What a nice channel... I'm very glad I found you from explosions and fire... You have all these cool unique chemicals that I haven't seen anywhere else on UA-cam
Liquid Ozone looked like tiny blue/lavender hemispheres in the dish. The liquid oxygen didn’t seem to coalesce the same way. Your photography cannot be beaten.
Mate, if my chemistry teacher in school was more like you, I would probably have Doctorat in chemistry too... Amazing reactions, a pinch of danger, and a ton of useful knowledge! Love it!
Ohhhh I love photochemistry, would be nice to see more of it, so far you are the only youtuber outside college student videos and demonstrations performing them.
It's one of those reactions where tarring occurs and tarring results in different reaction products every time! Which makes coming up with any chemical ecuations unreal. It's just a funny experiment that shows a clear example of photochemical reaction ;)
probably not a good idea from a legal point of view to show the equations (you only want qualified professionals doing this, not the average john q. public who might get hurt because the don't know the proper safety precautions.)
@@superdave6889 I think they meant the reaction equations (eg. NaOH + HCl => NaCl + H2O), not '3.2mL 1,4-dioxane, 1.3mL liquid Cl2' or whatever. Though I guess the dirtier radical reactions like this one are kinda hard to specify an equation for, since tarring suggests that many locations of what was once the original dioxane molecule are activated (alongside the obvious Cl2 -> 2Cl·).
He will not write any formulas or details! Can't you see what level his channel is and who is it for? It is designed for morons and assholes. The goals of his channel are not to enlighten and educate, but rather to make stupid idiots out of people! I wouldn't be surprised if he has or is going to make a video of how he will fart and set it on fire. And it will gain the maximum views, because such is its audience!
The halogen radical Cl° may only attack at two positions... 1) at one of the 4 equivalent CH2...(those are «activated by the linked electronegative O atom) thus leading to a 2-chloro-1,4-dioxane (chiral site thus forming R and S) setting a H° radical free that will be happy to fix to a Cl° one or to attack a Cl2 to form a Cl° and forming a HCl molecule. The halogen compound formed must be laccrymatory and irritant (closely related to yperite family wargases)... the halogen atom activates further the CH group for an easier removal of the H by a Cl radical... thus forming a 2,2-dichloro-1,4-dioxane. Then we may have ring opening to form two ends a - CCl3 and a °O-CH2 - (hidden form of O=CH- + H°)... Then further halogenation of the CH2 between the ether linkage and the (electron withdrawing group - EWG) -CCl3 or the one between the etheric bond and the aldehyde group (also a strong EWG)... You may have splitting of the °CCl3 of CO or even O=CH° and further halogenation. 2) Formation of unstable Cl-CH2-CH2-O-CH2-CH2-O-Cl Organic sp2 hypochlorites are explosive or spontaneously decomposed to HCl and aldehyde In this case Cl-CH2-CH2-O-CH2-CH=O wich will follow the same kind of reaction as the first scenario but first between the aldehydic EWG and the ether link... 3) a mix of 1) and 2) 4) a mix of photochemical, thermally induced chemical reactions and cracking... PHZ PHILOU Zrealone
@Eduardo Gentile Cl2 can display two kinds of cleavage... 1) heterolytic what means Cl-Cl --> Cl(+) + Cl(-) One of the two chlorine atoms has lost one external electron (therefore the + charge) 6 remains as 3 non binding electronic doublets... the other atom has gained one electron (what explains the negative charge)...that atom would then display 8 external electrons as 4 non binding doublets. 2) homolytic Cl-Cl --> 2 Cl° You thus get two identical atomic chlorine radicals displaying each 7 électrons... 3 non binding doublets and a reactive free electron. This last may happen under certain energy level by heat or by radiation (light in this case). The two phenomenons may happen at the same time but there is always a statistical occurence background linked to the surrounding (experimental conditions of heat/temperature, pressure, reactor wall nature, catalyst or inhibitor,... and light wavelenght) Here the laser light has sufficient energy to generate statistically enough free radicals that the reaction goes runnaway...self sustainable.
From what I could find it looks like the sky is the limit for chlorination of 1,4-dioxane (the sky being 7). The primary species is heptachloro-1,4-dioxane, which implies that you'll get everything between that and just chloro-1,4-dioxane below saturation. From what I've personally found, chlorination is worse than nitration when it comes to getting a single species. I've had a few experiments ruined/contaminated by exposure to fluorescent lights and blue based white LED lights.
@@philouzlouis2042 Doesn't make sense to me. I would have thought 8 would be the limit too if you can do 7. Realistically every additional chlorination usually takes a slightly higher temperature. I'm just speculating but maybe at the temperature required for that 8th chlorination the whole molecule becomes unstable enough that theres effectively no yield. Its a lot easier to break up 1,4-dioxane than it is to break cyclohexane. Or what I read could just be plain wrong. It wouldn't be the first time. Either way, using explosive amounts of liquid chlorine and dioxane at an uncontrolled temperature is just going to get you random stuff. Chlorinating acetone (don't) has to be done at a very controlled temperature and at slow rates or it will thermally run away on you and you get garbage.
@@htomerif You must be right. About runnaway of chloraceton... a long time ago (I did tiny amounts of aceton peroxide (cyclo-tri-aceton-peroxide / CTAP (wrongly named TCAP)... once I did the mistake to mix reactants at ambiant temp instead of frozen... so H2O2 (50%), HCl (27%) and propanon were mixed... it heated up, emitted a cloud of white fumes of chloraceton... probably because heat and radical formation from peroxide. PHZ (PHILOU Zrealone)
Fun fact: because the tube is mostly filled with dioxane and chlorine vapor those little pops of fire you see are actually chlorine fires. Chlorine is a strong enough oxidant to sustain combustion even without oxygen.
This reaction is similar to how they remove dioxane from waste water. Dioxane and chloromines react in the presence of UV and destoys the dioxane where the amine radical left react with other chemicals such as antibiotics. This also helps remove chloromines from water supplies.
I' d really love if u' d provide for your next videos mechanisms or at least equations explaining what' s goin on inside of the mixture, i get this is a radical one with tons of secondary products for each radical coupling so it' d be a mess, but take it into consideration. Keep it up dude
The dioxane & chlorine seemed to stop responding to the laser near the end. Were the reactants used up or the soot making the mixture opaque or something else entirely? Great video as always!
To get manageable synthetic pathway one would have to work with a large exces of 1,4-dioxane (or what is the same dilute Cl2 concentration) and/or dimmed light source.
I hate to be that guy, but can someone please tell me what the soundtrack is called? Thank you so much! My favorite scene is when you light the chunks of solid dioxane on fire. Something about the combination of well-defined, glassy crystals melting into a thin liquid while being flammable is uniquely beautiful
I love how you make no comment on the dangers of handling liquid chlorine... but you handle the test tube with a crescent wrench with a stick taped to it. XD
Well, ozone can make nitrates from plain ammonia with no catalysts or special conditions needed. Not only that, ozone can oxidise dinitrogen tetroxide into dinitrogen pentoxide. You can make nitric acid with concentrations _“above 100%”_ by dissolving N2O5 (the anhydride of nitric acid) into nitric acid. Ozone is the coolest substance to do reactions with.
Hey man. Another great video, god bless Chemistry. In 2018 I went to Munich for the 26th IUPAC Photochemistry conference, and my supervisor who's German told us that they were taught at that time that the energy of a triple bond > double bond > single bond doing explosions (combustion?) with alkynes, alkenes, alcanes. Could you compare these explosions ? :D
2:51 is that more green than yellow in real life? It looks yellow, but im told it should be green - does the camera not pick the greenish tinge up very well?
Photochemical reaction are very much interesting and therefore I have wery great request, Dear Mr. could you present reaction deuterium with the fluoride? Tthis reaction is running in the very high power gas laser of course. Other reaction is reaction chlorine with jodine and probably with hydrogen peroxide.
The real scary thing is when you mix something cold with ozonated liquid oxygen and *then* set it on fire. Usually all you get is an explosion. Carbon foam with ozonated LOX is also quite spectacular because of how “benign” the components are, yet it explodes as well. Even charcoal briquettes are enough to show it. Adding LOX to the fire is exciting of course, but spectacular stuff happens when it’s premixed. Of course when premixing you have to keep things clean or it’ll explode then, so eg. charcoal has to be made in the lab to ensure there’s no oil on it; even oil from handling with your fingers can sometimes set things off.
@@absurdengineering hey man, two things, #1 Im a dude posting on my sister's profile because she was the one logged in(still is since I never log in to my own account when im using the desktop) #2 you seem to have some incite about chemistry so I was wondering if I could ask a question that has been baffling me about charcoal vs carbon foam. Why is it that carbon foam is refractory and charcoal is a fuel? I get that charcoal is a hydrocarbon and Carbon foam is just Carbon, but wouldnt burning charcoal just leave carbon foam? I dont understand why carbon burns easily as a hydrocarbon, but is refractory as an element. I obviously haven't had a chemistry class since high school but this has been bothering me.
This was blue light, not UV. Quartz is always good of course, I’m sure everyone would prefer all-quartz glassware to regular glass if they could afford it, outside for some special applications that call for regular glass.
It probably is, but it's physical properties being different meant it didn't mix as thoroughly. If they were both atomised the ozone would surely be more reactive
@@mduckernz I think you are right. But it would be interesting to know what exactly causes that. Ozone seems to remain as drops, so maybe it has very low thermal conductivity compared to oxygen.
Actually, you can make iodine monofluoride from silver monofluoride and iodine, former from hydrofluoric acid and silver nitrate, then extract from acetone. Iodine monofluoride becomes iodine pentafluoride at higher than 0°C.
What a nice channel... I'm very glad I found you from explosions and fire... You have all these cool unique chemicals that I haven't seen anywhere else on UA-cam
Liquid Ozone looked like tiny blue/lavender hemispheres in the dish. The liquid oxygen didn’t seem to coalesce the same way. Your photography cannot be beaten.
"and now we will add liquid oxygen"
*all the chemists take a step back*
And here we get liquid ozone!
Why don't add liquid florine
unknow unknown
No one is _THAT_ suicidal.
exactly 😂
The slo-mo sounds during your chemical reactions are giving me some great ideas for my next noise project! 😄
Mate, if my chemistry teacher in school was more like you, I would probably have Doctorat in chemistry too... Amazing reactions, a pinch of danger, and a ton of useful knowledge! Love it!
Ohhhh I love photochemistry, would be nice to see more of it, so far you are the only youtuber outside college student videos and demonstrations performing them.
Spectacular! I can't wait til you upgrade to 4k60 cameras. This work deserves the best documentation
Photochemical reactions are awesome!
This is so fast! Love this channel and how it’s growing so good, keep up the good work!
You should add in the chemical ecuations.
It's one of those reactions where tarring occurs and tarring results in different reaction products every time! Which makes coming up with any chemical ecuations unreal. It's just a funny experiment that shows a clear example of photochemical reaction ;)
probably not a good idea from a legal point of view to show the equations (you only want qualified professionals doing this, not the average john q. public who might get hurt because the don't know the proper safety precautions.)
@@superdave6889 I think they meant the reaction equations (eg. NaOH + HCl => NaCl + H2O), not '3.2mL 1,4-dioxane, 1.3mL liquid Cl2' or whatever. Though I guess the dirtier radical reactions like this one are kinda hard to specify an equation for, since tarring suggests that many locations of what was once the original dioxane molecule are activated (alongside the obvious Cl2 -> 2Cl·).
He will not write any formulas or details! Can't you see what level his channel is and who is it for?
It is designed for morons and assholes. The goals of his channel are not to enlighten and educate, but rather to make stupid idiots out of people!
I wouldn't be surprised if he has or is going to make a video of how he will fart and set it on fire. And it will gain the maximum views, because such is its audience!
Wow that liquid ozone🤩🤩💯 . What a beautiful bluish color!
Liquid ozone is sooo beautiful! It is my favourite color :)
That ozonated LO2 was as rich in color as a strong solution of CuSo4, just not as dense when poured.
Nice Leidenfrost effect with the oxygen and ozone
The halogen radical Cl° may only attack at two positions...
1) at one of the 4 equivalent CH2...(those are «activated by the linked electronegative O atom) thus leading to a 2-chloro-1,4-dioxane (chiral site thus forming R and S) setting a H° radical free that will be happy to fix to a Cl° one or to attack a Cl2 to form a Cl° and forming a HCl molecule.
The halogen compound formed must be laccrymatory and irritant (closely related to yperite family wargases)... the halogen atom activates further the CH group for an easier removal of the H by a Cl radical... thus forming a 2,2-dichloro-1,4-dioxane.
Then we may have ring opening to form two ends a - CCl3 and a °O-CH2 - (hidden form of O=CH- + H°)...
Then further halogenation of the CH2 between the ether linkage and the (electron withdrawing group - EWG) -CCl3 or the one between the etheric bond and the aldehyde group (also a strong EWG)...
You may have splitting of the °CCl3 of CO or even O=CH° and further halogenation.
2) Formation of unstable Cl-CH2-CH2-O-CH2-CH2-O-Cl
Organic sp2 hypochlorites are explosive or spontaneously decomposed to HCl and aldehyde
In this case Cl-CH2-CH2-O-CH2-CH=O wich will follow the same kind of reaction as the first scenario but first between the aldehydic EWG and the ether link...
3) a mix of 1) and 2)
4) a mix of photochemical, thermally induced chemical reactions and cracking...
PHZ PHILOU Zrealone
@Eduardo Gentile
Cl2 can display two kinds of cleavage...
1) heterolytic what means
Cl-Cl --> Cl(+) + Cl(-)
One of the two chlorine atoms has lost one external electron (therefore the + charge) 6 remains as 3 non binding electronic doublets... the other atom has gained one electron (what explains the negative charge)...that atom would then display 8 external electrons as 4 non binding doublets.
2) homolytic
Cl-Cl --> 2 Cl°
You thus get two identical atomic chlorine radicals displaying each 7 électrons... 3 non binding doublets and a reactive free electron.
This last may happen under certain energy level by heat or by radiation (light in this case).
The two phenomenons may happen at the same time but there is always a statistical occurence background linked to the surrounding (experimental conditions of heat/temperature, pressure, reactor wall nature, catalyst or inhibitor,... and light wavelenght)
Here the laser light has sufficient energy to generate statistically enough free radicals that the reaction goes runnaway...self sustainable.
From what I could find it looks like the sky is the limit for chlorination of 1,4-dioxane (the sky being 7). The primary species is heptachloro-1,4-dioxane, which implies that you'll get everything between that and just chloro-1,4-dioxane below saturation.
From what I've personally found, chlorination is worse than nitration when it comes to getting a single species. I've had a few experiments ruined/contaminated by exposure to fluorescent lights and blue based white LED lights.
@@htomerif
Why only 7 and not 8 as the skyline limit? Thus O(CCl2-CCl2)2O... perchlorodioxane
@@philouzlouis2042 Doesn't make sense to me. I would have thought 8 would be the limit too if you can do 7.
Realistically every additional chlorination usually takes a slightly higher temperature. I'm just speculating but maybe at the temperature required for that 8th chlorination the whole molecule becomes unstable enough that theres effectively no yield.
Its a lot easier to break up 1,4-dioxane than it is to break cyclohexane.
Or what I read could just be plain wrong. It wouldn't be the first time.
Either way, using explosive amounts of liquid chlorine and dioxane at an uncontrolled temperature is just going to get you random stuff. Chlorinating acetone (don't) has to be done at a very controlled temperature and at slow rates or it will thermally run away on you and you get garbage.
@@htomerif
You must be right.
About runnaway of chloraceton... a long time ago (I did tiny amounts of aceton peroxide (cyclo-tri-aceton-peroxide / CTAP (wrongly named TCAP)... once I did the mistake to mix reactants at ambiant temp instead of frozen... so H2O2 (50%), HCl (27%) and propanon were mixed... it heated up, emitted a cloud of white fumes of chloraceton... probably because heat and radical formation from peroxide.
PHZ (PHILOU Zrealone)
Fun fact: because the tube is mostly filled with dioxane and chlorine vapor those little pops of fire you see are actually chlorine fires. Chlorine is a strong enough oxidant to sustain combustion even without oxygen.
Is liquid ozone more or less attracted to a magnet than liquid oxygen?
I did a Quick Google and found that it is diamagnetic meaning its reppeled by a Magnet
O2 is diradical therefore it's paramagnetic. O3 hasn't got any unpaired electrons therefore it's repelled by magnet.
@@ilgattopardo3231 Hmmm. Brings up some interesting ideas for concentrating ozone from liquid oxygen...
Everytime I see your videos I wished I had been able to cling onto chemistry :b man that looks nice :) awesome channel
This reaction is similar to how they remove dioxane from waste water. Dioxane and chloromines react in the presence of UV and destoys the dioxane where the amine radical left react with other chemicals such as antibiotics. This also helps remove chloromines from water supplies.
Saw ur channel 2 days ago and watched all videos 😍😍😍, I'm really thinking what I've missed in my life
Can you make a video about polyethylene glycol solution (the self pouring liquid)? (This is the best science channel ever!)
It would be very cool if the reactions were recorded in 60fps.
If you think so, feel free to support my man on patreon :P
I' d really love if u' d provide for your next videos mechanisms or at least equations explaining what' s goin on inside of the mixture, i get this is a radical one with tons of secondary products for each radical coupling so it' d be a mess, but take it into consideration. Keep it up dude
Very interesting and beautifull reactions as always! Never seen any photochemical reactions that are this exciting!
The dioxane & chlorine seemed to stop responding to the laser near the end. Were the reactants used up or the soot making the mixture opaque or something else entirely? Great video as always!
To get manageable synthetic pathway one would have to work with a large exces of 1,4-dioxane (or what is the same dilute Cl2 concentration) and/or dimmed light source.
Amazing 😍 never saw ozone before.
An equation explaining the reaction would be a cool thing. Never the less verry interesting Video
Congrats for passing 16K subs...
Awesome video! That's so crazy!
Really remarkable demos!
Can you do a video about triflic acid?
What is the reaction exactly? 1,4-Dioxane + Cl2 --> ???
Several products, some of which polymerize. But leading ones will be hydrogen chloride, phosgene and carbon tetrachloride.
@@michaelf7093 The devil’s cocktail for inhalation :)
@@absurdengineering Let's pray for the people near the fume hood exhaust...
it would first generate chlorodioxane, and then undergo a series of fancy chain reactions...
@@Mn-Fe-N Our entire body could be considered to run on fancy chain reactions, but I do like to draw a line somewhere and you found it 😅😂
Yassss!!! Wow! I'm loving these videos! OUTSTANDING SIR! ❤️❤️❤️
Vnloo
Photochemistry is pretty fancy. Excellent video, thank You.. :-)
I hate to be that guy, but can someone please tell me what the soundtrack is called? Thank you so much!
My favorite scene is when you light the chunks of solid dioxane on fire. Something about the combination of well-defined, glassy crystals melting into a thin liquid while being flammable is uniquely beautiful
I love fire!
Beautiful
Great video bro. Informative
maybe it's just me, since I'm new to chemistry, but your demonstrations seem to involve relatively exotic chemicals.
Beautiful
Can you a video about LiMnO2?
How has this channel only so few subs?
I love how you make no comment on the dangers of handling liquid chlorine... but you handle the test tube with a crescent wrench with a stick taped to it. XD
Considering how much more reactive ozone is compared to oxygen, I’d love to see liquid ozone reacting with various things
Well, ozone can make nitrates from plain ammonia with no catalysts or special conditions needed.
Not only that, ozone can oxidise dinitrogen tetroxide into dinitrogen pentoxide. You can make nitric acid with concentrations _“above 100%”_ by dissolving N2O5 (the anhydride of nitric acid) into nitric acid.
Ozone is the coolest substance to do reactions with.
Such a high quality video and few likes :(
How did this video go under the radar for me?
Hey man. Another great video, god bless Chemistry.
In 2018 I went to Munich for the 26th IUPAC Photochemistry conference, and my supervisor who's German told us that they were taught at that time that the energy of a triple bond > double bond > single bond doing explosions (combustion?) with alkynes, alkenes, alcanes.
Could you compare these explosions ? :D
Make potassium/rubidium/caesium ozonides by burning the alkali metals in ozone, please!
OZONE Its Beautiful
2:51 is that more green than yellow in real life? It looks yellow, but im told it should be green - does the camera not pick the greenish tinge up very well?
Could u please put an video on chemical...thermodynamics .....
the video quality blows me away each time i watch
You should try some explosion of organic dynamite like NitroGlycerin
Next time, do a reaction of ClF3 with metalic Cesium ! It may be a problem to get ClF3 though...
Amazing video
Photochemical reaction are very much interesting and therefore I have wery great request, Dear Mr. could you present reaction deuterium with the fluoride? Tthis reaction is running in the very high power gas laser of course. Other reaction is reaction chlorine with jodine and probably with hydrogen peroxide.
I love chemistry. I wanted to get into it when I was younger. How elements react. The reason why they do. What they do.
Stardust
Thumbs UP for a mad scientist using "lasers" !!!
Welcome back. Try mixing manganese heptoxide with Dioxane.
Very, very nice!
Have I just seen ozone under a flame of dioxane/oxygen burn a separate blue flame, forming that oxygen?
more reaxion scemes plz
love the videos
Let's make some pure manganese heptoxide !
Video about oxygen allotropes??
O4?
Maybe you should make a colab with nilered
Hey what was the rection but
Is the reaction a halogenation?
Is tarring the production of tar?
I might become a patron just so you can buy a pair of real lab tongs.
When you said you where going to add liquids oxygen to that burning alkane I almost panicked.
The real scary thing is when you mix something cold with ozonated liquid oxygen and *then* set it on fire. Usually all you get is an explosion. Carbon foam with ozonated LOX is also quite spectacular because of how “benign” the components are, yet it explodes as well. Even charcoal briquettes are enough to show it. Adding LOX to the fire is exciting of course, but spectacular stuff happens when it’s premixed. Of course when premixing you have to keep things clean or it’ll explode then, so eg. charcoal has to be made in the lab to ensure there’s no oil on it; even oil from handling with your fingers can sometimes set things off.
@@absurdengineering hey man, two things, #1 Im a dude posting on my sister's profile because she was the one logged in(still is since I never log in to my own account when im using the desktop) #2 you seem to have some incite about chemistry so I was wondering if I could ask a question that has been baffling me about charcoal vs carbon foam. Why is it that carbon foam is refractory and charcoal is a fuel? I get that charcoal is a hydrocarbon and Carbon foam is just Carbon, but wouldnt burning charcoal just leave carbon foam? I dont understand why carbon burns easily as a hydrocarbon, but is refractory as an element. I obviously haven't had a chemistry class since high school but this has been bothering me.
Awesome
Are u using quartz “glass” since ordinary glass absorbs UV light?
This was blue light, not UV. Quartz is always good of course, I’m sure everyone would prefer all-quartz glassware to regular glass if they could afford it, outside for some special applications that call for regular glass.
Where are the chemical equations? I understand these reactions are complex, but please give us some possible reactions.
Would be nice if you could add the reaction equation
could it work with chlorine tablets?
Do *HSbF6* ! And use a title like "floroantimonic acid vs x" !!! You will get more than 1m views.
How to get the difference between ozone and on ozone LO？
amazinggggggggggggg
Please do a video on 2,4,5 Trioxin🧟♂️
What in the world was the purple smoke?!
Liquid chlorine dioxide next lol
Does iodine or bromine work?
So, what are the products, here?
My favorite color is now liquid O3
Wow
Try to buy some " Cesium dodecafluoro-closo-dodecaborate " on sigma aldrich !
(I am joking it is faaaar to dangerous)
I expected liquid ozone to be *more* reactive, than liquid oxygen, not less!?
It probably is, but it's physical properties being different meant it didn't mix as thoroughly. If they were both atomised the ozone would surely be more reactive
@@mduckernz
I think you are right. But it would be interesting to know what exactly causes that. Ozone seems to remain as drops, so maybe it has very low thermal conductivity compared to oxygen.
anhydrous hydrazine?
Please show the reactions for the videos
I like this movies.I’m Japanese.
Iodine pentafluoride, when you get more subscribers.
Actually, you can make iodine monofluoride from silver monofluoride and iodine, former from hydrofluoric acid and silver nitrate, then extract from acetone.
Iodine monofluoride becomes iodine pentafluoride at higher than 0°C.
dioxane+chlorine=???????? ???????? Where the equation reactions?
LOL watch it burn as I add *liquid oxygen* ....nice
money heist😜
Za warudo
Nice video ..please watch Dr Zakir Naik's videos
3:16 There is no a super like for this. :/