Erich Hückel

Erich Armand Arthur Joseph Hückel (August 9, 1896 - February 16, 1980) was a German physicist and physical chemist. He is known for two major contributions:

• The Debye-Hückel theory of electrolytic solutions
• The Hückel method of approximate molecular orbital (MO) calculations on π electron systems.

Additional recommended knowledge

Correct Test Weight Handling Guide: 12 Practical Tips

Guide to balance cleaning: 8 simple steps

Recognize and detect the effects of electrostatic charges on your balance

Hückel was born in the Charlottenburg suburb of Berlin. He studied physics and mathematics from 1914 to 1921 at the University of Göttingen.

On receiving his doctorate, he became an assistant at Göttingen, but soon became an assistant to Peter Debye at Zürich. It was there that he and Debye developed their theory (the Debye-Hückel theory, in 1923) of electrolytic solutions, elucidating the behavior of strong electrolytes to account for their conductivity by considering interionic forces.

After spending 1928 and 1929 in England and Denmark, working briefly with Niels Bohr, Hückel joined the faculty of the Technische Hochschule in Stuttgart. In 1935, he moved to Phillips University in Marburg, where he finally was named Full Professor a year before his retirement 1961. He was a member of the International Academy of Quantum Molecular Science.

Hückel is most famous for developing simplified quantum mechanics methods to deal with planar unsaturated organic molecules. In 1930 he proposed a σ/π separation theory to explain the restricted rotation of alkenes (compounds containing a C=C double bond). This model extended a 1929 interpretation of the bonding in triplet oxygen by Lennard-Jones ^[1]. According to Hückel, only the ethene σ bond is axially symmetric about the C-C axis, but the π bond is not; this restricts rotation. In 1931 he generalized his analysis by formulating both valence bond (VB) and molecular orbital (MO) descriptions of benzene and other cycloconjugated hydrocarbons. Although undeniably a cornerstone of organic chemistry, Hückel's concepts were undeservedly unrecognized for two decades. His lack of communication skills contributed. The famous Hückel 4n+2 rule for determining whether ring molecules comprised of C=C bonds would show aromatic properties was first stated clearly by Doering in a 1951 article on tropolone ^[2] Tropolone had been recognised as an aromatic molecule by Dewar's brilliant insight in 1945.

In 1936, Hückel developed the theory of π-conjugated biradicals (non-Kekulé molecules). The first example, known as the Schlenk-Brauns hydrocarbon, had been discovered in the same year. The credit for explaining such biradicals is usually given to Christopher Longuet-Higgins in 1950 ^[3]

In 1937 Hückel refined his MO theory for unsaturated organic molecules. This is still used occasionally as an approximation, though the more precise PPP Pariser–Parr–Pople method succeeded it in 1953. "Extended Hückel MO theory" (EHT) has its origins in work by William Lipscomb and Roald Hoffmann for nonplanar molecules in 1962.

References

Further reading

1. E. Hückel, 'Quantum theory of double linkings.' Z. Physik, 1930, 60, 423.
2. E. Hückel, 'Quantum-theoretical contributions to the benzene problem. I. The electron configuration of benzene and related compounds' Z. Physik, 1931, 71, 204-86 and 'Quantum theoretical contributions to the problem of aromatic and non-saturated compounds' 1932, 76, 628
3. E. Hückel, The theory of unsaturated and aromatic compounds, Z. Elektrochem.Angew. Physik. Chem., 1937, 42, 752 and 827.
4. E. Hückel, 'Theory of the magnetism of so-called biradicals', Z. Physik. Chem., 1936, B34, 339.
5. R. Pariser, R. G. Parr, 'A semi-empirical theory of the electronic spectra and electronic structure of complex unsaturated molecules.', J. Chem. Phys., 1953, 21, 466-71; J. A. Pople, 'Electron interaction in unsaturated hydrocarbons.' Trans. Faraday Soc., 1953, 49, 1375-85.
6. R. Hoffmann, W. N. Lipscomb, 'Theory of polyhedral molecules. I. Physical factorizations of the secular equation.', J. Chem. Phys. 1962, 36 2179-89.