{"id":192251,"date":"2025-02-17T12:12:10","date_gmt":"2025-02-17T12:12:10","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=192251"},"modified":"2025-02-17T12:12:13","modified_gmt":"2025-02-17T12:12:13","slug":"draw-the-best-lewis-structure-for-ccl3-1","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/17\/draw-the-best-lewis-structure-for-ccl3-1\/","title":{"rendered":"Draw the best lewis structure for CCl3 +1"},"content":{"rendered":"\n

Draw the best lewis structure for CCl3 +1. What is the formal charge on the C?<\/p>\n\n\n\n

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

The molecular ion CCl\u2083\u207a<\/strong> consists of a carbon atom (C) bonded to three chlorine atoms (Cl). It carries a positive charge, meaning it has one less electron than a neutral molecule would have.<\/p>\n\n\n\n

Step-by-Step Approach to Drawing the Best Lewis Structure:<\/h3>\n\n\n\n
    \n
  1. Determine the total number of valence electrons<\/strong>:<\/li>\n<\/ol>\n\n\n\n
      \n
    • Carbon (C) has 4 valence electrons (group 14 element).<\/li>\n\n\n\n
    • Chlorine (Cl) has 7 valence electrons (group 17 element), and there are three chlorines.<\/li>\n\n\n\n
    • Since this is a CCl\u2083\u207a<\/strong> ion, we subtract 1 electron due to the positive charge. So, the total number of valence electrons is:
      [
      4 + (3 \\times 7) – 1 = 4 + 21 – 1 = 24 \\text{ electrons}
      ]<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Arrange the atoms<\/strong>:
        Carbon (C) will be the central atom because it is less electronegative than chlorine (Cl).<\/li>\n\n\n\n
      2. Place single bonds<\/strong>:
        Draw single bonds between the carbon and each chlorine atom. Each single bond consists of 2 electrons, so 6 electrons are used (3 bonds \u00d7 2 electrons).<\/li>\n\n\n\n
      3. Distribute remaining electrons<\/strong>:
        After placing the bonds, 18 electrons remain. These will be placed as lone pairs on the chlorine atoms to complete their octet. Each chlorine will get 3 lone pairs (6 electrons per chlorine), filling their octets.<\/li>\n\n\n\n
      4. Account for the positive charge<\/strong>:
        The positive charge means that carbon has lost an electron. This can be reflected by reducing the number of electrons on carbon. This means carbon will only have 6 electrons in its valence shell after bonding (2 from each bond with chlorine), which results in a formal charge of +1 on the carbon atom.<\/li>\n<\/ol>\n\n\n\n

        Formal Charge Calculation on Carbon:<\/h3>\n\n\n\n

        The formal charge formula is:
        [
        \\text{Formal charge} = \\text{Valence electrons of C} – \\text{Nonbonding electrons} – \\frac{\\text{Bonding electrons}}{2}
        ]<\/p>\n\n\n\n

        For C:<\/p>\n\n\n\n

          \n
        • Valence electrons = 4<\/li>\n\n\n\n
        • Nonbonding electrons = 0<\/li>\n\n\n\n
        • Bonding electrons = 6 (from the 3 C-Cl bonds)<\/li>\n<\/ul>\n\n\n\n

          So:
          [
          \\text{Formal charge} = 4 – 0 – \\frac{6}{2} = 4 – 3 = +1
          ]<\/p>\n\n\n\n

          Thus, the formal charge on the carbon atom is +1.<\/p>\n\n\n\n

          The Best Lewis Structure:<\/h3>\n\n\n\n
            \n
          • The carbon is in the center with three single bonds to the chlorine atoms, and each chlorine has three lone pairs of electrons.<\/li>\n\n\n\n
          • The formal charge on the carbon is +1, and the chlorines have no formal charge.<\/li>\n<\/ul>\n\n\n\n

            I’ll generate the image of this structure for you.<\/p>\n\n\n\n

            Here is the Lewis structure for the CCl\u2083\u207a ion. The carbon atom is at the center with three chlorine atoms bonded to it. Each chlorine atom has three lone pairs, and the carbon atom carries a formal charge of +1.<\/p>\n\n\n\n

            Let me know if you’d like further details or modifications!<\/p>\n\n\n\n

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

            Draw the best lewis structure for CCl3 +1. What is the formal charge on the C? The Correct Answer and Explanation is : The molecular ion CCl\u2083\u207a consists of a carbon atom (C) bonded to three chlorine atoms (Cl). It carries a positive charge, meaning it has one less electron than a neutral molecule would […]<\/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-192251","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192251","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=192251"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/192251\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=192251"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=192251"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=192251"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}