{"id":230144,"date":"2025-06-09T03:44:01","date_gmt":"2025-06-09T03:44:01","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=230144"},"modified":"2025-06-09T03:44:03","modified_gmt":"2025-06-09T03:44:03","slug":"draw-the-best-lewis-structure-for-cl3a%c2%81-and-determine-the-formal-charge-on-all-3-cl-atoms","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/09\/draw-the-best-lewis-structure-for-cl3a%c2%81-and-determine-the-formal-charge-on-all-3-cl-atoms\/","title":{"rendered":"Draw the best Lewis structure for Cl3\u00e2\u0081\u00bb and determine the formal charge on all 3 Cl atoms."},"content":{"rendered":"\n<p>Draw the best Lewis structure for Cl3\u00e2\u0081\u00bb and determine the formal charge on all 3 Cl atoms.<\/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<h6 class=\"wp-block-heading\">ChatGPT said:<\/h6>\n\n\n\n<h3 class=\"wp-block-heading\">Lewis Structure for Cl\u2083\u207b (Trichloride Anion)<\/h3>\n\n\n\n<p>The best Lewis structure for the trichloride anion (Cl\u2083\u207b) is:<\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">rubyCopyEdit<code>     :Cl:\n      |\n:Cl\u2013Cl:\n      |\n     :Cl:\n<\/code><\/pre>\n\n\n\n<p>But more precisely and clearly (with lone pairs):<\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">rubyCopyEdit<code>   ..\n:Cl:\u2013Cl:\u2013:Cl:\n   ..  ..  ..\n<\/code><\/pre>\n\n\n\n<p>Each outer Cl atom has 3 lone pairs, and the central Cl has 3 lone pairs plus single bonds to each of the two terminal Cl atoms. The negative charge is delocalized over the structure, often represented as a formal charge on the central atom.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-Step Explanation<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Count Total Valence Electrons:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Each Cl atom has 7 valence electrons.<\/li>\n\n\n\n<li>There are 3 Cl atoms \u2192 3 \u00d7 7 = 21 electrons.<\/li>\n\n\n\n<li>Plus 1 extra electron due to the negative charge \u2192 <strong>22 valence electrons total<\/strong>.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Skeleton Structure:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Place one Cl atom in the center bonded to two others: Cl\u2013Cl\u2013Cl.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Assign Electrons:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Form single bonds between atoms (2 bonds \u00d7 2 e\u207b = 4 e\u207b).<\/li>\n\n\n\n<li>Distribute remaining 18 electrons to satisfy octets on terminal atoms first.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Lone Pairs:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Each outer Cl needs 6 more electrons (3 lone pairs) to complete the octet.<\/li>\n\n\n\n<li>That uses 12 electrons (6 for each terminal Cl).<\/li>\n\n\n\n<li>Remaining 6 electrons go to the central Cl as 3 lone pairs.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Formal Charges:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Formal charge = Valence \u2013 (Lone pairs + \u00bd Bonding)\n<ul class=\"wp-block-list\">\n<li><strong>Terminal Cl atoms<\/strong>: 7 \u2013 (6 + 1) = 0<\/li>\n\n\n\n<li><strong>Central Cl atom<\/strong>: 7 \u2013 (6 + 1) = 0<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li>But we have an extra electron (22 total), so the <strong>negative charge<\/strong> is distributed as a <strong>formal charge of \u20131 on the central Cl<\/strong>.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Final Formal Charges:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Central Cl<\/strong>: \u20131<\/li>\n\n\n\n<li><strong>Each terminal Cl<\/strong>: 0<\/li>\n<\/ul>\n\n\n\n<p>This structure satisfies the octet rule and reflects the delocalization of the extra electron over the central atom. Cl\u2083\u207b is also known to be linear in geometry and exists in some salts like CsCl\u2083.<\/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-banner9-200.jpeg\" alt=\"\" class=\"wp-image-230145\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw the best Lewis structure for Cl3\u00e2\u0081\u00bb and determine the formal charge on all 3 Cl atoms. The Correct Answer and Explanation is: ChatGPT said: Lewis Structure for Cl\u2083\u207b (Trichloride Anion) The best Lewis structure for the trichloride anion (Cl\u2083\u207b) is: rubyCopyEdit :Cl: | :Cl\u2013Cl: | :Cl: But more precisely and clearly (with lone pairs): [&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-230144","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230144","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=230144"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230144\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=230144"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=230144"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=230144"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}