To calculate the formal charge of each atom in the nitrate ion NO3^- , we need to follow these steps:1. Determine the number of valence electrons for each atom.2. Calculate the number of non-bonding electrons for each atom.3. Calculate the number of bonding electrons for each atom.4. Calculate the formal charge for each atom.Step 1: Determine the number of valence electrons for each atom.- Nitrogen N has 5 valence electrons.- Oxygen O has 6 valence electrons.Step 2: Calculate the number of non-bonding electrons for each atom.In the nitrate ion, there are three oxygen atoms. Two of them are single-bonded to the nitrogen atom and have three lone pairs 6 non-bonding electrons . The third oxygen atom is double-bonded to the nitrogen atom and has two lone pairs 4 non-bonding electrons .Step 3: Calculate the number of bonding electrons for each atom.- Nitrogen N forms one double bond and two single bonds, so it has 2 + 1 + 1 = 4 bonding electrons.- Oxygen O forms one double bond and two single bonds in total , so it has 2 + 1 + 1 = 4 bonding electrons.Step 4: Calculate the formal charge for each atom.Formal charge = valence electrons - non-bonding electrons - 1/2 * bonding electrons - Nitrogen N : Formal charge = 5 - 0 - 1/2 * 4 = 5 - 2 = +1- Oxygen O with single bond: Formal charge = 6 - 6 - 1/2 * 2 = 6 - 6 - 1 = -1- Oxygen O with double bond: Formal charge = 6 - 4 - 1/2 * 4 = 6 - 4 - 2 = 0So, the formal charges for the nitrate ion NO3^- are:- Nitrogen N : +1- Oxygen O with single bond: -1 for each of the two oxygen atoms - Oxygen O with double bond: 0