Identify the incorrect statement from the following :

Nitrogen and oxygen both belong to the second period of the periodic table.

The valence shell electronic configuration of nitrogen is $2s^{2} 2p^{3}$ and that of oxygen is $2s^{2} 2p^{4}$.

Since the principal quantum number is $n=2$ for both elements, they do not have vacant d-orbitals in their valence shells.

Therefore, nitrogen cannot form $d\pi$-$p\pi$ bonds with oxygen. They can only form $p\pi$-$p\pi$ multiple bonds.

Statement (1) is correct as nitrogen forms $p\pi$-$p\pi$ multiple bonds with itself (e.g., in $N_{2}$).

Statement (2) is correct because phosphorus and arsenic have vacant d-orbitals and can act as $\pi$-acceptor ligands, forming $d\pi$-$d\pi$ back-bonds with the filled d-orbitals of transition metals.

Statement (3) is correct as phosphorus, arsenic, and antimony exhibit the property of catenation.

Thus, the incorrect statement is (4).

Answer: Nitrogen can form $d\pi$-$p\pi$ bond with oxygen.