Question

What is the hybridisation of \([Ni(CN)_4]^{2-}\)?

• A. sp\(^3\)
• B. sp\(^2\)d
• C. dsp\(^2\)
• D. sp\(^3\)d

Hint:

Square planar complexes typically exhibit dsp\(^2\) hybridization and are commonly seen in metal complexes involving transition metals such as nickel, platinum, and palladium.

Answer 1

The Correct Option is C

The complex \([Ni(CN)_4]^{2-}\) involves nickel (Ni) in the +2 oxidation state and is coordinated to four cyanide (CN\(^-\)) ligands. The central metal ion, Ni\(^{2+}\), has an electron configuration of \( [Ar]\,3d^8 \,4s^0 \). When four cyanide ions coordinate with the metal, the metal undergoes hybridization to accommodate the bonding with the ligands. Since the complex has a square planar geometry, the hybridization of the central metal ion is \(dsp^2\),
where:
The d orbitals from the metal ion mix with the s and p orbitals to form four hybrid orbitals that will align in a square planar shape.
This hybridization is typical of coordination complexes where the metal is in a +2 oxidation state, especially for transition metals like nickel.

Thus, the correct hybridization for \([Ni(CN)_4]^{2-}\) is \(dsp^2\), which leads to the square planar geometry.