{"id":232455,"date":"2025-06-12T01:08:36","date_gmt":"2025-06-12T01:08:36","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=232455"},"modified":"2025-06-12T01:08:38","modified_gmt":"2025-06-12T01:08:38","slug":"what-is-the-hybridization-of-the-carbon-atoms-in-benzene-c6h6","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/12\/what-is-the-hybridization-of-the-carbon-atoms-in-benzene-c6h6\/","title":{"rendered":"What is the hybridization of the carbon atoms in benzene, C6H6"},"content":{"rendered":"\n

What is the hybridization of the carbon atoms in benzene, C6H6? a. sp b. sp2 c. sp3 d. sp3d<\/p>\n\n\n\n

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

Correct Answer: b. sp\u00b2<\/strong><\/p>\n\n\n\n

In benzene (C\u2086H\u2086), all six carbon atoms are sp\u00b2 hybridized<\/strong>. Benzene is a planar, cyclic molecule with a hexagonal ring structure. Each carbon atom in benzene is bonded to two other carbon atoms and one hydrogen atom, forming a total of three sigma (\u03c3) bonds.<\/p>\n\n\n\n

To form these three sigma bonds, each carbon atom uses three sp\u00b2 hybrid orbitals<\/strong>. The sp\u00b2 hybridization arises from mixing one s orbital<\/strong> and two p orbitals<\/strong> from the carbon atom, which results in three equivalent sp\u00b2 hybrid orbitals arranged in a trigonal planar geometry<\/strong> with 120\u00b0 bond angles<\/strong>. These hybrid orbitals form sigma bonds with adjacent carbon atoms and hydrogen atoms.<\/p>\n\n\n\n

The remaining unhybridized p orbital<\/strong> on each carbon atom lies perpendicular to the plane of the ring. These unhybridized p orbitals overlap sideways with adjacent p orbitals, forming a continuous system of pi (\u03c0) bonds<\/strong> above and below the plane of the ring. This delocalization of \u03c0 electrons across all six carbon atoms creates a resonance structure<\/strong>, which stabilizes the benzene ring and gives it unique chemical properties such as increased stability and uniform bond lengths between carbon atoms.<\/p>\n\n\n\n

All carbon-carbon bonds in benzene are of equal length (~1.39 \u00c5), which is intermediate between a single bond and a double bond. This uniformity is a direct result of the delocalized \u03c0 electron cloud and the sp\u00b2 hybridization of the carbon atoms.<\/p>\n\n\n\n

In summary, each carbon atom in benzene:<\/p>\n\n\n\n