Bromine, chlorine and iodine can all be sealed in a glass container for display without the elements reacting with the glass.
But if you try to seal fluorine in glass I believe it will react and fog the surface making it harder to see the gas, right?
What's the best way, if at all possible for long term containment of fluorine for display?
As @JonCuster mentions, some materials are pretty resistant to fluorine gas at room temperature.
But out of curiosity, I checked Theodore Gray's website. He's made an effort to have a "periodic table" table with actual elements. He also has a beautiful book, called (naturally) The Elements.
Almost anything placed in the path of a stream of fluorine gas will spontaneously burst into flame. This includes things like, oh, say glass, steel, and other things not normally thought of as flammable. It is, therefore, fairly difficult to have a sample of it in an element collection. I used to have a statement here that there was no transparent container that could hold fluorine for any length of time, but I was corrected by a man who has figured out how to do it.
There's more here but I'll summarize. Basically, the problem with glass is the $\ce{Si-O-H}$ bonds, which will auto-catalytically react with $\ce{F2}$ to give $\ce{HF}$, and that etches the glass. So with a high quality quartz tube, a lot of annealing, and a fluorocarbon grease to coat the glass and minimize reactivity, it works.
Interestingly, I always had the idea that fluorine gas was a light blue-green. Instead, it's brownish.
Here's a slightly exotic, expensive solution: solid, crystaline $\ce{CaF2}$ tubing will do the job.
How to get the gas inside, then make a glass seal, is a bit of a challenge though. Surfaces can be optically polished ultra-flat, mated, and locally melted. Ultrasonic friction melting perhaps, or flame or IR. This is an expensive but viable option and would need some development.
According to the Periodic Table of Videos Fluorine Gas found in nature (NEWS) in 2012 existence of naturally occurring fluorine was found in "fetid fluorite" a form of fluorite where natural radioactivity has caused free fluorine to form and migrate within the crystal. The remaining Calcium has already fully reacted with fluorine and is therefore protected from attack.
A tube manufactured from polycrystalline $\ce{CaF2}$ might do the job nicely. It is a common optical material used in certain applications. For example, the UV transparency and resistance to UV damage and darkening (solarization) has made lenses of polycrystalline $\ce{CaF2}$ essential in the smallest dimension micro lithography for fabrication of computer chips.
above: Photonics.com back in 2003: In Search of Calcium Fluoride: Manufacturers face new production challenges as they attempt to meet rising need.
above: From optik-photonic.de Calcium Fluoride Crystals Blanks Offer Highest Transmission Rates at 193 nm and Below
Many sources for polycrystalline calcium fluoride or "$\ce{CaF2}$ glass" exist. Corning is one example, and it is possible that magnesium fluoride would work as well:
Angewandte Chemie International Edition: Secret of “Fetid Fluorite” Aired: Elemental fluorine F2 detected for the first time in a natural mineral:
Florian Kraus of the TU Munich, as well as Jörn Schmedt auf der Günne and Martin Mangstl at the Ludwig Maximilians University in Munich have now obtained direct proof: Elemental fluorine is the guilty party that causes the unpleasant odor. By using 19F nuclear magnetic resonance spectroscopy (NMR spectroscopy), they were able to show for the first time that elemental fluorine is contained in “antozonite”.
How is this possible for such a reactive gas? The researchers explain that “antozonite” contains a tiny amount of uranium that, together with its radioactive daughter nuclides, constantly releases radiation into the surrounding mineral. This causes fluorite to split into calcium and elemental fluorine, forming the calcium clusters that give “antozonite” its dark purple color. The fluorine is contained in tiny enclaves surrounded by nonreactive fluorite, which shields it from the calcium, allowing it to maintain its elemental form.
This is not something to speculate on...it has been done.
Fluorine gas was observed by Moissan, actually, (i.e. over a hundred years ago and by the man who first isolated the element). He used a platinum tube with CaF2 windows at the ends.
He actually published a color image--if you have access to a first class academic library or a good file server, may be able to see it there. But here is an image from Wikipedia Commons (fluorine in the middle):
Although perhaps looking in the journal hard copy would be better...then again, reproduction of observed color is a tricky deal (even nowadays, don't get me started on three wavelength color matching for car paint!).
Journal cite: H. Moissan, Ann. Chim. Phys. 25 (1892) 125
Also, I'm not clear if the Moissan image was a color photo or a drawing. Image on wiki is not clear enough to tell.
But in any case, it was a tough experiment then and still would be now. But if you have a good machine shop and the money...it's possible to do it again. I would advise a light source to shine through the tube. But the Pt cost and the seal of the flourite stoppers will be the hardest part.
Safety note: Do it in a fume hood, please, and with proper safety precautions (limited amounts of gas, manual transfers). Fluorine gas is no joke. Don't be a "martyr".
In addition to the suggestion of using metal fluorides like CaF2, I want to mention the possibility of using carbon-based fluoropolymers like polytetrafluoroethylene (PTFE), perfluoroalkoxy alkanes (PFA), and fluorinated ethylene propylene (FEP), all of which may be sold under the brand name "Teflon", which has become synonymous with PTFE for many people. These plastics are some of the most commonly used materials for dealing with highly reactive fluorine compounds like HF, UF6, and HSbF6, as well as other reactive compounds. All these plastics are colorless, but PTFE is more just translucent, and generally looks white, while FEP and PFA are the properly transparent ones.
You can see on this chemical resistance chart that PTFE is considered "resistant" to dry F2 up to at least 60°C, as well as everything else they have data for. PFA is apparently similar. FEP is also apparently compatible with F2 up to at least 60°C: https://www.polyfluor.nl/en/chemical-resistance/fep/ That page also mentions "better gas and vapor permeability", though, which sounds somewhat worrying if you want to hold gaseous fluorine in it. However, I think "better" might actually mean lower, since this pdf of general info on FEP films from Teflon.com mentions it having exceptionally low permeability to gases and non-gases.
Some rather vague comparisons of these 3 substances are given here.
These polymers may be cheaper than metal fluorides (though I'm not certain of that), but they are not fully fluorinated, and thus can still react with F2, e.g.:
(CF2)n(s) + nF2(g) → nCF4(g)
As this page by a company selling them puts it, "[t]he extremely potent oxidisers, fluorine (F2) and related compounds (e.g., chlorine trifluoride, ClF3 ), can be handled by PTFE/PFA only with great care and recognition of potential hazards. Fluorine is absorbed into the resins, and with such intimate contact the mixture becomes sensitive to a source of ignition such as impact." That quote implies that teflon can burn in fluorine (as can normal oxide-based glass). This makes sense because I know it can burn in oxygen, although it does not normally burn in air, because "teflon" fires in the liquid oxygen tanks are believed to have been part of the cause of the Apollo 13 disaster. Also, those chemical resistance sheets I linked to list FEP, PTFE, and PFA all as "not recommended" for use with F2 at 100°C, and that Teflon.com pdf specifically mentions that FEP reacts with "molten alkali metals, fluorine at elevated temperatures, and certain complex halogenated compounds, such as chlorine trifluoride, at elevated temperatures and pressures." When combined with the fact that these fluoropolymers melt and chemically decompose into (somewhat toxic) gases at temperatures fairly typical for plastics, this means they are not very resistant to fire-like temperatures. (Thus, for example, you probably should avoid trying to close F2 in an FEP ampule by melting the tip, though maybe it would work if the F2 was in the form of a liquid far from the part you were melting. I've seen specific references to FEP being good for cryogenic temperatures and not becoming brittle, so it probably is the best for liquid F2.)
(There is a question on this stack-exchange specifically about what can attack PTFE: Is there ANY chemical that can destroy PTFE, or Teflon? .)
Metal fluorides, on the other hand, are much more refractory (though not as refractory as oxides). CaF2, in particular, has one of the highest melting points (my best number for the melting point is 1423°C from my CRC Handbook), though ScF3, LaF3, and CeF3 at least have higher melting points (but much lower boiling points). There is also no way for CaF2 and many other metal fluorides to be further fluorinated or burned in any way. (Some can react to form higher fluorides, which may even be gases, but there's no reason to use those.) One potential problem with CaF2 and many other metal fluorides is that they have non-trivial solubilities in water. The solubility of CaF2 in water is still very low, though, (similar to CaCO3) so I'm guessing it won't dissolve unless you leave it in a large body of water or use it as plumbing for a really long time, let it be rained on for many years, or dump acid on it. (The latter is how HF is commercially produced.) CaF2 and many other metal fluorides can be very transparent if pure (fluorides and fluoride mixtures like ZBLAN are used for fiberoptics, lenses, and windows on lab equipment), and I'm not sure if that's true of fluoropolymers.
SiO2, Al2O3, and some other other non-fluorine compounds are highly transparent, refractory, and insoluble in water, and also quite resistant to oxidation by F2. They can, however, still theoretically be corroded by F2:
SiO2(s) + 2F2(g) → SiF4(g) + O2(g)
ΔG°298K,1atm = -172.55 kcal/mol for glass or -171.13 for quartz (reaction is spontaneous)
2Al2O3(s) + 6F2(g) → 4AlF3(s) + 3O2(g)
ΔG°298K,1atm = -303.0 kcal/mol for corrundum to crystalline AlF3 (reaction is spontaneous)
Note that SiF4(g) is a gas (boiling point somewhere around -86°C or -90.3°C), while AlF3 is a colorless refractory solid (sublimation point 1290~1291°C) that might form a protective layer on the inside of a container, similar the NiF2 layer that forms on the inside of the nickel containers commonly used to store F2 and other highly fluorinating compounds. Thus, I suspect that Al2O3 is a better option than SiO2. It's possible this advantage could also be gained with "aluminosilicate" glasses (made of just Al, Si, and O), and, in any case, these probably work at least as well as fused quartz (pure SiO2 glass).
As I mentioned, melting an ampule containing F2 closed is not a very good idea, unless it's made of metal fluorides (and some metal fluoride glasses do have very low glass-transition temperatures), because both fluoropolymers and oxide-glasses react with F2 at high temperature, and may ignite under such conditions. Sealed ampules are also quite difficult to put things into or take things out of without breaking the seal. Other methods of making air-tight seals I know of tend to involve some kind of rubbery material ("elastomer", at least if a polymer). This may be used as an O-ring underneath some kind of cap or tube attatchment, or could be used to make a self-sealing membrane. I've often seen that silicones are used as these elastomers, especially for self-sealing membranes. There are fluorosilicones that may be quite resistant to F2, but normal silicone should generally be attacked by F2. Silicones all involve Si-O-Si chains, and at least almost always contain Si-C or O-C bonds, and these bonds can be attacked by fluorine. Some websurfing shows that apparently there are quite rubbery fluorocarbon elastomers, too, though. If you look at page 19 of this pdf, you can see that 3 elastomers they consider ("PERLAST®", "FKM (fluorocarbon)", and "FVMQ (fluorosilicone)") are listed as having "good" (but not "excellent") compatibility with fluorine. ("Good" apparently means they swell 10~20% when used with F2, indicating something bad might be happening.) I think the first two are both fluorocarbon-based, with PERLAST® being "FFKM", which is specifically perfluorocarbon-based, like PTFE or FEP, based on the website selling it. In any case, whoever makes the normal nickel or whatever containers F2 is sold in must have already solved this problem. (Actually, the comments on uhoh's answer point towards Halocarbon 25-5s grease as being fluorine-proof and in-fact specifically recommended for use with gaseous F2. I don't know if that's good enough by itself for a long-term seal, though.)
I have sealed fluorine into glass ampoules routinely when I used it as an initiator for the polymerization of tetrafluoroethylene.
The borosilicate glass ampoules should be annealed before use and kept in an oven at 100°C
One must just know how to measure what is "condensed" in the glass ampoule. Fluorine never liquefies or solidifies when cooled in liquid nitrogen. As long as the pressure in the glass tube is sufficiently low the glass will collapse and seal.
A friend knew u could do this. He asked me to try fluorinating graphene in perfluoroheptane. We tried this and it worked. This led to a publication in the journal Carbon.
