The total number of hybrid orbitals present in benzene is
Answers
Explanation:
Each carbon atom has 3 regions of electron density (the shape is a trigonal planar). The carbon forms 2 single bonds and 1 double bond. Each single bonds form 1 sigma bonds and the double bond forms one sigma bond and one double bond (total of 3 sigma and 1 pi).
The hybridized orbitals are the 2sp2 orbitals that form the sigma bonds (2 for the single and one for the double) as mentioned above.
The unhybridized orbital is the 2p orbital that is associated with the pi bond of the double bond. And yes, this unhybridized orbital is the one that lies perpendicular to the benzene ring. Since there are 6 carbon atoms (each contributing 1 electron in the unhybridized p orbital), then there are a total of six perpendicular 2p orbitals in each benzene ring.