All eight valence electrons of xenon are involved in the bonds with the oxygen, and the oxidation state of the xenon atom is +8. Xenon trioxide is an unstable compound of xenon in its +6 oxidation state. It is a highly reactive compound of xenon. David S. Brock and Gary J. Schrobilgen . It is dangerously explosive upon contact with organic materials. [7] The crystals are stable for days in dry air, but readily absorb water from humid air to form a concentrated solution. [8][9], Except where otherwise noted, data are given for materials in their, "Crystal and Molecular Structure of Xenon Trioxide", Webelements periodic table: page on Xenon(VI) oxide, https://en.wikipedia.org/w/index.php?title=Xenon_trioxide&oldid=963056348, Articles with changed ChemSpider identifier, Pages using collapsible list with both background and text-align in titlestyle, Articles containing unverified chemical infoboxes, Creative Commons Attribution-ShareAlike License, This page was last edited on 17 June 2020, at 15:17. It is a very powerful oxidizing agent, and liberates oxygen from water slowly, accelerated by exposure to sunlight. 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 (O 2 ).
Xenon trioxide reacts with inorganic fluorides such as KF, RbF, or CsF to form stable solids of the form MXeO3F. The table shows element percentages for XeO 3 (xenon trioxide). Xenon trioxide is an unstable compound of xenon in its +6 oxidation state. [6], Hydrolysis of xenon hexafluoride or xenon tetrafluoride yields a solution from which colorless XeO3 crystals can be obtained by evaporation. It is dangerously explosive upon contact with organic materials. References. Above 25 °C, xenon trioxide is very prone to violent explosion: When it dissolves in water, an acidic solution of xenic acid is formed: This solution is stable at room temperature and lacks the explosive properties of xenon trioxide. The dialkali xenates do not appear to exist, as xenate disproportions in more alkaline conditions. It is a very powerful oxidizing agent, and liberates oxygen from water slowly, accelerated by exposure to sunlight.

[4] These are not stable and begin to disproportionate into perxenates (+8 oxidation state) and xenon and oxygen gas. [8], XeO3 should be handled with great caution. Except where otherwise noted, data are given for materials in their, "Crystal and Molecular Structure of Xenon Trioxide", Webelements periodic table: page on Xenon(VI) oxide. The density is 4.55 g/cm3.

At temperatures above −35.9 °C, xenon tetroxide is very prone to explosion, decomposing into xenon and oxygen gases with ΔH = −643 kJ/mol: Xenon tetroxide dissolves in water to form perxenic acid and in alkalis to form perxenate salts: Xenon tetroxide can also react with xenon hexafluoride to give xenon oxyfluorides: All syntheses start from the perxenates, which are accessible from the xenates through two methods. When it detonates, it releases xenon and oxygen gas. When it detonates, it releases xenon and oxygen gas. Samples have detonated when undisturbed at room temperature. Synthesis of the Missing Oxide of Xenon, XeO2, and Its Implications for Earth’s Missing Xenon. Any excess perxenic acid slowly undergoes a decomposition reaction to xenic acid and oxygen: Except where otherwise noted, data are given for materials in their, CS1 maint: multiple names: authors list (, https://en.wikipedia.org/w/index.php?title=Xenon_tetroxide&oldid=960620765, Pages using collapsible list with both background and text-align in titlestyle, Articles containing unverified chemical infoboxes, Creative Commons Attribution-ShareAlike License, This page was last edited on 3 June 2020, at 23:52. When it detonates, it releases xenon and oxygen 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]. Element % O: 26.77: Xe: 73.23: Isotope pattern for XeO 3. However, it is slow-acting and this reduces its usefulness.[2]. It is dangerously explosive upon contact with organic materials. The chart below shows the calculated isotope pattern for the formula XeO 3 with the most intense ion set to 100%. 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. DOI: 10.1021/jz502230b. Oxygen is the only element that can bring xenon up to its highest oxidation state; even fluorine can only give XeF6 (+6). It is a very powerful oxidizing agent, and liberates oxygen from water slowly, accelerated by exposure to sunlight. [3], Alternatively, it dissolves in alkaline solutions to form xenates. It is a very powerful oxidizing agent, and liberates oxygen from water slowly, accelerated by exposure to sunlight. The HXeO−4 anion is the predominant species in xenate solutions. XeO3F2 and XeO2F4 can be detected with mass spectrometry. Xenon tetroxide is a chemical compound of xenon and oxygen with molecular formula XeO 4, remarkable for being a relatively stable compound of a noble gas. Xenon trioxide is an unstable compound of xenon in its +6 oxidation state.

Xenon Suboxides Stable under Pressure. 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.

[5] Solid perxenates containing XeO4−6 have been isolated by reacting XeO3 with an aqueous solution of hydroxides. Dry crystals react explosively with cellulose. It is a powerful oxidizer. It oxidises carboxylic acids quantitatively to carbon dioxide and water. When it detonates, it releases xenon and oxy Xenon trioxide is an unstable compound of xenon in its +6 oxidation state. The perxenates are also compounds where xenon has the +8 oxidation state. The crystal structure is orthorhombic with a = 6.163 Å, b = 8.115 Å, c = 5.234 Å, and 4 molecules per unit cell. One is the disproportionation of xenates to perxenates and xenon: The other is oxidation of the xenates with ozone in basic solution: Barium perxenate is reacted with sulfuric acid and the unstable perxenic acid is dehydrated to give xenon tetroxide:[6].

The Journal of Physical Chemistry Letters 2014, 5 (24) , 4336-4342. Xenon trioxide is a strong oxidising agent and can oxidise most substances that are at all oxidisable. It is dangerously explosive upon contact with organic materials.
1.5H2O.


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