Chlorine pentafluoride
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| Identifiers | |||
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13637-63-3 
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| 3D model (Jmol) | Interactive image | ||
| ChemSpider | 55559 | ||
| ECHA InfoCard | 100.033.734 | ||
| PubChem | 61654 | ||
| RTECS number | FO2975000 | ||
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| Properties | |||
| ClF5 | |||
| Molar mass | 130.445 g mol−1 | ||
| Appearance | colorless gas | ||
| Density | 4.5 kg/m3 (g/L) | ||
| Melting point | −103 °C (−153 °F; 170 K) | ||
| Boiling point | −13.1 °C (8.4 °F; 260.0 K) | ||
| hydrolyzes | |||
| Structure | |||
| Square pyramidal | |||
| Thermochemistry | |||
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Std molar
entropy (S |
310.73 J K−1 mol−1 | ||
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Std enthalpy of
formation (ΔfH |
−238.49 kJ mol−1 | ||
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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 | |||
Chlorine pentafluoride is an interhalogen compound with formula ClF5. This colourless gas is a strong oxidant that was once a candidate oxidizer for rockets. The molecule adopts a square pyramidal structure with C4vsymmetry, as confirmed by its high resolution 19F NMR spectrum.
Some of the earliest research on the preparation was classified. It was first prepared by fluorination of chlorine trifluoride at high temperatures and high pressures:
NiF2 catalyzes this reaction.
Certain metal fluorides, MClF4 (i.e. KClF4, RbClF4, CsClF4) react with F2 to produce ClF5 and the corresponding alkali metal fluoride.
In a highly exothermic reaction, water hydrolyses ClF5 to produce chloryl fluoride and hydrogen fluoride:
It is also a strong fluorinating agent. At room temperature it reacts readily with all elements except noble gases, nitrogen, oxygen and fluorine.
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