{"id":196105,"date":"2025-03-02T10:02:43","date_gmt":"2025-03-02T10:02:43","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=196105"},"modified":"2025-03-02T10:02:46","modified_gmt":"2025-03-02T10:02:46","slug":"the-lewis-structure-for-alanine-is-shown-below","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/02\/the-lewis-structure-for-alanine-is-shown-below\/","title":{"rendered":"The Lewis structure for alanine is shown below"},"content":{"rendered":"\n<p>The Lewis structure for alanine is shown below. H 1 H H C 4 H 30 2 :0: ?. N H ?. a. What is the formal charge on the nitrogen atom? What are the formal charges on each of the oxygens, labeled 1 and 2 in red? b. What are the molecular geometries around the carbon atoms labeled 3 and 4?<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-92.png\" alt=\"\" class=\"wp-image-196106\"\/><\/figure>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/03\/image-93.png\" alt=\"\" class=\"wp-image-196107\"\/><\/figure>\n\n\n\n<p>Alanine is an \u03b1-amino acid that serves as a building block for proteins. Its structure consists of a central carbon atom bonded to an amino group (-NH\u2082), a carboxyl group (-COOH), a hydrogen atom, and a methyl group (-CH\u2083).\ue206<\/p>\n\n\n\n<p><strong>a. Formal Charges:<\/strong><\/p>\n\n\n\n<p>To determine the formal charges on the nitrogen and oxygen atoms, we apply the formal charge formula:<\/p>\n\n\n\n<p><strong>Formal Charge (FC) = Valence Electrons (VE) \u2013 Non-bonding Electrons (NBE) \u2013 (Bonding Electrons (BE) \/ 2)<\/strong>\ue206<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Nitrogen Atom:<\/strong><\/li>\n\n\n\n<li>Valence Electrons (VE): Nitrogen is in Group 15 of the periodic table, so it has 5 valence electrons.\ue206<\/li>\n\n\n\n<li>Non-bonding Electrons (NBE): Nitrogen has one lone pair, contributing 2 non-bonding electrons.\ue206<\/li>\n\n\n\n<li>Bonding Electrons (BE): Nitrogen forms three single bonds (one with hydrogen and two with carbon), contributing 6 bonding electrons.\ue206<\/li>\n\n\n\n<li>Applying the formula: FC = 5 \u2013 2 \u2013 (6 \/ 2) = 5 \u2013 2 \u2013 3 = 0\ue206 Therefore, the formal charge on the nitrogen atom is <strong>0<\/strong>.\ue206<\/li>\n\n\n\n<li><strong>Oxygen Atoms:<\/strong><\/li>\n\n\n\n<li><strong>Oxygen 1 (part of the carboxyl group):<\/strong><ul><li>Valence Electrons (VE): Oxygen has 6 valence electrons.<\/li><li>Non-bonding Electrons (NBE): Oxygen has two lone pairs, contributing 4 non-bonding electrons.<\/li><li>Bonding Electrons (BE): Oxygen forms one double bond with carbon, contributing 4 bonding electrons.<\/li><li>Applying the formula: FC = 6 \u2013 4 \u2013 (4 \/ 2) = 6 \u2013 4 \u2013 2 = 0<\/li><\/ul>Thus, the formal charge on oxygen 1 is <strong>0<\/strong>.<\/li>\n\n\n\n<li><strong>Oxygen 2 (part of the carboxyl group):<\/strong><ul><li>Valence Electrons (VE): 6 valence electrons.<\/li><li>Non-bonding Electrons (NBE): Three lone pairs, contributing 6 non-bonding electrons.<\/li><li>Bonding Electrons (BE): Oxygen forms one single bond with carbon, contributing 2 bonding electrons.<\/li><li>Applying the formula: FC = 6 \u2013 6 \u2013 (2 \/ 2) = 6 \u2013 6 \u2013 1 = \u20131<\/li><\/ul>Therefore, the formal charge on oxygen 2 is <strong>\u20131<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p><strong>b. Molecular Geometries:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Carbon Atom 3 (\u03b1-carbon):<\/strong><\/li>\n\n\n\n<li>This carbon is bonded to an amino group (-NH\u2082), a carboxyl group (-COOH), a hydrogen atom, and a methyl group (-CH\u2083).\ue206<\/li>\n\n\n\n<li>It has four substituents arranged tetrahedrally around it.\ue206<\/li>\n\n\n\n<li><strong>Electron Geometry:<\/strong> Tetrahedral\ue206<\/li>\n\n\n\n<li><strong>Molecular Geometry:<\/strong> Tetrahedral\ue206<\/li>\n\n\n\n<li><strong>Carbon Atom 4 (carboxyl carbon):<\/strong><\/li>\n\n\n\n<li>This carbon is double-bonded to oxygen 1 and single-bonded to oxygen 2.\ue206<\/li>\n\n\n\n<li>It has three substituents arranged trigonal planar around it.\ue206<\/li>\n\n\n\n<li><strong>Electron Geometry:<\/strong> Trigonal Planar\ue206<\/li>\n\n\n\n<li><strong>Molecular Geometry:<\/strong> Trigonal Planar\ue206<\/li>\n<\/ul>\n\n\n\n<p>These geometries arise from the sp\u00b3 hybridization of carbon 3, leading to a tetrahedral arrangement, and the sp\u00b2 hybridization of carbon 4, leading to a trigonal planar arrangement.\ue206<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The Lewis structure for alanine is shown below. H 1 H H C 4 H 30 2 :0: ?. N H ?. a. What is the formal charge on the nitrogen atom? What are the formal charges on each of the oxygens, labeled 1 and 2 in red? b. What are the molecular geometries around [&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-196105","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196105","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=196105"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196105\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=196105"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=196105"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=196105"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}