To calculate the formal charge of an atom in a molecule or ion, we use the following formula:Formal charge = Valence electrons - Non-bonding electrons - 1/2 Bonding electrons For the perchlorate ion ClO , we have one chlorine atom Cl and four oxygen atoms O . We will calculate the formal charge for both the oxygen and chlorine atoms.1. Oxygen atom:Valence electrons of oxygen = 6 as it is in group 16 of the periodic table In the ClO ion, each oxygen atom is bonded to the chlorine atom through a single bond. So, there are 2 bonding electrons for each oxygen atom.Non-bonding electrons = 6 - 2 = 4 as there are two lone pairs on each oxygen atom Now, we can calculate the formal charge of the oxygen atom:Formal charge of O = 6 - 4 - 1/2 2 = 6 - 4 - 1 = +12. Chlorine atom:Valence electrons of chlorine = 7 as it is in group 17 of the periodic table In the ClO ion, the chlorine atom forms a single bond with each of the four oxygen atoms. So, there are 4 x 2 = 8 bonding electrons for the chlorine atom.Non-bonding electrons = 0 as there are no lone pairs on the chlorine atom Now, we can calculate the formal charge of the chlorine atom:Formal charge of Cl = 7 - 0 - 1/2 8 = 7 - 0 - 4 = +3However, we need to consider the negative charge of the perchlorate ion ClO . This extra negative charge is distributed among the atoms in the ion. Since there are four oxygen atoms, each oxygen atom will share 1/4 of the extra negative charge. Therefore, the formal charge of each oxygen atom will be:Formal charge of O = +1 - 1/4 = +3/4The formal charge of the chlorine atom remains the same:Formal charge of Cl = +3In summary, the formal charge of the oxygen atom in the perchlorate ion is +3/4, and the formal charge of the chlorine atom is +3.