Question

Match each complex to its geometry:

Hint:

Square planar geometry is typically seen with strong field ligands like cyanide, while tetrahedral geometry is common with weak field ligands like chloride.

Answer 1

Step 1: Understanding the geometries.
- \([Ni(CN)_4]^{2-}\) typically forms a square planar geometry due to the strong field ligand \( \text{CN}^- \), which causes the d-orbitals to undergo pairing and leads to a square planar arrangement.
- \([NiCl_4]^{2-}\) generally forms a tetrahedral geometry because chloride ions are weaker field ligands, which do not cause significant pairing of d-electrons.
Step 2: Conclusion.
Thus, \([Ni(CN)_4]^{2-}\) has square planar geometry and \([NiCl_4]^{2-}\) has tetrahedral geometry.