Uranium hexachloride
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Names
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IUPAC name
Uranium(VI) chloride
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Other names
Uranium hexachloride
Peruranic chloride
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Identifiers
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ChemSpider
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InChI=1S/6ClH.U/h6*1H;/p-6
Key: XFCORTPUZRSUIZ-UHFFFAOYSA-H
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[Cl-].[Cl-].[Cl-].[Cl-].[Cl-].[Cl-].[U]
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Properties
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|
UCl
6
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Molar mass
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450.745 g/mol
|
Appearance
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dark green crystalline solid
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Density
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3.6 g/cm
3
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Melting point
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177 °C (351 °F; 450 K)
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Related compounds
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Uranium hexafluoride
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Tungsten hexachloride
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Related uranium chlorides
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Except where otherwise noted, data are given for materials in their
standard state
(at 25 °C [77 °F], 100 kPa).
|
Chemical compound
Uranium hexachloride
(
UCl
6
) is an
inorganic
chemical compound
of
uranium
in the +6
oxidation state
.
[1]
[2]
UCl
6
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]
UCl
6
is stable in a
vacuum
, dry air,
nitrogen
and
helium
at
room temperature
. It is soluble in
carbon tetrachloride
(
CCl
4
). Compared to the other uranium halides, little is known about
UCl
6
.
Structure and Bonding
[
edit
]
Uranium hexachloride has an
octahedral
geometry, with
point group
O
h
. Its
lattice
(dimensions: 10.95 ± 0.02 A x 6.03 ± 0.01 A) is hexagonal in shape with three molecules per cell; the average theoretical U-Cl bond is 2.472 A long (the experimental U-Cl length found by
X-ray diffraction
is 2.42 A),
[4]
and the distance between two adjacent chlorine atoms is 3.65 A.
Chemical properties
[
edit
]
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
[
edit
]
UCl
6
is stable up to temperatures between 120 °C and 150 °C. The
decomposition
of
UCl
6
results in a solid phase transition from one crystal form of
UCl
6
to another more stable form.
[6]
However, the
decomposition
of
gaseous
UCl
6
produces
UCl
5
. The
activation energy
for this reaction is about 40 kcal per
mole
.
- 2 UCl
6
(g) → 2 UCl
5
(s) + Cl
2
(g)
Solubility
[
edit
]
UCl
6
is not a very
soluble
compound. It dissolves in
CCl
4
to give a brown solution. It is slightly soluble in isobutyl bromide and in
fluorocarbon
(
C
7
F
16
).
[6]
Reaction with hydrogen fluoride
[
edit
]
When
UCl
6
is reacted with purified anhydrous liquid
hydrogen fluoride
(HF) at room temperature produces
UF
5
.
[6]
- 2 UCl
6
+ 10 HF → 2 UF
5
+ 10 HCl + Cl
2
Synthesis
[
edit
]
Uranium hexachloride can be synthesized from the reaction of
uranium trioxide
(
UO
3
) with a mixture of liquid
CCl
4
and hot
chlorine
(
Cl
2
). The yield can be increased if the reaction carried out in the presence of
UCl
5
.
[7]
The
UO
3
is converted to
UCl
5
, which in turn reacts with the excess
Cl
2
to form
UCl
6
. 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 UO
3
+ 5 Cl
2
→ 2 UCl
5
+ 3 O
2
Step 2:
2 UCl
5
+ Cl
2
→ 2 UCl
6
Overall reaction:
2 UO
3
+ 6 Cl
2
→ 2 UCl
6
+ 3 O
2
This metal hexahalide can also be synthesized by blowing
Cl
2
gas over sublimed
UCl
4
at 350 °C.
[8]
Step 1:
2 UCl
4
+ Cl
2
→ 2 UCl
5
Step 2:
2 UCl
5
+ Cl
2
→ 2 UCl
6
Overall Reaction:
UCl
4
+ Cl
2
→ UCl
6
References
[
edit
]
- ^
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
.
- ^
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
.
- ^
Van Dyke, R. E.; Evers, E. C. (1955). "Preparation of Uranium Hexachloride".
Google Patents
: 2.
- ^
Batista, E. R.; Martin, R. L.; Hay, P. J. (2004).
"Density Functional Investigations of the Properties and Thermodynamics of UF
n
and UCl
n
(n=1,...,6)"
.
J. Chem. Phys
.
121
(22): 11104?11.
doi
:
10.1063/1.1811607
.
PMID
15634063
.
- ^
Lipkin, D.; Wessman, S. (1955). "Process and Apparatus for protecting Uranium hexachloride from Deterioration and Contamination".
Google Patents
: 2.
- ^
a
b
c
Katz, J.J.; Rabinowitch,E. (1951).
The Chemistry of Uranium
. Ann Arbor: The McGraw-Hill Book Company.
- ^
Van Dyke, R. E.; Evers, E. C. (1955). "Preparation of Uranium Hexachloride".
Google Patents
: 2.
- ^
Thornton, G.; Edelstein, N.; Rosch, N.; Woodwark, D.R.; Edgell, R.G. (1979). "The Electronic Structure of UCl
6
: Photoelectron Spectra and Scattered Wave X
α
Calculations".
J. Chem. Phys
.
70
(11): 6.
Bibcode
:
1979JChPh..70.5218T
.
doi
:
10.1063/1.437313
.
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U(II)
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U(III)
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U(IV)
| Organouranium(IV) compounds
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U(IV,V)
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U(IV,VI)
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U(V)
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U(VI)
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U(XII)
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Salts and covalent derivatives of the
chloride
ion
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