Magnesium fluoride

Magnesium fluoride^[1]
Names
	Other names Sellaite; Irtran-1
Identifiers
CAS Number	7783-40-6 ;
3D model (JSmol)	Interactive image; Interactive image;
ChemSpider	22952 ;
ECHA InfoCard	100.029.086
EC Number	231-995-1;
PubChem CID	24546;
RTECS number	OM3325000;
UNII	5N014C7IWU ;
CompTox Dashboard (EPA)	DTXSID7052523 ;
	InChI InChI=1S/2FH.Mg/h21H;/q;;+2/p-2 Key: ORUIBWPALBXDOA-UHFFFAOYSA-L ; InChI=1/2FH.Mg/h21H;/q;;+2/p-2 Key: ORUIBWPALBXDOA-NUQVWONBAK;
	SMILES F[Mg]F; [Mg+2].[F-].[F-];
Properties
Chemical formula	MgF2
Molar mass	62.3018 g/mol
Appearance	Colorless to 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	Soluble in nitric acid; Slightly soluble in acetone; Insoluble in ethanol;
Magnetic susceptibility (χ)	−22.7⋅10−6 cm3/mol
Refractive index (nD)	1.37397
Structure
Crystal structure	Rutile (tetragonal), tP6
Space group	P42/mnm, No. 136
Thermochemistry
Heat capacity (C)	61.6 J/(mol⋅K)
Std molar; entropy (S⦵298)	57.2 J/(mol⋅K)
Std enthalpy of; formation (ΔfH⦵298)	−1124.2 kJ/mol
Gibbs free energy (ΔfG⦵)	−1071 kJ/mol
Hazards
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H303, H315, H319, H335
Precautionary statements	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	Magnesium chloride; Magnesium bromide; Magnesium iodide;
Other cations	Beryllium fluoride; Calcium fluoride; Strontium fluoride; Barium fluoride; Radium fluoride;
Related compounds	Hydrogen fluoride; Zinc fluoride; Aluminium fluoride;
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

Magnesium fluoride is an ionically bonded inorganic compound with the formula Mg F₂. The compound is a colorless to 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 ammonium bifluoride, by the breakdown of it:

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]

Coordination geometry in magnesium fluoride^[7]
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 3527306730.
^ 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

[hand-1] 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

[2] "Magnesium Fluoride Material Safety Data Sheet". Science Labs. May 21, 2013. Retrieved October 13, 2017.

[3] "Magnesium fluoride". CAS DataBase List. ChemicalBook. Retrieved October 13, 2017.

[Wells-4] Wells, A. F. (1984). Structural Inorganic Chemistry (5th ed.). Oxford University Press. pp. 413, 441. ISBN 978-0-19-965763-6.

[G&E-5] Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. pp. 117–119. ISBN 978-0-08-037941-8.

[Aigueperse-6] 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 3527306730.

[HLGKTL-7] 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.

[8] J. Chem. Soc., Faraday Trans., 1996, 92, 2753 - 2757. doi:10.1039/FT9969202753

[9] "Magnesium Fluoride Material Safety Data Sheet". ESPI Metals. August 2004. Archived from the original on 2017-10-28. Retrieved October 13, 2017.

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