{"id":250487,"date":"2025-07-10T09:47:52","date_gmt":"2025-07-10T09:47:52","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=250487"},"modified":"2025-07-10T09:47:54","modified_gmt":"2025-07-10T09:47:54","slug":"are-sulfur-tetrafluoride-sf4-and-nitrogen-trifluoride-nf3-polar-or-nonpolar","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/10\/are-sulfur-tetrafluoride-sf4-and-nitrogen-trifluoride-nf3-polar-or-nonpolar\/","title":{"rendered":"Are sulfur tetrafluoride (SF4) and nitrogen trifluoride (NF3) polar or nonpolar"},"content":{"rendered":"\n<p>Are sulfur tetrafluoride (SF4) and nitrogen trifluoride (NF3) polar or nonpolar? (Select all that apply: ) SF4 is polar; SF4 is nonpolar: NF3 is polar; NF3 is nonpolar:<\/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>The correct answer is:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>SF4 is polar<\/li>\n\n\n\n<li>NF3 is polar<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p><strong>1. Sulfur Tetrafluoride (SF4):<\/strong><br>SF4 is a polar molecule. This can be explained based on its molecular geometry and the electronegativity difference between sulfur and fluorine.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>SF4 has a <strong>see-saw<\/strong> molecular geometry due to the presence of one lone pair of electrons on the sulfur atom. This geometry is a result of the electron pairs in the valence shell of sulfur, which arrange themselves to minimize electron-electron repulsion.<\/li>\n\n\n\n<li>The electronegativity difference between sulfur and fluorine (where fluorine is more electronegative) causes a dipole moment to form. Since the molecule is not symmetrical due to the lone pair on sulfur, these dipoles do not cancel out, making SF4 a <strong>polar<\/strong> molecule.<\/li>\n<\/ul>\n\n\n\n<p><strong>2. Nitrogen Trifluoride (NF3):<\/strong><br>NF3 is also a <strong>polar<\/strong> molecule. Here&#8217;s why:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>NF3 has a <strong>trigonal pyramidal<\/strong> geometry, which is caused by the lone pair of electrons on nitrogen. In this geometry, the fluorine atoms are positioned around nitrogen in a way that leads to unequal distribution of electron density.<\/li>\n\n\n\n<li>The fluorine atoms, being highly electronegative, attract the shared electrons more strongly than nitrogen. This creates a dipole moment, and because the molecule is not symmetrical (due to the lone pair on nitrogen), these dipoles do not cancel out, resulting in an overall <strong>polar<\/strong> molecule.<\/li>\n<\/ul>\n\n\n\n<p><strong>Conclusion:<\/strong><br>Both SF4 and NF3 are <strong>polar molecules<\/strong> due to their molecular geometries and the electronegativity differences between the atoms involved.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-116.jpeg\" alt=\"\" class=\"wp-image-250491\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Are sulfur tetrafluoride (SF4) and nitrogen trifluoride (NF3) polar or nonpolar? (Select all that apply: ) SF4 is polar; SF4 is nonpolar: NF3 is polar; NF3 is nonpolar: The Correct Answer and Explanation is: The correct answer is: Explanation: 1. Sulfur Tetrafluoride (SF4):SF4 is a polar molecule. This can be explained based on its molecular [&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-250487","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/250487","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=250487"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/250487\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=250487"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=250487"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=250487"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}