{"id":228571,"date":"2025-06-07T11:57:14","date_gmt":"2025-06-07T11:57:14","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=228571"},"modified":"2025-06-07T11:57:16","modified_gmt":"2025-06-07T11:57:16","slug":"draw-the-lewis-structure-3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/07\/draw-the-lewis-structure-3\/","title":{"rendered":"Draw the Lewis structure."},"content":{"rendered":"\n

Draw the Lewis structure. B) Predict the electron group geometry. C) Predict the molecular shape. D) Predict the IDEAL bond angle(s). E) Predict the polarity (circle one): Polar \/ Non-polar. PO3 3- A) Draw the Lewis structure. B) Predict the electron group geometry. C) Predict the molecular shape. D) Predict the IDEAL bond angle(s). E) Predict the polarity (circle one): Polar \/ Non-polar.<\/p>\n\n\n\n

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

Compound 1: SCl\u2085F<\/strong><\/h3>\n\n\n\n

A) Lewis Structure:<\/h4>\n\n\n\n
    \n
  • Sulfur (S) is the central atom.<\/li>\n\n\n\n
  • It forms six single bonds: five to Cl atoms and one to F.<\/li>\n\n\n\n
  • Sulfur has 6 valence electrons, and it can expand its octet.<\/li>\n\n\n\n
  • Each Cl and F has 7 valence electrons, forming single bonds and completing octets with lone pairs.<\/li>\n<\/ul>\n\n\n\n

    B) Electron Group Geometry:<\/h4>\n\n\n\n
      \n
    • Octahedral<\/strong>, as there are six bonding groups around sulfur.<\/li>\n<\/ul>\n\n\n\n

      C) Molecular Shape:<\/h4>\n\n\n\n
        \n
      • Octahedral<\/strong>, since all positions are occupied by atoms (no lone pairs).<\/li>\n<\/ul>\n\n\n\n

        D) Ideal Bond Angles:<\/h4>\n\n\n\n
          \n
        • 90\u00b0 and 180\u00b0<\/strong> (typical for octahedral geometry).<\/li>\n<\/ul>\n\n\n\n

          E) Polarity:<\/h4>\n\n\n\n
            \n
          • Polar<\/strong>, due to the presence of one fluorine atom (much more electronegative than Cl), causing an uneven charge distribution.<\/li>\n<\/ul>\n\n\n\n
            \n\n\n\n

            Compound 2: PO\u2083\u00b3\u207b (Phosphite ion)<\/strong><\/h3>\n\n\n\n

            A) Lewis Structure:<\/h4>\n\n\n\n
              \n
            • Phosphorus (P) is the central atom.<\/li>\n\n\n\n
            • It forms three single bonds with three oxygen atoms.<\/li>\n\n\n\n
            • One of the oxygens carries a negative charge.<\/li>\n\n\n\n
            • The other two O atoms each carry a negative charge.<\/li>\n\n\n\n
            • P has one lone pair.<\/li>\n<\/ul>\n\n\n\n

              B) Electron Group Geometry:<\/h4>\n\n\n\n
                \n
              • Tetrahedral<\/strong>, due to three bonding pairs and one lone pair on phosphorus.<\/li>\n<\/ul>\n\n\n\n

                C) Molecular Shape:<\/h4>\n\n\n\n
                  \n
                • Trigonal pyramidal<\/strong>, due to one lone pair on phosphorus.<\/li>\n<\/ul>\n\n\n\n

                  D) Ideal Bond Angles:<\/h4>\n\n\n\n
                    \n
                  • <109.5\u00b0<\/strong>, slightly less due to lone pair repulsion.<\/li>\n<\/ul>\n\n\n\n

                    E) Polarity:<\/h4>\n\n\n\n
                      \n
                    • Polar<\/strong>, because of the lone pair on phosphorus and the asymmetric shape, leading to a dipole moment.<\/li>\n<\/ul>\n\n\n\n
                      \n\n\n\n

                      Explanation <\/strong><\/h3>\n\n\n\n

                      Understanding the geometry and polarity of molecules involves analyzing their Lewis structures<\/strong>, electron arrangements<\/strong>, and electronegativity differences<\/strong>. In SCl\u2085F<\/strong>, sulfur is the central atom surrounded by six atoms\u2014five chlorines and one fluorine\u2014forming six sigma bonds. This results in an octahedral electron geometry and molecular shape<\/strong>, which is highly symmetrical in a perfect case<\/strong>. However, because fluorine is significantly more electronegative than chlorine, it disrupts the symmetry, pulling electron density unevenly. This leads to a polar molecule<\/strong>, despite the symmetric shape.<\/p>\n\n\n\n

                      In contrast, PO\u2083\u00b3\u207b<\/strong> (phosphite ion) exhibits tetrahedral electron geometry<\/strong> because phosphorus is surrounded by three oxygen atoms and has one lone pair. Lone pairs occupy more space than bonding pairs, so the molecular shape becomes trigonal pyramidal<\/strong>\u2014similar to ammonia (NH\u2083). The presence of a lone pair and three oxygen atoms of varying charge distribution makes the molecule polar<\/strong>. Bond angles are slightly less than 109.5\u00b0 due to increased lone pair repulsion.<\/p>\n\n\n\n

                      In both molecules, shape and polarity are influenced by electron domain geometry and the nature of surrounding atoms. Molecular polarity<\/strong> is not just about individual bonds but how those bonds are arranged in 3D space. For SCl\u2085F<\/strong>, despite a symmetric octahedral shape, the differing atom (F) causes polarity. For PO\u2083\u00b3\u207b<\/strong>, the lone pair and asymmetric oxygen arrangement lead to a polar structure. Understanding these principles helps explain reactivity, intermolecular interactions, and physical properties.<\/p>\n\n\n\n

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

                      Draw the Lewis structure. B) Predict the electron group geometry. C) Predict the molecular shape. D) Predict the IDEAL bond angle(s). E) Predict the polarity (circle one): Polar \/ Non-polar. PO3 3- A) Draw the Lewis structure. B) Predict the electron group geometry. C) Predict the molecular shape. D) Predict the IDEAL bond angle(s). E) […]<\/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-228571","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/228571","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=228571"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/228571\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=228571"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=228571"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=228571"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}