Bond Lengths

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Bianca Barcelo 4I
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Joined: Fri Sep 28, 2018 12:17 am
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Bond Lengths

Postby Bianca Barcelo 4I » Sat Dec 08, 2018 1:12 am

How are bond lengths the same due to resonance structures?

Richard Ku 4H
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Joined: Fri Oct 05, 2018 12:16 am

Re: Bond Lengths

Postby Richard Ku 4H » Sat Dec 08, 2018 2:31 am

In resonance structures, the electrons of the pi bonds in double bonds are delocalized, meaning they move over the entire atom. This means the delocalized electron is shared between all bonds, resulting in equal bond lengths and strengths.

Aiden Metzner 2C
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Re: Bond Lengths

Postby Aiden Metzner 2C » Fri Oct 25, 2019 3:37 pm

Even though the bond lengths are represented as different, with double bonds, single bonds, etc. In resonance structures the electrons are delocalized, so the lewis structures aren't necessarily a good representation of how the molecule looks. In reality resonance structures share all the electrons equally, but this can't be represented in lewis structures

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Re: Bond Lengths

Postby BNgo_2L » Fri Oct 25, 2019 3:48 pm

Resonance structures are just different versions of the actual structure. This means that the resonance hybrid has a blend of all these structures. As a result, the bond lengths of the actual structure is a blend of both the single and double bonds thus creating equal bond lengths all around.

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Re: Bond Lengths

Postby Martina » Sat Oct 26, 2019 1:20 am

The resonance structure is a blend of the different possible lewis structures of a molecule. The bond lengths of the resonance structure will all be the same and will be somewhere between the lengths of all the possible bonds.

Sally Qiu 2E
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Joined: Fri Aug 30, 2019 12:18 am

Re: Bond Lengths

Postby Sally Qiu 2E » Sat Oct 26, 2019 8:59 am

the electrons in resonance structures are delocalized, and this spreads multiple-bond character over the whole molecule. the resonance structures don't depict how the molecule actually looks like, so the bond lengths are the average between the single and double bonds

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