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  • The magnetic moment (spin only) of <img alt="\mathrm{ \left [ NiCl_{4} \right ]^{2-}}" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cmathrm%7B%20%5Cleft%20%5B%20NiCl_%7B4%7D%20%5Cright%20

The magnetic moment (spin only) of \mathrm{ \left [ NiCl_{4} \right ]^{2-}} is

Option: 1

1.82 BM


Option: 2

5.46 BM


Option: 3

2.83 BM


Option: 4

1.41 BM


Answers (1)

best_answer

As we discussed in the concept

Magnetic Moments (spin only)  is given as 

\mu=\sqrt{n\left ( n+2 \right )} where n= number of unpaired electron.

 

Number of unpaired electrons and corresponding magnetic moments

\\ 1\rightarrow 1.7\\2\rightarrow 2.8\\3\rightarrow 3.9\\4\rightarrow 4.9\\5\rightarrow 5.9

Now, 

 In \mathrm{\left [ NiCl_{4} \right ]^{2-},\ Ni^{2+}} is found with weak field ligand \mathrm{Cl^-} which does not cause pairing, the \mathrm{[Ar]3d^8} configuration of \mathrm{Ni^{2+}} has two unpaired electrons

Thus, magnetic moment \mathrm{\mu = \sqrt{2(2+2)}=2.82\ BM}

Therefore, option (3) is correct.

Posted by

seema garhwal

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