{"id":198519,"date":"2025-03-10T06:23:37","date_gmt":"2025-03-10T06:23:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=198519"},"modified":"2025-03-10T06:23:40","modified_gmt":"2025-03-10T06:23:40","slug":"which-of-the-following-triatomic-molecules-will-have-a-bond-angles-closest-to-120","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/10\/which-of-the-following-triatomic-molecules-will-have-a-bond-angles-closest-to-120\/","title":{"rendered":"Which Of The Following Triatomic Molecules Will Have A Bond Angles Closest To 120\u00b0"},"content":{"rendered":"\n<p>Which Of The Following Triatomic Molecules Will Have A Bond Angles Closest To 120\u00b0?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>Here are some common triatomic molecules:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>CO\u2082 (Carbon Dioxide)<\/strong><\/li>\n\n\n\n<li><strong>SO\u2082 (Sulfur Dioxide)<\/strong><\/li>\n\n\n\n<li><strong>H\u2082O (Water)<\/strong><\/li>\n\n\n\n<li><strong>BF\u2083 (Boron Trifluoride, though it&#8217;s not a triatomic molecule, it&#8217;s planar and relevant for bond angle comparisons)<\/strong><\/li>\n\n\n\n<li><strong>O\u2083 (Ozone)<\/strong><\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Correct Answer: SO\u2082 (Sulfur Dioxide)<\/strong><\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Explanation:<\/strong><\/h4>\n\n\n\n<p>The bond angle of a molecule depends on its molecular geometry, which is determined using <strong>VSEPR (Valence Shell Electron Pair Repulsion) Theory<\/strong>.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>CO\u2082 (Carbon Dioxide) \u2013 180\u00b0<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Linear Geometry<\/strong><\/li>\n\n\n\n<li>Carbon dioxide has no lone pairs on the central atom (C). The two oxygen atoms are arranged in a straight line, leading to a bond angle of <strong>180\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>H\u2082O (Water) \u2013 104.5\u00b0<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Bent Geometry<\/strong><\/li>\n\n\n\n<li>Oxygen in H\u2082O has <strong>two lone pairs<\/strong>, which strongly repel the hydrogen atoms, reducing the bond angle from the ideal <strong>120\u00b0<\/strong> (trigonal planar) to about <strong>104.5\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>BF\u2083 (Boron Trifluoride) \u2013 120\u00b0 (Not a triatomic molecule)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Trigonal Planar<\/strong><\/li>\n\n\n\n<li>This molecule has three bonded atoms around the boron with <strong>no lone pairs<\/strong>, resulting in an exact <strong>120\u00b0 bond angle<\/strong>. However, this is not a triatomic molecule.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>O\u2083 (Ozone) \u2013 ~117\u00b0<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Bent Geometry<\/strong><\/li>\n\n\n\n<li>Ozone has <strong>one lone pair<\/strong> on the central oxygen, leading to a slight deviation from 120\u00b0, making the bond angle <strong>about 117\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>SO\u2082 (Sulfur Dioxide) \u2013 ~119\u00b0<\/strong> \u2705<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Bent Geometry<\/strong><\/li>\n\n\n\n<li>SO\u2082 has <strong>one lone pair<\/strong> on the central sulfur atom. Due to lone pair repulsion, the bond angle is slightly less than 120\u00b0 but remains <strong>very close to it (~119\u00b0)<\/strong>, making SO\u2082 the best answer.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Conclusion:<\/strong><\/h3>\n\n\n\n<p>Among the given triatomic molecules, <strong>SO\u2082 has a bond angle closest to 120\u00b0<\/strong> due to its <strong>bent molecular shape<\/strong> with <strong>one lone pair<\/strong> on the central sulfur atom, following <strong>VSEPR theory<\/strong>.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-711.png\" alt=\"\" class=\"wp-image-198520\"\/><\/figure>\n\n\n\n<p>Here is the molecular structure of <strong>Sulfur Dioxide (SO\u2082)<\/strong>, showing its <strong>bent shape<\/strong> and <strong>~119\u00b0 bond angle<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Which Of The Following Triatomic Molecules Will Have A Bond Angles Closest To 120\u00b0? The correct answer and explanation is : Here are some common triatomic molecules: Correct Answer: SO\u2082 (Sulfur Dioxide) Explanation: The bond angle of a molecule depends on its molecular geometry, which is determined using VSEPR (Valence Shell Electron Pair Repulsion) Theory. [&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-198519","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198519","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=198519"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/198519\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=198519"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=198519"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=198519"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}