Tungsten hexafluoride. Tungsten(VI) fluoride, also known as tungsten hexafluoride, is an inorganic compound with the formula . It is a toxic, corrosive, colorless gas, with a density of about  (roughly 11 times heavier than air). It is the densest known gas under standard ambient temperature and pressure (298 K, 1 atm).  is commonly used by the semiconductor industry to form tungsten films, through the process of chemical vapor deposition. This layer is used in a low-resistivity metallic "interconnect". It is one of seventeen known binary hexafluorides.

Properties
The  molecule is octahedral with the symmetry point group of Oh. The W–F bond distances are . Between , tungsten hexafluoride condenses into a colorless liquid having the density of  at . At  it freezes into a white solid having a cubic crystalline structure, the lattice constant of 628 pm and calculated density . At  this structure transforms into an orthorhombic solid with the lattice constants of a = 960.3 pm, b = 871.3 pm, and c = 504.4 pm, and the density of . In this phase, the W–F distance is 181 pm, and the mean closest molecular contacts are . Whereas  gas is one of the densest gases, with the density exceeding that of the heaviest elemental gas radon (9.73 g/L), the density of  in the liquid and solid state is rather moderate.
The vapor pressure of  between  can be described by the equation
,
where the P = vapor pressure (bar), T = temperature (°C).

History and synthesis
Tungsten hexafluoride was first obtained by conversion of tungsten hexachloride with hydrogen fluoride by Otto Ruff and Fritz Eisner in 1905.

The compound is now commonly produced by the exothermic reaction of fluorine gas with tungsten powder at a temperature between :

The gaseous product is separated from , a common impurity, by distillation. In a variation on the direct fluorination, the metal is placed in a heated reactor, slightly pressurized to , with a constant flow of  infused with a small amount of fluorine gas.

The fluorine gas in the above method can be substituted by ClF,  or . An alternative procedure for producing tungsten fluoride is to treat tungsten trioxide () with HF,  or . And besides HF, other fluorinating agents can also be used to convert tungsten hexachloride in a way similar to Ruff and Eisner original method:
 or

Reactions
On contact with water, tungsten hexafluoride gives hydrogen fluoride (HF) and tungsten oxyfluorides, eventually forming tungsten trioxide:

Unlike some other metal fluorides,  is not a useful fluorinating agent nor is it a powerful oxidant. It can be reduced to the yellow .

 forms a variety of 1:1 and 1:2 adducts with Lewis bases, examples being .

Applications in semiconductor industry
The dominant application of tungsten fluoride is in semiconductor industry, where it is widely used for depositing tungsten metal in a chemical vapor deposition (CVD) process. The expansion of the industry in the 1980s and 1990s resulted in the increase of  consumption, which remains at around 200 tonnes per year worldwide. Tungsten metal is attractive because of its relatively high thermal and chemical stability, as well as low resistivity (5.6 μΩ·cm) and very low electromigration.  is favored over related compounds, such as  or , because of its higher vapor pressure resulting in higher deposition rates. Since 1967, two  deposition routes have been developed and employed, thermal decomposition and hydrogen reduction. The required  gas purity is rather high and varies between 99.98% and 99.9995% depending on the application.

 molecules have to be split up in the CVD process. The decomposition is usually facilitated by mixing  with hydrogen, silane, germane, diborane, phosphine, and related hydrogen-containing gases.

Silicon
 reacts upon contact with a silicon substrate. The  decomposition on silicon is temperature-dependent:
 below 400 °C and
 above 400 °C.

This dependence is crucial, as twice as much silicon is being consumed at higher temperatures. The deposition occurs selectively on pure silicon only, but not on silicon oxide or silicon nitride, thus the reaction is highly sensitive to contamination or substrate pre-treatment. The decomposition reaction is fast, but saturates when the tungsten layer thickness reaches 10–15 micrometers. The saturation occurs because the tungsten layer stops diffusion of  molecules to the Si substrate which is the only catalyst of molecular decomposition in this process.

If the deposition occurs not in an inert atmosphere but in an oxygen-containing atmosphere (air), then instead of tungsten, a tungsten oxide layer is produced.

Hydrogen
The deposition process occurs at temperatures between 300 and 800 °C and results in formation of hydrogen fluoride vapors:

The crystallinity of the produced tungsten layers can be controlled by altering the / ratio and the substrate temperature: low ratios and temperatures result in (100) oriented tungsten crystallites whereas higher values favor the (111) orientation. Formation of HF is a drawback, as the HF vapor is very aggressive and etches away most materials. Also, the deposited tungsten shows poor adhesion to the silicon dioxide which is the main passivation material in semiconductor electronics. Therefore,  has to be covered with an extra buffer layer prior to the tungsten deposition. On the other hand, etching by HF may be beneficial to remove unwanted impurity layers.

Silane and germane
The characteristic features of tungsten deposition from the / are high speed, good adhesion and layer smoothness. The drawbacks are explosion hazard and high sensitivity of the deposition rate and morphology to the process parameters, such as mixing ratio, substrate temperature, etc. Therefore, silane is commonly used to create a thin tungsten nucleation layer. It is then switched to hydrogen, that slows down the deposition and cleans up the layer.

Deposition from / mixture is similar to that of /, but the tungsten layer becomes contaminated with relatively (compared to Si) heavy germanium up to concentrations of 10–15%. This increases tungsten resistance from about 5 to 200 μΩ·cm.

Other applications
 can be used for the production of tungsten carbide.

As a heavy gas,  can be used as a buffer to control gas reactions. For example, it slows down the chemistry of the Ar// flame and reduces the flame temperature.

Safety
Tungsten hexafluoride is an extremely corrosive compound that attacks any tissue. Because of the formation of hydrofluoric acid upon reaction of  with humidity,  storage vessels have Teflon gaskets.

References

Tungsten halides
Hexafluorides
Lachrymatory agents
Octahedral compounds
Industrial gases