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Uranium trioxide

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Uranium trioxide
Names
IUPAC names
Uranium trioxide
Uranium(VI) oxide
Other names
Uranyl oxide
Uranic oxide
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.014.274 Edit this at Wikidata
EC Number
  • 215-701-9
UNII
  • InChI=1S/3O.U
    Key: JCMLRUNDSXARRW-UHFFFAOYSA-N
  • O=[U](=O)=O
Properties
UO3
Molar mass 286.29 g/mol
Appearance yellow-orange powder
Density 5.5–8.7 g/cm3
Melting point ~200–650 °C (decomposes)
insoluble
Structure
see text
I41/amd (γ-UO3)
Thermochemistry
99 J·mol−1·K−1[1]
−1230 kJ·mol−1[1]
Hazards
GHS labelling:
GHS06: ToxicGHS08: Health hazardGHS09: Environmental hazard
Danger
H300, H330, H373, H411
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 4: Very short exposure could cause death or major residual injury. E.g. VX gasFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
4
0
1
OX
Flash point Non-flammable
Safety data sheet (SDS) External MSDS
Related compounds
Related uranium oxides
 Uranium dioxide
Triuranium octoxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Uranium trioxide (UO3), also called uranyl oxide, uranium(VI) oxide, and uranic oxide, is the hexavalent oxide of uranium. The solid may be obtained by heating uranyl nitrate to 400 °C. Its most commonly encountered polymorph is amorphous UO3.

Production and use

[edit]

There are three methods to generate uranium trioxide. As noted below, two are used industrially in the reprocessing of nuclear fuel and uranium enrichment.

Methods of forming uranium trioxide

  1. U3O8 can be oxidized at 500 °C with oxygen.[2] Note that above 750 °C even in 5 atm O2 UO3 decomposes into U3O8.[3]
  2. Uranyl nitrate, UO2(NO3)2·6H2O can be heated to yield UO3. This occurs during the reprocessing of nuclear fuel. Fuel rods are dissolved in HNO3 to separate uranyl nitrate from plutonium and the fission products (the PUREX method). The pure uranyl nitrate is converted to solid UO3 by heating at 400 °C. After reduction with hydrogen (with other inert gas present) to uranium dioxide, the uranium can be used in new MOX fuel rods.
  3. Ammonium diuranate or sodium diuranate (Na2U2O7·6H2O) may be decomposed. Sodium diuranate, also known as yellowcake, is converted to uranium trioxide in the enrichment of uranium. Uranium dioxide and uranium tetrafluoride are intermediates in the process which ends in uranium hexafluoride.[4]

Uranium trioxide is shipped between processing facilities in the form of a gel, most often from mines to conversion plants.

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

It has been reported that the corrosion of uranium in a silica rich aqueous solution forms uranium dioxide, uranium trioxide,[5] and coffinite.[6] In pure water, schoepite (UO2)8O2(OH)12·12(H2O) is formed[7] in the first week and then after four months studtite (UO2)O2·4(H2O) was produced. This alteration of uranium oxide also leads to the formation of metastudtite,[8][9] a more stable uranyl peroxide, often found in the surface of spent nuclear fuel exposed to water. Reports on the corrosion of uranium metal have been published by the Royal Society.[10][11]

Health and safety hazards

[edit]

Like all hexavalent uranium compounds, UO3 is hazardous by inhalation, ingestion, and through skin contact. It is a poisonous, slightly 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.[12][13] However, once ingested, uranium is mainly toxic for the kidneys and may severely affect their function.

Structure

[edit]

Solid state structure

[edit]

The only well characterized binary trioxide of any actinide is UO3, of which several polymorphs are known. Solid UO3 loses O2 on heating to give green-colored U3O8: reports of the decomposition temperature in air vary from 200 to 650 °C. Heating at 700 °C under H2 gives dark brown uranium dioxide (UO2), which is used in MOX nuclear fuel rods.

Alpha

[edit]
 The α (alpha) form: a layered solid where the 2D layers are linked by oxygen atoms (shown in red) Hydrated uranyl peroxide formed by the addition of hydrogen peroxide to an aqueous solution of uranyl nitrate when heated to 200–225 °C forms an amorphous uranium trioxide which on heating to 400–450 °C will form alpha-uranium trioxide.[3] It has been stated that the presence of nitrate will lower the temperature at which the exothermic change from the amorphous form to the alpha form occurs.[14]

Beta

[edit]
 The β (beta) UO3 form: This solid contains multiple unique uranium sites and distorted polyhedra. This form can be formed by heating ammonium diuranate, while P.C. Debets and B.O. Loopstra, found four solid phases in the UO3-H2O-NH3 system that they could all be considered as being UO2(OH)2·H2O where some of the water has been replaced with ammonia.[15][16] It was found that calcination at 500 °C in air forms the beta form of uranium trioxide.[3] Later experiments found the most reliable method for synthesizing pure β-UO3 was to calcinate uranyl nitrate hexahydrate at 450 °C for 6 days and cool slowly over 24 hours.[17]

Gamma

[edit]
 The γ (gamma) form: with the different uranium environments in green and yellow 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 [UO2]2+[UO4]2− , that is uranyl uranate.[18]
The environment of the uranium atoms shown as yellow in the gamma form
The chains of U2O2 rings in the gamma form in layers, alternate layers running at 90 degrees to each other. These chains are shown as containing the yellow uranium atoms, in an octahedral environment which are distorted towards square planar by an elongation of the axial oxygen-uranium bonds.

Delta

[edit]
 The delta (δ) form is a cubic solid where the oxygen atoms are arranged between the uranium atoms.[19]

Epsilon

[edit]
 The proposed crystal structure of the epsilon (ε) form consists of sheets of uranium hexagonal bipyramids connected through edge-sharing polyhedra. These sheets are connected through the axial uranyl oxygen atoms. The proposed structure is in the triclinic P-1 space group.[20]

High pressure form

[edit]

There is a high-pressure solid form with U2O2 and U3O3 rings in it.[21] [22]

Hydrates

[edit]
  • Hydrous and anhydrous forms of UO3
    Hydrous and anhydrous forms of UO3
  • Anhydrous forms of UO3
    Anhydrous forms of UO3

Several hydrates of uranium trioxide are known, e.g., UO3·6H2O, which are commonly known as "uranic acid" in older literature due to their similarity in formula to various metal oxyacids, although they are not in fact particularly acidic.[3]

Molecular forms

[edit]

While uranium trioxide is encountered as a polymeric solid under ambient conditions, some work has been done on the molecular form in the gas phase, in matrix isolations studies, and computationally.

Gas phase

[edit]

At elevated temperatures gaseous UO3 is in equilibrium with solid U3O8 and molecular oxygen.

2 U3O8(s) + O2(g) ⇌ 6 UO3(g)

With increasing temperature the equilibrium is shifted to the right. This system has been studied at temperatures between 900 °C and 2500 °C. The vapor pressure of monomeric UO3 in equilibrium with air and solid U3O8 at ambient pressure, about 10−5 mbar (1 mPa) at 980 °C, rising to 0.1 mbar (10 Pa) at 1400 °C, 0.34 mbar (34 Pa) at 2100 °C, 1.9 mbar (193 Pa) at 2300 °C, and 8.1 mbar (809 Pa) at 2500 °C.[23][24]

Matrix isolation

[edit]

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 molecular symmetry exhibited by most trioxides. From the force constants the authors deduct the U-O bond lengths to be between 1.76 and 1.79 Å (176 to 179 pm).[25]

Computational study

[edit]
The calculated geometry of molecular uranium trioxide has C2v symmetry.

Calculations predict that the point group of molecular UO3 is C2v, with an axial bond length of 1.75 Å, an equatorial bond length of 1.83 Å and an angle of 161° between the axial oxygens. The more symmetrical D3h species is a saddle point, 49 kJ/mol above the C2v minimum. The authors invoke a second-order Jahn–Teller effect as explanation.[26]

Cubic form of uranium trioxide

[edit]

The crystal structure of a uranium trioxide phase of composition UO2·82 has been determined by X-ray powder diffraction techniques using a Guinier-type focusing camera. The unit cell is cubic with a = 4·138 ± 0·005 kX. A uranium atom is located at (000) and oxygens at (View the MathML source), (View the MathML source), and (View the MathML source) with some anion vacancies. The compound is isostructural with ReO3. The U-O bond distance of 2·073 Å agrees with that predicted by Zachariasen for a bond strength S = 1.[27]

Reactivity

[edit]

Uranium trioxide reacts at 400 °C with freon-12 to form chlorine, phosgene, carbon dioxide and uranium tetrafluoride. The freon-12 can be replaced with freon-11 which forms carbon tetrachloride instead of carbon dioxide. This is a case of a hard perhalogenated freon which is normally considered to be inert being converted chemically at a moderate temperature.[28]

2 CF2Cl2 + UO3 → UF4 + CO2 + COCl2 + Cl2
4 CFCl3 + UO3 → UF4 + 3 COCl2 + CCl4 + Cl2

Uranium trioxide can be dissolved in a mixture of tributyl phosphate and thenoyltrifluoroacetone in supercritical carbon dioxide, ultrasound was employed during the dissolution.[29]

Electrochemical modification

[edit]

The reversible insertion of magnesium cations into the lattice of uranium trioxide by cyclic voltammetry using a graphite electrode modified with microscopic particles of the uranium oxide has been investigated. This experiment has also been done for U3O8. This is an example of electrochemistry of a solid modified electrode, the experiment which used for uranium trioxide is related to a carbon paste electrode experiment. It is also possible to reduce uranium trioxide with sodium metal to form sodium uranium oxides.[30]

It has been the case that it is possible to insert lithium[31][32][33] into the uranium trioxide lattice by electrochemical means, this is similar to the way that some rechargeable lithium ion batteries work. In these rechargeable cells one of the electrodes is a metal oxide which contains a metal such as cobalt which can be reduced, to maintain the electroneutrality for each electron which is added to the electrode material a lithium ion enters the lattice of this oxide electrode.

[edit]

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

As an acid

[edit]
UO3 + H2O → UO2−
4 + 2 H+

Dissolving uranium oxide in a strong base like sodium hydroxide forms the doubly negatively charged uranate anion (UO2−
4). Uranates tend to concatenate, forming diuranate, U
2O2−
7, or other poly-uranates. Important diuranates include ammonium diuranate ((NH4)2U2O7), sodium diuranate (Na2U2O7) and magnesium diuranate (MgU2O7), which forms part of some yellowcakes. It is worth noting that uranates of the form M2UO4 do not contain UO2−
4 ions, but rather flattened UO6 octahedra, containing a uranyl group and bridging oxygens.[34]

As a base

[edit]
UO3 + H2O → UO2+
2 + 2 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)2·6H2O) is soluble in ethers, alcohols, ketones and esters; for example, tributylphosphate. This solubility is used to separate uranium from other elements in nuclear reprocessing, which begins with the dissolution of nuclear fuel rods in nitric acid to form this salt. 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.

Uranium oxides in ceramics

[edit]

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.

References

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  1. ^ a b Zumdahl SS (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
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  20. ^ Spano T, Hunt R, Kapsimalis R, Niedziela J, Shields A, Miskowiec A (2022). "Optical vibrational spectra and proposed crystal structure of ε-UO3". Journal of Nuclear Materials. 559: 153386. doi:10.1016/j.jnucmat.2021.153386. OSTI 1843704. S2CID 244423124.
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  26. ^ Pyykkö P, Li J (1994). "Quasirelativistic pseudopotential study of species isoelectronic to uranyl and the equatorial coordination of uranyl". Journal of Physical Chemistry. 98 (18): 4809–4813. doi:10.1021/j100069a007.
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  31. ^ Dickens PG, Lawrence SD, Penny DJ, Powell AV (1989). "Insertion compounds of uranium oxides". Solid State Ionics. 32–33: 77–83. doi:10.1016/0167-2738(89)90205-1.
  32. ^ Dickens PG, Hawke SV, Weller MT (1985). "Lithium insertion into αUO3 and U3O8". Materials Research Bulletin. 20 (6): 635–641. doi:10.1016/0025-5408(85)90141-2.
  33. ^ Dickens PG, Hawke SV, Weller MT (1984). "Hydrogen insertion compounds of UO3". Materials Research Bulletin. 19 (5): 543–547. doi:10.1016/0025-5408(84)90120-X.
  34. ^ Cotton S (1991). Lanthanides and Actinides. New York: Oxford University Press. p. 128. ISBN 978-0-19-507366-9.
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