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 ❤️ 💛 💚
Every day, just a little bit closer to ClF3 :)
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.
Did you see the little droplets sparking as they fell? Or was that just me?
wait till you find that you can connect flourine with some noble gasses 😊
The fascinating part is that apparently it isn't a molecule: it's actually a salt, chloryl perchlorate ([ClO₂]⁺[ClO₄]⁻).
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.
@@yaykruser You can connect fluorine with chlorine, but it is a TERRIBLE idea.
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?
@@hanztimbreza6217 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...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. 😎
A chemical made with a potent acid, a potential poison, a powerful oxidizer, and ozone, which is sensitive enough that you have to turn the lights down.
That's why I love this channel.
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.
@@alexpotts6520 oh right, yea maybe the vapors from the molten sulfur or a bit of SO2 it produced
Fabulous footage of a substance that I hope never to encounter in person!
I especially liked the slow-motion view of the decaborane decomposition.
I encounter it all the time at my work and it sucks.
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!!!!
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.4286 That sounds like a pretty plausible suggestion.
@@alexpotts6520 then the additional heat from the hot vapors... Seems very plausible
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?
This is very cool! I love to see you carrying out some actual syntheses yourself! 😃
I am in awe, not only of your skills as a chemist, but also your presentation and videography.
Unbelievable, you keep on improving! High quality man, great stuff.
Hmm... will you finally be the person to mess around with the infamous FOOF on Youtube?
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.
"None of chlorine oxides like organic materials" - I'd say they like organic materials a bit too much.
Surrender all your electrons !
@@herrhaber9076 brilliant, thank you for your comment.
Really cool footage, appreciate the great work!
Interesting structure, I would have expected it to have a Cl-Cl bond but instead it is bridged via an oxygen atom...
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'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
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.
I love your channel very much CF. Makes chemistry so intriguing and interesting
AWESOME apparatus in the beginning!!
Always a great video thanks for sharing buddy
Loved the scheme of the video. Keep it up
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
You deserve a million subscribers!!!
Also I love your accent :)
Thanks for your experiments, be careful. You rock.
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.
i absolutely love these videos
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.
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
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
Using lasers to cause explosive detonation? Amazing! And such good footage! I love it, this is so cool!
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, I am afraid, there isn't really a source of electrons in this compound. For alkali metals, they have that one lonely valence electron, that they are very willing to get rid of. However for chlorine, it really hates to get rid of electrons and in this compound it already has "given" oxygen most of its electrons, so it would probably really not want to give up anymore of them. Oxygen and nitrogen probably also wouldn't want to get rid of their electrons and hydrogen in this case also has "given" its electron to nitrogen in ammonia. So I really don't believe there is a way of electrons being dissolved here.
I'd imagine the ammonia actually reacts with the Cl2O6 in this case forming some unstable "ammonium-oxochlorine" compounds that decompose in a short time to chlorine gas, oxygen gas (which we presumably can see forming bubbles) and some derivatives of ammonium and chlorine or something along those lines and the color comes from chlorine gas being dissolved in ammonia temporarily, since chlorine gas usually is yellowish to greenish and the shift in color can be caused by the ammonia environment, similarly to how iodine solutions can be brown with certain solvents instead of the purple color iodine usually has. Or the blue color comes from some of the intermediary products (probably some radicals, which usually also are colorful).
But that's also just a guess based on intuition, might as well be electrons trying to get the hell out of there
Wow , I really want to point out the pipet shattering at 8:24 ,, Amazing
CGI artists need to watch this channel for inspiration. Real explosions look cooler than what is often in movies.
You are getting closer and closer to ClF3 ;-)
interesting.. Thanks for such informative video
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.
Thanks for sharing this important vid + + +
Suuper! Thank you very much!
Well, with a formula like Cl2O6, I'm sure this chemical is very happy to exist and incredibly stable
Blue tinge in ammonia: Solvated electrons maybe?
That's it! 👍
I am loving this
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.
Great videos. It would great if you could add the time in ms during the slowered parts 😁. The quality is 👌
@spiderdude2099 - 2022-04-22
It’s entirely possible the sulfur burning emitted the same required wavelength of light to decompose the Cl2O6
@experimental_chemistry - 2022-04-22
That's it! 👍
@spiderdude2099 - 2022-04-22
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
@steam6626 - 2022-04-22
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.
@spiderdude2099 - 2022-04-22
@@steam6626 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.
@experimental_chemistry - 2022-04-23
@@steam6626 In science, the simplest solution is always the most likely... ;-)