Lewis structure for O3 (ozone)  [ENDORSED]

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JennaMinami1I
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Joined: Wed Sep 21, 2016 2:56 pm

Lewis structure for O3 (ozone)

Postby JennaMinami1I » Fri Oct 21, 2016 8:17 pm

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

Geoffrey Zhang 3I
Posts: 26
Joined: Wed Sep 21, 2016 3:00 pm

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

Postby Geoffrey Zhang 3I » Fri Oct 21, 2016 9:13 pm

For your second structure O=O=O the middle oxygen would have ten total electrons.

Ariana de Souza 4C
Posts: 99
Joined: Wed Sep 21, 2016 2:56 pm

Re: Lewis structure for O3 (ozone)

Postby Ariana de Souza 4C » Mon Oct 24, 2016 6:08 pm

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?

Chem_Mod
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Re: Lewis structure for O3 (ozone)

Postby Chem_Mod » Wed Oct 26, 2016 3:14 pm

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


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