{"id":238284,"date":"2025-06-18T03:58:45","date_gmt":"2025-06-18T03:58:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=238284"},"modified":"2025-06-18T03:58:48","modified_gmt":"2025-06-18T03:58:48","slug":"what-is-the-molecular-geometry-of-the-compound-ash3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/18\/what-is-the-molecular-geometry-of-the-compound-ash3\/","title":{"rendered":"What is the molecular geometry of the compound AsH3"},"content":{"rendered":"\n<p>What is the molecular geometry of the compound AsH3?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The molecular geometry of <strong>arsine (AsH\u2083)<\/strong> is <strong>trigonal pyramidal<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Arsine (AsH\u2083) consists of one arsenic (As) atom bonded to three hydrogen (H) atoms. To determine the molecular geometry, we use <strong>Valence Shell Electron Pair Repulsion (VSEPR) theory<\/strong>.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Valence electrons<\/strong>:\n<ul class=\"wp-block-list\">\n<li>Arsenic is in group 15, so it has 5 valence electrons.<\/li>\n\n\n\n<li>Each hydrogen contributes 1 electron, and there are 3 hydrogen atoms.<\/li>\n\n\n\n<li>Total valence electrons = 5 (As) + 3(1) = 8 electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Electron regions around the central atom (As)<\/strong>:\n<ul class=\"wp-block-list\">\n<li>Three bonding pairs (each with one hydrogen atom)<\/li>\n\n\n\n<li>One lone pair of electrons on the arsenic atom<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<p>This makes a total of <strong>four electron regions<\/strong> around arsenic. According to VSEPR theory, four regions of electron density arrange themselves in a <strong>tetrahedral electron geometry<\/strong> to minimize repulsion. However, because one of these regions is a <strong>lone pair<\/strong> rather than a bonding pair, the shape of the molecule is no longer perfectly tetrahedral.<\/p>\n\n\n\n<ol start=\"3\" class=\"wp-block-list\">\n<li><strong>Molecular geometry<\/strong>:\n<ul class=\"wp-block-list\">\n<li>When one of the four regions is a lone pair, the molecular shape becomes <strong>trigonal pyramidal<\/strong>.<\/li>\n\n\n\n<li>The three hydrogen atoms form the base of a pyramid, and the lone pair occupies the top position, pushing the hydrogen atoms slightly closer together.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Bond angle and influence of lone pair<\/strong>:\n<ul class=\"wp-block-list\">\n<li>The ideal bond angle for a tetrahedral geometry is about 109.5 degrees.<\/li>\n\n\n\n<li>However, lone pairs exert more repulsion than bonding pairs. This causes the H-As-H bond angle in AsH\u2083 to shrink slightly, typically to around <strong>91 to 93 degrees<\/strong>.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<p>In conclusion, although AsH\u2083 has a tetrahedral electron geometry due to four regions of electron density, its <strong>molecular geometry<\/strong> is <strong>trigonal pyramidal<\/strong> due to the presence of a lone pair on the central arsenic atom.<\/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-banner5-699.jpeg\" alt=\"\" class=\"wp-image-238285\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>What is the molecular geometry of the compound AsH3? The Correct Answer and Explanation is: The molecular geometry of arsine (AsH\u2083) is trigonal pyramidal. Explanation: Arsine (AsH\u2083) consists of one arsenic (As) atom bonded to three hydrogen (H) atoms. To determine the molecular geometry, we use Valence Shell Electron Pair Repulsion (VSEPR) theory. This makes [&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-238284","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/238284","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=238284"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/238284\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=238284"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=238284"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=238284"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}