{"id":184131,"date":"2025-01-19T10:34:45","date_gmt":"2025-01-19T10:34:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=184131"},"modified":"2025-01-19T10:34:46","modified_gmt":"2025-01-19T10:34:46","slug":"below-is-the-lewis-structure-of-the-hydrogen-cyanide-hcn-molecule","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/19\/below-is-the-lewis-structure-of-the-hydrogen-cyanide-hcn-molecule\/","title":{"rendered":"Below is the Lewis structure of the hydrogen cyanide (HCN) molecule"},"content":{"rendered":"\n<p>Below is the Lewis structure of the hydrogen cyanide (HCN) molecule. H:C:: N: Count the number of bonding pairs and the number of lone pairs around the carbon atom in this molecule. bonding pairs: lone pairs: None<\/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<h3 class=\"wp-block-heading\">Correct Answer:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Bonding pairs around the carbon atom<\/strong>: 4<\/li>\n\n\n\n<li><strong>Lone pairs around the carbon atom<\/strong>: 0<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The Lewis structure for hydrogen cyanide (<strong>HCN<\/strong>) is written as:<\/p>\n\n\n\n<p><strong>H : C \u2261 N :<\/strong><\/p>\n\n\n\n<p>Here\u2019s how the structure and pair counts are determined:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Bonding pairs<\/strong>:\n<ul class=\"wp-block-list\">\n<li>Carbon forms a <strong>single bond<\/strong> with hydrogen (H).<\/li>\n\n\n\n<li>Carbon forms a <strong>triple bond<\/strong> with nitrogen (N).<\/li>\n\n\n\n<li>A single bond corresponds to <strong>1 bonding pair<\/strong> (2 electrons), and a triple bond corresponds to <strong>3 bonding pairs<\/strong> (6 electrons).<\/li>\n\n\n\n<li>Total bonding pairs around the carbon atom = <strong>1 (from H-C) + 3 (from C\u2261N) = 4 bonding pairs.<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Lone pairs<\/strong>:\n<ul class=\"wp-block-list\">\n<li>Carbon contributes 4 valence electrons, and all 4 are involved in bonding. Therefore, there are <strong>no lone pairs<\/strong> on the carbon atom.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Context for the molecule<\/strong>:\n<ul class=\"wp-block-list\">\n<li>Hydrogen has 1 valence electron, and it forms a single bond with carbon, satisfying its octet.<\/li>\n\n\n\n<li>Nitrogen has 5 valence electrons, and in this structure:\n<ul class=\"wp-block-list\">\n<li>It forms a triple bond with carbon (uses 3 electrons for bonding).<\/li>\n\n\n\n<li>It has 1 lone pair of electrons left (2 non-bonded electrons).<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>The overall structure satisfies the octet rule for all atoms.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Why the carbon has no lone pairs<\/strong>:\n<ul class=\"wp-block-list\">\n<li>Carbon has exactly 4 valence electrons. It achieves a stable configuration by sharing these electrons through bonding (1 with hydrogen and 3 with nitrogen). Since all its valence electrons are used in bonds, no lone pairs remain on the carbon atom.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<p>Thus, carbon in HCN has <strong>4 bonding pairs<\/strong> and <strong>0 lone pairs<\/strong>, making it a linear molecule.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Below is the Lewis structure of the hydrogen cyanide (HCN) molecule. H:C:: N: Count the number of bonding pairs and the number of lone pairs around the carbon atom in this molecule. bonding pairs: lone pairs: None The correct answer and explanation is: Correct Answer: Explanation: The Lewis structure for hydrogen cyanide (HCN) is written [&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-184131","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184131","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=184131"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184131\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184131"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184131"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184131"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}