{"id":203020,"date":"2025-03-18T16:28:29","date_gmt":"2025-03-18T16:28:29","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203020"},"modified":"2025-03-18T16:28:31","modified_gmt":"2025-03-18T16:28:31","slug":"c2h5n","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/18\/c2h5n\/","title":{"rendered":"C2H5N"},"content":{"rendered":"\n<p>C2H5N<\/p>\n\n\n\n<p>a) Draw Lewis Structure with lines<\/p>\n\n\n\n<p>b) Molecular Geometry (VSEPR) sketch and bond angles. Show resultant polarity, if applicable<\/p>\n\n\n\n<p>c) State the central atom<\/p>\n\n\n\n<p>d) State the number of single, double and triple bonds, lone pairs and pi bonds<\/p>\n\n\n\n<p>e) State hybridization of central atom<\/p>\n\n\n\n<p>f) Names of electron arrangement and of molecular geometry<\/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>Let&#8217;s break down the molecule <strong>C2H5N<\/strong>, which is an <strong>ethylamine<\/strong> (also called <strong>ethanamine<\/strong>). Here is the step-by-step breakdown of your questions:<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">a) <strong>Lewis Structure with Lines:<\/strong><\/h3>\n\n\n\n<p>To draw the Lewis structure of C2H5N (Ethylamine):<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Count valence electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has 4 valence electrons \u00d7 2 (for two carbons) = 8<\/li>\n\n\n\n<li>Hydrogen (H) has 1 valence electron \u00d7 5 (for five hydrogens) = 5<\/li>\n\n\n\n<li>Nitrogen (N) has 5 valence electrons \u00d7 1 (for one nitrogen) = 5<\/li>\n\n\n\n<li>Total: 8 (C) + 5 (H) + 5 (N) = 18 valence electrons<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Structure<\/strong>:<br>The two carbon atoms (C) are bonded by a single bond. Each carbon atom is bonded to hydrogen atoms. The nitrogen (N) is bonded to the second carbon atom with a single bond and also has a lone pair of electrons. Here&#8217;s the structure:<\/li>\n<\/ol>\n\n\n\n<pre class=\"wp-block-code\"><code>   H   H\n   |   |\n   H-C-C-N-H\n       |\n       H<\/code><\/pre>\n\n\n\n<p>The bonds are:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>C-C: single bond<\/li>\n\n\n\n<li>C-H: single bonds<\/li>\n\n\n\n<li>N-H: single bonds<\/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\">b) <strong>Molecular Geometry (VSEPR)<\/strong> and <strong>Bond Angles<\/strong>:<\/h3>\n\n\n\n<p>The molecule <strong>C2H5N<\/strong> consists of a <strong>C-C<\/strong> chain with an <strong>NH2<\/strong> group attached to the second carbon. The nitrogen (N) is the central atom in this structure.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Central atom<\/strong>: Nitrogen (N)<\/li>\n\n\n\n<li><strong>Electron pairs around nitrogen<\/strong>: Nitrogen has one lone pair and forms three single bonds with carbon and hydrogen atoms.<\/li>\n\n\n\n<li><strong>Geometry of Nitrogen (N)<\/strong>: Since nitrogen has three bonding pairs and one lone pair, the geometry around nitrogen is <strong>trigonal pyramidal<\/strong>. The bond angles are <strong>less than 109.5\u00b0<\/strong> (around 107\u00b0).<\/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\">c) <strong>Central Atom<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The <strong>central atom<\/strong> in this molecule is <strong>Nitrogen (N)<\/strong>. It is directly bonded to the second carbon in the ethyl group and has a lone pair of electrons.<\/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\">d) <strong>Bonds, Lone Pairs, and Pi Bonds<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Single Bonds<\/strong>:<\/li>\n\n\n\n<li>C-H (5 bonds)<\/li>\n\n\n\n<li>C-C (1 bond)<\/li>\n\n\n\n<li>C-N (1 bond)<\/li>\n\n\n\n<li>N-H (2 bonds)<\/li>\n\n\n\n<li><strong>Double Bonds<\/strong>: None<\/li>\n\n\n\n<li><strong>Triple Bonds<\/strong>: None<\/li>\n\n\n\n<li><strong>Lone Pairs<\/strong>: Nitrogen has 1 lone pair of electrons.<\/li>\n\n\n\n<li><strong>Pi Bonds<\/strong>: None (All bonds are sigma bonds in this molecule).<\/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\">e) <strong>Hybridization of Central Atom<\/strong>:<\/h3>\n\n\n\n<p>The central atom is <strong>Nitrogen (N)<\/strong>. Since it has three sigma bonds and one lone pair, the hybridization of nitrogen is <strong>sp\u00b3<\/strong>. This hybridization leads to the <strong>trigonal pyramidal<\/strong> molecular geometry.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">f) <strong>Electron Arrangement and Molecular Geometry Names<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron Arrangement<\/strong>: The electron geometry around nitrogen is <strong>tetrahedral<\/strong> because it has four regions of electron density (three bonds and one lone pair).<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: The actual molecular geometry (considering only the positions of the atoms) is <strong>trigonal pyramidal<\/strong> due to the presence of one lone pair on nitrogen.<\/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\">300-Word Explanation:<\/h3>\n\n\n\n<p>Ethylamine (C2H5N) is a simple organic molecule with a nitrogen atom bonded to an ethyl group (C2H5). The molecule&#8217;s Lewis structure reveals a central nitrogen atom bonded to two hydrogen atoms and one carbon atom, with a lone pair of electrons on nitrogen. The molecule follows the basic principles of bonding and electron configuration.<\/p>\n\n\n\n<p>To determine the molecular geometry, we use <strong>VSEPR (Valence Shell Electron Pair Repulsion)<\/strong> theory. The nitrogen atom is the central atom in this molecule and has three single bonds (to two hydrogens and one carbon) and one lone pair of electrons. According to VSEPR, regions of electron density around a central atom arrange themselves to minimize repulsion. In this case, the nitrogen atom has four regions of electron density: three bonding pairs and one lone pair. This leads to a <strong>tetrahedral<\/strong> electron geometry. However, because the lone pair is not visible in the molecular structure, the <strong>molecular geometry<\/strong> is described as <strong>trigonal pyramidal<\/strong>.<\/p>\n\n\n\n<p>The bond angles around nitrogen are slightly less than 109.5\u00b0, typically around 107\u00b0, due to the lone pair occupying more space than the bonding pairs. The molecule is polar due to the presence of the lone pair on nitrogen, which creates an unequal distribution of charge, with the nitrogen end being slightly negative and the hydrogen end being slightly positive. The <strong>sp\u00b3 hybridization<\/strong> of nitrogen contributes to the tetrahedral electron arrangement, and the trigonal pyramidal geometry reflects the molecular structure after accounting for the lone pair.<\/p>\n\n\n\n<p>Thus, ethylamine has a <strong>polar<\/strong> molecular structure with a <strong>trigonal pyramidal<\/strong> geometry, resulting in a dipole moment.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>C2H5N a) Draw Lewis Structure with lines b) Molecular Geometry (VSEPR) sketch and bond angles. Show resultant polarity, if applicable c) State the central atom d) State the number of single, double and triple bonds, lone pairs and pi bonds e) State hybridization of central atom f) Names of electron arrangement and of molecular geometry [&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-203020","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203020","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=203020"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203020\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=203020"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=203020"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=203020"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}