Niobium(IV) chloride
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| Names | |
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| IUPAC name
Niobium(IV) chloride
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| Other names
Niobium tetrachloride
Niobium chloride | |
| Identifiers | |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| NbCl4 | |
| Molar mass | 234.718 g/mol |
| Appearance | Violet-Black Crystals |
| Density | 3.2 g/cm3 |
| Melting point | Dec. 800 °C |
| Boiling point | Subl. 275 °C/10−4 mmHg |
| Reacts | |
| Related compounds | |
Other anions
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Niobium(IV) bromide Niobium(IV) iodide |
Other cations
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Vanadium(IV) chloride Tantalum(IV) chloride |
Related niobium chlorides [1]
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Niobium(III) chloride Niobium(V) chloride |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Niobium(IV) chloride, also known as niobium tetrachloride, is the chemical compound of formula NbCl4. This compound exists as dark violet crystals, is highly sensitive to air and moisture, and disproportiates into niobium(III) chloride and niobium(V) chloride when heated.[2]
Structure and properties
[edit]In the solid state, niobium(IV) chloride exists as chains of edge-sharing octahedra with alternating Nb-Nb distances of lengths 302.9 and 379.4 pm. The shorter distances correspond to Nb-Nb bonds, which result in the compound's diamagnetism. Its structure is very similar to that of tungsten(IV) chloride.
Other coordination complexes with the formula NbCl4L2, such as tetrachlorobis(tetrahydrofuran) niobium, only form monomers resulting in one unpaired electron in the dxy orbital, making the compounds paramagnetic.[3]
Niobium chloride rapidly oxidizes and hydrolyzes in air to form niobium(V) oxide.
Preparation
[edit]Niobium(IV) chloride is typically produced by allowing elemental niobium and niobium(V) chloride crystals to react over several days in a temperature gradient, with the metal around 400 °C and the salt around 250 °C.[4]
- 4 NbCl5 + Nb → 5 NbCl4
Niobium (IV) chloride can also prepared by a similar reduction of niobium pentachloride with powdered aluminium.
- 3 NbCl5 + Al → 3 NbCl4 + AlCl3
A similar technique is also used in the synthesis of niobium(IV) bromide and tantalum(IV) chloride. Niobium(IV) iodide exists as well and may be synthesized by thermal decomposition of niobium(V) iodide.
At 400 °C NbCl4 disproportiates:
- 2 NbCl4 → NbCl3 + NbCl5
Reactions
[edit]The disproportiation of niobium(IV) chloride can be used to make tetrachlorobis(tetrahydrofuran) niobium, a useful synthon in NbIV chemistry due to the lability of the attached tetrahydrofuran ligands.[5] This compound can be synthesized by first reacting NbCl5 with aluminium in acetonitrile followed by addition of tetrahydrofuran to the resultant solid by the following reaction.[6]
- 3 NbCl5 + Al + 3 CH3CN → 3 NbCl4(NCCH3)3 + AlCl3
- 3 NbCl4(NCCH3)3 + AlCl3 + 3 C4H8O → 3 NbCl4(thf)2 + 9 MeCN + AlCl3(thf)
References
[edit]- ^ CRC, Handbook of Chemistry and Physics, 89th Ed., 2008/09, editor D. Lide, Cleveland, OH: CRC Press, p. 4-36.
- ^ Macintyre, J.E.; Daniel, F.M.; Chapman and Hall; Stirling, V.M. Dictionary of Inorganic Compounds. 1992, Cleveland, OH: CRC Press, p. 2957
- ^ Cotton, F. A..; Lu, J. (1995). "EPR and Crystallographic Studies of Some Reaction Products of VCl4, NbCl4, and TaCl4 with Trialkyl- and Triarylphosphines". Inorg. Chem. 34 (10): 2639. doi:10.1021/ic00114a023.
- ^ McCarley, Robert E.; Torp, Bruce A. (1963). "The preparation and properties of niobium(IV) compounds. I. Some niobium(IV) halides and their pyridine adducts". Inorg. Chem. 2 (3): 540. doi:10.1021/ic50007a029.
- ^ Hubert-Pfalzgraf, L.G. Niobium & Tantalum: Inorganic & Coordination Chemistry. 2006: John Wiley & Sons, Ltd.
- ^ Manzer, L.E. (1977). "Preparation of the paramagnetic alkyls bis(cyclopentadienyl)dimethylniobium and bis(methylcyclopentadienyl)dimethyltantalum and some six- and eight-coordinate phosphine derivatives of niobium(IV)". Inorg. Chem. 16 (3): 525–528. doi:10.1021/ic50169a004.