{"id":183387,"date":"2025-01-16T12:14:12","date_gmt":"2025-01-16T12:14:12","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=183387"},"modified":"2025-01-16T12:14:14","modified_gmt":"2025-01-16T12:14:14","slug":"construct-the-molecular-orbital-diagram-for-h2-and-then-identify-the-bond-order","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/16\/construct-the-molecular-orbital-diagram-for-h2-and-then-identify-the-bond-order\/","title":{"rendered":"Construct the molecular orbital diagram for H2- and then identify the bond order"},"content":{"rendered":"\n

Construct the molecular orbital diagram for H2- and then identify the bond order.<\/p>\n\n\n\n

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

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

Molecular Orbital Diagram for ( \\text{H}_2^- )<\/h3>\n\n\n\n

To construct the molecular orbital (MO) diagram for ( \\text{H}_2^- ) (a hydrogen molecule with one extra electron), follow these steps:<\/p>\n\n\n\n

    \n
  1. Atomic Orbitals<\/strong>: Each hydrogen atom contributes one 1s atomic orbital. These combine to form molecular orbitals.<\/li>\n\n\n\n
  2. Formation of Molecular Orbitals<\/strong>:<\/li>\n<\/ol>\n\n\n\n
      \n
    • The constructive interference of 1s orbitals forms a bonding molecular orbital (( \\sigma_{1s} )).<\/li>\n\n\n\n
    • The destructive interference forms an antibonding molecular orbital (( \\sigma_{1s}^* )).<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Electron Configuration<\/strong>:<\/li>\n<\/ol>\n\n\n\n
          \n
        • A neutral ( \\text{H}2 ) molecule has 2 electrons, which fill the lower-energy ( \\sigma<\/em>{1s} ) orbital.<\/li>\n\n\n\n
        • In ( \\text{H}2^- ), the extra electron is added to the higher-energy ( \\sigma<\/em>{1s}^* ) orbital.<\/li>\n<\/ul>\n\n\n\n

          Molecular Orbital Diagram:<\/h3>\n\n\n\n
            \n
          • Energy Levels<\/strong>:<\/li>\n\n\n\n
          • ( \\sigma_{1s} ) (lower energy, bonding)<\/li>\n\n\n\n
          • ( \\sigma_{1s}^* ) (higher energy, antibonding)<\/li>\n\n\n\n
          • Electron Distribution<\/strong>:<\/li>\n\n\n\n
          • ( \\sigma_{1s} ): 2 electrons<\/li>\n\n\n\n
          • ( \\sigma_{1s}^* ): 1 electron<\/li>\n<\/ul>\n\n\n\n

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

            The bond order is given by the formula:
            [
            \\text{Bond Order} = \\frac{\\text{Number of bonding electrons} – \\text{Number of antibonding electrons}}{2}
            ]<\/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

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

              The ( \\text{H}_2^- ) ion has a bond order of 0.5, indicating a weaker bond than neutral ( \\text{H}_2 ) (bond order = 1). The additional electron in the antibonding orbital partially cancels the stabilization provided by the bonding orbital. This bond is weaker and longer than in ( \\text{H}_2 ), but the molecule still exists due to the net bonding interaction. This explains why ( \\text{H}_2^- ) is less stable than ( \\text{H}_2 ).<\/p>\n\n\n\n

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

              Construct the molecular orbital diagram for H2- and then identify the bond order. The Correct Answer and Explanation is : Molecular Orbital Diagram for ( \\text{H}_2^- ) To construct the molecular orbital (MO) diagram for ( \\text{H}_2^- ) (a hydrogen molecule with one extra electron), follow these steps: Molecular Orbital Diagram: Bond Order Calculation: The […]<\/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-183387","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183387","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=183387"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183387\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183387"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183387"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183387"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}