Statement I: \(Ni(CO)_4\) is diamagnetic in nature

Statement II: Nickel atom undergoes sp³ hybridization

Both Statement I and statement II are true but statement II is not the correct explanation for statement I

The correct answer is: 2. Both Statement I and Statement II are true, but Statement II is not the correct explanation for Statement I.

Statement I: \(Ni(CO)_4\) is diamagnetic in nature.

Statement II: Nickel atom undergoes sp3 hybridization.

Both statements are true:

Statement I is true. \(Ni(CO)_4\) is indeed diamagnetic. In this complex, nickel (Ni) has a \(3d^8\) electronic configuration, which means all the 3d orbitals are completely filled with electrons, resulting in no unpaired electrons. Therefore, the complex is diamagnetic.

Statement II is also true. In forming the \(Ni(CO)_4\) complex, the nickel atom undergoes sp3 hybridization. Hybridization involves the mixing of one 3s orbital and three 3p orbitals to form four equivalent sp3 hybrid orbitals. These hybrid orbitals then overlap with the CO ligands to form sigma bonds.

However, Statement II is not the correct explanation for why \(Ni(CO)_4\) is diamagnetic. The diamagnetic nature of \(Ni(CO)_4\) is due to the electronic configuration of nickel in the complex (\(3d^8\)), which results in all 3d orbitals being fully occupied, and not due to its sp3 hybridization.