Identify the incorrect statement from the following :

(D) Nitrogen can form \(d \pi-p \pi\) bond with oxygen.
Nitrogen and oxygen both belong to the second period of the periodic table.
The valence shell electronic configuration of nitrogen is \(2 s^2 2 p^3\) and that of oxygen is \(2 s^2 2 p^4\).
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).