{"id":243991,"date":"2025-07-04T18:23:11","date_gmt":"2025-07-04T18:23:11","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=243991"},"modified":"2025-07-04T18:23:13","modified_gmt":"2025-07-04T18:23:13","slug":"draw-the-structure-and-predict-the-molecular-geometry-for-nh3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/04\/draw-the-structure-and-predict-the-molecular-geometry-for-nh3\/","title":{"rendered":"Draw the structure and predict the molecular geometry for NH3."},"content":{"rendered":"\n<p>Draw the structure and predict the molecular geometry for NH3. What do the geometries of these molecules have in common? How would the bond angles compare<\/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<h3 class=\"wp-block-heading\">Structure and Molecular Geometry of NH\u2083 (Ammonia)<\/h3>\n\n\n\n<p><strong>1. Lewis Structure<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Nitrogen (N) has 5 valence electrons, and each hydrogen (H) atom has 1 valence electron.<\/li>\n\n\n\n<li>In NH\u2083, nitrogen shares electrons with three hydrogen atoms, forming three N-H bonds.<\/li>\n\n\n\n<li>Nitrogen has a lone pair of electrons that occupies one of the positions in the valence shell.<\/li>\n<\/ul>\n\n\n\n<p>The Lewis structure is as follows:<\/p>\n\n\n\n<pre class=\"wp-block-preformatted\"><code>    H<br>     |<br>H - N - H<br>     |<br>    lone pair<br><\/code><\/pre>\n\n\n\n<p><strong>2. Electron Geometry<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The electron geometry around nitrogen is <strong>tetrahedral<\/strong> since nitrogen has three bonding pairs and one lone pair of electrons, making a total of four regions of electron density.<\/li>\n<\/ul>\n\n\n\n<p><strong>3. Molecular Geometry<\/strong>:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The presence of the lone pair on nitrogen alters the shape of the molecule. This results in a <strong>trigonal pyramidal<\/strong> molecular geometry.<\/li>\n\n\n\n<li>The lone pair repels the bonding pairs, causing the H-N-H bond angles to be slightly less than the ideal 109.5\u00b0 of a perfect tetrahedral structure.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Bond Angles:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>In NH\u2083, the bond angles between the hydrogen atoms (H-N-H) are approximately <strong>107\u00b0<\/strong>, which is slightly less than the ideal 109.5\u00b0 due to the lone pair occupying more space and causing increased repulsion on the bonding pairs.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Commonality in Geometries:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Both <strong>NH\u2083<\/strong> and molecules with similar structures (e.g., <strong>H\u2082O<\/strong>) have <strong>trigonal pyramidal<\/strong> geometries due to the lone pairs on the central atom.<\/li>\n\n\n\n<li>For example, <strong>H\u2082O<\/strong> has a bent molecular geometry due to two lone pairs on oxygen, while <strong>NH\u2083<\/strong> has a trigonal pyramidal geometry with one lone pair on nitrogen.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Comparison of Bond Angles:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Both <strong>NH\u2083<\/strong> and <strong>H\u2082O<\/strong> show bond angles that are <strong>less than 109.5\u00b0<\/strong> because the lone pairs cause greater electron repulsion.<\/li>\n\n\n\n<li><strong>NH\u2083<\/strong> has bond angles around 107\u00b0, while <strong>H\u2082O<\/strong> has even smaller bond angles (104.5\u00b0) because of two lone pairs.<\/li>\n<\/ul>\n\n\n\n<p>In summary, molecules like <strong>NH\u2083<\/strong> and <strong>H\u2082O<\/strong> share a common trait of having lone pairs that reduce their bond angles from the ideal tetrahedral angle of 109.5\u00b0. This results in trigonal pyramidal and bent molecular geometries, respectively.<\/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-banner5-377.jpeg\" alt=\"\" class=\"wp-image-243996\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw the structure and predict the molecular geometry for NH3. What do the geometries of these molecules have in common? How would the bond angles compare The Correct Answer and Explanation is: Structure and Molecular Geometry of NH\u2083 (Ammonia) 1. Lewis Structure: The Lewis structure is as follows: H |H &#8211; N &#8211; H | [&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-243991","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243991","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=243991"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/243991\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=243991"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=243991"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=243991"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}