Zirconium(IV) chloride
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| Names | |
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| IUPAC names
Zirconium tetrachloride
Zirconium(IV) chloride | |
| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.030.041 |
| EC Number |
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PubChem CID
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| UNII | |
CompTox Dashboard (EPA)
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| Properties | |
| ZrCl4 | |
| Molar mass | 233.04 g/mol |
| Appearance | white crystals |
| Density | 2.80 g/cm3 |
| Melting point | 437 °C (819 °F; 710 K) (triple point) |
| Boiling point | 331 °C (628 °F; 604 K) (sublimes) |
| hydrolysis | |
| Solubility | concentrated HCl (with reaction) |
| Structure | |
| Monoclinic, mP10 | |
| P12/c1, No. 13 | |
| Thermochemistry | |
Heat capacity (C)
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125.38 J K−1 mol−1 |
Std molar
entropy (S⦵298) |
181.41 J K−1 mol−1 |
Std enthalpy of
formation (ΔfH⦵298) |
−980.52 kJ/mol |
| Hazards | |
| GHS labelling:[2] | |
  
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| Danger | |
| H290, H302, H312, H314, H317, H332, H334 | |
| P234, P260, P261, P264, P270, P271, P272, P280, P285, P301+P312, P301+P330+P331, P302+P352, P303+P361+P353, P304+P312, P304+P340, P304+P341, P305+P351+P338, P310, P312, P321, P322, P330, P333+P313, P342+P311, P363, P390, P404, P405, P501 | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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1488-1500 mg/kg (oral, rat) 655 mg/kg (mouse, oral)[1] |
| Safety data sheet (SDS) | MSDS |
| Related compounds | |
Other anions
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Zirconium(IV) fluoride Zirconium(IV) bromide Zirconium(IV) iodide |
Other cations
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Titanium tetrachloride Hafnium tetrachloride |
Related compounds
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Zirconium(II) chloride, Zirconium(III) 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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Zirconium(IV) chloride, also known as zirconium tetrachloride, (ZrCl4) is an inorganic compound frequently used as a precursor to other compounds of zirconium. This white high-melting solid hydrolyzes rapidly in humid air.
Structure
[edit]Unlike molecular TiCl4, solid ZrCl4 adopts a polymeric structure wherein each Zr is octahedrally coordinated. This difference in structures is responsible for the disparity in their properties: TiCl
4 is distillable, but ZrCl
4 is a solid. In the solid state, ZrCl4 adopts a tape-like linear polymeric structure—the same structure adopted by HfCl4. This polymer degrades readily upon treatment with Lewis bases, which cleave the Zr-Cl-Zr linkages.[4]
Synthesis
[edit]This conversion entails treatment of zirconium oxide with carbon in the presence of chlorine at high temperature:
- ZrO2 + 2 C + 2 Cl2 → ZrCl4 + 2 CO
A laboratory scale process uses carbon tetrachloride in place of carbon and chlorine:[5]
- ZrO2 + 2 CCl4 → ZrCl4 + 2 COCl2
Applications
[edit]Precursor to zirconium metal
[edit]ZrCl4 is an intermediate in the conversion of zirconium minerals to metallic zirconium by the Kroll process. In nature, zirconium minerals usually exist as oxides (reflected also by the tendency of all zirconium chlorides to hydrolyze). For their conversion to bulk metal, these refractory oxides are first converted to the tetrachloride, which can be distilled at high temperatures. The purified ZrCl4 can be reduced with Zr metal to produce zirconium(III) chloride.
Other uses
[edit]ZrCl4 is the most common precursor for chemical vapor deposition of zirconium dioxide and zirconium diboride.[6]
In organic synthesis zirconium tetrachloride is used as a weak Lewis acid for the Friedel-Crafts reaction, the Diels-Alder reaction and intramolecular cyclisation reactions.[7] It is also used to make water-repellent treatment of textiles and other fibrous materials.
Properties and reactions
[edit]Hydrolysis of ZrCl4 gives the hydrated hydroxy chloride cluster called zirconyl chloride. This reaction is rapid and virtually irreversible, consistent with the high oxophilicity of zirconium(IV). For this reason, manipulations of ZrCl4 typically require air-free techniques.
ZrCl4 is the principal starting compound for the synthesis of many organometallic complexes of zirconium.[8] Because of its polymeric structure, ZrCl4 is usually converted to a molecular complex before use. It forms a 1:2 complex with tetrahydrofuran: CAS [21959-01-3], mp 175–177 °C.[9] Sodium cyclopentadienide (NaC5H5) reacts with ZrCl4(THF)2 to give zirconocene dichloride, ZrCl2(C5H5)2, a versatile organozirconium complex.[10] One of the most curious properties of ZrCl4 is its high solubility in the presence of methylated benzenes, such as durene. This solubilization arises through the formation of π-complexes.[11]
The log (base 10) of the vapor pressure of zirconium tetrachloride (from 480 to 689 K) is given by the equation: log10(P) = −5400/T + 11.766, where the pressure is measured in torrs and temperature in kelvins. The log (base 10) of the vapor pressure of solid zirconium tetrachloride (from 710 to 741 K) is given by the equation log10(P) = −3427/T + 9.088. The pressure at the melting point is 14,500 torrs.[12]
References
[edit]- ^ "Zirconium compounds (as Zr)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
- ^ GHS: PubChem
- ^ "New Environment Inc. - NFPA Chemicals". newenv.com. Retrieved 26 April 2017.
- ^ N. N. Greenwood & A. Earnshaw, Chemistry of the Elements (2nd ed.), Butterworth-Heinemann, Oxford, 1997.
- ^ Hummers, W. S.; Tyree, S. Y.; Yolles, S. (1953). "Zirconium and Hafnium Tetrachlorides". Inorganic Syntheses. Vol. IV. McGraw-Hill Book Company, Inc. p. 121. doi:10.1002/9780470132357.ch41. ISBN 978-0-470-13235-7.
- ^ Randich, E. (1 November 1979). "Chemical vapor deposited borides of the form (Ti,Zr)B2 and (Ta,Ti)B2". Thin Solid Films. 63 (2): 309–313. Bibcode:1979TSF....63..309R. doi:10.1016/0040-6090(79)90034-8.
- ^ Bora U. (2003). "Zirconium Tetrachloride". Synlett (7): 1073–1074. doi:10.1055/s-2003-39323.
- ^ Ilan Marek, ed. (2005). New Aspects of Zirconium Containing Organic Compounds. Topics in Organometallic Chemistry. Vol. 10. Springer: Berlin, Heidelberg, New York. doi:10.1007/b80198. ISBN 978-3-540-22221-7. ISSN 1436-6002.
- ^ L. E. Manzer; Joe Deaton (1982). "31. Tetragtdrfuran Complexes of Selected Early Transition Metals". Inorganic Syntheses. Vol. 21. pp. 135–140. doi:10.1002/9780470132524.ch31. ISBN 978-0-470-13252-4.
- ^ Wilkinson, G.; Birmingham, J. G. (1954). "Bis-cyclopentadienyl Compounds of Ti, Zr, V, Nb and Ta". J. Am. Chem. Soc. 76 (17): 4281–4284. doi:10.1021/ja01646a008.
- ^ Musso, F.; Solari, E.; Floriani, C.; Schenk, K. (1997). "Hydrocarbon Activation with Metal Halides: Zirconium Tetrachloride Catalyzing the Jacobsen Reaction and Assisting the Trimerization of Alkynes via the Formation of η6-Arene-Zirconium(IV) Complexes". Organometallics. 16 (22): 4889–4895. doi:10.1021/om970438g.
- ^ Palko, A. A.; Ryon, A. D.; Kuhn, D. W. (March 1958). "The Vapor Pressures of Zirconium Tetrachloride and Hafnium Tetrachloride". J. Phys. Chem. 62 (3): 319–322. doi:10.1021/j150561a017. hdl:2027/mdp.39015086513051.