Uranium hexafluoride

Names
IUPAC names Uranium hexafluoride Uranium(VI) fluoride
Identifiers
CAS Number	7783-81-5 Y
3D model (JSmol)	Interactive image
Abbreviations	hex
ChEBI	CHEBI:30235 Y
ChemSpider	22966 Y
ECHA InfoCard	100.029.116
EC Number	232-028-6
Gmelin Reference	2923
PubChem CID	24560
RTECS number	YR4720000
UNII	N06GJ1D94J Y
UN number	2978 (<1% 235U) 2977 (>1% 235U)
CompTox Dashboard (EPA)	DTXSID4074566
InChI InChI=1S/6FH.U/h6*1H;/q;;;;;;+6/p-6 Y Key: SANRKQGLYCLAFE-UHFFFAOYSA-H Y InChI=1/6FH.U/h6*1H;/q;;;;;;+6/p-6/rF6U/c1-7(2,3,4,5)6 Key: SANRKQGLYCLAFE-IIYYNVFAAT
SMILES F[U](F)(F)(F)(F)F
Properties
Chemical formula	UF6
Molar mass	352.02 g/mol
Appearance	Colorless solid
Density	5.09 g/cm3, solid
Boiling point	56.5 °C (133.7 °F; 329.6 K) (sublimes, at atmospheric pressure)
Solubility in water	Hydrolyzes
Solubility	Soluble in chloroform, CCl4, liquid chlorine, and bromine Dissolves in nitrobenzene; 151 kPa[1]
Structure
Crystal structure	Orthorhombic, oP28
Space group	Pnma, No. 62
Coordination geometry	Octahedral (Oh)
Dipole moment	0
Thermochemistry
Std molar entropy (S⦵298)	Solid, 227.8±1.3 J·K−1·mol−1[2] Gaseous, 377.8±1.3 J·K−1·mol−1[2]
Std enthalpy of formation (ΔfH⦵298)	Solid, −2197.7±1.8 kJ·mol−1[2] Gaseous, −2148.1±1.8 kJ·mol−1[2]
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Toxic, corrosive, radioactive[3]
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H300, H330, H373, H411
NFPA 704 (fire diamond)	4 0 2 W OX
Flash point	Non-flammable
Safety data sheet (SDS)	ICSC 1250
Related compounds
Other anions	Uranium hexachloride
Other cations	Neptunium hexafluoride Plutonium hexafluoride Americium hexafluoride Curium hexafluoride Tungsten hexafluoride
Related uranium fluorides	Uranium(III) fluoride Uranium(IV) fluoride Uranium(V) fluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Y verify (what is YN ?) Infobox references

Uranium hexafluoride, sometimes called hex, is an inorganic compound with the formula UF₆. Uranium hexafluoride is a volatile and toxic white solid that reacts with water, releasing corrosive hydrofluoric acid. The compound reacts mildly with aluminium, forming a thin surface layer of AlF₃ that resists any further reaction from the compound. UF₆ is used in the process of enriching uranium, which produces fuel for nuclear reactors and nuclear weapons.

Milled uranium ore—U₃O₈ or "yellowcake"—is dissolved in nitric acid, yielding a solution of uranyl nitrate UO₂(NO₃)₂. Pure uranyl nitrate is obtained by solvent extraction, then treated with ammonia to produce ammonium diuranate ("ADU", [NH₄]₂U₂O₇). Reduction with hydrogen gives UO₂, which is converted with hydrofluoric acid (HF) to uranium tetrafluoride, UF₄. Oxidation with fluorine yields UF₆.

The Honeywell Uranium Hexafluoride Processing Facility uses a different process.

During nuclear reprocessing, uranium is reacted with chlorine trifluoride to give UF₆:

U + 2 ClF₃ → UF₆ + Cl₂

At atmospheric pressure, UF₆ sublimes at 56.5 °C.^[4]

The solid-state structure was determined by neutron diffraction at 77 K and 293 K.^[5][6]

• 
  Ball-and-stick model of the unit cell of uranium hexafluoride^[7]
• 
  Bond lengths and angles of gaseous uranium hexafluoride^[8]

It has been shown that uranium hexafluoride is an oxidant^[9] and a Lewis acid that is able to bind to fluoride; for instance, the reaction of copper(II) fluoride with uranium hexafluoride in acetonitrile is reported to form copper(II) heptafluorouranate(VI), Cu²⁺[UF−7]₂.^[10]

Polymeric uranium(VI) fluorides containing organic cations have been isolated and characterized by X-ray diffraction.^[11]

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 UF₆; 64 °C(147 °F; 337 K) and 152 kPa (22 psi; 1.5 atm);^[12] 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 UF₆ differ in their molecular weight based solely on the uranium isotope present.^[13] 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 ²³⁸U isotopologue of UF₆ ("hex") to "U mass" is 0.676.^[14]

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 (DUF₆ or D-UF₆) as a waste product. The long-term storage of D-UF₆ presents environmental, health, and safety risks because of its chemical instability. When UF₆ is exposed to moist air, it reacts with the water in the air to produce UO₂F₂ (uranyl fluoride) and HF (hydrogen fluoride) both of which are highly corrosive and toxic. In 2005, 686,500 tonnes of D-UF₆ was housed in 57,122 storage cylinders located near Portsmouth, Ohio; Oak Ridge, Tennessee; and Paducah, Kentucky.^[15][16] Storage cylinders must be regularly inspected for signs of corrosion and leaks. The estimated lifetime of the steel cylinders is measured in decades.^[17]

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 UF₆ escaped.^{[18] [19]} The U.S. government has been converting DUF₆ to solid uranium oxides for disposal.^[20] Such disposal of the entire DUF₆ stockpile could cost anywhere from $15 million to $450 million.^[21]

• Gmelins Handbuch der anorganischen Chemie, System Nr. 55, Uran, Teil A, p. 121–123.
• Gmelins Handbuch der anorganischen Chemie, System Nr. 55, Uran, Teil C 8, p. 71–163.
• R. DeWitt: Uranium hexafluoride: A survey of the physico-chemical properties, Technical report, GAT-280; Goodyear Atomic Corp., Portsmouth, Ohio; 12. August 1960; doi:10.2172/4025868.
• Ingmar Grenthe, Janusz Drożdżynński, Takeo Fujino, Edgar C. Buck, Thomas E. Albrecht-Schmitt, Stephen F. Wolf: Uranium Archived 2012-01-18 at the Wayback Machine, in: Lester R. Morss, Norman M. Edelstein, Jean Fuger (Hrsg.): The Chemistry of the Actinide and Transactinide Elements, Springer, Dordrecht 2006; ISBN 1-4020-3555-1, p. 253–698; doi:10.1007/1-4020-3598-5_5 (p. 530–531, 557–564).
• US-Patent 2535572: Preparation of UF₆; 26. December 1950.
• US-Patent 5723837: Uranium Hexafluoride Purification; 3. March 1998.

Wikimedia Commons has media related to Uranium hexafluoride.

• Simon Cotton (Uppingham School, Rutland, UK): Uranium Hexafluoride.
• Uranium Hexafluoride (UF₆) – Physical and chemical properties of UF₆, and its use in uranium processing – Uranium Hexafluoride and Its Properties
• Uranium Hexafluoride at WebElements
• Import of Western depleted uranium hexafluoride (uranium tails) to Russia [dead link 30 June 2017]