Hexafluorobenzene

Hexafluorobenzene stands somewhat aside in the perhalogenbenzenes. When counting for bond angles and distances it is possible to calculate the distance between two ortho fluorine atoms. Also the non bonding radius of the halogens is known. The following table presents the results:[2]

The conclusion of the table is HFB is the only perhalobenzene being planar, the others all are buckled more or less. As a consequence in C₆F₆ the overlap between the p-orbitals is optimal, while in the others it is less, also giving rise to a lower aromaticity in those compounds.

The direct synthesis of hexafluorobenzene from benzene and fluorine is not possible. The synthetic route proceeds via the reaction of alkali-fluorides with halogenated benzene:[3]

C₆Cl₆ + 6 KF → C₆F₆ + 6 KCl

In the laboratory hexafluorobenzene is used for several purposes:

• standard in fluorine-19 NMR
• solvent and standard in carbon-13 NMR
• solvent in proton NMR
• solvent when studying some parts in the IR spectrum
• solvent in UV spectra, as hexafluorobenzene itself hardly shows any absorbance in the UV region.

Most reactions of HFB proceed with displacement of fluoride. One example is its reaction with sodium hydrosulfide to afford pentafluorothiophenol:[4]

C₆F₆ + NaSH → C₆F₅SH + NaF

The reaction of pentafluorophenyl derivatives has been long puzzling for its mechanism. Independent of the substituent, they all exhibit a para directing effect. The new introduced group too has no effect on the directing behaviour. In all cases, a 1,4-disubstituted-2,3,5,6-tetrafluorobenzene derivative shows up. Finally, the clue is found not in the nature of the non-fluorine substituent, but in the fluorines themselves. The π-electropositive effect introduces electrons into the aromatic ring. The non-fluorine substituent is not capable of doing so. As charge accumulates at the ortho and para positions relative to the donating group, the ortho and para-positions relative to the non-fluorine substituent receive less charge, so are less negative or more positive. Furthermore, the non-fluorine substituent in general is more bulky than fluorine, so its ortho-positions are sterically shielded, leaving the para-position as the sole reaction site for anionic entering groups.

Hexafluorobenzene has been used as a reporter molecule to investigate tissue oxygenation in vivo. It is exceedingly hydrophobic, but exhibits high gas solubility with ideal liquid gas interactions. Since molecular oxygen is paramagnetic it causes ¹⁹F NMR spin lattice relaxation (R1): specifically a linear dependence R1= a + bpO₂ has been reported.[5] HFB essentially acts as molecular amplifier, since the solubility of oxygen is greater than in water, but thermodynamics require that the pO2 in the HFB rapidly equilibrates with the surrounding medium. HFB has a single narrow ¹⁹F NMR signal and the spin lattice relaxation rate is highly sensitive to changes in pO₂, yet minimally responsive to temperature. HFB is typically injected directly into a tissue and ¹⁹F NMR may be used to measure local oxygenation. It has been extensively applied to examine changes in tumor oxygenation in response to interventions such as breathing hyperoxic gases or as a consequence of vascular disruption.[6] MRI measurements of HFB based on 19F relaxation have been shown to correlate with radiation response of tumors.[7] HFB has been used as a gold standard for investigating other potential prognostic biomarkers of tumor oxygenation such as BOLD (Blood Oxygen Level Dependent),[8] TOLD (Tissue Oxygen Level Dependent) [9] and MOXI (MR oximetry) [10] A 2013 review of applications has been published.[11]

Hexafluorobenzene may cause eye and skin irritation, respiratory and digestive tract irritation and can cause central nervous system depression per MSDS.[12] The National Institute for Occupational Safety and Health (NIOSH) lists it in its Registry of Toxic Effects of Chemical Substances as neurotoxicant.

• Pentafluorobenzene

• Pummer, W. J.; Wall, L. A. (1958). "Reactions of hexafluorobenzene". Science. 127 (3299): 643–644. doi:10.1126/science.127.3299.643. PMID 17808882.
• US patent 3277192, Fielding, H. C., "Preparation of hexafluorobenzene and fluorochlorobenzenes", issued 1966-10-04, assigned to Imperial Chemical Industries
• Bertolucci, M. D.; Marsh, R. E. (1974). "Lattice parameters of hexafluorobenzene and 1,3,5-trifluorobenzene at −17°C". Journal of Applied Crystallography. 7 (1): 87–88. doi:10.1107/S0021889874008764.
• Samojłowicz, C.; Bieniek, M.; Pazio, A.; Makal, A.; Woźniak, K.; Poater, A.; Cavallo, L.; Wójcik, J.; Zdanowski, K.; Grela, K. (2011). "The doping effect of fluorinated aromatic solvents on the rate of ruthenium‐catalysed olefin metathesis". Chemistry—A European Journal. 17 (46): 12981–12993. doi:10.1002/chem.201100160. PMID 21956694.