{"id":244154,"date":"2025-07-04T19:47:43","date_gmt":"2025-07-04T19:47:43","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=244154"},"modified":"2025-07-04T19:47:45","modified_gmt":"2025-07-04T19:47:45","slug":"chemical-bonding-using-the-mo-model-to-predict-bond-order-and-paramagnetism-complete-the-table-below-which-lists-information-about-some-diatomic-molecules-or-molecular-ions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/04\/chemical-bonding-using-the-mo-model-to-predict-bond-order-and-paramagnetism-complete-the-table-below-which-lists-information-about-some-diatomic-molecules-or-molecular-ions\/","title":{"rendered":"CHEMICAL BONDING Using the MO model to predict bond order and paramagnetism Complete the table below, which lists information about some diatomic molecules or molecular ions"},"content":{"rendered":"\n

CHEMICAL BONDING Using the MO model to predict bond order and paramagnetism Complete the table below, which lists information about some diatomic molecules or molecular ions. In particular: Decide whether each molecule is stable or not Decide whether each molecule would be diamagnetic or paramagnetic. Calculate each molecule’s bond order; diamagnetic or paramagnetic? molecule stable? bond order yes diamagnetic no paramagnetic 2 yes diamagnetic paramagnetic yes diamagnetic Ne2 no paramagnetic Liz<\/p>\n\n\n\n

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

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

Completed Table:<\/strong><\/p>\n\n\n\n

molecule<\/td>stable?<\/td>diamagnetic or paramagnetic?<\/td>bond order<\/td><\/tr>
Li\u2082\u207a<\/td>yes<\/strong><\/td>paramagnetic<\/strong><\/td>0.5<\/strong><\/td><\/tr>
O\u2082\u207a<\/td>yes<\/strong><\/td>paramagnetic<\/strong><\/td>2.5<\/strong><\/td><\/tr>
Ne\u2082\u207a<\/td>yes<\/strong><\/td>paramagnetic<\/strong><\/td>0.5<\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

Explanation:<\/strong><\/p>\n\n\n\n

To determine the properties of these diatomic species, we use Molecular Orbital (MO) theory. The stability, magnetic properties, and bond order are derived from the species’ MO electron configuration.<\/p>\n\n\n\n

    \n
  1. Stability:<\/strong>\u00a0A molecule or ion is considered stable if its bond order is greater than zero (BO > 0).<\/li>\n\n\n\n
  2. Bond Order (BO):<\/strong>\u00a0Calculated as BO = \u00bd (Number of electrons in bonding MOs – Number of electrons in antibonding MOs).<\/li>\n\n\n\n
  3. Magnetic Properties:<\/strong>\u00a0A species is\u00a0paramagnetic<\/strong>\u00a0if it has one or more unpaired electrons and is\u00a0diamagnetic<\/strong>\u00a0if all its electrons are paired.<\/li>\n<\/ol>\n\n\n\n

    Analysis of each species:<\/strong><\/p>\n\n\n\n

      \n
    • Li\u2082\u207a:<\/strong>\u00a0A lithium (Li) atom has 3 electrons. The Li\u2082\u207a ion has (2 \u00d7 3) – 1 = 5 electrons. Its MO configuration is (\u03c3\u2081s)\u00b2(\u03c3*\u2081s)\u00b2(\u03c3\u2082s)\u00b9.\n
        \n
      • Bond Order:<\/strong>\u00a0There are 3 electrons in bonding orbitals (\u03c3\u2081s, \u03c3\u2082s) and 2 in antibonding orbitals (\u03c3*\u2081s). BO = \u00bd (3 – 2) =\u00a00.5<\/strong>.<\/li>\n\n\n\n
      • Stability:<\/strong>\u00a0Since the bond order is 0.5 (> 0), Li\u2082\u207a is\u00a0stable<\/strong>.<\/li>\n\n\n\n
      • Magnetism:<\/strong>\u00a0The \u03c3\u2082s orbital contains one unpaired electron, making Li\u2082\u207a\u00a0paramagnetic<\/strong>.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • O\u2082\u207a:<\/strong>\u00a0An oxygen (O) atom has 8 electrons. The O\u2082\u207a ion has (2 \u00d7 8) – 1 = 15 electrons. Its valence electron MO configuration is (\u03c3\u2082s)\u00b2(\u03c3\u2082s)\u00b2(\u03c3\u2082p)\u00b2(\u03c0\u2082p)\u2074(\u03c0<\/em>\u2082p)\u00b9.\n
          \n
        • Bond Order:<\/strong>\u00a0There are 8 valence electrons in bonding orbitals (\u03c3\u2082s, \u03c3\u2082p, \u03c0\u2082p) and 3 in antibonding orbitals (\u03c3\u2082s, \u03c0<\/em>\u2082p). BO = \u00bd (8 – 3) =\u00a02.5<\/strong>.<\/li>\n\n\n\n
        • Stability:<\/strong>\u00a0With a bond order of 2.5, O\u2082\u207a is\u00a0stable<\/strong>.<\/li>\n\n\n\n
        • Magnetism:<\/strong>\u00a0The \u03c0*\u2082p antibonding orbitals have one unpaired electron, making O\u2082\u207a\u00a0paramagnetic<\/strong>.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Ne\u2082\u207a:<\/strong>\u00a0A neon (Ne) atom has 10 electrons. The Ne\u2082\u207a ion has (2 \u00d7 10) – 1 = 19 electrons. Its valence electron MO configuration is (\u03c3\u2082s)\u00b2(\u03c3\u2082s)\u00b2(\u03c3\u2082p)\u00b2(\u03c0\u2082p)\u2074(\u03c0<\/em>\u2082p)\u2074(\u03c3*\u2082p)\u00b9.\n
            \n
          • Bond Order:<\/strong>\u00a0There are 8 valence electrons in bonding orbitals and 7 in antibonding orbitals. BO = \u00bd (8 – 7) =\u00a00.5<\/strong>.<\/li>\n\n\n\n
          • Stability:<\/strong>\u00a0The bond order is 0.5, so Ne\u2082\u207a is predicted to be\u00a0stable<\/strong>, unlike the Ne\u2082 molecule which has a bond order of 0.<\/li>\n\n\n\n
          • Magnetism:<\/strong>\u00a0There is one unpaired electron in the \u03c3*\u2082p orbital, making Ne\u2082\u207a\u00a0paramagnetic<\/strong>.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
            \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

            CHEMICAL BONDING Using the MO model to predict bond order and paramagnetism Complete the table below, which lists information about some diatomic molecules or molecular ions. In particular: Decide whether each molecule is stable or not Decide whether each molecule would be diamagnetic or paramagnetic. Calculate each molecule’s bond order; diamagnetic or paramagnetic? molecule stable? […]<\/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-244154","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/244154","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=244154"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/244154\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=244154"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=244154"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=244154"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}