Which compound is known for its presence in various oxidation states and is used in redox reactions?

Permanganate is known for its variety of oxidation states, particularly in the case of manganese, which can exist from -3 to +7. The permanganate ion most commonly encountered is MnO₄⁻, where manganese is in the +7 oxidation state. This high oxidation state makes permanganate a strong oxidizing agent in redox reactions. It can easily gain electrons, allowing it to participate effectively in reactions where it reduces to lower oxidation states, such as in Mn²⁺ or MnO₂.

The versatility of permanganate in undergoing redox reactions is significant in various chemical processes, not limited to organic synthesis but also including analytical chemistry and environmental applications.

Other compounds, such as nitrate, phosphate, and oxalate, do not exhibit the same range of oxidation states. Nitrate primarily involves nitrogen in the +5 oxidation state, phosphate contains phosphorus in a +5 oxidation state, and oxalate is typically associated with carbon in a +3 state. This limited oxidation state range restricts their use as oxidizing agents compared to permanganate. Thus, permanganate stands out as a compound notable for its capability to exist in multiple oxidation states and its role in redox chemistry.