Rhodanide - 2019-06-22
The synthesis of Tin(IV) Iodide, or Stannic Iodide, is an interesting, fun and simple synthesis which yields a beautiful and peculiar product. Today, I'll show you the complete synthesis of this compound. I'm not responsible for damage to persons or property caused by the replication of this experiment. Consider supporting me! https://www.patreon.com/Rhodanide My Twitter: https://twitter.com/Rhodanide Song used: Saint Seduce & Winston - Sedna Outro song: Hexenkraft - A Flame in the Void https://www.youtube.com/watch?v=HOj3w...
Very nice! I've only done this using dichloromethane before. You got a great looking product. đ
Thx Rhodanide. I am going to give this video to my beginning chem students for stoichiometry practice. If I want 3g of product, how much I2 is needed?
Also good to observe some basic techniques such as crystallisation, filtering and drying. Nice stuff.
Great video! I tried a few times using acetone. I did get some SnI4 but the color is a bit darker. Initially it is almost a bit yellow but seems to darken as it dries in air. It was difficult with acetone it seems the SnI4 is not that soluble in acetone and it easily reach what appears to be an equilibrium and started converting back to iodine. So I had to do small amounts at a time in my small beaker and thus ended up with a lot of acetone to boil of. But I got there in the end.
I recommend DCM, which you can buy in most countries.
@Emme PombĂ€r yes I have been using DCM often since; the original post was a year ago đ
awesome video man, great job. I think it looks similar to powdered gold with that lustrous dark orange color
Very interesting thank you. Do you know if acetone can be used as the solvent for this purpose?
Apparently acetone reacts with I2 (exchanging one hydrogen with iodine), though it might only happen with acid catalysis.
Is it a good reactant to make alkyl (or aryl) iodides? Because it looks like it is capable to react with alcohols/phenols, but any data that I have found online is limited (kinda just says that "yeah, it do react with alcohols" but nothing more).
Anybody has some experience in that matter?
Obviously I'm a lovely law abiding citizen, but considering how prohibitively difficult it is to make hydroiodic acid, would hydrolysis of this in water and filtering of the tin dioxide be a roundabout way to make hydroiodic acid?
This is helping me prep for my lab tmr~ thank you
As you used an excess of tin, how do you exclude your product containing SnI2? Wikipedia claims the latter is similarly colored ("red to red-orange").
Maybe the hydrolysis you did tests this, but I'm not sure whether SnI2 also hydrolyzes with colorless products. It likely does since the tin(II) aquo complex is colorless.
I don't believe Tin(II) Iodide is soluble in Chloroform, is it?
Can you use any liquid that iodine is soluble in for this reaction?
Possibly, I've never tried it so I can't be 100% positive that it's a "yes". Give it a try on a small scale to see if it'll work, I'm curious to know!
Very interesting!
Why filter? Shouldn't it be sufficient just to evaporate the CCl3?
I've found the mechanical loss is basically negligible at that point. Was looking for nicer crystals. You're right, it'd probably be easier to just wait anyways.
@Rhodanide I made it by evaporation some hours ago and I must say, that I don't have nice crystals like you have. So I am going to recrystalize it again.
And it smells horribly (like iodine). Is this smell normal?
Also I used DCM instead of chloroform.
But it's a really nice orange color. Fits perfectly in my set of coloured salts :-)
What is the hydrolysis product? SnO2 and HI? I didn't expect that... I haven't done Sn chemistry at all...
Yeah, Sn(OH)4, SnO2, HI, SnI3(OH), and tons of other mixed products and such.
@Rhodanide
I would expect HI react with metal hydroxides...
@user255 I would too, but there was probably a basic Stannic Iodide of some composition ( SnI(OH)3, SnI2(OH)2, SnI3(OH), etc) formed.
@Rhodanide
Still kinda unsatisfactory due the stoichiometry... Seems that Sn can form very complex compounds. https://en.wikipedia.org/wiki/Tin(IV)_Oxide#Amphoterism
Ayuh bub, this one's a wicked pissah
and this stuff does what now?
Looking orange.
Lab Lulz - 2019-06-22
cool stuff! melting iodine under sulfuric acid is a good way to both consolidate and dry it... for very high purity you can then powder it with CaO and sublimate :)