Well I've got my bromine. At least, I've freed it from the NaBr, although I think I'm going to wait until the daytime heat is spent
before doing the distillation to recover it. Currently its just being left to sit in the flask, with a Dimroth condenser plugged into one of the flask necks, and a vigreaux column fitted to the top of the condenser, as due to the method used to produce it, namely hooking a flask full of potassium permanganate with a pressure-equalizing addition funnel to a piece of disposable plastic tubing with the glass part of a pipette shoved into it, the glass being the only portion of it that is allowed to contact the bromine, as otherwise, plastic would be attacked, and this passed through a hole in a stopper in a neck of the flask containing the NaBr solution, and the addition funnel being used to add concentrated hydrochloric acid to the permanganate, causing a vigorous stream of chlorine gas to evolve and be forced through the tubing/pipette arrangement, condensing any bromine vapor that is carried upwards through the condenser and vigreaux, whilst the byproduct, bromine monochloride, a HIGHLY toxic, strongly oxidizing gaseous interhalogen will either be vented to the atmosphere or perhaps condensed as a liquid (it boils at 8 degrees 'C) and then redistilled, so I can keep a sample of it in gaseous form in a chemically resistant vial, not a large volume of the compound of course, since having it turn from liquid to gaseous phase within a sealed container could easily cause it to shatter and the contents, if it were filled as liquid, to abruptly flashboil, spewing the entire lot into the atmosphere. NOT something I'd like to happen in my lab, since it would attack everything from my keck-clips, to clamp stands and clamps to the wood of the bench-top itself, and plastic reagent containers with the unholy aggressive tendencies of the interhalogens, and some reagents such as solid sticks of roll sulfur, which is just left out on the shelf without a container due to its benign nature would be ignited, and same goes for any such fumes contacting aluminium dust (going from the reaction of iodine monochloride), which would burst into searing, blazing white hot flames, or phosphorus (red, white), the reaction of ICl with red phosphorus, when tested with tiny quantities to examine reactivity (a few hundred mg of red P in powder form, and two drops of iodine monochloride), it didn't just burst into flame, but did so with such violence that it could almost be called explosive. Harmless on that scale of course, being done with only two drops of ICl and a couple of hundred mg of phosphorus, to ascertain the potential for hazardous interactions between the two, but were something like bromine monochloride, more reactive, and gaseous, compared to the 'more tame' ICl [comparatively speaking, that is, ICl is less reactive, but even so, it is very poisonous, and EXTREMELY corrosive, as well as being a powerful oxidizing agent, so tamer is relative. Its like saying one stick of dynamite is less dangerous than ten sticks, while either could quite easily turn somebody into pink fleshy mist]
Not what I'd want to contact the 2kg or so of red phosphorus I have, or start setting the sulfur, the metal powders (there are several, big bags of fine metal powders, namely magnesium, aluminium, zinc, iron and copper) or worse still, the sodium metal brick, currently sealed harmlessly inside a vacuum-packed, heat-sealed thick plastic liner, saturated with heavy mineral oil, and this inner liner itself sealed within a secondary pouch, again, hermetically sealed with heat, and filled with inert gas, the Na chunk being the size of a small brick, and saying nothing of the flammable solvents, compressed gas cylinders, hydride reducing agents such as sodium borohydride, and volatile, reactive things like iodine and bromine] and any number of other bits and pieces that need to have nothing to do with flames and reactive, oxidizing, highly toxic little nasties all ablaze. Because there are enough items of that kind around the lab to be able to cause a whopping conflagration the likes of which I can barely imagine; were a bottle of condensed bromine monochloride, below its boiling point, to be stored as a liquid, immediately to rupture and shatter the bottle as it warmed up past 8 'C. That would quite likely burn the house down if I were so stupid as to try it. With me in it, too.
Messy and unpleasant wouldn't even be the word for such an event. And hell, the fire service's response would be to throw water at it. And considering some of the things in there on my shelves...that would result in it's hitting large blocks of alkali metals, strips of lithium, stuff that would probably release silane gas (pyrophoric, extremely poisonous) and cause a big cloud of acidic smog to come belching forth like a fart straight out of hell.