{"id":222401,"date":"2025-05-31T10:06:16","date_gmt":"2025-05-31T10:06:16","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=222401"},"modified":"2025-05-31T10:06:19","modified_gmt":"2025-05-31T10:06:19","slug":"what-is-the-electron-pair-geometry-for-be-in-becl2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/31\/what-is-the-electron-pair-geometry-for-be-in-becl2\/","title":{"rendered":"What is the electron pair geometry for Be in BeCl2"},"content":{"rendered":"\n<p>A. What is the electron pair geometry for Be in BeCl2? <em><br>There are<\/em> lone pair(s) around the central atom, so the geometry of BeCl2 is <strong>_<\/strong><\/p>\n\n\n\n<p>B. What is the electron pair geometry for P in POCl3?<\/p>\n\n\n\n<p>There are <strong><em>_ lone pairs around the central atom, so the geometry of POCl3 is __<\/em><\/strong><\/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>A.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Electron pair geometry for Be in BeCl\u2082: <strong>Linear<\/strong><\/li>\n\n\n\n<li>There are <strong>0<\/strong> lone pair(s) around the central atom, so the geometry of BeCl\u2082 is <strong>Linear<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>B.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Electron pair geometry for P in POCl\u2083: <strong>Tetrahedral<\/strong><\/li>\n\n\n\n<li>There are <strong>0<\/strong> lone pairs around the central atom, so the geometry of POCl\u2083 is <strong>Tetrahedral<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>To determine molecular geometry, we use the <strong>Valence Shell Electron Pair Repulsion (VSEPR)<\/strong> theory, which predicts the spatial arrangement of atoms based on repulsions between electron pairs around a central atom.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">A. <strong>BeCl\u2082 (Beryllium Dichloride):<\/strong><\/h4>\n\n\n\n<p>Beryllium (Be) is the central atom, bonded to two chlorine (Cl) atoms. Be has 2 valence electrons and forms two single bonds with Cl atoms, using up all its valence electrons. Importantly, <strong>beryllium does not follow the octet rule<\/strong> \u2014 it is stable with only 4 electrons. Since there are <strong>no lone pairs<\/strong> on Be, the two bonding electron pairs repel each other and move as far apart as possible, resulting in a <strong>linear<\/strong> geometry with a bond angle of <strong>180\u00b0<\/strong>.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Electron domains: 2 (both bonding)<\/li>\n\n\n\n<li>Lone pairs on Be: 0<\/li>\n\n\n\n<li>Electron pair geometry: Linear<\/li>\n\n\n\n<li>Molecular geometry: Linear<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\">B. <strong>POCl\u2083 (Phosphoryl Chloride):<\/strong><\/h4>\n\n\n\n<p>Phosphorus (P) is the central atom bonded to one oxygen (double bond) and three chlorine atoms (single bonds). This gives a total of 4 regions of electron density around phosphorus: one double bond and three single bonds. Each double or single bond counts as <strong>one<\/strong> electron domain in VSEPR theory. There are <strong>no lone pairs<\/strong> on phosphorus.<\/p>\n\n\n\n<p>With 4 electron domains and no lone pairs, the electron pair geometry is <strong>tetrahedral<\/strong>. Since all electron domains are bonding and there are no lone pairs to distort the shape, the <strong>molecular geometry is also tetrahedral<\/strong>, with bond angles close to <strong>109.5\u00b0<\/strong>.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Electron domains: 4 (1 double bond, 3 single bonds)<\/li>\n\n\n\n<li>Lone pairs on P: 0<\/li>\n\n\n\n<li>Electron pair geometry: Tetrahedral<\/li>\n\n\n\n<li>Molecular geometry: Tetrahedral<\/li>\n<\/ul>\n\n\n\n<p>These geometries determine physical properties like polarity and molecular interactions, which are vital in chemical reactivity and function.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner4-202.jpeg\" alt=\"\" class=\"wp-image-222402\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>A. What is the electron pair geometry for Be in BeCl2? There are lone pair(s) around the central atom, so the geometry of BeCl2 is _ B. What is the electron pair geometry for P in POCl3? There are _ lone pairs around the central atom, so the geometry of POCl3 is __ The Correct [&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-222401","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222401","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=222401"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222401\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=222401"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=222401"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=222401"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}