Chlorine trifluoride
Chlorine trifluoride is a chemical compound. Its chemical formula is ClF3. It contains chlorine and fluoride ions. The chlorine is in its +3 oxidation state.
| Names | |
|---|---|
| Systematic IUPAC name
Trifluoro-λ3-chlorane[1] (substitutive) | |
| Other names
Chlorotrifluoride
| |
| Identifiers | |
| CAS number | |
| PubChem | |
| EC number | 232-230-4 |
| MeSH | |
| ChEBI | CHEBI:30123 |
| RTECS number | FO2800000 |
| SMILES | F[Cl](F)F |
| Gmelin Reference | 1439 |
| Properties | |
| Molecular formula | Cl3 |
| Molar mass | 92.45 g mol-1 |
| Appearance | Colorless gas or greenish-yellow liquid |
| Odor | Sweet, pungent, irritating, suffocating[2][3] |
| Density | 3.779 g/L[4] |
| Melting point |
−76.34 °C, 197 K, -105 °F |
| Boiling point | |
| Solubility in water | Reacts with water[1] |
| Solubility | Soluble in carbon tetrachloride but explosive in high concentrations. Reacts with hydrogen-containing compounds e.g. hydrogen, methane, benzene, ether, ammonia.[1] |
| Vapor pressure | 175 kPa |
| −26.5×10−6 cm3/mol[5] | |
| Viscosity | 91.82 μPa s |
| Structure | |
| Molecular shape | T-shaped molecular geometry |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
−163.2 kJ mol−1 |
| Standard molar entropy S |
281.6 J K−1 mol−1 |
| Specific heat capacity, C | 63.9 J K−1 mol−1 |
| Hazards | |
| Main hazards | Very toxic, very corrosive, powerful oxidizer, violent hydrolysis[3] |
| NFPA 704 |
0
4
4
|
| Flash point | Noncombustible |
| U.S. Permissible exposure limit (PEL) |
C 0.1 ppm (0.4 mg/m3)[3] |
Properties
Chlorine trifluoride is a colorless gas, but it can be compressed to a light yellow liquid. Chlorine trifluoride is normally sold compressed. It is an interhalogen, and is very reactive. It can burn plastics, sand,[6] skin, hydrogen sulfide, metals, phosphorus, and sulfur. Since it is a much stronger oxidizing agent than oxygen, it can burn things that normally can't burn, like concrete or sand. It reacts with water very violently to make hydrofluoric acid and hydrochloric acid. It can ignite glass after being in it for a while.
Preparation
Chlorine trifluoride is made by reacting chlorine with fluorine. This makes other chlorine fluorides which have to be taken out.
Uses
Chlorine trifluoride is used to make uranium hexafluoride by reacting it with uranium metal. It was looked at as a rocket propellant. It was also looked at as a poison gas. It is too difficult to make and store, though. Chlorine trifluoride can be used to clean areas where semiconductors are made.
Safety
Chlorine trifluoride is extremely toxic and dangerous. It is one of the most dangerous chemicals there is. It can catch many things on fire, including things that are usually non-flammable, such as asbestos, concrete, and glass. The fires are almost impossible to put out. It reacts with most things.
Related pages
Chlorine pentafluoride
Chlorine monofluoride
Chlorine dioxide
Bromine trifluoride
Iodine trifluoride.
References
- ↑ 1.0 1.1 1.2 Chlorine trifluoride. PubChem Compound (4 July 2023)National Center for Biotechnology Information. Retrieved 8 July 2023.
- ↑ ClF3/Hydrazine Archived 2007-02-02 at the Wayback Machine at the Encyclopedia Astronautica.
- ↑ 3.0 3.1 3.2 NIOSH Pocket Guide to Chemical Hazards. #0117National Institute for Occupational Safety and Health (NIOSH).
- ↑ CRC Handbook of Chemistry and Physics (2011)CRC Press. p. 4.58. ISBN 978-1-4398-5511-9.
- ↑ CRC Handbook of Chemistry and Physics (2011)CRC Press. p. 4.132. ISBN 978-1-4398-5511-9.
- ↑ OSHA. Occupational Safety and Health Guidelines for Chlorine TrifluorideOSHA. Retrieved 25 November 2010.