# Stability of Fluorosurfactant Adsorption on Mineral Surface for Water Removal in Tight Gas Reservoirs

Authors: Lijun You; Wanchun Zhang; Yili Kang; Zhangxin Chen; Xuefen Liu
Journal: Journal of Chemistry
 (2015)

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## Abstract

Long-term effectiveness of rock wettability alteration for water removal during gas production from tight reservoir depends on the surfactant adsorption on the pore surface of a reservoir. This paper selected typical cationic fluorosurfactant FW-134 as an example and took advantage of Fourier transform infrared spectroscopy (FTIR), X-ray photoelectron spectroscopy (XPS), and atomic force microscope (AFM) to investigate its adsorption stability on the rock mineral surface under the oscillation condition at high temperature for a long time. The experimental results indicate that the F element content on the sample surface increases obviously, the surface structure of fluorine-carbonization also undergoes a significant change, and the fluorine surfactant exhibits a good interfacial modification and wettability alteration ability due to its adsorption on the pore surface transforming the chemical structure of the original surface. The adsorption increases indistinctly with the concentration of over 0.05% due to a single layer adsorption structure and is mainly electrostatic adsorption because the chemical bonding between the fluorosurfactant and the rock mineral surface, the hydrogen bonding, is weak and inconspicuous.


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## Body

## 1. Introduction

Tight gas reservoirs, one of main development objectives in the future dozens of years, are characterized by a high water phase trapping damage potential owing to the characteristic of water-wet and high capillary pressure. The water phase trapping damage can induce a fluid sensitivity damage, an aggravate stress sensitivity damage, and other damage [1], seriously affects an economic development of the tight gas reservoirs [2–4], and is difficult to be removed due to high capillary pressure of tight sandstone.Surfactant interface modification is increasingly attracting more attention of reservoir engineers because it can reduce interface intension and alter wettability of rocks. Compared with ordinary hydrocarbon surfactant, fluorosurfactant possesses the outstanding characteristic of a high surface activity, high thermal stability, and high chemical stability [5], and its fluorine hydrocarbon exhibits a hydrophobic and oleophobic property. Owing to these properties, it has a very wide range of applications in the chemical, biological, mechanical, textile, papermaking, and oil industries. In the oil and gas industry, fluorine surfactant can be used as an oil-displacing agent, a wettability alternation agent, and a cleanup additive by improving the ability of fluid flow in porous media. Li and Firoozabadi [6] put forward the term “gas-wetness.” Their motive was to change rock wettability from water or oil wetness to gas-wetness for reduction or removal of liquid blocking or phase trapping damage. Since then, many papers presented research results about improving gas production by wettability alteration [7–15] and tested different surfactants at different reservoir temperatures. Li’s group [6–8, 10, 13] conducted experiments to change the wettability of tight sandstone with permeability of less than 0.1 mD and they also reported a pilot field test in a tight gas-condensate reservoir to improve the gas production by wettability alteration. The production of the test well was increased to about 30,000 m3/day, but the gas production declined very fast and it was only about 4,000 m3/day after four days [16]. However, there have been few reports about the reason that the period of validity of improving gas production by wettability alteration was so short. Fluorine surfactant can modify the interface of a gas-water-rock system by adsorption on mineral surface to alter the wettability and surfactant adsorption behavior on the mineral surface and influences the long-term effect of wettability alteration. A key to maintaining the long-term effectiveness of wettability alteration is understanding the interaction of chemicals and rock [17, 18]. Seiedi et al. [19] presented AFM images for quantitative assessment of the surface roughness for a wettability alteration investigation. Wu and Firoozabadi [17, 18] analyzed the long-term effectiveness of wettability alteration using core laboratory experiments.In this study, we select a kind of fluorine surfactant FW-134 which is able to successfully change water-wet tight sandstone into gas-wetness and improve the water flow rate by modifying the interface [12], and we select the mica to represent the main rock-forming minerals of tight sandstone. The purpose is to investigate the adsorption behavior and the ability of interface modification on the surface of rock mineral from microaspect under the conditions of simulated long-term water flow back from a high temperature gas reservoir.


## 2. Materials and Methods

### 2.1. Materials

Only a small part of clay minerals and carbonate cementation play an important role in surfactant adsorption, and their main components are layered silicate minerals, containing oxygen, silicon, aluminum, calcium, sodium, and potassium. Mica is easily split into pieces to obtain a smooth atomic hydrophilic surface [20], whose naked aluminum silicate lattice surface is similar to silica and many clay surfaces. In reality, we selected several rock-forming minerals like mica, kaolinite, and silica to conduct the adsorption, but this paper just selects fresh natural cleaved mica as a substrate to investigate fluorine surfactant adsorption on the high temperature solid-liquid interface. Fluorinated surfactant FW-134 used is a kind of typical cationic fluorinated surfactant C8F17 SO2NH(CH2)3(CH3)3NI containing a small amount of N, S, and O elements and its critical micelle concentration is 0.10%. The surfactant is 99.9% pure. Distilled water is used to simulate the retention liquid like condensate water in the reservoir in order to avoid the effect of water salinity on the interaction of surfactants and rock mineral.


### 2.2. Methods

Experimental procedures are as follows.(1)
Wash with distilled water to remove impurities from the mica surface and put them into a constant temperature oven to dry to a constant weight at 60°C.
(2)
Crush the mica into powder, sieve the powder with 100~200 meshes, and dry it to a constant weight at 60°C.
(3)
Make up 0.05% and 0.10% FW-134 solution with distilled water and FW-134 according to a 1 : 50 ratio of solid to liquid into the conical flask, respectively [21]. The 1 : 50 ratio of solid to liquid is from the results of a series of adsorption experiments of different solid-liquid ratio to avoid the effect of the solid-liquid ratio on the surfactant adsorption.
(4)
Shake up the mixtures, cover tightly the conical flasks with a plug, and immerse the flasks into the water bath oscillator to oscillate at 90°C for 40 hours. The purpose of oscillation is to simulate the reservoir detention water flow scouring to the pore surface during gas production. In order to ensure that the FW-134 reaches saturation adsorption on solid surfaces, we test the adsorptive capacity Γ changing with time on the mica surface. We can see from the results (Figure1) that the adsorption equilibrium time is not more than 2 hours. We conduct the adsorption experiments for 40 hours, which is much more than the adsorption equilibrium time.
(5)
Take out the conical flasks and leave them to rest for 30 minutes.
(6)
Filter the precipitation separation of solid particles and soak up the residual solution on the solid particle surface with a filter paper.
(7)
Dry solid particles to a constant weight at 60°C, number them sample A (distilled water), sample B (0.05% FW-134), and sample C (0.10% FW-134) according to the concentration of FW-134 from low to high, and seal them for WQF-520 Fourier infrared (FTIR) spectrometer and Thermo Scientific Escalab 250 X-ray photoelectron spectroscopy (XPS) tests.
(8)
Select fresh natural dissociated mica (1 cm × 1 cm, thickness < 2 mm) and immerse them into 0.1% FW-134 solution according to a 1 : 50 ratio of solid to liquid at 90°C constant temperature water bath.
(9)
Take out the mica plate after the oscillation for 40 hours, dry the surface with nitrogen flow to obtain the mica surface after the adsorption of FW-134, and fix the sample on a sample table of MMAFMLN 1728EX atomic force microscope (AFM) to test surface morphology. Nitrogen flow drying is to simulate gas flow scouring to the pore surface in the reservoir during gas production.
(10)
Measure the surface contact angle.Figure 1
FW-134 adsorption capability on mica versus time.


## 2.1. Materials

Only a small part of clay minerals and carbonate cementation play an important role in surfactant adsorption, and their main components are layered silicate minerals, containing oxygen, silicon, aluminum, calcium, sodium, and potassium. Mica is easily split into pieces to obtain a smooth atomic hydrophilic surface [20], whose naked aluminum silicate lattice surface is similar to silica and many clay surfaces. In reality, we selected several rock-forming minerals like mica, kaolinite, and silica to conduct the adsorption, but this paper just selects fresh natural cleaved mica as a substrate to investigate fluorine surfactant adsorption on the high temperature solid-liquid interface. Fluorinated surfactant FW-134 used is a kind of typical cationic fluorinated surfactant C8F17 SO2NH(CH2)3(CH3)3NI containing a small amount of N, S, and O elements and its critical micelle concentration is 0.10%. The surfactant is 99.9% pure. Distilled water is used to simulate the retention liquid like condensate water in the reservoir in order to avoid the effect of water salinity on the interaction of surfactants and rock mineral.


## 2.2. Methods

Experimental procedures are as follows.(1)
Wash with distilled water to remove impurities from the mica surface and put them into a constant temperature oven to dry to a constant weight at 60°C.
(2)
Crush the mica into powder, sieve the powder with 100~200 meshes, and dry it to a constant weight at 60°C.
(3)
Make up 0.05% and 0.10% FW-134 solution with distilled water and FW-134 according to a 1 : 50 ratio of solid to liquid into the conical flask, respectively [21]. The 1 : 50 ratio of solid to liquid is from the results of a series of adsorption experiments of different solid-liquid ratio to avoid the effect of the solid-liquid ratio on the surfactant adsorption.
(4)
Shake up the mixtures, cover tightly the conical flasks with a plug, and immerse the flasks into the water bath oscillator to oscillate at 90°C for 40 hours. The purpose of oscillation is to simulate the reservoir detention water flow scouring to the pore surface during gas production. In order to ensure that the FW-134 reaches saturation adsorption on solid surfaces, we test the adsorptive capacity Γ changing with time on the mica surface. We can see from the results (Figure1) that the adsorption equilibrium time is not more than 2 hours. We conduct the adsorption experiments for 40 hours, which is much more than the adsorption equilibrium time.
(5)
Take out the conical flasks and leave them to rest for 30 minutes.
(6)
Filter the precipitation separation of solid particles and soak up the residual solution on the solid particle surface with a filter paper.
(7)
Dry solid particles to a constant weight at 60°C, number them sample A (distilled water), sample B (0.05% FW-134), and sample C (0.10% FW-134) according to the concentration of FW-134 from low to high, and seal them for WQF-520 Fourier infrared (FTIR) spectrometer and Thermo Scientific Escalab 250 X-ray photoelectron spectroscopy (XPS) tests.
(8)
Select fresh natural dissociated mica (1 cm × 1 cm, thickness < 2 mm) and immerse them into 0.1% FW-134 solution according to a 1 : 50 ratio of solid to liquid at 90°C constant temperature water bath.
(9)
Take out the mica plate after the oscillation for 40 hours, dry the surface with nitrogen flow to obtain the mica surface after the adsorption of FW-134, and fix the sample on a sample table of MMAFMLN 1728EX atomic force microscope (AFM) to test surface morphology. Nitrogen flow drying is to simulate gas flow scouring to the pore surface in the reservoir during gas production.
(10)
Measure the surface contact angle.Figure 1
FW-134 adsorption capability on mica versus time.


## 3. Experimental Results

### 3.1. Characterization of Adsorption Behavior

Sample A, sample B, and sample C were analyzed by FTIR. These samples were obtained from mica powder immersed into distilled water, 0.05% and 0.10% FW-134 solution under 90°C for 40 hours’ oscillation, as mentioned above. The FTIR results can be seen in Figure1.The peak at 3,625 cm−1 is the O-H stretching vibration absorption peak of mica Al-OH and Mg-OH, 3,442 cm−1 the O-H stretching vibration absorption peak of mica surface adsorbing water, and 630~1,640 cm−1 the O-H bending vibration absorption peak; a high intensity peak at 1,024 cm−1 is the Si-O absorption peak of stretching vibration, the absorption peak at 950~600 cm−1 is O-H bending vibration, and a vibration zone at 800~500 cm−1 belongs to Si-O-Al spectral absorption peak. Using a comparative analysis of the FTIR diagram, methyl CH3 and methylene CH2 stretching vibration absorption peaks appeared obvious at 3,000~2,800 cm−1 in sample B and sample C, and the absorption peak of stretching vibration of fluoroalkyl groups CF3 and CF2 also appeared at 1,350~1,120 cm−1. These indicate that FW-134 produces a significant adsorption on mica surfaces under the conditions of high temperature and long-term oscillations, but there is basically no obvious change of displacement, strength, or shape of the absorption peak from the whole FTIR graph characteristics before and after adsorption, suggesting that the chemical bond between FW-134 and the mica surface is weak and the adsorption is mainly physical adsorption. The peaks 1800~1200 cm−1 in sample A and sample B are the same, which hardly appear in sample C. This shows that this peak is not related to the surfactant adsorption and will not affect the experiment results.A mica surface has a strong capacity of bonding hydroxyl groups, polar atoms like F, N, and O are easy to form a hydrogen bond with the surface hydroxyl groups, and mica surfaces in aqueous solution are negatively charged, so FW-134, a kind of cationic fluorinated surfactant, is easy to be adsorbed on mica surfaces due to the electrostatic force, dispersion force, hydrogen bond, and other physical and chemical effects. However, it can be seen in Figure2 that O-H stretching vibration absorption displacement, strength, and shape of surface water on the samples with different concentration of FW-134 are the same, and the peak is at 3,442 cm−1, which shows that the bonding force between FW-134 molecules and the mica surface hydroxyl bond is weak. This may be due to the fact that hydrogen bonds are destroyed at high temperature, or the hydrogen bonding adsorption effect is weak, and it is not reflected in the FTIR diagram. These suggest that the main mechanism of FW-134 adsorption under the condition of high temperature is not a hydrogen bond.Figure 2
FT-IR spectra of samples adsorbing FW-134.


### 3.2. Energy Spectrum Analysis of Surface Structure

We take an advantage of XPS to test the energy spectrum of sample A, sample B, and sample C, and the results are seen in Figure3. The XPS spectra curve analysis and fitting were conducted using the software XPS Peaks 4.1 developed by University of Hong Kong. We analyze the binding energy of Al2p, Si2p, C1s, K2p, O1s, F1s, N1s, and S2p of different samples. As shown in Figure 3, the binding energy of Al2p, Si2p, K2p, and O1s and the curve shape do not change with the concentration of FW-134; the binding energy of F1s, N1s, and S2p of sample B and sample C increases significantly compared with that of sample A and appears at 689 eV, 402 eV, and 169 eV, respectively.Figure 3
XPS spectra of sample systems adsorbing FW-134.The content and the binding energy of each element are calculated according to the peak area (Tables1 and 2).Table 1
XPS element content data of sample systems adsorbing FW-134.
Content (%)
Al2p
Si2p
C1s
K2p
O1s
F1s
N1s
S2p
Sample A
13.245
17.383
11.470
4.950
51.768
0.598
0.577
0.502
Sample B
10.269
13.458
7.588
4.689
43.194
17.545
2.092
1.166
Sample C
9.3410
11.949
10.377
4.327
37.953
22.037
2.616
1.400Table 2
XPSE
B data of sample systems adsorbing FW-134.
Binding energy (eV)
Al2p
Si2p
C1s
K2p
O1s
F1s
N1s
S2p
Sample A
74.26
102.42
284.76
293.1
531.58
685.07
401.92
169.16
Sample B
74.62
102.80
286.55
292.97
531.66
689.19
402.77
169.23
Sample C
74.50
102.65
286.31
292.67
531.69
689.06
402.79
169.02Sample A, with no FW-134 adsorption on the mica, only contains trace F, N, and S element, while the F, N, and S element contents in sample B and sample C with the adsorption of FW-134 increase significantly, and the content of the F element increases from 0.598% to 17.545% and 22.037%, the content of N element from 0.577% to 2.092% and 2.616%, and the S content from 0.502% to 1.166% and 1.400% (Table1), respectively. These showed that a large amount of FW-134 is adsorbed on the mica surface under the conditions of 40 hours’ oscillations at 90°C.The element binding energy (B.E.) in these samples can be seen in Table2. The binding energy of Al2p, Si2p, K2p, and O1s in samples B and C has little difference with that of sample A (Table 2), which shows that, under the conditions of high temperature, the chemical bonding force between FW-134 and the mica surface is weak. This is also consistent with the result from the infrared spectrum analysis. In order to further determine the FW-134 adsorption pattern on the mica surface, F1s XPS peaks of each sample were analyzed by Gauss fitting spectra, as shown in Figure 4.Figure 4
XPS C1s spectra of sample systems adsorbing FW-134 and contrast diagram.
(a)
(b)
(c)
(d)The F1s peaks of all samples are a single peak (Figure4), so the chemical structure of their F element is relatively single. The pulse signal of the F1s peak of sample A is strong, and the peak intensity and peak area are small, which show that there is less F content in sample A (Figures 4(a) and 4(d)). The curves of samples B and C in Figures 4(b) and 4(c) are smooth and orderly, and the intensity and peak area of the F1s peak are large, which suggests that a lot of the F element is in the surface structure of samples B and C and a great deal of FW-134 adsorption is on the mica surface.The F1s peak positions of samples B and C are different from those of sample A, and the F1s peak binding energy of sample B and sample C is basically the same (Figure4(d) and Table 2). That is, the F1s peak position and chemical structure of F atom before and after adsorption on the surface are different. The F1s peak binding energy of sample A is 685.2 eV, the Ca-F structure of mica; the F1s peak binding energies of sample B and sample C are about 689.1 eV, the structure of chain C-F; there are no hydrogen bonding peaks in sample B and sample C. These indicate that the chemical bonding strength between FW-134 and the mica surface is weak under the condition of high temperature, that covering is the main mechanism of different concentration of FW-134 adsorption on the surface of mica, and that physical adsorption rather than hydrogen bonding is the main mechanism of FW-134 adsorption under the condition of the 40 hours’ water oscillation.The Gauss fitting spectra of the C1s XPS peaks of samples are shown in Figure5. As shown in Figure 5(a), the C1s peak of sample A was split into four peaks; peak 1 and peak 2 are classified as a type of peak; the binding energies from low to high are for C-H

∖

C-C, C-O, and C=O peaks. As shown in Figures 5(b) and 5(c), the C1s peaks of sample B and sample C were divided into three peaks, respectively. Their binding energies from low to high are for C-H

∖

C-C, C-N

∖

C-C, and C-F peaks.Figure 5
XPS C1s spectra of samples adsorbing FW-134 and contrast diagram.
(a)
(b)
(c)
(d)The analysis results of the peak binding energy and peak area are shown in Table3. The C-H

∖

C-C peak area of sample A reaches 88.80%, and a small piece of the C-O and C=O peak area appears in the C1s peak (Table 3). This may be caused by the chemical structure of carbon on the sample original surface or adsorption of CO2 in the air on the surface. Compared with sample A, sample B and sample C have a large area of the C-F and C-N

∖

C-C peaks, whose total peak area is, respectively, 85.88% and 81.63%, while the peak area of C-H

∖

C-C is greatly reduced. The reason is that a large amount of FW-134 adsorbed covers on the mica surface to change the chemical structure of the original surface carbon under the high temperature water oscillation.Table 3
XPS results of samples adsorbing FW-134 calculated by Gauss method.
Sample
Type of structure
Binding energy (eV)
Peak area (%)
A
C-H C-C
285.0
88.80
C-O
286.5
5.70
C=O
288.8
5.50
B
C-H C-C
285.0
14.22
C-N C-C
285.7
46.07
C-F
286.8
39.81
C
C-H C-C
285.0
18.37
C-N C-C
285.7
38.90
C-F
286.8
42.73


### 3.3. Evaluation of Surface Conformation and Modification Effect

The water adsorption on modified surface of minerals depends on the surface structure [22]. In order to observe the morphology to further understand the FW-134 adsorption structure and interfacial modification effect on the mica surface, a mica surface treated by a 40 hours’ oscillation with 0.1% FW-134 solution and nitrogen flow drying under high temperature was tested by atomic force microscope (AFM). Figures 6 and 7 are the AFM scanning plane height map and three-dimensional map of the treated mica surface before and after cleaning of distilled water.Figure 6
AFM plane height map and the three-dimensional topography (before cleaning).Figure 7
AFM plane height map and the three-dimensional topography (after cleaning).As intuitively seen in Figure6, a lot of FW-134 molecules adsorbed on the mica surface are unequal granular and massive distribution phenomenon; the adsorption of FW-134 covers up to 80% of the testing scope with 10 μm × 10 μm; the adsorption layer is thin. The contact angles of water on the adsorption surface treated by 0.05%, 0.1%, and 0.2% are 71.9°, 101.2°, and 92.3°, respectively, which mean a good hydrophobic performance and interfacial modification ability of FW-134. After the mica surface is being cleaned with distilled water for 48 hours, there is still a lot of surfactant FW-134 adsorption on the mica surface (Figure 7). We conducted comparative experiments to verify whether the AFM data are reproducible. The adsorption area differences of FW-134 in 10 μm × 10 μm on mica surface in comparative experiments are less than ±6%, which verified that AFM data reproducibility was good. As seen in Figure 7, compared with Figure 6, a part of FW-134 molecules adsorbed on the mica surface are cleared away and the adsorption thickness is reduced, but the adsorbed layer still shows a uniform distribution, which indicts that 0.1% FW-134 has reached a saturated adsorption state on the surface of mica.


## 3.1. Characterization of Adsorption Behavior

Sample A, sample B, and sample C were analyzed by FTIR. These samples were obtained from mica powder immersed into distilled water, 0.05% and 0.10% FW-134 solution under 90°C for 40 hours’ oscillation, as mentioned above. The FTIR results can be seen in Figure1.The peak at 3,625 cm−1 is the O-H stretching vibration absorption peak of mica Al-OH and Mg-OH, 3,442 cm−1 the O-H stretching vibration absorption peak of mica surface adsorbing water, and 630~1,640 cm−1 the O-H bending vibration absorption peak; a high intensity peak at 1,024 cm−1 is the Si-O absorption peak of stretching vibration, the absorption peak at 950~600 cm−1 is O-H bending vibration, and a vibration zone at 800~500 cm−1 belongs to Si-O-Al spectral absorption peak. Using a comparative analysis of the FTIR diagram, methyl CH3 and methylene CH2 stretching vibration absorption peaks appeared obvious at 3,000~2,800 cm−1 in sample B and sample C, and the absorption peak of stretching vibration of fluoroalkyl groups CF3 and CF2 also appeared at 1,350~1,120 cm−1. These indicate that FW-134 produces a significant adsorption on mica surfaces under the conditions of high temperature and long-term oscillations, but there is basically no obvious change of displacement, strength, or shape of the absorption peak from the whole FTIR graph characteristics before and after adsorption, suggesting that the chemical bond between FW-134 and the mica surface is weak and the adsorption is mainly physical adsorption. The peaks 1800~1200 cm−1 in sample A and sample B are the same, which hardly appear in sample C. This shows that this peak is not related to the surfactant adsorption and will not affect the experiment results.A mica surface has a strong capacity of bonding hydroxyl groups, polar atoms like F, N, and O are easy to form a hydrogen bond with the surface hydroxyl groups, and mica surfaces in aqueous solution are negatively charged, so FW-134, a kind of cationic fluorinated surfactant, is easy to be adsorbed on mica surfaces due to the electrostatic force, dispersion force, hydrogen bond, and other physical and chemical effects. However, it can be seen in Figure2 that O-H stretching vibration absorption displacement, strength, and shape of surface water on the samples with different concentration of FW-134 are the same, and the peak is at 3,442 cm−1, which shows that the bonding force between FW-134 molecules and the mica surface hydroxyl bond is weak. This may be due to the fact that hydrogen bonds are destroyed at high temperature, or the hydrogen bonding adsorption effect is weak, and it is not reflected in the FTIR diagram. These suggest that the main mechanism of FW-134 adsorption under the condition of high temperature is not a hydrogen bond.Figure 2
FT-IR spectra of samples adsorbing FW-134.


## 3.2. Energy Spectrum Analysis of Surface Structure

We take an advantage of XPS to test the energy spectrum of sample A, sample B, and sample C, and the results are seen in Figure3. The XPS spectra curve analysis and fitting were conducted using the software XPS Peaks 4.1 developed by University of Hong Kong. We analyze the binding energy of Al2p, Si2p, C1s, K2p, O1s, F1s, N1s, and S2p of different samples. As shown in Figure 3, the binding energy of Al2p, Si2p, K2p, and O1s and the curve shape do not change with the concentration of FW-134; the binding energy of F1s, N1s, and S2p of sample B and sample C increases significantly compared with that of sample A and appears at 689 eV, 402 eV, and 169 eV, respectively.Figure 3
XPS spectra of sample systems adsorbing FW-134.The content and the binding energy of each element are calculated according to the peak area (Tables1 and 2).Table 1
XPS element content data of sample systems adsorbing FW-134.
Content (%)
Al2p
Si2p
C1s
K2p
O1s
F1s
N1s
S2p
Sample A
13.245
17.383
11.470
4.950
51.768
0.598
0.577
0.502
Sample B
10.269
13.458
7.588
4.689
43.194
17.545
2.092
1.166
Sample C
9.3410
11.949
10.377
4.327
37.953
22.037
2.616
1.400Table 2
XPSE
B data of sample systems adsorbing FW-134.
Binding energy (eV)
Al2p
Si2p
C1s
K2p
O1s
F1s
N1s
S2p
Sample A
74.26
102.42
284.76
293.1
531.58
685.07
401.92
169.16
Sample B
74.62
102.80
286.55
292.97
531.66
689.19
402.77
169.23
Sample C
74.50
102.65
286.31
292.67
531.69
689.06
402.79
169.02Sample A, with no FW-134 adsorption on the mica, only contains trace F, N, and S element, while the F, N, and S element contents in sample B and sample C with the adsorption of FW-134 increase significantly, and the content of the F element increases from 0.598% to 17.545% and 22.037%, the content of N element from 0.577% to 2.092% and 2.616%, and the S content from 0.502% to 1.166% and 1.400% (Table1), respectively. These showed that a large amount of FW-134 is adsorbed on the mica surface under the conditions of 40 hours’ oscillations at 90°C.The element binding energy (B.E.) in these samples can be seen in Table2. The binding energy of Al2p, Si2p, K2p, and O1s in samples B and C has little difference with that of sample A (Table 2), which shows that, under the conditions of high temperature, the chemical bonding force between FW-134 and the mica surface is weak. This is also consistent with the result from the infrared spectrum analysis. In order to further determine the FW-134 adsorption pattern on the mica surface, F1s XPS peaks of each sample were analyzed by Gauss fitting spectra, as shown in Figure 4.Figure 4
XPS C1s spectra of sample systems adsorbing FW-134 and contrast diagram.
(a)
(b)
(c)
(d)The F1s peaks of all samples are a single peak (Figure4), so the chemical structure of their F element is relatively single. The pulse signal of the F1s peak of sample A is strong, and the peak intensity and peak area are small, which show that there is less F content in sample A (Figures 4(a) and 4(d)). The curves of samples B and C in Figures 4(b) and 4(c) are smooth and orderly, and the intensity and peak area of the F1s peak are large, which suggests that a lot of the F element is in the surface structure of samples B and C and a great deal of FW-134 adsorption is on the mica surface.The F1s peak positions of samples B and C are different from those of sample A, and the F1s peak binding energy of sample B and sample C is basically the same (Figure4(d) and Table 2). That is, the F1s peak position and chemical structure of F atom before and after adsorption on the surface are different. The F1s peak binding energy of sample A is 685.2 eV, the Ca-F structure of mica; the F1s peak binding energies of sample B and sample C are about 689.1 eV, the structure of chain C-F; there are no hydrogen bonding peaks in sample B and sample C. These indicate that the chemical bonding strength between FW-134 and the mica surface is weak under the condition of high temperature, that covering is the main mechanism of different concentration of FW-134 adsorption on the surface of mica, and that physical adsorption rather than hydrogen bonding is the main mechanism of FW-134 adsorption under the condition of the 40 hours’ water oscillation.The Gauss fitting spectra of the C1s XPS peaks of samples are shown in Figure5. As shown in Figure 5(a), the C1s peak of sample A was split into four peaks; peak 1 and peak 2 are classified as a type of peak; the binding energies from low to high are for C-H

∖

C-C, C-O, and C=O peaks. As shown in Figures 5(b) and 5(c), the C1s peaks of sample B and sample C were divided into three peaks, respectively. Their binding energies from low to high are for C-H

∖

C-C, C-N

∖

C-C, and C-F peaks.Figure 5
XPS C1s spectra of samples adsorbing FW-134 and contrast diagram.
(a)
(b)
(c)
(d)The analysis results of the peak binding energy and peak area are shown in Table3. The C-H

∖

C-C peak area of sample A reaches 88.80%, and a small piece of the C-O and C=O peak area appears in the C1s peak (Table 3). This may be caused by the chemical structure of carbon on the sample original surface or adsorption of CO2 in the air on the surface. Compared with sample A, sample B and sample C have a large area of the C-F and C-N

∖

C-C peaks, whose total peak area is, respectively, 85.88% and 81.63%, while the peak area of C-H

∖

C-C is greatly reduced. The reason is that a large amount of FW-134 adsorbed covers on the mica surface to change the chemical structure of the original surface carbon under the high temperature water oscillation.Table 3
XPS results of samples adsorbing FW-134 calculated by Gauss method.
Sample
Type of structure
Binding energy (eV)
Peak area (%)
A
C-H C-C
285.0
88.80
C-O
286.5
5.70
C=O
288.8
5.50
B
C-H C-C
285.0
14.22
C-N C-C
285.7
46.07
C-F
286.8
39.81
C
C-H C-C
285.0
18.37
C-N C-C
285.7
38.90
C-F
286.8
42.73


## 3.3. Evaluation of Surface Conformation and Modification Effect

The water adsorption on modified surface of minerals depends on the surface structure [22]. In order to observe the morphology to further understand the FW-134 adsorption structure and interfacial modification effect on the mica surface, a mica surface treated by a 40 hours’ oscillation with 0.1% FW-134 solution and nitrogen flow drying under high temperature was tested by atomic force microscope (AFM). Figures 6 and 7 are the AFM scanning plane height map and three-dimensional map of the treated mica surface before and after cleaning of distilled water.Figure 6
AFM plane height map and the three-dimensional topography (before cleaning).Figure 7
AFM plane height map and the three-dimensional topography (after cleaning).As intuitively seen in Figure6, a lot of FW-134 molecules adsorbed on the mica surface are unequal granular and massive distribution phenomenon; the adsorption of FW-134 covers up to 80% of the testing scope with 10 μm × 10 μm; the adsorption layer is thin. The contact angles of water on the adsorption surface treated by 0.05%, 0.1%, and 0.2% are 71.9°, 101.2°, and 92.3°, respectively, which mean a good hydrophobic performance and interfacial modification ability of FW-134. After the mica surface is being cleaned with distilled water for 48 hours, there is still a lot of surfactant FW-134 adsorption on the mica surface (Figure 7). We conducted comparative experiments to verify whether the AFM data are reproducible. The adsorption area differences of FW-134 in 10 μm × 10 μm on mica surface in comparative experiments are less than ±6%, which verified that AFM data reproducibility was good. As seen in Figure 7, compared with Figure 6, a part of FW-134 molecules adsorbed on the mica surface are cleared away and the adsorption thickness is reduced, but the adsorbed layer still shows a uniform distribution, which indicts that 0.1% FW-134 has reached a saturated adsorption state on the surface of mica.


## 4. Discussions

Under the conditions of water oscillations, FW-134 on the mica surface is mainly physical adsorption, generally including the electrostatic and dispersion force adsorption. Because of characteristics of F atoms in fluorine surfactant molecules (the most electronegative and the minimum atomic polarizability) and the carbon chain of “shielding,” the C-F bond is not easy to be polarized, and dispersion forces of fluorine surfactant molecules are small. FW-134 adsorption on the mica surface force is electrostatic adsorption.With an increase of concentration, FW-134 reaches a saturated adsorption state on the surface of mica. Because of “hydrophobic effect” [9] of FW-134 molecules, micelle may form on the mica surface, but the low dispersion force of fluorine surfactant molecules and the thermodynamics effect under high temperature longtime oscillation lead to greatly weaken surface micelle formation and multilayer adsorption, so FW-134 adsorption on the mica surface has a single layer structure under the oscillation at 90°C when it reaches the saturated adsorption (Figure 8).Figure 8
FW-134 adsorption schematic diagram on mica surface.Owing to an outstanding high surface activity of fluorine surfactant, its 0.05%~0.1% solution concentrations can decrease the surface tension of the aqueous solution to below 20 mN/m. Low surface energy of fluorine or a silicon treatment agent is widely used in the surface modification to enhance the surface hydrophobicity. Genzer and Efimenko [21] and Peng et al. [23] used the fluorine surfactant treatment agent on the material surface fluorination modification treatment and successfully obtained a super hydrophobic surface.By electrostatic adsorption on the mica surface, a cationic hydrophilic ionic bond of FW-134 molecules is inward and its fluorocarbon hydrophobic chain is outward. The maximum C-F peak and the highest percentage of the area (Figure5 and Table 3) show that the micro- and nanostructure like a “lotus effect” is formed on a solid surface, so the wettability alteration effect is good due to low surface energy and the hydrophobic surface. Thus 0.05%~0.1% FW-134 solution can also have low surface tension and a good wettability reversal effect. Because of fluorinated surfactant being expensive, the compound and synergistic reaction of fluorine surfactant and common surfactant considering the cost and the effect might be worth developing, but it should be emphasized that counterions have great influence on the fluorine surfactant properties and adsorption behavior.


## 5. Conclusions

Fluorine surfactant adsorption on mica surfaces under the condition of oscillation at 90°C causes a hydrophilic surface to become hydrophobic structure with the strong ability of modifying interface and reversing wettability.Fluorine surfactant adsorption on the mica surface is mainly physical adsorption and has a single layer structure when it reaches the saturated adsorption, which may be the reason that the period of interface modification validity is short.0.05%~0.1% FW-134 can decrease the surface tension of the aqueous solution to below 20 mN/m and show high quality of wettability alteration effect.



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*Source: 980439-2015-09-27.xml*