{"id":238197,"date":"2025-06-17T21:23:13","date_gmt":"2025-06-17T21:23:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=238197"},"modified":"2025-06-17T21:23:15","modified_gmt":"2025-06-17T21:23:15","slug":"angle-explain-briefly","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/17\/angle-explain-briefly\/","title":{"rendered":"angle? Explain briefly"},"content":{"rendered":"\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/image-679.png\" alt=\"\" class=\"wp-image-238198\"\/><\/figure>\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<p>For question 34, the triiodide ion (I\u2083\u207b) is linear because the central iodine atom has three lone pairs that effectively balance out the repulsions from surrounding atoms, allowing a straight arrangement. However, the triiodide cation (I\u2083\u207a) lacks a lone pair on the central iodine, leading to an uneven distribution of electron density that forces the molecule into a bent shape.<\/p>\n\n\n\n<p>For question 35, diborane (B\u2082H\u2086) exhibits D\u2082h symmetry because it has bridging hydrogen atoms that create a symmetrical arrangement around the boron centers. On the other hand, iodine trichloride (I\u2082Cl\u2086) adopts a planar configuration due to electron repulsions and steric effects that favor a flat structure.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation<\/h3>\n\n\n\n<p>The shape of a molecule or ion is determined by its electronic configuration and the principles of valence shell electron pair repulsion (VSEPR) theory. In the case of I\u2083\u207b, the central iodine atom has three lone pairs of electrons that symmetrically arrange themselves around it. Since lone pairs repel each other strongly, the molecule adopts a linear shape to minimize repulsions. Conversely, I\u2083\u207a has fewer lone pairs, and the bonding electrons do not distribute evenly enough to maintain linearity. This causes a bend in its shape, as lone-pair interactions no longer enforce strict linear geometry.<\/p>\n\n\n\n<p>For B\u2082H\u2086, D\u2082h symmetry arises because the bridging hydrogen atoms are positioned in a staggered fashion, creating a balanced geometric framework. The boron atoms in diborane share electrons through three-center two-electron bonds, leading to a symmetrical, nonplanar configuration. Meanwhile, in I\u2082Cl\u2086, the large iodine atoms are surrounded by chlorine atoms in a manner that minimizes electron repulsions and steric hindrance, favoring a planar shape.<\/p>\n\n\n\n<p>The structural differences between these compounds highlight how electron arrangement and molecular interactions dictate spatial orientation and stability.<\/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-banner8-1002.jpeg\" alt=\"\" class=\"wp-image-238199\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>The Correct Answer and Explanation is: For question 34, the triiodide ion (I\u2083\u207b) is linear because the central iodine atom has three lone pairs that effectively balance out the repulsions from surrounding atoms, allowing a straight arrangement. However, the triiodide cation (I\u2083\u207a) lacks a lone pair on the central iodine, leading to an uneven distribution [&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-238197","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/238197","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=238197"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/238197\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=238197"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=238197"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=238197"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}