The carbonate ion CO3^2- has three resonance structures. In each resonance structure, one of the oxygen atoms forms a double bond with the central carbon atom, while the other two oxygen atoms form single bonds with the central carbon atom. The three resonance structures can be represented as follows:1. O=C-O - -O - 2. O - -C=O-O - 3. O - -O - -C=ONow, let's determine the formal charge on each atom in each resonance structure:1. O=C-O - -O - - Carbon C : Formal charge = 4 - 3 - 1/2 4 = 0 - Double-bonded Oxygen O : Formal charge = 6 - 4 - 1/2 4 = 0 - Single-bonded Oxygen O- : Formal charge = 6 - 6 - 1/2 2 = -1 x2 2. O - -C=O-O - - Carbon C : Formal charge = 4 - 3 - 1/2 4 = 0 - Double-bonded Oxygen O : Formal charge = 6 - 4 - 1/2 4 = 0 - Single-bonded Oxygen O- : Formal charge = 6 - 6 - 1/2 2 = -1 x2 3. O - -O - -C=O - Carbon C : Formal charge = 4 - 3 - 1/2 4 = 0 - Double-bonded Oxygen O : Formal charge = 6 - 4 - 1/2 4 = 0 - Single-bonded Oxygen O- : Formal charge = 6 - 6 - 1/2 2 = -1 x2 In summary, the carbonate ion CO3^2- has three resonance structures with the same formal charges on each atom: Carbon has a formal charge of 0, the double-bonded oxygen has a formal charge of 0, and each single-bonded oxygen has a formal charge of -1.