{"id":221556,"date":"2025-05-29T19:18:22","date_gmt":"2025-05-29T19:18:22","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=221556"},"modified":"2025-05-29T19:18:25","modified_gmt":"2025-05-29T19:18:25","slug":"how-many-of-the-following-molecules-are-polar","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/29\/how-many-of-the-following-molecules-are-polar\/","title":{"rendered":"How many of the following molecules are polar"},"content":{"rendered":"\n<p>How many of the following molecules are polar?<\/p>\n\n\n\n<p>BrF3, CS2, SiF4, SO3<\/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>To determine how many of the molecules <strong>BrF\u2083<\/strong>, <strong>CS\u2082<\/strong>, <strong>SiF\u2084<\/strong>, and <strong>SO\u2083<\/strong> are polar, we must examine both <strong>molecular geometry<\/strong> and <strong>electronegativity differences<\/strong>. A molecule is polar if it has a <strong>net dipole moment<\/strong>, meaning the distribution of electron density is uneven across the molecule due to its shape and the nature of its bonds.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">1. <strong>BrF\u2083 (Bromine trifluoride)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: Br is the central atom with three bonding pairs and two lone pairs.<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: T-shaped (based on a trigonal bipyramidal electron geometry).<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: <strong>Polar<\/strong>, because the shape causes an asymmetrical distribution of electron density, leading to a net dipole moment.<\/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\">2. <strong>CS\u2082 (Carbon disulfide)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: Linear molecule with double bonds between C and S atoms.<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Linear.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: <strong>Nonpolar<\/strong>, because the two polar C=S bonds are 180\u00b0 apart and cancel out each other\u2019s dipole moments.<\/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\">3. <strong>SiF\u2084 (Silicon tetrafluoride)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: Si is bonded to four fluorine atoms.<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Tetrahedral.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: <strong>Nonpolar<\/strong>, due to its symmetrical shape, the dipoles cancel out even though Si\u2013F bonds are polar.<\/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\">4. <strong>SO\u2083 (Sulfur trioxide)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure<\/strong>: S bonded to three O atoms with double bonds (resonance structures).<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: Trigonal planar.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: <strong>Nonpolar<\/strong>, because the molecular symmetry causes dipoles to cancel out.<\/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\">Final Answer:<\/h3>\n\n\n\n<p><strong>Only one molecule, BrF\u2083, is polar.<\/strong><br><strong>Correct Answer: 1<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p>Understanding molecular polarity is crucial in predicting a substance\u2019s physical properties, such as solubility and boiling point. Despite the presence of polar bonds, overall molecular symmetry often determines whether a molecule is polar. BrF\u2083\u2019s asymmetrical shape leads to a net dipole moment, making it the only polar molecule among the four.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner7-106.jpeg\" alt=\"\" class=\"wp-image-221557\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>How many of the following molecules are polar? BrF3, CS2, SiF4, SO3 The Correct Answer and Explanation is: To determine how many of the molecules BrF\u2083, CS\u2082, SiF\u2084, and SO\u2083 are polar, we must examine both molecular geometry and electronegativity differences. A molecule is polar if it has a net dipole moment, meaning the distribution [&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-221556","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221556","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=221556"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221556\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=221556"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=221556"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=221556"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}