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| 1. |
Magnetic moment of [MnCl_(4)]^(2-) is 5.92 BM. Explain giving reason |
| Answer» Solution :`mu=sqrt(N(n+2))BM, mu=5.92` BM means n=5, i.e., 5 unpaired ELECTRONS. `Mn^(2+)=3d^(5)4S^(0)4p^(0)`. To form `[MnCl_(4)]^(2-)`, HYBRIDISATION will be `sp^(3)`. Hence, the structure will be tetrahedral. | |