Magnesium fluoride
Chemical compound of magnesium and fluorine
 | |
| Names | |
|---|---|
| Other names Sellaite Irtran-1 | |
| Identifiers | |
CAS Number |
|
3D model (JSmol) |
|
| ChemSpider |
|
| ECHA InfoCard | 100.029.086  |
| EC Number |
|
PubChem CID |
|
| RTECS number |
|
| UNII |
|
CompTox Dashboard (EPA) |
|
InChI
| |
| |
| Properties | |
Chemical formula | MgF2 |
| Molar mass | 62.3018 g/mol |
| Appearance | White tetragonal crystals |
| Density | 3.148 g/cm3 |
| Melting point | 1,263 °C (2,305 °F; 1,536 K) |
| Boiling point | 2,260 °C (4,100 °F; 2,530 K) |
Solubility in water | 0.013 g/(100 mL) |
Solubility product (Ksp) | 5.16⋅10−11 |
| Solubility | |
| −22.7⋅10−6 cm3/mol | |
Refractive index (nD) | 1.37397 |
| Structure | |
| Rutile (tetragonal), tP6 | |
| P42/mnm, No. 136 | |
| Thermochemistry | |
Heat capacity (C) | 61.6 J⋅mol−1⋅K−1 |
Std molar entropy (S⦵298) | 57.2 J⋅mol−1⋅K−1 |
Std enthalpy of formation (ΔfH⦵298) | −1124.2 kJ⋅mol−1 |
Gibbs free energy (ΔfG⦵) | −1071 kJ/mol |
| Hazards[2][3] | |
| GHS labelling: | |
 | |
| Warning | |
| H303, H315, H319, H335 | |
| P261, P304+P340, P305+P351+P338, P405 | |
| NFPA 704 (fire diamond) |  3 0 0 |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) | 2330[clarification needed] (rat, oral) |
| Safety data sheet (SDS) | ChemicalBook |
| Related compounds | |
Other anions | |
Other cations | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).  Y verify (what is  Y N ?) Infobox references | |
Chemical compound
Magnesium fluoride is an ionically bonded 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
Magnesium fluoride is prepared from magnesium oxide with sources of hydrogen fluoride such as can be obtained from the breakdown of ammonium bifluoride:
- MgO + [NH4]HF2 → MgF2 + NH3 + H2O
Related metathesis reactions are also feasible:
- Mg(OH)2 + CuF2 → MgF2 + Cu(OH)2
Structure
The compound crystallizes as tetragonal birefringent crystals. The structure of the magnesium fluoride is similar to that of rutile,[4][5] featuring octahedral Mg2+ cations and 3-coordinate F− anions.[6]
| Magnesium coordination | Fluorine coordination |
|---|---|
 |  |
In the gas phase, monomeric MgF2 molecules adopt a linear molecular geometry.[4][5]
Uses
Optics
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 magnesium fluoride is one of two materials (the other being lithium fluoride) that will transmit in the vacuum ultraviolet range at 121 nm (Lyman alpha). Lower-grade magnesium fluoride is inferior to calcium fluoride in the infrared range.[citation needed]
Magnesium fluoride is tough and polishes well but is slightly birefringent and should therefore be cut with the optic axis perpendicular to the plane of the window or lens.[6] Due to its suitable refractive index of 1.37, magnesium fluoride is commonly applied in thin layers to the surfaces of optical elements as an inexpensive anti-reflective coating.[citation needed] Its Verdet constant is 0.00810 arcmin⋅G−1⋅cm−1 at 632.8 nm.[8]
Safety
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.[9]
References
- ^ W.M. Haynes, ed. (2016), "Physical Constants of Inorganic Compounds", Handbook of Chemistry and Physics (97th ed.), CRC Press, pp. 4–71 (789), ISBN 978-1-4987-5429-3
- ^ "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.
- ^ a b Wells, A. F. (1984). Structural Inorganic Chemistry (5th ed.). Oxford University Press. pp. 413, 441. ISBN 978-0-19-965763-6.
- ^ a b Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 117–119. ISBN 978-0-08-037941-8.
- ^ a b Aigueperse, Jean; Mollard, Paul; Devilliers, Didier; Chemla, Marius; Faron, Robert; Romano, René; Cuer, Jean Pierre (2000). "Fluorine Compounds, Inorganic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a11_307. ISBN 978-3527306732.
- ^ Haines, J.; Léger, J. M.; Gorelli, F.; Klug, D. D.; Tse, J. S.; Li, Z. Q. (2001). "X-ray diffraction and theoretical studies of the high-pressure structures and phase transitions in magnesium fluoride". Phys. Rev. B. 64 (13): 134110. Bibcode:2001PhRvB..64m4110H. doi:10.1103/PhysRevB.64.134110.
- ^ J. Chem. Soc., Faraday Trans., 1996, 92, 2753 - 2757. doi:10.1039/FT9969202753
- ^ "Magnesium Fluoride Material Safety Data Sheet". ESPI Metals. August 2004. Archived from the original on 2017-10-28. Retrieved October 13, 2017.
External links
- A java applet showing the effect of MgF2 on a lens
- Infrared windows at Lawrence Berkeley National Laboratory
- National Pollutant Inventory - Fluoride and compounds fact sheet
- Crystran Data Crystran MSDS[permanent dead link]
- v
- t
- e
