Step 1: Identify the central metal atom in the complex [Ni(CN)4]2-. The central atom is Nickel (Ni).
Step 2: Determine the oxidation state of Nickel in the complex. Since CN- is a -1 ligand and there are four CN- ligands, the oxidation state of Ni is +2.
Step 3: Write the electron configuration of Ni in its +2 oxidation state. Nickel has an atomic number of 28, so its electron configuration is [Ar] 3d8 4s2. In the +2 state, it loses 2 electrons from the 4s orbital, resulting in [Ar] 3d8.
Step 4: Count the number of ligands attached to the central metal atom. There are four CN- ligands in [Ni(CN)4]2-.
Step 5: Determine the geometry of the complex. With four ligands, the geometry is typically square planar for d8 metal complexes.
Step 6: Identify the type of hybridization that corresponds to square planar geometry. Square planar geometry corresponds to dsp2 hybridization.
