{"id":236312,"date":"2025-06-16T07:26:37","date_gmt":"2025-06-16T07:26:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=236312"},"modified":"2025-06-16T07:26:39","modified_gmt":"2025-06-16T07:26:39","slug":"the-molecular-geometry-for-icl4-________is-and-the-approximate-value-of-the-cl-i-cl-bond-angle-is","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/16\/the-molecular-geometry-for-icl4-________is-and-the-approximate-value-of-the-cl-i-cl-bond-angle-is\/","title":{"rendered":"The molecular geometry for ICl4- ________is and the approximate value of the Cl-I-Cl bond angle is"},"content":{"rendered":"\n<p>The molecular geometry for ICl4- <em>________is and the approximate value of the Cl-I-Cl bond angle is<\/em><\/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><strong>Correct Answer:<\/strong><\/p>\n\n\n\n<p>The molecular geometry for <strong>ICl\u2084\u207b<\/strong> is <strong>square planar<\/strong>, and the approximate value of the <strong>Cl\u2013I\u2013Cl bond angle<\/strong> is <strong>90 degrees<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>Explanation<\/strong><\/p>\n\n\n\n<p>Iodine tetrachloride anion, denoted as ICl\u2084\u207b, is a polyatomic ion consisting of one iodine atom and four chlorine atoms with a negative charge. To determine its molecular geometry and bond angles, the Valence Shell Electron Pair Repulsion (VSEPR) theory serves as a helpful guide. This theory is based on the repulsion between electron pairs surrounding a central atom, which shapes the molecule to minimize repulsive interactions.<\/p>\n\n\n\n<p>First, consider the number of valence electrons around the central iodine atom. Iodine belongs to group 17 and contributes 7 valence electrons. Each chlorine atom contributes one electron via the I\u2013Cl bond, and the ion carries an additional electron due to its negative charge, totaling <strong>36 valence electrons<\/strong> (7 from I + 4\u00d77 from Cl + 1 extra).<\/p>\n\n\n\n<p>When constructing the Lewis structure, iodine forms four single bonds with four chlorine atoms. This accounts for 8 electrons used in bonding. The remaining electrons are arranged as lone pairs. Iodine, being in Period 5, can expand its octet. After satisfying the octets of chlorine atoms, there are two lone pairs left on the central iodine atom.<\/p>\n\n\n\n<p>With four bonded atoms and two lone pairs on the central atom, the steric number is 6. According to VSEPR theory, a steric number of 6 corresponds to an <strong>octahedral<\/strong> electron geometry. However, the two lone pairs occupy axial positions to reduce repulsion, resulting in a <strong>square planar<\/strong> molecular geometry.<\/p>\n\n\n\n<p>The bond angles in an ideal square planar geometry are approximately <strong>90 degrees<\/strong> between adjacent Cl\u2013I\u2013Cl atoms. These angles remain close to ideal because the lone pairs are located opposite each other and do not distort the square plane significantly. Thus, ICl\u2084\u207b has a square planar shape with Cl\u2013I\u2013Cl bond angles around 90\u00b0.<\/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-banner10-167.jpeg\" alt=\"\" class=\"wp-image-236313\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The molecular geometry for ICl4- ________is and the approximate value of the Cl-I-Cl bond angle is The Correct Answer and Explanation is: Correct Answer: The molecular geometry for ICl\u2084\u207b is square planar, and the approximate value of the Cl\u2013I\u2013Cl bond angle is 90 degrees. Explanation Iodine tetrachloride anion, denoted as ICl\u2084\u207b, is a polyatomic ion [&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-236312","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/236312","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=236312"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/236312\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=236312"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=236312"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=236312"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}