To calculate the formal charge on each atom in the molecule CO3^2-, we need to follow these steps:1. Determine the number of valence electrons for each atom.2. Calculate the number of non-bonding lone pair electrons for each atom.3. Calculate the number of bonding electrons for each atom.4. Calculate the formal charge for each atom using the formula: Formal charge = Valence electrons - Non-bonding electrons + 1/2 Bonding electrons CO3^2- is a carbonate ion, which has a resonance structure. The molecule consists of one carbon atom and three oxygen atoms, with one of the oxygen atoms having a double bond with the carbon atom, and the other two oxygen atoms having single bonds with the carbon atom. The molecule has a -2 charge.Step 1: Valence electrons- Carbon C : 4 valence electrons- Oxygen O : 6 valence electronsStep 2: Non-bonding lone pair electrons- Carbon C : 0 lone pair electrons all electrons are involved in bonding - Oxygen with a double bond O : 4 lone pair electrons 2 lone pairs - Oxygen with a single bond O : 6 lone pair electrons 3 lone pairs Step 3: Bonding electrons- Carbon C : 4 bonding electrons 1 double bond and 2 single bonds - Oxygen with a double bond O : 4 bonding electrons 1 double bond - Oxygen with a single bond O : 2 bonding electrons 1 single bond Step 4: Calculate the formal charge for each atom- Carbon C : 4 - 0 + 1/2 * 4 = 4 - 2 = 0- Oxygen with a double bond O : 6 - 4 + 1/2 * 4 = 6 - 6 = 0- Oxygen with a single bond O : 6 - 6 + 1/2 * 2 = 6 - 7 = -1The formal charges for the atoms in the CO3^2- molecule are:- Carbon C : 0- Oxygen with a double bond O : 0- Oxygen with a single bond O : -1 for each of the two oxygen atoms Since there are two oxygen atoms with a single bond and a -1 charge, the overall charge of the molecule is -2, which matches the given charge of CO3^2-.