What is the change in oxidation number of manganes in the reaction represented by the following equation? MnO-4(aq) + 8H+(aq) + 5e- → Mn2+(aq) + 4H2O(l)

In the given redox reaction, the oxidation state of manganese (Mn) changes from +7 in MnO₄^- to +2 in Mn²⁺. Therefore, the change in oxidation state of manganese is from +7 to +2. The oxidation state is the hypothetical charge that an atom would have if all bonds to atoms of different elements were completely ionic. When an element undergoes oxidation, its oxidation state increases, and when it undergoes reduction, its oxidation state decreases. In this reaction, manganese is undergoing reduction since its oxidation state is decreasing from +7 to +2, which means it is gaining electrons.