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Article

On the Application of Bipolar Electrochemistry to Characterise the Localised Corrosion Behaviour of Type 420 Ferritic Stainless Steel

by
Yiqi Zhou
1,* and
Dirk Lars Engelberg
1,2
1
Corrosion & Protection Centre, Department of Materials, School of Natural Sciences, The University of Manchester, Manchester M13 9PL, UK
2
Materials Performance Centre, The University of Manchester, Manchester M13 9PL, UK
*
Author to whom correspondence should be addressed.
Metals 2020, 10(6), 794; https://doi.org/10.3390/met10060794
Submission received: 23 May 2020 / Revised: 10 June 2020 / Accepted: 13 June 2020 / Published: 15 June 2020
(This article belongs to the Special Issue Localized Corrosion of Metals and Alloys)
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Abstract

:
Bipolar electrochemistry has been applied to Type 420 ferritic stainless steel in order to determine the full spectrum of anodic-to-cathodic polarisation behaviour. The occurrence of crevice corrosion, pitting corrosion in combination with general corrosion, pitting corrosion only, general corrosion only, followed by a cathodic region has been observed. Instances of pitting corrosion initiated near chromium-rich carbides with Cr23C6, Cr3C2, and Cr7C3 identified as pit nucleation sites. The observed pit growth kinetics were independent of the electrochemical over-potential. Characterisation of the pit size distributions supports the presence of a critical dissolved volume for the transition of metastable to stable pit growth and pit coalescence.

Highlights: The application of bipolar electrochemistry for observing pit growth kinetics and pit coalescence has been demonstrated.
Cr23C6, Cr3C2, and Cr7C3 have been identified as pit nucleation sites.
A critical dissolved pit volume has been observed for the transition to stable pit growth.

1. Introduction

The application of bipolar electrochemistry provides access to the full spectrum of anodic-to-cathodic reactions along a bipolar electrode (BPE) [1,2,3,4]. In earlier studies, bipolar electrochemistry was applied for electro-syntheses, in photo electrochemical cells, for battery research, high throughput deposition of metals, and corrosion investigations [5,6,7]. In a nutshell, bipolar electrochemistry combines a non-contact experimental setup with the ability of fast throughput corrosion screening, with access to all anodic and cathodic reactions in one experiment [1,2,3].
Stainless steels are prone to pitting corrosion in halide containing environments. In general, pitting corrosion is a rapid metal dissolution process, affected by the applied electrochemical potential, concentration of halides, microstructure, and electrolyte temperature [8,9]. At the pit initiation stage, all pits are considered to be metastable, followed by either re-passivation or the formation of stable pits [10,11]. The development of stable pits requires a critical pitting potential (Epit) and minimum critical pitting temperature (CPT) [12,13]. Changes in exposure temperature typically do not affect pit morphology, but the applied potential, microstructure condition, and Cl− concentration can influence the resulting pit shape [1,9]. In duplex stainless steel, the pit morphology is also influenced by the ratio, size, and distribution of the austenite and ferrite crystallographic phases [14,15].
Ferritic stainless steels have a low thermal expansion, high yield strength and stiffness, and good deformation behaviour, with excellent stress corrosion cracking (SCC) resistance [16,17]. Type 420 ferritic stainless steel is a hardenable stainless steel grade, with a Cr concentration between 12% and 14% and a high carbon content [18]. Type 420 is typically in service with a martensitic microstructure, obtained via austenitisation treatment and quenching from annealed microstructures. The final microstructure contains chromium carbides, and the corrosion behaviour of this microstructure condition is dependent on austenitisation temperature, quench rate, and tempering treatments [19,20]. In its annealed condition, Type 420 stainless steel has a ferritic microstructure, which makes the microstructure easier to machine into shapes and structures [21]. After austenitisation treatment, the chromium carbides generally dissolve into the matrix, with subsequent tempering applied in order to improve the ductility and toughness by changing the microstructure, secondary phase and carbide distribution, and the fraction of the retained austenite [22,23,24].
The work reported in this paper provides insight into the pitting corrosion behaviour of annealed Type 420 ferritic stainless steel via the application of a bipolar electrochemistry approach. The aim is to obtain information about the relationship between the electrochemical potential and the corrosion behaviour of this alloy, with a focus on determining pit nucleation sites and the associated growth kinetics.

2. Materials and Experimental Methods

Solution annealed Type 420 stainless steel with a composition (wt %) of 13.7 Cr, 0.46 C, 0.47 Si, 0.39 Mn, and Fe (bal.) was used in this study. The stainless steel had a hardness of 198 ± 4 HV0.5, indicating a soft annealed microstructure condition. Micro hardness was measured with a Buehler Micromet Tester, using an applied load of 4.903 N (HV0.5), with the mean and standard deviation determined with five measurements.
Figure 1a shows the setup for the bipolar electrochemistry testing. With a sufficiently high potential across the BPE, oxidation reactions occur close to the negative feeder electrode, and vice versa for the reduction reactions which occur close to the positive feeder electrode. Two different BPE samples were used for carrying out the bipolar experiments, with dimensions of 30 × 10 × 1.2 mm3 (length × width × thickness) and 50 × 20 × 1.2 mm3. The BPE samples were mounted in Araldite resin, with the exposed area ground to 1200 grit, followed by polishing to a 1 μm diamond paste finish. The shorter (30 mm) sample was used to explore the pit nucleation sites, with the longer (50 mm) sample then applied for studying pit growth, demonstrating the versatility of this technique.
The 30 mm long BPE had a distance of 60 mm between the feeder electrodes. For the 50 mm BPE, the distance between the two feeder electrodes was set to 75 mm. Both BPEs were centred between the two feeder electrodes, with an applied potentio-static potential of 10 V acting on the feeder electrodes. The electrolyte was 0.1 M HCl with a volume of 200 mL, with experiments carried out up to 30 min. The surface area of each platinum feeder electrode was 4 cm2.
Figure 1b demonstrates the potential gradient acting along the BPE, which was measured using a Luggin capillary connected to a saturated calomel electrode (SCE). The Luggin capillary was set ≈1 mm above the centre line of the BPE surface, which was in turn connected to a copper wire and an IVIUM-Compactstat in order to determine the local potential. To measure the local potential during the bipolar electrochemistry experiments, the open circuit potential (OCP) was stabilised first, and the power supply of the feeder electrodes was then switched on. The reported potential change on the y-axis is the difference of the measured potential with respect to OCP, which can be described as the acting over-potential along the BPE.
All Type 420 ferritic BPE samples were washed with soap and dried in hot air after completing the bipolar electrochemistry experiments. The surface morphology of the tested samples was measured via laser scanning confocal microscopy, using a Keyence VK-X200K (Keyence Corporation, Osaka, Japan). For the electron backscatter diffraction (EBSD) and angle selective backscatter (AsB) microstructure analyses, the samples were ground to 4000 grit and polished to a 0.25 μm diamond paste finish, followed by fine polishing with oxide polishing suspensions (OPS) of colloidal silica. A Zeiss Sigma VP FEG-SEM (Zeiss, Jena, Germany) was used for scanning electron microscopy (SEM) imaging at 1.5 kV, with high-resolution EBSD analysis carried out at 15 kV and a step size of 33 nm. An FEG-FEI Quanta 250 SEM (FEI Company, Hillsboro, OR, USA) was used for the energy dispersive x-ray (EDX) elemental analysis using 20 kV.

3. Results and Discussion

The microstructure of Type 420 stainless steel is shown in Figure 2a, highlighting the different grain orientations of the annealed ferritic matrix. A small number of dark spots, shown by the arrows in Figure 2, were present in the micrograph, possibly due to the metallographic preparation method (OPS polish). Chromium carbides were omnipresent in the matrix, with Figure 2b showing typical morphologies in the form of one smaller (≈100 nm) and three larger ellipsoids (≈800 nm). The microstructure had typical chromium carbide sizes of up to ≈ 2 μm.
Figure 3a shows a SEM image of the Type 420 stainless steel with carbides present at triple junctions, along grain boundaries, and within grains, with the parameters of the possible carbides in this material listed in Table 1. The EDX images in Figure 3 confirm that all observed particles were chromium-rich carbides, with some containing higher Mn contents. The latter is related to the process annealing treatment, where Mn diffuses into the M23C6 [25]. M23C6 was homogenously distributed in the matrix, with the EBSD map in Figure 3b showing the carbides, identified as Cr23C6, Cr3C2, and Cr7C3. The other two carbide types (Cr3C, CrC) were not observed here in our study.
Chromium carbides and the ferritic matrix typically form via austenitisation heat treatments and subsequent cooling [26]. During the annealing process, M3C precipitate first and then transform into M7C3, and finally into M23C6 [27]. For long annealing times, metastable carbides either dissolve or transform into Cr23C6, which is the most thermodynamically stable carbide phase in this system [25]. The chromium carbide sizes shown in Figure 3b decrease from Cr23C6, Cr7C3 to Cr3C2 as the Cr3C2 is formed first.

3.1. Pit Nucleation Sites

Bipolar electrochemistry testing was carried out to identify the pit nucleation sites in this material. Figure 4 shows the 30 mm long BPE electrode with three distinctive regions highlighted after bipolar testing. From the BPE oxidation edge on the left to the reduction edge on the right, the overall corrosion response showed crevice corrosion at the edges, pitting corrosion surrounded by general corrosion, general corrosion only, and a large cathodic region.
All observed pits were open pits without lacy metal covers. The region containing pits had a length of 6 mm measured from the oxidation edge, with general corrosion thereafter observed until a depth of 17 mm was reached. The remaining 13 mm of the BPE was the cathodic region. The boundary between the anodic and cathodic site was not in the centre of the BPE electrode, due to non-symmetric differences in the anodic vs. cathodic current response. By comparing the corrosion response along the BPE and the potential distribution from Figure 1b, the critical pitting potential was estimated to be around +0.9 VOCP for this sample.
To identify the earliest onset of pit nucleation, the bipolar polarisation was applied for 5 s only, with Figure 5a highlighting the typical pit nucleation sites (labelled with arrows). From the EDX maps, a strong Cr and C signal confirms that the observed particles here were all chromium rich carbides. Localised corrosion was initiated at the interface between chromium carbides and the matrix, caused by either micro-galvanic effects [21] or Cr depletion [28], in combination with occluded crevice geometries around some of these carbides [29]. Chromium carbides are typically more electrochemical noble, so they can easily act as cathodes, and the surrounding matrix can act as the anode [21]. The associated Cr depleted regions are typically caused by Cr diffusion to form chromium carbides. These regions contain significantly reduced Cr concentrations and are not able to form stable passive films, especially in low Cr containing ferritic stainless steels [28]. Figure 5b shows the EDX map of a pit with a diameter of 5 μm, showing a large number of chromium carbides inside the dissolved pit volume. Chromium carbides dropped into the formed pit cavity after the surrounding stainless steel was corroded away, with the carbides remaining inside this cavity due to their higher electrochemical nobility.
Figure 6 summarises the images of the region containing pitting corrosion after 5 min of bipolar electrochemistry exposure. Figure 6a shows a pit with a diameter of 80 μm, surrounded by small voids which are indicative of the nucleation of several metastable pits. The circumference of the pit contained a ring of general corrosion. Pit growth ultimately results in the formation of an aggressive electrolyte (low pH, high Cl− concentration) inside the pit [30]. The electrolyte can diffuse out and corrode the matrix surrounding the pit mouth, before the solution dilutes. Figure 6b shows a higher magnification image of the pit mouth, with chromium carbides protruding out of the matrix, supporting the notion of their higher corrosion resistance.
Figure 6c provides another SEM image of the outer part of the corroded pit circumference, with Figure 6d showing an SEM image of the pit bottom. Grains with different heights can be seen, with larger sized chromium carbides at the surface. The cavities near the chromium carbides point towards the localised dissolution of the Type 420 matrix.

3.2. General Corrosion Behaviour

Figure 7 shows SEM images of the general corrosion region in Figure 4 after polarising the BPE for 30 min. A large number of chromium carbides are also here protruding out of the matrix in the corroded regions. Individual grains of the corroded matrix can be seen, with Figure 7b showing chromium carbides with typical sizes of ≈ 200 nm located at a grain boundary. The spherical shaped carbides remained at the grain surface, and ellipsoid chromium carbides were embedded within the matrix. Grains with different heights were observed within the general corrosion region, which were covered by fin-like surface structures, as shown in Figure 7c,d. The presence of these fins points towards the formation of α-FeOOH with sedimentary amorphous layers, which have been reported to be either whisker, rod, or fin shaped [31]. α-FeOOH is generally transformed from γ-FeOOH, via the formation of Fe3O4 [32,33]. The presence of γ-FeOOH and α-FeOOH can improve the corrosion resistance, as they are stable and protective passive films. However, Fe3O4 reduces the corrosion resistance, as highly conductive properties result in cathode, which accelerates the corrosion in the matrix [34,35].
Figure 8 shows images of the cathodic site of the BPE, containing discrete particles. The particle length varied from 10 μm to 50 μm, and their presence is believed to be related to local electrochemical reactions. The EDX spectrum showed carbon, chloride, and oxygen rich particles, which could be easily removed by soap water cleaning.
Cl2 and HClO are generated from electrochemical reactions in HCl electrolyte under high applied potentials [36]. Dissolved Cl2 gas results in highly active oxidants: Cl2O, ClO2, ClO−, HClO, Cl*, and HO2* (* indicates reactive free radicals) [36]. These highly active oxidants can diffuse to the cathodic sites and be deposited on the sample surface via electrochemical deposition reactions.

3.3. Pitting Corrosion Kinetics

The advantage of applying bipolar electrochemistry to pitting corrosion studies lies in the ability to observe pit nucleation and growth along the surface of the BPE, i.e., along the acting potential gradient. This allows researchers to investigate the earliest onset of pitting, the determination of pit growth kinetics, and associated pit coalescence.
An example of this is shown in Figure 9, which shows the 50 mm long BPE after exposure to bipolar electrochemistry for 30 min. Here, on the longer electrode, four distinct regions can clearly be seen along the BPE surface, labelled A–D. The left side of the BPE is the BPE oxidation edge, which had the highest degree of localised corrosion. Closer inspection of the regions revealed the presence of a large crevice around the edge of the sample and pitting corrosion surrounded by general corrosion, followed by a region with pitting corrosion only, general corrosion only, and no corrosion at all. The latter is indicative of the cathodic region. All the observed pits were open pits with a lower applied potential, resulting in general corrosion.
Figure 10a shows an optical image of the oxidation edge, highlighting the crevice, and both regions containing pits (A, B) from Figure 9. Close to the oxidation edge, pitting with general corrosion can be observed with a higher pit density. At a lower acting potential (further to the right), only pitting corrosion can be observed, with far fewer nucleated pits. Figure 10b shows the 3D images of these regions, supporting the presence of a heavily corroded crevice, which developed between the BPE and the surrounding resin.
The pit covered region in Figure 9 was divided into seven sub-regions, each with a size of 1.5 × 4 mm2 (length × width), as shown in Figure 11a. Region I represented the highest potential close to the oxidation edge, with region VII representing the lowest applied potential, 9 to 10.5 mm away from the oxidation edge. Region I contained the pit region with crevice, with regions II to IV showing pitting corrosion with general corrosion, whereas in regions V to VII, only pitting corrosion was observed. The pit density was reduced from region I to VII, with pits clearly coalesced in regions I, II, and III. The presence of numerous pits close to each other was found in regions IV and V, and predominantly isolated pits were found in regions VI and VII.
Figure 11b shows the total dissolved pit volume in each of the seven regions, with the highest volume determined in region I and the lowest in region VII. The pit volume reduced exponentially from the BPE oxidation edge to the centre. Since the potential was linearly distributed along the length of the sample, an exponential potential vs. current relationship could be assumed [37].
Figure 12a gives the number of pits with their corresponding pit volumes as a function of the seven investigated regions, with the reported data obtained via laser confocal microscopy. From regions III to VII, i.e., along a decreasing potential, the number and volume of pits decreased. Regions I and II gave a slightly different response, with fewer pits but typically larger volumes. This observation is linked to the presence of a crevice in region I and the coalescence of larger pits in regions closer to the oxidation edge. From regions IV to VII, the pit numbers and the pit volumes were both clearly reduced, following the expected trend of fewer and smaller pits at lower applied potentials.
Figure 12a describes the sizes of all pits found in regions I to VII, providing information about the total number of pits and their size distributions. The largest pits in regions II to VII had maximum values of 10+6.7 (0.005 mm3) to 10+7 μm3 (0.01 mm3). Since the exposure time was constant for all regions, a lower slope here indicated that more pits with smaller volumes grew, pointing towards a higher pit nucleation frequency. The overall shapes of all the curves shown in Figure 12a had similar features. Most of the curves contained two kinks, with one around a pit volume of 10+6.2 μm3 (≈0.002 mm3) and the second around 10+6.6 μm3 (≈0.004 mm3), defined by the different slopes in Figure 12a. These are also highlighted by the two horizontal lines.
The first kink can be explained for pits transforming from metastable to stable pit volumes, as the pit depth and overall volume act as diffusion lengths to stabilise pit growth [38]. The number of pits with stable and metastable volumes was not the same for all regions. The second kink possibly indicates the development of champion pits or pits that coalesced, resulting in significantly larger pit volumes. If we assume hemispherical pit shapes, the measured pit volumes would translate to a depth of 100 μm for achieving stable pit growth in this material. This means that at least two distinct populations of pits were present, defined by the observed critical volume. A number of smaller pits with dimensions up to the critical volume of 10+6.2 μm3 (≈0.002 mm3), followed by a larger accumulation of pits that were slightly larger, are present, evident by the lower slope of the curve defining larger pits.
Figure 12b gives the average pit growth factor calculated from the deepest ten pits in each of the seven regions, with the error bar defined by the standard deviation of these measurements. The deepest pits were assumed to nucleate at t = 0 s, with pit growth kinetics following the power law relationship in Equation (1) [39]:
d = Ktb
where (d) is the pit depth (μm), t is time (s), and K and b are experimental constants. The latter are influenced by the temperature and pH value of the electrolyte, with typical values of (b) from 0.3 to 0.5. If we assume the value of b = 0.5, with d measured from the laser confocal microscopy, the value of K can be calculated for each region.
The obtained K values in Figure 12b confirm that the pit growth kinetics here were independent of the acting potential in each region. The 10 largest pits in each region had similar dimensions, resulting in pit growth factors (K) of around 2.9 from region II to IV. In region I, K was far lower at 2.5. The difference in pit growth kinetics in region (I) was caused by several pits merging together, reducing the number of larger pits seen in the overall distribution in Figure 12a. The presence of crevice corrosion also affected the maximum current up-take in this region, which most likely also contributed to a reduced pit growth factor. The coalescence of pits is also expected to affect the acting local potential, in parallel influencing pit growth kinetics [40].
The results reported in this investigation demonstrate the versatility of bipolar electrochemistry testing for corrosion research, providing access to a broad range of corrosion behaviours and mechanisms. In contrast, by using the conventional three-electrode polarisation set-up, a similar breadth of results can only be achieved by undertaking a large number of potentio-static polarisation experiments at different set potentials. With the bipolar screening technique, the occurrence of metastable pits, associated critical pitting potentials, and pit growth factors, as well as pit nucleation sites, can be measured along one sample surface, in combination with far shorter experimental exposure times. The bipolar technique is, however, neither perfect nor fully understood yet, but the described advantages certainly warrant the further application and exploration of this method as a corrosion assessment tool.

4. Conclusions

(1)
Bipolar electrochemistry allows a broad range of corrosion responses to be observed in a single experiment.
(2)
Cr23C6, Cr3C2, and Cr7C3 are present in Type 420 stainless steel, with pits nucleating near these chromium-rich carbides.
(3)
Pit nucleation, growth, and coalescence have been observed.
(4)
Pit growth kinetics are independent of the acting potential.
(5)
A critical pit volume for the transition from metastable to stable pits has been determined.

Author Contributions

Y.Z.: conceptualization, methodology, validation, formal analysis, investigation, data curation, writing—original draft, visualization, funding acquisition; D.L.E.: conceptualization, methodology, validation, formal analysis, investigation, funding acquisition, writing—review and editing, supervision. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Zhou, Y.; Engelberg, D.L. Application of a modified bi-polar electrochemistry approach to determine pitting corrosion characteristics. Electrochem. Commun. 2018, 93, 158–161. [Google Scholar] [CrossRef]
  2. Munktell, S.; Tydén, M.; Högström, J.; Nyholm, L.; Björefors, F. Bipolar electrochemistry for high-throughput corrosion screening. Electrochem. Commun. 2013, 34, 274–277. [Google Scholar] [CrossRef]
  3. Pébère, N.; Vivier, V. Local Electrochemical Measurements in Bipolar Experiments for Corrosion Studies. ChemElectroChem 2016, 3, 415–421. [Google Scholar] [CrossRef]
  4. Crooks, R.M. Principles of Bipolar Electrochemistry. ChemElectroChem 2016, 3, 357–359. [Google Scholar] [CrossRef]
  5. Wiesener, K.; Ohms, D.; Benczúr-Ürmössy, G.; Berthold, M.; Haschka, F. High power metal hydride bipolar battery. J. Power Sources 1999, 84, 248–258. [Google Scholar] [CrossRef]
  6. Sequeira, C.A.C.; Cardoso, D.S.P.; Gameiro, M.L.F. Bipolar Electrochemistry, a Focal Point of Future Research. Chem. Eng. Commun. 2016, 203, 1001–1008. [Google Scholar] [CrossRef]
  7. Qi, Z.; You, S.; Ren, N. Wireless Electrocoagulation in Water Treatment Based on Bipolar Electrochemistry. Electrochim. Acta. 2017, 229, 96–101. [Google Scholar] [CrossRef]
  8. Yi, Y.; Cho, P.; Al Zaabi, A.; Addad, Y.; Jang, C. Potentiodynamic polarization behaviour of AISI type 316 stainless steel in NaCl solution. Corros. Sci. 2013, 74, 92–97. [Google Scholar] [CrossRef]
  9. Krawczyk, B.; Cook, P.; Hobbs, J.; Engelberg, D. Corrosion Behavior of Cold Rolled Type 316L Stainless Steel in HCl Containing Environments. Corrosion 2017, 73, 1346. [Google Scholar] [CrossRef]
  10. Moayed, M.H.; Newman, R.C. Evolution of current transients and morphology of metastable and stable pitting on stainless steel near the critical pitting temperature. Corros. Sci. 2006, 48, 1004–1018. [Google Scholar] [CrossRef]
  11. Al Saadi, S.; Yi, Y.; Cho, P.; Jang, C.; Beeley, P. Passivity breakdown of 316L stainless steel during potentiodynamic polarization in NaCl solution. Corros. Sci. 2016, 111, 720–727. [Google Scholar] [CrossRef]
  12. Pistorius, P.C.; Burstein, G.T. Metastable Pitting Corrosion of Stainless Steel and the Transition to Stability. Philos. Trans. R. Soc. A Math. Phys. Eng. Sci. 1992, 341, 531–559. [Google Scholar]
  13. Laycock, N.J. Metastable Pitting and the Critical Pitting Temperature. J. Electrochem. Soc. 1998, 145, 2622. [Google Scholar] [CrossRef]
  14. Örnek, C.; Léonard, F.; McDonald, S.A.; Prajapati, A.; Withers, P.J.; Engelberg, D.L. Time-dependent in situ measurement of atmospheric corrosion rates of duplex stainless steel wires. npj Mater. Degrad. 2018, 2, 1–15. [Google Scholar]
  15. Eguchi, K.; Burnett, T.L.; Engelberg, D.L. X-Ray tomographic characterisation of pitting corrosion in lean duplex stainless steel. Corros. Sci. 2019, 165, 108406. [Google Scholar] [CrossRef]
  16. Bond, A.P.; Dundas, H.J. Effects of Composition on the Stress Corrosion Cracking of Ferritic Stainless Steels. Corrosion 2013, 24, 344–352. [Google Scholar] [CrossRef]
  17. Newberg, R.T.; Uhlig, H.H. Stress Corrosion Cracking of 18% Cr Ferritic Stainless Steels. J. Electrochem. Soc. 1972, 119, 981. [Google Scholar] [CrossRef]
  18. Yin, Z.F.; Wang, X.Z.; Liu, L.; Wu, J.Q.; Zhang, Y.Q. Characterization of corrosion product layers from CO2corrosion of 13Cr stainless steel in simulated oilfield solution. J. Mater. Eng. Perform. 2011, 20, 1330–1335. [Google Scholar] [CrossRef]
  19. Anantha, K.H.; Örnek, C.; Ejnermark, S.; Medvedeva, A.; Sjöström, J.; Pan, J. In Situ AFM Study of Localized Corrosion Processes of Tempered AISI 420 Martensitic Stainless Steel: Effect of Secondary Hardening. J. Electrochem. Soc. 2017, 164, C810–C818. [Google Scholar] [CrossRef]
  20. Lei, X.; Feng, Y.; Zhang, J.; Fu, A.; Yin, C.; Macdonald, D.D. Impact of Reversed Austenite on the Pitting Corrosion Behavior of Super 13Cr Martensitic Stainless Steel. Electrochim. Acta. 2016, 191, 640–650. [Google Scholar] [CrossRef]
  21. Anantha, K.H.; Örnek, C.; Ejnermark, S.; Medvedeva, A.; Sjöström, J.; Pan, J. Correlative Microstructure Analysis and In Situ Corrosion Study of AISI 420 Martensitic Stainless Steel for Plastic Molding Applications. J. Electrochem. Soc. 2017, 164, C85–C93. [Google Scholar] [CrossRef]
  22. Candelaria, A.F.; Pinedo, C.E. Influence of the heat treatment on the corrosion resistance of the martensitic stainless steel type AISI 420. J. Mater. Sci. Lett. 2003, 22, 1151–1153. [Google Scholar] [CrossRef]
  23. Nakagawa, H.; Miyazaki, T. Effect of retained austenite on the microstructure and mechanical properties of martensitic precipitation hardening stainless steel. J. Mater. Sci. 1999, 34, 3901–3908. [Google Scholar] [CrossRef]
  24. de Moor, E.; Lacroix, S.; Clarke, A.J.; Penning, J.; Speer, J.G. Effect of retained austenite stabilized via quench and partitioning on the strain hardening of martensitic steels. Metall. Mater. Trans. A Phys. Metall. Mater. Sci. 2008, 39, 2586–2595. [Google Scholar] [CrossRef]
  25. Godec, M.; Balantič, D.A.S. Coarsening behaviour of M23C6 carbides in creep-resistant steel exposed to high temperatures. Sci. Rep. 2016, 6, 29734. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  26. Du Toit, M.; Van Rooyen, G.T.; Smith, D. Heat-affected zone sensitization and stress corrosion cracking behaviour of 12% chromium type 1.4003 ferritic stainless steel. Weld. World 2007, 51, 41–50. [Google Scholar] [CrossRef] [Green Version]
  27. Bjärbo, A.; Hättestrand, M. Complex carbide growth, dissolution, and coarsening in a modified 12 pet chromium steel-an experimental and theoretical study. Metall. Mater. Trans. A Phys. Metall. Mater. Sci. 2001, 32, 19–27. [Google Scholar] [CrossRef]
  28. Gellings, P.J.; de Jongh, M.A. Grain boundary oxidation and the chromium-depletion theory of intercrystalline corrosion of austenitic stainless steels. Corros. Sci. 1967, 7, 413–421. [Google Scholar] [CrossRef] [Green Version]
  29. Jung, K.; Oh, K.; Nam, D.H.; Ahn, S.; Oh, S.; Kwon, H. Effects of Centerline Segregation of Cr Carbides and Non-Metallic Inclusions on the Pitting Corrosion of Fe-13Cr-0.3C Stainless Steel Produced by Continuous Casting and Strip Casting. Corrosion 2017, 73, 979–987. [Google Scholar] [CrossRef]
  30. Frankel, G.S.; Stockert, L.; Hunkeler, F.; Boehni, H. Metastable pitting of stainless steel. Corrosion 1987, 43, 429–436. [Google Scholar] [CrossRef]
  31. Liu, J.; Wong, L.M.; Wong, L.H.; Chiam, S.Y.; Li, S.F.; Ren, Y. Immobilization of dye pollutants on iron hydroxide coated substrates: kinetics, efficiency and the adsorption mechanism. J. Mater. Chem. A 2016, 4, 13280–13288. [Google Scholar] [CrossRef]
  32. N Dai, N.; Zhang, J.; Chen, Q.; Yi, B.; Cao, F.; Zhang, J. Effect of the direct current electric field on the initial corrosion of steel in simulated industrial atmospheric environment. Corros. Sci. 2015, 99, 295–303. [Google Scholar] [CrossRef]
  33. Asami, K.; Kikuchi, M. In-depth distribution of rusts on a plain carbon steel and weathering steels exposed to coastal-industrial atmosphere for 17 years. Corros. Sci. 2003, 45, 2671–2688. [Google Scholar] [CrossRef]
  34. Hao, L.; Zhang, S.; Dong, J.; Ke, W. Evolution of corrosion of MnCuP weathering steel submitted to wet/dry cyclic tests in a simulated coastal atmosphere. Corros. Sci. 2012, 58, 175–180. [Google Scholar] [CrossRef]
  35. Stratmann, M.; Bohnenkamp, K.; Ramchandran, T. The influence of copper upon the atmospheric corrosion of iron. Corros. Sci. 1987, 27, 905–926. [Google Scholar] [CrossRef]
  36. Ignatov, I.; Mosin, O.; Gluhchev, G.; Karadzhov, S.; Miloshev, G.; Ivanov, N. Studying Electrochemically Activated NaCl Solutions of Anolyte and Catholyte by Methods of Non-Equilibrium Energy Spectrum (NES) and Differential Non-Equilibrium Energy Spectrum (DNES). J. Med. Physiol. Biophys. 2016, 20, 13–23. [Google Scholar]
  37. Duval, J.; Kleijn, J.M.; Van Leeuwen, H.P. Bipolar electrode behaviour of the aluminium surface in a lateral electric field. J. Electroanal. Chem. 2001, 505, 1–11. [Google Scholar] [CrossRef]
  38. Tian, W.; Li, S.; Du, N.; Chen, S.; Wu, Q. Effects of applied potential on stable pitting of 304 stainless steel. Corros. Sci. 2015, 93, 242–255. [Google Scholar] [CrossRef]
  39. Ernst, P.; Newman, R.C. Pit growth studies in stainless steel foils I. Introduction and pit growth kinetics. Corros. Sci. 2002, 44, 927–941. [Google Scholar]
  40. Laycock, N.J.; Krouse, D.P.; Hendy, S.C.; Williams, D.E. Computer Simulation of Pitting Corrosion of Stainless Steels. Electrochem. Soc. Interface 2014, 23, 65–71. [Google Scholar] [CrossRef]
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Figure 1. (a) A schematic diagram of the bipolar electrochemistry setup, and (b) the measured potential distribution on the bipolar electrode (BPE) (30 mm length) using a Luggin capillary connected to the saturated calomel electrode (SCE).
Figure 1. (a) A schematic diagram of the bipolar electrochemistry setup, and (b) the measured potential distribution on the bipolar electrode (BPE) (30 mm length) using a Luggin capillary connected to the saturated calomel electrode (SCE).
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Figure 2. (a) AsB SEM image of Type 420 stainless steel with the arrows showing voids, and (b) typical size and shape of chromium carbides.
Figure 2. (a) AsB SEM image of Type 420 stainless steel with the arrows showing voids, and (b) typical size and shape of chromium carbides.
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Figure 3. (a) SEM image of Type 420 ferritic stainless steel with EDX elemental maps of Cr, Fe, C, and Mn, and (b) high-resolution EBSD map highlighting chromium carbides (BCC = body centred cubic, ferritic matrix).
Figure 3. (a) SEM image of Type 420 ferritic stainless steel with EDX elemental maps of Cr, Fe, C, and Mn, and (b) high-resolution EBSD map highlighting chromium carbides (BCC = body centred cubic, ferritic matrix).
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Figure 4. Appearance of the 30 mm long BPE after bipolar electrochemistry testing for 30 min, with the left side showing large pits at the oxidation edge and the right side showing the reduction edge.
Figure 4. Appearance of the 30 mm long BPE after bipolar electrochemistry testing for 30 min, with the left side showing large pits at the oxidation edge and the right side showing the reduction edge.
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Figure 5. (a) SEM images with EDX maps of Type 420 stainless steel after 5 s exposure time, with the arrow highlighting a pit nucleation site, and (b) EDX maps of a pitting with 5 um diameter with corresponding EDX maps.
Figure 5. (a) SEM images with EDX maps of Type 420 stainless steel after 5 s exposure time, with the arrow highlighting a pit nucleation site, and (b) EDX maps of a pitting with 5 um diameter with corresponding EDX maps.
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Figure 6. (a) SEM image of a pit with a corroded circumference, (b) higher magnification image of the corroded circumference of the pit, (c) the corroded outer part of the pit ring, and (d) SEM image of the pit bottom.
Figure 6. (a) SEM image of a pit with a corroded circumference, (b) higher magnification image of the corroded circumference of the pit, (c) the corroded outer part of the pit ring, and (d) SEM image of the pit bottom.
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Figure 7. General corrosion on the BPE, with (a) carbides protruding out of the matrix, (b) grains with different heights and carbides at grain boundaries, and (c,d) the presence of FeOOH.
Figure 7. General corrosion on the BPE, with (a) carbides protruding out of the matrix, (b) grains with different heights and carbides at grain boundaries, and (c,d) the presence of FeOOH.
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Figure 8. SEM images and corresponding EDX images of the cathodic region on the BPE.
Figure 8. SEM images and corresponding EDX images of the cathodic region on the BPE.
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Figure 9. The surface appearance of the 50 mm long BPE after 30 min bipolar exposure.
Figure 9. The surface appearance of the 50 mm long BPE after 30 min bipolar exposure.
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Figure 10. (a) The optical image of the pitting corrosion region on BPE (50 mm), and (b) the corresponding 3D laser confocal image of this region.
Figure 10. (a) The optical image of the pitting corrosion region on BPE (50 mm), and (b) the corresponding 3D laser confocal image of this region.
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Figure 11. (a) Overview of the seven pit covered regions, with (b) the corresponding pit volumes measured using laser confocal microscopy.
Figure 11. (a) Overview of the seven pit covered regions, with (b) the corresponding pit volumes measured using laser confocal microscopy.
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Figure 12. (a) The relationship between pit number and corresponding pit volumes, and (b) the corresponding pit growth factor (K) for each region (I-VII) in Figure 11.
Figure 12. (a) The relationship between pit number and corresponding pit volumes, and (b) the corresponding pit growth factor (K) for each region (I-VII) in Figure 11.
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Table
Table 1. Database with crystallographic parameters for electron backscatter diffraction (EBSD) phase identification from Inorganic Crystal Structure Database (ICSD) and the Aztec EBSD software (Version 4.2, Oxford Instruments, Abingdon, UK).
Table 1. Database with crystallographic parameters for electron backscatter diffraction (EBSD) phase identification from Inorganic Crystal Structure Database (ICSD) and the Aztec EBSD software (Version 4.2, Oxford Instruments, Abingdon, UK).
PhaseABCAlphaBetaGammaSpace GroupDatabase
Fe3C5.11 Å6.78 Å4.54 Å90.00°90.00°90.00°62HKL
Iron bcc2.87 Å2.87 Å2.87 Å90.00°90.00°90.00°229HKL
Cr3C5.12 Å6.80 Å4.58 Å90.00°90.00°90.00°62ICSD
Cr3C25.53 Å11.49 Å2.83 Å90.00°90.00°90.00°62ICSD
Cr7C34.53 Å7.01 Å12.14 Å90.00°90.00°90.00°62ICSD
Cr23C610.66 Å10.66 Å10.66 Å90.00°90.00°90.00°225ICSD
CrC4.03 Å4.03 Å4.03 Å90.00°90.00°90.00°225ICSD

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Zhou, Y.; Engelberg, D.L. On the Application of Bipolar Electrochemistry to Characterise the Localised Corrosion Behaviour of Type 420 Ferritic Stainless Steel. Metals 2020, 10, 794. https://doi.org/10.3390/met10060794

AMA Style

Zhou Y, Engelberg DL. On the Application of Bipolar Electrochemistry to Characterise the Localised Corrosion Behaviour of Type 420 Ferritic Stainless Steel. Metals. 2020; 10(6):794. https://doi.org/10.3390/met10060794

Chicago/Turabian Style

Zhou, Yiqi, and Dirk Lars Engelberg. 2020. "On the Application of Bipolar Electrochemistry to Characterise the Localised Corrosion Behaviour of Type 420 Ferritic Stainless Steel" Metals 10, no. 6: 794. https://doi.org/10.3390/met10060794

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