{"id":157069,"date":"2024-10-18T04:15:03","date_gmt":"2024-10-18T04:15:03","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=157069"},"modified":"2024-10-18T04:15:07","modified_gmt":"2024-10-18T04:15:07","slug":"what-is-the-electron-pair-geometry-for-n-in-no2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/18\/what-is-the-electron-pair-geometry-for-n-in-no2\/","title":{"rendered":"What is the electron-pair geometry for N in NO2-"},"content":{"rendered":"\n

What is the electron-pair geometry for N in NO2-?
There are lone pair(s) around the central atom, so the geometry of NO2- is .<\/p>\n\n\n\n

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

The electron-pair geometry for the nitrogen atom (N) in the nitrite ion (NO\u2082\u207b) is trigonal planar<\/strong>. However, there is also one lone pair on the nitrogen, making the molecular geometry bent<\/strong> or V-shaped<\/strong>.<\/p>\n\n\n\n

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

To understand the electron-pair geometry of NO\u2082\u207b, let’s break it down step by step:<\/p>\n\n\n\n

    \n
  1. Valence Electrons<\/strong>: Nitrogen (N) has 5 valence electrons, and each oxygen (O) has 6 valence electrons. In NO\u2082\u207b, there is also an additional electron due to the negative charge. Thus, the total number of valence electrons is:
    [
    5\\ (\\text{from N}) + 6 \\times 2\\ (\\text{from two O atoms}) + 1\\ (\\text{from negative charge}) = 18\\ \\text{valence electrons}
    ]<\/li>\n\n\n\n
  2. Lewis Structure<\/strong>: In the Lewis structure of NO\u2082\u207b, nitrogen is the central atom, and it forms two bonds with the oxygen atoms. One of these bonds is a single bond, and the other is a double bond. Additionally, there is a lone pair of electrons on the nitrogen atom.<\/li>\n\n\n\n
  3. Electron-Pair Geometry<\/strong>: According to VSEPR (Valence Shell Electron Pair Repulsion) theory, the electron-pair geometry is determined by the number of regions of electron density (bonds or lone pairs) around the central atom. Nitrogen has three regions of electron density: two bonding regions (the N-O bonds) and one lone pair of electrons. These three regions of electron density arrange themselves as far apart as possible, leading to a trigonal planar<\/strong> electron-pair geometry.<\/li>\n\n\n\n
  4. Molecular Geometry<\/strong>: The presence of a lone pair changes the molecular geometry. The lone pair exerts more repulsion than the bonding pairs, causing the molecule to adopt a bent<\/strong> shape, rather than maintaining the ideal trigonal planar structure.<\/li>\n<\/ol>\n\n\n\n

    In conclusion, the electron-pair geometry for nitrogen in NO\u2082\u207b is trigonal planar, but the molecular geometry is bent due to the lone pair.<\/p>\n","protected":false},"excerpt":{"rendered":"

    What is the electron-pair geometry for N in NO2-?There are lone pair(s) around the central atom, so the geometry of NO2- is . The Correct Answer and Explanation is : The electron-pair geometry for the nitrogen atom (N) in the nitrite ion (NO\u2082\u207b) is trigonal planar. However, there is also one lone pair on the […]<\/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-157069","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/157069","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=157069"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/157069\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=157069"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=157069"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=157069"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}