{"id":216065,"date":"2025-05-18T12:46:31","date_gmt":"2025-05-18T12:46:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=216065"},"modified":"2025-05-18T12:46:33","modified_gmt":"2025-05-18T12:46:33","slug":"draw-the-lewis-structure-of-the-hypochlorite-ion-clo%e2%88%92-which-is-used-to-clean-swimming-pools-as-its-calcium-salt","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/18\/draw-the-lewis-structure-of-the-hypochlorite-ion-clo%e2%88%92-which-is-used-to-clean-swimming-pools-as-its-calcium-salt\/","title":{"rendered":"Draw the Lewis structure of the hypochlorite ion, ClO\u2212, which is used to clean swimming pools as its calcium salt."},"content":{"rendered":"\n<p>Draw the Lewis structure of the hypochlorite ion, ClO\u2212, which is used to clean swimming pools as its calcium salt.<\/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<h3 class=\"wp-block-heading\">Lewis Structure of Hypochlorite Ion (ClO\u207b)<\/h3>\n\n\n\n<p>The correct Lewis structure for the hypochlorite ion, ClO\u207b, is:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>:Cl\u2013O:\u207b\n<\/code><\/pre>\n\n\n\n<p>Or more clearly represented with lone pairs:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>  ..\n:Cl:\u2013O:\u207b\n  ..\n<\/code><\/pre>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-Step Explanation (Approx. 300 Words)<\/h3>\n\n\n\n<p>The hypochlorite ion (ClO\u207b) consists of one chlorine (Cl) atom and one oxygen (O) atom, with an overall charge of -1. Drawing the Lewis structure requires considering the valence electrons and ensuring that the octet rule is satisfied for both atoms, where applicable.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">1. <strong>Count Total Valence Electrons<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Chlorine (Cl) has <strong>7 valence electrons<\/strong> (Group 17).<\/li>\n\n\n\n<li>Oxygen (O) also has <strong>6 valence electrons<\/strong> (Group 16).<\/li>\n\n\n\n<li>The negative charge (\u207b1) adds <strong>one extra electron<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p><strong>Total = 7 (Cl) + 6 (O) + 1 (extra electron) = 14 valence electrons<\/strong><\/p>\n\n\n\n<h4 class=\"wp-block-heading\">2. <strong>Determine the Skeleton Structure<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Place Cl and O next to each other: <strong>Cl\u2014O<\/strong><\/li>\n<\/ul>\n\n\n\n<p>We\u2019ll start with a single bond between Cl and O.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">3. <strong>Distribute Remaining Electrons<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>A single bond uses <strong>2 electrons<\/strong>, leaving <strong>12 electrons<\/strong>.<\/li>\n\n\n\n<li>Distribute these as lone pairs to complete octets:\n<ul class=\"wp-block-list\">\n<li>Give O three lone pairs (6 electrons).<\/li>\n\n\n\n<li>Give Cl three lone pairs (6 electrons).<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<p>Now each atom has 8 electrons (2 from the bond + 6 from lone pairs).<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">4. <strong>Check Formal Charges<\/strong><\/h4>\n\n\n\n<p>Formal charge = (Valence e\u207b) \u2013 (Non-bonding e\u207b) \u2013 (Bonding e\u207b \/ 2)<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen: 6 \u2013 6 \u2013 1 = <strong>-1<\/strong><\/li>\n\n\n\n<li>Chlorine: 7 \u2013 6 \u2013 1 = <strong>0<\/strong><\/li>\n<\/ul>\n\n\n\n<p>The total formal charge is <strong>\u20131<\/strong>, matching the ion\u2019s actual charge. This confirms the structure is valid.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">5. <strong>Octet Rule and Stability<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen follows the octet rule.<\/li>\n\n\n\n<li>Chlorine can expand its octet but does not need to here.<\/li>\n\n\n\n<li>The structure is stable and reflects the actual electron distribution in hypochlorite.<\/li>\n<\/ul>\n\n\n\n<p>This structure explains why hypochlorite is a good oxidizing agent: the negatively charged oxygen can donate an electron pair or participate in redox reactions, which is useful in disinfection applications like pool cleaning.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure of the hypochlorite ion, ClO\u2212, which is used to clean swimming pools as its calcium salt. The Correct Answer and Explanation is: Lewis Structure of Hypochlorite Ion (ClO\u207b) The correct Lewis structure for the hypochlorite ion, ClO\u207b, is: Or more clearly represented with lone pairs: Step-by-Step Explanation (Approx. 300 Words) The [&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-216065","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/216065","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=216065"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/216065\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=216065"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=216065"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=216065"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}