CH3COO- Lewis Structure: How to Draw the Lewis Structure for CH3COO-

For the CH3COO- Lewis structure, we have a total of 24 valence electrons. We’ll put the Carbons next to each.


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.

6 thoughts on “CH3COO- Lewis Structure: How to Draw the Lewis Structure for CH3COO-”

  1. Sir I ve one doubt…while placing d electrons around d atoms y dindt we simply put 8 around first and 8 around second directly at the first go…but u placed 8 around first C and left second carbon with 6 electons…plz clear my doubt

  2. Why would H2C=CH-O-O(-)be wrong? ( I know it wrong but I have been told to choose the correct structure and I cannot explain why). The formal charges are exactly same as the correct structure and all octets are complete. How would you explain this?

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