{"id":170162,"date":"2024-11-19T17:01:04","date_gmt":"2024-11-19T17:01:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=170162"},"modified":"2024-11-19T17:01:07","modified_gmt":"2024-11-19T17:01:07","slug":"draw-the-lewis-structure-and-predict-the-molecu-lar-geometry-of-the-following-molecules","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/19\/draw-the-lewis-structure-and-predict-the-molecu-lar-geometry-of-the-following-molecules\/","title":{"rendered":"Draw the Lewis structure and predict the molecu- lar geometry of the following molecules"},"content":{"rendered":"\n<p>Draw the Lewis structure and predict the molecu- lar geometry of the following molecules: a. SO2 b. CI4 c. BCl3<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>Let&#8217;s go over the Lewis structures and molecular geometries for the molecules: <strong>SO\u2082<\/strong>, <strong>CCl\u2084<\/strong>, and <strong>BCl\u2083<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">a) <strong>SO\u2082 (Sulfur Dioxide)<\/strong><\/h3>\n\n\n\n<p><strong>Step 1: Lewis Structure<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sulfur (S) is the central atom, with oxygen (O) atoms bonded to it.<\/li>\n\n\n\n<li>Sulfur has 6 valence electrons, and each oxygen has 6 valence electrons. SO\u2082 has 16 valence electrons in total (6 + 2 \u00d7 6 = 18).<\/li>\n\n\n\n<li>Draw a single bond between sulfur and each oxygen, and distribute the remaining electrons to satisfy the octet rule.<\/li>\n\n\n\n<li>A double bond is formed between sulfur and each oxygen to complete the octet for both oxygen atoms and satisfy sulfur&#8217;s requirement for 12 valence electrons (octet expanded in sulfur).<\/li>\n<\/ul>\n\n\n\n<p>The Lewis structure will be:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>O = S = O<\/code><\/pre>\n\n\n\n<p><strong>Step 2: Molecular Geometry<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>In SO\u2082, the sulfur atom has two bonding pairs of electrons and one lone pair. The electron pairs around the sulfur will arrange themselves to minimize repulsion.<\/li>\n\n\n\n<li>This results in a <strong>bent<\/strong> molecular geometry with a bond angle of approximately <strong>120\u00b0<\/strong>, characteristic of a molecule with <strong>sp\u00b2 hybridization<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">b) <strong>CCl\u2084 (Carbon Tetrachloride)<\/strong><\/h3>\n\n\n\n<p><strong>Step 1: Lewis Structure<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) is the central atom, with chlorine (Cl) atoms bonded to it.<\/li>\n\n\n\n<li>Carbon has 4 valence electrons, and each chlorine atom has 7 valence electrons. CCl\u2084 has 32 valence electrons in total (4 + 4 \u00d7 7 = 32).<\/li>\n\n\n\n<li>Form single bonds between carbon and each chlorine atom and place the remaining electrons as lone pairs on the chlorine atoms.<\/li>\n<\/ul>\n\n\n\n<p>The Lewis structure will be:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>     Cl\n     |\nCl - C - Cl\n     |\n     Cl<\/code><\/pre>\n\n\n\n<p><strong>Step 2: Molecular Geometry<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>In CCl\u2084, carbon has four bonding pairs of electrons and no lone pairs. These bonding pairs will arrange themselves in a way that minimizes repulsion, forming a <strong>tetrahedral<\/strong> geometry with bond angles of <strong>109.5\u00b0<\/strong>.<\/li>\n\n\n\n<li>The carbon atom is <strong>sp\u00b3 hybridized<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">c) <strong>BCl\u2083 (Boron Trichloride)<\/strong><\/h3>\n\n\n\n<p><strong>Step 1: Lewis Structure<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Boron (B) is the central atom, with chlorine (Cl) atoms bonded to it.<\/li>\n\n\n\n<li>Boron has 3 valence electrons, and each chlorine atom has 7 valence electrons. BCl\u2083 has 24 valence electrons in total (3 + 3 \u00d7 7 = 24).<\/li>\n\n\n\n<li>Form single bonds between boron and each chlorine atom, and place the remaining electrons as lone pairs on chlorine.<\/li>\n<\/ul>\n\n\n\n<p>The Lewis structure will be:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>     Cl\n     |\nCl - B - Cl<\/code><\/pre>\n\n\n\n<p><strong>Step 2: Molecular Geometry<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>In BCl\u2083, boron has three bonding pairs of electrons and no lone pairs. These bonding pairs will arrange themselves to minimize repulsion, resulting in a <strong>trigonal planar<\/strong> molecular geometry with bond angles of <strong>120\u00b0<\/strong>.<\/li>\n\n\n\n<li>The boron atom is <strong>sp\u00b2 hybridized<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Summary of Molecular Geometries:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>SO\u2082<\/strong>: Bent (120\u00b0), sp\u00b2 hybridization.<\/li>\n\n\n\n<li><strong>CCl\u2084<\/strong>: Tetrahedral (109.5\u00b0), sp\u00b3 hybridization.<\/li>\n\n\n\n<li><strong>BCl\u2083<\/strong>: Trigonal planar (120\u00b0), sp\u00b2 hybridization.<\/li>\n<\/ul>\n\n\n\n<p>Each molecule follows the general rules of the Valence Shell Electron Pair Repulsion (VSEPR) theory, predicting the geometry based on the electron pairs around the central atom.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure and predict the molecu- lar geometry of the following molecules: a. SO2 b. CI4 c. BCl3 The Correct Answer and Explanation is: Let&#8217;s go over the Lewis structures and molecular geometries for the molecules: SO\u2082, CCl\u2084, and BCl\u2083. a) SO\u2082 (Sulfur Dioxide) Step 1: Lewis Structure The Lewis structure will be: [&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-170162","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/170162","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=170162"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/170162\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=170162"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=170162"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=170162"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}