Why is NH3 classified as a polar molecule<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n Answer:<\/strong> NH\u2083 (Ammonia) is classified as a polar molecule because of its molecular shape and the distribution of electrons.<\/p>\n\n\n\n Ammonia (NH\u2083) is a polar molecule due to two key factors: its molecular geometry and the electronegativity difference between nitrogen and hydrogen.<\/p>\n\n\n\n In conclusion, NH\u2083’s polar nature arises from its asymmetrical shape and the difference in electronegativity between nitrogen and hydrogen, leading to a molecule with a net dipole moment.<\/p>\n","protected":false},"excerpt":{"rendered":" Why is NH3 classified as a polar molecule The Correct Answer and Explanation is: Answer: NH\u2083 (Ammonia) is classified as a polar molecule because of its molecular shape and the distribution of electrons. Explanation: Ammonia (NH\u2083) is a polar molecule due to two key factors: its molecular geometry and the electronegativity difference between nitrogen and […]<\/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-167979","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167979","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=167979"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167979\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=167979"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=167979"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=167979"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Explanation:<\/h3>\n\n\n\n
\n
Ammonia has a trigonal pyramidal shape, which is a result of the lone pair of electrons on the nitrogen atom. In this structure, the nitrogen atom is at the center, with three hydrogen atoms bonded to it. The nitrogen atom has a lone pair of electrons that repels the bonding pairs, causing the molecule to adopt a pyramidal shape rather than a flat, symmetrical arrangement. This asymmetry in the shape prevents the individual bond dipoles from canceling each other out, resulting in an overall dipole moment for the entire molecule.<\/li>\n\n\n\n
Nitrogen (N) is more electronegative than hydrogen (H), meaning it attracts the shared electrons in the N-H bonds more strongly. The electronegativity of nitrogen is 3.04, while that of hydrogen is 2.20. This creates a partial negative charge on the nitrogen atom and a partial positive charge on the hydrogen atoms. Because the molecule is not symmetrical (due to the lone pair on nitrogen), these individual dipoles do not cancel each other out, resulting in a net dipole moment pointing from the hydrogen atoms toward the nitrogen atom.<\/li>\n\n\n\n
The combination of the trigonal pyramidal shape and the electronegativity difference leads to an overall dipole moment. The molecule has a positive pole near the hydrogen atoms and a negative pole near the nitrogen atom, making NH\u2083 a polar molecule.<\/li>\n<\/ol>\n\n\n\n