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Tungsten disulfide

From Wikipedia, the free encyclopedia

Tungsten disulfide
Molybdenite-3D-balls.png
WS2 on sapphire.jpg

Left: WS2 film on sapphire. Right: dark exfoliated WS2 film floating on water.
Names
IUPAC names
Tungsten sulfur
Bis(sulfanylidene)tungsten
Systematic IUPAC name
Dithioxotungsten
Other names
Tungsten(IV) sulfide
Tungstenite
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.032.027
EC Number
  • 235-243-3
Properties
WS2
Molar mass 247.98 g/mol
Appearance blue-gray powder[1]
Density 7.5 g/cm3, solid[1]
Melting point 1,250 °C (2,280 °F; 1,520 K) decomposes[1]
slightly soluble
Band gap ~1.35 eV (optical, indirect, bulk)[2][3]
~2.05 eV (optical, direct, monolayer)[4]
+5850·10−6 cm3/mol[5]
Structure
Molybdenite
Trigonal prismatic (WIV)
Pyramidal (S2−)
Related compounds
Other anions
Tungsten(IV) oxide
Tungsten diselenide
Tungsten ditelluride
Other cations
Molybdenum disulfide
Tantalum disulfide
Rhenium disulfide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is ☑Y☒N ?)
Infobox references

Tungsten disulfide is an inorganic chemical compound composed of tungsten and sulfur with the chemical formula WS2. This compound is part of the group of materials called the transition metal dichalcogenides. It occurs naturally as the rare mineral tungstenite. This material is a component of certain catalysts used for hydrodesulfurization and hydrodenitrification.

WS2 adopts a layered structure similar, or isotypic with MoS2, instead with W atoms situated in trigonal prismatic coordination sphere (in place of Mo atoms). Owing to this layered structure, WS2 forms inorganic nanotubes, which were discovered after heating a thin sample of WS2 in 1992.[6]

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Transcription

Contents

Structure and Physical Properties

Atomic image (top) and model (bottom) of Nb-doped WS2. Blue, red, and yellow spheres indicate W, Nb, and S atoms, respectively. Nb doping allows to reduce the WS2 bandgap.[7]
Atomic image (top) and model (bottom) of Nb-doped WS2. Blue, red, and yellow spheres indicate W, Nb, and S atoms, respectively. Nb doping allows to reduce the WS2 bandgap.[7]

Bulk WS2 forms dark gray hexagonal crystals with a layered structure. Like the closely related MoS2, it exhibits properties of a dry lubricant.

Although it has long been thought that WS2 is relatively stable in ambient, recent reports on the ambient air oxidation of monolayer WS2 have found this to not be the case. In the monolayer form, WS2 is converted rather rapidly (over the course of days in ambient light and atmosphere, as observed with a light microscope) to tungsten oxide via a photooxidation reaction involving visible wavelengths of light readily absorbed by WS2 (< ~660 nm/ > ~1.88 eV, or the edge of the absorption spectrum); it is thought that this oxidation occurs via a Dexter electron transfer or Förster resonance energy transfer (FRET) mechanism involving one or more reactive oxygen species.[8] In addition to light of suitable wavelength, the reaction requires oxygen and water to proceed, with the water thought to act as a catalyst for oxidation. The products of the reaction include tungsten oxide and sulfuric acid. The oxidation of other semiconductor transition metal dichalcogenides (S-TMDs) such as MoS2, has similarly been observed to occur in ambient light and atmospheric conditions.[9] The photooxidation of semiconductors (esp. direct bandgap ones) in ambient atmosphere has been an overlooked phenomenon in S-TMD materials research. Since photo-excitation can also occur in bulk WS2, this effect should also be observable in bulk samples (slower than monolayer samples, since photo-excitation occurs with less efficiency in in-direct bandgap materials).

WS2 is also attacked by a mixture of nitric and hydrofluoric acid. When heated in oxygen-containing atmosphere, WS2 converts to tungsten trioxide. When heated in absence of oxygen, WS2 does not melt but decomposes to tungsten and sulfur, but only at 1250 °C.[1]

Historically monolayer WS2 was isolated using chemical exfoliation via intercalation with lithium from n-butyl lithium (in hexane), followed by exfoliation of the Li intercalated compound by sonication in water.[10] WS2 also undergoes exfoliation by treatment with various reagents such as chlorosulfonic acid[11] and the lithium halides.[12]

Synthesis

WS2 is produced by a number of methods.[1][13] Many of these methods involve treating oxides with sources of sulfide or hydrosulfide, supplied as hydrogen sulfide or generated in situ.

Thin films and monolayers

Widely used techniques for the growth of monolayer WS2 include chemical vapor deposition (CVD), physical vapor deposition (PVD) or Metal Organic Chemical Vapor Deposition (MOCVD), though most current methods produce sulfur vacancy defects in excess of 1×1013 cm-2.[14] Other routes entail thermolysis of tungsten(VI) sulfides (e.g., (R4N)2WS4) or the equivalent (e.g., WS3).[13]

Freestanding WS2 films can be produced as follows. WS2 is deposited on a hydrophilic substrate, such as sapphire, and then coated with a polymer, such as polystyrene. After dipping the sample in water for a few minutes, the hydrophobic WS2 film spontaneously peels off.[15]

Applications

WS2 is used, in conjunction with other materials, as catalyst for hydrotreating of crude oil.[13]

Lamellar tungsten disulfide is used as a dry lubricant for fasteners, bearings, and molds under the brand name Dicronite.[16]

Research

Like MoS2, nanostructured WS2 is actively studied for potential applications, such as storage of hydrogen and lithium.[11] WS2 also catalyses hydrogenation of carbon dioxide:[11][17][18]

CO2 + H2 → CO + H2O

Nanotubes

Tungsten disulfide is the first material which was found to form inorganic nanotubes, in 1992.[6] This ability is related to the layered structure of WS2, and macroscopic amounts of WS2 have been produced by the methods mentioned above.[13] WS2 nanotubes have been investigated as reinforcing agents to improve the mechanical properties of polymeric nanocomposites. In a study, WS2 nanotubes reinforced biodegradable polymeric nanocomposites of polypropylene fumarate (PPF) showed significant increases in the Young's modulus, compression yield strength, flexural modulus and flexural yield strength, compared to single- and multi-walled carbon nanotubes reinforced PPF nanocomposites, suggesting that WS2 nanotubes may be better reinforcing agents than carbon nanotubes.[19] The addition of WS2 nanotubes to epoxy resin improved adhesion, fracture toughness and strain energy release rate. The wear of the nanotubes-reinforced epoxy is lower than that of pure epoxy.[20] WS2 nanotubes were embedded into a poly(methyl methacrylate) (PMMA) nanofiber matrix via electrospinning. The nanotubes were well dispersed and aligned along fiber axis. The enhanced stiffness and toughness of PMMA fiber meshes by means of inorganic nanotubes addition may have potential uses as impact-absorbing materials, e.g. for ballistic vests.[21][22]

WS2 nanotubes are hollow and can be filled with another material, to preserve or guide it to a desired location, or to generate new properties in the filler material which is confined within a nanometer-scale diameter. To this goal, inorganic nanotube hybrids were made by filling WS2 nanotubes with molten lead, antimony or bismuth iodide salt by a capillary wetting process, resulting in PbI2@WS2, SbI3@WS2 or BiI3@WS2 core–shell nanotubes.[23]

Nanosheets

WS2 can also exist in the form of atomically thin sheets.[24] Such materials exhibit room-temperature photoluminescence in the monolayer limit.[25]

Transistors

Taiwan Semiconductor Manufacturing Company (TSMC) is investigating use of WS
2
as a channel material in field effect transistors. The approximately 6-layer thick material is created using chemical vapor deposition (CVD).[26]

References

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