{"id":168776,"date":"2024-11-18T10:21:00","date_gmt":"2024-11-18T10:21:00","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=168776"},"modified":"2024-11-18T10:21:09","modified_gmt":"2024-11-18T10:21:09","slug":"draw-a-lewis-structure-for-each-covalent-molecule","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/18\/draw-a-lewis-structure-for-each-covalent-molecule\/","title":{"rendered":"Draw a Lewis structure for each covalent molecule."},"content":{"rendered":"\n<p>Draw a Lewis structure for each covalent molecule. a. CH3F b. N2H4<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>Let&#8217;s draw and explain the Lewis structures for the given covalent molecules: <strong>CH\u2083F<\/strong> (methyl fluoride) and <strong>N\u2082H\u2084<\/strong> (hydrazine).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">a. <strong>CH\u2083F (Methyl Fluoride)<\/strong><\/h3>\n\n\n\n<p><strong>Step 1: Count the valence electrons.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has 4 valence electrons.<\/li>\n\n\n\n<li>Each hydrogen (H) atom has 1 valence electron, and there are 3 hydrogens, contributing 3 electrons.<\/li>\n\n\n\n<li>Fluorine (F) has 7 valence electrons.<\/li>\n<\/ul>\n\n\n\n<p>Total valence electrons = 4 (C) + 3(1 H) + 7 (F) = 14 electrons.<\/p>\n\n\n\n<p><strong>Step 2: Draw the skeletal structure.<\/strong><br>Carbon is the central atom (it can form four bonds), with three hydrogen atoms and one fluorine atom bonded to it.<\/p>\n\n\n\n<p><strong>Step 3: Distribute the electrons.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon will form single bonds with each of the three hydrogen atoms and the fluorine atom. This accounts for 4 bonds, each using 2 electrons.<\/li>\n\n\n\n<li>The remaining electrons (14 total &#8211; 8 used for bonds) will be placed as lone pairs on the fluorine atom.<\/li>\n<\/ul>\n\n\n\n<p><strong>Step 4: Check for octet rule.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has 4 bonds, which gives it 8 electrons (satisfied octet).<\/li>\n\n\n\n<li>Hydrogen atoms each have 2 electrons (satisfied duet rule).<\/li>\n\n\n\n<li>Fluorine has 3 lone pairs and one bond, which gives it 8 electrons (satisfied octet).<\/li>\n<\/ul>\n\n\n\n<p>The Lewis structure of <strong>CH\u2083F<\/strong> is:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>     H\n     |\nH\u2014C\u2014F\n     |\n     H<\/code><\/pre>\n\n\n\n<h3 class=\"wp-block-heading\">b. <strong>N\u2082H\u2084 (Hydrazine)<\/strong><\/h3>\n\n\n\n<p><strong>Step 1: Count the valence electrons.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each nitrogen (N) atom has 5 valence electrons, and there are 2 nitrogen atoms, contributing 10 electrons.<\/li>\n\n\n\n<li>Each hydrogen (H) atom has 1 valence electron, and there are 4 hydrogens, contributing 4 electrons.<\/li>\n<\/ul>\n\n\n\n<p>Total valence electrons = 10 (N) + 4 (H) = 14 electrons.<\/p>\n\n\n\n<p><strong>Step 2: Draw the skeletal structure.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The two nitrogen atoms will be connected by a single bond.<\/li>\n\n\n\n<li>Each nitrogen atom will form single bonds with two hydrogen atoms.<\/li>\n<\/ul>\n\n\n\n<p><strong>Step 3: Distribute the electrons.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The nitrogen-nitrogen single bond uses 2 electrons.<\/li>\n\n\n\n<li>Each nitrogen-hydrogen bond uses 2 electrons, accounting for 8 electrons in total for the bonds.<\/li>\n\n\n\n<li>The remaining 4 electrons will be placed as lone pairs on the nitrogen atoms.<\/li>\n<\/ul>\n\n\n\n<p><strong>Step 4: Check for octet rule.<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each nitrogen atom will have 2 single bonds with hydrogen and a single bond to the other nitrogen. Each nitrogen has 8 electrons in total (6 from bonds and 2 from lone pairs), satisfying the octet rule.<\/li>\n\n\n\n<li>Each hydrogen atom has 2 electrons, fulfilling the duet rule.<\/li>\n<\/ul>\n\n\n\n<p>The Lewis structure of <strong>N\u2082H\u2084<\/strong> is:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>H\u2014N\u2014N\u2014H\n     |\n     H\n     |\n     H<\/code><\/pre>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>In <strong>CH\u2083F<\/strong>, carbon bonds to three hydrogens and one fluorine atom, with fluorine having lone pairs to complete its octet.<\/li>\n\n\n\n<li>In <strong>N\u2082H\u2084<\/strong>, each nitrogen bonds to two hydrogens and the other nitrogen, with lone pairs completing the nitrogen octets.<\/li>\n<\/ul>\n\n\n\n<p>Both molecules satisfy the octet (or duet for hydrogen) rule, making the structures stable.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw a Lewis structure for each covalent molecule. a. CH3F b. N2H4 The Correct Answer and Explanation is: Let&#8217;s draw and explain the Lewis structures for the given covalent molecules: CH\u2083F (methyl fluoride) and N\u2082H\u2084 (hydrazine). a. CH\u2083F (Methyl Fluoride) Step 1: Count the valence electrons. Total valence electrons = 4 (C) + 3(1 H) [&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-168776","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/168776","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=168776"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/168776\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=168776"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=168776"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=168776"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}