{"id":16399,"date":"2025-06-11T12:33:29","date_gmt":"2025-06-11T12:33:29","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=16399"},"modified":"2025-06-11T12:33:30","modified_gmt":"2025-06-11T12:33:30","slug":"draw-the-lewis-structure-for-brf3","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/draw-the-lewis-structure-for-brf3\/","title":{"rendered":"Draw the Lewis structure for BrF3"},"content":{"rendered":"\n<p>Draw the Lewis structure for BrF3. What is the formal charge on the bromine atom?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\"><strong>The correct answer and explanation is:<\/strong><\/mark><\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Correct Answer:<\/strong><\/h3>\n\n\n\n<p>The Lewis structure of <strong>BrF\u2083 (bromine trifluoride)<\/strong> shows <strong>three bonding pairs<\/strong> and <strong>two lone pairs<\/strong> around the central <strong>bromine (Br)<\/strong> atom. The <strong>formal charge<\/strong> on the bromine atom in BrF\u2083 is <strong>0<\/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 (Approximately 300 Words):<\/strong><\/h3>\n\n\n\n<p>To draw the Lewis structure of <strong>BrF\u2083<\/strong>, we begin by determining the total number of valence electrons:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Bromine (Br)<\/strong> is in group 17 \u2192 7 valence electrons<\/li>\n\n\n\n<li><strong>Fluorine (F)<\/strong> is also in group 17 \u2192 7 valence electrons each \u00d7 3 = 21<\/li>\n<\/ul>\n\n\n\n<p><strong>Total valence electrons = 7 (Br) + 21 (3 F) = 28 electrons<\/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>Step 1: Skeleton Structure<\/strong><\/h3>\n\n\n\n<p>Place bromine in the center (less electronegative than fluorine), and attach the three fluorine atoms around it using single bonds. Each single bond uses 2 electrons \u00d7 3 = 6 electrons.<\/p>\n\n\n\n<p><strong>Remaining electrons: 28 \u2212 6 = 22 electrons<\/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>Step 2: Complete Octets of Fluorine Atoms<\/strong><\/h3>\n\n\n\n<p>Each fluorine needs 6 more electrons (3 lone pairs).<br>3 F \u00d7 6 = 18 electrons used<\/p>\n\n\n\n<p><strong>Remaining electrons: 22 \u2212 18 = 4 electrons<\/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>Step 3: Place Remaining Electrons on Central Atom<\/strong><\/h3>\n\n\n\n<p>Place the remaining 4 electrons (2 lone pairs) on bromine.<\/p>\n\n\n\n<p>Now bromine has:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>3 bonding pairs (from the Br\u2013F bonds)<\/li>\n\n\n\n<li>2 lone pairs<br>\u2192 <strong>5 regions of electron density<\/strong> \u2192 <strong>Trigonal bipyramidal electron geometry<\/strong><br>\u2192 <strong>T-shaped molecular geometry<\/strong><\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Step 4: Determine Formal Charge on Bromine<\/strong><\/h3>\n\n\n\n<p><strong>Formal charge = Valence \u2212 (Lone electrons + \u00bd Bonding electrons)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Valence electrons of Br = 7<\/li>\n\n\n\n<li>Lone electrons on Br = 4<\/li>\n\n\n\n<li>Bonding electrons = 6 (3 bonds \u00d7 2 electrons)<\/li>\n<\/ul>\n\n\n\n<p><strong>Formal charge = 7 \u2212 (4 + 3) = 0<\/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>Conclusion<\/strong><\/h3>\n\n\n\n<p>The correct Lewis structure shows a <strong>T-shaped BrF\u2083<\/strong> molecule, and the <strong>formal charge on bromine is 0<\/strong>, meaning it\u2019s in its most stable, neutral form in this structure.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure for BrF3. What is the formal charge on the bromine atom? The correct answer and explanation is: Correct Answer: The Lewis structure of BrF\u2083 (bromine trifluoride) shows three bonding pairs and two lone pairs around the central bromine (Br) atom. The formal charge on the bromine atom in BrF\u2083 is 0. [&hellip;]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[],"class_list":["post-16399","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16399","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/comments?post=16399"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16399\/revisions"}],"predecessor-version":[{"id":16400,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/16399\/revisions\/16400"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=16399"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=16399"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=16399"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}