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Question

Consider following complexes :

I: [Fe(H2O)6]2+
II :[Fe(CN)6]4−
III :[Ni(CO)4]
IV :[Ni(H2O)4]2+
V :[Ni(CN)4]2−

Out of this, select the complex with equal magnetic moment :

A
[Fe(CN)6]4 and [Ni(CN)4]2
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B
[Ni(CO)4] and [Fe(CN)6]4
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C
[Ni(H2O)4]2+ and [Ni(CO)4]
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D
None of these
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Solution

The correct option is D None of these
[Fe(H2O)6]2+

Fe is in +2 state in above compound as H2O don't have any charge on it.

Fe2+[Ar]3d6

There are four unpaired electrons in 3d orbital as H2O is a weak ligand.

Magnetic Moment- n(n+2)- 24 BM

[Fe(CN)6]4
x6=4
x=+2

Fe is in +2 state in above compound.

Fe2+[Ar]3d6

There is no unpaired electron because CN is a strong field ligand and paired the electrons due to high energy difference between t2g level and eg level.

Magnetic Moment = 0

[Ni(H2O)4]2+

Ni is in +2 state in above compound as H2O is neutral.

Ni2+[Ar]3d8

There are two unpaired electron in eg level.

Magnetic Moment- n(n+2)- 8 BM

[Ni(CN)4]2
x4=2
x=+2

Ni is in +2 state in above compound.

Ni2+[Ar]3d8

There are two unpaired electron in eg level.

Magnetic Moment- n(n+2)- 8 BM

Therefore, option D is correct.

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