Ammonium dinitramide has been developed in liquid monopropellants for a while and has been used for 10-20 years. The LMP-103S monopropellant is meant as a replacement for hydrazine with higher density impulse, lower toxicity and less likely to explode. Its catalytic decomposition is somewhat more difficult--apparently requires preheating--but in general it is a good replacement and one of several new propellants based on ammonium dinitramide. They are less hair-raising than yesterday's propellants. Probably the US military (and others) is going to use it if they can for solid propellants, because it is an oxidizer that can be used to make a propellant with very low smoke signature, which is increasingly desirable.
@@That_Chemist Modern rocket propellants are generally less cursed than old school rocket propellants. In the beginning there was all the cold war impetus to use whatever worked at all, and the chemistry was less powerful. Hence all the interest, for example, in dense liquid Cl O and F compounds. Which entirely deserve their reputation, mostly. These days people are less tolerant of rockets doing wild and wacky things and have better tools to prevent such.
@@sealpiercing8476 It's kind of terrifying that people even momentarily considered things like Hg compounds, 30% O3 in liquid F2, ClF5, nitroglycerin, or finely divided Al in liquid O2 as rocket propellants.
@@seth094978 The really wildcat stuff, that you listed, was only ever "Is this usable, practically?" to which the answer was mostly no. ClF5 came closest to being a real propellant, because at least it wouldn't just explode like the other things you mentioned except Hg. The Hg compounds were never fired AFAIK but there was one experiment using liquid Hg metal with a liquid nitrate salt-in-nitric acid monoprop to increase density impulse. It accomplished that but solid propellants have better density impulse and are just so much better to handle in general. The arrival of high performance solid propellants is partly the thing that kept all the really weird liquid chemistries from military use. By the time they were ready they had been overtaken. That and lower cost of turbojets, in the US at least. If it needs long range, give it a jet engine burning hydrocarbons with air, if it needs high acceleration give it a solid rocket motor. Mix and match with staging to suit.
What I really want to know, is whether Seleno-selenonoesters (the hypothetical product of reacting a selenoacyl chloride with a selenol) exist. Tell me, are silly no silly no no esters a no-no!?
@@methanbreather saddly Sci show failed us on this one. It is very powerful and decently sensitive. But the German lab didn't say that it was "too sensitive to be tested at all" but that it was too unstable to determine its stability with THEIR equipment. Other labs have done this with better equipment and its more stable than silver fulminate and other fulminates But ya know one paper says to sensitive to test sensitivity. Some random person at a paper sees this and they make a super exaggerated version of the line "the most unstable compound on earth, so unstable it can't even be tested". Then this gets spread around and eventually everyone thinks that it is definitely a super explosive with the most sensitive touch. But in reality it's able to be hit by a hammer and it won't go off unless you really put your back into the swing
As an organometallic chemistry researcher. I work with organolithium compounds without a concern… But that Einsteinium complex… that thing give me chills
Btw I really reaaaally like that gold complex since it’s a compound which includes both an inert transition metal and a noble gas. Its very interesting. I will make a research for syntesis of it
Gretchen Wilson's equivalent to here hold my beer ❤😂 just say it in plain English you're no better than anyone else cause you made it a chemistry joke #badhabits
Or they might be another organic family. Exobiology theories sometimes consider the possibility that other planets may have life and organics without carbon as the base element.
It seems than WikiPedia avoids the subject entirely. When I checked for buckminsterfullerene there was no mention of it being organic/inorganic. I checked the English, German, French and the Dutch editions. Then again: there is also no mention of melting point, boiling point and many other common characteristics. Maybe it's just a hoax. 😂
Don't worry: eventually, it will tunnel out. Might take some time as nuclei that large behave as classical objects mostly and not quantum. But it will escape at some point. But it will be heartbroken to see it's fluorine soulmate has bonded with some plain carbon atom.
"It's believed to be the first molecule that came into existence." Nature: "alright, does any stuff wanna combine into more interesting stuff?" He-H: "look at me!" Nature: "No that's stupid. Next!"
@@numberhaver7795 H-H may become HeH through nuclear fusion at sufficiently low temperature, if the Deuterium is provided by another molecule. Alternatively, HeH might form from atomic H and atomic He as fusion waste cools sufficiently in a universe with no higher atoms. I have insufficient knowledge to discount either path to spontaneous formation.
@@rubikscubedude4028 In very thin gas (i.e. in the outer space) protons may combine with He atoms to form HeH+, which is among the strongest known acids as the He atom will transfer the proton to (almost ?) anything it comes in contact with. So of course you can not isolate it, but it can be found spectroscopicly. And it might be indeed among the first molecules to come inte existin in the early universe before anything heavier than Li and Be was produced in stars.
The Einsteinium complex looks very much like Switzerland, where Einstein spent a portion of his life (in a place that even roughly corresponds with the location of the Einsteinium in the complex). This alone makes this one God tier
It's cool to notice myself recognizing more and more of the chemical concepts you mention as my ochem class goes along, maybe one day I'll be able to fully understand an Extractions and Ire video, a girl can hope...
True, every osmium compound I worked with were varying shades of yellow, orange, and red. This made my PI's colorblindness a little bit funnier than usual.
@@aloysiuskurnia7643 We have colours in organic synthesis as well! We have white powders, grey powders, brown gunk and black tar! Those sure are colours!
Used to work in a lab where another PI did uranium chemistry, not as dangerous or cursed as you would think, however beryllium chemisty scared the crap out of almost everyone.
Natural uranium isotope mix just has a too long half-life to be seriously creepy; it’s a bit more chemically toxic than lead. The really scary stuff has a half-life of hours to decades. The really cursed thing with uranium is when there is a risk of putting too much enriched uranium in one place. There have been many criticality accidents with uranium solutions and lax worker safety protocols.
I asked my main group metal organics prof when we were talking about Grignards, why people don't do Beryllium Grignards. And he just replied: "Nobody wants to deal with that coctail of death". And I think one of the reasons why Uranium chemistry scares a lot of people is, because you can't see radioactivity, but you know it's there and causes harm. But that makes it interesting. At least for me. Nonetheless I would have too much respect of Beryllium chemistry or HF too to work with it. (I don't say that I fear it, because fear makes you freeze. Having respect is the right approach.)
I actually made a very similar looking complex to the einsteinium complex, except it was europium, and the ligand were a tiny tiny bit different. It glows pink under uv light. Very cool
I have a bachelor's degree in Biochemistry, and never in my life have I heard of or even thought about the possibility of bonds beyond triple bonds. My entire perception of everything has been thoroughly shattered by the mere existence of quadruple bonds. I am a broken man.
May I add the electron-deficient Boron-compounds to the list of compouds shattering the world of innocent by-standers. Diborane was in. Pd-I-Pd is also pretty cursed
If you need very specific conditions like 4K and laserbeams to make argon fluorohydride, Figueroa can do it room temp by hand stirring for 24 hours, no special requirements needed!
I seem to remember the helium hydride cation as being the strongest known acid (besides the theoretical naked proton.) Love to see it here, along with some real zany structures that made me laugh out loud.
Examples of higher than quadruple bonds can be quite odd. For example, the quintuple Cr-Cr bond in a dichromium complex using terphenyl ligands. Sextuple bonds are perhaps less interesting, appearing in Mo2 and W2, but only under extreme conditions. Quadruple bond chemistry does have its own oddities, such as RhB.
Since you mentioned quite a few noble gases compounds, I would include in this list, probably A tier, the compound that made Neil Bartlett think noble gases compounds were possible in the first place, namely dioxygenil hexafluoroplatinate, O2PtF6
So in the hopes that you're reading this for the next batch of stories... In my first year B.Sc. I somehow ended up spilling every inorganic acid that we used (H2SO4, HCL, H3PO4 and HNO3) except HF, which was used by the professors only due to the gases it forms. Well, I can say that in stock solutions of these four acids, three out of four gives really soft smooth skin if washed immediately. So one day I was working with a new lab partner and everything was going incredibly smoothly until suddenly there was a little pool of fluid in the hood, I was stupid enough to not clean it up immediately thinking that the person who spilled it should clean it up so I worked around it. Somehow my lab partner thought the same thing and he denied being responsible for the spillage, it wasn't me either. So I momentarily forget that there was this unknown spillage to avoid, I accidentally put my forearm down into it and it immediately started burning. Turns out that it was the nitric acid and I hadn't used it that morning, I'm certain my lab partner did and just didn't clean up his spillage. I can tell you that nitric acid out of these five inorganic acids is the one that causes burns the fastest and the worst. I immediately started washing off the acid and it kept burning so much for so long. Afterwards I had this big boil on my forearm for weeks and a scar for months. Eventually the scar disappeared completely though.
Really appreciate the zero down time in these vids man. Straight to the point, entertaining, and a perfect balance of complex chemistry without being overbearing.
Borazine is getting more and more intersting, hexaphenyl borazines and borazine doped coronenes have interesting optoelectronic properties. There is a european project called STiBNite that is working on this.
I don't know why youtube recommended this to me as I know just about nothing about chemistry but I gotta say your delivery is very similar to Casually Explained and I'm here for it.
Just wanted to say that I'm a big fan of how this video looks. The night mode plus having the names of all the compounds makes it look super clean. Great video!
When I took advanced inorganic synthesis class at UC Berkeley in 1977, my friend made Uranocene as his special project. We were allowed to do these projects in our undergraduate research labs because most of the equipment in the designated lab was broken. I remember the professor criticised one of my experiments because I did not measure my product's magnetic susceptibility. When I told him his Gouy balance in the lab was broken he got mad at me. Nobody liked the professor and the professor didn't believe that my friend made Uranocene even though he had access to starting materials from Streitwieser's group where the compound was first discovered and synthesized, and I witnessed his synthesis. That professor did not get tenure and was forced to leave so he took it out on his students in that class. Kenneth Raymond was my inorganic chemistry professor and he was the best chemistry professors that I had at UC Berkeley.
For 8 months i was working contract for theoretical ocean geochemistry, and thiomolybdates came up A LOT. Probably the only one in the list that forms naturally on a large scale. Id put it in F tier, i dont think its cursed at all. It makes a lot of pretty red salts:)
If you ever do a part 2 of this you gotta include this dication: DOI: 10.1038/s42004-018-0057-4 This dication displays double aromaticity (i.e both the π and σ-electrons are in respective flat, ringclosed systems within the dication).
In the preliminary year chemistry class, our lecturer quite seriously told us about the perils of forming compounds with the noble gases. All the energy you put into the compound will be returned to you all at once including fragments of the containing vessel. This was on a par with advice about lab safety such as strong acids and bases and fire prevention but I thought combining noble gases with other elements is not something that budding chemists are likely to do. Another topic, I love the book by Sidgewick The Chemical Elements and their Compounds 1950 (Two volumes). I enjoyed reading about perchloric esters where researchesrs had to use tongs and iron masks and destroyed a lot of glassware. Apparently it was decided that perchloric esters were too unstable to be useful.
Another great chemistry video! But what did you mean by "cursed"? Toxic? Unstable? Reactive? Difficult to prepare? There are plenty of scary stories about some simple inorganics like F2, ammonium nitrate, LOX, ClF3, etc. At any rate, keep 'em coming!
LOX is not that scary, neither is ammonium nitrate...anything that will be allowed to be transported several tons at a time by a truck is relatively benign...
@@AKAtheA Until there is an industrial level accident/disaster. Arguably one of the things that makes LOX, LPG, Chlorine and Ammonium Nitrate etc scary is that single sites can have tonnes literally lying around due to their industrial or commercial uses.
It's still worth watching these videos, even though I could never be a chemist, due to the diagrams making my entire body itch. These inorganics are so cursed I have to put excema cream on my hands just from looking at them
FOOF absolutely deserves S-tier. I cant believe that some lab is actually using this stuff to do chemistry. I read that it can literally make ice catch fire. I hope i will never have to deal with this stuff in my whole life
I have no clue about chemistry but I watch these tierlists, and it always amazes me how always the smallest and most innocent looking are always the most cursed/toxic/deadly/explosive etc 😂
I saw the Krypton inside of the fullerene and legitimately burst into tears it was so funny. I wish I learned more about these cursed molecules when I took Inorganic Chemistry in my undergrad. You just earned a sub. Also, how would you even confirm the structures of these? X-Ray Crystallography?
I think ClF5 should be in this list - even if only because one of the major sources of it's properties is a now declassified US military document. Though the wanting to burn everything part and the stupid amount of bonds on the chlorine are pretty cursed as well.
Bright orange dicobalt octacarbonyl is widely used as a precursor for the classic hydroformylation catalyst hydridocobalt tetracarbonyl. Also, its (fluxional) structure contains two bridging and six terminal carbonyls, along with a cobalt-cobalt bond. In the absence of carbon monoxide, it decomposes to black tetracobalt dodecacarbonyl (tetrahedron of cobalt atoms with six Co-Co bonds, three bridging and nine terminal carbonyls), which likewise decomposes to cobalt metal, often a very nice mirror on glassware. Other fun inorganics I've handled include: dinitrogen tetroxide, which is a fine oxidant for rocket fuels (often hypergolic, depending on the fuel); chromyl chloride (a volatile Cr(VI) compound, aka liquid cancer); chlorine (fun fact: steel ignites spontaneously in chlorine, if the temperature exceeds 100C [one of my previous employers managed to burn down a chlorine pipeline when a pump overheated]); tetrakis(trimethylphosphino)nickel (explodes on contact with air); antimony pentafluoride (super Lewis acid); diphosphene (HP=PH, a by-product of PH3 generation that is pyrophoric); sodium-potassium alloy (NaK, ignites in moist air, sometimes hypergolic with Teflon) to name a few.
Can we get some Lithium-Chlorine compounds with some nitrogen triple bonds. Those are always fun when you make them in the lab and they displace the Silicates in your glasswear as soon as you let the argon out and pump in the chlorine-tetrafluoride. And some Azadoazide-azide for the extra oomph. 😈
Me, who knows practically nothing about chemistry: Yo this molecule looks like a 3D kaleidoscope image, must be a solid S tier! The video: Ok here we have a big fat lame molecule that's also purposeless and unoriginal so it's a B tier. No I'm not admitting that I'm feeling sorry for a lifeless molecule.
I regret that I dropped out of Chemistry in University. You make me want to study it again. Love organic chemistry the most, it's so interesting and clever. OC Lab was so fun. It's basically magic, making a compound with clever reactions.
If you want to learn the material, you can do so without doing do in an academic context - especially if you aren't planning to go into the field of chemistry for a career
Wait ok so I’m in AP Chem rn and I’ve always wondered why at some point chemists stop using Lewis structures and start just drawing shapes. What are those random rectangles and what do they mean?
I got brought here by the algorithm and I spent the whole video weirdly fascinated while barely understanding how some of these are more cursed than others. It's not like I have zero knowledge in chemistry but it's really not my field. Fascinating to watch though.
Explosions and Fire synthesized some C2N16. Dude saw the compound being called "The most dangerous explosive" and took it as a challenge. In the end it wasn't nearly as reactive or energetic as made out to be.
The stuff Klapotke had was C2N14 - one tetrazole ring with three azide groups attached to it, one directly off the tetrazole ring and the other two bonded through a carbon atom. Apparently that second tetrazole ring mellows it out quite a bit.
Yaaay dark mode tier list. Thank you because I always watch your vid before sleeping as it reduce my stress from office working... Man i missed working in the lab
My biggest inorganic chemical bane is attempting to recover gold plating from an 8% tin, phosphor bronze substrate. Copper chloride etching results in the plating disappearing into the solution, probably in some form of Purple of Cassius, which is then difficult to extract the gold from. Any method involving nitric acid results in metastanic acid goo. Electrolytic methods using various concentrations of sulphuric acid results in insoluble tin sulfates that are almost as bad as the metastanic, but in a more solid form. It would help if the material was not pre granulated, but it is what it is.
@@That_Chemist I've had some success using a mock up process of electrolysis in concentrated sulphuric acid in a rotating container, since that process tends to stall due to Faraday effects. But it was a small mock up, and tended to overheat from the current flow. It being a flint glass container, I was concerned about themal shock failures and hot sulphuric acid spills. So that process is on hold awaiting inspiration. Supposedly a similar process using a concentrated brine solution holds promise.
1:30 what are the applications? ClF3 is useful in semiconductor industry because downtime is extraordinarily expensive. Interhalogen + hydrolysis to HF+HCl should give it a decent rank by yikes factor alone. Also it burns sand and concrete
