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Xenon difluoride is a powerful fluorinating agent with the chemical formula XeF 2, and one of the most stable xenon compounds. Like most covalent inorganic fluorides it is moisture-sensitive. It decomposes on contact with water vapor, but is otherwise stable in storage. Xenon difluoride is a dense, colourless crystalline solid.
Xenon compounds are compounds containing the element xenon (Xe). After Neil Bartlett's discovery in 1962 that xenon can form chemical compounds, a large number of xenon compounds have been discovered and described. Almost all known xenon compounds contain the electronegative atoms fluorine or oxygen.
Xenon tetrafluoride crystals. The binary compounds xenon include xenon difluoride, xenon tetrafluoride, and xenon hexafluoride. [102] Xenon forms several oxyfluorides, such as xenon oxydifluoride, XeOF 2, by hydrolysis of xenon tetrafluoride. [103] Its lighter neighbor, krypton also forms well-characterized compounds, e.g., krypton difluoride.
Xenon difluoride, XeF 2; Xenon tetrafluoride, XeF 4; Xenon hexafluoride, XeF 6 This page was last edited on 28 November 2023, at 08:20 (UTC). Text is available under ...
Xenon oxydifluoride is an inorganic compound with the molecular formula XeOF 2. The first definitive isolation of the compound was published on 3 March 2007, producing it by the previously-examined route of partial hydrolysis of xenon tetrafluoride. [1] XeF 4 + H 2 O → XeOF 2 + 2 HF. The compound has a T-shaped geometry. [1]
Most of the organoxenon compounds are more unstable than xenon fluorides due to the high polarity. The molecular dipoles of xenon difluoride and xenon tetrafluoride are both 0 D. The early synthesized ones only contain perfluoro groups, but later some other groups were found, e.g. 2,4,6-trifluorophenyl. [2]
Xenon difluoride is used as an etchant for silicon, particularly in the production of microelectromechanical systems (MEMS). [194] The anticancer drug 5-fluorouracil can be produced by reacting xenon difluoride with uracil. [195] Xenon is also used in protein crystallography.
Theoretical studies on this molecule predict that it should have a Rn–F bond distance of 2.08 ångström (Å), and that the compound is thermodynamically more stable and less volatile than its lighter counterpart xenon difluoride (XeF 2). [8] The octahedral molecule RnF 6 was predicted to have an even lower enthalpy of formation than the ...