{"id":249597,"date":"2025-07-09T17:41:20","date_gmt":"2025-07-09T17:41:20","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=249597"},"modified":"2025-07-09T17:41:22","modified_gmt":"2025-07-09T17:41:22","slug":"describe-the-bonding-in-the-c2-2-ion-in-terms-of-molecular-orbital-theory-and-compare-the-bond-order-to-that-of-c2-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/09\/describe-the-bonding-in-the-c2-2-ion-in-terms-of-molecular-orbital-theory-and-compare-the-bond-order-to-that-of-c2-2\/","title":{"rendered":"Describe the bonding in the C2 2- ion in terms of molecular orbital theory and compare the bond order to that of C2."},"content":{"rendered":"\n

Describe the bonding in the C2 2- ion in terms of molecular orbital theory and compare the bond order to that of C2.<\/p>\n\n\n\n

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

The bonding in the C\u2082\u00b2\u207b ion can be explained using molecular orbital theory. In this theory, atomic orbitals combine to form molecular orbitals, which are filled according to the Pauli Exclusion Principle and Hund’s Rule.<\/p>\n\n\n\n

    \n
  1. Atomic Orbitals<\/strong>: Carbon (C) has an atomic number of 6, meaning its electrons are arranged as 1s\u00b2 2s\u00b2 2p\u00b2. For the C\u2082 molecule, each carbon atom contributes two 2s and two 2p orbitals.<\/li>\n\n\n\n
  2. Molecular Orbitals<\/strong>: When two carbon atoms bond, their atomic orbitals combine to form molecular orbitals. The bonding orbitals are called \u03c3 and \u03c0 orbitals. The molecular orbitals for the C\u2082\u00b2\u207b ion are:
    • From the two 2s orbitals: one \u03c3(2s) (bonding), one \u03c3*(2s) (antibonding).<\/li>
    • From the two 2p orbitals: one \u03c3(2p) (bonding), two \u03c0(2p) (bonding), and one \u03c0*(2p) (antibonding).<\/li><\/ul>In the case of the C\u2082\u00b2\u207b ion, there are two additional electrons compared to the neutral C\u2082 molecule. These electrons occupy the antibonding \u03c0*(2p) orbitals, which lowers the bond order.<\/li>\n\n\n\n
    • Bond Order Calculation<\/strong>: The bond order is given by the formula: Bond\u00a0Order=12(Bonding\u00a0Electrons\u2212Antibonding\u00a0Electrons)\\text{Bond Order} = \\frac{1}{2} (\\text{Bonding Electrons} – \\text{Antibonding Electrons})Bond\u00a0Order=21\u200b(Bonding\u00a0Electrons\u2212Antibonding\u00a0Electrons) For C\u2082\u00b2\u207b:\n
        \n
      • Bonding electrons: 2 (\u03c3(2s)) + 2 (\u03c0(2p)) = 4.<\/li>\n\n\n\n
      • Antibonding electrons: 2 (\u03c3*(2s)) + 2 (\u03c0*(2p)) = 4.<\/li>\n\n\n\n
      • Bond order = \u00bd(4 – 4) = 0.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Comparison with C\u2082<\/strong>: In the neutral C\u2082 molecule, the bond order is calculated as: Bond\u00a0Order=12(8\u22124)=2.\\text{Bond Order} = \\frac{1}{2} (8 – 4) = 2.Bond\u00a0Order=21\u200b(8\u22124)=2. Therefore, the bond order in C\u2082\u00b2\u207b is 0, indicating no net bonding between the carbon atoms, while the bond order in C\u2082 is 2, suggesting a stable double bond between the carbon atoms.<\/li>\n<\/ol>\n\n\n\n
        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

        Describe the bonding in the C2 2- ion in terms of molecular orbital theory and compare the bond order to that of C2. The Correct Answer and Explanation is: The bonding in the C\u2082\u00b2\u207b ion can be explained using molecular orbital theory. In this theory, atomic orbitals combine to form molecular orbitals, which are filled […]<\/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-249597","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249597","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=249597"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249597\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=249597"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=249597"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=249597"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}