{"id":244159,"date":"2025-07-04T19:54:40","date_gmt":"2025-07-04T19:54:40","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=244159"},"modified":"2025-07-04T19:54:42","modified_gmt":"2025-07-04T19:54:42","slug":"chemical-bonding","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/04\/chemical-bonding\/","title":{"rendered":"Chemical Bonding"},"content":{"rendered":"\n

Chemical Bonding: Predicting Bond Order and Paramagnetism Using the MO Model To determine the stability and magnetic properties of diatomic molecules, we can use the molecular orbital (MO) model. The table below provides information about some diatomic molecules. Please complete the table by deciding whether each molecule is stable or not, whether it would be diamagnetic or paramagnetic, and calculating the bond order for each molecule. Molecule Stable? Bond Order Magnetic Properties ——————————————————– Yes Diamagnetic No Paramagnetic Yes Diamagnetic Yes Paramagnetic No Diamagnetic Yes Paramagnetic<\/p>\n\n\n\n

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

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

Based on the principles of Molecular Orbital (MO) theory, here are the completed answers for the table and a detailed explanation.<\/p>\n\n\n\n

Correct Answer<\/h3>\n\n\n\n

Here is the completed table with the correct properties for each diatomic molecule:<\/p>\n\n\n\n

Molecule<\/td>Stable?<\/td>Diamagnetic or Paramagnetic?<\/td>Bond Order<\/td><\/tr>
F\u2082\u207a<\/strong><\/td>yes<\/strong><\/td>paramagnetic<\/strong><\/td>1.5<\/strong><\/td><\/tr>
Ne\u2082<\/strong><\/td>no<\/strong><\/td>diamagnetic<\/strong><\/td>0<\/strong><\/td><\/tr>
O\u2082\u207b<\/strong><\/td>yes<\/strong><\/td>paramagnetic<\/strong><\/td>1.5<\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
\n\n\n\n

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

To determine the properties of these diatomic molecules, we use the Molecular Orbital (MO) model. The stability of a molecule is determined by its bond order; if the bond order is greater than zero, the molecule is considered stable. The magnetic property depends on the presence of unpaired electrons; if there are unpaired electrons, the molecule is paramagnetic, and if all electrons are paired, it is diamagnetic. The bond order is calculated as:<\/p>\n\n\n\n

Bond Order = \u00bd (Number of bonding electrons – Number of anti-bonding electrons)<\/strong><\/p>\n\n\n\n

The order of filling for the valence molecular orbitals for O\u2082, F\u2082, and Ne\u2082 is:
\u03c3(2s), \u03c3*(2s), \u03c3(2p), \u03c0(2p), \u03c0*(2p), \u03c3*(2p)<\/p>\n\n\n\n

1. F\u2082\u207a (Fluoride Cation)<\/strong><\/p>\n\n\n\n

    \n
  • Valence Electrons:<\/strong>\u00a0A neutral fluorine atom (F) has 7 valence electrons. F\u2082 has 14, and the F\u2082\u207a ion has lost one electron, giving it a total of\u00a013 valence electrons<\/strong>.<\/li>\n\n\n\n
  • MO Configuration:<\/strong>\u00a0(\u03c32s)\u00b2 (\u03c32s)\u00b2 (\u03c32p)\u00b2 (\u03c02p)\u2074 (\u03c0<\/em>2p)\u00b3<\/li>\n\n\n\n
  • Bond Order:<\/strong>\u00a0There are 8 bonding electrons (in \u03c32s, \u03c32p, \u03c02p) and 5 anti-bonding electrons (in \u03c32s, \u03c0<\/em>2p).
    Bond Order = \u00bd (8 – 5) =\u00a01.5<\/strong>. Since the bond order is > 0, F\u2082\u207a is\u00a0stable<\/strong>.<\/li>\n\n\n\n
  • Magnetic Properties:<\/strong>\u00a0The (\u03c0*2p)\u00b3 orbital contains one unpaired electron. Therefore, F\u2082\u207a is\u00a0paramagnetic<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    2. Ne\u2082 (Dineon)<\/strong><\/p>\n\n\n\n

      \n
    • Valence Electrons:<\/strong>\u00a0A neutral neon atom (Ne) has 8 valence electrons. The Ne\u2082 molecule has 8 + 8 =\u00a016 valence electrons<\/strong>.<\/li>\n\n\n\n
    • MO Configuration:<\/strong>\u00a0(\u03c32s)\u00b2 (\u03c32s)\u00b2 (\u03c32p)\u00b2 (\u03c02p)\u2074 (\u03c0<\/em>2p)\u2074 (\u03c3*2p)\u00b2<\/li>\n\n\n\n
    • Bond Order:<\/strong>\u00a0There are 8 bonding electrons and 8 anti-bonding electrons.
      Bond Order = \u00bd (8 – 8) =\u00a00<\/strong>. A bond order of zero indicates that no net bond is formed, so Ne\u2082 is\u00a0unstable<\/strong>.<\/li>\n\n\n\n
    • Magnetic Properties:<\/strong>\u00a0All molecular orbitals are completely filled, meaning there are no unpaired electrons. Therefore, Ne\u2082 is\u00a0diamagnetic<\/strong>.<\/li>\n<\/ul>\n\n\n\n

      3. O\u2082\u207b (Superoxide Ion)<\/strong><\/p>\n\n\n\n

        \n
      • Valence Electrons:<\/strong>\u00a0A neutral oxygen atom (O) has 6 valence electrons. O\u2082 has 12, and the O\u2082\u207b ion has gained one electron, giving it a total of\u00a013 valence electrons<\/strong>.<\/li>\n\n\n\n
      • MO Configuration:<\/strong>\u00a0(\u03c32s)\u00b2 (\u03c32s)\u00b2 (\u03c32p)\u00b2 (\u03c02p)\u2074 (\u03c0<\/em>2p)\u00b3<\/li>\n\n\n\n
      • Bond Order:<\/strong>\u00a0There are 8 bonding electrons and 5 anti-bonding electrons.
        Bond Order = \u00bd (8 – 5) =\u00a01.5<\/strong>. Since the bond order is > 0, O\u2082\u207b is\u00a0stable<\/strong>.<\/li>\n\n\n\n
      • Magnetic Properties:<\/strong>\u00a0The (\u03c0*2p)\u00b3 orbital has one unpaired electron, making O\u2082\u207b\u00a0paramagnetic<\/strong>.<\/li>\n<\/ul>\n\n\n\n
        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

        Chemical Bonding: Predicting Bond Order and Paramagnetism Using the MO Model To determine the stability and magnetic properties of diatomic molecules, we can use the molecular orbital (MO) model. The table below provides information about some diatomic molecules. Please complete the table by deciding whether each molecule is stable or not, whether it would be […]<\/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-244159","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/244159","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=244159"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/244159\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=244159"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=244159"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=244159"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}