Carbonyl reduction

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Oxidation ladders such as this one are used to illustrate sequences of carbonyls which can be interconverted through oxidations or reductions. Redox ladder.png
Oxidation ladders such as this one are used to illustrate sequences of carbonyls which can be interconverted through oxidations or reductions.

In organic chemistry, carbonyl reduction is the conversion of any carbonyl group, usually to an alcohol. It is a common transformation that is practiced in many ways. [1] Ketones, aldehydes, carboxylic acids, esters, amides, and acid halides - some of the most pervasive functional groups, -comprise carbonyl compounds. Carboxylic acids, esters, and acid halides can be reduced to either aldehydes or a step further to primary alcohols, depending on the strength of the reducing agent. Aldehydes and ketones can be reduced respectively to primary and secondary alcohols. In deoxygenation, the alcohol group can be further reduced and removed altogether by replacement with H.

Contents

Two broad strategies exist for carbonyl reduction. One method, which is favored in industry, uses hydrogen as the reductant. This approach is called hydrogenation and requires metal catalysts. The other broad approach employs stoichiometric reagents that deliver H− and H+ separately. This article focuses on the use of these reagents. Prominent among these reagents are the alkali metal salts of borohydrides and aluminium hydrides.

General considerations

Resonance structures of different carbonyls, ordered from most stable (least reactive) to least stable (most reactive) Carbonyl resonance.png
Resonance structures of different carbonyls, ordered from most stable (least reactive) to least stable (most reactive)

In terms of reaction mechanism, metal hydrides effect nucleophilic addition of hydride to the carbonyl carbon. The ease of addition of hydride to the carbonyl is affected by electrophilicity and bulk of the carbonyl as well as the corresponding electronic and steric properties of the hydride reagent. The result of these trends is that acid halides, ketones, and aldehydes are usually the most readily reduced compounds, while acids and esters require stronger reducing agents. Importantly and characteristically, these hydride reagents generally do not attack C=C bonds. [2]

Several factors contribute to the strength of metal hydride reducing agents. The reducing power of borohydride reagents is affected by the counter ion, such as Na+ vs Li+ which can activate carbonyls by coordinating to the carbonyl oxygen. Li+ binds to carbonyl oxygen more strongly than does Na+. [3] In the case of tetrahydroaluminates, however, NaAlH4 and LiAlH4 behave similarly. [2] Many metal additives have been investigated. For example, zinc borohydride, nominally Zn(BH4)2, is used for mild selective reduction of aldehydes and ketones in the presence of other reducible groups. [4]

The central metal (usually B vs Al) strongly influences reducing agent's strength. Aluminum hydrides are more nucleophilic and better reducing agents relative to borohydrides. [5] The relatively weak reducer sodium borohydride is typically used for reducing ketones and aldehydes. It tolerates many functional groups (nitro group, nitrile, ester). [6]

In their handling properties, lithium aluminium hydride and sodium borohydride (and their derivatives) strongly differ. NaBH4 is far easier to handle than LiAlH4, being air stable for weeks. It can be used with water or ethanol as solvents, whereas LiAlH4 reacts explosively with protic solvents.

Substituents on the boron or aluminium modulate the power, selectivity, and handling properties of these reducing agents. Electron-withdrawing groups such as acetoxy and cyano lower the reducing power such that NaBH(OAc)3 and NaBH3(CN) are weak reducing agents. Electron-donating groups such as alkyl groups enhance the reducing strength. superhydride (lithium triethylborohydride) and L-selectride are strong reductant. They are correspondingly hazardous to handle.

The following table [7] illustrates which carbonyl functional groups can be reduced by which reducing agents (some of these reagents vary in efficacy depending on reaction conditions):

Table of possible reactions between carbonyl groups and reducing agents Hydride reduction table.png
Table of possible reactions between carbonyl groups and reducing agents

Substrates

Carboxylic acid and esters

Relative to aldehydes and ketones, carboxylic acid are difficult to reduce. Lithium aluminium hydride is typically effective. The first step involves deprotonation of the carboxylic acid. The final step in the reduction of carboxylic acids and esters is hydrolysis of the aluminium alcoxide. [8] Esters (and amides) are more easily reduced than the parent carboxylic acids. Their reduction affords alcohols and amines, respectively. [9] The idealized equation for the reduction of an ester by lithium aluminium hydride is:

2 RCO2R' + LiAlH4 → LiAl(OCH2R)2(OR')
LiAl(OCH2R)2(OR') + 4 H2O → LiAl(OH)4 + 2 HOCH2R + 2 HOR'

Sodium borohydride can, under some circumstances, be used for ester reduction, especially with additives. [1]

Forming aldehydes from carboxylic acid derivatives is challenging because weaker reducing agents (NaBH4) are often very slow at reducing esters and carboxylic acids, whereas stronger reducing agents (LiAlH4) immediately reduce the formed aldehyde to an alcohol. [10]

Conversion to thioester followed by Fukuyama reduction Fukuyama scheme.png
Conversion to thioester followed by Fukuyama reduction

In the Fukuyama reduction, a carboxylic acid is first converted to a thioester through addition of a thiol (with a mechanism similar to esterification). [11] The thioester is then reduced to an aldehyde by a silyl hydride with a palladium catalyst.

Acid chlorides to aldehydes

Acid chlorides can be reduced to give aldehydes with sterically hindered hydride donors. The reducing agent DIBAL-H (diisobutylaluminium hydride) is often used for this purpose, although it normally reduces any carbonyl. DIBAL-H can selectively reduce acid chlorides to the aldehyde level if only one equivalent is used at low temperatures. [12] LiAlH(OtBu)3 (formed from LiAlH4 and tBuOH in situ) behaves similarly. [13] The idealized equation for the reduction of an acid chloride to an aldehyde by lithium aluminium hydride is:

RCOCl + LiAlH(OtBu)3 → LiCl + "Al(OtBu)3" + RCHO

The traditional method of forming aldehydes without reducing to alcohols - by using hindered hydrides and reactive carbonyls - is limited by its narrow substrate scope and great dependence on reaction conditions. One workaround to avoid this method is to reduce the carboxylic acid derivative all the way down to an alcohol, then oxidize the alcohol back to an aldehyde. Other alternatives include forming a thioester or a Weinreb amide, then reducing the new species to an aldehyde through the Fukuyama reduction or Weinreb reaction respectively, or using catalytic hydrogenation as in the Rosenmund reaction.

In the Weinreb ketone synthesis, an acyl chloride is first converted to the Weinreb amide, then treated with an organometallic reagent to form a ketone, or lithium aluminum hydride to form an aldehyde: [14]

Weinreb scheme.png

The Weinreb amide is reduced via a stable chelate, rather than the electrophilic carbonyl that is formed through metal hydride reductions; the chelate is therefore only reduced once, as illustrated below:

Weinreb mechanism.png

The Rosenmund reaction reduces acyl chlorides to aldehydes using hydrogen gas with a catalyst of palladium on barium sulfate, whose small surface area prevents over-reduction. [15]

Aldehydes and ketones

Ketones are less reactive than aldehydes, because of greater steric effects, and because the extra alkyl group contributes electron density to the C=O bond, making it less electrophilic. [16] Since, aldehydes reduce more easily than ketones, they require milder reagents and milder conditions. At the other extreme, carboxylic acids, amides, and esters are poorly electrophilic and require strong reducing agents. [17]

The idealized equation for the reduction of a ketone by sodium borohydride is:

4 RCOR' + NaBH4 → NaB(OCHRR')4
NaB(OCHRR')4) + 4 H2O → "NaB(OH)4" + 4 HOCHRR' + 4 HOR'
Complete idealized mechanism for the reduction of ketone with sodium borohydride. Ketone reduction via sodium borohydride.svg
Complete idealized mechanism for the reduction of ketone with sodium borohydride.

Reductive amination

RedveAm.svg

In addition to their reduction to alcohols, aldehydes and ketones can be converted to amines, i.e., reductive amination. [18] Because of its cyano substituent, NaBH3CN is a weak reducer at moderate pH (>4), so it preferentially reduces iminium cations that exist in the presence of carbonyls:

α,β-unsaturated carbonyls

1,4 vs 1,2 reduction.png

When an α,β-unsaturated carbonyl is reduced, three products can result: an allyl alcohol from simple carbonyl reduction, a saturated ketone or aldehyde resulting from 1,4‑reduction (also called conjugate reduction), or the saturated alcohol from double reduction. [19] Use of NaBH4 can give any of these results, but InCl3 or NiCl2 catalyze specifically 1,4‑reductions. [1] Potassium or lithium tri(sec‑butyl)­borohydride sometimes selects 1,4‑reductions, but can be stymied by steric hindrance. [20] Triphenylphosphino­copper hydride clusters directs catalytic hydrogenation to perform specifically conjugate reduction.

To selectively form the allyl alcohol and avoid the 1,4 product, the Luche reduction uses "cerium borohydride" generated in situ from NaBH4 and CeCl3(H2O)7 [21] [22] The hydride source Zn(BH4)2 also shows 1,2 selectivity, as well as greater diastereoselectivity. It does so by coordinating not only to the carbonyl oxygen but also to adjacent atoms: [23]

Zinc borohydride.png

Hydrogenolysis

A special case of carbonyl reduction entails complete deoxygenation, i.e. hydrogenolysis. This result is often undesirable because it involves defunctionalization.

Some reactions for this transformation include the Clemmensen reduction (in strongly acidic conditions) and the Wolff–Kishner reduction (in strongly basic conditions), as well as the various modifications of Wolff-Kishner reaction. The Caglioti modification, for instance, uses tosylhydrazone with a hydride donor in milder conditions with no base; [24] the Myers modification substitutes hydrazine with bis(tert-butyldimethylsilyl)-hydrazine, uses milder conditions at room temperature, and is rapid and efficient. [25]

Mechanism of Wolff-Kishner reduction Wolff-Kishner mechanism-s.png
Mechanism of Wolff-Kishner reduction

Aromatic carbonyls are more readily reduced to their respective alkanes than aliphatic compounds. [26] For example, ketones are reduced to their respective alkyl benzenes by catalytic hydrogenation [27] [28] or by Birch reduction [29] under mild conditions.

Stereoselectivity

Diastereoselective reduction

In the reduction of cyclohexanones, the hydride source can attack axially to produce an equatorial alcohol, or equatorially to produce an axial alcohol. In axial attack (shown in red), the hydride encounters 1,3-diaxial strain. In equatorial attack (shown in blue), the hydride avoids the 1,3-diaxial interaction, but the substrate undergoes unfavorable torsional strain when the newly formed alcohol and added hydrogen atom eclipse each other in the reaction intermediate (as shown in the Newman projection for the axial alcohol).

Axial vs equatorial.png

Large reducing agents, such as LiBH(Me2CHCHMe)3, are hindered by the 1,3-axial interactions and therefore attack equatorially. [6] Small reducing agents, such as NaBH4, preferentially attack axially in order to avoid the eclipsing interactions, because the 1,3-diaxial interaction for small molecules is minimal; stereoelectronic reasons have also been cited for small reducing agents' axial preference. [30] Making the substrate bulkier (and increasing 1,3-axial interactions), however, decreases the prevalence of axial attacks, even for small hydride donors. [31]

Enantioselective reduction

When asymmetrical ketones are reduced, the resulting secondary alcohol has a chiral center whose can be controlled using chiral transition states or catalysts. In the Evans-Saksena reduction, a nearby alcohol directs the reduction.

Well-known carbonyl reductions in asymmetric synthesis are the Noyori asymmetric hydrogenation (beta-ketoester reduction/Ru/BINAP) and the CBS reduction (BH3, proline derived chiral catalyst).

History and alternative methods

The Bouveault–Blanc reduction, employing a mixture of sodium metal in the presence of alcohols, was an early method for reduction of carbonyls. [32] It is now largely obsolete. Subsequent to the discovery of the Bouveault–Blanc reduction, many methods were developed, including the major breakthrough of catalytic hydrogenation where H2 serves as the reductant. [33] Salts boron and aluminium hydrides, discovered starting in the 1940s, proved to be highly convenient reagents for carbonyl reduction.

In the Meerwein-Ponndorf-Verley reduction, aluminium isopropoxide functions as the hydride source. The status of this reaction has been summarized thusly "the synthetic organic chemist will rarely attempt to use such a conventional technique as the Meerwein−Ponndorf−Verley (MPV) reaction". [34]

See also

Related Research Articles

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<span class="mw-page-title-main">Diborane</span> Chemical compound

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<span class="mw-page-title-main">Lithium aluminium hydride</span> Chemical compound

Lithium aluminium hydride, commonly abbreviated to LAH, is an inorganic compound with the chemical formula Li[AlH4] or LiAlH4. It is a white solid, discovered by Finholt, Bond and Schlesinger in 1947. This compound is used as a reducing agent in organic synthesis, especially for the reduction of esters, carboxylic acids, and amides. The solid is dangerously reactive toward water, releasing gaseous hydrogen (H2). Some related derivatives have been discussed for hydrogen storage.

<span class="mw-page-title-main">Sodium borohydride</span> Chemical compound

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<span class="mw-page-title-main">Organic redox reaction</span> Redox reaction that takes place with organic compounds

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<span class="mw-page-title-main">Diisobutylaluminium hydride</span> Chemical compound

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<span class="mw-page-title-main">Sodium cyanoborohydride</span> Chemical compound

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<span class="mw-page-title-main">Lithium triethylborohydride</span> Chemical compound

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<span class="mw-page-title-main">Sodium aluminium hydride</span> Chemical compound

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4 anions.

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<span class="mw-page-title-main">Sodium triacetoxyborohydride</span> Chemical compound

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References

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