{"id":233977,"date":"2025-06-13T16:08:38","date_gmt":"2025-06-13T16:08:38","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=233977"},"modified":"2025-06-13T16:08:40","modified_gmt":"2025-06-13T16:08:40","slug":"which-pair-of-molecules-has-the-strongest-dipole-dipole-interactions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/13\/which-pair-of-molecules-has-the-strongest-dipole-dipole-interactions\/","title":{"rendered":"Which pair of molecules has the strongest dipole-dipole interactions"},"content":{"rendered":"\n<p>Which pair of molecules has the strongest dipole-dipole interactions? a. NH3 and CH4 b. CO2 and CH4 c. NH3 and NH3 d. CO2 and CO2 e. CH4 and CH4<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p><strong>Correct Answer: c. NH\u2083 and NH\u2083<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<p>Dipole-dipole interactions are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule. These interactions only occur between molecules that have a permanent dipole moment, meaning the molecules must be <strong>polar<\/strong>.<\/p>\n\n\n\n<p>Let\u2019s examine the molecules listed in the options:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>NH\u2083 (ammonia):<\/strong> A <strong>polar molecule<\/strong>. It has a trigonal pyramidal geometry due to the lone pair on nitrogen, and a significant difference in electronegativity between nitrogen and hydrogen. This gives NH\u2083 a <strong>permanent dipole<\/strong>.<\/li>\n\n\n\n<li><strong>CH\u2084 (methane):<\/strong> A <strong>nonpolar molecule<\/strong>. It has a tetrahedral shape with equal electronegativity pulling in all directions, cancelling out dipoles.<\/li>\n\n\n\n<li><strong>CO\u2082 (carbon dioxide):<\/strong> A <strong>nonpolar molecule<\/strong>, even though the C=O bonds are polar. Its linear geometry causes the dipoles to cancel out, resulting in <strong>no net dipole moment<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Now, evaluating the options:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>a. NH\u2083 and CH\u2084:<\/strong> NH\u2083 is polar, CH\u2084 is nonpolar \u2192 <strong>no dipole-dipole interaction<\/strong>.<\/li>\n\n\n\n<li><strong>b. CO\u2082 and CH\u2084:<\/strong> Both are nonpolar \u2192 <strong>no dipole-dipole interaction<\/strong>.<\/li>\n\n\n\n<li><strong>c. NH\u2083 and NH\u2083:<\/strong> Both are polar \u2192 <strong>strong dipole-dipole interactions<\/strong>. Additionally, NH\u2083 can form <strong>hydrogen bonds<\/strong>, a special type of strong dipole-dipole interaction, due to the N-H bond.<\/li>\n\n\n\n<li><strong>d. CO\u2082 and CO\u2082:<\/strong> Both are nonpolar \u2192 <strong>no dipole-dipole interaction<\/strong>.<\/li>\n\n\n\n<li><strong>e. CH\u2084 and CH\u2084:<\/strong> Both are nonpolar \u2192 <strong>no dipole-dipole interaction<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Therefore, <strong>NH\u2083 and NH\u2083<\/strong> not only exhibit <strong>dipole-dipole interactions<\/strong> but also <strong>hydrogen bonding<\/strong>, which is among the strongest intermolecular forces for neutral molecules. This makes them the pair with the <strong>strongest<\/strong> dipole-dipole interactions in the given list.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-380.jpeg\" alt=\"\" class=\"wp-image-233978\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Which pair of molecules has the strongest dipole-dipole interactions? a. NH3 and CH4 b. CO2 and CH4 c. NH3 and NH3 d. CO2 and CO2 e. CH4 and CH4 The Correct Answer and Explanation is: Correct Answer: c. NH\u2083 and NH\u2083 Explanation: Dipole-dipole interactions are attractive forces between the positive end of one polar molecule [&hellip;]<\/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-233977","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233977","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=233977"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233977\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=233977"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=233977"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=233977"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}