{"id":223100,"date":"2025-06-01T08:36:06","date_gmt":"2025-06-01T08:36:06","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=223100"},"modified":"2025-06-01T08:36:08","modified_gmt":"2025-06-01T08:36:08","slug":"how-many-shared-electrons-are-there-in-the-lewis-structure-of-sbf3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/01\/how-many-shared-electrons-are-there-in-the-lewis-structure-of-sbf3\/","title":{"rendered":"How many shared electrons are there in the Lewis structure of SbF3"},"content":{"rendered":"\n<p>How many shared electrons are there in the Lewis structure of SbF3?<br>How many shared electrons are there in the Lewis structure of SbF3?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p><strong>Answer:<\/strong><br>There are <strong>6 shared electrons<\/strong> in the Lewis structure of <strong>SbF\u2083<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation<\/strong><\/h3>\n\n\n\n<p><strong>Antimony trifluoride (SbF\u2083)<\/strong> is a covalent compound composed of one antimony (Sb) atom and three fluorine (F) atoms. In its Lewis structure, we examine how electrons are distributed to satisfy the <strong>octet rule<\/strong> and determine how many electrons are <strong>shared<\/strong> between atoms via covalent bonds.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\">Step 1: Count valence electrons<\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Sb (Group 15)<\/strong> has <strong>5 valence electrons<\/strong>.<\/li>\n\n\n\n<li><strong>F (Group 17)<\/strong> has <strong>7 valence electrons<\/strong>, and there are <strong>3 fluorine atoms<\/strong>.<br>\u2192 Total from fluorines = 3 \u00d7 7 = 21 valence electrons<\/li>\n\n\n\n<li><strong>Total valence electrons<\/strong> in SbF\u2083 = 5 (Sb) + 21 (F) = <strong>26 electrons<\/strong><\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\">Step 2: Determine bonding<\/h4>\n\n\n\n<p>In the Lewis structure:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sb forms <strong>three single covalent bonds<\/strong> with each of the three fluorine atoms.<\/li>\n\n\n\n<li>Each <strong>single bond<\/strong> consists of <strong>2 shared electrons<\/strong>.<br>\u2192 Total shared electrons = 3 bonds \u00d7 2 electrons = <strong>6 shared electrons<\/strong><\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\">Step 3: Assign lone pairs<\/h4>\n\n\n\n<p>After forming the three Sb\u2013F bonds (6 electrons), we have <strong>20 electrons<\/strong> left (26 total \u2013 6 shared = 20).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each fluorine atom requires 3 lone pairs (6 electrons) to complete its octet.<br>\u2192 3 fluorines \u00d7 6 electrons = 18 electrons<\/li>\n\n\n\n<li>The remaining <strong>2 electrons<\/strong> go as a <strong>lone pair on Sb<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h4 class=\"wp-block-heading\">Final Structure:<\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sb is at the center with <strong>three single bonds<\/strong> to fluorine atoms.<\/li>\n\n\n\n<li>Each F has 6 non-bonding electrons (3 lone pairs).<\/li>\n\n\n\n<li>Sb has one lone pair.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Summary:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Number of shared electrons = 6 (from 3 single bonds)<\/strong><\/li>\n\n\n\n<li>These shared electrons are what make up the <strong>covalent bonds<\/strong> holding SbF\u2083 together.<\/li>\n<\/ul>\n\n\n\n<p>This understanding is crucial for predicting molecular geometry (SbF\u2083 is <strong>trigonal pyramidal<\/strong>) and the polarity of the molecule.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner4-35.jpeg\" alt=\"\" class=\"wp-image-223101\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>How many shared electrons are there in the Lewis structure of SbF3?How many shared electrons are there in the Lewis structure of SbF3? The Correct Answer and Explanation is: Answer:There are 6 shared electrons in the Lewis structure of SbF\u2083. Explanation Antimony trifluoride (SbF\u2083) is a covalent compound composed of one antimony (Sb) atom and [&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-223100","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/223100","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=223100"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/223100\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=223100"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=223100"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=223100"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}