Instructor: Chad Snyder, PhD, Grace College
Topic: Structure and Synthesis of Alcohols, Organic Chemistry, 9th Edition, L. G. Wade, Jr.
Year Published: 2017
Alcohols are organic compounds that contain hydroxyl (OH) groups.
Importance: Widely used in nature, industry, and in household products.
Hybridization: Oxygen is sp3 hybridized, forming a tetrahedral structure.
Angles:
H—O—H angle in water: 104.5°.
C—O—H angle in methyl alcohol (methanol): 108.9°.
Carbinol Carbon: Refers to the carbon atom that is bonded to the hydroxyl group.
Primary Alcohol: The carbon bonded to the —OH group is attached to one other carbon.
Secondary Alcohol: The carbon with —OH is connected to two other carbons.
Tertiary Alcohol: The carbon with —OH is bonded to three other carbons.
Aromatic (Phenol): The hydroxyl group is attached to a benzene ring.
Primary: CH3-CH2-CH2OH (1-Propanol)
Secondary: CH3-CHOH-CH2-CH3 (2-Butanol)
Steps:
Identify the longest carbon chain containing the —OH group.
Modify the alkane name by dropping the -e and adding -ol.
Number the chain to provide the lowest number to the —OH group.
Number substituents and list them alphabetically.
Types of Alcohols and Examples:
Primary: Ethanol (ethyl alcohol)
Secondary: 2-Methylpropan-1-ol (Isobutyl alcohol)
Tertiary: 2-Methylpropan-2-ol (tert-Butyl alcohol)
Hydroxyl group has precedence in naming; assign lowest number to the carbon with —OH.
Use the suffix -ene before -ol.
Example: pent-4-ene-2-ol
Highest to lowest priority:
Acids
Esters
Aldehydes
Ketones
Alcohols
Amines
Alkenes, Alkynes
Alkanes
Ethers
Halides
When the —OH group is part of a higher priority compound, it is named as hydroxy.
Example: 4-hydroxybutanoic acid (gamma-hydroxybutyric acid, GHB)
Alcohols can be named as alkyl alcohols but generally for smaller groups.
Examples: Isobutyl alcohol (2-methylpropan-1-ol), sec-butyl alcohol (butan-2-ol)
Diols: Two hydroxyl groups require two locational numbers.
Suffix -diol is used.
Example: Hexane-1,6-diol
1,2-diols are referred to as glycols; commonly named using the alkenes they derive from.
Examples include ethylene glycol (ethane-1,2-diol) and propylene glycol (propane-1,2-diol).
The —OH group on phenol is assumed to be on carbon 1.
Use ortho-, meta-, and para- for di-substituted phenols.
Example: 3-chlorophenol is meta-chlorophenol.
Alcohols generally have higher boiling points than alkanes and ethers due to hydrogen bonding.
Miscibility in water: Small alcohols are miscible in water; solubility decreases with increased alkyl group size.
Table of Selected Alcohols: Physical Properties
Methanol (CH3OH): bp = 65°C, mp = -97°C
Ethanol (C2H5OH): bp = 78°C, mp = -114°C
Propan-1-ol (C3H7OH): bp = 97°C, mp = -126°C
Butan-2-ol (C4H10O): bp = 100°C, mp = -90°C
Cyclohexanol: bp = 162°C
Higher boiling points relative to ethers and alkanes due to hydrogen bonding.
More energy is required to break hydrogen bonds, which results in higher boiling points.
Commonly known as wood alcohol.
Industrial applications as a solvent; toxic dose: ~100 mL.
Used as fuel: low emissions and high octane rating.
Produced via fermentation; distillation for liquor production.
95% ethanol = constant boiling azeotrope.
Toxic dose: ~200 mL.
Produced by catalytic hydration of propylene.
Commonly used as rubbing alcohol.
pKa range for alcohols: 15.5–18.0.
Acidity decreases with increased substitution on alkyl groups; halogens enhance acidity.
Example: Phenol is markedly more acidic than cyclohexanol.
Formation of Alkoxide Ions: Reaction of ethanol with sodium metal yields sodium ethoxide.
Phenoxide Ion Formation: Aromatic alcohols like phenol exhibit increased acidity.
Synthesis Methods: Nucleophilic substitution (SN2) and water addition to double bonds produce alcohols... ...