{"id":183890,"date":"2025-01-17T08:04:22","date_gmt":"2025-01-17T08:04:22","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=183890"},"modified":"2025-01-17T08:04:24","modified_gmt":"2025-01-17T08:04:24","slug":"gebr4-cbr2h2-sif4-ccl4-xecl2-sih2br2-chbr3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/17\/gebr4-cbr2h2-sif4-ccl4-xecl2-sih2br2-chbr3\/","title":{"rendered":"GeBr4, CBr2H2, SiF4, CCl4, XeCl2, SiH2Br2, CHBr3"},"content":{"rendered":"\n<p>GeBr4, CBr2H2, SiF4, CCl4, XeCl2, SiH2Br2, CHBr3 -Total number of valence Electrons -The Lewis Structure -The total regions of electrons -Number of bonding regions of electrons, -The shape -And if they are polar or not?<\/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>Let&#8217;s analyze each compound step by step.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">1. <strong>GeBr\u2084<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons<\/strong>: Ge (4) + 4\u00d7Br (4\u00d77) = 32.<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Ge in the center with 4 single bonds to Br atoms, each Br having 3 lone pairs.<\/li>\n\n\n\n<li><strong>Total Regions of Electrons<\/strong>: 4 (all bonding pairs).<\/li>\n\n\n\n<li><strong>Bonding Regions<\/strong>: 4.<\/li>\n\n\n\n<li><strong>Shape<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar (symmetrical bond dipoles cancel out).<\/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\">2. <strong>CBr\u2082H\u2082<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons<\/strong>: C (4) + 2\u00d7Br (2\u00d77) + 2\u00d7H (2\u00d71) = 20.<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: C in the center, single bonds to 2 Br atoms and 2 H atoms.<\/li>\n\n\n\n<li><strong>Total Regions of Electrons<\/strong>: 4 (all bonding pairs).<\/li>\n\n\n\n<li><strong>Bonding Regions<\/strong>: 4.<\/li>\n\n\n\n<li><strong>Shape<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar (Br creates stronger dipoles compared to H).<\/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\">3. <strong>SiF\u2084<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons<\/strong>: Si (4) + 4\u00d7F (4\u00d77) = 32.<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Si in the center with 4 single bonds to F atoms, each F having 3 lone pairs.<\/li>\n\n\n\n<li><strong>Total Regions of Electrons<\/strong>: 4 (all bonding pairs).<\/li>\n\n\n\n<li><strong>Bonding Regions<\/strong>: 4.<\/li>\n\n\n\n<li><strong>Shape<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar (symmetrical bond dipoles cancel out).<\/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\">4. <strong>CCl\u2084<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons<\/strong>: C (4) + 4\u00d7Cl (4\u00d77) = 32.<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: C in the center with 4 single bonds to Cl atoms, each Cl having 3 lone pairs.<\/li>\n\n\n\n<li><strong>Total Regions of Electrons<\/strong>: 4 (all bonding pairs).<\/li>\n\n\n\n<li><strong>Bonding Regions<\/strong>: 4.<\/li>\n\n\n\n<li><strong>Shape<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar (symmetrical bond dipoles cancel out).<\/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\">5. <strong>XeCl\u2082<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons<\/strong>: Xe (8) + 2\u00d7Cl (2\u00d77) = 22.<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Xe in the center with 2 single bonds to Cl atoms and 3 lone pairs.<\/li>\n\n\n\n<li><strong>Total Regions of Electrons<\/strong>: 5 (2 bonding pairs + 3 lone pairs).<\/li>\n\n\n\n<li><strong>Bonding Regions<\/strong>: 2.<\/li>\n\n\n\n<li><strong>Shape<\/strong>: Linear.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar (symmetrical bond dipoles cancel out).<\/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\">6. <strong>SiH\u2082Br\u2082<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons<\/strong>: Si (4) + 2\u00d7H (2\u00d71) + 2\u00d7Br (2\u00d77) = 20.<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Si in the center with single bonds to 2 H atoms and 2 Br atoms.<\/li>\n\n\n\n<li><strong>Total Regions of Electrons<\/strong>: 4 (all bonding pairs).<\/li>\n\n\n\n<li><strong>Bonding Regions<\/strong>: 4.<\/li>\n\n\n\n<li><strong>Shape<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar (Br creates stronger dipoles compared to H).<\/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\">7. <strong>CHBr\u2083<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons<\/strong>: C (4) + H (1) + 3\u00d7Br (3\u00d77) = 26.<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: C in the center with single bonds to H and 3 Br atoms.<\/li>\n\n\n\n<li><strong>Total Regions of Electrons<\/strong>: 4 (all bonding pairs).<\/li>\n\n\n\n<li><strong>Bonding Regions<\/strong>: 4.<\/li>\n\n\n\n<li><strong>Shape<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar (Br creates strong dipoles compared to H).<\/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 (300 words):<\/h3>\n\n\n\n<p>The molecular geometry and polarity of a compound depend on the number of valence electrons, bonding regions, lone pairs, and electronegativity. Using the VSEPR (Valence Shell Electron Pair Repulsion) theory, molecules with 4 electron regions around the central atom (like GeBr\u2084, SiF\u2084, and CCl\u2084) form a tetrahedral shape, minimizing electron pair repulsions.<\/p>\n\n\n\n<p>Symmetry plays a key role in polarity. For instance, symmetrical tetrahedrals like GeBr\u2084 and CCl\u2084 are nonpolar because bond dipoles cancel. However, molecules with different atoms bonded to the central atom (e.g., CBr\u2082H\u2082 or SiH\u2082Br\u2082) tend to be polar as dipoles do not cancel due to differing electronegativities.<\/p>\n\n\n\n<p>In linear structures like XeCl\u2082, the symmetry of bond dipoles (Cl atoms on opposite sides) ensures nonpolarity. Conversely, in molecules like CHBr\u2083, asymmetry leads to a polar molecule.<\/p>\n\n\n\n<p>Understanding these principles helps predict molecular properties, interactions, and behavior in chemical reactions.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>GeBr4, CBr2H2, SiF4, CCl4, XeCl2, SiH2Br2, CHBr3 -Total number of valence Electrons -The Lewis Structure -The total regions of electrons -Number of bonding regions of electrons, -The shape -And if they are polar or not? The Correct Answer and Explanation is : Let&#8217;s analyze each compound step by step. 1. GeBr\u2084 2. CBr\u2082H\u2082 3. SiF\u2084 [&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-183890","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183890","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=183890"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183890\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183890"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183890"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183890"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}