{"id":251269,"date":"2025-07-10T16:04:57","date_gmt":"2025-07-10T16:04:57","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=251269"},"modified":"2025-07-10T16:04:59","modified_gmt":"2025-07-10T16:04:59","slug":"draw-the-molecular-orbital-diagrams-for-the-following-molecules-and-determine-the-bond-order-and-magnetic-properties","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/10\/draw-the-molecular-orbital-diagrams-for-the-following-molecules-and-determine-the-bond-order-and-magnetic-properties\/","title":{"rendered":"Draw the molecular orbital diagrams for the following molecules and determine the bond order and magnetic properties."},"content":{"rendered":"\n

Draw the molecular orbital diagrams for the following molecules and determine the bond order and magnetic properties. N2 N2 N2 Bond Order: BO: BO: BO: Paramagnetic diamagnetic Paramagnetic diamagnetic Paramagnetic diamagnetic Which molecule has the shortest bond? Which molecule has the highest bond enthalpy? Which molecule has the weakest bond?<\/p>\n\n\n\n

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

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

Here are the completed answers for the problem.<\/p>\n\n\n\n

For N\u2082<\/strong>
Bond Order:<\/strong> 3
Paramagnetic diamagnetic<\/strong> (circle diamagnetic)<\/p>\n\n\n\n

For N\u2082\u207a<\/strong>
BO:<\/strong> 2.5
Paramagnetic<\/strong> diamagnetic (circle paramagnetic)<\/p>\n\n\n\n

For N\u2082\u00b2\u207b<\/strong>
BO:<\/strong> 2
Paramagnetic<\/strong> diamagnetic (circle paramagnetic)<\/p>\n\n\n\n

For N\u2082\u00b3\u207b<\/strong>
BO:<\/strong> 1.5
Paramagnetic<\/strong> diamagnetic (circle paramagnetic)<\/p>\n\n\n\n

a. Which molecule has the shortest bond?<\/strong>
N\u2082<\/strong> N\u2082\u207a N\u2082\u00b2\u207b N\u2082\u00b3\u207b (circle N\u2082)<\/p>\n\n\n\n

b. Which molecule has the highest bond enthalpy?<\/strong>
N\u2082<\/strong> N\u2082\u207a N\u2082\u00b2\u207b N\u2082\u00b3\u207b (circle N\u2082)<\/p>\n\n\n\n

c. Which molecule has the weakest bond?<\/strong>
N\u2082 N\u2082\u207a N\u2082\u00b2\u207b N\u2082\u00b3\u207b<\/strong> (circle N\u2082\u00b3\u207b)<\/p>\n\n\n\n

\n\n\n\n

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

This problem is solved using Molecular Orbital (MO) theory. For diatomic molecules of elements lighter than oxygen, like nitrogen, s-p mixing occurs. This makes the energy of the \u03c3\u2082p orbital higher than the \u03c0\u2082p orbitals. The valence molecular orbital filling order is: \u03c3\u2082s, \u03c3\u2082s, \u03c0\u2082p, \u03c3\u2082p, \u03c0<\/em>\u2082p, \u03c3*\u2082p. Bond order (BO) is calculated as \u00bd (bonding electrons minus antibonding electrons). Magnetic properties depend on unpaired electrons; molecules with unpaired electrons are paramagnetic, while those with only paired electrons are diamagnetic.<\/p>\n\n\n\n

N\u2082:<\/strong> A neutral nitrogen atom has 5 valence electrons, so the N\u2082 molecule has a total of 10 valence electrons. Its MO configuration is (\u03c3\u2082s)\u00b2(\u03c3*\u2082s)\u00b2(\u03c0\u2082p)\u2074(\u03c3\u2082p)\u00b2.<\/p>\n\n\n\n

    \n
  • Bond Order:<\/strong>\u00a0There are 8 bonding electrons (in \u03c3\u2082s, \u03c0\u2082p, \u03c3\u2082p) and 2 antibonding electrons (in \u03c3*\u2082s). BO = \u00bd(8 – 2) = 3.<\/li>\n\n\n\n
  • Magnetic Properties:<\/strong>\u00a0All 10 electrons are paired, so N\u2082 is diamagnetic.<\/li>\n<\/ul>\n\n\n\n

    N\u2082\u207a:<\/strong> This ion has lost one electron, leaving it with 9 valence electrons. The electron is removed from the highest occupied molecular orbital (HOMO), which is the \u03c3\u2082p. The configuration is (\u03c3\u2082s)\u00b2(\u03c3*\u2082s)\u00b2(\u03c0\u2082p)\u2074(\u03c3\u2082p)\u00b9.<\/p>\n\n\n\n

      \n
    • Bond Order:<\/strong>\u00a0BO = \u00bd(7 – 2) = 2.5.<\/li>\n\n\n\n
    • Magnetic Properties:<\/strong>\u00a0There is one unpaired electron in the \u03c3\u2082p orbital, making N\u2082\u207a paramagnetic.<\/li>\n<\/ul>\n\n\n\n

      N\u2082\u00b2\u207b:<\/strong> This ion has gained two electrons, for a total of 12 valence electrons. The two electrons are added to the lowest unoccupied molecular orbital (LUMO), which is the degenerate \u03c0\u2082p set. According to Hund’s rule, they occupy separate orbitals with parallel spins. The configuration is (\u03c3\u2082s)\u00b2(\u03c3<\/em>\u2082s)\u00b2(\u03c0\u2082p)\u2074(\u03c3\u2082p)\u00b2(\u03c0*\u2082p)\u00b2.<\/p>\n\n\n\n

        \n
      • Bond Order:<\/strong>\u00a0BO = \u00bd(8 – 4) = 2.<\/li>\n\n\n\n
      • Magnetic Properties:<\/strong>\u00a0It has two unpaired electrons, making it paramagnetic.<\/li>\n<\/ul>\n\n\n\n

        N\u2082\u00b3\u207b:<\/strong> This ion has 13 valence electrons. The configuration is (\u03c3\u2082s)\u00b2(\u03c3\u2082s)\u00b2(\u03c0\u2082p)\u2074(\u03c3\u2082p)\u00b2(\u03c0<\/em>\u2082p)\u00b3.<\/p>\n\n\n\n

          \n
        • Bond Order:<\/strong>\u00a0BO = \u00bd(8 – 5) = 1.5.<\/li>\n\n\n\n
        • Magnetic Properties:<\/strong>\u00a0There is one unpaired electron in the \u03c0*\u2082p orbitals, so it is paramagnetic.<\/li>\n<\/ul>\n\n\n\n

          Bond strength and bond length are directly related to the bond order. A higher bond order indicates a stronger, shorter bond with higher bond enthalpy. A lower bond order indicates a weaker, longer bond.<\/p>\n\n\n\n

            \n
          • Shortest Bond \/ Highest Enthalpy:<\/strong>\u00a0N\u2082 has the highest bond order (3), so it has the shortest and strongest bond.<\/li>\n\n\n\n
          • Weakest Bond:<\/strong>\u00a0N\u2082\u00b3\u207b has the lowest bond order (1.5), so it has the weakest bond.<\/li>\n<\/ul>\n\n\n\n
            \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

            Draw the molecular orbital diagrams for the following molecules and determine the bond order and magnetic properties. N2 N2 N2 Bond Order: BO: BO: BO: Paramagnetic diamagnetic Paramagnetic diamagnetic Paramagnetic diamagnetic Which molecule has the shortest bond? Which molecule has the highest bond enthalpy? Which molecule has the weakest bond? The Correct Answer and Explanation […]<\/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-251269","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/251269","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=251269"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/251269\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=251269"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=251269"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=251269"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}