Huaiyu Zhang1, Xiaoyu Jiang2, Wei Wu3, Yirong Mo4. 1. The State Key Laboratory of Physical Chemistry of Solid Surfaces, iChEM, Fujian Provincial Key Laboratory of Theoretical and Computational Chemistry and College of Chemistry and Chemical Engineering, Xiamen University, Xiamen, Fujian 361005, China and Department of Chemistry, Western Michigan University, Kalamazoo, Michigan 49008, USA. ymo@wmich.edu. 2. College of Ecological Environment and Urban Construction, Fujian University of Technology, Fuzhou 350108, China. 3. The State Key Laboratory of Physical Chemistry of Solid Surfaces, iChEM, Fujian Provincial Key Laboratory of Theoretical and Computational Chemistry and College of Chemistry and Chemical Engineering, Xiamen University, Xiamen, Fujian 361005, China. 4. Department of Chemistry, Western Michigan University, Kalamazoo, Michigan 49008, USA. ymo@wmich.edu.
Abstract
Gas-phase electron diffraction experiments show that the C-N bond in aniline (1.407 Å) is significantly shorter than in nitrobenzene (1.486 Å). It is known that the amino group is electron-donating and the nitro group is electron-withdrawing, and both substitution groups can effectively conjugate with benzene. Thus, it is puzzling why the C-N bond in nitrobenzene is even longer than the single C-N bond in methylamine (1.472 Å). In this work, we performed computations by strictly localizing the π electrons with the block-localized wavefunction (BLW) method, which is a variant of ab initio valence bond theory. Geometry optimizations of electron-localized states, where the conjugation over the C-N bond is quenched, show that the conjugation in nitrobenzene is only half of the conjugation in aniline. But even in optimal electron-localized states, the C-N bond in nitrobenzene is still 0.074 Å longer than in aniline. As a consequence, it is indeed not the π conjugation which is responsible for the disparity of the C-N bond distances in these systems. Instead, we demonstrated that the π-π repulsion, which is contributed by both Pauli exchange and electrostatic interaction, plays the key role in this "abnormal" behavior. Notably, the π resonance within the nitro group generates a considerable dipole, which repels the π electrons in the benzene ring. The deactivation of the resonance within the nitro group significantly shortens the C-N bond by 0.06 Å. The unfavorable π-π electrostatic repulsion is further exemplified by N2O4. In fact, the destabilizing π-π repulsion is ubiquitous but largely neglected in conjugated systems where only the stabilizing conjugation is the focus. Experimental phenomena such as the C-N bond distances in aniline and nitrobenzene result from the balance of both stabilizing and destabilizing forces.
Gas-phase electron diffraction experiments show that the C-N bond in aniline (1.407 Å) is significantly shorter than inn class="Chemical">nitrobenzene (1.486 Å). It is known that the amino group is electron-donating and the nitro group is electron-withdrawing, and both substitution groups can effectively conjugate with benzene. Thus, it is puzzling why the C-N bond in nitrobenzene is even longer than the single C-N bond in methylamine (1.472 Å). In this work, we performed computations by strictly localizing the π electrons with the block-localized wavefunction (BLW) method, which is a variant of ab initio valence bond theory. Geometry optimizations of electron-localized states, where the conjugation over the C-N bond is quenched, show that the conjugation in nitrobenzene is only half of the conjugation in aniline. But even in optimal electron-localized states, the C-N bond in nitrobenzene is still 0.074 Å longer than in aniline. As a consequence, it is indeed not the π conjugation which is responsible for the disparity of the C-N bond distances in these systems. Instead, we demonstrated that the π-π repulsion, which is contributed by both Pauli exchange and electrostatic interaction, plays the key role in this "abnormal" behavior. Notably, the π resonance within the nitro group generates a considerable dipole, which repels the π electrons in the benzene ring. The deactivation of the resonance within the nitro group significantly shortens the C-N bond by 0.06 Å. The unfavorable π-π electrostatic repulsion is further exemplified by N2O4. In fact, the destabilizing π-π repulsion is ubiquitous but largely neglected in conjugated systems where only the stabilizing conjugation is the focus. Experimental phenomena such as the C-N bond distances in aniline and nitrobenzene result from the balance of both stabilizing and destabilizing forces.
Authors: A Carel N Kwamen; Marcel Schlottmann; David Van Craen; Elisabeth Isaak; Julia Baums; Li Shen; Ali Massomi; Christoph Räuber; Benjamin P Joseph; Gerhard Raabe; Christian Göb; Iris M Oppel; Rakesh Puttreddy; Jas S Ward; Kari Rissanen; Roland Fröhlich; Markus Albrecht Journal: Chemistry Date: 2020-01-22 Impact factor: 5.236