{"id":179611,"date":"2025-01-01T20:11:31","date_gmt":"2025-01-01T20:11:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=179611"},"modified":"2025-01-01T20:11:33","modified_gmt":"2025-01-01T20:11:33","slug":"draw-the-lewis-structure-for-sf3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/01\/draw-the-lewis-structure-for-sf3\/","title":{"rendered":"Draw the lewis structure for SF3"},"content":{"rendered":"\n<p>Draw the lewis structure for SF3 , and indicate how many electron groups are around the central sulfur atom in SF3 , and What is electron geometry and molecular geometry? (Note: You need to show complete solution map by drawing the Lewis structure of SF, in your Quiz 3 Honor Pledge to receive Full credit).<\/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>To draw the Lewis structure for SF\u2083 (sulfur trifluoride), we will go through the following steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Determine the Total Number of Valence Electrons<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sulfur (S)<\/strong>: Sulfur is in Group 16 of the periodic table, so it has 6 valence electrons.<\/li>\n\n\n\n<li><strong>Fluorine (F)<\/strong>: Fluorine is in Group 17, so each fluorine atom has 7 valence electrons. Since there are three fluorine atoms, we multiply by 3: 7 * 3 = 21 valence electrons from fluorine.<\/li>\n<\/ul>\n\n\n\n<p>So, the total number of valence electrons for SF\u2083 is:<br>6 (from sulfur) + 21 (from fluorine) = <strong>27 valence electrons<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Draw the Skeleton Structure<\/h3>\n\n\n\n<p>Place sulfur as the central atom since it is less electronegative than fluorine. Connect each fluorine atom to the sulfur atom with a single bond (which uses 2 electrons per bond).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Distribute the Electrons<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each single bond between sulfur and fluorine uses 2 electrons, so 3 bonds will use 6 electrons (3 bonds * 2 electrons = 6 electrons).<\/li>\n\n\n\n<li>We have 27 total electrons, so after placing the bonds, we are left with 27 &#8211; 6 = 21 electrons.<\/li>\n\n\n\n<li>Distribute these remaining 21 electrons as lone pairs around the fluorine atoms first. Each fluorine needs 3 lone pairs (6 electrons) to satisfy the octet rule.<\/li>\n\n\n\n<li>After placing 3 lone pairs on each of the three fluorine atoms (18 electrons), we have 3 electrons remaining, which will go to the sulfur atom.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Assign Lone Pairs to the Central Atom<\/h3>\n\n\n\n<p>Sulfur can have an expanded octet, so it can accommodate more than 8 electrons. Place the remaining 3 electrons as a lone pair on the sulfur atom.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 5: Final Structure<\/h3>\n\n\n\n<p>The Lewis structure is as follows:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sulfur<\/strong> is the central atom with a lone pair of electrons.<\/li>\n\n\n\n<li>Each <strong>fluorine<\/strong> is attached by a single bond and has 3 lone pairs.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 6: Electron Groups and Geometry<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The central sulfur atom has three single bonds to fluorine and one lone pair of electrons, so there are <strong>4 electron groups<\/strong> around sulfur (3 bonding groups + 1 lone pair).<\/li>\n\n\n\n<li>The <strong>electron geometry<\/strong> is based on the number of electron groups around the central atom. With 4 electron groups, the electron geometry is <strong>tetrahedral<\/strong>.<\/li>\n\n\n\n<li>The <strong>molecular geometry<\/strong> is based on the positions of the atoms, excluding the lone pair. With 3 bonding groups and 1 lone pair, the molecular geometry is <strong>trigonal pyramidal<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Conclusion<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The Lewis structure for SF\u2083 shows sulfur with three bonds to fluorine atoms and one lone pair on sulfur.<\/li>\n\n\n\n<li>There are <strong>4 electron groups<\/strong> around the sulfur atom, which gives the molecule a <strong>tetrahedral electron geometry<\/strong>.<\/li>\n\n\n\n<li>The <strong>molecular geometry<\/strong> is <strong>trigonal pyramidal<\/strong> due to the lone pair on sulfur.<\/li>\n<\/ul>\n\n\n\n<p>This solution involves a tetrahedral arrangement, which corresponds to a trigonal pyramidal shape for the molecular geometry due to the presence of the lone pair. The central sulfur atom&#8217;s expanded octet allows it to accommodate more than 8 electrons.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the lewis structure for SF3 , and indicate how many electron groups are around the central sulfur atom in SF3 , and What is electron geometry and molecular geometry? (Note: You need to show complete solution map by drawing the Lewis structure of SF, in your Quiz 3 Honor Pledge to receive Full credit). [&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-179611","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/179611","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=179611"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/179611\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=179611"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=179611"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=179611"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}