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Krypton difluoride, KrF 2 is a chemical compound of krypton and fluorine. It was the first compound of krypton discovered. [2] It is a volatile, colourless solid at room temperature. The structure of the KrF 2 molecule is linear, with Kr−F distances of 188.9 pm. It reacts with strong Lewis acids to form salts of the KrF + and Kr 2 F + 3 ...
Its lighter neighbor, krypton also forms well-characterized compounds, e.g., krypton difluoride. Krypton tetrafluoride was reported in 1963, [104] but was subsequently shown to be a mistaken identification; the compound seems to be very hard to synthesize now (although even the hexafluoride may exist). [105]
Krypton compounds with other than Kr–F bonds (compounds with atoms other than fluorine) have also been described. KrF 2 reacts with B(OTeF 5) 3 to produce the unstable compound, Kr(OTeF 5) 2, with a krypton-oxygen bond.
Although most compounds are referred to by their IUPAC systematic names (following IUPAC nomenclature), ... Krypton difluoride – KrF 2; L. La
Until the 1960s no noble gas compounds had been synthesized. [27] Following the first successful synthesis of xenon compounds in 1962, synthesis of krypton difluoride (KrF 2) was reported in 1963. In the same year, KrF 4 was reported by Grosse, et al., [28] but was subsequently shown to be a mistaken identification. [29]
Among other noble gases, krypton forms a difluoride, [150] and radon and fluorine generate a solid suspected to be radon difluoride. [ 151 ] [ 152 ] Binary fluorides of lighter noble gases are exceptionally unstable: argon and hydrogen fluoride combine under extreme conditions to give argon fluorohydride . [ 41 ]
In addition to compounds where xenon forms a chemical bond, xenon can form clathrates—substances where xenon atoms or pairs are trapped by the crystalline lattice of another compound. One example is xenon hydrate (Xe· 5 + 3 ⁄ 4 H 2 O), where xenon atoms occupy vacancies in a lattice of water molecules. [32]
Molecules of theoretical curiosity such as neon difluoride (NeF 2) and beryllium dilithide (BeLi 2) represent examples of inverted electronegativity. [13] As a result of unusual bonding situation, the donor lone pair ends up with significant electron density on the central atom, while the acceptor is the "out-of-phase" combination of the p ...