I've been retaking my A level chemistry exam by myself this year cause i need an A and your vids are the only thing helping me push my grade up. Just wanted to tell you thank you so much for the vids.
Sir,my book has the structure you made at 11:53 and it says underneath it "According to this molecular orbital picture each c-c bond in benzene consists of full sigma and half pi bond.Because of this reason c-c bond is equal and benzene shows substitution as well as additional reaction" Could you kindly elaborate this? I don't get it any of it.
Hello, thank you for all your help sir, I really understand this well now :) , I just had one question or confusion, you know the electron configuration of c is 1s2,2s2,2p2 so the carbon has 2 electrons in its outer shell ? Where does the 2 other electrons come from. I did research and hybridization kept coming up it was hard to understand and if this is the case do all atoms undergo hybridization or is carbon an exception. Thanks for your help
August Kekule was "energetic and intense" I'm not sure what he took if he did take anything, or if being German had something to do with him, but you should speed up your thoughts a little. tea is great( green tea, caffeine and theanine), but I recommend espresso.
Hi, thank you so much for your videos!! You make learning Chemistry bearable :P are you going to be doing anymore videos for F324 and F325 or have you finished now?
Thanks for the comment, glad the videos help. I'm struggling to find the time to make any more at the moment. Hopefully I'll be able to do a few more over Easter but my original plan to have the whole of F324 and F325 done this year isn't looking likely at present. Thanks again and keep watching!
It's been a while since I've done AS so I feel like I've forgotten the basics but can someone explain how each carbon has four electrons, three form sigma bonds and 1 forms a pi bond when there's four outer electrons so shouldn't it be 1s^2, 2s^2 making the fourth electron still in the s?
+A Saeed I know that the first bond a carbon atom makes with another atom is always a sigma bond and if it has a second or third bond with that atom, those are pi bonds. In benzene there are 3 double bonds so each carbon has a double bond with another carbon and a single bond with a carbon and a hydrogen. So the bonds that the carbon has to the hydrogen and the singly bonded carbon are both sigma bonds (its the first and only bond the carbon has with the other atom) but in the case of the carbon-carbon double bond one of the bonds is sigma so the second has to be a pi bond. So that's why there are 3 sigma bonds and 1 pi bond, I think. Hahahha i hope I'm correct and I hope this helps :) Its something to do with hybridization I think but I don't know much about that, its not on my curriculum.
DEAdmanstree 2ok It's chemically stable. It's volatile because they only have induced-dipole intermolecular forces of attraction to keep them together. Benzenes delocalised π electron cloud is good at dissipating electron density so these are especially weak.
@@MaChemGuy I know but still you are monotonous but that's the only problem and you should also increase the audio of your videos because I have to put it to max to listen
I really have no idea how to thank you!!!! You Sir, are a life saver!!
Kareem Abourafia There's my good deed for the day sorted then
It would be really useful if you put a relevant exam q in your videos as a plenary! Your vids are v helpful!
I've been retaking my A level chemistry exam by myself this year cause i need an A and your vids are the only thing helping me push my grade up. Just wanted to tell you thank you so much for the vids.
Khaled Jama Really kind of you to get in touch to say that. Good luck, you’ll have to let me know how you get on
So glad i was recommended your channel, you're the best
A much better explanation than any textbook or a level science website I've looked at. Wish I'd found this channel sooner!!
Better late than never. Thanks for that 😊
This is an absolutely terrific explanation. Thank you!
the way you explain it makes it sound so simple and intresting, thank you alot!
wow this man has really help me to understand how the pie bonds forms the delocalised cloud. thank you very much sir
Oh my! Thank you so much for this I can't even begin to explain how much this has helped me! :)
Catherine Haas You're very welcome, glad they're helpful :)
thank you. was struggling conceptualising the delocalised electrons in the p-oribitals. helped a lot
Thank you so much!! This is exactly what I needed.
this is awesome, thank you so much!!
Thank you!! Finally understand this.
Thank you ! So helpful!
this was explained so beautifully
Sir,my book has the structure you made at 11:53 and it says underneath it
"According to this molecular orbital picture each c-c bond in benzene consists of full sigma and half pi bond.Because of this reason c-c bond is equal and benzene shows substitution as well as additional reaction"
Could you kindly elaborate this? I don't get it any of it.
It really helps!!! Thank u so much!
wonderful sir.I am just speechless.may god blesses you sir :D
This helped me so much! Thank you!
Glad to hear it! You're welcome
thankyou so much, this was great!! :)
Matilda Colman Glad you thought so! Thanks
Life saver 💙
This was very helpful. Thank you !!
You're welcome
I LOVE YOU FAM!!!
Hello, thank you for all your help sir, I really understand this well now :) ,
I just had one question or confusion, you know the electron configuration of c is 1s2,2s2,2p2 so the carbon has 2 electrons in its outer shell ? Where does the 2 other electrons come from. I did research and hybridization kept coming up it was hard to understand and if this is the case do all atoms undergo hybridization or is carbon an exception.
Thanks for your help
August Kekule was "energetic and intense" I'm not sure what he took if he did take anything, or if being German had something to do with him, but you should speed up your thoughts a little. tea is great( green tea, caffeine and theanine), but I recommend espresso.
you genius !!
Thank you
you legend ;)
You said electrons will pair up and will be found in this new region, but would they pair up if they repel each other ??
who else watches this to sleep :D
VeriZon Pulse You just made everyone in my house laugh 😭
I watch them before I sleep every night lol😂
Same
Hi, thank you so much for your videos!! You make learning Chemistry bearable :P are you going to be doing anymore videos for F324 and F325 or have you finished now?
Thanks for the comment, glad the videos help. I'm struggling to find the time to make any more at the moment. Hopefully I'll be able to do a few more over Easter but my original plan to have the whole of F324 and F325 done this year isn't looking likely at present. Thanks again and keep watching!
This makes sense... my teachers notes were overwhelming
I've heard that a lot from students. Thanks for getting in touch :)
is everything you need to know for the f324 exam in these videos?
Why would they pair up?
It's been a while since I've done AS so I feel like I've forgotten the basics but can someone explain how each carbon has four electrons, three form sigma bonds and 1 forms a pi bond when there's four outer electrons so shouldn't it be 1s^2, 2s^2 making the fourth electron still in the s?
+A Saeed I know that the first bond a carbon atom makes with another atom is always a sigma bond and if it has a second or third bond with that atom, those are pi bonds.
In benzene there are 3 double bonds so each carbon has a double bond with another carbon and a single bond with a carbon and a hydrogen.
So the bonds that the carbon has to the hydrogen and the singly bonded carbon are both sigma bonds (its the first and only bond the carbon has with the other atom) but in the case of the carbon-carbon double bond one of the bonds is sigma so the second has to be a pi bond.
So that's why there are 3 sigma bonds and 1 pi bond, I think.
Hahahha i hope I'm correct and I hope this helps :) Its something to do with hybridization I think but I don't know much about that, its not on my curriculum.
⌬
Cali Fresh hahahhahaaa guess I'm wrong then. Back to the books! 😎😎
Why does benzene evaporate in room temperature when its stable
DEAdmanstree 2ok It's chemically stable. It's volatile because they only have induced-dipole intermolecular forces of attraction to keep them together. Benzenes delocalised π electron cloud is good at dissipating electron density so these are especially weak.
Think I get it
How shall I ever repay you, Sir?!
Benzene ke outer bond kyo nhi lga skte sir
Increase your volume
when I watch his vids your volume is so low that i need to be on max
and then when an ad plays it breaks my ears cuz it so loud
now also ..its very confusing
Your videos are good
But don't be monotonous cuz i seem to have my mind drift away very easily
Just wait till you get to university then
@@MaChemGuy I know but still you are monotonous but that's the only problem and you should also increase the audio of your videos because I have to put it to max to listen
@@RuhabDabeer good job you don't have to pay for it
Good thing you don’t have to pay for them then
I think you have a better range than Freddie Mercury your videos need more content on salt bridges though tbh
Thank you