{"id":194703,"date":"2025-02-24T18:47:45","date_gmt":"2025-02-24T18:47:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194703"},"modified":"2025-02-24T18:47:50","modified_gmt":"2025-02-24T18:47:50","slug":"transcribed-image-text-the-lewis-structure-of-nitrous-acid-hno2-is-shown-below","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/24\/transcribed-image-text-the-lewis-structure-of-nitrous-acid-hno2-is-shown-below\/","title":{"rendered":"Transcribed image text:\u00a0The Lewis structure of nitrous acid (HNO2) is shown below"},"content":{"rendered":"\n

Transcribed image text<\/strong>: The Lewis structure of nitrous acid (HNO2) is shown below. =a. What is the formal charge for each atom in this structure? H N O (1) O (2)<\/p>\n\n\n\n

The correct answer and explanation is:<\/p>\n\n\n\n

Formal Charges in the Lewis Structure of Nitrous Acid (HNO\u2082)<\/h3>\n\n\n\n

To determine the formal charges on each atom in HNO\u2082<\/strong>, we use the formula: Formal Charge=Valence Electrons\u2212Nonbonding Electrons\u2212Bonding Electrons2\\text{Formal Charge} = \\text{Valence Electrons} – \\text{Nonbonding Electrons} – \\frac{\\text{Bonding Electrons}}{2}<\/p>\n\n\n\n

Step 1: Draw the Lewis Structure of HNO\u2082<\/strong><\/h4>\n\n\n\n
    \n
  • Hydrogen (H)<\/strong> has 1 valence electron<\/strong> and forms one single bond<\/strong> with oxygen<\/strong>.<\/li>\n\n\n\n
  • Nitrogen (N)<\/strong> has 5 valence electrons<\/strong> and forms one single bond with oxygen<\/strong> and one double bond with another oxygen<\/strong>.<\/li>\n\n\n\n
  • Oxygen (O1, single bonded to H and N)<\/strong> has 6 valence electrons<\/strong>.<\/li>\n\n\n\n
  • Oxygen (O2, double bonded to N)<\/strong> has 6 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    The correct Lewis structure follows the octet rule and minimizes formal charges.<\/p>\n\n\n\n

    Step 2: Calculate the Formal Charges<\/strong><\/h4>\n\n\n\n
      \n
    1. Hydrogen (H)<\/strong>\n
        \n
      • Valence electrons: 1<\/strong><\/li>\n\n\n\n
      • Nonbonding electrons: 0<\/strong><\/li>\n\n\n\n
      • Bonding electrons: 2<\/strong><\/li>\n\n\n\n
      • Formal Charge: 1 – 0 – (2\/2) = 0<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Nitrogen (N)<\/strong>\n
          \n
        • Valence electrons: 5<\/strong><\/li>\n\n\n\n
        • Nonbonding electrons: 0<\/strong><\/li>\n\n\n\n
        • Bonding electrons: 8 (2 single + 1 double bond)<\/strong><\/li>\n\n\n\n
        • Formal Charge: 5 – 0 – (8\/2) = 5 – 4 = +1<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Oxygen (O1) – Single bonded to H and N<\/strong>\n
            \n
          • Valence electrons: 6<\/strong><\/li>\n\n\n\n
          • Nonbonding electrons: 6<\/strong><\/li>\n\n\n\n
          • Bonding electrons: 2<\/strong><\/li>\n\n\n\n
          • Formal Charge: 6 – 6 – (2\/2) = 6 – 6 – 1 = -1<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Oxygen (O2) – Double bonded to N<\/strong>\n
              \n
            • Valence electrons: 6<\/strong><\/li>\n\n\n\n
            • Nonbonding electrons: 4<\/strong><\/li>\n\n\n\n
            • Bonding electrons: 4<\/strong><\/li>\n\n\n\n
            • Formal Charge: 6 – 4 – (4\/2) = 6 – 4 – 2 = 0<\/strong><\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

              Final Formal Charges:<\/strong><\/h3>\n\n\n\n
                \n
              • H = 0<\/strong><\/li>\n\n\n\n
              • N = +1<\/strong><\/li>\n\n\n\n
              • O1 (Single bonded to H and N) = -1<\/strong><\/li>\n\n\n\n
              • O2 (Double bonded to N) = 0<\/strong><\/li>\n<\/ul>\n\n\n\n

                Thus, the overall charge of HNO\u2082 is neutral<\/strong> because the sum of formal charges equals zero.<\/p>\n\n\n\n

                Now, I’ll generate an image of the correct Lewis structure.<\/p>\n\n\n\n

                Here is the Lewis structure of nitrous acid (HNO\u2082) with formal charges labeled. Let me know if you need any modifications or further explanations!<\/p>\n\n\n\n

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

                Transcribed image text: The Lewis structure of nitrous acid (HNO2) is shown below. =a. What is the formal charge for each atom in this structure? H N O (1) O (2) The correct answer and explanation is: Formal Charges in the Lewis Structure of Nitrous Acid (HNO\u2082) To determine the formal charges on each atom in […]<\/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-194703","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194703","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=194703"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194703\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194703"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194703"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194703"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}