Lactone

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Lactones are cyclic esters of hydroxycarboxylic acids, containing a 1-oxacycloalkan-2-one structure, or analogues having unsaturation or heteroatoms replacing one or more carbon atoms of the ring.[1]

Lactones are formed by intramolecular esterification of the corresponding hydroxycarboxylic acids, which takes place spontaneously when the ring that is formed is five- or six-membered. Lactones with three- or four-membered rings (α-lactones and β-lactones) are very reactive, making their isolation difficult. Special methods are normally required for the laboratory synthesis of small-ring lactones as well as those that contain rings larger than six-membered.[2]

Nomenclature[edit]

Lactone nomenclature: α-acetolactone, β-propiolactone, γ-butyrolactone, and δ-valerolactone

Lactones are usually named according to the precursor acid molecule (aceto = 2 carbons, propio = 3, butyro = 4, valero = 5, capro = 6, etc.), with a -lactone suffix and a Greek letter prefix that specifies the number of carbons in the heterocyle — that is, the distance between the relevant -OH and the -COOH groups along said backbone. The first carbon atom after the carbon in the -COOH group on the parent compound is labelled α, the second will be labeled β, and so forth. Therefore, the prefixes also indicate the size of the lactone ring: α-lactone = 3-membered ring, β-lactone = 4-membered, γ-lactone = 5-membered, etc.

The other suffix used to denote a lactone is -olide, used in substance class names like butenolide, macrolide, cardenolide or bufadienolide.

Etymology[edit]

The name lactone derives from the ring compound called lactide, which is formed from the dehydration of 2-hydroxypropanoic acid (lactic acid) CH3-CH(OH)-COOH. Lactic acid, in turn, derives its name from its original isolation from soured milk (Latin: lac, lactis). An internal dehydration within the same molecule of lactic acid would have produced alpha-propiolactone, a lactone with a 3-membered ring.

Natural sources[edit]

Naturally occuring lactones are mainly saturated and unsaturated γ- and δ-lactones, and to a lesser extent macrocyclic lactones. The γ- and δ-lactones are intramolecular esters of the corresponding hydroxy fatty acids. They contribute to the aroma of butter, cheese and various foods and fruits. Cyclopentadecanolide is responsible for the musklike odor of angelica root oil. Of the naturally occurring bicyclic lactones, phthalides are responsible for the odors of celery and lovage oils, and coumarin for woodruff.[3]

Lactone rings occur widely as building blocks in nature, such as in ascorbic acid, kavain, nepetalactone, gluconolactone, hormones (spironolactone, mevalonolactone), enzymes (lactonase), neurotransmitters (butyrolactone, avermectins), antibiotics (macrolides like erythromycin; amphotericin B), anticancer drugs (vernolepin, damsin, epothilones), phytoestrogens (resorcylic acid lactones, cardiac glycosides).

Synthesis[edit]

Oxandrolone Synthesis

Many methods in ester synthesis can also be applied to that of lactones. In one industrial synthesis of oxandrolone the key lactone-forming step is an organic reduction - esterification.[4][5]

iodolactonization

In halolactonization, an alkene is attacked by a halogen via electrophilic addition with the cationic intermediate captured intramolecularly by an adjacent carboxylic acid (See also iodolactamization).[6]

Specific methods include Yamaguchi esterification, Baeyer–Villiger oxidation and nucleophilic abstraction.

γ-Lactone synthesis from fatty alcohols and acrylic acid

The γ-lactones γ-octalactone, γ-nonalactone, γ-decalactone, γ-undecalactone can be prepared in good yield in a one-step process by radical addition of primary fatty alcohols to acrylic acid, using di-tert-butyl peroxide as a catalyst.[3]

Reactions[edit]

The most stable structure for lactones are the 5-membered γ-lactones and 6-membered δ-lactones because, as in all organic cycles, 5 and 6 membered rings minimize the strain of bond angles. γ-lactones are so stable that, in the presence of dilute acids at room temperature, 4-hydroxy acids (R-CH(OH)-(CH2)2-COOH) immediately undergo spontaneous esterification and cyclisation to the lactone. β-lactones do exist, but can only be made by special methods. α-lactones can be detected as transient species in mass spectrometry experiments.[7]

The reactions of lactones are similar to those of esters, as exemplified by gamma-lactone in the following sections:

Hydrolysis[edit]

Heating a lactone with a base (sodium hydroxide) will hydrolyse the lactone to its parent compound, the straight chained bifunctional compound. Like straight-chained esters, the hydrolysis-condensation reaction of lactones is a reversible reaction, with an equilibrium. However, the equilibrium constant of the hydrolysis reaction of the lactone is lower than that of the straight-chained ester i.e. the products (hydroxyacids) are less favored in the case of the lactones. This is because although the enthalpies of the hydrolysis of esters and lactones are about the same, the entropy of the hydrolysis of lactones is less than the entropy of straight-chained esters. Straight-chained esters give two products upon hydrolysis, making the entropy change more favorable than in the case of lactones which give only a single product.

Reduction[edit]

Lactones can be reduced to diols using lithium aluminium hydride in dry ether. The reduction reaction will first break the ester bond of the lactone, and then reduce the carboxylic acid group (-COOH) to the alcohol group (-OH). For instance, gamma-lactones will be reduced to butan-1,4-diol, (CH2(OH)-(CH2)2-CH2(OH).

Aminolysis[edit]

Lactones also react with ethanolic ammonia, which will first break the ester bond and then react with the acidic -COOH group, because of the basic properties of ammonia, to form a difunctional group, i.e. alcohol and amide. Gamma-lactones will react to yield CH2(OH)-(CH2)2-CO-NH2.

Polymerization[edit]

Lactones readily form polyesters according to the formula:[8]

Lactone polymerization.png

Michael reaction[edit]

Sesquiterpene lactones, found in many plants, can react with other molecules via a Michael reaction.

Uses[edit]

Flavors and fragrances[edit]

Lactones are used as flavors and fragrances, e. g., γ-octalactone, γ-nonalactone, γ-decalactone, γ-undecalactone, δ-decalactone.[3]

Macrocyclic lactones (cyclopentadecanolide, 15-pentadec-11/12-enolide) have odors similar to macrocyclic ketones of animal origin (muscone, civetone), but they can be prepared more easily, for example, by depolymerization of the corresponding linear polyesters. Replacement of a methylene unit by oxygen barely affects the odor of these compounds, and oxalactones with 15 – 17-membered rings are produced in addition to cyclopentadecanolide (e. g., 12-oxa-16-hexadecanolide).[3]

Plastics[edit]

Polycaprolactone is an important plastic.

Examples[edit]

dilactones[edit]

See also[edit]

References & notes[edit]

  1. ^ "lactones", Compendium of Chemical Terminology, 2.3.3, International Union of Pure and Applied Chemistry, 2014-02-24, p. 817 
  2. ^ Francis A. Carey; Robert M. Giuliano (2011), Organic Chemistry (8th ed.), McGraw-Hill, pp. 798–799 
  3. ^ a b c d Karl-Georg Fahlbusch et al. (2007), "Flavors and Fragrances", Ullmann's Encyclopedia of Industrial Chemistry (7th ed.), Wiley, pp. 74‒78 
  4. ^ Development of a Commercial Process to Produce Oxandrolone John E. Cabaj, David Kairys, and Thomas R. Benson Org. Process Res. Dev.; 2007; 11(3) pp 378 - 388; (Article) doi:10.1021/op060231b
  5. ^ The complete reaction sequence is bromination to a haloketone (not displayed), elimination reaction with lithium chloride to an enone, organic oxidation by osmiumtetroxide and lead tetraacetate with ring-opening and finally reduction of the aldehyde to the alcohol with sodium borohydride and intramolecular lactone formation
  6. ^ Organic Syntheses, Coll. Vol. 7, p.164 (1990); Vol. 64, p.175 (1986) Article link.
  7. ^ Detlef Schröder, Norman Goldberg, Waltraud Zummack, Helmut Schwarz, John C. Poutsma and Robert R. Squires (1997), Generation of α-acetolactone and the acetoxyl diradical •CH2COO• in the gas phase. International Journal of Mass Spectrometry and Ion Processes, Volumes 165-166, November issue, Pages 71-82. doi:10.1016/S0168-1176(97)00150-X
  8. ^ Wilhelm Riemenschneider; Hermann M. Bolt (2007), "Esters, Organic", Ullmann's Encyclopedia of Industrial Chemistry (7th ed.), Wiley