Hexafluorobenzene
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| Names | |||
|---|---|---|---|
| Preferred IUPAC name
Hexafluorobenzene | |||
| Other names
Perfluorobenzene
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| Identifiers | |||
3D model (JSmol)
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| Abbreviations | HFB | ||
| 1683438 | |||
| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.006.252 | ||
| EC Number |
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| 101976 | |||
PubChem CID
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| UNII | |||
CompTox Dashboard (EPA)
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| Properties | |||
| C6F6 | |||
| Molar mass | 186.056 g·mol−1 | ||
| Appearance | Colorless liquid | ||
| Density | 1.6120 g/cm3 | ||
| Melting point | 5.2 °C (41.4 °F; 278.3 K) | ||
| Boiling point | 80.1 °C (176.2 °F; 353.2 K) | ||
Refractive index (nD)
|
1.377 | ||
| Viscosity | cP (1.200 mPa•s) (20 °C) | ||
| 0.00 D (gas) | |||
| Hazards[1] | |||
| GHS labelling: | |||
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| Warning | |||
| H225 | |||
| P210, P233, P240, P241, P242, P243 | |||
| Flash point | 10 °C (50 °F; 283 K)[2] | ||
| Related compounds | |||
Related compounds
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Benzene Hexachlorobenzene Polytetrafluoroethylene Perfluorotoluene | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Hexafluorobenzene, HFB, C
6F
6, or perfluorobenzene is an organofluorine compound. In this derivative of benzene, all hydrogen atoms have been replaced by fluorine atoms. The technical uses of the compound are limited, although it has some specialized uses in the laboratory owing to distinctive spectroscopic properties.
Geometry of the aromatic ring
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:[3]
| Formula | Name | Calculated inter-halogen distance, aromatic ring assumed planar |
Twice nonbonding radius | Consequent symmetry of the benzene |
|---|---|---|---|---|
| C6F6 | hexafluorobenzene | 279 | 270 | D6h |
| C6Cl6 | hexachlorobenzene | 312 | 360 | D3d |
| C6Br6 | hexabromobenzene | 327 | 390 | D3d |
| C6I6 | hexaiodobenzene | 354 | 430 | D3d |
Hexafluorobenzene is the only perhalobenzene being planar, the other perhalobenzene species exhibiting buckling. As a consequence, in C6F6 the overlap between the p-orbitals is optimal versus the other perhalobenzenes, resulting in lower aromaticity of those compounds compared to C6F6.
Synthesis
The direct synthesis of hexafluorobenzene from benzene and fluorine has not been useful. Instead it is prepared by the reaction of alkali-fluorides with halogenated benzene:[4]
- C6Cl6 + 6 KF → C6F6 + 6 KCl
Reactions
Most reactions of hexafluorobenzene proceed with displacement of fluoride. One example is its reaction with sodium hydrosulfide to afford pentafluorothiophenol:[5]
- 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.
UV light causes gaseous HFB to isomerize to hexafluoro derivative of Dewar benzene.[6]
Laboratory applications
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.[7] 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.[8] MRI measurements of HFB based on 19F relaxation have been shown to correlate with radiation response of tumors.[9] HFB has been used as a gold standard for investigating other potential prognostic biomarkers of tumor oxygenation such as BOLD (Blood Oxygen Level Dependent),[10] TOLD (Tissue Oxygen Level Dependent) [11] and MOXI (MR oximetry) [12] A 2013 review of applications has been published.[13]
HFB has been evaluated as standard in fluorine-19 NMR spectroscopy.[14]
Toxicity
Hexafluorobenzene may cause eye and skin irritation, respiratory and digestive tract irritation and can cause central nervous system depression per MSDS.[15] The National Institute for Occupational Safety and Health (NIOSH) lists it in its Registry of Toxic Effects of Chemical Substances as neurotoxicant.
See also
References
- ^ "Hexafluorobenzene 99%". Sigma Aldrich.
- ^ Acros Organics:Catalog of fine Chemicals (1999)
- ^ Delorme, P.; Denisselle, F.; Lorenzelli, V. (1967). "Spectre infrarouge et vibrations fondamentales des dérivés hexasubstitués halogénés du benzène" [Infrared spectrum and fundamental vibrations of the hexasubstituted halogen derivatives of benzene]. Journal de Chimie Physique (in French). 64: 591–600. Bibcode:1967JCP....64..591D. doi:10.1051/jcp/1967640591.
- ^ Vorozhtsov, N. N. Jr.; Platonov, V. E.; Yakobson, G. G. (1963). "Preparation of hexafluorobenzene from hexachlorobenzene". Bulletin of the Academy of Sciences of the USSR, Division of Chemical Science. 12 (8): 1389. doi:10.1007/BF00847820.
- ^ Robson, P.; Stacey, M.; Stephens, R.; Tatlow, J. C. (1960). "Aromatic polyfluoro-compounds. Part VI. Penta- and 2,3,5,6-tetra-fluorothiophenol". Journal of the Chemical Society (4): 4754–4760. doi:10.1039/JR9600004754.
- ^ Lemal, David M. (2001). "Hexafluorobenzene Photochemistry: Wellspring of Fluorocarbon Structures". Accounts of Chemical Research. 34 (8): 662–671. doi:10.1021/ar960057j. PMID 11513574.
- ^ Zhao, D.; Jiang, L.; Mason, R. P. (2004). "Measuring changes in tumor oxygenation". In Conn, P. M. (ed.). Imaging in Biological Research, Part B. Methods in Enzymology. Vol. 386. Elsevier. pp. 378–418. doi:10.1016/S0076-6879(04)86018-X. ISBN 978-0-12-182791-5. PMID 15120262.
- ^ Zhao, D.; Jiang, L.; Hahn, E. W.; Mason, R. P. (2005). "Tumor physiologic response to combretastatin A4 phosphate assessed by MRI". International Journal of Radiation Oncology, Biology, Physics. 62 (3): 872–880. doi:10.1016/j.ijrobp.2005.03.009. PMID 15936572.
- ^ Zhao, D.; Constantinescu, A.; Chang, C.-H.; Hahn, E. W.; Mason, R. P. (2003). "Correlation of tumor oxygen dynamics with radiation response of the Dunning prostate R3327-HI tumor". Radiation Research. 159 (5): 621–631. doi:10.1667/0033-7587(2003)159[0621:COTODW]2.0.CO;2. PMID 12710873.
- ^ Zhao, D.; Jiang, L.; Hahn, E. W.; Mason, R. P. (2009). "Comparison of 1H blood oxygen level–dependent (BOLD) and 19F MRI to investigate tumor oxygenation". Magnetic Resonance in Medicine. 62 (2): 357–364. doi:10.1002/mrm.22020. PMC 4426862. PMID 19526495.
- ^ Hallac, R. R.; Zhou, H.; Pidikiti, R.; Song, K.; Stojadinovic, S.; Zhao, D.; Solberg, T.; Peschke, P.; Mason, R. P. (2014). "Correlations of noninvasive BOLD and TOLD MRI with pO2 and relevance to tumor radiation response". Magnetic Resonance in Medicine. 71 (5): 1863–1873. doi:10.1002/mrm.24846. PMC 3883977. PMID 23813468.
- ^ Zhang, Z.; Hallac, R. R.; Peschke, P.; Mason, R. P. (2014). "A noninvasive tumor oxygenation imaging strategy using magnetic resonance imaging of endogenous blood and tissue water". Magnetic Resonance in Medicine. 71 (2): 561–569. doi:10.1002/mrm.24691. PMC 3718873. PMID 23447121.
- ^ Yu, J.-X.; Hallac, R. R.; Chiguru, S.; Mason, R. P. (2013). "New frontiers and developing applications in 19F NMR". Progress in Nuclear Magnetic Resonance Spectroscopy. 70: 25–49. doi:10.1016/j.pnmrs.2012.10.001. PMC 3613763. PMID 23540575.
- ^ Rosenau, Carl Philipp; Jelier, Benson J.; Gossert, Alvar D.; Togni, Antonio (2018). "Exposing the Origins of Irreproducibility in Fluorine NMR Spectroscopy". Angewandte Chemie International Edition. 57 (30): 9528–9533. doi:10.1002/anie.201802620. PMID 29663671.
- ^ "Material safety data sheet: Hexafluorobenzene, 99%". Fisher Scientific. Thermo Fisher Scientific. n.d. Retrieved 2020-02-08.
Further reading
- Pummer, W. J.; Wall, L. A. (1958). "Reactions of hexafluorobenzene". Science. 127 (3299): 643–644. Bibcode:1958Sci...127..643P. 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. Bibcode:1974JApCr...7...87B. 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.