Give the number of lone pair electrons around the central atom and identify the molecular geometry of sulfur dichloride, Sci2. Hint:<\/p>\n\n\n\n
a) Zero Lone Pairs; Linear
b) One Lone Pair; Bent
c) Two Lone Pairs; Bent
d) Three Lone Pairs; Bent
e) Three Lone Pairs; Linear<\/p>\n\n\n\n
The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n The correct answer is: c) Two Lone Pairs; Bent<\/strong><\/p>\n\n\n\n Sulfur dichloride (SCl\u2082)<\/strong> is a covalent compound consisting of one sulfur (S) atom as the central atom bonded to two chlorine (Cl) atoms. To determine the number of lone pair electrons<\/strong> on the sulfur atom and the molecular geometry<\/strong>, we need to examine the Lewis structure<\/strong> and apply the VSEPR theory (Valence Shell Electron Pair Repulsion)<\/strong>.<\/p>\n\n\n\n So, sulfur has two bonding pairs<\/strong> (S\u2013Cl) and two lone pairs<\/strong>.<\/p>\n\n\n\n This is similar to the geometry of water (H\u2082O)<\/strong>, which also has 2 bonding pairs and 2 lone pairs.<\/p>\n\n\n\n (c) Two Lone Pairs; Bent<\/strong><\/p>\n","protected":false},"excerpt":{"rendered":" Give the number of lone pair electrons around the central atom and identify the molecular geometry of sulfur dichloride, Sci2. Hint: a) Zero Lone Pairs; Linearb) One Lone Pair; Bentc) Two Lone Pairs; Bentd) Three Lone Pairs; Bente) Three Lone Pairs; Linear The correct answer and explanation is : The correct answer is: c) Two […]<\/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-212015","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/212015","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=212015"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/212015\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=212015"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=212015"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=212015"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\nExplanation (\u2248300 words):<\/h3>\n\n\n\n
Step 1: Count Valence Electrons<\/h4>\n\n\n\n
\n
Step 2: Draw the Lewis Structure<\/h4>\n\n\n\n
\n
Step 3: Apply VSEPR Theory<\/h4>\n\n\n\n
\n
Step 4: Determine Molecular Geometry and Lone Pairs<\/h4>\n\n\n\n
\n
\n\n\n\nFinal Answer:<\/h3>\n\n\n\n