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Xenon tetroxide

From Wikipedia, the free encyclopedia
Noble gas compound
Xenon tetroxide
Xenon tetroxide
Xenon tetroxide
Space-filling model of the xenon tetroxide molecule
Space-filling model of the xenon tetroxide molecule
Names
IUPAC names
Xenon tetraoxide
Xenon(VIII) oxide
Other names
Xenon tetroxide
Perxenic anhydride
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/O4Xe/c1-5(2,3)4 checkY
    Key: VHWKDFQUJRCZDZ-UHFFFAOYSA-N checkY
  • InChI=1/O4Xe/c1-5(2,3)4
    Key: VHWKDFQUJRCZDZ-UHFFFAOYAS
  • O=[Xe](=O)(=O)=O
Properties
XeO4
Molar mass195.289 g·mol−1
AppearanceYellow solid below −36 °C (−33 °F; 237 K)
Melting point−35.9 °C (−32.6 °F; 237.2 K)
Boiling point0 °C (32 °F; 273 K)[1]
reacts
Structure
Tetrahedral[2]
0 D
Thermochemistry
+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 theirstandard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
Chemical compound

Xenon tetroxide is achemical compound ofxenon andoxygen with molecular formula XeO4, remarkable for being a relatively stablecompound of a noble gas. It is a yellowcrystallinesolid 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 eightvalence electrons of xenon are involved in the bonds with the oxygen, and theoxidation state of the xenon atom is +8. Oxygen is the onlyelement that can bring xenon up to its highest oxidation state; evenfluorine can only giveXeF6 (+6), though attempts to synthesizeXeF8 (+8) are still being made.

Two other short-livedxenon compounds with an oxidation state of +8,XeO3F2 andXeO2F4, are accessible by the reaction of xenon tetroxide withxenon hexafluoride.XeO3F2 andXeO2F4 can be detected withmass spectrometry. Theperxenates are also compounds where xenon has the +8 oxidation state.

Reactions

[edit]

At temperatures above −35.9 °C (−32.6 °F), 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 formperxenic acid and in alkalis to formperxenate salts:

XeO4 + 2 H2O → H4XeO6
XeO4 + 4 NaOH → Na4XeO6 + 2 H2O

Xenon tetroxide can also react withxenon hexafluoride to give xenon oxyfluorides:

XeO4 + XeF6 → XeOF4 + XeO3F2
XeO4 + 2XeF6 → XeO2F4 + 2 XeOF4

Synthesis

[edit]

All syntheses start from theperxenates, which are accessible from thexenates through two methods. One is thedisproportionation of xenates to perxenates and xenon:

2 HXeO−4 + 2 OH− → XeO4−6 + Xe + O2 + 2 H2O

The other is oxidation of the xenates withozone in basic solution:

HXeO−4 + O3 + 3 OH− → XeO4−6 + O2 + 2 H2O

Barium perxenate is reacted withsulfuric acid and the unstable perxenic acid is dehydrated to give xenon tetroxide:[6]

Ba2XeO6 + 2 H2SO4 → 2 BaSO4 + H4XeO6
H4XeO6 → 2 H2O + XeO4

Any excessperxenic acid slowly undergoes a decomposition reaction toxenic acid and oxygen:

2 H4XeO6 → O2 + 2 H2XeO4 + 2 H2O

References

[edit]
  1. ^Lide, David R. (1998).Handbook of Chemistry and Physics (87 ed.). Boca Raton, Florida: CRC Press. p. 494.ISBN 0-8493-0594-2.
  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.
  3. ^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.
  4. ^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)
  5. ^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.
  6. ^A. Earnshaw; Norman Greenwood (1997).Chemistry of the Elements (2nd ed.). Elsevier. p. 901.ISBN 9780080501093.
Xenon(0)
Xenon(I)
Xenon(II)
Organoxenon(II) compounds
  • XeC6F5F
  • XeC6F5C2F3
  • XeC6F5CF3
  • Xe(C6F5)2
  • XeC6F5C6H2F3
  • XeC6F5CN
  • Xe(CF3)2
    • Xenon(IV)
    Organoxenon(IV) compounds
  • XeF2C6F5BF4
    • Xenon(VI)
    Xenon(VIII)
    Helium compounds
    Neon compounds
    Argon compounds
    Krypton compounds
    Xenon compounds
    Xe(0)
    Xe(I)
    Xe(II)
    Xe(IV)
    Xe(VI)
    Xe(VIII)
    Radon compounds
    Rn(II)
    Rn(IV)
    Rn(VI)
    Oganesson compounds
    (predicted)
    Og(0)
    • Og2‡
    • OgH+‡
    Og(II)
    • OgF2‡
    • OgCl2‡
    • OgO‡
    Og(IV)
    • OgF4‡
    • OgO2‡
    • OgTs4‡
    Og(VI)
    • OgF6‡
    Mixed oxidation states
    +1 oxidation state
    +2 oxidation state
    +3 oxidation state
    +4 oxidation state
    +5 oxidation state
    +6 oxidation state
    +7 oxidation state
    +8 oxidation state
    Related
    Oxides are sorted byoxidation state.Category:Oxides
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