Uranium dioxide

Names
IUPAC names

Uranium dioxide
Uranium(IV) oxide

Other names

Urania
Uranous oxide

Identifiers

CAS Number

* 1344-57-6 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 10454 Y

EC Number |

* 215-700-3

PubChem CID

* 10916

RTECS number |

* YR4705000

UNII |

* L70487KUZO Y

InChI

* InChI=1S/2O.U

Key: FCTBKIHDJGHPPO-UHFFFAOYSA-N

SMILES

* O=[U]=O

Properties

Chemical formula

| UO2
Molar mass | 270.03 g/mol
Appearance  | black powder
Density | 10.97 g/cm3
Melting point |  2,865 °C (5,189 °F; 3,138 K)

Solubility in water

| insoluble
Structure

Crystal structure

| Fluorite (cubic), cF12

Space group

| Fm3m, No. 225

Lattice constant

a = 547.1 pm [1]

Coordination geometry

| Tetrahedral (O2−); cubic (UIV)
Thermochemistry

Std molar
entropy (S ~~o~~ 298)

| 78 J·mol−1·K−1[2]

Std enthalpy of
formation (ΔfH⦵298)

| −1084 kJ·mol−1[2]
Hazards
Safety data sheet | ICSC 1251
GHS pictograms |
GHS Signal word | Danger

GHS hazard statements

| H300, H330, H373, H410

GHS precautionary statements

| P260, P264, P270, P271, P273, P284, P301+310, P304+340, P310, P314, P320, P321, P330, P391, P403+233, P405, P501
NFPA 704 (fire diamond)  |

Flash point | N/A
Related compounds

Other anions

| Uranium(IV) sulfide
Uranium(IV) selenide

Other cations

| Protactinium(IV) oxide
Neptunium(IV) oxide

Related uranium oxides

| Triuranium octoxide
Uranium trioxide

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Uranium dioxide or uranium(IV) oxide (UO
2), also known as urania or uranous 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. It has been used as an orange, yellow, green, and black color in ceramic glazes and glass.

## Contents

* 1 Production
* 2 Chemistry
* 2.1 Structure
* 2.2 Oxidation
* 2.3 Reaction with carbon
* 3 Uses
* 3.1 Nuclear fuel
* 3.2 Color for glass ceramic glaze
* 3.3 Other uses
* 3.4 Semiconductor properties
* 4 Health dangers
* 5 See also
* 6 References
* 7 Further reading
* 8 External links

## Production

Uranium dioxide is produced by reducing uranium trioxide with hydrogen. This reaction often creates triuranium octoxide as an intermediate.[3][4][5]

UO3 \+ H2 → UO2 \+ H2O at 700 °C (973 K)

This reaction plays an important part in the creation of nuclear fuel through nuclear reprocessing and uranium enrichment.[5]

## Chemistry

### Structure

The solid is isostructural with (has the same structure as) fluorite (calcium fluoride), where each U is surrounded by eight O nearest neighbors in a cubic arrangement. In addition, the dioxides of cerium, thorium, and the transuranic elements from neptunium through californium have the same structures.[6] No other elemental dioxides have the fluorite structure. Upon melting, the measured average U-O coordination reduces from 8 in the crystalline solid (UO8 cubes), down to 6.7±0.5 (at 3270 K) in the melt.[7] Models consistent with these measurements show the melt to consist mainly of UO6 and UO7 polyhedral units, where roughly ​2⁄3 of the connections between polyhedra are corner sharing and ​1⁄3 are edge sharing.[7]

* Uranium dioxide

* Sintered uranium dioxide pellet

### Oxidation

Uranium dioxide is oxidized in contact with oxygen to form triuranium octoxide:[8]

3 UO2 \+ O2 → U3O8 at 250 °C (523 K)

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.[clarification needed] See spent nuclear fuel for further details. Water increases the oxidation rate of plutonium and uranium metals.[9]

### Reaction with carbon

Uranium dioxide reacts with carbon at high temperatures, forming uranium carbide and carbon monoxide.[10]

2 \+ 4 C → UC
2 \+ 2 CO

This process must be done under an inert gas as uranium carbide is easily oxidized back into uranium oxide.

## Uses

### 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), in the form of fuel rods in nuclear reactors.[11]

The thermal conductivity of uranium dioxide is very low when compared with elemental uranium, uranium nitride, uranium carbide and zircaloy cladding material as well as most uranium-based alloys.[12][13][14] This low thermal conductivity can result in localised overheating in the centres of fuel pellets.[15]

The thermal conductivity of zirconium metal and uranium dioxide as a function of temperature

* Uranium oxide fuel pellet

* Starting material containers for uranium dioxide fuel pellet production at a plant in Russia

### Color for glass ceramic glaze

File:FiestaWare Velleman-K2645 GeigerCounter.ogvGeiger counter (kit without housing) audibly reacting to an orange Fiestaware shard.

Uranium oxide (urania) was used to color glass and ceramics prior to World War II, and until the applications of radioactivity were discovered this was its main use. In 1958 the military in both the US and Europe allowed its commercial use again as depleted uranium, and its use began again on a more limited scale. Urania-based ceramic glazes are dark green or black when fired in a reduction or when UO2 is used; more commonly it is used in oxidation to produce bright yellow, orange and red glazes.[16] Orange-colored Fiestaware is a well-known example of a product with a urania-colored glaze.[17] Uranium glass is pale green to yellow and often has strong fluorescent properties.[18] Urania has also been used in formulations of enamel and porcelain.[19] It is possible to determine with a Geiger counter if a glaze or glass produced before 1958 contains urania.

### Other uses

Prior to the realisation of the harmfulness of radiation, uranium was included in false teeth and dentures, as its slight fluorescence made the dentures appear more like real teeth in a variety of lighting conditions.[20]

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.[21] 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.[22]

Depleted uranium dioxide can be also used as a catalyst, e.g. 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.[23]

The use of uranium dioxide as a material for rechargeable batteries is being investigated.[24] The batteries could have a high power density and a reduction potential of -4.7 V per cell.[25] Another investigated application is in photoelectrochemical cells for solar-assisted hydrogen production where UO2 is used as a photoanode. In earlier times, uranium dioxide was also used as heat conductor for current limitation (URDOX-resistor), which was the first use of its semiconductor properties. Uranium dioxide displays strong piezomagnetism in the antiferromagnetic state, observed at cryogenic temperatures below 30 kelvins. Accordingly, the linear magnetostriction found in UO2 changes sign with the applied magnetic field and exhibits magnetoelastic memory switching phenomena at record high switch-fields of 180,000 Oe.[26] The microscopic origin of the material magnetic properties lays in the face-centered-cubic crystal lattice symmetry of uranium atoms, and its response to applied magnetic fields.[27]

### Semiconductor properties

The band gap of uranium dioxide is comparable to those of 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.[28]

The dielectric constant of uranium dioxide is about 21.5,[29] which is almost twice as high as of silicon (11.7)[30] and GaAs (12.4).[31] This is an advantage over Si and GaAs in the construction of integrated circuits, as it may allow higher density integration with higher breakdown voltages and with lower susceptibility to the CMOS tunnelling breakdown.[32]

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)[32] and the −170 μV/K (n-type) / 160 μV/K (p-type) of bismuth telluride,[33] other materials promising for thermoelectric power generation applications[32] and Peltier elements. The radioactive decay impact of the 235U and 238U on its semiconducting properties was not measured as of 2005[update]. 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 high-performance integrated circuits. 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.[32]

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.[32]

Uranium dioxide is also resistant to radiation damage,[32] making it useful for rad-hard devices for special military and aerospace applications.[32]

A Schottky diode of U3O8 and a p-n-p transistor of UO2 were successfully manufactured in a laboratory.[34]

## Health dangers

Uranium dioxide is dangerous in two ways: heavy metal toxicity, and radiation. Uranium dioxide decays primarily by emission of alpha particles and gamma radiation, which is cumulatively dangerous to biologic organisms including animals and humans. It can be severely toxic or even fatal if swallowed, inhaled, absorbed through the skin and eyes.[35]

If inhaled, short term effects include irreversible kidney damage or acute necrotic arterial lesions. Inhalation of large particles of uranium materials or chronic exposure to uranium powders may result in radiation damage to internal tissues, especially the lungs and bones. Long term, in addition to effects from short term exposure, damage may include pulmonary fibrosis and malignant pulmonary neoplasia, anemia and blood disorders, liver damage, bone effects, sterility, and cancers. Skin contact with uranium powders may result in dermatitis. If ingested, it may cause kidney damage or acute necrotic arterial lesions. Ingestion may also affect the liver, and cause radiation damage to internal tissues.[35]

## See also

* Cleveite
* Ducrete
* Uranium oxide
* Uranium glass
* Uranium tile

## References

1. ↑ Leinders, Gregory; Cardinaels, Thomas; Binnemans, Koen; Verwerft, Marc (2015). "Accurate lattice parameter measurements of stoichiometric uranium dioxide". Journal of Nuclear Materials 459: 135–42. doi:10.1016/j.jnucmat.2015.01.029. Bibcode: 2015JNuM..459..135L. https://zenodo.org/record/884499.
2. ↑ 2.0 2.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.
3. ↑ A.H. Le Page; A.G. Fane (1974). "The kinetics of hydrogen reduction of UO3 and U3O8 derived from ammonium diuranate". Journal of Inorganic and Nuclear Chemistry 36 (1): 87–92. doi:10.1016/0022-1902(74)80663-9.
4. ↑ Notz, K.J.; Huntington, C.W.; Burkhardt, W. (1 July 1962). "Hydrogen Reduction of Uranium Oxides. A Phase Study by Means of a Controlled-Atmosphere Diffractometer Hot Stage". Industrial & Engineering Chemistry Process Design and Development 1 (3): 213–217. doi:10.1021/i260003a010.
5. ↑ 5.0 5.1 "Conversion and Deconversion". 20 Nov 2024. https://world-nuclear.org/information-library/nuclear-fuel-cycle/conversion-enrichment-and-fabrication/conversion-and-deconversion.
6. ↑ Petit, L.; Svane, A.; Szotek, Z.; Temmerman, W. M.; Stocks, G. M. (2010-01-07). "Electronic structure and ionicity of actinide oxides from first principles". Physical Review B 81 (4). doi:10.1103/PhysRevB.81.045108. Bibcode: 2010PhRvB..81d5108P. https://link.aps.org/doi/10.1103/PhysRevB.81.045108.
7. ↑ 7.0 7.1 Skinner, L. B.; Benmore, C. J.; Weber, J. K. R.; Williamson, M. A.; Tamalonis, A.; Hebden, A.; Wiencek, T.; Alderman, O. L. G. et al. (2014). "Molten uranium dioxide structure and dynamics". Science 346 (6212): 984–7. doi:10.1126/science.1259709. PMID 25414311. Bibcode: 2014Sci...346..984S. https://www.osti.gov/biblio/1174101.
8. ↑ G. Rousseau; L. Desgranges; F. Charlot; N. Millot; J.C. Nièpce; M. Pijolat; F. Valdivieso; G. Baldinozzi et al. (2006). "A detailed study of UO2 to U3O8 oxidation phases and the associated rate-limiting steps". Journal of Nuclear Materials 355 (1–3): 10–20. doi:10.1016/j.jnucmat.2006.03.015.
9. ↑ Haschke, John M; Allen, Thomas H; Morales, Luis A (2001). "Reactions of plutonium dioxide with water and hydrogen–oxygen mixtures: Mechanisms for corrosion of uranium and plutonium". Journal of Alloys and Compounds 314 (1–2): 78–91. doi:10.1016/S0925-8388(00)01222-6.
10. ↑ Buchel, Gerald L. (1963). Equilibrium studies of the uranium dioxide - carbon and neodymium sesquioxide - carbon systems (M.S. thesis). Michigan State University.
11. ↑ "Mixed Oxide (MOX) Fuel". 10 Oct 2017. https://world-nuclear.org/information-library/nuclear-fuel-cycle/fuel-recycling/mixed-oxide-fuel-mox.
12. ↑ Peakman, Aiden; Rossiter, Glyn (2024). "Incorporation of uranium nitride fuel capability into the ENIGMA fuel performance code: Model development and validation". Nuclear Engineering and Design 429. doi:10.1016/j.nucengdes.2024.113604. ISSN 0029-5493. Bibcode: 2024NuEnD.42913604P.
13. ↑ Dr. Celine Hin. "Thermal Conductivity of Metallic Uranium". https://www.osti.gov/servlets/purl/1433931.
14. ↑ R. R. Hammer (September 1967). "Zircaloy-4, Uranium Dioxide, and Materials Formed by their Interaction: A Literature Review with Extrapolation of Physical Properties to High Temperatures". Idaho Nuclear Corporation. https://www.osti.gov/servlets/purl/4136888.
15. ↑ "Thermal Conductivity of Uranium Dioxide". https://www.nuclear-power.com/nuclear-engineering/heat-transfer/thermal-conduction/thermal-conductivity/thermal-conductivity-of-uranium-dioxide/.
16. ↑ Örtel, Stefan. Uran in der Keramik. Geschichte - Technik - Hersteller. http://www.uranglasuren.com/.
17. ↑ Radon, Health and Natural Hazards, Editors: G.K. Gillmore, F.E. Perrier, R.G.M. Crockett, pp. 50-52, 2018, Geological Society of London, ISBN 1786203081, 9781786203083, Google Books
18. ↑ Amber Davis (22 Jan 2025). "A 'glowing' review of uranium glass". Oak Ridge Associated Universities. https://www.orau.org/blog/museum/a-glowing-review-of-uranium-glass.html.
19. ↑ Donna Strahan (19 Jul 2013). "Uranium in glass, glazes and enamels: history, identification and handling". Studies in Conservation 46 (3): 181–195. doi:10.1179/sic.2001.46.3.181.
20. ↑ Toor, R. S. S.; Brar, G. S. (2012). "Uranium: A Dentist's perspective". Journal of International Society of Preventive and Community Dentistry 2 (1): 1–7. doi:10.4103/2231-0762.103447. PMID 24478959.
21. ↑ Lessing, Paul A. (1 Mar 1995). ﻿Development of "DUCRETE"﻿ (Report). Idaho National Engineering Laboratory. doi:10.2172/366558. https://digital.library.unt.edu/ark:/67531/metadc676180/.
22. ↑ Forsberg, Charles W.; Swaney, Paul M.; Tiegs, Terry N.. Characteristics and Fabrication of Cermet Spent Nuclear Fuel Casks: Ceramic Particles Embedded in Steel. 14th International Symposium on the Packaging and Transportation of Radioactive Materials (PATRAM 2004). https://www.osti.gov/etdeweb/servlets/purl/20773271
23. ↑ Hutchings, Graham J.; Heneghan, Catherine S.; Hudson, Ian D.; Taylor, Stuart H. (1996). "Uranium-oxide-based catalysts for the destruction of volatile chloro-organic compounds". Nature 384 (6607): 341–3. doi:10.1038/384341a0. Bibcode: 1996Natur.384..341H.
24. ↑ Wu, Binbin; Yu, Jianguo (10 Jun 2013). "From Used Oxide Nuclear Fuel to Rechargeable Battery: A First-Principles Study". MRS Proceedings 1541. doi:10.1557/opl.2013.732.
25. ↑ Dunbar, Paul; Lee-Desautels, Rhonda. "Initial Development of a Depleted Uranium Battery". University of Kentucky. https://scholars.uky.edu/en/projects/initial-development-of-a-depleted-uranium-battery.
26. ↑ Jaime, Marcelo; Saul, Andres; Salamon, Myron B.; Zapf, Vivien; Harrison, Neil; Durakiewicz, Tomasz; Lashley, Jason C.; Andersson, David A. et al. (2017). "Piezomagnetism and magnetoelastic memory in uranium dioxide.". Nature Communications 8 (1): 99. doi:10.1038/s41467-017-00096-4. PMID 28740123. Bibcode: 2017NatCo...8...99J.
27. ↑ Antonio, Daniel J.; Weiss, Joel T.; Shanks, Katherine S.; Ruff, Jacob P.C.; Jaime, Marcelo; Saul, Andres; Swinburne, Thomas; Salamon, Myron B. et al. (2021). "Piezomagnetic switching and complex phase equilibria in uranium dioxide.". Communications Materials 2 (1): 17. doi:10.1038/s43246-021-00121-6. Bibcode: 2021CoMat...2...17A.
28. ↑ An, Yong Q.; Taylor, Antoinette J.; Conradson, Steven D.; Trugman, Stuart A.; Durakiewicz, Tomasz; Rodriguez, George (2011). "Ultrafast Hopping Dynamics of 5f Electrons in the Mott Insulator UO2 Studied by Femtosecond Pump-Probe Spectroscopy". Physical Review Letters 106 (20). doi:10.1103/PhysRevLett.106.207402. PMID 21668262. Bibcode: 2011PhRvL.106t7402A.
29. ↑ Hampton, R. N.; Saunders, G. A.; Harding, J. H.; Stoneham, A. M. (1 Sep 1987). "The pressure dependence of the dielectric constant and electrical conductivity of single crystal uranium dioxide". Journal of Nuclear Materials 150 (1): 17–23. doi:10.1016/0022-3115(87)90089-4. Bibcode: 1987JNuM..150...17H.
30. ↑ Yang, Xiaofan; Liu, Xiaoming; Yu, Shuo; Gan, Lu; Zhou, Jun; Zeng, Yonghu (Aug 2019). "Permittivity of Undoped Silicon in the Millimeter Wave Range". Electronics 8 (8): 886. doi:10.3390/electronics8080886.
31. ↑ Fox, Mark (2010). Optical Properties of Solids (2 ed.). Oxford University Press. p. 283. ISBN 978-0-19-957337-0. https://global.oup.com/academic/product/optical-properties-of-solids-9780199573370?lang=en&cc=no.
32. ↑ 32.0 32.1 32.2 32.3 32.4 32.5 32.6 Meek, Thomas; Hu, Michael; Haire, M. Jonathan (25 Feb – 1 Mar 2001). "Semiconductive Properties of Uranium Oxides" (DOC). Waste Management Symposium 2001. Tucson. https://archivedproceedings.econference.io/wmsym/2001/14/14-3.pdf. Retrieved 13 Apr 2025.
33. ↑ Goldsmid, H. Julian (28 Mar 2014). "Bismuth Telluride and Its Alloys as Materials for Thermoelectric Generation". Materials 7 (4): 2577–2592. doi:10.3390/ma7042577. PMID 28788584. Bibcode: 2014Mate....7.2577G.
34. ↑ Meek, Thomas T.; von Roedern, B. (2008). "Semiconductor devices fabricated from actinide oxides". Vacuum 83 (1): 226–8. doi:10.1016/j.vacuum.2008.04.005. Bibcode: 2008Vacuu..83..226M.
35. ↑ 35.0 35.1 "Safety Data Sheet: Uranium Dioxide". U. S. Department of Energy. June 23, 2020. https://www.energy.gov/nnsa/articles/sds-uranium-oxide-uo2.

## Further reading

* Barrett, S. A.; Jacobson, A. J.; Tofield, B. C.; Fender, B. E. F. (1982). "The preparation and structure of barium uranium oxide BaUO3+x". Acta Crystallographica Section B 38 (11): 2775. doi:10.1107/S0567740882009935. Bibcode: 1982AcCrB..38.2775B.

## External links

* Semiconducting properties of uranium oxides
* Free Dictionary Listing for Uranium Dioxide
* The Uranium dioxide International Bio-Analytical Industries, Inc.

* v
* t
* e

Uranium compounds

U(II)|

* UB2
* US

U(III)|

* UF3
* UCl3
* UI3
* UP
* U(OH)3
* UH3
* UN

| Organouranium(III) compounds|

* U(C5H5)3

|

U(IV)|

* U(BH4)4
* UCl4
* UF4
* UBr4
* UI4
* UO2
* USi2
* US2
* U(SO4)2

| Organouranium(IV) compounds|

* U(C8H8)2
* U(C5H5)4
* U(C5H5)3Cl

|

U(IV,V)|

* U2N3

U(V)|

* UCl5
* UF5
* UBr5
* UI5
* U2O5

U(V,VI)|

* U3O8

U(VI)|

* (NH4)2U2O7
* Na2U2O7
* UCl6
* UF6
* U(PO4)2
* UO3
* UO4
* UO2(CH3COO)2
* UO2(CHO2)2
* UO2CO3
* UO2CO3·2(NH4)2CO3
* UO2Cl2
* UO2F2
* UO2(NO3)2
* UO2(OH)2
* UO2(SO4)2
* ZnUO2(CH3COO)4
* UN2
* H2UO4
* UO6 (hypothetical)

U(XII)|

* UO6 (hypothetical)

* v
* t
* e

Oxides

Mixed oxidation states|

* Antimony tetroxide (Sb2O4)
* Cobalt(II,III) oxide (Co3O4)
* Europium(II,III) oxide (Eu3O4)
* Iron(II,III) oxide (Fe<sub>3O4)
* Lead(II,IV) oxide (Pb3O4)
* Manganese(II,III) oxide (Mn3O4)
* Silver(I,III) oxide (Ag2O2)
* Triuranium octoxide (U3O8)
* Carbon suboxide (C3O2)
* Mellitic anhydride (C12O9)
* [[Chemistry:Praseodymium(III,IV) Praseodymium(III,IV) oxide]] (Pr6O11)
* Terbium(III,IV) oxide (Tb4O7)

+1 oxidation state|

* Copper(I) oxide (Cu<sub>2O)
* Caesium oxide (Cs2O)
* Dicarbon monoxide (C2O)
* Dichlorine monoxide (Cl2O)
* Gallium(I) oxide (Ga2O)
* Lithium oxide (Li2O)
* Potassium oxide (K2O)
* Rubidium oxide (Rb2O)
* Silver oxide (Ag2O)
* Thallium(I) oxide (Tl2O)
* Sodium oxide (Na2O)
* Water (hydrogen oxide) (H2O)

+2 oxidation state|

* Aluminium(II) oxide (AlO)
* Barium oxide (BaO)
* Beryllium oxide (BeO)
* Cadmium oxide (CdO)
* Calcium oxide (CaO)
* Carbon monoxide (CO)
* Chromium(II) oxide (CrO)
* Cobalt(II) oxide (CoO)
* Copper(II) oxide (CuO)
* Europium(II) oxide (EuO)
* Germanium monoxide (GeO))
* Iron(II) oxide (FeO)
* Lead(II) oxide (PbO)
* Magnesium oxide (MgO)
* Manganese(II) oxide (MnO)
* Mercury(II) oxide (HgO)
* Nickel(II) oxide (NiO)
* Nitric oxide (NO)
* Palladium(II) oxide (PdO)
* Silicon monoxide (SiO)
* Strontium oxide (SrO)
* Sulfur monoxide (SO)
* Disulfur dioxide (S2O2)
* Thorium monoxide (ThO)
* Tin(II) oxide (SnO)
* Titanium(II) oxide (TiO)
* Vanadium(II) oxide (VO)
* Zinc oxide (ZnO)

+3 oxidation state|

* Aluminium oxide (Al<sub>2O3)
* Antimony trioxide (Sb2O3)
* Arsenic trioxide (As2O3)
* Bismuth(III) oxide (Bi2O3)
* Boron trioxide (B2O3)
* Cerium(III) oxide (Ce2O3)
* Dibromine trioxide (Br2O3)
* Chromium(III) oxide (Cr2O3)
* Dinitrogen trioxide (N2O3)
* Dysprosium(III) oxide (Dy2O3)
* Erbium(III) oxide (Er2O3)
* Europium(III) oxide (Eu2O3)
* Gadolinium(III) oxide (Gd2O3)
* Gallium(III) oxide (Ga2O3)
* Holmium(III) oxide (Ho2O3)
* Indium(III) oxide (In<sub>2O3)
* Iron(III) oxide (Fe2O3)
* Lanthanum oxide (La2O3)
* Lutetium(III) oxide (Lu2O3)
* Manganese(III) oxide (Mn2O3)
* Neodymium(III) oxide (Nd2O3)
* Nickel(III) oxide (Ni2O3)
* Phosphorus trioxide (P4O6)
* Praseodymium(III) oxide (Pr2O3)
* Promethium(III) oxide (Pm2O3)
* Rhodium(III) oxide (Rh2O3)
* [[Chemistry:Samarium(III) Samarium(III) oxide]] (Sm2O3)
* Scandium oxide (Sc2O3)
* Terbium(III) oxide (Tb2O3)
* Thallium(III) oxide (Tl2O3)
* Thulium(III) oxide (Tm2O3)
* Titanium(III) oxide (Ti2O3)
* Tungsten(III) oxide (W2O3)
* Vanadium(III) oxide (V2O3)
* Ytterbium(III) oxide (Yb2O3)
* Yttrium(III) oxide (Y2O3)

+4 oxidation state|

* Americium dioxide (AmO2)
* Carbon dioxide (CO2)
* Carbon trioxide (CO3)
* Cerium(IV) oxide (CeO2)
* Chlorine dioxide (ClO2)
* Chromium(IV) oxide (CrO<sub>2)
* Dinitrogen tetroxide (N2O4)
* Germanium dioxide (GeO<sub>2)
* [[Chemistry:Hafnium(IV) Hafnium(IV) oxide]] (HfO2)
* Lead dioxide (PbO2)
* Manganese dioxide (MnO2)
* Neptunium(IV) oxide (NpO2)
* Nitrogen dioxide (NO2)
* Osmium dioxide (OsO2)
* Plutonium(IV) oxide (PuO2)
* Praseodymium(IV) oxide (PrO2)
* Protactinium(IV) oxide (PaO2)
* Rhodium(IV) oxide (RhO2)
* Ruthenium(IV) oxide (RuO<sub>2)
* Selenium dioxide (SeO2)
* Silicon dioxide (SiO2)
* Sulfur dioxide (SO2)
* Tellurium dioxide (TeO<sub>2)
* [[Chemistry:Terbium(IV) Terbium(IV) oxide]] (TbO2)
* Thorium dioxide (ThO2)
* Tin dioxide (SnO2)
* Titanium dioxide (TiO<sub>2)
* Tungsten(IV) oxide (WO2)
* Uranium dioxide (UO2)
* Vanadium(IV) oxide (VO2)
* Zirconium dioxide (ZrO2)

+5 oxidation state|

* Antimony pentoxide (Sb2O5)
* Arsenic pentoxide (As2O5)
* Dinitrogen pentoxide (N2O5)
* Niobium pentoxide (Nb2O5)
* Phosphorus pentoxide (P2O5)
* Protactinium(V) oxide (Pa2O5)
* Tantalum pentoxide (Ta2O5)
* Vanadium(V) oxide (V2O5)

+6 oxidation state|

* Chromium trioxide (CrO3)
* Molybdenum trioxide (MoO3)
* Rhenium trioxide (ReO3)
* Selenium trioxide (SeO3)
* Sulfur trioxide (SO3)
* Tellurium trioxide (TeO3)
* Tungsten trioxide (WO3)
* Uranium trioxide (UO3)
* Xenon trioxide (XeO3)
* Iridium trioxide (IrO3)

+7 oxidation state|

* Dichlorine heptoxide (Cl2O7)
* Manganese heptoxide (Mn2O7)
* [[Chemistry:Rhenium(VII) Rhenium(VII) oxide]] (Re2O7)
* Technetium(VII) oxide (Tc2O7)

+8 oxidation state|

* Osmium tetroxide (OsO4)
* Ruthenium tetroxide (RuO4)
* Xenon tetroxide (XeO4)
* Iridium tetroxide (IrO4)
* Hassium tetroxide (HsO4)

Related|

* Oxocarbon
* Suboxide
* Oxyanion
* Ozonide
* Peroxide
* Superoxide

Oxides are sorted by oxidation state. Category:Oxides

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Original source: https://en.wikipedia.org/wiki/Uranium dioxide. Read more

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Retrieved from "https://handwiki.org/wiki/index.php?title=Chemistry:Uranium_dioxide&oldid=3839337"
*[CID]: Compound ID
*[H300]: Fatal if swallowed
*[H330]: Fatal if inhaled
*[H373]: May cause damage to organs through prolonged or repeated exposure
*[H410]: Very toxic to aquatic life with long lasting effects
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