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!?
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
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. 😂
"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.
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.
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
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!
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...
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
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.)
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
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!
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.
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
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.
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.
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.
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:)
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.
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
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).
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.
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.
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
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.
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
me looking through the weird shapes. sees chemical second from the bottom to the right. My first thought: hey thats… *OH* …thats a lot of fucking nitrogen
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 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 😂
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
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!
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.
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.
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.
why do the Einsteinium(III) complex and the hexaferrocenylbenzene look more like depictions of biblically accurate angels than actual chemical compounds?
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.
I absolutely disagree with your ranking/appraisal of rhodium (ii) acetate! At first, there is a single metal-metal bond, not a triple one (there is a similar mixed Ru(II,III) paddle-wheel type complex with a bond order 2.5, by the way, though it's paramagnetic and not as convenient to work with as rhodium analog). Yeah, rhodium itself is the most expensive precious metal nowadays, but for academic research it's not always a big issue. For the carbene transformations you would preferably take Cu(I) complexes as an alternative, but these are way less reactive, so one should usually extend the reaction times and/or increase the temperatures while working with copper catalysts. Besides, the loadings for the Cu(I) salts are frequently 5-10-20 mol%, while for the Rh(II) it's usually enough only 1 mol% or even less. Another cool thing is that you can easily displace the acetate ligand with chiral carboxylates, which are extremely affordable, so it's a great way for catalyst screening in asymmetric catalysis. Despite the fact formal oxidation state +2 is pretty uncommon for Rh (it usually forms +1 or +3 complexes), these rhodium(II) carboxylates are of extraordinary stability, so one can literally purify them by passing through a standard flash chromatography on silica gel with PE/EA as eluent. Sooo, there are many reasons, why people are so into this type of catalyst :)
Silver can also be used - I’m not sure why ChemDraw automatically made it triple bonded - I thought it was correct based on similar complexes on the web with other metals
@@That_Chemist Silver might be used for non-stereospecific carbene transformations, though it's quite light-sensitive and less convenient then copper. There are other metal complexes that are capable of promoting carbenoid transformations as well: iron triflate, cobalt porphyrins, some ruthenium complexes, gold(I) derivatives etc, but none of these is as reactive as Rh(II) carboxylates, which can activate diazo compounds even at -78 oC. As for the bond orders, these depend on the metal itself, let's say Cr(II) and Mo(II) also form the same acetates but with the bond order 4
Agreed. And as a footnote now elements like Rhodium and Palladium are very expensive nowadays. Due to the increase prices, many researchers are tend to use alternative transitions metals such as Silver or Cobalt.
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?
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'm voting for azidoazide azide because literally nothing can make it explode. By witch I mean you can leave it undisturbed in a perfectly temperature controlled in chamber with no light, movement, interactions, and pray to god that it stays that way and it'll hear you praying in a science lab and decide to t no linger wishes to be.
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. 😈
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
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.
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.
Wow that’s super cool!
@@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.
IDK, more like crazy molecules
as someone who has no idea how chemistry works, these all look like biblically accurate angels
haha
@@That_Chemist why do you feel the need to reply to everything even if you don't have anything useful to say?
@@k2_x376 ironic
don't you worry. only half of them are
Biblically accurate compounds.
I think S tier here should be described as 'furthest from God' because there is no other way to justify putting 3 noble gases in one molecule
Haha
Your scientists were so concerned with whether or not they could, they didn't stop to ask themselves if they should
Wait wait wait what ? I just started the video but 3 noble gases in one molecule ? Who ? Why ? How ? I agree with your classification because wow.
How about interhalogen compounds like Chlorine trifluoride then? i somewhat miss it here.
Hubris
"It does have an application"
Let me guess, it's used for making nukes, semiconductors, or as exotic rocket fuel?
"synthesis of plutoni-" Of course.
Imagine being in a field that has something called "silly no-no esthers"
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!?
goofy ahh chemical
Are any chemists named Esther?
LOL I have a Fisher diagram of L-Dopamine methyl ester tattooed on my shoulder cause my wife’s name is Esther. 😂😂😂
As an organometallic chemistry researcher. I work with organolithium compounds without a concern… But that Einsteinium complex… that thing give me chills
Haha
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
@@I_saw_that. I have a list of over 200 interesting and cursed compounds I want to synthesize lol.
The thing looks like Switzerland!
Well the Es-complex might have some use in 3-10 laboratories in the world, if it's Es-specific enough...
If inorganics look like organics, they're cutsed by default
Haha
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.
@@johndododoe1411 Then it wouldn't be organic by definition, right?
I fail to see how some of these are even inorganic
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. 😂
"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!"
HeH, what a funny joke
What about H-H?
@@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.
Ok but like, why did HeH form but not H2? What is it that made HeH more favorable that it would occur first?
That kripton Is in a cage because it dared to react with something
I hope it learns it’s lesson
Krypton jail
Tha Phantom Zone
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.
Noble Gases: Inert, unreactive, will not form compounds-- meanwhile, Fluroine: "Hold my electron."
100%
You mean Francium?
fluorine is more like 'gimme your electron', 'hold my electron' would be elements to the left of the tabl like sodium and potassium
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
Moments after the big bang, the universe invented chemistry by forming the first molecule, and thought to itself: "H-He+ this is going to get funny."
"H He" is the sound of the universe laughing.
Synthesised using a Van Der Graaf Generator
I'm kinda sad you didn't include my favorite cursed molecule: chlorine trifluoride. It would rather be bonded to almost literally anything else.
Or to put it another way, it's hypergolic as sin.
Except for the passivation layer when you put it in steel containers.
"two noble gases in one complex" and THAT'S the weirdest thing about Schrobilgen's Special? not the fluorine with two bonds?
Ok that’s fair
my brain refuses to accept both the F double bond with two separate noble gases.
Being able to rationalize calling it “sele no no compound” makes it S tier
haha
Silly nono compound
Let's be honest dude, inorganic chemistry is just cursed period. Didn't stop it from being my favorite branch of chemistry to study/research
:)
On the other side, you got colorful bunch of cursed mess :^)
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!
@@hamstsorkxxor ah yes, tar, every ochemist's beloved[citation needed] byproduct color~
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...
:)
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
cool!
Shiny and tasty
Wait, _pink??_ As in, it's fluorescent at two frequencies at once?
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.
It’s so small, but still toxic
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.
It wasn't the Braunschweig Lab, was it? :D
@@Bigcubefan no, this was a while back, very possible the PI has since retired
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.)
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
Before watching, I predict that xenon tetroxide is on the list and that it is S tier.
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've expected him to leave C2N16 for the last, and for whole table to explode the moment he clicks on it.
"So it exists, but most of the time it doesn't wanna exist." relatable, honestly
:(
The AuXe4 paper mentions that dark red crystals could be grown at -78°C with the Sb2F11 anion. I want to see a chem youtuber synthesize that SO BAD.
Nobel gas chemistry is really dangerous
@@That_Chemist That's why we trust professionals to do it. Professionals like youtubers filming from their shed.
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.
This list is a bit heavy on metalorganic and organometallic molecules for a inorganic list. But still nice.
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
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.
"Did he include one of these nitrogen monstrosities? quick scan. Yes, of course!"
@@sharpfang azides for days!
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.
Haha, that's a mineral
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.
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:)
Yeah. This and its tungsten analog are not particularly noteworthy.
ah yes, chemical horrors beyond my comprehension
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.
Welcome to the channel :)
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
Yeah but I already talked about him in another video (not sure if I posted it yet - it might be in tomorrow’s video)
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).
You should read things I won't work with by Derek Lowe, he has also one about FOOF along with other absolutely terrifying and cursed compounds.
Ah yes the interhalogens that oxidize *sand*
(ClF3 reference)
There is no way he hasn't read all the "how not to do it" and "things I won't work with" posts
Pretty sure Lowe mentioned the C2N16 compound too.
Sand won't save you this time.
Next Figueroa paper: Synthesis of Argon Fluorohydride without Specific Conditions, and he just bubbles Argon through a solution of HF in acetonitrile
100%
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.
F - i thought that nitric isn’t supposed to be that bad on skin, maybe it was a mixture
Helium hydride looks like god made a mistake while creating the universe now its too late to change it back
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.
God, please forgive me for what I'm about to do with the Einsteinium III complex
👀👀👀
Welcome back to the Tier List of "That Chemist Tier List Videos". This video clearly goes in S Tier.
A curious class of organometallic compounds are hexa-aurated methanium dications, [C(AuL)6]2+. An hexa-coordinated carbon is definitely cursed
Love the dark mode. Also love the videos! Keep up the good work :)
Thank you :)
You know the tier list is good when the first molecule is a polyhedron
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
It's cool to hear your own personal accounts dealing with some of these chemicals. It makes the tier list a lot more personable.
thanks!
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.
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
9:24 I wasn't paying attention and the "silly no-no esters" killed me. I know that you're trying to push this as a real name, but it sounds hilarious.
Haha
i love watching these videos because it makes me really excited to learn about new concepts in my ap chem class. awesome video dude!
Thank you!
Inorganic Molecule Structures: 😎
Inorganic Molecules complete IUPAC names: 💀💀💀
7:25 that is not an inorganic chemical, it is an organometallic
And you might be asking what is the practical applications of these chemicals.......there isn't. Love it.
me looking through the weird shapes. sees chemical second from the bottom to the right.
My first thought: hey thats… *OH* …thats a lot of fucking nitrogen
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 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 😂
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
never say never!
Me not understanding a thing he's saying: I like your funny words magic man.
My therapist: Hexaferrocenylbenzene is not real, it can't hurt you.
The Hexaferrocenylbenzene: Be not afraid!
i know nothing about these chemicals but I find these videos very entertaining.
I only did 1st and 2nd year chemistry for my biomedicine degree so ALL of these look cursed. I didn’t even know half of all these bonds existed.
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!
Thanks for letting me know!
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!
Visually striking
Unexpected
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.
@@chrisb3585 And then the richest man in the world tosses tonnes around at a beach resort.
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.
Cool 😎
As someone who is just starting chemistry, I am absolutely terrified of what's about to come
endohedral fullerene kypton is the closest we'll get to kryptonite
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.
Wow!
Isn't CLF5 actually more stable than ClF3?
I really thought you said "Silly-No-No-Esters" back then...
Haha
At first glance I thought Rhodium Acetate was a bar magnet diagram and not a compound.
As something of an aside, doing chemical engineering calculations for uranium chemistry is cancer. It's not well documented in ASPEN.
Can provide references for the S and A tier molecules in the description?
why do the Einsteinium(III) complex and the hexaferrocenylbenzene look more like depictions of biblically accurate angels than actual chemical compounds?
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.
I'd also include trifluornitrosomethane in this list. No C-C or C-H bonds, so I would count it as inorganic.
It’s so cool
I agree that fullerenes are not organic, just like diamond and graphite are. You need some other atoms in there.
like hydrogen
@@That_Chemist *cheeky*😜
I absolutely disagree with your ranking/appraisal of rhodium (ii) acetate! At first, there is a single metal-metal bond, not a triple one (there is a similar mixed Ru(II,III) paddle-wheel type complex with a bond order 2.5, by the way, though it's paramagnetic and not as convenient to work with as rhodium analog). Yeah, rhodium itself is the most expensive precious metal nowadays, but for academic research it's not always a big issue. For the carbene transformations you would preferably take Cu(I) complexes as an alternative, but these are way less reactive, so one should usually extend the reaction times and/or increase the temperatures while working with copper catalysts. Besides, the loadings for the Cu(I) salts are frequently 5-10-20 mol%, while for the Rh(II) it's usually enough only 1 mol% or even less. Another cool thing is that you can easily displace the acetate ligand with chiral carboxylates, which are extremely affordable, so it's a great way for catalyst screening in asymmetric catalysis. Despite the fact formal oxidation state +2 is pretty uncommon for Rh (it usually forms +1 or +3 complexes), these rhodium(II) carboxylates are of extraordinary stability, so one can literally purify them by passing through a standard flash chromatography on silica gel with PE/EA as eluent. Sooo, there are many reasons, why people are so into this type of catalyst :)
Silver can also be used - I’m not sure why ChemDraw automatically made it triple bonded - I thought it was correct based on similar complexes on the web with other metals
@@That_Chemist Silver might be used for non-stereospecific carbene transformations, though it's quite light-sensitive and less convenient then copper. There are other metal complexes that are capable of promoting carbenoid transformations as well: iron triflate, cobalt porphyrins, some ruthenium complexes, gold(I) derivatives etc, but none of these is as reactive as Rh(II) carboxylates, which can activate diazo compounds even at -78 oC. As for the bond orders, these depend on the metal itself, let's say Cr(II) and Mo(II) also form the same acetates but with the bond order 4
Agreed. And as a footnote now elements like Rhodium and Palladium are very expensive nowadays. Due to the increase prices, many researchers are tend to use alternative transitions metals such as Silver or Cobalt.
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?
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'm voting for azidoazide azide because literally nothing can make it explode. By witch I mean you can leave it undisturbed in a perfectly temperature controlled in chamber with no light, movement, interactions, and pray to god that it stays that way and it'll hear you praying in a science lab and decide to t no linger wishes to be.
vinyl figures in mason jars is out, noble gas atoms trapped inside buckyballs is IN
:(
0:23 i don't want to do reactions with tiny basketballs
A: What is it used for?
B: Writing papers about it.
Borazine, the "inorganic benzene"
I probably won't be sleeping tonight
F
Nobody:
Hexaferrocenlybenzene: “ *BE NOT AFRAID* ”
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. 😈
I don’t know what you’re talking about at all, only have completed high school chemistry, but these videos are so interesting
Glad to hear it :)
There's an old joke about the first chemist who discovered helium hydride, but he had to give it up - he couldn't find a container to keep it in.
it's just a matter of time until we find some chemical in the shape of among us bro.....
bromic acid - I featured it in this video - ua-cam.com/video/xgjJBJdPCKw/v-deo.html
7:54 "Foof" caught me off guard xD
😳What if we kissed😳
😳Inside the fullerene cage?😳
7 minutes in fullerene heaven
guy just died and he still got in c tier
I have just seen Bertrands lecture on 2022 ICOMC in Prague. These structures are far from cursed. Also decamercuroferrocenes were quite crazy to see.
Cool
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
"Endohedral fullerenes"
I wonder how big a cage of carbon you need to contain a UF6 molecule? Or would it react and fluorinate its containment vessel?
it would absolutely do so
I like your channel a lot, but I really fall out of understanding frequently. I’ll try to persevere.
As somone who is about to start chemistry at uni this video gave me goosebumps
🤙
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.
9:22 I also tried to make silly no-no esters at some point.