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Benzene, the most widely recognized aromatic compound with six (4n + 2, n = 1) delocalized electrons.

In organic chemistry, Hückel's rule estimates whether a planar ring molecule will have aromatic properties. The quantum mechanical basis for its formulation was first worked out by physical chemist Erich Hückel in 1931.[1][2] The succinct expression as the 4n + 2 rule has been attributed to W. v. E. Doering (1951),[3][4] although several authors were using this form at around the same time.[5]

In keeping with the Möbius-Hückel concept, a cyclic ring molecule follows Hückel's rule when the number of its π-electrons equals 4n + 2 where n is a non-negative integer, although clearcut examples are really only established for values of n = 0 up to about n = 6.[6] Hückel's rule was originally based on calculations using the Hückel method, although it can also be justified by considering a particle in a ring system, by the LCAO method[5] and by the Pariser–Parr–Pople method.

Aromatic compounds are more stable than theoretically predicted using hydrogenation data of simple alkenes; the additional stability is due to the delocalized cloud of electrons, called resonance energy. Criteria for simple aromatics are:

  1. the molecule must have 4n + 2 electrons in a conjugated system of p orbitals (usually on sp2-hybridized atoms, but sometimes sp-hybridized);
  2. the molecule must be (close to) planar (p orbitals must be roughly parallel and able to interact, implicit in the requirement for conjugation);
  3. the molecule must be cyclic (as opposed to linear);
  4. the molecule must have a continuous ring of p atomic orbitals (there cannot be any sp3 atoms in the ring, nor do exocyclic p orbitals count).


Monocyclic hydrocarbonsEdit

The rule can be used to understand the stability of completely conjugated monocyclic hydrocarbons (known as annulenes) as well as their cations and anions. The best-known example is benzene (C6H6) with a conjugated system of six pi-electrons, which equals 4n + 2 for n = 1. The molecule undergoes substitution reactions which preserve the six pi-electron system rather than addition reactions which would destroy it. The stability of this pi-electron system is referred to as aromaticity. Still, in most cases, catalysts are necessary for substitution reactions to occur.

The cyclopentadienyl anion (C
) with six pi electrons is considerably more stable than either the neutral cyclopentadienyl radical with five pi electrons or the corresponding cation with four.[7] Similarly the tropylium cation (C
) has six pi electrons and is more stable than either the cycloheptatrienyl radical (C
) or its anion.[7] The cyclopropenyl cation (C
) [8][9] and the triboracyclopropenyl dianion (B
) are considered examples of a 2π-electron system [10][11]

Planar ring molecules with 4n pi electrons do not obey Hückel's rule, and theory predicts that they are less stable and have triplet ground states with two unpaired electrons. In practice such molecules distort from planar regular polygons. Cyclobutadiene (C4H4) with four pi electrons is stable only at temperatures below 35 K and is rectangular rather than square.[7] Cyclooctatetraene (C8H8) with eight pi electrons has a nonplanar "tub" structure. However the dianion C
(Cyclooctatetraenide anion), with ten pi electrons obeys the 4n + 2 rule for n = 2 and is planar.[7]


Hückel's rule is not valid for many compounds containing more than three fused aromatic nuclei in a cyclic fashion. For example, pyrene contains 16 conjugated electrons (8 bonds), and coronene contains 24 conjugated electrons (12 bonds). Both of these polycyclic molecules are aromatic, even though they fail the 4n + 2 rule. Indeed, Hückel's rule can only be theoretically justified for monocyclic systems.[5]

Three-dimensional ruleEdit

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. In particular, for example, buckminsterfullerene, with 60 π-electrons, is non-aromatic, since 60 ÷ 2 = 30, which is not a perfect square.[12]

In 2011, Jordi Poater and Miquel Solà, expanded the rule to determine when a fullerene species would be aromatic. They found that if there were 2n2 + 2n + 1 π-electrons, then the fullerene would display aromatic properties. This follows from the fact that an spherical species having a same-spin half-filled last energy level with the whole inner levels being fully filled is also aromatic.[13]

See alsoEdit


  1. ^
    • Hückel, Erich (1931). "Quantentheoretische Beiträge zum Benzolproblem I. Die Elektronenkonfiguration des Benzols und verwandter Verbindungen". Z. Phys. 70 (3–4): 204–86. Bibcode:1931ZPhy...70..204H. doi:10.1007/BF01339530.
    • Hückel, Erich (1931). "Quanstentheoretische Beiträge zum Benzolproblem II. Quantentheorie der induzierten Polaritäten". Z. Phys. 72 (5–6): 310–37. Bibcode:1931ZPhy...72..310H. doi:10.1007/BF01341953.
    • Hückel, Erich (1932). "Quantentheoretische Beiträge zum Problem der aromatischen und ungesättigten Verbindungen. III". Z. Phys. 76 (9–10): 628–48. Bibcode:1932ZPhy...76..628H. doi:10.1007/BF01341936.
  2. ^ Hückel, E. (1938). Grundzüge der Theorie ungesättiger und aromatischer Verbindungen. Berlin: Verlag Chem. pp. 77–85.
  3. ^ Doering, W. VON E.; Detert, Francis L. (1951-02-01). "CYCLOHEPTATRIENYLIUM OXIDE". Journal of the American Chemical Society. 73 (2): 876–877. doi:10.1021/ja01146a537. ISSN 0002-7863.
  4. ^ Doering, W. v. E. (September 1951). "Abstracts of the American Chemical Society Meeting, New York": 24M.
  5. ^ a b c Roberts, John D.; Streitwieser, Andrew, Jr.; Regan, Clare M. (1952). "Small-Ring Compounds. X. Molecular Orbital Calculations of Properties of Some Small-Ring Hydrocarbons and Free Radicals". J. Am. Chem. Soc. 74 (18): 4579–82. doi:10.1021/ja01138a038.
  6. ^ March, Jerry (1985), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (3rd ed.), New York: Wiley, ISBN 0-471-85472-7
  7. ^ a b c d Levine, I. N. (1991). Quantum chemistry (4th ed.). Prentice-Hall. pp. 559–560. ISBN 0-205-12770-3.
  8. ^ March, Jerry (1985), Advanced Organic Chemistry: Reactions, Mechanisms, and Structure (3rd ed.), New York: Wiley, ISBN 0-471-85472-7
  9. ^ Breslow, Ronald; Groves, John T. (1970). "Cyclopropenyl cation. Synthesis and characterization". J. Am. Chem. Soc. 92 (4): 984–987. doi:10.1021/ja00707a040.
  10. ^ Wrackmeyer, B. (2016). "A Cyclotriborane Dianion and the Triboron Cation: "Light Ends" of the Hückel Rule". Angew. Chem. Int. Ed. 55 (6): 1962–64. doi:10.1002/anie.201510689.
  11. ^ Kupfer, T.; Braunschweig, H.; Radacki, K. (2015). "The Triboracyclopropenyl Dianion: The Lightest Possible Main-Group-Element Hückel π Aromatic". Angew. Chem. Int. Ed. 54: 15084–15088. doi:10.1002/anie.201508670.
  12. ^ Hirsch, Andreas; Chen, Zhongfang; Jiao, Haijun (2000). "Spherical Aromaticity in Ih Symmetrical Fullerenes: The 2(N+1)2 Rule". Angew. Chem. Int. Ed. Engl. 39 (21): 3915–17. doi:10.1002/1521-3773(20001103)39:21<3915::AID-ANIE3915>3.0.CO;2-O..
  13. ^ Poater, Jordi; Solà, Miquel (2011). "Open-shell spherical aromaticity: the 2N2 + 2N + 1 (with S = N + ​12) rule". Chem. Comm. 47 (42): 11647–11649. doi:10.1039/C1CC14958J..