|Molar mass||83.9767 g/mol (anhydrous)
101.022 g/mol (monohydrate)
|Appearance||white, crystalline solid
|Density||3.1 g/cm3 (anhydrous)
2.1 g/cm3 (monohydrate)
1.914 g/cm3 (trihydrate)
|Melting point||1,291 °C (2,356 °F; 1,564 K) (anhydrous) (sublimes)|
|0.56 g/100 mL (0 °C)
0.67 g/100 mL (20 °C)
1.72 g/100 mL (100 °C)
|R-3c, No. 167|
|EU classification||No classification according to EU Regulation (EC) No. 1272/2008.|
|US health exposure limits (NIOSH):|
IDLH (Immediate danger
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is: / ?)(|
Production and occurrence
- H2SiF6 + Al2O3 → 2 AlF3 + SiO2 + H2O
Alternatively, it is manufactured by thermal decomposition of ammonium hexafluoroaluminate. For small scale laboratory preparations, AlF3 can also be prepared by treating aluminium hydroxide or aluminium metal with HF.
Aluminium fluoride trihydrate is found in nature as the rare mineral rosenbergite.
Its structure adopts the rhenium trioxide motif, featuring distorted AlF6 octahedra. Each fluoride is connected to two Al centers. Because of its 3-dimensional polymeric structure, AlF3 has a high melting point. The other trihalides of aluminium in the solid state differ, AlCl3 has a layer structure and AlBr3 and AlI3, are molecular dimers. Also they have low melting points and evaporate readily to give dimers. In the gas phase aluminium fluoride exists as trigonal molecules of D3h symmetry. The Al-F bond lengths of this gaseous molecule are 163 pm.
Aluminium fluoride is an important additive for the production of aluminium by electrolysis. Together with cryolite, it lowers the melting point to below 1000 °C and increases the conductivity of the solution. It is into this molten salt that aluminium oxide is dissolved and then electrolyzed to give bulk Al metal.
It is also used to inhibit fermentation.
It is a sputtering target for preparation of low index films.
AlF3 has low toxicity (LD50 600 mg/kg).
- "NIOSH Pocket Guide to Chemical Hazards #0024". National Institute for Occupational Safety and Health (NIOSH).
- J. Aigueperse, P. Mollard, D. Devilliers, M. Chemla, R. Faron, R. Romano, J. P. Cuer, "Fluorine Compounds, Inorganic" in Ullmann’s Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005.doi:10.1002/14356007.a11_307
- Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0080379419.
- Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.