{"id":168225,"date":"2024-11-16T20:58:34","date_gmt":"2024-11-16T20:58:34","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=168225"},"modified":"2024-11-16T20:58:36","modified_gmt":"2024-11-16T20:58:36","slug":"draw-the-lewis-structure-for-a-hydroxide-oh-ion","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/16\/draw-the-lewis-structure-for-a-hydroxide-oh-ion\/","title":{"rendered":"Draw the Lewis structure for a hydroxide (OH^-) ion"},"content":{"rendered":"\n<p>Draw the Lewis structure for a hydroxide (OH^-) ion<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Lewis Structure of Hydroxide Ion (OH\u207b)<\/h3>\n\n\n\n<p>To draw the Lewis structure for the hydroxide ion (OH\u207b), follow these steps:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Count the Total Valence Electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen (O) is in Group 16 of the periodic table, so it has 6 valence electrons.<\/li>\n\n\n\n<li>Hydrogen (H) is in Group 1, so it has 1 valence electron.<\/li>\n\n\n\n<li>The hydroxide ion has a negative charge (OH\u207b), meaning there is an additional electron.<\/li>\n\n\n\n<li>Total valence electrons = 6 (from oxygen) + 1 (from hydrogen) + 1 (extra electron) = <strong>8 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Determine the Central Atom<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen will be the central atom since it is more electronegative than hydrogen.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Arrange the Atoms<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Place oxygen in the center, with a single bond connecting it to hydrogen. This bond will use 2 electrons (1 from oxygen and 1 from hydrogen).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Distribute the Remaining Electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>After placing the single bond (2 electrons), there are 6 electrons left to be placed.<\/li>\n\n\n\n<li>These remaining 6 electrons will be placed as lone pairs on the oxygen atom. Oxygen will have three lone pairs, using up the remaining 6 electrons.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Account for the Negative Charge<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The negative charge indicates an extra electron. This extra electron is added as a lone pair on the oxygen atom.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Final Structure:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Oxygen<\/strong>: It has one single bond to hydrogen, two lone pairs, and a third lone pair with an extra electron due to the negative charge.<\/li>\n\n\n\n<li><strong>Hydrogen<\/strong>: It is bonded to oxygen with a single bond and has no lone pairs.<\/li>\n<\/ul>\n\n\n\n<p>The Lewis structure for the hydroxide ion is:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>    H\n    |\nO :  :  \n    :  (lone pair)<\/code><\/pre>\n\n\n\n<p>Where:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>&#8220;O&#8221; represents oxygen.<\/li>\n\n\n\n<li>&#8220;:&#8221; represents lone pairs of electrons on oxygen.<\/li>\n\n\n\n<li>&#8220;H&#8221; represents hydrogen, which is bonded to oxygen via a single bond.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen has 6 valence electrons and forms a single bond with hydrogen, using 2 electrons.<\/li>\n\n\n\n<li>The remaining 6 electrons are placed as three lone pairs on oxygen.<\/li>\n\n\n\n<li>The negative charge on OH\u207b results from an extra electron, which is added to the oxygen atom.<\/li>\n\n\n\n<li>The Lewis structure accurately represents the bonding and lone pairs in the hydroxide ion, illustrating the ion&#8217;s overall charge and electron distribution.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure for a hydroxide (OH^-) ion The Correct Answer and Explanation is: Lewis Structure of Hydroxide Ion (OH\u207b) To draw the Lewis structure for the hydroxide ion (OH\u207b), follow these steps: Final Structure: The Lewis structure for the hydroxide ion is: Where: Explanation:<\/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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