1. Alcohols, Ethers and Thiols Bettelheim, Brown, Campbell and Farrell Chapter 14

2. Review of Carbon Classification Type of CAttached to 1 o (primary) C one other carbon 2 o (secondary) Ctwo other carbons 3 o (tertiary) C three other carbons 4 o (quaternary) Cfour other carbons

3. Alcohols Alcohol:OH(hydroxyl) groupAlcohol: Has an -OH (hydroxyl) group bonded to a tetrahedral carbon –methanol, CH 3 OH, is the simplest alcohol

4. Classification of Alcohols Depends on the C which has the –OH group attached 1 o Alcohol— attached to one C 2 o Alcohol— attached to two Cs 3 o Alcohol-- attached to three Cs

5. Alcohol Nomenclature 1.Find longest carbon chain that contains the -OH group (parent chain) 2.Number chain from end that gives the -OH the lower number eol 3.Change the ending -e to -ol 4.Use a number to show the location of the -OH group For cyclic alcohols, the carbon with the -OH group is C-1 5.Name and number substituents and list them in alphabetical order

6. Nomenclature

7. Write the IUPAC name for each alcohol

8. Nomenclature

9. dioltriol –Alcohols containing more than one hydroxyl groups are named as a diol, a triol, and so on –IUPAC names for diols, triols, and so on retain the final "-e" in the name of the parent alkane glycols –Compounds containing two hydroxyl groups on adjacent carbons are commonly called glycols

10. Name the following

11. 1,3-propanediol trans-1,3-cyclohexanediol

12. Physical Properties Alcohols are polar molecules –the C-O and O-H bonds are both polar covalent

13. Physical Properties Alcohol molecules can form hydrogen bonds with each other Alcohols can also form hydrogen bonds with water

14. Physical Properties of Alcohols –Boiling point increases as MW increases –Solubility in water decreases as MW increases

15. Chemical Properties of Alcohols Combustion Reactions (they burn in O 2 ) Acid-Base Chemistry Dehydration Oxidation

16. Acidity of Alcohols Alcohols have about the same pK a values as water –Aqueous solutions of alcohols have the same pH as that of pure water –Phenols have lower pK a values than normal alcohols do (are more acidic)

17. Acidity of Alcohols Alcohols and phenols both contain an OH group –Phenols are weak acids and react with strong bases such as NaOH to form water-soluble salts –pK a = 9.89 for phenol –Alcohols are much weaker acids and do not react in this manner

18. Why are phenols more acidic than alcohols? Aromatic ring and O have delocalization of electrons. Less pull on H, so it is more acidic.

19. Dehydration Dehydration:Dehydration: Removal of water from adjacent carbons to form an alkene –most often occurs by heating an alcohol with either 85% H 3 PO 4 or concentrated H 2 SO 4

20. Dehydration essentially the reverse of hydration (addition of water to double bond) Conditions required depend on kind of alcohol

21. Acid-Catalyzed Dehydration 1 o ca 180 o C needed Hard 2 o lower temperatures Moderate 3 o slightly above room temperature Easy

22. Dehydration –Zaitsev’s Rule: When two alkene products are possible, the alkene having the greater number of alkyl groups (i.e., C atoms) on the double bond generally predominates (forms major product) –Major product favored. (minor product)

24. Dehydration-Hydration Related Acid-catalyzed hydration of alkenes and acid- catalyzed dehydration of alcohols are competing reactions Equilibrium between alkene and alcohol exists –Large amounts of water favor alcohol formation, while removal of water from the equilibrium mixture favors alkene formation (Le Chatelier's principle)

25. Dehydration vs Oxidation Dehydration: Remove –OH and –H –OH from one C: H from adjacent C Oxidation: Remove two –H atoms –One H from OH group: Other H from C that has the –OH attached

26. Oxidation of Alcohols Oxidation of a 1° alcohol gives an aldehyde or a carboxylic acid, depending on the experimental conditions –Oxidation of a 1° alcohol to a carboxylic acid is carried out using an oxidizing agent such as potassium dichromate, K 2 Cr 2 O 7, in aqueous sulfuric acid

27. Oxidation of Alcohols –Can sometimes stop the oxidation at the aldehyde stage by distilling the mixture (Aldehydes usually have lower boiling points than either the 1° alcohol or the carboxylic acid) Carboxylic acidAldehyde Alcohol

28. Oxidation of Alcohol –Oxidation of a 2° alcohol gives a ketone –Tertiary alcohols are resistant to oxidation

30. Common Alcohols Ethanol –Ethyl alcohol, “grain alcohol” –Produced by fermentation –Natural fermentation of sugars and starches in grains, corn, molasses, fruits, vegetables –Found in beer, wine, and other “spirits” C 6 H 12 O 6 → 2 CH 3 CH 2 OH + 2 CO 2 glucoseethanol carbon dioxide

31. Common Alcohols Methanol –Methyl alcohol or “wood alcohol” –Distilled from wood pulp originally –Very toxic, even in small amounts –Reacts to make formaldehyde (a fixative) CH 3 OH → CH 2 =O methanolformaldehyde

32. Common Alcohols Isopropyl alcohol –2-propanol “rubbing alcohol” –Evaporates quickly—used to reduce fever –Solvent in many cosmetics, perfumes, etc.

33. Common Alcohols 1,2-ethanediol –Ethylene glycol –Very soluble in water –Used as antifreeze Glycerol –1,2,3-propanetriol –Very soluble in water –Sweet taste –Part of fats and oils

34. Preparation of Important Alcohols Many alcohols (or their derivatives) can be formed by reacting smaller molecules.

35. Preparation of Important Alcohols

36. Ethers etherThe functional group of an ether is an oxygen atom bonded to two carbon atoms –Simplest ether is dimethyl ether –Most common ether is diethyl ether Often called just “ether”

37. Ether Nomenclature Generally use common names for small (low- molecular-weight) ethers –common names are derived by listing the alkyl groups bonded to oxygen in alphabetical order and adding the word "ether” –alternatively, name one of the groups on oxygen as an alkoxy group

38. Ether Nomenclature Cyclic ether:Cyclic ether: an ether in which one of the atoms in a ring is oxygen –Cyclic ethers also known by their common names –ethylene oxide is an important building block for the organic chemical industry; it is also used as a fumigant in foodstuffs and textiles, and in hospitals to sterilize surgical instruments –tetrahydrofuran is a useful laboratory and industrial solvent

40. Physical Properties of Ethers Ethers are polar compounds –O has a partial negative charge –Each C bonded to it has a partial positive charge Only weak forces of attraction exist between ether molecules in the pure liquid Boiling points of ethers are close to those of hydrocarbons of similar molecular weight Have lower boiling points than alcohols of the same molecular formula

41. Reactions of Ethers Ethers not very reactive (like hydrocarbons) –Do not react with oxidizing agents such as potassium dichromate –Do not react with reducing agents such as H 2 in the presence of a transition metal catalyst –Not affected by most acids or bases at moderate temperatures Good solvents for carrying out organic reactions, because of their general inertness and good solvent properties –Diethyl ether and THF (tetrahydrofuran)

42. Thiols Thiol:SH (sulfhydryl)groupThiol: a compound containing an -SH (sulfhydryl) group –Also called mercaptans –Low-molecular-weight thiols STINK –Responsible for smells such as those from rotten eggs and sewage –the scent of skunks is due primarily to these two thiols

43. Thiols - Nomenclature IUPAC names are derived in the same manner as are the names of alcohols -e -thiol –Retain the final -e of the parent alkane and add the suffix -thiol mercaptan –Common names for simple thiols are derived by naming the alkyl group bonded to -SH and adding the word "mercaptan"

45. Thiol Physical Properties S-H bonds are nonpolar covalent –Small difference in electronegativity between sulfur and hydrogen (2.5 - 2.1 = 0.4) –No hydrogen bonding –Lower boiling points than comparable alcohols –Less soluble in water and other polar solvents than comparable alcohols

46. Reactions of Thiols Thiols are weak acids (pK a ~10), and are comparable in strength to phenols –thiols react with strong bases such as NaOH to form water-soluble thiolate salts

47. Reactions of Thiols The most important thiol reaction in biological systems is their oxidation to disulfides disulfide(-S-S-)bond –Functional group is a disulfide (-S-S-) bond Disulfide bonds important in protein structure –Thiols are readily oxidized to disulfides by O 2 –-SH group very susceptible to oxidation and must be protected from contact with air during storage –disulfides, in turn, are easily reduced to thiols by several reducing agents.

48. Reactions of Thiols Oxidation of –SH groups to form S-S bonds Reduction of S-S bonds to form –SH groups