{"id":146638,"date":"2024-10-01T12:12:41","date_gmt":"2024-10-01T12:12:41","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=146638"},"modified":"2024-10-01T12:12:44","modified_gmt":"2024-10-01T12:12:44","slug":"examine-the-lewis-structure-below","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/01\/examine-the-lewis-structure-below\/","title":{"rendered":"Examine the Lewis structure below"},"content":{"rendered":"\n<p>Examine the Lewis structure below. If it is a correct structure for formaldehyde, CH,O, explain how it obeys the rules<\/p>\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<p>To examine the Lewis structure for formaldehyde (CH\u2082O), we need to verify its adherence to the rules of drawing Lewis structures, including the octet rule, formal charge calculation, and overall stability of the molecule. The correct Lewis structure for formaldehyde is as follows:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Total Valence Electrons:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has 4 valence electrons.<\/li>\n\n\n\n<li>Each Hydrogen (H) has 1 valence electron, and there are two hydrogens (2 x 1 = 2).<\/li>\n\n\n\n<li>Oxygen (O) has 6 valence electrons.<\/li>\n\n\n\n<li>Therefore, the total number of valence electrons in formaldehyde is (4 + 2 + 6 = 12).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Central Atom Selection:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon is the central atom because it can form four bonds, while oxygen can typically form two, and hydrogen can form only one bond.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Bond Formation:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon forms two single bonds with the two hydrogen atoms and one double bond with the oxygen atom. This structure can be represented as:<br>[<br>H &#8211; C = O<br>]<\/li>\n\n\n\n<li>In this arrangement, the carbon atom shares two of its electrons with each hydrogen atom (forming two single bonds) and shares two electrons with the oxygen atom (forming a double bond).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Octet Rule:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon has four bonds (eight electrons total) fulfilling the octet rule.<\/li>\n\n\n\n<li>Each hydrogen has two electrons (one bond), which satisfies their requirement (since hydrogen is stable with two electrons).<\/li>\n\n\n\n<li>Oxygen, involved in a double bond with carbon, has four electrons from the double bond and two lone pairs, achieving a total of eight electrons around it, thus obeying the octet rule.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Formal Charges:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The formal charge for each atom in this structure is calculated as:\n<ul class=\"wp-block-list\">\n<li>Carbon: (4 &#8211; (0 + \\frac{1}{2}(4)) = 0)<\/li>\n\n\n\n<li>Each Hydrogen: (1 &#8211; (0 + \\frac{1}{2}(2)) = 0)<\/li>\n\n\n\n<li>Oxygen: (6 &#8211; (4 + 0) = 2) (1 from the double bond and 4 from lone pairs)<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>The formal charge on oxygen is -1, indicating a stable structure as the charges are minimized.<\/li>\n<\/ul>\n\n\n\n<p>In conclusion, the Lewis structure of formaldehyde satisfies the requirements of valence electron count, central atom selection, bonding arrangements, octet fulfillment, and formal charge balance. Thus, it is a correct representation of CH\u2082O.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Examine the Lewis structure below. If it is a correct structure for formaldehyde, CH,O, explain how it obeys the rules The Correct Answer and Explanation is : To examine the Lewis structure for formaldehyde (CH\u2082O), we need to verify its adherence to the rules of drawing Lewis structures, including the octet rule, formal charge calculation, [&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-146638","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/146638","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=146638"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/146638\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=146638"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=146638"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=146638"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}