{"id":222540,"date":"2025-05-31T12:45:09","date_gmt":"2025-05-31T12:45:09","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=222540"},"modified":"2025-05-31T12:45:12","modified_gmt":"2025-05-31T12:45:12","slug":"what-is-the-molecular-geometry-of-nh3cl-and-nh2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/31\/what-is-the-molecular-geometry-of-nh3cl-and-nh2\/","title":{"rendered":"What is the molecular geometry of NH3Cl+ and NH2-"},"content":{"rendered":"\n<p>What is the molecular geometry of NH3Cl+ and NH2-? Are they polar or non-polar? Briefly explain. After you examined the ball-and-stick model, what influenced the angle and shape of these molecules? Briefly explain using the VSEPR theory. What is the molecular geometry of the individual central atom of CH3COCH3 and CH3COOH? What is the overall polarity of each molecule? Briefly explain. After you examined the ball-and-stick model, what influenced the angle and shape of these molecules? Briefly explain using the VSEPR theory.<br>What is the molecular geometry of NH3Cl+ and NH2-? Are they polar or non-polar? Briefly explain. After you examined the ball-and-stick model, what influenced the angle and shape of these molecules? Briefly explain using the VSEPR theory. What is the molecular geometry of the individual central atom of CH3COCH3 and CH3COOH? What is the overall polarity of each molecule? Briefly explain. After you examined the ball-and-stick model, what influenced the angle and shape of these molecules? Briefly explain using the VSEPR theory.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>1. NH\u2083Cl\u207a (Ammonium chloride cation)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Molecular Geometry<\/strong>: <strong>Tetrahedral<\/strong><\/li>\n\n\n\n<li><strong>Polarity<\/strong>: <strong>Polar<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>Explanation<\/strong>: NH\u2083Cl\u207a is derived from NH\u2084\u207a (ammonium ion) by replacing one hydrogen with a chlorine atom. The nitrogen atom has four regions of electron density (three N\u2013H bonds and one N\u2013Cl bond) and no lone pairs. According to VSEPR (Valence Shell Electron Pair Repulsion) theory, four bonding pairs around nitrogen form a tetrahedral geometry with bond angles close to 109.5\u00b0. However, the molecule is <strong>polar<\/strong> because Cl is significantly more electronegative than H, causing an uneven distribution of electron density.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>2. NH\u2082\u207b (Amide anion)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Molecular Geometry<\/strong>: <strong>Bent (Angular)<\/strong><\/li>\n\n\n\n<li><strong>Polarity<\/strong>: <strong>Polar<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>Explanation<\/strong>: The NH\u2082\u207b ion has two bonding pairs and two lone pairs on nitrogen, for a total of four electron domains. VSEPR predicts a <strong>bent geometry<\/strong>, similar to H\u2082O, with bond angles slightly less than 109.5\u00b0. The lone pairs repel more strongly than bonding pairs, reducing the H\u2013N\u2013H bond angle. The molecule is polar due to the lone pair and asymmetrical electron distribution.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>3. CH\u2083COCH\u2083 (Acetone)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Geometry around central atoms<\/strong>:\n<ul class=\"wp-block-list\">\n<li><strong>C (in CH\u2083)<\/strong>: Tetrahedral<\/li>\n\n\n\n<li><strong>C=O (carbonyl carbon)<\/strong>: Trigonal planar<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Overall Polarity<\/strong>: <strong>Polar<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>Explanation<\/strong>: The carbonyl carbon in acetone is sp\u00b2 hybridized with trigonal planar geometry (120\u00b0 bond angles). The methyl groups are sp\u00b3 hybridized with tetrahedral geometry. The polar C=O bond makes the whole molecule polar despite the symmetrical CH\u2083 groups.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>4. CH\u2083COOH (Acetic acid)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Geometry around central atoms<\/strong>:\n<ul class=\"wp-block-list\">\n<li><strong>C (in CH\u2083)<\/strong>: Tetrahedral<\/li>\n\n\n\n<li><strong>C=O (carboxyl carbon)<\/strong>: Trigonal planar<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Overall Polarity<\/strong>: <strong>Polar<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>Explanation<\/strong>: Similar to acetone, the carbonyl carbon is sp\u00b2 hybridized (trigonal planar), and the methyl carbon is tetrahedral. The presence of both C=O and O\u2013H bonds contributes to a strong dipole moment, making acetic acid highly polar.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>VSEPR Theory Summary<\/strong><\/h3>\n\n\n\n<p>VSEPR theory explains the shape and angles based on electron domain repulsion. Lone pairs exert greater repulsion than bonding pairs, influencing bond angles and molecular shape. Polar molecules arise from asymmetrical shapes or bonds with differing electronegativities.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner4-222.jpeg\" alt=\"\" class=\"wp-image-222541\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>What is the molecular geometry of NH3Cl+ and NH2-? Are they polar or non-polar? Briefly explain. After you examined the ball-and-stick model, what influenced the angle and shape of these molecules? Briefly explain using the VSEPR theory. What is the molecular geometry of the individual central atom of CH3COCH3 and CH3COOH? What is the overall [&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-222540","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222540","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=222540"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222540\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=222540"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=222540"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=222540"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}