# Cerium(IV) oxide

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For the other compound also known as cerium oxide, see [Cerium(III) oxide](/source/Cerium(III)_oxide).

Cerium(IV) oxide Cerium(IV) oxide Names IUPAC name Cerium(IV) oxide Other names Ceric oxide, Ceria, Cerium dioxide Identifiers CAS Number 1306-38-3 Y 23322-64-7 (hydrate) Y 3D model (JSmol) Interactive image ChEBI CHEBI:79089 N ChemSpider 8395107 Y ECHA InfoCard 100.013.774 PubChem CID 73963 UNII 619G5K328Y N 20GT4M7CWG (hydrate) Y CompTox Dashboard (EPA) DTXSID4040214 InChI InChI=1S/Ce.2O/q+4;2*-2 Y Key: OFJATJUUUCAKMK-UHFFFAOYSA-N Y InChI=1/Ce.2O/q+4;2*-2 Key: OFJATJUUUCAKMK-UHFFFAOYAX SMILES [O-2]=[Ce+4]=[O-2] Properties Chemical formula CeO2 Molar mass 172.115 g/mol Appearance white or pale yellow solid, slightly hygroscopic Density 7.215 g/cm3 Melting point 2,400 °C (4,350 °F; 2,670 K) Boiling point 3,500 °C (6,330 °F; 3,770 K) Solubility in water insoluble Magnetic susceptibility (χ) +26.0·10−6 cm3/mol Structure Crystal structure cubic crystal system, cF12 (fluorite)[1] Space group Fm3m, #225 Lattice constant a = 5.41 Å [2], b = 5.41 Å, c = 5.41 Å α = 90°, β = 90°, γ = 90° Coordination geometry Ce, 8, cubic O, 4, tetrahedral Hazards NFPA 704 (fire diamond) 1 0 0 Related compounds Related compounds Cerium(III) oxide 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

Chemical compound

**Cerium(IV) oxide**, also known as **ceric oxide**, **ceric dioxide**, **ceria**, **cerium oxide** or **cerium dioxide**, is an [oxide](/source/Oxide) of the [rare-earth metal](/source/Rare-earth_metal) [cerium](/source/Cerium). It is a pale yellow-white powder with the chemical formula CeO2. It is an important commercial product and an intermediate in the purification of the element from the ores.[3] The distinctive property of this material is its reversible conversion to a [non-stoichiometric oxide](/source/Non-stoichiometric_compound).

## Production

[Cerium](/source/Cerium) occurs naturally as oxides, always as a mixture with other rare-earth elements. Its principal ores are [bastnaesite](/source/Bastnaesite) and [monazite](/source/Monazite). After extraction of the metal ions into aqueous base, Ce is separated from that mixture by addition of an oxidant followed by adjustment of the pH. This step exploits the low solubility of CeO2 and the fact that other rare-earth elements resist oxidation.[3]

Cerium(IV) oxide is formed by the [calcination](/source/Calcination) of [cerium oxalate](/source/Cerium_oxalate) or [cerium hydroxide](/source/Cerium_hydroxide).

Cerium also forms [cerium(III) oxide](/source/Cerium(III)_oxide), Ce 2O 3, which oxidizes in air to cerium(IV) oxide.[3][4]

## Structure and defect behavior

Cerium oxide adopts the [fluorite structure](/source/Fluorite_structure), space group Fm3m, #225 containing 8-coordinate Ce4+ and 4-coordinate O2−. At high temperatures it releases oxygen to give a [non-stoichiometric, anion deficient form](/source/Nonstoichiometric_compound) that retains the fluorite lattice.[5] This material has the formula CeO(2−*x*), where 0 < *x* < 0.28.[6] The value of *x* depends on both the temperature, surface termination and the oxygen partial pressure. The equation

- x 0.35 − x = ( 106 000 Pa P O 2 ) 0.217 exp ⁡ ( − 195.6 kJ/mol R T ) {\displaystyle {\frac {x}{0.35-x}}=\left({\frac {106\,000{\text{ Pa}}}{P_{\mathrm {O} _{2}}}}\right)^{0.217}\exp \left({\frac {-195.6{\text{ kJ/mol}}}{RT}}\right)}

has been shown to predict the equilibrium non-stoichiometry *x* over a wide range of oxygen partial pressures (103–10−4 Pa) and temperatures (1000–1900 °C).[7]

The non-stoichiometric form, which has a blue to black appearance, exhibits both ionic and electronic conduction with ionic being the most significant at temperatures > 500 °C.[8]

The number of oxygen vacancies is frequently measured by using [X-ray photoelectron spectroscopy](/source/X-ray_photoelectron_spectroscopy) to compare the ratio of Ce3+ to Ce4+ .

The loss of oxygen continues into the molten liquid state where the local Ce-O coordination number drops to predominantly 6-fold, compared to 8-fold in the stoichiometric fluorite structure. This has been shown to be directly analogous to plutonium oxides, once differences in oxygen potential are accounted for.[9]

### Defect chemistry

In the most stable [fluorite](/source/Fluorite_structure) phase of ceria, it exhibits several defects depending on partial pressure of oxygen or stress state of the material.[10][11][12][13]

The primary defects of concern are oxygen vacancies and small [polarons](/source/Polaron) (electrons localized on cerium cations). Increasing the concentration of oxygen defects increases the diffusion rate of oxide anions in the lattice as reflected in an increase in [ionic conductivity](/source/Ionic_conductivity_(solid_state)). These factors give ceria favorable performance in applications as a solid electrolyte in [solid-oxide fuel cells](/source/Solid-oxide_fuel_cell). Undoped and doped ceria also exhibit high electronic conductivity at low partial pressures of oxygen due to reduction of the cerium ion leading to the formation of small [polarons](/source/Polaron). Since the oxygen atoms in a ceria crystal occur in planes, diffusion of these anions is facile. The diffusion rate increases as the defect concentration increases.[*[citation needed](https://en.wikipedia.org/wiki/Wikipedia:Citation_needed)*]

## Natural occurrence

Cerium(IV) oxide occurs naturally as the mineral [cerianite-(Ce)](/source/Cerianite-(Ce)).[14][15] It is a rare example of tetravalent cerium mineral, the other examples being [stetindite-(Ce)](https://en.wikipedia.org/w/index.php?title=Stetindite-(Ce)&action=edit&redlink=1) and [dyrnaesite-(La)](/source/Dyrnaesite-(La)). The "-(Ce)" suffix is known as Levinson modifier and is used to show which element dominates in a particular site in the structure.[16] It is often found in names of minerals bearing [rare earth elements](/source/Rare_earth_elements) (REEs). Occurrence of cerianite-(Ce) is related to some examples of [cerium anomaly](/source/Cerium_anomaly), where Ce - which is oxidized easily - is separated from other REEs that remain trivalent and thus fit to structures of other minerals than cerianite-(Ce).[17][14][15]

## Applications

The principal industrial application of ceria is for polishing, especially [chemical-mechanical planarization](/source/Chemical-mechanical_polishing) (CMP).[3] For this purpose, it has displaced many other oxides that were previously used, such as [iron oxide](/source/Iron_oxide) and [zirconia](/source/Zirconia). For hobbyists, it is also known as "opticians' rouge".[18][19]

In its other main application, CeO2 is used to decolorize glass. It functions by converting green-tinted ferrous impurities to nearly colorless ferric oxides.[3]

### Other niche and emerging applications

#### Catalysis

CeO2 has attracted attention in the area of [heterogeneous catalysis](/source/Heterogeneous_catalysis). It catalyses the [water-gas shift reaction](/source/Water-gas_shift_reaction). It oxidizes [carbon monoxide](/source/Carbon_monoxide). Its reduced derivative Ce2O3 reduces water, with release of hydrogen.[20][21][22][23]

The interconvertibility of CeO*x* materials is the basis of the use of ceria for an oxidation catalyst. One small but illustrative use is its use in the walls of [self-cleaning ovens](/source/Self-cleaning_ovens) as a hydrocarbon oxidation catalyst during the high-temperature cleaning process. Another small scale but famous example is its role in oxidation of natural gas in [gas mantles](/source/Gas_mantle).[24]

A glowing [Coleman](/source/Coleman_Company) [white gas](/source/White_gas) lantern mantle. The glowing element is mainly [ThO2](/source/Thorium_dioxide) doped with CeO2, heated by the Ce-catalyzed oxidation of the natural gas with air.

Building on its distinct surface interactions, ceria finds further use as a sensor in [catalytic converters](/source/Catalytic_converter) in automotive applications, controlling the air-exhaust ratio to reduce [NO*x*](/source/Nitrogen_oxide) and [carbon monoxide](/source/Carbon_monoxide) emissions.[25]

#### Energy & fuels

Due to the significant [ionic](/source/Ionic_compound) and [electronic](/source/Electron) [conduction](/source/Electrical_conductor) of cerium oxide, it is well suited to be used as a [mixed conductor](/source/Mixed_conductor).[26] As such, cerium oxide is a material of interest for [solid oxide fuel cells](/source/Solid_oxide_fuel_cell) (SOFCs) in comparison to [zirconium oxide](/source/Zirconium_dioxide).[27]

Thermochemically, the [cerium(IV) oxide–cerium(III) oxide cycle](/source/Cerium(IV)_oxide%E2%80%93cerium(III)_oxide_cycle) or CeO2/Ce2O3 cycle is a two-step [water splitting](/source/Water_splitting) process that has been used for [hydrogen production](/source/Hydrogen_production).[28][29] Because it leverages the oxygen vacancies between systems, this allows ceria in water to form hydroxyl (OH) groups.[30] The hydroxyl groups can then be released as oxygen oxidizes, thus providing a source of clean energy.

#### Optics

Cerium oxide is highly valued in the optics industry for its exceptional polishing capabilities.[31] It effectively removes minor scratches and imperfections from glass surfaces through both mechanical [abrasion](/source/Abrasion_(mechanical)) and chemical interaction, producing a smooth, high-gloss finish.[32] Cerium oxide can also enhance the [durability](/source/Durability) of optical surfaces by forming a protective layer that increases resistance to scratches and environmental wear.[33]

Cerium oxide has also found use in [infrared filters](/source/Infrared) and as a replacement for [thorium dioxide](/source/Thorium_dioxide) in [incandescent mantles](/source/Gas_mantle)[34]

#### Welding

Cerium oxide is used as an addition to tungsten electrodes for Gas Tungsten Arc Welding. It provides advantages over pure Tungsten electrodes such as reducing electrode consumption rate and easier arc starting & stability. Ceria electrodes were first introduced in the US market in 1987, and are useful in AC, DC Electrode Positive, and DC Electrode Negative.

## Safety aspects

Cerium oxide nanoparticles (nanoceria) have been investigated for their antibacterial and antioxidant activity.[35][36][37]

Nanoceria is a prospective replacement of [zinc oxide](/source/Zinc_oxide) and [titanium dioxide](/source/Titanium_dioxide) in [sunscreens](/source/Sunscreen), as it has lower [photocatalytic](/source/Photocatalysis) activity.[38]

## See also

- [Cerium](/source/Cerium)

- [Cerium anomaly](/source/Cerium_anomaly)

- [Zircon](/source/Zircon)

## References

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## External links

Wikimedia Commons has media related to [Cerium(IV) oxide](https://commons.wikimedia.org/wiki/Category:Cerium(IV)_oxide).

- [Webelements at University of Sheffield](http://www.webelements.com/compounds/cerium/)

- [Synthesis and properties of ceria (in English/Russian)](https://web.archive.org/web/20100523171310/http://ceria.ru/)

v t e Cerium compounds Cerium(II) CeI2 CeSe Cerium(III) CeBr3 Ce2(CO3)3 CeCl3 CeF3 CeI3 Ce(OH)3 CeN Ce2O3 Ce2(SO4)3 Ce2(SeO4)3 Ce2S3 CeP Ce(NO3)3 Ce(ClO4)3 Organocerium(III) Ce(acac)3 Ce(C8H8)2 Ce2(C2O4)3 Ce(CH3SO3)3 CeC54H105O6 Cerium(III,IV) Ce3O4 CeS Cerium(IV) (NH4)4Ce(SO4)4·2H2O (NH4)2Ce(NO3)6 CeB6 Ce(NO3)4 Ce(OH)4 CeO2 Ce(SO4)2 Ce(SeO4)2 CeF4 Ce(ClO4)4

v t e Salts and covalent derivatives of the oxide ion H2O He Li2O BeO B6O BO B2O3 C2O C12O9 C3O2 CO CO2 CO3 CxOy N2O NO N2O2 N2O3 N2O4 NO2 N2O5 NxOy O2−2 F Ne Na2O MgO Al2O AlO Al2O3 SiO SiO2 PO P4O6 P4O10 SO S2O2 SO2 SO3 Cl2O ClO Cl2O4 ClO2 Cl2O5? Cl2O6 Cl2O7 Ar K2O CaO Sc2O3 TiO Ti2O3 TiO2 VO V2O3 VO2 V2O5 CrO Cr2O3 CrO2 CrO3 MnO Mn3O4 Mn2O3 MnO2 Mn2O7 FeO Fe3O4 Fe2O3 CoO Co3O4 Co2O3 NiO Ni2O3 Cu2O CuO ZnO Ga2O Ga2O3 GeO GeO2 As2O3 As2O5 SeO2 SeO3 Br2O BrO BrO2 Br3O8 Kr Rb2O SrO YO Y2O3 ZrO ZrO2 NbO NbO2 Nb2O5 MoO2 MoO3 TcO2 Tc2O7 RuO2 RuO4 Rh2O3 RhO2 PdO Ag2O Ag4O4 Ag2O3 CdO In2O3 SnO SnO2 Sb2O3 Sb2O4 Sb2O5 TeO2 TeO3 I2O IO IO2 I2O5 XeO3 XeO4 Cs2O BaO * Lu2O3 HfO2 Ta2O5 W2O3 WO2 "W2O5" WO3 ReO2 ReO3 Re2O7 OsO2 OsO4 IrO2 IrO4 PtO2 Au2O3 Hg2O HgO Tl2O Tl2O3 PbO Pb3O4 PbO2 Bi2O3 Bi2O5 PoO PoO2 PoO3 At Rn Fr RaO ** Lr RfO2? Db2O5? SgO3 Bh2O7? HsO4 Mt Ds Rg Cn Nh Fl Mc Lv Ts Og * La2O3 Ce2O3 CeO2 Pr2O3 Pr6O11 PrO2 Nd2O3 Pm2O3 Sm2O3 EuO Eu2O3 Gd2O3 Tb2O3 Tb4O7 TbO2 Dy2O3 Ho2O3 Er2O3 Tm2O3 Yb2O3 ** Ac2O3 ThO ThO2 PaO PaO2 Pa2O5 UO2 U2O5 U3O8 UO3 Np2O3 NpO2 Np2O5 NpO3 Pu2O3 PuO2 PuO3 Am2O3 AmO2 Cm2O3 CmO2 BkO Bk2O3 BkO2 Cf2O3 CfO2 Es2O3 Fm Md No

v t e Oxygen compounds Ag4O4 Al2O3 AmO2 Am2O3 As2O3 As2O5 Au2O3 B2O3 BaO BeO Bi2O3 BiO2 Bi2O5 BrO2 Br2O3 Br2O5 Br 3O 8 CO CO2 C3O2 CaO CaO2 CdO CeO2 Ce3O4 Ce2O3 ClO2 Cl2O Cl2O2 Cl2O3 Cl2O4 Cl2O6 Cl2O7 CoO Co2O3 Co3O4 CrO3 Cr2O3 Cr2O5 Cr5O12 CsO2 Cs2O3 CuO Dy2O3 Er2O3 Eu2O3 FeO Fe2O3 Fe3O4 Ga2O Ga2O3 GeO GeO2 H2O 2H2O 3H2O H218O H2O2 HfO2 HgO Hg2O Ho2O3 IO I2O4 I2O5 I2O6 I4O9 In2O3 IrO2 KO2 K2O2 La2O3 Li2O Li2O2 Lu2O3 MgO Mg2O3 MnO MnO2 Mn2O3 Mn2O7 MoO2 MoO3 Mo2O3 NO NO2 N2O N2O3 N2O4 N2O5 NaO2 Na2O Na2O2 NbO NbO2 Nd2O3 O2F OF OF2 O2F2 O3F2 O4F2 O5F2 O6F2 O2PtF6 more...

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Adapted from the Wikipedia article [Cerium(IV) oxide](https://en.wikipedia.org/wiki/Cerium(IV)_oxide) by Wikipedia contributors ([contributor history](https://en.wikipedia.org/wiki/Cerium(IV)_oxide?action=history)). Available under [Creative Commons Attribution-ShareAlike 4.0 International](https://creativecommons.org/licenses/by-sa/4.0/). Changes may have been made.