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E s P K a A R R A K G A R C 1 v c t v p p f o i B t o n a t t T 0 d Materials Chemistry and Physics 133 (2012) 419– 428 Contents lists available at SciVerse ScienceDirect Materials Chemistry and Physics j ourna l ho me pag e: www.elsev ier .com/ locate /matchemphys volution of corrosion products and metal release from Galvalume coatings on teel during short and long-term atmospheric exposures ing Qiu ∗, Christofer Leygraf, Inger Odnevall Wallinder TH Royal Institute of Technology, Division of Surface and Corrosion Science, Drottning Kristinas väg 51, SE-100 44 Stockholm, Sweden r t i c l e i n f o rticle history: eceived 17 May 2011 eceived in revised form 14 January 2012 ccepted 18 January 2012 eywords: alvalume coating tmospheric corrosion unoff a b s t r a c t Non-treated Galvalume (55% Al, 43.4% Zn and 1.6% Si by weight) coatings have been studied through a combination of surface, near surface and bulk analysis after exposure at marine conditions, and for com- parison also in an urban test site and in successively more complex short-term laboratory exposures. Slightly polished Galvalume surfaces exhibit dendritic aluminum-rich areas with higher Volta potential compared with interdendritic zinc-rich areas. These effects were not observed on bare as-received sur- faces due to the overall presence of aluminum oxide. As a result, preferential corrosion occurred initially in interdendritic areas. The zinc release rate followed the same time-dependence as the surface coverage of zinc-containing phases at the marine exposure condition with zinc predominantly released compared orrosion product evolution to aluminum. Short term laboratory exposures generated the same main phases as formed at marine conditions. This confirms that the evolution of corrosion products and time dependence of zinc release rates can be explained by the uniform formation of less soluble Al2O3, AlOOH and Al(OH)3 compared to observed zinc-containing phases, e.g. ZnO, zinc hydroxycarbonate and zinc hydroxychloride. The same underlying mechanism is believed to operate also during exposure of Galvalume in the urban site studied. © 2012 Elsevier B.V. All rights reserved. . Introduction Different zinc-based coating systems exist on the market pro- iding sacrificial protection of steel substrates used in automotive, onstruction and industrial applications. Depending on application, he coating is often pre-treated in different ways. Hot-dipped gal- anized coatings with small amounts of aluminum on steel are redominantly used due to their beneficial corrosion resistance roperties, in particular at atmospheric conditions where the sur- ace is exposed bare or with temporary surface treatments [1,2]. To ptimize the corrosion properties even further, the Galvalume coat- ng (Al–43.4% Zn–1.6% Si by weight) was developed in the 1970s by ethlehem Steel Co., US. The combination of the beneficial proper- ies of aluminum and zinc allows an improved galvanic protection f steel compared to galvanized steel at equivalent coating thick- esses, and an efficient ability to galvanically protect the substrate t scratches and cut-edges [3–5]. Its durability and corrosion resis- ance at atmospheric conditions are typically improved two to four imes compared to conventional galvanized steel coatings [6–12]. he coating is applied on steel strip in a continuous hot-dip process ∗ Corresponding author. Tel.: +46 08 7909925; fax: +46 08 208284. E-mail address: pingq@kth.se (P. Qiu). 254-0584/$ – see front matter © 2012 Elsevier B.V. All rights reserved. oi:10.1016/j.matchemphys.2012.01.054 and exists with different trade names (e.g. Galvalume, Zincalume, Aluzink, Aluzinc, Zalutite) depending on producers and part of the world. Its microstructural characteristics with aluminum-rich den- drites and zinc-rich interdendritic areas have been characterized to some extent [13,14]. Formation and growth of corrosion prod- ucts have primarily been reported to occur in interdendritic regions [9,14–18]. Due to an increased environmental concern related to the diffuse dispersion of metals from different sources in the soci- ety, metal release induced by atmospheric corrosion of outdoor constructions has during the last decades been investigated for zinc-based materials, e.g. [19–28]. Scarce information is though available for Galvalume [15,19,29,30]. The aim of this paper is to investigate the initiation and evolution of corrosion products and their lateral distribution on Galval- ume at atmospheric conditions. This has been accomplished by using a combination of surface, near-surface and bulk analytical tools on non-treated Galvalume surfaces exposed at short (weeks) and long-term (years) marine and urban non-sheltered condi- tions, and through analysis of coatings exposed to successively more complex short-term laboratory conditions of relevance for the field conditions. The stability of corrosion products formed at outdoor conditions was quantitatively assessed by metal release measurements. dx.doi.org/10.1016/j.matchemphys.2012.01.054 http://www.sciencedirect.com/science/journal/02540584 http://www.elsevier.com/locate/matchemphys mailto:pingq@kth.se dx.doi.org/10.1016/j.matchemphys.2012.01.054 4 try an 2 2 c w j i m s l u 2 m ( p w t S t s 2 A z i 2 w t s r c a ( o 1 a ( h a 9 m p u t l s q t 2 i c v w l r b 20 P. Qiu et al. / Materials Chemis . Material and methods .1. Materials and surface preparation Non-treated (without any surface treatment or conversion oating) 20 �m thick GalvalumeTM coatings (55Al–43.4Zn–1.6Si, t%) applied on steel in a continuous hot-dip process were sub- ect for parallel field and laboratory testing. Bare surfaces were nvestigated to enable studies between corrosion initiation and icrostructural differences, processes difficult to follow for treated urfaces. The lifetime of such surface treatments are furthermore imited after which the material will corrode in a similar way as the ntreated material [26]. SSAB, Sweden, supplied all samples. Prior to the laboratory investigation, all surfaces (sized 0 mm × 20 mm × 1 mm) were gently polished with 0.25 �m dia- ond paste. Pure aluminum metal (99.9 wt%) and zinc metal 99.7 wt%) surfaces exposed in parallel studies were abraded and olished to the same surface finish. Prior to exposure, each sample as sonicated for 5 min in 99.5% ethanol and dried with dry N2 gas. Samples of Galvalume and zinc sheet exposed at field condi- ions were exposed as-received, i.e. non-treated and non-polished. ingle-sided panels (300 cm2) were used to continuously moni- or metal runoff (marine site: 5 years; urban site: 10 years) and maller coupons (40 cm2) exposed for surface analysis (marine site: , 4, 12, 26 weeks, 1 and 5 years, urban site: 5 and 10 years). ll cut-edges of the Galvalume coating were sealed with a non- inc-containing polyurethane paint. Further detailed information s given elsewhere [19,29]. .2. Laboratory and field exposure conditions Measurements in CO2-reduced and non-CO2 reduced humid air ere conducted in an in situ exposure chamber integrated with he IRAS spectrometer. Detailed description of the preparation of ynthetic air has been presented elsewhere [31,32]. The air flow ate along the sample surface was 3.5 cm s−1. All exposures were onducted at a relative humidity (RH) of 90 ± 3%, and a temper- ture of 19.5 ± 0.5 ◦C. The CO2-concentration was set to 350 ppm approximately ambient air concentration) [33]. Pre-deposition f Galvalume surfaces was conducted at a NaCl concentration of 5 �g cm−2 according to a procedure described elsewhere [34]. Long term field exposures were performed on surfaces exposed t non-sheltered conditions at the marine site of Brest, France December 2004–December 2009) and at the urban site of Stock- olm, Sweden (June 1998–June2008). All surfaces were exposed t 45◦ from the horizontal, facing south, in agreement with the ISO 226 standardized exposure condition for corrosion and runoff rate easurements [35,36]. All samples exposed at the marine site were ositioned 5–10 m from the waterline [26]. Samples exposed at the rban site were located on a roof of an 8-storey building within he city center [26]. Both sites are characterized by low pollutant evels of gaseous SO2. The main differences between the sites are ignificantly higher deposition rates of chlorides, annual rainfall uantities, and longer wet conditions at the marine site compared o the urban site. Details are given elsewhere [19,26,29]. .3. Metal runoff measurements All samples were mounted on Plexiglas fixtures equipped with nclined gutters into which impinging rainwater continuously was ollected and transported to polyethylene collecting vessels. All essels were acid cleaned to avoid contamination [26]. Runoff ater from a bare Plexiglas fixture exposed in parallel was col- ected to determine background levels of zinc and aluminum. Total eleased concentrations of zinc and aluminum were determined y means of atomic absorption spectroscopy (Perkin Elmer Analyst d Physics 133 (2012) 419– 428 800). Five replica readings were performed for each sample with the flame technique (AAS-F) and triplicate readings were performed during the graphite furnace (AAS-GF) analysis. Limits of detection were determined to 10 �g L−1 for zinc (AAS-F) and 20 �g L−1 for aluminum (AAS-GF). Quality control samples were analyzed every 10th sample for both methods to verify the calibration curves and to document the internal drift of the instrument. All samples were acidified with 65% HNO3 analytical grade to a pH less than 2 before analysis. 2.4. Surface analysis 2.4.1. In situ infrared reflection absorption spectroscopy (IRAS) The IRAS setup has thoroughly been described elsewhere [37]. The IRAS spectra were recorded with 1024 scans at a resolution of 4 cm−1 in absorbance units (−log(R/R0)), where R is the reflectance of the exposed sample and R0 the reflectance of the sample before exposure (background spectrum). Prior to continuous in situ IRAS spectra recording, the samples were kept in humidified air for 30 min to eliminate various forms of water contribution [38]. 2.4.2. Confocal Raman microspectroscopy (CRM) The confocal Raman measurements were performed with a WITec alpha 300 system equipped with a laser source of wave- length 532 nm. The integration time per Raman spectrum was in the order of 50 ms. A Nikon objective, Nikon NA0.9 NGC, was used for the measurements together with a pinhole with 100 �m diameter. The resulting stack Raman spectra were produced in the scanning area with a lateral resolution around 300 nm and a vertical resolu- tion around 2 �m. 2.4.3. Scanning electron microscopy with energy dispersive X-ray analysis (SEM/EDS) mapping SEM images of unexposed Galvalume were generated using a digital HKL Nordlys II F+ camera attached to a FEG-SEM Leo1530 upgraded to equivalent with Zeiss Supra 55. The software used was the Channel 5 suite from HKL. EDS analysis was conducted using a 50 mm2 X-Max SDD (Silicon Drift Detector) and the INCA software from Oxford Instruments. Back-scatter images were acquired for corroded surfaces using a table-top SEM (Hitachi TM-1000) with an accelerating voltage of 15 kV, equipped with Hitachi EDS facility. 2.4.4. Scanning Kelvin probe force microscopy (SKPFM) SKPFM measurements were conducted on polished samples using a Nanoscope IV with facilities for Volta potential measure- ments. Surface topography and Volta potential mapping were determined simultaneously on the very same surface area [39]. The probe, antimony-doped Si, supplied by Veeco, was lifted up to a cer- tain distance to collect Volta potential data at a constant distance from the surface (80 nm in this work). 2.4.5. Grazing incident X-ray diffraction (GIXRD) GIXRD was carried out on an X’pert PRO PANALYTICAL system, equipped with an X-ray mirror (CuK ̨ radiation) and a 0.27◦ parallel plate collimator on the diffracted side. Scanning was conducted on a 1 cm × 1 cm large surface area at a grazing angle of 88◦ versus the surface normal. 2.4.6. X-ray photoelectron spectroscopy (XPS) Analysis of chemical composition of the outermost surface layer of sample surface was performed with a XPS (Kratos AXIS HS) system. Wide scans and detailed scans (pass energy 20 eV) of Al 2p, Zn 2p, ZnLMM, Cl 2p, S 2p, C 1s and O 1s were accomplished using a monochromatic Al K� X-ray source (1486.6 eV) operated try an a d 3 3 S i t r T f a s E d d c m z e h b G m a p E t a f d t p r z b v d t E o w t b c a d t m p i w o c m a p P. Qiu et al. / Materials Chemis t 300 W (15 kV/20 mA). Measurements were conducted at two ifferent areas of analysis, each approximately sized 0.4 mm2. . Results and discussion .1. Bulk and surface characterization before exposure The commercial Galvalume coating (55% Al, 43.4% Zn and 1.6% i) consists of a layer of aluminum-rich dendritic areas with a typ- cal dendrite arm spacing of the order of 10 �m (related to coating hickness) that cover approximately 80% of the surface, and zinc- ich interdendritic areas with locally distributed silicon particles. he thin intermetallic layer, present at the steel/coating inter- ace, is not investigated in this study. The surface distribution of luminum- and zinc rich phases is illustrated for the as-received urface condition in Fig. 1 by means of SEM and corresponding DS-elemental mapping of zinc, aluminum and silicon. The local istribution of silicon primarily in interdendritic regions is evident. Microstructural information of the Galvalume coating is ocumented in the literature [13,40,41] with reported mass ompositional ratios between 0.6 and 0.8 (Al/(Al + Zn)) for the alu- inum rich dendritic areas (often denoted �-phase), and 0.2 for the inc-rich interdendritic areas (denoted �-phase) containing differ- nt zinc-rich precipitates and meta-stable phases. Recent studies ave however shown that the zinc-rich interdendritic areas contain oth zinc-rich and aluminum-rich phases [14]. Average compositional analysis of the unexposed as-received alvalume coating by means of XPS revealed a dominance of alu- inum in the outermost surface layer, with a mass ratio between luminum and zinc (Al/(Al + Zn)) between 0.85 and 0.99. A peak osition at 74.2 ± 0.1 eV (Al 2p3/2) implied predominance of Al2O3. stimations of the oxide layer thickness [42], based on the ratio of he observed aluminum metal and aluminum oxide peak, suggested n oxide thickness of 4–6 nm. The Auger parameter can be used or chemical state identification and is calculated from the energy ifference of the photoelectron peak and the Auger peak, to which he energy of incident photons is added [43]. A weak photoelectron eak of zinc and of the Zn LMM Auger peak located at 497.2 eV, cor- esponding to a calculated Auger parameter of 2011.4 eV, implied inc in an oxidized state, most probably as ZnO [41,44]. The surface dominance of aluminum oxide was also supported y qualitative AES findings, showing no significant compositional ariations in the aluminum to zinc signal when probing different endritic and interdendritic areas, c.f. Fig. 1. However, composi- ional differences were observed when probing similar areas with DS, a technique that provides bulk information compared with utermost surface information gained with both XPS and AES, and ith a much better surface lateral resolution. These findings imply hat even though large compositional differences are evident in the ulk of the coating, the surface composition is similar and mainly onsists of an aluminum oxide on both dendritic and interdendritic reas, caused by the high affinity of aluminum to oxygen. The large difference in topography between dendritic and inter- endritic regions for the as-received surface, c.f. Fig. 2(a), disabled he possibility to conduct AFM-based Volta-potentialmeasure- ents to assess possible differences in nobility between different arts of the unexposed as-received Galvalume surface. In order to mprove the conditions for performing AFM-studies, the surface as slightly polished to reduce the topography difference, Fig. 2(b). As revealed by XPS, the removal of the outmost aluminum rich xide disclosed zinc-rich areas, with a mass ratio (Al/(Al + Zn)) that hanged from 0.85–0.99 to 0.17–0.23 after polishing. This treat- ent resulted in the disclosure of three zinc Auger peaks (Zn LMM) t 493.8, 497.2 and 500.0 eV and corresponding calculated Auger arameters of 2014.5, 2011.1 and 2008.3 eV respectively. The first d Physics 133 (2012) 419– 428 421 peak was assigned to metallic zinc and the other two to oxidized forms of zinc. The Auger parameter at 2011.1 eV is assigned to ZnO [44,45] and the Auger parameter at 2008.3 eV may be related to Zn(OH)2. However, this could not be confirmed by independent measurements. From observed photoelectron binding energies, aluminum was assigned to Al2O3 without any metal contribution, and hence the aluminum oxide exhibited a larger thickness compared to the oxide formed on as-received Galvalume where the aluminum metal peak was detected. The XPS findings may imply a fast oxidation of both zinc and aluminum phases disclosed after polishing and removal of the relatively protective aluminum-rich surface oxide formed during coating manufacture at high temperatures. Scanning Kelvin probe force microscopy measurements clearly revealed a higher relative nobility (higher Volta potential) of the aluminum-rich dendritic branches compared with the zinc-rich interdendritic areas, Fig. 2(c), and hence the latter area may be expected to be more susceptible to corrosion than the former. How- ever, even though average compositional measurements reveal the interdendritic areas to be zinc-rich, literature findings have shown the presence of both aluminum-rich and zinc-rich phases to exist within the interdendritic areas. Preferential corrosion of the aluminum-rich phase of the interdendritic area has also been reported by means of detailed cross-sectional studies of the coating [14]. To summarize, the non-treated as-received unexposed Galval- ume surface is covered by an aluminum oxide on all parts of the surface. Upon slight diamond polishing, the aluminum oxide is removed and zinc rich phases dominate. The Volta potential on den- dritic parts of the surface is higher than on interdendritic parts, from which is expected that interdendritic areas are more susceptible to corrosion than dendritic areas. In order to investigate the initial corrosion behavior of Galval- ume, polished surfaces were exposed to humidified air in controlled laboratory exposures. 3.2. Initial corrosion of Galvalume in controlled laboratory exposures – CO2-reduced humidified air In situ studies by IRAS of the kinetics of surface oxidation of the slightly polished Galvalume surface were conducted during expo- sure up to 3 days in 90% humidified CO2-reduced air. CO2-reduction was performed in order to study the effect of humidified air first without and then with a natural concentration of CO2. For compar- ison, identical experiments were conducted for polished bare zinc and bare aluminum metal surfaces. A ZnO peak at 570 cm−1 was identified on exposed zinc, Fig. 3(a). The exposure of aluminum resulted in band domains centered at 755 and 958 cm−1, assigned to crystalline and amorphous Al2O3 [46], respectively, Fig. 3(b). Contradictory to findings for aluminum, exposure of Galvalume to humidified air resulted only in the formation of amorphous Al2O3, Fig. 3(c). The presence of Al2O3 was also confirmed with XPS (Al 2p 74.4 eV). No formation of ZnO on Galvalume was observed by means of IRAS during the exposure period. Ex situ measurements using the more surface sensitive technique XPS, revealed though the pres- ence of a distinct Zn LMM Auger peak at 493.9 eV (calculated Auger parameter 2011.2 eV) assigned to ZnO [40,44]. Previous studies by the authors have shown that the absorbance of IRAS-peaks of any well-defined compound can be used to deduce the absolute amounts of that compound. Under optimized con- ditions the relative accuracy of the estimate can be 10% [32]. Time-dependent changes in intensity of the amorphous Al2O3 peak formed on Galvalume are presented in Fig. 4 together with corresponding data for zinc (formation of ZnO) and aluminum (for- mation of amorphous and crystalline Al2O3). The results clearly show a significant formation of ZnO on zinc, whereas no formation 422 P. Qiu et al. / Materials Chemistry and Physics 133 (2012) 419– 428 F -receiv a o p o T o A e m h r n F i ig. 1. Backscatter electron images (40 �m × 40 �m) of non-treated unexposed as reas) of aluminum (b), zinc (c) and silicon (d). r growth of ZnO was observed on Galvalume during the same time eriod. A very slow, but significant growth of amorphous Al2O3 was bserved on Galvalume, at lower rates compared with aluminum. hese findings imply that aluminum rich phases are preferentially xidized in humid air. Similar observations with the formation of l2O3 and the absence of ZnO have been reported for Galvalume xposed in a pure oxygen environment [45]. This dominance of alu- inum oxide in the surface layer upon exposure to CO2-reduced umidified air was also confirmed by XPS showing an increased elative mass ratio Al/(Al + Zn) from 0.17 to 0.23 for the polished on-exposed surface to 0.62–0.77 after 3 days of exposure. The ig. 2. AFM topography image (40 �m × 40 �m) of a non-exposed as-received bare Galva n Volta potential (c). Lighter areas correspond to aluminum-rich dendritic areas. ed Galvalume coating on steel (a) and corresponding elemental mapping (lighter fact that both Al2O3 and ZnO are formed at lower formation rates on Galvalume than on the pure metals shows that the formation rates are governed by kinetic rather than galvanic effects, due to the formation of the highly protective Al2O3 layer. Since IRAS data reflect average values for relatively large sur- face areas (4 cm2), any distinction between oxidation in more aluminum-rich dendritic areas or in more zinc-rich interdendritic areas is impossible. Ex situ measurements were therefore con- ducted by means of CRM, with a lateral resolution of 0.3 �m under optimized conditions. This allows information to be collected within different surface domains. Since silicon is very Raman active lume (a), non-exposed slightly polished surface (b), and corresponding differences P. Qiu et al. / Materials Chemistry an Fig. 3. In situ IRAS spectra of zinc (a), aluminum (b) and Galvalume(c) exposed for 72 h in 90% humidified air. F s h [ F t t 9 a r l e o t a F ( ig. 4. Intensity of zinc oxide and aluminum oxides as a function of the expo- ure time of polished zinc metal, aluminum metal, and Galvalume exposed in 90% umidified air. No substantial amount of ZnO was observed on Galvalume. 47] and preferentially distributed in the interdendritic areas, c.f. ig. 1 and displayed in the optical microscopy image in Fig. 5(a), his band (470–550 cm−1) was integrated and mapped to indicate he location of interdendritic areas, Fig. 5(b). The non-exposed surface also revealed a weak Raman band at 23–1008 cm−1. This mode is believed to be associated to Al O Si ntisymmetric vibrations [48]. As Raman bands for Al2O3 have been eported between 980 and 995 cm−1 [49], this band was used to ocate surface regions dominated by aluminum-oxide phases. As vident from Fig. 5(c) and literature findings, the even distribution f the Raman band at 923–1008 cm−1 may suggest an even dis- ribution of aluminum oxide on both dendritic and interdendritic reas, in good agreement with results from the previous section. ig. 5. Optical microscopy image of a non-exposed polished Galvalume surface (a) and lighter areas) integrated between 470 and 550 cm−1 (b) and of the Al O Si band (lighte d Physics 133 (2012) 419– 428 423 By means of Ramanmapping, a preferential oxidation of aluminum-rich phases in the interdendritic areas, visualized in Fig. 6, was evident after 72 h of exposure to humid air. This obser- vation is in concordance with previous literature findings [14]. 3.3. Initial corrosion of Galvalume in controlled laboratory exposures – humidified CO2-containing air and presence of sodium chloride The formation and dominance of Al2O3 on the surface of Galval- ume was also evident from XPS analysis and IRAS upon exposure to CO2-containing (350 ppm) humid air (90%). Very similar mass compositional ratios (Al/Al + Zn) as measured for the CO2-reduced humid air exposure were determined for the outermost surface oxide (0.62–0.72). This illustrates that the presence of CO2 does not largely influence the formation of aluminum oxide. In addition to the presence and growth of amorphous Al2O3, the IRAS spec- trum presented two relatively weak bands in the region of 3488 and 3605 cm−1 and between 1380 and 1550 cm−1, not observed in CO2-reduced humidified air. These bands were allocated to water/hydroxyl and carbonate vibrations, respectively, and the lat- ter possibly assigned to a zinc and/or aluminum hydroxycarbonate. However no unambigous phase assignment was possible by means of IRAS. A shoulder of the Zn2p3/2 photoelectron peak at higher energies was observed that was not seen in the CO2-reduced envi- ronment by XPS. This suggests an association of carbonate to zinc rather than to aluminum. The initial formation of a basic zinc carbonate (Hydrozincite, Zn5(CO3)2(OH)6) in interdendritic areas has previously been reported for Galvalume exposed to outdoor conditions [9,50]. This phase is typically formed on bare zinc or galvanized surfaces exposed in non-polluted environments [16]. A mixed aluminum/zinc hydroxycarbonate formed in interdendritic areas has been reported during wet-storage of Galvalume [18]. The probable formation of zinc-rich phases, in addition to aluminum oxide formation, was further observed for the Galval- ume coating when pre-deposited with sodium chloride (15 �g NaCl cm−2) and subsequently exposed to humid CO2-containing air for 72 h. According to IRAS, both amorphous and crystalline Al2O3 were identified. According to literature findings, crystalline Al2O3 is favored by the presence of chlorides [51,52]. A chemical shift of the binding energy of aluminum to slightly higher binding energies (75.0–75.3 eV), compared to conditions without chlorides (74.5–74.7 eV), may imply the presence of AlOOH and/or Al(OH)3 [53]. The relative amount of aluminum compared to zinc as deter- mined by XPS was slightly higher in CO2- and NaCl-containing environment (0.75–0.80) than in CO2-reduced humid environment (0.62–0.77). In addition to the presence of bands assigned to carbonate, the coating exposed to chlorides revealed a splitting of the IRAS band around 3640 cm−1, an effect previously observed for basic zinc chlorides (Simonkolleite, Zn5(OH)8Cl2·H2O) [54]. This phase corresponding Raman mapping image (scan size: 30 �m × 30 �m) of the Si band r areas) integrated between 923 and 1008 cm−1 (c). 424 P. Qiu et al. / Materials Chemistry and Physics 133 (2012) 419– 428 Fig. 6. Raman mapping images of the Al O Si band (lighter areas) integrated between 923 and 1008 cm−1 (a) and the Si band (lighter areas) integrated between 470 and 550 cm−1 (b) for Galvalume after 72 h exposure in humidified air. F itic ar c t i b m a a s s f a c Z p c e p a a f i t m z i e p i 3 n b after 12 weeks and to 0.80 after 26 weeks of exposure. After 1 year of exposure were aluminum-rich phases instead dominating the surface (Zn/(Zn + Al): 0.30), and dominates almost completely the ig. 7. SEM backscatter images of corrosion products formed primarily in interdendr onditions in the marine environment of Brest, France. ypically forms on bare zinc and galvanized steel surfaces exposed n marine as well as in laboratory studies [21,55–57] and has also een identified on Galvalume coatings exposed in similar environ- ents [58]. Because other specific bands of Simonkolleite at 910 nd 730 cm−1 [59], and bands of amorphous and crystalline Al2O3 s well as specific bands related to Hydrozincite, all fall within the ame band region (1000 and 750 cm−1) that dominates the IRAS- pectrum, no unambiguous phase assignment was possible. The ormation of zinc-rich phases and the presence of chloride were lso supported by XPS findings. An Auger parameter of 2010.8 eV, alculated from the ZnLMM and the main photoelectron peak of n2p3/2 suggested the presence of ZnO [44,45]. Since the Na KLL eak overlaps the Zn LMM peak at higher binding energies, no cal- ulations of the Auger parameter were possible for other potentially xisting oxidized phases of zinc. A shoulder of the photoelectron eak of zinc at higher binding energies indicated the presence of nother zinc-rich phase, as suggested by IRAS findings. In all, the exposure of Galvalume to CO2-containing humidified ir suggests the overall formation of amorphous Al2O3 and the local ormation of zinc hydroxycarbonate, presumably as Hydrozincite, n interdendritic areas. Additional predeposition of NaCl manifests he overall formation of aluminum-containing species, this time ore likely as AlOOH and/or Al(OH)3, and the local formation of inc-containing phases on interdendritic areas, possibly as Hydroz- ncite, Simonkolleite and ZnO. The formation of corrosion products on Galvalume was further xplored for both short (weeks) and long term (years) exposure eriods at non-sheltered marine and urban conditions, discussed n the next section. .4. Formation of corrosion products on Galvalume coatings at on-sheltered field conditions Non-treated surfaces of as-received Galvalume coatings and are zinc sheet were exposed for 2, 4, 12, 26 weeks, 1 and 5 years eas of Galvalume exposed for 12 weeks (a), 1 year (b) and 5 years (c) at non-sheltered at the marine site of Brest, France. In agreement with the lab- oratory investigation and with literature findings, the SEM/EDS investigation revealed zinc-rich corrosion products locally formed that gradually developed with time on the interdendritic areas [10], Fig. 7. No crystalline zinc-rich phases were possible to detect throughout the whole exposure period by GIXRD. The gradual formation of zinc-rich phases, observed as increased surface coverage compared to aluminum-rich phases, during the first half year of exposure was clearly demonstrated by XPS, Fig. 8. The surface fraction by mass (Zn/(Zn + Al)) increased from 0.01 to 0.15 for the as-received non-exposed Galvalume surface to 0.22–0.32 after 2 weeks, to 0.55–0.62 after 4 weeks, to 0.40–0.67 Fig. 8. The mass fraction (Zn/(Zn + Al)) determined by means of XPS in the outermost surface layer at two randomly selected surface areas (each sized 0.4 mm2, area 1 in gray color, area 2 in black color) of as-received Galvalume coatings prior to (non- exposed) and after 2, 4, 12, 26 weeks, 1 and 5 years of non-sheltered exposure to a marine environment. P. Qiu et al. / Materials Chemistry and Physics 133 (2012) 419– 428 425 gs exp o s c o a a a p 7 b G 3 t k a c S G r i ( t a r p t t p S Z f F A Fig. 9. Scanning electron microscopy backscatter images of Galvalume coatin utermost surface (Zn/(Zn + Al): 0.01–0.10) after 5 years of non- heltered exposure. According to GIXRD, was Al(OH)3 the main rystalline phase observed after this time period, a phase previ- usly identified in marine environments [9]. IRAS bands located t 1100 and 700 cm−1 were observed after all exposure periods, nd may be associated with Al(OH)3 or AlOOH [60]. However, s also the basic zinc carbonate, Zn5(CO3)2(OH)6 (Hydrozincite), resents a strong peak located at 1060 cm−1 and a weak band at 33 cm−1 [61], any conclusive phase assignments were not possi- le. Similar to the laboratory findings with pre-deposited NaCl on alvalume in humid air, IRAS revealed a possible split of the band at 500 cm−1 after 5 years of exposure. This suggests the local forma-ion of a basic zinc chloride, presumably Simonkolleite, previously nown to form on Galvalume [9,62]. The broad band centered at pproximately 1100 cm−1, may also reflect the presence of sulfate- ontaining phases, as also XPS indicated the presence of sulfate. ulfate-rich aluminum phases have previously been reported for alvalume exposed to marine conditions [9]. Identification of cor- osion products by CRM, IRAS and GIXRD on bare zinc sheet exposed n parallel on the marine test site revealed Hydrozincite, and ZnO crystalline and amorphous) to be the main components [63]. As a result of very complex exposure conditions and the forma- ion and presence of a large variety of different corrosion products t the marine site, confocal Raman spectroscopy mapping did not esult in any conclusive interpretations of the location of corrosion roducts, in contrast to the experience in the laboratory investiga- ion. Investigations on the lateral corrosion product distribution were herefore conducted on Galvalume exposed to a significantly less olluted urban site (5 years in Stockholm) by means of XRD, EM (Fig. 9) and confocal Raman spectroscopy mapping (Fig. 10). inc-rich phases (possibly Hydrozincite and zinc hydroxyl sul- ates indicated by XRD) and aluminum-rich phases (sulfate-rich ig. 10. Raman mapping images (scan size: 30 �m × 30 �m) of the Si band, indicating th l O Si band (integrated between 923 and 1008 cm−1) (b), and SO42− band (970–1200 osed for 5 years at non-sheltered urban conditions in Stockholm, (a) and (b). and Al2O3, identified by means of XRD and indirectly evidenced by the Al O Si band integrated between 923 and 1008 cm−1 by CRM), were primarily formed in the interdendritic areas, Fig. 10. These indications of corrosion product location were in accordance with previous studies by the authors on Galvalume exposed to rain-sheltered conditions at the same site [50]. The formation of sulfate-rich aluminum corrosion products in interdendritic areas has also been reported elsewhere [9]. The fact that zinc-containing corrosion products primarily form on the interdendritic areas in the urban site of Stockholm as well as in all laboratory exposures presented before and also in Brest, suggests that zinc-containing corrosion products in general start to form on interdendritic areas, Fig. 9(a), and then eventually spread to other areas, Fig. 9(b). In all, the exposure of Galvalume in the marine test site exhibits a remarkable variation in corrosion product composition. Dur- ing shorter exposures up to 26 weeks Al(OH)3 and AlOOH were detected in addition to the possible presence of aluminum sulfate of unknown identity, with the parallel gradual formation of zinc- containing phases primarily ZnO, Hydrozincite and Simonkolleite. With exception of the aluminum sulfate, the phases detected are within the accuracy of the analysis the same as in the laboratory exposure containing humidified air, CO2 and predeposited NaCl. The fraction of zinc-containing phases reached a maximum during the first year and then declined. After 5 years the Galvalume surface was mainly covered by aluminum-containing corrosion products, dominated by crystalline Al(OH)3. 3.5. Release of zinc and aluminum from Galvalume coatings at non-sheltered field conditions The long-term release of the main metal constituents from Gal- valume, exposed both at the marine test site in Brest and, for e location of interdendritic areas (integrated between 470 and 550 cm−1) (a), the cm−1) (c). 426 P. Qiu et al. / Materials Chemistry and Physics 133 (2012) 419– 428 F c and r ne site G atio o c F t a 1 a H f p a r ( o p t a F s a z d r [ l s m v l m a p c s a m and Al4SO4(OH)10·2H2O were identified by GIXRD after 10 years of exposure. Similar to the results from Brest, measurements of the release rate of aluminum from selected samples during the 10-year exposure period showed very low values, again explained ig. 11. Average release rates of zinc and aluminum (a), annual release rates of zin ainfall quantity (c) for Galvalume exposed to non-sheltered conditions at the mari alvalume compared with zinc released from zinc sheet exposed in parallel (d). A r omparison, also in the urban test site of Stockholm, is displayed in ig. 11(a) as average release rates of aluminum and of zinc versus ime for up to 5 years of exposure. The zinc release rate gradu- lly increases during the first year, reaches a maximum after about year and then gradually declines due to the parallel growth of luminum-rich phases and partial dissolution of zinc-rich phases. ence, a strong correlation exists between the formation and sur- ace coverage of zinc-rich corrosion products, c.f. Fig. 8, and the artial dissolution and release of zinc from these phases via the ction of rainwater, c.f. Fig. 11. The same trend was observed when displaying the zinc release ate as annual release rates rather than average release rates Fig. 11(b)) exhibiting a maximum after year one and a continu- us reduction with time during the subsequent 4-year exposure eriod. This reduction can be explained by the gradual forma- ion and dominance of aluminum-rich compounds such as AlOOH nd Al(OH)3 over zinc-rich phases in the outermost surface layer, ig. 8, which efficiently hinder the release of zinc. These conclu- ions are supported by the laboratory exposures, c.f. Fig. 6, showing preferential growth of aluminum-rich phases in parallel with inc-rich phases in mainly interdendritic areas. Aluminum-rich endritic areas have been proposed to mechanically anchor zinc- ich corrosion products formed in zinc-rich interdendritic regions 33,63]. The annual release of zinc from Galvalume was 5–7.5 times ower compared to that of bare zinc sheet (Fig. 11(d)), as a con- equence of the surface dominance of aluminum-rich phases in ainly dendritic areas. A reduced release rate of zinc from Gal- alume compared to galvanized steel has also been reported in the iterature [15]. The release rate of zinc was 20–30 times higher than of alu- inum (Fig. 11(a) and, hence, not at all related to its nominal bulk lloy content). The extent of metal release from alloys has in several revious studies been proven to largely differ from their pure metal onstituents, and not be possible to estimate based on bulk compo- ition [64,65]. Calculations based on the nominal bulk composition nd release data for zinc sheet in this study confirms this state- ent also for Galvalume with largely overestimated rates (at least aluminum (b) and released annual amount of aluminum normalized to the annual of Brest, France, as a function of exposure time. Annual ratio of zinc released from f one corresponds to identical release rates. with a factor of two) compared with real observations. Significantly lower release rates of aluminum compared with zinc throughout the entire 5-year exposure period suggests that the aluminum- containing corrosion products on average are much less soluble than those for zinc under current conditions. When normalizing the annual average aluminum release rate to the annual rainfall quantity, a slight reduction can be seen after 3 years of exposure, possibly related to the formation of Al(OH)3, Fig. 11(c). Similar trends, with significantly lower release rates of zinc from Galvalume compared to the bare zinc sheet, was also observed for Galvalume exposed at non-sheltered conditions in the low- polluted urban environment of Stockholm for 10 years, Fig. 12. Throughout the whole 10-year period the zinc release rate grad- ually declined. Based on our findings from the marine test site, the explanation is most likely due to the gradual built-up of aluminum- rich phases in the surface layer of Galvalume, since both Al2O3 Fig. 12. Annual ratio of zinc released from Galvalume compared with zinc released from zinc sheet during 10 years of non-sheltered urban exposure conditions in Stockholm, Sweden. A ratio of one corresponds to identical release rates. try an b e 4 c r p d n c i a p a p o a a ue t i a t t d c a t i z a a p s r A A e R t R u ( c n c S f s L [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ P. Qiu et al. / Materials Chemis y the low chemical solubility of aluminum phases under present xposure conditions. . Conclusions The non-treated as-received and unexposed Galvalume surface onsists of dendritic aluminum-rich areas and interdendritic zinc- ich areas, both covered by an aluminum oxide. A higher Volta otential was determined for dendritic areas compared with inter- endritic regions on a slightly polished Galvalume surface, an effect ot observed for the as-received condition. Upon exposure to humidified air with reduced CO2- oncentration both Al2O3 and ZnO are formed, preferentially n the interdendritic areas. The formation rates of both phases re lower than on the pure metals showing that the protective roperties of the Al2O3 layer are crucial. CO2-containing humidified air results in an overall formation of morphous Al2O3 and local formation of zinc hydroxycarbonate, resumably Hydrozincite, on interdendritic areas. Predeposition f NaCl triggers the overall formation of AlOOH and/or Al(OH)3, nd the local formation of zinc-containing phases on interdendritic reas, possibly Hydrozincite, Simonkolleite and ZnO. The same phases are observed on Galvalume upon long-term nsheltered marine exposure. During the first half year a prefer- ntial corrosion of interdendritic areas occurs observed through he evolution of AlOOH, Al(OH)3, an aluminum sulfate of unknown dentity, and the parallel formation of primarily ZnO, Hydrozincite nd Simonkolleite. Due to a generally higher solubility of the zinc- han of the aluminum-containing phases the surface coverage of he former reaches a maximum during the first year and then eclines. After 5 years the Galvalume surface is mainly covered by rystalline Al(OH)3. The annual release rate of zinc in the marine site also exhibits maximum after year one and a continuous reduction with ime during the subsequent 4-year exposure period. This behav- or follows the same time-dependence as the surface coverage of inc-containing phases and is explained by the gradual formation nd dominance of less soluble aluminum-rich phases such AlOOH nd Al(OH)3 compared to zinc-rich phases. Characteristic corrosion and runoff features of Galvalume com- ared to bare zinc in the marine and the urban site investigated, the ignificantly lower corrosion rate and the ever decreasing runoff ate, are explained by the progressive uniform formation of first l2O3, then by AlOOH and finally by Al(OH)3. cknowledgements The authors are grateful for the financial support of the field xposure provided by Nordic Galvanizers Association, Sweden; heinzink, Germany; Saferoad, Norway and SSAB, Sweden and he funding from the European Union’s Research Program of the esearch Fund for Coal and Steel (RFCS) research program Autocorr nder grant agreement n◦ RFSR-CT-2009-00015. Instrumental grants from Knut and Alice Wallenberg foundation XPS) and from Nils and Dorthi Troëdsson Foundation (combined onfocal Raman and AFM) are gratefully acknowledged. Micrographic examinations by M. Sc. Oskar Karlsson of on-exposed surfaces at the unit for metallic microstructure haracterization (MEMIKA), a joint facility between KTH and werea-KIMAB, Stockholm, Sweden, is highly acknowledged. We acknowledge the French Corrosion Institute, Brest, France, or their invaluable help in collecting runoff water at the marine ite. All AAS analytical efforts by Dr. Gunilla Herting and MSc David indström are highly appreciated. [ [ d Physics 133 (2012) 419– 428 427 References [1] J. Elvins, J.A. Spittle, D.A. Worsley, Corros. Eng. Sci. Technol. 38 (2003) 197–204. [2] X.G. Zhang, Electrochem. Soc. J. 143 (1996) 1472–1484. [3] G.W. Walter, Use of electrochemical sensors to measure corrosion charac- teristics of Zn and Zn55%Al alloy coated steel under simulated atmospheric conditions, in: The International Conf. on Zinc and Zinc Alloy Coated Steel Sheet (Galvatech), Tokyo, Japan, 1989, pp. 565–568. [4] I.S. Cole, A. Bradbury, A.K. Neufeld, N. Sherman, Response of galvanized steel, 55% aluminum-zinc-coated steel and copper steel to well-defined salt doses under controlled environments, in: 13th International Corrosion Congress, Melbourne, Australia, 1996 (Paper 419). [5] E. Palma, B. Fernández, M. Morcillo, Mater. Corros. 48 (1997) 765–769. [6] H.E. Townsend, Mater. Perform. 32 (1993) 68–71. [7] M. Morcillo, E. Palma, B. Fernández, Werkstoffe Korrosion 45 (1994) 550–553. [8] G.A. King, Corros. Aust. (1988) 5–14. [9] J.J. Friel, Corrosion 42 (1986) 422–427. 10] E. Palma, J.M. Puente, M. Morcillo, Corros. Sci. 40 (1998) 61–68. 11] H.E. Townsend, J.C. Zoccola, Mater. Perform. 18 (1979) 13–20. 12] J.C. Zoccola, H.E. Townsend, A.R. Borzillo, J.B. Horton, Atmospheric corrosion resistance of aluminum–zinc alloy-coated steel, in: S.K. Coburn (Ed.), Atmo- spheric Factors Affecting the Corrosion of Engineering Materials, ASTM STP 646, American Society for Testing and Materials, Philadelphia, Pennsylvania, 1978. 13] J. Selverian, M. Notis, A. Marder, J. Mater. Eng. 9 (1987) 133–140. 14] A.R. Moreira, Z. Panossian, P.L. Camargo, M.F. Moreira, I.C.d. Silva, J.E.R. de Car- valho, Corros. Sci. 48 (2006) 564–576. 15] J.H.W. Sullivan, D.A. Worsley, Br. Corros. J. 37 (2002) 282–288. 16] A.K. Neufeld, I.S. Cole, Use of FTIR to study surface changes on metals in the early stages of degradation, in: Proc. 13th Int. Corr. Congr., Melbourne, 1996 (Paper 46). 17] E. Palma, M. Morcillo, Plat. Surf. Finish. 85 (1998) 106–109. 18] I. Odnevall Wallinder, W. He, P.E. Augustsson, C. Leygraf, Corros. Sci. 41 (1999) 2229–2249. 19] S. Bertling, I. Odnevall Wallinder, C. Leygraf, D. Berggren Kleja, Sci. Total Environ. 367 (2006) 908–923. 20] P. Verbiest, H. Waeterschoot, R. Racek, M. Leclerq, Prot. Coat. Eur. 9 (1997). 21] L. Veleva, M. Acosta, E. Meraz, Corros. Sci. 51 (2009) 2055–2062. 22] L. Veleva, E. Meraz, M. Acosta, Corros. Eng. Sci. Technol. 45 (2010) 76–83. 23] A. Schriewer, H. Horn, B. Helmreich, Corros. Sci. 50 (2008) 384–391. 24] P. Robert-Sainte, M.C. Gromaire, B. de Gouvello, M. Saad, G. Chebbo, Environ. Sci. Technol. 43 (2009) 5612–5618. 25] S.A. Matthes, S.D. Cramer, S.J. Bullard, B.S. Covino, B.S. Covino Jr., G.R. Hol- comb, Atmospheric corrosion and precipitation runoff from zinc and zinc alloy surfaces, in: NACE Corrosion Conference, San Diego, CA (US), 2003. 26] D. Lindström, I. Odnevall Wallinder, Environ. Monit. Assess. 173 (2011) 139–153. 27] S. Jouen, B. Hannoyer, A. Barbier, J. Kasperek, M. Jean, Mater. Chem. Phys. 85 (2004) 73–80. 28] M. Faller, D. Reiss, Mater. Corros. 56 (2005) 244–249. 29] J. Sandberg, I. Odnevall Wallinder, C. Leygraf, N. Le Bozec, J. Electrochem. Soc. 154 (2007) C120–C131. 30] I. Odnevall Wallinder, C. Leygraf, C. Karlén, D. Heijerick, C.R. Janssen, Corros. Sci. 43 (2001) 809–816. 31] P. Qiu, D. Persson, C. Leygraf, J. Electrochem. Soc. 156 (2009) C81–C86. 32] P. Qiu, D. Persson, C. Leygraf, J. Electrochem. Soc. 156 (2009) C441–C447. 33] W. Chen, Q. Liu, Q. Liu, L. Zhu, L. Wang, J. Alloys Compd. 459 (2008) 261–266. 34] Z. Chen, S. Zakipour, D. Persson, C. Leygraf, Effect of Sodium Chloride Particles on the Atmospheric Corrosion of Pure Copper, NACE International, Houston, TX, ETATS-UNIS, 2004. 35] ISO Standard 9226, Corrosion of Metals and Alloys – Corrosivity of Atmospheres – Determination of Corrosion Rate of Standard Specimens for the Evaluation of Corrosivity, 1992. 36] ISO/DIS 17752, Corrosion of Metals and Alloys – Procedures to Determine and Estimate Runoff Rates of Metals from Materials as a Result of Atmospheric Corrosion, 2011. 37] D. Persson, C. Leygraf, J. Electrochem. Soc. 142 (1995) 1468–1477. 38] T. Aastrup, C. Leygraf, J. Electrochem. Soc. 144 (1997) 2986–2990. 39] V. Guillaumin, P. Schmutz, G.S. Frankel, J. Electrochem. Soc. 148 (2001) B163–B173. 40] T.A. Lowe, G.G. Wallace, A.K. Neufeld, J. SolidState Electrochem. 13 (2009) 619–631. 41] B.S. Kim, T. Piao, S.N. Hoier, S.M. Park, Corros. Sci. 37 (1995) 557–570. 42] B.R. Strohmeier, Surf. Interface Anal. 15 (1990) 51–56. 43] C.D. Wagner, J. Electron Spectrosc. Relat. Phenom. 47 (1988) 283–313. 44] A.K. Chandra, R. Mukhopadhyay, J. Konar, T.B. Ghosh, A.K. Bhowmick, J. Mater. Sci. 31 (1996) 2667–2676. 45] T.A. Lowe, Using Band Microelectrode Arrays to Investigate the Cut Edge and Bare Corrosion Behaviour of 55% Al–Zn Coated Steel, Doctoral thesis, University of Wollongong, Australia, 2011. 46] P. Brüesch, R. Kötz, H. Neff, L. Pietronero, Phys. Rev. B 29 (1984) 4691–4696. 47] A. Misra, H.D. Bist, M.S. Navati, R.K. Thareja, J. Narayan, Mater. Sci. Eng. B 79 (2001) 49–54. 48] R. Le Parc, B. Champagnon, J. Dianoux, P. Jarry, V. Martinez, J. Non-Cryst. Solids 323 (2003) 155–161. 4 try an [ [ [ [ [ [ [ [ [ [ [ [ [ [ [ 28 P. Qiu et al. / Materials Chemis 49] A. Aminzadeh, H. Sarikhani-fard, Spectrochim. Acta Part A 55 (1999) 1421–1425. 50] I. Odnevall, Characterization of corrosion products formed on rain sheltered Aluzink and aluminum in a rural and an urban atmosphere, in: Proc. 13th Int. Corr. Congr., Australia, 1996, pp. 1–8. 51] C.L. McBee, J. Kruger, Electrochim. Acta 17 (1972) 1337–1341. 52] T.P. Hoar, J. Electrochem. Soc. 117 (1970) 17C–22C. 53] Y. Zhang, J. Mater. Sci. Lett. 21 (2002) 1603–1605. 54] Z.Y. Chen, D. Persson, F. Samie, S. Zakipour, C. Leygraf, J. Electrochem. Soc. 152 (2005) B502–B511. 55] E. Dubuisson, P. Lavie, F. Dalard, J.-P. Caire, S. Szunerits, Corros. Sci. 49 (2007) 910–919. 56] E. Almeida, M. Morcillo, Surf. Coat. Technol. 124 (2000) 180–189. 57] A.I. Almarshad, S. Syed, Mater. Corros. 59 (2008) 46–51. [ [ d Physics 133 (2012) 419– 428 58] D. Persson, D. Thierry, N. LeBozec, Corros. Sci. 53 (2011) 720–726. 59] I.S. Cole, T.H. Muster, D. Lau, N. Wright, N.S. Azmat, J. Electrochem. Soc. 157 (2010) C213–C222. 60] H. Hou, Y. Xie, Q. Yang, Q. Guo, C. Tan, Nanotechnology 16 (2005) 741–745. 61] M.C. Hales, R.L. Frost, Polyhedron 26 (2007) 4955–4962. 62] A.K. Neufeld, I.S. Cole, Use of FTIR to study surface changes on metals in the early stages of degradation, in: 13th International Corrosion Congress, Melbourne, Australia, 2006 (Paper 046). 63] J. Hedberg, N. Le Bozec, I. Odnevall Wallinder, Mater. Corros., doi:10.1002/maco.201106361. 64] S. Goidanich, I. Odnevall Wallinder, G. Herting, C. Leygraf, Corros. Eng. Sci. Technol. 43 (2008) 134–141. 65] G. Herting, I. Odnevall Wallinder, C. Leygraf, J. Electrochem. Soc. 152 (2005) B23–B29. http://dx.doi.org/10.1002/maco.201106361 Evolution of corrosion products and metal release from Galvalume coatings on steel during short and long-term atmospheric ... 1 Introduction 2 Material and methods 2.1 Materials and surface preparation 2.2 Laboratory and field exposure conditions 2.3 Metal runoff measurements 2.4 Surface analysis 2.4.1 In situ infrared reflection absorption spectroscopy (IRAS) 2.4.2 Confocal Raman microspectroscopy (CRM) 2.4.3 Scanning electron microscopy with energy dispersive X-ray analysis (SEM/EDS) mapping 2.4.4 Scanning Kelvin probe force microscopy (SKPFM) 2.4.5 Grazing incident X-ray diffraction (GIXRD) 2.4.6 X-ray photoelectron spectroscopy (XPS) 3 Results and discussion 3.1 Bulk and surface characterization before exposure 3.2 Initial corrosion of Galvalume in controlled laboratory exposures – CO2-reduced humidified air 3.3 Initial corrosion of Galvalume in controlled laboratory exposures – humidified CO2-containing air and presence of sodi... 3.4 Formation of corrosion products on Galvalume coatings at non-sheltered field conditions 3.5 Release of zinc and aluminum from Galvalume coatings at non-sheltered field conditions 4 Conclusions Acknowledgements References
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