{"id":216262,"date":"2025-05-19T03:30:34","date_gmt":"2025-05-19T03:30:34","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=216262"},"modified":"2025-05-19T07:43:20","modified_gmt":"2025-05-19T07:43:20","slug":"question-2-1-pts-consider-the-lewis-structure-for-sf6-there-are-a-total-of-valence-electrons","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/19\/question-2-1-pts-consider-the-lewis-structure-for-sf6-there-are-a-total-of-valence-electrons\/","title":{"rendered":"Consider the Lewis structure for SF6 There are a total of valence electrons."},"content":{"rendered":"\n<p class=\"wp-block-paragraph\">Consider the Lewis structure for SF6 There are a total of valence electrons. There are bonding electrons, non-bonding electrons, and lone pairs of electrons.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Question 3 1 pts Using VSEPR theory, a molecule with the general formula AX Ex (A is the central atom, X is the bonded atom and E is a lone pair of electrons), how many regions of electron density around the central atom in AXs? (the E subscript is zero) [Select] axs will have what kind of electron-group arrangement? [select] axs will have what kind of molecular shape?<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Question 2: Lewis Structure of SF\u2086<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total valence electrons<\/strong>: <strong>48<\/strong><\/li>\n\n\n\n<li><strong>Bonding electrons<\/strong>: <strong>12<\/strong><\/li>\n\n\n\n<li><strong>Non-bonding electrons<\/strong>: <strong>36<\/strong><\/li>\n\n\n\n<li><strong>Lone pairs of electrons<\/strong>: <strong>18<\/strong><\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Question 3: AX\u2086 Molecule Based on VSEPR Theory<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Regions of electron density<\/strong>: <strong>6<\/strong><\/li>\n\n\n\n<li><strong>Electron-group arrangement<\/strong>: <strong>Octahedral<\/strong><\/li>\n\n\n\n<li><strong>Molecular shape<\/strong>: <strong>Octahedral<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation (300+ words)<\/strong><\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Question 2: Lewis Structure of SF\u2086<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">Sulfur hexafluoride (SF\u2086) is a molecule consisting of one sulfur atom (S) and six fluorine atoms (F). To determine the number of valence electrons:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sulfur (group 16) has <strong>6 valence electrons<\/strong>.<\/li>\n\n\n\n<li>Fluorine (group 17) has <strong>7 valence electrons<\/strong> each \u00d7 6 = <strong>42 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Total = 6 (S) + 42 (F) = 48 valence electrons.<\/strong><\/p>\n\n\n\n<p class=\"wp-block-paragraph\">In the Lewis structure:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sulfur forms <strong>six single bonds<\/strong> with each fluorine atom.<\/li>\n\n\n\n<li>Each bond contains <strong>2 electrons<\/strong>, so <strong>6 bonds \u00d7 2 = 12 bonding electrons<\/strong>.<\/li>\n\n\n\n<li>The remaining <strong>36 electrons<\/strong> (48 total \u2013 12 bonding) are assigned as <strong>non-bonding electrons<\/strong> (lone pairs) on the fluorine atoms.<\/li>\n\n\n\n<li>Each fluorine gets 3 lone pairs (6 electrons), and 6 fluorines \u00d7 6 electrons = 36 non-bonding electrons.<\/li>\n\n\n\n<li>These 36 non-bonding electrons are grouped into <strong>18 lone pairs<\/strong>.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Question 3: AX\u2086 Molecule Using VSEPR Theory<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">VSEPR (Valence Shell Electron Pair Repulsion) theory helps predict molecular geometry by minimizing repulsions between regions of electron density (bonds or lone pairs) around a central atom.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">For an AX\u2086 molecule:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>A<\/strong> is the central atom.<\/li>\n\n\n\n<li><strong>X\u2086<\/strong> indicates <strong>six bonded atoms<\/strong>.<\/li>\n\n\n\n<li>There are <strong>no lone pairs on the central atom<\/strong> (E = 0).<\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">This gives <strong>six regions of electron density<\/strong>, all bonding pairs. To minimize repulsion, these arrange themselves in an <strong>octahedral geometry<\/strong>.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron-group arrangement<\/strong>: Octahedral<\/li>\n\n\n\n<li><strong>Molecular shape<\/strong>: Octahedral (since there are no lone pairs altering the shape)<\/li>\n\n\n\n<li><strong>Bond angles<\/strong>: 90\u00b0 between all adjacent atoms.<\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">Examples of AX\u2086 molecules include SF\u2086, where sulfur is bonded to six fluorine atoms symmetrically. The octahedral shape is highly symmetrical and stable, which is why SF\u2086 is used as an inert electrical insulator.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">In summary:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>SF\u2086 has 48 valence electrons: 12 bonding, 36 non-bonding.<\/li>\n\n\n\n<li>AX\u2086 molecules have 6 electron regions, an octahedral geometry, and an octahedral molecular shape.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Consider the Lewis structure for SF6 There are a total of valence electrons. There are bonding electrons, non-bonding electrons, and lone pairs of electrons. Question 3 1 pts Using VSEPR theory, a molecule with the general formula AX Ex (A is the central atom, X is the bonded atom and E is a lone pair [&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-216262","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/216262","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=216262"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/216262\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=216262"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=216262"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=216262"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}