{"id":204050,"date":"2025-03-21T09:06:40","date_gmt":"2025-03-21T09:06:40","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=204050"},"modified":"2025-03-21T09:06:51","modified_gmt":"2025-03-21T09:06:51","slug":"draw-the-lewis-structure-for-n3-you-can-use-the-back-of-sheet-to-draw-ls","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/21\/draw-the-lewis-structure-for-n3-you-can-use-the-back-of-sheet-to-draw-ls\/","title":{"rendered":"Draw the Lewis structure for N3 (You can use the back of sheet to draw LS)"},"content":{"rendered":"\n

Draw the Lewis structure for N3 (You can use the back of sheet to draw LS).<\/p>\n\n\n\n

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

The Lewis structure<\/strong> for the azide ion (N\u2083\u207b)<\/strong> consists of three nitrogen atoms connected in a linear arrangement. To construct the correct Lewis structure<\/strong>, follow these steps:<\/p>\n\n\n\n

Step 1: Count the Valence Electrons<\/strong><\/h3>\n\n\n\n
    \n
  • Nitrogen (N) has 5 valence electrons<\/strong>.<\/li>\n\n\n\n
  • Since there are three nitrogen atoms<\/strong>, the total valence electrons from nitrogen atoms = 5 \u00d7 3 = 15<\/strong>.<\/li>\n\n\n\n
  • The negative charge (\u207b1)<\/strong> means one additional electron<\/strong>, making the total 16 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    Step 2: Draw a Skeleton Structure<\/strong><\/h3>\n\n\n\n
      \n
    • The three nitrogen atoms are placed linearly<\/strong>: N \u2013 N \u2013 N<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      Step 3: Distribute Electrons<\/strong><\/h3>\n\n\n\n
        \n
      1. Assign single bonds between nitrogen atoms:
        N \u2013 N \u2013 N<\/strong> (uses 2 electrons).<\/li>\n\n\n\n
      2. Distribute remaining 14 electrons<\/strong> to satisfy the octet rule<\/strong>.<\/li>\n\n\n\n
      3. To satisfy the octet rule<\/strong>, resonance structures<\/strong> are considered.<\/li>\n<\/ol>\n\n\n\n

        Step 4: Assign Formal Charges<\/strong><\/h3>\n\n\n\n

        Formal charge is calculated as:
        [
        \\text{Formal Charge} = \\text{Valence Electrons} – \\text{Nonbonding Electrons} – \\frac{\\text{Bonding Electrons}}{2}
        ]
        The best Lewis structure<\/strong> has two possible resonance forms<\/strong>:<\/p>\n\n\n\n

          \n
        1. [N\u2261N\u2013N]\u207b<\/strong><\/li>\n\n\n\n
        2. [N\u2013N\u2261N]\u207b<\/strong><\/li>\n<\/ol>\n\n\n\n
            \n
          • The central nitrogen<\/strong> carries a +1 charge<\/strong>.<\/li>\n\n\n\n
          • One terminal nitrogen has a -1 charge<\/strong>.<\/li>\n\n\n\n
          • The overall charge remains -1<\/strong>.<\/li>\n<\/ul>\n\n\n\n

            Conclusion<\/strong><\/h3>\n\n\n\n

            The azide ion (N\u2083\u207b)<\/strong> exhibits resonance<\/strong>, making it more stable<\/strong>. It has a linear shape<\/strong> and sp hybridization<\/strong>. Due to delocalized electrons, azide is highly reactive<\/strong>, often used in explosives<\/strong> like sodium azide (NaN\u2083).<\/p>\n","protected":false},"excerpt":{"rendered":"

            Draw the Lewis structure for N3 (You can use the back of sheet to draw LS). The correct answer and explanation is : The Lewis structure for the azide ion (N\u2083\u207b) consists of three nitrogen atoms connected in a linear arrangement. To construct the correct Lewis structure, follow these steps: Step 1: Count the Valence […]<\/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-204050","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/204050","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=204050"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/204050\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=204050"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=204050"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=204050"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}