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To calculate the formal charges on each Oxygen atom in the O3 molecule, the first thing we
need to do is look at the Lewis structure. Then, we'll use the formula below to find
the formal charges for O3. For the first Oxygen, we have 6 valence electrons; and we found
that on the periodic table. Oxygen is in group 6 or 16. Minus nonbonding, we have 4 nonbonding
valence electrons. Minus the bonding, and we have two bonds, a double bond; so we have
4 bonding electrons. We'll divide that by 2. So the formal charge on the Oxygen with
the double bond is zero. Next, we'll look at the Oxygen at the center of the O3 molecule.
We have 6, minus nonbonding, and we only have 2 nonbonding valence electrons. Minus bonding,
we have 1, 2, 3 bonds; so we have 6 bonding valence electrons, we'll divide that by 2.
Six minus 2 minus 3 gives us a +1. So the formal charge on that central Oxygen is +1.
Let's do the final Oxygen with the single bond. Again, we have 6 valence electrons from
the periodic table. Minus nonbonding, we have 2, 4, 6 nonbonding. And then bonding, we have
2, which we'll divide by 2. So 6 minus 6 minus 1 gives us negative 1. So the formal charge
for that final Oxygen with the single bond is -1. If we add the formal charges up for
each individual atom, we have zero, plus 1 and a minus 1, the total charge for the molecule
is going to be zero. So those are the formal charges for the O3 molecule. This is Dr. B.,
and thanks for watching.