{"id":257734,"date":"2025-07-17T16:41:54","date_gmt":"2025-07-17T16:41:54","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=257734"},"modified":"2025-07-17T16:41:56","modified_gmt":"2025-07-17T16:41:56","slug":"draw-a-valid-lewis-structure-for-the-molecule-ch3no-in-which-there-are-no-nonzero-formal-charges-on-any-of-the-atoms","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/17\/draw-a-valid-lewis-structure-for-the-molecule-ch3no-in-which-there-are-no-nonzero-formal-charges-on-any-of-the-atoms\/","title":{"rendered":"Draw a valid Lewis structure for the molecule CH3NO in which there are no nonzero formal charges on any of the atoms."},"content":{"rendered":"\n<p>Draw a valid Lewis structure for the molecule CH3NO in which there are no nonzero formal charges on any of the atoms. This structure should not include any bonds between N and O.<\/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<p>To draw the Lewis structure for <strong>CH\u2083NO<\/strong> (formaldehyde oxime) where there are no nonzero formal charges on any of the atoms and without a bond between nitrogen and oxygen, follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">1. <strong>Count the total valence electrons:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C): 4 valence electrons (since C is in group 14).<\/li>\n\n\n\n<li>Hydrogen (H): 1 valence electron each, for 3 H atoms \u2192 3 electrons.<\/li>\n\n\n\n<li>Nitrogen (N): 5 valence electrons (since N is in group 15).<\/li>\n\n\n\n<li>Oxygen (O): 6 valence electrons (since O is in group 16).<\/li>\n<\/ul>\n\n\n\n<p><strong>Total valence electrons<\/strong> = 4 (C) + 3 (H) + 5 (N) + 6 (O) = <strong>18 valence electrons<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">2. <strong>Determine the skeleton structure:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon typically forms four bonds, so it will be the central atom.<\/li>\n\n\n\n<li>Hydrogen atoms will be attached to carbon, as carbon can only form single bonds.<\/li>\n\n\n\n<li>Nitrogen and oxygen will be attached to carbon, but we will not directly connect nitrogen and oxygen.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">3. <strong>Place atoms and connect them with single bonds:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Attach each hydrogen atom to the carbon atom.<\/li>\n\n\n\n<li>Attach nitrogen and oxygen atoms to the carbon atom via single bonds.<\/li>\n<\/ul>\n\n\n\n<p>The skeleton structure looks like this:<\/p>\n\n\n\n<p>H\u2014C\u2014N\u2014O<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">4. <strong>Distribute the electrons:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each bond represents 2 electrons. For 4 C\u2014H bonds (3 H atoms), we use 8 electrons.<\/li>\n\n\n\n<li>The C\u2014N and C\u2014O single bonds use 2 more electrons, making 10 electrons used so far.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">5. <strong>Complete the octets:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen needs 2 more electrons to complete its octet. Place these electrons as lone pairs on oxygen.<\/li>\n\n\n\n<li>Nitrogen needs 2 more electrons to complete its octet. Place these electrons as lone pairs on nitrogen.<\/li>\n<\/ul>\n\n\n\n<p>Now, there are <strong>18 total electrons<\/strong> used (8 for C\u2014H bonds, 2 for C\u2014N, 2 for C\u2014O, and 6 for lone pairs).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">6. <strong>Check for formal charges:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon: The formal charge is calculated by subtracting the number of bonds (4) and lone pairs (0) from the valence electrons (4), resulting in a formal charge of 0.<\/li>\n\n\n\n<li>Hydrogen: Each hydrogen has 1 bond, which is correct for its 1 valence electron, resulting in no formal charge on hydrogen.<\/li>\n\n\n\n<li>Nitrogen: Nitrogen has 1 bond to carbon and 2 lone pairs. This gives a formal charge of 0 (5 valence electrons minus 1 bond and 2 lone pairs).<\/li>\n\n\n\n<li>Oxygen: Oxygen has 1 bond to carbon and 3 lone pairs, giving a formal charge of 0 (6 valence electrons minus 1 bond and 3 lone pairs).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">7. <strong>Final structure:<\/strong><\/h3>\n\n\n\n<pre class=\"wp-block-preformatted\">mathematicaCopyEdit<code>H\u2014C\u2014N\u2014O\n  |     |\n  H     H\n  |\n  H\n<\/code><\/pre>\n\n\n\n<p>This structure has no formal charges on any atom and follows the given conditions.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-827.jpeg\" alt=\"\" class=\"wp-image-257737\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw a valid Lewis structure for the molecule CH3NO in which there are no nonzero formal charges on any of the atoms. This structure should not include any bonds between N and O. The Correct Answer and Explanation is: To draw the Lewis structure for CH\u2083NO (formaldehyde oxime) where there are no nonzero formal charges [&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-257734","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/257734","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=257734"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/257734\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=257734"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=257734"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=257734"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}