How are xenon trioxide and xenon oxygen pentafluoride are prepared?
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At temperatures above −35.9 °C, xenon tetroxide is very prone to explosion, decomposing into xenon gas and oxygen with ΔH = −643 kJ/mol:
XeO4 → Xe + 2 O2
Xenon tetroxide dissolves in water to formperxenic acid and in alkalis to form perxenatesalts:
XeO4 + 2 H2O → H4XeO6XeO4 + 4 NaOH → Na4XeO6 + 2 H2O
Xenon tetroxide can also react with xenon hexafluoride to give xenon oxyfluorides:
XeO4 + XeF6 → XeOF4 + XeO3F2XeO4 + 2XeF6 → XeO2F4 + XeOF4
Xenon tetroxide is a chemical compound ofxenon and oxygen with molecular formula XeO4, remarkable for being a relatively stablecompound of a noble gas. It is a yellowcrystalline 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; evenfluorine 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 XeO2F4can be detected with mass spectrometry. Theperxenates are also compounds where xenon has the +8 oxidation state.
XeO4 → Xe + 2 O2
Xenon tetroxide dissolves in water to formperxenic acid and in alkalis to form perxenatesalts:
XeO4 + 2 H2O → H4XeO6XeO4 + 4 NaOH → Na4XeO6 + 2 H2O
Xenon tetroxide can also react with xenon hexafluoride to give xenon oxyfluorides:
XeO4 + XeF6 → XeOF4 + XeO3F2XeO4 + 2XeF6 → XeO2F4 + XeOF4
Xenon tetroxide is a chemical compound ofxenon and oxygen with molecular formula XeO4, remarkable for being a relatively stablecompound of a noble gas. It is a yellowcrystalline 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; evenfluorine 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 XeO2F4can be detected with mass spectrometry. Theperxenates are also compounds where xenon has the +8 oxidation state.
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