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Hyperconjugation made literally no sense in class earlier, but watching you draw it out made it so plain and obvious I'm just like "oh...it's that simple....Lol"!
I am one of those university students who attend lecture classes because I want to be marked present on the register. Otherwise my real lecturer is this one🤗 no complications modules and topics, just a straight foward🤌🔥🤞
In the last example, why can't the double bond on the oxygen transfer electrons to the single C-C bond, negating the carbocation and giving the O a + charge??
@@meeblings6 In the structures containing nitrogen the electron deficient carbon is right next to N and there is a single bond between N and C so Nitrogen can donate lone pair to the carbon atom. But in the last structure the carbonation is not right next to oxygen and oxygen already has a double bond with C and if it were to further donate l.p a triple bond would be highly unstable. Even the carbon would have 5 bonds which would mean it has to break bond with another carbon. So the double bond breaks and electrons of the bond go to oxygen as it is more electronegative.
Hi, just a question. For the last example, can't the right structure make a resonance structure that's more stable by donating the electrons in the double that's in between the "O" and the "C" to the bond to the left making the oxygen have a positive charge on it? And thus that would make it more stable?
That would happen in 2 steps, first the carbon attains -ve charge and then it passes it on (that's what you're trying to say? correct me if I'm wrong) But then the carbon would be unstable and it can't accept electrons to destabilise itself. So it won't happen that way Anyway thats what I think I may be wrong
methly group is electron donating group, moreover R groups doesn't matter as long as methyl group is attached to the +ve carbon, it will stabilize using inductive effect and hyperconjugation, compared to stability by hyperconjugation, stability due to inductive effect is negligible.
Sir pls take neet and jee main syllabus it is one of the toughest exams in India ....pls do that otherwise to should set a playlist for physics and chemistry for this exams ❤
at about 10:30, why can't we draw a resonance structure where one of the bonds from the Carbon oxygen bonds moves to form a double bond between the two carbons. In this case, oxygen will have the positive charge and both carbons will be neutral. Will this just not happen due to Oxygen's high electronegativity and because oxygen will no longer have an octet?
The resonance is between that double bond shifting between 2 positions, it doesn't a a whole loop because the electron is loses to break the first double bond gets to the positively charged carbon right next to it, so there isn't much movement, and hence, the resonance is only between 2 spots
If the oxygen atom aquires an unit positive charge it'll be able to form 3 bonds because it'll now have 3 half vacant p orbitals as it lost one elrctron from one of it's 2 lone pairs
U can also understand it in terms of hybridization, initially in neutral stage the oxygen atom was sp3 hybridised now after acquiring a positive charge it's sp2 as it has formed a pi bond with that carbon atom which means the hybridised orbital which was initially holding the lone pair is now formed a pi bond with the carbon
@@mizzi3136 I have been wondering if oxygen could, in theory, give 4 bonds, since it has 2 lone pairs? I think this would just be extremely unstable, but would it be possible?
Carbocations is more stabilised due to: A.) INDUCTIVE EFFECT B.) HYPERCONJUGATION C.) INDUCTIVE AND MESOMERIC EFFECT D.) INDUCTIVE AND HYPERCONJUGATION EFFECT
In the last example, the positive change is not on the carbon that is attached to the oxygen atom, so having the double bond there doesn’t affect that positive charge. He draws the resonance structure to show how the carbonyl group is an electron withdrawing group and forms another positively charged carbon, which further destabilizes the molecule
I think it's because of the position of the atomic orbitals. they're both the p-Orbitals, and they can overlap from side to side... ( I am sorry, English is not my mother language. I'm trying my best) :)
As far as my understanding goes, resonance is kind of the schrodingers cat of (organic) chemistry. This meaning, two resonant structures (such as the two benzene options) both exist at the same time. Instead of there being an equilibrium, both products don't actually exist seperately but the form the individual molecules take is in between the forms, and the drawn resonance structures are the two "ultimate" forms
Resonance is basically you rolling around in bed trying to find the more comfortable position, and the resonance structure is basically all your positions represented as one (kinda overlapped)
how the hell does the ressoance effect make it better? the positive charge is still there its still has unstable its not doing anything to stabilize it just moving the positive charge to another atom in the samr molecule
For 3:21 I agree that oxygen really have an higher electronegativity, but it's only an partial charged , while the adjacent carbon carry positive chaged ,can the oxgen really draw the electron density towards it-self ? positive charge should have an stronger charge attractions than the partial negative charge ,by means the electron density should draw to positive charged carbon🧐🧐🧐🧐
partial charge is only used to tell which one is more electronegative than the others, while formal negative/ positive charge (as the carbocation that have positive charge) indicates gain or loss of electrons, and we know that oxygen atoms are more electronegative than carbon, so oxygen have the partial negative charge and carbon have the partial positive charge. carbocation is a carbon atom that loses electrons, so if we compare carbocation with oxygen, the oxygen is still having more electronegativity (partial negative charged) than carbocation (partial positive charged). so the oxygen atom there is more likely to pull electrons from the carbocation.
5:45 I agree that the last structure is more stable than the rest but I think the order of stability is wrong cuz the 2nd structure is aromatic and the 3rd structure is Anti aromatic so the 2nd structure has got to be more stable right?pls crct me if I'm wrong
Feel free to stop doing what you are doing! You're confusing as heck and always make things complicated by not thoroughyl explaining things like other people such as Khan!
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Hyperconjugation made literally no sense in class earlier, but watching you draw it out made it so plain and obvious I'm just like "oh...it's that simple....Lol"!
I am one of those university students who attend lecture classes because I want to be marked present on the register. Otherwise my real lecturer is this one🤗 no complications modules and topics, just a straight foward🤌🔥🤞
That last example was especially helpful, thank you!!
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This video help me understand about radican stability and hyperconjugation. Thank you so much
how you make understand concepts no one goes near you. keep making such videos. And make video on every topic possible.
In the last example, why can't the double bond on the oxygen transfer electrons to the single C-C bond, negating the carbocation and giving the O a + charge??
Carbo cation is already present there and based upon there electronegativity difference oxygen atom will except e and will make carbon positive charge
@@asharibimran5645 Why doesn't this happen in the resonance examples where nitrogen is within a ring structure?
@@meeblings6 revise the order of inductive effect first
Oxygen is more electronegative than Carbon. So π bond will not break towards carbon.
@@meeblings6 In the structures containing nitrogen the electron deficient carbon is right next to N and there is a single bond between N and C so Nitrogen can donate lone pair to the carbon atom. But in the last structure the carbonation is not right next to oxygen and oxygen already has a double bond with C and if it were to further donate l.p a triple bond would be highly unstable. Even the carbon would have 5 bonds which would mean it has to break bond with another carbon. So the double bond breaks and electrons of the bond go to oxygen as it is more electronegative.
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Hi, just a question. For the last example, can't the right structure make a resonance structure that's more stable by donating the electrons in the double that's in between the "O" and the "C" to the bond to the left making the oxygen have a positive charge on it? And thus that would make it more stable?
That would happen in 2 steps, first the carbon attains -ve charge and then it passes it on (that's what you're trying to say? correct me if I'm wrong)
But then the carbon would be unstable and it can't accept electrons to destabilise itself. So it won't happen that way
Anyway thats what I think I may be wrong
Very lucid and clear explanation
2:26
How would the inductive effect apply to a methyl group considering there are no R groups attached to the carbocation?
methly group is electron donating group, moreover R groups doesn't matter as long as methyl group is attached to the +ve carbon, it will stabilize using inductive effect and hyperconjugation, compared to stability by hyperconjugation, stability due to inductive effect is negligible.
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Hi, at 5:46 shouldn't 2 be less stable than 3 since 2 is antiaromatic, i.e. conjugation of 4 pi electrons?
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Sir pls take neet and jee main syllabus it is one of the toughest exams in India ....pls do that otherwise to should set a playlist for physics and chemistry for this exams ❤
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at about 10:30, why can't we draw a resonance structure where one of the bonds from the Carbon oxygen bonds moves to form a double bond between the two carbons. In this case, oxygen will have the positive charge and both carbons will be neutral. Will this just not happen due to Oxygen's high electronegativity and because oxygen will no longer have an octet?
Why carbocation has stability has
3°>2°>1°
Where as carbo anion
1°>2°>3°
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THANKS! I finally figured it out
6:22 that ring has a resonance structure??how??if we pin every carbon could we get 6 resonance structure?
The resonance is between that double bond shifting between 2 positions, it doesn't a a whole loop because the electron is loses to break the first double bond gets to the positively charged carbon right next to it, so there isn't much movement, and hence, the resonance is only between 2 spots
Thankyou sir
Great explanation... thanks a lot
Yeah you r the best
@3:56 how is the resonance structure possible? Since the OH has a double bond, it would mean that the Oxygen atom has 3 bonds which is not possible
why is it not possible? the oxygen atom have 2 lone pairs, and OH are bonded with a single sigma bond
If the oxygen atom aquires an unit positive charge it'll be able to form 3 bonds because it'll now have 3 half vacant p orbitals as it lost one elrctron from one of it's 2 lone pairs
U can also understand it in terms of hybridization, initially in neutral stage the oxygen atom was sp3 hybridised now after acquiring a positive charge it's sp2 as it has formed a pi bond with that carbon atom which means the hybridised orbital which was initially holding the lone pair is now formed a pi bond with the carbon
@@mizzi3136 I have been wondering if oxygen could, in theory, give 4 bonds, since it has 2 lone pairs? I think this would just be extremely unstable, but would it be possible?
thank you so much
Carbocations is more stabilised due to:
A.) INDUCTIVE EFFECT
B.) HYPERCONJUGATION
C.) INDUCTIVE AND MESOMERIC EFFECT
D.) INDUCTIVE AND HYPERCONJUGATION EFFECT
C) Resonance is stronger than both hyperconjugation and inductive effect.
In the last example, why can't pair of e of the O atom make a double bond with the + charge?!
like the one at 3:55
In the last example, the positive change is not on the carbon that is attached to the oxygen atom, so having the double bond there doesn’t affect that positive charge. He draws the resonance structure to show how the carbonyl group is an electron withdrawing group and forms another positively charged carbon, which further destabilizes the molecule
@@clarissarojas3980 ty for the explanation
thank-you for remembering this topic
Literally now i can die in peace.
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Thank you.
Resonance effect
Can someone explain me, why at 2:05 the atomic orbitals will overlap?
I think it's because of the position of the atomic orbitals. they're both the p-Orbitals, and they can overlap from side to side... ( I am sorry, English is not my mother language. I'm trying my best) :)
What is the mdp orbital??😢😢😢😢
empty p orbital
Thank you :-)
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Goat
How exactly do you define resonance?
As far as my understanding goes, resonance is kind of the schrodingers cat of (organic) chemistry. This meaning, two resonant structures (such as the two benzene options) both exist at the same time. Instead of there being an equilibrium, both products don't actually exist seperately but the form the individual molecules take is in between the forms, and the drawn resonance structures are the two "ultimate" forms
Resonance is basically you rolling around in bed trying to find the more comfortable position, and the resonance structure is basically all your positions represented as one (kinda overlapped)
how the hell does the ressoance effect make it better? the positive charge is still there its still has unstable its not doing anything to stabilize it just moving the positive charge to another atom in the samr molecule
forget it its because the positive charge is shared around them
3:43
love u
For 3:21 I agree that oxygen really have an higher electronegativity, but it's only an partial charged , while the adjacent carbon carry positive chaged ,can the oxgen really draw the electron density towards it-self ? positive charge should have an stronger charge attractions than the partial negative charge ,by means the electron density should draw to positive charged carbon🧐🧐🧐🧐
partial charge is only used to tell which one is more electronegative than the others, while formal negative/ positive charge (as the carbocation that have positive charge) indicates gain or loss of electrons, and we know that oxygen atoms are more electronegative than carbon, so oxygen have the partial negative charge and carbon have the partial positive charge. carbocation is a carbon atom that loses electrons, so if we compare carbocation with oxygen, the oxygen is still having more electronegativity (partial negative charged) than carbocation (partial positive charged). so the oxygen atom there is more likely to pull electrons from the carbocation.
5:45 I agree that the last structure is more stable than the rest but I think the order of stability is wrong cuz the 2nd structure is aromatic and the 3rd structure is Anti aromatic so the 2nd structure has got to be more stable right?pls crct me if I'm wrong
Second structure is not aromatic as it has sp3 carbon atom
Arranged in iit jee form
If only you taught at every university
no we dont wanna share him with a university . he is our tutor . one of the professer might try to take his life outta jealousy !
Feel free to stop doing what you are doing! You're confusing as heck and always make things complicated by not thoroughyl explaining things like other people such as Khan!
Can you speak Arabic ?that 's better
For the last example, this resonance structure would also work: snipboard.io/BelxDS.jpg
So it's not clear which structure is more stable.
But then you'd have a positive charge on the atom that is more electronegative which is not stable
Thank you
Thanks a lot.