What can be inferred from the magnetic moment values of the following complex species?Example Magnetic Moment (BM)K4[Mn(CN)6] 2.2[Fe(H2O)6]2+ 5.3K2[MnCl4] 5.9

The magnetic moment values of a complex species can give us information about the number of unpaired electrons in the species. This is because the magnetic moment is related to the number of unpaired electrons through the formula:

μ = √(n(n+2)) Bohr Magneton (BM)

where n is the number of unpaired electrons.

1. K4[Mn(CN)6] has a magnetic moment of 2.2 BM. This suggests that it has 1 unpaired electron. This is consistent with the fact that Mn in this complex is in the +2 oxidation state, which gives it a d5 configuration. One of these 5 electrons is unpaired.

2. [Fe(H2O)6]2+ has a magnetic moment of 5.3 BM. This suggests that it has 5 unpaired electrons. This is consistent with the fact that Fe in this complex is in the +2 oxidation state, which gives it a d6 configuration. Five of these 6 electrons are unpaired.

3. K2[MnCl4] has a magnetic moment of 5.9 BM. This suggests that it has 5 unpaired electrons. This is consistent with the fact that Mn in this complex is in the +2 oxidation state, which gives it a d5 configuration. All 5 of these electrons are unpaired.

In summary, the magnetic moment values of these complex species suggest that they have 1, 5, and 5 unpaired electrons respectively.