Column - I Complex		Column - II Hybidisation
a)	$\left[\mathrm{Ni}{\left(CO\right)}_4\right]$	p)	sp3
b)	${\left[\mathrm{Ni}(\mathrm{CN}{)}_4\right]}^{2-}$	q)	dsp2
c)	${\left[\mathrm{Fe}(\mathrm{CN}{)}_6\right]}^{4-}$	r)	sp3d2
d)	${\left[{\mathrm{MnF}}_6\right]}^{-4}$	s)	d2sp3

In $\mathrm{Ni}{\left(\mathrm{CO}\right)}_4$, Ni has zero oxidation state and its outer electronic configuration is $3{\mathrm{d}}^{8}4{\mathrm{s}}^2.$ As CO is a strong ligand, so all 3d and 4s electrons are paired and complex shows sp³ hybridization.

In ${\left[\mathrm{Ni}{\left(\mathrm{CN}\right)}_4\right]}^{2-}$, Ni has +2 oxidation state and its outer electronic configuration is $3{\mathrm{d}}^{8}4{\mathrm{s}}^0.$ As CN is a strong ligand so all 3d electrons are paired and complex shows dsp² hybridization.

In ${\left[\mathrm{Fe}{\left(\mathrm{CN}\right)}_6\right]}^{4-}$, Fe has +2 oxidation state and its outer electronic configuration is $3{\mathrm{d}}^{6}4{\mathrm{s}}^0.$ As CN is a strong ligand, so all 3d electrons are paired and complex shows d²sp³ hybridization.

In ${\left[{\mathrm{MnF}}_6\right]}^{4-}$, Mn has +2 oxidation state and its outer electronic configuration is $3{\mathrm{d}}^{5}4{\mathrm{s}}^0.$ As F is a weak ligand, so 3d electrons remain unpaired and complex shows sp³d² hybridization.