{"id":191174,"date":"2025-02-14T08:08:57","date_gmt":"2025-02-14T08:08:57","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=191174"},"modified":"2025-02-14T08:08:59","modified_gmt":"2025-02-14T08:08:59","slug":"lewis-structure-of-cl4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/14\/lewis-structure-of-cl4\/","title":{"rendered":"Lewis structure of Cl4"},"content":{"rendered":"\n

Lewis structure of Cl4<\/p>\n\n\n\n

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

The Lewis structure of Cl\u2084 is a bit unusual, as chlorine typically forms bonds with other elements. Cl\u2084 is not a common molecule in chemical bonding, and it’s often considered to be an unstable molecule that doesn’t typically exist in isolated form under normal conditions. However, for the sake of the question, let’s consider the hypothetical bonding arrangement for Cl\u2084.<\/p>\n\n\n\n

Lewis Structure of Cl\u2084:<\/h3>\n\n\n\n
    \n
  1. Chlorine atoms:<\/strong> Chlorine (Cl) is a halogen with 7 valence electrons. For Cl\u2084, we would have 4 chlorine atoms, each contributing 7 valence electrons, which gives us a total of 28 valence electrons.<\/li>\n\n\n\n
  2. Bonding:<\/strong> In this hypothetical molecule, each chlorine atom would typically try to bond with another chlorine atom to share electrons. If we attempt to form a structure, we might expect a central chlorine atom to form bonds with the other three chlorine atoms. This would involve single bonds between chlorine atoms.<\/li>\n\n\n\n
  3. Electron Distribution:<\/strong> After bonding, there will still be extra electrons that need to be assigned as lone pairs on each chlorine atom. The chlorine atoms need 8 electrons in their valence shells to achieve a stable configuration (following the octet rule).<\/li>\n<\/ol>\n\n\n\n

    Steps to Draw the Lewis Structure:<\/h3>\n\n\n\n
      \n
    • Place one chlorine atom in the center and arrange the other three chlorine atoms around it.<\/li>\n\n\n\n
    • Draw single bonds between the central chlorine and each of the surrounding chlorine atoms. This accounts for 6 electrons (3 single bonds).<\/li>\n\n\n\n
    • Now, distribute the remaining 22 electrons (28 total valence electrons minus 6 for the bonds) as lone pairs on the chlorine atoms.<\/li>\n\n\n\n
    • Place 3 lone pairs on each of the three outer chlorine atoms. This uses up 18 electrons (3 x 6 electrons).<\/li>\n\n\n\n
    • The remaining 4 electrons will be placed as lone pairs on the central chlorine atom, completing its octet.<\/li>\n<\/ul>\n\n\n\n

      Final Structure:<\/h3>\n\n\n\n
        \n
      • Each outer chlorine atom will have 3 lone pairs and 1 bond with the central chlorine.<\/li>\n\n\n\n
      • The central chlorine atom will have 2 lone pairs and 3 bonds with the surrounding chlorines.<\/li>\n<\/ul>\n\n\n\n

        However, it\u2019s important to note that Cl\u2084 is not a stable or commonly encountered molecule, and such a structure is more of a theoretical model.<\/p>\n\n\n\n

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

        The Lewis structure of Cl\u2084 follows general principles for Lewis structures, where atoms form bonds to share electrons to reach a stable configuration. Chlorine, being a halogen, follows the octet rule, and this configuration involves sharing electrons in a way that all chlorine atoms achieve an octet. The molecule, however, does not have significant real-world existence due to its instability.<\/p>\n","protected":false},"excerpt":{"rendered":"

        Lewis structure of Cl4 The Correct Answer and Explanation is : The Lewis structure of Cl\u2084 is a bit unusual, as chlorine typically forms bonds with other elements. Cl\u2084 is not a common molecule in chemical bonding, and it’s often considered to be an unstable molecule that doesn’t typically exist in isolated form under normal […]<\/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-191174","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191174","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=191174"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191174\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191174"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191174"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191174"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}