OK, we're going to do the Lewis dot structure
for O2.
Let's start.
Looking on the periodic table, we can find
Oxygen in group 6 or 16, and that means it
has 6 valence electrons.
But we have two of them so we'll multiply
that by 2.
That gives us a total of 12 valence electrons.
We're going to distribute those valence electrons
around the atoms, the Oxygen atoms.
So we draw one Oxygen, and another Oxygen.
And let's put two between here to form a chemical
bond.
So we've used 2, 4, 6, 8, 10, 12.
We've used 12 valence electrons, what we have
to use.
Let's see if we have an octet, or 8 valence
electrons.
For that Oxygen, 2, 4, 6, 8; that's fine.
But for this Oxygen, we only have 2, 4, 6.
Not an octet, and that's not going to be stable.
What we can do is, we can take two of these
electrons here and move them between the Oxygens.
So now let's see what happened with our octet.
Two, 4, 6, 8; that's fine.
And then over here, 2, 4, 6, 8.
That also has an octet.
And we have 2, 4, 6, 8, 10, 12; twelve valence
electrons, just like we started with.
Everything's good: our octets are satisfied,
we've used all the valence electrons.
If we want to write it out in a structural
formula, we can take and write it like this,
where this double bond right here represents
these two pairs of electrons.
This is Dr. B., and thanks for watching.
