{"id":160147,"date":"2024-11-02T08:22:06","date_gmt":"2024-11-02T08:22:06","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=160147"},"modified":"2024-11-02T08:22:09","modified_gmt":"2024-11-02T08:22:09","slug":"even-though-the-following-molecules-contain-polar-bonds-the-only-polar-molecule-is","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/02\/even-though-the-following-molecules-contain-polar-bonds-the-only-polar-molecule-is\/","title":{"rendered":"Even though the following molecules contain polar bonds, the only polar molecule is"},"content":{"rendered":"\n<p>Even though the following molecules contain polar bonds, the only polar molecule is:<br>A. CCl4 <\/p>\n\n\n\n<p>B. CO2 <\/p>\n\n\n\n<p>C. NH3 <\/p>\n\n\n\n<p>D. CH4<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The correct answer is <strong>C. NH3 (ammonia)<\/strong>.<\/p>\n\n\n\n<p>To understand why NH3 is the only polar molecule among the given options, it is important to consider both the polarity of individual bonds and the overall molecular geometry.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Polar Bonds<\/strong>: A polar bond occurs when there is a significant difference in electronegativity between the atoms involved, causing a distribution of charge. For instance, in NH3, the nitrogen atom is more electronegative than the hydrogen atoms, resulting in polar N-H bonds.<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: The shape of a molecule significantly affects its polarity. NH3 has a trigonal pyramidal shape due to the presence of a lone pair of electrons on the nitrogen atom. This geometry prevents the bond dipoles from cancelling each other out, leading to a net dipole moment that makes the entire molecule polar.<\/li>\n\n\n\n<li><strong>Other Options<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>A. CCl4 (carbon tetrachloride)<\/strong>: Although C-Cl bonds are polar, CCl4 has a tetrahedral geometry. The symmetry of the molecule allows the dipole moments of the polar bonds to cancel each other out, resulting in a nonpolar molecule.<\/li>\n\n\n\n<li><strong>B. CO2 (carbon dioxide)<\/strong>: CO2 has polar C=O bonds, but its linear geometry allows the bond dipoles to cancel out, making the molecule nonpolar.<\/li>\n\n\n\n<li><strong>D. CH4 (methane)<\/strong>: In CH4, the C-H bonds are slightly polar; however, the symmetrical tetrahedral shape results in the cancellation of bond dipoles, rendering the molecule nonpolar as well.<\/li>\n<\/ul>\n\n\n\n<p>In summary, while CCl4, CO2, and CH4 contain polar bonds, their symmetrical geometries lead to an overall nonpolar character. In contrast, NH3, with its trigonal pyramidal structure and unbalanced dipole moments, is a polar molecule. This polarity affects its properties, such as higher boiling points and solubility in water, which are characteristic of polar substances.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Even though the following molecules contain polar bonds, the only polar molecule is:A. CCl4 B. CO2 C. NH3 D. CH4 The Correct Answer and Explanation is: The correct answer is C. NH3 (ammonia). To understand why NH3 is the only polar molecule among the given options, it is important to consider both the polarity 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-160147","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/160147","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=160147"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/160147\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=160147"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=160147"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=160147"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}