Ok so for some reason this video has gotten a lot of views in the past week or so and I have gotten a lot of comments, so let me clarify some stuff. First of all, yes, I know I missed the beaker on every single pour. It’s hard to aim it into a small 50ml beaker when trying to stand as far away as possible and me being scared of the possibility of violent reactions didn’t help my aim. Secondly, this is literally the second video I ever made right when I started home chemistry, so my “skills” suck. I’m not saying I’m good at chem today, but I am for sure exponentially better than i was at this time. Thirdly, I know I wasn’t wearing shoes for some reason when I was breaking glass ampoules which was really stupid. So yea don’t do that, wear shoes. As for the pollution comments, driving is worse for the environment based on the small amount of bromine that I leaked into the atmosphere.
@@lulslime1066 Then stop being in the RU-vid comments, go do what Bill Cosby did and be a comedian with a horrific downfall. At least you'll make the world a little bit better after your downfall, better yet go work for McDonald's because they pay 15 an hour and it's actually pretty good not gonna lie. Real advice work towards college and slam a revolving door.
I was surprised that these reactions weren't more spontaneous. Especially the steel wool and lithium. I think they are covered in oxides that protect them a bit.
That first step is a little un-necessary: A solution of either sodium carbonate or sodium hydroxide (or the potassium analogues of those) in water will strip the oxide layer off aluminium foil (or any lump of aluminium) pretty quickly - the oxide is dissolved off by conversion to sodium aluminate, which is water-soluble. Aqueous sodium aluminate is NaAl(OH)4, while anhydrous solid sodium aluminate is NaAlO2. The latter can be made by dissolving aluminium oxide into molten sodium hydroxide, or by calcining a mixture of aluminium oxide and sodium carbonate, which I think is how it is done industrially.
@@lloydevans2900 what does that have to do with this though? None of that is necessary with bromine and aluminum. Just give it a few seconds and it'll react without having to have the oxide layer removed.
Burning lithium will actually react with the glass itself. I forget the product, but it will literally eat it like what happened here. Thunderf00t has a video on making cesium and the same thing happened to him, only under vacuum while distilling cesium.
Your comment has enlightened me on what happened, burning lithium produces lithium oxides which react with water to make hydroxides. Since these hydroxides and oxides were very hot, they both melted the glass and dissolved it. Thank you for pointing that out, I hadn’t thought of that before. As for the cesium, I have made some before but it was before I had a RU-vid, so I don’t have a vid on it.
BackYardScience 2000 I would recommend the way Cody’s lab makes it with the black iron pipe and steel tube welded to the side of the cap. All I did next was use a charcoal foundry to get it to distill.
@@reactivechem7408 , that's exactly what I have in mind and I already have the reaction vessel made, I am just waiting on my argon to get here. Though, Cody did it without an inert atmosphere. I may try that too, but I only have a couple hundred grams of CsCl to work with. So we'll see what I decide to do in that regard.
BackYardScience 2000 please take a vid an upload it, I would love to see how you do it. Also where did you get argon, I have been looking for some but can’t seem to find a good amount at a good price anywhere
The reaction of elemental bromine with isopropanol most likely produced bromoform as the major product. This does of course work with an aqueous solution of bromine or sodium hypobromite, albeit more slowly and the bromoform appears as an oily layer at the bottom, since it is far more dense than water. The neat reaction is just faster and therefore more exothermic. The first step of that reaction is usually the oxidation of the isopropanol to acetone - so you could probably get the same product by reacting bromine with acetone instead of isopropanol. This would also explain why the product was non-flammable, since bromoform doesn't burn and can actually be used as a fire extinguisher, similar to the old "fire extinguishing grenades" which were sealed glass bulbs full of either chloroform or carbon tetrachloride.
@@OK-on1ze Under aqueous conditions, not likely. In fact, 2-bromopropane would probably be hydrolysed back to isopropanol. If you exposed a mixture of isopropanol and bromine in the vapour phase to some UV radiation, you could get some radical substitution products where the bromine radicals exchange with hydrogens, the byproduct being HBr. However, radical reactions of that type are messy and unpredictable, so while you might get some 2-bromopropane, you would also get a whole mish-mash of other products with bromine substituted for hydrogens at all the other positions. Separating the mixture out afterwards would be a real PITA.
If you guys keep doing things like this you will get hurt, its only a matter of time. Cover up. Put the most dangerous/volatile material in the beaker first Do this stuff in a tray so you don't contaminate things. Put some shoes on. You only need to clip the end of an ampule. If you are worried about getting injured whilst putting something into a beaker, use tongs. Have a quenching solution in excess on hand at all times, and afterwards put everything that comes into contact with bromine into it. Know what your end products are, you seem to have no real idea what you are making, brominating an alcohol isn't a little thing. You seems to have other people running around, keep them away! You obviously wasn't wearing a mask, wear a mask! you're going to gas yourself, yes even outside.
The bromine vapors will suffocate the fire and make it difficult to react, also bromine and chlorine aren’t as reactive as oxygen or fluorine so they do not support combustion very well.
Everyone else: SCIENCE!! Me a history junkie: Osoweic, then and again, attack of the dead, hundred men, facing the lead once again, hundred men, charge again, die again...
I laughed so loud at 8.12 like that reaction doesn't support you😂😂😂😂 And actually I hate chemistry but I saw a short about bromine and.... I'm here 😅 So I'm interested in chemistry now..
I think the mixture of isopropyl and bromine boiled because the reaction of Bromine and Isupropyl might be exithermic. I think it makes Bromoform. One of the haloforms!
Just an FYI.......but if you add pure Br2 to pure ethanol you will only produce 2 products........ethyl acetate and HBr acid. AND YES I KNOW HE USED ISOPROPANOL .AND WATER (azeotrope)............this is just an FYI
@@potatoboy549 ........Yeah it does not seem to make sense but i never looked up the mechanism. No water can be present though. And just my opinion....Br2 is not a tame compound...lol.
@@potatoboy549 ............I made some acetone from rubbing alcohol/bleach/acetic acid. SO...........Right now i am trying to make acetaldehyde with bleach/acetic acid and ethanol. Also trying to make acetaldehyde with hot copper and ethanol. I got them all to work but with crappy yields. Need to tweek things. The rubbing alcohol worked best making acetone. I got a 35% yield of SUPER PURE acetone. But i think i can improve the yields
GREAT VIDEO...........JUST A GUESS on mixing Br2 and isopropanol. Since there is NO strong base it can not go through the haloform reaction where the first step would be turning the isopropanol into acetone. So it is probably ANALOGOUS to adding bromine to water. Br2 + H OH > HOBr + HBr so therefore Br2 + isopropyl OH > HOBr + isopropyl Br which is also ANALOGOUS to adding bromine and NaOH.......Br2 + Na OH > HOBr + NaBr ' I wander if i am right. Cause that would be a WILD way to make isopropyl bromide.
So potentially, if I combine rubbing alcohol with bromine, waited for the alcohol to dissolve the bromine and coated it on the surface of something, it would become fire retardant?
I wonder if the lithium would have reacted without catching it on fire if it didn’t have so much oxidation covering it. You’ve come quite a long way in your videos.
Idk if some of these were chemical reactions with the elements you placed inside. It would appear you heated and element to a point high enough for a thermal reaction with the bromine. This lead to a chain reaction of the bromine getting hot enough to burn the secondary element.
The fact that you keep spilling the bromine leads me to guess that you aren't a trained chemist, in which case you REALLY shouldn't be handling chemicals like this, like at all. You got lucky, but you made a number of sloppy and potentially deadly mistakes in your handling of this chemical. You're lucky you didn't come out of this with some serious injuries or worse.
