{"id":221270,"date":"2025-05-29T11:11:47","date_gmt":"2025-05-29T11:11:47","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=221270"},"modified":"2025-05-29T11:11:49","modified_gmt":"2025-05-29T11:11:49","slug":"describe-the-lewis-structure-for-the-ionic-compound-calcium-chloride-cacl2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/29\/describe-the-lewis-structure-for-the-ionic-compound-calcium-chloride-cacl2\/","title":{"rendered":"Describe the Lewis structure for the ionic compound calcium chloride, CaCl2."},"content":{"rendered":"\n<p>Describe the Lewis structure for the ionic compound calcium chloride, CaCl2.<\/p>\n\n\n\n<p>The structure would include a Cl with 7 dots a 1- charge but with no square brackets. The structure would include a Cl with 8 dots in square brackets with a 2+ charge. The structure would include a Ca with no dots a 2+ charge but with no square brackets. The structure would include a Ca with no dots in square brackets with a 2+ charge.<\/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\">Lewis Structure for Calcium Chloride (CaCl\u2082)<\/h3>\n\n\n\n<p>The correct Lewis structure for <strong>CaCl\u2082<\/strong>, an <strong>ionic compound<\/strong>, shows the <strong>transfer<\/strong> of electrons from the metal (calcium) to the non-metal (chlorine):<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Ca:<\/strong> Calcium atom has <strong>2 valence electrons<\/strong>. It <strong>loses both electrons<\/strong> to become <strong>Ca\u00b2\u207a<\/strong>, a cation with no dots (no valence electrons left). Since it is an ion, we show it as:<br><strong>[Ca]\u00b2\u207a<\/strong> (in square brackets with 2+ charge and no dots)<\/li>\n\n\n\n<li><strong>Cl:<\/strong> Each chlorine atom has <strong>7 valence electrons<\/strong>. It <strong>gains 1 electron<\/strong> to complete its octet, becoming <strong>Cl\u207b<\/strong> with <strong>8 electrons (dots)<\/strong> around it. Since it\u2019s an ion, it should be written in <strong>square brackets<\/strong> with the charge:<br><strong>[Cl\u207b]<\/strong> (in square brackets with 8 dots and 1\u2013 charge)<\/li>\n<\/ul>\n\n\n\n<p>So, the correct Lewis structure for CaCl\u2082 would be:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>&#91;Ca]\u00b2\u207a  &#91;Cl]\u207b   &#91;Cl]\u207b\n        :Cl:     :Cl:\n      ..    ..  ..    ..\n<\/code><\/pre>\n\n\n\n<p>Each Cl\u207b has a <strong>full octet (8 dots)<\/strong> around it in square brackets with a <strong>\u20131 charge<\/strong>, and Ca\u00b2\u207a is in square brackets with no dots and a <strong>+2 charge<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation (Approx. 300 Words)<\/h3>\n\n\n\n<p>Calcium chloride (CaCl\u2082) is an <strong>ionic compound<\/strong> formed between a <strong>metal<\/strong> (calcium) and a <strong>non-metal<\/strong> (chlorine). In ionic bonding, <strong>electrons are transferred<\/strong> from the metal to the non-metal.<\/p>\n\n\n\n<p>Calcium (Ca), a Group 2 element, has two valence electrons. To become stable, it <strong>loses both electrons<\/strong>, forming a <strong>Ca\u00b2\u207a ion<\/strong>. This ion has no valence electrons (hence no dots in the Lewis structure) and is shown with a <strong>2+ charge<\/strong>. Because it is an ion, it should be placed in <strong>square brackets<\/strong>: <strong>[Ca]\u00b2\u207a<\/strong>.<\/p>\n\n\n\n<p>Chlorine (Cl), a Group 17 element, has <strong>7 valence electrons<\/strong> and needs <strong>one more<\/strong> to complete its octet. Each Cl atom <strong>gains one electron<\/strong>, forming a <strong>Cl\u207b ion<\/strong> with <strong>8 valence electrons<\/strong> (represented as 8 dots). Each Cl\u207b is placed in <strong>square brackets with a 1\u2013 charge<\/strong>: <strong>[Cl]\u207b<\/strong>.<\/p>\n\n\n\n<p>Since one Ca\u00b2\u207a gives up <strong>2 electrons<\/strong>, and each Cl\u207b only accepts <strong>1 electron<\/strong>, <strong>two chlorine atoms<\/strong> are needed to balance the charge. The resulting compound is <strong>electrically neutral<\/strong>, with a ratio of 1:2 (CaCl\u2082).<\/p>\n\n\n\n<p>In summary, the Lewis structure of CaCl\u2082 consists of one <strong>[Ca]\u00b2\u207a ion (no dots)<\/strong> and two <strong>[Cl]\u207b ions (8 dots each)<\/strong>. The use of square brackets and charges correctly shows the ionic nature and electron transfer in the compound.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner5-113.jpeg\" alt=\"\" class=\"wp-image-221271\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Describe the Lewis structure for the ionic compound calcium chloride, CaCl2. The structure would include a Cl with 7 dots a 1- charge but with no square brackets. The structure would include a Cl with 8 dots in square brackets with a 2+ charge. The structure would include a Ca with no dots a 2+ [&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-221270","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221270","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=221270"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221270\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=221270"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=221270"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=221270"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}