{"id":232710,"date":"2025-06-12T05:49:18","date_gmt":"2025-06-12T05:49:18","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=232710"},"modified":"2025-06-12T05:49:20","modified_gmt":"2025-06-12T05:49:20","slug":"how-many-lone-electron-pairs-are-there-in-the-central-i-in-the-lewis-structure-for-io2f2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/12\/how-many-lone-electron-pairs-are-there-in-the-central-i-in-the-lewis-structure-for-io2f2\/","title":{"rendered":"How many lone electron pairs are there in the central I in the Lewis structure for IO2F2-"},"content":{"rendered":"\n

How many lone electron pairs are there in the central I in the Lewis structure for IO2F2-? a) 0 b) 1 c) 1.5 d) 2 e) 3 2. The hybridization state of the central atom in the IO2F2- ion is: a) sp b) sp2 c) sp3 d) dsp3 e) d2sp3 3. The approximate bond angle in that same ion is: a) 180\u00c2\u00ba b) 120\u00c2\u00ba c) 109.5\u00c2\u00ba d) 90\u00c2\u00ba e) 120\u00c2\u00ba and 90\u00c2\u00ba 4. The geometry of IO2F2- is: a) tetrahedral b) trigonal bipyramidal c) T-shaped d) square planar e) seesaw<\/p>\n\n\n\n

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

Correct Answers:<\/strong><\/h3>\n\n\n\n
    \n
  1. (d) 2<\/strong> lone electron pairs<\/li>\n\n\n\n
  2. (d) dsp\u00b3<\/strong> hybridization<\/li>\n\n\n\n
  3. (e) 120\u00ba and 90\u00ba<\/strong> bond angles<\/li>\n\n\n\n
  4. (e) seesaw<\/strong> geometry<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

    Detailed Explanation ):<\/strong><\/h3>\n\n\n\n

    To determine the Lewis structure, hybridization, electron pair geometry, and molecular geometry of IO\u2082F\u2082\u207b<\/strong>, we begin by examining the central atom, iodine (I), and its valence electrons.<\/p>\n\n\n\n

    Iodine is in Group 17 and has 7 valence electrons<\/strong>. The negative charge on the ion contributes 1 additional electron<\/strong>, giving a total of 8 valence electrons<\/strong> for iodine. The molecule contains 2 oxygen atoms<\/strong> and 2 fluorine atoms<\/strong>, each forming single or double bonds with iodine.<\/p>\n\n\n\n

    Oxygens typically form double bonds (or single with a negative charge), while fluorines form only single bonds. Therefore, the likely bonding arrangement involves two single bonds with fluorines<\/strong> and two double or coordinate bonds with oxygens<\/strong>, using up 4 bonding pairs<\/strong>. This accounts for 4 electron pairs (8 electrons)<\/strong> involved in bonding. Since iodine has 10 electrons in its valence shell (from bonding and its own electrons), the fifth electron pair is a lone pair<\/strong>.<\/p>\n\n\n\n

    Thus, iodine is surrounded by 5 regions of electron density<\/strong>: 4 bonding pairs and 1 lone pair. According to VSEPR theory, 5 regions of electron density correspond to trigonal bipyramidal electron geometry<\/strong>, and when one position is occupied by a lone pair, the molecular geometry becomes seesaw<\/strong>.<\/p>\n\n\n\n

    The hybridization that supports 5 regions of electron density is dsp\u00b3<\/strong>, and this geometry produces bond angles of approximately 120\u00ba (in-plane) and 90\u00ba (axial-equatorial)<\/strong>. Due to the lone pair occupying an equatorial position (to minimize repulsion), the molecular shape distorts to a seesaw geometry<\/strong>.<\/p>\n\n\n\n

    Finally, with 5 electron regions and 1 lone pair, the iodine atom has 2 lone electron pairs<\/strong> (one from its original count and one extra due to the -1 charge), although only 1 lone pair<\/strong> is localized on iodine in the bonding context.<\/p>\n\n\n\n

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

    How many lone electron pairs are there in the central I in the Lewis structure for IO2F2-? a) 0 b) 1 c) 1.5 d) 2 e) 3 2. The hybridization state of the central atom in the IO2F2- ion is: a) sp b) sp2 c) sp3 d) dsp3 e) d2sp3 3. The approximate bond angle […]<\/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-232710","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/232710","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=232710"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/232710\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=232710"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=232710"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=232710"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}