{"id":196610,"date":"2025-03-05T14:32:29","date_gmt":"2025-03-05T14:32:29","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=196610"},"modified":"2025-03-05T14:32:32","modified_gmt":"2025-03-05T14:32:32","slug":"when-a-carbon-atom-has-sp3-hybridization","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/05\/when-a-carbon-atom-has-sp3-hybridization\/","title":{"rendered":"When a carbon atom has sp3 hybridization"},"content":{"rendered":"\n

When a carbon atom has sp3 hybridization, it has
A. four \u03c0 bonds.<\/p>\n\n\n\n

B. three \u03c0 bonds and one \u03c3 bond.<\/p>\n\n\n\n

C. two \u03c0 bonds and two \u03c3 bonds.<\/p>\n\n\n\n

D. one \u03c0 bond and three \u03c3 bonds.<\/p>\n\n\n\n

E. four \u03c3 bonds.<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The correct answer is:<\/p>\n\n\n\n

E. four \u03c3 bonds.<\/strong><\/p>\n\n\n\n

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

Hybridization is the process by which atomic orbitals mix to form new hybrid orbitals that influence molecular bonding. The hybridization of a carbon atom depends on the number of regions of electron density (bonds or lone pairs) surrounding it.<\/p>\n\n\n\n

    \n
  1. Understanding sp\u00b3 Hybridization:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • Carbon has an atomic number of 6 and an electron configuration of 1s\u00b2 2s\u00b2 2p\u00b2<\/strong>.<\/li>\n\n\n\n
    • In its ground state, carbon has two unpaired electrons in the 2p orbitals, which would only allow it to form two bonds.<\/li>\n\n\n\n
    • To form four bonds (as in methane, CH\u2084), carbon undergoes sp\u00b3 hybridization<\/strong>, where one 2s orbital and three 2p orbitals mix to form four sp\u00b3 hybrid orbitals<\/strong>.<\/li>\n\n\n\n
    • Each hybrid orbital forms a \u03c3 (sigma) bond<\/strong>, leading to a tetrahedral geometry with bond angles of approximately 109.5\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Nature of Bonds in sp\u00b3 Hybridization:<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • Since all four hybrid orbitals are used for bonding, only sigma (\u03c3) bonds are present<\/strong>.<\/li>\n\n\n\n
        • \u03c0 (pi) bonds arise from unhybridized p orbitals overlapping sideways, but in sp\u00b3 hybridization, there are no unhybridized p orbitals left<\/strong>.<\/li>\n\n\n\n
        • Therefore, sp\u00b3 hybridized carbon forms only sigma bonds (\u03c3 bonds) and has no \u03c0 bonds<\/strong>.<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Examples of sp\u00b3 Hybridized Carbon Compounds:<\/strong><\/li>\n<\/ol>\n\n\n\n
              \n
            • Methane (CH\u2084)<\/strong> \u2013 Each C-H bond is a sigma bond.<\/li>\n\n\n\n
            • Ethane (C\u2082H\u2086)<\/strong> \u2013 Each C-H and C-C bond is a sigma bond.<\/li>\n\n\n\n
            • Tetrahedral geometry is a characteristic of sp\u00b3 hybridization.<\/strong><\/li>\n<\/ul>\n\n\n\n

              Image Representation:<\/h3>\n\n\n\n

              I will generate an image showing the sp\u00b3 hybridization of carbon, tetrahedral shape, and sigma bonds<\/strong>.<\/p>\n\n\n\n

              \"\"<\/figure>\n\n\n\n

              Here is an image illustrating the sp\u00b3 hybridization<\/strong> of a carbon atom, showing the tetrahedral geometry and sigma (\u03c3) bonds.<\/p>\n","protected":false},"excerpt":{"rendered":"

              When a carbon atom has sp3 hybridization, it hasA. four \u03c0 bonds. B. three \u03c0 bonds and one \u03c3 bond. C. two \u03c0 bonds and two \u03c3 bonds. D. one \u03c0 bond and three \u03c3 bonds. E. four \u03c3 bonds. The correct answer and explanation is : The correct answer is: E. four \u03c3 bonds. […]<\/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-196610","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196610","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=196610"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196610\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=196610"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=196610"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=196610"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}