{"id":267071,"date":"2025-07-23T09:10:33","date_gmt":"2025-07-23T09:10:33","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=267071"},"modified":"2025-07-23T09:10:35","modified_gmt":"2025-07-23T09:10:35","slug":"what-is-the-electron-pair-geometry-for-br-in-brf5","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/23\/what-is-the-electron-pair-geometry-for-br-in-brf5\/","title":{"rendered":"What is the electron-pair geometry for Br in BrF5"},"content":{"rendered":"\n<p>What is the electron-pair geometry for Br in BrF5? <strong><em>_ There are<\/em><\/strong> lone pair(s) around the central atom, so the geometry of BrF5 is <strong><em>_ B. What is the electron-pair geometry for P in PCl6- ? There are lone pair(s) around the central atom, so the geometry of PCl6- is _<\/em><\/strong><\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>For <strong>Br in BrF5<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron-pair geometry:<\/strong> The central bromine atom in BrF5 is surrounded by five fluorine atoms and has one lone pair of electrons. This makes a total of six electron pairs around the bromine atom.<\/li>\n\n\n\n<li>The electron-pair geometry is based on six electron pairs, which results in an <strong>octahedral geometry<\/strong>.<\/li>\n\n\n\n<li><strong>Lone pairs:<\/strong> There is <strong>one lone pair<\/strong> on the bromine atom.<\/li>\n\n\n\n<li><strong>Molecular geometry:<\/strong> With five bonding pairs and one lone pair, the geometry of BrF5 is <strong>square pyramidal<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Explanation:<br>BrF5 is a molecule where bromine acts as the central atom and is surrounded by five fluorine atoms. The presence of a lone pair causes a distortion in the ideal octahedral geometry, giving it a square pyramidal shape. In an octahedral arrangement, the bond angles would ideally be 90\u00b0 and 180\u00b0, but the lone pair occupies one of the positions, thus altering the structure.<\/p>\n\n\n\n<p>For <strong>P in PCl6-<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron-pair geometry:<\/strong> The phosphorus atom in PCl6- is surrounded by six chlorine atoms, resulting in six electron pairs around the central phosphorus atom.<\/li>\n\n\n\n<li>The electron-pair geometry is <strong>octahedral<\/strong> because there are six bonding pairs of electrons.<\/li>\n\n\n\n<li><strong>Lone pairs:<\/strong> There are <strong>no lone pairs<\/strong> on the phosphorus atom, as all six positions are occupied by chlorine atoms.<\/li>\n\n\n\n<li><strong>Molecular geometry:<\/strong> The geometry of PCl6- is <strong>octahedral<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Explanation:<br>PCl6- is an example of a molecule where the central phosphorus atom is surrounded by six chlorine atoms in a symmetrical arrangement. Because there are no lone pairs on phosphorus, the geometry remains perfectly octahedral, with the chlorine atoms arranged at 90\u00b0 angles to each other and 180\u00b0 between opposite atoms.<\/p>\n\n\n\n<p>So, the answers are:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>For Br in BrF5: The electron-pair geometry is <strong>octahedral<\/strong>. There are <strong>one lone pair<\/strong> around the central atom, so the geometry of BrF5 is <strong>square pyramidal<\/strong>.<\/li>\n\n\n\n<li>For P in PCl6-: The electron-pair geometry is <strong>octahedral<\/strong>. There are <strong>no lone pairs<\/strong> around the central atom, so the geometry of PCl6- is <strong>octahedral<\/strong>.<\/li>\n<\/ul>\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-banner6-1655.jpeg\" alt=\"\" class=\"wp-image-267072\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>What is the electron-pair geometry for Br in BrF5? _ There are lone pair(s) around the central atom, so the geometry of BrF5 is _ B. What is the electron-pair geometry for P in PCl6- ? There are lone pair(s) around the central atom, so the geometry of PCl6- is _ The Correct Answer and [&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-267071","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267071","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=267071"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/267071\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=267071"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=267071"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=267071"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}