{"id":185737,"date":"2025-01-23T05:19:04","date_gmt":"2025-01-23T05:19:04","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185737"},"modified":"2025-01-23T05:19:06","modified_gmt":"2025-01-23T05:19:06","slug":"steric-number-on-central-atom","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/23\/steric-number-on-central-atom\/","title":{"rendered":"Steric Number on central atom"},"content":{"rendered":"\n<p>ICl3 and ICl5<\/p>\n\n\n\n<p>Steric Number on central atom<\/p>\n\n\n\n<p>Hybridization in Central atom<\/p>\n\n\n\n<p>Electron geometry on central atom<\/p>\n\n\n\n<p>Molecular geometry<\/p>\n\n\n\n<p>Symmetrical or not<\/p>\n\n\n\n<p>Bonds polar or nonpolar<\/p>\n\n\n\n<p>Sym bond dipoles polar or nonpolar<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>Let&#8217;s analyze the two compounds: <strong>ICl\u2083 (Iodine trichloride)<\/strong> and <strong>ICl\u2085 (Iodine pentachloride)<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">1. <strong>ICl\u2083 (Iodine trichloride)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Steric Number on the Central Atom<\/strong>: The central atom is iodine (I), which is bonded to three chlorine atoms. Additionally, iodine has two lone pairs of electrons. Therefore, the steric number is <strong>5<\/strong> (3 bonding pairs + 2 lone pairs).<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: With a steric number of 5, the hybridization of iodine is <strong>sp\u00b3d<\/strong>. This involves one s orbital, three p orbitals, and one d orbital.<\/li>\n\n\n\n<li><strong>Electron Geometry<\/strong>: The electron geometry around iodine in ICl\u2083 is <strong>trigonal bipyramidal<\/strong> due to the presence of 5 electron regions (3 bonds + 2 lone pairs).<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: The molecular geometry in ICl\u2083 is <strong>T-shaped<\/strong> because the lone pairs occupy equatorial positions to minimize repulsion, leaving the 3 bonds in a T-shape.<\/li>\n\n\n\n<li><strong>Symmetrical or Not<\/strong>: ICl\u2083 is <strong>not symmetrical<\/strong>. The T-shaped arrangement of atoms creates a molecular geometry that results in an overall dipole moment.<\/li>\n\n\n\n<li><strong>Bonds (Polar or Nonpolar)<\/strong>: The I-Cl bond is <strong>polar<\/strong> due to the difference in electronegativity between iodine and chlorine.<\/li>\n\n\n\n<li><strong>Bond Dipoles (Polar or Nonpolar)<\/strong>: Because of the T-shaped molecular geometry and polar bonds, the bond dipoles do not cancel out, making the overall molecular dipole <strong>polar<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">2. <strong>ICl\u2085 (Iodine pentachloride)<\/strong>:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Steric Number on the Central Atom<\/strong>: The central atom is iodine, which is bonded to five chlorine atoms. Iodine also has one lone pair of electrons, making the steric number <strong>6<\/strong> (5 bonding pairs + 1 lone pair).<\/li>\n\n\n\n<li><strong>Hybridization<\/strong>: With a steric number of 6, the hybridization of iodine is <strong>sp\u00b3d\u00b2<\/strong> (one s orbital, three p orbitals, and two d orbitals).<\/li>\n\n\n\n<li><strong>Electron Geometry<\/strong>: The electron geometry of ICl\u2085 is <strong>octahedral<\/strong> due to 6 electron regions (5 bonds + 1 lone pair).<\/li>\n\n\n\n<li><strong>Molecular Geometry<\/strong>: The molecular geometry is <strong>square pyramidal<\/strong> because the lone pair occupies one of the axial positions, leaving the 5 bonds arranged in a square pyramid.<\/li>\n\n\n\n<li><strong>Symmetrical or Not<\/strong>: ICl\u2085 is <strong>not symmetrical<\/strong>. The square pyramidal shape leads to an overall dipole moment.<\/li>\n\n\n\n<li><strong>Bonds (Polar or Nonpolar)<\/strong>: The I-Cl bonds are <strong>polar<\/strong> due to the electronegativity difference between iodine and chlorine.<\/li>\n\n\n\n<li><strong>Bond Dipoles (Polar or Nonpolar)<\/strong>: As the molecular geometry is not symmetrical, the bond dipoles do not cancel out, making the overall molecular dipole <strong>polar<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Summary:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>ICl\u2083<\/strong> has a T-shaped geometry, is polar with polar bonds and bond dipoles.<\/li>\n\n\n\n<li><strong>ICl\u2085<\/strong> has a square pyramidal geometry, is also polar with polar bonds and bond dipoles. Both compounds have non-symmetrical shapes that lead to a net molecular dipole moment.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>ICl3 and ICl5 Steric Number on central atom Hybridization in Central atom Electron geometry on central atom Molecular geometry Symmetrical or not Bonds polar or nonpolar Sym bond dipoles polar or nonpolar The Correct Answer and Explanation is : Let&#8217;s analyze the two compounds: ICl\u2083 (Iodine trichloride) and ICl\u2085 (Iodine pentachloride). 1. ICl\u2083 (Iodine trichloride): [&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-185737","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185737","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=185737"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185737\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185737"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185737"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185737"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}