Magnesium oxide

Magnesium oxide
Names
	IUPAC name Magnesium oxide
	Other names Magnesia; Periclase
Properties
Chemical formula	MgO
Molar mass	40.304 g/mol
Appearance	White powder
Odor	Odorless
Density	3.6 g/cm3
Melting point	2,852 °C (5,166 °F; 3,125 K)
Boiling point	3,600 °C (6,510 °F; 3,870 K)
Solubility	Soluble in acid, ammonia ; insoluble in alcohol
Band gap	7.8 eV
Magnetic susceptibility (χ)	−10.2·10−6 cm3/mol
Thermal conductivity	45–60 W·m−1·K−1
Refractive index (nD)	1.7355
Dipole moment	6.2 ± 0.6 D
Structure
Crystal structure	Halite (cubic), cF8
Space group	Fm3m, No. 225
Lattice constant	a = 4.212Å ; ;
Coordination geometry	Octahedral (Mg2+); octahedral (O2−)
Thermochemistry
Std enthalpy of; formation ΔfHo298	−601.6 ± 0.3 kJ·mol−1
Standard molar; entropy So298	26.95 ± 0.15 J·mol−1·K−1
Specific heat capacity, C	37.2 J/mol K
Pharmacology
ATC code	A02AA02 (WHO) A06AD02 (WHO), A12CC10 (WHO)
Hazards
Main hazards	Metal fume fever, Irritant
	0 1 0
R-phrases	R36, R37, R38
Flash point	Non-flammable
U.S. Permissible; exposure limit (PEL)	TWA 15 mg/m3 (fume)
Related compounds
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Other cations	{{{value}}}
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	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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	Infobox references

Magnesium oxide, or magnesia, is a white solid mineral, made of one part magnesium and one part oxygen. Its chemical formula is MgO. Magnesium oxide is used by libraries to make books last longer. It is also used as an insulator for some electrical wires, and to help crucibles resist high temperatures. Magnesium oxide is also used to treat heartburn and upset stomachs.

References

↑ ^1.0 ^1.1 ^1.2 ^1.3 Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.74. ISBN 1439855110.
↑ Taurian, O.E.; Springborg, M.; Christensen, N.E. (1985). "Self-consistent electronic structures of MgO and SrO" (PDF). Solid State Communications. 55 (4): 351–5. Bibcode:1985SSCom..55..351T. doi:10.1016/0038-1098(85)90622-2. Archived from the original (PDF) on 2016-03-03. Retrieved 2014-03-31.
↑ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.133. ISBN 1439855110.
↑ Application of magnesium compounds to insulating heat-conductive fillers Archived 2013-12-30 at the Wayback Machine. konoshima.co.jp
↑ ^5.0 ^5.1 Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.2. ISBN 1439855110.
↑ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.15. ISBN 1439855110.

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[b92-1] 1.0 ^1.1 ^1.2 ^1.3 Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.74. ISBN 1439855110.

[2] Taurian, O.E.; Springborg, M.; Christensen, N.E. (1985). "Self-consistent electronic structures of MgO and SrO" (PDF). Solid State Communications. 55 (4): 351–5. Bibcode:1985SSCom..55..351T. doi:10.1016/0038-1098(85)90622-2. Archived from the original (PDF) on 2016-03-03. Retrieved 2014-03-31.

[3] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.133. ISBN 1439855110.

[4] Application of magnesium compounds to insulating heat-conductive fillers Archived 2013-12-30 at the Wayback Machine. konoshima.co.jp

[b92b-5] 5.0 ^5.1 Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.2. ISBN 1439855110.

[b92c-6] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.15. ISBN 1439855110.

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