MnO4 - is a stronger oxidizing agent than ReO4 - . Both ions have charge-transfer (LMCT) bands; however, the charge-transfer band for ReO4 - is in the ultraviolet, whereas the corresponding band for MnO4 - is responsible for its intensely purple color. Are the relative positions of the charge-transfer absorptions consistent with the oxidizing abilities of these ions? Explain

 is a strong oxidizing agent.

Explanation:

The 5d orbitals of Re are higher in energy than 3 d orbitals of Mn. So an LMCT ligand to metal charge transfer excitation requires more energy of .

Also, since the molecular orbitals are derived primarily from  3d orbitals of are lower in energy than the corresponding MO's of   ,  is better able to accept the electrons.

So it is a better oxidizing agent.

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