note-Greenwood804-26">[25]</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> Iodine is quite reactive, but it is less so than the lighter halogens, and it is a weaker oxidant. For example, it does not <a href="/wiki/Halogenation" title="Halogenation">halogenate</a> <a href="/wiki/Carbon_monoxide" title="Carbon monoxide">carbon monoxide</a>, <a href="/wiki/Nitric_oxide" title="Nitric oxide">nitric oxide</a>, and <a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a>, which <a href="/wiki/Chlorine" title="Chlorine">chlorine</a> does. Many metals react with iodine.<a href="#cite_note-Greenwood800-24">[23]</a> By the same token, however, since iodine has the lowest ionisation energy among the halogens and is the most easily oxidised of them, it has a more significant cationic chemistry and its higher oxidation states are rather more stable than those of bromine and chlorine, for example in <a href="/wiki/Iodine_heptafluoride" title="Iodine heptafluoride">iodine heptafluoride</a>.<a href="#cite_note-Greenwood804-26">[25]</a> <div class="mw-heading mw-heading3"><h3 id="Charge-transfer_complexes">Charge-transfer complexes</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=5" title="Edit section: Charge-transfer complexes">edit</a>]</div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Iodine-triphenylphosphine_charge-transfer_complex_in_dichloromethane.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/7c/Iodine-triphenylphosphine_charge-transfer_complex_in_dichloromethane.jpg/400px-Iodine-triphenylphosphine_charge-transfer_complex_in_dichloromethane.jpg" decoding="async" width="400" height="170" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/7c/Iodine-triphenylphosphine_charge-transfer_complex_in_dichloromethane.jpg/600px-Iodine-triphenylphosphine_charge-transfer_complex_in_dichloromethane.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/7c/Iodine-triphenylphosphine_charge-transfer_complex_in_dichloromethane.jpg/800px-Iodine-triphenylphosphine_charge-transfer_complex_in_dichloromethane.jpg 2x" data-file-width="6220" data-file-height="2650" /></a><figcaption>I2•<a href="/wiki/Triphenylphosphine" title="Triphenylphosphine">PPh3</a> charge-transfer complexes in <a href="/wiki/Dichloromethane" title="Dichloromethane">CH2Cl2</a>. From left to right: (1) I2 dissolved in dichloromethane – no CT complex. (2) A few seconds after excess PPh3 was added – CT complex is forming. (3) One minute later after excess PPh3 was added, the CT complex [Ph3PI]+I− has been formed. (4) Immediately after excess I2 was added, which contains [Ph3PI]+[I3]−.<a href="#cite_note-InorgChem-46">[45]</a></figcaption></figure> The iodine molecule, I2, dissolves in CCl4 and aliphatic hydrocarbons to give bright violet solutions. In these solvents the absorption band maximum occurs in the 520 – 540 nm region and is assigned to a π* to σ* transition. When I2 reacts with Lewis bases in these solvents a blue shift in I2 peak is seen and the new peak (230 – 330 nm) arises that is due to the formation of adducts, which are referred to as charge-transfer complexes.<a href="#cite_note-Greenwood806-47">[46]</a> <div class="mw-heading mw-heading3"><h3 id="Hydrogen_iodide">Hydrogen iodide</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=6" title="Edit section: Hydrogen iodide">edit</a>]</div> The simplest compound of iodine is <a href="/wiki/Hydrogen_iodide" title="Hydrogen iodide">hydrogen iodide</a>, HI. It is a colourless gas that reacts with oxygen to give water and iodine. Although it is useful in <a href="/wiki/Halogenation" title="Halogenation">iodination</a> reactions in the laboratory, it does not have large-scale industrial uses, unlike the other hydrogen halides. Commercially, it is usually made by reacting iodine with <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">hydrogen sulfide</a> or <a href="/wiki/Hydrazine" title="Hydrazine">hydrazine</a>:<a href="#cite_note-Greenwood809-48">[47]</a> <style data-mw-deduplicate="TemplateStyles:r996643573">.mw-parser-output .block-indent{padding-left:3em;padding-right:0;overflow:hidden}</style><div class="block-indent">2 I2 + N2H4 H2O⟶ 4 HI + N2</div> At room temperature, it is a colourless gas, like all of the hydrogen halides except <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 large and only mildly electronegative iodine atom. It melts at −51.0 °C (−59.8 °F) and boils at −35.1 °C (−31.2 °F). It is an <a href="/wiki/Endothermic_process" title="Endothermic process">endothermic</a> compound that can exothermically dissociate at room temperature, although the process is very slow unless a <a href="/wiki/Catalysis" title="Catalysis">catalyst</a> is present: the reaction between hydrogen and iodine at room temperature to give hydrogen iodide does not proceed to completion. The H–I <a href="/wiki/Bond-dissociation_energy" title="Bond-dissociation energy">bond dissociation energy</a> is likewise the smallest of the hydrogen halides, at 295 kJ/mol.<a href="#cite_note-Greenwood812-49">[48]</a> Aqueous hydrogen iodide is known as <a href="/wiki/Hydroiodic_acid" title="Hydroiodic acid">hydroiodic acid</a>, which is a strong acid. Hydrogen iodide is exceptionally soluble in water: one litre of water will dissolve 425 litres of hydrogen iodide, and the saturated solution has only four water molecules per molecule of hydrogen iodide.<a href="#cite_note-50">[49]</a> Commercial so-called "concentrated" hydroiodic acid usually contains 48–57% HI by mass; the solution forms an <a href="/wiki/Azeotrope" title="Azeotrope">azeotrope</a> with boiling point 126.7 °C (260.1 °F) at 56.7 g HI per 100 g solution. Hence hydroiodic acid cannot be concentrated past this point by evaporation of water.<a href="#cite_note-Greenwood812-49">[48]</a> Unlike gaseous hydrogen iodide, hydroiodic acid has major industrial use in the manufacture of <a href="/wiki/Acetic_acid" title="Acetic acid">acetic acid</a> by the <a href="/wiki/Cativa_process" title="Cativa process">Cativa process</a>.<a href="#cite_note-Cativa-51">[50]</a><a href="#cite_note-52">[51]</a> <div class="mw-heading mw-heading3"><h3 id="Other_binary_iodine_compounds">Other binary iodine compounds</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=7" title="Edit section: Other binary iodine compounds">edit</a>]</div> With the exception of the <a href="/wiki/Noble_gas" title="Noble gas">noble gases</a>, nearly all elements on the periodic table up to einsteinium (<a href="/wiki/Einsteinium(III)_iodide" title="Einsteinium(III) iodide">EsI3</a> is known) are known to form binary compounds with iodine. Until 1990, <a href="/wiki/Nitrogen_triiodide" title="Nitrogen triiodide">nitrogen triiodide</a><a href="#cite_note-53">[52]</a> was only known as an ammonia adduct. Ammonia-free NI3 was found to be isolable at –196 °C but spontaneously decomposes at 0 °C.<a href="#cite_note-54">[53]</a> For thermodynamic reasons related to electronegativity of the elements, neutral sulfur and selenium iodides that are stable at room temperature are also nonexistent, although S2I2 and SI2 are stable up to 183 and 9 K, respectively. As of 2022, no neutral binary selenium iodide has been unambiguously identified (at any temperature).<a href="#cite_note-55">[54]</a> Sulfur- and selenium-iodine polyatomic cations (e.g., [S2I42+][AsF6–]2 and [Se2I42+][Sb2F11–]2) have been prepared and characterized crystallographically.<a href="#cite_note-56">[55]</a> Given the large size of the iodide anion and iodine's weak oxidising power, high oxidation states are difficult to achieve in binary iodides, the maximum known being in the pentaiodides of <a href="/wiki/Niobium" title="Niobium">niobium</a>, <a href="/wiki/Tantalum" title="Tantalum">tantalum</a>, and <a href="/wiki/Protactinium" title="Protactinium">protactinium</a>. Iodides can be made by reaction of an element or its oxide, hydroxide, or carbonate with hydroiodic acid, and then dehydrated by mildly high temperatures combined with either low pressure or anhydrous hydrogen iodide gas. These methods work best when the iodide product is stable to hydrolysis. Other syntheses include high-temperature oxidative iodination of the element with iodine or hydrogen iodide, high-temperature iodination of a metal oxide or other halide by iodine, a volatile metal halide, <a href="/wiki/Carbon_tetraiodide" title="Carbon tetraiodide">carbon tetraiodide</a>, or an organic iodide. For example, <a href="/wiki/Molybdenum_dioxide" title="Molybdenum dioxide">molybdenum(IV) oxide</a> reacts with <a href="/wiki/Aluminium_iodide" title="Aluminium iodide">aluminium(III) iodide</a> at 230 °C to give <a href="/wiki/Molybdenum(II)_iodide" title="Molybdenum(II) iodide">molybdenum(II) iodide</a>. An example involving halogen exchange is given below, involving the reaction of <a href="/wiki/Tantalum(V)_chloride" title="Tantalum(V) chloride">tantalum(V) chloride</a> with excess aluminium(III) iodide at 400 °C to give <a href="/wiki/Tantalum(V)_iodide" title="Tantalum(V) iodide">tantalum(V) iodide</a>:<a href="#cite_note-Greenwood821-57">[56]</a> <math display="block" xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle {\ce {3TaCl5 + {\underset {(excess)}{5AlI3}}-> 3TaI5 + 5AlCl3}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <mn>3</mn> <mspace width="thinmathspace" /> <msubsup> <mtext>TaCl</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>5</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mo>+</mo> <mrow class="MJX-TeXAtom-ORD"> <munder> <mrow> <mn>5</mn> <mspace width="thinmathspace" /> <msubsup> <mtext>AlI</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>3</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mo stretchy="false">(</mo> <mtext>excess</mtext> <mo stretchy="false">)</mo> </mrow> </munder> </mrow> <mo stretchy="false">⟶</mo> <mn>3</mn> <mspace width="thinmathspace" /> <msubsup> <mtext>TaI</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>5</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mo>+</mo> <mn>5</mn> <mspace width="thinmathspace" /> <msubsup> <mtext>AlCl</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>3</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {\ce {3TaCl5 + {\underset {(excess)}{5AlI3}}-> 3TaI5 + 5AlCl3}}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/33501eea373660bbd0b9b2b3ff66a2e0244bdfd4" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -3.338ex; width:37.982ex; height:5.176ex;" alt="{\displaystyle {\ce {3TaCl5 + {\underset {(excess)}{5AlI3}}-> 3TaI5 + 5AlCl3}}}"> Lower iodides may be produced either through thermal decomposition or disproportionation, or by reducing the higher iodide with hydrogen or a metal, for example:<a href="#cite_note-Greenwood821-57">[56]</a> <math display="block" xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle {\ce {TaI5{}+Ta->[{\text{thermal gradient}}][{\ce {630^{\circ }C\ ->\ 575^{\circ }C}}]Ta6I14}}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mrow class="MJX-TeXAtom-ORD"> <msubsup> <mtext>TaI</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>5</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <mrow class="MJX-TeXAtom-ORD"> </mrow> <mo>+</mo> <mtext>Ta</mtext> <mrow class="MJX-TeXAtom-REL"> <munderover> <mo>→</mo> <mpadded width="+0.611em" lspace="0.278em" voffset="-.24em"> <mrow class="MJX-TeXAtom-ORD"> <mn>630</mn> <msup> <mspace width="thinmathspace" /> <mrow class="MJX-TeXAtom-ORD"> <mo>∘</mo> </mrow> </msup> <mtext>C</mtext> <mtext> </mtext> <mo stretchy="false">⟶</mo> <mtext> </mtext> <mn>575</mn> <msup> <mspace width="thinmathspace" /> <mrow class="MJX-TeXAtom-ORD"> <mo>∘</mo> </mrow> </msup> <mtext>C</mtext> </mrow> </mpadded> <mpadded width="+0.611em" lspace="0.278em" voffset=".15em"> <mrow class="MJX-TeXAtom-ORD"> <mtext>thermal gradient</mtext> </mrow> </mpadded> </munderover> </mrow> <msubsup> <mtext>Ta</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>6</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> <msubsup> <mtext>I</mtext> <mrow class="MJX-TeXAtom-ORD"> <mn>14</mn> </mrow> <mrow class="MJX-TeXAtom-ORD"> <mspace width="0pt" height="0pt" depth=".2em" /> </mrow> </msubsup> </mrow> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle {\ce {TaI5{}+Ta->[{\text{thermal gradient}}][{\ce {630^{\circ }C\ ->\ 575^{\circ }C}}]Ta6I14}}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/2bccb303062c4ab95661541d583e04d60a434c25" class="mwe-math-fallback-image-display mw-invert skin-invert" aria-hidden="true" style="vertical-align: -1.874ex; margin-top: -0.342ex; margin-bottom: -0.63ex; width:33.234ex; height:6.009ex;" alt="{\displaystyle {\ce {TaI5{}+Ta->[{\text{thermal gradient}}][{\ce {630^{\circ }C\ ->\ 575^{\circ }C}}]Ta6I14}}}"> Most metal iodides with the metal in low oxidation states (+1 to +3) are ionic. Nonmetals tend to form covalent molecular iodides, as do metals in high oxidation states from +3 and above. Both ionic and covalent iodides are known for metals in oxidation state +3 (e.g. <a href="/wiki/Scandium_triiodide" title="Scandium triiodide">scandium iodide</a> is mostly ionic, but <a href="/wiki/Aluminium_iodide" title="Aluminium iodide">aluminium iodide</a> is not). Ionic iodides MIn tend to have the lowest melting and boiling points among the halides MXn of the same element, because the electrostatic forces of attraction between the cations and anions are weakest for the large iodide anion. In contrast, covalent iodides tend to instead have the highest melting and boiling points among the halides of the same element, since iodine is the most polarisable of the halogens and, having the most electrons among them, can contribute the most to van der Waals forces. Naturally, exceptions abound in intermediate iodides where one trend gives way to the other. Similarly, solubilities in water of predominantly ionic iodides (e.g. <a href="/wiki/Potassium" title="Potassium">potassium</a> and <a href="/wiki/Calcium" title="Calcium">calcium</a>) are the greatest among ionic halides of that element, while those of covalent iodides (e.g. <a href="/wiki/Silver" title="Silver">silver</a>) are the lowest of that element. In particular, <a href="/wiki/Silver_iodide" title="Silver iodide">silver iodide</a> is very insoluble in water and its formation is often used as a qualitative test for iodine.<a href="#cite_note-Greenwood821-57">[56]</a> <div class="mw-heading mw-heading3"><h3 id="Iodine_halides">Iodine halides</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=8" title="Edit section: Iodine halides">edit</a>]</div> The halogens form many binary, <a href="/wiki/Diamagnetism" title="Diamagnetism">diamagnetic</a> <a href="/wiki/Interhalogen" title="Interhalogen">interhalogen</a> compounds with stoichiometries XY, XY3, XY5, and XY7 (where X is heavier than Y), and iodine is no exception. Iodine forms all three possible diatomic interhalogens, a trifluoride and trichloride, as well as a pentafluoride and, exceptionally among the halogens, a heptafluoride. Numerous cationic and anionic derivatives are also characterised, such as the wine-red or bright orange compounds of ICl+ 2 and the dark brown or purplish black compounds of I2Cl+. Apart from these, some <a href="/wiki/Pseudohalogen" title="Pseudohalogen">pseudohalides</a> are also known, such as <a href="/wiki/Cyanogen_iodide" title="Cyanogen iodide">cyanogen iodide</a> (ICN), iodine <a href="/wiki/Thiocyanate" title="Thiocyanate">thiocyanate</a> (ISCN), and iodine <a href="/wiki/Azide" title="Azide">azide</a> (IN3).<a href="#cite_note-Greenwood824-58">[57]</a> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Iodine_monochloride1.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/48/Iodine_monochloride1.jpg/220px-Iodine_monochloride1.jpg" decoding="async" width="220" height="313" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/48/Iodine_monochloride1.jpg/330px-Iodine_monochloride1.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/4/48/Iodine_monochloride1.jpg 2x" data-file-width="338" data-file-height="481" /></a><figcaption>Iodine monochloride</figcaption></figure> <a href="/wiki/Iodine_monofluoride" title="Iodine monofluoride">Iodine monofluoride</a> (IF) is unstable at room temperature and disproportionates very readily and irreversibly to iodine and <a href="/wiki/Iodine_pentafluoride" title="Iodine pentafluoride">iodine pentafluoride</a>, and thus cannot be obtained pure. It can be synthesised from the reaction of iodine with fluorine gas in <a href="/wiki/Trichlorofluoromethane" title="Trichlorofluoromethane">trichlorofluoromethane</a> at −45 °C, with <a href="/wiki/Iodine_trifluoride" title="Iodine trifluoride">iodine trifluoride</a> in trichlorofluoromethane at −78 °C, or with <a href="/wiki/Silver(I)_fluoride" title="Silver(I) fluoride">silver(I) fluoride</a> at 0 °C.<a href="#cite_note-Greenwood824-58">[57]</a> <a href="/wiki/Iodine_monochloride" title="Iodine monochloride">Iodine monochloride</a> (ICl) and <a href="/wiki/Iodine_monobromide" title="Iodine monobromide">iodine monobromide</a> (IBr), on the other hand, are moderately stable. The former, a volatile red-brown compound, was discovered independently by <a href="/wiki/Joseph_Louis_Gay-Lussac" title="Joseph Louis Gay-Lussac">Joseph Louis Gay-Lussac</a> and <a href="/wiki/Humphry_Davy" title="Humphry Davy">Humphry Davy</a> in 1813–1814 not long after the discoveries of chlorine and iodine, and it mimics the intermediate halogen bromine so well that <a href="/wiki/Justus_von_Liebig" title="Justus von Liebig">Justus von Liebig</a> was misled into mistaking bromine (which he had found) for iodine monochloride. Iodine monochloride and iodine monobromide may be prepared simply by reacting iodine with chlorine or bromine at room temperature and purified by <a href="/wiki/Fractional_crystallization_(chemistry)" title="Fractional crystallization (chemistry)">fractional crystallisation</a>. Both are quite reactive and attack even <a href="/wiki/Platinum" title="Platinum">platinum</a> and <a href="/wiki/Gold" title="Gold">gold</a>, though not <a href="/wiki/Boron" title="Boron">boron</a>, <a href="/wiki/Carbon" title="Carbon">carbon</a>, <a href="/wiki/Cadmium" title="Cadmium">cadmium</a>, <a href="/wiki/Lead" title="Lead">lead</a>, <a href="/wiki/Zirconium" title="Zirconium">zirconium</a>, <a href="/wiki/Niobium" title="Niobium">niobium</a>, <a href="/wiki/Molybdenum" title="Molybdenum">molybdenum</a>, and <a href="/wiki/Tungsten" title="Tungsten">tungsten</a>. Their reaction with organic compounds depends on conditions. Iodine chloride vapour tends to chlorinate <a href="/wiki/Phenol" title="Phenol">phenol</a> and <a href="/wiki/Salicylic_acid" title="Salicylic acid">salicylic acid</a>, since when iodine chloride undergoes <a href="/wiki/Homolysis_(chemistry)" title="Homolysis (chemistry)">homolytic fission</a>, chlorine and iodine are produced and the former is more reactive. However, iodine chloride in <a href="/wiki/Carbon_tetrachloride" title="Carbon tetrachloride">carbon tetrachloride</a> solution results in iodination being the main reaction, since now <a href="/wiki/Heterolysis_(chemistry)" title="Heterolysis (chemistry)">heterolytic fission</a> of the I–Cl bond occurs and I+ attacks phenol as an electrophile. However, iodine monobromide tends to brominate phenol even in carbon tetrachloride solution because it tends to dissociate into its elements in solution, and bromine is more reactive than iodine.<a href="#cite_note-Greenwood824-58">[57]</a> When liquid, iodine monochloride and iodine monobromide dissociate into I 2X+ and IX− 2 ions (X = Cl, Br); thus they are significant conductors of electricity and can be used as ionising solvents.<a href="#cite_note-Greenwood824-58">[57]</a> <a href="/wiki/Iodine_trifluoride" title="Iodine trifluoride">Iodine trifluoride</a> (IF3) is an unstable yellow solid that decomposes above −28 °C. It is thus little-known. It is difficult to produce because fluorine gas would tend to oxidise iodine all the way to the pentafluoride; reaction at low temperature with <a href="/wiki/Xenon_difluoride" title="Xenon difluoride">xenon difluoride</a> is necessary. <a href="/wiki/Iodine_trichloride" title="Iodine trichloride">Iodine trichloride</a>, which exists in the solid state as the planar dimer I2Cl6, is a bright yellow solid, synthesised by reacting iodine with liquid chlorine at −80 °C; caution is necessary during purification because it easily dissociates to iodine monochloride and chlorine and hence can act as a strong chlorinating agent. Liquid iodine trichloride conducts electricity, possibly indicating dissociation to ICl+ 2 and ICl− 4 ions.<a href="#cite_note-Greenwood828-59">[58]</a> <a href="/wiki/Iodine_pentafluoride" title="Iodine pentafluoride">Iodine pentafluoride</a> (IF5), a colourless, volatile liquid, is the most thermodynamically stable iodine fluoride, and can be made by reacting iodine with fluorine gas at room temperature. It is a fluorinating agent, but is mild enough to store in glass apparatus. Again, slight electrical conductivity is present in the liquid state because of dissociation to IF+ 4 and IF− 6. The <a href="/wiki/Pentagonal_bipyramidal_molecular_geometry" title="Pentagonal bipyramidal molecular geometry">pentagonal bipyramidal</a> <a href="/wiki/Iodine_heptafluoride" title="Iodine heptafluoride">iodine heptafluoride</a> (IF7) is an extremely powerful fluorinating agent, behind only <a href="/wiki/Chlorine_trifluoride" title="Chlorine trifluoride">chlorine trifluoride</a>, <a href="/wiki/Chlorine_pentafluoride" title="Chlorine pentafluoride">chlorine pentafluoride</a>, and <a href="/wiki/Bromine_pentafluoride" title="Bromine pentafluoride">bromine pentafluoride</a> among the interhalogens: it reacts with almost all the elements even at low temperatures, fluorinates <a href="/wiki/Pyrex" title="Pyrex">Pyrex</a> glass to form iodine(VII) oxyfluoride (IOF5), and sets <a href="/wiki/Carbon_monoxide" title="Carbon monoxide">carbon monoxide</a> on fire.<a href="#cite_note-Greenwood832-60">[59]</a> <div class="mw-heading mw-heading3"><h3 id="Iodine_oxides_and_oxoacids">Iodine oxides and oxoacids</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=9" title="Edit section: Iodine oxides and oxoacids">edit</a>]</div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Iodine-pentoxide-3D-balls.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/47/Iodine-pentoxide-3D-balls.png/150px-Iodine-pentoxide-3D-balls.png" decoding="async" width="150" height="77" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/47/Iodine-pentoxide-3D-balls.png/225px-Iodine-pentoxide-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/47/Iodine-pentoxide-3D-balls.png/300px-Iodine-pentoxide-3D-balls.png 2x" data-file-width="1100" data-file-height="564" /></a><figcaption>Structure of iodine pentoxide</figcaption></figure> <a href="/wiki/Iodine_oxide" title="Iodine oxide">Iodine oxides</a> are the most stable of all the halogen oxides, because of the strong I–O bonds resulting from the large electronegativity difference between iodine and oxygen, and they have been known for the longest time.<a href="#cite_note-King-28">[27]</a> The stable, white, <a href="/wiki/Hygroscopy" title="Hygroscopy">hygroscopic</a> <a href="/wiki/Iodine_pentoxide" title="Iodine pentoxide">iodine pentoxide</a> (I2O5) has been known since its formation in 1813 by Gay-Lussac and Davy. It is most easily made by the dehydration of <a href="/wiki/Iodic_acid" title="Iodic acid">iodic acid</a> (HIO3), of which it is the anhydride. It will quickly oxidise carbon monoxide completely to <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> at room temperature, and is thus a useful reagent in determining carbon monoxide concentration. It also oxidises <a href="/wiki/Nitrogen_oxide" title="Nitrogen oxide">nitrogen oxide</a>, <a href="/wiki/Ethylene" title="Ethylene">ethylene</a>, and <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">hydrogen sulfide</a>. It reacts with <a href="/wiki/Sulfur_trioxide" title="Sulfur trioxide">sulfur trioxide</a> and peroxydisulfuryl difluoride (S2O6F2) to form salts of the iodyl cation, [IO2]+, and is reduced by concentrated <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> to iodosyl salts involving [IO]+. It may be fluorinated by <a href="/wiki/Fluorine" title="Fluorine">fluorine</a>, <a href="/wiki/Bromine_trifluoride" title="Bromine trifluoride">bromine trifluoride</a>, <a href="/wiki/Sulfur_tetrafluoride" title="Sulfur tetrafluoride">sulfur tetrafluoride</a>, or <a href="/wiki/Chloryl_fluoride" title="Chloryl fluoride">chloryl fluoride</a>, resulting <a href="/wiki/Iodine_pentafluoride" title="Iodine pentafluoride">iodine pentafluoride</a>, which also reacts with <a href="/wiki/Iodine_pentoxide" title="Iodine pentoxide">iodine pentoxide</a>, giving iodine(V) oxyfluoride, IOF3. A few other less stable oxides are known, notably I4O9 and I2O4; their structures have not been determined, but reasonable guesses are IIII(IVO3)3 and [IO]+[IO3]− respectively.<a href="#cite_note-Greenwood851-61">[60]</a> <table class="wikitable" style="float:right; width:25%;"> <caption>Standard reduction potentials for aqueous I species<a href="#cite_note-Greenwood853-62">[61]</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>I2/I−</td> <td>+0.535</td> <td>I2/I−</td> <td>+0.535 </td></tr> <tr> <td>HOI/I−</td> <td>+0.987</td> <td>IO−/I−</td> <td>+0.48 </td></tr> <tr> <td>0</td> <td>0</td> <td>IO− 3/I−</td> <td>+0.26 </td></tr> <tr> <td>HOI/I2</td> <td>+1.439</td> <td>IO−/I2</td> <td>+0.42 </td></tr> <tr> <td>IO− 3/I2</td> <td>+1.195</td> <td>0</td> <td>0 </td></tr> <tr> <td>IO− 3/HOI</td> <td>+1.134</td> <td>IO− 3/IO−</td> <td>+0.15 </td></tr> <tr> <td>IO− 4/IO− 3</td> <td>+1.653</td> <td>0</td> <td>0 </td></tr> <tr> <td>H5IO6/IO− 3</td> <td>+1.601</td> <td>H 3IO2− 6/IO− 3</td> <td>+0.65 </td></tr></tbody></table> More important are the four oxoacids: <a href="/wiki/Hypoiodous_acid" title="Hypoiodous acid">hypoiodous acid</a> (HIO), <a href="/wiki/Iodite" title="Iodite">iodous acid</a> (HIO2), <a href="/wiki/Iodic_acid" title="Iodic acid">iodic acid</a> (HIO3), and <a href="/wiki/Periodic_acid" title="Periodic acid">periodic acid</a> (HIO4 or H5IO6). When iodine dissolves in aqueous solution, the following reactions occur:<a href="#cite_note-Greenwood853-62">[61]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"> <table> <tbody><tr> <td> </td></tr> <tr> <td>I2 + H2O</td> <td>⇌ HIO + H+ + I−</td> <td>- </td> <td>I2 + 2 OH−</td> <td>⇌ IO− + H2O + I−</td> <td>Kalk = 30 mol2 L−2 </td></tr></tbody></table></div> Hypoiodous acid is unstable to disproportionation. The hypoiodite ions thus formed disproportionate immediately to give iodide and iodate:<a href="#cite_note-Greenwood853-62">[61]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"> 3 IO− ⇌ 2 I− + IO− 3 K = 1020</div> Iodous acid and iodite are even less stable and exist only as a fleeting intermediate in the oxidation of iodide to iodate, if at all.<a href="#cite_note-Greenwood853-62">[61]</a> Iodates are by far the most important of these compounds, which can be made by oxidising <a href="/wiki/Alkali_metal" title="Alkali metal">alkali metal</a> iodides with oxygen at 600 °C and high pressure, or by oxidising iodine with <a href="/wiki/Chlorate" title="Chlorate">chlorates</a>. Unlike chlorates, which disproportionate very slowly to form chloride and perchlorate, iodates are stable to disproportionation in both acidic and alkaline solutions. From these, salts of most metals can be obtained. Iodic acid is most easily made by oxidation of an aqueous iodine suspension by <a href="/wiki/Electrolysis" title="Electrolysis">electrolysis</a> or fuming <a href="/wiki/Nitric_acid" title="Nitric acid">nitric acid</a>. Iodate has the weakest oxidising power of the halates, but reacts the quickest.<a href="#cite_note-Greenwood863-63">[62]</a> Many periodates are known, including not only the expected tetrahedral IO− 4, but also square-pyramidal IO3− 5, octahedral orthoperiodate IO5− 6, [IO3(OH)3]2−, [I2O8(OH2)]4−, and I 2O4− 9. They are usually made by oxidising alkaline <a href="/wiki/Sodium_iodate" title="Sodium iodate">sodium iodate</a> electrochemically (with <a href="/wiki/Lead_dioxide" title="Lead dioxide">lead(IV) oxide</a> as the anode) or by chlorine gas:<a href="#cite_note-Greenwood872-64">[63]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">IO− 3 + 6 OH− → IO5− 6 + 3 H2O + 2 e−</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">IO− 3 + 6 OH− + Cl2 → IO5− 6 + 2 Cl− + 3 H2O</div> They are thermodymically and kinetically powerful oxidising agents, quickly oxidising Mn2+ to <a href="/wiki/Permanganate" title="Permanganate">MnO− 4</a>, and cleaving <a href="/wiki/Diol" title="Diol">glycols</a>, α-<a href="/wiki/Dicarbonyl" title="Dicarbonyl">diketones</a>, α-<a href="/wiki/Hydroxy_ketone" title="Hydroxy ketone">ketols</a>, α-<a href="/wiki/Alkanolamine" title="Alkanolamine">aminoalcohols</a>, and α-<a href="/wiki/Diamine" title="Diamine">diamines</a>.<a href="#cite_note-Greenwood872-64">[63]</a> Orthoperiodate especially stabilises high oxidation states among metals because of its very high negative charge of −5. <a href="/wiki/Periodic_acid" title="Periodic acid">Orthoperiodic acid</a>, H5IO6, is stable, and dehydrates at 100 °C in a vacuum to <a href="/wiki/Periodic_acid" title="Periodic acid">Metaperiodic acid</a>, HIO4. Attempting to go further does not result in the nonexistent iodine heptoxide (I2O7), but rather iodine pentoxide and oxygen. Periodic acid may be protonated by <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> to give the I(OH)+ 6 cation, isoelectronic to Te(OH)6 and Sb(OH)− 6, and giving salts with bisulfate and sulfate.<a href="#cite_note-King-28">[27]</a> <div class="mw-heading mw-heading3"><h3 id="Polyiodine_compounds">Polyiodine compounds</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=10" title="Edit section: Polyiodine compounds">edit</a>]</div> When iodine dissolves in strong acids, such as fuming sulfuric acid, a bright blue <a href="/wiki/Paramagnetism" title="Paramagnetism">paramagnetic</a> solution including I+ 2 cations is formed. A solid salt of the diiodine cation may be obtained by oxidising iodine with <a href="/wiki/Antimony_pentafluoride" title="Antimony pentafluoride">antimony pentafluoride</a>:<a href="#cite_note-King-28">[27]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">2 I2 + 5 SbF5 SO2⟶20 °C 2 I2Sb2F11 + SbF3</div> The salt I2Sb2F11 is dark blue, and the blue <a href="/wiki/Tantalum" title="Tantalum">tantalum</a> analogue I2Ta2F11 is also known. Whereas the I–I bond length in I2 is 267 pm, that in I+ 2 is only 256 pm as the missing electron in the latter has been removed from an antibonding orbital, making the bond stronger and hence shorter. In <a href="/wiki/Fluorosulfuric_acid" title="Fluorosulfuric acid">fluorosulfuric acid</a> solution, deep-blue I+ 2 reversibly dimerises below −60 °C, forming red rectangular diamagnetic I2+ 4. Other polyiodine cations are not as well-characterised, including bent dark-brown or black I+ 3 and centrosymmetric C2h green or black I+ 5, known in the AsF− 6 and AlCl− 4 salts among others.<a href="#cite_note-King-28">[27]</a><a href="#cite_note-Greenwood842-65">[64]</a> The only important polyiodide anion in aqueous solution is linear <a href="/wiki/Triiodide" title="Triiodide">triiodide</a>, I− 3. Its formation explains why the solubility of iodine in water may be increased by the addition of potassium iodide solution:<a href="#cite_note-King-28">[27]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent">I2 + I− ⇌ I− 3 (Keq = c. 700 at 20 °C)</div> Many other polyiodides may be found when solutions containing iodine and iodide crystallise, such as I− 5, I− 9, I2− 4, and I2− 8, whose salts with large, weakly polarising cations such as <a href="/wiki/Caesium" title="Caesium">Cs+</a> may be isolated.<a href="#cite_note-King-28">[27]</a><a href="#cite_note-Greenwood835-66">[65]</a> <div class="mw-heading mw-heading3"><h3 id="Organoiodine_compounds">Organoiodine compounds</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=11" title="Edit section: Organoiodine compounds">edit</a>]</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/Organoiodine_compound" class="mw-redirect" title="Organoiodine compound">Organoiodine compound</a></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:IBXAcid.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/2/25/IBXAcid.png/220px-IBXAcid.png" decoding="async" width="220" height="207" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/25/IBXAcid.png/330px-IBXAcid.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/25/IBXAcid.png/440px-IBXAcid.png 2x" data-file-width="506" data-file-height="476" /></a><figcaption>Structure of the oxidising agent <a href="/wiki/2-Iodoxybenzoic_acid" title="2-Iodoxybenzoic acid">2-iodoxybenzoic acid</a></figcaption></figure> Organoiodine compounds have been fundamental in the development of organic synthesis, such as in the <a href="/wiki/Hofmann_elimination" title="Hofmann elimination">Hofmann elimination</a> of <a href="/wiki/Amine" title="Amine">amines</a>,<a href="#cite_note-67">[66]</a> the <a href="/wiki/Williamson_ether_synthesis" title="Williamson ether synthesis">Williamson ether synthesis</a>,<a href="#cite_note-68">[67]</a> the <a href="/wiki/Wurtz_reaction" title="Wurtz reaction">Wurtz coupling reaction</a>,<a href="#cite_note-69">[68]</a> and in <a href="/wiki/Grignard_reagent" title="Grignard reagent">Grignard reagents</a>.<a href="#cite_note-70">[69]</a> The <a href="/wiki/Carbon" title="Carbon">carbon</a>–iodine bond is a common functional group that forms part of core <a href="/wiki/Organic_chemistry" title="Organic chemistry">organic chemistry</a>; formally, these compounds may be thought of as organic derivatives of the <a href="/wiki/Iodide" title="Iodide">iodide anion</a>. The simplest <a href="/wiki/Organoiodine_chemistry" title="Organoiodine chemistry">organoiodine compounds</a>, <a href="/wiki/Organoiodine_chemistry" title="Organoiodine chemistry">alkyl iodides</a>, may be synthesised by the reaction of <a href="/wiki/Alcohol_(chemistry)" title="Alcohol (chemistry)">alcohols</a> with <a href="/wiki/Phosphorus_triiodide" title="Phosphorus triiodide">phosphorus triiodide</a>; these may then be used in <a href="/wiki/Nucleophilic_substitution" title="Nucleophilic substitution">nucleophilic substitution</a> reactions, or for preparing <a href="/wiki/Grignard_reagent" title="Grignard reagent">Grignard reagents</a>. The C–I bond is the weakest of all the carbon–halogen bonds due to the minuscule difference in electronegativity between carbon (2.55) and iodine (2.66). As such, iodide is the best <a href="/wiki/Leaving_group" title="Leaving group">leaving group</a> among the halogens, to such an extent that many organoiodine compounds turn yellow when stored over time due to decomposition into elemental iodine; as such, they are commonly used in <a href="/wiki/Organic_synthesis" title="Organic synthesis">organic synthesis</a>, because of the easy formation and cleavage of the C–I bond.<a href="#cite_note-71">[70]</a> They are also significantly denser than the other organohalogen compounds thanks to the high atomic weight of iodine.<a href="#cite_note-blanksby-72">[71]</a> A few organic oxidising agents like the <a href="/wiki/Hypervalent_organoiodine_compounds" title="Hypervalent organoiodine compounds">iodanes</a> contain iodine in a higher oxidation state than −1, such as <a href="/wiki/2-Iodoxybenzoic_acid" title="2-Iodoxybenzoic acid">2-iodoxybenzoic acid</a>, a common reagent for the oxidation of alcohols to <a href="/wiki/Aldehyde" title="Aldehyde">aldehydes</a>,<a href="#cite_note-73">[72]</a> and <a href="/wiki/Iodobenzene_dichloride" title="Iodobenzene dichloride">iodobenzene dichloride</a> (PhICl2), used for the selective chlorination of <a href="/wiki/Alkene" title="Alkene">alkenes</a> and <a href="/wiki/Alkyne" title="Alkyne">alkynes</a>.<a href="#cite_note-74">[73]</a> One of the more well-known uses of organoiodine compounds is the so-called <a href="/wiki/Haloform_reaction" title="Haloform reaction">iodoform test</a>, where <a href="/wiki/Iodoform" title="Iodoform">iodoform</a> (CHI3) is produced by the exhaustive iodination of a <a href="/wiki/Ketone" title="Ketone">methyl ketone</a> (or another compound capable of being oxidised to a methyl ketone), as follows:<a href="#cite_note-March-75">[74]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"><a href="/wiki/File:Iodoform_synthesis.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0f/Iodoform_synthesis.svg/450px-Iodoform_synthesis.svg.png" decoding="async" width="450" height="207" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/0f/Iodoform_synthesis.svg/675px-Iodoform_synthesis.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/0f/Iodoform_synthesis.svg/900px-Iodoform_synthesis.svg.png 2x" data-file-width="620" data-file-height="285" /></a></div> Some drawbacks of using organoiodine compounds as compared to organochlorine or organobromine compounds is the greater expense and toxicity of the iodine derivatives, since iodine is expensive and organoiodine compounds are stronger alkylating agents.<a href="#cite_note-76">[75]</a> For example, <a href="/wiki/Iodoacetamide" title="Iodoacetamide">iodoacetamide</a> and <a href="/wiki/Iodoacetic_acid" title="Iodoacetic acid">iodoacetic acid</a> denature proteins by irreversibly alkylating <a href="/wiki/Cysteine" title="Cysteine">cysteine</a> residues and preventing the reformation of <a href="/wiki/Disulfide" title="Disulfide">disulfide</a> linkages.<a href="#cite_note-77">[76]</a> Halogen exchange to produce iodoalkanes by the <a href="/wiki/Finkelstein_reaction" title="Finkelstein reaction">Finkelstein reaction</a> is slightly complicated by the fact that iodide is a better leaving group than chloride or bromide. The difference is nevertheless small enough that the reaction can be driven to completion by exploiting the differential solubility of halide salts, or by using a large excess of the halide salt.<a href="#cite_note-March-75">[74]</a> In the classic Finkelstein reaction, an <a href="/wiki/Organochlorine_chemistry" title="Organochlorine chemistry">alkyl chloride</a> or an <a href="/wiki/Organobromine_chemistry" title="Organobromine chemistry">alkyl bromide</a> is converted to an <a href="/wiki/Organoiodine_chemistry" title="Organoiodine chemistry">alkyl iodide</a> by treatment with a solution of <a href="/wiki/Sodium_iodide" title="Sodium iodide">sodium iodide</a> in <a href="/wiki/Acetone" title="Acetone">acetone</a>. Sodium iodide is soluble in acetone and <a href="/wiki/Sodium_chloride" title="Sodium chloride">sodium chloride</a> and <a href="/wiki/Sodium_bromide" title="Sodium bromide">sodium bromide</a> are not.<a href="#cite_note-78">[77]</a> The reaction is driven toward products by <a href="/wiki/Law_of_mass_action" title="Law of mass action">mass action</a> due to the precipitation of the insoluble salt.<a href="#cite_note-79">[78]</a><a href="#cite_note-80">[79]</a> <div class="mw-heading mw-heading2"><h2 id="Occurrence_and_production">Occurrence and production</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=12" title="Edit section: Occurrence and production">edit</a>]</div> Iodine is the least abundant of the stable halogens, comprising only 0.46 <a href="/wiki/Parts-per_notation" title="Parts-per notation">parts per million</a> of Earth's crustal rocks (compare: <a href="/wiki/Fluorine" title="Fluorine">fluorine</a>: 544 ppm, <a href="/wiki/Chlorine" title="Chlorine">chlorine</a>: 126 ppm, <a href="/wiki/Bromine" title="Bromine">bromine</a>: 2.5 ppm) making it the 60th most abundant element.<a href="#cite_note-Greenwood795-81">[80]</a> Iodide minerals are rare, and most deposits that are concentrated enough for economical extraction are iodate minerals instead. Examples include <a href="/wiki/Calcium_iodate" title="Calcium iodate">lautarite</a>, Ca(IO3)2, and dietzeite, 7Ca(IO3)2·8CaCrO4.<a href="#cite_note-Greenwood795-81">[80]</a> These are the minerals that occur as trace impurities in the <a href="/wiki/Caliche" title="Caliche">caliche</a>, found in <a href="/wiki/Chile" title="Chile">Chile</a>, whose main product is <a href="/wiki/Sodium_nitrate" title="Sodium nitrate">sodium nitrate</a>. In total, they can contain at least 0.02% and at most 1% iodine by mass.<a href="#cite_note-Elzea-82">[81]</a> <a href="/wiki/Sodium_iodate" title="Sodium iodate">Sodium iodate</a> is extracted from the caliche and reduced to iodide by <a href="/wiki/Sodium_bisulfite" title="Sodium bisulfite">sodium bisulfite</a>. This solution is then reacted with freshly extracted iodate, resulting in <a href="/wiki/Comproportionation" title="Comproportionation">comproportionation</a> to iodine, which may be filtered off.<a href="#cite_note-Greenwood800-24">[23]</a> The caliche was the main source of iodine in the 19th century and continues to be important today, replacing <a href="/wiki/Kelp" title="Kelp">kelp</a> (which is no longer an economically viable source),<a href="#cite_note-83">[82]</a> but in the late 20th century <a href="/wiki/Brine" title="Brine">brines</a> emerged as a comparable source. The Japanese <a href="/wiki/Minami_Kant%C5%8D_gas_field" title="Minami Kantō gas field">Minami Kantō gas field</a> east of <a href="/wiki/Tokyo" title="Tokyo">Tokyo</a> and the American <a href="/wiki/Anadarko_Basin" title="Anadarko Basin">Anadarko Basin</a> gas field in northwest <a href="/wiki/Oklahoma" title="Oklahoma">Oklahoma</a> are the two largest such sources. The brine is hotter than 60 °C from the depth of the source. The brine is first <a href="/wiki/List_of_purification_methods_in_chemistry" title="List of purification methods in chemistry">purified</a> and acidified using <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a>, then the iodide present is oxidised to iodine with chlorine. An iodine solution is produced, but is dilute and must be concentrated. Air is blown into the solution to <a href="/wiki/Evaporation" title="Evaporation">evaporate</a> the iodine, which is passed into an absorbing tower, where <a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a> reduces the iodine. The <a href="/wiki/Hydrogen_iodide" title="Hydrogen iodide">hydrogen iodide</a> (HI) is reacted with chlorine to precipitate the iodine. After filtering and purification the iodine is packed.<a href="#cite_note-Elzea-82">[81]</a><a href="#cite_note-84">[83]</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"> 2 HI + Cl2 → I2↑ + 2 HCl</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"> I2 + 2 H2O + SO2 → 2 HI + H2SO4</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r996643573"><div class="block-indent"> 2 HI + Cl2 → I2↓ + 2 HCl</div> These sources ensure that Chile and Japan are the largest producers of iodine today.<a href="#cite_note-Greenwood795-81">[80]</a> Alternatively, the brine may be treated with <a href="/wiki/Silver_nitrate" title="Silver nitrate">silver nitrate</a> to precipitate out iodine as <a href="/wiki/Silver_iodide" title="Silver iodide">silver iodide</a>, which is then decomposed by reaction with iron to form metallic silver and a solution of <a href="/wiki/Iron(II)_iodide" title="Iron(II) iodide">iron(II) iodide</a>. The iodine is then liberated by displacement with <a href="/wiki/Chlorine" title="Chlorine">chlorine</a>.<a href="#cite_note-Greenwood799-85">[84]</a> <div class="mw-heading mw-heading2"><h2 id="Applications">Applications</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=13" title="Edit section: Applications">edit</a>]</div> About half of all produced iodine goes into various <a href="/wiki/Organoiodine_chemistry" title="Organoiodine chemistry">organoiodine compounds</a>, another 15% remains as the pure element, another 15% is used to form <a href="/wiki/Potassium_iodide" title="Potassium iodide">potassium iodide</a>, and another 15% for other <a href="/wiki/Iodine_compounds" title="Iodine compounds">inorganic iodine compounds</a>.<a href="#cite_note-Greenwood800-24">[23]</a> Among the major uses of iodine compounds are <a href="/wiki/Catalysis" title="Catalysis">catalysts</a>, animal feed supplements, stabilisers, dyes, colourants and pigments, pharmaceutical, sanitation (from <a href="/wiki/Tincture_of_iodine" title="Tincture of iodine">tincture of iodine</a>), and photography; minor uses include <a href="/wiki/Smog_tower" title="Smog tower">smog inhibition</a>, <a href="/wiki/Cloud_seeding" title="Cloud seeding">cloud seeding</a>, and various uses in <a href="/wiki/Analytical_chemistry" title="Analytical chemistry">analytical chemistry</a>.<a href="#cite_note-Greenwood800-24">[23]</a> <div class="mw-heading mw-heading3"><h3 id="X-ray_imaging">X-ray imaging</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=14" title="Edit section: X-ray imaging">edit</a>]</div> As an element with high <a href="/wiki/Electron_density" title="Electron density">electron density</a> and atomic number, iodine efficiently absorbs X-rays. X-ray <a href="/wiki/Radiocontrast_agent" title="Radiocontrast agent">radiocontrast</a> agents is the top application for iodine.<a href="#cite_note-Ullmann-86">[85]</a> In this application, Organoiodine compounds are injected intravenously. This application is often in conjunction with advanced X-ray techniques such as <a href="/wiki/Angiography" title="Angiography">angiography</a> and <a href="/wiki/CT_scan" title="CT scan">CT scanning</a>. At present, all water-soluble radiocontrast agents rely on <a href="/wiki/Iodinated_contrast" title="Iodinated contrast">iodine-containing compounds</a>. Iodine absorbs X-rays with energies lessthan 33.3 keV due to the <a href="/wiki/Photoelectric_effect" title="Photoelectric effect">photoelectric effect</a> of the innermost electrons.<a href="#cite_note-87">[86]</a> <div class="mw-heading mw-heading3"><h3 id="Biocide">Biocide</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=15" title="Edit section: Biocide">edit</a>]</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/Iodine_(medical_use)" title="Iodine (medical use)">Iodine (medical use)</a></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Diatrizoic_acid.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Diatrizoic_acid.svg/220px-Diatrizoic_acid.svg.png" decoding="async" width="220" height="172" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Diatrizoic_acid.svg/330px-Diatrizoic_acid.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Diatrizoic_acid.svg/440px-Diatrizoic_acid.svg.png 2x" data-file-width="750" data-file-height="588" /></a><figcaption><a href="/wiki/Diatrizoate" title="Diatrizoate">Diatrizoic acid</a>, an iodine-containing radio<a href="/wiki/Contrast_agent" title="Contrast agent">contrast agent</a></figcaption></figure> Use of iodine as a biocide represents a major application of the element, ranked 2nd by weight.<a href="#cite_note-Ullmann-86">[85]</a> Elemental iodine (I2) is used as an <a href="/wiki/Antiseptic" title="Antiseptic">antiseptic</a> in medicine.<a href="#cite_note-WHO2008-88">[87]</a> A number of water-soluble compounds, from <a href="/wiki/Triiodide" title="Triiodide">triiodide</a> (I3−, generated in situ by adding <a href="/wiki/Iodide" title="Iodide">iodide</a> to poorly water-soluble elemental iodine) to various <a href="/wiki/Iodophor" title="Iodophor">iodophors</a>, slowly decompose to release I2 when applied.<a href="#cite_note-89">[88]</a> <div class="mw-heading mw-heading3"><h3 id="Optical_polarizing_films">Optical polarizing films</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=16" title="Edit section: Optical polarizing films">edit</a>]</div> <a href="/wiki/Thin-film-transistor_liquid_crystal_display" class="mw-redirect" title="Thin-film-transistor liquid crystal display">Thin-film-transistor liquid crystal displays</a> rely on <a href="/wiki/Polarization_(waves)" title="Polarization (waves)"> polarization</a>. The liquid crystal transistor is sandwiched between two polarizing films and illuminated from behind. The two films prevent light transmission unless the transistor in the middle of the sandwich rotates the light.<a href="#cite_note-90">[89]</a> Iodine-impregnated polymer films are used in <a href="/wiki/Polarization_(waves)" title="Polarization (waves)"> polarizing</a> optical components with the highest transmission and degree of polarization.<a href="#cite_note-91">[90]</a> <div class="mw-heading mw-heading3"><h3 id="Co-catalyst">Co-catalyst</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=17" title="Edit section: Co-catalyst">edit</a>]</div> Another significant use of iodine is as a cocatalyst for the production of <a href="/wiki/Acetic_acid" title="Acetic acid">acetic acid</a> by the <a href="/wiki/Monsanto_process" title="Monsanto process">Monsanto</a> and <a href="/wiki/Cativa_process" title="Cativa process">Cativa processes</a>. In these technologies, <a href="/wiki/Hydroiodic_acid" title="Hydroiodic acid">hydroiodic acid</a> converts the <a href="/wiki/Methanol" title="Methanol">methanol</a> feedstock into methyl iodide, which undergoes <a href="/wiki/Carbonylation" title="Carbonylation">carbonylation</a>. Hydrolysis of the resulting acetyl iodide regenerates hydroiodic acid and gives acetic acid. The majority of acetic acid is produced by these approaches.<a href="#cite_note-UllmannAA-92">[91]</a><a href="#cite_note-93">[92]</a> <div class="mw-heading mw-heading3"><h3 id="Nutrition">Nutrition</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=18" title="Edit section: Nutrition">edit</a>]</div> Salts of iodide and iodate are used extensively in human and animal nutrition. This application reflects the status of iodide as an <a href="/wiki/Essential_element" class="mw-redirect" title="Essential element">essential element</a>, being required for two hormones. The production of <a href="/wiki/Ethylenediamine_dihydroiodide" title="Ethylenediamine dihydroiodide">ethylenediamine dihydroiodide</a>, provided as a <a href="/wiki/Nutrition" title="Nutrition">nutritional supplement</a> for livestock, consumes a large portion of available iodine.<a href="#cite_note-Ullmann-86">[85]</a> Iodine is a component of <a href="/wiki/Iodised_salt" title="Iodised salt">iodised salt</a>. A saturated solution of <a href="/wiki/Potassium_iodide" title="Potassium iodide">potassium iodide</a> is used to treat acute <a href="/wiki/Hyperthyroidism" title="Hyperthyroidism">thyrotoxicosis</a>. It is also used to block uptake of <a href="/wiki/Iodine-131" title="Iodine-131">iodine-131</a> in the thyroid gland (see isotopes section above), when this isotope is used as part of radiopharmaceuticals (such as <a href="/wiki/Iobenguane" title="Iobenguane">iobenguane</a>) that are not targeted to the thyroid or thyroid-type tissues.<a href="#cite_note-94">[93]</a><a href="#cite_note-95">[94]</a> <div class="mw-heading mw-heading3"><h3 id="Others">Others</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=19" title="Edit section: Others">edit</a>]</div> Inorganic iodides find specialised uses. <a href="/wiki/Titanium" title="Titanium">Titanium</a>, <a href="/wiki/Zirconium" title="Zirconium">zirconium</a>, <a href="/wiki/Hafnium" title="Hafnium">hafnium</a>, and <a href="/wiki/Thorium" title="Thorium">thorium</a> are purified by the <a href="/wiki/Van_Arkel%E2%80%93de_Boer_process" title="Van Arkel–de Boer process">Van Arkel–de Boer process</a>, which involves the reversible formation of the tetraiodides of these elements. Silver iodide is a major ingredient to traditional photographic film. Thousands of kilograms of silver iodide are used annually for <a href="/wiki/Cloud_seeding" title="Cloud seeding">cloud seeding</a> to induce rain.<a href="#cite_note-Ullmann-86">[85]</a> The organoiodine compound <a href="/wiki/Erythrosine" title="Erythrosine">erythrosine</a> is an important food coloring agent. Perfluoroalkyl iodides are precursors to important surfactants, such as <a href="/wiki/Perfluorooctanesulfonic_acid" title="Perfluorooctanesulfonic acid">perfluorooctanesulfonic acid</a>.<a href="#cite_note-Ullmann-86">[85]</a> 125I is used as the <a href="/wiki/Radioactive_tracer" title="Radioactive tracer">radiolabel</a> in investigating which <a href="/wiki/Ligand_(biochemistry)" title="Ligand (biochemistry)">ligands</a> go to which <a href="/wiki/Pattern_recognition_receptor" title="Pattern recognition receptor">plant pattern recognition receptors</a> (PRRs).<a href="#cite_note-Boutrot-Zipfel-2017-96">[95]</a> An iodine based thermochemical cycle has been evaluated for hydrogen production using energy from nuclear paper.<a href="#cite_note-Corgnale-Review-2020-97">[96]</a> The cycle has three steps. At 120 °C (248 °F), iodine reacts with <a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a> and water to give hydrogen iodide and <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a>: <dl><dd><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle I_{2}+SO_{2}+2H_{2}O\rightarrow 2HI+H_{2}SO_{4}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <msub> <mi>I</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mo>+</mo> <mi>S</mi> <msub> <mi>O</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mo>+</mo> <mn>2</mn> <msub> <mi>H</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mi>O</mi> <mo stretchy="false">→</mo> <mn>2</mn> <mi>H</mi> <mi>I</mi> <mo>+</mo> <msub> <mi>H</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mi>S</mi> <msub> <mi>O</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>4</mn> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle I_{2}+SO_{2}+2H_{2}O\rightarrow 2HI+H_{2}SO_{4}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/a7ba74215a7445665d6fbcabb3c7abffd9a09f35" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:36.171ex; height:2.509ex;" alt="{\displaystyle I_{2}+SO_{2}+2H_{2}O\rightarrow 2HI+H_{2}SO_{4}}"></dd></dl> After a separation stage, at 830–850 °C (1,530–1,560 °F) sulfuric acid splits in sulfur dioxide and oxygen: <dl><dd><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle 2H_{2}SO_{4}\rightarrow 2SO_{2}+2H_{2}O+O_{2}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mn>2</mn> <msub> <mi>H</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mi>S</mi> <msub> <mi>O</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>4</mn> </mrow> </msub> <mo stretchy="false">→</mo> <mn>2</mn> <mi>S</mi> <msub> <mi>O</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mo>+</mo> <mn>2</mn> <msub> <mi>H</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mi>O</mi> <mo>+</mo> <msub> <mi>O</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle 2H_{2}SO_{4}\rightarrow 2SO_{2}+2H_{2}O+O_{2}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/12b4eec2f6aec36527b148cbd472d4becb602e34" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:32.008ex; height:2.509ex;" alt="{\displaystyle 2H_{2}SO_{4}\rightarrow 2SO_{2}+2H_{2}O+O_{2}}"></dd></dl> Hydrogen iodide, at 300–320 °C (572–608 °F), gives hydrogen and the initial element, iodine: <dl><dd><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle 2HI\rightarrow I_{2}+H_{2}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mn>2</mn> <mi>H</mi> <mi>I</mi> <mo stretchy="false">→</mo> <msub> <mi>I</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> <mo>+</mo> <msub> <mi>H</mi> <mrow class="MJX-TeXAtom-ORD"> <mn>2</mn> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle 2HI\rightarrow I_{2}+H_{2}}</annotation> </semantics> </math><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/c42d700bfd1be527af3d63b1e3cd2bdd727fcc93" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:15.915ex; height:2.509ex;" alt="{\displaystyle 2HI\rightarrow I_{2}+H_{2}}"></dd></dl> The yield of the cycle (ratio between lower heating value of the produced hydrogen and the consumed energy for its production, is approximately 38%. As of 2020<a class="external text" href="https://en.wikipedia.org/w/index.php?title=Iodine&action=edit">[update]</a>, the cycle is not a competitive means of producing hydrogen.<a href="#cite_note-Corgnale-Review-2020-97">[96]</a> <div class="mw-heading mw-heading2"><h2 id="Spectroscopy">Spectroscopy</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=20" title="Edit section: Spectroscopy">edit</a>]</div> The spectrum of the iodine molecule, I2, consists of (not exclusively) tens of thousands of sharp spectral lines in the wavelength range 500–700 nm. It is therefore a commonly used wavelength reference (secondary standard). By measuring with a <a href="/wiki/Saturated_absorption_spectroscopy" title="Saturated absorption spectroscopy">spectroscopic Doppler-free technique</a> while focusing on one of these lines, the <a href="/wiki/Hyperfine_structure" title="Hyperfine structure">hyperfine</a> structure of the iodine molecule reveals itself. A line is now resolved such that either 15 components (from even rotational quantum numbers, Jeven), or 21 components (from odd rotational quantum numbers, Jodd) are measurable.<a href="#cite_note-98">[97]</a> Caesium iodide and thallium-doped sodium iodide are used in crystal <a href="/wiki/Scintillator" title="Scintillator">scintillators</a> for the detection of gamma rays. The efficiency is high and energy dispersive spectroscopy is possible, but the resolution is rather poor. <div class="mw-heading mw-heading2"><h2 id="Chemical_analysis">Chemical analysis</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=21" title="Edit section: Chemical analysis">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Testing_seed_for_starch.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c6/Testing_seed_for_starch.jpg/220px-Testing_seed_for_starch.jpg" decoding="async" width="220" height="170" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c6/Testing_seed_for_starch.jpg/330px-Testing_seed_for_starch.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c6/Testing_seed_for_starch.jpg/440px-Testing_seed_for_starch.jpg 2x" data-file-width="860" data-file-height="664" /></a><figcaption>Testing a seed for starch with a solution of iodine</figcaption></figure> The iodide and iodate anions can be used for quantitative volumetric analysis, for example in <a href="/wiki/Iodometry" title="Iodometry">iodometry</a>. Iodine and starch form a blue complex, and this reaction is often used to test for either starch or iodine and as an <a href="/wiki/Redox_indicator" title="Redox indicator">indicator</a> in iodometry. The iodine test for starch is still used to detect <a href="/wiki/Counterfeit" title="Counterfeit">counterfeit</a> banknotes printed on starch-containing paper.<a href="#cite_note-Emsley-99">[98]</a> The <a href="/wiki/Iodine_value" title="Iodine value">iodine value</a> is the mass of iodine in grams that is consumed by 100 grams of a <a href="/wiki/Chemical_substance" title="Chemical substance">chemical substance</a> typically fats or oils. Iodine numbers are often used to determine the amount of unsaturation in <a href="/wiki/Fatty_acid" title="Fatty acid">fatty acids</a>. This unsaturation is in the form of <a href="/wiki/Double_bond" title="Double bond">double bonds</a>, which react with iodine compounds. <a href="/wiki/Potassium_tetraiodomercurate(II)" title="Potassium tetraiodomercurate(II)">Potassium tetraiodomercurate(II)</a>, K2HgI4, is also known as Nessler's reagent. It is once was used as a sensitive spot test for <a href="/wiki/Ammonia" title="Ammonia">ammonia</a>. Similarly, <a href="/wiki/Mayer%27s_reagent" title="Mayer's reagent">Mayer's reagent</a> (potassium tetraiodomercurate(II) solution) is used as a precipitating reagent to test for <a href="/wiki/Alkaloid" title="Alkaloid">alkaloids</a>.<a href="#cite_note-100">[99]</a> Aqueous alkaline iodine solution is used in the <a href="/wiki/Iodoform" title="Iodoform">iodoform</a> test for <a href="/wiki/Ketone" title="Ketone">methyl ketones</a>.<a href="#cite_note-March-75">[74]</a> <div class="mw-heading mw-heading2"><h2 id="Biological_role">Biological role</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=22" title="Edit section: Biological role">edit</a>]</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/Iodine_in_biology" title="Iodine in biology">Iodine in biology</a></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Thyroid_system.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d1/Thyroid_system.svg/260px-Thyroid_system.svg.png" decoding="async" width="260" height="301" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d1/Thyroid_system.svg/390px-Thyroid_system.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d1/Thyroid_system.svg/520px-Thyroid_system.svg.png 2x" data-file-width="871" data-file-height="1010" /></a><figcaption>The <a href="/wiki/Thyroid" title="Thyroid">thyroid</a> system of the thyroid hormones <a href="/wiki/Triiodothyronine" title="Triiodothyronine">T3</a> and <a href="/wiki/Levothyroxine" title="Levothyroxine">T4</a></figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Carte_iodurie_france_%C2%B5g_par_jour_d%27apr%C3%A8s_Mornex_1987_Le_Guen_2000.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/15/Carte_iodurie_france_%C2%B5g_par_jour_d%27apr%C3%A8s_Mornex_1987_Le_Guen_2000.jpg/260px-Carte_iodurie_france_%C2%B5g_par_jour_d%27apr%C3%A8s_Mornex_1987_Le_Guen_2000.jpg" decoding="async" width="260" height="345" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/15/Carte_iodurie_france_%C2%B5g_par_jour_d%27apr%C3%A8s_Mornex_1987_Le_Guen_2000.jpg/390px-Carte_iodurie_france_%C2%B5g_par_jour_d%27apr%C3%A8s_Mornex_1987_Le_Guen_2000.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/15/Carte_iodurie_france_%C2%B5g_par_jour_d%27apr%C3%A8s_Mornex_1987_Le_Guen_2000.jpg/520px-Carte_iodurie_france_%C2%B5g_par_jour_d%27apr%C3%A8s_Mornex_1987_Le_Guen_2000.jpg 2x" data-file-width="665" data-file-height="882" /></a><figcaption>Comparison of the iodine content in urine in France (in microgramme/day), for some regions and departments (average levels of urine iodine, measured in micrograms per liter at the end of the twentieth century (1980 to 2000))<a href="#cite_note-101">[100]</a></figcaption></figure> Iodine is an <a href="/wiki/Mineral_(nutrient)" title="Mineral (nutrient)">essential element</a> for life and, at atomic number Z = 53, is the heaviest element commonly needed by living organisms. (<a href="/wiki/Lanthanum" title="Lanthanum">Lanthanum</a> and the other <a href="/wiki/Lanthanide" title="Lanthanide">lanthanides</a>, as well as <a href="/wiki/Tungsten" title="Tungsten">tungsten</a> with Z = 74 and <a href="/wiki/Uranium" title="Uranium">uranium</a> with Z = 92, are used by a few microorganisms.<a href="#cite_note-102">[101]</a><a href="#cite_note-103">[102]</a><a href="#cite_note-104">[103]</a>) It is required for the synthesis of the growth-regulating thyroid hormones <a href="/wiki/Levothyroxine" title="Levothyroxine">tetraiodothyronine</a> and <a href="/wiki/Triiodothyronine" title="Triiodothyronine">triiodothyronine</a> (T4 and T3 respectively, named after their number of iodine atoms). A deficiency of iodine leads to decreased production of T3 and T4 and a concomitant enlargement of the <a href="/wiki/Thyroid" title="Thyroid">thyroid tissue</a> in an attempt to obtain more iodine, causing the disease <a href="/wiki/Goitre" title="Goitre">goitre</a>. The major form of thyroid hormone in the blood is tetraiodothyronine (T4), which has a longer life than triiodothyronine (T3). In humans, the ratio of T4 to T3 released into the blood is between 14:1 and 20:1. T4 is converted to the active T3 (three to four times more potent than T4) within <a href="/wiki/Cell_(biology)" title="Cell (biology)">cells</a> by <a href="/wiki/Deiodinase" title="Deiodinase">deiodinases</a> (5'-iodinase). These are further processed by <a href="/wiki/Decarboxylation" title="Decarboxylation">decarboxylation</a> and deiodination to produce <a href="/wiki/3-Iodothyronamine" title="3-Iodothyronamine">iodothyronamine</a> (T1a) and <a href="/wiki/Thyronamine" title="Thyronamine">thyronamine</a> (T0a'). All three isoforms of the deiodinases are <a href="/wiki/Selenium" title="Selenium">selenium</a>-containing enzymes; thus metallic selenium is needed for triiodothyronine and tetraiodothyronine production.<a href="#cite_note-105">[104]</a> Iodine accounts for 65% of the molecular weight of T4 and 59% of T3. Fifteen to 20 mg of iodine is concentrated in thyroid tissue and hormones, but 70% of all iodine in the body is found in other tissues, including mammary glands, <a href="/wiki/Eye" title="Eye">eyes</a>, gastric mucosa, thymus, <a href="/wiki/Cerebrospinal_fluid" title="Cerebrospinal fluid">cerebrospinal fluid</a>, choroid plexus, arteries, <a href="/wiki/Cervix" title="Cervix">cervix</a>, salivary glands. During pregnancy, the <a href="/wiki/Placenta" title="Placenta">placenta</a> is able to store and accumulate iodine.<a href="#cite_note-106">[105]</a><a href="#cite_note-107">[106]</a> In the cells of those tissues, iodine enters directly by <a href="/wiki/Sodium/iodide_cotransporter" title="Sodium/iodide cotransporter">sodium-iodide symporter</a> (NIS). The action of iodine in mammal tissues is related to fetal and neonatal development, and in the other tissues, it is known.<a href="#cite_note-Patrick2008-108">[107]</a> <div class="mw-heading mw-heading3"><h3 id="Dietary_recommendations_and_intake">Dietary recommendations and intake</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=23" title="Edit section: Dietary recommendations and intake">edit</a>]</div> The daily levels of intake recommended by the <a href="/wiki/United_States" title="United States">United States</a> <a href="/wiki/National_Academy_of_Medicine" title="National Academy of Medicine">National Academy of Medicine</a> are between 110 and 130 <a href="/wiki/Microgram" title="Microgram">μg</a> for infants up to 12 months, 90 μg for children up to eight years, 130 μg for children up to 13 years, 150 μg for adults, 220 μg for pregnant women and 290 μg for lactating women.<a href="#cite_note-lpi-8">[7]</a><a href="#cite_note-109">[108]</a> The Tolerable Upper Intake Level (TUIL) for adults is 1,100 μg/day.<a href="#cite_note-InstituteofMedicine-110">[109]</a> This upper limit was assessed by analyzing the effect of supplementation on <a href="/wiki/Thyroid-stimulating_hormone" title="Thyroid-stimulating hormone">thyroid-stimulating hormone</a>.<a href="#cite_note-Patrick2008-108">[107]</a> The <a href="/wiki/European_Food_Safety_Authority" title="European Food Safety Authority">European Food Safety Authority</a> (EFSA) refers to the collective set of information as Dietary Reference Values, with Population Reference Intake (PRI) instead of RDA, and Average Requirement instead of EAR; AI and UL are defined the same as in the United States. For women and men ages 18 and older, the PRI for iodine is set at 150 μg/day; the PRI during pregnancy and lactation is 200 μg/day. For children aged 1–17 years, the PRI increases with age from 90 to 130 μg/day. These PRIs are comparable to the U.S. RDAs with the exception of that for lactation.<a href="#cite_note-111">[110]</a> The thyroid gland needs 70 μg/day of iodine to synthesise the requisite daily amounts of T4 and T3.<a href="#cite_note-lpi-8">[7]</a> The higher recommended daily allowance levels of iodine seem necessary for optimal function of a number of body systems, including <a href="/wiki/Mammary_gland" title="Mammary gland">mammary glands</a>, <a href="/wiki/Gastric_mucosa" title="Gastric mucosa">gastric mucosa</a>, <a href="/wiki/Salivary_gland" title="Salivary gland">salivary glands</a>, <a href="/wiki/Brain_cell" title="Brain cell">brain cells</a>, <a href="/wiki/Choroid_plexus" title="Choroid plexus">choroid plexus</a>, <a href="/wiki/Thymus" title="Thymus">thymus</a>, <a href="/wiki/Artery" title="Artery">arteries</a>.<a href="#cite_note-lpi-8">[7]</a><a href="#cite_note-112">[111]</a><a href="#cite_note-113">[112]</a><a href="#cite_note-Venturi,_Sebastiano_2014_185–205-114">[113]</a> Natural food sources of iodine include <a href="/wiki/Seafood" title="Seafood">seafood</a> which contains <a href="/wiki/Fish" title="Fish">fish</a>, <a href="/wiki/Seaweed" title="Seaweed">seaweeds</a>, <a href="/wiki/Kelp" title="Kelp">kelp</a>, <a href="/wiki/Shellfish" title="Shellfish">shellfish</a> and other <a href="/wiki/Food" title="Food">foods</a> which contain <a href="/wiki/Dairy_product" title="Dairy product">dairy products</a>, <a href="/wiki/Eggs_as_food" title="Eggs as food">eggs</a>, <a href="/wiki/Meat" title="Meat">meats</a>, <a href="/wiki/Vegetable" title="Vegetable">vegetables</a>, so long as the animals ate iodine richly, and the plants are grown on iodine-rich soil.<a href="#cite_note-115">[114]</a><a href="#cite_note-medlineplus002421-116">[115]</a> <a href="/wiki/Iodised_salt" title="Iodised salt">Iodised salt</a> is fortified with <a href="/wiki/Potassium_iodate" title="Potassium iodate">potassium iodate</a>, a salt of iodine, potassium, oxygen.<a href="#cite_note-medlineplus002421-116">[115]</a><a href="#cite_note-American_Thyroid_Association-117">[116]</a><a href="#cite_note-118">[117]</a> As of 2000, the median intake of iodine from food in the United States was 240 to 300 μg/day for men and 190 to 210 μg/day for women.<a href="#cite_note-InstituteofMedicine-110">[109]</a> The general US population has adequate iodine nutrition,<a href="#cite_note-119">[118]</a><a href="#cite_note-Lueng-120">[119]</a> with lactating women and pregnant women having a mild risk of deficiency.<a href="#cite_note-Lueng-120">[119]</a> In Japan, consumption was considered much higher, ranging between 5,280 μg/day to 13,800 μg/day from <a href="/wiki/Wakame" title="Wakame">wakame</a> and <a href="/wiki/Kombu" title="Kombu">kombu</a> that are eaten,<a href="#cite_note-Patrick2008-108">[107]</a> both in the form of kombu and wakame and kombu and wakame <a href="/wiki/Umami" title="Umami">umami</a> <a href="/wiki/Extract" title="Extract">extracts</a> for <a href="/wiki/Stock_(food)" title="Stock (food)">soup stock</a> and <a href="/wiki/Potato_chip" title="Potato chip">potato chips</a>. However, new studies suggest that Japan's consumption is closer to 1,000–3,000 μg/day.<a href="#cite_note-121">[120]</a> The adult UL in Japan was last revised to 3,000 μg/day in 2015.<a href="#cite_note-122">[121]</a> After iodine fortification programs such as iodisation of <a href="/wiki/Sodium_chloride" title="Sodium chloride">salt</a> have been done, some cases of iodine-induced <a href="/wiki/Hyperthyroidism" title="Hyperthyroidism">hyperthyroidism</a> have been observed (so-called <a href="/wiki/Jod-Basedow_phenomenon" title="Jod-Basedow phenomenon">Jod-Basedow phenomenon</a>). The condition occurs mainly in people above 40 years of age, and the risk is higher when iodine deficiency is high and the first rise in iodine consumption is high.<a href="#cite_note-123">[122]</a> <div class="mw-heading mw-heading3"><h3 id="Deficiency">Deficiency</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=24" title="Edit section: Deficiency">edit</a>]</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/Iodine_deficiency" title="Iodine deficiency">Iodine deficiency</a></div> In areas where there is little iodine in the diet,<a href="#cite_note-Dissanayake-124">[123]</a> which are remote inland areas and faraway mountainous areas where no iodine rich foods are eaten, <a href="/wiki/Iodine_deficiency" title="Iodine deficiency">iodine deficiency</a> gives rise to <a href="/wiki/Hypothyroidism" title="Hypothyroidism">hypothyroidism</a>, symptoms of which are <a href="/wiki/Fatigue" title="Fatigue">extreme fatigue</a>, <a href="/wiki/Goitre" title="Goitre">goitre</a>, <a href="/wiki/Intellectual_disability" title="Intellectual disability">mental slowing</a>, <a href="/wiki/Depression_(mood)" title="Depression (mood)">depression</a>, <a href="/wiki/Weight_gain" title="Weight gain">low weight gain</a>, and <a href="/wiki/Hypothermia" title="Hypothermia">low basal body temperatures</a>.<a href="#cite_note-125">[124]</a> Iodine deficiency is the leading cause of preventable <a href="/wiki/Intellectual_disability" title="Intellectual disability">intellectual disability</a>, a result that occurs primarily when babies or small children are rendered <a href="/wiki/Hypothyroidism" title="Hypothyroidism">hypothyroidic</a> by no iodine. The addition of iodine to salt has largely destroyed this problem in wealthier areas, but iodine deficiency remains a serious public health problem in poorer areas today.<a href="#cite_note-126">[125]</a> Iodine deficiency is also a problem in certain areas of all continents of the world. Information processing, fine motor skills, and visual problem solving are normalised by iodine repletion in iodine-deficient people.<a href="#cite_note-127">[126]</a> <div class="mw-heading mw-heading2"><h2 id="Precautions">Precautions</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=25" title="Edit section: Precautions">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="Toxicity">Toxicity</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=26" title="Edit section: Toxicity">edit</a>]</div> <style data-mw-deduplicate="TemplateStyles:r1084375498">.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%}</style> <table class="infobox ib-chembox"> <caption>Iodine </caption> <tbody><tr> <th colspan="2" style="background: #f8eaba; text-align: center;">Hazards </th></tr> <tr> <td colspan="2" style="text-align:left; background-color:#eaeaea;"><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>: </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-exclam.svg" class="mw-file-description" title="GHS07: Exclamation mark"><img alt="GHS07: Exclamation mark" src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c3/GHS-pictogram-exclam.svg/50px-GHS-pictogram-exclam.svg.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c3/GHS-pictogram-exclam.svg/75px-GHS-pictogram-exclam.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c3/GHS-pictogram-exclam.svg/100px-GHS-pictogram-exclam.svg.png 2x" data-file-width="512" data-file-height="512" /></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="H312: Harmful in contact with skin">H312</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="H332: Harmful if inhaled">H332</abbr>, <abbr class="abbr" title="H335: May cause respiratory irritation">H335</abbr>, <abbr class="abbr" title="H372: Causes damage to organs through prolonged or repeated exposure">H372</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="P261: Avoid breathing dust/fume/gas/mist/vapours/spray.">P261</abbr>, <abbr class="abbr" title="P273: Avoid release to the environment.">P273</abbr>, <abbr class="abbr" title="P280: Wear protective gloves/protective clothing/eye protection/face protection.">P280</abbr>, <abbr class="abbr" title="P305: IF IN EYES:">P305</abbr>, <abbr class="abbr" title="P314: Get Medical advice/attention if you feel unwell.">P314</abbr>, <abbr class="abbr" title="P338: Remove contact lenses if present and easy to do. Continue rinsing.">P338</abbr>, <abbr class="abbr" title="P351: Rinse cautiously with water for several minutes.">P351</abbr><a href="#cite_note-128">[127]</a> </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-129">[128]</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_7b3d73138c259557" /><map name="ImageMap_7b3d73138c259557"><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 hazards (white): no code" title="Special hazards (white): no code" /></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></div></div> </td></tr> </tbody></table><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical compound</div> Elemental iodine (I2) is <a href="/wiki/Toxicity" title="Toxicity">toxic</a> if taken orally undiluted. The lethal dose for an adult human is 30 mg/kg, which is about 2.1–2.4 grams for a human weighing 70 to 80 kg (even when experiments on rats demonstrated that these animals could survive after eating a 14000 mg/kg dose and are still living after that). Excess iodine is more <a href="/wiki/Cytotoxicity" title="Cytotoxicity">cytotoxic</a> in the presence of <a href="/wiki/Selenium_deficiency" title="Selenium deficiency">selenium deficiency</a>.<a href="#cite_note-130">[129]</a> Iodine supplementation in selenium-deficient populations is problematic for this reason.<a href="#cite_note-Patrick2008-108">[107]</a> The toxicity derives from its oxidizing properties, through which it denaturates proteins (including enzymes).<a href="#cite_note-131">[130]</a> Elemental iodine is also a skin irritant. Solutions with high elemental iodine concentration, such as <a href="/wiki/Tincture_of_iodine" title="Tincture of iodine">tincture of iodine</a> and <a href="/wiki/Lugol%27s_iodine" title="Lugol's iodine">Lugol's solution</a>, are capable of causing <a href="/wiki/Dermatotoxin" title="Dermatotoxin">tissue damage</a> if used in prolonged cleaning or antisepsis; similarly, liquid <a href="/wiki/Povidone-iodine" title="Povidone-iodine">Povidone-iodine</a> (Betadine) trapped against the skin resulted in chemical burns in some reported cases.<a href="#cite_note-Lowe-132">[131]</a> <div class="mw-heading mw-heading4"><h4 id="Occupational_exposure">Occupational exposure</h4>[<a href="/w/index.php?title=Iodine&action=edit&section=27" title="Edit section: Occupational exposure">edit</a>]</div> The U.S. <a href="/wiki/Occupational_Safety_and_Health_Administration" title="Occupational Safety and Health Administration">Occupational Safety and Health Administration</a> (OSHA) has set the legal limit (<a href="/wiki/Permissible_exposure_limit" title="Permissible exposure limit">Permissible exposure limit</a>) for iodine exposure in the workplace at 0.1 ppm (1 mg/m3) during an 8-hour workday. 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> (NIOSH) has set a <a href="/wiki/Recommended_exposure_limit" title="Recommended exposure limit">Recommended exposure limit</a> (REL) of 0.1 ppm (1 mg/m3) during an 8-hour workday. At levels of 2 ppm, iodine is <a href="/wiki/Immediately_dangerous_to_life_or_health" title="Immediately dangerous to life or health">immediately dangerous to life and health</a>.<a href="#cite_note-133">[132]</a> <div class="mw-heading mw-heading4"><h4 id="Allergic_reactions">Allergic reactions</h4>[<a href="/w/index.php?title=Iodine&action=edit&section=28" title="Edit section: Allergic reactions">edit</a>]</div> Some people develop a <a href="/wiki/Hypersensitivity" title="Hypersensitivity">hypersensitivity</a> to products and foods containing iodine. Applications of tincture of iodine or Betadine can cause rashes, sometimes severe.<a href="#cite_note-dermnet-134">[133]</a> <a href="https://en.wiktionary.org/wiki/parenteral" class="extiw" title="wikt:parenteral">Parenteral</a> use of iodine-based contrast agents (see above) can cause reactions ranging from a mild rash to fatal <a href="/wiki/Anaphylaxis" title="Anaphylaxis">anaphylaxis</a>. Such reactions have led to the misconception (widely held, even among physicians) that some people are allergic to iodine itself; even allergies to iodine-rich foods have been so construed.<a href="#cite_note-135">[134]</a> In fact, there has never been a confirmed report of a true iodine allergy, as an allergy to iodine or iodine salts is biologically impossible. Hypersensitivity reactions to products and foods containing iodine are apparently related to their other molecular components;<a href="#cite_note-ucsf-136">[135]</a> thus, a person who has demonstrated an allergy to one food or product containing iodine may not have an allergic reaction to another. Patients with various food allergies (fishes, shellfishes, eggs, milk, seaweeds, kelp, meats, vegetables, kombu, wakame) do not have an increased risk for a contrast medium hypersensitivity.<a href="#cite_note-pmid31153557-137">[136]</a><a href="#cite_note-ucsf-136">[135]</a> The patient's allergy history is relevant.<a href="#cite_note-138">[137]</a> <div style="clear:right;" class=""></div> <div class="mw-heading mw-heading3"><h3 id="US_DEA_List_I_status">US DEA List I status</h3>[<a href="/w/index.php?title=Iodine&action=edit&section=29" title="Edit section: US DEA List I status">edit</a>]</div> <a href="/wiki/Phosphorus" title="Phosphorus">Phosphorus</a> reduces iodine to <a href="/wiki/Hydroiodic_acid" title="Hydroiodic acid">hydroiodic acid</a>, which is a reagent effective for reducing <a href="/wiki/Ephedrine" title="Ephedrine">ephedrine</a> and <a href="/wiki/Pseudoephedrine" title="Pseudoephedrine">pseudoephedrine</a> to <a href="/wiki/Methamphetamine" title="Methamphetamine">methamphetamine</a>.<a href="#cite_note-139">[138]</a> For this reason, iodine was designated by the United States <a href="/wiki/Drug_Enforcement_Administration" title="Drug Enforcement Administration">Drug Enforcement Administration</a> as a <a href="/wiki/DEA_list_of_chemicals#List_I_chemicals" title="DEA list of chemicals">List I precursor chemical</a> under <a href="/wiki/Code_of_Federal_Regulations" title="Code of Federal Regulations">21 CFR 1310.02</a>.<a href="#cite_note-140">[139]</a> <div class="mw-heading mw-heading2"><h2 id="Notes">Notes</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=30" title="Edit section: Notes">edit</a>]</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 reflist-lower-alpha"> <div class="mw-references-wrap"><ol class="references"> <li id="cite_note-5"><a href="#cite_ref-5">^</a> The thermal expansion of crystalline iodine is <a href="/wiki/Anisotropy" title="Anisotropy">anisotropic</a>: the parameters (at 20 °C) for each axis are αa = 86.5×10−6/K, αb = 126×10−6/K, αc = 12.3×10−6/K, and αaverage = αV/3 = 74.9×10−6/K.<a href="#cite_note-Arblaster_2018-3">[3]</a> </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="References">References</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=31" title="Edit section: References">edit</a>]</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-1"><a href="#cite_ref-1">^</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 class="citation web cs1"><a rel="nofollow" class="external text" href="https://www.ciaaw.org/iodine.htm">"Standard Atomic Weights: Iodine"</a>. <a href="/wiki/Commission_on_Isotopic_Abundances_and_Atomic_Weights" title="Commission on Isotopic Abundances and Atomic Weights">CIAAW</a>. 1985.</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+Iodine&rft.pub=CIAAW&rft.date=1985&rft_id=https%3A%2F%2Fwww.ciaaw.org%2Fiodine.htm&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" 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 T, Irrgeher J, Benefield J, Böhlke JK, Chesson LA, Coplen TB, et al. (4 May 2022). <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%3AIodine" class="Z3988"> </li> <li id="cite_note-Arblaster_2018-3">^ <a href="#cite_ref-Arblaster_2018_3-0">a</a> <a href="#cite_ref-Arblaster_2018_3-1">b</a> <a href="#cite_ref-Arblaster_2018_3-2">c</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFArblaster2018" class="citation book cs1">Arblaster JW (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%3AIodine" class="Z3988"> </li> <li id="cite_note-4"><a href="#cite_ref-4">^</a> I(II) is known to exist in monoxide (IO); see <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFNikitin2008" class="citation journal cs1">Nikitin IV (31 August 2008). "Halogen monoxides". Russian Chemical Reviews. 77 (8): 739–749. <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/2008RuCRv..77..739N">2008RuCRv..77..739N</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1070%2FRC2008v077n08ABEH003788">10.1070/RC2008v077n08ABEH003788</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:250898175">250898175</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Russian+Chemical+Reviews&rft.atitle=Halogen+monoxides&rft.volume=77&rft.issue=8&rft.pages=739-749&rft.date=2008-08-31&rft_id=https%3A%2F%2Fapi.semanticscholar.org%2FCorpusID%3A250898175%23id-name%3DS2CID&rft_id=info%3Adoi%2F10.1070%2FRC2008v077n08ABEH003788&rft_id=info%3Abibcode%2F2008RuCRv..77..739N&rft.aulast=Nikitin&rft.aufirst=I+V&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-6"><a href="#cite_ref-6">^</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 Handbook of Chemistry and Physics 81st edition, CRC press. </li> <li id="cite_note-7"><a href="#cite_ref-7">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWeast1984" class="citation book cs1">Weast R (1984). CRC, <a href="/wiki/Handbook_of_Chemistry_and_Physics" class="mw-redirect" title="Handbook of Chemistry and Physics">Handbook of Chemistry and Physics</a>. 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%3AIodine" class="Z3988"> </li> <li id="cite_note-lpi-8">^ <a href="#cite_ref-lpi_8-0">a</a> <a href="#cite_ref-lpi_8-1">b</a> <a href="#cite_ref-lpi_8-2">c</a> <a href="#cite_ref-lpi_8-3">d</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="http://lpi.oregonstate.edu/mic/minerals/iodine">"Iodine"</a>. Micronutrient Information Center, <a href="/wiki/Linus_Pauling_Institute" title="Linus Pauling Institute">Linus Pauling Institute</a>, <a href="/wiki/Oregon_State_University" title="Oregon State University">Oregon State University</a>, Corvallis. 2015. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20150417055246/http://lpi.oregonstate.edu/mic/minerals/iodine">Archived</a> from the original on 17 April 2015. Retrieved 20 November 2017.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Iodine&rft.pub=Micronutrient+Information+Center%2C+Linus+Pauling+Institute%2C+Oregon+State+University%2C+Corvallis&rft.date=2015&rft_id=http%3A%2F%2Flpi.oregonstate.edu%2Fmic%2Fminerals%2Fiodine&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-9"><a href="#cite_ref-9">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFMcNeil_Jr2006" class="citation news cs1">McNeil Jr DG (16 December 2006). <a rel="nofollow" class="external text" href="https://query.nytimes.com/gst/fullpage.html?res=9E05E3D81231F935A25751C1A9609C8B63">"In Raising the World's I.Q., the Secret's in the Salt"</a>. The New York Times. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20100712011551/http://query.nytimes.com/gst/fullpage.html?res=9E05E3D81231F935A25751C1A9609C8B63">Archived</a> from the original on 12 July 2010. Retrieved 21 July 2009.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=The+New+York+Times&rft.atitle=In+Raising+the+World%27s+I.Q.%2C+the+Secret%27s+in+the+Salt&rft.date=2006-12-16&rft.aulast=McNeil+Jr&rft.aufirst=DG&rft_id=https%3A%2F%2Fquery.nytimes.com%2Fgst%2Ffullpage.html%3Fres%3D9E05E3D81231F935A25751C1A9609C8B63&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-WHO22nd-10"><a href="#cite_ref-WHO22nd_10-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWorld_Health_Organization2021" class="citation book cs1"><a href="/wiki/World_Health_Organization" title="World Health Organization">World Health Organization</a> (2021). World Health Organization model list of essential medicines: 22nd list (2021). Geneva: World Health Organization. <a href="/wiki/Hdl_(identifier)" class="mw-redirect" title="Hdl (identifier)">hdl</a>:<a rel="nofollow" class="external text" href="https://hdl.handle.net/10665%2F345533">10665/345533</a>. WHO/MHP/HPS/EML/2021.02.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=World+Health+Organization+model+list+of+essential+medicines%3A+22nd+list+%282021%29&rft.place=Geneva&rft.pub=World+Health+Organization&rft.date=2021&rft_id=info%3Ahdl%2F10665%2F345533&rft.au=World+Health+Organization&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-court-11">^ <a href="#cite_ref-court_11-0">a</a> <a href="#cite_ref-court_11-1">b</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFCourtois1813" class="citation journal cs1 cs1-prop-foreign-lang-source">Courtois B (1813). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=YGwri-w7sMAC&pg=RA2-PA304">"Découverte d'une substance nouvelle dans le Vareck"</a> [Discovery of a new substance in seaweed]. <a href="/wiki/Annales_de_chimie" class="mw-redirect" title="Annales de chimie">Annales de chimie</a> (in French). 88: 304–310.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Annales+de+chimie&rft.atitle=D%C3%A9couverte+d%27une+substance+nouvelle+dans+le+Vareck&rft.volume=88&rft.pages=304-310&rft.date=1813&rft.aulast=Courtois&rft.aufirst=B&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DYGwri-w7sMAC%26pg%3DRA2-PA304&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> In French, seaweed that had been washed onto the shore was called "varec", "varech", or "vareck", whence the English word "wrack". Later, "varec" also referred to the ashes of such seaweed: the ashes were used as a source of iodine and salts of sodium and potassium. </li> <li id="cite_note-12"><a href="#cite_ref-12">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSwain2005" class="citation journal cs1">Swain PA (2005). <a rel="nofollow" class="external text" href="https://web.archive.org/web/20100714110757/http://www.scs.uiuc.edu/~mainzv/HIST/awards/OPA%20Papers/2007-Swain.pdf">"Bernard Courtois (1777–1838) famed for discovering iodine (1811), and his life in Paris from 1798"</a> (PDF). Bulletin for the History of Chemistry. 30 (2): 103. Archived from <a rel="nofollow" class="external text" href="http://www.scs.uiuc.edu/~mainzv/HIST/awards/OPA%20Papers/2007-Swain.pdf">the original</a> (PDF) on 14 July 2010. Retrieved 2 April 2009.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Bulletin+for+the+History+of+Chemistry&rft.atitle=Bernard+Courtois+%281777%E2%80%931838%29+famed+for+discovering+iodine+%281811%29%2C+and+his+life+in+Paris+from+1798&rft.volume=30&rft.issue=2&rft.pages=103&rft.date=2005&rft.aulast=Swain&rft.aufirst=PA&rft_id=http%3A%2F%2Fwww.scs.uiuc.edu%2F~mainzv%2FHIST%2Fawards%2FOPA%2520Papers%2F2007-Swain.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-Greenwood794-13"><a href="#cite_ref-Greenwood794_13-0">^</a> Greenwood and Earnshaw, p. 794 </li> <li id="cite_note-vdK-14">^ <a href="#cite_ref-vdK_14-0">a</a> <a href="#cite_ref-vdK_14-1">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="http://elements.vanderkrogt.net/element.php?sym=i">"53 Iodine"</a>. Elements.vanderkrogt.net. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20100123001444/http://elements.vanderkrogt.net/element.php?sym=I">Archived</a> from the original on 23 January 2010. Retrieved 23 October 2016.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=53+Iodine&rft.pub=Elements.vanderkrogt.net&rft_id=http%3A%2F%2Felements.vanderkrogt.net%2Felement.php%3Fsym%3Di&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-15"><a href="#cite_ref-15">^</a> Desormes and Clément made their announcement at the Institut impérial de France on 29 November 1813; a summary of their announcement appeared in the Gazette nationale ou Le Moniteur Universel of 2 December 1813. See: <ul><li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREF(Staff)1813" class="citation journal cs1 cs1-prop-foreign-lang-source">(Staff) (2 December 1813). <a rel="nofollow" class="external text" href="https://www.retronews.fr/journal/gazette-nationale-ou-le-moniteur-universel/02-decembre-1813/149/1332251/2">"Institut Imperial de France"</a>. Le Moniteur Universel (in French) (336): 1344. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20221128171041/https://www.retronews.fr/journal/gazette-nationale-ou-le-moniteur-universel/02-decembre-1813/149/1332251/2">Archived</a> from the original on 28 November 2022. Retrieved 2 May 2021.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Le+Moniteur+Universel&rft.atitle=Institut+Imperial+de+France&rft.issue=336&rft.pages=1344&rft.date=1813-12-02&rft.au=%28Staff%29&rft_id=https%3A%2F%2Fwww.retronews.fr%2Fjournal%2Fgazette-nationale-ou-le-moniteur-universel%2F02-decembre-1813%2F149%2F1332251%2F2&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFChattaway1909" class="citation journal cs1">Chattaway FD (23 April 1909). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=Rco_AQAAIAAJ&pg=PA193">"The discovery of iodine"</a>. Chemical News and Journal of Industrial Science. 99 (2578): 193–195.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Chemical+News+and+Journal+of+Industrial+Science&rft.atitle=The+discovery+of+iodine&rft.volume=99&rft.issue=2578&rft.pages=193-195&rft.date=1909-04-23&rft.aulast=Chattaway&rft.aufirst=FD&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DRco_AQAAIAAJ%26pg%3DPA193&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"></li></ul> </li> <li id="cite_note-Gay-Lussac-16">^ <a href="#cite_ref-Gay-Lussac_16-0">a</a> <a href="#cite_ref-Gay-Lussac_16-1">b</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGay-Lussac1813" class="citation journal cs1 cs1-prop-foreign-lang-source">Gay-Lussac J (1813). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=YGwri-w7sMAC&pg=PA311">"Sur un nouvel acide formé avec la substance décourverte par M. Courtois"</a> [On a new acid formed by the substance discovered by Mr. Courtois]. Annales de Chimie (in French). 88: 311–318. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20240319070023/https://books.google.com/books?id=YGwri-w7sMAC&pg=PA311#v=onepage&q&f=false">Archived</a> from the original on 19 March 2024. Retrieved 2 May 2021.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Annales+de+Chimie&rft.atitle=Sur+un+nouvel+acide+form%C3%A9+avec+la+substance+d%C3%A9courverte+par+M.+Courtois&rft.volume=88&rft.pages=311-318&rft.date=1813&rft.aulast=Gay-Lussac&rft.aufirst=J&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DYGwri-w7sMAC%26pg%3DPA311&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </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="CITEREFGay-Lussac1813" class="citation journal cs1 cs1-prop-foreign-lang-source">Gay-Lussac J (1813). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=YGwri-w7sMAC&pg=PA319">"Sur la combination de l'iode avec d'oxigène"</a> [On the combination of iodine with oxygen]. Annales de Chimie (in French). 88: 319–321. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20240319070022/https://books.google.com/books?id=YGwri-w7sMAC&pg=PA319#v=onepage&q&f=false">Archived</a> from the original on 19 March 2024. Retrieved 2 May 2021.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Annales+de+Chimie&rft.atitle=Sur+la+combination+de+l%27iode+avec+d%27oxig%C3%A8ne&rft.volume=88&rft.pages=319-321&rft.date=1813&rft.aulast=Gay-Lussac&rft.aufirst=J&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DYGwri-w7sMAC%26pg%3DPA319&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-18"><a href="#cite_ref-18">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGay-Lussac1814" class="citation journal cs1 cs1-prop-foreign-lang-source">Gay-Lussac J (1814). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=Efms0Fri1CQC&pg=PA5">"Mémoire sur l'iode"</a> [Memoir on iodine]. Annales de Chimie (in French). 91: 5–160.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Annales+de+Chimie&rft.atitle=M%C3%A9moire+sur+l%27iode&rft.volume=91&rft.pages=5-160&rft.date=1814&rft.aulast=Gay-Lussac&rft.aufirst=J&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DEfms0Fri1CQC%26pg%3DPA5&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-19"><a href="#cite_ref-19">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFDavy1813" class="citation journal cs1 cs1-prop-foreign-lang-source"><a href="/wiki/Humphry_Davy" title="Humphry Davy">Davy H</a> (1813). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=YGwri-w7sMAC&pg=PA322">"Sur la nouvelle substance découverte par M. Courtois, dans le sel de Vareck"</a> [On the new substance discovered by Mr. Courtois in the salt of seaweed]. Annales de Chimie (in French). 88: 322–329. <a rel="nofollow" class="external text" href="https://web.archive.org/web/20240319070024/https://books.google.com/books?id=YGwri-w7sMAC&pg=PA322#v=onepage&q&f=false">Archived</a> from the original on 19 March 2024. 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Retrieved 30 June 2019.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Annalen+der+Chemie+und+Pharmacie&rft.atitle=Ueber+eine+neue+Klasse+organischer+Radicale&rft.volume=96&rft.issue=3&rft.pages=364-375&rft.date=1855&rft_id=info%3Adoi%2F10.1002%2Fjlac.18550960310&rft.aulast=Wurtz&rft.aufirst=A&rft_id=https%3A%2F%2Fzenodo.org%2Frecord%2F1427074&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> <li id="cite_note-70"><a href="#cite_ref-70">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFGrignard1900" class="citation journal cs1"><a href="/wiki/Victor_Grignard" title="Victor Grignard">Grignard V</a> (1900). <a rel="nofollow" class="external text" href="http://gallica.bnf.fr/ark:/12148/bpt6k3086n/f1322.table">"Sur quelques nouvelles combinaisons organométaliques du magnésium et leur application à des synthèses d'alcools et d'hydrocabures"</a>. 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Archived from <a rel="nofollow" class="external text" href="https://www.deadiversion.usdoj.gov/21cfr/cfr/1310/1310_02.htm">the original</a> on 17 October 2017. Retrieved 5 December 2019.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=PART+1310+-+Section+1310.02+Substances+covered&rft_id=https%3A%2F%2Fwww.deadiversion.usdoj.gov%2F21cfr%2Fcfr%2F1310%2F1310_02.htm&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIodine" class="Z3988"> </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="Bibliography">Bibliography</h2>[<a href="/w/index.php?title=Iodine&action=edit&section=32" title="Edit section: Bibliography">edit</a>]</div> <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 NN</a>, Earnshaw A (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%3AIodine" class="Z3988"></li></ul> <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 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.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="" 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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">Iodine 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/iodine" class="extiw" title="wikt:iodine">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/Iodine" class="extiw" title="c:Iodine">Media</a> from Commons</li><li class="sister-bar-item"><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikiquote-logo.svg/16px-Wikiquote-logo.svg.png" decoding="async" width="16" height="19" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikiquote-logo.svg/24px-Wikiquote-logo.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Wikiquote-logo.svg/32px-Wikiquote-logo.svg.png 2x" data-file-width="300" data-file-height="355" /><a href="https://en.wikiquote.org/wiki/Iodine" class="extiw" title="q:Iodine">Quotations</a> from Wikiquote</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/Special:Search/Iodine" class="extiw" title="s:Special:Search/Iodine">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/Iodine" class="extiw" title="b:Wikijunior:The Elements/Iodine">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/Iodine_atom" class="extiw" title="v:Iodine atom">Resources</a> from Wikiversity</li></ul></div> <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 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.navbox{display:none!important}}</style></div><div role="navigation" class="navbox" aria-labelledby="Periodic_table" 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 this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Periodic_table_(navbox)" title="Special:EditPage/Template:Periodic table (navbox)"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Periodic_table" style="font-size:114%;margin:0 4em"><a href="/wiki/Periodic_table" title="Periodic table">Periodic table</a></div></th></tr><tr><td colspan="2" class="navbox-list navbox-odd wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"> <table style="table-layout:fixed; width:100%;" aria-describedby="periodic-table-legend"> <tbody><tr> <td style="line-height:100%;"> </td> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Alkali_metal" title="Alkali metal">1</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Alkaline_earth_metal" title="Alkaline earth metal">2</a> </th> <td colspan="14"> </td> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_3_element" title="Group 3 element">3</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_4_element" title="Group 4 element">4</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_5_element" title="Group 5 element">5</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_6_element" title="Group 6 element">6</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_7_element" title="Group 7 element">7</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_8_element" title="Group 8 element">8</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_9_element" title="Group 9 element">9</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_10_element" title="Group 10 element">10</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_11_element" title="Group 11 element">11</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Group_12_element" title="Group 12 element">12</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Boron_group" title="Boron group">13</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Carbon_group" title="Carbon group">14</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Pnictogen" title="Pnictogen">15</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Chalcogen" title="Chalcogen">16</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Halogen" title="Halogen">17</a> </th> <th scope="col" style="background:transparent; font-weight:normal;"><a href="/wiki/Noble_gas" title="Noble gas">18</a> </th></tr> <tr> <th scope="row" style="background:transparent; 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; 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; border:none; ;"><a href="/wiki/Helium" title="Helium">He</a> </td></tr> <tr> <th scope="row" style="background:transparent; 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; border:none; ;"><a href="/wiki/Lithium" title="Lithium">Li</a> </td> <td title="Be, Beryllium" style="text-align:center; background-color:#ff9999; 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; border:none; ;"><a href="/wiki/Boron" title="Boron">B</a> </td> <td title="C, Carbon" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Carbon" title="Carbon">C</a> </td> <td title="N, Nitrogen" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Nitrogen" title="Nitrogen">N</a> </td> <td title="O, Oxygen" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Oxygen" title="Oxygen">O</a> </td> <td title="F, Fluorine" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Fluorine" title="Fluorine">F</a> </td> <td title="Ne, Neon" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Neon" title="Neon">Ne</a> </td></tr> <tr> <th scope="row" style="background:transparent; 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; border:none; ;"><a href="/wiki/Sodium" title="Sodium">Na</a> </td> <td title="Mg, Magnesium" style="text-align:center; background-color:#ff9999; 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; border:none; ;"><a href="/wiki/Aluminium" title="Aluminium">Al</a> </td> <td title="Si, Silicon" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Silicon" title="Silicon">Si</a> </td> <td title="P, Phosphorus" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Phosphorus" title="Phosphorus">P</a> </td> <td title="S, Sulfur" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Sulfur" title="Sulfur">S</a> </td> <td title="Cl, Chlorine" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Chlorine" title="Chlorine">Cl</a> </td> <td title="Ar, Argon" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Argon" title="Argon">Ar</a> </td></tr> <tr> <th scope="row" style="background:transparent; 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; border:none; ;"><a href="/wiki/Potassium" title="Potassium">K</a> </td> <td title="Ca, Calcium" style="text-align:center; background-color:#ff9999; 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; border:none; ;"><a href="/wiki/Scandium" title="Scandium">Sc</a> </td> <td title="Ti, Titanium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Titanium" title="Titanium">Ti</a> </td> <td title="V, Vanadium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Vanadium" title="Vanadium">V</a> </td> <td title="Cr, Chromium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Chromium" title="Chromium">Cr</a> </td> <td title="Mn, Manganese" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Manganese" title="Manganese">Mn</a> </td> <td title="Fe, Iron" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Iron" title="Iron">Fe</a> </td> <td title="Co, Cobalt" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Cobalt" title="Cobalt">Co</a> </td> <td title="Ni, Nickel" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Nickel" title="Nickel">Ni</a> </td> <td title="Cu, Copper" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Copper" title="Copper">Cu</a> </td> <td title="Zn, Zinc" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Zinc" title="Zinc">Zn</a> </td> <td title="Ga, Gallium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Gallium" title="Gallium">Ga</a> </td> <td title="Ge, Germanium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Germanium" title="Germanium">Ge</a> </td> <td title="As, Arsenic" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Arsenic" title="Arsenic">As</a> </td> <td title="Se, Selenium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Selenium" title="Selenium">Se</a> </td> <td title="Br, Bromine" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Bromine" title="Bromine">Br</a> </td> <td title="Kr, Krypton" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Krypton" title="Krypton">Kr</a> </td></tr> <tr> <th scope="row" style="background:transparent; 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; border:none; ;"><a href="/wiki/Rubidium" title="Rubidium">Rb</a> </td> <td title="Sr, Strontium" style="text-align:center; background-color:#ff9999; 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; border:none; ;"><a href="/wiki/Yttrium" title="Yttrium">Y</a> </td> <td title="Zr, Zirconium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Zirconium" title="Zirconium">Zr</a> </td> <td title="Nb, Niobium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Niobium" title="Niobium">Nb</a> </td> <td title="Mo, Molybdenum" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Molybdenum" title="Molybdenum">Mo</a> </td> <td title="Tc, Technetium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Technetium" title="Technetium">Tc</a> </td> <td title="Ru, Ruthenium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Ruthenium" title="Ruthenium">Ru</a> </td> <td title="Rh, Rhodium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Rhodium" title="Rhodium">Rh</a> </td> <td title="Pd, Palladium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Palladium" title="Palladium">Pd</a> </td> <td title="Ag, Silver" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Silver" title="Silver">Ag</a> </td> <td title="Cd, Cadmium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Cadmium" title="Cadmium">Cd</a> </td> <td title="In, Indium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Indium" title="Indium">In</a> </td> <td title="Sn, Tin" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Tin" title="Tin">Sn</a> </td> <td title="Sb, Antimony" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Antimony" title="Antimony">Sb</a> </td> <td title="Te, Tellurium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Tellurium" title="Tellurium">Te</a> </td> <td title="I, Iodine" style="text-align:center; background-color:#fdff8c; border:3px solid black; ;"><a class="mw-selflink selflink">I</a> </td> <td title="Xe, Xenon" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Xenon" title="Xenon">Xe</a> </td></tr> <tr> <th scope="row" style="background:transparent; 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; border:none; ;"><a href="/wiki/Caesium" title="Caesium">Cs</a> </td> <td title="Ba, Barium" style="text-align:center; background-color:#ff9999; border:none; ;"><a href="/wiki/Barium" title="Barium">Ba</a> </td> <td title="La, Lanthanum" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Lanthanum" title="Lanthanum">La</a> </td> <td title="Ce, Cerium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Cerium" title="Cerium">Ce</a> </td> <td title="Pr, Praseodymium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Praseodymium" title="Praseodymium">Pr</a> </td> <td title="Nd, Neodymium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Neodymium" title="Neodymium">Nd</a> </td> <td title="Pm, Promethium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Promethium" title="Promethium">Pm</a> </td> <td title="Sm, Samarium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Samarium" title="Samarium">Sm</a> </td> <td title="Eu, Europium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Europium" title="Europium">Eu</a> </td> <td title="Gd, Gadolinium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Gadolinium" title="Gadolinium">Gd</a> </td> <td title="Tb, Terbium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Terbium" title="Terbium">Tb</a> </td> <td title="Dy, Dysprosium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Dysprosium" title="Dysprosium">Dy</a> </td> <td title="Ho, Holmium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Holmium" title="Holmium">Ho</a> </td> <td title="Er, Erbium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Erbium" title="Erbium">Er</a> </td> <td title="Tm, Thulium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Thulium" title="Thulium">Tm</a> </td> <td title="Yb, Ytterbium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Ytterbium" title="Ytterbium">Yb</a> </td> <td title="Lu, Lutetium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Lutetium" title="Lutetium">Lu</a> </td> <td title="Hf, Hafnium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Hafnium" title="Hafnium">Hf</a> </td> <td title="Ta, Tantalum" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Tantalum" title="Tantalum">Ta</a> </td> <td title="W, Tungsten" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Tungsten" title="Tungsten">W</a> </td> <td title="Re, Rhenium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Rhenium" title="Rhenium">Re</a> </td> <td title="Os, Osmium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Osmium" title="Osmium">Os</a> </td> <td title="Ir, Iridium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Iridium" title="Iridium">Ir</a> </td> <td title="Pt, Platinum" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Platinum" title="Platinum">Pt</a> </td> <td title="Au, Gold" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Gold" title="Gold">Au</a> </td> <td title="Hg, Mercury" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Mercury_(element)" title="Mercury (element)">Hg</a> </td> <td title="Tl, Thallium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Thallium" title="Thallium">Tl</a> </td> <td title="Pb, Lead" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Lead" title="Lead">Pb</a> </td> <td title="Bi, Bismuth" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Bismuth" title="Bismuth">Bi</a> </td> <td title="Po, Polonium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Polonium" title="Polonium">Po</a> </td> <td title="At, Astatine" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Astatine" title="Astatine">At</a> </td> <td title="Rn, Radon" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Radon" title="Radon">Rn</a> </td></tr> <tr> <th scope="row" style="background:transparent; 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; border:none; ;"><a href="/wiki/Francium" title="Francium">Fr</a> </td> <td title="Ra, Radium" style="text-align:center; background-color:#ff9999; border:none; ;"><a href="/wiki/Radium" title="Radium">Ra</a> </td> <td title="Ac, Actinium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Actinium" title="Actinium">Ac</a> </td> <td title="Th, Thorium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Thorium" title="Thorium">Th</a> </td> <td title="Pa, Protactinium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Protactinium" title="Protactinium">Pa</a> </td> <td title="U, Uranium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Uranium" title="Uranium">U</a> </td> <td title="Np, Neptunium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Neptunium" title="Neptunium">Np</a> </td> <td title="Pu, Plutonium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Plutonium" title="Plutonium">Pu</a> </td> <td title="Am, Americium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Americium" title="Americium">Am</a> </td> <td title="Cm, Curium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Curium" title="Curium">Cm</a> </td> <td title="Bk, Berkelium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Berkelium" title="Berkelium">Bk</a> </td> <td title="Cf, Californium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Californium" title="Californium">Cf</a> </td> <td title="Es, Einsteinium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Einsteinium" title="Einsteinium">Es</a> </td> <td title="Fm, Fermium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Fermium" title="Fermium">Fm</a> </td> <td title="Md, Mendelevium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Mendelevium" title="Mendelevium">Md</a> </td> <td title="No, Nobelium" style="text-align:center; background-color:#9bff99; border:none; ;"><a href="/wiki/Nobelium" title="Nobelium">No</a> </td> <td title="Lr, Lawrencium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Lawrencium" title="Lawrencium">Lr</a> </td> <td title="Rf, Rutherfordium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Rutherfordium" title="Rutherfordium">Rf</a> </td> <td title="Db, Dubnium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Dubnium" title="Dubnium">Db</a> </td> <td title="Sg, Seaborgium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Seaborgium" title="Seaborgium">Sg</a> </td> <td title="Bh, Bohrium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Bohrium" title="Bohrium">Bh</a> </td> <td title="Hs, Hassium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Hassium" title="Hassium">Hs</a> </td> <td title="Mt, Meitnerium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Meitnerium" title="Meitnerium">Mt</a> </td> <td title="Ds, Darmstadtium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Darmstadtium" title="Darmstadtium">Ds</a> </td> <td title="Rg, Roentgenium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Roentgenium" title="Roentgenium">Rg</a> </td> <td title="Cn, Copernicium" style="text-align:center; background-color:#99ccff; border:none; ;"><a href="/wiki/Copernicium" title="Copernicium">Cn</a> </td> <td title="Nh, Nihonium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Nihonium" title="Nihonium">Nh</a> </td> <td title="Fl, Flerovium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Flerovium" title="Flerovium">Fl</a> </td> <td title="Mc, Moscovium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Moscovium" title="Moscovium">Mc</a> </td> <td title="Lv, Livermorium" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Livermorium" title="Livermorium">Lv</a> </td> <td title="Ts, Tennessine" style="text-align:center; background-color:#fdff8c; border:none; ;"><a href="/wiki/Tennessine" title="Tennessine">Ts</a> </td> <td title="Og, Oganesson" style="text-align:center; background-color:#fdff8c; 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; margin:0; 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href="/wiki/Special:EditPage/Template:Iodine_compounds" title="Special:EditPage/Template:Iodine compounds"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Iodine_compounds" style="font-size:114%;margin:0 4em"><a href="/wiki/Iodine_compounds" title="Iodine compounds">Iodine compounds</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%">Iodine(−I)</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_iodide" title="Hydrogen iodide">HI</a></li> <li><a href="/wiki/Tetraiodonickelate" title="Tetraiodonickelate">NiI2−4</a></li> <li><a href="/wiki/Astatine_iodide" title="Astatine iodide">AtI</a></li> <li><a href="/wiki/Template:Iodides" title="Template:Iodides">other</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Iodine(I)</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/Diiodine_oxide" title="Diiodine oxide">I2O</a></li> <li><a href="/wiki/Hypoiodous_acid" title="Hypoiodous acid">HIO</a></li> <li><a href="/wiki/Iodine_azide" title="Iodine azide">IN3</a></li> <li><a href="/wiki/Cyanogen_iodide" title="Cyanogen iodide">ICN</a></li> <li><a href="/wiki/Iodine_monochloride" title="Iodine monochloride">ICl</a></li> <li><a href="/wiki/Iodine_monofluoride" title="Iodine monofluoride">IF</a></li> <li><a href="/wiki/Nitrogen_triiodine" class="mw-redirect" title="Nitrogen triiodine">NI3</a></li> <li><a href="/wiki/Iodine_monobromide" title="Iodine monobromide">IBr</a></li> <li><a href="/wiki/Iodine_nitrate" title="Iodine nitrate">INO3</a></li> <li><a href="/wiki/Iodocyclopropane" title="Iodocyclopropane">C3H5I</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Iodine(II)</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/Iodine_monoxide" title="Iodine monoxide">IO</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Iodine(III)</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/Iodous_acid" title="Iodous acid">HIO2</a></li> <li><a href="/wiki/Iodine_trichloride" title="Iodine trichloride">ICl3</a></li> <li><a href="/wiki/Iodine_trifluoride" title="Iodine trifluoride">IF3</a></li> <li><a href="/wiki/Iodine_tribromide" title="Iodine tribromide">IBr3</a></li> <li><a href="/wiki/Iodine_sulfate" title="Iodine sulfate">I2(SO4)3</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Iodine(IV)</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/Iodine_dioxide" title="Iodine dioxide">IO 2</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Iodine(V)</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/Iodic_acid" title="Iodic acid">HIO3</a></li> <li><a href="/wiki/Iodine_pentafluoride" title="Iodine pentafluoride">IF5</a></li> <li><a href="/wiki/Iodine_pentoxide" title="Iodine pentoxide">I2O5</a></li> <li><a href="/wiki/Iodyl_fluoride" title="Iodyl fluoride">IO2F</a></li> <li><a href="/wiki/Iodosyl_trifluoride" title="Iodosyl trifluoride">IOF3</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Iodine(VII)</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/Periodic_acid" title="Periodic acid">HIO4</a></li> <li><a href="/wiki/Periodic_acid" title="Periodic acid">H5IO6</a></li> <li><a href="/wiki/Iodine_heptafluoride" title="Iodine heptafluoride">IF7</a></li> <li><a href="/wiki/Periodyl_fluoride" title="Periodyl fluoride">IO3F</a></li> <li><a href="/wiki/Iodyl_trifluoride" class="mw-redirect" title="Iodyl trifluoride">IO2F3</a></li> <li><a href="/wiki/Iodosyl_pentafluoride" title="Iodosyl pentafluoride">IOF5</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: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_elements" 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_elements" 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 href="/wiki/Chlorine" title="Chlorine">Cl2</a></li> <li><a href="/wiki/Bromine" title="Bromine">Br2</a></li> <li><a class="mw-selflink selflink">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="Thyroid_hormone_receptor_modulators" style="padding:3px"><table class="nowraplinks hlist 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:Thyroid_hormone_receptor_modulators" title="Template:Thyroid hormone receptor modulators"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Thyroid_hormone_receptor_modulators" title="Template talk:Thyroid hormone receptor modulators"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Thyroid_hormone_receptor_modulators" title="Special:EditPage/Template:Thyroid hormone receptor modulators"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Thyroid_hormone_receptor_modulators" style="font-size:114%;margin:0 4em"><a href="/wiki/Thyroid_hormone_receptor" title="Thyroid hormone receptor">Thyroid hormone receptor</a> <a href="/wiki/Receptor_modulator" title="Receptor modulator">modulators</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%;text-align:center;"><a href="/wiki/Receptor_(biochemistry)" title="Receptor (biochemistry)">Receptor</a> (<a href="/wiki/Ligand_(biochemistry)" title="Ligand (biochemistry)">ligands</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 id="THRTooltip_Thyroid_hormone_receptor" scope="row" class="navbox-group" style="width:3em;;text-align:center;"><a href="/wiki/Thyroid_hormone_receptor" title="Thyroid hormone receptor"><abbr title="Thyroid hormone receptor">THR</abbr></a><span class="sr-only" style="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; white-space: nowrap;">Tooltip Thyroid hormone receptor</th><td class="navbox-list-with-group navbox-list navbox-odd" style="padding:0"><div style="padding:0 0.25em"></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th id="Agonists" scope="row" class="navbox-group" style="width:3em;;text-align:center;">Agonists</th><td class="navbox-list-with-group navbox-list navbox-odd" style="padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Dextrothyroxine" title="Dextrothyroxine">Dextrothyroxine</a></li> <li><a href="/w/index.php?title=DIMIT&action=edit&redlink=1" class="new" title="DIMIT (page does not exist)">DIMIT</a></li> <li><a href="/w/index.php?title=DITPA&action=edit&redlink=1" class="new" title="DITPA (page does not exist)">DITPA</a></li> <li><a href="/wiki/Levothyroxine" title="Levothyroxine">Levothyroxine</a></li> <li><a href="/wiki/Liothyronine" title="Liothyronine">Liothyronine</a></li> <li><a href="/wiki/Liotrix" title="Liotrix">Liotrix</a></li> <li><a href="/wiki/Thyroxine" class="mw-redirect" title="Thyroxine">Thyroxine</a></li> <li><a href="/wiki/Tiratricol" title="Tiratricol">Tiratricol (TRIAC)</a></li> <li><a href="/wiki/Triiodothyronine" title="Triiodothyronine">Triiodothyronine</a></li> <li><a href="/wiki/Desiccated_thyroid_extract" title="Desiccated thyroid extract">Thyroid extract</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:3em;;text-align:center;"><a href="/wiki/Thyromimetic" title="Thyromimetic">Thyromimetics</a> (selective agonists)</th><td class="navbox-list-with-group navbox-list navbox-even" style="padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Eprotirome" title="Eprotirome">Eprotirome (KB-2115)</a></li> <li><a href="/w/index.php?title=KB-141&action=edit&redlink=1" class="new" title="KB-141 (page does not exist)">KB-141</a></li> <li><a href="/w/index.php?title=KB-2611&action=edit&redlink=1" class="new" title="KB-2611 (page does not exist)">KB-2611</a></li> <li><a href="/w/index.php?title=KB-130015&action=edit&redlink=1" class="new" title="KB-130015 (page does not exist)">KB-130015</a></li> <li><a href="/w/index.php?title=MB-07344&action=edit&redlink=1" class="new" title="MB-07344 (page does not exist)">MB-07344</a></li> <li><a href="/w/index.php?title=MB-07811&action=edit&redlink=1" class="new" title="MB-07811 (page does not exist)">MB-07811</a></li> <li><a href="/wiki/Resmetirom" title="Resmetirom">Resmetirom</a></li> <li><a href="/wiki/Sobetirome" title="Sobetirome">Sobetirome (GC-1, GRX-431)</a></li> <li><a href="/w/index.php?title=VK-0214&action=edit&redlink=1" class="new" title="VK-0214 (page does not exist)">VK-0214</a></li> <li><a href="/wiki/VK-2809" class="mw-redirect" title="VK-2809">VK-2809</a></li> <li><a href="/w/index.php?title=ZYT1&action=edit&redlink=1" class="new" title="ZYT1 (page does not exist)">ZYT1</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:3em;;text-align:center;">Antagonists</th><td class="navbox-list-with-group navbox-list navbox-odd" style="padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/w/index.php?title=1-850&action=edit&redlink=1" class="new" title="1-850 (page does not exist)">1-850</a></li> <li><a href="/w/index.php?title=NH3_(THR_antagonist)&action=edit&redlink=1" class="new" title="NH3 (THR antagonist) (page does not exist)">NH3</a></li> <li><a href="/w/index.php?title=Tetraiodothyroacetic_acid&action=edit&redlink=1" class="new" title="Tetraiodothyroacetic acid (page does not exist)">Tetraiodothyroacetic acid (Tetrac)</a></li></ul> </div></td></tr></tbody></table><div></div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;text-align:center;"><a href="/wiki/Membrane_transport_protein" title="Membrane transport protein">Transporter</a> (<a href="/wiki/Transporter_blocker" class="mw-redirect" title="Transporter blocker">blockers</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 id="NISTooltip_Sodium-iodide_symporter" scope="row" class="navbox-group" style="width:3em;;text-align:center;"><a href="/wiki/Sodium-iodide_symporter" class="mw-redirect" title="Sodium-iodide symporter"><abbr title="Sodium-iodide symporter">NIS</abbr></a><span class="sr-only" style="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; white-space: nowrap;">Tooltip Sodium-iodide symporter  </th><td class="navbox-list-with-group navbox-list navbox-even" style="padding:0"><div style="padding:0 0.25em"> <ul><li>Inhibitors: <a href="/wiki/Cyanogenic_glycoside" class="mw-redirect" title="Cyanogenic glycoside">Cyanogenic glycosides</a></li> <li><a href="/wiki/Perchlorate" title="Perchlorate">Perchlorates</a> (e.g., <a href="/wiki/Potassium_perchlorate" title="Potassium perchlorate">potassium perchlorate</a>)</li> <li><a href="/wiki/Pertechnetate" title="Pertechnetate">Pertechnetates</a> (e.g., <a href="/wiki/Sodium_pertechnetate" title="Sodium pertechnetate">sodium pertechnetate</a>)</li> <li><a href="/wiki/Thiocyanate" title="Thiocyanate">Thiocyanates</a> </li></ul> </div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;text-align:center;"><a href="/wiki/Enzyme" title="Enzyme">Enzyme</a> (<a href="/wiki/Enzyme_inhibitor" title="Enzyme inhibitor">inhibitors</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:3em;;text-align:center;"><a href="/wiki/Thyroid_peroxidase" title="Thyroid peroxidase"><abbr title="Thyroid peroxidase">TPO</abbr></a><span class="sr-only" style="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; white-space: nowrap;">Tooltip Thyroid peroxidase</th><td class="navbox-list-with-group navbox-list navbox-odd" style="padding:0"><div style="padding:0 0.25em"> <ul><li>Inhibitors: <a href="/wiki/Benzylthiouracil" title="Benzylthiouracil">Benzylthiouracil</a></li> <li><a href="/wiki/Carbimazole" title="Carbimazole">Carbimazole</a></li> <li><a href="/wiki/Genistein" title="Genistein">Genistein</a></li> <li><a href="/wiki/Methimazole" class="mw-redirect" title="Methimazole">Methimazole</a></li> <li><a href="/wiki/Methylthiouracil" title="Methylthiouracil">Methylthiouracil</a></li> <li><a href="/wiki/Propylthiouracil" title="Propylthiouracil">Propylthiouracil</a></li> <li><a href="/wiki/2-Thiouracil" title="2-Thiouracil">2-Thiouracil</a></li> <li><a href="/wiki/Thiourea" title="Thiourea">Thiourea</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:3em;;text-align:center;"><a href="/wiki/Iodothyronine_deiodinase" title="Iodothyronine deiodinase"><abbr title="Iodothyronine deiodinase">DIO</abbr></a><span class="sr-only" style="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; white-space: nowrap;">Tooltip Iodothyronine deiodinase</th><td class="navbox-list-with-group navbox-list navbox-even" style="padding:0"><div style="padding:0 0.25em"> <ul><li>Inhibitors: <a href="/wiki/Dexpropranolol" class="mw-redirect" title="Dexpropranolol">Dexpropranolol</a></li> <li><a href="/wiki/Iopanoic_acid" title="Iopanoic acid">Iopanoic acid</a></li> <li><a href="/wiki/Ipodate_sodium" title="Ipodate sodium">Ipodate sodium (sodium iopodate)</a></li> <li><a href="/wiki/Propranolol" title="Propranolol">Propranolol</a></li> <li><a href="/wiki/Propylthiouracil" title="Propylthiouracil">Propylthiouracil</a></li></ul> </div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%;text-align:center;">Others</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">Iodine</a></li> <li><a href="/wiki/Iodine-131" title="Iodine-131">Iodine-131</a></li> <li><a href="/wiki/Selenium" title="Selenium">Selenium</a></li> <li><a href="/wiki/Thyroglobulin" title="Thyroglobulin">Thyroglobulin</a></li> <li><a href="/wiki/Tyrosine" title="Tyrosine">Tyrosine</a></li></ul> </div></td></tr><tr><td class="navbox-abovebelow" colspan="2"><div> <ul><li>See also: <a href="/wiki/Template:Receptor_modulators" title="Template:Receptor modulators">Receptor/signaling modulators</a></li></ul> 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