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Characterization of vermiculite by XRD and spectroscopic techniques.

1. Introduction

Vermiculite is a clay mineral usually of secondary origin due to the alteration of mica, pyroxene, chlorite or similar minerals (Brown 1961).

The substitutions of Si by Al in tetrahedral sheet predominate in vermiculite. In this way, the negative charge generated on the tetrahedral sheets limits the expansion properties of the clay and this factor determines the high layer staking of its structure (Mac Ewan and Wilson 1980; Tunega et al. 2003).

From the catalytic point of view, the vermiculite is a very attractive material due to the thermal resistance (Suvorov and Skurikhin 2003) and the number of tetrahedral substitutions, which ensure the presence of a larger number of Br0nsted-type acid sites (del Rey-Perez-Caballero and Poncelet et al. 2000); these substitutions are less numerous in other hydrous 2: 1 minerals such as smectites. On the whole, these properties offer considerable interest in the production of pillared clays, which are distinguishable from an intercalated layered solid due to their micro and/or mesoporosity and high thermal stability with preservation of the layer stacking (Moreno et al. 1997, Schoonheydt et al. 1999; Stefanis etal. 2006).

The development of pillared clays from vermiculite during the past few years has offered particular interest especially as a heterogeneous catalyst in acid-catalyzed reactions (Campos et al. 2005; Campos et al. 2007; Campos and Gagea et al. 2008; Campos and Moreno et al. 2008; Cristiano et al. 2005; del Rey-Perez-Caballero and Poncelet et al. 2000; del Rey-Perez-Caballero and Sanchez et al. 2000, Hernandez et al. 2007). However, as direct intercalation of vermiculite is impossible due to a very high potential of stabilization of interlayer cations (Suvorov and Skurikhin 2003) it has been necessary to develop alternative methodologies to achieve pillared vermiculite (Cristiano et al. 2005; F. del Rey-Perez Caballero 2000).

One of these methodologies has been the hydrothermal treatmentprior to a conventional process of intercalation, in order to reduce negative charge and make possible the subsequent cationic exchange (Cristiano et al. 2005). The catalytic profile of Al and Al-Zr modified vermiculites by means of this methodology has confirmed the potential expected for this acidic acid solid, since they are highly active with respect to other clays in alkane hydroisomerization (Campos 2005; Campos et al. 2007; Campos and Gagea et al. 2008; Campos and Moreno et al. 2008; Cristiano et al. 2005; del Rey-Perez-Caballero and Poncelet 2000; del Rey-Perez-Caballero and Sanchez et al. 2000; Hernandez et al. 2007).

In order to produce practical information to control the modification processes described previously, to achieve a clay mineral with potential catalytic and adsorptive properties, this paper focuses on the characterization of natural vermiculite issued from a Colombian deposit. X-ray diffraction (XRD) and several spectroscopic techniques such as electronic paramagnetic resonance (EPR) and nuclear magnetic resonance (NMR)wereused.

2. Experimental

2.1 Materials

The vermiculite selected for this work was labeled V, and it corresponds to a commercial mineral, which comes from a natural deposit in the Santa Marta region in Colombia. Its characterization was carried out with the fraction of a particle size smaller than 150 [micro]m, separated from the commercial form by sieve, without purification or fractioning treatment.

2.2 Characterization methods

The cationic exchange capacity was determined on the clay previously interchanged with an ammonium acetate solution, by means of the micro-Kjeldahl method (Chapman 1965).

The X-ray diffraction study obtained from flakes, which had been gently pressed onto the plates by using a Philips PW 1820 diffractometer (K[alpha] radiation of Cu, [lambda]=1.54056 [Angstrom], 40 mA, 40 kV) in 2[theta] geometry and Bragg-Brentano configuration, a step size of 0.05 and a step time of 2 s. Diffraction patterns were taken at room temperature, 20 [degrees]C and 65% of humidity on the average.

The identification of the mineral was assessed according to the position of basal reflection 001 in three patterns: i) natural sample, ii) after solvation in the presence of ethylene glycol for 24h and iii) after heating at 500 [degrees]C for 2 h. In addition, [Mg.sup.2+] and [K.sup.+] saturations were performed in the mineral to achieve a better characterization (Thorez 1976).

Adsorption-desorption isotherms of nitrogen at the temperature of liquid nitrogen were analyzed using a Micromeritics Tristar 3000 instrument on samples previously degassed at 200 [degrees]C for 6 h.

Scanning electron microscopy images were recorded in a Philips Scanning Electron Microscope XL30 FEG.

The gravimetric and differential thermal-analysis were performed at a heating speed of 10 [degrees]C min-1 in air atmosphere using a Thermal Analyzer TG and DSC Rheometric instruments.

The chemical analysis was performed by X-ray fluorescence in an XRF 2400 instrument. In addition, the [Fe.sup.2+] analysis was carried out through the analytic method described in Wilson M. (Wilson 1995).

Electron paramagnetic resonance spectra in the X band (9.8 GHz) was carried out in a Brucker ESP 3220 spectrometer adopting a modulation frequency of 100 kHz whose width was fixed at 0.4 mT for wide lines and reduced to 0.05 mT for acute bands, at a temperature of 100 K.

The nuclear magnetic resonance of[sup.27]Al was performed in a Brucker Advance 400 spectrometer; the sample was placed in 2.5mm rotors, while 1200 scannings were accumulated with a time of 100ms of recycle. Rotor speed was 5000 Hz.

XRF, EPR and NMR measurements were done additionally in the mineral washed with nitric acid 0.01 M (10 ml [g.sup.-1] clay) by 1h at 30 [degrees]C.

3. Results and discussion

3.1 X-ray fluorescence (XRF) and cation exchange capacity (CEC)

Table 1 records the chemical composition of the mineral obtained by X-ray fluorescence. The structural formula of the Colombian vermiculite estimated from its chemical composition and following the methodology described in Wilson M. (Wilson 1995) is:


On the other hand, the cationic exchange carried out with ammonium-vermiculite is 1.10 meq [NH.sup.+.sub.4] [g.sup.-1].

3.2 X-raydiffraction analysis

Table 2 shows the comparison between the reflections in XRD for Mg-vermiculite (Brown 1961), those corresponding to a diffraction pattern calculated using DIFK software (Wiewiora et al. 2003) and the reflections observed in the pattern for natural vermiculite V.

This parallel makes it possible to observe an analogue pattern between the clays; thus the clay mineral under study corresponds to vermiculite (Wiewiora et al. 2003). Likewise, a high layer stacking is highlighted, which is verified by the presence of reflections in series 02l and 11 l (Wiewiora et al. 2003).

Reflection 060 located in 0.154 nm indicates that the vermiculite structure is of the trioctahedral type (Dixon and Weed 1989). In general, vermiculite can be dioctahedral or trioctahedral, but trioctahedral type is common in soils with a similar morphology to that of mica (Moore and Reynolds 1997), as observed in vermiculite (Figure 3).

On the other hand, 6th,8th, and 10th order reflections located at 0.480, 0.360 and 0.288 nm respectively show a growing intensities serie typical for vermiculites (Wiewiora et al. 2003). Interstratified material is absent; otherwise the sequence should be abnormal (Wiewiora et al. 2003).

Trioctahedral vermiculites usually formed bythe weathering of biotite (Gordeeva et al. 2002) may be found in the company of this mineral and also talc is possible. In the case of clay V we can suggest that talc is found as a non significant impurity, indicated by its characteristic diffractions in 0.93 nm, 0.48 nm and 0.31 nm (Fagel et al. 2001) (Figure 1). In parallel, starting from the positions of reflections 001 and 004 it can be estimated that the vermiculite is found in a proportion larger than 90 % (Thorez 1976).

In order to verify the purity of the mineral, Table 3 records the follow up on reflection 00l of raw natural clay powder, when the sample is solvated in the presence of ethylene glycol and, when the latter is calcined at 500 [degrees]C. This table shows that the V material exhibits the sequence typical of vermiculites (Thorez 1976; Dixon and Weed 1989).

However different authors (Thorez 1976, Dixon and Weed 1989, Malla and Douglas 1987) suggest complementary analysis XRD in [Mg.sup.2+] and [K.sup.+]-vermiculite to distinguish between soil vermiculites and OH-interlayer vermiculites. As well they suggest a relation between the d001 signal and the layer charge.

After saturation with magnesium followed by glycerol the basal reflection should be located in 1.4 nm compared with 1.8 nm if the clay 2:1 were a smectite (Thorez 1976; Fagel et al. 2001). In this sense, the basal reflection of V located at 1.4 nm was not modified. The impossibility for expansion in Mg-V is then a consequence of the strong retention of magnesium between layers with a high negative

Natural clay (N), after solvation treatment with ethylene glycol (EG) and the latter heated at 500[degrees]C (500). density like vermiculites (Slade et al. 1976, Tunega et al. 2003) (Table 4).

Malla and Douglas (Malla and Douglas 1987) established that the saturation with this potassium originates interlayer space reduction in the region between 1.12 -1.20 nm if the charge is lower than 0.57 and, between 1.00 and 1.06 nm when it is at least 0.6.

In this sense, when clay V was saturated in the presence of [K.sup.+] the basal spacing of 1.4 nm was reduced to 1.0 nm after dried at room temperature and calcinations of the sample at 500 [degrees]C (Table 4). The reduction of interlayer space after potassium saturation, qualitatively indicate that the layer charge must be higher than 0.57 (Malla and Douglas 1987).

In addition, the previous characteristic is a tool for the clear distinction between vermiculite and chlorite, due to the fact that the latter keeps the 001 reflection at 1.4 nm when K-chlorite, while the basal spacing of K-vermiculite is reducedto 1.0 nm (Dixon and Weed 1989). For this reason, the absence of chlorite is verified as a possible impurity in the mineral.

3.3 Thermal analysis

The thermal-gravimetric (TG) and differential (DTA) analysis of vermiculite is presented in the Figure 2 where a total weight loss of 21.1 % is distributed in several regions. In the first one, the dehydration of the clay takes place in two stages: i) between 20 and 110 [degrees]C which corresponds to the loss of water physically absorbed on the surface and ii)from 110 [degrees]C to 500 [degrees]C, with a weight loss of 14.3 % attributed to the exit of water molecules, which are in contact with the cations in the interlayer region (Perez et al. 2003).



The region between 500 and 850 [degrees]C records a loss of 6.8 % in weight with a linear tendency with respect to temperature, which is attributed to dehydroxilation (PerezRodriguez et al. 2004). In fact, the unusual endothermic peak at 800 [degrees]C is associated with the thermal stability on vermiculite which is characteristic of this mineral as well this signal could be assigned to the formation of a new enstatite crystalline phase, which has been reported previously (Perez

et al 2003).

3.4 Texture and morphology

The selected fraction for vermiculite V corresponds to the mineral observed in Figure 3, where large vermiculite layer crystals are detected, which display soft surfaces, with small protuberances. Polygonal sheets with flaked borders are observed in vermiculite formed by the alteration of parental materials (Kishk and Barshad 1969).

The specific surface area (7.41 [m.sup.2] [g.sup.-1]) corresponding to external surface area without any microporosity. The low surface area is related to the particle but as well with the surface charge, since micas with similar particle size and charge higher than vermiculites have less surface area (del Rey-Perez-Caballero and Sanchez et al. 2000).

The strong hydrogen bonds between the tetrahedral sheet and the water of interlayer cations in vermiculite can keep the interlayer zone obstructed (Tunega D. et al. 2003), which could reduce superficial nitrogen adsorption considerably.

By other hand, the relation observed between the interchange cations and the penetration in the interlayer space has been indicated by different authors (Perez et al. 2003). In fact, when monovalent cations in the interlayer region are replaced by those of divalent type, a significant reduction in the superficial area for this mineral clay is observed (Perez et al 2003).


3.5 Electronic paramagnetic resonance (EPR) and nuclear magnetic resonance of aluminum ([sup.27]Al-NMR)

Natural vermiculite can be accompanied by iron oxides and hydroxides on its surface (iron that is not substituting aluminum in the octahedral sheet), which will cause an overestimation of iron in vermiculite if it is evaluated by chemical analysis. In this way, EPR could be used to determine the presence of structural [Fe.sup.3+] in vermiculite. Additionally, to evaluate the structural environment of paramagnetic ions found in the clay.

As can be observed in Figure 4, the EPR of V is dominated by signals associated with [Fe.sup.3+] g = 4.3 and 2.1. In addition, a sextet of lines in g = 2 can be appreciated, which is typical of [Mn.sup.2+] species with distorted octahedral symmetry (Tus!ar et al. 2005).

The signal at g = 4.3 is related with [Fe.sup.3+] located at an orthorhombic environment within the clay structure (Bensimon et al. 2000). In general, smectites exhibit signals for [Fe.sup.3+] between g = 4.3 and g = 2.0, which can be attributed to the combination of two different octahedral and two tetrahedral environments. Their formation depends on the possible organizations of the OH groups in the FeO4(OH)2 unit (Wilson 1995).

Mc Bride et al. (Mc Bride et al 1975) suggest that the difference between the two octahedral sites occupied by [Fe.sup.3+] ions depends on the nature of the adjacent octahedral cation (divalent or trivalent). According to Timofeeva et al. (Timofeeva et al. 2005), the iron found in the form of aggregates in the surface is related with signals in the region comprised between g = 2.3-2.6. Alternatively, different contributions to the wide signal located around g = 2.1 are related with FexOy or FeOOH species (Chung et al. 2004).

In the case of the smectite minerals the signal at g = 4.3 is assigned to the presence of isolated [Fe.sup.3+] in tetrahedral or octahedral coordination, which corresponds to the iron located in the interior of the clay sheets (iron substituting aluminum in the octahedral layers). On the other hand, the signal at g = 2.0 is associated to the presence of clusters of iron (iron extra-red species) (Carriazo et al. 2005).



As observed in Figure 4a, several signals point to the presence of iron extra-red species on the surface of the clay V. For this reason, the clay was submitted to a soft acid wash to remove impurities from its surface. In Figure 4b, the absence of signals between g = 2.3-2.6 indicates that these species had been removed.

Likewise, signals of [Mn.sup.2+] ions located in the region at g = 2, and g = 1.9 (Figure 4a), and the multiple signal recorded is interpreted in terms of the interaction between structural ions [Mn.sup.2+] and [Fe.sup.3+] and other environments (Kessissoglou 1999). After acid wash [Mn.sup.2+] signals remain invariable which suggest structural positions for this cation.

Respect to aluminum, in order to evaluate the structural environment as well as the AL(IV)/AL(VI) ratio to compare with the ratio estimated in the structural formula, 27Al MAS-NMR spectra was made. The spectrum is shown in Figure 5, in which an intense signal at 60 ppm is observed (with two sidebands at -60 and 190 ppm). This signal is associated with Al(IV) substituting the silica in the tetrahedral sheets (Klinowski 1999). A second signal corresponding to Al(IV) at 0 ppm (Klinowski 1999) was observed. The intensity ratio Al (IV)/ Al (VI) was 10.4.

3.6 Correlation of Results

Weaver (Weaver 1958) suggested that vermiculite derived from mica weathering has a high laminar charge and its 001 reflection decrease to 1.0 nm after potassium saturation, as happens in clay V (Table 4). In contrast, vermiculites generated by the weathering of materials like amphiboles or volcanic material exhibit a limited layer contraction with the same treatment.

In fact, the laminar charge is a fundamental element in identification of 2:1 silicates. In fact, the AIPEA (International Association for the Study of Clays) established that vermiculite is a phylosilicate 2:1 with a charge of 0.6 to 0.9 per unit cell (Guggenheim et al. 2006). In this sense, to determine the layer charge of V, it was performed with the structural formula, which was determined through XRF elemental analysis. In it formula can be deduced that the tetrahedral sheet originate an excess negative charge of -0.9 e/ [O.sub.10][(OH).sub.2], which is compensated by [Ca.sup.2+],[Na.sup.+] and [K.sup.+] cations. As regards to the octahedral sheet, formed specially by [Fe.sup.3+] and [Mg.sup.2+] it carries a positive charge of 0.35, resulting in a total negative charge of 0.6 e- / [O.sub.10][(OH).sub.2].

In order to confirm the approach to the elemental organization and to evaluate the environment of the elements found in the structure, EPR and NMR provide very valuable information. Thus, by means of EPR spectroscopy, iron species on the natural clay surface were detected, which can be easily removed through a soft acid wash (Figure 4b). In consequence, the chemical analysis by XRF to evaluate the structural formula was done in the mineral washed with soft acid because unwashed sample could overestimate the iron content.

Regarding the NMR the Al (IV)/Al (VI) ratio (10.4) compared with the ratio estimated with the structural formula (8.9) is a satisfactory approach of vermiculite structure take into account that paramagnetic species such as iron can modify the tetrahedral/octahedral ratio (Gates et al. 1996).

The total negative charge (Malla and Douglas 1987; Guggenheim et al. 2006) observed in the structural formula and the slight difference with the CEC as well as the XRD signals and the follow up of the basal reflection 001 after submitting the sample to different treatments (Thorez 1976; Wilson 1995; Moore and Reynolds 1997) indicate that mineral V is trioctahedral vermiculite.

The knowledge derived from the present work is very useful in further understanding, controlling and predicting the modifications that can be performed on this attractive natural mineral in order to obtain materials with technological impact such as catalyst and adsorbents (Campos et al. 2005; Cristiano et al. 2005; Campos et al. 2007; Campos and Gagea et al. 2008; Campos and Moreno et al. 2008, Hernandez et al. 2007).

5. Conclusion

Mineral clay from a deposit in the region of Santa Marta, Colombia has been characterized through different techniques. The correlation of results indicates that the mineral corresponds to trioctaheral vermiculite as result of the mica-biotite weathering process. The layer stacking, its high thermal stability, low superficial area and the magnitude of its negative charge are characteristic of vermiculite. The details about the structure of this mineral are highly useful in the latter pillaring process of these mineral to enhance their catalytic applications.


This research has been supported by Projects Code HERMES 9887 VRI-DIB-Universidad Nacional de Colombia. The authors wish to thank Professor Pierre Jacobs, director of the Centrum voor Oppervlaktechemie en Katalyse at Katholieke University of Leuven for carrying out the NMR and EPR analysis.


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Manuscript received: 24/03/2009 Accepted for publication: 26/05/2009

A. Campos, S. Moreno, R. Molina (1)

(1) Estado solido y catalisis ambiental, Departamento de Quimica, Facultad de Ciencias, Universidad Nacional de Colombia. AK 30 No. 45-03, Bogota, Colombia; Fax: 57-1- 3165220

Table 1. Chemical composition of Colombian vermiculite.

Oxide [Al.sub.2][O.sub.3] Si[O.sub.2] [Fe.sub.2][O.sub.3] FeO

% 13.06 45.40 6.91 1.24

Oxide MgO MnO CaO [K.sub.2]O [Na.sub.2]O Ti[O.sub.2]

% 24.10 0.11 2.88 0.60 0.26 0.73

Table 2. XRD patterns of Mg-vermiculites, for simulated
pattern and the pattern of Colombian vermiculite.

hkl V Reference (nm)
 1a 2b

002 1.430 1.44 1.43
004 0.719 0.718
006 0.480 0.479 0.477
020 0.468 0.460 0.460
008 0.360 0.360 0.358
115 0.339 0.341
0010 0.288 0.287 0.287
200 0.265 0.265 0.264
132 0.259 0.260 0.258
202 0.254 0.255 0.254
204, 0012 0.240 0.238 0.239
136 0.221 0.227
138, 206 0.206 0.209
208 0.201
2012, 1310 0.187
2010 0.185 0.184
0016, 2014 0.179 0.174
2012 0.168 0.167
1314, 2016 1.580 0.158
060 0.154 0.154 0.154
062, 330 0.153
2018, 0020 0.144 0.144
338 0.136 0.136

a Mg-vermiculite macroscopic of West Chester (Brown 1961).
b Simulated pattern (Wieiora et al. 2003).

Table 3. Identification of vermiculite from the basal reflection
001 (nm).

Clay Mineral N EG 500

Vermiculite 1.4 1.4 0.96-1.0
Smectite 1.2-1.5 1.7 1.0
Chlorite 1.4 1.4 1.4
V 1.4 1.4 1.0

Table 4. Comparison of the first order reflection (nm) for high
and low charge vermiculites and the Colombian mineral

Vermiculite N EG 500 [M.sub.gN]

Low charge 1.4 1.6 1.0 1.4
High charge 1.4 1.4 1.0 1.4
V 1.4 1.4 1.0 1.4

Vermiculite [Mg.sub.EG] [K.sub.N] K500

Low charge 1.6 1.1 1.0
High charge 1.4 1.0 1.0
V 1.4 1.0 9.3

Natural vermiculite after [Mg.sup.2+] saturation
(MgN). MgN after solvation with ethylene glycol ([Mg.sub.EG]).
Natural vermiculite after [K.sup.+] saturation ([K.sub.N]). [K.sub.N]
heated at 500 [grados]C (K500).
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Author:Campos, A.; Moreno, S.; Molina, R.
Publication:Earth Sciences Research Journal
Date:Dec 1, 2009
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