Question

Manganese (VI) has ability to disproportionate in acidic solution. The difference in oxidation states of two ions it forms in acidic solution is _____.

Answer 1

Correct Answer: 3

To determine the difference in oxidation states when Manganese (VI) disproportionates in an acidic solution, we start by identifying the chemical reaction involved. Disproportionation is a redox reaction where a substance simultaneously undergoes oxidation and reduction. For Manganese (VI), represented as Mn^VIO₄²⁻, in acidic solution, it typically disproportionates into Mn^II and Mn^VII species.

The reaction can be written as:

3MnO₄²⁻ + 4H⁺ → 2MnO₄⁻ + MnO₂ + 2H₂O

Here's the analysis of oxidation states:

1. Initially, in MnO₄²⁻, Manganese has an oxidation state of +6.
2. In MnO₄⁻, Manganese is in the +7 oxidation state.
3. In MnO₂, Manganese is in the +4 oxidation state.

Thus, when Mn^VIO₄²⁻ disproportionates, the two resulting ions have oxidation states of +7 and +4. Therefore, the difference in oxidation states is calculated as:

Difference = 7 - 4 = 3

This value (3) falls within the specified range of 3,3, confirming the expected result.