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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?

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    $\begingroup$ Alumina and several other ceramics are pretty resistant to fluorine gas at room temperatures. Not sure what optical clarity you can get easily - I doubt you want to try and drill out a sapphire. You could still seal the top with glass. $\endgroup$ – Jon Custer Nov 14 '14 at 21:50
  • $\begingroup$ Sealing fluorine in regular glass will do more than fog the surface. It will fairly quickly etch the glass and escape. $\endgroup$ – Geoff Hutchison Nov 15 '14 at 15:20
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    $\begingroup$ @uhoh I assume they select a proper material for the pressure vessel that does react with the fluorine in a manner to create a thin layer of metal fluoride that eventually becomes impermeable to the elemental gas. So it self-passivates the surface. The answers I'm getting here don't look to promising for any clear material that won't fog and won't disintegrate over time. $\endgroup$ – docscience Nov 12 '18 at 21:04
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    $\begingroup$ Thanks! Here's a quite exotic solution: youtu.be/TQDjILTly3s $\endgroup$ – uhoh Nov 12 '18 at 21:08
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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.

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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.

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above: Photonics.com back in 2003: In Search of Calcium Fluoride: Manufacturers face new production challenges as they attempt to meet rising need.

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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.

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