Holmium(III) oxide

Names
IUPAC name

Holmium(III) oxide

Other names

Holmium oxide, Holmia

Identifiers

CAS Number

* 12055-62-8 Y

3D model (JSmol)

* Interactive image
* Interactive image

ChemSpider |

* 3441223 Y

EC Number |

* 235-015-3

PubChem CID

* 4232365

UNII |

* 6A1MAM6A4J Y

InChI

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

Key: JYTUFVYWTIKZGR-UHFFFAOYSA-N Y

* InChI=1/2Ho.3O/rHo2O3/c3-1-5-2-4

Key: JYTUFVYWTIKZGR-VLHOCPAZAL

SMILES

* [O][Ho]O[Ho][O]

* O=[Ho]O[Ho]=O

Properties

Chemical formula

| Ho2O3
Molar mass | 377.858 g·mol−1
Appearance  | Pale yellow, opaque powder.
Density | 8.41 g cm−3
Melting point |  2,415 °C (4,379 °F; 2,688 K)
Boiling point |  3,900 °C (7,050 °F; 4,170 K)
Band gap | 5.3 eV [1]

Magnetic susceptibility (χ)

| +88,100·10−6 cm3/mol

Refractive index (nD)

| 1.8 [1]
Structure

Crystal structure

| Cubic, cI80

Space group

| Ia-3, No. 206
Thermochemistry

Heat capacity (C)

| 115.0 J mol−1 K−1

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

| 158.2 J mol−1 K−1

Std enthalpy of
formation (ΔfH⦵298)

| -1880.7 kJ mol−1
Hazards
Safety data sheet | External MSDS
GHS pictograms |
GHS Signal word | Warning

GHS hazard statements

| H319, H410

GHS precautionary statements

| P264, P273, P280, P305+351+338, P337+313, P391, P501
Related compounds

Other anions

| Holmium(III) chloride

Other cations

| Dysprosium(III) oxide
Erbium(III) oxide

Related compounds

| Bismuth(III) oxide

Europium(III) oxide
Gold(III) oxide
Lanthanum(III) oxide
Lutetium(III) oxide
Praseodymium(III) oxide
Promethium(III) oxide
Terbium(III) oxide
Thallium(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

Holmium(III) oxide, or holmium oxide is a chemical compound of a rare-earth element holmium and oxygen with the formula Ho2O3. Together with dysprosium(III) oxide (Dy2O3), holmium oxide is one of the most powerfully paramagnetic substances known. The oxide, also called holmia, occurs as a component of the related erbium oxide mineral called erbia. Typically, the oxides of the trivalent lanthanides coexist in nature, and separation of these components requires specialized methods. Holmium oxide is used in making specialty colored glasses. Glass containing holmium oxide and holmium oxide solutions have a series of sharp optical absorption peaks in the visible spectral range. They are therefore traditionally used as a convenient calibration standard for optical spectrophotometers.

## Contents

* 1 Properties
* 1.1 Appearance
* 1.2 Crystalline structure
* 1.3 Chemical
* 2 History
* 3 Occurrence
* 4 Production
* 5 Applications
* 6 Health effects
* 7 References

## Properties

### Appearance

Holmium oxide has some fairly dramatic color changes depending on the lighting conditions. In daylight, it is a tannish yellow color. Under trichromatic light, it is a fiery orange red, almost indistinguishable from the way erbium oxide looks under this same lighting. This is related to the sharp emission bands of the phosphors.[2] Holmium oxide has a wide band gap of 5.3 eV[1] and thus should appear colorless. The yellow color originates from abundant lattice defects (such as oxygen vacancies) and is related to internal transitions at the Ho3+ ions.[2]

### Crystalline structure

Room-temperature structure of Ho2O3 viewed along a cubic axis. Red atoms are oxygens Electron micrograph of lamellar particles and aggregates of holmium oxide. Scale bar at bottom shows 10 μm.

Holmium oxide has a cubic, yet rather complex bixbyite structure, with many atoms per unit cell and a large lattice constant of 1.06 nm. This structure is characteristic of oxides of heavy rare-earth elements, such as Tb2O3, Dy2O3, Er2O3, Tm2O3, Yb2O3 and Lu2O3. The thermal expansion coefficient of Ho2O3 is also relatively large at 7.4 ×10−6/°C.[3]

### Chemical

Treating holmium oxide with hydrogen chloride or with ammonium chloride affords the corresponding holmium chloride:[4]

Ho2O3 \+ 6 NH4Cl → 2 HoCl3 \+ 6 NH3 \+ 3 H2O

Holmium(III) oxide can also react with hydrogen sulfide to form holmium(III) sulfide at high temperatures.[5]

## History

Holmium (Holmia, Latin name for Stockholm) was discovered by Marc Delafontaine and Jacques-Louis Soret in 1878 who noticed the aberrant spectrographic absorption bands of the then-unknown element (they called it "Element X").[6][7] Later in 1878, Per Teodor Cleve independently discovered the element while he was working on erbia earth (erbium oxide).[8][9]

Using the method developed by Carl Gustaf Mosander, Cleve first removed all of the known contaminants from erbia. The result of that effort was two new materials, one brown and one green. He named the brown substance holmia (after the Latin name for Cleve's home town, Stockholm) and the green one thulia. Holmia was later found to be the holmium oxide and thulia was thulium oxide.[10]

## Occurrence

Gadolinite contains traces of holmium(III) oxide

Holmium oxide occurs in trace amounts in the minerals gadolinite, monazite, and in other rare-earth minerals. Holmium metal readily oxidizes in air; therefore presence of holmium in nature is synonymous with that of holmia. With the abundance of 1.4 mg/kg, holmium is the 56th most abundant element.[10] The main mining areas are China , United States , Brazil , India , Sri Lanka and Australia with reserves of holmium oxide estimated as 400,000 tonnes.[10]

## Production

A typical extraction process of holmium oxide can be simplified as follows: the mineral mixtures are crushed and ground. Monazite, because of its magnetic properties can be separated by repeated electromagnetic separation. After separation, it is treated with hot concentrated sulfuric acid to produce water-soluble sulfates of several rare earth elements. The acidic filtrates are partially neutralized with sodium hydroxide to pH 3-4. Thorium precipitates out of solution as hydroxide and is removed. After that, the solution is treated with ammonium oxalate to convert rare earths in to their insoluble oxalates. The oxalates are converted to oxides by annealing. The oxides are dissolved in nitric acid that excludes one of the main components, cerium, whose oxide is insoluble in HNO3.

The most efficient separation routine for holmium oxide from the rare-earths is ion exchange. In this process, rare-earth ions are adsorbed onto suitable ion-exchange resin by exchange with hydrogen, ammonium or cupric ions present in the resin. The rare earth ions are then selectively washed out by suitable complexing agent, such as ammonium citrate or nitrilotriacetate.[4]

## Applications

A solution of 4% holmium oxide in 10% perchloric acid, permanently fused into a quartz cuvette as an optical calibration standard

Holmium oxide is one of the colorants used for cubic zirconia and glass, providing yellow or red coloring.[11] Glass containing holmium oxide and holmium oxide solutions (usually in perchloric acid) have sharp optical absorption peaks in the spectral range 200-900 nm. They are therefore used as a calibration standard for optical spectrophotometers[12][13] and are available commercially.[14] As most other oxides of rare-earth elements, holmium oxide is used as a specialty catalyst, phosphor and a laser material. Holmium laser operates at wavelength of about 2.08 micrometres, either in pulsed or continuous regime. This laser is eye safe and is used in medicine, lidars, wind velocity measurements and atmosphere monitoring.[15]

## Health effects

Holmium-166m oxide, an isotopologue

Holmium(III) oxide is, compared to many other compounds, not very dangerous, although repeated overexposure can cause granuloma and hemoglobinemia. It has low oral, dermal and inhalation toxicities and is non-irritating. The acute oral median lethal dose (LD50) is greater than 1 g per kilogram of body weight.[16]

## References

1. ↑ 1.0 1.1 1.2 Wiktorczyk, T (2002). "Preparation and optical properties of holmium oxide thin films". Thin Solid Films 405 (1–2): 238–242. doi:10.1016/S0040-6090(01)01760-6. Bibcode: 2002TSF...405..238W.
2. ↑ 2.0 2.1 Su, Yiguo; Li, Guangshe; Chen, Xiaobo; Liu, Junjie; Li, Liping (2008). "Hydrothermal Synthesis of GdVO4:Ho3+ Nanorods with a Novel White-light Emission". Chemistry Letters 37 (7): 762. doi:10.1246/cl.2008.762.
3. ↑ Adachi, Gin-ya; Imanaka, Nobuhito (1998). "The Binary Rare Earth Oxides". Chemical Reviews 98 (4): 1479–1514. doi:10.1021/cr940055h. PMID 11848940.
4. ↑ 4.0 4.1 Patnaik, Pradyot (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. pp. 340;445. ISBN 0-07-049439-8. https://books.google.com/books?id=Xqj-TTzkvTEC&pg=PA445. Retrieved 2009-06-06.
5. ↑ Synthesis of Lanthanide and Actinide Compounds. Kluwer Academic Publishers. 1991. pp. 329–335. ISBN 0792310187. https://books.google.com/books?id=bnS5elHL2w8C&pg=PA329. Retrieved 18 August 2022.
6. ↑ Jacques-Louis Soret (1878). "Sur les spectres d'absorption ultra-violets des terres de la gadolinite". Comptes rendus de l'Académie des sciences 87: 1062. http://gallica.bnf.fr/ark:/12148/bpt6k3043m/f1124.table.
7. ↑ Jacques-Louis Soret (1879). "Sur le spectre des terres faisant partie du groupe de l'yttria". Comptes rendus de l'Académie des sciences 89: 521. https://gallica.bnf.fr/ark:/12148/bpt6k3046j/f550.table.
8. ↑ . 1879. https://gallica.bnf.fr/ark:/12148/bpt6k3046j/f499.table.
9. ↑ Per Teodor Cleve (1879). "Sur l'erbine". Comptes rendus de l'Académie des sciences 89: 708. http://gallica.bnf.fr/ark:/12148/bpt6k3046j/f759.table.
10. ↑ 10.0 10.1 10.2 John Emsley (2001). Nature's building blocks: an A-Z guide to the elements. US: Oxford University Press. pp. 180–181. ISBN 0-19-850341-5. https://books.google.com/books?id=Yhi5X7OwuGkC&pg=PA180.
11. ↑ "Cubic zirconia". http://www.geologyrocks.co.uk/tutorials/cubic_zirconia.
12. ↑ R. P. MacDonald (1964). "Uses for a Holmium Oxide Filter in Spectrophotometry". Clinical Chemistry 10 (12): 1117–20. doi:10.1093/clinchem/10.12.1117. PMID 14240747. http://www.clinchem.org/cgi/reprint/10/12/1117.pdf.
13. ↑ Travis, John C.; Zwinkels, JC; Mercader, F; Ruíz, A; Early, EA; Smith, MV; Noël, M; Maley, M et al. (2002). "An International Evaluation of Holmium Oxide Solution Reference Materials for Wavelength Calibration in Molecular Absorption Spectrophotometry". Analytical Chemistry 74 (14): 3408–15. doi:10.1021/ac0255680. PMID 12139047.
14. ↑ "Holmium Glass Filter for Spectrophotometer Calibration". http://www.labshoponline.com/holmium-glass-filter-spectrophotometer-calibration-p-88.html.
15. ↑ Yehoshua Y. Kalisky (2006). The physics and engineering of solid state lasers. SPIE Press. p. 125. ISBN 0-8194-6094-X. https://books.google.com/books?id=0BFHEev-pMgC&pg=PA127.
16. ↑ "External MSDS". http://www.espimetals.com/msds's/holmiumoxide.pdf.

* v
* t
* e

Holmium compounds

* HoBr3
* HoCl3
* Ho2O3
* Ho2Ti2O7

* 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

* v
* t
* e

Oxygen compounds

* AgO
* Al2O3
* AmO2
* Am2O3
* As2O3
* As2O5
* Au2O3
* B2O3
* BaO
* BeO
* Bi2O3
* BiO2
* Bi2O5
* BrO2
* Br2O3
* Br2O5
* CO
* CO2
* C2O3
* CaO
* CaO2
* CdO
* CeO2
* Ce3O4
* Ce2O3
* ClO2
* Cl2O
* Cl2O3
* Cl2O4
* Cl2O6
* Cl2O7
* CoO
* Co2O3
* Co3O4
* CrO3
* Cr2O3
* Cr2O5
* Cr5O12
* CsO2
* Cs2O3
* CuO
* D2O
* Dy2O3
* Er2O3
* Eu2O3
* FeO
* Fe2O3
* Fe3O4
* Ga2O
* Ga2O3
* GeO
* GeO2
* H2O
* H218O
* H2O2
* HfO2
* HgO
* Hg2O
* Ho2O3
* I2O4
* I2O5
* I2O6
* I4O9
* In2O3
* IrO2
* KO2
* K2O2
* La2O3
* Li2O
* Li2O2
* Lu2O3
* MgO
* Mg2O3
* MnO
* MnO2
* Mn2O3
* Mn2O7
* MoO2
* MoO3
* Mo2O3
* NO
* NO2
* N2O
* N2O3
* N2O4
* N2O5
* NaO2
* Na2O
* Na2O2
* NbO
* NbO2
* Nd2O3
* OF2
* O2F2
* O3F2
* O4F2
* O2PtF6

Chemical formulas

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*[CID]: Compound ID
*[H319]: Causes serious eye irritation
*[H410]: Very toxic to aquatic life with long lasting effects
*[P264]: Wash … thoroughly after handling
*[P273]: Avoid release to the environment
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*[P305+351+338]: IF IN EYES: Rinse continuously with water for several minutes. Remove contact lenses if present and easy to do – continue rinsing
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