All right, this is Dr. B. Let's do the Lewis
structure for H2S: Dihydrogen Sulfide.
On the periodic table: Hydrogen, group 1,
has 1 valence electron, but we have two Hydrogens
here so let's multiply that by 2.
Plus Sulfur is in group 6 or 16 on the periodic
table, so it has 6 valence electrons.
Total of 8 valence electrons.
Let's draw this thing.
We'll put Sulfur here.
Hydrogen always goes on the outside, we'll
put it out there.
Now we want to take some of these valence
electrons and spread them around the atoms.
Let's start by forming a chemical bond between
the Hydrogens and Sulfur.
So we've used 4 valence electrons, and we
have 8.
Hydrogen only needs 2 for a full outer shell,
which it has.
So Hydrogen's good.
We'll put the remaining valence electrons
around the Sulfur, which needs eight for a
full outer shell.
It has eight valence electrons.
We've used all the 8 of valence electrons
we had to do the Lewis structure for H2S.
So that's fine; we're done with that.
We can draw a structural formula for it like
this here.
The structural formula is bent, because it
is a bent molecule.
These valence electrons, these unbonded valence
electrons kind of push the Hydrogens down.
This is Dr. B., thanks for watching.
