{"id":185436,"date":"2025-01-22T14:16:17","date_gmt":"2025-01-22T14:16:17","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185436"},"modified":"2025-01-22T14:16:19","modified_gmt":"2025-01-22T14:16:19","slug":"sketch-the-molecular-orbital-energy-level-diagrams-for-brcl-and-deduce-its-ground-state-electron-configurations","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/sketch-the-molecular-orbital-energy-level-diagrams-for-brcl-and-deduce-its-ground-state-electron-configurations\/","title":{"rendered":"Sketch the molecular orbital energy level diagrams for BrCl and deduce its ground-state electron configurations"},"content":{"rendered":"\n

Sketch the molecular orbital energy level diagrams for BrCl and deduce its ground-state electron configurations. Is BrCl likely to have a shorter bond length than BrCl-?<\/p>\n\n\n\n

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

The molecular orbital energy level diagram for a diatomic molecule like BrCl involves filling the molecular orbitals formed by the combination of atomic orbitals from the constituent atoms (bromine and chlorine in this case). The molecular orbitals can be formed from the combination of atomic orbitals, and based on the symmetry and energy levels, these orbitals will be filled with electrons according to the Pauli exclusion principle and Hund’s rule.<\/p>\n\n\n\n

Molecular Orbital Energy Level Diagram for BrCl:<\/h3>\n\n\n\n
    \n
  1. Atomic Orbitals:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • Bromine (Br) has 7 valence electrons (from the 4p orbital).<\/li>\n\n\n\n
    • Chlorine (Cl) also has 7 valence electrons (from the 3p orbital).<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Molecular Orbitals:<\/strong>
        The molecular orbitals formed will be \u03c3, \u03c3, \u03c0, and \u03c0<\/em> orbitals from the combination of the atomic p-orbitals. The diagram will involve:<\/li>\n<\/ol>\n\n\n\n
          \n
        • \u03c3(2pz) and \u03c3*(2pz) molecular orbitals.<\/li>\n\n\n\n
        • \u03c0(2px) and \u03c0(2py) and their respective antibonding orbitals \u03c0(2px) and \u03c0<\/em>(2py).<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Electron Configuration:<\/strong>
            For BrCl, since both atoms contribute 7 valence electrons each, the total number of valence electrons will be 14. These electrons will fill the molecular orbitals from lowest to highest energy:<\/li>\n<\/ol>\n\n\n\n
              \n
            • \u03c3(2pz) will be filled with 2 electrons.<\/li>\n\n\n\n
            • \u03c0(2px) and \u03c0(2py) will be filled with 4 electrons (2 in each).<\/li>\n\n\n\n
            • \u03c3*(2pz) will be filled with 2 electrons.<\/li>\n\n\n\n
            • The antibonding \u03c0* orbitals (\u03c0(2px) and \u03c0<\/em>(2py)) will not be filled.<\/li>\n<\/ul>\n\n\n\n

              Thus, the electron configuration of BrCl would be:
              [ \\sigma(2pz)^2 \\, \\pi(2px)^2 \\, \\pi(2py)^2 \\, \\sigma^*(2pz)^2 ]<\/p>\n\n\n\n

              Ground-State Electron Configuration:<\/h3>\n\n\n\n
                \n
              • For BrCl, the electrons fill in a way that results in a bond order of 2 (because 10 bonding electrons and 4 antibonding electrons give a bond order of ( \\frac{10-4}{2} = 3 )).<\/li>\n<\/ul>\n\n\n\n

                Is BrCl likely to have a shorter bond length than BrCl-?<\/h3>\n\n\n\n

                No, BrCl is likely to have a shorter bond length than BrCl-. This is because BrCl- has an extra electron, leading to increased electron-electron repulsion. The additional electron occupies an antibonding molecular orbital, weakening the bond. In contrast, BrCl has a more stable bond with fewer electrons in antibonding orbitals, leading to a stronger bond and thus a shorter bond length.<\/p>\n","protected":false},"excerpt":{"rendered":"

                Sketch the molecular orbital energy level diagrams for BrCl and deduce its ground-state electron configurations. Is BrCl likely to have a shorter bond length than BrCl-? The Correct Answer and Explanation is : The molecular orbital energy level diagram for a diatomic molecule like BrCl involves filling the molecular orbitals formed by the combination of […]<\/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-185436","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185436","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=185436"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185436\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185436"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185436"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185436"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}