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Manganese(II) chlorate

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Manganese(II) chlorate
Names
Systematic IUPAC name
Manganese(II) dichlorate[1]
Other names
  • Manganese dichlorate
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/2ClHO3.Mn/c2*2-1(3)4;/h2*(H,2,3,4);/q;;+2/p-2
    Key: CRPBAQAXWCOQOC-UHFFFAOYSA-L
  • (hexahydrate): InChI=1S/2ClHO3.Mn.6H2O/c2*2-1(3)4;;;;;;;/h2*(H,2,3,4);;6*1H2/q;;+2;;;;;;/p-2
    Key: WIYJGRGEFGGGLP-UHFFFAOYSA-L
  • [O-]Cl(=O)=O.[O-]Cl(=O)=O.[Mn+2]
  • (hexahydrate): [O-]Cl(=O)=O.[O-]Cl(=O)=O.[Mn+2].O.O.O.O.O.O
Properties
Mn(ClO3)2
Appearance Viscous pink liquid
Melting point −18 °C (0 °F; 255 K)
Boiling point 6 °C (43 °F; 279 K) (decomposes)
Soluble
Hazards
GHS labelling:
GHS01: Explosive
Related compounds
Other anions
 Manganese(II) perchlorate
Other cations
 Copper(II) chlorate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Manganese(II) chlorate is an unstable chemical compound with the formula Mn(ClO3)2. It is unstable even in dilute solution. As a hexahydrate, it is solid below −18°C. Above this it melts, to form an extremely explosive pink liquid.[2]

Preparation

Manganese(II) chlorate was produced by the reaction of manganese(II) sulfate and barium chlorate.[3] The water was removed by boiling in vacuum. Then the temperature was lowered to -80°C which resulted in a pink solid. Then it was cleaned with liquid nitrogen and potassium hydroxide to remove the decomposition products.[2]

Properties

Manganese(II) chlorate forms the hexahydrate when solid, the water that cannot be removed. It decomposes above 6°C, to manganese(IV) oxide, chlorine dioxide, and water. In liquid form it is very viscous and extremely explosive. When heated to room temperature, it explodes with a sharp report.[2]

References

  1. ^ "Manganese(2+) chlorate hydrate (1:2:6)". ChemSpider. ChemSpider. Retrieved 23 August 2021.
  2. ^ a b c Brown, F. E.; Woods, J. D. ( (1953). "Preparation and Some Properties of Manganese (II) Chlorate". Proceedings of the Iowa Academy of Science. 60 (34). UNI Scholar Works: 6. Retrieved 23 August 2021.
  3. ^ R. D. W. Kemmitt; R. D. Peacock; J. C. Bailar; H. J. Emeléus; Ronald Nyholm (January 26, 2016). Nyholm, Nyholm (ed.). The Chemistry of Manganese, Technetium and Rhenium. Elsevier Science. p. 226. ISBN 9781483187624.
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