Rubidium fluoride

It is a cubic crystal with rock-salt structure.

There are several methods for synthesising rubidium fluoride.

One involves reacting rubidium hydroxide with hydrofluoric acid:[1] Another method is to neutralize rubidium carbonate with hydrofluoric acid:[1] Another possible method is to react rubidium hydroxide with ammonium fluoride: The least used method due to expense of rubidium metal is to react it directly with fluorine gas, as rubidium reacts violently with halogens:[1] Rubidium fluoride is a white crystalline substance with a cubic crystal structure that looks very similar to common salt (NaCl).

[2] Rubidium fluoride colors a flame (Bunsen burner flame) purple or magenta red (spectral analysis).

[7] The enthalpy of solution of rubidium fluoride was determined to be −24.28 kJ/mol.

NFPA 704 four-colored diamond Health 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gas Flammability 0: Will not burn. E.g. water Instability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogen Special hazards (white): no code