Explanation:

In order to determine the hybrid orbitals at carbon 2 and 3 in the compound CH3CH=CHCH3, we need to first identify the hybridization state of each carbon atom.

Carbon 2:
- Carbon 2 is bonded to three hydrogen atoms and one carbon atom.
- The carbon atom is connected to another carbon atom through a double bond.
- Since carbon 2 is bonded to four atoms in total, it undergoes sp2 hybridization.

Carbon 3:
- Carbon 3 is bonded to two hydrogen atoms and one carbon atom.
- The carbon atom is connected to another carbon atom through a double bond and a single bond.
- Since carbon 3 is bonded to three atoms in total, it undergoes sp2 hybridization.

Hybrid Orbitals:
- The sp2 hybridization of carbon 2 and carbon 3 means that each carbon atom will have three sp2 hybrid orbitals and one unhybridized p orbital.
- The three sp2 hybrid orbitals will be used to form sigma bonds with the three atoms bonded to carbon 2 and carbon 3 (hydrogen atoms and the other carbon atom).
- The unhybridized p orbital will be involved in the formation of the pi bond between the carbon atoms.

Summary:
In the compound CH3CH=CHCH3, carbon 2 and carbon 3 are sp2 hybridized. Carbon 2 and carbon 3 each have three sp2 hybrid orbitals and one unhybridized p orbital. The sp2 hybrid orbitals form sigma bonds with the atoms bonded to carbon 2 and carbon 3, while the unhybridized p orbital forms a pi bond between the carbon atoms.