{"id":227939,"date":"2025-06-06T15:34:05","date_gmt":"2025-06-06T15:34:05","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=227939"},"modified":"2025-06-06T15:34:07","modified_gmt":"2025-06-06T15:34:07","slug":"draw-the-lewis-dot-structures-for-each-of-the-following-molecules-h2s-ch2br2-hcn-so3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/06\/draw-the-lewis-dot-structures-for-each-of-the-following-molecules-h2s-ch2br2-hcn-so3\/","title":{"rendered":"Draw the Lewis dot structures for each of the following molecules: H2S, CH2Br2, HCN, SO3."},"content":{"rendered":"\n<p>Draw the Lewis dot structures for each of the following molecules: H2S, CH2Br2, HCN, SO3.<\/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\"><strong>Lewis Dot Structures<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>H\u2082S (Hydrogen sulfide):<\/strong><\/li>\n<\/ol>\n\n\n\n<pre class=\"wp-block-preformatted\">markdownCopyEdit<code>   H \u2013 S \u2013 H\n       ..\n<\/code><\/pre>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sulfur (S) has 6 valence electrons and forms two single bonds with hydrogen (H), which each contribute 1 electron.<\/li>\n\n\n\n<li>Two lone pairs remain on sulfur to complete its octet.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<ol start=\"2\" class=\"wp-block-list\">\n<li><strong>CH\u2082Br\u2082 (Dibromomethane):<\/strong><\/li>\n<\/ol>\n\n\n\n<pre class=\"wp-block-preformatted\">markdownCopyEdit<code>     H\n     |\nH \u2013 C \u2013 Br\n     |\n    Br\n<\/code><\/pre>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) has 4 valence electrons and forms 4 single bonds: 2 with hydrogen atoms and 2 with bromine atoms.<\/li>\n\n\n\n<li>Each bromine (Br) has 7 valence electrons and shares one electron with carbon, keeping three lone pairs.<\/li>\n\n\n\n<li>Carbon completes its octet via four sigma bonds.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<ol start=\"3\" class=\"wp-block-list\">\n<li><strong>HCN (Hydrogen cyanide):<\/strong><\/li>\n<\/ol>\n\n\n\n<pre class=\"wp-block-preformatted\">mathematicaCopyEdit<code>H \u2013 C \u2261 N:\n<\/code><\/pre>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Hydrogen (H) forms a single bond with carbon (C).<\/li>\n\n\n\n<li>Carbon forms a triple bond with nitrogen (N).<\/li>\n\n\n\n<li>Nitrogen has one lone pair.<\/li>\n\n\n\n<li>This satisfies the octet rule for both C and N.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<ol start=\"4\" class=\"wp-block-list\">\n<li><strong>SO\u2083 (Sulfur trioxide):<\/strong><\/li>\n<\/ol>\n\n\n\n<p><strong>Resonance structures:<\/strong><\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">mathematicaCopyEdit<code>O=S(\u2013O)\u2082   (One double bond and two single bonds with formal charges)\n\nor more accurately:\n\n       O\n       ||\n   O = S = O\n<\/code><\/pre>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The actual structure is a <strong>resonance hybrid<\/strong> of three forms where the double bond is delocalized over the three oxygen atoms.<\/li>\n\n\n\n<li>Sulfur can exceed the octet rule (it&#8217;s in Period 3), allowing expanded valence shells.<\/li>\n\n\n\n<li>Each oxygen with a single bond carries a negative formal charge; sulfur carries a partial positive.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation <\/strong><\/h3>\n\n\n\n<p>Lewis dot structures represent the valence electrons of atoms within a molecule. These structures are essential in understanding molecular shape, bonding, and reactivity. The goal of drawing these is to ensure atoms (especially main group elements) achieve a full valence shell\u2014typically 8 electrons (the octet rule).<\/p>\n\n\n\n<p>In <strong>H\u2082S<\/strong>, sulfur (group 16) has six valence electrons and forms two single bonds with hydrogen, using two electrons. The remaining four electrons stay as two lone pairs. Hydrogen, needing only two electrons, completes its duet with one bond.<\/p>\n\n\n\n<p><strong>CH\u2082Br\u2082<\/strong> has a central carbon (group 14), which forms four single bonds: two with hydrogen and two with bromine. Bromine (group 17) forms one bond each and retains three lone pairs to complete their octets. Carbon&#8217;s four bonds fulfill its octet.<\/p>\n\n\n\n<p><strong>HCN<\/strong> is a linear molecule. Carbon is the central atom, forming a triple bond with nitrogen (which has five valence electrons) and a single bond with hydrogen. The triple bond ensures both carbon and nitrogen have full octets. Nitrogen also retains a lone pair.<\/p>\n\n\n\n<p><strong>SO\u2083<\/strong> is more complex due to <strong>resonance<\/strong> and <strong>expanded octet<\/strong>. Sulfur can have more than eight electrons because it is in period 3. The molecule has three resonance structures with one double bond and two single bonds rotating among the three oxygen atoms. The true structure is a resonance hybrid where the double bond character is delocalized, stabilizing the molecule.<\/p>\n\n\n\n<p>Understanding these Lewis structures helps predict molecular geometry, polarity, and reactivity\u2014key concepts in chemistry.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner4-549.jpeg\" alt=\"\" class=\"wp-image-227940\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis dot structures for each of the following molecules: H2S, CH2Br2, HCN, SO3. The Correct Answer and Explanation is: Lewis Dot Structures markdownCopyEdit H \u2013 S \u2013 H .. markdownCopyEdit H | H \u2013 C \u2013 Br | Br mathematicaCopyEditH \u2013 C \u2261 N: Resonance structures: mathematicaCopyEditO=S(\u2013O)\u2082 (One double bond and two single [&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-227939","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227939","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=227939"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/227939\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=227939"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=227939"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=227939"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}