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class="vector-toc-list"> </ul> </li> <li id="toc-Strength_of_the_bonding" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Strength_of_the_bonding"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Strength of the bonding</span> </div> </a> <ul id="toc-Strength_of_the_bonding-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Polarization_power_effects" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Polarization_power_effects"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>Polarization power effects</span> </div> </a> <ul id="toc-Polarization_power_effects-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Comparison_with_covalent_bonding" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Comparison_with_covalent_bonding"> <div class="vector-toc-text"> <span class="vector-toc-numb">6</span> <span>Comparison with covalent bonding</span> </div> </a> <ul id="toc-Comparison_with_covalent_bonding-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">7</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">8</span> <span>References</span> </div> </a> <ul id="toc-References-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">9</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 id="vector-page-titlebar-toc" class="vector-dropdown vector-page-titlebar-toc vector-button-flush-left" > <input type="checkbox" id="vector-page-titlebar-toc-checkbox" role="button" aria-haspopup="true" data-event-name="ui.dropdown-vector-page-titlebar-toc" class="vector-dropdown-checkbox " aria-label="Toggle the table of contents" > <label id="vector-page-titlebar-toc-label" for="vector-page-titlebar-toc-checkbox" class="vector-dropdown-label cdx-button cdx-button--fake-button cdx-button--fake-button--enabled cdx-button--weight-quiet cdx-button--icon-only " aria-hidden="true" ><span class="vector-icon mw-ui-icon-listBullet mw-ui-icon-wikimedia-listBullet"></span> <span class="vector-dropdown-label-text">Toggle the table of contents</span> </label> <div class="vector-dropdown-content"> <div id="vector-page-titlebar-toc-unpinned-container" class="vector-unpinned-container"> </div> </div> </div> </nav> <h1 id="firstHeading" class="firstHeading mw-first-heading"><span class="mw-page-title-main">Ionic bonding</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/Ioniese_binding" title="Ioniese binding – Afrikaans" lang="af" hreflang="af" data-title="Ioniese binding" data-language-autonym="Afrikaans" data-language-local-name="Afrikaans" class="interlanguage-link-target"><span>Afrikaans</span></a></li><li class="interlanguage-link interwiki-am mw-list-item"><a href="https://am.wikipedia.org/wiki/%E1%8A%A0%E1%8B%AE%E1%8A%92%E1%8A%AD_%E1%89%A6%E1%8A%95%E1%8B%B5" title="አዮኒክ ቦንድ – Amharic" lang="am" hreflang="am" data-title="አዮኒክ ቦንድ" data-language-autonym="አማርኛ" data-language-local-name="Amharic" class="interlanguage-link-target"><span>አማርኛ</span></a></li><li class="interlanguage-link interwiki-ar mw-list-item"><a href="https://ar.wikipedia.org/wiki/%D8%B1%D8%A7%D8%A8%D8%B7%D8%A9_%D8%A3%D9%8A%D9%88%D9%86%D9%8A%D8%A9" title="رابطة أيونية – Arabic" lang="ar" hreflang="ar" data-title="رابطة أيونية" data-language-autonym="العربية" data-language-local-name="Arabic" class="interlanguage-link-target"><span>العربية</span></a></li><li class="interlanguage-link interwiki-an mw-list-item"><a href="https://an.wikipedia.org/wiki/Enlace_ionico" title="Enlace ionico – Aragonese" lang="an" hreflang="an" data-title="Enlace ionico" data-language-autonym="Aragonés" data-language-local-name="Aragonese" class="interlanguage-link-target"><span>Aragonés</span></a></li><li class="interlanguage-link interwiki-ast mw-list-item"><a href="https://ast.wikipedia.org/wiki/Enllaz_i%C3%B3nicu" title="Enllaz iónicu – Asturian" lang="ast" hreflang="ast" data-title="Enllaz iónicu" data-language-autonym="Asturianu" data-language-local-name="Asturian" class="interlanguage-link-target"><span>Asturianu</span></a></li><li class="interlanguage-link interwiki-az mw-list-item"><a href="https://az.wikipedia.org/wiki/%C4%B0on_rabit%C9%99si" title="İon rabitəsi – Azerbaijani" lang="az" hreflang="az" data-title="İon rabitəsi" data-language-autonym="Azərbaycanca" data-language-local-name="Azerbaijani" class="interlanguage-link-target"><span>Azərbaycanca</span></a></li><li class="interlanguage-link interwiki-bn mw-list-item"><a href="https://bn.wikipedia.org/wiki/%E0%A6%86%E0%A6%AF%E0%A6%BC%E0%A6%A8%E0%A6%BF%E0%A6%95_%E0%A6%AC%E0%A6%A8%E0%A7%8D%E0%A6%A7%E0%A6%A8" title="আয়নিক বন্ধন – Bangla" lang="bn" hreflang="bn" data-title="আয়নিক বন্ধন" 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/L%C4%AB-ch%C3%BA_kiat-ha%CC%8Dp" title="Lī-chú kiat-ha̍p – Minnan" lang="nan" hreflang="nan" data-title="Lī-chú kiat-ha̍p" 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-be mw-list-item"><a href="https://be.wikipedia.org/wiki/%D0%86%D0%BE%D0%BD%D0%BD%D0%B0%D1%8F_%D1%81%D1%83%D0%B2%D1%8F%D0%B7%D1%8C" title="Іонная сувязь – Belarusian" lang="be" hreflang="be" data-title="Іонная сувязь" data-language-autonym="Беларуская" data-language-local-name="Belarusian" class="interlanguage-link-target"><span>Беларуская</span></a></li><li class="interlanguage-link interwiki-bg mw-list-item"><a href="https://bg.wikipedia.org/wiki/%D0%99%D0%BE%D0%BD%D0%BD%D0%B0_%D0%B2%D1%80%D1%8A%D0%B7%D0%BA%D0%B0" title="Йонна връзка – Bulgarian" lang="bg" hreflang="bg" data-title="Йонна връзка" 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/Ionska_veza" title="Ionska veza – Bosnian" lang="bs" hreflang="bs" data-title="Ionska veza" 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/Enlla%C3%A7_i%C3%B2nic" title="Enllaç iònic – Catalan" lang="ca" hreflang="ca" data-title="Enllaç iònic" 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%98%D0%BE%D0%BD%D0%BB%D0%B0_%C3%A7%D1%8B%D1%85%C4%83%D0%BD%D1%83" title="Ионла çыхăну – Chuvash" lang="cv" hreflang="cv" data-title="Ионла çыхăну" 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/Iontov%C3%A1_vazba" title="Iontová vazba – Czech" lang="cs" hreflang="cs" data-title="Iontová vazba" 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/Bond_%C3%AFonig" title="Bond ïonig – Welsh" lang="cy" hreflang="cy" data-title="Bond ïonig" 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/Ionbinding" title="Ionbinding – Danish" lang="da" hreflang="da" data-title="Ionbinding" 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/Ionische_Bindung" title="Ionische Bindung – German" lang="de" hreflang="de" data-title="Ionische Bindung" 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/Iooniline_side" title="Iooniline side – Estonian" lang="et" hreflang="et" data-title="Iooniline side" 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%95%CF%84%CE%B5%CF%81%CE%BF%CF%80%CE%BF%CE%BB%CE%B9%CE%BA%CF%8C%CF%82_%CE%B4%CE%B5%CF%83%CE%BC%CF%8C%CF%82" title="Ετεροπολικός δεσμός – Greek" lang="el" hreflang="el" data-title="Ετεροπολικός δεσμός" 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/Enlace_i%C3%B3nico" title="Enlace iónico – Spanish" lang="es" hreflang="es" data-title="Enlace iónico" 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/Jona_ligo" title="Jona ligo – Esperanto" lang="eo" hreflang="eo" data-title="Jona ligo" 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/Lotura_ioniko" title="Lotura ioniko – Basque" lang="eu" hreflang="eu" data-title="Lotura ioniko" 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/%D9%BE%DB%8C%D9%88%D9%86%D8%AF_%DB%8C%D9%88%D9%86%DB%8C" title="پیوند یونی – Persian" lang="fa" hreflang="fa" data-title="پیوند یونی" 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/Liaison_ionique" title="Liaison ionique – French" lang="fr" hreflang="fr" data-title="Liaison ionique" data-language-autonym="Français" data-language-local-name="French" class="interlanguage-link-target"><span>Français</span></a></li><li class="interlanguage-link interwiki-ga mw-list-item"><a href="https://ga.wikipedia.org/wiki/Nascadh_ianach" title="Nascadh ianach – Irish" lang="ga" hreflang="ga" data-title="Nascadh ianach" data-language-autonym="Gaeilge" data-language-local-name="Irish" class="interlanguage-link-target"><span>Gaeilge</span></a></li><li class="interlanguage-link interwiki-gv mw-list-item"><a href="https://gv.wikipedia.org/wiki/Kiangley_eeaneagh" title="Kiangley eeaneagh – Manx" lang="gv" hreflang="gv" data-title="Kiangley eeaneagh" data-language-autonym="Gaelg" data-language-local-name="Manx" class="interlanguage-link-target"><span>Gaelg</span></a></li><li class="interlanguage-link interwiki-gl mw-list-item"><a href="https://gl.wikipedia.org/wiki/Enlace_i%C3%B3nico" title="Enlace iónico – Galician" lang="gl" hreflang="gl" data-title="Enlace iónico" 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%9D%B4%EC%98%A8_%EA%B2%B0%ED%95%A9" title="이온 결합 – Korean" lang="ko" hreflang="ko" data-title="이온 결합" data-language-autonym="한국어" data-language-local-name="Korean" class="interlanguage-link-target"><span>한국어</span></a></li><li class="interlanguage-link interwiki-hy mw-list-item"><a href="https://hy.wikipedia.org/wiki/%D4%BB%D5%B8%D5%B6%D5%A1%D5%B5%D5%AB%D5%B6_%D5%AF%D5%A1%D5%BA" title="Իոնային կապ – Armenian" lang="hy" hreflang="hy" data-title="Իոնային կապ" data-language-autonym="Հայերեն" data-language-local-name="Armenian" class="interlanguage-link-target"><span>Հայերեն</span></a></li><li class="interlanguage-link interwiki-hi mw-list-item"><a href="https://hi.wikipedia.org/wiki/%E0%A4%86%E0%A4%AF%E0%A4%A8%E0%A5%80_%E0%A4%86%E0%A4%AC%E0%A4%A8%E0%A5%8D%E0%A4%A7" title="आयनी आबन्ध – Hindi" lang="hi" hreflang="hi" data-title="आयनी आबन्ध" 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/Ionska_veza" title="Ionska veza – Croatian" lang="hr" hreflang="hr" data-title="Ionska veza" data-language-autonym="Hrvatski" data-language-local-name="Croatian" class="interlanguage-link-target"><span>Hrvatski</span></a></li><li class="interlanguage-link interwiki-id mw-list-item"><a href="https://id.wikipedia.org/wiki/Ikatan_ionik" title="Ikatan ionik – Indonesian" lang="id" hreflang="id" data-title="Ikatan ionik" 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-is mw-list-item"><a href="https://is.wikipedia.org/wiki/J%C3%B3natengi" title="Jónatengi – Icelandic" lang="is" hreflang="is" data-title="Jónatengi" data-language-autonym="Íslenska" data-language-local-name="Icelandic" class="interlanguage-link-target"><span>Íslenska</span></a></li><li class="interlanguage-link interwiki-it mw-list-item"><a href="https://it.wikipedia.org/wiki/Legame_ionico" title="Legame ionico – Italian" lang="it" hreflang="it" data-title="Legame ionico" 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%A7%D7%A9%D7%A8_%D7%99%D7%95%D7%A0%D7%99" title="קשר יוני – Hebrew" lang="he" hreflang="he" data-title="קשר יוני" data-language-autonym="עברית" data-language-local-name="Hebrew" class="interlanguage-link-target"><span>עברית</span></a></li><li class="interlanguage-link interwiki-ka mw-list-item"><a href="https://ka.wikipedia.org/wiki/%E1%83%98%E1%83%9D%E1%83%9C%E1%83%A3%E1%83%A0%E1%83%98_%E1%83%91%E1%83%9B%E1%83%90" title="იონური ბმა – Georgian" lang="ka" hreflang="ka" data-title="იონური ბმა" 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%98%D0%BE%D0%BD%D0%B4%D1%8B%D2%9B_%D0%B1%D0%B0%D0%B9%D0%BB%D0%B0%D0%BD%D1%8B%D1%81" title="Иондық байланыс – Kazakh" lang="kk" hreflang="kk" data-title="Иондық байланыс" data-language-autonym="Қазақша" data-language-local-name="Kazakh" class="interlanguage-link-target"><span>Қазақша</span></a></li><li class="interlanguage-link interwiki-ky mw-list-item"><a href="https://ky.wikipedia.org/wiki/%D0%98%D0%BE%D0%BD%D0%B4%D1%83%D0%BA_%D0%B1%D0%B0%D0%B9%D0%BB%D0%B0%D0%BD%D1%8B%D1%88" title="Иондук байланыш – Kyrgyz" lang="ky" hreflang="ky" data-title="Иондук байланыш" data-language-autonym="Кыргызча" data-language-local-name="Kyrgyz" class="interlanguage-link-target"><span>Кыргызча</span></a></li><li class="interlanguage-link interwiki-lv mw-list-item"><a href="https://lv.wikipedia.org/wiki/Jonu_saite" title="Jonu saite – Latvian" lang="lv" hreflang="lv" data-title="Jonu saite" data-language-autonym="Latviešu" data-language-local-name="Latvian" class="interlanguage-link-target"><span>Latviešu</span></a></li><li class="interlanguage-link interwiki-lt mw-list-item"><a href="https://lt.wikipedia.org/wiki/Joninis_ry%C5%A1ys" title="Joninis ryšys – Lithuanian" lang="lt" hreflang="lt" data-title="Joninis ryšys" 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/Ionos_k%C3%B6t%C3%A9s" title="Ionos kötés – Hungarian" lang="hu" hreflang="hu" data-title="Ionos kötés" 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%88%D0%BE%D0%BD%D1%81%D0%BA%D0%B0_%D0%B2%D1%80%D1%81%D0%BA%D0%B0" title="Јонска врска – Macedonian" lang="mk" hreflang="mk" data-title="Јонска врска" 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%85%E0%B4%AF%E0%B5%8B%E0%B4%A3%E0%B4%BF%E0%B4%95_%E0%B4%AC%E0%B4%A8%E0%B5%8D%E0%B4%A7%E0%B4%A8%E0%B4%82" title="അയോണിക ബന്ധനം – Malayalam" lang="ml" hreflang="ml" data-title="അയോണിക ബന്ധനം" data-language-autonym="മലയാളം" data-language-local-name="Malayalam" class="interlanguage-link-target"><span>മലയാളം</span></a></li><li class="interlanguage-link interwiki-mr mw-list-item"><a href="https://mr.wikipedia.org/wiki/%E0%A4%86%E0%A4%AF%E0%A4%A8%E0%A4%BF%E0%A4%95_%E0%A4%AC%E0%A4%82%E0%A4%A7" title="आयनिक बंध – Marathi" lang="mr" hreflang="mr" data-title="आयनिक बंध" data-language-autonym="मराठी" data-language-local-name="Marathi" class="interlanguage-link-target"><span>मराठी</span></a></li><li class="interlanguage-link interwiki-ms mw-list-item"><a href="https://ms.wikipedia.org/wiki/Ikatan_ionik" title="Ikatan ionik – Malay" lang="ms" hreflang="ms" data-title="Ikatan ionik" 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-mni mw-list-item"><a href="https://mni.wikipedia.org/wiki/%EA%AF%8F%EA%AF%82%EA%AF%A6%EA%AF%9B%EA%AF%87%EA%AF%AD%EA%AF%94%EA%AF%A3%EA%AF%9A%EA%AF%A6%EA%AF%82%EA%AF%A6%EA%AF%9F%EA%AF%A0_%EA%AF%82%EA%AF%A4%EA%AF%84%EA%AF%A8%EA%AF%9F" title="ꯏꯂꯦꯛꯇ꯭ꯔꯣꯚꯦꯂꯦꯟꯠ ꯂꯤꯄꯨꯟ – Manipuri" lang="mni" hreflang="mni" data-title="ꯏꯂꯦꯛꯇ꯭ꯔꯣꯚꯦꯂꯦꯟꯠ ꯂꯤꯄꯨꯟ" data-language-autonym="ꯃꯤꯇꯩ ꯂꯣꯟ" data-language-local-name="Manipuri" class="interlanguage-link-target"><span>ꯃꯤꯇꯩ ꯂꯣꯟ</span></a></li><li class="interlanguage-link interwiki-cdo mw-list-item"><a href="https://cdo.wikipedia.org/wiki/Li%C3%AA-c%E1%B9%B3%CC%84-gi%C3%B4ng" title="Liê-cṳ̄-giông – Mindong" lang="cdo" hreflang="cdo" data-title="Liê-cṳ̄-giông" data-language-autonym="閩東語 / Mìng-dĕ̤ng-ngṳ̄" data-language-local-name="Mindong" class="interlanguage-link-target"><span>閩東語 / Mìng-dĕ̤ng-ngṳ̄</span></a></li><li class="interlanguage-link interwiki-my mw-list-item"><a href="https://my.wikipedia.org/wiki/%E1%80%A1%E1%80%AD%E1%80%AF%E1%80%84%E1%80%BA%E1%80%9A%E1%80%BD%E1%80%94%E1%80%BA%E1%80%85%E1%80%8A%E1%80%BA%E1%80%B8" title="အိုင်ယွန်စည်း – Burmese" lang="my" hreflang="my" data-title="အိုင်ယွန်စည်း" data-language-autonym="မြန်မာဘာသာ" data-language-local-name="Burmese" class="interlanguage-link-target"><span>မြန်မာဘာသာ</span></a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Ionaire_binding" title="Ionaire binding – Dutch" lang="nl" hreflang="nl" data-title="Ionaire binding" 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/%E3%82%A4%E3%82%AA%E3%83%B3%E7%B5%90%E5%90%88" title="イオン結合 – Japanese" lang="ja" hreflang="ja" data-title="イオン結合" 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/Ionebinding" title="Ionebinding – Norwegian Bokmål" lang="nb" hreflang="nb" data-title="Ionebinding" 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/Ionebinding" title="Ionebinding – Norwegian Nynorsk" lang="nn" hreflang="nn" data-title="Ionebinding" 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/Ligam_ionic" title="Ligam ionic – Occitan" lang="oc" hreflang="oc" data-title="Ligam ionic" data-language-autonym="Occitan" data-language-local-name="Occitan" class="interlanguage-link-target"><span>Occitan</span></a></li><li class="interlanguage-link interwiki-om mw-list-item"><a href="https://om.wikipedia.org/wiki/Hidhoo_ayoonii" title="Hidhoo ayoonii – Oromo" lang="om" hreflang="om" data-title="Hidhoo ayoonii" data-language-autonym="Oromoo" data-language-local-name="Oromo" class="interlanguage-link-target"><span>Oromoo</span></a></li><li class="interlanguage-link interwiki-uz mw-list-item"><a href="https://uz.wikipedia.org/wiki/Ion_bog%CA%BBlanish" title="Ion bogʻlanish – Uzbek" lang="uz" hreflang="uz" data-title="Ion bogʻlanish" data-language-autonym="Oʻzbekcha / ўзбекча" data-language-local-name="Uzbek" class="interlanguage-link-target"><span>Oʻzbekcha / ўзбекча</span></a></li><li class="interlanguage-link interwiki-pnb mw-list-item"><a href="https://pnb.wikipedia.org/wiki/%D8%A2%D8%A6%D9%86%DB%8C_%D8%AC%D9%88%DA%91" title="آئنی جوڑ – Western Punjabi" lang="pnb" hreflang="pnb" data-title="آئنی جوڑ" 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/Wi%C4%85zanie_jonowe" title="Wiązanie jonowe – Polish" lang="pl" hreflang="pl" data-title="Wiązanie jonowe" 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/Liga%C3%A7%C3%A3o_i%C3%B4nica" title="Ligação iônica – Portuguese" lang="pt" hreflang="pt" data-title="Ligação iônica" data-language-autonym="Português" data-language-local-name="Portuguese" class="interlanguage-link-target"><span>Português</span></a></li><li class="interlanguage-link interwiki-kaa mw-list-item"><a href="https://kaa.wikipedia.org/wiki/Ion_baylan%C4%B1s%C4%B1w" title="Ion baylanısıw – Kara-Kalpak" lang="kaa" hreflang="kaa" data-title="Ion baylanısıw" data-language-autonym="Qaraqalpaqsha" data-language-local-name="Kara-Kalpak" class="interlanguage-link-target"><span>Qaraqalpaqsha</span></a></li><li class="interlanguage-link interwiki-ro mw-list-item"><a href="https://ro.wikipedia.org/wiki/Leg%C4%83tur%C4%83_ionic%C4%83" title="Legătură ionică – Romanian" lang="ro" hreflang="ro" data-title="Legătură ionică" data-language-autonym="Română" data-language-local-name="Romanian" class="interlanguage-link-target"><span>Română</span></a></li><li class="interlanguage-link interwiki-rue mw-list-item"><a href="https://rue.wikipedia.org/wiki/%D0%99%D0%BE%D0%BD%D0%BE%D0%B2%D0%B0_%D0%B2%D1%8F%D0%B7%D0%B1%D0%B0" title="Йонова вязба – Rusyn" lang="rue" hreflang="rue" data-title="Йонова вязба" data-language-autonym="Русиньскый" data-language-local-name="Rusyn" class="interlanguage-link-target"><span>Русиньскый</span></a></li><li class="interlanguage-link interwiki-ru mw-list-item"><a href="https://ru.wikipedia.org/wiki/%D0%98%D0%BE%D0%BD%D0%BD%D0%B0%D1%8F_%D1%81%D0%B2%D1%8F%D0%B7%D1%8C" title="Ионная связь – Russian" lang="ru" hreflang="ru" data-title="Ионная связь" 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/Lidhja_jonike" title="Lidhja jonike – Albanian" lang="sq" hreflang="sq" data-title="Lidhja jonike" data-language-autonym="Shqip" data-language-local-name="Albanian" class="interlanguage-link-target"><span>Shqip</span></a></li><li class="interlanguage-link interwiki-si mw-list-item"><a href="https://si.wikipedia.org/wiki/%E0%B6%85%E0%B6%BA%E0%B6%B1%E0%B7%92%E0%B6%9A_%E0%B6%B6%E0%B6%B1%E0%B7%8A%E0%B6%B0%E0%B6%B1" title="අයනික බන්ධන – Sinhala" lang="si" hreflang="si" data-title="අයනික බන්ධන" data-language-autonym="සිංහල" data-language-local-name="Sinhala" class="interlanguage-link-target"><span>සිංහල</span></a></li><li class="interlanguage-link interwiki-simple mw-list-item"><a href="https://simple.wikipedia.org/wiki/Ionic_bond" title="Ionic bond – Simple English" lang="en-simple" hreflang="en-simple" data-title="Ionic bond" data-language-autonym="Simple English" data-language-local-name="Simple English" class="interlanguage-link-target"><span>Simple English</span></a></li><li class="interlanguage-link interwiki-sk mw-list-item"><a href="https://sk.wikipedia.org/wiki/I%C3%B3nov%C3%A1_v%C3%A4zba" title="Iónová väzba – Slovak" lang="sk" hreflang="sk" data-title="Iónová väzba" 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/Ionska_vez" title="Ionska vez – Slovenian" lang="sl" hreflang="sl" data-title="Ionska vez" 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%A8%DB%95%D9%86%D8%AF%DB%8C_%D8%A6%D8%A7%DB%8C%DB%86%D9%86%DB%8C" title="بەندی ئایۆنی – Central Kurdish" lang="ckb" hreflang="ckb" data-title="بەندی ئایۆنی" 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%88%D0%BE%D0%BD%D1%81%D0%BA%D0%B0_%D0%B2%D0%B5%D0%B7%D0%B0" title="Јонска веза – Serbian" lang="sr" hreflang="sr" data-title="Јонска веза" 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/Jonska_veza" title="Jonska veza – Serbo-Croatian" lang="sh" hreflang="sh" data-title="Jonska veza" data-language-autonym="Srpskohrvatski / српскохрватски" data-language-local-name="Serbo-Croatian" class="interlanguage-link-target"><span>Srpskohrvatski / српскохрватски</span></a></li><li class="interlanguage-link interwiki-fi mw-list-item"><a href="https://fi.wikipedia.org/wiki/Ionisidos" title="Ionisidos – Finnish" lang="fi" hreflang="fi" data-title="Ionisidos" 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/Jonbindning" title="Jonbindning – Swedish" lang="sv" hreflang="sv" data-title="Jonbindning" 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%85%E0%AE%AF%E0%AE%A9%E0%AE%BF%E0%AE%AA%E0%AF%8D_%E0%AE%AA%E0%AE%BF%E0%AE%A3%E0%AF%88%E0%AE%AA%E0%AF%8D%E0%AE%AA%E0%AF%81" title="அயனிப் பிணைப்பு – Tamil" lang="ta" hreflang="ta" data-title="அயனிப் பிணைப்பு" data-language-autonym="தமிழ்" data-language-local-name="Tamil" class="interlanguage-link-target"><span>தமிழ்</span></a></li><li class="interlanguage-link interwiki-th mw-list-item"><a href="https://th.wikipedia.org/wiki/%E0%B8%9E%E0%B8%B1%E0%B8%99%E0%B8%98%E0%B8%B0%E0%B9%84%E0%B8%AD%E0%B8%AD%E0%B8%AD%E0%B8%99%E0%B8%B4%E0%B8%81" title="พันธะไอออนิก – Thai" lang="th" hreflang="th" data-title="พันธะไอออนิก" 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/%C4%B0yonik_ba%C4%9F" title="İyonik bağ – Turkish" lang="tr" hreflang="tr" data-title="İyonik bağ" 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%86%D0%BE%D0%BD%D0%BD%D0%B8%D0%B9_%D0%B7%D0%B2%27%D1%8F%D0%B7%D0%BE%D0%BA" title="Іонний зв'язок – Ukrainian" lang="uk" hreflang="uk" data-title="Іонний зв'язок" data-language-autonym="Українська" data-language-local-name="Ukrainian" class="interlanguage-link-target"><span>Українська</span></a></li><li class="interlanguage-link interwiki-vi mw-list-item"><a href="https://vi.wikipedia.org/wiki/Li%C3%AAn_k%E1%BA%BFt_ion" title="Liên kết ion – Vietnamese" lang="vi" hreflang="vi" data-title="Liên kết ion" 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/%E9%9B%A2%E5%AD%90%E9%8D%B5" title="離子鍵 – Literary Chinese" lang="lzh" hreflang="lzh" data-title="離子鍵" 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/%E7%A6%BB%E5%AD%90%E9%94%AE" title="离子键 – Wu" lang="wuu" hreflang="wuu" data-title="离子键" 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/%E9%9B%A2%E5%AD%90%E9%8D%B5" title="離子鍵 – Cantonese" lang="yue" hreflang="yue" data-title="離子鍵" 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/%E7%A6%BB%E5%AD%90%E9%94%AE" title="离子键 – Chinese" lang="zh" hreflang="zh" data-title="离子键" data-language-autonym="中文" data-language-local-name="Chinese" class="interlanguage-link-target"><span>中文</span></a></li> </ul> <div class="after-portlet after-portlet-lang"><span class="wb-langlinks-edit wb-langlinks-link"><a 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typeof="mw:File"><a href="/wiki/Wikipedia:Protection_policy#semi" title="This article is semi-protected."><img alt="Page semi-protected" src="//upload.wikimedia.org/wikipedia/en/thumb/1/1b/Semi-protection-shackle.svg/20px-Semi-protection-shackle.svg.png" decoding="async" width="20" height="20" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/1/1b/Semi-protection-shackle.svg/30px-Semi-protection-shackle.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/1/1b/Semi-protection-shackle.svg/40px-Semi-protection-shackle.svg.png 2x" data-file-width="512" data-file-height="512" /></a></span></div></div> </div> <div id="siteSub" class="noprint">From Wikipedia, the free encyclopedia</div> </div> <div id="contentSub"><div id="mw-content-subtitle"></div></div> <div id="mw-content-text" class="mw-body-content"><div class="mw-content-ltr mw-parser-output" lang="en" dir="ltr"><p class="mw-empty-elt"> </p> <div class="shortdescription nomobile noexcerpt noprint searchaux" style="display:none">Chemical bonding involving attraction between ions</div> <figure class="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/300px-NaF.gif" decoding="async" width="300" height="131" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/a/a8/NaF.gif/450px-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> and <a href="/wiki/Fluorine" title="Fluorine">fluorine</a> atoms undergoing a redox reaction to form sodium ions and fluoride ions. Sodium loses its outer <a href="/wiki/Electron" title="Electron">electron</a> to give it a stable <a href="/wiki/Electron_configuration" title="Electron configuration">electron configuration</a>, and this electron enters the fluorine atom <a href="/wiki/Exothermic" class="mw-redirect" title="Exothermic">exothermically</a>. The oppositely charged ions – typically a great many of them – are then attracted to each other to form solid <a href="/wiki/Sodium_fluoride" title="Sodium fluoride">sodium fluoride</a>.</figcaption></figure> <p><b>Ionic bonding</b> is a type of <a href="/wiki/Chemical_bond" title="Chemical bond">chemical bonding</a> that involves the <a href="/wiki/Coulomb%27s_law" title="Coulomb's law">electrostatic attraction</a> between oppositely charged <a href="/wiki/Ion" title="Ion">ions</a>, or between two <a href="/wiki/Atoms" class="mw-redirect" title="Atoms">atoms</a> with sharply different <a href="/wiki/Electronegativities" class="mw-redirect" title="Electronegativities">electronegativities</a>,<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> and is the primary interaction occurring in <a href="/wiki/Ionic_compound" class="mw-redirect" title="Ionic compound">ionic compounds</a>. It is one of the main types of bonding, along with <a href="/wiki/Covalent_bond" title="Covalent bond">covalent bonding</a> and <a href="/wiki/Metallic_bonding" title="Metallic bonding">metallic bonding</a>. Ions are atoms (or groups of atoms) with an electrostatic charge. Atoms that gain electrons make negatively charged ions (called <a href="/wiki/Anion" class="mw-redirect" title="Anion">anions</a>). Atoms that lose electrons make positively charged ions (called <a href="/wiki/Cations" class="mw-redirect" title="Cations">cations</a>). This transfer of electrons is known as <b>electrovalence</b> in contrast to <a href="/wiki/Covalent_bond" title="Covalent bond">covalence</a>. In the simplest case, the cation is a <a href="/wiki/Metal" title="Metal">metal</a> atom and the anion is a <a href="/wiki/Nonmetal_(chemistry)" class="mw-redirect" title="Nonmetal (chemistry)">nonmetal</a> atom, but these ions can be more complex, e.g. <a href="/wiki/Polyatomic_ions" class="mw-redirect" title="Polyatomic ions">molecular ions</a> like <span class="chemf nowrap">NH<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></span> or <span class="chemf nowrap">SO<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">4</sub></span></span></span>. In simpler words, an ionic bond results from the transfer of electrons from a <a href="/wiki/Metal" title="Metal">metal</a> to a <a href="/wiki/Non-metal" class="mw-redirect" title="Non-metal">non-metal</a> to obtain a full valence shell for both atoms. </p><p><i>Clean</i> ionic bonding — in which one atom or molecule completely transfers an electron to another — cannot exist: all ionic compounds have some degree of <a href="/wiki/Covalent_bond" title="Covalent bond">covalent bonding</a> or electron sharing. Thus, the term "ionic bonding" is given when the ionic character is greater than the covalent character – that is, a bond in which there is a large difference in <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a> between the two atoms, causing the bonding to be more polar (ionic) than in covalent bonding where electrons are shared more equally. Bonds with partially ionic and partially covalent characters are called <a href="/wiki/Polar_covalent_bond" class="mw-redirect" title="Polar covalent bond">polar covalent bonds</a>.<sup id="cite_ref-Seifert_2-0" class="reference"><a href="#cite_note-Seifert-2"><span class="cite-bracket">[</span>2<span class="cite-bracket">]</span></a></sup> </p><p>Ionic compounds conduct <a href="/wiki/Electricity" title="Electricity">electricity</a> when molten or in solution, typically not when solid. Ionic compounds generally have a high <a href="/wiki/Melting_point" title="Melting point">melting point</a>, depending on the charge of the ions they consist of. The higher the charges the stronger the cohesive forces and the higher the melting point. They also tend to be <a href="/wiki/Solubility" title="Solubility">soluble</a> in water; the stronger the cohesive forces, the lower the solubility.<sup id="cite_ref-3" class="reference"><a href="#cite_note-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Overview">Overview</h2></div> <p>Atoms that have an almost full or almost empty <a href="/wiki/Valence_shell" class="mw-redirect" title="Valence shell">valence shell</a> tend to be very <a href="/wiki/Chemical_reaction" title="Chemical reaction">reactive</a>. Strongly electronegative atoms (such as <a href="/wiki/Halogens" class="mw-redirect" title="Halogens">halogens</a>) often have only one or two empty electron states in their <a href="/wiki/Valence_shell" class="mw-redirect" title="Valence shell">valence shell</a>, and frequently <a href="/wiki/Chemical_bond" title="Chemical bond">bond</a> with other atoms or gain electrons to form <a href="/wiki/Anions" class="mw-redirect" title="Anions">anions</a>. Weakly electronegative atoms (such as <a href="/wiki/Alkali_metals" class="mw-redirect" title="Alkali metals">alkali metals</a>) have relatively few <a href="/wiki/Valence_electron" title="Valence electron">valence electrons</a>, which can easily be lost to strongly electronegative atoms. As a result, weakly electronegative atoms tend to distort their <a href="/wiki/Electron_cloud" class="mw-redirect" title="Electron cloud">electron cloud</a> and form <a href="/wiki/Cations" class="mw-redirect" title="Cations">cations</a>. </p> <div class="mw-heading mw-heading3"><h3 id="Properties_of_ionic_bonds">Properties of ionic bonds</h3></div> <ul><li>They are considered to be among the <b>strongest</b> of all types of chemical bonds. This often causes ionic compounds to be very stable.</li> <li>Ionic bonds have <b>high <a href="/wiki/Bond_energy" title="Bond energy">bond energy</a></b>. Bond energy is the mean amount of energy required to break the bond in the gaseous state.</li> <li>Most ionic compounds exist in the form of a <b><a href="/wiki/Crystal" title="Crystal">crystal</a> structure</b>, in which the ions occupy the corners of the crystal. Such a structure is called a <a href="/wiki/Crystal_structure" title="Crystal structure">crystal lattice</a>.</li> <li>Ionic compounds <b>lose their crystal lattice structure</b> and break up into ions when dissolved in <a href="/wiki/Water" title="Water">water</a> or any other <a href="/wiki/Polar_solvent" class="mw-redirect" title="Polar solvent">polar</a> solvent. This process is called solvation. The presence of these free ions makes aqueous ionic compound solutions good conductors of electricity. The same occurs when the compounds are heated above their <a href="/wiki/Melting_point" title="Melting point">melting point</a> in a process known as <a href="/wiki/Melting" title="Melting">melting</a>.</li></ul> <div class="mw-heading mw-heading2"><h2 id="Formation">Formation</h2></div> <p>Ionic bonding can result from a <a href="/wiki/Redox" title="Redox">redox</a> reaction when atoms of an element (usually <a href="/wiki/Metal" title="Metal">metal</a>), whose <a href="/wiki/Ionization_energy" title="Ionization energy">ionization energy</a> is low, give some of their electrons to achieve a stable electron configuration. In doing so, cations are formed. An atom of another element (usually nonmetal) with greater <a href="/wiki/Electron_affinity" title="Electron affinity">electron affinity</a> accepts one or more electrons to attain a stable <a href="/wiki/Electron_configuration" title="Electron configuration">electron configuration</a>, and after accepting electrons an atom becomes an anion. Typically, the stable electron configuration is one of the <a href="/wiki/Noble_gases" class="mw-redirect" title="Noble gases">noble gases</a> for elements in the <a href="/wiki/S-block" class="mw-redirect" title="S-block">s-block</a> and the <a href="/wiki/P-block" class="mw-redirect" title="P-block">p-block</a>, and particular <a href="/wiki/Electron_configuration" title="Electron configuration">stable electron configurations</a> for <a href="/wiki/D-block" class="mw-redirect" title="D-block">d-block</a> and <a href="/wiki/F-block" class="mw-redirect" title="F-block">f-block</a> elements. The electrostatic attraction between the anions and cations leads to the formation of a solid with a <a href="/wiki/Crystallographic_lattice" class="mw-redirect" title="Crystallographic lattice">crystallographic lattice</a> in which the ions are stacked in an alternating fashion. In such a lattice, it is usually not possible to distinguish discrete molecular units, so that the compounds formed are not molecular. However, the ions themselves can be complex and form molecular ions like the acetate anion or the ammonium cation. </p> <figure class="mw-halign-right" typeof="mw:File/Thumb"><a href="/wiki/File:Ionic_Bonding_LiF.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/2/22/Ionic_Bonding_LiF.svg/250px-Ionic_Bonding_LiF.svg.png" decoding="async" width="250" height="106" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/22/Ionic_Bonding_LiF.svg/375px-Ionic_Bonding_LiF.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/22/Ionic_Bonding_LiF.svg/500px-Ionic_Bonding_LiF.svg.png 2x" data-file-width="512" data-file-height="218" /></a><figcaption>Representation of ionic bonding between <a href="/wiki/Lithium" title="Lithium">lithium</a> and <a href="/wiki/Fluorine" title="Fluorine">fluorine</a> to form <a href="/wiki/Lithium_fluoride" title="Lithium fluoride">lithium fluoride</a>. Lithium has a low ionization energy and readily gives up its lone <a href="/wiki/Valence_electron" title="Valence electron">valence electron</a> to a fluorine atom, which has a positive electron affinity and accepts the electron that was donated by the lithium atom. The end-result is that lithium is <a href="/wiki/Isoelectronicity" title="Isoelectronicity">isoelectronic</a> with <a href="/wiki/Helium" title="Helium">helium</a> and fluorine is isoelectronic with <a href="/wiki/Neon" title="Neon">neon</a>. Electrostatic interaction occurs between the two resulting ions, but typically aggregation is not limited to two of them. Instead, aggregation into a whole lattice held together by ionic bonding is the result.</figcaption></figure> <p>For example, common <a href="/wiki/Table_salt" class="mw-redirect" title="Table salt">table salt</a> is <a href="/wiki/Sodium_chloride" title="Sodium chloride">sodium chloride</a>. When <a href="/wiki/Sodium" title="Sodium">sodium</a> (Na) and <a href="/wiki/Chlorine" title="Chlorine">chlorine</a> (Cl) are combined, the sodium atoms each lose an <a href="/wiki/Electron" title="Electron">electron</a>, forming cations (Na<sup>+</sup>), and the chlorine atoms each gain an electron to form anions (Cl<sup>−</sup>). These ions are then attracted to each other in a 1:1 ratio to form sodium chloride (NaCl). </p> <dl><dd>Na + Cl → Na<sup>+</sup> + Cl<sup>−</sup> → NaCl</dd></dl> <p>However, to maintain charge neutrality, strict ratios between anions and cations are observed so that ionic compounds, in general, obey the rules of stoichiometry despite not being molecular compounds. For compounds that are transitional to the alloys and possess mixed ionic and metallic bonding, this may not be the case anymore. Many sulfides, e.g., do form non-stoichiometric compounds. </p><p>Many ionic compounds are referred to as <b>salts</b> as they can also be formed by the neutralization reaction of an Arrhenius base like NaOH with an Arrhenius acid like HCl </p> <dl><dd>NaOH + HCl → NaCl + H<sub>2</sub>O</dd></dl> <p>The salt NaCl is then said to consist of the acid rest Cl<sup>−</sup> and the base rest Na<sup>+</sup>. </p><p>The removal of electrons to form the cation is endothermic, raising the system's overall energy. There may also be energy changes associated with breaking of existing bonds or the addition of more than one electron to form anions. However, the action of the anion's accepting the cation's valence electrons and the subsequent attraction of the ions to each other releases (lattice) energy and, thus, lowers the overall energy of the system. </p><p>Ionic bonding will occur only if the overall energy change for the reaction is favorable. In general, the reaction is exothermic, but, e.g., the formation of mercuric oxide (HgO) is endothermic. The charge of the resulting ions is a major factor in the strength of ionic bonding, e.g. a salt C<sup>+</sup>A<sup>−</sup> is held together by electrostatic forces roughly four times weaker than C<sup>2+</sup>A<sup>2−</sup> according to <a href="/wiki/Coulomb%27s_law" title="Coulomb's law">Coulomb's law</a>, where C and A represent a generic cation and anion respectively. The sizes of the ions and the particular packing of the lattice are ignored in this rather simplistic argument. </p> <div class="mw-heading mw-heading2"><h2 id="Structures">Structures</h2></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">Main article: <a href="/wiki/Ionic_compound" class="mw-redirect" title="Ionic compound">Ionic compound</a></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:NaCl_bonds.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/d/dd/NaCl_bonds.svg/220px-NaCl_bonds.svg.png" decoding="async" width="220" height="191" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/dd/NaCl_bonds.svg/330px-NaCl_bonds.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/dd/NaCl_bonds.svg/440px-NaCl_bonds.svg.png 2x" data-file-width="1152" data-file-height="1001" /></a><figcaption>In the rock salt lattice, each sodium ion (purple sphere) has an <a href="/wiki/Electrostatic" class="mw-redirect" title="Electrostatic">electrostatic</a> interaction with its eight nearest-neighbour chloride ions (green spheres)</figcaption></figure> <p>Ionic compounds in the solid state form lattice structures. The two principal factors in determining the form of the lattice are the relative charges of the ions and their relative sizes. Some structures are adopted by a number of compounds; for example, the structure of the rock salt <a href="/wiki/Sodium_chloride" title="Sodium chloride">sodium chloride</a> is also adopted by many <a href="/wiki/Alkali_metals" class="mw-redirect" title="Alkali metals">alkali</a> halides, and binary oxides such as <a href="/wiki/Magnesium_oxide" title="Magnesium oxide">magnesium oxide</a>. <a href="/wiki/Pauling%27s_rules" title="Pauling's rules">Pauling's rules</a> provide guidelines for predicting and rationalizing the crystal structures of ionic crystals </p> <div class="mw-heading mw-heading2"><h2 id="Strength_of_the_bonding">Strength of the bonding</h2></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1236090951"><div role="note" class="hatnote navigation-not-searchable">Main article: <a href="/wiki/Lattice_energy" title="Lattice energy">Lattice energy</a></div> <p>For a solid crystalline ionic compound the <a href="/wiki/Enthalpy" title="Enthalpy">enthalpy</a> change in forming the solid from gaseous ions is termed the <a href="/wiki/Lattice_energy" title="Lattice energy">lattice energy</a>. The experimental value for the <a href="/wiki/Lattice_energy" title="Lattice energy">lattice energy</a> can be determined using the <a href="/wiki/Born%E2%80%93Haber_cycle" title="Born–Haber cycle">Born–Haber cycle</a>. It can also be calculated (predicted) using the <a href="/wiki/Born%E2%80%93Land%C3%A9_equation" title="Born–Landé equation">Born–Landé equation</a> as the sum of the <a href="/wiki/Electrostatic_potential_energy" class="mw-redirect" title="Electrostatic potential energy">electrostatic potential energy</a>, calculated by summing interactions between cations and anions, and a short-range repulsive potential energy term. The <a href="/wiki/Electrostatic_potential" class="mw-redirect" title="Electrostatic potential">electrostatic potential</a> can be expressed in terms of the interionic separation and a constant (<a href="/wiki/Madelung_constant" title="Madelung constant">Madelung constant</a>) that takes account of the geometry of the crystal. The further away from the nucleus the weaker the shield. The <a href="/wiki/Born%E2%80%93Land%C3%A9_equation" title="Born–Landé equation">Born–Landé equation</a> gives a reasonable fit to the lattice energy of, e.g., sodium chloride, where the calculated (predicted) value is −756 kJ/mol, which compares to −787 kJ/mol using the <a href="/wiki/Born%E2%80%93Haber_cycle" title="Born–Haber cycle">Born–Haber cycle</a>.<sup id="cite_ref-4" class="reference"><a href="#cite_note-4"><span class="cite-bracket">[</span>4<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-5" class="reference"><a href="#cite_note-5"><span class="cite-bracket">[</span>5<span class="cite-bracket">]</span></a></sup> In aqueous solution the binding strength can be described by the <a href="/wiki/Bjerrum_plot" title="Bjerrum plot">Bjerrum</a> or Fuoss equation as function of the ion charges, rather independent of the nature of the ions such as polarizability or size.<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> The strength of salt bridges is most often evaluated by measurements of equilibria between molecules containing cationic and anionic sites, most often in solution.<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> Equilibrium constants in water indicate additive free energy contributions for each salt bridge. Another method for the identification of hydrogen bonds also in complicated molecules is <a href="/wiki/Crystallography" title="Crystallography">crystallography</a>, sometimes also NMR-spectroscopy. </p><p>The attractive forces defining the strength of ionic bonding can be modeled by <a href="/wiki/Coulomb%27s_law" title="Coulomb's law">Coulomb's Law</a>. Ionic bond strengths are typically (cited ranges vary) between 170 and 1500 kJ/mol.<sup id="cite_ref-8" class="reference"><a href="#cite_note-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup><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> <div class="mw-heading mw-heading2"><h2 id="Polarization_power_effects">Polarization power effects</h2></div> <p><a href="/wiki/Ion" title="Ion">Ions</a> in <a href="/wiki/Crystal_lattice" class="mw-redirect" title="Crystal lattice">crystal lattices</a> of purely ionic compounds are <a href="/wiki/Sphere" title="Sphere">spherical</a>; however, if the positive ion is small and/or highly charged, it will distort the electron cloud of the negative ion, an effect summarised in <a href="/wiki/Fajans%27_rules" title="Fajans' rules">Fajans' rules</a>. This <a href="/wiki/Polarization_(electrostatics)" class="mw-redirect" title="Polarization (electrostatics)">polarization</a> of the negative ion leads to a build-up of extra charge density between the two <a href="/wiki/Atomic_nucleus" title="Atomic nucleus">nuclei</a>, that is, to partial covalency. Larger negative ions are more easily polarized, but the effect is usually important only when positive ions with <a href="/wiki/Electrical_charge" class="mw-redirect" title="Electrical charge">charges</a> of 3+ (e.g., Al<sup>3+</sup>) are involved. However, 2+ ions (Be<sup>2+</sup>) or even 1+ (Li<sup>+</sup>) show some polarizing power because their sizes are so small (e.g., LiI is ionic but has some covalent bonding present). Note that this is not the <a href="/wiki/Ionic_polarization" class="mw-redirect" title="Ionic polarization">ionic polarization</a> effect that refers to displacement of ions in the lattice due to the application of an electric field. </p> <div class="mw-heading mw-heading2"><h2 id="Comparison_with_covalent_bonding">Comparison with covalent bonding</h2></div> <p>In ionic bonding, the atoms are bound by attraction of oppositely charged ions, whereas, in <a href="/wiki/Covalent_bond" title="Covalent bond">covalent bonding</a>, atoms are bound by sharing electrons to attain stable electron configurations. In covalent bonding, the <a href="/wiki/Molecular_geometry" title="Molecular geometry">molecular geometry</a> around each atom is determined by valence shell electron pair repulsion <a href="/wiki/VSEPR" class="mw-redirect" title="VSEPR">VSEPR</a> rules, whereas, in ionic materials, the geometry follows maximum <a href="/wiki/Close-packing" class="mw-redirect" title="Close-packing">packing</a> rules. One could say that covalent bonding is more <i>directional</i> in the sense that the energy penalty for not adhering to the optimum bond angles is large, whereas ionic bonding has no such penalty. There are no shared electron pairs to repel each other, the ions should simply be packed as efficiently as possible. This often leads to much higher <a href="/wiki/Coordination_number" title="Coordination number">coordination numbers</a>. In NaCl, each ion has 6 bonds and all bond angles are 90°. In CsCl the coordination number is 8. By comparison carbon typically has a maximum of four bonds. </p><p>Purely ionic bonding cannot exist, as the proximity of the entities involved in the bonding allows some degree of sharing <a href="/wiki/Electron_density" title="Electron density">electron density</a> between them. Therefore, all ionic bonding has some covalent character. Thus, bonding is considered ionic where the ionic character is greater than the covalent character. The larger the difference in <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a> between the two types of atoms involved in the bonding, the more ionic (polar) it is. Bonds with partially ionic and partially covalent character are called <a href="/wiki/Polar_covalent_bond" class="mw-redirect" title="Polar covalent bond">polar covalent bonds</a>. For example, Na–Cl and Mg–O interactions have a few percent covalency, while Si–O bonds are usually ~50% ionic and ~50% covalent. <a href="/wiki/Linus_Pauling" title="Linus Pauling">Pauling</a> estimated that an electronegativity difference of 1.7 (on the <a href="/wiki/Electronegativity#Pauling_electronegativity" title="Electronegativity">Pauling scale</a>) corresponds to 50% ionic character, so that a difference greater than 1.7 corresponds to a bond which is predominantly ionic.<sup id="cite_ref-10" class="reference"><a href="#cite_note-10"><span class="cite-bracket">[</span>10<span class="cite-bracket">]</span></a></sup> </p><p>Ionic character in covalent bonds can be directly measured for atoms having quadrupolar nuclei (<sup>2</sup>H, <sup>14</sup>N, <sup>81,79</sup>Br, <sup>35,37</sup>Cl or <sup>127</sup>I). These nuclei are generally objects of NQR <a href="/wiki/Nuclear_quadrupole_resonance" title="Nuclear quadrupole resonance">nuclear quadrupole resonance</a> and NMR <a href="/wiki/Nuclear_magnetic_resonance" title="Nuclear magnetic resonance">nuclear magnetic resonance</a> studies. Interactions between the nuclear quadrupole moments <i>Q</i> and the electric field gradients (EFG) are characterized via the nuclear quadrupole coupling constants </p> <dl><dd>QCC = <style data-mw-deduplicate="TemplateStyles:r1214402035">.mw-parser-output .sfrac{white-space:nowrap}.mw-parser-output .sfrac.tion,.mw-parser-output .sfrac .tion{display:inline-block;vertical-align:-0.5em;font-size:85%;text-align:center}.mw-parser-output .sfrac .num{display:block;line-height:1em;margin:0.0em 0.1em;border-bottom:1px solid}.mw-parser-output .sfrac .den{display:block;line-height:1em;margin:0.1em 0.1em}.mw-parser-output .sr-only{border:0;clip:rect(0,0,0,0);clip-path:polygon(0px 0px,0px 0px,0px 0px);height:1px;margin:-1px;overflow:hidden;padding:0;position:absolute;width:1px}</style><span class="sfrac">⁠<span class="tion"><span class="num"><i>e</i><sup>2</sup><i>q</i><sub>zz</sub><i>Q</i></span><span class="sr-only">/</span><span class="den"><i>h</i></span></span>⁠</span></dd></dl> <p>where the <i>eq</i><sub>zz</sub> term corresponds to the principal component of the EFG tensor and <i>e</i> is the elementary charge. In turn, the electric field gradient opens the way to description of bonding modes in molecules when the QCC values are accurately determined by NMR or NQR methods. </p><p>In general, when ionic bonding occurs in the solid (or liquid) state, it is not possible to talk about a single "ionic bond" between two individual atoms, because the cohesive forces that keep the lattice together are of a more collective nature. This is quite different in the case of covalent bonding, where we can often speak of a distinct bond localized between two particular atoms. However, even if ionic bonding is combined with some covalency, the result is <i>not</i> necessarily discrete bonds of a localized character.<sup id="cite_ref-Seifert_2-1" class="reference"><a href="#cite_note-Seifert-2"><span class="cite-bracket">[</span>2<span class="cite-bracket">]</span></a></sup> In such cases, the resulting bonding often requires description in terms of a band structure consisting of gigantic molecular orbitals spanning the entire crystal. Thus, the bonding in the solid often retains its collective rather than localized nature. When the difference in electronegativity is decreased, the bonding may then lead to a <a href="/wiki/Semiconductor" title="Semiconductor">semiconductor</a>, a <a href="/wiki/Semimetal" title="Semimetal">semimetal</a> or eventually a metallic conductor with metallic bonding. </p> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2></div> <ul><li><a href="/wiki/Coulomb%27s_law" title="Coulomb's law">Coulomb's law</a></li> <li><a href="/wiki/Salt_bridge_(protein_and_supramolecular)" title="Salt bridge (protein and supramolecular)">Salt bridge (protein and supramolecular)</a></li> <li><a href="/wiki/Ionic_potential" title="Ionic potential">Ionic potential</a></li> <li><a href="/wiki/Linear_combination_of_atomic_orbitals" title="Linear combination of atomic orbitals">Linear combination of atomic orbitals</a></li> <li><a href="/wiki/Orbital_hybridization" class="mw-redirect" title="Orbital hybridization">Hybridization</a></li> <li><a href="/wiki/Chemical_polarity" title="Chemical polarity">Chemical polarity</a></li> <li><a href="/wiki/Ioliomics" title="Ioliomics">Ioliomics</a></li> <li><a href="/wiki/Electron_configuration" title="Electron configuration">Electron configuration</a></li> <li><a href="/wiki/Aufbau_principle" title="Aufbau principle">Aufbau principle</a></li> <li><a href="/wiki/Quantum_numbers" class="mw-redirect" title="Quantum numbers">Quantum numbers</a> <ul><li><a href="/wiki/Azimuthal_quantum_number" title="Azimuthal quantum number">Azimuthal quantum number</a></li> <li><a href="/wiki/Principal_quantum_number" title="Principal quantum number">Principal quantum number</a></li> <li><a href="/wiki/Magnetic_quantum_number" title="Magnetic quantum number">Magnetic quantum number</a></li> <li><a href="/wiki/Spin_quantum_number" title="Spin quantum number">Spin quantum number</a></li></ul></li></ul> <div class="mw-heading mw-heading2"><h2 id="References">References</h2></div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist"> <div class="mw-references-wrap"><ol class="references"> <li id="cite_note-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 .id-lock-limited.id-lock-limited a,.mw-parser-output .id-lock-registration.id-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/d/d6/Lock-gray-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .id-lock-subscription.id-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/a/aa/Lock-red-alt-2.svg")right 0.1em center/9px no-repeat}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/4/4c/Wikisource-logo.svg")right 0.1em center/12px no-repeat}body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-free a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-limited a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-registration a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .id-lock-subscription a,body:not(.skin-timeless):not(.skin-minerva) .mw-parser-output .cs1-ws-icon a{background-size:contain;padding:0 1em 0 0}.mw-parser-output .cs1-code{color:inherit;background:inherit;border:none;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;color:var(--color-error,#d33)}.mw-parser-output .cs1-visible-error{color:var(--color-error,#d33)}.mw-parser-output .cs1-maint{display:none;color:#085;margin-left:0.3em}.mw-parser-output .cs1-kern-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right{padding-right:0.2em}.mw-parser-output .citation .mw-selflink{font-weight:inherit}@media screen{.mw-parser-output .cs1-format{font-size:95%}html.skin-theme-clientpref-night .mw-parser-output .cs1-maint{color:#18911f}}@media screen and (prefers-color-scheme:dark){html.skin-theme-clientpref-os .mw-parser-output .cs1-maint{color:#18911f}}</style><cite class="citation book cs1"><a rel="nofollow" class="external text" href="https://doi.org/10.1351/goldbook.IT07058">"Ionic bond"</a>. <i>IUPAC Compendium of Chemical Terminology</i>. 2009. <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.IT07058">10.1351/goldbook.IT07058</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-9678550-9-7" title="Special:BookSources/978-0-9678550-9-7"><bdi>978-0-9678550-9-7</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Ionic+bond&rft.btitle=IUPAC+Compendium+of+Chemical+Terminology&rft.date=2009&rft_id=info%3Adoi%2F10.1351%2Fgoldbook.IT07058&rft.isbn=978-0-9678550-9-7&rft_id=https%3A%2F%2Fdoi.org%2F10.1351%2Fgoldbook.IT07058&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIonic+bonding" class="Z3988"></span></span> </li> <li id="cite_note-Seifert-2"><span class="mw-cite-backlink">^ <a href="#cite_ref-Seifert_2-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Seifert_2-1"><sup><i><b>b</b></i></sup></a></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSeifert2023" class="citation web cs1">Seifert, Vanessa (27 November 2023). <a rel="nofollow" class="external text" href="https://www.chemistryworld.com/opinion/do-bond-classifications-help-or-hinder-chemistry/4018431.article">"Do bond classifications help or hinder chemistry?"</a>. <i>chemistryworld.com</i><span class="reference-accessdate">. Retrieved <span class="nowrap">22 January</span> 2024</span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=chemistryworld.com&rft.atitle=Do+bond+classifications+help+or+hinder+chemistry%3F&rft.date=2023-11-27&rft.aulast=Seifert&rft.aufirst=Vanessa&rft_id=https%3A%2F%2Fwww.chemistryworld.com%2Fopinion%2Fdo-bond-classifications-help-or-hinder-chemistry%2F4018431.article&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIonic+bonding" class="Z3988"></span></span> </li> <li id="cite_note-3"><span class="mw-cite-backlink"><b><a href="#cite_ref-3">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFSchneider2012" class="citation book cs1">Schneider, Hans-Jörg (2012). "Ionic Interactions in Supramolecular Complexes". <i>Ionic Interactions in Natural and Synthetic Macromolecules</i>. pp. 35–47. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<a rel="nofollow" class="external text" href="https://doi.org/10.1002%2F9781118165850.ch2">10.1002/9781118165850.ch2</a>. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/9781118165850" title="Special:BookSources/9781118165850"><bdi>9781118165850</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=bookitem&rft.atitle=Ionic+Interactions+in+Supramolecular+Complexes&rft.btitle=Ionic+Interactions+in+Natural+and+Synthetic+Macromolecules&rft.pages=35-47&rft.date=2012&rft_id=info%3Adoi%2F10.1002%2F9781118165850.ch2&rft.isbn=9781118165850&rft.aulast=Schneider&rft.aufirst=Hans-J%C3%B6rg&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIonic+bonding" class="Z3988"></span></span> </li> <li id="cite_note-4"><span class="mw-cite-backlink"><b><a href="#cite_ref-4">^</a></b></span> <span class="reference-text">David Arthur Johnson, <i>Metals and Chemical Change</i>, Open University, Royal Society of Chemistry, 2002, <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/0-85404-665-8" title="Special:BookSources/0-85404-665-8">0-85404-665-8</a></span> </li> <li id="cite_note-5"><span class="mw-cite-backlink"><b><a href="#cite_ref-5">^</a></b></span> <span class="reference-text">Linus Pauling, <i>The Nature of the Chemical Bond and the Structure of Molecules and Crystals: An Introduction to Modern Structural Chemistry</i>, Cornell University Press, 1960 <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/0-801-40333-2" title="Special:BookSources/0-801-40333-2">0-801-40333-2</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/10.1021%2Fja01355a027">10.1021/ja01355a027</a></span> </li> <li id="cite_note-6"><span class="mw-cite-backlink"><b><a href="#cite_ref-6">^</a></b></span> <span class="reference-text">Schneider, H.-J.; Yatsimirsky, A. 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"Experimental Binding Energies in Supramolecular Complexes". <i>Chemical Reviews</i>. <b>116</b> (9): 5216–300. <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%2Facs.chemrev.5b00583">10.1021/acs.chemrev.5b00583</a>. <a href="/wiki/PMID_(identifier)" class="mw-redirect" title="PMID (identifier)">PMID</a> <a rel="nofollow" class="external text" href="https://pubmed.ncbi.nlm.nih.gov/27136957">27136957</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Chemical+Reviews&rft.atitle=Experimental+Binding+Energies+in+Supramolecular+Complexes&rft.volume=116&rft.issue=9&rft.pages=5216-300&rft.date=2016-05&rft_id=info%3Adoi%2F10.1021%2Facs.chemrev.5b00583&rft_id=info%3Apmid%2F27136957&rft.aulast=Biedermann&rft.aufirst=F&rft.au=Schneider%2C+HJ&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIonic+bonding" class="Z3988"></span></span> </li> <li id="cite_note-8"><span class="mw-cite-backlink"><b><a href="#cite_ref-8">^</a></b></span> <span class="reference-text">Soboyejo, W.O (2003). Mechanical properties of engineered materials. Marcel Dekker. pp. 16–17. <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/0-203-91039-7" title="Special:BookSources/0-203-91039-7">0-203-91039-7</a>. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/OCLC_(identifier)" class="mw-redirect" title="OCLC (identifier)">OCLC</a> <a rel="nofollow" class="external text" href="https://www.worldcat.org/oclc/54091550">54091550</a>.</span> </li> <li id="cite_note-9"><span class="mw-cite-backlink"><b><a href="#cite_ref-9">^</a></b></span> <span class="reference-text">Askeland, Donald R. (January 2015). The science and engineering of materials. Wright, Wendelin J. (Seventh ed.). Boston, MA. pp. 38. <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/978-1-305-07676-1" title="Special:BookSources/978-1-305-07676-1">978-1-305-07676-1</a>. <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><a href="/wiki/OCLC_(identifier)" class="mw-redirect" title="OCLC (identifier)">OCLC</a> <a rel="nofollow" class="external text" href="https://www.worldcat.org/oclc/903959750">903959750</a>.</span> </li> <li id="cite_note-10"><span class="mw-cite-backlink"><b><a href="#cite_ref-10">^</a></b></span> <span class="reference-text">L. Pauling <i>The Nature of the Chemical Bond</i> (3rd ed., Oxford University Press 1960) p.98-100.</span> </li> </ol></div></div> <div class="mw-heading mw-heading2"><h2 id="External_links">External links</h2></div> <ul><li><a rel="nofollow" class="external text" href="http://www.chemteam.info/Bonding/Ionic-Bond.html">Ionic bonding tutorial</a></li> <li><a rel="nofollow" class="external text" href="https://web.archive.org/web/20080116044400/http://sciencehack.com/videos/view/xTx_DWboEVs">Video on ionic bonding</a></li></ul> <div class="navbox-styles"><style data-mw-deduplicate="TemplateStyles:r1129693374">.mw-parser-output .hlist dl,.mw-parser-output .hlist ol,.mw-parser-output .hlist ul{margin:0;padding:0}.mw-parser-output .hlist dd,.mw-parser-output .hlist dt,.mw-parser-output .hlist li{margin:0;display:inline}.mw-parser-output .hlist.inline,.mw-parser-output .hlist.inline dl,.mw-parser-output .hlist.inline ol,.mw-parser-output .hlist.inline ul,.mw-parser-output .hlist dl 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href="/wiki/Metal%E2%80%93ligand_multiple_bond" title="Metal–ligand multiple bond">Metal–ligand multiple bond</a></li> <li><a href="/wiki/Charge-shift_bond" title="Charge-shift bond">Charge-shift</a></li> <li><a href="/wiki/Hapticity" title="Hapticity">Hapticity</a></li> <li><a href="/wiki/Conjugated_system" title="Conjugated system">Conjugation</a></li> <li><a href="/wiki/Hyperconjugation" title="Hyperconjugation">Hyperconjugation</a></li> <li><a href="/wiki/Aromaticity" title="Aromaticity">Aromaticity</a> <ul><li><a href="/wiki/Homoaromaticity" title="Homoaromaticity">homo</a></li> <li><a href="/wiki/Bicycloaromaticity" title="Bicycloaromaticity">bicyclo</a></li></ul></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Metallic_bonding" title="Metallic bonding">Metallic</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Metal_aromaticity" title="Metal aromaticity">Metal aromaticity</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a class="mw-selflink selflink">Ionic</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li class="mw-empty-elt"></li></ul> </div></td></tr></tbody></table><div></div></td><td class="noviewer navbox-image" rowspan="4" style="width:1px;padding:0 0 0 2px"><div><span typeof="mw:File"><a href="/wiki/File:Ligatio-covalens.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/2/21/Ligatio-covalens.svg/200px-Ligatio-covalens.svg.png" decoding="async" width="200" height="89" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/2/21/Ligatio-covalens.svg/300px-Ligatio-covalens.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/2/21/Ligatio-covalens.svg/400px-Ligatio-covalens.svg.png 2x" data-file-width="597" data-file-height="265" /></a></span><br /><span typeof="mw:File"><a href="/wiki/File:Chemfm_carbon_monoxide_3_1.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/77/Chemfm_carbon_monoxide_3_1.svg/200px-Chemfm_carbon_monoxide_3_1.svg.png" decoding="async" width="200" height="113" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/77/Chemfm_carbon_monoxide_3_1.svg/300px-Chemfm_carbon_monoxide_3_1.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/77/Chemfm_carbon_monoxide_3_1.svg/400px-Chemfm_carbon_monoxide_3_1.svg.png 2x" data-file-width="99" data-file-height="56" /></a></span><br /><span typeof="mw:File"><a href="/wiki/File:Pi-Bond.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/7/70/Pi-Bond.svg/200px-Pi-Bond.svg.png" decoding="async" width="200" height="113" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/7/70/Pi-Bond.svg/300px-Pi-Bond.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/7/70/Pi-Bond.svg/400px-Pi-Bond.svg.png 2x" data-file-width="1920" data-file-height="1080" /></a></span></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Intermolecular_force" title="Intermolecular force">Intermolecular</a><br />(weak)</th><td class="navbox-list-with-group navbox-list navbox-odd hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"></div><table class="nowraplinks navbox-subgroup" style="border-spacing:0"><tbody><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Van_der_Waals_force" title="Van der Waals force">Van der Waals<br />forces</a></th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/London_dispersion_force" title="London dispersion force">London dispersion</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Hydrogen_bond" title="Hydrogen bond">Hydrogen</a></th><td class="navbox-list-with-group navbox-list navbox-odd" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Low-barrier_hydrogen_bond" title="Low-barrier hydrogen bond">Low-barrier</a></li> <li><a href="/wiki/Resonance-assisted_hydrogen_bond" class="mw-redirect" title="Resonance-assisted hydrogen bond">Resonance-assisted</a></li> <li><a href="/wiki/Symmetric_hydrogen_bond" title="Symmetric hydrogen bond">Symmetric</a></li> <li><a href="/wiki/Dihydrogen_bond" title="Dihydrogen bond">Dihydrogen bonds</a></li> <li><a href="/wiki/C%E2%80%93H%C2%B7%C2%B7%C2%B7O_interaction" title="C–H···O interaction">C–H···O interaction</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Non-covalent_interactions" class="mw-redirect" title="Non-covalent interactions">Noncovalent</a><br />other</th><td class="navbox-list-with-group navbox-list navbox-even" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Mechanically_interlocked_molecular_architectures" title="Mechanically interlocked molecular architectures">Mechanical</a></li> <li><a href="/wiki/Halogen_bond" title="Halogen bond">Halogen</a></li> <li><a href="/wiki/Chalcogen_bond" title="Chalcogen bond">Chalcogen</a></li> <li><a href="/wiki/Metallophilic_interaction" title="Metallophilic interaction">Metallophilic</a> (<a href="/wiki/Aurophilicity" title="Aurophilicity">aurophilic</a>)</li> <li><a href="/wiki/Intercalation_(chemistry)" title="Intercalation (chemistry)">Intercalation</a></li> <li><a href="/wiki/Stacking_(chemistry)" title="Stacking (chemistry)">Stacking</a></li> <li><a href="/wiki/Cation%E2%80%93pi_interaction" class="mw-redirect" title="Cation–pi interaction">Cation–pi</a></li> <li><a href="/wiki/Cation%E2%80%93pi_interaction#Anion–π_interaction" class="mw-redirect" title="Cation–pi interaction">Anion–pi</a></li> <li><a href="/wiki/Salt_bridge_(protein_and_supramolecular)" title="Salt bridge (protein and supramolecular)">Salt bridge</a></li></ul> </div></td></tr></tbody></table><div></div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Bond_cleavage" title="Bond cleavage">Bond cleavage</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/Heterolysis_(chemistry)" title="Heterolysis (chemistry)">Heterolysis</a></li> <li><a href="/wiki/Homolysis_(chemistry)" title="Homolysis (chemistry)">Homolysis</a></li></ul> </div></td></tr><tr><th scope="row" class="navbox-group" style="width:1%"><a href="/wiki/Electron_counting" title="Electron counting">Electron counting</a> rules</th><td class="navbox-list-with-group navbox-list navbox-even 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