This is Dr. B. Let's do the SCl2 Lewis structure.
On the periodic table, Sulfur--group 6 or
16-- has 6 valence electrons.
Chlorine, group 7 or 17 has 7; but we have
two Chlorines so let's multiply that by 2.
Six plus 14 equals 20 valence electrons.
Let's put the Sulfur at the center; it's the
least electronegative.
Put the Chlorines on either side of it and
we'll put two electrons between the Sulfur
and the Chlorine to form a chemical bond.
We've used four.
Then on the outside atoms, the Chlorines,
6, 8, 10, over here 12, 14, 16; and then we
go to the center, 18, 20.
We've used all our valence electrons.
Let's check and see if we have octets.
This Chlorine has 8 valence electrons, as
does this Chlorine.
So they have octets.
And then in the center, Sulfur also has 8
valence electrons.
So we've used all 20 of the valence electrons.
Each of these atoms has an octet, and we're
done.
That's the SCl2 Lewis structure: sulfur dichloride.
This is Dr. B., thanks for watching.
