Hello guys! This is My sixtieth video and it will be about interhalogen compound.
I know you often ask to show ClF3, but it's too exotic even for this channel (at least for now, sorry).
So, today I will show you reactions with iodine trichloride
I am holding an ampoule with iodine trichloride,
also called diiodine hexachloride sometimes, because in the solid state it is presented as a dimer.
So, let's open the ampoule, this must be done very-very carefully.
This substance is extremely volatile, you can see its dark orange fumes on a light-gray background.
We don’t have much time because Iodine trichloride is very sensitive to air humidity,
so let's enjoy this beauty until these crystals didn’t decay in the air
Wikipedia says that it is a bright yellow powder, but it’s not yellow at all in the ampoule next to its picture,
yet it’s of the same color as mine.
The thing is that during prolonged storage or keeping in the light,
iodine trichloride gets covered with elemental iodine, that adds such a burgundy color to it,
so if we scrape off this thin layer, we will see the yellow color of iodine trichloride that we need
At temperature above 60 degrees Celsius,
iodine trichloride decomposes into chlorine and iodine monochloride (that’s a red-brown liquid)
Now you can observe iodine monochloride flowing to the bottom of the tube
Iodine trichloride reacts with water in different ways,
depending on the temperature of the latter.
So at low temperature it is hydrolysed by water slowly but completely,
with the formation of iodine monochloride.
In the reaction with hot water, you can observe gas evolution -
hydrogen chloride is actively released during the reaction
In the reaction with a concentrated alkali solution, we can detect chloride, iodide and iodate ions
If there are no other oxidizing agents in the solution besides iodate,
the presence of iodate ion in the solution with iodide can be determined by the evolution of elemental iodine,
that occurs due to acidifying the solution.
Keep in mind, that the acid must lack oxidizing properties in the solution.
For this reaction I use diluted sulfuric acid
Now I will show you a very interesting reaction with tin (II) chloride,
keep in mind that it must be anhydrous, this is very important.
Tin (II) chloride is colorless crystals with strong reducing properties.
Now I will add it to iodine trichloride
Have you noticed how quickly tin chloride crystals turned yellow?
It’s tin chloro-iodide that gives this cream color.
The main reaction leads to the formation of tin tetrachloride, iodine monochloride and elemental iodine
The smoking liquid, formed during the reaction, is tin tetrachloride,
polluted with iodine-containing reaction products apparently.
By the way, check this out, it is pure tin tetrachloride,
see how nicely its heavy vapors spread around bottle walls.
Well, now I will show you a couple of homogeneous reactions where self-ignition occurs.
It is exceptionally cool to observe when both substances are solid.
Red phosphorus instantly lights up on contact with iodine trichloride
Highly-flammable lithium borohydride self-ignites too
Well, here’s our favorite decaboran, that ignites on contact with almost any oxidizing agent.
Oh, guys, if you are still watching this video, then you are totally hooked on chemical reactions
and you really like my videos as much as I like making them for you.
And if you'd like to see even more awesome videos with more exotic chemical reactions
and more hard-to-get reagents and make sure they come out more often,
you can now support me on Patreon.
I can guarantee slightly more advanced videos with the reactions .
that were not included in the final cut to EACH AND EVERY membership level
because It wouldn't be fair if any of my patrons lacked access to exclusive videos
But, no matter what your decision is,
I'm not going to stop making new videos,
because I still have many intriguing ideas and rare chemicals to share with you!
Now let's take a look at the reaction of iodine trichloride with hydrazine hydrate,
that likes to reduce iodine in compounds with a positive oxidation number of iodine.
Iodine reduction is completed.
And this video is completed too!
I hope you really enjoyed the selection of reactions I have prepared for you.
Thank you for viewing this channel. Many more exotic chemicals await you ahead.
See ya next video