Carbon tetrachloride

2008/9 Schools Wikipedia Selection. Related subjects: Chemical compounds

Carbon tetrachloride
IUPAC name	Carbon tetrachloride Tetrachloromethane
Other names	Benziform, Carbon chloride, Methane tetrachloride, Perchloromethane, Carbon tet, Benzinoform, Tetraform, Tetrasol, Freon 10, Halon 104, UN 1846
Identifiers
CAS number	[56-23-5]
PubChem
EINECS number
KEGG
ChEBI
RTECS number	FG4900000
SMILES	C(Cl)(Cl)(Cl)Cl
InChI	1/CCl4/c2-1(3,4)5
Properties
Molecular formula	CCl4
Molar mass	153.82 g/mol
Appearance	Colorless liquid
Density	1.5842 g/cm3, liquid 1.831 g.cm-3 at -186 °C (solid) 1.809 g.cm-3 at -80 °C (solid)
Melting point	-22.92 °C (250 K)
Boiling point	76.72 °C (350 K)
Solubility in water	0.8 g/L at 25 °C
log P	2.64
Vapor pressure	11.94 kPa at 20 °C
kH	365 kJ.mol-1 at 24.8 °C
Structure
Crystal structure	Monoclinic
Molecular shape	Tetrahedral
Hazards
MSDS	External MSDS
EU classification	Toxic (T), Carc. Cat. 2B, Dangerous for the environment (N)
NFPA 704	0 3 0
R-phrases	R23/24/25, R40, R48/23, R59, R52/53
S-phrases	(S1/2), S23, S36/37, S45, S59, S61
Flash point	Not flammable
Supplementary data page
Structure and properties	n, εr, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references

Carbon tetrachloride, also known by many other names (see Table) is the chemical compound with the formula CCl₄. It is a reagent in synthetic chemistry and was formerly widely used in fire extinguishers and as a precursor to refrigerants. It is a colorless liquid with a "sweet" smell that can be detected at low levels.

Both carbon tetrachloride and tetrachloromethane are acceptable names under IUPAC nomenclature. Colloquially, it is called "carbon tet".

History and synthesis

The production of carbon tetrachloride has steeply declined since the 1980's due to environmental concerns and the decreased demand for CFCs, which were derived from carbon tetrachloride. In 1992, production in the U.S.-Europe-Japan was estimated at 720,000,000 kg.

Carbon tetrachloride was originally synthesised in 1839 by reaction of chloroform with chlorine, from the french chemist Henri Victor Regnault, but now it is mainly synthesized from methane:

CH₄ + 4 Cl₂ → CCl₄ + 4 HCl

The production often utilizes by-products of other chlorination reactions, such as the syntheses of dichloromethane and chloroform. Higher chlorocarbons are also subjected to "chlorinolysis:"

C₂Cl₆ + Cl₂ → 2 CCl₄

Prior to the 1950's, carbon tetrachloride was manufactured by the chlorination of carbon disulfide at 105 to 130 °C:

CS₂ + 3Cl₂ → CCl₄ + S₂Cl₂

Properties

In the carbon tetrachloride molecule, four chlorine atoms are positioned symmetrically as corners in a tetrahedral configuration joined to a carbon atom, in the centre, by single covalent bonds. Because of this symmetrical geometry, the molecule has no net dipole moment; that is, CCl₄ is non-polar. As a solvent, it is well suited to dissolving other non-polar compounds, fats and oils. It is somewhat volatile, giving off vapors having a smell characteristic of other chlorinated solvents, somewhat similar to the tetrachloroethylene smell reminiscent of dry cleaners' shops.

Solid tetrachloromethane has 2 allotropes: crystaline II below -47.5 °C (225.6 K) and crystaline I above -47.5 °C.

At -47.3 °C it has monoclinic crystal structure with space group C2/c and lattice constants a = 20.3, b = 11.6, c = 19.9 (.10^-1 nm), β = 111°.

Uses

In the early 20th century, carbon tetrachloride was widely used as a dry cleaning solvent, as a refrigerant, and in fire extinguishers. However, once it became apparent that carbon tetrachloride exposure had severe adverse health effects, safer alternatives such as tetrachloroethylene were found for these applications, and its use in these roles declined from about 1940 onward. Carbon tetrachloride persisted as a pesticide to kill insects in stored grain, but in 1970, it was banned in consumer products in the United States.

Prior to the Montreal Protocol, large quantities of carbon tetrachloride were used to produce the freon refrigerants R-11 ( trichlorofluoromethane) and R-12 ( dichlorodifluoromethane). However, these refrigerants are now believed to play a role in ozone depletion and have been phased out. Carbon tetrachloride is still used to manufacture less destructive refrigerants.

Carbon tetrachloride has also been used in the detection of neutrinos. Carbon tetrachloride is one of the most potent hepatotoxins, and is widly used in scientific research to evaluate hepatoprotective agents 7,8

Reactivity

Carbon tetrachloride has practically no flammability at lower temperatures. Under high temperatures in air, it forms poisonous phosgene.

Because it has no C-H bonds, carbon tetrachloride does not easily undergo free-radical reactions. Hence it is a useful solvent for halogenations either by the elemental halogen, or by a halogenation reagent such as N-bromosuccinimide.

In organic chemistry, carbon tetrachloride serves as a source of chlorine in the Appel reaction.

Solvent

It is used as a solvent in synthetic chemistry research, but because of its adverse health effects, it is no longer commonly used, and chemists generally try to substitute it with other solvents. It is sometimes useful as a solvent for infrared spectroscopy because there are no significant absorption bands > 1600 cm^-1. Because carbon tetrachloride does not have any hydrogen atoms, it was historically used in proton NMR spectroscopy. However, carbon tetrachloride is toxic, and its dissolving power is low. Its use has been largely superseded by deuterated solvents, which offer superior solvating properties and allow for deuterium lock by the spectrometer.

Safety

Exposure to high concentrations of carbon tetrachloride (including vapor) can affect the central nervous system, degenerate the liver and kidneys and may result (after prolonged exposure) in coma and even death. Chronic exposure to carbon tetrachloride can cause liver and kidney damage and could result in cancer More information can be found in Material safety data sheets.

Carbon tetrachloride is also both ozone-depleting and a greenhouse gas. However, since 1992 its atmospheric concentrations have been in decline for the reasons described above (see also the atmospheric time-series figure).

Time-series of atmospheric concentrations of CCl₄ (Walker et al., 2000).