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Polyatomic ions often are useful in the context of acid–base chemistry and in the formation of salts. Often, a polyatomic ion can be considered as the conjugate acid or base of a neutral molecule. For example, the conjugate base of sulfuric acid (H 2 SO 4) is the polyatomic hydrogen sulfate anion (HSO − 4).
For ions, the charge on a particular atom may be denoted with a right-hand superscript. For example, Na +, or Cu 2+. The total charge on a charged molecule or a polyatomic ion may also be shown in this way, such as for hydronium, H 3 O +, or sulfate, SO 2− 4. Here + and − are used in place of +1 and −1, respectively.
Functional groups can also be charged, e.g. in carboxylate salts (−COO −), which turns the molecule into a polyatomic ion or a complex ion. Functional groups binding to a central atom in a coordination complex are called ligands. Complexation and solvation are also caused by specific interactions of functional groups.
A carbonate is a salt of carbonic acid, (H 2 CO 3), [2] characterized by the presence of the carbonate ion, a polyatomic ion with the formula CO 2− 3. The word "carbonate" may also refer to a carbonate ester , an organic compound containing the carbonate group O=C(−O−) 2 .
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