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Manganese(II) molybdate
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Manganese(II) molybdate
Manganese(II) molybdate
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Manganese(II) molybdate
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Manganese(II) molybdate
Manganese(II) molybdate
Names
IUPAC name
Manganese(2+) molybdate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.034.371 Edit this at Wikidata
EC Number
  • 237-823-1
  • InChI=1S/Mn.Mo.4O/q+2;;;;2*-1
    Key: QYZFLCQIQOHNTP-UHFFFAOYSA-N
  • [O-][Mo](=O)(=O)[O-].[Mn+2]
Properties
MnMoO4
Molar mass 214.876 g/mol (anhydrous)
232.901 g/mol (monohydrate)
Appearance white-yellow to beige crystals or powder [1]
Density 4.02 g/cm3
Melting point 1,130 °C (2,070 °F; 1,400 K)
insoluble
2.11
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
3
0
0
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Manganese(II) molybdate is an inorganic compound with the chemical formula MnMoO4. α-MnMoO4 has a monoclinic crystal structure.[2] It is also antiferromagnetic at low temperatures.[3]

Synthesis

[edit]

Manganese(II) molybdate can be prepared through a double displacement reaction between sodium molybdate and manganese sulphate:[1]

Na2MoO4 + MnSO4 → Na2SO4 + MnMoO4

Manganese(II) molybdate has minimal solubility in water and will form a white-yellow precipitate which turns beige upon being refluxed.[1] The precipitate can then be filtered from solution, which gives the monohydrate (MnMoO4·H2O); heating to 360 °C then provides the anhydrous salt.[1]

Manganese(II) molybdate may also be prepared by heating various manganese oxides and molybdenum trioxide to 700 °C.[4]

Potential applications

[edit]

MnMoO4 serves as the active material in electrodes for aqueous supercapacitors[2][5] due to fast pseudocapacitive redox reactions. It has been evaluated as catalyst for hydrogen evolution.[5]

References

[edit]
  1. ^ a b c d Clearfield, A.; Moini, A.; Rudolf, P. R. (1985-12-01). "Preparation and Structure of Manganese Molybdates". Inorganic Chemistry. 24 (26): 4606–4609. doi:10.1021/ic00220a035.
  2. ^ a b "Synthesis and Characterization of Manganese Molybdate for Symmetric Capacitor Applications (PDF Download Available)". ResearchGate. Retrieved 2017-03-10.
  3. ^ Ehrenberg, H.; Schwarz, B.; Weitzel, H. (2006-10-01). "Magnetic phase diagrams of -MnMoO4". Journal of Magnetism and Magnetic Materials. 305 (1): 57–62. doi:10.1016/j.jmmm.2005.11.027.
  4. ^ Doyle, W. P.; McGuire, G.; Clark, G. M. (1996-05-01). "Preparation and Properties of Transition Metal Molybates (VI)". Inorganic and Nuclear Chemistry. 28 (5): 1185–1190. doi:10.1016/0022-1902(66)80444-X.
  5. ^ a b Yan, Xiaodong; Tian, Lihong; Murowchick, James; Chen, Xiaobo (2016-03-01). "Partially amorphized MnMoO4for highly efficient energy storage and the hydrogen evolution reaction". J. Mater. Chem. A. 4 (10): 3683–3688. doi:10.1039/c6ta00744a. ISSN 2050-7496.


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