Silver tetrafluoroborate

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Silver tetrafluoroborate
Silver tetrafluoroborate.png
Silver-tetrafluoroborate-xtal-3D-SF.png
Identifiers
CAS number 14104-20-2 YesY
PubChem 159722
ChemSpider 140438 YesY
EC number 237-956-5
RTECS number ED2875000
Jmol-3D images Image 1
Properties
Molecular formula 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)
Solubility in water soluble
Hazards
MSDS External MSDS
EU classification 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
Except where noted otherwise, 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 formula AgBF4. It is a white solid that dissolves in polar organic solvents as well as water. In solid, the Ag+ centers are bound to fluoride.[1]

Preparation[edit]

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

Laboratory uses[edit]

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[edit]

  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.