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22.5: Acidity of Alpha Hydrogen Atoms: Enolate Ion Formation

  • Page ID
    36416
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    Objectives

    After completing this section, you should be able to

    1. explain why the alpha hydrogens of carbonyl compounds are more acidic than the hydrogens in a typical hydrocarbon.
    2. list the properties that make lithium diisopropylamide a suitable reagent for converting a wide range of carbonyl compounds into their enolate anions.
    3. arrange a given list of carbonyl compounds in order of increasing or decreasing acidity.
    4. determine whether a given carbonyl‑containing compound is more or less acidic than selected other compounds, such as water, ammonia, alcohols, alkanes, alkenes, alkynes and amines.
    5. explain why dicarbonyl compounds, such as β‑diketones, are more acidic than compounds that contain only a single carbonyl group.
    Key Terms

    Make certain that you can define, and use in context, the key terms below.

    • β‑diketone
    • β‑keto ester

    α hydrogens are weakly acidic because the conjugate base, called an enolate, is stabilized though conjugation with the π orbitals of the adjacent carbonyl. Removal of an α-hydrogen creates an sp2 hybridized enolate carbon with a negative charge and lone pair electrons contained in an unhybridized p orbital. Orbital overlap with the adjacent p orbitals from the carbonyl pi bond allows for the lone pair electrons and negative charge to be shared with the electronegative oxygen, stabilizing the enolate ion.

     

    Enolate conjugation can be represent by two major resonance forms represented by structure A and B which share the negative charge. In structure A the negative charge is on carbon while structure B has the negative change on oxygen.

    Enolate Resonance.svg

    Structure A is preferred because oxygen is highly electronegative and better able to stabilize the negative charge. Both resonance structures contribute to an overall resonance hybrid but not equally. Due to its stability, structure A makes a greater contribution to the resonance hybrid structure. Structure A’s increased contribution to the hybrid is seen when considering the electrostatic potential map of the enolate of acetone. The red/yellow color shows there is a high electron density around the oxygen. The yellow/green color around the enolate carbon shows that there is a lower but still significant electron density. Notice that the electron density on the enolate carbon is much larger than the non-enolate carbon (blue color).

    Enolate Hybrid ESD.jpg

    The effect of an adjacent carbonyl on acidity is seen when comparing the α-hydrogen pKa of aldehydes (~16-18) and ketones (~19-21) the to the pKa of an alkane (~50). Also, the importance of the electronegative oxygen is seen when considering the pKa of an allyl C-H bond which means a C-H bond adjacent to a C=C double bond (~42). Although the conjugate base is stabilized through conjugation, the stability gained only provides a 108 increase in acidity. In comparison, the presence of an oxygen in the carbonyl increases the acidity of an α-hydrogen by 1020 times.

    PKa Al and Ket.svg

     

    Double Bond Resonance.svg

    Although α-hydrogens are weakly acidic, typical strong bases such as hydroxide or alkoxide are only capable of forming the enolate ion in very low concentrations. This leaves a significant concentration of the electrophilic carbonyl remaining, which can react with the bases or the enolate. To achieve complete deprotonation of aldehyde or ketone reactants to their enolate conjugate bases, a very strong base such as LDA (lithium diisopropylamide) must be used. Complete deprotonation removes the carbonyl compounds from the reaction mixture and prevents their ability to form unwanted products. Also, the large alkyl substituents sterically hinder the ability of LDA and its corresponding amine (diisopropyl amine) to undergo nucleophilic addition to the carbonyl. Ether solvents like tetrahydrofuran (THF) are commonly used for enolate formation reactions using LDA. Certain other strong bases, such as alkyl lithium and Grignard reagents, cannot be used to make enolate anions because they rapidly and irreversibly add to carbonyl groups. Nevertheless, these very strong bases are useful in the preparation of LDA. By reacting n-butyllithium with diisopropylamine (pKa 36), LDA can be easily formed.

    LDA formation.png

    Example

    Deprotonation Cyclohexanone.png

    Hydrogen atoms with two or more adjacent carbonyl groups are more acidic than typical α hydrogens.

    Acidity diketones.png

    The enolate ions of compound such as β-diketones, β-keto-esters, and β-diesters are stabilized through additional resonance forms which share the negative charge with multiple carbonyl carbons. The acidity of these compounds is increased to the point where weaker bases, such as sodium ethoxide (NaOCH2CH3) can be used to form the enolate.

    In addition to aldehydes and ketones, LDA readily deprotonates a wide variety of carbonyl containing functional groups including esters, amides and nitriles. The pka and acidic hydrogens of multiple functional groups are shown in the table below.

    * = a funtional group with two ketones.

    Functional Group Structure pKa
    carboxylic acid HO–(C=O)R 5
    nitro RCH2–NO2 9
    β-diketone * R(O=C)–CH2–(C=O)R 9
    β-ketoester * R(O=C)–CH2–(C=O)OR 11
    β-diester * RO(O=C)–CH2–(C=O)OR 13
    amide RNH–(C=O)R 15
    alcohol RCH2–OH 16
    aldehyde RCH2–(C=O)H 17
    ketone RCH2–(C=O)R 20
    thioester RCH2–(C=O)SR 21
    ester RCH2–(C=O)OR 25
    nitrile RCH2–C≡N 25
    sulfone RCH2–SO2R 25
    amide RCH2–(C=O)N(CH3)2 30
    alkane CH3–R 50

    22.5: Acidity of Alpha Hydrogen Atoms: Enolate Ion Formation is shared under a CC BY-SA 4.0 license and was authored, remixed, and/or curated by Steven Farmer, Dietmar Kennepohl, Layne Morsch, William Reusch, & William Reusch.