# Dynamics of Kaolinite-Urea Nanocomposites via Coupled DMSO-Hydroxyaluminum Oligomeric Intermediates

Authors: Siafu Ibahati Sempeho; Hee Taik Kim; Egid Mubofu; Alexander Pogrebnoi; Godlisten Shao; Askwar Hilonga
Journal: Indian Journal of Materials Science
 (2015)

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## Abstract

Kaolinite-urea nanocomposites were prepared via intercalation reactions in an attempt to investigate the dynamic nature of kaolinite morphology for advanced applications in controlled release systems (CRS). Characterization was done using SEM-EDX, XRF, ATR-FTIR, XRD, and DT/DTG; Andreasen pipette sedimentation technique was used to determine the grain size distribution of the raw kaolinite. The X-ray diffraction pattern revealed the existence of an FCC Bravais lattice where the intercalation ratios attained were 51.2%, 32.4%, 7.0%, and 38.4% for hydroxyaluminum oligomeric intercalated kaolinite, substituted urea intercalated kaolinite, calcined DMSO intercalated kaolinite, and hydroxyaluminum reintercalated kaolinite, respectively, along with their respective crystallite sizes of 33.51–31.73 nm, 41.92–39.69 nm, 22.31–21.13 nm, and 41.86–39.63 nm. The outcomes demonstrated that the employed intercalation routes require improvements as the intercalation reactions were in average only ≈32.3%. The observations unveiled that it is possible to manipulate kaolinite structure into various morphologies including dense-tightly packed overlapping euhedral pseudo hexagonal platelets, stacked vermiform morphologies, postulated forms, and unique patterns exhibiting self-assembled curled glomeruli-like morphologies. Such a diversity of kaolinite morphologies expedites its advanced applications in the controlled release systems (CRS) such as drug delivery systems and controlled release fertilizers (CRFs).


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## Body

## 1. Introduction

Contemporaneously, researchers have been interested in the investigation of the intercalation reactions (IRs) that involves kaolinite layered phyllosilicates for the purpose of scientific and technological advancements in the areas of catalysis; water filtration; composites; nanotechnology; controlled released formulations [1, 2] such as drug delivery systems (DDSs) and controlled release fertilizers (CRFs) [3–10]. Progressive application of kaolinite in the engineering designs has been practically feasible owing to the fact that kaolinite (which is an inexpensive chemical mineral) can be modified through ion exchange mechanisms by just intercalation of ionic species into the kaolinite interlayer spaces. Primarily, the hydrated form of the kaolinite mineral consists of kaolinite sheets interspersed with monomolecular sheets of water molecules. This is an essential feature for intercalation reactions; elsewhere this property was termed asclay’ advantageous properties[11, 12]. According to [13], the fate of the mentioned ion-exchange mechanism includes (i) the widening of gap between the single sheets thereby facilitating the insertion of organic species into the interlayer spaces and (ii) the alteration of the surface charges of each single sheets from being hydrophilic to organophilic [14]. The likelihood that an intercalation reaction will be feasible depends on the interactions between polar functional group-containing compounds and layered phyllosilicates such as kaolinite; in most cases the mechanism involves the interaction between clays with exchangeable cations plus interactions with siloxane surfaces via surface adsorption [15]. In addition, the ion-dipole mechanism is also known to influence kaolinite interactions [15]; this mechanism involves either the direct interactions of organic compounds with exchangeable cations or in-direct interaction through the intermediation of water molecules surrounding the cations. By the same token, an increase in the charge valence of exchangeable cation is known to enhance the ion-dipole interactions [15–18]. However, it has been evidenced that nonpolar surface interactions between organic compounds and the siloxane surfaces of the clays may also occur. Likewise, the weakening of ion-dipole interactions may take place at times when water molecules surrounding strongly hydrated cations such as Ca2+ and Mg2+ inhibit the direct interaction between polar functional groups and the exchangeable cations [15, 19–21].Profoundly, the presence of charges on the clay minerals is an inherent property which facilitate most intercalation reactions and the main source of these charges on the clay minerals is isomorphous substitution reactions (permanent charge due to isomorphous substitution) for the reason that it confers permanent charge on their surface of the layers [1].Furthermore, the development of charges on the clay surfaces can also be attributed to (i) the ionization of hydroxyl groups and (ii) the presence of surface and broken-edge OH− groups apart from the major isomorphous substitution reactions [1]. That is to say, pH-dependent charge (which is not permanent as for the isomorphous substitution) develops when there is ionization of hydroxyl groups on the surfaces of other particles (pH-dependent charges on the edges describing the fact that, at lower pH, H+ are tightly bound and so have less tendency to intercalations). Besides, the presence of surface and broken-edge OH− groups (which exposes the functional groups for maximum interactions) gives rise to the ideal electronegativity (which is a necessary property in this context) along with the kaolinite particles’ ability to adsorb and so intercalate ionic species. Thus, as pointed out by [1], clay particles are stacked in layers like sheets of papers where each sheet is slightly separated from those on either side and has negative charges on it which could be balanced by positive ionic species, phenomena which are critical for the kaolinite interactions including intercalations reactions among others.In this paper, we report the dynamic morphological changes in the kaolinite nanocomposite structures based on the urea intercalated kaolinite as a function of DMSO-hydroxyaluminum oligomeric intermediate intercalation compounds and calcination reactions. The aim was to study the changes associated with coupling DMSO intercalated kaolinite along with hydroxyaluminum oligomeric cations to prepare well-ordered self-assembled nanocomposite excipients (for use in the CRFs and DDs) exhibiting unique curled patterns.


## 2. Materials, Preparation, and Characterization

### 2.1. Materials

Kaolinite was collected at Pugu hills in the Coast region Kisarawe Tanzania by using quartering sampling technique described in [22]. Urea (ACS reagent, 99-100%) was supplied by Sigma Aldrich, DMSO (Extra pure, ≥99.5%) was supplied by Daejung Chemicals & Metals Co. Ltd., Gyonggi-do, Korea, sodium chloride (Extra pure, ≥99.0%) was supplied by Samchun Pure Chemicals Co., Ltd., Gyonggi-do, Korea, silver chloride (ACS reagent, 99.0%) was supplied by Sigma Aldrich, deionized distilled water (D.I.) was supplied by Professor Kim’s Lab, sodium hydroxide (extra pure grade, min 93.0%) was supplied by Duksan Pure Chemical, Ansan City, Kyungkido, South Korea, and aluminium chloride (99.99%) was supplied by Junsei Chemical Co., Ltd., Japan.


### 2.2. Materials Preparation

#### 2.2.1. Beneficiation and Treatment of Raw Samples

Wet beneficiation technique was achieved by simple size separation using “classifier.” The method involved the separation of fine platy kaolinite from coarser quartz, feldspar mica, and other impurities using different setting velocities associated with particle size as governed by Stockes’s law [43–50]. The entire procedure which involved crushing to pulverization and soaking as well as running the classifier unit to drying has been comprehensively described in [51]. Pugu kaolinite (10 g) was dispersed in 1000 cm3 of 0.1 M NaCl solution and treated ultrasonically at 50°C for 30 hours and then constantly magnetically stirred for more 30 hours. The product was filtered under vacuum filter and washed several times to remove excessive chlorides; washing was stopped after negative reaction with AgNO3. The washed product was dried in a vacuum oven at 60°C and stockpiled as B1.


#### 2.2.2. Preparation of Kaolinite-Intercalation Nanomaterials

AlCl3 solution (0.1 M) was mixed with 0.1 M NaOH solution at a 1 : 2 molar mixing ratio, respectively. The mixture was stirred at 85°C for 6 hours and then aged for 12 hours. A 5% beneficiated kaolinite suspension was prepared and was ultrasonically mixed with an excess of hydroxyaluminum oligomeric solution at 70°C for 3 hours. The product was named B2 which was then washed in a vacuum pump to remove unreacted materials and chloride ions as tested by AgNO3 solution. By using B2 powder as a starting material, a small portion was taken and then mixed with 5 g of urea and stirred for 72 hours at 60°C. The urea-kaolinite nanocomposite obtained was washed in a vacuum pump with excess water and dried at 60°C in a vacuum oven and stored as B3. A small portion of beneficiated and modified Pugu kaolinite was magnetically stirred with DMSO solution in a ratio of 1 : 6 for 21 days at 80°C with a very small addition of water droplets. The suspension was then aged for 7 days and then washed with excess isopropanol and dried at 60°C in a vacuum oven to obtain powder. The DMSO intercalated kaolinite obtained in powder form was calcined at 850°C (10°C/min) for 8 hours with 6-hour holding time and cooling rate of 7°C/min. The calcined sample was named B4. To the calcined powdered sample, 0.38 g was measured in a Sartorius analytical balance and mixed with 0.98 g of urea in excess of hydroxyaluminum oligomeric solution prepared as described above. The mixture was stirred at 105°C to dryness and the powder obtained was named B5.


### 2.3. Characterization

#### 2.3.1. Infrared Spectroscopy

By using a Bruker Optic GmbH (alpha model, Laser class 1) Spectrometer with attenuated total reflectance (ATR) the FTIR-ATR measurements were performed in the near infrared region at wavelength between 7500 and 360 cm−1.


#### 2.3.2. X-Ray Diffraction

SIEMENS D-5005 X-ray Diffractometer (Cu Kα1 radiation and 2θ scan range which was between 2° and 65°) was used to determine raw kaolinite mineralogy whereas the XRD patterns for the intercalation compounds were executed on RIGAKU COORPERATION, D/MAX-2500/PC X-ray Diffractometer (Cu Kα1) equipped with a back monochromator operating at 40 kV and 100 mA at the scanning range of 5°–80° with a step of 0.1° and a time/step of 1 s.


#### 2.3.3. Thermogravimetry (TG/DTG)

Thermograms were taken using TG/STA Linseis STA PT 1000 simultaneous TG/DTG thermal analyzer at a scanning rate of 5°C per min from room temperature to 800°C under nitrogen atmosphere.


#### 2.3.4. Scanning Electron Microscopy-Energy-Dispersive X-Ray Spectroscopy (SEM-EDAX)

The samples surfaces morphology was investigated by using Field Emission Scanning Electron Microscopy (SEM-Hitachi-s-4800, Japan) coupled with EDX device. The accelerated voltage was 15 kV.


#### 2.3.5. XRF Analysis

The raw kaolinite was analyzed for chemical composition using X-ray Fluorescence (XRF) employing the Semi Quantitative XRF Analysis technique (SIEMENS SRS 3000 X-ray Fluorescence (Rhodium anode, 8 analyzer crystals) with beryllium windows 125μm).


#### 2.3.6. Indexing the Diffraction Patterns and Particle Size Determination

The X-ray diffraction patterns were indexed by using mathematical method by first determining the unit cell parameter from the peak position and then Miller indices. For the nanocomposites, the crystallite sizes were estimated using X-ray diffraction patterns and the Scherrer’s equation whereas the analysis of particle size distribution of the raw kaolinite was done with subsieve analysis technique by applying Andreasen pipette sedimentation method [22, 52].


## 2.1. Materials

Kaolinite was collected at Pugu hills in the Coast region Kisarawe Tanzania by using quartering sampling technique described in [22]. Urea (ACS reagent, 99-100%) was supplied by Sigma Aldrich, DMSO (Extra pure, ≥99.5%) was supplied by Daejung Chemicals & Metals Co. Ltd., Gyonggi-do, Korea, sodium chloride (Extra pure, ≥99.0%) was supplied by Samchun Pure Chemicals Co., Ltd., Gyonggi-do, Korea, silver chloride (ACS reagent, 99.0%) was supplied by Sigma Aldrich, deionized distilled water (D.I.) was supplied by Professor Kim’s Lab, sodium hydroxide (extra pure grade, min 93.0%) was supplied by Duksan Pure Chemical, Ansan City, Kyungkido, South Korea, and aluminium chloride (99.99%) was supplied by Junsei Chemical Co., Ltd., Japan.


## 2.2. Materials Preparation

### 2.2.1. Beneficiation and Treatment of Raw Samples

Wet beneficiation technique was achieved by simple size separation using “classifier.” The method involved the separation of fine platy kaolinite from coarser quartz, feldspar mica, and other impurities using different setting velocities associated with particle size as governed by Stockes’s law [43–50]. The entire procedure which involved crushing to pulverization and soaking as well as running the classifier unit to drying has been comprehensively described in [51]. Pugu kaolinite (10 g) was dispersed in 1000 cm3 of 0.1 M NaCl solution and treated ultrasonically at 50°C for 30 hours and then constantly magnetically stirred for more 30 hours. The product was filtered under vacuum filter and washed several times to remove excessive chlorides; washing was stopped after negative reaction with AgNO3. The washed product was dried in a vacuum oven at 60°C and stockpiled as B1.


### 2.2.2. Preparation of Kaolinite-Intercalation Nanomaterials

AlCl3 solution (0.1 M) was mixed with 0.1 M NaOH solution at a 1 : 2 molar mixing ratio, respectively. The mixture was stirred at 85°C for 6 hours and then aged for 12 hours. A 5% beneficiated kaolinite suspension was prepared and was ultrasonically mixed with an excess of hydroxyaluminum oligomeric solution at 70°C for 3 hours. The product was named B2 which was then washed in a vacuum pump to remove unreacted materials and chloride ions as tested by AgNO3 solution. By using B2 powder as a starting material, a small portion was taken and then mixed with 5 g of urea and stirred for 72 hours at 60°C. The urea-kaolinite nanocomposite obtained was washed in a vacuum pump with excess water and dried at 60°C in a vacuum oven and stored as B3. A small portion of beneficiated and modified Pugu kaolinite was magnetically stirred with DMSO solution in a ratio of 1 : 6 for 21 days at 80°C with a very small addition of water droplets. The suspension was then aged for 7 days and then washed with excess isopropanol and dried at 60°C in a vacuum oven to obtain powder. The DMSO intercalated kaolinite obtained in powder form was calcined at 850°C (10°C/min) for 8 hours with 6-hour holding time and cooling rate of 7°C/min. The calcined sample was named B4. To the calcined powdered sample, 0.38 g was measured in a Sartorius analytical balance and mixed with 0.98 g of urea in excess of hydroxyaluminum oligomeric solution prepared as described above. The mixture was stirred at 105°C to dryness and the powder obtained was named B5.


## 2.2.1. Beneficiation and Treatment of Raw Samples

Wet beneficiation technique was achieved by simple size separation using “classifier.” The method involved the separation of fine platy kaolinite from coarser quartz, feldspar mica, and other impurities using different setting velocities associated with particle size as governed by Stockes’s law [43–50]. The entire procedure which involved crushing to pulverization and soaking as well as running the classifier unit to drying has been comprehensively described in [51]. Pugu kaolinite (10 g) was dispersed in 1000 cm3 of 0.1 M NaCl solution and treated ultrasonically at 50°C for 30 hours and then constantly magnetically stirred for more 30 hours. The product was filtered under vacuum filter and washed several times to remove excessive chlorides; washing was stopped after negative reaction with AgNO3. The washed product was dried in a vacuum oven at 60°C and stockpiled as B1.


## 2.2.2. Preparation of Kaolinite-Intercalation Nanomaterials

AlCl3 solution (0.1 M) was mixed with 0.1 M NaOH solution at a 1 : 2 molar mixing ratio, respectively. The mixture was stirred at 85°C for 6 hours and then aged for 12 hours. A 5% beneficiated kaolinite suspension was prepared and was ultrasonically mixed with an excess of hydroxyaluminum oligomeric solution at 70°C for 3 hours. The product was named B2 which was then washed in a vacuum pump to remove unreacted materials and chloride ions as tested by AgNO3 solution. By using B2 powder as a starting material, a small portion was taken and then mixed with 5 g of urea and stirred for 72 hours at 60°C. The urea-kaolinite nanocomposite obtained was washed in a vacuum pump with excess water and dried at 60°C in a vacuum oven and stored as B3. A small portion of beneficiated and modified Pugu kaolinite was magnetically stirred with DMSO solution in a ratio of 1 : 6 for 21 days at 80°C with a very small addition of water droplets. The suspension was then aged for 7 days and then washed with excess isopropanol and dried at 60°C in a vacuum oven to obtain powder. The DMSO intercalated kaolinite obtained in powder form was calcined at 850°C (10°C/min) for 8 hours with 6-hour holding time and cooling rate of 7°C/min. The calcined sample was named B4. To the calcined powdered sample, 0.38 g was measured in a Sartorius analytical balance and mixed with 0.98 g of urea in excess of hydroxyaluminum oligomeric solution prepared as described above. The mixture was stirred at 105°C to dryness and the powder obtained was named B5.


## 2.3. Characterization

### 2.3.1. Infrared Spectroscopy

By using a Bruker Optic GmbH (alpha model, Laser class 1) Spectrometer with attenuated total reflectance (ATR) the FTIR-ATR measurements were performed in the near infrared region at wavelength between 7500 and 360 cm−1.


### 2.3.2. X-Ray Diffraction

SIEMENS D-5005 X-ray Diffractometer (Cu Kα1 radiation and 2θ scan range which was between 2° and 65°) was used to determine raw kaolinite mineralogy whereas the XRD patterns for the intercalation compounds were executed on RIGAKU COORPERATION, D/MAX-2500/PC X-ray Diffractometer (Cu Kα1) equipped with a back monochromator operating at 40 kV and 100 mA at the scanning range of 5°–80° with a step of 0.1° and a time/step of 1 s.


### 2.3.3. Thermogravimetry (TG/DTG)

Thermograms were taken using TG/STA Linseis STA PT 1000 simultaneous TG/DTG thermal analyzer at a scanning rate of 5°C per min from room temperature to 800°C under nitrogen atmosphere.


### 2.3.4. Scanning Electron Microscopy-Energy-Dispersive X-Ray Spectroscopy (SEM-EDAX)

The samples surfaces morphology was investigated by using Field Emission Scanning Electron Microscopy (SEM-Hitachi-s-4800, Japan) coupled with EDX device. The accelerated voltage was 15 kV.


### 2.3.5. XRF Analysis

The raw kaolinite was analyzed for chemical composition using X-ray Fluorescence (XRF) employing the Semi Quantitative XRF Analysis technique (SIEMENS SRS 3000 X-ray Fluorescence (Rhodium anode, 8 analyzer crystals) with beryllium windows 125μm).


### 2.3.6. Indexing the Diffraction Patterns and Particle Size Determination

The X-ray diffraction patterns were indexed by using mathematical method by first determining the unit cell parameter from the peak position and then Miller indices. For the nanocomposites, the crystallite sizes were estimated using X-ray diffraction patterns and the Scherrer’s equation whereas the analysis of particle size distribution of the raw kaolinite was done with subsieve analysis technique by applying Andreasen pipette sedimentation method [22, 52].


## 2.3.1. Infrared Spectroscopy

By using a Bruker Optic GmbH (alpha model, Laser class 1) Spectrometer with attenuated total reflectance (ATR) the FTIR-ATR measurements were performed in the near infrared region at wavelength between 7500 and 360 cm−1.


## 2.3.2. X-Ray Diffraction

SIEMENS D-5005 X-ray Diffractometer (Cu Kα1 radiation and 2θ scan range which was between 2° and 65°) was used to determine raw kaolinite mineralogy whereas the XRD patterns for the intercalation compounds were executed on RIGAKU COORPERATION, D/MAX-2500/PC X-ray Diffractometer (Cu Kα1) equipped with a back monochromator operating at 40 kV and 100 mA at the scanning range of 5°–80° with a step of 0.1° and a time/step of 1 s.


## 2.3.3. Thermogravimetry (TG/DTG)

Thermograms were taken using TG/STA Linseis STA PT 1000 simultaneous TG/DTG thermal analyzer at a scanning rate of 5°C per min from room temperature to 800°C under nitrogen atmosphere.


## 2.3.4. Scanning Electron Microscopy-Energy-Dispersive X-Ray Spectroscopy (SEM-EDAX)

The samples surfaces morphology was investigated by using Field Emission Scanning Electron Microscopy (SEM-Hitachi-s-4800, Japan) coupled with EDX device. The accelerated voltage was 15 kV.


## 2.3.5. XRF Analysis

The raw kaolinite was analyzed for chemical composition using X-ray Fluorescence (XRF) employing the Semi Quantitative XRF Analysis technique (SIEMENS SRS 3000 X-ray Fluorescence (Rhodium anode, 8 analyzer crystals) with beryllium windows 125μm).


## 2.3.6. Indexing the Diffraction Patterns and Particle Size Determination

The X-ray diffraction patterns were indexed by using mathematical method by first determining the unit cell parameter from the peak position and then Miller indices. For the nanocomposites, the crystallite sizes were estimated using X-ray diffraction patterns and the Scherrer’s equation whereas the analysis of particle size distribution of the raw kaolinite was done with subsieve analysis technique by applying Andreasen pipette sedimentation method [22, 52].


## 3. Results and Discussion

### 3.1. Raw Kaolinite Analysis

Oriented as well as randomly oriented whole rock X-ray diffraction as a function of air-drying, glycolation, and heating at 550°C revealed the presence of quartz (SiO2), clinochlore [Mg5AlSi,Al4O10OH8], and microcline [KAlSi3O8] as nonkaolinite portions in the raw kaolinite after beneficiation quartz and microcline disappeared. After beneficiation, kaolinite [Al2Si2O5(OH)4] was observed to be a dominant phase along with illite [KAl2(Si3AlO10)(OH)2] as minor phase. The chemical composition of raw and beneficiated kaolinite used revealed a reduction of silica content from 63.64 to 54.99% and an increase in alumina content from 31.43 to 40.2% (Table 1).Table 1
Chemical composition of the raw materials.
Sample
Oxide composition
SiO2
Al2O3
Na2O
MgO
SO3
Cl
K2O
CaO
TiO2
Cr2O3
MnO
Fe2O3
LOI
Pugu kaolinite
63.64
31.43
0.43
0.16
0.25
0.76
1.39
0.06
0.80
0.03
0.01
1.01
0.03
Beneficiated kaolinite
54.99
40.20
0.09
0.13
0.08
0.04
0.96
0.04
1.02
0.04
0.01
2.00
0.40


### 3.2. X-Ray Indexing and Particle Size Analysis

Miller indices sequence (Table2) obtained using the X-ray diffraction pattern (Figure 1) indicated that the kaolinite used had an FCC crystal Bravais lattice structure with the average lattice parameter of 12.597 Å. The X-ray diffraction (Figure 1) revealed that the intercalation of oligomeric cations into the kaolinite interlayer spaces (B2) proceeded at an apparent intercalation ratio of 51.2% (Table 3) corresponding to the expansion of basal lattice space of about 0.098 Å. For the B3 nanocomposite the intercalation compound was formed at an intercalation ratio of 32.4% related to the basal expansion of lattice parameter of about 0.186 Å. The intermediate DMSO intercalated kaolinite was found to have an intercalation ratio of 89.2% prior to calcination; this intercalation ratio dropped to 7.0% after calcination (for the calcined B4 in Figure 1) and this was attributed to the disintegration of an intercalant DMSO present in the kaolinite interlayer spaces to form corresponding DMSO decomposition material. This drastic drop from 89.2% to 7.0% of intercalation ratio is associated with the contraction (instead of the usual expansion of interlayer distances) of about 3.778 Å. Following reintercalation of B4 with hydroxyaluminum oligomeric cations the intercalation ratio was raised to 38.4% (for B5) from 7.0% of B4; this corresponds to the expansion of 0.634 Å in the basal lattice spaces from the compact calcined B4. The particle size of each sample is given in Table 2; the order of particle sizes was observed to be in the following trend: B3 ≈ B5 > B2 > B4. Calcination caused a drastic size reduction as seen in Table 2.Table 2
Indexed X-ray diffraction patterns.
Peak
2
θ
sin
2
⁡
θ
3
sin
2
⁡
θ
/
sin
2
⁡
θ
min
⁡
h
2
+
k
2
+
l
2
h
k
l
a (Å)
d (nm)
1
12.402
0.011668
3.158
3
111
12.352
0.713
2
24.911
0.046518
12.592
13
320
12.877
0.357
3
12.233
0.011353
3.073
3
111
12.522
0.723
4
24.746
0.045914
12.428
12
222
12.453
0.360
5
12.086
0.011083
3.000
3
111
12.673
0.732
6
24.592
0.045353
12.276
12
222
12.529
0.362
7
26.562
0.052775
14.285
14
321
12.546
0.335
8
19.581
0.028916
7.820
8
220
12.813
0.453
9
22.279
0.037326
10.104
10
310
12.608
0.399Table 3
Scherrer’s particle size and intercalation ratio.
Material
A.I.R. (%)
Averagel (nm)
B2
51.2
33.51–31.73
B3
32.4
41.92–39.69
B4
7.0
22.31–21.13
B5
38.4
41.86–39.63
A.I.R.: apparent intercalation ratio.
l: particle size.Figure 1
X-ray diffractograms for B1, B2, B3, B4, and B5.


### 3.3. FT-IR Analysis

The discussion regarding the IR absorption bands on the intercalated kaolinite minerals is mainly limited to the OH and Si-O near infrared absorptions (Figure2). The presence of characteristic stretching vibrations indicated that the intercalation interactions between the kaolinite interlayer spaces with the intercalating species as well as with urea fertilizer took place. These vibrations have been summarized in Table 4.Table 4
Band assignments for the ATR-FTIR absorption bands.
Wavenumber (cm−1)
Band assignment
Reference
3683, 3684, and 3693
OH stretch for the Si-O-Si  bonds on the  lower octahedral  surfaces of kaolinite
[23, 24]
3618–3620
Inner hydroxyl groups between  tetrahedral and octahedral kaolinite sheets
[24–26]
3650
In-phase symmetrical stretch due to kaolinite sheets
[25, 26]
3426
N-H out-phase stretch due to urea
[27, 28]
3340
In-phase N-H stretch due to urea
[28, 29]
3256
OH stretching for H bonding associated with urea-oligomer substitution within kaolinite interlayer spaces
[30, 31]
2970
CH stretch/dimeric OH stretch associated with DMSO decomposition during calcination to form paraformaldehyde complexes
[32, 33]
1738
C=O stretch due to intercalated urea
[32, 33]
1669
Free C=O stretch and free NH2  bending
[34, 35]
1587
C-N stretch due to urea
[34, 35]
1461
In-phase CH3 bending + scissoring C-N vibrations
[34, 35]
1438
S=O sulfate ester stretching
[32, 33]
1365
S=O sulfonyl stretching
[32, 33]
1202–1216
Amorphous SiO2 associated with calcination
[36, 37]
1113–1149
Apical Si-O stretching
[23, 24, 26, 38]
1047
Si-O & Si-O-Al stretching due to the presence of DMSO in the kaolinite
[37]
1023–1027
In-phase Si-O planar stretching
[23, 24, 26, 39]
1001–997
Out-phase Si-O planar stretching and alternating Si-O & Al-O bonds
[23, 24, 26, 39, 40]
910–900
OH deformation of inner hydroxyl group due to Al(VI⁡)-OH bending vibrations
[23, 24, 39, 41]
788–749
Al-O-Si asymmetric bending
[23, 24, 26, 39, 41]
777 and 434
OH stretch associated with a change from octahedral Al3+ in kaolinite to tetrahedral coordination in metakaolinite
[23, 24, 26, 39, 41]
525
Si-O-Al(VI⁡) bending vibration for the Al3+ in the octahedral configuration
[42]Figure 2
ATR-FTIR diffractograms for B2, B3, and B4.Essentially, the intercalating species (DMSO) is known to be highly stable at temperatures below 150°C above which gradual decomposition starts to form relatively volatile materials in the form of paraformaldehyde including among others dimethyl sulfide, dimethyl disulfide, bis(methylthio)methane, water vapor, and traces of methyl mercaptan and dimethyl sulfoneR1–R4 attributable to the reactions which took place during calcination process to form B4 which corresponds to the absorption bands observed at 1365, 1438, 1738, and 2970 cm−1, for S=O sulfonyl stretching, S=O sulfate ester stretching, C=O stretch, and either CH stretch or dimeric OH carboxylic acid stretch, respectively, as seen in the reactions R1 to R4 [32, 33]: R1H3CSOCH3⟶H3CSH+HCHO⟹HCHOxR22H3CSH+HCHO⟶H3CS2CH2+H2OR32H3CSH+CH3SOCH3⟶H3CSSCH3+H3CSCH3+H2OR42H3CSOCH3⟶H3CSO2CH3+H2CSCH3


### 3.4. SEM-EDAX Analysis

The SEM micrographs were taken to determine the morphology of the nanomaterials prepared. The existence of overlapping euhedral pseudo hexagonal platelets exhibiting dense-tight-thick layers was observed in the beneficiated kaolinite (Figures3 and 4), a feature which is typical to most kaolinite minerals [53]. Following chemical treatment with salt solution this stacking sequence was observed to change to vermiform shaped particles mixed with skinny stacked euhedral pseudo hexagonal platelets (Figure 5). Salt treatment was therefore seen to possess the capacity to expose and activate the kaolinite functional layers thereby increasing the active surface area necessary for intercalation process.Figure 3
SEM micrograph of beneficiated kaolinite.Figure 4
SEM micrograph of beneficiated kaolinite.Figure 5
SEM micrograph of B1.The stacking sequence of the intermediate kaolinite-hydroxyaluminum intercalation compound (B2) when compared with the beneficiated kaolinite and the treated kaolinite (B1) revealed substantial changes in the morphology of kaolinite layers (Figures 3–5 and Figures 6(a) and 6(b)). As seen in B2 (Figures 6(a) and 6(b)), the kaolinite morphology was still vermicular, but the distance between layers has broadened as compared to beneficiated kaolinite and B1 which in turn explicates the expansion of interlayer distance following the intercalation of oligomeric cation.Figure 6
SEM micrograph of B2.
(a)
(b)Eventually, a complete disappearance of stacked layer sequences when urea replaced hydroxyaluminum oligomers in the kaolinite interlayer spaces was observed (Figures7(a) and 7(b)). This observation was attributed to the formation of a well-packed urea-kaolinite intercalation compound.Figure 7
SEM micrograph of B3.
(a)
(b)Furthermore, during the first attempt of coupling: DMSO-kaolinite intercalation→ calcination → hydroxyaluminum-kaolinite reintercalation and then urea substitution in the hydroxyaluminum reintercalated kaolinite, there was a transitional transformation from the vermicular morphology observed before into nanostructures resembling like a “pimpled surfaces” or rather like a “pustulated skin” wherein the particles were self-assembled into a woven network pattern (Figures 8(a) and 8(b)). A complete transformation was observed after aging and maturation of B5 (observed in Figure 8) to B5 (observed in Figure 9) which exhibited a unique curling behavior resembling like a perforated glomeruli embedded on each other to form a pattern like desert cactus. These phenomena were associated with the tendency of hydroxyaluminum oligomer to curl during air drying thereby creating an alternating aluminum chlorohydrate water arrangement and then diffusion of water between the aluminum chlorohydrate layers during air drying resulting in a curled film [54].Figure 8
SEM micrograph of transitional B5.
(a)
(b)Figure 9
SEM micrograph of B5.
(a)
(b)The self-assembled nanostructures observed in B5 were analyzed for elemental composition with EDX (Figure 10) and results indicated the presence of nitrogen from urea so revealing the fact the nanocomposites (B5) can be used in the formulation of controlled release systems such as (urea) controlled release fertilizers and the drug delivery systems.Figure 10
Composition of B5 from EDAX.


### 3.5. TG-DTG Analysis

Thermogravimetric analysis was done under N2 atmosphere to investigate the thermal degradation and stability of aluminum oligomer intercalated kaolinite compounds to a maximum of about 800°C.As can be seen in Figure11, B2 was characterized by 4 degradation phases which include 25–250°C, 250–450°C, 500–650°C, and 670–800°C, respectively, corresponding to the removal of moisture that is externally adsorbed on the surfaces as well the decomposition of Kegging ions or Kegging cluster (resulting from polymerization of hydroxyaluminum oligomers into large discrete anions in the form of [H2W12O40]6− which undergo condensation in the interlayer spaces thereby forming higher polymers such as the Al24-polycations) associated with the calcination of B2 [55–57]; also, it corresponds to the removal of water molecules bonded to the aluminum atoms on the Keggin cluster [58]. This observation agrees with the fact that “water molecules bonded to the aluminum atoms on the Keggin cluster are more likely to be removed around 150–300°C” [58, 59]. The decomposition along 250–450°C and 500–650°C corresponds to the liberation of interlayer water, kaolinite hydroxylation reactions, and CO2 associated with the decomposition of B2 [58] whereas the phase around 670–800°C corresponds to both kaolinite dehydroxylation and the kaolinite dehydroxylation transformation phases [60–62].Figure 11
TGA thermograms for Urea, B1, B2, B3, and B4.When urea replaced hydroxyaluminum oligomer, the externally adsorbed water and the elimination of structural water were observed in the first and second degradation phases that is 25–70 and 75–230°C, respectively. The second and third degradation phases around 75–230°C and 250–320°C correspond to both urea vaporization and its complementary degradation compound biuret [NH(CO)2(NH2)2], respectively. Preliminary kaolinite dehydroxylation as well as continuous sublimation of urea to its complex decomposition product corresponds to fourth and fifth degradation phases seen at 350–550°C and 550–800°C [63], respectively.


## 3.1. Raw Kaolinite Analysis

Oriented as well as randomly oriented whole rock X-ray diffraction as a function of air-drying, glycolation, and heating at 550°C revealed the presence of quartz (SiO2), clinochlore [Mg5AlSi,Al4O10OH8], and microcline [KAlSi3O8] as nonkaolinite portions in the raw kaolinite after beneficiation quartz and microcline disappeared. After beneficiation, kaolinite [Al2Si2O5(OH)4] was observed to be a dominant phase along with illite [KAl2(Si3AlO10)(OH)2] as minor phase. The chemical composition of raw and beneficiated kaolinite used revealed a reduction of silica content from 63.64 to 54.99% and an increase in alumina content from 31.43 to 40.2% (Table 1).Table 1
Chemical composition of the raw materials.
Sample
Oxide composition
SiO2
Al2O3
Na2O
MgO
SO3
Cl
K2O
CaO
TiO2
Cr2O3
MnO
Fe2O3
LOI
Pugu kaolinite
63.64
31.43
0.43
0.16
0.25
0.76
1.39
0.06
0.80
0.03
0.01
1.01
0.03
Beneficiated kaolinite
54.99
40.20
0.09
0.13
0.08
0.04
0.96
0.04
1.02
0.04
0.01
2.00
0.40


## 3.2. X-Ray Indexing and Particle Size Analysis

Miller indices sequence (Table2) obtained using the X-ray diffraction pattern (Figure 1) indicated that the kaolinite used had an FCC crystal Bravais lattice structure with the average lattice parameter of 12.597 Å. The X-ray diffraction (Figure 1) revealed that the intercalation of oligomeric cations into the kaolinite interlayer spaces (B2) proceeded at an apparent intercalation ratio of 51.2% (Table 3) corresponding to the expansion of basal lattice space of about 0.098 Å. For the B3 nanocomposite the intercalation compound was formed at an intercalation ratio of 32.4% related to the basal expansion of lattice parameter of about 0.186 Å. The intermediate DMSO intercalated kaolinite was found to have an intercalation ratio of 89.2% prior to calcination; this intercalation ratio dropped to 7.0% after calcination (for the calcined B4 in Figure 1) and this was attributed to the disintegration of an intercalant DMSO present in the kaolinite interlayer spaces to form corresponding DMSO decomposition material. This drastic drop from 89.2% to 7.0% of intercalation ratio is associated with the contraction (instead of the usual expansion of interlayer distances) of about 3.778 Å. Following reintercalation of B4 with hydroxyaluminum oligomeric cations the intercalation ratio was raised to 38.4% (for B5) from 7.0% of B4; this corresponds to the expansion of 0.634 Å in the basal lattice spaces from the compact calcined B4. The particle size of each sample is given in Table 2; the order of particle sizes was observed to be in the following trend: B3 ≈ B5 > B2 > B4. Calcination caused a drastic size reduction as seen in Table 2.Table 2
Indexed X-ray diffraction patterns.
Peak
2
θ
sin
2
⁡
θ
3
sin
2
⁡
θ
/
sin
2
⁡
θ
min
⁡
h
2
+
k
2
+
l
2
h
k
l
a (Å)
d (nm)
1
12.402
0.011668
3.158
3
111
12.352
0.713
2
24.911
0.046518
12.592
13
320
12.877
0.357
3
12.233
0.011353
3.073
3
111
12.522
0.723
4
24.746
0.045914
12.428
12
222
12.453
0.360
5
12.086
0.011083
3.000
3
111
12.673
0.732
6
24.592
0.045353
12.276
12
222
12.529
0.362
7
26.562
0.052775
14.285
14
321
12.546
0.335
8
19.581
0.028916
7.820
8
220
12.813
0.453
9
22.279
0.037326
10.104
10
310
12.608
0.399Table 3
Scherrer’s particle size and intercalation ratio.
Material
A.I.R. (%)
Averagel (nm)
B2
51.2
33.51–31.73
B3
32.4
41.92–39.69
B4
7.0
22.31–21.13
B5
38.4
41.86–39.63
A.I.R.: apparent intercalation ratio.
l: particle size.Figure 1
X-ray diffractograms for B1, B2, B3, B4, and B5.


## 3.3. FT-IR Analysis

The discussion regarding the IR absorption bands on the intercalated kaolinite minerals is mainly limited to the OH and Si-O near infrared absorptions (Figure2). The presence of characteristic stretching vibrations indicated that the intercalation interactions between the kaolinite interlayer spaces with the intercalating species as well as with urea fertilizer took place. These vibrations have been summarized in Table 4.Table 4
Band assignments for the ATR-FTIR absorption bands.
Wavenumber (cm−1)
Band assignment
Reference
3683, 3684, and 3693
OH stretch for the Si-O-Si  bonds on the  lower octahedral  surfaces of kaolinite
[23, 24]
3618–3620
Inner hydroxyl groups between  tetrahedral and octahedral kaolinite sheets
[24–26]
3650
In-phase symmetrical stretch due to kaolinite sheets
[25, 26]
3426
N-H out-phase stretch due to urea
[27, 28]
3340
In-phase N-H stretch due to urea
[28, 29]
3256
OH stretching for H bonding associated with urea-oligomer substitution within kaolinite interlayer spaces
[30, 31]
2970
CH stretch/dimeric OH stretch associated with DMSO decomposition during calcination to form paraformaldehyde complexes
[32, 33]
1738
C=O stretch due to intercalated urea
[32, 33]
1669
Free C=O stretch and free NH2  bending
[34, 35]
1587
C-N stretch due to urea
[34, 35]
1461
In-phase CH3 bending + scissoring C-N vibrations
[34, 35]
1438
S=O sulfate ester stretching
[32, 33]
1365
S=O sulfonyl stretching
[32, 33]
1202–1216
Amorphous SiO2 associated with calcination
[36, 37]
1113–1149
Apical Si-O stretching
[23, 24, 26, 38]
1047
Si-O & Si-O-Al stretching due to the presence of DMSO in the kaolinite
[37]
1023–1027
In-phase Si-O planar stretching
[23, 24, 26, 39]
1001–997
Out-phase Si-O planar stretching and alternating Si-O & Al-O bonds
[23, 24, 26, 39, 40]
910–900
OH deformation of inner hydroxyl group due to Al(VI⁡)-OH bending vibrations
[23, 24, 39, 41]
788–749
Al-O-Si asymmetric bending
[23, 24, 26, 39, 41]
777 and 434
OH stretch associated with a change from octahedral Al3+ in kaolinite to tetrahedral coordination in metakaolinite
[23, 24, 26, 39, 41]
525
Si-O-Al(VI⁡) bending vibration for the Al3+ in the octahedral configuration
[42]Figure 2
ATR-FTIR diffractograms for B2, B3, and B4.Essentially, the intercalating species (DMSO) is known to be highly stable at temperatures below 150°C above which gradual decomposition starts to form relatively volatile materials in the form of paraformaldehyde including among others dimethyl sulfide, dimethyl disulfide, bis(methylthio)methane, water vapor, and traces of methyl mercaptan and dimethyl sulfoneR1–R4 attributable to the reactions which took place during calcination process to form B4 which corresponds to the absorption bands observed at 1365, 1438, 1738, and 2970 cm−1, for S=O sulfonyl stretching, S=O sulfate ester stretching, C=O stretch, and either CH stretch or dimeric OH carboxylic acid stretch, respectively, as seen in the reactions R1 to R4 [32, 33]: R1H3CSOCH3⟶H3CSH+HCHO⟹HCHOxR22H3CSH+HCHO⟶H3CS2CH2+H2OR32H3CSH+CH3SOCH3⟶H3CSSCH3+H3CSCH3+H2OR42H3CSOCH3⟶H3CSO2CH3+H2CSCH3


## 3.4. SEM-EDAX Analysis

The SEM micrographs were taken to determine the morphology of the nanomaterials prepared. The existence of overlapping euhedral pseudo hexagonal platelets exhibiting dense-tight-thick layers was observed in the beneficiated kaolinite (Figures3 and 4), a feature which is typical to most kaolinite minerals [53]. Following chemical treatment with salt solution this stacking sequence was observed to change to vermiform shaped particles mixed with skinny stacked euhedral pseudo hexagonal platelets (Figure 5). Salt treatment was therefore seen to possess the capacity to expose and activate the kaolinite functional layers thereby increasing the active surface area necessary for intercalation process.Figure 3
SEM micrograph of beneficiated kaolinite.Figure 4
SEM micrograph of beneficiated kaolinite.Figure 5
SEM micrograph of B1.The stacking sequence of the intermediate kaolinite-hydroxyaluminum intercalation compound (B2) when compared with the beneficiated kaolinite and the treated kaolinite (B1) revealed substantial changes in the morphology of kaolinite layers (Figures 3–5 and Figures 6(a) and 6(b)). As seen in B2 (Figures 6(a) and 6(b)), the kaolinite morphology was still vermicular, but the distance between layers has broadened as compared to beneficiated kaolinite and B1 which in turn explicates the expansion of interlayer distance following the intercalation of oligomeric cation.Figure 6
SEM micrograph of B2.
(a)
(b)Eventually, a complete disappearance of stacked layer sequences when urea replaced hydroxyaluminum oligomers in the kaolinite interlayer spaces was observed (Figures7(a) and 7(b)). This observation was attributed to the formation of a well-packed urea-kaolinite intercalation compound.Figure 7
SEM micrograph of B3.
(a)
(b)Furthermore, during the first attempt of coupling: DMSO-kaolinite intercalation→ calcination → hydroxyaluminum-kaolinite reintercalation and then urea substitution in the hydroxyaluminum reintercalated kaolinite, there was a transitional transformation from the vermicular morphology observed before into nanostructures resembling like a “pimpled surfaces” or rather like a “pustulated skin” wherein the particles were self-assembled into a woven network pattern (Figures 8(a) and 8(b)). A complete transformation was observed after aging and maturation of B5 (observed in Figure 8) to B5 (observed in Figure 9) which exhibited a unique curling behavior resembling like a perforated glomeruli embedded on each other to form a pattern like desert cactus. These phenomena were associated with the tendency of hydroxyaluminum oligomer to curl during air drying thereby creating an alternating aluminum chlorohydrate water arrangement and then diffusion of water between the aluminum chlorohydrate layers during air drying resulting in a curled film [54].Figure 8
SEM micrograph of transitional B5.
(a)
(b)Figure 9
SEM micrograph of B5.
(a)
(b)The self-assembled nanostructures observed in B5 were analyzed for elemental composition with EDX (Figure 10) and results indicated the presence of nitrogen from urea so revealing the fact the nanocomposites (B5) can be used in the formulation of controlled release systems such as (urea) controlled release fertilizers and the drug delivery systems.Figure 10
Composition of B5 from EDAX.


## 3.5. TG-DTG Analysis

Thermogravimetric analysis was done under N2 atmosphere to investigate the thermal degradation and stability of aluminum oligomer intercalated kaolinite compounds to a maximum of about 800°C.As can be seen in Figure11, B2 was characterized by 4 degradation phases which include 25–250°C, 250–450°C, 500–650°C, and 670–800°C, respectively, corresponding to the removal of moisture that is externally adsorbed on the surfaces as well the decomposition of Kegging ions or Kegging cluster (resulting from polymerization of hydroxyaluminum oligomers into large discrete anions in the form of [H2W12O40]6− which undergo condensation in the interlayer spaces thereby forming higher polymers such as the Al24-polycations) associated with the calcination of B2 [55–57]; also, it corresponds to the removal of water molecules bonded to the aluminum atoms on the Keggin cluster [58]. This observation agrees with the fact that “water molecules bonded to the aluminum atoms on the Keggin cluster are more likely to be removed around 150–300°C” [58, 59]. The decomposition along 250–450°C and 500–650°C corresponds to the liberation of interlayer water, kaolinite hydroxylation reactions, and CO2 associated with the decomposition of B2 [58] whereas the phase around 670–800°C corresponds to both kaolinite dehydroxylation and the kaolinite dehydroxylation transformation phases [60–62].Figure 11
TGA thermograms for Urea, B1, B2, B3, and B4.When urea replaced hydroxyaluminum oligomer, the externally adsorbed water and the elimination of structural water were observed in the first and second degradation phases that is 25–70 and 75–230°C, respectively. The second and third degradation phases around 75–230°C and 250–320°C correspond to both urea vaporization and its complementary degradation compound biuret [NH(CO)2(NH2)2], respectively. Preliminary kaolinite dehydroxylation as well as continuous sublimation of urea to its complex decomposition product corresponds to fourth and fifth degradation phases seen at 350–550°C and 550–800°C [63], respectively.


## 4. Conclusion

The effect of coupling DMSO and oligomeric hydroxyaluminum intercalating species via calcination as an intermediate step on the properties of kaolinite morphology was investigated. The raw kaolinite was wet beneficiated and then modified with sodium chloride solution. Matured and aged hydroxyaluminum cationic oligomers were prepared and used as intermediate intercalation compounds for the intercalation of urea into the kaolinite interlayer spaces. The effect of reintercalating urea into the calcined DMSO intercalated kaolinite via hydroxyaluminum oligomeric cations as intermediate step was also investigated; the resulting nanomaterials were characterized with XRF, ATR-FTIR, XRD DT/DTG, SEM, and EDX. The percentage intercalation ratios attained were 89.2, 51.2, 32.4, 7.0, and 38.4 for the DMSO intercalated kaolinite, hydroxyaluminum intercalated kaolinite, urea intercalated kaolinite, calcined DMSO intercalated kaolinite, and the urea-kaolinite reintercalated nanocomposites; their particle sizes were in average 60.01 nm, 32.62 nm, 40.81 nm, 21.72 nm, and 40.75 nm, respectively. Despite the variations in the kaolinite treatments, the average lattice parameter was in average 12.59 Å and the Bravais crystal lattice was FCC structure. Unique curling patterns were observed when kaolinite was treated with the intermediate intercalating species and calcined and then reintercalated with urea. These include a change from the normal stacked frequency of euhedral pseudo hexagonal platelets of the kaolinite to vermiform morphologies and then to pustulated form and finally into a unique curled pattern which exhibited what we have called a curled glomeruli-like shape organized into self-assembled structure resembling a desert cactus.



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*Source: 920835-2015-09-13.xml*