{"id":185153,"date":"2025-01-22T07:21:50","date_gmt":"2025-01-22T07:21:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185153"},"modified":"2025-01-22T07:21:52","modified_gmt":"2025-01-22T07:21:52","slug":"the-correct-lewis-structure-for-bf3-would-have-exactly","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/the-correct-lewis-structure-for-bf3-would-have-exactly\/","title":{"rendered":"The correct Lewis structure for BF3 would have exactly"},"content":{"rendered":"\n

The correct Lewis structure for BF3 would have exactly: no double bonds. O2 double bonds. 1 triple bond. 1 double bond<\/p>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The correct answer is “no double bonds.”<\/strong><\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

The Lewis structure of ( BF_3 ) (boron trifluoride) is drawn by distributing the valence electrons around boron and the three fluorine atoms. Here’s how it works:<\/p>\n\n\n\n

    \n
  1. Determine total valence electrons:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • Boron (( B )) has 3 valence electrons.<\/li>\n\n\n\n
    • Fluorine (( F )) has 7 valence electrons, and there are 3 fluorine atoms.<\/li>\n\n\n\n
    • Total valence electrons: ( 3 + (7 \\times 3) = 24 ).<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Form bonds:<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • Boron forms single covalent bonds with each of the three fluorine atoms. Each bond uses 2 electrons.<\/li>\n\n\n\n
        • Total electrons used in bonds: ( 3 \\times 2 = 6 ).<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Distribute remaining electrons:<\/strong><\/li>\n<\/ol>\n\n\n\n
              \n
            • After forming bonds, ( 24 – 6 = 18 ) electrons remain.<\/li>\n\n\n\n
            • These electrons are placed as lone pairs on the fluorine atoms, with each fluorine receiving 6 electrons (3 lone pairs), completing their octets.<\/li>\n<\/ul>\n\n\n\n
                \n
              1. Check boron’s octet:<\/strong><\/li>\n<\/ol>\n\n\n\n
                  \n
                • Boron has only 6 electrons around it (from three single bonds), which does not complete an octet.<\/li>\n\n\n\n
                • However, boron is an exception to the octet rule and is stable with only 6 valence electrons in this molecule.<\/li>\n<\/ul>\n\n\n\n
                    \n
                  1. No double or triple bonds:<\/strong><\/li>\n<\/ol>\n\n\n\n
                      \n
                    • Fluorine is highly electronegative and does not share additional electrons to form double bonds.<\/li>\n\n\n\n
                    • Boron lacks the necessary electrons to form multiple bonds.<\/li>\n<\/ul>\n\n\n\n

                      Thus, the correct Lewis structure for ( BF_3 ) has three single bonds<\/strong> and no double or triple bonds. Each fluorine atom has a full octet, and boron is stable despite having fewer than 8 electrons. The absence of double or triple bonds in ( BF_3 ) aligns with its actual molecular geometry, which is trigonal planar.<\/p>\n","protected":false},"excerpt":{"rendered":"

                      The correct Lewis structure for BF3 would have exactly: no double bonds. O2 double bonds. 1 triple bond. 1 double bond The Correct Answer and Explanation is : The correct answer is “no double bonds.” Explanation: The Lewis structure of ( BF_3 ) (boron trifluoride) is drawn by distributing the valence electrons around boron and […]<\/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-185153","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185153","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=185153"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185153\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185153"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185153"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185153"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}