Silver tetrafluoroborate

Silver tetrafluoroborate
Names
IUPAC name
Silver tetrafluoridoborate(1–)
Other names
Borate(1-), tetrafluoro-, silver(1+)
Identifiers
14104-20-2 YesY
3D model (Jmol) Interactive image
ChemSpider 140438 YesY
ECHA InfoCard 100.034.491
EC Number 237-956-5
PubChem 159722
RTECS number ED2875000
Properties
AgBF4
Molar mass 194.673 g/mol
Appearance Off-white powder
Odor almost odorless
Density 0.936 g/cm3
Melting point 71.5 °C (160.7 °F; 344.6 K)
soluble
Hazards
Safety data sheet External MSDS
Corrosive (C)
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g., liquid nitrogen Special hazards (white): no codeNFPA 704 four-colored diamond
0
3
0
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Infobox references

Silver tetrafluoroborate is an inorganic compound with the chemical formula AgBF4. It is a white solid that dissolves in polar organic solvents as well as water. In its solid state, the Ag+ centers are bound to fluoride.[1]

Preparation

Silver tetrafluoroborate is prepared by the reaction between boron trifluoride and silver oxide in the presence of benzene.

Laboratory uses

In the inorganic and organometallic chemistry laboratory, silver tetrafluoroborate, sometimes referred to "silver BF-4", is a useful reagent. In dichloromethane, silver tetrafluoroborate is a moderately strong oxidant.[2] Similar to silver hexafluorophosphate, it is commonly used to replace halide anions or ligands with the weakly coordinating tetrafluoroborate anions. The abstraction of the halide is driven by the precipitation of the appropriate silver halide.

References

  1. ↑ Evgeny Goreshnik, Zoran Mazej, "X-ray single crystal structure and vibrational spectra of AgBF4" Solid State Sciences 2005, Volume 7, pp. 1225–1229. doi:10.1016/j.solidstatesciences.2005.06.007
  2. ↑ N. G. Connelly, W. E. Geiger (1996). "Chemical Redox Agents for Organometallic Chemistry". Chemical Reviews. 96 (2): 877–910. doi:10.1021/cr940053x. PMID 11848774.
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