Chlorine trifluoride

Chlorine trifluoride
	Systematic name Trifluoro-λ3-chlorane (substitutive)
Other names	Chlorotrifluoride
Identifiers
CAS number	7790-91-2
PubChem	24637
EC number	232-230-4
MeSH	chlorine+trifluoride
ChEBI	CHEBI:30123
RTECS number	FO2800000
SMILES	F[Cl](F)F
	InChI
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
Density	3.779 g/L
Melting point	−76.34 °C, 197 K, -105 °F
Boiling point
Solubility in water	Reacts with water
Solubility	Soluble in carbon tetrachloride but explosive in high concentrations. Reacts with hydrogen-containing compounds e.g. hydrogen, methane, benzene, ether, ammonia.
Vapor pressure	175 kPa
Magnetic susceptibility (χ)	−26.5×10−6 cm3/mol
Viscosity	91.82 μPa s
Structure
Molecular shape	T-shaped molecular geometry
Thermochemistry
Std enthalpy of; formation ΔfHo298	−163.2 kJ mol−1
Standard molar; entropy So298	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
NFPA 704	0 4 4
Flash point	Noncombustible
U.S. Permissible; exposure limit (PEL)	C 0.1 ppm (0.4 mg/m3)
	Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)

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.

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.

References

↑ ^1.0 ^1.1 ^1.2 "Chlorine trifluoride". PubChem Compound. National Center for Biotechnology Information. 4 July 2023. 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. "#0117". National Institute for Occupational Safety and Health (NIOSH).
↑ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.58. ISBN 978-1-4398-5511-9.
↑ Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.132. ISBN 978-1-4398-5511-9.
↑ OSHA. "Occupational Safety and Health Guidelines for Chlorine Trifluoride". OSHA. Archived from the original on 22 March 2011. Retrieved 25 November 2010.

[pubchem-1] 1.0 ^1.1 ^1.2 "Chlorine trifluoride". PubChem Compound. National Center for Biotechnology Information. 4 July 2023. Retrieved 8 July 2023.

[CLFazine-2] ClF₃/Hydrazine Archived 2007-02-02 at the Wayback Machine at the Encyclopedia Astronautica.

[PGCH-3] 3.0 ^3.1 ^3.2 NIOSH Pocket Guide to Chemical Hazards. "#0117". National Institute for Occupational Safety and Health (NIOSH).

[crc1-4] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.58. ISBN 978-1-4398-5511-9.

[5] Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.132. ISBN 978-1-4398-5511-9.

[6] OSHA. "Occupational Safety and Health Guidelines for Chlorine Trifluoride". OSHA. Archived from the original on 22 March 2011. Retrieved 25 November 2010.

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