Chapter 17 alcohols and phenols
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Chapter 17: Alcohols and Phenols. Based on McMurry’s Organic Chemistry , 7 th edition. Alcohols and Phenols. Alcohols contain an OH group connected to a a saturated C (sp 3 ) They are important solvents and synthesis intermediates

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Chapter 17 alcohols and phenols

Chapter 17: Alcohols and Phenols

Based on McMurry’s Organic Chemistry, 7th edition

Alcohols and phenols
Alcohols and Phenols

  • Alcohols contain an OH group connected to a a saturated C (sp3)

  • They are important solvents and synthesis intermediates

  • Phenols contain an OH group connected to a carbon in a benzene ring

  • Methanol, CH3OH, called methyl alcohol, is a common solvent, a fuel additive, produced in large quantities

  • Ethanol, CH3CH2OH, called ethyl alcohol, is a solvent, fuel, beverage

  • Phenol, C6H5OH (“phenyl alcohol”) has diverse uses - it gives its name to the general class of compounds

  • OH groups bonded to vinylic, sp2-hybridized carbons are called enols

Why this chapter
Why this Chapter?

  • To begin to study oxygen-containing functional groups

  • These groups lie at the heart of biological chemistry

17 1 naming alcohols and phenols
17.1 Naming Alcohols and Phenols

  • General classifications of alcohols based on substitution on C to which OH is attached

  • Methyl (C has 3 H’s), Primary (1°) (C has two H’s, one R), secondary (2°) (C has one H, two R’s), tertiary (3°) (C has no H, 3 R’s),

Iupac rules for naming alcohols
IUPAC Rules for Naming Alcohols

  • Select the longest carbon chain containing the hydroxyl group, and derive the parent name by replacing the -e ending of the corresponding alkane with -ol

  • Number the chain from the end nearer the hydroxyl group

  • Number substituents according to position on chain, listing the substituents in alphabetical order

Naming phenols
Naming Phenols

  • Use “phenol” (the French name for benzene) as the parent hydrocarbon name, not benzene

  • Name substituents on aromatic ring by their position from OH

17 2 properties of alcohols and phenols
17.2 Properties of Alcohols and Phenols

  • The structure around O of the alcohol or phenol is similar to that in water, sp3 hybridized

  • Alcohols and phenols have much higher boiling points than similar alkanes and alkyl halides

  • A positively polarized OH hydrogen atom from one molecule is attracted to a lone pair of electrons on a negatively polarized oxygen atom of another molecule

  • This produces a force that holds the two molecules together

  • These intermolecular attractions are present in solution but not in the gas phase, thus elevating the boiling point of the solution

Properties of alcohols and phenols acidity and basicity
Properties of Alcohols and Phenols: Acidity and Basicity

  • Weakly basic and weakly acidic

  • Alcohols are weak Brønsted bases

  • Protonated by strong acids to yield oxonium ions, ROH2+

Alcohols and phenols are weak br nsted acids
Alcohols and Phenols are Weak Brønsted Acids

  • Can transfer a proton to water to a very small extent

  • Produces H3O+ and an alkoxide ion, RO, or a phenoxide ion, ArO

Acidity measurements
Acidity Measurements

  • The acidity constant, Ka, measures the extent to which a Brønsted acid transfers a proton to water

    [A] [H3O+]Ka = ————— and pKa = log Ka


  • Relative acidities are more conveniently presented on a logarithmic scale, pKa, which is directly proportional to the free energy of the equilibrium

  • Differences in pKa correspond to differences in free energy

  • Table 17.1 presents a range of acids and their pKa values

Pk a values for typical oh compounds
pKa Values for Typical OH Compounds

Relative acidities of alcohols
Relative Acidities of Alcohols

  • Simple alcohols are about as acidic as water

  • Alkyl groups make an alcohol a weaker acid

  • The more easily the alkoxide ion is solvated by water the more its formation is energetically favored

  • Steric effects are important

Inductive effects
Inductive Effects

  • Electron-withdrawing groups make an alcohol a stronger acid by stabilizing the conjugate base (alkoxide)

Generating alkoxides from alcohols
Generating Alkoxides from Alcohols

  • Alcohols are weak acids – requires a strong base to form an alkoxide such as NaH, sodium amide NaNH2, and Grignard reagents (RMgX)

  • Alkoxides are bases used as reagents in organic chemistry

Phenol acidity
Phenol Acidity

  • Phenols (pKa ~10) are much more acidic than alcohols (pKa ~ 16) due to resonance stabilization of the phenoxide ion

  • Phenols react with NaOH solutions (but alcohols do not), forming salts that are soluble in dilute aqueous solution

  • A phenolic component can be separated from an organic solution by extraction into basic aqueous solution and is isolated after acid is added to the solution

Nitro phenols

  • Phenols with nitro groups at the ortho and para positions are much stronger acids

17 3 preparation of alcohols a review
17.3 Preparation of Alcohols: A Review

  • Alcohols are derived from many types of compounds

  • The alcohol hydroxyl can be converted to many other functional groups

  • This makes alcohols useful in synthesis

Review preparation of alcohols by regiospecific hydration of alkenes
Review: Preparation of Alcohols by Regiospecific Hydration of Alkenes

  • Hydroboration/oxidation: syn, non-Markovnikov hydration

  • Oxymercuration/reduction: Markovnikov hydration

1 2 diols
1,2-Diols of Alkenes

  • Review: Cis-1,2-diols from hydroxylation of an alkene with OsO4 followed by reduction with NaHSO3

  • Trans-1,2-diols from acid-catalyzed hydrolysis of epoxides

17 4 alcohols from reduction of carbonyl compounds
17.4 Alcohols from Reduction of Carbonyl Compounds of Alkenes

  • Reduction of a carbonyl compound in general gives an alcohol

  • Note that organic reduction reactions add the equivalent of H2 to a molecule

Reduction of aldehydes and ketones
Reduction of Aldehydes and Ketones of Alkenes

  • Aldehydes gives primary alcohols

  • Ketones gives secondary alcohols

Reduction reagent sodium borohydride
Reduction Reagent: Sodium Borohydride of Alkenes

  • NaBH4 is not sensitive to moisture and it does not reduce other common functional groups

  • Lithium aluminum hydride (LiAlH4) is more powerful, less specific, and very reactive with water

  • Both add the equivalent of “H-”

Mechanism of reduction
Mechanism of Reduction of Alkenes

  • The reagent adds the equivalent of hydride to the carbon of C=O and polarizes the group as well

Reduction of carboxylic acids and esters
Reduction of Carboxylic Acids and Esters of Alkenes

  • Carboxylic acids and esters are reduced to give primary alcohols

  • LiAlH4 is used because NaBH4 is not effective

17 5 alcohols from reaction of carbonyl compounds with grignard reagents
17.5 Alcohols from Reaction of Carbonyl Compounds with Grignard Reagents

  • Alkyl, aryl, and vinylic halides react with magnesium in ether or tetrahydrofuran to generate Grignard reagents, RMgX

  • Grignard reagents react with carbonyl compounds to yield alcohols

Reactions of esters and grignard reagents
Reactions of Esters and Grignard Reagents Grignard Reagents

  • Yields tertiary alcohols in which two of the substituents carbon come from the Grignard reagent

  • Grignard reagents do not add to carboxylic acids – they undergo an acid-base reaction, generating the hydrocarbon of the Grignard reagent

Grignard reagents and other functional groups in the same molecule
Grignard Reagents and Other Functional Groups in the Same Molecule

  • Can't be prepared if there are reactive functional groups in the same molecule, including proton donors

Mechanism of the addition of a grignard reagent
Mechanism of the Addition of a Grignard Reagent Molecule

  • Grignard reagents act as nucleophilic carbon anions (carbanions, : R) in adding to a carbonyl group

  • The intermediate alkoxide is then protonated to produce the alcohol

17 6 reactions of alcohols
17.6 Reactions of Alcohols Molecule

  • Conversion of alcohols into alkyl halides:

  • 3˚ alcohols react with HCl or HBr by SN1 through carbocation intermediate

  • 1˚ and 2˚ alcohols converted into halides by treatment with SOCl2 or PBr3 via SN2 mechanism

Conversion of alcohols into tosylates
Conversion of Alcohols into Tosylates Molecule

  • Reaction with p-toluenesulfonyl chloride (tosyl chloride, p-TosCl) in pyridine yields alkyl tosylates, ROTos

  • Formation of the tosylate does not involve the C–O bond so configuration at a chirality center is maintained

  • Alkyl tosylates react like alkyl halides

Stereochemical uses of tosylates
Stereochemical Uses of Tosylates Molecule

  • The SN2 reaction of an alcohol via a tosylate, produces inversion at the chirality center

  • The SN2 reaction of an alcohol via an alkyl halide proceeds with two inversions, giving product with same arrangement as starting alcohol

Dehydration of alcohols to yield alkenes
Dehydration of Alcohols to Yield Alkenes Molecule

  • The general reaction: forming an alkene from an alcohol through loss of O-H and H (hence dehydration) of the neighboring C–H to give  bond

  • Specific reagents are needed

Acid catalyzed dehydration
Acid- Catalyzed Dehydration Molecule

  • Tertiary alcohols are readily dehydrated with acid

  • Secondary alcohols require severe conditions (75% H2SO4, 100°C) - sensitive molecules don't survive

  • Primary alcohols require very harsh conditions – impractical

  • Reactivity is the result of the nature of the carbocation intermediate

Dehydration with pocl 3
Dehydration with POCl Molecule3

  • Phosphorus oxychloride in the amine solvent pyridine can lead to dehydration of secondary and tertiary alcohols at low temperatures

  • An E2 via an intermediate ester of POCl2 (see Figure 17.7)

17 7 oxidation of alcohols
17.7 Oxidation of Alcohols Molecule

  • Can be accomplished by inorganic reagents, such as KMnO4, CrO3, and Na2Cr2O7 or by more selective, expensive reagents

Oxidation of primary alcohols
Oxidation of Primary Alcohols Molecule

  • To aldehyde: pyridinium chlorochromate (PCC, C5H6NCrO3Cl) in dichloromethane

  • Other reagents produce carboxylic acids

Oxidation of secondary alcohols
Oxidation of Secondary Alcohols Molecule

  • Effective with inexpensive reagents such as Na2Cr2O7 in acetic acid

  • PCC is used for sensitive alcohols at lower temperatures

Mechanism of chromic acid oxidation
Mechanism of Chromic Acid Oxidation Molecule

  • Alcohol forms a chromate ester followed by elimination with electron transfer to give ketone

  • The mechanism was determined by observing the effects of isotopes on rates

17 8 protection of alcohols
17.8 Protection of Alcohols Molecule

  • Hydroxyl groups can easily transfer their proton to a basic reagent

  • This can prevent desired reactions

  • Converting the hydroxyl to a (removable) functional group without an acidic proton protects the alcohol

Methods to protect alcohols
Methods to Protect Alcohols Molecule

  • Reaction with chlorotrimethylsilane in the presence of base yields an unreactive trimethylsilyl (TMS) ether

  • The ether can be cleaved with acid or with fluoride ion to regenerate the alcohol

Protection deprotection
Protection-Deprotection Molecule

  • An example of TMS-alcohol protection in a synthesis

17 9 phenols and their uses
17.9 Phenols Molecule and Their Uses

  • Industrial process from readily available cumene

  • Forms cumene hydroperoxide with oxygen at high temperature

  • Converted into phenol and acetone by acid

17 10 reactions of phenols
17.10 Reactions of Phenols Molecule

  • The hydroxyl group is a strongly activating, making phenols substrates for electrophilic halogenation, nitration, sulfonation, and Friedel–Crafts reactions

  • Reaction of a phenol with strong oxidizing agents yields a quinone

  • Fremy's salt [(KSO3)2NO] works under mild conditions through a radical mechanism

Quinones in nature
Quinones in Nature Molecule

  • Ubiquinones mediate electron-transfer processes involved in energy production through their redox reactions

17 11 spectroscopy of alcohols and phenols
17.11 Spectroscopy of Alcohols and Phenols Molecule

  • Characteristic O–H stretching absorption at 3300 to 3600 cm1 in the infrared

  • Sharp absorption near 3600 cm-1 except if H-bonded: then broad absorption 3300 to 3400 cm1 range

  • Strong C–O stretching absorption near 1050 cm1 (See Figure 17.11)

  • Phenol OH absorbs near 3500 cm-1

Nuclear magnetic resonance spectroscopy
Nuclear Magnetic Resonance Spectroscopy Molecule

  • 13C NMR: C bonded to OH absorbs at a lower field,  50 to 80

  • 1H NMR: electron-withdrawing effect of the nearby oxygen, absorbs at  3.5 to 4 (See Figure 17-13)

    • Usually no spin-spin coupling between O–H proton and neighboring protons on C due to exchange reactions with moisture or acids

    • Spin–spin splitting is observed between protons on the oxygen-bearing carbon and other neighbors

  • Phenol O–H protons absorb at  3 to 8

Mass spectrometry
Mass Spectrometry Molecule

  • Alcohols undergo alpha cleavage, a C–C bond nearest the hydroxyl group is broken, yielding a neutral radical plus a charged oxygen-containing fragment

  • Alcohols undergo dehydration to yield an alkene radical anion