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==Health and safety hazards== ==Health and safety hazards==
Like all uranium(VI) compounds, UO<sub>3</sub> is hazardous by inhalation, ingestion, and through skin contact. It is a poisonous, radioactive substance, which may cause shortness of breath, coughing, acute arterial lesions, and changes in the chromosomes of ]s and ] leading to ] if inhaled. Like all hexavalent uranium, or "uranium(VI)" compounds, UO<sub>3</sub> is hazardous by inhalation, ingestion, and through skin contact. It is a poisonous, radioactive substance, which may cause shortness of breath, coughing, acute arterial lesions, and changes in the chromosomes of ]s and ] leading to ] if inhaled.


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Revision as of 01:51, 29 March 2006

Uranium trioxide
O
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O = {\displaystyle =\,} U = {\displaystyle =\,} O

 
γ-UO3:

Systematic name Uranium trioxide
Other names Uranium(VI) oxide

Uranyl oxide

Uranic oxide

Molecular formula UO3 (or O3U, NIST)
Molar mass 286.03 g mol
CAS number
Density 5.5-8.7 g cm
Solubility (water) Insoluble
Solubility (dog lung fluid) < 5 days half time
Melting point ca. 500 °C decomp.(s)
Disclaimer and references

Uranium trioxide (UO3), also called uranyl oxide and uranic oxide, is the hexavalent oxide of uranium. The toxic, teratogenic, and radioactive solid may be obtained by heating uranyl nitrate to 400 °C, or burning uranium in air, producing a gas which condenses at standard temperature and pressure.

Its most commonly encountered polymorph, γ-UO3, is a yellow-orange powder.

Cameco Corporation, which operates at the world's largest uranium refinery at Blind River, Ontario, produces high-purity uranium trioxide.

Health and safety hazards

Like all hexavalent uranium, or "uranium(VI)" compounds, UO3 is hazardous by inhalation, ingestion, and through skin contact. It is a poisonous, radioactive substance, which may cause shortness of breath, coughing, acute arterial lesions, and changes in the chromosomes of white blood cells and gonads leading to congenital malformations if inhaled.

UO3-Material Safety Data Sheet.

Chemistry

Solid UO3 may be obtained by heating uranyl nitrate (UO2(NO3)2·6H2O) at 400 °C. This conversion is used in the reprocessing of nuclear fuel, which begins with the dissolution of the fuel rods in HNO3.

Uranium trioxide is also an intermediary compound in the conversion of sodium diuranate yellowcake (Na2U2O7·6H2O) to uranium hexafluoride and is shipped between processing facilities in the form of a UO3 gel. In the jargon of the uranium refining industry, the chemical solution containing the concentrated uranium trioxide is called "OK liquor". Upon heating, this material liberates ammonia, giving UO3.

Chemical and structural properties

The only well characterized binary trioxide of any actinide is UO3, of which several polymorphs are known. At 800-900 °C, UO3 releases some O2 to give green-colored U3O8. Heating at 700 °C under H2 gives dark brown uranium dioxide (UO2), which is used in MOX nuclear fuel rods.

The most frequently encountered polymorph is γ-UO3, whose x-ray structure has been solved from powder diffraction data. The compound crystallizes in the space group I41/amd with two uranium atoms in the asymmetric unit. Both are surrounded by somewhat distorted octahedra of oxygen atoms. One uranium atom has two closer and four more distant oxygen atoms whereas the other has four close and two more distant oxygen atoms as neighbors. Thus it is not incorrect to describe the structure as , that is uranyl uranate. (Engmann 1963).

Infrared spectroscopy of molecular UO3 isolated in an argon matrix indicates a T-shaped structure (point group C2v) for the molecule. This is in contrast to the commonly encountered D3h symmetry exhibited by most trioxides. One could think of the compound as "uranyl monoxide", O. From the force constants the authors deduct the U-O bond lengths to be between 1.76 and 1.79 angstroms. The authors did not attempt to deduce bond angles. (Gabelnick, Reedy, Chasanov 1970)

Combustion product of uranium

Monomeric UO3 is produced by combustion of uranium metal in air from 2200-2800 Kelvin (Ackermann et al. 1960; Mouradian et al. 1963.) UO3 gas will eventully condense under normal atmospheric conditions, and hence the gaseous form is "not infrequently ignored" (Gmelin vol. U-C1, p. 98); however, UO3 is an important intermediate state in full combustion of uranium.

Uranium trioxide gas molecules are a known intermediate in the chemical transition reactions forming U3O8 crystals from combustion products including uranium oxides. According to Wilson (1961), Ackermann et al. (1960) show that U3O8 crystals result from the two step process:

/3 U3O8(s) + /6 O2(g) → UO3(g) at T1;
UO3(g) → /3 U3O8 + /6 O2(g) at T2;
where T2 < T1.

Individual UO3 molecules will not decompose below the burning temperature of uranium in air, because uranium monoxide requires additional energy to form, as does the release of O2 by a single UO3 molecule. (Hoekstra and Siegel 1958; Wanner and Forest (2004) p. 98.)

Uranium oxide in ceramics

UO3-based ceramics become green or black when fired in a reducing atmosphere and yellow to orange when fired with oxygen. Orange-coloured Fiestaware is a well-known example of a product with a uranium-based glaze. UO3-has also been used in formulations of enamel, uranium glass, and porcelain.

Prior to 1960, UO3 was used as an agent of crystallization in crystalline coloured glazes. It is possible to determine with a Geiger counter if a glaze or glass was made from UO3.

Related anions and cations

Uranium oxide is amphoteric and reacts as acid and as a base, depending on the conditions.

As an acid:

UO3 + H2O → UO4 + H

Dissolving uranium oxide in a strong base like sodium hydroxide forms the doubly negatively charged uranate anion (UO4). Uranates tend to agglomerate, forming diuranate, U2O7

As a base:

UO3 + H2O → UO2 + OH

Dissolving uranium oxide in a strong acid like sulfuric or nitric acid forms the double positive charged uranyl cation. The uranyl nitrate formed (UO2(NO3)2ˑ6H2O) is soluble in ethers, alcohols, ketones and esters; for example, tributylphosphate. This solubilty is used to separate uranium from other elements in nuclear reprocessing, which begins with the dissolution of nuclear fuel rods in nitric acid. The uranyl nitrate is then converted to uranium trioxide by heating.

From nitric acid one obtains uranyl nitrate, trans-UO2(NO3)2·2H2O, consisting of eight-coordinated uranium with two bidentate nitrato ligands and two water ligands as well as the familiar O=U=O core.

See also

Accidental teratogens:

References

Peer-reviewed
  • Wilson, W.B. (1961) "High-Pressure High-Temperature Investigation of the Uranium-Oxygen System," Journal Of Inorganic and Nuclear Chemistry, 19, 212-222.
  • R.J. Ackermann, et al., "Free Energies of Formation of Gaseous Uranium, Molybdenum, and Tungsten Trioxides," Journal of Physical Chemistry, vol. 64 (1960) pp. 350-355
  • Mouradian and Baker (1963) "Burning Temperatures of Uranium and Zirconium in Air," Nuclear Science and Engineering, 15, 388-394
  • Morrow et al. (1972) "Inhalation studies of uranium trioxide" Health Physics 23, 273-280
  • Stuart et al. (1979) "Solubility and Hemolytic Activity of Uranium Trioxide." Environmental Research 18, 385-396
  • Nakajima, K.; Arai, Y. (2001) "Mass-spectrometric investigation of UO{sub 3}(g)", Journal of Nuclear Materials, 294, 250-255.
  • Green, D.W. (1980) "Relationship between spectroscopic data and thermodynamic functions; application to uranium, plutonium, and thorium oxide vapor species," Journal of Nuclear Materials, 88, 51-63.
  • Ackermann, R.J. and A.T. Chang (1973) "Thermodynamic Characterization of U3O8-z Phase," Journal Of Chemical Thermodynamics, 5, 873-890.
  • Chapman, A.T. and Meadows, R.E. (1964) "Volatility of UO2+/-x and Phase Relations in the System Uranium Oxygen," Journal of the American Ceramic Society, 47, 614-621.
  • Drowart, J., A. Pattoret, and S. Smoes (1964) "Heat of sublimation of uranium and consistency of thermodynamic data for uranium compounds," Journal of Nuclear Materials, 12, 319-322.
  • Roberts, L.E.J. and A.J. Walter (1961) "Equilibrium Pressures and Phase Relations in the Uranium Oxide System," Journal of Inorganic and Nuclear Chemistry, 22, 213-229.
  • Hoekstra, H.R. and Siegel, S. (1970) "Uranium-Oxygen System at high pressure," Journal of Inorganic and Nuclear Chemistry, 32, 3237-3248.
  • Cort, B., et al. (1987) "Infrared Characterization of Uranium Oxide Powders Using a Metal Light Pipe," Applied Spectroscopy, 41, 493-495.
  • Batrakov, Y.F., et al. (2000) "Identification of the uranium state in minerals by the chemical shift of hard X-ray lines," Radiochemistry, 42, 112-118.
  • Batrakov, Y.F., et al. (2004) "Effect of the chemical state of uranium atom on the energy of spin-orbital splitting of its inner orbitals," Radiochimica Acta, 92, 73-80.
  • Rauh, E.G. and R.J. Ackermann (1974) "First ionization potentials of some refractory oxide vapors," J. Chem. Phys., 60, 1396.
  • S.D. Gabelnick, G.T. Reedy, M.G. Chasanov (1973) "Infrared spectra of matrix-isolated uranium oxide species. II: Spectral interpretation and structure of UO3," J. Chem. Phys., 59, 6397.
  • R. Engmann, P.M. de Wolff (1963) "The Crystal Structure of γ-UO3," Acta Cryst., 16, 993.
  • Chazel, V., et al. (1998) "Effect of U3O8 specific surface area on in vitro dissolution, biokinetics, and dose coefficients," Radiation Protection Dosimetry, 79, 39-42.
  • Khaskelis, A.I. (2004) "Uranium oxide weathering: spectroscopy and kinetics," Transactions of the American Nuclear Society, 91, 890-891. Abstract: "During nuclear fuel fabrication or reprocessing stages of a nuclear fuel cycle, it is possible for small particles of uranium oxides to escape into the environment. This paper reports measurements of rates of oxidation of uranium dioxide particles in controlled gas environments using in-situ phosphorescence spectroscopy. Comparison is made with reduction and reoxidation of uranium trioxide...."
  • Ansoborlo, E. (1998) "Exposure implications for uranium aerosols formed at a new laser enrichment facility: application of the ICRP respiratory tract and systemic model," Radiation Protection Dosimetry, 79, 23-27. Abstract: "... urine assay could be useful, provided that measurements are made soon after a known acute intake."
  • Ansoborlo, E. (2002) "Determination of the physical and chemical properties, biokinetics, and dose coefficients of uranium compounds handled during nuclear fuel fabrication in France," Health Physics, 82, 279-289.
  • Sutton, M. and S.R. Burastero (2004) "Uranium(VI) solubility and speciation in simulated elemental human biological fluids," Chemical Research in Toxicology, 17, 1468-1480.
  • Stradling, G.N., et al. (2000) Radiation Protection Dosimetry, 87, 41-50.
  • Chazel, V., et al. (2000) "Variation of solubility, biokinetics and dose coefficient of industrial uranium oxides according to specific surface area," Radiation Protection Dosimetry, 88, 223-231.
United Nations invitation-only
  • H. R. Hoekstra and S. Siegel (1958) "Recent Developments in the Chemistry of the Uranium-Oxygen System," in the Proceedings of the Second International Conference on Peaceful Uses of Atomic Energy, (Geneva: UN) 7, 394-400.
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