Neodymium(III) oxide
Neodymium(III) oxide or neodymium sesquioxide is the chemical compound composed of neodymium and oxygen with the formula Nd2O3. It forms very light grayish-blue hexagonal crystals.[1] The rare-earth mixture didymium, previously believed to be an element, partially consists of neodymium(III) oxide.[2]
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| Names | |
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| IUPAC name
Neodymium(III) oxide | |
| Other names
Neodymium oxide, Neodymium sesquioxide | |
| Identifiers | |
3D model (JSmol) |
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| ECHA InfoCard | 100.013.832  |
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CompTox Dashboard (EPA) |
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| Properties | |
| Nd2O3 | |
| Molar mass | 336.48 g/mol |
| Appearance | light bluish gray hexagonal crystals |
| Density | 7.24 g/cm3 |
| Melting point | 2,233 °C (4,051 °F; 2,506 K) |
| Boiling point | 3,760 °C (6,800 °F; 4,030 K)[1] |
| .0003 g/100 mL (75 °C) | |
| +10,200.0·10−6 cm3/mol | |
| Structure | |
| Hexagonal, hP5 | |
| P-3m1, No. 164 | |
| Thermochemistry | |
Heat capacity (C) |
111.3 J·mol−1·K−1[1] |
Std molar entropy (S |
158.6 J·mol−1·K−1 |
Std enthalpy of formation (ΔfH⦵298) |
−1807.9 kJ·mol−1 |
| Related compounds | |
Other anions |
Neodymium(II) chloride Neodymium(III) chloride |
Other cations |
Uranium(VI) oxide Praseodymium(III) oxide Promethium(III) oxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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| Infobox references | |
Uses
Neodymium(III) oxide is used to dope glass, including sunglasses, to make solid-state lasers, and to color glasses and enamels.[3] Neodymium-doped glass turns purple due to the absorbance of yellow and green light, and is used in welding goggles.[4] Some neodymium-doped glass is dichroic; that is, it changes color depending on the lighting. One kind of glass named for the mineral alexandrite appears blue in sunlight and red in artificial light.[5] About 7000 tonnes of neodymium(III) oxide are produced worldwide each year. Neodymium(III) oxide is also used as a polymerization catalyst.[4]
Reactions
Neodymium(III) oxide is formed when neodymium(III) nitride or neodymium(III) hydroxide is burned in air.[6]
References
- Lide, David R. (1998), Handbook of Chemistry and Physics (87 ed.), Boca Raton, FL: CRC Press, pp. 471, 552, ISBN 0-8493-0594-2
- Brady, George Stuart; Clauser, Henry R.; Vaccari, John A. (2002), Materials Handbook (15 ed.), New York: McGraw-Hill Professional, p. 779, ISBN 978-0-07-136076-0, retrieved 2009-03-18
- Eagleson, Mary (1994), Concise Encyclopedia of Chemistry, Springer, p. 680, ISBN 978-3-11-011451-5, retrieved 2009-03-18
- Emsley, John (2003), Nature's Building Blocks, Oxford University Press, pp. 268–9, ISBN 978-0-19-850340-8, retrieved 2009-03-18
- Bray, Charles (2001), Dictionary of Glass (2 ed.), University of Pennsylvania Press, p. 103, ISBN 978-0-8122-3619-4, retrieved 2009-03-18
- Spencer, James Frederick (1919), The Metals of the Rare Earths, London: Longmans, Green, and Co, p. 115, retrieved 2009-03-18