Niobium(V) chloride
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| Names | |
|---|---|
| IUPAC names
Niobium(V) chloride Niobium pentachloride | |
| Identifiers | |
| 10026-12-7 NbCl5 17499-28-4 Nb2Cl10 | |
| EC Number | 233-059-8 |
| PubChem | 24818 |
| RTECS number | QU0350000 |
| Properties | |
| NbCl5 | |
| Molar mass | 270.17 g/mol |
| Appearance | yellow monoclinic crystals deliquescent |
| Density | 2.75 g/cm3 |
| Melting point | 204.7 °C (400.5 °F; 477.8 K) |
| Boiling point | 248.2 °C (478.8 °F; 521.3 K) |
| decomposes | |
| Solubility | soluble in alcohol, HCl, chloroform, CCl4 |
| Thermochemistry | |
| Std molar entropy (S |
214.05 J K−1 mol−1 |
| Std enthalpy of formation (ΔfH |
-797.47 kJ/mol |
| Hazards | |
| Flash point | Non-flammable |
| Related compounds | |
| Other anions |
Niobium(V) fluoride Niobium(V) bromide Niobium(V) iodide |
| Other cations |
Vanadium(IV) chloride Tantalum(V) chloride |
| Related niobium chlorides |
Niobium(III) chloride Niobium(IV) chloride |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
 verify (what is  ?) | |
| Infobox references | |
Niobium(V) chloride, also known as niobium pentachloride, is a yellow crystalline solid. It hydrolyzes in air, and samples are often contaminated with small amounts of NbOCl3. It is often used as a precursor to other compounds of niobium. NbCl5 may be purified by sublimation.[1]
Structure and properties
Niobium(V) chloride forms chloro-bridged dimers in the solid state (see figure). Each niobium centre is six-coordinate, but the octahedral coordination is significantly distorted. The equatorial niobium–chlorine bond lengths are 225 pm (terminal) and 256 pm (bridging), whilst the axial niobium-chlorine bonds are 229.2 pm and are deflected inwards to form an angle of 83.7° with the equatorial plane of the molecule. The Nb–Cl–Nb angle at the bridge is 101.3°. The Nb–Nb distance is 398.8 pm, too long for any metal-metal interaction.[2] NbBr5, TaCl5 and TaBr5 are isostructural with NbCl5, but NbI5 and TaI5 have different structures.
Preparation
Industrially, niobium pentachloride is obtained by direct chlorination of niobium metal at 300 to 350 °C:[3]
- 2 Nb + 5 Cl2 → 2 NbCl5
In the laboratory, niobium pentachloride is often prepared from Nb2O5, the main problem being incomplete reaction to give the oxyhalides. The conversion can be effected with thionyl chloride:[4] It also can be prepared by chlorination of niobium pentoxide in the presence of carbon at 300 °C. The products, however, contain small amounts of NbOCl3.
Uses
Niobium(V) chloride is the main precursor to the alkoxides of niobium, which find niche uses in sol-gel processing. It is also the precursor to many other laboratory reagents.
In organic synthesis, NbCl5 is a specialized Lewis acid in activating alkenes for the carbonyl-ene reaction and the Diels-Alder reaction. Niobium chloride can also generate N-acyliminium compounds from certain pyrrolidines which are substrates for nucleophiles such as allyltrimethylsilane, indole, or the silyl enol ether of benzophenone.[5]
References
- ↑ Cotton, F. Albert; Wilkinson, Geoffrey (1980), Advanced Inorganic Chemistry (4th ed.), New York: Wiley, ISBN 0-471-02775-8
- ↑ Cotton, F.A., P. A. Kibala, M. Matusz and R. B. W. Sandor (1991). "Structure of the Second Polymorph of Niobium Pentachloride". Acta Crystallogr. C 47 (11): 2435–2437. doi:10.1107/S0108270191000239.
- ↑ Joachim Eckert, Hermann C. Starck "Niobium and Niobium Compounds" Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a17_251
- ↑ D. Brown "Niobium(V) Chloride and Hexachloroniobates(V)" Inorganic Syntheses, 1957 Volume 9, pp. 88–92.doi:10.1002/9780470132401.ch24
- ↑ Andrade, C. K. Z.; Rocha, R. O.; Russowsky, D.; & Godoy, M. N. (2005). "Studies on the Niobium Pentachloride-Mediated Nucleophilic Additions to an Enantiopure Cyclic N-acyliminium Ion Derived from (S)-malic acid" (PDF). J. Braz. Chem. Soc. 16 (3b): 535–539. doi:10.1590/S0103-50532005000400007.
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