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| Names | |||
|---|---|---|---|
| IUPAC names
Xenon tetraoxide
Xenon(VIII) oxide | |||
| Other names
Xenon tetroxide
Perxenic anhydride | |||
| Identifiers | |||
3D model (JSmol)
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| ChemSpider | |||
CompTox Dashboard (EPA)
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| Properties | |||
| XeO4 | |||
| Molar mass | 195.29 g mol−1 | ||
| Appearance | Yellow solid below −36 °C | ||
| Melting point | −35.9 °C (−32.6 °F; 237.2 K) | ||
| Boiling point | 0 °C (32 °F; 273 K)[1] | ||
| reacts | |||
| Structure | |||
| Tetrahedral[2] | |||
| 0 D | |||
| Thermochemistry | |||
Std enthalpy of
formation (ΔfH⦵298) |
+153.5 kcal mol−1 [3] | ||
| Hazards | |||
| Occupational safety and health (OHS/OSH): | |||
Main hazards
|
powerful explosive | ||
| Related compounds | |||
Related compounds
|
Perxenic acid Xenon trioxide | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Xenon tetroxide is a chemical compound of xenon and oxygen with molecular formula XeO4, remarkable for being a relatively stable compound of a noble gas. It is a yellow crystalline solid that is stable below −35.9 °C; above that temperature it is very prone to exploding and decomposing into elemental xenon and oxygen (O2).[4][5]
All eight valence electrons of xenon are involved in the bonds with the oxygen, and the oxidation state of the xenon atom is +8. Oxygen is the only element that can bring xenon up to its highest oxidation state; even fluorine can only give XeF6 (+6).
Two other short-lived xenon compounds with an oxidation state of +8, XeO3F2 and XeO2F4, are accessible by the reaction of xenon tetroxide with xenon hexafluoride. XeO3F2 and XeO2F4 can be detected with mass spectrometry. The perxenates are also compounds where xenon has the +8 oxidation state.
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Transcription
Reactions
At temperatures above −35.9 °C, xenon tetroxide is very prone to explosion, decomposing into xenon and oxygen gases with ΔH = −643 kJ/mol:
- XeO4 → Xe + 2 O2
Xenon tetroxide dissolves in water to form perxenic acid and in alkalis to form perxenate salts:
- XeO4 + 2 H2O → H4XeO6
- XeO4 + 4 NaOH → Na4XeO6 + 2 H2O
Xenon tetroxide can also react with xenon hexafluoride to give xenon oxyfluorides:
- XeO4 + XeF6 → XeOF4 + XeO3F2
- XeO4 + 2XeF6 → XeO2F4 + 2 XeOF4
Synthesis
All syntheses start from the perxenates, which are accessible from the xenates through two methods. One is the disproportionation of xenates to perxenates and xenon:
- 2 HXeO−
4 + 2 OH− → XeO4−
6 + Xe + O2 + 2 H2O
The other is oxidation of the xenates with ozone in basic solution:
- HXeO−
4 + O3 + 3 OH− → XeO4−
6 + O2 + 2 H2O
Barium perxenate is reacted with sulfuric acid and the unstable perxenic acid is dehydrated to give xenon tetroxide:[6]
- Ba
2XeO
6 + 2 H
2SO
4 → 2 BaSO
4 + H
4XeO
6 - H
4XeO
6 → 2 H
2O + XeO
4
Any excess perxenic acid slowly undergoes a decomposition reaction to xenic acid and oxygen:
- 2 H
4XeO
6 → O
2 + 2 H
2XeO
4 + 2 H
2O
References
- ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. p. 494. ISBN 0-8493-0594-2.
- ^ G. Gundersen; K. Hedberg; J. L.Huston (1970). "Molecular Structure of Xenon Tetroxide, XeO4". J. Chem. Phys. 52 (2): 812–815. Bibcode:1970JChPh..52..812G. doi:10.1063/1.1673060.
- ^ Gunn, S. R. (May 1965). "The Heat of Formation of Xenon Tetroxide". Journal of the American Chemical Society. 87 (10): 2290–2291. doi:10.1021/ja01088a038.
- ^
H.Selig, J. G. Malm, H. H. Claassen, C. L. Chernick, J. L. Huston (1964). "Xenon tetroxide – Preparation & Some Properties". Science. 143 (3612): 1322–3. Bibcode:1964Sci...143.1322S. doi:10.1126/science.143.3612.1322. JSTOR 1713238. PMID 17799234. S2CID 29205117.
{{cite journal}}: CS1 maint: multiple names: authors list (link) - ^ J. L. Huston; M. H. Studier; E. N. Sloth (1964). "Xenon tetroxide — Mass Spectrum". Science. 143 (3611): 1162–3. Bibcode:1964Sci...143.1161H. doi:10.1126/science.143.3611.1161-a. JSTOR 1712675. PMID 17833897. S2CID 28547895.
- ^ A. Earnshaw; Norman Greenwood (1997). Chemistry of the Elements (2nd ed.). Elsevier. p. 901. ISBN 9780080501093.
- Lide, D. R., ed. (2002). CRC Handbook of Chemistry and Physics (83rd ed.). Boca Raton, FL: CRC Press. ISBN 0-8493-0483-0.
This page was last edited on 24 September 2023, at 23:58