{"id":199360,"date":"2025-03-11T15:44:32","date_gmt":"2025-03-11T15:44:32","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=199360"},"modified":"2025-03-11T15:44:54","modified_gmt":"2025-03-11T15:44:54","slug":"in-the-best-lewis-structure-for-no-what-is-the-formal-charge-on-the-n-atom","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/11\/in-the-best-lewis-structure-for-no-what-is-the-formal-charge-on-the-n-atom\/","title":{"rendered":"In the best Lewis structure for NO+"},"content":{"rendered":"\n

In the best Lewis structure for NO+, what is the formal charge on the N atom?<\/p>\n\n\n\n

A) -1<\/p>\n\n\n\n

B) 0<\/p>\n\n\n\n

C) +1<\/p>\n\n\n\n

D) +2<\/p>\n\n\n\n

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

Correct Answer: C) +1<\/strong><\/h3>\n\n\n\n

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

To determine the formal charge<\/strong> on the nitrogen atom in the best Lewis structure for NO\u207a (nitrosonium ion)<\/strong>, follow these steps:<\/p>\n\n\n\n

\n\n\n\n

Step 1: Count Valence Electrons<\/strong><\/h3>\n\n\n\n
    \n
  • Nitrogen (N)<\/strong> has 5<\/strong> valence electrons.<\/li>\n\n\n\n
  • Oxygen (O)<\/strong> has 6<\/strong> valence electrons.<\/li>\n\n\n\n
  • Since the molecule has a +1 charge<\/strong>, we subtract 1 electron<\/strong> from the total count.<\/li>\n<\/ul>\n\n\n\n

    [
    5 (N) + 6 (O) – 1 = 10 \\text{ total valence electrons}
    ]<\/p>\n\n\n\n

    \n\n\n\n

    Step 2: Draw the Skeleton Structure<\/strong><\/h3>\n\n\n\n
      \n
    • N is less electronegative<\/strong> than O, so it is the central atom<\/strong>.<\/li>\n\n\n\n
    • Connect N to O with a single bond first<\/strong> and distribute electrons to satisfy the octet rule.<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      Step 3: Complete the Octets & Assign Formal Charges<\/strong><\/h3>\n\n\n\n
        \n
      • The best Lewis structure has a triple bond<\/strong> between N and O<\/strong> because it allows for the most stable configuration.<\/li>\n\n\n\n
      • This structure ensures both atoms have an octet<\/strong> and minimizes formal charges<\/strong>.<\/li>\n<\/ul>\n\n\n\n

        Formal charge is calculated using:<\/p>\n\n\n\n

        [
        \\text{Formal Charge} = \\text{Valence Electrons} – \\text{Nonbonding Electrons} – \\frac{\\text{Bonding Electrons}}{2}
        ]<\/p>\n\n\n\n

        For Nitrogen (N):<\/strong>
        [
        \\text{Formal Charge} = 5 – 0 – \\frac{6}{2} = 5 – 3 = +1
        ]<\/p>\n\n\n\n

        For Oxygen (O):<\/strong>
        [
        \\text{Formal Charge} = 6 – 4 – \\frac{6}{2} = 6 – 3 = 0
        ]<\/p>\n\n\n\n

        \n\n\n\n

        Step 4: Confirming Stability<\/strong><\/h3>\n\n\n\n
          \n
        • The best structure<\/strong> has a triple bond<\/strong> between N and O, and a +1 formal charge on nitrogen<\/strong>.<\/li>\n\n\n\n
        • This structure obeys the octet rule<\/strong> and minimizes formal charges<\/strong>.<\/li>\n<\/ul>\n\n\n\n

          Thus, the correct answer is C) +1<\/strong>.<\/p>\n\n\n\n

          \n\n\n\n

          Image Representation of the Lewis Structure:<\/strong><\/h3>\n\n\n\n

          tLewis structure<\/strong> for NO\u207a<\/strong> <\/p>\n\n\n\n

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

          The image above shows the best Lewis structure<\/strong> for NO\u207a (nitrosonium ion)<\/strong>, with a triple bond<\/strong> between N and O<\/strong> and a +1 formal charge on nitrogen<\/strong>, confirming that the correct answer is C) +1<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"

          In the best Lewis structure for NO+, what is the formal charge on the N atom? A) -1 B) 0 C) +1 D) +2 The correct answer and explanation is : Correct Answer: C) +1 Explanation: To determine the formal charge on the nitrogen atom in the best Lewis structure for NO\u207a (nitrosonium ion), follow […]<\/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-199360","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199360","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=199360"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199360\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=199360"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=199360"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=199360"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}