{"id":225293,"date":"2025-06-04T06:37:38","date_gmt":"2025-06-04T06:37:38","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=225293"},"modified":"2025-06-04T06:37:40","modified_gmt":"2025-06-04T06:37:40","slug":"the-most-reasonable-lewis-structure-for-hocl-is-select-one-h-c-h-o-cl-h-o-ct-h-o-ci","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/04\/the-most-reasonable-lewis-structure-for-hocl-is-select-one-h-c-h-o-cl-h-o-ct-h-o-ci\/","title":{"rendered":"The most reasonable Lewis structure for HOCl is Select one: H: C: %: H: o: Cl: H: o: :Ct: H: O: : CI:"},"content":{"rendered":"\n<p>The most reasonable Lewis structure for HOCl is Select one: H: C: %: H: o: Cl: H: o: :Ct: H: O: : CI:<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The most reasonable Lewis structure for <strong>HOCl (hypochlorous acid)<\/strong> is:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>H\u2013O\u2013Cl\n<\/code><\/pre>\n\n\n\n<p>Or, in Lewis structure format with lone pairs:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>H\u2013O\u2013Cl\n   ..\n   ..\n   ..\n<\/code><\/pre>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Hydrogen (H)<\/strong> forms a single bond with <strong>oxygen (O)<\/strong>.<\/li>\n\n\n\n<li><strong>Oxygen (O)<\/strong> forms a single bond with <strong>chlorine (Cl)<\/strong>.<\/li>\n\n\n\n<li>Oxygen has two lone pairs of electrons, and chlorine has three lone pairs.<\/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\">Explanation <\/h3>\n\n\n\n<p>The Lewis structure is a way to represent the bonding between atoms and the lone pairs of electrons in a molecule. For <strong>HOCl<\/strong>, we analyze each atom:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Hydrogen (H)<\/strong> has <strong>1 valence electron<\/strong> and can form only <strong>1 bond<\/strong>. It bonds to oxygen.<\/li>\n\n\n\n<li><strong>Oxygen (O)<\/strong> has <strong>6 valence electrons<\/strong>. It typically forms <strong>2 bonds<\/strong> and has <strong>2 lone pairs<\/strong>.<\/li>\n\n\n\n<li><strong>Chlorine (Cl)<\/strong> has <strong>7 valence electrons<\/strong>. It typically forms <strong>1 bond<\/strong> and has <strong>3 lone pairs<\/strong>.<\/li>\n<\/ol>\n\n\n\n<p>We start by connecting the atoms. Since hydrogen can only make one bond, and oxygen usually bonds to both hydrogen and chlorine, the backbone is <strong>H\u2013O\u2013Cl<\/strong>.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The <strong>H\u2013O<\/strong> bond uses 2 electrons (1 from H, 1 from O).<\/li>\n\n\n\n<li>The <strong>O\u2013Cl<\/strong> bond also uses 2 electrons (1 from each atom).<\/li>\n\n\n\n<li>This accounts for 4 bonding electrons (2 bonds).<\/li>\n\n\n\n<li>The oxygen still needs 4 more electrons (2 lone pairs) to complete its octet.<\/li>\n\n\n\n<li>Chlorine needs 6 more electrons (3 lone pairs) to reach its octet.<\/li>\n<\/ul>\n\n\n\n<p>The total number of valence electrons is:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>H: 1<\/li>\n\n\n\n<li>O: 6<\/li>\n\n\n\n<li>Cl: 7<br><strong>Total = 14 electrons<\/strong><\/li>\n<\/ul>\n\n\n\n<p>We\u2019ve used:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>4 electrons in bonds (2 bonds)<\/li>\n\n\n\n<li>4 electrons on oxygen (2 lone pairs)<\/li>\n\n\n\n<li>6 electrons on chlorine (3 lone pairs)<br><strong>Total = 14 electrons<\/strong>, which matches.<\/li>\n<\/ul>\n\n\n\n<p>This structure is the most reasonable because:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>All atoms follow the octet rule (except hydrogen, which follows the duet rule).<\/li>\n\n\n\n<li>The formal charges on all atoms are zero.<\/li>\n\n\n\n<li>Oxygen is the central atom bonded to both hydrogen and chlorine, which reflects oxygen&#8217;s higher electronegativity compared to chlorine.<\/li>\n<\/ul>\n\n\n\n<p>Therefore, the correct Lewis structure for HOCl is <strong>H\u2013O\u2013Cl<\/strong>, with lone pairs shown on oxygen and chlorine<\/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-banner4-293.jpeg\" alt=\"\" class=\"wp-image-225294\"\/><\/figure>\n\n\n\n<p>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>The most reasonable Lewis structure for HOCl is Select one: H: C: %: H: o: Cl: H: o: :Ct: H: O: : CI: The Correct Answer and Explanation is: The most reasonable Lewis structure for HOCl (hypochlorous acid) is: Or, in Lewis structure format with lone pairs: Explanation The Lewis structure is a way to [&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 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