Tetrafluoroborate

Tetrafluoroborate is the anion BF−
4. This tetrahedral species is isoelectronic with tetrafluoroberyllate (BeF2−
4), tetrafluoromethane (CF4), and tetrafluoroammonium (NF+
4) and is valence isoelectronic with many stable and important species including the perchlorate anion, ClO−
4, which is used in similar ways in the laboratory. It arises by the reaction of fluoride salts with the Lewis acid BF3, treatment of tetrafluoroboric acid with base, or by treatment of boric acid with hydrofluoric acid.

The structure of the tetrafluoroborate anion, BF−
4

As an anion in inorganic and organic chemistry

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, one can usually assume 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.

Illustrative of a fluoroborate salt is [Ni(CH3CH2OH)6](BF4)2, a kinetically labile octahedral complex, which is used as a source of Ni2+.[1]

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 less 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.[2]

Despite the low reactivity of the tetrafluoroborate anion in general, BF−
4 serves as a fluorine source to deliver an equivalent of fluoride to highly electrophilic carbocationic species to generate carbon–fluorine bonds. 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]

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.

Examples of salts

Potassium fluoroborate is obtained by treating potassium carbonate with boric acid and hydrofluoric acid.

B(OH)3 + 4 HF → HBF4 + 3 H2O
2 HBF4 + K2CO3 → 2 KBF4 + H2CO3

Fluoroborates of alkali metals and ammonium ions crystallize as water-soluble hydrates with the exception of potassium, rubidium, and cesium.

Fluoroborate is often used to isolate highly electrophilic cations. Some examples include:

An electrochemical cycle involving ferrous/ferric tetrafluoroborate is being used to replace thermal smelting of lead sulfide ores by the Doe Run Company.

Imidazolium and formamidinium salts, ionic liquids and precursors to stable carbenes, are often isolated as tetrafluoroborates.

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See also

References
  1. Willem L. Driessen, Jan Reedijk (1992). "Solid Solvates: The Use of Weak Ligands in Coordination Chemistry". Inorganic Syntheses. Inorganic Syntheses. 29. pp. 111–118. doi:10.1002/9780470132609.ch27. ISBN 978-0-470-13260-9.
  2. Abadie, Marc-Antoine; Trivelli, Xavier; Medina, Florian; Capet, Frédéric; Roussel, Pascal; Agbossou-Niedercorn, Francine; Michon, Christophe (2014-08-01). "Asymmetric Intramolecular Hydroamination of Alkenes in Mild and Wet Conditions—Structure and Reactivity of Cationic Binuclear Gold(I) Catalysts". ChemCatChem. 6 (8): 2235–2239. doi:10.1002/cctc.201402350. ISSN 1867-3899.
  3. 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. ISSN 0009-2665. PMID 25084541.
  4. Guo, Rui; Qi, Xiaotian; Xiang, Hengye; Geaneotes, Paul; Wang, Ruihan; Liu, Peng; Wang, Yi-Ming (2020-06-02). "Stereodivergent Alkyne Hydrofluorination Using Protic Tetrafluoroborates as Tunable Reagents". Angewandte Chemie International Edition. n/a (n/a). doi:10.1002/anie.202006278. ISSN 1521-3773.
  5. 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. ISSN 2196-7105.
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