Fluorination of Xenon

Hoppe, R.; Dähne, Wolfgang; Mattauch, H.; Rödder, Karl‐Martin

doi:10.1002/anie.196205992

Cited by 90 publications

(63 citation statements)

References 1 publication

Supporting

Mentioning

Contrasting

Order By: Relevance

“…They are critical elements [9] because their abundances constrain the models for giant planet formation and the origin of their atmospheres. Among noble gases, Xe has the largest atomic core and is polarizable to form Xe fluorides [10] (or Xe noble metal hexafluorides [11]) and Xe oxides [12] in certain circumstances at ambient conditions due to its low ionization energy and large relativistic effect. [13] However, other Xe compounds are only synthesizable by using Xe fluoride precursors, instead of Xe gas, in the reaction with other organics or inorganics.…”

mentioning

confidence: 99%

Stable xenon nitride at high pressures

Peng

Wang

et al. 2015

Phys. Rev. B

View full text Add to dashboard Cite

Nitrides in many ways are fascinating since they often appear as superconductors, high energy density and hard materials. Though there exist a large variety of nitrides, noble gas nitrides are long missing in nature. Pursuit of noble gas nitrides has therefore become the subject of topical interests, but remains as a great challenge since molecular nitrogen (N 2 , a major form of nitrogen) and noble gases are both inert systems and do not interact at normal conditions. We show through a swarm structure searching simulation that high pressure can lift the reactivity of both N 2 and xenon (Xe), making chemical reaction of them possible. The resultant nitride has a peculiar stoichiometry of XeN 6 , possessing a high-energy-density of approximately 2.4 kJg -1 , rivaling that of the modern explosives. Chemically, XeN 6 is more intriguing with the appearance of chaired N 6 hexagons and an emergent 12-fold Xe by acceptance of unprecedentedly 12 Xe-N weak covalent bonds. Our work opens up the possibility of achieving Xe nitrides whose formation is long sought as impossible.PACS numbers: 61.66.fn, 71.15.Mb, 81.40.Vw Nitrogen (N) is the most abundant element in the Earth's atmosphere and is one of most important constituents of our universe. In air, N exists in the form of diatomic N 2 molecules and has the strongest-known triple N≡N bond. As a result, N 2 is chemically inert[1] and hardly interacts with other elements or substances under normal conditions. Syntheses of useful nitrides for industrial applications rely on chemical methods [2] via, e.g., temperature-programmed reaction, thermal decomposition, electrochemical synthesis, or with the aid of catalysts (e.g., the synthesis of NH 3 ). [3] Nitrides have a variety of intriguing properties, such as superconductivity[4], high energy density [5], and high hardness [6], as well as extraordinary chemical and thermal stability [7].Noble gases (e.g., Ar, Kr, and Xe) as typical closed-shell systems are inert prototype examples and where the famous octet rule[8] originated. They are critical elements[9] because their abundances constrain the models for giant planet formation and the origin of their atmospheres. Among noble gases, Xe has the largest atomic core and is polarizable to form Xe fluorides[10] (or Xe noble metal hexafluorides [11]) and Xe oxides [12] in certain circumstances at ambient conditions due to its low ionization energy and large relativistic effect.[13] However, other Xe compounds are only synthesizable by using Xe fluoride precursors, instead of Xe gas, in the reaction with other organics or inorganics.Since both N 2 and Xe are inert, they do not directly interact at ambient conditions. Although Xe and N containing compounds have been seen at ambient pressure in (FXe)[N(SO 2 F) 2 ] salts [14], the syntheses of these salts relied on the precursors of the cationic (FXe) + and anionic Ncontaining ligands, while not the uses of N 2 and Xe gases [13]. All of these as-synthesized complex salts have poor thermal stability, and most of them decompose explosi...

show abstract

mentioning

confidence: 99%

Stable xenon nitride at high pressures

Peng

Wang

et al. 2015

Phys. Rev. B

View full text Add to dashboard Cite

show abstract

“…Among the salts that have been prepared in this manner or by alternative procedures are Na 4 (9). The salts are kinetically very stable, losing water gradually when heated; eg, Na 4 XeO 6 Á6H 2 O becomes anhydrous at 100 C and decomposes at 360 C. Several transition metal and actinide perxenates have been prepared but have not been thoroughly characterized and include those of copper, lead, silver, zinc, thorium, and uranium.…”

Section: Xenates and Perxenates Alkali Metal Xenates Of Compositionmentioning

confidence: 99%

Noble‐Gas Compounds

Schrobilgen

Brock

Mercier

2012

Kirk-Othmer Encyclopedia of Chemical Technology

View full text Add to dashboard Cite

Noble‐gas reactivity was discovered on March 23, 1962 when Neil Bartlett (1932–2008) showed that xenon gas was oxidized by PtF 6 . The product obtained by Bartlett was initially formulated as XePtF 6 . Pursuant to his discovery, numerous xenon and krypton compounds were synthesized in macroscopic quantities. Among the noble‐gas elements, xenon has the most extensive chemistry, and it can possess formal oxidation states of 0, +2, +4, +6, and +8 in its compounds by forming fluorides, oxides, and oxide fluorides, as well as derivatives in which xenon is bonded to polyatomic groups through oxygen, nitrogen, and carbon. In addition, compounds containing Xe–Au, Xe–Xe, Xe–Cl, and Hg–Xe bonds are known. Other xenon‐element bonds are known in the gas phase or in low‐temperature matrices, which are exemplified by Xe–H, Xe–Si, Xe–S, Xe–X (X=Cl, Br, I), and Xe–U bonds. Krypton chemistry is more limited. Only compounds with krypton in the +2 oxidation state are known, namely, KrF 2 , salts of the KrF + and Kr 2 F 3 + cations, by analogy with xenon, the Kr–O bonded compound, Kr(OTeF 5 ) 2 , and several species containing Kr–N bonds. Several gas‐phase and matrix‐isolated species in which krypton is bonded to carbon, hydrogen, and halides other than fluorine are also known. Radon is believed to form RnF 2 and RnF + by analogy with krypton and xenon. The only argon species that are known are the ArF + cation, which has been observed in the gas phase, and HArF, which has been stabilized in a low‐temperature argon matrix. To date, no argon, neon, or helium compounds have been isolated in macroscopic amounts. Noble‐gas compounds have been used as oxidizers and as oxidative fluorinating agents in chemical syntheses.

show abstract

“…The story of the decade-long failures and the circumstances which eventually led to the first syntheses of noble gas compounds by Bartlett [1] and Hoppe [2] is a fascinating example of the endurance and the creativity of great chemists who were determined to overcome the obstacles posed by nature. [3] A large number of noble gas compounds have since been isolated in the condensed phase; however, until recently only molecules of xenon and krypton were chemically synthesized, because chemical inertness increases with decreasing atomic number of the noble gas (Ng) atom.…”

mentioning

confidence: 99%