{"id":186893,"date":"2025-01-26T11:46:19","date_gmt":"2025-01-26T11:46:19","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=186893"},"modified":"2025-01-26T11:46:22","modified_gmt":"2025-01-26T11:46:22","slug":"draw-the-lewis-structure-of-acetone","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/26\/draw-the-lewis-structure-of-acetone\/","title":{"rendered":"Draw the Lewis structure of acetone"},"content":{"rendered":"\n<p>Draw the Lewis structure of acetone, CH3COCH3 and chloroform, CHCl3 using correct bond angle relationships; include partial charges on each atom (if any). Show how these two molecules position themselves when next to each other and show the attraction using a dotted line. Answer questions? a) List the primary and secondary intermolecular forces (in the order of significance or strength) in acetone: <strong><em><strong><em>____<\/em><\/strong><\/em><\/strong> , <strong><em><strong><em>_____<\/em><\/strong><\/em><\/strong> b) Is acetone a polar or nonpolar molecule? <strong><em><strong><em>___<\/em><\/strong><\/em><\/strong> , c) Which is more polar, acetone or chloroform? <strong><em><strong><em>____<\/em><\/strong><\/em><\/strong> . d) Do you predict the ?Hsln for mixing acetone with chloroform to be positive (>0), negative<\/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<h3 class=\"wp-block-heading\">Lewis Structures and Intermolecular Interactions<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Acetone (CH3COCH3CH_3COCH_3)<\/strong>:\n<ul class=\"wp-block-list\">\n<li>The central carbon (C=O) is double-bonded to oxygen and single-bonded to two methyl groups (CH3CH_3).<\/li>\n\n\n\n<li>Oxygen is more electronegative, bearing a partial negative charge (\u03b4\u2212\\delta^-), while the carbonyl carbon bears a partial positive charge (\u03b4+\\delta^+).<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Chloroform (CHCl3CHCl_3)<\/strong>:\n<ul class=\"wp-block-list\">\n<li>The central carbon is bonded to one hydrogen atom and three chlorine atoms.<\/li>\n\n\n\n<li>Chlorine atoms are more electronegative than carbon and hydrogen, bearing partial negative charges (\u03b4\u2212\\delta^-), while carbon bears a partial positive charge (\u03b4+\\delta^+).<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Positioning of Acetone and Chloroform<\/strong>:\n<ul class=\"wp-block-list\">\n<li>Acetone and chloroform are positioned such that the partially negative oxygen atom in acetone (\u03b4\u2212\\delta^-) is attracted to the partially positive hydrogen atom (\u03b4+\\delta^+) in chloroform. This forms a <strong>hydrogen bond<\/strong>, which is represented by a dotted line.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Answering the Questions:<\/h3>\n\n\n\n<p><strong>a) Primary and Secondary Intermolecular Forces in Acetone:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Primary: <strong>Dipole-dipole interactions<\/strong> (due to the polar C=OC=O bond).<\/li>\n\n\n\n<li>Secondary: <strong>London dispersion forces<\/strong> (weak forces due to temporary dipoles).<\/li>\n<\/ul>\n\n\n\n<p><strong>b) Is acetone polar or nonpolar?<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Polar<\/strong>, because of the C=OC=O bond and asymmetric geometry.<\/li>\n<\/ul>\n\n\n\n<p><strong>c) Which is more polar, acetone or chloroform?<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Acetone<\/strong> is more polar because the C=OC=O bond contributes a stronger dipole moment compared to chloroform&#8217;s dipole-dipole interactions from its asymmetric distribution of C\u2212HC-H and C\u2212ClC-Cl bonds.<\/li>\n<\/ul>\n\n\n\n<p><strong>d) Prediction of \u0394Hsln\\Delta H_{\\text{sln}} for Acetone-Chloroform Mixing and Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Negative (&lt;0&lt; 0)<\/strong>, because acetone and chloroform form hydrogen bonds when mixed. These strong interactions release energy, making the mixing process exothermic.<\/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\">Explanation:<\/h3>\n\n\n\n<p>When acetone and chloroform mix, they form strong hydrogen bonds between the partially negative oxygen (\u03b4\u2212\\delta^-) in acetone and the partially positive hydrogen (\u03b4+\\delta^+) in chloroform. These hydrogen bonds represent a favorable interaction that lowers the overall energy of the system. Intermolecular forces in acetone are dominated by dipole-dipole interactions from the polar C=OC=O group, while chloroform\u2019s intermolecular forces primarily stem from dipole-dipole interactions and weak hydrogen bonding due to the C\u2212HC-H bond.<\/p>\n\n\n\n<p>Acetone, being more polar due to its C=OC=O group, forms stronger dipole interactions compared to chloroform. However, when mixed, the \u0394Hsln\\Delta H_{\\text{sln}} is negative because the energy released from forming hydrogen bonds between acetone and chloroform compensates for the energy required to overcome their original intermolecular forces. This results in a net exothermic process.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure of acetone, CH3COCH3 and chloroform, CHCl3 using correct bond angle relationships; include partial charges on each atom (if any). Show how these two molecules position themselves when next to each other and show the attraction using a dotted line. Answer questions? a) List the primary and secondary intermolecular forces (in 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-186893","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186893","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=186893"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186893\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=186893"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=186893"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=186893"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}