Correct Answer Summary for Sulfur Hexafluoride (SF\u2086):<\/strong><\/p>\n\n\n\n Explanation<\/strong><\/p>\n\n\n\n Sulfur hexafluoride (SF\u2086) is a highly symmetrical molecule with interesting structural and electronic characteristics. To begin, we calculate the total number of valence electrons<\/strong>: sulfur has 6 valence electrons, and each of the six fluorine atoms contributes 7, giving a total of 6+(6\u00d77)=486 + (6 \\times 7) = 486+(6\u00d77)=48 valence electrons.<\/p>\n\n\n\n The Lewis structure<\/strong> places sulfur in the center with six single bonds to six fluorine atoms. Each fluorine completes its octet with three lone pairs. Sulfur, as a third-period element, can expand its octet<\/strong>, accommodating 12 electrons (six bonds). There are no formal charges<\/strong> on any atoms in the most stable structure, and no resonance structures<\/strong> are necessary since each F atom is equivalent and forms a single bond.<\/p>\n\n\n\n The electron domain geometry<\/strong> around sulfur is octahedral<\/strong>, based on six bonding pairs and no lone pairs. This leads directly to the molecular shape<\/strong>, which is also octahedral. As a result, bond angles<\/strong> are all 90\u00b0, characteristic of octahedral geometry.<\/p>\n\n\n\n Each S\u2013F bond is polar<\/strong> due to fluorine\u2019s high electronegativity. However, the molecule is nonpolar overall<\/strong> because the symmetrical arrangement of identical polar bonds causes dipole moments to cancel out.<\/p>\n\n\n\n The hybridization<\/strong> of the sulfur atom in SF\u2086 is sp\u00b3d\u00b2<\/strong>, involving one s orbital, three p orbitals, and two d orbitals. This hybridization supports the six sigma bonds needed to form the octahedral shape.<\/p>\n\n\n\n In summary, SF\u2086 is a nonpolar molecule with polar bonds, an octahedral shape, and expanded octet hybridization. Its structure makes it very stable and inert, explaining its use as an insulator in electrical applications.<\/p>\n\n\n\n Instructor initials Sulfur hexafluoride Formula: SF6 Lewis Structure (including appropriate resonance forms and formal charges) Number of valence electrons: 48 Electron domain geometry: Octahedral Molecular shape: Octahedral Bond angles: 90 degrees Polarity of individual bonds: Nonpolar Overall polarity of molecule: Nonpolar Hybridization of the central atom: sp3d2 The Correct Answer and Explanation is: Correct Answer […]<\/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-227203","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227203","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=227203"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227203\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=227203"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=227203"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=227203"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}\n
Central sulfur (S) atom with six fluorine (F) atoms bonded via single bonds; no lone pairs on S; each F has three lone pairs.
No resonance forms are needed.
Formal charges: 0 on all atoms.<\/li>\n\n\n\n
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