{"id":211930,"date":"2025-05-05T12:07:46","date_gmt":"2025-05-05T12:07:46","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=211930"},"modified":"2025-05-05T12:07:48","modified_gmt":"2025-05-05T12:07:48","slug":"draw-the-best-lewis-structure-for-ch2f2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/05\/draw-the-best-lewis-structure-for-ch2f2\/","title":{"rendered":"Draw the best Lewis structure for CH2F2"},"content":{"rendered":"\n<p>Draw the best Lewis structure for CH2F2. Which of the following is\/are true? Select all that apply.<\/p>\n\n\n\n<p>CHF2 is nonpolar<br>There are dispersion forces between two CH2F2 molecules<br>There are dipole-dipole forces between two CH2F2 molecules<br>There is hydrogen bonding between two CH2F2 molecules<br>The strongest intermolecular force between two CH2F2 molecules is ion-dipole forces<br>CHF2 should have a lower boiling point than CH4<br>The molecular geometry for CH2F2 is tetrahedral<\/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>To analyze <strong>CH\u2082F\u2082 (difluoromethane)<\/strong>, let\u2019s first draw its <strong>Lewis structure<\/strong> and evaluate its properties.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Lewis Structure of CH\u2082F\u2082:<\/strong><\/h3>\n\n\n\n<p>Carbon (C) is the central atom:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon forms 4 single bonds: 2 with H atoms, and 2 with F atoms.<\/li>\n\n\n\n<li>Each H has 1 bond (full shell).<\/li>\n\n\n\n<li>Each F has 3 lone pairs (6 electrons) and 1 bond to C.<\/li>\n<\/ul>\n\n\n\n<p>So, the structure looks like:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>    H\n    |\nF - C - F\n    |\n    H<\/code><\/pre>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Molecular Geometry:<\/strong><\/h3>\n\n\n\n<p>Using <strong>VSEPR theory<\/strong>, CH\u2082F\u2082 has 4 bonding regions and no lone pairs on carbon, resulting in a <strong>tetrahedral<\/strong> geometry.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Polarity:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Fluorine<\/strong> is much more electronegative than hydrogen, so the <strong>C\u2013F<\/strong> bonds are strongly polar.<\/li>\n\n\n\n<li>The molecule is not symmetrical because the F atoms are not evenly distributed around the carbon.<\/li>\n\n\n\n<li><strong>Dipoles do not cancel out<\/strong>, so <strong>CH\u2082F\u2082 is polar<\/strong>.<\/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\"><strong>Intermolecular Forces:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Dispersion forces<\/strong>: Always present in all molecules.<\/li>\n\n\n\n<li><strong>Dipole-dipole forces<\/strong>: Present due to polarity.<\/li>\n\n\n\n<li><strong>Hydrogen bonding<\/strong>: Requires H bonded to N, O, or F <strong>within the same molecule<\/strong>, which CH\u2082F\u2082 lacks. So, <strong>no hydrogen bonding between molecules<\/strong>.<\/li>\n\n\n\n<li><strong>Ion-dipole forces<\/strong>: Occur between ions and polar molecules\u2014not applicable here since CH\u2082F\u2082 is neutral.<\/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\"><strong>Boiling Point Comparison (CH\u2082F\u2082 vs CH\u2084):<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>CH\u2084 (methane)<\/strong> is nonpolar, has only dispersion forces, and a very low boiling point (\u2212161\u00b0C).<\/li>\n\n\n\n<li><strong>CH\u2082F\u2082<\/strong> is polar with dipole-dipole interactions \u2192 <strong>higher boiling point<\/strong> than CH\u2084.<\/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\">\u2705 <strong>Correct Statements:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\u2705 There are <strong>dispersion forces<\/strong> between two CH\u2082F\u2082 molecules.<\/li>\n\n\n\n<li>\u2705 There are <strong>dipole-dipole forces<\/strong> between two CH\u2082F\u2082 molecules.<\/li>\n\n\n\n<li>\u2705 The <strong>molecular geometry for CH\u2082F\u2082 is tetrahedral<\/strong>.<\/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\">\u274c <strong>Incorrect Statements:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>\u274c <strong>CHF\u2082 is nonpolar<\/strong> \u2192 CH\u2082F\u2082 is <strong>polar<\/strong>.<\/li>\n\n\n\n<li>\u274c <strong>There is hydrogen bonding<\/strong> \u2192 No H bonded to O\/N\/F in this context.<\/li>\n\n\n\n<li>\u274c <strong>Strongest force is ion-dipole<\/strong> \u2192 No ions present.<\/li>\n\n\n\n<li>\u274c <strong>CHF\u2082 has lower boiling point than CH\u2084<\/strong> \u2192 CH\u2082F\u2082 has a <strong>higher<\/strong> boiling point.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n","protected":false},"excerpt":{"rendered":"<p>Draw the best Lewis structure for CH2F2. Which of the following is\/are true? Select all that apply. CHF2 is nonpolarThere are dispersion forces between two CH2F2 moleculesThere are dipole-dipole forces between two CH2F2 moleculesThere is hydrogen bonding between two CH2F2 moleculesThe strongest intermolecular force between two CH2F2 molecules is ion-dipole forcesCHF2 should have a lower [&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-211930","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/211930","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=211930"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/211930\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=211930"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=211930"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=211930"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}