{"id":223766,"date":"2025-06-02T10:25:35","date_gmt":"2025-06-02T10:25:35","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=223766"},"modified":"2025-06-02T10:25:37","modified_gmt":"2025-06-02T10:25:37","slug":"what-is-the-molecular-geometry-of-ibr3-according-to-the-vsepr-theory","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/02\/what-is-the-molecular-geometry-of-ibr3-according-to-the-vsepr-theory\/","title":{"rendered":"What is the molecular geometry of IBr3 according to the VSEPR theory"},"content":{"rendered":"\n

What is the molecular geometry of IBr3 according to the VSEPR theory? Seesaw B. T-shaped Bent or V-shaped D, Trigonal planar Tetrahedral<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

The correct answer is: B. T-shaped<\/strong><\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

To determine the molecular geometry of IBr\u2083<\/strong> using VSEPR (Valence Shell Electron Pair Repulsion) theory<\/strong>, we follow these steps:<\/p>\n\n\n\n

\n\n\n\n

Step 1: Determine the central atom and valence electrons<\/h3>\n\n\n\n

Iodine (I) is the central atom because it’s less electronegative than bromine (Br).<\/p>\n\n\n\n

    \n
  • Iodine is in Group 17 (halogens), so it has 7 valence electrons<\/strong>.<\/li>\n\n\n\n
  • Each bromine atom forms a single bond with iodine, using 1 electron from iodine per bond.<\/li>\n\n\n\n
  • 3 Br atoms form 3 bonds, using 3 of iodine\u2019s 7 electrons.<\/li>\n\n\n\n
  • That leaves 4 electrons (2 lone pairs)<\/strong> on iodine.<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    Step 2: Count the regions of electron density around iodine<\/h3>\n\n\n\n
      \n
    • There are 3 bonding pairs<\/strong> (one for each I\u2013Br bond).<\/li>\n\n\n\n
    • There are 2 lone pairs<\/strong> of electrons on iodine.<\/li>\n<\/ul>\n\n\n\n

      So, iodine has 5 regions of electron density<\/strong>. According to VSEPR theory, 5 regions correspond to a trigonal bipyramidal electron geometry<\/strong>.<\/p>\n\n\n\n

      \n\n\n\n

      Step 3: Determine molecular geometry<\/h3>\n\n\n\n

      In a trigonal bipyramidal electron geometry:<\/p>\n\n\n\n

        \n
      • Lone pairs prefer the equatorial positions<\/strong> (to minimize repulsion).<\/li>\n\n\n\n
      • If two lone pairs occupy equatorial positions, the three Br atoms occupy two axial and one equatorial position<\/strong>.<\/li>\n<\/ul>\n\n\n\n

        This leads to a T-shaped molecular geometry<\/strong>, where:<\/p>\n\n\n\n

          \n
        • Two Br atoms are opposite each other (axial).<\/li>\n\n\n\n
        • One Br atom is in the equatorial plane.<\/li>\n\n\n\n
        • The lone pairs occupy the other two equatorial positions.<\/li>\n<\/ul>\n\n\n\n
          \n\n\n\n

          Final Result:<\/h3>\n\n\n\n
            \n
          • Electron Geometry<\/strong>: Trigonal bipyramidal<\/li>\n\n\n\n
          • Molecular Geometry<\/strong>: T-shaped<\/strong><\/li>\n<\/ul>\n\n\n\n

            Therefore, the correct answer is B. T-shaped<\/strong>, due to the presence of two lone pairs and three bonding pairs on the central iodine atom<\/p>\n\n\n\n

            \"\"<\/figure>\n\n\n\n

            .<\/p>\n","protected":false},"excerpt":{"rendered":"

            What is the molecular geometry of IBr3 according to the VSEPR theory? Seesaw B. T-shaped Bent or V-shaped D, Trigonal planar Tetrahedral The Correct Answer and Explanation is: The correct answer is: B. T-shaped Explanation: To determine the molecular geometry of IBr\u2083 using VSEPR (Valence Shell Electron Pair Repulsion) theory, we follow these steps: Step […]<\/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-223766","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/223766","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=223766"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/223766\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=223766"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=223766"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=223766"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}