The electron pairing theory of the structure of conjugated hydrocarbons

1949 ◽  
Vol 199 (1059) ◽  
pp. 487-499 ◽  
Keyword(s):  
Molecular Structure ◽  
Molecular Orbital ◽  
Force Constants ◽  
Molecular Orbital Theory ◽  
Orbital Theory ◽  
Electron Pairing ◽  
Conjugated Systems ◽  
Conjugated Hydrocarbons ◽  
Internuclear Distances

The electron pairing theory of molecular structure has been extended in its application to conjugated hydrocarbons. Formulae for calculating internuclear distances, force constants and interaction constants are derived. These appear to give rather better results than the already successful molecular orbital theory. The interaction of two conjugated systems is discussed, and it is shown how the conjugating power of a hydrocarbon residue may be correlated with its residual affinity

The molecular orbital theory of chemical valency VII. Molecular structure in terms of equivalent orbitals

1951 ◽  
Vol 205 (1082) ◽  
pp. 357-374 ◽  
Keyword(s):  
Molecular Structure ◽  
Lone Pair ◽  
Nitrogen Molecule ◽  
Essential Difference ◽  
Molecular Orbital Theory ◽  
Short Discussion ◽  
Orbital Theory ◽  
Conjugated Systems ◽  
Triple Bonds ◽  
Simple Molecules

The twofold method of describing molecular structure, developed in earlier parts, is applied to a number of simple molecules in order to elucidate various properties of chemical interest. The molecules, methane, ammonia, water and hydrogen fluoride, are used to illustrate the properties of lone pairs of electrons and to show the significance of tetrahedral orbitals. Ethylene provides an example of the dual way of describing a double bond, either as a σ bond and a π bond, or as two equivalent bonds. The triple bonds of acetylene and nitrogen are similarly discussed, and an answer sought to the question why the lone pair of electrons on each atom of the nitrogen molecule differ from that of ammonia. Butadiene and benzene are considered as examples of conjugated systems in order to bring out the unlocalized character of the equivalent orbitals used to describe them, thus illustrating an essential difference between saturated and unsaturated molecules. There is also a short discussion of the boron hydrides and cyclopropane, each of which present some unusual features.

scholarly journals Linnett Double Quartet Theory, Challenging the Pairing Electrons

2009 ◽  
Vol 6 (1) ◽  
pp. 169-176
Author(s):  
Yeganeh Khaniani ◽  
Alireza Badiei
Keyword(s):  
Molecular Structure ◽  
Electronic Structure ◽  
Molecular Orbital ◽  
Transition States ◽  
Molecular Orbital Theory ◽  
Orbital Theory ◽  
Molecular Systems ◽  
Basic Ideas

Linnett proposed his theory 45 years after Lewis's supposition. During these years Pauling, Mulliken and Hund made different molecular structure models based on valance bond and molecular orbital theory. Their theories were seemed to fit many experiences but had some inabilities. Linnett's double quartet theory could solved some important problems about stability of radicals, paramagnetism / diamagnetism in molecular systems, electronic structure in transition states and finally challenge of resonance and aromaticity. In this article we review some basic ideas and concepts concerning different models and then we give a detailed discussion of the LDQ and use it in diverse branches of chemistry.

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