Uranium hexachloride
IUPAC name
Uranium(VI) chloride
Other names
Uranium hexachloride
Peruranic chloride
3D model (JSmol)
  • InChI=1S/6ClH.U/h6*1H;/p-6
  • [Cl-].[Cl-].[Cl-].[Cl-].[Cl-].[Cl-].[U]
Molar mass 450.745 g/mol
Appearance dark green crystalline solid
Density 3.6 g/cm3
Melting point 177 °C (351 °F; 450 K)
Related compounds
Other anions
Uranium hexafluoride
Other cations
Tungsten hexachloride
Related uranium chlorides
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Uranium hexachloride (UCl6) is an inorganic chemical compound of uranium in the +6 oxidation state.[1][2] UCl6 is a metal halide composed of uranium and chlorine. It is a multi-luminescent dark green crystalline solid with a vapor pressure between 1-3 mmHg at 373.15 K.[3] UCl6 is stable in a vacuum, dry air, nitrogen and helium at room temperature. It is soluble in carbon tetrachloride (CCl4). Compared to the other uranium halides, little is known about UCl6.

Structure and Bonding

Uranium hexachloride has an octahedral geometry, with point group Oh. Its lattice (dimensions: 10.95 ± 0.02 Å x 6.03 ± 0.01 Å) is hexagonal in shape with three molecules per cell; the average theoretical U-Cl bond is 2.472 Å long (the experimental U-Cl length found by X-ray diffraction is 2.42 Å),[4] and the distance between two adjacent chlorine atoms is 3.65 Å.

Chemical properties

Uranium hexachloride is a highly hygroscopic compound and decomposes readily when exposed to ordinary atmospheric conditions.[5] therefore it should be handled in either a vacuum apparatus or in a dry box.

Thermal decomposition

UCl6 is stable up to temperatures between 120 °C and 150 °C. The decomposition of UCl6 results in a solid phase transition from one crystal form of UCl6 to another more stable form.[6] However, the decomposition of gaseous UCl6 produces UCl5. The activation energy for this reaction is about 40 kcal per mole.

2 UCl6 (g) → 2 UCl5 (s) + Cl2 (g)


UCl6 is not a very soluble compound. It dissolves in CCl4 to give a brown solution. It is slightly soluble in isobutyl bromide and in fluorocarbon (C7F16).[6]

Solvents Temperature (°C) Grams of UCl6/100g of solution
CCl4 −18 2.64
CCl4 0 4.9
CCl4 20 7.8
6.6% Cl2 : 93.4% CCl4 −20 2.4
12.5% Cl2 : 87.5% CCl4 −20 2.23
12.5% Cl2 : 87.5% CCl4 0 3.98
Liquid Cl2 −33 2.20
CH3Cl −24 1.16
Benzene 80 Insoluble
Freon 113 45 1.83

Reaction with hydrogen fluoride

When UCl6 is reacted with purified anhydrous liquid hydrogen fluoride (HF) at room temperature produces UF5.[6]

2 UCl6 + 10 HF → 2 UF5 + 10 HCl + Cl2


Uranium hexachloride can be synthesized from the reaction of uranium trioxide (UO3) with a mixture of liquid CCl4 and hot chlorine (Cl2). The yield can be increased if the reaction carried out in the presence of UCl5.[7] The UO3 is converted to UCl5, which in turn reacts with the excess Cl2 to form UCl6. It requires a substantial amount of heat for the reaction to take place; the temperature range is from 65 °C to 170 °C depending on the amount of reactant (ideal temperature 100 °C - 125 °C). The reaction is carried out in a closed gas-tight vessel (for example a glovebox) that can withstand the pressure that builds up.

Step 1: 2 UO3 + 5 Cl2 → 2 UCl5 + 3 O2

Step 2: 2 UCl5 + Cl2 → 2 UCl6

Overall reaction: 2 UO3 + 6 Cl2 → 2 UCl6 + 3 O2

This metal hexahalide can also be synthesized by blowing Cl2 gas over sublimed UCl4 at 350 °C.[8]

Step 1: 2 UCl4 + Cl2 → 2 UCl5

Step 2: 2 UCl5 + Cl2 → 2 UCl6

Overall Reaction: UCl4 + Cl2 → UCl6


  1. ^ Zachariasen, W. H. (1948). "Crystal chemical studies of the 5f-series of elements. V. The crystal structure of uranium hexachloride". Acta Crystallographica. 1 (6): 285–287. Bibcode:1948AcCry...1..285Z. doi:10.1107/S0365110X48000788.
  2. ^ Taylor, J. C.; Wilson, P. W. (1974). "Neutron and X-ray powder diffraction studies of the structure of uranium hexachloride". Acta Crystallographica Section B. 30 (6): 1481. Bibcode:1974AcCrB..30.1481T. doi:10.1107/S0567740874005115.
  3. ^ Van Dyke, R. E.; Evers, E. C. (1955). "Preparation of Uranium Hexachloride". Google Patents: 2.
  4. ^ Batista, E. R.; Martin, R. L.; Hay, P. J. (2004). "Density Functional Investigations of the Properties and Thermodynamics of UFn and UCln (n=1,...,6)". J. Chem. Phys. 121 (22): 11104–11. doi:10.1063/1.1811607. PMID 15634063.
  5. ^ Lipkin, D.; Wessman, S. (1955). "Process and Apparatus for protecting Uranium hexachloride from Deterioration and Contamination". Google Patents: 2.
  6. ^ a b c Katz, J.J.; Rabinowitch,E. (1951). The Chemistry of Uranium. Ann Arbor: The McGraw-Hill Book Company.
  7. ^ Van Dyke, R. E.; Evers, E. C. (1955). "Preparation of Uranium Hexachloride". Google Patents: 2.
  8. ^ Thornton, G.; Edelstein, N.; Rösch, N.; Woodwark, D.R.; Edgell, R.G. (1979). "The Electronic Structure of UCl6: Photoelectron Spectra and Scattered Wave Xα Calculations". J. Chem. Phys. 70 (11): 6. Bibcode:1979JChPh..70.5218T. doi:10.1063/1.437313.