The lobes of which orbital(s) lies in the nodal plane of $d{z}^2$ :

The lobes of orbital(s) does not lie in the nodal plane of $d{z}^2$ is, $d_{x^2-y^2}$$d_{xy}$$d_{xy}$

Nodal planes of the orbital plane $d{z}^2$:

Azimuthal quantum number, or “$\text{ l }$”, has a value of 2 for the d orbital. Thus, the primary quantum number n has a minimum value of 3. It is not possible for $\text{ l }$ to exceed $\mathrm{n}-1$ in value.

Therefore, the $d{z}^2$ orbital lacks a nodal plane.

Hence, option D is correct.