Considering that the angles of a regular pentagon are 108º, why is cyclopentane not planar?

all the carbons are sp2 hybridized, so there is considerable angle strain.

The C-C bonds are formed by overlap of p-orbitals, so the 90º angle results in large angle strain.

The cyclic overlap of bonding orbitals results in anti-aromaticity destabilization

The five C-C bonds have eclipsing strain

Considering that the angles of a regular pentagon are 108º, why is cy

1.	Considering that the angles of a regular pentagon are 108º, why is cyclopentane not planar?
A.	all the carbons are sp2 hybridized, so there is considerable angle strain.
B.	The C-C bonds are formed by overlap of p-orbitals, so the 90º angle results in large angle strain.
C.	The cyclic overlap of bonding orbitals results in anti-aromaticity destabilization
D.	The five C-C bonds have eclipsing strain
Answer» E.