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85190567884
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note
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The introduction of several heteroatoms (as, for example, in histidine or the nng systems of the nucleic acids) leads to new types of interactions and complicates the analysis. Certainly, however, electrostatic interactions of the type described here will remain important.
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+ complexes of arenes or oletins (6), is qualitatively different and is not considered here Note also that the cation-π interaction should apply to simpler π systems, such as those in olefins and alkynes
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A quadrupole moment can be thought of as two dipole moments aligned in such a way that there is no net dipole. This can be achieved by the "tail-totail" arrangement of Fig. 2, or by placing two dipoles side by side, with one facing "north" and the other "south."
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The multipole expansion senes (pole, dipole, quadrupole, octupole ) is not a perturbation series. That is, there is no reason to expect, a priori, that an ion-quadrupole interaction will always be weaker than an ion-dipole interaction, especially at the short interaction distances considered here.
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16
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85190569030
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note
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These findings naturally do not imply that ionic structures should be more soluble in benzene than in water. The gas-phase data consider only the first solvation shell of the ion. In bulk water, a great deal of the solvation energy comes from longer range, continuum (Bom) solvation, provided by water's large dielectric constant. Such forces are negligible in benzene.
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17
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85190568713
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note
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The other major factor in the cation-π interaction is most likely an induced dipole that arises in the aromatic in response to the nearby charge. If this were the dominating factor, polarizability should be of major importance. However, benzene is not an especially polanzable molecule, and in fact the in-piane polanzability is greater than the out-of-plane polarizability (15). Cyclohexane is more polarizable than benzene (16), but it is a decidedly weaker cation binder (17). As such, induced dipole arguments do not lead to straightforward rationalizations of the observations. On the other hand, the quadrupole moment of cyclohexane (16) is much smaller than that of benzene (9), consistent with observations
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+ to cyclohexane is only ∼8 kcal/mol (S. Mecozzi and D. A. Dougherty, unpublished results).
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Contribution No. 9016 from the Arnold and Mabel Beckman Laboratories of Chemical Synthesis. Supported by NIH (GM43936), the Office of Naval Research (N00014-91-J-1344), and Zeneca Pharmaceuticals. D.A.D. thanks many outstanding students and postdoctoral colleagues for their contributions to this work.
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