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[Cr(NH3)6]3+ Is Paramagnetic While [Ni(CN)4]2− Is Diamagnetic. Explain Why? - Chemistry

[Cr(NH3)6]3+ is paramagnetic while [Ni(CN)4]2− is diamagnetic. Explain why?

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Cr is in the +3 oxidation state i.e., d3 configuration. Also, NH3 is a weak field ligand that does not cause the pairing of the electrons in the 3d orbital.


Therefore, it undergoes d2sp3 hybridization and the electrons in the 3d orbitals remain unpaired. Hence, it is paramagnetic in nature.

In [Ni(CN)4]2−, Ni exists in the +2 oxidation state i.e., d8 configuration.


CN− is a strong field ligand. It causes the pairing of the 3d orbital electrons. Then, Ni2+ undergoes dsp2hybridization.

As there are no unpaired electrons, it is diamagnetic.

Concept: Bonding in Coordination Compounds - Magnetic Properties of Coordination Compounds
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NCERT Class 12 Chemistry Textbook
Chapter 9 Coordinate Compounds
Q 19 | Page 259
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