Manganese(II) chlorate

Manganese(II) chlorate  Names

Systematic IUPAC name

Manganese(II) dichlorate[1]

Other names

* Manganese dichlorate

Identifiers

3D model (JSmol)

* Interactive image
* (hexahydrate): Interactive image

ChemSpider |

* (hexahydrate): 26667097

PubChem CID

* 24983783

InChI

* 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

SMILES

* [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

Chemical formula

| Mn(ClO3)2
Appearance  | Viscous pink liquid
Melting point |  −18 °C (0 °F; 255 K)
Boiling point |  6 °C (43 °F; 279 K) (decomposes)

Solubility in water

| Soluble
Hazards
GHS pictograms |
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).

Infobox references

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)" (in English). ChemSpider. http://www.chemspider.com/Chemical-Structure.26667097.html.
2. ↑ 2.0 2.1 2.2 Brown, F. E.; Woods, J. D. ( (1953). "Preparation and Some Properties of Manganese (II) Chlorate" (in English). Proceedings of the Iowa Academy of Science (UNI Scholar Works) 60 (34): 6. https://scholarworks.uni.edu/pias/vol60/iss1/34. 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 (in English). The Chemistry of Manganese, Technetium and Rhenium. Elsevier Science. pp. 226. ISBN 9781483187624.

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Manganese compounds

* MnO
* Mn3O4
* Mn5O8
* MnS
* MnS2
* MnSO4
* MnSe2
* MnSe
* MnTe
* Mn(NO3)2
* MnCO3
* MnCl2
* MnCl3
* MnCl4
* MnF2
* MnBr2
* MnI2
* MnTiO3
* MnMoO4
* Mn(CH3COO)2
* Mn2O3
* MnF3
* K6Mn2O6
* MnO2
* Mn(OH)2
* MnO3
* K3MnO4
* MnF4
* Na2MnO4
* K2MnO4
* Mn2O7
* NaMnO4
* KMnO4
* NH4MnO4
* AgMnO4
* Ca(MnO4)2
* Ba(MnO4)2
* MnH(CO)5
* Mn2(CO)10

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