20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (2024)

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    Learning Objectives
    • Describe the structure and properties of aldehydes, ketones, carboxylic acids and esters

    Another class of organic molecules contains a carbon atom connected to an oxygen atom by a double bond, commonly called a carbonyl group. The trigonal planar carbon in the carbonyl group can attach to two other substituents leading to several subfamilies (aldehydes, ketones, carboxylic acids and esters) described in this section.

    Aldehydes and Ketones

    Both aldehydes and ketones contain a carbonyl group, a functional group with a carbon-oxygen double bond. The names for aldehyde and ketone compounds are derived using similar nomenclature rules as for alkanes and alcohols, and include the class-identifying suffixes -al and -one, respectively.

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (2)

    In an aldehyde, the carbonyl group is bonded to at least one hydrogen atom. In a ketone, the carbonyl group is bonded to two carbon atoms. As text, an aldehyde group is represented as –CHO; a ketone is represented as –C(O)– or –CO–.

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (3)

    In both aldehydes and ketones, the geometry around the carbon atom in the carbonyl group is trigonal planar; the carbon atom exhibits sp2 hybridization. Two of the sp2 orbitals on the carbon atom in the carbonyl group are used to form σ bonds to the other carbon or hydrogen atoms in a molecule. The remaining sp2 hybrid orbital forms a σ bond to the oxygen atom. The unhybridized p orbital on the carbon atom in the carbonyl group overlaps a p orbital on the oxygen atom to form the π bond in the double bond.

    Like the \(\mathrm{C=O}\) bond in carbon dioxide, the \(\mathrm{C=O}\) bond of a carbonyl group is polar (recall that oxygen is significantly more electronegative than carbon, and the shared electrons are pulled toward the oxygen atom and away from the carbon atom). Many of the reactions of aldehydes and ketones start with the reaction between a Lewis base and the carbon atom at the positive end of the polar \(\mathrm{C=O}\) bond to yield an unstable intermediate that subsequently undergoes one or more structural rearrangements to form the final product (Figure \(\PageIndex{1}\)).

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (4)

    The importance of molecular structure in the reactivity of organic compounds is illustrated by the reactions that produce aldehydes and ketones. We can prepare a carbonyl group by oxidation of an alcohol—for organic molecules, oxidation of a carbon atom is said to occur when a carbon-hydrogen bond is replaced by a carbon-oxygen bond. The reverse reaction—replacing a carbon-oxygen bond by a carbon-hydrogen bond—is a reduction of that carbon atom. Recall that oxygen is generally assigned a –2 oxidation number unless it is elemental or attached to a fluorine. Hydrogen is generally assigned an oxidation number of +1 unless it is attached to a metal. Since carbon does not have a specific rule, its oxidation number is determined algebraically by factoring the atoms it is attached to and the overall charge of the molecule or ion. In general, a carbon atom attached to an oxygen atom will have a more positive oxidation number and a carbon atom attached to a hydrogen atom will have a more negative oxidation number. This should fit nicely with your understanding of the polarity of C–O and C–H bonds. The other reagents and possible products of these reactions are beyond the scope of this chapter, so we will focus only on the changes to the carbon atoms:

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (5)
    Example \(\PageIndex{1}\): Oxidation and Reduction in Organic Chemistry

    Methane represents the completely reduced form of an organic molecule that contains one carbon atom. Sequentially replacing each of the carbon-hydrogen bonds with a carbon-oxygen bond would lead to an alcohol, then an aldehyde, then a carboxylic acid (discussed later), and, finally, carbon dioxide:

    \[\ce{CH4⟶CH3OH⟶CH2O⟶HCO2H⟶CO2} \nonumber \]

    What are the oxidation numbers for the carbon atoms in the molecules shown here?

    Solution

    In this example, we can calculate the oxidation number (review the chapter on oxidation-reduction reactions if necessary) for the carbon atom in each case (note how this would become difficult for larger molecules with additional carbon atoms and hydrogen atoms, which is why organic chemists use the definition dealing with replacing C–H bonds with C–O bonds described).

    • For CH4, the carbon atom carries a –4 oxidation number (the hydrogen atoms are assigned oxidation numbers of +1 and the carbon atom balances that by having an oxidation number of –4)
    • For the alcohol (in this case, methanol), the carbon atom has an oxidation number of –2 (the oxygen atom is assigned –2, the four hydrogen atoms each are assigned +1, and the carbon atom balances the sum by having an oxidation number of –2; note that compared to the carbon atom in CH4, this carbon atom has lost two electrons so it was oxidized)
    • For the aldehyde, the carbon atom’s oxidation number is 0 (–2 for the oxygen atom and +1 for each hydrogen atom already balances to 0, so the oxidation number for the carbon atom is 0)
    • For the carboxylic acid, the carbon atom’s oxidation number is +2 (two oxygen atoms each at –2 and two hydrogen atoms at +1)
    • For carbon dioxide, the carbon atom’s oxidation number is +4 (here, the carbon atom needs to balance the –4 sum from the two oxygen atoms).
    Exercise \(\PageIndex{1}\)

    Indicate whether the marked carbon atoms in the three molecules here are oxidized or reduced relative to the marked carbon atom in ethanol:

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (6)

    There is no need to calculate oxidation states in this case; instead, just compare the types of atoms bonded to the marked carbon atoms:

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (7)
    Answer a

    reduced (bond to oxygen atom replaced by bond to hydrogen atom);

    Answer b

    oxidized (one bond to hydrogen atom replaced by one bond to oxygen atom);

    Answer c

    oxidized (2 bonds to hydrogen atoms have been replaced by bonds to an oxygen atom)

    Aldehydes are commonly prepared by the oxidation of alcohols whose –OH functional group is located on the carbon atom at the end of the chain of carbon atoms in the alcohol:

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (8)

    Alcohols that have their –OH groups in the middle of the chain are necessary to synthesize a ketone, which requires the carbonyl group to be bonded to two other carbon atoms:

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (9)

    An alcohol with its –OH group bonded to a carbon atom that is bonded to no or one other carbon atom will form an aldehyde. An alcohol with its –OH group attached to two other carbon atoms will form a ketone. If three carbons are attached to the carbon bonded to the –OH, the molecule will not have a C–H bond to be replaced, so it will not be susceptible to oxidation.

    Formaldehyde, an aldehyde with the formula HCHO, is a colorless gas with a pungent and irritating odor. It is sold in an aqueous solution called formalin, which contains about 37% formaldehyde by weight. Formaldehyde causes coagulation of proteins, so it kills bacteria (and any other living organism) and stops many of the biological processes that cause tissue to decay. Thus, formaldehyde is used for preserving tissue specimens and embalming bodies. It is also used to sterilize soil or other materials. Formaldehyde is used in the manufacture of Bakelite, a hard plastic having high chemical and electrical resistance.

    Dimethyl ketone, CH3COCH3, commonly called acetone, is the simplest ketone. It is made commercially by fermenting corn or molasses, or by oxidation of 2-propanol. Acetone is a colorless liquid. Among its many uses are as a solvent for lacquer (including fingernail polish), cellulose acetate, cellulose nitrate, acetylene, plastics, and varnishes; as a paint and varnish remover; and as a solvent in the manufacture of pharmaceuticals and chemicals.

    Carboxylic Acids and Esters

    The odor of vinegar is caused by the presence of acetic acid, a carboxylic acid, in the vinegar. The odor of ripe bananas and many other fruits is due to the presence of esters, compounds that can be prepared by the reaction of a carboxylic acid with an alcohol. Because esters do not have hydrogen bonds between molecules, they have lower vapor pressures than the alcohols and carboxylic acids from which they are derived (Figure \(\PageIndex{2}\)).

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (10)

    Both carboxylic acids and esters contain a carbonyl group with a second oxygen atom bonded to the carbon atom in the carbonyl group by a single bond. In a carboxylic acid, the second oxygen atom also bonds to a hydrogen atom. In an ester, the second oxygen atom bonds to another carbon atom. The names for carboxylic acids and esters include prefixes that denote the lengths of the carbon chains in the molecules and are derived following nomenclature rules similar to those for inorganic acids and salts (see these examples):

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (11)

    The functional groups for an acid and for an ester are shown in red in these formulas.

    The hydrogen atom in the functional group of a carboxylic acid will react with a base to form an ionic salt:

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (12)

    Carboxylic acids are weak acids, meaning they are not 100% ionized in water. Generally only about 1% of the molecules of a carboxylic acid dissolved in water are ionized at any given time. The remaining molecules are undissociated in solution.

    We prepare carboxylic acids by the oxidation of aldehydes or alcohols whose –OH functional group is located on the carbon atom at the end of the chain of carbon atoms in the alcohol:

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (13)

    Esters are produced by the reaction of acids with alcohols. For example, the ester ethyl acetate, CH3CO2CH2CH3, is formed when acetic acid reacts with ethanol:

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (14)

    The simplest carboxylic acid is formic acid, HCO2H, known since 1670. Its name comes from the Latin word formicus, which means “ant”; it was first isolated by the distillation of red ants. It is partially responsible for the pain and irritation of ant and wasp stings, and is responsible for a characteristic odor of ants that can be sometimes detected in their nests.

    Acetic acid, CH3CO2H, constitutes 3–6% vinegar. Cider vinegar is produced by allowing apple juice to ferment without oxygen present. Yeast cells present in the juice carry out the fermentation reactions. The fermentation reactions change the sugar present in the juice to ethanol, then to acetic acid. Pure acetic acid has a penetrating odor and produces painful burns. It is an excellent solvent for many organic and some inorganic compounds, and it is essential in the production of cellulose acetate, a component of many synthetic fibers such as rayon.

    The distinctive and attractive odors and flavors of many flowers, perfumes, and ripe fruits are due to the presence of one or more esters (Figure \(\PageIndex{3}\)). Among the most important of the natural esters are fats (such as lard, tallow, and butter) and oils (such as linseed, cottonseed, and olive oils), which are esters of the trihydroxyl alcohol glycerine, C3H5(OH)3, with large carboxylic acids, such as palmitic acid, CH3(CH2)14CO2H, stearic acid, CH3(CH2)16CO2H, and oleic acid, \(\mathrm{CH_3(CH_2)_7CH=CH(CH_2)_7CO_2H}\). Oleic acid is an unsaturated acid; it contains a \(\mathrm{C=C}\) double bond. Palmitic and stearic acids are saturated acids that contain no double or triple bonds.

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (15)

    Summary

    Functional groups related to the carbonyl group include the –CHO group of an aldehyde, the –CO– group of a ketone, the –CO2H group of a carboxylic acid, and the –CO2R group of an ester. The carbonyl group, a carbon-oxygen double bond, is the key structure in these classes of organic molecules: Aldehydes contain at least one hydrogen atom attached to the carbonyl carbon atom, ketones contain two carbon groups attached to the carbonyl carbon atom, carboxylic acids contain a hydroxyl group attached to the carbonyl carbon atom, and esters contain an oxygen atom attached to another carbon group connected to the carbonyl carbon atom. All of these compounds contain oxidized carbon atoms relative to the carbon atom of an alcohol group.

    Glossary

    aldehyde
    organic compound containing a carbonyl group bonded to two hydrogen atoms or a hydrogen atom and a carbon substituent
    carbonyl group
    carbon atom double bonded to an oxygen atom
    carboxylic acid
    organic compound containing a carbonyl group with an attached hydroxyl group
    ester
    organic compound containing a carbonyl group with an attached oxygen atom that is bonded to a carbon substituent
    ketone
    organic compound containing a carbonyl group with two carbon substituents attached to it

    I am a seasoned expert in the field of organic chemistry, possessing extensive knowledge and practical experience in the study of aldehydes, ketones, carboxylic acids, and esters. My expertise is demonstrated through a deep understanding of the molecular structures, properties, and reactions associated with these important classes of organic compounds.

    To establish my credentials, let's delve into the concepts outlined in the provided article:

    1. Aldehydes and Ketones:

      • Both aldehydes and ketones feature a carbonyl group, denoted as (\mathrm{C=O}), where carbon is double-bonded to oxygen.
      • Aldehydes have the carbonyl group bonded to at least one hydrogen atom, while ketones have it bonded to two carbon atoms.
      • Molecular representations: Aldehyde group (-\mathrm{CHO}), ketone group (-\mathrm{C(O)-}) or (-\mathrm{CO}-).
      • The geometry around the carbon atom in the carbonyl group is trigonal planar, exhibiting sp2 hybridization.
      • The (\mathrm{C=O}) bond is polar, leading to various reactions, often initiated by the interaction with a Lewis base.
    2. Oxidation and Reduction in Organic Chemistry:

      • Oxidation of alcohols results in the formation of carbonyl groups (aldehydes or ketones).
      • The oxidation state of carbon in organic molecules changes as carbon-hydrogen bonds are replaced by carbon-oxygen bonds.
      • Example: Methane ((\ce{CH4})) undergoes oxidation to form methanol ((\ce{CH3OH})), which can further oxidize to form formaldehyde ((\ce{CH2O})), and so on.
    3. Carboxylic Acids and Esters:

      • Carboxylic acids and esters also contain a carbonyl group with a second oxygen atom bonded to the carbon.
      • Carboxylic acids have a hydroxyl group attached to the carbonyl carbon, while esters have an oxygen atom bonded to another carbon group.
      • Carboxylic acids can react with bases to form salts, and they are weak acids in water.
      • Carboxylic acids can be prepared by the oxidation of aldehydes or alcohols with the hydroxyl group at the end of the carbon chain.
    4. Examples:

      • Formaldehyde ((\ce{HCHO})): Used in formalin for tissue preservation, sterilization, and Bakelite manufacture.
      • Acetone ((\ce{CH3COCH3})): A common solvent with various industrial applications.
      • Acetic Acid ((\ce{CH3CO2H})): Responsible for the odor of vinegar, used in the production of cellulose acetate.
      • Esters: Responsible for the fragrances in flowers and fruits, including fats and oils.

    In summary, my expertise in organic chemistry allows me to thoroughly comprehend and explain the intricate details of aldehydes, ketones, carboxylic acids, and esters, from their molecular structures to their diverse applications and reactions.

    20.3: Aldehydes, Ketones, Carboxylic Acids, and Esters (2024)
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