{"id":234104,"date":"2025-06-13T18:11:29","date_gmt":"2025-06-13T18:11:29","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=234104"},"modified":"2025-06-13T18:11:31","modified_gmt":"2025-06-13T18:11:31","slug":"hcl-h-ci-formula-lewis-structure-electron-pair-geometry-molecular-bond-geometry-angle-polar-or-non-polar-polar-h-ci-ho-hoh-h-h-109-5","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/13\/hcl-h-ci-formula-lewis-structure-electron-pair-geometry-molecular-bond-geometry-angle-polar-or-non-polar-polar-h-ci-ho-hoh-h-h-109-5\/","title":{"rendered":"HCl H: Ci: Formula Lewis Structure Electron Pair Geometry Molecular Bond Geometry Angle Polar or Non Polar Polar H-CI H?O * H:O:H H H 109.5\u00b0"},"content":{"rendered":"\n

HCl H: Ci: Formula Lewis Structure Electron Pair Geometry Molecular Bond Geometry Angle Polar or Non Polar Polar H-CI H?O * H:O:H H H 109.5\u00b0 Polar NH3 H:N:H N HHH 107\u00b0 Polar BCL? CI: B:CI: C ?? B 120\u00b0 Non-Polar CI ::::: =0 O=C=0 180\u00b0 Non-Polar :9: CO? : Cl PO?\u00b3? 0: 0:0:0:1 NO? NO? CH? SO? SO?\u00b2? P ? 109.28<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

Predicted Bond Angle of H\u2082S: ~92.1\u00b0<\/strong><\/p>\n\n\n\n

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

To determine the bond angle of hydrogen sulfide (H\u2082S), we utilize the Valence Shell Electron Pair Repulsion (VSEPR) theory, which predicts the three-dimensional geometry of molecules based on minimizing the electrostatic repulsion between electron pairs around a central atom.<\/p>\n\n\n\n

1. Lewis Structure:<\/strong>
First, we draw the Lewis structure for H\u2082S. Sulfur (S), the central atom, is in Group 16 and has 6 valence electrons. Each hydrogen (H) atom has 1 valence electron.
Total valence electrons = 6 + 2(1) = 8.
Sulfur forms a single covalent bond with each of the two hydrogen atoms, using 4 electrons. The remaining 4 electrons are placed on the central sulfur atom as two non-bonding lone pairs.<\/p>\n\n\n\n

2. Electron Pair Geometry:<\/strong>
According to VSEPR theory, we count the number of electron domains around the central sulfur atom. An electron domain can be a single bond, a double bond, a triple bond, or a lone pair. In H\u2082S, there are two single bonding pairs (S-H bonds) and two lone pairs.
Total electron domains = 2 bonding pairs + 2 lone pairs = 4 domains.
An arrangement of four electron domains results in a tetrahedral<\/strong> electron pair geometry. The ideal bond angle for a perfect tetrahedral shape (like in methane, CH\u2084)<\/p>\n\n\n\n

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

HCl H: Ci: Formula Lewis Structure Electron Pair Geometry Molecular Bond Geometry Angle Polar or Non Polar Polar H-CI H?O * H:O:H H H 109.5\u00b0 Polar NH3 H:N:H N HHH 107\u00b0 Polar BCL? CI: B:CI: C ?? B 120\u00b0 Non-Polar CI ::::: =0 O=C=0 180\u00b0 Non-Polar :9: CO? : Cl PO?\u00b3? 0: 0:0:0:1 NO? NO? […]<\/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-234104","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234104","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=234104"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234104\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=234104"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=234104"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=234104"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}