1,1,2-Trichloro-1,2,2-trifluoroethane
| |||
Names | |||
---|---|---|---|
Preferred IUPAC name 1,1,2-Trichloro-1,2,2-trifluoroethane | |||
Other names Arklone P CFC-113 Freon 113 Frigen 113 TR Freon TF Valclene 1,1,2-trichlorotrifluoroethane TCTFE Solvent 113 | |||
Identifiers | |||
CAS Number |
| ||
3D model (JSmol) |
| ||
ChEMBL |
| ||
ChemSpider |
| ||
ECHA InfoCard | 100.000.852 ![]() | ||
PubChem CID |
| ||
UNII |
| ||
CompTox Dashboard (EPA) |
| ||
InChI
| |||
| |||
Properties | |||
Chemical formula | CClF2CCl2F | ||
Molar mass | 187.37 g·mol−1 | ||
Appearance | Colorless liquid | ||
Odor | like carbon tetrachloride[1] | ||
Density | 1.56 g/mL | ||
Melting point | −35 °C (−31 °F; 238 K) | ||
Boiling point | 47.7 °C (117.9 °F; 320.8 K) | ||
Solubility in water | 170 mg/L | ||
Vapor pressure | 285 mmHg (20 °C)[1] | ||
Thermal conductivity | 0.0729 W m−1 K−1 (300 K)[2] | ||
Hazards | |||
Lethal dose or concentration (LD, LC): | |||
LCLo (lowest published) | 250,000 ppm (mouse, 1.5 hr) 87,000 (rat, 6 hr)[3] | ||
NIOSH (US health exposure limits): | |||
PEL (Permissible) | TWA 1000 ppm (7600 mg/m3)[1] | ||
REL (Recommended) | TWA 1000 ppm (7600 mg/m3) ST 1250 ppm (9500 mg/m3)[1] | ||
IDLH (Immediate danger) | 2000 ppm[1] | ||
Hazards | |||
GHS labelling:[4] | |||
![]() ![]() | |||
Warning | |||
NFPA 704 (fire diamond) | ![]() 3 0 1 | ||
Safety data sheet (SDS) | https://datasheets.scbt.com/sc-251541.pdf | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). ![]() ![]() ![]() Infobox references |
1,1,2-Trichloro-1,2,2-trifluoroethane, also called trichlorotrifluoroethane (often abbreviated as TCTFE) or CFC-113, is a chlorofluorocarbon. It has the formula Cl2FC−CClF2. This colorless, volatile liquid is a versatile solvent.[5]
Production
CFC-113 can be prepared from hexachloroethane and hydrofluoric acid:[6]
This reaction may require catalysts such as antimony, chromium, iron and alumina at high temperatures.[7]
Another synthesis method uses HF on tetrachloroethylene instead.[8]
Atmospheric reactions
![](http://upload.wikimedia.org/wikipedia/commons/thumb/4/43/CFC-113_mm.png/220px-CFC-113_mm.png)
![](http://upload.wikimedia.org/wikipedia/commons/thumb/1/18/Hats_f113_global.png/220px-Hats_f113_global.png)
CFC-113 is a very unreactive chlorofluorocarbon. It remains in the atmosphere about 90 years,[9] sufficiently long that it will cycle out of the troposphere and into the stratosphere. In the stratosphere, CFC-113 can be broken up by ultraviolet radiation (UV, sunlight in the 190-225 nm range), generating chlorine radicals (Cl•), which initiate degradation of ozone requiring only a few minutes:[10][11]
- CClF2CCl2F → C2F3Cl2 + Cl•
- Cl• + O3 → ClO• + O2
This reaction is followed by:
- ClO• + O → Cl• + O2
The process regenerates Cl• to destroy more O3. The Cl• will destroy an average of 100,000 O3 molecules during its atmospheric lifetime of 1–2 years.[12]
Uses
CFC-113 was one of the most heavily produced CFCs. In 1989, an estimated 250,000 tons were produced.[5] It has been used as a cleaning agent for electrical and electronic components.[12] CFC-113’s low flammability and low toxicity made it ideal for use as a cleaner for delicate electrical equipment, fabrics, and metals. It would not harm the product it was cleaning, ignite with a spark or react with other chemicals.[13] It was used as a dry-cleaning solvent, introduced by Du Pont in March 1961 as "Valclene"[14] and was also marketed as the "solvent of the future" by Imperial Chemical Industries in the 1970s under the tradename Arklone. Others from this series were Perklone (Tetrachloroethylene), Triklone (Trichloroethylene), Methoklone (Dichloromethane) and Genklene (1,1,1-Trichloroethane).[15][16]
CFC-113 is one of the three most popular CFCs, along with CFC-11 and CFC-12.[17]
CFC-113 in laboratory analytics has been replaced by other solvents.[18]
Reduction of CFC-113 with zinc gives chlorotrifluoroethylene:[5]
- CFCl2−CClF2 + Zn → CClF=CF2 + ZnCl2
Dangers
Aside from its immense environmental impacts, Freon 113, like most chlorofluoroalkanes, forms phosgene gas when exposed to a naked flame.[19]
See also
References
- ^ a b c d e NIOSH Pocket Guide to Chemical Hazards. "#0632". National Institute for Occupational Safety and Health (NIOSH).
- ^ Touloukian, Y.S., Liley, P.E., and Saxena, S.C. Thermophysical properties of matter - the TPRC data series. Volume 3. Thermal conductivity - nonmetallic liquids and gases. Data book. 1970.
- ^ "1,1,2-Trichloro-1,2,2-trifluoroethane". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
- ^ Safety Data Sheet fishersci.com
- ^ a b c Siegemund, Günter; Schwertfeger, Werner; Feiring, Andrew; Smart, Bruce; Behr, Fred; Vogel, Herward; McKusick, Blaine (2002). "Fluorine Compounds, Organic". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a11_349. ISBN 978-3527306732.
- ^ Social and Economic Implications of Controlling the Use of Chlorofluorocarbons in the EEC pitt.edu
- ^ Kirk-Othmer Encyclopedia of Chemical Technology. 4th ed. Volumes 1: New York, NY. John Wiley and Sons, 1991-Present., p. V11 507 (1994)
- ^ Robert D. Ashford: Ashford's Dictionary of Industrial Chemicals, p. 1131. 2nd Edition. Wavelength Publications, 2001
- ^ "Global Change 2: Climate Change". University of Michigan. January 4, 2006. Archived from the original on 2008-04-20. Retrieved 2008-05-28.
- ^ Molina, Mario J. (1996). "Role of chlorine in the stratospheric chemistry". Pure and Applied Chemistry. 68 (9): 1749–1756. doi:10.1351/pac199668091749. S2CID 22107229.
- ^ "Guides | SEDAC".
- ^ a b "Chlorofluorocarbons". Columbia Encyclopedia. 2008. Retrieved 2008-05-28.
- ^ "Guides | SEDAC". sedac.ciesin.columbia.edu.
- ^ Coin-Op 1961-04: Vol 2 Iss 4 P. 61
- ^ Industrial Finishing and Surface Coatings. (1973). UK: Wheatland journals, Limited.
- ^ Morrison, R. D., Murphy, B. L. (2013). Chlorinated Solvents: A Forensic Evaluation. Royal Society of Chemistry
- ^ Zumdahl, Steven (1995). Chemical Principles. Lexington: D. C. Heath. ISBN 978-0-669-39321-7.
- ^ "Use of Ozone Depleting Substances in Laboratories. TemaNord 516/2003" (PDF). Archived from the original (PDF) on 2008-02-27. Retrieved 2008-05-06.
- ^ "False Alarms: The Legacy of Phosgene Gas". HVAC School. Retrieved 9 May 2022.
- v
- t
- e
HF | He | |||||||||||||||||
LiF | BeF2 | BF BF3 B2F4 | CF4 CxFy | NF3 N2F4 | OF OF2 O2F2 O2F | F− | Ne | |||||||||||
NaF | MgF2 | AlF AlF3 | SiF4 | P2F4 PF3 PF5 | S2F2 SF2 S2F4 SF4 S2F10 SF6 | ClF ClF3 ClF5 | HArF ArF2 | |||||||||||
KF | CaF2 | ScF3 | TiF3 TiF4 | VF2 VF3 VF4 VF5 | CrF2 CrF3 CrF4 CrF5 CrF6 | MnF2 MnF3 MnF4 | FeF2 FeF3 | CoF2 CoF3 | NiF2 NiF3 | CuF CuF2 | ZnF2 | GaF3 | GeF4 | AsF3 AsF5 | SeF4 SeF6 | BrF BrF3 BrF5 | KrF2 KrF4 KrF6 | |
RbF | SrF2 | YF3 | ZrF4 | NbF4 NbF5 | MoF4 MoF5 MoF6 | TcF6 | RuF3 RuF4 RuF5 RuF6 | RhF3 RhF5 RhF6 | PdF2 Pd[PdF6] PdF4 PdF6 | AgF AgF2 AgF3 Ag2F | CdF2 | InF3 | SnF2 SnF4 | SbF3 SbF5 | TeF4 TeF6 | IF IF3 IF5 IF7 | XeF2 XeF4 XeF6 XeF8 | |
CsF | BaF2 | * | LuF3 | HfF4 | TaF5 | WF4 WF6 | ReF6 ReF7 | OsF4 OsF5 OsF6 OsF 7 OsF8 | IrF3 IrF5 IrF6 | PtF2 Pt[PtF6] PtF4 PtF5 PtF6 | AuF AuF3 Au2F10 AuF5·F2 | HgF2 Hg2F2 HgF4 | TlF TlF3 | PbF2 PbF4 | BiF3 BiF5 | PoF4 PoF6 | At | RnF2 RnF6 |
Fr | RaF2 | ** | Lr | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og |
↓ | ||||||||||||||||||
* | LaF3 | CeF3 CeF4 | PrF3 PrF4 | NdF3 | PmF3 | SmF2 SmF3 | EuF2 EuF3 | GdF3 | TbF3 TbF4 | DyF3 | HoF3 | ErF3 | TmF2 TmF3 | YbF2 YbF3 | ||||
** | AcF3 | ThF4 | PaF4 PaF5 | UF3 UF4 UF5 UF6 | NpF3 NpF4 NpF5 NpF6 | PuF3 PuF4 PuF5 PuF6 | AmF3 AmF4 AmF6 | CmF3 | BkF3 | CfF3 | EsF3 | Fm | Md | No |
- AgPF6
- KAsF6
- LiAsF6
- NaAsF6
- HPF6
- HSbF6
- NH4PF6
- LiSbF6
- KPF6
- KSbF6
- LiPF6
- NaPF6
- NaSbF6
- TlPF6
- (NH4)3[AlF6]
- Cs2AlF5
- Li3AlF6
- K3AlF6
- Na3AlF6
and pseudohalogenides
- BaSiF6
- BaGeF6
- (NH4)2SiF6
- Na2[SiF6]
- K2[SiF6]
- Li2GeF6
- Li2SiF6
- CBrF3
- CBr2F2
- CBr3F
- CClF3
- CCl2F2
- CCl3F
- CF2O
- CF3I
- CHF3
- CH2F2
- CH3F
- C2Cl3F3
- C2H3F
- C6H5F
- C7H5F3
- C15F33N
- C3H5F
- C6H11F
lanthanide, actinide, ammonium
- VOF3
- CrOF4
- CrF2O2
- NH4F
- (NH4)3CrF6
- (NH4)2GeF6
- (NH4)3FeF6
- (NH4)3InF6
- (NH4)2SnF6
- NH4TaF6
- (NH4)3VF6
- (NH4)2ZrF6
- CsXeF7
- Li2SnF6
- Li2TiF6
- LiWF6
- Li2ZrF6
- K2TiF6
- Rb2TiF6
- Na2TiF6
- Na2ZrF6
- K2NbF7
- K2TaF7
- K2ZrF6
- UO2F2
- FNO
- FNO2
- FNO3
- KHF2
- NaHF2
- NH4HF2
and iodosyl
- F2OS
- F3OP
- PSF3
- IOF3
- IO3F
- IOF5
- IO2F
- IO2F3