Fluoroform

Fluoroform

Names
IUPAC name Trifluoromethane
Other names Fluoroform, carbon trifluoride,[citation needed] methyl trifluoride, Fluoryl, Freon 23, Arcton 1
Identifiers
CAS Number	75-46-7 Y
3D model (JSmol)	Interactive image
Abbreviations	HFC 23, R-23, FE-13, UN 1984
ChEBI	CHEBI:24073 N
ChemSpider	21106179 Y
ECHA InfoCard	100.000.794
EC Number	200-872-4
PubChem CID	6373
RTECS number	PB6900000
UNII	ZJ51L9A260 Y
CompTox Dashboard (EPA)	DTXSID0026410
InChI InChI=1S/CHF3/c2-1(3)4/h1H Y Key: XPDWGBQVDMORPB-UHFFFAOYSA-N Y InChI=1/CHF3/c2-1(3)4/h1H Key: XPDWGBQVDMORPB-UHFFFAOYAM
SMILES FC(F)F
Properties
Chemical formula	CHF3
Molar mass	70.014 g·mol−1
Appearance	Colorless gas
Density	2.946 kg/m3 (gas, 1 bar, 15 °C)
Melting point	−155.2 °C (−247.4 °F; 118.0 K)
Boiling point	−82.1 °C (−115.8 °F; 191.1 K)
Solubility in water	1 g/l
Solubility in organic solvents	Soluble
Vapor pressure	4.38 MPa at 20 °C
Henry's law constant (kH)	0.013 mol·kg−1·bar−1
Acidity (pKa)	25–28
Structure
Molecular shape	Tetrahedral
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Nervous system depression
GHS labelling:[1]
Pictograms
Signal word	Warning
Hazard statements	H280
Precautionary statements	P403
NFPA 704 (fire diamond)	2 0 0
Flash point	Non-flammable
Related compounds
Related compounds	Fluoromethane CH3F Difluoromethane CH2F2 Tetrafluoromethane CF4 Chloroform CHCl3 Bromoform CHBr3 Iodoform CHI3 Chlorodifluoromethane CHF2Cl Dichlorofluoromethane CHFCl2 Bromodichloromethane CHCl2Br Dibromochloromethane CHClBr2 Bromodifluoromethane CHF2Br Dibromofluoromethane CHFBr2 Deuterated chloroform CDCl3
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). N verify (what is YN ?) Infobox references

Fluoroform, or trifluoromethane, is the chemical compound with the formula CHF₃. It is a hydrofluorocarbon as well as being a part of the haloforms, a class of compounds with the formula CHX₃ (X = halogen) with C_3v symmetry. Fluoroform is used in diverse applications in organic synthesis. It is not an ozone depleter but is a greenhouse gas.^[2]

About 20 million kg per year are produced industrially as both a by-product of and precursor to the manufacture of Teflon.^[2] It is produced by reaction of chloroform with HF:^[3]

CHCl₃ + 3 HF → CHF₃ + 3 HCl

It is also generated biologically in small amounts apparently by decarboxylation of trifluoroacetic acid.^[4]

Fluoroform was first obtained by Maurice Meslans in the violent reaction of iodoform with dry silver fluoride in 1894.^[5] The reaction was improved by Otto Ruff by substitution of silver fluoride by a mixture of mercury fluoride and calcium fluoride.^[6] The exchange reaction works with iodoform and bromoform, and the exchange of the first two halogen atoms by fluorine is vigorous. By changing to a two step process, first forming a bromodifluoromethane in the reaction of antimony trifluoride with bromoform and finishing the reaction with mercury fluoride the first efficient synthesis method was found by Henne.^[6]

CHF₃ is used in the semiconductor industry in plasma etching of silicon oxide and silicon nitride. Known as R-23 or HFC-23, it was also a useful refrigerant, sometimes as a replacement for chlorotrifluoromethane (CFC-13) and is a byproduct of its manufacture.

When used as a fire suppressant, the fluoroform carries the DuPont trade name, FE-13. CHF₃ is recommended for this application because of its low toxicity, its low reactivity, and its high density. HFC-23 has been used in the past as a replacement for Halon 1301(CFC-13B1) in fire suppression systems as a total flooding gaseous fire suppression agent.

Fluoroform is weakly acidic with a pK_a = 25–28 and quite inert. Attempted deprotonation results in defluorination to generate F⁻ and difluorocarbene (CF₂). Some organocopper and organocadmium compounds have been developed as trifluoromethylation reagents.^[7]

Fluoroform is a precursor of the Ruppert-Prakash reagent CF₃Si(CH₃)₃, which is a source of the nucleophilic CF−3 anion.^[8][9]

CHF₃ is a potent greenhouse gas. A ton of HFC-23 in the atmosphere has the same effect as 11,700 tons of carbon dioxide. This equivalency, also called a 100-yr global warming potential, is slightly larger at 14,800 for HFC-23.^[10] The atmospheric lifetime is 270 years.^[10]

HFC-23 was the most abundant HFC in the global atmosphere until around 2001, when the global mean concentration of HFC-134a (1,1,1,2-tetrafluoroethane), the chemical now used extensively in automobile air conditioners, surpassed those of HFC-23. Global emissions of HFC-23 have in the past been dominated by the inadvertent production and release during the manufacture of the refrigerant HCFC-22 (chlorodifluoromethane).

Substantial decreases in HFC-23 emissions by developed countries were reported from the 1990s to the 2000s: from 6-8 Gg/yr in the 1990s to 2.8 Gg/yr in 2007.^[11]

The UNFCCC Clean Development Mechanism provided funding and facilitated the destruction of HFC-23.

Developing countries have become the largest producers of HCFC-23 in recent years according to data compiled by the Ozone Secretariat of the World Meteorological Organization.^[12][13][14] Emissions of all HFCs are included in the UNFCCCs Kyoto Protocol. To mitigate its impact, CHF₃ can be destroyed with electric plasma arc technologies or by high temperature incineration.^[15]

• McBee E. T. (1947). "Fluorine Chemistry". Industrial & Engineering Chemistry. 39 (3): 236–237. doi:10.1021/ie50447a002.
• Oram D. E.; Sturges W. T.; Penkett S. A.; McCulloch A.; Fraser P. J. (1998). "Growth of fluoroform (CHF₃, HFC-23) in the background atmosphere". Geophysical Research Letters. 25 (1): 236–237. Bibcode:1998GeoRL..25...35O. doi:10.1029/97GL03483.
• McCulloch A. (2003). "Fluorocarbons in the global environment: a review of the important interactions with atmospheric chemistry and physics". Journal of Fluorine Chemistry. 123 (1): 21–29. doi:10.1016/S0022-1139(03)00105-2.

• International Chemical Safety Card 0577
• MSDS at Oxford University
• MSDS at mathesontrigas.com
• Coupling of fluoroform with aldehydes using an electrogenerated base