Magnesium oxide

Magnesium oxide
Names
IUPAC name
Magnesium oxide
Other names
Magnesia
Periclase
Properties
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
−10.2·10−6 cm3/mol
Thermal conductivity 45–60 W·m−1·K−1
1.7355
6.2 ± 0.6 D
Structure
Halite (cubic), cF8
Fm3m, No. 225
a = 4.212Å



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
A02AA02 (WHO) A06AD02 (WHO), A12CC10 (WHO)
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Metal fume fever, Irritant
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
1
0
0
Flash point Non-flammable
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 15 mg/m3 (fume)
REL (Recommended)
 None designated
IDLH (Immediate danger)
 750 mg/m3 (fume)
Safety data sheet (SDS) ICSC 0504
Related compounds
Other anions
 Magnesium sulfide
Other cations
 Beryllium oxide
Calcium oxide
Strontium oxide
Barium oxide
Related compounds
 Magnesium hydroxide
Magnesium nitride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
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 made to treat heartburn and upset stomachs.[verification needed]

References

  1. 1 2 3 4 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
  5. 1 2 Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.2. ISBN 1439855110.
  6. ↑ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.15. ISBN 1439855110.
  7. ↑ NIOSH Pocket Guide to Chemical Hazards. "#0374". National Institute for Occupational Safety and Health (NIOSH).