{"id":226151,"date":"2025-06-04T21:48:13","date_gmt":"2025-06-04T21:48:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=226151"},"modified":"2025-06-04T21:48:15","modified_gmt":"2025-06-04T21:48:15","slug":"draw-a-lewis-diagram-for-ch","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/04\/draw-a-lewis-diagram-for-ch\/","title":{"rendered":"Draw a Lewis diagram for CH"},"content":{"rendered":"\n<p>Draw a Lewis diagram for CH<br>C<br>H. \u2022 Remember to include all valence lone pairs in your answer.<\/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<h3 class=\"wp-block-heading\">Correct Lewis Structure for <strong>CH\u2083CH\u2083<\/strong> (Ethane):<\/h3>\n\n\n\n<p>Let\u2019s first draw the <strong>Lewis structure<\/strong> of <strong>CH\u2083CH\u2083<\/strong>:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>      H   H\n       \\ \/\n   H - C - C - H\n       \/ \\\n      H   H\n<\/code><\/pre>\n\n\n\n<p>Each carbon atom (C) forms <strong>4 covalent bonds<\/strong> to satisfy the octet rule. Each hydrogen atom (H) forms <strong>1 single bond<\/strong> (as it only needs 2 electrons to be stable). In CH\u2083CH\u2083:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each C is bonded to <strong>three H atoms<\/strong> and <strong>one C atom<\/strong>.<\/li>\n\n\n\n<li>Each H is bonded to <strong>one C<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>There are <strong>no lone pairs<\/strong> on any of the atoms in this molecule.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-Step Explanation<\/h3>\n\n\n\n<p><strong>CH\u2083CH\u2083<\/strong>, commonly known as <strong>ethane<\/strong>, is a simple alkane made of <strong>carbon (C)<\/strong> and <strong>hydrogen (H)<\/strong> atoms. To draw its <strong>Lewis structure<\/strong>, follow these steps:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Count the total valence electrons:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has 4 valence electrons.<\/li>\n\n\n\n<li>Hydrogen (H) has 1 valence electron.<\/li>\n\n\n\n<li>There are 2 carbon atoms and 6 hydrogen atoms:\n<ul class=\"wp-block-list\">\n<li>Total = (2 \u00d7 4) + (6 \u00d7 1) = 8 + 6 = <strong>14 valence electrons<\/strong>.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Determine the central atoms:<\/strong>\n<ul class=\"wp-block-list\">\n<li>The two carbon atoms are central and bonded to each other.<\/li>\n\n\n\n<li>Each carbon is then surrounded by 3 hydrogen atoms.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Connect atoms with single bonds:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Each C\u2013H bond uses 2 electrons.<\/li>\n\n\n\n<li>Each C\u2013C bond uses 2 electrons.<\/li>\n\n\n\n<li>So, there are 6 C\u2013H bonds and 1 C\u2013C bond:\n<ul class=\"wp-block-list\">\n<li>Electrons used = (6 \u00d7 2) + (1 \u00d7 2) = 12 + 2 = <strong>14 electrons<\/strong>.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Check the octet rule:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Each carbon has 4 bonds (8 electrons): satisfies the octet rule.<\/li>\n\n\n\n<li>Each hydrogen has 1 bond (2 electrons): satisfies the duet rule.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Assign lone pairs:<\/strong>\n<ul class=\"wp-block-list\">\n<li>All 14 valence electrons are used in bonding.<\/li>\n\n\n\n<li>Therefore, there are <strong>no lone pairs<\/strong> on any atom in CH\u2083CH\u2083.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<p><strong>Conclusion:<\/strong><br>The Lewis structure of ethane (CH\u2083CH\u2083) features all atoms with complete outer shells, all bonds are single covalent bonds, and no lone pairs exist in this molecule. It\u2019s a typical saturated hydrocarbon (alkane).<\/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-banner5-95.jpeg\" alt=\"\" class=\"wp-image-226152\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw a Lewis diagram for CHCH. \u2022 Remember to include all valence lone pairs in your answer. The Correct Answer and Explanation is: Correct Lewis Structure for CH\u2083CH\u2083 (Ethane): Let\u2019s first draw the Lewis structure of CH\u2083CH\u2083: Each carbon atom (C) forms 4 covalent bonds to satisfy the octet rule. Each hydrogen atom (H) forms [&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-226151","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/226151","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=226151"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/226151\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=226151"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=226151"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=226151"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}