|Color||Colorless, white, pale yellow, pale brown, faintly pink, lilac-rose|
|Crystal habit||Usually massive, rarely as rhombohedrons or hexagonal prisms|
|Crystal system||Trigonal - Hexagonal Scalenohedral H-M Symbol 32/m Space Group: R3c|
|Mohs scale hardness||3.5 - 4.5|
|Diaphaneity||Transparent to translucent|
|Specific gravity||3.0 - 3.2|
|Optical properties||Uniaxial (-)|
|Refractive index||nω=1.508 - 1.510 nε=1.700|
|Solubility||Effervesces in hot HCl|
|Other characteristics||May exhibit pale green to pale blue fluorescence and phosphorescence under UV; triboluminescent|
Magnesite is a mineral with the chemical formula MgCO3 (magnesium carbonate). Mixed crystals of iron II carbonate and magnesite (mixed crystals known as ankerite) possess a layered structure: monolayers of carbonate groups alternate with magnesium monolayers as well as iron II carbonate monolayers.  Manganese, cobalt and nickel may also occur in small amounts.
Magnesite occurs as veins in and an alteration product of ultramafic rocks, serpentinite and other magnesium rich rock types in both contact and regional metamorphic terrains. These magnesites often are cryptocrystalline and contain silica in the form of opal or chert.
Magnesite is also present within the regolith above ultramafic rocks as a secondary carbonate within soil and subsoil, where it is deposited as a consequence of dissolution of magnesium-bearing minerals by carbon dioxide within groundwaters.
Magnesite can be formed via talc carbonate metasomatism of peridotite and other ultrabasic rocks. Magnesite is formed via carbonation of olivine in the presence of water and carbon dioxide at elevated temperatures and high pressures typical of the greenschist facies.
- 2 Mg3 Si2O5(OH)4 + 3 CO2 → Mg3Si4O10(OH)2 + 3 MgCO3 + H2O.
However when performing this reaction in the laboratory, the trihydrated form of magnesium carbonate (nesquehonite) will form at room temperature.  This very observation led to the postulation of a "dehydration barrier" being involved in the low-temperature formation of anhydrous magnesium carbonate. Laboratory experiments with formamide, a liquid resembling water, have shown how no such dehydration barrier can be involved. The fundamental difficulty to nucleate anhydrous magnesium carbonate remains when using this non-aqueous solution. Not cation dehydration, but rather the spatial configuration of carbonate anions creates the barrier in the low-temperature nucleation of magnesite. 
Magnesite was detected in meteorite ALH84001 and on planet Mars itself. Magnesite was identified on Mars using infra-red spectroscopy from satellite orbit. Controversy still exists over the temperature of formation of this magnesite. Low-temperature formation has been suggested for the magnesite from the Mars derived ALH84001 meteorite. The low-temperature formation of magnesite might well be of significance toward large-scale carbon sequestration.
Similar to the production of lime, magnesite can be burned in the presence of charcoal to produce MgO, which in the form of a mineral is known as periclase. Large quantities of magnesite are burnt to make magnesium oxide: an important refractory material used as a lining in blast furnaces, kilns and incinerators.
Magnesite can also be used as a binder in flooring material. Furthermore it is being used as a catalyst and filler in the production of synthetic rubber and in the preparation of magnesium chemicals and fertilizers.
In fire assay, magnesite cupels can be used for cupellation as the magnesite cupel will resist the high temperatures involved.
At times magnesite is dyed to make beads used as ornaments.
- http://rruff.geo.arizona.edu/doclib/hom/magnesite.pdf Handbook of Mineralogy
- http://www.mindat.org/min-2482.html Mindat.org
- http://webmineral.com/data/Magnesite.shtml Webmineral data
- Klein, Cornelis and Cornelius S. Hurlbut, Jr., Manual of Mineralogy, Wiley, 20th ed., p. 332 ISBN 0-471-80580-7
- Beran, A. and Zemann, J. (1977): Refinement and comparison of the crystal structures of dolomite and of an Fe-rich ankerite. Tschermaks Mineralogische und Petrographische Mitteilungen, vol.24, pp.279-286.
- Leitmeier, H.(1916): Einige Bemerkungen über die Entstehung von Magnesit und Sideritlagerstätten, Mitteilungen der Geologischen Gesellschaft in Wien, vol.9, pp. 159–166.
- Lippmann, F. (1973): Sedimentary carbonate minerals. Springer Verlag, Berlin, 228 p.
- Xu, J; Yan, C.; Zhang, F.; Konishi, H., Xu, H. & Teng, H. H. (2013): Testing the cation-hydration effect on the crystallization of Ca - Mg- CO3 systems. Proc. Natl. Acad. Sci. US, vol.110 (44), pp.17750-17755.
- Deelman, J.C. (1999): "Low-temperature nucleation of magnesite and dolomite", Neues Jahrbuch für Mineralogie, Monatshefte, pp. 289–302.
- Alves dos Anjos et al. (2011): Synthesis of magnesite at low temperature. Carbonates and Evaporites, vol.26, pp.213-215.
- Ehlmann, B. L. et al. (2008): Orbital identification of carbonate-bearing rocks on Mars. Science, vol.322, no.5909, pp.1828-1832.
- McSween Jr, H. Y and Harvey, R. P.(1998): An evaporation model for formation of carbonates in the ALH84001 Martian meteorite. International Geology Review, vol.49, pp.774-783.
- Warren, P. H. (1998): Petrologic evidence for low-temperature, possibly flood evaporitic origin of carbonates in the ALH84001 meteorite. Journal of Geophysical Research, vol.103, no.E7, 16759-16773.
- Oelkers, E. H.; Gislason, S. R. and Matter, J. (2008): Mineral carbonation of CO2. Elements, vol.4, pp.333-337.
- Smithsonian Rock and Gem ISBN 0-7566-0962-3