Carbon tetrachloride

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, dense, colourless liquid with a "sweet" chloroform-like odour that can be detected at low levels. It was formerly widely used in fire extinguishers, as a precursor to refrigerants, an anthelmintic and 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.

Quick Facts Names, Identifiers ...

Carbon tetrachloride

Names
Preferred IUPAC name Tetrachloromethane
Other names Benzinoform carbon(IV) chloride carbon tet Carboneum Tetrachloratum / Carbonei tetrachloridum Carboneum Chloratum / Carbonei chlorurum chloride of carbon Freon-10 Halon-104 methane tetrachloride methyl tetrachloride Necatorina perchloromethane Refrigerant-10 Tetrachloretum Carbonicum Tetrachlorocarbon Tetraform Tetrasol
Identifiers
CAS Number	56-23-5 Y
3D model (JSmol)	Interactive image
Abbreviations	CTC, TCM, PCM, R-10
Beilstein Reference	1098295
ChEBI	CHEBI:27385 Y
ChEMBL	ChEMBL44814 Y
ChemSpider	5730 Y
ECHA InfoCard	100.000.239
EC Number	200-262-8
Gmelin Reference	2347
KEGG	C07561 Y
PubChem CID	5943
RTECS number	FG4900000
UNII	CL2T97X0V0 Y
UN number	1846
CompTox Dashboard (EPA)	DTXSID8020250
InChI InChI=1S/CCl4/c2-1(3,4)5 Y Key: VZGDMQKNWNREIO-UHFFFAOYSA-N Y InChI=1/CCl4/c2-1(3,4)5 Key: VZGDMQKNWNREIO-UHFFFAOYAV
SMILES ClC(Cl)(Cl)Cl
Properties
Chemical formula	CCl4
Molar mass	153.81 g·mol−1
Appearance	Colourless liquid
Odor	chloroform-like odor
Density	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)
Solubility in water	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
Henry's law constant (kH)	2.76×10−2 atm·m3/mol
Magnetic susceptibility (χ)	−66.60×10−6 cm3/mol
Thermal conductivity	0.1036 W/m·K (300 K)[1]
Refractive index (nD)	1.4607
Viscosity	0.86 mPa·s[2]
Dipole moment	0 D
Structure
Crystal structure	Monoclinic
Coordination geometry	Tetragonal
Molecular shape	Tetrahedral
Dipole moment	0 D
Thermochemistry
Heat capacity (C)	132.6 J/mol·K
Std molar entropy (S⦵298)	214.39 J/mol·K
Std enthalpy of formation (ΔfH⦵298)	−95.6 kJ/mol
Gibbs free energy (ΔfG⦵)	−87.34 kJ/mol[3]
Hazards
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:
Pictograms
Signal word	Danger
Hazard statements	H301, H302, H311, H331, H351, H372, H412, H420
Precautionary statements	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)	3 0 0
Flash point	non-flammable
Lethal dose or concentration (LD, LC):
LD50 (median dose)	7749 mg/kg (oral, mouse); 5760 mg/kg (oral, rabbit); 2350 mg/kg (oral, rat)[4]
LC50 (median concentration)	5400 ppm (mammal) 8000 ppm (rat, 4 hr) 9526 ppm (mouse, 8 hr)[5]
LCLo (lowest published)	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)[6]
REL (Recommended)	Ca ST 2 ppm (12.6 mg/m3) [60-minute][6]
IDLH (Immediate danger)	200 ppm[6]
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	Chloromethane Dichloromethane Trichloromethane
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). Y verify (what is YN ?) Infobox references

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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 an odor characteristic of other chlorinated solvents, somewhat similar to the tetrachloroethylene odor 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 spilt in the environment.

Despite being generally inert, carbon tetrachloride can undergo various reactions. Hydrogen or an acid in the presence of an iron catalyst can reduce carbon tetrachloride to chloroform, dichloromethane, chloromethane and even methane.^[9] When its vapours are 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:

${\displaystyle {\ce {CCl4 + HF -> CCl3F + HCl}}}$ CCl3F + HCl}}}">

${\displaystyle {\ce {CCl4 + 2HF -> CCl2F2 + 2 HCl}}}$ CCl2F2 + 2 HCl}}}">

${\displaystyle {\ce {CCl4 + 3HF -> CClF3 + 3 HCl}}}$ CClF3 + 3 HCl}}}">

${\displaystyle {\ce {CCl4 + 4HF -> CF4 + 4 HCl}}}$ CF4 + 4 HCl}}}">

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]

${\displaystyle {\ce {CCl4 + 6KOH -> 4KCl + K2CO3 + 3H2O}}}$ 4KCl + K2CO3 + 3H2O}}}">

Carbon is sufficiently oxophilic that many compounds react to give phosgene:

Reaction with hydrogen sulfide gives thiophosgene:^[13]

${\displaystyle {\ce {CCl4 + H2S -> CCl2S + 2HCl}}}$ CCl2S + 2HCl}}}">

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 because it can be 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 + 3 Cl₂ → 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 because of 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]

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] and there have been deaths due to its conversion to phosgene reported.^[22]

Carbon tetrachloride is a suspected human carcinogen but there is no sufficient evidence of carcinogenicity in humans.^[23] The World Health Organization reports carbon tetrachloride can induce hepatocellular carcinomas (hepatomas) in mice and rats. The doses inducing hepatic tumors in mice and rats 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][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.

Carbon tetrachloride made from heavy chlorine-37 has been used in the detection of neutrinos and antineutrinos. Raymond Davis Jr. used carbon tetrachloride in his experiments to detect antineutrinos.^[41]

Carbon tetrachloride was widely used as a dry cleaning solvent, as a refrigerant, and in lava lamps.^[42] In the last case, carbon tetrachloride is a key ingredient that adds weight to the otherwise buoyant wax.

One speciality 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.

Cleaning

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 1890^[43] or 1892^[44] and as Benzinoform later.

Carbon tetrachloride was recommended for regularly cleaning the type slugs of typewriters in office settings in the 1940s.^[45]

Carbon tetrachloride was the first chlorinated solvent to be used in dry-cleaning and was used until the 1950s.^[46] It had the downsides of being corrosive to the dry-cleaning equipment and causing illness among dry-cleaning operators, and was replaced by trichloroethylene, tetrachloroethylene^[46] and methyl chloroform (trichloroethane).^[47]

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.^[48][49]

It is assumed that carbon tetrachloride was still used as a dry cleaning solvent in North Korea as of 2006.^[50]

Medical uses

Anaesthetic and analgesic

Carbon tetrachloride was briefly used as a volatile inhalation anaesthetic and analgesic for intense menstruation pains and headaches in the mid-19th century.^[51] Its anaesthetic effects were known as early as 1847 or 1848.^[52][53]

It was introduced as a safer alternative to chloroform by the doctor Protheroe Smith in 1864.^[54] 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.^[55] 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".^[56]

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.^[51] Its anaesthetic action was likened to ether, rather than the related chloroform.^[55] It is less volatile than chloroform, therefore it was more difficult to apply and needed warm water to evaporate.^[55] Its smell has been described as "fruity",^[55] quince-like^[57] and "more pleasant than chloroform",^[51] and had a "pleasant taste".^[55] 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.^[58] During anaesthesia, carbon tetrachloride has caused such violent muscular contractions and negative effects on the heart in some patients that it had to be replaced with chloroform or ether.^[55][59] Such use was experimental and the anaesthetic use of carbon tetrachloride never gained popularity due to its potential toxicity.

Parasite medication

The veterinary doctor Maurice Crowther Hall (1881-1938) discovered in 1921 that carbon tetrachloride was incredibly effective as an anthelminthic in eradicating hookworm via ingestion. In one of the clinical trials of carbon tetrachloride, it was tested on criminals to determine its safety for use in human beings.^[60] 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.^[61][62] Its toxicity was not well understood at the time and toxic effects were attributed to impurities in the capsules rather than carbon tetrachloride itself.^[63] Due to carbon tetrachloride's toxicity, tetrachloroethylene (which was also investigated by Hall in 1925) replaced its use as an anthelmintic by the 1940s.^[64]

Fire suppression

Between 1902 and 1908, carbon tetrachloride-based fire extinguishers began to appear in the United States, years after Europe.^[43]

In 1910, the Pyrene Manufacturing Company of Delaware filed a patent to use carbon tetrachloride to extinguish fires.^[66] 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 displaced oxygen in the area near the fire, but later research found that the gas inhibited the chemical chain reaction of the combustion process.^{[citation needed]}

In 1911, Pyrene patented a small, portable extinguisher that used the chemical.^[67] 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.^[68] 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.^[22]

In the first half of the 20th century, another common fire extinguisher was a single-use, sealed glass globe, a "fire grenade, " filled with 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.^[69]

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.^{[70][dead link‍]}

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 the extinguishing mixture's freezing point down to temperatures as low as –45 °C. The extinguishers with 10% trichloroethylene would contain 1% carbon disulfide as a stabiliser.^[43]

• The French writer René Daumal intoxicated himself by inhalation of carbon tetrachloride which he used to kill the beetles he collected, to "encounter other worlds" by voluntarily plunging himself into intoxications close to comatose states.^[77]
• Carbon tetrachloride is listed (along with salicylic acid, toluene, sodium tetraborate, silica gel, methanol, potassium carbonate, ethyl acetate and "BHA") as an ingredient in Peter Parker's (Spider-Man) custom web fluid formula in the book The Wakanda Files: A Technological Exploration of the Avengers and Beyond.^[78]
• Australian YouTuber Tom of Explosions&Fire and Extractions&Ire made a video on extracting carbon tetrachloride from an old fire extinguisher in 2019,^[79] and later experimenting with it by mixing it with sodium,^[80] and the chemical gained a fan base called "Tet Gang" on social media (especially on Reddit). The channel owner later used carbon tetrachloride-themed designs in the channel's merch.
• In the Ramones song "Carbona Not Glue" released in 1977, the narrator says that huffing the vapours of Carbona, a carbon tetrachloride-based stain remover, was better than huffing glue. They later removed the song from the album as Carbona was a corporate trademark.^[81]

• 
  CCl₄ measured by the Advanced Global Atmospheric Gases Experiment (AGAGE) in the lower atmosphere (troposphere) at stations around the world. Abundances are given as pollution-free monthly mean mole fractions in parts-per-trillion.
• 
  Hemispheric and Global mean concentrations of CCl₄ (NOAA/ESRL).
• 
  Time-series of atmospheric concentrations of CCl₄ (Walker et al., 2000).