1. As an anion in inorganic and organic chemistry

2. Examples of salts

3. See also

4. References

Tetrafluoroborate is the anion {{chem|BF|4|−}}. This tetrahedral species is isoelectronic with tetrafluoromethane, CF₄ and tetrafluoroammonium {{chem|NF|4|+}}, and is valence isoelectronic with many stable and important species including the perchlorate anion, {{chem|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.

As an anion in inorganic and organic chemistry

The popularization of {{chem|BF|4|−}} has led to decreased use of {{chem|ClO|4|−}} in the laboratory as a weakly coordinating anion. With organic compounds, especially amine derivatives, {{chem|ClO|4|−}} forms potentially explosive derivatives. Disadvantages to {{chem|BF|4|−}} include its slight sensitivity to hydrolysis and decomposition via loss of a fluoride ligand, whereas {{chem|ClO|4|−}} does not suffer from these problems. Safety considerations, however, overshadow this inconvenience. With a formula weight of 86.8, BF₄^– 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 {{chem|BF|4|−}} anion is less nucleophilic and basic (and therefore more weakly coordinating) than nitrates, halides or even triflates. Thus, when using salts of {{chem|BF|4|−}}, one can usually assume that the cation is the reactive agent and this tetrahedral anion is inert. {{chem|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, {{chem|BF|4|−}} salts are often more soluble in organic solvents (lipophilic) than the related nitrate or halide salts. Related to {{chem|BF|4|−}} are hexafluorophosphate, {{chem|PF|6|−}}, and hexafluoroantimonate, {{chem|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 {{chem|BF|4|−}}, so in such cases {{chem|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]

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

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 caesium.

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

• Diazonium compounds ({{chem|ArN|2|+}}).
• Meerwein reagents such as {{chem|OEt|3|+}}, the strongest commercial alkylating agents.
• NO⁺ a one-electron oxidizing agent and nitrosylation reagent.
• NO₂⁺, a nitration reagent.
• Ferrocenium, {{chem|Fe(C|5|H|5|)|2|+}}, and other cationic metallocenes.
• Selectfluor, a fluorination agent, and other N–F electrophilic fluorine sources.
• Silver tetrafluoroborate and thallium tetrafluoroborate^[3] 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.
• Transition metal nitrile complexes, e.g. [Cu(NCMe)₄]BF₄.

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.

See also

• Non-coordinating anion

References

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