Chemistry:Phenol

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Short description: Organic compound (C6H5OH)
Phenol
Phenol2.svg
Phenol-2.svg
Phenol-3D-balls.png
Phenol-3D-vdW.png
Phenol 2 grams.jpg
Names
Preferred IUPAC name
Phenol[1]
Systematic IUPAC name
Benzenol
Other names
  • Carbolic acid
  • Phenolic acid
  • Phenylic acid
  • Hydroxybenzene
  • Phenic acid
  • Phenyl alcohol
  • Phenyl hydroxide
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
DrugBank
KEGG
RTECS number
  • SJ3325000
UNII
Properties
C6H6O
Molar mass 94.113 g/mol
Appearance Transparent crystalline solid
Odor Sweet and tarry
Density 1.07 g/cm3
Melting point 40.5 °C (104.9 °F; 313.6 K)
Boiling point 181.7 °C (359.1 °F; 454.8 K)
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]
1.224 D
Pharmacology
1=ATC code }} C05BB05 (WHO) D08AE03 (WHO), N01BX03 (WHO), R02AA19 (WHO)
Hazards
Safety data sheet [1]
GHS pictograms GHS05: CorrosiveGHS06: ToxicGHS08: Health hazard[6]
GHS Signal word Danger
H301, H311, H314, H331, H341, H373[6]
P261, P280, P301+310, P305+351+338, P310[6]
NFPA 704 (fire diamond)
Flammability code 2: Must be moderately heated or exposed to relatively high ambient temperature before ignition can occur. Flash point between 38 and 93 °C (100 and 200 °F). E.g. diesel fuelHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no codeNFPA 704 four-colored diamond
2
3
0
Flash point 79 °C (174 °F; 352 K)
Explosive limits 1.8–8.6%[3]
Lethal dose or concentration (LD, LC):
  • 317 mg/kg (rat, oral)
  • 270 mg/kg (mouse, oral)[7]
  • 420 mg/kg (rabbit, oral)
  • 500 mg/kg (dog, oral)
  • 80 mg/kg (cat, oral)[7]
  • 19 ppm (mammal)
  • 81 ppm (rat)
  • 69 ppm (mouse)[7]
NIOSH (US health exposure limits):
PEL (Permissible)
 TWA 5 ppm (19 mg/m3) [skin][3]
REL (Recommended)
  • TWA 5 ppm (19 mg/m3)
  • C 15.6 ppm (60 mg/m3) [15-minute] [skin][3]
IDLH (Immediate danger)
 250 ppm[3]
Related compounds
Related compounds
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references
Tracking categories (test):

Phenol, or Benzenol, (also known as carbolic acid or phenolic acid) is an aromatic organic compound with the molecular formula C
6H
5OH.[5] It is a white crystalline solid that is volatile. The molecule consists of a phenyl group (–C
6H
5) bonded to a hydroxy group (–OH). Mildly acidic, it requires careful handling because it can cause chemical burns.[5]

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, explosives, Bakelite, nylon, detergents, herbicides such as phenoxy herbicides, and numerous pharmaceutical drugs.[9]

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. It is a combustible solid (NFPA rating = 2). When heated, phenol produces flammable vapors that are explosive at concentrations of 3 to 10% in air. Carbon dioxide or dry chemical extinguishers should be used to fight phenol fires.[5]

Acidity

Phenol is a weak acid (pH 6.6). In aqueous solution in the pH range ca. 8 - 12 it is in equilibrium with the phenolate anion C
6H
5O−
 (also called phenoxide or carbolate):[10]

[math]\ce{ C6H5OH <=> C6H5O- + H+ }[/math]
Resonance structures of the phenoxide anion

Phenol is more acidic than aliphatic alcohols. Its enhanced acidity is attributed to resonance stabilization of phenolate anion. In this way, the negative charge on oxygen is delocalized on to the ortho and para carbon atoms through the pi system.[11] 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 pKa of the enol of acetone in water is 10.9, making it only slightly less acidic than phenol (pKa 10.0).[5] Thus, the greater number of resonance structures available to phenoxide compared to acetone enolate seems to contribute little to its stabilization. However, the situation changes when solvation effects are excluded.

Hydrogen bonding

In carbon tetrachloride and in 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 compiled.[12] Phenol is classified as a hard acid.[13][14]

Tautomerism

Phenol-cyclohexadienone tautomerism

Phenol exhibits keto-enol tautomerism with its unstable keto tautomer cyclohexadienone, but the effect is nearly negligible. 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.[15] 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.[16] 4, 4' Substituted cyclohexadienone can undergo a dienone–phenol rearrangement in acid conditions and form stable 3,4‐disubstituted phenol.[17]

For substituted phenols, several factors can favor the keto tautomer: (a) additional hydroxy groups (see resorcinol) (b) annulation as in the formation of naphthols, and (c) deprotonation to give the phenolate.[18]

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".[19]

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 enhanced 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 is so strongly activated that bromination and chlorination lead readily to polysubstitution.[20] The reaction affords 2- and 4-substituted derivatives. The regiochemistry of halogenation changes in strongly acidic solutions where PhOH
2]+
 predominates. 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. Friedel Crafts alkylations of phenol and its derivatives often proceed without catalysts. Alkylating agents include alkyl halides, alkenes, and ketones. Thus, adamantyl-1-bromide, dicyclopentadiene), and cyclohexanones give respectively 4-adamantylphenol, a bis(2-hydroxyphenyl) derivative, and a 4-cyclohexylphenols. Alcohols and hydroperoxides alkylate phenols in the presence of solid acid catalysts (e.g. certain zeolite). Cresols and cumyl phenols can be produced in that way.[21]

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.

C
6H
5OH + NaOH → C
6H
5ONa + H
2O

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:

C
6H
5COCl + HOC
6H
5 → C
6H
5CO
2C
6H
5 + 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:[22]

C
6H
5OH + Zn → C
6H
6 + ZnO

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

C
6H
5OH + CH
2N
2 → C
6H
5OCH
3 + N
2

Phenol and its derivatives react with iron(III) chloride to give intensely colored solutions containing phenoxide complexes.

Production

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


== Production of Phenol from Benzene

The production of phenol from benzene involves several methods, two of which are notable for their efficiency and significance in the industry.

V2O5-Catalyzed One-Step Process

This method utilizes V2O5 as a catalyst in a one-step reaction converting benzene to phenol. The process involves the introduction of partial oxygen to benzene, resulting in the formation of phenol. This efficient approach has been widely employed in industrial settings.

Process Overview

[

    • Introduction:**

The conversion of benzene to phenol is a significant chemical transformation with various industrial applications. One of the methods employed for this conversion is the partial oxidation using V2O5 as a catalyst. This process involves introducing oxygen into the benzene molecule under controlled conditions to yield phenol.

    • Chemical Reaction:**

The chemical equation representing the partial oxidation of benzene to phenol using V2O5 is:

\[ \text{C6H6 + O2} \xrightarrow{\text{V2O5}} \text{C6H5OH (phenol) + H2O} \]

Here, benzene reacts with oxygen in the presence of vanadium pentoxide as a catalyst, leading to the formation of phenol and water. The use of V2O5 is crucial as it acts as a catalyst, facilitating the reaction without being consumed in the process.

    • Mechanism of V2O5 Catalysis:**

The detailed mechanism involves the interaction between benzene, oxygen, and V2O5. The V2O5 catalyst provides a surface for the adsorption of reactants, facilitating the breaking of C-H bonds in benzene and the incorporation of oxygen atoms into the benzene ring. This step is crucial for the formation of the hydroxyl group, resulting in the production of phenol.

    • Reaction Conditions:**

The success of the partial oxidation process relies heavily on controlling reaction conditions. Temperature and pressure are critical factors. Elevated temperatures are often employed to favor the reaction kinetics, but excessive heat can lead to undesired by-products. The pressure is maintained to ensure the presence of sufficient oxygen for the oxidation reaction.

    • Catalyst Regeneration:**

One notable advantage of using V2O5 as a catalyst is its ability to be regenerated. The catalyst may undergo changes in its oxidation state during the reaction, but it can be restored to its original state through a regeneration process. This characteristic contributes to the economic viability of the partial oxidation method.

    • By-Product Formation:**

While the primary objective is to obtain phenol, side reactions can occur, leading to the formation of by-products. These undesired compounds may include quinones, hydroquinone, and catechol. Optimization of reaction conditions and catalyst usage aims to minimize the formation of these by-products.

    • Industrial Applications:**

The benzene to phenol conversion using V2O5 partial oxidation has widespread industrial applications. Phenol is a key precursor in the production of plastics, pharmaceuticals, and various chemicals. The efficiency of this method contributes significantly to the overall production of phenol on an industrial scale.

    • Environmental Considerations:**

Environmental considerations are crucial in chemical processes. The choice of V2O5 as a catalyst aligns with the need for sustainable and environmentally friendly practices. The catalyst's ability to be regenerated reduces waste and contributes to the overall environmental impact of the process.

In conclusion, the partial oxidation of benzene to phenol using V2O5 as a catalyst is a complex yet essential process in the chemical industry. Understanding the detailed mechanism, optimizing reaction conditions, and considering the environmental implications are key aspects of the successful implementation of this conversion method.. ]

Significance

[ **Advantages of Benzene to Phenol Conversion using V2O5 Partial Oxidation:**

1. **High Selectivity:** The V2O5 partial oxidation process tends to exhibit high selectivity for the production of phenol. This means that, under optimized conditions, the majority of the benzene is converted into the desired product without significant formation of unwanted by-products.

2. **Catalyst Regeneration:** V2O5 can be regenerated, making it a cost-effective choice for industrial applications. The ability to reuse the catalyst enhances the overall economic feasibility of the process.

3. **Versatility:** This method provides versatility in terms of the range of conditions under which the reaction can occur. This flexibility allows for optimization based on factors such as temperature, pressure, and catalyst concentration.

4. **Industrial Scale Application:** The partial oxidation of benzene to phenol using V2O5 has been successfully implemented on an industrial scale. The robustness of the process makes it suitable for large-scale production, meeting the demands of various industries.

5. **Environmental Considerations:** Compared to some alternative methods, the V2O5 partial oxidation process can be considered environmentally friendly. The ability to regenerate the catalyst and control reaction conditions contributes to reducing overall waste and environmental impact.

    • Disadvantages of Benzene to Phenol Conversion using V2O5 Partial Oxidation:**

1. **By-Product Formation:** Despite efforts to optimize conditions, there is a tendency for the formation of by-products such as quinones, hydroquinone, and catechol. These by-products may require additional processing or separation steps, impacting the overall efficiency of the process.

2. **Energy Intensive:** The partial oxidation process often requires elevated temperatures, which can make it energy-intensive. Balancing the need for high temperatures for efficient reaction kinetics with energy efficiency is a challenge in the implementation of this method.

3. **Catalyst Deactivation:** Although V2O5 is known for its regenerability, prolonged use may lead to catalyst deactivation. This can necessitate more frequent regeneration or replacement, affecting the overall cost-effectiveness of the process.

4. **Process Complexity:** The partial oxidation process is complex, involving multiple steps and factors that need careful control. Maintaining optimal conditions for the reaction can be challenging, especially at an industrial scale, requiring sophisticated engineering and control systems.

5. **Raw Material Dependency:** The process is dependent on the availability and cost of raw materials, including benzene and oxygen. Fluctuations in the prices of these materials can impact the overall economic viability of the process.

In summary, while the partial oxidation of benzene to phenol using V2O5 as a catalyst offers several advantages, such as high selectivity and catalyst regenerability, it is not without challenges. Managing by-products, energy consumption, catalyst deactivation, and process complexity are aspects that require careful consideration in the industrial implementation of this conversion method ]

Dow Process for Direct Phenol Production

The Dow process stands as a prominent method for the direct production of phenol from benzene. This method has gained widespread adoption for its efficiency and direct synthesis of phenol.

Process Description

[Describe the Dow process, outlining the key steps involved in the direct production of phenol from benzene.]

Industrial Application

[The process involves preparing benzene and oxygen, using V2O5 as a catalyst, and subjecting them to controlled conditions, resulting in the partial oxidation of benzene to phenol. Key steps include catalyst activation, managing by-products, and catalyst regeneration. The process is chosen for its high selectivity, catalyst regenerability, and applications in various industries. Challenges include by-product formation and the need for careful process optimization..]

References

1. [. https://en.m.wikipedia.org/wiki/Dow_proces ]


See Also

  • [Link to Related Topic 1]
  • [Link to Related Topic 2]

External Links And cummene process


Cumene process

The Hock process leading to phenol via autoxidation of cumene.

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 mild conditions and inexpensive raw materials. For the process to be economical, both phenol and the acetone by-product must be in demand.[23][24] 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.[25]

Oxidation of benzene, toluene, cyclohexylbenzene

The direct oxidation of benzene (C
6H
6) to phenol is theoretically possible and of great interest, but it has not been commercialized:

C
6H
6 + O → C
6H
5OH

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.[26][23][25]

An electrosynthesis employing alternating current gives phenol from benzene.[27]

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

C
6H
5CH
3 + 2 O
2 → C
6H
5OH + CO
2 + H
2O

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:[28]

C
6H
5SO
3H + 2 NaOH → C
6H
5OH + Na
2SO
3 + H
2O

Hydrolysis of chlorobenzene

Chlorobenzene can be hydrolyzed to phenol using base (Dow process) or steam (Raschig–Hooker process):[24][25][29]

C
6H
5Cl + NaOH → C
6H
5OH + NaCl
C
6H
5Cl + H
2O → C
6H
5OH + 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.[29] In the Lummus Process, the oxidation of toluene to benzoic acid is conducted separately.

Miscellaneous methods

Amine to phenol[30]

Phenyldiazonium salts hydrolyze to phenol. The method is of no commercial interest since the precursor is expensive.[30]

C
6H
5NH
2 + HCl + NaNO
2 → C
6H
5OH + N
2 + H
2O + NaCl
Übersichtsreaktion der Phenolverkochung.svg

Salicylic acid decarboxylates to phenol.[31]

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,[32] 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 was 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 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 phenol 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 also 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]

Due to safety concerns, phenol is banned from use in cosmetic products in the European Union[36][37] and Canada .[38][39]

History

Phenol was discovered in 1834 by Friedlieb Ferdinand Runge, who extracted it (in impure form) from coal tar.[40] 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.[41]

In 1836, Auguste Laurent coined the name "phène" for benzene;[42] this is the root of the word "phenol" and "phenyl". In 1843, French chemist Charles Gerhardt coined the name "phénol".[43]

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[44] 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. Lister's work was inspired by the works and experiments of his contemporary, Louis Pasteur in sterilizing various biological media. 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.[45]

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.[46]

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[46]

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[47]

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.[48] Injections of phenol were used as a means of individual execution by Nazi Germany during the Second World War.[49] It was originally used by the Nazis in 1939 as part of the mass-murder of undesirables under Aktion T4.[50] 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 murdered 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.[51]

Occurrences

Phenol is a normal metabolic product, excreted in quantities up to 40 mg/L in human urine.[48]

The temporal gland secretion of male elephants showed the presence of phenol and 4-methylphenol during musth.[52][53]

It is also one of the chemical compounds found in castoreum. This compound is ingested from the plants the beaver eats.[54]

Occurrence in whisky

Phenol is a measurable component in the aroma and taste of the distinctive Islay scotch whisky,[55] generally ~30 ppm, but it can be over 160ppm in the malted barley used to produce whisky.[56] This amount is different from and presumably higher than the amount in the distillate.[55]

Biodegradation

Cryptanaerobacter phenolicus is a bacterium species that produces benzoate from phenol via 4-hydroxybenzoate.[57] Rhodococcus phenolicus is a bacterium species able to degrade phenol as sole carbon source.[58]

Toxicity

Phenol and its vapors are corrosive to the eyes, the skin, and the respiratory tract.[59] Its corrosive effect on skin and mucous membranes is due to a protein-degenerating effect.[48] Repeated or prolonged skin contact with phenol may cause dermatitis, or even second and third-degree burns.[60] Inhalation of phenol vapor may cause lung edema.[59] The substance may cause harmful effects on the central nervous system and heart, resulting in dysrhythmia, seizures, and coma.[61] The kidneys may be affected as well. Long-term or repeated exposure of the substance may have harmful effects on the liver and kidneys.[62] There is no evidence that phenol causes cancer in humans.[63] Besides its hydrophobic effects, another mechanism for the toxicity of phenol may be the formation of phenoxyl radicals.[64]

Since phenol is absorbed through the skin relatively quickly, systemic poisoning can occur in addition to the local caustic burns.[48] 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 -1">50 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.[48] 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.[65]

Chemical burns from skin exposures can be decontaminated by washing with polyethylene glycol,[66] isopropyl alcohol,[67] or perhaps even copious amounts of water.[68] 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).[citation needed] Phenol is also a reproductive toxin causing increased risk of miscarriage and low birth weight indicating retarded development in utero.[5]

Phenols

Main page: Chemistry: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

References

  1. ↑ "Front Matter". Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. p. 690. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4. "Only one name is retained, phenol, for C6H5-OH, both as a preferred name and for general nomenclature." 
  2. ↑ "Phenol_msds". https://www.chemsrc.com/en/cas/108-95-2_1101388.html. 
  3. ↑ 3.0 3.1 3.2 3.3 3.4 NIOSH Pocket Guide to Chemical Hazards. "#0493". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0493.html. 
  4. ↑ Kütt, Agnes; Movchun, Valeria; Rodima, Toomas et al. (2008). "Pentakis(trifluoromethyl)phenyl, a Sterically Crowded and Electron-withdrawing Group: Synthesis and Acidity of Pentakis(trifluoromethyl)benzene, -toluene, -phenol, and -aniline". The Journal of Organic Chemistry 73 (7): 2607–20. doi:10.1021/jo702513w. PMID 18324831. 
  5. ↑ 5.0 5.1 5.2 5.3 5.4 5.5 "Phenol". PubChem, US National Library of Medicine. 10 June 2023. https://pubchem.ncbi.nlm.nih.gov/compound/996. 
  6. ↑ 6.0 6.1 6.2 Sigma-Aldrich Co., Phenol. Retrieved on 2022-02-15.
  7. ↑ 7.0 7.1 7.2 "Phenol". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/108952.html. 
  8. ↑ 8.0 8.1 8.2 8.3 8.4 Weber, Manfred; Weber, Markus; Kleine-Boymann, Michael (2004). "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a19_299.pub3. 
  9. ↑ Zvi Rappoport, ed (2003). The Chemistry of Phenols. PATAI'S Chemistry of Functional Groups. John Wiley & Sons. doi:10.1002/0470857277. ISBN 9780470857274. 
  10. ↑ Smith, Michael B.; March, Jerry (2007), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (6th ed.), New York: Wiley-Interscience, ISBN 978-0-471-72091-1, https://books.google.com/books?id=JDR-nZpojeEC&printsec=frontcover 
  11. ↑ Organic Chemistry 2nd Ed. John McMurry ISBN:0-534-07968-7
  12. ↑ Drago, R S. Physical Methods For Chemists, (Saunders College Publishing 1992), ISBN 0-03-075176-4
  13. ↑ Laurence, C. and Gal, J-F. Lewis Basicity and Affinity Scales, Data and Measurement, (Wiley 2010) pp 50-51 ISBN 978-0-470-74957-9
  14. ↑ Cramer, R. E.; Bopp, T. T. (1977). "Graphical display of the enthalpies of adduct formation for Lewis acids and bases". Journal of Chemical Education 54: 612–613. doi:10.1021/ed054p612.  The plots shown in this paper used older parameters. Improved E&C parameters are listed in ECW model.
  15. ↑ Capponi, Marco; Gut, Ivo G.; Hellrung, Bruno; Persy, Gaby; Wirz, Jakob (1999). "Ketonization equilibria of phenol in aqueous solution". Can. J. Chem. 77 (5–6): 605–613. doi:10.1139/cjc-77-5-6-605. 
  16. ↑ Clayden, Jonathan; Greeves, Nick; Warren, Stuart; Wothers, Peter (2001). Organic Chemistry (1st ed.). Oxford University Press. p. 531. ISBN 978-0-19-850346-0. 
  17. ↑ Arnold, Richard T.; Buckley, Jay S. (1 May 1949). "The Dienone-Phenol Rearrangement. II. Rearrangement of 1-Keto-4-methyl-4-phenyl-1,4-dihydronaphthalene". J. Am. Chem. Soc. 71 (5): 1781. doi:10.1021/ja01173a071. 
  18. ↑ Sergei M. Lukyanov, Alla V. Koblik (2003). "Tautomeric Equilibria and Rearrangements Involving Phenols". in Zvi Rappoport. The Chemistry of Phenols. PATAI'S Chemistry of Functional Groups. John Wiley & Sons. pp. 713–838. doi:10.1002/0470857277.ch11. ISBN 0471497371. 
  19. ↑ David Y. Curtin; Allan R. Stein (1966). "2,6,6-Trimethyl-2,4-Cyclohexadione". Organic Syntheses 46: 115. doi:10.15227/orgsyn.046.0115. http://www.orgsyn.org/orgsyn/prep.asp?prep=cv5p1092. Retrieved 2010-03-31. 
  20. ↑ "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. 2011. doi:10.1002/14356007.a07_001.pub2. 
  21. ↑ V. Prakash Reddy. G. K. Surya Prakash (2003). "Electrophilic reactions of phenols". in Zvi Rappoport. The Chemistry of Phenols. PATAI'S Chemistry of Functional Groups. John Wiley & Sons. pp. 605–660. doi:10.1002/0470857277.ch9. ISBN 0471497371. 
  22. ↑ Roscoe, Henry (1891). A treatise on chemistry, Volume 3, Part 3. London: Macmillan & Co.. pp. 23. https://books.google.com/books?id=HEY9AAAAYAAJ&q=zinc&pg=PA199. 
  23. ↑ 23.0 23.1 "Phenol -- The essential chemical industry online". 2017-01-11. http://www.essentialchemicalindustry.org/chemicals/phenol.html. 
  24. ↑ 24.0 24.1 "Direct Routes to Phenol". http://www.chemistry.org/portal/a/c/s/1/feature_pro.html?id=c373e908e6e847ac8f6a17245d830100. 
  25. ↑ 25.0 25.1 25.2 Plotkin, Jeffrey S. (2016-03-21). "What's New in Phenol Production?". American Chemical Society. https://www.acs.org/content/acs/en/pressroom/cutting-edge-chemistry/what-s-new-in-phenol-production-.html. 
  26. ↑ Parmon, V. N.; Panov, G. I.; Uriarte, A.; Noskov, A. S. (2005). "Nitrous oxide in oxidation chemistry and catalysis application and production". Catalysis Today 100 (2005): 115–131. doi:10.1016/j.cattod.2004.12.012. 
  27. ↑ Lee, Byungik; Naito, Hiroto; Nagao, Masahiro; Hibino, Takashi (9 July 2012). "Alternating-Current Electrolysis for the Production of Phenol from Benzene". Angewandte Chemie International Edition 51 (28): 6961–6965. doi:10.1002/anie.201202159. PMID 22684819. 
  28. ↑ Wittcoff, H.A., Reuben, B.G. Industrial Organic Chemicals in Perspective. Part One: Raw Materials and Manufacture. Wiley-Interscience, New York. 1980.
  29. ↑ 29.0 29.1 Franck, H.-G., Stadelhofer, J.W. Industrial Aromatic Chemistry. Springer-Verlag, New York. 1988. pp. 148-155.
  30. ↑ 30.0 30.1 Kazem-Rostami, Masoud (2017). "Amine to phenol conversion". Synlett 28 (13): 1641–1645. doi:10.1055/s-0036-1588180. 
  31. ↑ Kaeding, Warren W. (1 September 1964). "Oxidation of Aromatic Acids. IV. Decarboxylation of Salicylic Acids". The Journal of Organic Chemistry 29 (9): 2556–2559. doi:10.1021/jo01032a016. 
  32. ↑ Musser, Michael T.. "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a08_217.pub2. 
  33. ↑ "Phenol spray". drugs.com. https://www.drugs.com/cdi/phenol-spray.html. 
  34. ↑ "How Does Our Lip Balm Work". Carmex. https://mycarmex.com/works. 
  35. ↑ "CH207 Aircraft paintstripper, phenolic, acid". Callington. 14 October 2009. https://www.callingtonhaven.com/_assets/paint_strippers/ch207.pdf. 
  36. ↑ "Prohibited substances in cosmetic product (Annex II, #1175, Phenol) - European Commission" (in en). http://ec.europa.eu/growth/tools-databases/cosing/index.cfm?fuseaction=search.results. 
  37. ↑ "CosIng - Cosmetics - GROWTH - European Commission" (in en). http://ec.europa.eu/growth/tools-databases/cosing/index.cfm?fuseaction=search.details_v2&id=29394. 
  38. ↑ Canada, Health (2004-06-18). "Cosmetic Ingredient Hotlist - Canada.ca" (in en). https://www.canada.ca/en/health-canada/services/consumer-product-safety/cosmetics/cosmetic-ingredient-hotlist-prohibited-restricted-ingredients/hotlist.html#t1p. 
  39. ↑ Canada, Health (2004-06-18). "Cosmetic Ingredient Hotlist: Prohibited and Restricted Ingredients - Canada.ca" (in en). https://www.canada.ca/en/health-canada/services/consumer-product-safety/cosmetics/cosmetic-ingredient-hotlist-prohibited-restricted-ingredients.html. 
  40. ↑ 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.
  41. ↑ 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".
  42. ↑ 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.)
  43. ↑ 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.
  44. ↑ Lister, Joseph (1867). "Antiseptic Principle Of The Practice Of Surgery". https://sourcebooks.fordham.edu/mod/1867lister.asp. 
  45. ↑ Hollingham, Richard (2008). Blood and Guts: A History of Surgery. BBC Books - Random House. p. 61. ISBN 9781407024530. 
  46. ↑ 46.0 46.1 Hollingham, Richard (2008). Blood and Guts: A History of Surgery. BBC Books - Random House. p. 62. ISBN 9781407024530. 
  47. ↑ Hollingham, Richard (2008). Blood and Guts: A History of Surgery. BBC Books - Randomhouse. p. 63. ISBN 9781407024530. 
  48. ↑ 48.0 48.1 48.2 48.3 48.4 "Ullmann's Encyclopedia of Industrial Chemistry". Ullmann's Encyclopedia of Industrial Chemistry. 25. Wiley-VCH. 2003. pp. 589–604. 
  49. ↑ The Experiments by Peter Tyson. NOVA
  50. ↑ The Nazi Doctors , Chapter 14, Killing with Syringes: Phenol Injections. By Dr. Robert Jay Lifton
  51. ↑ "Killing through phenol injection". Auschwitz: Final Station Extermination. Linz, Austria: Johannes Kepler University. http://www.wsg-hist.uni-linz.ac.at/AUSCHWITZ/HTML/Phenol.html. 
  52. ↑ Rasmussen, L.E.L; Perrin, Thomas E (1999). "Physiological Correlates of Musth". Physiology & Behavior 67 (4): 539–49. doi:10.1016/S0031-9384(99)00114-6. PMID 10549891. 
  53. ↑ Musth in elephants. Deepa Ananth, Zoo's print journal, 15(5), pages 259-262 (article)
  54. ↑ The Beaver: Its Life and Impact. Dietland Muller-Schwarze, 2003, page 43 (book at google books)
  55. ↑ 55.0 55.1 "Peat, Phenol and PPM, by Dr P. Brossard". http://www.whisky-news.com/En/reports/Peat_phenol_ppm.pdf. 
  56. ↑ "Bruichladdich". BDCL. http://www.bruichladdich.com/the-whisky/octomore. 
  57. ↑ Juteau, P.; Côté, V; Duckett, MF; Beaudet, R; Lépine, F; Villemur, R; Bisaillon, JG (2005). "Cryptanaerobacter phenolicus gen. nov., sp. nov., an anaerobe that transforms phenol into benzoate via 4-hydroxybenzoate". International Journal of Systematic and Evolutionary Microbiology 55 (Pt 1): 245–50. doi:10.1099/ijs.0.02914-0. PMID 15653882. 
  58. ↑ 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. PMID 16261859. 
  59. ↑ 59.0 59.1 Budavari, S, ed (1996). The Merck Index: An Encyclopedia of Chemical, Drugs, and Biologicals. Whitehouse Station, NJ: Merck. 
  60. ↑ "Phenol burn". Burns: Journal of the International Society for Burn Injuries 32 (4): 517–21. June 2006. doi:10.1016/j.burns.2005.12.016. PMID 16621299. 
  61. ↑ Warner, MA; Harper, JV (1985). "Cardiac dysrhythmias associated with chemical peeling with phenol". Anesthesiology 62 (3): 366–7. doi:10.1097/00000542-198503000-00030. PMID 2579602. 
  62. ↑ World Health Organization/International Labour Organization: International Chemical Safety Cards, http://www.inchem.org/documents/icsc/icsc/eics0070.htm
  63. ↑ U.S. Department of Health and Human Services. "How can phenol affect my health?". Toxicological Profile for Phenol: 24. https://www.atsdr.cdc.gov/toxprofiles/tp115.pdf. 
  64. ↑ Hanscha, Corwin; McKarns, Susan C; Smith, Carr J; Doolittle, David J (June 15, 2000). "Comparative QSAR evidence for a free-radical mechanism of phenol-induced toxicity". Chemico-Biological Interactions 127 (1): 61–72. doi:10.1016/S0009-2797(00)00171-X. PMID 10903419. 
  65. ↑ "Medical Management Guidelines for Phenol (C6H6O)". U.S. Department of Health and Human Services. October 21, 2014. https://www.atsdr.cdc.gov/MMG/MMG.asp?id=144&tid=27. 
  66. ↑ Brown, VKH; Box, VL; Simpson, BJ (1975). "Decontamination procedures for skin exposed to phenolic substances". Archives of Environmental Health 30 (1): 1–6. doi:10.1080/00039896.1975.10666623. PMID 1109265. 
  67. ↑ Hunter, DM; Timerding, BL; Leonard, RB; McCalmont, TH; Schwartz, E (1992). "Effects of isopropyl alcohol, ethanol, and polyethylene glycol/industrial methylated spirits in the treatment of acute phenol burns". Annals of Emergency Medicine 21 (11): 1303–7. doi:10.1016/S0196-0644(05)81891-8. PMID 1416322. 
  68. ↑ Pullin, TG; Pinkerton, MN; Johnston, RV; Kilian, DJ (1978). "Decontamination of the skin of swine following phenol exposure: a comparison of the relative efficacy of water versus polyethylene glycol/industrial methylated spirits". Toxicol Appl Pharmacol 43 (1): 199–206. doi:10.1016/S0041-008X(78)80044-1. PMID 625760. 

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