Vanadium(II) oxide
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| Names | |
|---|---|
| IUPAC name
Vanadium(II) oxide
| |
| Other names
Vanadium oxide
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| Identifiers | |
CAS Number
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3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.031.655 |
| EC Number |
|
Gmelin Reference
|
532274 |
PubChem CID
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CompTox Dashboard (EPA)
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InChI
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SMILES
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| Properties | |
Chemical formula
|
VO |
| Molar mass | 66.9409 g/mol |
| Appearance | grey solid with metallic lustre |
| Density | 5.758 g/cm3 |
| Melting point | 1,789 °C (3,252 °F; 2,062 K) |
| Boiling point | 2,627 °C (4,761 °F; 2,900 K) |
Refractive index (nD)
|
1.5763 |
| Structure | |
Crystal structure
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Halite (cubic), cF8 |
Space group
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Fm3m, No. 225 |
Coordination geometry
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Octahedral (V2+) Octahedral (O2−) |
| Thermochemistry | |
Std molar
entropy (S⦵298) |
39.01 J/mol·K[1] |
Std enthalpy of
formation (ΔfH⦵298) |
−431.790 kJ/mol[1] |
Gibbs free energy (ΔfG⦵)
|
−404.219 kJ/mol[1] |
| Hazards | |
| GHS labelling:[2] | |
Pictograms
|
 
|
Signal word
|
Danger |
Hazard statements
|
H319, H332, H335, H372 |
Precautionary statements
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P260, P264, P264+P265, P270, P271, P280, P304+P340, P305+P351+P338, P317, P319, P337+P317, P403+P233, P405, P501 |
| Flash point | Non-flammable |
| Related compounds | |
Other anions
|
Vanadium monosulfide Vanadium monoselenide Vanadium monotelluride |
Other cations
|
Niobium(II) oxide Tantalum(II) oxide |
Related vanadium oxides
|
Vanadium(III) oxide Vanadium(IV) oxide Vanadium(V) oxide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references
| |
Vanadium(II) oxide is the inorganic compound with the idealized formula VO. It is one of the several binary vanadium oxides. It adopts a distorted NaCl structure and contains weak V−V metal to metal bonds. VO is a semiconductor owing to delocalisation of electrons in the t2g orbitals. VO is a non-stoichiometric compound, its composition varying from VO0.8 to VO1.3.[3]
Diatomic VO is one of the molecules found in the spectrum of relatively cool M-type stars.[4] A potential use of vanadium(II) monoxide is as a molecular vapor in synthetic chemical reagents in low-temperature matrices.[5]
References
- ^ 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.
- ^ PubChem. "Vanadium(II) oxide". pubchem.ncbi.nlm.nih.gov. Retrieved 2026-02-03.
- ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 982. doi:10.1016/C2009-0-30414-6. ISBN 978-0-08-037941-8.
- ^ Tsuji, T. (1986). "Molecules in Stars". Annu. Rev. Astron. Astrophys. 24: 94. Bibcode:1986ARA&A..24...89T. doi:10.1146/annurev.aa.24.090186.000513.
- ^ Groshens, Thomas J.; Klabunde, Kenneth J. (August 1990). "Molecular vapor synthesis: the use of titanium monoxide and vanadium monoxide vapors as reagents". Inorganic Chemistry. 29 (16): 2979–2982. doi:10.1021/ic00341a025. ISSN 0020-1669.