Starting with the orbital diagram of a boron atom, EXPLAIN the steps needed to construct hybrid orbitals which describes the bonding in BH3?

Here's what I get  

Explanation:

1. Are there any polar bonds?

Check the electronegativity difference (ΔEN) between the atoms in each bond. If ΔEN < 0.5, the bond is nonpolar.

(a) If all bonds are nonpolar, the molecule is nonpolar

(b) If one bond is polar, the molecule is polar

2. Do the bond dipoles cancel?

If there is more than one polar bond, the bond dipoles may cancel.

(a) If the molecular geometry makes the bond dipoles cancel, the molecule will be nonpolar.

(b) If the bond dipoles do not cancel, the molecule will be polar.

the answer is c

tell me if wrong