{"id":186164,"date":"2025-01-24T08:16:17","date_gmt":"2025-01-24T08:16:17","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=186164"},"modified":"2025-01-24T08:16:19","modified_gmt":"2025-01-24T08:16:19","slug":"draw-the-electron-dot-formula-for-silicon-disulfide-5152","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/24\/draw-the-electron-dot-formula-for-silicon-disulfide-5152\/","title":{"rendered":"Draw the electron dot formula for silicon disulfide, 5152"},"content":{"rendered":"\n<p>Draw the electron dot formula for silicon disulfide, 5152. How many pairs of nonbonding electrons are in a silicon disulfide molecule? 02 06 01  hone of the above G4<\/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 draw the electron dot structure (also known as the Lewis structure) for silicon disulfide (SiS\u2082), we follow these steps:<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 1: Count the valence electrons<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Silicon (Si) is in group 14 of the periodic table, so it has 4 valence electrons.<\/li>\n\n\n\n<li>Sulfur (S) is in group 16, so each sulfur atom has 6 valence electrons.<\/li>\n<\/ul>\n\n\n\n<p>Thus, for SiS\u2082:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Silicon has 1 \u00d7 4 = 4 valence electrons.<\/li>\n\n\n\n<li>Sulfur has 2 \u00d7 6 = 12 valence electrons.<\/li>\n<\/ul>\n\n\n\n<p>The total number of valence electrons = 4 (from Si) + 12 (from S) = 16 valence electrons.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Step 2: Sketch the skeleton structure<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The silicon atom will be the central atom since it is less electronegative than sulfur.<\/li>\n\n\n\n<li>Place two sulfur atoms around the silicon atom, and form single bonds between silicon and sulfur. This uses 2 electrons (1 for each bond).<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 3: Distribute remaining electrons<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>After forming the bonds, 16 electrons &#8211; 2 electrons used in the bonds = 14 electrons remain.<\/li>\n\n\n\n<li>Distribute the remaining electrons as lone pairs around the sulfur atoms first, as sulfur is more electronegative than silicon.<\/li>\n\n\n\n<li>Each sulfur atom needs 6 more electrons to complete its octet (as each already shares 1 electron with silicon).<\/li>\n\n\n\n<li>Place 3 lone pairs (6 electrons) around each sulfur atom. This uses up all 12 remaining electrons.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Step 4: Check the structure<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The silicon atom now has 2 electrons from each bond (total 4 electrons), which satisfies its octet.<\/li>\n\n\n\n<li>Each sulfur atom has 6 electrons from lone pairs and 2 electrons from the bond with silicon, fulfilling its octet.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Electron Dot Formula<\/h3>\n\n\n\n<p>The electron dot structure for silicon disulfide is:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>   :S:   :S:\n    |     |\n    Si<\/code><\/pre>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each sulfur atom has 3 lone pairs of electrons and shares 1 pair with silicon, completing its octet.<\/li>\n\n\n\n<li>Silicon shares 2 pairs of electrons, completing its octet.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Number of Nonbonding Electron Pairs<\/h3>\n\n\n\n<p>In the silicon disulfide molecule, the nonbonding electrons are those on the sulfur atoms. Each sulfur atom has 3 lone pairs, for a total of 6 lone pairs of electrons.<\/p>\n\n\n\n<p>Thus, the answer is <strong>6 pairs of nonbonding electrons<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the electron dot formula for silicon disulfide, 5152. How many pairs of nonbonding electrons are in a silicon disulfide molecule? 02 06 01 hone of the above G4 The Correct Answer and Explanation is : To draw the electron dot structure (also known as the Lewis structure) for silicon disulfide (SiS\u2082), we follow these [&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-186164","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186164","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=186164"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/186164\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=186164"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=186164"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=186164"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}