Which of the following are paramagnetic? Choose the correct answer from the options given below: [2025]

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Solution

Q.
Which of the following are paramagnetic

A. ${[{NiCl}_{4}]}^{2 -}$
B. ${Ni(CO)}_{4}$
C. ${[{Ni(CN)}_{4}]}^{2 -}$
D. ${[{Ni(H}_{2} {O)}_{6}]}^{2 +}$
E. $Ni({PPh}_{3})_{4}$

Choose the correct answer from the options given below: [2025]

1 A and D only

2 A, D and E only

3 A and C only

4 B and E only

Ans.
(1)

A) In ${[{NiCl}_{4}]}^{2 -}$ , there are two unpaired electrons because ${Cl}^{-}$ is a weak field ligand. Therefore, it is paramagnetic in nature.

B) In $[Ni {(CO)}_{4}]$

${Ni}^{0} (Z = 28) : 3 d^{8} 4 s^{2}$

Since CO is a strong field ligand, it forces electrons to pair up. Therefore, it is diamagnetic in nature.

C) In ${[Ni {(CN)}_{4}]}^{2 -}$ , there is no unpaired electron because ${CN}^{-}$ is a strong field ligand. Therefore, it is diamagnetic in nature.

D) Oxidation state of Ni in ${[Ni {(H_{2} O)}_{6}]}^{2 +} = + 2$

${Ni}^{2 +} (Z = 28) : 3 d^{8}$

$H_{2} O$ is a weak field ligand hence pairing of electrons does not take place and compound is paramagnetic on account of two unpaired electrons.

E) In $[Ni {({PPh}_{3})}_{4}]$ , oxidation state of Ni = 0

It is diamagnetic in nature.

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