At $$25^\circ C$$, nitrogen exists as $$N_2$$ and phosphorous exists as $$P_4$$ because

A

$$N_2$$ has valence electrons only in bonding and nonbonding orbitals, while P has valence electrons in both bonding and antibonding orbitals

B

higher electronegativity of N favours formation of multiple bonds

C

bigger size of P does not favour multiple bonds

D

P has preference to adapt structures with small bond angles