{"id":35972,"date":"2025-06-25T00:34:24","date_gmt":"2025-06-25T00:34:24","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=35972"},"modified":"2025-06-25T00:34:25","modified_gmt":"2025-06-25T00:34:25","slug":"draw-lewis-structure-for-xef4-and-answer-the-following-questions-based-on-your-drawing","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/draw-lewis-structure-for-xef4-and-answer-the-following-questions-based-on-your-drawing\/","title":{"rendered":"Draw Lewis structure for XeF4 and answer the following questions based on your drawing"},"content":{"rendered":"\n<p>Draw Lewis structure for XeF4 and answer the following questions based on your drawing: 1. For the central xenon atom: The number of lone pairs The number of single bonds The number of double bonds 2. The central xenon atom: A. Obeys the octet rule B. Has an incomplete octet C. Has an expanded octet.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-vivid-cyan-blue-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p><strong>Lewis Structure of XeF\u2084 (Xenon Tetrafluoride):<\/strong><\/p>\n\n\n\n<p>To draw the Lewis structure of XeF\u2084:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Count the total valence electrons:<\/strong>\n<ul class=\"wp-block-list\">\n<li>Xenon (Xe) has 8 valence electrons.<\/li>\n\n\n\n<li>Each fluorine (F) has 7 valence electrons. With 4 fluorines, that gives 4 \u00d7 7 = 28.<\/li>\n\n\n\n<li>Total valence electrons = 8 (Xe) + 28 (F) = 36 electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Place Xe in the center<\/strong> since it is the least electronegative, and attach the four fluorine atoms to it using single bonds.\n<ul class=\"wp-block-list\">\n<li>Each single bond uses 2 electrons: 4 bonds \u00d7 2 = 8 electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Subtract used electrons:<\/strong> 36 \u2212 8 = 28 electrons remaining.<\/li>\n\n\n\n<li><strong>Distribute remaining electrons to satisfy octets of the fluorines.<\/strong>\n<ul class=\"wp-block-list\">\n<li>Each F needs 6 more electrons to complete its octet (3 lone pairs).<\/li>\n\n\n\n<li>4 fluorines \u00d7 6 electrons = 24 electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n<li><strong>Remaining electrons after fluorine octets:<\/strong> 28 \u2212 24 = 4 electrons.<\/li>\n\n\n\n<li><strong>Place the remaining 4 electrons (2 lone pairs) on the central xenon atom.<\/strong><\/li>\n<\/ol>\n\n\n\n<h3 class=\"wp-block-heading\">Answers:<\/h3>\n\n\n\n<p><strong>1. For the central xenon atom:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Number of lone pairs:<\/strong> 2<\/li>\n\n\n\n<li><strong>Number of single bonds:<\/strong> 4<\/li>\n\n\n\n<li><strong>Number of double bonds:<\/strong> 0<\/li>\n<\/ul>\n\n\n\n<p><strong>2. The central xenon atom:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>C. Has an expanded octet<\/strong><\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation<\/h3>\n\n\n\n<p>Xenon tetrafluoride (XeF\u2084) is a molecule composed of one xenon atom bonded to four fluorine atoms. Xenon is a noble gas, and it might seem unusual for it to form compounds. However, due to the availability of empty d-orbitals, xenon can expand its valence shell and accommodate more than eight electrons. This is evident in XeF\u2084, where the central xenon atom is surrounded by twelve electrons: eight from the four single bonds with fluorine atoms and four from two lone pairs.<\/p>\n\n\n\n<p>In the Lewis structure, each fluorine atom forms a single bond with xenon and holds three lone pairs to satisfy the octet rule. The central xenon atom, after forming four bonds (8 electrons), still has 4 more electrons (2 lone pairs) placed on it. This gives a total of 12 electrons around xenon, meaning xenon exceeds the octet rule.<\/p>\n\n\n\n<p>The presence of an expanded octet is typical for elements in period 3 and beyond of the periodic table. These elements have access to d-orbitals, which allow them to accommodate more than eight electrons. In the case of xenon, this is chemically feasible and energetically favorable in compounds like XeF\u2084.<\/p>\n\n\n\n<p>There are no double bonds in this structure. The fluorine atoms are highly electronegative and typically form only single bonds. The geometry of XeF\u2084 is square planar due to the presence of two lone pairs on xenon, which repel each other and the bonding pairs, arranging the atoms in a flat square around the central atom to minimize repulsion.<\/p>\n\n\n\n<p>Thus, the central xenon atom in XeF\u2084 has 2 lone pairs, 4 single bonds, no double bonds, and an expanded octet.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"852\" height=\"1024\" src=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-720.jpeg\" alt=\"\" class=\"wp-image-35973\" srcset=\"https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-720.jpeg 852w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-720-250x300.jpeg 250w, https:\/\/gaviki.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner8-720-768x923.jpeg 768w\" sizes=\"auto, (max-width: 852px) 100vw, 852px\" \/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw Lewis structure for XeF4 and answer the following questions based on your drawing: 1. For the central xenon atom: The number of lone pairs The number of single bonds The number of double bonds 2. The central xenon atom: A. Obeys the octet rule B. Has an incomplete octet C. Has an expanded octet. [&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-35972","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/35972","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=35972"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/35972\/revisions"}],"predecessor-version":[{"id":35974,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/35972\/revisions\/35974"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=35972"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=35972"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=35972"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}