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In chemistry, aromaticity means a molecule has a cyclic (ring-shaped) structure with pi bonds in resonance (those containing delocalized electrons).[1] Aromatic rings give increased stability compared to saturated compounds having single bonds, and other geometric or connective non-cyclic arrangements with the same set of atoms. Aromatic rings are very stable and do not break apart easily. Organic compounds that are not aromatic are classified as aliphatic compounds—they might be cyclic, but only aromatic rings have enhanced stability. The term aromaticity with this meaning is historically related to the concept of having an aroma, but is a distinct property from that meaning.[2]
Since the most common aromatic compounds are derivatives of benzene (an aromatic hydrocarbon common in petroleum and its distillates), the word aromatic occasionally refers informally to benzene derivatives, and so it was first defined. Nevertheless, many non-benzene aromatic compounds exist. In living organisms, for example, the most common aromatic rings are the double-ringed bases (Purine) in RNA and DNA. An aromatic functional group or other substituent is called an aryl group.
In terms of the electronic nature of the molecule, aromaticity describes a conjugated system often represented in Lewis diagrams as alternating single and double bonds in a ring. In reality, the electrons represented by the double bonds in the Lewis diagram are actually distributed evenly around the ring ("delocalized"), increasing the molecule's stability. Due to the restrictions imposed by the way Lewis diagrams are drawn, the molecule cannot be represented by one diagram, but rather a hybrid of multiple different diagrams (called resonance), such as with the two resonance structures of benzene. These molecules cannot be found in either one of these representations, with the longer single bonds in one location and the shorter double bond in another (see § Theory below). Rather, the molecule exhibits all equal bond lengths, which are between those of typical single and double bonds. This commonly seen model of aromatic rings, namely the idea that benzene was formed from a six-membered carbon ring with alternating single and double bonds (cyclohexatriene), was developed by August Kekulé (see § History below). The model for benzene consists of two resonance forms, which corresponds to a superposition of double and single bonds to produce six one-and-a-half bonds. Benzene is a more stable molecule than would be expected without accounting for charge delocalization.
Theory and structure
Modern depiction of benzene
The C-C lengths in benzene are 1.40 Å, indicating it to be the average of single and double bond.[3][2] One representation is that of the circular π-bond (Armstrong's inner cycle), in which the electron density is evenly distributed through a π-bond above and below the ring.
In the language of valence bond theory, single bonds are formed from overlap of hybridized atomic sp2-orbitals in line between the carbon nuclei—these are called σ-bonds. Double bonds consist of a σ-bond and a π-bond. The π-bonds are formed from overlap of atomic p-orbitals above and below the plane of the ring. The following diagram shows the positions of these p-orbitals:
Since they are out of the plane of the atoms, these orbitals can interact with each other, allowing electrons to delocalize.
Benzene orbital delocalization
History
The term "aromatic"
The first known use of the word "aromatic" as a chemical term—namely, to apply to compounds that contain the phenyl group—occurred in an article by August Wilhelm Hofmann in 1855.[4][5] Hofmann used the term for a class of benzene compounds, many of which have odors (aromas), unlike pure saturated hydrocarbons. Aromaticity as a chemical property bears no general relationship with the olfactory properties of such compounds (how they smell), although in 1855, before the structure of benzene or organic compounds was understood, chemists like Hofmann were beginning to understand that odiferous molecules from plants, such as terpenes, had chemical properties that we recognize today are similar to unsaturated petroleum hydrocarbons like benzene. If this was indeed the earliest introduction of the term, it is curious that Hofmann says nothing about why he introduced an adjective indicating olfactory character to apply to a group of chemical substances, of which only some have notable aromas. Also, some of the most odoriferous organic substances known are terpenes, which are not aromatic in the chemical sense. Terpenes and benzenoid substances do have a chemical characteristic in common, that is, higher unsaturation than many aliphatic compounds, and Hofmann may not have made a distinction between the two categories. Many of the earliest-known examples of aromatic compounds, such as benzene and toluene, have distinctive pleasant smells. This property led to the term "aromatic" for this class of compounds, and hence the term "aromaticity" for the eventually discovered electronic property.[6][7]
The structure of the benzene ring
Historic benzene formulae as proposed by August Kekulé in 1865.[8]
The ouroboros, Kekulé's inspiration for the structure of benzene.
In the 19th century, chemists found it puzzling that benzene could be so unreactive toward addition reactions, given its presumed high degree of unsaturation. The cyclohexatriene structure for benzene was first proposed by August Kekulé in 1865.[9][10] Most chemists were quick to accept this structure, since it accounted for most of the known isomeric relationships of aromatic chemistry. The hexagonal structure explains why only one isomer of benzene exists and why disubstituted compounds have three isomers.[5]
Between 1897 and 1906, J. J. Thomson, the discoverer of the electron, proposed three equivalent electrons between each pair of carbon atoms in benzene. An explanation for the exceptional stability of benzene is conventionally attributed to Sir Robert Robinson, who was apparently the first (in 1925)[11] to coin the term aromatic sextet as a group of six electrons that resists disruption.
In fact, this concept can be traced further back, via Ernest Crocker in 1922,[12] to Henry Edward Armstrong, who in 1890 wrote "the [six] centric affinities act within a cycle … benzene may be represented by a double ring … and when an additive compound is formed, the inner cycle of affinity suffers disruption, the contiguous carbon-atoms to which nothing has been attached of necessity acquire the ethylenic condition".[13]
Here, Armstrong is describing at least four modern concepts.[verification needed] First, his "affinity" is better known nowadays as the electron, which was to be discovered only seven years later by J. J. Thomson. Second, he is describing electrophilic aromatic substitution, proceeding (third) through a Wheland intermediate, in which (fourth) the conjugation of the ring is broken. He introduced the symbol C centered on the ring as a shorthand for the inner cycle, thus anticipating Erich Clar's notation. It is argued[by whom?] that he also anticipated the nature of wave mechanics, since he recognized that his affinities had direction, not merely being point particles, and collectively having a distribution that could be altered by introducing substituents onto the benzene ring (much as the distribution of the electric charge in a body is altered by bringing it near to another body).
The quantum mechanical origins of this stability, or aromaticity, were first modelled by Hückel in 1931. He was the first to separate the bonding electrons into sigma and pi electrons.
Aromaticity of an arbitrary aromatic compound can be measured quantitatively by the nucleus-independent chemical shift (NICS) computational method[14] and aromaticity percentage[15] methods.
Characteristics of aromatic systems
An aromatic (or aryl) ring contains a set of covalently bound atoms with specific characteristics:
A delocalized conjugated π system, most commonly an arrangement of alternating single and double bonds
Coplanar structure, with all the contributing atoms in the same plane
Contributing atoms arranged in one or more rings
A number of π delocalized electrons that is even, but not a multiple of 4. That is, 4n + 2 π-electrons, where n = 0, 1, 2, 3, and so on. This is known as Hückel's rule.
According to Hückel's rule, if a molecule has 4n + 2 π-electrons, it is aromatic, but if it has 4n π-electrons and has characteristics 1–3 above, the molecule is said to be antiaromatic. Whereas benzene is aromatic (6 electrons, from 3 double bonds), cyclobutadiene is antiaromatic, since the number of π delocalized electrons is 4, which of course is a multiple of 4. The cyclobutadienide(2−) ion, however, is aromatic (6 electrons). An atom in an aromatic system can have other electrons that are not part of the system, and are therefore ignored for the 4n + 2 rule. In furan, the oxygen atom is sp2 hybridized. One lone pair is in the π system and the other in the plane of the ring (analogous to the C–H bond in the other positions). There are 6 π-electrons, so furan is aromatic.
Aromatic molecules typically display enhanced chemical stability, compared with similar non-aromatic molecules. A molecule that can be aromatic will tend to change toward aromaticity, and the added stability changes the chemistry of the molecule. Aromatic compounds undergo electrophilic aromatic substitution and nucleophilic aromatic substitution reactions, but not electrophilic addition reactions as happens with carbon–carbon double bonds.
In the presence of a magnetic field, the circulating π-electrons in an aromatic molecule produce an aromatic ring current that induces an additional magnetic field, an important effect in nuclear magnetic resonance.[16] The NMR signal of protons in the plane of an aromatic ring are shifted substantially further down-field than those on non-aromatic sp2 carbons. This is an important way of detecting aromaticity. By the same mechanism, the signals of protons located near the ring axis are shifted upfield.
Aromatic molecules are able to interact with each other by a type of π interaction called π–π stacking. The π systems form two parallel rings overlap in a "face-to-face" orientation. Aromatic molecules are also able to interact with each other in an "edge-to-face" orientation: The slight positive charge of the substituents on the ring atoms of one molecule are attracted to the slight negative charge of the aromatic system on another molecule.
Planar monocyclic molecules containing 4n π-electrons are called antiaromatic and are, in general, unstable. Molecules that could be antiaromatic will tend to change from this electronic or conformation, thereby becoming non-aromatic. For example, cyclooctatetraene (COT) distorts out of planarity, breaking π overlap between adjacent double bonds. Recent studies have determined that cyclobutadiene adopts an asymmetric, rectangular configuration in which single and double bonds indeed alternate, with no resonance; the single bonds are markedly longer than the double bonds, reducing unfavorable p-orbital overlap. This reduction of symmetry lifts the degeneracy of the two formerly non-bonding molecular orbitals, which by Hund's rule forces the two unpaired electrons into a new, weakly bonding orbital (and also creates a weakly antibonding orbital). Hence, cyclobutadiene is non-aromatic; the strain of the asymmetric configuration outweighs the anti-aromatic destabilization that would afflict the symmetric, square configuration.
Hückel's rule of aromaticity treats molecules in their singlet ground states (S0). The stability trends of the compounds described here are found to be reversed in the lowest lying triplet and singlet excited states (T1 and S1), according to Baird's rule. This means that compounds like benzene, with 4n + 2 π-electrons and aromatic properties in the ground state, become antiaromatic and often adopt less symmetric structures in the excited state.[17]
Compounds
Main article: Aromatic compound
Neutral homocyclics
Benzene, as well as most other annulenes with the formula C4n+2H4n+2 where n is a natural number, such as cyclotetradecaheptaene (n=3). Many chemical compounds are aromatic rings with other functional groups attached. Examples include trinitrotoluene (TNT), acetylsalicylic acid (aspirin), paracetamol, and the nucleotides of DNA.
Heterocyclics
In heterocyclic aromatics (heteroaromatics), one or more of the atoms in the ring is an element other than carbon. The scope is large as it includes benzannulated analogs.
Prominent "aromatic heterocycles" have these parents: pyridine, pyrazine, pyrrole, imidazole, pyrazole, oxazole, and thiophene. In all these examples, the number of π-electrons is 6, due to the π-electrons from the double bonds as well as the electrons from the heteroatoms. Although these compounds are planar and have 6-pi electrons, they are less aromatic than benzene, often significantly less.[18]
Electron counting in pyridine follows: the five sp2-hybridized carbons each contribute one π-electron to the pi-system. The nitrogen atom, which is also sp2-hybridized, also contribute one electron to the p-orbital, resulting in a total of 6 p-electrons. By this arithmetic, pyridine is aromatic. The lone pair on the nitrogen is not part of the aromatic π system.
Electron counting in pyrrole follows: the four sp2-hybridized carbons each contributes one π-electron. The nitrogen atom, which is also sp2-hybridized, also contributes two π-electrons from its lone pair.
Electron counting in imidazole follows the pattern seen for pyridine and pyrrole: one N center contributes one pair and the two-coordinate N center contributes one electron.[19]
Fused aromatics and polycyclics
Polycyclic aromatic hydrocarbons are molecules containing two or more simple aromatic rings fused together by sharing two neighboring carbon atoms. Examples are naphthalene, anthracene, and phenanthrene. In fused aromatics, not all carbon–carbon bonds are necessarily equivalent, as the electrons are not delocalized over the entire molecule. The aromaticity of these molecules can be explained using their orbital picture. Like benzene and other monocyclic aromatic molecules, polycyclics have a cyclic conjugated pi system with p-orbital overlap above and below the plane of the ring.[19]
Aromatic ions
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Aromatic molecules need not be neutral molecules. Ions that satisfy Huckel's rule of 4n + 2 π-electrons in a planar, cyclic, conjugated molecule are considered to be aromatic ions. For example, the cyclopentadienyl anion and the cycloheptatrienylium cation are both considered to be aromatic ions, and the azulene molecule can be approximated as a combination of both.
In order to convert the atom from sp3 to sp2, a carbocation, carbanion, or carbon radical must be formed. These leave sp2-hybridized carbons that can partake in the π system of an aromatic molecule. Like neutral aromatic compounds, these compounds are stable and form easily. The cyclopentadienyl anion is formed very easily and thus 1,3-cyclopentadiene is a very acidic hydrocarbon with a pKa of 16.[19] Other examples of aromatic ions include the cyclopropenium cation (2 π-electrons) and cyclooctatetraenyl dianion (10 π electrons).
Atypical aromatic compounds
Aromaticity also occurs in rings consisting only of chemical elements that are not carbon. Inorganic six-membered-ring compounds analogous to benzene have been synthesized. For example, borazine is a six-membered ring composed of alternating boron and nitrogen atoms, each with one hydrogen atom attached to each atom of the ring. It has a delocalized π system and undergoes electrophilic substitution reactions appropriate to aromatic rings rather than reactions expected of non-aromatic molecules.[20]
Quite recently, the aromaticity of planar Si6−
5 rings occurring in the Zintl phase Li12Si7 was experimentally evinced by Li solid-state NMR.[21][non-primary source needed] Metal aromaticity is believed to exist in certain clusters of aluminium and gallium, specifically Ga32- and Al42-, for example.[22]
Homoaromaticity is the state of systems where conjugation is interrupted by a single sp3 hybridized carbon atom.[23]
Y-aromaticity is used to describe a Y-shaped, planar (flat) molecule with resonance bonds. The concept was developed to explain the extraordinary stability and high basicity of the guanidinium cation. Guanidinium is not a ring molecule, and is cross-conjugated rather than a π system of consecutively attached atoms, but is reported to have its six π-electrons delocalized over the whole molecule. The concept is controversial and some authors emphasize different effects.[24][25][26] This has also been suggested as the reason that the trimethylenemethane dication is more stable than the butadienyl dication.[27]
σ-aromaticity refers to stabilization arising from the delocalization of sigma bonds. It is often invoked in cluster chemistry and is closely related to Wade's Rule. Furthermore, in 2021 a σ-aromatic Th3 complex was reported, indicating that the concept of σ-aromaticity remains relevant for orbitals with principle quantum number 6.[28]
Other symmetries
See also: Antiaromaticity
Type Cyclic symmetry Electron rule Occurrence
Hückel aromaticity Cylindrical 4n + 2 Aromatic rings
Möbius aromaticity Möbius 4n Trans aromatic rings
Spherical aromaticity Spherical 2(n+1)2 Fullerenes
Möbius aromaticity occurs when a cyclic system of molecular orbitals, formed from pπ atomic orbitals and populated in a closed shell by 4n (n is an integer) electrons, is given a single half-twist to form a Möbius strip. A π system with 4n electrons in a flat (non-twisted) ring would be antiaromatic, and therefore highly unstable, due to the symmetry of the combinations of p atomic orbitals. By twisting the ring, the symmetry of the system changes and becomes allowed (see also Möbius–Hückel concept for details). Because the twist can be left-handed or right-handed, the resulting Möbius aromatics are dissymmetric or chiral. But as of 2012, no Möbius aromatic molecules had been synthesized.[29][30] Aromatics with two half-twists corresponding to the paradromic topologies were first suggested by Johann Listing.[31] In one form of carbo-benzene, the ring is expanded and contains alkyne and allene groups.
Spherical aromaticity is aromaticity that occurs in fullerenes. In 2000, Andreas Hirsch and coworkers in Erlangen, Germany, formulated a rule to determine when a fullerene would be aromatic. They found that if there were 2(n + 1)2 π-electrons, then the fullerene would display aromatic properties. This follows from the fact that an aromatic fullerene must have full icosahedral (or other appropriate) symmetry, so the molecular orbitals must be entirely filled. This is possible only if there are exactly 2(n + 1)2 electrons, where n is a nonnegative integer.
See also
Wikiquote has quotations related to Aromaticity.
Look up aromaticity in Wiktionary, the free dictionary.
Aromatization
Aromatic amine
List of benzo compounds
Avoided crossing
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