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Finally, an understandable explanation. Thank you. Given the quality of your videos, its only a matter of time before your channel blows up. Happy to be one of the early subscribers!
Hey, thanks a bunch for your comment! I'm stoked that you found my video helpful and that you appreciate the quality of my content. It means a lot to me, really. I'm excited to have you as one of my early subscribers. Let's keep rocking this TH-cam thing together!
Such a good Video Thank you! Finaly i get to understand how HOMO-LUMO interactions is working on top of that i really had to laugh at 13:42 "No matter how many shamanic dances with drums your perform around them"!
HAHA, thanks! I'm glad my narrative there gave you a good laugh. And yeah, MO theory is a challenging topic which very poorly represented in pretty much every textbook and is barely covered by instructors hoping it's something that students picked up in general chemistry, while gen chem profs hope it's something that organic folks cover later on... so, it never ends up covered in any appreciable depth.
can you use LUMO & HOMO interactions to explain the selectivity of a carbonyl unsaturated beta carbon as an acceptor for a michael donor? ie a cuprate, and why an organolithium would still attack the carbonyl carbon?
Not sure if it's a question or a request... and yes, we can use the corresponding orbital energies to show that the HOMO-LUMO overlap is different in those cases yielding different outcomes.
Hi. At around 21:19 why is the accepting orbital on the cyclic carbocation designated as non-bonding orbital , similar to the one on Br-, O, or S-?? I thought it could be Π* ...
Well, what's accepting an electron pair there, is the carbocation, right? And the carbocation is an empty p-orbital. So, if it's an empty orbital which is not used in any bonding in the cyclohexyl carbocation, it's a non-bonding orbital. There's no π* at that point, the π bond no longer exists!
@@VictortheOrganicChemistryTutor wow thank you. I came to edit my comment and replace π* by something else (not sure what :), since as you mentioned in your comment, π is no longer in the carbocation. I just didn't know what to call that empty orbital .... I am used to non-bonding orbitals being occupied with an e- doublet or maybe it's just me confusing lone pair of e- with non-bonding e-.
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Please, like, share, and comment to help promote this video!
If you would like to support the channel, you can do so by either donating or becoming a member:
Donate: www.organicchemistrytutor.com/donate/
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Finally, an understandable explanation. Thank you. Given the quality of your videos, its only a matter of time before your channel blows up. Happy to be one of the early subscribers!
Hey, thanks a bunch for your comment! I'm stoked that you found my video helpful and that you appreciate the quality of my content. It means a lot to me, really. I'm excited to have you as one of my early subscribers. Let's keep rocking this TH-cam thing together!
love your explanation sir helped a lot!
Thank you so much for this!
You're so welcome!
Such a good Video Thank you! Finaly i get to understand how HOMO-LUMO interactions is working on top of that i really had to laugh at 13:42 "No matter how many shamanic dances with drums your perform around them"!
HAHA, thanks! I'm glad my narrative there gave you a good laugh.
And yeah, MO theory is a challenging topic which very poorly represented in pretty much every textbook and is barely covered by instructors hoping it's something that students picked up in general chemistry, while gen chem profs hope it's something that organic folks cover later on... so, it never ends up covered in any appreciable depth.
well explained
Great video
Glad you enjoyed it
can you use LUMO & HOMO interactions to explain the selectivity of a carbonyl unsaturated beta carbon as an acceptor for a michael donor? ie a cuprate, and why an organolithium would still attack the carbonyl carbon?
Not sure if it's a question or a request... and yes, we can use the corresponding orbital energies to show that the HOMO-LUMO overlap is different in those cases yielding different outcomes.
Hi. At around 21:19 why is the accepting orbital on the cyclic carbocation designated as non-bonding orbital , similar to the one on Br-, O, or S-?? I thought it could be Π* ...
Well, what's accepting an electron pair there, is the carbocation, right? And the carbocation is an empty p-orbital. So, if it's an empty orbital which is not used in any bonding in the cyclohexyl carbocation, it's a non-bonding orbital. There's no π* at that point, the π bond no longer exists!
@@VictortheOrganicChemistryTutor wow thank you. I came to edit my comment and replace π* by something else (not sure what :), since as you mentioned in your comment, π is no longer in the carbocation. I just didn't know what to call that empty orbital .... I am used to non-bonding orbitals being occupied with an e- doublet or maybe it's just me confusing lone pair of e- with non-bonding e-.