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What does it mean when the bonds of the resonance structures are all the same length? How does that compare to a molecule with bonds that have different lengths? And how do we know which of the resonance structures exist in real life?
None of the resonance structures we draw as Lewis symbols actually exist in real life, because in an actual molecule that has resonance structures, the double bond is divided up in between the atoms equally. For example, for a nitrate ion, NO3-, we draw the Lewis structure as nitrogen having a double bond with one of the oxygens and a single bond with the other two; but in reality, the actual structure of nitrate has a 1 1/3 bond in between nitrogen and each oxygen. Therefore, the bond's strength is equal in between nitrogen and each oxygen, so each bond is the same length.
If you're interested, you can search up "ozone lewis structure" and you'll see that it has two resonance structures, but in reality it exists as something in between like this: https://upload.wikimedia.org/wikipedia/ ... dipole.png
Yukta Italia 3I wrote:When we have to draw Lewis Structures on the midterm do you think we'll have to draw every resonance structure possible?
I think you only need to draw the resonance structures for the most stable structure.
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