Erbium(III) oxide

From Wikipedia, the free encyclopedia
Erbium oxide[1]
Erbium oxide crystal structure
ErOPulver.jpg
Names
Other names
Erbium oxide, erbia
Identifiers
  • 12061-16-4 checkY
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.031.847 Edit this at Wikidata
  • InChI=1S/2Er.3O checkY
    Key: VQCBHWLJZDBHOS-UHFFFAOYSA-N checkY
  • InChI=1/2Er.3O/rEr2O3/c3-1-5-2-4
    Key: VQCBHWLJZDBHOS-YMHUIQTEAQ
  • O=[Er]O[Er]=O
  • ionic: [O-2].[Er+3].[O-2].[Er+3].[O-2]
Properties
Er2O3
Molar mass 382.56 g/mol
Appearance pink crystals
Density 8.64 g/cm3
Melting point 2,344 °C (4,251 °F; 2,617 K)
Boiling point 3,290 °C (5,950 °F; 3,560 K)
insoluble in water
+73,920·10−6 cm3/mol
Structure
Cubic, cI80
Ia-3, No. 206
Thermochemistry
108.5 J·mol−1·K−1
155.6 J·mol−1·K−1
Std enthalpy of
formation (ΔfH⦵298)
 −1897.9 kJ·mol−1
Related compounds
Other anions
 Erbium(III) chloride
Other cations
 Holmium(III) oxide, Thulium(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

Erbium(III) oxide, is synthesized from the lanthanide metal erbium. It was partially isolated by Carl Gustaf Mosander in 1843, and first obtained in pure form in 1905 by Georges Urbain and Charles James.[2] It has a pink color with a cubic crystal structure. Under certain conditions erbium oxide can also have a hexagonal form.[3]

Reactions[]

Erbium burns readily to form erbium (III) oxide:

The formation of erbium oxide is accomplished via the reaction 4 Er + 3 O2 → 2 Er2O3.[4] Erbium oxide is insoluble in water and soluble in mineral acids. Er2O3 readily absorbs moisture and carbon dioxide from the atmosphere.[3] It can react with acids to form the corresponding erbium(III) salts.

For example, with hydrochloric acid, the oxide follows the reaction Er2O3 + 6 HCl → 2 ErCl3 + 3 H2O to form erbium chloride.

Properties[]

One interesting property of erbium oxides is their ability to up convert photons. Photon upconversion takes place when infrared or visible radiation, low energy light, is converted to ultraviolet or violet radiation higher energy light via multiple transfer or absorption of energy.[5] Erbium oxide nanoparticles also possess photoluminescence properties. Erbium oxide nanoparticles can be formed by applying ultrasound (20 kHz, 29 W·cm−2) in the presence of multiwall carbon nanotubes. The erbium oxide nanoparticles that have been successfully made by employing ultrasound are erbium carboxioxide, hexagonal and spherical geometry erbium oxide. Each ultrasonically formed erbium oxide is photoluminescence in the visible region of the electromagnetic spectrum under excitation of 379 nm in water. Hexagonal erbium oxide photoluminescence is long lived and allows higher energy transitions (4S3/2 - 4I15/2). Spherical erbium oxide does not experience 4S3/2 - 4I15/2 energy transitions.[6]

Uses[]

The applications of Er2O3 are varied due to their electrical, optical and photoluminescence properties. Nanoscale materials doped with Er3+ are of much interest because they have special particle-size-dependent optical and electrical properties.[7] Erbium oxide doped nanoparticle materials can be dispersed in glass or plastic for display purposes, such as display monitors. The spectroscopy of Er3+ electronic transitions in host crystals lattices of nanoparticles combined with ultrasonically formed geometries in aqueous solution of carbon nanotubes is of great interest for synthesis of photoluminescence nanoparticles in 'green' chemistry.[6] Erbium oxide is among the most important rare earth metals used in biomedicine.[8] The photoluminescence property of erbium oxide nanoparticles on carbon nanotubes makes them useful in biomedical applications. For example, erbium oxide nanoparticles can be surface modified for distribution into aqueous and non-aqueous media for bioimaging.[7] Erbium oxides are also used as gate dielectrics in semi conductor devices since it has a high dielectric constant (10–14) and a large band gap. Erbium is sometimes used as a coloring for glasses[9] and erbium oxide can also be used as a burnable neutron poison for nuclear fuel.

References[]

  1. ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, FL: CRC Press. pp. 4–57. ISBN 978-0-8493-0594-8.
  2. ^ Aaron John Ihde (1984). The development of modern chemistry. Courier Dover Publications. pp. 378–379. ISBN 978-0-486-64235-2.
  3. ^ a b Singh, M.P; C.S Thakur; K Shalini; N Bhat; S.A Shivashankar (3 February 2003). "Structural and electrical characterization of erbium oxide films grown on Si(100) by low-pressure metalorganic chemical vapor deposition". Applied Physics Letters. 83 (14): 2889. doi:10.1063/1.1616653. Archived from the original on 8 July 2012. Retrieved April 17, 2012.
  4. ^ Emsley, John (2001). "Erbium" Nature's Building Blocks: An A-Z Guide to Elements. Oxford, England, Uk: Oxford University Press. pp. 136–139. ISBN 978-0-19-850340-8.
  5. ^ "Rare-earth-doped nanoparticles prove illuminating". SPIE. Retrieved April 10, 2012.
  6. ^ a b Radziuk, Darya; Andre Skirtach; Andre Geßner; Michael U. Kumke; Wei Zhang; Helmuth M€ohwald; Dmitry Shchukin (24 October 2011). "Ultrasonic Approach for Formation of Erbium Oxide Nanoparticles with Variable Geometries". Langmuir. 27 (23): 14472–14480. doi:10.1021/la203622u. PMID 22022886.
  7. ^ a b Richard, Scheps (12 February 1996). "Upconversion laser processes" (PDF). Progress in Quantum Electronics. 20 (4): 271–358. doi:10.1016/0079-6727(95)00007-0.
  8. ^ Andre, Skirtach; Almudena Javier; Oliver Kref; Karen Kohler; Alicia Alberola; Helmuth Mohwald; Wolfgang Parak; Gleb Sukhorukov (2006). "Laser-Induced Release of Encapsulated Materials inside Living Cells" (PDF). Angew. Chem. Int. Ed. 38 (28): 4612–4617. doi:10.1002/anie.200504599. PMID 16791887. Retrieved April 15, 2012.
  9. ^ Lide, David (1998). Handbook of Chemistry and Physics. Boca, Raton Fl: CRC Press. pp. 4–57. ISBN 978-0849305948.
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