OK, this is Dr. B.
We're going to do the Lewis structure for
F2, Fluorine gas: a yellow, extremely reactive
gas.
And we'll start looking on the periodic table.
Fluorine is in group 7, or, sometimes called
17, and that means that it will have 7 valence
electrons.
But we have 2 Fluorine atoms, so we need to
multiply that by 2, and that gives us a total
of 14 valence electrons.
Let's draw the two Fluorines next to each
other.
And we have 14 valence electrons to bond and
then spread around and try to satisfy the
octets, or give each Fluorine 8 valence electrons.
We'll put these two here.
That pair bonds them together.
And so we've used 2, 4, 6, 8, 10, 12, 14.
We've used all our valence electrons up, and
let's see if we have octets.
Two, 4, 6, 8; that Fluorine has 8.
And over here, 2, 4, 6, 8; that Fluorine has
8, as well.
So we're actually done with the dot structure
for F2.
We could write it, though, like a structural
formula, and that would look like this right
here where this bond is represented by a single
line.
So that single line is a pair of electrons
bonding the two F's together.
And then the rest of the electrons are valence
electrons around the Fluorine atom.
This is Dr. B., and thanks for watching.
