Resonance

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Saachi_Kotia_4E
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Resonance

Postby Saachi_Kotia_4E » Tue Oct 30, 2018 10:53 am

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?

Reva Kakaria 1J
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Re: Resonance

Postby Reva Kakaria 1J » Tue Oct 30, 2018 11:12 am

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.

Ashley Zhu 1A
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Joined: Fri Sep 28, 2018 12:16 am

Re: Resonance

Postby Ashley Zhu 1A » Wed Oct 31, 2018 2:57 pm

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

Tinisha 1G
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Re: Resonance

Postby Tinisha 1G » Wed Oct 31, 2018 6:12 pm

The bond length allows to have more insight on how strong the bond is as well!

Charles Gu 1D
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Re: Resonance

Postby Charles Gu 1D » Thu Nov 01, 2018 11:24 am

A double bond is stronger than a single bond but single bonds are longer than double bonds.

Yukta Italia 3I
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Re: Resonance

Postby Yukta Italia 3I » Thu Nov 01, 2018 12:44 pm

When we have to draw Lewis Structures on the midterm do you think we'll have to draw every resonance structure possible?

Manas_Varma_4B
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Joined: Fri Sep 28, 2018 12:29 am

Re: Resonance

Postby Manas_Varma_4B » Thu Nov 01, 2018 12:52 pm

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.

Hannah Pham 1D
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Re: Resonance

Postby Hannah Pham 1D » Thu Nov 01, 2018 3:26 pm

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.

Brandon Mo 4K
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Re: Resonance

Postby Brandon Mo 4K » Thu Nov 01, 2018 6:40 pm

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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