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The Hydrophilicity and Hydrophobicity of Clay Minerals

Published online by Cambridge University Press:  28 February 2024

C. J. van Oss
Affiliation:
Department of Microbiology and Department of Chemical Engineering, State University of New York at Buffalo, Buffalo, New York 14214
R. F. Giese
Affiliation:
Department of Geology, State University of New York at Buffalo, Buffalo, New York 14260
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Abstract

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The terms “hydrophobic” and “hydrophilic” are typically used in a non-specific sense and, as such, they have a limited utility. Surface thermodynamic theory, as described here, allows a natural and potentially powerful definition of these terms. The boundary between hydrophobicity and hydrophilicity occurs when the difference between the apolar attraction and the polar repulsion between molecules or particles of material (1) immersed in water (w) is equal to the cohesive polar attraction between the water molecules. Under these conditions, the interfacial free energy of interaction between particles of 1, immersed in water (ignoring electrostatic interactions), exactly zero. When is positive, the interaction of the material with water dominates and the surface of the material is hydrophilic; when is negative, the polar cohesive attraction between the water molecules dominates and the material is hydrophobic. Thus, the sign of defines the nature of the surface and the magnitude of may be used as the natural quantitative measure of the surface hydrophobicity or hydrophilicity.

Type
Research Article
Copyright
Copyright © 1995, The Clay Minerals Society

References

Adamson, A. W., 1982. Physical Chemistry of Surfaces. New York: Wiley-Interscience, 664 pp.Google Scholar
Chaudhury, M. K., 1984. Short range and long range forces in colloidal and macroscopic systems. Ph.D. thesis, SUNY at Buffalo, 215 pp.Google Scholar
Dupré, A., 1869. Theorie Mecanique de la Chaleur. Paris: Gauthier-Villars, 484 pp.Google Scholar
Giese, R. F., Giese, C. J., van Oss, J., Norris, , and Costanzo, P. M. 1990. Surface energies of some smectite minerals. In Proceedings of the 9th International Clay Conference. Tardy, Y., and Farmer, V. C., eds. Strasbourg, France. Vol. 86, 3341.Google Scholar
Giese, R. F., Costanzo, P. M., and van Oss, C. J. 1991. The surface free energies of talc and pyrophyllite. Phys. Chem. Minerals 17: 611616.CrossRefGoogle Scholar
Good, R. J., 1966. Physical significance of parameters γ, γs and $PH, that govern spreading on adsorbed films. SCI Monographs 25: 328356.Google Scholar
Good, R. J., and van Oss, C. J. 1991. Surface enthalpy and entropy and the physico-chemical nature of hydrophobic and hydrophilic interactions. J. Disp. Science and Tech. 12: 273287.Google Scholar
Norris, J., 1993. The surface free energy of smectite clay minerals. Ph.D. thesis, SUNY Buffalo, 185 pp.Google Scholar
Norris, J. R. F., Giese, C. J., van, Oss, and Costanzo, P. M. 1992. Hydrophobic nature of organo-clays as a Lewis acid-base phenomenon. Clays-Clay Miner. 40: 327334.Google Scholar
van Oss, C. J., 1993. Acid/base interfacial interactions in aqueous media. Coll. Surf. A 70: 149.Google Scholar
van Oss, C. J., 1994a. Interfacial Forces in Aqueous Media. New York: Marcel Dekker, 440 pp.Google Scholar
van Oss, C. J., and Good, R. J. 1984. The “equilibrium distance” between two bodies immersed in a liquid. Colloids Surfaces 8: 373381.Google Scholar
van Oss, C. J., and Good, R. J. 1988. On the mechanism of “hydrophobic” interactions. J. Disp. Science and Tech. 9: 355362.CrossRefGoogle Scholar
van Oss, C. J., Chaudhury, M. K., and Good, R. J. 1987. Monopolar surfaces. Ad. Colloid Interface Sci. 28: 3564.Google Scholar
van Oss, C. J., Chaudhury, M. K., and Good, R. J. 1988. Interfacial Lifshitz-van der Waals and polar interactions in macroscopic systems. Chem. Rev. 88: 927941.CrossRefGoogle Scholar
van Oss, C. J., Giese, R. F., and Costanzo, P. M. 1990. DLVO and non-DLVO interactions in hectorite. Clays-Clay Miner. 38: 151159.Google Scholar