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interwiki-bs mw-list-item"><a href="https://bs.wikipedia.org/wiki/Unutarmolekulska_sila" title="Unutarmolekulska sila – Bosnian" lang="bs" hreflang="bs" data-title="Unutarmolekulska sila" data-language-autonym="Bosanski" data-language-local-name="Bosnian" class="interlanguage-link-target"><span>Bosanski</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 – Persian" lang="fa" hreflang="fa" data-title="نیروی درون‌مولکولی" 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/Force_intramol%C3%A9culaire" title="Force intramoléculaire – French" lang="fr" hreflang="fr" data-title="Force intramoléculaire" data-language-autonym="Français" 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src="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/50px-Question_book-new.svg.png" decoding="async" width="50" height="39" class="mw-file-element" srcset="//upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/75px-Question_book-new.svg.png 1.5x, //upload.wikimedia.org/wikipedia/en/thumb/9/99/Question_book-new.svg/100px-Question_book-new.svg.png 2x" data-file-width="512" data-file-height="399" /></a></span></div></td><td class="mbox-text"><div class="mbox-text-span">This article <b>needs additional citations for <a href="/wiki/Wikipedia:Verifiability" title="Wikipedia:Verifiability">verification</a></b>.<span class="hide-when-compact"> Please help <a href="/wiki/Special:EditPage/Intramolecular_force" title="Special:EditPage/Intramolecular force">improve this article</a> by <a href="/wiki/Help:Referencing_for_beginners" title="Help:Referencing for beginners">adding citations to reliable sources</a>. Unsourced material may be challenged and removed.<br /><small><span class="plainlinks"><i>Find sources:</i> <a rel="nofollow" class="external text" href="https://www.google.com/search?as_eq=wikipedia&q=%22Intramolecular+force%22">"Intramolecular force"</a> – <a rel="nofollow" class="external text" href="https://www.google.com/search?tbm=nws&q=%22Intramolecular+force%22+-wikipedia&tbs=ar:1">news</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.google.com/search?&q=%22Intramolecular+force%22&tbs=bkt:s&tbm=bks">newspapers</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.google.com/search?tbs=bks:1&q=%22Intramolecular+force%22+-wikipedia">books</a> <b>·</b> <a rel="nofollow" class="external text" href="https://scholar.google.com/scholar?q=%22Intramolecular+force%22">scholar</a> <b>·</b> <a rel="nofollow" class="external text" href="https://www.jstor.org/action/doBasicSearch?Query=%22Intramolecular+force%22&acc=on&wc=on">JSTOR</a></span></small></span> <span class="date-container"><i>(<span class="date">October 2017</span>)</i></span><span class="hide-when-compact"><i> (<small><a href="/wiki/Help:Maintenance_template_removal" title="Help:Maintenance template removal">Learn how and when to remove this message</a></small>)</i></span></div></td></tr></tbody></table> <p>An <b>intramolecular force</b> (from Latin <i>intra-</i> 'within') is any <a href="/wiki/Force" title="Force">force</a> that binds together the <a href="/wiki/Atom" title="Atom">atoms</a> making up a <a href="/wiki/Molecule" title="Molecule">molecule</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> Intramolecular forces are stronger than the <a href="/wiki/Intermolecular_force" title="Intermolecular force">intermolecular forces</a> that govern the interactions between molecules.<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> </p> <meta property="mw:PageProp/toc" /> <div class="mw-heading mw-heading2"><h2 id="Types">Types</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Intramolecular_force&action=edit&section=1" title="Edit section: Types"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p>The classical model identifies three main types of chemical bonds — ionic, covalent, and metallic — distinguished by the degree of charge separation between participating atoms.<sup id="cite_ref-Principles_of_Modern_Chemistry_3-0" class="reference"><a href="#cite_note-Principles_of_Modern_Chemistry-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> The characteristics of the bond formed can be predicted by the properties of constituent atoms, namely electronegativity. They differ in the magnitude of their <a href="/wiki/Bond-dissociation_energy" title="Bond-dissociation energy">bond enthalpies</a>, a measure of bond strength, and thus affect the physical and chemical properties of compounds in different ways. % of ionic character is directly proportional difference in electronegativity of bonded atom.<sup class="noprint Inline-Template" style="margin-left:0.1em; white-space:nowrap;">[<i><a href="/wiki/Wikipedia:Please_clarify" title="Wikipedia:Please clarify"><span title="The text near this tag may need clarification or removal of jargon. (August 2018)">clarification needed</span></a></i>]</sup> </p> <div class="mw-heading mw-heading3"><h3 id="Ionic_bond">Ionic bond</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Intramolecular_force&action=edit&section=2" title="Edit section: Ionic bond"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File: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>Ionic bonding between sodium and chlorine</figcaption></figure> <p>An <a href="/wiki/Ionic_bond" class="mw-redirect" title="Ionic bond">ionic bond</a> can be approximated as complete transfer of one or more valence electrons of atoms participating in bond formation, resulting in a positive ion and a negative ion bound together by electrostatic forces.<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> Electrons in an ionic bond tend to <a href="/wiki/Atomic_orbital" title="Atomic orbital">be mostly found</a> around one of the two constituent atoms due to the large <a href="/wiki/Electronegativity" title="Electronegativity">electronegativity</a> difference between the two atoms, generally more than 1.9, (greater difference in electronegativity results in a stronger bond); this is often described as one atom giving electrons to the other.<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> This type of bond is generally formed between a <a href="/wiki/Metal" title="Metal">metal</a> and <a href="/wiki/Nonmetal_(chemistry)" class="mw-redirect" title="Nonmetal (chemistry)">nonmetal</a>, such as <a href="/wiki/Sodium" title="Sodium">sodium</a> and <a href="/wiki/Chlorine" title="Chlorine">chlorine</a> in <a href="/wiki/Sodium_chloride" title="Sodium chloride">NaCl</a>. Sodium would give an electron to chlorine, forming a positively charged sodium ion and a negatively charged chloride ion. </p> <div class="mw-heading mw-heading3"><h3 id="Covalent_bond">Covalent bond</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Intramolecular_force&action=edit&section=3" title="Edit section: Covalent bond"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File: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>This is a ball and stick model of a water molecule. It has a permanent dipole pointing to the bottom left hand side.</figcaption></figure> <p>In a true <a href="/wiki/Covalent_bond" title="Covalent bond">covalent bond</a>, the electrons are shared evenly between the two atoms of the bond; there is little or no charge separation. <a href="/wiki/Covalent_bond" title="Covalent bond">Covalent bonds</a> are generally formed between two nonmetals. There are several types of covalent bonds: in <a href="/wiki/Chemical_polarity#Polarity_of_molecules" title="Chemical polarity">polar covalent bonds</a>, electrons are more likely to be found around one of the two atoms, whereas in nonpolar covalent bonds, electrons are evenly shared. <a href="/wiki/Homonuclear_molecule" title="Homonuclear molecule">Homonuclear</a> <a href="/wiki/Diatomic_molecule" title="Diatomic molecule">diatomic molecules</a> are purely covalent. The polarity of a covalent bond is determined by the <a href="/wiki/Electronegativity" title="Electronegativity">electronegativities</a> of each atom and thus a polar covalent bond has a <a href="/wiki/Bond_dipole_moment" class="mw-redirect" title="Bond dipole moment">dipole moment</a> pointing from the partial positive end to the partial negative end.<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> Polar covalent bonds represent an intermediate type in which the electrons are neither completely transferred from one atom to another nor evenly shared. </p> <div class="mw-heading mw-heading3"><h3 id="Metallic_bond">Metallic bond</h3><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Intramolecular_force&action=edit&section=4" title="Edit section: Metallic bond"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <p><a href="/wiki/Metallic_bond" class="mw-redirect" title="Metallic bond">Metallic bonds</a> generally form within a pure metal or metal <a href="/wiki/Alloy" title="Alloy">alloy</a>. Metallic electrons are generally <a href="/wiki/Delocalized_electron" title="Delocalized electron">delocalized</a>; the result is a large number of free electrons around positive <a href="/wiki/Atomic_nucleus" title="Atomic nucleus">nuclei</a>, sometimes called an electron sea. </p> <div class="mw-heading mw-heading2"><h2 id="Bond_formation">Bond formation</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Intramolecular_force&action=edit&section=5" title="Edit section: Bond formation"><span>edit</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;" class=""></div> <div class="thumbcaption">Comparison of the bond lengths between carbon and oxygen in a double and triple bond.</div> </div> </div> <p>Bonds are formed by atoms so that they are able to achieve a lower energy state. Free atoms will have more energy than a bonded atom. This is because some energy is released during bond formation, allowing the entire system to achieve a lower energy state. The bond length, or the minimum separating distance between two atoms participating in bond formation, is determined by their repulsive and attractive forces along the internuclear direction.<sup id="cite_ref-Principles_of_Modern_Chemistry_3-1" class="reference"><a href="#cite_note-Principles_of_Modern_Chemistry-3"><span class="cite-bracket">[</span>3<span class="cite-bracket">]</span></a></sup> As the two atoms get closer and closer, the positively charged nuclei repel, creating a force that attempts to push the atoms apart. As the two atoms get further apart, attractive forces work to pull them back together. Thus an equilibrium bond length is achieved and is a good measure of bond stability. </p> <div class="mw-heading mw-heading2"><h2 id="Biochemistry">Biochemistry</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Intramolecular_force&action=edit&section=6" title="Edit section: Biochemistry"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <figure class="mw-default-size" typeof="mw:File/Thumb"><a href="/wiki/File:Alpha_Helix_Ribbon.svg" class="mw-file-description"><img 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>The alpha helix structure necessary for the stability of DNA is held together by the electrostatic intramolecular forces in the protein.</figcaption></figure> <p>Intramolecular forces are extremely important in the field of biochemistry, where it comes into play at the most basic levels of biological structures. Intramolecular forces such as <a href="/wiki/Disulfide_bond_formation_protein_B" title="Disulfide bond formation protein B">disulfide bonds</a> give proteins and <a href="/wiki/DNA" title="DNA">DNA</a> their structure. <a href="/wiki/Protein" title="Protein">Proteins</a> derive their structure from the intramolecular forces that shape them and hold them together. The main source of structure in these molecules is the interaction between the <a href="/wiki/Amino_acid" title="Amino acid">amino acid</a> residues that form the foundation of proteins.<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> The interactions between <a href="/wiki/Residue_(amino_acid)" class="mw-redirect" title="Residue (amino acid)">residues</a> of the same proteins forms the secondary structure of the protein, allowing for the formation of <a href="/wiki/Beta_sheet" title="Beta sheet">beta sheets</a> and <a href="/wiki/Alpha_helix" title="Alpha helix">alpha helices</a>, which are important structures for proteins and in the case of alpha helices, for DNA. </p> <div class="mw-heading mw-heading2"><h2 id="See_also">See also</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Intramolecular_force&action=edit&section=7" title="Edit section: See also"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <ul><li><a href="/wiki/Chemical_bond" title="Chemical bond">Chemical bond</a></li> <li><a href="/wiki/Intermolecular_force" title="Intermolecular force">Intermolecular force</a></li></ul> <div class="mw-heading mw-heading2"><h2 id="References">References</h2><span class="mw-editsection"><span class="mw-editsection-bracket">[</span><a href="/w/index.php?title=Intramolecular_force&action=edit&section=8" title="Edit section: References"><span>edit</span></a><span class="mw-editsection-bracket">]</span></span></div> <style data-mw-deduplicate="TemplateStyles:r1239543626">.mw-parser-output .reflist{margin-bottom:0.5em;list-style-type:decimal}@media screen{.mw-parser-output .reflist{font-size:90%}}.mw-parser-output .reflist .references{font-size:100%;margin-bottom:0;list-style-type:inherit}.mw-parser-output .reflist-columns-2{column-width:30em}.mw-parser-output .reflist-columns-3{column-width:25em}.mw-parser-output .reflist-columns{margin-top:0.3em}.mw-parser-output .reflist-columns ol{margin-top:0}.mw-parser-output .reflist-columns li{page-break-inside:avoid;break-inside:avoid-column}.mw-parser-output .reflist-upper-alpha{list-style-type:upper-alpha}.mw-parser-output .reflist-upper-roman{list-style-type:upper-roman}.mw-parser-output .reflist-lower-alpha{list-style-type:lower-alpha}.mw-parser-output .reflist-lower-greek{list-style-type:lower-greek}.mw-parser-output .reflist-lower-roman{list-style-type:lower-roman}</style><div class="reflist"> <div class="mw-references-wrap"><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 id="CITEREFZumdahlZumdahl2007" class="citation book cs1">Zumdahl, Steven S.; Zumdahl, Susan A. (2007). <i>Chemistry</i> (7th ed.). Boston: Houghton Mifflin. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0618713707" title="Special:BookSources/978-0618713707"><bdi>978-0618713707</bdi></a>. <a href="/wiki/OCLC_(identifier)" class="mw-redirect" title="OCLC (identifier)">OCLC</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/oclc/85824942">85824942</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Chemistry&rft.place=Boston&rft.edition=7th&rft.pub=Houghton+Mifflin&rft.date=2007&rft_id=info%3Aoclcnum%2F85824942&rft.isbn=978-0618713707&rft.aulast=Zumdahl&rft.aufirst=Steven+S.&rft.au=Zumdahl%2C+Susan+A.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIntramolecular+force" class="Z3988"></span></span> </li> <li id="cite_note-2"><span class="mw-cite-backlink"><b><a href="#cite_ref-2">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFFischerWendland2023" class="citation journal cs1">Fischer, Johann; Wendland, Martin (2023). <a rel="nofollow" class="external text" href="https://linkinghub.elsevier.com/retrieve/pii/S0378381223001565">"On the history of key empirical intermolecular potentials"</a>. <i>Fluid Phase Equilibria</i>. <b>573</b>: 113876. <a href="/wiki/Doi_(identifier)" class="mw-redirect" title="Doi (identifier)">doi</a>:<span class="id-lock-free" title="Freely accessible"><a rel="nofollow" class="external text" href="https://doi.org/10.1016%2Fj.fluid.2023.113876">10.1016/j.fluid.2023.113876</a></span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Fluid+Phase+Equilibria&rft.atitle=On+the+history+of+key+empirical+intermolecular+potentials&rft.volume=573&rft.pages=113876&rft.date=2023&rft_id=info%3Adoi%2F10.1016%2Fj.fluid.2023.113876&rft.aulast=Fischer&rft.aufirst=Johann&rft.au=Wendland%2C+Martin&rft_id=https%3A%2F%2Flinkinghub.elsevier.com%2Fretrieve%2Fpii%2FS0378381223001565&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIntramolecular+force" class="Z3988"></span></span> </li> <li id="cite_note-Principles_of_Modern_Chemistry-3"><span class="mw-cite-backlink">^ <a href="#cite_ref-Principles_of_Modern_Chemistry_3-0"><sup><i><b>a</b></i></sup></a> <a href="#cite_ref-Principles_of_Modern_Chemistry_3-1"><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="CITEREFOxtobyGillsCampion2012" class="citation book cs1">Oxtoby, David W.; Gills, H. P.; Campion, Alan (2012). <i>Principles of modern chemistry</i> (7th ed.). Belmont, Calif.: Brooks/Cole Cengage Learning. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/978-0-8400-4931-5" title="Special:BookSources/978-0-8400-4931-5"><bdi>978-0-8400-4931-5</bdi></a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Principles+of+modern+chemistry&rft.place=Belmont%2C+Calif.&rft.edition=7th&rft.pub=Brooks%2FCole+Cengage+Learning&rft.date=2012&rft.isbn=978-0-8400-4931-5&rft.aulast=Oxtoby&rft.aufirst=David+W.&rft.au=Gills%2C+H.+P.&rft.au=Campion%2C+Alan&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIntramolecular+force" class="Z3988"></span></span> </li> <li id="cite_note-4"><span class="mw-cite-backlink"><b><a href="#cite_ref-4">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFBaderHenneker1965" class="citation journal cs1">Bader, R. F. W.; Henneker, W. H. (1965). "The Ionic Bond". <i>Journal of the American Chemical Society</i>. <b>87</b> (14): 3063–3068. <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%2Fja01092a008">10.1021/ja01092a008</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=article&rft.jtitle=Journal+of+the+American+Chemical+Society&rft.atitle=The+Ionic+Bond&rft.volume=87&rft.issue=14&rft.pages=3063-3068&rft.date=1965&rft_id=info%3Adoi%2F10.1021%2Fja01092a008&rft.aulast=Bader&rft.aufirst=R.+F.+W.&rft.au=Henneker%2C+W.+H.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIntramolecular+force" class="Z3988"></span></span> </li> <li id="cite_note-5"><span class="mw-cite-backlink"><b><a href="#cite_ref-5">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite class="citation web cs1"><a rel="nofollow" class="external text" href="https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introduction_to_General_Chemistry_(Malik)/03%3A_Compounds/3.09%3A_Intramolecular_forces_and_intermolecular_forces">"3.9: Intramolecular forces and intermolecular forces"</a>. <i>Chemistry LibreTexts</i>. 2022-04-05<span class="reference-accessdate">. Retrieved <span class="nowrap">2022-10-09</span></span>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=Chemistry+LibreTexts&rft.atitle=3.9%3A+Intramolecular+forces+and+intermolecular+forces&rft.date=2022-04-05&rft_id=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FIntroductory_Chemistry%2FIntroduction_to_General_Chemistry_%28Malik%29%2F03%253A_Compounds%2F3.09%253A_Intramolecular_forces_and_intermolecular_forces&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIntramolecular+force" class="Z3988"></span></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"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFHelmenstine" class="citation web cs1">Helmenstine, Anne Marie. <a rel="nofollow" class="external text" href="https://www.thoughtco.com/definition-of-covalent-bond-604414">"Understand What a Covalent Bond Is in Chemistry"</a>. <i>ThoughtCo</i>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Ajournal&rft.genre=unknown&rft.jtitle=ThoughtCo&rft.atitle=Understand+What+a+Covalent+Bond+Is+in+Chemistry&rft.aulast=Helmenstine&rft.aufirst=Anne+Marie&rft_id=https%3A%2F%2Fwww.thoughtco.com%2Fdefinition-of-covalent-bond-604414&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIntramolecular+force" class="Z3988"></span></span> </li> <li id="cite_note-7"><span class="mw-cite-backlink"><b><a href="#cite_ref-7">^</a></b></span> <span class="reference-text"><link rel="mw-deduplicated-inline-style" href="mw-data:TemplateStyles:r1238218222"><cite id="CITEREFNelsonCoxLehninger2013" class="citation book cs1">Nelson, David L.; Cox, Michael M.; Lehninger, Albert L. (2013). <i>Lehninger principles of biochemistry</i> (6th ed.). New York: W.H. Freeman and Company. <a href="/wiki/ISBN_(identifier)" class="mw-redirect" title="ISBN (identifier)">ISBN</a> <a href="/wiki/Special:BookSources/9781429234146" title="Special:BookSources/9781429234146"><bdi>9781429234146</bdi></a>. <a href="/wiki/OCLC_(identifier)" class="mw-redirect" title="OCLC (identifier)">OCLC</a> <a rel="nofollow" class="external text" href="https://search.worldcat.org/oclc/824794893">824794893</a>.</cite><span title="ctx_ver=Z39.88-2004&rft_val_fmt=info%3Aofi%2Ffmt%3Akev%3Amtx%3Abook&rft.genre=book&rft.btitle=Lehninger+principles+of+biochemistry&rft.place=New+York&rft.edition=6th&rft.pub=W.H.+Freeman+and+Company&rft.date=2013&rft_id=info%3Aoclcnum%2F824794893&rft.isbn=9781429234146&rft.aulast=Nelson&rft.aufirst=David+L.&rft.au=Cox%2C+Michael+M.&rft.au=Lehninger%2C+Albert+L.&rfr_id=info%3Asid%2Fen.wikipedia.org%3AIntramolecular+force" class="Z3988"></span></span> </li> </ol></div></div> <div class="navbox-styles"><style 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class="mw-selflink selflink">Intramolecular</a><br />(strong)</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/Covalent_bond" title="Covalent bond">Covalent</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/Electron_deficiency" title="Electron deficiency">Electron deficiency</a> <ul><li><a href="/wiki/Three-center_two-electron_bond" title="Three-center two-electron bond">3c–2e</a></li> <li><a href="/wiki/Four-center_two-electron_bond" title="Four-center two-electron bond">4c–2e</a></li> <li><a href="/wiki/Eight-center_two-electron_bond" class="mw-redirect" title="Eight-center two-electron bond">8c–2e</a></li></ul></li> <li><a href="/wiki/Hypervalent_molecule" title="Hypervalent molecule">Hypervalence</a> <ul><li><a href="/wiki/Three-center_four-electron_bond" title="Three-center four-electron bond">3c–4e</a></li></ul></li> <li><a href="/wiki/Agostic_interaction" title="Agostic interaction">Agostic</a></li> <li><a href="/wiki/Bent_bond" title="Bent bond">Bent</a></li> <li><a href="/wiki/Coordinate_covalent_bond" title="Coordinate covalent bond">Coordinate (dipolar)</a></li> <li><a href="/wiki/Pi_backbonding" title="Pi backbonding">Pi backbond</a></li> <li><a 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 href="/wiki/Ionic_bonding" title="Ionic bonding">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 hlist" style="width:100%;padding:0"><div style="padding:0 0.25em"> <ul><li><a href="/wiki/Aromaticity" title="Aromaticity">Aromaticity</a> <ul><li><a href="/wiki/H%C3%BCckel%27s_rule" title="Hückel's rule">Hückel's rule</a></li> <li><a href="/wiki/Baird%27s_rule" title="Baird's rule">Baird's rule</a></li> <li><a href="/wiki/M%C3%B6bius_aromaticity" title="Möbius aromaticity">Möbius</a></li> <li><a href="/wiki/Spherical_aromaticity" title="Spherical aromaticity">spherical</a></li></ul></li> <li><a href="/wiki/Polyhedral_skeletal_electron_pair_theory" title="Polyhedral skeletal electron pair theory">Polyhedral skeletal electron pair theory</a></li> <li><a href="/wiki/Jemmis_mno_rules" title="Jemmis mno rules">Jemmis mno rules</a></li></ul> </div></td></tr></tbody></table></div>    </div><noscript><img src="https://login.wikimedia.org/wiki/Special:CentralAutoLogin/start?type=1x1" alt="" width="1" height="1" style="border: none; position: absolute;"></noscript> <div class="printfooter" data-nosnippet="">Retrieved from "<a dir="ltr" href="https://en.wikipedia.org/w/index.php?title=Intramolecular_force&oldid=1255825667">https://en.wikipedia.org/w/index.php?title=Intramolecular_force&oldid=1255825667</a>"</div></div> <div id="catlinks" class="catlinks" data-mw="interface"><div id="mw-normal-catlinks" class="mw-normal-catlinks"><a href="/wiki/Help:Category" title="Help:Category">Category</a>: <ul><li><a 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