Manganese(II) perchlorate
| Names | |
|---|---|
Other names
| |
| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| EC Number |
|
PubChem CID
|
|
| |
| |
| Properties | |
| Mn(ClO4)2 | |
| Molar mass | 253.84 g/mol |
| Appearance | White solid (anhydrous) Rose-colored solid (hexahydrate) |
| Density | 2.10 g/cm3 |
| Melting point | 150 °C (302 °F; 423 K)[2] (decomposes, hexahydrate) |
| 292 g/100 mL (25 °C)[1] | |
| Hazards | |
| GHS labelling: | |
| |
| Danger | |
| NFPA 704 (fire diamond) | |
| Related compounds | |
Other cations
|
Iron(II) perchlorate Cobalt(II) perchlorate Nickel(II) perchlorate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Manganese(II) perchlorate is an inorganic chemical compound with the formula Mn(ClO4)2. It forms a white-colored anhydrous and a rose-colored hexahydrate, both of which are hygroscopic. As a perchlorate, it is a strong oxidizing agent.[3]
Production and reactions
[edit]The hexahydrate can be produced by reacting manganese metal or manganese(II) carbonate with perchloric acid, followed by the evaporation of the solution. The hexahydrate does not dehydrate when heating but instead oxidizes to manganese dioxide at 150 °C.[4][2]
To produce the anhydrous form, manganese(II) nitrate is reacted with dichlorine hexoxide at 5 °C:[3]
- Mn(NO3)2 + 4 Cl2O6 → NO2Mn(ClO4)3 + NO2ClO4 + 4 ClO2 + O2
The resulting nitryl salt is subsequently heated at 105 °C in a vacuum to produce the anhydrous perchlorate.[3]
- NO2Mn(ClO4)3 → Mn(ClO4)2 + NO2ClO4
Structure
[edit]The anhydrous form is predicted to be isostructural with cobalt(II) perchlorate, based on the IR spectrum and the Raman spectrum of the compound.[3]
The hexahydrate consists of discreet [Mn(H2O)6]2+ octahedrons and perchlorate anions with lattice constants a = 7.85 Å, b = 13.60 Å and c = 5.30 Å. The hexahydrate undergoes phase transitions at low temperatures.[4][5]
References
[edit]- ^ Nevil Vincent Sidgwick (1963). The Chemical Elements and Their Compounds. Oxford: Clarendon Press. p. 1285. Retrieved 1 June 2024.
- ^ a b Kemmitt, R. D. W.; Peacock, R. D. (1973). The Chemistry of Manganese, Technetium and Rhenium. Pergamon Texts in Inorganic Chemistry. Saint Louis: Elsevier Science. p. 778. ISBN 978-1-4831-3806-0. OCLC 961064866.
- ^ a b c d J.L. Pascal; J. Potier; C.S. Zhang (1984). "Réaction du trioxyde de chlore avec le chlorure et le nitrate de manganèse (II). Synthèse du diperchloratomanganèse(II) : Mn(ClO4)2 et du triperchloratomanganate (II) de nitryle : NO2Mn(ClO4)3". Comptes Rendus de l'Académie des Sciences, Série 2 (in French). 298 (14): 579–582. Retrieved 9 April 2024.
- ^ a b M.B. Patel; Sushama Patel; D.P. Khandelwal; H.D. Bist (1983). "Vibrational studies and phase transitions in Co(ClO4)2·6H2O and Mn(ClO4)2·6H2O". Chemical Physics Letters. 101 (1): 93–99. doi:10.1016/0009-2614(83)80311-X.
- ^ B.K. Chaudhuri (1975). "A new type of phase transition in M(ClO4)2(H2O)6 M = Fe, Co, Ni and Mn". Solid State Communications. 16 (5): 767–772. doi:10.1016/0038-1098(75)90071-X.