Complete the exercises below. Select the more acidic member of each of the following pairs: a. Mn₂O₇ and MnO₂, b. SnO and SnO₂, c. SO₂ and SO₃, d. SiO₂ and SO₂, e. Ga₂O₃ and In₂O₃, f. SO₂ and SeO₂.

The acidity of oxides is determined by their ability to react with water to form acids. Generally, non-metal oxides are more acidic, while metal oxides tend to be basic. The oxidation state of the metal in the oxide also plays a crucial role; higher oxidation states typically correlate with greater acidity due to increased electronegativity and the ability to stabilize negative charges.

Oxidation states indicate the degree of oxidation of an atom in a compound. In the context of oxides, elements in higher oxidation states often form more acidic oxides. For example, in the pair Mn₂O₇ and MnO₂, Mn in Mn₂O₇ has a higher oxidation state (+7) compared to Mn in MnO₂ (+4), making Mn₂O₇ more acidic.

Comparative acidity involves evaluating the relative strengths of acids or acidic oxides. This can be assessed through their ability to donate protons or form acidic solutions in water. Understanding the trends in acidity among different oxides, such as the transition from basic to acidic as you move from left to right across the periodic table, is essential for determining which oxide is more acidic in a given pair.