{"id":182453,"date":"2025-01-13T20:01:20","date_gmt":"2025-01-13T20:01:20","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=182453"},"modified":"2025-01-13T20:01:23","modified_gmt":"2025-01-13T20:01:23","slug":"what-is-the-molecular-geometry-of-br3br3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/13\/what-is-the-molecular-geometry-of-br3br3\/","title":{"rendered":"What is the molecular geometry of Br3+Br3+"},"content":{"rendered":"\n<p>What is the molecular geometry of Br3+Br3+ ? bent T-shaped trigonal pyramidal tetrahedral linear<\/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<p>The correct molecular geometry of Br3+\\text{Br}_3^+ is <strong>T-shaped<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Valence Shell Electron Pair Repulsion (VSEPR) Theory<\/strong>: VSEPR theory helps predict molecular geometry by considering electron pair repulsion. The central bromine atom in Br3+\\text{Br}_3^+ is surrounded by bonding and lone pairs of electrons.<\/li>\n\n\n\n<li><strong>Electron Configuration<\/strong>: Bromine has 7 valence electrons. For Br3+\\text{Br}_3^+, the positive charge indicates one fewer electron, so we account for 20 valence electrons in total for the Br3+\\text{Br}_3^+ ion:\n<ul class=\"wp-block-list\">\n<li>7 electrons from each bromine atom (\u00d73) = 21<\/li>\n\n\n\n<li>Remove 1 electron for the positive charge = 20 total valence electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: The central bromine atom forms bonds with two terminal bromine atoms. These two bonds account for 4 electrons, leaving 16 electrons as lone pairs. Distribute these around the atoms to satisfy the octet rule:\n<ul class=\"wp-block-list\">\n<li>Each terminal bromine gets 3 lone pairs (12 electrons total).<\/li>\n\n\n\n<li>The central bromine gets 2 lone pairs (4 electrons).<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Electron Geometry<\/strong>: The central bromine has 5 regions of electron density (2 bonding pairs and 3 lone pairs). This corresponds to a trigonal bipyramidal <strong>electron geometry<\/strong>.<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Of the 5 regions of electron density, the 3 lone pairs occupy the equatorial positions to minimize repulsion. The 2 bonding pairs occupy axial positions, forming a <strong>T-shaped molecular geometry<\/strong>.<\/li>\n\n\n\n<li><strong>Conclusion<\/strong>: The Br3+\\text{Br}_3^+ ion adopts a T-shaped geometry due to the arrangement of bonding and lone pairs around the central bromine. This geometry minimizes electron repulsion while accommodating the lone pairs in the most stable configuration.<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"<p>What is the molecular geometry of Br3+Br3+ ? bent T-shaped trigonal pyramidal tetrahedral linear The correct answer and explanation is: The correct molecular geometry of Br3+\\text{Br}_3^+ is T-shaped. Explanation:<\/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-182453","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182453","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=182453"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/182453\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=182453"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=182453"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=182453"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}