Benzene exhibits resonance due to its unique structure, where carbon atoms are sp2 hybridized. Despite common misconceptions, benzene does not contain double bonds; instead, it features delocalized pi electrons that contribute to its aromaticity. The perpendicular arrangement of sp2 and p orbitals facilitates the resonance stabilization of benzene, allowing pi electrons to be effectively shared across the carbon framework. Understanding these orbital interactions is crucial for grasping the concept of aromatic compounds.
PREREQUISITESChemistry students, organic chemists, and educators seeking to deepen their understanding of aromatic compounds and resonance in molecular structures.
ajaysabarish said:the p orbital is involved in double bond
thank you for replying sir,but sir as far as i know,a pair of pi electrons get transferred to carbon orbitals the + and - charges form a bond.and it proceeds,iam asking how does the pi electron get transferred to carbon orbital,because the hybridized orbitals of carbon and pi orbital in which electrons are perpendicular.please replyBorek said:There are no double bonds in benzene.
Google "aromaticity".