Hi, this is Dr. B. Let's draw the Lewis structure
of O3 or ozone.
Start out by looking at Oxygen on the periodic
table.
It's in group 6 or 16, has 6 valence electrons,
but we have three of them so let's multiply
that by 3 to give us a total of 18 valence
electrons.
That's how many we have to work with.
Draw our three Oxygens right here, and, so
we have 18 valence electrons.
Let's start by putting two between each of
the Oxygens there, that forms a chemical bond.
So we have 2, 4, 6, 8, 10, 12, 14, 16, 18.
Let's check now and see if we have octets.
Over here, 8; over here, as well, so those
have octets.
But in the center, this Oxygen here only has
six.
So we need two more valence electrons.
What we can do is take two from the outside
and share them.
When we do that, we form a double bond.
And, let's see, now we have 2, 4, 6, 8 there.
We have 8 for the center, and then we have
8 over here.
So we've fulfilled the octet rule for each
of the Oxygens.
The only problem is, we could've had the double
bond over here and the single bond here.
Both are correct.
When you have structures when you can draw
it two different ways, those are called resonance
structures.
We end up with something like this right here
where we draw it both ways and we put an arrow
between to show that it could be either.
You could have a single here and a double
here, or a double here and a single here.
It's really the same thing.
This is Dr. B., and thanks for watching.
