Dichlorine Hexoxide - this liquid EXPLODES on laser beam exposure!😱

[@LabCoatz_Science]

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!

[@thehulkamaniabrother2.089]

I know what you mean, me too. 😎

[@spiderdude2099]

It’s entirely possible the sulfur burning emitted the same required wavelength of light to decompose the Cl2O6

[@experimental_chemistry]

That's it! 👍

[@spiderdude2099]

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]

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]

@@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]

@@steam6626 In science, the simplest solution is always the most likely... ;-)

[@AsymptoteInverse]

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.

[@ultrathicc4272]

Every day, just a little bit closer to ClF3 :)

[@AtlasReburdened]

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.

[@hammerth1421]

That's the most likely explanation.

[@hanztimbreza6217]

Why would electrons emit a blue colour when solvated?

[@AtlasReburdened]

@@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.

[@bdnugget]

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

[@AlphaBeta-cf5wf]

Lol, that was my initial resposne too. Liquid ammonia? Blue tinge? Probably something to do with electrons.

[@StuffandThings_]

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]

Did you see the little droplets sparking as they fell? Or was that just me?

[@yaykruser]

wait till you find that you can connect flourine with some noble gasses 😊

[@fat_pigeon]

The fascinating part is that apparently it *isn't* a molecule: it's actually a salt, chloryl perchlorate ([ClO₂]⁺[ClO₄]⁻).

[@philosophersthought9780]

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.

[@supertornadogun1690]

@@yaykruser You can connect fluorine with chlorine, but it is a TERRIBLE idea.

[@nigeldepledge3790]

Fabulous footage of a substance that I hope never to encounter in person! I especially liked the slow-motion view of the decaborane decomposition.

[@kid_missive]

I encounter it all the time at my work and it sucks.

[@garycard1456]

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.

[@heisenbergstayouttamyterri1508]

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 KZbin!!!!

[@ormarion552]

Very powerful reagent indeed , feel like the molten sulfur explosion just made à detonation so strong it blew up the pipette

[@alexpotts6520]

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.

[@ormarion552]

@@alexpotts6520 oh right, yea maybe the vapors from the molten sulfur or a bit of SO2 it produced

[@eshik1255]

I think that Cl2O6 in pipette might explode because of the light coming of the burning sulphur.

[@LFTRnow]

Very good theory. If he tried it again but wrapped the pipette in say black paper it should block enough light to verify this.

[@h.a.4286]

Another sugestion would be that the burning sulfurs gases contained sulfur vapor or S02 which might react further to S03

[@alexpotts6520]

@@h.a.4286 That sounds like a pretty plausible suggestion.

[@h.a.4286]

@@alexpotts6520 then the additional heat from the hot vapors... Seems very plausible

[@chrispza]

I am in awe, not only of your skills as a chemist, but also your presentation and videography.

[@AJ-qv9yo]

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.

[@Gameboygenius]

Are you a fellow thunderf00t viewer?

[@Ambient_Scenes]

This is very cool! I love to see you carrying out some actual syntheses yourself! 😃

[@Dr_Mario2007]

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.

[@reneceulemans]

Unbelievable, you keep on improving! High quality man, great stuff.

[@BradSchmor]

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.

[@StuffandThings_]

Hmm... will you finally be the person to mess around with the infamous FOOF on KZbin?

[@Mirthfull]

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.

[@LiborTinka]

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.

[@ArchDudeify]

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

[@alllove1754]

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

[@lashamartashvili]

I bet what captured at 7:23 surpasses any CGI or filmed special effect in whole history of cinema.

[@pimpz7409]

Really cool footage, appreciate the great work!

[@FarhanAmin1994]

You deserve a million subscribers!!! Also I love your accent :)

[@VendettaProspecting]

AWESOME apparatus in the beginning!!

[@herrbrahms]

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.

[@LaserJake99]

The blue in the ammonia is probably free solvated electrons.

[@GianmarioScotti]

"None of chlorine oxides like organic materials" - I'd say they like organic materials a bit too much.

[@herrhaber9076]

Surrender all your electrons !

[@GianmarioScotti]

@@herrhaber9076 brilliant, thank you for your comment.

[@EPICGUYDUDE]

Interesting structure, I would have expected it to have a Cl-Cl bond but instead it is bridged via an oxygen atom...

[@zodiakofficial4093]

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

[@lukebowers536]

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.

[@quint3ssent1a]

Oh wow, but there was no light flash from sulphur ... although it seems plausible enough.

[@JohnLeePettimoreIII]

9:18 my undereducated guess would be "solvated electrons".

[@alllove1754]

I had the weirdest idea you were right on that. Halogenated electron solvation..

[@chemlab5038]

Wow , I really want to point out the pipet shattering at 8:24 ,, Amazing

[@treelineresearch3387]

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.

[@justsayin...1158]

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

[@andrewlawson4901]

I love your channel very much CF. Makes chemistry so intriguing and interesting

[@garycard1456]

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.

[@EdwardTriesToScience]

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

[@todddunn4719]

Thanks for your experiments, be careful. You rock.

[@EliasExperiments]

You are getting closer and closer to ClF3 ;-)

[@tiriviento9433]

Loved the scheme of the video. Keep it up

[@alex-dn9to]

i absolutely love these videos

[@craigpater6278]

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

[@Dasycottus]

Well, with a formula like Cl2O6, I'm sure this chemical is very happy to exist and incredibly stable

[@ch1pnd413]

Using lasers to cause explosive detonation? Amazing! And such good footage! I love it, this is so cool!

[@rplatt9829]

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.

[@cezarcatalin1406]

You could’ve used chlorine and ozone directly since ozone oxidises chlorine to chlorine dioxide. Actually, if you added a blue light to the setup too, you would’ve made dichlorine heptoxide. It’s important that the blue light is only used with the chlorine plus ozone setup though since if chlorine dioxide or other oxides besides the heptoxide accumulate and then get illuminated, those can explode.

[@ChemicalForce]

Hey! I tried direct oxidation of chlorine with ozone, I also used a UV laser for this, but didn't notice any changes. After an unsuccessful experiment, I carried out the synthesis through ClO2 and everything worked out, which I then repeated in the video.

[@Psychx_]

The reaction with Methacrylate was very violent. Was this the notorious "explosive polymerisation" I've heared about?

[@lagomoof]

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?

[@washingtonirving1345]

CGI artists need to watch this channel for inspiration. Real explosions look cooler than what is often in movies.

[@逸一时误一世-b6w]

for the first time I realize these glass apparatus might made in China ,for the Chinese characters on it

[@kuebbisch]

Blue tinge in ammonia: Solvated electrons maybe?

[@experimental_chemistry]

That's it! 👍

[@jozefnovak7750]

Suuper! Thank you very much!

[@АндрейКотомцев-ц8ь]

SUPER !!!

[@buckstarchaser2376]

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.

[@ramesharamakrishna9852]

interesting.. Thanks for such informative video

[@fireandcopper]

Every video he uploads it's a new aggressive chemical or unusual reaction, the camera quality is professional, he's a chemist and a videographer

[@koukouzee2923]

I learned this existed few days ago and tagged explosions and fire on twitter to check it out but I think I tagged the wrong person xD

[@sorryplease5071]

There may be a little too much yellow here for his liking.

[@michaelperrone3867]

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.

[@vitalijslebedevs1629]

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?

[@ebrylkation9538]

Thanks for sharing this important vid + + +

[@gok7455]

I am loving this

[@evansp12]

Fascinating videos. I think the blue color from reaction with Liquid Ammonia is probably Dinitrogen Trioxide (N2O3).

[@viktormartinsson9964]

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 :)

[@Дмитрий_1981]

The content is truly unique. Although the experiments are very dangerous

[@hsr03]

I believe that, in the reaction with liquid ammonia, could be something like this: Cl2O6 + NH3 -> ClO2 + NO2 + NH4Cl, something like this.

[@idea-shack]

Please do a demo with xenon compounds

[@ZoonCrypticon]

@4:17 Looks like the red matter in the Star Trek Movie from 2009, except that it does not swallow your table into a black hole as it did with the planet "Vulcan".

[@rashedusman9717]

Maybe it oxidises liquid ammonia to nitrogen dioxide with some chlorine and nitrogen trichloride as sideproducts. All of these whould react with the excess ammonia to form colorless products. As for the pipete, it is posible that the initial reaction with molten sulfur produced blue light which caused the dichlorine hexoxide to decompose.

[@Guds777]

And BOOM goes the Dichlorine hexoxide...

[@BradSchmor]

Hmmmm.... ammonia with dichlorine hexoxide gives a blue color which disappears quickly. Here is my speculation. Dichlorine hexoxide is more accurately thought of as chloryl perchlorate. The chloryl species is responsible for the color, and the exact nature of the color depends on interaction with the counterion (perchlorate). However, ammonia can solvate (coordinate to, via the lone pair) cations and probably would do so on the chloryl ion, which can accept four coordination interactions. This changes the energy for transition of the electrons to antibonding orbitals and shifts it to blue. This species is short-lived, though, because the oxidation of nitrogen by the chloryl cation should happen quickly, destroying the +5 oxidation state which gave us the color in the first place.

[@davidgriffiths7696]

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.

[@w__a__l__e]

@9:28 could it be electrons in solution?

[@diablominero]

It looks like it'd be a good radical initiator.

[@YodaWhat]

At 9:24 - When added to liquid ammonia, the funny bluish material is probably *solvated electrons.* See the experiments of Thunderf00t full a full exploration of *solvated electrons,* both in and out of ammonia.

[@lazyobject5797]

The blue thing could be a the NH3Cl2O6 with partial free electrons released during the reaction giving the blue colour

[@keithbrown2458]

Wow that’s amazing I know for certain I’m not going to try to make any of that stuff

[@sebastiand152]

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.

[@brianbarrett2487]

Watching the small drops spray up I think your right.

[@winkus8586]

I am interested on whether you got any injuries or not from the exploding glass

[@m_i_g_5108]

I want to be rich, not for impressing others with materialistic crap, but to spend time and money on science/tech hobbies! Haha! And other things that make me use my brain.

[@bernardlaval6248]

Great videos. It would great if you could add the time in ms during the slowered parts 😁. The quality is 👌

[@lazyobject5797]

Its enthalpy change is positive so it could have reacted with tge gaseous sulfur and the wavelength of burning sulfur also gives the required shift of equilibrium

[@leguetflorian6023]

Very cool video, hope you were wearing tough gloves when the pipette blew up!

[@madmattdigs9518]

This channel is so cool.

[@simonstergaard]

If textbooks was as vivid as this i would have passed all my exams !

[@Surgeeon]

I wonder if you could make a combustion engine out of that stuff and replace the spark plugs with lasers

[@skeeviesteve1071]

...that first watchglass explsion was...shall we say...energetic?

[@Ang3lUki]

It's crazy seeing the CL2O6 reacting before the laser actually touches it, due to reflected light

[@trentonthelen4813]

I believe the blue green tinge is dissolved electrons coming off of the radical chloride species and dispersing in the ammonia. It also happens when lithium is dissolved in liquid ammonium.

[@fat_pigeon]

However, the solid- and liquid-state structure is [ClO₂]⁺[ClO₄]⁻, neither of whose components is a radical. So it's not obvious where the electron would come from.

[@franksantis7403]

Man you should link up with the slo mo guys this would be amazing

[@chuckcrunch1]

8:55 maybe some vapor , droplet, or gas from the molten sulfur reacted with 2nd drop on the pipet . the timing would be about right .

[@marcopozzi522]

Is it possibile to use it in car instead of gasoline?

[@quint3ssent1a]

That experiment with molten sulphur... Did the first drop stirred sulphur vapours enough for them to reach the pipette and react with hexoxide inside?

[@heorhiypavlovych9779]

Cool stuff! Btw Never seen reactions with chlorine heptoxide ie. Cl2O7 would be cool to see one too!

[@christopherleubner6633]

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 🤓😲😁

[@aqdrobert]

Luke Skywalker: Found a new use for my blue lightsaber...

[@PvPbomber009]

would it detonate from the rays of the sun?

[@JohnLeePettimoreIII]

Dichlorine Hexoxide: "I don't want to be here." Manganese Heptoxide: "I hear ya, pal."

[@garycard1456]

Nitrogen triiodide and nitrogen trichloride: hey, don't forget us!

[@bugabateinc971]

The light and a spec of dust likely caused the pipet explosion. Freshly synthesized materials are more active biologically as well, from antibiotics and antivirals to psychoactive materials. The physical properties such as m.p. and crystallization are the same, so what is mechanism responsible for the higher activity?

[@A13tech]

I would be super interested to see FOOF or CIF3, does it even exists ?