Reactions at the Solid/Solution InterfaceStructure and composition of copper(II)-2,2′-bipyridine sorption complexes on amorphous SiO2
Introduction
This study examines the effect of a specific organic ligand, 2,2′-bipyridine (hereafter referred to as bipy) (Fig. 1 ) on the sorption behavior of aqueous Cu(II) [Cu(H2O)62+] on amorphous silica (am-SiO2) using a combination of macroscopic uptake measurements and spectroscopic techniques. This particular system serves as a simplified example of more complex natural aquatic and soil systems in which metal ions are often complexed or bound by organic matter or mineral surfaces, or both. Such complexation affects the distribution of metal ions between solid and aqueous phases and their speciation in each. This, in turn, affects the mobility, transport, cycling, bioavailability, and toxicity (Babich and Stotzky, 1983) of these ions. Similarly, the thermodynamic stability and the degradation rates of contaminant organic compounds depend on the composition and structure of aqueous and surface complexes in which they are present.
We chose to examine the effects of bipy on the sorption of Cu(II) on am-SiO2 because bipy is a simple, yet important, organic molecule that has been well studied and exhibits interesting effects on the adsorption of metal ions on am-SiO2 and other oxides Bourg et al 1979, Park et al 1993, Ludwig and Schindler 1995. Bipy belongs to a class of organic compounds referred to as nitrogen-containing polycyclic aromatic compounds. Some compounds in this class, which are acutely toxic and have teratogenic activities, have been introduced into the environment. Bipy is the raw starting material for the synthesis of diquat and paraquat (Reglone® and Gramoxone®), which are important herbicides Summers 1980, Matolcsy et al 1988. Related monocyclic compounds are also potentially dangerous environmental contaminants. Pyridine and its derivatives, for example, are present naturally in the environment in trace amounts. They have also been introduced in localized areas at toxic concentrations through agricultural and industrial activities; in particular, the production of synthetic fossil fuel (Ronen et al., 1994). The interaction of these ligands with metal cations can affect the fate and transport of both the ligands and the cations. Among these ligands, bipy has been most studied in the context of coadsorption of metal cations and organic compounds on various metal oxides.
A previous study of the sorption of Cu(II)-bipy complexes on the surface of Aerosil-300 (an amorphous silica made by Degussa) (Ettlinger et al., 1991) revealed that bipy dramatically shifts the pH of Cu(II) sorption on am-silica surfaces to lower values; that is, bipy increases the sorption of Cu(II) on am-silica (Bourg et al., 1979) while retaining the “cation-like” pH dependence. Assuming the formation of type A ternary complexes (complexes where the metal cation bonds directly to the oxygen or hydroxyl group on the mineral surface while retaining its bonding to an organic ligand; Schindler, 1990) and negligible sorption of free bipy, Bourg et al. (1979) were able to fit the uptake data. They and other researchers suggested that increased affinity of Cu(II) for the am-SiO2 surface in the presence of bipy might result from a change in the electronic structure of Cu(II) induced by the coordinated bipy molecules Bourg et al 1979, von Zelewsky and Bemtgen 1982, Schindler 1990 or a more negative free energy of sorption caused by additional interaction of the ligand with the solid surface (Schindler and Stumm, 1987).
Bourg et al. (1979) suggested that Cu(II)-bipy may have a higher affinity for surface functional groups with oxygen donors than free Cu(II) because π-acceptor ligands, like bipy, can draw electron density from the d-orbitals of the metal ion, and therefore, enhance the positive charge of the Cu(II) center Bourg et al 1979, Schindler 1990. This hypothesis is based on the observation that for the analogous reactions in solution, Cu(II)-bipy1 has higher affinity than free Cu(II) for oxalate and phthalate, which are ligands with oxygen donor functional groups (Sigel, 1975). However, the hypothesis is not supported by extended Hückel MO calculations (Schindler, 1990).
von Zelewsky and Bemtgen (1982) studied the influence of a number of organic ligands on Cu(II) sorption on Aerosil 300 using electron paramagnetic resonance (EPR) spectroscopy. Uptake of Cu(II) as a function of pH was also estimated based on the amplitudes of the EPR spectra. Their results confirm that bipy increases sorption of Cu(II) on Aerosil 300. Furthermore, they interpreted the EPR results as indicating that when the ratio of total bipy (bipytot) to total Cu(II) (Cu(II)tot) is 1 or 2 the surface complexes formed are (≡SiO−)Cubipy1 and (≡SiO−)Cubipy2, respectively. The surface complex is (≡SiO−)Cubipy2 when bipytot/Cu(II)tot increases to ≥2. von Zelewsky and Bemtgen (1982) also estimated the stability of the surface complexes to be in the order: (≡SiO−)Cubipy1 ≥ (≡SiO−)Cubipy2 ≫ (≡SiO−)Cu. However, these stability estimates are not sufficient to distinguish among different modes of surface attachment of Cu(II) and Cu(II)-bipy complexes. In summary, EPR spectra suggest that the sorbed Cu(II) and bipy are bonded to each other and that the resulting surface complex is relatively immobile, thus adding weight to the hypothesis of an inner sphere ternary complex with surface SiO− groups.
An alternative explanation for the increased sorption of Cu(II)-bipy, involving hydrophobic interaction of bipy with the surface, was first suggested by Schindler and Stumm (1987). Park et al. (1993) report uptake data that generally support bipy-induced enhancement of Cu(II) sorption. They find weak pH dependence at low pH and increasing enhancement of Cu(II) sorption at higher bipytot/Cu(II)tot ratios, and interpret these observations as evidence that hydrophobic expulsion or bonding contributes to the stability of the ternary surface complex.
The predominant hypothesis adopted by previous investigators suggests that Cu(II) sorbs onto am-SiO2 from aqueous solutions dominated by Cu(II)-bipy1 or Cu(II)-bipy2 as one or more ternary type A complexes bonded to the surface through the Cu(II) ion, perhaps augmented by hydrophobic bonding. In recent work on the system Cu(II)/bipy/TiO2(anatase), Ludwig and Schindler (1995) have also considered the possibility of type B sorption complexes (complexes where the organic ligand bonds directly to the mineral surface and the metal cation is bonded to the organic ligand but not to the mineral surface; Schindler, 1990). Here we test these possibilities for the Cu(II)/bipy/am-SiO2 system in several ways, including:
- 1.
verifying that Cu(II) sorption is enhanced by bipy;
- 2.
determining the stoichiometry of adsorbed bipy to adsorbed Cu(II) on the surface;
- 3.
determining that Cu(II) and bipy are associated in the sorption complex;
- 4.
determining whether any Cu(OH)2 or polynuclear Cu complexes form on the surface in the presence of bipy;
- 5.
determining the mode of sorption, in particular, whether the complex is inner sphere or outer sphere; and
- 6.
assuming the sorption complex is inner sphere, determining whether it is type A (bound to the surface through Cu(II) ions) or type B (bound to the surface through the bipy ligand).
We have used a combination of macroscopic sorption measurements, X-ray absorption fine structure (XAFS), and EPR spectroscopies to determine whether Cu(II) and bipy adsorb independently or are bonded together as a Cu(II)-bipy surface complex. Direct measurement of the sorption densities of both Cu(II) and bipy permit qualitative definition of the influence of bipy on Cu(II) sorption and quantitative calculation of the average bipy/Cu(II) ratio on the surface, and hence help to define the average composition of sorption complexes. The pH dependence of Cu(II) uptake will help to determine whether the sorbed Cu(II) or Cu(II)-bipy complex behaves more like a cation, a neutral complex, or an anion Benjamin and Leckie 1981, Schindler 1990. The infrared (IR) spectra of free aqueous bipy and bipy coordinated to Cu(II) are different Cheah 1997, Cheah et al 1999b, thus IR spectra of the sorption complex can be used to determine whether the majority of sorbed bipy is free or bonded to Cu(II). Similarly, because the EPR parameters of “free” aqueous Cu(II) ion are different from those of Cu(II)-bipy Noack and Gordon 1968, Walker and Sigel 1971, EPR spectroscopy can help determine whether the sorbed copper and bipy are bonded or associated in a complex. This technique can also provide information about the coordination geometry of sorbed Cu(II) (Hathaway and Billing, 1970), and hence about the structure of the sorption complex, because EPR spectra are sensitive to the different stereochemistries of Cu(II) complexes.
X-ray absorption fine structure spectroscopy can provide valuable information on the local structural environment of the Cu(II) center in Cu(II)/bipy/am-SiO2 surface complexes. Most important in this context, quantitative interpretation of Cu-XAFS spectra may permit identification of silicon among second neighbor atoms in the coordination environment of sorbed Cu(II)—and the Cu–Si interatomic distance, RCu–Si. If RCu–Si is so short that neither bipy nor water of hydration can be present between Cu(II) and the Si atom, then we can conclude that Cu(II) forms a direct chemical bond with oxygen on the am-SiO2 surface. Furthermore, any statistically significant difference in the copper to first neighbor (oxygen and possibly nitrogen) distance between the ligand-present and the ligand-absent system is also important information. For instance, a shorter distance in the presence of the ligand would be consistent with the hypothesis that bipy draws electron density from Cu(II) and thus, increases the affinity of Cu(II) for oxygen donor groups on the am-SiO2 surface.
Section snippets
Materials and reagents
Amorphous SiO2 solids were obtained from Degussa under the brand name Aerosil 200. Schindler et al. (1976) had determined the surface area of Aerosil 200 to be 160 m2/g. Water used in the sample preparation was Milli-Q doubly deionized (DDI) grade. It was boiled under nitrogen or sparged with nitrogen before use.
For all experiments in this study, 0.01 or 0.02 M Cu(II)-bipy stock solutions with defined bipy to Cu(II) ratio were used. These Cu(II)-bipy stock solutions were prepared by first
Results
Cu(II)-bipy uptake on am-SiO2 was studied as a function of pH, bipytot/Cu(II)tot, Cu(II) concentration (keeping bipytot/Cu(II)tot constant), and ionic strength. Results of these experiments are discussed later. On the basis of the uptake studies, four sorption samples prepared at different conditions were chosen for spectroscopic study, with the objective of assessing the effects of the surface concentration of the adsorbate and the ratio bipytot/Cu(II)tot on the type of surface complexes
Composition and structure of the surface complexes
Uptake experiments show that bipy enhances Cu(II) sorption onto am-SiO2 at our lowest Cu concentration (Cutot = 0.0001 M), and that bipy inhibits Cu(II) sorption at Cutot = 0.0016 M, for solution bipytot/Cu(II)tot ratios of 1 and 2.
To determine the composition and structure of the surface complexes, it is necessary to combine results from the macroscopic uptake measurements and spectroscopic techniques. Table 4summarizes results from the four sorption samples selected for spectroscopic studies.
Conclusions
Evidence from macroscopic uptake studies and from XAFS, EPR, and FTIR spectroscopic measurements allows us to determine the composition and structure of ternary surface complexes. Uptake experiments show that at bipytot/Cu(II)tot of 1 or 2, bipy enhances Cu sorption onto am-SiO2 at a lower concentration of Cu(II)tot = 0.0001 M, but inhibits Cu sorption at Cu(II)tot = 0.0016 M. The enhancement or inhibition is more pronounced at higher bipy-to-Cu(II) ratios. The ratio of bipy to Cu(II) sorbed is
Acknowledgements
This paper is dedicated to our friend Werner Stumm in recognition of the many contributions he has made in the field of aquatic surface chemistry. We thank Professor Brian J. Hathaway (University College Cork, Ireland) for providing two Cu(II)-bipy model compounds. Gratitude is expressed to Uma Sundaram (Stanford University) for providing the EPR spectrum of Cu(ClO4)2 solution and to Professor Edward Solomon (Stanford University) for allowing us to use his EPR spectrometer. We also thank Drs.
References (42)
- et al.
The chemistry of adsorbed Cu(II) and Mn(II) in aqueous titanium dioxide suspensions
J. Colloid Interface Sci.
(1986) - et al.
XAFS spectroscopy study of Cu(II) sorption on amorphous SiO2 and γ-Al2O3Effect of substrate and time on sorption complexes
J. Colloid Interface Sci.
(1998) - et al.
Adsorption of Cu(II) on the (0001) plane of micaA REFLEXAFS and XPS study
J. Colloid Interface Sci.
(1996) - et al.
The electronic properties and stereochemistry of mono-nuclear complexes of the copper(II) ion
Coordination Chemistry Rev
(1970) - et al.
Surface complexation on TiO2. II. Ternary surface complexesCoadsorption of Cu(II) and organic ligands (2,2′-bipyridyl, 8-aminoquinoline, and o-phenylenediamine) onto TiO2 (anatase)
J. Colloid Interface Sci.
(1995) - et al.
Measurement of soft X-ray absorption with a fluorescence ion chamber detector
Nucl. Instrum. Methods
(1984) - et al.
Hydrophobic effects of o-phenanthroline and 2,2′-bipyridine on adsorption of metal(II) ions onto silica gel surface
J. Colloid Interface Sci.
(1993) - et al.
Ligand properties of surface silanol groups. I. Surface complex formation with Fe2+, Cu2+, Cd2+, and Pb2+
J. Colloid Interface Sci.
(1976) - et al.
Complexation of carbonate species at the goethite surfaceImplications for adsorption of metal ions in natural waters
Geochim. Cosmochim. Acta
(1994) Polycyclic aromatic hydrocarbonsBinary non-aqueous systems
Influence of chemical speciation on the toxicity of heavy metals to the microbiota
The magnetic properties of a series of hydroxo-bridged complexes of 2,2′-dipyridyl and copper(II)
Inorg. Chem.
Conceptual model for metal–ligand–surface interactions during adsorption
Environ. Sci. Technol.
Ternary surface complexes1. Complex formation in the system silica-Cu(II)-ethylenediamine
Chimia
Ternary surface complexes2. Complex formation in the system silica-Cu(II)-2,2′ bipyridyl
Chimia
Basic Characteristics and Applications of AEROSIL
EXAFSPAKA Suite of Computer Programs for Analysis of X-ray Absorption Spectra
Copper
Cited by (7)
Chapter 12.3 X-ray Absorption Spectroscopy
2006, Developments in Clay ScienceCitation Excerpt :Interestingly, these same metals and metaloids behave differently with respect to other mineral surfaces from what was described above for smectites. Thus, the following divalent metals generally form isolated IS complexes at low concentrations, but multinuclear IS complexes at higher sorption densities: Co(II) (Chisholm-Brause et al., 1989a, 1990a, 1991; Towle et al., 1995, 1999a, 1999b), Pb(II) (Chisholm-Brause et al., 1989b, 1990b; Roe et al., 1991; Trainor et al., 2002; Bargar et al., 2004), Cu(II) (Weesner and Bleam, 1997; Xia et al., 1997; Cheah et al., 1998, 1999, 2000; Bochatay et al., 1997) and Zn(II) (Trainor et al., 1999; Trivedi et al. 2001a, 2001b; Roberts et al., 2003). The reasons for these differences in sorption complexes are probably as varied as the number of studies.
Chapter 2 Interactions of heavy metals
2005, Interface Science and TechnologyEXAFS study of mercury(II) sorption to Fe- and Al-(hydr)oxides - II. Effects of chloride and sulfate
2004, Journal of Colloid and Interface ScienceFormation of ternary surface complexes by adsorption of 2,2′-bipyridine onto silica modified with copper ions
2001, Journal of Colloid and Interface ScienceLead sorption on ruthenium oxide: A macroscopic and spectroscopic study
2004, Environmental Science and TechnologyAn overview of synchrotron radiation applications to low temperature geochemistry and environmental science
2002, Reviews in Mineralogy and Geochemistry
- †
Present address: University of California-Berkeley, Division of Ecosystem Sciences—ESPM, Hilgard Hall #3110, Berkeley, CA 94720-3110 USA.