Tris(pentafluorophenyl)borane

Tris(pentafluorophenyl)borane, sometimes referred to as "BCF", is the chemical compound (C6F5)3B. It is a white, volatile solid. The molecule consists of three pentafluorophenyl groups attached in a "paddle-wheel" manner to a central boron atom; the BC3 core is planar. It has been described as the “ideal Lewis acid” because of its high thermal stability and the relative inertness of the B-C bonds. Related fluoro-substituted boron compounds, such as those containing B-CF3 groups, decompose with formation of B-F bonds. Tris(pentafluorophenyl)borane is thermally stable at temperatures wide over 200 °C, resistant to oxygen and water-tolerant.[1]

Tris(pentafluorophenyl)borane
Names
IUPAC name
Tris(pentafluorophenyl)borane
Other names
Perfluorotriphenylboron
Tris(pentafluorophenyl)boron
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.101.316
UNII
Properties
C18F15B
Molar mass 511.98 g/mol
Appearance colorless solid
Melting point 126 to 131 °C (259 to 268 °F; 399 to 404 K)
forms adduct
Structure
trigonal planar
0 D
Hazards
R-phrases (outdated) R36/37/38
S-phrases (outdated) S26 S36
Related compounds
Related compounds
 Triphenylborane (C6H5)3B
BF3
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

Preparation

Tris(pentafluorophenyl)borane is prepared using a Grignard reagent derived from bromopentafluorobenzene:

3 C6F5MgBr + BCl3 → (C6F5)3B + 3MgBrCl

Originally the synthesis employed C6F5Li, but this reagent can detonate with elimination of LiF.[1]

Structure

The structure of tris(pentafluorophenyl)borane (BCF) was determined by gas electron diffraction.[2] It has a propeller-like arrangement of its three pentafluorophenyl groups with a torsional angle of 40.6(3)° for the deviation of these groups from a hypothetically planar arrangement. Compared with a torsional angle of 56.8(4)° for tris(perfluoro-para-tolyl)borane (BTolF), which is a stronger Lewis acid than BCF, this shows that there is some delocalization of electron density from the para-fluorine atoms to the boron atom that reduces its acidity.

Lewis acidity

The most noteworthy property of this molecule is its strong Lewis acidity. Its acid strength, as determined by the Gutmann-Beckett method and the Childs[3] method, is comparable to BF3 but weaker than BCl3. This property indicates that the electronegativity of the C6F5 group and a halide are similar. Owing to the Lewis acidity of the boron center, this compound is quite sensitive to the presence of water and is irreversibly deactivated by it.

Applications in catalysis

In one application (C6F5)3B forms noncoordinating anions by removing anionic ligands from metal centers.[4] Illustrative is a reaction that give rise to alkene polymerization catalysts where tris(pentafluorophenyl)boron is used as an activator or cocatalyst:

(C6F5)3B + (C5H5)2Zr(CH3)2 → [(C5H5)2ZrCH3]+[(C6F5)3BCH3]−

In this process, the strongly coordinating methyl group transfers to the boron to expose a reactive site on zirconium. The resulting cationic zirconocene species is stabilised by the non coordinating borane anion. The exposed site on the zirconium allows for coordination of alkenes, whereupon migratory insertion into the remaining carbon-methyl ligand gives rise to a propyl ligand this process continues resulting in the growth of a polymer chain. This reagent has led to the development of immobilised catalyst/activator species; where the catalyst/activator is immobilised on an inert inorganic support such as silica.[5]

Tris(pentafluorophenyl)borane is also capable of abstracting hydride to give [(C6F5)3BH]−, and it catalyzes hydrosilylation of aldehydes. Otherwise (C6F5)3B binds to a wide range of Lewis bases, even weak ones.[6] The compound is hygroscopic, forming the trihydrate [(C6F5)3BOH2](H2O)2, wherein one water in coordinated to boron and the other two waters are hydrogen-bonded to the coordinated water.

Related compounds are pentafluorophenylboron halides.[7]

Frustrated Lewis pair

Tris(pentafluorophenyl)borane is a key reagent leading to the concept of frustrated Lewis pairs. The combination of BCF and bulky basic phosphines, such as tricyclohexylphosphine (PCy3) cleaves H2:[8]

(C6F5)3B + PCy3 + H2 → (C6F5)3BH− + HPCy3+

Many related phosphines, boranes, and substrates participate in related reactions.

Other reactions

(C6F5)3B was used to prepare a compound containing a Xe-C bond:

(C6F5)3B + XeF2 → [C6F5Xe]+[(C6F5)2BF2]−

Upon reaction with pentafluorophenyllithium, the salt of the noncoordinating anion lithium tetrakis(pentafluorophenyl)borate is formed.

(C6F5)3B + C6F5Li → Li[(C6F5)4B]
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References
  1. Piers, Warren E.; Chivers, Tristram (1997). "Pentafluorophenylboranes: from obscurity to applications". Chemical Society Reviews. 26 (5): 345. doi:10.1039/cs9972600345.
  2. Körte, Leif A.; Schwabedissen, Jan; Soffner, Marcel; Blomeyer, Sebastian; Reuter, Christian G.; Vishnevskiy, Yury V.; Neumann, Beate; Stammler, Hans-Georg; Mitzel, Norbert W. (2017-06-09). "Tris(perfluorotolyl)borane-A Boron Lewis Superacid". Angewandte Chemie International Edition. 56 (29): 8578–8582. doi:10.1002/anie.201704097. ISSN 1433-7851. PMID 28524451.
  3. Childs, R.F; Mulholland, D.L; Nixon, A. "Lewis acid adducts of α,β-unsaturated carbonyl and nitrile compounds. A nuclear magnetic resonance study" Can. J. Chem., 1982, 60, 801-808. doi:10.1139/v82-117.
  4. Fuhrmann, H.; Brenner, S.; Arndt, P.; Kempe, R. “Octahedral Group 4 Metal Complexes That Contain Amine, Amido, and Aminopyridinato Ligands: Synthesis, Structure, and Application in α-Olefin Oligo- and Polymerization”, Inorganic Chemistry, 1996, 35, 6742-6745.doi:10.1021/ic960182r
  5. Severn, J. R., Chadwick, J. C., Duchateau, R., Friederichs, N., "Bound but Not Gagged‚ Immobilizing Single-Site α-Olefin Polymerization Catalysts", Chemical Reviews 2005, volume 105, p. 4073. doi:10.1021/cr040670d
  6. Erker, G. "Tris(pentafluorophenyl)borane: A Special Boron Lewis Acid for Special Reactions", Dalton Transactions, 2005, 1883-1890. doi:10.1039/B503688G
  7. Chivers, T. “Pentafluorophenylboron halides: 40 years later”, Journal of Fluorine Chemistry, 2002, 115, 1-8. doi:10.1016/S0022-1139(02)00011-8
  8. Stephan, D. W., ""Frustrated Lewis Pairs": A New Strategy to Small Molecule Activation and Hydrogenation Catalysis", Dalton Trans. 2009, 3129.doi:10.1039/B819621D

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