{"id":181301,"date":"2025-01-10T09:54:34","date_gmt":"2025-01-10T09:54:34","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=181301"},"modified":"2025-01-10T09:54:37","modified_gmt":"2025-01-10T09:54:37","slug":"select-the-atoms-or-ions-drawn-with-valid-lewis-dot-structures","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/10\/select-the-atoms-or-ions-drawn-with-valid-lewis-dot-structures\/","title":{"rendered":"Select the atoms or ions drawn with valid Lewis dot structures"},"content":{"rendered":"\n<p>1.Select the atoms or ions drawn with valid Lewis dot structures.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/01\/image-92.png\" alt=\"\" class=\"wp-image-181302\"\/><\/figure>\n\n\n\n<p>2.a) Draw the Lewis structure of acetone, (CH3)2CO<\/p>\n\n\n\n<p>Step 1: Identify the number of valence electrons.<\/p>\n\n\n\n<p>Step 2: Identify the central atom.<\/p>\n\n\n\n<p>Step 3: Establish connectivity of single bonds.<\/p>\n\n\n\n<p>Step 4: Identify the number of electrons unaccounted for.<\/p>\n\n\n\n<p>Step 5: Complete the structure.<\/p>\n\n\n\n<p>b) Identify the central atom in (CH3)2CO, which is it out of the following?<\/p>\n\n\n\n<p>carbon<br>oxygen<br>hydrogen<\/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><strong>1. Validity of Lewis Dot Structures:<\/strong><\/p>\n\n\n\n<p>The image you&#8217;ve provided contains several atoms and ions. To determine which have valid Lewis dot structures, we need to consider the following:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons:<\/strong> Each atom&#8217;s valence electrons are represented as dots around the element symbol.<\/li>\n\n\n\n<li><strong>Octet Rule:<\/strong> Atoms (except hydrogen) tend to form bonds to achieve a full valence shell of eight electrons.<\/li>\n\n\n\n<li><strong>Formal Charges:<\/strong> The distribution of electrons should minimize formal charges, leading to a more stable structure.<\/li>\n<\/ul>\n\n\n\n<p>Without specific details about each atom or ion in the image, I can&#8217;t provide a definitive assessment. However, atoms like noble gases (e.g., Ne, Ar) naturally have complete valence shells and thus have stable Lewis structures. Ions such as Na\u207a or Cl\u207b also have valid Lewis structures, with Na\u207a having no dots (indicating a full valence shell) and Cl\u207b having eight dots.<\/p>\n\n\n\n<p><strong>2. Drawing the Lewis Structure of Acetone ((CH\u2083)\u2082CO):<\/strong><\/p>\n\n\n\n<p><strong>a) Steps to Draw the Lewis Structure:<\/strong><\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Identify the Number of Valence Electrons:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C): 4 valence electrons \u00d7 3 atoms = 12 electrons<\/li>\n\n\n\n<li>Hydrogen (H): 1 valence electron \u00d7 6 atoms = 6 electrons<\/li>\n\n\n\n<li>Oxygen (O): 6 valence electrons \u00d7 1 atom = 6 electrons<\/li>\n\n\n\n<li>Total valence electrons = 12 + 6 + 6 = 24 electrons<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Identify the Central Atom:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Oxygen (O) is the central atom, as it is double-bonded to one carbon and single-bonded to another.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Establish Connectivity of Single Bonds:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Connect the two methyl groups (CH\u2083) to the central carbonyl group (C=O).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Identify the Number of Electrons Unaccounted For:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each single bond uses 2 electrons.<\/li>\n\n\n\n<li>There are 3 single bonds (2 C-H and 1 C-C), using 6 electrons.<\/li>\n\n\n\n<li>The double bond (C=O) uses 4 electrons.<\/li>\n\n\n\n<li>Total electrons used = 6 + 4 = 10 electrons.<\/li>\n\n\n\n<li>Electrons remaining = 24 &#8211; 10 = 14 electrons.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Complete the Structure:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Distribute the remaining electrons as lone pairs on the oxygen atom and the carbon atoms to satisfy the octet rule.<\/li>\n<\/ul>\n\n\n\n<p><strong>b) Identifying the Central Atom in Acetone ((CH\u2083)\u2082CO):<\/strong><\/p>\n\n\n\n<p>The central atom in acetone is <strong>carbon<\/strong>. It is double-bonded to oxygen and single-bonded to two other carbon atoms, forming a ketone functional group. This central carbon atom is sp\u00b2 hybridized, leading to a trigonal planar geometry around it. The oxygen atom is double-bonded to this central carbon, and each of the two methyl groups (CH\u2083) is single-bonded to the central carbon. This arrangement results in a molecule with a trigonal planar structure around the central carbon atom.<\/p>\n\n\n\n<p>Understanding the central atom&#8217;s role is crucial in determining the molecule&#8217;s geometry and reactivity. In acetone, the central carbon atom&#8217;s sp\u00b2 hybridization and the presence of the carbonyl group (C=O) contribute to its polarity and solvent properties. Acetone&#8217;s polarity allows it to dissolve a wide range of substances, making it an effective solvent in various industrial and laboratory applications.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>1.Select the atoms or ions drawn with valid Lewis dot structures. 2.a) Draw the Lewis structure of acetone, (CH3)2CO Step 1: Identify the number of valence electrons. Step 2: Identify the central atom. Step 3: Establish connectivity of single bonds. Step 4: Identify the number of electrons unaccounted for. Step 5: Complete the structure. b) [&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-181301","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/181301","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=181301"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/181301\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=181301"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=181301"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=181301"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}