Oxides and Hydroxides
An early classification of substances arose from the differences observed in their solubility in acidic and basic solutions. This led to the classification of oxides and hydroxides as being either acidic or basic. Acidic oxides or hydroxides either reacted with water to produce an acidic solution or were soluble in aqueous base. Basic oxides and hydroxides either reacted with water to produce a basic solution or readily dissolved in aqueous acids. The diagram below shows there is strong correlation between the acidic or basic character of oxides (ExOy) and the position of the element, E, in the periodic table.
Oxides of metallic elements are generally basic oxides, and oxides of nonmetallic elements acidic oxides. Take for example, the reactions with water of calcium oxide, a metallic oxide, and carbon dioxide, a nonmetallic oxide:
CO2(g) + H2O(l) → H2CO3(aq)
There is a gradual transition from basic oxides to acidic oxides from the lower left to the upper right in the periodic table.
BeO < MgO < CaO < SrO < BaO
MnO < Mn2O3 < MnO2 < Mn2O7
in keeping with the increase in covalency.
For example, zinc oxide (ZnO) reacts with both acids and with bases:
In base: ZnO + 2OH- + H2O→ [Zn(OH)4]2-
This reactivity can be used to separate different cations, such as zinc(II), which dissolves in base, from manganese(II), which does not dissolve in base.
Aluminium hydroxide is another amphoteric species:
As an acid (neutralizing a base): Al(OH)3 + NaOH → Na[Al(OH)4]