{"id":216393,"date":"2025-05-19T07:38:10","date_gmt":"2025-05-19T07:38:10","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=216393"},"modified":"2025-05-19T07:38:12","modified_gmt":"2025-05-19T07:38:12","slug":"draw-the-lewis-structure-for-each-of-the-following-molecules-or-ions-and-predict-their-electron","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/19\/draw-the-lewis-structure-for-each-of-the-following-molecules-or-ions-and-predict-their-electron\/","title":{"rendered":"Draw the lewis structure for each of the following molecules or ions, and predict their electron"},"content":{"rendered":"\n<p class=\"wp-block-paragraph\">Draw the lewis structure for each of the following molecules or ions, and predict their electron<br>Draw the lewis structure for each of the following molecules or ions, and predict their electron domain and molecules geometries: Asf3, CH+3+, BrF3, CIO3-, XeF2, BrO2<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">\u00c3\u201a\u00c2<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">\u00c3\u201a\u00c2<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">\u00c3\u201a\u00c2<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Let&#8217;s examine the Lewis structures, <strong>electron-domain geometries<\/strong>, and <strong>molecular geometries<\/strong> of each of the given species: <strong>AsF\u2083<\/strong>, <strong>CH\u2083\u207a<\/strong>, <strong>BrF\u2083<\/strong>, <strong>ClO\u2083\u207b<\/strong>, <strong>XeF\u2082<\/strong>, and <strong>BrO\u2082<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>1. AsF\u2083 (Arsenic trifluoride)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>:<br>Arsenic (As) has 5 valence electrons. Each fluorine (F) contributes 7. Total: 5 + (3\u00d77) = 26 electrons.<br>Three single bonds with F (6 electrons), leaving 20 electrons \u2192 6 go on each F as lone pairs (18), remaining 2 on As as a lone pair.<\/li>\n\n\n\n<li><strong>Electron-Domain Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Trigonal pyramidal<\/li>\n\n\n\n<li><strong>Explanation<\/strong>: One lone pair on As causes a bent pyramidal shape, similar to NH\u2083.<\/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>2. CH\u2083\u207a (Methyl cation)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>:<br>Carbon (C) has 4 valence electrons, each H has 1. For CH\u2083: 4 + 3 = 7, subtract 1 (positive charge) = 6 electrons.<br>Three C\u2013H bonds (6 electrons). No lone pairs on carbon.<\/li>\n\n\n\n<li><strong>Electron-Domain Geometry<\/strong>: Trigonal planar<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Trigonal planar<\/li>\n\n\n\n<li><strong>Explanation<\/strong>: Carbon has only 3 bonding domains and no lone pair \u2014 flat triangular structure.<\/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>3. BrF\u2083 (Bromine trifluoride)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>:<br>Br has 7 valence electrons, each F has 7. Total: 7 + (3\u00d77) = 28 electrons.<br>Br forms 3 bonds with F (6 electrons), 3 lone pairs go to Fs (18), leaving 4 electrons \u2192 2 lone pairs on Br.<\/li>\n\n\n\n<li><strong>Electron-Domain Geometry<\/strong>: Trigonal bipyramidal<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: T-shaped<\/li>\n\n\n\n<li><strong>Explanation<\/strong>: Five domains (3 bonds + 2 lone pairs) give a trigonal bipyramidal EDG. Lone pairs occupy equatorial positions, leaving T-shaped geometry.<\/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>4. ClO\u2083\u207b (Chlorate ion)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>:<br>Cl = 7, O = 6\u00d73 = 18, plus 1 for negative charge \u2192 26 electrons.<br>One double bond and two single bonds (with formal charges minimized).<\/li>\n\n\n\n<li><strong>Electron-Domain Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Trigonal pyramidal<\/li>\n\n\n\n<li><strong>Explanation<\/strong>: Four domains (3 bonds, 1 lone pair) result in a trigonal pyramidal shape.<\/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>5. XeF\u2082 (Xenon difluoride)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>:<br>Xe = 8, F = 7\u00d72 = 14, total = 22 electrons.<br>Two Xe\u2013F bonds (4 electrons), 12 electrons on Fs, 6 on Xe \u2192 3 lone pairs.<\/li>\n\n\n\n<li><strong>Electron-Domain Geometry<\/strong>: Trigonal bipyramidal<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n<li><strong>Explanation<\/strong>: Lone pairs occupy equatorial positions; linear shape remains on axial 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\"><strong>6. BrO\u2082 (Bromine dioxide)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>:<br>Br = 7, O = 6\u00d72 = 12; total = 19 electrons \u2192 odd electron species (radical).<br>Likely has one double bond and one single bond with Br having a lone pair and one unpaired electron.<\/li>\n\n\n\n<li><strong>Electron-Domain Geometry<\/strong>: Trigonal planar<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Bent<\/li>\n\n\n\n<li><strong>Explanation<\/strong>: Three electron regions (2 bonds + 1 lone pair), gives a bent structure.<\/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\">Summary Table:<\/h3>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-fixed-layout\"><thead><tr><th>Species<\/th><th>Electron-Domain Geometry<\/th><th>Molecular Geometry<\/th><\/tr><\/thead><tbody><tr><td>AsF\u2083<\/td><td>Tetrahedral<\/td><td>Trigonal pyramidal<\/td><\/tr><tr><td>CH\u2083\u207a<\/td><td>Trigonal planar<\/td><td>Trigonal planar<\/td><\/tr><tr><td>BrF\u2083<\/td><td>Trigonal bipyramidal<\/td><td>T-shaped<\/td><\/tr><tr><td>ClO\u2083\u207b<\/td><td>Tetrahedral<\/td><td>Trigonal pyramidal<\/td><\/tr><tr><td>XeF\u2082<\/td><td>Trigonal bipyramidal<\/td><td>Linear<\/td><\/tr><tr><td>BrO\u2082<\/td><td>Trigonal planar<\/td><td>Bent (radical species)<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Final Notes:<\/h3>\n\n\n\n<p class=\"wp-block-paragraph\">The <strong>electron-domain geometry<\/strong> considers all electron regions (bonding and lone pairs), while the <strong>molecular geometry<\/strong> describes the actual shape considering only the atoms. Lone pairs distort the geometry by repelling bonded pairs more strongly than bonding pairs repel each other.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the lewis structure for each of the following molecules or ions, and predict their electronDraw the lewis structure for each of the following molecules or ions, and predict their electron domain and molecules geometries: Asf3, CH+3+, BrF3, CIO3-, XeF2, BrO2 \u00c3\u201a\u00c2 \u00c3\u201a\u00c2 \u00c3\u201a\u00c2 Let&#8217;s examine the Lewis structures, electron-domain geometries, and molecular geometries of [&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-216393","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/216393","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=216393"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/216393\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=216393"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=216393"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=216393"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}