{"id":163597,"date":"2024-11-09T03:39:25","date_gmt":"2024-11-09T03:39:25","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=163597"},"modified":"2024-11-09T03:39:27","modified_gmt":"2024-11-09T03:39:27","slug":"what-is-the-molecular-shape-of-ocl2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/09\/what-is-the-molecular-shape-of-ocl2\/","title":{"rendered":"What is the molecular shape of OCl2"},"content":{"rendered":"\n<p>What is the molecular shape of OCl2<br>a) trigonal planar<br>b) trigonal pyramidal<br>c) linear<br>d) angular<br>e) tetrahedral<\/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>The correct molecular shape of <strong>OCl\u2082<\/strong> (oxygen dichloride) is <strong>angular<\/strong> (option <strong>d<\/strong>).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>To determine the molecular shape of a molecule like <strong>OCl\u2082<\/strong>, we need to consider the <strong>valence shell electron pair repulsion (VSEPR) theory<\/strong>, which helps predict the arrangement of atoms and lone pairs around a central atom.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Electron Configuration of Oxygen:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen (O) has 6 valence electrons, and each chlorine (Cl) atom has 7 valence electrons.<\/li>\n\n\n\n<li>When forming OCl\u2082, oxygen shares electrons with two chlorine atoms, resulting in two single bonds (O-Cl). This uses up two of oxygen&#8217;s valence electrons, leaving four electrons in the form of two lone pairs on the oxygen atom.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Electron Domain:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen in OCl\u2082 has two bonding pairs of electrons (from the O-Cl bonds) and two lone pairs of electrons.<\/li>\n\n\n\n<li>The total number of electron pairs around the oxygen atom is therefore <strong>4<\/strong> (2 bonding + 2 lone pairs).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Electron Geometry:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>With 4 electron pairs, the <strong>electron geometry<\/strong> around the oxygen atom is <strong>tetrahedral<\/strong>. This is based on the fact that the electron pairs want to be as far apart as possible to minimize repulsion, forming a tetrahedral arrangement.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Molecular Geometry:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>However, the <strong>molecular geometry<\/strong> describes only the arrangement of atoms, not the lone pairs.<\/li>\n\n\n\n<li>The presence of two lone pairs on oxygen will cause the molecule to adopt an <strong>angular<\/strong> (or bent) shape, which is similar to the geometry seen in water (H\u2082O), where two lone pairs also push the hydrogen atoms closer together.<\/li>\n\n\n\n<li>The bond angle in OCl\u2082 is less than 109.5\u00b0 due to the repulsion from the lone pairs.<\/li>\n<\/ul>\n\n\n\n<p>Thus, OCl\u2082 adopts an <strong>angular<\/strong> molecular shape, with a <strong>tetrahedral electron geometry<\/strong>. The correct answer is <strong>d) angular<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the molecular shape of OCl2a) trigonal planarb) trigonal pyramidalc) lineard) angulare) tetrahedral The Correct Answer and Explanation is : The correct molecular shape of OCl\u2082 (oxygen dichloride) is angular (option d). Explanation: To determine the molecular shape of a molecule like OCl\u2082, we need to consider the valence shell electron pair repulsion (VSEPR) [&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-163597","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/163597","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=163597"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/163597\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=163597"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=163597"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=163597"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}