{"id":186686,"date":"2025-01-26T05:59:32","date_gmt":"2025-01-26T05:59:32","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=186686"},"modified":"2025-01-26T05:59:34","modified_gmt":"2025-01-26T05:59:34","slug":"compare-the-shapes-and-bond-angles-of-these-oxynitrogen-ions","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/26\/compare-the-shapes-and-bond-angles-of-these-oxynitrogen-ions\/","title":{"rendered":"Compare the shapes and bond angles of these oxynitrogen ions"},"content":{"rendered":"\n<p>Compare the shapes and bond angles of these oxynitrogen ions. NO2+ NO2- NO3- NO43-<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>Let&#8217;s analyze the shapes and bond angles of the oxynitrogen ions: <strong>NO\u2082\u207a<\/strong>, <strong>NO\u2082\u207b<\/strong>, <strong>NO\u2083\u207b<\/strong>, and <strong>NO\u2084\u00b3\u207b<\/strong>.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>NO\u2082\u207a (Nitronium ion)<\/strong>:\n<ul class=\"wp-block-list\">\n<li><strong>Shape<\/strong>: Linear<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 180\u00b0<\/li>\n\n\n\n<li>The NO\u2082\u207a ion has a linear shape with two oxygen atoms bonded to a central nitrogen atom. The nitrogen atom in NO\u2082\u207a is sp hybridized, and it has no lone pairs, which leads to the linear shape. The ion has a formal positive charge, which means it has lost an electron and the nitrogen atom is electron-deficient, making it more electropositive.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>NO\u2082\u207b (Nitrite ion)<\/strong>:\n<ul class=\"wp-block-list\">\n<li><strong>Shape<\/strong>: Bent (V-shaped)<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: ~120\u00b0<\/li>\n\n\n\n<li>The NO\u2082\u207b ion has a bent shape because the nitrogen atom is sp\u00b2 hybridized, with one lone pair of electrons. There are two bonding regions (the two O-N bonds), and the lone pair repels the bonding electrons, resulting in a bond angle slightly less than 120\u00b0, creating a bent structure. The negative charge on the oxygen contributes to the distortion of the bond angle.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>NO\u2083\u207b (Nitrate ion)<\/strong>:\n<ul class=\"wp-block-list\">\n<li><strong>Shape<\/strong>: Trigonal planar<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 120\u00b0<\/li>\n\n\n\n<li>The NO\u2083\u207b ion has a trigonal planar geometry with three oxygen atoms bonded to the central nitrogen atom. The nitrogen in NO\u2083\u207b is sp\u00b2 hybridized with no lone pairs, leading to a bond angle of 120\u00b0. The negative charge is delocalized over the three oxygens through resonance, stabilizing the ion and giving it a planar shape.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>NO\u2084\u00b3\u207b (Tetrahydroxidodinitrogen ion)<\/strong>:\n<ul class=\"wp-block-list\">\n<li><strong>Shape<\/strong>: Tetrahedral<\/li>\n\n\n\n<li><strong>Bond Angle<\/strong>: 109.5\u00b0<\/li>\n\n\n\n<li>NO\u2084\u00b3\u207b has a tetrahedral shape, with four oxygen atoms symmetrically bonded to the central nitrogen atom. The nitrogen in NO\u2084\u00b3\u207b is sp\u00b3 hybridized, and the electron pairs around the nitrogen atom create a symmetric, tetrahedral structure. The bond angles between the oxygen atoms are about 109.5\u00b0.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>NO\u2082\u207a<\/strong> is linear (180\u00b0) because it has no lone pairs and minimal electron repulsion.<\/li>\n\n\n\n<li><strong>NO\u2082\u207b<\/strong> is bent (slightly less than 120\u00b0) due to a lone pair on nitrogen.<\/li>\n\n\n\n<li><strong>NO\u2083\u207b<\/strong> is trigonal planar (120\u00b0) due to resonance and no lone pairs on nitrogen.<\/li>\n\n\n\n<li><strong>NO\u2084\u00b3\u207b<\/strong> is tetrahedral (109.5\u00b0) due to four bonding pairs and no lone pairs on nitrogen.<\/li>\n<\/ul>\n\n\n\n<p>These variations arise from differences in hybridization, lone pairs, and resonance, which influence the shape and bond angles.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Compare the shapes and bond angles of these oxynitrogen ions. NO2+ NO2- NO3- NO43- The Correct Answer and Explanation is : Let&#8217;s analyze the shapes and bond angles of the oxynitrogen ions: NO\u2082\u207a, NO\u2082\u207b, NO\u2083\u207b, and NO\u2084\u00b3\u207b. Conclusion: These variations arise from differences in hybridization, lone pairs, and resonance, which influence the shape and bond [&hellip;]<\/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-186686","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186686","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=186686"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186686\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=186686"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=186686"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=186686"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}