Uranium hexafluoride

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Uranium hexafluoride, sometimes called hex, is the inorganic compound with the formula Template:Chem2. Uranium hexafluoride is a volatile, white solid that is used in enriching uranium for nuclear reactors and nuclear weapons.<ref name=Ull/>

PreparationEdit

Uranium dioxide is converted with hydrofluoric acid (HF) to uranium tetrafluoride:<ref name=Ull>Template:Cite book</ref>

Template:Chem2

In samples contaminated with uranium trioxide, the oxyfluoride is produced in the HF step:

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The resulting Template:Chem2 is subsequently oxidized with fluorine to give the hexafluoride:

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PropertiesEdit

Physical propertiesEdit

At atmospheric pressure, Template:Chem2 sublimes at 56.5 °C.<ref>Template:Cite journal</ref>

The solid-state structure was determined by neutron diffraction at 77 K and 293 K.<ref>Template:Cite journal</ref><ref>Template:Cite journal</ref><ref name="UF6_1973">J. C. Taylor, P. W. Wilson, J. W. Kelly: „The structures of fluorides. I. Deviations from ideal symmetry in the structure of crystalline UF₆: a neutron diffraction analysis", Acta Crystallogr., 1973, B29, p. 7–12; {{#invoke:doi|main}}.</ref>

File:Uranium-hexafluoride-unit-cell-3D-balls.png

Packing of UF₆ in its unit cell.<ref name="UF6_1968">Template:Cite journal</ref>

Chemical propertiesEdit

UF₆ reacts with water, releasing hydrofluoric acid. The compound reacts with aluminium, forming a surface layer of [[aluminium fluoride|Template:Chem2]] that resists any further reaction from the compound.

Uranium hexafluoride is a mild oxidant.<ref>Template:Cite journal</ref> It is a Lewis acid as evidenced by its binding to form heptafluorouranate(VI), Template:Chem2.<ref>Template:Cite journal</ref>

Polymeric uranium(VI) fluorides containing organic cations have been isolated and characterized by X-ray diffraction.<ref>Template:Cite journal</ref>

Application in the fuel cycleEdit

File:Uranium hexafluoride phase diagram.gif

Phase diagram of Template:Chem2

As one of the most volatile compounds of uranium, uranium hexafluoride is relatively convenient to process and is used in both of the main uranium enrichment methods, namely gaseous diffusion and the gas centrifuge method. Since the triple point of Template:Chem2; 64 °C(147 °F; 337 K) and 152 kPa (22 psi; 1.5 atm);<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> is close to ambient conditions, phase transitions can be achieved with little thermodynamic work.

Fluorine has only a single naturally occurring stable isotope, so isotopologues of Template:Chem2 differ in their molecular weight based solely on the uranium isotope present.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> This difference is the basis for the physical separation of isotopes in enrichment.

All the other uranium fluorides are nonvolatile solids that are coordination polymers.

The conversion factor for the Template:Chem2 isotopologue of Template:Chem2 ("hex") to "U mass" is 0.676.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref>

Gaseous diffusion requires about 60 times as much energy as the gas centrifuge process: gaseous diffusion-produced nuclear fuel produces 25 times more energy than is used in the diffusion process, while centrifuge-produced fuel produces 1,500 times more energy than is used in the centrifuge process.

In addition to its use in enrichment, uranium hexafluoride has been used in an advanced reprocessing method (fluoride volatility), which was developed in the Czech Republic. In this process, spent nuclear fuel is treated with fluorine gas to transform the oxides or elemental metals into a mixture of fluorides. This mixture is then distilled to separate the different classes of material. Some fission products form nonvolatile fluorides which remain as solids and can then either be prepared for storage as nuclear waste or further processed either by solvation-based methods or electrochemically.

Uranium enrichment produces large quantities of depleted uranium hexafluoride (DTemplate:Chem2 or D-Template:Chem2) as a waste product. The long-term storage of D-Template:Chem2 presents environmental, health, and safety risks because of its chemical instability. When Template:Chem2 is exposed to moist air, it reacts with the water in the air to produce Template:Chem2 (uranyl fluoride) and HF (hydrogen fluoride) both of which are highly corrosive and toxic. In 2005, 686,500 tonnes of D-Template:Chem2 was housed in 57,122 storage cylinders located near Portsmouth, Ohio; Oak Ridge, Tennessee; and Paducah, Kentucky.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref><ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> Storage cylinders must be regularly inspected for signs of corrosion and leaks. The estimated lifetime of the steel cylinders is measured in decades.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref>

Accidents and disposalEdit

There have been several accidents involving uranium hexafluoride in the US, including a cylinder-filling accident and material release at the Sequoyah Fuels Corporation in 1986 where an estimated 29 500 pounds of gaseous Template:Chem2 escaped.<ref>Template:Cite journal</ref><ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> The U.S. government has been converting DTemplate:Chem2 to solid uranium oxides for disposal.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> Such disposal of the entire DTemplate:Chem2 stockpile could cost anywhere from $15 million to $450 million.<ref>{{#invoke:citation/CS1|citation |CitationClass=web }}</ref> {{#invoke:Gallery|gallery}}