{"id":188063,"date":"2025-02-06T10:05:23","date_gmt":"2025-02-06T10:05:23","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=188063"},"modified":"2025-02-06T10:05:25","modified_gmt":"2025-02-06T10:05:25","slug":"for-the-molecules-sih4-and-cse2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/06\/for-the-molecules-sih4-and-cse2\/","title":{"rendered":"For the molecules SiH4 and CSe2"},"content":{"rendered":"\n<p>For the molecules SiH4 and CSe2, give<br>total number of valence electrons present<br>Lewis structure<br>electron and molecular geometry<br>bond angle<br>polarity of molecule<\/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 molecules SiH\u2084 (silane) and CSe\u2082 (carbon diselenide) in terms of their valence electrons, Lewis structures, electron and molecular geometries, bond angles, and polarity.<\/p>\n\n\n\n<p><strong>SiH\u2084 (Silane):<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons:<\/strong> &#8211; Silicon (Si): 4 valence electrons &#8211; Hydrogen (H): 1 valence electron per atom \u00d7 4 atoms = 4 valence electrons &#8211; <strong>Total:<\/strong> 4 (Si) + 4 (H) = 8 valence electrons<\/li>\n\n\n\n<li><strong>Lewis Structure:<\/strong> &#8211; Silicon is the central atom, forming single bonds with four hydrogen atoms. &#8211; Each Si-H bond involves two electrons, utilizing all 8 valence electrons.<\/li>\n\n\n\n<li><strong>Electron and Molecular Geometry:<\/strong> &#8211; <strong>Electron Geometry:<\/strong> Tetrahedral, as there are four bonding pairs around the central silicon atom. &#8211; <strong>Molecular Geometry:<\/strong> Tetrahedral, since there are no lone pairs on silicon.<\/li>\n\n\n\n<li><strong>Bond Angle:<\/strong> &#8211; Approximately 109.5\u00b0, characteristic of a tetrahedral arrangement.<\/li>\n\n\n\n<li><strong>Polarity:<\/strong> &#8211; The Si-H bonds are slightly polar due to the difference in electronegativity between Si and H. &#8211; However, the symmetrical tetrahedral shape causes the individual dipoles to cancel out, resulting in a nonpolar molecule.<br><strong>CSe\u2082 (Carbon Diselenide):<\/strong><\/li>\n\n\n\n<li><strong>Valence Electrons:<\/strong> &#8211; Carbon (C): 4 valence electrons &#8211; Selenium (Se): 6 valence electrons per atom \u00d7 2 atoms = 12 valence electrons &#8211; <strong>Total:<\/strong> 4 (C) + 12 (Se) = 16 valence electrons<\/li>\n\n\n\n<li><strong>Lewis Structure:<\/strong> &#8211; Carbon is the central atom, forming double bonds with two selenium atoms. &#8211; Each double bond uses 4 electrons, totaling 8 electrons. &#8211; The remaining 8 electrons are placed as lone pairs on the selenium atoms.<\/li>\n\n\n\n<li><strong>Electron and Molecular Geometry:<\/strong> &#8211; <strong>Electron Geometry:<\/strong> Linear, as there are two regions of electron density (the two double bonds) around the central carbon atom. &#8211; <strong>Molecular Geometry:<\/strong> Linear, since there are no lone pairs on carbon.<\/li>\n\n\n\n<li><strong>Bond Angle:<\/strong> &#8211; 180\u00b0, characteristic of a linear arrangement.<\/li>\n\n\n\n<li><strong>Polarity:<\/strong> &#8211; The C=Se bonds are polar due to the difference in electronegativity between carbon and selenium. &#8211; The linear shape causes the dipoles to cancel out, resulting in a nonpolar molecule.<br>For a visual explanation of SiH\u2084&#8217;s molecular geometry and bond angles, you might find the following video helpful:<\/li>\n<\/ul>\n\n\n\n<p>\ue200video\ue202SiH\u2084 Molecular Geometry, Bond Angles\ue202turn0search0\ue201<\/p>\n","protected":false},"excerpt":{"rendered":"<p>For the molecules SiH4 and CSe2, givetotal number of valence electrons presentLewis structureelectron and molecular geometrybond anglepolarity of molecule The Correct Answer and Explanation is : Let&#8217;s analyze the molecules SiH\u2084 (silane) and CSe\u2082 (carbon diselenide) in terms of their valence electrons, Lewis structures, electron and molecular geometries, bond angles, and polarity. SiH\u2084 (Silane): \ue200video\ue202SiH\u2084 [&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-188063","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/188063","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=188063"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/188063\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=188063"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=188063"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=188063"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}