{"id":234315,"date":"2025-06-14T04:14:05","date_gmt":"2025-06-14T04:14:05","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=234315"},"modified":"2025-06-14T04:14:08","modified_gmt":"2025-06-14T04:14:08","slug":"draw-the-electron-dot-structure-of-carbon-dioxide-and-write-the-natural-of-bonding-between-carbon-and-oxygen-in-molecule","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/14\/draw-the-electron-dot-structure-of-carbon-dioxide-and-write-the-natural-of-bonding-between-carbon-and-oxygen-in-molecule\/","title":{"rendered":"Draw the electron dot structure of carbon dioxide and write the natural of bonding between carbon and oxygen in molecule"},"content":{"rendered":"\n

Draw the electron dot structure of carbon dioxide and write the natural of bonding between carbon and oxygen in molecule<\/p>\n\n\n\n

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

Electron Dot Structure of Carbon Dioxide (CO\u2082)<\/h3>\n\n\n\n

Electron Dot Structure (Lewis Structure):<\/strong><\/p>\n\n\n\n

mathematicaCopyEditO = C = O\n<\/code><\/pre>\n\n\n\n
Each oxygen atom forms a double covalent bond<\/strong> with the central carbon atom. In the Lewis structure:<\/p>\n\n\n\n
    \n
  • Carbon (C) has 4 valence electrons.<\/li>\n\n\n\n
  • Oxygen (O) has 6 valence electrons.<\/li>\n\n\n\n
  • Each double bond represents 4 shared electrons<\/strong> (2 pairs) between carbon and oxygen.<\/li>\n\n\n\n
  • Each oxygen also has 4 nonbonding electrons (2 lone pairs) remaining.<\/li>\n<\/ul>\n\n\n\n
    Dot version:<\/strong><\/p>\n\n\n\n
    rubyCopyEdit..     ..  \n:O::C::O:\n..     ..\n<\/code><\/pre>\n\n\n\n
    Each “:” represents a pair of electrons (either bonding or lone pair).<\/p>\n\n\n\n
    \n\n\n\n
    Nature of Bonding Between Carbon and Oxygen in CO\u2082<\/h3>\n\n\n\n
    The bonding between carbon and oxygen atoms in carbon dioxide is covalent<\/strong>, specifically double covalent bonds<\/strong>. A double covalent bond involves two shared pairs of electrons<\/strong> between two atoms. Here’s the breakdown:<\/p>\n\n\n\n
      \n
    1. Covalent Bonding:<\/strong>
      Covalent bonds occur when two atoms share electrons to achieve stability. In CO\u2082, carbon shares electrons with two oxygen atoms to complete its octet (8 valence electrons).<\/li>\n\n\n\n
    2. Double Bond Formation:<\/strong>
      Since each oxygen needs 2 electrons to complete its octet and carbon needs 4, each oxygen shares two electrons with carbon, forming a double bond. This satisfies the octet rule for both carbon and oxygen atoms.<\/li>\n\n\n\n
    3. Bond Polarity:<\/strong>
      Although the C=O bonds are polar due to the difference in electronegativity (oxygen is more electronegative than carbon), the molecule is linear and symmetrical<\/strong>, so the dipoles cancel out, making CO\u2082 a non-polar molecule overall<\/strong>.<\/li>\n\n\n\n
    4. Molecular Geometry:<\/strong>
      The shape of the molecule is linear<\/strong> with a bond angle of 180\u00b0<\/strong>, due to the repulsion between electron domains as predicted by VSEPR (Valence Shell Electron Pair Repulsion) theory.<\/li>\n<\/ol>\n\n\n\n
      In conclusion, the electron dot structure of carbon dioxide shows two double bonds between carbon and oxygen. The bonding is covalent, and due to the molecule’s linear shape, CO\u2082 is non-polar in nature despite having polar bonds.<\/p>\n\n\n\n
      \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
      Draw the electron dot structure of carbon dioxide and write the natural of bonding between carbon and oxygen in molecule The Correct Answer and Explanation is: Electron Dot Structure of Carbon Dioxide (CO\u2082) Electron Dot Structure (Lewis Structure): mathematicaCopyEditO = C = O Each oxygen atom forms a double covalent bond with the central carbon […]<\/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-234315","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234315","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=234315"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/234315\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=234315"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=234315"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=234315"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}