Thorium dioxide

Thorium dioxide

Names
IUPAC names Thorium dioxide Thorium(IV) oxide
Other names thoria thorium anhydride
Identifiers
CAS Number	1314-20-1 N
Jmol interactive 3D	Image
PubChem	14808
InChI InChI=1S/2O.Th
SMILES O=[Th]=O
Properties
Chemical formula	ThO2
Molar mass	264.04 g/mol
Appearance	white solid
Odor	odorless
Density	10.00 g/cm3
Melting point	3,390 °C (6,130 °F; 3,660 K)
Boiling point	4,400 °C (7,950 °F; 4,670 K)
Solubility in water	insoluble
Solubility	insoluble in alkali slightly soluble in acid
Refractive index (nD)	2.200 (thorianite)
Structure
Crystal structure	Fluorite (cubic), cF12
Space group	Fm3m, No. 225
Lattice constant	a = 559.74(6) pm[1]
Coordination geometry	Tetrahedral (O2−); cubic (ThIV)
Thermochemistry
Std molar entropy (So298)	65.2(2) J K−1 mol−1
Std enthalpy of formation (ΔfHo298)	−1226(4) kJ/mol
Hazards
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LD50 (Median dose)	400 mg/kg
Related compounds
Other cations	Hafnium(IV) oxide Cerium(IV) oxide
Related compounds	Protactinium(IV) oxide Uranium(IV) 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

Thorium dioxide (ThO₂), also called thorium (IV) oxide, is a crystalline solid, often white or yellow in color. It was formerly known as thoria. It is produced mainly as a by-product of lanthanide and uranium production.^[1] Thorianite is the name of the mineralogical form of thorium dioxide. It is moderately rare and crystallizes in isometric system. The melting point of thorium oxide is 3300 °C – the highest of all known oxides. Only a few elements (including tungsten and carbon) and a few compounds (including tantalum carbide) have higher melting points.^[2]

Chemistry

The compound is radioactive due to the radioactivity of thorium. Thorium dioxide can be turned into a nuclear fuel by breeding it into uranium-233 (see below and refer to the article on thorium for more information on this). The high thermal stability of thorium dioxide allows applications in flame spraying and high-temperature ceramics. Thoria has the fluorite crystal structure. This is uncommon among binary dioxides (other examples include cerium dioxide, hafnium dioxide, uranium dioxide and plutonium dioxide). The band gap of thoria is about 6 eV.

Applications

Thorium dioxide is used as a stabilizer in tungsten electrodes in TIG welding, electron tubes, and aircraft engines. As an alloy, thoriated tungsten metal is not easily deformed because the high-fusion material thoria augments the high-temperature mechanical properties, and thorium helps stimulate the emission of electrons (thermions). It is the most popular oxide additive because of its low cost, but is being phased out in favor of non-radioactive elements such as cerium, lanthanum and zirconium.

Thorium dioxide is a catalyst in many chemical reactions, including the Ruzicka large ring synthesis, petroleum cracking, conversion of ammonia to nitric acid and preparation of sulfuric acid.^[3]

Thoria dispersed nickel finds its applications in various high temperature operations like combustion engines because it is a good creep resistant material. It can also be used for hydrogen trapping.^[4][5]

Thorium dioxide was the primary ingredient in the once-common radiocontrast agent Thorotrast. Its use was abandoned when it was found to be a carcinogen, sometimes causing cholangiocarcinoma. As many as 10 million patients were treated with Thorotrast. It offered excellent image enhancement and almost no immediate side effects but was associated with a significantly higher incidence of cancer later in life, often occurring decades following its administration (with one large study showing a median life-expectancy reduction of 14 years experienced by those treated with it). Today, iodinated solutions (injected) or barium sulfate (ingested) are the standard X-ray contrast agents.

Another major use in the past was in gas mantle of lanterns, which were frequently composed of 99 percent ThO₂ and 1% cerium(IV) oxide. Even as late as the 1980s it was estimated that about half of all ThO₂ produced (several hundred tonnes per year) was used for this purpose.^[6] Some mantles still use thorium, but yttrium oxide (or sometimes zirconium oxide) is used increasingly as a replacement.

Thorium dioxide was formerly added to glasses during manufacture to increase their refractive index, producing thoriated glass with up to 40% ThO₂ content. These glasses were used in the construction of high-quality photographic lenses. However, the radioactivity of the thorium caused both a safety and pollution hazard and self-degradation of the glass (turning it yellow or brown over time). Lanthanum oxide has replaced thorium dioxide in almost all modern high-index glasses.

Thorium dioxide (thoria) can be used in nuclear reactors as ceramic fuel pellets, typically contained in nuclear fuel rods clad with zirconium alloys. Thorium is not fissile (but is "fertile", breeding fissile uranium-233 under neutron bombardment); hence, it must be used as a nuclear reactor fuel in conjunction with fissile isotopes of either uranium or plutonium. This can be achieved by blending thorium with uranium or plutonium, or using it in its pure form in conjunction with separate fuel rods containing uranium or plutonium. Thorium dioxide offers advantages over conventional uranium dioxide fuel pellets, because of its higher thermal conductivity (lower operating temperature), considerably higher melting point, and chemical stability (does not oxidize in the presence of water/oxygen, unlike uranium dioxide).

Thorium dioxide is a Welsbach material. It has been suggested^[7] that these chemicals could be sprayed into the upper atmosphere to reflect sunlight and thus lower the global temperature. However, due to its density and radioactivity, thorium dioxide would be a poor choice for this application.

References

1. 1 2 Yamashita, Toshiyuki; Nitani, Noriko; Tsuji, Toshihide; Inagaki, Hironitsu (1997). "Thermal expansions of NpO₂ and some other actinide dioxides". J. Nucl. Mat. 245 (1): 72–78. doi:10.1016/S0022-3115(96)00750-7. 
2. ↑ Emsley, John (2001). Nature's Building Blocks ((Hardcover, First Edition) ed.). Oxford University Press. p. 441. ISBN 0-19-850340-7. 
3. ↑ Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. p. 931. ISBN 0-07-049439-8. Retrieved 2009-06-06. 
4. ↑ Mitchell, Brian S (2004). An Introduction to Materials Engineering. and Science for Chemical and Materials. p. 473. ISBN 978-0-471-43623-2. 
5. ↑ Robertson, Wayne M. (1979). "Measurement and evaluation of hydrogen trapping in thoria dispersed nickel". Metallurgical and Materials Transactions A 10 (4): 489–501. doi:10.1007/BF02697077. 
6. ↑ Greenwood, Norman N.; Earnshaw, Alan (1984). Chemistry of the Elements. Oxford: Pergamon Press. pp. 1425, 1456. ISBN 0-08-022057-6. 
7. ↑ Chang, David B; Shih, I-fu "Stratospheric Welsbach seeding for reduction of global warming", US Patent No. 5003186.