{"id":203638,"date":"2025-03-20T11:04:39","date_gmt":"2025-03-20T11:04:39","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203638"},"modified":"2025-03-20T11:04:41","modified_gmt":"2025-03-20T11:04:41","slug":"what-is-the-molecular-geometry-of-the-ion","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/20\/what-is-the-molecular-geometry-of-the-ion\/","title":{"rendered":"What is the molecular geometry of the ion"},"content":{"rendered":"\n<p>What is the molecular geometry of the ion?<br>Choose one:<br>A linear<br>B T-shaped<br>C seesaw<br>D trigonal planar<br>E square planar<br>F octahedral<br>G trigonal bypyramidal<br>H trigonal pyramidal<br>I square pyramidal<br>J tetrahedral<br>K bent<\/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>To determine the molecular geometry of an ion, we need to know its <strong>Lewis structure<\/strong>, <strong>valence shell electron pair repulsion (VSEPR) theory<\/strong>, and <strong>electron domain geometry<\/strong>. However, you haven\u2019t specified which ion you are referring to, so I&#8217;ll explain the general approach and then consider an example.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Steps to Determine Molecular Geometry<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Draw the Lewis Structure<\/strong> \u2013 Identify the number of valence electrons and arrange them around the central atom.<\/li>\n\n\n\n<li><strong>Count Electron Domains<\/strong> \u2013 Count bonding pairs and lone pairs around the central atom.<\/li>\n\n\n\n<li><strong>Apply VSEPR Theory<\/strong> \u2013 Predict the molecular shape based on the number of electron pairs and lone pairs.<\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Example: Sulfate Ion (SO\u2084\u00b2\u207b)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure:<\/strong> Sulfur is the central atom, forming four single bonds with oxygen.<\/li>\n\n\n\n<li><strong>Electron Domains:<\/strong> 4 (all bonding pairs, no lone pairs).<\/li>\n\n\n\n<li><strong>VSEPR Shape:<\/strong> Since there are four bonding pairs and no lone pairs, the shape is <strong>tetrahedral<\/strong>.<\/li>\n\n\n\n<li><strong>Correct Answer:<\/strong> <strong>J) Tetrahedral<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Example: Nitrite Ion (NO\u2082\u207b)<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis Structure:<\/strong> Nitrogen is the central atom with one lone pair and two bonded oxygen atoms (one with a double bond, one with a single bond and a negative charge).<\/li>\n\n\n\n<li><strong>Electron Domains:<\/strong> 3 (two bonding pairs, one lone pair).<\/li>\n\n\n\n<li><strong>VSEPR Shape:<\/strong> <strong>Bent (K)<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>General Rule for Common Molecular Geometries<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Linear (A)<\/strong> \u2013 Two bonding groups, no lone pairs (e.g., CO\u2082).<\/li>\n\n\n\n<li><strong>Trigonal Planar (D)<\/strong> \u2013 Three bonding groups, no lone pairs (e.g., NO\u2083\u207b).<\/li>\n\n\n\n<li><strong>Tetrahedral (J)<\/strong> \u2013 Four bonding groups, no lone pairs (e.g., SO\u2084\u00b2\u207b).<\/li>\n\n\n\n<li><strong>Bent (K)<\/strong> \u2013 Two bonding groups, one or two lone pairs (e.g., NO\u2082\u207b, H\u2082O).<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>What is the molecular geometry of the ion?Choose one:A linearB T-shapedC seesawD trigonal planarE square planarF octahedralG trigonal bypyramidalH trigonal pyramidalI square pyramidalJ tetrahedralK bent The correct answer and explanation is : To determine the molecular geometry of an ion, we need to know its Lewis structure, valence shell electron pair repulsion (VSEPR) theory, and [&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 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