Question:
Regarding magnetic properties of the complexes \(Ni(CO)_4\) [I], \(NiCl_4^{2-}\) [II], which of the following is correct?
Regarding magnetic properties of the complexes \(Ni(CO)_4\) [I], \(NiCl_4^{2-}\) [II], which of the following is correct?
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Strong field ligands (like CO) cause electron pairing → diamagnetism; weak field ligands (like Cl⁻) often give paramagnetism.
Updated On: Jun 19, 2026
- I = Diamagnetic, II = Paramagnetic
- I = Paramagnetic, II = Paramagnetic
- I = Diamagnetic, II = Diamagnetic
- I = Paramagnetic, II = Diamagnetic
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The Correct Option is A
Solution and Explanation
Step 1: Determining oxidation state and electron count of Ni.
In \(Ni(CO)_4\), CO is a neutral ligand, so Ni is in oxidation state 0 with 10 valence electrons. In \(NiCl_4^{2-}\), each Cl is \(-1\), so Ni is in +2 oxidation state with \(d^8\) configuration.
Step 2: Nature of ligand field in \(Ni(CO)_4\).
CO is a strong field ligand, causing pairing of electrons. Ni(0) adopts \(sp^3\) hybridization with all electrons paired, making it diamagnetic.
Step 3: Nature of \(NiCl_4^{2-}\).
Cl⁻ is a weak field ligand, so it does not cause pairing. The complex is tetrahedral with \(d^8\) configuration having unpaired electrons, hence paramagnetic.
Step 4: Magnetic behavior conclusion.
Thus: - \(Ni(CO)_4\): diamagnetic - \(NiCl_4^{2-}\): paramagnetic
Step 5: Final verification.
This matches ligand field theory and observed magnetic behavior of Ni complexes.
Final Answer: \[ \boxed{\text{I = Diamagnetic, II = Paramagnetic}} \]
In \(Ni(CO)_4\), CO is a neutral ligand, so Ni is in oxidation state 0 with 10 valence electrons. In \(NiCl_4^{2-}\), each Cl is \(-1\), so Ni is in +2 oxidation state with \(d^8\) configuration.
Step 2: Nature of ligand field in \(Ni(CO)_4\).
CO is a strong field ligand, causing pairing of electrons. Ni(0) adopts \(sp^3\) hybridization with all electrons paired, making it diamagnetic.
Step 3: Nature of \(NiCl_4^{2-}\).
Cl⁻ is a weak field ligand, so it does not cause pairing. The complex is tetrahedral with \(d^8\) configuration having unpaired electrons, hence paramagnetic.
Step 4: Magnetic behavior conclusion.
Thus: - \(Ni(CO)_4\): diamagnetic - \(NiCl_4^{2-}\): paramagnetic
Step 5: Final verification.
This matches ligand field theory and observed magnetic behavior of Ni complexes.
Final Answer: \[ \boxed{\text{I = Diamagnetic, II = Paramagnetic}} \]
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