Thanks a lot. You don't understand how much you are helping people from around the world. I can't thank Khan Academy enough for doing what they do. Keep it up!
I personally think that Khan Academy is the best source of online learning. When I first encountered this youtube channel i thought for a second. wait "Would I be able to understand,possibility are there might be few terms which might be used in the video which might not be explained or talked about in my reference book" But trust me, it covers every single term and concept. I sometime wander whether he had read my course book or what lol
Ok. I barely studied this entire semester, got 71, 42 and 50 on my 3 tests and 90 on my final. Thank you so much, I literally learned organic chem I in one night, and aced my final. I honestly just dont get it why cant the teachers be like you, you're so clear and your explanations are wonderful! Thanks again Sal :)
Hey Khan, it would be cool if you could put up some videos about retrosynthesis(working backwards) and Lindlar's, NaH, NaNH2, Pd/C and all that jazz. That'd help me out a lot in my ochem class
when you realise even at alevel uk they dont go over basic uni notation... ie sn11/2 e1/2 i mean we are taugh it but not explicitly told what sn2 is etc or the differences
During a UV free radical chlorination you say to use UV light. So just for fun I used the formula E=hf and figured out the charge in joules of a 400 nm UV light (6.626 X 10*-19 J) which is the WEAKEST UV wavelength and I found out it is more than enough joules for homolytic bond cleavage not only in the chlorine BUT ALSO in a Cl/C bond. I found the dissociation bond energies from charts on line. So let us say I have DCM and want to make tetrachloromethane. So if I use the weakest UV...…..400 nm then I have enough energy in the UV to not only break Cl/Cl bonds but also the Cl/C bonds that I want to make. THAT DOES NOT MAKE SENSE ?????????????????? Let us say I want to make benzyl chloride. 400 nm UV light is SLIGHTLY more joules needed to break a benzyl C/H bond (6.26 X 10*-19 J) and WAY MORE THAN ENOUGH to break a benzyl C/Cl bond. Do you see my point. As I make the product the UV light is enough energy to destroy what I make. So how does it work??????????????????? Also the UV light at 400 nm is enough to turn the whole pot of toluene into benzyl radicals that combine with each other as much as the chlorine.....it seems like that would not be good??????????????????????????? Also I looked up the energy needed to break a Cl/Cl bond (4 X 10*-19 J) and that corresponds to a light source of ABOUT 500 nm...……..WHICH IS GREEN VISABLE LIGHT. Although at this point I was really frustrated and started doing math in my head but it is close. So now I am really confused because that means you do not even need UV light to make Cl free radicals. SO is this true?????????? Can I make Cl free radicals with green visible light?????????? IF SO THEN WOULD IT NOT BE BETTER to use 450 nm blue visible light with NO UV light. That way the photons are slightly under the energy needed to break benzyl Cl/C bonds and benzyl C/H bonds and in the case of an ALKYL chloride blue light is not enough to break Cl/C bonds. BUT blue light is good enough to break Cl/Cl bonds so your product wont be destroyed as you make it by UV light. I thought I had a good understanding of free radical halogenation until I did the math. WHAT IS THE DEAL. HELP ME HELP ME HELP ME PLEASE
the overall reaction is CH4 + Cl2 > CH3Cl + HCl so if once through homolysis chlorine free radicals are formed after breaking the only Cl molecule..then where did another Chlorine molecule come from?
+Heisenberg Edison dude, do u kno about the conditions of Pakistan which is an Islamic Republic? if we are Muslims, why would we be killing our own kin? These things hav to be thought about with a chilled mind.
Hey there! I wanted to stay thanks for helping me throughout my MCAT studying! However, I thought when Methane reacts with the first chlorine radical and becomes methyl chloride, a second Chlorine is NOT able to react with the methyl chloride create because the C-H bond is no longer weak? In fact, the weakest bond becomes the C-Cl bond because the carbon becomes somewhat positive, so the C-H bond is not that polar, and thus, strong. So it would just replace the current C-Cl bond for another
i love how he says everything twice, like he knows i am easily distracted XD
i wonder what this guy is up to nowadays.
@@OER888 he's into... oh wait, he got distracted
I love how casually you guys are chatting like frd😏😂😆
@MrUnladenswallow definitely 😂
How are u all.... Still alive ?
Thanks a lot. You don't understand how much you are helping people from around the world. I can't thank Khan Academy enough for doing what they do. Keep it up!
make donations if you really wanna help them
Behnam Ghane is this your voice in above videos
@@rezapahlaviisking .
Baba Khan no
I only liked ur comment bcuz u like GnR
I personally think that Khan Academy is the best source of online learning. When I first encountered this youtube channel i thought for a second. wait "Would I be able to understand,possibility are there might be few terms which might be used in the video which might not be explained or talked about in my reference book" But trust me, it covers every single term and concept. I sometime wander whether he had read my course book or what lol
I also had the same problem to. Thank God n thank Khan Academy for making it easy for us.
explained better than my professor!
Ok. I barely studied this entire semester, got 71, 42 and 50 on my 3 tests and 90 on my final. Thank you so much, I literally learned organic chem I in one night, and aced my final. I honestly just dont get it why cant the teachers be like you, you're so clear and your explanations are wonderful! Thanks again Sal :)
How's life now? It's been 10 years 😄
@@kyonhihorahipadhaifr r u a scientist now a doctor what happened 😂
@@hegresal-jubury8839 Yeah, we're curious 😸
No reply unsuccessful 😂
why cant you teach at my uni!! you are the best seriously Ive been watching your videos since high school .
Not all Heroes wear caps
Leen Minr capes
moops
Idk any heroes that wear caps tbh
So True
some wear capes
btw... 4 mins 55 secs (approx) in he says ''the carbon does the same'', i think he means chlorine
Imagine making a video that is watchable even after 13 years
1:42 "if it was upto me"................well dont worry sal its completely upto you....the future of chemistry is in ur hands :P
You made me love chemistry. Thank you so much.
Had to watch it twice..got distracted by my face staring back at me.🙃
🤣🤣
At first I was put off by the rough diagrams but you helped me understand this a lil more. Will surely be returning throughout my A-levels! :)
Love how you repeat words :P Thanks man
Respected sir ,
I am just mesmerised with your teaching .I am from India sir lots of love to you sir
Explanation that even a dumb like me can understand! Thank you so much, and nice job!
but a dumb like me don't even understand :´´(
@@03raq lol
Thank you so much for posting this! Now, I've finally understand what free radical reaction really is about..! =)) Keep up the good work! ^^
I love how he repeats stuff! :)
this is one of the best educational channels out there .
Thank you so much for this video!!! 😭😭❤️❤️❤️❤️❤️💕💕💕💕💕💕
You've helped me a lot!!!!! Love yaaa! ❤️💕💕💕💕💕
Love you Sal beautiful voice but most importantly you have the ability to teach concepts better than any other
I love this guy. Seriously 😂😂. He can explain in simpler way than my chemistry lecturer.
I got an A on my quiz because of this video!!
i have no words to thanks the great khan academy....
thank you so much, it makes so much more sense
how to know which molecule forms bonds with which molecule.
11:26 .
why chlorine formed bond with hydrogen only, why not other molecules??
Thank you for the clear presentation. very helpful
Thank you so much! You're a life saver. When I become rich I'll make sure to donate lots to Khan Academy. You guys are absolute legends!
i hope youre a millionaire by now
@@bonk_rl i failed my A levels LOL
Dw just ask me again in 5 years and I’ll say yes
@@STICKY_ that's the spirit!
@@STICKY_ i hope ur a billionare by now 😅...
Explained better than my Ph.D
Thank you so much Mr Khan! After weeks of trying to understand this process it finally makes sense after watching your video. Thank you.
Nice explanation sir!!!
many thanks khan, using your videos for a lot of my upper division classes now
Thanks a lot it has really helped me
These videos help me out soo much! Thanks @khanacademy and this man's voice! :D
at 4:54 did he mean Cl and not carbon?
THANKS A BILLION!!!
Hey Khan, it would be cool if you could put up some videos about retrosynthesis(working backwards) and Lindlar's, NaH, NaNH2, Pd/C and all that jazz. That'd help me out a lot in my ochem class
thanks khan academy.............u helped me for my chem exam
You just have to love the voice of sal😅
when you realise even at alevel uk they dont go over basic uni notation... ie sn11/2 e1/2
i mean we are taugh it but not explicitly told what sn2 is etc or the differences
Thanks for the help! Science Fair in a couple of days... So pumped!
During a UV free radical chlorination you say to use UV light. So just for fun I used the formula E=hf and figured out the charge in joules of a 400 nm UV light (6.626 X 10*-19 J) which is the WEAKEST UV wavelength and I found out it is more than enough joules for homolytic bond cleavage not only in the chlorine BUT ALSO in a Cl/C bond. I found the dissociation bond energies from charts on line. So let us say I have DCM and want to make tetrachloromethane. So if I use the weakest UV...…..400 nm then I have enough energy in the UV to not only break Cl/Cl bonds but also the Cl/C bonds that I want to make. THAT DOES NOT MAKE SENSE ?????????????????? Let us say I want to make benzyl chloride. 400 nm UV light is SLIGHTLY more joules needed to break a benzyl C/H bond (6.26 X 10*-19 J) and WAY MORE THAN ENOUGH to break a benzyl C/Cl bond. Do you see my point. As I make the product the UV light is enough energy to destroy what I make. So how does it work??????????????????? Also the UV light at 400 nm is enough to turn the whole pot of toluene into benzyl radicals that combine with each other as much as the chlorine.....it seems like that would not be good??????????????????????????? Also I looked up the energy needed to break a Cl/Cl bond (4 X 10*-19 J) and that corresponds to a light source of ABOUT 500 nm...……..WHICH IS GREEN VISABLE LIGHT. Although at this point I was really frustrated and started doing math in my head but it is close. So now I am really confused because that means you do not even need UV light to make Cl free radicals. SO is this true?????????? Can I make Cl free radicals with green visible light?????????? IF SO THEN WOULD IT NOT BE BETTER to use 450 nm blue visible light with NO UV light. That way the photons are slightly under the energy needed to break benzyl Cl/C bonds and benzyl C/H bonds and in the case of an ALKYL chloride blue light is not enough to break Cl/C bonds. BUT blue light is good enough to break Cl/Cl bonds so your product wont be destroyed as you make it by UV light. I thought I had a good understanding of free radical halogenation until I did the math. WHAT IS THE DEAL. HELP ME HELP ME HELP ME PLEASE
I had lost my mind after reading this sir🤣😂
You are the best😢😢😢😢😢😢😢
lol I am so subscribing!!! you are really good explaining! I get extremely lost in my chemistry class. Thank you so much!!
I think that's cause youre smart - with all due respect and acknowledgement to Sal.
You the man Khan. Never change #ATownBeBallin
You help me a lot! I am ever so grateful : ) Keep it up, you're great!
Love khan academy...amazing !!!!
best teacher ever!
God bless you😭💜💜
Man you're a genius teacher.
very useful thank u !! 😫😫❤️❤️
superb.. thankss a lot i really gotr a lot of help
the way of teaching is very good 👍
I wish you were my lecturer
thank you so much...i'm am goin to ace my first year finals...oh yeah....:D
its been 8 yrs how did u do?
@@ZAsym I don't need sleep, I need answers.
@@kamaya9907 mine went well, I’m happy with my grade :D
thank-you, lots of love
bless Sal Khan's soul
Thanks Khan.
Thank you. You saved my life.
the overall reaction is CH4 + Cl2 > CH3Cl + HCl
so if once through homolysis chlorine free radicals are formed after breaking the only Cl molecule..then where did another Chlorine molecule come from?
your explanations are great!
excellent explanation !! Thanks a lot !!
Thank You so much!!
Great stuff man! The repeating is fine and actually helps.
Keep doing what you do!
You should've seen my face when everything started making sense lol. Thanks for the amazing explanation
Godly explanation cheers!
thank for this vedio..
cheers khan academy, first time watching one of your videos and I am very impressed
Like, i really love your videos and just the whole institution. Thank you.
Why would the free radical of methane not react with the other free radical of chlorine?
Thank you very much Khan Academy, you have really been a great help to me, very clear and easy to understand. Keep up the good work. :-)
+Heisenberg Edison what's your problem. u have issues big one at that
shut up
yes, u, world @#$%$!
any prob? then keep it to ur butt
+Heisenberg Edison
dude, do u kno about the conditions of Pakistan which is an Islamic Republic? if we are Muslims, why would we be killing our own kin? These things hav to be thought about with a chilled mind.
THANK YOUUUUUU I LOVE YOU MAN !!!!! YOU SAVED MY LIFE
What :(
lol okay
excuse me?!
Thanks so much I have never thought I would understand this reaction😊❤
THANK YOU SO SO MUCH! I WOULD FAIL SCHOOL WITHOUT KHAN ACADEMY
Great video!
It saved my Chemistry exam!!!!!
Beautifully explained sir !!!
Thank u
thanks sir .. u really gave me a proper understanding about the steps and radicals
thank you khan sir
Watching from Bangladesh
may god bless u brother, like fr
Thank you sal!
Thanks a lot!
thank you sooooooooooo much!
thanks!!
720p looks amazing!
THANKS AGAIN......
Thank you
wow! radical man.
THANK YOU MY BROTHER
i like this video!
Thanks for ur help!! :D
Thank you very much
love the video really good
Gracias.
Hey there! I wanted to stay thanks for helping me throughout my MCAT studying! However, I thought when Methane reacts with the first chlorine radical and becomes methyl chloride, a second Chlorine is NOT able to react with the methyl chloride create because the C-H bond is no longer weak? In fact, the weakest bond becomes the C-Cl bond because the carbon becomes somewhat positive, so the C-H bond is not that polar, and thus, strong. So it would just replace the current C-Cl bond for another
Instructor non-verbal cues purssued im a punk. Glad this video! Diction is good for academic colab commnication.
you saved me
ektu pore presemtatiom ase
Good. Keep on going.