Editing Phenol (section)

==Properties==
Phenol is an organic compound appreciably [[solubility|soluble]] in water, with about 84.2&nbsp;g dissolving in 1000&nbsp;ml (0.895 [[Molar concentration|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.<ref name=pubchem/>

===Acidity===
Phenol is a weak acid, with a pH range of 5 to 6. In aqueous solution in the pH range ca. 8 - 12 it is in equilibrium with the '''phenolate''' [[anion]] {{chem2|C6H5O-}} (also called '''phenoxide''' or '''carbolate'''):<ref>{{March6th}}</ref>
:{{chem2 | C6H5OH <-> C6H5O- + H+ }}

:[[File:Phenol-phenolate equilibrium.svg|class=skin-invert-image|thumb|left|upright=1.5|[[Resonance structures]] of the phenoxide anion]]{{clear-left}}

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 [[arene substitution patterns|ortho and para]] carbon atoms through the pi system.<ref>''Organic Chemistry'' 2nd Ed. John McMurry {{ISBN|0-534-07968-7}}</ref> An alternative explanation involves the sigma framework, postulating that the dominant effect is the [[inductive effect|induction]] from the more electronegative [[orbital hybridisation|sp<sup>2</sup> hybridised carbons]]; the comparatively more powerful inductive withdrawal of electron density that is provided by the sp<sup>2</sup> system compared to an sp<sup>3</sup> system allows for great stabilization of the oxyanion. In support of the second explanation, the [[acid dissociation constant|p''K''<sub>a</sub>]] of the [[enol]] of [[acetone]] in water is 10.9, making it only slightly less acidic than phenol (p''K''<sub>a</sub> 10.0).<ref name=pubchem/> 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 acids and bases|Lewis bases]] such as [[pyridine]], [[diethyl ether]], and [[diethyl sulfide]].  The enthalpies of adduct formation and the {{chem2|\sOH}} IR frequency shifts accompanying adduct formation have been compiled.<ref>Drago, R S. Physical Methods For Chemists, (Saunders College Publishing 1992), ISBN 0-03-075176-4</ref>  Phenol is classified as a [[HSAB theory|hard acid]].<ref>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</ref><ref>{{cite journal|author1=Cramer, R. E. |author2=Bopp, T. T. |year=1977|title= Graphical display of the enthalpies of adduct formation for Lewis acids and bases |journal= Journal of Chemical Education |volume=54|pages=612–613|doi= 10.1021/ed054p612}} The plots shown in this paper used older parameters. Improved E&C parameters are listed in [[ECW model]].</ref>

====Tautomerism====
[[File:Phenol tautomers.svg|class=skin-invert-image|left|thumb|upright=.75|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<sup>−13</sup>, which means only one in every ten trillion molecules is in the keto form at any moment.<ref>{{cite journal |title=Ketonization equilibria of phenol in aqueous solution |first1=Marco |last1=Capponi |first2=Ivo G. |last2=Gut |first3=Bruno |last3=Hellrung |first4=Gaby |last4=Persy |first5=Jakob |last5=Wirz |journal=[[Canadian Journal of Chemistry|Can. J. Chem.]] |year=1999 |volume=77 |pages=605–613 |doi=10.1139/cjc-77-5-6-605 |issue=5–6}}</ref> 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.<ref>{{Clayden|page=531}}</ref> 4,4' Substituted cyclohexadienone can undergo a [[dienone–phenol rearrangement]] in acid conditions and form stable 3,4‐disubstituted phenol.<ref>{{cite journal |last1=Arnold |first1=Richard T. |last2=Buckley |first2=Jay S. |title=The Dienone-Phenol Rearrangement. II. Rearrangement of 1-Keto-4-methyl-4-phenyl-1,4-dihydronaphthalene |journal=J. Am. Chem. Soc. |date=1 May 1949 |volume=71 |issue=5 |page=1781 |doi=10.1021/ja01173a071|bibcode=1949JAChS..71.1781A }}</ref>

For substituted phenols, several factors can favor the keto tautomer: (a) additional hydroxy groups (see [[resorcinol]]) (b) annulation as in the formation of [[naphthol]]s, and (c) deprotonation to give the phenolate.<ref>{{cite book|title=The Chemistry of Phenols|editor=Zvi Rappoport |series = PATAI'S Chemistry of Functional Groups | chapter=Tautomeric Equilibria and Rearrangements Involving Phenols |doi=10.1002/0470857277.ch11
| year=2003 |publisher=John Wiley & Sons| author=Sergei M. Lukyanov, Alla V. Koblik|pages=713–838 |isbn=0471497371 }}</ref>

Phenoxides are [[enolate]]s 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".<ref>{{cite journal |title=2,6,6-Trimethyl-2,4-Cyclohexadione |author1=David Y. Curtin |author2=Allan R. Stein |name-list-style=amp |journal=[[Organic Syntheses]] |year=1966 |volume=46 |pages=115 |url=http://www.orgsyn.org/orgsyn/prep.asp?prep=cv5p1092 |doi=10.15227/orgsyn.046.0115 |access-date=2010-03-31 |archive-url=https://web.archive.org/web/20110605132001/http://www.orgsyn.org/orgsyn/prep.asp?prep=cv5p1092 |archive-date=2011-06-05 |url-status=dead }}</ref>

===Reactions===
[[File:Hockpart2.svg|class=skin-invert-image|thumb|right|The Hock process leading to phenol via [[autoxidation]] of cumene.]]
[[File:Phenol-elpot-3D-vdW.png|right|thumb|[[Polar surface area]] of a "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.]]
[[File:Phenol in water.PNG|class=skin-invert-image|thumb|right|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.<ref>{{Ullmann|vauthors=Muller F,  Caillard L |title=Chlorophenols|year=2011|doi=10.1002/14356007.a07_001.pub2}}</ref> The reaction affords 2- and 4-substituted derivatives. The regiochemistry of halogenation changes in strongly acidic solutions where {{chem2|PhOH2]+}} 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 [[Picric acid|2,4,6-trinitrophenol]].  [[Friedel Crafts alkylation]]s of phenol and its derivatives often proceed without catalysts.  Alkylating agents include alkyl halides, alkenes, and ketones.  Thus, [[1-Bromoadamantane|adamantyl-1-bromide]], [[dicyclopentadiene]]), and [[cyclohexanone]]s give respectively 4-adamantylphenol, a bis(2-hydroxyphenyl) derivative, and a 4-cyclohexylphenols.  [[Alcohol (chemistry)|Alcohol]]s and [[hydroperoxide]]s alkylate phenols in the presence of [[solid acid]] [[catalyst]]s (e.g. certain [[zeolite]]).  [[Cresol]]s and cumyl phenols can be produced in that way.<ref name=reddy>{{cite book|title=The Chemistry of Phenols|editor=Zvi Rappoport |series = PATAI'S Chemistry of Functional Groups | chapter=Electrophilic reactions of phenols |doi=10.1002/0470857277.ch9|year=2003 |publisher =John Wiley & Sons|author=V. Prakash Reddy. G. K. Surya Prakash|pages=605–660 |isbn=0471497371 }}</ref>

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]].
:{{chem2|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]]:
:{{chem2|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&nbsp;°C:<ref>{{cite book|last=Roscoe|first=Henry|title=A treatise on chemistry, Volume 3, Part 3|year=1891|publisher=Macmillan & Co.|location=London|pages=23|url=https://books.google.com/books?id=HEY9AAAAYAAJ&q=zinc&pg=PA199}}</ref>
:{{chem2|C6H5OH + Zn -> C6H6 + ZnO}}

When phenol is treated with [[diazomethane]] in the presence of [[boron trifluoride]] ({{chem2|BF3}}), [[anisole]] is obtained as the main product and nitrogen gas as a byproduct.
:{{chem2|C6H5OH + CH2N2 -> C6H5OCH3 + N2}}

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