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Contents

   



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1 Production  





2 Properties  





3 Uses  





4 Hazards  





5 References  














Magnesium chlorate






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Magnesium chlorate
Names
IUPAC name

Magnesium dichlorate hexahydrate

Systematic IUPAC name

Magnesium dichlorate

Other names
  • Magnesium(II) chlorate
Identifiers

CAS Number

  • (dihydrate): 36355-97-2
  • (hexahydrate): 7791-19-7
  • 3D model (JSmol)

  • (dihydrate): Interactive image
  • (hexahydrate): Interactive image
  • ChemSpider
  • (dihydrate): 80564724
  • (hexahydrate): 128878
  • ECHA InfoCard 100.030.634 Edit this at Wikidata
    EC Number
    • 233-711-1

    PubChem CID

  • (dihydrate): 71437298
  • (hexahydrate): 146100
  • UNII
    UN number 2723

    CompTox Dashboard (EPA)

  • (hexahydrate): DTXSID30999110
    • 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

    Chemical formula

    Mg(ClO3)2
    Molar mass 191.20 g/mol
    Appearance White crystalline solid
    Density 1.747 g/cm3 (hexahydrate)[1]
    Melting point 35 °C (95 °F; 308 K)[2]
    Boiling point 120 °C (248 °F; 393 K)[2] (decomposition)

    Solubility in water

    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)[2]
    Solubility in acetone Soluble
    Structure[1]

    Crystal structure

    Monoclinic

    Space group

    P21/c

    Lattice constant

    a = 6.39 Å, b = 6.51 Å, c = 13.90 Å

    α = 90°, β = 100.3°, γ = 90°

    Lattice volume (V)

    590.1 Å3
    Hazards
    GHS labelling:

    Pictograms

    GHS07: Exclamation mark

    Signal word

    Warning

    Hazard statements

    H302, H332
    Lethal dose or concentration (LD, LC):

    LD50 (median dose)

    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

    Magnesium chlorate refers to inorganic compounds with the chemical formula Mg(ClO3)2(H2O)x. The anhydrous (x = 0), dihydrate (x = 2), and hexahydrate (x = 6) are known. These are thermally labile white solids. The hexahydrate has been identified on the Martian surface.[3]

    Production[edit]

    Samples of magnesium chlorate were first claimed in 1920 as the result of treating magnesium oxide with chlorine. A more modern method involves electrolysis of magnesium chloride.[4] The magnesium chlorate can be purified by exploiting its solubility in acetone.[4]

    Properties[edit]

    The hexahydrate Mg(ClO3)2·6H2O 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]

    As confirmed by X-ray crystallography, the di- and hexahydrates feature octahedral Mg2+ centers. The other ligands are water, exclusively in the hexahydrate. In the dihydrate, chlorate is also coordinated and functions as a bridging ligand.[1]

    Uses[edit]

    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.[5]

    Hazards[edit]

    Magnesium chlorate is an oxidizer and can in principle form explosive mixtures.

    References[edit]

    1. ^ a b c Kossev, K; Tsvetanova, L.; Dimowa, L.; Nikolova, R.; Shivachev, B. (2013). "Synthesis and Crystal Structure of Magnesium Chlorate Dihydrate and Magnesium Chlorate Hexahydrate". Bulgarian Chemical Communications. 45: 543–548.
  • ^ a b c d Joseph William Mellor (1922). Supplement to Mellor's Comprehensive Treatise on Inorganic and Theoretical Chemistry: suppl. 3. K, Rb, Cs, Fr. Longmans, Green and Company.
  • ^ Ojha, Lujendra; Wilhelm, Mary Beth; Murchie, Scott L.; McEwen, Alfred S.; Wray, James J.; Hanley, Jennifer; Massé, Marion; Chojnacki, Matt (2015). "Spectral evidence for hydrated salts in recurring slope lineae on Mars". Nature Geoscience. 8 (11): 829–832. Bibcode:2015NatGe...8..829O. doi:10.1038/ngeo2546.
  • ^ a b Herbert Maxim (1948). The electrolytic production of magnesium chlorate and perchlorate. the Department of Chemical Engineering: University of Southern California.
  • ^ "MAGNESIUM CHLORATE". National Center for Advancing Translational Sciences. U.S. Department of Health & Human Services. Retrieved 27 August 2021.

  • Retrieved from "https://en.wikipedia.org/w/index.php?title=Magnesium_chlorate&oldid=1225986667"

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    Magnesium compounds
    Chlorates
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    This page was last edited on 27 May 2024, at 22:48 (UTC).

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