{"id":205790,"date":"2025-03-25T16:50:47","date_gmt":"2025-03-25T16:50:47","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=205790"},"modified":"2025-03-25T16:50:50","modified_gmt":"2025-03-25T16:50:50","slug":"fact-when-the-lewis-structure-of-the-sulfate-ion","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/25\/fact-when-the-lewis-structure-of-the-sulfate-ion\/","title":{"rendered":"Fact: When the Lewis structure of the sulfate ion"},"content":{"rendered":"\n<p>Fact: When the Lewis structure of the sulfate ion, SO42- is drawn, the central atom S expands its octet to allow for 16 valence electrons to be present in the valence shell, resulting in two of the O atoms each forming a double bond with S while the other two O atoms each forming a single bond with S. The average bond length of a single S-O bond is 157 picometers (pm), while the average bond length of a double bond between S and O is 143 pm. However, the actual length of all of the bonds between S and O is known to be 149 pm in SO42-. The H-H bond length is about 74 pm. Despite what happens to S, the shape of SO42- remains as tetrahedral. True or false: There are six (6) resonance structures for SO42-. False O True<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p><strong>Correct Answer: False<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The sulfate ion (<strong>SO\u2084\u00b2\u207b<\/strong>) has <strong>four resonance structures<\/strong>, not six. Resonance structures are different ways to represent the distribution of electrons in a molecule while keeping the atomic positions unchanged.<\/p>\n\n\n\n<p>In the <strong>Lewis structure<\/strong> of sulfate, sulfur is the central atom bonded to four oxygen atoms. Sulfur has an expanded octet, meaning it can accommodate more than eight valence electrons. The <strong>formal charge minimization<\/strong> leads to a resonance hybrid where two of the oxygen atoms have <strong>double bonds (S=O)<\/strong> and two have <strong>single bonds (S-O\u207b)<\/strong> with negative charges on them.<\/p>\n\n\n\n<p>However, since <strong>any two oxygen atoms can be chosen to form double bonds<\/strong>, we can <strong>rotate the positions<\/strong> of the double bonds among the four oxygen atoms, leading to <strong>four equivalent resonance structures<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Why Not Six?<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Only Four Ways to Arrange the Double Bonds:<\/strong> There are four oxygen atoms, and each resonance structure places two <strong>double bonds<\/strong> and two <strong>single bonds<\/strong> differently while maintaining overall charge distribution.<\/li>\n\n\n\n<li><strong>All S-O Bonds Are Identical in Reality:<\/strong> Experimental data shows that all S-O bond lengths are <strong>149 pm<\/strong>, which is between the typical single (157 pm) and double bond (143 pm) lengths. This suggests <strong>delocalization of electrons<\/strong>, meaning no single structure fully represents the molecule. Instead, the <strong>resonance hybrid<\/strong> is a weighted blend of these structures.<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\">Molecular Shape:<\/h3>\n\n\n\n<p>Despite resonance, <strong>SO\u2084\u00b2\u207b remains tetrahedral<\/strong> due to four regions of electron density around sulfur, following <strong>VSEPR (Valence Shell Electron Pair Repulsion) theory<\/strong>.<\/p>\n\n\n\n<p>Thus, the correct answer is <strong>False\u2014SO\u2084\u00b2\u207b has four resonance structures, not six<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Image Generation Request:<\/h3>\n\n\n\n<p>A <strong>ball-and-stick model<\/strong> of the sulfate ion, showing:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sulfur in the center<\/strong>,<\/li>\n\n\n\n<li><strong>Four oxygen atoms symmetrically arranged<\/strong>,<\/li>\n\n\n\n<li><strong>Delocalized electron representation<\/strong>,<\/li>\n\n\n\n<li><strong>Tetrahedral geometry<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Here is the ball-and-stick model of the sulfate ion (<strong>SO\u2084\u00b2\u207b<\/strong>), showing its <strong>tetrahedral geometry<\/strong> and <strong>delocalized bonding<\/strong> due to resonance. Let me know if you need any modifications!<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-1417.png\" alt=\"\" class=\"wp-image-205791\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Fact: When the Lewis structure of the sulfate ion, SO42- is drawn, the central atom S expands its octet to allow for 16 valence electrons to be present in the valence shell, resulting in two of the O atoms each forming a double bond with S while the other two O atoms each forming a [&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-205790","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/205790","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=205790"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/205790\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=205790"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=205790"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=205790"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}