A) \[{{[Mn{{({{H}_{2}}O)}_{6}}]}^{2+}}\]
B) \[{{[Fe{{({{H}_{2}}O)}_{6}}]}^{2+}}\]
C) \[{{[Ni{{({{H}_{2}}O)}_{6}}]}^{2+}}\]
D) \[{{[Cr{{({{H}_{2}}O)}_{6}}]}^{2+}}\] (At. no. Cr = 24, Mn = 25, Fe = 26, Ni = 28)
Correct Answer: A
Solution :
As the number of unpaired electron increases, the magnetic moment increases and hence the paramagnetic behaviour increases. So, \[C{{r}^{2+}}(22)\,=3{{d}^{4}}\,-4\] unpaired electrons \[M{{n}^{2+}}(23)=3{{d}^{5}}-5\] unpaired electrons \[F{{e}^{2+}}(24)=3{{d}^{6}}\,-4\] unpaired electrons \[N{{i}^{2+}}(26)=3{{d}^{8}}-2\] unpaired electrons So, \[{{[Ni{{({{H}_{2}}O)}_{6}}]}^{2+}}\] exhibit minimum paramagnetic behaviour.
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