Silver(II) fluoride is a chemical compound with the formula AgF2. It is a rare example of a silver(II) compound - silver usually exists in its +1 oxidation state. It is used as a fluorinating agent.
Composition and structure
AgF2 is a white crystalline powder, but it is usually black/brown due to impurities. The F/Ag ratio for most samples is < 2, typically approaching 1.75 due to contamination with Ag and oxides and carbon.[1]
For some time, it was doubted that silver was actually in the +2 oxidation state, rather than some combination of states such as AgI[AgIIIF4], which would be similar to silver(I,III) oxide. Neutron diffraction studies, however, confirmed its description as silver(II). The AgI[AgIIIF4] was found to be present at high temperatures, but it was unstable with respect to AgF2.[2]
AgF2 can be synthesized by fluorinating Ag2O with elemental fluorine. Also, at 200°C (473 K) elemental fluorine will react with AgF or AgCl to produce AgF2.[4][5]
Uses
AgF2 is a strong fluorinating and oxidising agent. It is formed as an intermediate in the catalysis of gaseous reactions with fluorine by silver. With fluoride ions, it forms complex ions such as AgF− 3, the blue-violet AgF2− 4, and AgF4− 6.[6]
It is used in the fluorination and preparation of organic perfluorocompounds.[7] This type of reaction can occur in three different ways (here Z refers to any element or group attached to carbon, X is a halogen):
CZ3H + 2 AgF2 → CZ3F + HF + 2 AgF
CZ3X + 2AgF2 → CZ3F + X2 + 2 AgF
Z2C=CZ2 + 2 AgF2 → Z2CFCFZ2 + 2 AgF
Similar transformations can also be effected using other high valence metallic fluorides such as CoF3, MnF3, CeF4, and PbF4.
AgF 2 is also used in the fluorination of aromatic compounds, although selective monofluorinations are more difficult:[8]
AgF 2 can be used to selectively fluorinate pyridine at the ortho position under mild conditions.[10]
Safety
AgF 2 is a very strong oxidizer that reacts violently with water,[11] reacts with dilute acids to produce ozone, oxidizes iodide to iodine,[11][12] and upon contact with acetylene forms the contact explosive silver acetylide.[13] It is light-sensitive,[11] very hygroscopic and corrosive. It decomposes violently on contact with hydrogen peroxide, releasing oxygen gas.[13] It also liberates HF, F 2, and elemental silver.[12]
↑Encyclopedia of Chemical Technology. Kirk-Othermer. Vol.11, 4th Ed. (1991)
↑Egon Wiberg; Nils Wiberg; Arnold Frederick Holleman (2001). Inorganic chemistry. Academic Press. pp.1272–1273. ISBN0-12-352651-5.
↑Rausch, D.; Davis, r.; Osborne, D. W. (1963). "The Addition of Fluorine to Halogenated Olefins by Means of Metal Fluorides". J. Org. Chem.28 (2): 494–497. doi:10.1021/jo01037a055.
↑Zweig, A.; Fischer, R. G.; Lancaster, J. (1980). "New Methods for Selective Monofluorination of Aromatics Using Silver Difluoride". J. Org. Chem.45 (18): 3597. doi:10.1021/jo01306a011.
↑Levec, J.; Slivnik, J.; Zemva, B. (1974). "On the Reaction Between Xenon and Fluorine". Journal of Inorganic and Nuclear Chemistry. 36 (5): 997. doi:10.1016/0022-1902(74)80203-4.
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