{"id":249860,"date":"2025-07-10T05:59:24","date_gmt":"2025-07-10T05:59:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=249860"},"modified":"2025-07-10T05:59:26","modified_gmt":"2025-07-10T05:59:26","slug":"what-is-the-axe-description-of-the-periodate-io4-anion","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/10\/what-is-the-axe-description-of-the-periodate-io4-anion\/","title":{"rendered":"What is the “AXE” description of the periodate (IO4-) anion"},"content":{"rendered":"\n

What is the “AXE” description of the periodate (IO4-) anion? AXE 0 0<\/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 AXE description for the periodate (IO\u2084\u207b) anion is AX\u2084E\u2080<\/strong>.<\/p>\n\n\n\n

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

The “AXE” notation is a way to describe the geometry of a molecule based on the Valence Shell Electron Pair Repulsion (VSEPR) theory. Here is a step-by-step breakdown of how to determine the AXE description for the periodate anion (IO\u2084\u207b):<\/p>\n\n\n\n

    \n
  1. Understand the AXE Components:<\/strong>\n
      \n
    • A<\/strong>\u00a0represents the central atom in the molecule.<\/li>\n\n\n\n
    • X<\/strong>\u00a0represents the number of atoms bonded to the central atom. The subscript next to X is this number.<\/li>\n\n\n\n
    • E<\/strong>\u00a0represents the number of non-bonding electron pairs (lone pairs) on the central atom only. The subscript next to E is this number.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Determine the Central Atom (A):<\/strong>
      In the IO\u2084\u207b anion, Iodine (I) is the central atom because it is the least electronegative element and there is only one of it.<\/li>\n\n\n\n
    • Count the Total Valence Electrons:<\/strong>
      To find the number of lone pairs, we must first determine the Lewis structure by counting the total valence electrons.\n
        \n
      • Iodine (I) is in Group 17, so it has\u00a07<\/strong>\u00a0valence electrons.<\/li>\n\n\n\n
      • Oxygen (O) is in Group 16, so each of the four atoms has\u00a06<\/strong>\u00a0valence electrons (4 \u00d7 6 = 24).<\/li>\n\n\n\n
      • The anion has a negative one charge (-1), which means there is one extra electron.<\/li>\n\n\n\n
      • Total valence electrons = 7 (from I) + 24 (from 4 O’s) + 1 (from charge) =\u00a032 electrons<\/strong>.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Determine X (Number of Bonded Atoms):<\/strong>
        The formula is IO\u2084\u207b, which clearly shows that there are\u00a0four<\/strong>\u00a0oxygen atoms bonded to the central iodine atom.\n
          \n
        • Therefore, the value for X is\u00a04<\/strong>.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Determine E (Number of Lone Pairs on the Central Atom):<\/strong>\n
            \n
          • Start by drawing a skeleton structure with the central iodine single-bonded to the four oxygen atoms. This uses 4 bonds \u00d7 2 electrons\/bond = 8 electrons.<\/li>\n\n\n\n
          • Subtract these from the total: 32 – 8 = 24 electrons remaining.<\/li>\n\n\n\n
          • Distribute the remaining 24 electrons as lone pairs to the outer oxygen atoms to satisfy their octets. Each oxygen needs 6 more electrons (3 lone pairs). 4 oxygen atoms \u00d7 6 electrons = 24 electrons.<\/li>\n\n\n\n
          • After distributing these 24 electrons, there are no electrons left over to place on the central iodine atom.<\/li>\n\n\n\n
          • Therefore, the number of lone pairs on the central iodine atom is\u00a00<\/strong>. The value for E is\u00a00<\/strong>.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

            By combining these parts, we get the final AXE description: AX\u2084E\u2080<\/strong>. This notation corresponds to a tetrahedral electron geometry and a tetrahedral molecular geometry.<\/p>\n\n\n\n

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

            What is the “AXE” description of the periodate (IO4-) anion? AXE 0 0 The Correct Answer and Explanation is: The correct AXE description for the periodate (IO\u2084\u207b) anion is AX\u2084E\u2080. Explanation: The “AXE” notation is a way to describe the geometry of a molecule based on the Valence Shell Electron Pair Repulsion (VSEPR) theory. Here is […]<\/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-249860","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249860","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=249860"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/249860\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=249860"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=249860"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=249860"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}