{"id":200717,"date":"2025-03-14T02:48:19","date_gmt":"2025-03-14T02:48:19","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=200717"},"modified":"2025-03-14T02:48:22","modified_gmt":"2025-03-14T02:48:22","slug":"lewis-structure-for-pf4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/14\/lewis-structure-for-pf4\/","title":{"rendered":"Lewis structure for PF4"},"content":{"rendered":"\n

Lewis structure for PF4+<\/p>\n\n\n\n

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

The Lewis structure of PF4+PF_4^+<\/strong> (phosphorus tetrafluoride cation) consists of phosphorus (P) as the central atom, bonded to four fluorine (F) atoms, and carrying a +1 charge<\/strong>.<\/p>\n\n\n\n

Steps to Draw the Lewis Structure of PF4+PF_4^+<\/strong>:<\/h3>\n\n\n\n
    \n
  1. Determine the total number of valence electrons:<\/strong>
    • Phosphorus (P) is in group 15<\/strong>, so it has 5 valence electrons<\/strong>.<\/li>
    • Fluorine (F) is in group 17<\/strong>, so each fluorine has 7 valence electrons<\/strong>.<\/li>
    • Since there are four fluorine atoms<\/strong>, their total contribution is 4 \u00d7 7 = 28<\/strong> electrons.<\/li>
    • The +1 charge<\/strong> means one electron is lost<\/strong>, reducing the total count by 1.<\/li><\/ul>Total valence electrons = 5 + 28 – 1 = 32 electrons.<\/strong><\/li>\n\n\n\n
    • Identify the central atom and arrange the atoms:<\/strong>\n
        \n
      • Phosphorus<\/strong> is the central atom because it is less electronegative than fluorine.<\/li>\n\n\n\n
      • The four fluorine atoms are symmetrically arranged around phosphorus.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Form single bonds between phosphorus and fluorine:<\/strong>\n
          \n
        • Each P\u2013F single bond requires 2 electrons<\/strong>.<\/li>\n\n\n\n
        • With 4 bonds, 4 \u00d7 2 = 8 electrons<\/strong> are used.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Distribute the remaining electrons:<\/strong>\n
            \n
          • After forming bonds, 32 – 8 = 24 electrons<\/strong> remain.<\/li>\n\n\n\n
          • These electrons are placed as lone pairs<\/strong> on the fluorine atoms<\/strong> (each gets 6 electrons to complete the octet).<\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Check for formal charges:<\/strong>\n
              \n
            • Formal charge on phosphorus<\/strong>: (5 – 0 – 4) = +1<\/strong>.<\/li>\n\n\n\n
            • Each fluorine has a formal charge of (7 – 6 – 1) = 0<\/strong>.<\/li>\n\n\n\n
            • Since the molecule has an overall +1 charge<\/strong>, the structure is correct.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

              Molecular Shape and Hybridization<\/strong>:<\/h3>\n\n\n\n
                \n
              • The electron geometry<\/strong> is tetrahedral<\/strong>.<\/li>\n\n\n\n
              • Due to the +1 charge<\/strong>, the molecule is somewhat distorted<\/strong> compared to a neutral PF4PF_4.<\/li>\n\n\n\n
              • The hybridization<\/strong> of phosphorus in PF4+PF_4^+ is sp\u00b3<\/strong>.<\/li>\n<\/ul>\n\n\n\n

                Here is the Lewis structure image<\/strong> of PF4+PF_4^+:<\/p>\n\n\n\n

                Here is the Lewis structure of PF4+PF_4^+<\/strong> with the correct arrangement of atoms, bonds, lone pairs on fluorine, and the +1 charge. Let me know if you need further explanations!<\/p>\n\n\n\n

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

                Lewis structure for PF4+ The correct answer and explanation is: The Lewis structure of PF4+PF_4^+ (phosphorus tetrafluoride cation) consists of phosphorus (P) as the central atom, bonded to four fluorine (F) atoms, and carrying a +1 charge. Steps to Draw the Lewis Structure of PF4+PF_4^+: Molecular Shape and Hybridization: Here is the Lewis structure image […]<\/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-200717","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/200717","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=200717"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/200717\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=200717"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=200717"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=200717"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}