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Topic: trimethylxanthine, common name caffeine  (Read 6271 times)

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alon

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trimethylxanthine, common name caffeine
« on: February 24, 2005, 11:46:00 AM »
What is the basicisity difference of the nitrogens on cafffiene?
I believe that the two unpaired electrons on the nitrogen next to the double bond are more delocalized  thus this nitrogen is a better lewis base than the other two nitrogens.
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Offline Mitch

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Re:trimethylxanthine, common name caffeine
« Reply #1 on: February 25, 2005, 06:27:53 AM »
Quote from: alon on February 24, 2005, 11:46:00 AM
the nitrogen next to the double bond are more delocalized  thus this nitrogen is a better lewis base than the other two nitrogens.

That is the exact reason why it's a poor lewis base. If it gave up it's electrons it would no longer be delocalized in the ring system.
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alon

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Re:trimethylxanthine, common name caffeine
« Reply #2 on: February 25, 2005, 08:43:58 AM »
thanks mitch :D
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