{"id":194949,"date":"2025-02-25T10:00:52","date_gmt":"2025-02-25T10:00:52","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=194949"},"modified":"2025-02-25T10:00:55","modified_gmt":"2025-02-25T10:00:55","slug":"what-is-the-shape-of-iof4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/25\/what-is-the-shape-of-iof4\/","title":{"rendered":"What is the shape of IOF4+"},"content":{"rendered":"\n

What is the shape of IOF4+?
square planar
square pyramidal
trigonal bipyramidal
see-saw
octahedral<\/p>\n\n\n\n

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

The shape of IOF\u2084\u207a<\/strong> (Iodine Oxytetrafluoride cation) is square pyramidal<\/strong>.<\/p>\n\n\n\n

Explanation (300 Words)<\/strong><\/h3>\n\n\n\n

To determine the molecular shape of IOF\u2084\u207a<\/strong>, we follow the VSEPR (Valence Shell Electron Pair Repulsion) Theory<\/strong>:<\/p>\n\n\n\n

    \n
  1. Valence Electrons Calculation<\/strong>:<\/li>\n<\/ol>\n\n\n\n
      \n
    • Iodine (I)<\/strong>: Group 17 \u2192 7 valence electrons<\/strong>.<\/li>\n\n\n\n
    • Oxygen (O)<\/strong>: Group 16 \u2192 6 valence electrons<\/strong>.<\/li>\n\n\n\n
    • Fluorine (F)<\/strong>: Group 17 \u2192 7 valence electrons each<\/strong> (4 Fluorine atoms \u2192 4 \u00d7 7 = 28<\/strong>).<\/li>\n\n\n\n
    • Total electrons before charge adjustment<\/strong>:
      [
      7 (I) + 6 (O) + 28 (F) = 41
      ]<\/li>\n\n\n\n
    • Charge on the ion<\/strong>: +1<\/strong>, meaning one electron is lost<\/strong>, so the total count is 40 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Lewis Structure and Steric Number<\/strong>:<\/li>\n<\/ol>\n\n\n\n
          \n
        • Iodine (I) is the central atom, bonded to one oxygen (O) and four fluorine (F) atoms<\/strong>.<\/li>\n\n\n\n
        • Five regions of electron density<\/strong> (four single bonds with F, one double bond with O).<\/li>\n\n\n\n
        • One lone pair<\/strong> remains on iodine.<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Molecular Geometry<\/strong>:<\/li>\n<\/ol>\n\n\n\n
              \n
            • With five electron groups<\/strong>, the electron geometry is trigonal bipyramidal<\/strong>.<\/li>\n\n\n\n
            • The presence of one lone pair<\/strong> makes the actual molecular shape square pyramidal<\/strong>, where four fluorine atoms form a square base and the oxygen occupies an axial position.<\/li>\n<\/ul>\n\n\n\n
                \n
              1. Confirmation<\/strong>:<\/li>\n<\/ol>\n\n\n\n
                  \n
                • This shape is consistent with other known iodine pentahalides<\/strong> and follows expected bond angles (approx. 90\u00b0<\/strong> in the square base and <90\u00b0<\/strong> between axial and base atoms).<\/li>\n<\/ul>\n\n\n\n

                  Thus, the correct answer is square pyramidal<\/strong>.<\/p>\n\n\n\n

                  Now, I will generate an image of the molecular structure.<\/p>\n\n\n\n

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

                  Here is the 3D molecular model of IOF\u2084\u207a<\/strong> in its square pyramidal<\/strong> shape. The structure shows the iodine atom at the center, bonded to four fluorine atoms forming a square base, with an oxygen atom positioned at the top. Let me know if you need further modifications or explanations!<\/p>\n","protected":false},"excerpt":{"rendered":"

                  What is the shape of IOF4+?square planarsquare pyramidaltrigonal bipyramidalsee-sawoctahedral The Correct Answer and Explanation is : The shape of IOF\u2084\u207a (Iodine Oxytetrafluoride cation) is square pyramidal. Explanation (300 Words) To determine the molecular shape of IOF\u2084\u207a, we follow the VSEPR (Valence Shell Electron Pair Repulsion) Theory: Thus, the correct answer is square pyramidal. Now, I […]<\/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-194949","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194949","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=194949"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/194949\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=194949"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=194949"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=194949"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}