Uranium dioxide: Wikis

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Uranium dioxide
UO2lattice.jpg
IUPAC name
Other names Urania
Uranous oxide
Identifiers
CAS number 1344-57-6 Yes check.svgY
RTECS number YR4705000
Properties
Molecular formula UO2
Molar mass 270.03 g/mol
Appearance black powder
Density 10.97 g/cm3
Melting point

2865 °C (3140 K)

Solubility in water insoluble
Structure
Crystal structure Fluorite (cubic), cF12
Space group Fm3m, No. 225
Coordination
geometry
Tetrahedral (O2–); cubic (UIV)
Hazards
MSDS ICSC 1251
EU Index 092-002-00-3
EU classification Very toxic (T+)
Dangerous for the environment (N)
R-phrases R26/28, R33, R51/53
S-phrases (S1/2), S20/21, S45, S61
Flash point Non-flammable
Related compounds
Related uranium oxides Triuranium octoxide
Uranium trioxide
 Yes check.svgY (what is this?)  (verify)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Uranium dioxide or uranium(IV) oxide (UO2), also known as urania or uranic oxide, is an oxide of uranium, and is a black, radioactive, crystalline powder that naturally occurs in the mineral uraninite. It is used in nuclear fuel rods in nuclear reactors. A mixture of uranium and plutonium dioxides is used as MOX fuel. Prior to 1960 it was used as yellow and black color in ceramic glazes and glass.

Contents

Production

Uranium dioxide is produced by reducing uranium trioxide with hydrogen.

UO3 + H2 → UO2 + H2O at 700 °C (970 K)

This reaction takes part in the reprocessing of nuclear fuel and enrichment of uranium for nuclear fuel.

Chemistry

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Structure

The solid is isostructural with (has the same structure as) fluorite (calcium fluoride). In addition, the dioxides of plutonium and neptunium have the same structures

Oxidation

Uranium dioxide is oxidized in contact with oxygen to the triuranium octaoxide.

3UO2 + O2 → U3O8 at 700 °C (970 K)

Aqueous electrochemistry

The electrochemistry of uranium dioxide has been investigated in detail as the galvanic corrosion of uranium dioxide controls the rate at which used nuclear fuel dissolves. See the spent nuclear fuel page for further details.

Oxidation of uranium metal

It has been reported that water causes the rate of the oxidation of both plutonium and uranium metal to increase when compared with the situation which exists when water is absent.[1]

Uses

Uranium oxide fuel pellet

Nuclear Fuel

UO2 is used mainly as nuclear fuel, specifically as UO2 or as a mixture of UO2 and PuO2 (plutonium dioxide) called a mixed oxide (MOX fuel) for fuel rods in nuclear reactors.

Note that the thermal conductivity of uranium dioxide is very low when compared with uranium, uranium nitride, uranium carbide and zirconium cladding material. This low thermal conductivity can result in localised overheating in the centres of fuel pellets. The graph below shows the different temperature gradients in different fuel compounds. For these fuels the thermal power density is the same and the diameter of all the pellets are the same.

Color for ceramics glaze

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

Prior to 1960, uranium oxides were used as colored glazes. It is possible to determine with a Geiger counter if a glaze or glass contains uranium oxides.

Other use

Depleted UO2 (DUO2) can be used as a material for radiation shielding. For example, DUCRETE is a "heavy concrete" material where gravel is replaced with uranium dioxide aggregate; this material is investigated for use for casks for radioactive waste. Casks can be also made of DUO2-steel cermet, a composite material made of an aggregate of uranium dioxide serving as radiation shielding, graphite and/or silicon carbide serving as neutron radiation absorber and moderator, and steel as the matrix, whose high thermal conductivity allows easy removal of decay heat.

Depleted uranium dioxide can be also used as a catalyst, eg. for degradation of volatile organic compounds in gaseous phase, oxidation of methane to methanol, and removal of sulfur from petroleum. It has high efficiency and long-term stability when used to destroy VOCs when compared with some of the commercial catalysts, such as precious metals, TiO2, and Co3O4 catalysts. Much research is being done in this area, DU being favoured for the uranium component due to its low radioactivity. [1] Use of uranium dioxide as a material for rechargeable batteries is investigated. The batteries could have high power density and potential of 4.7V per cell.

Another investigated application is in photoelectrochemical cells, for solar-assisted hydrogen production. UO2 is used as a photoanode.

In earlier times it was also used as heat conductor for current limitation ( URDOX-resistor), which was the first use of its semiconductor properties.

Semiconductor properties

Uranium dioxide is a semiconductor material. Its band gap is about 1.3 eV, which lies between the band gap for silicon and gallium arsenide, near the optimum for efficiency vs band gap curve for absorption of solar radiation, suggesting its possible use for very efficient solar cells based on Schottky diode structure; it also absorbs at five different wavelengths, including infrared, further enhancing its efficiency. Its intrinsic conductivity at room temperature is about the same as of single crystal silicon.

In earlier time it was used as material conducting in the heat ( URDOX-resistor).

Its dielectric constant is about 22, which is almost twice as high as of silicon (11.2) and GaAs (14.1), which poses an advantage over Si and GaAs for construction of integrated circuits, as it may allow higher density integration with higher breakdown voltages and with lower susceptibility to the CMOS tunneling breakdown.

The Seebeck coefficient of uranium dioxide at room temperature is about 750 µV/K, a value significantly higher than the 270 µV/K of thallium tin telluride (Tl2SnTe5) and thallium germanium telluride (Tl2GeTe5) and of bismuth-tellurium alloys, other materials promising for thermopower applications and Peltier elements.

The radioactive decay impact of the235U and238U on its semiconducting properties was not measured as of 2005. Due to the slow decay rate of these isotopes, it should not meaningfully influence the properties of uranium dioxide solar cells and thermoelectric devices, but it may become an important factor for VLSI chips. Use of depleted uranium oxide is necessary for this reason. The capture of alpha particles emitted during radioactive decay as helium atoms in the crystal lattice may also cause gradual long-term changes in its properties.

The stoichiometry of the material dramatically influences its electrical properties. For example, the electrical conductivity of UO1.994 is orders of magnitude lower at higher temperatures than the conductivity of UO2.001.

Uranium dioxide, like U3O8, is a ceramic material capable of withstanding high temperatures (about 2300 °C, in comparison with at most 200 °C for silicon or GaAs), making it suitable for high-temperature applications like thermophotovoltaic devices.

Uranium dioxide is also resistant to radiation damage, making it useful for rad-hard devices for special military and aerospace applications.

A Schottky diode of U3O8 and a p-n-p transistor of UO2 were successfully manufactured in a laboratory.

Toxicity

Uranium dioxide is known to be absorbed by phagocytosis in the lungs.[2]

See also

References

  1. ^ Barrett SA, Jacobson AJ, Tofield BC, Fender BEF (1982). "The preparation and structure of barium uranium oxide BaUO3+x". Acta Crystallographica B 38: 2775–2781. doi:10.1107/S0567740882009935.   DOI
  2. ^ Hutchings GJ (1996). "A Uranium-Oxide-Based Catalysts for the Destruction of Volatile Chloro-Organic compounds". Nature 384: 341–343. doi:10.1038/384341a0.  

External links


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