Erbium(III) oxide

Erbium oxide[1]

Names
Other names

Erbium oxide, erbia

Identifiers

CAS Number

* 12061-16-4 Y

3D model (JSmol)

* Interactive image
* ionic: Interactive image

ChemSpider |

* 4298039 Y

EC Number |

* 235-045-7

PubChem CID

* 159426

InChI

* InChI=1S/2Er.3O Y

Key: VQCBHWLJZDBHOS-UHFFFAOYSA-N Y

* InChI=1/2Er.3O/rEr2O3/c3-1-5-2-4

Key: VQCBHWLJZDBHOS-YMHUIQTEAQ

SMILES

* O=[Er]O[Er]=O

* ionic: [O-2].[Er+3].[O-2].[Er+3].[O-2]

Properties

Chemical formula

| 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)

Solubility in water

| insoluble in water

Magnetic susceptibility (χ)

| +73,920·10−6 cm3/mol
Structure

Crystal structure

| Cubic, cI80

Space group

| Ia-3, No. 206
Thermochemistry

Heat capacity (C)

| 108.5 J·mol−1·K−1

Std molar
entropy (S ~~o~~ 298)

| 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).

Y verify (what is YN ?)
Infobox references

Tracking categories (test):

* SizeSet

Erbium(III) oxide is the inorganic compound with the formula Er

3. It is a pink paramagnetic solid. It finds uses in various optical materials.[2]

## Contents

* 1 Structure
* 2 Reactions
* 3 Properties
* 4 Uses
* 5 History
* 6 References

## Structure

Erbium(III) oxide has a cubic structure resembling the bixbyite motif. The Er3+ centers are octahedral.[2]

## Reactions

The formation of erbium oxide is accomplished by burning erbium metal.[3] Erbium oxide is insoluble in water and soluble in mineral acids. Er2O3 does not readily absorb moisture and carbon dioxide from the atmosphere. It can react with acids to form the corresponding erbium(III) salts. For example, with hydrochloric acid, the oxide follows the following idealized reaction leading to erbium chloride:

3 \+ 6 HCl → 2 ErCl
3 \+ 3 H

In practice, such simple acid-base reactions are accompanied by hydration:

ErCl
3 \+ 9 H
2O → [Er(H
2O)
9]Cl

## 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.[4] 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.[5]

## 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.[6] 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.[5] Erbium oxide is among the most important rare earth metals used in biomedicine.[7] 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.[6] 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[8] and erbium oxide can also be used as a burnable neutron poison for nuclear fuel.

## History

Impure erbium(III) oxide was isolated by Carl Gustaf Mosander in 1843, and first obtained in pure form in 1905 by Georges Urbain and Charles James.[9]

## 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. ↑ 2.0 2.1 Adachi, Gin-ya; Imanaka, Nobuhito (1998). "The Binary Rare Earth Oxides". Chemical Reviews 98 (4): 1479–1514. doi:10.1021/cr940055h. PMID 11848940.
3. ↑ 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. https://archive.org/details/naturesbuildingb0000emsl/page/136.
4. ↑ "Rare-earth-doped nanoparticles prove illuminating". SPIE. http://spie.org/x30412.xml.
5. ↑ 5.0 5.1 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.
6. ↑ 6.0 6.1 Richard, Scheps (12 February 1996). "Upconversion laser processes". Progress in Quantum Electronics 20 (4): 271–358. doi:10.1016/0079-6727(95)00007-0. Bibcode: 1996PQE....20..271S. https://zenodo.org/record/1258293.
7. ↑ 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". Angew. Chem. Int. Ed. 38 (28): 4612–4617. doi:10.1002/anie.200504599. PMID 16791887. http://www.df.uba.ar/users/bragas/Optica en la nanoescala/Papers/2006_Skirtcah_AngewChem inte_Nanoheaters.pdf. Retrieved April 15, 2012.
8. ↑ Lide, David (1998). Handbook of Chemistry and Physics. Boca, Raton Fl: CRC Press. pp. 4–57. ISBN 978-0849305948.
9. ↑ Aaron John Ihde (1984). The development of modern chemistry. Courier Dover Publications. pp. 378–379. ISBN 978-0-486-64235-2. https://books.google.com/books?id=34KwmkU4LG0C&pg=PA377.

* v
* t
* e

Erbium compounds

* ErCl3
* ErBr3
* ErI3
* Er2O3
* ErB4
* ErB6

* v
* t
* e

Oxides

Mixed oxidation states|

* Antimony tetroxide (Sb2O4)
* Cobalt(II,III) oxide (Co3O4)
* Europium(II,III) oxide (Eu3O4)
* Iron(II,III) oxide (Fe<sub>3O4)
* Lead(II,IV) oxide (Pb3O4)
* Manganese(II,III) oxide (Mn3O4)
* Silver(I,III) oxide (Ag2O2)
* Triuranium octoxide (U3O8)
* Carbon suboxide (C3O2)
* Mellitic anhydride (C12O9)
* [[Chemistry:Praseodymium(III,IV) Praseodymium(III,IV) oxide]] (Pr6O11)
* Terbium(III,IV) oxide (Tb4O7)

+1 oxidation state|

* Copper(I) oxide (Cu<sub>2O)
* Caesium oxide (Cs2O)
* Dicarbon monoxide (C2O)
* Dichlorine monoxide (Cl2O)
* Gallium(I) oxide (Ga2O)
* Lithium oxide (Li2O)
* Potassium oxide (K2O)
* Rubidium oxide (Rb2O)
* Silver oxide (Ag2O)
* Thallium(I) oxide (Tl2O)
* Sodium oxide (Na2O)
* Water (hydrogen oxide) (H2O)

+2 oxidation state|

* Aluminium(II) oxide (AlO)
* Barium oxide (BaO)
* Beryllium oxide (BeO)
* Cadmium oxide (CdO)
* Calcium oxide (CaO)
* Carbon monoxide (CO)
* Chromium(II) oxide (CrO)
* Cobalt(II) oxide (CoO)
* Copper(II) oxide (CuO)
* Europium(II) oxide (EuO)
* Germanium monoxide (GeO))
* Iron(II) oxide (FeO)
* Lead(II) oxide (PbO)
* Magnesium oxide (MgO)
* Manganese(II) oxide (MnO)
* Mercury(II) oxide (HgO)
* Nickel(II) oxide (NiO)
* Nitric oxide (NO)
* Palladium(II) oxide (PdO)
* Silicon monoxide (SiO)
* Strontium oxide (SrO)
* Sulfur monoxide (SO)
* Disulfur dioxide (S2O2)
* Thorium monoxide (ThO)
* Tin(II) oxide (SnO)
* Titanium(II) oxide (TiO)
* Vanadium(II) oxide (VO)
* Zinc oxide (ZnO)

+3 oxidation state|

* Aluminium oxide (Al<sub>2O3)
* Antimony trioxide (Sb2O3)
* Arsenic trioxide (As2O3)
* Bismuth(III) oxide (Bi2O3)
* Boron trioxide (B2O3)
* Cerium(III) oxide (Ce2O3)
* Dibromine trioxide (Br2O3)
* Chromium(III) oxide (Cr2O3)
* Dinitrogen trioxide (N2O3)
* Dysprosium(III) oxide (Dy2O3)
* Erbium(III) oxide (Er2O3)
* Europium(III) oxide (Eu2O3)
* Gadolinium(III) oxide (Gd2O3)
* Gallium(III) oxide (Ga2O3)
* Holmium(III) oxide (Ho2O3)
* Indium(III) oxide (In<sub>2O3)
* Iron(III) oxide (Fe2O3)
* Lanthanum oxide (La2O3)
* Lutetium(III) oxide (Lu2O3)
* Manganese(III) oxide (Mn2O3)
* Neodymium(III) oxide (Nd2O3)
* Nickel(III) oxide (Ni2O3)
* Phosphorus trioxide (P4O6)
* Praseodymium(III) oxide (Pr2O3)
* Promethium(III) oxide (Pm2O3)
* Rhodium(III) oxide (Rh2O3)
* [[Chemistry:Samarium(III) Samarium(III) oxide]] (Sm2O3)
* Scandium oxide (Sc2O3)
* Terbium(III) oxide (Tb2O3)
* Thallium(III) oxide (Tl2O3)
* Thulium(III) oxide (Tm2O3)
* Titanium(III) oxide (Ti2O3)
* Tungsten(III) oxide (W2O3)
* Vanadium(III) oxide (V2O3)
* Ytterbium(III) oxide (Yb2O3)
* Yttrium(III) oxide (Y2O3)

+4 oxidation state|

* Americium dioxide (AmO2)
* Carbon dioxide (CO2)
* Carbon trioxide (CO3)
* Cerium(IV) oxide (CeO2)
* Chlorine dioxide (ClO2)
* Chromium(IV) oxide (CrO<sub>2)
* Dinitrogen tetroxide (N2O4)
* Germanium dioxide (GeO<sub>2)
* [[Chemistry:Hafnium(IV) Hafnium(IV) oxide]] (HfO2)
* Lead dioxide (PbO2)
* Manganese dioxide (MnO2)
* Neptunium(IV) oxide (NpO2)
* Nitrogen dioxide (NO2)
* Osmium dioxide (OsO2)
* Plutonium(IV) oxide (PuO2)
* Praseodymium(IV) oxide (PrO2)
* Protactinium(IV) oxide (PaO2)
* Rhodium(IV) oxide (RhO2)
* Ruthenium(IV) oxide (RuO<sub>2)
* Selenium dioxide (SeO2)
* Silicon dioxide (SiO2)
* Sulfur dioxide (SO2)
* Tellurium dioxide (TeO<sub>2)
* [[Chemistry:Terbium(IV) Terbium(IV) oxide]] (TbO2)
* Thorium dioxide (ThO2)
* Tin dioxide (SnO2)
* Titanium dioxide (TiO<sub>2)
* Tungsten(IV) oxide (WO2)
* Uranium dioxide (UO2)
* Vanadium(IV) oxide (VO2)
* Zirconium dioxide (ZrO2)

+5 oxidation state|

* Antimony pentoxide (Sb2O5)
* Arsenic pentoxide (As2O5)
* Dinitrogen pentoxide (N2O5)
* Niobium pentoxide (Nb2O5)
* Phosphorus pentoxide (P2O5)
* Protactinium(V) oxide (Pa2O5)
* Tantalum pentoxide (Ta2O5)
* Vanadium(V) oxide (V2O5)

+6 oxidation state|

* Chromium trioxide (CrO3)
* Molybdenum trioxide (MoO3)
* Rhenium trioxide (ReO3)
* Selenium trioxide (SeO3)
* Sulfur trioxide (SO3)
* Tellurium trioxide (TeO3)
* Tungsten trioxide (WO3)
* Uranium trioxide (UO3)
* Xenon trioxide (XeO3)
* Iridium trioxide (IrO3)

+7 oxidation state|

* Dichlorine heptoxide (Cl2O7)
* Manganese heptoxide (Mn2O7)
* [[Chemistry:Rhenium(VII) Rhenium(VII) oxide]] (Re2O7)
* Technetium(VII) oxide (Tc2O7)

+8 oxidation state|

* Osmium tetroxide (OsO4)
* Ruthenium tetroxide (RuO4)
* Xenon tetroxide (XeO4)
* Iridium tetroxide (IrO4)
* Hassium tetroxide (HsO4)

Related|

* Oxocarbon
* Suboxide
* Oxyanion
* Ozonide
* Peroxide
* Superoxide

Oxides are sorted by oxidation state. Category:Oxides

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