“…al. ; 51,70 chemo-mechanical model first proposed by Hoar; 5 and ion migration to and reaction at the oxide/metal interface suggested by many 3,5,7,10,12,14,39,51,52,70,91 and recently refined by McCafferty 13,14 are plausible theories considering the experimental results. At the present time McCafferty's stepwise model shows the most significant agreement with the overall experimental data predicting: Cl − is adsorbed and incorporated in the oxide film, moves toward the metal-oxide interface, a lower i pass with Cl − incorporation, oxide thinning prior to E pit , and the formation and rupture of blisters.…”
Section: Authors' Interpretation Of the Resultsmentioning
confidence: 99%
“…Also, the physical appearance showed the development of cracks, which would indicate stress build up. The stress build up can occur by Cl − migration and formation of Cl-Al islands at the oxide/metal interface, 51,70 Cl − migration and Al dissolution leading to hydrogen production at the oxide/metal interface, 13,14,[122][123][124][125][126] or oxide cracking caused by the presence of Cl − within the oxide film.…”
Section: Oxide Blister Formation and Rupturementioning
Metals and alloys such as aluminum (Al), stainless steels, and nickel-based alloys exhibit corrosion resistance in a wide range of environments due to the presence of protective, passive oxides. However, in environments that contain aggressive anions such as chloride, Cl − , the passive film becomes unstable and degrades locally causing film breakdown and pitting corrosion. A number of theories describing the initiation of pitting corrosion have been postulated and discussed but to date there is no consensus on the mechanism of breakdown. Since all current mechanisms require Cl − interactions for oxide film breakdown in Cl − containing environments, the question is what is the nature of the interaction of aggressive anions such as Cl − with the passive film, adsorption and/or absorption, leading to pitting? This communication focuses on the interaction of Cl − with the passive oxide film on pure aluminum by reviewing and summarizing the available experimental data concerning Cl − interactions. It should also be noted that the observations for Cl − interactions with Al reviewed and summarized herein might not be applicable to all metals and alloys. Technologically important metals and alloys such as aluminum (Al), stainless steels, and nickel-based alloys exhibit corrosion resistance in a wide range of environments due to the presence of protective, passive oxides.1-90 The passive oxides behave as kinetic barriers, which inhibit further oxidation of the underlying thermodynamically reactive metals. However, in environments that contain aggressive anions such as chloride, Cl − , the passive film becomes unstable and degrades locally causing film breakdown and localized corrosion, which in turn decreases the service life of the materials. The consequence of discrete oxide failure is localized corrosion, which occurs in the forms of crevice corrosion in occluded sites and metastable or stable pitting corrosion on open surfaces. It is generally agreed that localized corrosion occurs in two distinct steps: initiation and propagation.A number of theories describing the initiation of pitting corrosion have been postulated and discussed.
“…al. ; 51,70 chemo-mechanical model first proposed by Hoar; 5 and ion migration to and reaction at the oxide/metal interface suggested by many 3,5,7,10,12,14,39,51,52,70,91 and recently refined by McCafferty 13,14 are plausible theories considering the experimental results. At the present time McCafferty's stepwise model shows the most significant agreement with the overall experimental data predicting: Cl − is adsorbed and incorporated in the oxide film, moves toward the metal-oxide interface, a lower i pass with Cl − incorporation, oxide thinning prior to E pit , and the formation and rupture of blisters.…”
Section: Authors' Interpretation Of the Resultsmentioning
confidence: 99%
“…Also, the physical appearance showed the development of cracks, which would indicate stress build up. The stress build up can occur by Cl − migration and formation of Cl-Al islands at the oxide/metal interface, 51,70 Cl − migration and Al dissolution leading to hydrogen production at the oxide/metal interface, 13,14,[122][123][124][125][126] or oxide cracking caused by the presence of Cl − within the oxide film.…”
Section: Oxide Blister Formation and Rupturementioning
Metals and alloys such as aluminum (Al), stainless steels, and nickel-based alloys exhibit corrosion resistance in a wide range of environments due to the presence of protective, passive oxides. However, in environments that contain aggressive anions such as chloride, Cl − , the passive film becomes unstable and degrades locally causing film breakdown and pitting corrosion. A number of theories describing the initiation of pitting corrosion have been postulated and discussed but to date there is no consensus on the mechanism of breakdown. Since all current mechanisms require Cl − interactions for oxide film breakdown in Cl − containing environments, the question is what is the nature of the interaction of aggressive anions such as Cl − with the passive film, adsorption and/or absorption, leading to pitting? This communication focuses on the interaction of Cl − with the passive oxide film on pure aluminum by reviewing and summarizing the available experimental data concerning Cl − interactions. It should also be noted that the observations for Cl − interactions with Al reviewed and summarized herein might not be applicable to all metals and alloys. Technologically important metals and alloys such as aluminum (Al), stainless steels, and nickel-based alloys exhibit corrosion resistance in a wide range of environments due to the presence of protective, passive oxides.1-90 The passive oxides behave as kinetic barriers, which inhibit further oxidation of the underlying thermodynamically reactive metals. However, in environments that contain aggressive anions such as chloride, Cl − , the passive film becomes unstable and degrades locally causing film breakdown and localized corrosion, which in turn decreases the service life of the materials. The consequence of discrete oxide failure is localized corrosion, which occurs in the forms of crevice corrosion in occluded sites and metastable or stable pitting corrosion on open surfaces. It is generally agreed that localized corrosion occurs in two distinct steps: initiation and propagation.A number of theories describing the initiation of pitting corrosion have been postulated and discussed.
“…Most authorities now refer to critical concentrations of order 1M or higher in Me n+ , which for believable anodic current densities (say, less than 100 A cm -2 in the most extreme case 10 ), entails an effective diffusion length of at least 0.1-1 μm. For "perfectly" flat surfaces, this leads to the speculation that a slow blistering type of corrosion occurs under the passive film, with only molecular-sized channels for communication with the bulk solution; then this structure pops open, leading to pit growth-similar to a proposal of Mattin and Burstein, 11 and recalling earlier work by authors who referred to "salt islands" or "blisters." This critical chemistry is postulated to correspond to a thermodynamic criterion : a critical solubility of metal cations in equilibrium with the relevant oxide or hydroxide.…”
Pitting corrosion of metals is one of the most important electrochemical corrosion phenomena. Corrosion of steel reinforcement in concrete is always in the news, and it starts off as pitting, caused by chloride ions-so it is feasible that pitting is the most costly form of corrosion. Such an assessment might not be the same in every decade, and it is hard to measure the cost of corrosion Synthetic Diamond: Emerging CVD Science and Technology Edited by K. E. Spear and J. P. Dismukes (1994) 688 pages. ISBN 978-0-471-53589-8 Electrochemical Oxygen Technology by K. Kinoshita (1992) 444 pages. ISBN 978-0-471-57043-1 ECS Members will receive a discount. All prices subject to change without notice.
“…They demonstrated and proved that the pit stable or metastable growth is controlled by corrosion products diffusion, since the pitting current density is independent of the applied potential. As is well known, a chloride-induced pit must be either enriched in chloride, or of a lower pH, or both relative to the bulk solution, in order to sustain continuous propagation of pit [18][19][20][21]23,26]. This mechanism is also suitable for crevice corrosion [27,28].…”
Section: Introductionmentioning
confidence: 96%
“…Burstein et al [3,4,[18][19][20][21][22][23][24][25] used a tiny specimen, a microelectrode to study pit nucleation and propagation, and obtained single and separated current transients. They demonstrated and proved that the pit stable or metastable growth is controlled by corrosion products diffusion, since the pitting current density is independent of the applied potential.…”
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