{"id":227874,"date":"2025-06-06T14:49:23","date_gmt":"2025-06-06T14:49:23","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=227874"},"modified":"2025-06-06T14:49:25","modified_gmt":"2025-06-06T14:49:25","slug":"draw-the-lewis-structure-of-ch2cl2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/06\/draw-the-lewis-structure-of-ch2cl2\/","title":{"rendered":"Draw the lewis structure of CH2Cl2."},"content":{"rendered":"\n<p>Draw the lewis structure of CH2Cl2. include all lone pairs<\/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<h3 class=\"wp-block-heading\">Lewis Structure of CH\u2082Cl\u2082 (Dichloromethane)<\/h3>\n\n\n\n<p>Here&#8217;s the Lewis structure of <strong>CH\u2082Cl\u2082<\/strong>:<\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">markdownCopyEdit<code>       H\n       |\nCl \u2014 C \u2014 H\n       |\n      Cl\n<\/code><\/pre>\n\n\n\n<p>Now, let&#8217;s include <strong>all lone pairs<\/strong>:<\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">makefileCopyEdit<code>       H\n       |\n:Cl:\u2014 C \u2014 H\n       |\n     :Cl:\n<\/code><\/pre>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Carbon (C)<\/strong> has <strong>4 valence electrons<\/strong> and forms <strong>4 bonds<\/strong>: two single bonds with hydrogen atoms and two single bonds with chlorine atoms.<\/li>\n\n\n\n<li>Each <strong>Hydrogen (H)<\/strong> has <strong>1 valence electron<\/strong> and forms <strong>1 single bond<\/strong> (no lone pairs).<\/li>\n\n\n\n<li>Each <strong>Chlorine (Cl)<\/strong> has <strong>7 valence electrons<\/strong>. In the molecule, each chlorine shares one electron with carbon (a single bond), and retains <strong>3 lone pairs<\/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>The <strong>Lewis structure<\/strong> of <strong>CH\u2082Cl\u2082 (dichloromethane)<\/strong> helps us understand how atoms are bonded and where electrons are located within the molecule. First, we count the total number of <strong>valence electrons<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C): 4 valence electrons<\/li>\n\n\n\n<li>Hydrogen (H): 1 \u00d7 2 = 2 valence electrons<\/li>\n\n\n\n<li>Chlorine (Cl): 7 \u00d7 2 = 14 valence electrons<\/li>\n\n\n\n<li><strong>Total<\/strong> = 4 + 2 + 14 = <strong>20 valence electrons<\/strong><\/li>\n<\/ul>\n\n\n\n<p>Next, we arrange the atoms. Since carbon is the central atom (it\u2019s the least electronegative among non-hydrogen atoms and can form 4 bonds), it connects to 2 hydrogen atoms and 2 chlorine atoms.<\/p>\n\n\n\n<p>We form single bonds (each 2 electrons) between carbon and each of the other atoms:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>4 single bonds = 4 \u00d7 2 = 8 electrons used<\/li>\n<\/ul>\n\n\n\n<p>Now we distribute the remaining electrons (20 &#8211; 8 = <strong>12 electrons<\/strong>) as lone pairs:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Hydrogen atoms have no lone pairs (only 1 bond each)<\/li>\n\n\n\n<li>Chlorine atoms need <strong>3 lone pairs each<\/strong> to complete their octets (6 electrons per Cl)<\/li>\n\n\n\n<li>So: 2 Cl \u00d7 6 = 12 electrons used as lone pairs<\/li>\n<\/ul>\n\n\n\n<p>Carbon has 4 bonds (8 shared electrons), so it obeys the <strong>octet rule<\/strong>. Each chlorine atom has a complete octet (1 bond + 3 lone pairs = 8 electrons). Hydrogens have 2 electrons each, fulfilling their duet requirement.<\/p>\n\n\n\n<p>This structure reflects the correct bonding and lone pairs for each atom, making it the valid Lewis structure for CH\u2082Cl\u2082.<\/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-banner4-535.jpeg\" alt=\"\" class=\"wp-image-227875\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw the lewis structure of CH2Cl2. include all lone pairs The Correct Answer and Explanation is: Lewis Structure of CH\u2082Cl\u2082 (Dichloromethane) Here&#8217;s the Lewis structure of CH\u2082Cl\u2082: markdownCopyEdit H | Cl \u2014 C \u2014 H | Cl Now, let&#8217;s include all lone pairs: makefileCopyEdit H | :Cl:\u2014 C \u2014 H | :Cl: Explanation 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 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-227874","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227874","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=227874"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227874\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=227874"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=227874"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=227874"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}