Page 1 of 1

Lewis structure for O3 (ozone)

Posted: Fri Oct 21, 2016 8:17 pm
by JennaMinami1I
Hi Chemistry Friends!

I was wondering why the Lewis structure for O3 is

O-O=O (where the Formal charge from left to right is -1,+1,0)
(3 e- pairs on left oxygen, 1 e- pair on middle oxygen, 2 e- pairs on right oxygen)


and not

O=O=O (where all formal charges are 0)
(2 e- pairs on left and right oxygen, 1 e- pair on middle oxygen)


I understand that the first structure has a total charge of 0, but two out of the three atoms in the molecule are charged.
In the bottom structure, none of the atoms have a charge... so why isn't that one correct?

Help greatly appreciated!
**imagine the electron pairs floating around the Os where necessary

Re: Lewis structure for O3 (ozone)  [ENDORSED]

Posted: Fri Oct 21, 2016 9:13 pm
by Geoffrey Zhang 3I
For your second structure O=O=O the middle oxygen would have ten total electrons.

Re: Lewis structure for O3 (ozone)

Posted: Mon Oct 24, 2016 6:08 pm
by Ariana de Souza 4C
I also had a question on O3
Why is the structure linear, and not like a triangle? Wouldn't it be more stable that way, because then the middle one wouldn't have a charge of +1?

Re: Lewis structure for O3 (ozone)

Posted: Wed Oct 26, 2016 3:14 pm
by Chem_Mod
You are correct, the VSEPR shape is going to be "bent" due to the electron repulsion. However, the charges were correct. It's also in resonance. See below:
Screen Shot 2016-10-26 at 3.08.20 PM.png