{"id":203383,"date":"2025-03-19T17:00:14","date_gmt":"2025-03-19T17:00:14","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203383"},"modified":"2025-03-19T17:00:19","modified_gmt":"2025-03-19T17:00:19","slug":"what-is-the-lewis-structure-for-brf2-and-the-number-of-valence","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/19\/what-is-the-lewis-structure-for-brf2-and-the-number-of-valence\/","title":{"rendered":"what is the lewis structure for BrF2+ and the number of valence"},"content":{"rendered":"\n

what is the lewis structure for BrF2+ and the number of valence<\/p>\n\n\n\n

The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n

Lewis Structure of BrF\u2082\u207a and Valence Electrons Calculation<\/strong><\/h3>\n\n\n\n

Valence Electrons Calculation:<\/strong><\/h4>\n\n\n\n
    \n
  1. Bromine (Br) Contribution:<\/strong> Bromine belongs to Group 17 and has 7 valence electrons<\/strong>.<\/li>\n\n\n\n
  2. Fluorine (F) Contribution:<\/strong> Each fluorine atom also belongs to Group 17 and has 7 valence electrons<\/strong>. Since there are two fluorine atoms<\/strong>, the total contribution from fluorine is 2 \u00d7 7 = 14 valence electrons<\/strong>.<\/li>\n\n\n\n
  3. Cation (+1) Effect:<\/strong> Since BrF\u2082\u207a has a +1 charge<\/strong>, it means one electron is lost from the total count.<\/li>\n<\/ol>\n\n\n\n

    Total valence electrons calculation:<\/strong> 7(Br)+(2\u00d77)(F)\u22121(for +1 charge)=7+14\u22121=20 valence electrons.7 (Br) + (2 \\times 7) (F) – 1 (\\text{for +1 charge}) = 7 + 14 – 1 = 20 \\text{ valence electrons}.<\/p>\n\n\n\n

    Lewis Structure Construction:<\/strong><\/h4>\n\n\n\n
      \n
    1. Central Atom Selection:<\/strong> Bromine is less electronegative than fluorine, so it is the central atom<\/strong>.<\/li>\n\n\n\n
    2. Bonding:<\/strong> Two fluorine atoms are bonded to bromine via single bonds<\/strong>. This uses up 2 \u00d7 2 = 4 electrons<\/strong>.<\/li>\n\n\n\n
    3. Remaining Electrons:<\/strong> After bonding, 16 electrons<\/strong> remain.<\/li>\n\n\n\n
    4. Lone Pairs Assignment:<\/strong>\n
        \n
      • Fluorine atoms need 3 lone pairs<\/strong> each (total 2 \u00d7 6 = 12 electrons<\/strong>).<\/li>\n\n\n\n
      • The remaining 4 electrons<\/strong> are placed as two lone pairs<\/strong> on bromine.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

        Molecular Geometry & Formal Charge:<\/strong><\/h4>\n\n\n\n
          \n
        • Formal Charge Calculation:<\/strong>\n
            \n
          • Br:<\/strong> 7\u2212(4+2)=+17 – (4 + 2) = +1<\/li>\n\n\n\n
          • F:<\/strong> 7\u2212(6+1)=07 – (6 + 1) = 0<\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Structure Shape:<\/strong> Bent (T-Shaped)<\/strong> due to lone pairs and the AX\u2082E\u2083 arrangement (based on VSEPR theory).<\/li>\n<\/ul>\n\n\n\n

            Now, generating the image for the Lewis structure of BrF\u2082\u207a<\/strong>:<\/p>\n\n\n\n

            Here is the Lewis structure of BrF\u2082\u207a. The diagram shows bromine in the center with two fluorine atoms bonded via single bonds, two lone pairs on bromine, and a +1 charge indicated. The molecular geometry follows a T-shape due to the electron repulsions. Let me know if you need further explanations!<\/p>\n\n\n\n

            \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

            what is the lewis structure for BrF2+ and the number of valence The correct answer and explanation is: Lewis Structure of BrF\u2082\u207a and Valence Electrons Calculation Valence Electrons Calculation: Total valence electrons calculation: 7(Br)+(2\u00d77)(F)\u22121(for +1 charge)=7+14\u22121=20 valence electrons.7 (Br) + (2 \\times 7) (F) – 1 (\\text{for +1 charge}) = 7 + 14 – 1 = 20 \\text{ valence […]<\/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-203383","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203383","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=203383"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203383\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=203383"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=203383"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=203383"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}