Ampholytes behave as bases towards strong acids but as acids towards strong bases. Therefore, it is understandable that they lie between the strong acids and bases and are also capable of both donating and accepting protons - do my assignment . Typical amphoteric compounds or ions are therefore found among the weak bases and acids.
In addition, the oxides of the lighter elements of the II. and III. main groups as well as the heavier elements of the IV. and V. main groups are also amphoteres. main group as well as the heavier elements of the IV. and V. main group are amphoteric - do my math homework for me . For example, Al2O3 that is not heated too high reacts with both strong acids and strong bases:
Al2O3 + 6 H3O^+ + 3 H2O ⇌ 2 [Al(H2O)6]3+Al2O3 + 2 OH- + 3 H2O ⇌ 2 [Al(OH)4]-.
In the first case, aluminium oxide reacts as a base with the absorption of protons and forms the corresponding acid [Al(H2O)6]3+. In the second case, aluminium oxide reacts as an acid to form the corresponding base [Al(OH)4]-. In the neutral range, pH ≈ 7, these oxides are usually very difficult to dissolve, but dissolve in both acidic and basic environments with the formation of their hydrated cation complexes or formation of their anionic hydroxometalates - statistics homework help . The other amphoteric element oxides react in the same way. These separate the strongly basic oxides, which are formed by the electropositive elements on the left side of the PSE, and the markedly acidic oxides, which are formed by the more electronegative elements on the right side of the PSE.