Barium manganate

Barium manganate
Identifiers
3D model (JSmol)
ECHA InfoCard 100.029.190 Edit this at Wikidata
EC Number
  • 232-109-6
UNII
  • InChI=1S/Ba.Mn.4O/q+2;;;;2*-1
    Key: ZZCNKSMCIZCVDR-UHFFFAOYSA-N
  • [O-][Mn](=O)(=O)[O-].[Ba+2]
Properties
BaMnO4
Molar mass 256.26 g/mol
Appearance light blue to dark blue and black powder
Density 4.85 g/cm3
insoluble[1]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 GHS03, GHS07: oxidizing, skin and eye irritant
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Barium manganate is an inorganic compound with the formula BaMnO4. It is used as an oxidant in organic chemistry.[2] It belongs to a class of compounds known as manganates in which the manganese resides in a +6 oxidation state. Manganate should not be confused with permanganate which contains manganese(VII). Barium manganate is a powerful oxidant, popular in organic synthesis and can be used in a wide variety of oxidation reactions.

Properties

The manganate(VI) ion is a d1 ion and is tetrahedral with bond angles of approximately 109.5°. The Mn−O bond lengths in BaMnO4 and K2MnO4 are identical at 1.66 Å. In comparison, the Mn-O bond length in MnO2−4 is longer than in MnO4− of 1.56 Å and shorter than the Mn−O bond found in MnO2, 1.89 Å.[3][4] Barium manganate is isomorphous with BaCrO4 and BaSO4. Barium manganate can appear as a dark blue or green to black crystals.[5] Barium manganate is indefinitely stable, active and can be stored for months in dry conditions.[5]

Preparation

Barium manganate can be prepared from potassium manganate and barium chloride by salt metathesis to give insoluble barium manganate:[6]

BaCl2 + K2MnO4 → 2 KCl + BaMnO4↓

Applications

Barium manganate oxidizes a number of functional groups efficiently and selectively: alcohols to carbonyls, diols to lactones, thiols to disulfides, aromatic amines to azo-compounds, hydroquinone to p-benzoquinone, benzylamine to benzaldehyde, hydrazones to diazo compounds, etc.[7] It does not oxidize saturated hydrocarbons, alkenes, unsaturated ketones, and tertiary amines. Barium manganate is a common substitute for MnO2. It is easier to prepare, reacts more efficiently, and the substrate:oxidant ratios are closer to theory.

Another use for barium manganate was as a reagent in the synthesis of the inorganic pigment manganese blue, which is no longer produced on an industrial scale.

References

  1. ^ Olsen, J. C. (1900). Permanganic Acid by Electrolysys. Easton, PA: The Chemical Publishing Company.
  2. ^ Garry Procter, Steven V. Ley, Grant H. Castle, "Barium Manganate" Encyclopedia of Reagents for Organic Synthesis 2001. doi:10.1002/047084289X.rb003
  3. ^ Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford:Pergamon Press. Vol. 15, "Manganese Compounds". ISBN 0-08-022057-6.
  4. ^ Jellinek, F. J. Inorg. Nucl. Chem. 1960. 13, 329-331. {{doi: 10.1016/0022-1902(60)80316-8}}
  5. ^ a b Firouzabadi, H.; Mostafavipoor,Z. (1983), "Barium Manganate. A Versatile Oxidant in Organic Synthesis", Bull. Chem. Soc. Jpn. 56 (3): p914-917. {{doi: 10.1246/bcsj.56.914}}.
  6. ^ Carrington, A.; Symons, M. C. R. "Structure and reactivity of the oxy-anions of transition metals. Part I. The managese oxy-anions", J. Chem. Soc. 1956, p3373-3380. doi:10.1039/JR9560003373.
  7. ^ Procter.G.; Ley, S. V.; Castle, G.H. (2004), "Barium Manganate", in Paquette,L., Encyclopedia of Reagents for Organic Synthesis, New York:Wiley, {{doi:10.1002/047084289X}}.