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Article

Comprehensive Characterization of the Structure and Gel Property of Organo-Montmorillonite: Effect of Layer Charge Density of Montmorillonite and Carbon Chain Length of Alkyl Ammonium

by
Jun Qiu
1,*,
Dongliang Liu
2,
Yueting Wang
2,
Guowei Chen
2,
Shan Jiang
2,
Guoqing Li
2,
Yaqi Wang
1,
Wenxin Wang
1,
Peng Wu
1,
Xiaodong Liu
1,
Guifang Wang
3 and
Xianjun Lyu
1
1
College of Chemical and Biological Engineering, Shandong University of Science and Technology, Qingdao 266590, China
2
College of Safety and Environmental Engineering, Shandong University of Science and Technology, Qingdao 266590, China
3
School of Resources Environment and Materials, Guangxi University, Nanning 530004, China
*
Author to whom correspondence should be addressed.
Minerals 2020, 10(4), 378; https://doi.org/10.3390/min10040378
Submission received: 1 April 2020 / Revised: 21 April 2020 / Accepted: 22 April 2020 / Published: 22 April 2020
(This article belongs to the Section Mineral Processing and Extractive Metallurgy)
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Abstract

:
In this work, the effect of layer charge density of Na-montmorillonite (Na-MT) and carbon chain length of alkyl ammonium on the structure and gel property of organo-montmorillonite (organo-MT) was studied by using X-ray diffraction (XRD), Fourier transform infrared (FTIR), thermogravimetric (TG) analysis, contact angle test, molecular dynamics (MD) simulation, and gel apparent viscosity determination experiment. The results of XRD show that Na-MT with lower layer charge density is easier to swell after intercalation of alkyl ammonium, and the basal spacing of organo-MT increases with the increase of carbon chain length. The results of FTIR show that the absorption bands at 2924 cm−1 and 2853 cm−1 shift towards low frequency region with the increase of carbon chain length, and the absorption bands at 515 cm−1 and 463 cm−1 move towards high frequency region when the layer charge density increases. The mass loss of organo-MT evidently increases with the increase of layer charge density of Na-MT or carbon chain length of alkyl ammonium. The contact angle test results are well in line with the TG data and reveal that alkyl ammonium with longer carbon chain can significantly improve the hydrophobicity of organo-MT. MD simulation indicates that, when the layer charge density is low, the distribution of alkyl ammonium gradually changes from parallel double layers to partially inclined distribution with the increase of carbon chain length, but when the layer charge density is high, the distribution of alkyl ammonium gradually changes from three layers into four layers. The test results of the apparent viscosity of the gel formed by organo-MT in xylene show that the apparent viscosity of organo-MT gel is negatively correlated with the layer charge density of Na-MT and positively correlated with the carbon chain length of alkyl ammonium.

1. Introduction

Montmorillonite (MT) is a kind of typical phyllosilicate clay mineral and is rich in nature. Its structure is an octahedral sheet sandwiched by two tetrahedral layers [1,2]. Because of its large specific surface area (SSA), low cost, high cation exchange capacity (CEC), and good swelling ability in aqueous solution, MT has attracted wide attention both in academia and in industry [3,4,5,6]. The occurrence of non-equivalent isomorphic substitution of Al3+ for Si4+ in the tetrahedral sheets and Mg2+ for Al3+ in the octahedral layers makes MT layers negatively charged [7]. To balance the negative layer charge density of MT, some hydrophilic exchangeable cations, such as Na+, K+, and Ca2+, are usually attracted into the interlayer domain, and due to the hydration of inorganic cation [8,9], confined basal spacing, and high surface energy, natural MT performs badly in organic phase environment [6,10].
In order to expand the application of MT in industry, organo-MT is synthesized by intercalating surfactant into interlayer space of natural MT [11]. In this way, interlayer distance of MT obviously increase and new sorption sites can be formed [12], besides, inorganic cation can be exchanged by surfactant, which results in that the surface property of MT converts from hydrophilic to hydrophobic. As a result, the organo-MT can be applied in many fields, such as polymer MT nanocomposite [13,14], adsorbent for organic contaminant [15,16], oil-based drilling fluid [17], pharmaceutical, cosmetic additives, thixotropic agent in paint, etc. [18].
So far, in the research process of organo-MT, various kinds of cationic [17], anionic [14], nonionic [19], amphoteric, and even hybrid surfactants have been used [5,20,21,22], and many scholars found that the structure and property of organo-MT were closely related to many factors, such as carbon chain length and concentration of surfactant. Zhang et al. and Ma et al. found that cationic surfactant with long carbon chain could significantly increase the interlayer distance of organo-MT, and organo-MT had better adsorption capacity to organic contaminant than natural MT [12,15]. Yunfei Xi and his co-writers reported that variation in the d(001) was a step function of octadecyl trimethyl ammonium bromide concentration, the arrangement of surfactant between MT layers changed stepwise from monolayer to pseudo trimolecular layer with the increase of concentration of surfactant [7]. Taleb et al. proposed that the thermal stability of organo-MT was better when Na-MT is modified by surfactant with higher concentration and longer carbon chain [23]. Zhuang et al. concluded that organo-MT prepared by surfactant with bigger size and lower Hydrophile-Lipophile Balance value could be easier to exfoliate in oil [17]. Similar rules were also verified by other investigators [24,25,26].
Moreover, layer charge density of MT, type of interlayer cation, modification condition, and so on can also influence the structure and property of organo-MT. Wu et al. and Chen et al. studied the influence of type of interlayer cation on organic intercalation of MT, and they found that, the weaker the electrostatic attraction between interlayer cation and MT sheets, the easier the organic intercalation of surfactant into MT layers [11,27]. Peng et al. studied the effect of pH on the adsorption of dodecyl amine (DDA) on MT surfaces in aqueous solution and found that the hydrophobicity of DDA-MT was the best when the pH of aqueous solution is 8.0 [28].
Although large amounts of works on the organic modification of MT have been done, but to our knowledge, there is no systemic comparative study about the effect of layer charge density of Na-MT and carbon chain length of alkyl ammonium on the structure and gel property of organo-MT. For this purpose, four types of alkyl ammonium with different carbon chain length are used as intercalated modifier, two kinds of MT with different layer charge density are used as research materials, and the prepared organo-MT under different conditions are comprehensively characterized by XRD, FTIR, TG analysis, contact angle test, and gel apparent viscosity test combined with molecular dynamics (MD) simulation. The research results of this work can bring new insights into the influence mechanism of layer charge density of MT and carbon chain length of alkyl ammonium on the structure and gel property of organo-MT, which can pave the way to apply organo-MT in industry.

2. Materials and Methods

2.1. Materials

The two kinds of Ca-MT are obtained from Shandong and Inner Mongolia of China, respectively, and are purified by natural sedimentation method. Their chemical compositions are presented in Table 1. Their semi-cell structure formulas are (Ca0.17K0.02Mg0.01)0.38·{(Al1.63Fe0.01Mg0.36)2.00[(Si3.98Al0.02)4.00O10](OH)2} and (Na0.03Ca0.29K0.04Mg0.02)0.69·{(Al1.27Fe0.04Ti0.03Mg0.66)2.00[(Si3.94Al0.06)4.00O10](OH)2}, and their corresponding layer charge density is 0.38 and 0.69, respectively. In order to improve the dispersity of Ca-MT in water, both of them were sodium-modified by Na2CO3 of 4.0% (wt %) for 1.0 h at room temperature, dehydrated by centrifugation in the centrifugal machine (TD5A-WS, Jiangsu Jintan Instrument Factory, Jintan, China), dried in the oven (302, Shandong Longkou Xianke Instrument Co., Ltd., Longkou, China) at 80.0 °C for 24.0 h, and then ground to less than 200 mesh by vibrating grinder (XZM-100, Wuhan Prospecting Machinery Factory, Wuhan, China). The prepared Na-MT were denoted as Na-MT1 and Na-MT2, respectively, and their SSA, pore volume (PV), average pore diameter (APD), and cation exchange capacity (CEC) are measured and showed in Table 2.
Both absolute ethyl alcohol and xylene were purchased from Tianjin Fuyu Fine Chemical Co., Ltd. (Tianjin, China). The four types of alkyl ammonium are dodecyl trimethyl ammonium chloride (DTAC), tetradecyl trimethyl ammonium chloride (TTAC), hexadecyl trimethyl ammonium chloride (HTAC), and octadecyl trimethyl ammonium chloride (OTAC), respectively. The DTAC with 98.0% purity was purchased from Shanghai Shanpu Chemical Co., Ltd. (Shanghai, China). The TTAC with 99.0% purity was purchased from Shanghai Macklin Biochemical Co., Ltd. (Shanghai, China). The HTAC with 98.0% purity was purchased from Tianjin Zhiyuan Chemical Reagent Co., Ltd. (Tianjin, China). The OTAC with 99.0% purity was purchased from Sinopharm Chemical Reagent Co., Ltd. (Shanghai, China). All the alkyl ammonium were directly used without further purification, and their molecular structures are shown in Figure 1.

2.2. Preparation of Organo-MT

Organo-MT were prepared by dissolving 10.0 g of Na-MT into distilled water at 80.0 °C in a 250.0 mL beaker, then slowly adding the dispersed solution of DTAC, TTAC, HTAC, or OTAC under the same temperature condition. The mass of alkyl ammonium added was equivalent to 1.0 CEC of Na-MT, and the mass ratio of water to dried Na-MT was 20:1. The mixture was stirred for 2.0 h at 80.0 °C, then the prepared organo-MT was collected by centrifugation at 4000 r/min, washed with distilled water until there is no Cl− examined by AgNO3, dried in the drying oven (302, Shandong Longkou Xianke Instrument Co., Ltd., Longkou, China) at 80.0 °C for 48.0 h, and ground to less than 200 mesh by vibrating grinder (XZM-100, Wuhan Prospecting Machinery Factory, Wuhan, China). The obtained samples are denoted as Cn-MT1 or Cn-MT2, where n = 12, 14, 16, or 18, respectively.

2.3. Analytical Methods

Powder XRD patterns of samples were recorded with a D/max-r B diffractometer using Cu Kα radiation at 40.0 KV and 100.0 mA (Rigaku Corporation, Akishima-shi, Japan). The diffraction angle of patterns was collected from 3.0° to 20.0° with a scanning speed of 3.0°/min.
FTIR spectrum of Na-MT and corresponding organo-MT were collected by using the Nicolet Is 50 fourier infrared spectrometer (Thermo Fisher Scientific, Waltham, MA, USA) with the KBr pellet method (1.00 mg of sample homogenized with 200.00 mg KBr). The wavenumber range was 4000–400 cm−1 with resolution of 4.0 cm−1.
TG analysis was performed on TG/SDTA851e thermogravimetric/differential thermal synchronization analyzer (Mettler-Toledo, Zurich, Switzerland). The sample was heated from 30.0 °C to 1000.0 °C at a rate of 20.0 °C/min. The flow of high purity nitrogen was 20.0 mL/min.
Contact angle test was performed on DSA 30 optical contact angle analyzer (Kruss, Hamburg, Germany). For this purpose, a pellet was prepared under 5.0–10.0 MPa pressure using about 0.50 g sample.
MD simulation was performed by Materials Studio 7.0 software (Accelrys, San Diego, CA, USA) to further investigate the conformation of alkyl ammonium within organo-MT interlayer. According to the semi-cell structural formula, 4a × 2b × 1c super-cell models were established for simulation study. Our previous study had proved that when the mass of modifier is equivalent to the 1.0 CEC of Na-MT, alkyl ammonium cation can totally enter into the interlayer of Na-MT [29]; therefore, according to the calculation result, we, respectively, added six alkyl ammonium cation into Cn-MT1 interlayer and eleven alkyl ammonium cation into Cn-MT2 interlayer to ensure total charge balance of the crystal. Then we added different amounts of H2O to ensure that the d001 value of simulation result was consistent with XRD data. The number of alkyl ammonium cation and H2O added is shown in Table 3.
The geometry optimization task was performed to relax the structure of organo-MT model under the following conditions: the organo-MT layers were assumed to be rigid, the cell parameters a, b, α, γ remained unchanged, and c and β were variable. The algorithm selected was Smart Minimizer, the long-range electrostatic interaction used was Ewald summation method, and the short-range van der Waals used was atom-based summation method. The vacuum cutoff radius was 12.5 Å, the spline width was 1.0 Å, the buffer width was 0.5 Å, and the number of iteration steps was 5000. The geometry optimization results of organo-MT models are shown in Table 4. After geometry optimization, molecular dynamics simulation was carried out under NPT ensemble and NVT ensemble, respectively. The simulation temperature was 298.0 K, pressure was 1.0 × 10−4 GPa, the time step length was 1.0 fs, the numbers of steps were 2 × 106, and the total simulation time was 2.0 ns. During the simulation, atomic coordinates and lattice parameters were allowed to change freely, and the output data was used for result analysis.
Before gel apparent viscosity measurement, we weighed 65.80 g xylene solvent in a 50.0 mL beaker, put the beaker at high speed mixer (GFJ-QA, Jiangyin Shuangye Machinery Co., Ltd., Jiangyin, China), submerged solvent dispersion plate to highly 1/3 volume of the beaker, adjusted the speed of high-speed mixer to 500 r/min, added 6.00 g of organo-MT sample under the condition, stirred for 3 min at 1500 r/min, added 95% ethanol solution of 3.8 mL and stirred for 2 min, and then stirred for 5.0 min at 3000 r/min. Then, we removed the beaker after stopping.
We placed the beaker on the digital viscometer (SNB-2, Shanghai Fangrui Instrument Co., Ltd., Shanghai, China) to test the apparent viscosity of organo-MT gel. Using the No. 3 rotor, we adjusted the viscometer until the groove (immersion mark) on the shaft of the rotor just touches the sample. We slowly moved the beaker on the horizontal surface to ensure that the rotor was located in the center of the beaker. We adjusted the measured speed of the viscometer to 6 r/min and read the number of the display screen after rotating it 10 times.

3. Results and Discussion

3.1. XRD Analysis

XRD patterns of Ca(Na)-MT and organo-MT prepared by alkyl ammonium with different carbon chain length are shown in Figure 2.
Figure 2 shows the XRD patterns of Ca(Na)-MT and organo-MT prepared by alkyl ammonium with different carbon chain length. It can be seen from Figure 2a that the diffraction peaks of (001) of the two kinds of Ca-MT appear at about 5.89°, and the basal spacing d(001) of Ca-MT1 and Ca-MT2 is 15.0685 Å and 14.9669 Å, respectively. After Ca-MT was modified by Na2CO3, the diffraction peaks of (001) shift towards 7.12°, and the corresponding basal spacing d(001) decreases to 12.4389 Å and 12.6541 Å, respectively. This result proves that Ca-MT have been sodium modified successfully [7].
From Figure 2a,b, we can find that the diffraction peaks of (001) of organo-MT appear at smaller angle than that of Na-MT, which indicates that the interlayer distance of Na-MT is expanded after intercalation of alkyl ammonium [3,30]. Besides, it can be seen that the d(001) value of the two kinds of organo-MT shows stepwise increment with the increase of carbon chain length, for example, the d(001) of C12-MT1, C14-MT1, C16-MT1, and C18-MT1 increases from 12.4389 Å to 23.4840 Å, 26.1226 Å, 29.0324 Å, and 36.1958 Å, respectively. The reason is that the size of alkyl ammonium cation increases with the increase of carbon chain length, when Na-MT is modified by alkyl ammonium with long carbon chain, the d(001) of Cn-MT1 will evidently increase due to the spatial volume effect. Previous studies also found similar conclusions [11,30,31]. But the d(001) values acquired by us are obviously higher than that obtained by Brito et al. [32], this difference may be mainly caused by different modification method, drying time and layer charge density of Na-MT.
Comparing Figure 2b,c, we can find that the layer charge density of Na-MT can also evidently influence the d(001) values of organo-MT. For the same type of alkyl ammonium, the d(001) value of Cn-MT1 is higher than that of Cn-MT2. The reason is that the lower the layer charge density of Na-MT, the weaker the electrostatic attraction between Na+ and tetrahedral surfaces, during the process of organic modification, a large amount of alkyl ammonium are absorbed into interlayer of domain, Na-MT1 sheets expand easier along the direction of z-axis due to the spatial volume effect of alkyl ammonium, which results in that the d(001) of Cn-MT1 is higher than that of Cn-MT2.

3.2. FTIR Measurement

FTIR of Na-MT and organo-MT prepared under different conditions is shown in Figure 3.
It can be seen from the Figure 3 that the position of most absorption peaks of organo-MT does not change after the organic modifier is inserted into Na-MT interlayer, which indicates that the intercalation of organic modifier does not destroy the crystal structure of Na-MT. The absorption bands at 3621 cm−1 for Cn-MT1 and 3619 cm−1 for Cn-MT2 are assigned to the stretching vibration of H2O on the surfaces of MT and –OH groups within the octahedral sheets [10]. The broad absorption bands at 3449 cm−1 for Cn-MT1 and at 3440 cm−1 for Cn-MT2 are ascribed to the –OH stretching vibration, and the absorption bands at 1638 cm−1 for Cn-MT1 and at 1639 cm−1 for Cn-MT2 are corresponding to –OH bending vibration in H2O. The intensity of these characteristic peaks is lower in organo-MT than that in Na-MT, which indicates that the water content of organo-MT interlayer is lower than that in corresponding Na-MT. The reason is that after the intercalation of alkyl ammonium, Na+ are exchanged by hydrophobic alkyl ammonium cation; as a result, the hydrophility of the prepared organo-MT decreases, which leads to the decrease of the content of H2O between organo-MT sheets [33]. The absorption bands at 2924 cm−1 and 2853 cm−1 can be assigned to the –CH2 asymmetric stretching vibration and –CH2 symmetric stretching vibration, respectively [15,20]. The intensity of these characteristic peaks gradually increases from C12-MT to C18-MT, which also reflects that the hydrophobicity of organo-MT increases with the increase of carbon chain length [30]. The absorption band at about 1478 cm−1 is the –CH2 bending vibration. The strong absorption bands near 1033 cm−1 for Cn-MT1 and 1040 cm−1 for Cn-MT2 belong to the stretching vibration of Si–O groups of tetrahedral sheets. The change of their shape after intercalation of alkyl ammonium implies that there may be an interaction between Si–O surfaces and alkyl ammonium cation [34]. In addition, the absorption bands at 515 cm−1 and 463 cm−1 for Cn-MT1 and 518 cm−1 and 471 cm−1 for Cn-MT2 are attributed to Mg–O–Si and Mg–O bending vibration, respectively. Apparently, when layer charge density increases, these characteristic bands move towards high frequency region. The reason is that the higher the layer charge density, the more the number of Mg2+ in octahedra, and the more obvious the bending vibration of Si–O–Mg and Mg–O in high frequency zone.

3.3. TG Experiment

TG curves of Na-MT and corresponding organo-MT prepared under different conditions are shown in Figure 4. The mass loss of organo-MT at different temperature is shown in Table 5.
The mass loss of organo-MT below 200 °C is due to that H2O absorbed in organo-MT pores and layers are released [35]. In this temperature range, the mass loss of organo-MT is lower than that of Na-MT, which further indicates that there are less H2O within organo-MT interlayer, this phenomenon is consistent with the result of FTIR that the intensity of characteristic peaks at 3449 cm−1 for Cn-MT1 and at 3440 cm−1 for Cn-MT2 is low. It can be explained by that the intercalary or adsorbed alkyl ammonium cation reduce the surface energy of Na-MT and change the hydrophilic surfaces to the hydrophobic [6]. The mass loss of organo-MT between 200–670 °C is related to the thermal decomposition of the physically adsorbed alkyl ammonium and intercalated alkyl ammonium cation [16]. In this temperature range, the mass loss between 200 °C and 440 °C is attributed to the oxidation of alkyl ammonium, and the mass loss between 440 °C and 670 °C indicates that the complete oxidation of carbonaceous is formed by previous thermal decomposition [36]. In addition, The mass loss above 670 °C is ascribed to the dehydroxylation of organo-MT [10].
As shown in Figure 5 and Table 5, we can also find that both the carbon chain length of alkyl ammonium and the layer charge density of Na-MT have an evident influence on the mass loss of organo-MT prepared under different conditions, for example, the mass loss of alkyl ammonium in Cn-MT1 gradually increases from 16.0% to 23.4%, and the mass loss of alkyl ammonium in Cn-MT2 gradually increases from 24.8% to 30.0%. This may be attributed to two factors, on the one hand, SSA of Na-MT2 is higher than that of Na-MT1 (Table 2), which results in that the adsorption capacity of Na-MT2 on alkyl ammonium is higher than that of Na-MT1, on the other hand, layer charge density of Na-MT2 is also higher than that of Na-MT1; thus, more alkyl ammonium are exchanged into Na-MT2 interlayer domain by cation exchange. However, the difference of mass loss between C14-MT2 and C16-MT2 is not apparent, and the reason may be that Na-MT2 layers cannot be fully dispersed in aqueous solution because of the stronger electrostatic attraction between Na-MT2 sheets, and the pore diameter of Na-MT2 particles is smaller than that of Na-MT1; as a result, the larger alkyl ammonium cation (HTA+) do not fully intercalate into the interlayer of Na-MT2.

3.4. Contact Angle Test

In order to further study the influence of layer charge density of Na-MT and carbon chain length of alkyl ammonium on the surface property of organo-MT, we tested the contact angle of different organo-MT, and the results are shown in Figure 5.
From Figure 5, we can see that the contact angle of C12-MT1, C14-MT1, C16-MT1, C18-MT1, C12-MT2, C14-MT2, C16-MT2, and C18-MT2 is 55.31°, 64.79°, 82.80°, 83.26° 64.81°, 75.11°, 85.84°, and 83.86°, respectively. Apparently, the layer charge density of Na-MT and carbon chain length of alkyl ammonium have significant influence on the surface property of organ-MT, the higher the layer charge density, and the bigger the contact angle of organo-MT. The rule is similar to the analysis results of XRD and TG analysis. This can be explained by that both layer charge density and SSA of Na-MT2 are higher than that of Na-MT1, which results in that the adsorption amount of alkyl ammonium on Na-MT2 surfaces and into Na-MT layers is higher than that of Na-MT1; thus, the hydrophobicity of Cn-MT2 is higher than that of Cn-MT1. Moreover, either in Cn-MT1 or Cn-MT2, the contact angle increases with the increase of carbon chain length of alkyl ammonium. The reason is that alkyl ammonium with long carbon chain can cover the organo-MT surfaces better. In addition, it can be seen from Figure 5 that, when the carbon chain length of alkyl ammonium reaches sixteen (HTAC), the contact angle of C16-MT suddenly increases, and it does not change much after that. That is why alkyl ammonium with long carbon chain, such as HTAC and OTAC, are usually selected as organic modifiers in industrial production.

3.5. MD Simulation

In order to further investigate the microstructure characteristics of organo-MT interlayer domain, MD simulation method was used to study the z-axis concentration distribution of C and N elements and the arrangement of modifier within organo-MT sheets. The results are shown in Figure 6 and Figure 7.

3.5.1. Z-Axis Concentration Distribution

It can be seen that the layer charge density of Na-MT and carbon chain length of alkyl ammonium can evidently influence the concentration distribution of C, N, and H2O within organ-MT interlayer. From Figure 6a, we can find that in Cn-MT1, with the increase of carbon chain length, the concentration distribution of C gradually changes from two symmetrical peaks in C12-MT1 into three asymmetrical peaks in C18-MT1, and the corresponding distribution range increases from −6.5–+6.5 Å to −12.5–+12.5 Å along the direction of z-axis. The reason is that alkyl ammonium with long carbon chain can evidently increase the interlayer distance of Na-MT due to the spatial volume effect (Figure 2), and, because of electrostatic attraction, alkyl ammonium cation gradually moves towards tetrahedral sheets of Cn-MT1, which results in that alkyl ammonium is distributed over wider area with the increase of carbon chain length. In Cn-MT2, the concentration distribution of C gradually changes from three peaks in C12-MT2 into four peaks in C18-MT2, and the corresponding distribution zone increases from −4.5–+7.0 Å to −10.0–+7.5 Å.
It can be seen from Figure 6b that the concentration distribution rule of N is similar to that of C, in Cn-MT1, the N element exhibits evident double layers distribution in C12-MT1, and gradually forms three layers asymmetrical distribution with the increase of carbon chain length, which indicates that some of alkyl ammonium tend to arrange obliquely within Cn-MT1 interlayer when the carbon chain length of modifier increases. But when the layer charge density of Na-MT is high, the N element mainly shows three layers distribution in C12-MT2 and changes into uneven four layers distribution in C18-MT2. The distribution range of N increases from −5.2–+5.2 Å to −12.4–+12.4 Å for Cn-MT1, and from −3.8–+5.2 Å to −7.5–+6.2 Å for Cn-MT2. Thus, we can conclude that the concentration distribution of C and N in Cn-MT2 is closer to tetrahedral surfaces than that in Cn-MT1. The reason is that the layer charge density of Na-MT2 is higher, so the polar force between Cn-MT2 layers is stronger, which results in that alkyl ammonium cation between Cn-MT2 sheets arrange more compact than that in Cn-MT1. This simulation results can explain the XRD results well (Figure 2).
In addition, it can be seen from Figure 6c that, in Cn-MT1, the concentration distribution of H2O exhibits four peaks in C12-MT1, but their intensity decreases with the increase of carbon chain length, and the distribution range of H2O increases from −7.5–+7.5 Å to −13.0–+13.0 Å along the direction of z-axis, which indicates that H2O gradually distribute evenly in interlayer of Cn-MT1. When the layer charge density of Na-MT is high, H2O gradually shows an obvious four layers of distribution as the carbon chain length of modifier increases, and the corresponding distribution range increases from −6.0–+7.5 Å to −10.2–+10.0 Å. The reason is that the concentration distribution of H2O is influenced by alkyl ammonium and MT sheets, so when the carbon chain length of modifier increases, some of alkyl ammonium tends to move towards tetrahedral surfaces of Cn-MT2, which results in that part of H2O being squeezed and eventually forming an arrangement of four layers.

3.5.2. Arrangement of Alkyl Ammonium Cation within Organo-MT Interlayer

The snapshots of alkyl ammonium within organo-MT layers are shown in Figure 7, and according the z-axis concentration of C, N, and H2O within organo-MT interlayer, it can be inferred that, in C12-MT1, alkyl ammonium tend to form double layers distribution, and, with the increase of carbon chain length, some of alkyl ammonium are still parallel distributed to Cn-MT1 sheets, but others are obliquely distributed within the Cn-MT1 sheets, which results in that the concentration of C and N exhibits three asymmetrical peaks (Figure 6). When the layer charge density is high, with the increase of carbon chain length, the distribution of alkyl ammonium gradually changes from three layers into an arrangement of four layers within Cn-MT2 sheets.

3.6. Gel Apparent Viscosity of Organo-MT

In order to further study the effect of layer charge density of Na-MT and carbon chain length of alkyl ammonium on the application performance of organo-MT, we tested the gel apparent viscosity of different organo-MT in xylene/ethyl alcohol system, and the results are shown in Table 6.
It can be seen that both layer charge density of Na-MT and carbon chain length of alkyl ammonium can evidently influence the gel apparent viscosity of organo-MT. The gel apparent viscosity of Cn-MT1 is overall higher than that of Cn-MT2. The reason is that, when the layer charge density of Na-MT is low, the electrostatic attraction between Na-MT sheets is weak; in an xylene/ethyl alcohol system, xylene is adsorbed into Cn-MT1 interlayer domain due to van der Waals interaction force, and, because of the spatial volume effect, large amounts of Cn-MT1 sheets are gradually separated, and, as is known to us, the end face of Na-MT sheets are positively charged, and the interlayer planes are negatively charged, so the stripped Cn-MT1 sheets can form house-of-cards structure easily, which leads to the result that the gel apparent viscosity of Cn-MT1 is higher. But, in Cn-MT2, although large amounts of alkyl ammonium and xylene are adsorbed into the interlayer domain, it is difficult to strip Cn-MT2 sheets and form house-of-cards due to its strong electrostatic attraction, which results in the gel apparent viscosity of Cn-MT2 being lower than that of Cn-MT1.
In addition, from Table 6, we can also find that the gel apparent viscosity of organo-MT in xylene/ethyl alcohol system increases with the increase of carbon chain length. This phenomenon is more obvious when the layer charge density is low (Cn-MT1) and is also consistent with the contact angle test result. The reason is that when the alkyl ammonium with long carbon chain enters into Na-MT1 interlayer by cation exchange, and, because of the spatial volume effect, Cn-MT1 sheets gradually expand along the direction of z-axis (this phenomenon can also be seen in Figure 2 and Figure 7), and the electrostatic attraction between Cn-MT1 layers decreases as the distance between the layers increases; therefore, in the xylene/ethyl alcohol system, when large amounts of xylene are adsorbed into Cn-MT1 interlayer, Cn-MT1 sheets are more easily separated and form a house-of-cards. As a result, the gel apparent viscosity of Cn-MT1 prepared by alkyl ammonium with long carbon chain is higher.

4. Conclusions

In the work, the effect of layer charge density of Na-MT and carbon chain length of alkyl ammonium on the structure and gel property of organo-MT was systematically studied by using many characterization techniques. The result shows that the interlayer distance of organo-MT increases with the increase of carbon chain length, and when the layer charge density is low, this phenomenon is more obvious. The characteristic absorption bands at 2924 cm−1 and 2853 cm−1 appear in FTIR decrease with the increase of carbon chain length, and, when the layer charge density increases, the characteristic peaks at 515 cm−1 and 463 cm−1 shift towards high frequency region. The mass loss of organo-MT with high layer charge density is larger than that of organo-MT with low layer charge density, and, when carbon chain length of modifier increases, the mass loss of organo-MT also increases. In addition, the contact angle of Cn-MT2 is higher than that of Cn-MT1 when the carbon chain length of modifier is the same, and alkyl ammonium with long carbon chain can significantly improve the hydrophobicity of Na-MT. MD simulation results show that the concentration distribution of C and N in Cn-MT2 is closer to tetrahedral surfaces than that in Cn-MT1. In Cn-MT1, alkyl ammonium cation forms obvious double layers when the carbon chain length of modifier is short, and, with the increase of carbon chain length, some of alkyl ammonium tend to be tilt with Cn-MT1 surfaces. In Cn-MT2, the arrangement of alkyl ammonium gradually changes from three layers into four layers with the increase of carbon chain length. The gel apparent viscosity of organo-MT in xylene/ethanol system increases with the increase of the layer charge density of Na-MT or the carbon chain length of alkyl ammonium.

Author Contributions

Conceptualization, J.Q.; methodology, D.L.; software, D.L. and Y.W. (Yueting Wang); validation, S.J., G.C., G.W. and X.L. (Xianjun Lyu); formal analysis, G.L., Y.W. (Yaqi Wang) and W.W.; investigation, D.L., Y.W. (Yueting Wang) and P.W.; Resources, X.L. (Xianjun Lyu); data curation, D.L., S.J. and X.L. (Xiaodong Liu); Writing—original draft preparation, D.L.; Writing—review & editing, J.Q., Y.W. (Yueting Wang) and G.C; visualization, J.Q.; supervision, G.W.; project administration, X.L. (Xianjun Lyu); funding acquisition, J.Q. and G.W. All authors have read and agreed to the published version of the manuscript.

Funding

This work was supported by the National Nature Science Foundation of China—“Design of structure and gelling performance of Montmorillonite/Alkylammonium based on the adsorption properties of Alkylammonium on Montmorillonite (No: 51774200)” and “Study on the immobilization effect and mechanism of heavy metal in sulfide-mine tailings by chelating agent modified bentonite (No: 51764003)”.

Conflicts of Interest

The authors declare no conflict of interest.

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Minerals 10 00378 g001 550
Figure 1. The structure of alkyl ammonium, (a) dodecyl trimethyl ammonium chloride (DTAC), (b) tetradecyl trimethyl ammonium chloride (TTAC), (c) hexadecyl trimethyl ammonium chloride (HTAC), (d) octadecyl trimethyl ammonium chloride (OTAC).
Figure 1. The structure of alkyl ammonium, (a) dodecyl trimethyl ammonium chloride (DTAC), (b) tetradecyl trimethyl ammonium chloride (TTAC), (c) hexadecyl trimethyl ammonium chloride (HTAC), (d) octadecyl trimethyl ammonium chloride (OTAC).
Minerals 10 00378 g001
Minerals 10 00378 g002a 550Minerals 10 00378 g002b 550
Figure 2. XRD patterns of MT, (a) Ca(Na)-MT, (b) Cn-MT1, (c) Cn-MT2.
Figure 2. XRD patterns of MT, (a) Ca(Na)-MT, (b) Cn-MT1, (c) Cn-MT2.
Minerals 10 00378 g002aMinerals 10 00378 g002b
Minerals 10 00378 g003 550
Figure 3. FTIR of Na-MT and prepared organo-MT, (a) MT1; (b) MT2.
Figure 3. FTIR of Na-MT and prepared organo-MT, (a) MT1; (b) MT2.
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Minerals 10 00378 g004 550
Figure 4. Thermogravimetric (TG) curves of Na-MT and prepared organo-MT, (a) MT1; (b) MT2.
Figure 4. Thermogravimetric (TG) curves of Na-MT and prepared organo-MT, (a) MT1; (b) MT2.
Minerals 10 00378 g004
Minerals 10 00378 g005 550
Figure 5. Contact angle of organo-MT.
Figure 5. Contact angle of organo-MT.
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Minerals 10 00378 g006 550
Figure 6. The z-axis concentration curves of C, N, and H2O within organo-MT sheets. (a) C, (b) N, and (c) H2O.
Figure 6. The z-axis concentration curves of C, N, and H2O within organo-MT sheets. (a) C, (b) N, and (c) H2O.
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Minerals 10 00378 g007 550
Figure 7. The snapshot of alkyl ammonium cation in organo-MT layers. (a) C12-MT1; (b) C14-MT1; (c) C16-MT1; (d) C18-MT1; (e) C12-MT2; (f) C14-MT2; (g) C16-MT2; (h) C18-MT2.
Figure 7. The snapshot of alkyl ammonium cation in organo-MT layers. (a) C12-MT1; (b) C14-MT1; (c) C16-MT1; (d) C18-MT1; (e) C12-MT2; (f) C14-MT2; (g) C16-MT2; (h) C18-MT2.
Minerals 10 00378 g007
Table
Table 1. Chemical composition of two kinds of Ca-MT (wt %). MT = montmorillonite.
Table 1. Chemical composition of two kinds of Ca-MT (wt %). MT = montmorillonite.
TypeSiO2Al2O3MgONa2OFe2O3K2OCaOTiO2
Ca-MT168.6516.044.151.992.982.863.330
Ca-MT266.8318.796.440.342.800.413.980.41
Table
Table 2. Specific surface area (SSA), pore structure, and cation exchange capacity (CEC) of two kinds of Na-MT.
Table 2. Specific surface area (SSA), pore structure, and cation exchange capacity (CEC) of two kinds of Na-MT.
TypesSSA (m2/g)PV (cm3/g)APD (nm)CEC (mmol/100g)
Na-MT132.69450.05757.037090.69
Na-MT244.95580.06325.6280108.23
Table
Table 3. The number of alkyl ammonium cation and H2O added in the interlayer domain of organo-MT.
Table 3. The number of alkyl ammonium cation and H2O added in the interlayer domain of organo-MT.
TypeC12-MT1C14-MT1C16-MT1C18-MT1
H2O110140170219
alkyl ammonium cation6666
TypeC12-MT2C14-MT2C16-MT2C18-MT2
H2O30405070
alkyl ammonium cation11111111
Table
Table 4. The geometry optimization results of organo-MT models.
Table 4. The geometry optimization results of organo-MT models.
TypeC12-MT1C14-MT1C16-MT1C18-MT1
Volume/Å37391.348455.928784.6313224.80
c/Å22.660625.774629.213235.5689
β/°97.891999.8504103.7590101.2330
TypeC12-MT2C14-MT2C16-MT2C18-MT2
Volume/Å37153.537036.727849.238609.17
c/Å21.381922.818624.065528.6229
β/°98.8988104.47199.0000107.4760
Table
Table 5. The mass loss of organo-MT at different temperature range (wt %).
Table 5. The mass loss of organo-MT at different temperature range (wt %).
T (°C)C12-MT1C14-MT1C16-MT1C18-MT1
0–2002.43.33.33.3
200–67016.018.319.523.4
T (°C)C12-MT2C14-MT2C16-MT2C18-MT2
0–2004.15.26.45.2
200–67024.826.526.630.0
Table
Table 6. Gel apparent viscosity of organo-MT (Pa·s).
Table 6. Gel apparent viscosity of organo-MT (Pa·s).
TypeC12-MT1C14-MT1C16-MT1C18-MT1
Gel apparent viscosity1.872.283.7113.31
TypeC12-MT2C14-MT2C16-MT2C18-MT2
Gel apparent viscosity1.201.921.603.49

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MDPI and ACS Style

Qiu, J.; Liu, D.; Wang, Y.; Chen, G.; Jiang, S.; Li, G.; Wang, Y.; Wang, W.; Wu, P.; Liu, X.; et al. Comprehensive Characterization of the Structure and Gel Property of Organo-Montmorillonite: Effect of Layer Charge Density of Montmorillonite and Carbon Chain Length of Alkyl Ammonium. Minerals 2020, 10, 378. https://doi.org/10.3390/min10040378

AMA Style

Qiu J, Liu D, Wang Y, Chen G, Jiang S, Li G, Wang Y, Wang W, Wu P, Liu X, et al. Comprehensive Characterization of the Structure and Gel Property of Organo-Montmorillonite: Effect of Layer Charge Density of Montmorillonite and Carbon Chain Length of Alkyl Ammonium. Minerals. 2020; 10(4):378. https://doi.org/10.3390/min10040378

Chicago/Turabian Style

Qiu, Jun, Dongliang Liu, Yueting Wang, Guowei Chen, Shan Jiang, Guoqing Li, Yaqi Wang, Wenxin Wang, Peng Wu, Xiaodong Liu, and et al. 2020. "Comprehensive Characterization of the Structure and Gel Property of Organo-Montmorillonite: Effect of Layer Charge Density of Montmorillonite and Carbon Chain Length of Alkyl Ammonium" Minerals 10, no. 4: 378. https://doi.org/10.3390/min10040378

APA Style

Qiu, J., Liu, D., Wang, Y., Chen, G., Jiang, S., Li, G., Wang, Y., Wang, W., Wu, P., Liu, X., Wang, G., & Lyu, X. (2020). Comprehensive Characterization of the Structure and Gel Property of Organo-Montmorillonite: Effect of Layer Charge Density of Montmorillonite and Carbon Chain Length of Alkyl Ammonium. Minerals, 10(4), 378. https://doi.org/10.3390/min10040378

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