{"id":185174,"date":"2025-01-22T07:43:19","date_gmt":"2025-01-22T07:43:19","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185174"},"modified":"2025-01-22T07:43:41","modified_gmt":"2025-01-22T07:43:41","slug":"answer-the-following-questions-about-the-lewis-structure-for-ammon","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/answer-the-following-questions-about-the-lewis-structure-for-ammon\/","title":{"rendered":"Answer the following questions about the Lewis structure for ammonium carbonate"},"content":{"rendered":"\n

Answer the following questions about the Lewis structure for ammonium carbonate, (NH4)2CO3 There are Each ammonium ion has The carbonate ion has In each ammonium ion, the central N has shape is (x), and the bond angles are The single carbonate ion has a. 0 j. 14 m. 20 diatomic v. linear z. bent For the carbonate ion, the shape at the central C is and the bond angles are about d. 3 b. 1 k. 16 c. 2 n. 24 I. 18 o. 26 u. pyramidal carbonate ions. There are ionic bonds in the molecule. valence electrons. ammonium ions and valence electrons. double covalent bonds, and triple covalent bonds. p. 30 w. monoatomic ions aa. 120\u00e2\ufffd\u00b0 bb. 180\u00c2\u00b0 cc. no bond angles, no central atom nonpolar gg. ionic e. 4 f. 5 q. 32 hh. O and O dd. 109.5\u00c2\u00b0 central atoms and x. tetrahedral single covalent bonds, g. 8 r. 34 REDs and h. 10 s. 36 REDS, t ee. polar i. 12 t. y. trigonal planar ff.<\/p>\n\n\n\n

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

Answer:<\/h3>\n\n\n\n
    \n
  1. There are<\/strong>: 20 valence electrons<\/strong> in total for the molecule.<\/li>\n\n\n\n
  2. Each ammonium ion has<\/strong>: tetrahedral shape<\/strong>, and the bond angles are about 109.5\u00b0<\/strong>.<\/li>\n\n\n\n
  3. The carbonate ion has<\/strong>: trigonal planar shape<\/strong>, and the bond angles are about 120\u00b0<\/strong>.<\/li>\n\n\n\n
  4. In each ammonium ion, the central N has<\/strong>: tetrahedral shape<\/strong>.<\/li>\n\n\n\n
  5. The single carbonate ion has<\/strong>: three resonance structures, one double covalent bond per resonance structure, and all bonds are equivalent.<\/strong><\/li>\n\n\n\n
  6. For the carbonate ion, the shape at the central C is<\/strong>: trigonal planar<\/strong> and the bond angles are about 120\u00b0<\/strong>.<\/li>\n\n\n\n
  7. There are<\/strong>: ionic bonds between ammonium and carbonate ions<\/strong>.<\/li>\n\n\n\n
  8. There are<\/strong>: no triple covalent bonds in the molecule<\/strong>.<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

    Explanation (Approx. 300 Words):<\/h3>\n\n\n\n

    Ammonium carbonate, ((\\text{NH}_4)_2\\text{CO}_3), is an ionic compound comprising two ammonium ions ((\\text{NH}_4^+)) and one carbonate ion ((\\text{CO}_3^{2-})). To understand its Lewis structure, we analyze each component:<\/p>\n\n\n\n

      \n
    1. Ammonium Ion ((\\text{NH}_4^+))<\/strong>: Each nitrogen atom in (\\text{NH}_4^+) has a tetrahedral geometry due to its four single covalent bonds to hydrogen atoms. The bond angles are approximately (109.5^\\circ), typical for tetrahedral shapes. Each ammonium ion contributes (8) valence electrons ((5) from nitrogen and (3) from three hydrogens). However, since it loses one electron as a positive ion, its effective electron count becomes (7) for the Lewis structure.<\/li>\n\n\n\n
    2. Carbonate Ion ((\\text{CO}_3^{2-}))<\/strong>: The carbonate ion has a trigonal planar shape with a central carbon atom double-bonded to one oxygen and single-bonded to two others, with resonance distributing the charge evenly across the three oxygen atoms. Each bond is equivalent due to resonance, and the bond angles are about (120^\\circ), consistent with a trigonal planar geometry. The carbonate ion contributes (24) valence electrons.<\/li>\n\n\n\n
    3. Total Valence Electrons<\/strong>: Adding the valence electrons of two (\\text{NH}_4^+) ions ((2 \\times 7 = 14)) and one (\\text{CO}_3^{2-}) ion ((24)), the molecule has (36) valence electrons.<\/li>\n<\/ol>\n\n\n\n

      The ((\\text{NH}_4)_2\\text{CO}_3) compound is stabilized by ionic bonds<\/strong> between the ammonium cations and carbonate anion. This ionic interaction and resonance ensure the molecule’s overall stability.<\/p>\n","protected":false},"excerpt":{"rendered":"

      Answer the following questions about the Lewis structure for ammonium carbonate, (NH4)2CO3 There are Each ammonium ion has The carbonate ion has In each ammonium ion, the central N has shape is (x), and the bond angles are The single carbonate ion has a. 0 j. 14 m. 20 diatomic v. linear z. bent 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-185174","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185174","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=185174"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185174\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185174"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185174"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185174"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}