Magnesium chlorate

Magnesium chlorate is an inorganic chemical consisting of a magnesium cation and two chlorate anions: its chemical formula is Mg(ClO3)2.

Magnesium chlorate
Names
Systematic IUPAC name
Magnesium dichlorate
Other names
  • Magnesium(II) chlorate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.634
EC Number
  • 233-711-1
UNII
UN number 2723
  • InChI=1S/2ClHO3.Mg/c2*2-1(3)4;/h2*(H,2,3,4);/q;;+2/p-2
    Key: NNNSKJSUQWKSAM-UHFFFAOYSA-L
  • (dihydrate): InChI=1S/2ClHO3.Mg.2H2O/c2*2-1(3)4;;;/h2*(H,2,3,4);;2*1H2/q;;+2;;/p-2
    Key: YTXOASNCVSJHNM-UHFFFAOYSA-L
  • (hexahydrate): InChI=1S/2ClHO3.Mg.6H2O/c2*2-1(3)4;;;;;;;/h2*(H,2,3,4);;6*1H2/q;;+2;;;;;;/p-2
    Key: XKPLAISKKLSAQQ-UHFFFAOYSA-L
  • Cl(=O)(=O)[O-].Cl(=O)(=O)[O-].[Mg+2]
  • (dihydrate): O.O.[Mg+2].[O-]Cl(=O)=O.[O-]Cl(=O)=O
  • (hexahydrate): O.O.O.O.O.O.[O-]Cl(=O)=O.[O-]Cl(=O)=O.[Mg+2]
Properties
Mg(ClO3)2
Molar mass 191.20 g/mol
Appearance White crystalline solid
Density 1.80 g/cm3[1]
Melting point 35 °C (95 °F; 308 K)[2]
Boiling point 120 °C (248 °F; 393 K)[2] (decomposition)
114 g/100 ml (0 °C)
123 g/100 ml (10 °C)
135 g/100 ml (20 °C)
155 g/100 ml (30 °C)
178 g/100 ml (50 °C)
242 g/100 ml (60 °C)
268 g/100 ml (100 °C)[1]
Solubility in acetone Soluble
Hazards
GHS labelling:
GHS07: Exclamation mark
Warning
H302, H332
Lethal dose or concentration (LD, LC):
6348 mg/kg (rat, oral)
Related compounds
Other cations
 Calcium chlorate
Strontium chlorate
Barium chlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Production

Magnesium chlorate was first produced in 1920 by reacting magnesium oxide with chlorine gas to produce a mixture of magnesium chloride and magnesium chlorate. They were not able to separate the magnesium chlorate from the magnesium chloride. Other production methods were reported such as reacting chlorine gas with magnesium hydroxide or magnesium carbonate to create magnesium hypochlorite then converting the hypochlorite to the chlorate. But, not a lot of studies have been done on the properties of magnesium chlorate. The most modern method is converting magnesium chloride electrochemically:[3]

MgCl2 + 6 H2O + e− → Mg(ClO3)2 + 6 H2

After, the magnesium chlorate was separated from the magnesium chloride by using the solubility of magnesium chlorate in acetone.[3]

Properties

Magnesium chlorate forms a hexahydrate Mg(ClO3)2·6H2O which decomposes to the tetrahydrate at 35 °C. At 65 °C, it dehydrates to the dihydrate, then at 80 °C forms a basic salt. If further heated to 120 °C it decomposes to water, oxygen, chlorine, and magnesium oxide.[2]

Hazards

Magnesium chlorate forms explosive mixtures with glucose, charcoal, shellac, sulfur, starch, and other organic substances, sulfuric acid, and other acidic substances, potassium cyanide, phosphorus, antimony trisulfide, and some other compounds. This can be prevented by mixing a small amount of sodium carbonate to prevent exploding when near organic substances.[3]

Uses

Magnesium(II) chlorate is used as a powerful desiccant and a defoliant for cotton, potato, and rice. It is also found as a lubricant in eye drops as an inactive ingredient.[4]

Natural occurrence

The hydrated version of this compound has been spotted on Martian surfaces such as the Hale crater by the Mars Reconnaissance Orbiter, which suggests that the compound absorbs water from the Martian surface by the moisture present on the surface to form a very concentrated solution. When these solutions form, the solution can stay liquid down to –70 °C.[5]

References
  1. R. C. Ropp (2012). Encyclopedia of the Alkaline Earth Compounds. Elsevier Science. ISBN 9780444595539.
  2. Joseph William Mellor (1922). Supplement to Mellor's Comprehensive Treatise on Inorganic and Theoretical Chemistry: suppl. 3. K, Rb, Cs, Fr. University of Illinois at Urbana-Champaign: Longmans, Green and Company.
  3. Herbert Maxim (1948). The electrolytic production of magnesium chlorate and perchlorate. the Department of Chemical Engineering: University of Southern California.
  4. "MAGNESIUM CHLORATE". National Center for Advancing Translational Sciences. U.S. Department of Health & Human Services. Retrieved 27 August 2021.
  5. Denis Delbecq (2015). "De l'eau liquide répérée sur les pentes martiennes". LE TEMPS (in French). NASA. Retrieved 24 September 2021.
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