To analyze the problem, we consider two properties:
- Ligand-to-Metal Charge Transfer (LMCT): LMCT occurs when there is a transfer of electrons from the ligand (oxygen) to the metal ion (Mn or Cr) due to a significant energy difference between the ligand and metal orbitals.
- Paramagnetism: Paramagnetic species have unpaired electrons in their electronic configuration.
Analysis of the given species:
- MnO−4 (Permanganate ion): In MnO−4, Mn is in the +7 oxidation state with no unpaired electrons (electronic configuration: 3d0). This species shows LMCT but is diamagnetic.
- MnO2−4 (Manganate ion): In MnO2−4, Mn is in the +6 oxidation state with one unpaired electron (electronic configuration: 3d1). This species exhibits both LMCT and paramagnetism.
- Cr2O2−7 (Dichromate ion): In Cr2O2−7, Cr is in the +6 oxidation state with no unpaired electrons (electronic configuration: 3d0). This species is diamagnetic and shows LMCT.
- CrO2−4 (Chromate ion): In CrO2−4, Cr is also in the +6 oxidation state with no unpaired electrons. This species shows LMCT but is diamagnetic.
Conclusion: Among the given options, only MnO2−4 exhibits both LMCT and paramagnetism due to the presence of one unpaired electron and the ability of oxygen ligands to transfer charge to Mn. Therefore, the correct answer is: 2. MnO2−4.