ChemicalForce - 2022-04-22
In this video we'll get Cl2O6 by pouring dilute H2SO4 to the mixture of oxalic acid and KClO3 REACTION TIMING: 🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥 0:00 Dichlorine Hexoxide making 2:08 Freshly made Cl2O6 testing 4:09 Dichlorine Hexoxide + Lithium Aluminum Hydride 4:34 Dichlorine Hexoxide + Acetone 5:03 Dichlorine Hexoxide + Methyl acrylate 5:45 not fresh Cl2O6 testing 7:10 Dichlorine Hexoxide + Decaborane 7:32 Carbon disulfide + Chlorine dioxide (CS2+ClO2) 7:38 Dichlorine Hexoxide + Carbon disulfide (CS2+Cl2O6) 8:33 Dichlorine Hexoxide + Molten sulfur 9:17 Dichlorine Hexoxide + NH3 liquid 9:55 Patrons ❤️ 🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥🔥 ✔️ So if you enjoy what I do, and would like to help me to buy chemical reagents and equipment, as some of my viewers do, I will be glad to see you as a member of my Patreon! 😍 ❤️ 💛 💚 Creating these videos is very expensive and hard. But your support helps me a lot! Patreon: https://www.patreon.com/ChemicalForce Ko-Fi: https://ko-fi.com/chemicalforce PayPal: @chemicalforce Bitcoin BTC: 1828WxhTtqohRiQBHgKtdqrmxsGncsjva2 ❤️ 💛 💚
It’s entirely possible the sulfur burning emitted the same required wavelength of light to decompose the Cl2O6
That's it! 👍
You could even test this by lighting some sulfur and bringing a watch glass or small vial with some Cl2O6 in it and holding it over it. If it detonates it couldn't possibly be because it was contacting the sulfur, but just because the light from the sulfur initiated the decomposition
It‘s also possible that a droplet of molten sulfur flew into the drop of chlorine hexoxide on the pipette, some of the sulfur was flying in the right direction die this to happen.
@Steam yeah I think it’d be interesting to do a test where detonation due to contact or vapors would be impossible, but light could get through and to see what happens.
@Steam In science, the simplest solution is always the most likely... ;-)
Man...I've been wanting to synthesize this stuff for months, mainly to see what it's like. So glad I could see it for the first time on your channel, and in such high quality! Keep it up man!
I know what you mean, me too. 😎
Any time I hear 'liquid ammonia" and there's smokey blue colors involved, I'm always going to guess that it's solvated electrons in high enough concentration to be 'seen' in aggregate.
That's the most likely explanation.
Why would electrons emit a blue colour when solvated?
@Hanz Timbreza Well, it may be a phenomenon attributed more to the solvent than the electrons for all I know, but I know solvated electrons in liquid ammonia looks blue.
This was my first thought too. Maybe you can test it by adding something that can be Birch-reduced as some sort of "trapping agent", like a methoxynaphthalene => tetralone
Lol, that was my initial resposne too. Liquid ammonia? Blue tinge? Probably something to do with electrons.
Man, Dichloride Hexoxide is some exciting stuff, especially with a powerful detonation with Methylacrylate, and some certain organic compounds. I am also surprised that the Dichloride Hexoxide liquid just detonate instantly in the pipette when it's in the Sulfur vapor (the smoke that's coming off the molten Sulfur). That's scary.
What a potent oxidiser! I've read about its fabled reactivity in the trusty chemistry textbooks, but this is the first time I have ever seen its oxidising power being demonstrated.
STUNNING IMAGES of even more stunning and exotic chemicals. Love it! I had hoped to see more of the synthesis and physical properties of the stuff. More melting, crystalization, viscosity, stability (time-lapse), reaction to the 405nm light, and hardness at, and at ultra deep temperatures (LN2), even if this seems boring. The Oso4 and Cs melting and crystalization a few weeks ago were out of this world.
Are you a fellow thunderf00t viewer?
I'm curious about the stability of this compound over time. If fresh product is more reactive than aged product, i would assume there is some spontaneous decomposition or subreactions going on. It would be interesting to test the reactivity over time to see if there is a predictable arc.
You are definitely the chemist I learn the most advanced stuff from. I mean, each person does have their own new thing they add, but this kind of chemical just didn't have a way of existing in my imagination and I love it when I learn like that. Thanks for the learning lesson
I am in awe, not only of your skills as a chemist, but also your presentation and videography.
This is very cool! I love to see you carrying out some actual syntheses yourself! 😃
Fabulous footage of a substance that I hope never to encounter in person!
I especially liked the slow-motion view of the decaborane decomposition.
Awesome! As Sulfur burns with a blue flame and the explosion occurred immediately after the first drop of Cl2O6 reacted with the Sulfur I suspect, that the emitted wavelengh was just the right one to decompose the rest of it.
I saw on Wikipedia, that Decaborane is supposed to react explosively with CCl4. There was also a big explosion in a company because of this. Could you maybe test that? I would love to test it myself, but sadly I don't have any Decaborane and beside this also no real use for this expensive stuff :D
This video is the best. A while back, Feliks asked for compounds the audience wanted investigated. I mentioned extreme oxidizers like the oxygen fluorides.
While those are too hot to handle (and he may not have access to an elemental fluorine lab,) this is the next best thing.
Well done! That was a complicated set up but by far my favorite video to date. The close up explosion shot in slow mo was beautiful.
This is some of the fastest unique chemical explosions I've ever seen. Great work.
Too bad you missed key frames in the sulfur reaction.
Interesting structure, I would have expected it to have a Cl-Cl bond but instead it is bridged via an oxygen atom...
Unbelievable, you keep on improving! High quality man, great stuff.
Awesome! I love these kinds of crazy reagents, the kind that even the most experienced chemists rarely have an opportunity (or need, aside from causing mayhem) to use.
I take it that this method of chlorine dioxide generation is relative safe compared to a number of other methods. The carbon dioxide co-product, which is inert in this reaction, acts as a diluent, preventing the chlorine dioxide from undergoing explosive decomposition (although, measures to cut out UV defintely help). Some other methods of chlorine dioxide generation are verydangerous. For example, conc. sulphuric acid added dropwise to solid potassium chlorate.
Seeing all the PTFE sleeves we knew from start some serious chemistry is going to happen!
One note: Although the gas is correctly named dichlorine hexoxide with structure resembling that of manganese heptoxide, the dark red liquid condensate is an ionic compound, a mixed anhydride of chloric and perchloric acids.
Think the blue tinge has something to do with solvated electrons like when you dissolve alkali metals in ammonia? I'm nothing approaching a chemist so there's probably many reasons why this isn't the case, but it looks a bit similar to the alkali metals demo at least for a short period of time. Love the high quality footage of these exotic reactions.
Well, with a formula like Cl2O6, I'm sure this chemical is very happy to exist and incredibly stable
That looks like a really dangerous chemical to handle I'm grateful for experienced chemists who know how to conduct these dangerous chemical reactions safely because these types of reactions are far too dangerous for me to attempt so I wouldn't get the chance to see reactions like these without experienced chemists like this channel conducting these experiments safely
This stuff seems like it would be a good candidate for fueling one of those mythical "Pulse Detonation Engines" that used to be all the rage, but suddenly lost popularity among mystery-guessers.
My guess for what happened at 8:56 is the drop from the dropper reacts with contamination from the spattered mixture. You can see it bolt up the tube, and it probably reacted with the rubber squeezy bulb, or simply mixed intimately with the mixtures in the larger diameter part of the pipette, which set it off.
The blue color in ammonia are probably solvated ions or electrons, though I'm surprised they're forming with an oxidizer instead of a reducing agent. That's worth a paper or two: I bet Thunderf00t would be interested.
I think that Cl2O6 in pipette might explode because of the light coming of the burning sulphur.
Very good theory. If he tried it again but wrapped the pipette in say black paper it should block enough light to verify this.
Another sugestion would be that the burning sulfurs gases contained sulfur vapor or S02 which might react further to S03
@H. A. That sounds like a pretty plausible suggestion.
@Alex Potts then the additional heat from the hot vapors... Seems very plausible
Really nice Video!!
But you easily could turn it into a "great" one if you would add / describe the reactions a bit more in detail.
It is really entertaining for now.
But you could also teach the chemistry behind (maybe 1part showing the compound in action + 1part where you describe the reactions in theory!? Especially the photo-reactivity is a very interesting property to look at!)
Thanks for your work, keep going!
I'm surely not the only one who enjoys both the way you present and your accent 😎🙇♂️ it's like the perfect combination of calming and informative
"None of chlorine oxides like organic materials" - I'd say they like organic materials a bit too much.
Surrender all your electrons !
@Herr Haber brilliant, thank you for your comment.
I'm surprised you used teflon tape with that brand of condenser, I've had a bad experience with that exact brand of glassware and using teflon tape to seal the joints, the condenser joint snapped and I impaled my wrist on it (4 stitches needed), along with the other flasks and glassware from that brand has multiple defects and also bubbles in the joints
great video as always though
Many people don't even know Cl2O6 and you are here working with it! My dream has come true cause I always wanted to see these extremely rare ones!!! Thanks a bunch man! Your channel is one of the few reason I'm still into Youtube!!!!
This guy knows what's he doing.
On potential understated danger scale beats Nile Red, Styropyro, Cody, Creosan and even Explosions&Fire (Extractions&Ire) singlehandedly.
This seems close in volatility to what i did in adolescence, but there were no cameras and the apparent impeccable safety precautions 25 years ago at mine. Pity i haven't touched volatile chemistry since, cannot answer exactly what the Cl2O6 turns into therevand why it's dark greenish. I can just say, that it's that color, because of it's emulsion reflecting that spectrum wavelengths and absorbing the rest.😆
Getting less than 1/1000 of engagement in comparison to mentioned youtubers might be not fair, but at least it looks like quality over quantity here in comments.
Does anyone knows, what country is this guy from?
Very powerful reagent indeed , feel like the molten sulfur explosion just made à detonation so strong it blew up the pipette
It didn't though, you watch the slow-motion footage and the stuff on the spatula doesn't react, the explosion is happening in the pipette.
My theory is that it's nothing to do with the sulfur at all, it might be as simple as a previous explosion getting trace amounts of the stuff into the pipette, which then caused a further explosion.
@Alex Potts oh right, yea maybe the vapors from the molten sulfur or a bit of SO2 it produced
Using lasers to cause explosive detonation? Amazing! And such good footage! I love it, this is so cool!
Regarding the question with decomposition in the pipette: perhaps the sulfur catalyzed the self decomposition, when a tiny drop came into contact with the Cl2O6 in the pipette.
You could test it, by adding a tiny piece (vastly sub stochiometric) of sulfur to some drops of Cl2O6.
Watching the small drops spray up I think your right.
Low hanging fruit: Acetone is three syllables. Ah-seh-tone. (I had to go check to make sure I hadn't been saying it wrong!)
Higher branch: Surprised myself when I guessed the blue in the reaction with ammonia was free electrons (assuming the other comments are right). Does that also account for the green, or is that the blue colour mixing with the diluted orange colour?
It's crazy seeing the CL2O6 reacting before the laser actually touches it, due to reflected light
I love your channel very much CF. Makes chemistry so intriguing and interesting
Really cool footage, appreciate the great work!
Great videos. It would great if you could add the time in ms during the slowered parts 😁. The quality is 👌
The reaction with Methacrylate was very violent. Was this the notorious "explosive polymerisation" I've heared about?
What a fascinating energetic, no way ide be brave enough to try the synthases of that one, i wonder if as some one else pointed out, weather the initial combustion of the sulfur which burns with a deep blue 447'ish nanometer flame was enough to trigger photo-decomposition of the Cl2O6, fascinating & scary compound, does Cl2O6 have any practical real world use apart from making big bangs in the fume hood & smelling horrific & deadly ?
Excellent video as always, you get to work with some amazing & downright strange compounds.
Oh wow, but there was no light flash from sulphur ... although it seems plausible enough.
Collab with The slow-mo guys! I love your slow motion content and interesting reactions, when they are super fast like with these super reactive compounds it would be cool to see even slower, and bring out some great chemistry content to a wider audience :)
Cl2O7... pcerchloric acid anahydride, reactive is an understatement. Pretty brissant and stupidly sensitive as an explosive too. You are a god level chemist. Tbh i would be scared to make that much of this compound which is a little to the left of Mn2O7 🤓😲😁
The content is truly unique. Although the experiments are very dangerous
We should try and pour sodium/potassium NaK liquid alloy into the red stuff and see what happens next. It might be a “ground breaking” result.
Can this channel get million subscribers ? It deserve that, keep your good work! 👍😇
Thanks for your experiments, be careful. You rock.
Fascinating videos. I think the blue color from reaction with Liquid Ammonia is probably Dinitrogen Trioxide (N2O3).
StuffandThings - 2022-04-22
I'm more surprised that such a molecule can exist at all than I am at how reactive it is. That is... a concerning amount of highly reactive atoms packed together.
Mollykinni - 2022-04-28
Did you see the little droplets sparking as they fell? Or was that just me?
Yay KRUSER - 2022-12-26
wait till you find that you can connect flourine with some noble gasses 😊
Fattest Pigeon - 2022-12-30
The fascinating part is that apparently it isn't a molecule: it's actually a salt, chloryl perchlorate ([ClO₂]⁺[ClO₄]⁻).
Philosophersthought - 2023-01-02
Not really surprizing at all, since this molecule (or salt) doesnt exist freely in nature i.e has to be synthesized. Any naturally made (if conditions are right, unlikely) would just decompose into other more stable agents.
Reason why dont find nitroglycerin rocks or mountains (just imagine ! )
Interestingly on the Nitroglucerin front - naturally, we do get volatile amonia based products as byproduct of lightening strikes splitting Nitrogen in air.
SuperTornadoGun - 2023-08-11
@Yay KRUSER You can connect fluorine with chlorine, but it is a TERRIBLE idea.