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The Kinetics of Calcite Growth: Interpreting Chemical Affinity-Based Rate Laws Through the Lens of Direct Observation

Published online by Cambridge University Press:  14 March 2011

Henry H. Teng
Affiliation:
Department of GeologyGeorge Washington University, Washington, D.C. 20052
Patricia M. Dove
Affiliation:
Department of Geological Sciences Virginia Polytechnic Institute and State University Blacksburg, VA 24061
James J. De Yoreo
Affiliation:
Department of Chemistry and Materials Science Lawrence Livermore National Laboratory Livermore, CA 94550
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Abstract

Chemical affinity-based rate laws are used across the geochemical and materials communities to quantify mineral/material corrosion and growth kinetics. These rate expressions are founded in assumptions regarding reaction mechanism with little evidence for surface processes. Using Atomic Force Microscopy (AFM), this study demonstrates the dependence of growth kinetics upon the structures of dislocation sources. In situ observations show that the dominant mode of growth occurs by hillock development initiated at complex sources. Derivations of surface process-based rate expressions show a complex dependence of rate on chemical affinity. This dependence is approximated by second order affinity-based rate laws only under the special conditions that 1) growth proceeds by development of single sourced spirals and 2) growth occurs at very near equilibrium conditions where spiral formation is the only operative mechanism. This suggests that growth experiments that measure temporal changes in solution chemistry yield a composite rate that arises from the contributions of the different hillock types. Hence, chemical affinity-based rate laws do not generally give meaningful interpretations of growth mechanism. By combining direct observations with macroscopic methods that monitor temporal changes in solution chemistry, rate laws with greater predictive capabilities may be possible.

Type
Research Article
Copyright
Copyright © Materials Research Society 2000

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References

1. Nancollas, G. H. and Reddy, M. M. (1971) The crystallization of calcium carbonate II: Calcite growth mechanism. J. Colloid Interface Sci. 37, 843–830.Google Scholar
2. Plummer, L. N., Wigley, T. M. L., and Parkhurst, D. L. (1978) The kinetics of calcite dissolution in CO2-water systems at 5-60°C and 0.0-1.0 atm CO2 . Amer. J. Sci. 278, 179216.Google Scholar
3. Busenberg, E. and Plummer, L. N. (1986) A comparison study of the dissolution and crystal growth kinetics of calcite and aragonite. USGS Bull. 1578, 139168.Google Scholar
4. Christoffersen, J. and Christoffersen, M. R. (1990) Kinetics of spiral growth of calcite crystals and determination of the absolute rate constant. J. Crystal. Growth 100, 203211.Google Scholar
5. Shiraki, R. and Brantley, S. L. (1995) Kinetics of near-equilibrium calcite precipitation at 1000C: An evaluation of elementary reaction-based and affinity based rate laws. Geochim. Cosmochim. Acta 59, 14571471.Google Scholar
6. Nilsson, Ö and Sternbeck, J. (1998) A mechanistic model for calcite crystal growth using surface speciation. Geochim. Cosmochim. Acta 63, 217226.Google Scholar
7. Arakaki, T. and Mucci, A. (1995) A continuous and mechanistic representation of calcite reaction-controlled kinetics in dilute solutions at 25°C and 1 Atm total pressure. Aquatic Geochemistry, 1, 105130.Google Scholar
8. Smallwood, P. V. (1977) Some aspects of the surface chemistry of calcite and aragonite. Colloid and Polyner Sci. 255, 9941000.Google Scholar
9. Reddy, M. M. (1977) Crystallization of calcium carbonate in the presence of trace concentrations of phosphorous-containing anions. J. Crystal Growth 41, 287295.Google Scholar
10. Reddy, M. M. and Gaillard, W. D. (1980) Kinetics of calcium carbonate (calcite)-seeded crystallization: Influence of solid/solution ratio on the reaction rate constant. J. Colloid and Interface Science, 80, 171178.Google Scholar
11. Reddy, M. M. (1988) Physical-Chemical mechanisms that affect regulation of crystallization. In Chemical Aspects of Regulation of Mineralization (eds. Sikes, C. S. and Wheeler, A. P.), 3-8, University of South Alabama Pub. Ser., Mobile, Alabama.Google Scholar
12. Compton, R. G. and Daly, P. J. (1987) The dissolution/precipitation kinetics of calcium carbonate: An assessment of various kinetic equations using a rotating disk method. J. Colloid. Interface Sci. 115, 493498.Google Scholar
13. Reddy, M. M. and Nancollas, G. H. (1971) The crystallization of calcium carbonate I. Isotopic exchange and kinetics. J. Colloid and Interface Science, 36, 166172.Google Scholar
14. Morse, J. W. (1978) Dissolution kinetics on calcium carbonate in sea water VI: The near equilibrium dissolution kinetics of calcium carbonate-rich deep sea sediments. Amer. J. Sci. 278, 344353.Google Scholar
15. House, W. (1981) Kinetics of crystallisation of calcite from calcium bicarbonate solutions. J. Chem. Soc. Faraday Trans. 77, 341359.Google Scholar
16. Nielsen, A. E. (1983) Precipitates: formation, coprecipitation, and aging. In Treatise on Analytical Chemistry (eds. Kolthoff, I. M. and Elving, P. J.), 269374, Wiley, New York.Google Scholar
17. Mucci, A. (1983) The solubility of calcite and aragonite in seawater at various salinities, temperatures, and one atmosphere total pressure. Amer. J. Sci. 283, 780799.Google Scholar
18. Mucci, A. and Morse, J. W. (1983) The incorporation of Mg and Sr into calcite overgrowths: Influences of growth rate and solution composition. Geochim. Cosmochim. Acta 47, 217233.Google Scholar
19. Mucci, A. (1986) Growth kinetics and composition of magnesian calcite overgrowths precipitated from seawater: Quantitative influence of orthophosphate ions. Geochim. Cosmochim. Acta 50, 22552265.Google Scholar
20. Kazmierczak, T. F., Tomson, M. B., and Nancollas, G. H (1982) Crystal growth of calcium carbonate: A controlled composition kinetic study. J. Phys. Chem. 86, 103107.Google Scholar
21. Lasaga, A. C. (1981) Transition state theory. In Kinetics of Geochemiscal Processes (eds. Lasaga, A. C. and Kirkpatrick, R. J.); Rev. Mineral., 135-169.Google Scholar
22. Blum, A. E. and Lasaga, A. C. (1987) Monte Carlo simulations of surface reaction rate laws. In Aquatic Surface Chemistry (ed. Stumm, W.), 255292, Wiley, New York.Google Scholar
23. Reddy, M. M. and Nancollas, G. H. (1973) Calcite crystal growth inhibition by phosphates. Desalination 12, 6173.Google Scholar
24. Inskeep, W. P. and Bloom, P. R. (1985) An evaluation of rate equations for calcite precipitation kinetics at Pco2 less than 0.01 atm and pH greater than 8. Geochimica et Cosmochimica Acta 49, 21652180.Google Scholar
25. Burton, W. K., Cabrera, N., and Frank, F. C. (1951) The growth of crystals and the equilibrium structure of their surfaces. Royal Soc. London Philos. Trans. A243, 299358.Google Scholar
26. Rashkovich, L. N. (1991) KDP-family single crystals. 100165, IOP Pub., Norfold, England.Google Scholar
27. Vekilov, P. G. and Kuznetsov, Yu. G. (1992) Growth kinetics irregularities due to changed dislocation source activity: (101) ADP face. J. Crystal Growth, 119, 248260.Google Scholar
28. Vekilov, P. G. and Rosenberger, F. (1996) Dependence of lysozyme growth kinetics on step sources and impurities. J. Crystal Growth, 158, 540551.Google Scholar
29. Land, T. A., De Yoreo, J. J., and Lee, J. D. (1997) An in situ AFM investigation of canavalin crystallization kinetics. Surf. Sci. 384, 136155.Google Scholar
30. Teng, H. H., Dove, P. M., Orme, C. A., and DeYoreo, J. J. (2000) Kinetics of calcite growth: Surface processes and relationships to macroscopic rate laws. Geochimica et Cosmochimica Acta, 64, in press.Google Scholar
31. Teng, H. H., Dove, P. M., Orme, C. A., and DeYoreo, J. J. (1998) Thermodynamics of calcite growth: Baseline for understanding biomineral formation. Science, 282, 724727.Google Scholar
32. Teng, H. H. and Dove, P. M. (1997) Surface site-specific interactions of aspartate with calcite during dissolution: Implications for biomineralization. Amer. Mineral. 82, 878887.Google Scholar
33. Stipp, S. L., Eggleston, C. M., and Nielsen, B. S. (1994) Calcite surface structure observed at microtopographic and molecular scales with atomic force microscopy (AFM). Geochimica et Cosmochimica Acta, 58, 30233033.Google Scholar
34. Teng, H. H., Dove, P. M., and DeYoreo, J. J. (1999) Reversed calcium carbonate morphologies induced by microscopic growth kinetics: Insight into biomineralization. Geochimica et Cosmochimica Acta, 63, 25072512.Google Scholar
35. Chernov, A. A. (1961) The spiral growth of crystals. Soviet Phys. 4, 116148.Google Scholar
36. Chernov, A. A. and Komatsu, H. (1995) Topics in crystal growth kinetics. In Science and Technology of Crystal Growth (eds. Eerden, J. P. van and Bruinsma, O. S. L.), 6780, Kluwer Acad. Pub., Amsterdam.Google Scholar
37. Van der Eerden, J.P. (1993) Crystal Growth Mechanisms. In Handbook of Crystal Growth (ed. Hurle, D.J.T.) 1A, 307475.Google Scholar