| |
| Identifiers | |
|---|---|
3D model (
JSmol)
|
|
PubChem
CID
|
|
| |
| |
| Properties | |
| Cl4Xe | |
| Molar mass | 273.09 g·mol−1 |
| Related compounds | |
Related compounds
|
XeF4, XeCl2, XeCl |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
| |
Xenon tetrachloride is an unstable
[1]
inorganic compound with the
chemical formula XeCl4. Unlike other
noble gas/
halide compounds, it cannot be
synthesized by simply combining the
elements, by using a more-active halogenating agent, or by
substitution of other halides on tetrahaloxenon compounds. Instead, a
decay technique can be used, starting with K129ICl4. The
iodine-129 atom of the 129
ICl–
4
covalent cluster is
radioactive and undergoes
beta decay to become
xenon-129.
[2]
[3] The resulting XeCl4 molecule has a
square planar molecular geometry analogous to
xenon tetrafluoride.
[4]
Alternately, the product can be obtained by subjecting the elements to an electric discharge. [1]
References
- ^ a b Holleman, A.F.; Wiberg, E.; Wiberg, N.; Eagleson, M.; Brewer, W. (2001). Inorganic Chemistry. Academic Press. p. 394. ISBN 9780123526519. LCCN 2001091215.
- ^ Bell, C.F. (2013). Syntheses and Physical Studies of Inorganic Compounds. Elsevier Science. p. 143. ISBN 9781483280608.
- ^ Cockett, A.H.; Smith, K.C.; Bartlett, N. (2013). The Chemistry of the Monatomic Gases: Pergamon Texts in Inorganic Chemistry. Elsevier Science. p. 292. ISBN 9781483157368.
- ^ Perlow, G. J.; Perlow, M. R. (15 August 1964). "Mössbauer Effect Evidence for the Existence and Structure of XeCl4". The Journal of Chemical Physics. 41 (4): 1157–1158. Bibcode: 1964JChPh..41.1157P. doi: 10.1063/1.1726022.
|
| |
| Identifiers | |
|---|---|
3D model (
JSmol)
|
|
PubChem
CID
|
|
| |
| |
| Properties | |
| Cl4Xe | |
| Molar mass | 273.09 g·mol−1 |
| Related compounds | |
Related compounds
|
XeF4, XeCl2, XeCl |
Except where otherwise noted, data are given for materials in their
standard state (at 25 °C [77 °F], 100 kPa).
| |
Xenon tetrachloride is an unstable
[1]
inorganic compound with the
chemical formula XeCl4. Unlike other
noble gas/
halide compounds, it cannot be
synthesized by simply combining the
elements, by using a more-active halogenating agent, or by
substitution of other halides on tetrahaloxenon compounds. Instead, a
decay technique can be used, starting with K129ICl4. The
iodine-129 atom of the 129
ICl–
4
covalent cluster is
radioactive and undergoes
beta decay to become
xenon-129.
[2]
[3] The resulting XeCl4 molecule has a
square planar molecular geometry analogous to
xenon tetrafluoride.
[4]
Alternately, the product can be obtained by subjecting the elements to an electric discharge. [1]
References
- ^ a b Holleman, A.F.; Wiberg, E.; Wiberg, N.; Eagleson, M.; Brewer, W. (2001). Inorganic Chemistry. Academic Press. p. 394. ISBN 9780123526519. LCCN 2001091215.
- ^ Bell, C.F. (2013). Syntheses and Physical Studies of Inorganic Compounds. Elsevier Science. p. 143. ISBN 9781483280608.
- ^ Cockett, A.H.; Smith, K.C.; Bartlett, N. (2013). The Chemistry of the Monatomic Gases: Pergamon Texts in Inorganic Chemistry. Elsevier Science. p. 292. ISBN 9781483157368.
- ^ Perlow, G. J.; Perlow, M. R. (15 August 1964). "Mössbauer Effect Evidence for the Existence and Structure of XeCl4". The Journal of Chemical Physics. 41 (4): 1157–1158. Bibcode: 1964JChPh..41.1157P. doi: 10.1063/1.1726022.