phenol

—phenolic /fi noh"lik, -nol"ik/, adj.

/fee"nawl, -nol/, n. Chem.

1. Also called carbolic acid, hydroxybenzene, oxybenzene, phenylic acid. a white, crystalline, water-soluble, poisonous mass, C₆H₅OH, obtained from coal tar, or a hydroxyl derivative of benzene: used chiefly as a disinfectant, as an antiseptic, and in organic synthesis.

2. any analogous hydroxyl derivative of benzene.

[1850-55; PHEN- + -OL¹]

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Any of a class of organic compounds with a hydroxyl group (-OH; see functional group) attached to a carbon atom in a ring of an aromatic compound.

The simplest one, carbolic acid (C₆H₅OH), is also called phenol; its most important reaction is with formaldehyde, with which it forms widely used polymers called phenol-formaldehyde (phenolic) resins. Phenols are similar to alcohols but form stronger hydrogen bonds (see bonding), so they dissolve more readily in water and boil at higher temperatures. They may be colourless liquids or white solids; many have a sharp, spicy odour. Some are found in essential oils. Phenols with higher molecular weights and phenol derivatives have supplanted phenol itself as industrial antiseptics (germicidal cleaners). See also Leo Baekeland.

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▪ chemical compound

Introduction

 any of a family of organic compounds (organic compound) characterized by a hydroxyl (−OH) group attached to a carbon atom that is part of an aromatic ring. Besides serving as the generic name for the entire family, the term phenol is also the specific name for its simplest member, monohydroxybenzene (C₆H₅OH), also known as benzenol, or carbolic acid.

      Phenols are similar to alcohols (alcohol) but form stronger hydrogen bonds. Thus, they are more soluble in water than are alcohols and have higher boiling points (boiling point). Phenols occur either as colourless liquids (liquid) or white solids (solid) at room temperature and may be highly toxic and caustic.

      Phenols are widely used in household products and as intermediates for industrial synthesis. For example, phenol itself is used (in low concentrations) as a disinfectant in household cleaners and in mouthwash. Phenol may have been the first surgical antiseptic. In 1865 the British surgeon Joseph Lister (Lister, Joseph, Baron Lister, Of Lyme Regis) used phenol as an antiseptic to sterilize his operating field. With phenol used in this manner, the mortality rate from surgical amputations fell from 45 to 15 percent in Lister's ward. Phenol is quite toxic, however, and concentrated solutions cause severe but painless burns of the skin and mucous membranes. Less-toxic phenols, such as n-hexylresorcinol, have supplanted phenol itself in cough drops and other antiseptic applications. Butylated hydroxytoluene (BHT) has a much lower toxicity and is a common antioxidant in foods.

      In industry, phenol is used as a starting material to make plastics (plastic), explosives (explosive) such as picric acid, and drugs (drug) such as aspirin. The common phenol hydroquinone is the component of photographic developer that reduces exposed silver bromide crystals to black metallic silver. Other substituted phenols are used in the dye industry to make intensely coloured azo dyes (azo dye). Mixtures of phenols (especially the cresols (cresol)) are used as components in wood preservatives such as creosote.

Natural sources of phenols

 Phenols are common in nature; examples include tyrosine, one of the standard amino acids (amino acid) found in most proteins (protein); epinephrine (epinephrine and norepinephrine) (adrenaline), a stimulant hormone produced by the adrenal medulla; serotonin, a neurotransmitter in the brain; and urushiol, an irritant secreted by poison ivy to prevent animals from eating its leaves. Many of the more complex phenols used as flavourings and aromas are obtained from essential oils (essential oil) of plants. For example, vanillin, the principal flavouring in vanilla, is isolated from vanilla beans, and methyl salicylate, which has a characteristic minty taste and odour, is isolated from wintergreen. Other phenols obtained from plants include thymol, isolated from thyme, and eugenol, isolated from cloves (clove).

      Phenol, the cresols (cresol) (methylphenols), and other simple alkylated phenols can be obtained from the distillation of coal tar or crude petroleum.

Nomenclature of phenols

      Many phenolic compounds were discovered and used long before chemists were able to determine their structures. Therefore, trivial names (i.e., vanillin, salicylic acid, pyrocatechol, resorcinol, cresol, hydroquinone, and eugenol) are often used for the most common phenolic compounds.

      Systematic names are more useful, however, because a systematic name specifies the actual structure of the compound. If the hydroxyl group is the principal functional group of a phenol, the compound can be named as a substituted phenol, with carbon atom 1 bearing the hydroxyl group. For example, the systematic name for thymol is 5-methyl-2-isopropylphenol. Phenols with only one other substituent can be named using either the appropriate numbers or the ortho (1,2), meta (1,3), and para (1,4) system. Compounds with other principal functional groups can be named with the hydroxyl group as a hydroxy substituent. For example, the systematic name for vanillin is 4-hydroxy-3-methoxybenzaldehyde.

Physical properties of phenols

      Similar to alcohols, phenols have hydroxyl groups that can participate in intermolecular hydrogen bonding; in fact, phenols tend to form stronger hydrogen bonds than alcohols. (See chemical bonding: Intermolecular forces (chemical bonding) for more information about hydrogen bonding.) Hydrogen bonding results in higher melting points (melting point) and much higher boiling points (boiling point) for phenols than for hydrocarbons (hydrocarbon) with similar molecular weights. For example, phenol (molecular weight [MW] 94, boiling point [bp] 182 °C [359.6 °F]) has a boiling point more than 70 degrees higher than that of toluene (C₆H₅CH₃; MW 92, bp 111 °C [231.8 °F]).

       Physical properties of phenolsThe ability of phenols to form strong hydrogen bonds also enhances their solubility in water. Phenol dissolves to give a 9.3 percent solution in water, compared with a 3.6 percent solution for cyclohexanol in water. The association between water and phenol is unusually strong; when crystalline phenol is left out in a humid environment, it picks up enough water from the air to form liquid droplets. Physical properties of phenols

Synthesis of phenols

      Most of the phenol used today is produced from benzene, through either hydrolysis of chlorobenzene or oxidation of isopropylbenzene (cumene).

Hydrolysis of chlorobenzene (the Dow process)

      Benzene is easily converted to chlorobenzene by a variety of methods, one of which is the Dow process. Chlorobenzene is hydrolyzed by a strong base at high temperatures to give a phenoxide salt, which is acidified to phenol.

Oxidation of isopropylbenzene

      Benzene is converted to isopropylbenzene (cumene) by treatment with propylene and an acidic catalyst. Oxidation yields a hydroperoxide (cumene hydroperoxide), which undergoes acid-catalyzed rearrangement to phenol and acetone. Although this process seems more complicated than the Dow process, it is advantageous because it produces two valuable industrial products: phenol and acetone.

General synthesis of phenols

      To make more-complicated phenolic compounds, a more general synthesis is needed. The cumene hydroperoxide reaction is fairly specific to phenol itself. The Dow process is somewhat more general, but the stringent conditions required often lead to low yields, and they may destroy any other functional groups (functional group) on the molecule. A milder, more general reaction is the diazotization of an arylamine (a derivative of aniline, C₆H₅NH₂) to give a diazonium salt, which hydrolyzes to a phenol. Most functional groups can survive this technique, as long as they are stable in the presence of dilute acid.

Reactions of phenols

      Much of the chemistry of phenols is like that of alcohols (alcohol). For example, phenols react with acids to give esters (ester), and phenoxide ions (ArO⁻) can be good nucleophiles (nucleophile) in Williamson ether synthesis.

Acidity of phenols

      Although phenols are often considered simply as aromatic alcohols, they do have somewhat different properties. The most obvious difference is the enhanced acidity of phenols. Phenols are not as acidic as carboxylic acids (carboxylic acid), but they are much more acidic than aliphatic alcohols, and they are more acidic than water. Unlike simple alcohols, most phenols are completely deprotonated by sodium hydroxide (NaOH).

Oxidation

      Like other alcohols, phenols undergo oxidation, but they give different types of products from those seen with aliphatic alcohols. For example, chromic acid oxidizes most phenols to conjugated 1,4-diketones called quinones (quinone). In the presence of oxygen in the air, many phenols slowly oxidize to give dark mixtures containing quinones.

       hydroquinone (1,4-benzenediol) is a particularly easy compound to oxidize, because it has two hydroxyl groups in the proper relationship to give up hydrogen atoms to form a quinone. Hydroquinone is used in developing photographic film by reducing activated (exposed to light) silver bromide (AgBr) to black metallic silver (Ag↓). Unexposed grains of silver bromide react more slowly than the exposed grains.

Electrophilic aromatic substitution

      Phenols are highly reactive toward electrophilic aromatic substitution, because the nonbonding electrons (electron) on oxygen stabilize the intermediate cation. This stabilization is most effective for attack at the ortho or para position of the ring; therefore, the hydroxyl group of a phenol is considered to be activating (i.e., its presence causes the aromatic ring to be more reactive than benzene) and ortho- or para-directing.

       picric acid (2,4,6-trinitrophenol) is an important explosive that was used in World War I. An effective explosive needs a high proportion of oxidizing groups such as nitro groups. Nitro groups are strongly deactivating (i.e., make the aromatic ring less reactive), however, and it is often difficult to add a second or third nitro group to an aromatic compound. Three nitro groups are more easily substituted onto phenol, because the strong activation of the hydroxyl group helps to counteract the deactivation of the first and second nitro groups.

      Phenoxide ions, generated by treating a phenol with sodium hydroxide, are so strongly activated that they undergo electrophilic aromatic substitution even with very weak electrophiles (electrophile) such as carbon dioxide (CO₂). This reaction is used commercially to make salicylic acid for conversion to aspirin and methyl salicylate.

Formation of phenol-formaldehyde resins

      Phenolic resins (resin) account for a large portion of phenol production. Under the trade name Bakelite, a phenol-formaldehyde resin was one of the earliest plastics (plastic), invented by American industrial chemist Leo Baekeland (Baekeland, Leo Hendrik) and patented in 1909. Phenol-formaldehyde resins are inexpensive, heat-resistant, and waterproof, though somewhat brittle. The polymerization of phenol with formaldehyde involves electrophilic aromatic substitution at the ortho and para positions of phenol (probably somewhat randomly), followed by cross-linking of the polymeric chains.

Leroy G. Wade, Jr.

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