The correct order of hybridisation of the central atom in the following species; ${\left[\mathrm{Ni}(\mathrm{CN}{)}_4\right]}^{2-},{\mathrm{XeO}}_4$ and ${\mathrm{SF}}_4$and ${\mathrm{NO}}_3^{-}$ is : 

The $\mathrm{Ni}(\mathrm{CN}{)}_4$ has the electrical configuration $3{\mathrm{d}}^{8}4\mathrm{s}0$ in the valence shell. All of the electrons are coupled up in the presence of CN- ions with a strong field. Through dsp2 hybridization, the empty 3d, 3s, and two 4p orbitals are created.
In order to create ${\mathrm{XeO}}_4$, xenon must go through sp3 hybridization in its fourth excited state. state of fourth excitement.
${\mathrm{SF}}_4$hybridises in an ${\mathrm{sp}}^3\mathrm{d}$ manner.
${\mathrm{NO}}^3-$ hybridization is of the ${\mathrm{sp}}_2$ kind.