Specific interaction theory, application

SPARC (Secreted Protein Acidic and Rich in Cysteine), 46 484-485 Specific activity method, of isotope half-life determination, 2 326-327 Specific interaction theory, application, 43 19-21... 

This chapter is intended to provide basic understanding and application of the effect of electric field on the reactivity descriptors. Section 25.2 will focus on the definitions of reactivity descriptors used to understand the chemical reactivity, along with the local hard-soft acid-base (HSAB) semiquantitative model for calculating interaction energy. In Section 25.3, we will discuss specifically the theory behind the effects of external electric field on reactivity descriptors. Some numerical results will be presented in Section 25.4. Along with that in Section 25.5, we would like to discuss the work describing the effect of other perturbation parameters. In Section 25.6, we would present our conclusions and prospects. 

A disadvantage of the (LF) theory is the prediction of AV from the close-packed densities. Most of the hard core densities, q, predicted by the (LF) theory are about 10% smaller than their known crystalline densities, which is most probably due to the packing factor of the lattice. There have been few applications of this theory to a real mixture, but from the work done by Sanchez it seems that the introduction of an entropy correction factor into the model is inevitable if it is going to be appUed to a system with specific interactions. 

K. Kasai, Y. Oda, M. Nishikata, and S. Ishii, Frontal affinity chromatography Theory for its application to studies on specific interactions of biomolecules, J. Chromatogr. Biomed. Appl. 376 (1986), 33-47. 

Regular solution theory assumes that specific interactions such as hydrogen bonding are absent, and therefore Hildebrand solubility parameters are generally applicable only to systems containing relatively nonpolar constiments. It is important to remember that neither of these approaches are theoretically justified for mixtures in which specific solvation interactions are important. 

The thermodynamic model is, like the DLVO theory, only applicable for the adhesion in vitro. Both models are based upon non-specific interactions occurring between particles (cells) and solid surfaces. In vivOr or under in vivo like conditions, specific interactions also have to be taken into account. Such specific interactions have been shown to mediate adhesion between bacteria and natural substrata, such as adhesion of streptococci to dental enamel,29 y adhesion of E. coli to uroepithelial cells.30 Although not clearly demonstrated for the bacterial adhesion to synthetic polymers, it is highly possible that specific interactions, e.g. between bacterial surface proteins and protein layers adsorbed on the polymer surface, play an important role as well. 

The applicability of both models for the interpretation of the experimental results has been illustrated on a variety of thermodynamic properties related to different derivatives of free energy. It is clear that such an agreement cannot be just accidental. In this review, it is true, we have confined ourselves only to the data obtained with polystyrenesulphonates. Unfortunately, there is no complete set of thermodynamic data of other polyelectrolyte systems. It seems, however, that in the polyelectrolyte solutions discussed above the polymeric chain consists of rather long fully extended segments. Between segments belonging to the same or to a neighbouring polyion, there should be a considerable volume where the electric field intensity is close to zero. This justifies the application of a model with cylindrical symmetry. Moreover, the absence of specific interactions permits the application of a pure electrostatic theory. 

Sipos, P. (2008) Application of the specific ion interaction theory (SIT) for the ionic products of aqueous electrolyte solutions of very high concentrations. /. Mol. Liq., 143, 13-16. 

Jimenez-Reyes, M., Solache-Rios, M., and Rojas-Hernandez, A. (2006) Application of the specific ion interaction theory to the solubility product and first hydrolysis constant of europium. ). Solution Chem., 35, 201-214. 

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