{"id":27454,"date":"2025-06-19T23:02:18","date_gmt":"2025-06-19T23:02:18","guid":{"rendered":"https:\/\/gaviki.com\/blog\/?p=27454"},"modified":"2025-06-19T23:02:26","modified_gmt":"2025-06-19T23:02:26","slug":"which-of-the-following-molecule-is-of-t-shape","status":"publish","type":"post","link":"https:\/\/gaviki.com\/blog\/which-of-the-following-molecule-is-of-t-shape\/","title":{"rendered":"Which of the following molecule is of T &#8211; shape"},"content":{"rendered":"\n<p>Which of the following molecule is of T &#8211; shape? A. I3 B. ClF3 C. SF4 D. XeF4<\/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<p><strong>Correct Answer: B. ClF\u2083<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation (Approx. 300 words):<\/h3>\n\n\n\n<p>The molecule that adopts a <strong>T-shape<\/strong> molecular geometry is <strong>ClF\u2083 (chlorine trifluoride)<\/strong>.<\/p>\n\n\n\n<p>To understand why ClF\u2083 has a T-shaped geometry, we must apply the principles of <strong>VSEPR theory<\/strong> (Valence Shell Electron Pair Repulsion Theory), which is used to predict the shape of molecules based on the repulsion between electron pairs (bonding and nonbonding) around a central atom.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Step-by-step Analysis of ClF\u2083:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Central Atom<\/strong>: Chlorine (Cl)<\/li>\n\n\n\n<li><strong>Valence Electrons in Cl<\/strong>: 7<\/li>\n\n\n\n<li><strong>Bonds with Fluorine<\/strong>: 3 Cl\u2013F single bonds use 3 bonding pairs of electrons.<\/li>\n\n\n\n<li><strong>Lone Pairs on Cl<\/strong>: Remaining 4 electrons = 2 lone pairs.<\/li>\n\n\n\n<li><strong>Total Electron Pairs Around Cl<\/strong>: 3 bonding pairs + 2 lone pairs = 5 electron domains.<\/li>\n<\/ol>\n\n\n\n<p>According to VSEPR theory, 5 electron domains arrange themselves in a <strong>trigonal bipyramidal<\/strong> electron geometry to minimize repulsion. In this geometry:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The <strong>equatorial<\/strong> positions are more spacious than the <strong>axial<\/strong> ones.<\/li>\n\n\n\n<li>Lone pairs prefer equatorial positions to minimize repulsion.<\/li>\n<\/ul>\n\n\n\n<p>So, in ClF\u2083:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The two lone pairs occupy two equatorial positions.<\/li>\n\n\n\n<li>The three fluorine atoms occupy the two axial positions and one remaining equatorial position.<\/li>\n<\/ul>\n\n\n\n<p>This results in a <strong>T-shaped<\/strong> molecular geometry.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Why the Others Are Not T-Shaped:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>A. I\u2083\u207b<\/strong>: Linear geometry (3 atoms with 2 lone pairs on central atom).<\/li>\n\n\n\n<li><strong>C. SF\u2084<\/strong>: See-saw shape (5 electron domains: 4 bonding, 1 lone pair).<\/li>\n\n\n\n<li><strong>D. XeF\u2084<\/strong>: Square planar shape (6 electron domains: 4 bonding, 2 lone pairs opposite each other).<\/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\">Conclusion:<\/h3>\n\n\n\n<p>ClF\u2083 has 5 electron pairs (3 bonding + 2 lone), and the geometry that minimizes repulsion with this configuration is <strong>T-shaped<\/strong>. Thus, <strong>option B is correct<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Which of the following molecule is of T &#8211; shape? A. I3 B. ClF3 C. SF4 D. XeF4 The correct answer and explanation is: Correct Answer: B. ClF\u2083 Explanation (Approx. 300 words): The molecule that adopts a T-shape molecular geometry is ClF\u2083 (chlorine trifluoride). To understand why ClF\u2083 has a T-shaped geometry, we must apply [&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-27454","post","type-post","status-publish","format-standard","hentry","category-quiz-questions"],"_links":{"self":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27454","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=27454"}],"version-history":[{"count":1,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27454\/revisions"}],"predecessor-version":[{"id":27455,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/posts\/27454\/revisions\/27455"}],"wp:attachment":[{"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/media?parent=27454"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/categories?post=27454"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/gaviki.com\/blog\/wp-json\/wp\/v2\/tags?post=27454"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}