3D model (JSmol)
|Molar mass||62.3018 g/mol|
|Appearance||white tetragonal crystals|
|Melting point||1,263 °C (2,305 °F; 1,536 K)|
|Boiling point||2,260 °C (4,100 °F; 2,530 K)|
|0.013 g/100 mL|
Solubility product (Ksp)
|Solubility||Insoluble in ethanol|
Refractive index (nD)
|Rutile (tetragonal), tP6|
|P42/mnm, No. 136|
Std enthalpy of
Gibbs free energy (ΔfG˚)
|Safety data sheet||ChemicalBook|
|GHS signal word||WARNING|
|H303, H315, H319, H335|
|P261, P304+340, P305+351+338, P405|
|Lethal dose or concentration (LD, LC):|
LD50 (median dose)
|2330 (rat, oral)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Magnesium fluoride is an inorganic compound with the formula MgF2. The compound is a white crystalline salt and is transparent over a wide range of wavelengths, with commercial uses in optics that are also used in space telescopes. It occurs naturally as the rare mineral sellaite.
Production and structure
- MgO + (NH4)HF2 → MgF2 + NH3 + H2O
Related metathesis reactions are also feasible.
Magnesium fluoride is transparent over an extremely wide range of wavelengths. Windows, lenses, and prisms made of this material can be used over the entire range of wavelengths from 0.120 μm (vacuum ultraviolet) to 8.0 μm (infrared). High quality synthetic VUV grade MgF2 is quite expensive, in the region of $3/kg (2007) but the real cost of optics in this material is due to relatively low volume manufacture. However, with lithium fluoride it is one of the two materials that will transmit in the vacuum ultraviolet range at 121 nm (Lyman alpha) and this is where it finds its application. Lower grade MgF2 is sometimes used in the infrared but here it is inferior to calcium fluoride. MgF2 is tough and works and polishes well, but it is slightly birefringent and should be cut with the optic axis perpendicular to the plane of the window or lens.
Chronic exposure to magnesium fluoride may affect the skeleton, kidneys, central nervous system, respiratory system, eyes and skin, and may cause or aggravate attacks of asthma.
- Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, Florida: CRC Press, pp. 4–67; 1363, ISBN 0-8493-0594-2
- "Magnesium Fluoride Material Safety Data Sheet". Science Labs. May 21, 2013. Retrieved October 13, 2017.
- "Magnesium fluoride". CAS DataBase List. ChemicalBook. Retrieved October 13, 2017.
- Aigueperse, Jean; Mollard, Paul; Devilliers, Didier; Chemla, Marius; Faron, Robert; Romano, Renée; Cuer, Jean Pierre (2005), "Fluorine Compounds, Inorganic", Ullmann's Encyclopedia of Industrial Chemistry, Weinheim: Wiley-VCH, doi:10.1002/14356007.a11_307
- J. Chem. Soc., Faraday Trans., 1996, 92, 2753 - 2757. doi:10.1039/FT9969202753
- "Magnesium Fluoride Material Safety Data Sheet". ESPI Metals. August 2004. Retrieved October 13, 2017.[dead link]