Chemistry - Coordination Chemistry Question with Solution | TestHub

$[Ni(en{)}_3{]}^{2+}$: $N{i}^{2+}$ is $d^8$; even with strong ligands, it must use outer $4d$ orbitals, resulting in $s{p}^3{d}^2$ hybridization.

$[Ni{F}_6{]}^{2-}$: $N{i}^{4+}$ is $d^6$ and $F^{-}$ acts as a strong field ligand in higher oxidation states, causing pairing to create two vacant $3d$ orbitals for $d^{2}s{p}^3$ hybridization.

$[Ni{F}_6{]}^{4-}$: $N{i}^{2+}$ is $d^8$ with weak field $F^{-}$, leading to an outer orbital $s{p}^3{d}^2$ configuration.

$[PtC{l}_6{]}^{2-}$: $P{t}^{4+}$ is $5d^6$; for $4d$ and $5d$ series metals, all ligands cause pairing, creating an inner orbital $d^{2}s{p}^3$ complex.