In this chapter, we will concentrate on reactions where the nucleophile is an oxygen or nitrogen. Carbonyl compounds with leaving groups have reactions similar to aldehydes and ketones. The main difference is the presence of an electronegative substituent that can act as a leaving group during a nucleophile substitution reaction. Although there are many types of carboxylic acid derivatives known, this article focuses on four: acid halides, acid anhydrides, esters, and amides. Although aldehydes and ketones also contain carbonyls, their chemistry is distinctly different because they do not contain suitable leaving groups.
Once a tetrahedral intermediate is formed, aldehydes and ketones cannot reform their carbonyls. Because of this, aldehydes and ketones typically undergo nucleophilic additions and not substitutions. Aldehydes and ketones are widespread in nature, often combined with other functional groups.
Example are shown in the following diagram. The compounds in the top row are found chiefly in plants or microorganisms; those in the bottom row have animal origins. With the exception of the first three compounds top row these molecular structures are all chiral. When chiral compounds are found in nature they are usually enantiomerically pure, although different sources may yield different enantiomers. For example, carvone is found as its levorotatory R -enantiomer in spearmint oil, whereas, caraway seeds contain the dextrorotatory S -enantiomer.
Note that the aldehyde function is often written as —CHO in condensed or complex formulas. Aldehydes and ketones are obtained as products from many reactions discussed in previous sections of this text.
The following diagram summarizes the most important of these. To review the previous discussion of any of these reaction classes simply click on the number 1 to 5 or descriptive heading for the group. With the exception of Friedel-Crafts acylation, these methods do not increase the size or complexity of molecules. In the following sections of this chapter we shall find that one of the most useful characteristics of aldehydes and ketones is their reactivity toward carbon nucleophiles, and the resulting elaboration of molecular structure that results.
In short, aldehydes and ketones are important intermediates for the assembly or synthesis of complex organic molecules. A comparison of the properties and reactivity of aldehydes and ketones with those of the alkenes is warranted, since both have a double bond functional group. Because of the greater electronegativity of oxygen, the carbonyl group is polar, and aldehydes and ketones have larger molecular dipole moments D than do alkenes.
The resonance structures on the right illustrate this polarity, and the relative dipole moments of formaldehyde, other aldehydes and ketones confirm the stabilizing influence that alkyl substituents have on carbocations the larger the dipole moment the greater the polar character of the carbonyl group. We expect, therefore, that aldehydes and ketones will have higher boiling points than similar sized alkenes.
Furthermore, the presence of oxygen with its non-bonding electron pairs makes aldehydes and ketones hydrogen-bond acceptors, and should increase their water solubility relative to hydrocarbons.
Specific examples of these relationships are provided in the following table. For a review of the intermolecular forces that influence boiling points and water solubility Click Here. Compound Mol. The polarity of the carbonyl group also has a profound effect on its chemical reactivity, compared with the non-polar double bonds of alkenes. Thus, reversible addition of water to the carbonyl function is fast, whereas water addition to alkenes is immeasurably slow in the absence of a strong acid catalyst.
Curiously, relative bond energies influence the thermodynamics of such addition reactions in the opposite sense. This suggests that addition reactions to carbonyl groups should be thermodynamically disfavored, as is the case for the addition of water.
Although the addition of water to an alkene is exothermic and gives a stable product an alcohol , the uncatalyzed reaction is extremely slow due to a high activation energy. The reverse reaction dehydration of an alcohol is even slower, and because of the kinetic barrier, both reactions are practical only in the presence of a strong acid.
The microscopically reversible mechanism for both reactions was described earlier. In contrast, both the endothermic addition of water to a carbonyl function, and the exothermic elimination of water from the resulting geminal -diol are fast. The inherent polarity of the carbonyl group, together with its increased basicity compared with alkenes , lowers the transition state energy for both reactions, with a resulting increase in rate.
Acids and bases catalyze both the addition and elimination of water. Proof that rapid and reversible addition of water to carbonyl compounds occurs is provided by experiments using isotopically labeled water. If a carbonyl reactant composed of 16 O colored blue above is treated with water incorporating the 18 O isotope colored red above , a rapid exchange of the oxygen isotope occurs. This can only be explained by the addition-elimination mechanism shown here. It has been demonstrated above that water adds rapidly to the carbonyl function of aldehydes and ketones.
In most cases the resulting hydrate a geminal-diol is unstable relative to the reactants and cannot be isolated. Exceptions to this rule exist, one being formaldehyde a gas in its pure monomeric state. Here the weaker pi-component of the carbonyl double bond, relative to other aldehydes or ketones, and the small size of the hydrogen substituents favor addition.
Thus, a solution of formaldehyde in water formalin is almost exclusively the hydrate, or polymers of the hydrate. Similar reversible additions of alcohols to aldehydes and ketones take place. The equally unstable addition products are called hemiacetals. Stable Hydrates and Hemiacetals To see examples of exceptional aldehydes and ketones that form stable hydrates or hemiacetals Click Here.
Acetals are geminal-diether derivatives of aldehydes or ketones, formed by reaction with two equivalents of an alcohol and elimination of water. Ketone derivatives of this kind were once called ketals, but modern usage has dropped that term. The following equation shows the overall stoichiometric change in acetal formation, but a dashed arrow is used because this conversion does not occur on simple mixing of the reactants.
In order to achieve effective acetal formation two additional features must be implemented. First, an acid catalyst must be used; and second, the water produced with the acetal must be removed from the reaction.
The latter is important, since acetal formation is reversible. Indeed, once pure acetals are obtained they may be hydrolyzed back to their starting components by treatment with aqueous acid. The mechanism shown here applies to both acetal formation and acetal hydrolysis by the principle of microscopic reversibility. Some examples of acetal formation are presented in the following diagram. Two equivalents of the alcohol reactant are needed, but these may be provided by one equivalent of a diol example 2.
Intramolecular involvement of a gamma or delta hydroxyl group as in examples 3 and 4 may occur, and is often more facile than the intermolecular reaction. Thiols sulfur analogs of alcohols give thioacetals example 5. In this case the carbonyl functions are relatively hindered, but by using excess ethanedithiol as the solvent and the Lewis acid BF 3 as catalyst a good yield of the bis-thioacetal is obtained.
Thioacetals are generally more difficult to hydrolyze than are acetals. The importance of acetals as carbonyl derivatives lies chiefly in their stability and lack of reactivity in neutral to strongly basic environments. As long as they are not treated by acids, especially aqueous acid, acetals exhibit all the lack of reactivity associated with ethers in general.
Among the most useful and characteristic reactions of aldehydes and ketones is their reactivity toward strongly nucleophilic and basic metallo-hydride, alkyl and aryl reagents to be discussed shortly. If the carbonyl functional group is converted to an acetal these powerful reagents have no effect; thus, acetals are excellent protective groups, when these irreversible addition reactions must be prevented.
Water is eliminated in the reaction, which is acid-catalyzed and reversible in the same sense as acetal formation. An addition-elimination mechanism for this reaction was proposed, and an animation showing this mechanism is activated by the button.
Imines are sometimes difficult to isolate and purify due to their sensitivity to hydrolysis. Some of these reagents are listed in the following table, together with the structures and names of their carbonyl reaction products. An interesting aspect of these carbonyl derivatives is that stereoisomers are possible when the R-groups of the carbonyl reactant are different. Thus, benzaldehyde forms two stereoisomeric oximes, a low-melting isomer, having the hydroxyl group cis to the aldehyde hydrogen called syn , and a higher melting isomer in which the hydroxyl group and hydrogen are trans the anti isomer.
Amount of positive charge on the electrophile is an important factor that influences reactivity. Factors that place more positive charge on the carbonyl electron withdrawing groups nearby make the carbonyl more positive and more reactive.
Factors that place additional electron density on the carbonyl electron donors nearby make the carbonyl less reactive. There is another resonance structure that we can think about that illustrates the electrophilicity of a carbonyl. That structure places a full negative charge on the oxygen and a full positive charge on the carbon. Nevertheless, when taken together with the regular Lewis structure, it suggests something real about the nature of the carbonyl: there is partial positive charge on the carbon and partial negative charge on the oxygen.
There is a general rule about cation stability on carbon atoms: a carbocation with more carbons attached to it is more stable than a carbocation with more hydrogens attached to it. This observation is sometimes explained as an inductive effect.
The positively charged carbon is more electronegative than the uncharged carbons, so it draws electrons away from them. It can polarize the neighbouring carbons, drawing some negative charge towards itself and leaving some positive charge on the other carbons.
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