Vanadium oxytrichloride
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| Names | |
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| IUPAC name
Vanadium trichloride oxide
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Other names
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| ECHA InfoCard | 100.028.892 |
| EC Number |
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| MeSH | trichlorooxo+vanadium |
PubChem CID
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| RTECS number |
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| UNII | |
| UN number | 2443 |
CompTox Dashboard (EPA)
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| Properties | |
| VOCl 3 | |
| Molar mass | 173.300 g mol−1 |
| Appearance | yellow liquid |
| Density | 1.826 g mL−1 |
| Melting point | −76.5 °C (−105.7 °F; 196.7 K) |
| Boiling point | 126.7 °C (260.1 °F; 399.8 K) |
| Decomposes | |
| Vapor pressure | 1.84 kPa (at 20 °C) |
| Structure | |
| Tetrahedral | |
| Hazards | |
| GHS labelling: | |
  
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| Danger | |
| H301, H314 | |
| P280, P301+P310, P305+P351+P338, P310 | |
| NFPA 704 (fire diamond) | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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140 mg kg−1 (oral, rat) |
| Related compounds | |
Related vanadiums
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Vanadium oxytrichloride is the inorganic compound with the formula VOCl3. This yellow distillable liquid hydrolyzes readily in air. It is an oxidizing agent. It is used as a reagent in organic synthesis.[1] Samples often appear red or orange owing to an impurity of vanadium tetrachloride.[2]
Properties
[edit]VOCl3 is a vanadium compound with vanadium in the +5 oxidation state and as such is diamagnetic. It is tetrahedral with O-V-Cl bond angles of 111° and Cl-V-Cl bond angles of 108°. The V-O and V-Cl bond lengths are 157 and 214 pm, respectively. VOCl3 is highly reactive toward water and evolves HCl upon standing. It is soluble in nonpolar solvents such as benzene, CH2Cl2, and hexane. In some aspects, the chemical properties of VOCl3 and POCl3 are similar. One distinction is that VOCl3 is a strong oxidizing agent, whereas the phosphorus compound is not.[3] Neat VOCl3 is the usual chemical shift standard for 51V NMR spectroscopy.[4]
Preparation
[edit]VOCl3 arises by the chlorination of V2O5. The reaction proceeds near 600 °C:[5]
- 3 Cl2 + V2O5 → 2 VOCl3 + 1.5 O2
Heating an intimate (well-blended with tiny particles) mixture of V2O5, chlorine, and carbon at 200–400 °C also gives VOCl3. In this case the carbon serves as a deoxygenation agent akin to its use in the chloride process for the manufacturing of TiCl4 from TiO2.
Vanadium(III) oxide can also be used as a precursor:[2]
- 3 Cl2 + V2O3 → 2 VOCl3 + 0.5 O2
A more typical laboratory synthesis involves the chlorination of V2O5 using SOCl2.[6]
- V2O5 + 3 SOCl2 → 2 VOCl3 + 3 SO2
Reactions
[edit]Hydrolysis and alcoholysis
[edit]VOCl3 quickly hydrolyzes resulting in vanadium pentoxide and hydrochloric acid. An intermediate in this process is VO2Cl:
- 2 VOCl3 + 3 H2O → V2O5 + 6 HCl
VOCl3 reacts with alcohols especially in the presence of a proton-acceptor to give alkoxides, as illustrated by this synthesis of vanadyl isopropoxide:
- VOCl3 + 3 HOCH(CH3)2 → VO(OCH(CH3)2)3 + 3 HCl
Interconversions to other V-O-Cl compounds
[edit]VOCl3 is also used in the synthesis of vanadium oxydichloride.
- V2O5 + 3 VCl3 + VOCl3 → 6 VOCl2
VO2Cl can be prepared by an unusual reaction involving Cl2O.[7]
- VOCl3 + Cl2O → VO2Cl + 2 Cl2
At >180 °C, VO2Cl decomposes to V2O5 and VOCl3. Similarly, VOCl2 also decomposes to give VOCl3, together with VOCl.
Adduct formation
[edit]VOCl3 is strongly Lewis acidic, as demonstrated by its tendency to form adducts with various bases such as acetonitrile and amines. In forming the adducts, vanadium changes from four-coordinate tetrahedral geometry to six-coordinate octahedral geometry:
- VOCl3 + 2 H2NEt → VOCl3(H2NEt)2
Organic chemistry
[edit]VOCl3 is a catalyst or precatalyst in production of ethylene-propylene rubbers (EPDM). In organic synthesis, it has been used for oxidative coupling of phenols and anisoles.[8]
References
[edit]- ^ O'Brien, Michael K.; Vanasse, Benoit (2001). "Vanadyl Trichloride". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rv004. ISBN 0-471-93623-5.
- ^ a b F. E. Brown; F. A. Griffitts (1939). "Hypovanadous Oxide and Vanadium Oxytrichloride". Inorganic Syntheses. Vol. I. pp. 106–108. doi:10.1002/9780470132326.ch38. ISBN 978-0-470-13232-6.
{{cite book}}:|journal=ignored (help) - ^ A. Earnshaw, N. Greenwood (1997). The Chemistry of the Elements - Second Edition. pp. 513–514.
- ^ Rehder, D.; Polenova, T.; Bühl, M. (2007). Vanadium-51 NMR. Annual Reports on NMR Spectroscopy. Vol. 62. pp. 49–114. doi:10.1016/S0066-4103(07)62002-X. ISBN 978-0-12-373919-3.
- ^ Holleman, Arnold Frederik; Wiberg, Egon; Wiberg, Nils (2001). Inorganic Chemistry. Academic Press. ISBN 978-0-12-352651-9.
- ^ G. Brauer "Vanadium oxytrichloride" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 1264.
- ^ Oppermann, H. (1967). "Untersuchungen an Vanadinoxidchloriden und Vanadinchloriden. I. Gleichgewichte mit VOCl3, VO2Cl und VOCl2". Zeitschrift für anorganische und allgemeine Chemie. 351 (3–4): 113–126. doi:10.1002/zaac.19673510302.
- ^ O'Brien, Michael K.; Vanasse, Benoit (2001). "Vanadyl Trichloride". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.rv004. ISBN 0-471-93623-5.