{"id":249626,"date":"2025-07-09T18:04:53","date_gmt":"2025-07-09T18:04:53","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=249626"},"modified":"2025-07-09T18:04:55","modified_gmt":"2025-07-09T18:04:55","slug":"what-is-the-electron-pair-geometry-for-s-in-sof4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/09\/what-is-the-electron-pair-geometry-for-s-in-sof4\/","title":{"rendered":"What is the electron-pair geometry for S in SOF4"},"content":{"rendered":"\n

A. What is the electron-pair geometry for S in SOF4? _ There are <\/em><\/strong>lone pair(s) around the central atom, so the molecular geometry (shape) of SOF4 is B. What is the electron-pair geometry for Cl in ClF5? <\/strong><\/em>There are lone pair(s) around the central atom, so the molecular geometry (shape) of ClF5<\/em> 2. A. What is the electron-pair geometry for N in NH3? There are lone pair(s) around the central atom, so the molecular geometry (shape) of NH3 is B. What is the electron-pair geometry for Be in BeBr2? _<\/strong><\/em> There are lone pair(s) around the central atom, so the molecular geometry (shape) of BeBr2 is __<\/em><\/strong><\/p>\n\n\n\n

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

SOF4 (Sulfur Tetrafluoride Oxide)<\/strong><\/h3>\n\n\n\n
    \n
  • Electron-pair geometry for S<\/strong>: In SOF4, sulfur is the central atom, and it is bonded to four fluorine atoms and one oxygen atom. The sulfur atom has a total of 5 regions of electron density around it: 4 single bonds with fluorine and 1 single bond with oxygen. This leads to a trigonal bipyramidal<\/strong> electron-pair geometry.<\/li>\n\n\n\n
  • Number of lone pairs around the central atom<\/strong>: There are no lone pairs on sulfur in SOF4 because all the electron pairs are involved in bonding.<\/li>\n\n\n\n
  • Molecular geometry (shape)<\/strong>: Since there are no lone pairs, the molecular geometry will also be trigonal bipyramidal<\/strong>, which reflects the electron-pair geometry.<\/li>\n<\/ul>\n\n\n\n

    2. ClF5 (Chlorine Pentafluoride)<\/strong><\/h3>\n\n\n\n
      \n
    • Electron-pair geometry for Cl<\/strong>: In ClF5, chlorine is the central atom, bonded to five fluorine atoms. There are 5 bonding regions and 1 lone pair of electrons on chlorine, resulting in a octahedral<\/strong> electron-pair geometry.<\/li>\n\n\n\n
    • Number of lone pairs around the central atom<\/strong>: There is 1 lone pair<\/strong> on chlorine in ClF5.<\/li>\n\n\n\n
    • Molecular geometry (shape)<\/strong>: The presence of one lone pair distorts the electron-pair geometry, making the molecular geometry square pyramidal<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      3. NH3 (Ammonia)<\/strong><\/h3>\n\n\n\n
        \n
      • Electron-pair geometry for N<\/strong>: In NH3, nitrogen is the central atom, bonded to three hydrogen atoms. There are three bonding regions and one lone pair on nitrogen, leading to a tetrahedral<\/strong> electron-pair geometry.<\/li>\n\n\n\n
      • Number of lone pairs around the central atom<\/strong>: There is 1 lone pair<\/strong> on nitrogen in NH3.<\/li>\n\n\n\n
      • Molecular geometry (shape)<\/strong>: The molecular geometry is trigonal pyramidal<\/strong>, as the lone pair on nitrogen pushes the bonding pairs closer together, creating a pyramid-like shape.<\/li>\n<\/ul>\n\n\n\n

        4. BeBr2 (Beryllium Bromide)<\/strong><\/h3>\n\n\n\n
          \n
        • Electron-pair geometry for Be<\/strong>: In BeBr2, beryllium is the central atom, bonded to two bromine atoms. There are no lone pairs on beryllium, and only two bonding pairs of electrons, which results in a linear<\/strong> electron-pair geometry.<\/li>\n\n\n\n
        • Number of lone pairs around the central atom<\/strong>: There are 0 lone pairs<\/strong> on beryllium in BeBr2.<\/li>\n\n\n\n
        • Molecular geometry (shape)<\/strong>: Since there are no lone pairs, the molecular geometry is also linear<\/strong>.<\/li>\n<\/ul>\n\n\n\n

          Summary:<\/h3>\n\n\n\n
            \n
          1. SOF4<\/strong>:\n
              \n
            • Electron-pair geometry: Trigonal bipyramidal<\/li>\n\n\n\n
            • Lone pairs: 0<\/li>\n\n\n\n
            • Molecular geometry: Trigonal bipyramidal<\/li>\n<\/ul>\n<\/li>\n\n\n\n
            • ClF5<\/strong>:\n
                \n
              • Electron-pair geometry: Octahedral<\/li>\n\n\n\n
              • Lone pairs: 1<\/li>\n\n\n\n
              • Molecular geometry: Square pyramidal<\/li>\n<\/ul>\n<\/li>\n\n\n\n
              • NH3<\/strong>:\n
                  \n
                • Electron-pair geometry: Tetrahedral<\/li>\n\n\n\n
                • Lone pairs: 1<\/li>\n\n\n\n
                • Molecular geometry: Trigonal pyramidal<\/li>\n<\/ul>\n<\/li>\n\n\n\n
                • BeBr2<\/strong>:\n
                    \n
                  • Electron-pair geometry: Linear<\/li>\n\n\n\n
                  • Lone pairs: 0<\/li>\n\n\n\n
                  • Molecular geometry: Linear<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
                    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

                    A. What is the electron-pair geometry for S in SOF4? _ There are lone pair(s) around the central atom, so the molecular geometry (shape) of SOF4 is B. What is the electron-pair geometry for Cl in ClF5? There are lone pair(s) around the central atom, so the molecular geometry (shape) of ClF5 2. A. What […]<\/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-249626","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249626","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=249626"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249626\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=249626"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=249626"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=249626"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}