{"id":154480,"date":"2024-10-14T18:09:40","date_gmt":"2024-10-14T18:09:40","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=154480"},"modified":"2024-10-14T18:09:43","modified_gmt":"2024-10-14T18:09:43","slug":"write-the-molecular-orbital-configuration-of-be2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/14\/write-the-molecular-orbital-configuration-of-be2\/","title":{"rendered":"Write the molecular orbital configuration of Be2."},"content":{"rendered":"\n

Write the molecular orbital configuration of Be2. Calculate its bond order and predict its magnetic behavior and stability.<\/p>\n\n\n\n

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

Molecular Orbital Configuration of Be\u2082<\/h3>\n\n\n\n

Beryllium (Be) has an atomic number of 4, and its electron configuration is ( 1s^2 2s^2 ). When two beryllium atoms combine to form the diatomic molecule Be\u2082, the molecular orbital theory is used to determine the molecular orbital configuration.<\/p>\n\n\n\n

The molecular orbitals for Be\u2082 can be represented as follows:<\/p>\n\n\n\n

    \n
  1. Bonding Molecular Orbitals:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • ( \\sigma_{1s} ): Filled with 2 electrons from the 1s orbitals of each Be atom.<\/li>\n\n\n\n
    • ( \\sigma_{2s} ): Filled with 2 electrons from the 2s orbitals of each Be atom.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Antibonding Molecular Orbitals:<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • ( \\sigma^*_{2s} ): Unoccupied (0 electrons).<\/li>\n<\/ul>\n\n\n\n

          Thus, the molecular orbital configuration for Be\u2082 is:<\/p>\n\n\n\n

          [
          \\text{Be}2: ( \\sigma<\/em>{1s} )^2 ( \\sigma_{2s} )^2 ( \\sigma^*_{2s} )^0
          ]<\/p>\n\n\n\n

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

          The bond order can be calculated using the formula:<\/p>\n\n\n\n

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

          For Be\u2082:<\/p>\n\n\n\n

            \n
          • Electrons in bonding MOs: ( 2 (\\sigma_{1s}) + 2 (\\sigma_{2s}) = 4 )<\/li>\n\n\n\n
          • Electrons in antibonding MOs: ( 0 (\\sigma^*_{2s}) = 0 )<\/li>\n<\/ul>\n\n\n\n

            Therefore, the bond order is:<\/p>\n\n\n\n

            [
            \\text{Bond Order} = \\frac{4 – 0}{2} = 2
            ]<\/p>\n\n\n\n

            Magnetic Behavior and Stability<\/h3>\n\n\n\n
              \n
            1. Magnetic Behavior:<\/strong> Be\u2082 has no unpaired electrons in its molecular orbitals, making it diamagnetic<\/strong>. This means that it will not be attracted to a magnetic field.<\/li>\n\n\n\n
            2. Stability:<\/strong> The bond order of 2 indicates that Be\u2082 has a strong double bond, suggesting that the molecule is stable. However, due to the relatively small size of beryllium and the resulting weak overlapping of the ( s ) orbitals, Be\u2082 is not a very stable molecule under normal conditions. In fact, it is considered less stable than other diatomic molecules like O\u2082 or N\u2082.<\/li>\n<\/ol>\n\n\n\n

              In summary, the molecular orbital configuration of Be\u2082 reveals a bond order of 2, indicating a stable diatomic molecule that is diamagnetic due to the absence of unpaired electrons.<\/p>\n","protected":false},"excerpt":{"rendered":"

              Write the molecular orbital configuration of Be2. Calculate its bond order and predict its magnetic behavior and stability. The Correct Answer and Explanation is: Molecular Orbital Configuration of Be\u2082 Beryllium (Be) has an atomic number of 4, and its electron configuration is ( 1s^2 2s^2 ). When two beryllium atoms combine to form the diatomic […]<\/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-154480","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/154480","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=154480"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/154480\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=154480"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=154480"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=154480"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}