{"id":253031,"date":"2025-07-11T17:22:34","date_gmt":"2025-07-11T17:22:34","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=253031"},"modified":"2025-07-11T17:22:36","modified_gmt":"2025-07-11T17:22:36","slug":"draw-lewis-structures-for-these-ions-and-show-which-atom-or-atoms-in-each-bears-the-formal-charge","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/11\/draw-lewis-structures-for-these-ions-and-show-which-atom-or-atoms-in-each-bears-the-formal-charge\/","title":{"rendered":"Draw Lewis structures for these ions and show which atom (or atoms) in each bears the formal charge"},"content":{"rendered":"\n

Draw Lewis structures for these ions and show which atom (or atoms) in each bears the formal charge. Q.) CH3NH3+<\/p>\n\n\n\n

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

To draw the Lewis structure for CH\u2083NH\u2083\u207a<\/strong> (methylammonium ion), let’s break it down step by step:<\/p>\n\n\n\n

Step 1: Count the Valence Electrons<\/h3>\n\n\n\n
    \n
  • Carbon (C)<\/strong> is in Group 14, so it has 4 valence electrons.<\/li>\n\n\n\n
  • Hydrogen (H)<\/strong> is in Group 1, so each hydrogen atom contributes 1 valence electron.<\/li>\n\n\n\n
  • Nitrogen (N)<\/strong> is in Group 15, so it has 5 valence electrons.<\/li>\n\n\n\n
  • The positive charge on the ion indicates that one electron has been lost, reducing the total valence electrons by 1.<\/li>\n<\/ul>\n\n\n\n

    Total valence electrons = 4 (from C) + 3\u00d71 (from H in CH\u2083) + 5 (from N) + 3\u00d71 (from H in NH\u2083) = 4 + 3 + 5 + 3 = 15 electrons.<\/h4>\n\n\n\n
      \n
    • Since the ion has a positive charge, we subtract 1 electron, giving us a total of 14 valence electrons<\/strong> to use in the structure.<\/li>\n<\/ul>\n\n\n\n

      Step 2: Determine the Connectivity<\/h3>\n\n\n\n
        \n
      • Carbon (C)<\/strong> will form three bonds with three hydrogen (H)<\/strong> atoms, making it the central atom in the CH\u2083 group.<\/li>\n\n\n\n
      • Nitrogen (N)<\/strong> will form three bonds with three hydrogen (H)<\/strong> atoms, making it the central atom in the NH\u2083 group.<\/li>\n\n\n\n
      • The CH\u2083<\/strong> and NH\u2083<\/strong> groups are attached to each other by a single bond between the carbon (C)<\/strong> and nitrogen (N)<\/strong> atoms.<\/li>\n<\/ul>\n\n\n\n

        Step 3: Draw the Structure<\/h3>\n\n\n\n
          \n
        • Place C<\/strong> at the center, attached to three H<\/strong> atoms, and N<\/strong> attached to three H<\/strong> atoms as well.<\/li>\n\n\n\n
        • There will be a single bond between the C<\/strong> and N<\/strong> atoms.<\/li>\n\n\n\n
        • Since the ion has a positive charge, N<\/strong> will carry the positive formal charge because it is one electron short of its full complement (5 valence electrons). The C<\/strong> atom and the H<\/strong> atoms do not have any formal charges.<\/li>\n<\/ul>\n\n\n\n

          Step 4: Formal Charge Calculation<\/h3>\n\n\n\n

          The formal charge can be calculated using the formula: Formal Charge=Valence Electrons\u2212(Lone Pair Electrons+12\u00d7Bonding Electrons)\\text{Formal Charge} = \\text{Valence Electrons} – (\\text{Lone Pair Electrons} + \\frac{1}{2} \\times \\text{Bonding Electrons})Formal Charge=Valence Electrons\u2212(Lone Pair Electrons+21\u200b\u00d7Bonding Electrons)<\/p>\n\n\n\n

            \n
          • For Carbon (C)<\/strong>: Carbon forms 4 bonds (to three hydrogens and one nitrogen), and it has no lone pairs. Its formal charge is: Formal\u00a0Charge\u00a0on\u00a0C=4\u2212(0+4)=0\\text{Formal Charge on C} = 4 – (0 + 4) = 0Formal\u00a0Charge\u00a0on\u00a0C=4\u2212(0+4)=0<\/li>\n\n\n\n
          • For Nitrogen (N)<\/strong>: Nitrogen forms 4 bonds (three with hydrogens and one with carbon), and it has no lone pairs in this structure. Its formal charge is: Formal\u00a0Charge\u00a0on\u00a0N=5\u2212(0+4)=+1\\text{Formal Charge on N} = 5 – (0 + 4) = +1Formal\u00a0Charge\u00a0on\u00a0N=5\u2212(0+4)=+1<\/li>\n\n\n\n
          • For Hydrogens (H)<\/strong>: Each hydrogen has a bond with either carbon or nitrogen and does not have any lone pairs. Therefore, all hydrogens have a formal charge of 0.<\/li>\n<\/ul>\n\n\n\n

            Final Structure<\/h3>\n\n\n\n
              \n
            • CH\u2083NH\u2083\u207a<\/strong> has a formal charge of +1<\/strong> on the nitrogen atom. This positive charge results because nitrogen has one fewer electron than it would in a neutral state. The carbon and hydrogen atoms in the molecule are neutral, with no formal charge.<\/li>\n<\/ul>\n\n\n\n

              Summary<\/h3>\n\n\n\n
                \n
              • Formal Charge<\/strong>: The N (nitrogen)<\/strong> atom bears the formal charge of +1<\/strong> in the CH\u2083NH\u2083\u207a<\/strong> structure.<\/li>\n\n\n\n
              • The structure shows carbon (C) bonded to three hydrogens and nitrogen (N) bonded to three hydrogens, with the positive charge localized on nitrogen.<\/li>\n<\/ul>\n\n\n\n

                This explains the structure and formal charge distribution in the CH\u2083NH\u2083\u207a<\/strong> ion.<\/p>\n\n\n\n

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

                Draw Lewis structures for these ions and show which atom (or atoms) in each bears the formal charge. Q.) CH3NH3+ The Correct Answer and Explanation is: To draw the Lewis structure for CH\u2083NH\u2083\u207a (methylammonium ion), let’s break it down step by step: Step 1: Count the Valence Electrons Total valence electrons = 4 (from C) […]<\/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-253031","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/253031","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=253031"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/253031\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=253031"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=253031"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=253031"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}