A. What is the hybridization of the central atom in NOCl? Hybridization- What are the approximate bond angles in this Bond angles substan<\/p>\n\n\n\n
B. What is the hybridization of the central atom in NH,CIT Hybridization What are the approximate bond angles in this Bond angles substan<\/p>\n\n\n\n
Submit Answer Retry Entire Group 9 more group attempts remaining<\/p>\n\n\n\n
The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n Below are the answers along with detailed explanations and illustrative diagrams.<\/p>\n\n\n\n Hybridization:<\/strong> The central nitrogen in NOCl is sp\u00b2 hybridized<\/strong>. Explanation:<\/strong> Hybridization:<\/strong> The central nitrogen in NH\u2082Cl (chloramine) is sp\u00b3 hybridized<\/strong>. Explanation:<\/strong> Below are simplified structural diagrams illustrating the bonding and approximate angles:<\/p>\n\n\n\n NOCl Diagram:<\/strong><\/p>\n\n\n\n NH\u2082Cl Diagram:<\/strong><\/p>\n\n\n\n These diagrams summarize the connectivity and the expected bond angles based on the VSEPR model.<\/p>\n","protected":false},"excerpt":{"rendered":" A. What is the hybridization of the central atom in NOCl? Hybridization- What are the approximate bond angles in this Bond angles substan B. What is the hybridization of the central atom in NH,CIT Hybridization What are the approximate bond angles in this Bond angles substan Submit Answer Retry Entire Group 9 more group attempts […]<\/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-194725","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194725","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=194725"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194725\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194725"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194725"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194725"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nA. Nitrosyl Chloride (NOCl)<\/h3>\n\n\n\n
Bond Angles:<\/strong> With three electron domains\u2014one double bond to oxygen, one single bond to chlorine, and one lone pair\u2014the electron geometry is trigonal planar. However, the lone pair exerts a stronger repulsive force, compressing the O\u2013N\u2013Cl bond angle to slightly less than the ideal 120\u00b0. In practice, the bond angle is approximately 115\u00b0<\/strong>.<\/p>\n\n\n\n
Nitrosyl chloride (NOCl) has a structure that can be drawn as O=N\u2013Cl. Here, nitrogen serves as the central atom. It forms a double bond with oxygen and a single bond with chlorine. Despite only two bonds being present, nitrogen also retains one lone pair of electrons. In Valence Shell Electron Pair Repulsion (VSEPR) theory, these three electron domains (the double bond, single bond, and lone pair) would ideally adopt a trigonal planar arrangement, which normally features bond angles of 120\u00b0. However, lone pairs are more repulsive than bonding pairs. This extra repulsion pushes the bonded atoms slightly closer together, reducing the bond angle to around 115\u00b0. Thus, while the electron-domain geometry remains trigonal planar (sp\u00b2), the observed molecular shape is bent.<\/p>\n\n\n\n
\n\n\n\nB. Chloramine (NH\u2082Cl)<\/h3>\n\n\n\n
Bond Angles:<\/strong> With four electron groups\u2014three bonding pairs (two N\u2013H bonds and one N\u2013Cl bond) and one lone pair\u2014the ideal tetrahedral angle of 109.5\u00b0 is slightly reduced by the lone pair\u2019s repulsion, resulting in bond angles of roughly 107\u00b0<\/strong>.<\/p>\n\n\n\n
In chloramine, nitrogen forms three sigma bonds (two to hydrogen and one to chlorine) and carries one lone pair, totaling four electron groups. According to VSEPR theory, four electron groups around a central atom arrange themselves in a tetrahedral geometry. The ideal bond angle in a perfect tetrahedron is 109.5\u00b0. However, the lone pair occupies more space than bonding pairs due to its higher electron density, leading to stronger repulsion. This repulsion pushes the bonded atoms closer together, causing the bond angles between the atoms to decrease to approximately 107\u00b0. The overall molecular shape is thus trigonal pyramidal. This pattern is analogous to what is observed in ammonia (NH\u2083), where the lone pair similarly reduces the bond angle from 109.5\u00b0 to around 107\u00b0.<\/p>\n\n\n\n
\n\n\n\nDiagrams<\/h3>\n\n\n\n
O\n ||\n N <-- Lone Pair (not shown for clarity)\n |\n Cl\n\u2248 115\u00b0 (O\u2013N\u2013Cl)\n<\/code><\/pre>\n\n\n\n H\n \\\n N <-- Lone Pair (not shown for clarity)\n \/ \\\n H Cl\n\u2248 107\u00b0 (between bonds)\n<\/code><\/pre>\n\n\n\n