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class="vector-toc-list"> <li id="toc-Oxidants" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Oxidants"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.1</span> <span>Oxidants</span> </div> </a> <ul id="toc-Oxidants-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Reductants" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Reductants"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.2</span> <span>Reductants</span> </div> </a> <ul id="toc-Reductants-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Electronation_and_deelectronation" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Electronation_and_deelectronation"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.3</span> <span>Electronation and deelectronation</span> </div> </a> <ul id="toc-Electronation_and_deelectronation-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Rates,_mechanisms,_and_energies" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Rates,_mechanisms,_and_energies"> <div class="vector-toc-text"> <span class="vector-toc-numb">2</span> <span>Rates, mechanisms, and energies</span> </div> </a> <ul id="toc-Rates,_mechanisms,_and_energies-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Standard_electrode_potentials_(reduction_potentials)" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Standard_electrode_potentials_(reduction_potentials)"> <div class="vector-toc-text"> <span class="vector-toc-numb">3</span> <span>Standard electrode potentials (reduction potentials)</span> </div> </a> <ul id="toc-Standard_electrode_potentials_(reduction_potentials)-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Examples_of_redox_reactions" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Examples_of_redox_reactions"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Examples of redox reactions</span> </div> </a> <button aria-controls="toc-Examples_of_redox_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 Examples of redox reactions subsection</span> </button> <ul id="toc-Examples_of_redox_reactions-sublist" class="vector-toc-list"> <li id="toc-Metal_displacement" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Metal_displacement"> <div class="vector-toc-text"> <span class="vector-toc-numb">4.1</span> <span>Metal displacement</span> </div> </a> <ul id="toc-Metal_displacement-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Other_examples" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Other_examples"> <div class="vector-toc-text"> <span class="vector-toc-numb">4.2</span> <span>Other examples</span> </div> </a> <ul id="toc-Other_examples-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Corrosion_and_rusting" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Corrosion_and_rusting"> <div class="vector-toc-text"> <span class="vector-toc-numb">4.3</span> <span>Corrosion and rusting</span> </div> </a> <ul id="toc-Corrosion_and_rusting-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Disproportionation" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Disproportionation"> <div class="vector-toc-text"> <span class="vector-toc-numb">4.4</span> <span>Disproportionation</span> </div> </a> <ul id="toc-Disproportionation-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Redox_reactions_in_industry" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Redox_reactions_in_industry"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>Redox reactions in industry</span> </div> </a> <ul id="toc-Redox_reactions_in_industry-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Redox_reactions_in_biology" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Redox_reactions_in_biology"> <div class="vector-toc-text"> <span class="vector-toc-numb">6</span> <span>Redox reactions in biology</span> </div> </a> <button aria-controls="toc-Redox_reactions_in_biology-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 Redox reactions in biology subsection</span> </button> <ul id="toc-Redox_reactions_in_biology-sublist" class="vector-toc-list"> <li id="toc-Redox_cycling" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Redox_cycling"> <div class="vector-toc-text"> <span class="vector-toc-numb">6.1</span> <span>Redox cycling</span> </div> </a> <ul id="toc-Redox_cycling-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Redox_reactions_in_geology" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Redox_reactions_in_geology"> <div class="vector-toc-text"> <span class="vector-toc-numb">7</span> <span>Redox reactions in geology</span> </div> </a> <ul id="toc-Redox_reactions_in_geology-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Redox_reactions_in_soils" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Redox_reactions_in_soils"> <div class="vector-toc-text"> <span class="vector-toc-numb">8</span> <span>Redox reactions in soils</span> </div> </a> <ul id="toc-Redox_reactions_in_soils-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Mnemonics" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Mnemonics"> <div class="vector-toc-text"> <span class="vector-toc-numb">9</span> <span>Mnemonics</span> </div> </a> <ul id="toc-Mnemonics-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-See_also" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#See_also"> <div class="vector-toc-text"> <span class="vector-toc-numb">10</span> <span>See also</span> </div> </a> <ul id="toc-See_also-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">11</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">12</span> <span>Further reading</span> </div> </a> <ul id="toc-Further_reading-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-External_links" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#External_links"> <div class="vector-toc-text"> <span class="vector-toc-numb">13</span> <span>External links</span> </div> </a> <ul id="toc-External_links-sublist" class="vector-toc-list"> </ul> </li> </ul> </div> </div> </nav> </div> </div> <div class="mw-content-container"> <main id="content" class="mw-body"> <header class="mw-body-header vector-page-titlebar"> <nav aria-label="Contents" class="vector-toc-landmark"> <div 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class="mw-page-title-main">Redox</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 81 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-81" 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">81 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/Redoksreaksie" title="Redoksreaksie – Afrikaans" lang="af" hreflang="af" data-title="Redoksreaksie" 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/%D8%A3%D9%83%D8%B3%D8%AF%D8%A9_%D9%88%D8%A7%D8%AE%D8%AA%D8%B2%D8%A7%D9%84" title="أكسدة واختزال – Arabic" lang="ar" hreflang="ar" data-title="أكسدة واختزال" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target"><span>العربية</span></a></li><li class="interlanguage-link interwiki-ast mw-list-item"><a href="https://ast.wikipedia.org/wiki/Amenorgamientu-oxidaci%C3%B3n" title="Amenorgamientu-oxidación – Asturian" lang="ast" hreflang="ast" data-title="Amenorgamientu-oxidación" data-language-autonym="Asturianu" data-language-local-name="Asturian" class="interlanguage-link-target"><span>Asturianu</span></a></li><li class="interlanguage-link interwiki-bn mw-list-item"><a href="https://bn.wikipedia.org/wiki/%E0%A6%9C%E0%A6%BE%E0%A6%B0%E0%A6%A3" title="জারণ – Bangla" lang="bn" hreflang="bn" data-title="জারণ" data-language-autonym="বাংলা" data-language-local-name="Bangla" class="interlanguage-link-target"><span>বাংলা</span></a></li><li class="interlanguage-link interwiki-zh-min-nan mw-list-item"><a href="https://zh-min-nan.wikipedia.org/wiki/Sng-h%C3%B2a_ho%C3%A2n-go%C3%A2n_ho%C3%A1n-%C3%A8ng" title="Sng-hòa hoân-goân hoán-èng – Minnan" lang="nan" hreflang="nan" data-title="Sng-hòa hoân-goân hoán-èng" data-language-autonym="閩南語 / Bân-lâm-gú" data-language-local-name="Minnan" class="interlanguage-link-target"><span>閩南語 / Bân-lâm-gú</span></a></li><li class="interlanguage-link interwiki-ba mw-list-item"><a href="https://ba.wikipedia.org/wiki/%D0%9E%D0%BA%D0%B8%D1%81%D0%BB%D0%B0%D0%BD%D1%8B%D1%83-%D2%A1%D0%B0%D0%B9%D1%82%D0%B0%D1%80%D1%8B%D0%BB%D1%8B%D1%83_%D1%80%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%8F%D0%BB%D0%B0%D1%80%D1%8B" title="Окисланыу-ҡайтарылыу реакциялары – Bashkir" lang="ba" hreflang="ba" data-title="Окисланыу-ҡайтарылыу реакциялары" data-language-autonym="Башҡортса" data-language-local-name="Bashkir" class="interlanguage-link-target"><span>Башҡортса</span></a></li><li class="interlanguage-link interwiki-be mw-list-item"><a href="https://be.wikipedia.org/wiki/%D0%90%D0%BA%D1%96%D1%81%D0%BB%D1%8F%D0%BB%D1%8C%D0%BD%D0%B0-%D0%B0%D0%B4%D0%BD%D0%B0%D1%9E%D0%BB%D0%B5%D0%BD%D1%87%D1%8B%D1%8F_%D1%80%D1%8D%D0%B0%D0%BA%D1%86%D1%8B%D1%96" title="Акісляльна-аднаўленчыя рэакцыі – Belarusian" lang="be" hreflang="be" data-title="Акісляльна-аднаўленчыя рэакцыі" data-language-autonym="Беларуская" data-language-local-name="Belarusian" class="interlanguage-link-target"><span>Беларуская</span></a></li><li class="interlanguage-link interwiki-be-x-old mw-list-item"><a href="https://be-tarask.wikipedia.org/wiki/%D0%97%D0%B0%D1%82%D0%BB%D1%8F%D0%BD%D1%8F%D0%BB%D1%8C%D0%BD%D0%B0-%D0%B0%D0%B4%D0%BD%D0%B0%D1%9E%D0%BB%D0%B5%D0%BD%D1%87%D1%8B%D1%8F_%D1%80%D1%8D%D0%B0%D0%BA%D1%86%D1%8B%D1%96" title="Затляняльна-аднаўленчыя рэакцыі – Belarusian (Taraškievica orthography)" lang="be-tarask" hreflang="be-tarask" data-title="Затляняльна-аднаўленчыя рэакцыі" data-language-autonym="Беларуская (тарашкевіца)" data-language-local-name="Belarusian (Taraškievica orthography)" class="interlanguage-link-target"><span>Беларуская (тарашкевіца)</span></a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%9E%D0%BA%D0%B8%D1%81%D0%BB%D0%B8%D1%82%D0%B5%D0%BB%D0%BD%D0%BE-%D1%80%D0%B5%D0%B4%D1%83%D0%BA%D1%86%D0%B8%D0%BE%D0%BD%D0%BD%D0%B8_%D0%BF%D1%80%D0%BE%D1%86%D0%B5%D1%81%D0%B8" title="Окислително-редукционни процеси – Bulgarian" lang="bg" hreflang="bg" data-title="Окислително-редукционни процеси" data-language-autonym="Български" data-language-local-name="Bulgarian" class="interlanguage-link-target"><span>Български</span></a></li><li class="interlanguage-link interwiki-bs mw-list-item"><a href="https://bs.wikipedia.org/wiki/Redoks-reakcija" title="Redoks-reakcija – Bosnian" lang="bs" hreflang="bs" data-title="Redoks-reakcija" data-language-autonym="Bosanski" data-language-local-name="Bosnian" class="interlanguage-link-target"><span>Bosanski</span></a></li><li class="interlanguage-link interwiki-ca mw-list-item"><a href="https://ca.wikipedia.org/wiki/Reacci%C3%B3_d%27oxidaci%C3%B3_reducci%C3%B3" title="Reacció d'oxidació reducció – Catalan" lang="ca" hreflang="ca" data-title="Reacció d'oxidació reducció" data-language-autonym="Català" data-language-local-name="Catalan" class="interlanguage-link-target"><span>Català</span></a></li><li class="interlanguage-link interwiki-cv mw-list-item"><a href="https://cv.wikipedia.org/wiki/%D0%9E%D0%BA%D1%81%D0%B8%D0%B4%D0%BB%D0%B0%D0%B2-%D1%82%D0%B0%D0%B2%D1%80%C4%83%D0%BD%D0%B0%D0%B2_%D1%80%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D0%B9%C4%95" title="Оксидлав-таврăнав реакцийĕ – Chuvash" lang="cv" hreflang="cv" data-title="Оксидлав-таврăнав реакцийĕ" data-language-autonym="Чӑвашла" data-language-local-name="Chuvash" class="interlanguage-link-target"><span>Чӑвашла</span></a></li><li class="interlanguage-link interwiki-cs mw-list-item"><a href="https://cs.wikipedia.org/wiki/Redoxn%C3%AD_reakce" title="Redoxní reakce – Czech" lang="cs" hreflang="cs" data-title="Redoxní reakce" data-language-autonym="Čeština" data-language-local-name="Czech" class="interlanguage-link-target"><span>Čeština</span></a></li><li class="interlanguage-link interwiki-cy mw-list-item"><a href="https://cy.wikipedia.org/wiki/Rhydocs" title="Rhydocs – Welsh" lang="cy" hreflang="cy" data-title="Rhydocs" data-language-autonym="Cymraeg" data-language-local-name="Welsh" class="interlanguage-link-target"><span>Cymraeg</span></a></li><li class="interlanguage-link interwiki-da mw-list-item"><a href="https://da.wikipedia.org/wiki/Redoxreaktion" title="Redoxreaktion – Danish" lang="da" hreflang="da" data-title="Redoxreaktion" data-language-autonym="Dansk" data-language-local-name="Danish" class="interlanguage-link-target"><span>Dansk</span></a></li><li class="interlanguage-link interwiki-de mw-list-item"><a href="https://de.wikipedia.org/wiki/Redoxreaktion" title="Redoxreaktion – German" lang="de" hreflang="de" data-title="Redoxreaktion" data-language-autonym="Deutsch" data-language-local-name="German" class="interlanguage-link-target"><span>Deutsch</span></a></li><li class="interlanguage-link interwiki-et mw-list-item"><a href="https://et.wikipedia.org/wiki/Redoksreaktsioon" title="Redoksreaktsioon – Estonian" lang="et" hreflang="et" data-title="Redoksreaktsioon" data-language-autonym="Eesti" data-language-local-name="Estonian" class="interlanguage-link-target"><span>Eesti</span></a></li><li class="interlanguage-link interwiki-el mw-list-item"><a href="https://el.wikipedia.org/wiki/%CE%9F%CE%BE%CE%B5%CE%B9%CE%B4%CE%BF%CE%B1%CE%BD%CE%B1%CE%B3%CF%89%CE%B3%CE%AE" title="Οξειδοαναγωγή – Greek" lang="el" hreflang="el" data-title="Οξειδοαναγωγή" 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/Reducci%C3%B3n-oxidaci%C3%B3n" title="Reducción-oxidación – Spanish" lang="es" hreflang="es" data-title="Reducción-oxidación" 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/Redoksa_reakcio" title="Redoksa reakcio – Esperanto" lang="eo" hreflang="eo" data-title="Redoksa reakcio" data-language-autonym="Esperanto" data-language-local-name="Esperanto" class="interlanguage-link-target"><span>Esperanto</span></a></li><li class="interlanguage-link interwiki-eu mw-list-item"><a href="https://eu.wikipedia.org/wiki/Erredox_erreakzio" title="Erredox erreakzio – Basque" lang="eu" hreflang="eu" data-title="Erredox erreakzio" data-language-autonym="Euskara" data-language-local-name="Basque" class="interlanguage-link-target"><span>Euskara</span></a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%D8%A7%DA%A9%D8%B3%D8%A7%DB%8C%D8%B4-%DA%A9%D8%A7%D9%87%D8%B4" title="اکسایش-کاهش – Persian" lang="fa" hreflang="fa" data-title="اکسایش-کاهش" 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/R%C3%A9action_d%27oxydor%C3%A9duction" title="Réaction d'oxydoréduction – French" lang="fr" hreflang="fr" data-title="Réaction d'oxydoréduction" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target"><span>Français</span></a></li><li class="interlanguage-link interwiki-fy mw-list-item"><a href="https://fy.wikipedia.org/wiki/Redoksreaksje" title="Redoksreaksje – Western Frisian" lang="fy" hreflang="fy" data-title="Redoksreaksje" data-language-autonym="Frysk" data-language-local-name="Western Frisian" class="interlanguage-link-target"><span>Frysk</span></a></li><li class="interlanguage-link interwiki-ga mw-list-item"><a href="https://ga.wikipedia.org/wiki/Ocsd%C3%AD" title="Ocsdí – Irish" lang="ga" hreflang="ga" data-title="Ocsdí" data-language-autonym="Gaeilge" data-language-local-name="Irish" class="interlanguage-link-target"><span>Gaeilge</span></a></li><li class="interlanguage-link interwiki-gl mw-list-item"><a href="https://gl.wikipedia.org/wiki/Oxidorreduci%C3%B3n" title="Oxidorredución – Galician" lang="gl" hreflang="gl" data-title="Oxidorredución" data-language-autonym="Galego" data-language-local-name="Galician" class="interlanguage-link-target"><span>Galego</span></a></li><li class="interlanguage-link interwiki-ko mw-list-item"><a href="https://ko.wikipedia.org/wiki/%EC%82%B0%ED%99%94%C2%B7%ED%99%98%EC%9B%90_%EB%B0%98%EC%9D%91" title="산화·환원 반응 – Korean" lang="ko" hreflang="ko" data-title="산화·환원 반응" 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/%D5%95%D6%84%D5%BD%D5%AB%D5%A4%D5%A1%D6%81%D5%B8%D6%82%D5%B4_%D6%87_%D5%BE%D5%A5%D6%80%D5%A1%D5%AF%D5%A1%D5%B6%D5%A3%D5%B6%D5%B8%D6%82%D5%B4" title="Օքսիդացում և վերականգնում – Armenian" lang="hy" hreflang="hy" data-title="Օքսիդացում և վերականգնում" 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%B0%E0%A5%87%E0%A4%A1%E0%A5%89%E0%A4%95%E0%A5%8D%E0%A4%B8" title="रेडॉक्स – Hindi" lang="hi" hreflang="hi" data-title="रेडॉक्स" 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/Redoks" title="Redoks – Croatian" lang="hr" hreflang="hr" data-title="Redoks" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target"><span>Hrvatski</span></a></li><li class="interlanguage-link interwiki-io mw-list-item"><a href="https://io.wikipedia.org/wiki/Degrado_per_oxidigo" title="Degrado per oxidigo – Ido" lang="io" hreflang="io" data-title="Degrado per oxidigo" data-language-autonym="Ido" data-language-local-name="Ido" class="interlanguage-link-target"><span>Ido</span></a></li><li class="interlanguage-link interwiki-id mw-list-item"><a href="https://id.wikipedia.org/wiki/Redoks" title="Redoks – Indonesian" lang="id" hreflang="id" data-title="Redoks" 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-ia mw-list-item"><a href="https://ia.wikipedia.org/wiki/Redox" title="Redox – Interlingua" lang="ia" hreflang="ia" data-title="Redox" data-language-autonym="Interlingua" data-language-local-name="Interlingua" class="interlanguage-link-target"><span>Interlingua</span></a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Ossidoriduzione" title="Ossidoriduzione – Italian" lang="it" hreflang="it" data-title="Ossidoriduzione" data-language-autonym="Italiano" data-language-local-name="Italian" class="interlanguage-link-target"><span>Italiano</span></a></li><li class="interlanguage-link interwiki-he mw-list-item"><a href="https://he.wikipedia.org/wiki/%D7%97%D7%9E%D7%A6%D7%95%D7%9F-%D7%97%D7%99%D7%96%D7%95%D7%A8" title="חמצון-חיזור – Hebrew" lang="he" hreflang="he" data-title="חמצון-חיזור" data-language-autonym="עברית" data-language-local-name="Hebrew" class="interlanguage-link-target"><span>עברית</span></a></li><li class="interlanguage-link interwiki-kn mw-list-item"><a href="https://kn.wikipedia.org/wiki/%E0%B2%89%E0%B2%A4%E0%B3%8D%E0%B2%95%E0%B2%B0%E0%B3%8D%E0%B2%B7%E0%B2%A3_-_%E0%B2%85%E0%B2%AA%E0%B2%95%E0%B2%B0%E0%B3%8D%E0%B2%B7%E0%B2%A3" title="ಉತ್ಕರ್ಷಣ - ಅಪಕರ್ಷಣ – Kannada" lang="kn" hreflang="kn" data-title="ಉತ್ಕರ್ಷಣ - ಅಪಕರ್ಷಣ" data-language-autonym="ಕನ್ನಡ" data-language-local-name="Kannada" class="interlanguage-link-target"><span>ಕನ್ನಡ</span></a></li><li class="interlanguage-link interwiki-ka mw-list-item"><a href="https://ka.wikipedia.org/wiki/%E1%83%9F%E1%83%90%E1%83%9C%E1%83%92%E1%83%95%E1%83%90-%E1%83%90%E1%83%A6%E1%83%93%E1%83%92%E1%83%94%E1%83%9C%E1%83%98%E1%83%97%E1%83%98_%E1%83%A0%E1%83%94%E1%83%90%E1%83%A5%E1%83%AA%E1%83%98%E1%83%94%E1%83%91%E1%83%98" title="ჟანგვა-აღდგენითი რეაქციები – Georgian" lang="ka" hreflang="ka" data-title="ჟანგვა-აღდგენითი რეაქციები" data-language-autonym="ქართული" data-language-local-name="Georgian" class="interlanguage-link-target"><span>ქართული</span></a></li><li class="interlanguage-link interwiki-kk mw-list-item"><a href="https://kk.wikipedia.org/wiki/%D0%A2%D0%BE%D1%82%D1%8B%D2%93%D1%83-%D1%82%D0%BE%D1%82%D1%8B%D2%9B%D1%81%D1%8B%D0%B7%D0%B4%D0%B0%D0%BD%D1%83_%D1%80%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%8F%D1%81%D1%8B" title="Тотығу-тотықсыздану реакциясы – Kazakh" lang="kk" hreflang="kk" data-title="Тотығу-тотықсыздану реакциясы" data-language-autonym="Қазақша" data-language-local-name="Kazakh" class="interlanguage-link-target"><span>Қазақша</span></a></li><li class="interlanguage-link interwiki-ht mw-list-item"><a href="https://ht.wikipedia.org/wiki/Oksidasyon" title="Oksidasyon – Haitian Creole" lang="ht" hreflang="ht" data-title="Oksidasyon" data-language-autonym="Kreyòl ayisyen" data-language-local-name="Haitian Creole" class="interlanguage-link-target"><span>Kreyòl ayisyen</span></a></li><li class="interlanguage-link interwiki-lv mw-list-item"><a href="https://lv.wikipedia.org/wiki/Oksid%C4%93%C5%A1an%C4%81s-reduc%C4%93%C5%A1an%C4%81s_reakcijas" title="Oksidēšanās-reducēšanās reakcijas – Latvian" lang="lv" hreflang="lv" data-title="Oksidēšanās-reducēšanās reakcijas" data-language-autonym="Latviešu" data-language-local-name="Latvian" class="interlanguage-link-target"><span>Latviešu</span></a></li><li class="interlanguage-link interwiki-lb mw-list-item"><a href="https://lb.wikipedia.org/wiki/Oxidatiouns-Reaktioun" title="Oxidatiouns-Reaktioun – Luxembourgish" lang="lb" hreflang="lb" data-title="Oxidatiouns-Reaktioun" data-language-autonym="Lëtzebuergesch" data-language-local-name="Luxembourgish" class="interlanguage-link-target"><span>Lëtzebuergesch</span></a></li><li class="interlanguage-link interwiki-lt mw-list-item"><a href="https://lt.wikipedia.org/wiki/Oksidacijos-redukcijos_reakcija" title="Oksidacijos-redukcijos reakcija – Lithuanian" lang="lt" hreflang="lt" data-title="Oksidacijos-redukcijos reakcija" data-language-autonym="Lietuvių" data-language-local-name="Lithuanian" class="interlanguage-link-target"><span>Lietuvių</span></a></li><li class="interlanguage-link interwiki-hu mw-list-item"><a href="https://hu.wikipedia.org/wiki/Redoxireakci%C3%B3" title="Redoxireakció – Hungarian" lang="hu" hreflang="hu" data-title="Redoxireakció" 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%9E%D0%BA%D1%81%D0%B8%D0%B4%D0%B0%D1%86%D0%B8%D0%BE%D0%BD%D0%BE-%D1%80%D0%B5%D0%B4%D1%83%D0%BA%D1%86%D0%B8%D0%BE%D0%BD%D0%B0_%D1%80%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%98%D0%B0" title="Оксидационо-редукциона реакција – Macedonian" lang="mk" hreflang="mk" data-title="Оксидационо-редукциона реакција" data-language-autonym="Македонски" data-language-local-name="Macedonian" class="interlanguage-link-target"><span>Македонски</span></a></li><li class="interlanguage-link interwiki-ml mw-list-item"><a href="https://ml.wikipedia.org/wiki/%E0%B4%B1%E0%B4%BF%E0%B4%A1%E0%B5%8B%E0%B4%95%E0%B5%8D%E0%B4%B8%E0%B5%8D_%E0%B4%AA%E0%B5%8D%E0%B4%B0%E0%B4%B5%E0%B5%BC%E0%B4%A4%E0%B5%8D%E0%B4%A4%E0%B4%A8%E0%B4%82" title="റിഡോക്സ് പ്രവർത്തനം – Malayalam" lang="ml" hreflang="ml" data-title="റിഡോക്സ് പ്രവർത്തനം" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target"><span>മലയാളം</span></a></li><li class="interlanguage-link interwiki-ms mw-list-item"><a href="https://ms.wikipedia.org/wiki/Tindak_balas_redoks" title="Tindak balas redoks – Malay" lang="ms" hreflang="ms" data-title="Tindak balas redoks" data-language-autonym="Bahasa Melayu" data-language-local-name="Malay" class="interlanguage-link-target"><span>Bahasa Melayu</span></a></li><li class="interlanguage-link interwiki-mn mw-list-item"><a href="https://mn.wikipedia.org/wiki/%D0%98%D1%81%D1%8D%D0%BB%D0%B4%D1%8D%D0%BB%D1%82" title="Исэлдэлт – Mongolian" lang="mn" hreflang="mn" data-title="Исэлдэлт" data-language-autonym="Монгол" data-language-local-name="Mongolian" class="interlanguage-link-target"><span>Монгол</span></a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Redoxreactie" title="Redoxreactie – Dutch" lang="nl" hreflang="nl" data-title="Redoxreactie" 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/%E9%85%B8%E5%8C%96%E9%82%84%E5%85%83%E5%8F%8D%E5%BF%9C" title="酸化還元反応 – Japanese" lang="ja" hreflang="ja" data-title="酸化還元反応" 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-no mw-list-item"><a href="https://no.wikipedia.org/wiki/Redoksreaksjon" title="Redoksreaksjon – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Redoksreaksjon" data-language-autonym="Norsk bokmål" data-language-local-name="Norwegian Bokmål" class="interlanguage-link-target"><span>Norsk bokmål</span></a></li><li class="interlanguage-link interwiki-nn mw-list-item"><a href="https://nn.wikipedia.org/wiki/Redoksreaksjon" title="Redoksreaksjon – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Redoksreaksjon" data-language-autonym="Norsk nynorsk" data-language-local-name="Norwegian Nynorsk" class="interlanguage-link-target"><span>Norsk nynorsk</span></a></li><li class="interlanguage-link interwiki-oc mw-list-item"><a href="https://oc.wikipedia.org/wiki/Reaccion_d%27oxidoreduccion" title="Reaccion d'oxidoreduccion – Occitan" lang="oc" hreflang="oc" data-title="Reaccion d'oxidoreduccion" data-language-autonym="Occitan" data-language-local-name="Occitan" class="interlanguage-link-target"><span>Occitan</span></a></li><li class="interlanguage-link interwiki-pa mw-list-item"><a href="https://pa.wikipedia.org/wiki/%E0%A8%B0%E0%A8%BF%E0%A8%A1%E0%A8%BE%E0%A8%95%E0%A8%B8" title="ਰਿਡਾਕਸ – Punjabi" lang="pa" hreflang="pa" data-title="ਰਿਡਾਕਸ" data-language-autonym="ਪੰਜਾਬੀ" data-language-local-name="Punjabi" class="interlanguage-link-target"><span>ਪੰਜਾਬੀ</span></a></li><li class="interlanguage-link interwiki-pnb mw-list-item"><a href="https://pnb.wikipedia.org/wiki/%D8%B1%DA%88%D8%A7%DA%A9%D8%B3" title="رڈاکس – Western Punjabi" lang="pnb" hreflang="pnb" data-title="رڈاکس" data-language-autonym="پنجابی" data-language-local-name="Western Punjabi" class="interlanguage-link-target"><span>پنجابی</span></a></li><li class="interlanguage-link interwiki-pl mw-list-item"><a href="https://pl.wikipedia.org/wiki/Reakcja_redoks" title="Reakcja redoks – Polish" lang="pl" hreflang="pl" data-title="Reakcja redoks" 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/Oxirredu%C3%A7%C3%A3o" title="Oxirredução – Portuguese" lang="pt" hreflang="pt" data-title="Oxirredução" 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/Reac%C8%9Bie_de_oxido-reducere" title="Reacție de oxido-reducere – Romanian" lang="ro" hreflang="ro" data-title="Reacție de oxido-reducere" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target"><span>Română</span></a></li><li class="interlanguage-link interwiki-qu mw-list-item"><a href="https://qu.wikipedia.org/wiki/Uksiday" title="Uksiday – Quechua" lang="qu" hreflang="qu" data-title="Uksiday" data-language-autonym="Runa Simi" data-language-local-name="Quechua" class="interlanguage-link-target"><span>Runa Simi</span></a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%9E%D0%BA%D0%B8%D1%81%D0%BB%D0%B8%D1%82%D0%B5%D0%BB%D1%8C%D0%BD%D0%BE-%D0%B2%D0%BE%D1%81%D1%81%D1%82%D0%B0%D0%BD%D0%BE%D0%B2%D0%B8%D1%82%D0%B5%D0%BB%D1%8C%D0%BD%D1%8B%D0%B5_%D1%80%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D0%B8" title="Окислительно-восстановительные реакции – Russian" lang="ru" hreflang="ru" data-title="Окислительно-восстановительные реакции" data-language-autonym="Русский" data-language-local-name="Russian" class="interlanguage-link-target"><span>Русский</span></a></li><li class="interlanguage-link interwiki-sq mw-list-item"><a href="https://sq.wikipedia.org/wiki/Reaksionet_redoks" title="Reaksionet redoks – Albanian" lang="sq" hreflang="sq" data-title="Reaksionet redoks" data-language-autonym="Shqip" data-language-local-name="Albanian" class="interlanguage-link-target"><span>Shqip</span></a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Redox" title="Redox – Simple English" lang="en-simple" hreflang="en-simple" data-title="Redox" 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-sd mw-list-item"><a href="https://sd.wikipedia.org/wiki/%D8%B1%D9%8A%DA%8A%D9%88%DA%AA%D8%B3" title="ريڊوڪس – Sindhi" lang="sd" hreflang="sd" data-title="ريڊوڪس" data-language-autonym="سنڌي" data-language-local-name="Sindhi" class="interlanguage-link-target"><span>سنڌي</span></a></li><li class="interlanguage-link interwiki-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/Oxida%C4%8Dno-reduk%C4%8Dn%C3%A1_reakcia" title="Oxidačno-redukčná reakcia – Slovak" lang="sk" hreflang="sk" data-title="Oxidačno-redukčná reakcia" 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/Redoks_reakcija" title="Redoks reakcija – Slovenian" lang="sl" hreflang="sl" data-title="Redoks reakcija" data-language-autonym="Slovenščina" data-language-local-name="Slovenian" class="interlanguage-link-target"><span>Slovenščina</span></a></li><li class="interlanguage-link interwiki-ckb mw-list-item"><a href="https://ckb.wikipedia.org/wiki/%D8%A6%DB%86%DA%A9%D8%B3%D8%A7%D9%86" title="ئۆکسان – Central Kurdish" lang="ckb" hreflang="ckb" data-title="ئۆکسان" data-language-autonym="کوردی" data-language-local-name="Central Kurdish" class="interlanguage-link-target"><span>کوردی</span></a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/%D0%9E%D0%BA%D1%81%D0%B8%D0%B4%D0%BE-%D1%80%D0%B5%D0%B4%D1%83%D0%BA%D1%86%D0%B8%D1%98%D0%B0" title="Оксидо-редукција – Serbian" lang="sr" hreflang="sr" data-title="Оксидо-редукција" 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/Oksido-redukcija" title="Oksido-redukcija – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Oksido-redukcija" 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-su mw-list-item"><a href="https://su.wikipedia.org/wiki/%E1%AE%87%E1%AE%8A%E1%AE%AA%E1%AE%9E%E1%AE%A4%E1%AE%93%E1%AE%9E%E1%AE%A4" title="ᮇᮊ᮪ᮞᮤᮓᮞᮤ – Sundanese" lang="su" hreflang="su" data-title="ᮇᮊ᮪ᮞᮤᮓᮞᮤ" data-language-autonym="Sunda" data-language-local-name="Sundanese" class="interlanguage-link-target"><span>Sunda</span></a></li><li class="interlanguage-link interwiki-fi mw-list-item"><a href="https://fi.wikipedia.org/wiki/Hapetus-pelkistysreaktio" title="Hapetus-pelkistysreaktio – Finnish" lang="fi" hreflang="fi" data-title="Hapetus-pelkistysreaktio" 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/Redox" title="Redox – Swedish" lang="sv" hreflang="sv" data-title="Redox" 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%92%E0%AE%9F%E0%AF%81%E0%AE%95%E0%AF%8D%E0%AE%95-%E0%AE%8F%E0%AE%B1%E0%AF%8D%E0%AE%B1_%E0%AE%B5%E0%AF%87%E0%AE%A4%E0%AE%BF%E0%AE%B5%E0%AE%BF%E0%AE%A9%E0%AF%88%E0%AE%95%E0%AE%B3%E0%AF%8D" title="ஒடுக்க-ஏற்ற வேதிவினைகள் – Tamil" lang="ta" hreflang="ta" data-title="ஒடுக்க-ஏற்ற வேதிவினைகள்" data-language-autonym="தமிழ்" data-language-local-name="Tamil" class="interlanguage-link-target"><span>தமிழ்</span></a></li><li class="interlanguage-link interwiki-tt mw-list-item"><a href="https://tt.wikipedia.org/wiki/%D0%9E%D0%BA%D1%81%D0%B8%D0%B4%D0%BB%D0%B0%D1%88%D1%83-%D0%BA%D0%B0%D0%B9%D1%82%D0%B0%D1%80%D1%83_%D1%80%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%8F%D0%BB%D3%99%D1%80%D0%B5" title="Оксидлашу-кайтару реакцияләре – Tatar" lang="tt" hreflang="tt" data-title="Оксидлашу-кайтару реакцияләре" data-language-autonym="Татарча / tatarça" data-language-local-name="Tatar" class="interlanguage-link-target"><span>Татарча / tatarça</span></a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B8%9B%E0%B8%8F%E0%B8%B4%E0%B8%81%E0%B8%B4%E0%B8%A3%E0%B8%B4%E0%B8%A2%E0%B8%B2%E0%B8%A3%E0%B8%B5%E0%B8%94%E0%B8%AD%E0%B8%81%E0%B8%8B%E0%B9%8C" title="ปฏิกิริยารีดอกซ์ – Thai" lang="th" hreflang="th" data-title="ปฏิกิริยารีดอกซ์" 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/Redoks" title="Redoks – Turkish" lang="tr" hreflang="tr" data-title="Redoks" 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%9E%D0%BA%D0%B8%D1%81%D0%BD%D0%BE-%D0%B2%D1%96%D0%B4%D0%BD%D0%BE%D0%B2%D0%BD%D0%B0_%D1%80%D0%B5%D0%B0%D0%BA%D1%86%D1%96%D1%8F" title="Окисно-відновна реакція – Ukrainian" lang="uk" hreflang="uk" data-title="Окисно-відновна реакція" data-language-autonym="Українська" data-language-local-name="Ukrainian" class="interlanguage-link-target"><span>Українська</span></a></li><li class="interlanguage-link interwiki-ur mw-list-item"><a href="https://ur.wikipedia.org/wiki/%D8%AA%D8%AE%D8%B3%DB%8C%D8%AF" title="تخسید – Urdu" lang="ur" hreflang="ur" data-title="تخسید" data-language-autonym="اردو" data-language-local-name="Urdu" class="interlanguage-link-target"><span>اردو</span></a></li><li class="interlanguage-link interwiki-vi mw-list-item"><a href="https://vi.wikipedia.org/wiki/Ph%E1%BA%A3n_%E1%BB%A9ng_oxy_h%C3%B3a_kh%E1%BB%AD" title="Phản ứng oxy hóa khử – Vietnamese" lang="vi" hreflang="vi" data-title="Phản ứng oxy hóa khử" 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-classical mw-list-item"><a href="https://zh-classical.wikipedia.org/wiki/%E6%B0%A7%E5%8C%96%E9%82%84%E5%8E%9F%E5%8F%8D%E6%87%89" title="氧化還原反應 – Literary Chinese" lang="lzh" hreflang="lzh" data-title="氧化還原反應" data-language-autonym="文言" data-language-local-name="Literary Chinese" class="interlanguage-link-target"><span>文言</span></a></li><li class="interlanguage-link interwiki-wuu mw-list-item"><a href="https://wuu.wikipedia.org/wiki/%E6%B0%A7%E5%8C%96%E8%BF%98%E5%8E%9F%E5%8F%8D%E5%BA%94" title="氧化还原反应 – Wu" lang="wuu" hreflang="wuu" data-title="氧化还原反应" data-language-autonym="吴语" data-language-local-name="Wu" class="interlanguage-link-target"><span>吴语</span></a></li><li class="interlanguage-link interwiki-zh-yue mw-list-item"><a href="https://zh-yue.wikipedia.org/wiki/%E6%B0%A7%E5%8C%96%E9%82%84%E5%8E%9F%E5%8F%8D%E6%87%89" title="氧化還原反應 – Cantonese" lang="yue" hreflang="yue" data-title="氧化還原反應" data-language-autonym="粵語" data-language-local-name="Cantonese" class="interlanguage-link-target"><span>粵語</span></a></li><li class="interlanguage-link interwiki-zh mw-list-item"><a href="https://zh.wikipedia.org/wiki/%E6%B0%A7%E5%8C%96%E8%BF%98%E5%8E%9F%E5%8F%8D%E5%BA%94" title="氧化还原反应 – Chinese" lang="zh" hreflang="zh" data-title="氧化还原反应" data-language-autonym="中文" data-language-local-name="Chinese" class="interlanguage-link-target"><span>中文</span></a></li> </ul> <div 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class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical reaction in which oxidation states of atoms are changed</div> <style data-mw-deduplicate="TemplateStyles:r1236090951">.mw-parser-output .hatnote{font-style:italic}.mw-parser-output div.hatnote{padding-left:1.6em;margin-bottom:0.5em}.mw-parser-output .hatnote i{font-style:normal}.mw-parser-output .hatnote+link+.hatnote{margin-top:-0.5em}@media print{body.ns-0 .mw-parser-output .hatnote{display:none!important}}</style><div role="note" class="hatnote navigation-not-searchable">For other uses, see <a href="/wiki/Redox_(disambiguation)" class="mw-disambig" title="Redox (disambiguation)">Redox (disambiguation)</a>.</div> <p class="mw-empty-elt"> </p> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:NaF.gif" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/a/a8/NaF.gif/350px-NaF.gif" decoding="async" width="350" height="153" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a8/NaF.gif/525px-NaF.gif 1.5x, //upload.wikimedia.org/wikipedia/commons/a/a8/NaF.gif 2x" data-file-width="560" data-file-height="245" /></a><figcaption><a href="/wiki/Sodium" title="Sodium">Sodium</a> "gives" one outer electron to <a href="/wiki/Fluorine" title="Fluorine">fluorine</a>, bonding them to form <a href="/wiki/Sodium_fluoride" title="Sodium fluoride">sodium fluoride</a>. The sodium atom is oxidized, and fluorine is reduced.</figcaption></figure> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><span><video id="mwe_player_0" poster="//upload.wikimedia.org/wikipedia/commons/thumb/2/20/16._%D0%A0%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%98%D0%B0_%D0%BC%D0%B5%D1%93%D1%83_%D1%81%D0%B8%D0%BB%D0%BD%D0%BE_%D0%BE%D0%BA%D1%81%D0%B8%D0%B4%D0%B0%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D0%B8_%D1%80%D0%B5%D0%B4%D1%83%D0%BA%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D1%81%D1%80%D0%B5%D0%B4%D1%81%D1%82%D0%B2%D0%BE.webm/280px--16._%D0%A0%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%98%D0%B0_%D0%BC%D0%B5%D1%93%D1%83_%D1%81%D0%B8%D0%BB%D0%BD%D0%BE_%D0%BE%D0%BA%D1%81%D0%B8%D0%B4%D0%B0%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D0%B8_%D1%80%D0%B5%D0%B4%D1%83%D0%BA%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D1%81%D1%80%D0%B5%D0%B4%D1%81%D1%82%D0%B2%D0%BE.webm.jpg" controls="" preload="none" data-mw-tmh="" class="mw-file-element" width="280" height="158" data-durationhint="47" data-mwtitle="16._Реакција_меѓу_силно_оксидационо_и_редукционо_средство.webm" data-mwprovider="wikimediacommons" resource="/wiki/File:16._%D0%A0%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%98%D0%B0_%D0%BC%D0%B5%D1%93%D1%83_%D1%81%D0%B8%D0%BB%D0%BD%D0%BE_%D0%BE%D0%BA%D1%81%D0%B8%D0%B4%D0%B0%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D0%B8_%D1%80%D0%B5%D0%B4%D1%83%D0%BA%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D1%81%D1%80%D0%B5%D0%B4%D1%81%D1%82%D0%B2%D0%BE.webm"><source src="//upload.wikimedia.org/wikipedia/commons/transcoded/2/20/16._%D0%A0%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%98%D0%B0_%D0%BC%D0%B5%D1%93%D1%83_%D1%81%D0%B8%D0%BB%D0%BD%D0%BE_%D0%BE%D0%BA%D1%81%D0%B8%D0%B4%D0%B0%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D0%B8_%D1%80%D0%B5%D0%B4%D1%83%D0%BA%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D1%81%D1%80%D0%B5%D0%B4%D1%81%D1%82%D0%B2%D0%BE.webm/16._%D0%A0%D0%B5%D0%B0%D0%BA%D1%86%D0%B8%D1%98%D0%B0_%D0%BC%D0%B5%D1%93%D1%83_%D1%81%D0%B8%D0%BB%D0%BD%D0%BE_%D0%BE%D0%BA%D1%81%D0%B8%D0%B4%D0%B0%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D0%B8_%D1%80%D0%B5%D0%B4%D1%83%D0%BA%D1%86%D0%B8%D0%BE%D0%BD%D0%BE_%D1%81%D1%80%D0%B5%D0%B4%D1%81%D1%82%D0%B2%D0%BE.webm.480p.vp9.webm" type="video/webm; 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codecs="vp8, vorbis"" data-transcodekey="360p.webm" data-width="640" data-height="360" /></video></span><figcaption>When a few drops of <a href="/wiki/Glycerol" title="Glycerol">glycerol</a> (mild reducing agent) are added to powdered <a href="/wiki/Potassium_permanganate" title="Potassium permanganate">potassium permanganate</a> (strong oxidizing agent), a violent redox reaction accompanied by self-ignition starts.</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Redox_example.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/19/Redox_example.svg/170px-Redox_example.svg.png" decoding="async" width="170" height="302" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/19/Redox_example.svg/255px-Redox_example.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/19/Redox_example.svg/340px-Redox_example.svg.png 2x" data-file-width="512" data-file-height="910" /></a><figcaption>Example of a <a class="mw-selflink selflink">reduction–oxidation</a> reaction between sodium and chlorine, with the <span class="nowrap"><i>OIL RIG</i></span> mnemonic<sup id="cite_ref-1" class="reference"><a href="#cite_note-1"><span class="cite-bracket">[</span>1<span class="cite-bracket">]</span></a></sup></figcaption></figure> <p><b>Redox</b> (<span class="rt-commentedText nowrap"><span class="IPA nopopups noexcerpt" lang="en-fonipa"><a href="/wiki/Help:IPA/English" title="Help:IPA/English">/<span style="border-bottom:1px dotted"><span title="/ˈ/: primary stress follows">ˈ</span><span title="'r' in 'rye'">r</span><span title="/ɛ/: 'e' in 'dress'">ɛ</span><span title="'d' in 'dye'">d</span><span title="/ɒ/: 'o' in 'body'">ɒ</span><span title="'k' in 'kind'">k</span><span title="'s' in 'sigh'">s</span></span>/</a></span></span> <a href="/wiki/Help:Pronunciation_respelling_key" title="Help:Pronunciation respelling key"><i title="English pronunciation respelling"><span style="font-size:90%">RED</span>-oks</i></a>, <span class="rt-commentedText nowrap"><span class="IPA nopopups noexcerpt" lang="en-fonipa"><a href="/wiki/Help:IPA/English" title="Help:IPA/English">/<span style="border-bottom:1px dotted"><span title="/ˈ/: primary stress follows">ˈ</span><span title="'r' in 'rye'">r</span><span title="/iː/: 'ee' in 'fleece'">iː</span><span title="'d' in 'dye'">d</span><span title="/ɒ/: 'o' in 'body'">ɒ</span><span title="'k' in 'kind'">k</span><span title="'s' in 'sigh'">s</span></span>/</a></span></span> <a href="/wiki/Help:Pronunciation_respelling_key" title="Help:Pronunciation respelling key"><i title="English pronunciation respelling"><span style="font-size:90%">REE</span>-doks</i></a>, <b>reduction–oxidation</b><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> or <b>oxidation–reduction</b><sup id="cite_ref-Petrucci2002_3-0" class="reference"><a href="#cite_note-Petrucci2002-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: 150">: 150 </span></sup>) is a type of <a href="/wiki/Chemical_reaction" title="Chemical reaction">chemical reaction</a> in which the <a href="/wiki/Oxidation_state" title="Oxidation state">oxidation states</a> of the <a href="/wiki/Reactant" class="mw-redirect" title="Reactant">reactants</a> change.<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> Oxidation is the loss of <a href="/wiki/Electron" title="Electron">electrons</a> or an increase in the oxidation state, while reduction is the gain of electrons or a decrease in the oxidation state. The oxidation and reduction processes occur simultaneously in the chemical reaction. </p><p>There are two classes of redox reactions: </p> <ul><li><a href="/wiki/Electron_transfer" title="Electron transfer">Electron-transfer</a> – Only one (usually) electron flows from the atom, ion, or molecule being oxidized to the atom, ion, or molecule that is reduced. This type of redox reaction is often discussed in terms of redox couples and electrode potentials.</li> <li>Atom transfer – An atom transfers from one <a href="/wiki/Substrate_(chemistry)" title="Substrate (chemistry)">substrate</a> to another. For example, in the <a href="/wiki/Rusting" class="mw-redirect" title="Rusting">rusting</a> of <a href="/wiki/Iron" title="Iron">iron</a>, the oxidation state of iron atoms increases as the iron converts to an <a href="/wiki/Oxide" title="Oxide">oxide</a>, and simultaneously, the oxidation state of oxygen decreases as it accepts electrons released by the iron. Although oxidation reactions are commonly associated with forming oxides, other chemical species can serve the same function.<sup id="cite_ref-gale_5-0" class="reference"><a href="#cite_note-gale-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> In <a href="/wiki/Hydrogenation" title="Hydrogenation">hydrogenation</a>, bonds like <a href="/wiki/Alkene" title="Alkene">C=C</a> are reduced by <a href="/wiki/Transfer_hydrogenation" title="Transfer hydrogenation">transfer of hydrogen atoms</a>.</li></ul> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Terminology">Terminology</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=1" title="Edit section: Terminology"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>"Redox" is a <a href="/wiki/Portmanteau" class="mw-redirect" title="Portmanteau">portmanteau</a> of the words "REDuction" and "OXidation." The term "redox" was first used in 1928.<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> </p><p>Oxidation is a process in which a substance loses electrons. Reduction is a process in which a substance gains electrons. </p><p>The processes of oxidation and reduction occur simultaneously and cannot occur independently.<sup id="cite_ref-gale_5-1" class="reference"><a href="#cite_note-gale-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> In redox processes, the reductant transfers electrons to the oxidant. Thus, in the reaction, the reductant or <a href="/wiki/Reducing_agent" title="Reducing agent">reducing agent</a> loses electrons and is oxidized, and the oxidant or <a href="/wiki/Oxidizing_agent" title="Oxidizing agent">oxidizing agent</a> gains electrons and is reduced. The pair of an oxidizing and reducing agent that is involved in a particular reaction is called a redox pair. A redox couple is a reducing species and its corresponding oxidizing form,<sup id="cite_ref-7" class="reference"><a href="#cite_note-7"><span class="cite-bracket">[</span>7<span class="cite-bracket">]</span></a></sup> e.g., <span class="chemf nowrap"><a href="/wiki/Iron" title="Iron">Fe<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:0.8em;line-height:1em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">2+</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sub></span></span></a></span>/ <span class="chemf nowrap"><a href="/wiki/Iron" title="Iron">Fe<span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:0.8em;line-height:1em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">3+</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline"></sub></span></span></a></span>.The oxidation alone and the reduction alone are each called a <i><a href="/wiki/Half-reaction" title="Half-reaction">half-reaction</a></i> because two half-reactions always occur together to form a whole reaction.<sup id="cite_ref-gale_5-2" class="reference"><a href="#cite_note-gale-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> </p><p>In <a href="/wiki/Electrochemistry" title="Electrochemistry">electrochemical reactions</a> the oxidation and reduction processes do occur simultaneously but are separated in space. </p> <div class="mw-heading mw-heading3"><h3 id="Oxidants">Oxidants</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=2" title="Edit section: Oxidants"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Oxidizing_agent" title="Oxidizing agent">Oxidizing agent</a></div> <p>Oxidation originally implied a reaction with oxygen to form an oxide. Later, the term was expanded to encompass <a href="/wiki/Chemical_substance" title="Chemical substance">substances</a> that accomplished chemical reactions similar to those of oxygen. Ultimately, the meaning was generalized to include all processes involving the loss of electrons or the increase in the oxidation state of a chemical species.<sup id="cite_ref-Petrucci2017_8-0" class="reference"><a href="#cite_note-Petrucci2017-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: A49">: A49 </span></sup> Substances that have the ability to oxidize other substances (cause them to lose electrons) are said to be oxidative or oxidizing, and are known as <a href="/wiki/Oxidizing_agent" title="Oxidizing agent">oxidizing agents</a>, oxidants, or oxidizers. The oxidant removes electrons from another substance, and is thus itself reduced.<sup id="cite_ref-Petrucci2017_8-1" class="reference"><a href="#cite_note-Petrucci2017-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: A50">: A50 </span></sup> Because it "accepts" electrons, the oxidizing agent is also called an <a href="/wiki/Electron_acceptor" title="Electron acceptor">electron acceptor</a>. Oxidants are usually chemical substances with elements in high oxidation states<sup id="cite_ref-Petrucci2002_3-1" class="reference"><a href="#cite_note-Petrucci2002-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: 159">: 159 </span></sup> (e.g., <span class="chemf nowrap"><a href="/wiki/Dinitrogen_tetroxide" title="Dinitrogen tetroxide">N<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">2</sub></span></span>O<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">4</sub></span></span></a></span>, <span class="chemf nowrap"><a href="/wiki/Permanganate" title="Permanganate">MnO<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">4</sub></span></span></a></span>, <span class="chemf nowrap"><a href="/wiki/Chromium_trioxide" title="Chromium trioxide">CrO<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">3</sub></span></span></a></span>, <span class="chemf nowrap"><a href="/wiki/Dichromate" class="mw-redirect" title="Dichromate">Cr<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">2</sub></span></span>O<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">2−</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">7</sub></span></span></a></span>, <span class="chemf nowrap"><a href="/wiki/Osmium(VIII)_oxide" class="mw-redirect" title="Osmium(VIII) oxide">OsO<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">4</sub></span></span></a></span>), or else highly <a href="/wiki/Electronegativity" title="Electronegativity">electronegative</a> elements (e.g. <a href="/wiki/Oxygen" title="Oxygen">O<sub>2</sub></a>, <a href="/wiki/Fluorine" title="Fluorine">F<sub>2</sub></a>, <a href="/wiki/Chlorine" title="Chlorine">Cl<sub>2</sub></a>, <a href="/wiki/Bromine" title="Bromine">Br<sub>2</sub></a>, <a href="/wiki/Iodine" title="Iodine">I<sub>2</sub></a>) that can gain extra electrons by oxidizing another substance.<sup id="cite_ref-Petrucci2002_3-2" class="reference"><a href="#cite_note-Petrucci2002-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: 909">: 909 </span></sup> </p><p>Oxidizers are oxidants, but the term is mainly reserved for sources of oxygen, particularly in the context of explosions. <a href="/wiki/Nitric_acid" title="Nitric acid">Nitric acid</a> is a strong oxidizer.<sup id="cite_ref-9" class="reference"><a href="#cite_note-9"><span class="cite-bracket">[</span>9<span class="cite-bracket">]</span></a></sup> </p> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:GHS-pictogram-rondflam.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e5/GHS-pictogram-rondflam.svg/170px-GHS-pictogram-rondflam.svg.png" decoding="async" width="170" height="170" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/e5/GHS-pictogram-rondflam.svg/255px-GHS-pictogram-rondflam.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/e5/GHS-pictogram-rondflam.svg/340px-GHS-pictogram-rondflam.svg.png 2x" data-file-width="724" data-file-height="724" /></a><figcaption>The <a href="/wiki/Globally_Harmonized_System_of_Classification_and_Labeling_of_Chemicals" class="mw-redirect" title="Globally Harmonized System of Classification and Labeling of Chemicals">international</a> <a href="/wiki/GHS_hazard_pictograms" title="GHS hazard pictograms">pictogram</a> for oxidizing chemicals</figcaption></figure> <div class="mw-heading mw-heading3"><h3 id="Reductants"><span class="anchor" id="reducing_equivalent"></span>Reductants</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=3" title="Edit section: Reductants"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Reducing_agent" title="Reducing agent">Reducing agent</a></div> <p>Substances that have the ability to reduce other substances (cause them to gain electrons) are said to be reductive or reducing and are known as <a href="/wiki/Reducing_agent" title="Reducing agent">reducing agents</a>, reductants, or reducers. The reductant transfers electrons to another substance and is thus itself oxidized.<sup id="cite_ref-Petrucci2002_3-3" class="reference"><a href="#cite_note-Petrucci2002-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: 159">: 159 </span></sup> Because it donates electrons, the reducing agent is also called an <a href="/wiki/Electron_donor" title="Electron donor">electron donor</a>. Electron donors can also form <a href="/wiki/Charge_transfer_complex" class="mw-redirect" title="Charge transfer complex">charge transfer complexes</a> with electron acceptors. The word reduction originally referred to the loss in weight upon heating a metallic <a href="/wiki/Ore" title="Ore">ore</a> such as a <a href="/wiki/Metal_oxide" class="mw-redirect" title="Metal oxide">metal oxide</a> to extract the metal. In other words, ore was "reduced" to metal.<sup id="cite_ref-Whitten_10-0" class="reference"><a href="#cite_note-Whitten-10"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> <a href="/wiki/Antoine_Lavoisier" title="Antoine Lavoisier">Antoine Lavoisier</a> demonstrated that this loss of weight was due to the loss of oxygen as a gas. Later, scientists realized that the metal atom gains electrons in this process. The meaning of reduction then became generalized to include all processes involving a gain of electrons.<sup id="cite_ref-Whitten_10-1" class="reference"><a href="#cite_note-Whitten-10"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> Reducing equivalent refers to <a href="/wiki/Chemical_species" title="Chemical species">chemical species</a> which transfer the equivalent of one <a href="/wiki/Electron" title="Electron">electron</a> in redox reactions. The term is common in <a href="/wiki/Biochemistry" title="Biochemistry">biochemistry</a>.<sup id="cite_ref-11" class="reference"><a href="#cite_note-11"><span class="cite-bracket">[</span>11<span class="cite-bracket">]</span></a></sup> A reducing equivalent can be an electron or a hydrogen atom as a <a href="/wiki/Hydrogen_anion" title="Hydrogen anion">hydride ion</a>.<sup id="cite_ref-Lehninger-2017_12-0" class="reference"><a href="#cite_note-Lehninger-2017-12"><span class="cite-bracket">[</span>12<span class="cite-bracket">]</span></a></sup> </p><p>Reductants in chemistry are very diverse. <a href="/wiki/Electropositive" class="mw-redirect" title="Electropositive">Electropositive</a> elemental <a href="/wiki/Metal" title="Metal">metals</a>, such as <a href="/wiki/Lithium" title="Lithium">lithium</a>, <a href="/wiki/Sodium" title="Sodium">sodium</a>, <a href="/wiki/Magnesium" title="Magnesium">magnesium</a>, <a href="/wiki/Iron" title="Iron">iron</a>, <a href="/wiki/Zinc" title="Zinc">zinc</a>, and <a href="/wiki/Aluminium" title="Aluminium">aluminium</a>, are good reducing agents. These metals donate electrons relatively readily.<sup id="cite_ref-13" class="reference"><a href="#cite_note-13"><span class="cite-bracket">[</span>13<span class="cite-bracket">]</span></a></sup> </p><p><a href="/w/index.php?title=Hydride_transfer_reagents&action=edit&redlink=1" class="new" title="Hydride transfer reagents (page does not exist)">Hydride transfer reagents</a>, such as <a href="/wiki/Sodium_borohydride" title="Sodium borohydride">NaBH<sub>4</sub></a> and <a href="/wiki/Lithium_aluminium_hydride" title="Lithium aluminium hydride">LiAlH<sub>4</sub></a>, reduce by atom transfer: they transfer the equivalent of hydride or H<sup>−</sup>. These reagents are widely used in the reduction of <a href="/wiki/Carbonyl" class="mw-redirect" title="Carbonyl">carbonyl</a> compounds to <a href="/wiki/Alcohols" class="mw-redirect" title="Alcohols">alcohols</a>.<sup id="cite_ref-14" class="reference"><a href="#cite_note-14"><span class="cite-bracket">[</span>14<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-15" class="reference"><a href="#cite_note-15"><span class="cite-bracket">[</span>15<span class="cite-bracket">]</span></a></sup> A related method of reduction involves the use of hydrogen gas (H<sub>2</sub>) as sources of H atoms.<sup id="cite_ref-Petrucci2002_3-4" class="reference"><a href="#cite_note-Petrucci2002-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: 288">: 288 </span></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Electronation_and_deelectronation">Electronation and deelectronation</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=4" title="Edit section: Electronation and deelectronation"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The <a href="/wiki/Electrochemistry" title="Electrochemistry">electrochemist</a> <a href="/wiki/John_Bockris" title="John Bockris">John Bockris</a> proposed the words electronation and de-electronation to describe reduction and oxidation processes, respectively, when they occur at <a href="/wiki/Electrode" title="Electrode">electrodes</a>.<sup id="cite_ref-16" class="reference"><a href="#cite_note-16"><span class="cite-bracket">[</span>16<span class="cite-bracket">]</span></a></sup> These words are analogous to <a href="/wiki/Protonation" title="Protonation">protonation</a> and <a href="/wiki/Deprotonation" title="Deprotonation">deprotonation</a>.<sup id="cite_ref-17" class="reference"><a href="#cite_note-17"><span class="cite-bracket">[</span>17<span class="cite-bracket">]</span></a></sup> They have not been widely adopted by chemists worldwide,<sup class="noprint Inline-Template Template-Fact" style="white-space:nowrap;">[<i><a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed"><span title="This claim needs references to reliable sources. (December 2023)">citation needed</span></a></i>]</sup> although <a href="/wiki/IUPAC" class="mw-redirect" title="IUPAC">IUPAC</a> has recognized the terms electronation<sup id="cite_ref-18" class="reference"><a href="#cite_note-18"><span class="cite-bracket">[</span>18<span class="cite-bracket">]</span></a></sup> and de-electronation.<sup id="cite_ref-19" class="reference"><a href="#cite_note-19"><span class="cite-bracket">[</span>19<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Rates,_mechanisms,_and_energies"><span id="Rates.2C_mechanisms.2C_and_energies"></span>Rates, mechanisms, and energies</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=5" title="Edit section: Rates, mechanisms, and energies"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1251242444">.mw-parser-output .ambox{border:1px solid #a2a9b1;border-left:10px solid #36c;background-color:#fbfbfb;box-sizing:border-box}.mw-parser-output .ambox+link+.ambox,.mw-parser-output .ambox+link+style+.ambox,.mw-parser-output .ambox+link+link+.ambox,.mw-parser-output .ambox+.mw-empty-elt+link+.ambox,.mw-parser-output .ambox+.mw-empty-elt+link+style+.ambox,.mw-parser-output .ambox+.mw-empty-elt+link+link+.ambox{margin-top:-1px}html body.mediawiki .mw-parser-output .ambox.mbox-small-left{margin:4px 1em 4px 0;overflow:hidden;width:238px;border-collapse:collapse;font-size:88%;line-height:1.25em}.mw-parser-output .ambox-speedy{border-left:10px solid #b32424;background-color:#fee7e6}.mw-parser-output .ambox-delete{border-left:10px solid #b32424}.mw-parser-output .ambox-content{border-left:10px solid #f28500}.mw-parser-output .ambox-style{border-left:10px solid #fc3}.mw-parser-output .ambox-move{border-left:10px solid #9932cc}.mw-parser-output .ambox-protection{border-left:10px solid #a2a9b1}.mw-parser-output .ambox .mbox-text{border:none;padding:0.25em 0.5em;width:100%}.mw-parser-output .ambox .mbox-image{border:none;padding:2px 0 2px 0.5em;text-align:center}.mw-parser-output .ambox .mbox-imageright{border:none;padding:2px 0.5em 2px 0;text-align:center}.mw-parser-output .ambox .mbox-empty-cell{border:none;padding:0;width:1px}.mw-parser-output .ambox .mbox-image-div{width:52px}@media(min-width:720px){.mw-parser-output .ambox{margin:0 10%}}@media print{body.ns-0 .mw-parser-output .ambox{display:none!important}}</style><table class="box-Expand_section plainlinks metadata ambox mbox-small-left ambox-content" role="presentation"><tbody><tr><td class="mbox-image"><span typeof="mw:File"><a href="/wiki/File:Wiki_letter_w_cropped.svg" class="mw-file-description"><img alt="[icon]" src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Wiki_letter_w_cropped.svg/20px-Wiki_letter_w_cropped.svg.png" decoding="async" width="20" height="14" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Wiki_letter_w_cropped.svg/30px-Wiki_letter_w_cropped.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/1c/Wiki_letter_w_cropped.svg/40px-Wiki_letter_w_cropped.svg.png 2x" data-file-width="44" data-file-height="31" /></a></span></td><td class="mbox-text"><div class="mbox-text-span">This section <b>needs expansion</b>. You can help by <a class="external text" href="https://en.wikipedia.org/w/index.php?title=Redox&action=edit&section=">adding to it</a>. <span class="date-container"><i>(<span class="date">April 2023</span>)</i></span></div></td></tr></tbody></table> <p>Redox reactions can occur slowly, as in the formation of <a href="/wiki/Rust" title="Rust">rust</a>, or rapidly, as in the case of burning <a href="/wiki/Fuel" title="Fuel">fuel</a>. Electron transfer reactions are generally fast, occurring within the time of mixing.<sup id="cite_ref-20" class="reference"><a href="#cite_note-20"><span class="cite-bracket">[</span>20<span class="cite-bracket">]</span></a></sup> </p><p>The mechanisms of atom-transfer reactions are highly variable because many kinds of atoms can be transferred. Such reactions can also be quite complex, involving many steps. The mechanisms of electron-transfer reactions occur by two distinct pathways, <a href="/wiki/Inner_sphere_electron_transfer" title="Inner sphere electron transfer">inner sphere electron transfer</a><sup id="cite_ref-21" class="reference"><a href="#cite_note-21"><span class="cite-bracket">[</span>21<span class="cite-bracket">]</span></a></sup> and <a href="/wiki/Outer_sphere_electron_transfer" title="Outer sphere electron transfer">outer sphere electron transfer</a>.<sup id="cite_ref-22" class="reference"><a href="#cite_note-22"><span class="cite-bracket">[</span>22<span class="cite-bracket">]</span></a></sup> </p><p>Analysis of bond energies and <a href="/wiki/Ionization_energy" title="Ionization energy">ionization energies</a> in water allows calculation of the thermodynamic aspects of redox reactions.<sup id="cite_ref-23" class="reference"><a href="#cite_note-23"><span class="cite-bracket">[</span>23<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Standard_electrode_potentials_(reduction_potentials)"><span id="Standard_electrode_potentials_.28reduction_potentials.29"></span>Standard electrode potentials (reduction potentials)</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=6" title="Edit section: Standard electrode potentials (reduction potentials)"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1251242444"><table class="box-More_citations_needed plainlinks metadata ambox ambox-content ambox-Refimprove" role="presentation"><tbody><tr><td class="mbox-image"><div class="mbox-image-div"><span typeof="mw:File"><a href="/wiki/File:Question_book-new.svg" class="mw-file-description"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/50px-Question_book-new.svg.png" decoding="async" width="50" height="39" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/75px-Question_book-new.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/100px-Question_book-new.svg.png 2x" data-file-width="512" data-file-height="399" /></a></span></div></td><td class="mbox-text"><div class="mbox-text-span">This section <b>needs additional citations for <a href="/wiki/Wikipedia:Verifiability" title="Wikipedia:Verifiability">verification</a></b>.<span class="hide-when-compact"> Please help <a href="/wiki/Special:EditPage/Redox" title="Special:EditPage/Redox">improve this article</a> by <a href="/wiki/Help:Referencing_for_beginners" title="Help:Referencing for beginners">adding citations to reliable sources</a> in this section. Unsourced material may be challenged and removed.<br /><small><span class="plainlinks"><i>Find sources:</i> <a rel="nofollow" class="external text" href="https://www.google.com/search?as_eq=wikipedia&q=%22Redox%22">"Redox"</a> – <a rel="nofollow" class="external text" href="https://www.google.com/search?tbm=nws&q=%22Redox%22+-wikipedia&tbs=ar:1">news</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.google.com/search?&q=%22Redox%22&tbs=bkt:s&tbm=bks">newspapers</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.google.com/search?tbs=bks:1&q=%22Redox%22+-wikipedia">books</a> <b>·</b> <a rel="nofollow" class="external text" href="https://scholar.google.com/scholar?q=%22Redox%22">scholar</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.jstor.org/action/doBasicSearch?Query=%22Redox%22&acc=on&wc=on">JSTOR</a></span></small></span> <span class="date-container"><i>(<span class="date">December 2023</span>)</i></span><span class="hide-when-compact"><i> (<small><a href="/wiki/Help:Maintenance_template_removal" title="Help:Maintenance template removal">Learn how and when to remove this message</a></small>)</i></span></div></td></tr></tbody></table> <p>Each half-reaction has a standard <a href="/wiki/Electrode_potential" title="Electrode potential">electrode potential</a> (<i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">cell</sub></span></span>), which is equal to the potential difference or <a href="/wiki/Voltage" title="Voltage">voltage</a> at equilibrium under <a href="/wiki/Standard_state" title="Standard state">standard conditions</a> of an <a href="/wiki/Electrochemical_cell" title="Electrochemical cell">electrochemical cell</a> in which the <a href="/wiki/Cathode" title="Cathode">cathode</a> reaction is the <a href="/wiki/Half-reaction" title="Half-reaction">half-reaction</a> considered, and the <a href="/wiki/Anode" title="Anode">anode</a> is a <a href="/wiki/Standard_hydrogen_electrode" title="Standard hydrogen electrode">standard hydrogen electrode</a> where hydrogen is oxidized:<sup id="cite_ref-24" class="reference"><a href="#cite_note-24"><span class="cite-bracket">[</span>24<span class="cite-bracket">]</span></a></sup> </p> <dl><dd><style data-mw-deduplicate="TemplateStyles:r1154941027">.mw-parser-output .frac{white-space:nowrap}.mw-parser-output .frac .num,.mw-parser-output .frac .den{font-size:80%;line-height:0;vertical-align:super}.mw-parser-output .frac .den{vertical-align:sub}.mw-parser-output .sr-only{border:0;clip:rect(0,0,0,0);clip-path:polygon(0px 0px,0px 0px,0px 0px);height:1px;margin:-1px;overflow:hidden;padding:0;position:absolute;width:1px}</style><span class="frac"><span class="num">1</span>⁄<span class="den">2</span></span>H<sub>2</sub> → H<sup>+</sup> + e<sup>−</sup></dd></dl> <p>The electrode potential of each half-reaction is also known as its reduction potential (<i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">red</sub></span></span>), or potential when the half-reaction takes place at a cathode. The reduction potential is a measure of the tendency of the oxidizing agent to be reduced. Its value is zero for H<sup>+</sup> + e<sup>−</sup> → <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1154941027"><span class="frac"><span class="num">1</span>⁄<span class="den">2</span></span>H<sub>2</sub> by definition, positive for oxidizing agents stronger than H<sup>+</sup> (e.g., +2.866 V for F<sub>2</sub>) and negative for oxidizing agents that are weaker than H<sup>+</sup> (e.g., −0.763V for Zn<sup>2+</sup>).<sup id="cite_ref-Petrucci2017_8-2" class="reference"><a href="#cite_note-Petrucci2017-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: 873">: 873 </span></sup> </p><p>For a redox reaction that takes place in a cell, the potential difference is: </p> <dl><dd><i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">cell</sub></span></span> = <i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">cathode</sub></span></span> – <i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">anode</sub></span></span></dd></dl> <p>However, the potential of the reaction at the anode is sometimes expressed as an <i>oxidation potential</i>: </p> <dl><dd><i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">ox</sub></span></span> = –<i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">red</sub></span></span></dd></dl> <p>The oxidation potential is a measure of the tendency of the reducing agent to be oxidized but does not represent the physical potential at an electrode. With this notation, the cell voltage equation is written with a plus sign </p> <dl><dd><i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">cell</sub></span></span> = <i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">red(cathode)</sub></span></span> + <i>E</i><span class="nowrap"><span style="display:inline-block;margin-bottom:-0.3em;vertical-align:-0.4em;line-height:1.2em;font-size:80%;text-align:left"><sup style="font-size:inherit;line-height:inherit;vertical-align:baseline">o</sup><br /><sub style="font-size:inherit;line-height:inherit;vertical-align:baseline">ox(anode)</sub></span></span></dd></dl> <div class="mw-heading mw-heading2"><h2 id="Examples_of_redox_reactions">Examples of redox reactions</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=7" title="Edit section: Examples of redox reactions"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1251242444"><table class="box-Unreferenced_section plainlinks metadata ambox ambox-content ambox-Unreferenced" role="presentation"><tbody><tr><td class="mbox-image"><div class="mbox-image-div"><span typeof="mw:File"><a href="/wiki/File:Question_book-new.svg" class="mw-file-description"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/50px-Question_book-new.svg.png" decoding="async" width="50" height="39" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/75px-Question_book-new.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/100px-Question_book-new.svg.png 2x" data-file-width="512" data-file-height="399" /></a></span></div></td><td class="mbox-text"><div class="mbox-text-span">This section <b>does not <a href="/wiki/Wikipedia:Citing_sources" title="Wikipedia:Citing sources">cite</a> any <a href="/wiki/Wikipedia:Verifiability" title="Wikipedia:Verifiability">sources</a></b>.<span class="hide-when-compact"> Please help <a href="/wiki/Special:EditPage/Redox" title="Special:EditPage/Redox">improve this section</a> by <a href="/wiki/Help:Referencing_for_beginners" title="Help:Referencing for beginners">adding citations to reliable sources</a>. Unsourced material may be challenged and <a href="/wiki/Wikipedia:Verifiability#Burden_of_evidence" title="Wikipedia:Verifiability">removed</a>.</span> <span class="date-container"><i>(<span class="date">December 2023</span>)</i></span><span class="hide-when-compact"><i> (<small><a href="/wiki/Help:Maintenance_template_removal" title="Help:Maintenance template removal">Learn how and when to remove this message</a></small>)</i></span></div></td></tr></tbody></table><figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Redox_reaction.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/ee/Redox_reaction.png/300px-Redox_reaction.png" decoding="async" width="300" height="129" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/e/ee/Redox_reaction.png 1.5x" data-file-width="391" data-file-height="168" /></a><figcaption>Illustration of a redox reaction</figcaption></figure> <p>In the reaction between <a href="/wiki/Hydrogen" title="Hydrogen">hydrogen</a> and <a href="/wiki/Fluorine" title="Fluorine">fluorine</a>, hydrogen is being oxidized and fluorine is being reduced: </p> <dl><dd><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">H<sub class="template-chem2-sub">2</sub> + F<sub class="template-chem2-sub">2</sub> → 2 HF</span></dd></dl> <p>This spontaneous reaction releases 542 kJ per 2 g of hydrogen because the H-F bond is much stronger than the F-F bond. This reaction can be analyzed as two <a href="/wiki/Half-reaction" title="Half-reaction">half-reactions</a>. The oxidation reaction converts hydrogen to <a href="/wiki/Proton" title="Proton">protons</a>: </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> → 2 <a href="/wiki/Hydrogen_ion" title="Hydrogen ion">H<sup>+</sup></a> + 2 <a href="/wiki/Electron" title="Electron">e<sup>−</sup></a></span></dd></dl> <p>The reduction reaction converts <a href="/wiki/Fluorine" title="Fluorine">fluorine</a> to the fluoride anion: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">F<sub class="template-chem2-sub">2</sub> + 2 e<sup>−</sup> → 2 <a href="/wiki/Fluoride" title="Fluoride">F<sup>−</sup></a></span></dd></dl> <p>The half-reactions are combined so that the electrons cancel: </p> <dl><dd><table> <tbody><tr> <td align="right"><span class="chemf nowrap">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">2</sub></span></span></span> </td> <td>→ </td> <td align="left">2 H<sup>+</sup> + 2 e<sup>−</sup> </td></tr> <tr> <td align="right"><span class="chemf nowrap">F<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">2</sub></span></span></span> + 2 e<sup>−</sup> </td> <td>→ </td> <td align="left">2 F<sup>−</sup> </td></tr> <tr> <td colspan="3"><hr /> </td></tr> <tr> <td align="right">H<sub>2</sub> + F<sub>2</sub> </td> <td>→ </td> <td align="left">2 H<sup>+</sup> + 2 F<sup>−</sup> </td></tr></tbody></table></dd></dl> <p>The protons and fluoride combine to form <a href="/wiki/Hydrofluoric_acid" title="Hydrofluoric acid">hydrogen fluoride</a> in a non-redox reaction: </p> <dl><dd>2 H<sup>+</sup> + 2 F<sup>−</sup> → 2 HF</dd></dl> <p>The overall reaction is: </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> + F<sub class="template-chem2-sub">2</sub> → 2 HF</span></dd></dl> <div class="mw-heading mw-heading3"><h3 id="Metal_displacement">Metal displacement</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=8" title="Edit section: Metal displacement"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Galvanic_cell_with_no_cation_flow.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/6/6d/Galvanic_cell_with_no_cation_flow.svg/350px-Galvanic_cell_with_no_cation_flow.svg.png" decoding="async" width="350" height="203" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/6/6d/Galvanic_cell_with_no_cation_flow.svg/525px-Galvanic_cell_with_no_cation_flow.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/6/6d/Galvanic_cell_with_no_cation_flow.svg/700px-Galvanic_cell_with_no_cation_flow.svg.png 2x" data-file-width="512" data-file-height="297" /></a><figcaption>A redox reaction is the force behind an <a href="/wiki/Electrochemical_cell" title="Electrochemical cell">electrochemical cell</a> like the <a href="/wiki/Galvanic_cell" title="Galvanic cell">Galvanic cell</a> pictured. The battery is made out of a zinc electrode in a ZnSO<sub>4</sub> solution connected with a wire and a porous disk to a copper electrode in a CuSO<sub>4</sub> solution.</figcaption></figure> <p>In this type of reaction, a <a href="/wiki/Metal" title="Metal">metal</a> atom in a compound or solution is replaced by an atom of another metal. For example, <a href="/wiki/Copper" title="Copper">copper</a> is deposited when <a href="/wiki/Zinc" title="Zinc">zinc</a> metal is placed in a <a href="/wiki/Copper(II)_sulfate" title="Copper(II) sulfate">copper(II) sulfate</a> solution: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Zn (s) + CuSO<sub class="template-chem2-sub">4</sub> (aq) → ZnSO<sub class="template-chem2-sub">4</sub> (aq) + Cu (s)</span></dd></dl> <p>In the above reaction, zinc metal displaces the copper(II) ion from the copper sulfate solution, thus liberating free copper metal. The reaction is spontaneous and releases 213 kJ per 65 g of zinc. </p><p>The ionic equation for this reaction is: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Zn + Cu<sup>2+</sup> → Zn<sup>2+</sup> + Cu</span></dd></dl> <p>As two <a href="/wiki/Half-reaction" title="Half-reaction">half-reactions</a>, it is seen that the zinc is oxidized: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Zn → Zn<sup>2+</sup> + 2 e<sup>−</sup></span></dd></dl> <p>And the copper is reduced: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Cu<sup>2+</sup> + 2 e<sup>−</sup> → Cu</span></dd></dl> <div class="mw-heading mw-heading3"><h3 id="Other_examples">Other examples</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=9" title="Edit section: Other examples"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li>The reduction of <a href="/wiki/Nitrate" title="Nitrate">nitrate</a> to <a href="/wiki/Nitrogen" title="Nitrogen">nitrogen</a> in the presence of an acid (<a href="/wiki/Denitrification" title="Denitrification">denitrification</a>):</li></ul> <dl><dd><dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 NO<span class="template-chem2-su"><span>−</span><span>3</span></span> + 10 e<sup>−</sup> + 12 H<sup>+</sup> → N<sub class="template-chem2-sub">2</sub> + 6 H<sub class="template-chem2-sub">2</sub>O</span></dd></dl></dd></dl> <ul><li>The <a href="/wiki/Combustion" title="Combustion">combustion</a> of <a href="/wiki/Hydrocarbon" title="Hydrocarbon">hydrocarbons</a>, such as in an <a href="/wiki/Internal_combustion_engine" title="Internal combustion engine">internal combustion engine</a>, produces <a href="/wiki/Water" title="Water">water</a>, <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a>, some partially oxidized forms such as <a href="/wiki/Carbon_monoxide" title="Carbon monoxide">carbon monoxide</a>, and heat <a href="/wiki/Energy" title="Energy">energy</a>. Complete oxidation of materials containing <a href="/wiki/Carbon" title="Carbon">carbon</a> produces carbon dioxide.</li> <li>The stepwise oxidation of a hydrocarbon by oxygen, in <a href="/wiki/Organic_chemistry" title="Organic chemistry">organic chemistry</a>, produces water and, successively: an <a href="/wiki/Alcohol_(chemistry)" title="Alcohol (chemistry)">alcohol</a>, an <a href="/wiki/Aldehyde" title="Aldehyde">aldehyde</a> or a <a href="/wiki/Ketone" title="Ketone">ketone</a>, a <a href="/wiki/Carboxylic_acid" title="Carboxylic acid">carboxylic acid</a>, and then a <a href="/wiki/Peroxide" title="Peroxide">peroxide</a>.</li></ul> <div class="mw-heading mw-heading3"><h3 id="Corrosion_and_rusting">Corrosion and rusting</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=10" title="Edit section: Corrosion and rusting"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Rust_screw.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4d/Rust_screw.jpg/220px-Rust_screw.jpg" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4d/Rust_screw.jpg/330px-Rust_screw.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/4d/Rust_screw.jpg/440px-Rust_screw.jpg 2x" data-file-width="1024" data-file-height="768" /></a><figcaption>Oxides, such as <a href="/wiki/Iron(III)_oxide" title="Iron(III) oxide">iron(III) oxide</a> or <a href="/wiki/Rust" title="Rust">rust</a>, which consists of hydrated <a href="/wiki/Iron(III)_oxide" title="Iron(III) oxide">iron(III) oxides</a> Fe<sub>2</sub>O<sub>3</sub>·<i>n</i>H<sub>2</sub>O and <a href="/wiki/Iron(III)_oxide-hydroxide" title="Iron(III) oxide-hydroxide">iron(III) oxide-hydroxide</a> (FeO(OH), Fe(OH)<sub>3</sub>), form when oxygen combines with other elements.</figcaption></figure> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:PyOx.JPG" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/e/e1/PyOx.JPG/220px-PyOx.JPG" decoding="async" width="220" height="165" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/e/e1/PyOx.JPG/330px-PyOx.JPG 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/e/e1/PyOx.JPG/440px-PyOx.JPG 2x" data-file-width="3648" data-file-height="2736" /></a><figcaption>Iron rusting in <a href="/wiki/Pyrite" title="Pyrite">pyrite</a> cubes</figcaption></figure> <ul><li>The term <a href="/wiki/Corrosion" title="Corrosion">corrosion</a> refers to the electrochemical oxidation of metals in reaction with an oxidant such as oxygen. <a href="/wiki/Rust" title="Rust">Rusting</a>, the formation of <a href="/wiki/Iron_oxide" title="Iron oxide">iron oxides</a>, is a well-known example of electrochemical corrosion: it forms as a result of the oxidation of <a href="/wiki/Iron" title="Iron">iron</a> metal. Common rust often refers to <a href="/wiki/Iron(III)_oxide" title="Iron(III) oxide">iron(III) oxide</a>, formed in the following chemical reaction:</li></ul> <dl><dd><dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">4 Fe + 3 O<sub class="template-chem2-sub">2</sub> → 2 Fe<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">3</sub></span></dd></dl></dd></dl> <ul><li>The oxidation of iron(II) to iron(III) by <a href="/wiki/Hydrogen_peroxide" title="Hydrogen peroxide">hydrogen peroxide</a> in the presence of an <a href="/wiki/Acid" title="Acid">acid</a>:</li></ul> <dl><dd><dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">Fe<sup>2+</sup> → Fe<sup>3+</sup> + e<sup>−</sup></span></dd> <dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">H<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">2</sub> + 2 e<sup>−</sup> → 2 OH<sup>−</sup></span></dd></dl></dd> <dd>Here the overall equation involves adding the reduction equation to twice the oxidation equation, so that the electrons cancel: <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">2 Fe<sup>2+</sup> + H<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">2</sub> + 2 H<sup>+</sup> → 2 Fe<sup>3+</sup> + 2 H<sub class="template-chem2-sub">2</sub>O</span></dd></dl></dd></dl> <div class="mw-heading mw-heading3"><h3 id="Disproportionation">Disproportionation</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=11" title="Edit section: Disproportionation"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>A <a href="/wiki/Disproportionation" title="Disproportionation">disproportionation</a> reaction is one in which a single substance is both oxidized and reduced. For example, <a href="/wiki/Thiosulfate" title="Thiosulfate">thiosulfate</a> ion with sulfur in oxidation state +2 can react in the presence of acid to form elemental sulfur (oxidation state 0) and <a href="/wiki/Sulfur_dioxide" title="Sulfur dioxide">sulfur dioxide</a> (oxidation state +4). </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">S<sub class="template-chem2-sub">2</sub>O<span class="template-chem2-su"><span>2−</span><span>3</span></span> + 2 H<sup>+</sup> → S + SO<sub class="template-chem2-sub">2</sub> + H<sub class="template-chem2-sub">2</sub>O</span></dd></dl> <p>Thus one sulfur atom is reduced from +2 to 0, while the other is oxidized from +2 to +4.<sup id="cite_ref-Petrucci2017_8-3" class="reference"><a href="#cite_note-Petrucci2017-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup><sup class="reference nowrap"><span title="Page / location: 176">: 176 </span></sup> </p> <div class="mw-heading mw-heading2"><h2 id="Redox_reactions_in_industry">Redox reactions in industry</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=12" title="Edit section: Redox reactions in industry"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p><a href="/wiki/Cathodic_protection" title="Cathodic protection">Cathodic protection</a> is a technique used to control the corrosion of a metal surface by making it the <a href="/wiki/Cathode" title="Cathode">cathode</a> of an <a href="/wiki/Electrochemical_cell" title="Electrochemical cell">electrochemical cell</a>. A simple method of protection connects protected metal to a more easily corroded "<a href="/wiki/Sacrificial_anode" class="mw-redirect" title="Sacrificial anode">sacrificial anode</a>" to act as the <a href="/wiki/Anode" title="Anode">anode</a>. The sacrificial metal, instead of the protected metal, then corrodes. A common application of cathodic protection is in <a href="/wiki/Galvanization" title="Galvanization">galvanized</a> steel, in which a sacrificial zinc coating on steel parts protects them from rust.<sup class="noprint Inline-Template Template-Fact" style="white-space:nowrap;">[<i><a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed"><span title="This claim needs references to reliable sources. (February 2024)">citation needed</span></a></i>]</sup> </p><p>Oxidation is used in a wide variety of industries, such as in the production of <a href="/wiki/Category:Cleaning_products" title="Category:Cleaning products">cleaning products</a> and oxidizing <a href="/wiki/Ammonia" title="Ammonia">ammonia</a> to produce <a href="/wiki/Nitric_acid" title="Nitric acid">nitric acid</a>.<sup class="noprint Inline-Template Template-Fact" style="white-space:nowrap;">[<i><a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed"><span title="This claim needs references to reliable sources. (February 2024)">citation needed</span></a></i>]</sup> </p><p>Redox reactions are the foundation of electrochemical cells, which can generate electrical energy or support <a href="/wiki/Electrosynthesis" title="Electrosynthesis">electrosynthesis</a>. Metal <a href="/wiki/Ore" title="Ore">ores</a> often contain metals in oxidized states, such as oxides or sulfides, from which the pure metals are extracted by <a href="/wiki/Smelting" title="Smelting">smelting</a> at high temperatures in the presence of a reducing agent. The process of <a href="/wiki/Electroplating" title="Electroplating">electroplating</a> uses redox reactions to coat objects with a thin layer of a material, as in <a href="/wiki/Chrome_plating" title="Chrome plating">chrome-plated</a> <a href="/wiki/Automotive" class="mw-redirect" title="Automotive">automotive</a> parts, <a href="/wiki/Plating#Silver_plating" title="Plating">silver plating</a> <a href="/wiki/Cutlery" title="Cutlery">cutlery</a>, <a href="/wiki/Galvanization" title="Galvanization">galvanization</a> and <a href="/wiki/Gold-plated" class="mw-redirect" title="Gold-plated">gold-plated</a> <a href="/wiki/Jewelry" class="mw-redirect" title="Jewelry">jewelry</a>.<sup class="noprint Inline-Template Template-Fact" style="white-space:nowrap;">[<i><a href="/wiki/Wikipedia:Citation_needed" title="Wikipedia:Citation needed"><span title="This claim needs references to reliable sources. (February 2024)">citation needed</span></a></i>]</sup> </p> <div class="mw-heading mw-heading2"><h2 id="Redox_reactions_in_biology">Redox reactions in biology</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=13" title="Edit section: Redox reactions in biology"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1251242444"><table class="box-Unreferenced_section plainlinks metadata ambox ambox-content ambox-Unreferenced" role="presentation"><tbody><tr><td class="mbox-image"><div class="mbox-image-div"><span typeof="mw:File"><a href="/wiki/File:Question_book-new.svg" class="mw-file-description"><img alt="" src="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/50px-Question_book-new.svg.png" decoding="async" width="50" height="39" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/75px-Question_book-new.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/100px-Question_book-new.svg.png 2x" data-file-width="512" data-file-height="399" /></a></span></div></td><td class="mbox-text"><div class="mbox-text-span">This section <b>does not <a href="/wiki/Wikipedia:Citing_sources" title="Wikipedia:Citing sources">cite</a> any <a href="/wiki/Wikipedia:Verifiability" title="Wikipedia:Verifiability">sources</a></b>.<span class="hide-when-compact"> Please help <a href="/wiki/Special:EditPage/Redox" title="Special:EditPage/Redox">improve this section</a> by <a href="/wiki/Help:Referencing_for_beginners" title="Help:Referencing for beginners">adding citations to reliable sources</a>. Unsourced material may be challenged and <a href="/wiki/Wikipedia:Verifiability#Burden_of_evidence" title="Wikipedia:Verifiability">removed</a>.</span> <span class="date-container"><i>(<span class="date">December 2023</span>)</i></span><span class="hide-when-compact"><i> (<small><a href="/wiki/Help:Maintenance_template_removal" title="Help:Maintenance template removal">Learn how and when to remove this message</a></small>)</i></span></div></td></tr></tbody></table><div class="thumb tleft" style="background-color: #f9f9f9; border: 1px solid #CCCCCC; margin:0.5em;"> <table border="0" width="150px" cellpadding="2" cellspacing="0" style="font-size: 85%; border: 1px solid #CCCCCC; margin: 0.3em;"> <tbody><tr> <td><span typeof="mw:File"><a href="/wiki/File:Ascorbic_acid_structure.svg" class="mw-file-description" title="ascorbic acid"><img alt="ascorbic acid" src="//upload.wikimedia.org/wikipedia/commons/thumb/5/57/Ascorbic_acid_structure.svg/150px-Ascorbic_acid_structure.svg.png" decoding="async" width="150" height="150" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/57/Ascorbic_acid_structure.svg/225px-Ascorbic_acid_structure.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/57/Ascorbic_acid_structure.svg/300px-Ascorbic_acid_structure.svg.png 2x" data-file-width="128" data-file-height="128" /></a></span> </td></tr></tbody></table> <table border="0" width="150px" cellpadding="2" cellspacing="0" style="font-size: 85%; border: 1px solid #CCCCCC; margin: 0.3em;"> <tbody><tr> <td><span typeof="mw:File"><a href="/wiki/File:Dehydroascorbic_acid_2.svg" class="mw-file-description" title="dehydroascorbic acid"><img alt="dehydroascorbic acid" src="//upload.wikimedia.org/wikipedia/commons/thumb/3/3a/Dehydroascorbic_acid_2.svg/150px-Dehydroascorbic_acid_2.svg.png" decoding="async" width="150" height="150" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/3/3a/Dehydroascorbic_acid_2.svg/225px-Dehydroascorbic_acid_2.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/3/3a/Dehydroascorbic_acid_2.svg/300px-Dehydroascorbic_acid_2.svg.png 2x" data-file-width="128" data-file-height="128" /></a></span> </td></tr></tbody></table> <div style="border: none; width:150px;"><div class="thumbcaption"><small>Top: <a href="/wiki/Ascorbic_acid" class="mw-redirect" title="Ascorbic acid">ascorbic acid</a> (<a href="/wiki/Reducing_agent" title="Reducing agent">reduced form</a> of <a href="/wiki/Vitamin_C" title="Vitamin C">Vitamin C</a>)<br />Bottom: <a href="/wiki/Dehydroascorbic_acid" title="Dehydroascorbic acid">dehydroascorbic acid</a> (<a href="/wiki/Oxidizing_agent" title="Oxidizing agent">oxidized form</a> of <a href="/wiki/Vitamin_C" title="Vitamin C">Vitamin C</a>)</small></div></div></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Extremely_overripe_banana.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/5/51/Extremely_overripe_banana.jpg/170px-Extremely_overripe_banana.jpg" decoding="async" width="170" height="212" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/51/Extremely_overripe_banana.jpg/255px-Extremely_overripe_banana.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/51/Extremely_overripe_banana.jpg/340px-Extremely_overripe_banana.jpg 2x" data-file-width="6279" data-file-height="7848" /></a><figcaption><a href="/wiki/Food_browning#Enzymatic_browning" title="Food browning">Enzymatic browning</a> is an example of a redox reaction that takes place in most fruits and vegetables.</figcaption></figure> <p>Many essential <a href="/wiki/Biology" title="Biology">biological</a> processes involve redox reactions. Before some of these processes can begin, iron must be <a href="/wiki/Assimilation_(biology)" title="Assimilation (biology)">assimilated</a> from the environment.<sup id="cite_ref-25" class="reference"><a href="#cite_note-25"><span class="cite-bracket">[</span>25<span class="cite-bracket">]</span></a></sup> </p><p><a href="/wiki/Cellular_respiration" title="Cellular respiration">Cellular respiration</a>, for instance, is the oxidation of <a href="/wiki/Glucose" title="Glucose">glucose</a> (C<sub>6</sub>H<sub>12</sub>O<sub>6</sub>) to <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">CO<sub>2</sub></a> and the reduction of <a href="/wiki/Oxygen" title="Oxygen">oxygen</a> to <a href="/wiki/Water" title="Water">water</a>. The summary equation for cellular respiration is: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">C<sub class="template-chem2-sub">6</sub>H<sub class="template-chem2-sub">12</sub>O<sub class="template-chem2-sub">6</sub> + 6 O<sub class="template-chem2-sub">2</sub> → 6 CO<sub class="template-chem2-sub">2</sub> + 6 H<sub class="template-chem2-sub">2</sub>O + Energy</span></dd></dl> <p>The process of cellular respiration also depends heavily on the reduction of <a href="/wiki/Nicotinamide_adenine_dinucleotide" title="Nicotinamide adenine dinucleotide">NAD<sup>+</sup></a> to NADH and the reverse reaction (the oxidation of NADH to NAD<sup>+</sup>). <a href="/wiki/Photosynthesis" title="Photosynthesis">Photosynthesis</a> and cellular respiration are complementary, but photosynthesis is not the reverse of the redox reaction in cellular respiration: </p> <dl><dd><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1123817410"><span class="chemf nowrap">6 CO<sub class="template-chem2-sub">2</sub> + 6 H<sub class="template-chem2-sub">2</sub>O + <a href="/wiki/Photon" title="Photon">light energy</a> → C<sub class="template-chem2-sub">6</sub>H<sub class="template-chem2-sub">12</sub>O<sub class="template-chem2-sub">6</sub> + 6 O<sub class="template-chem2-sub">2</sub></span></dd></dl> <p><a href="/wiki/Biological_energy" class="mw-redirect" title="Biological energy">Biological energy</a> is frequently stored and released using redox reactions. Photosynthesis involves the reduction of <a href="/wiki/Carbon_dioxide" title="Carbon dioxide">carbon dioxide</a> into <a href="/wiki/Sugar" title="Sugar">sugars</a> and the oxidation of <a href="/wiki/Water_(molecule)" class="mw-redirect" title="Water (molecule)">water</a> into molecular oxygen. The reverse reaction, respiration, oxidizes sugars to produce carbon dioxide and water. As intermediate steps, the reduced carbon compounds are used to reduce <a href="/wiki/Nicotinamide_adenine_dinucleotide" title="Nicotinamide adenine dinucleotide">nicotinamide adenine dinucleotide</a> (NAD<sup>+</sup>) to NADH, which then contributes to the creation of a <a href="/wiki/Proton_gradient" class="mw-redirect" title="Proton gradient">proton gradient</a>, which drives the synthesis of <a href="/wiki/Adenosine_triphosphate" title="Adenosine triphosphate">adenosine triphosphate</a> (ATP) and is maintained by the reduction of oxygen. In animal cells, <a href="/wiki/Mitochondria" class="mw-redirect" title="Mitochondria">mitochondria</a> perform similar functions. </p> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">See also: <a href="/wiki/Membrane_potential" title="Membrane potential">Membrane potential</a></div> <p><a href="/wiki/Free_radical" class="mw-redirect" title="Free radical">Free radical</a> reactions are redox reactions that occur as part of <a href="/wiki/Homeostasis" title="Homeostasis">homeostasis</a> and killing <a href="/wiki/Microorganism" title="Microorganism">microorganisms</a>. In these reactions, an electron detaches from a molecule and then re-attaches almost instantly. Free radicals are part of redox molecules and can become harmful to the human body if they do not reattach to the redox molecule or an <a href="/wiki/Antioxidant" title="Antioxidant">antioxidant</a>. </p><p>The term <i>redox state</i> is often used to describe the balance of <a href="/wiki/Glutathione" title="Glutathione">GSH/GSSG</a>, NAD<sup>+</sup>/NADH and <a href="/wiki/Nicotinamide_adenine_dinucleotide_phosphate" title="Nicotinamide adenine dinucleotide phosphate">NADP<sup>+</sup>/NADPH</a> in a biological system such as a <a href="/wiki/Cell_(biology)" title="Cell (biology)">cell</a> or <a href="/wiki/Organ_(biology)" title="Organ (biology)">organ</a>. The redox state is reflected in the balance of several sets of metabolites (e.g., <a href="/wiki/Lactic_acid" title="Lactic acid">lactate</a> and <a href="/wiki/Pyruvate" class="mw-redirect" title="Pyruvate">pyruvate</a>, <a href="/wiki/Beta-hydroxybutyrate" class="mw-redirect" title="Beta-hydroxybutyrate">beta-hydroxybutyrate</a> and <a href="/wiki/Acetoacetate" class="mw-redirect" title="Acetoacetate">acetoacetate</a>), whose interconversion is dependent on these ratios. Redox mechanisms also control some cellular processes. Redox proteins and their genes must be co-located for redox regulation according to the <a href="/wiki/CoRR_hypothesis" title="CoRR hypothesis">CoRR hypothesis</a> for the function of <a href="/wiki/DNA" title="DNA">DNA</a> in <a href="/wiki/Mitochondrion" title="Mitochondrion">mitochondria</a> and <a href="/wiki/Chloroplast" title="Chloroplast">chloroplasts</a>. </p> <div class="mw-heading mw-heading3"><h3 id="Redox_cycling">Redox cycling</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=14" title="Edit section: Redox cycling"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Wide varieties of <a href="/wiki/Aromaticity" title="Aromaticity">aromatic compounds</a> are <a href="/wiki/Enzyme" title="Enzyme">enzymatically</a> reduced to form <a href="/wiki/Radical_(chemistry)" title="Radical (chemistry)">free radicals</a> that contain one more electron than their parent compounds. In general, the electron donor is any of a wide variety of <a href="/wiki/Flavoenzyme" class="mw-redirect" title="Flavoenzyme">flavoenzymes</a> and their <a href="/wiki/Coenzyme" class="mw-redirect" title="Coenzyme">coenzymes</a>. Once formed, these anion free radicals reduce molecular oxygen to <a href="/wiki/Superoxide" title="Superoxide">superoxide</a> and regenerate the unchanged parent compound. The net reaction is the oxidation of the flavoenzyme's coenzymes and the reduction of molecular oxygen to form superoxide. This catalytic behavior has been described as a <a href="/wiki/Futile_cycle" title="Futile cycle">futile cycle</a> or redox cycling. </p> <div class="mw-heading mw-heading2"><h2 id="Redox_reactions_in_geology">Redox reactions in geology</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=15" title="Edit section: Redox reactions in geology"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:VysokePece1.jpg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/f/f4/VysokePece1.jpg/250px-VysokePece1.jpg" decoding="async" width="250" height="188" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/f/f4/VysokePece1.jpg/375px-VysokePece1.jpg 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/f/f4/VysokePece1.jpg/500px-VysokePece1.jpg 2x" data-file-width="1024" data-file-height="768" /></a><figcaption>Blast furnaces of <a href="/wiki/T%C5%99inec_Iron_and_Steel_Works" title="Třinec Iron and Steel Works">Třinec Iron and Steel Works</a>, Czech Republic</figcaption></figure> <p>Minerals are generally oxidized derivatives of metals. Iron is mined as its <a href="/wiki/Magnetite" title="Magnetite">magnetite</a> (Fe<sub>3</sub>O<sub>4</sub>). Titanium is mined as its dioxide, usually in the form of <a href="/wiki/Rutile" title="Rutile">rutile</a> (TiO<sub>2</sub>). These oxides must be reduced to obtain the corresponding metals, often achieved by heating these oxides with carbon or carbon monoxide as reducing agents. <a href="/wiki/Blast_furnace" title="Blast furnace">Blast furnaces</a> are the reactors where iron oxides and coke (a form of carbon) are combined to produce molten iron. The main chemical reaction producing the molten iron is:<sup id="cite_ref-26" class="reference"><a href="#cite_note-26"><span class="cite-bracket">[</span>26<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<sub class="template-chem2-sub">2</sub>O<sub class="template-chem2-sub">3</sub> + 3 CO → 2 Fe + 3 CO<sub class="template-chem2-sub">2</sub></span></dd></dl> <div class="mw-heading mw-heading2"><h2 id="Redox_reactions_in_soils">Redox reactions in soils</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=16" title="Edit section: Redox reactions in soils"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p><a href="/wiki/Electron_transfer" title="Electron transfer">Electron transfer</a> reactions are central to myriad processes and properties in soils, and <a href="/wiki/Redox_potential" class="mw-redirect" title="Redox potential">redox potential</a>, quantified as Eh (platinum electrode potential (<a href="/wiki/Voltage" title="Voltage">voltage</a>) relative to the standard hydrogen electrode) or pe (analogous to pH as -log electron activity), is a master variable, along with pH, that controls and is governed by chemical reactions and biological processes. Early theoretical research with applications to flooded soils and <a href="/wiki/Paddy_rice" class="mw-redirect" title="Paddy rice">paddy rice</a> production was seminal for subsequent work on thermodynamic aspects of redox and plant root growth in soils.<sup id="cite_ref-27" class="reference"><a href="#cite_note-27"><span class="cite-bracket">[</span>27<span class="cite-bracket">]</span></a></sup> Later work built on this foundation, and expanded it for understanding redox reactions related to heavy metal oxidation state changes, <a href="/wiki/Pedogenesis" class="mw-redirect" title="Pedogenesis">pedogenesis</a> and morphology, organic compound degradation and formation, <a href="/wiki/Free_radical" class="mw-redirect" title="Free radical">free radical</a> chemistry, <a href="/wiki/Wetland" title="Wetland">wetland</a> delineation, <a href="/wiki/Soil_remediation" class="mw-redirect" title="Soil remediation">soil remediation</a>, and various methodological approaches for characterizing the redox status of soils.<sup id="cite_ref-28" class="reference"><a href="#cite_note-28"><span class="cite-bracket">[</span>28<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-29" class="reference"><a href="#cite_note-29"><span class="cite-bracket">[</span>29<span class="cite-bracket">]</span></a></sup> </p><p><br /> </p> <div class="mw-heading mw-heading2"><h2 id="Mnemonics">Mnemonics</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=17" title="Edit section: Mnemonics"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/List_of_chemistry_mnemonics" title="List of chemistry mnemonics">List of chemistry mnemonics</a></div> <p>The key terms involved in redox can be confusing.<sup id="cite_ref-Robertson_30-0" class="reference"><a href="#cite_note-Robertson-30"><span class="cite-bracket">[</span>30<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Chemistry_ConceptsAndApplications_31-0" class="reference"><a href="#cite_note-Chemistry_ConceptsAndApplications-31"><span class="cite-bracket">[</span>31<span class="cite-bracket">]</span></a></sup> For example, a reagent that is oxidized loses electrons; however, that reagent is referred to as the reducing agent. Likewise, a reagent that is reduced gains electrons and is referred to as the oxidizing agent.<sup id="cite_ref-Rodgers_32-0" class="reference"><a href="#cite_note-Rodgers-32"><span class="cite-bracket">[</span>32<span class="cite-bracket">]</span></a></sup> These <a href="/wiki/Mnemonics" class="mw-redirect" title="Mnemonics">mnemonics</a> are commonly used by students to help memorise the terminology:<sup id="cite_ref-Zumhahl_33-0" class="reference"><a href="#cite_note-Zumhahl-33"><span class="cite-bracket">[</span>33<span class="cite-bracket">]</span></a></sup> </p> <ul><li>"<a href="/wiki/Oil_rig" title="Oil rig">OIL RIG</a>" — <b>o</b>xidation <b>i</b>s <b>l</b>oss of electrons, <b>r</b>eduction <b>i</b>s <b>g</b>ain of electrons<sup id="cite_ref-Robertson_30-1" class="reference"><a href="#cite_note-Robertson-30"><span class="cite-bracket">[</span>30<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Chemistry_ConceptsAndApplications_31-1" class="reference"><a href="#cite_note-Chemistry_ConceptsAndApplications-31"><span class="cite-bracket">[</span>31<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Rodgers_32-1" class="reference"><a href="#cite_note-Rodgers-32"><span class="cite-bracket">[</span>32<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Zumhahl_33-1" class="reference"><a href="#cite_note-Zumhahl-33"><span class="cite-bracket">[</span>33<span class="cite-bracket">]</span></a></sup></li> <li>"LEO the lion says GER [grr]" — <b>l</b>oss of <b>e</b>lectrons is <b>o</b>xidation, <b>g</b>ain of <b>e</b>lectrons is <b>r</b>eduction<sup id="cite_ref-Robertson_30-2" class="reference"><a href="#cite_note-Robertson-30"><span class="cite-bracket">[</span>30<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Chemistry_ConceptsAndApplications_31-2" class="reference"><a href="#cite_note-Chemistry_ConceptsAndApplications-31"><span class="cite-bracket">[</span>31<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Rodgers_32-2" class="reference"><a href="#cite_note-Rodgers-32"><span class="cite-bracket">[</span>32<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-Zumhahl_33-2" class="reference"><a href="#cite_note-Zumhahl-33"><span class="cite-bracket">[</span>33<span class="cite-bracket">]</span></a></sup></li> <li>"LEORA says GEROA" — the loss of electrons is called oxidation (reducing agent); the gain of electrons is called reduction (oxidizing agent).<sup id="cite_ref-Rodgers_32-3" class="reference"><a href="#cite_note-Rodgers-32"><span class="cite-bracket">[</span>32<span class="cite-bracket">]</span></a></sup></li> <li>"RED CAT" and "AN OX", or "AnOx RedCat" ("an ox-red cat") — reduction occurs at the cathode and the anode is for oxidation</li> <li>"RED CAT gains what AN OX loses" – reduction at the cathode gains (electrons) what anode oxidation loses (electrons)</li> <li>"PANIC" – Positive Anode and Negative is Cathode. This applies to <a href="/wiki/Electrolytic_cell" title="Electrolytic cell">electrolytic cells</a> which release stored electricity, and can be recharged with electricity. PANIC does not apply to cells that can be recharged with redox materials. These <a href="/wiki/Galvanic_cell" title="Galvanic cell">galvanic or voltaic cells</a>, such as <a href="/wiki/Fuel_cell" title="Fuel cell">fuel cells</a>, produce electricity from internal redox reactions. Here, the positive electrode is the cathode and the negative is the anode.</li></ul> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=18" title="Edit section: See also"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1184024115">.mw-parser-output .div-col{margin-top:0.3em;column-width:30em}.mw-parser-output .div-col-small{font-size:90%}.mw-parser-output .div-col-rules{column-rule:1px solid #aaa}.mw-parser-output .div-col dl,.mw-parser-output .div-col ol,.mw-parser-output .div-col ul{margin-top:0}.mw-parser-output .div-col li,.mw-parser-output .div-col dd{page-break-inside:avoid;break-inside:avoid-column}</style><div class="div-col" style="column-width: 20em;"> <ul><li><a href="/wiki/Anaerobic_respiration" title="Anaerobic respiration">Anaerobic respiration</a></li> <li><a href="/wiki/Bessemer_process" title="Bessemer process">Bessemer process</a></li> <li><a href="/wiki/Bioremediation" title="Bioremediation">Bioremediation</a></li> <li><a href="/wiki/Calvin_cycle" title="Calvin cycle">Calvin cycle</a></li> <li><a href="/wiki/Chemical_equation" title="Chemical equation">Chemical equation</a></li> <li><a href="/wiki/Chemical_looping_combustion" title="Chemical looping combustion">Chemical looping combustion</a></li> <li><a href="/wiki/Citric_acid_cycle" title="Citric acid cycle">Citric acid cycle</a></li> <li><a href="/wiki/Electrochemical_series" class="mw-redirect" title="Electrochemical series">Electrochemical series</a></li> <li><a href="/wiki/Electrochemistry" title="Electrochemistry">Electrochemistry</a></li> <li><a href="/wiki/Electrolysis" title="Electrolysis">Electrolysis</a></li> <li><a href="/wiki/Electron_equivalent" class="mw-redirect" title="Electron equivalent">Electron equivalent</a></li> <li><a href="/wiki/Electron_transport_chain" title="Electron transport chain">Electron transport chain</a></li> <li><a href="/wiki/Electrosynthesis" title="Electrosynthesis">Electrosynthesis</a></li> <li><a href="/wiki/Galvanic_cell" title="Galvanic cell">Galvanic cell</a></li> <li><a href="/wiki/Hydrogenation" title="Hydrogenation">Hydrogenation</a></li> <li><a href="/wiki/Membrane_potential" title="Membrane potential">Membrane potential</a></li> <li><a href="/wiki/Microbial_fuel_cell" title="Microbial fuel cell">Microbial fuel cell</a></li> <li><a href="/wiki/Murburn_concept" title="Murburn concept">Murburn concept</a></li> <li><a href="/wiki/Nucleophilic_abstraction" title="Nucleophilic abstraction">Nucleophilic abstraction</a></li> <li><a href="/wiki/Organic_redox_reaction" title="Organic redox reaction">Organic redox reaction</a></li> <li><a href="/wiki/Oxidative_addition" title="Oxidative addition">Oxidative addition and reductive elimination</a></li> <li><a href="/wiki/Oxidative_phosphorylation" title="Oxidative phosphorylation">Oxidative phosphorylation</a></li> <li><a href="/wiki/Partial_oxidation" title="Partial oxidation">Partial oxidation</a></li> <li><a href="/wiki/Pro-oxidant" title="Pro-oxidant">Pro-oxidant</a></li> <li><a href="/wiki/Redox_gradient" title="Redox gradient">Redox gradient</a></li> <li><a href="/wiki/Redox_potential" class="mw-redirect" title="Redox potential">Redox potential</a></li> <li><a href="/wiki/Redox_therapy" title="Redox therapy">Redox therapy</a></li> <li><a href="/wiki/Reducing_agent" title="Reducing agent">Reducing agent</a></li> <li><a href="/wiki/Reducing_atmosphere" title="Reducing atmosphere">Reducing atmosphere</a></li> <li><a href="/wiki/Reduction_potential" title="Reduction potential">Reduction potential</a></li> <li><a href="/wiki/Exothermic" class="mw-redirect" title="Exothermic">Thermic reaction</a></li> <li><a href="/wiki/Transmetalation" title="Transmetalation">Transmetalation</a></li> <li><a href="/wiki/Sulfur_cycle" title="Sulfur cycle">Sulfur cycle</a></li></ul> </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=Redox&action=edit&section=19" title="Edit section: References"><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 mw-references-columns"><ol class="references"> <li id="cite_note-1"><span class="mw-cite-backlink"><b><a href="#cite_ref-1">^</a></b></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 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0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://www.bbc.co.uk/bitesize/guides/zx2bh39/revision/5">"Metals"</a>. <i>Bitesize</i>. 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Washington, D.C.: American Chemical Society. pp. <a rel="nofollow" class="external text" href="https://archive.org/details/oxidationsinorga00hudl/page/456">456</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-8412-1780-5" title="Special:BookSources/978-0-8412-1780-5"><bdi>978-0-8412-1780-5</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Oxidations+in+Organic+Chemistry&rft.place=Washington%2C+D.C.&rft.pages=456&rft.pub=American+Chemical+Society&rft.date=1990&rft.isbn=978-0-8412-1780-5&rft.aulast=Hudlick%C3%BD&rft.aufirst=Milo%C5%A1&rft_id=https%3A%2F%2Farchive.org%2Fdetails%2Foxidationsinorga00hudl%2Fpage%2F456&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> <li id="cite_note-16"><span class="mw-cite-backlink"><b><a href="#cite_ref-16">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFBockrisReddy1970" class="citation book cs1">Bockris, John O'M.; Reddy, Amulya K. 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Retrieved <span class="nowrap">March 29,</span> 2020</span>. <q>The homogeneous proton-transfer reactions described are similar to homogeneous electron-transfer reactions in that the overall electron-transfer reaction can be decomposed into one electronation reaction and one deelectronation reaction.</q></cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Modern+Electrochemistry&rft.pages=494&rft.pub=Springer+Science+%26+Business+Media&rft.date=2013&rft.isbn=9781461574675&rft.aulast=Bockris&rft.aufirst=John+O%27M.&rft.au=Reddy%2C+Amulya+K.N.&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3D0xzlBwAAQBAJ%26pg%3DPA494&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> <li id="cite_note-18"><span class="mw-cite-backlink"><b><a href="#cite_ref-18">^</a></b></span> <span class="reference-text">IUPAC. Compendium of Chemical Terminology, 2nd ed. (the "Gold Book"). Compiled by A. D. McNaught and A. Wilkinson. Blackwell Scientific Publications, Oxford (1997). Online version (2019-) created by S. J. Chalk. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-9678550-9-8" title="Special:BookSources/0-9678550-9-8">0-9678550-9-8</a>. <a rel="nofollow" class="external free" href="https://goldbook.iupac.org/terms/view/R05222">https://goldbook.iupac.org/terms/view/R05222</a></span> </li> <li id="cite_note-19"><span class="mw-cite-backlink"><b><a href="#cite_ref-19">^</a></b></span> <span class="reference-text">IUPAC. Compendium of Chemical Terminology, 2nd ed. (the "Gold Book"). Compiled by A. D. McNaught and A. Wilkinson. Blackwell Scientific Publications, Oxford (1997). Online version (2019-) created by S. J. Chalk. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/0-9678550-9-8" title="Special:BookSources/0-9678550-9-8">0-9678550-9-8</a>. <a rel="nofollow" class="external free" href="https://goldbook.iupac.org/terms/view/O04362">https://goldbook.iupac.org/terms/view/O04362</a></span> </li> <li id="cite_note-20"><span class="mw-cite-backlink"><b><a href="#cite_ref-20">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFMailloux2015" class="citation journal cs1">Mailloux, Ryan J. 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(the "Gold Book") (1997). Online corrected version: (2006–) "<a rel="nofollow" class="external text" href="https://goldbook.iupac.org/terms/view/I03052.html">Inner-sphere electron transfer</a>". <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1351%2Fgoldbook.I03052">10.1351/goldbook.I03052</a></span> </li> <li id="cite_note-22"><span class="mw-cite-backlink"><b><a href="#cite_ref-22">^</a></b></span> <span class="reference-text"><a href="/wiki/International_Union_of_Pure_and_Applied_Chemistry" title="International Union of Pure and Applied Chemistry">IUPAC</a>, <i><a href="/wiki/IUPAC_books#Gold_Book" class="mw-redirect" title="IUPAC books">Compendium of Chemical Terminology</a></i>, 2nd ed. (the "Gold Book") (1997). 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(1972). <i>The Chemistry of Submerged Soils</i>. Advances in Agronomy. Vol. 24. pp. 29–96. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1016%2FS0065-2113%2808%2960633-1">10.1016/S0065-2113(08)60633-1</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-12-000724-0" title="Special:BookSources/978-0-12-000724-0"><bdi>978-0-12-000724-0</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=The+Chemistry+of+Submerged+Soils&rft.series=Advances+in+Agronomy&rft.pages=29-96&rft.date=1972&rft_id=info%3Adoi%2F10.1016%2FS0065-2113%2808%2960633-1&rft.isbn=978-0-12-000724-0&rft.aulast=Ponnamperuma&rft.aufirst=F.N.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> <li id="cite_note-28"><span class="mw-cite-backlink"><b><a href="#cite_ref-28">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFBartlettJames1991" class="citation journal cs1">Bartlett, Richmond J.; James, Bruce R. (1991). "Redox chemistry of soils". <i>Advances in Agronomy</i>. <b>39</b>: 151–208.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Advances+in+Agronomy&rft.atitle=Redox+chemistry+of+soils&rft.volume=39&rft.pages=151-208&rft.date=1991&rft.aulast=Bartlett&rft.aufirst=Richmond+J.&rft.au=James%2C+Bruce+R.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> <li id="cite_note-29"><span class="mw-cite-backlink"><b><a href="#cite_ref-29">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFJamesBrose2012" class="citation book cs1">James, Bruce R.; Brose, Dominic A. (2012). "Oxidation-reduction phenomena". In Huang, Pan Ming; Li, Yuncong; Sumner, Malcolm E. (eds.). <i>Handbook of soil sciences: properties and processes</i> (second ed.). Boca Raton, Florida: <a href="/wiki/CRC_Press" title="CRC Press">CRC Press</a>. pp. 14-1 -- 14-24. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-1-4398-0305-9" title="Special:BookSources/978-1-4398-0305-9"><bdi>978-1-4398-0305-9</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Oxidation-reduction+phenomena&rft.btitle=Handbook+of+soil+sciences%3A+properties+and+processes&rft.place=Boca+Raton%2C+Florida&rft.pages=14-1+--+14-24&rft.edition=second&rft.pub=CRC+Press&rft.date=2012&rft.isbn=978-1-4398-0305-9&rft.aulast=James&rft.aufirst=Bruce+R.&rft.au=Brose%2C+Dominic+A.&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> <li id="cite_note-Robertson-30"><span class="mw-cite-backlink">^ <a href="#cite_ref-Robertson_30-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Robertson_30-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-Robertson_30-2"><sup><i><b>c</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFRobertson2010" class="citation book cs1">Robertson, William (2010). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=hIzuarlXtH4C&pg=PA82"><i>More Chemistry Basics</i></a>. National Science Teachers Association. p. 82. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-1-936137-74-9" title="Special:BookSources/978-1-936137-74-9"><bdi>978-1-936137-74-9</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=More+Chemistry+Basics&rft.pages=82&rft.pub=National+Science+Teachers+Association&rft.date=2010&rft.isbn=978-1-936137-74-9&rft.aulast=Robertson&rft.aufirst=William&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DhIzuarlXtH4C%26pg%3DPA82&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> <li id="cite_note-Chemistry_ConceptsAndApplications-31"><span class="mw-cite-backlink">^ <a href="#cite_ref-Chemistry_ConceptsAndApplications_31-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Chemistry_ConceptsAndApplications_31-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-Chemistry_ConceptsAndApplications_31-2"><sup><i><b>c</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFPhillipsStrozakWistrom2000" class="citation book cs1">Phillips, John; Strozak, Victor; Wistrom, Cheryl (2000). <i>Chemistry: Concepts and Applications</i>. Glencoe McGraw-Hill. p. 558. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-02-828210-7" title="Special:BookSources/978-0-02-828210-7"><bdi>978-0-02-828210-7</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry%3A+Concepts+and+Applications&rft.pages=558&rft.pub=Glencoe+McGraw-Hill&rft.date=2000&rft.isbn=978-0-02-828210-7&rft.aulast=Phillips&rft.aufirst=John&rft.au=Strozak%2C+Victor&rft.au=Wistrom%2C+Cheryl&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> <li id="cite_note-Rodgers-32"><span class="mw-cite-backlink">^ <a href="#cite_ref-Rodgers_32-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Rodgers_32-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-Rodgers_32-2"><sup><i><b>c</b></i></sup></a> <a href="#cite_ref-Rodgers_32-3"><sup><i><b>d</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFRodgers2012" class="citation book cs1">Rodgers, Glen (2012). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=g_ybia0hGw8C&pg=PA330"><i>Descriptive Inorganic, Coordination, and Solid-State Chemistry</i></a>. Brooks/Cole, Cengage Learning. p. 330. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-8400-6846-0" title="Special:BookSources/978-0-8400-6846-0"><bdi>978-0-8400-6846-0</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Descriptive+Inorganic%2C+Coordination%2C+and+Solid-State+Chemistry&rft.pages=330&rft.pub=Brooks%2FCole%2C+Cengage+Learning&rft.date=2012&rft.isbn=978-0-8400-6846-0&rft.aulast=Rodgers&rft.aufirst=Glen&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3Dg_ybia0hGw8C%26pg%3DPA330&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> <li id="cite_note-Zumhahl-33"><span class="mw-cite-backlink">^ <a href="#cite_ref-Zumhahl_33-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Zumhahl_33-1"><sup><i><b>b</b></i></sup></a> <a href="#cite_ref-Zumhahl_33-2"><sup><i><b>c</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFZumdahlZumdahl2009" class="citation book cs1">Zumdahl, Steven; Zumdahl, Susan (2009). <a rel="nofollow" class="external text" href="https://books.google.com/books?id=IdhYqXy37KIC&pg=PA160"><i>Chemistry</i></a>. Houghton Mifflin. p. 160. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-547-05405-6" title="Special:BookSources/978-0-547-05405-6"><bdi>978-0-547-05405-6</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry&rft.pages=160&rft.pub=Houghton+Mifflin&rft.date=2009&rft.isbn=978-0-547-05405-6&rft.aulast=Zumdahl&rft.aufirst=Steven&rft.au=Zumdahl%2C+Susan&rft_id=https%3A%2F%2Fbooks.google.com%2Fbooks%3Fid%3DIdhYqXy37KIC%26pg%3DPA160&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></span> </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="Further_reading">Further reading</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=20" title="Edit section: Further reading"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSchüringSchulzFischerBöttcher1999" class="citation book cs1">Schüring, J.; Schulz, H. D.; Fischer, W. R.; Böttcher, J.; Duijnisveld, W. H., eds. (1999). <i>Redox: Fundamentals, Processes and Applications</i>. Heidelberg: Springer-Verlag. p. 246. <a href="/wiki/Hdl_(identifier)" class="mw-redirect" title="Hdl (identifier)">hdl</a>:<a rel="nofollow" class="external text" href="https://hdl.handle.net/10013%2Fepic.31694.d001">10013/epic.31694.d001</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-3-540-66528-1" title="Special:BookSources/978-3-540-66528-1"><bdi>978-3-540-66528-1</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Redox%3A+Fundamentals%2C+Processes+and+Applications&rft.place=Heidelberg&rft.pages=246&rft.pub=Springer-Verlag&rft.date=1999&rft_id=info%3Ahdl%2F10013%2Fepic.31694.d001&rft.isbn=978-3-540-66528-1&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></li> <li><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFTratnyekGrundlHaderlein2011" class="citation book cs1">Tratnyek, Paul G.; Grundl, Timothy J.; Haderlein, Stefan B., eds. (2011). <i>Aquatic Redox Chemistry</i>. ACS Symposium Series. Vol. 1071. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1021%2Fbk-2011-1071">10.1021/bk-2011-1071</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-8412-2652-4" title="Special:BookSources/978-0-8412-2652-4"><bdi>978-0-8412-2652-4</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Aquatic+Redox+Chemistry&rft.series=ACS+Symposium+Series&rft.date=2011&rft_id=info%3Adoi%2F10.1021%2Fbk-2011-1071&rft.isbn=978-0-8412-2652-4&rfr_id=info%3Asid%2Fen.wikipedia.org%3ARedox" class="Z3988"></span></li></ul> <div class="mw-heading mw-heading2"><h2 id="External_links">External links</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Redox&action=edit&section=21" title="Edit section: External links"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1235681985">.mw-parser-output .side-box{margin:4px 0;box-sizing:border-box;border:1px solid #aaa;font-size:88%;line-height:1.25em;background-color:var(--background-color-interactive-subtle,#f8f9fa);display:flow-root}.mw-parser-output .side-box-abovebelow,.mw-parser-output .side-box-text{padding:0.25em 0.9em}.mw-parser-output .side-box-image{padding:2px 0 2px 0.9em;text-align:center}.mw-parser-output .side-box-imageright{padding:2px 0.9em 2px 0;text-align:center}@media(min-width:500px){.mw-parser-output .side-box-flex{display:flex;align-items:center}.mw-parser-output .side-box-text{flex:1;min-width:0}}@media(min-width:720px){.mw-parser-output .side-box{width:238px}.mw-parser-output .side-box-right{clear:right;float:right;margin-left:1em}.mw-parser-output .side-box-left{margin-right:1em}}</style><style 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href="/wiki/Template:Reaction_mechanisms" title="Template:Reaction mechanisms"><abbr title="View this template">v</abbr></a></li><li class="nv-talk"><a href="/wiki/Template_talk:Reaction_mechanisms" title="Template talk:Reaction mechanisms"><abbr title="Discuss this template">t</abbr></a></li><li class="nv-edit"><a href="/wiki/Special:EditPage/Template:Reaction_mechanisms" title="Special:EditPage/Template:Reaction mechanisms"><abbr title="Edit this template">e</abbr></a></li></ul></div><div id="Basic_reaction_mechanisms" style="font-size:114%;margin:0 4em">Basic <a href="/wiki/Reaction_mechanism" title="Reaction mechanism">reaction mechanisms</a></div></th></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Nucleophilic_substitution" title="Nucleophilic substitution">Nucleophilic substitutions</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/SN1_reaction" title="SN1 reaction">Unimolecular nucleophilic substitution</a> (S<sub>N</sub>1)</li> <li><a href="/wiki/SN2_reaction" title="SN2 reaction">Bimolecular nucleophilic substitution</a> (S<sub>N</sub>2)</li> <li><a href="/wiki/Nucleophilic_aromatic_substitution" title="Nucleophilic aromatic substitution">Nucleophilic aromatic substitution</a> (S<sub>N</sub>Ar)</li> <li><a href="/wiki/SNi" title="SNi">Nucleophilic internal substitution</a> (S<sub>N</sub>i)</li> <li><a href="/wiki/Nucleophilic_acyl_substitution" class="mw-redirect" title="Nucleophilic acyl substitution">Nucleophilic acyl substitution</a> (S<sub>N</sub>Acyl)</li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Electrophilic_substitution" title="Electrophilic substitution">Electrophilic substitutions</a></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Electrophilic_aromatic_substitution" title="Electrophilic aromatic substitution">Electrophilic aromatic substitution</a> (S<sub>E</sub>Ar)</li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Elimination_reaction" title="Elimination reaction">Elimination reactions</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/E1_elimination" class="mw-redirect" title="E1 elimination">Unimolecular elimination</a> (E1)</li> <li><a href="/wiki/E1cB-elimination_reaction" title="E1cB-elimination reaction">E1cB-elimination</a></li> <li><a href="/wiki/E2_elimination" class="mw-redirect" title="E2 elimination">Bimolecular elimination</a> (E2)</li> <li><a href="/wiki/Ei_mechanism" title="Ei mechanism">E<sub>i</sub> elimination</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Addition_reaction" title="Addition reaction">Addition reactions</a></th><td class="navbox-list-with-group navbox-list navbox-even hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Electrophilic_addition" title="Electrophilic addition">Electrophilic addition</a> (A<sub>E</sub>)</li> <li><a href="/wiki/Nucleophilic_addition" title="Nucleophilic addition">Nucleophilic addition</a> (A<sub>N</sub>)</li> <li><a href="/wiki/Free-radical_addition" title="Free-radical addition">Free-radical addition</a></li> <li><a href="/wiki/Cycloaddition" title="Cycloaddition">Cycloaddition</a></li> <li><a href="/wiki/Oxidative_addition" title="Oxidative addition">Oxidative addition</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Unimolecular reactions</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/Intramolecular_reaction" title="Intramolecular reaction">Intramolecular reaction</a></li> <li><a href="/wiki/Isomerization" title="Isomerization">Isomerization</a></li> <li><a href="/wiki/Photodissociation" title="Photodissociation">Photodissociation</a></li> <li><a href="/wiki/Lindemann%E2%80%93Hinshelwood_mechanism" class="mw-redirect" title="Lindemann–Hinshelwood mechanism">Lindemann–Hinshelwood mechanism</a></li> <li><a href="/wiki/RRKM_theory" title="RRKM theory">RRKM theory</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Electron_transfer" title="Electron transfer">Electron/Proton transfer</a> reactions</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 class="mw-selflink selflink">Redox</a></li> <li><a href="/wiki/Harpoon_reaction" title="Harpoon reaction">Harpoon reaction</a></li> <li><a href="/wiki/Grotthuss_mechanism" title="Grotthuss mechanism">Grotthuss mechanism</a></li> <li><a href="/wiki/Marcus_theory" title="Marcus theory">Marcus theory</a></li> <li><a href="/wiki/Inner_sphere_electron_transfer" title="Inner sphere electron transfer">Inner sphere electron transfer</a></li> <li><a href="/wiki/Outer_sphere_electron_transfer" title="Outer sphere electron transfer">Outer sphere electron transfer</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Medium effects</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/Solvent_effects" title="Solvent effects">Solvent effects</a></li> <li><a href="/wiki/Cage_effect" title="Cage effect">Cage effect</a></li> <li><a href="/wiki/Matrix_isolation" title="Matrix isolation">Matrix isolation</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%">Related topics</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/Elementary_reaction" title="Elementary reaction">Elementary reaction</a></li> <li><a href="/wiki/Reaction_dynamics" title="Reaction dynamics">Reaction dynamics</a></li> <li><a href="/wiki/Reactive_intermediate" title="Reactive intermediate">Reactive intermediate</a></li> <li><a href="/wiki/Radical_(chemistry)" title="Radical (chemistry)">Radical (chemistry)</a></li> <li><a href="/wiki/Molecularity" title="Molecularity">Molecularity</a></li> <li><a href="/wiki/Stereochemistry" title="Stereochemistry">Stereochemistry</a></li> <li><a href="/wiki/Catalysis" title="Catalysis">Catalysis</a></li> <li><a href="/wiki/Collision_theory" title="Collision theory">Collision theory</a></li> <li><a href="/wiki/Arrow_pushing" title="Arrow pushing">Arrow pushing</a></li> <li><a href="/wiki/Potential_energy_surface" title="Potential energy surface">Potential energy surface</a></li> <li><a href="/wiki/More_O%27Ferrall%E2%80%93Jencks_plot" title="More O'Ferrall–Jencks plot">More O'Ferrall–Jencks plot</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Chemical_kinetics" title="Chemical kinetics">Chemical kinetics</a></th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Rate_equation" title="Rate equation">Rate equation</a></li> <li><a href="/wiki/Equilibrium_constant" title="Equilibrium constant">Equilibrium constant</a></li> <li><a href="/wiki/Rate-determining_step" title="Rate-determining step">Rate-determining step</a></li> <li><a href="/wiki/Reaction_coordinate" title="Reaction coordinate">Reaction coordinate</a></li> <li><a href="/wiki/Energy_profile_(chemistry)" title="Energy profile (chemistry)">Energy profile (chemistry)</a></li> <li><a href="/wiki/Transition_state_theory" title="Transition state theory">Transition state theory</a></li> <li><a href="/wiki/Activation_energy" title="Activation energy">Activation energy</a></li> <li><a href="/wiki/Activated_complex" title="Activated complex">Activated complex</a></li> <li><a href="/wiki/Arrhenius_equation" title="Arrhenius equation">Arrhenius equation</a></li> <li><a href="/wiki/Eyring_equation" title="Eyring equation">Eyring equation</a></li> <li><a href="/wiki/Michaelis%E2%80%93Menten_kinetics" title="Michaelis–Menten kinetics">Michaelis–Menten kinetics</a></li> <li><a href="/wiki/Diffusion-controlled_reaction" title="Diffusion-controlled reaction">Diffusion-controlled reaction</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"><style data-mw-deduplicate="TemplateStyles:r1038841319">.mw-parser-output .tooltip-dotted{border-bottom:1px dotted;cursor:help}</style><link rel="mw-deduplicated-inline-style" 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