1	Chemistry 121(01) Winter 2009
2	Chapter 14: Alcohols, Phenols and Ethers Sections 14.1-4.21
3	Chapter 14: Alcohols, Phenols, and Ethers
4	Chapter 5. Alcohols, Phenols, and Ethers Functional groups: alcohol: R-O-H phenols: Ar-OH ether: R-O-R' thiol: R-S-H
5	Nomenclature of compounds containing functional groups The IUPAC system deals with functional groups two different ways. Modification of the hydrocarbon name to indicate the presence of a functional group. alcohol, -OH use -ol ending. ether: CH₃CH₂-O-CH₃ use methoxy methoxy ethane thiol: R-S-H use -thiol ending.
6	Alcohol example
7	Alcohols - Structure The functional group of an alcohol is an -OH group bonded to an sp³ hybridized carbon bond angles about the hydroxyl oxygen atom are approximately 109.5° Oxygen is also sp³ hybridized two sp³ hybrid orbitals form sigma bonds to carbon and hydrogen the remaining two sp³ hybrid orbitals each contain an unshared pair of electrons
8	Alcohols - Nomenclature IUPAC names the parent chain is the longest chain that contains the -OH group number the parent chain in the direction that gives the -OH group the lower number change the suffix -e to -ol Common names name the alkyl group bonded to oxygen followed by the word alcohol
9	Alcohols - Nomenclature Problem: Write the IUPAC name of each alcohol
10	Alcohols - Nomenclature Compounds containing two -OH groups are named as diols, three -OH groups are named as triols, etc.
11	Alcohols - Nomenclature Unsaturated alcohols the double bond is shown by the infix -en- the hydroxyl group is shown by the suffix -ol number the chain to give OH the lower number
12	Alcohols - Nomenclature Examples:
13	Name the alcohol
14	Common names Ethyl alcohol ethylene glycol glycerol
15	Classification of alcohols Primary Secondary Tertiary.
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20	Physical Properties Alcohols are polar compounds both the C-O and O-H bonds are polar covalent
21	Hydrogen Bonding Alcohols associate in the liquid state by hydrogen bonding Hydrogen bonding: the attractive force between a partial positive charge on hydrogen and a partial negative charge on a nearby oxygen, nitrogen, or fluorine atom the strength of hydrogen bonding in alcohols is approximately 2 to 5 kcal/mol hydrogen bonds are considerably weaker than covalent bonds (for example, 110 kcal/mol for an O-H bond) nonetheless, hydrogen bonding can have a significant effect on physical properties
22	Hydrogen Bonding Figure 8.3 shows the association of ethanol molecules in the liquid state (only two of the three possible hydrogen bonds to the upper oxygen are shown here).
23	Boiling Points alcohols have higher boiling points and are more soluble in water than hydrocarbons
24	Conversion of ROH to RX water-soluble 3° alcohols react very rapidly with HCl, HBr, and HI low-molecular-weight 1° and 2° alcohols are unreactive under these conditions
25	Conversion of ROH to RX water-insoluble 3° alcohols react by bubbling gaseous HCl through a solution of the alcohol dissolved in diethyl ether or THF 1° and 2° alcohols require concentrated HBr and HI to form alkyl bromides and iodides
26	Reaction of a 3° ROH with HX Step 2: loss of H₂O from the oxonium ion gives a 3° carbocation intermediate Step 3: reaction with halide ion completes the reaction
27	Reaction with SOCl₂ Thionyl chloride, SOCl₂, is the most widely used reagent for conversion of alcohols to alkyl chlorides
28	Dehydration of Alcohols An alcohol can be converted to an alkene by elimination of H and OH from adjacent carbons (a b-elimination) 1° alcohols must be heated at high temperature in the presence of an acid catalyst, such as H₂SO₄ or H₃PO₄ 2° alcohols undergo dehydration at somewhat lower temperatures 3° alcohols often require temperatures only at or slightly above room temperature
29	Dehydration of Alcohols examples:
30	Hydration-Dehydration Acid-catalyzed hydration of an alkene and dehydration of an alcohol are competing processes large amounts of water favor alcohol formation scarcity of water or experimental conditions where water is removed favor alkene formation
31	Oxidation of Alcohols Oxidation of a 1° alcohol gives an aldehyde or a carboxylic acid, depending on the oxidizing agent and experimental conditions the most common oxidizing agent is chromic acid chromic acid oxidation of 1-octanol gives octanoic acid
32	Oxidation of Alcohols to oxidize a 1° alcohol to an aldehyde, use PCC PCC oxidation of geraniol gives geranial Tertiary alcohols are not oxidized by either of these reagents; they are resistant to oxidation
33	Acidity of Alcohols pK_a values for several low-molecular-weight alcohols
34	Reaction with Active Metals Alcohols react with Li, Na, K, and other active metals to liberate hydrogen gas and form metal alkoxides Na is oxidized to Na⁺ and H⁺ is reduced to H₂ alkoxides are somewhat stronger bases that OH^- alkoxides can be used as nucleophiles in nucleophilic substitution reactions they can also be used as bases in b-elimination reactions
35	Conversion of ROH to RX Conversion of an alcohol to an alkyl halide involves substitution of halogen for -OH at a saturated carbon the most common reagents for this purpose are the halogen acids, HX, and thionyl chloride, SOCl₂
36	Ethers - Structure The functional group of an ether is an oxygen atom bonded to two carbon atoms oxygen is sp³ hybridized with bond angles of approximately 109.5° in dimethyl ether, the C-O-C bond angle is 110.3°
37	Naming Ethers 2-propoxybutane 2-methoxyphenol ethoxycyclopropane isopropyl propyl ether methyl phenyl ether
38	Ethers - Nomenclature IUPAC the longest carbon chain is the parent alkane name the -OR group as an alkoxy substituent Common names: name the groups bonded to oxygen followed by the word ether
39	Ethers - Nomenclature Although cyclic ethers have IUPAC names, their common names are more widely used
40	Ethers - Physical Properties Ethers are polar molecules each C-O bond is polar covalent however, only weak attractive forces exist between ether molecules
41	Ethers - Physical Properties boiling points are lower than those of alcohols
42	Ethers - Physical Properties ethers are hydrogen bond donors
43	Ethers - Physical Properties the effect of hydrogen bonding is illustrated by comparing the boiling points of ethanol and dimethyl ether
44	Reactions of Ethers Ethers resemble hydrocarbons in their resistance to chemical reaction they do not react with strong oxidizing agents such as chromic acid, H₂CrO₄ they are not affected by most acids and bases at moderate temperatures Because of their good solvent properties and general inertness to chemical reaction, ethers are excellent solvents in which to carry out organic reactions
45	Epoxides Epoxide: a cyclic ether in which oxygen is one atom of a three-membered ring ethylene oxide is synthesized from ethylene and O₂
46	Epoxides other epoxides are synthesized from an alkene and a peroxycarboxylic acid, RCO₃H
47	Reactions of Epoxides ethers are generally unreactive to aqueous acid epoxides, however, react readily because of the angle strain in the three-membered ring reaction of an epoxide with aqueous acid gives a glycol
48	A Cycloalkene to a Glycol both cis and trans glycols can be prepared
49	Other Epoxide Ring Openings the value of epoxides lies in the number of nucleophiles that will bring about ring opening, and the combinations of functional groups that can be synthesized from them
50	Epoxides as Building Blocks following are structural formulas for two common drugs, each synthesized in part from ethylene oxide
51	Phenols The functional group of a phenol is an -OH group bonded to a benzene ring
52	Phenols some phenols
53	Acidity of Phenols Phenols are significantly more acidic than alcohols
54	Naming Phenols
55	Naming thiols
56	Thiols - Structure The functional group of a thiol is an -SH (sulfhydryl) group bonded to an sp³ hybridized carbon
57	Thiols - Nomenclature IUPAC names: the parent chain is the longest chain containing the -SH group add -thiol to the name of the parent chain Common names: name the alkyl group bonded to sulfur followed by the word mercaptan alternatively, indicate the -SH by the prefix mercapto
58	Thiols - Physical Properties Low-molecular-weight thiols have a STENCH
59	Thiols - Physical Properties The difference in electronegativity between S and H is 2.5 - 2.1 = 0.4 Because of their low polarity, thiols show little association by hydrogen bonding have lower boiling points and are less soluble in water than alcohols of comparable MW
60	Acidity of Thiols Thiols are stronger acids than alcohols Thiols react with strong bases to form salts
61	Oxidation of Thiols thiols are oxidized by a variety of oxidizing agents, including O₂, to disulfides disulfides, in turn, are easily reduced to thiols by several reagents this easy interconversion between thiols and disulfides is very important in protein chemistry