{"id":218586,"date":"2025-05-24T05:53:50","date_gmt":"2025-05-24T05:53:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=218586"},"modified":"2025-05-24T05:53:52","modified_gmt":"2025-05-24T05:53:52","slug":"determine-the-shape-and-bond-angle-of-these-oxynitrogen-ions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/24\/determine-the-shape-and-bond-angle-of-these-oxynitrogen-ions\/","title":{"rendered":"Determine the shape and bond angle of these oxynitrogen ions."},"content":{"rendered":"\n

Determine the shape and bond angle of these oxynitrogen ions. Linear Trigonal planar Tetrahedral Bent Pyramidal 180\u00b0 120\u00b0 109.5\u00b0 ~120\u00b0 ~109\u00b0 ~109\u00b0 Answer Bank NO- NO3- NO2- None<\/p>\n\n\n\n

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

To determine the shape and bond angles of the oxynitrogen ions (NO\u207b, NO\u2083\u207b, and NO\u2082\u207b), we use Valence Shell Electron Pair Repulsion (VSEPR) theory<\/strong>, which predicts the geometry of a molecule based on the repulsion between electron pairs around a central atom.<\/p>\n\n\n\n

\n\n\n\n

1. NO\u207b (Nitrosyl anion)<\/strong><\/h3>\n\n\n\n
    \n
  • Lewis structure<\/strong>: One nitrogen atom is bonded to one oxygen atom with a double bond<\/strong> and has a lone pair<\/strong> on nitrogen.<\/li>\n\n\n\n
  • Electron domains<\/strong> around N: 2 (1 bonding region, 1 lone pair).<\/li>\n\n\n\n
  • Electron geometry<\/strong>: Linear.<\/li>\n\n\n\n
  • Molecular shape<\/strong>: Linear<\/strong>.<\/li>\n\n\n\n
  • Bond angle<\/strong>: 180\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    2. NO\u2083\u207b (Nitrate ion)<\/strong><\/h3>\n\n\n\n
      \n
    • Lewis structure<\/strong>: Nitrogen is bonded to three oxygens. It forms one double bond and two single bonds with resonance, making all N\u2013O bonds equivalent.<\/li>\n\n\n\n
    • Electron domains<\/strong> around N: 3 bonding pairs, no lone pairs.<\/li>\n\n\n\n
    • Electron geometry<\/strong>: Trigonal planar.<\/li>\n\n\n\n
    • Molecular shape<\/strong>: Trigonal planar<\/strong>.<\/li>\n\n\n\n
    • Bond angle<\/strong>: 120\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

      3. NO\u2082\u207b (Nitrite ion)<\/strong><\/h3>\n\n\n\n
        \n
      • Lewis structure<\/strong>: Nitrogen is bonded to two oxygens with one double bond and one single bond (resonance between them). There is also a lone pair<\/strong> on nitrogen.<\/li>\n\n\n\n
      • Electron domains<\/strong> around N: 3 (2 bonding pairs, 1 lone pair).<\/li>\n\n\n\n
      • Electron geometry<\/strong>: Trigonal planar.<\/li>\n\n\n\n
      • Molecular shape<\/strong>: Bent<\/strong>.<\/li>\n\n\n\n
      • Bond angle<\/strong>: Slightly less than 120\u00b0, due to lone pair repulsion, typically ~115\u2013118\u00b0<\/strong> (approximately ~120\u00b0<\/strong>).<\/li>\n<\/ul>\n\n\n\n
        \n\n\n\n

        Final Answers:<\/h3>\n\n\n\n
        Ion<\/th>Shape<\/th>Bond Angle<\/th><\/tr><\/thead>
        NO\u207b<\/strong><\/td>Linear<\/td>180\u00b0<\/td><\/tr>
        NO\u2083\u207b<\/strong><\/td>Trigonal planar<\/td>120\u00b0<\/td><\/tr>
        NO\u2082\u207b<\/strong><\/td>Bent<\/td>~120\u00b0<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

        These geometries arise from minimizing electron pair repulsions. Lone pairs repel more strongly than bonding pairs, distorting ideal angles slightly, as seen in NO\u2082\u207b. Resonance also plays a role, especially in NO\u2083\u207b, where the structure is delocalized.<\/p>\n\n\n\n

        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

        Determine the shape and bond angle of these oxynitrogen ions. Linear Trigonal planar Tetrahedral Bent Pyramidal 180\u00b0 120\u00b0 109.5\u00b0 ~120\u00b0 ~109\u00b0 ~109\u00b0 Answer Bank NO- NO3- NO2- None The Correct Answer and Explanation is: To determine the shape and bond angles of the oxynitrogen ions (NO\u207b, NO\u2083\u207b, and NO\u2082\u207b), we use Valence Shell Electron Pair […]<\/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-218586","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/218586","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=218586"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/218586\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=218586"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=218586"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=218586"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}