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class="vector-toc-numb">1.1</span> <span>Legame ionico</span> </div> </a> <ul id="toc-Legame_ionico-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Legame_covalente" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Legame_covalente"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.2</span> <span>Legame covalente</span> </div> </a> <ul id="toc-Legame_covalente-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Legame_metallico" class="vector-toc-list-item vector-toc-level-2"> <a class="vector-toc-link" href="#Legame_metallico"> <div class="vector-toc-text"> <span class="vector-toc-numb">1.3</span> <span>Legame metallico</span> </div> </a> <ul id="toc-Legame_metallico-sublist" class="vector-toc-list"> </ul> </li> </ul> </li> <li id="toc-Formazione_del_legame" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Formazione_del_legame"> <div class="vector-toc-text"> <span class="vector-toc-numb">2</span> <span>Formazione del legame</span> </div> </a> <ul id="toc-Formazione_del_legame-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Definire_il_legame" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Definire_il_legame"> <div class="vector-toc-text"> <span class="vector-toc-numb">3</span> <span>Definire il legame</span> </div> </a> <ul id="toc-Definire_il_legame-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Forma_e_struttura_del_legame" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Forma_e_struttura_del_legame"> <div class="vector-toc-text"> <span class="vector-toc-numb">4</span> <span>Forma e struttura del legame</span> </div> </a> <ul id="toc-Forma_e_struttura_del_legame-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Biochimica" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Biochimica"> <div class="vector-toc-text"> <span class="vector-toc-numb">5</span> <span>Biochimica</span> </div> </a> <ul id="toc-Biochimica-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Note" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Note"> <div class="vector-toc-text"> <span class="vector-toc-numb">6</span> <span>Note</span> </div> </a> <ul id="toc-Note-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Bibliografia" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Bibliografia"> <div class="vector-toc-text"> <span class="vector-toc-numb">7</span> <span>Bibliografia</span> </div> </a> <ul id="toc-Bibliografia-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Voci_correlate" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Voci_correlate"> <div class="vector-toc-text"> <span class="vector-toc-numb">8</span> <span>Voci correlate</span> </div> </a> <ul id="toc-Voci_correlate-sublist" class="vector-toc-list"> </ul> </li> <li id="toc-Collegamenti_esterni" class="vector-toc-list-item vector-toc-level-1 vector-toc-list-item-expanded"> <a class="vector-toc-link" href="#Collegamenti_esterni"> <div class="vector-toc-text"> <span class="vector-toc-numb">9</span> <span>Collegamenti esterni</span> </div> </a> <ul id="toc-Collegamenti_esterni-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="Indice" 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="Mostra/Nascondi l'indice" > <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">Mostra/Nascondi l'indice</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">Forza intramolecolare</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="Vai a una voce in un'altra lingua. Disponibile in 13 lingue" > <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-13" 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">13 lingue</span> </label> <div class="vector-dropdown-content"> <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li class="interlanguage-link interwiki-ar mw-list-item"><a href="https://ar.wikipedia.org/wiki/%D9%82%D9%88%D8%A9_%D8%AF%D8%A7%D8%AE%D9%84_%D8%A7%D9%84%D8%AC%D8%B2%D9%8A%D8%A1" title="قوة داخل الجزيء - arabo" lang="ar" hreflang="ar" data-title="قوة داخل الجزيء" data-language-autonym="العربية" data-language-local-name="arabo" class="interlanguage-link-target"><span>العربية</span></a></li><li class="interlanguage-link interwiki-bs mw-list-item"><a href="https://bs.wikipedia.org/wiki/Unutarmolekulska_sila" title="Unutarmolekulska sila - bosniaco" lang="bs" hreflang="bs" data-title="Unutarmolekulska sila" data-language-autonym="Bosanski" data-language-local-name="bosniaco" class="interlanguage-link-target"><span>Bosanski</span></a></li><li class="interlanguage-link interwiki-en mw-list-item"><a href="https://en.wikipedia.org/wiki/Intramolecular_force" title="Intramolecular force - inglese" lang="en" hreflang="en" data-title="Intramolecular force" data-language-autonym="English" data-language-local-name="inglese" class="interlanguage-link-target"><span>English</span></a></li><li class="interlanguage-link interwiki-fa mw-list-item"><a href="https://fa.wikipedia.org/wiki/%D9%86%DB%8C%D8%B1%D9%88%DB%8C_%D8%AF%D8%B1%D9%88%D9%86%E2%80%8C%D9%85%D9%88%D9%84%DA%A9%D9%88%D9%84%DB%8C" title="نیروی درون‌مولکولی - persiano" lang="fa" hreflang="fa" data-title="نیروی درون‌مولکولی" data-language-autonym="فارسی" data-language-local-name="persiano" 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/Force_intramol%C3%A9culaire" title="Force intramoléculaire - francese" lang="fr" hreflang="fr" data-title="Force intramoléculaire" data-language-autonym="Français" data-language-local-name="francese" class="interlanguage-link-target"><span>Français</span></a></li><li class="interlanguage-link interwiki-hi mw-list-item"><a href="https://hi.wikipedia.org/wiki/%E0%A4%85%E0%A4%82%E0%A4%A4%E0%A4%83%E0%A4%85%E0%A4%A3%E0%A5%81%E0%A4%95_%E0%A4%AC%E0%A4%B2" title="अंतःअणुक बल - hindi" lang="hi" hreflang="hi" data-title="अंतःअणुक बल" data-language-autonym="हिन्दी" data-language-local-name="hindi" class="interlanguage-link-target"><span>हिन्दी</span></a></li><li class="interlanguage-link interwiki-nl mw-list-item"><a href="https://nl.wikipedia.org/wiki/Intramoleculaire_krachten" title="Intramoleculaire krachten - olandese" lang="nl" hreflang="nl" data-title="Intramoleculaire krachten" data-language-autonym="Nederlands" data-language-local-name="olandese" class="interlanguage-link-target"><span>Nederlands</span></a></li><li class="interlanguage-link interwiki-pt mw-list-item"><a href="https://pt.wikipedia.org/wiki/For%C3%A7a_intramolecular" title="Força intramolecular - portoghese" lang="pt" hreflang="pt" data-title="Força intramolecular" data-language-autonym="Português" data-language-local-name="portoghese" 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/For%C8%9B%C4%83_intramolecular%C4%83" title="Forță intramoleculară - rumeno" lang="ro" hreflang="ro" data-title="Forță intramoleculară" data-language-autonym="Română" data-language-local-name="rumeno" class="interlanguage-link-target"><span>Română</span></a></li><li class="interlanguage-link interwiki-sh mw-list-item"><a href="https://sh.wikipedia.org/wiki/Intramolekulska_sila" title="Intramolekulska sila - serbo-croato" lang="sh" hreflang="sh" data-title="Intramolekulska sila" data-language-autonym="Srpskohrvatski / српскохрватски" data-language-local-name="serbo-croato" class="interlanguage-link-target"><span>Srpskohrvatski / српскохрватски</span></a></li><li class="interlanguage-link interwiki-sr mw-list-item"><a href="https://sr.wikipedia.org/wiki/Intramolekulska_sila" title="Intramolekulska sila - serbo" lang="sr" hreflang="sr" data-title="Intramolekulska sila" data-language-autonym="Српски / srpski" data-language-local-name="serbo" class="interlanguage-link-target"><span>Српски / srpski</span></a></li><li class="interlanguage-link interwiki-sv mw-list-item"><a href="https://sv.wikipedia.org/wiki/Intramolekyl%C3%A4r_bindning" title="Intramolekylär bindning - svedese" lang="sv" hreflang="sv" data-title="Intramolekylär bindning" data-language-autonym="Svenska" data-language-local-name="svedese" class="interlanguage-link-target"><span>Svenska</span></a></li><li class="interlanguage-link interwiki-zh mw-list-item"><a href="https://zh.wikipedia.org/wiki/%E5%88%86%E5%AD%90%E5%86%85%E4%BD%9C%E7%94%A8%E5%8A%9B" title="分子内作用力 - cinese" lang="zh" hreflang="zh" data-title="分子内作用力" data-language-autonym="中文" data-language-local-name="cinese" 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 href="https://www.wikidata.org/wiki/Special:EntityPage/Q1571801#sitelinks-wikipedia" title="Modifica collegamenti interlinguistici" class="wbc-editpage">Modifica collegamenti</a></span></div> </div> </div> </div> </header> <div class="vector-page-toolbar"> <div class="vector-page-toolbar-container"> <div id="left-navigation"> <nav aria-label="Namespace"> <div id="p-associated-pages" class="vector-menu vector-menu-tabs mw-portlet mw-portlet-associated-pages" > <div 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class="vector-more-collapsible-item mw-list-item"><a href="/w/index.php?title=Forza_intramolecolare&action=history"><span>Cronologia</span></a></li> </ul> </div> </div> <div id="p-tb" class="vector-menu mw-portlet mw-portlet-tb" > <div class="vector-menu-heading"> Generale </div> <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li id="t-whatlinkshere" class="mw-list-item"><a href="/wiki/Speciale:PuntanoQui/Forza_intramolecolare" title="Elenco di tutte le pagine che sono collegate a questa [j]" accesskey="j"><span>Puntano qui</span></a></li><li id="t-recentchangeslinked" class="mw-list-item"><a href="/wiki/Speciale:ModificheCorrelate/Forza_intramolecolare" rel="nofollow" title="Elenco delle ultime modifiche alle pagine collegate a questa [k]" accesskey="k"><span>Modifiche correlate</span></a></li><li id="t-specialpages" class="mw-list-item"><a href="/wiki/Speciale:PagineSpeciali" title="Elenco di tutte le pagine speciali [q]" accesskey="q"><span>Pagine 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href="/w/index.php?title=Speciale:QrCode&url=https%3A%2F%2Fit.wikipedia.org%2Fwiki%2FForza_intramolecolare"><span>Scarica codice QR</span></a></li> </ul> </div> </div> <div id="p-coll-print_export" class="vector-menu mw-portlet mw-portlet-coll-print_export" > <div class="vector-menu-heading"> Stampa/esporta </div> <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li id="coll-create_a_book" class="mw-list-item"><a href="/w/index.php?title=Speciale:Libro&bookcmd=book_creator&referer=Forza+intramolecolare"><span>Crea un libro</span></a></li><li id="coll-download-as-rl" class="mw-list-item"><a href="/w/index.php?title=Speciale:DownloadAsPdf&page=Forza_intramolecolare&action=show-download-screen"><span>Scarica come PDF</span></a></li><li id="t-print" class="mw-list-item"><a href="/w/index.php?title=Forza_intramolecolare&printable=yes" title="Versione stampabile di questa pagina [p]" accesskey="p"><span>Versione stampabile</span></a></li> </ul> </div> </div> <div id="p-wikibase-otherprojects" class="vector-menu mw-portlet mw-portlet-wikibase-otherprojects" > <div class="vector-menu-heading"> In altri progetti </div> <div class="vector-menu-content"> <ul class="vector-menu-content-list"> <li id="t-wikibase" class="wb-otherproject-link wb-otherproject-wikibase-dataitem mw-list-item"><a href="https://www.wikidata.org/wiki/Special:EntityPage/Q1571801" title="Collegamento all'elemento connesso dell'archivio dati [g]" accesskey="g"><span>Elemento Wikidata</span></a></li> </ul> </div> </div> </div> </div> </div> </div> </nav> </div> </div> </div> <div class="vector-column-end"> <div class="vector-sticky-pinned-container"> <nav class="vector-page-tools-landmark" aria-label="Strumenti pagine"> <div id="vector-page-tools-pinned-container" class="vector-pinned-container"> </div> </nav> <nav class="vector-appearance-landmark" aria-label="Aspetto"> <div id="vector-appearance-pinned-container" class="vector-pinned-container"> <div id="vector-appearance" class="vector-appearance vector-pinnable-element"> <div class="vector-pinnable-header vector-appearance-pinnable-header vector-pinnable-header-pinned" data-feature-name="appearance-pinned" data-pinnable-element-id="vector-appearance" data-pinned-container-id="vector-appearance-pinned-container" data-unpinned-container-id="vector-appearance-unpinned-container" > <div class="vector-pinnable-header-label">Aspetto</div> <button class="vector-pinnable-header-toggle-button vector-pinnable-header-pin-button" data-event-name="pinnable-header.vector-appearance.pin">sposta nella barra laterale</button> <button class="vector-pinnable-header-toggle-button vector-pinnable-header-unpin-button" data-event-name="pinnable-header.vector-appearance.unpin">nascondi</button> </div> </div> </div> </nav> </div> </div> <div id="bodyContent" class="vector-body" aria-labelledby="firstHeading" data-mw-ve-target-container> <div class="vector-body-before-content"> <div class="mw-indicators"> </div> <div id="siteSub" class="noprint">Da Wikipedia, l'enciclopedia libera.</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="it" dir="ltr"><p>Una <b>forza intramolecolare</b> è una forza che mantiene assieme gli <a href="/wiki/Atomo" title="Atomo">atomi</a> formando <a href="/wiki/Molecola" title="Molecola">molecole</a> o <a href="/wiki/Composto_chimico" title="Composto chimico">composti</a>, da non confondere con la forza intermolecolare, che è presente tra le molecole e non tra gli atomi.<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> La differenza nel nome deriva dalla radice latina, sia "inter" che "intra" possono essere tradotti con "tra" con la differenza che "inter" viene usato per indicare l'esterno mentre "intra" l'interno.<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> Queste forze sono spesso più forti delle <a href="/wiki/Forze_intermolecolari" class="mw-redirect" title="Forze intermolecolari">forze intermolecolari</a>, che sono presenti tra atomi o molecole che non sono legate. </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Tipi">Tipi</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=1" title="Modifica la sezione Tipi" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=1" title="Edit section's source code: Tipi"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>Il modello classico vede tre principali tipi di legami chimici - ionico, covalente e metallico - differenti per il grado di separazione delle cariche tra gli atomi coinvolti. Le caratteristiche di un legame si possono prevedere dalle proprietà degli atomi costituenti, in particolare dall’elettronegatività. Essi si distinguono per il valore delle loro entalpie di legame, una misura della forza di legame, e questo caratterizza le proprietà chimiche e fisiche dei composti in vari modi. La percentuale di carattere ionico è direttamente proporzionale alla differenza di elettronegatività degli atomi di legame.<sup id="cite_ref-:1_3-0" class="reference"><a href="#cite_note-:1-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> </p> <div class="mw-heading mw-heading3"><h3 id="Legame_ionico">Legame ionico</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=2" title="Modifica la sezione Legame ionico" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=2" title="Edit section's source code: Legame ionico"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:IonicBondingRH11.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/0/0c/IonicBondingRH11.png/170px-IonicBondingRH11.png" decoding="async" width="170" height="154" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/0/0c/IonicBondingRH11.png/255px-IonicBondingRH11.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/0/0c/IonicBondingRH11.png/340px-IonicBondingRH11.png 2x" data-file-width="702" data-file-height="634" /></a><figcaption>Legame ionico tra sodio e cloro.</figcaption></figure> <p>Un <a href="/wiki/Legame_ionico" title="Legame ionico">legame ionico</a> consiste in un completo trasferimento di uno o più <a href="/wiki/Elettroni_di_valenza" class="mw-redirect" title="Elettroni di valenza">elettroni di valenza</a> verso gli atomi coinvolti nel processo, dando origine ad un <a href="/wiki/Catione" title="Catione">catione</a> (ione positivo) o ad un <a href="/wiki/Anione" title="Anione">anione</a> (ione negativo) mantenuti assieme dalla <a href="/wiki/Forza_elettrostatica" class="mw-redirect" title="Forza elettrostatica">forza elettrostatica</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> Gli elettroni nel legame ionico tendono ad essere trovati principalmente attorno ad uno o due atomi costituenti a causa della elevata differenza di <a href="/wiki/Elettronegativit%C3%A0" title="Elettronegatività">elettronegatività</a> tra gli atomi stessi (elevata elettronegatività è conseguenza di legami più forti); spesso è descritto come il processo di cessione di un elettrone verso un atomo. Questo tipo di legame generalmente si forma tra <a href="/wiki/Metallo" title="Metallo">metalli</a> e <a href="/wiki/Non_metallo" title="Non metallo">non-metalli</a>, come <a href="/wiki/Sodio" title="Sodio">sodio</a> e <a href="/wiki/Cloro" title="Cloro">cloro</a> nella formazione del <a href="/wiki/Cloruro_di_sodio" title="Cloruro di sodio">cloruro di sodio</a> (<span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle NaCl}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>N</mi> <mi>a</mi> <mi>C</mi> <mi>l</mi> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle NaCl}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/5ecad937cdb19eec2d35925f4231126038161082" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:5.753ex; height:2.176ex;" alt="{\displaystyle NaCl}"></span>). In tale processo il sodio (elemento a bassa energia di ionizzazione) cede un elettrone, trasformandosi in un catione (<span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle Na^{+}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>N</mi> <msup> <mi>a</mi> <mrow class="MJX-TeXAtom-ORD"> <mo>+</mo> </mrow> </msup> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle Na^{+}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/447edc65f655d69f851a0b501b7708b8f8b0c14e" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:4.804ex; height:2.509ex;" alt="{\displaystyle Na^{+}}"></span>), mentre il cloro (elemento ad alta affinità elettronica), ottenendo l'elettrone, assume carica negativa diventando un anione (<span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle Cl^{-}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>C</mi> <msup> <mi>l</mi> <mrow class="MJX-TeXAtom-ORD"> <mo>−</mo> </mrow> </msup> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle Cl^{-}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/5d5ca81893589d2837e9fab67bc3d2df1ac93842" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:3.97ex; height:2.509ex;" alt="{\displaystyle Cl^{-}}"></span>). Per il naturale bilanciamento delle cariche, il legame può essere definito come pura attrazione coulombiana tra cariche di segno opposto, formando il cloruro di sodio (<span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle NaCl}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi>N</mi> <mi>a</mi> <mi>C</mi> <mi>l</mi> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle NaCl}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/5ecad937cdb19eec2d35925f4231126038161082" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:5.753ex; height:2.176ex;" alt="{\displaystyle NaCl}"></span>).<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> </p> <div class="mw-heading mw-heading3"><h3 id="Legame_covalente">Legame covalente</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=3" title="Modifica la sezione Legame covalente" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=3" title="Edit section's source code: Legame covalente"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Ball_and_stick_model_of_a_water_molecule.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/4/4e/Ball_and_stick_model_of_a_water_molecule.png/170px-Ball_and_stick_model_of_a_water_molecule.png" decoding="async" width="170" height="149" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/4/4e/Ball_and_stick_model_of_a_water_molecule.png/255px-Ball_and_stick_model_of_a_water_molecule.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/4/4e/Ball_and_stick_model_of_a_water_molecule.png/340px-Ball_and_stick_model_of_a_water_molecule.png 2x" data-file-width="1078" data-file-height="942" /></a><figcaption>Questo è un modello palla-bastone di una molecola d'acqua. Ha un dipolo permanente che punta verso il lato in basso a sinistra.</figcaption></figure> <p>In un vero <a href="/wiki/Legame_covalente" title="Legame covalente">legame covalente</a>, gli elettroni sono condivisi in modo uniforme tra i due atomi del legame con poca o scarsa separazione di carica. I legami covalenti sono generalmente formati tra due non-metalli. Esistono diversi tipi di legami covalenti: nei <a href="/wiki/Legame_covalente#Tipologia_di_legami_covalenti" title="Legame covalente">legami covalenti polari</a>, è più probabile che gli elettroni si trovino intorno a uno dei due atomi, mentre nei legami covalenti non polari, gli elettroni sono equamente condivisi. Le molecole biatomiche omonucleari sono puramente covalenti. La polarità di un legame covalente è determinata dalle elettronegatività di ciascun atomo e quindi un legame covalente polare ha un momento di dipolo che punta dall'estremità parziale positiva a quella parziale negativa.<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> I legami covalenti polari rappresentano un tipo intermedio in cui gli elettroni non sono né completamente trasferiti da un atomo all'altro né condivisi in modo uniforme. </p> <div class="mw-heading mw-heading3"><h3 id="Legame_metallico">Legame metallico</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=4" title="Modifica la sezione Legame metallico" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=4" title="Edit section's source code: Legame metallico"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>I <a href="/w/index.php?title=Legami_metallici&action=edit&redlink=1" class="new" title="Legami metallici (la pagina non esiste)">legami metallici</a> generalmente si formano all'interno di un <a href="/wiki/Metallo" title="Metallo">metallo puro</a> o di una <a href="/wiki/Lega_metallica" class="mw-redirect" title="Lega metallica">lega metallica</a>. Gli elettroni metallici sono generalmente delocalizzati; il risultato è un gran numero di elettroni liberi attorno a nuclei positivi, a volte chiamato mare elettronico. </p> <div class="mw-heading mw-heading2"><h2 id="Formazione_del_legame">Formazione del legame</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=5" title="Modifica la sezione Formazione del legame" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=5" title="Edit section's source code: Formazione del legame"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="thumb tleft"><div class="thumbinner" style="width:150px;"><figure class="mw-halign-right" typeof="mw:File"><a href="/wiki/File:Carbon-dioxide-2D-dimensions.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/1/1f/Carbon-dioxide-2D-dimensions.svg/150px-Carbon-dioxide-2D-dimensions.svg.png" decoding="async" width="150" height="67" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/1/1f/Carbon-dioxide-2D-dimensions.svg/225px-Carbon-dioxide-2D-dimensions.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/1/1f/Carbon-dioxide-2D-dimensions.svg/300px-Carbon-dioxide-2D-dimensions.svg.png 2x" data-file-width="740" data-file-height="330" /></a><figcaption></figcaption></figure> <figure class="mw-halign-right" typeof="mw:File"><a href="/wiki/File:Carbon_monoxide_2D.svg" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/5/57/Carbon_monoxide_2D.svg/80px-Carbon_monoxide_2D.svg.png" decoding="async" width="80" height="42" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/5/57/Carbon_monoxide_2D.svg/120px-Carbon_monoxide_2D.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/5/57/Carbon_monoxide_2D.svg/160px-Carbon_monoxide_2D.svg.png 2x" data-file-width="850" data-file-height="450" /></a><figcaption></figcaption></figure> <div style="clear:both;"></div> <div class="thumbcaption">Confronto delle lunghezze dei legami tra carbonio e ossigeno in un legame doppio e triplo.</div> </div> </div> <p>Gli atomi formano legami in modo che siano in grado di raggiungere uno stato energetico inferiore. Gli atomi liberi avrebbero più energia di un atomo legato, in quanto, durante la formazione del legame si libera <a href="/wiki/Energia" title="Energia">energia</a>, consentendo all'intero sistema di raggiungere uno stato energetico inferiore. La lunghezza del legame, o la distanza minima di separazione tra due atomi che partecipano alla formazione del legame, è determinata dalle loro forze repulsive e attrattive lungo la direzione internucleare.<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> Man mano che i due atomi si avvicinano sempre di più, i <a href="/wiki/Nucleo_atomico" title="Nucleo atomico">nuclei</a> caricati positivamente si respingono, creando una forza che tenta di allontanare gli atomi. Mentre i due atomi si allontanano, le forze attrattive lavorano per rimetterli insieme. In questo modo si ottiene una lunghezza del legame di equilibrio ed è una buona misura della stabilità del legame. </p> <div class="mw-heading mw-heading2"><h2 id="Definire_il_legame">Definire il legame</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=6" title="Modifica la sezione Definire il legame" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=6" title="Edit section's source code: Definire il legame"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>È possibile difinire matematicamente il tipo di legame che si viene a formare tra due atomi sulla base dell'elettronegatività caratteristica dell'atomo, dato presente in ogni tavola periodica. Chiamato <span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle E_{a}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <msub> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>a</mi> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle E_{a}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/46a5c4699f75d498b504e59bfd8b5496aa20351a" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:2.817ex; height:2.509ex;" alt="{\displaystyle E_{a}}"></span>l'elettronegatività del primo atomo ed <span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle E_{b}}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <msub> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>b</mi> </mrow> </msub> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle E_{b}}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/69d2e3ccd9bce33b1ae1562c2e7e831eb8f55bf3" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.671ex; width:2.653ex; height:2.509ex;" alt="{\displaystyle E_{b}}"></span>quella del secondo, il tipo di legame è definito dalla <a href="/wiki/Sottrazione" title="Sottrazione">differenza</a> in <a href="/wiki/Modulo_(algebra)" title="Modulo (algebra)">modulo</a> di tali valori<sup id="cite_ref-:0_8-0" class="reference"><a href="#cite_note-:0-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup> </p><p><span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle \Delta e=\mid E_{a}-E_{b}\mid }"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi mathvariant="normal">Δ</mi> <mi>e</mi> <mo>=∣</mo> <msub> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>a</mi> </mrow> </msub> <mo>−</mo> <msub> <mi>E</mi> <mrow class="MJX-TeXAtom-ORD"> <mi>b</mi> </mrow> </msub> <mo stretchy="false">∣</mo> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \Delta e=\mid E_{a}-E_{b}\mid }</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/226931e777118acc86f9c3e169995ce814e94e26" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.838ex; width:15.722ex; height:2.843ex;" alt="{\displaystyle \Delta e=\mid E_{a}-E_{b}\mid }"></span> </p><p>In particolare se: </p> <ul><li><span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle \Delta e<0.9}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi mathvariant="normal">Δ</mi> <mi>e</mi> <mo><</mo> <mn>0.9</mn> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \Delta e<0.9}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/7c6057a863d103c713f96e6a90ff4532d354b5f4" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:9.09ex; height:2.176ex;" alt="{\displaystyle \Delta e<0.9}"></span> il legame è covalente puro</li> <li><span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle 0.9\leq \Delta e\leq 1.9}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mn>0.9</mn> <mo>≤</mo> <mi mathvariant="normal">Δ</mi> <mi>e</mi> <mo>≤</mo> <mn>1.9</mn> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle 0.9\leq \Delta e\leq 1.9}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/e9b69b1b6df09ee299b1410f9776777a147ad092" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.505ex; width:15.16ex; height:2.343ex;" alt="{\displaystyle 0.9\leq \Delta e\leq 1.9}"></span> il legame è covalente polare</li> <li><span class="mwe-math-element"><span class="mwe-math-mathml-inline mwe-math-mathml-a11y" style="display: none;"><math xmlns="http://www.w3.org/1998/Math/MathML" alttext="{\displaystyle \Delta e>1.9}"> <semantics> <mrow class="MJX-TeXAtom-ORD"> <mstyle displaystyle="true" scriptlevel="0"> <mi mathvariant="normal">Δ</mi> <mi>e</mi> <mo>></mo> <mn>1.9</mn> </mstyle> </mrow> <annotation encoding="application/x-tex">{\displaystyle \Delta e>1.9}</annotation> </semantics> </math></span><img src="https://wikimedia.org/api/rest_v1/media/math/render/svg/fe074390aa01d93785373a3b39c047d5807212da" class="mwe-math-fallback-image-inline mw-invert skin-invert" aria-hidden="true" style="vertical-align: -0.338ex; width:9.09ex; height:2.176ex;" alt="{\displaystyle \Delta e>1.9}"></span> il legame è ionico</li></ul> <div class="mw-heading mw-heading2"><h2 id="Forma_e_struttura_del_legame">Forma e struttura del legame</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=7" title="Modifica la sezione Forma e struttura del legame" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=7" title="Edit section's source code: Forma e struttura del legame"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r130657691">body:not(.skin-minerva) .mw-parser-output .vedi-anche{font-size:95%}</style><style data-mw-deduplicate="TemplateStyles:r139142988">.mw-parser-output .hatnote-content{align-items:center;display:flex}.mw-parser-output .hatnote-icon{flex-shrink:0}.mw-parser-output .hatnote-icon img{display:flex}.mw-parser-output .hatnote-text{font-style:italic}body:not(.skin-minerva) .mw-parser-output .hatnote{border:1px solid #CCC;display:flex;margin:.5em 0;padding:.2em .5em}body:not(.skin-minerva) .mw-parser-output .hatnote-text{padding-left:.5em}body.skin-minerva .mw-parser-output .hatnote-icon{padding-right:8px}body.skin-minerva .mw-parser-output .hatnote-icon img{height:auto;width:16px}body.skin--responsive .mw-parser-output .hatnote a.new{color:#d73333}body.skin--responsive .mw-parser-output .hatnote a.new:visited{color:#a55858}</style> <div class="hatnote noprint vedi-anche"> <div class="hatnote-content"><span class="noviewer hatnote-icon" typeof="mw:File"><span><img src="//upload.wikimedia.org/wikipedia/commons/thumb/8/87/Magnifying_glass_icon_mgx2.svg/18px-Magnifying_glass_icon_mgx2.svg.png" decoding="async" width="18" height="18" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/87/Magnifying_glass_icon_mgx2.svg/27px-Magnifying_glass_icon_mgx2.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/87/Magnifying_glass_icon_mgx2.svg/36px-Magnifying_glass_icon_mgx2.svg.png 2x" data-file-width="286" data-file-height="280" /></span></span> <span class="hatnote-text">Lo stesso argomento in dettaglio: <b><a href="/wiki/Teoria_VSEPR" title="Teoria VSEPR">Teoria VSEPR</a></b>.</span></div> </div> <p>Nella formazione di un legame la disposizione degli atomi che formano la molecola non è casuale. In particolare, con la formazione di un legame covalente (sia esso puro o polare), ciò che conferisce alla molecola determinate proprietà è l'<a href="/wiki/Angolo_di_legame" title="Angolo di legame">angolo di legame</a>, ovvero l'angolo che si forma tra gli assi congiungenti i nuclei degli atomi legati tra loro. Tale angolo presenta rapporti matematici precisi studiati ed esposti nella <a href="/wiki/Teoria_VSEPR" title="Teoria VSEPR">teoria VSEPR</a> (<i>Valence Shell Electron-Pair Repulsion</i>) che studia quindi la struttura del legame sulla base delle forze repulsive tra gli elettroni del guscio di valenza.<sup id="cite_ref-:0_8-1" class="reference"><a href="#cite_note-:0-8"><span class="cite-bracket">[</span>8<span class="cite-bracket">]</span></a></sup><sup id="cite_ref-:1_3-1" class="reference"><a href="#cite_note-:1-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> </p><p>Secondo tale teoria, avendo gli elettroni segno concorde, sviluppano un comportamento repulsivo tra loro, maggiore nel caso di elettroni liberi e minore tra quelli condivisi in legame, ma sempre minore dell'<a href="/wiki/Energia_di_legame" title="Energia di legame">energia di legame</a>. Nel dettaglio, nel caso di due coppie l'angolo è di 180°, tre coppie determinano un assetto triangolare equilatero con angoli di 120° mentre quattro coppie formano una struttura tetraedrica con angoli di 109,5°; legami doppi o tripli valgono come un singolo legame nella determinazione dell'angolo di legame.<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-halign-center" typeof="mw:File"><a href="/wiki/File:Principali_strutture_molecolari_VESPR.png" class="mw-file-description"><img src="//upload.wikimedia.org/wikipedia/commons/thumb/c/c9/Principali_strutture_molecolari_VESPR.png/800px-Principali_strutture_molecolari_VESPR.png" decoding="async" width="800" height="224" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/c/c9/Principali_strutture_molecolari_VESPR.png/1200px-Principali_strutture_molecolari_VESPR.png 1.5x, //upload.wikimedia.org/wikipedia/commons/c/c9/Principali_strutture_molecolari_VESPR.png 2x" data-file-width="1254" data-file-height="351" /></a><figcaption></figcaption></figure> <div class="mw-heading mw-heading2"><h2 id="Biochimica">Biochimica</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=8" title="Modifica la sezione Biochimica" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=8" title="Edit section's source code: Biochimica"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r130657691"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r139142988"> <div class="hatnote noprint vedi-anche"> <div class="hatnote-content"><span class="noviewer hatnote-icon" typeof="mw:File"><span><img src="//upload.wikimedia.org/wikipedia/commons/thumb/8/87/Magnifying_glass_icon_mgx2.svg/18px-Magnifying_glass_icon_mgx2.svg.png" decoding="async" width="18" height="18" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/8/87/Magnifying_glass_icon_mgx2.svg/27px-Magnifying_glass_icon_mgx2.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/8/87/Magnifying_glass_icon_mgx2.svg/36px-Magnifying_glass_icon_mgx2.svg.png 2x" data-file-width="286" data-file-height="280" /></span></span> <span class="hatnote-text">Lo stesso argomento in dettaglio: <b><a href="/wiki/Biochimica" title="Biochimica">Biochimica</a></b>.</span></div> </div><figure class="mw-default-size" typeof="mw:File/Thumb"><a href="https://en.wikipedia.org/wiki/File:Alpha_Helix_Ribbon.svg"><img resource="/wiki/File:Alpha_Helix_Ribbon.svg" src="//upload.wikimedia.org/wikipedia/commons/thumb/d/d2/Alpha_Helix_Ribbon.svg/170px-Alpha_Helix_Ribbon.svg.png" decoding="async" width="170" height="469" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/commons/thumb/d/d2/Alpha_Helix_Ribbon.svg/255px-Alpha_Helix_Ribbon.svg.png 1.5x, //upload.wikimedia.org/wikipedia/commons/thumb/d/d2/Alpha_Helix_Ribbon.svg/340px-Alpha_Helix_Ribbon.svg.png 2x" data-file-width="304" data-file-height="839" /></a><figcaption>La struttura alfa-elica necessaria per la stabilità del DNA è tenuta insieme dalle forze elettrostatiche intramolecolari nella proteina.</figcaption></figure> <p>Le forze intramolecolari sono estremamente importanti nel campo della biochimica, dove giocano un ruolo importante nella struttura base di strutture biologiche. Le forze intramolecolari come legami disolfuro determinano la struttura di proteine e <a href="/wiki/DNA" title="DNA">DNA</a>. La struttura delle <a href="/wiki/Proteine" title="Proteine">Proteine</a> deriva dalle forze intramolecolari che le formano e le tengono insieme. La principale fonte di struttura in queste molecole è l'interazione tra i residui di <a href="/wiki/Amminoacido" title="Amminoacido">amminoacidi</a> nella formazione delle <a href="/wiki/Proteine" title="Proteine">proteine</a>.<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> Le interazioni tra i residui delle stesse proteine formano la struttura secondaria della proteina, consentendo la formazione di strutture <a href="/wiki/Foglietto_%CE%B2" title="Foglietto β">beta-foglietto</a> e <a href="/wiki/Alfa_elica" title="Alfa elica">alfa-elica</a>, strutture di fondamentale importanza per le proteine e, nel caso di alfa-eliche, per il DNA. </p> <div class="mw-heading mw-heading2"><h2 id="Note">Note</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=9" title="Modifica la sezione Note" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=9" title="Edit section's source code: Note"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <div class="mw-references-wrap"><ol class="references"> <li id="cite_note-1"><a href="#cite_ref-1"><b>^</b></a> <span class="reference-text"><cite class="citation libro" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) Steven S. Zumdahl e Susan A. Zumdahl, <span style="font-style:italic;">Chemistry</span>, 7th, Boston, Houghton Mifflin, 2007, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-0-618-71370-7" title="Speciale:RicercaISBN/978-0-618-71370-7">978-0-618-71370-7</a>, <a href="/wiki/Online_Computer_Library_Center" title="Online Computer Library Center">OCLC</a> <a rel="nofollow" class="external text" href="//www.worldcat.org/oclc/85824942">85824942</a>.</cite></span> </li> <li id="cite_note-2"><a href="#cite_ref-2"><b>^</b></a> <span class="reference-text"><cite class="citation web" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) <a rel="nofollow" class="external text" href="https://www.grammar.com/inter_vs._intra"><span style="font-style:italic;">Inter vs. Intra</span></a>, su <span style="font-style:italic;">grammar.com</span>. <small>URL consultato il 26 aprile 2018</small>.</cite></span> </li> <li id="cite_note-:1-3"><span class="mw-cite-backlink"><b>^</b> <sup><i><a href="#cite_ref-:1_3-0">a</a></i></sup> <sup><i><a href="#cite_ref-:1_3-1">b</a></i></sup></span> <span class="reference-text"><cite class="citation libro" style="font-style:normal"> Petrucci, Herring, Maduria, Bissonnette, <span style="font-style:italic;">cap. 10</span>, in <span style="font-style:italic;">Chimica Generale, Principi ed applicazioni moderne</span>, 10ª ed., Piccin, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-88-299-2692-3" title="Speciale:RicercaISBN/978-88-299-2692-3">978-88-299-2692-3</a>.</cite></span> </li> <li id="cite_note-4"><a href="#cite_ref-4"><b>^</b></a> <span class="reference-text"><cite class="citation pubblicazione" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) R. F. W. Bader e W. H. Henneker, <a rel="nofollow" class="external text" href="https://oadoi.org/10.1021/ja01092a008"><span style="font-style:italic;">The Ionic Bond</span></a>, in <span style="font-style:italic;">Journal of the American Chemical Society</span>, vol. 87, n. 14, 1965, pp. 3063–3068, <a href="/wiki/Digital_object_identifier" title="Digital object identifier">DOI</a>:<a rel="nofollow" class="external text" href="https://dx.doi.org/10.1021%2Fja01092a008">10.1021/ja01092a008</a>.</cite></span> </li> <li id="cite_note-5"><a href="#cite_ref-5"><b>^</b></a> <span class="reference-text"><cite class="citation web" style="font-style:normal"> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20190517181932/http://venus.unive.it/miche/chimrestau/capitoli/05-2re.htm"><span style="font-style:italic;">Venus Unive - Legame ionico</span></a>, su <span style="font-style:italic;">venus.unive.it</span>. <small>URL consultato il 14 maggio 2019</small> <small>(archiviato dall'<abbr title="http://venus.unive.it/miche/chimrestau/capitoli/05-2re.htm">url originale</abbr> il 17 maggio 2019)</small>.</cite></span> </li> <li id="cite_note-6"><a href="#cite_ref-6"><b>^</b></a> <span class="reference-text"><cite class="citation web" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) Anne Marie Helmenstine, Ph D. Dr Helmenstine holds a Ph D. in biomedical sciences, Is a Science Writer, educator, consultant She has taught science courses at the high school, college, <a rel="nofollow" class="external text" href="https://www.thoughtco.com/definition-of-covalent-bond-604414"><span style="font-style:italic;">A Covalent Bond in Chemistry Is a Link Between Two Atoms or Ions</span></a>, su <span style="font-style:italic;">ThoughtCo</span>. <small>URL consultato il 15 maggio 2019</small>.</cite></span> </li> <li id="cite_note-7"><a href="#cite_ref-7"><b>^</b></a> <span class="reference-text"><cite class="citation libro" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) Oxtoby, David W. e Campion, Alan., <a rel="nofollow" class="external text" href="https://www.worldcat.org/oclc/663950016"><span style="font-style:italic;">Principles of modern chemistry</span></a>, 7th ed, Brooks/Cole Cengage Learning, 2012, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-0-8400-4931-5" title="Speciale:RicercaISBN/978-0-8400-4931-5">978-0-8400-4931-5</a>, <a href="/wiki/Online_Computer_Library_Center" title="Online Computer Library Center">OCLC</a> <a rel="nofollow" class="external text" href="//www.worldcat.org/oclc/663950016">663950016</a>.</cite></span> </li> <li id="cite_note-:0-8"><span class="mw-cite-backlink"><b>^</b> <sup><i><a href="#cite_ref-:0_8-0">a</a></i></sup> <sup><i><a href="#cite_ref-:0_8-1">b</a></i></sup></span> <span class="reference-text"><cite class="citation libro" style="font-style:normal"> Valitutti, Falasca, Tifi, Gentile, <span style="font-style:italic;">Chimica, concetti e modelli.blu : volume unico con videolab</span>, Zanichelli, 2014, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-88-08-83547-5" title="Speciale:RicercaISBN/978-88-08-83547-5">978-88-08-83547-5</a>, <a href="/wiki/Online_Computer_Library_Center" title="Online Computer Library Center">OCLC</a> <a rel="nofollow" class="external text" href="//www.worldcat.org/oclc/963878223">963878223</a>.</cite></span> </li> <li id="cite_note-9"><a href="#cite_ref-9"><b>^</b></a> <span class="reference-text"><cite class="citation web" style="font-style:normal"> Valeria Costantino, <a rel="nofollow" class="external text" href="http://www.federica.unina.it/farmacia/chimica-generale-ed-inorganica-far/strutture-di-risonanza-teoria-vsepr/"><span style="font-style:italic;">Strutture di risonanza. Teoria VSEPR</span></a>, su <span style="font-style:italic;">federica.unina.it</span>, pp. 33-35. <small>URL consultato il 6 maggio 2019</small>.</cite></span> </li> <li id="cite_note-10"><a href="#cite_ref-10"><b>^</b></a> <span class="reference-text"><cite class="citation libro" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) David L. Nelson, Michael M. Cox e Albert L. Lehninger, <a rel="nofollow" class="external text" href="https://archive.org/details/lehningerprincip0000lehn"><span style="font-style:italic;">Lehninger principles of biochemistry</span></a>, 6th, New York, W.H. Freeman and Company, 2013, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-1-4292-3414-6" title="Speciale:RicercaISBN/978-1-4292-3414-6">978-1-4292-3414-6</a>, <a href="/wiki/Online_Computer_Library_Center" title="Online Computer Library Center">OCLC</a> <a rel="nofollow" class="external text" href="//www.worldcat.org/oclc/824794893">824794893</a>.</cite></span> </li> </ol></div> <div class="mw-heading mw-heading2"><h2 id="Bibliografia">Bibliografia</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=10" title="Modifica la sezione Bibliografia" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=10" title="Edit section's source code: Bibliografia"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><cite class="citation libro" style="font-style:normal"> Valitutti, Falasca, Tifi, Gentile, <span style="font-style:italic;">Chimica concetti e modelli.blu</span>, 2014, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-88-08-83547-5" title="Speciale:RicercaISBN/978-88-08-83547-5">978-88-08-83547-5</a>.</cite></li> <li><cite class="citation libro" style="font-style:normal"> Petrucci, Herring, Maduria, Bissonnette, <span style="font-style:italic;">Chimica Generale, Principi ed applicazioni moderne</span>, 10ª ed., Piccin, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-88-299-2692-3" title="Speciale:RicercaISBN/978-88-299-2692-3">978-88-299-2692-3</a>.</cite></li> <li><cite class="citation libro" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) Steven S. Zumdahl e Susan A. Zumdahl, <span style="font-style:italic;">Chemistry</span>, 7th, Boston, Houghton Mifflin, 2007, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-0-618-71370-7" title="Speciale:RicercaISBN/978-0-618-71370-7">978-0-618-71370-7</a>, <a href="/wiki/Online_Computer_Library_Center" title="Online Computer Library Center">OCLC</a> <a rel="nofollow" class="external text" href="//www.worldcat.org/oclc/85824942">85824942</a>.</cite></li> <li><cite class="citation libro" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) Oxtoby, David W. e Campion, Alan., <a rel="nofollow" class="external text" href="https://www.worldcat.org/oclc/663950016"><span style="font-style:italic;">Principles of modern chemistry</span></a>, 7th ed, Brooks/Cole Cengage Learning, 2012, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-0-8400-4931-5" title="Speciale:RicercaISBN/978-0-8400-4931-5">978-0-8400-4931-5</a>, <a href="/wiki/Online_Computer_Library_Center" title="Online Computer Library Center">OCLC</a> <a rel="nofollow" class="external text" href="//www.worldcat.org/oclc/663950016">663950016</a>.</cite></li> <li><cite class="citation libro" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) David L. Nelson, Michael M. Cox e Albert L. Lehninger, <a rel="nofollow" class="external text" href="https://archive.org/details/lehningerprincip0000lehn"><span style="font-style:italic;">Lehninger principles of biochemistry</span></a>, 6th, New York, W.H. Freeman and Company, 2013, <a href="/wiki/ISBN" title="ISBN">ISBN</a> <a href="/wiki/Speciale:RicercaISBN/978-1-4292-3414-6" title="Speciale:RicercaISBN/978-1-4292-3414-6">978-1-4292-3414-6</a>, <a href="/wiki/Online_Computer_Library_Center" title="Online Computer Library Center">OCLC</a> <a rel="nofollow" class="external text" href="//www.worldcat.org/oclc/824794893">824794893</a>.</cite></li></ul> <div class="mw-heading mw-heading2"><h2 id="Voci_correlate">Voci correlate</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=11" title="Modifica la sezione Voci correlate" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=11" title="Edit section's source code: Voci correlate"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><a href="/wiki/Legame_chimico" title="Legame chimico">Legame chimico</a></li> <li><a href="/wiki/Forza_intermolecolare" class="mw-redirect" title="Forza intermolecolare">Forza intermolecolare</a></li></ul> <div class="mw-heading mw-heading2"><h2 id="Collegamenti_esterni">Collegamenti esterni</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Forza_intramolecolare&veaction=edit&section=12" title="Modifica la sezione Collegamenti esterni" class="mw-editsection-visualeditor"><span>modifica</span></a><span class="mw-editsection-divider"> | </span><a href="/w/index.php?title=Forza_intramolecolare&action=edit&section=12" title="Edit section's source code: Collegamenti esterni"><span>modifica wikitesto</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><cite class="citation web" style="font-style:normal"> Valeria Costantino, <a rel="nofollow" class="external text" href="http://www.federica.unina.it/farmacia/chimica-generale-ed-inorganica-far/strutture-di-risonanza-teoria-vsepr/"><span style="font-style:italic;">Strutture di risonanza. Teoria VSEPR</span></a>, su <span style="font-style:italic;">federica.unina.it</span>. <small>URL consultato il 6 maggio 2019</small>.</cite></li> <li><cite class="citation web" style="font-style:normal"> <a rel="nofollow" class="external text" href="https://web.archive.org/web/20190517181932/http://venus.unive.it/miche/chimrestau/capitoli/05-2re.htm"><span style="font-style:italic;">Venus Unive - Legame ionico</span></a>, su <span style="font-style:italic;">venus.unive.it</span>. <small>URL consultato il 14 maggio 2019</small> <small>(archiviato dall'<abbr title="http://venus.unive.it/miche/chimrestau/capitoli/05-2re.htm">url originale</abbr> il 17 maggio 2019)</small>.</cite></li> <li><cite class="citation web" style="font-style:normal">(<span style="font-weight:bolder; font-size:80%"><abbr title="inglese">EN</abbr></span>) Anne Marie Helmenstine, <a rel="nofollow" class="external text" href="https://www.thoughtco.com/definition-of-covalent-bond-604414"><span style="font-style:italic;">A Covalent Bond in Chemistry Is a Link Between Two Atoms or Ions</span></a>, su <span style="font-style:italic;">thoughtco.com</span>. <small>URL consultato il 15 maggio 2019</small>.</cite></li></ul>    </div><noscript><img src="https://login.wikimedia.org/wiki/Special:CentralAutoLogin/start?type=1x1" alt="" width="1" height="1" style="border: none; position: absolute;"></noscript> <div class="printfooter" data-nosnippet="">Estratto da "<a dir="ltr" href="https://it.wikipedia.org/w/index.php?title=Forza_intramolecolare&oldid=134460726">https://it.wikipedia.org/w/index.php?title=Forza_intramolecolare&oldid=134460726</a>"</div></div> <div id="catlinks" class="catlinks" data-mw="interface"><div id="mw-normal-catlinks" class="mw-normal-catlinks"><a href="/wiki/Categoria:Categorie" title="Categoria:Categorie">Categoria</a>: <ul><li><a href="/wiki/Categoria:Ingegneria_dei_materiali" title="Categoria:Ingegneria dei materiali">Ingegneria dei materiali</a></li></ul></div></div> </div> </main> </div> <div class="mw-footer-container"> <footer id="footer" class="mw-footer" > <ul id="footer-info"> <li id="footer-info-lastmod"> Questa pagina è stata modificata per l'ultima volta il 14 lug 2023 alle 04:25.</li> <li id="footer-info-copyright">Il testo è disponibile secondo la <a rel="nofollow" class="external text" href="https://creativecommons.org/licenses/by-sa/4.0/deed.it">licenza Creative Commons Attribuzione-Condividi allo stesso modo</a>; possono applicarsi condizioni ulteriori. 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