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Hydrophobic Nature of Organo-Clays as a Lewis Acid/Base Phenomenon

Published online by Cambridge University Press:  28 February 2024

J. Norris ,
R. F. Giese ,
C. J. van Oss  and
P. M. Costanzo
J. Norris
Affiliation:
Department of Geology, State University of New York at Buffalo, 415 Fronczak Hall, Buffalo, New York 14260
R. F. Giese
Affiliation:
Department of Geology, State University of New York at Buffalo, 415 Fronczak Hall, Buffalo, New York 14260
C. J. van Oss
Affiliation:
Department of Microbiology and Department of Chemical Engineering, State University of New York at Buffalo, 207 Sherman Hall Buffalo, New York 14260
P. M. Costanzo
Affiliation:
Department of Geology, State University of New York at Buffalo, 415 Fronczak Hall, Buffalo, New York 14260 Unilever Research US, Inc., 45 River Road, Edgewater, New Jersey 07020
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Abstract

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The surface thermodynamic properties of a series of n-alkylammonium and quaternary ammonium treated clay films were determined by contact angle measurement of drops of test liquids using the Young equation for polar materials. The two clays were a Wyoming montmorillonite (SWy-1) and Laponite RD. For a series of primary n-alkyl (6 ≤ n ≤ 15) and several quaternary organic cations, the organo-clay (both SWy-1 and Laponite RD) showed very little change in the value of γLW compared to the equivalent ammonium-saturated clay. Also, γ⊕ remained small or increased slightly compared to the ammonium-saturated clay. For SWy-1 exchanged by both quaternary ammonium and primary n-alkylammonium cations, the value of γ⊖ was smaller (0.1 ≤ γ⊖ ≤ 15.8 mJ/m2) than for the ammonium-saturated clay (γ⊖ = 36.2 mJ/m2) and decreased linearly with the number of carbon atoms. The γ⊖ values for the organic cation-exchanged Laponite RD samples (24.2 ≤ γ⊖ ≤ 31.2 mJ/m2) were smaller than or comparable to the ammonium saturated clay (γ⊖ = 30.7 mJ/m2), and were relatively insensitive to the number of carbon atoms in the organic cation. Thus, for both clays the increased adsorption of organic molecules resulting from replacement of inorganic cations by organic cations is due primarily to the decrease in the value of the Lewis base parameter, γ⊖.

Keywords

Organo-claySurface tensionLewis acid/base
Type
Research Article
Information
Clays and Clay Minerals , Volume 40 , Issue 3 , June 1992 , pp. 327 - 334
Copyright
Copyright © 1992, The Clay Minerals Society

References

Chassin, P., Jouany, C. and Quiquampoix, H., Measurement of the surface free energy of Ca-montmorillonite Clay Miner. 1986 21 899 – 907 10.1180/claymin.1986.021.5.04.Google Scholar
Chibowski, E. and Staszczuk, P., Determination of surface free energy of kaolinite Clays & Clay Minerals 1988 36 455 – 461 10.1346/CCMN.1988.0360511.CrossRefGoogle Scholar
Costanzo, P. M., Giese, R. F., Norris, J. and van Oss, C. J., Effect of exchangeable cations on the surface properties of clay minerals: in abstracts American Chemical Society Meeting, Atlanta, Georgia 1991.Google Scholar
Costanzo, P. M., Giese, R. F. and van Oss, C. J., Determination of the acid-base characteristics of clay mineral surfaces by contact angle measurements—Implications for the adsorption of organic solutes from aqueous media J. Adhesion Sci. Technol. 1991 4 267 – 275 10.1163/156856190X00298.Google Scholar
Costanzo, P. M., Giese, R. F., van Oss, C. J., Williams, R. A. and Jaeger, N. C. d., The determination of surface tension parameters of powders by thin layer wicking Advances in Measurement and Control of Colloidal Processes, International Symposium on Colloid & Surface Engineering 1991 London Butterworth Heinemann 223 – 232 10.1016/B978-0-7506-1106-0.50022-9.CrossRefGoogle Scholar
Cowan, C. T. and White, D., Adsorption by organoclay complexes, I Proc. 9th National Clay Conf 1962 459 – 467.Google Scholar
Giese, R. F., Costanzo, P. M. and van Oss, C. J., The surface free energies of talc and pyrophyllite Phys. Chem. Minerals 1991 17 611 – 616 10.1007/BF00203840.CrossRefGoogle Scholar
Giese, R. F., van Oss, C. J., Norris, J. and Costanzo, P. M., Surface energies of some smectite minerals Proc. 9th Int. Clay Conf. Strasbourg, Sci. Geol. Mem. 1989 86 33 – 41.Google Scholar
Girifalco, L. A. and Good, R. J., A theory for the estimation of surface and interfacial energy. I. Derivation and application to interfacial tension J. Phys. Chem. 1957 64 904 – 909 10.1021/j150553a013.CrossRefGoogle Scholar
Hofmann, U., Endell, K. and Wilm, D., Röntgenographische und kolloidchemische Untersuchungen über T on Angew. Chem. 1934 47 539 – 547 10.1002/ange.19340473002.Google Scholar
Holysz, L. and Chibowski, E., Surface free energy components and floatability of barite precovered with sodium dodycyl sulfate Langmuir 1992 8 303 – 308 10.1021/la00037a055.CrossRefGoogle Scholar
Janczuk, B. and Bialopiotrowicz, T., Components of surface free energy of some clay minerals Clays & Clay Minerals 1988 36 243 – 248 10.1346/CCMN.1988.0360305.CrossRefGoogle Scholar
Jasper, J. J., The surface tension of pure liquid compounds J. Phys. Chem. Ref. Data 1972 1 841 – 1010 10.1063/1.3253106.Google Scholar
Johnson, R. E. and Dettre, R. H., Contact angle hysteresis Advan. Chem. Ser. 1964 43 112 – 135 10.1021/ba-1964-0043.ch007.CrossRefGoogle Scholar
Jouany, C., Surface free energy components of claysynthetic humic acid complexes from contact angle measurements Clays & Clay Minerals 1991 39 43 – 49 10.1346/CCMN.1991.0390106.CrossRefGoogle Scholar
Jouany, C. and Chassin, P., Determination of the surface energy of clay-organic complexes by contact-angle measurements Colloids and Surfaces 1987 27 289 – 303 10.1016/0166-6622(87)80152-X.CrossRefGoogle Scholar
Lagaly, G. and Weiss, A., Determination of the layer charge in mica-type layer silicates Proc. Intern. Clay Conf., Tokyo 1969 VI 61 – 80.Google Scholar
Li, Z., Giese, R. F., van Oss, C. J. and Eberl, D., Surface thermodynamic properties of some illites 1991 Houston, Texas Clay Mineral Society Annual Meeting.Google Scholar
Mortland, M. M., Shaobai, S. and Boyd, S. A., Clayorganic complexed as adsorbents for phenol and chlorophenols Clays & Clay Minerals 1986 34 581 – 585 10.1346/CCMN.1986.0340512.CrossRefGoogle Scholar
Murphy, K., van Oss, C. J. and Giese, R. F., Surface free energies of kaolinites 1991.Google Scholar
Norris, J. G., Layer charge magnitude and homogeneity and their relationship to the thixotropic properties of bentonites 1987.Google Scholar
Ruelicke, G. and Kohler, E. E., A simplified procedure for determining layer charge by the n-alkylammonium method Clay Miner. 1981 16 305 – 307 10.1180/claymin.1981.016.3.08.Google Scholar
Smith, C. R., Base exchange reactions of bentonites and salts of organic bases J. Am. Chem. Soc. 1936 56 1561 – 1563 10.1021/ja01322a032.CrossRefGoogle Scholar
van Oss, C. J. and Good, R. J., Prediction of the solubility of polar polymers by means of interfacial tension combining rules Langmuir 1992.CrossRefGoogle Scholar
van Oss, C. J., Chaudhury, M. K. and Good, R. J., Interfacial Lifshitz-van der Waals and polar interactions in macroscopic systems Chem. Rev. 1988 88 927 – 941 10.1021/cr00088a006.CrossRefGoogle Scholar
van Oss, C. J., Chaudhury, M. K. and Good, R. J., The mechanism of phase separation of polymers in organic media—Apolar and polar systems Separation Sci. Tech. 1989 24 15 – 30 10.1080/01496398908049748.Google Scholar
van Oss, C. J., Giese, R. F. and Costanzo, P. M., DLVO and non-DLVO interactions in hectorite Clays & Clay Minerals 1990 38 151 – 159 10.1346/CCMN.1990.0380206.Google Scholar
van Oss, C. J., Giese, R. F., Li, Z., Murphy, K., Norris, J., Chaudhury, M. K. and Good, R. F., Determination of contact angles and pore sizes of porous media by column and thin layer wicking J. Adhesion Sci. Technol. 1992 6 413 – 428 10.1163/156856192X00755.Google Scholar