{"id":240482,"date":"2025-07-03T09:43:29","date_gmt":"2025-07-03T09:43:29","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=240482"},"modified":"2025-07-03T09:43:31","modified_gmt":"2025-07-03T09:43:31","slug":"lewis-structure","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/03\/lewis-structure\/","title":{"rendered":"Lewis Structure"},"content":{"rendered":"\n

Lewis Structure :N-C-C-N: Total # O Sigma Bonds Total # of Pi Bonds<\/p>\n\n\n\n

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

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

Total # of Sigma Bonds:<\/strong> 3
Total # of Pi Bonds:<\/strong> 4<\/p>\n\n\n\n

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

To determine the number of sigma (\u03c3) and pi (\u03c0) bonds in the Lewis structure for dicyanogen, :N\u2261C\u2212C\u2261N:, we must first understand the composition of single, double, and triple covalent bonds.<\/p>\n\n\n\n

Sigma (\u03c3) Bonds:<\/strong> A sigma bond is the first covalent bond formed between two atoms. It is created by the direct, head-on overlap of atomic orbitals along the imaginary line connecting the two nuclei. Every covalent bond, regardless of whether it is single, double, or triple, contains exactly one sigma bond. These bonds are the strongest type of covalent bond.<\/p>\n\n\n\n

Pi (\u03c0) Bonds:<\/strong> Pi bonds are formed by the parallel, or sideways, overlap of p-orbitals. They can only form after a sigma bond has already been established between two atoms. Pi bonds constitute the second bond in a double bond and the second and third bonds in a triple bond. They are generally weaker than sigma bonds.<\/p>\n\n\n\n

The rules are as follows:<\/p>\n\n\n\n

    \n
  • A\u00a0single bond<\/strong>\u00a0consists of 1 sigma bond.<\/li>\n\n\n\n
  • A\u00a0double bond<\/strong>\u00a0consists of 1 sigma bond and 1 pi bond.<\/li>\n\n\n\n
  • A\u00a0triple bond<\/strong>\u00a0consists of 1 sigma bond and 2 pi bonds.<\/li>\n<\/ul>\n\n\n\n

    Now, let’s analyze the molecule :N\u2261C\u2212C\u2261N: step by step:<\/p>\n\n\n\n

      \n
    1. Central C\u2212C Bond:<\/strong>\u00a0There is a single bond connecting the two carbon atoms. According to our rules, this single bond consists of\u00a01 sigma bond<\/strong>.<\/li>\n\n\n\n
    2. Two N\u2261C Bonds:<\/strong>\u00a0The molecule has two identical triple bonds, one between each nitrogen and carbon atom. Each triple bond is composed of\u00a01 sigma bond and 2 pi bonds<\/strong>.<\/li>\n<\/ol>\n\n\n\n

      To find the total number of each type of bond, we sum the counts from each part of the molecule:<\/p>\n\n\n\n

        \n
      • Total Sigma (\u03c3) Bonds:<\/strong>\u00a0We add the sigma bond from the central C\u2212C bond and one sigma bond from each of the two N\u2261C triple bonds.
        Total \u03c3 = 1 (from C\u2212C) + 1 (from N\u2261C) + 1 (from C\u2261N) =\u00a03 sigma bonds<\/strong>.<\/li>\n\n\n\n
      • Total Pi (\u03c0) Bonds:<\/strong>\u00a0We add the pi bonds from the two N\u2261C triple bonds. The central C\u2212C single bond contributes no pi bonds.
        Total \u03c0 = 2 (from the first N\u2261C) + 2 (from the second C\u2261N) =\u00a04 pi bonds<\/strong>.<\/li>\n<\/ul>\n\n\n\n

        Therefore, the dicyanogen molecule contains a total of 3 sigma bonds and 4 pi bonds. The lone pairs on the nitrogen atoms are non-bonding electrons and do not contribute to this count<\/p>\n\n\n\n

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

        Lewis Structure :N-C-C-N: Total # O Sigma Bonds Total # of Pi Bonds The Correct Answer and Explanation is: Total # of Sigma Bonds: 3Total # of Pi Bonds: 4 Explanation To determine the number of sigma (\u03c3) and pi (\u03c0) bonds in the Lewis structure for dicyanogen, :N\u2261C\u2212C\u2261N:, we must first understand the composition of single, […]<\/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-240482","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240482","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=240482"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/240482\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=240482"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=240482"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=240482"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}