Hafnium tetrachloride

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Hafnium(IV) chloride
CAS number 13499-05-3 YesY
PubChem 37715
ChemSpider 34591 YesY
Jmol-3D images Image 1
Molecular formula HfCl4
Molar mass 320.302 g/mol
Appearance white crystalline solid
Melting point 432 °C (705 K)
Solubility in water decomposes
Vapor pressure 1 mmHg at 190 °C
Crystal structure Monoclinic
EU Index Not listed
Main hazards irritant and corrosive
Flash point Non-flammable
Related compounds
Other anions Hafnium(IV) fluoride
Hafnium(IV) bromide
Hafnium(IV) iodide
Other cations Titanium(IV) chloride
Zirconium(IV) chloride
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Hafnium(IV) chloride is the inorganic compound with the formula HfCl4. This colourless solid is the precursor to most hafnium organometallic compounds. It has a variety of highly specialized applications, mainly in materials science and as a catalyst.


HfCl4 can be produced by several related procedures:

HfO2 + 2 CCl4 → HfCl4 + 2 COCl2
HfO2 + 2 Cl2 + C → HfCl4 + CO2

Separation of Zr and Hf[edit]

Hafnium and zirconium occur together in minerals such as zircon, cyrtolite and baddeleyite. Zircon contains 0.05 to 2.0 percent hafnium dioxide HfO2, cyrtolite with 5.5 to 17 percent HfO2 and baddeleyite contains 1.0 to 1.8 percent HfO2.[6] Hafnium and zirconium compounds are extracted from ores together and converted to a mixture of the tetrachlorides.

The separation of HfCl4 and ZrCl4 is difficult because the compounds of Hf and Zr have very similar chemical and physical properties. Their atomic radii are similar: the atomic radius is 156.4 pm for hafnium, whereas that of Zr is 160 pm).[7] These two metals undergo similar reactions and form the similar coordination complexes.

A number of processes have been proposed to purify HfCl4 from ZrCl4 including fractional distillation, fractional precipitation, fractional crystallization and ion exchange. The log (base 10) of the vapor pressure of solid hafnium chloride (from 476 to 681 K) is given by the equation: log10(P) =-5197/T +11.712; where the pressure is measured in torr and temperature in kelvin. (The pressure at the melting point is 23,000 torr.)[8]

One method is based on the difference in the reducibility between the two tetrahalides.[6] The tetrahalides can in be separated by selectively reducing the zirconium compound to one or more lower halides or even zirconium. The hafnium tetrachloride remains substantially unchanged during the reduction and may be recovered readily from the zirconium subhalides. Hafnium tetrachloride is volatile and can therefore easily be separated from the involatile zirconium trihalide.

Structure and bonding[edit]

This Group 4 halide contains hafnium in the +4 oxidation state. Solid HfCl4 is a polymer with octahedral Hf centers. Of the six chloride ligands surrounding each Hf centre, two chloride ligands are terminal and four bridge to another Hf centre. In the gas phase, both ZrCl4 and HfCl4 adopt the monomeric tetrahedral structure seen for TiCl4.[9] Electronographic investigations of HfCl4 in gas phase showed that the Hf-Cl internuclear distance is 2.33 Å and the Cl…Cl internuclear distance is 3.80 Å. The ratio of intenuclear distances r(Me-Cl)/r(Cl…Cl) is 1.630 and this value agrees well with the value for the regular tetrahedron model (1.633).[10]


The compound is highly reactive toward water, evolving hydrogen chloride:

HfCl4 + H2O → HfOCl2 + 2 HCl

Aged samples thus often are contaminated with oxychlorides, which are also colourless.

THF forms a monomeric 2:1 complex:[11]

HfCl4 + 2 OC4H8 → HfCl4(OC4H8)2

Because this complex is soluble in organic solvents, it is a useful reagent for preparing other complexes of hafnium.

HfCl4 undergoes salt metathesis with Grignard reagents. In this way, tetrabenzylhafnium can be prepared.

With alcohols, alkoxides are formed.

HfCl4 + 4 ROH → Hf(OR)4 + 4 HCl

These compounds adopt complicated structures.


Reduction of HfCl4 is especially difficult. In the presence of phosphine ligands, reduction can be effected with potassium-sodium alloy:[12]

2 HfCl4 + 2 K + 4 P(C2H5)3 → Hf2Cl6[P(C2H5)3]4 + 2 KCl

The deep green dihafnium product is diamagnetic. X-ray crystallography shows that the complex adopts an edge-shared bioctahedral structure, very similar to the Zr analogue.


Hafnium tetrachloride is the precursor to highly active catalysts for the Ziegler-Natta polymerization of alkenes, especially propylene.[13] Typical catalysts are derived from tetrabenzylhafnium.

HfCl4 is an effective Lewis acid for various applications in organic synthesis. For example, ferrocene is alkylated with allyldimethylchlorosilane more efficiently using hafnium chloride relative to aluminium trichloride. The greater size of Hf may diminish HfCl4's tendency to complex to ferrocene.[14]

HfCl4 increases the rate and control of 1,3-dipolar cycloadditions.[15] It was found to yield better results than other Lewis acids when used with aryl and aliphatic aldoximes, allowing specific exo-isomer formation.

Materials science applications[edit]

HfCl4 is a standard precursor for chemical vapor deposition of hafnium dioxide and hafnium silicate, used as high-k dielectrics in manufacture of modern high-density integrated circuits.


  1. ^ Encyclopedia of Chemical Technology. Kirk-Othermer. Vol. 11, 4th Ed. (1991)
  2. ^ W. S. Hummers, S. Y. Tyree, S. Yolles "Zirconium and Hafnium Tetrachlorides" Inorganic Syntheses, 1953, Volume IV, p. 121. doi:10.1002/9780470132357.ch41
  3. ^ B. S. Hopkins. Chapters in the chemistry of less familiar elements, Chapter 13 Hafnium; p. 7
  4. ^ Hala, J. Halides, Oxyhalides and Salts of Halogen Complexes of Titanium, Zirconium, Hafnium, Vanadium, Niobium and Tantalum. Vol. 40, 176–177, (1970).
  5. ^ S. V. Elinson, K. I. Petrov Analytical Chemistry of the Elements: Zirconium and Hafnium. 11, (1969).
  6. ^ a b Ivan Edgar Newnham. Purification of Hafnium Tetrachloride. U.S. patent 2,961,293 November 22, 1960.
  7. ^ V. P. Spiridonov, P. A. Akishin and V. I. Tsirel'nikov, M. V. Lomonosov. "Electronographic Investigation of the structure of Zirconium and Hafnium Tetrachloride Molecules in Gas Phase". Journal of Structural Chemistry [Online] Vol. 3, 1962, pp. 329–330
  8. ^ A. A. Palko, A. D. Ryon, D. W. Kuhn, "The Vapor Pressures of Zirconium Tetrachloride and Hafnium Tetrachloride" J. Phys. Chem., 1958, volume 62, pp 319–322. doi:10.1021/j150561a017
  9. ^ Greenwood, N. N., Earnshaw, A. Chemistry of the Elements Second Ed. Butterworth-Heinemann, Boston, (1997).
  10. ^ V. P. Spiridonov, P. A. Akishin and V. I. Tsirel'nikov, M. V. Lomonosov. "Electronographic Investigation of the structure of Zirconium and Hafnium Tetrachloride Molecules in Gas Phase". Journal of Structural Chemistry [Online] Vol. 3, 1962, pp. 329–330.
  11. ^ Manzer, L. E. (1982). "Tetrahydrofuran Complexes of Selected Early Transition Metals". Inorg. Synth. Inorganic Syntheses 21. doi:10.1002/9780470132524.ch31. ISBN 978-0-470-13252-4. 
  12. ^ M. E. Riehl, S. R. Wilson, and G. S. Girolami (1993). "Synthesis, X-ray Crystal Structure, and Phosphine-Exchange Reactions of the Hafnium(III)-Hafnium(III) Dimer Hf2Cl6[P(C2H5)3]4". Inorg. Chem. 32 (2): 218–222. doi:10.1021/ic00054a017. 
  13. ^ Ron Dagani (2003-04-07). "Combinatorial Materials: Finding Catalysts Faster". Chemical and Engineering News. p. 10. 
  14. ^ S. Ahn, Y. Song, B. Yoo, I. Jung (2000). "Lewis Acid-Catalyzed Friedel-Crafts Alkylation of Ferrocene with Allylchlorosilanes". Organometallics 19 (14): 2777–2780. doi:10.1021/om0000865. 
  15. ^ P. Dunn, A. Graham, R. Grigg, P. Higginson (2000). "Tandem 1,3-azaprotiocyclotransfer–cycloaddition reactions between aldoximes and divinyl ketone. Remarkable rate enhancement and control of cycloaddition regiochemistry by hafnium(IV) chloride". Chem. Commun. (20): 2035–2036. doi:10.1039/b005389i. 

Further reading[edit]

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