{"id":187326,"date":"2025-02-04T06:36:39","date_gmt":"2025-02-04T06:36:39","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187326"},"modified":"2025-02-04T06:36:41","modified_gmt":"2025-02-04T06:36:41","slug":"draw-the-lewis-structure-for-the-ionic-compound-na2so4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/04\/draw-the-lewis-structure-for-the-ionic-compound-na2so4\/","title":{"rendered":"Draw the Lewis Structure for the ionic compound Na2SO4"},"content":{"rendered":"\n<p>Draw the Lewis Structure for the ionic compound Na2SO4.<\/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\"><strong>Lewis Structure of Na\u2082SO\u2084 (Sodium Sulfate)<\/strong><\/h3>\n\n\n\n<p>To draw the <strong>Lewis structure<\/strong> for sodium sulfate (<strong>Na\u2082SO\u2084<\/strong>), follow these steps:<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 1: Identify the Atoms and Their Valence Electrons<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sodium (Na)<\/strong>: Belongs to Group 1, so it has <strong>1 valence electron<\/strong>.<\/li>\n\n\n\n<li><strong>Sulfur (S)<\/strong>: Belongs to Group 16, so it has <strong>6 valence electrons<\/strong>.<\/li>\n\n\n\n<li><strong>Oxygen (O)<\/strong>: Belongs to Group 16, so each oxygen has <strong>6 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 2: Determine the Ionic Nature<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sodium sulfate is an <strong>ionic compound<\/strong>, meaning sodium donates electrons to form <strong>Na\u207a<\/strong> ions, and sulfate forms a <strong>polyatomic ion (SO\u2084\u00b2\u207b)<\/strong>.<\/li>\n\n\n\n<li>Each Na atom loses <strong>1 electron<\/strong>, creating <strong>Na\u207a<\/strong> ions.<\/li>\n\n\n\n<li>The sulfate ion (<strong>SO\u2084\u00b2\u207b<\/strong>) has an overall charge of <strong>-2<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 3: Draw the Lewis Structure of SO\u2084\u00b2\u207b<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sulfur<\/strong> is the <strong>central atom<\/strong>, surrounded by <strong>four oxygens<\/strong>.<\/li>\n\n\n\n<li><strong>Sulfur forms double bonds with two oxygens<\/strong> and <strong>single bonds with the other two oxygens<\/strong>, which carry <strong>negative charges<\/strong>.<\/li>\n\n\n\n<li>The <strong>total valence electrons<\/strong> used:<\/li>\n\n\n\n<li>Sulfur: 6<\/li>\n\n\n\n<li>Oxygen: (6 \u00d7 4) = 24<\/li>\n\n\n\n<li>Extra <strong>2 electrons<\/strong> (from the -2 charge).<\/li>\n\n\n\n<li>Total: <strong>32 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Step 4: Place the Ions Together<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sodium ions (Na\u207a)<\/strong> are placed separately <strong>outside<\/strong> the sulfate ion since ionic bonds do not involve shared electrons.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Final Lewis Structure<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Na\u2082SO\u2084 is represented as:<\/strong><\/li>\n\n\n\n<li><strong>[ SO\u2084\u00b2\u207b ]<\/strong> with its correct oxygen bonding.<\/li>\n\n\n\n<li>Two separate <strong>Na\u207a ions<\/strong> are placed outside the bracket.<\/li>\n<\/ul>\n\n\n\n<p>This structure <strong>shows ionic bonding<\/strong> between Na\u207a and SO\u2084\u00b2\u207b while <strong>SO\u2084\u00b2\u207b itself has covalent bonding<\/strong> within.<\/p>\n\n\n\n<p>Would you like a diagram to visualize it?<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis Structure for the ionic compound Na2SO4. The Correct Answer and Explanation is : Lewis Structure of Na\u2082SO\u2084 (Sodium Sulfate) To draw the Lewis structure for sodium sulfate (Na\u2082SO\u2084), follow these steps: Step 1: Identify the Atoms and Their Valence Electrons Step 2: Determine the Ionic Nature Step 3: Draw the Lewis Structure [&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-187326","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187326","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=187326"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187326\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187326"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187326"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187326"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}