Magnesium oxide
 | |
 | |
| Names | |
|---|---|
| IUPAC name
Magnesium oxide | |
| Other names
Magnesia Periclase | |
| Properties | |
| MgO | |
| Molar mass | 40.304 g/mol[1] |
| Appearance | White powder |
| Odor | Odorless |
| Density | 3.6 g/cm3[1] |
| Melting point | 2,852 °C (5,166 °F; 3,125 K)[1] |
| Boiling point | 3,600 °C (6,510 °F; 3,870 K)[1] |
| Solubility | Soluble in acid, ammonia insoluble in alcohol |
| Band gap | 7.8 eV[2] |
| −10.2·10−6 cm3/mol[3] | |
| Thermal conductivity | 45–60 W·m−1·K−1[4] |
Refractive index (nD) |
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 ΔfH |
−601.6 ± 0.3 kJ·mol−1[5] |
| Standard molar entropy S |
26.95 ± 0.15 J·mol−1·K−1[5] |
| Specific heat capacity, C | 37.2 J/mol K[6] |
| Pharmacology | |
| A02AA02 (WHO) A06AD02 (WHO), A12CC10 (WHO) | |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards |
Metal fume fever, Irritant |
| NFPA 704 (fire diamond) | |
| 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)[7] |
| 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). | |
 verify (what is  ?) | |
| 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
[change | change source]- 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.
- ↑ 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
- 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.
- ↑ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 5.15. ISBN 1439855110.
- ↑ NIOSH Pocket Guide to Chemical Hazards. "#0374". National Institute for Occupational Safety and Health (NIOSH).