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Historically, aromatic compounds referred to any compound producing a fragrant smell, such as benzaldehydes which produce the scent of cherries, peaches, and almonds. However, some aromatic compounds were later discovered that do not exhibit this property. Therefore, aromatic compounds are currently classified according to their chemical behavior.
Biologically relevant examples of aromatic compounds
Classification of aromatic compounds
Aromatic compounds are a large family of compounds comprised of a six-membered ring or more complex structure. Notably, aromatic compounds are not limited to hydrocarbons as there are aromatic compounds like thiophene and pyridine which have S and N in their structure. Ions can also be considered aromatic as long as they exhibit the properties noted above.
Compounds are classified as aromatic if they are able to exhibit the following properties:
- The molecule is cyclic and contain conjugated high or low electron density areas.
- The molecule is very stable compared to their aliphatic counterparts.
- The molecule is planar to allow easier delocalization of the π electrons.
- All atoms in the cycle contain a p-orbital for overlap.
- The molecule follows the Huckel 4n + 2 π electron rule where n should be an integer.
The compound is considered to be aromatic if it is able to exhibit all of the properties included in the list. Otherwise, the compound can be classified as either a non-aromatic or anti-aromatic compound.
An aromatic compound is considered a big family of compounds as it comprises of compounds with a six-membered ring, to more complex structures. Aromatic compounds are also not limited to hydrocarbons as there are also aromatic compounds like thiophene and pyridine that are considered aromatic, even if they have S and N in their structure. Ions can also be considered as aromatic, as long as it will exhibit the properties included above.
Biologically relevant examples of aromatic compounds
Steroids are aromatic compounds which are important to biological organisms and include hormones responsible for growth and the development of physical features. In the pharmaceutical industry, compounds such as atorvastatin, a cholesterol-lowering drug, are also aromatic. Pyridine, C5H5N, is a common aromatic compound present in vitamins and other pharmaceuticals. Most of the essential vitamins we need are also aromatic. Benzene, the most common aromatic compound, is used in manufacturing polystyrene plastics, pesticides, and some pharmaceutical drugs.
Benzene is a hydrocarbon with the molecular formula C6H6 and has a cyclic structure with alternating or conjugated double bonds. Although benzene is unsaturated, it does not exhibit the relative reactivity of its other alkene and acyclic counterparts. For example, cyclohexene readily reacts with Br2 to produce 1,2-dibromocyclohexane. Conversely, benzene reacts very slowly with Br2 to form bromobenzene which still retains the presence of three double bonds, demonstrating the relative stability of benzene.
Another important observation is the bond lengths in a benzene molecule. In ordinary compounds, single bonds are expected to be longer than double bonds. However, the bond length analysis of benzene shows that the C to C bond lengths are all equal, regardless of being a single or double bond. The bond angle in each C-C-C segment is 120°, forming a perfect hexagon shape. The electrostatic potential map shows that the electron density is identical in all six carbon-carbon bonds. Each carbon also has a p-orbital that lies perpendicular to the plane of the six-membered ring.
Because of the peculiar properties of benzene, each double bond is not considered to be localized, but rather, overlapping to only one other p-orbital. These properties are only possible if the compound has all p-orbitals equally overlapping adjacent p-orbitals. This overlap of orbitals enables delocalization of the 6 π electrons around the ring. Because of this, it is difficult to isolate the two possible isomers of benzene. Instead, a circle is included inside the 6 sides of the molecule to indicate delocalization of the π electrons.
Electrophilic Aromatic Substitution Reaction
Electrophilic aromatic substitution (EAS) occurs when an electrophile reacts with an aromatic ring, substituting one of the H atoms in the ring. A number of different electrophiles may be used in EAS. Possible electrophiles include halogens (-Cl, -Br, -I), the sulfonic acid group (-SO3H), hydroxyl group (-OH), nitro group (-NO2), acyl groups (-COR), and alkyl groups (-R). Even with benzene alone, one can come up with some compounds because of the number of possible electrophiles for the reaction.
Aromatic compounds, unlike ordinary alkenes, are less reactive compared to their acyclic counterparts due to their relative stability afforded by π electron delocalization. In a halogenation reaction known as bromination, Br2 can readily react with ethane to produce dibromoethane. This is not true for benzene. For the bromination reaction to proceed in benzene, a catalyst such as FeBr3 is needed which provides a different mechanism for the reaction to proceed.
The 1st step in the reaction is the polarization of the Br2 molecule by FeBr3. In the process, a more electrophilic molecule is produced in the form of FeBr4– Br+. The presence of Br+ makes FeBr4– Br+ more electrophilic than an ordinary Br2 molecule. The FeBr4– Br+ will then attack the benzene molecule and a base will remove the proton in the process. Below is the mechanism of the reaction:
Nitration of aromatic rings can be achieved using a mixture of concentrated nitric and sulfuric acids. The electrophile in the reaction is the nitronium ion, NO2+, which is produced by the protonation and loss of water in the form of HNO3. Just as in halogenation, a carbocation intermediate is produced when the nitronium ion interacts with the benzene ring. Upon loss of a proton, the neutral substitution product nitrobenzene is produced. Below is the basic mechanism for the nitration of benzene:
Sulfonation of Benzene
A sulfonation reaction of aromatic rings is achieved by reacting benzenes with fuming sulfuric acid (a mixture of H2SO4 and SO3). The electrophile for the reaction is either HSO3+ or neutral SO3, depending on the reaction conditions. This reaction mechanism is similar to the bromination and nitration reactions previously discussed. A sulfonation reaction is favored in the presence of strong acids, while desulfonation is favored in hot, dilute aqueous acids. The mechanism for sulfonation is as follow:
A hydroxylation reaction of aromatic rings is very difficult to achieve in ordinary reaction conditions and requires the presence of biological enzymes. An example of a hydroxylation reaction catalyzed through a biological pathway is the hydroxylation of p-hydroxyphenylacetate using the enzyme p-hydroxyphenylacetate-3-hydroxylase to produce 3,4-dihydroxyphenylacetate. The process requires molecular oxygen plus the coenzyme-reduced flavin adenine dinucleotide, FADH2.
An alkylation reaction proceeds when an alkylchloride is combined with AlCl3. AlCl3 enables the dissociation of R-X to produce the carbocation that will serve as the electrophile. The electrophile then attacks the benzene ring and the reaction is completed by proton loss. The mechanism of the reaction is shown below:
The mechanism of the acylation reaction is similar to the alkylation reaction. The alkyl halide is just replaced by an acyl halide. For example, for the acylation reaction of benzene, the first step is the generation of a strong electrophile by the interaction between the acyl chloride and the AlCl3 molecule. The acyl cation is then stabilized by rearrangement in the acyl cation with the + charge present in the C atom. The +C then interacts with the double bond in the benzene molecule, forming a carbocation that can be stabilized by abstracting one of the protons using the AlCl4– ion produced in the first step. The mechanism for acylation is shown in the figure below:
The correct answers can be found below the references.
- Conjugated double bond
- All atoms in the cycle contain a p-orbital.
- Huckel rule (4n + 2 π electrons)