Xenon nitrate: Difference between revisions
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{{Short description|Chemical compound}} |
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'''Xenon nitrate''' is a transient compound made by reacting [[xenon difluoride]] with anhydrous nitric acid. Although xenon dinitrate (Xe(NO<sub>3</sub>)<sub>2</sub>) has not been isolated and characterised a related mononitrate: '''xenon fluoride nitrate''' has been made and studied. |
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{{Chembox |
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|Section1={{Chembox Identifiers |
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|SMILES = [O-][N+](=O)O[Xe]O[N+](=O)[O-] |
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|StdInChI=1S/N2O6Xe/c3-1(4)7-9-8-2(5)6 |
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|StdInChIKey=DDUBBJJTDIIEIU-UHFFFAOYSA-N |
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}} |
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|Section2={{Chembox Properties |
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|Xe=1|N=2|O=6 |
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}} |
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|Section3={{Chembox Related |
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|OtherCompounds = [[xenon fluoride nitrate|FXeNO<sub>3</sub>]] |
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'''Xenon nitrate''', also called '''xenon dinitrate''', is an [[inorganic compound]] consisting of one [[xenon]] atom bonded to two [[nitrate]] groups. It can be made by reacting [[xenon difluoride]] with [[anhydrous]] [[nitric acid]], but it only exists transiently before decomposing, and therefore it has not been isolated and fully characterized. A related compound, [[xenon fluoride nitrate]], has been made and is stable enough to be studied in more detail. |
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==Production== |
==Production== |
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Attempted production has used |
Attempted production has used the following reaction:<ref name="MoranM2007">{{cite thesis|type=PhD|last=Moran|first=Matthew D.|title=Synthesis and Structural Characterization of new Xenon(II) Compounds and the Use of a Xenon(II) Cation as an Oxidant for the Preparation of Halogenated Hydrocarbons|url=https://macsphere.mcmaster.ca/bitstream/11375/14167/1/fulltext.pdf|access-date=4 Oct 2014|year=2007|publisher=McMaster University|pages=42, 99–145}}</ref><ref name="Eisenberg1970">{{cite journal|last=Eisenberg|first=Max|author2=Darryl D. DesMarteau|year=1970|title=The reaction of xenon difluoride with some strong oxy-acids|journal=Inorganic and Nuclear Chemistry Letters|volume=6|issue=1|pages=29–34|issn=0020-1650|doi=10.1016/0020-1650(70)80279-3}}</ref> |
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XeF<sub>2</sub> + 2HNO<sub>3</sub> → Xe(NO<sub>3</sub>)<sub>2</sub> + 2HF<ref name="Eisenberg1970">{{cite journal|last=Eisenberg|first=Max|coauthors=Darryl D. DesMarteau|year=1970|title=The reaction of xenon difluoride with some strong oxy-acids|journal=Inorganic and Nuclear Chemistry Letters|volume=6|issue=1|pages=29–34|issn=00201650|doi=10.1016/0020-1650(70)80279-3}}</ref><ref name="Zefirov91">{{cite journal|last=Zefirov|first=N. S|coauthors=Gakh, A. A.; Zhdankin, V. V.; Stang, P. J.|year=1991|title=Interaction of Fluoroxenonium Triflate, Fluorosulfate, and Νitrate with Alkenes. Stereochemical Evidence for the Electrophilic Noble Gas Cation Addition to the Carbon-Carbon Double Bond|journal=J. Org. Chem|volume=56|pages=1416–1418}}</ref> |
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This reaction |
This reaction makes a red-brown solid. However, it decomposes spontaneously at 23 °C, turning blue temporarily while doing so:<ref name="Eisenberg1970"/> |
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:Xe(NO<sub>3</sub>)<sub>2</sub> → Xe + O<sub>2</sub>NOONO<sub>2</sub> (an unstable nitrogen [[main group peroxides|peroxide]]) |
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However a nixed nitrate definitely exists FXeONO<sub>2</sub>.<ref name="MoranM2007"/> This has been called '''fluoroxenonium nitrate'''<ref name="Atta-ur-Rahman2006">{{cite book|last=Atta-ur-Rahman|first=|title=Advances in Organic Synthesis: Modern Organofluorine Chemistry-Synthetic Aspects|url=http://books.google.com/books?id=vkcLOFEo9xIC&pg=PA78|accessdate=5 October 2014|date=2006-01-01|publisher=Bentham Science Publishers|isbn=9781608051984|page=78}}</ref> and xenon fluoride nitrate.<ref name="Moran2010">{{cite journal|last=Moran|first=Matthew D.|coauthors=David S. Brock, Hélène P. A. Mercier, Gary J. Schrobilgen|year=2010|title=Xe3OF3+, a Precursor to a Noble-Gas Nitrate; Syntheses and Structural Characterizations of FXeONO2, XeF2·HNO3, and XeF2·N2O4|journal=Journal of the American Chemical Society|volume=132|issue=39|pages=13823–13839|issn=0002-7863|doi=10.1021/ja105618w}}</ref> |
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This is formed via the reaction:<ref name="MoranM2007"/> |
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[FXeOXeFXeF][AsF<sub>6</sub>] + 2NO<sub>2</sub>F → FXeONO<sub>2</sub> +NO<sub>2</sub>AsF<sub>6</sub>. |
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Purification of FXeONO<sub>2</sub> can take place by dissolving in SO<sub>2</sub>ClF which leaves the nitronium arsenic hexafluoride behind as a solid.<ref name="MoranM2007"/> |
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An alternate low yield method to make FXeONO<sub>2</sub> is to dissolve [[xenon difluoride]] in liquid [[dinitrogen tetroxide]].<ref name="MoranM2007"/> |
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Xe<sub>2</sub> + NO<sup>+</sup> + NO<sub>3</sub><sup>-</sup> → FXeONO<sub>2</sub> + NOF at 0°C |
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This method is inefficient as not much nitrate ion exists in the liquid and the xenon nitrate decomposes.<ref name="MoranM2007"/> |
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Another method claimed to make this substance is:<ref name="MoranM2007"/> |
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==Properties== |
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FXeONO<sub>2</sub> is a white crystalline material.<ref name="MoranM2007"/> The [[space group]] of the crystals is P2<sub>1</sub>/c which is [[monoclinic]]. The unit cell contains four molecules with a total volume of 386.6 Å<sup>3</sup>. The unit cell dimensions are a=4.6663, b=8.799 Å c=9.415 Å, and non-perpendicular angle β=90.325° and with other axes angles α and γ = 90°.<ref name="MoranM2007"/> With a molecular weight of 212.3 the crystal has density 3.648. (These measurements at -173°C.)<ref name="MoranM2007"/> |
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The molecule has bond lengths of xenon to fluorine 1.992 Å, xenon to oxygen 2.126 Å, xenon bonded oxygen to nitrogen 1.36 Å, and other nitrate oxygen bonds are 1.199 (cis) and 1.224 Å (trans).<ref name="MoranM2007"/> The bond angles are FXeO 177.6°, XeON 114.7°, (Xe)ONO 114.5° (cis), other (Xe)ONO 118.4° (trans) and (non-Xe)ONO is 127.1°.<ref name="MoranM2007"/> The bond lengths and angles on the xenon atom are similar to that in FXeOSO<sub>2</sub>F and FXeOTeF<sub>5</sub> indicating a polar oxygen bond. The Xe-O-N angle is larger than halogen nitrates, which indicates a lower bond density for Xe-O bond. N-O<sub>cis</sub> bond length is longer than the N-O<sub>trans</sub> bond length, the opposite to other halogen nitrates.<ref name="MoranM2007"/> |
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FXeONO<sub>2</sub> is not particularly stable and slowly breaks down at -78°C yielding XeF<sub>2</sub>.N<sub>2</sub>O<sub>4</sub>. This happens on a timescale of several days.<ref name="MoranM2007"/> |
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At 0°C FXeONO<sub>2</sub> has a half life of seven hours decomposing to XeF<sub>2</sub>.<ref name="MoranM2007"/> |
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==References== |
==References== |
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{{reflist}} |
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<references /> |
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{{Xenon compounds}} |
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{{nitrates}} |
{{nitrates}} |
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{{noble gas compounds}} |
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[[Category:Xenon(II) compounds]] |
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[[Category:Nitrates]] |
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Latest revision as of 18:34, 16 March 2024
| Identifiers | |
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3D model (JSmol)
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| Properties | |
| N2O6Xe | |
| Molar mass | 255.301 g·mol−1 |
| Related compounds | |
Related compounds
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FXeNO3 |
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 nitrate, also called xenon dinitrate, is an inorganic compound consisting of one xenon atom bonded to two nitrate groups. It can be made by reacting xenon difluoride with anhydrous nitric acid, but it only exists transiently before decomposing, and therefore it has not been isolated and fully characterized. A related compound, xenon fluoride nitrate, has been made and is stable enough to be studied in more detail.
Production
[edit]Attempted production has used the following reaction:[1][2]
- XeF2 + 2 HNO3 → Xe(NO3)2 + 2 HF
This reaction makes a red-brown solid. However, it decomposes spontaneously at 23 °C, turning blue temporarily while doing so:[2]
- Xe(NO3)2 → Xe + O2NOONO2 (an unstable nitrogen peroxide)
References
[edit]- ^ Moran, Matthew D. (2007). Synthesis and Structural Characterization of new Xenon(II) Compounds and the Use of a Xenon(II) Cation as an Oxidant for the Preparation of Halogenated Hydrocarbons (PDF) (PhD). McMaster University. pp. 42, 99–145. Retrieved 4 Oct 2014.
- ^ a b Eisenberg, Max; Darryl D. DesMarteau (1970). "The reaction of xenon difluoride with some strong oxy-acids". Inorganic and Nuclear Chemistry Letters. 6 (1): 29–34. doi:10.1016/0020-1650(70)80279-3. ISSN 0020-1650.