User:LossIsNotMore/Uranium trioxide

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, γ-UO3, is a yellow-orange powder.

Uranium trioxide is a product of uranium metal combustion and corrosion. It is a poisonous genotoxin and teratogen in all its forms.

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


 * 1) U3O8 can be oxidized at 500°C with oxygen. Note that above 750°C even in 5 Atm O{{sub|2 UO 3 decomposes into U 3 O 8.
 * 2) Uranyl nitrate, (UO{{sub|2}}(NO3){{sub|2}}·6H{{sub|2}}O) can be heated to yield UO{{sub|3}}.  This occurs during the reprocessing of nuclear fuel.  Fuel rods are dissolved in HNO{{sub|3}} to separate uranyl nitrate from plutonium and the fission products (the PUREX method).  The pure uranyl nitrate is converted to solid UO{{sub|3}} 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 (Na{{sub|2}}U{{sub|2}}O{{sub|7}}·6H{{sub|2}}O) 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.



Uranium trioxide is shipped between processing facilities in the form of a gel.

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 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.

During nuclear fuel fabrication or reprocessing stages of a nuclear fuel cycle, it is possible for small particles of uranium oxides including UO3 to escape into the environment. The extent of immediate inhalation intake of uranium oxides is inversely proportional to the size of particles inhaled; uranium oxide gases are absorbed immediately into the bloodstream. Urine assay for UO3 exposure can be useful, provided that measurements are made soon after a known acute intake. Treatment for UO3 inhalation primarily involves decorporation therapy.

Solid state structure
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 200–650 °C. Heating at 700 °C under H2 gives dark brown uranium dioxide (UO2), which is used in MOX nuclear fuel rods.

High pressure form
There is a high-pressure solid form with U 2 O 2 and U 3 O 3 rings in it.

Hydrates
Several hydrates of uranium trioxide are known, e.g., UO3•6H2O.

Molecular forms
While uranium trioxide is mostly encountered as a polymeric solid, work has been done on molecular forms in inert gas matrices and in the vapor phase, too.

Gas phase
Uranium trioxide is produced when uranium burns. Uranyl ion contamination in uranium oxides has been detected in the residue of depleted uranium munitions fires.

At elevated temperatures gaseous UO3 and O2 are in equilibrium with solid U3O8.


 * 1/3 U3O8(s) + 1/6 O2(g) $$\overrightarrow{\gets}$$ UO3(g)

With increasing temperature the equilibrium is shifted to the right. This system has been studied at temperatures between 900 °C and 2200 Kelvin. The vapor pressure of monomeric UO3 is low but appreciable, about 10&minus;5 mbar (1 mPa) at 980 °C, rising to 0.1 mbar (10 Pa) at 1400 °C, 0.34 mbar (34 Pa) at 1800 K, 1.9 mbar (193 Pa) at 2000 K, and 8.1 mbar (809 Pa) at 2200 K.  Small pieces of uranium burn at temperatures exceeding 2500 Kelvin.

Matrix isolation


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. From the force constants the authors deduct the U-O bond lengths to be between 1.76 and 1.79 angstroms (176 to 179 picometers).

Calculations indicate that the point group of gaseous 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.

Reactivity
Uranium trioxide reacts at 400 °C with freon-12 to form chlorine, phosgene, carbon dioxide and uranium(IV) fluoride. 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.

2 CF 2 Cl 2 + UO 3 → UF 4 + CO 2 + COCl 2 + Cl 2

4 CF 2 Cl 2 + UO 3 → UF 4 + 3COCl 2 + CCl 4 + Cl 2

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

Corrosion of uranium metal
It has been reported that the corrosion of uranium in a silica rich aqueous solution forms both uranium dioxide and uranium trioxide. Reports on the corrosion of uranium metal have been published by the Royal Society.

Electrochemistry
The reversible insertion of magnesium cations into the lattice of uranium trioxide by cyclic voltammetry using a graphite electrode modifed 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 modifed 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. The Journal of Solid State Electrochemistry is devoted to this type of electrochemistry.

It has been the case that it is possible to insert lithium ions and protons 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. (Li+) (H+)

Uranium oxides 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 → UO42− + H+

Dissolving uranium oxide in a strong base like sodium hydroxide forms the doubly negatively charged uranate anion (UO42−). Uranates tend to agglomerate, forming diuranate, U2O7 2− or other poly-uranates. Important diuranates include ammonium diuranate ((NH4 ) 2U2 O 7 ), sodium diuranate (Na 2U2O7) and magnesium diuranate (MgU2O7), which forms part of some yellowcakes. It is worth noting that uranates of the form M2UO4 do not contain UO42− ions, but rather flattened UO6 octahedra, containing a uranyl group and bridging oxygens.


 * As a base:


 * UO3 + H2O → UO22+ + 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.