To determine which molecule in each pair has the greater dipole moment, we must examine factors such as molecular shape, electronegativity differences, and symmetry. Here’s the breakdown for each pair:<\/p>\n\n\n\n
(a) ClO\u2082 vs SO\u2082<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: SO\u2082<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
Both molecules are bent, but SO\u2082 has a higher electronegativity difference between sulfur and oxygen (S-O bond) than ClO\u2082 does (Cl-O bond). Additionally, sulfur has a higher charge distribution due to its larger size, resulting in a stronger dipole. Although chlorine is more electronegative than sulfur, the Cl-O bond is less polar, and chlorine’s larger atomic radius reduces the overall dipole moment. Therefore, SO\u2082 has a greater dipole moment because the sulfur-oxygen bonds contribute more to the polarity of the molecule than chlorine-oxygen bonds.<\/li>\n<\/ul>\n\n\n\n(b) HBr vs HCl<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: HCl<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
Both HBr and HCl are polar molecules due to the difference in electronegativity between hydrogen and the halogens. However, chlorine<\/strong> is more electronegative than bromine, meaning the H-Cl bond is more polar than the H-Br bond. Since the dipole moment depends on both the bond polarity and the distance between the nuclei, HCl has a larger dipole moment due to the greater electronegativity difference between hydrogen and chlorine.<\/li>\n<\/ul>\n\n\n\n(c) BeCl\u2082 vs SCl\u2082<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: SCl\u2082<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
BeCl\u2082 is a linear molecule with symmetrical charge distribution, which means its dipole moments cancel each other out. In contrast, SCl\u2082 is bent, and its molecular shape doesn’t allow the dipoles to cancel out. This results in a net dipole moment for SCl\u2082. Moreover, sulfur is more electronegative than beryllium, contributing to a larger dipole moment in SCl\u2082.<\/li>\n<\/ul>\n\n\n\n(d) AsF\u2083 vs AsF\u2085<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: AsF\u2083<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
AsF\u2083 has a trigonal pyramidal structure, which is asymmetrical, so the dipoles do not cancel out. In contrast, AsF\u2085 has a trigonal bipyramidal shape, which is symmetrical, meaning the dipoles cancel out and the molecule has no net dipole moment. Even though fluorine is highly electronegative, the symmetry of AsF\u2085 results in a dipole moment of zero, while the asymmetry of AsF\u2083 ensures a non-zero dipole moment.<\/li>\n<\/ul>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- SO\u2082<\/strong> > ClO\u2082<\/strong><\/li>\n\n\n\n
- HCl<\/strong> > HBr<\/strong><\/li>\n\n\n\n
- SCl\u2082<\/strong> > BeCl\u2082<\/strong><\/li>\n\n\n\n
- AsF\u2083<\/strong> > AsF\u2085<\/strong><\/li>\n<\/ul>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-358.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"Which molecule in each pair has the greater dipole moment? Give the reason for your choice. (a) ClO2 or SO2 (b) HBr or HCl (c) BeCl2 or SCl2 (d) AsF3 or AsF5 The Correct Answer and Explanation is: To determine which molecule in each pair has the greater dipole moment, we must examine factors such […]<\/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-243776","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776","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=243776"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=243776"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=243776"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=243776"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Both molecules are bent, but SO\u2082 has a higher electronegativity difference between sulfur and oxygen (S-O bond) than ClO\u2082 does (Cl-O bond). Additionally, sulfur has a higher charge distribution due to its larger size, resulting in a stronger dipole. Although chlorine is more electronegative than sulfur, the Cl-O bond is less polar, and chlorine’s larger atomic radius reduces the overall dipole moment. Therefore, SO\u2082 has a greater dipole moment because the sulfur-oxygen bonds contribute more to the polarity of the molecule than chlorine-oxygen bonds.<\/li>\n<\/ul>\n\n\n\n
(b) HBr vs HCl<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: HCl<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
Both HBr and HCl are polar molecules due to the difference in electronegativity between hydrogen and the halogens. However, chlorine<\/strong> is more electronegative than bromine, meaning the H-Cl bond is more polar than the H-Br bond. Since the dipole moment depends on both the bond polarity and the distance between the nuclei, HCl has a larger dipole moment due to the greater electronegativity difference between hydrogen and chlorine.<\/li>\n<\/ul>\n\n\n\n(c) BeCl\u2082 vs SCl\u2082<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: SCl\u2082<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
BeCl\u2082 is a linear molecule with symmetrical charge distribution, which means its dipole moments cancel each other out. In contrast, SCl\u2082 is bent, and its molecular shape doesn’t allow the dipoles to cancel out. This results in a net dipole moment for SCl\u2082. Moreover, sulfur is more electronegative than beryllium, contributing to a larger dipole moment in SCl\u2082.<\/li>\n<\/ul>\n\n\n\n(d) AsF\u2083 vs AsF\u2085<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: AsF\u2083<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
AsF\u2083 has a trigonal pyramidal structure, which is asymmetrical, so the dipoles do not cancel out. In contrast, AsF\u2085 has a trigonal bipyramidal shape, which is symmetrical, meaning the dipoles cancel out and the molecule has no net dipole moment. Even though fluorine is highly electronegative, the symmetry of AsF\u2085 results in a dipole moment of zero, while the asymmetry of AsF\u2083 ensures a non-zero dipole moment.<\/li>\n<\/ul>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- SO\u2082<\/strong> > ClO\u2082<\/strong><\/li>\n\n\n\n
- HCl<\/strong> > HBr<\/strong><\/li>\n\n\n\n
- SCl\u2082<\/strong> > BeCl\u2082<\/strong><\/li>\n\n\n\n
- AsF\u2083<\/strong> > AsF\u2085<\/strong><\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Which molecule in each pair has the greater dipole moment? Give the reason for your choice. (a) ClO2 or SO2 (b) HBr or HCl (c) BeCl2 or SCl2 (d) AsF3 or AsF5 The Correct Answer and Explanation is: To determine which molecule in each pair has the greater dipole moment, we must examine factors such […]<\/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-243776","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776","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=243776"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=243776"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=243776"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=243776"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Both HBr and HCl are polar molecules due to the difference in electronegativity between hydrogen and the halogens. However, chlorine<\/strong> is more electronegative than bromine, meaning the H-Cl bond is more polar than the H-Br bond. Since the dipole moment depends on both the bond polarity and the distance between the nuclei, HCl has a larger dipole moment due to the greater electronegativity difference between hydrogen and chlorine.<\/li>\n<\/ul>\n\n\n\n
(c) BeCl\u2082 vs SCl\u2082<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: SCl\u2082<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
BeCl\u2082 is a linear molecule with symmetrical charge distribution, which means its dipole moments cancel each other out. In contrast, SCl\u2082 is bent, and its molecular shape doesn’t allow the dipoles to cancel out. This results in a net dipole moment for SCl\u2082. Moreover, sulfur is more electronegative than beryllium, contributing to a larger dipole moment in SCl\u2082.<\/li>\n<\/ul>\n\n\n\n(d) AsF\u2083 vs AsF\u2085<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: AsF\u2083<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
AsF\u2083 has a trigonal pyramidal structure, which is asymmetrical, so the dipoles do not cancel out. In contrast, AsF\u2085 has a trigonal bipyramidal shape, which is symmetrical, meaning the dipoles cancel out and the molecule has no net dipole moment. Even though fluorine is highly electronegative, the symmetry of AsF\u2085 results in a dipole moment of zero, while the asymmetry of AsF\u2083 ensures a non-zero dipole moment.<\/li>\n<\/ul>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- SO\u2082<\/strong> > ClO\u2082<\/strong><\/li>\n\n\n\n
- HCl<\/strong> > HBr<\/strong><\/li>\n\n\n\n
- SCl\u2082<\/strong> > BeCl\u2082<\/strong><\/li>\n\n\n\n
- AsF\u2083<\/strong> > AsF\u2085<\/strong><\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Which molecule in each pair has the greater dipole moment? Give the reason for your choice. (a) ClO2 or SO2 (b) HBr or HCl (c) BeCl2 or SCl2 (d) AsF3 or AsF5 The Correct Answer and Explanation is: To determine which molecule in each pair has the greater dipole moment, we must examine factors such […]<\/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-243776","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776","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=243776"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=243776"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=243776"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=243776"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
BeCl\u2082 is a linear molecule with symmetrical charge distribution, which means its dipole moments cancel each other out. In contrast, SCl\u2082 is bent, and its molecular shape doesn’t allow the dipoles to cancel out. This results in a net dipole moment for SCl\u2082. Moreover, sulfur is more electronegative than beryllium, contributing to a larger dipole moment in SCl\u2082.<\/li>\n<\/ul>\n\n\n\n
(d) AsF\u2083 vs AsF\u2085<\/strong><\/h3>\n\n\n\n\n- Answer<\/strong>: AsF\u2083<\/strong> has the greater dipole moment.<\/li>\n\n\n\n
- Explanation<\/strong>:
AsF\u2083 has a trigonal pyramidal structure, which is asymmetrical, so the dipoles do not cancel out. In contrast, AsF\u2085 has a trigonal bipyramidal shape, which is symmetrical, meaning the dipoles cancel out and the molecule has no net dipole moment. Even though fluorine is highly electronegative, the symmetry of AsF\u2085 results in a dipole moment of zero, while the asymmetry of AsF\u2083 ensures a non-zero dipole moment.<\/li>\n<\/ul>\n\n\n\nIn summary:<\/p>\n\n\n\n
\n- SO\u2082<\/strong> > ClO\u2082<\/strong><\/li>\n\n\n\n
- HCl<\/strong> > HBr<\/strong><\/li>\n\n\n\n
- SCl\u2082<\/strong> > BeCl\u2082<\/strong><\/li>\n\n\n\n
- AsF\u2083<\/strong> > AsF\u2085<\/strong><\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Which molecule in each pair has the greater dipole moment? Give the reason for your choice. (a) ClO2 or SO2 (b) HBr or HCl (c) BeCl2 or SCl2 (d) AsF3 or AsF5 The Correct Answer and Explanation is: To determine which molecule in each pair has the greater dipole moment, we must examine factors such […]<\/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-243776","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776","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=243776"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=243776"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=243776"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=243776"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
AsF\u2083 has a trigonal pyramidal structure, which is asymmetrical, so the dipoles do not cancel out. In contrast, AsF\u2085 has a trigonal bipyramidal shape, which is symmetrical, meaning the dipoles cancel out and the molecule has no net dipole moment. Even though fluorine is highly electronegative, the symmetry of AsF\u2085 results in a dipole moment of zero, while the asymmetry of AsF\u2083 ensures a non-zero dipole moment.<\/li>\n<\/ul>\n\n\n\n
In summary:<\/p>\n\n\n\n
- \n
- SO\u2082<\/strong> > ClO\u2082<\/strong><\/li>\n\n\n\n
- HCl<\/strong> > HBr<\/strong><\/li>\n\n\n\n
- SCl\u2082<\/strong> > BeCl\u2082<\/strong><\/li>\n\n\n\n
- AsF\u2083<\/strong> > AsF\u2085<\/strong><\/li>\n<\/ul>\n\n\n\n
<\/figure>\n","protected":false},"excerpt":{"rendered":"Which molecule in each pair has the greater dipole moment? Give the reason for your choice. (a) ClO2 or SO2 (b) HBr or HCl (c) BeCl2 or SCl2 (d) AsF3 or AsF5 The Correct Answer and Explanation is: To determine which molecule in each pair has the greater dipole moment, we must examine factors such […]<\/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-243776","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776","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=243776"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243776\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=243776"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=243776"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=243776"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- HCl<\/strong> > HBr<\/strong><\/li>\n\n\n\n