{"id":169178,"date":"2024-11-19T05:50:26","date_gmt":"2024-11-19T05:50:26","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=169178"},"modified":"2024-11-19T05:50:29","modified_gmt":"2024-11-19T05:50:29","slug":"draw-the-lewis-structure-for-the-hydronium-ion-h%e2%82%83o%e2%81%ba","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/19\/draw-the-lewis-structure-for-the-hydronium-ion-h%e2%82%83o%e2%81%ba\/","title":{"rendered":"Draw the Lewis structure for the hydronium ion, H\u2083O\u207a."},"content":{"rendered":"\n<p>Draw the Lewis structure for the hydronium ion, H\u2083O\u207a.<\/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<p>The hydronium ion, ( H_3O^+ ), is a polyatomic ion formed when a proton (H\u207a) is added to a water molecule (H\u2082O). Here\u2019s how to draw its Lewis structure and a detailed explanation:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Steps to Draw the Lewis Structure for ( H_3O^+ ):<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Determine the Total Number of 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>Each hydrogen (H) atom contributes 1 valence electron, and since there are 3 hydrogens, this gives 3 electrons.<\/li>\n\n\n\n<li>The positive charge ( + ) means the ion has lost one electron, so we subtract 1 from the total count.<\/li>\n\n\n\n<li>The total number of valence electrons is:<br>[<br>6 (\\text{from O}) + 3 (\\text{from H}) &#8211; 1 (\\text{for the + charge}) = 8 \\text{ valence electrons}.<br>]<\/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 is the most electronegative atom and will be the central atom, with hydrogens attached to it.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Connect the Atoms<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen (O) will be at the center, and the three hydrogen (H) atoms will be bonded to it. Each bond between oxygen and hydrogen is a single bond, using two electrons per bond.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Distribute the Electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each O-H bond uses two electrons, so 3 bonds will use 6 electrons in total (3 \u00d7 2 electrons).<\/li>\n\n\n\n<li>The remaining 2 electrons will be placed as a lone pair on the oxygen atom.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Consider the Charge<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Since the hydronium ion has a ( + ) charge, we need to place the positive charge on the oxygen atom. This occurs because oxygen has a lone pair, but it shares its electron density with hydrogen atoms in a way that leaves it electron-deficient.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Final Lewis Structure:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen (O) is at the center with three single bonds to hydrogen atoms.<\/li>\n\n\n\n<li>Oxygen also has one lone pair of electrons.<\/li>\n\n\n\n<li>The hydronium ion has a positive charge, which is typically shown near the oxygen atom.<\/li>\n<\/ul>\n\n\n\n<pre class=\"wp-block-code\"><code>   H\n   |\nH\u2014O\u2014H\n   |\n   H<\/code><\/pre>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>The hydronium ion consists of a central oxygen atom bonded to three hydrogen atoms. In this ion, oxygen forms single bonds with each hydrogen, utilizing 6 electrons for these bonds. The remaining 2 electrons on oxygen form a lone pair. The positive charge indicates that one electron is lost, which is often represented as being removed from the oxygen atom. This electron loss contributes to the creation of a positively charged ion. The structure ensures that oxygen satisfies the octet rule, while each hydrogen atom achieves a duet rule (2 electrons in its valence shell). The overall structure is stable due to the formation of covalent bonds and the appropriate distribution of electrons.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure for the hydronium ion, H\u2083O\u207a. The Correct Answer and Explanation is: The hydronium ion, ( H_3O^+ ), is a polyatomic ion formed when a proton (H\u207a) is added to a water molecule (H\u2082O). Here\u2019s how to draw its Lewis structure and a detailed explanation: Steps to Draw the Lewis Structure for [&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-169178","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/169178","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=169178"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/169178\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=169178"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=169178"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=169178"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}