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Organoxenon compounds in organic chemistry contain carbon to xenon chemical bonds. The first organoxenon compounds were divalent, such as (C₆F₅)₂Xe. The first tetravalent organoxenon compound, [C₆F₅XeF₂][BF₄], was synthesized in 2004. So far, more than one hundred organoxenon compounds have been researched.

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.

Xe(II)

The most common bivalent organoxenon compound is C₆F₅XeF, which is always used as a precursor to other organoxenon compounds. Due to the unstability of xenon fluoride, it is impossible to synthesize organoxenon compound by using general organic reagents. Most frequently used fluorinating agents include Cd(Ar_F)₂(subscript "F" means fluorine-including aryl), C₆F₅SiF₃, and C₆F₅SiMe₃ (should be used along with fluoride).

With the use of stronger Lewis acids, such as C₆F₅BF₂, ionic compounds like [RXe][Ar_FBF₃] can be produced. Alkenyl and alkyl organoxenon compounds are prepared in this way as well, for example, C₆F₅XeCF=CF₂ and C₆F₅XeCF₃.

Some typical reactions are listed below:

$\mathrm{2}{\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}\mathrm{X}\mathrm{e}\mathrm{F}+\mathrm{C}\mathrm{d}\mathrm{(}{\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}{\mathrm{)}}_{\mathrm{2}}\mathrm{\to }\mathrm{X}\mathrm{e}\mathrm{(}{\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}{\mathrm{)}}_{\mathrm{2}}+\mathrm{C}\mathrm{d}{\mathrm{F}}_{\mathrm{2}}\mathrm{\downarrow }$

${\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}\mathrm{X}\mathrm{e}\mathrm{F}+\mathrm{M}{\mathrm{e}}_{\mathrm{3}}\mathrm{S}\mathrm{i}\mathrm{C}\mathrm{N}\mathrm{\to }{\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}\mathrm{X}\mathrm{e}\mathrm{C}\mathrm{N}+\mathrm{M}{\mathrm{e}}_{\mathrm{3}}\mathrm{S}\mathrm{i}\mathrm{F}$

${\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}\mathrm{X}\mathrm{e}\mathrm{F}+\mathrm{C}\mathrm{d}\mathrm{(}\mathrm{2},\mathrm{4},\mathrm{6}\mathrm{-}{\mathrm{C}}_{\mathrm{6}}{\mathrm{H}}_{\mathrm{2}}{\mathrm{F}}_{\mathrm{3}}{\mathrm{)}}_{\mathrm{2}}\mathrm{\to }\mathrm{2},\mathrm{4},\mathrm{6}\mathrm{-}{\mathrm{C}}_{\mathrm{6}}{\mathrm{H}}_{\mathrm{2}}{\mathrm{F}}_{\mathrm{3}}\mathrm{X}\mathrm{e}{\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}+\mathrm{C}\mathrm{d}{\mathrm{F}}_{\mathrm{2}}\mathrm{\downarrow }$

The third reaction also produces (C₆F₅)₂Xe, Xe(2,4,6-C₆H₂F₃)₂ and so on.

The precursor C₆F₅XeF can be prepared by the reaction of trimethyl(pentaflurophenyl)silane(C₆F₅SiMe₃) and xenon difluoride. Adding fluoride to the adduct of C₆F₅XeF and arsenic pentafluoride is another method.

Xe(IV)

In 2000, Karel Lutar and Boris Žemva et al. produced an ionic compound. They treated xenon tetrafluoride and difluoro(pentaflurophenyl)borane in dichloromethane at -55°C:

$\mathrm{X}\mathrm{e}{\mathrm{F}}_{\mathrm{4}}+{\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}\mathrm{B}{\mathrm{F}}_{\mathrm{2}}\underset{-55^{o}C}{\overset{C{H}_{2}C{l}_2}{\to }}\mathrm{[}{\mathrm{C}}_{\mathrm{6}}{\mathrm{F}}_{\mathrm{5}}\mathrm{X}\mathrm{e}{\mathrm{F}}_{\mathrm{2}}{\mathrm{]}}^{+}\mathrm{B}{F}_{\mathrm{4}}^{\mathrm{-}}$

The compound is an extremely strong fluorinating agent, and it is capable of converting (C₆F₅)₃P to (C₆F₅)₃PF₂, C₆F₅I to C₆F₅IF₂, even iodine to iodine pentafluoride.

See also

• Compounds of carbon with other elements in the periodic table:

References

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