Chloroform
IUPAC name Chloroform
Systematic name Trichloromethane
Other names Formyl trichloride, Methane trichloride, Methyl trichloride, Methenyl trichloride, TCM, Freon 20, R-20, UN 1888
Identifiers
CAS number	67-66-3 Y
PubChem	6212
ChemSpider	5977 Y
UNII	7V31YC746X Y
EC number	200-663-8
KEGG	C13827 Y
ChEBI	CHEBI:35255 Y
ChEMBL	CHEMBL44618 Y
RTECS number	FS9100000
Jmol-3D images	Image 1
SMILES ClC(Cl)Cl
InChI InChI=1S/CHCl3/c2-1(3)4/h1H Y Key: HEDRZPFGACZZDS-UHFFFAOYSA-N Y InChI=1/CHCl3/c2-1(3)4/h1H Key: HEDRZPFGACZZDS-UHFFFAOYAG
Properties
Molecular formula	CHCl3
Molar mass	119.38 g mol−1
Appearance	Colorless liquid
Density	1.483 g/cm3
Melting point	-63.5 °C, 210 K, -82 °F
Boiling point	61.2 °C, 334 K, 142 °F
Solubility in water	0.8 g/100 mL (20 °C)
Refractive index (nD)	1.4459
Structure
Molecular shape	Tetrahedral
Hazards
MSDS	External MSDS
R-phrases	R22, R38, R40, R48/20/22
S-phrases	(S2), S36/37
Main hazards	Harmful (Xn), Irritant (Xi), Carc. Cat. 2B
NFPA 704	0 2 0
Flash point	Non-flammable
U.S. Permissible exposure limit (PEL)	50 ppm (240 mg/m3) (OSHA)
Supplementary data page
Structure and properties	n, εr, etc.
Thermodynamic data	Phase behaviour Solid, liquid, gas
Spectral data	UV, IR, NMR, MS
Y (verify) (what is: Y/N?) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Chloroform in its liquid state shown in a test tube

Chloroform is an organic compound with formula CHCl₃. It is one of the four chloromethanes.^[1] The colorless, sweet-smelling, dense liquid is a trihalomethane, and is considered somewhat hazardous. Several million tons are produced annually as a precursor to Teflon and refrigerants, but its use for refrigerants is being phased out.^[1]

Occurrence[link]

Chloroform has a multitude of natural sources, both biogenic and abiotic. It is estimated that greater than 90% of atmospheric chloroform is of natural origin.^[2]

Marine[link]

In particular, chloroform is produced by brown seaweeds (Laminaria digitata, Laminaria saccharina, Fucus serratus, Pelvetia canaliculata, Ascophyllum nodosum), red seaweeds (Gigartina stellata, Corallina officinalis, Polysiphonia lanosa), and green seaweeds (Ulva lactuca, Enteromorpha sp., Cladophora albida).^[3] Similarly, the macroalga Eucheuma denticulatum, which is cultivated and harvested on a large scale for carrageenan production, produces chloroform,^[4] as do Hypnea spinella, Falkenbergia hillebrandii, and Gracilara cornea along with seven indigenous macroalgae inhabiting a rock pool.^[5] These studies show increased chloroform production with increased light intensity, presumably when photosynthesis is at a maximum. Chloroform is also produced by the brown algae Fucus vesiculosus, the green algae Cladophora glomerata, Enteromorpha ahlneriana, Enteromorpha flexuosa, and Enteromorpha intestinalis, and the diatom Pleurosira laevis.^[6] Other studies observe chloroform in Fucus serratus, Corallina officinalis, Cladophora pellucida, and Ulva lactuca,^[7] and Desmarestia antarctica, Lambia antarctica, Laminaria saccharina, Neuroglossum ligulatum.^[8]

Production[link]

Chloroform was discovered by three researchers independently of one another. Chloroform was reported in 1831 by the French chemist Eugène Soubeiran, who prepared it from acetone (2-propanone) as well as ethanol through the action of chlorine bleach powder (calcium hypochlorite).^[9] The American physician Samuel Guthrie prepared gallons of the material and described its "deliciousness of flavor."^[10] Independently, Justus von Liebig also described the same compound.^[11] All early preparations used variations of the haloform reaction. Chloroform was named and chemically characterized in 1834 by Jean-Baptiste Dumas.^[12]

Industrial routes[link]

In industry, chloroform is produced by heating a mixture of chlorine and either chloromethane or methane.^[1] At 400–500 °C, a free radical halogenation occurs, converting these precursors to progressively more chlorinated compounds:

CH₄ + Cl₂ → CH₃Cl + HCl

CH₃Cl + Cl₂ → CH₂Cl₂ + HCl

CH₂Cl₂ + Cl₂ → CHCl₃ + HCl

Chloroform undergoes further chlorination to yield carbon tetrachloride (CCl₄):

CHCl₃ + Cl₂ → CCl₄ + HCl

The output of this process is a mixture of the four chloromethanes (chloromethane, dichloromethane, chloroform, and carbon tetrachloride), which can then be separated by distillation.^[1]

Deuterochloroform[link]

Deuterated chloroform is an isotopologue of chloroform with a single deuterium atom. CDCl₃ is a common solvent used in NMR Spectroscopy. Deuterochloroform is produced by the haloform reaction^{[citation needed]}, the reaction of acetone (or ethanol) with sodium hypochlorite or calcium hypochlorite.^[1] The haloform process is now obsolete for the production of ordinary chloroform. Deuterochloroform can also be prepared by the reaction of sodium deuteroxide with chloral hydrate,^{[citation needed]} or from ordinary chloroform.^[13]

Inadvertent formation of chloroform[link]

The haloform reaction can also occur inadvertently in domestic settings.^{[citation needed]} Sodium hypochlorite solution (chlorine bleach) mixed with common household liquids such as acetone, butanone, ethanol, or isopropyl alcohol can produce some chloroform, in addition to other compounds such as chloroacetone or dichloroacetone.^{[citation needed]}

Uses[link]

The major use of chloroform today is in the production of the chlorodifluoromethane (R-22), a major precursor to tetrafluoroethylene:

CHCl₃ + 2 HF → CHClF₂ + 2 HCl

The reaction is conducted in the presence of a catalytic amount of antimony pentafluoride. Chlorodifluoromethane is then converted into tetrafluoroethylene, the main precursor to Teflon. Before the Montreal Protocol, chlorodifluoromethane (R22) was also a popular refrigerant.

As a solvent[link]

Chloroform is a common solvent in the laboratory because it is relatively unreactive, miscible with most organic liquids, and conveniently volatile. Chloroform is used as a solvent in the pharmaceutical industry and for producing dyes and pesticides. Chloroform is an effective solvent for alkaloids in their base form and thus plant material is commonly extracted with chloroform for pharmaceutical processing. For example, it is used in commerce to extract morphine from poppies and scopolamine from Datura plants.

It can be used to bond pieces of acrylic glass (also known under the trade names Perspex and Plexiglas).

A solvent of phenol:chloroform:isoamyl alcohol 25:24:1 is used to dissolve non-nucleic acid biomolecules in DNA and RNA extractions.

Chloroform containing deuterium (heavy hydrogen), CDCl₃, is a common solvent used in NMR spectroscopy.

As a reagent in organic synthesis[link]

As a reagent, chloroform serves as a source of the dichlorocarbene CCl₂ group.^[14] It reacts with aqueous sodium hydroxide usually in the presence of a phase transfer catalyst to produce dichlorocarbene, CCl₂.^[15][16] This reagent affects ortho-formylation of activated aromatic rings such as phenols, producing aryl aldehydes in a reaction known as the Reimer-Tiemann reaction. Alternatively the carbene can be trapped by an alkene to form a cyclopropane derivative. In the Kharasch addition chloroform forms the CHCl₂ free radical in addition to alkenes.

As an anesthetic[link]

Antique bottles of Chloroform

Chloroform was once a widely used anesthetic. Its vapor depresses the central nervous system of a patient, allowing a doctor to perform various otherwise painful procedures. On 4 November 1847, the Scottish obstetrician James Young Simpson discovered the anaethestic qualities of chloroform when he and his friends were experimenting with different substances on themselves in search of a replacement for ether as a general anesthesia. He was so astounded by the success of his own trial that the next morning he hired a chemist and within the next few days was administering it to his patients during childbirth.^[17] The use of chloroform during surgery expanded rapidly thereafter in Europe. In the 1850s, chloroform was used during the birth of Queen Victoria's last two children.^[18] In the United States, chloroform began to replace ether as an anesthetic at the beginning of the 20th century; however, it was quickly abandoned in favor of ether upon discovery of its toxicity, especially its tendency to cause fatal cardiac arrhythmia analogous to what is now termed "sudden sniffer's death". Ether is still the preferred anesthetic in some developing nations due to its high therapeutic index, and low price. One possible mechanism of action for chloroform is that it increases movement of potassium ions through certain types of potassium channels in nerve cells.^[19] Chloroform could also be mixed with other anaesthetic agents such as ether to make C.E. mixture, or ether and alcohol to make A.C.E. mixture.

Chloroform has been used by criminals to knock out, daze or even murder their victims. Joseph Harris was charged with using chloroform in 1894 to rob people.^[20] Chloroform was used to murder a woman in 1991 as a toxic dose was delivered while she was sleeping.^[21] In 2007 a man was convicted of using chloroform to sexually assault minors.^[22][23]

Safety[link]

Fatal oral dose of chloroform may be as low as 10 mL (14.8 g), with death due to respiratory or cardiac arrest.^[24]

As might be expected for an anesthetic, chloroform vapors depress the central nervous system. It is immediately dangerous to life and health at approximately 500 ppm, according to the U.S. National Institute for Occupational Safety and Health. Breathing about 900 ppm for a short time can cause dizziness, fatigue, and headache. Chronic chloroform exposure can damage the liver (where chloroform is metabolized to phosgene) and the kidneys, and some people develop sores when the skin is immersed in chloroform.

Animal studies have shown that miscarriages occur in rats and mice that have breathed air containing 30 to 300 ppm of chloroform during pregnancy and also in rats that have ingested chloroform during pregnancy. Offspring of rats and mice that breathed chloroform during pregnancy have a higher incidence of birth defects, and abnormal sperm have been found in male mice that have breathed air containing 400 ppm chloroform for a few days. The effect of chloroform on reproduction in humans is unknown.

Chloroform once appeared in toothpastes, cough syrups, ointments, and other pharmaceuticals, but it has been banned as a consumer product in the US since 1976.^[25] Cough syrups containing chloroform can still be legally purchased in pharmacies and supermarkets in the UK.

The US National Toxicology Program's twelfth report on carcinogens^[26] implicates it as reasonably anticipated to be a human carcinogen, a designation equivalent to International Agency for Research on Cancer class 2A. The IARC itself classifies chloroform as possibly carcinogenic to humans, a Group 2B designation.^[27] It has been most readily associated with hepatocellular carcinoma.^[28][29] Caution is mandated during its handling in order to minimize unnecessary exposure; safer alternatives, such as dichloromethane, have resulted in a substantial reduction of its use as a solvent.

Conversion to phosgene[link]

During prolonged storage in the presence of oxygen chloroform converts slowly to phosgene. To prevent accidents, commercial chloroform is stabilized with ethanol or amylene, but samples that have been recovered or dried no longer contain any stabilizer. Amylene has been found ineffective, and the phosgene can affect analytes in samples, lipids, and nucleic acids dissolved in or extracted with chloroform.^[30] Dissolved phosgene cannot be removed by distillation or carbon filters, but it is removed by calcium hydroxide or activated alumina.^[31]

Suspected samples can be tested for phosgene using filter paper (treated with 5% diphenylamine, 5% dimethylaminobenzaldehyde in alcohol, and then dried), which turns yellow in phosgene vapor. There are several colorimetric and fluorometric reagents for phosgene, and it can also be quantified with mass spectrometry.

References[link]

External links[link]

• Chloroform "The Molecular Lifesaver" An article at Oxford University providing facts about chloroform.
• Concise International Chemical Assessment Document 58
• IARC Summaries & Evaluations: Vol. 1 (1972), Vol. 20 (1979), Suppl. 7 (1987), Vol. 73 (1999)
• International Chemical Safety Card 0027
• NIOSH Pocket Guide to Chemical Hazards 0127
• National Pollutant Inventory - Chloroform and trichloromethane
• NIST Standard Reference Database
• Story on Chloroform from BBC's The Material World (28 July 2005)
• Sudden Sniffer's Death Syndrome article at Carolinas Poison Center
• Calculation of vapor pressure, liquid density, dynamic liquid viscosity, surface tension of chloroform
• ChemSub Online: Chloroform - Methane, trichloro-

Kirsten Prout (born September 28, 1990) is a Canadian actress born in Vancouver, British Columbia. She starred in ABC Family's drama Kyle XY as Amanda Bloom. She is also known for playing Charlotte "Char" Chamberlin on ABC Family's teen drama The Lying Game.

Early life[link]

After completing high school, Prout attended McGill University for one year, where she majored in English literature.^[1] The following summer she booked two new acting projects, and so decided to drop out of the university.^[1] Prout has a younger sister named Jennifer.^[2]

Career[link]

Prout started acting at the age of 10.^[1] She has said that the decision to go into acting was in response to a "horrible teacher in grade 2" who stifled her and made her withdraw; in response Prout's mother asked 'what can I do to make you happy again?'. The answer was acting and starting Tae Kwon Do lessons.^[3]

Prout made her feature film debut as Abby Miller in the 2005 movie Elektra, which was a commercial as well as critical failure.^[1] She has also had guest appearances on television shows such as Stargate SG-1, Cold Squad, The Dead Zone.^[4] In 2010, Prout portrayed the vampire Lucy in The Twilight Saga: Eclipse.^[5]

In 2010, Prout starred as Miranda in Seven Deadly Sins, a two-part miniseries which premiered on Lifetime on May 23. She is also set to be cast in an unnamed short film filmed in Hawaii.^{[citation needed]}

Also in 2010, Kirsten got one of the main roles in My Super Psycho Sweet 16: Part 2 as Alex Bell, Skye's little sister that she did not know about.

In 2012 she reprised her role Alex Bell in My Super Psycho Sweet 16: Part 3, the third and final installment of the franchise.

Filmography[link]

References[link]

External links[link]

• Kirsten Prout at the Internet Movie Database
• Kirsten Prout on Twitter
• Kirsten Prout Interview at DaemonsTV.com