{"id":213719,"date":"2025-05-12T08:24:53","date_gmt":"2025-05-12T08:24:53","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=213719"},"modified":"2025-05-12T08:24:56","modified_gmt":"2025-05-12T08:24:56","slug":"selenium-tetrafluoride-sef4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/12\/selenium-tetrafluoride-sef4\/","title":{"rendered":"selenium tetrafluoride, SeF4"},"content":{"rendered":"\n<p>selenium tetrafluoride, SeF4<\/p>\n\n\n\n<p>valence electrons: Lewis structure: tribromide ion, Brs<\/p>\n\n\n\n<p>valence electrons: dre (indi Geometry description: Hybridization of central atom; Bonding description: Geometry description: Hybridization of central atom; Bonding description<\/p>\n\n\n\n<p>Draw the molecule with the correct shape.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>Let&#8217;s analyze <strong>selenium tetrafluoride (SeF\u2084)<\/strong> and <strong>tribromide ion (Br\u2083\u207b)<\/strong> in terms of:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence electrons<\/strong><\/li>\n\n\n\n<li><strong>Lewis structure<\/strong><\/li>\n\n\n\n<li><strong>Electron geometry<\/strong><\/li>\n\n\n\n<li><strong>Molecular geometry<\/strong><\/li>\n\n\n\n<li><strong>Hybridization<\/strong><\/li>\n\n\n\n<li><strong>Bonding description<\/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>1. Selenium Tetrafluoride (SeF\u2084)<\/strong><\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Valence Electrons:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Selenium (Se) has <strong>6<\/strong> valence electrons.<\/li>\n\n\n\n<li>Each fluorine (F) has <strong>7<\/strong> valence electrons.<\/li>\n\n\n\n<li>Total = 6 (Se) + 4\u00d77 (F) = <strong>34 valence electrons<\/strong><\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Lewis Structure:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Se is the central atom.<\/li>\n\n\n\n<li>Place single bonds between Se and four F atoms.<\/li>\n\n\n\n<li>Each bond uses 2 electrons \u00d7 4 = 8 electrons.<\/li>\n\n\n\n<li>Remaining: 34 \u2013 8 = 26 electrons \u2192 distributed as lone pairs on F and Se.<\/li>\n\n\n\n<li>Each F gets 6 electrons as lone pairs (24 total for 4 F atoms).<\/li>\n\n\n\n<li>Remaining 2 electrons are placed as a <strong>lone pair on Se<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Electron Geometry:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>There are <strong>5 electron regions<\/strong> (4 bonding pairs, 1 lone pair) around Se.<\/li>\n\n\n\n<li>Geometry: <strong>Trigonal bipyramidal<\/strong> (based on VSEPR)<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Molecular Geometry:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>With one lone pair, actual shape is <strong>see-saw<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Hybridization:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>5 electron regions = <strong>sp\u00b3d<\/strong><\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Bonding Description:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Se forms 4 sigma bonds with F atoms using sp\u00b3d hybrid orbitals.<\/li>\n\n\n\n<li>One lone pair resides in the equatorial position to minimize repulsion.<\/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>2. Tribromide Ion (Br\u2083\u207b)<\/strong><\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Valence Electrons:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each Br has 7 valence electrons \u2192 3\u00d77 = 21<\/li>\n\n\n\n<li>Add 1 for the negative charge \u2192 <strong>22 valence electrons<\/strong><\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Lewis Structure:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Linear arrangement: Br\u2013Br\u2013Br\u207b<\/li>\n\n\n\n<li>The central Br forms two single bonds with the outer Br atoms.<\/li>\n\n\n\n<li>Lone pairs complete octets; central Br has 3 lone pairs, outer Br atoms each have 3.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Electron Geometry:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>5 electron domains on central Br (2 bonding, 3 lone pairs) = <strong>trigonal bipyramidal<\/strong><\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Molecular Geometry:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>With 3 lone pairs, the shape is <strong>linear<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Hybridization:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>5 regions = <strong>sp\u00b3d<\/strong><\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Bonding Description:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The central Br uses sp\u00b3d orbitals to form sigma bonds.<\/li>\n\n\n\n<li>The linear shape minimizes repulsion from the lone pairs in equatorial positions.<\/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>Summary Table<\/strong><\/h3>\n\n\n\n<figure class=\"wp-block-table\"><table class=\"has-fixed-layout\"><thead><tr><th>Molecule\/Ion<\/th><th>Valence e\u207b<\/th><th>Electron Geometry<\/th><th>Molecular Geometry<\/th><th>Hybridization<\/th><th>Shape Description<\/th><\/tr><\/thead><tbody><tr><td>SeF\u2084<\/td><td>34<\/td><td>Trigonal bipyramidal<\/td><td>See-saw<\/td><td>sp\u00b3d<\/td><td>Four bonds + 1 lone pair<\/td><\/tr><tr><td>Br\u2083\u207b<\/td><td>22<\/td><td>Trigonal bipyramidal<\/td><td>Linear<\/td><td>sp\u00b3d<\/td><td>Two bonds + 3 lone pairs<\/td><\/tr><\/tbody><\/table><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>selenium tetrafluoride, SeF4 valence electrons: Lewis structure: tribromide ion, Brs valence electrons: dre (indi Geometry description: Hybridization of central atom; Bonding description: Geometry description: Hybridization of central atom; Bonding description Draw the molecule with the correct shape. The Correct Answer and Explanation is: Let&#8217;s analyze selenium tetrafluoride (SeF\u2084) and tribromide ion (Br\u2083\u207b) in terms of: [&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-213719","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/213719","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=213719"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/213719\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=213719"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=213719"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=213719"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}