Environ. Sci. Technol. 1994, 28, 204-289 Mechanisms of Chromium( I I I ) Sorption on Silica. 1. Cr( 1I I ) Surface Structure Derived by Extended X-ray Absorption Fine Structure Spectroscopy Scott E. Fendorf,’lt Gerry M. Lamble,* Michael G. Stapleton,$ Michael J. Kelley,ii and Donald L. Sparks5 Soil Science Division, University of Idaho, Moscow, Idaho 83844, Brookhaven National Laboratory, Upton, New York 11973, Department of Plant and Soil Sciences, University of Delaware, Newark, Delaware 197 17, and Engineering Technology Laboratory, DuPont Company, P.O. Box 80304, Wilmington, Delaware 19880-0304 Metal ion reactions at the solid/solution interface are important in an array of disciplines and are of environmental significance as such reactions can greatly affect the risk imposed by metals. The structural environment of metals at the solid/water interface determines their potential for remobilization to the aqueous environment and the physical/chemical modifications of the sorbent. In this study, extended X-ray absorption fine structure (EXAFS) spectroscopy was used to discern the local structural environment of Cr(II1) sorbed on silica. Chromium(II1)formed a monodentate surface complexon silica, with a Cr-Si distance of 3.39 A. At the surface coverages investigated, a polynuclear chromium hydroxide surface phase occurred with Cr-Cr distances of 2.99 A, indicative of edge-sharingCr octahedra. Crystallographicparameters resulting from the measured atomic distances dictate that the surface phase was most likely of the y-CrOOH-type local structure. Environmental considerations of Cr(II1) remobilization must therefore consider the chemical/ physical properties of the monodentate surface-complexed Cr(II1) and surface-nucleated chromium hydroxide. Introduction Inorganic compounds are potential pollutants that can be particularly problematic due to their stability in the environment (i.e., lack of degradation). Chromium is an environmentally significant metal used in various industrial processes: tanneries, plating and alloying industries, and as a cooling water anticorrosion agent. Chromium primarily enters soils and waters at hazardous levels from industrial wastes or spills. Two oxidation states of Cr are stable under surficial conditions, Cr(II1) and Cr(V1). Chromium(V1) is much more hazardous than Cr(II1) because it is mobile through plant and animal membranes and is toxic to cells due to its strong oxidizing nature. In addition, anionic Cr(V1) species are very mobile in the environment. Due to the toxicity and mobility of Cr (VI), the maximum allowable concentration of Cr in drinking water is M (1). It is therefore important to determine reactions that affect the oxidation state of Cr. Chromium(111)oxidation is an important process as the rather benign trivalent species is transformed into the hazardous Cr(VI) species. Fortunately, the only known naturally occurring oxidants of Cr(II1) are manganese oxides (2). The oxidation of Cr(II1) by manganese oxides is dependent upon the formation of a Cr(III)-Mn02 complex; * To whom correspondence should be addressed. University of Idaho. Brookhaven National Laboratory. f University of Delaware. 11 DuPont Company. t t 284 Envlron. Scl. Technoi., Voi. 28, No. 2, 1994 thus, reactions which limit the formation of this complex may decrease the potential for Cr(V1) production. One possible mechanism for retarding Cr(II1) oxidation is its retention by other nonredox reactive sorbents present in soils or waters. This process prevents Cr(II1)complexation with manganese oxides and, consequently, limits its oxidation. An array of studies have investigated the retention of metals by soils and soil components. Although permanently charged aluminosilicate clay minerals often are the dominant sorbents in soils, hydrous oxides can play an important role in the environmental behavior of metal ions. The influence of hydrous oxides, e.g., silica (SiOz), is enhanced by the formation of high surface area particles and surface coatings on other soil materials. Moreover, sorption reactions regulate the risk of metal ions in the environment since the metals are removed from the aqueous phase. Hence, to determine the hazard and risk of Cr in the environment, knowledgeof Cr(II1)sorption on nonredox reactive solids is necessary. Mechanistic interpretations and models have been developed for metal sorption reactions at the oxidelwater interface; however, they have largely been based on macroscopic data without direct atomic-level evidence. Although the heterogeneous nature of hydrous oxide surfaces has been recognized (31, surface complexation models have predominantly been based on the conception of a homogeneous surface with a single surface site, which is composed of a hydroxyl species bound to a central cation, that can undergo protonation (forming a surface water group) or deprotonation (forming an oxo group) reactions. Additionally, the sorbing species is depicted as one that binds only at isolated sites (3-7). Only a few models have considered surface precipitation reactions (8, 9). Recent experimental evidence has indicated that surface nucleation of metal hydroxides occurs much more frequently than previously believed ( I 0-1 5 ) . In this paper, we use the term surface nucleation to denote the general process that marks the onset of a three-dimensional growth mechanism. Polymerization is used to denote the formation of small multinuclear species, such as dimers or trimers, which may lead to nucleation. When a precipitate grows away from the surface before distributing over it, we use the connotation ‘surfacecluster’or ‘island structure’; those which are distributed across the surface are simply termed ‘surface precipitates’. Multinuclear metal hydroxides of Pb, Co, and Cr(II1) on oxides and aluminosilicate minerals have been discerned with extended X-ray absorption fine structure (EXAFS) spectroscopy (10-13, 16). The number of cations present in the polymerized moiety was observed to vary depending on the sorbent. At surface loadings of 1.1-1.2 pmol m-2, Co-hydroxide nucleation was greater on y-Al203 than on rutile or kaolinite (11, 12). Copper(I1) sorption on aluminum oxides was 0013-936X/94/0928-0284$04.50/0 0 1994 American Chemical Society investigated with electron paramagnetic resonance (EPR) spectroscopy (14,15) and was found to progress from an isolated site-binding mechanism to Cu(OH)2 surface nucleation at fractional surface coverage. Only surface functional groups singly coordinated to A1 were observed to be reactive with Cu2+. Advances in understanding metal ion retention mechanisms have been made with the employment of atomic resolution experimentation, but many sorption mechanisms and reaction factors influencing these mechanisms (e.g., pH, ionic strength, competing ions, etc.) remain unresolved. It is important for researchers to utilize techniques, or preferably a multitude of techniques, which give direct evidence for reaction mechanisms. The results of such studies should enhance the development of physically accurate surface complexation models. EXAFS spectroscopy can yield direct information on the local chemical and structural environment of an element. This makes EXAFS a useful method for studying metals ions sorbed on oxides. One should recognize that EXAFS probes the average state of an element in a sample, and thus if the sorbed ion resides in a spectrum of structural environments within a sample it may not be possible to resolve these states. The objective of this study was to determine the structural environment of Cr(II1) on silica using EXAFS spectroscopy. Materials and Methods Batch Studies. The silica used in this study was a Huber Zeothix 265 amorphous Si02 colloid, synthesized as described by Wason (17). The oxide was washed in pH 3.5 HN03and then dialyzed in doubly-distilled deionized water unit a stable conductivity resulted for 24 h. The surface area was 221 m2/g, as determined by the ethylene glycolmonoethyl ether (EGME)method (18). The particle size of the oxide was less than 2.0 pm. Batch studies were performed to determine the amount of Cr(II1) sorbed on Si02 as a function of pH and initial Cr(II1) concentration ([Crl,). A pH range of 3-7 was investigated with initial concentrations of 100, 200,400, and 5 X 103 pM Cr(II1). For the batch studies, 0.5 g of Si02 was dispersed in reaction vessels with 2 L of 0.1 M NaNO3. A 10mM Cr(II1)stock solution was used to obtain the desired Cr(II1) concentrations. The stock solutions were made from ACS reagent-grade Cr(N03)~9H20, with acidified deionized water (pH I2) and were never allowed to age more than 5 days to limit potential polymerization. The oxide was allowed to hydrate for 48 h prior to reaction. After the hydration period, the pH was adjusted, the desired amount of Cr(II1) was added, and the final volume was brought to 2 L, yielding a suspension density of 0.25 g/L. The pH was held constant with a pH-stat system; upon reaching a steady pH, the vessels were placed in a water bath reciprocating shaker. After 48 h, the samples were filtered through a 0.22-pm pore membrane, and the solution was analyzed for Cr with a JY-70 ICP spectrophotometer. The solids were also digested with 12 N "03 and analyzed for total Cr. The sorbed quantities are reported from the loss of Cr(II1)in solution (i.e., changes in Cr solution concentration induced by the silica). The sorption data and structural information gleaned in this study are representative of the reaction after a 48-h time period and, therefore, may not be indicative of sorption at equilibrium (19). Table 1. Solution Speciation and Saturation Indices for 50 pM Cr(II1) at pH 6, As Predicted by the Computer Program MINTEQA2 (23) Using Thermodynamic Values from Rai et al. (24) species %" SI*b Cr3+ 3 Cr(OH)2+ 68 Cr(OH)Z+ 17 Cr(OH)3(aq) 6 . Crz(OH)z4+ <6c 1.5 Cr(OH)s(s) Calculated for species in 0.1 M NaN03. b SI (saturation index) = log (IAP/K,,), where IAP and Kapare the ion activity and solubility products, respectively. c Maximum value based on solubility data of Rai et al. (24) and polymeric Cr(II1) speciation values of Stunzi and Marty (32). All reactions were carried out at 25 f 0.5 "C at 1 atm pressure in aNz(g) environment to eliminate the influences of C02. The initial solutions were purged with Ndg) prior to the addition of the oxide. Thereafter, a Nz(g) stream was maintained over the surface of the fluid when the vessels were exposed to the surrounding environment. Several mechanisms can be operational for the retention of metals on oxides; the term sorption is used to describe the general uptake of a sorptive without implying a specific mechanism, e.g., adsorption or precipitation. Various terms have been used to describe the amount of a metal sorbed on an oxide. In this study the data are referenced to the potential surface site occupancy, 4 4 = (mol of Cr sorbed)/(mol of surface sites) (1) One should be aware that this does not imply a site occupancy but only a potential maximum if each sorbed Cr(II1) occupied a single site. If polymerization or nucleation occurs, then a different amount of the surface sites would be occupied (i.e., an amount less than 4 would be covered). This parameter, 4, is employed because it allows one to easily recognize the quantity of sorbed Cr necessary for monolayer coverage; at less than potential monolayer coverage, isolated site binding can account for the total sorption quantity, but at 4 > 1, nucleation or multilayer adsorption is required. An estimated reactive surface site density of 5.5 site/nm (20)was used to calculate the site density for silica. For XAFS studies, samples reacted at pH 6 were employed for analysis because this pH is common to soils and waters and represents the complete uptake of aqueous Cr onto the silica surface (vide infra). To minimize potential solution polymerization or precipitation, Cr was dispensed in stepwise additions so as to never exceed an aqueous concentration of 50 pM. This concentration was chosen because the solution is only slightly saturated with respect to chromium hydroxide, solution polymerization is minimal (Table 11, and changes in concentration at this level are easily and accurately measured with the methods employed in this study. Solids were consolidated prior to XAFS analysis to maximize the amount of sorbed material analyzed. After 48 h, the suspensions were passed through a 45-mm diameter 0.22-pm membrane filter. The filtrate was then rinsed with 100 mL of high-purity water to remove the entrained electrolyte. In addition, a hydrous chromium oxide (HCO) was precipitated by titrating 20 mM Cr(II1) to pH 6, with pH maintained at this level for 24 h. This procedure was similar to that used by Charlet and Manceau Environ. Scl. Technol., Vol. 28, No. 2, 1994 285 (10). The solid material was then placed in a vial and sealed. The samples remained moist and were never allowed to dry. XAFS Studies. XAFS spectroscopy was performed at the National Synchrotron Light Source, Brookhaven National Laboratory, under dedicated running conditions on beam line X-11A. The electron storage ring operated at 2.528 GeV with currents ranging from ~ 2 1 5mA immediately after a fill to a refill current of 110 mA. A Si(ll1) water-cooled double-crystal monochromator was employed with a sagitally focused beam (21). The focused beam provided an intensity greater than three times that provided by the conventional flat monochromator arrangement over the energy range used for this study. A 0.5-mm pre-monochromator slit width was employed, which was readjusted as necessary to compensate for vertical motion of the stored electron beam. Higher order harmonics were rejected by detuning 30% from the maximum incident intensity (Io). The incident X-ray intensity was measured with a 15cm-long N2(g) filled ionization chamber. Reference materials were run in transmission mode, and the transmitted intensity was measured with a second ionization chamber. All Cr(III)-Si02 systems were analyzed by fluorescence detection. The Cr K edge (5989 eV) was used for analysis. For fluorescence detection, the samples were placed at a 45O angle to the incident beam, and a wide angle collector with an ionization chamber, a Lytle detector (EXAFS Co.), was located 45O off the sample (Le., normal to the incident beam). The Lytle detector was filled with Ar(g) for Cr K a fluorescence detection. A V filter and Soller slits were placed between the sample and the detector to reduce elastically scattered incident X-rays from entering the fluorescence detector. Samples were analyzed at ambient and Nz(1) temperatures (298 and 77 K); no structural differences were discerned between these temperatures, and consequently, the 77 K spectra are reported due to the reduction in thermal disorder. Fluorescence samples were mounted in a 4 X 6 X 25 mm slot cut in an A1 block, which provided good thermal conductance necessary for temperature variation of the samples. These dimensions provided 1mm on each side of the beam and a depth in excessof four adsorption lengths when mounted at 45O to the incident beam. The sample cell was sealed with 0.0005-in. thick Kapton polymide film (CHR Industries, type K-104) to prevent moisture loss while minimizing X-ray absorption. The samples were mounted on a Cu cold finger that was connected to an Nz(1) reservoir. To minimize the heat transfer imposed on the cold finger, samples were precooled by immersion into Nz(1) for several minutes prior to analysis. All samples were run at least in triplicate. Data analyses were accomplished by optimizing the fit of the predicted spectra with Fourier filtered experimental spectra using the program EXCURVE (22). Phase shifts for 0, Si, and Cr were determined by first-principlecalculations and then refined by using model compounds: Cr using a Cr metal and a-Cr203,O with a-Cr203, and Si with Nisi. Amplitude parameters were defined based on a-Cr203. Successive shells were isolated in the Fourier transformed spectra, back-transformed, and the interatomic distances (r's), coordination numbers (CNs), and Debye-Waller factors ( 2 ~ 2 )varied until the best fit was obtained between the predicted and the experimental curves. After obtaining the structural information for each successive shell out to 288 Envlron. Scl. Technol., Vol. 28, No. 2, 1994 100 Initial Aqueous Cr(I1I) 90-1 A rA A 100pM 0 200pM 400 pM 0 0 0 b 0 9 0 0 70 G. 1UJ OYU S & + d Results The sorption of Cr(II1) as a function of pH at various initial aqueous Cr(II1) concentrations is presented in Figure 1. With all the initial concentrations, complete (100%)Cr(II1) sorption occurred by pH 6. Thus, at pH 6 the aqueous concentrations of 100,200,400, and 5 X 103 pM Cr(II1)correspond to potential surface site occupancies (4) of 0.20, 0.40, 0.79, and 9.9, respectively. In addition to surface coverages, the speciation of Cr(II1) in solution can play an important role in affecting the sorption mechanism. In order to equate the solution effects of the different surface loadings investigated and, therefore, isolate the influences induced by the surface, the solution concentrations never exceeded 50 pM Cr(II1). This upper concentration limit was imposed to diminish the potential for solution polymerization or precipitation. Table 1gives the predictedspeciation of 50pM Cr(II1)at pH 6 computed with the program MINTEQA2 (23) using thermodynamic values form Rai et al. (24). These reaction conditions were used for further structural analysis. The extended portion of the XAFS (EXAFS) was utilized to discern the local structural environment of Cr(111)sorbed on silica under reaction conditions conducive for complete Cr(II1)sorption, Le., pH 6. The experimental spectra for the Cr-Si02 systems are shown in Figure 2 along with that of hydrous chromium oxide (HC0)-Cr(OH)3.nH20.Due to possible influencesof self-absorption, spectra of the highest surface loading (4 = 9.9) are not reported. The structural parameters derived from EXAFS analysis are summaried in Table 2. In all of the Cr specimens, approximately six 0 coordinated the Cr at 1.99 A. In the HCO, a second shell composed of two Cr at 2.99 A (edge-sharing CrOe octahedra) and a third shell of 1.5 Cr at 3.98 A (corner-sharing octahedra) were discerned. Thus, the HCO had the y-CrOOH local structure. These results are in good agreement with the structural parameters determined by others for y-CrOOH (16, 25). The first two shells (i.e., six 0 at 1.99 A and Cr at 2.99 A) in all the Cr(III)-Si02 samples were similar to those of - experimental .... predicted n ' .y, x n l ry, x ' , ' \ ' , ' , ' , - experimental .'.. predicted I I 4 6 , 8 I I 10 12 Figure 2. Experimental EXAFS spectra of Cr(II1) sorbed on silica. m Table 2. Structural Information Derived from EXAFS Analysis: Interatomic Distances (r,A), Coordination Numbers (CN), and Debye-Waller Factors (2u2,# ) a Cr-0 r ( A ) CN 7-CrOOH 6 = 0.7gb 6 = 0.40b 6 = O.2Ob 1.99 1.99 1.99 1.98 5.7 6.2 6.0 6.2 Edge: Cr-Cr 2a2 r ( A ) CN 0.008 0.005 0.005 0.005 2.99 3.00 2.98 3.01 1.5 2.3 2.5 2.9 Si-Cr 2a2 r ( A ) CN n ry, x 2a2 0.006 0.010 3.38 1.1 0.009 0.010 3.40 1.0 0.008 0.011 3.39 0.71 0.009 a The 0, edge-sharing Cr octahedra, and Si coordination shell of a central Cr are reported. Based on standards and internal deviation, the reported values are accurate to within r f 0.03 A, CNc,.o f 20%, and CNc,-c, and CNsixr f40%. Potential surface site coverage for Cr(II1) sorbed on silica (mol of Cr/mol of surface sites). ' I 6 I , I 10 8 7 - 7 12 A-1 the chromium hydroxide, with higher CN values. However, the fit between the predicted and the experimental curves was greatly improved with the inclusion of a Si atom. Thus, a different third shell resided in these materials: a single Si atom at 3.39 8, (Figure 3). The SiCr distance of 3.39 A represents a monodentate complex, in agreement with the CN, and would necessitate a 150' Cr-0-Si bond angle. Consolidating the structural parameters derived from the isolated shells resulted in good agreement between the predicted and the experimental functions for the samples (Figure 4). Beyond the Si shell, the EXAFS intensity is much weaker than the inner-shells, and therefore, we could not place confidence in the derived structural values. Nonetheless, further structural information was obtained based on crystallographic considerations and the measured atomic distances. With a Cr0-Si bond angle of 150°, adjacent Cr atoms would necessitate a Cr-Cr distance of approximately 3.9 A, assuming the silica surface to be composed of alternating Si tetrahedra. These values indicate that the surfacenucleated chromium hydroxide phase had the local y-CrOOH-type structure-similar to that of the homogeneous HCO precipitate. In the second part of this sereis (23,infrared spectra are presented which confirm the Figure 4. EXAFS function for the Fourier back-transformed spectra. The theoreticalline was derivedwith parametersobtainedfrom analysis of the isolated shells. presence of a y-CrOOH-type phase-as noted by the CrOH-Cr deformation mode. Although chromium hydroxide nucleation was observed in all of the Cr-Si02 systems, the extent of nucleation varied depending on 4. Figure 5 gives the relative intensities of the atomic shells in the Fourier transformed spectra (the radial structure function, RSF). The second peak (centered at approximately 3 A) composed of Si and edge-sharing Cr octahedra is apparent in all of the RSFs. Figure 6 illustrates the chromium silica surface structure derived from EXAFS analysis and crystallographic considerations. For alternating silicon tetrahedra linkages (261,the distances arising between apical 0 would produce favorable distances for hydroxyl bridging of surfacecomplexed Cr, provided the Cr are angled toward each other, as depicted in Figure 6. Thus, it appears that chromium(II1) hydroxide nucleation occurs on silica with a y-CrOOH-type local structure, similar to that observed for precipitation on 6-MnOz (27,28) and homogeneous solution precipitation (i.e., HCO). The second paper of Environ. Scl. Technol., Vol. 28. No. 2, 1994 287 - .... 1 I I 2 3 , 4 experimental predicted I 5 A Flgure 5. Fourier transformed spectra resulting in the radial structure function (RSF) of the inner 4 &shells: HCO and Cr sorbed on silica are shown. The first peak results from six 0 at 1.99 A; the second from Cr at 2.99 8.In the presence of Si, the second peak incorporates SI at 3.39 A. /*' Flgure 6. Depiction of the surface structure derived by EXAFS analysis (a) showing the interatomic distances for Cr sorbed on silica. The y-CrOOH-type structure is shown forming in panel a, and in panel b the interatomic distances of this phase are given. this series (25) gives further evidence for the 7-CrOOHtype local structure structure on silica. Discussion EXAFS analysis indicates that Cr(II1) formed an innersphere monodentate surface complex on silica. A Si-Cr 288 Environ. Sci. Technoi., Vol. 28, No. 2, 1994 distance of 3.39 A was determined; a linear Cr-0-Si arrangement would result in a distance of 3.59A, and thus, a bond angle of 150' is necessary to produce the observed distance. This Cr-Si distance and angle are similar to that observed for Mn in MnSiOs (29). Monodentate coordination with a bond angle of 150' implies that the reactive surface 0 atoms are singly coordinated by Si. This complexation structure agrees with the multisite surface complexation (MUSIC) model (30, 3I), which indicates that only the singly-coordinated 0 of Si02 are reactive in the pH range of 2-10. McBride et al. (15) and McBride (14) also observed that Cu2+ sorbed only to singlycoordinated 0 groups on aluminum oxides. A t coverages equal to and exceeding 0.20, surface nucleation of the y-CrOOH-type structure occurred. Chromium hydroxide nucleation on goethite was also observed (IO). However, a deviation from the yCrOOH local structure occurred at the goethite interface (IO); surface-nucleated Cr(II1) formed the a-CrOOH-type structure ( I O ) . As surface coverageincreased, nucleation growth expanded over the surface before expanding outward (away from the surface). Further increases in Cr(II1) levels resulted in nucleation progressing outward from the a-FeOOH surface, and there was a phase transition from the a- to the y-CrOOH-type structure. It appears that Cr(II1) sorption on silica is similar to that on goethite in that surface precipitation occurred prior to monolayer coverageand under conditions where solution precipitation was not observed (25). In contrast to sorption on goethite, however, a monodentate surface complex formed on silica, and the nucleation of y-CrOOH was not extensively distributed over the surface but appears to have formed surface clusters-island structures (25). Determining the sorption mechanism of metal ions at the oxide/solution interface is necessary for evaluating their hazard in the environment. The accuracy of mechanistic models utilized for predicting the fate of metals in colloidalsystems will be enhanced by incorporating results from atomic level experimentation. The surface structure of sorbed metals determines their potential for remobilization. The strength of retention will differ depending on whether nucleation of a metal hydroxide has occurred, and it will depend on the structure of the metal hydroxide (i.e.,different polymorphs often have different solubilities). Furthermore, the sorbent will be modified by the sorption process and the resulting chemical/physical properties determined by the sorption mechanism. For Cr(II1) sorption on silica, at potential surface coverages greater than 20 % ,surface nucleation of chromium hydroxide with the y-CrOOH-type local structure occurred in addition to a monodentate surface complex; the final conglomerated colloid would exhibit chemical/physical properties of the surface clusters and the unreacted silica. One should be aware, however, that since XAFS probes the average state of an element there is the potential for small quantities of Cr(II1) to reside in other surface structures. Additionally, the surface clusters may underto a structural rearrangement with time. Nevertheless, the dominant processes influencing Cr(II1) sorption on silica can be modeling considering both monodentate and surface nucleation sorption mechanisms. In this portion of the study, the surface structure of Cr(II1) on silica was discerned. In the second part of this series (25),the reaction factors (degree of surface coverage, pH, and initial aqueous Cr concentration) are investigated as to their effects on the sorption mechanism and the resulting surface structure. Acknowledgments We would like to acknowledge the US.Department of Energy, Division of Materials Sciences, under Contract DE-FG05-89ER45384, for its role in the operation and the development of beam line X-11A at the National Synchrotron Light Source. The NSLS is supported by the Department of Energy, Division of Materials Sciences and Division of Chemical Sciences, under Contract DEAC02-76CH00016. L i t e r a t u r e Cited U.SEPA. Code of Federal Regulations. Title 40, National Interim Primary Drinking Water Regulations, Part 141. U.S.EPA: Washington, DC, 1984. (2) Eary, L. E.; Rai, D. Environ. Sci. Technol. 1987, 21, 547. (3) Schindler, P. W.; Stumm, W. In Aquaticsurface chemistry; Stumm, W., Ed., Wiley and Sons: New York, 1987; pp 83110. (4) Davis, J. A.; James, R. 0.;Leckie, J. 0.J. Colloid Interface Sci. 1978, 63, 480. (5) Hayes, K. F.; Leckie, J. 0. In Geochemical processes at mineral surfaces; Davis, J. A., Hayes, K. F., Eds.; ACS Symposium Series 323; American Chemical Society: Washington, DC, 1986; pp 141-158. (6) Berube, Y. G.; De Bruyn, P. L. J. Colloid Interface Sci. 1968, 27, 305. (7) Yates, D. E.; Levine, S.;Healy, T. W. J. Chem. SOC.Faraday Trans. 1974, 70, 1807. (8) Farley, K. J.; Dzombak, D. A.; Morel, F. M. M. J . Colloid Interface Sci. 1985, 106, 226. (9) James, R. 0.;Healy, T. W. J. Colloid Interface Sci. 1972, 40, 53. (10) Charlet, L.; Manceau, A. J. Colloid Interface Sci. 1992,148, 443. (11) Chisholm-Brause, C. J.; O'Day, P. A.; Brown, G. E., Jr.; Parks, G. A. Nature 1990, 348, 528. (12) Chisholm-Brause, C. J.; Row, A. L.; Hayes, K. F.; Brown, G. E., Jr.; Parks, G. A.; Leckie, J. 0. Geochim. Cosmochim. Acta 1990,54, 1897. (1) (13) Bleam, W. F.;McBride, M. B. J. Colloid Interface Sci. 1986, 110, 335. (14) McBride, M. B. Clays Clay Miner. 1982, 30, 21. (15) McBride, M. B.; Fraser, A. R.; McHardy, W. J. Clays Clay Miner. 1984, 32, 12. (16) Corker, J. M.; Evans, J.; Rummey, J. M. Mater. Chem. Phys. 1991,29, 201. (17) Wason, S. K. J. SOC.Cosmet. Chem. 1978,29, 307. (18) Heilman, M. C.; Carter, D. L.; Gonzalez, C. L. Soil Sci. 1965, 100, 409. (19) Wehrli, B.; Ibric, S.; Stumm, W. Colloids Surf. 1990,51,77. (20) Fouad, N. E.; Knozinger, H.; Zaki, M. I.; Mansour, A. A. 2. Phys. Chem. (Munich) 1991, 171, 75. (21) Lamble, G. M.; Heald, S. M. Rev. Sci. Instrum. 1991, 63, 880. (22) Gurman, S. J.; Binstead, N.; Ross, 1. J. Phys. C 1984, 17, 143. (23) Allison, J.; Brown, D. S.; Nova-Gradac, K. J. MINTEQA2I PRODEFA2, A geochemical assessment model for enuironmental systems: Version 3.0; U.S. Environmental Protection Agency: Athens, GA, 1990. (24) Rai, Do; Sass, B. M.; Moore, D. A. Inorg. Chem. 1987, 26, 345. (25) Fendorf, S. E.; Sparks, D. L. Environ Sci. Technol. 1994, following paper in this issue. (26) Wells, A. F. Structural inorganic chemistry; Clarendon Press: Oxford, U.K., 1984. (27) Fendorf, S. E.; Fendorf, M.; Sparks, D. L.; Gronsky, R. J . Colloid Interface Sci. 1992, 148, 37. (28) Manceau, A.; Charlet, L. J. Colloid Interface Sci. 1992,148, 425. (29) Wyckoff, R. W. G. Crystal Structures; Interscience Publishing: New York, 1963. (30) Hiemstra, T.;Van Riemsdijk, W. H.; Bolt, G. H. J. Colloid Interface Sci. 1989, 133, 91. (31) Hiemstra, T.; De Wit, J. C. M.; Van Riemsdijk, W. H. J. Colloid Interface Sci. 1989, 133, 105. (32) Stiinzi, H.; Marty, W. Inorg. Chem. 1983,22, 2145. Received for review April 19, 1993. Revised manuscript received September 10, 1993. Accepted October 20, 1993.' Abstract published in Advance ACS Abstracts, December 1, 1993. @ Environ. Scl. Technol., Vol. 28, No. 2, 1994 289