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Phenol is an aromaticorganic compound with the molecular formula C₆H₅OH. It is a white crystallinesolid that is volatile. The molecule consists of a phenyl group (−C₆H₅) bonded to a hydroxy group (−OH). It is mildly acidic and requires careful handling due to its propensity for causing chemical burns.

Phenol was first extracted from coal tar, but today is produced on a large scale (about 7 billion kg/year) from petroleum. 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.

• 1Properties
  • 1.1Acidity
• 3Uses
• 4History
• 5Occurrences

Properties[edit]

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[edit]

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

C₆H₅OH ⇌ C₆H₅O^- + H⁺

One explanation for why phenol is more acidic than aliphatic compounds containing an -OH group is resonance stabilization of the phenoxide anion by the aromatic ring. 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]

Phenoxide anion[edit]

The phenoxide anion has a similar nucleophilicity to free amines, with the further advantage that its conjugate acid (neutral phenol) does not become entirely deactivated as a nucleophile even in moderately acidic conditions. Phenolate esters are more stable toward hydrolysis than acid anhydrides and acyl halides but are sufficiently reactive under mild conditions to facilitate the formation of amide bonds.

Tautomerism[edit]

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.^[13] 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.^[14]

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'.^[15]

Reactions[edit]

Phenol is highly reactive toward electrophilic aromatic substitution as the oxygen atom's pi electrons donate electron density into the ring. By this general approach, many groups can be appended to the ring, via halogenation, acylation, sulfonation, and other processes. However, phenol's ring is so strongly activated—second only to aniline—that bromination or chlorination of phenol leads to substitution on all carbon atoms ortho and para to the hydroxy group, not only on one carbon. Phenol reacts with dilute nitric acid at room temperature to give a mixture of 2-nitrophenol and 4-nitrophenol while with concentrated nitric acid, more nitro groups get substituted on the ring to give 2,4,6-trinitrophenol which is known as picric acid.

Aqueous solutions of phenol are weakly acidic and turn blue litmus slightly to red. Phenol is easily 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.

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:

C₆H₅OH + C₆H₅COCl → C₆H₅OCOC₆H₅ + HCl

Phenol is reduced to benzene when it is distilled with zinc dust, or when phenol vapour is passed over granules of zinc at 400 °C:^[16]

C₆H₅OH + Zn → C₆H₆ + ZnO

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

C₆H₅OH + CH₂N₂ → C₆H₅OCH₃ + N₂

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

Production[edit]

Because of phenol's commercial importance, many methods have been developed for its production. The dominant current route, accounting for 95% of production (2003), is the cumene process, which uses benzene and propene as feedstock and involves the partial oxidation of cumene (isopropylbenzene) via the Hock rearrangement:^[8]

Acetone is produced as a by-product. Compared to most other processes, the cumene process uses relatively mild synthesis conditions, and relatively inexpensive raw materials. However, to operate economically, there must be demand for both phenol, and the acetone by-product.^[17][18] 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.

ExxonMobil developed a process in which benzene is hydroalkylated to cyclohexylbenzene. This latter product is oxidized to a hydroperoxide and then cleaved to phenol and cyclohexanone. Cyclohexanone is an important reaction intermediate for making nylon.^[19] Therefore, this newer process without producing the acetone by-product appears attractive and is similar to the Cumene process as a hydroperoxide is formed and then decomposed to yield two key products.^[17]

An early commercial route, developed by Bayer and Monsanto in the early 1900s, begins with the reaction of a strong base with benzenesulfonate:^[20]

C₆H₅SO₃H + 2 NaOH → C₆H₅OH + Na₂SO₃ + H₂O

Other methods of production and preparation under consideration involve:^[18][19]

• hydrolysis of chlorobenzene, using base (Dow process) or steam (Raschig–Hooker process):^[19][21]

C₆H₅Cl + H₂O → C₆H₅OH + HCl

• direct oxidation of benzene with nitrous oxide,^[22] a potentially 'green' process:^[17][19]

C₆H₆ + N₂O → C₆H₅OH + N₂

• oxidation of toluene, as developed by Dow Chemical:

C₆H₅CH₃ + 2 O₂ → C₆H₅OH + CO₂ + H₂O

• Phenol is also a recoverable byproduct of coal pyrolysis.^[21]
• In the Lummus Process, the oxidation of toluene to benzoic acid is conducted separately.

• In the thermal decomposition of aryldiazonium salts, the salts are converted to phenol.^[23]

C₆H₅NH₂ + HCl/NaNO₂ → C₆H₅OH + N₂ + H₂O + NaCl

• An electrosynthesis employing alternating current prepares phenol at both the cathode and the anode.^[24]

Uses[edit]

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/liquidphenol–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[edit]

Phenol was once widely used as an antiseptic, its use pioneered by Joseph Lister (see History section).

From the early 1900s to the 1970s it was used as a soap, known as 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. Phenol is also used as a preservative in some vaccines.^[25]

Phenol spray is used medically to help sore throat.^[26] It is the active ingredient in some oral analgesics such as Chloraseptic spray, TCP and Carmex, commonly used to temporarily treat pharyngitis.^[27]

Niche uses[edit]

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.^[28]

Phenol derivatives have been used in the preparation of cosmetics including sunscreens,^[29]hair colorings, skin lightening preparations^[30], as well as in skin toners/exfoliators.^[31] However, due to safety concerns, phenol is banned from use in cosmetic products in the European Union^[32][33] and Canada.^[34][35]

History[edit]

Applied Pharmaceutics In Contemporary Compounding Free Download 2017

Phenol was discovered in 1834 by Friedlieb Ferdinand Runge, who extracted it (in impure form) from coal tar.^[36] Runge called phenol 'Karbolsäure' (coal-oil-acid, carbolic acid). Coal tar remained the primary source until the development of the petrochemical industry. In 1841, the French chemist Auguste Laurent obtained phenol in pure form.^[37]

In 1836, Auguste Laurent coined the name 'phène' for benzene;^[38] this is the root of the word 'phenol' and 'phenyl'. In 1843, French chemist Charles Gerhardt coined the name 'phénol'.^[39]

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^[40] covered in phenol, or carbolic acid as he called it. 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.^[41]

Meanwhile, in Carlisle, England, officials were experimenting with a sewage treatment, using carbolic acid to reduce the smell of sewage cess pools. 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, Lister 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.^[42]

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^[42]

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^[43]

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[edit]

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.^[44] Injections of phenol were used as a means of individual execution by Germany during the Second World War.^[45] It was originally used by the Germans in 1939 as part of Aktion T4.^[46] 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.^[47]

Occurrences[edit]

Phenol is a normal metabolic product, excreted in quantities up to 40 mg/L in human urine.^[44]

The temporal gland secretion of male elephants showed the presence of phenol and 4-methylphenol during musth.^[48][49]

It is also one of the chemical compounds found in castoreum. This compound is ingested from the plants the beaver eats.^[50]

Occurrence in whisky[edit]

Phenol is a measurable component in the aroma and taste of the distinctive Islay scotch whisky,^[51] generally ~30 ppm, but it can be over 160ppm in the malted barley used to produce whisky.^[52] This amount is different from and presumably higher than the amount in the distillate.^[51]

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Biodegradation[edit]

Cryptanaerobacter phenolicus is a bacterium species that produces benzoate from phenol via 4-hydroxybenzoate.^[53]Rhodococcus phenolicus is a bacterium species able to degrade phenol as sole carbon sources.^[54]

Toxicity[edit]

Phenol and its vapors are corrosive to the eyes, the skin, and the respiratory tract.^[55] Its corrosive effect on skin and mucous membranes is due to a protein-degenerating effect.^[44] Repeated or prolonged skin contact with phenol may cause dermatitis, or even second and third-degree burns.^[56] Inhalation of phenol vapor may cause lung edema.^[55] The substance may cause harmful effects on the central nervous system and heart, resulting in dysrhythmia, seizures, and coma.^[57] The kidneys may be affected as well. Long-term or repeated exposure of the substance may have harmful effects on the liver and kidneys.^[58] There is no evidence that phenol causes cancer in humans.^[59] Besides its hydrophobic effects, another mechanism for the toxicity of phenol may be the formation of phenoxylradicals.^[60]

Since phenol is absorbed through the skin relatively quickly, systemic poisoning can occur in addition to the local caustic burns.^[44] 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.^[44] 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.^[61]

Chemical burns from skin exposures can be decontaminated by washing with polyethylene glycol,^[62]isopropyl alcohol,^[63] or perhaps even copious amounts of water.^[64] 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 abortion and low birth weight indicating retarded development in utero.^[65]

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Phenols[edit]

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[edit]

References[edit]

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2. ^'Phenol_msds'.
3. ^ ^abcdeNIOSH Pocket Guide to Chemical Hazards. '#0493'. National Institute for Occupational Safety and Health (NIOSH).
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36. ^F. F. Runge (1834) 'Ueber einige Produkte der Steinkohlendestillation' (On some products of coal distillation), Annalen der Physik und Chemie, 31 : 65-78. On page 69 of volume 31, Runge names phenol 'Karbolsäure' (coal-oil-acid, carbolic acid). Runge characterizes phenol in: F. F. Runge (1834) 'Ueber einige Produkte der Steinkohlendestillation,'Annalen der Physik und Chemie, 31 : 308-328.
37. ^Auguste Laurent (1841) 'Mémoire sur le phényle et ses dérivés' (Memoir on benzene and its derivatives), Annales de Chimie et de Physique, series 3, 3 : 195-228. On page 198, Laurent names phenol 'hydrate de phényle' and 'l'acide phénique'.
38. ^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.)
39. ^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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54. ^Rehfuss, Marc; Urban, James (2005). 'Rhodococcus phenolicus sp. nov., a novel bioprocessor isolated actinomycete with the ability to degrade chlorobenzene, dichlorobenzene and phenol as sole carbon sources'. Systematic and Applied Microbiology. 28 (8): 695–701. doi:10.1016/j.syapm.2005.05.011. PMID16261859.
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57. ^Warner, MA; Harper, JV (1985). 'Cardiac dysrhythmias associated with chemical peeling with phenol'. Anesthesiology. 62 (3): 366–7. doi:10.1097/00000542-198503000-00030. PMID2579602.
58. ^World Health Organization/International Labour Organization:International Chemical Safety Cards, http://www.inchem.org/documents/icsc/icsc/eics0070.htm
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61. ^'Medical Management Guidelines for Phenol (C6H6O)'. Agency for Toxic Substances and Disease Registry. U.S. Department of Health and Human Services. October 21, 2014. Retrieved 8 August 2015.
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