Noble gas compound - wikipedia Noble gas compound This article has multiple issues. Please help improve it or discuss these issues on the talk page. ( Learn how and when to remove these template messages ) This article needs additional citations for verification. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. ( January 2015 ) This article relies too much on references to primary sources. Please improve this by adding secondary or tertiary sources. ( January 2015 ) Noble gas compounds are chemical compounds that include an element from the noble gases, group 18 of the periodic table. Although the noble gases are generally unreactive elements, many such compounds have been observed, particularly involving the element xenon. From the standpoint of chemistry, the noble gases may be divided into two groups : the relatively reactive krypton ( ionisation energy 14.0 eV ), xenon ( 12.1 eV ), and radon ( 10.7 eV ) on one side, and the very unreactive argon ( 15.8 eV ), neon ( 21.6 eV ), and helium ( 24.6 eV ) on the other. The heavier noble gases have more electron shells than the lighter ones. Hence, the outermost electrons are subject to a shielding effect from the inner electrons that makes them more easily ionized, since they are less strongly attracted to the positively charged nucleus. This results in an ionization energy low enough to form stable compounds with the most electronegative elements, fluorine and oxygen, and even with less electronegative elements such as nitrogen and carbon under certain circumstances. Contents 1 History and background 2 True noble gas compounds 2.1 Radon compounds 2.2 Xenon compounds 2.3 Krypton compounds 2.4 Argon compounds 2.5 Neon and helium compounds 3 Reports prior to xenon hexafluoroplatinate and xenon tetrafluoride 3.1 Clathrates 3.2 Coordination compounds 3.3 Hydrates 4 Fullerene adducts 5 Applications 6 References 7 Resources History and background When the family of noble gases was first identified at the end of the nineteenth century, none of them was observed to form any compounds and it was initially believed that they were all inert gases ( as they were then known ) which could not form compounds. With the development of atomic theory in the early twentieth century, their inertness was ascribed to a full valence shell of electrons which render them very chemically stable and nonreactive. All noble gases have full s and p outer electron shells ( except helium, which has no p sublevel ), and so do not form chemical compounds easily. Their high ionization energy and almost zero electron affinity explain their non-reactivity. In 1933, Linus Pauling predicted that the heavier noble gases would be able to form compounds with fluorine and oxygen. Specifically, he predicted the existence of krypton hexafluoride ( Kr F ) and xenon hexafluoride ( Xe F ), speculated that XeF might exist as an unstable compound, and suggested that xenic acid would form perxenate salts. These predictions proved quite accurate, although subsequent predictions for XeF indicated that it would be not only thermodynamically unstable, but kinetically unstable. As of 2013, XeF has not been made, although the octafluoroxenate ( VI ) anion ( XeF ) has been observed. By 1960, no compound with a covalently bound noble gas atom had yet been synthesized. The first published report, in June 1962, of a noble gas compound was by Neil Bartlett, who noticed that the highly oxidising compound platinum hexafluoride ionised O to O. As the ionisation energy of O to O ( 1165 kJ mol ) is nearly equal to the ionisation energy of Xe to Xe ( 1170 kJ mol ), he tried the reaction of Xe with PtF. This yielded a crystalline product, xenon hexafluoroplatinate, whose formula was proposed to be Xe ( PtF. It was later shown that the compound is actually more complex, containing both XeFPtF and XeFPt F. Nonetheless, this was the first real compound of any noble gas. The first binary noble gas compounds were reported later in 1962. Neil Bartlett synthesized Xenon tetrafluoride ( XeF ) by subjecting a mixture of xenon and fluorine to high temperature. Rudolf Hoppe, among other groups, synthesized xenon difluoride ( XeF ) by the reaction of the elements. Following the first successful synthesis of xenon compounds, synthesis of krypton difluoride ( KrF ) was reported in 1963. True noble gas compounds These compounds are listed in order of decreasing order of the atomic weight of the noble gas, which generally reflects the priority of their discovery, and the breadth of available information for these compounds, with the exception of radon due to its radioactivity. Radon compounds Radon is not chemically inert, but its short half - life and the high energy of its radioactivity make it difficult to investigate its sole described fluoride ( RnF ), its sole described oxide ( RnO ), and their reaction products. Xenon compounds After the initial 1962 studies on XeF and XeF, xenon compounds that have been synthesized include other fluorides ( XeF ), oxyfluorides ( XeOF, XeOF, XeO F, XeO F, XeO F ) and oxides ( XeO, XeO and XeO ). Xenon difluoride has been produced by the exposure of Xe and F gases to sunlight, a result which eluded observation for 50 years. Xenon fluorides react with several other fluorides to form fluoroxenates, such as sodium octafluoroxenate ( Na XeF ), and fluoroxenonium salts, such as trifluoroxenonium hexafluoroantimoniate ( XeF SbF ). In terms of other halide reactivity, short - lived excimers of noble gas halides such as XeCl are prepared in situ, and are used in the function of excimer lasers. Recently, xenon has been shown to produce a wide variety of compounds of the type XeO X where n is 1, 2 or 3 and X is any electronegative group, such as CF, C ( SO CF ), N ( SO F ), N ( SO CF ), OTeF, O ( IO F ), etc. ; the range of compounds is impressive, similar to that seen with the neighbouring element iodine, running into the thousands and involving bonds between xenon and oxygen, nitrogen, carbon, boron and even gold, as well as perxenic acid, several halides, and complex ions. The compound Xe Sb F contains a Xe -- Xe bond, which is the longest element - element bond known ( 308.71 pm = 3.0871 Å ). Short - lived excimers of Xe are reported to exist as a part of the function of excimer lasers. Krypton compounds Krypton gas reacts with fluorine gas under extreme forcing conditions, forming KrF according to the following equation : Kr + F → KrF KrF reacts with strong Lewis acids to form salts of the KrF and Kr cations. The preparation of KrF reported by Grosse in 1963, using the Claasen method, was subsequently shown to be a mistaken identification. Krypton compounds with other than Kr - F bonds ( compounds with atoms other than fluorine ) have also been described. KrF reacts with B ( OTeF ) to produces the unstable compound, Kr ( OTeF ), with a krypton - oxygen bond. A krypton - nitrogen bond is found in the cation ( HC ≡ N -- Kr -- F ), produced by the reaction of KrF with ( HC ≡ NH ) ( AsF ) below − 50 ° C. Argon compounds Main article : Argon compounds This section needs expansion. You can help by adding to it. ( January 2015 ) The discovery of HArF was announced in 2000. The compound can exist in low temperature argon matrices for experimental studies, and it has also been studied computationally. Argon hydride ion ArH was obtained in the 1970s. This molecular ion has also been identified in the Crab nebula, based on the frequency of its light emissions. Neon and helium compounds Main articles : Helium compounds and Neon compounds A neon compound has yet to be described. There is some empirical and theoretical evidence for a few metastable helium compounds which may exist at very low temperatures or extreme pressures. The stable cation HeH was reported in 1925. Reports prior to xenon hexafluoroplatinate and xenon tetrafluoride Clathrates Kr ( H ) and H solids formed in a diamond anvil cell. Ruby was added for pressure measurement. Structure of Kr ( H ). Krypton octahedra ( green ) are surrounded by randomly oriented hydrogen molecules. Prior to 1962, the only isolated compounds of noble gases were clathrates ( including clathrate hydrates ) ; other compounds such as coordination compounds were observed only by spectroscopic means. Clathrates ( also known as cage compounds ) are compounds of noble gases in which they are trapped within cavities of crystal lattices of certain organic and inorganic substances. The essential condition for their formation is that the guest ( noble gas ) atoms should be of appropriate size to fit in the cavities of the host crystal lattice ; for instance, Ar, Kr, and Xe can form clathrates with crystalline β - quinol, but He and Ne can not fit because they are too small. As well, Kr and Xe can appear as guests in crystals of melanophlogite. Helium - nitrogen ( He ( N ) ) crystals have been grown at room temperature at pressures ca. 10 GPa in a diamond anvil cell. Solid argon - hydrogen clathrate ( Ar ( H ) ) has the same crystal structure as the MgZn Laves phase. It forms at pressures between 4.3 and 220 GPa, though Raman measurements suggest that the H molecules in Ar ( H ) dissociate above 175 GPa. A similar Kr ( H ) solid forms at pressures above 5 GPa. It has a face - centered cubic structure where krypton octahedra are surrounded by randomly oriented hydrogen molecules. Meanwhile, in solid Xe ( H ) xenon atoms form dimers inside solid hydrogen. Coordination compounds Coordination compounds such as Ar BF have been postulated to exist at low temperatures, but have never been confirmed. Also, compounds such as WHe and HgHe were reported to have been formed by electron bombardment, but recent research has shown that these are probably the result of He being adsorbed on the surface of the metal ; therefore, these compounds can not truly be considered chemical compounds. Hydrates Hydrates are formed by compressing noble gases in water, where it is believed that the water molecule, a strong dipole, induces a weak dipole in the noble gas atoms, resulting in dipole - dipole interaction. Heavier atoms are more influenced than smaller ones, hence Xe 5.75 H O was reported to have been the most stable hydrate ; it has a melting point of 24 ° C. The deuterated version of this hydrate has also been produced. Fullerene adducts Main article : Non-metal doped fullerenes Structure of a noble - gas atom caged within a buckminsterfullerene ( C60 ) molecule. Noble gases can also form endohedral fullerene compounds where the noble gas atom is trapped inside a fullerene molecule. In 1993, it was discovered that when C is exposed to a pressure of around 3 bar of He or Ne, the complexes He@C and Ne@C are formed. Under these conditions, only about one out of every 650,000 C cages was doped with a helium atom ; with higher pressures ( 3000 bar ), it is possible to achieve a yield of up to 0.1 %. Endohedral complexes with argon, krypton and xenon have also been obtained, as well as numerous adducts of He@C. Applications This section has multiple issues. Please help improve it or discuss these issues on the talk page. ( Learn how and when to remove these template messages ) This section needs additional citations for verification. Please help improve this article by adding citations to reliable sources. Unsourced material may be challenged and removed. ( January 2015 ) This section needs expansion. You can help by adding to it. ( January 2015 ) Most applications of noble gas compounds are either as oxidising agents or as a means to store noble gases in a dense form. Xenic acid is a valuable oxidising agent because it has no potential for introducing impurities -- xenon is simply liberated as a gas -- and so is rivalled only by ozone in this regard. The perxenates are even more powerful oxidizing agents. Xenon - based oxidants have also been used for synthesizing carbocations stable at room temperature, in SO ClF solution. Stable salts of xenon containing very high proportions of fluorine by weight ( such as tetrafluoroammonium heptafluoroxenate, NF XeF, and the related tetrafluoroammonium octafluoroxenate ( NF ) XeF ), have been developed as highly energetic oxidisers for use as propellants in rocketry. The xenon fluorides are good fluorinating agents. Clathrates have been used for separation of He and Ne from Ar, Kr, and Xe, and also for the transportation of Ar, Kr, and Xe. ( For instance, radioactive isotopes of krypton and xenon are difficult to store and dispose, and compounds of these elements may be more easily handled than the gaseous forms. ) In addition, clathrates of radioisotopes may provide suitable formulations for experiments requiring sources of particular types of radiation ; hence. Kr clathrate provides a safe source of beta particles, while Xe clathrate provides a useful source of gamma rays. References This section may require cleanup to meet Wikipedia 's quality standards. The specific problem is : overload of primary sources ( 15 of 22 sources, with OR / interpretation required in reporting ), and absolute absence of sources for vast numbers of clear factual statements Please help improve this section if you can. ( January 2015 ) Jump up ^ Smith GL, Mercier HP, Schrobilgen GJ ( February 2007 ). `` Synthesis of ( F S ≡ NXeF ) ( AsF ) and structural study by multi-NMR and Raman spectroscopy, electronic structure calculations, and X-ray crystallography ''. Inorganic Chemistry. 46 ( 4 ) : 1369 -- 78. doi : 10.1021 / ic061899+. PMID 17256847. Jump up ^ Smith GL, Mercier HP, Schrobilgen GJ ( May 2008 ). `` F SN ( H ) Xe ; a rare example of xenon bonded to sp - hybridized nitrogen ; synthesis and structural characterization of ( F SN ( H ) Xe ) ( AsF ) ''. Inorganic Chemistry. 47 ( 10 ) : 4173 -- 84. doi : 10.1021 / ic702039f. PMID 18407626. Jump up ^ Pauling, Linus ( June 1933 ). `` The Formulas of Antimonic Acid and the Antimonates ''. J. Am. Chem. Soc. 55 ( 5 ) : 1895 -- 1900. doi : 10.1021 / ja01332a016. ^ Jump up to : Holloway, John H. ( 1968 ). Noble - Gas Chemistry. London : Methuen. ISBN 0 - 416 - 03270 - 2. Jump up ^ Seppelt, Konrad ( June 1979 ). `` Recent developments in the Chemistry of Some Electronegative Elements ''. Accounts of Chemical Research. 12 ( 6 ) : 211 -- 216. doi : 10.1021 / ar50138a004. Jump up ^ Miessler, Gary L. ; Tarr, Donald A. ( 1999 ). Inorganic Chemistry ( 2nd ed. ). Prentice Hall. p. 272. ISBN 0 - 13 - 841891 - 8. Jump up ^ Bartlett, N. ( 1962 ). `` Xenon hexafluoroplatinate Xe ( PtF ) ''. Proceedings of the Chemical Society of London ( 6 ) : 218. doi : 10.1039 / PS9620000197. Jump up ^ Graham, L. ; Graudejus, O. ; Jha N.K. ; Bartlett, N. ( 2000 ). `` Concerning the nature of XePtF ''. Coordination Chemistry Reviews. 197 : 321 -- 334. doi : 10.1016 / S0010 - 8545 ( 99 ) 00190 - 3. Jump up ^ Claassen, H.H. ; Selig, H. ; Malm, J.G. ( 1962 ). `` Xenon Tetrafluoride ''. J. Am. Chem. Soc. 84 ( 18 ) : 3593. doi : 10.1021 / ja00877a042. Jump up ^ Hoppe, R. ; Daehne, W. ; Mattauch, H. ; Roedder, K. ( 1962 - 11 - 01 ). `` FLUORINATION OF XENON ''. Angew. Chem. Int. Ed. Engl. 1 ( 11 ) : 599. doi : 10.1002 / anie. 196205992. ^ Jump up to : Lehmann, J ( 2002 ). `` The chemistry of krypton ''. Coordination Chemistry Reviews. 233 -- 234 : 1 -- 39. doi : 10.1016 / S0010 - 8545 ( 02 ) 00202 - 3. Jump up ^ Kenneth S. Pitzer ( 1975 ). `` Fluorides of radon and element 118 ''. J. Chem. Soc., Chem. Commun. ( 18 ) : 760b -- 761. doi : 10.1039 / C3975000760b. Jump up ^ Drews, Thomas ; Seppelt, Konrad ( 1997 ). `` The Xe Ion -- Preparation and Structure ''. Angewandte Chemie International Edition. 36 : 273 -- 274. doi : 10.1002 / anie. 199702731. Jump up ^ Prusakov, V.N. ; Sokolov, V.B. ( 1971 ). `` Krypton difluoride ''. Soviet Atomic Energy. 31 ( 3 ) : 990 -- 999. doi : 10.1007 / BF01375764. Jump up ^ John H. Holloway ; Eric G. Hope ( 1998 ). A.G. Sykes, ed. Advances in Inorganic Chemistry. Academic Press. p. 57. ISBN 0 - 12 - 023646 - X. Jump up ^ Khriachtchev, L., Pettersson, M., Runeberg, N., Lundell, J., Räsänen, M. ( 2000 ). `` A stable argon compound ''. Nature. 406 ( 6798 ) : 874 -- 876. doi : 10.1038 / 35022551. PMID 10972285. CS1 maint : Multiple names : authors list ( link ) ^ Jump up to : Bochenkova, Anastasia V. ; Bochenkov, Vladimir E. ; Khriachtchev, Leonid ( 2 July 2009 ). `` HArF in Solid Argon Revisited : Transition from Unstable to Stable Configuration ''. The Journal of Physical Chemistry A. 113 ( 26 ) : 7654 -- 7659. Bibcode : 2009JPCA... 113.7654 B. doi : 10.1021 / jp810457h. Jump up ^ Wyatt, J.R. ; Strattan, L.W. ; Snyder, S.C. ; Hierl, P.M. ( 1975 ). `` Chemical accelerator studies of reaction dynamics : Ar + CH → ArH + CH ``. The Journal of Chemical Physics. 62 ( 7 ) : 2555. Bibcode : 1975JChPh... 62.2555 W. doi : 10.1063 / 1.430836. Jump up ^ Barlow, M.J. ; Swinyard, B.M. ; Owen, P.J. ; Cernicharo, J. ; Gomez, H.L. ; Ivison, R.J. ; Krause, O. ; Lim, T.L. ; Matsuura, M. ; Miller, S. ; Olofsson, G. ; Polehampton, E.T. ( 12 December 2013 ). `` Detection of a Noble Gas Molecular Ion, ArH, in the Crab Nebula ``. Science. 342 ( 6164 ) : 1343 -- 1345. arXiv : 1312.4843. Bibcode : 2013Sci... 342.1343 B. doi : 10.1126 / science. 1243582. PMID 24337290. Jump up ^ Hogness, T.R. ; Lunn, E.G. ( 1925 ). `` The Ionization of Hydrogen by Electron Impact as Interpreted by Positive Ray Analysis ''. Phys. Rev. Lett. The American Physical Society. 26 ( 1 ) : 44 -- 55. Bibcode : 1925PhRv... 26... 44H. doi : 10.1103 / PhysRev. 26.44. Retrieved 15 December 2013. ^ Jump up to : Kleppe, Annette K. ; Amboage, Mónica ; Jephcoat, Andrew P. ( 2014 ). `` New high - pressure van der Waals compound Kr ( H ) discovered in the krypton - hydrogen binary system ''. Scientific Reports. 4. Bibcode : 2014NatSR... 4E4989K. doi : 10.1038 / srep04989. Jump up ^ Vos, W.L. ; Finger, L.W. ; Hemley, R.J. ; Hu, J.Z. ; Mao, H.K. ; Schouten, J.A. ( 1992 ). `` A high - pressure van der Waals compound in solid nitrogen - helium mixtures ''. Nature. 358 ( 6381 ) : 46 -- 48. Bibcode : 1992Natur. 358... 46V. doi : 10.1038 / 358046a0. Jump up ^ Pauling, L. ( 1961 ). `` A molecular theory of general anesthesia ''. Science. 134 ( 3471 ) : 15 -- 21. Bibcode : 1961Sci... 134... 15P. doi : 10.1126 / science. 134.3471. 15. PMID 13733483. Reprinted as Pauling, Linus ; Kamb, Barclay, eds. ( 2001 ). Linus Pauling : Selected Scientific Papers. 2. River Edge, New Jersey : World Scientific. pp. 1328 -- 1334. ISBN 981 - 02 - 2940 - 2. Jump up ^ Henderson, W. ( 2000 ). Main group chemistry. Great Britain : Royal Society of Chemistry. p. 148. ISBN 0 - 85404 - 617 - 8. Jump up ^ Ikeda, Tomoko ; Mae, Shinji ; Yamamuro, Osamu ; Matsuo, Takasuke ; Ikeda, Susumu ; Ibberson, Richard M. ( November 23, 2000 ). `` Distortion of Host Lattice in Clathrate Hydrate as a Function of Guest Molecule and Temperature ''. Journal of Physical Chemistry A. 104 ( 46 ) : 10623 -- 10630. Bibcode : 2000JPCA... 10410623I. doi : 10.1021 / jp001313j. Jump up ^ Saunders, M. ; Jiménez - Vázquez, H.A. ; Cross, R.J. & Poreda, R.J. ( 1993 ). `` Stable compounds of helium and neon. He@C60 and Ne@C60 ''. Science. 259 ( 5100 ) : 1428 -- 1430. Bibcode : 1993Sci... 259.1428 S. doi : 10.1126 / science. 259.5100. 1428. PMID 17801275. Jump up ^ Saunders, Martin ; Jimenez - Vazquez, Hugo A. ; Cross, R. James ; Mroczkowski, Stanley ; Gross, Michael L. ; Giblin, Daryl E. & Poreda, Robert J. ( 1994 ). `` Incorporation of helium, neon, argon, krypton, and xenon into fullerenes using high pressure ''. J. Am. Chem. Soc. 116 ( 5 ) : 2193 -- 2194. doi : 10.1021 / ja00084a089. Jump up ^ Mercier, H.P.A. ; Moran, M.D. ; Schrobilgen, G.J. ; Steinberg, C. ; Suontamo, R.J. ( 2004 ). `` The Syntheses of Carbocations by Use of the Noble - Gas Oxidant, ( XeOTeF ) ( Sb ( OTeF ) ) : The Syntheses and Characterization of the CX ( X = Cl, Br, OTeF ) and CBr ( OTeF ) Cations and Theoretical Studies of CX and BX ( X = F, Cl, Br, I, OTeF ) ``. J. Am. Chem. Soc. 126 ( 17 ) : 5533 -- 5548. doi : 10.1021 / ja030649e. PMID 15113225. Jump up ^ Christe, KO ; Wilson, WW ( Dec 1982 ). `` Perfluoroammonium and alkali - metal salts of the heptafluoroxenate ( VI ) and octafluoroxenate ( VI ) anions ''. Inorganic Chemistry. 21 ( 12 ) : 4113 -- 4117. doi : 10.1021 / ic00142a001. Jump up ^ Karl O. Christe, William W. Wilson. Perfluoroammonium salt of heptafluoroxenon anion. U.S. Patent 4,428,913, June 24, 1982 Resources Khriachtchev, Leonid ; Räsänen, Markku ; Gerber, R. Benny ( 2009 ). `` Noble - Gas Hydrides : New Chemistry at Low Temperatures ''. Accounts of Chemical Research. 42 ( 1 ) : 183 -- 91. doi : 10.1021 / ar800110q. PMID 18720951. Noble gas compounds Helium compounds helium compounds HeH LiHe Na He He He Neon compounds neon compounds Argon compounds argon compounds ArH HArF MgAr ArCF Krypton compounds KrF HKrCN HKrC H Kr ( OTeF ) HCNKrF Xenon compounds Xe ( 0 ) AuXe ( Sb F ) Xe ( I ) XePtF XeRhF Xe ( II ) XeF XeFPtF XeFPt F Xe F PtF XeCl Organoxenon ( II ) compounds Xe ( IV ) XeO XeF XeOF N ( CH ) XeF Organoxenon ( IV ) compounds Xe ( VI ) XeO XeF XeOF H XeO ( NO ) XeF Xe ( VIII ) XeO H XeO Radon compounds Rn ( II ) RnF RnFSb F Rn ( VI ) RnO Retrieved from `` https://en.wikipedia.org/w/index.php?title=Noble_gas_compound&oldid=833942170 '' Categories : Noble gas compounds Hidden categories : CS1 maint : Multiple names : authors list Articles needing additional references from January 2015 All articles needing additional references Articles lacking reliable references from January 2015 All articles lacking reliable references Articles with multiple maintenance issues All articles with unsourced statements Articles with unsourced statements from January 2015 All articles with vague or ambiguous time Vague or ambiguous time from January 2015 Articles to be expanded from January 2015 All articles to be expanded All pages needing factual verification Wikipedia articles needing factual verification from January 2015 All articles with specifically marked weasel - worded phrases Articles with specifically marked weasel - worded phrases from January 2015 Articles needing cleanup from January 2015 All pages needing cleanup Cleanup tagged articles with a reason field from January 2015 Wikipedia pages needing cleanup from January 2015 Talk Contents About Wikipedia Български Català Deutsch Español Esperanto Euskara Français 한국어 Italiano Bahasa Melayu Nederlands 日本 語 ਪੰਜਾਬੀ Русский Simple English Suomi Svenska ไทย Türkçe 中文 12 more Edit links This page was last edited on 3 April 2018, at 03 : 37. 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Question: name an element of group 18 which can form compounds
Answer: xenon