{"id":224772,"date":"2025-06-03T13:06:27","date_gmt":"2025-06-03T13:06:27","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=224772"},"modified":"2025-06-03T13:06:29","modified_gmt":"2025-06-03T13:06:29","slug":"draw-the-lewis-structure-of-krf2-molecule","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/03\/draw-the-lewis-structure-of-krf2-molecule\/","title":{"rendered":"Draw the Lewis structure of KrF2 molecule."},"content":{"rendered":"\n<p>Draw the Lewis structure of KrF2 molecule. What is the polarity of this molecule and the hybridization on the central atom, krypton, respectively?<\/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\/image-74.png\" alt=\"\" class=\"wp-image-224773\"\/><\/figure>\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>Correct Answer:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Polarity:<\/strong> Nonpolar<\/li>\n\n\n\n<li><strong>Hybridization of central atom (Krypton):<\/strong> sp\u00b3d<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>Explanation<\/strong><\/p>\n\n\n\n<p>The molecule <strong>KrF\u2082<\/strong> (krypton difluoride) consists of one krypton (Kr) atom bonded to two fluorine (F) atoms. To determine the Lewis structure, start by calculating the total number of valence electrons. Krypton is a noble gas in group 18 with <strong>8 valence electrons<\/strong>, and each fluorine atom (group 17) has <strong>7 valence electrons<\/strong>. Therefore, KrF\u2082 has:<\/p>\n\n\n\n<p><strong>Total valence electrons = 8 (Kr) + 2 \u00d7 7 (F) = 22 electrons<\/strong><\/p>\n\n\n\n<p>In the Lewis structure, krypton is the central atom. Place one single bond between Kr and each F atom, using 2 electrons per bond (4 electrons total). Each F atom then completes its octet with 6 more electrons (3 lone pairs), using <strong>12 electrons total<\/strong>. That leaves <strong>6 electrons<\/strong> (22 &#8211; 4 &#8211; 12 = 6), which are placed as <strong>3 lone pairs on krypton<\/strong>.<\/p>\n\n\n\n<p>Thus, the Lewis structure of KrF\u2082 shows:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Two bonding pairs (Kr\u2013F)<\/li>\n\n\n\n<li>Three lone pairs on Kr<\/li>\n<\/ul>\n\n\n\n<p>This gives a <strong>total of five electron domains<\/strong> around krypton. According to <strong>VSEPR theory<\/strong>, five electron domains correspond to <strong>trigonal bipyramidal electron geometry<\/strong>. To minimize electron pair repulsion, the lone pairs occupy the equatorial positions, and the fluorine atoms occupy the axial positions. This results in a <strong>linear molecular shape<\/strong>.<\/p>\n\n\n\n<p>Because the two fluorine atoms are identical and symmetrically placed around the central atom in a linear geometry, their dipoles cancel out. Therefore, <strong>KrF\u2082 is a nonpolar molecule<\/strong>, despite having highly electronegative fluorine atoms.<\/p>\n\n\n\n<p>To accommodate five electron regions, the central atom (Kr) undergoes <strong>sp\u00b3d hybridization<\/strong>\u2014one s orbital, three p orbitals, and one d orbital mix to form five hybrid orbitals.<\/p>\n\n\n\n<p>In summary:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Lewis structure:<\/strong> Kr with two F atoms and three lone pairs<\/li>\n\n\n\n<li><strong>Molecular shape:<\/strong> Linear<\/li>\n\n\n\n<li><strong>Polarity:<\/strong> Nonpolar<\/li>\n\n\n\n<li><strong>Hybridization:<\/strong> sp\u00b3d<\/li>\n<\/ul>\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-banner7-126.jpeg\" alt=\"\" class=\"wp-image-224774\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Draw the Lewis structure of KrF2 molecule. What is the polarity of this molecule and the hybridization on the central atom, krypton, respectively? The Correct Answer and Explanation is: Correct Answer: Explanation The molecule KrF\u2082 (krypton difluoride) consists of one krypton (Kr) atom bonded to two fluorine (F) atoms. To determine the Lewis structure, start [&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-224772","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/224772","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=224772"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/224772\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=224772"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=224772"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=224772"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}