{"id":217533,"date":"2025-05-22T05:00:37","date_gmt":"2025-05-22T05:00:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=217533"},"modified":"2025-05-22T05:00:40","modified_gmt":"2025-05-22T05:00:40","slug":"raw-the-lewis-structure-for-ethylamine-ch3ch2nh2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/22\/raw-the-lewis-structure-for-ethylamine-ch3ch2nh2\/","title":{"rendered":"raw the Lewis structure For ethylamine (CH3CH2NH2)"},"content":{"rendered":"\n<p class=\"wp-block-paragraph\">raw the Lewis structure For ethylamine (CH3CH2NH2). (Assign lone pairs where appropriate.) l Marvin as @ Help I Edit drawing \u00a33 (b) Determine the number of nonbonding valence electrons present in a molecule of ethylamine (CH3CH2NH2). There are _ nonbonding valence electron(s) within a molecule of ethylamine. They all belong to the nitrogen atom.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><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\"><strong>Correct Answer:<\/strong><\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">There are <strong>2 nonbonding valence electrons<\/strong> in a molecule of ethylamine (CH\u2083CH\u2082NH\u2082), and <strong>they are located on the nitrogen atom<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation (300+ words):<\/strong><\/h3>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Ethylamine (CH\u2083CH\u2082NH\u2082)<\/strong> is an organic compound containing carbon (C), hydrogen (H), and nitrogen (N). To determine the number of nonbonding valence electrons, we first examine the <strong>Lewis structure<\/strong> and then focus on the <strong>electron configuration of nitrogen<\/strong>, the atom responsible for the lone pair.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 1: Draw the Lewis Structure of Ethylamine<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">Ethylamine consists of an ethyl group (CH\u2083CH\u2082\u2013) bonded to an amino group (\u2013NH\u2082). Here&#8217;s the step-by-step breakdown:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The first carbon (C1) is bonded to three hydrogen atoms and to the second carbon (C2).<\/li>\n\n\n\n<li>The second carbon (C2) is bonded to two hydrogen atoms and to a nitrogen atom.<\/li>\n\n\n\n<li>The nitrogen atom is bonded to two hydrogen atoms and to the second carbon (C2).<\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">So, the bonding structure looks like this:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>H   H   H   H   H\n |   |   |   |   |\nH\u2014C\u2014C\u2014N\u2014H\n       |\n       H<\/code><\/pre>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Each dash represents a shared pair of bonding electrons (a single covalent bond).<\/strong><\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 2: Valence Electrons and Bonding<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon has <strong>4 valence electrons<\/strong> and forms <strong>4 bonds<\/strong> (no lone pairs).<\/li>\n\n\n\n<li>Hydrogen has <strong>1 valence electron<\/strong> and forms <strong>1 bond<\/strong> (no lone pairs).<\/li>\n\n\n\n<li><strong>Nitrogen<\/strong> has <strong>5 valence electrons<\/strong>. In ethylamine, nitrogen forms <strong>three sigma bonds<\/strong>: one with carbon and two with hydrogen. This uses <strong>3 electrons<\/strong>, forming <strong>3 bonding pairs<\/strong>.<\/li>\n\n\n\n<li>The remaining <strong>2 valence electrons<\/strong> (1 pair) on nitrogen are <strong>nonbonding<\/strong>, also known as a <strong>lone pair<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 3: Nonbonding Electrons in the Molecule<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">Only the <strong>nitrogen atom<\/strong> carries a lone pair in ethylamine. The <strong>carbon and hydrogen atoms do not have nonbonding electrons<\/strong>, as all of their valence electrons are involved in bonding.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Conclusion<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">Therefore, <strong>ethylamine (CH\u2083CH\u2082NH\u2082)<\/strong> has <strong>only one lone pair of electrons<\/strong>, consisting of <strong>2 nonbonding valence electrons<\/strong>, and <strong>they reside entirely on the nitrogen atom<\/strong>. These nonbonding electrons are crucial for ethylamine\u2019s ability to act as a <strong>Lewis base<\/strong> in chemical reactions, especially in forming hydrogen bonds and donating electrons in nucleophilic attacks.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>raw the Lewis structure For ethylamine (CH3CH2NH2). (Assign lone pairs where appropriate.) l Marvin as @ Help I Edit drawing \u00a33 (b) Determine the number of nonbonding valence electrons present in a molecule of ethylamine (CH3CH2NH2). There are _ nonbonding valence electron(s) within a molecule of ethylamine. They all belong to the nitrogen atom. The [&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-217533","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/217533","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=217533"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/217533\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=217533"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=217533"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=217533"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}