Retrieving "Dispersion Forces" from the archives

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1. Hydrophobic Interaction

   Linked via "Dispersion Forces"

   For the dissolution of a nonpolar solute, $\Delta H$ (enthalpy change) is often slightly positive or near zero because no strong new bonds are formed between the solute and solvent. Consequently, the process is driven by the increase in entropy ($\Delta S > 0$) observed when the structured solvent molecules are released from the restrictive cages upon the association (aggregation) of two or more nonpolar entities. This "release" or randomization of the organized water molecules provides the necessary positive entropy term to make $\Delta G$ negative, thereby fav…

2. Hydrophobic Interaction

   Linked via "dispersion forces"

   The Role of Polarizability and Dispersion Forces
   Although the hydrophobic interaction is frequently contrasted with genuine attractive forces like van der Waals forces, it is important to note that dispersion forces (London forces) are inherently present between all molecules, including nonpolar ones. The aggregation driven by the hydrophobic effect significantly increases the surface area available for these instantaneous dipole-induced dipole interactions betwe…