{"id":160530,"date":"2024-11-03T06:15:37","date_gmt":"2024-11-03T06:15:37","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=160530"},"modified":"2024-11-03T06:15:40","modified_gmt":"2024-11-03T06:15:40","slug":"draw-the-lewis-structure-for-hcch-ethyne","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/03\/draw-the-lewis-structure-for-hcch-ethyne\/","title":{"rendered":"Draw the Lewis structure for HCCH (ethyne)."},"content":{"rendered":"\n

Draw the Lewis structure for HCCH (ethyne). – Draw the molecule by placing atoms on the grid and connecting them with bonds. – Include all hydrogen atoms and all lone pairs of electrons. Submit your answer.<\/p>\n\n\n\n

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

To draw the Lewis structure for ethyne (HCCH)<\/strong>, also known as acetylene<\/strong>, we need to determine the arrangement of the atoms and bonds. Ethyne has the molecular formula C\u2082H\u2082<\/strong>. Here’s the step-by-step structure and explanation:<\/p>\n\n\n\n

Step 1: Count the Total Valence Electrons<\/h3>\n\n\n\n
    \n
  • Carbon (C) has 4 valence electrons<\/strong>, and there are 2 carbon atoms<\/strong> in the molecule: 4 x 2 = 8 electrons.<\/li>\n\n\n\n
  • Hydrogen (H) has 1 valence electron<\/strong>, and there are 2 hydrogen atoms<\/strong>: 1 x 2 = 2 electrons.<\/li>\n\n\n\n
  • Total valence electrons = 8 + 2 = 10 valence electrons<\/strong>.<\/li>\n<\/ul>\n\n\n\n

    Step 2: Arrange the Atoms<\/h3>\n\n\n\n

    The structure of ethyne is linear<\/strong> with hydrogen atoms bonded to each carbon, and the carbons are bonded to each other. Arrange the atoms in this order: H\u2013C\u2261C\u2013H.<\/p>\n\n\n\n

    Step 3: Connect Atoms with Bonds<\/h3>\n\n\n\n
      \n
    • Place a single bond<\/strong> between each hydrogen and carbon atom (H\u2013C).<\/li>\n\n\n\n
    • Place a triple bond<\/strong> between the two carbon atoms (C\u2261C).<\/li>\n<\/ul>\n\n\n\n

      Step 4: Distribute Remaining Electrons<\/h3>\n\n\n\n

      Each hydrogen is satisfied with 2 electrons<\/strong> (a single bond with carbon), and each carbon needs 8 electrons<\/strong> in total to satisfy the octet rule:<\/p>\n\n\n\n

        \n
      • Each C\u2013H bond has 2 electrons (1 bond).<\/li>\n\n\n\n
      • Each C\u2261C triple bond has 6 electrons (3 bonds).<\/li>\n<\/ul>\n\n\n\n

        Step 5: Verify Octet Rule and Electron Count<\/h3>\n\n\n\n

        Each carbon has 8 electrons<\/strong> (6 from the C\u2261C triple bond and 2 from the C\u2013H bond). Hydrogens are satisfied with 2 electrons each.<\/p>\n\n\n\n

        Final Structure<\/h3>\n\n\n\n

        The Lewis structure for HCCH (ethyne)<\/strong> is:<\/p>\n\n\n\n

        H\u2013C\u2261C\u2013H<\/code><\/pre>\n\n\n\n
        This structure has:<\/p>\n\n\n\n
          \n
        • No lone pairs<\/strong> on any atom.<\/li>\n\n\n\n
        • Triple bond<\/strong> between the two carbons.<\/li>\n\n\n\n
        • Single bond<\/strong> between each carbon and hydrogen.<\/li>\n<\/ul>\n\n\n\n
          Explanation<\/h3>\n\n\n\n
          In ethyne, each carbon forms three bonds with the other carbon (a triple bond) and a single bond with one hydrogen atom. This gives each carbon atom an sp hybridization<\/strong>, creating a linear shape with a bond angle of 180\u00b0<\/strong>. Triple bonds consist of one sigma (\u03c3) bond<\/strong> and two pi (\u03c0) bonds<\/strong>. The pi bonds arise from the sideways overlap of p orbitals, while the sigma bond is a direct overlap along the internuclear axis.<\/p>\n\n\n\n
          The lack of lone pairs in the structure and the triple bond give ethyne unique properties, such as a high bond dissociation energy and a short C\u2261C bond length. Ethyne is also a relatively small molecule and is commonly used as a fuel in welding due to the high-energy bonds between carbon atoms.<\/p>\n","protected":false},"excerpt":{"rendered":"
          Draw the Lewis structure for HCCH (ethyne). – Draw the molecule by placing atoms on the grid and connecting them with bonds. – Include all hydrogen atoms and all lone pairs of electrons. Submit your answer. The Correct Answer and Explanation is: To draw the Lewis structure for ethyne (HCCH), also known as acetylene, we […]<\/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-160530","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/160530","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=160530"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/160530\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=160530"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=160530"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=160530"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}