{"id":202228,"date":"2025-03-17T09:36:50","date_gmt":"2025-03-17T09:36:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=202228"},"modified":"2025-03-17T09:36:52","modified_gmt":"2025-03-17T09:36:52","slug":"draw-the-lewis-structure-of-co-in-its-best-resonance-form","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/17\/draw-the-lewis-structure-of-co-in-its-best-resonance-form\/","title":{"rendered":"Draw the Lewis structure of CO in its best resonance form"},"content":{"rendered":"\n<p>Draw the Lewis structure of CO in its best resonance form. Include all unshared electrons in your drawing.<\/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 best resonance form of carbon monoxide (CO) has a triple bond between the carbon and oxygen atoms, with a lone pair on each atom. The Lewis structure is as follows:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>:C\u2261O:<\/code><\/pre>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-Step Explanation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Count the Valence Electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has 4 valence electrons.<\/li>\n\n\n\n<li>Oxygen (O) has 6 valence electrons.<\/li>\n\n\n\n<li>Total valence electrons = 4 + 6 = <strong>10 electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Determine the Bonding<\/strong>:<br>Since carbon and oxygen are bonded together, we arrange them with at least a single bond and distribute the remaining electrons. However, a single bond would not satisfy the octet rule for both atoms.<\/li>\n\n\n\n<li><strong>Create a Triple Bond<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>To satisfy the octet rule, carbon and oxygen form a <strong>triple bond (one sigma and two pi bonds)<\/strong>.<\/li>\n\n\n\n<li>Carbon donates one of its lone pairs to form a coordinate covalent bond, resulting in a formal charge on both atoms.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Assign Formal Charges<\/strong>:<br>Formal charge is calculated using:<br>[<br>\\text{Formal Charge} = \\text{Valence Electrons} &#8211; \\text{Nonbonding Electrons} &#8211; \\frac{\\text{Bonding Electrons}}{2}<br>]<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Carbon<\/strong>: (4 &#8211; 2 &#8211; \\frac{6}{2} = -1) \u2192 <strong>Negative charge<\/strong><\/li>\n\n\n\n<li><strong>Oxygen<\/strong>: (6 &#8211; 4 &#8211; \\frac{6}{2} = +1) \u2192 <strong>Positive charge<\/strong><\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Final Structure<\/strong>:<br>The best resonance form has a triple bond with a <strong>negative charge on carbon<\/strong> and a <strong>positive charge on oxygen<\/strong>:<\/li>\n<\/ol>\n\n\n\n<pre class=\"wp-block-code\"><code>   :C\u2261O:\n     -   +<\/code><\/pre>\n\n\n\n<ol start=\"6\" class=\"wp-block-list\">\n<li><strong>Why This is the Best Form<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>It satisfies the <strong>octet rule<\/strong> for both atoms.<\/li>\n\n\n\n<li>The <strong>formal charges are minimal<\/strong>, and carbon (less electronegative) holds the negative charge.<\/li>\n\n\n\n<li>Other structures (double bond or single bond forms) would lead to incomplete octets or higher formal charges.<\/li>\n<\/ul>\n\n\n\n<p>Thus, this Lewis structure represents CO\u2019s most stable resonance form.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure of CO in its best resonance form. Include all unshared electrons in your drawing. The correct answer and explanation is : The best resonance form of carbon monoxide (CO) has a triple bond between the carbon and oxygen atoms, with a lone pair on each atom. The Lewis structure is as [&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-202228","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/202228","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=202228"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/202228\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=202228"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=202228"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=202228"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}