{"id":228096,"date":"2025-06-07T03:09:15","date_gmt":"2025-06-07T03:09:15","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=228096"},"modified":"2025-06-07T03:09:17","modified_gmt":"2025-06-07T03:09:17","slug":"cn-draw-the-lewis-dot-structure-for-cn-include-all-lone-pairs-of-electrons_","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/07\/cn-draw-the-lewis-dot-structure-for-cn-include-all-lone-pairs-of-electrons_\/","title":{"rendered":"CN Draw the Lewis dot structure for CN Include all lone pairs of electrons_"},"content":{"rendered":"\n
CN Draw the Lewis dot structure for CN Include all lone pairs of electrons_<\/pre>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
Lewis Dot Structure for CN\u207b (Cyanide Ion)<\/h3>\n\n\n\n
The Lewis dot structure for CN\u207b<\/strong> (cyanide ion) is:<\/p>\n\n\n\n
mathematicaCopyEdit:\u207bC\u2261N:\n<\/code><\/pre>\n\n\n\n
or more fully:<\/p>\n\n\n\n
mathematicaCopyEdit..   ..\n:C\u2261N:\u207b\n<\/code><\/pre>\n\n\n\n
Where:<\/p>\n\n\n\n
    \n
  • Carbon (C) and Nitrogen (N) are triple bonded (\u2261).<\/li>\n\n\n\n
  • Carbon has one lone pair (two dots).<\/li>\n\n\n\n
  • Nitrogen has one lone pair.<\/li>\n\n\n\n
  • The overall structure carries a negative charge<\/strong> (\u207b).<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n
    Explanation:<\/h3>\n\n\n\n
    The cyanide ion (CN\u207b) is a diatomic ion<\/strong> composed of a carbon atom bonded to a nitrogen atom. To understand and draw its Lewis structure, we follow these steps:<\/p>\n\n\n\n
    1. Determine Total Valence Electrons<\/strong>:<\/h4>\n\n\n\n
      \n
    • Carbon has 4 valence electrons.<\/li>\n\n\n\n
    • Nitrogen has 5 valence electrons.<\/li>\n\n\n\n
    • The negative charge (\u207b) adds 1 extra electron.<\/li>\n\n\n\n
    • Total = 4 + 5 + 1 = 10 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n
      2. Arrange Atoms<\/strong>:<\/h4>\n\n\n\n
      Carbon and nitrogen are placed side by side: C \u2014 N.<\/p>\n\n\n\n
      3. Create Bonds<\/strong>:<\/h4>\n\n\n\n
      Start by forming single, double, and then triple bonds between C and N to satisfy the octet rule. A triple bond (\u2261)<\/strong> is necessary to fulfill the octet rule for both atoms efficiently while using the fewest electrons.<\/p>\n\n\n\n
      4. Assign Lone Pairs<\/strong>:<\/h4>\n\n\n\n
      After forming the C\u2261N bond (6 electrons used), we place the remaining 4 electrons (10 total – 6 bonding = 4 left) as lone pairs:<\/p>\n\n\n\n
        \n
      • 2 electrons on carbon \u2192 1 lone pair.<\/li>\n\n\n\n
      • 2 electrons on nitrogen \u2192 1 lone pair.<\/li>\n<\/ul>\n\n\n\n
        Each atom now has 8 electrons around it:<\/p>\n\n\n\n
          \n
        • Carbon: 6 (bonding) + 2 (lone pair) = 8.<\/li>\n\n\n\n
        • Nitrogen: 6 (bonding) + 2 (lone pair) = 8.<\/li>\n<\/ul>\n\n\n\n
          5. Assign Formal Charges<\/strong>:<\/h4>\n\n\n\n
          Formal charge = (Valence e\u207b) \u2013 (Nonbonding e\u207b) \u2013 (\u00bd \u00d7 Bonding e\u207b)<\/p>\n\n\n\n
            \n
          • Carbon: 4 \u2013 2 \u2013 (6\/2) = 4 \u2013 2 \u2013 3 = -1<\/strong><\/li>\n\n\n\n
          • Nitrogen: 5 \u2013 2 \u2013 (6\/2) = 5 \u2013 2 \u2013 3 = 0<\/strong><\/li>\n<\/ul>\n\n\n\n
            This gives an overall charge of \u20131<\/strong>, consistent with the CN\u207b ion.<\/p>\n\n\n\n
            Thus, the Lewis structure of CN\u207b shows a triple bond<\/strong> and lone pairs on both atoms, with the negative charge residing on the carbon atom<\/strong>.<\/p>\n\n\n\n
            \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
            CN Draw the Lewis dot structure for CN Include all lone pairs of electrons_ The Correct Answer and Explanation is: Lewis Dot Structure for CN\u207b (Cyanide Ion) The Lewis dot structure for CN\u207b (cyanide ion) is: mathematicaCopyEdit:\u207bC\u2261N: or more fully: mathematicaCopyEdit.. .. :C\u2261N:\u207b Where: Explanation: The cyanide ion (CN\u207b) is a diatomic ion composed of […]<\/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-228096","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/228096","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=228096"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/228096\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=228096"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=228096"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=228096"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}