|Molar mass||130.45 g mol−1|
| Std enthalpy of
|−238.49 kJ mol−1|
| Standard molar
|310.73 J K−1 mol−1|
| Except where noted otherwise, data are given for|
materials in their standard state
(at 25 °C, 100 kPa)
Infobox disclaimer and references
Chlorine pentafluoride has formula ClF5. It was first synthesized in 1963.
Its square pyramidal structure with C4v symmetry was confirmed by its high resolution19F NMR spectrum.
Initially, a common method for synthesis of this hypervalent molecule was to react ClF3 with F2 at high temperatures and high pressures. Also, reacting metal fluorides, MClF4 (i.e. KClF4, RbClF4, CsClF4) with F2 produced ClF5 and the corresponding MF. In 1981, researchers found that NiF2 is an excellent catalyst for generating ClF5.
ClF5 reacts readily with water to produce FClO4 and HF. It also a strong fluorinating agent. While unreactive with first row nonmetals, it reacts readily with second and third row nonmetals at room temperature.
- Smith D. F. (1967). "Chlorine Pentafluoride". Science. 141 (3585): 1039–1040. doi:10.1126/science.141.3585.1039.
- Pilipovich, D., Maya, W., Lawton, E.A., Bauer, H.F., Sheehan, D. F., Ogimachi, N. N., Wilson, R. D., Gunderloy, F. C., Bedwell, V. E. (1967). "Chlorine pentafluoride. Preparation and Properties". Inorganic Chemistry. 6 (10): 1918. doi:10.1021/ic50056a036.
- Šmalc, A., Žemva, B., Slivnik, J., and Lutar K. (1981). "On the Synthesis of Chlorine Pentafluoride". Journal of Fluorine Chemistry. 17: 381–383. doi:10.1016/S0022-1139(00)81783-2.