{"id":204500,"date":"2025-03-22T08:03:09","date_gmt":"2025-03-22T08:03:09","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=204500"},"modified":"2025-03-22T08:03:11","modified_gmt":"2025-03-22T08:03:11","slug":"write-the-electron-dot-structure-for-ethylene","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/22\/write-the-electron-dot-structure-for-ethylene\/","title":{"rendered":"Write the electron dot structure for ethylene"},"content":{"rendered":"\n<p>Write the electron dot structure for ethylene, C2H4.<br>a. What is the total number of available valence electrons?<strong>_<\/strong><br>b. In the space below, write the atomic symbols, then add the bonding electron pairs. Finally distribute any<br>non-bonding electron pairs.<br>c. If there are not enough valence electrons remaining for the carbon atoms, consider the possibility of<br>having a multiple bond between the two carbon atoms. If there is a double covalent bond between the<br>carbon atoms (sharing of 4 valence electrons), can each carbon satisfy the Octet Rule?<\/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<h3 class=\"wp-block-heading\">Ethylene (C\u2082H\u2084) Electron Dot Structure<\/h3>\n\n\n\n<p>Ethylene (C\u2082H\u2084) is a simple hydrocarbon consisting of two carbon (C) atoms and four hydrogen (H) atoms. Here&#8217;s how to draw the electron dot structure for ethylene and answer your questions.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">a. Total Number of Available Valence Electrons<\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Carbon (C) is in Group 14 of the periodic table, so each carbon atom has 4 valence electrons.<\/li>\n\n\n\n<li>Hydrogen (H) is in Group 1, so each hydrogen atom has 1 valence electron.<\/li>\n<\/ul>\n\n\n\n<p>The total number of valence electrons is:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>For 2 carbon atoms: ( 2 \\times 4 = 8 ) valence electrons<\/li>\n\n\n\n<li>For 4 hydrogen atoms: ( 4 \\times 1 = 4 ) valence electrons<\/li>\n<\/ul>\n\n\n\n<p>Thus, the total number of valence electrons = ( 8 + 4 = 12 ) valence electrons.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">b. Drawing the Atomic Symbols, Bonding Pairs, and Non-Bonding Electrons<\/h4>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Carbon and Hydrogen Configuration:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each hydrogen atom forms a single bond with a carbon atom. This uses 2 valence electrons for each hydrogen-carbon bond.<\/li>\n\n\n\n<li>Ethylene has 2 carbon atoms, each bonded to 2 hydrogen atoms.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Bonding Between Carbon Atoms:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each carbon atom needs 4 electrons to complete its octet, but they are only sharing 2 electrons with each hydrogen atom (forming single bonds).<\/li>\n\n\n\n<li>Thus, the two carbon atoms will share 4 electrons (forming a <strong>double bond<\/strong>) to complete their octet.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Electron Dot Structure:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each carbon atom is shown with 4 valence electrons in total, including 2 electrons for each bond with a hydrogen and 4 shared electrons between the two carbon atoms.<\/li>\n\n\n\n<li>The hydrogen atoms each have 1 bond (and no lone pairs).<\/li>\n<\/ul>\n\n\n\n<p>So, the electron dot structure of ethylene looks like this:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>H     H\n |     |\nC = C\n |     |\nH     H<\/code><\/pre>\n\n\n\n<p>In this structure, the &#8220;=&#8221; sign represents the double bond (2 shared electron pairs) between the two carbon atoms.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">c. Can Each Carbon Satisfy the Octet Rule with a Double Bond?<\/h4>\n\n\n\n<p>Yes, each carbon atom can satisfy the <strong>Octet Rule<\/strong> by forming a double bond between the two carbon atoms. Here&#8217;s how:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each carbon atom has 4 valence electrons. By forming two single bonds with hydrogen atoms (each hydrogen contributing 1 electron), each carbon shares 2 electrons with each hydrogen.<\/li>\n\n\n\n<li>The carbon-carbon double bond involves the sharing of 4 electrons (2 electrons in each bond), bringing the total number of electrons shared by each carbon atom to 8 (4 from hydrogen bonds + 4 from the carbon-carbon double bond).<\/li>\n<\/ul>\n\n\n\n<p>Thus, each carbon atom effectively has 8 electrons in its valence shell, fulfilling the octet rule.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Hydrogen<\/strong> atoms, on the other hand, only need 2 electrons to complete their valence shell (following the duet rule), which they achieve by sharing 1 electron with the carbon atoms.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation (300 words):<\/h3>\n\n\n\n<p>The electron dot structure for <strong>ethylene (C\u2082H\u2084)<\/strong> reveals how atoms achieve stable electron configurations by sharing electrons. Carbon atoms, with 4 valence electrons, seek 4 more electrons to fill their valence shell and satisfy the <strong>Octet Rule<\/strong>, which states that atoms tend to form bonds until they have 8 electrons in their outer shell (except for hydrogen, which follows the duet rule).<\/p>\n\n\n\n<p>The <strong>hydrogen atoms<\/strong> each need just 2 electrons to complete their outer shell. In the ethylene molecule, each hydrogen forms a <strong>single bond<\/strong> with a carbon atom, providing each hydrogen with its required 2 electrons.<\/p>\n\n\n\n<p>The two <strong>carbon atoms<\/strong> in ethylene bond with each other by a <strong>double bond<\/strong> (represented by a &#8220;=&#8221; in the dot structure). A double bond involves sharing 4 electrons (2 pairs), which allows each carbon atom to achieve an octet of electrons, satisfying the Octet Rule. Without the double bond, each carbon atom would only have 6 electrons in its valence shell, which would not satisfy the octet rule.<\/p>\n\n\n\n<p>The total number of valence electrons in the molecule (12) is used up in the bonding process: 8 electrons are used for the carbon-hydrogen bonds (4 bonds), and 4 electrons are shared between the two carbon atoms in the double bond. As a result, all atoms\u2014carbon and hydrogen\u2014achieve stable electron configurations, with the carbon atoms following the Octet Rule and the hydrogen atoms following the Duet Rule.<\/p>\n\n\n\n<p>This bonding arrangement ensures the stability of the ethylene molecule.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Write the electron dot structure for ethylene, C2H4.a. What is the total number of available valence electrons?_b. In the space below, write the atomic symbols, then add the bonding electron pairs. Finally distribute anynon-bonding electron pairs.c. If there are not enough valence electrons remaining for the carbon atoms, consider the possibility ofhaving a multiple bond [&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-204500","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/204500","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=204500"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/204500\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=204500"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=204500"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=204500"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}