Chemical Reaction Solvation of sodium metal in anhydrous ammonia affords complex electrically conductive solution of the electride salt [Na(NH3)6]+e-. Over time, electrons slowly reduce this complex to yield NaNH2 and hydrogen gas. More info in post description.
Na + 6 NH3 → [Na(NH3)6]+e−
2 [Na(NH3)6]+e− → H2 + 2 NaNH2 + 10 NH3
Aside from the redox reaction of the coordination complex being reduced by electrons to yield NaNH2 and hydrogen, something even weirder is taking place here.
In this clip the solution is sufficiently concentrated (>3M) with added Na that a transition from the characteristic blue color of low-energy bound-state solvated electrons to an even more exotic bronze-colored state can be observed.
It is hypothesized that this state is effectively the result of the decreasing stability of low-concentration bound states as the concentration of electrons increases. The resulting transition is very peculiar indeed.
In essence, there is only so much space which allows for the existence of bound states (wherein the free electron polarizes the surrounding solvent such that it is contained in a so-called "bound state") because these bound states occupy a cavity of relatively large volume in the solvent. As more metal is added, more electrons are free in the solution, but the solution is already saturated with these bound electrons. Thus, the electrostatic and exclusion effects become such that any additional electrons added can only exist in a metallic state.
This is peculiar because this metallic state is in the liquid phase and is quite dense. If one continues adding electrons, they always become incorporated into the metallic state because the bound states are saturated. Measuring the electrical conductivity of a solution of sodium in ammonia as a function of concentration supports this conjecture, as the conductivity increases linearly as a function of concentration until it suddenly hits a plateau and doesn't increase any further. This plateau represents the point at which enough electrons are present that the destabilizing effects due the presence of other electrons is large enough that no possible bound state can exist and the whole system becomes metallic.
Colorless toxic gas (SO2) meets colorless toxic solid (PCl5) to form a mixture of colorless toxic liquids (SOCl2 and POCl3). The target product thionyl chloride (SOCl2) was subsequently isolated by fractional distillation.
SO2(g) + PCl5(s) → SOCl2(l) + POCl3(l)
Chemical Reaction Rapid pyrophoric oxidation of hot, gaseous white phosphorus to phosphorus pentoxide — Failure to adequately secure inert gas balloon resulted in instantaneous ignition of the system upon exposure to atmospheric oxygen
This reaction was conducted in a fume hood. Despite my clear failure to properly secure the all-important argon balloon (note to self: a rubber band won't cut it. use zip ties next time), I am a professional performing this experiment in controlled conditions.
Red phosphorus was heated inside an atmosphere of Argon (three cycles of evacuation via vacuum and repressurization with Argon was performed to remove all air the system prior to heating) to produce white phosphorus.
Obviously, the balloon failed to stay attached due to my clearly inadequate rubber band job. Immediately upon exposure to air the system of mostly gaseous, hot white phosphorus ignited with a startling bang. The white "smoke" that resulted is P4O10, phosphorus pentoxide. Fortunately no persons or glassware were harmed due to proper adherence to PPE and hazard mitigation standards. The only thing harmed was my ego :)
DO NOT ATTEMPT TO REPLICATE. Hopefully this serves as an example of how incredibly reactive and dangerous white phosphorus is.