{"id":48354,"date":"2023-09-19T21:53:55","date_gmt":"2023-09-19T16:08:55","guid":{"rendered":"https:\/\/thechemistrynotes.com\/?p=48354"},"modified":"2023-09-19T21:53:59","modified_gmt":"2023-09-19T16:08:59","slug":"dipole-moment-factors-uses-examples","status":"publish","type":"post","link":"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/","title":{"rendered":"Dipole Moment: Factors, Uses, Examples"},"content":{"rendered":"\n<figure class=\"wp-block-image size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"536\" src=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/dipole-moment-1024x536.jpg\" alt=\"dipole moment\" class=\"wp-image-48358\" srcset=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/dipole-moment-1024x536.jpg 1024w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/dipole-moment-300x157.jpg 300w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/dipole-moment-768x402.jpg 768w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/dipole-moment.jpg 1205w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><\/figure>\n\n\n\n<p>The dipole moment is a quantity that describes the separation of two opposite charges.\u00a0 It is a quantity that can be measured in the lab for a molecule and used to calculate the size of the partial charges on the molecule (assuming the bond length is known).\u00a0 It is defined as the product of the magnitude of the separated charge and the separation distance.<\/p>\n\n\n\n<div id=\"ez-toc-container\" class=\"ez-toc-v2_0_65 counter-hierarchy ez-toc-counter ez-toc-custom ez-toc-container-direction\">\n<div class=\"ez-toc-title-container\">\n<p class=\"ez-toc-title \" >Table of Contents<\/p>\n<span class=\"ez-toc-title-toggle\"><a href=\"#\" class=\"ez-toc-pull-right ez-toc-btn ez-toc-btn-xs ez-toc-btn-default ez-toc-toggle\" aria-label=\"Toggle Table of Content\"><span class=\"ez-toc-js-icon-con\"><span class=\"\"><span class=\"eztoc-hide\" style=\"display:none;\">Toggle<\/span><span class=\"ez-toc-icon-toggle-span\"><svg style=\"fill: #0a0a0a;color:#0a0a0a\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" class=\"list-377408\" width=\"20px\" height=\"20px\" viewBox=\"0 0 24 24\" fill=\"none\"><path d=\"M6 6H4v2h2V6zm14 0H8v2h12V6zM4 11h2v2H4v-2zm16 0H8v2h12v-2zM4 16h2v2H4v-2zm16 0H8v2h12v-2z\" fill=\"currentColor\"><\/path><\/svg><svg style=\"fill: #0a0a0a;color:#0a0a0a\" class=\"arrow-unsorted-368013\" xmlns=\"http:\/\/www.w3.org\/2000\/svg\" width=\"10px\" height=\"10px\" viewBox=\"0 0 24 24\" version=\"1.2\" baseProfile=\"tiny\"><path d=\"M18.2 9.3l-6.2-6.3-6.2 6.3c-.2.2-.3.4-.3.7s.1.5.3.7c.2.2.4.3.7.3h11c.3 0 .5-.1.7-.3.2-.2.3-.5.3-.7s-.1-.5-.3-.7zM5.8 14.7l6.2 6.3 6.2-6.3c.2-.2.3-.5.3-.7s-.1-.5-.3-.7c-.2-.2-.4-.3-.7-.3h-11c-.3 0-.5.1-.7.3-.2.2-.3.5-.3.7s.1.5.3.7z\"\/><\/svg><\/span><\/span><\/span><\/a><\/span><\/div>\n<nav><ul class='ez-toc-list ez-toc-list-level-1 ' ><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-1\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#what-is-a-dipole-moment\" title=\"What is a dipole moment?\">What is a dipole moment?<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-2\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#unit-of-dipole-moment\" title=\"Unit of dipole moment\">Unit of dipole moment<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-3\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#what-are-polar-molecules\" title=\"What are polar molecules?\">What are polar molecules?<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-4\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#facts-about-the-dipole-moment\" title=\"Facts about the Dipole Moment\">Facts about the Dipole Moment<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-5\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#dipole-moment-in-monoatomic-species\" title=\"Dipole moment in monoatomic species\">Dipole moment in monoatomic species<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-6\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#dipole-moment-in-homonuclear-diatomic-molecule\" title=\"Dipole moment in homonuclear diatomic molecule\">Dipole moment in homonuclear diatomic molecule<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-7\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#dipole-moment-in-heteronuclear-species\" title=\"Dipole moment in heteronuclear species\">Dipole moment in heteronuclear species<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-8\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#the-dipole-moment-of-nf3\" title=\"The dipole moment of NF3\">The dipole moment of NF3<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-9\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#factors-affecting-dipole-moment\" title=\"Factors affecting dipole moment\">Factors affecting dipole moment<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-10\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#chemical-properties-dipole-moment\" title=\"Chemical properties: Dipole moment\">Chemical properties: Dipole moment<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-11\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#uses-of-dipole-moment\" title=\"Uses of dipole moment\">Uses of dipole moment<\/a><\/li><li class='ez-toc-page-1 ez-toc-heading-level-2'><a class=\"ez-toc-link ez-toc-heading-12\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/#references\" title=\"References\">References<\/a><\/li><\/ul><\/nav><\/div>\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"what-is-a-dipole-moment\"><\/span><strong>What is a dipole moment?<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>In chemistry, it expresses the polar nature or polarity of the molecules. It is defined as the product of charge and the distance between atoms in a chemical bond.\u00a0 It happens when there is a charge separation. A single atom or molecule has a dipole moment. When it\u00a0occurs molecule, it might occur between two atoms in an ionic or covalent bond.<\/p>\n\n\n\n<p class=\"has-text-align-center has-accent-color has-text-color\">\u03bc = q x r<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"unit-of-dipole-moment\"><\/span><strong>Unit of dipole moment<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>The charge in the CGS system is given in esu\u00a0and the bond length in cm. As a result, it is measured in esu cm. The charge is in the order of 10<sup>-10<\/sup> esu, while the separation is in the order of 10<sup>-8<\/sup> cm. As a result, the order\u00a0is 10<sup>-18<\/sup> esu cm. This magnitude is known as 1 Debye. As a result, 1 Debye = 10<sup>-18<\/sup> esu cm.<\/p>\n\n\n\n<p>The charge in the SI system is given in coulombs\u00a0and the length in meters. As a result, the coulomb meter is it&#8217;s SI unit.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"what-are-polar-molecules\"><\/span><strong>What are polar molecules?<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>Polarity occurs in molecules when the center of gravity of the positive charge does not coincide with the center of gravity of the negative charge. These are known as polar molecules. Polar molecules include hydrogen chloride, water, methyl chloride, and benzyl chloride.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"facts-about-the-dipole-moment\"><\/span><strong>Facts about the Dipole Moment<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>The bond dipole moment is the dipole moment of a single bond in a polyatomic molecule, which differs from the molecule&#8217;s overall dipole moment.<\/li>\n\n\n\n<li>It is a vector quantity, which means it has both magnitude and definite directions. As it is a vector variable, it can be 0 because two opposing bond dipoles can cancel each other out.<\/li>\n\n\n\n<li>According to the\u00a0convention, it is represented by a tiny arrow with its tail in the negative center and its head in the positive center.<\/li>\n\n\n\n<li>It is symbolized in chemistry by a modest variant of the arrow sign. A cross in the positive center and an arrowhead in the negative center represent the dipole moment. This arrow depicts the molecule&#8217;s shift in electron density.<\/li>\n\n\n\n<li>In the case of a polyatomic molecule, it is the vector sum of all bond dipoles.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"dipole-moment-in-monoatomic-species\"><\/span><strong>Dipole moment in monoatomic species<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>In chemistry, it is used to specify the structure, bond angle, bond energy, and polarity of various compounds. Because the charge of the constituent atom is spread symmetrically, monoatomic noble gases like benzene are non-polar.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"dipole-moment-in-homonuclear-diatomic-molecule\"><\/span><strong>Dipole moment in homonuclear diatomic molecule<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>Because of their symmetrical charge distributions and equal electronegativity and ionization energy, homonuclear diatomic molecules such as nitrogen, oxygen, and chlorine have zero dipole values.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"dipole-moment-in-heteronuclear-species\"><\/span><strong>Dipole moment in heteronuclear species<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>A dipole\/dipole moment does not exist in molecules with symmetrical\/opposite dipoles. Because the bond polarities cancel each other out, there is no net dipole.<\/p>\n\n\n\n<p>For example:<\/p>\n\n\n\n<p>In the beryllium fluoride molecule, the bond angle between the two beryllium-fluorine bonds is 180o. As fluorine is a more electronegative atom than Beryllium, it causes the electron density to move towards itself. In a BeF<sub>2<\/sub> molecule, the two individual bond dipole moments cancel each other out. The net dipole moment of a BeF<sub>2<\/sub> molecule is 0 since they are equal in magnitude but opposite in direction.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"375\" height=\"70\" src=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/image-56.png\" alt=\"\" class=\"wp-image-48356\" srcset=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/image-56.png 375w, https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/image-56-300x56.png 300w\" sizes=\"(max-width: 375px) 100vw, 375px\" \/><\/figure><\/div>\n\n\n<p>Even though a molecule has symmetry, it still has a dipole moment. Because the oxygen atom is far more electronegative than the hydrogen atom, the electrons in a water molecule are concentrated around it. According to the Valence shell electron pair repulsion theory, the presence of a lone pair of electrons in the oxygen atom causes the water molecule to have a bent shape. As a result, unlike in the BeF<sub>2<\/sub> molecule, the individual bond dipole moments do not cancel each other out. A <a href=\"https:\/\/thechemistrynotes.com\/amazing-properties-of-water\/\">water<\/a> H<sub>2<\/sub>O molecule has a bond angle of 104.5<sup>o<\/sup>. An oxygen-hydrogen bond in a water molecule has an individual bond moment of 1.5 D. A water H<sub>2<\/sub>O molecule has a net dipole moment of 1.84 D.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"233\" height=\"157\" src=\"https:\/\/thechemistrynotes.com\/wp-content\/uploads\/2023\/09\/image-55.png\" alt=\"\" class=\"wp-image-48355\" \/><\/figure><\/div>\n\n\n<p>We are particularly interested in the symmetry of the dipoles. The dipoles in water point in the same direction, whereas in BeCl2, they point in opposing directions, which is why they cancel.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"the-dipole-moment-of-nf3\"><\/span><strong>The dipole moment of NF<sub>3<\/sub><\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>Although there is a significant difference in electronegativity and electron affinity between nitrogen and fluorine atoms, NF<sub>3<\/sub> has a relatively modest bond moment and a comparable structure to NH<sub>3<\/sub>.<\/p>\n\n\n\n<p>The fact that the resultant bond moment of the three nitrogen-fluorine bonds acts in the opposite direction to that of the lone pair inserted at the nitrogen atom explains the low value of, NF<sub>3<\/sub>. However, in NH<sub>3<\/sub>, the generated bond moment acts in the same direction as the lone pair electrons.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"factors-affecting-dipole-moment\"><\/span><strong>Factors affecting dipole moment<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p><strong>Bond length<\/strong><\/p>\n\n\n\n<p>It increases as the bond length increases.<\/p>\n\n\n\n<p><strong>Polarity<\/strong><\/p>\n\n\n\n<p>The bigger the polarity difference, the greater the dipole value The magnitude of the charges (Q) is influenced by the polarity difference.<\/p>\n\n\n\n<p><strong>Geometry<\/strong><\/p>\n\n\n\n<p>If a molecule has opposing dipoles, it has no dipole moment (for example, BeCl<sub>2<\/sub>)<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"chemical-properties-dipole-moment\"><\/span><strong>Chemical properties: Dipole moment<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<p>It is useful for determining certain chemical characteristics. It is, for instance, may affect the following attributes:<\/p>\n\n\n\n<p><strong>Solubility<\/strong><\/p>\n\n\n\n<p>The larger its dipole value, the greater the likelihood that the molecule will dissolve in a polar solution.<\/p>\n\n\n\n<p><strong>Melting\/Boiling point<\/strong><\/p>\n\n\n\n<p>The boiling\/melting point increases with increasing dipole moment.<\/p>\n\n\n\n<p>Molecules having a higher dipole have stronger intermolecular forces. As a result, these forces are more difficult to break.<\/p>\n\n\n\n<p><strong>Stability\/Reactivity<\/strong><\/p>\n\n\n\n<p>The larger the dipole value, the more reactive the system.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"uses-of-dipole-moment\"><\/span><strong>Uses of dipole moment<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>It&nbsp;is used to determine the polarity of the connection. The polarity of the bond in a molecule rises as the amount of the dipole moment grows.<\/li>\n\n\n\n<li> It is used to determine a molecule&#8217;s structure or form. Because molecules with specified dipole moment values can be bent or angular in shape, they do not have a symmetrical structure. While molecules with zero dipole moment have a symmetrical structure or form.<\/li>\n\n\n\n<li>It is used to differentiate between cis- and trans-isomers. Trans-isomers have a higher value than cis-isomers, which have a lower dipole value.<\/li>\n\n\n\n<li>It is used to differentiate ortho, meta, and para isomers. Para-isomers often have dipole moments of zero, whereas ortho-isomers have dipole values larger than those of meta-isomers.<\/li>\n\n\n\n<li>The percentage ionic nature of covalent or ionic heteronuclear diatomic compounds is calculated using dipole data. Consider\u00a0molecule AB, which has an observable dipole moment = \u03bcobs and a bond length of\u00a0l cm.<\/li>\n\n\n\n<li>If the shared pair is located in the middle of the atoms, the connection is fully covalent, and the percentage ionic character is zero.<\/li>\n\n\n\n<li>However, if the connection is entirely ionic and B is more electronegative than A,\u00a0A has a unit positive charge and B has a unit negative charge.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\"><span class=\"ez-toc-section\" id=\"references\"><\/span><strong>References<\/strong><span class=\"ez-toc-section-end\"><\/span><\/h2>\n\n\n\n<ul>\n<li>https:\/\/unacademy.com\/content\/cbse-class-11\/study-material\/chemistry\/dipole-moment\/<\/li>\n\n\n\n<li>https:\/\/collegedunia.com\/exams\/dipole-moment-chemistry-articleid-528<\/li>\n\n\n\n<li>https:\/\/www.hellovaia.com\/explanations\/chemistry\/physical-chemistry\/dipole-moment\/<\/li>\n\n\n\n<li>https:\/\/www.chemistrylearner.com\/dipole-moment.html<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>The dipole moment is a quantity that describes the separation of two opposite charges.\u00a0 It is a quantity that can be measured in the lab for a molecule and used &#8230; <a title=\"Dipole Moment: Factors, Uses, Examples\" class=\"read-more\" href=\"https:\/\/thechemistrynotes.com\/dipole-moment-factors-uses-examples\/\" aria-label=\"Read more about Dipole Moment: Factors, Uses, Examples\">Read more<\/a><\/p>\n","protected":false},"author":4,"featured_media":48358,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[24],"tags":[2890,2893,2891,2892],"_links":{"self":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/48354"}],"collection":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/users\/4"}],"replies":[{"embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/comments?post=48354"}],"version-history":[{"count":2,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/48354\/revisions"}],"predecessor-version":[{"id":48359,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/posts\/48354\/revisions\/48359"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/media\/48358"}],"wp:attachment":[{"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/media?parent=48354"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/categories?post=48354"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/thechemistrynotes.com\/wp-json\/wp\/v2\/tags?post=48354"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}