Supporting Information One-step spray-coating process for the ...
Supporting Information One-step spray-coating process for the fabrication of colorful superhydrophobic coatings with excellent corrosion resistance Jian Li *, Runni Wu, ‡ Zhijiao Jing, ‡ Long Yan, Fei Zha and Ziqiang Lei * Key Laboratory of Eco-Environment-Related Polymer Materials, Ministry of Education of China, Key Laboratory of Gansu Polymer Materials, College of Chemistry and Chemical Engineering, Northwest Normal University, Lanzhou 730070, China Corresponding authors email: [email protected], [email protected]. ‡
These authors contributed equally.
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Supporting figure captions: Figure S1. XPS analysis for CuSA2 coating: (a) survey spectra, (b) Cu 2p spectra, (c) C 1s spectra. Figure S2. FT-IR spectra for (a) copper stearate, (b) ferric stearate, (c) cobaltous stearate, (d) chromium stearate, (e) zinc stearate and stearic acid, respectively. Figure S3. FE-SEM images of typical single stearate particles. Figure S4.The aggregate size of stearate particles distribution by DLS. Figure S5. XPS analysis for CuSA2 coating after immersion in 3.5 wt % NaCl solution for one month: (a) survey spectra and (b) Cl 1s spectra. Figure S6. EIS results of bare and FeSA3 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots. Figure S7. EIS results of bare and CoSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots. Figure S8. EIS results of bare and CrSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots. Figure S9. EIS results of bare and ZnSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots.
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Figure S1. XPS analysis for CuSA2 coating: (a) survey spectra, (b) Cu 2p spectra, (c) C 1s spectra. XPS is used to characterize the sample, and it does provides valuable information on the chemical compositions of the sample. From survey spectrum of CuSA2 coating in Figure S1a, it can be obviously observed that oxygen, carbon and Cu are main composition of the as-prepared particles. The peaks centered at 934.8 and 954.3 eV (Figure S1b) are ascribed to Cu2p3/2 and Cu2p1/2 of Cu2+, respectively.1 Figure S1c exhibits the multielement spectra of C1s, which are resolved into two components belonged to C–C/C–H and –COO groups.2 The peak signals centered at 288.6 eV is attributed to the –COO. Quantitative analysis of the surface chemical composition unambiguously supported that the atomic ratio of Cu and carbon (coordinated COO) is about 1:2, confirming successful formation of CuSA2, which is consistent with the reported work.2 Figure S2a presents the FT-IR spectra of copper stearate (CuSA2) and stearic acid particles, respectively. The peak centered at around 1702 cm−1 is assigned to carbonyl stretch of stearic acid, which is absent in the spectrum of copper stearate. Meanwhile, the appearance of the peaks at about 1587 cm−1 and 1471 cm−1 in the spectrum of copper stearate are attributed to m(COO)asym and m(COO)sym, stemming from the 3
formation of stearate.3 The FT-IR spectra of other stearate salts were also shown in Figure S2b-S2e.
Figure S2. FT-IR spectra for (a) copper stearate, (b) ferric stearate, (c) cobaltous stearate, (d) chromium stearate, (e) zinc stearate and stearic acid, respectively.
Figure S3. FE-SEM images of typical single stearate particles.
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Figure S4. The aggregate size of stearate particles distribution by DLS.
Figure S5. XPS analysis for CuSA2 coating after immersion in 3.5 wt % NaCl solution for one month: (a) survey spectra and (b) Cl 2p spectra.
Figure S6. EIS results of bare and FeSA3 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots.
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Figure S7. EIS results of bare and CoSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots.
Figure S8. EIS results of bare and CrSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots.
Figure S9. EIS results of bare and ZnSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots. 6
References (1) Li, J.; Liu, X.; Ye, Y.; Zhou, H.; Chen, J. Fabrication of Superhydrophobic CuO Surfaces with Tunable Water Adhesion. J. Phys. Chem. C 2011, 115, 4726–4729. (2) Wang, S. T.; Feng, L.; Jiang, L. One-Step Solution-Immersion Process for the Fabrication of Stable Bionic Superhydrophobic Surfaces. Adv. Mater. 2006, 18, 767–770. (3) Li, J.; Wan, H.; Ye, Y.; Zhou, H.; Chen, J. One-Step Process for the Fabrication of Superhydrophobic Surfaces with Easy Repairability. Appl. Surf. Sci. 2012, 258, 3115–3118.
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These authors contributed equally.
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Supporting figure captions: Figure S1. XPS analysis for CuSA2 coating: (a) survey spectra, (b) Cu 2p spectra, (c) C 1s spectra. Figure S2. FT-IR spectra for (a) copper stearate, (b) ferric stearate, (c) cobaltous stearate, (d) chromium stearate, (e) zinc stearate and stearic acid, respectively. Figure S3. FE-SEM images of typical single stearate particles. Figure S4.The aggregate size of stearate particles distribution by DLS. Figure S5. XPS analysis for CuSA2 coating after immersion in 3.5 wt % NaCl solution for one month: (a) survey spectra and (b) Cl 1s spectra. Figure S6. EIS results of bare and FeSA3 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots. Figure S7. EIS results of bare and CoSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots. Figure S8. EIS results of bare and CrSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots. Figure S9. EIS results of bare and ZnSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots.
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Figure S1. XPS analysis for CuSA2 coating: (a) survey spectra, (b) Cu 2p spectra, (c) C 1s spectra. XPS is used to characterize the sample, and it does provides valuable information on the chemical compositions of the sample. From survey spectrum of CuSA2 coating in Figure S1a, it can be obviously observed that oxygen, carbon and Cu are main composition of the as-prepared particles. The peaks centered at 934.8 and 954.3 eV (Figure S1b) are ascribed to Cu2p3/2 and Cu2p1/2 of Cu2+, respectively.1 Figure S1c exhibits the multielement spectra of C1s, which are resolved into two components belonged to C–C/C–H and –COO groups.2 The peak signals centered at 288.6 eV is attributed to the –COO. Quantitative analysis of the surface chemical composition unambiguously supported that the atomic ratio of Cu and carbon (coordinated COO) is about 1:2, confirming successful formation of CuSA2, which is consistent with the reported work.2 Figure S2a presents the FT-IR spectra of copper stearate (CuSA2) and stearic acid particles, respectively. The peak centered at around 1702 cm−1 is assigned to carbonyl stretch of stearic acid, which is absent in the spectrum of copper stearate. Meanwhile, the appearance of the peaks at about 1587 cm−1 and 1471 cm−1 in the spectrum of copper stearate are attributed to m(COO)asym and m(COO)sym, stemming from the 3
formation of stearate.3 The FT-IR spectra of other stearate salts were also shown in Figure S2b-S2e.
Figure S2. FT-IR spectra for (a) copper stearate, (b) ferric stearate, (c) cobaltous stearate, (d) chromium stearate, (e) zinc stearate and stearic acid, respectively.
Figure S3. FE-SEM images of typical single stearate particles.
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Figure S4. The aggregate size of stearate particles distribution by DLS.
Figure S5. XPS analysis for CuSA2 coating after immersion in 3.5 wt % NaCl solution for one month: (a) survey spectra and (b) Cl 2p spectra.
Figure S6. EIS results of bare and FeSA3 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots.
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Figure S7. EIS results of bare and CoSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots.
Figure S8. EIS results of bare and CrSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots.
Figure S9. EIS results of bare and ZnSA2 coated Al surfaces in 3.5 wt% NaCl solution. (a) Nyquist plots, (b) bode |Z| versus frequency plots, and (c) bode–phase angle versus frequency plots. 6
References (1) Li, J.; Liu, X.; Ye, Y.; Zhou, H.; Chen, J. Fabrication of Superhydrophobic CuO Surfaces with Tunable Water Adhesion. J. Phys. Chem. C 2011, 115, 4726–4729. (2) Wang, S. T.; Feng, L.; Jiang, L. One-Step Solution-Immersion Process for the Fabrication of Stable Bionic Superhydrophobic Surfaces. Adv. Mater. 2006, 18, 767–770. (3) Li, J.; Wan, H.; Ye, Y.; Zhou, H.; Chen, J. One-Step Process for the Fabrication of Superhydrophobic Surfaces with Easy Repairability. Appl. Surf. Sci. 2012, 258, 3115–3118.
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