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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.
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
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.
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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