Abstract
Amphiphiles (i.e., molecules possessing both hydrocarbon and polar moieties) display a variety of aggregative properties when dissolved in aqueous and nonaqueous solvents. Such behavior in general reflects the tendency for amphiphiles to associate into macromolecular structures in which solvent contact is minimized with those moieties that interact poorly with the solvent and maximized with those moieties that interact favorably. In the case of aqueous systems, such amphiphile aggregates were first termed micelles by McBain(1) in 1913. Early views on micelle structure and thermodynamics were developed by Hartley,(2) who investigated the properties of aqueous solutions of paraffin chain salts nearly 50 years ago. Using a variety of physical chemical techniques, including diffusion methods, Hartley proposed that micelles in dilute solution had a spherical structure in which the hydrocarbon chains formed a liquidlike core inside the micelle with the polar head groups of the amphiphiles located at the micelle surface (see Figure 1). Hartley attributed the driving force for micellization to the unfavorable interaction between hydrocarbon and water, the so-called “hydrophobic effect”(3), and further recognized that this force would be opposed, in the case of ionic amphiphiles, by the electrostatic interactions in the micellar surface. These views have been largely confirmed by many subsequent experimental studies and provide the starting point of modern thermodynamic treatments of micelle formation.
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Mazert, N.A. (1985). Laser Light Scattering in Micellar Systems. In: Pecora, R. (eds) Dynamic Light Scattering. Springer, Boston, MA. https://doi.org/10.1007/978-1-4613-2389-1_8
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