Electrodeposition of Oriented Cerium Oxide Films

Wang, Adele Qi; Golden, Teresa D.

doi:https://doi.org/10.1155/2013/482187

International Journal of Electrochemistry

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Abstract Introduction Experimental Results and Discussion Conclusion References Copyright Related Articles

Research Article | Open Access

Volume 2013 | Article ID 482187 | https://doi.org/10.1155/2013/482187

Electrodeposition of Oriented Cerium Oxide Films

Adele Qi Wang¹and Teresa D. Golden¹

Academic Editor: Benjamín R. Scharifker

Received19 Jul 2013

Revised12 Sept 2013

Accepted13 Sept 2013

Published27 Oct 2013

Abstract

Cerium oxide films of preferred orientation are electrodeposited under anodic conditions. A complexing ligand, acetate, was used to stabilize the cerium (III) ion in solution for deposition of the thin films. Fourier transform infrared spectroscopy showed that the ligand and metal tended to bind as a weakly bidentate complex. The crystallite size of the films was in the nanometer range as shown by Raman spectroscopy and was calculated from X-ray diffraction data. Crystallite sizes from 6 to 20 nm were obtained under the anodic deposition conditions. Sintering of the (111) oriented films showed an increase in the (111) orientation with temperatures up to 900°C. Also, the crystallite size increased from 20 nm to 120 nm under sintering conditions. Addition of the deposited films to the substrate improved corrosion resistance for the substrate.

1. Introduction

The fabrication of cerium oxide films is of interest due to broad applications for these films [1–6]. Cerium oxide can function as a catalyst, structure barrier for insulator on silicon, buffer layer on superconductor materials, and an anticorrosion coating on metals [7–12]. The texture of these thin films can affect the mechanical, electronic, and corrosion properties.

Electrochemical deposition is an attractive method for the synthesis of thin films. It offers the advantages of low processing temperature, high purity of deposition, and controlled thickness of the film. Cathodic electrodeposition (i.e., base generation electrochemical methods) was first introduced for the plating of cerium oxide films [13–17]. However, producing CeO₂ films with the base generation method is limited since the as-produced films tend to be powdery and loosely adherent.

It is possible to obtain thin films of cerium oxide by stabilizing Ce³⁺ in solution with a weakly bound ligand [18–20]. With a high enough oxidation potential at the electrode surface, an equilibrium can be established where Ce()- has a slow release of Ce³⁺ from the complex for available oxidation. This mechanism has been described previously in greater detail [19]. These films can be electrodeposited under potentiostatic control and produce polycrystalline films of random orientation [18–21]. XANE study on electrodeposited cerium-related thin films revealed that anodic deposition preferred the Ce() compounds, while cathodic base generation method led to the formation of high percentage of Ce() species in the composition [22].

For corrosion protection, cerium oxide has been used as coatings on stainless steel. While stainless steel can give protection against corrosion in certain environments, there is a need for resistance in other environments. This can be especially true for such places as coal and heavy oil plants [23] or in marine environments [24]. Since nickel has been increasing in price over recent years, there is an interest in shifting from austenitic to ferritic steels where possible. One of the largest drawbacks to using ferritic stainless steels, such as type 430, is less resistance to corrosion. Pitting corrosion especially in chloride containing environments can be a problem for type 430 stainless steel [25].

In this work, CeO₂ is deposited with a preferred crystalline orientation. This is accomplished by precisely controlling the deposition parameters. The resulting films are characterized by scanning electron microscopy, X-ray diffraction, Fourier transform infrared spectroscopy, and Raman spectroscopy. The sintering ability and corrosion protection of the films are also studied.

2. Experimental

An EG&G Princeton Applied Research (PAR) Model 273A potentiostat/galvanostat was used to electrochemically deposit CeO₂ films. The electrochemical cell was kept at constant temperature with a Fisher Scientific Model 1016D circulator. The deposition was conducted in an undivided cell and regular three-electrode configuration. The working electrode was prepared by mounting stainless steel (type 430, nominal composition 0.12% C, 1% Mn, 1% Si, 0.04% P, 0.03% S, 0.75% Ni, 17% Cr, Fe) or platinum in epoxy and then polished, rinsed, and ultrasonicated to a mirror finish. Platinum wire or mesh was used as the counter electrode and a saturated calomel electrode (SCE) as the reference. The electrolyte consisted of 0.1 M Ce(NO₃)₃·6H₂O (99.5% pure, Alfa AESAR) and sodium acetate (Fisher) as a ligand. Ce(NO₃)₃ and ligand concentrations were 0.1 M throughout the study. All the solutions were prepared using deionized water. Solution pH was adjusted with NaOH and monitored with a Corning pH meter and Pasco Scientific pH electrode throughout the deposition experiments. Each deposition was completed in 24–48 hours.

The deposited film together with the substrate was sintered in air. A temperature ramping procedure was used starting at 260°C with a ramping rate of 1°C/min to the desired temperature value, keeping the value for one hour, and finally decreasing the temperature at a ramping rate of 1°C/min to 260°C.

The structure and phase composition of the electrochemical deposited films were identified by X-ray diffraction (XRD) with a Siemens D500 diffractometer using Cu K radiation ( = 0.15405 nm). The tube source was operated at 40 kV and 30 mA.

The surface morphology of the films was characterized by a scanning electron microscope (SEM), JOEL JSM-T300 with an accelerating voltage of 5–25 kV.

Raman spectra were obtained using a Yvon Dilor XY800 Raman microprobe equipped with a nitrogen-cooled multichannel (CCD) detector, with an excitation wavelength of 514.54 nm laser radiation at 10 mW of power to prevent local heating of the sample. All the spectra were recorded between 200 and 4000 cm⁻¹ with 3 cm⁻¹ spectra resolution, 719 mm focal length, 600 lines/mm gratings, and 10x objective focused to 10 m spot size. At least three spectra were randomly collected from different areas of the films and plotted.

Infrared spectra were obtained using a Perkin-Elmer 1760X FTIR spectrophotometer. For each sample, 40 scans were collected in the range of 4000–400 cm⁻¹ with a resolution of 4 cm⁻¹.

Linear polarization and Tafel experiment were done with EG&G 273A potentiostat using EG&G 352 softcorr .

3. Results and Discussion

Ce³⁺ has the electronic structure of 4f¹5d⁰6s⁰, and as a trivalent member of lanthanide series, the most stable complexes are those with chelating oxygen ligands [26]. Previously, acetate and lactate have been shown as ligands to result in film formation of CeO₂ on substrates [18–21]. Kulp et al. studied acetate ions as stabilizing agents for cerium (III) to determine the predominant species in the deposition solution. At a pH of 6.1, the main species was CeOAc²⁺, and the cerium ()-ligand complex proved significant for the anodic deposition of CeO₂films [21]. As a complexing agent, the acetate ion may be bound with the metal as a unidentate, bidentate, or bridging type with the later two classified as symmetrical or unsymmetrical (Figure 1) [27–29]. Unidentate oxygen ligands are less stable than the others and are prone to dissociation.

FTIR can be useful to probe the coordination between acetate and cerium () species [28, 30–32]. Symmetrical and antisymmetric C–O stretching modes are at ~1415 ± 20 and ~1570 ± 20 cm⁻¹, respectively. These two characteristic IR bands will alter in position and shape with different coordination modes. If acetate is a unidentate, one of the oxygen is used in bonding with the metal, leaving a double-bond (C=O) giving a 1590–1650 cm⁻¹ peak for the antisymmetric stretch mode. The large increase in the antisymmetric band and the corresponding decrease in the symmetrical band increase the frequency difference between these two emissions. With acetate as a bidentate ligand, the two C–O bonds retain equivalent stretching, giving no enhancement for the two bands [28]. Coupling between different acetate groups leads to multiple bands in the range of 1400–1550 cm⁻¹, if more than one acetate bonds to a metal ion [32]. Bridging can also be regarded as an intermediate mode between uni- and bidentate coordinations [32].

Solutions of cerium () nitrate-acetate with a molar ratio of cerium () to acetate in the range of 1 : 1 to 1 : 9 were run using FTIR. The results are shown in Figures 2 and 3. The acetate ligand alone in solution exists as ions and the two C–O stretching bands are equivalent indicating C=O and C–O⁻, as would be expected for the free ion (Figure 2). Figure 3 shows the IR spectrum changes with the molar ratio between cerium () and acetate increasing from 1 : 1 to 1 : 10. At lower concentrations of acetate, the ~1415 cm⁻¹ bands (symmetrical) are enhanced and split into two bands, at 1404 and 1352 cm⁻¹, respectively, with weak peaks around 1560 and 1577 cm⁻¹ (Figure 3). The pair of 1404 and 1560 cm⁻¹, which results in the difference of ~156 cm⁻¹ (Table 1), shows an enhanced bidentate complex [28]. The higher frequency of 1577 cm⁻¹ is very weak so the predominant binding is with C–O⁻. The stronger intensities of the lower frequencies can be attributed to the complex having symmetrical properties, pointing to a symmetrical bidentate complex. These 1 : 1 metal : acetate results coincide with the luminescence and NMR results reported by Azenha et al. which show that the dominant mode of complexation involved a weak, predominately bidentate binding of the metal ion, suggesting a species (where = 6 or 7) [33]. Kulp et al., also calculated this species as the predominant form in the electrodeposition solution [21].

(a)

(b)

(c)

With increasing amount of acetate, the 1350 cm⁻¹ band decreases, but the splitting is still sustained (Figure 3), indicating, the coordination is two modes but with the bridging gradually dominating. Also the higher frequency band, ~1560 cm⁻¹ gives a strong signal. FTIR results showed that for molar ratios of 1 : 2 to 1 : 7, similar IR spectra were obtained suggesting the saturation of coordination with increasing amounts of acetate. When the molar ratio is increased to as high as 8–10, the 1570 and 1550 cm⁻¹ bands merge and give higher intensities. Considering the saturation of metal coordination, the extra free ions of acetate contribute more to the IR spectra. The coordination number of the Ce()-acetate complex is estimated at 6-7 with weak bidentate coordination for the 1 : 1 complex and bridging at higher concentrations. More accurate determination of complex coordination number can be acquired by combining IR and solid-state NMR with single-crystal X-ray diffraction. Since the 1 : 1 ratio provided the least complicated complexation, this molar ratio was used in the deposition of the oriented films.

Several parameters were explored to optimize the deposition of the CeO₂ films with preferred orientation. The linear sweep voltammogram is shown in Figure 4 for the plating solution used for the cerium oxide film deposition. A small oxidation peak can be seen around a potential of ~0.95 V that is attributed to the conversion of Ce() to Ce() species [19]. While potentiostatic and galvanostatic modes were both shown to give CeO₂ films, galvanostatic mode resulted in preferred orientation of the films when higher temperatures were used. A range of current densities were studied at 25°C for anodic current densities between −0.06 and –0.90 mA/cm². The deposited films exhibited a random pattern, with increasing current, and the intensity of the (111) reflection decreases. The lower currents (i.e., –0.06 mA/cm²) are more conducive to the formation of preferred orientation. The effect of deposition temperature was then investigated at these lower current densities.

Increasing the temperature increases the steady state current density for the cerium-acetate system. The X-ray diffraction patterns of the deposited films are shown for higher temperatures of 70° and 80°C (Figure 5). With increasing temperature, for the galvanostatic deposition, the CeO₂ (111) reflection increases in intensity producing films with a preferred (111) orientation, while the potentiostatic deposition only produces random oriented films. The intensity ratios () for the CeO₂ patterns in Figure 5 are shown in Table 2. While the (111) intensity of the CeO₂ increases, the substrate peak remains about the same intensity, indicating that the film thickness is approximately the same at all temperatures. The film thicknesses for all depositions tend to be thin since CeO₂ is not very conducting.

(a)

(b)

The potential monitored during galvanostatic deposition for a current density of −0.06 mA/cm² is in the range of 0.7–1.0 V versus SCE. Progressing through the deposition, the potential increases to 0.9–1.1 V. However, when these corresponding potentials are applied in the potentiostatic deposition, a random structure is obtained, not preferred oriented films.

Raman spectroscopy is an effective tool to investigate the structure of cerium oxide and crystalline size of the CeO₂ [34–37]. Crystallite size is a significant parameter for the properties and application of the cerium oxide film. Smaller particle sizes and minimum film thickness of cerium oxide films lead to improvements for corrosion protection. Other researchers have demonstrated this for CeO₂ films deposited by sol-gel and reactive sputtering methods [38, 39]. In Wang’s report, when the crystallite is larger than 20 nm, there will be one major shift for the 463 cm⁻¹ peak in Raman; however, for crystallite sizes smaller than 10 nm, two more shifts at 270, 315 cm⁻¹ appear and the intensities increase with decreasing crystal sizes [34]. The Raman spectra of the anodically deposited CeO₂ are shown in Figure 6 for galvanostatic deposited CeO₂ films with an applied current density of –0.06 mA/cm².

The reproducible spectra in each Raman spectra figure demonstrate the homogeneities of the deposited CeO₂ film samples. The peak observed at ~450 cm⁻¹ is about 14 cm⁻¹ lower relative to the reported peak (464 cm⁻¹) for microsized CeO₂, indicating that the crystallites are in the nanosize range. The lattice calculations, from the XRD patterns, support this observation for Raman.

For XRD patterns which exhibit preferred orientation, the following Scherrer equation is used to estimate the crystallite size [40]; where is the wavelength of the X-rays, is the diffraction angle, is the crystallite size, is a constant dependent on the crystal shape, and is the corrected FWHM of the given peak. From the (111) reflection of the CeO₂ films, the crystallite sizes for the preferred oriented films ranged from 6 nm for films deposited at 25°C and increased to ~20 nm at higher deposition temperatures of 70°–80°C (Figure 7).

Type 430 is used extensively in SOFC interconnects and is exposed to high temperatures [41]. However, type 430 can become sensitized with continuous annealing at higher temperatures of 900°C or above [42]. The (111) preferred oriented CeO₂ deposited films were sintered at various temperatures for short time periods (1 hr). The CeO₂ (111) reflection in XRD becomes shaper and more intense as the sintering temperature increases up to 900°C (Figure 8). As the temperature is raised to 1100°C at a constant rate for the thin electrodeposited CeO₂ film, the XRD pattern shows a change in both composition and orientation. The CeO₂ reverts to a random arrangement with 100-fold lower intensity. Accompanied with this is the evolution of strong substrate peaks indicating higher concentration of substrate components on the surface. Above 900°C, oxidation of the substrate occurs during thermal treatment and migration of substrate ions to the surface. Sintering in an inert atmosphere may improve the temperature range at the higher limits. Crystallite size also changes with sintering temperature for the preferred oriented CeO₂ films (Figure 9). The estimated crystallite size increases from ~10 nm for the unsintered sample to ~120 nm at 900°C. A crystallite size minimum is obtained at a sintering temperature of 300°C. It is reasonable to attribute this to the drying and dehydration of green films [43].

The microstructure features of the preferred oriented CeO₂ films with sintering are shown in Figure 10. The unsintered CeO₂ film exhibits a very smooth surface with cracking and this is probably due to a large mismatch between the substrate and film or drying process [16, 43]. This type of cracking of CeO₂ has also been observed for other wet chemical methods of deposition such as electrophoresis [14]. The cracking of the film is retained during sintering and shrinkage of the sample, and the cracking extends its width (Figures 10(b) and 10(c)), as the sintering temperature reaches 500 and 900°C [44]. For the 1100°C sintered sample, corrosion is seen to progress on the CeO₂ surface, with the appearance of bulk corrosion products (Fe₂O₃, etc.) discerned in the SEM.

(a)

(b)

(c)

(d)

Linear polarization and Tafel plots were applied to test the corrosion protection effect of the as deposited cerium oxide oriented films. The electrochemical corrosion parameters are summarized in Table 3. Calculated from the Tafel plots (Figure 11), the corrosion current decreases from ~7.94 × 10⁻⁹ for the substrate to 7.59 × 10⁻¹⁰ A·cm⁻² for the CeO₂ film coated substrate in a 0.1 M NaCl solution. Correspondingly, the decreases from 2.63 × 10⁶ for the substrate to 6.69 × 10⁷Ω·cm² for the CeO₂film coated stainless steel. The CeO₂ coated substrate exhibits a corrosion positive of the bare stainless steel, indicating an anodic corrosion inhibition mechanism involved for CeO₂ coatings. A compact and intact CeO₂ film on the surface impedes the ejection of metal ions into the electrolyte, thereby inhibiting corrosion reactions. Generally the immersion experiment suggested cerium oxide/hydroxide as a cathodic inhibitor [10]. However, Crossland and coworkers investigated the formation of anodized cerium oxide/hydroxide film out of Al/Ce alloys and substantiated that this cerium-rich layer provides anodic inhibition to aluminum corrosion [11], which agrees with this study.

4. Conclusion

Cerium oxide (111) oriented thin films were successfully grown on stainless steel substrate with an anodic electrodeposition technique. A solution of cerium () and a weak organic ligand (acetate) at pH = 7.5 were used for the deposition. Preliminary investigation of the coordination between Ce() and the acetate ligand points to a bidentate complex for the 1 : 1 molar metal : acetate solutions. Preferred orientation of CeO₂ films was obtained by tailoring the deposition conditions, suggesting that the optimized deposition parameters for oriented polycrystalline CeO₂ include current density lower than –0.06 mA/cm² with galvanostatic deposition mode and deposition temperatures higher than 50°C. X-ray diffraction showed the deposited films crystallite size in the nanometer size range, which was further confirmed with Raman. Scanning electron microscopy shows a smooth surface and cracked appearance of the deposits. Sintering and corrosion experiments were conducted on the deposited films to further illustrate the properties and the possible applications of these thin films. Detailed investigations about optical, electrical, and catalytic properties of cerium oxide films may expand its application perspective. Also, anodic electrodeposition is a relatively novel synthesis technique for ceramic oxides and worthwhile to extend to other materials. Praseodymium and neodymium oxide depositions with this method are underway in our research group.

References

N. Özer, J. P. Cronin, and S. Akyuz, “Electrochromic performance of sol-gel deposited CeO₂ films,” in Proceedings of the Society of Photo-Optical Instrumentation, vol. 3788, pp. 103–110, July 1999.
View at: Google Scholar
A. Wang, J. A. Belot, T. J. Marks et al., “Buffers for high temperature superconductor coatings. Low temperature growth of CeO₂ films by metal-organic chemical vapor deposition and their implementation as buffers,” Physica C, vol. 320, no. 3, pp. 154–160, 1999.
View at: Publisher Site | Google Scholar
A. Trovarelli, “Catalytic properties of ceria and CeO₂-containing materials,” Catalysis Reviews, vol. 38, no. 4, pp. 439–520, 1996.
View at: Google Scholar
J. Gerblinger, W. Lohwasser, U. Lampe, and H. Meixner, “High temperature oxygen sensor based on sputtered cerium oxide,” Sensors and Actuators B, vol. 26, no. 1–3, pp. 93–96, 1995.
View at: Google Scholar
E. S. Putna, J. Stubenrauch, J. M. Vohs, and R. J. Gorte, “Ceria-based anodes for the direct oxidation of methane in solid oxide fuel cells,” Langmuir, vol. 11, no. 12, pp. 4832–4837, 1995.
View at: Google Scholar
A. L. Rudd, C. B. Breslin, and F. Mansfeld, “The corrosion protection afforded by rare earth conversion coatings applied to magnesium,” Corrosion Science, vol. 42, no. 2, pp. 275–288, 2000.
View at: Publisher Site | Google Scholar
X. D. Wu, R. C. Dye, R. E. Muenchausen et al., “Epitaxial CeO₂ films as buffer layers for high-temperature superconducting thin films,” Applied Physics Letters, vol. 58, no. 19, pp. 2165–2167, 1991.
View at: Publisher Site | Google Scholar
T. Inoue, Y. Yamamoto, S. Koyama, S. Suzuki, and Y. Ueda, “Epitaxial growth of CeO₂ layers on silicon,” Applied Physics Letters, vol. 56, no. 14, pp. 1332–1333, 1990.
View at: Publisher Site | Google Scholar
M. W. Denhoff and J. P. McCaffrey, “Epitaxial Y₁Ba₂Cu₃O₇ thin films on CeO₂ buffer layers on sapphire substrates,” Journal of Applied Physics, vol. 70, no. 7, pp. 3986–3988, 1991.
View at: Publisher Site | Google Scholar
D. R. Arnott, B. R. W. Hinton, and N. E. Ryan, “Cationic-film-forming inhibitors for the protection of the AA 7075 aluminum alloy against corrosion in aqueous chloride solution,” Corrosion, vol. 45, no. 1, pp. 12–18, 1989.
View at: Google Scholar
A. C. Crossland, G. E. Thompson, P. Skeldon et al., “Anodic oxidation of Al-Ce alloys and inhibitive behaviour of cerium species,” Corrosion Science, vol. 40, no. 6, pp. 871–885, 1998.
View at: Publisher Site | Google Scholar
M. A. Arenas, A. Conde, and J. J. de Damborenea, “Cerium: a suitable green corrosion inhibitor for tinplate,” Corrosion Science, vol. 44, no. 3, pp. 511–520, 2002.
View at: Publisher Site | Google Scholar
J. A. Switzer, “Electrochemical synthesis of ceramic films and powders,” American Ceramic Society Bulletin, vol. 66, no. 10, pp. 1521–1524, 1987.
View at: Google Scholar
I. Zhitomirsky and A. Petric, “Electrolytic and electrophoretic deposition of CeO₂ films,” Materials Letters, vol. 40, no. 6, pp. 263–268, 1999.
View at: Publisher Site | Google Scholar
F.-B. Li and G. E. Thompson, “In situ atomic force microscopy studies of the deposition of cerium oxide films on regularly corrugated surfaces,” Journal of the Electrochemical Society, vol. 146, no. 5, pp. 1809–1815, 1999.
View at: Publisher Site | Google Scholar
Y. Zhou and J. A. Switzer, “Growth of cerium(IV) oxide films by the electrochemical generation of base method,” Journal of Alloys and Compounds, vol. 237, no. 1-2, pp. 1–5, 1996.
View at: Google Scholar
A. J. Aldykiewicz Jr., A. J. Davenport, and H. S. Isaacs, “Studies of the formation of cerium-rich protective films using X-ray absorption near-edge spectroscopy and rotating disk electrode methods,” Journal of the Electrochemical Society, vol. 143, no. 1, pp. 147–154, 1996.
View at: Google Scholar
A. Q. Wang and T. D. Golden, “Anodic deposition of cerium oxide: I. Formation of crystalline thin films,” Journal of the Electrochemical Society, vol. 150, no. 9, pp. C616–C620, 2003.
View at: Publisher Site | Google Scholar
T. D. Golden and A. Q. Wang, “Anodic deposition of cerium oxide thin films: II. Mechanism studies,” Journal of the Electrochemical Society, vol. 150, no. 9, pp. C621–C624, 2003.
View at: Publisher Site | Google Scholar
A. Q. Wang, P. Punchaipetch, R. M. Wallace, and T. D. Golden, “X-ray photoelectron spectroscopy study of electrodeposited nanostructured CeO₂ films,” Journal of Vacuum Science and Technology B, vol. 21, no. 3, pp. 1169–1175, 2003.
View at: Google Scholar
E. A. Kulp, S. J. Limmer, E. W. Bohannan, and J. A. Switzer, “Electrodeposition of nanometer-thick ceria films by oxidation of cerium(III)-acetate,” Solid State Ionics, vol. 178, no. 11-12, pp. 749–757, 2007.
View at: Publisher Site | Google Scholar
M. Balasubramanian, C. A. Melendres, and A. N. Mansour, “X-ray absorption study of the local structure of cerium in electrochemically deposited thin films,” Thin Solid Films, vol. 347, no. 1-2, pp. 178–183, 1999.
View at: Publisher Site | Google Scholar
E. Stoyanova and D. Stoychev, “Corrosion behavior of stainless steels modified by cerium oxides layers,” in Corrosion Resistance, H. Shih, Ed., pp. 239–270, InTech Press, 2012.
View at: Google Scholar
S. Hastuty, A. Nishikata, and T. Tsuru, “Pitting corrosion of Type 430 stainless steel under chloride solution droplet,” Corrosion Science, vol. 52, no. 6, pp. 2035–2043, 2010.
View at: Publisher Site | Google Scholar
M. Finšgar, S. Fassbender, S. Hirth, and I. Milošev, “Electrochemical and XPS study of polyethyleneimines of different molecular sizes as corrosion inhibitors for AISI 430 stainless steel in near-neutral chloride media,” Materials Chemistry and Physics, vol. 116, no. 1, pp. 198–206, 2009.
View at: Publisher Site | Google Scholar
F. A. Cotton, G. Wilkinson, C. A. Murillo, and M. Bochmann, Advanced Inorganic Chemistry: A Comprehensive Text, John Wiley & Sons, New York, NY, USA, 4th edition, 1980.
N. W. Alcock, V. M. Tracy, and T. C. Waddington, “Acetates and acetate-complexes. Part 1. Preparation of acetato-complexes and conductimetric studies in the acetic anhydride solvent system,” Journal of the Chemical Society, Dalton Transactions, no. 21, pp. 2238–2242, 1976.
View at: Publisher Site | Google Scholar
N. W. Alcock, V. M. Tracy, and T. C. Waddington, “Acetates and acetato-complexes. Part 2. Spectroscopic studies,” Journal of the Chemical Society, Dalton Transactions, no. 21, pp. 2243–2246, 1976.
View at: Publisher Site | Google Scholar
N. W. Alcock and V. L. Tracy, “Acetates and acetato-complexes. Part 3. The crystal and molecular structure of tetramethylammonium penta-acetatostannate(IV),” Journal of the Chemical Society, Dalton Transactions, no. 21, pp. 2246–2249, 1976.
View at: Publisher Site | Google Scholar
Y. Mathey, D. R. Greig, and D. F. Shriver, “Variable-temperature Raman and infrared spectra of the copper acetate dimer Cu₂(O₂CCH₃)₄(H₂O)₂ and its derivatives,” Inorganic Chemistry, vol. 21, no. 9, pp. 3409–3413, 1982.
View at: Google Scholar
J. Stubenrauch and J. M. Vohs, “Interaction of CO with Rh supported on stoichiometric and reduced CeO₂(111) and CeO₂(100) surfaces,” Journal of Catalysis, vol. 159, no. 1, pp. 50–57, 1996.
View at: Google Scholar
F. Vratny, C. N. R. Rao, and M. Dilling, “Infrared spectra of metal acetates,” Analytical Chemistry, vol. 33, no. 10, p. 1455, 1961.
View at: Google Scholar
M. E. Azenha, H. D. Burrows, S. M. Fonseca et al., “Luminescence from cerium(III) acetate complexes in aqueous solution: considerations on the nature of carboxylate binding to trivalent lanthanides,” New Journal of Chemistry, vol. 32, no. 9, pp. 1531–1535, 2008.
View at: Publisher Site | Google Scholar
S. Wang, W. Wang, J. Zuo, and Y. Qian, “Study of the Raman spectrum of CeO₂ nanometer thin films,” Materials Chemistry and Physics, vol. 68, no. 1–3, pp. 246–248, 2001.
View at: Publisher Site | Google Scholar
W. H. Weber, K. C. Hass, and J. R. McBride, “Raman study of CeO₂: second-order scattering, lattice dynamics, and particle-size effects,” Physical Review B, vol. 48, no. 1, pp. 178–185, 1993.
View at: Publisher Site | Google Scholar
M. S. P. Francisco, V. R. Mastelaro, P. A. P. Nascente, and A. O. J. Florentino, “Activity and characterization by XPS, HR-TEM, Raman spectroscopy, and bet surface area of CuO/CeO₂-TiO₂ catalysts,” Journal of Physical Chemistry B, vol. 105, no. 43, pp. 10515–10522, 2001.
View at: Publisher Site | Google Scholar
J. Twu, C. J. Chuang, K. I. Chang, C. H. Yang, and K. H. Chen, “Raman spectroscopic studies on the sulfation of cerium oxide,” Applied Catalysis B, vol. 12, no. 4, pp. 309–324, 1997.
View at: Publisher Site | Google Scholar
P. Papaiacovou, R. J. Hussey, D. F. Mitchell, and M. J. Graham, “The effect of CeO₂ coatings on the oxidation behaviour of Fe-20Cr alloys in O₂ at 1173 K,” Corrosion Science, vol. 30, no. 4-5, pp. 451–460, 1990.
View at: Google Scholar
F. Czerwinski and J. A. Szpunar, “Optimizing properties of CeO₂ sol-gel coatings for protection of metallic substrates against high temperature oxidation,” Thin Solid Films, vol. 289, no. 1-2, pp. 213–219, 1996.
View at: Google Scholar
H. P. Klug and L. E. Alexander, X-Ray Diffraction Procedures For Polycrystalline and Amorphous Materials, John Wiley & Sons, New York, NY, USA, 2nd edition, 1974.
N. Shaigan, W. Qu, D. G. Ivey, and W. Chen, “A review of recent progress in coatings, surface modifications and alloy developments for solid oxide fuel cell ferritic stainless steel interconnects,” Journal of Power Sources, vol. 195, no. 6, pp. 1529–1542, 2010.
View at: Publisher Site | Google Scholar
F. Martín, C. García, P. de Tiedra, Y. Blanco, and M. L. Aparicio, “Sensitization of powder metallurgy type 430L stainless steel sintered in nitrogen-hydrogen atmosphere,” Corrosion, vol. 64, no. 1, pp. 70–82, 2008.
View at: Google Scholar
I. Zhitomirsky and A. Petric, “The electrodeposition of ceramic and organoceramic films for fuel cells,” Journal of Organic Materials, vol. 53, no. 9, pp. 48–50, 2001.
View at: Google Scholar
R. M. German, Sintering Theory and Practice, John Wiley &. Sons, 1996.

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Copyright © 2013 Adele Qi Wang and Teresa D. Golden. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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