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class="vector-toc-list"> </ul> </li> <li id="toc-Solution" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Solution"> <div class="vector-toc-text"> <span class="vector-toc-numb">2.3</span> <span>Solution</span> </div> </a> <ul id="toc-Solution-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Preparation" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Preparation"> <div class="vector-toc-text"> <span class="vector-toc-numb">3</span> <span>Preparation</span> </div> </a> <ul id="toc-Preparation-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Reactions" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Reactions"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Reactions</span> </div> </a> <button aria-controls="toc-Reactions-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Reactions subsection</span> </button> <ul id="toc-Reactions-sublist" class="vector-toc-list"> <li id="toc-Anhydrous_FeCl3" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Anhydrous_FeCl3"> <div class="vector-toc-text"> <span class="vector-toc-numb">4.1</span> <span>Anhydrous FeCl<sub>3</sub></span> </div> </a> <ul id="toc-Anhydrous_FeCl3-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Hydrated_FeCl3" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Hydrated_FeCl3"> <div class="vector-toc-text"> <span class="vector-toc-numb">4.2</span> <span>Hydrated FeCl<sub>3</sub></span> </div> </a> <ul id="toc-Hydrated_FeCl3-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Organometallic_chemistry" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Organometallic_chemistry"> <div class="vector-toc-text"> <span class="vector-toc-numb">4.3</span> <span>Organometallic chemistry</span> </div> </a> <ul id="toc-Organometallic_chemistry-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Uses" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Uses"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>Uses</span> </div> </a> <button aria-controls="toc-Uses-sublist" class="cdx-button cdx-button--weight-quiet cdx-button--icon-only vector-toc-toggle"> <span class="vector-icon mw-ui-icon-wikimedia-expand"></span> <span>Toggle Uses subsection</span> </button> <ul id="toc-Uses-sublist" class="vector-toc-list"> <li id="toc-Water_treatment" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Water_treatment"> <div class="vector-toc-text"> <span class="vector-toc-numb">5.1</span> <span>Water treatment</span> </div> </a> <ul id="toc-Water_treatment-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Etching_and_metal_cleaning" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Etching_and_metal_cleaning"> <div class="vector-toc-text"> <span class="vector-toc-numb">5.2</span> <span>Etching and metal cleaning</span> </div> </a> <ul id="toc-Etching_and_metal_cleaning-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Organic_chemistry" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Organic_chemistry"> <div class="vector-toc-text"> <span class="vector-toc-numb">5.3</span> <span>Organic chemistry</span> </div> </a> <ul id="toc-Organic_chemistry-sublist" class="vector-toc-list"> <li id="toc-Organic_synthesis_research" class="vector-toc-list-item vector-toc-level-3"> <a class="vector-toc-link" href="#Organic_synthesis_research"> <div class="vector-toc-text"> <span class="vector-toc-numb">5.3.1</span> <span>Organic synthesis research</span> </div> </a> <ul id="toc-Organic_synthesis_research-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Histology" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Histology"> <div class="vector-toc-text"> <span class="vector-toc-numb">5.4</span> <span>Histology</span> </div> </a> <ul id="toc-Histology-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Natural_occurrence" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Natural_occurrence"> <div class="vector-toc-text"> <span class="vector-toc-numb">6</span> <span>Natural occurrence</span> </div> </a> <ul id="toc-Natural_occurrence-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Safety" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Safety"> <div class="vector-toc-text"> <span class="vector-toc-numb">7</span> <span>Safety</span> </div> </a> <ul id="toc-Safety-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Notes" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Notes"> <div class="vector-toc-text"> <span class="vector-toc-numb">8</span> <span>Notes</span> </div> </a> <ul id="toc-Notes-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-References" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#References"> <div class="vector-toc-text"> <span class="vector-toc-numb">9</span> <span>References</span> </div> </a> <ul id="toc-References-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Further_reading" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Further_reading"> <div class="vector-toc-text"> <span class="vector-toc-numb">10</span> <span>Further reading</span> </div> </a> <ul id="toc-Further_reading-sublist" class="vector-toc-list"> </ul> </li> </ul> </div> </div> </nav> </div> </div> <div class="mw-content-container"> <main id="content" class="mw-body"> <header class="mw-body-header vector-page-titlebar"> <nav aria-label="Contents" class="vector-toc-landmark"> <div id="vector-page-titlebar-toc" class="vector-dropdown vector-page-titlebar-toc vector-button-flush-left" > <input type="checkbox" id="vector-page-titlebar-toc-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-vector-page-titlebar-toc" class="vector-dropdown-checkbox " aria-label="Toggle the table of contents" > <label id="vector-page-titlebar-toc-label" for="vector-page-titlebar-toc-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--icon-only " aria-hidden="true" ><span class="vector-icon mw-ui-icon-listBullet mw-ui-icon-wikimedia-listBullet"></span> <span class="vector-dropdown-label-text">Toggle the table of contents</span> </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"><span class="mw-page-title-main">Iron(III) chloride</span></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 44 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-44" aria-hidden="true" ><span class="vector-icon mw-ui-icon-language-progressive mw-ui-icon-wikimedia-language-progressive"></span> <span class="vector-dropdown-label-text">44 languages</span> </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/Yster(III)chloried" title="Yster(III)chloried – Afrikaans" lang="af" hreflang="af" data-title="Yster(III)chloried" data-language-autonym="Afrikaans" data-language-local-name="Afrikaans" class="interlanguage-link-target"><span>Afrikaans</span></a></li><li class="interlanguage-link interwiki-ar mw-list-item"><a href="https://ar.wikipedia.org/wiki/%D9%83%D9%84%D9%88%D8%B1%D9%8A%D8%AF_%D8%A7%D9%84%D8%AD%D8%AF%D9%8A%D8%AF_%D8%A7%D9%84%D8%AB%D9%84%D8%A7%D8%AB%D9%8A" title="كلوريد الحديد الثلاثي – Arabic" lang="ar" hreflang="ar" data-title="كلوريد الحديد الثلاثي" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target"><span>العربية</span></a></li><li class="interlanguage-link interwiki-azb mw-list-item"><a href="https://azb.wikipedia.org/wiki/%DA%A9%D9%88%D9%84%D9%88%D8%B1%DB%8C%D8%AF_%D8%AF%D9%85%DB%8C%D8%B1_(III)" title="کولورید دمیر (III) – South Azerbaijani" lang="azb" hreflang="azb" data-title="کولورید دمیر (III)" data-language-autonym="تۆرکجه" data-language-local-name="South Azerbaijani" class="interlanguage-link-target"><span>تۆرکجه</span></a></li><li class="interlanguage-link interwiki-bn mw-list-item"><a href="https://bn.wikipedia.org/wiki/%E0%A6%AB%E0%A7%87%E0%A6%B0%E0%A6%BF%E0%A6%95_%E0%A6%95%E0%A7%8D%E0%A6%B2%E0%A7%8B%E0%A6%B0%E0%A6%BE%E0%A6%87%E0%A6%A1" title="ফেরিক ক্লোরাইড – Bangla" lang="bn" hreflang="bn" data-title="ফেরিক ক্লোরাইড" data-language-autonym="বাংলা" data-language-local-name="Bangla" class="interlanguage-link-target"><span>বাংলা</span></a></li><li class="interlanguage-link interwiki-ca mw-list-item"><a href="https://ca.wikipedia.org/wiki/Clorur_de_ferro(III)" title="Clorur de ferro(III) – Catalan" lang="ca" hreflang="ca" data-title="Clorur de ferro(III)" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target"><span>Català</span></a></li><li class="interlanguage-link interwiki-cs mw-list-item"><a href="https://cs.wikipedia.org/wiki/Chlorid_%C5%BEelezit%C3%BD" title="Chlorid železitý – Czech" lang="cs" hreflang="cs" data-title="Chlorid železitý" data-language-autonym="Čeština" data-language-local-name="Czech" class="interlanguage-link-target"><span>Čeština</span></a></li><li class="interlanguage-link interwiki-da mw-list-item"><a href="https://da.wikipedia.org/wiki/Jern(III)klorid" title="Jern(III)klorid – Danish" lang="da" hreflang="da" data-title="Jern(III)klorid" data-language-autonym="Dansk" data-language-local-name="Danish" class="interlanguage-link-target"><span>Dansk</span></a></li><li class="interlanguage-link interwiki-se mw-list-item"><a href="https://se.wikipedia.org/wiki/Ruovde(III)kloriida" title="Ruovde(III)kloriida – Northern Sami" lang="se" hreflang="se" data-title="Ruovde(III)kloriida" data-language-autonym="Davvisámegiella" data-language-local-name="Northern Sami" class="interlanguage-link-target"><span>Davvisámegiella</span></a></li><li class="interlanguage-link interwiki-de mw-list-item"><a href="https://de.wikipedia.org/wiki/Eisen(III)-chlorid" title="Eisen(III)-chlorid – German" lang="de" hreflang="de" data-title="Eisen(III)-chlorid" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target"><span>Deutsch</span></a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%9C%CE%BF%CE%BB%CF%85%CF%83%CE%AF%CF%84%CE%B7%CF%82" title="Μολυσίτης – Greek" lang="el" hreflang="el" data-title="Μολυσίτης" data-language-autonym="Ελληνικά" data-language-local-name="Greek" class="interlanguage-link-target"><span>Ελληνικά</span></a></li><li class="interlanguage-link interwiki-es mw-list-item"><a href="https://es.wikipedia.org/wiki/Cloruro_de_hierro(III)" title="Cloruro de hierro(III) – Spanish" lang="es" hreflang="es" data-title="Cloruro de hierro(III)" data-language-autonym="Español" data-language-local-name="Spanish" class="interlanguage-link-target"><span>Español</span></a></li><li class="interlanguage-link interwiki-eo mw-list-item"><a href="https://eo.wikipedia.org/wiki/Fera_(III)_klorido" title="Fera (III) klorido – Esperanto" lang="eo" hreflang="eo" data-title="Fera (III) klorido" data-language-autonym="Esperanto" data-language-local-name="Esperanto" class="interlanguage-link-target"><span>Esperanto</span></a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%D8%A2%D9%87%D9%86(III)_%DA%A9%D9%84%D8%B1%DB%8C%D8%AF" title="آهن(III) کلرید – Persian" lang="fa" hreflang="fa" data-title="آهن(III) کلرید" data-language-autonym="فارسی" data-language-local-name="Persian" class="interlanguage-link-target"><span>فارسی</span></a></li><li class="interlanguage-link interwiki-fr mw-list-item"><a href="https://fr.wikipedia.org/wiki/Chlorure_de_fer(III)" title="Chlorure de fer(III) – French" lang="fr" hreflang="fr" data-title="Chlorure de fer(III)" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target"><span>Français</span></a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%EC%97%BC%ED%99%94_%EC%B2%A0(III)" title="염화 철(III) – Korean" lang="ko" hreflang="ko" data-title="염화 철(III)" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target"><span>한국어</span></a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D4%B5%D6%80%D5%AF%D5%A1%D5%A9%D5%AB_%D5%A5%D5%BC%D6%84%D5%AC%D5%B8%D6%80%D5%AB%D5%A4" title="Երկաթի եռքլորիդ – Armenian" lang="hy" hreflang="hy" data-title="Երկաթի եռքլորիդ" data-language-autonym="Հայերեն" data-language-local-name="Armenian" class="interlanguage-link-target"><span>Հայերեն</span></a></li><li class="interlanguage-link interwiki-hi mw-list-item"><a href="https://hi.wikipedia.org/wiki/%E0%A4%86%E0%A4%AF%E0%A4%B0%E0%A4%A8(III)_%E0%A4%95%E0%A5%8D%E0%A4%B2%E0%A5%8B%E0%A4%B0%E0%A4%BE%E0%A4%87%E0%A4%A1" title="आयरन(III) क्लोराइड – Hindi" lang="hi" hreflang="hi" data-title="आयरन(III) क्लोराइड" data-language-autonym="हिन्दी" data-language-local-name="Hindi" class="interlanguage-link-target"><span>हिन्दी</span></a></li><li class="interlanguage-link interwiki-hr mw-list-item"><a href="https://hr.wikipedia.org/wiki/%C5%BDeljezov(III)_klorid" title="Željezov(III) klorid – Croatian" lang="hr" hreflang="hr" data-title="Željezov(III) klorid" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target"><span>Hrvatski</span></a></li><li class="interlanguage-link interwiki-id mw-list-item"><a href="https://id.wikipedia.org/wiki/Besi(III)_klorida" title="Besi(III) klorida – Indonesian" lang="id" hreflang="id" data-title="Besi(III) klorida" data-language-autonym="Bahasa Indonesia" data-language-local-name="Indonesian" class="interlanguage-link-target"><span>Bahasa Indonesia</span></a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Cloruro_ferrico" title="Cloruro ferrico – Italian" lang="it" hreflang="it" data-title="Cloruro ferrico" data-language-autonym="Italiano" data-language-local-name="Italian" class="interlanguage-link-target"><span>Italiano</span></a></li><li class="interlanguage-link interwiki-lv mw-list-item"><a href="https://lv.wikipedia.org/wiki/Dzelzs(III)_hlor%C4%ABds" title="Dzelzs(III) hlorīds – Latvian" lang="lv" hreflang="lv" data-title="Dzelzs(III) hlorīds" data-language-autonym="Latviešu" data-language-local-name="Latvian" class="interlanguage-link-target"><span>Latviešu</span></a></li><li class="interlanguage-link interwiki-hu mw-list-item"><a href="https://hu.wikipedia.org/wiki/Vas(III)-klorid" title="Vas(III)-klorid – Hungarian" lang="hu" hreflang="hu" data-title="Vas(III)-klorid" data-language-autonym="Magyar" data-language-local-name="Hungarian" class="interlanguage-link-target"><span>Magyar</span></a></li><li class="interlanguage-link interwiki-mk mw-list-item"><a href="https://mk.wikipedia.org/wiki/%D0%96%D0%B5%D0%BB%D0%B5%D0%B7%D0%BE(III)_%D1%85%D0%BB%D0%BE%D1%80%D0%B8%D0%B4" title="Железо(III) хлорид – Macedonian" lang="mk" hreflang="mk" data-title="Железо(III) хлорид" data-language-autonym="Македонски" data-language-local-name="Macedonian" class="interlanguage-link-target"><span>Македонски</span></a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/IJzer(III)chloride" title="IJzer(III)chloride – Dutch" lang="nl" hreflang="nl" data-title="IJzer(III)chloride" data-language-autonym="Nederlands" data-language-local-name="Dutch" class="interlanguage-link-target"><span>Nederlands</span></a></li><li class="interlanguage-link interwiki-ja mw-list-item"><a href="https://ja.wikipedia.org/wiki/%E5%A1%A9%E5%8C%96%E9%89%84(III)" title="塩化鉄(III) – Japanese" lang="ja" hreflang="ja" data-title="塩化鉄(III)" data-language-autonym="日本語" data-language-local-name="Japanese" class="interlanguage-link-target"><span>日本語</span></a></li><li class="interlanguage-link interwiki-ps mw-list-item"><a href="https://ps.wikipedia.org/wiki/%D9%88%D8%B3%D9%BE%D9%86%DB%90_(III)_%DA%A9%D9%84%D9%88%D8%B1%D8%A7%DB%8C%DA%89" title="وسپنې (III) کلورایډ – Pashto" lang="ps" hreflang="ps" data-title="وسپنې (III) کلورایډ" data-language-autonym="پښتو" data-language-local-name="Pashto" class="interlanguage-link-target"><span>پښتو</span></a></li><li class="interlanguage-link interwiki-pl mw-list-item"><a href="https://pl.wikipedia.org/wiki/Chlorek_%C5%BCelaza(III)" title="Chlorek żelaza(III) – Polish" lang="pl" hreflang="pl" data-title="Chlorek żelaza(III)" data-language-autonym="Polski" data-language-local-name="Polish" class="interlanguage-link-target"><span>Polski</span></a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/Cloreto_de_ferro(III)" title="Cloreto de ferro(III) – Portuguese" lang="pt" hreflang="pt" data-title="Cloreto de ferro(III)" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target"><span>Português</span></a></li><li class="interlanguage-link interwiki-ro mw-list-item"><a href="https://ro.wikipedia.org/wiki/Clorur%C4%83_de_fier_(III)" title="Clorură de fier (III) – Romanian" lang="ro" hreflang="ro" data-title="Clorură de fier (III)" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target"><span>Română</span></a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B6%D0%B5%D0%BB%D0%B5%D0%B7%D0%B0(III)" title="Хлорид железа(III) – Russian" lang="ru" hreflang="ru" data-title="Хлорид железа(III)" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target"><span>Русский</span></a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Iron(III)_chloride" title="Iron(III) chloride – Simple English" lang="en-simple" hreflang="en-simple" data-title="Iron(III) chloride" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target"><span>Simple English</span></a></li><li class="interlanguage-link interwiki-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/Chlorid_%C5%BEelezit%C3%BD" title="Chlorid železitý – Slovak" lang="sk" hreflang="sk" data-title="Chlorid železitý" data-language-autonym="Slovenčina" data-language-local-name="Slovak" class="interlanguage-link-target"><span>Slovenčina</span></a></li><li class="interlanguage-link interwiki-sl mw-list-item"><a href="https://sl.wikipedia.org/wiki/%C5%BDelezov(III)_klorid" title="Železov(III) klorid – Slovenian" lang="sl" hreflang="sl" data-title="Železov(III) klorid" data-language-autonym="Slovenščina" data-language-local-name="Slovenian" class="interlanguage-link-target"><span>Slovenščina</span></a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/Gvo%C5%BE%C4%91e(III)_hlorid" title="Gvožđe(III) hlorid – Serbian" lang="sr" hreflang="sr" data-title="Gvožđe(III) hlorid" data-language-autonym="Српски / srpski" data-language-local-name="Serbian" class="interlanguage-link-target"><span>Српски / srpski</span></a></li><li class="interlanguage-link interwiki-sh mw-list-item"><a href="https://sh.wikipedia.org/wiki/Gvo%C5%BE%C4%91e(III)_hlorid" title="Gvožđe(III) hlorid – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Gvožđe(III) hlorid" data-language-autonym="Srpskohrvatski / српскохрватски" data-language-local-name="Serbo-Croatian" class="interlanguage-link-target"><span>Srpskohrvatski / српскохрватски</span></a></li><li class="interlanguage-link interwiki-fi mw-list-item"><a href="https://fi.wikipedia.org/wiki/Rauta(III)kloridi" title="Rauta(III)kloridi – Finnish" lang="fi" hreflang="fi" data-title="Rauta(III)kloridi" data-language-autonym="Suomi" data-language-local-name="Finnish" class="interlanguage-link-target"><span>Suomi</span></a></li><li class="interlanguage-link interwiki-sv mw-list-item"><a href="https://sv.wikipedia.org/wiki/J%C3%A4rn(III)klorid" title="Järn(III)klorid – Swedish" lang="sv" hreflang="sv" data-title="Järn(III)klorid" data-language-autonym="Svenska" data-language-local-name="Swedish" class="interlanguage-link-target"><span>Svenska</span></a></li><li class="interlanguage-link interwiki-ta mw-list-item"><a href="https://ta.wikipedia.org/wiki/%E0%AE%87%E0%AE%B0%E0%AF%81%E0%AE%AE%E0%AF%8D%E0%AE%AA%E0%AF%81(III)_%E0%AE%95%E0%AF%81%E0%AE%B3%E0%AF%8B%E0%AE%B0%E0%AF%88%E0%AE%9F%E0%AF%81" title="இரும்பு(III) குளோரைடு – Tamil" lang="ta" hreflang="ta" data-title="இரும்பு(III) குளோரைடு" data-language-autonym="தமிழ்" data-language-local-name="Tamil" class="interlanguage-link-target"><span>தமிழ்</span></a></li><li class="interlanguage-link interwiki-te mw-list-item"><a href="https://te.wikipedia.org/wiki/%E0%B0%90%E0%B0%B0%E0%B0%A8%E0%B1%8D_(III)_%E0%B0%95%E0%B1%8D%E0%B0%B2%E0%B1%8B%E0%B0%B0%E0%B1%88%E0%B0%A1%E0%B1%8D" title="ఐరన్ (III) క్లోరైడ్ – Telugu" lang="te" hreflang="te" data-title="ఐరన్ (III) క్లోరైడ్" data-language-autonym="తెలుగు" data-language-local-name="Telugu" class="interlanguage-link-target"><span>తెలుగు</span></a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B9%84%E0%B8%AD%E0%B9%80%E0%B8%AD%E0%B8%B4%E0%B8%A3%E0%B9%8C%E0%B8%99(III)_%E0%B8%84%E0%B8%A5%E0%B8%AD%E0%B9%84%E0%B8%A3%E0%B8%94%E0%B9%8C" title="ไอเอิร์น(III) คลอไรด์ – Thai" lang="th" hreflang="th" data-title="ไอเอิร์น(III) คลอไรด์" data-language-autonym="ไทย" data-language-local-name="Thai" class="interlanguage-link-target"><span>ไทย</span></a></li><li class="interlanguage-link interwiki-tr mw-list-item"><a href="https://tr.wikipedia.org/wiki/Demir(III)_klor%C3%BCr" title="Demir(III) klorür – Turkish" lang="tr" hreflang="tr" data-title="Demir(III) klorür" data-language-autonym="Türkçe" data-language-local-name="Turkish" class="interlanguage-link-target"><span>Türkçe</span></a></li><li class="interlanguage-link interwiki-uk mw-list-item"><a href="https://uk.wikipedia.org/wiki/%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B7%D0%B0%D0%BB%D1%96%D0%B7%D0%B0(III)" title="Хлорид заліза(III) – Ukrainian" lang="uk" hreflang="uk" data-title="Хлорид заліза(III)" data-language-autonym="Українська" data-language-local-name="Ukrainian" class="interlanguage-link-target"><span>Українська</span></a></li><li class="interlanguage-link interwiki-vi mw-list-item"><a href="https://vi.wikipedia.org/wiki/S%E1%BA%AFt(III)_chloride" title="Sắt(III) chloride – Vietnamese" lang="vi" hreflang="vi" data-title="Sắt(III) chloride" data-language-autonym="Tiếng Việt" data-language-local-name="Vietnamese" class="interlanguage-link-target"><span>Tiếng Việt</span></a></li><li class="interlanguage-link interwiki-zh mw-list-item"><a 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Click here for more information."><img alt="This is a good article. Click here for more information." src="//upload.wikimedia.org/wikipedia/en/thumb/9/94/Symbol_support_vote.svg/19px-Symbol_support_vote.svg.png" decoding="async" width="19" height="20" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/94/Symbol_support_vote.svg/29px-Symbol_support_vote.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/94/Symbol_support_vote.svg/39px-Symbol_support_vote.svg.png 2x" data-file-width="180" data-file-height="185" /></a></span></div></div> </div> <div id="siteSub" class="noprint">From Wikipedia, the free encyclopedia</div> </div> <div id="contentSub"><div id="mw-content-subtitle"><span class="mw-redirectedfrom">(Redirected from <a href="/w/index.php?title=Ferric_chloride&redirect=no" class="mw-redirect" title="Ferric chloride">Ferric chloride</a>)</span></div></div> <div id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><p class="mw-empty-elt"> </p> <div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Inorganic compound</div> <p> <style data-mw-deduplicate="TemplateStyles:r1084375498">.mw-parser-output .ib-chembox{border-collapse:collapse;text-align:left}.mw-parser-output .ib-chembox td,.mw-parser-output .ib-chembox th{border:1px solid #a2a9b1;width:40%}.mw-parser-output .ib-chembox td+td{width:60%}</style> </p> <table class="infobox ib-chembox"> <caption>Iron(III) chloride </caption> <tbody><tr> <td colspan="2" class="borderless" style="text-align:center"> <table border="0" style="width:100%;display:inline-table;"> <tbody><tr> <td style="border-right:1px solid #aaa; width:50%;"><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Iron(III)_chloride_anhydrate.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/40/Iron%28III%29_chloride_anhydrate.jpg/110px-Iron%28III%29_chloride_anhydrate.jpg" decoding="async" width="110" height="147" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/40/Iron%28III%29_chloride_anhydrate.jpg/165px-Iron%28III%29_chloride_anhydrate.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/40/Iron%28III%29_chloride_anhydrate.jpg/220px-Iron%28III%29_chloride_anhydrate.jpg 2x" data-file-width="2448" data-file-height="3264" /></a><figcaption></figcaption></figure><div style="text-align:center">Iron(III) chloride (anhydrous)</div> </td> <td style="width:50%;"><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B6%D0%B5%D0%BB%D0%B5%D0%B7%D0%B0.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e6/%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B6%D0%B5%D0%BB%D0%B5%D0%B7%D0%B0.jpg/110px-%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B6%D0%B5%D0%BB%D0%B5%D0%B7%D0%B0.jpg" decoding="async" width="110" height="235" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/e6/%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B6%D0%B5%D0%BB%D0%B5%D0%B7%D0%B0.jpg/165px-%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B6%D0%B5%D0%BB%D0%B5%D0%B7%D0%B0.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/e6/%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B6%D0%B5%D0%BB%D0%B5%D0%B7%D0%B0.jpg/220px-%D0%A5%D0%BB%D0%BE%D1%80%D0%B8%D0%B4_%D0%B6%D0%B5%D0%BB%D0%B5%D0%B7%D0%B0.jpg 2x" data-file-width="838" data-file-height="1788" /></a><figcaption></figcaption></figure><div style="text-align:center">Iron(III) chloride (hydrate)</div> </td></tr></tbody></table> </td></tr> <tr> <td colspan="2" class="borderless" style="text-align:center"> <table border="0" style="width:100%;display:inline-table;"> <tbody><tr> <td style="border-right:1px solid #aaa; width:50%;"><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Iron-trichloride-sheet-3D-polyhedra.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/07/Iron-trichloride-sheet-3D-polyhedra.png/110px-Iron-trichloride-sheet-3D-polyhedra.png" decoding="async" width="110" height="76" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/07/Iron-trichloride-sheet-3D-polyhedra.png/165px-Iron-trichloride-sheet-3D-polyhedra.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/07/Iron-trichloride-sheet-3D-polyhedra.png/220px-Iron-trichloride-sheet-3D-polyhedra.png 2x" data-file-width="1100" data-file-height="757" /></a><figcaption></figcaption></figure> </td> <td style="width:50%;"><figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:Iron-trichloride-sheets-stacking-3D-polyhedra.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/9/95/Iron-trichloride-sheets-stacking-3D-polyhedra.png/110px-Iron-trichloride-sheets-stacking-3D-polyhedra.png" decoding="async" width="110" height="84" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/9/95/Iron-trichloride-sheets-stacking-3D-polyhedra.png/165px-Iron-trichloride-sheets-stacking-3D-polyhedra.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/9/95/Iron-trichloride-sheets-stacking-3D-polyhedra.png/220px-Iron-trichloride-sheets-stacking-3D-polyhedra.png 2x" data-file-width="1100" data-file-height="843" /></a><figcaption></figcaption></figure> </td></tr></tbody></table> </td></tr> <tr> <th colspan="2" style="background: #f8eaba; text-align: center;">Names </th></tr> <tr> <td colspan="2" style="text-align:left;"><a href="/wiki/Chemical_nomenclature" title="Chemical nomenclature">IUPAC names</a> <div style="max-width:22em; word-wrap:break-word; padding-left:1.7em;">Iron(III) chloride<br />Iron trichloride</div> </td></tr> <tr> <td colspan="2" style="text-align:left;">Other names <div style="max-width:22em; word-wrap:break-word; padding-left:1.7em;"><style data-mw-deduplicate="TemplateStyles:r1126788409">.mw-parser-output .plainlist ol,.mw-parser-output .plainlist ul{line-height:inherit;list-style:none;margin:0;padding:0}.mw-parser-output .plainlist ol li,.mw-parser-output .plainlist ul li{margin-bottom:0}</style><div class="plainlist"><ul><li>Ferric chloride</li><li>Molysite</li><li>Flores martis</li></ul></div></div> </td></tr> <tr> <th colspan="2" style="background: #f8eaba; text-align: center;">Identifiers </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/CAS_Registry_Number" title="CAS Registry Number">CAS Number</a></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="commonchemistry.cas.org"><a rel="nofollow" class="external text" href="https://commonchemistry.cas.org/detail?cas_rn=7705-08-0">7705-08-0</a></span><sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li><li><span title="commonchemistry.cas.org"><a rel="nofollow" class="external text" href="https://commonchemistry.cas.org/detail?cas_rn=10025-77-1">10025-77-1</a></span> (hexahydrate)<sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li><li><span title="commonchemistry.cas.org"><a rel="nofollow" class="external text" href="https://commonchemistry.cas.org/detail?cas_rn=54862-84-9">54862-84-9</a></span> (dihydrate)<sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li><li><span title="commonchemistry.cas.org"><a rel="nofollow" class="external text" href="https://commonchemistry.cas.org/detail?cas_rn=64333-00-2">64333-00-2</a></span> (3.5hydrate)</li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">3D model (<a href="/wiki/JSmol" class="mw-redirect" title="JSmol">JSmol</a>)</div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="chemapps.stolaf.edu (3D interactive model)"><a rel="nofollow" class="external text" href="https://chemapps.stolaf.edu/jmol/jmol.php?model=Cl%5BFe%5D%28Cl%29Cl">Interactive image</a></span></li></ul></div> </td></tr> <tr> <td><a href="/wiki/ChEBI" title="ChEBI">ChEBI</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="www.ebi.ac.uk"><a rel="nofollow" class="external text" href="https://www.ebi.ac.uk/chebi/searchId.do?chebiId=30808">CHEBI:30808</a></span><sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li></ul></div> </td></tr> <tr> <td><a href="/wiki/ChemSpider" title="ChemSpider">ChemSpider</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="www.chemspider.com"><a rel="nofollow" class="external text" href="https://www.chemspider.com/Chemical-Structure.22792.html">22792</a></span><sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li></ul></div> </td></tr> <tr> <td><a href="/wiki/ECHA_InfoCard" class="mw-redirect" title="ECHA InfoCard"><span title="echa.europa.eu">ECHA InfoCard</span></a> </td> <td><a rel="nofollow" class="external text" href="https://echa.europa.eu/substance-information/-/substanceinfo/100.028.846">100.028.846</a> <span class="mw-valign-text-top noprint" typeof="mw:File/Frameless"><a href="https://www.wikidata.org/wiki/Q399771#P2566" 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></span> </td></tr> <tr> <td><a href="/wiki/European_Community_number" title="European Community number"><span title="European Community number (chemical identifier)">EC Number</span></a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>231-729-4</li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/PubChem" title="PubChem">PubChem</a> <abbr title="Compound ID">CID</abbr></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="pubchem.ncbi.nlm.nih.gov"><a rel="nofollow" class="external text" href="https://pubchem.ncbi.nlm.nih.gov/compound/24380">24380</a></span></li></ul></div> </td></tr> <tr> <td><a href="/wiki/RTECS" class="mw-redirect" title="RTECS">RTECS number</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>LJ9100000</li></ul></div> </td></tr> <tr> <td><a href="/wiki/Unique_Ingredient_Identifier" title="Unique Ingredient Identifier">UNII</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="precision.fda.gov"><a rel="nofollow" class="external text" href="https://precision.fda.gov/uniisearch/srs/unii/U38V3ZVV3V">U38V3ZVV3V</a></span><sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li><li><span title="precision.fda.gov"><a rel="nofollow" class="external text" href="https://precision.fda.gov/uniisearch/srs/unii/0I2XIN602U">0I2XIN602U</a></span> (hexahydrate)<sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li><li><span title="precision.fda.gov"><a rel="nofollow" class="external text" href="https://precision.fda.gov/uniisearch/srs/unii/Y048945596">Y048945596</a></span> (dihydrate)<sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></li></ul></div> </td></tr> <tr> <td><a href="/wiki/UN_number" title="UN number">UN number</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>1773 (anhydrous)</li><li>2582 (aqueous solution)</li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/CompTox_Chemicals_Dashboard" title="CompTox Chemicals Dashboard">CompTox Dashboard</a> <span style="font-weight:normal">(<abbr title="U.S. Environmental Protection Agency">EPA</abbr>)</span></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span title="comptox.epa.gov"><a rel="nofollow" class="external text" href="https://comptox.epa.gov/dashboard/chemical/details/DTXSID8020622">DTXSID8020622</a> <span class="mw-valign-text-top noprint" typeof="mw:File/Frameless"><a href="https://www.wikidata.org/wiki/Q399771#P3117" 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></span></span></li></ul></div> </td></tr> <tr> <td colspan="2"><div class="collapsible-list mw-collapsible mw-collapsed" style="text-align: left;"> <div style="line-height: 1.6em; font-weight: bold; text-align:left; font-weight:normal; background:transparent;"><div><a href="/wiki/International_Chemical_Identifier" title="International Chemical Identifier">InChI</a></div></div> <ul class="mw-collapsible-content" style="margin-top: 0; margin-bottom: 0; line-height: inherit; list-style: none; margin-left: 0; word-break:break-all;"><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.5em; text-align:left;"><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">InChI=1S/3ClH.Fe/h3*1H;/q;;;+3/p-3<sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></div><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">Key: RBTARNINKXHZNM-UHFFFAOYSA-K<sup> <span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span></sup></div></div></li><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.5em; text-align:left;"><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">InChI=1S/3ClH.Fe/h3*1H;/q;;;+3/p-3</div><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">Key: RBTARNINKXHZNM-DFZHHIFOAF</div></div></li><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.5em; text-align:left;"><div style="word-wrap:break-word; text-indent:-1.5em; font-size:97%; line-height:120%;">Key: RBTARNINKXHZNM-UHFFFAOYSA-K</div></div></li></ul> </div> </td></tr> <tr> <td colspan="2"><div class="collapsible-list mw-collapsible mw-collapsed" style="text-align: left;"> <div style="line-height: 1.6em; font-weight: bold; text-align:left; font-weight:normal; background:transparent;"><div><a href="/wiki/Simplified_molecular-input_line-entry_system" class="mw-redirect" title="Simplified molecular-input line-entry system">SMILES</a></div></div> <ul class="mw-collapsible-content" style="margin-top: 0; margin-bottom: 0; line-height: inherit; list-style: none; margin-left: 0; word-break:break-all;"><li style="line-height: inherit; margin: 0"><div style="border-top:1px solid #ccc; padding:0.2em 0 0.2em 1.6em; word-wrap:break-word; text-indent:-1.5em; text-align:left; font-size:97%; line-height:120%;">Cl[Fe](Cl)Cl</div></li></ul> </div> </td></tr> <tr> <th colspan="2" style="background: #f8eaba; text-align: center;">Properties </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Chemical_formula" title="Chemical formula">Chemical formula</a></div> </td> <td><style data-mw-deduplicate="TemplateStyles:r1123817410">.mw-parser-output .template-chem2-su{display:inline-block;font-size:80%;line-height:1;vertical-align:-0.35em}.mw-parser-output .template-chem2-su>span{display:block;text-align:left}.mw-parser-output sub.template-chem2-sub{font-size:80%;vertical-align:-0.35em}.mw-parser-output sup.template-chem2-sup{font-size:80%;vertical-align:0.65em}</style><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub></span>  </td></tr> <tr> <td><a href="/wiki/Molar_mass" title="Molar mass">Molar mass</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>162.204<span class="nowrap"> </span>g/mol (anhydrous)</li><li>270.295<span class="nowrap"> </span>g/mol (hexahydrate)<sup id="cite_ref-crc_1-0" class="reference"><a href="#cite_note-crc-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup></li></ul></div>    </td></tr> <tr> <td>Appearance </td> <td>Green-black by reflected light; purple-red by transmitted light; yellow solid as hexahydrate; brown as aqueous solution </td></tr> <tr> <td><a href="/wiki/Odor" title="Odor">Odor</a> </td> <td>Slight <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">HCl</a> </td></tr> <tr> <td><a href="/wiki/Density" title="Density">Density</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>2.90<span class="nowrap"> </span>g/cm<sup>3</sup> (anhydrous)</li><li>1.82<span class="nowrap"> </span>g/cm<sup>3</sup> (hexahydrate)<sup id="cite_ref-crc_1-1" class="reference"><a href="#cite_note-crc-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup></li></ul></div> </td></tr> <tr> <td><a href="/wiki/Melting_point" title="Melting point">Melting point</a> </td> <td>307.6 °C (585.7 °F; 580.8 K) (anhydrous)<br />37 °C (99 °F; 310 K) (hexahydrate)<sup id="cite_ref-crc_1-5" class="reference"><a href="#cite_note-crc-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> </td></tr> <tr> <td><a href="/wiki/Boiling_point" title="Boiling point">Boiling point</a> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li>316 °C (601 °F; 589 K) (anhydrous, decomposes)<sup id="cite_ref-crc_1-2" class="reference"><a href="#cite_note-crc-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup></li><li>280 °C (536 °F; 553 K) (hexahydrate, decomposes)</li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Aqueous_solution" title="Aqueous solution">Solubility in water</a></div> </td> <td>912<span class="nowrap"> </span>g/L (anhydrous or hexahydrate, 25<span class="nowrap"> </span>°C)<sup id="cite_ref-crc_1-3" class="reference"><a href="#cite_note-crc-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup> </td></tr> <tr> <td><a href="/wiki/Solubility" title="Solubility">Solubility</a> in <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a href="/wiki/Acetone" title="Acetone">Acetone</a></li><li><a href="/wiki/Methanol" title="Methanol">Methanol</a></li><li><a href="/wiki/Ethanol" title="Ethanol">Ethanol</a></li><li><a href="/wiki/Diethyl_ether" title="Diethyl ether">Diethyl ether</a><sup id="cite_ref-crc_1-4" class="reference"><a href="#cite_note-crc-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup></li></ul></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><span class="nowrap"> </span></li><li>630 g/L (18 °C)</li><li>Highly soluble</li><li>830 g/L</li><li>Highly soluble</li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Magnetic_susceptibility" title="Magnetic susceptibility">Magnetic susceptibility</a> (χ)</div> </td> <td>+13,450·10<sup>−6</sup><span class="nowrap"> </span>cm<sup>3</sup>/mol<sup id="cite_ref-2" class="reference"><a href="#cite_note-2"><span class="cite-bracket">[</span>2<span class="cite-bracket">]</span></a></sup> </td></tr> <tr> <td><a href="/wiki/Viscosity" title="Viscosity">Viscosity</a> </td> <td>12 c<a href="/wiki/Poise_(unit)" title="Poise (unit)">P</a> (40% solution) </td></tr> <tr> <th colspan="2" style="background: #f8eaba; text-align: center;">Hazards<sup id="cite_ref-4" class="reference"><a href="#cite_note-4"><span class="cite-bracket">[</span>4<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-5" class="reference"><a href="#cite_note-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-7" class="reference"><a href="#cite_note-7"><span class="cite-bracket">[</span>Note 1<span class="cite-bracket">]</span></a></sup> </th></tr> <tr> <td colspan="2" style="text-align:left; background-color:#eaeaea;"><a href="/wiki/Globally_Harmonized_System_of_Classification_and_Labelling_of_Chemicals" title="Globally Harmonized System of Classification and Labelling of Chemicals"><b>GHS</b> 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><span typeof="mw:File"><a href="/wiki/File:GHS-pictogram-acid.svg" class="mw-file-description" title="Corr. Met. 1; Skin Corr. 1C; Eye Dam. 1"><img alt="Corr. Met. 1; Skin Corr. 1C; Eye Dam. 1" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a1/GHS-pictogram-acid.svg/50px-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/75px-GHS-pictogram-acid.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a1/GHS-pictogram-acid.svg/100px-GHS-pictogram-acid.svg.png 2x" data-file-width="724" data-file-height="724" /></a></span><span typeof="mw:File"><a href="/wiki/File:GHS-pictogram-exclam.svg" class="mw-file-description" title="Acute Tox. 4 (oral)"><img alt="Acute Tox. 4 (oral)" 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></span> </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><b>Danger</b> </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="H290: May be corrosive to metals">H290</abbr>, <abbr class="abbr" title="H302: Harmful if swallowed">H302</abbr>, <abbr class="abbr" title="H314: Causes severe skin burns and eye damage">H314</abbr> </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/GHS_precautionary_statements" title="GHS precautionary statements">Precautionary statements</a></div> </td> <td><abbr class="abbr" title="P234: Keep only in original container/packaging.">P234</abbr>, <abbr class="abbr" title="P260: Do not breathe dust/fume/gas/mist/vapours/spray.">P260</abbr>, <abbr class="abbr" title="P264: Wash ... thoroughly after handling.">P264</abbr>, <abbr class="abbr" title="P270: Do not eat, drink or smoke when using this product.">P270</abbr>, <abbr class="abbr" title="P273: Avoid release to the environment.">P273</abbr>, <abbr class="abbr" title="P280: Wear protective gloves/protective clothing/eye protection/face protection.">P280</abbr>, <abbr class="abbr" title="P301+P312: IF SWALLOWED: Call a POISON CENTER or doctor/physician if you feel unwell.">P301+P312</abbr>, <abbr class="abbr" title="P301+P330+P331: IF SWALLOWED: Rinse mouth. Do NOT induce vomiting.">P301+P330+P331</abbr>, <abbr class="abbr" title="P303+P361+P353: IF ON SKIN (or hair): Remove/Take off immediately all contaminated clothing. Rinse skin with water [or shower].">P303+P361+P353</abbr>, <abbr class="abbr" title="P304+P340: IF INHALED: Remove victim to fresh air and keep at rest in a position comfortable for breathing.">P304+P340</abbr>, <abbr class="abbr" title="P305+P351+P338: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do. Continue rinsing.">P305+P351+P338</abbr>, <abbr class="abbr" title="P310: Immediately call a POISON CENTER or doctor/physician.">P310</abbr>, <abbr class="abbr" title="P321: Specific treatment (see ... on this label).">P321</abbr>, <abbr class="abbr" title="P363: Wash contaminated clothing before reuse.">P363</abbr>, <abbr class="abbr" title="P390: Absorb spillage to prevent material damage.">P390</abbr>, <abbr class="abbr" title="P405: Store locked up.">P405</abbr>, <abbr class="abbr" title="P406: Store in a corrosive resistant/... container with a resistant inner liner.">P406</abbr>, <abbr class="abbr" title="P501: Dispose of contents/container to ...">P501</abbr> </td></tr> <tr> <td><a href="/wiki/NFPA_704" title="NFPA 704"><b>NFPA 704</b></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"><span><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_b27845110d7e52b0" /></span><map name="ImageMap_b27845110d7e52b0"><area href="/wiki/NFPA_704#Blue" shape="poly" coords="23,23,47,47,23,70,0,47" alt="Health 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroform" title="Health 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroform" /><area href="/wiki/NFPA_704#Red" shape="poly" coords="47,0,70,23,47,47,23,23" alt="Flammability 0: Will not burn. E.g. water" title="Flammability 0: Will not burn. E.g. water" /><area href="/wiki/NFPA_704#Yellow" shape="poly" coords="70,23,94,47,70,70,47,47" alt="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" title="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" /><area href="/wiki/NFPA_704#White" shape="poly" coords="47,47,70,70,47,94,23,70" alt="Special hazards (white): no code" title="Special hazards (white): no code" /></map><figcaption></figcaption></figure></div><div class="nfpa-704-diamond-code nfpa-704-diamond-blue"> <a href="/wiki/NFPA_704#Blue" title="NFPA 704"><span title="Health 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroform" class="notheme mw-no-invert">2</span></a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-red"> <a href="/wiki/NFPA_704#Red" title="NFPA 704"><span title="Flammability 0: Will not burn. E.g. water" class="notheme mw-no-invert">0</span></a></div><div class="nfpa-704-diamond-code nfpa-704-diamond-yellow"> <a href="/wiki/NFPA_704#Yellow" title="NFPA 704"><span title="Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen" class="notheme mw-no-invert">0</span></a></div></div></div></div> </td></tr> <tr> <td><a href="/wiki/Flash_point" title="Flash point">Flash point</a> </td> <td>Non-flammable </td></tr> <tr> <td colspan="2" style="text-align:left; background-color:#eaeaea;"><a href="/wiki/National_Institute_for_Occupational_Safety_and_Health" title="National Institute for Occupational Safety and Health"><b>NIOSH</b></a> (US health exposure limits): </td></tr> <tr> <td style="padding-left:1em;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Recommended_exposure_limit" title="Recommended exposure limit">REL</a> (Recommended)</div> </td> <td>TWA 1<span class="nowrap"> </span>mg/m<sup>3</sup><sup id="cite_ref-3" class="reference"><a href="#cite_note-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> </td></tr> <tr> <td><a href="/wiki/Safety_data_sheet" title="Safety data sheet">Safety data sheet</a> (SDS) </td> <td><a href="/wiki/International_Chemical_Safety_Card" class="mw-redirect" title="International Chemical Safety Card">ICSC</a> <span class="plainlinks noexpand"><a rel="nofollow" class="external text" href="http://www.inchem.org/documents/icsc/icsc/eics1499.htm">1499</a></span> </td></tr> <tr> <th colspan="2" style="background: #f8eaba; text-align: center;">Related compounds </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Other <a href="/wiki/Ion" title="Ion">anions</a></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a href="/wiki/Iron(III)_fluoride" title="Iron(III) fluoride">Iron(III) fluoride</a></li><li><a href="/wiki/Iron(III)_bromide" title="Iron(III) bromide">Iron(III) bromide</a></li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Other <a href="/wiki/Ion" title="Ion">cations</a></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a href="/wiki/Iron(II)_chloride" title="Iron(II) chloride">Iron(II) chloride</a></li><li><a href="/wiki/Manganese(II)_chloride" title="Manganese(II) chloride">Manganese(II) chloride</a></li><li><a href="/wiki/Cobalt(II)_chloride" title="Cobalt(II) chloride">Cobalt(II) chloride</a></li><li><a href="/wiki/Ruthenium(III)_chloride" title="Ruthenium(III) chloride">Ruthenium(III) chloride</a></li></ul></div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Related <a href="/wiki/Flocculation" title="Flocculation">coagulants</a></div> </td> <td><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1126788409"><div class="plainlist"><ul><li><a href="/wiki/Iron(II)_sulfate" title="Iron(II) sulfate">Iron(II) sulfate</a></li><li><a href="/wiki/Aluminium_chloride" title="Aluminium chloride">Polyaluminium chloride</a></li></ul></div> </td></tr> <tr> <th colspan="2" style="background: #f8eaba; text-align: center;">Structure </th></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Crystal_structure" title="Crystal structure">Crystal structure</a></div> </td> <td><a href="/wiki/Hexagonal_crystal_system" class="mw-redirect" title="Hexagonal crystal system">Hexagonal</a>, <a href="/wiki/Pearson_symbol" title="Pearson symbol">hR24</a> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Space_group" title="Space group">Space group</a></div> </td> <td>R<span style="text-decoration:overline;">3</span>, No. 148<sup id="cite_ref-str_8-0" class="reference"><a href="#cite_note-str-8"><span class="cite-bracket">[</span>7<span class="cite-bracket">]</span></a></sup> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Lattice_constant" title="Lattice constant">Lattice constant</a></div> </td> <td><div><i>a</i> = 0.6065<span class="nowrap"> </span>nm, <i>b</i> = 0.6065<span class="nowrap"> </span>nm, <i>c</i> = 1.742<span class="nowrap"> </span>nm</div><div>α = 90°, β = 90°, γ = 120°</div> </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Formula_unit" title="Formula unit">Formula units</a> (<i>Z</i>)</div> </td> <td>6 </td></tr> <tr> <td><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;"><a href="/wiki/Coordination_geometry" title="Coordination geometry">Coordination geometry</a></div> </td> <td><a href="/wiki/Octahedral" class="mw-redirect" title="Octahedral">Octahedral</a> </td></tr> <tr> <td colspan="2" style="text-align:left; background:#f8eaba; border:1px solid #a2a9b1;"><div style="display: inline-block; line-height: 1.2em; padding: .1em 0;">Except where otherwise noted, data are given for materials in their <a href="/wiki/Standard_state" title="Standard state">standard state</a> (at 25 °C [77 °F], 100 kPa).</div> <div style="margin-top: 0.3em;"><div style="text-align:center;"><span typeof="mw:File"><span><img alt="☒" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/12px-X_mark.svg.png" decoding="async" width="12" height="14" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/18px-X_mark.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/24px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" /></span></span><span style="display:none">N</span> <span class="reflink plainlinks nourlexpansion"><a class="external text" href="https://en.wikipedia.org/w/index.php?title=Special:ComparePages&rev1=476995973&page2=Iron%28III%29+chloride">verify</a></span> (<a href="/wiki/Wikipedia:WikiProject_Chemicals/Chembox_validation" title="Wikipedia:WikiProject Chemicals/Chembox validation">what is</a> <sup><span typeof="mw:File"><span><img alt="check" src="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/7px-Yes_check.svg.png" decoding="async" width="7" height="7" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/11px-Yes_check.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/f/fb/Yes_check.svg/14px-Yes_check.svg.png 2x" data-file-width="600" data-file-height="600" /></span></span><span style="display:none">Y</span><span typeof="mw:File"><span><img alt="☒" src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/7px-X_mark.svg.png" decoding="async" width="7" height="8" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/11px-X_mark.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/a/a2/X_mark.svg/14px-X_mark.svg.png 2x" data-file-width="525" data-file-height="600" /></span></span><span style="display:none">N</span></sup> ?) </div></div> <div style="margin-top: 0.3em; text-align: center;"><a href="/wiki/Wikipedia:Chemical_infobox#References" title="Wikipedia:Chemical infobox">Infobox references</a></div> </td></tr> </tbody></table><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical compound</div> <p><b>Iron(III) chloride</b> describes the inorganic compounds with the formula <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Iron" title="Iron">Fe</a><a href="/wiki/Chloride" title="Chloride">Cl</a><sub class="template-chem2-sub">3</sub></span>(H<sub>2</sub>O)<sub>x</sub>. Also called <b>ferric chloride</b>, these compounds are some of the most important and commonplace compounds of iron. They are available both in anhydrous and in hydrated forms, which are both <a href="/wiki/Hygroscopic" class="mw-redirect" title="Hygroscopic">hygroscopic</a>. They feature iron in its +3 <a href="/wiki/Oxidation_state" title="Oxidation state">oxidation state</a>. The anhydrous derivative is a <a href="/wiki/Lewis_acid" class="mw-redirect" title="Lewis acid">Lewis acid</a>, while all forms are mild oxidizing agents. It is used as a <a href="/wiki/Water_treatment" title="Water treatment">water cleaner</a> and as an <a href="/wiki/Chemical_milling" title="Chemical milling">etchant</a> for metals. </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Electronic_and_optical_properties">Electronic and optical properties</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=1" title="Edit section: Electronic and optical properties"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Aluminium-trichloride-dimer-3D-balls.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Aluminium-trichloride-dimer-3D-balls.png/144px-Aluminium-trichloride-dimer-3D-balls.png" decoding="async" width="144" height="81" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Aluminium-trichloride-dimer-3D-balls.png/216px-Aluminium-trichloride-dimer-3D-balls.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/fa/Aluminium-trichloride-dimer-3D-balls.png/288px-Aluminium-trichloride-dimer-3D-balls.png 2x" data-file-width="1100" data-file-height="617" /></a><figcaption>Anhydrous iron(III) chloride evaporates at relatively low temperatures to give the bitetrahedral dimer.</figcaption></figure> <p>All forms of ferric chloride are <a href="/wiki/Paramagnetic" class="mw-redirect" title="Paramagnetic">paramagnetic</a>, owing to the presence of unpaired electrons residing in 3d orbitals. Although Fe(III) chloride can be octahedral or tetrahedral (or both, see structure section), all of these forms have five unpaired electrons, one per <a href="/wiki/D-orbital" class="mw-redirect" title="D-orbital">d-orbital</a>. The <a href="/wiki/Spin_states_(d_electrons)" title="Spin states (d electrons)">high spin</a> d<sup>5</sup> electronic configuration requires that d-d electronic transitions are <a href="/wiki/Spin_forbidden" class="mw-redirect" title="Spin forbidden">spin forbidden</a>, in addition to violating the <a href="/wiki/Laporte_rule" title="Laporte rule">Laporte rule</a>. This double forbidden-ness results in its solutions being only pale colored. Or, stated more technically, the optical transitions are non-intense. Aqueous <a href="/wiki/Ferric_sulfate" class="mw-redirect" title="Ferric sulfate">ferric sulfate</a> and <a href="/wiki/Ferric_nitrate" class="mw-redirect" title="Ferric nitrate">ferric nitrate</a>, which contain <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[Fe(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">6</sub>]<sup>3+</sup></span>, are nearly colorless, whereas the chloride solutions are yellow. Thus, the chloride ligands significantly influence the optical properties of the iron center.<sup id="cite_ref-9" class="reference"><a href="#cite_note-9"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Cotton_10-0" class="reference"><a href="#cite_note-Cotton-10"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Structure">Structure</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=2" title="Edit section: Structure"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Iron(III) chloride can exist as an anhydrous material and a series of hydrates, which results in distinct structures. </p> <div class="mw-heading mw-heading3"><h3 id="Anhydrous">Anhydrous</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=3" title="Edit section: Anhydrous"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The <a href="/wiki/Anhydrous" title="Anhydrous">anhydrous</a> compound is a hygroscopic crystalline solid with a melting point of 307.6 °C. The colour depends on the viewing angle: by reflected light, the crystals appear dark green, but by <a href="/wiki/Transmitted_light" class="mw-redirect" title="Transmitted light">transmitted light</a>, they appear purple-red. Anhydrous iron(III) chloride has the <a href="/wiki/Bismuth(III)_iodide" title="Bismuth(III) iodide"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">BiI<sub class="template-chem2-sub">3</sub></span></a> structure, with <a href="/wiki/Octahedral" class="mw-redirect" title="Octahedral">octahedral</a> Fe(III) centres interconnected by two-coordinate chloride <a href="/wiki/Ligand" title="Ligand">ligands</a>.<sup id="cite_ref-str_8-1" class="reference"><a href="#cite_note-str-8"><span class="cite-bracket">[</span>7<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-UllmannFe_11-0" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> </p><p>Iron(III) chloride has a relatively low melting point and boils at around 315 °C. The vapor consists of the <a href="/wiki/Dimer_(chemistry)" class="mw-redirect" title="Dimer (chemistry)">dimer</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Fe<sub class="template-chem2-sub">2</sub>Cl<sub class="template-chem2-sub">6</sub></span>, much like <a href="/wiki/Aluminium_chloride" title="Aluminium chloride">aluminium chloride</a>. This dimer dissociates into the <a href="/wiki/Monomeric" class="mw-redirect" title="Monomeric">monomeric</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub></span> (with D<sub>3h</sub> <a href="/wiki/Symmetry_group" title="Symmetry group">point group</a> <a href="/wiki/Molecular_symmetry" title="Molecular symmetry">molecular symmetry</a>) at higher temperatures, in competition with its reversible decomposition to give <a href="/wiki/Iron(II)_chloride" title="Iron(II) chloride">iron(II) chloride</a> and <a href="/wiki/Chlorine" title="Chlorine">chlorine</a> gas.<sup id="cite_ref-12" class="reference"><a href="#cite_note-12"><span class="cite-bracket">[</span>11<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Hydrates">Hydrates</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=4" title="Edit section: Hydrates"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Ferric chloride form <a href="/wiki/Hydrate" title="Hydrate">hydrates</a> upon exposure to water, reflecting its Lewis acidity. All hydrates exhibit <a href="/wiki/Deliquescence" class="mw-redirect" title="Deliquescence">deliquescence</a>, meaning that they become liquid by absorbing moisture from the air. Hydration invariably gives derivatives of <a href="/wiki/Aquo_complex" class="mw-redirect" title="Aquo complex">aquo complexes</a> with the formula <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[FeCl<sub class="template-chem2-sub">2</sub>(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">4</sub>]<sup class="template-chem2-sup">+</sup></span>. This cation can adopt either <a href="/wiki/Cis-trans_isomer" class="mw-redirect" title="Cis-trans isomer"><i>trans</i> or <i>cis</i></a> <a href="/wiki/Stereochemistry" title="Stereochemistry">stereochemistry</a>, reflecting the relative location of the chloride <a href="/wiki/Ligand" title="Ligand">ligands</a> on the <a href="/wiki/Octahedral_molecular_geometry" title="Octahedral molecular geometry">octahedral</a> Fe center. Four hydrates have been characterized by <a href="/wiki/X-ray_crystallography" title="X-ray crystallography">X-ray crystallography</a>: the dihydrate <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub>·2H<sub>2</sub>O</span>, the disesquihydrate <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub>·2.5H<sub>2</sub>O</span>, the trisesquihydrate <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub>·3.5H<sub>2</sub>O</span>, and finally the hexahydrate <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub>·6H<sub>2</sub>O</span>. These species differ with respect to the stereochemistry of the octahedral iron cation, the identity of the anions, and the presence or absence of <a href="/wiki/Water_of_crystallization" title="Water of crystallization">water of crystallization</a>.<sup id="cite_ref-Cotton_10-1" class="reference"><a href="#cite_note-Cotton-10"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup> The structural formulas are <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[<i>trans</i>−FeCl<sub class="template-chem2-sub">2</sub>(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">4</sub>][FeCl<sub class="template-chem2-sub">4</sub>]</span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[<i>cis</i>−FeCl<sub class="template-chem2-sub">2</sub>(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">4</sub>][FeCl<sub class="template-chem2-sub">4</sub>]·H<sub>2</sub>O</span>, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[<i>cis</i>−FeCl<sub class="template-chem2-sub">2</sub>(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">4</sub>][FeCl<sub class="template-chem2-sub">4</sub>]·H<sub>2</sub>O</span>, and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[<i>trans</i>−FeCl<sub class="template-chem2-sub">2</sub>(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">4</sub>]Cl·2H<sub>2</sub>O</span>. The first three members of this series have the tetrahedral <a href="/wiki/Tetrachloroferrate" title="Tetrachloroferrate">tetrachloroferrate</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[FeCl<sub class="template-chem2-sub">4</sub>]<sup class="template-chem2-sup">−</sup></span>) anion.<sup id="cite_ref-13" class="reference"><a href="#cite_note-13"><span class="cite-bracket">[</span>12<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Solution">Solution</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=5" title="Edit section: Solution"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:Iron(III)_chloride_2.JPG" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4e/Iron%28III%29_chloride_2.JPG/220px-Iron%28III%29_chloride_2.JPG" decoding="async" width="220" height="192" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4e/Iron%28III%29_chloride_2.JPG/330px-Iron%28III%29_chloride_2.JPG 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/4e/Iron%28III%29_chloride_2.JPG/440px-Iron%28III%29_chloride_2.JPG 2x" data-file-width="844" data-file-height="736" /></a><figcaption>A brown, acidic solution of iron(III) chloride.</figcaption></figure> <p>Like the solid hydrates, aqueous solutions of ferric chloride also consist of the octahedral <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[FeCl<sub class="template-chem2-sub">2</sub>(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">4</sub>]<sup class="template-chem2-sup">+</sup></span> of unspecified stereochemistry.<sup id="cite_ref-Cotton_10-2" class="reference"><a href="#cite_note-Cotton-10"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup> Detailed speciation of aqueous solutions of ferric chloride is challenging because the individual components do not have distinctive spectroscopic signatures. Iron(III) complexes, with a high spin d<sup>5</sup> configuration, is kinetically labile, which means that ligands rapidly dissociate and reassociate. A further complication is that these solutions are strongly acidic, as expected for <a href="/wiki/Aquo_complex" class="mw-redirect" title="Aquo complex">aquo complexes</a> of a tricationic metal. Iron aquo complexes are prone to <a href="/wiki/Olation" title="Olation">olation</a>, the formation of <a href="/wiki/Polymeric" class="mw-redirect" title="Polymeric">polymeric</a> <a href="/wiki/Oxo_complex" class="mw-redirect" title="Oxo complex">oxo</a> derivatives. Dilute solutions of ferric chloride produce soluble nanoparticles with <a href="/wiki/Molecular_weight" class="mw-redirect" title="Molecular weight">molecular weight</a> of 10<sup>4</sup>, which exhibit the property of "aging", i.e., the structure change or evolve over the course of days.<sup id="cite_ref-14" class="reference"><a href="#cite_note-14"><span class="cite-bracket">[</span>13<span class="cite-bracket">]</span></a></sup> The polymeric species formed by the hydrolysis of ferric chlorides are key to the use of ferric chloride for water treatment. </p><p>In contrast to the complicated behavior of its aqueous solutions, solutions of iron(III) chloride in <a href="/wiki/Diethyl_ether" title="Diethyl ether">diethyl ether</a> and <a href="/wiki/Tetrahydrofuran" title="Tetrahydrofuran">tetrahydrofuran</a> are well-behaved. Both <a href="/wiki/Ether" title="Ether">ethers</a> form 1:2 <a href="/wiki/Adduct" title="Adduct">adducts</a> of the general formula FeCl<sub>3</sub>(ether)<sub>2</sub>. In these complexes, the iron is pentacoordinate.<sup id="cite_ref-ZaaC_15-0" class="reference"><a href="#cite_note-ZaaC-15"><span class="cite-bracket">[</span>14<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Preparation">Preparation</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=6" title="Edit section: Preparation"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Several hundred tons of anhydrous iron(III) chloride are produced annually. The principal method, called <i>direct chlorination</i>, uses scrap iron as a precursor:<sup id="cite_ref-UllmannFe_11-1" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 Fe + 3 Cl<sub class="template-chem2-sub">2</sub> → 2 FeCl<sub class="template-chem2-sub">3</sub></span></dd></dl> <p>The reaction is conducted at several hundred degrees such that the product is gaseous. Using excess chlorine guarantees that the intermediate ferrous chloride is converted to the ferric state.<sup id="cite_ref-UllmannFe_11-2" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> A similar but laboratory-scale process also has been described.<sup id="cite_ref-16" class="reference"><a href="#cite_note-16"><span class="cite-bracket">[</span>15<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Brauer_17-0" class="reference"><a href="#cite_note-Brauer-17"><span class="cite-bracket">[</span>16<span class="cite-bracket">]</span></a></sup> </p><p><i>Aqueous</i> solutions of iron(III) chloride are also produced industrially from a number of iron precursors, including iron oxides: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Fe<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">3</sub> + 6 HCl + 9 H<sub class="template-chem2-sub">2</sub>O → 2 FeCl<sub class="template-chem2-sub">3</sub>(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">6</sub></span></dd></dl> <p>In complementary route, iron metal can be oxidized by <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">hydrochloric acid</a> followed by chlorination:<sup id="cite_ref-UllmannFe_11-3" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Fe + 2 HCl → FeCl<sub class="template-chem2-sub">2</sub> + H<sub class="template-chem2-sub">2</sub></span></dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">2</sub> + 0.5 Cl<sub class="template-chem2-sub">2</sub> + 6 H<sub class="template-chem2-sub">2</sub>O → FeCl<sub class="template-chem2-sub">3</sub>(H<sub class="template-chem2-sub">2</sub>O)<sub class="template-chem2-sub">6</sub></span></dd></dl> <p>A number of variables apply to these processes, including the oxidation of iron by ferric chloride and the hydration of intermediates.<sup id="cite_ref-UllmannFe_11-4" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> Hydrates of iron(III) chloride do not readily yield anhydrous ferric chloride. Attempted thermal dehydration yields hydrochloric acid and <a href="/wiki/Iron_oxychloride" title="Iron oxychloride">iron oxychloride</a>. In the laboratory, hydrated iron(III) chloride can be converted to the anhydrous form by treatment with <a href="/wiki/Thionyl_chloride" title="Thionyl chloride">thionyl chloride</a><sup id="cite_ref-18" class="reference"><a href="#cite_note-18"><span class="cite-bracket">[</span>17<span class="cite-bracket">]</span></a></sup> or <a href="/wiki/Trimethylsilyl_chloride" title="Trimethylsilyl chloride">trimethylsilyl chloride</a>:<sup id="cite_ref-19" class="reference"><a href="#cite_note-19"><span class="cite-bracket">[</span>18<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub>·6H<sub>2</sub>O + 12 (CH<sub class="template-chem2-sub">3</sub>)<sub class="template-chem2-sub">3</sub>SiCl → FeCl<sub class="template-chem2-sub">3</sub> + 6 ((CH<sub class="template-chem2-sub">3</sub>)<sub class="template-chem2-sub">3</sub>Si)<sub class="template-chem2-sub">2</sub>O + 12 HCl</span></dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub>·6H<sub>2</sub>O + 6 SOCl<sub class="template-chem2-sub">2</sub> → FeCl<sub class="template-chem2-sub">3</sub> + 6 SO<sub class="template-chem2-sub">2</sub> + 12 HCl</span></dd></dl> <div class="mw-heading mw-heading2"><h2 id="Reactions">Reactions</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=7" title="Edit section: Reactions"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Being <a href="/wiki/Spin_states_(d_electrons)" title="Spin states (d electrons)">high spin</a> d<sup>5</sup> electronic configuration iron(III) chlorides are <a href="/wiki/Labile" class="mw-redirect" title="Labile">labile</a>, meaning that its Cl- and H<sub>2</sub>O ligands exchange rapidly with free chloride and water.<sup id="cite_ref-Cotton_10-3" class="reference"><a href="#cite_note-Cotton-10"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-greenwood_20-0" class="reference"><a href="#cite_note-greenwood-20"><span class="cite-bracket">[</span>19<span class="cite-bracket">]</span></a></sup> In contrast to their kinetic lability, iron(III) chlorides are thermodynamically robust, as reflected by the vigorous methods applied to their synthesis, as described above. </p> <div class="mw-heading mw-heading3"><h3 id="Anhydrous_FeCl3">Anhydrous FeCl<sub>3</sub></h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=8" title="Edit section: Anhydrous FeCl3"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Aside from lability, which applies to anhydrous and hydrated forms, the reactivity of anhydrous ferric chloride reveals two trends: It is a <a href="/wiki/Lewis_acid" class="mw-redirect" title="Lewis acid">Lewis acid</a> and an <a href="/wiki/Redox" title="Redox">oxidizing agent</a>.<sup id="cite_ref-EROS_21-0" class="reference"><a href="#cite_note-EROS-21"><span class="cite-bracket">[</span>20<span class="cite-bracket">]</span></a></sup> </p><p>Reactions of anhydrous iron(III) chloride reflect its description as both <a href="/wiki/Oxophilic" class="mw-redirect" title="Oxophilic">oxophilic</a> and a <a href="/wiki/HSAB_theory" title="HSAB theory">hard Lewis acid</a>. Myriad manifestations of the oxophiliicty of iron(III) chloride are available. When heated with <a href="/wiki/Iron(III)_oxide" title="Iron(III) oxide">iron(III) oxide</a> at 350 °C it reacts to give <a href="/wiki/Iron_oxychloride" title="Iron oxychloride">iron oxychloride</a>:<sup id="cite_ref-22" class="reference"><a href="#cite_note-22"><span class="cite-bracket">[</span>21<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub> + Fe<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">3</sub> → 3FeOCl</span></dd></dl> <p>Alkali metal <a href="/wiki/Alkoxide" title="Alkoxide">alkoxides</a> react to give the iron(III) <a href="/wiki/Metal_alkoxide" class="mw-redirect" title="Metal alkoxide">alkoxide complexes</a>. These products have more complicated structures than anhydrous iron(III) chloride.<sup id="cite_ref-23" class="reference"><a href="#cite_note-23"><span class="cite-bracket">[</span>22<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-24" class="reference"><a href="#cite_note-24"><span class="cite-bracket">[</span>23<span class="cite-bracket">]</span></a></sup> In the solid phase a variety of multinuclear complexes have been described for the nominal stoichiometric reaction between <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub></span> and <a href="/wiki/Sodium_ethoxide" title="Sodium ethoxide">sodium ethoxide</a>: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub> + 3 CH<sub class="template-chem2-sub">3</sub>CH<sub class="template-chem2-sub">2</sub>ONa → "Fe(OCH<sub class="template-chem2-sub">2</sub>CH<sub class="template-chem2-sub">3</sub>)<sub class="template-chem2-sub">3</sub>" + 3 NaCl</span></dd></dl> <p>Iron(III) chloride forms a 1:2 <a href="/wiki/Adduct" title="Adduct">adduct</a> with <a href="/wiki/Lewis_base" class="mw-redirect" title="Lewis base">Lewis bases</a> such as <a href="/wiki/Triphenylphosphine_oxide" title="Triphenylphosphine oxide">triphenylphosphine oxide</a>; e.g., <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub>(OP(C<sub class="template-chem2-sub">6</sub>H<sub class="template-chem2-sub">5</sub>)<sub class="template-chem2-sub">3</sub>)<sub class="template-chem2-sub">2</sub></span>. The related 1:2 complex <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub>(OEt<sub class="template-chem2-sub">2</sub>)<sub class="template-chem2-sub">2</sub>, where Et = C<sub class="template-chem2-sub">2</sub>H<sub class="template-chem2-sub">5</sub>)</span>, has been crystallized from ether solution.<sup id="cite_ref-ZaaC_15-1" class="reference"><a href="#cite_note-ZaaC-15"><span class="cite-bracket">[</span>14<span class="cite-bracket">]</span></a></sup> </p><p>Iron(III) chloride also reacts with <a href="/wiki/Tetraethylammonium_chloride" title="Tetraethylammonium chloride">tetraethylammonium chloride</a> to give the yellow salt of the <a href="/wiki/Tetrachloroferrate" title="Tetrachloroferrate">tetrachloroferrate</a> ion (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">(Et<sub class="template-chem2-sub">4</sub>N)[FeCl<sub class="template-chem2-sub">4</sub>]</span>). Similarly, combining FeCl<sub>3</sub> with NaCl and KCl gives <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Na[FeCl<sub class="template-chem2-sub">4</sub>]</span> and <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">K[FeCl<sub class="template-chem2-sub">4</sub>]</span>, respectively.<sup id="cite_ref-25" class="reference"><a href="#cite_note-25"><span class="cite-bracket">[</span>24<span class="cite-bracket">]</span></a></sup> </p><p>In addition to these simple <a href="/wiki/Stoichiometric" class="mw-redirect" title="Stoichiometric">stoichiometric</a> reactions, the Lewis acidity of ferric chloride enables its use in a variety of acid-<a href="/wiki/Catalysis" title="Catalysis">catalyzed</a> reactions as described below in the section on organic chemistry.<sup id="cite_ref-UllmannFe_11-5" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> </p><p>In terms of its being an oxidant, iron(III) chloride oxidizes iron powder to form iron(II) chloride via a <a href="/wiki/Comproportionation" title="Comproportionation">comproportionation</a> reaction:<sup id="cite_ref-UllmannFe_11-6" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 FeCl<sub class="template-chem2-sub">3</sub> + Fe → 3 FeCl<sub class="template-chem2-sub">2</sub></span></dd></dl> <p>A traditional synthesis of anhydrous <a href="/wiki/Ferrous_chloride" class="mw-redirect" title="Ferrous chloride">ferrous chloride</a> is the reduction of <a href="/wiki/Ferric_chloride" class="mw-redirect" title="Ferric chloride">FeCl<sub>3</sub></a> with <a href="/wiki/Chlorobenzene" title="Chlorobenzene">chlorobenzene</a>:<sup id="cite_ref-26" class="reference"><a href="#cite_note-26"><span class="cite-bracket">[</span>25<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 FeCl<sub class="template-chem2-sub">3</sub> + C<sub class="template-chem2-sub">6</sub>H<sub class="template-chem2-sub">5</sub>Cl → 2 FeCl<sub class="template-chem2-sub">2</sub> + C<sub class="template-chem2-sub">6</sub>H<sub class="template-chem2-sub">4</sub>Cl<sub class="template-chem2-sub">2</sub> + HCl</span></dd></dl> <p>iron(III) chloride releases chlorine gas when heated above 160 °C, generating <a href="/wiki/Ferrous_chloride" class="mw-redirect" title="Ferrous chloride">ferrous chloride</a>:<sup id="cite_ref-Brauer_17-1" class="reference"><a href="#cite_note-Brauer-17"><span class="cite-bracket">[</span>16<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2FeCl<sub class="template-chem2-sub">3</sub> → 2FeCl<sub class="template-chem2-sub">2</sub> + Cl<sub class="template-chem2-sub">2</sub></span></dd></dl> <p>To suppress this reaction, the preparation of iron(III) chloride requires an excess of chlorinating agent, as discussed above.<sup id="cite_ref-Brauer_17-2" class="reference"><a href="#cite_note-Brauer-17"><span class="cite-bracket">[</span>16<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-UllmannFe_11-7" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Hydrated_FeCl3">Hydrated FeCl<sub>3</sub></h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=9" title="Edit section: Hydrated FeCl3"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Unlike the anhydrous material, hydrated ferric chloride is not a particularly strong Lewis acid since water ligands have quenched the Lewis acidity by binding to Fe(III). </p><p>Like the anhydrous material, hydrated ferric chloride is oxophilic. For example, <a href="/wiki/Oxalic_acid" title="Oxalic acid">oxalate</a> salts react rapidly with aqueous iron(III) chloride to give <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">[Fe(C<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">4</sub>)<sub class="template-chem2-sub">3</sub>]<sup>3−</sup></span>, known as <a href="/wiki/Ferrioxalate" title="Ferrioxalate">ferrioxalate</a>. Other <a href="/wiki/Carboxylate" title="Carboxylate">carboxylate</a> sources, e.g., <a href="/wiki/Citric_acid" title="Citric acid">citrate</a> and <a href="/wiki/Tartaric_acid" title="Tartaric acid">tartrate</a>, bind as well to give <a href="/wiki/Carboxylate_complex" class="mw-redirect" title="Carboxylate complex">carboxylate complexes</a>. The affinity of iron(III) for oxygen ligands was the basis of qualitative tests for phenols. Although superseded by spectroscopic methods, the <a href="/wiki/Ferric_chloride_test" title="Ferric chloride test">ferric chloride test</a> is a traditional <a href="/wiki/Colorimetric" class="mw-redirect" title="Colorimetric">colorimetric</a> test.<sup id="cite_ref-27" class="reference"><a href="#cite_note-27"><span class="cite-bracket">[</span>26<span class="cite-bracket">]</span></a></sup> The affinity of iron(III) for phenols is exploited in the <a href="/wiki/Trinder_spot_test" title="Trinder spot test">Trinder spot test</a>.<sup id="cite_ref-28" class="reference"><a href="#cite_note-28"><span class="cite-bracket">[</span>27<span class="cite-bracket">]</span></a></sup> </p><p>Aqueous iron(III) chloride serves as a one-electron oxidant illustrated by its reaction with <a href="/wiki/Copper(I)_chloride" title="Copper(I) chloride">copper(I) chloride</a> to give <a href="/wiki/Copper(II)_chloride" title="Copper(II) chloride">copper(II) chloride</a> and iron(II) chloride. </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub> + CuCl → FeCl<sub class="template-chem2-sub">2</sub> + CuCl<sub class="template-chem2-sub">2</sub></span></dd></dl> <p>This fundamental reaction is relevant to the use of ferric chloride solutions in etching copper. </p> <div class="mw-heading mw-heading3"><h3 id="Organometallic_chemistry">Organometallic chemistry</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=10" title="Edit section: Organometallic chemistry"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The interaction of anhydrous iron(III) chloride with <a href="/wiki/Organolithium" class="mw-redirect" title="Organolithium">organolithium</a> and <a href="/wiki/Organomagnesium_compound" class="mw-redirect" title="Organomagnesium compound">organomagnesium compounds</a> has been examined often. These studies are enabled because of the solubility of FeCl<sub>3</sub> in ethereal solvents, which avoids the possibility of hydrolysis of the <a href="/wiki/Nucleophilic" class="mw-redirect" title="Nucleophilic">nucleophilic</a> <a href="/wiki/Alkylating_agent" class="mw-redirect" title="Alkylating agent">alkylating agents</a>. Such studies may be relevant to the mechanism of FeCl<sub>3</sub>-catalyzed <a href="/wiki/Cross-coupling_reaction" title="Cross-coupling reaction">cross-coupling reactions</a>.<sup id="cite_ref-Byers_29-0" class="reference"><a href="#cite_note-Byers-29"><span class="cite-bracket">[</span>28<span class="cite-bracket">]</span></a></sup> The isolation of organoiron(III) intermediates requires low-temperature reactions, lest the [FeR<sub>4</sub>]<sup>−</sup> intermediates degrade. Using <a href="/wiki/Methylmagnesium_bromide" class="mw-redirect" title="Methylmagnesium bromide">methylmagnesium bromide</a> as the alkylation agent, salts of Fe(CH<sub>3</sub>)<sub>4</sub>]<sup>−</sup> have been isolated.<sup id="cite_ref-30" class="reference"><a href="#cite_note-30"><span class="cite-bracket">[</span>29<span class="cite-bracket">]</span></a></sup> Illustrating the sensitivity of these reactions, <a href="/wiki/Methyl_lithium" class="mw-redirect" title="Methyl lithium">methyl lithium</a> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">LiCH<sub class="template-chem2-sub">3</sub></span> reacts with iron(III) chloride to give lithium <a href="/wiki/Tetrachloroferrate" title="Tetrachloroferrate">tetrachloroferrate</a>(II) <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Li<sub class="template-chem2-sub">2</sub>[FeCl<sub class="template-chem2-sub">4</sub>]</span>:<sup id="cite_ref-31" class="reference"><a href="#cite_note-31"><span class="cite-bracket">[</span>30<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 FeCl<sub class="template-chem2-sub">3</sub> + LiCH<sub class="template-chem2-sub">3</sub> → FeCl<sub class="template-chem2-sub">2</sub> + Li[FeCl<sub class="template-chem2-sub">4</sub>] + 0.5 CH<sub class="template-chem2-sub">3</sub>CH<sub class="template-chem2-sub">3</sub></span></dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Li[FeCl<sub class="template-chem2-sub">4</sub>] + LiCH<sub class="template-chem2-sub">3</sub> → Li<sub class="template-chem2-sub">2</sub>[FeCl<sub class="template-chem2-sub">4</sub>] + 0.5 CH<sub class="template-chem2-sub">3</sub>CH<sub class="template-chem2-sub">3</sub></span></dd></dl> <p>To a significant extent, <a href="/wiki/Iron(III)_acetylacetonate" class="mw-redirect" title="Iron(III) acetylacetonate">iron(III) acetylacetonate</a> and related beta-diketonate complexes are more widely used than FeCl<sub>3</sub> as ether-soluble sources of ferric ion.<sup id="cite_ref-EROS_21-1" class="reference"><a href="#cite_note-EROS-21"><span class="cite-bracket">[</span>20<span class="cite-bracket">]</span></a></sup> These diketonate complexes have the advantages that they do not form hydrates, unlike iron(III) chloride, and they are more soluble in relevant solvents.<sup id="cite_ref-Byers_29-1" class="reference"><a href="#cite_note-Byers-29"><span class="cite-bracket">[</span>28<span class="cite-bracket">]</span></a></sup> <a href="/wiki/Cyclopentadienyl_magnesium_bromide" title="Cyclopentadienyl magnesium bromide">Cyclopentadienyl magnesium bromide</a> undergoes a complex reaction with iron(III) chloride, resulting in <a href="/wiki/Ferrocene" title="Ferrocene">ferrocene</a>:<sup id="cite_ref-32" class="reference"><a href="#cite_note-32"><span class="cite-bracket">[</span>31<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">3 C<sub class="template-chem2-sub">5</sub>H<sub class="template-chem2-sub">5</sub>MgBr + FeCl<sub class="template-chem2-sub">3</sub> → Fe(C<sub class="template-chem2-sub">5</sub>H<sub class="template-chem2-sub">5</sub>)<sub class="template-chem2-sub">2</sub> + 1/n (C<sub class="template-chem2-sub">5</sub>H<sub class="template-chem2-sub">5</sub>)<sub class="template-chem2-sub">n</sub> + 3 MgBrCl</span></dd></dl> <p>This conversion, although not of practical value, was important in the history of <a href="/wiki/Organometallic_chemistry" title="Organometallic chemistry">organometallic chemistry</a> where ferrocene is emblematic of the field.<sup id="cite_ref-Pauson2001_33-0" class="reference"><a href="#cite_note-Pauson2001-33"><span class="cite-bracket">[</span>32<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Uses">Uses</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=11" title="Edit section: Uses"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-heading mw-heading3"><h3 id="Water_treatment">Water treatment</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=12" title="Edit section: Water treatment"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The largest applications of iron(III) chloride are <a href="/wiki/Sewage_treatment" title="Sewage treatment">sewage treatment</a> and <a href="/wiki/Water_treatment" title="Water treatment">drinking water production</a>. By forming highly dispersed networks of Fe-O-Fe containing materials, ferric chlorides serve as coagulant and flocculants.<sup id="cite_ref-wtcbrochure_34-0" class="reference"><a href="#cite_note-wtcbrochure-34"><span class="cite-bracket">[</span>33<span class="cite-bracket">]</span></a></sup> In this application, an aqueous solution of <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub></span> is treated with base to form a <a href="/wiki/Flocculation" title="Flocculation">floc</a> of <a href="/wiki/Iron(III)_hydroxide" class="mw-redirect" title="Iron(III) hydroxide">iron(III) hydroxide</a> (<link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Fe(OH)<sub class="template-chem2-sub">3</sub></span>), also formulated as FeO(OH) (<a href="/wiki/Ferrihydrite" title="Ferrihydrite">ferrihydrite</a>). This floc facilitates the separation of suspended materials, clarifying the water.<sup id="cite_ref-UllmannFe_11-8" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> </p><p>Iron(III) chloride is also used to remove soluble <a href="/wiki/Phosphate" title="Phosphate">phosphate</a> from wastewater. <a href="/wiki/Iron(III)_phosphate" title="Iron(III) phosphate">Iron(III) phosphate</a> is <a href="/wiki/Insoluble" class="mw-redirect" title="Insoluble">insoluble</a> and thus precipitates as a solid.<sup id="cite_ref-35" class="reference"><a href="#cite_note-35"><span class="cite-bracket">[</span>34<span class="cite-bracket">]</span></a></sup> One potential advantage of its use in water treatment, is that the ferric ion oxidizes (deodorizes) <a href="/wiki/Hydrogen_sulfide" title="Hydrogen sulfide">hydrogen sulfide</a>.<sup id="cite_ref-36" class="reference"><a href="#cite_note-36"><span class="cite-bracket">[</span>35<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Etching_and_metal_cleaning">Etching and metal cleaning</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=13" title="Edit section: Etching and metal cleaning"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>It is also used as a <a href="/wiki/Leaching_(chemistry)" title="Leaching (chemistry)">leaching</a> agent in chloride hydrometallurgy,<sup id="cite_ref-37" class="reference"><a href="#cite_note-37"><span class="cite-bracket">[</span>36<span class="cite-bracket">]</span></a></sup> for example in the production of Si from FeSi (Silgrain process by <a href="/wiki/Elkem" title="Elkem">Elkem</a>).<sup id="cite_ref-38" class="reference"><a href="#cite_note-38"><span class="cite-bracket">[</span>37<span class="cite-bracket">]</span></a></sup> </p><p>In another commercial application, a solution of iron(III) chloride is useful for etching <a href="/wiki/Copper" title="Copper">copper</a> according to the following equation: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 FeCl<sub class="template-chem2-sub">3</sub> + Cu → 2 FeCl<sub class="template-chem2-sub">2</sub> + CuCl<sub class="template-chem2-sub">2</sub></span></dd></dl> <p>The soluble <a href="/wiki/Copper(II)_chloride" title="Copper(II) chloride">copper(II) chloride</a> is rinsed away, leaving a copper pattern. This chemistry is used in the production of <a href="/wiki/Printed_circuit_boards" class="mw-redirect" title="Printed circuit boards">printed circuit boards</a> (PCB).<sup id="cite_ref-greenwood_20-1" class="reference"><a href="#cite_note-greenwood-20"><span class="cite-bracket">[</span>19<span class="cite-bracket">]</span></a></sup> </p><p>Iron(III) chloride is used in many other hobbies involving metallic objects.<sup id="cite_ref-39" class="reference"><a href="#cite_note-39"><span class="cite-bracket">[</span>38<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-40" class="reference"><a href="#cite_note-40"><span class="cite-bracket">[</span>39<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-41" class="reference"><a href="#cite_note-41"><span class="cite-bracket">[</span>40<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-42" class="reference"><a href="#cite_note-42"><span class="cite-bracket">[</span>41<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-43" class="reference"><a href="#cite_note-43"><span class="cite-bracket">[</span>42<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Organic_chemistry">Organic chemistry</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=14" title="Edit section: Organic chemistry"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size mw-halign-left" typeof="mw:File/Thumb"><a href="/wiki/File:UJIMUV.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/UJIMUV.jpg/220px-UJIMUV.jpg" decoding="async" width="220" height="335" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/04/UJIMUV.jpg/330px-UJIMUV.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/04/UJIMUV.jpg/440px-UJIMUV.jpg 2x" data-file-width="1557" data-file-height="2371" /></a><figcaption>Structure of FeCl<sub>3</sub>(diethylether)<sub>2</sub>. Color code: Cl=green,Fe = blue, O = red.</figcaption></figure> <p>In industry, iron(III) chloride is used as a catalyst for the reaction of <a href="/wiki/Ethylene" title="Ethylene">ethylene</a> with <a href="/wiki/Chlorine" title="Chlorine">chlorine</a>, forming ethylene dichloride (<a href="/wiki/1,2-dichloroethane" class="mw-redirect" title="1,2-dichloroethane">1,2-dichloroethane</a>):<sup id="cite_ref-44" class="reference"><a href="#cite_note-44"><span class="cite-bracket">[</span>43<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">H<sub class="template-chem2-sub">2</sub>C=CH<sub class="template-chem2-sub">2</sub> + Cl<sub class="template-chem2-sub">2</sub> → ClCH<sub class="template-chem2-sub">2</sub>CH<sub class="template-chem2-sub">2</sub>Cl</span></dd></dl> <p>Ethylene dichloride is a <a href="/wiki/Commodity_chemicals" title="Commodity chemicals">commodity chemical</a>, which is mainly used for the industrial production of <a href="/wiki/Vinyl_chloride" title="Vinyl chloride">vinyl chloride</a>, the <a href="/wiki/Monomer" title="Monomer">monomer</a> for making <a href="/wiki/Polyvinyl_chloride" title="Polyvinyl chloride">PVC</a>.<sup id="cite_ref-45" class="reference"><a href="#cite_note-45"><span class="cite-bracket">[</span>44<span class="cite-bracket">]</span></a></sup> </p><p>Illustrating it use as a <a href="/wiki/Lewis_acid" class="mw-redirect" title="Lewis acid">Lewis acid</a>, iron(III) chloride <a href="/wiki/Catalyst" class="mw-redirect" title="Catalyst">catalyses</a> <a href="/wiki/Electrophilic_aromatic_substitution" title="Electrophilic aromatic substitution">electrophilic aromatic substitution</a> and <a href="/wiki/Chlorination_reaction" class="mw-redirect" title="Chlorination reaction">chlorinations</a>. In this role, its function is similar to that of <a href="/wiki/Aluminium_chloride" title="Aluminium chloride">aluminium chloride</a>. In some cases, mixtures of the two are used.<sup id="cite_ref-46" class="reference"><a href="#cite_note-46"><span class="cite-bracket">[</span>45<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading4"><h4 id="Organic_synthesis_research">Organic synthesis research</h4><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=15" title="Edit section: Organic synthesis research"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Although iron(III) chlorides are seldom used in practical <a href="/wiki/Organic_synthesis" title="Organic synthesis">organic synthesis</a>, they have received considerable attention as <a href="/wiki/Reagent" title="Reagent">reagents</a> because they are inexpensive, earth abundant, and relatively nontoxic. Many experiments probe both its redox activity and its Lewis acidity.<sup id="cite_ref-EROS_21-2" class="reference"><a href="#cite_note-EROS-21"><span class="cite-bracket">[</span>20<span class="cite-bracket">]</span></a></sup> For example, iron(III) chloride oxidizes naphthols to naphthoquinones:<sup id="cite_ref-EROS_21-3" class="reference"><a href="#cite_note-EROS-21"><span class="cite-bracket">[</span>20<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-47" class="reference"><a href="#cite_note-47"><span class="cite-bracket">[</span>46<span class="cite-bracket">]</span></a></sup> 3-Alkyl<a href="/wiki/Thiophene" title="Thiophene">thiophenes</a> are polymerized to <a href="/wiki/Polythiophene" title="Polythiophene">polythiophenes</a> upon treatment with ferric chloride.<sup id="cite_ref-48" class="reference"><a href="#cite_note-48"><span class="cite-bracket">[</span>47<span class="cite-bracket">]</span></a></sup> Iron(III) chloride has been shown to promote C-C <a href="/wiki/Coupling_reaction" title="Coupling reaction">coupling reaction</a>.<sup id="cite_ref-49" class="reference"><a href="#cite_note-49"><span class="cite-bracket">[</span>48<span class="cite-bracket">]</span></a></sup> </p><p>Several reagents have been developed based on <a href="/wiki/Catalyst_support" title="Catalyst support">supported</a> iron(III) chloride. On <a href="/wiki/Silica_gel" title="Silica gel">silica gel</a>, the anhydrous salt has been applied to certain <a href="/wiki/Dehydration_reaction" title="Dehydration reaction">dehydration</a> and <a href="/wiki/Pinacol_rearrangement" title="Pinacol rearrangement">pinacol-type rearrangement</a> reactions. A similar reagent but moistened induces hydrolysis or <a href="/wiki/Epimerization" class="mw-redirect" title="Epimerization">epimerization</a> reactions.<sup id="cite_ref-50" class="reference"><a href="#cite_note-50"><span class="cite-bracket">[</span>49<span class="cite-bracket">]</span></a></sup> On <a href="/wiki/Alumina" class="mw-redirect" title="Alumina">alumina</a>, ferric chloride has been shown to accelerate <a href="/wiki/Ene_reaction" title="Ene reaction">ene reactions</a>.<sup id="cite_ref-51" class="reference"><a href="#cite_note-51"><span class="cite-bracket">[</span>50<span class="cite-bracket">]</span></a></sup> </p><p>When pretreated with <a href="/wiki/Sodium_hydride" title="Sodium hydride">sodium hydride</a>, iron(III) chloride gives a hydride <a href="/wiki/Reducing_agent" title="Reducing agent">reducing agent</a> that convert <a href="/wiki/Alkene" title="Alkene">alkenes</a> and <a href="/wiki/Ketone" title="Ketone">ketones</a> into <a href="/wiki/Alkane" title="Alkane">alkanes</a> and <a href="/wiki/Alcohol_(chemistry)" title="Alcohol (chemistry)">alcohols</a>, respectively.<sup id="cite_ref-52" class="reference"><a href="#cite_note-52"><span class="cite-bracket">[</span>51<span class="cite-bracket">]</span></a></sup> </p> <figure class="mw-halign-center" typeof="mw:File"><a href="/wiki/File:FeCl3oxidation.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/41/FeCl3oxidation.svg/386px-FeCl3oxidation.svg.png" decoding="async" width="386" height="106" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/41/FeCl3oxidation.svg/579px-FeCl3oxidation.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/41/FeCl3oxidation.svg/772px-FeCl3oxidation.svg.png 2x" data-file-width="375" data-file-height="103" /></a><figcaption></figcaption></figure> <div class="mw-heading mw-heading3"><h3 id="Histology">Histology</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=16" title="Edit section: Histology"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Iron(III) chloride is a component of useful stains, such as <a href="/wiki/Carnoy%27s_solution" title="Carnoy's solution">Carnoy's solution</a>, a <a href="/wiki/Fixation_(histology)" title="Fixation (histology)">histological fixative</a> with many applications. Also, it is used to prepare <a href="/wiki/Verhoeff%27s_stain" title="Verhoeff's stain">Verhoeff's stain</a>.<sup id="cite_ref-ucdavis_53-0" class="reference"><a href="#cite_note-ucdavis-53"><span class="cite-bracket">[</span>52<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Natural_occurrence">Natural occurrence</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=17" title="Edit section: Natural occurrence"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Like many metal halides, <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub></span> naturally occurs as a trace mineral. The rare mineral <b>molysite</b> is usually associated with <a href="/wiki/Volcano" title="Volcano">volcanoes</a> and <a href="/wiki/Fumarole" title="Fumarole">fumaroles</a>.<sup id="cite_ref-54" class="reference"><a href="#cite_note-54"><span class="cite-bracket">[</span>53<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-IMA_55-0" class="reference"><a href="#cite_note-IMA-55"><span class="cite-bracket">[</span>54<span class="cite-bracket">]</span></a></sup> </p><p><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub></span>-based aerosol are produced by a reaction between iron-rich dust and <a href="/wiki/Hydrochloric_acid" title="Hydrochloric acid">hydrochloric acid</a> from sea salt. This iron salt aerosol causes about 1-5% of naturally-occurring oxidization of <a href="/wiki/Methane" title="Methane">methane</a> and is thought to have a range of cooling effects; thus, it has been proposed as a catalyst for <a href="/wiki/Atmospheric_methane_removal" title="Atmospheric methane removal">Atmospheric Methane Removal</a>.<sup id="cite_ref-56" class="reference"><a href="#cite_note-56"><span class="cite-bracket">[</span>55<span class="cite-bracket">]</span></a></sup> </p><p>The clouds of <a href="/wiki/Venus" title="Venus">Venus</a> are hypothesized to contain approximately 1% <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub></span> dissolved in <a href="/wiki/Sulfuric_acid" title="Sulfuric acid">sulfuric acid</a>.<sup id="cite_ref-kras006_57-0" class="reference"><a href="#cite_note-kras006-57"><span class="cite-bracket">[</span>56<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-58" class="reference"><a href="#cite_note-58"><span class="cite-bracket">[</span>57<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Safety">Safety</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=18" title="Edit section: Safety"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Iron(III) chlorides are widely used in the <a href="/wiki/Water_treatment" title="Water treatment">treatment of drinking water</a>,<sup id="cite_ref-UllmannFe_11-9" class="reference"><a href="#cite_note-UllmannFe-11"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> so they pose few problems as poisons, at low concentrations.<sup class="noprint Inline-Template" style="white-space:nowrap;">[<i><a href="/wiki/Wikipedia:No_original_research#Synthesis_of_published_material" title="Wikipedia:No original research"><span title="The material near this tag may be based upon an improper synthesis of sources. (June 2024)">improper synthesis?</span></a></i>]</sup> Nonetheless, anhydrous iron(III) chloride, as well as concentrated <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap"><a href="/wiki/Iron" title="Iron">Fe</a><a href="/wiki/Chloride" title="Chloride">Cl</a><sub class="template-chem2-sub">3</sub></span> aqueous solution, is highly <a href="/wiki/Corrosive_substance" class="mw-redirect" title="Corrosive substance">corrosive</a>, and must be handled using proper protective equipment.<sup id="cite_ref-EROS_21-4" class="reference"><a href="#cite_note-EROS-21"><span class="cite-bracket">[</span>20<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Notes">Notes</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=19" title="Edit section: Notes"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist"> <div class="mw-references-wrap"><ol class="references"> <li id="cite_note-7"><span class="mw-cite-backlink"><b><a href="#cite_ref-7">^</a></b></span> <span class="reference-text">An alternative GHS classification from the Japanese GHS Inter-ministerial Committee (2006)<sup id="cite_ref-6" class="reference"><a href="#cite_note-6"><span class="cite-bracket">[</span>6<span class="cite-bracket">]</span></a></sup> notes the possibility of respiratory tract irritation from <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">FeCl<sub class="template-chem2-sub">3</sub></span> and differs slightly in other respects from the classification used here.</span> </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="References">References</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Iron(III)_chloride&action=edit&section=20" title="Edit section: References"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1239543626"><div class="reflist reflist-columns references-column-width" style="column-width: 30em;"> <ol class="references"> <li id="cite_note-crc-1"><span class="mw-cite-backlink">^ <a href="#cite_ref-crc_1-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-crc_1-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-crc_1-2"><sup><i><b>c</b></i></sup></a> <a href="#cite_ref-crc_1-3"><sup><i><b>d</b></i></sup></a> <a href="#cite_ref-crc_1-4"><sup><i><b>e</b></i></sup></a> <a href="#cite_ref-crc_1-5"><sup><i><b>f</b></i></sup></a></span> <span class="reference-text"><style data-mw-deduplicate="TemplateStyles:r1238218222">.mw-parser-output cite.citation{font-style:inherit;word-wrap:break-word}.mw-parser-output .citation q{quotes:"\"""\"""'""'"}.mw-parser-output .citation:target{background-color:rgba(0,127,255,0.133)}.mw-parser-output .id-lock-free.id-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/6/65/Lock-green.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-subscription.id-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-free a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-limited a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-registration a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain;padding:0 1em 0 0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite id="CITEREFHaynes2011" class="citation book cs1">Haynes WM, ed. (2011). <i><a href="/wiki/CRC_Handbook_of_Chemistry_and_Physics" title="CRC Handbook of Chemistry and Physics">CRC Handbook of Chemistry and Physics</a></i> (92nd ed.). Boca Raton, FL: <a href="/wiki/CRC_Press" title="CRC Press">CRC Press</a>. p. 4.69. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/1-4398-5511-0" title="Special:BookSources/1-4398-5511-0"><bdi>1-4398-5511-0</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=CRC+Handbook+of+Chemistry+and+Physics&rft.place=Boca+Raton%2C+FL&rft.pages=4.69&rft.edition=92nd&rft.pub=CRC+Press&rft.date=2011&rft.isbn=1-4398-5511-0&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></span> </li> <li id="cite_note-2"><span class="mw-cite-backlink"><b><a href="#cite_ref-2">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFHaynes2011" class="citation book cs1">Haynes WM, ed. 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Boca Raton, FL: <a href="/wiki/CRC_Press" title="CRC Press">CRC Press</a>. p. 4.133. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/1-4398-5511-0" title="Special:BookSources/1-4398-5511-0"><bdi>1-4398-5511-0</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=CRC+Handbook+of+Chemistry+and+Physics&rft.place=Boca+Raton%2C+FL&rft.pages=4.133&rft.edition=92nd&rft.pub=CRC+Press&rft.date=2011&rft.isbn=1-4398-5511-0&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></span> </li> <li id="cite_note-3"><span class="mw-cite-backlink"><b><a href="#cite_ref-3">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFNIOSH_Pocket_Guide_to_Chemical_Hazards" class="citation web cs1">NIOSH Pocket Guide to Chemical Hazards. <a rel="nofollow" class="external text" href="https://www.cdc.gov/niosh/npg/npgd0346.html">"#0346"</a>. <a href="/wiki/National_Institute_for_Occupational_Safety_and_Health" title="National Institute for Occupational Safety and Health">National Institute for Occupational Safety and Health</a> (NIOSH).</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=unknown&rft.btitle=%230346&rft.pub=National+Institute+for+Occupational+Safety+and+Health+%28NIOSH%29&rft.au=NIOSH+Pocket+Guide+to+Chemical+Hazards&rft_id=https%3A%2F%2Fwww.cdc.gov%2Fniosh%2Fnpg%2Fnpgd0346.html&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></span> </li> <li id="cite_note-4"><span class="mw-cite-backlink"><b><a href="#cite_ref-4">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation cs2"><a rel="nofollow" class="external text" href="http://www.epa.govt.nz/search-databases/Pages/ccid-details.aspx?SubstanceID=10764"><i>HSNO Chemical Classification Information Database</i></a>, New Zealand Environmental Risk Management Authority<span class="reference-accessdate">, retrieved <span class="nowrap">19 Sep</span> 2010</span></cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=HSNO+Chemical+Classification+Information+Database&rft.pub=New+Zealand+Environmental+Risk+Management+Authority&rft_id=http%3A%2F%2Fwww.epa.govt.nz%2Fsearch-databases%2FPages%2Fccid-details.aspx%3FSubstanceID%3D10764&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></span> </li> <li id="cite_note-5"><span class="mw-cite-backlink"><b><a href="#cite_ref-5">^</a></b></span> <span class="reference-text"><a rel="nofollow" class="external text" href="http://webcomm.bcd.tamhsc.edu/bcdfacilities/msds9.html">Various suppliers</a>, collated by the Baylor College of Dentistry, <a href="/wiki/Texas_A%26M_University" title="Texas A&M University">Texas A&M University</a>. 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Crystallogr.</a></i> <b>22</b> (2): 173–180. <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/1989JApCr..22..173H">1989JApCr..22..173H</a>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1107%2FS0021889888013913">10.1107/S0021889888013913</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=J.+Appl.+Crystallogr.&rft.atitle=Structure+refinement+of+an+FeCl%3Csub%3E3%3C%2Fsub%3E+crystal+using+a+thin+plate+sample&rft.volume=22&rft.issue=2&rft.pages=173-180&rft.date=1989&rft_id=info%3Adoi%2F10.1107%2FS0021889888013913&rft_id=info%3Abibcode%2F1989JApCr..22..173H&rft.aulast=Hashimoto&rft.aufirst=S&rft.au=Forster%2C+K&rft.au=Moss%2C+SC&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></span> </li> <li id="cite_note-9"><span class="mw-cite-backlink"><b><a href="#cite_ref-9">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFHousecroftSharpe2012" class="citation book cs1">Housecroft CE, Sharpe AG (2012). <i>Inorganic Chemistry</i> (4th ed.). 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Cotton (2018). "Iron(III) Chloride and Its Coordination Chemistry". <i>Journal of Coordination Chemistry</i>. <b>71</b> (21): 3415–3443. <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%2F00958972.2018.1519188">10.1080/00958972.2018.1519188</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:105925459">105925459</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Journal+of+Coordination+Chemistry&rft.atitle=Iron%28III%29+Chloride+and+Its+Coordination+Chemistry&rft.volume=71&rft.issue=21&rft.pages=3415-3443&rft.date=2018&rft_id=info%3Adoi%2F10.1080%2F00958972.2018.1519188&rft_id=https%3A%2F%2Fapi.semanticscholar.org%2FCorpusID%3A105925459%23id-name%3DS2CID&rft.au=Simon+A.+Cotton&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></span> </li> <li id="cite_note-UllmannFe-11"><span class="mw-cite-backlink">^ <a href="#cite_ref-UllmannFe_11-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-2"><sup><i><b>c</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-3"><sup><i><b>d</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-4"><sup><i><b>e</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-5"><sup><i><b>f</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-6"><sup><i><b>g</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-7"><sup><i><b>h</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-8"><sup><i><b>i</b></i></sup></a> <a href="#cite_ref-UllmannFe_11-9"><sup><i><b>j</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWildermuthStarkFriedrichEbenhöch2000" class="citation book cs1">Wildermuth E, Stark H, Friedrich G, Ebenhöch FL, Kühborth B, Silver J, Rituper R (2000). "Iron Compounds". <i>Ullmann's Encyclopedia of Industrial Chemistry</i>. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1002%2F14356007.a14_591">10.1002/14356007.a14_591</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/3527306730" title="Special:BookSources/3527306730"><bdi>3527306730</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Iron+Compounds&rft.btitle=Ullmann%27s+Encyclopedia+of+Industrial+Chemistry&rft.date=2000&rft_id=info%3Adoi%2F10.1002%2F14356007.a14_591&rft.isbn=3527306730&rft.aulast=Wildermuth&rft.aufirst=Egon&rft.au=Stark%2C+Hans&rft.au=Friedrich%2C+Gabriele&rft.au=Ebenh%C3%B6ch%2C+Franz+Ludwig&rft.au=K%C3%BChborth%2C+Brigitte&rft.au=Silver%2C+Jack&rft.au=Rituper%2C+Rafael&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></span> </li> <li id="cite_note-12"><span class="mw-cite-backlink"><b><a href="#cite_ref-12">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFHollemanWiberg2001" class="citation book cs1">Holleman AF, Wiberg E (2001). 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(1990). <i><a href="/wiki/CRC_Handbook_of_Chemistry_and_Physics" title="CRC Handbook of Chemistry and Physics">CRC Handbook of Chemistry and Physics</a></i> (71st ed.). Ann Arbor, Michigan, US: CRC Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/9780849304712" title="Special:BookSources/9780849304712"><bdi>9780849304712</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=CRC+Handbook+of+Chemistry+and+Physics&rft.place=Ann+Arbor%2C+Michigan%2C+US&rft.edition=71st&rft.pub=CRC+Press&rft.date=1990&rft.isbn=9780849304712&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFStecherFinkelSiegmund1960" class="citation book cs1">Stecher PG, Finkel MJ, Siegmund OH, eds. (1960). <i>The Merck Index of Chemicals and Drugs</i> (7th ed.). Rahway, New Jersey, US: Merck & Co.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=The+Merck+Index+of+Chemicals+and+Drugs&rft.place=Rahway%2C+New+Jersey%2C+US&rft.edition=7th&rft.pub=Merck+%26+Co&rft.date=1960&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFNicholls1974" class="citation book cs1">Nicholls D (1974). <i>Complexes and First-Row Transition Elements, Macmillan Press, London, 1973</i>. A Macmillan chemistry text. London: Macmillan Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/9780333170885" title="Special:BookSources/9780333170885"><bdi>9780333170885</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Complexes+and+First-Row+Transition+Elements%2C+Macmillan+Press%2C+London%2C+1973.&rft.place=London&rft.series=A+Macmillan+chemistry+text&rft.pub=Macmillan+Press&rft.date=1974&rft.isbn=9780333170885&rft.aulast=Nicholls&rft.aufirst=D&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFWells1984" class="citation book cs1">Wells AF (1984). <i>Structural Inorganic Chemistry</i>. Oxford science publications (5th ed.). Oxford, UK: Oxford University Press. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/9780198553700" title="Special:BookSources/9780198553700"><bdi>9780198553700</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Structural+Inorganic+Chemistry&rft.place=Oxford%2C+UK&rft.series=Oxford+science+publications&rft.edition=5th&rft.pub=Oxford+University+Press&rft.date=1984&rft.isbn=9780198553700&rft.aulast=Wells&rft.aufirst=AF&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFReichRigby1999" class="citation book cs1">Reich HJ, Rigby HJ, eds. (1999). <i>Acidic and Basic Reagents</i>. Handbook of Reagents for Organic Synthesis. New York: John Wiley & Sons, Inc. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/9780471979258" title="Special:BookSources/9780471979258"><bdi>9780471979258</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Acidic+and+Basic+Reagents&rft.place=New+York&rft.series=Handbook+of+Reagents+for+Organic+Synthesis&rft.pub=John+Wiley+%26+Sons%2C+Inc.&rft.date=1999&rft.isbn=9780471979258&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIron%28III%29+chloride" class="Z3988"></span></li></ol> <div class="navbox-styles"><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 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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"><style data-mw-deduplicate="TemplateStyles:r1239400231">.mw-parser-output .navbar{display:inline;font-size:88%;font-weight:normal}.mw-parser-output .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 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style="font-size:114%;margin:0 4em"><a href="/wiki/Iron_compounds" title="Iron compounds">Iron compounds</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(−II)</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Iron_tetracarbonyl_dihydride" title="Iron tetracarbonyl dihydride">H<sub>2</sub>Fe(CO)<sub>4</sub></a></li> <li><a href="/wiki/Disodium_tetracarbonylferrate" title="Disodium tetracarbonylferrate">Na<sub>2</sub>Fe(CO)<sub>4</sub></a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(0)</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/Iron_pentacarbonyl" title="Iron pentacarbonyl">Fe(CO)<sub>5</sub></a></li> <li><a href="/wiki/Diiron_nonacarbonyl" title="Diiron nonacarbonyl">Fe<sub>2</sub>(CO)<sub>9</sub></a></li> <li><a href="/wiki/Triiron_dodecacarbonyl" title="Triiron dodecacarbonyl">Fe<sub>3</sub>(CO)<sub>12</sub></a></li> <li><a href="/wiki/(Benzylideneacetone)iron_tricarbonyl" title="(Benzylideneacetone)iron tricarbonyl">Fe(CO)<sub>3</sub>CH<sub>3</sub>COC<sub>2</sub>H<sub>2</sub>C<sub>6</sub>H<sub>6</sub></a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(I)</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Iron(I)_hydride" title="Iron(I) hydride">FeH</a></li></ul></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th id="Organoiron(I)_compounds" scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Organoiron_chemistry" title="Organoiron chemistry">Organoiron</a>(I) compounds</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <li><a href="/wiki/Cyclopentadienyliron_dicarbonyl_dimer" title="Cyclopentadienyliron dicarbonyl dimer">(C<sub>5</sub>H<sub>5</sub>FeCO)<sub>2</sub>(CO)<sub>2</sub></a></li> </div></td></tr></tbody></table><div> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(0,II)</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Iron_carbide" class="mw-redirect" title="Iron carbide">Fe<sub>3</sub>C</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(II)</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/Iron(II)_hydride" title="Iron(II) hydride">FeH<sub>2</sub></a></li> <li><a href="/wiki/Magnesium_iron_hexahydride" title="Magnesium iron hexahydride">Mg<sub>2</sub>FeH<sub>6</sub></a></li> <li><a href="/wiki/Iron(II)_fluoride" title="Iron(II) fluoride">FeF<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_chloride" title="Iron(II) chloride">FeCl<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_perchlorate" title="Iron(II) perchlorate">Fe(ClO<sub>4</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_bromide" title="Iron(II) bromide">FeBr<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_iodide" title="Iron(II) iodide">FeI<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_oxide" title="Iron(II) oxide">FeO</a></li> <li><a href="/wiki/Iron(II)_hydroxide" title="Iron(II) hydroxide">Fe(OH)<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_sulfide" title="Iron(II) sulfide">FeS</a></li> <li><a href="/wiki/Iron(II)_sulfate" title="Iron(II) sulfate">FeSO<sub>4</sub></a></li> <li><a href="/wiki/Ammonium_iron(II)_sulfate" title="Ammonium iron(II) sulfate">(NH<sub>4</sub>)<sub>2</sub>Fe(SO<sub>4</sub>)<sub>2</sub>·6H<sub>2</sub>O</a></li> <li><a href="/wiki/Iron(II)_selenide" title="Iron(II) selenide">FeSe</a></li> <li><a href="/wiki/Iron(II)_selenate" title="Iron(II) selenate">FeSeO<sub>4</sub></a></li> <li><a href="/wiki/Iron(II)_nitrate" title="Iron(II) nitrate">Fe(NO<sub>3</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_phosphate" title="Iron(II) phosphate">Fe<sub>3</sub>(PO<sub>4</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Iron_disilicide" title="Iron disilicide">FeSi<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_tetrafluoroborate" title="Iron(II) tetrafluoroborate">Fe(BF<sub>4</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_chromite" title="Iron(II) chromite">FeCr<sub>2</sub>O<sub>4</sub></a></li> <li><a href="/wiki/Iron(II)_molybdate" title="Iron(II) molybdate">FeMoO<sub>4</sub></a></li> <li><a href="/wiki/Iron(II)_titanate" class="mw-redirect" title="Iron(II) titanate">FeTiO<sub>3</sub></a></li> <li><a href="/wiki/Iron(II)_carbonate" title="Iron(II) carbonate">FeCO<sub>3</sub></a></li> <li><a href="/wiki/Iron(II)_oxalate" title="Iron(II) oxalate">FeC<sub>2</sub>O<sub>4</sub></a></li> <li><a href="/wiki/Iron(II)_acetate" title="Iron(II) acetate">Fe(C<sub>2</sub>H<sub>3</sub>O<sub>2</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_lactate" title="Iron(II) lactate">Fe(C<sub>3</sub>H<sub>5</sub>O<sub>3</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Iron(II)_citrate" title="Iron(II) citrate">FeC<sub>6</sub>H<sub>6</sub>O<sub>7</sub></a></li> <li><a href="/wiki/Iron(II)_gluconate" title="Iron(II) gluconate">FeC<sub>12</sub>H<sub>22</sub>O<sub>14</sub></a></li> <li><a href="/wiki/Iron_tetracarbonyl_diiodide" title="Iron tetracarbonyl diiodide">FeI<sub>2</sub>(CO)<sub>4</sub></a></li></ul> </div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th id="Organoiron(II)_compounds" scope="row" class="navbox-group" style="width:1%">Organoiron(II) compounds</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Ferrocene" title="Ferrocene">Fe(C<sub>5</sub>H<sub>5</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Cyclopentadienyliron_dicarbonyl_iodide" title="Cyclopentadienyliron dicarbonyl iodide">Fe(C<sub>5</sub>H<sub>5</sub>)(CO)<sub>2</sub>I</a></li> <li><a href="/wiki/1,1%27-Bis(diphenylphosphino)ferrocene" title="1,1'-Bis(diphenylphosphino)ferrocene">Fe(C<sub>5</sub>H<sub>4</sub>P(C<sub>6</sub>H<sub>5</sub>)<sub>2</sub>)<sub>2</sub></a></li> <li><a href="/wiki/Cyclobutadieneiron_tricarbonyl" title="Cyclobutadieneiron tricarbonyl">C<sub>4</sub>H<sub>4</sub>Fe(CO)<sub>3</sub></a></li> <li><a href="/wiki/(Butadiene)iron_tricarbonyl" title="(Butadiene)iron tricarbonyl">C<sub>4</sub>H<sub>6</sub>Fe(CO)<sub>3</sub></a></li></ul> </div></td></tr></tbody></table><div> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(0,III)</th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Iron_monosilicide" title="Iron monosilicide">FeSi</a></li> <li><a href="/wiki/Iron_germanide" title="Iron germanide">FeGe</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(II,III)</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/Iron(II,III)_oxide" title="Iron(II,III) oxide">Fe<sub>3</sub>O<sub>4</sub></a></li> <li><a href="/wiki/Iron(II,III)_sulfide" title="Iron(II,III) sulfide">Fe<sub>3</sub>S<sub>4</sub></a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(III)</th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Iron(III)_iodide" title="Iron(III) iodide">FeI<sub>3</sub></a></li> <li><a href="/wiki/Iron(III)_bromide" title="Iron(III) bromide">FeBr<sub>3</sub></a></li> <li><a class="mw-selflink selflink">FeCl<sub>3</sub></a></li> <li><a href="/wiki/Iron(III)_fluoride" title="Iron(III) fluoride">FeF<sub>3</sub></a></li> <li><a href="/wiki/Iron_phosphide" title="Iron phosphide">FeP</a></li> <li><a href="/wiki/Iron(III)_nitrate" title="Iron(III) nitrate">Fe(NO<sub>3</sub>)<sub>3</sub></a></li> <li><a href="/wiki/Tris(acetylacetonato)iron(III)" title="Tris(acetylacetonato)iron(III)">Fe(acac)<sub>3</sub></a></li> <li><a href="/wiki/Iron_oxychloride" title="Iron oxychloride">FeOCl</a></li> <li><a href="/wiki/Tetraethylammonium_diiron_oxyhexachloride" title="Tetraethylammonium diiron oxyhexachloride">[(C<sub>2</sub>H<sub>5</sub>)<sub>4</sub>N][O(FeCl<sub>3</sub>)<sub>2</sub>]</a></li> <li><a href="/wiki/Iron(III)_oxide-hydroxide" title="Iron(III) oxide-hydroxide">FeO(OH)</a></li> <li><a href="/wiki/Iron(III)_phosphate" title="Iron(III) phosphate">FePO<sub>4</sub></a></li> <li><a href="/wiki/Iron(III)_pyrophosphate" title="Iron(III) pyrophosphate">Fe<sub>4</sub>(P<sub>2</sub>O<sub>7</sub>)<sub>3</sub></a></li> <li><a href="/wiki/Iron(III)_chromate" title="Iron(III) chromate">Fe<sub>2</sub>(CrO<sub>4</sub>)<sub>3</sub></a></li> <li><a href="/wiki/Ferric_oxalate" title="Ferric oxalate">Fe<sub>2</sub>(C<sub>2</sub>O<sub>4</sub>)<sub>3</sub></a></li> <li><a href="/wiki/Iron(III)_oxide" title="Iron(III) oxide">Fe<sub>2</sub>O<sub>3</sub></a></li> <li><a href="/wiki/Iron(III)_selenite" title="Iron(III) selenite">Fe<sub>2</sub>(SeO<sub>3</sub>)<sub>3</sub></a></li> <li><a href="/wiki/Iron(III)_sulfide" title="Iron(III) sulfide">Fe<sub>2</sub>S<sub>3</sub></a></li> <li><a href="/wiki/Iron(III)_sulfate" title="Iron(III) sulfate">Fe<sub>2</sub>(SO<sub>4</sub>)<sub>3</sub></a></li> <li><a href="/wiki/Iron(III)_azide" title="Iron(III) azide">Fe(N<sub>3</sub>)<sub>3</sub></a></li> <li><a href="/wiki/Ammonium_iron(III)_sulfate" title="Ammonium iron(III) sulfate">NH<sub>4</sub>Fe(SO<sub>4</sub>)<sub>2</sub>·12H<sub>2</sub>O</a></li></ul> </div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th id="Organoiron(III)_compounds" scope="row" class="navbox-group" style="width:1%">Organoiron(III) compounds</th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Ferrocenium_tetrafluoroborate" title="Ferrocenium tetrafluoroborate">Fe(C<sub>5</sub>H<sub>5</sub>)<sub>2</sub>BF<sub>4</sub></a></li> <li><a href="/wiki/Ammonium_ferric_citrate" title="Ammonium ferric citrate">C<sub>6</sub>H<sub>8</sub>O<sub>7</sub>·<i>x</i>Fe<sup>3+</sup>·<i>y</i>NH<sub>3</sub></a></li> <li><a href="/wiki/Ferric_stearate" title="Ferric stearate"><span class="chemf nowrap">C<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">54</sub></span></span>H<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">105</sub></span></span>FeO<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">6</sub></span></span></span></a></li></ul> </div></td></tr></tbody></table><div> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(IV)</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/Iron_tetrafluoride" title="Iron tetrafluoride"><span class="chemf nowrap">FeF<sub class="template-chem2-sub">4</sub></span></a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Fe(VI)</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/Potassium_ferrate" title="Potassium ferrate">K<sub>2</sub>FeO<sub>4</sub></a></li> <li><a href="/wiki/Barium_ferrate" title="Barium ferrate">BaFeO<sub>4</sub></a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Purported</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/Hemolithin" title="Hemolithin">Hemolithin (protein)</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">sort</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/Potassium_ferricyanide" title="Potassium ferricyanide"><span class="chemf nowrap">K<sub class="template-chem2-sub">3</sub>Fe(CN)<sub class="template-chem2-sub">6</sub></span></a></li> <li><a href="/wiki/Potassium_ferrocyanide" title="Potassium ferrocyanide"><span class="chemf nowrap">K<sub class="template-chem2-sub">4</sub>Fe(CN)<sub class="template-chem2-sub">6</sub></span></a></li> <li><a href="/wiki/Potassium_ferrioxalate" title="Potassium ferrioxalate"><span class="chemf nowrap">K<sub class="template-chem2-sub">3</sub>Fe(C<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">4</sub>)<sub class="template-chem2-sub">3</sub></span></a></li> <li><a href="/wiki/Potassium_ferrooxalate" title="Potassium ferrooxalate"><span class="chemf nowrap">K<sub class="template-chem2-sub">2</sub>Fe(C<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">4</sub>)<sub class="template-chem2-sub">2</sub></span></a></li> <li><a href="/wiki/Sodium_ferrioxalate" title="Sodium ferrioxalate"><span class="chemf nowrap">Na<sub class="template-chem2-sub">3</sub>Fe(C<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">4</sub>)<sub class="template-chem2-sub">3</sub></span></a></li> <li><a href="/wiki/Prussian_blue" title="Prussian blue">Prussian blue</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="Salts_and_covalent_derivatives_of_the_chloride_ion" style="display:table;;padding:3px"><table class="nowraplinks mw-collapsible autocollapse navbox-inner" style="border-spacing:0;background:transparent;color:inherit;table-layout:fixed;"><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:Chlorides" title="Template:Chlorides"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Chlorides" title="Template talk:Chlorides"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Chlorides" title="Special:EditPage/Template:Chlorides"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Salts_and_covalent_derivatives_of_the_chloride_ion" style="font-size:114%;margin:0 4em">Salts and covalent derivatives of the <a href="/wiki/Chloride" title="Chloride">chloride</a> ion</div></th></tr><tr><td colspan="2" class="navbox-list navbox-odd" style="width:100%;padding:0;border-width:0;"><div style="padding:0"><div class="mw-collapsible-content" style="overflow-x:auto"> <table class="center"> <tbody><tr style="background-color:mistyrose"> <td><a href="/wiki/Hydrogen_chloride" title="Hydrogen chloride">HCl</a> </td> <td style="background-color:white;border:none"> </td> <td style="background-color:white;border:none" colspan="11" rowspan="3"> </td> <td style="background-color:white;border:none" colspan="5"> </td> <td>He </td></tr> <tr style="background-color:mistyrose"> <td><a href="/wiki/Lithium_chloride" title="Lithium chloride">LiCl</a> </td> <td><a href="/wiki/Beryllium_chloride" title="Beryllium chloride">BeCl<sub>2</sub></a> </td> <td><a href="/wiki/Boron_trichloride#Reduction" title="Boron trichloride">B<sub>4</sub>Cl<sub>4</sub></a><br /><a href="/w/index.php?title=Dodecaboron_dodecachloride&action=edit&redlink=1" class="new" title="Dodecaboron dodecachloride (page does not exist)">B<sub>12</sub>Cl<sub>12</sub></a><br /><a href="/wiki/Boron_trichloride" title="Boron trichloride">BCl<sub>3</sub></a><br /><a href="/wiki/Diboron_tetrachloride" title="Diboron tetrachloride">B<sub>2</sub>Cl<sub>4</sub></a><br /><a href="/wiki/Borate_chloride" title="Borate chloride">+BO<sub>3</sub></a> </td> <td><a href="/wiki/Dichloroacetylene" title="Dichloroacetylene">C<sub>2</sub>Cl<sub>2</sub></a><br /><a href="/wiki/Tetrachloroethylene" title="Tetrachloroethylene">C<sub>2</sub>Cl<sub>4</sub></a><br /><a href="/wiki/Hexachloroethane" title="Hexachloroethane">C<sub>2</sub>Cl<sub>6</sub></a><br /><a href="/wiki/Carbon_tetrachloride" title="Carbon tetrachloride">CCl<sub>4</sub></a><br /><a href="/wiki/Carbide_chloride" title="Carbide chloride">+C</a><br /><a href="/wiki/Carbonate_chloride" title="Carbonate chloride">+CO<sub>3</sub></a> </td> <td><a href="/wiki/Nitrogen_trichloride" title="Nitrogen trichloride">NCl<sub>3</sub></a><br /><a href="/wiki/Chlorine_azide" title="Chlorine azide">ClN<sub>3</sub></a><br /><a href="/wiki/Nitride_chloride" title="Nitride chloride">+N</a><br /><a href="/wiki/Nitrate_chlorides" title="Nitrate chlorides">+NO<sub>3</sub></a> </td> <td><a href="/wiki/Chlorine_oxide" title="Chlorine oxide">Cl<sub>x</sub>O<sub>y</sub></a><br /><a href="/wiki/Dichlorine_monoxide" title="Dichlorine monoxide">Cl<sub>2</sub>O</a><br /><a href="/wiki/Chlorine_peroxide" title="Chlorine peroxide">Cl<sub>2</sub>O<sub>2</sub></a><br /><a href="/wiki/Chlorine_monoxide" title="Chlorine monoxide">ClO</a><br /><a href="/wiki/Chlorine_dioxide" title="Chlorine dioxide">ClO<sub>2</sub></a><br /><a href="/wiki/Chlorine_perchlorate" title="Chlorine perchlorate">Cl<sub>2</sub>O<sub>4</sub></a><br /><a href="/wiki/Chloryl_perchlorate" class="mw-redirect" title="Chloryl perchlorate">Cl<sub>2</sub>O<sub>6</sub></a><br /><a href="/wiki/Dichlorine_heptoxide" title="Dichlorine heptoxide">Cl<sub>2</sub>O<sub>7</sub></a><br /><a href="/wiki/Chlorine_tetroxide" title="Chlorine tetroxide">ClO<sub>4</sub></a><br /><a href="/wiki/Oxychloride" class="mw-redirect" title="Oxychloride">+O</a> </td> <td><a href="/wiki/Chlorine_monofluoride" title="Chlorine monofluoride">ClF</a><br /><a href="/wiki/Chlorine_trifluoride" title="Chlorine trifluoride">ClF<sub>3</sub></a><br /><a href="/wiki/Chlorine_pentafluoride" title="Chlorine pentafluoride">ClF<sub>5</sub></a> </td> <td>Ne </td></tr> <tr style="background-color:mistyrose"> <td><a href="/wiki/Sodium_chloride" title="Sodium chloride">NaCl</a> </td> <td><a href="/wiki/Magnesium_chloride" title="Magnesium chloride">MgCl<sub>2</sub></a> </td> <td><a href="/wiki/Aluminium_monochloride" title="Aluminium monochloride">AlCl</a><br /><a href="/wiki/Aluminium_chloride" title="Aluminium chloride">AlCl<sub>3</sub></a> </td> <td><a href="/w/index.php?title=Dodecachloroneopentasilane&action=edit&redlink=1" class="new" title="Dodecachloroneopentasilane (page does not exist)">Si<sub>5</sub>Cl<sub>12</sub></a><br /><a href="/wiki/Hexachlorodisilane" title="Hexachlorodisilane">Si<sub>2</sub>Cl<sub>6</sub></a><br /><a href="/wiki/Silicon_tetrachloride" title="Silicon tetrachloride">SiCl<sub>4</sub></a> </td> <td><a href="/wiki/Diphosphorus_tetrachloride" title="Diphosphorus tetrachloride">P<sub>2</sub>Cl<sub>4</sub></a><br /><a href="/wiki/Phosphorus_trichloride" title="Phosphorus trichloride">PCl<sub>3</sub></a><br /><a href="/wiki/Phosphorus_pentachloride" title="Phosphorus pentachloride">PCl<sub>5</sub></a><br /><a href="/wiki/Phosphide_chloride" title="Phosphide chloride">+P</a> </td> <td><a href="/wiki/Disulfur_dichloride" title="Disulfur dichloride">S<sub>2</sub>Cl<sub>2</sub></a><br /><a href="/wiki/Sulfur_dichloride" title="Sulfur dichloride">SCl<sub>2</sub></a><br /><a href="/wiki/Sulfur_tetrachloride" title="Sulfur tetrachloride">SCl<sub>4</sub></a><br /><a href="/wiki/Sulfate_chloride" title="Sulfate chloride">+SO<sub>4</sub></a> </td> <td><a href="/wiki/Chlorine" title="Chlorine">Cl<sub>2</sub></a> </td> <td>Ar </td></tr> <tr style="background-color:mistyrose"> <td><a href="/wiki/Potassium_chloride" title="Potassium chloride">KCl</a> </td> <td><a href="/wiki/Calcium(I)_chloride" title="Calcium(I) chloride">CaCl</a><br /><a href="/wiki/Calcium_chloride" title="Calcium chloride">CaCl<sub>2</sub></a> </td> <td style="background-color:white;border:none"> </td> <td><a href="/wiki/Scandium_chloride" title="Scandium chloride">ScCl<sub>3</sub></a> </td> <td><a href="/wiki/Titanium(II)_chloride" title="Titanium(II) chloride">TiCl<sub>2</sub></a><br /><a href="/wiki/Titanium(III)_chloride" title="Titanium(III) chloride">TiCl<sub>3</sub></a><br /><a href="/wiki/Titanium_tetrachloride" title="Titanium tetrachloride">TiCl<sub>4</sub></a> </td> <td><a href="/wiki/Vanadium(II)_chloride" title="Vanadium(II) chloride">VCl<sub>2</sub></a><br /><a href="/wiki/Vanadium(III)_chloride" title="Vanadium(III) chloride">VCl<sub>3</sub></a><br /><a href="/wiki/Vanadium_tetrachloride" title="Vanadium tetrachloride">VCl<sub>4</sub></a><br /><a href="/wiki/Vanadium(V)_chloride" title="Vanadium(V) chloride">VCl<sub>5</sub></a> </td> <td><a href="/wiki/Chromium(II)_chloride" title="Chromium(II) chloride">CrCl<sub>2</sub></a><br /><a href="/wiki/Chromium(III)_chloride" title="Chromium(III) chloride">CrCl<sub>3</sub></a><br /><a href="/wiki/Chromium(IV)_chloride" title="Chromium(IV) chloride">CrCl<sub>4</sub></a> </td> <td><a href="/wiki/Manganese(II)_chloride" title="Manganese(II) chloride">MnCl<sub>2</sub></a><br /><a href="/wiki/Manganese(III)_chloride" title="Manganese(III) chloride">MnCl<sub>3</sub></a> </td> <td><a href="/wiki/Iron(II)_chloride" title="Iron(II) chloride">FeCl<sub>2</sub></a><br /><a class="mw-selflink selflink">FeCl<sub>3</sub></a> </td> <td><a href="/wiki/Cobalt(II)_chloride" title="Cobalt(II) chloride">CoCl<sub>2</sub></a><br /><a href="/wiki/Cobalt(III)_chloride" title="Cobalt(III) chloride">CoCl<sub>3</sub></a> </td> <td><a href="/wiki/Nickel(II)_chloride" title="Nickel(II) chloride">NiCl<sub>2</sub></a> </td> <td><a href="/wiki/Copper(I)_chloride" title="Copper(I) chloride">CuCl</a><br /><a href="/wiki/Copper(II)_chloride" title="Copper(II) chloride">CuCl<sub>2</sub></a> </td> <td><a href="/wiki/Zinc_chloride" title="Zinc chloride">ZnCl<sub>2</sub></a> </td> <td><a href="/w/index.php?title=Gallium_monochloride&action=edit&redlink=1" class="new" title="Gallium monochloride (page does not exist)">GaCl</a><br /><a href="/wiki/Gallium_trichloride" class="mw-redirect" title="Gallium trichloride">GaCl<sub>3</sub></a> </td> <td><a href="/wiki/Germanium_dichloride" title="Germanium dichloride">GeCl<sub>2</sub></a><br /><a href="/wiki/Germanium_tetrachloride" title="Germanium tetrachloride">GeCl<sub>4</sub></a> </td> <td><a href="/wiki/Arsenic_trichloride" title="Arsenic trichloride">AsCl<sub>3</sub></a><br /><a href="/wiki/Arsenic_pentachloride" title="Arsenic pentachloride">AsCl<sub>5</sub></a><br /><a href="/wiki/Arsenide_chloride" title="Arsenide chloride">+As</a> </td> <td><a href="/wiki/Selenium_monochloride" title="Selenium monochloride">Se<sub>2</sub>Cl<sub>2</sub></a><br /><a href="/wiki/Selenium_dichloride" title="Selenium dichloride">SeCl<sub>2</sub></a><br /><a href="/wiki/Selenium_tetrachloride" title="Selenium tetrachloride">SeCl<sub>4</sub></a> </td> <td><a href="/wiki/Bromine_monochloride" title="Bromine monochloride">BrCl</a> </td> <td>Kr </td></tr> <tr style="background-color:mistyrose"> <td><a href="/wiki/Rubidium_chloride" title="Rubidium chloride">RbCl</a> </td> <td><a href="/wiki/Strontium_chloride" title="Strontium chloride">SrCl<sub>2</sub></a> </td> <td style="background-color:white;border:none"> </td> <td><a href="/wiki/Yttrium(III)_chloride" title="Yttrium(III) chloride">YCl<sub>3</sub></a> </td> <td><a href="/wiki/Zirconium(II)_chloride" class="mw-redirect" title="Zirconium(II) chloride">ZrCl<sub>2</sub></a><br /><a href="/wiki/Zirconium(III)_chloride" title="Zirconium(III) chloride">ZrCl<sub>3</sub></a><br /><a href="/wiki/Zirconium(IV)_chloride" title="Zirconium(IV) chloride">ZrCl<sub>4</sub></a> </td> <td><a href="/wiki/Niobium(III)_chloride" title="Niobium(III) chloride">NbCl<sub>3</sub></a><br /><a href="/wiki/Niobium(IV)_chloride" title="Niobium(IV) chloride">NbCl<sub>4</sub></a><br /><a href="/wiki/Niobium(V)_chloride" title="Niobium(V) chloride">NbCl<sub>5</sub></a> </td> <td><a href="/wiki/Molybdenum(II)_chloride" title="Molybdenum(II) chloride">MoCl<sub>2</sub></a><br /><a href="/wiki/Molybdenum(III)_chloride" title="Molybdenum(III) chloride">MoCl<sub>3</sub></a><br /><a href="/wiki/Molybdenum_tetrachloride" title="Molybdenum tetrachloride">MoCl<sub>4</sub></a><br /><a href="/wiki/Molybdenum(V)_chloride" title="Molybdenum(V) chloride">MoCl<sub>5</sub></a><br /><a href="/wiki/Molybdenum(VI)_chloride" title="Molybdenum(VI) chloride">MoCl<sub>6</sub></a> </td> <td><a href="/wiki/Technetium_trichloride" class="mw-redirect" title="Technetium trichloride">TcCl<sub>3</sub></a><br /><a href="/wiki/Technetium(IV)_chloride" title="Technetium(IV) chloride">TcCl<sub>4</sub></a> </td> <td><a href="/wiki/Ruthenium(II)_chloride" title="Ruthenium(II) chloride">RuCl<sub>2</sub></a><br /><a href="/wiki/Ruthenium(III)_chloride" title="Ruthenium(III) chloride">RuCl<sub>3</sub></a><br /><a href="/wiki/Ruthenium_tetrachloride" title="Ruthenium tetrachloride">RuCl<sub>4</sub></a> </td> <td><a href="/wiki/Rhodium(III)_chloride" title="Rhodium(III) chloride">RhCl<sub>3</sub></a> </td> <td><a href="/wiki/Palladium(II)_chloride" title="Palladium(II) chloride">PdCl<sub>2</sub></a> </td> <td><a href="/wiki/Silver_chloride" title="Silver chloride">AgCl</a> </td> <td><a href="/wiki/Cadmium_chloride" title="Cadmium chloride">CdCl<sub>2</sub></a> </td> <td><a href="/wiki/Indium(I)_chloride" title="Indium(I) chloride">InCl</a><br /><a href="/wiki/Indium(II)_chloride" title="Indium(II) chloride">InCl<sub>2</sub></a><br /><a href="/wiki/Indium(III)_chloride" title="Indium(III) chloride">InCl<sub>3</sub></a> </td> <td><a href="/wiki/Tin(II)_chloride" title="Tin(II) chloride">SnCl<sub>2</sub></a><br /><a href="/wiki/Tin(IV)_chloride" title="Tin(IV) chloride">SnCl<sub>4</sub></a> </td> <td><a href="/wiki/Antimony_trichloride" title="Antimony trichloride">SbCl<sub>3</sub></a><br /><a href="/wiki/Antimony_pentachloride" title="Antimony pentachloride">SbCl<sub>5</sub></a> </td> <td><a href="/wiki/Tritellurium_dichloride" title="Tritellurium dichloride">Te<sub>3</sub>Cl<sub>2</sub></a><br /><a href="/wiki/Tellurium_dichloride" title="Tellurium dichloride">TeCl<sub>2</sub></a><br /><a href="/wiki/Tellurium_tetrachloride" title="Tellurium tetrachloride">TeCl<sub>4</sub></a> </td> <td><a href="/wiki/Iodine_monochloride" title="Iodine monochloride">ICl</a><br /><a href="/wiki/Iodine_trichloride" title="Iodine trichloride">ICl<sub>3</sub></a> </td> <td><a href="/wiki/Xenon_monochloride" title="Xenon monochloride">XeCl</a><br /><a href="/wiki/Xenon_dichloride" title="Xenon dichloride">XeCl<sub>2</sub></a><br /><a href="/wiki/Xenon_tetrachloride" title="Xenon tetrachloride">XeCl<sub>4</sub></a> </td></tr> <tr style="background-color:mistyrose"> <td><a href="/wiki/Caesium_chloride" title="Caesium chloride">CsCl</a> </td> <td><a href="/wiki/Barium_chloride" title="Barium chloride">BaCl<sub>2</sub></a> </td> <td style="background-color:white;border:none">* </td> <td><a href="/wiki/Lutetium(III)_chloride" title="Lutetium(III) chloride">LuCl<sub>3</sub></a> </td> <td><a href="/wiki/Hafnium_tetrachloride" title="Hafnium tetrachloride">HfCl<sub>4</sub></a> </td> <td><a href="/wiki/Tantalum(III)_chloride" title="Tantalum(III) chloride">TaCl<sub>3</sub></a><br /><a href="/w/index.php?title=Tantalum(IV)_chloride&action=edit&redlink=1" class="new" title="Tantalum(IV) chloride (page does not exist)">TaCl<sub>4</sub></a><br /><a href="/wiki/Tantalum(V)_chloride" title="Tantalum(V) chloride">TaCl<sub>5</sub></a> </td> <td><a href="/wiki/Tungsten(II)_chloride" title="Tungsten(II) chloride">WCl<sub>2</sub></a><br /><a href="/wiki/Tungsten(III)_chloride" title="Tungsten(III) chloride">WCl<sub>3</sub></a><br /><a href="/wiki/Tungsten(IV)_chloride" title="Tungsten(IV) chloride">WCl<sub>4</sub></a><br /><a href="/wiki/Tungsten(V)_chloride" title="Tungsten(V) chloride">WCl<sub>5</sub></a><br /><a href="/wiki/Tungsten_hexachloride" title="Tungsten hexachloride">WCl<sub>6</sub></a> </td> <td><a href="/wiki/Rhenium(III)_chloride" class="mw-redirect" title="Rhenium(III) chloride">ReCl<sub>3</sub></a><br /><a href="/wiki/Rhenium(IV)_chloride" title="Rhenium(IV) chloride">ReCl<sub>4</sub></a><br /><a href="/wiki/Rhenium_pentachloride" title="Rhenium pentachloride">ReCl<sub>5</sub></a><br /><a href="/wiki/Rhenium(VI)_chloride" title="Rhenium(VI) chloride">ReCl<sub>6</sub></a> </td> <td><a href="/wiki/Osmium(II)_chloride" title="Osmium(II) chloride">OsCl<sub>2</sub></a><br /><a href="/wiki/Osmium(III)_chloride" title="Osmium(III) chloride">OsCl<sub>3</sub></a><br /><a href="/wiki/Osmium(IV)_chloride" title="Osmium(IV) chloride">OsCl<sub>4</sub></a><br /><a href="/wiki/Osmium(V)_chloride" title="Osmium(V) chloride">OsCl<sub>5</sub></a> </td> <td><a href="/wiki/Iridium(II)_chloride" title="Iridium(II) chloride">IrCl<sub>2</sub></a><br /><a href="/wiki/Iridium(III)_chloride" title="Iridium(III) chloride">IrCl<sub>3</sub></a><br /><a href="/wiki/Iridium_tetrachloride" title="Iridium tetrachloride">IrCl<sub>4</sub></a> </td> <td><a href="/wiki/Platinum(II)_chloride" title="Platinum(II) chloride">PtCl<sub>2</sub></a><br /><a href="/wiki/Platinum(IV)_chloride" title="Platinum(IV) chloride">PtCl<sub>4</sub></a> </td> <td><a href="/wiki/Gold(I)_chloride" title="Gold(I) chloride">AuCl</a><br /><a href="/wiki/Gold(I,III)_chloride" title="Gold(I,III) chloride">(Au[AuCl<sub>4</sub>])<sub>2</sub></a><br /><a href="/wiki/Gold(III)_chloride" title="Gold(III) chloride">AuCl<sub>3</sub></a> </td> <td><a href="/wiki/Mercury(I)_chloride" title="Mercury(I) chloride">Hg<sub>2</sub>Cl<sub>2</sub></a><br /><a href="/wiki/Mercury(II)_chloride" title="Mercury(II) chloride">HgCl<sub>2</sub></a> </td> <td><a href="/wiki/Thallium(I)_chloride" title="Thallium(I) chloride">TlCl</a><br /><a href="/wiki/Thallium_trichloride" class="mw-redirect" title="Thallium trichloride">TlCl<sub>3</sub></a> </td> <td><a href="/wiki/Lead(II)_chloride" title="Lead(II) chloride">PbCl<sub>2</sub></a><br /><a href="/wiki/Lead(IV)_chloride" title="Lead(IV) chloride">PbCl<sub>4</sub></a> </td> <td><a href="/wiki/Bismuth_chloride" title="Bismuth chloride">BiCl<sub>3</sub></a> </td> <td><a href="/wiki/Polonium_dichloride" title="Polonium dichloride">PoCl<sub>2</sub></a><br /><a href="/wiki/Polonium_tetrachloride" title="Polonium tetrachloride">PoCl<sub>4</sub></a> </td> <td><a href="/wiki/Astatine_monochloride" class="mw-redirect" title="Astatine monochloride">AtCl</a> </td> <td>Rn </td></tr> <tr style="background-color:mistyrose"> <td><a href="/wiki/Francium_chloride" title="Francium chloride">FrCl</a> </td> <td><a href="/wiki/Radium_chloride" title="Radium chloride">RaCl<sub>2</sub></a> </td> <td style="background-color:white;border:none">** </td> <td><a href="/wiki/Lawrencium#Chemical" title="Lawrencium">LrCl<sub>3</sub></a> </td> <td><a href="/wiki/Rutherfordium#Experimental_chemistry" title="Rutherfordium">RfCl<sub>4</sub></a> </td> <td><a href="/wiki/Dubnium#Experimental_chemistry" title="Dubnium">DbCl<sub>5</sub></a> </td> <td><a href="/wiki/Seaborgium#Experimental_chemistry" title="Seaborgium">SgO<sub>2</sub>Cl<sub>2</sub></a> </td> <td><a href="/wiki/Bohrium#Experimental_chemistry" title="Bohrium">BhO<sub>3</sub>Cl</a> </td> <td>Hs </td> <td>Mt </td> <td>Ds </td> <td>Rg </td> <td>Cn </td> <td>Nh </td> <td>Fl </td> <td>Mc </td> <td>Lv </td> <td>Ts </td> <td>Og </td></tr> <tr> <td style="background-color:white;border:none" colspan="2" rowspan="3"> </td> <td style="background-color:white;border:none" colspan="20">  </td></tr> <tr style="background-color:mistyrose"> <td style="background-color:white;border:none">* </td> <td><a href="/wiki/Lanthanum(III)_chloride" title="Lanthanum(III) chloride">LaCl<sub>3</sub></a> </td> <td><a href="/wiki/Cerium(III)_chloride" title="Cerium(III) chloride">CeCl<sub>3</sub></a> </td> <td><a href="/wiki/Praseodymium(III)_chloride" title="Praseodymium(III) chloride">PrCl<sub>3</sub></a> </td> <td><a href="/wiki/Neodymium(II)_chloride" title="Neodymium(II) chloride">NdCl<sub>2</sub></a><br /><a href="/wiki/Neodymium(III)_chloride" title="Neodymium(III) chloride">NdCl<sub>3</sub></a> </td> <td><a href="/wiki/Promethium(III)_chloride" title="Promethium(III) chloride">PmCl<sub>3</sub></a> </td> <td><a href="/wiki/Samarium(II)_chloride" title="Samarium(II) chloride">SmCl<sub>2</sub></a><br /><a href="/wiki/Samarium(III)_chloride" title="Samarium(III) chloride">SmCl<sub>3</sub></a> </td> <td><a href="/wiki/Europium_dichloride" class="mw-redirect" title="Europium dichloride">EuCl<sub>2</sub></a><br /><a href="/wiki/Europium(III)_chloride" title="Europium(III) chloride">EuCl<sub>3</sub></a> </td> <td><a href="/wiki/Gadolinium(III)_chloride" title="Gadolinium(III) chloride">GdCl<sub>3</sub></a> </td> <td><a href="/wiki/Terbium(III)_chloride" title="Terbium(III) chloride">TbCl<sub>3</sub></a> </td> <td><a href="/wiki/Dysprosium(II)_chloride" title="Dysprosium(II) chloride">DyCl<sub>2</sub></a><br /><a href="/wiki/Dysprosium(III)_chloride" title="Dysprosium(III) chloride">DyCl<sub>3</sub></a> </td> <td><a href="/wiki/Holmium(III)_chloride" title="Holmium(III) chloride">HoCl<sub>3</sub></a> </td> <td><a href="/wiki/Erbium(III)_chloride" title="Erbium(III) chloride">ErCl<sub>3</sub></a> </td> <td><a href="/wiki/Thulium(II)_chloride" title="Thulium(II) chloride">TmCl<sub>2</sub></a><br /><a href="/wiki/Thulium(III)_chloride" title="Thulium(III) chloride">TmCl<sub>3</sub></a> </td> <td><a href="/wiki/Ytterbium(II)_chloride" title="Ytterbium(II) chloride">YbCl<sub>2</sub></a><br /><a href="/wiki/Ytterbium(III)_chloride" title="Ytterbium(III) chloride">YbCl<sub>3</sub></a> </td></tr> <tr style="background-color:mistyrose"> <td style="background-color:white;border:none">** </td> <td><a href="/wiki/Actinium(III)_chloride" title="Actinium(III) chloride">AcCl<sub>3</sub></a> </td> <td><a href="/wiki/Thorium(III)_chloride" class="mw-redirect" title="Thorium(III) chloride">ThCl<sub>3</sub></a><br /><a href="/wiki/Thorium(IV)_chloride" title="Thorium(IV) chloride">ThCl<sub>4</sub></a> </td> <td><a href="/wiki/Protactinium(IV)_chloride" title="Protactinium(IV) chloride">PaCl<sub>4</sub></a><br /><a href="/wiki/Protactinium(V)_chloride" title="Protactinium(V) chloride">PaCl<sub>5</sub></a> </td> <td><a href="/wiki/Uranium(III)_chloride" title="Uranium(III) chloride">UCl<sub>3</sub></a><br /><a href="/wiki/Uranium_tetrachloride" title="Uranium tetrachloride">UCl<sub>4</sub></a><br /><a href="/wiki/Uranium_pentachloride" title="Uranium pentachloride">UCl<sub>5</sub></a><br /><a href="/wiki/Uranium_hexachloride" title="Uranium hexachloride">UCl<sub>6</sub></a> </td> <td><a href="/wiki/Neptunium(III)_chloride" title="Neptunium(III) chloride">NpCl<sub>3</sub></a> </td> <td><a href="/wiki/Plutonium(III)_chloride" title="Plutonium(III) chloride">PuCl<sub>3</sub></a> </td> <td><a href="/wiki/Americium(II)_chloride" title="Americium(II) chloride">AmCl<sub>2</sub></a><br /><a href="/wiki/Americium(III)_chloride" title="Americium(III) chloride">AmCl<sub>3</sub></a> </td> <td><a href="/wiki/Curium(III)_chloride" title="Curium(III) chloride">CmCl<sub>3</sub></a> </td> <td><a href="/wiki/Berkelium(III)_chloride" title="Berkelium(III) chloride">BkCl<sub>3</sub></a> </td> <td><a href="/wiki/Californium(III)_chloride" title="Californium(III) chloride">CfCl<sub>3</sub></a><br /><a href="/wiki/Californium_dichloride" title="Californium dichloride"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">CfCl<sub class="template-chem2-sub">2</sub></span></a> </td> <td><a href="/wiki/Einsteinium(II)_chloride" title="Einsteinium(II) chloride">EsCl<sub>2</sub></a><br /><a href="/wiki/Einsteinium(III)_chloride" title="Einsteinium(III) chloride">EsCl<sub>3</sub></a> </td> <td><a href="/wiki/Fermium#Chemistry" title="Fermium">FmCl<sub>2</sub></a> </td> <td><a href="/wiki/Mendelevium#Chemical" title="Mendelevium">MdCl<sub>2</sub></a> </td> <td><a href="/wiki/Nobelium#Chemical" title="Nobelium">NoCl<sub>2</sub></a> </td></tr></tbody></table></div> </div></td></tr></tbody></table></div>    </div><noscript><img src="https://login.wikimedia.org/wiki/Special:CentralAutoLogin/start?type=1x1" alt="" width="1" height="1" style="border: none; position: 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