Name: cyclopentadienyl anion and aromaticity
Uploaded: 2023-04-30T10:31:23.000Z
Duration: 1 min 18 s
Channel: JoVE

Obojętne monocykliczne nienasycone węglowodory o nieparzystej liczbie atomów węgla nie mają aromatyczności ze względu na obecność w pierścieniu węgla sp3.
Na przykład cyklopentadien nie jest aromatyczny, ponieważ ma tylko 4 elektrony π i węgiel sp3, który zakłóca ciągłe nakładanie się orbitali p.
Warto zauważyć, że usunięcie wodoru z grupyCH2 z obydwoma, jednym lub żadnym z elektronów wiążących przekształca węgiel sp3 w sp2, generując odpowiednio kation, rodnik i anion.
W porównaniu do kationu i rodnika tylko anion ma wymaganą liczbę (4n + 2) π elektronów.
Co więcej, dostępność orbitalu 2p na węglu sp2 ułatwia ciągłe nakładanie się orbitali p i delokalizację ładunku ujemnego w całym pierścieniu, dzięki czemu anion cyklopentadienylu jest aromatyczny.
Dodatkowo, elektrony π zajmujące wiążące orbitale molekularne i pięć struktur rezonansowych dodatkowo potwierdzają niezwykłą stabilność anionu aromatycznego.

aniony węglowodorów aromatycznych: przegląd strukturalny

Aromatic Hydrocarbon Anions: Structural Overview

Węglowodory obojętne, takie jak cyklopentadien, z nieparzystą liczbą atomów węgla i jedną grupą CH_2 w pierścieniu, nie są aromatyczne. 

Cyklopentadien z 4 elektronami π nie spełnia reguły elektronów 4n + 2 π. Dodatkowo znajdująca się pomiędzy nimi grupa CH_2 ma hybrydyzację sp^3 i brakuje jej wolnego orbitalu p, co przerywa w sposób ciągły nakładanie się orbitali p i zapobiega delokalizacji elektronów π w całym pierścieniu.

Ze względu na brak ciągłego nakładania się orbitali p, cyklopentadien nie spełnia kryteriów aromatyczności. Jednakże usunięcie jednego wodoru z obydwoma lub jednym elektronem lub bez elektronów z grupy CH_2 powoduje konwersję węgla sp^3 do sp^2, przekształcając w ten sposób cyklopentadien odpowiednio w kation, rodnik i anion cyklopentadienylu, mające wolny orbital p. Spośród wszystkich trzech gatunków kation cyklopentadienylowy i rodnik odpowiednio z czterema i pięcioma elektronami π nie spełniają kryteriów 4n + 2 elektronów π i nie są aromatyczne. Z drugiej strony anion cyklopentadienylowy z 6 elektronami π, ciągłym nakładającym się pierścieniem orbitali p i zdelokalizowaną gęstością elektronów π staje się aromatyczny. Mapa potencjału elektrostatycznego anionu potwierdza delokalizację elektronów π w całym pierścieniu. Ponadto, pięć struktur rezonansowych anionu cyklopentadienylowego i zajęcie orbitali molekularnych wiążących przez wszystkie 6 elektronów π na diagramie mrozu potwierdzają niezwykłą stabilność anionu.

Aniony węglowodorów aromatycznych: przegląd strukturalny

Neutralne węglowodory, takie jak cyklopentadien, z nieparzystą liczbą atomów węgla i jedną pośrednią grupą CH2 w pierścieniu, nie są aromatyczne. Cyklopentadien ...

aromatic-hydrocarbon-anions-structural-overview

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Organic Chemistry

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Aromatic Compounds

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cyclopentadienyl anion and aromaticity

Cyclopentadiene is a neutral hydrocarbon that is not aromatic. It contains an odd number of carbon atoms and one CH2 group in the ring. With only 4 pi electrons, it does not follow the 4n + 2 pi electron rule. The CH2 carbon is sp3 hybridized, so it has no vacant p orbital to keep p orbitals overlapped around the ring.

That break in overlap stops pi electrons from spreading across the entire ring. As a result, cyclopentadiene does not meet the usual aromaticity criteria. If one hydrogen is removed from the CH2 group, the carbon changes from sp3 to sp2 hybridization. This creates a vacant p orbital and gives three related species: the cyclopentadienyl cation, radical, and anion.

These three species do not behave the same way. The cyclopentadienyl cation has 4 pi electrons, and the radical has 5 pi electrons. Neither one satisfies the 4n + 2 rule, so neither is aromatic. The cyclopentadienyl anion has 6 pi electrons, a continuous ring of overlapping p orbitals, and delocalized pi electron density. That makes it aromatic and unusually stable.

The electrostatic potential map of the anion supports this electron delocalization across the ring. Its five resonance structures also show how the electrons can be spread out. The frost diagram gives the same result, since all 6 pi electrons fill bonding molecular orbitals. Together, these features explain why the cyclopentadienyl anion is more stable than the neutral ring, the cation, or the radical.

Cyclopentadienyl Anion and Aromaticity

aromatic compounds: overview

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Aromatic compounds are linked to both pleasant smells and important chemical structures. The word aromatic first came from fragrant natural sources such as fresh flowers and spices. Early organic chemists isolated benzene derivatives from oils of plants, including vanillin from vanilla, methyl salicylate from wintergreen, and cinnamaldehyde from cinnamon. The history of benzene also helped shape the idea of aromatic compounds. In 1825, Faraday isolated benzene from compressed illuminating gas,...

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Benzene derivatives with one substituent are named by attaching the substituent name to benzene. Benzene is the simplest aromatic hydrocarbon, also called an arene. For simple monosubstituted benzene compounds, IUPAC naming uses the group name as a prefix. Halogen-substituted benzene compounds follow this pattern. The halogen prefix can be fluoro, chloro, bromo, or iodo. When an alkyl group is attached to the benzene ring, the name depends on the chain length of that group. If the alkyl chain...

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Naming benzene rings with multiple groups depends on how many substituents are attached. For benzene derivatives with two groups, three constitutional isomers are possible. The position of each group is described with IUPAC naming rules. For disubstituted benzene compounds, the relative positions can be shown with ortho, meta, and para. These terms are also written as o, m, and p. They can also be written with numbers, such as 1,2- for ortho, 1,3- for meta, and 1,4- for para. Dimethyl benzene,...

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Kekule’s benzene model describes benzene as a six-carbon ring with alternating pi bonds. August Kekule proposed this structure in 1865 from the formula C6H6, the idea that all benzene hydrogens are equivalent, and the rule that each carbon has four bonds because of tetravalency. In this model, each carbon is attached to one hydrogen atom. It also predicts two isomers for 1,2-disubstituted benzene derivatives. In one form, the substituted carbons are linked by a double bond, and in the other...

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Benzene has a planar ring structure with delocalized π electrons. Its six carbon atoms form a regular hexagon, and each carbon is sp2 hybridized. The C–C–C and H–C–C bond angles are 120°, which matches the flat shape of the ring. Each carbon is bonded to three other atoms. The C–H bond length is 109 pm, and the C–C bond length is 139 pm. That C–C distance is midway between the single bond length of sp3 hybridized carbons, 154 pm, and the sp2 value, 133 pm. Beneath and above the ring plane,...

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H&uuml;ckel Rule and Aromatic Ring Criteria

Aromatic rings follow H&amp;uuml;ckel’s rule, also called the 4n + 2 rule. This rule helps identify which unsaturated cyclic compounds are aromatic and why some ring systems are unstable instead. Benzene is the classic example, while cyclobutadiene and cyclooctatetraene show different behavior and are not aromatic. Eric H&amp;uuml;ckel, a German chemical physicist, first described the structural features needed for aromaticity. An aromatic compound must be cyclic, planar, and continuously...

h&uuml;ckel's rule diagram of &pi; mos: frost circle

Frost Circle for Pi Orbital Energies

The Frost circle is a graphical method for showing the relative energies of pi molecular orbitals in planar, fully conjugated, monocyclic compounds. It is also called the inscribed polygon method. A. A. Frost and Boris Musulin first described this method in 1953. To build a Frost circle, draw a polygon with the same number of edges as the number of carbons in the cyclic system. Place one vertex pointing downward. Then draw a circle around the polygon so that every vertex touches the circle.

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Frost circles help test whether a cyclic compound is aromatic by using the inscribed polygon method and Hückel’s 4n + 2 rule. A compound is stable and aromatic when every bonding molecular orbital (MO) is completely filled with a pair of electrons. If electrons occupy non-bonding or antibonding orbitals, the compound is unstable and not aromatic. Frost circle diagrams for cycloalkenes with 4 to 8 carbons show a clear pattern. The number of bonding MOs is always odd. The electrons needed to...

aromatic hydrocarbon anions: structural overview

Cyclopentadiene is a neutral hydrocarbon that is not aromatic. It contains an odd number of carbon atoms and one CH2 group in the ring. With only 4 pi electrons, it does not follow the 4n + 2 pi electron rule. The CH2 carbon is sp3 hybridized, so it has no vacant p orbital to keep p orbitals overlapped around the ring. That break in overlap stops pi electrons from spreading across the entire ring. As a result, cyclopentadiene does not meet the usual aromaticity criteria. If one hydrogen is...

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Cycloheptatrienyl Cation and Aromaticity

Cycloheptatriene is a neutral monocyclic unsaturated hydrocarbon with seven carbon atoms. One carbon in the ring is sp3 hybridized, which breaks the continuous overlap of p orbitals. Even though the ring has three double bonds and 6 π electrons, cycloheptatriene is not aromatic because the p orbitals do not form one uninterrupted loop. Removing one hydrogen from the CH2 group changes the ring. If that hydrogen is removed with both, one, or no electrons, the products are the cycloheptatrienyl...

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Five-Membered Aromatic Rings with Heteroatoms

Five-membered aromatic rings with heteroatoms are cyclic compounds that contain one or more atoms other than carbon in the ring. They are aromatic and can have either five or six atoms in the ring. Common examples include pyrrole, furan, thiophene, and imidazole. These rings differ by the heteroatom present. Pyrrole has one nitrogen atom with one lone pair of electrons. Furan has one oxygen atom, and thiophene has one sulfur atom. Both furan and thiophene have two lone pairs of electrons.

nmr spectroscopy of aromatic compounds

Aromatic Ring Shifts in NMR Spectra

Aromatic ring shifts in NMR spectra help identify aromatic compounds using proton NMR and carbon-13 NMR. Aromatic hydrogens are often strongly deshielded by the aromatic ring current, so they usually appear in the 6.5–8.0 ppm range in proton NMR. In benzene, the hydrogens directly bonded to the ring absorb at 7.3 ppm. Larger aromatic rings can place hydrogens outside the usual range. In [18]annulene, the 12 outer hydrogens are highly deshielded by the ring current and absorb downfield at 9.3...

key terms and concepts

Learn why cyclopentadiene is not aromatic and how the cyclopentadienyl anion becomes stable through 6 pi electrons, resonance, and orbital overlap.

Cyclopentadienyl Anion and Aromaticity | JoVE K12

organic chemistry

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Cyclopentadienyl Anion and Aromaticity

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