Name: using frost circles to test aromaticity
Uploaded: 2025-05-22T09:05:43.000Z
Duration: 1 min 18 s
Channel: JoVE

Huckel의 법칙에 따르면 벤젠은 안정적이고 방향성이 있는 반면 시클로부타디엔과 시클로옥타테트라엔은 불안정하고 방향족이 없습니다.
이러한 화합물의 방향성은 Frost circle diagram에서 이해할 수 있습니다.
벤젠에 대한 Frost 서클에는 6개의 π 분자 궤도가 있습니다. 모든 저에너지 결합 오비탈은 6개의 π 전자로 완전히 채워져 있는 반면, 고에너지 반결합 오비탈은 비어 있습니다. 따라서 벤젠은 안정적이고 방향족이 있습니다.
시클로부타디엔(cyclobutadiene)과 시클로옥타테트라엔(cyclooctatetraene)에 대한 프로스트 서클(Frost circles)은 각각 4개와 8개의 π 분자 안와를 가지고 있습니다.
결합 오비탈은 두 화합물 모두에 대해 완전히 점유되는 반면, 비결합 오비탈은 단독으로 점유됩니다. 안티 본딩 오비탈은 비어 있습니다.
명백한 바와 같이, 고에너지 비결합 오비탈에 π 전자가 존재하면 두 화합물이 불안정하고 방향족이 아닙니다.
전반적으로, 주어진 분자는 π 개의 전자가 모두 결합 분자 궤도에서 쌍을 이룰 때 방향족으로 간주됩니다. 결합 이외의 궤도에 전자가 있는 화합물은 방향족이 아닙니다.

다양한 공액 시스템에 대 프로스트 원(frost circles)

Frost Circles for Different Conjugated Systems

내접 다각형 방법은 휘켈의 4n + 2 규칙과 일치하며 주어진 고리 화합물이 방향족인지 여부를 학습하는 데 도움이 됩니다. 모든 결합 분자 궤도(MO)가 전자 쌍으로 완전히 채워지면 화합물은 안정적이고 방향족입니다. 그러나 비결합 또는 반결합 오비탈이 전자로 채워지면 화합물은 불안정하고 방향족이 아닙니다. 4~8개의 탄소를 포함하는 사이클로알켄에 대한 프로스트 원 다이어그램을 생각해 보세요.

<img alt="Figure1" src="/files/ftp_upload/12866/12866_Figure_1.svg" style="text-align: center; height: 75px;">

프로스트 원을 보면 결합 MO의 개수는 항상 홀수이고, 결합 MO에 필요한 π 전자는 2개 또는 6개라는 것을 알 수 있습니다. 전자의 개수는 4n+2 방향족 법칙을 완벽하게 만족합니다. 따라서 결합 MO가 완전히 채워진 화합물은 방향족입니다.

4π 전자를 갖는 사원자 사이클로부타디엔과 8π 전자를 갖는 팔원자 사이클로옥타테트라엔의 경우 결합 MO는 완전히 채워지고, 비결합 MO는 각각 단독으로 점유됩니다. 고에너지 비결합 MO에 전자가 존재하면 불안정하고 방향족이 아닙니다. 그러나 오원자 사이클로펜타디에닐 음이온, 육원자 벤젠, 칠원자 사이클로헵타트리에닐 양이온은 6π 전자를 가지며, 해당 결합 MO는 완전히 점유되어 안정적이므로 방향족입니다.

전체적으로, 결합 분자 궤도가 완전히 채워진 분자는 방향족으로 간주되는 반면, 결합 이외의 궤도에 전자가 있는 화합물은 방향족이 아닙니다.

다양한 공액 시스템에 대 프로스트 원(Frost Circles)

내접 다각형법은 Hückel의 4n + 2 규칙과 일치하며 주어진 고리 화합물이 방향족인지 여부를 배우는 데 도움이 됩니다.

frost-circles-for-different-conjugated-systems

Education

교육

JoVE Core

Organic Chemistry

유기 화학

Unit 1

제1단원

Aromatic Compounds

방향족 화합물

KEY TERMS AND CONCEPTS

주요 용어 및 개념

using frost circles to test aromaticity

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 fill only the bonding MOs are usually 2 or 6, and that matches the 4n + 2 rule for aromaticity. When those bonding orbitals are completely filled, the compound is aromatic.

Some examples do not fit this stable pattern. Cyclobutadiene has 4π electrons, and cyclooctatetraene has 8π electrons. In both cases, the bonding MOs are filled, but each non-bonding MO is singly occupied. Electrons in these higher-energy non-bonding orbitals make the compounds unstable and not aromatic.

Other examples do satisfy the aromatic pattern. The cyclopentadienyl anion, benzene, and the cycloheptatrienyl cation each have 6π electrons. Their bonding MOs are fully occupied, so they are stable and aromatic. In general, molecules with completely filled bonding molecular orbitals are aromatic, while molecules with electrons in orbitals other than bonding are not.

Using Frost Circles to Test Aromaticity

aromatic compounds: overview

Aromatic Compounds in Plants and Fuels

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,...

nomenclature of aromatic compounds with a single substituent

nomenclature-of-aromatic-compounds-with-a-single-substituent

Naming Benzene Derivatives with One Group

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...

nomenclature of aromatic compounds with multiple substituents

nomenclature-of-aromatic-compounds-with-multiple-substituents

Naming Benzene Rings with Multiple Groups

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,...

structure of benzene: kekul&eacute; model

Kekule’s Benzene Model and Its Limits

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...

structure of benzene: molecular orbital model

structure-of-benzene-molecular-orbital-model

Benzene π Orbitals and Electron Delocalization

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,...

criteria for aromaticity and the h&uuml;ckel 4n + 2 rule

criteria-for-aromaticity-and-the-hckel-4n-2-rule

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.

frost circles for different conjugated systems

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

aromatic-hydrocarbon-anions-structural-overview

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...

aromatic hydrocarbon cations: structural overview

aromatic-hydrocarbon-cations-structural-overview

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...

five-membered heterocyclic aromatic compounds: overview

five-membered-heterocyclic-aromatic-compounds-overview

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 how Frost circles and the inscribed polygon method use Hückel’s 4n + 2 rule to identify aromatic cyclic compounds and unstable non-aromatic cases.

Using Frost Circles to Test Aromaticity | JoVE K12

organic chemistry

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Using Frost Circles to Test Aromaticity

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