Which of the following complexes involves $4p$ orbitals for hybridization?

Which of the following statements is not correct?

How many unpaired electrons are present in the cobalt ion in the $+3$ oxidation state prior to hybridization in the $[CoF_6]^{3-}$ complex ion?

For octahedral $Mn(II)$ and tetrahedral $Ni(II)$ complexes,consider the following statements:
$(I)$ Both the complexes can be high spin.
$(II)$ $Ni(II)$ complex can very rarely be low spin.
$(III)$ With strong field ligands,$Mn(II)$ complexes can be low spin.
$(IV)$ Aqueous solution of $Mn(II)$ ions is yellow in color.

Which of the following has a square planar geometry?
(At. nos.: $Fe=26, Co=27, Ni=28, Pt=78$)

Given below are two statements:
Statement $I$: $[Mn(CN)_6]^{3-}$,$[Fe(CN)_6]^{3-}$ and $[Co(C_2O_4)_3]^{3-}$ are $d^2sp^3$ hybridized.
Statement $II$: $[MnCl_6]^{3-}$ and $[FeF_6]^{3-}$ are paramagnetic and have $4$ and $5$ unpaired electrons,respectively.
In the light of the above statements,choose the correct answer from the options given below: