{"id":203054,"date":"2025-03-18T17:11:47","date_gmt":"2025-03-18T17:11:47","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203054"},"modified":"2025-03-18T17:11:50","modified_gmt":"2025-03-18T17:11:50","slug":"draw-a-suitable-lewis-structure-for-li2s-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/18\/draw-a-suitable-lewis-structure-for-li2s-2\/","title":{"rendered":"Draw a suitable Lewis structure for Li2S"},"content":{"rendered":"\n<p>Draw a suitable Lewis structure for Li2S. In the structure,<\/p>\n\n\n\n<p>there are two sulfide ions and one lithium ion.<br>there are two lithium atoms and one sulfur atom with 6 electrons.<br>each lithium atom makes one bond to sulfur.<br>there are two lithium ions each with a +1 charge and one sulfide ion with four pairs of electrons and a -2 charge.<\/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<h3 class=\"wp-block-heading\">Lewis Structure for Lithium Sulfide (Li\u2082S)<\/h3>\n\n\n\n<p>To draw the Lewis structure of lithium sulfide (Li\u2082S), we need to follow these steps:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Determine the number of valence electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lithium (Li)<\/strong> is an alkali metal in Group 1, so each lithium atom has <strong>1 valence electron<\/strong>.<\/li>\n\n\n\n<li><strong>Sulfur (S)<\/strong> is a Group 16 element, so sulfur has <strong>6 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Total number of valence electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>There are 2 lithium atoms, each contributing 1 electron, and 1 sulfur atom contributing 6 electrons.<\/li>\n\n\n\n<li>Total valence electrons = 2 (from Li) + 6 (from S) = <strong>8 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Structure Formation<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Lithium forms <strong>Li\u207a ions<\/strong> by losing its single valence electron. Each lithium atom gives up 1 electron, leaving a <strong>+1 charge<\/strong> on each lithium atom.<\/li>\n\n\n\n<li>Sulfur, which has 6 valence electrons, needs 2 more electrons to complete its octet. Sulfur accepts the 2 electrons from the lithium atoms to form a <strong>S\u00b2\u207b ion<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Bonding<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each lithium atom donates 1 electron to sulfur, forming an ionic bond between each lithium and sulfur.<\/li>\n\n\n\n<li>The <strong>sulfide ion (S\u00b2\u207b)<\/strong> now has a full octet (8 electrons) and carries a <strong>-2 charge<\/strong>.<\/li>\n\n\n\n<li>The <strong>lithium ions (Li\u207a)<\/strong> each have a <strong>+1 charge<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Final Structure<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The resulting ionic compound consists of two lithium cations (<strong>Li\u207a<\/strong>) and one sulfide anion (<strong>S\u00b2\u207b<\/strong>).<\/li>\n\n\n\n<li>In the Lewis structure, lithium ions are shown with their positive charges, and the sulfide ion has 8 electrons around it (4 pairs), with a <strong>-2 charge<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>In lithium sulfide (Li\u2082S), the bonding is ionic. Lithium atoms lose electrons to form <strong>Li\u207a ions<\/strong> and sulfur gains electrons to form a <strong>S\u00b2\u207b ion<\/strong>. Since lithium only has one electron to donate, it forms a bond with sulfur by transferring its electron. The result is an ionic compound where the two lithium ions (Li\u207a) are attracted to the sulfide ion (S\u00b2\u207b) due to electrostatic forces.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Lewis Structure:<\/h3>\n\n\n\n<pre class=\"wp-block-code\"><code>Li\u207a      Li\u207a\n  \\     \/\n   S\u00b2\u207b<\/code><\/pre>\n\n\n\n<p>The structure shows each lithium ion (Li\u207a) with a positive charge, the sulfide ion (S\u00b2\u207b) with eight electrons (four pairs), and a negative charge of -2.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw a suitable Lewis structure for Li2S. In the structure, there are two sulfide ions and one lithium ion.there are two lithium atoms and one sulfur atom with 6 electrons.each lithium atom makes one bond to sulfur.there are two lithium ions each with a +1 charge and one sulfide ion with four pairs of electrons [&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-203054","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203054","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=203054"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203054\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=203054"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=203054"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=203054"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}