Open up a glass syringe and dig out some iodine that has crystallized in there after using the syringe itself to transfer some iodine monochloride onto various substrates for testing its reactivity towards various substances.
(magnesium dust, something like 500 mesh, surprisingly less reactive than expected. Aluminium powder, 30 micron particle size-no spontaneous reaction other than starting to turn to white solid, either AlI3 or AlCl3 anhydrous, didn't test which, ignition to the point of glowing white hot upon the slightest flame being applied. Sulfur-solid, small chunk, dissolved into a stinking puddle of blackish goo, smoked plenty, stank some more, oddly, became very difficult to ignite at all with a blowtorch, held flame on it sufficiently long to thermally decompose the interhalogen into its component chlorine gas and iodine and it would only burn for a second or two after withdrawal of the flame. Have yet to try powdered sulfur. Will also, once I take up somebody's offer, try it on tellurium, staying masked and WELL downwind. Because Te has a nasty side effect of absorption of even traces. You stink. And stink for a long time, badly enough that I've heard the term for it, 'tellurium breath' being used as an insult, and of people killing themselves, as well as any object they touch becoming contaminated by the traces of alkyl tellurides coming out in sweat, such as uni books forevermore stinking and having to be retired lest somebody else happen to touch them and suffer the same.
Contact with phosphorus (red)-instant hypergolic ignition the second the two chemicals contacted each other. One drop of ICl and the small sample of red P burst into an intense flaring flame.
Something odd happened too-there was later, 7-8 HOURS later, and in a place in the garden I did not DO these experiments near, with this air- and atmospheric moisture-sensitive compound, observed by my old man, a sudden occurrence of a patch of what used to be grass and soil, but had become a crater full of black, bubbling, smoking goo where part of the lawn used to be. That I am actually perplexed by, since it was far away from the experiments, and ICl is highly volatile, and it isn't stable near either things that can be oxidized, near water, exposure to air, or even atmospheric water vapor content. It would, if placed in a glass petri dish and left outside, just vaporize away, perhaps leaving behind a little iodine, more likely evaporate totally. So I am actually perplexed by whatever caused that blackened, bubbling hole in the lawn, where both soil and grass as well as wet moss around it were replaced by a liquefied pit, filled with something slimy looking, giving off smoke, almost 8 hours later, after a frost.
What am I going to do today...harvest the remainder of my iodine monochloride from its flask, transfer it to bottle with chemically very resistant cap and seal that I know will tolerate ICl having held a sample of a fraction of 1ml for months and months without being eaten through or damaged in any way, with the screw threads wrapped in a thick layer of teflon tape. It doesn't eat glass, at least, and presumably the cap is made from teflon. Stupid pork left quite a few of those chemical-resistant sample bottles after 'taking samples' of many of my reagents allegedly for analysis and then leaving them on my benchtop. Now they just serve me as something to use for containment of some of the nastier, more dangerous and volatile reagents I have, which would burn through, set on fire or disintegrate most plastics. Those vials must be highly resistant as they'd need to be able to sample nearly anything.
And also, I'll finish gutting some batteries for their potassium hydroxide (caustic potash, KOH) electrolyte and the manganese dioxide content serving as depolarizer so I can purify the MnO2 and turn it to a salt of manganese, such as the sulfate, and then work on trying to isolate some Mn metal. (its one of the transition metals, quite reactive, and in small quantities vital as a micronutrient to humans, although too much, especially via inhalational route is known to cause manganism, a form of poisoning characterized by a progressive parkinsonian-like neurological damage.
Going to (outside of course, wearing mask with additional particle filters attached) attempt electrorefining of the sulfate or chloride salts to manganese metal, which I have never actually seen. I've used its compounds plenty often, either as the dioxide, MnO2, or KMnO4/NaMnO4 respectively. I've also produced as a byproduct, what I believe is sodium manganate or manganite, bright apple-green crystalline compound with a color similar to day-glow greenish yellow highlighter pen ink.
And have when younger, encountered the rather dangerous, and powerful permanganic acid anhydride, Mn2O7, formed via the action of concentrated sulfuric acid on potassium or sodium permanganate, its a dark greeny black, more or less violet black with a slight greenish sheen depending on the angle of light, extremely powerful oxidizer, but not something I'd keep around, since it can explode with very little provocation, such as organic dust motes in the air settling down and coming into contact with this manganese heptoxide.
The green compound would have been either manganese (II) oxide, or potassium or sodium manganate, K2MnO4 or Na2MnO4. Not sure which.
