{"id":231602,"date":"2025-06-11T08:25:59","date_gmt":"2025-06-11T08:25:59","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=231602"},"modified":"2025-06-11T08:26:02","modified_gmt":"2025-06-11T08:26:02","slug":"what-is-the-formal-charge-on-each-atom-in-cbr2f2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/11\/what-is-the-formal-charge-on-each-atom-in-cbr2f2\/","title":{"rendered":"What is the formal charge on each atom in CBr2F2"},"content":{"rendered":"\n<p>What is the formal charge on each atom in CBr2F2? a. C = 0, Br = 0, F = 0 b. C = 0, Br = -1, F = +1 c. C = 0, Br = +1, F = -1 d. C = -2, Br = +1, F = +1 e. C = +4, Br = -1, F = -1<\/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>The correct answer is <strong>a. C = 0, Br = 0, F = 0<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Formal charge is a concept used in chemistry to determine the distribution of electrons within a molecule. It helps assess whether atoms bear extra electrons or have lost electrons in a covalent bonding arrangement. The formal charge (FCFC) on an atom is calculated using the formula:<\/p>\n\n\n\n<p>FC=Valence&nbsp;electrons\u2212Nonbonding&nbsp;electrons\u2212Bonding&nbsp;electrons2FC = \\text{Valence electrons} &#8211; \\text{Nonbonding electrons} &#8211; \\frac{\\text{Bonding electrons}}{2}<\/p>\n\n\n\n<p>For <strong>carbon (C)<\/strong> in <strong>CBr\u2082F\u2082<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon has <strong>4 valence electrons<\/strong>.<\/li>\n\n\n\n<li>It forms <strong>four single bonds<\/strong> (two with bromine and two with fluorine).<\/li>\n\n\n\n<li>Carbon does <strong>not have nonbonding electrons<\/strong>.<\/li>\n\n\n\n<li>Bonding electrons = <strong>8<\/strong> (four single bonds, each containing two electrons).<\/li>\n<\/ul>\n\n\n\n<p>FC=4\u22120\u221282=0FC = 4 &#8211; 0 &#8211; \\frac{8}{2} = 0<\/p>\n\n\n\n<p>For <strong>bromine (Br)<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Bromine belongs to Group 17 and has <strong>7 valence electrons<\/strong>.<\/li>\n\n\n\n<li>In this molecule, each bromine atom forms a <strong>single bond<\/strong> with carbon.<\/li>\n\n\n\n<li>Bromine has <strong>six nonbonding electrons<\/strong> (three lone pairs).<\/li>\n\n\n\n<li>Bonding electrons = <strong>2<\/strong> (one single bond).<\/li>\n<\/ul>\n\n\n\n<p>FC=7\u22126\u221222=0FC = 7 &#8211; 6 &#8211; \\frac{2}{2} = 0<\/p>\n\n\n\n<p>For <strong>fluorine (F)<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Fluorine also belongs to Group 17 and has <strong>7 valence electrons<\/strong>.<\/li>\n\n\n\n<li>It forms a <strong>single bond<\/strong> with carbon.<\/li>\n\n\n\n<li>Fluorine retains <strong>six nonbonding electrons<\/strong>.<\/li>\n\n\n\n<li>Bonding electrons = <strong>2<\/strong> (one single bond).<\/li>\n<\/ul>\n\n\n\n<p>FC=7\u22126\u221222=0FC = 7 &#8211; 6 &#8211; \\frac{2}{2} = 0<\/p>\n\n\n\n<p>Since all atoms have a formal charge of <strong>zero<\/strong>, CBr\u2082F\u2082 is a neutral molecule with a stable electron distribution. The formal charge analysis confirms that <strong>option (a) is correct<\/strong>.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner4-927.jpeg\" alt=\"\" class=\"wp-image-231603\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>What is the formal charge on each atom in CBr2F2? a. C = 0, Br = 0, F = 0 b. C = 0, Br = -1, F = +1 c. C = 0, Br = +1, F = -1 d. C = -2, Br = +1, F = +1 e. C = +4, Br [&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-231602","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231602","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=231602"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/231602\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=231602"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=231602"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=231602"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}