The popularization of BF− 4 has led to decreased use of ClO− 4 in the laboratory as a weakly coordinating anion. With organic compounds, especially amine derivatives, ClO− 4 forms potentially explosive derivatives. Disadvantages to BF− 4 include its slight sensitivity to hydrolysis and decomposition via loss of a fluoride ligand, whereas ClO− 4 does not suffer from these problems. Safety considerations, however, overshadow this inconvenience. With a formula weight of 86.8, BF– 4 is also conveniently the smallest weakly coordinating anion from the point of view of equivalent weight, often making it the anion of choice for preparing cationic reagents or catalysts for use in synthesis, in the absence of other substantial differences in chemical or physical factors.
The BF− 4 anion is less nucleophilic and basic (and therefore more weakly coordinating) than nitrates, halides or even triflates. Thus, when using salts of BF− 4, it is usually assumed that the cation is the reactive agent and this tetrahedral anion is inert. BF− 4 owes its inertness to two factors: (i) it is symmetrical so that the negative charge is distributed equally over four atoms, and (ii) it is composed of highly electronegative fluorine atoms, which diminish the basicity of the anion. In addition to the weakly coordinating nature of the anion, BF− 4 salts are often more soluble in organic solvents (lipophilic) than the related nitrate or halide salts. Related to BF− 4 are hexafluorophosphate, PF− 6, and hexafluoroantimonate, SbF− 6, both of which are even more stable toward hydrolysis and other chemical reactions and whose salts tend to be more lipophilic.
Extremely reactive cations such as those derived from Ti, Zr, Hf, and Si do in fact abstract fluoride from BF− 4, so in such cases BF− 4 is not an "innocent" anion and weakly coordinating anions (e.g., SbF6–, BARF–, or [Al((CF3)3CO)4]–) must be employed. Moreover, in other cases of ostensibly "cationic" complexes, the fluorine atom in fact acts as a bridging ligand between boron and the cationic center. For instance, the gold complex [μ-(DTBM-SEGPHOS)(Au–BF4)2] was found crystallographically to contain two Au–F–B bridges.[1]
Transition and heavy metal fluoroborates are produced in the same manner as other fluoroborate salts; the respective metal salts are added to reacted boric and hydrofluoric acids. Tin, lead, copper, and nickel fluoroborates are prepared through electrolysis of these metals in a solution containing HBF4.
As a fluoride donor
Despite the low reactivity of the tetrafluoroborate anion in general, BF− 4 serves as a fluorine source to deliver an equivalent of fluoride.[2] The Balz–Schiemann reaction for the synthesis of aryl fluorides is the best known example of such a reaction.[3] Ether and halopyridine adducts of HBF4 have been reported to be effective reagents for the hydrofluorination of alkynes.[4]
Examples of salts
Potassium fluoroborate is obtained by treating potassium carbonate with boric acid and hydrofluoric acid.
Silver tetrafluoroborate and thallium tetrafluoroborate[6] are convenient halide abstracting agents (although the thallium salt is highly toxic). Most other transition metal tetrafluoroborates only exist as solvates of water, alcohols, ethers, or nitriles.
An electrochemical cycle involving ferrous/ferric tetrafluoroborate is being used to replace thermal smelting of lead sulfide ores by the Doe Run Company.
^Cresswell, Alexander J.; Davies, Stephen G.; Roberts, Paul M.; Thomson, James E. (2015). "Beyond the Balz–Schiemann Reaction: The Utility of Tetrafluoroborates and Boron Trifluoride as Nucleophilic Fluoride Sources". Chemical Reviews. 115 (2): 566–611. doi:10.1021/cr5001805. PMID25084541.
^Cresswell, Alexander J.; Davies, Stephen G.; Roberts, Paul M.; Thomson, James E. (2015-01-28). "Beyond the Balz–Schiemann Reaction: The Utility of Tetrafluoroborates and Boron Trifluoride as Nucleophilic Fluoride Sources". Chemical Reviews. 115 (2): 566–611. doi:10.1021/cr5001805. ISSN0009-2665. PMID25084541.
^Willem L. Driessen, Jan Reedijk (1992). "Solid Solvates: The Use of Weak Ligands in Coordination Chemistry". Inorganic Syntheses. Vol. 29. pp. 111–118. doi:10.1002/9780470132609.ch27. ISBN978-0-470-13260-9.
^Möller, H.; Lutz, H. D. (2010). "Crystal structure of thallium tetrafluoroborate, TlBF4". Zeitschrift für Kristallographie - Crystalline Materials. 201 (3–4): 285–286. doi:10.1524/zkri.1992.201.3-4.285. ISSN2196-7105.
