{"id":156971,"date":"2024-10-17T19:34:09","date_gmt":"2024-10-17T19:34:09","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=156971"},"modified":"2024-10-17T19:34:11","modified_gmt":"2024-10-17T19:34:11","slug":"the-f-s-f-bond-angles-in-sf6-are","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/17\/the-f-s-f-bond-angles-in-sf6-are\/","title":{"rendered":"The F &#8211; S &#8211; F bond angles in SF6 are"},"content":{"rendered":"\n<p>The F &#8211; S &#8211; F bond angles in SF6 are<br>A) 90\u00b0 and 180\u00b0 <\/p>\n\n\n\n<p>B) 109.5\u00b0 <\/p>\n\n\n\n<p>C) 120\u00b0 <\/p>\n\n\n\n<p>D) 180\u00b0 <\/p>\n\n\n\n<p>E) 90\u00b0 and 120\u00b0<\/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<p>The correct answer is <strong>A) 90\u00b0 and 180\u00b0<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>SF\u2086 (sulfur hexafluoride) is a molecule in which a central sulfur (S) atom is bonded to six fluorine (F) atoms. The shape of the SF\u2086 molecule can be understood using VSEPR (Valence Shell Electron Pair Repulsion) theory, which predicts the geometry of molecules based on repulsions between electron pairs around the central atom.<\/p>\n\n\n\n<p>In SF\u2086, sulfur has six bonding pairs of electrons and no lone pairs. The six fluorine atoms are arranged around sulfur in such a way that the repulsions between these electron pairs are minimized. This leads to an <strong>octahedral geometry<\/strong>.<\/p>\n\n\n\n<p>In an octahedral geometry:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The six bonds are arranged symmetrically around the central atom.<\/li>\n\n\n\n<li>Four fluorine atoms are placed in the same plane, forming a square around the sulfur atom, and two fluorine atoms are located along the axis perpendicular to this plane.<\/li>\n<\/ul>\n\n\n\n<p>This arrangement results in two distinct bond angles:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>90\u00b0 bond angles<\/strong>: These occur between any two adjacent fluorine atoms in the octahedral structure, such as between atoms in the equatorial (square planar) plane and atoms in the axial positions.<\/li>\n\n\n\n<li><strong>180\u00b0 bond angles<\/strong>: These occur between two fluorine atoms positioned directly opposite each other along the axial positions.<\/li>\n<\/ol>\n\n\n\n<p>Thus, the F-S-F bond angles in SF\u2086 are 90\u00b0 (between adjacent fluorine atoms) and 180\u00b0 (between opposite fluorine atoms). There are no 120\u00b0 or 109.5\u00b0 bond angles, which are characteristic of different molecular geometries like trigonal planar or tetrahedral, respectively.<\/p>\n\n\n\n<p>The octahedral geometry is also highly symmetrical, contributing to SF\u2086 being non-polar despite its polar S-F bonds, as the dipoles cancel out due to the symmetric shape.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The F &#8211; S &#8211; F bond angles in SF6 areA) 90\u00b0 and 180\u00b0 B) 109.5\u00b0 C) 120\u00b0 D) 180\u00b0 E) 90\u00b0 and 120\u00b0 The Correct Answer and Explanation is : The correct answer is A) 90\u00b0 and 180\u00b0. Explanation: SF\u2086 (sulfur hexafluoride) is a molecule in which a central sulfur (S) atom is bonded [&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-156971","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/156971","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=156971"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/156971\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=156971"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=156971"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=156971"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}