Hey guys!
We are getting dichlorine hexoxide by pouring dilute sulfuric acid to the mixture of oxalic acid and potassium chlorate.
and then oxidize in the resulting chlorine dioxide with ozone
None of chlorine oxides like organic materials
that’s why we’re getting this reagent by using glass equipment only, with no rubber tubes whatsoever
For drying, formed gases pass through the flask filled with phosphorus pentoxide.
Then they get into the U-shaped tube, where the ozone flow will go
This setup for getting dichlorine hexoxide is a little far from perfect,
but it will do for getting rather small amount of the reagent
So, I start to slowly add dilute sulfuric acid from a drip funnel to the mixture of oxalic acid and potassium chlorate
while constantly stirring and slightly heating it.
So, the interaction of oxalic acid and potassium chlorate mixture with sulfuric acid
results in the formation of chlorine dioxide and carbon dioxide
Now I turn on the ozone flow,
which will go to the U-shaped tube through a special ozone resistant tube,
where chlorine dioxide will oxidize to dichlorine hexoxide
To be safe, I also had to decrease brightness on my lighting equipment for this video
A few minutes later red oily drops of dichlorine hexoxide appear on cold tube walls.
At a lower temperature these drops turn into yellow crystals
Actually, the resulting red liquid is chlorine dioxide solution in dichlorine hexoxide.
Besides, dichlorine hexoxide itself emits chlorine dixoxide constantly.
So you can see an initially transparent flask filling with yellowy-orange chlorine dixoxide
Now, let’s take a look at the reactions with this reagent
First I’m going to pour a few drops of dichlorine hexoxide on a rubber stopper.
To initiate the reaction, I will use a blue laser from time to time, just like in this case
Exposing this reagent to a blue laser results in various reactions,
but basically they all come down to the formation of numerous chlorine free radicals
that have a high reactive capacity.
This is the reaction with natural rubber.
With sawdust.
And with paper
As we can see, not all of the reactions come with combustion
Here we can see the impact of a blue laser beam that results in an instant decomposing of dichlorine hexoxide
without any reaction with chicken skin
Lithium aluminum hydride flares up on contact with it in no time.
I will pour some acetone in a metal spoon, add a few drops of dichlorine hexoxide and aimed the laser at it.
And here’s what happens if I perform this reaction in a watch glass,
but using methylacrylate instead of acetone
Only freshly made dichlorine hexoxide has reactive capacity this high
I recreated similar reactions a few days after I had got dichlorine hexoxide
which I was storing in the fridge
So, the reaction with methylacrylate turned out to be not that strong
And to make not-so-fresh dichlorine hexoxide react with lithium aluminum hydride,
photoinitiation is required
Photoinitiation was necessary for the reaction with decaborane as well,
though a quite insignificant amount of fresh dichlorine hexoxide reacted with it without any additional impact
We know that carbon disulfide combusts in chlorine dioxide vapors.
So it would make sense to expect a violent reaction by adding liquid dichlorine hexoxide to carbon disulfide too
It’s quite interesting that in an attempt to add a few drops of dichlorine hexoxide to molten sulfur,
dichlorine hexoxide exploded in a pipette.
Here, take a look at this reaction in slow-mo.
Why do you think that happened?
Now I have a question for you.
Adding dichlorine hexoxide to liquid ammonia leads to the formation of some blue-green tinge,
that disappears very quickly.
So what exactly is going on in this reaction?
Let me know what you think in the comments!
In the end, I poured the remainings of dichlorine hexoxide out of our pointed flask
and aimed a laser beam at it.
Thanks for watching guys,
hope you really enjoyed this video about chlorine oxide,
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