{"id":181642,"date":"2025-01-11T08:14:28","date_gmt":"2025-01-11T08:14:28","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=181642"},"modified":"2025-01-11T08:14:30","modified_gmt":"2025-01-11T08:14:30","slug":"borane-bh3-lewis-dot-structure-electron-pair-geometry","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/11\/borane-bh3-lewis-dot-structure-electron-pair-geometry\/","title":{"rendered":"Borane: BH3 Lewis Dot Structure: Electron Pair Geometry"},"content":{"rendered":"\n

Borane: BH3 Lewis Dot Structure: Electron Pair Geometry: Atoms # of valence e- per atom # of atoms in molecule B Molecular Shape: H AXE Notation: Polar or Non-Polar Total # of valence e-in molecule: Formaldehyde: CH20 Atoms Lewis Dot Structure: Electron Pair Geometry: # of valence e per atom # of atoms in molecule ? Molecular Shape: H O AXE Notation: Polar or Non-Polar Total # of valence e-in molecule: Nitrite ion: NO2- Lewis Dot Structure: Electron Pair Geometry: Atoms # of valence e per atom # of atoms in molecule N Molecular Shape: AXE Notation: Polar or Non-Polar Total # of valence e-in molecule:<\/p>\n\n\n\n

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

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

Here are the answers to your questions along with a 300-word explanation.<\/p>\n\n\n\n

\n\n\n\n

1. Borane (BH\u2083):<\/strong><\/h3>\n\n\n\n
    \n
  • Lewis Dot Structure:<\/strong> Boron in the center with three single bonds to hydrogen atoms. Boron has an incomplete octet.<\/li>\n\n\n\n
  • Electron Pair Geometry:<\/strong> Trigonal planar.<\/li>\n\n\n\n
  • Atoms:<\/strong><\/li>\n\n\n\n
  • Boron: 3 valence electrons.<\/li>\n\n\n\n
  • Hydrogen: 1 valence electron each (3 hydrogens = 3 electrons).<\/li>\n\n\n\n
  • Molecular Shape:<\/strong> Trigonal planar.<\/li>\n\n\n\n
  • AXE Notation:<\/strong> AX\u2083 (3 bonding regions, no lone pairs).<\/li>\n\n\n\n
  • Polar or Non-Polar:<\/strong> Non-polar (symmetrical charge distribution).<\/li>\n\n\n\n
  • Total # of Valence Electrons in Molecule:<\/strong> 6 (3 from Boron, 3 from Hydrogen).<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    2. Formaldehyde (CH\u2082O):<\/strong><\/h3>\n\n\n\n
      \n
    • Lewis Dot Structure:<\/strong> Carbon in the center bonded to two hydrogens and double-bonded to oxygen.<\/li>\n\n\n\n
    • Electron Pair Geometry:<\/strong> Trigonal planar.<\/li>\n\n\n\n
    • Atoms:<\/strong><\/li>\n\n\n\n
    • Carbon: 4 valence electrons.<\/li>\n\n\n\n
    • Hydrogen: 1 valence electron each (2 hydrogens = 2 electrons).<\/li>\n\n\n\n
    • Oxygen: 6 valence electrons.<\/li>\n\n\n\n
    • Molecular Shape:<\/strong> Trigonal planar.<\/li>\n\n\n\n
    • AXE Notation:<\/strong> AX\u2083 (3 bonding regions, no lone pairs on carbon).<\/li>\n\n\n\n
    • Polar or Non-Polar:<\/strong> Polar (oxygen is more electronegative, causing a dipole moment).<\/li>\n\n\n\n
    • Total # of Valence Electrons in Molecule:<\/strong> 12 (4 from Carbon, 2 from Hydrogen, 6 from Oxygen).<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      3. Nitrite Ion (NO\u2082\u207b):<\/strong><\/h3>\n\n\n\n
        \n
      • Lewis Dot Structure:<\/strong> Nitrogen is bonded to two oxygens, one with a single bond and one with a double bond. There is one lone pair on nitrogen and additional lone pairs on oxygens.<\/li>\n\n\n\n
      • Electron Pair Geometry:<\/strong> Trigonal planar.<\/li>\n\n\n\n
      • Atoms:<\/strong><\/li>\n\n\n\n
      • Nitrogen: 5 valence electrons.<\/li>\n\n\n\n
      • Oxygen: 6 valence electrons each (2 oxygens = 12 electrons).<\/li>\n\n\n\n
      • Plus one extra electron for the negative charge.<\/li>\n\n\n\n
      • Molecular Shape:<\/strong> Bent (due to the lone pair on nitrogen).<\/li>\n\n\n\n
      • AXE Notation:<\/strong> AX\u2082E (2 bonding regions, 1 lone pair).<\/li>\n\n\n\n
      • Polar or Non-Polar:<\/strong> Polar (asymmetrical charge distribution).<\/li>\n\n\n\n
      • Total # of Valence Electrons in Molecule:<\/strong> 18 (5 from Nitrogen, 12 from Oxygen, 1 from the negative charge).<\/li>\n<\/ul>\n\n\n\n
        \n\n\n\n

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

        The geometry and polarity of molecules are determined using the VSEPR theory. Borane (BH\u2083) has no lone pairs on boron, leading to a symmetrical trigonal planar structure, making it non-polar. Formaldehyde (CH\u2082O) has a polar bond due to the electronegativity difference between oxygen and carbon, causing a dipole moment. The nitrite ion (NO\u2082\u207b) has a bent shape because of the lone pair on nitrogen, making it polar. Calculating the total valence electrons helps confirm the correct structure, ensuring bonds and lone pairs are accounted for.<\/p>\n","protected":false},"excerpt":{"rendered":"

        Borane: BH3 Lewis Dot Structure: Electron Pair Geometry: Atoms # of valence e- per atom # of atoms in molecule B Molecular Shape: H AXE Notation: Polar or Non-Polar Total # of valence e-in molecule: Formaldehyde: CH20 Atoms Lewis Dot Structure: Electron Pair Geometry: # of valence e per atom # of atoms in molecule […]<\/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-181642","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/181642","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=181642"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/181642\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=181642"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=181642"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=181642"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}