{"id":240666,"date":"2025-07-03T11:09:15","date_gmt":"2025-07-03T11:09:15","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=240666"},"modified":"2025-07-03T11:09:17","modified_gmt":"2025-07-03T11:09:17","slug":"draw-lewis-structure-for-sf4sulfur-tetrafluoride-determine-its-point-group-and-list-all-symmetry-elements","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/03\/draw-lewis-structure-for-sf4sulfur-tetrafluoride-determine-its-point-group-and-list-all-symmetry-elements\/","title":{"rendered":"Draw Lewis structure for SF4(sulfur tetrafluoride), determine its point group, and list all symmetry elements"},"content":{"rendered":"\n
    \n
  1. Draw Lewis structure for SF4
    (sulfur tetrafluoride), determine its point group, and list all symmetry elements (9 points).<\/li>\n<\/ol>\n\n\n\n

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

    Lewis Structure for SF\u2084 (Sulfur Tetrafluoride)<\/h3>\n\n\n\n

    Sulfur tetrafluoride (SF\u2084) consists of a central sulfur (S) atom surrounded by four fluorine (F) atoms. To draw the Lewis structure, follow these steps:<\/p>\n\n\n\n

      \n
    1. Count the valence electrons<\/strong>:\n
        \n
      • Sulfur (S) is in Group 16, so it has 6 valence electrons.<\/li>\n\n\n\n
      • Each fluorine (F) atom is in Group 17, so it has 7 valence electrons.<\/li>\n\n\n\n
      • Total valence electrons = 6 (for S) + 4 \u00d7 7 (for F) = 34 electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Place sulfur in the center<\/strong>: Sulfur is less electronegative than fluorine, so it will be in the center.<\/li>\n\n\n\n
      • Connect the fluorine atoms to sulfur<\/strong>: Use single bonds to connect each fluorine atom to sulfur.<\/li>\n\n\n\n
      • Complete the octet of fluorine atoms<\/strong>: Each fluorine atom needs 6 more electrons to complete its octet, so place 3 lone pairs of electrons around each fluorine.<\/li>\n\n\n\n
      • Distribute remaining electrons on sulfur<\/strong>: Sulfur has 2 remaining electrons. These will be placed as lone pairs on sulfur. Since sulfur can have an expanded octet, it can hold more than 8 electrons.<\/li>\n\n\n\n
      • Final Structure<\/strong>:\n
          \n
        • Sulfur is bonded to four fluorine atoms by single bonds.<\/li>\n\n\n\n
        • Each fluorine has 3 lone pairs.<\/li>\n\n\n\n
        • Sulfur has 2 lone pairs.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

          The structure looks like a seesaw<\/strong> shape, due to one lone pair on the sulfur atom.<\/p>\n\n\n\n

          Point Group of SF\u2084<\/h3>\n\n\n\n

          SF\u2084 is classified under the C\u2083v<\/strong> point group.<\/p>\n\n\n\n

          Symmetry Elements:<\/h4>\n\n\n\n
            \n
          1. E (Identity operation)<\/strong>: The structure is invariant under no operation, meaning the molecule remains unchanged.<\/li>\n\n\n\n
          2. C\u2083 (Rotation axis)<\/strong>: SF\u2084 has a 3-fold rotational axis passing through the sulfur atom and the two fluorine atoms in the plane. Rotating by 120\u00b0 or 240\u00b0 around this axis does not change the structure.<\/li>\n\n\n\n
          3. \u03c3\u2093 (Mirror plane)<\/strong>: There are two mirror planes in SF\u2084:\n
              \n
            • One plane containing the sulfur atom and the two opposite fluorine atoms (plane of symmetry).<\/li>\n\n\n\n
            • Another plane that contains sulfur and one fluorine atom, bisecting the angle between the other two fluorines.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
            • \u03c3\u1d67 (Mirror plane)<\/strong>: A plane that includes the C\u2083 axis (same as above).<\/li>\n\n\n\n
            • S\u2083 (Improper rotation)<\/strong>: A combination of a 120\u00b0 rotation about the C\u2083 axis followed by a reflection in the mirror plane leaves the molecule unchanged.<\/li>\n<\/ol>\n\n\n\n

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

              SF\u2084 is a trigonal bipyramidal<\/strong> molecule with one lone pair on sulfur, resulting in a seesaw-shaped geometry. This shape explains its symmetry, including the presence of a 3-fold rotation axis (C\u2083) and mirror planes (\u03c3). The symmetry elements describe how the molecule behaves under certain operations, which is important for predicting its spectroscopic properties and behavior in molecular interactions.<\/p>\n\n\n\n

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

              The Correct Answer and Explanation is: Lewis Structure for SF\u2084 (Sulfur Tetrafluoride) Sulfur tetrafluoride (SF\u2084) consists of a central sulfur (S) atom surrounded by four fluorine (F) atoms. To draw the Lewis structure, follow these steps: The structure looks like a seesaw shape, due to one lone pair on the sulfur atom. Point Group of […]<\/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-240666","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240666","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=240666"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240666\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=240666"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=240666"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=240666"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}