I have a question about this problem, because I got that benzene had an energy of 5,580 kJ and that its Kekule structure had an energy of 5,352 kJ. I got the right answer, but I thought that benzene would have a lower energy with resonance than its Kekule structure, because resonance stabilizes the molecule. If someone could help explain this, I would greatly appreciate it!
Textbook Problem 4.E.9 [ENDORSED]
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Ryan Khiev 1L
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Textbook Problem 4.E.9
I have a question about this problem, because I got that benzene had an energy of 5,580 kJ and that its Kekule structure had an energy of 5,352 kJ. I got the right answer, but I thought that benzene would have a lower energy with resonance than its Kekule structure, because resonance stabilizes the molecule. If someone could help explain this, I would greatly appreciate it!
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Chem_Mod
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Re: Textbook Problem 4.E.9 [ENDORSED]
Check your calculations.
Benzene does have lower energy due to resonance.
These are the values to break the bonds. Higher more positive means more stable.
Benzene does have lower energy due to resonance.
These are the values to break the bonds. Higher more positive means more stable.
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