Question

\([NiCl_4]^{2-}\)

Hint:

Weak field ligands (like Cl$^-$) favor high spin configurations and tetrahedral geometry.

Answer 1

- Oxidation State of Ni: \[ x + 4(-1) = -2 \Rightarrow x = +2 \] Thus, Ni is in the \( +2 \) oxidation state. 
- Electronic Configuration of \( Ni^{2+} \): \[ [Ar] 3d^8 4s^0 \] 
- Nature of Ligand:
- Chloride \( Cl^- \) is a weak field ligand, so it does not cause strong pairing.
- The tetrahedral geometry is favored.
- Unpaired Electrons & Hybridization: 
- Hybridization: \( sp^3 \) 
- Unpaired electrons: 2
- Geometry: Tetrahedral