{"id":39975,"date":"2025-06-27T11:59:15","date_gmt":"2025-06-27T11:59:15","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=39975"},"modified":"2025-06-27T11:59:16","modified_gmt":"2025-06-27T11:59:16","slug":"draw-a-reasonable-lewis-structure-for-each-of-the-following-formulas","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/draw-a-reasonable-lewis-structure-for-each-of-the-following-formulas\/","title":{"rendered":"Draw a reasonable Lewis structure for each of the following formulas"},"content":{"rendered":"\n<p>Draw a reasonable Lewis structure for each of the following formulas. a. H2S b. CHBr3 c. NF3 d. Br2O e. H2CO3 f. H2S2 g. HOCl h. BBr3 i. CH3CH2CHCH2<\/p>\n\n\n\n<p>Here are the reasonable Lewis structures for each given molecular formula, followed by an explanation.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>a. H\u2082S (Hydrogen sulfide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sulfur is the central atom with two single bonds to hydrogen atoms.<\/li>\n\n\n\n<li>Sulfur has two lone pairs.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>H\u2013S\u2013H (with two lone pairs on S)<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>b. CHBr\u2083 (Bromoform)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon is central, bonded to one hydrogen and three bromine atoms.<\/li>\n\n\n\n<li>Carbon has four single bonds; bromines have three lone pairs each.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>H\u2013C\u2013Br\u2083 (tetrahedral geometry)<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>c. NF\u2083 (Nitrogen trifluoride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Nitrogen is central, bonded to three fluorine atoms with one lone pair.<\/li>\n\n\n\n<li>Each fluorine has three lone pairs.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>F\u2013N\u2013F with a lone pair on N and three lone pairs on each F<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>d. Br\u2082O (Dibromine monoxide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen is central, bonded to two bromine atoms with two lone pairs.<\/li>\n\n\n\n<li>Each bromine has three lone pairs.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>Br\u2013O\u2013Br<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>e. H\u2082CO\u2083 (Carbonic acid)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon is central with one double bond to oxygen and two single bonds to OH groups.<\/li>\n\n\n\n<li>Each O has two lone pairs.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>HO\u2013C(=O)\u2013OH<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>f. H\u2082S\u2082 (Disulfane)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Two sulfur atoms bonded together.<\/li>\n\n\n\n<li>Each sulfur also bonds to a hydrogen and has two lone pairs.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>H\u2013S\u2013S\u2013H<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>g. HOCl (Hypochlorous acid)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen is central, bonded to hydrogen and chlorine.<\/li>\n\n\n\n<li>Oxygen has two lone pairs; chlorine has three.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>H\u2013O\u2013Cl<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>h. BBr\u2083 (Boron tribromide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Boron is central, bonded to three bromine atoms.<\/li>\n\n\n\n<li>Boron has no lone pairs; each Br has three.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>Br\u2013B\u2013Br (trigonal planar)<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>i. CH\u2083CH\u2082CHCH\u2082 (1-butene)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>A four-carbon chain with a double bond between the third and fourth carbons.<\/li>\n\n\n\n<li>Hydrogen atoms fill in to satisfy valence.<\/li>\n<\/ul>\n\n\n\n<p><strong>Structure:<\/strong><br>CH\u2083\u2013CH\u2082\u2013CH=CH\u2082<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>Explanation:<\/strong><br>Lewis structures show how valence electrons are arranged among atoms in a molecule. They help predict geometry, reactivity, and polarity. In each of the molecules above, the central atom is usually the least electronegative (except hydrogen, which can never be central).<\/p>\n\n\n\n<p>For example, in <strong>H\u2082S<\/strong>, sulfur forms two single bonds with hydrogen and keeps two lone pairs, following the octet rule. In <strong>CHBr\u2083<\/strong>, carbon has four bonds forming a tetrahedral structure, with bromines completing octets with lone pairs.<\/p>\n\n\n\n<p><strong>NF\u2083<\/strong> resembles ammonia (NH\u2083) but with fluorines. Nitrogen forms three bonds and retains one lone pair. Fluorine, being highly electronegative, doesn&#8217;t form more than one bond and completes its octet with lone pairs.<\/p>\n\n\n\n<p>In <strong>Br\u2082O<\/strong>, oxygen is more electronegative and central, forming two single bonds with bromine. <strong>H\u2082CO\u2083<\/strong>, an acid, has a central carbon double-bonded to one oxygen and single-bonded to two hydroxyl groups.<\/p>\n\n\n\n<p><strong>H\u2082S\u2082<\/strong> is similar in bonding to hydrogen peroxide, with a sulfur\u2013sulfur single bond and each sulfur also bonded to a hydrogen. Lone pairs on sulfur affect molecular shape and reactivity.<\/p>\n\n\n\n<p><strong>HOCl<\/strong> is a small molecule where oxygen bonds to hydrogen and chlorine. <strong>BBr\u2083<\/strong> is an electron-deficient compound where boron forms three bonds without achieving a full octet, making it a strong Lewis acid.<\/p>\n\n\n\n<p>Lastly, <strong>1-butene (CH\u2083CH\u2082CHCH\u2082)<\/strong> contains a carbon\u2013carbon double bond, creating a region of high electron density and affecting the geometry with sp\u00b2 hybridization around the double bond.<\/p>\n\n\n\n<p>These Lewis structures follow valence rules and help in understanding chemical behavior.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"852\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1203.jpeg\" alt=\"\" class=\"wp-image-39987\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1203.jpeg 852w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1203-250x300.jpeg 250w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-1203-768x923.jpeg 768w\" sizes=\"auto, (max-width: 852px) 100vw, 852px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw a reasonable Lewis structure for each of the following formulas. a. H2S b. CHBr3 c. NF3 d. Br2O e. H2CO3 f. H2S2 g. HOCl h. BBr3 i. CH3CH2CHCH2 Here are the reasonable Lewis structures for each given molecular formula, followed by an explanation. a. H\u2082S (Hydrogen sulfide) Structure:H\u2013S\u2013H (with two lone pairs on S) [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-39975","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39975","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=39975"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39975\/revisions"}],"predecessor-version":[{"id":39991,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/39975\/revisions\/39991"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=39975"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=39975"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=39975"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}