{"id":228547,"date":"2025-06-07T11:10:47","date_gmt":"2025-06-07T11:10:47","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=228547"},"modified":"2025-06-07T11:10:49","modified_gmt":"2025-06-07T11:10:49","slug":"total-valence-electrons-34-rough-lewis-structure-tef4-molecular-geometry-electron-group-geometry-see-saw-trigonal-bipyramidal-formula-te_e-solubility-more-soluble-in-hexane-or-water","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/07\/total-valence-electrons-34-rough-lewis-structure-tef4-molecular-geometry-electron-group-geometry-see-saw-trigonal-bipyramidal-formula-te_e-solubility-more-soluble-in-hexane-or-water\/","title":{"rendered":"Total Valence Electrons: 34 Rough Lewis Structure: TeF4 Molecular Geometry \/ Electron-Group Geometry: See-saw\/trigonal bipyramidal Formula: #-Te_E Solubility: More soluble in hexane or water"},"content":{"rendered":"\n<p>Total Valence Electrons: 34 Rough Lewis Structure: TeF4 Molecular Geometry \/ Electron-Group Geometry: See-saw\/trigonal bipyramidal Formula: #-Te_E Solubility: More soluble in hexane or water? Bond Polarity (AEN): Te &#8211; F = 2.1 4.0 = 1.9 Molecule Polarity: water<\/p>\n\n\n\n<p><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<p><strong>Correct Answers:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Total Valence Electrons:<\/strong> 34<\/li>\n\n\n\n<li><strong>Rough Lewis Structure:<\/strong><br>Central atom: Te (Tellurium)<br>Four single bonds to F atoms and one lone pair on Te<\/li>\n\n\n\n<li><strong>Molecular Geometry \/ Electron-Group Geometry:<\/strong>\n<ul class=\"wp-block-list\">\n<li><strong>Molecular Geometry:<\/strong> See-saw<\/li>\n\n\n\n<li><strong>Electron-Group Geometry:<\/strong> Trigonal bipyramidal<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Formula:<\/strong> TeF\u2084<\/li>\n\n\n\n<li><strong>Solubility:<\/strong> More soluble in <strong>water<\/strong><\/li>\n\n\n\n<li><strong>Bond Polarity (\u0394EN):<\/strong><br>\u0394EN = |4.0 (F) \u2013 2.1 (Te)| = <strong>1.9<\/strong><\/li>\n\n\n\n<li><strong>Molecule Polarity:<\/strong> <strong>Polar<\/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\">Explanation<\/h3>\n\n\n\n<p>Tellurium tetrafluoride (<strong>TeF\u2084<\/strong>) is a molecule consisting of a central tellurium atom bonded to four fluorine atoms. To determine the number of valence electrons, we sum the valence electrons of tellurium (6 valence electrons from Group 16) and fluorine (7 valence electrons from Group 17):<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Te: 6 electrons<\/li>\n\n\n\n<li>F: 4 \u00d7 7 = 28 electrons<\/li>\n\n\n\n<li><strong>Total = 6 + 28 = 34 valence electrons<\/strong><\/li>\n<\/ul>\n\n\n\n<p>In the Lewis structure, tellurium is the central atom with four single bonds to fluorine atoms and one lone pair. This results in five electron regions (4 bonding pairs + 1 lone pair), giving it a <strong>trigonal bipyramidal<\/strong> electron-group geometry. However, because one of those regions is a lone pair, the <strong>molecular geometry<\/strong> is <strong>see-saw<\/strong>.<\/p>\n\n\n\n<p>Fluorine is much more electronegative (4.0) than tellurium (2.1), making each Te\u2013F bond <strong>polar<\/strong>, with a significant electronegativity difference of <strong>1.9<\/strong>. Since the molecular shape is asymmetrical due to the lone pair, the individual bond dipoles do not cancel out. Therefore, <strong>TeF\u2084 is a polar molecule<\/strong>.<\/p>\n\n\n\n<p>In terms of <strong>solubility<\/strong>, polar molecules tend to dissolve better in <strong>polar solvents<\/strong>, following the principle \u201clike dissolves like.\u201d <strong>Water<\/strong>, being highly polar, is a better solvent for TeF\u2084 than <strong>hexane<\/strong>, a nonpolar solvent. Thus, <strong>TeF\u2084 is more soluble in water<\/strong> than in hexane.<\/p>\n\n\n\n<p>In summary, TeF\u2084 has 34 valence electrons, a see-saw molecular geometry, polar bonds, and an overall polar structure, making it more soluble in polar solvents like water.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner6-118.jpeg\" alt=\"\" class=\"wp-image-228548\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Total Valence Electrons: 34 Rough Lewis Structure: TeF4 Molecular Geometry \/ Electron-Group Geometry: See-saw\/trigonal bipyramidal Formula: #-Te_E Solubility: More soluble in hexane or water? Bond Polarity (AEN): Te &#8211; F = 2.1 4.0 = 1.9 Molecule Polarity: water The Correct Answer and Explanation is: Correct Answers: Explanation Tellurium tetrafluoride (TeF\u2084) is a molecule consisting 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-228547","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/228547","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=228547"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/228547\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=228547"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=228547"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=228547"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}