A. Is XeF\u2082 polar or nonpolar?<\/strong> B. Is SOCl\u2082 polar or nonpolar?<\/strong> C. Is NOCl polar or nonpolar?<\/strong> The polarity of a molecule depends on both the polarity of its individual bonds<\/strong> and the shape of the molecule<\/strong>, which determines whether the dipole moments cancel out.<\/p>\n\n\n\n A. Xenon Difluoride (XeF\u2082)<\/strong> B. Thionyl Chloride (SOCl\u2082)<\/strong> C. Nitrosyl Chloride (NOCl)<\/strong> A. Is XeFpolar or nonpolar? B. Is SOClpolar or nonpolar? C. Is NOCl polar or nonpolar? The Correct Answer and Explanation is: A. Is XeF\u2082 polar or nonpolar?Correct Answer: Nonpolar B. Is SOCl\u2082 polar or nonpolar?Correct Answer: Polar C. Is NOCl polar or nonpolar?Correct Answer: Polar Textbook-Style Explanation The polarity of a molecule depends on […]<\/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-233700","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233700","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=233700"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233700\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=233700"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=233700"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=233700"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
Correct Answer: Nonpolar<\/strong><\/p>\n\n\n\n
Correct Answer: Polar<\/strong><\/p>\n\n\n\n
Correct Answer: Polar<\/strong><\/p>\n\n\n\n
\n\n\n\nTextbook-Style Explanation <\/h3>\n\n\n\n
\n\n\n\n
XeF\u2082 has a linear molecular geometry<\/strong>, resulting from the AX\u2082E\u2083<\/strong> electron domain configuration. Xenon has 5 electron groups (2 bonding pairs and 3 lone pairs), and the three lone pairs occupy equatorial positions to minimize repulsion. The two fluorine atoms are positioned 180\u00b0 apart. Although each Xe\u2013F bond is polar due to the high electronegativity of fluorine, the linear shape causes the bond dipoles to cancel out symmetrically.
Therefore, XeF\u2082 is a nonpolar molecule<\/strong> despite having polar bonds.<\/p>\n\n\n\n
\n\n\n\n
SOCl\u2082 has a trigonal pyramidal geometry<\/strong>. Sulfur is the central atom, bonded to one oxygen atom (via a double bond) and two chlorine atoms. It also has one lone pair. This gives it an AX\u2083E<\/strong> shape, which is asymmetrical<\/strong>. The electronegativity differences between S\u2013O and S\u2013Cl bonds, combined with the asymmetry due to the lone pair, create a net dipole moment.
Thus, SOCl\u2082 is polar.<\/strong><\/p>\n\n\n\n
\n\n\n\n
NOCl has a bent molecular shape<\/strong> around the nitrogen atom. It consists of nitrogen single bonded to chlorine and double bonded to oxygen. Due to the differing electronegativities of oxygen and chlorine and the bent shape, the dipoles do not cancel.
As a result, the molecule has a net dipole moment<\/strong>.
Therefore, NOCl is polar.<\/strong><\/p>\n\n\n\n
\n\n\n\nSummary<\/h3>\n\n\n\n
\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-307.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"