Carbon tetrachloride
Structural formula of tetrachloride
Structural formula of tetrachloride
Space-filling model carbon tetrachloride
Space-filling model carbon tetrachloride
Carbon tetrachloride
Preferred IUPAC name
Other names
carbon(IV) chloride
carbon tet
Carboneum Tetrachloratum / Carbonei tetrachloridum
Carboneum Chloratum / Carbonei chlorurum
chloride of carbon
methane tetrachloride
methyl tetrachloride
perchloromethane, PCM
Tetrachloretum Carbonicum
3D model (JSmol)
ECHA InfoCard 100.000.239 Edit this at Wikidata
EC Number
  • 200-262-8
RTECS number
  • FG4900000
UN number 1846
  • InChI=1S/CCl4/c2-1(3,4)5 checkY
  • InChI=1/CCl4/c2-1(3,4)5
  • ClC(Cl)(Cl)Cl
Molar mass 153.81 g·mol−1
Appearance Colourless liquid
Odor Sweet, chloroform-like odor
  • 1.5867 g·cm−3 (liquid)
  • 1.831 g·cm−3 at −186 °C (solid)
  • 1.809 g·cm−3 at −80 °C (solid)
Melting point −22.92 °C (−9.26 °F; 250.23 K)
Boiling point 76.72 °C (170.10 °F; 349.87 K)
  • 0.097 g/100 mL (0 °C)
  • 0.081 g/100 mL (25 °C)
Solubility Soluble in alcohol, ether, chloroform, benzene, naphtha, CS2, formic acid
log P 2.64
Vapor pressure 11.94 kPa at 20 °C
2.76×10−2 atm·m3/mol
−66.60×10−6 cm3/mol
Thermal conductivity 0.1036 W/m·K (300 K)[1]
Viscosity 0.86 mPa·s[2]
0 D
0 D
132.6 J/mol·K
214.39 J/mol·K
−95.6 kJ/mol
−87.34 kJ/mol[3]
Occupational safety and health (OHS/OSH):
Main hazards
extremely toxic to the liver and kidneys, potential occupational carcinogen, harmful to the ozone layer
GHS labelling:
GHS06: ToxicGHS07: Exclamation markGHS08: Health hazard
H301, H302, H311, H331, H351, H372, H412, H420
P201, P202, P260, P261, P264, P270, P271, P273, P280, P281, P301+P310, P302+P352, P304+P340, P308+P313, P311, P312, P314, P321, P322, P330, P361, P363, P403+P233, P405, P501, P502
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
Lethal dose or concentration (LD, LC):
250 mg/kg[citation needed]
  • 5400 ppm (mammal)
  • 8000 ppm (rat, 4 hr)
  • 9526 ppm (mouse, 8 hr)[5]
  • 1000 ppm (human)
  • 20,000 ppm (guinea pig, 2 hr)
  • 38,110 ppm (cat, 2 hr)
  • 50,000 ppm (human, 5 min)
  • 14,620 ppm (dog, 8 hr)[5]
NIOSH (US health exposure limits):
PEL (Permissible)
TWA 10 ppm C 25 ppm 200 ppm (5-minute maximum peak in any 4 hours)[4]
REL (Recommended)
Ca ST 2 ppm (12.6 mg/m3) [60-minute][4]
IDLH (Immediate danger)
200 ppm[4]
Safety data sheet (SDS) ICSC 0024
Related compounds
Other anions
Carbon tetrafluoride
Carbon tetrabromide
Carbon tetraiodide
Other cations
Silicon tetrachloride
Germanium tetrachloride
Tin tetrachloride
Lead tetrachloride
Related chloromethanes
Supplementary data page
Carbon tetrachloride (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Carbon tetrachloride, also known by many other names (such as carbon tet for short and tetrachloromethane, also recognised by the IUPAC) is a chemical compound with the chemical formula CCl4. It is a non-flammable, colourless liquid with a "sweet" chloroform-like smell that can be detected at low levels. It was formerly widely used in fire extinguishers, as a precursor to refrigerants and as a cleaning agent, but has since been phased out because of environmental and safety concerns. Exposure to high concentrations of carbon tetrachloride can affect the central nervous system and degenerate the liver and kidneys. Prolonged exposure can be fatal.

Tradenames include: Carbon-Tet, Katharin (Germany, 1890s),[6] Benzinoform, Carbona and Thawpit in the cleaning industry, Halon-104 in firefighting, Refrigerant-10 in HVACR, and Necatorina and Seretin as a medication.


In the carbon tetrachloride molecule, four chlorine atoms are positioned symmetrically as corners in a tetrahedral configuration joined to a central carbon atom by single covalent bonds. Because of this symmetric geometry, CCl4 is non-polar. Methane gas has the same structure, making carbon tetrachloride a halomethane. As a solvent, it is well suited to dissolving other non-polar compounds such as fats and oils. It can also dissolve iodine. It is volatile, giving off vapors with a smell characteristic of other chlorinated solvents, somewhat similar to the tetrachloroethylene smell reminiscent of dry cleaners' shops.

Solid tetrachloromethane has two polymorphs: crystalline II below −47.5 °C (225.6 K) and crystalline I above −47.5 °C.[7] 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°.[8]

With a specific gravity greater than 1, carbon tetrachloride will be present as a dense nonaqueous phase liquid if sufficient quantities are spilled in the environment.


Despite being generally inert, carbon tetrachloride can undergo various reactions. Hydrogen or an acid in presence of an iron catalyst can reduce carbon tetrachloride to chloroform, dichloromethane, chloromethane and even methane.[9] When its vapours passed through a red-hot tube, carbon tetrachloride dechlorinates to Tetrachloroethylene and hexachloroethane. [10]

Carbon tetrachloride, when treated with HF, gives various compounds such as trichlorofluoromethane (R-11), dichlorodifluoromethane (R-12), chlorotrifluoromethane (R-13) and carbon tetrafluoride with HCl as the by-product:

This was once one of the main uses of carbon tetrachloride, as R-11 and R-12 were widely used as refrigerants.

An alcohol solution of potassium hydroxide decomposes it to potassium chloride and potassium carbonate in water:[11]

When a mixture of carbon tetrachloride and carbon dioxide is heated to 350 degrees C, it gives phosgene: [12] A similar reaction with carbon monoxide instead gives phosgene and tetrachloroethylene:


Reaction with hydrogen sulfide gives thiophosgene:[13]

Reaction with sulfur trioxide gives phosgene and pyrosulfuryl chloride:[13]

Reaction with phosphoric anhydride gives phosgene and phosphoryl chloride:[13]

Carbon tetrachloride reacts with dry zinc oxide at 200 degrees Celsius to yield zinc chloride, phosgene and carbon dioxide:[12]

History and synthesis

Carbon tetrachloride was originally synthesized in 1820 by Michael Faraday, who named it "protochloride of carbon", by decomposition of hexachloroethane ("perchloride of carbon") which he synthesized by chlorination of ethylene.[14][15] The protochloride of carbon has been previously misidentified as tetrachloroethylene due to being made with the same reaction of hexachloroethane. Later in the 19th century, the name protochloride of carbon was used for tetrachloroethylene, and carbon tetrachloride was called "bichloride of carbon" or "perchloride of carbon". Henri Victor Regnault developed another method to synthesise carbon tetrachloride from chloroform, chloroethane or methanol with excess chlorine in 1839.[16]

Kolbe made carbon tetrachloride in 1845 by passing chlorine over carbon disulfide through a porcelain tube.[16] Prior to the 1950s, carbon tetrachloride was manufactured by the chlorination of carbon disulfide at 105 to 130 °C:[17]

CS2 + 3Cl2 → CCl4 + S2Cl2

But now it is mainly produced from methane:

CH4 + 4 Cl2 → CCl4 + 4 HCl

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

C2Cl6 + Cl2 → 2 CCl4

The production of carbon tetrachloride has steeply declined since the 1980s 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 tonnes.[17]

Natural occurrence

Carbon Tetrachloride was discovered along with chloromethane and chloroform in oceans, marine algae and volcanoes.[18] The natural emissions of carbon tetrachloride are too little compared to those from anthropogenic sources; for example, the Momotombo Volcano in Nicaragua emits carbon tetrachloride at a flux of 82 grams per year while the global industrial emissions were at 2 × 1010 grams per year.[19]

Carbon tetrachloride was found in Red algae Asparagopsis taxiformis and Asparagopsis armata.[20] It was detected in Southern California ecosystems, salt lakes of Kalmykian Steppe and a common liverwort in Czechia.[19]


At high temperatures in air, it decomposes or burns to produce poisonous phosgene. This was a common problem when carbon tetrachloride was used as a fire extinguisher:[21] there have been deaths due to its conversion to phosgene reported.[22]

Carbon tetrachloride is a suspected human carcinogen based on sufficient evidence of carcinogenicity from studies in experimental animals.[23] The World Health Organization reports carbon tetrachloride can induce hepatocellular carcinomas (hepatomas) in mice and rats. The doses inducing hepatic tumours are higher than those inducing cell toxicity.[24] The International Agency for Research on Cancer (IARC) classified this compound in Group 2B, "possibly carcinogenic to humans".[25] Carbon tetrachloride is one of the most potent hepatotoxins (toxic to the liver), so much so that it is widely used in scientific research to evaluate hepatoprotective agents.[26][27] Exposure to high concentrations of carbon tetrachloride (including vapor) can affect the central nervous system and degenerate the liver[27] and kidneys,[28] and prolonged exposure may lead to coma or death.[29] Chronic exposure to carbon tetrachloride can cause liver[30][31] and kidney damage and could result in cancer.[32] See safety data sheets.[33]

Consumption of alcohol increases the toxic effects of carbon tetrachloride and may cause more severe organ damage, such as acute renal failure, in heavy drinkers. The doses that can cause mild toxicity to non-drinkers can be fatal to drinkers.[34]

The effects of carbon tetrachloride on human health and the environment have been assessed under REACH in 2012 in the context of the substance evaluation by France.[35]

In 2008, a study of common cleaning products found the presence of carbon tetrachloride in "very high concentrations" (up to 101 mg/m3) as a result of manufacturers' mixing of surfactants or soap with sodium hypochlorite (bleach).[36]

Carbon tetrachloride is also both ozone-depleting[37] and a greenhouse gas.[38] However, since 1992[39] its atmospheric concentrations have been in decline for the reasons described above (see atmospheric concentration graphs in the gallery). CCl4 has an atmospheric lifetime of 85 years.[40]


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

The mechanism of the Appel reaction
The mechanism of the Appel reaction

Carbon tetrachloride made from heavy chlorine-37 has been used in the detection of neutrinos.

Historical uses

Carbon tetrachloride was widely used as a dry cleaning solvent, as a refrigerant, and in lava lamps.[41] In the last case, carbon tetrachloride is a key ingredient that adds weight to the otherwise buoyant wax.

One specialty use of carbon tetrachloride was in stamp collecting, to reveal watermarks on postage stamps without damaging them. A small amount of the liquid is placed on the back of a stamp, sitting in a black glass or obsidian tray. The letters or design of the watermark can then be seen clearly. Today, this is done on lit tables without using carbon tetrachloride.


Being a good solvent for many materials (such as grease and tar), carbon tetrachloride was widely used as a cleaning fluid for nearly 70 years. It is nonflammable and nonexplosive, and did not leave any odour on the cleaned material unlike gasoline which was also used for cleaning at the time. It was used as a "safe" alternative to gasoline. It was first marketed as Katharin, in 1892[42] and as Benzinoform later.

German advertisement stamp for Benzinoform (carbon tetrachloride) stain remover, 1912

Carbon tetrachloride was the first chlorinated solvent to be used in dry-cleaning and used until the 1950s.[43] It was corrosive to the dry-cleaning equipment and caused illness among dry-cleaning operators and was replaced by trichloroethylene, tetrachloroethylene[43] and methyl chloroform (trichloroethane).[44]

Carbon tetrachloride was also used as an alternative to petrol (gasoline) in dry shampoos, from the beginning of 1903 to the 1930s. Several women had fainted from its fumes during the hair wash in barber shops, the hairdressers often used electric fans to blow the fumes away. In 1909, a baronet's daughter, Helenora Elphinstone-Dalrymple (aged 29), died after having her hair shampooed with carbon tetrachloride.[45][46]

It is assumed that carbon tetrachloride was still used as a dry cleaning solvent in North Korea as of 2006.[47]

Medical uses

Carbon tetrachloride has been briefly used as a volatile inhalation anaesthetic and analgesic for intense menstruation pains and headaches in the mid-19th century.[48] Its anaesthetic effects were known as early as 1847 or 1848.[49][50]

It was introduced as a safer alternative to Chloroform by Doctor Protheroe Smith in 1864.[51] In December 1865, the Scottish obstetrician who discovered the anaesthetic effects of chloroform on humans, James Young Simpson, had experimented with carbon tetrachloride as an anaesthetic.[52] Simpson named the compound "Chlorocarbon" for its similarity to chloroform. His experiments involved injecting carbon tetrachloride into two women's vaginas. Simpson orally consumed carbon tetrachloride and described it as having "the same effect as swallowing a capsule of chloroform".[53]

Because of the higher amount of chlorine atoms (compared to chloroform) in its molecule, carbon tetrachloride has a stronger anaesthetic effect than chloroform and required a smaller amount.[48] Its anaesthetic action was likened to ether, rather than the relates chloroform.[52] It is less volatile than chloroform, therefore it was more difficult to apply and needed warm water to evaporate.[52] Its smell has been described as "fruity",[52] quince-like[54] and "more pleasant than chloroform",[48] and had a "pleasant taste".[52] Carbon tetrachloride for anaesthetic use was made by the chlorination of carbon disulfide. It was used on at least 50 patients, of which most were women in labour.[55] During anaesthesia, carbon tetrachloride has caused violent muscular contractions and negative effects on the heart in some patients that it had to be substituted with chloroform or ether.[52][56] Such use was experimental and the anaesthetic use of carbon tetrachloride never gained popularity due to its potential toxicity.

No hay que desesperarse, la Necatorina salva (do not despair, Necatorina saves)
Advertisement for Merck's Necatorina, Colombia, 1942

The veterinary doctor Maurice Crowther Hall (1881-1938) discovered in 1921 that carbon tetrachloride was incredibly effective as an anthelminthic in eradicating hookworm by ingesting it. Beginning in 1922, capsules of pure carbon tetrachloride were marketed by Merck under the name Necatorina (variants include Neo-necatorina and Necatorine). Necatorina was used as a medication against parasitic diseases in humans. This medication was most prevalently used in Latin American countries.[57][58] Its toxicity was not well-understood at the time and toxic effects were attributed to impurities in the capsules rather than carbon tetrachloride itself.[59]


It once was a popular solvent in organic chemistry, but because of its adverse health effects, it is rarely used today.[26] It is sometimes useful as a solvent for infrared spectroscopy, because there are no significant absorption bands above 1600 cm−1. Because carbon tetrachloride does not have any hydrogen atoms, it was historically used in proton NMR spectroscopy. In addition to being toxic, its dissolving power is low.[60] Its use in NMR spectroscopy has been largely superseded by deuterated solvents (mainly deuterochloroform). Use of carbon tetrachloride in determination of oil has been replaced by various other solvents, such as tetrachloroethylene.[26] Because it has no C–H bonds, carbon tetrachloride does not easily undergo free-radical reactions. It is a useful solvent for halogenations either by the elemental halogen or by a halogenation reagent such as N-bromosuccinimide (these conditions are known as Wohl–Ziegler bromination).

Fire suppression

A brass Pyrene carbon tetrachloride fire extinguisher
A Red Comet brand glass globe ("fire grenade") containing carbon tetrachloride

In 1910, the Pyrene Manufacturing Company of Delaware filed a patent to use carbon tetrachloride to extinguish fires.[61] The liquid was vaporized by the heat of combustion and extinguished flames, an early form of gaseous fire suppression. At the time it was believed the gas simply displaced oxygen in the area near the fire, but later research found that the gas actually inhibits the chemical chain reaction of the combustion process.[citation needed]

In 1911, Pyrene patented a small, portable extinguisher that used the chemical.[62] The extinguisher consisted of a brass bottle with an integrated hand-pump that was used to expel a jet of liquid toward the fire. As the container was unpressurized, it could easily be refilled after use.[63] Carbon tetrachloride was suitable for liquid and electrical fires and the extinguishers were often carried on aircraft or motor vehicles. However, as early as 1920, there were reports of fatalities caused by the chemical when used to fight a fire in a confined space.[64]

In the first half of the 20th century, another common fire extinguisher was a single-use, sealed glass globe known as a "fire grenade", filled with either carbon tetrachloride or salt water. The bulb could be thrown at the base of the flames to quench the fire. The carbon tetrachloride type could also be installed in a spring-loaded wall fixture with a solder-based restraint. When the solder melted by high heat, the spring would either break the globe or launch it out of the bracket, allowing the extinguishing agent to be automatically dispersed into the fire.[65]

A well-known brand of fire grenade was the "Red Comet", which was variously manufactured with other fire-fighting equipment in the Denver, Colorado area by the Red Comet Manufacturing Company from its founding in 1919 until manufacturing operations were closed in the early 1980s.[66]

Since carbon tetrachloride freezes at –23 °C, the fire extinguishers would contain only 89-90% carbon tetrachloride and 10% trichloroethylene (m.p. –85 °C) or chloroform (m.p. –63 °C) for lowering its freezing point. The extinguishers with 10% trichloroethylene would contain 1% carbon disulfide as a stabiliser.[67]


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


Carbon tetrachloride was widely used as a fumigant to kill insect pests in stored grain.[68] It was employed in a mixture known as 80/20, that was 80% carbon tetrachloride and 20% Carbon disulfide.[69] The United States Environmental Protection Agency banned its use in 1985.[70]

Society and culture

Famous deaths from carbon tetrachloride poisoning



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