{"id":190726,"date":"2025-02-13T07:39:27","date_gmt":"2025-02-13T07:39:27","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=190726"},"modified":"2025-02-13T07:39:30","modified_gmt":"2025-02-13T07:39:30","slug":"which-lists-information-about-some-diatomic-molecules-or-molecular-ions-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/13\/which-lists-information-about-some-diatomic-molecules-or-molecular-ions-2\/","title":{"rendered":"which lists information about some diatomic molecules or molecular ions"},"content":{"rendered":"\n

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.<\/p>\n\n\n\n

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

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

The image you referred to shows a table with various diatomic molecules or ions, and asks for stability, magnetic properties (diamagnetic or paramagnetic), and bond order. Here’s the completed table along with an explanation for each parameter:<\/p>\n\n\n\n

Molecule\/Ion<\/th>Stable?<\/th>Diamagnetic\/Paramagnetic?<\/th>Bond Order<\/th><\/tr><\/thead>
( H_2 )<\/td>Stable<\/td>Diamagnetic<\/td>1<\/td><\/tr>
( H_2^+ )<\/td>Stable<\/td>Paramagnetic<\/td>0.5<\/td><\/tr>
( He_2 )<\/td>Unstable<\/td>Diamagnetic<\/td>0<\/td><\/tr>
( He_2^+ )<\/td>Stable<\/td>Paramagnetic<\/td>0.5<\/td><\/tr>
( O_2 )<\/td>Stable<\/td>Paramagnetic<\/td>2<\/td><\/tr>
( O_2^+ )<\/td>Stable<\/td>Paramagnetic<\/td>2.5<\/td><\/tr>
( N_2 )<\/td>Stable<\/td>Diamagnetic<\/td>3<\/td><\/tr>
( N_2^+ )<\/td>Stable<\/td>Paramagnetic<\/td>2.5<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

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

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

    \n
  • Molecules or ions are generally considered stable if they have a positive bond order (more bonding electrons than antibonding).<\/li>\n\n\n\n
  • ( H_2 ), ( H_2^+ ), ( He_2^+ ), ( O_2 ), ( O_2^+ ), ( N_2 ), and ( N_2^+ ) are stable with positive bond orders.<\/li>\n\n\n\n
  • ( He_2 ) is unstable due to a bond order of 0, indicating equal numbers of bonding and antibonding electrons.<\/li>\n<\/ul>\n\n\n\n

    Diamagnetic or Paramagnetic:<\/strong><\/p>\n\n\n\n

      \n
    • A molecule\/ion is diamagnetic<\/strong> if all of its electrons are paired.<\/li>\n\n\n\n
    • A molecule\/ion is paramagnetic<\/strong> if it has unpaired electrons.<\/li>\n\n\n\n
    • ( H_2 ) and ( N_2 ) are diamagnetic because they have no unpaired electrons.<\/li>\n\n\n\n
    • ( H_2^+ ), ( He_2^+ ), ( O_2 ), ( O_2^+ ), and ( N_2^+ ) are paramagnetic as they have unpaired electrons.<\/li>\n<\/ul>\n\n\n\n

      Bond Order:<\/strong><\/p>\n\n\n\n

        \n
      • Bond order can be calculated using the molecular orbital theory formula: ( \\text{Bond Order} = \\frac{1}{2} (\\text{number of bonding electrons} – \\text{number of antibonding electrons}) ).<\/li>\n\n\n\n
      • For ( H_2 ), the bond order is 1 (2 bonding electrons, 0 antibonding).<\/li>\n\n\n\n
      • For ( H_2^+ ), the bond order is 0.5 (1 bonding electron, 0 antibonding).<\/li>\n\n\n\n
      • ( He_2 ) has a bond order of 0 (2 bonding electrons, 2 antibonding), reflecting its instability.<\/li>\n\n\n\n
      • ( He_2^+ ) has a bond order of 0.5 (1 bonding electron, 0 antibonding).<\/li>\n\n\n\n
      • ( O_2 ) has a bond order of 2 (10 bonding electrons, 6 antibonding).<\/li>\n\n\n\n
      • ( O_2^+ ) has a bond order of 2.5 (10 bonding electrons, 5 antibonding).<\/li>\n\n\n\n
      • ( N_2 ) has the highest bond order of 3 (10 bonding electrons, 4 antibonding), corresponding to its very strong triple bond.<\/li>\n\n\n\n
      • ( N_2^+ ) has a bond order of 2.5 (10 bonding electrons, 5 antibonding).<\/li>\n<\/ul>\n\n\n\n

        The bond order indicates the stability and strength of the bonds between atoms in a molecule or ion, with higher values indicating stronger and more stable molecular structures. The paramagnetism and diamagnetism properties are important in applications involving magnetic fields, such as MRI and spectroscopy.<\/p>\n","protected":false},"excerpt":{"rendered":"

        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. The Correct Answer and Explanation is : The image you referred to shows a table with various diatomic molecules or ions, […]<\/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-190726","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/190726","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=190726"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/190726\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=190726"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=190726"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=190726"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}