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Manganese(II) chlorate

From Wikipedia, the free encyclopedia
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).
Chemical compound

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

[edit ]

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

[edit ]

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

[edit ]
  1. ^ "Manganese(2+) chlorate hydrate (1:2:6)". 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.
Salts and covalent derivatives of the chlorate ion
HClO3 He
LiClO3 Be B C NH4ClO3 O F Ne
NaClO3 Mg(ClO3)2 Al(ClO3)3 Si P S Cl Ar
KClO3 Ca(ClO3)2 Sc Ti V Cr Mn(ClO3)2 Fe(ClO3)3 Co(ClO3)2 Ni(ClO3)2 Cu(ClO3)2 Zn(ClO3)2 Ga(ClO3)3 Ge As Se Br Kr
RbClO3 Sr(ClO3)2 Y(ClO3)3 Zr Nb Mo Tc Ru Rh Pd AgClO3 Cd(ClO3)2 In Sn Sb Te I Xe
CsClO3 Ba(ClO3)2 * Lu Hf Ta W Re Os Ir Pt AuClO3 Hg(ClO3)2 Tl Pb(ClO3)2 Bi Po At Rn
Fr Ra(ClO3)2 ** Lr Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
 
* La(ClO3)2 Ce Pr(ClO3)2 Nd Pm Sm Eu Gd Tb Dy Ho Er(ClO3)2 Tm Yb
** Ac Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No

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