Phenol

This article is about the molecule. For the group of chemicals that contains a phenol group, see Phenols.

"Carbolic acid" redirects here. Not to be confused with carbonic acid or carboxylic acid.

Phenol (systematically named Benzenol, also called carbolic acid or phenolic acid) is an aromatic organic compound with the molecular formula C₆H₅OH. It is a white crystalline solid that is volatile. The molecule consists of a phenyl group (−C₆H₅) bonded to a hydroxy group (−OH). Mildly acidic, it requires careful handling because it can cause chemical burns.

Phenol

Names
Preferred IUPAC name Phenol^[1]
Systematic IUPAC name Benzenol
Other names Carbolic acid Phenolic acid Phenylic acid Hydroxybenzene Phenic acid Phenyl alcohol
Identifiers
CAS Number	108-95-2^Y
3D model (JSmol)	Interactive image
ChEBI	CHEBI:15882^Y
ChEMBL	ChEMBL14060^Y
ChemSpider	971^Y
DrugBank	DB03255^Y
ECHA InfoCard	100.003.303
KEGG	D00033^Y
PubChem CID	996
RTECS number	SJ3325000
UNII	339NCG44TV^Y
CompTox Dashboard (EPA)	DTXSID5021124
InChI InChI=1S/C6H6O/c7-6-4-2-1-3-5-6/h1-5,7H^Y Key: ISWSIDIOOBJBQZ-UHFFFAOYSA-N^Y InChI=1/C6H6O/c7-6-4-2-1-3-5-6/h1-5,7H
SMILES Oc1ccccc1
Properties
Chemical formula	C6H6O
Molar mass	94.113 g/mol
Appearance	Transparent crystalline solid
Odor	Sweet and tarry
Density	1.07 g/cm^3
Melting point	40.5 °C (104.9 °F; 313.6 K)
Boiling point	181.7 °C (359.1 °F; 454.8 K)
Solubility in water	8.3 g/100 mL (20 °C)
log P	1.48^[2]
Vapor pressure	0.4 mmHg (20 °C)^[3]
Acidity (pKa)	9.95 (in water), 18.0 (in DMSO), 29.1 (in acetonitrile)^[4]
Conjugate base	Phenoxide
UV-vis (λmax)	270.75 nm^[5]
Dipole moment	1.224 D
Pharmacology
ATC code	C05BB05 (WHO) D08AE03 (WHO), N01BX03 (WHO), R02AA19 (WHO)
Hazards
GHS labelling:
Pictograms	^[6]
Hazard statements	H301, H311, H314, H331, H341, H373^[6]
Precautionary statements	P261, P280, P301+P310, P305+P351+P338, P310^[6]
NFPA 704 (fire diamond)	3 2 0
Flash point	79 °C (174 °F; 352 K)
Explosive limits	1.8–8.6%^[3]
Lethal dose or concentration (LD, LC):
LD50 (median dose)	317 mg/kg (rat, oral) 270 mg/kg (mouse, oral)^[7]
LDLo (lowest published)	420 mg/kg (rabbit, oral) 500 mg/kg (dog, oral) 80 mg/kg (cat, oral)^[7]
LC50 (median concentration)	19 ppm (mammal) 81 ppm (rat) 69 ppm (mouse)^[7]
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 5 ppm (19 mg/m^3) [skin]^[3]
REL (Recommended)	TWA 5 ppm (19 mg/m^3) C 15.6 ppm (60 mg/m^3) [15-minute] [skin]^[3]
IDLH (Immediate danger)	250 ppm^[3]
Safety data sheet (SDS)	[2]
Related compounds
Related compounds	Thiophenol Sodium phenoxide
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

Phenol was first extracted from coal tar, but today is produced on a large scale (about 7 million tonnes a year) from petroleum-derived feedstocks. It is an important industrial commodity as a precursor to many materials and useful compounds.^[8] It is primarily used to synthesize plastics and related materials. Phenol and its chemical derivatives are essential for production of polycarbonates, epoxies, Bakelite, nylon, detergents, herbicides such as phenoxy herbicides, and numerous pharmaceutical drugs.

Properties

Phenol is an organic compound appreciably soluble in water, with about 84.2 g dissolving in 1000 mL (0.895 M). Homogeneous mixtures of phenol and water at phenol to water mass ratios of ~2.6 and higher are possible. The sodium salt of phenol, sodium phenoxide, is far more water-soluble.

Acidity

Phenol is a weak acid. In aqueous solution in the pH range ca. 8 - 12 it is in equilibrium with the phenolate anion C₆H₅O⁻ (also called phenoxide or carbolate):^[9]

${\displaystyle {\ce {C6H5OH <=> C6H5O- + H+}}}$ 

 

Resonance structures of the phenoxide anion

Phenol is more acidic than aliphatic alcohols. The differing pKa is attributed to resonance stabilization of the phenoxide anion. In this way, the negative charge on oxygen is delocalized on to the ortho and para carbon atoms through the pi system.^[10] An alternative explanation involves the sigma framework, postulating that the dominant effect is the induction from the more electronegative sp² hybridised carbons; the comparatively more powerful inductive withdrawal of electron density that is provided by the sp² system compared to an sp³ system allows for great stabilization of the oxyanion. In support of the second explanation, the pK_a of the enol of acetone in water is 10.9, making it only slightly less acidic than phenol (pK_a 10.0).^[11] Thus, the greater number of resonance structures available to phenoxide compared to acetone enolate seems to contribute very little to its stabilization. However, the situation changes when solvation effects are excluded. A recent in silico comparison of the gas phase acidities of the vinylogues of phenol and cyclohexanol in conformations that allow for or exclude resonance stabilization leads to the inference that about 1⁄3 of the increased acidity of phenol is attributable to inductive effects, with resonance accounting for the remaining difference.^[12]

Hydrogen bonding

In carbon tetrachloride and alkane solvents phenol hydrogen bonds with a wide range of Lewis bases such as pyridine, diethyl ether, and diethyl sulfide. The enthalpies of adduct formation and the −OH IR frequency shifts accompanying adduct formation have been studied.^[13] Phenol is classified as a hard acid which is compatible with the C/E ratio of the ECW model with E_A = 2.27 and C_A = 1.07. The relative acceptor strength of phenol toward a series of bases, versus other Lewis acids, can be illustrated by C-B plots.^[14][15]

Phenoxide anion

The phenoxide anion is a strong nucleophile with a nucleophilicity comparable to the one of carbanions or tertiary amines.^[16] It can react at both its oxygen or carbon sites as an ambident nucleophile (see HSAB theory). Generally, oxygen attack of phenoxide anions is kinetically favored, while carbon-attack is thermodynamically preferred (see Thermodynamic versus kinetic reaction control). Mixed oxygen/carbon attack and by this a loss of selectivity is usually observed if the reaction rate reaches diffusion control.^[17]

Tautomerism

 

Phenol-cyclohexadienone tautomerism

Phenol exhibits keto-enol tautomerism with its unstable keto tautomer cyclohexadienone, but only a tiny fraction of phenol exists as the keto form. The equilibrium constant for enolisation is approximately 10⁻¹³, which means only one in every ten trillion molecules is in the keto form at any moment.^[18] The small amount of stabilisation gained by exchanging a C=C bond for a C=O bond is more than offset by the large destabilisation resulting from the loss of aromaticity. Phenol therefore exists essentially entirely in the enol form.^[19] 4, 4' Substituted cyclohexadienone can undergo a dienone–phenol rearrangement in acid conditions and form stable 3,4‐disubstituted phenol.^[20]

Phenoxides are enolates stabilised by aromaticity. Under normal circumstances, phenoxide is more reactive at the oxygen position, but the oxygen position is a "hard" nucleophile whereas the alpha-carbon positions tend to be "soft".^[21]

Reactions

 

Neutral phenol substructure "shape". An image of a computed electrostatic surface of neutral phenol molecule, showing neutral regions in green, electronegative areas in orange-red, and the electropositive phenolic proton in blue.

 

Phenol water phase diagram: Certain combinations of phenol and water can make two solutions in one bottle.

Phenol is highly reactive toward electrophilic aromatic substitution. The enhance nucleophilicity is attributed to donation pi electron density from O into the ring. Many groups can be attached to the ring, via halogenation, acylation, sulfonation, and related processes. Phenol's ring is so strongly activated that bromination and chlorination lead readily to polysubstitution.^[22] Phenol reacts with dilute nitric acid at room temperature to give a mixture of 2-nitrophenol and 4-nitrophenol while with concentrated nitric acid, additional nitro groups are introduced, e.g. to give 2,4,6-trinitrophenol.

Aqueous solutions of phenol are weakly acidic and turn blue litmus slightly to red. Phenol is neutralized by sodium hydroxide forming sodium phenate or phenolate, but being weaker than carbonic acid, it cannot be neutralized by sodium bicarbonate or sodium carbonate to liberate carbon dioxide.

${\displaystyle {\ce {C6H5OH + NaOH -> C6H5ONa + H2O}}}$ 

When a mixture of phenol and benzoyl chloride are shaken in presence of dilute sodium hydroxide solution, phenyl benzoate is formed. This is an example of the Schotten–Baumann reaction:

${\displaystyle {\ce {C6H5COCl + HOC6H5 -> C6H5CO2C6H5 + HCl}}}$ 

Phenol is reduced to benzene when it is distilled with zinc dust or when its vapour is passed over granules of zinc at 400 °C:^[23]

${\displaystyle {\ce {C6H5OH + Zn -> C6H6 + ZnO}}}$ 

When phenol is treated with diazomethane in the presence of boron trifluoride (BF₃), anisole is obtained as the main product and nitrogen gas as a byproduct.

${\displaystyle {\ce {C6H5OH + CH2N2 -> C6H5OCH3 + N2}}}$ 

When phenol reacts with iron(III) chloride solution, an intense violet-purple solution is formed.

Production

Because of phenol's commercial importance, many methods have been developed for its production, but the cumene process is the dominant technology.

Cumene process

 

Accounting for 95% of production (2003) is the cumene process, also called Hock process. It involves the partial oxidation of cumene (isopropylbenzene) via the Hock rearrangement:^[8] Compared to most other processes, the cumene process uses relatively mild conditions and relatively inexpensive raw materials. For the process to be economical, both phenol and the acetone by-product must be in demand.^[24][25] In 2010, worldwide demand for acetone was approximately 6.7 million tonnes, 83 percent of which was satisfied with acetone produced by the cumene process.

A route analogous to the cumene process begins with cyclohexylbenzene. It is oxidized to a hydroperoxide, akin to the production of cumene hydroperoxide. Via the Hock rearrangement, cyclohexylbenzene hydroperoxide cleaves to give phenol and cyclohexanone. Cyclohexanone is an important precursor to some nylons.^[26]

Oxidation of benzene, toluene, cyclohexylbenzene

The direct oxidation of benzene (C₆H₆) to phenol is theoretically possible and of great interest, but it has not been commercialized:

${\displaystyle {\ce {C6H6 + O -> C6H5OH}}}$ 

Nitrous oxide is a potentially "green" oxidant that is a more potent oxidant than O₂. Routes for the generation of nitrous oxide however remain uncompetitive.^[27][24][26]

An electrosynthesis employing alternating current gives phenol from benzene.^[28]

The oxidation of toluene, as developed by Dow Chemical, involves copper-catalyzed reaction of molten sodium benzoate with air:

${\displaystyle {\ce {C6H5CH3 + 2 O2 -> C6H5OH + CO2 + H2O}}}$ 

The reaction is proposed to proceed via formation of benzyoylsalicylate.^[8]

Autoxidation of cyclohexylbenzene give the hydroperoxide. Decomposition of this hydroperoxide affords cyclohexanone and phenol.^[8]

Older methods

Early methods relied on extraction of phenol from coal derivatives or the hydrolysis of benzene derivatives.

Hydrolysis of benzenesulfonic acid

The original commercial route was developed by Bayer and Monsanto in the early 1900s, based on discoveries by Wurtz and Kekule. The method involves the reaction of strong base with benzenesulfonic acid, proceeding by the reaction of hydroxide with sodium benzenesulfonate to give sodium phenoxide. Acidification of the latter gives phenol. The net conversion is:^[29]

${\displaystyle {\ce {C6H5SO3H + 2 NaOH -> C6H5OH + Na2SO3 + H2O}}}$ 

Hydrolysis of chlorobenzene

Chlorobenzene can be hydrolyzed to phenol using base (Dow process) or steam (Raschig–Hooker process):^[25][26][30]

${\displaystyle {\ce {C6H5Cl + NaOH -> C6H5OH + NaCl}}}$ 

${\displaystyle {\ce {C6H5Cl + H2O -> C6H5OH + HCl}}}$ 

These methods suffer from the cost of the chlorobenzene and the need to dispose of the chloride by product.

Coal pyrolysis

Phenol is also a recoverable byproduct of coal pyrolysis.^[30] In the Lummus Process, the oxidation of toluene to benzoic acid is conducted separately.

Miscellaneous methods

 

Amine to phenol^[31]

Phenyldiazonium salts hydrolyze to phenol. The method is of no commercial interest since the precursor is expensive.^[31]

${\displaystyle {\ce {C6H5NH2 + HCl + NaNO2 -> C6H5OH + N2 + H2O + NaCl}}}$ 

 

Salicylic acid decarboxylates to phenol.^[32]

Uses

The major uses of phenol, consuming two thirds of its production, involve its conversion to precursors for plastics. Condensation with acetone gives bisphenol-A, a key precursor to polycarbonates and epoxide resins. Condensation of phenol, alkylphenols, or diphenols with formaldehyde gives phenolic resins, a famous example of which is Bakelite. Partial hydrogenation of phenol gives cyclohexanone, a precursor to nylon. Nonionic detergents are produced by alkylation of phenol to give the alkylphenols, e.g., nonylphenol, which are then subjected to ethoxylation.^[8]

Phenol is also a versatile precursor to a large collection of drugs, most notably aspirin but also many herbicides and pharmaceutical drugs.

Phenol is a component in liquid–liquid phenol–chloroform extraction technique used in molecular biology for obtaining nucleic acids from tissues or cell culture samples. Depending on the pH of the solution either DNA or RNA can be extracted.

Medical

Phenol is widely used as an antiseptic. Its use was pioneered by Joseph Lister (see § History section).

From the early 1900s to the 1970s it was used in the production of carbolic soap. Concentrated phenol liquids are commonly used for permanent treatment of ingrown toe and finger nails, a procedure known as a chemical matrixectomy. The procedure was first described by Otto Boll in 1945. Since that time it has become the chemical of choice for chemical matrixectomies performed by podiatrists.

Concentrated liquid phenol can be used topically as a local anesthetic for otology procedures, such as myringotomy and tympanotomy tube placement, as an alternative to general anesthesia or other local anesthetics. It also has hemostatic and antiseptic qualities that make it ideal for this use.

Phenol spray, usually at 1.4% phenol as an active ingredient, is used medically to treat sore throat.^[33] It is the active ingredient in some oral analgesics such as Chloraseptic spray, TCP and Carmex.^[34]

Niche uses

Phenol is so inexpensive that it attracts many small-scale uses. It is a component of industrial paint strippers used in the aviation industry for the removal of epoxy, polyurethane and other chemically resistant coatings.^[35]

Phenol derivatives have been used in the preparation of cosmetics including sunscreens,^[36] hair colorings, and skin lightening preparations.^[37] However, due to safety concerns, phenol is banned from use in cosmetic products in the European Union^[38][39] and Canada.^[40][41]

History

Phenol was discovered in 1834 by Friedlieb Ferdinand Runge, who extracted it (in impure form) from coal tar.^[42] Runge called phenol "Karbolsäure" (coal-oil-acid, carbolic acid). Coal tar remained the primary source until the development of the petrochemical industry. The French chemist Auguste Laurent extracted phenol in its pure form, as a derivative of benzene, in 1841.^[43]

In 1836, Auguste Laurent coined the name "phène" for benzene;^[44] this is the root of the word "phenol" and "phenyl". In 1843, French chemist Charles Gerhardt coined the name "phénol".^[45]

The antiseptic properties of phenol were used by Sir Joseph Lister (1827–1912) in his pioneering technique of antiseptic surgery. Lister decided that the wounds themselves had to be thoroughly cleaned. He then covered the wounds with a piece of rag or lint^[46] covered in carbolic acid (phenol). The skin irritation caused by continual exposure to phenol eventually led to the introduction of aseptic (germ-free) techniques in surgery.

Joseph Lister was a student at University College London under Robert Liston, later rising to the rank of Surgeon at Glasgow Royal Infirmary. Lister experimented with cloths covered in carbolic acid after studying the works and experiments of his contemporary, Louis Pasteur in sterilizing various biological media. Lister was inspired to try to find a way to sterilize living wounds, which could not be done with the heat required by Pasteur's experiments. In examining Pasteur's research, Lister began to piece together his theory: that patients were being killed by germs. He theorized that if germs could be killed or prevented, no infection would occur. Lister reasoned that a chemical could be used to destroy the micro-organisms that cause infection.^[47]

Meanwhile, in Carlisle, England, officials were experimenting with sewage treatment using carbolic acid to reduce the smell of sewage cesspools. Having heard of these developments, and having himself previously experimented with other chemicals for antiseptic purposes without much success, Lister decided to try carbolic acid as a wound antiseptic. He had his first chance on August 12, 1865, when he received a patient: an eleven-year-old boy with a tibia bone fracture which pierced the skin of his lower leg. Ordinarily, amputation would be the only solution. However, Lister decided to try carbolic acid. After setting the bone and supporting the leg with splints, he soaked clean cotton towels in undiluted carbolic acid and applied them to the wound, covered with a layer of tin foil, leaving them for four days. When he checked the wound, Lister was pleasantly surprised to find no signs of infection, just redness near the edges of the wound from mild burning by the carbolic acid. Reapplying fresh bandages with diluted carbolic acid, the boy was able to walk home after about six weeks of treatment.^[48]

By 16 March 1867, when the first results of Lister's work were published in the Lancet, he had treated a total of eleven patients using his new antiseptic method. Of those, only one had died, and that was through a complication that was nothing to do with Lister's wound-dressing technique. Now, for the first time, patients with compound fractures were likely to leave the hospital with all their limbs intact

— Richard Hollingham, Blood and Guts: A History of Surgery, p. 62^[48]

Before antiseptic operations were introduced at the hospital, there were sixteen deaths in thirty-five surgical cases. Almost one in every two patients died. After antiseptic surgery was introduced in the summer of 1865, there were only six deaths in forty cases. The mortality rate had dropped from almost 50 per cent to around 15 per cent. It was a remarkable achievement

— Richard Hollingham, Blood and Guts: A History of Surgery, p. 63^[49]

Phenol was the main ingredient of the Carbolic Smoke Ball, an ineffective device marketed in London in the 19th century as protection against influenza and other ailments, and the subject of the famous law case Carlill v Carbolic Smoke Ball Company.

Second World War

The toxic effect of phenol on the central nervous system, discussed below, causes sudden collapse and loss of consciousness in both humans and animals; a state of cramping precedes these symptoms because of the motor activity controlled by the central nervous system.^[50] Injections of phenol were used as a means of individual execution by Nazi Germany during the Second World War.^[51] It was originally used by the Nazis in 1939 as part of the Aktion T4 euthanasia program.^[52] The Germans learned that extermination of smaller groups was more economical by injection of each victim with phenol. Phenol injections were given to thousands of people. Maximilian Kolbe was also killed with a phenol injection after surviving two weeks of dehydration and starvation in Auschwitz when he volunteered to die in place of a stranger. Approximately one gram is sufficient to cause death.^[53]

Occurrences

Phenol is a normal metabolic product, excreted in quantities up to 40 mg/L in human urine.^[50]

The temporal gland secretion of male elephants showed the presence of phenol and 4-methylphenol during musth.^[54][55]

It is also one of the chemical compounds found in castoreum. This compound is ingested from the plants the beaver eats.^[56]

Occurrence in whisky

Phenol is a measurable component in the aroma and taste of the distinctive Islay scotch whisky,^[57] generally ~30 ppm, but it can be over 160ppm in the malted barley used to produce whisky.^[58] This amount is different from and presumably higher than the amount in the distillate.^[57]

Biodegradation

Cryptanaerobacter phenolicus is a bacterium species that produces benzoate from phenol via 4-hydroxybenzoate.^[59] Rhodococcus phenolicus is a bacterium species able to degrade phenol as sole carbon source.^[60]

Toxicity

Phenol and its vapors are corrosive to the eyes, the skin, and the respiratory tract.^[61] Its corrosive effect on skin and mucous membranes is due to a protein-degenerating effect.^[50] Repeated or prolonged skin contact with phenol may cause dermatitis, or even second and third-degree burns.^[62] Inhalation of phenol vapor may cause lung edema.^[61] The substance may cause harmful effects on the central nervous system and heart, resulting in dysrhythmia, seizures, and coma.^[63] The kidneys may be affected as well. Long-term or repeated exposure of the substance may have harmful effects on the liver and kidneys.^[64] There is no evidence that phenol causes cancer in humans.^[65] Besides its hydrophobic effects, another mechanism for the toxicity of phenol may be the formation of phenoxyl radicals.^[66]

Since phenol is absorbed through the skin relatively quickly, systemic poisoning can occur in addition to the local caustic burns.^[50] Resorptive poisoning by a large quantity of phenol can occur even with only a small area of skin, rapidly leading to paralysis of the central nervous system and a severe drop in body temperature. The LD₅₀ for oral toxicity is less than 500 mg/kg for dogs, rabbits, or mice; the minimum lethal human dose was cited as 140 mg/kg.^[50] The Agency for Toxic Substances and Disease Registry (ATSDR), U.S. Department of Health and Human Services states the fatal dose for ingestion of phenol is from 1 to 32 g.^[67]

Chemical burns from skin exposures can be decontaminated by washing with polyethylene glycol,^[68] isopropyl alcohol,^[69] or perhaps even copious amounts of water.^[70] Removal of contaminated clothing is required, as well as immediate hospital treatment for large splashes. This is particularly important if the phenol is mixed with chloroform (a commonly used mixture in molecular biology for DNA and RNA purification). Phenol is also a reproductive toxin causing increased risk of miscarriage and low birth weight indicating retarded development in utero.^[71]

Phenols

Main article: Phenols

The word phenol is also used to refer to any compound that contains a six-membered aromatic ring, bonded directly to a hydroxyl group (-OH). Thus, phenols are a class of organic compounds of which the phenol discussed in this article is the simplest member.

See also

• Bamberger rearrangement
• Claisen rearrangement
• Cresol
• Fries rearrangement
• Polyphenol

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44. Auguste Laurent (1836) "Sur la chlorophénise et les acides chlorophénisique et chlorophénèsique," Annales de Chemie et de Physique, vol. 63, pp. 27–45, see p. 44: Je donne le nom de phène au radical fondamental des acides précédens (φαινω, j'éclaire), puisque la benzine se trouve dans le gaz de l'éclairage. (I give the name of "phène" (φαινω, I illuminate) to the fundamental radical of the preceding acid, because benzene is found in illuminating gas.)
45. Gerhardt, Charles (1843) "Recherches sur la salicine," Annales de Chimie et de Physique, series 3, 7: 215-229. Gerhardt coins the name "phénol" on page 221.
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External links

 

Look up phenol in Wiktionary, the free dictionary.

 

Wikiquote has quotations related to Phenol.

 

Wikisource has the text of the 1911 Encyclopædia Britannica article "Carbolic Acid".

• International Chemical Safety Card 0070
• Phenol Material Safety Data Sheet
• National Pollutant Inventory: Phenol Fact Sheet
• NIOSH Pocket Guide to Chemical Hazards
• CDC - Phenol - NIOSH Workplace Safety and Health Topic
• Arcane Radio Trivia outlines competing uses for Phenol circa 1915