{"id":240049,"date":"2025-07-03T07:02:32","date_gmt":"2025-07-03T07:02:32","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=240049"},"modified":"2025-07-03T07:02:34","modified_gmt":"2025-07-03T07:02:34","slug":"compound-lewis-structure-with-dipoles-and-wedge-hash-structure","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/03\/compound-lewis-structure-with-dipoles-and-wedge-hash-structure\/","title":{"rendered":"Compound Lewis Structure (with dipoles) and Wedge-Hash Structure"},"content":{"rendered":"\n

Compound Lewis Structure (with dipoles) and Wedge-Hash Structure # of e groups Electronic Geometry Molecular Shape Bond angles Polar molecule? Hybridization XeF? SF? BrF? XeF? phosphate<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

1. XeF2 (Xenon Difluoride)<\/strong><\/h3>\n\n\n\n
    \n
  • Lewis Structure<\/strong>: Xe in the center, two F atoms attached, and three lone pairs on Xe.<\/li>\n\n\n\n
  • # of e groups<\/strong>: 5 (2 bonding pairs, 3 lone pairs).<\/li>\n\n\n\n
  • Electronic Geometry<\/strong>: Trigonal bipyramidal (due to 5 electron groups).<\/li>\n\n\n\n
  • Molecular Shape<\/strong>: Linear (due to the three lone pairs, which cause repulsion to arrange the bonding pairs opposite each other).<\/li>\n\n\n\n
  • Bond Angles<\/strong>: 180\u00b0.<\/li>\n\n\n\n
  • Polar Molecule?<\/strong>: Yes, due to the lone pairs on Xe, leading to a dipole moment.<\/li>\n\n\n\n
  • Hybridization<\/strong>: sp\u00b3d.<\/li>\n<\/ul>\n\n\n\n

    2. SF6 (Sulfur Hexafluoride)<\/strong><\/h3>\n\n\n\n
      \n
    • Lewis Structure<\/strong>: S in the center with six F atoms attached, no lone pairs on S.<\/li>\n\n\n\n
    • # of e groups<\/strong>: 6 (all bonding pairs).<\/li>\n\n\n\n
    • Electronic Geometry<\/strong>: Octahedral.<\/li>\n\n\n\n
    • Molecular Shape<\/strong>: Octahedral.<\/li>\n\n\n\n
    • Bond Angles<\/strong>: 90\u00b0 and 180\u00b0.<\/li>\n\n\n\n
    • Polar Molecule?<\/strong>: No, the symmetrical shape cancels out dipoles.<\/li>\n\n\n\n
    • Hybridization<\/strong>: sp\u00b3d\u00b2.<\/li>\n<\/ul>\n\n\n\n

      3. BrF5 (Bromine Pentafluoride)<\/strong><\/h3>\n\n\n\n
        \n
      • Lewis Structure<\/strong>: Br in the center, five F atoms attached, one lone pair on Br.<\/li>\n\n\n\n
      • # of e groups<\/strong>: 6 (5 bonding pairs, 1 lone pair).<\/li>\n\n\n\n
      • Electronic Geometry<\/strong>: Octahedral.<\/li>\n\n\n\n
      • Molecular Shape<\/strong>: Square pyramidal (due to the lone pair).<\/li>\n\n\n\n
      • Bond Angles<\/strong>: 90\u00b0 and 180\u00b0.<\/li>\n\n\n\n
      • Polar Molecule?<\/strong>: Yes, due to the asymmetry from the lone pair.<\/li>\n\n\n\n
      • Hybridization<\/strong>: sp\u00b3d\u00b2.<\/li>\n<\/ul>\n\n\n\n

        4. XeF4 (Xenon Tetrafluoride)<\/strong><\/h3>\n\n\n\n
          \n
        • Lewis Structure<\/strong>: Xe in the center, four F atoms attached, two lone pairs on Xe.<\/li>\n\n\n\n
        • # of e groups<\/strong>: 6 (4 bonding pairs, 2 lone pairs).<\/li>\n\n\n\n
        • Electronic Geometry<\/strong>: Octahedral.<\/li>\n\n\n\n
        • Molecular Shape<\/strong>: Square planar (due to lone pairs).<\/li>\n\n\n\n
        • Bond Angles<\/strong>: 90\u00b0 and 180\u00b0.<\/li>\n\n\n\n
        • Polar Molecule?<\/strong>: No, symmetrical shape.<\/li>\n\n\n\n
        • Hybridization<\/strong>: sp\u00b3d\u00b2.<\/li>\n<\/ul>\n\n\n\n

          5. Phosphate (PO\u2084\u00b3\u207b)<\/strong><\/h3>\n\n\n\n
            \n
          • Lewis Structure<\/strong>: P in the center with four O atoms attached, one double bond, and three single bonds with O atoms carrying negative charges.<\/li>\n\n\n\n
          • # of e groups<\/strong>: 4 (all bonding pairs).<\/li>\n\n\n\n
          • Electronic Geometry<\/strong>: Tetrahedral.<\/li>\n\n\n\n
          • Molecular Shape<\/strong>: Tetrahedral.<\/li>\n\n\n\n
          • Bond Angles<\/strong>: 109.5\u00b0.<\/li>\n\n\n\n
          • Polar Molecule?<\/strong>: No, the molecule is symmetrical.<\/li>\n\n\n\n
          • Hybridization<\/strong>: sp\u00b3.<\/li>\n<\/ul>\n\n\n\n

            Each molecule’s structure influences its bonding, geometry, and polarity. Feel free to ask for more details!<\/p>\n\n\n\n

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

            Compound Lewis Structure (with dipoles) and Wedge-Hash Structure # of e groups Electronic Geometry Molecular Shape Bond angles Polar molecule? Hybridization XeF? SF? BrF? XeF? phosphate The Correct Answer and Explanation is: 1. XeF2 (Xenon Difluoride) 2. SF6 (Sulfur Hexafluoride) 3. BrF5 (Bromine Pentafluoride) 4. XeF4 (Xenon Tetrafluoride) 5. Phosphate (PO\u2084\u00b3\u207b) Each molecule’s structure influences […]<\/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-240049","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240049","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=240049"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240049\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=240049"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=240049"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=240049"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}