{"id":203731,"date":"2025-03-20T14:35:29","date_gmt":"2025-03-20T14:35:29","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203731"},"modified":"2025-03-20T14:35:32","modified_gmt":"2025-03-20T14:35:32","slug":"construct-an-mo-diagram-for-the-he2-ion","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/20\/construct-an-mo-diagram-for-the-he2-ion\/","title":{"rendered":"Construct an MO diagram for the He+2 ion"},"content":{"rendered":"\n

Construct an MO diagram for the He+2 ion.<\/p>\n\n\n\n

a.Determine if the He+2 ion is stable or unstable?<\/p>\n\n\n\n

b.What is its bond order?<\/p>\n\n\n\n

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

To construct the Molecular Orbital (MO) diagram for the ( \\text{He}_2^+ ) ion, follow these steps:<\/p>\n\n\n\n

MO Diagram Construction:<\/strong><\/h3>\n\n\n\n
    \n
  1. Atomic Orbitals:<\/strong> Each helium atom has an electron configuration of ( 1s^2 ). In ( \\text{He}_2^+ ), we consider two helium atoms, but since one electron is removed, we have three electrons in total.<\/li>\n\n\n\n
  2. Molecular Orbitals Formation:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • The ( 1s ) orbitals of the two helium atoms combine to form:\n
        \n
      • A bonding molecular orbital (( \\sigma_{1s} ))<\/li>\n\n\n\n
      • An antibonding molecular orbital (( \\sigma_{1s}^* ))<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
          \n
        1. Electron Filling:<\/strong> The three electrons are placed in these orbitals following the Aufbau principle, Pauli-exclusion principle, and Hund’s rule.<\/li>\n<\/ol>\n\n\n\n
            \n
          • Two electrons fill the bonding ( \\sigma_{1s} ) orbital.<\/li>\n\n\n\n
          • The third electron goes into the antibonding ( \\sigma_{1s}^* ) orbital.<\/li>\n<\/ul>\n\n\n\n
            \n\n\n\n

            Bond Order Calculation:<\/strong><\/h3>\n\n\n\n

            The bond order is given by the formula:<\/p>\n\n\n\n

            [
            \\text{Bond Order} = \\frac{(\\text{Number of bonding electrons}) – (\\text{Number of antibonding electrons})}{2}
            ]<\/p>\n\n\n\n

            From the MO diagram:<\/p>\n\n\n\n

              \n
            • Bonding electrons: 2 (in ( \\sigma_{1s} ))<\/li>\n\n\n\n
            • Antibonding electrons: 1 (in ( \\sigma_{1s}^* ))<\/li>\n<\/ul>\n\n\n\n

              [
              \\text{Bond Order} = \\frac{2 – 1}{2} = 0.5
              ]<\/p>\n\n\n\n

              \n\n\n\n

              Stability of ( \\text{He}_2^+ ):<\/strong><\/h3>\n\n\n\n

              A molecule is considered stable if it has a positive bond order. Since ( \\text{He}_2^+ ) has a bond order of 0.5<\/strong>, it suggests a weakly bound species, meaning it is more stable than ( \\text{He}_2 ) (which has a bond order of 0) but still relatively weak compared to molecules with higher bond orders.<\/p>\n\n\n\n

              This suggests that ( \\text{He}_2^+ ) can exist, but it is not very stable. The single bond formed is weak and can dissociate easily.<\/p>\n\n\n\n

              \n\n\n\n

              Conclusion:<\/strong><\/h3>\n\n\n\n
                \n
              • Bond Order:<\/strong> 0.5<\/li>\n\n\n\n
              • Stability:<\/strong> Weakly stable but more stable than ( \\text{He}_2 ).<\/li>\n\n\n\n
              • Physical Implication:<\/strong> The bond is weak, meaning ( \\text{He}_2^+ ) exists only under certain conditions (such as in plasma or ionized gases).<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

                Construct an MO diagram for the He+2 ion. a.Determine if the He+2 ion is stable or unstable? b.What is its bond order? The correct answer and explanation is : To construct the Molecular Orbital (MO) diagram for the ( \\text{He}_2^+ ) ion, follow these steps: MO Diagram Construction: Bond Order Calculation: The bond order is […]<\/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-203731","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203731","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=203731"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203731\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=203731"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=203731"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=203731"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}