Chapter 17 alcohols and phenols
This presentation is the property of its rightful owner.
Sponsored Links
1 / 50

Chapter 17: Alcohols and Phenols PowerPoint PPT Presentation


  • 139 Views
  • Uploaded on
  • Presentation posted in: General

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

Download Presentation

Chapter 17: Alcohols and Phenols

An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript


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

    [HA]

  • 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

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

  • 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

  • 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

  • Aldehydes gives primary alcohols

  • Ketones gives secondary alcohols


Reduction reagent sodium borohydride

Reduction Reagent: Sodium Borohydride

  • 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

  • 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

  • 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 grignard reagents with carbonyl compounds

Reactions of Grignard Reagents with Carbonyl Compounds


Reactions of esters and grignard reagents

Reactions of Esters and 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

  • 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

  • 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

  • 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

  • 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

  • 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

  • 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 POCl3

  • 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)


Conversion of alcohols into esters

Conversion of Alcohols into Esters


17 7 oxidation of alcohols

17.7 Oxidation of Alcohols

  • 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

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

  • Other reagents produce carboxylic acids


Oxidation of secondary alcohols

Oxidation of Secondary Alcohols

  • 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

  • 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

  • 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

  • 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

  • An example of TMS-alcohol protection in a synthesis


17 9 phenols and their uses

17.9 Phenols 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

  • 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

  • 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

  • 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

  • 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

  • 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


  • Login