{"id":183209,"date":"2025-01-16T05:27:52","date_gmt":"2025-01-16T05:27:52","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=183209"},"modified":"2025-01-16T05:27:54","modified_gmt":"2025-01-16T05:27:54","slug":"nh4cio2-indicate-the-electron-pair-geometry-and-molecular-shape-around-each-ion","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/16\/nh4cio2-indicate-the-electron-pair-geometry-and-molecular-shape-around-each-ion\/","title":{"rendered":"NH4CIO2 (indicate the electron pair geometry and molecular shape around each ion)"},"content":{"rendered":"\n

SF3 20. BrF5 1. SiO3 2. NH4CIO2 (indicate the electron pair geometry and molecular shape around each ion.) 2- Molecular Lewis DotAXE Type Electron Formula Structure on Central Molecular onic, 2 Shape polar,<\/p>\n\n\n\n

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

To address this question, let’s go through the electron pair geometry and molecular shapes for each molecule or ion (SF3, BrF5, SiO3, NH4ClO2) using the AXE method (A = central atom, X = atoms bonded to A, E = lone pairs on A).<\/p>\n\n\n\n

1. SF3 (Sulfur Trifluoride)<\/strong><\/h3>\n\n\n\n
    \n
  • Lewis Structure<\/strong>: Sulfur (S) is the central atom, bonded to three fluorine (F) atoms, with one lone pair of electrons on sulfur.<\/li>\n\n\n\n
  • Electron Pair Geometry (EPG)<\/strong>: Tetrahedral (4 regions of electron density: 3 bonding regions and 1 lone pair)<\/li>\n\n\n\n
  • Molecular Shape<\/strong>: Trigonal pyramidal (due to the lone pair on sulfur)<\/li>\n\n\n\n
  • Polarity<\/strong>: The molecule is polar because the fluorine atoms are highly electronegative, creating a dipole.<\/li>\n<\/ul>\n\n\n\n

    2. BrF5 (Bromine Pentafluoride)<\/strong><\/h3>\n\n\n\n
      \n
    • Lewis Structure<\/strong>: Bromine (Br) is the central atom, bonded to five fluorine (F) atoms, with one lone pair of electrons on bromine.<\/li>\n\n\n\n
    • Electron Pair Geometry (EPG)<\/strong>: Octahedral (6 regions of electron density: 5 bonding regions and 1 lone pair)<\/li>\n\n\n\n
    • Molecular Shape<\/strong>: Square pyramidal (due to the lone pair on bromine)<\/li>\n\n\n\n
    • Polarity<\/strong>: The molecule is polar because of the asymmetry of the fluorine atoms around the central bromine atom.<\/li>\n<\/ul>\n\n\n\n

      3. SiO3 (Silicate Ion)<\/strong><\/h3>\n\n\n\n
        \n
      • Lewis Structure<\/strong>: Silicon (Si) is the central atom, bonded to three oxygen (O) atoms, each with a negative charge, forming a trigonal planar structure.<\/li>\n\n\n\n
      • Electron Pair Geometry (EPG)<\/strong>: Trigonal planar (3 regions of electron density: 3 bonding regions)<\/li>\n\n\n\n
      • Molecular Shape<\/strong>: Trigonal planar<\/li>\n\n\n\n
      • Polarity<\/strong>: This ion is nonpolar due to the symmetry of the three oxygen atoms surrounding the central silicon atom.<\/li>\n<\/ul>\n\n\n\n

        4. NH4ClO2 (Ammonium Chlorite)<\/strong><\/h3>\n\n\n\n
          \n
        • Lewis Structure<\/strong>: Nitrogen (N) is the central atom, bonded to four hydrogen (H) atoms. The chlorite ion (ClO2) is attached to the nitrogen via a coordinate bond.<\/li>\n\n\n\n
        • Electron Pair Geometry (EPG)<\/strong>: Tetrahedral (4 regions of electron density: 4 bonding regions)<\/li>\n\n\n\n
        • Molecular Shape<\/strong>: Tetrahedral<\/li>\n\n\n\n
        • Polarity<\/strong>: The ammonium ion (NH4+) is nonpolar due to the symmetrical distribution of the hydrogen atoms.<\/li>\n<\/ul>\n\n\n\n

          Summary<\/h3>\n\n\n\n
            \n
          • SF3<\/strong>: Tetrahedral EPG, Trigonal Pyramidal Molecular Shape, Polar<\/li>\n\n\n\n
          • BrF5<\/strong>: Octahedral EPG, Square Pyramidal Molecular Shape, Polar<\/li>\n\n\n\n
          • SiO3<\/strong>: Trigonal Planar EPG, Trigonal Planar Molecular Shape, Nonpolar<\/li>\n\n\n\n
          • NH4ClO2<\/strong>: Tetrahedral EPG, Tetrahedral Molecular Shape, Nonpolar<\/li>\n<\/ul>\n\n\n\n

            These geometries are based on the VSEPR (Valence Shell Electron Pair Repulsion) theory, which predicts the arrangement of atoms and electron pairs to minimize repulsion.<\/p>\n\n\n\n

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

            SF3 20. BrF5 1. SiO3 2. NH4CIO2 (indicate the electron pair geometry and molecular shape around each ion.) 2- Molecular Lewis DotAXE Type Electron Formula Structure on Central Molecular onic, 2 Shape polar, The Correct Answer and Explanation is : To address this question, let’s go through the electron pair geometry and molecular shapes for […]<\/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-183209","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183209","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=183209"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183209\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183209"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183209"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183209"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}