{"id":218939,"date":"2025-05-24T17:11:16","date_gmt":"2025-05-24T17:11:16","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=218939"},"modified":"2025-05-24T17:11:18","modified_gmt":"2025-05-24T17:11:18","slug":"sketch-and-bond-angles-for-o3-asf5-krcl4-secl4-and-ch2cl2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/24\/sketch-and-bond-angles-for-o3-asf5-krcl4-secl4-and-ch2cl2\/","title":{"rendered":"Sketch and bond angles for O3, AsF5, KrCl4, SeCL4, and CH2Cl2"},"content":{"rendered":"\n

Can someone help me with 3-D Sketch and bond angles for O3, AsF5, KrCl4, SeCL4, and CH2Cl2? Also I’m not sure if I got the Lewis Structure correct for SeCl4. Thanks!<\/p>\n\n\n\n

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

\n\n\n\n

\u2705 1. O\u2083 (Ozone)<\/strong><\/h3>\n\n\n\n
    \n
  • Lewis Structure<\/strong>: O=O\u2013O with one double bond and one single bond, and a lone pair on each terminal O. The structure is resonance stabilized<\/strong>.<\/li>\n\n\n\n
  • Molecular Geometry<\/strong>: Bent<\/strong><\/li>\n\n\n\n
  • Bond Angle<\/strong>: ~117\u00b0<\/li>\n\n\n\n
  • Explanation<\/strong>: 3 electron regions (2 bonding, 1 lone pair) around the central O leads to trigonal planar electron geometry<\/strong>, but the lone pair reduces the angle.<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    \u2705 2. AsF\u2085 (Arsenic Pentafluoride)<\/strong><\/h3>\n\n\n\n
      \n
    • Lewis Structure<\/strong>: As is bonded to 5 F atoms with no lone pairs.<\/li>\n\n\n\n
    • Molecular Geometry<\/strong>: Trigonal Bipyramidal<\/strong><\/li>\n\n\n\n
    • Bond Angles<\/strong>: 120\u00b0<\/strong> (equatorial), 90\u00b0<\/strong> (axial-equatorial)<\/li>\n\n\n\n
    • Explanation<\/strong>: 5 bonding pairs around As, no lone pairs \u2192 ideal geometry.<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      \u2705 3. KrCl\u2084 (Krypton Tetrachloride)<\/strong><\/h3>\n\n\n\n
        \n
      • Lewis Structure<\/strong>: Kr surrounded by 4 Cl atoms and 2 lone pairs<\/strong>.<\/li>\n\n\n\n
      • Molecular Geometry<\/strong>: Square Planar<\/strong><\/li>\n\n\n\n
      • Bond Angles<\/strong>: 90\u00b0<\/strong><\/li>\n\n\n\n
      • Explanation<\/strong>: 6 electron regions (4 bonding, 2 lone pairs), lone pairs go opposite each other, yielding square planar shape.<\/li>\n<\/ul>\n\n\n\n
        \n\n\n\n

        \u2705 4. SeCl\u2084 (Selenium Tetrachloride)<\/strong><\/h3>\n\n\n\n
          \n
        • Correct Lewis Structure<\/strong>: Se is bonded to 4 Cl atoms, and has one lone pair<\/strong>.<\/li>\n\n\n\n
        • Molecular Geometry<\/strong>: See-saw<\/strong><\/li>\n\n\n\n
        • Bond Angles<\/strong>: ~101\u00b0 and ~120\u00b0<\/li>\n\n\n\n
        • Explanation<\/strong>: 5 electron regions (4 bonding, 1 lone pair), based on trigonal bipyramidal<\/strong> geometry, lone pair in equatorial position distorts bond angles.<\/li>\n<\/ul>\n\n\n\n
          \n\n\n\n

          \u2705 5. CH\u2082Cl\u2082 (Dichloromethane)<\/strong><\/h3>\n\n\n\n
            \n
          • Lewis Structure<\/strong>: Central carbon single bonded to 2 H and 2 Cl atoms.<\/li>\n\n\n\n
          • Molecular Geometry<\/strong>: Tetrahedral<\/strong><\/li>\n\n\n\n
          • Bond Angles<\/strong>: ~109.5\u00b0<\/li>\n\n\n\n
          • Explanation<\/strong>: 4 bonding pairs around C, no lone pairs. Tetrahedral geometry with slight variation due to different atom sizes and electronegativity.<\/li>\n<\/ul>\n\n\n\n
            \n\n\n\n

            \ud83d\udd0d Summary:<\/h3>\n\n\n\n
            Molecule<\/th>Lewis Structure Key<\/th>Geometry<\/th>Bond Angles<\/th><\/tr><\/thead>
            O\u2083<\/td>Resonance with lone pairs<\/td>Bent<\/td>~117\u00b0<\/td><\/tr>
            AsF\u2085<\/td>5 F atoms, no lone pair<\/td>Trigonal Bipyramidal<\/td>90\u00b0, 120\u00b0<\/td><\/tr>
            KrCl\u2084<\/td>4 Cl, 2 lone pairs<\/td>Square Planar<\/td>90\u00b0<\/td><\/tr>
            SeCl\u2084<\/td>4 Cl, 1 lone pair<\/td>See-saw<\/td>~101\u00b0, ~120\u00b0<\/td><\/tr>
            CH\u2082Cl\u2082<\/td>4 single bonds, no lone pair<\/td>Tetrahedral<\/td>~109.5\u00b0<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
            \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

            Can someone help me with 3-D Sketch and bond angles for O3, AsF5, KrCl4, SeCL4, and CH2Cl2? Also I’m not sure if I got the Lewis Structure correct for SeCl4. Thanks! The Correct Answer and Explanation is: \u2705 1. O\u2083 (Ozone) \u2705 2. AsF\u2085 (Arsenic Pentafluoride) \u2705 3. KrCl\u2084 (Krypton Tetrachloride) \u2705 4. SeCl\u2084 (Selenium […]<\/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-218939","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/218939","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=218939"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/218939\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=218939"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=218939"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=218939"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}