That is probably true to some degree, Hannah-the lone pair on N is involved in resonance with the benzene π electrons in J (aniline). One way to explore this is to look at the boiling point of cyclohexylamine (no π electrons and no resonance) versus aniline. In fact, aniline's BP is much higher than cyclohexylamines, suggesting that hydrogen bonding is just as important for aniline, despite resonance delocalization of the lone pair! The boiling point of benzylamine, with an extra CH2 jammed between the NH2 and phenyl groups, is just 1 ºC higher than aniline's-again suggesting that hydrogen bonding is important in both.
the thing with that is that H-bonding isn't necessarily happening at the acceptor you pointed at in the video (the N atom). it will to some extent, but aromatic rings are also weak acceptors. especially when you have hetero atoms donating electron density towards them. in the benzylamine and aniline you also have pi stacking affecting the boiling point. the two forces can work in conjunction where you get pi-teeing and amine moiety H-bonding at the same time. its not to say it's not happening, it's just to say that the picture you paint might be a bit misleading, only in the sense that it may not apply to aniline or other aryl-amines outside of the context of a pure liquid compound. for example, if you're designing a drug to target a protein where the magnitude of the dipole and the directionality really matter, then you may not consider aniline to be a Hydrogen bond acceptor. you might opt for a benzyl amine or a pyridine or something where the lone pair isn't in conjugation with the ring.
Thanks! this was an effective review for my biochem test! I had completely forgotton about the rules that make up Donors and Acceptors. Your explanation was simple and easy! Thanks a bunch! :)
Thank you !!! My chemistry teacher in high school can't explain well and I didn't really understand the Hydrogen bond (with donors and acceptors).... And I have to make a chemistry test tomorrow, so was a bit upset but you have saved me! :)
would molecule B was in water (assuming they are both polar) would the water make 3 bonds with OH in that B molecule? for example would the O bond with an H from H20 in each lone pair O has ? and then the H (from the OH) would it bond with an O from an H20 molecule?
Yes and no. While three hydrogen bonds are possible just as you describe, the exact number of bonds can vary (the molecules are bouncing around in solution!) and the structure of the solution is temperature dependent. At very low temperatures, we might expect the ethanol and water to freeze in a configuration with all three H-bonds intact. At higher temperatures, only 1 or 2 bonds are most likely to exist.
For the 'J ' some bookd said NH2 only can work as hydrogen donor, not a acceptor. For example, H2N, HN in cysteine or guanine. Please let me know the difference
In the case of cysteine or guanine, the nonbonding lone pair on nitrogen is involved in delocalization with an adjacent pi system (i.e., resonance). Amino nitrogens involved in resonance generally do not act as hydrogen bond acceptors.
Pure hydrogen bond donors are rare because usually where an appropriate X-H bond shows up, X also has a lone pair. About the only example I can think of are ammonium cations (HNR3)+, which lack a lone pair at nitrogen but have the N-H bond for hydrogen bonding.
These are both hydrogen bond acceptors, not donors. They "accept" the X-H bond as one of the lone pairs on chlorine interacts with it. Some would argue that chlorine can't really hydrogen bond in this fashion, though.
This has been the best and simplest Chemistry tutorial of my life.
Thank you! You are an exceptional teacher.
GOD BLESS YOU
This is so helpful yet something we didn't even talk about in class. Thank you!!!
Really helpful sir
I was stuck in how to know whether an organic compound is H donor or acceptor untill I saw your video
Once again thanks a lot
This Question is from M S Chouhan ( Advance Problems in Organic Chemistry), right?
This video is excellent. I watch this every time I start a new chemistry course to freshen my memory up about this.
this was the perfect explanation.. Thank you so much. You save my life in pharmacy school.
Same goes to me hahaa
This is a Ms Chouhan questions.thank you for uploading it.😍😍😍
That is probably true to some degree, Hannah-the lone pair on N is involved in resonance with the benzene π electrons in J (aniline). One way to explore this is to look at the boiling point of cyclohexylamine (no π electrons and no resonance) versus aniline. In fact, aniline's BP is much higher than cyclohexylamines, suggesting that hydrogen bonding is just as important for aniline, despite resonance delocalization of the lone pair!
The boiling point of benzylamine, with an extra CH2 jammed between the NH2 and phenyl groups, is just 1 ºC higher than aniline's-again suggesting that hydrogen bonding is important in both.
the thing with that is that H-bonding isn't necessarily happening at the acceptor you pointed at in the video (the N atom). it will to some extent, but aromatic rings are also weak acceptors. especially when you have hetero atoms donating electron density towards them. in the benzylamine and aniline you also have pi stacking affecting the boiling point. the two forces can work in conjunction where you get pi-teeing and amine moiety H-bonding at the same time. its not to say it's not happening, it's just to say that the picture you paint might be a bit misleading, only in the sense that it may not apply to aniline or other aryl-amines outside of the context of a pure liquid compound. for example, if you're designing a drug to target a protein where the magnitude of the dipole and the directionality really matter, then you may not consider aniline to be a Hydrogen bond acceptor. you might opt for a benzyl amine or a pyridine or something where the lone pair isn't in conjugation with the ring.
@@ericfortin5612 author should correct this.
Thanks! this was an effective review for my biochem test! I had completely forgotton about the rules that make up Donors and Acceptors. Your explanation was simple and easy! Thanks a bunch! :)
This video saved my life, thank you so much! Explained it better than any teachers did!
Thank you so much ❤
Finally after years i can understand organic chem so well 🎉❤️🧿
Thank you so much for this video. This has been a great tutorial for helping me refresh for organic chem
His explanation is really good 4:01 👍👍👍👍👍👍
Amazing teacher.
I was stuck in this question from MS Chauhan, then Google show me way to this video.
Thanks.
Right before my drug design exam I needed this for solving Lipinski rule of 5 questions thank you very much.
Thank you so much ! Was stuck on this concept for hours but within 3 min of your video it was all cleared up!
Out here doing the Lord’s work
Thank you, sir, for your service
For J, isnt it that the benzene ring will pull the lone pair from nitrogen to help its conjugation, and make the nitrogen a sucky H-bond accepter?
That’s what I was thinking. I don’t think J is a hydrogen bond acceptor
Thank you !!! My chemistry teacher in high school can't explain well and I didn't really understand the Hydrogen bond (with donors and acceptors).... And I have to make a chemistry test tomorrow, so was a bit upset but you have saved me! :)
YOU JUST SAVED MY SEMESTER!!! thanks
would molecule B was in water (assuming they are both polar) would the water make 3 bonds with OH in that B molecule? for example would the O bond with an H from H20 in each lone pair O has ? and then the H (from the OH) would it bond with an O from an H20 molecule?
Yes and no. While three hydrogen bonds are possible just as you describe, the exact number of bonds can vary (the molecules are bouncing around in solution!) and the structure of the solution is temperature dependent. At very low temperatures, we might expect the ethanol and water to freeze in a configuration with all three H-bonds intact. At higher temperatures, only 1 or 2 bonds are most likely to exist.
It is an excellent explanation. Thanks a lot Michael!
how make semi-conducter when makes mount of donor?
First time I got it clear . Thanks
Very useful vedio. Thank you for uploading
wow, so simple the way you explained it. thank you!
This question is of M.S.Chouhan Organic Chemistry, pg 36
But answers are different
@@aquasaaziz7125 because the the is a bit different in that book
In second question it is asked the which servers as both acceptor and donor.
Beautifully explained ☺😊😀😃😄
Really, best explanation
Really helpful! Great examples.
I'm in pharmacy school and here I am again!! haha! great video!!
Hey, congrats Kelli! :-D
Wtf?!! Sameeee!!!!😭😭😭
For the 'J ' some bookd said NH2 only can work as hydrogen donor, not a acceptor. For example, H2N, HN in cysteine or guanine. Please let me know the difference
In the case of cysteine or guanine, the nonbonding lone pair on nitrogen is involved in delocalization with an adjacent pi system (i.e., resonance). Amino nitrogens involved in resonance generally do not act as hydrogen bond acceptors.
But incase of J. It also seems like work as resonance but why it can work as acceptor and donor?
AYYYY this helps a lot studying for chem finals
Small doubt: does electronegativity of N, O, F have any effect on hydrogen bonding?
Can F atom acts as H bond acceptor and or donor?
Thank you so much for this video, really helpful
REALLY HELPFUL.. AND GOOD EXAMPLES...!
Why Acetone can form Hydrogen bond with either Water (H2O) or Chloroform (CHCl3), but Chloroform cannot form Hydrogen bond with Water?
really clear video thanks for this
does that mean that NH2 can be H donor and acceptor
Yes, just like water
thanks
Why must be heteroatom can be hydrogen bond donor , Why not carbon atom? Why not C-H bond can be the donor as well ?
This was extremely helpful 🙏🏾
I'm confused why the
-NH2 can serve as a H bond donor and not the
-CH3?
Carbon isn't electronegative enough; that is, the C-H bond is not polarized enough to engage in hydrogen bonding.
carbon isnt a heteroatom
could you give an example where only H-bond donor occurs? ( examples here are both h-bond acceptros and H-bond donors)
Pure hydrogen bond donors are rare because usually where an appropriate X-H bond shows up, X also has a lone pair. About the only example I can think of are ammonium cations (HNR3)+, which lack a lone pair at nitrogen but have the N-H bond for hydrogen bonding.
I believe Ammonium, NH4, can also donate but not accept.
thank you so much!! im in orgo and i still didn't fully understand this until now lol
Great job ♥️ thank you ♥️
you are amazing sir!!
Thank you so much, great video!
Thank you very much !!! I finally understood!
This was so helpful. Thank you!
Very interactive ✨
why are Chlorophrom and dichloromethane H-bond donors?
These are both hydrogen bond acceptors, not donors. They "accept" the X-H bond as one of the lone pairs on chlorine interacts with it. Some would argue that chlorine can't really hydrogen bond in this fashion, though.
It really helped, thanks 😊.
This was really helpful thank you!
Thanks for watching!
Thank you for clarifying this.
Tq it's very useful
literally god bless ur soul
Thanks! Cleared it up!
This is fantastic, thanks a lot!
thanks. this portion was very slim in mcmurry 9e
well explained
So helpful!! thanks a lot.
SOOOOOO HELPFUL
THANK U
Thank you so much!!! This was extremely helpful!!!!
Thanks for watching, Melissa!
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It really helpful
Thanks for this video man🙌🏻:-)
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Thanks for watching!