{"id":203310,"date":"2025-03-19T05:05:24","date_gmt":"2025-03-19T05:05:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203310"},"modified":"2025-03-19T05:05:26","modified_gmt":"2025-03-19T05:05:26","slug":"provide-the-lewis-structure-and-molecular-geometry-as-predicted-by-vsepr","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/19\/provide-the-lewis-structure-and-molecular-geometry-as-predicted-by-vsepr\/","title":{"rendered":"Provide the Lewis structure and molecular geometry as predicted by VSEPR"},"content":{"rendered":"\n<p>Provide the Lewis structure and molecular geometry as predicted by VSEPR (with solution) of<br>the following:<br>(a) Xenon dichloride, XeCl2<\/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<h3 class=\"wp-block-heading\"><strong>Lewis Structure and Molecular Geometry of Xenon Dichloride (XeCl\u2082)<\/strong><\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 1: Determine the Total Valence Electrons<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Xenon (Xe) is a noble gas in Group 18 with <strong>8 valence electrons<\/strong>.<\/li>\n\n\n\n<li>Chlorine (Cl) is in Group 17, and each chlorine atom has <strong>7 valence electrons<\/strong>.<\/li>\n\n\n\n<li>Since there are two chlorine atoms, their total contribution is <strong>2 \u00d7 7 = 14<\/strong> valence electrons.<\/li>\n\n\n\n<li>The total number of valence electrons in <strong>XeCl\u2082<\/strong> is:<br>[<br>8 + 14 = 22 \\text{ valence electrons}<br>]<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 2: Draw the Skeletal Structure<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Xenon (Xe) is the central atom because it is the least electronegative element.<\/li>\n\n\n\n<li>Two chlorine (Cl) atoms are attached to Xe via single bonds.<\/li>\n\n\n\n<li>Each single bond accounts for <strong>2 electrons<\/strong>, so <strong>2 \u00d7 2 = 4<\/strong> electrons are used for bonding.<\/li>\n\n\n\n<li>The remaining <strong>22 &#8211; 4 = 18<\/strong> electrons are placed as lone pairs on Xe and Cl.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 3: Assign Lone Pairs<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each Cl needs <strong>8 valence electrons<\/strong> (octet rule). Since each Cl is already bonded to Xe (2 electrons), it needs <strong>6 more electrons<\/strong> as lone pairs.<\/li>\n\n\n\n<li>Placing <strong>3 lone pairs (6 electrons) on each Cl<\/strong> satisfies their octet.<\/li>\n\n\n\n<li>After assigning 6 electrons to each Cl, <strong>6 electrons remain<\/strong>, which are placed as <strong>three lone pairs on Xe<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Thus, the <strong>Lewis structure<\/strong> of <strong>XeCl\u2082<\/strong> consists of:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Xenon (Xe) at the center with <strong>three lone pairs<\/strong>.<\/li>\n\n\n\n<li>Two chlorine (Cl) atoms each having <strong>three lone pairs<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 4: Determine Molecular Geometry Using VSEPR Theory<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron domains:<\/strong> Xenon has <strong>five electron domains<\/strong> (two bonding pairs and three lone pairs).<\/li>\n\n\n\n<li><strong>VSEPR Shape Prediction:<\/strong><\/li>\n\n\n\n<li>According to the <strong>AX\u2082E\u2083<\/strong> notation, <strong>XeCl\u2082<\/strong> adopts a <strong>linear molecular geometry<\/strong> because lone pairs arrange themselves to minimize electron repulsion.<\/li>\n\n\n\n<li>The lone pairs on Xe are positioned <strong>equatorially<\/strong>, and the bonding pairs (Cl-Xe-Cl) are positioned <strong>axially<\/strong> in a <strong>trigonal bipyramidal electron geometry<\/strong>, but the molecular shape is <strong>linear<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Final Answer:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure:<\/strong> Xe with three lone pairs and single bonds to two Cl atoms.<\/li>\n\n\n\n<li><strong>Molecular Geometry:<\/strong> <strong>Linear<\/strong> (bond angle \u2248 <strong>180\u00b0<\/strong>).<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Provide the Lewis structure and molecular geometry as predicted by VSEPR (with solution) ofthe following:(a) Xenon dichloride, XeCl2 The correct answer and explanation is : Lewis Structure and Molecular Geometry of Xenon Dichloride (XeCl\u2082) Step 1: Determine the Total Valence Electrons Step 2: Draw the Skeletal Structure Step 3: Assign Lone Pairs Thus, the Lewis [&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 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