Answer:<\/strong> Explanation<\/strong> In H\u2082S, sulfur forms two single bonds<\/strong> with two hydrogen atoms. This uses two of sulfur\u2019s valence electrons<\/strong>, one for each S\u2013H bond. The remaining four valence electrons<\/strong> exist as two lone pairs<\/strong> on the sulfur atom. Therefore, the electron domain geometry around sulfur consists of four regions of electron density<\/strong> (two bonding pairs and two lone pairs), which suggests a tetrahedral<\/strong> electron geometry.<\/p>\n\n\n\n However, due to the repulsion caused by lone pairs, the molecular geometry<\/strong> is not tetrahedral but rather bent (angular)<\/strong>. Lone pairs exert greater repulsion than bonding pairs, so they push the bonding pairs closer together, reducing the bond angle.<\/p>\n\n\n\n While an ideal tetrahedral angle is 109.5\u00b0<\/strong>, the actual H\u2013S\u2013H bond angle<\/strong> in H\u2082S is much smaller. Due to the large size of sulfur and its relatively diffuse 3p orbitals<\/strong>, the overlap with hydrogen\u2019s 1s orbitals is weak<\/strong>, and no significant hybridization (like sp\u00b3)<\/strong> occurs. As a result, the S\u2013H bonds are considered to arise mainly from unhybridized 3p orbitals<\/strong> overlapping with the hydrogen 1s orbitals.<\/p>\n\n\n\n This absence of hybridization and the presence of two lone pairs result in a bond angle close to the p-orbital angle of 90\u00b0<\/strong>. Experimentally, the angle is about 92\u00b0,<\/strong> consistent with this explanation. Therefore, valence bond theory predicts a bent structure<\/strong> with a bond angle close to 92\u00b0<\/strong>, based on the geometry and bonding orbitals involved.<\/p>\n\n\n\n Find the predicted bond angle of hydrogen sulfide (H2S) using the valence bond theory. Also describe the bonding in H2S based on the theory. The Correct Answer and Explanation is: Answer:The predicted bond angle of hydrogen sulfide (H\u2082S) using valence bond theory is approximately 92\u00b0. ExplanationAccording to valence bond theory, bonding in molecules is explained […]<\/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-234082","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234082","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=234082"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234082\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=234082"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=234082"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=234082"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
The predicted bond angle of hydrogen sulfide (H\u2082S) using valence bond theory is approximately 92\u00b0<\/strong>.<\/p>\n\n\n\n
\n\n\n\n
According to valence bond theory<\/strong>, bonding in molecules is explained through the overlap of atomic orbitals from adjacent atoms. In the case of hydrogen sulfide (H\u2082S)<\/strong>, the central atom is sulfur (S)<\/strong>, which is in group 16<\/strong> of the periodic table. It has the electron configuration:
[Ne] 3s\u00b2 3p\u2074<\/strong>, meaning it has six valence electrons.<\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner5-462.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"