{"id":256497,"date":"2025-07-16T09:49:53","date_gmt":"2025-07-16T09:49:53","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=256497"},"modified":"2025-07-16T09:49:56","modified_gmt":"2025-07-16T09:49:56","slug":"for-each-of-the-following-molecules-draw-a-lewis-structure","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/16\/for-each-of-the-following-molecules-draw-a-lewis-structure\/","title":{"rendered":"For each of the following molecules, draw a Lewis structure"},"content":{"rendered":"\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/image-475.png\" alt=\"\" class=\"wp-image-256498\"\/><\/figure>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>Let&#8217;s analyze each compound one by one with Lewis structures, molecular geometry, bond angles, hybridization, and polarity.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>a. SF\u2084<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: S is central with 4 single bonds to F and 1 lone pair.<\/li>\n\n\n\n<li><strong>Electron Groups<\/strong>: 5 (4 bonding + 1 lone pair)<\/li>\n\n\n\n<li><strong>Geometry<\/strong>: Seesaw<\/li>\n\n\n\n<li><strong>Bond Angles<\/strong>: Approximately 102\u00b0 (equatorial) and 173\u00b0 (axial)<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: sp\u00b3d<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar (asymmetrical shape causes dipole moment)<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>b. AlCl\u2084\u207b<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: Al is central with 4 single bonds to Cl; gains one electron to complete octet<\/li>\n\n\n\n<li><strong>Electron Groups<\/strong>: 4 (no lone pairs)<\/li>\n\n\n\n<li><strong>Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n<li><strong>Bond Angles<\/strong>: 109.5\u00b0<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: sp\u00b3<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar (symmetrical charge distribution)<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>c. SF\u2086<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: S is central with 6 single bonds to F<\/li>\n\n\n\n<li><strong>Electron Groups<\/strong>: 6 (no lone pairs)<\/li>\n\n\n\n<li><strong>Geometry<\/strong>: Octahedral<\/li>\n\n\n\n<li><strong>Bond Angles<\/strong>: 90\u00b0<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: sp\u00b3d\u00b2<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar (symmetrical)<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>d. POCl\u2083<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: P is central with double bond to O and single bonds to 3 Cl<\/li>\n\n\n\n<li><strong>Electron Groups<\/strong>: 4 (no lone pairs)<\/li>\n\n\n\n<li><strong>Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n<li><strong>Bond Angles<\/strong>: 109.5\u00b0<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: sp\u00b3<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar (due to differing atoms and dipole moments)<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>e. SOCl\u2082<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: S is central, double bond to O, single bonds to 2 Cl, and 1 lone pair<\/li>\n\n\n\n<li><strong>Electron Groups<\/strong>: 4 (3 bonding + 1 lone pair)<\/li>\n\n\n\n<li><strong>Geometry<\/strong>: Trigonal pyramidal<\/li>\n\n\n\n<li><strong>Bond Angles<\/strong>: Around 107\u00b0<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: sp\u00b3<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>f. IBr\u2082\u207a<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: I is central with 2 single bonds to Br and 2 lone pairs<\/li>\n\n\n\n<li><strong>Electron Groups<\/strong>: 4 (2 bonding + 2 lone pairs)<\/li>\n\n\n\n<li><strong>Geometry<\/strong>: Bent<\/li>\n\n\n\n<li><strong>Bond Angles<\/strong>: Less than 109.5\u00b0<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: sp\u00b3<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>g. IF\u2085<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: I is central with 5 single bonds to F and 1 lone pair<\/li>\n\n\n\n<li><strong>Electron Groups<\/strong>: 6 (5 bonding + 1 lone pair)<\/li>\n\n\n\n<li><strong>Geometry<\/strong>: Square pyramidal<\/li>\n\n\n\n<li><strong>Bond Angles<\/strong>: 90\u00b0 and &lt;90\u00b0<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: sp\u00b3d\u00b2<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p>Each structure involves determining electron domains, geometry, and molecular symmetry to predict polarity and hybridization accurately.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-635.jpeg\" alt=\"\" class=\"wp-image-256499\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The Correct Answer and Explanation is: Let&#8217;s analyze each compound one by one with Lewis structures, molecular geometry, bond angles, hybridization, and polarity. a. SF\u2084 b. AlCl\u2084\u207b c. SF\u2086 d. POCl\u2083 e. SOCl\u2082 f. IBr\u2082\u207a g. IF\u2085 Each structure involves determining electron domains, geometry, and molecular symmetry to predict polarity and hybridization accurately.<\/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-256497","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/256497","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=256497"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/256497\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=256497"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=256497"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=256497"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}