Birnessite Explained

Birnessite
Category:Oxide mineral
Formula:MnO2·nH2O
δ-
Imasymbol:Bir[1]
System:Triclinic or Hexagonal
Color:Dark brown to black
Habit:Extremely finely crystalline
Cleavage:[001] perfect
Mohs:1.5
Luster:Sub-metallic, dull
Refractive:nω = 1.730 nε = 1.690
Opticalprop:Uniaxial (−)
Birefringence:δ = 0.040
Gravity:3.0
Diaphaneity:Nearly opaque
Other:Identification by optical properties is impossible.
References:[2] [3] [4]

Birnessite (nominally MnO2·nH2O), also known as δ-, is a hydrous manganese dioxide mineral with a chemical formula of Na0.7Ca0.3Mn7O14·2.8H2O.[5] It is the main manganese mineral species at the Earth's surface, and commonly occurs as fine-grained, poorly crystallized aggregates in soils, sediments, grain and rock coatings (e.g., desert varnish), and marine ferromanganese nodules and crusts.[6] [7] [8] [9] [10] [11] [12] It was discovered at Birness, Aberdeenshire, Scotland.

Formation

Its precipitation from the oxidation of Mn(II) in oxygenated aqueous solutions is kinetically hindered and slow on mineral surfaces. Biological Mn(II) oxidation is generally fast relative to abiotic Mn(II) oxidation processes, and for this reason the majority of natural birnessites is believed to be produced by microorganisms, especially bacteria, but also fungi.[13]

Composition and structure

Birnessite is a non-stoichiometric compound, in which variable amounts of Mn4+ ions in the nominal MnO2·nH2O formula either are missing, or are replaced primarily by Mn3+ ions and secondarily by Mn2+ ions. Because a solid is overall electrically neutral, birnessite contains foreign cations to balance the net negative charge created by Mn4+ vacancies and heterovalent Mn substitutions.

Two crystallographic structures are known, triclinic birnessite (TcBi)[14] and hexagonal birnessite (HBi).[15] [16] [17] The two of them consist of layers of edge-sharing MnO6 octahedra separated by one or two layers of water molecules. The one-water layer compounds have a characteristic ~7 Å repeat in the layer stacking direction, and addition of a second water layer expands the layer spacing to ~10 Å. The 10 Å form is named buserite.

The layer composition of TcBi is typically Mn4+0.69Mn3+0.31. The Mn3+O6 and Mn4+O6 octahedra are fully ordered in raws in the MnO2 layers, such that every Mn3+-rich row alternates with two Mn4+-rich rows.10,11 The layer charge is offset by alkaline and alkali-earth cations (e.g., Na, K, Ca, Ba) into the interlayer region along with water molecules, and therefore TcBi has a cation-exchange capacity. A typical chemical formula of Na-exchanged TcBi is Na0.31(Mn4+0.69 Mn3+0.31)O2·0.4H2O.

The layer structure of HBi differs from that of TcBi by the presence of octahedral Mn4+ vacancies (Vac). The chemical formula of synthetic HBi depends on pH. The generic formula is H+x Mn3+y Mn2+z (Mn4+u Mn3+vVacw)O2, with x + 3y + 2z = v + 4w for neutrality.

The MnO2 layers are stacked periodically in synthetic triclinic and hexagonal birnessite crystals. It is, however, rarely the case in natural materials. In addition to being chemically complex, natural birnessite crystals are structurally disordered with respect to the layer stacking and the flatness of the layers.[18] A natural birnessite crystal may contain only a few layers, and they are often bent and always imperfectly stacked with orientational and translational loss of registry. The stacking disorder is referred to as "turbostratic" when the layers are oriented completely at random. Natural birnessite with turbostratically stacked layers is named vernadite,[19] [20] [21] and the synthetic analog is named δ-MnO2. The layer spacing of vernadite can be also ~7 Å or ~10 Å, and interstratification of the two types of layers has been observed on quartz coatings and in ferromanganese crusts.[22]

Surface reactivity

The +4 charge deficit of a vacancy can be balanced by a large variety of interlayer cations forming inner-sphere complexes above and below the vacancies (e.g., Ca, Cu, Zn, Pb, Cd, Tl).[23] [24] [25] [26] [27] [28] [29] [30] The relative stability of the interlayer cations has been evaluated experimentally[31] [32] and theoretically by surface complexation modeling[33] and computational chemistry.[34] [35] Pb2+ has the highest stability at the HBi surface, and the high geochemical affinity of Pb2+ for birnessite probably explains its billion-fold enrichment in marine ferromanganese deposits compared to seawater, which surpasses those of all other elements.

Transition metal cations sorbed on vacancies were also observed to enter the underlying vacancies and become incorporated into the MnO2 layer, when their effective ionic radius[36] is close to that of Mn4+ (r = 0.53 Å). For example, Zn2+ (r = 0.74 Å) was never observed to enter a vacancy site, while Ni2+ (r = 0.69 Å) partly enters, and Co3+ (r = 0.54 Å) always does.[37] [38] Octahedral high-spin Co2+ (r = 0.74 Å) sorbed on a vacancy is transformed into a smaller tetrahedral complex (r = 0.58 Å) to penetrate into the octahedral Mn vacancy, and is subsequently converted to the low-spin state before being oxidized to Co3+ by Mn4+, which is reduced to Mn3+.[39] The surface-catalyzed, redox-driven uptake of Co leads also to a billion-fold enrichment in marine ferromanganese deposits compared to Co between ferromanganese deposits and Pb2+.

Properties and applications

In nature, photosynthetic organisms use the high oxidative ability of birnessite-type Mn4CaO5 clusters to oxidize water into molecular oxygen through the photosystem II membrane protein complex.[40]

Because of their semiconducting properties, birnessite-type materials are used in a variety of areas, including catalysis and electrochemical energy storage (batteries and pseudocapacitors). The ordering of the Mn3+ cations in triclinic birnessite, and the Mn4+ vacancies in hexagonal birnessite, both reduce the band gap,[41] [42] [43] and therefore enhance electrical conductivity. Half-metallic behavior was observed for MnO2 nanosheets with Mn vacancies, rendering them promising candidates for applications in spintronics.[44]

Birnessite is able to break down prions via oxidation.[45] How well this process works outside the laboratory is unclear.

See also

Other manganese oxides:

References

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  2. http://www.handbookofmineralogy.org/pdfs/birnessite.pdf Handbook of Mineralogy
  3. http://www.mindat.org/min-680.html Mindat with location data
  4. http://www.webmineral.com/data/Birnessite.shtml Webmineral data
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