{"id":204532,"date":"2025-03-22T08:27:13","date_gmt":"2025-03-22T08:27:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=204532"},"modified":"2025-03-22T08:27:15","modified_gmt":"2025-03-22T08:27:15","slug":"from-your-models-of-sf4-brf3-and-xef4-deduce-whether-different-atom-arrangements-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/22\/from-your-models-of-sf4-brf3-and-xef4-deduce-whether-different-atom-arrangements-2\/","title":{"rendered":"From your models of SF4 , BrF3, and XeF4 deduce whether different atom arrangements"},"content":{"rendered":"\n<p>From your models of SF4 , BrF3, and XeF4 deduce whether different atom arrangements, called geometrical isomers are possible; if so, sketch them below. Indicate the preferred geometry for each case and suggest a reason for your choice. Indicate which structures have dipole moments and show their direction.<\/p>\n\n\n\n<p>(A) SF4<\/p>\n\n\n\n<p>(B) BrF3<\/p>\n\n\n\n<p>(C) XeF4<\/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<h3 class=\"wp-block-heading\">(A) SF4 (Sulfur Tetrafluoride)<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Geometry<\/strong>: The molecule has a <strong>see-saw<\/strong> shape, which is derived from a trigonal bipyramidal electron geometry, with one of the equatorial positions occupied by a lone pair.<\/li>\n\n\n\n<li><strong>Isomer Possibility<\/strong>: There are no significant geometrical isomers for SF4 because the lone pair occupies one of the equatorial positions, leading to a unique see-saw shape.<\/li>\n\n\n\n<li><strong>Dipole Moment<\/strong>: SF4 has a <strong>net dipole moment<\/strong> because the molecule is asymmetrical. The electronegativity of fluorine pulls electrons away from sulfur, and the shape causes these dipoles to not cancel out.<\/li>\n\n\n\n<li><strong>Direction of Dipole Moment<\/strong>: The dipole moment points toward the fluorine atoms and away from the sulfur atom.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">(B) BrF3 (Bromine Trifluoride)<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Geometry<\/strong>: BrF3 adopts a <strong>T-shaped<\/strong> geometry, similar to the structure of SF4 but with two lone pairs in the axial positions, resulting in a more compact shape.<\/li>\n\n\n\n<li><strong>Isomer Possibility<\/strong>: Geometrical isomerism is not possible for BrF3, as the lone pairs on the axial positions restrict any alternate spatial arrangements.<\/li>\n\n\n\n<li><strong>Dipole Moment<\/strong>: BrF3 has a <strong>net dipole moment<\/strong> because of the T-shaped structure, which is polar.<\/li>\n\n\n\n<li><strong>Direction of Dipole Moment<\/strong>: The dipole points towards the fluorine atoms, away from the central bromine atom.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">(C) XeF4 (Xenon Tetrafluoride)<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Geometry<\/strong>: XeF4 adopts a <strong>square planar<\/strong> geometry, which is typical for molecules with 4 bonding pairs and 2 lone pairs in an octahedral electron geometry.<\/li>\n\n\n\n<li><strong>Isomer Possibility<\/strong>: There are no geometrical isomers for XeF4. The presence of two lone pairs on opposite sides of the xenon atom ensures symmetry, resulting in a single, well-defined geometry.<\/li>\n\n\n\n<li><strong>Dipole Moment<\/strong>: XeF4 has <strong>no net dipole moment<\/strong>. The square planar geometry is symmetric, and the individual bond dipoles cancel out.<\/li>\n\n\n\n<li><strong>Direction of Dipole Moment<\/strong>: Since there is no net dipole moment, there is no direction.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Summary of Preferred Geometries and Dipole Moments:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>SF4<\/strong>: See-saw geometry with a dipole moment.<\/li>\n\n\n\n<li><strong>BrF3<\/strong>: T-shaped geometry with a dipole moment.<\/li>\n\n\n\n<li><strong>XeF4<\/strong>: Square planar geometry with no dipole moment.<\/li>\n<\/ol>\n\n\n\n<p><strong>Explanation<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Electron Pair Geometry<\/strong>: The geometry of each molecule is influenced by the number of bonding pairs and lone pairs around the central atom, determined by the VSEPR (Valence Shell Electron Pair Repulsion) theory.<\/li>\n\n\n\n<li><strong>Dipole Moment<\/strong>: A dipole moment arises in molecules with asymmetrical charge distributions. In SF4 and BrF3, the presence of lone pairs and the resulting asymmetry lead to a non-zero dipole moment, while XeF4&#8217;s symmetry cancels out individual dipoles.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>From your models of SF4 , BrF3, and XeF4 deduce whether different atom arrangements, called geometrical isomers are possible; if so, sketch them below. Indicate the preferred geometry for each case and suggest a reason for your choice. Indicate which structures have dipole moments and show their direction. (A) SF4 (B) BrF3 (C) XeF4 The [&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-204532","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/204532","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=204532"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/204532\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=204532"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=204532"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=204532"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}