What are the intermolecular forces that ethylene glycol exhibit(s)?<\/p>\n\n\n\n
Dispersion and dipole-dipole
Dispersion and H-bonding
Dispersion, dipole-dipole, and H-bonding
dipole-dipole and H-bonding<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/strong><\/p>\n\n\n\n Correct Answer: Dispersion, dipole-dipole, and H-bonding<\/strong><\/p>\n\n\n\n Ethylene glycol (chemical formula: C\u2082H\u2086O\u2082<\/strong>, also known as HO\u2013CH\u2082\u2013CH\u2082\u2013OH<\/strong>) is a small organic molecule with two hydroxyl (\u2013OH<\/strong>) groups. Its structure plays a significant role in the types of intermolecular forces (IMFs)<\/strong> it can exhibit. Understanding these forces helps explain its physical properties, such as high boiling point and solubility in water.<\/p>\n\n\n\n Dispersion forces are present in all molecules<\/strong>, regardless of polarity. These arise due to temporary fluctuations in electron density<\/strong>, which create temporary dipoles. In ethylene glycol, even though it has polar functional groups, the nonpolar carbon-hydrogen framework still contributes to dispersion forces. Therefore, dispersion forces are present<\/strong> in ethylene glycol.<\/p>\n\n\n\n Ethylene glycol is a polar molecule<\/strong>. Each hydroxyl group (\u2013OH) contains a polar O\u2013H bond, and the molecule itself has an overall net dipole. Because of the permanent dipole moments<\/strong> due to electronegativity differences (oxygen is more electronegative than hydrogen or carbon), dipole-dipole interactions occur<\/strong> between neighboring ethylene glycol molecules. These interactions are stronger than dispersion forces but weaker than hydrogen bonds.<\/p>\n\n\n\n Hydrogen bonding is a strong type of dipole-dipole interaction<\/strong> that occurs when hydrogen is directly bonded to a highly electronegative atom such as oxygen (O), nitrogen (N), or fluorine (F)<\/strong>. In ethylene glycol, the O\u2013H groups allow both donation and acceptance of hydrogen bonds<\/strong>. Each \u2013OH group can:<\/p>\n\n\n\n Thus, ethylene glycol molecules can form extensive hydrogen bonding networks<\/strong>, making this the strongest IMF present<\/strong> in the substance.<\/p>\n\n\n\n Because of its molecular structure, ethylene glycol exhibits<\/strong>:<\/p>\n\n\n\n Hence, the correct choice is: What are the intermolecular forces that ethylene glycol exhibit(s)? Dispersion and dipole-dipoleDispersion and H-bondingDispersion, dipole-dipole, and H-bondingdipole-dipole and H-bonding The Correct Answer and Explanation is: Correct Answer: Dispersion, dipole-dipole, and H-bonding Explanation (300+ words): Ethylene glycol (chemical formula: C\u2082H\u2086O\u2082, also known as HO\u2013CH\u2082\u2013CH\u2082\u2013OH) is a small organic molecule with two hydroxyl (\u2013OH) groups. Its structure […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-217169","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/217169","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=217169"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/217169\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=217169"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=217169"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=217169"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Explanation (300+ words):<\/h3>\n\n\n\n
\n\n\n\n1. Dispersion Forces (London Dispersion Forces):<\/strong><\/h3>\n\n\n\n
\n\n\n\n2. Dipole-Dipole Interactions:<\/strong><\/h3>\n\n\n\n
\n\n\n\n3. Hydrogen Bonding:<\/strong><\/h3>\n\n\n\n
\n
\n\n\n\nSummary:<\/h3>\n\n\n\n
\n
Dispersion, dipole-dipole, and H-bonding<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"