My watch list  

Cerium(IV) oxide

Cerium(IV) oxide
IUPAC name Cerium(IV) oxide
Other names ceric oxide, ceria,
cerium oxide, cerium dioxide
CAS number 1306-38-3
Molecular formula CeO2
Molar mass 172.115 g/mol
Appearance white or pale yellow solid,
slightly hygroscopic
Density 7.65 g/cm3, solid
7.215 g/cm3, fluorite phase
Melting point

Approximately 2400 K (2100 °C)

Boiling point

3500 °C (? K)

Solubility in water not soluble — ? g/100 ml (? °C)
Related Compounds
Related compounds Ce2O3
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Cerium(IV) oxide, ceric oxide, ceria, or sometimes simply cerium oxide or cerium dioxide, is a pale yellow-white powder, CeO2. It is used in ceramics, to polish glass, and to sensitize photosensitive glass. It is also used in lapidary as "jeweller's rouge"; it is also known as "optician's rouge".[1] Ceria is used in the walls of self-cleaning ovens as a hydrocarbon catalyst during the high-temperature cleaning process. It has high absorption of ultraviolet radiation while it is transparent for visible light, so it is a prospective replacement of zinc oxide and titanium dioxide in sunscreens, as it has lower photocatalytic activity. However its thermal catalytic properties have to be decreased by coating the particles with amorphous silica or boron nitride.

Ceria is slightly hygroscopic and will also absorb a small amount of carbon dioxide from the atmosphere.

Note that cerium also forms cerium(III) oxide, Ce2O3.


As a fuel cell electrolyte

In the doped form, ceria has seen interest as a material for solid oxide fuel cells or SOFCs because of its relatively high oxygen ion conductivity (i.e. oxygen atoms readily move through it) at intermediate temperatures (500-800 °C). Undoped and doped ceria also exhibit high electronic conductivity at low partial pressures of oxygen due to the formation of small polarons. However, doped ceria has an extended electrolytic region (area of predominant ionic conductivity), over that of ceria, that allows its use as an electrolyte in SOFCs. Substituting a fraction of the ceria with gadolinium or samarium will introduce oxygen vacancies in the crystal without adding electronic charge carriers. This increases the ionic conductivity and results in a better electrolyte.

Under reducing conditions, those experienced on the anode side of the fuel cell, a large amount of oxygen vacancies within the ceria electrolyte can be formed. This results in the normally pale yellow ceria to turn black or grey as the result of color center formation. Some of the cerium(IV) oxide is also reduced to cerium(III) oxide under these conditions which consequently increases the electronic conductivity of the material. Finally, ceria undergoes what is described as a chemical expansion under reducing conditions as a result of reduction of the cerium cation from a 4+ to a 3+ state in order to charge compensate for oxygen vacancy formation.

As a catalyst

Ceria has been used in catalytic converters in automotive applications. Since ceria can become non-stoichioimetric in oxygen content (i.e. it can give up oxygen without decomposing) depending on its ambient partial pressure of oxygen, it can release or take in oxygen in the exhaust stream of a combustion engine. In association with other catalysts, ceria can effectively reduce NOx emissions as well as convert harmful carbon monoxide to the less harmful carbon dioxide.


In the fluorite structure, ceria exhibits several defects depending on partial pressure of oxygen. The primary defects of concern are oxygen vacancies and small polarons (electrons localized on cerium cations) because these two are located in the "useful" range of ceria.


  1. ^
  • Webelements at University of Sheffield
  • Center for Advanced Microstructures and Devices at Louisiana State University
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Cerium(IV)_oxide". A list of authors is available in Wikipedia.
Your browser is not current. Microsoft Internet Explorer 6.0 does not support some functions on Chemie.DE