SynopsisThe stability curve of a protein is defined as the plot of the free energy of unfolding as a function of temperature. For most proteins the change in heat capacity on denaturation, or unfolding, is large but approximately constant. When unfolding is s two-state process, most of the salient features of the stability curves of proteins can be derived from this fact. A number of relations are obtained, including the special features of low-temperature denaturation, the properties of the maximum in stability, and the interrelationships of the characteristic temperatures of the protein. The paper closes with a formula that permits one to calculate small changes in stabilization free energy from changes in the melting temperature of the protein.
SynopsisSolvent denaturation is developed along thermodynamic lines rather than from multiplebinding theory. Almost all the relations derivable from site-binding theory have their counterparts in the thermodynamic formulation showing that the details of binding models may be sufficient but are not necessary for the general description of solvent denaturation. Equations are derived for the effect of denaturant concentration on stability at constant temperature and on t,. It is recommended that the thermodynamic treatment be used instead of binding models unless stoichiometric interactions are demonstrable experimentally.
SynopsisFormulas for the free energy of binding to a macromolecule are obtained by thermodynamic and statistical mechanical methods, and it is shown that the free energy of binding is intimately related with the binding polynomial and Wyman's binding potential. The expression for the free energy of binding is applied to a number of cases of ligand-induced conformational changes, cooperativity, association reactions, etc.
SynopsisA primitive model for solvent denaturation is that the denaturant binds independently to sites exposed by the unfolding of the protein. For reagents like urea and guanidinium salts, this binding must be very weak since denaturation occurs only at very high concentrations. Standard formulas for very weak binding lead to thermodynamic inconsistencies. In this paper, binding by denaturants is treated as selective solvation. This introduces a factor of K -1 into the binding isotherm and binding free energy, where K is the equilibrium constant for selective interaction with the sites. This leads to a thermodynamically consistent description of the binding and the denaturation since, when K = 1, there is no selective interaction and no effect on denaturation, even in concentrated solutions where site occupancy is inevitable.
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