Doug's Lab - 2015-09-11
In this video, I make and purify sulfur monochloride from the elements.
hi doug,
in the last two weeks or so i watched your uploads and have really enjoyed them!
since i am not so much into chemistry i definitely don`t understand all the reactions going on but i have the feeling, of quite-getting-your-explainations-right, though this might be dunning-kruger-effect ;)
anyway, keep on your great work!
greetings from germany!
Just wanted to say this was an awesome video!
I love these big glass setups, you just earned a subscriber.
Such a well done video!! Can't wait for the next one. I teach high school chem so it's been years since I've been in a real lab. I live vicariously through your videos now hahah. Keep 'em coming!
+lightvsdark21 Hey, thanks! Let me know if you want to see anything. Maybe I can make a video for you.
Excellent demonstration and performance. This is indeed a dangerous chemical to work with and your whole setup can handle it, especially the fume hood.
Love the videos. Would you consider adding more of the analytic work of your reactions? I would love to see your calculations.
Thanks for the cooking tutorial!
Beautiful work with a foul compound!
Great! I love this kind of reaction (and I love reactions with sulfur in general).
I would have added another distillation just for good measure (maybe fractional, although allowing it to reach the top of the coloumn would have required a ton of heat), but you know the boiling point of the stuff that came over and I guess that it was reasonably pure.
Really liked it, good production.
Nice job! This is really helpful
love all the glass ware
I agree the beaker usage is top notch
Very cool. Never really worked with liquid sulfur compounds.
May I submit a proposal for the preparation of Thionylchloride? I found a hint, that it should be possible to prepare SOCl2 in lab- scale out of Sulfurdichloride and Sulfurtrioxyde according SO3 + SCl2 -> SOCl2 + SO2. Thionylchloride is known to be a useful chlorinating agent and may replace the phosphorous-clorine compounds in many cases (PCl3, PCl5 and POCl3), which are very hard to obtain, due to their "dual-use" characteristics.
it would be great to see more videos from you, Unfortunately you haven't uploaded any videos for a long time, for example I would be very interested in the synthesis of thionyl chloride or phosphorus trichloride
I'd like to see more experiments with hydroiodic acid. Also more Mercury chemistry.
no mercury chemistry! Yes, its interesting, but if there is soluble or even organic mercury anywhere around me id escape asap its not a fucking joke to play with these kinds of things
Wanting to make meth, are we?
I love your videos, man! it's a pity that you're not that active anymore :(
theawt Not in 2018 Bro!! He is posting more videos
@@KTEX78 and now he's awol again. He disappears about every other year and never updates on whether he will continue making videos or not.
Hi Doug, I have been watching your videos with great interest. I watched nurdrage's making of potassium metal using the catalyzed magnesium reduction method.
And he/she said that this method replacing the potassium hydroxide with sodium hydroxide it should be possible to make sodium metal if you got a longer chain of alcohol's. Would be fun to watch if you tried to make sodium metal using this method.
Nurdrage never got it to work do.
Morten Harrysson he's getting it to work right now bro
He got it to work about a year ago and posted a video on it.
Great Video !!
My research is based around phosphines and phosphorus compounds so I'm used to stenches, but I've heard the smell of this described as a mix of extreme BO and a decomposing corpse. Bleugh.
you heard correctly :)
the smell sounds lovely. It's good we do not have smell-a-vision :)
+mechadrake I can only imagine. Some of the phosphorus compounds I work with are truly foul but I'm pretty sure S2Cl2 is on another level.
@@elnombre91 The smell is not easily described, but it is by far the worst I have encountered. I wouldn't say it necessarily smells like rotting flesh, although it is reminiscent of that. It smells more like what you would expect a chlorine compound and hydrogen sulfide to smell like. For the most part, however, you do not come into contact with it during this synthesis since it must not contact the air.
Brave one, working with such a great quantity of chlorine gas! Could you somehow make thionyl chloride to be used to introduce Cl in place of OH in syntheses? ;)
Very interesting!
Very nice work! After the chlorination was finished you're still left with a chlorine generator setup filled with chlorine gas. How did you clean that one up without exposing yourself to chlorine gas? I used a two-neck RBF as the generator flask, and when things were finished, through the free neck I'd connect an aquarium air pump and blow the excess chlorine out into a beaker of aq. NaOH..
apart from alkalies, a lot of reducing agents come to mind for dealing with chlorine (FeCl2, sodium sulfite and thiosulfate, even carbonate and bicarbonate)
Excellent video! can you explain what this is used for?
That was very interesting, and rather intensive too. That stuff almost looks like whiskey.
+Barnekkid But it certainly won't taste like whiskey!
+Zmrzlinafication Or smell like it.
Hey Doug, is there any chance that the “carbon” that you said was left over in the reaction flask was actually amorphous sulfur? I made a video exploring the physical properties on my channel and I think the “carbon” is just some plastic sulfur converting back to crystalline sulfur. Love your vids and can’t wait for the upload later today.
It's probably not necessary, but I also added in a bubbler in between the drying tube and the sulfur flask, I filled it with sulfuric acid just to dry the chlorine gas even more.
Ever thought about going a step further with this and making sulfur tetrachloride? It only exists at low temps (like dry ice acetone bath theps), but it does exist and seems like interesting stuff! It hydrolyses to thionyl chloride and I'd be really interested in seeing what it does to an anhydrous carboxylic acid. Maybe make an acid anhydride and thionyl chloride, which then reacts with another acid to make an acid chloride? Nothing like making two usefull things at the same time lol!
Doug, why do you use a wattage regulator to the heating mantle. Doesn't the knob on the unit itself accomplish the same thing?
Not a bit necessary to melt the sulfur beforehand. Cl2 reacts with the solid easily and the S2Cl2 can be distilled odd easily.
Have you tried synthesis of A anhydride from sodium acetate and S2Cl2?
Would love to see this in action!
The lack of subscribers here makes me sad
Agreed! Amazing channel
Sodium Percarbonate is great for cleaning dirty glassware.
Did you damage your glassware IE stained your glassware doing this?
Another interesting video, thank you. Your glassware is super clean, I wonder how you do that. But never mind that. What was the powder, the something hypochlorite? I didn't think sodium hypochlorite could exist safely as a solid. My hearing is good, and you do speak a little fast :-) but I heard you say it was some percent something-or-other-hypochlorite. Is there an OTC source for that? Like TCCA or other pool chlorinator? Very nicely done though – the end product had a nice color.
Calcium hypochlorite.
convert S2Cl2 o SCl2, react the dichloride with SO2 and Cl2 and you get SOCl2, which is a very useful reagent (acyl chlorides, alkyl halides, alkyl sulfites and other interesting things can be obtained from it; unlike phosphorus chlorides, it is a much cheaper chlorinating agent, albeit more volatile and toxic)
GOOD WORKE
Can sulfur monochloride chlorinate alcohols into alkyl chlorides and acetic acid into acetyl chloride?
18:45
Lab jack: I need some oil!
What's some of the uses of sulfur monochloride? And how do you avoid breathing in chlorine gas when you disassemble the apparatus after it has had the generator running?
+WeekendScience
There are quite a few uses. I will hopefully be demonstrating some in upcoming videos! When I disassemble the chlorine generator I use a spray bottle with aqueous ammonia to neutralize the remaining gas. The fan sucks out the NH4Cl smoke.
"SCl4 just before it's melting point..." What molecule is the minus 30C referring to? The SCl4, or the precursor(s)?
the SCl4
Although an overall great video I can't help but wonder WTF you going to do with it now....
"not very friendly". Do all chemists have a penchant for understatement, or just the YouTubers?
What was this used for? Just curious
Hey guys, I have a question, since the reaction that this guy is doing involves Cl2 generation, how does he prevent his system from blowing up from pressure build up? He cant really use a breathing hole, or the Cl2 would leak out, which is a no no, and as far as I know, CaCl2 wouldnt absorb Cl2 or anything.
The Cl2 is getting used up so if the rate of Cl2 production is low enough it should all get taken up by the S without any excess getting past the reaction flask
Also at 8:52 of the video you can see a line attached to the vacuum adaptor which likely leads to the back of the fund hood for any excess Cl2 to vent.
excellent demonstration ! knowing that you are such a good and cautious chemist I hope you will not react this compound with ethylene...
I had to google that... Mustard gas >_<
sweet, you live in MI too! :D
If the structure is molecular, nobody should call it sulfur monochloride
What you said about there being only 3 types of sulfur chloride is not true. Other sulfur chlorides can be made with a common chlorosulfane and a sulfane. For ex S7Cl2 is made from S2Cl2 and H2S3
@firstmkb - 2020-06-27
Thoroughly enjoyed the video, ESPECIALLY the setup and cleanup tips. The reaction wouldn't be tough to find online, but making it safe and repeatable is golden. I was just about to start typing questions about cleanup at the end, when you started talking about cleanup!
Great video.