{"id":202209,"date":"2025-03-17T09:23:42","date_gmt":"2025-03-17T09:23:42","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=202209"},"modified":"2025-03-17T09:23:44","modified_gmt":"2025-03-17T09:23:44","slug":"draw-the-lewis-structure-for-h2so4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/17\/draw-the-lewis-structure-for-h2so4\/","title":{"rendered":"Draw the Lewis structure for H2SO4"},"content":{"rendered":"\n<p>Draw the Lewis structure for H2SO4, a neutral 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>The Lewis structure of <strong>sulfuric acid (H\u2082SO\u2084)<\/strong> consists of a <strong>central sulfur atom<\/strong> bonded to <strong>four oxygen atoms<\/strong>, with two of those oxygens also bonded to hydrogen atoms. Below is the correct Lewis structure:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step-by-Step Construction:<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Determine the Total Valence Electrons:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Hydrogen (H) = 1 \u00d7 2 = 2<\/li>\n\n\n\n<li>Sulfur (S) = 6 \u00d7 1 = 6<\/li>\n\n\n\n<li>Oxygen (O) = 6 \u00d7 4 = 24<\/li>\n\n\n\n<li><strong>Total Valence Electrons<\/strong> = 2 + 6 + 24 = <strong>32 electrons<\/strong><\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Identify the Central Atom:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sulfur<\/strong> (S) is the least electronegative (except hydrogen) and can expand its octet.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Draw Single Bonds:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Connect <strong>sulfur to four oxygens<\/strong> via single bonds.<\/li>\n\n\n\n<li>Attach <strong>hydrogens to two oxygens<\/strong>, making hydroxyl (-OH) groups.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Complete the Octets:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The two <strong>OH oxygens<\/strong> have 8 electrons (2 from bonding, 6 as lone pairs).<\/li>\n\n\n\n<li>The remaining <strong>two oxygens form double bonds<\/strong> with sulfur to satisfy the octet rule.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Check Formal Charges:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The double-bonded oxygens have a formal charge of <strong>0<\/strong>.<\/li>\n\n\n\n<li>The <strong>OH groups keep neutral charges<\/strong>.<\/li>\n\n\n\n<li>Sulfur follows the expanded octet rule (12 valence electrons) but remains neutral.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Final Structure:<\/strong><\/h3>\n\n\n\n<pre class=\"wp-block-code\"><code>    O\n    ||\nH\u2014O\u2014S\u2014O\u2014H\n    ||\n    O<\/code><\/pre>\n\n\n\n<p>The molecule is <strong>tetrahedral<\/strong> around <strong>sulfur<\/strong>, and <strong>resonance occurs<\/strong> in the double-bonded oxygens.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation:<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Strong Acid Properties:<\/strong> H\u2082SO\u2084 is a strong acid because the <strong>O-H bonds<\/strong> readily dissociate in water.<\/li>\n\n\n\n<li><strong>Octet Expansion:<\/strong> Sulfur can <strong>hold more than 8 electrons<\/strong> due to its position in <strong>Period 3<\/strong>.<\/li>\n\n\n\n<li><strong>Resonance:<\/strong> The two <strong>S=O bonds resonate<\/strong>, making the structure more stable.<\/li>\n<\/ul>\n\n\n\n<p>This structure correctly follows <strong>valence and charge rules<\/strong>, explaining <strong>H\u2082SO\u2084\u2019s strong acidity and molecular stability<\/strong>. <\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure for H2SO4, a neutral molecule. The correct answer and explanation is : The Lewis structure of sulfuric acid (H\u2082SO\u2084) consists of a central sulfur atom bonded to four oxygen atoms, with two of those oxygens also bonded to hydrogen atoms. Below is the correct Lewis structure: Step-by-Step Construction: Final Structure: The [&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-202209","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/202209","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=202209"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/202209\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=202209"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=202209"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=202209"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}