Ytterbium(III) oxide
Ytterbium(III) oxide
IUPAC name
Ytterbium(III) oxide.
Other names
diytterbium trioxide
ytterbium sesquioxide
ECHA InfoCard 100.013.850 Edit this at Wikidata
EC Number
  • 215-234-0
Molar mass 394.08 g/mol
Appearance White solid.
Density 9.17 g/cm3, solid.
Melting point 2,355 °C (4,271 °F; 2,628 K)
Boiling point 4,070 °C (7,360 °F; 4,340 K)
Cubic, cI80
Ia-3, No. 206
133.05 J/mol·K [1]
-1814.600 kJ/mol [1]
-1726.844 kJ/mol [1]
GHS labelling:
GHS07: Exclamation mark
H315, H319, H335
P261, P305+P351+P338[2]
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 1: Exposure would cause irritation but only minor residual injury. E.g. turpentineFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no code
Flash point Non-flammable.
Related compounds
Other anions
Ytterbium(III) sulfide, Ytterbium(III) chloride
Other cations
Thulium(III) oxide
Lutetium(III) oxide
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Ytterbium(III) oxide is the chemical compound with the formula Yb2O3. It is one of the more commonly encountered compounds of ytterbium. It occurs naturally in trace amounts in the mineral gadolinite. It was first isolated from this in 1878 by Jean Charles Galissard de Marignac.[3]


Ytterbium(III) oxide can be obtained by directly reacting ytterbium with oxygen:[4]

4 Yb + 3 O2 → 2 Yb2O3

It can also be obtained by the thermal decomposition of ytterbium carbonate or ytterbium oxalate at temperatures around 700 °C:[5]

Yb2(CO3)3 → Yb2O3 + 3CO2
Yb2(C2O4)3 → Yb2O3 + 3 CO2 + 3CO



Ytterbium(III) oxide is a white powder.[2] It reacts with carbon tetrachloride[6] or hot hydrochloric acid to form ytterbium(III) chloride:[7]

2 Yb2O3 + 3 CCl4 → 4 YbCl3 + 3 CO2
Yb2O3 + 6 HCl → 2 YbCl3 + 3 H2O


Like the other trivalent oxides of the heavier lanthanides, ytterbium(III) oxide has the "rare-earth C-type sesquioxide" structure which is related to the fluorite structure with one quarter of the anions removed, leading to ytterbium atoms in two different six coordinate (non-octahedral) environments.[8]


See also


  1. ^ a b c R. Robie, B. Hemingway, and J. Fisher, “Thermodynamic Properties of Minerals and Related Substances at 298.15K and 1bar Pressure and at Higher Temperatures,” US Geol. Surv., vol. 1452, 1978.[1]
  2. ^ a b Sigma Aldrich; rev. 2012-09-19
  3. ^ Krebs, Robert E.; Déjur, Rae (2006). The history and use of our earth's chemical elements: a reference guide (2nd ed.). Westport, Conn.: Greenwood Press. ISBN 978-0-313-33438-2.
  4. ^ Wiberg, Egon; Wiberg, Nils (2007). Holleman, Arnold F.; Fischer, Gerd (eds.). Lehrbuch der anorganischen Chemie (102., stark umgearbeitete und verbesserte Auflage ed.). Berlin New York: Walter de Gruyter. ISBN 978-3-11-017770-1.
  5. ^ Meyer, Gerd, ed. (1991). Synthesis of lanthanide and actinide compounds. Topics in f element chemistry. Dordrecht: Kluwer. ISBN 978-0-7923-1018-1.
  6. ^ GORYUSHKIN, V. F.; ASTAKHOVA, I. S.; POSHEVNEVA, A. I.; ZALYMOVA, S. A. (1989-12-19). "ChemInform Abstract: Crystalline Holmium Dichloride". ChemInform. 20 (51). doi:10.1002/chin.198951025. ISSN 0931-7597.
  7. ^ Sebastian, Jörg; Seifert, Hans-Joachim (1998-09-07). "Ternary chlorides in the systems ACl/YbCl3 (A=Cs,Rb,K)". Thermochimica Acta. 318 (1): 29–37. doi:10.1016/S0040-6031(98)00326-8. ISSN 0040-6031.
  8. ^ Wells, Alexander Frank (1991). Structural inorganic chemistry. Oxford science publications (5th ed.). Oxford: Clarendon press. ISBN 978-0-19-855370-0.
  9. ^ Milne, G. W. A. (2005-09-02). Gardner's Commercially Important Chemicals: Synonyms, Trade Names, and Properties. John Wiley & Sons. ISBN 978-0-471-73661-5.