Resonance
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Resonance
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?
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Re: Resonance
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.
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Re: Resonance
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
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Re: Resonance
A double bond is stronger than a single bond but single bonds are longer than double bonds.
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Re: Resonance
When we have to draw Lewis Structures on the midterm do you think we'll have to draw every resonance structure possible?
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Re: Resonance
The resonance structures themselves don't actually exist in real life, but that's how we are able to model what the structure of the molecule actually looks like, which is an average of all the resonance structures.
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Re: Resonance
Double bonds are stronger than single bonds and require more energy to break. Triple bonds are stronger than double bonds. They all have different lengths because they have different strengths.
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Re: Resonance
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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