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The hybridization of Ni in [Ni(CN)₄]²⁻ is:

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1. **Ni²⁺ configuration**: Nickel ($Z=28$) is $[Ar] 3d^8 4s^2$. Ni²⁺ is $[Ar] 3d^8$.
2. **Ligand Influence**: $CN^-$ is a **strong field ligand**. According to Valence Bond Theory, it causes the pairing of the two unpaired electrons in the $3d$ shell.
3. **Hybridization**: Pairing clears one $3d$ orbital. The metal uses $1$ inner $3d$ orbital, $1$ $4s$ orbital, and $2$ $4p$ orbitals for bonding.
- Hybridization: **$dsp^2$**.
- Geometry: **Square Planar**.
- The complex is **diamagnetic** (no unpaired electrons).

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