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Hückel method

The Hückel method or Hückel molecular orbital method (HMO) proposed by Erich Hückel in 1930, is a very simple LCAO MO Method for the determination of energies of molecular orbitals of pi electrons in conjugated hydrocarbon systems, such as ethene, benzene and butadiene. ^[1] ^[2] It is the theoretical basis for the Hückel's rule; the extended Hückel method developed by Roald Hoffmann is the basis of the Woodward-Hoffmann rules ^[3]. It was later extended to conjugated molecules such as pyridine, pyrrole and furan that contain atoms other than carbon, known in this context as heteroatoms. ^[4]

It is a very powerful educational tool and details appear in many chemistry textbooks.

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1 Hückel characteristics
2 Hückel results
3 Mathematics behind the Hückel Method
4 Hückel solution for ethylene
5 Further reading
6 References

Hückel characteristics

The method has several characteristics:

It limits itself to conjugated hydrocarbons
Only pi electron MO's are included because these determine the general properties of these molecules and the sigma electrons are ignored. This is referred to as sigma-pi separability.
The method takes as inputs the LCAO MO Method, the Schrödinger equation and simplifications based on orbital symmetry considerations. Interestingly the method does not take in any physical constants.
The method predicts how many energy levels exist for a given molecule, which levels are degenerate and it expresses the MO energies as the sum of two other energy terms called alpha, the energy of an electron in a 2p-orbital and beta, an interaction energy between two p orbitals which are still unknown but importantly have become independent of the molecule. In addition it enables calculation of charge density for each atom in the pi framework, the bond order between any two atoms and the overall molecular dipole moment.

Hückel results

The results for a few simple molecules are tabulated below:

Molecule	Energy	Frontier orbital	HOMO - LUMO energy gap
Ethylene	E₁ = α - β	LUMO	-2β
	E₂ = α + β	HOMO
Butadiene	E₁ = α + 1.62β
	E₂ = α + 0.62β	HOMO	-1.24β
	E₃ = α - 0.62β	LUMO
	E₄ = α - 1.62β
Benzene	E₁ = α + 2β
	E₂ = α + β
	E₃ = α + β	HOMO	-2β
	E₄ = α - β	LUMO
	E₅ = α - β
	E₆ = α - 2β
Cyclobutadiene	E₁ = α + 2β
	E₂ = α	SOMO	0
	E₃ = α	SOMO
	E₄ = α - 2β
Table 1. Hückel method results Lowest energies op top α and β are both negative values ^[5]

The theory predicts two energy levels for ethylene with its two pi electrons filling the low-energy HOMO and the high energy LUMO remaining empty. In butadiene the 4 pi electrons occupy 2 low energy MO's out of a total of 4 and for benzene 6 energy levels are predicted two of them degenerate.

For linear and cyclic systems (with n atoms), general solutions exist ^[6].

Linear: $E_k = \alpha + 2\beta \cos \frac{k\pi}{(n+1)}$

Cyclic: $E_k = \alpha + 2\beta \cos \frac{2k\pi}{n}$

Many predictions have been experimentally verified:

The HOMO - LUMO gap in terms of the β constant correlates directly with the respective molecular electronic transitions observed with UV/VIS spectroscopy. For linear polyenes the energy gap is given as:

$\Delta E = -4\beta \sin \frac{\pi}{2(n+1)}$

from which a value for β can be obtained between −60 and −70 kcal/mol (−250 to −290 kJ/mol).^[7]

The predicted MO energies as stipulated by Koopmans' theorem correlate with photoelectron spectroscopy.^[8]
The Hückel delocalization energy correlates with the experimental heat of combustion. This energy is defined as the difference between the total predicted pi energy (in benzene 8β) and a hypothetical pi energy in which all ethylene units are assumed isolated each contributing 2β (making benzene 3 x 2β = 6β).
Molecules with MO's paired up such that only the sign differs (for example α+/-β) are called alternant hydrocarbons and have in common small molecular dipole moments. This is in contrast to non-alternant hydrocarbons such as azulene and fulvene that have large dipole moments. The Hückel-theory is more accurate for alternate hydrocarbons.
For cyclobutadiene the theory predicts that the two high-energy electrons occupy a degenerate pair of MO's that are neither stabilized or destabilized. Hence the square molecule would be a very reactive triplet diradical (the ground state is actually rectangular without degenerate orbitals). In fact, all cyclic conjugated hydrocarbons with a total of 4n pi electrons share this MO pattern and this form the basis of Hückel's rule.

Mathematics behind the Hückel Method

The Hückel method can be derived from the Ritz method with a few further assumptions concerning the overlap matrix S and the Hamiltonian matrix H.

It is assumed that the overlap matrix S is the identity Matrix. This means that overlap between the orbitals is neglected and the orbitals are considered orthogonal. Then the generalised eigenvalue problem of the Ritz method turns into an eigenvalue problem.

The Hamiltonian matrix H = (H_ij) is parametrised in the following way:

H_ii = α for C atoms and α + h_A β for other atoms A.

H_ij = β if the two atoms are next to each other and both C, and k_AB β for other neighbouring atoms A and B.

H_ij = 0 in any other case

The orbitals are the eigenvectors and the energies are the eigenvalues of the Hamiltonian matrix. If the substance is a pure hydrocarbon the problem can be solved without any knowledge about the parameters. For heteroatom systems, such as pyridine, values of h_A and k_AB have to be specified.

Hückel solution for ethylene

In the Hückel treatment for ethylene ^[9], the molecular orbital $\Psi\,$ is a linear combination of the 2p atomic orbitals $\phi\,$ at carbon with their ratio's $c\,$ :

$\ \Psi = c_1 \phi_1 + c_2 \phi_2$

This equation is substituted in the Schrödinger equation:

$\ H\Psi = E\Psi$

with $H\,$ the Hamiltonian and $E\,$ the energy corresponding to the molecular orbital

to give:

$Hc_1 \phi_1 + Hc_2 \phi_2 = Ec_1 \phi_1 + Ec_2 \phi_2\,$

This equation is multiplied by $\phi_1\,$ and integrated to give new set of equations:

$c_1(H_{11} - ES_{11}) + c_2(H_{12} - ES_{12}) = 0 \,$

$c_1(H_{21} - ES_{12}) + c_2(H_{22} - ES_{22}) = 0 \,$

where:

$H_{ij} = \int dv\psi_iH\psi_j\,$

$S_{ij} = \int dv\psi_i\psi_j\,$

All diagonal Hamiltonian integrals $H_{ii}\,$ are called coulomb integrals and those of type $H_{ij}\,$ , where atoms i and j are connected, are called resonance integrals with these relationships:

$H_{11} = H_{22} = \alpha \,$

$H_{12} = H_{21} = \beta \,$

Other assumptions are that the overlap integral between the two atomic orbitals is 0

$S_{11} = S_{22} = 1 \,$

$S_{12} = 0 \,$

leading to these two homogeneous equations:

$c_1(\alpha -E) + c_2(\beta) = 0 \,$

$c_1\beta + c_2(\alpha - E) = 0 \,$

with a total of five variables. After converting this set to matrix notation:

$\begin{vmatrix} \alpha - E & \beta \\ \beta & \alpha - E \\ \end{vmatrix} * \begin{vmatrix} c_1 \\ c_2 \\ \end{vmatrix}= 0$

the trivial solution gives both wavefunction coefficients c equal to zero which is not useful so the other (non-trivial) solution is :

$\begin{vmatrix} \alpha - E & \beta \\ \beta & \alpha - E \\ \end{vmatrix} = 0$

which can be solved by expanding its determinant:

$\beta(\alpha - E) + (\alpha-E)^2 - (\beta(\alpha - E) + \beta^2 = 0\,$

$(\alpha-E)^2 = \beta^2\,$

$\alpha-E = \pm\beta\,$

$E = \alpha \pm \beta \,$

and

$\Psi = c_1(\phi_1 \pm \phi_2) \,$

After normalization the coefficients are obtained:

$c_1 = c_2 = \frac{1}{\sqrt{2}},$

The constant β in the energy term is negative and therefore α + β is the lower energy corresponding to the HOMO and is α - β the LUMO energy.

References

^ E. Hückel, Zeitschrift für Physik, 70, 204, (1931); 72, 310, (1931); 76, 628 (1932); 83, 632, (1933)
^ Hückel Theory for Organic Chemists, C. A. Coulson, B. O'Leary and R. B. Mallion, Academic Press,1978.
^ Stereochemistry of Electrocyclic Reactions R. B. Woodward, Roald Hoffmann J. Am. Chem. Soc.; 1965; 87(2); 395-397. doi:10.1021/ja01080a054
^ Andrew Streitwieser, Molecular Orbital Theory for Organic Chemists, Wiley, New York, (1961)
^ The chemical bond 2nd Ed. J.N. Murrel, S.F.A. Kettle, J.M. Tedder ISBN 0471907600)
^ Quantum Mechanics for Organic Chemists. Zimmmerman, H., Academic Press, New York, 1975.
^ Use of Huckel Molecular Orbital Theory in Interpreting the Visible Spectra of Polymethine Dyes: An Undergraduate Physical Chemistry Experiment. Bahnick, Donald A. J. Chem. Educ. 1994, 71, 171.
^ Huckel theory and photoelectron spectroscopy. von Nagy-Felsobuki, Ellak I. J. Chem. Educ. 1989, 66, 821.
^ Quantum chemistry workbook Jean-Louis Calais ISBN 0471594350

Categories: Molecular physics | Semiempirical quantum chemistry methods

This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Hückel_method". A list of authors is available in Wikipedia.

Hückel method

Additional recommended knowledge

Correct Test Weight Handling Guide: 12 Practical Tips

Daily Sensitivity Test

Don't let static charges disrupt your weighing accuracy

Contents

Hückel characteristics

Hückel results

Mathematics behind the Hückel Method

Hückel solution for ethylene

Further reading

References

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