{"id":258955,"date":"2025-07-18T15:31:40","date_gmt":"2025-07-18T15:31:40","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=258955"},"modified":"2025-07-18T15:31:43","modified_gmt":"2025-07-18T15:31:43","slug":"place-the-following-in-order-of-decreasing-x-o-bond-length-x-indicates-the-central-atom","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/18\/place-the-following-in-order-of-decreasing-x-o-bond-length-x-indicates-the-central-atom\/","title":{"rendered":"Place the following in order of decreasing X-O bond length (“X” indicates the central atom"},"content":{"rendered":"\n
Place the following in order of decreasing X-O bond length (\"X\" indicates the central atom<\/pre>\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 SiO\u2083\u00b2\u207b > CO\u2083\u00b2\u207b > CO\u2082<\/strong>.<\/p>\n\n\n\n
To determine the order of decreasing X-O bond length, we need to consider two main factors: bond order and the atomic radius of the central atom (X).<\/p>\n\n\n\n
First, let’s analyze the bond order for each species. Bond order is the number of chemical bonds between a pair of atoms. A higher bond order results in a stronger attraction between the atoms, pulling them closer together and thus decreasing the bond length.<\/p>\n\n\n\n
    \n
  1. CO\u2082 (Carbon Dioxide):<\/strong>\u00a0The Lewis structure for CO\u2082 is O=C=O. It consists of two carbon-oxygen double bonds. Therefore, the C-O bond order is 2.<\/li>\n\n\n\n
  2. CO\u2083\u00b2\u207b (Carbonate ion):<\/strong>\u00a0The carbonate ion has three resonance structures. In each structure, there is one C=O double bond and two C-O single bonds. The actual structure is a resonance hybrid, where the electrons are delocalized across all three C-O bonds. The bond order is calculated as the average number of bonds, which is (2 + 1 + 1) \/ 3 = 4\/3, or approximately 1.33.<\/li>\n\n\n\n
  3. SiO\u2083\u00b2\u207b (Silicate ion):<\/strong>\u00a0This ion is isoelectronic and isostructural with the carbonate ion. It also exhibits resonance, and its Si-O bond order is also 4\/3, or approximately 1.33.<\/li>\n<\/ol>\n\n\n\n
    Based on bond order alone, CO\u2082 (bond order 2) has the shortest bond. Both CO\u2083\u00b2\u207b and SiO\u2083\u00b2\u207b have a lower bond order (1.33), so their bonds will be longer than the bond in CO\u2082.<\/p>\n\n\n\n
    Next, we compare CO\u2083\u00b2\u207b and SiO\u2083\u00b2\u207b, which have the same bond order. Here, we must consider the size of the central atom. Carbon (C) is in Period 2 of the periodic table, while Silicon (Si) is directly below it in Period 3. Atomic radius increases as you move down a group. Therefore, the silicon atom is significantly larger than the carbon atom. A larger central atom leads to a longer bond length. Consequently, the Si-O bond in SiO\u2083\u00b2\u207b is longer than the C-O bond in CO\u2083\u00b2\u207b.<\/p>\n\n\n\n
    Combining these points, we can establish the final order of decreasing bond length (from longest to shortest):<\/p>\n\n\n\n
      \n
    1. SiO\u2083\u00b2\u207b<\/strong>\u00a0(longest, due to the large Si atom)<\/li>\n\n\n\n
    2. CO\u2083\u00b2\u207b<\/strong>\u00a0(intermediate, smaller central atom than Si)<\/li>\n\n\n\n
    3. CO\u2082<\/strong>\u00a0(shortest, due to the highest bond order)<\/li>\n<\/ol>\n\n\n\n
      This gives the order: SiO\u2083\u00b2\u207b > CO\u2083\u00b2\u207b > CO\u2082.<\/p>\n\n\n\n
      \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
      Place the following in order of decreasing X-O bond length (“X” indicates the central atom The Correct Answer and Explanation is: The correct answer is SiO\u2083\u00b2\u207b > CO\u2083\u00b2\u207b > CO\u2082. To determine the order of decreasing X-O bond length, we need to consider two main factors: bond order and the atomic radius of the central atom […]<\/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-258955","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/258955","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=258955"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/258955\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=258955"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=258955"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=258955"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}