Wikipedia:WikiProject Chemicals/Chembox validation/VerifiedDataSandbox and Xenon trioxide: Difference between pages

| Verifiedfields = changed

| verifiedrevid = 476998178

| Name = Xenon trioxide

| ImageFile = Xenon-trioxide-2D.png

| ImageSize = 180px

| ImageName = Structural formula, showing lone pair

| ImageFile1 = Xenon-trioxide-3D-vdW.png

| ImageSize1 = 160px

| ImageName1 = Space-filling model

| IUPACName = Xenon trioxide<br />Xenon(VI) oxide

| OtherNames = Xenic anhydride

|Section1={{Chembox Identifiers

| InChI = 1/O3Xe/c1-4(2)3

| InChIKey = ZWAWYSBJNBVQHP-UHFFFAOYAR

| SMILES = [O-] [Xe+3]([O-])[O-]

| StdInChI = 1S/O3Xe/c1-4(2)3

| StdInChIKey = ZWAWYSBJNBVQHP-UHFFFAOYSA-N

| CASNo_Ref = {{cascite|correct|CAS}}

| CASNo = 13776-58-4

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = IM8XMX5O5Q

| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}

| ChemSpiderID =21106493

|Section2={{Chembox Properties

| Formula = XeO₃

| MolarMass = 179.288 g/mol

| Appearance = colourless crystalline solid

| Density = 4.55 g/cm³, solid

| Solubility = Soluble (with reaction)

| MeltingPtC = 25

| MeltingPt_notes = ''Violent decomposition''

| pKa =

|Section3={{Chembox Structure

| MolShape = [[Trigonal pyramidal molecular geometry|trigonal pyramidal]] (C_3v)

|Section4={{Chembox Thermochemistry

| DeltaHf = 402&nbsp;kJ·mol⁻¹<ref name=b1>{{cite book| author = Zumdahl, Steven S.|title =Chemical Principles 6th Ed.| publisher = Houghton Mifflin Company| year = 2009| isbn = 978-0-618-94690-7|page=A23}}</ref>

| Entropy =

}}

|Section7={{Chembox Hazards

| NFPA-H = 4 | NFPA-R=4 | NFPA-F=0 | NFPA-S = OX}}

|Section8={{Chembox Related

| OtherCompounds = [[Xenon tetroxide]]<br>[[Xenic acid]]

'''Xenon trioxide''' is an unstable [[Noble gas compounds|compound]] of [[xenon]] in its +6 [[oxidation state]]. It is a very powerful [[oxidizing agent]], and liberates oxygen from water slowly, accelerated by exposure to sunlight. It is dangerously explosive upon contact with organic materials. When it detonates, it releases xenon and oxygen gas.

==Chemistry==

Synthesis of xenon trioxide is by aqueous hydrolysis of {{chem|XeF|6|link=Xenon hexafluoride}}:<ref name=Advances />

:{{chem|XeF|6}} + 3 {{chem|H|2|O}} → {{chem|XeO|3}} + 6 HF

The resulting xenon trioxide crystals are a strong oxidising agent and can oxidise most substances that are at all oxidisable. However, it is slow-acting and this reduces its usefulness.<ref>{{cite book | title = Chemistry of the Elements | author1 = Greenwood, N. | author2 = Earnshaw, A. | publisher = Butterworth-Heinemann | year = 1997 | location = Oxford }}</ref>

Above 25 °C, xenon trioxide is very prone to violent explosion:

:2 XeO₃ → 2 Xe + 3 O₂ {{pad|5em}}(Δ_f''H'' = −403&nbsp;[[Joule|kJ]]/[[Mole (unit)|mol]])

When it dissolves in water, an acidic solution of [[xenic acid]] is formed:

:XeO₃(aq) + H₂O → H₂XeO₄ {{eqm}} H⁺ + {{chem|HXeO|4|-}}

This solution is stable at room temperature and lacks the explosive properties of xenon trioxide. It oxidises [[carboxylic acid]]s quantitatively to [[carbon dioxide]] and [[properties of water|water]].<ref>{{cite journal | journal = Talanta |date=July 1966 | volume = 13 | issue = 7 | pages = 945–949 | title = Titrimetric determination of some organic acids by xenon trioxide oxidation | author1 = Jaselskis B. | author2 = Krueger R. H. | pmid = 18959958 | doi = 10.1016/0039-9140(66)80192-3 }}</ref>

Alternatively, it dissolves in alkaline solutions to form ''xenates''. The {{chem|HXeO|4|-}} anion is the predominant species in xenate solutions.<ref>{{Cite journal| last1 = Peterson | first1 = J. L.| last2 = Claassen | first2 = H. H.| last3 = Appelman | first3 = E. H.| title = Vibrational spectra and structures of xenate(VI) and perxenate(VIII) ions in aqueous solution| journal = Inorganic Chemistry | volume = 9| issue = 3| pages = 619–621 | date=March 1970 | doi = 10.1021/ic50085a037}}</ref> These are not stable and begin to [[disproportionation|disproportionate]] into [[perxenate]]s (+8 oxidation state) and xenon and oxygen gas.<ref>{{cite book

| title = Main group chemistry

| url = https://archive.org/details/maingroupchemist00hend_891

| url-access = limited

| author = W. Henderson

| location = Great Britain

| publisher = Royal Society of Chemistry

| year = 2000

| isbn = 0-85404-617-8

| pages = [https://archive.org/details/maingroupchemist00hend_891/page/n161 152]–153

}}</ref> Solid perxenates containing {{chem|XeO|6|4-}} have been isolated by reacting {{chem|XeO|3|}} with an aqueous solution of hydroxides. Xenon trioxide reacts with inorganic fluorides such as KF, RbF, or CsF to form stable solids of the form {{chem|MXeO|3|F}}.<ref>{{cite book

| title = Inorganic chemistry

| author1 = Egon Wiberg

| author2 = Nils Wiberg

| author3 = Arnold Frederick Holleman

| publisher = Academic Press

| year = 2001

| isbn = 0-12-352651-5

| page = 399

}}</ref>

==Physical properties==

Hydrolysis of [[xenon hexafluoride]] or [[xenon tetrafluoride]] yields a solution from which colorless XeO₃ crystals can be obtained by evaporation.<ref name=Advances>{{cite book | series = Advances in Inorganic Chemistry, Volume 46 | title = Recent Advances in Noble-gas Chemistry | author1 = John H. Holloway | author2 = Eric G. Hope | editor = A. G. Sykes | publisher = Academic Press | year = 1998 | isbn = 0-12-023646-X | page = 65 }}</ref> The crystals are stable for days in dry air, but readily absorb water from humid air to form a concentrated solution. The crystal structure is [[orthorhombic]] with ''a'' = 6.163 Å, ''b'' = 8.115 Å, ''c'' = 5.234 Å, and 4 molecules per unit cell. The density is 4.55 g/cm³.<ref name="xe">{{Cite journal | doi = 10.1021/ja00889a037 | year = 1963 | last1 = Templeton | first1 = D. H. | title = Crystal and Molecular Structure of Xenon Trioxide | last2 = Zalkin | first2 = A. | last3 = Forrester | first3 = J. D. | last4 = Williamson | first4 = S. M. | journal = Journal of the American Chemical Society | volume = 85 | issue = 6| pages = 817 | url = https://escholarship.org/uc/item/4d31b0pf }}</ref>

{| class="wikitable" style="margin:1em auto; text-align:center;"

| [[File:Xenon-trioxide-xtal-1963-3D-balls.png|200px]]||[[File:Xenon-trioxide-xtal-1963-3D-SF.png|200px]]||[[File:Xenon-trioxide-xtal-1963-Xe-coordination-3D-balls.png|180px]]

|-

| <small>[[ball-and-stick model]] of part of<br />the crystal structure of XeO₃</small>||<small>[[space-filling model]]</small>||<small>coordination geometry of XeO₃</small>

|}

==Safety==

XeO₃ should be handled with great caution. Samples have detonated when undisturbed at room temperature. Dry crystals react explosively with cellulose.<ref name="xe"/><ref>{{Cite journal | doi = 10.1126/science.139.3554.506 | title = Xenon Hydroxide: an Experimental Hazard | year = 1963 | last1 = Bartlett | first1 = N. | last2 = Rao | first2 = P. R. | journal = Science | volume = 139 | issue = 3554| pages = 506 | pmid = 17843880|bibcode = 1963Sci...139..506B }}</ref>

==References==

{{reflist}}

==External links==

* [http://www.webelements.com/webelements/compounds/text/Xe/O3Xe1-13776584.html Webelements periodic table: page on Xenon(VI) oxide]

{{Xenon compounds}}

{{Noble gas compounds}}

{{Oxides}}

[[Category:Oxides]]

[[Category:Xenon(VI) compounds]]

[[Category:Inorganic compounds]]