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If it had two double bonds, then it would violate the octet rule on oxygen since it is 2p and does not have any d orbitals to expand its valence shell. Also keep in mind that the Lewis structure is not an accurate representation since the actual ozone structure exhibits resonance.
Ghadir Seder 4F wrote:Why is ozone's lewis structure drawn as one double bond and one single bond? Why is it not two double bonds with the formal charges on the oxygens all equal 0?
If you draw ozone with two double bonds, then there isn't the 18 electrons that is needed for the lewis stucture of ozone (3x6 = 18), there are only 16 e-. if you add two e- to any of the oxygens, you violate the octet rule.
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