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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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Solution

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.

Cr3+

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.

Ni2+:

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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APPEARS IN

NCERT Class 12 Chemistry Textbook
Chapter 9 Coordinate Compounds
Q 19 | Page 259
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