Given below are two statements: Statement (I): A solution of $$[Ni(H_2O)_6]^{2+}$$ is green in colour. Statement (II): A solution of $$[Ni(CN)_4]^{2-}$$ is colourless. In the light of the above statements, choose the most appropriate answer from the options given below:

The color of transition metal complexes depends on d-d transitions, which require unpaired electrons and an energy gap corresponding to visible light. Nickel(II) has a d⁸ electron configuration.

Statement (I): $$[Ni(H_2O)_6]^{2+}$$ is an octahedral complex with water, a weak field ligand. This results in a high-spin configuration with two unpaired electrons. The complex absorbs light in the red region and appears green, which is a known property. Thus, Statement (I) is correct.

Statement (II): $$[Ni(CN)_4]^{2-}$$ is a square planar complex with cyanide, a strong field ligand. The d⁸ configuration leads to all electrons being paired, so no d-d transitions occur. The complex is diamagnetic and appears colorless. Thus, Statement (II) is correct.

Both statements are correct, so the appropriate answer is option B.