# Optical and Thermal Properties of Zn/Al-Layered Double Hydroxide Nanocomposite Intercalated with Sodium Dodecyl Sulfate

Authors: Samaneh Babakhani; Zainal Abidin Talib; Mohd Zobir Hussein; Abdullah Ahmed Ali Ahmed
Journal: Journal of Spectroscopy
 (2014)

---

## Abstract

Zn/Al-LDH-SDS nanocomposites have been prepared using a coprecipitation method in different molar ratio of Zn2+/Al3+ = 2, 3, and 4 at pH = 10 and different concentrations of sodium dodecyl sulfate solution (0.2 M, 0.4 M, and 0.8 M). The XRD and FTIR data show the successful intercalation of SDS into the LDH interlayer. The XRD diffractogram showed that the basal spacing for Zn
/
Al–
NO
3
- is 0.89 nm compared to 2.54–2.61 nm for the Zn/Al-SDS nanocomposite. Optical band gap of the samples was calculated using Kubelka-Munk model. Due to the presence of LDH phase, two band gap energies (E
g
1 and E
g
2) were observed. The values of E
g
1 and E
g
2 were found around 4.8 eV and 3.75 eV for Zn/Al-LDH (r = 2, 3, and 4). The values of band gap of LDH-SDS nanocomposites were found to increase to around 4.2 eV and 5.2 eV. For Zn4Al-LDH-SDS with 0.4 M and 0.8 M of SDS, only one energy gap at around 3.23 eV was observed. The optical band gap of SO
4
2
- phase increased as the amount of SDS increases. Thermal diffusivity of the resulted nanocomposite was also investigated.


---

## Body

## 1. Introduction

One ideal host for the organic-inorganic nanohybrid materials or nanocomposites can be a two-dimensional layered structure that includes thin crystalline inorganic layers that have a molecular scale thickness of a nanometer range. Layered double hydroxide (LDH) can be named as an example for this structure. Planting various anionic species as guests inside interlayer spaces of the LDH leads to having a growth in the interlayer distance toward a nanometer size dimension that shapes a new nanohybrid material [1]. LDHs are currently under spotlight because of their capabilities in industrial and medical applications. They have a key role in the fields of separation process, catalysis, DNA or biomolecule carriers, and drug delivery (controlled drug release). In addition to their role as working nanostructures, they also put on show a large number of electronic and magnetic properties.Since organic-inorganic hybrid materials have improved and better properties rather than their counterparts, development of these types of materials provides excellence aspects of applications in different areas of technology and science. This also is because their property can be tailor-made to special application such as photochromic coating, photochemical reaction, and selective optical transmission, to name a few. For the formation of a nanolayered composite of organic-inorganic hybrid type or the so-called nanocomposite materials, LDHs or hydrotalcite-like material can be one of the popular inorganic hosts for the formation of an organic-inorganic hybrid type. Several studies have focused on intercalation of various dye molecules, especially organic dyes, into the layered inorganic lamella, in particular anionic clays for different applications and purposes [2].Considering the above findings, an idea to study the properties of novel nanocomposites with intercalated anion has been generated. Sodium dodecyl sulfate has been specially chosen to study the physical properties of the obtained nanocomposite. We report here the synthesis of Zn/Al-LDHs by coprecipitation method, intercalation of Sodium dodecyl sulfate into the interlayer of the LDHs, a comparative study of the UV absorption ability of the LDH-SDS nanocomposites, thermal diffusivity of the resulted nanocomposites, and the effect of intercalation on the morphology.


## 2. Experimental

### 2.1. Materials

The metal nitrates of aluminum nitrate Al(NO3)3·9H2O (Hamburg Chemicals Co., 99.4%), zinc nitrate Zn(NO3)2·6H2O (System, 98%), and NaOH (Merck Co., 99%) were used without further purification. Sodium dodecyl sulfate (SDS) (Merck Co., 98%) was used as the organic compound for the intercalation process. The solvent used throughout this study was deionized water.


### 2.2.  Synthesis of Zn/Al-NO3 Hydrotalcite and Zn/Al-Sodium Dodecyl Sulfate Nanocomposite

Zn
/
Al–
NO
3
- LDH precursor was synthesized using coprecipitation method with a molar ratio of Zn2+/Al3+, r
=
2, 3, and 4. The slow mixing of metal nitrates solution of Al(NO3)3·9H2O and Zn(NO3)2·6H2O was carried out under constant stirring. The titration process was done by dropwise addition of aqueous NaOH (1.0 M) until pH
=
10. In order to avoid the contamination of CO2 from the atmosphere or at least to minimize it, the titration of NaOH was carried out under a constant flow of N2 gas. For the next step, the resulting slurry was placed in an oil bath shaker (70 rpm) for 18 h and aged at 70°C. The precipitate was centrifuged and washed with deionized water many times and dried in an oven at 70°C for 2 days. After grinding the resulting nanocomposite into a fine powder, it was stored in sample bottles and labeled as ZnrAl-LDH for further use (r represents the molar ratio). To produce LDH with SDS, before the titration with NaOH, the desired amount of sodium dodecyl sulfate was added into a solution containing Zn (NO3)2·6H2O and Al (NO3)3·9H2O. A 50 mL of solution containing 0.2 M, 0.4 M, and 0.8 M of SDS was added to a 100 mL of Zn/Al solution. The dropwise addition of NaOH was continued until the pH of the solution reached pH 10. The samples were ground into a fine powder, stored in sample bottles, and labeled as ZnrAl-LDH-SDS for further use.


### 2.3. Characterization

Powder X-ray diffraction (PXRD) patterns of the samples were recorded on a diffractometer (X’PERT-PROPANALYTICAL) using CuKα (1.54187Å) at 40 kV and 30 mA. The FTIR spectra were obtained using a Thermo Nicolet NEXUS FTIR spectrophotometer (model: SMART ORBIT) in the range of 400–4000 cm−1. The powdered samples were ground with KBr in 1 : 20 ratio and pressed into pellets for recording the spectra. The band gap was calculated using the optical measurements that were performed on a UV-VIS-NIR diffuse reflectance spectrophotometer (Shimadzu, UV-3600). Thermal diffusivity measurements were performed using NETZSCH, model LFA 457 MicroFlash. The surface morphologies of the samples were observed by a field emission scanning electron microscope (FESEM), model NOVA NANOSEM 230.


## 2.1. Materials

The metal nitrates of aluminum nitrate Al(NO3)3·9H2O (Hamburg Chemicals Co., 99.4%), zinc nitrate Zn(NO3)2·6H2O (System, 98%), and NaOH (Merck Co., 99%) were used without further purification. Sodium dodecyl sulfate (SDS) (Merck Co., 98%) was used as the organic compound for the intercalation process. The solvent used throughout this study was deionized water.


## 2.2.  Synthesis of Zn/Al-NO3 Hydrotalcite and Zn/Al-Sodium Dodecyl Sulfate Nanocomposite

Zn
/
Al–
NO
3
- LDH precursor was synthesized using coprecipitation method with a molar ratio of Zn2+/Al3+, r
=
2, 3, and 4. The slow mixing of metal nitrates solution of Al(NO3)3·9H2O and Zn(NO3)2·6H2O was carried out under constant stirring. The titration process was done by dropwise addition of aqueous NaOH (1.0 M) until pH
=
10. In order to avoid the contamination of CO2 from the atmosphere or at least to minimize it, the titration of NaOH was carried out under a constant flow of N2 gas. For the next step, the resulting slurry was placed in an oil bath shaker (70 rpm) for 18 h and aged at 70°C. The precipitate was centrifuged and washed with deionized water many times and dried in an oven at 70°C for 2 days. After grinding the resulting nanocomposite into a fine powder, it was stored in sample bottles and labeled as ZnrAl-LDH for further use (r represents the molar ratio). To produce LDH with SDS, before the titration with NaOH, the desired amount of sodium dodecyl sulfate was added into a solution containing Zn (NO3)2·6H2O and Al (NO3)3·9H2O. A 50 mL of solution containing 0.2 M, 0.4 M, and 0.8 M of SDS was added to a 100 mL of Zn/Al solution. The dropwise addition of NaOH was continued until the pH of the solution reached pH 10. The samples were ground into a fine powder, stored in sample bottles, and labeled as ZnrAl-LDH-SDS for further use.


## 2.3. Characterization

Powder X-ray diffraction (PXRD) patterns of the samples were recorded on a diffractometer (X’PERT-PROPANALYTICAL) using CuKα (1.54187Å) at 40 kV and 30 mA. The FTIR spectra were obtained using a Thermo Nicolet NEXUS FTIR spectrophotometer (model: SMART ORBIT) in the range of 400–4000 cm−1. The powdered samples were ground with KBr in 1 : 20 ratio and pressed into pellets for recording the spectra. The band gap was calculated using the optical measurements that were performed on a UV-VIS-NIR diffuse reflectance spectrophotometer (Shimadzu, UV-3600). Thermal diffusivity measurements were performed using NETZSCH, model LFA 457 MicroFlash. The surface morphologies of the samples were observed by a field emission scanning electron microscope (FESEM), model NOVA NANOSEM 230.


## 3. Results and Discussion

### 3.1.  Powder X-Ray Diffraction (XRD) Study

SDS (sodium dodecyl sulfate) intercalated Zn/Al-LDH nanocomposites were prepared using precipitation method. Figure2 shows that the powder XRD patterns of the Zn/Al–NO3 and SDS intercalated LDHs synthesized in different concentration of SDS. The sharpness of the peaks suggests ordered and regular stacking of the LDH layers. XRD of the ZnrAl–NO3–LDH samples (Figure 1(d)) for r
=
2 and 3 displays (003), (006), (009), (101), (110), and (113) crystal planes [3] with the basal spacing of 0.890 nm for (003), while for ratio 4 a new phase formed with different reflections for planes (003) (Figure 2(d)). This phase can be attributed to the presence of Zn/Al–CO3–LDH within prepared sample at ratio 4. A CO2 capture process from air based on the carbonation of NaOH aqueous solution has been estimated [4]. The FTIR spectra further confirm the presence of CO
3
- for LDH sample at ratio 4. Basal spacing is equal to the thickness of one brucite-like layer (4.8 Å) plus one interlayer which accounts for the interlayer gallery distance and can be calculated from Bragg’s equation.Figure 1
Schematic figure of (a) LDH and (b) LDH-SDS.Powder XRD patterns of ZnrAl-LDH and LDH-SDS with different SDS concentrations at (a) r
=
2, (b) r
=
3, (c) r
=
4, and (d) Zn/Al-LDH at ratios 2, 3, and 4.
(a)
(b)
(c)
(d)By intercalation of SDS into the LDH interlayer, SDS can increase the layer thickness considering its large molecular weight as seen in Figure1. As expected, the (003), (006), and (009) crystal planes [5] were observed in XRD patterns of the SDS intercalated samples as shown in Figure 2. The appearance of higher order peaks as well as the characteristic intense basal reflection peaks gives evidence of highly oriented in c-direction of intercalated LDH structure for all samples. SDS intercalation within the galleries was indicated from the shifting in the basal spacing. The basal spacing d
003 shifted from 0.89 nm for Zn4Al–NO3–LDH to 2.555 nm, 2.617 nm, and 2.560 nm for LDH-SDS with 0.2 M, 0.4 M, and 0.8 M of SDS, respectively. Similar basal spacing values were reported for LDH-SDS prepared by other methods [6]. The increasing of PXRD intensity of the LDH and LDH-SDS peaks was observed as the Zn2+/Al3+ molar ratio and the SDS concentration increases.The indexing of PXRD indicating the lattice parametersa, c, and c
′ for ZnrAl-LDH and LDH-SDS samples is shown in Table 1. Averaging the positions of the three harmonics can be used to calculate the interlayer spacing: c
=
(
1
/
3
) (3d
003 + 6d
006 + 9d
009), a
=
2
d
110 and c
=
3
c
′ [3]. Accepting the full length of SDS molecules as 2.08 nm, SDS molecules should form a tilted interdigitated bilayer between the Zn/Al sheets. The FT-IR spectra can further confirm the successful cointercalation of the SDS anions as shown in Figure 3.Table 1
The indexing and lattice parameters (a, c, and c
′) of the PXRD for the ZnrAl-LDH and LDH-SDS with different concentration of SDS.
Parameter (nm)
a
c
c
′
Interlayer thicknessa
D
b
Zn2-Al-LDH
0.30
2.64
0.88
0.40
30.29
LDH-SDS 0.2 M
0.30
7.67
2.55
2.07
29.99
LDH-SDS 0.4 M
0.30
7.74
2.58
2.10
42.89
LDH-SDS 0.8 M
0.30
7.78
2.59
2.11
51.44
Zn3-Al-LDH
0.30
2.65
0.88
0.40
23.67
LDH-SDS 0.2 M
0.30
7.81
2.60
2.12
45.97
LDH-SDS 0.4 M
0.30
7.66
2.55
2.07
28.07
LDH-SDS 0.8 M
0.30
7.76
2.58
2.10
34.38
Zn4-Al-LDH
0.30
2.66
0.88
0.40
28.85
LDH-SDS 0.2 M
0.30
7.69
2.56
2.08
23.42
LDH-SDS 0.4 M
0.30
7.84
2.65
2.12
31.57
LDHS-DS 0.8 M
0.30
7.73
2.57
2.09
33.09
aInterlayer thickness = (c
′—brucite-like sheet thickness).
b
D (average crystallite size in c direction) = value calculated from the values of (003), (006), and (009) diffraction peaks using the Scherrer equation.FT-IR spectra of ZnrAl-LDH and LDH-SDS with different concentrations of SDS at (a) r
=
2, (b) r
=
3, and (c) r
=
4.
(a)
(b)
(c)


### 3.2.  Fourier Transform Infrared (FTIR)

Figure3 shows the FT-IR spectra of ZnrAl–NO3–LDH and LDH-SDS in different concentration of SDS and at different molar ratio of Zn/Al. The FTIR spectra of the LDH precursor indicate a broad band at around 3398 cm−1. This band is attributed to the O–H stretching vibration in the brucite-like layers and the interlamellar water molecules [7] while the broadening of the band is assigned to formation of hydrogen bond [8]. The appearance of the strong absorption band located at 1387 cm−1 is attributed to the υ
3 stretching vibration of the NO
3
- groups in the LDH interlayer [9]. The sharpness of this peak of sample ratio 4 is lower than that in the other samples which may indicate the presence of Zn/Al–CO3–LDH phase [3]. A weak band located at 764 cm−1 and 1765 cm−1 arises from the stretching modes which confirm the presence of nitrate group, the intergallery anion with D
3
h symmetry in the Zn/Al LDH interlayer [9]. The bending vibration of the interlayer water molecules is indicated with the band at 1639 cm−1 [7].The appearance of the bands at around 414 cm−1 and 557 cm−1 is attributed to O–M–O vibrations in the brucite-like layers [10] and the lattice vibration modes corresponding to the translation vibration of Zn–OH [7], respectively. The relative intensity of band at 422 is clearly high for molar ratio of 4, but at ratio 2 and 3 it starts to decrease. This may suggest that the M–O vibrations of the LDH layers decreased due to the formation of new phases (CO
3
2
-).The FT-IR spectra of LDH-SDS were shown in Figure3. The wide band was found at 3464 cm−1 and it is attributed to the OH mode which is due to the hydroxyl groups and the interlayer water molecules in the brucite-like layers. The vibrations at 1197 and 1054 cm−1 are attributed to the OSO
3
- asymmetric and symmetric stretching vibration of the sulfonate group while the characteristic absorption peaks at 2919 and 2852 cm−1 arise from the asymmetric (CH2) and symmetric (CH2) vibration bands of SDS [11] (the observation of bands at around 1000–1370 cm−1 can imply the presence of SO
3
- group). The weak band observed at 1624 cm−1 is assigned to H2O from the interlayer water [12].The surfactant (SDS) displays two prominent vibrations at 2919 cm−1 and 2852 cm−1, corresponding to the symmetric and antisymmetric C–H– stretching modes of the terminal  –CH3 groups and a C–H bending vibration band at 1465 cm−1. The bands observed at around 414 cm−1 and 557 cm−1 for LDH samples were found at around 417 cm−1 (it was observed for all samples except Zn2Al-LDH-SDS 0.2 M) and 574 cm−1, respectively, for LDH-SDS samples which are assigned to the lattice vibrations of the metal hydroxide sheets [13]. The nitrate ion vibration mode at 1387 cm−1 disappears in SDS-LDH which is due to the ion exchange process and thus suggests that the SDS can completely replace the nitrate anions in the LDH interlayer. It is noteworthy that the extra weak band at around 2040 cm−1 is observed for samples with ratio 4 which can be assigned to adsorbed CO
3
2
- species [14].


### 3.3.  Optical Properties (UV-VIS-NIR)

UV-VIS-NIR diffuse reflectance spectra by using the Kubelka-Munk equation shown below were used to obtain the energy gap [15]:
(1)
F
(
R
∞
)
=
(
1
-
R
)
2
2
R
∞
,
(2)
(
F
(
R
∞
)
h
υ
)
2
=
C
(
h
υ
-
E
g
)
,
where F
(
R
∞
)is called Kubelka-Munk function or the remission and the diffuse reflectance (R
∞) of the samples is R
∞
=
R
sample
/
R
standard [16], h
υ is the photon energy, and C is a proportionality constant. The energy gap of Zn/Al-LDH can be obtained based on the Kubelka-Munk model according to (2). The F
(
R
∞
)from (1) was plotted as (
F
(
R
∞
)
h
υ
)
2 against h
υ, from which the energy gap (E
g) of the samples can be easily extracted.The energy gaps of ZnrAl–NO3–LDH and LDH-SDS in different concentrations were investigated by these measurements and are shown in Figures 4 and 5. Figure 4 shows the energy gap (E
g) of Zn3Al–NO3–LDH and LDH-SDS in different concentrations. Due to the presence of LDH phase, two band gap energies (E
g
1 and E
g
2) were observed. The first band gap (E
g
1) for ZnrAl–NO3–LDH is 4.8 and 4.75 eV for r
=
2 and 3, respectively. The second one (E
g
2) is 3.75 eV for r
=
2 and 3.72 eV for r
=
3. All values of band gap energy for the different prepared samples were tabulated in Table 2. E
g
1 and E
g
2 can be attributed to the presence of NO
3
- groups in the LDH interlayer [10]. In addition, E
g
1 also can be ascribed to the electronic transition of Zn-Al-LDH which is a direct process from oxygen2p to metalns ornp levels (n
=
4 for Zn and n
=
3 for Al) [17]. These results are in good agreement with the literature [14]. The peak corresponding to the NO
3
- radical at 300 nm in Figure 6 confirms this suggestion.Table 2
The energy gaps of ZnrAl–NO3–LDH and LDH-SDS in different concentrations of SDS.
Sample
E
g
2 (eV)
E
g
1 (eV)
Zn2Al-LDH
3.75
4.80
Zn2Al-LDH-SDS 0.2 M
4.10
5.20
Zn2Al-LDH-SDS 0.4 M
4.10
5.20
Zn2Al-LDH-SDS 0.8 M
4.15
5.20
Zn3Al-LDH
3.72
4.75
Zn3Al-LDH-SDS 0.2 M
3.90
5.10
Zn3Al-LDH-SDS 0.4 M
3.75
4.95
Zn3Al-LDH-SDS 0.8 M
3.90
5.10
Zn4Al-LDH
3.75
4.80
Zn4Al-LDH-SDS 0.2 M
3.20
4.30
Zn4Al-LDH-SDS 0.4 M
3.23
—
Zn4Al-LDH-SDS 0.8 M
3.24
—Kubelka-Munk transformed reflectance spectra of Zn3Al–NO3–LDH and LDH-SDS in different concentrations.
(a)
(b)
(c)
(d)Kubelka-Munk transformed reflectance spectra of Zn4Al–NO3–LDH and LDH-SDS in different concentrations.
(a)
(b)
(c)
(d)Diffuse reflectance UV-visible absorption spectra of ZnrAl–NO3–LDH and LDH-SDS in different concentrations.
(a)
(b)
(c)
(d)Due to the intercalation of SDS into the LDH interlayer, SDS is replaced withNO
3
- in the interlayer galleries. Consequently, for ZnrAl-LDH-SDS samples in different concentration of SDS, for r
=
2, the band gap energy of E
g
1 and E
g
2 is found to increase to 5.2 eV and 4.1 eV, respectively, and for r
=
3, E
g
1 and E
g
2 increased to around 5.1 eV and 3.9 eV, respectively. These E
g values can be due to the electronic transition of the oxygen from the DS anion (SO
4
2
-) and a nearby Al nucleus (I
=
5
/
2) from the LDH sheets. When r
=
4, for sample with 0.2 M of SDS, the values of E
g
1 and E
g
2 were found around 4.3 eV and 3.2 eV, respectively, while, for 0.4 M and 0.8 M of SDS, only one energy gap in 3.2 eV was observed.Figure6 shows the diffuse reflectance UV-visible absorption spectra of different samples, which exhibits a clear peak at 300 nm for LDH samples corresponding to the existence of NO
3
- ions in LDH interlayer [14]. The relative intensity of 300 nm peak for Zn3Al-LDH is higher than that of ratios 2 and 4 which suggests the increase in the crystallinity of LDH at ratio 3. For LDH-SDS samples with molar ratios 2 and 3, the absorption peaks at around 265 nm are assigned to the SO
4
2
- nanostructures formed within LDH samples due to the intercalation process. The broad peaks at around 355 nm for LDH-SDS samples with ratio 4 may suggest that they include more than an absorption peak with different degree of crystallinity due to the presence of CO
3
2
- anions (as was observed in FTIR) and SO
4
2
- phase.


### 3.4. Thermal Diffusivity

One of greatest importance thermal properties which is used to study the conductive heat of materials is thermal diffusivity (α). Equation (3) displays the dependency of thermal diffusivity to physical properties such as specific heat capacity (c
p), density (ρ), and thermal conductivity (k)
(3)
α
=
k
ρ
c
p
.A nonlinear relation of thermal diffusivity versus in situ temperatures for Zn4Al-LDH and LDH-SDS in different concentration of SDS is shown in Figure7. The results display that the thermal diffusivity of pure LDH is increasing as the temperature increases. Thermal diffusivity of LDH-SDS samples were decreased compared to Zn/Al-LDH. The results explain that the value of thermal diffusivity was also decreased as the amount of SDS increased at room temperature. By increasing the temperature typically it was observed to increase up to 90°C and decrease up to the higher temperature.Figure 7
In situ temperature versus thermal diffusivity for Zn4Al-LDH and LDH-SDS in different concentrations of SDS.


### 3.5. Field Emission Scanning Electron Microscopy (FESEM)

The FESEM micrographs of Zn/Al–NO3–LDH and Zn/Al-LDH-SDS samples prepared at Zn2+/Al3+ molar ratio of 4 are shown in Figure 8.FESEM images of Zn4Al-LDH synthesized in the presence of (a) no SDS, (b) 0.2 M SDS, (c) 0.4 M SDS, and (d) 0.8 M SDS.
(a)
(b)
(c)
(d)The LDH sample shows darkness micrograph with rough texture some smooth regions and plate-like particles with roughly hexagonal shapes which indicate presynthesized LDH sheets. Observation of some flakes and rod-like structures on the surface for LDH-SDS sample identifies the new phase. It is also clear that by increasing the amount of SDS the flakes and rod-like structures increased on surface. The FESEM images of LDH-SDS samples revealed that they show agglomerates of compact and nonporous plate-like structures, not much different from the observed structure for LDH, and there is no significant difference in the morphology of all samples. It is also very similar to the morphology of other nanocomposites, such as Zn-Al-poly(acrylic acid)-LDH, Zn-Al-poly(vinyl sulfonate)-LDH, and Zn-Al-poly(styrene sulfonate)-LDH [18].


## 3.1.  Powder X-Ray Diffraction (XRD) Study

SDS (sodium dodecyl sulfate) intercalated Zn/Al-LDH nanocomposites were prepared using precipitation method. Figure2 shows that the powder XRD patterns of the Zn/Al–NO3 and SDS intercalated LDHs synthesized in different concentration of SDS. The sharpness of the peaks suggests ordered and regular stacking of the LDH layers. XRD of the ZnrAl–NO3–LDH samples (Figure 1(d)) for r
=
2 and 3 displays (003), (006), (009), (101), (110), and (113) crystal planes [3] with the basal spacing of 0.890 nm for (003), while for ratio 4 a new phase formed with different reflections for planes (003) (Figure 2(d)). This phase can be attributed to the presence of Zn/Al–CO3–LDH within prepared sample at ratio 4. A CO2 capture process from air based on the carbonation of NaOH aqueous solution has been estimated [4]. The FTIR spectra further confirm the presence of CO
3
- for LDH sample at ratio 4. Basal spacing is equal to the thickness of one brucite-like layer (4.8 Å) plus one interlayer which accounts for the interlayer gallery distance and can be calculated from Bragg’s equation.Figure 1
Schematic figure of (a) LDH and (b) LDH-SDS.Powder XRD patterns of ZnrAl-LDH and LDH-SDS with different SDS concentrations at (a) r
=
2, (b) r
=
3, (c) r
=
4, and (d) Zn/Al-LDH at ratios 2, 3, and 4.
(a)
(b)
(c)
(d)By intercalation of SDS into the LDH interlayer, SDS can increase the layer thickness considering its large molecular weight as seen in Figure1. As expected, the (003), (006), and (009) crystal planes [5] were observed in XRD patterns of the SDS intercalated samples as shown in Figure 2. The appearance of higher order peaks as well as the characteristic intense basal reflection peaks gives evidence of highly oriented in c-direction of intercalated LDH structure for all samples. SDS intercalation within the galleries was indicated from the shifting in the basal spacing. The basal spacing d
003 shifted from 0.89 nm for Zn4Al–NO3–LDH to 2.555 nm, 2.617 nm, and 2.560 nm for LDH-SDS with 0.2 M, 0.4 M, and 0.8 M of SDS, respectively. Similar basal spacing values were reported for LDH-SDS prepared by other methods [6]. The increasing of PXRD intensity of the LDH and LDH-SDS peaks was observed as the Zn2+/Al3+ molar ratio and the SDS concentration increases.The indexing of PXRD indicating the lattice parametersa, c, and c
′ for ZnrAl-LDH and LDH-SDS samples is shown in Table 1. Averaging the positions of the three harmonics can be used to calculate the interlayer spacing: c
=
(
1
/
3
) (3d
003 + 6d
006 + 9d
009), a
=
2
d
110 and c
=
3
c
′ [3]. Accepting the full length of SDS molecules as 2.08 nm, SDS molecules should form a tilted interdigitated bilayer between the Zn/Al sheets. The FT-IR spectra can further confirm the successful cointercalation of the SDS anions as shown in Figure 3.Table 1
The indexing and lattice parameters (a, c, and c
′) of the PXRD for the ZnrAl-LDH and LDH-SDS with different concentration of SDS.
Parameter (nm)
a
c
c
′
Interlayer thicknessa
D
b
Zn2-Al-LDH
0.30
2.64
0.88
0.40
30.29
LDH-SDS 0.2 M
0.30
7.67
2.55
2.07
29.99
LDH-SDS 0.4 M
0.30
7.74
2.58
2.10
42.89
LDH-SDS 0.8 M
0.30
7.78
2.59
2.11
51.44
Zn3-Al-LDH
0.30
2.65
0.88
0.40
23.67
LDH-SDS 0.2 M
0.30
7.81
2.60
2.12
45.97
LDH-SDS 0.4 M
0.30
7.66
2.55
2.07
28.07
LDH-SDS 0.8 M
0.30
7.76
2.58
2.10
34.38
Zn4-Al-LDH
0.30
2.66
0.88
0.40
28.85
LDH-SDS 0.2 M
0.30
7.69
2.56
2.08
23.42
LDH-SDS 0.4 M
0.30
7.84
2.65
2.12
31.57
LDHS-DS 0.8 M
0.30
7.73
2.57
2.09
33.09
aInterlayer thickness = (c
′—brucite-like sheet thickness).
b
D (average crystallite size in c direction) = value calculated from the values of (003), (006), and (009) diffraction peaks using the Scherrer equation.FT-IR spectra of ZnrAl-LDH and LDH-SDS with different concentrations of SDS at (a) r
=
2, (b) r
=
3, and (c) r
=
4.
(a)
(b)
(c)


## 3.2.  Fourier Transform Infrared (FTIR)

Figure3 shows the FT-IR spectra of ZnrAl–NO3–LDH and LDH-SDS in different concentration of SDS and at different molar ratio of Zn/Al. The FTIR spectra of the LDH precursor indicate a broad band at around 3398 cm−1. This band is attributed to the O–H stretching vibration in the brucite-like layers and the interlamellar water molecules [7] while the broadening of the band is assigned to formation of hydrogen bond [8]. The appearance of the strong absorption band located at 1387 cm−1 is attributed to the υ
3 stretching vibration of the NO
3
- groups in the LDH interlayer [9]. The sharpness of this peak of sample ratio 4 is lower than that in the other samples which may indicate the presence of Zn/Al–CO3–LDH phase [3]. A weak band located at 764 cm−1 and 1765 cm−1 arises from the stretching modes which confirm the presence of nitrate group, the intergallery anion with D
3
h symmetry in the Zn/Al LDH interlayer [9]. The bending vibration of the interlayer water molecules is indicated with the band at 1639 cm−1 [7].The appearance of the bands at around 414 cm−1 and 557 cm−1 is attributed to O–M–O vibrations in the brucite-like layers [10] and the lattice vibration modes corresponding to the translation vibration of Zn–OH [7], respectively. The relative intensity of band at 422 is clearly high for molar ratio of 4, but at ratio 2 and 3 it starts to decrease. This may suggest that the M–O vibrations of the LDH layers decreased due to the formation of new phases (CO
3
2
-).The FT-IR spectra of LDH-SDS were shown in Figure3. The wide band was found at 3464 cm−1 and it is attributed to the OH mode which is due to the hydroxyl groups and the interlayer water molecules in the brucite-like layers. The vibrations at 1197 and 1054 cm−1 are attributed to the OSO
3
- asymmetric and symmetric stretching vibration of the sulfonate group while the characteristic absorption peaks at 2919 and 2852 cm−1 arise from the asymmetric (CH2) and symmetric (CH2) vibration bands of SDS [11] (the observation of bands at around 1000–1370 cm−1 can imply the presence of SO
3
- group). The weak band observed at 1624 cm−1 is assigned to H2O from the interlayer water [12].The surfactant (SDS) displays two prominent vibrations at 2919 cm−1 and 2852 cm−1, corresponding to the symmetric and antisymmetric C–H– stretching modes of the terminal  –CH3 groups and a C–H bending vibration band at 1465 cm−1. The bands observed at around 414 cm−1 and 557 cm−1 for LDH samples were found at around 417 cm−1 (it was observed for all samples except Zn2Al-LDH-SDS 0.2 M) and 574 cm−1, respectively, for LDH-SDS samples which are assigned to the lattice vibrations of the metal hydroxide sheets [13]. The nitrate ion vibration mode at 1387 cm−1 disappears in SDS-LDH which is due to the ion exchange process and thus suggests that the SDS can completely replace the nitrate anions in the LDH interlayer. It is noteworthy that the extra weak band at around 2040 cm−1 is observed for samples with ratio 4 which can be assigned to adsorbed CO
3
2
- species [14].


## 3.3.  Optical Properties (UV-VIS-NIR)

UV-VIS-NIR diffuse reflectance spectra by using the Kubelka-Munk equation shown below were used to obtain the energy gap [15]:
(1)
F
(
R
∞
)
=
(
1
-
R
)
2
2
R
∞
,
(2)
(
F
(
R
∞
)
h
υ
)
2
=
C
(
h
υ
-
E
g
)
,
where F
(
R
∞
)is called Kubelka-Munk function or the remission and the diffuse reflectance (R
∞) of the samples is R
∞
=
R
sample
/
R
standard [16], h
υ is the photon energy, and C is a proportionality constant. The energy gap of Zn/Al-LDH can be obtained based on the Kubelka-Munk model according to (2). The F
(
R
∞
)from (1) was plotted as (
F
(
R
∞
)
h
υ
)
2 against h
υ, from which the energy gap (E
g) of the samples can be easily extracted.The energy gaps of ZnrAl–NO3–LDH and LDH-SDS in different concentrations were investigated by these measurements and are shown in Figures 4 and 5. Figure 4 shows the energy gap (E
g) of Zn3Al–NO3–LDH and LDH-SDS in different concentrations. Due to the presence of LDH phase, two band gap energies (E
g
1 and E
g
2) were observed. The first band gap (E
g
1) for ZnrAl–NO3–LDH is 4.8 and 4.75 eV for r
=
2 and 3, respectively. The second one (E
g
2) is 3.75 eV for r
=
2 and 3.72 eV for r
=
3. All values of band gap energy for the different prepared samples were tabulated in Table 2. E
g
1 and E
g
2 can be attributed to the presence of NO
3
- groups in the LDH interlayer [10]. In addition, E
g
1 also can be ascribed to the electronic transition of Zn-Al-LDH which is a direct process from oxygen2p to metalns ornp levels (n
=
4 for Zn and n
=
3 for Al) [17]. These results are in good agreement with the literature [14]. The peak corresponding to the NO
3
- radical at 300 nm in Figure 6 confirms this suggestion.Table 2
The energy gaps of ZnrAl–NO3–LDH and LDH-SDS in different concentrations of SDS.
Sample
E
g
2 (eV)
E
g
1 (eV)
Zn2Al-LDH
3.75
4.80
Zn2Al-LDH-SDS 0.2 M
4.10
5.20
Zn2Al-LDH-SDS 0.4 M
4.10
5.20
Zn2Al-LDH-SDS 0.8 M
4.15
5.20
Zn3Al-LDH
3.72
4.75
Zn3Al-LDH-SDS 0.2 M
3.90
5.10
Zn3Al-LDH-SDS 0.4 M
3.75
4.95
Zn3Al-LDH-SDS 0.8 M
3.90
5.10
Zn4Al-LDH
3.75
4.80
Zn4Al-LDH-SDS 0.2 M
3.20
4.30
Zn4Al-LDH-SDS 0.4 M
3.23
—
Zn4Al-LDH-SDS 0.8 M
3.24
—Kubelka-Munk transformed reflectance spectra of Zn3Al–NO3–LDH and LDH-SDS in different concentrations.
(a)
(b)
(c)
(d)Kubelka-Munk transformed reflectance spectra of Zn4Al–NO3–LDH and LDH-SDS in different concentrations.
(a)
(b)
(c)
(d)Diffuse reflectance UV-visible absorption spectra of ZnrAl–NO3–LDH and LDH-SDS in different concentrations.
(a)
(b)
(c)
(d)Due to the intercalation of SDS into the LDH interlayer, SDS is replaced withNO
3
- in the interlayer galleries. Consequently, for ZnrAl-LDH-SDS samples in different concentration of SDS, for r
=
2, the band gap energy of E
g
1 and E
g
2 is found to increase to 5.2 eV and 4.1 eV, respectively, and for r
=
3, E
g
1 and E
g
2 increased to around 5.1 eV and 3.9 eV, respectively. These E
g values can be due to the electronic transition of the oxygen from the DS anion (SO
4
2
-) and a nearby Al nucleus (I
=
5
/
2) from the LDH sheets. When r
=
4, for sample with 0.2 M of SDS, the values of E
g
1 and E
g
2 were found around 4.3 eV and 3.2 eV, respectively, while, for 0.4 M and 0.8 M of SDS, only one energy gap in 3.2 eV was observed.Figure6 shows the diffuse reflectance UV-visible absorption spectra of different samples, which exhibits a clear peak at 300 nm for LDH samples corresponding to the existence of NO
3
- ions in LDH interlayer [14]. The relative intensity of 300 nm peak for Zn3Al-LDH is higher than that of ratios 2 and 4 which suggests the increase in the crystallinity of LDH at ratio 3. For LDH-SDS samples with molar ratios 2 and 3, the absorption peaks at around 265 nm are assigned to the SO
4
2
- nanostructures formed within LDH samples due to the intercalation process. The broad peaks at around 355 nm for LDH-SDS samples with ratio 4 may suggest that they include more than an absorption peak with different degree of crystallinity due to the presence of CO
3
2
- anions (as was observed in FTIR) and SO
4
2
- phase.


## 3.4. Thermal Diffusivity

One of greatest importance thermal properties which is used to study the conductive heat of materials is thermal diffusivity (α). Equation (3) displays the dependency of thermal diffusivity to physical properties such as specific heat capacity (c
p), density (ρ), and thermal conductivity (k)
(3)
α
=
k
ρ
c
p
.A nonlinear relation of thermal diffusivity versus in situ temperatures for Zn4Al-LDH and LDH-SDS in different concentration of SDS is shown in Figure7. The results display that the thermal diffusivity of pure LDH is increasing as the temperature increases. Thermal diffusivity of LDH-SDS samples were decreased compared to Zn/Al-LDH. The results explain that the value of thermal diffusivity was also decreased as the amount of SDS increased at room temperature. By increasing the temperature typically it was observed to increase up to 90°C and decrease up to the higher temperature.Figure 7
In situ temperature versus thermal diffusivity for Zn4Al-LDH and LDH-SDS in different concentrations of SDS.


## 3.5. Field Emission Scanning Electron Microscopy (FESEM)

The FESEM micrographs of Zn/Al–NO3–LDH and Zn/Al-LDH-SDS samples prepared at Zn2+/Al3+ molar ratio of 4 are shown in Figure 8.FESEM images of Zn4Al-LDH synthesized in the presence of (a) no SDS, (b) 0.2 M SDS, (c) 0.4 M SDS, and (d) 0.8 M SDS.
(a)
(b)
(c)
(d)The LDH sample shows darkness micrograph with rough texture some smooth regions and plate-like particles with roughly hexagonal shapes which indicate presynthesized LDH sheets. Observation of some flakes and rod-like structures on the surface for LDH-SDS sample identifies the new phase. It is also clear that by increasing the amount of SDS the flakes and rod-like structures increased on surface. The FESEM images of LDH-SDS samples revealed that they show agglomerates of compact and nonporous plate-like structures, not much different from the observed structure for LDH, and there is no significant difference in the morphology of all samples. It is also very similar to the morphology of other nanocomposites, such as Zn-Al-poly(acrylic acid)-LDH, Zn-Al-poly(vinyl sulfonate)-LDH, and Zn-Al-poly(styrene sulfonate)-LDH [18].


## 4. Conclusion

Zn/Al-LDH-SDS nanocomposites of different concentration of SDS have been prepared using a coprecipitation method. The XRD and FTIR data show the successful intercalation of SDS into the LDH interlayer. The crystallinity of the LDH-SDS nanocomposites increases by increasing the amount of SDS. The energy band gap of LDH-SDS samples was found to increase with respect to the unmodified LDH. Thermal diffusivity was observed to decrease in the form of LDH-SDS nanocomposite.



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*Source: 467064-2014-10-28.xml*