For the CH3COO- Lewis structure, we have a
total of 24 valence electrons.
We'll put the Carbons next to each other.
We'll put an Oxygen on the end here, and we'll
put another Oxygen here.
Then we have those three Hydrogens, which
we'll place around the Carbon on the end.
We have 24 valence electrons for the CH3COOH-
Lewis structure.
We'll put two between atoms to form chemical
bonds.
We've used 12 valence electrons.
Then we'll go around the Oxygens to complete
their octet, until we use 24 valence electrons.
So we had 12, 14, and 24 valence electrons.
So you can see the Hydrogens each have two
valence electrons; their outer shells are
full.
The Oxygens have eight; their outer shells
are full.
The Carbon on the left has eight, but that
Carbon in the middle only has six, so it does
not have an octet.
Let's take two valence electrons here from
this Oxygen and share them to form a double
bond with the Carbon.
The Oxygen still has eight valence electrons,
but now the Carbon also has eight valence
electrons and we're only using the 24 valence
electrons we have for the CH3COO- Lewis structure.
So that's the Lewis structure for the acetate
ion.
This is Dr. B., and thanks for watching.
