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Manganese(II) perchlorate
Names
Other names
  • Manganous perchlorate
  • Manganese diperchlorate
Identifiers
3D model (JSmol)
ChemSpider
EC Number
  • 237-390-9
  • InChI=1S/2ClHO4.Mn/c2*2-1(3,4)5;/h2*(H,2,3,4,5);/q;;+2/p-2
  • [O-]Cl(=O)(=O)=O.[O-]Cl(=O)(=O)=O.[Mn+2]
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)
227 g/100 mL (25 °C)[1]
Hazards
GHS labelling:
GHS03: Oxidizing
Danger
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
1
0
2
OX
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]

  1. ^ Nevil Vincent Sidgwick (1963). The Chemical Elements and Their Compounds (PDF). Oxford: Clarendon Press. p. 835. Retrieved 9 April 2024.
  2. ^ 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.
  3. ^ 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 - Mécanique-physique, Chimie, Sciences de l'univers, Sciences de la Terre (in French). 298 (14): 579–582. Retrieved 9 April 2024.
  4. ^ 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.
  5. ^ 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.
source: https://en.wikipedia.org/wiki/Manganese(II)_perchlorate

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