{"id":222328,"date":"2025-05-31T08:44:19","date_gmt":"2025-05-31T08:44:19","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=222328"},"modified":"2025-05-31T08:44:21","modified_gmt":"2025-05-31T08:44:21","slug":"which-of-the-following-is-not-a-characteristic-of-the-structure-of-benzene","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/31\/which-of-the-following-is-not-a-characteristic-of-the-structure-of-benzene\/","title":{"rendered":"Which of the following is not a characteristic of the structure of benzene"},"content":{"rendered":"\n

Which of the following is not a characteristic of the structure of benzene? O carbon atoms have trigonal planar geometry with bond angles of 120\u00c3\u201a\u00c2\u00b0 O carbon atoms are sp2 hybridized O planar, six-membered ring C-C bonds of equal length at 1.39 \u00c3\u0192\u00e2\u20ac\u00a6 O sp orbitals are responsible for the delocalized n bonding None<\/p>\n\n\n\n

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

Correct Answer: \u274c sp orbitals are responsible for the delocalized \u03c0 bonding<\/em><\/strong><\/p>\n\n\n\n

\n\n\n\n

Explanation <\/strong><\/h3>\n\n\n\n

Benzene (C\u2086H\u2086) is an aromatic hydrocarbon with a highly symmetrical and stable structure that has fascinated chemists for over a century. Let\u2019s analyze each option to identify the incorrect statement.<\/p>\n\n\n\n

    \n
  1. Carbon atoms have trigonal planar geometry with bond angles of 120\u00b0<\/strong>
    \u2705 True<\/strong>: Each carbon in benzene is bonded to two other carbon atoms and one hydrogen atom, forming three sigma (\u03c3) bonds in a trigonal planar arrangement. This leads to bond angles of approximately 120\u00b0, consistent with sp\u00b2 hybridization.<\/li>\n\n\n\n
  2. Carbon atoms are sp\u00b2 hybridized<\/strong>
    \u2705 True<\/strong>: In benzene, all carbon atoms use sp\u00b2 hybrid orbitals<\/em> to form sigma bonds with adjacent carbons and hydrogen atoms. The unhybridized p orbitals on each carbon overlap to form the delocalized \u03c0 system.<\/li>\n\n\n\n
  3. Planar, six-membered ring C\u2013C bonds of equal length at 1.39 \u00c5<\/strong>
    \u2705 True<\/strong>: X-ray diffraction studies have shown that all carbon\u2013carbon bonds in benzene are of equal length, approximately 1.39 \u00c5, intermediate between a typical single (1.54 \u00c5) and double bond (1.34 \u00c5). This uniformity is due to electron delocalization.<\/li>\n\n\n\n
  4. sp orbitals are responsible for the delocalized \u03c0 bonding<\/strong>
    \u274c False<\/strong>: This is the incorrect statement.<\/strong> The delocalized \u03c0 bonding<\/em> in benzene arises from the sideways overlap of unhybridized p orbitals<\/strong>, not sp orbitals<\/em>. The sp\u00b2 orbitals form \u03c3 bonds, while the remaining unhybridized 2p orbital on each carbon atom overlaps with adjacent 2p orbitals to create the \u03c0 system above and below the ring plane.<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

    Conclusion:<\/strong><\/h3>\n\n\n\n

    The mistaken statement is that \u201csp orbitals are responsible for the delocalized \u03c0 bonding.\u201d In reality, the \u03c0 bonding is due to unhybridized p orbitals<\/strong>, not the hybridized sp or sp\u00b2 orbitals. Thus, this choice is not<\/strong> a characteristic of benzene\u2019s structure.<\/p>\n\n\n\n

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

    Which of the following is not a characteristic of the structure of benzene? O carbon atoms have trigonal planar geometry with bond angles of 120\u00c3\u201a\u00c2\u00b0 O carbon atoms are sp2 hybridized O planar, six-membered ring C-C bonds of equal length at 1.39 \u00c3\u0192\u00e2\u20ac\u00a6 O sp orbitals are responsible for the delocalized n bonding None The […]<\/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-222328","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222328","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=222328"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222328\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=222328"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=222328"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=222328"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}