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aria-controls="toc-Occurrence-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Occurrence subsection </button> <ul id="toc-Occurrence-sublist" class="vector-toc-list"> <li id="toc-Universe" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Universe"> <div class="vector-toc-text"> 2.1 Universe </div> </a> <ul id="toc-Universe-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Earth" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Earth"> <div class="vector-toc-text"> 2.2 Earth </div> </a> <ul id="toc-Earth-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-History" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#History"> <div class="vector-toc-text"> 3 History </div> </a> <button aria-controls="toc-History-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle History subsection </button> <ul id="toc-History-sublist" class="vector-toc-list"> <li id="toc-Early_discoveries" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Early_discoveries"> <div class="vector-toc-text"> 3.1 Early discoveries </div> </a> <ul id="toc-Early_discoveries-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Isolation" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Isolation"> <div class="vector-toc-text"> 3.2 Isolation </div> </a> <ul id="toc-Isolation-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Later_uses" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Later_uses"> <div class="vector-toc-text"> 3.3 Later uses </div> </a> <ul id="toc-Later_uses-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Compounds" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Compounds"> <div class="vector-toc-text"> 4 Compounds </div> </a> <button aria-controls="toc-Compounds-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Compounds subsection </button> <ul id="toc-Compounds-sublist" class="vector-toc-list"> <li id="toc-Oxidation_states" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Oxidation_states"> <div class="vector-toc-text"> 4.1 Oxidation states </div> </a> <ul id="toc-Oxidation_states-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Metals" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Metals"> <div class="vector-toc-text"> 4.2 Metals </div> </a> <ul id="toc-Metals-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Hydrogen" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Hydrogen"> <div class="vector-toc-text"> 4.3 Hydrogen </div> </a> <ul id="toc-Hydrogen-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Other_reactive_nonmetals" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Other_reactive_nonmetals"> <div class="vector-toc-text"> 4.4 Other reactive nonmetals </div> </a> <ul id="toc-Other_reactive_nonmetals-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Noble_gases" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Noble_gases"> <div class="vector-toc-text"> 4.5 Noble gases </div> </a> <ul id="toc-Noble_gases-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Organic_compounds" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Organic_compounds"> <div class="vector-toc-text"> 4.6 Organic compounds </div> </a> <ul id="toc-Organic_compounds-sublist" class="vector-toc-list"> <li id="toc-Discrete_molecules" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Discrete_molecules"> <div class="vector-toc-text"> 4.6.1 Discrete molecules </div> </a> <ul id="toc-Discrete_molecules-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Polymers" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Polymers"> <div class="vector-toc-text"> 4.6.2 Polymers </div> </a> <ul id="toc-Polymers-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> </ul> </li> <li id="toc-Production" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Production"> <div class="vector-toc-text"> 5 Production </div> </a> <button aria-controls="toc-Production-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Production subsection </button> <ul id="toc-Production-sublist" class="vector-toc-list"> <li id="toc-Industrial_routes_to_F2" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Industrial_routes_to_F2"> <div class="vector-toc-text"> 5.1 Industrial routes to F2 </div> </a> <ul id="toc-Industrial_routes_to_F2-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Laboratory_routes" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Laboratory_routes"> <div class="vector-toc-text"> 5.2 Laboratory routes </div> </a> <ul id="toc-Laboratory_routes-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Industrial_applications" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Industrial_applications"> <div class="vector-toc-text"> 6 Industrial applications </div> </a> <button aria-controls="toc-Industrial_applications-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Industrial applications subsection </button> <ul id="toc-Industrial_applications-sublist" class="vector-toc-list"> <li id="toc-Inorganic_fluorides" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Inorganic_fluorides"> <div class="vector-toc-text"> 6.1 Inorganic fluorides </div> </a> <ul id="toc-Inorganic_fluorides-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Organic_fluorides" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Organic_fluorides"> <div class="vector-toc-text"> 6.2 Organic fluorides </div> </a> <ul id="toc-Organic_fluorides-sublist" class="vector-toc-list"> <li id="toc-Refrigerant_gases" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Refrigerant_gases"> <div class="vector-toc-text"> 6.2.1 Refrigerant gases </div> </a> <ul id="toc-Refrigerant_gases-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Polymers_2" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Polymers_2"> <div class="vector-toc-text"> 6.2.2 Polymers </div> </a> <ul id="toc-Polymers_2-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Surfactants" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Surfactants"> <div class="vector-toc-text"> 6.2.3 Surfactants </div> </a> <ul id="toc-Surfactants-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Agrichemicals" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Agrichemicals"> <div class="vector-toc-text"> 6.2.4 Agrichemicals </div> </a> <ul id="toc-Agrichemicals-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> </ul> </li> <li id="toc-Medicinal_applications" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Medicinal_applications"> <div class="vector-toc-text"> 7 Medicinal applications </div> </a> <button aria-controls="toc-Medicinal_applications-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Medicinal applications subsection </button> <ul id="toc-Medicinal_applications-sublist" class="vector-toc-list"> <li id="toc-Dental_care" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Dental_care"> <div class="vector-toc-text"> 7.1 Dental care </div> </a> <ul id="toc-Dental_care-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Pharmaceuticals" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Pharmaceuticals"> <div class="vector-toc-text"> 7.2 Pharmaceuticals </div> </a> <ul id="toc-Pharmaceuticals-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-PET_scanning" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#PET_scanning"> <div class="vector-toc-text"> 7.3 PET scanning </div> </a> <ul id="toc-PET_scanning-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Oxygen_carriers" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Oxygen_carriers"> <div class="vector-toc-text"> 7.4 Oxygen carriers </div> </a> <ul id="toc-Oxygen_carriers-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Biological_role" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Biological_role"> <div class="vector-toc-text"> 8 Biological role </div> </a> <ul id="toc-Biological_role-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Toxicity" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Toxicity"> <div class="vector-toc-text"> 9 Toxicity </div> </a> <button aria-controls="toc-Toxicity-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Toxicity subsection </button> <ul id="toc-Toxicity-sublist" class="vector-toc-list"> <li id="toc-Hydrofluoric_acid" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Hydrofluoric_acid"> <div class="vector-toc-text"> 9.1 Hydrofluoric acid </div> </a> <ul id="toc-Hydrofluoric_acid-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Fluoride_ion" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Fluoride_ion"> <div class="vector-toc-text"> 9.2 Fluoride ion </div> </a> <ul id="toc-Fluoride_ion-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Environmental_concerns" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Environmental_concerns"> <div class="vector-toc-text"> 10 Environmental concerns </div> </a> <button aria-controls="toc-Environmental_concerns-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Environmental concerns subsection </button> <ul id="toc-Environmental_concerns-sublist" class="vector-toc-list"> <li id="toc-Atmosphere" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Atmosphere"> <div class="vector-toc-text"> 10.1 Atmosphere </div> </a> <ul id="toc-Atmosphere-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Biopersistence" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Biopersistence"> <div class="vector-toc-text"> 10.2 Biopersistence </div> </a> <ul id="toc-Biopersistence-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-See_also" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#See_also"> <div class="vector-toc-text"> 11 See also </div> </a> <ul id="toc-See_also-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Notes" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Notes"> <div class="vector-toc-text"> 12 Notes </div> </a> <ul id="toc-Notes-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Sources" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#Sources"> <div class="vector-toc-text"> 13 Sources </div> </a> <button aria-controls="toc-Sources-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> Toggle Sources subsection </button> <ul id="toc-Sources-sublist" class="vector-toc-list"> <li id="toc-Citations" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Citations"> <div class="vector-toc-text"> 13.1 Citations </div> </a> <ul id="toc-Citations-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Indexed_references" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Indexed_references"> <div class="vector-toc-text"> 13.2 Indexed references </div> </a> <ul id="toc-Indexed_references-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-External_links" class="vector-toc-list-item vector-toc-level-1"> <a class="vector-toc-link" href="#External_links"> <div class="vector-toc-text"> 14 External links </div> </a> <ul id="toc-External_links-sublist" class="vector-toc-list"> </ul> </li> </ul> </div> </div> </nav> </div> </div> <div class="mw-content-container"> <main id="content" class="mw-body"> <header class="mw-body-header vector-page-titlebar"> <nav aria-label="Contents" class="vector-toc-landmark"> <div id="vector-page-titlebar-toc" class="vector-dropdown vector-page-titlebar-toc vector-button-flush-left" title="Table of Contents" > <input type="checkbox" id="vector-page-titlebar-toc-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-vector-page-titlebar-toc" class="vector-dropdown-checkbox " aria-label="Toggle the table of contents" > <label id="vector-page-titlebar-toc-label" for="vector-page-titlebar-toc-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--icon-only " aria-hidden="true" > Toggle the table of contents </label> <div class="vector-dropdown-content"> <div id="vector-page-titlebar-toc-unpinned-container" class="vector-unpinned-container"> </div> </div> </div> </nav> <h1 id="firstHeading" class="firstHeading mw-first-heading">Fluorine</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 167 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-167" aria-hidden="true" > 167 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/Fluoor" title="Fluoor – Afrikaans" lang="af" hreflang="af" data-title="Fluoor" 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%8D%8D%E1%88%8E%E1%88%AA%E1%8A%95" title="ፍሎሪን – Amharic" lang="am" hreflang="am" data-title="ፍሎሪን" data-language-autonym="አማርኛ" data-language-local-name="Amharic" class="interlanguage-link-target">አማርኛ</a></li><li class="interlanguage-link interwiki-smn mw-list-item"><a href="https://smn.wikipedia.org/wiki/Fluori" title="Fluori – Inari Sami" lang="smn" hreflang="smn" data-title="Fluori" data-language-autonym="Anarâškielâ" data-language-local-name="Inari Sami" class="interlanguage-link-target">Anarâškielâ</a></li><li class="interlanguage-link interwiki-anp mw-list-item"><a href="https://anp.wikipedia.org/wiki/%E0%A4%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A5%80%E0%A4%A8" title="फ्लोरीन – Angika" lang="anp" hreflang="anp" data-title="फ्लोरीन" data-language-autonym="अंगिका" data-language-local-name="Angika" class="interlanguage-link-target">अंगिका</a></li><li class="interlanguage-link interwiki-ar badge-Q17437796 badge-featuredarticle mw-list-item" title="featured article badge"><a href="https://ar.wikipedia.org/wiki/%D9%81%D9%84%D9%88%D8%B1" title="فلور – Arabic" lang="ar" hreflang="ar" data-title="فلور" 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/Fl%C3%BAor" title="Flúor – Aragonese" lang="an" hreflang="an" data-title="Flúor" data-language-autonym="Aragonés" data-language-local-name="Aragonese" class="interlanguage-link-target">Aragonés</a></li><li class="interlanguage-link interwiki-hyw mw-list-item"><a href="https://hyw.wikipedia.org/wiki/%D5%93%D5%B2%D5%B8%D6%82%D5%B8%D6%80" title="Փղուոր – Western Armenian" lang="hyw" hreflang="hyw" data-title="Փղուոր" data-language-autonym="Արեւմտահայերէն" data-language-local-name="Western Armenian" class="interlanguage-link-target">Արեւմտահայերէն</a></li><li class="interlanguage-link interwiki-roa-rup mw-list-item"><a href="https://roa-rup.wikipedia.org/wiki/Fluoru" title="Fluoru – Aromanian" lang="rup" hreflang="rup" data-title="Fluoru" data-language-autonym="Armãneashti" data-language-local-name="Aromanian" class="interlanguage-link-target">Armãneashti</a></li><li class="interlanguage-link interwiki-ast badge-Q17437796 badge-featuredarticle mw-list-item" title="featured article badge"><a href="https://ast.wikipedia.org/wiki/Fl%C3%BAor" title="Flúor – Asturian" lang="ast" hreflang="ast" data-title="Flúor" data-language-autonym="Asturianu" data-language-local-name="Asturian" class="interlanguage-link-target">Asturianu</a></li><li class="interlanguage-link interwiki-awa mw-list-item"><a href="https://awa.wikipedia.org/wiki/%E0%A4%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="फ्लोरिन – Awadhi" lang="awa" hreflang="awa" data-title="फ्लोरिन" data-language-autonym="अवधी" data-language-local-name="Awadhi" class="interlanguage-link-target">अवधी</a></li><li class="interlanguage-link interwiki-az mw-list-item"><a href="https://az.wikipedia.org/wiki/Fl%C3%BCor" title="Flüor – Azerbaijani" lang="az" hreflang="az" data-title="Flüor" data-language-autonym="Azərbaycanca" data-language-local-name="Azerbaijani" class="interlanguage-link-target">Azərbaycanca</a></li><li class="interlanguage-link interwiki-ban mw-list-item"><a href="https://ban.wikipedia.org/wiki/Fluorin" title="Fluorin – Balinese" lang="ban" hreflang="ban" data-title="Fluorin" 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%AB%E0%A7%8D%E0%A6%B2%E0%A7%8B%E0%A6%B0%E0%A6%BF%E0%A6%A8" title="ফ্লোরিন – Bangla" lang="bn" hreflang="bn" data-title="ফ্লোরিন" 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/Hut-s%C3%B2%CD%98" title="Hut-sò͘ – Minnan" lang="nan" hreflang="nan" data-title="Hut-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%A4%D1%82%D0%BE%D1%80" title="Фтор – Bashkir" lang="ba" hreflang="ba" data-title="Фтор" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Belarusian" lang="be" hreflang="be" data-title="Фтор" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Belarusian (Taraškievica orthography)" lang="be-tarask" hreflang="be-tarask" data-title="Фтор" 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%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A5%80%E0%A4%A8" title="फ्लोरीन – Bhojpuri" lang="bh" hreflang="bh" data-title="फ्लोरीन" 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/Plurina" title="Plurina – Central Bikol" lang="bcl" hreflang="bcl" data-title="Plurina" data-language-autonym="Bikol Central" data-language-local-name="Central Bikol" class="interlanguage-link-target">Bikol Central</a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%A4%D0%BB%D1%83%D0%BE%D1%80" title="Флуор – Bulgarian" lang="bg" hreflang="bg" data-title="Флуор" 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%96%E0%BD%9E%E0%BD%B4%E0%BD%A2%E0%BC%8B%E0%BD%A2%E0%BE%B3%E0%BD%B4%E0%BD%84%E0%BC%8B%E0%BC%8D" title="བཞུར་རླུང་། – Tibetan" lang="bo" hreflang="bo" data-title="བཞུར་རླུང་།" data-language-autonym="བོད་ཡིག" data-language-local-name="Tibetan" class="interlanguage-link-target">བོད་ཡིག</a></li><li class="interlanguage-link interwiki-bs mw-list-item"><a href="https://bs.wikipedia.org/wiki/Fluor" title="Fluor – Bosnian" lang="bs" hreflang="bs" data-title="Fluor" 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/Fluor" title="Fluor – Breton" lang="br" hreflang="br" data-title="Fluor" 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/Fluor" title="Fluor – Catalan" lang="ca" hreflang="ca" data-title="Fluor" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Chuvash" lang="cv" hreflang="cv" data-title="Фтор" 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/Fluor" title="Fluor – Cebuano" lang="ceb" hreflang="ceb" data-title="Fluor" 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/Fluor" title="Fluor – Czech" lang="cs" hreflang="cs" data-title="Fluor" data-language-autonym="Čeština" data-language-local-name="Czech" class="interlanguage-link-target">Čeština</a></li><li class="interlanguage-link interwiki-sn mw-list-item"><a href="https://sn.wikipedia.org/wiki/Flourine" title="Flourine – Shona" lang="sn" hreflang="sn" data-title="Flourine" data-language-autonym="ChiShona" data-language-local-name="Shona" class="interlanguage-link-target">ChiShona</a></li><li class="interlanguage-link interwiki-co mw-list-item"><a href="https://co.wikipedia.org/wiki/Fluoru" title="Fluoru – Corsican" lang="co" hreflang="co" data-title="Fluoru" 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/Fflworin" title="Fflworin – Welsh" lang="cy" hreflang="cy" data-title="Fflworin" 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/Fluor" title="Fluor – Danish" lang="da" hreflang="da" data-title="Fluor" 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%81%D9%84%D9%8A%D9%88%D8%B1" title="فليور – Moroccan Arabic" lang="ary" hreflang="ary" data-title="فليور" data-language-autonym="الدارجة" data-language-local-name="Moroccan Arabic" class="interlanguage-link-target">الدارجة</a></li><li class="interlanguage-link interwiki-de badge-Q17437798 badge-goodarticle mw-list-item" title="good article badge"><a href="https://de.wikipedia.org/wiki/Fluor" title="Fluor – German" lang="de" hreflang="de" data-title="Fluor" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target">Deutsch</a></li><li class="interlanguage-link interwiki-et mw-list-item"><a href="https://et.wikipedia.org/wiki/Fluor" title="Fluor – Estonian" lang="et" hreflang="et" data-title="Fluor" 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%A6%CE%B8%CF%8C%CF%81%CE%B9%CE%BF" title="Φθόριο – Greek" lang="el" hreflang="el" data-title="Φθόριο" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Erzya" lang="myv" hreflang="myv" data-title="Фтор" 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/Fl%C3%BAor" title="Flúor – Spanish" lang="es" hreflang="es" data-title="Flúor" 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/Fluoro" title="Fluoro – Esperanto" lang="eo" hreflang="eo" data-title="Fluoro" data-language-autonym="Esperanto" data-language-local-name="Esperanto" class="interlanguage-link-target">Esperanto</a></li><li class="interlanguage-link interwiki-ext mw-list-item"><a href="https://ext.wikipedia.org/wiki/Fl%C3%BAol" title="Flúol – Extremaduran" lang="ext" hreflang="ext" data-title="Flúol" data-language-autonym="Estremeñu" data-language-local-name="Extremaduran" class="interlanguage-link-target">Estremeñu</a></li><li class="interlanguage-link interwiki-eu mw-list-item"><a href="https://eu.wikipedia.org/wiki/Fluor" title="Fluor – Basque" lang="eu" hreflang="eu" data-title="Fluor" 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/%D9%81%D9%84%D9%88%D8%A6%D9%88%D8%B1" title="فلوئور – Persian" lang="fa" hreflang="fa" data-title="فلوئور" 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/Fluorine" title="Fluorine – Fiji Hindi" lang="hif" hreflang="hif" data-title="Fluorine" 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/Fluor" title="Fluor – Faroese" lang="fo" hreflang="fo" data-title="Fluor" 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/Fluor" title="Fluor – French" lang="fr" hreflang="fr" data-title="Fluor" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target">Français</a></li><li class="interlanguage-link interwiki-fy mw-list-item"><a href="https://fy.wikipedia.org/wiki/Fluor" title="Fluor – Western Frisian" lang="fy" hreflang="fy" data-title="Fluor" data-language-autonym="Frysk" data-language-local-name="Western Frisian" class="interlanguage-link-target">Frysk</a></li><li class="interlanguage-link interwiki-fur mw-list-item"><a href="https://fur.wikipedia.org/wiki/Flu%C3%B4r" title="Fluôr – Friulian" lang="fur" hreflang="fur" data-title="Fluôr" 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/Fluair%C3%ADn" title="Fluairín – Irish" lang="ga" hreflang="ga" data-title="Fluairín" 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/Fluoreen" title="Fluoreen – Manx" lang="gv" hreflang="gv" data-title="Fluoreen" 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/Fluarain" title="Fluarain – Scottish Gaelic" lang="gd" hreflang="gd" data-title="Fluarain" 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/Fl%C3%BAor" title="Flúor – Galician" lang="gl" hreflang="gl" data-title="Flúor" data-language-autonym="Galego" data-language-local-name="Galician" class="interlanguage-link-target">Galego</a></li><li class="interlanguage-link interwiki-gan mw-list-item"><a href="https://gan.wikipedia.org/wiki/%E6%B0%9F" title="氟 – Gan" lang="gan" hreflang="gan" data-title="氟" 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%AB%E0%AB%8D%E0%AA%B2%E0%AB%8B%E0%AA%B0%E0%AA%BF%E0%AA%A8" title="ફ્લોરિન – Gujarati" lang="gu" hreflang="gu" data-title="ફ્લોરિન" 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/Fuk" title="Fuk – Hakka Chinese" lang="hak" hreflang="hak" data-title="Fuk" 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%A4%D0%BB%D2%AF%D1%80" title="Флүр – Kalmyk" lang="xal" hreflang="xal" data-title="Флүр" 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/%ED%94%8C%EB%A3%A8%EC%98%A4%EB%A6%B0" title="플루오린 – Korean" lang="ko" hreflang="ko" data-title="플루오린" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target">한국어</a></li><li class="interlanguage-link interwiki-haw mw-list-item"><a href="https://haw.wikipedia.org/wiki/Fluorine" title="Fluorine – Hawaiian" lang="haw" hreflang="haw" data-title="Fluorine" data-language-autonym="Hawaiʻi" data-language-local-name="Hawaiian" class="interlanguage-link-target">Hawaiʻi</a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D5%96%D5%BF%D5%B8%D6%80" title="Ֆտոր – Armenian" lang="hy" hreflang="hy" data-title="Ֆտոր" 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%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A5%80%E0%A4%A8" title="फ्लोरीन – Hindi" lang="hi" hreflang="hi" data-title="फ्लोरीन" 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/Fluor" title="Fluor – Croatian" lang="hr" hreflang="hr" data-title="Fluor" 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/Fluoro" title="Fluoro – Ido" lang="io" hreflang="io" data-title="Fluoro" 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/Fluorin" title="Fluorin – Indonesian" lang="id" hreflang="id" data-title="Fluorin" 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/Fluor" title="Fluor – Interlingua" lang="ia" hreflang="ia" data-title="Fluor" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Ossetic" lang="os" hreflang="os" data-title="Фтор" 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/UFusihwe" title="UFusihwe – Zulu" lang="zu" hreflang="zu" data-title="UFusihwe" 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/Fl%C3%BAor" title="Flúor – Icelandic" lang="is" hreflang="is" data-title="Flúor" 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/Fluoro" title="Fluoro – Italian" lang="it" hreflang="it" data-title="Fluoro" 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%A4%D7%9C%D7%95%D7%90%D7%95%D7%A8" title="פלואור – Hebrew" lang="he" hreflang="he" data-title="פלואור" 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/Florin" title="Florin – Javanese" lang="jv" hreflang="jv" data-title="Florin" 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/F%CA%8Al%CA%8Ay%C9%94r%C9%A9" title="Fʊlʊyɔrɩ – Kabiye" lang="kbp" hreflang="kbp" data-title="Fʊlʊyɔrɩ" 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%AB%E0%B3%8D%E0%B2%B2%E0%B3%82%E0%B2%B0%E0%B3%80%E0%B2%A8%E0%B3%8D" title="ಫ್ಲೂರೀನ್ – Kannada" lang="kn" hreflang="kn" data-title="ಫ್ಲೂರೀನ್" 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%A4%E1%83%97%E1%83%9D%E1%83%A0%E1%83%98" title="ფთორი – Georgian" lang="ka" hreflang="ka" data-title="ფთორი" data-language-autonym="ქართული" data-language-local-name="Georgian" class="interlanguage-link-target">ქართული</a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%A4%D1%82%D0%BE%D1%80" title="Фтор – Kazakh" lang="kk" hreflang="kk" data-title="Фтор" 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/Fluorin" title="Fluorin – Cornish" lang="kw" hreflang="kw" data-title="Fluorin" 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/Florini" title="Florini – Swahili" lang="sw" hreflang="sw" data-title="Florini" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Komi" lang="kv" hreflang="kv" data-title="Фтор" 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/Fliy%C3%B2" title="Fliyò – Haitian Creole" lang="ht" hreflang="ht" data-title="Fliyò" data-language-autonym="Kreyòl ayisyen" data-language-local-name="Haitian Creole" class="interlanguage-link-target">Kreyòl ayisyen</a></li><li class="interlanguage-link interwiki-ku mw-list-item"><a href="https://ku.wikipedia.org/wiki/Fluor" title="Fluor – Kurdish" lang="ku" hreflang="ku" data-title="Fluor" data-language-autonym="Kurdî" data-language-local-name="Kurdish" class="interlanguage-link-target">Kurdî</a></li><li class="interlanguage-link interwiki-ky mw-list-item"><a href="https://ky.wikipedia.org/wiki/%D0%A4%D1%82%D0%BE%D1%80" title="Фтор – Kyrgyz" lang="ky" hreflang="ky" data-title="Фтор" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Western Mari" lang="mrj" hreflang="mrj" data-title="Фтор" data-language-autonym="Кырык мары" data-language-local-name="Western Mari" class="interlanguage-link-target">Кырык мары</a></li><li class="interlanguage-link interwiki-lo mw-list-item"><a href="https://lo.wikipedia.org/wiki/%E0%BA%9F%E0%BA%A5%E0%BA%B9%E0%BA%AD%E0%BB%8D%E0%BA%A3%E0%BA%B4%E0%BA%99" title="ຟລູອໍຣິນ – Lao" lang="lo" hreflang="lo" data-title="ຟລູອໍຣິນ" 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/Fluorum" title="Fluorum – Latin" lang="la" hreflang="la" data-title="Fluorum" 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/Fluors" title="Fluors – Latvian" lang="lv" hreflang="lv" data-title="Fluors" 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/Fluor" title="Fluor – Luxembourgish" lang="lb" hreflang="lb" data-title="Fluor" 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/Fluoras" title="Fluoras – Lithuanian" lang="lt" hreflang="lt" data-title="Fluoras" 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/Flu%C3%B6" title="Fluö – Ligurian" lang="lij" hreflang="lij" data-title="Fluö" 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/Fluor" title="Fluor – Limburgish" lang="li" hreflang="li" data-title="Fluor" data-language-autonym="Limburgs" data-language-local-name="Limburgish" class="interlanguage-link-target">Limburgs</a></li><li class="interlanguage-link interwiki-ln mw-list-item"><a href="https://ln.wikipedia.org/wiki/Folina" title="Folina – Lingala" lang="ln" hreflang="ln" data-title="Folina" data-language-autonym="Lingála" data-language-local-name="Lingala" class="interlanguage-link-target">Lingála</a></li><li class="interlanguage-link interwiki-olo mw-list-item"><a href="https://olo.wikipedia.org/wiki/Ftor" title="Ftor – Livvi-Karelian" lang="olo" hreflang="olo" data-title="Ftor" 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/li%27orkliru" title="li'orkliru – Lojban" lang="jbo" hreflang="jbo" data-title="li'orkliru" 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/Fololiini" title="Fololiini – Ganda" lang="lg" hreflang="lg" data-title="Fololiini" 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/Fluoro" title="Fluoro – Lombard" lang="lmo" hreflang="lmo" data-title="Fluoro" data-language-autonym="Lombard" data-language-local-name="Lombard" class="interlanguage-link-target">Lombard</a></li><li class="interlanguage-link interwiki-hu badge-Q17437796 badge-featuredarticle mw-list-item" title="featured article badge"><a href="https://hu.wikipedia.org/wiki/Fluor" title="Fluor – Hungarian" lang="hu" hreflang="hu" data-title="Fluor" 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%A4%D0%BB%D1%83%D0%BE%D1%80" title="Флуор – Macedonian" lang="mk" hreflang="mk" data-title="Флуор" 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%AB%E0%B5%8D%E0%B4%B2%E0%B5%82%E0%B4%B1%E0%B4%BF%E0%B5%BB" title="ഫ്ലൂറിൻ – Malayalam" lang="ml" hreflang="ml" data-title="ഫ്ലൂറിൻ" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target">മലയാളം</a></li><li class="interlanguage-link interwiki-mi mw-list-item"><a href="https://mi.wikipedia.org/wiki/Hauk%C5%8Dwhai" title="Haukōwhai – Māori" lang="mi" hreflang="mi" data-title="Haukōwhai" data-language-autonym="Māori" data-language-local-name="Māori" class="interlanguage-link-target">Māori</a></li><li class="interlanguage-link interwiki-mr mw-list-item"><a href="https://mr.wikipedia.org/wiki/%E0%A4%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A5%80%E0%A4%A8" title="फ्लोरीन – Marathi" lang="mr" hreflang="mr" data-title="फ्लोरीन" 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%81%D9%84%D9%88%D8%B1" title="فلور – Egyptian Arabic" lang="arz" hreflang="arz" data-title="فلور" 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/Fluorin" title="Fluorin – Malay" lang="ms" hreflang="ms" data-title="Fluorin" data-language-autonym="Bahasa Melayu" data-language-local-name="Malay" class="interlanguage-link-target">Bahasa Melayu</a></li><li class="interlanguage-link interwiki-mni mw-list-item"><a href="https://mni.wikipedia.org/wiki/%EA%AF%90%EA%AF%AD%EA%AF%82%EA%AF%A3%EA%AF%94%EA%AF%A4%EA%AF%9F" title="ꯐ꯭ꯂꯣꯔꯤꯟ – Manipuri" lang="mni" hreflang="mni" data-title="ꯐ꯭ꯂꯣꯔꯤꯟ" data-language-autonym="ꯃꯤꯇꯩ ꯂꯣꯟ" data-language-local-name="Manipuri" class="interlanguage-link-target">ꯃꯤꯇꯩ ꯂꯣꯟ</a></li><li class="interlanguage-link interwiki-cdo mw-list-item"><a href="https://cdo.wikipedia.org/wiki/H%C3%B3k_(ngu%C3%B2ng-s%C3%B3)" title="Hók (nguòng-só) – Mindong" lang="cdo" hreflang="cdo" data-title="Hók (nguòng-só)" data-language-autonym="閩東語 / Mìng-dĕ̤ng-ngṳ̄" data-language-local-name="Mindong" class="interlanguage-link-target">閩東語 / Mìng-dĕ̤ng-ngṳ̄</a></li><li class="interlanguage-link interwiki-mn mw-list-item"><a href="https://mn.wikipedia.org/wiki/%D0%A4%D1%82%D0%BE%D1%80" title="Фтор – Mongolian" lang="mn" hreflang="mn" data-title="Фтор" 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%96%E1%80%9C%E1%80%AD%E1%80%AF%E1%80%9B%E1%80%84%E1%80%BA%E1%80%B8" title="ဖလိုရင်း – Burmese" lang="my" hreflang="my" data-title="ဖလိုရင်း" 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/Fluor_(element)" title="Fluor (element) – Dutch" lang="nl" hreflang="nl" data-title="Fluor (element)" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target">Nederlands</a></li><li class="interlanguage-link interwiki-ne mw-list-item"><a href="https://ne.wikipedia.org/wiki/%E0%A4%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="फ्लोरिन – Nepali" lang="ne" hreflang="ne" data-title="फ्लोरिन" data-language-autonym="नेपाली" data-language-local-name="Nepali" class="interlanguage-link-target">नेपाली</a></li><li class="interlanguage-link interwiki-new mw-list-item"><a href="https://new.wikipedia.org/wiki/%E0%A4%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="फ्लोरिन – Newari" lang="new" hreflang="new" data-title="फ्लोरिन" 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%95%E3%83%83%E7%B4%A0" title="フッ素 – Japanese" lang="ja" hreflang="ja" data-title="フッ素" 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/Fluor" title="Fluor – Northern Frisian" lang="frr" hreflang="frr" data-title="Fluor" 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/Fluor" title="Fluor – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Fluor" 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/Fluor" title="Fluor – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Fluor" data-language-autonym="Norsk nynorsk" data-language-local-name="Norwegian Nynorsk" class="interlanguage-link-target">Norsk nynorsk</a></li><li class="interlanguage-link interwiki-nov mw-list-item"><a href="https://nov.wikipedia.org/wiki/Fluore" title="Fluore – Novial" lang="nov" hreflang="nov" data-title="Fluore" data-language-autonym="Novial" data-language-local-name="Novial" class="interlanguage-link-target">Novial</a></li><li class="interlanguage-link interwiki-oc mw-list-item"><a href="https://oc.wikipedia.org/wiki/Fluor" title="Fluor – Occitan" lang="oc" hreflang="oc" data-title="Fluor" 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%AB%E0%AD%8D%E0%AC%B2%E0%AD%8B%E0%AC%B0%E0%AC%BF%E0%AC%A8" title="ଫ୍ଲୋରିନ – Odia" lang="or" hreflang="or" data-title="ଫ୍ଲୋରିନ" data-language-autonym="ଓଡ଼ିଆ" data-language-local-name="Odia" class="interlanguage-link-target">ଓଡ଼ିଆ</a></li><li class="interlanguage-link interwiki-om mw-list-item"><a href="https://om.wikipedia.org/wiki/Filooriinii" title="Filooriinii – Oromo" lang="om" hreflang="om" data-title="Filooriinii" data-language-autonym="Oromoo" data-language-local-name="Oromo" class="interlanguage-link-target">Oromoo</a></li><li class="interlanguage-link interwiki-uz mw-list-item"><a href="https://uz.wikipedia.org/wiki/Ftor" title="Ftor – Uzbek" lang="uz" hreflang="uz" data-title="Ftor" 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%AB%E0%A8%BC%E0%A8%B2%E0%A9%8B%E0%A8%B0%E0%A9%80%E0%A8%A8" title="ਫ਼ਲੋਰੀਨ – Punjabi" lang="pa" hreflang="pa" data-title="ਫ਼ਲੋਰੀਨ" 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%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="फ्लोरिन – Pali" lang="pi" hreflang="pi" data-title="फ्लोरिन" 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/%D9%81%D9%84%D9%88%D8%B1%DB%8C%D9%86" title="فلورین – Western Punjabi" lang="pnb" hreflang="pnb" data-title="فلورین" data-language-autonym="پنجابی" data-language-local-name="Western Punjabi" class="interlanguage-link-target">پنجابی</a></li><li class="interlanguage-link interwiki-blk mw-list-item"><a href="https://blk.wikipedia.org/wiki/%E1%80%96%E1%80%9C%E1%80%AD%E1%80%AF%E1%80%9B%E1%80%89%E1%80%BA%E1%80%B8" title="ဖလိုရဉ်း – Pa'O" lang="blk" hreflang="blk" data-title="ဖလိုရဉ်း" data-language-autonym="ပအိုဝ်ႏဘာႏသာႏ" data-language-local-name="Pa'O" class="interlanguage-link-target">ပအိုဝ်ႏဘာႏသာႏ</a></li><li class="interlanguage-link interwiki-ps mw-list-item"><a href="https://ps.wikipedia.org/wiki/%D9%81%D9%84%D9%88%D8%B1%D9%8A%D9%86" title="فلورين – Pashto" lang="ps" hreflang="ps" data-title="فلورين" 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/Flu%C3%B2r" title="Fluòr – Piedmontese" lang="pms" hreflang="pms" data-title="Fluòr" 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/Fluor" title="Fluor – Low German" lang="nds" hreflang="nds" data-title="Fluor" 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/Fluor" title="Fluor – Polish" lang="pl" hreflang="pl" data-title="Fluor" 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/Fl%C3%BAor" title="Flúor – Portuguese" lang="pt" hreflang="pt" data-title="Flúor" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target">Português</a></li><li class="interlanguage-link interwiki-ro mw-list-item"><a href="https://ro.wikipedia.org/wiki/Fluor" title="Fluor – Romanian" lang="ro" hreflang="ro" data-title="Fluor" 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/Flur" title="Flur – Quechua" lang="qu" hreflang="qu" data-title="Flur" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Russian" lang="ru" hreflang="ru" data-title="Фтор" 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%AB%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BF%E0%A4%A8" title="फ्लोरिन – Sanskrit" lang="sa" hreflang="sa" data-title="फ्लोरिन" data-language-autonym="संस्कृतम्" data-language-local-name="Sanskrit" class="interlanguage-link-target">संस्कृतम्</a></li><li class="interlanguage-link interwiki-sat mw-list-item"><a href="https://sat.wikipedia.org/wiki/%E1%B1%AF%E1%B1%B7%E1%B1%9E%E1%B1%9A%E1%B1%A8%E1%B1%A4%E1%B1%B1" title="ᱯᱷᱞᱚᱨᱤᱱ – Santali" lang="sat" hreflang="sat" data-title="ᱯᱷᱞᱚᱨᱤᱱ" data-language-autonym="ᱥᱟᱱᱛᱟᱲᱤ" data-language-local-name="Santali" class="interlanguage-link-target">ᱥᱟᱱᱛᱟᱲᱤ</a></li><li class="interlanguage-link interwiki-sco mw-list-item"><a href="https://sco.wikipedia.org/wiki/Fluorine" title="Fluorine – Scots" lang="sco" hreflang="sco" data-title="Fluorine" data-language-autonym="Scots" data-language-local-name="Scots" class="interlanguage-link-target">Scots</a></li><li class="interlanguage-link interwiki-stq mw-list-item"><a href="https://stq.wikipedia.org/wiki/Fluor" title="Fluor – Saterland Frisian" lang="stq" hreflang="stq" data-title="Fluor" 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/Fluori" title="Fluori – Albanian" lang="sq" hreflang="sq" data-title="Fluori" 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/Fluoru" title="Fluoru – Sicilian" lang="scn" hreflang="scn" data-title="Fluoru" data-language-autonym="Sicilianu" data-language-local-name="Sicilian" class="interlanguage-link-target">Sicilianu</a></li><li class="interlanguage-link interwiki-si mw-list-item"><a href="https://si.wikipedia.org/wiki/%E0%B7%86%E0%B7%8A%E0%B6%BD%E0%B7%96%E0%B7%80%E0%B7%9C%E0%B6%BB%E0%B7%92%E0%B6%B1%E0%B7%8A" title="ෆ්ලූවොරින් – Sinhala" lang="si" hreflang="si" data-title="ෆ්ලූවොරින්" data-language-autonym="සිංහල" data-language-local-name="Sinhala" class="interlanguage-link-target">සිංහල</a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Fluorine" title="Fluorine – Simple English" lang="en-simple" hreflang="en-simple" data-title="Fluorine" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target">Simple English</a></li><li class="interlanguage-link interwiki-sd mw-list-item"><a href="https://sd.wikipedia.org/wiki/%D9%81%D9%84%D9%88%D8%B1%D9%8A%D9%86" title="فلورين – Sindhi" lang="sd" hreflang="sd" data-title="فلورين" data-language-autonym="سنڌي" data-language-local-name="Sindhi" class="interlanguage-link-target">سنڌي</a></li><li class="interlanguage-link interwiki-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/Flu%C3%B3r" title="Fluór – Slovak" lang="sk" hreflang="sk" data-title="Fluór" 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/Fluor" title="Fluor – Slovenian" lang="sl" hreflang="sl" data-title="Fluor" data-language-autonym="Slovenščina" data-language-local-name="Slovenian" class="interlanguage-link-target">Slovenščina</a></li><li class="interlanguage-link interwiki-szl mw-list-item"><a href="https://szl.wikipedia.org/wiki/Fluor" title="Fluor – Silesian" lang="szl" hreflang="szl" data-title="Fluor" data-language-autonym="Ślůnski" data-language-local-name="Silesian" class="interlanguage-link-target">Ślůnski</a></li><li class="interlanguage-link interwiki-so mw-list-item"><a href="https://so.wikipedia.org/wiki/Foloriin" title="Foloriin – Somali" lang="so" hreflang="so" data-title="Foloriin" 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/%D9%81%D9%84%DB%86%D8%B1" title="فلۆر – Central Kurdish" lang="ckb" hreflang="ckb" data-title="فلۆر" 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%A4%D0%BB%D1%83%D0%BE%D1%80" title="Флуор – Serbian" lang="sr" hreflang="sr" data-title="Флуор" 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/Fluor" title="Fluor – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Fluor" 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/Fluor" title="Fluor – Sundanese" lang="su" hreflang="su" data-title="Fluor" 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/Fluori" title="Fluori – Finnish" lang="fi" hreflang="fi" data-title="Fluori" 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/Fluor" title="Fluor – Swedish" lang="sv" hreflang="sv" data-title="Fluor" 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/Plurina" title="Plurina – Tagalog" lang="tl" hreflang="tl" data-title="Plurina" 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%AA%E0%AF%81%E0%AE%B3%E0%AF%8B%E0%AE%B0%E0%AE%BF%E0%AE%A9%E0%AF%8D" title="புளோரின் – Tamil" lang="ta" hreflang="ta" data-title="புளோரின்" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Tatar" lang="tt" hreflang="tt" data-title="Фтор" 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%AB%E0%B1%8D%E0%B0%B2%E0%B1%8B%E0%B0%B0%E0%B0%BF%E0%B0%A8%E0%B1%8D" title="ఫ్లోరిన్ – Telugu" lang="te" hreflang="te" data-title="ఫ్లోరిన్" data-language-autonym="తెలుగు" data-language-local-name="Telugu" class="interlanguage-link-target">తెలుగు</a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B8%9F%E0%B8%A5%E0%B8%B9%E0%B8%AD%E0%B8%AD%E0%B8%A3%E0%B8%B5%E0%B8%99" title="ฟลูออรีน – Thai" lang="th" hreflang="th" data-title="ฟลูออรีน" 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%A4%D1%82%D0%BE%D1%80" title="Фтор – Tajik" lang="tg" hreflang="tg" data-title="Фтор" data-language-autonym="Тоҷикӣ" data-language-local-name="Tajik" class="interlanguage-link-target">Тоҷикӣ</a></li><li class="interlanguage-link interwiki-chr mw-list-item"><a href="https://chr.wikipedia.org/wiki/%E1%8F%A9%E1%8E%B6%E1%8F%AB%E1%8F%82" title="ᏩᎶᏫᏂ – Cherokee" lang="chr" hreflang="chr" data-title="ᏩᎶᏫᏂ" data-language-autonym="ᏣᎳᎩ" data-language-local-name="Cherokee" class="interlanguage-link-target">ᏣᎳᎩ</a></li><li class="interlanguage-link interwiki-tr mw-list-item"><a href="https://tr.wikipedia.org/wiki/Flor" title="Flor – Turkish" lang="tr" hreflang="tr" data-title="Flor" data-language-autonym="Türkçe" data-language-local-name="Turkish" class="interlanguage-link-target">Türkçe</a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a href="https://uk.wikipedia.org/wiki/%D0%A4%D1%82%D0%BE%D1%80" title="Фтор – Ukrainian" lang="uk" hreflang="uk" data-title="Фтор" 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/%D9%81%D9%84%D9%88%D8%B1%DB%8C%D9%86" title="فلورین – Urdu" lang="ur" hreflang="ur" data-title="فلورین" 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%81%D9%89%D8%AA%D9%88%D8%B1" title="فىتور – Uyghur" lang="ug" hreflang="ug" data-title="فىتور" 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/Ftor" title="Ftor – Veps" lang="vep" hreflang="vep" data-title="Ftor" data-language-autonym="Vepsän kel’" data-language-local-name="Veps" class="interlanguage-link-target">Vepsän kel’</a></li><li class="interlanguage-link interwiki-vi badge-Q17437796 badge-featuredarticle mw-list-item" title="featured article badge"><a href="https://vi.wikipedia.org/wiki/Fluor" title="Fluor – Vietnamese" lang="vi" hreflang="vi" data-title="Fluor" data-language-autonym="Tiếng Việt" data-language-local-name="Vietnamese" class="interlanguage-link-target">Tiếng Việt</a></li><li class="interlanguage-link interwiki-wa mw-list-item"><a href="https://wa.wikipedia.org/wiki/Fluw%C3%B4r" title="Fluwôr – Walloon" lang="wa" hreflang="wa" data-title="Fluwôr" data-language-autonym="Walon" data-language-local-name="Walloon" class="interlanguage-link-target">Walon</a></li><li class="interlanguage-link interwiki-zh-classical mw-list-item"><a href="https://zh-classical.wikipedia.org/wiki/%E6%B0%9F" title="氟 – Literary Chinese" lang="lzh" hreflang="lzh" data-title="氟" 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/Fluor" title="Fluor – Waray" lang="war" hreflang="war" data-title="Fluor" 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/%E6%B0%9F" title="氟 – Wu" lang="wuu" hreflang="wuu" data-title="氟" 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%A4%D7%9C%D7%95%D7%90%D7%A8" title="פלואר – Yiddish" lang="yi" hreflang="yi" data-title="פלואר" 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/Fluor%C3%ADn%C3%AC" title="Fluorínì – Yoruba" lang="yo" hreflang="yo" data-title="Fluorínì" 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/%E6%B0%9F" title="氟 – Cantonese" lang="yue" hreflang="yue" data-title="氟" data-language-autonym="粵語" data-language-local-name="Cantonese" class="interlanguage-link-target">粵語</a></li><li class="interlanguage-link interwiki-zh mw-list-item"><a href="https://zh.wikipedia.org/wiki/%E6%B0%9F" title="氟 – Chinese" lang="zh" hreflang="zh" data-title="氟" data-language-autonym="中文" data-language-local-name="Chinese" class="interlanguage-link-target">中文</a></li><li class="interlanguage-link interwiki-zgh mw-list-item"><a href="https://zgh.wikipedia.org/wiki/%E2%B4%B0%E2%B4%BC%E2%B5%8D%E2%B5%A2%E2%B5%93%E2%B5%94" title="ⴰⴼⵍⵢⵓⵔ – Standard Moroccan Tamazight" lang="zgh" hreflang="zgh" data-title="ⴰⴼⵍⵢⵓⵔ" data-language-autonym="ⵜⴰⵎⴰⵣⵉⵖⵜ ⵜⴰⵏⴰⵡⴰⵢⵜ" data-language-local-name="Standard Moroccan Tamazight" class="interlanguage-link-target">ⵜⴰⵎⴰⵣⵉⵖⵜ ⵜⴰⵏⴰⵡⴰⵢⵜ</a></li> </ul> <div class="after-portlet after-portlet-lang"><a href="https://www.wikidata.org/wiki/Special:EntityPage/Q650#sitelinks-wikipedia" title="Edit interlanguage links" class="wbc-editpage">Edit links</a></div> </div> </div> </div> </header> <div class="vector-page-toolbar"> <div class="vector-page-toolbar-container"> <div id="left-navigation"> <nav 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Click here for more information."><img alt="Featured article" src="//upload.wikimedia.org/wikipedia/en/thumb/e/e7/Cscr-featured.svg/20px-Cscr-featured.svg.png" decoding="async" width="20" height="19" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/e/e7/Cscr-featured.svg/30px-Cscr-featured.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/e/e7/Cscr-featured.svg/40px-Cscr-featured.svg.png 2x" data-file-width="466" data-file-height="443" /></a></div></div> </div> <div id="siteSub" class="noprint">From Wikipedia, the free encyclopedia</div> </div> <div id="contentSub"><div id="mw-content-subtitle"></div></div> <div id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><style data-mw-deduplicate="TemplateStyles:r1236090951">.mw-parser-output .hatnote{font-style:italic}.mw-parser-output div.hatnote{padding-left:1.6em;margin-bottom:0.5em}.mw-parser-output .hatnote i{font-style:normal}.mw-parser-output .hatnote+link+.hatnote{margin-top:-0.5em}@media print{body.ns-0 .mw-parser-output .hatnote{display:none!important}}</style><div role="note" class="hatnote navigation-not-searchable">Not to be confused with <a href="/wiki/Florin" title="Florin">Florin</a>, <a href="/wiki/Fluorene" title="Fluorene">Fluorene</a>, <a href="/wiki/Fluoride" title="Fluoride">Fluoride</a>, <a href="/wiki/Fluorone" title="Fluorone">Fluorone</a>, or <a href="/wiki/Florine" title="Florine">Florine</a>.</div> <div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical element with atomic number 9 (F)</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">Fluorine, 9F</caption><tbody><tr><td colspan="2" class="infobox-image"><a href="/wiki/File:Fluoro_liquido_a_-196%C2%B0C_1.jpg" class="mw-file-description"><img alt="Small sample of pale yellow liquid fluorine condensed in liquid nitrogen" src="//upload.wikimedia.org/wikipedia/commons/thumb/2/2c/Fluoro_liquido_a_-196%C2%B0C_1.jpg/220px-Fluoro_liquido_a_-196%C2%B0C_1.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/2c/Fluoro_liquido_a_-196%C2%B0C_1.jpg/330px-Fluoro_liquido_a_-196%C2%B0C_1.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/2c/Fluoro_liquido_a_-196%C2%B0C_1.jpg/440px-Fluoro_liquido_a_-196%C2%B0C_1.jpg 2x" data-file-width="1177" data-file-height="883" /></a><div class="infobox-caption">Liquid fluorine (F2 at <a href="/wiki/Cryogenics" title="Cryogenics">extremely low temperature</a>)</div></td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Fluorine</th></tr><tr><th scope="row" class="infobox-label">Pronunciation</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" style="margin: 0; text-align: left;"><ul><li style="margin: 0; text-indent: -1em; padding-left: 1em;"><a href="/wiki/Help:IPA/English" title="Help:IPA/English">/ˈflʊəriːn/</a></li><li style="margin: 0; text-indent: -1em; padding-left: 1em;"><a href="/wiki/Help:IPA/English" title="Help:IPA/English">/ˈflɔːriːn/</a> (<a href="/wiki/Help:Pronunciation_respelling_key" title="Help:Pronunciation respelling key">FLOR-een</a>)</li></ul></div></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Allotropy" title="Allotropy">Allotropes</a></th><td class="infobox-data">alpha, beta (see <a href="/wiki/Allotropes_of_fluorine" class="mw-redirect" title="Allotropes of fluorine">Allotropes of fluorine</a>)</td></tr><tr><th scope="row" class="infobox-label">Appearance</th><td class="infobox-data">gas: very pale yellow liquid: bright yellow solid: alpha is opaque, beta is transparent</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°(F)</th></tr><tr><th scope="row" class="infobox-label"></th><td class="infobox-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409" /><div class="plainlist"><ul><li>18.998403162±0.000000005<a href="#cite_note-CIAAW-1">[1]</a></li><li>18.998±0.001 (<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">Fluorine in the <a href="/wiki/Periodic_table" title="Periodic table">periodic table</a></th></tr><tr><td colspan="2" class="infobox-full-data"> <table class="wikitable" style="text-align:center; width:100%; margin:0;"> <tbody><tr> <td> <table class="periodictable" style="margin:0 auto"> <tbody><tr> <td style="border:none; width:5px"><div style="background-color:transparent; color:inherit; margin:0; padding:0; text-align:center; border:none;"> <table style="empty-cells:hidden; border:none; padding:0; border-spacing:1px; border-collapse:separate; margin:0;"> <tbody><tr> <td style="border:none;padding:0;"><a href="/wiki/Hydrogen" title="Hydrogen">Hydrogen</a> </td> <td colspan="30" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Helium" title="Helium">Helium</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Lithium" title="Lithium">Lithium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Beryllium" title="Beryllium">Beryllium</a> </td> <td colspan="24" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Boron" title="Boron">Boron</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Carbon" title="Carbon">Carbon</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nitrogen" title="Nitrogen">Nitrogen</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Oxygen" title="Oxygen">Oxygen</a> </td> <td style="border:none;padding:0;"><a class="mw-selflink selflink">Fluorine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Neon" title="Neon">Neon</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Sodium" title="Sodium">Sodium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Magnesium" title="Magnesium">Magnesium</a> </td> <td colspan="24" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Aluminium" title="Aluminium">Aluminium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Silicon" title="Silicon">Silicon</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Phosphorus" title="Phosphorus">Phosphorus</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Sulfur" title="Sulfur">Sulfur</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Chlorine" title="Chlorine">Chlorine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Argon" title="Argon">Argon</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Potassium" title="Potassium">Potassium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Calcium" title="Calcium">Calcium</a> </td> <td colspan="14" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Scandium" title="Scandium">Scandium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Titanium" title="Titanium">Titanium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Vanadium" title="Vanadium">Vanadium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Chromium" title="Chromium">Chromium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Manganese" title="Manganese">Manganese</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Iron" title="Iron">Iron</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Cobalt" title="Cobalt">Cobalt</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nickel" title="Nickel">Nickel</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Copper" title="Copper">Copper</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Zinc" title="Zinc">Zinc</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Gallium" title="Gallium">Gallium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Germanium" title="Germanium">Germanium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Arsenic" title="Arsenic">Arsenic</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Selenium" title="Selenium">Selenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Bromine" title="Bromine">Bromine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Krypton" title="Krypton">Krypton</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Rubidium" title="Rubidium">Rubidium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Strontium" title="Strontium">Strontium</a> </td> <td style="border:none;padding:0;; width:0;"> </td> <td colspan="13" style="border:none;padding:0;"> </td> <td style="border:none;padding:0;"><a href="/wiki/Yttrium" title="Yttrium">Yttrium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Zirconium" title="Zirconium">Zirconium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Niobium" title="Niobium">Niobium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Molybdenum" title="Molybdenum">Molybdenum</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Technetium" title="Technetium">Technetium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Ruthenium" title="Ruthenium">Ruthenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Rhodium" title="Rhodium">Rhodium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Palladium" title="Palladium">Palladium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Silver" title="Silver">Silver</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Cadmium" title="Cadmium">Cadmium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Indium" title="Indium">Indium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tin" title="Tin">Tin</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Antimony" title="Antimony">Antimony</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tellurium" title="Tellurium">Tellurium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Iodine" title="Iodine">Iodine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Xenon" title="Xenon">Xenon</a> </td></tr> <tr style="border:none;padding:0;"> <td style="border:none;padding:0;"><a href="/wiki/Caesium" title="Caesium">Caesium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Barium" title="Barium">Barium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lanthanum" title="Lanthanum">Lanthanum</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Cerium" title="Cerium">Cerium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Praseodymium" title="Praseodymium">Praseodymium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Neodymium" title="Neodymium">Neodymium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Promethium" title="Promethium">Promethium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Samarium" title="Samarium">Samarium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Europium" title="Europium">Europium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Gadolinium" title="Gadolinium">Gadolinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Terbium" title="Terbium">Terbium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Dysprosium" title="Dysprosium">Dysprosium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Holmium" title="Holmium">Holmium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Erbium" title="Erbium">Erbium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Thulium" title="Thulium">Thulium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Ytterbium" title="Ytterbium">Ytterbium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lutetium" title="Lutetium">Lutetium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Hafnium" title="Hafnium">Hafnium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tantalum" title="Tantalum">Tantalum</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tungsten" title="Tungsten">Tungsten</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Rhenium" title="Rhenium">Rhenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Osmium" title="Osmium">Osmium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Iridium" title="Iridium">Iridium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Platinum" title="Platinum">Platinum</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Gold" title="Gold">Gold</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Mercury_(element)" title="Mercury (element)">Mercury (element)</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Thallium" title="Thallium">Thallium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lead" title="Lead">Lead</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Bismuth" title="Bismuth">Bismuth</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Polonium" title="Polonium">Polonium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Astatine" title="Astatine">Astatine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Radon" title="Radon">Radon</a> </td></tr> <tr> <td style="border:none;padding:0;"><a href="/wiki/Francium" title="Francium">Francium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Radium" title="Radium">Radium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Actinium" title="Actinium">Actinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Thorium" title="Thorium">Thorium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Protactinium" title="Protactinium">Protactinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Uranium" title="Uranium">Uranium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Neptunium" title="Neptunium">Neptunium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Plutonium" title="Plutonium">Plutonium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Americium" title="Americium">Americium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Curium" title="Curium">Curium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Berkelium" title="Berkelium">Berkelium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Californium" title="Californium">Californium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Einsteinium" title="Einsteinium">Einsteinium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Fermium" title="Fermium">Fermium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Mendelevium" title="Mendelevium">Mendelevium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nobelium" title="Nobelium">Nobelium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Lawrencium" title="Lawrencium">Lawrencium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Rutherfordium" title="Rutherfordium">Rutherfordium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Dubnium" title="Dubnium">Dubnium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Seaborgium" title="Seaborgium">Seaborgium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Bohrium" title="Bohrium">Bohrium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Hassium" title="Hassium">Hassium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Meitnerium" title="Meitnerium">Meitnerium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Darmstadtium" title="Darmstadtium">Darmstadtium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Roentgenium" title="Roentgenium">Roentgenium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Copernicium" title="Copernicium">Copernicium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Nihonium" title="Nihonium">Nihonium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Flerovium" title="Flerovium">Flerovium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Moscovium" title="Moscovium">Moscovium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Livermorium" title="Livermorium">Livermorium</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Tennessine" title="Tennessine">Tennessine</a> </td> <td style="border:none;padding:0;"><a href="/wiki/Oganesson" title="Oganesson">Oganesson</a> </td></tr></tbody></table> </div> </td> <td style="vertical-align:middle; text-align:center; font-size:90%; line-height:100%; width:10px; border:none;">– ↑ F ↓ <a href="/wiki/Chlorine" title="Chlorine">Cl</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/Oxygen" title="Oxygen">oxygen</a> ← fluorine → <a href="/wiki/Neon" title="Neon">neon</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">9</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_2_element" title="Period 2 element">period 2</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/Helium" title="Helium">He</a>] 2s2 2p5<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000381-3">[3]</a></td></tr><tr><th scope="row" class="infobox-label">Electrons per shell</th><td class="infobox-data">2, 7</td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">Physical properties</th></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Phase_(matter)" title="Phase (matter)">Phase</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r886047488" />at <a href="/wiki/Standard_temperature_and_pressure" title="Standard temperature and pressure">STP</a></th><td class="infobox-data"><a href="/wiki/Gas" title="Gas">gas</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Melting_point" title="Melting point">Melting point</a></th><td class="infobox-data">(F2) 53.48 <a href="/wiki/Kelvin" title="Kelvin">K</a> (−219.67 °C, −363.41 °F)<a href="#cite_note-FOOTNOTEHaynes20114.121-4">[4]</a> </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">(F2) 85.03 K (−188.11 °C, −306.60 °F)<a href="#cite_note-FOOTNOTEHaynes20114.121-4">[4]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Density" title="Density">Density</a> (at STP)</th><td class="infobox-data">1.696 g/L<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000382-5">[5]</a></td></tr><tr><th scope="row" class="infobox-label">when liquid (at <a href="/wiki/Boiling_point" title="Boiling point">b.p.</a>)</th><td class="infobox-data">1.505 g/cm3<a href="#cite_note-FOOTNOTECompressed_Gas_Association1999365-6">[6]</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">53.48 K, .252 kPa<a href="#cite_note-7">[7]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Critical_point_(thermodynamics)" title="Critical point (thermodynamics)">Critical point</a></th><td class="infobox-data">144.41 K, 5.1724 MPa<a href="#cite_note-FOOTNOTEHaynes20114.121-4">[4]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Enthalpy_of_vaporization" title="Enthalpy of vaporization">Heat of vaporization</a></th><td class="infobox-data">6.51 kJ/mol<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000382-5">[5]</a> </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">Cp: 31 J/(mol·K)<a href="#cite_note-FOOTNOTECompressed_Gas_Association1999365-6">[6]</a> (at 21.1 °C) Cv: 23 J/(mol·K)<a href="#cite_note-FOOTNOTECompressed_Gas_Association1999365-6">[6]</a> (at 21.1 °C)</td></tr><tr><td colspan="2" class="infobox-full-data"><a href="/wiki/Vapor_pressure" title="Vapor pressure">Vapor pressure</a><div style="position:relative; margin:0 auto; padding:0; text-align:initial; width:-moz-fit-content; width:-webkit-fit-content; width:fit-content;"> <table class="wikitable" style="text-align:center; font-size:90%; border-collapse:collapse; margin:0"> <tbody><tr> <th><abbr title="Pressure">P</abbr> (Pa) </th> <th>1 </th> <th>10 </th> <th>100 </th> <th>1 k </th> <th>10 k </th> <th>100 k </th></tr> <tr> <th>at <abbr title="Temperature">T</abbr> (K) </th> <td>38 </td> <td>44 </td> <td>50 </td> <td>58 </td> <td>69 </td> <td>85 </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 0<a href="#cite_note-8">[8]</a></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Electronegativity" title="Electronegativity">Electronegativity</a></th><td class="infobox-data">Pauling scale: 3.98<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000381-3">[3]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Ionization_energy" title="Ionization energy">Ionization energies</a></th><td class="infobox-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409" /><div class="plainlist"><ul><li>1st: 1681 kJ/mol </li><li>2nd: 3374 kJ/mol </li><li>3rd: 6147 kJ/mol </li><li>(<a href="/wiki/Molar_ionization_energies_of_the_elements#fluorine" title="Molar ionization energies of the elements">more</a>)<a href="#cite_note-FOOTNOTEDean19994.6-9">[9]</a> </li></ul></div></td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Covalent_radius" title="Covalent radius">Covalent radius</a></th><td class="infobox-data">64 <a href="/wiki/Picometre" title="Picometre">pm</a><a href="#cite_note-FOOTNOTEDean19994.35-10">[10]</a> </td></tr><tr><th scope="row" class="infobox-label"><a href="/wiki/Van_der_Waals_radius" title="Van der Waals radius">Van der Waals radius</a></th><td class="infobox-data">135 pm<a href="#cite_note-FOOTNOTEMatsui2006257-11">[11]</a> </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:9_(F_I)_NIST_ASD_emission_spectrum.png" class="mw-file-description"><img alt="Color lines in a spectral range" src="//upload.wikimedia.org/wikipedia/commons/thumb/1/18/9_%28F_I%29_NIST_ASD_emission_spectrum.png/240px-9_%28F_I%29_NIST_ASD_emission_spectrum.png" decoding="async" width="240" height="29" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/18/9_%28F_I%29_NIST_ASD_emission_spectrum.png/360px-9_%28F_I%29_NIST_ASD_emission_spectrum.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/18/9_%28F_I%29_NIST_ASD_emission_spectrum.png/480px-9_%28F_I%29_NIST_ASD_emission_spectrum.png 2x" data-file-width="4000" data-file-height="480" /></a><figcaption></figcaption></figure><a href="/wiki/Spectral_line" title="Spectral line">Spectral lines</a> of fluorine</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/Cubic_crystal_system" title="Cubic crystal system">cubic</a><div style="float:right;"><a href="/wiki/File:Cubic.svg" class="mw-file-description"><img alt="Cubic crystal structure for fluorine" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/55/Cubic.svg/60px-Cubic.svg.png" decoding="async" width="50" height="58" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/55/Cubic.svg/75px-Cubic.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/55/Cubic.svg/100px-Cubic.svg.png 2x" data-file-width="109" data-file-height="127" /></a></div></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">0.02591 W/(m⋅K)<a href="#cite_note-FOOTNOTEYawsBraker2001385-12">[12]</a> </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> (−1.2×10−4)<a href="#cite_note-FOOTNOTEMackayMackayHenderson200272-13">[13]</a><a href="#cite_note-FOOTNOTECheng_et_al.1999-14">[14]</a> </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">7782-41-4<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000381-3">[3]</a> </td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c">History</th></tr><tr><th scope="row" class="infobox-label">Naming</th><td class="infobox-data">after the mineral <a href="/wiki/Fluorite" title="Fluorite">fluorite</a>, itself named after Latin fluo (to flow, in smelting)</td></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></th><td class="infobox-data"><a href="/wiki/Andr%C3%A9-Marie_Amp%C3%A8re" title="André-Marie Ampère">André-Marie Ampère</a> (1810)</td></tr><tr><th scope="row" class="infobox-label">First isolation</th><td class="infobox-data"><a href="/wiki/Henri_Moissan" title="Henri Moissan">Henri Moissan</a><a href="#cite_note-FOOTNOTEJaccaud_et_al.2000381-3">[3]</a> (June 26, 1886)</td></tr><tr><th scope="row" class="infobox-label">Named by</th><td class="infobox-data"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409" /><div class="plainlist"> <ul><li><a href="/wiki/Humphry_Davy" title="Humphry Davy">Humphry Davy</a></li> <li><a href="/wiki/Andr%C3%A9-Marie_Amp%C3%A8re" title="André-Marie Ampère">André-Marie Ampère</a></li></ul> </div></td></tr><tr><th colspan="2" class="infobox-header" style="color:inherit; background:#fdff8c"><a href="/wiki/Isotopes_of_fluorine" title="Isotopes of fluorine">Isotopes of fluorine</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 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.navbar-collapse{float:left;text-align:left}.mw-parser-output .navbar-boxtext{word-spacing:0}.mw-parser-output .navbar ul{display:inline-block;white-space:nowrap;line-height:inherit}.mw-parser-output .navbar-brackets::before{margin-right:-0.125em;content:"[ "}.mw-parser-output .navbar-brackets::after{margin-left:-0.125em;content:" ]"}.mw-parser-output .navbar li{word-spacing:-0.125em}.mw-parser-output .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_fluorine_isotopes" title="Template:Infobox fluorine isotopes"><abbr title="View this template">v</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Infobox_fluorine_isotopes" title="Special:EditPage/Template:Infobox fluorine 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/Fluorine-18" title="Fluorine-18">18F</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;">109.734 min </td> <td style="text-align: left; vertical-align: top;"><a href="/wiki/Beta_plus_decay" class="mw-redirect" title="Beta plus decay">β+</a> </td> <td style="text-align: right; vertical-align: middle;">18O </td></tr> <tr> <th rowspan="1" style="vertical-align: top;">19F </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></tbody></table><div style="text-align:left; padding-left:0.5em; background: #F8F9FA;"><a href="#cite_note-FOOTNOTEChistéBé2011-15">[15]</a></div></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:Fluorine" title="Category:Fluorine">Category: Fluorine</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_fluorine" title="Template:Infobox fluorine">view</a></li><li class="nv-talk"><a href="/wiki/Template_talk:Infobox_fluorine" title="Template talk:Infobox fluorine">talk</a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Infobox_fluorine" title="Special:EditPage/Template:Infobox fluorine">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> Fluorine 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> F and <a href="/wiki/Atomic_number" title="Atomic number">atomic number</a> 9. It is the lightest <a href="/wiki/Halogen" title="Halogen">halogen</a><a href="#cite_note-16">[note 1]</a> and exists at <a href="/wiki/Standard_temperature_and_pressure" title="Standard temperature and pressure">standard conditions</a> as pale yellow <a href="/wiki/Diatomic_molecule" title="Diatomic molecule">diatomic</a> gas. Fluorine is extremely <a href="/wiki/Reactivity_(chemistry)" title="Reactivity (chemistry)">reactive</a> as it reacts with all other <a href="/wiki/Periodic_table" title="Periodic table">elements</a> except for the light <a href="/wiki/Noble_gas" title="Noble gas">noble gases</a>. It is highly <a href="/wiki/Toxicity" title="Toxicity">toxic</a>. Among the elements, fluorine ranks <a href="/wiki/Abundance_of_the_chemical_elements" title="Abundance of the chemical elements">24th in cosmic abundance and 13th in crustal abundance</a>. <a href="/wiki/Fluorite" title="Fluorite">Fluorite</a>, the primary mineral source of fluorine, which gave the element its name, was first described in 1529; as it was added to metal <a href="/wiki/Ore" title="Ore">ores</a> to lower their melting points for <a href="/wiki/Smelting" title="Smelting">smelting</a>, the Latin verb fluo meaning 'to flow' gave the mineral its name. Proposed as an element in 1810, fluorine proved difficult and dangerous to separate from its compounds, and several early experimenters died or sustained injuries from their attempts. Only in 1886 did French chemist <a href="/wiki/Henri_Moissan" title="Henri Moissan">Henri Moissan</a> isolate elemental fluorine using low-temperature <a href="/wiki/Electrolysis" title="Electrolysis">electrolysis</a>, a process still employed for modern production. Industrial production of fluorine gas for <a href="/wiki/Enriched_uranium#Enrichment_methods" title="Enriched uranium">uranium enrichment</a>, its largest application, began during the <a href="/wiki/Manhattan_Project" title="Manhattan Project">Manhattan Project</a> in <a href="/wiki/World_War_II" title="World War II">World War II</a>. Owing to the expense of refining pure fluorine, most commercial applications use fluorine compounds, with about half of mined fluorite used in <a href="/wiki/Steelmaking" title="Steelmaking">steelmaking</a>. The rest of the fluorite is converted into <a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">hydrogen fluoride</a> en route to various organic fluorides, or into <a href="/wiki/Cryolite" title="Cryolite">cryolite</a>, which plays a key role in <a href="/wiki/Hall%E2%80%93H%C3%A9roult_process" title="Hall–Héroult process">aluminium refining</a>. The <a href="/wiki/Carbon%E2%80%93fluorine_bond" title="Carbon–fluorine bond">carbon–fluorine bond</a> is usually very stable. Organofluorine compounds are widely used as <a href="/wiki/Refrigerant" title="Refrigerant">refrigerants</a>, electrical insulation, and <a href="/wiki/Polytetrafluoroethylene" title="Polytetrafluoroethylene">PTFE</a> (Teflon). Pharmaceuticals such as <a href="/wiki/Atorvastatin" title="Atorvastatin">atorvastatin</a> and <a href="/wiki/Fluoxetine" title="Fluoxetine">fluoxetine</a> contain C−F bonds. The <a href="/wiki/Fluoride" title="Fluoride">fluoride ion</a> from dissolved fluoride salts inhibits dental cavities and so finds use in <a href="/wiki/Toothpaste" title="Toothpaste">toothpaste</a> and <a href="/wiki/Water_fluoridation" title="Water fluoridation">water fluoridation</a>. <a href="/wiki/Fluorochemical_industry" title="Fluorochemical industry">Global fluorochemical</a> sales amount to more than <a href="/wiki/United_States_dollar" title="United States dollar">US$</a>15 billion a year. <a href="/wiki/Fluorocarbon" title="Fluorocarbon">Fluorocarbon</a> gases are generally <a href="/wiki/Greenhouse_gas" title="Greenhouse gas">greenhouse gases</a> with <a href="/wiki/Global_warming_potential" title="Global warming potential">global-warming potentials</a> 100 to 23,500 times that of <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a>, and <a href="/wiki/Sulfur_hexafluoride" title="Sulfur hexafluoride">SF6</a> has the highest global warming potential of any known substance. <a href="/wiki/Organofluorine_chemistry" title="Organofluorine chemistry">Organofluorine compounds</a> often persist in the environment due to the strength of the carbon–fluorine bond. Fluorine has no known metabolic role in mammals; a few <a href="/wiki/Plant" title="Plant">plants</a> and <a href="/wiki/Sponge" title="Sponge">marine sponges</a> synthesize organofluorine poisons (most often <a href="/wiki/Fluoroacetic_acid" title="Fluoroacetic acid">monofluoroacetates</a>) that help deter predation.<a href="#cite_note-FOOTNOTELee_et_al.2014-17">[16]</a> <style data-mw-deduplicate="TemplateStyles:r886046785">.mw-parser-output .toclimit-2 .toclevel-1 ul,.mw-parser-output .toclimit-3 .toclevel-2 ul,.mw-parser-output .toclimit-4 .toclevel-3 ul,.mw-parser-output .toclimit-5 .toclevel-4 ul,.mw-parser-output .toclimit-6 .toclevel-5 ul,.mw-parser-output .toclimit-7 .toclevel-6 ul{display:none}</style><div class="toclimit-3"><meta property="mw:PageProp/toc" /></div> <div class="mw-heading mw-heading2"><h2 id="Characteristics">Characteristics</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=1" title="Edit section: Characteristics">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="Electron_configuration">Electron configuration</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=2" title="Edit section: Electron configuration">edit</a>]</div> Fluorine atoms have nine electrons, one fewer than <a href="/wiki/Neon" title="Neon">neon</a>, and <a href="/wiki/Electron_configuration" title="Electron configuration">electron configuration</a> 1s22s22p5: two electrons in a filled inner shell and seven in an outer shell requiring one more to be filled. The outer electrons are ineffective at nuclear <a href="/wiki/Shielding_effect" title="Shielding effect">shielding</a>, and experience a high <a href="/wiki/Effective_nuclear_charge" title="Effective nuclear charge">effective nuclear charge</a> of 9 − 2 = 7; this affects the atom's physical properties.<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000381-3">[3]</a> Fluorine's <a href="/wiki/Ionization_energy" title="Ionization energy">first ionization energy</a> is third-highest among all elements, behind helium and neon,<a href="#cite_note-FOOTNOTEDean1999564-18">[17]</a> which complicates the removal of electrons from neutral fluorine atoms. It also has a high <a href="/wiki/Electron_affinity" title="Electron affinity">electron affinity</a>, second only to <a href="/wiki/Chlorine" title="Chlorine">chlorine</a>,<a href="#cite_note-FOOTNOTELide200410.137–10.138-19">[18]</a> and tends to capture an electron to become <a href="/wiki/Isoelectronicity" title="Isoelectronicity">isoelectronic</a> with the noble gas neon;<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000381-3">[3]</a> it has the highest <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a> of any reactive element.<a href="#cite_note-20">[19]</a> Fluorine atoms have a small <a href="/wiki/Covalent_radius_of_fluorine" title="Covalent radius of fluorine">covalent radius</a> of around 60 <a href="/wiki/Picometer" class="mw-redirect" title="Picometer">picometers</a>, similar to those of its <a href="/wiki/Period_2_element" title="Period 2 element">period</a> neighbors oxygen and neon.<a href="#cite_note-CSD-21">[20]</a><a href="#cite_note-22">[21]</a><a href="#cite_note-23">[note 2]</a> <div style="clear:left;" class=""></div> <div class="mw-heading mw-heading3"><h3 id="Reactivity">Reactivity</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=3" title="Edit section: Reactivity">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1257001546" /><table class="infobox" style="width: 240px; clear: right; float:right;margin:0 0 1.5em 1.5em"><tbody><tr><th colspan="2" class="infobox-above" style="font-size:115%">External videos</th></tr><tr><td colspan="2" class="infobox-full-data" style="text-align: left"><img alt="video icon" src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1b/Nuvola_apps_kaboodle.svg/16px-Nuvola_apps_kaboodle.svg.png" decoding="async" width="16" height="16" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/1b/Nuvola_apps_kaboodle.svg/24px-Nuvola_apps_kaboodle.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/1b/Nuvola_apps_kaboodle.svg/32px-Nuvola_apps_kaboodle.svg.png 2x" data-file-width="128" data-file-height="128" /> <a rel="nofollow" class="external text" href="https://www.youtube.com/watch?v=vtWp45Eewtw">Bright flames</a> during fluorine reactions</td></tr><tr><td colspan="2" class="infobox-full-data" style="text-align: left"><img alt="video icon" src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1b/Nuvola_apps_kaboodle.svg/16px-Nuvola_apps_kaboodle.svg.png" decoding="async" width="16" height="16" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/1b/Nuvola_apps_kaboodle.svg/24px-Nuvola_apps_kaboodle.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/1b/Nuvola_apps_kaboodle.svg/32px-Nuvola_apps_kaboodle.svg.png 2x" data-file-width="128" data-file-height="128" /> Fluorine <a rel="nofollow" class="external text" href="https://www.youtube.com/watch?v=TLOFaWdPxB0">reacting with caesium</a></td></tr></tbody></table> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Fluorine_molecule_ball.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/8/8c/Fluorine_molecule_ball.svg/250px-Fluorine_molecule_ball.svg.png" decoding="async" width="220" height="161" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/8c/Fluorine_molecule_ball.svg/330px-Fluorine_molecule_ball.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/8c/Fluorine_molecule_ball.svg/500px-Fluorine_molecule_ball.svg.png 2x" data-file-width="639" data-file-height="469" /></a><figcaption>Fluorine 3D molecule</figcaption></figure> The <a href="/wiki/Bond_energy" title="Bond energy">bond energy</a> of <a href="/wiki/Compounds_of_fluorine#Difluorine" class="mw-redirect" title="Compounds of fluorine">difluorine</a> is much lower than that of either Cl 2 or Br 2 and similar to the easily cleaved <a href="/wiki/Peroxide" title="Peroxide">peroxide</a> bond; this, along with high electronegativity, accounts for fluorine's easy <a href="/wiki/Dissociation_(chemistry)" title="Dissociation (chemistry)">dissociation</a>, high reactivity, and strong bonds to non-fluorine atoms.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998804-24">[22]</a><a href="#cite_note-25">[23]</a> Conversely, bonds to other atoms are very strong because of fluorine's high electronegativity. Unreactive substances like <a href="/wiki/Powder_coating" title="Powder coating">powdered steel</a>, glass fragments, and <a href="/wiki/Asbestos" title="Asbestos">asbestos</a> fibers react quickly with cold fluorine gas; wood and water spontaneously combust under a fluorine jet.<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000382-5">[5]</a><a href="#cite_note-pop_mechanics_F_reactivity-26">[24]</a> Reactions of elemental fluorine with metals require varying conditions. <a href="/wiki/Alkali_metal" title="Alkali metal">Alkali metals</a> cause explosions and <a href="/wiki/Alkaline_earth_metal" title="Alkaline earth metal">alkaline earth metals</a> display vigorous activity in bulk; to prevent <a href="/wiki/Passivation_(chemistry)" title="Passivation (chemistry)">passivation</a> from the formation of metal fluoride layers, most other metals such as aluminium and iron must be powdered,<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998804-24">[22]</a> and <a href="/wiki/Noble_metal" title="Noble metal">noble metals</a> require pure fluorine gas at 300–450 °C (572–842 °F).<a href="#cite_note-FOOTNOTELidinMolochkoAndreeva2000442–455-27">[25]</a> Some solid nonmetals (sulfur, phosphorus) react vigorously in liquid fluorine.<a href="#cite_note-FOOTNOTEWibergWibergHolleman2001404-28">[26]</a> <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">Hydrogen sulfide</a><a href="#cite_note-FOOTNOTEWibergWibergHolleman2001404-28">[26]</a> and <a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a><a href="#cite_note-FOOTNOTEPatnaik2007472-29">[27]</a> combine readily with fluorine, the latter sometimes explosively; <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a> exhibits much less activity, requiring elevated temperatures.<a href="#cite_note-FOOTNOTEAigueperse_et_al.2000400-30">[28]</a> <a href="/wiki/Hydrogen" title="Hydrogen">Hydrogen</a>, like some of the alkali metals, reacts explosively with fluorine.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw199876,_804-31">[29]</a> <a href="/wiki/Carbon" title="Carbon">Carbon</a>, as <a href="/wiki/Lamp_black" class="mw-redirect" title="Lamp black">lamp black</a>, reacts at room temperature to yield <a href="/wiki/Tetrafluoromethane" class="mw-redirect" title="Tetrafluoromethane">tetrafluoromethane</a>. Graphite combines with fluorine above 400 °C (752 °F) to produce <a href="/wiki/Non-stoichiometric_compound" title="Non-stoichiometric compound">non-stoichiometric</a> <a href="/wiki/Carbon_monofluoride" title="Carbon monofluoride">carbon monofluoride</a>; higher temperatures generate gaseous <a href="/wiki/Fluorocarbon" title="Fluorocarbon">fluorocarbons</a>, sometimes with explosions.<a href="#cite_note-Kuriakose,_A._K.-32">[30]</a> Carbon dioxide and carbon monoxide react at or just above room temperature,<a href="#cite_note-Hasegawa,_Yasuo-33">[31]</a> whereas <a href="/wiki/Paraffin_wax" title="Paraffin wax">paraffins</a> and other organic chemicals generate strong reactions:<a href="#cite_note-34">[32]</a> even completely substituted <a href="/wiki/Haloalkane" title="Haloalkane">haloalkanes</a> such as <a href="/wiki/Carbon_tetrachloride" title="Carbon tetrachloride">carbon tetrachloride</a>, normally incombustible, may explode.<a href="#cite_note-Navarrini,_Walter-35">[33]</a> Although <a href="/wiki/Nitrogen_trifluoride" title="Nitrogen trifluoride">nitrogen trifluoride</a> is stable, nitrogen requires an <a href="/wiki/Electric_discharge_in_gases" title="Electric discharge in gases">electric discharge</a> at elevated temperatures for reaction with fluorine to occur, due to the very strong <a href="/wiki/Triple_bond" title="Triple bond">triple bond</a> in elemental nitrogen;<a href="#cite_note-FOOTNOTELidinMolochkoAndreeva2000252-36">[34]</a> ammonia may react explosively.<a href="#cite_note-Anhydrous_ammonia_MSDS-37">[35]</a><a href="#cite_note-Scott_I._Morrow-38">[36]</a> <a href="/wiki/Oxygen" title="Oxygen">Oxygen</a> does not combine with fluorine under ambient conditions, but can be made to react using electric discharge at low temperatures and pressures; the products tend to disintegrate into their constituent elements when heated.<a href="#cite_note-Emeléus_Sharpe_1974_111-39">[37]</a><a href="#cite_note-FOOTNOTEWibergWibergHolleman2001457-40">[38]</a><a href="#cite_note-41">[39]</a> Heavier halogens<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000383-42">[40]</a> react readily with fluorine as does the noble gas <a href="/wiki/Radon" title="Radon">radon</a>;<a href="#cite_note-43">[41]</a> of the other noble gases, only <a href="/wiki/Xenon" title="Xenon">xenon</a> and <a href="/wiki/Krypton" title="Krypton">krypton</a> react, and only under special conditions.<a href="#cite_note-Khriachtchev_et_al._2000-44">[42]</a> <a href="/wiki/Argon" title="Argon">Argon</a> does not react with fluorine gas; however, it does form a compound with fluorine, <a href="/wiki/Argon_fluorohydride" title="Argon fluorohydride">argon fluorohydride</a>. <div style="clear:left;" class=""></div> <div class="mw-heading mw-heading3"><h3 id="Phases">Phases</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=4" title="Edit section: Phases">edit</a>]</div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Beta_fluorine_unit_cell.svg" class="mw-file-description"><img alt="Cube with spherical shapes on the corners and center and spinning molecules in planes in faces" src="//upload.wikimedia.org/wikipedia/commons/thumb/8/88/Beta_fluorine_unit_cell.svg/220px-Beta_fluorine_unit_cell.svg.png" decoding="async" width="220" height="220" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/88/Beta_fluorine_unit_cell.svg/330px-Beta_fluorine_unit_cell.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/88/Beta_fluorine_unit_cell.svg/440px-Beta_fluorine_unit_cell.svg.png 2x" data-file-width="406" data-file-height="406" /></a><figcaption>Crystal structure of β-fluorine. Spheres indicate F 2 molecules that may assume any angle. Other molecules are constrained to planes.</figcaption></figure> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Phases_of_fluorine" title="Phases of fluorine">Phases of fluorine</a></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Beta-fluorine_crystal_structure.gif" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/dc/Beta-fluorine_crystal_structure.gif/220px-Beta-fluorine_crystal_structure.gif" decoding="async" width="220" height="220" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/dc/Beta-fluorine_crystal_structure.gif/330px-Beta-fluorine_crystal_structure.gif 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/dc/Beta-fluorine_crystal_structure.gif/440px-Beta-fluorine_crystal_structure.gif 2x" data-file-width="640" data-file-height="640" /></a><figcaption>Animation showing the crystal structure of beta-fluorine. Molecules on the faces of the unit cell have rotations constrained to a plane.</figcaption></figure> At room temperature, fluorine is a gas of <a href="/wiki/Diatomic_molecule" title="Diatomic molecule">diatomic molecules</a>,<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000382-5">[5]</a> pale yellow when pure (sometimes described as yellow-green).<a href="#cite_note-45">[43]</a> It has a characteristic halogen-like pungent and biting odor detectable at 20 <a href="/wiki/Parts_per_billion" class="mw-redirect" title="Parts per billion">ppb</a>.<a href="#cite_note-FOOTNOTELide20044.12-46">[44]</a> Fluorine condenses into a bright yellow liquid at −188 °C (−306.4 °F), a transition temperature similar to those of oxygen and nitrogen.<a href="#cite_note-FOOTNOTEDean1999523-47">[45]</a> Fluorine has two solid forms, α- and β-fluorine. The latter crystallizes at −220 °C (−364.0 °F) and is transparent and soft, with the same disordered <a href="/wiki/Cubic_crystal_system" title="Cubic crystal system">cubic</a> structure of freshly crystallized solid oxygen,<a href="#cite_note-FOOTNOTEDean1999523-47">[45]</a><a href="#cite_note-49">[note 3]</a> unlike the <a href="/wiki/Orthorhombic_crystal_system" title="Orthorhombic crystal system">orthorhombic</a> systems of other solid halogens.<a href="#cite_note-FOOTNOTEYoung197510-50">[47]</a><a href="#cite_note-Barrett_1967-51">[48]</a> Further cooling to −228 °C (−378.4 °F) induces a <a href="/wiki/Phase_transition" title="Phase transition">phase transition</a> into opaque and hard α-fluorine, which has a <a href="/wiki/Monoclinic_crystal_system" title="Monoclinic crystal system">monoclinic</a> structure with dense, angled layers of molecules. The transition from β- to α-fluorine is more <a href="/wiki/Exothermic" class="mw-redirect" title="Exothermic">exothermic</a> than the condensation of fluorine, and can be violent.<a href="#cite_note-FOOTNOTEYoung197510-50">[47]</a><a href="#cite_note-Barrett_1967-51">[48]</a> <div class="mw-heading mw-heading3"><h3 id="Isotopes">Isotopes</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=5" 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_fluorine" title="Isotopes of fluorine">Isotopes of fluorine</a></div> Only one <a href="/wiki/Isotope" title="Isotope">isotope</a> of fluorine occurs naturally in abundance, the stable isotope 19 F.<a href="#cite_note-52">[49]</a> It has a high <a href="/wiki/Magnetogyric_ratio" class="mw-redirect" title="Magnetogyric ratio">magnetogyric ratio</a><a href="#cite_note-54">[note 4]</a> and exceptional sensitivity to magnetic fields; because it is also <a href="/wiki/Monoisotopic_element" title="Monoisotopic element">the only stable isotope</a>, it is <a href="/wiki/Fluorine-19_nuclear_magnetic_resonance" class="mw-redirect" title="Fluorine-19 nuclear magnetic resonance">used</a> in <a href="/wiki/Magnetic_resonance_imaging" title="Magnetic resonance imaging">magnetic resonance imaging</a>.<a href="#cite_note-55">[51]</a> Eighteen <a href="/wiki/Radioisotope" class="mw-redirect" title="Radioisotope">radioisotopes</a> with <a href="/wiki/Mass_number" title="Mass number">mass numbers</a> 13–31 have been synthesized, of which <a href="/wiki/Fluorine-18" title="Fluorine-18">18 F</a> is the most stable with a <a href="/wiki/Half-life" title="Half-life">half-life</a> of 109.734 minutes.<a href="#cite_note-NUBASE2020-56">[52]</a><a href="#cite_note-57">[53]</a> 18 F is a natural <a href="/wiki/Trace_radioisotope" title="Trace radioisotope">trace radioisotope</a> produced by <a href="/wiki/Cosmic_ray_spallation" title="Cosmic ray spallation">cosmic ray spallation</a> of atmospheric <a href="/wiki/Argon" title="Argon">argon</a> as well as by reaction of protons with natural oxygen: 18O + p → 18F + n.<a href="#cite_note-SCOPE50-58">[54]</a> Other radioisotopes have half-lives less than 70 seconds; most decay in less than half a second.<a href="#cite_note-isotopes-59">[55]</a> The isotopes 17 F and 18 F undergo <a href="/wiki/Positron_emission" title="Positron emission">β+ decay</a> and <a href="/wiki/Electron_capture" title="Electron capture">electron capture</a>, lighter isotopes decay by <a href="/wiki/Proton_emission" title="Proton emission">proton emission</a>, and those heavier than 19 F undergo <a href="/wiki/Beta_minus_decay" class="mw-redirect" title="Beta minus decay">β− decay</a> (the heaviest ones with delayed <a href="/wiki/Neutron_emission" title="Neutron emission">neutron emission</a>).<a href="#cite_note-isotopes-59">[55]</a><a href="#cite_note-60">[56]</a> Two <a href="/wiki/Nuclear_isomer" title="Nuclear isomer">metastable isomers</a> of fluorine are known, 18m F, with a half-life of 162(7) nanoseconds, and 26m F, with a half-life of 2.2(1) milliseconds.<a href="#cite_note-61">[57]</a> <div class="mw-heading mw-heading2"><h2 id="Occurrence">Occurrence</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=6" title="Edit section: Occurrence">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/Origin_and_occurrence_of_fluorine" title="Origin and occurrence of fluorine">Origin and occurrence of fluorine</a></div> <div class="mw-heading mw-heading3"><h3 id="Universe">Universe</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=7" title="Edit section: Universe">edit</a>]</div> <table class="wikitable" style="float:right; margin-left:15px; margin-top:0; font-size:10pt; line-height:11pt;"> <caption style="margin-bottom: 5px;">Solar System abundances<a href="#cite_note-Cameron-62">[58]</a> </caption> <tbody><tr> <th style="text-align:center;">Atomic number </th> <th style="width:45%;">Element </th> <th style="padding-right: 5px; padding-left: 10px;">Relative amount </th></tr> <tr> <td style="text-align:center;">6 </td> <td style="text-align:center;">Carbon </td> <td style="padding-right:5px; text-align:right;">4,800 </td></tr> <tr> <td style="text-align:center;">7 </td> <td style="text-align:center;">Nitrogen </td> <td style="padding-right:5px; text-align:right;">1,500 </td></tr> <tr> <td style="text-align:center;">8 </td> <td style="text-align:center;">Oxygen </td> <td style="padding-right:5px; text-align:right;">8,800 </td></tr> <tr style="background:#ff9;"> <td style="text-align:center;">9 </td> <td style="text-align:center;">Fluorine </td> <td style="padding-right:5px; text-align:right;">1 </td></tr> <tr> <td style="text-align:center;">10 </td> <td style="text-align:center;">Neon </td> <td style="padding-right:5px; text-align:right;">1,400 </td></tr> <tr> <td style="text-align:center;">11 </td> <td style="text-align:center;">Sodium </td> <td style="padding-right:5px; text-align:right;">24 </td></tr> <tr> <td style="text-align:center;">12 </td> <td style="text-align:center;">Magnesium </td> <td style="padding-right:5px; text-align:right;">430 </td></tr></tbody></table> Among the lighter elements, fluorine's abundance value of 400 <a href="/wiki/Parts-per_notation" title="Parts-per notation">ppb</a> (parts per billion) – 24th among elements in the universe – is exceptionally low: other elements from carbon to magnesium are twenty or more times as common.<a href="#cite_note-Crosswell-63">[59]</a> This is because <a href="/wiki/Stellar_nucleosynthesis" title="Stellar nucleosynthesis">stellar nucleosynthesis</a> processes bypass fluorine, and any fluorine atoms otherwise created have high <a href="/wiki/Nuclear_cross_section" title="Nuclear cross section">nuclear cross sections</a>, allowing collisions with hydrogen or helium to generate oxygen or neon respectively.<a href="#cite_note-Crosswell-63">[59]</a><a href="#cite_note-64">[60]</a> Beyond this transient existence, three explanations have been proposed for the presence of fluorine:<a href="#cite_note-Crosswell-63">[59]</a><a href="#cite_note-Milky_Way-65">[61]</a> <ul><li>during <a href="/wiki/Type_II_supernova" title="Type II supernova">type II supernovae</a>, bombardment of neon atoms by <a href="/wiki/Neutrino" title="Neutrino">neutrinos</a> could transmute them to fluorine;</li> <li>the solar wind of <a href="/wiki/Wolf%E2%80%93Rayet_star" title="Wolf–Rayet star">Wolf–Rayet stars</a> could blow fluorine away from any hydrogen or helium atoms; or</li> <li>fluorine is borne out on convection currents arising from fusion in <a href="/wiki/Asymptotic_giant_branch" title="Asymptotic giant branch">asymptotic giant branch</a> stars.</li></ul> <div class="mw-heading mw-heading3"><h3 id="Earth">Earth</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=8" title="Edit section: Earth">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/List_of_countries_by_fluorite_production" title="List of countries by fluorite production">List of countries by fluorite production</a></div> Fluorine is the 13th most <a href="/wiki/Abundance_of_elements_in_Earth%27s_crust" title="Abundance of elements in Earth's crust">abundant element in Earth's crust</a> at 600–700 ppm (parts per million) by mass.<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000384-66">[62]</a> Though believed not to occur naturally, elemental fluorine has been shown to be present as an occlusion in antozonite, a variant of fluorite.<a href="#cite_note-FOOTNOTESchmedtMangstlKraus2012-67">[63]</a> Most fluorine exists as fluoride-containing minerals. <a href="/wiki/Fluorite" title="Fluorite">Fluorite</a>, <a href="/wiki/Fluorapatite" title="Fluorapatite">fluorapatite</a> and <a href="/wiki/Cryolite" title="Cryolite">cryolite</a> are the most industrially significant.<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000384-66">[62]</a><a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998795-68">[64]</a> Fluorite (CaF 2), also known as fluorspar, abundant worldwide, is the main source of fluoride, and hence fluorine. China and Mexico are the major suppliers.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998795-68">[64]</a><a href="#cite_note-KGS_fluorite_terminology-69">[65]</a><a href="#cite_note-AcountF-70">[66]</a><a href="#cite_note-historical_fluorspar_statistics-71">[67]</a><a href="#cite_note-UK_fluorspar-72">[68]</a> Fluorapatite (Ca5(PO4)3F), which contains most of the world's fluoride, is an inadvertent source of fluoride as a byproduct of fertilizer production.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998795-68">[64]</a> Cryolite (Na 3AlF 6), used in the production of aluminium, is the most fluorine-rich mineral. Economically viable natural sources of cryolite have been exhausted, and most is now synthesised commercially.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998795-68">[64]</a> <ul class="gallery mw-gallery-packed"> <li class="gallerybox" style="width: 158.66666666667px"> <div class="thumb" style="width: 156.66666666667px;"><a href="/wiki/File:Fluorite-270246.jpg" class="mw-file-description" title="Fluorite: Pink globular mass with crystal facets"><img alt="Fluorite: Pink globular mass with crystal facets" src="//upload.wikimedia.org/wikipedia/commons/thumb/3/3c/Fluorite-270246.jpg/235px-Fluorite-270246.jpg" decoding="async" width="157" height="200" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/3/3c/Fluorite-270246.jpg/353px-Fluorite-270246.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/3/3c/Fluorite-270246.jpg 2x" data-file-width="471" data-file-height="600" /></a></div> <div class="gallerytext">Fluorite: Pink globular mass with crystal facets</div> </li> <li class="gallerybox" style="width: 159.33333333333px"> <div class="thumb" style="width: 157.33333333333px;"><a href="/wiki/File:Apatite_Canada.jpg" class="mw-file-description" title="Fluorapatite: Long, prismatic crystal, dull in lustre, protruding, at an angle, from matrix of aggregate-like rock"><img alt="Fluorapatite: Long, prismatic crystal, dull in lustre, protruding, at an angle, from matrix of aggregate-like rock" src="//upload.wikimedia.org/wikipedia/commons/thumb/2/23/Apatite_Canada.jpg/236px-Apatite_Canada.jpg" decoding="async" width="158" height="200" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/23/Apatite_Canada.jpg/354px-Apatite_Canada.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/23/Apatite_Canada.jpg/472px-Apatite_Canada.jpg 2x" data-file-width="4808" data-file-height="6112" /></a></div> <div class="gallerytext">Fluorapatite: Long, prismatic crystal, dull in <a href="/wiki/Lustre_(mineralogy)" title="Lustre (mineralogy)">lustre</a>, protruding, at an angle, from <a href="/wiki/Matrix_(geology)" title="Matrix (geology)">matrix</a> of aggregate-like rock</div> </li> <li class="gallerybox" style="width: 159.33333333333px"> <div class="thumb" style="width: 157.33333333333px;"><a href="/wiki/File:Ivigtut_cryolite_edit.jpg" class="mw-file-description" title="Cryolite: A parallelogram-shaped outline with diatomic molecules arranged in two layers"><img alt="Cryolite: A parallelogram-shaped outline with diatomic molecules arranged in two layers" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/af/Ivigtut_cryolite_edit.jpg/250px-Ivigtut_cryolite_edit.jpg" decoding="async" width="158" height="200" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/af/Ivigtut_cryolite_edit.jpg/500px-Ivigtut_cryolite_edit.jpg 1.5x" data-file-width="3782" data-file-height="4805" /></a></div> <div class="gallerytext">Cryolite: A parallelogram-shaped outline with diatomic molecules arranged in two layers</div> </li> </ul> Other minerals such as <a href="/wiki/Topaz" title="Topaz">topaz</a> contain fluorine. Fluorides, unlike other halides, are insoluble and do not occur in commercially favorable concentrations in saline waters.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998795-68">[64]</a> Trace quantities of organofluorines of uncertain origin have been detected in volcanic eruptions and geothermal springs.<a href="#cite_note-FOOTNOTEGribble2002-73">[69]</a> The existence of gaseous fluorine in crystals, suggested by the smell of crushed <a href="/wiki/Antozonite" title="Antozonite">antozonite</a>, is contentious;<a href="#cite_note-FOOTNOTERichterHahnFuchs20013-74">[70]</a><a href="#cite_note-FOOTNOTESchmedtMangstlKraus2012-67">[63]</a> a 2012 study reported the presence of 0.04% F 2 by weight in antozonite, attributing these <a href="/wiki/Inclusion_(mineral)" title="Inclusion (mineral)">inclusions</a> to radiation from the presence of tiny amounts of <a href="/wiki/Uranium" title="Uranium">uranium</a>.<a href="#cite_note-FOOTNOTESchmedtMangstlKraus2012-67">[63]</a> <div class="mw-heading mw-heading2"><h2 id="History">History</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=9" title="Edit section: History">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/History_of_fluorine" title="History of fluorine">History of fluorine</a></div> <div class="mw-heading mw-heading3"><h3 id="Early_discoveries">Early discoveries</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=10" title="Edit section: Early discoveries">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Book9-25.gif" class="mw-file-description"><img alt="Woodcut image showing man at open hearth with tongs and machine bellows to the side in background, man at water-operated hammer with quenching sluice nearby in foreground" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a0/Book9-25.gif/250px-Book9-25.gif" decoding="async" width="170" height="289" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a0/Book9-25.gif/330px-Book9-25.gif 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a0/Book9-25.gif/500px-Book9-25.gif 2x" data-file-width="1505" data-file-height="2560" /></a><figcaption>Steelmaking illustration from <a href="/wiki/De_re_metallica" title="De re metallica">De re metallica</a></figcaption></figure> In 1529, <a href="/wiki/Georgius_Agricola" title="Georgius Agricola">Georgius Agricola</a> described fluorite as an additive used to lower the melting point of metals during <a href="/wiki/Smelting" title="Smelting">smelting</a>.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998790-75">[71]</a><a href="#cite_note-assassinated-76">[72]</a><a href="#cite_note-80">[note 5]</a> He penned the Latin word fluorēs (fluor, flow) for fluorite rocks. The name later evolved into fluorspar (still commonly used) and then fluorite.<a href="#cite_note-KGS_fluorite_terminology-69">[65]</a><a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998109-81">[76]</a><a href="#cite_note-82">[77]</a> The composition of fluorite was later determined to be <a href="/wiki/Calcium_difluoride" class="mw-redirect" title="Calcium difluoride">calcium difluoride</a>.<a href="#cite_note-Weeks-83">[78]</a> <a href="/wiki/Hydrofluoric_acid" title="Hydrofluoric acid">Hydrofluoric acid</a> was used in <a href="/wiki/Glass_etching" title="Glass etching">glass etching</a> from 1720 onward.<a href="#cite_note-85">[note 6]</a> <a href="/wiki/Andreas_Sigismund_Marggraf" title="Andreas Sigismund Marggraf">Andreas Sigismund Marggraf</a> first characterized it in 1764 when he heated fluorite with sulfuric acid, and the resulting solution corroded its glass container.<a href="#cite_note-86">[80]</a><a href="#cite_note-ModFcchem-87">[81]</a> Swedish chemist <a href="/wiki/Carl_Wilhelm_Scheele" title="Carl Wilhelm Scheele">Carl Wilhelm Scheele</a> repeated the experiment in 1771, and named the acidic product fluss-spats-syran (fluorspar acid).<a href="#cite_note-ModFcchem-87">[81]</a><a href="#cite_note-88">[82]</a> In 1810, the French physicist <a href="/wiki/Andr%C3%A9-Marie_Amp%C3%A8re" title="André-Marie Ampère">André-Marie Ampère</a> suggested that hydrogen and an element analogous to chlorine constituted hydrofluoric acid.<a href="#cite_note-89">[83]</a> He also proposed in a letter to <a href="/wiki/Humphry_Davy" title="Humphry Davy">Sir Humphry Davy</a> dated August 26, 1812 that this then-unknown substance may be named fluorine from fluoric compounds and the -ine suffix of other halogens.<a href="#cite_note-90">[84]</a><a href="#cite_note-FOOTNOTEDavy1813[httpsbooksgooglecombooksiddhdGAAAAMAAJpgPA278_278]-91">[85]</a> This word, often with modifications, is used in most European languages; however, Greek, Russian, and some others, following Ampère's later suggestion, use the name ftor or derivatives, from the Greek φθόριος (phthorios, destructive).<a href="#cite_note-FOOTNOTEBanks198611-92">[86]</a> The New Latin name fluorum gave the element its current symbol F; Fl was used in early papers.<a href="#cite_note-dissolve-93">[87]</a><a href="#cite_note-94">[note 7]</a> <div class="mw-heading mw-heading3"><h3 id="Isolation">Isolation</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=11" title="Edit section: Isolation">edit</a>]</div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Recherches_sur_l%E2%80%99isolement_du_fluor,_Fig._5.PNG" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/77/Recherches_sur_l%E2%80%99isolement_du_fluor%2C_Fig._5.PNG/170px-Recherches_sur_l%E2%80%99isolement_du_fluor%2C_Fig._5.PNG" decoding="async" width="170" height="216" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/77/Recherches_sur_l%E2%80%99isolement_du_fluor%2C_Fig._5.PNG/255px-Recherches_sur_l%E2%80%99isolement_du_fluor%2C_Fig._5.PNG 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/77/Recherches_sur_l%E2%80%99isolement_du_fluor%2C_Fig._5.PNG/340px-Recherches_sur_l%E2%80%99isolement_du_fluor%2C_Fig._5.PNG 2x" data-file-width="590" data-file-height="750" /></a><figcaption>1887 drawing of Moissan's apparatus</figcaption></figure> Initial studies on fluorine were so dangerous that several 19th-century experimenters were deemed "fluorine martyrs" after misfortunes with hydrofluoric acid.<a href="#cite_note-96">[note 8]</a> Isolation of elemental fluorine was hindered by the extreme corrosiveness of both elemental fluorine itself and hydrogen fluoride, as well as the lack of a simple and suitable <a href="/wiki/Electrolyte" title="Electrolyte">electrolyte</a>.<a href="#cite_note-Weeks-83">[78]</a><a href="#cite_note-Toon-95">[88]</a> <a href="/wiki/Edmond_Fr%C3%A9my" title="Edmond Frémy">Edmond Frémy</a> postulated that <a href="/wiki/Electrolysis" title="Electrolysis">electrolysis</a> of pure hydrogen fluoride to generate fluorine was feasible and devised a method to produce anhydrous samples from acidified <a href="/wiki/Potassium_bifluoride" title="Potassium bifluoride">potassium bifluoride</a>; instead, he discovered that the resulting (dry) hydrogen fluoride <a href="/wiki/Insulator_(electricity)" title="Insulator (electricity)">did not conduct</a> electricity.<a href="#cite_note-Weeks-83">[78]</a><a href="#cite_note-Toon-95">[88]</a><a href="#cite_note-Asimov-97">[89]</a> Frémy's former student <a href="/wiki/Henri_Moissan" title="Henri Moissan">Henri Moissan</a> persevered, and after much trial and error found that a mixture of potassium bifluoride and dry hydrogen fluoride was a conductor, enabling electrolysis. To prevent rapid corrosion of the platinum in his <a href="/wiki/Electrochemical_cell" title="Electrochemical cell">electrochemical cells</a>, he cooled the reaction to extremely low temperatures in a special bath and forged cells from a more resistant mixture of platinum and <a href="/wiki/Iridium" title="Iridium">iridium</a>, and used fluorite stoppers.<a href="#cite_note-Toon-95">[88]</a><a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998789–791-98">[90]</a> In 1886, after 74 years of effort by many chemists, Moissan isolated elemental fluorine.<a href="#cite_note-Asimov-97">[89]</a><a href="#cite_note-'qwen'-99">[91]</a> In 1906, two months before his death, Moissan received the <a href="/wiki/Nobel_Prize_in_Chemistry" title="Nobel Prize in Chemistry">Nobel Prize in Chemistry</a>,<a href="#cite_note-Chem_Nobel_laureates-100">[92]</a> with the following citation:<a href="#cite_note-Toon-95">[88]</a> <style data-mw-deduplicate="TemplateStyles:r1244412712">.mw-parser-output .templatequote{overflow:hidden;margin:1em 0;padding:0 32px}.mw-parser-output .templatequotecite{line-height:1.5em;text-align:left;margin-top:0}@media(min-width:500px){.mw-parser-output .templatequotecite{padding-left:1.6em}}</style><blockquote class="templatequote">[I]n recognition of the great services rendered by him in his investigation and isolation of the element fluorine ... The whole world has admired the great experimental skill with which you have studied that savage beast among the elements.<a href="#cite_note-101">[note 9]</a></blockquote> <div class="mw-heading mw-heading3"><h3 id="Later_uses">Later uses</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=12" title="Edit section: Later uses">edit</a>]</div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Uranium_hexafluoride_crystals_sealed_in_an_ampoule.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/94/Uranium_hexafluoride_crystals_sealed_in_an_ampoule.jpg/250px-Uranium_hexafluoride_crystals_sealed_in_an_ampoule.jpg" decoding="async" width="250" height="99" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/94/Uranium_hexafluoride_crystals_sealed_in_an_ampoule.jpg/500px-Uranium_hexafluoride_crystals_sealed_in_an_ampoule.jpg 1.5x" data-file-width="683" data-file-height="270" /></a><figcaption>An ampoule of <a href="/wiki/Uranium_hexafluoride" title="Uranium hexafluoride">uranium hexafluoride</a></figcaption></figure> The <a href="/wiki/Frigidaire" title="Frigidaire">Frigidaire</a> division of <a href="/wiki/General_Motors" title="General Motors">General Motors</a> (GM) experimented with chlorofluorocarbon refrigerants in the late 1920s, and <a href="/wiki/Kinetic_Chemicals" class="mw-redirect" title="Kinetic Chemicals">Kinetic Chemicals</a> was formed as a joint venture between GM and <a href="/wiki/DuPont" title="DuPont">DuPont</a> in 1930 hoping to market Freon-12 (<a href="/wiki/Dichlorodifluoromethane" title="Dichlorodifluoromethane">CCl 2F 2</a>) as one such <a href="/wiki/Refrigerant" title="Refrigerant">refrigerant</a>. It replaced earlier and more toxic compounds, increased demand for kitchen refrigerators, and became profitable; by 1949 DuPont had bought out Kinetic and marketed several other <a href="/wiki/Freon" title="Freon">Freon</a> compounds.<a href="#cite_note-ModFcchem-87">[81]</a><a href="#cite_note-Jstg-102">[93]</a><a href="#cite_note-FOOTNOTEHounshellSmith1988156–157-103">[94]</a><a href="#cite_note-DD_Freon_history-104">[95]</a> <a href="/wiki/Polytetrafluoroethylene" title="Polytetrafluoroethylene">Polytetrafluoroethylene</a> (Teflon) was serendipitously discovered in 1938 by <a href="/wiki/Roy_J._Plunkett" title="Roy J. Plunkett">Roy J. Plunkett</a> while working on refrigerants at Kinetic, and its superlative chemical and thermal resistance lent it to accelerated commercialization and mass production by 1941.<a href="#cite_note-ModFcchem-87">[81]</a><a href="#cite_note-Jstg-102">[93]</a><a href="#cite_note-FOOTNOTEHounshellSmith1988156–157-103">[94]</a> Large-scale production of elemental fluorine began during World War II. Germany used high-temperature electrolysis to make tons of the planned incendiary <a href="/wiki/Chlorine_trifluoride" title="Chlorine trifluoride">chlorine trifluoride</a><a href="#cite_note-105">[96]</a> and the <a href="/wiki/Manhattan_Project" title="Manhattan Project">Manhattan Project</a> used huge quantities to produce <a href="/wiki/Uranium_hexafluoride" title="Uranium hexafluoride">uranium hexafluoride</a> for uranium enrichment. Since UF 6 is as corrosive as fluorine, <a href="/wiki/Gaseous_diffusion" title="Gaseous diffusion">gaseous diffusion</a> plants required special materials: nickel for membranes, fluoropolymers for seals, and liquid fluorocarbons as coolants and lubricants. This burgeoning nuclear industry later drove post-war fluorochemical development.<a href="#cite_note-106">[97]</a> <div class="mw-heading mw-heading2"><h2 id="Compounds">Compounds</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=13" title="Edit section: 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/Fluorine_compounds" title="Fluorine compounds">Fluorine compounds</a></div> Fluorine has a rich chemistry, encompassing organic and inorganic domains. It combines with metals, nonmetals, <a href="/wiki/Metalloid" title="Metalloid">metalloids</a>, and most noble gases.<a href="#cite_note-Riedel_Kaupp_2009-107">[98]</a> Fluorine's high electron affinity results in a preference for <a href="/wiki/Ionic_bonding" title="Ionic bonding">ionic bonding</a>; when it forms <a href="/wiki/Covalent_bond" title="Covalent bond">covalent bonds</a>, these are polar, and almost always <a href="/wiki/Single_bond" title="Single bond">single</a>.<a href="#cite_note-NF_charge-108">[99]</a><a href="#cite_note-109">[100]</a><a href="#cite_note-110">[note 10]</a> <div class="mw-heading mw-heading3"><h3 id="Oxidation_states">Oxidation states</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=14" title="Edit section: Oxidation states">edit</a>]</div> In compounds, fluorine almost exclusively assumes an <a href="/wiki/Oxidation_state" title="Oxidation state">oxidation state</a> of −1. Fluorine in F 2 is defined to have oxidation state 0. The unstable species F− 2 and F− 3, which decompose at around 40 K, have intermediate oxidation states;<a href="#cite_note-FOOTNOTEWibergWibergHolleman2001422-111">[101]</a> F+ 4 and a few related species are predicted to be stable.<a href="#cite_note-112">[102]</a> <div class="mw-heading mw-heading3"><h3 id="Metals">Metals</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=15" title="Edit section: Metals">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Fluoride_volatility" title="Fluoride volatility">Fluoride volatility</a></div> Alkali metals form ionic and highly soluble <a href="/wiki/Monofluoride" title="Monofluoride">monofluorides</a>; these have the <a href="/wiki/Cubic_crystal_system#Rock-salt_structure" title="Cubic crystal system">cubic arrangement of sodium chloride</a> and analogous chlorides.<a href="#cite_note-113">[103]</a><a href="#cite_note-FOOTNOTEAigueperse_et_al.2000420–422-114">[104]</a> Alkaline earth <a href="/wiki/Difluoride" title="Difluoride">difluorides</a> possess strong ionic bonds but are insoluble in water,<a href="#cite_note-dissolve-93">[87]</a> with the exception of <a href="/wiki/Beryllium_difluoride" class="mw-redirect" title="Beryllium difluoride">beryllium difluoride</a>, which also exhibits some covalent character and has a <a href="/wiki/Silicon_dioxide" title="Silicon dioxide">quartz</a>-like structure.<a href="#cite_note-Beryllium_chemistry-115">[105]</a> <a href="/wiki/Rare_earth_element" class="mw-redirect" title="Rare earth element">Rare earth elements</a> and many other metals form mostly ionic <a href="/wiki/Trifluoride" title="Trifluoride">trifluorides</a>.<a href="#cite_note-FOOTNOTEEmeléusSharpe198389–97-116">[106]</a><a href="#cite_note-Crystal_chemistry_of_fluorides-117">[107]</a><a href="#cite_note-118">[108]</a> Covalent bonding first comes to prominence in the <a href="/wiki/Tetrafluoride" title="Tetrafluoride">tetrafluorides</a>: those of <a href="/wiki/Zirconium" title="Zirconium">zirconium</a>, <a href="/wiki/Hafnium" title="Hafnium">hafnium</a><a href="#cite_note-119">[109]</a><a href="#cite_note-Perry_2011_193-120">[110]</a> and several <a href="/wiki/Actinides" class="mw-redirect" title="Actinides">actinides</a><a href="#cite_note-121">[111]</a> are ionic with high melting points,<a href="#cite_note-FOOTNOTELide20044.60,_4.76,_4.92,_4.96-122">[112]</a><a href="#cite_note-125">[note 11]</a> while those of <a href="/wiki/Titanium" title="Titanium">titanium</a>,<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998964-126">[115]</a> <a href="/wiki/Vanadium" title="Vanadium">vanadium</a>,<a href="#cite_note-127">[116]</a> and <a href="/wiki/Niobium" title="Niobium">niobium</a> are polymeric,<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998990-128">[117]</a> melting or decomposing at no more than 350 °C (662 °F).<a href="#cite_note-FOOTNOTELide20044.72,_4.91,_4.93-129">[118]</a> <a href="/wiki/Pentafluoride" title="Pentafluoride">Pentafluorides</a> continue this trend with their linear polymers and <a href="/wiki/Oligomer" title="Oligomer">oligomeric</a> complexes.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998561–563-130">[119]</a><a href="#cite_note-FOOTNOTEEmeléusSharpe1983256–277-131">[120]</a><a href="#cite_note-FOOTNOTEMackayMackayHenderson2002355–356-132">[121]</a> Thirteen metal <a href="/wiki/Hexafluoride" title="Hexafluoride">hexafluorides</a> are known,<a href="#cite_note-133">[note 12]</a> all octahedral, and are mostly volatile solids but for liquid <a href="/wiki/Molybdenum_hexafluoride" title="Molybdenum hexafluoride">MoF 6</a> and <a href="/wiki/Rhenium_hexafluoride" title="Rhenium hexafluoride">ReF 6</a>, and gaseous <a href="/wiki/Tungsten_hexafluoride" title="Tungsten hexafluoride">WF 6</a>.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998(various_pages,_by_metal_in_respective_chapters)-134">[122]</a><a href="#cite_note-FOOTNOTELide20044.71,_4.78,_4.92-135">[123]</a><a href="#cite_note-D_BLOCK_XF6-136">[124]</a> <a href="/wiki/Rhenium_heptafluoride" title="Rhenium heptafluoride">Rhenium heptafluoride</a>, the only characterized metal <a href="/wiki/Heptafluoride" title="Heptafluoride">heptafluoride</a>, is a low-melting molecular solid with <a href="/wiki/Pentagonal_bipyramidal_molecular_geometry" title="Pentagonal bipyramidal molecular geometry">pentagonal bipyramidal molecular geometry</a>.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998819-137">[125]</a> <a href="/wiki/Gold_heptafluoride" title="Gold heptafluoride">Gold heptafluoride</a> is a low-temperature complex of molecular F2 with AuF5, with NPA calculations indicating that the fluorine in the F2 ligand is nearly neutral while those in the AuF5 portion of the molecule have strong negative partial charges. This is consistent with the F2 ligand representing fluorine in the zero oxidation state.<a href="#cite_note-himmel-138">[126]</a> Metal fluorides with more fluorine atoms are particularly reactive.<a href="#cite_note-139">[127]</a> <table cellpadding="3" style="margin:1em auto 1em auto; text-align:center;"> <tbody><tr> <td colspan="3" style="text-align:center;">Structural progression of metal fluorides </td></tr> <tr> <td><a href="/wiki/File:Sodium-fluoride-unit-cell-3D.png" class="mw-file-description" title="Sodium fluoride: cubic lattice of alternating sodium and fluorine atoms with no distinct molecules"><img alt="Checkerboard-like lattice of small blue and large yellow balls, going in three dimensions so that each ball has 6 nearest neighbors of opposite type" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f7/Sodium-fluoride-unit-cell-3D.png/250px-Sodium-fluoride-unit-cell-3D.png" decoding="async" width="132" height="126" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f7/Sodium-fluoride-unit-cell-3D.png/330px-Sodium-fluoride-unit-cell-3D.png 2x" data-file-width="1100" data-file-height="1050" /></a> </td> <td><a href="/wiki/File:Bismuth-pentafluoride-chain-from-xtal-1971-3D-balls.png" class="mw-file-description" title="Bismuth pentafluoride: arbitrarily long, straight chain of atoms"><img alt="Straight chain of alternating balls, violet and yellow, with violet ones also linked to four more yellow perpendicularly to the chain and each other" src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c2/Bismuth-pentafluoride-chain-from-xtal-1971-3D-balls.png/500px-Bismuth-pentafluoride-chain-from-xtal-1971-3D-balls.png" decoding="async" width="500" height="126" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c2/Bismuth-pentafluoride-chain-from-xtal-1971-3D-balls.png/750px-Bismuth-pentafluoride-chain-from-xtal-1971-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/c/c2/Bismuth-pentafluoride-chain-from-xtal-1971-3D-balls.png/1000px-Bismuth-pentafluoride-chain-from-xtal-1971-3D-balls.png 2x" data-file-width="2000" data-file-height="503" /></a> </td> <td><a href="/wiki/File:Rhenium-heptafluoride-3D-balls.png" class="mw-file-description" title="Rhenium heptafluoride: discrete small molecule"><img alt="Ball and stick drawing showing central violet ball with a yellow one directly above and below and then an equatorial belt of 5 surrounding yellow balls" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/51/Rhenium-heptafluoride-3D-balls.png/121px-Rhenium-heptafluoride-3D-balls.png" decoding="async" width="121" height="126" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/51/Rhenium-heptafluoride-3D-balls.png/182px-Rhenium-heptafluoride-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/51/Rhenium-heptafluoride-3D-balls.png/242px-Rhenium-heptafluoride-3D-balls.png 2x" data-file-width="1032" data-file-height="1071" /></a> </td></tr> <tr style="text-align:center;"> <td><a href="/wiki/Sodium_fluoride" title="Sodium fluoride">Sodium fluoride</a>, ionic </td> <td><a href="/wiki/Bismuth_pentafluoride" title="Bismuth pentafluoride">Bismuth pentafluoride</a>, polymeric </td> <td><a href="/wiki/Rhenium_heptafluoride" title="Rhenium heptafluoride">Rhenium heptafluoride</a>, molecular </td></tr></tbody></table> <div class="mw-heading mw-heading3"><h3 id="Hydrogen">Hydrogen</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=16" title="Edit section: Hydrogen">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">Main articles: <a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">Hydrogen fluoride</a> and <a href="/wiki/Hydrofluoric_acid" title="Hydrofluoric acid">hydrofluoric acid</a></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Boiling-points_Chalcogen-Halogen.svg" class="mw-file-description"><img alt="Graph showing water and hydrogen fluoride breaking the trend of lower boiling points for lighter molecules" src="//upload.wikimedia.org/wikipedia/commons/thumb/2/2b/Boiling-points_Chalcogen-Halogen.svg/250px-Boiling-points_Chalcogen-Halogen.svg.png" decoding="async" width="220" height="146" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/2b/Boiling-points_Chalcogen-Halogen.svg/330px-Boiling-points_Chalcogen-Halogen.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/2b/Boiling-points_Chalcogen-Halogen.svg/440px-Boiling-points_Chalcogen-Halogen.svg.png 2x" data-file-width="337" data-file-height="224" /></a><figcaption>Boiling points of hydrogen halides and chalcogenides, showing the unusually high values for hydrogen fluoride and water</figcaption></figure> Hydrogen and fluorine combine to yield hydrogen fluoride, in which discrete molecules form clusters by hydrogen bonding, resembling water more than <a href="/wiki/Hydrogen_chloride" title="Hydrogen chloride">hydrogen chloride</a>.<a href="#cite_note-Pauling_HF_hydrogen_bonds-140">[128]</a><a href="#cite_note-Atkins_HF-141">[129]</a><a href="#cite_note-New_Scientist_HF-142">[130]</a> It boils at a much higher temperature than heavier hydrogen halides and unlike them is <a href="/wiki/Miscible" class="mw-redirect" title="Miscible">miscible</a> with water.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998812–816-143">[131]</a> Hydrogen fluoride readily hydrates on contact with water to form aqueous hydrogen fluoride, also known as hydrofluoric acid. Unlike the other hydrohalic acids, which are <a href="/wiki/Strong_acids" class="mw-redirect" title="Strong acids">strong</a>, hydrofluoric acid is a <a href="/wiki/Weak_acid" class="mw-redirect" title="Weak acid">weak acid</a> at low concentrations.<a href="#cite_note-FOOTNOTEWibergWibergHolleman2001425-144">[132]</a><a href="#cite_note-145">[133]</a> However, it can attack glass, something the other acids cannot do.<a href="#cite_note-H+-146">[134]</a> <div class="mw-heading mw-heading3"><h3 id="Other_reactive_nonmetals">Other reactive nonmetals</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=17" title="Edit section: Other reactive nonmetals">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Chlorine-trifluoride-3D-balls.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a5/Chlorine-trifluoride-3D-balls.png/220px-Chlorine-trifluoride-3D-balls.png" decoding="async" width="220" height="143" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a5/Chlorine-trifluoride-3D-balls.png/330px-Chlorine-trifluoride-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a5/Chlorine-trifluoride-3D-balls.png/440px-Chlorine-trifluoride-3D-balls.png 2x" data-file-width="1100" data-file-height="716" /></a><figcaption><a href="/wiki/Chlorine_trifluoride" title="Chlorine trifluoride">Chlorine trifluoride</a>, whose corrosive potential ignites asbestos, concrete, sand and other fire retardants<a href="#cite_note-FOOTNOTEAir_Products_and_Chemicals20041-147">[135]</a></figcaption></figure> Binary fluorides of metalloids and p-block nonmetals are generally covalent and volatile, with varying reactivities. <a href="/wiki/Period_3" class="mw-redirect" title="Period 3">Period 3</a> and heavier nonmetals can form <a href="/wiki/Hypervalent_molecule" title="Hypervalent molecule">hypervalent</a> fluorides.<a href="#cite_note-Noury-148">[136]</a> <a href="/wiki/Boron_trifluoride" title="Boron trifluoride">Boron trifluoride</a> is planar and possesses an incomplete octet. It functions as a <a href="/wiki/Lewis_acids_and_bases" title="Lewis acids and bases">Lewis acid</a> and combines with Lewis bases like ammonia to form <a href="/wiki/Adduct" title="Adduct">adducts</a>.<a href="#cite_note-149">[137]</a> <a href="/wiki/Carbon_tetrafluoride" title="Carbon tetrafluoride">Carbon tetrafluoride</a> is tetrahedral and inert;<a href="#cite_note-150">[note 13]</a> <a href="/wiki/Carbon_group" title="Carbon group">its group</a> analogues, silicon and germanium tetrafluoride, are also tetrahedral<a href="#cite_note-151">[138]</a> but behave as Lewis acids.<a href="#cite_note-FOOTNOTEAigueperse_et_al.2000423-152">[139]</a><a href="#cite_note-FOOTNOTEWibergWibergHolleman2001897-153">[140]</a> The <a href="/wiki/Pnictogen" title="Pnictogen">pnictogens</a> form trifluorides that increase in reactivity and basicity with higher molecular weight, although <a href="/wiki/Nitrogen_trifluoride" title="Nitrogen trifluoride">nitrogen trifluoride</a> resists hydrolysis and is not basic.<a href="#cite_note-PnFx-154">[141]</a> The pentafluorides of phosphorus, arsenic, and antimony are more reactive than their respective trifluorides, with <a href="/wiki/Antimony_pentafluoride" title="Antimony pentafluoride">antimony pentafluoride</a> the strongest neutral Lewis acid known, only behind <a href="/wiki/Gold_pentafluoride" class="mw-redirect" title="Gold pentafluoride">gold pentafluoride</a>.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998561–563-130">[119]</a><a href="#cite_note-Arsenic-155">[142]</a><a href="#cite_note-FOOTNOTEAigueperse_et_al.2000432-156">[143]</a> <a href="/wiki/Chalcogen" title="Chalcogen">Chalcogens</a> have diverse fluorides: unstable difluorides have been reported for oxygen (the only known compound with oxygen in an oxidation state of +2), sulfur, and selenium; tetrafluorides and hexafluorides exist for sulfur, selenium, and tellurium. The latter are stabilized by more fluorine atoms and lighter central atoms, so <a href="/wiki/Sulfur_hexafluoride" title="Sulfur hexafluoride">sulfur hexafluoride</a> is especially inert.<a href="#cite_note-(O,S,Se,Te)Fn-157">[144]</a><a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998638–640,_683–689,_767–778-158">[145]</a> Chlorine, bromine, and iodine can each form mono-, tri-, and pentafluorides, but only <a href="/wiki/Iodine_heptafluoride" title="Iodine heptafluoride">iodine heptafluoride</a> has been characterized among possible <a href="/wiki/Interhalogen" title="Interhalogen">interhalogen</a> heptafluorides.<a href="#cite_note-FOOTNOTEWibergWibergHolleman2001435–436-159">[146]</a> Many of them are powerful sources of fluorine atoms, and industrial applications using chlorine trifluoride require precautions similar to those using fluorine.<a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998828–830-160">[147]</a><a href="#cite_note-Patnaik-161">[148]</a> <div class="mw-heading mw-heading3"><h3 id="Noble_gases">Noble gases</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=18" title="Edit section: Noble gases">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/Noble_gas_compound" title="Noble gas compound">Noble gas compound</a></div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Xenon_tetrafluoride_crop.gif" class="mw-file-description"><img alt="Black-and-white photo showing transparent crystals in a dish" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b2/Xenon_tetrafluoride_crop.gif/170px-Xenon_tetrafluoride_crop.gif" decoding="async" width="170" height="170" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/b/b2/Xenon_tetrafluoride_crop.gif/255px-Xenon_tetrafluoride_crop.gif 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/b/b2/Xenon_tetrafluoride_crop.gif/340px-Xenon_tetrafluoride_crop.gif 2x" data-file-width="400" data-file-height="400" /></a><figcaption>These xenon tetrafluoride crystals were photographed in 1962. The compound's synthesis, as with xenon hexafluoroplatinate, surprised many chemists.<a href="#cite_note-FOOTNOTEMoellerBailarKleinberg1980236-162">[149]</a></figcaption></figure> <a href="/wiki/Noble_gas" title="Noble gas">Noble gases</a>, having complete electron shells, defied reaction with other elements until 1962 when <a href="/wiki/Neil_Bartlett_(chemist)" title="Neil Bartlett (chemist)">Neil Bartlett</a> reported synthesis of <a href="/wiki/Xenon_hexafluoroplatinate" title="Xenon hexafluoroplatinate">xenon hexafluoroplatinate</a>;<a href="#cite_note-FOOTNOTEWibergWibergHolleman2001392–393-163">[150]</a> <a href="/wiki/Xenon_difluoride" title="Xenon difluoride">xenon difluoride</a>, <a href="/wiki/Xenon_tetrafluoride" title="Xenon tetrafluoride">tetrafluoride</a>, <a href="/wiki/Xenon_hexafluoride" title="Xenon hexafluoride">hexafluoride</a>, and multiple oxyfluorides have been isolated since then.<a href="#cite_note-FOOTNOTEWibergWibergHolleman2001395–397,_400-164">[151]</a> Among other noble gases, krypton forms a <a href="/wiki/Krypton_difluoride" title="Krypton difluoride">difluoride</a>,<a href="#cite_note-FOOTNOTELewars200868-165">[152]</a> and radon and fluorine generate a solid suspected to be <a href="/wiki/Radon_difluoride" title="Radon difluoride">radon difluoride</a>.<a href="#cite_note-astatineradon-166">[153]</a><a href="#cite_note-FOOTNOTELewars200867-167">[154]</a> Binary fluorides of lighter noble gases are exceptionally unstable: argon and hydrogen fluoride combine under extreme conditions to give <a href="/wiki/Argon_fluorohydride" title="Argon fluorohydride">argon fluorohydride</a>.<a href="#cite_note-Khriachtchev_et_al._2000-44">[42]</a> Helium has no long-lived fluorides,<a href="#cite_note-HeNeCompounds-168">[155]</a> and no neon fluoride has ever been observed;<a href="#cite_note-FOOTNOTELewars200871-169">[156]</a> helium fluorohydride has been detected for milliseconds at high pressures and low temperatures.<a href="#cite_note-HeNeCompounds-168">[155]</a> <div class="mw-heading mw-heading3"><h3 id="Organic_compounds">Organic compounds</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=19" title="Edit section: Organic compounds">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:FluorocarbonCrabFish.JPG" class="mw-file-description"><img alt="Beaker with two layers of liquid, goldfish and crab in top, coin sunk in the bottom" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/5c/FluorocarbonCrabFish.JPG/220px-FluorocarbonCrabFish.JPG" decoding="async" width="220" height="162" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/5c/FluorocarbonCrabFish.JPG/330px-FluorocarbonCrabFish.JPG 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/5c/FluorocarbonCrabFish.JPG/440px-FluorocarbonCrabFish.JPG 2x" data-file-width="2574" data-file-height="1892" /></a><figcaption><a href="/wiki/Miscibility" title="Miscibility">Immiscible</a> layers of colored water (top) and much denser <a href="/wiki/Perfluoroheptane" title="Perfluoroheptane">perfluoroheptane</a> (bottom) in a beaker; a goldfish and crab cannot penetrate the boundary; <a href="/wiki/Quarter_(United_States_coin)" title="Quarter (United States coin)">quarters</a> rest at the bottom.</figcaption></figure> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Organofluorine_chemistry" title="Organofluorine chemistry">Organofluorine chemistry</a></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Nafion2.svg" class="mw-file-description"><img alt="Skeletal chemical formula" src="//upload.wikimedia.org/wikipedia/commons/thumb/3/3d/Nafion2.svg/330px-Nafion2.svg.png" decoding="async" width="300" height="130" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/3/3d/Nafion2.svg/500px-Nafion2.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/3/3d/Nafion2.svg/960px-Nafion2.svg.png 2x" data-file-width="1063" data-file-height="461" /></a><figcaption>Chemical structure of <a href="/wiki/Nafion" title="Nafion">Nafion</a>, a fluoropolymer used in fuel cells and many other applications<a href="#cite_note-FOOTNOTEHoogers20024–12-170">[157]</a></figcaption></figure> The <a href="/wiki/Carbon%E2%80%93fluorine_bond" title="Carbon–fluorine bond">carbon–fluorine bond</a> is <a href="/wiki/Organic_chemistry" title="Organic chemistry">organic chemistry</a>'s strongest,<a href="#cite_note-hagan-171">[158]</a> and gives stability to organofluorines.<a href="#cite_note-FOOTNOTESiegemund_et_al.2005444-172">[159]</a> It is almost non-existent in nature, but is used in artificial compounds. Research in this area is usually driven by commercial applications;<a href="#cite_note-173">[160]</a> the compounds involved are diverse and reflect the complexity inherent in organic chemistry.<a href="#cite_note-Jstg-102">[93]</a> <div class="mw-heading mw-heading4"><h4 id="Discrete_molecules">Discrete molecules</h4>[<a href="/w/index.php?title=Fluorine&action=edit&section=20" title="Edit section: Discrete molecules">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">Main articles: <a href="/wiki/Fluorocarbon" title="Fluorocarbon">Fluorocarbon</a> and <a href="/wiki/Perfluorinated_compound" title="Perfluorinated compound">Perfluorinated compound</a></div> The substitution of hydrogen atoms in an <a href="/wiki/Alkane" title="Alkane">alkane</a> by progressively more fluorine atoms gradually alters several properties: melting and boiling points are lowered, density increases, solubility in hydrocarbons decreases and overall stability increases. <a href="/wiki/Perfluorocarbon" class="mw-redirect" title="Perfluorocarbon">Perfluorocarbons</a>,<a href="#cite_note-174">[note 14]</a> in which all hydrogen atoms are substituted, are insoluble in most organic solvents, reacting at ambient conditions only with sodium in liquid ammonia.<a href="#cite_note-FOOTNOTESiegemund_et_al.2005451–452-175">[161]</a> The term <a href="/wiki/Perfluorinated_compound" title="Perfluorinated compound">perfluorinated compound</a> is used for what would otherwise be a perfluorocarbon if not for the presence of a <a href="/wiki/Functional_group" title="Functional group">functional group</a>,<a href="#cite_note-176">[162]</a><a href="#cite_note-178">[note 15]</a> often a <a href="/wiki/Carboxylic_acid" title="Carboxylic acid">carboxylic acid</a>. These compounds share many properties with perfluorocarbons such as stability and <a href="/wiki/Hydrophobicity" class="mw-redirect" title="Hydrophobicity">hydrophobicity</a>,<a href="#cite_note-fluorotelomer-179">[164]</a> while the functional group augments their reactivity, enabling them to adhere to surfaces or act as <a href="/wiki/Surfactant" title="Surfactant">surfactants</a>.<a href="#cite_note-Salager2002-180">[165]</a> <a href="/wiki/Fluorosurfactant" class="mw-redirect" title="Fluorosurfactant">Fluorosurfactants</a>, in particular, can lower the <a href="/wiki/Surface_tension" title="Surface tension">surface tension</a> of water more than their hydrocarbon-based analogues. <a href="/wiki/Fluorotelomer" title="Fluorotelomer">Fluorotelomers</a>, which have some unfluorinated carbon atoms near the functional group, are also regarded as perfluorinated.<a href="#cite_note-fluorotelomer-179">[164]</a> <div class="mw-heading mw-heading4"><h4 id="Polymers">Polymers</h4>[<a href="/w/index.php?title=Fluorine&action=edit&section=21" title="Edit section: Polymers">edit</a>]</div> Polymers exhibit the same stability increases afforded by fluorine substitution (for hydrogen) in discrete molecules; their melting points generally increase too.<a href="#cite_note-FOOTNOTECarlsonSchmiegel20003-181">[166]</a> <a href="/wiki/Polytetrafluoroethylene" title="Polytetrafluoroethylene">Polytetrafluoroethylene</a> (PTFE), the simplest fluoropolymer and perfluoro analogue of <a href="/wiki/Polyethylene" title="Polyethylene">polyethylene</a> with <a href="/wiki/Structural_unit" title="Structural unit">structural unit</a> –CF 2–, demonstrates this change as expected, but its very high melting point makes it difficult to mold.<a href="#cite_note-FOOTNOTECarlsonSchmiegel20003–4-182">[167]</a> Various PTFE derivatives are less temperature-tolerant but easier to mold: <a href="/wiki/Fluorinated_ethylene_propylene" title="Fluorinated ethylene propylene">fluorinated ethylene propylene</a> replaces some fluorine atoms with <a href="/wiki/Trifluoromethyl" class="mw-redirect" title="Trifluoromethyl">trifluoromethyl</a> groups, <a href="/wiki/Perfluoroalkoxy_alkane" title="Perfluoroalkoxy alkane">perfluoroalkoxy alkanes</a> do the same with <a href="/wiki/Trifluoromethoxy" class="mw-redirect" title="Trifluoromethoxy">trifluoromethoxy</a> groups,<a href="#cite_note-FOOTNOTECarlsonSchmiegel20003–4-182">[167]</a> and <a href="/wiki/Nafion" title="Nafion">Nafion</a> contains perfluoroether side chains capped with <a href="/wiki/Sulfonic_acid" title="Sulfonic acid">sulfonic acid</a> groups.<a href="#cite_note-183">[168]</a><a href="#cite_note-184">[169]</a> Other fluoropolymers retain some hydrogen atoms; <a href="/wiki/Polyvinylidene_fluoride" title="Polyvinylidene fluoride">polyvinylidene fluoride</a> has half the fluorine atoms of PTFE and <a href="/wiki/Polyvinyl_fluoride" title="Polyvinyl fluoride">polyvinyl fluoride</a> has a quarter, but both behave much like perfluorinated polymers.<a href="#cite_note-FOOTNOTECarlsonSchmiegel20004-185">[170]</a> <div class="mw-heading mw-heading2"><h2 id="Production">Production</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=22" title="Edit section: Production">edit</a>]</div> Elemental fluorine and virtually all fluorine compounds are produced from <a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">hydrogen fluoride</a> or its aqueous solution, <a href="/wiki/Hydrofluoric_acid" title="Hydrofluoric acid">hydrofluoric acid</a>. Hydrogen fluoride is produced in <a href="/wiki/Kiln" title="Kiln">kilns</a> by the <a href="/wiki/Endothermic_reaction" class="mw-redirect" title="Endothermic reaction">endothermic reaction</a> of <a href="/wiki/Fluorite" title="Fluorite">fluorite</a> (CaF2) with sulfuric acid:<a href="#cite_note-FOOTNOTEAigueperse_et_al.2000-186">[171]</a> <dl><dd>CaF2 + H2SO4 → 2 HF(g) + CaSO4</dd></dl> The gaseous HF can then be absorbed in water or liquefied.<a href="#cite_note-187">[172]</a> About 20% of manufactured HF is a byproduct of fertilizer production, which produces <a href="/wiki/Hexafluorosilicic_acid" title="Hexafluorosilicic acid">hexafluorosilicic acid</a> (H2SiF6), which can be degraded to release HF thermally and by hydrolysis: <dl><dd>H2SiF6 → 2 HF + SiF4</dd> <dd>SiF4 + 2 H2O → 4 HF + SiO2</dd></dl> <div class="mw-heading mw-heading3"><h3 id="Industrial_routes_to_F2">Industrial routes to F2</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=23" title="Edit section: Industrial routes to F2">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Fluorine_cell_room.jpg" class="mw-file-description"><img alt="A machine room" src="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/Fluorine_cell_room.jpg/250px-Fluorine_cell_room.jpg" decoding="async" width="220" height="170" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/Fluorine_cell_room.jpg/330px-Fluorine_cell_room.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/04/Fluorine_cell_room.jpg/440px-Fluorine_cell_room.jpg 2x" data-file-width="480" data-file-height="370" /></a><figcaption>Industrial fluorine cells at <a href="/wiki/City_of_Preston,_Lancashire" title="City of Preston, Lancashire">Preston</a></figcaption></figure> Moissan's method is used to produce industrial quantities of fluorine, via the electrolysis of a <a href="/wiki/Potassium_bifluoride" title="Potassium bifluoride">potassium bifluoride</a>/<a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">hydrogen fluoride</a> mixture: hydrogen ions are reduced at a steel container <a href="/wiki/Cathode" title="Cathode">cathode</a> and fluoride ions are oxidized at a carbon block <a href="/wiki/Anode" title="Anode">anode</a>, under 8–12 volts, to generate hydrogen and fluorine gas respectively.<a href="#cite_note-AcountF-70">[66]</a><a href="#cite_note-FOOTNOTEJaccaud_et_al.2000386-188">[173]</a> Temperatures are elevated, KF•2HF melting at 70 °C (158 °F) and being electrolyzed at 70–130 °C (158–266 °F). KF, which acts to provide electrical conductivity, is essential since pure HF cannot be electrolyzed because it is virtually non-conductive.<a href="#cite_note-ModFcchem-87">[81]</a><a href="#cite_note-FOOTNOTEJaccaud_et_al.2000384–285-189">[174]</a><a href="#cite_note-FOOTNOTEGreenwoodEarnshaw1998796–797-190">[175]</a> Fluorine can be stored in steel cylinders that have passivated interiors, at temperatures below 200 °C (392 °F); otherwise nickel can be used.<a href="#cite_note-ModFcchem-87">[81]</a><a href="#cite_note-FOOTNOTEJaccaud_et_al.2000384–385-191">[176]</a> Regulator valves and pipework are made of nickel, the latter possibly using <a href="/wiki/Monel" title="Monel">Monel</a> instead.<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000390–391-192">[177]</a> Frequent passivation, along with the strict exclusion of water and greases, must be undertaken. In the laboratory, glassware may carry fluorine gas under low pressure and anhydrous conditions;<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000390–391-192">[177]</a> some sources instead recommend nickel-Monel-PTFE systems.<a href="#cite_note-Shriver_Inorganic-193">[178]</a> <div class="mw-heading mw-heading3"><h3 id="Laboratory_routes">Laboratory routes</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=24" title="Edit section: Laboratory routes">edit</a>]</div> While preparing for a 1986 conference to celebrate the centennial of Moissan's achievement, <a href="/wiki/Karl_O._Christe" title="Karl O. Christe">Karl O. Christe</a> reasoned that chemical fluorine generation should be feasible since some metal fluoride anions have no stable neutral counterparts; their acidification potentially triggers oxidation instead. He devised a method which evolves fluorine at high yield and atmospheric pressure:<a href="#cite_note-'year'-194">[179]</a> <dl><dd>2 <a href="/wiki/Potassium_permanganate" title="Potassium permanganate">KMnO4</a> + 2 <a href="/wiki/Potassium_fluoride" title="Potassium fluoride">KF</a> + 10 <a href="/wiki/Hydrogen_fluoride" title="Hydrogen fluoride">HF</a> + 3 <a href="/wiki/Hydrogen_peroxide" title="Hydrogen peroxide">H2O2</a> → 2 K2MnF6 + 8 <a href="/wiki/Water" title="Water">H2O</a> + 3 <a href="/wiki/Molecular_oxygen" class="mw-redirect" title="Molecular oxygen">O2</a>↑</dd> <dd>2 K2MnF6 + 4 <a href="/wiki/Antimony_pentafluoride" title="Antimony pentafluoride">SbF5</a> → 4 KSbF6 + 2 <a href="/wiki/Manganese(III)_fluoride" title="Manganese(III) fluoride">MnF3</a> + F2↑</dd></dl> Christe later commented that the reactants "had been known for more than 100 years and even Moissan could have come up with this scheme."<a href="#cite_note-195">[180]</a> As late as 2008, some references still asserted that fluorine was too reactive for any chemical isolation.<a href="#cite_note-196">[181]</a> <div class="mw-heading mw-heading2"><h2 id="Industrial_applications">Industrial applications</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=25" title="Edit section: Industrial applications">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/Fluorochemical_industry" title="Fluorochemical industry">Fluorochemical industry</a></div> Fluorite mining, which supplies most global fluorine, peaked in 1989 when 5.6 million <a href="/wiki/Metric_ton" class="mw-redirect" title="Metric ton">metric tons</a> of ore were extracted. Chlorofluorocarbon restrictions lowered this to 3.6 million tons in 1994; production has since been increasing. Around 4.5 million tons of ore and revenue of <a href="/wiki/United_States_dollar" title="United States dollar">US$</a>550 million were generated in 2003; later reports estimated 2011 global fluorochemical sales at $15 billion and predicted 2016–18 production figures of 3.5 to 5.9 million tons, and revenue of at least $20 billion.<a href="#cite_note-ModFcchem-87">[81]</a><a href="#cite_note-197">[182]</a><a href="#cite_note-198">[183]</a><a href="#cite_note-199">[184]</a><a href="#cite_note-200">[185]</a> <a href="/wiki/Froth_flotation" title="Froth flotation">Froth flotation</a> separates mined fluorite into two main metallurgical grades of equal proportion: 60–85% pure metspar is almost all used in iron smelting whereas 97%+ pure acidspar is mainly converted to the key industrial <a href="/wiki/Chemical_intermediate" class="mw-redirect" title="Chemical intermediate">intermediate</a> hydrogen fluoride.<a href="#cite_note-AcountF-70">[66]</a><a href="#cite_note-ModFcchem-87">[81]</a><a href="#cite_note-SME_mining_2006-201">[186]</a> <figure class="mw-halign-center noresize" typeof="mw:File/Thumb"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/5/57/The_fluorine_economy.svg/675px-The_fluorine_economy.svg.png" decoding="async" width="675" height="392" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/57/The_fluorine_economy.svg/1013px-The_fluorine_economy.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/57/The_fluorine_economy.svg/1350px-The_fluorine_economy.svg.png 2x" data-file-width="625" data-file-height="363" usemap="#ImageMap_ebfa7fe28b15da4d" resource="/wiki/File:The_fluorine_economy.svg" /><map name="ImageMap_ebfa7fe28b15da4d"><area href="/wiki/Fluorite" shape="rect" coords="10,6,87,37" alt="Fluorite" title="Fluorite" /><area href="/wiki/Fluorapatite" shape="rect" coords="10,186,87,215" alt="Fluorapatite" title="Fluorapatite" /><area href="/wiki/Hydrogen_fluoride" shape="rect" coords="153,5,264,37" alt="Hydrogen fluoride" title="Hydrogen fluoride" /><area href="/wiki/Smelting" shape="rect" coords="153,70,265,105" alt="Metal smelting" title="Metal smelting" /><area href="/wiki/Glass_production" shape="rect" coords="153,131,264,166" alt="Glass production" title="Glass production" /><area href="/wiki/Organofluorine" shape="rect" coords="334,5,444,36" alt="Fluorocarbons" title="Fluorocarbons" /><area href="/wiki/Sodium_hexafluoroaluminate" shape="rect" coords="335,68,446,99" alt="Sodium hexafluoroaluminate" title="Sodium hexafluoroaluminate" /><area href="/wiki/Pickling_(metal)" shape="rect" coords="336,131,447,166" alt="Pickling (metal)" title="Pickling (metal)" /><area href="/wiki/Hexafluorosilicic_acid" shape="rect" coords="335,185,445,216" alt="Fluorosilicic acid" title="Fluorosilicic acid" /><area href="/wiki/Cracking_(chemistry)" shape="rect" coords="334,228,445,262" alt="Alkane cracking" title="Alkane cracking" /><area href="/wiki/Hydrofluorocarbon" shape="rect" coords="522,6,632,37" alt="Hydrofluorocarbon" title="Hydrofluorocarbon" /><area href="/wiki/Chlorofluorocarbon#Development_of_alternatives_for_CFCs" shape="rect" coords="523,51,632,82" alt="Hydrochlorofluorocarbons" title="Hydrochlorofluorocarbons" /><area href="/wiki/Chlorofluorocarbon" shape="rect" coords="522,95,633,125" alt="Chlorofluorocarbon" title="Chlorofluorocarbon" /><area href="/wiki/Polytetrafluoroethylene" shape="rect" coords="522,138,632,173" alt="Teflon" title="Teflon" /><area href="/wiki/Water_fluoridation" shape="rect" coords="523,184,633,216" alt="Water fluoridation" title="Water fluoridation" /><area href="/wiki/Enriched_uranium" shape="rect" coords="522,227,633,257" alt="Uranium enrichment" title="Uranium enrichment" /><area href="/wiki/Sulfur_hexafluoride" shape="rect" coords="523,279,633,310" alt="Sulfur hexafluoride" title="Sulfur hexafluoride" /><area href="/wiki/Tungsten_hexafluoride" shape="rect" coords="523,321,632,386" alt="Tungsten hexafluoride" title="Tungsten hexafluoride" /><area href="/wiki/Phosphogypsum" shape="rect" coords="30,266,191,316" alt="Phosphogypsum" title="Phosphogypsum" /></map><figcaption>Clickable diagram of the fluorochemical industry according to mass flows</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:SF6_current_transformer_TGFM-110_Russia.jpg" class="mw-file-description"><img alt="Minaret-like electrical devices with wires around them, thicker at the bottom" src="//upload.wikimedia.org/wikipedia/commons/thumb/0/03/SF6_current_transformer_TGFM-110_Russia.jpg/250px-SF6_current_transformer_TGFM-110_Russia.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/03/SF6_current_transformer_TGFM-110_Russia.jpg/330px-SF6_current_transformer_TGFM-110_Russia.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/03/SF6_current_transformer_TGFM-110_Russia.jpg/500px-SF6_current_transformer_TGFM-110_Russia.jpg 2x" data-file-width="1000" data-file-height="750" /></a><figcaption>SF 6 current transformers at a Russian railway</figcaption></figure> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Industrial_gas" title="Industrial gas">Industrial gas</a></div> At least 17,000 metric tons of fluorine are produced each year. It costs only $5–8 per kilogram as uranium or sulfur hexafluoride, but many times more as an element because of handling challenges. Most processes using free fluorine in large amounts employ in situ generation under <a href="/wiki/Vertical_integration" title="Vertical integration">vertical integration</a>.<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000392-202">[187]</a> The largest application of fluorine gas, consuming up to 7,000 metric tons annually, is in the preparation of UF 6 for the <a href="/wiki/Nuclear_fuel_cycle" title="Nuclear fuel cycle">nuclear fuel cycle</a>. Fluorine is used to fluorinate <a href="/wiki/Uranium_tetrafluoride" title="Uranium tetrafluoride">uranium tetrafluoride</a>, itself formed from uranium dioxide and hydrofluoric acid.<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000392-202">[187]</a> Fluorine is monoisotopic, so any mass differences between UF 6 molecules are due to the presence of 235 U or 238 U, enabling uranium enrichment via gaseous diffusion or <a href="/wiki/Gas_centrifuge" title="Gas centrifuge">gas centrifuge</a>.<a href="#cite_note-FOOTNOTEJaccaud_et_al.2000382-5">[5]</a><a href="#cite_note-AcountF-70">[66]</a> About 6,000 metric tons per year go into producing the inert <a href="/wiki/Dielectric" title="Dielectric">dielectric</a> SF 6 for high-voltage transformers and circuit breakers, eliminating the need for hazardous <a href="/wiki/Polychlorinated_biphenyl" title="Polychlorinated biphenyl">polychlorinated biphenyls</a> associated with oil-filled devices.<a href="#cite_note-FOOTNOTEAigueperse_et_al.2000430-203">[188]</a> Several fluorine compounds are used in electronics: rhenium and tungsten hexafluoride in <a href="/wiki/Chemical_vapor_deposition" title="Chemical vapor deposition">chemical vapor deposition</a>, <a href="/wiki/Tetrafluoromethane" class="mw-redirect" title="Tetrafluoromethane">tetrafluoromethane</a> in <a href="/wiki/Plasma_etching" title="Plasma etching">plasma etching</a><a href="#cite_note-FOOTNOTEJaccaud_et_al.2000391–392-204">[189]</a><a href="#cite_note-205">[190]</a><a href="#cite_note-206">[191]</a> and <a href="/wiki/Nitrogen_trifluoride" title="Nitrogen trifluoride">nitrogen trifluoride</a> in cleaning equipment.<a href="#cite_note-AcountF-70">[66]</a> Fluorine is also used in the synthesis of organic fluorides, but its reactivity often necessitates conversion first to the gentler ClF 3, BrF 3, or IF 5, which together allow calibrated fluorination. Fluorinated pharmaceuticals use <a href="/wiki/Sulfur_tetrafluoride" title="Sulfur tetrafluoride">sulfur tetrafluoride</a> instead.<a href="#cite_note-AcountF-70">[66]</a> <div class="mw-heading mw-heading3"><h3 id="Inorganic_fluorides">Inorganic fluorides</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=26" title="Edit section: Inorganic fluorides">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Hall-Heroult_cell_schematic.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fb/Hall-Heroult_cell_schematic.svg/330px-Hall-Heroult_cell_schematic.svg.png" decoding="async" width="300" height="180" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fb/Hall-Heroult_cell_schematic.svg/500px-Hall-Heroult_cell_schematic.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fb/Hall-Heroult_cell_schematic.svg/600px-Hall-Heroult_cell_schematic.svg.png 2x" data-file-width="640" data-file-height="384" /></a><figcaption>Aluminium extraction depends critically on cryolite</figcaption></figure> As with other iron alloys, around 3 kg (6.6 lb) metspar is added to each metric ton of steel; the fluoride ions lower its melting point and <a href="/wiki/Viscosity" title="Viscosity">viscosity</a>.<a href="#cite_note-AcountF-70">[66]</a><a href="#cite_note-USGS-207">[192]</a> Alongside its role as an additive in materials like enamels and welding rod coats, most acidspar is reacted with sulfuric acid to form hydrofluoric acid, which is used in steel <a href="/wiki/Pickling_(metal)" title="Pickling (metal)">pickling</a>, glass etching and <a href="/wiki/Cracking_(chemistry)" title="Cracking (chemistry)">alkane cracking</a>.<a href="#cite_note-AcountF-70">[66]</a> One-third of HF goes into synthesizing <a href="/wiki/Sodium_hexafluoroaluminate" title="Sodium hexafluoroaluminate">cryolite</a> and <a href="/wiki/Aluminium_trifluoride" class="mw-redirect" title="Aluminium trifluoride">aluminium trifluoride</a>, both fluxes in the <a href="/wiki/Hall%E2%80%93H%C3%A9roult_process" title="Hall–Héroult process">Hall–Héroult process</a> for aluminium extraction; replenishment is necessitated by their occasional reactions with the smelting apparatus. Each metric ton of aluminium requires about 23 kg (51 lb) of flux.<a href="#cite_note-AcountF-70">[66]</a><a href="#cite_note-208">[193]</a> Fluorosilicates consume the second largest portion, with <a href="/wiki/Sodium_fluorosilicate" title="Sodium fluorosilicate">sodium fluorosilicate</a> used in water fluoridation and laundry effluent treatment, and as an intermediate en route to cryolite and silicon tetrafluoride.<a href="#cite_note-FOOTNOTEAigueperse_et_al.2000428-209">[194]</a> Other important inorganic fluorides include those of <a href="/wiki/Cobalt_difluoride" class="mw-redirect" title="Cobalt difluoride">cobalt</a>, <a href="/wiki/Nickel_difluoride" class="mw-redirect" title="Nickel difluoride">nickel</a>, and <a href="/wiki/Ammonium_fluoride" title="Ammonium fluoride">ammonium</a>.<a href="#cite_note-AcountF-70">[66]</a><a href="#cite_note-FOOTNOTEAigueperse_et_al.2000420–422-114">[104]</a><a href="#cite_note-210">[195]</a> <div class="mw-heading mw-heading3"><h3 id="Organic_fluorides">Organic fluorides</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=27" title="Edit section: Organic fluorides">edit</a>]</div> Organofluorides consume over 20% of mined fluorite and over 40% of hydrofluoric acid, with <a href="#Refrigerant_gases">refrigerant gases</a> dominating and <a href="#Fluoropolymers">fluoropolymers</a> increasing their market share.<a href="#cite_note-AcountF-70">[66]</a><a href="#cite_note-GIA_f-chem_report_description-211">[196]</a> <a href="#Surfactants">Surfactants</a> are a minor application but generate over $1 billion in annual revenue.<a href="#cite_note-fluorosurfactant_market-212">[197]</a> Due to the danger from direct hydrocarbon–fluorine reactions above −150 °C (−238 °F), industrial fluorocarbon production is indirect, mostly through <a href="/wiki/Finkelstein_reaction" title="Finkelstein reaction">halogen exchange reactions</a> such as <a href="/wiki/Swarts_fluorination" title="Swarts fluorination">Swarts fluorination</a>, in which chlorocarbon chlorines are substituted for fluorines by hydrogen fluoride under catalysts. <a href="/wiki/Electrochemical_fluorination" title="Electrochemical fluorination">Electrochemical fluorination</a> subjects hydrocarbons to electrolysis in hydrogen fluoride, and the <a href="/wiki/Fowler_process" title="Fowler process">Fowler process</a> treats them with solid fluorine carriers like <a href="/wiki/Cobalt_trifluoride" class="mw-redirect" title="Cobalt trifluoride">cobalt trifluoride</a>.<a href="#cite_note-Jstg-102">[93]</a><a href="#cite_note-213">[198]</a> <div class="mw-heading mw-heading4"><h4 id="Refrigerant_gases">Refrigerant gases</h4>[<a href="/w/index.php?title=Fluorine&action=edit&section=28" title="Edit section: Refrigerant gases">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Refrigerant" title="Refrigerant">Refrigerant</a></div> Halogenated refrigerants, termed Freons in informal contexts,<a href="#cite_note-214">[note 16]</a> are identified by <a href="/wiki/Refrigerant#Classification_of_refrigerants" title="Refrigerant">R-numbers</a> that denote the amount of fluorine, chlorine, carbon, and hydrogen present.<a href="#cite_note-AcountF-70">[66]</a><a href="#cite_note-215">[199]</a> <a href="/wiki/Chlorofluorocarbons" class="mw-redirect" title="Chlorofluorocarbons">Chlorofluorocarbons</a> (CFCs) like <a href="/wiki/Trichlorofluoromethane" title="Trichlorofluoromethane">R-11</a>, <a href="/wiki/Dichlorodifluoromethane" title="Dichlorodifluoromethane">R-12</a>, and <a href="/wiki/1,2-dichlorotetrafluoroethane" class="mw-redirect" title="1,2-dichlorotetrafluoroethane">R-114</a> once dominated organofluorines, peaking in production in the 1980s. Used for air conditioning systems, propellants and solvents, their production was below one-tenth of this peak by the early 2000s, after widespread international prohibition.<a href="#cite_note-AcountF-70">[66]</a> Hydrochlorofluorocarbons (HCFCs) and hydrofluorocarbons (HFCs) were designed as replacements; their synthesis consumes more than 90% of the fluorine in the organic industry. Important HCFCs include R-22, <a href="/wiki/Chlorodifluoromethane" title="Chlorodifluoromethane">chlorodifluoromethane</a>, and <a href="/wiki/1,1-Dichloro-1-fluoroethane" title="1,1-Dichloro-1-fluoroethane">R-141b</a>. The main HFC is <a href="/wiki/1,1,1,2-Tetrafluoroethane" title="1,1,1,2-Tetrafluoroethane">R-134a</a><a href="#cite_note-AcountF-70">[66]</a> with a new type of molecule <a href="/wiki/2,3,3,3-Tetrafluoropropene" title="2,3,3,3-Tetrafluoropropene">HFO-1234yf</a>, a <a href="/wiki/Hydrofluoroolefin" title="Hydrofluoroolefin">Hydrofluoroolefin</a> (HFO) coming to prominence owing to its <a href="/wiki/Global_warming_potential" title="Global warming potential">global warming potential</a> of less than 1% that of HFC-134a.<a href="#cite_note-HFO-216">[200]</a> <div class="mw-heading mw-heading4"><h4 id="Polymers_2">Polymers</h4>[<a href="/w/index.php?title=Fluorine&action=edit&section=29" title="Edit section: Polymers">edit</a>]</div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:A_water_droplet_DWR-coated_surface2_edit1.jpg" class="mw-file-description"><img alt="Shiny spherical drop of water on blue cloth" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f4/A_water_droplet_DWR-coated_surface2_edit1.jpg/220px-A_water_droplet_DWR-coated_surface2_edit1.jpg" decoding="async" width="220" height="185" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f4/A_water_droplet_DWR-coated_surface2_edit1.jpg/330px-A_water_droplet_DWR-coated_surface2_edit1.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f4/A_water_droplet_DWR-coated_surface2_edit1.jpg/440px-A_water_droplet_DWR-coated_surface2_edit1.jpg 2x" data-file-width="1016" data-file-height="856" /></a><figcaption>Fluorosurfactant-treated fabrics are often <a href="/wiki/Hydrophobe" title="Hydrophobe">hydrophobic</a>.</figcaption></figure> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Fluoropolymer" title="Fluoropolymer">Fluoropolymer</a></div> About 180,000 metric tons of fluoropolymers were produced in 2006 and 2007, generating over $3.5 billion revenue per year.<a href="#cite_note-yearly_FP_production-217">[201]</a> The global market was estimated at just under $6 billion in 2011.<a href="#cite_note-218">[202]</a> Fluoropolymers can only be formed by <a href="/wiki/Polymerization" title="Polymerization">polymerizing</a> free radicals.<a href="#cite_note-FOOTNOTECarlsonSchmiegel20003-181">[166]</a> Polytetrafluoroethylene (PTFE), sometimes called by its DuPont name Teflon,<a href="#cite_note-encyc_of_structure-219">[203]</a> represents 60–80% by mass of the world's fluoropolymer production.<a href="#cite_note-yearly_FP_production-217">[201]</a> The largest application is in <a href="/wiki/Electrical_insulation" class="mw-redirect" title="Electrical insulation">electrical insulation</a> since PTFE is an excellent <a href="/wiki/Dielectric" title="Dielectric">dielectric</a>. It is also used in the chemical industry where corrosion resistance is needed, in coating pipes, tubing, and gaskets. Another major use is in PFTE-coated <a href="/wiki/Fabric_structure" title="Fabric structure">fiberglass cloth</a> for stadium roofs. The major consumer application is for <a href="/wiki/Non-stick_surface" title="Non-stick surface">non-stick cookware</a>.<a href="#cite_note-encyc_of_structure-219">[203]</a> Jerked PTFE film becomes expanded PTFE (ePTFE), a fine-pored <a href="/wiki/Synthetic_membrane" title="Synthetic membrane">membrane</a> sometimes referred to by the brand name <a href="/wiki/Gore-Tex" title="Gore-Tex">Gore-Tex</a> and used for rainwear, <a href="/wiki/Personal_protective_equipment" title="Personal protective equipment">protective apparel</a>, and <a href="/wiki/Filtration" title="Filtration">filters</a>; <a href="/wiki/PTFE_fiber" title="PTFE fiber">ePTFE fibers</a> may be made into <a href="/wiki/Seal_(mechanical)" title="Seal (mechanical)">seals</a> and <a href="/wiki/Dust_collector" title="Dust collector">dust filters</a>.<a href="#cite_note-encyc_of_structure-219">[203]</a> Other fluoropolymers, including <a href="/wiki/Fluorinated_ethylene_propylene" title="Fluorinated ethylene propylene">fluorinated ethylene propylene</a>, mimic PTFE's properties and can substitute for it; they are more moldable, but also more costly and have lower thermal stability. Films from two different fluoropolymers replace glass in solar cells.<a href="#cite_note-encyc_of_structure-219">[203]</a><a href="#cite_note-DeBergalis-220">[204]</a> The chemically resistant (but expensive) fluorinated <a href="/wiki/Ionomer" title="Ionomer">ionomers</a> are used as electrochemical cell membranes, of which the first and most prominent example is <a href="/wiki/Nafion" title="Nafion">Nafion</a>. Developed in the 1960s, it was initially deployed as fuel cell material in spacecraft and then replaced mercury-based <a href="/wiki/Chloralkali_process" title="Chloralkali process">chloralkali process</a> cells. Recently, the fuel cell application has reemerged with efforts to install <a href="/wiki/Proton_exchange_membrane" class="mw-redirect" title="Proton exchange membrane">proton exchange membrane</a> fuel cells into automobiles.<a href="#cite_note-Fluorinated_Ionomers-221">[205]</a><a href="#cite_note-Functional_Materials-222">[206]</a><a href="#cite_note-Chlor-alkali_and_chlorate_technology-223">[207]</a> <a href="/wiki/Fluoroelastomer" title="Fluoroelastomer">Fluoroelastomers</a> such as <a href="/wiki/Viton" class="mw-redirect" title="Viton">Viton</a> are <a href="/wiki/Crosslink" class="mw-redirect" title="Crosslink">crosslinked</a> fluoropolymer mixtures mainly used in <a href="/wiki/O-ring" title="O-ring">O-rings</a>;<a href="#cite_note-encyc_of_structure-219">[203]</a> <a href="/wiki/Perfluorobutane" title="Perfluorobutane">perfluorobutane</a> (C4F10) is used as a fire-extinguishing agent.<a href="#cite_note-FOOTNOTESlye201210-224">[208]</a> <div class="mw-heading mw-heading4"><h4 id="Surfactants">Surfactants</h4>[<a href="/w/index.php?title=Fluorine&action=edit&section=30" title="Edit section: Surfactants">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">Main articles: <a href="/wiki/Fluorinated_surfactant" class="mw-redirect" title="Fluorinated surfactant">Fluorinated surfactant</a> and <a href="/wiki/Durable_water_repellent" title="Durable water repellent">Durable water repellent</a></div> Fluorosurfactants are small organofluorine molecules used for repelling water and stains. Although expensive (comparable to pharmaceuticals at $200–2000 per kilogram), they yielded over $1 billion in annual revenues by 2006; <a href="/wiki/Scotchgard" title="Scotchgard">Scotchgard</a> alone generated over $300 million in 2000.<a href="#cite_note-fluorosurfactant_market-212">[197]</a><a href="#cite_note-Fluorinated_surfactants-225">[209]</a><a href="#cite_note-Ullman_fibers-226">[210]</a> Fluorosurfactants are a minority in the overall surfactant market, most of which is taken up by much cheaper hydrocarbon-based products. Applications in <a href="/wiki/Surfactants_in_paint" title="Surfactants in paint">paints</a> are burdened by <a href="/wiki/Compounding" title="Compounding">compounding</a> costs; this use was valued at only $100 million in 2006.<a href="#cite_note-fluorosurfactant_market-212">[197]</a> <div class="mw-heading mw-heading4"><h4 id="Agrichemicals">Agrichemicals</h4>[<a href="/w/index.php?title=Fluorine&action=edit&section=31" title="Edit section: Agrichemicals">edit</a>]</div> About 30% of <a href="/wiki/Agrichemical" class="mw-redirect" title="Agrichemical">agrichemicals</a> contain fluorine,<a href="#cite_note-227">[211]</a> most of them <a href="/wiki/Herbicide" title="Herbicide">herbicides</a> and <a href="/wiki/Fungicide" title="Fungicide">fungicides</a> with a few <a href="/wiki/Plant_hormone" title="Plant hormone">crop regulators</a>. Fluorine substitution, usually of a single atom or at most a <a href="/wiki/Trifluoromethyl" class="mw-redirect" title="Trifluoromethyl">trifluoromethyl</a> group, is a robust modification with effects analogous to fluorinated pharmaceuticals: increased biological stay time, membrane crossing, and altering of molecular recognition.<a href="#cite_note-Theodoridis-228">[212]</a> <a href="/wiki/Trifluralin" title="Trifluralin">Trifluralin</a> is a prominent example, with large-scale use in the U.S. as a weedkiller,<a href="#cite_note-Theodoridis-228">[212]</a><a href="#cite_note-trifluralin-229">[213]</a> but it is a suspected carcinogen and has been banned in many European countries.<a href="#cite_note-230">[214]</a> <a href="/wiki/Sodium_monofluoroacetate" class="mw-redirect" title="Sodium monofluoroacetate">Sodium monofluoroacetate</a> (1080) is a mammalian poison in which one <a href="/wiki/Sodium_acetate" title="Sodium acetate">sodium acetate</a> hydrogen is replaced with fluorine; it disrupts cell metabolism by replacing acetate in the <a href="/wiki/Citric_acid_cycle" title="Citric acid cycle">citric acid cycle</a>. First synthesized in the late 19th century, it was recognized as an <a href="/wiki/Insecticide" title="Insecticide">insecticide</a> in the early 20th century, and was later deployed in its current use. New Zealand, the largest consumer of 1080, uses it to protect <a href="/wiki/Kiwi_(bird)" title="Kiwi (bird)">kiwis</a> from the invasive Australian <a href="/wiki/Common_brushtail_possum" title="Common brushtail possum">common brushtail possum</a>.<a href="#cite_note-Beasley-231">[215]</a> Europe and the U.S. have banned 1080.<a href="#cite_note-FOOTNOTEProudfootBradberryVale2006-232">[216]</a><a href="#cite_note-FOOTNOTEEisler1995-233">[217]</a><a href="#cite_note-234">[note 17]</a> <div class="mw-heading mw-heading2"><h2 id="Medicinal_applications">Medicinal applications</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=32" title="Edit section: Medicinal applications">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="Dental_care">Dental care</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=33" title="Edit section: Dental care">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:US_Navy_090526-F-1333S-023_A_service_member_embarked_aboard_the_Military_Sealift_Command_hospital_ship_USNS_Comfort_(T-AH_20)_gives_a_Fluoride_treatment_to_a_patient_during_a_Continuing_Promise_2009_medical_civil_service_projec.jpg" class="mw-file-description"><img alt="Man holding plastic tray with brown material in it and sticking a small stick into a boy's open mouth" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f3/US_Navy_090526-F-1333S-023_A_service_member_embarked_aboard_the_Military_Sealift_Command_hospital_ship_USNS_Comfort_%28T-AH_20%29_gives_a_Fluoride_treatment_to_a_patient_during_a_Continuing_Promise_2009_medical_civil_service_projec.jpg/220px-thumbnail.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f3/US_Navy_090526-F-1333S-023_A_service_member_embarked_aboard_the_Military_Sealift_Command_hospital_ship_USNS_Comfort_%28T-AH_20%29_gives_a_Fluoride_treatment_to_a_patient_during_a_Continuing_Promise_2009_medical_civil_service_projec.jpg/330px-thumbnail.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f3/US_Navy_090526-F-1333S-023_A_service_member_embarked_aboard_the_Military_Sealift_Command_hospital_ship_USNS_Comfort_%28T-AH_20%29_gives_a_Fluoride_treatment_to_a_patient_during_a_Continuing_Promise_2009_medical_civil_service_projec.jpg/440px-thumbnail.jpg 2x" data-file-width="1860" data-file-height="1395" /></a><figcaption>Topical fluoride treatment in Panama</figcaption></figure> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">Main articles: <a href="/wiki/Fluoride_therapy" title="Fluoride therapy">Fluoride therapy</a>, <a href="/wiki/Water_fluoridation" title="Water fluoridation">Water fluoridation</a>, and <a href="/wiki/Water_fluoridation_controversy" class="mw-redirect" title="Water fluoridation controversy">Water fluoridation controversy</a></div> Population studies from the mid-20th century onwards show <a href="/wiki/Topical_medication" title="Topical medication">topical</a> fluoride reduces <a href="/wiki/Dental_caries" class="mw-redirect" title="Dental caries">dental caries</a>. This was first attributed to the conversion of tooth enamel <a href="/wiki/Hydroxyapatite" title="Hydroxyapatite">hydroxyapatite</a> into the more durable fluorapatite, but studies on pre-fluoridated teeth refuted this hypothesis, and current theories involve fluoride aiding enamel growth in small caries.<a href="#cite_note-Pizzo-235">[218]</a> After studies of children in areas where fluoride was naturally present in drinking water, controlled <a href="/wiki/Water_supply" title="Water supply">public water supply</a> fluoridation to fight tooth decay<a href="#cite_note-236">[219]</a> began in the 1940s and is now applied to water supplying 6 percent of the global population, including two-thirds of Americans.<a href="#cite_note-Ripa-237">[220]</a><a href="#cite_note-Cheng_Chalmers_Sheldon_2007-238">[221]</a> Reviews of the scholarly literature in 2000 and 2007 associated water fluoridation with a significant reduction of tooth decay in children.<a href="#cite_note-NHMRC-239">[222]</a> Despite such endorsements and evidence of no adverse effects other than mostly benign <a href="/wiki/Dental_fluorosis" title="Dental fluorosis">dental fluorosis</a>,<a href="#cite_note-240">[223]</a> <a href="/wiki/Water_fluoridation_controversy" class="mw-redirect" title="Water fluoridation controversy">opposition</a> still exists on ethical and safety grounds.<a href="#cite_note-Cheng_Chalmers_Sheldon_2007-238">[221]</a><a href="#cite_note-241">[224]</a> The benefits of fluoridation have lessened, possibly due to other fluoride sources, but are still measurable in low-income groups.<a href="#cite_note-Dental_caries-242">[225]</a> <a href="/wiki/Sodium_monofluorophosphate" title="Sodium monofluorophosphate">Sodium monofluorophosphate</a> and sometimes sodium or <a href="/wiki/Tin(II)_fluoride" title="Tin(II) fluoride">tin(II) fluoride</a> are often found in fluoride <a href="/wiki/Toothpaste" title="Toothpaste">toothpastes</a>, first introduced in the U.S. in 1955 and now ubiquitous in developed countries, alongside fluoridated mouthwashes, gels, foams, and varnishes.<a href="#cite_note-Dental_caries-242">[225]</a><a href="#cite_note-Crest_continuing_ed-243">[226]</a> <div class="mw-heading mw-heading3"><h3 id="Pharmaceuticals">Pharmaceuticals</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=34" title="Edit section: Pharmaceuticals">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Prozac_pills.jpg" class="mw-file-description"><img alt="Capsules with "Prozac" and "DISTA" visible" src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fe/Prozac_pills.jpg/250px-Prozac_pills.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fe/Prozac_pills.jpg/330px-Prozac_pills.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fe/Prozac_pills.jpg/500px-Prozac_pills.jpg 2x" data-file-width="2592" data-file-height="1944" /></a><figcaption><a href="/wiki/Fluoxetine" title="Fluoxetine">Fluoxetine</a> capsules</figcaption></figure> Twenty percent of modern pharmaceuticals contain fluorine.<a href="#cite_note-Emsley_2011_178-244">[227]</a> One of these, the cholesterol-reducer <a href="/wiki/Atorvastatin" title="Atorvastatin">atorvastatin</a> (Lipitor), made more revenue than any other drug until it became generic in 2011.<a href="#cite_note-url_Crain's_2011-245">[228]</a> The combination asthma prescription <a href="/wiki/Seretide" class="mw-redirect" title="Seretide">Seretide</a>, a top-ten revenue drug in the mid-2000s, contains two active ingredients, one of which – <a href="/wiki/Fluticasone" title="Fluticasone">fluticasone</a> – is fluorinated.<a href="#cite_note-Swinson-246">[229]</a> Many drugs are fluorinated to delay inactivation and lengthen dosage periods because the carbon–fluorine bond is very stable.<a href="#cite_note-Hagmann-247">[230]</a> Fluorination also increases <a href="/wiki/Lipophilicity" title="Lipophilicity">lipophilicity</a> because the bond is more hydrophobic than the <a href="/wiki/Carbon%E2%80%93hydrogen_bond" title="Carbon–hydrogen bond">carbon–hydrogen bond</a>, and this often helps in cell membrane penetration and hence <a href="/wiki/Bioavailability" title="Bioavailability">bioavailability</a>.<a href="#cite_note-Swinson-246">[229]</a> <a href="/wiki/Tricyclic_antidepressant" title="Tricyclic antidepressant">Tricyclics</a> and other pre-1980s <a href="/wiki/Antidepressant" title="Antidepressant">antidepressants</a> had several side effects due to their non-selective interference with <a href="/wiki/Neurotransmitter" title="Neurotransmitter">neurotransmitters</a> other than the <a href="/wiki/Serotonin" title="Serotonin">serotonin</a> target; the fluorinated <a href="/wiki/Fluoxetine" title="Fluoxetine">fluoxetine</a> was selective and one of the first to avoid this problem. Many current antidepressants receive this same treatment, including the <a href="/wiki/Selective_serotonin_reuptake_inhibitor" title="Selective serotonin reuptake inhibitor">selective serotonin reuptake inhibitors</a>: <a href="/wiki/Citalopram" title="Citalopram">citalopram</a>, its <a href="/wiki/Enantiomer" title="Enantiomer">enantiomer</a> <a href="/wiki/Escitalopram" title="Escitalopram">escitalopram</a>, and <a href="/wiki/Fluvoxamine" title="Fluvoxamine">fluvoxamine</a> and <a href="/wiki/Paroxetine" title="Paroxetine">paroxetine</a>.<a href="#cite_note-248">[231]</a><a href="#cite_note-249">[232]</a> <a href="/wiki/Quinolones" class="mw-redirect" title="Quinolones">Quinolones</a> are artificial <a href="/wiki/Broad-spectrum_antibiotic" title="Broad-spectrum antibiotic">broad-spectrum antibiotics</a> that are often fluorinated to enhance their effects. These include <a href="/wiki/Ciprofloxacin" title="Ciprofloxacin">ciprofloxacin</a> and <a href="/wiki/Levofloxacin" title="Levofloxacin">levofloxacin</a>.<a href="#cite_note-250">[233]</a><a href="#cite_note-251">[234]</a><a href="#cite_note-pmid17342653-252">[235]</a><a href="#cite_note-253">[236]</a> Fluorine also finds use in steroids:<a href="#cite_note-254">[237]</a> <a href="/wiki/Fludrocortisone" title="Fludrocortisone">fludrocortisone</a> is a blood pressure-raising <a href="/wiki/Mineralocorticoid" title="Mineralocorticoid">mineralocorticoid</a>, and <a href="/wiki/Triamcinolone" title="Triamcinolone">triamcinolone</a> and <a href="/wiki/Dexamethasone" title="Dexamethasone">dexamethasone</a> are strong <a href="/wiki/Glucocorticoid" title="Glucocorticoid">glucocorticoids</a>.<a href="#cite_note-dontburn-255">[238]</a> The majority of inhaled <a href="/wiki/Anesthetic" title="Anesthetic">anesthetics</a> are heavily fluorinated; the prototype <a href="/wiki/Halothane" title="Halothane">halothane</a> is much more inert and potent than its contemporaries. Later compounds such as the fluorinated <a href="/wiki/Ether" title="Ether">ethers</a> <a href="/wiki/Sevoflurane" title="Sevoflurane">sevoflurane</a> and <a href="/wiki/Desflurane" title="Desflurane">desflurane</a> are better than halothane and are almost insoluble in blood, allowing faster waking times.<a href="#cite_note-fut-256">[239]</a><a href="#cite_note-anestetics-257">[240]</a> <div class="mw-heading mw-heading3"><h3 id="PET_scanning">PET scanning</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=35" title="Edit section: PET scanning">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/Positron_emission_tomography" title="Positron emission tomography">Positron emission tomography</a></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:PET-MIPS-anim.gif" class="mw-file-description"><img alt="Rotating transparent image of a human figure with targeted organs highlighted" src="//upload.wikimedia.org/wikipedia/commons/thumb/3/3d/PET-MIPS-anim.gif/220px-PET-MIPS-anim.gif" decoding="async" width="220" height="331" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/3/3d/PET-MIPS-anim.gif/330px-PET-MIPS-anim.gif 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/3/3d/PET-MIPS-anim.gif/440px-PET-MIPS-anim.gif 2x" data-file-width="446" data-file-height="672" /></a><figcaption>A full-body 18 F PET scan with glucose tagged with radioactive fluorine-18. The normal brain and kidneys take up enough glucose to be imaged. A malignant tumor is seen in the upper abdomen. Radioactive fluorine is seen in urine in the bladder.</figcaption></figure> Fluorine-18 is often found in <a href="/wiki/Radioactive_tracer" title="Radioactive tracer">radioactive tracers</a> for positron emission tomography, as its half-life of almost two hours is long enough to allow for its transport from production facilities to imaging centers.<a href="#cite_note-18F-258">[241]</a> The most common tracer is <a href="/wiki/Fluorodeoxyglucose" class="mw-redirect" title="Fluorodeoxyglucose">fluorodeoxyglucose</a><a href="#cite_note-18F-258">[241]</a> which, after intravenous injection, is taken up by glucose-requiring tissues such as the brain and most malignant tumors;<a href="#cite_note-259">[242]</a> <a href="/wiki/X-ray_computed_tomography" class="mw-redirect" title="X-ray computed tomography">computer-assisted tomography</a> can then be used for detailed imaging.<a href="#cite_note-260">[243]</a> <div class="mw-heading mw-heading3"><h3 id="Oxygen_carriers">Oxygen carriers</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=36" title="Edit section: Oxygen carriers">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Blood_substitute" title="Blood substitute">Blood substitute</a> and <a href="/wiki/Liquid_breathing" title="Liquid breathing">Liquid breathing</a></div> Liquid fluorocarbons can hold large volumes of oxygen or carbon dioxide, more so than blood, and have attracted attention for their possible uses in artificial blood and in liquid breathing.<a href="#cite_note-Gabrielet-261">[244]</a> Because fluorocarbons do not normally mix with water, they must be mixed into emulsions (small droplets of perfluorocarbon suspended in water) to be used as blood.<a href="#cite_note-262">[245]</a><a href="#cite_note-Schimmeyer-263">[246]</a> One such product, <a href="/wiki/Oxycyte" class="mw-redirect" title="Oxycyte">Oxycyte</a>, has been through initial clinical trials.<a href="#cite_note-264">[247]</a> These substances can aid endurance athletes and are banned from sports; one cyclist's near death in 1998 prompted an investigation into their abuse.<a href="#cite_note-265">[248]</a><a href="#cite_note-266">[249]</a> Applications of pure perfluorocarbon liquid breathing (which uses pure perfluorocarbon liquid, not a water emulsion) include assisting burn victims and premature babies with deficient lungs. Partial and complete lung filling have been considered, though only the former has had any significant tests in humans.<a href="#cite_note-ReferenceA-267">[250]</a> An Alliance Pharmaceuticals effort reached clinical trials but was abandoned because the results were not better than normal therapies.<a href="#cite_note-Alliance_stock_drop-268">[251]</a> <div class="mw-heading mw-heading2"><h2 id="Biological_role">Biological role</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=37" 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/Biological_aspects_of_fluorine" title="Biological aspects of fluorine">Biological aspects of fluorine</a></div> Fluorine is not <a href="/wiki/Dietary_mineral" class="mw-redirect" title="Dietary mineral">essential</a> for humans and other mammals, but small amounts are known to be beneficial for the strengthening of dental enamel (where the formation of fluorapatite makes the enamel more resistant to attack, from acids produced by bacterial fermentation of sugars). Small amounts of fluorine may be beneficial for bone strength, but the latter has not been definitively established.<a href="#cite_note-FOOTNOTENielsen2009-269">[252]</a> Both the WHO and the Institute of Medicine of the US National Academies publish recommended daily allowance (RDA) and upper tolerated intake of fluorine, which varies with age and gender.<a href="#cite_note-FOOTNOTEOlivaresUauy2004-270">[253]</a><a href="#cite_note-FOOTNOTEFood_and_Nutrition_Board-271">[254]</a> Natural organofluorines have been found in microorganisms, plants<a href="#cite_note-FOOTNOTEGribble2002-73">[69]</a> and, recently, animals.<a href="#cite_note-272">[255]</a> The most common is <a href="/wiki/Sodium_fluoroacetate" title="Sodium fluoroacetate">fluoroacetate</a>, which is used as a <a href="/wiki/Plant_defense_against_herbivory" title="Plant defense against herbivory">defense against herbivores</a> by at least 40 plants in Africa, Australia and Brazil.<a href="#cite_note-FOOTNOTEProudfootBradberryVale2006-232">[216]</a> Other examples include terminally fluorinated <a href="/wiki/Fatty_acid" title="Fatty acid">fatty acids</a>, <a href="/wiki/Fluoroacetone" title="Fluoroacetone">fluoroacetone</a>, and <a href="/wiki/2-fluorocitrate" class="mw-redirect" title="2-fluorocitrate">2-fluorocitrate</a>.<a href="#cite_note-Murphy2003-273">[256]</a> An enzyme that binds fluorine to carbon – <a href="/wiki/Adenosyl-fluoride_synthase" class="mw-redirect" title="Adenosyl-fluoride synthase">adenosyl-fluoride synthase</a> – was discovered in bacteria in 2002.<a href="#cite_note-FOOTNOTEO'Hagan_et_al.2002-274">[257]</a> <div class="mw-heading mw-heading2"><h2 id="Toxicity">Toxicity</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=38" title="Edit section: Toxicity">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/Biological_aspects_of_fluorine#Hazards" title="Biological aspects of fluorine">Fluorine-related hazards</a></div> Elemental fluorine is highly toxic to living organisms. Its effects in humans start at concentrations lower than <a href="/wiki/Hydrogen_cyanide" title="Hydrogen cyanide">hydrogen cyanide</a>'s 50 ppm<a href="#cite_note-275">[258]</a> and are similar to those of chlorine:<a href="#cite_note-276">[259]</a> significant irritation of the eyes and respiratory system as well as liver and kidney damage occur above 25 ppm, which is the <a href="/wiki/IDLH" class="mw-redirect" title="IDLH">immediately dangerous to life and health</a> value for fluorine.<a href="#cite_note-Keplinger-277">[260]</a> The eyes and nose are seriously damaged at 100 ppm,<a href="#cite_note-Keplinger-277">[260]</a> and inhalation of 1,000 ppm fluorine will cause death in minutes,<a href="#cite_note-278">[261]</a> compared to 270 ppm for hydrogen cyanide.<a href="#cite_note-279">[262]</a> <div style="clear:both;" class=""></div> <div class="mw-heading mw-heading3"><h3 id="Hydrofluoric_acid">Hydrofluoric acid</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=39" title="Edit section: Hydrofluoric acid">edit</a>]</div> <style data-mw-deduplicate="TemplateStyles:r1268415487">.mw-parser-output .ib-chembox{border-collapse:collapse;text-align:left}.mw-parser-output .ib-chembox td,.mw-parser-output .ib-chembox th{border:1px solid #a2a9b1;width:40%}.mw-parser-output .ib-chembox td+td{width:60%}@media screen{html.skin-theme-clientpref-night .mw-parser-output .ib-chembox figure:not(.skin-invert-image):not(.skin-invert):not(.bg-transparent){background:var(--background-color-inverted,#f8f9fa)}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .ib-chembox figure:not(.skin-invert-image):not(.skin-invert):not(.bg-transparent){background:var(--background-color-inverted,#f8f9fa)}}</style> <table class="infobox ib-chembox"> <caption>Fluorine </caption> <tbody><tr> <th colspan="2" style="background: #f8eaba;color:inherit; text-align: center;">Hazards </th></tr> <tr> <td colspan="2" style="text-align:left; background-color:#eaeaea;color:inherit;"><a href="/wiki/Globally_Harmonized_System_of_Classification_and_Labelling_of_Chemicals" title="Globally Harmonized System of Classification and Labelling of Chemicals">GHS labelling</a>: </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/GHS_hazard_pictograms" title="GHS hazard pictograms">Pictograms</a></div> </td> <td><a href="/wiki/File:GHS-pictogram-rondflam.svg" class="mw-file-description" title="GHS03: Oxidizing"><img alt="GHS03: Oxidizing" src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e5/GHS-pictogram-rondflam.svg/60px-GHS-pictogram-rondflam.svg.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/e5/GHS-pictogram-rondflam.svg/120px-GHS-pictogram-rondflam.svg.png 1.5x" data-file-width="724" data-file-height="724" /></a><a href="/wiki/File:GHS-pictogram-acid.svg" class="mw-file-description" title="GHS05: Corrosive"><img alt="GHS05: Corrosive" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a1/GHS-pictogram-acid.svg/60px-GHS-pictogram-acid.svg.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a1/GHS-pictogram-acid.svg/120px-GHS-pictogram-acid.svg.png 1.5x" data-file-width="724" data-file-height="724" /></a><a href="/wiki/File:GHS-pictogram-skull.svg" class="mw-file-description" title="GHS06: Toxic"><img alt="GHS06: Toxic" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/58/GHS-pictogram-skull.svg/60px-GHS-pictogram-skull.svg.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/58/GHS-pictogram-skull.svg/120px-GHS-pictogram-skull.svg.png 1.5x" data-file-width="724" data-file-height="724" /></a><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-silhouette.svg" class="mw-file-description" title="GHS08: Health hazard"><img alt="GHS08: Health hazard" src="//upload.wikimedia.org/wikipedia/commons/thumb/2/21/GHS-pictogram-silhouette.svg/50px-GHS-pictogram-silhouette.svg.png" decoding="async" width="50" height="50" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/21/GHS-pictogram-silhouette.svg/75px-GHS-pictogram-silhouette.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/21/GHS-pictogram-silhouette.svg/100px-GHS-pictogram-silhouette.svg.png 2x" data-file-width="724" data-file-height="724" /></a><a href="/wiki/File:GHS-pictogram-pollu.svg" class="mw-file-description" title="GHS09: Environmental hazard"><img alt="GHS09: Environmental hazard" src="//upload.wikimedia.org/wikipedia/commons/thumb/b/b9/GHS-pictogram-pollu.svg/60px-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/120px-GHS-pictogram-pollu.svg.png 1.5x" data-file-width="724" data-file-height="724" /></a> </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Globally_Harmonized_System_of_Classification_and_Labelling_of_Chemicals#Signal_word" title="Globally Harmonized System of Classification and Labelling of Chemicals">Signal word</a></div> </td> <td>Danger </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/GHS_hazard_statements" title="GHS hazard statements">Hazard statements</a></div> </td> <td><abbr class="abbr" title="H270: May cause or intensify fire: oxidizer">H270</abbr>, <abbr class="abbr" title="H310+H330: Fatal in contact with skin or if inhaled">H310+H330</abbr>, <abbr class="abbr" title="H314: Causes severe skin burns and eye damage">H314</abbr><a href="#cite_note-280">[263]</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-704-diamond-container"><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_32988c54f9009b08" /><map name="ImageMap_32988c54f9009b08"><area href="/wiki/NFPA_704#Blue" shape="poly" coords="23,23,47,47,23,70,0,47" alt="Health 4: Very short exposure could cause death or major residual injury. E.g. VX gas" title="Health 4: Very short exposure could cause death or major residual injury. E.g. VX 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 4: Readily capable of detonation or explosive decomposition at normal temperatures and pressures. E.g. nitroglycerin" title="Instability 4: Readily capable of detonation or explosive decomposition at normal temperatures and pressures. E.g. nitroglycerin" /><area href="/wiki/NFPA_704#White" shape="poly" coords="47,47,70,70,47,94,23,70" alt="Special hazard W+OX: Reacts with water in an unusual or dangerous manner AND is oxidizer" title="Special hazard W+OX: Reacts with water in an unusual or dangerous manner AND is oxidizer" /></map><figcaption></figcaption></figure></div><div class="nfpa-704-diamond-code nfpa-704-diamond-blue"> <a href="/wiki/NFPA_704#Blue" title="NFPA 704">4</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">4</a></div><div class="nfpa-704-diamond-white-text mw-no-invert"><a href="/wiki/NFPA_704#White" title="NFPA 704">W OX</a></div></div></div></div> </td></tr> </tbody></table><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical compound</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:HF_burned_hands.jpg" class="mw-file-description"><img alt="left and right hands, two views, burned index fingers" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/HF_burned_hands.jpg/220px-HF_burned_hands.jpg" decoding="async" width="220" height="148" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/HF_burned_hands.jpg/330px-HF_burned_hands.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/aa/HF_burned_hands.jpg/440px-HF_burned_hands.jpg 2x" data-file-width="500" data-file-height="336" /></a><figcaption>Hydrofluoric acid burns may not be evident for a day, after which calcium treatments are less effective.<a href="#cite_note-Eaton-281">[264]</a></figcaption></figure> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Chemical_burn" title="Chemical burn">Chemical burn</a></div> Hydrofluoric acid is the weakest of the <a href="/wiki/Hydrohalic_acid" class="mw-redirect" title="Hydrohalic acid">hydrohalic acids</a>, having a <a href="/wiki/Acid_dissociation_constant" title="Acid dissociation constant">pKa</a> of 3.2 at 25 °C.<a href="#cite_note-282">[265]</a> Pure hydrogen fluoride is a volatile liquid due to the presence of hydrogen bonding, while the other hydrogen halides are gases. It is able to attack glass, concrete, metals, and organic matter.<a href="#cite_note-283">[266]</a> Hydrofluoric acid is a contact poison with greater hazards than many strong acids like sulfuric acid even though it is weak: it remains neutral in aqueous solution and thus penetrates tissue faster, whether through inhalation, ingestion or the skin, and at least nine U.S. workers died in such accidents from 1984 to 1994. It reacts with calcium and magnesium in the blood leading to <a href="/wiki/Hypocalcemia" title="Hypocalcemia">hypocalcemia</a> and possible death through <a href="/wiki/Cardiac_arrhythmia" class="mw-redirect" title="Cardiac arrhythmia">cardiac arrhythmia</a>.<a href="#cite_note-OSHA-284">[267]</a> Insoluble calcium fluoride formation triggers strong pain<a href="#cite_note-Goldfrank-285">[268]</a> and burns larger than 160 cm2 (25 in2) can cause serious systemic toxicity.<a href="#cite_note-RMTHFE-286">[269]</a> Exposure may not be evident for eight hours for 50% HF, rising to 24 hours for lower concentrations, and a burn may initially be painless as hydrogen fluoride affects nerve function. If skin has been exposed to HF, damage can be reduced by rinsing it under a jet of water for 10–15 minutes and removing contaminated clothing.<a href="#cite_note-287">[270]</a> <a href="/wiki/Calcium_gluconate" title="Calcium gluconate">Calcium gluconate</a> is often applied next, providing calcium ions to bind with fluoride; skin burns can be treated with 2.5% calcium gluconate gel or special rinsing solutions.<a href="#cite_note-pmid2741315-288">[271]</a><a href="#cite_note-pmid17091088-289">[272]</a><a href="#cite_note-pmid15461243-290">[273]</a> Hydrofluoric acid absorption requires further medical treatment; calcium gluconate may be injected or administered intravenously. Using calcium chloride – a common laboratory reagent – in lieu of calcium gluconate is contraindicated, and may lead to severe complications. Excision or amputation of affected parts may be required.<a href="#cite_note-RMTHFE-286">[269]</a><a href="#cite_note-291">[274]</a> <div class="mw-heading mw-heading3"><h3 id="Fluoride_ion">Fluoride ion</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=40" title="Edit section: Fluoride ion">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Fluoride_toxicity" title="Fluoride toxicity">Fluoride toxicity</a></div> Soluble fluorides are moderately toxic: 5–10 g sodium fluoride, or 32–64 mg fluoride ions per kilogram of body mass, represents a lethal dose for adults.<a href="#cite_note-292">[275]</a> One-fifth of the lethal dose can cause adverse health effects,<a href="#cite_note-Nochimson-293">[276]</a> and chronic excess consumption may lead to <a href="/wiki/Skeletal_fluorosis" title="Skeletal fluorosis">skeletal fluorosis</a>, which affects millions in Asia and Africa, and, in children, to reduced intelligence.<a href="#cite_note-Nochimson-293">[276]</a><a href="#cite_note-pmid19305069-294">[277]</a> Ingested fluoride forms hydrofluoric acid in the stomach which is easily absorbed by the intestines, where it crosses cell membranes, binds with calcium and interferes with various enzymes, before urinary <a href="/wiki/Excretion" title="Excretion">excretion</a>. Exposure limits are determined by urine testing of the body's ability to clear fluoride ions.<a href="#cite_note-Nochimson-293">[276]</a><a href="#cite_note-295">[278]</a> Historically, most cases of fluoride poisoning have been caused by accidental ingestion of insecticides containing inorganic fluorides.<a href="#cite_note-Augenstein_et_al._1991-296">[279]</a> Most current calls to poison control centers for possible fluoride poisoning come from the ingestion of fluoride-containing toothpaste.<a href="#cite_note-Nochimson-293">[276]</a> Malfunctioning water fluoridation equipment is another cause: one incident in Alaska affected almost 300 people and killed one person.<a href="#cite_note-Gessner94-297">[280]</a> Dangers from toothpaste are aggravated for small children, and the <a href="/wiki/Centers_for_Disease_Control_and_Prevention" title="Centers for Disease Control and Prevention">Centers for Disease Control and Prevention</a> recommends supervising children below six brushing their teeth so that they do not swallow toothpaste.<a href="#cite_note-298">[281]</a> One regional study examined a year of pre-teen fluoride poisoning reports totaling 87 cases, including one death from ingesting insecticide. Most had no symptoms, but about 30% had stomach pains.<a href="#cite_note-Augenstein_et_al._1991-296">[279]</a> A larger study across the U.S. had similar findings: 80% of cases involved children under six, and there were few serious cases.<a href="#cite_note-299">[282]</a> <div class="mw-heading mw-heading2"><h2 id="Environmental_concerns">Environmental concerns</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=41" title="Edit section: Environmental concerns">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="Atmosphere">Atmosphere</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=42" title="Edit section: Atmosphere">edit</a>]</div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Future_ozone_layer_concentrations.gif" class="mw-file-description"><img alt="Animation showing colored representation of ozone distribution by year above North America in 6 steps. It starts with a lot of ozone but by 2060 is all gone." src="//upload.wikimedia.org/wikipedia/commons/thumb/4/46/Future_ozone_layer_concentrations.gif/250px-Future_ozone_layer_concentrations.gif" decoding="async" width="220" height="160" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/46/Future_ozone_layer_concentrations.gif/330px-Future_ozone_layer_concentrations.gif 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/46/Future_ozone_layer_concentrations.gif/500px-Future_ozone_layer_concentrations.gif 2x" data-file-width="1280" data-file-height="932" /></a><figcaption>NASA projection of stratospheric ozone over North America without the Montreal Protocol<a href="#cite_note-300">[283]</a></figcaption></figure> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Ozone_depletion" title="Ozone depletion">Ozone depletion</a> and <a href="/wiki/Global_warming" class="mw-redirect" title="Global warming">global warming</a></div> The <a href="/wiki/Montreal_Protocol" title="Montreal Protocol">Montreal Protocol</a>, signed in 1987, set strict regulations on chlorofluorocarbons (CFCs) and <a href="/wiki/Bromofluorocarbon" title="Bromofluorocarbon">bromofluorocarbons</a> due to their ozone damaging potential (ODP). The high stability which suited them to their original applications also meant that they were not decomposing until they reached higher altitudes, where liberated chlorine and bromine atoms attacked ozone molecules.<a href="#cite_note-UNEP_FAQ_Ozone-301">[284]</a> Even with the ban, and early indications of its efficacy, predictions warned that several generations would pass before full recovery.<a href="#cite_note-302">[285]</a><a href="#cite_note-303">[286]</a> With one-tenth the ODP of CFCs, hydrochlorofluorocarbons (HCFCs) are the current replacements,<a href="#cite_note-EPA_OLP_Science-304">[287]</a> and are themselves scheduled for substitution by 2030–2040 by hydrofluorocarbons (HFCs) with no chlorine and zero ODP.<a href="#cite_note-HCFC0-305">[288]</a> In 2007 this date was brought forward to 2020 for developed countries;<a href="#cite_note-HCFC_Elim_speedup-306">[289]</a> the <a href="/wiki/Environmental_Protection_Agency" class="mw-redirect" title="Environmental Protection Agency">Environmental Protection Agency</a> had already prohibited one HCFC's production and capped those of two others in 2003.<a href="#cite_note-HCFC0-305">[288]</a> Fluorocarbon gases are generally <a href="/wiki/Greenhouse_gas" title="Greenhouse gas">greenhouse gases</a> with <a href="/wiki/Global-warming_potential" class="mw-redirect" title="Global-warming potential">global-warming potentials</a> (GWPs) of about 100 to 10,000; sulfur hexafluoride has a value of around 20,000.<a href="#cite_note-FOOTNOTEForster_et_al.2007212–213-307">[290]</a> An outlier is <a href="/wiki/HFO-1234yf" class="mw-redirect" title="HFO-1234yf">HFO-1234yf</a> which is a new type of refrigerant called a <a href="/wiki/Hydrofluoroolefin" title="Hydrofluoroolefin">Hydrofluoroolefin</a> (HFO) and has attracted global demand due to its GWP of less than 1 compared to 1,430 for the current refrigerant standard <a href="/wiki/HFC-134a" class="mw-redirect" title="HFC-134a">HFC-134a</a>.<a href="#cite_note-HFO-216">[200]</a> <div class="mw-heading mw-heading3"><h3 id="Biopersistence">Biopersistence</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=43" title="Edit section: Biopersistence">edit</a>]</div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:PFOS-3D-vdW.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/PFOS-3D-vdW.png/220px-PFOS-3D-vdW.png" decoding="async" width="220" height="100" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/PFOS-3D-vdW.png/330px-PFOS-3D-vdW.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d6/PFOS-3D-vdW.png/440px-PFOS-3D-vdW.png 2x" data-file-width="1100" data-file-height="500" /></a><figcaption><a href="/wiki/Perfluorooctanesulfonic_acid" title="Perfluorooctanesulfonic acid">Perfluorooctanesulfonic acid</a>, a key <a href="/wiki/Scotchgard" title="Scotchgard">Scotchgard</a> component until 2000<a href="#cite_note-FOOTNOTESchwarcz200437-308">[291]</a></figcaption></figure> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951" /><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Biological_aspects_of_fluorine#Biopersistence" title="Biological aspects of fluorine">Biopersistence of fluorinated organics</a></div> Organofluorines exhibit biopersistence due to the strength of the carbon–fluorine bond. <a href="/wiki/Perfluoroalkyl_acid" class="mw-redirect" title="Perfluoroalkyl acid">Perfluoroalkyl acids</a> (PFAAs), which are sparingly water-soluble owing to their acidic functional groups, are noted <a href="/wiki/Persistent_organic_pollutant" title="Persistent organic pollutant">persistent organic pollutants</a>;<a href="#cite_note-309">[292]</a> <a href="/wiki/Perfluorooctanesulfonic_acid" title="Perfluorooctanesulfonic acid">perfluorooctanesulfonic acid</a> (PFOS) and <a href="/wiki/Perfluorooctanoic_acid" title="Perfluorooctanoic acid">perfluorooctanoic acid</a> (PFOA) are most often researched.<a href="#cite_note-PFOA-310">[293]</a><a href="#cite_note-PFOA_evidence-311">[294]</a><a href="#cite_note-312">[295]</a> PFAAs have been found in trace quantities worldwide from polar bears to humans, with PFOS and PFOA known to reside in breast milk and the blood of newborn babies. A 2013 review showed a slight correlation between groundwater and soil PFAA levels and human activity; there was no clear pattern of one chemical dominating, and higher amounts of PFOS were correlated to higher amounts of PFOA.<a href="#cite_note-PFOA-310">[293]</a><a href="#cite_note-PFOA_evidence-311">[294]</a><a href="#cite_note-313">[296]</a> In the body, PFAAs bind to proteins such as <a href="/wiki/Serum_albumin" title="Serum albumin">serum albumin</a>; they tend to concentrate within humans in the liver and blood before excretion through the kidneys. Dwell time in the body varies greatly by species, with half-lives of days in rodents, and years in humans.<a href="#cite_note-PFOA-310">[293]</a><a href="#cite_note-PFOA_evidence-311">[294]</a><a href="#cite_note-tox-314">[297]</a> High doses of PFOS and PFOA cause cancer and death in newborn rodents but human studies have not established an effect at current exposure levels.<a href="#cite_note-PFOA-310">[293]</a><a href="#cite_note-PFOA_evidence-311">[294]</a><a href="#cite_note-tox-314">[297]</a> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=44" title="Edit section: See also">edit</a>]</div> <style data-mw-deduplicate="TemplateStyles:r1266661725">.mw-parser-output .portalbox{padding:0;margin:0.5em 0;display:table;box-sizing:border-box;max-width:175px;list-style:none}.mw-parser-output .portalborder{border:1px solid var(--border-color-base,#a2a9b1);padding:0.1em;background:var(--background-color-neutral-subtle,#f8f9fa)}.mw-parser-output .portalbox-entry{display:table-row;font-size:85%;line-height:110%;height:1.9em;font-style:italic;font-weight:bold}.mw-parser-output .portalbox-image{display:table-cell;padding:0.2em;vertical-align:middle;text-align:center}.mw-parser-output .portalbox-link{display:table-cell;padding:0.2em 0.2em 0.2em 0.3em;vertical-align:middle}@media(min-width:720px){.mw-parser-output .portalleft{margin:0.5em 1em 0.5em 0}.mw-parser-output .portalright{clear:right;float:right;margin:0.5em 0 0.5em 1em}}</style><ul role="navigation" aria-label="Portals" class="noprint portalbox portalborder portalright"> <li class="portalbox-entry"><img alt="" src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/28px-Papapishu-Lab-icon-6.svg.png" decoding="async" width="28" height="28" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/42px-Papapishu-Lab-icon-6.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/ed/Papapishu-Lab-icon-6.svg/56px-Papapishu-Lab-icon-6.svg.png 2x" data-file-width="512" data-file-height="512" /><a href="/wiki/Portal:Chemistry" title="Portal:Chemistry">Chemistry portal</a></li></ul> <style data-mw-deduplicate="TemplateStyles:r1184024115">.mw-parser-output .div-col{margin-top:0.3em;column-width:30em}.mw-parser-output .div-col-small{font-size:90%}.mw-parser-output .div-col-rules{column-rule:1px solid #aaa}.mw-parser-output .div-col dl,.mw-parser-output .div-col ol,.mw-parser-output .div-col ul{margin-top:0}.mw-parser-output .div-col li,.mw-parser-output .div-col dd{page-break-inside:avoid;break-inside:avoid-column}</style><div class="div-col" style="column-width: 18em;"> <ul><li><a href="/wiki/Argon_fluoride_laser" title="Argon fluoride laser">Argon fluoride laser</a></li> <li><a href="/wiki/Electrophilic_fluorination" title="Electrophilic fluorination">Electrophilic fluorination</a></li> <li><a href="/wiki/Fluoride_selective_electrode" title="Fluoride selective electrode">Fluoride selective electrode</a>, which measures fluoride concentration</li> <li><a href="/wiki/Fluorine_absorption_dating" title="Fluorine absorption dating">Fluorine absorption dating</a></li> <li><a href="/wiki/Fluorous_chemistry" title="Fluorous chemistry">Fluorous chemistry</a>, a process used to separate reagents from organic solvents</li> <li><a href="/wiki/Krypton_fluoride_laser" title="Krypton fluoride laser">Krypton fluoride laser</a></li> <li><a href="/wiki/Radical_fluorination" title="Radical fluorination">Radical fluorination</a></li></ul> </div> <div class="mw-heading mw-heading2"><h2 id="Notes">Notes</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=45" 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"> <div class="mw-references-wrap mw-references-columns"><ol class="references"> <li id="cite_note-16"><a href="#cite_ref-16">^</a> Assuming that <a href="/wiki/Hydrogen" title="Hydrogen">hydrogen</a> is not considered a halogen. </li> <li id="cite_note-23"><a href="#cite_ref-23">^</a> Sources disagree on the radii of oxygen, fluorine, and neon atoms. Precise comparison is thus impossible. </li> <li id="cite_note-49"><a href="#cite_ref-49">^</a> α-Fluorine has a regular pattern of molecules and is a crystalline solid, but its molecules do not have a specific orientation. β-Fluorine's molecules have fixed locations and minimal rotational uncertainty.<a href="#cite_note-48">[46]</a> </li> <li id="cite_note-54"><a href="#cite_ref-54">^</a> The ratio of the angular momentum to magnetic moment is called the gyromagnetic ratio. "Certain nuclei can for many purposes be thought of as spinning round an axis like the Earth or like a top. In general the spin endows them with angular momentum and with a magnetic moment; the first because of their mass, the second because all or part of their electric charge may be rotating with the mass."<a href="#cite_note-53">[50]</a> </li> <li id="cite_note-80"><a href="#cite_ref-80">^</a> <a href="/wiki/Basilius_Valentinus" class="mw-redirect" title="Basilius Valentinus">Basilius Valentinus</a> supposedly described fluorite in the late 15th century, but because his writings were uncovered 200 years later, this work's veracity is doubtful.<a href="#cite_note-PopSci-77">[73]</a><a href="#cite_note-78">[74]</a><a href="#cite_note-79">[75]</a> </li> <li id="cite_note-85"><a href="#cite_ref-85">^</a> Or perhaps from as early as 1670 onwards; Partington<a href="#cite_note-Partington-84">[79]</a> and Weeks<a href="#cite_note-Weeks-83">[78]</a> give differing accounts. </li> <li id="cite_note-94"><a href="#cite_ref-94">^</a> Fl, since 2012, is used for <a href="/wiki/Flerovium" title="Flerovium">flerovium</a>. </li> <li id="cite_note-96"><a href="#cite_ref-96">^</a> <a href="/wiki/Humphry_Davy" title="Humphry Davy">Davy</a>, <a href="/wiki/Joseph_Louis_Gay-Lussac" title="Joseph Louis Gay-Lussac">Gay-Lussac</a>, <a href="/wiki/Louis_Jacques_Th%C3%A9nard" title="Louis Jacques Thénard">Thénard</a>, and the Irish chemists Thomas and George Knox were injured. Belgian chemist <a href="/w/index.php?title=Paulin_Louyet&action=edit&redlink=1" class="new" title="Paulin Louyet (page does not exist)">Paulin Louyet</a> and French chemist <a href="/w/index.php?title=J%C3%A9r%C3%B4me_Nickl%C3%A8s&action=edit&redlink=1" class="new" title="Jérôme Nicklès (page does not exist)">Jérôme Nicklès</a> [<a href="https://de.wikipedia.org/wiki/J%C3%A9r%C3%B4me_Nickl%C3%A8s" class="extiw" title="de:Jérôme Nicklès">de</a>] died. Moissan also experienced serious hydrogen fluoride poisoning.<a href="#cite_note-Weeks-83">[78]</a><a href="#cite_note-Toon-95">[88]</a> </li> <li id="cite_note-101"><a href="#cite_ref-101">^</a> Also honored was his invention of the <a href="/wiki/Electric_arc_furnace" title="Electric arc furnace">electric arc furnace</a>. </li> <li id="cite_note-110"><a href="#cite_ref-110">^</a> The metastable <a href="/wiki/Boron_monofluoride" title="Boron monofluoride">boron</a> and <a href="/wiki/Nitrogen_monofluoride" title="Nitrogen monofluoride">nitrogen monofluoride</a> have higher-order fluorine bonds, and some <a href="/wiki/Metal_complex" class="mw-redirect" title="Metal complex">metal complexes</a> use it as a <a href="/wiki/Bridging_ligand" title="Bridging ligand">bridging ligand</a>. <a href="/wiki/Hydrogen_bonding" class="mw-redirect" title="Hydrogen bonding">Hydrogen bonding</a> is another possibility. </li> <li id="cite_note-125"><a href="#cite_ref-125">^</a> ZrF 4 melts at 932 °C (1,710 °F),<a href="#cite_note-FOOTNOTELide20044.96-123">[113]</a> HfF 4 sublimes at 968 °C (1,774 °F),<a href="#cite_note-Perry_2011_193-120">[110]</a> and UF 4 melts at 1,036 °C (1,897 °F).<a href="#cite_note-FOOTNOTELide20044.92-124">[114]</a> </li> <li id="cite_note-133"><a href="#cite_ref-133">^</a> These thirteen are those of molybdenum, technetium, ruthenium, rhodium, tungsten, rhenium, osmium, iridium, platinum, polonium, uranium, neptunium, and plutonium. </li> <li id="cite_note-150"><a href="#cite_ref-150">^</a> Carbon tetrafluoride is formally organic, but is included here rather than in the <a href="#Organic_compounds">organofluorine chemistry section</a> – where more complex carbon-fluorine compounds are discussed – for comparison with SiF 4 and GeF 4. </li> <li id="cite_note-174"><a href="#cite_ref-174">^</a> Perfluorocarbon and fluorocarbon are <a href="/wiki/IUPAC" class="mw-redirect" title="IUPAC">IUPAC</a> synonyms for molecules containing carbon and fluorine only, but in colloquial and commercial contexts the latter term may refer to any carbon- and fluorine-containing molecule, possibly with other elements. </li> <li id="cite_note-178"><a href="#cite_ref-178">^</a> This terminology is imprecise, and perfluorinated substance is also used.<a href="#cite_note-177">[163]</a> </li> <li id="cite_note-214"><a href="#cite_ref-214">^</a> This DuPont trademark is sometimes further misused for CFCs, HFCs, or HCFCs. </li> <li id="cite_note-234"><a href="#cite_ref-234">^</a> American sheep and cattle collars may use 1080 against predators like coyotes. </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="Sources">Sources</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=46" title="Edit section: Sources">edit</a>]</div> <div class="mw-heading mw-heading3"><h3 id="Citations">Citations</h3>[<a href="/w/index.php?title=Fluorine&action=edit&section=47" title="Edit section: Citations">edit</a>]</div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239543626" /><div class="reflist reflist-columns references-column-width" style="column-width: 21em;"> <ol class="references"> <li id="cite_note-CIAAW-1"><a href="#cite_ref-CIAAW_1-0">^</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/fluorine.htm">"Standard Atomic Weights: Fluorine"</a>. <a href="/wiki/Commission_on_Isotopic_Abundances_and_Atomic_Weights" title="Commission on Isotopic Abundances and Atomic Weights">CIAAW</a>. 2021.</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+Fluorine&rft.pub=CIAAW&rft.date=2021&rft_id=https%3A%2F%2Fwww.ciaaw.org%2Ffluorine.htm&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"> </li> <li id="cite_note-CIAAW2021-2"><a href="#cite_ref-CIAAW2021_2-0">^</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFProhaskaIrrgeherBenefieldBöhlke2022" class="citation journal cs1">Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. 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href="#cite_ref-227">^</a> <a href="#CITEREFICIS2006">ICIS 2006</a>. </li> <li id="cite_note-Theodoridis-228">^ <a href="#cite_ref-Theodoridis_228-0">a</a> <a href="#cite_ref-Theodoridis_228-1">b</a> <a href="#CITEREFTheodoridis2006">Theodoridis 2006</a>. </li> <li id="cite_note-trifluralin-229"><a href="#cite_ref-trifluralin_229-0">^</a> <a href="#CITEREFEPA1996">EPA 1996</a>. </li> <li id="cite_note-230"><a href="#cite_ref-230">^</a> <a href="#CITEREFDG_Environment2007">DG Environment 2007</a>. </li> <li id="cite_note-Beasley-231"><a href="#cite_ref-Beasley_231-0">^</a> <a href="#CITEREFBeasley2002">Beasley 2002</a>. </li> <li id="cite_note-FOOTNOTEProudfootBradberryVale2006-232">^ <a href="#cite_ref-FOOTNOTEProudfootBradberryVale2006_232-0">a</a> <a href="#cite_ref-FOOTNOTEProudfootBradberryVale2006_232-1">b</a> <a href="#CITEREFProudfootBradberryVale2006">Proudfoot, Bradberry & Vale 2006</a>. </li> <li id="cite_note-FOOTNOTEEisler1995-233"><a 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.refbegin-columns{margin-top:0.3em}.mw-parser-output .refbegin-columns ul{margin-top:0}.mw-parser-output .refbegin-columns li{page-break-inside:avoid;break-inside:avoid-column}@media screen{.mw-parser-output .refbegin{font-size:90%}}</style><div class="refbegin refbegin-hanging-indents refbegin-columns references-column-width" style="column-width: 30em"> <ul><li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFAgricolaHooverHoover1912" class="citation book cs1"><a href="/wiki/Georgius_Agricola" title="Georgius Agricola">Agricola, Georgius</a>; Hoover, Herbert Clark; Hoover, Lou Henry (1912). <a rel="nofollow" class="external text" href="https://archive.org/stream/georgiusagricola00agririch#page/n5/mode/2up">De Re Metallica</a>. London: The Mining Magazine.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=De+Re+Metallica&rft.place=London&rft.pub=The+Mining+Magazine&rft.date=1912&rft.aulast=Agricola&rft.aufirst=Georgius&rft.au=Hoover%2C+Herbert+Clark&rft.au=Hoover%2C+Lou+Henry&rft_id=https%3A%2F%2Farchive.org%2Fstream%2Fgeorgiusagricola00agririch%23page%2Fn5%2Fmode%2F2up&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFAigueperse_et_al.2000" class="citation encyclopaedia cs1">Aigueperse, J.; Mollard, P.; Devilliers, D.; Chemla, M.; Faron, R.; Romano, R. E.; Cue, J. P. (2000). "Fluorine Compounds, Inorganic". <a href="/wiki/Ullmann%27s_Encyclopedia_of_Industrial_Chemistry" title="Ullmann's Encyclopedia of Industrial Chemistry">Ullmann's Encyclopedia of Industrial Chemistry</a>. 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Air Products and Chemicals. Archived from <a rel="nofollow" class="external text" href="http://www.airproducts.com/nr/rdonlyres/8479ed55-2170-4651-a3d4-223b2957a9f3/0/safetygram39.pdf">the original</a> (PDF) on 18 March 2006. Retrieved 16 February 2014.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=Safetygram+%2339+Chlorine+Trifluoride&rft.pub=Air+Products+and+Chemicals&rft.date=2004&rft.au=Air+Products+and+Chemicals&rft_id=http%3A%2F%2Fwww.airproducts.com%2Fnr%2Frdonlyres%2F8479ed55-2170-4651-a3d4-223b2957a9f3%2F0%2Fsafetygram39.pdf&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFAlaviHuang2007" class="citation book cs1">Alavi, Abbas; Huang, Steve S. (2007). "Positron Emission Tomography in Medicine: An Overview". In Hayat, M. A. (ed.). Cancer Imaging, Volume 1: Lung and Breast Carcinomas. 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Australia and New Zealand Health Policy. 4: 25. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1186%2F1743-8462-4-25">10.1186/1743-8462-4-25</a>. <a href="/wiki/PMC_(identifier)" class="mw-redirect" title="PMC (identifier)">PMC</a> <a rel="nofollow" class="external text" href="https://www.ncbi.nlm.nih.gov/pmc/articles/PMC2222595">2222595</a>. <a href="/wiki/PMID_(identifier)" class="mw-redirect" title="PMID (identifier)">PMID</a> <a rel="nofollow" class="external text" href="https://pubmed.ncbi.nlm.nih.gov/18067684">18067684</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Australia+and+New+Zealand+Health+Policy&rft.atitle=When+Public+Action+Undermines+Public+Health%3A+A+Critical+Examination+of+Antifluoridationist+Literature&rft.volume=4&rft.pages=25&rft.date=2007&rft_id=https%3A%2F%2Fwww.ncbi.nlm.nih.gov%2Fpmc%2Farticles%2FPMC2222595%23id-name%3DPMC&rft_id=info%3Apmid%2F18067684&rft_id=info%3Adoi%2F10.1186%2F1743-8462-4-25&rft.aulast=Armfield&rft.aufirst=J.+M.&rft_id=https%3A%2F%2Fwww.ncbi.nlm.nih.gov%2Fpmc%2Farticles%2FPMC2222595&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFAsimov1966" class="citation book cs1"><a href="/wiki/Isaac_Asimov" title="Isaac Asimov">Asimov, Isaac</a> (1966). 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Contemporary Physics. 2 (5): 360–366. <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/1961ConPh...2..360V">1961ConPh...2..360V</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1080%2F00107516108205282">10.1080/00107516108205282</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:5092147">5092147</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Contemporary+Physics&rft.atitle=The+Gyromagnetic+Ratio+of+the+Proton&rft.volume=2&rft.issue=5&rft.pages=%3Cspan+class%3D%22nowrap%22%3E360-%3C%2Fspan%3E366&rft.date=1961&rft_id=https%3A%2F%2Fapi.semanticscholar.org%2FCorpusID%3A5092147%23id-name%3DS2CID&rft_id=info%3Adoi%2F10.1080%2F00107516108205282&rft_id=info%3Abibcode%2F1961ConPh...2..360V&rft.aulast=Vigoureux&rft.aufirst=P.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFVillalbaAyresSchroder2008" class="citation journal cs1">Villalba, Gara; Ayres, Robert U.; Schroder, Hans (2008). 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Inorganic Chemistry. San Diego: Academic Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-12-352651-9" title="Special:BookSources/978-0-12-352651-9"><bdi>978-0-12-352651-9</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Inorganic+Chemistry&rft.place=San+Diego&rft.pub=Academic+Press&rft.date=2001&rft.isbn=978-0-12-352651-9&rft.aulast=Wiberg&rft.aufirst=Egon&rft.au=Wiberg%2C+Nils&rft.au=Holleman%2C+Arnold+Frederick&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFWilley2007" class="citation book cs1">Willey, Ronald R. (2007). Practical Equipment, Materials, and Processes for Optical Thin Films. 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Parsippany: Matheson Tri-Gas. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-07-135854-5" title="Special:BookSources/978-0-07-135854-5"><bdi>978-0-07-135854-5</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Fluorine&rft.btitle=Matheson+Gas+Data+Book&rft.place=Parsippany&rft.edition=7th&rft.pub=Matheson+Tri-Gas&rft.date=2001&rft.isbn=978-0-07-135854-5&rft.aulast=Yaws&rft.aufirst=Carl+L.&rft.au=Braker%2C+William&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFYeung2008" class="citation journal cs1">Yeung, C. A. (2008). <a rel="nofollow" class="external text" href="https://doi.org/10.1038%2Fsj.ebd.6400578">"A Systematic Review of the Efficacy and Safety of Fluoridation"</a>. Evidence-Based Dentistry. 9 (2): 39–43. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1038%2Fsj.ebd.6400578">10.1038/sj.ebd.6400578</a>. <a href="/wiki/PMID_(identifier)" class="mw-redirect" title="PMID (identifier)">PMID</a> <a rel="nofollow" class="external text" href="https://pubmed.ncbi.nlm.nih.gov/18584000">18584000</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Evidence-Based+Dentistry&rft.atitle=A+Systematic+Review+of+the+Efficacy+and+Safety+of+Fluoridation&rft.volume=9&rft.issue=2&rft.pages=%3Cspan+class%3D%22nowrap%22%3E39-%3C%2Fspan%3E43&rft.date=2008&rft_id=info%3Adoi%2F10.1038%2Fsj.ebd.6400578&rft_id=info%3Apmid%2F18584000&rft.aulast=Yeung&rft.aufirst=C.+A.&rft_id=https%3A%2F%2Fdoi.org%2F10.1038%252Fsj.ebd.6400578&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222" /><cite id="CITEREFYoung1975" class="citation report cs1">Young, David A. 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Handbook of Quality Integrated Circuit Manufacturing. San Diego: Academic Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-323-14055-3" title="Special:BookSources/978-0-323-14055-3"><bdi>978-0-323-14055-3</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Handbook+of+Quality+Integrated+Circuit+Manufacturing&rft.place=San+Diego&rft.pub=Academic+Press&rft.date=1991&rft.isbn=978-0-323-14055-3&rft.aulast=Zorich&rft.aufirst=Robert&rfr_id=info%3Asid%2Fen.wikipedia.org%3AFluorine" class="Z3988"></li></ul> </div> <div class="mw-heading mw-heading2"><h2 id="External_links">External links</h2>[<a href="/w/index.php?title=Fluorine&action=edit&section=49" title="Edit section: External links">edit</a>]</div> <ul><li><a href="/wiki/File:Commons-logo.svg" class="mw-file-description"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/4/4a/Commons-logo.svg/20px-Commons-logo.svg.png" 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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_table18" 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="font-weight:normal;"><a href="/wiki/Alkali_metal" title="Alkali metal">1</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Alkaline_earth_metal" title="Alkaline earth metal">2</a> </th> <td colspan="14"> </td> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_3_element" title="Group 3 element">3</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_4_element" title="Group 4 element">4</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_5_element" title="Group 5 element">5</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_6_element" title="Group 6 element">6</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_7_element" title="Group 7 element">7</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_8_element" title="Group 8 element">8</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_9_element" title="Group 9 element">9</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_10_element" title="Group 10 element">10</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_11_element" title="Group 11 element">11</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Group_12_element" title="Group 12 element">12</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Boron_group" title="Boron group">13</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Carbon_group" title="Carbon group">14</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Pnictogen" title="Pnictogen">15</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Chalcogen" title="Chalcogen">16</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Halogen" title="Halogen">17</a> </th> <th scope="col" style="font-weight:normal;"><a href="/wiki/Noble_gas" title="Noble gas">18</a> </th></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_1_element" title="Period 1 element">1</a> </th> <td title="H, Hydrogen" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Hydrogen" title="Hydrogen">H</a> </td> <td colspan="30"> </td> <td title="He, Helium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Helium" title="Helium">He</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_2_element" title="Period 2 element">2</a> </th> <td title="Li, Lithium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Lithium" title="Lithium">Li</a> </td> <td title="Be, Beryllium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Beryllium" title="Beryllium">Be</a> </td> <td colspan="24"> </td> <td title="B, Boron" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Boron" title="Boron">B</a> </td> <td title="C, Carbon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Carbon" title="Carbon">C</a> </td> <td title="N, Nitrogen" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Nitrogen" title="Nitrogen">N</a> </td> <td title="O, Oxygen" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Oxygen" title="Oxygen">O</a> </td> <td title="F, Fluorine" style="text-align:center; background-color:#fdff8c; color:inherit; border:3px solid black; ;"><a class="mw-selflink selflink">F</a> </td> <td title="Ne, Neon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Neon" title="Neon">Ne</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_3_element" title="Period 3 element">3</a> </th> <td title="Na, Sodium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Sodium" title="Sodium">Na</a> </td> <td title="Mg, Magnesium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Magnesium" title="Magnesium">Mg</a> </td> <td colspan="24"> </td> <td title="Al, Aluminium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Aluminium" title="Aluminium">Al</a> </td> <td title="Si, Silicon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Silicon" title="Silicon">Si</a> </td> <td title="P, Phosphorus" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Phosphorus" title="Phosphorus">P</a> </td> <td title="S, Sulfur" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Sulfur" title="Sulfur">S</a> </td> <td title="Cl, Chlorine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Chlorine" title="Chlorine">Cl</a> </td> <td title="Ar, Argon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Argon" title="Argon">Ar</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_4_element" title="Period 4 element">4</a> </th> <td title="K, Potassium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Potassium" title="Potassium">K</a> </td> <td title="Ca, Calcium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Calcium" title="Calcium">Ca</a> </td> <td colspan="14"> </td> <td title="Sc, Scandium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Scandium" title="Scandium">Sc</a> </td> <td title="Ti, Titanium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Titanium" title="Titanium">Ti</a> </td> <td title="V, Vanadium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Vanadium" title="Vanadium">V</a> </td> <td title="Cr, Chromium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Chromium" title="Chromium">Cr</a> </td> <td title="Mn, Manganese" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Manganese" title="Manganese">Mn</a> </td> <td title="Fe, Iron" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Iron" title="Iron">Fe</a> </td> <td title="Co, Cobalt" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Cobalt" title="Cobalt">Co</a> </td> <td title="Ni, Nickel" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Nickel" title="Nickel">Ni</a> </td> <td title="Cu, Copper" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Copper" title="Copper">Cu</a> </td> <td title="Zn, Zinc" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Zinc" title="Zinc">Zn</a> </td> <td title="Ga, Gallium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Gallium" title="Gallium">Ga</a> </td> <td title="Ge, Germanium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Germanium" title="Germanium">Ge</a> </td> <td title="As, Arsenic" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Arsenic" title="Arsenic">As</a> </td> <td title="Se, Selenium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Selenium" title="Selenium">Se</a> </td> <td title="Br, Bromine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Bromine" title="Bromine">Br</a> </td> <td title="Kr, Krypton" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Krypton" title="Krypton">Kr</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_5_element" title="Period 5 element">5</a> </th> <td title="Rb, Rubidium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Rubidium" title="Rubidium">Rb</a> </td> <td title="Sr, Strontium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Strontium" title="Strontium">Sr</a> </td> <td colspan="14"> </td> <td title="Y, Yttrium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Yttrium" title="Yttrium">Y</a> </td> <td title="Zr, Zirconium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Zirconium" title="Zirconium">Zr</a> </td> <td title="Nb, Niobium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Niobium" title="Niobium">Nb</a> </td> <td title="Mo, Molybdenum" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Molybdenum" title="Molybdenum">Mo</a> </td> <td title="Tc, Technetium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Technetium" title="Technetium">Tc</a> </td> <td title="Ru, Ruthenium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Ruthenium" title="Ruthenium">Ru</a> </td> <td title="Rh, Rhodium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Rhodium" title="Rhodium">Rh</a> </td> <td title="Pd, Palladium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Palladium" title="Palladium">Pd</a> </td> <td title="Ag, Silver" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Silver" title="Silver">Ag</a> </td> <td title="Cd, Cadmium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Cadmium" title="Cadmium">Cd</a> </td> <td title="In, Indium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Indium" title="Indium">In</a> </td> <td title="Sn, Tin" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Tin" title="Tin">Sn</a> </td> <td title="Sb, Antimony" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Antimony" title="Antimony">Sb</a> </td> <td title="Te, Tellurium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Tellurium" title="Tellurium">Te</a> </td> <td title="I, Iodine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Iodine" title="Iodine">I</a> </td> <td title="Xe, Xenon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Xenon" title="Xenon">Xe</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_6_element" title="Period 6 element">6</a> </th> <td title="Cs, Caesium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Caesium" title="Caesium">Cs</a> </td> <td title="Ba, Barium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Barium" title="Barium">Ba</a> </td> <td title="La, Lanthanum" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Lanthanum" title="Lanthanum">La</a> </td> <td title="Ce, Cerium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Cerium" title="Cerium">Ce</a> </td> <td title="Pr, Praseodymium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Praseodymium" title="Praseodymium">Pr</a> </td> <td title="Nd, Neodymium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Neodymium" title="Neodymium">Nd</a> </td> <td title="Pm, Promethium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Promethium" title="Promethium">Pm</a> </td> <td title="Sm, Samarium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Samarium" title="Samarium">Sm</a> </td> <td title="Eu, Europium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Europium" title="Europium">Eu</a> </td> <td title="Gd, Gadolinium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Gadolinium" title="Gadolinium">Gd</a> </td> <td title="Tb, Terbium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Terbium" title="Terbium">Tb</a> </td> <td title="Dy, Dysprosium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Dysprosium" title="Dysprosium">Dy</a> </td> <td title="Ho, Holmium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Holmium" title="Holmium">Ho</a> </td> <td title="Er, Erbium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Erbium" title="Erbium">Er</a> </td> <td title="Tm, Thulium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Thulium" title="Thulium">Tm</a> </td> <td title="Yb, Ytterbium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Ytterbium" title="Ytterbium">Yb</a> </td> <td title="Lu, Lutetium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Lutetium" title="Lutetium">Lu</a> </td> <td title="Hf, Hafnium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Hafnium" title="Hafnium">Hf</a> </td> <td title="Ta, Tantalum" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Tantalum" title="Tantalum">Ta</a> </td> <td title="W, Tungsten" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Tungsten" title="Tungsten">W</a> </td> <td title="Re, Rhenium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Rhenium" title="Rhenium">Re</a> </td> <td title="Os, Osmium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Osmium" title="Osmium">Os</a> </td> <td title="Ir, Iridium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Iridium" title="Iridium">Ir</a> </td> <td title="Pt, Platinum" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Platinum" title="Platinum">Pt</a> </td> <td title="Au, Gold" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Gold" title="Gold">Au</a> </td> <td title="Hg, Mercury" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Mercury_(element)" title="Mercury (element)">Hg</a> </td> <td title="Tl, Thallium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Thallium" title="Thallium">Tl</a> </td> <td title="Pb, Lead" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Lead" title="Lead">Pb</a> </td> <td title="Bi, Bismuth" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Bismuth" title="Bismuth">Bi</a> </td> <td title="Po, Polonium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Polonium" title="Polonium">Po</a> </td> <td title="At, Astatine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Astatine" title="Astatine">At</a> </td> <td title="Rn, Radon" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Radon" title="Radon">Rn</a> </td></tr> <tr> <th scope="row" style="font-weight:normal;"><a href="/wiki/Period_7_element" title="Period 7 element">7</a> </th> <td title="Fr, Francium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Francium" title="Francium">Fr</a> </td> <td title="Ra, Radium" style="text-align:center; background-color:#ff9999; color:inherit; border:none; ;"><a href="/wiki/Radium" title="Radium">Ra</a> </td> <td title="Ac, Actinium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Actinium" title="Actinium">Ac</a> </td> <td title="Th, Thorium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Thorium" title="Thorium">Th</a> </td> <td title="Pa, Protactinium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Protactinium" title="Protactinium">Pa</a> </td> <td title="U, Uranium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Uranium" title="Uranium">U</a> </td> <td title="Np, Neptunium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Neptunium" title="Neptunium">Np</a> </td> <td title="Pu, Plutonium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Plutonium" title="Plutonium">Pu</a> </td> <td title="Am, Americium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Americium" title="Americium">Am</a> </td> <td title="Cm, Curium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Curium" title="Curium">Cm</a> </td> <td title="Bk, Berkelium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Berkelium" title="Berkelium">Bk</a> </td> <td title="Cf, Californium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Californium" title="Californium">Cf</a> </td> <td title="Es, Einsteinium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Einsteinium" title="Einsteinium">Es</a> </td> <td title="Fm, Fermium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Fermium" title="Fermium">Fm</a> </td> <td title="Md, Mendelevium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Mendelevium" title="Mendelevium">Md</a> </td> <td title="No, Nobelium" style="text-align:center; background-color:#9bff99; color:inherit; border:none; ;"><a href="/wiki/Nobelium" title="Nobelium">No</a> </td> <td title="Lr, Lawrencium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Lawrencium" title="Lawrencium">Lr</a> </td> <td title="Rf, Rutherfordium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Rutherfordium" title="Rutherfordium">Rf</a> </td> <td title="Db, Dubnium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Dubnium" title="Dubnium">Db</a> </td> <td title="Sg, Seaborgium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Seaborgium" title="Seaborgium">Sg</a> </td> <td title="Bh, Bohrium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Bohrium" title="Bohrium">Bh</a> </td> <td title="Hs, Hassium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Hassium" title="Hassium">Hs</a> </td> <td title="Mt, Meitnerium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Meitnerium" title="Meitnerium">Mt</a> </td> <td title="Ds, Darmstadtium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Darmstadtium" title="Darmstadtium">Ds</a> </td> <td title="Rg, Roentgenium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Roentgenium" title="Roentgenium">Rg</a> </td> <td title="Cn, Copernicium" style="text-align:center; background-color:#99ccff; color:inherit; border:none; ;"><a href="/wiki/Copernicium" title="Copernicium">Cn</a> </td> <td title="Nh, Nihonium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Nihonium" title="Nihonium">Nh</a> </td> <td title="Fl, Flerovium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Flerovium" title="Flerovium">Fl</a> </td> <td title="Mc, Moscovium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Moscovium" title="Moscovium">Mc</a> </td> <td title="Lv, Livermorium" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Livermorium" title="Livermorium">Lv</a> </td> <td title="Ts, Tennessine" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Tennessine" title="Tennessine">Ts</a> </td> <td title="Og, Oganesson" style="text-align:center; background-color:#fdff8c; color:inherit; border:none; ;"><a href="/wiki/Oganesson" title="Oganesson">Og</a> </td></tr></tbody></table> </div></td></tr><tr><td colspan="2" class="navbox-list navbox-even wraplinks" style="width:100%;padding:0"><div style="padding:0 0.25em"><div role="presentation" id="periodic-table-legend" style="border: 1px solid #a2a9b1; width:100%; line-height:120%; text-align:center; vertical-align:top; background:#f8f8f8;color:inherit; margin:0; margin:0;"><div style="padding:0.3em;"> <table style="width:100%; line-height:1.2em; table-layout:fixed; overflow:hidden; text-align:center;"> <tbody><tr> <td style="padding:0 1px; background:#ff9999;color:inherit;"><a href="/wiki/S-block" class="mw-redirect" title="S-block">s-block</a> </td> <td style="padding:0 1px; background:#9bff99;color:inherit;"><a href="/wiki/F-block" class="mw-redirect" title="F-block">f-block</a> </td> <td style="padding:0 1px; background:#99ccff;color:inherit;"><a href="/wiki/D-block" class="mw-redirect" title="D-block">d-block</a> </td> <td style="padding:0 1px; background:#fdff8c;color:inherit;"><a href="/wiki/P-block" class="mw-redirect" title="P-block">p-block</a> </td></tr></tbody></table> </div> </div></div></td></tr></tbody></table></div> <div class="navbox-styles"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1129693374" /><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236075235" /></div><div role="navigation" class="navbox" aria-labelledby="Dietary_supplements155" 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:Dietary_supplement" title="Template:Dietary supplement"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Dietary_supplement" title="Template talk:Dietary supplement"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Dietary_supplement" title="Special:EditPage/Template:Dietary supplement"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Dietary_supplements155" style="font-size:114%;margin:0 4em"><a href="/wiki/Dietary_supplement" title="Dietary supplement">Dietary supplements</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%">Types</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/Bodybuilding_supplement" title="Bodybuilding supplement">Bodybuilding supplement</a></li> <li><a href="/wiki/Energy_drink" title="Energy drink">Energy drink</a></li> <li><a href="/wiki/Energy_bar" title="Energy bar">Energy bar</a></li> <li><a href="/wiki/Essential_fatty_acid" title="Essential fatty acid">Fatty acids</a></li> <li><a href="/wiki/Herbal_medicine" title="Herbal medicine">Herbal supplements</a></li> <li><a href="/wiki/Mineral_(nutrient)" title="Mineral (nutrient)">Minerals</a></li> <li><a href="/wiki/Prebiotic_(nutrition)" title="Prebiotic (nutrition)">Prebiotics</a></li> <li><a href="/wiki/Probiotic" title="Probiotic">Probiotics</a> (<a href="/wiki/Lactobacillus" title="Lactobacillus">Lactobacillus</a></li> <li><a href="/wiki/Bifidobacterium" title="Bifidobacterium">Bifidobacterium</a>)</li> <li><a href="/wiki/Protein_supplement" title="Protein supplement">Protein supplements</a></li> <li><a href="/wiki/Vitamin" title="Vitamin">Vitamins</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Vitamin" title="Vitamin">Vitamins</a> and <a href="/wiki/Mineral_(nutrient)" title="Mineral (nutrient)">chemical elements ("minerals")</a></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Vitamin_A" title="Vitamin A">Retinol (Vitamin A)</a></li> <li><a href="/wiki/B_vitamins" title="B vitamins">B vitamins</a> <ul><li><a href="/wiki/Thiamine" title="Thiamine">Thiamine (B1)</a></li> <li><a href="/wiki/Riboflavin" title="Riboflavin">Riboflavin (B2)</a></li> <li><a href="/wiki/Niacin_(nutrient)" class="mw-redirect" title="Niacin (nutrient)">Niacin (B3)</a></li> <li><a href="/wiki/Pantothenic_acid" title="Pantothenic acid">Pantothenic acid (B5)</a></li> <li><a href="/wiki/Vitamin_B6" title="Vitamin B6">Pyridoxine (B6)</a></li> <li><a href="/wiki/Biotin" title="Biotin">Biotin (B7)</a></li> <li><a href="/wiki/Folate" title="Folate">Folic acid (B9)</a></li> <li><a href="/wiki/Cyanocobalamin" title="Cyanocobalamin">Cyanocobalamin (B12)</a></li></ul></li> <li><a href="/wiki/Vitamin_C" title="Vitamin C">Ascorbic acid (Vitamin C)</a></li> <li><a href="/wiki/Vitamin_D" title="Vitamin D">Ergocalciferol and Cholecalciferol (Vitamin D)</a></li> <li><a href="/wiki/Vitamin_E" title="Vitamin E">Tocopherol (Vitamin E)</a></li> <li><a href="/wiki/Vitamin_K" title="Vitamin K">Naphthoquinone (Vitamin K)</a></li></ul> <ul><li><a href="/wiki/Calcium_supplement" title="Calcium supplement">Calcium</a></li> <li><a href="/wiki/Choline" title="Choline">Choline</a></li> <li><a href="/wiki/Chromium" title="Chromium">Chromium</a></li> <li><a href="/wiki/Cobalt" title="Cobalt">Cobalt</a></li> <li><a href="/wiki/Copper" title="Copper">Copper</a></li> <li><a class="mw-selflink selflink">Fluorine</a></li> <li><a href="/wiki/Iodine" title="Iodine">Iodine</a></li> <li><a href="/wiki/Iron" title="Iron">Iron</a></li> <li><a href="/wiki/Magnesium" title="Magnesium">Magnesium</a></li> <li><a href="/wiki/Manganese" title="Manganese">Manganese</a></li> <li><a href="/wiki/Molybdenum" title="Molybdenum">Molybdenum</a></li> <li><a href="/wiki/Phosphorus" title="Phosphorus">Phosphorus</a></li> <li><a href="/wiki/Potassium" title="Potassium">Potassium</a></li> <li><a href="/wiki/Selenium" title="Selenium">Selenium</a></li> <li><a href="/wiki/Sodium" title="Sodium">Sodium</a></li> <li><a href="/wiki/Sulfur" title="Sulfur">Sulfur</a></li> <li><a href="/wiki/Zinc" title="Zinc">Zinc</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Other common ingredients</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/Arginine_alpha-ketoglutarate" title="Arginine alpha-ketoglutarate">AAKG</a></li> <li><a href="/wiki/Beta-Hydroxy_beta-methylbutyric_acid" class="mw-redirect" title="Beta-Hydroxy beta-methylbutyric acid">β-hydroxy β-methylbutyrate</a></li> <li><a href="/wiki/Carnitine" title="Carnitine">Carnitine</a></li> <li><a href="/wiki/Chondroitin_sulfate" title="Chondroitin sulfate">Chondroitin sulfate</a></li> <li><a href="/wiki/Cod_liver_oil" title="Cod liver oil">Cod liver oil</a></li> <li><a href="/wiki/Copper_gluconate" title="Copper gluconate">Copper gluconate</a></li> <li><a href="/wiki/Creatine" title="Creatine">Creatine</a></li> <li><a href="/wiki/Dietary_fiber" title="Dietary fiber">Dietary fiber</a></li> <li><a href="/wiki/Echinacea#Medicinal_effects" title="Echinacea">Echinacea</a></li> <li><a href="/wiki/Ephedra_(medicine)" title="Ephedra (medicine)">Ephedra</a></li> <li><a href="/wiki/Fish_oil" title="Fish oil">Fish oil</a></li> <li><a href="/wiki/Folate" title="Folate">Folic acid</a></li> <li><a href="/wiki/Ginseng" title="Ginseng">Ginseng</a></li> <li><a href="/wiki/Glucosamine" title="Glucosamine">Glucosamine</a></li> <li><a href="/wiki/Glutamine" title="Glutamine">Glutamine</a></li> <li><a href="/wiki/Grape_seed_extract" title="Grape seed extract">Grape seed extract</a></li> <li><a href="/wiki/Guarana" title="Guarana">Guarana</a></li> <li><a href="/wiki/Iron_supplement" title="Iron supplement">Iron supplements</a></li> <li><a href="/wiki/Lonicera_japonica" title="Lonicera japonica">Japanese honeysuckle</a></li> <li><a href="/wiki/Krill_oil" title="Krill oil">Krill oil</a></li> <li><a href="/wiki/Lingzhi_(mushroom)" title="Lingzhi (mushroom)">Lingzhi</a></li> <li><a href="/wiki/Linseed_oil" title="Linseed oil">Linseed oil</a></li> <li><a href="/wiki/Lipoic_acid" title="Lipoic acid">Lipoic acid</a></li> <li><a href="/wiki/Silybum_marianum#Health_benefits" title="Silybum marianum">Milk thistle</a></li> <li><a href="/wiki/Melatonin_(supplement)" class="mw-redirect" title="Melatonin (supplement)">Melatonin</a></li> <li><a href="/wiki/Red_yeast_rice" title="Red yeast rice">Red yeast rice</a></li> <li><a href="/wiki/Royal_jelly" title="Royal jelly">Royal jelly</a></li> <li><a href="/wiki/Saw_palmetto_extract" title="Saw palmetto extract">Saw palmetto</a></li> <li><a href="/wiki/Spirulina_(dietary_supplement)" title="Spirulina (dietary supplement)">Spirulina</a></li> <li><a href="/wiki/Hypericum_perforatum#Medicinal_uses" title="Hypericum perforatum">St John's wort</a></li> <li><a href="/wiki/Taurine" title="Taurine">Taurine</a></li> <li><a href="/wiki/Wheatgrass" title="Wheatgrass">Wheatgrass</a></li> <li><a href="/wiki/Goji" title="Goji">Wolfberry</a></li> <li><a href="/wiki/Yohimbine" title="Yohimbine">Yohimbine</a></li> <li><a href="/wiki/Zinc_gluconate" title="Zinc gluconate">Zinc gluconate</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Related articles</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/Codex_Alimentarius" title="Codex Alimentarius">Codex Alimentarius</a></li> <li><a href="/wiki/Enzyte" title="Enzyte">Enzyte</a></li> <li><a href="/wiki/Hadacol" title="Hadacol">Hadacol</a></li> <li><a href="/wiki/Herbal_tea" title="Herbal tea">Herbal tea</a></li> <li><a href="/wiki/Nutraceutical" title="Nutraceutical">Nutraceutical</a></li> <li><a href="/wiki/Multivitamin" title="Multivitamin">Multivitamin</a></li> <li><a href="/wiki/Nutrition" title="Nutrition">Nutrition</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="Halogens12" 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:Halogens" title="Template:Halogens"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Halogens" title="Template talk:Halogens"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Halogens" title="Special:EditPage/Template:Halogens"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Halogens12" style="font-size:114%;margin:0 4em"><a href="/wiki/Halogen" title="Halogen">Halogens</a></div></th></tr><tr><td colspan="2" class="navbox-list navbox-odd" style="width:100%;padding:0;background:transparent;color:inherit;"><div style="padding:0px"><table class="navbox-columns-table" style="border-spacing: 0px; text-align:left;width:auto; margin-left:auto; margin-right:auto;"><tbody><tr style="vertical-align:top"><td style="width:5em">   </td><td class="navbox-list" style="padding:0px;text-align:center;width:16%;"><div> <a class="mw-selflink selflink">Fluorine</a> F Atomic Number: 9 Atomic Weight: 18.9984032 Melting Point: 53.63 K Boiling Point: 85.03 K Specific mass: 0.001696 g/cm3 Electronegativity: 3.98 </div></td><td class="navbox-list" style="border-left:2px solid #fdfdfd;padding:0px;text-align:center;width:16%;"><div> <a href="/wiki/Chlorine" title="Chlorine">Chlorine</a> Cl Atomic Number: 17 Atomic Weight: 35.453 Melting Point: 172.31 K Boiling Point: 239.11 K Specific mass: 0.003214 g/cm3 Electronegativity: 3.16 </div></td><td class="navbox-list" style="border-left:2px solid #fdfdfd;padding:0px;text-align:center;width:16%;"><div> <a href="/wiki/Bromine" title="Bromine">Bromine</a> Br Atomic Number: 35 Atomic Weight: 79.904 Melting Point: 266.05 K Boiling Point: 332.0 K Specific mass: 3.122 g/cm3 Electronegativity: 2.96 </div></td><td class="navbox-list" style="border-left:2px solid #fdfdfd;padding:0px;text-align:center;width:16%;"><div> <a href="/wiki/Iodine" title="Iodine">Iodine</a> I Atomic Number: 53 Atomic Weight: 126.90447 Melting Point: 386.65 K Boiling Point: 475.4 K Specific mass: 4.93 g/cm3 Electronegativity: 2.66 </div></td><td class="navbox-list" style="border-left:2px solid #fdfdfd;padding:0px;text-align:center;width:16%;"><div> <a href="/wiki/Astatine" title="Astatine">Astatine</a> At Atomic Number: 85 Atomic Weight: [210] Melting Point: 575.15 K Boiling Point: 610 K Specific mass: 7 g/cm3 Electronegativity: 2.2 </div></td><td class="navbox-list" style="border-left:2px solid #fdfdfd;padding:0px;text-align:center;width:16%;"><div> <a href="/wiki/Tennessine" title="Tennessine">Tennessine</a> Ts Atomic Number: 117 Atomic Weight: [294] Melting Point: ? 573–773 K Boiling Point: ? 823 K Specific mass: ? g/cm3 Electronegativity: ? </div></td></tr></tbody></table></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" /><style data-mw-deduplicate="TemplateStyles:r1038841319">.mw-parser-output .tooltip-dotted{border-bottom:1px dotted;cursor:help}</style><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1038841319" /></div><div role="navigation" class="navbox authority-control" aria-label="Navbox1349" style="padding:3px"><table class="nowraplinks hlist navbox-inner" style="border-spacing:0;background:transparent;color:inherit"><tbody><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Help:Authority_control" title="Help:Authority control">Authority control databases</a>: National <a href="https://www.wikidata.org/wiki/Q650#identifiers" title="Edit this at Wikidata"><img alt="Edit this at Wikidata" src="//upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/10px-OOjs_UI_icon_edit-ltr-progressive.svg.png" decoding="async" width="10" height="10" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/15px-OOjs_UI_icon_edit-ltr-progressive.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/8/8a/OOjs_UI_icon_edit-ltr-progressive.svg/20px-OOjs_UI_icon_edit-ltr-progressive.svg.png 2x" data-file-width="20" data-file-height="20" /></a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"><ul><li><a rel="nofollow" class="external text" href="https://d-nb.info/gnd/4017696-4">Germany</a></li><li><a rel="nofollow" class="external text" href="https://id.loc.gov/authorities/sh85049424">United States</a></li><li><a rel="nofollow" class="external text" href="https://catalogue.bnf.fr/ark:/12148/cb11976289w">France</a></li><li><a rel="nofollow" class="external text" href="https://data.bnf.fr/ark:/12148/cb11976289w">BnF data</a></li><li><a rel="nofollow" class="external text" href="https://id.ndl.go.jp/auth/ndlna/00563785">Japan</a></li><li><a rel="nofollow" class="external text" href="https://aleph.nkp.cz/F/?func=find-c&local_base=aut&ccl_term=ica=ph171329&CON_LNG=ENG">Czech Republic</a></li><li><a rel="nofollow" class="external text" href="https://datos.bne.es/resource/XX531809">Spain</a></li><li><a rel="nofollow" class="external text" href="https://www.nli.org.il/en/authorities/987007538444105171">Israel</a></li></ul></div></td></tr></tbody></table></div>    </div><noscript><img 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class="mw-portlet mw-portlet-dock-bottom emptyPortlet" id="p-dock-bottom"> <ul> </ul> </div> <script>(RLQ=window.RLQ||[]).push(function(){mw.config.set({"wgHostname":"mw-web.codfw.main-74b7bb4b44-7fk7k","wgBackendResponseTime":395,"wgPageParseReport":{"limitreport":{"cputime":"4.188","walltime":"4.732","ppvisitednodes":{"value":52473,"limit":1000000},"postexpandincludesize":{"value":1159502,"limit":2097152},"templateargumentsize":{"value":66704,"limit":2097152},"expansiondepth":{"value":56,"limit":100},"expensivefunctioncount":{"value":41,"limit":500},"unstrip-depth":{"value":1,"limit":20},"unstrip-size":{"value":778262,"limit":5000000},"entityaccesscount":{"value":1,"limit":400},"timingprofile":["100.00% 4031.110 1 -total"," 36.55% 1473.298 4 Template:Infobox"," 30.19% 1217.174 1 Template:Infobox_fluorine"," 30.04% 1210.996 1 Template:Infobox_element"," 15.37% 619.484 100 Template:Cite_journal"," 11.38% 458.607 87 Template:Cite_book"," 10.54% 424.783 125 Template:Sfn"," 8.30% 334.651 2 Template:Reflist"," 6.67% 269.033 36 Template:Cite_web"," 5.06% 204.064 2 Template:Navbox"]},"scribunto":{"limitreport-timeusage":{"value":"2.414","limit":"10.000"},"limitreport-memusage":{"value":33541003,"limit":52428800},"limitreport-logs":"anchor_id_list = table#1 {\n [\"CITEREFAgricolaHooverHoover1912\"] = 1,\n [\"CITEREFAir_Products_and_Chemicals2004\"] = 1,\n [\"CITEREFAlaviHuang2007\"] = 1,\n [\"CITEREFAmpère1816\"] = 1,\n [\"CITEREFArana_et_al.2007\"] = 1,\n [\"CITEREFArmfield2007\"] = 1,\n [\"CITEREFAsimov1966\"] = 1,\n [\"CITEREFAtkinsJones2007\"] = 1,\n [\"CITEREFAucampBjörn2010\"] = 1,\n [\"CITEREFAugenstein_et_al.1991\"] = 1,\n [\"CITEREFBabelTressaud1985\"] = 1,\n [\"CITEREFBaelumSheihamBurt2008\"] = 1,\n [\"CITEREFBaezBaezMarthaler2000\"] = 1,\n [\"CITEREFBanks1986\"] = 1,\n [\"CITEREFBarbeeMcCormackVartanian2000\"] = 1,\n [\"CITEREFBarrettMeyerWasserman1967\"] = 1,\n [\"CITEREFBarryPhillips2006\"] = 1,\n [\"CITEREFBartlett1962\"] = 1,\n [\"CITEREFBeasley2002\"] = 1,\n [\"CITEREFBeckNewmanSchindlerPerkins2011\"] = 1,\n [\"CITEREFBeckerMüller1990\"] = 1,\n [\"CITEREFBetts2007\"] = 1,\n [\"CITEREFBiharyChabanGerber2002\"] = 1,\n [\"CITEREFBiller2007\"] = 1,\n [\"CITEREFBlodgettSurudaCrouch2001\"] = 1,\n [\"CITEREFBombourg2012\"] = 1,\n [\"CITEREFBrantley1949\"] = 1,\n [\"CITEREFBrody2012\"] = 1,\n [\"CITEREFBrown_et_al.2005\"] = 1,\n [\"CITEREFBurdonEmsonEdwards1987\"] = 1,\n [\"CITEREFBurney1999\"] = 1,\n [\"CITEREFBustamantePedersen1977\"] = 1,\n [\"CITEREFBuznik2009\"] = 1,\n [\"CITEREFBéguéBonnet-Delpon2008\"] = 1,\n [\"CITEREFCDC2001\"] = 1,\n [\"CITEREFCDC2013\"] = 1,\n [\"CITEREFCameron1973\"] = 1,\n [\"CITEREFCarey2008\"] = 1,\n [\"CITEREFChambersHolliday1975\"] = 1,\n [\"CITEREFChangGoldsby2013\"] = 1,\n [\"CITEREFChengChalmersSheldon2007\"] = 1,\n [\"CITEREFCheng_et_al.1999\"] = 1,\n [\"CITEREFChistéBé2011\"] = 1,\n [\"CITEREFChriste1986\"] = 1,\n [\"CITEREFChriste_Research_Groupn.d.\"] = 1,\n [\"CITEREFClark2002\"] = 1,\n [\"CITEREFClayton2003\"] = 1,\n [\"CITEREFCompressed_Gas_Association1999\"] = 1,\n [\"CITEREFCordero_et_al.2008\"] = 1,\n [\"CITEREFCracher2012\"] = 1,\n [\"CITEREFCroswell2003\"] = 1,\n [\"CITEREFDG_Environment2007\"] = 1,\n [\"CITEREFDavis2006\"] = 1,\n [\"CITEREFDavy1813\"] = 1,\n [\"CITEREFDeBergalis2004\"] = 1,\n [\"CITEREFDean1999\"] = 1,\n [\"CITEREFDrews_et_al.2006\"] = 1,\n [\"CITEREFDuPont2013a\"] = 1,\n [\"CITEREFDuPont2013b\"] = 1,\n [\"CITEREFEPA1996\"] = 1,\n [\"CITEREFEPA2012\"] = 1,\n [\"CITEREFEPA2013a\"] = 1,\n [\"CITEREFEPA2013b\"] = 1,\n [\"CITEREFEaton1997\"] = 1,\n [\"CITEREFEdwards1994\"] = 1,\n [\"CITEREFEinstein_et_al.1967\"] = 1,\n [\"CITEREFEisler1995\"] = 1,\n [\"CITEREFEl-Kareh1994\"] = 1,\n [\"CITEREFEl_Saadi_et_al.1989\"] = 1,\n [\"CITEREFEllis2001\"] = 1,\n [\"CITEREFEmeléusSharpe1974\"] = 1,\n [\"CITEREFEmeléusSharpe1983\"] = 1,\n [\"CITEREFEmsley1981\"] = 1,\n [\"CITEREFEmsley2011\"] = 1,\n [\"CITEREFEnergetics,_Inc.1997\"] = 1,\n [\"CITEREFFillerSaha2009\"] = 1,\n [\"CITEREFFischman2001\"] = 1,\n [\"CITEREFFood_and_Nutrition_Board\"] = 1,\n [\"CITEREFForster_et_al.2007\"] = 1,\n [\"CITEREFFultonMiller2006\"] = 1,\n [\"CITEREFGabriel_et_al.1996\"] = 1,\n [\"CITEREFGains1998\"] = 1,\n [\"CITEREFGessner_et_al.1994\"] = 1,\n [\"CITEREFGiesyKannan2002\"] = 1,\n [\"CITEREFGodfrey_et_al.1998\"] = 1,\n [\"CITEREFGreenSlinnSimpsonWoytek1994\"] = 1,\n [\"CITEREFGreenwoodEarnshaw1998\"] = 1,\n [\"CITEREFGribble2002\"] = 1,\n [\"CITEREFGrot2011\"] = 1,\n [\"CITEREFHSM2006\"] = 1,\n [\"CITEREFHagmann2008\"] = 1,\n [\"CITEREFHarbison2002\"] = 1,\n [\"CITEREFHasegawa_et_al.2007\"] = 1,\n [\"CITEREFHaxelHedrickOrris2005\"] = 1,\n [\"CITEREFHaynes2011\"] = 1,\n [\"CITEREFHimmelRiedel2007\"] = 1,\n [\"CITEREFHoffman_et_al.2007\"] = 1,\n [\"CITEREFHoogers2002\"] = 1,\n [\"CITEREFHounshellSmith1988\"] = 1,\n [\"CITEREFHultén_et_al.2004\"] = 1,\n [\"CITEREFICIS2006\"] = 1,\n [\"CITEREFJohnson2011\"] = 1,\n [\"CITEREFKacmarek_et_al.2006\"] = 1,\n [\"CITEREFKahlbow2024\"] = 1,\n [\"CITEREFKatakuse_et_al.1999\"] = 1,\n [\"CITEREFKellyMiller2005\"] = 1,\n [\"CITEREFKeplingerSuissa1968\"] = 1,\n [\"CITEREFKern_et_al.1994\"] = 1,\n [\"CITEREFKhriachtchev_et_al.2000\"] = 1,\n [\"CITEREFKingMaloneLilley2000\"] = 1,\n [\"CITEREFKirsch2004\"] = 1,\n [\"CITEREFKissa2001\"] = 1,\n [\"CITEREFKuriakoseMargrave1965\"] = 1,\n [\"CITEREFLagow1970\"] = 1,\n [\"CITEREFLau_et_al.2007\"] = 1,\n [\"CITEREFLee_et_al.2014\"] = 1,\n [\"CITEREFLewars2008\"] = 1,\n [\"CITEREFLide2004\"] = 1,\n [\"CITEREFLidinMolochkoAndreeva2000\"] = 1,\n [\"CITEREFLiteplo_et_al.2002\"] = 1,\n [\"CITEREFLusty_et_al.2008\"] = 1,\n [\"CITEREFMackayMackayHenderson2002\"] = 1,\n [\"CITEREFMacomber1996\"] = 1,\n [\"CITEREFMarggraf1770\"] = 1,\n [\"CITEREFMartin2007\"] = 1,\n [\"CITEREFMarya2011\"] = 1,\n [\"CITEREFMatsui2006\"] = 1,\n [\"CITEREFMcCoy2007\"] = 1,\n [\"CITEREFMeyer1977\"] = 1,\n [\"CITEREFMiller2003a\"] = 1,\n [\"CITEREFMiller2003b\"] = 1,\n [\"CITEREFMitchell2004\"] = 1,\n [\"CITEREFMitchell_Crow2011\"] = 1,\n [\"CITEREFMoellerBailarKleinberg1980\"] = 1,\n [\"CITEREFMoissan1886\"] = 1,\n [\"CITEREFMooreStanitskiJurs2010\"] = 1,\n [\"CITEREFMorrowPerryCohen1959\"] = 1,\n [\"CITEREFMurphySchaffrathO\u0026#039;Hagan2003\"] = 1,\n [\"CITEREFMurthyMehdi_AliAshok1995\"] = 1,\n [\"CITEREFNHMRC2007\"] = 1,\n [\"CITEREFNUBASE2016\"] = 1,\n [\"CITEREFNational_Nuclear_Data_CenterNuDat_2.1\"] = 1,\n [\"CITEREFNational_Oceanic_and_Atmospheric_Administration\"] = 1,\n [\"CITEREFNavarrini_et_al.2012\"] = 1,\n [\"CITEREFNelson1947\"] = 1,\n [\"CITEREFNelson_et_al.2007\"] = 1,\n [\"CITEREFNielsen2009\"] = 1,\n [\"CITEREFNorris_ShreveJoseph_Brink,_Jr.1977\"] = 1,\n [\"CITEREFNorwoodFohs1907\"] = 1,\n [\"CITEREFNourySilviGillespie2002\"] = 1,\n [\"CITEREFO\u0026#039;Hagan2008\"] = 1,\n [\"CITEREFO\u0026#039;Hagan_et_al.2002\"] = 1,\n [\"CITEREFOkada_et_al.1998\"] = 1,\n [\"CITEREFOkazoe2009\"] = 1,\n [\"CITEREFOlivaresUauy2004\"] = 1,\n [\"CITEREFPRWeb2010\"] = 1,\n [\"CITEREFPRWeb2012\"] = 1,\n [\"CITEREFPRWeb2013\"] = 1,\n [\"CITEREFParente2001\"] = 1,\n [\"CITEREFPartington1923\"] = 1,\n [\"CITEREFPatnaik2007\"] = 1,\n [\"CITEREFPauling1960\"] = 1,\n [\"CITEREFPaulingKeavenyRobinson1970\"] = 1,\n [\"CITEREFPerry2011\"] = 1,\n [\"CITEREFPitzer1975\"] = 1,\n [\"CITEREFPitzer1993\"] = 1,\n [\"CITEREFPizzo_et_al.2007\"] = 1,\n [\"CITEREFPosner2011\"] = 1,\n [\"CITEREFPosner_et_al.2013\"] = 1,\n [\"CITEREFPreskorn1996\"] = 1,\n [\"CITEREFPrincipe2012\"] = 1,\n [\"CITEREFProudfootBradberryVale2006\"] = 1,\n [\"CITEREFPyykköAtsumi2009\"] = 1,\n [\"CITEREFRaghavan1998\"] = 1,\n [\"CITEREFRajErdine2012\"] = 1,\n [\"CITEREFRamkumar2012\"] = 1,\n [\"CITEREFReddy2009\"] = 1,\n [\"CITEREFRenda_et_al.2004\"] = 1,\n [\"CITEREFRenner2006\"] = 1,\n [\"CITEREFRhoades2008\"] = 1,\n [\"CITEREFRichterHahnFuchs2001\"] = 1,\n [\"CITEREFRiedelKaupp2009\"] = 1,\n [\"CITEREFRipa1993\"] = 1,\n [\"CITEREFRoblin_et_al.2006\"] = 1,\n [\"CITEREFSalager2002\"] = 1,\n [\"CITEREFSandford2000\"] = 1,\n [\"CITEREFSarkar2008\"] = 1,\n [\"CITEREFScheele1771\"] = 1,\n [\"CITEREFSchimmeyer2002\"] = 1,\n [\"CITEREFSchlöderRiedel2012\"] = 1,\n [\"CITEREFSchmedtMangstlKraus2012\"] = 1,\n [\"CITEREFSchmitz_et_al.2000\"] = 1,\n [\"CITEREFSchulze-MakuchIrwin2008\"] = 1,\n [\"CITEREFSchwarcz2004\"] = 1,\n [\"CITEREFSenning2007\"] = 1,\n [\"CITEREFShafferWolfsonClark1992\"] = 1,\n [\"CITEREFShinSilverberg2013\"] = 1,\n [\"CITEREFShriverAtkins2010\"] = 1,\n [\"CITEREFShulmanWells1997\"] = 1,\n [\"CITEREFSlye2012\"] = 1,\n [\"CITEREFSteenlandFletcherSavitz2010\"] = 1,\n [\"CITEREFStillman1912\"] = 1,\n [\"CITEREFStorer1864\"] = 1,\n [\"CITEREFSwinson2005\"] = 1,\n [\"CITEREFTMR2013\"] = 1,\n [\"CITEREFTaber1999\"] = 1,\n [\"CITEREFTanner_Industries2011\"] = 1,\n [\"CITEREFThe_National_Institute_for_Occupational_Safety_and_Health1994a\"] = 1,\n [\"CITEREFThe_National_Institute_for_Occupational_Safety_and_Health1994b\"] = 1,\n [\"CITEREFTheodoridis2006\"] = 1,\n [\"CITEREFToon2011\"] = 1,\n [\"CITEREFTressaud2018\"] = 1,\n [\"CITEREFUllmann2008\"] = 1,\n [\"CITEREFVielGoldwhite1993\"] = 1,\n [\"CITEREFVigoureux1961\"] = 1,\n [\"CITEREFVillalbaAyresSchroder2008\"] = 1,\n [\"CITEREFWalsh2009\"] = 1,\n [\"CITEREFWalter2013\"] = 1,\n [\"CITEREFWeeks1932\"] = 1,\n [\"CITEREFWerner_et_al.2011\"] = 1,\n [\"CITEREFWibergWibergHolleman2001\"] = 1,\n [\"CITEREFWilley2007\"] = 1,\n [\"CITEREFXiao-HuaGuang-MinYan-MingJian-Hua2003\"] = 1,\n [\"CITEREFYawsBraker2001\"] = 1,\n [\"CITEREFYeung2008\"] = 1,\n [\"CITEREFYoung1975\"] = 1,\n [\"CITEREFZareitalabadSiemensHamerAmelung2013\"] = 1,\n [\"CITEREFZorich1991\"] = 1,\n}\ntemplate_list = table#1 {\n [\"Authority control\"] = 1,\n [\"Blockquote\"] = 1,\n [\"Chem\"] = 39,\n [\"Chembox\"] = 1,\n [\"Chembox Hazards\"] = 1,\n [\"Cite book\"] = 87,\n [\"Cite journal\"] = 96,\n [\"Cite magazine\"] = 1,\n [\"Cite news\"] = 2,\n [\"Cite report\"] = 7,\n [\"Cite thesis\"] = 1,\n [\"Cite web\"] = 34,\n [\"Clear\"] = 1,\n [\"Clear left\"] = 2,\n [\"Commons category-inline\"] = 1,\n [\"Convert\"] = 15,\n [\"Dietary supplement\"] = 1,\n [\"Distinguish\"] = 1,\n [\"Div col\"] = 1,\n [\"Div col end\"] = 1,\n [\"External media\"] = 1,\n [\"Featured article\"] = 1,\n [\"GHS03\"] = 1,\n [\"GHS05\"] = 1,\n [\"GHS06\"] = 1,\n [\"GHS07\"] = 1,\n [\"GHS08\"] = 1,\n [\"GHS09\"] = 1,\n [\"Gloss\"] = 1,\n [\"H-phrases\"] = 1,\n [\"Halogens\"] = 1,\n [\"Harvid\"] = 51,\n [\"Harvnb\"] = 192,\n [\"Ill\"] = 1,\n [\"Infobox fluorine\"] = 1,\n [\"Lang\"] = 1,\n [\"Main\"] = 17,\n [\"NUBASE2016\"] = 1,\n [\"NUBASE2020\"] = 1,\n [\"Nowrap\"] = 1,\n [\"Periodic table (navbox)\"] = 1,\n [\"Portal\"] = 1,\n [\"Refbegin\"] = 1,\n [\"Refend\"] = 1,\n [\"Reflist\"] = 2,\n [\"Refn\"] = 16,\n [\"See also\"] = 8,\n [\"Sfn\"] = 106,\n [\"Sfn whitelist\"] = 1,\n [\"TOC limit\"] = 1,\n [\"Ullmann\"] = 5,\n [\"Use dmy dates\"] = 1,\n [\"Webarchive\"] = 1,\n}\narticle_whitelist = table#1 {\n [\"CITEREFAigueperse_et_al.2000\"] = 1,\n [\"CITEREFCarlsonSchmiegel2000\"] = 1,\n [\"CITEREFJaccaud_et_al.2000\"] = 1,\n [\"CITEREFMeusingerChippendaleFairhurst2012\"] = 1,\n [\"CITEREFNUBASE2016\"] = 1,\n [\"CITEREFSiegemund_et_al.2005\"] = 1,\n}\nciteref_patterns = table#1 {\n}\n","limitreport-profile":[["?","940","33.8"],["dataWrapper \u003Cmw.lua:672\u003E","320","11.5"],["recursiveClone \u003CmwInit.lua:45\u003E","200","7.2"],["MediaWiki\\Extension\\Scribunto\\Engines\\LuaSandbox\\LuaSandboxCallback::anchorEncode","140","5.0"],["MediaWiki\\Extension\\Scribunto\\Engines\\LuaSandbox\\LuaSandboxCallback::callParserFunction","120","4.3"],["MediaWiki\\Extension\\Scribunto\\Engines\\LuaSandbox\\LuaSandboxCallback::gsub","120","4.3"],["MediaWiki\\Extension\\Scribunto\\Engines\\LuaSandbox\\LuaSandboxCallback::find","100","3.6"],["MediaWiki\\Extension\\Scribunto\\Engines\\LuaSandbox\\LuaSandboxCallback::plain","80","2.9"],["\u003Cmw.lua:694\u003E","80","2.9"],["MediaWiki\\Extension\\Scribunto\\Engines\\LuaSandbox\\LuaSandboxCallback::match","60","2.2"],["[others]","620","22.3"]]},"cachereport":{"origin":"mw-web.codfw.main-684955989f-ffgkf","timestamp":"20250331194425","ttl":2592000,"transientcontent":false}}});});</script> <script type="application/ld+json">{"@context":"https:\/\/schema.org","@type":"Article","name":"Fluorine","url":"https:\/\/en.wikipedia.org\/wiki\/Fluorine","sameAs":"http:\/\/www.wikidata.org\/entity\/Q650","mainEntity":"http:\/\/www.wikidata.org\/entity\/Q650","author":{"@type":"Organization","name":"Contributors to Wikimedia projects"},"publisher":{"@type":"Organization","name":"Wikimedia Foundation, Inc.","logo":{"@type":"ImageObject","url":"https:\/\/www.wikimedia.org\/static\/images\/wmf-hor-googpub.png"}},"datePublished":"2001-05-17T12:48:41Z","dateModified":"2025-03-31T19:43:19Z","image":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/2\/2c\/Fluoro_liquido_a_-196%C2%B0C_1.jpg","headline":"chemical element with symbol F and atomic number 9"}</script> </body> </html>