# Salt Spray Corrosion of 2060-T8 Al–Li Alloy in an Aggressive Environment

Authors: Zhengquan Zhang; Yuling Wang; Li Liangfeng
Journal: Advances in Materials Science and Engineering
 (2022)

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## Abstract

The phase and microstructure of corrosion product formed on 2060-T8 Al–Li alloy have been investigated effectively by SEM and XRD after salt spray corrosion. It was found that the corrosion product growth rate can be divided into three stages: the main phases of corrosion product were Al2O3, Al(OH)3, and AlOOH phases; as the increasing of salt spray time, the phase angle of A12O3 shifts slightly to the left at 31.8°; and the phase angle of A12O3 first shifts to the left, then to the right at 38.6°. The formation and evolution model of salt spray droplet was built, and the formation mechanism of corrosion product was also analyzed. This alloy shows a sensitive corrosion performance to the salt spray environment.


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## Body

## 1. Introduction

Al–Li alloy is one of the age-hardenable aluminum alloys and is used to reduce the weight, improve the fuel efficiency of aircraft, and increase the payload in the aerospace industry [1–3]. Compared with traditional aluminum alloys, the Al–Li alloy has a great deal of excellent performance, such as lower density, higher elastic modulus, higher specific strength, and more favorable damage tolerance properties [4–7]. 2060 Al–Li alloy, launched in 2011, is considered as a potential candidate for the use at wing/fuselage forgings, lower wing, and fuselage/pressure cabin [1–7].Al–Li alloys are susceptible to corrosion after prolonged exposure to high-salt or humidity environment, which influences the use for structural applications. The salt fog phenomenon is commonly found in snowy or ocean environment, which usually induces galvanic corrosion and speeds up electrolytic and galvanic corrosion due to the presence of chloride ion [8–16]. To be accepted for production, components must pass a defined number of neutral salt spray corrosion hours [15]. Salt spray corrosion is able to give fast results and reproduce most of the atmospheric corrosion processes; therefore, it is used extensively in many industries, including the aerospace industry [10, 15]. The evaluation criterion is commonly based on the time taken for corrosion product to appear on the sample’s surface [12, 15].The corrosive characterization of AL-Li alloys depends upon the electrochemical property of matrix, feature of intermetallic, their size of phase and distribution composition of homogeneity element [17–26]. Al–Li alloys contain a wide variety of complex secondary precipitates, including Guinier–Preston(GP) zones, θ′,θ,δ′,T1,T2,TB,Ω, and S [27–37]. As an age-hardenable aluminum alloy, Al–Li alloy is not resistance to localized corrosion due to its deliberately developed heterogeneous microstructure in corrosive environment, which contains chloride ion [4]. Ahmad reported the exfoliation corrosion of alloy 2060 in an aggressive environment and found there were continuous pits along the grain boundaries and intergranular corrosion. White gelatinous corrosion products formed under the grains [4]. Ma et al. investigated the effect of thermo mechanical treatments on local corrosion susceptibility of 2099 Al–Li alloy and found severe localized corrosion was associated with not only localized plastic deformation occurring during cold working but also heterogeneous precipitation of T1 phase. These alloys displayed crystallographic corrosion morphology, selective attack of grain boundaries, and grain interiors [34, 35]. Macdonald et al. studied the pitting corrosion of 2098 Al–Li alloy, they thought the Al interstitial comprise the majority of the point defects in the barrier layer of this alloy, the formation of a passive layer had lower capacitance, which is associated with the point defect structure of the barrier layer [38]. Queiroz reported the EIS behavior of anodized and primer coated 2198 AL-Li alloy, they found the uncoated surface of this alloy showed higher pitting susceptibility, larger amounts of corrosion products formed on the anodized and primer coated surface of this alloy, and the diffusion was associated with large amounts of porous corrosion products on the exposed surface of this alloy to the corrosive environment [14]. Moreto et al. thought the localized feature of 2198 Al–Li alloy was essentially related to the existence of intermetallic, which was cathodic or anodic in relation to the aluminum matrix, and this alloy presented a higher long-time resistance to pitting corrosion due to the lower limiting cathodic current [21]. Jiang et al. found the intergranular corrosion of 2197Al–Li alloy is caused by the alternate anodic dissolution of T1 and PFZ, and the increase of the size of T1 at grain boundaries and the width of PFZ along grain boundaries lead to an increase in the susceptibility to intergranular corrosion and exfoliation corrosion [22, 23]. Li et al. found at the beginning, the precipitates of T1 and T2 are anodic to the alloy base and corrosion occurs on their surface; the corroded T1 and T2 precipitates become cathodic to the alloy base at a later stage, leading to the anodic dissolution and corrosion of the alloy base at its adjacent periphery [25–27]; they also discovered the electrode conversion of T2 from anode to cathode is more superficial than that of T1, and the corrosion mainly occurs in T2; they speculated the precipitate of θ is cathodic to the alloy base, resulting in the anodic dissolution and corrosion of the alloy base at its adjacent periphery [23, 25], and the precipitate of η containing active element Mg is anodic to the alloy base, anodic dissolution and corrosion occur on its surface [22, 23]; and they deduced the anodic dissolution of S cause its pitting corrosion [23, 25, 29]. Lv found the corrosion resistance of the 2099 Al–Li alloy was improved by grain refinement and refined precipitation phases due to decreasing of electron work function and the forming of thicker passive film [30]. Navaser inferred in the heat affected zone the corrosion attack was pitting corrosion no intergranular corrosion was detected [39]. Ma considered the copper-rich nanoparticles support local cathodic reactions, which support the anodic dissolution of the adjacent aluminum matrix [33, 34].The variety of corrosion of Al–Li alloys has been publicly reported in the past few decades, however, salt spray corrosion of these alloys has not been extensively studied. In this study, we investigated salt spray corrosion behavior of 2060 Al–Li alloy in an aggressive environment, analyzed phases, and microstructures of corrosion products after salt spray corrosion.


## 2. Materials and Experimental Procedures

The chemical composition of the 2060-T8 Al–Li alloy is listed in Table1. The metallographic image of the 2060-T8 alloy after Keller reagent treating is shown in Figure 1, which shows that the alloy is mainly composed of fine equiaxed grain and large elongated grain. Specimens were cut to 10 × 10 × 2 mm3 for salt spray corrosion. The backsides and rims of these specimens were mounted in an epoxy resin, leaving an exposed area of about 1.0 cm2. Then, these specimens were ground using SiC sandpaper from 600 to 2000 grit and polished using 0.5 μm Al2O3 paste, cleaned ultrasonically in ethanol, and finally dried with compressed nitrogen before use. The processes for continuing salt spray corrosion were performed in salt spray chamber with salt fog deposition rate of 1.5 mL/cm2·h in accordance to the given ASTM-B117 standard in an electrolyte solution at room temperature. The electrolyte solution with pH about 4.0 was prepared by mixing 0.3 M borate (buffer material), 0.5 M sodium chloride, and 1L deionized water. After salt spray corrosion, the specimens were saved in a glove chamber.Table 1
Nominal composition of 2060-T8 Al–Li alloy, wt%.
ElementCuLiMgMnZnAgZrAl%3.950.750.850.30.40.250.1BalanceFigure 1
Metallographic image of 2060-T8 alloy after Keller reagent treating.Before or after salt spray corrosion, the mass of the specimens was weighted by XP 408 weighing balance. The compositions and microstructures of corrosion products formed on 2060-T8 Al–Li alloy after salt spray corrosion were characterized using Carl-Zeiss field emission scanning electron microscope (FE-SEM) at an accelerating voltage of 20 kV equipped with Oxford light elements energy dispersive spectrometry (EDS) detector. The phases of corrosion product were analyzed using PAN analytical model X-ray diffractometer (XRD) with Cu K-radiation between 3° and 90°. Water contact angle tests were performed on a contact angle analyzer (JC2000 C).


## 3. Results and Discussion

### 3.1. Formation and Evolution Model of Salt Spray Droplet

Corrosive property is dependent on the presence of chloride ions, which causes pit nucleation; the presence of humidity, which cause galvanic corrosion; and the drying phase, which trap chloride ions beneath the corrosion by-products [13, 40]. The sizes and areas of slat spray droplets can influence the corrosion characterization of 2060-T8 Al–Li alloy. A formation and evolution model of salt spray droplets was established. As shown in Figure 2, at the beginning stage, the salt spray droplets adsorbed and spread on the surface of this alloy, and the sizes and areas of salt spray droplets were very small and discrete (Figure 2(a))). As salt spray time increases, the sizes and areas of the salt spray droplets increase, because part of the smaller salt spray droplets get together to form larger salt spray droplets (Figure 2(b))). After that, the sizes and areas of the salt spray droplets change much larger, because part of the smaller or larger salt spray droplets deeply get together (Figure 2(c))). Finally, the length, width, and thickness of a single salt spray droplet become larger, so that most parts of the surface were covered with the larger salt spray droplets (Figure 2(d)). The smaller the size, the smaller the coverage area, the lower the chloride ion content, and the fewer corrosion products; the larger the size, the larger the coverage area, the higher the chloride ion content, and the more corrosion products. Water contact angle at different salt spray time is shown in Figure 3. At a short time, the surface is very smooth and a little corrosion product can form, the contact angle is larger. For a long time, the surface is rough, and many corrosion product can form, the contact angle is smaller, which accelerates the attachment of salt spray droplets. As shown in Figure 4, we obtained superficial morphology of Al–Li alloy at different salt spray time, which is accordance to the model of salt spray droplets.Figure 2
The formation and evolution model of salt spray droplets: (a) salt spray droplets adsorbed and spread on the surface; (b) the smaller salt spray droplets get together to form larger droplets; (c) part of the smaller or larger salt spray droplets deeply get together; (d) most part of the surface was covered with the larger salt spray droplets.Figure 3
The water contact angle at 0.5 h and 8h.Figure 4
Superficial morphology of Al–Li alloy at different salt spray time.


### 3.2. Mass vs. Time Behavior of Corrosion Product

Mass of corrosion product formed on 2060-T8 Al–Li alloy has been determined by XP 408 weighing balance. As shown in Figure5, the formation of corrosion product can be divided into three stages during salt spray corrosion. In the first stage (from 0.5 to 8 h), the mass of corrosion product increases with a highest slope; in the second stage (from 8 to 32 h), it increases slowly with a lowest slope; in the third stage (from 32 to 72 h), it increases faster than the second stage but slower than the first stage with a medium slope. As we all known, the 2060-T8 Al–Li alloy was covered with a thin layer of contact alumina passive film with Al and O atoms as the main compositions. After the compact alumina film is destroyed, active metal atoms of Al–Li alloys (i.e., Li, Mg) are directly contact with electrolyte solution containing aggressive ions (i.e., Cl-, Br-), which leads to active metal atoms dissolved and corrosion product formed on the alloys [41–43].Figure 5
Mass vs. time of corrosion product formed on 2060 Al–Li alloy after salt spray corrosion.


### 3.3. XRD Spectra of Corrosion Products

This passive behavior of Al–Li alloys is attributed to a duplex film, with an inner compact part composed of Al2O3.xH2O and an outer porous part composed of and Al2O3.xH2O [40, 44–49]. XRD spectra was conducted to identify the phase of corrosion product after salt spray corrosion at different time. The XRD patterns of 2060 Al–Li alloy at different time are shown in Figure 6. 2060-T8 Al–Li alloy contains a lot of precipitate phases (e.g., δ (Al3Li), θ(Al2Cu), T1(Al2CuLi) and S (Al2CuMg) phase), which is consistent with reported literature [1–9]. After salt spray corrosion, the diffraction peak of T1 and δ phase disappeared, which means that the first dissolution occurs at T1 or δ phase, as reported in the public literature [19–26]. There are no obvious diffraction peaks from 3 to 25°, which means the presence of amorphous microstructure formed on the surface of this alloy. We discovered that corrosion products mainly contained monoclinic Al2O3, aluminum hydroxide cubic Al(OH)3, and hexagonal AlOOH phases. Davo thought the pH increase permits the precipitation of a porous and open Al(OH)3 compounds, which is corresponding to the voluminous nonprotective aluminum oxides/hydroxides [18]. Bockris also discovered that it is of a porous outer layer, which consists predominantly of Al(OH)3 and (Al2O3), and an inner layer, which is a mixed crystal of (Al2O3) and AlOOH [48]. As the increasing of salt spray time, the phase angle of A12O3 shifts slightly to the left at 31.8°. There is a tensile stress in the A12O3 layer. As the salt spray time increases, the compact A12O3 passivity film becomes thinner, the morphologies changed from compact to porous, resulting in an increase in tensile stress. After 0.5 hour corrosion, no diffraction peak of A12O3 was found, we think that there is a crystal phase transition. The phase angle of A12O3 or AlOOH first shifts to the left, then to the right at 38.6°; at the same time, the peak intensity first increases and then decreases. We thought at the beginning that the tensile played a leading role. When the time exceeds 4 hours, compressive stress plays a major role. When the salt spray time was less than 4 hours, the AlOOH phase appeared and grew up with time increasing, and then changed into A12O3 or Al(OH)3 phase. Therefore, when the corrosion time exceeded 4 hours, diffraction peaks of Al(OH)3 were discovered and Al(OH)3 was formed on the surface of 2060-T8 Al–Li alloy, which is in accordance with the reported [18, 33, 40, 45–49].Figure 6
XRD patterns of 2060 Al–Li alloy at different time.


### 3.4. Morphology of Corrosion Products

Individual specimens were examined to determine the surface morphology of corrosion product formed on the 2060-T8 alloy at different salt spray corrosion time. As shown in Figure7, there was difference in the areas and distributions of corrosion products. After a shorter time, there were almost a few corrosion products formed on this alloy. After salt spray corrosion time over 24h, severe corrosion occurs, and parts of corrosion products peeled off from the surface of specimen. Spalling corrosion products accumulated on the surface of this alloy, and cracks in the form of mud-cracking were found on the surface of alloys. The oxidation film exposed to salt spray as a sacrificial anode to protect basic metal. The gelatinous Al(OH)3, which is pumped out by pits dries up eventually and cracks [25–28]. The corrosion products covered the cracks and pores so that the numbers of the cracks and pores seemed apparently smaller. Cheng et al. thought it may be a result of continuous dissolution of the metal elements on the alloy surface [1, 37]. Meanwhile, chloride anions migrate from surface electrolytes into corrosion product layer to keep electrical neutrality and lead to form second powdery aspect corrosion products on the top of corrosion cracks. Gharbi proposed a highly heterogeneous surface, with the evidence of surface mud or cracking feature, was induced by the dehydration of the hydroxide film or several precipitate particles on the surface [28]. Ma thought the distribution of surface cracks also depends on grain orientation [33, 34]. Local breakdown of some corrosion products leads to abrupt potential drops, which associated with an initiation of localized corrosion attack along the grain boundaries. Network cracking of corrosion products appears at part of specimen. It is believed that the cracks were introduced after water evaporation [30]. Subsequently, the corrosion products represented as dry mud grooves or cracking feature [18]. Cheng et al. thought it may be a result of continuous dissolution of the metal elements on the alloy surface [1, 37]. Meanwhile, chloride anions migrate from surface electrolytes into corrosion product layer to keep electrical neutrality and lead to form second powdery aspect corrosion products on the top of corrosion cracks. Gharbi proposed a highly heterogeneous surface, with the evidence of surface mud or cracking feature, was induced by the dehydration of the hydroxide film or several precipitate particles on the surface [28]. Ma et al. thought the distribution of surface cracks also depends on grain orientation [33, 34]. We obtained the three-dimensional (3D) images at 48h and 72h to reveal the surface of the localized corroded areas, as shown in Figure 8, which displayed that the time of salt spray droplet had an effect on depth of corrosion. We found that the time was shorter, the depth of pit cavity was less. As shown in Figure 9, we have performed the surface elemental distribution analysis on the surface of Al–Li alloy, we found that the surface elements were Mg,O, Cu, Cl, and Al, which showed the corrosion product formed on the surface.Figure 7
SEM images of corrosion product of 2060 Al–Li alloy after salt spray corrosion at different times: (a) 1, (b) 2, (c) 4, (d) 8, (e) 16, (f) 24, (g) 32, (h) 48, and (i) 72h.Figure 8
Image of three-dimensional (3D) profiles of sample surfaces.Figure 9
Element distribution map at 1 hour.


## 3.1. Formation and Evolution Model of Salt Spray Droplet

Corrosive property is dependent on the presence of chloride ions, which causes pit nucleation; the presence of humidity, which cause galvanic corrosion; and the drying phase, which trap chloride ions beneath the corrosion by-products [13, 40]. The sizes and areas of slat spray droplets can influence the corrosion characterization of 2060-T8 Al–Li alloy. A formation and evolution model of salt spray droplets was established. As shown in Figure 2, at the beginning stage, the salt spray droplets adsorbed and spread on the surface of this alloy, and the sizes and areas of salt spray droplets were very small and discrete (Figure 2(a))). As salt spray time increases, the sizes and areas of the salt spray droplets increase, because part of the smaller salt spray droplets get together to form larger salt spray droplets (Figure 2(b))). After that, the sizes and areas of the salt spray droplets change much larger, because part of the smaller or larger salt spray droplets deeply get together (Figure 2(c))). Finally, the length, width, and thickness of a single salt spray droplet become larger, so that most parts of the surface were covered with the larger salt spray droplets (Figure 2(d)). The smaller the size, the smaller the coverage area, the lower the chloride ion content, and the fewer corrosion products; the larger the size, the larger the coverage area, the higher the chloride ion content, and the more corrosion products. Water contact angle at different salt spray time is shown in Figure 3. At a short time, the surface is very smooth and a little corrosion product can form, the contact angle is larger. For a long time, the surface is rough, and many corrosion product can form, the contact angle is smaller, which accelerates the attachment of salt spray droplets. As shown in Figure 4, we obtained superficial morphology of Al–Li alloy at different salt spray time, which is accordance to the model of salt spray droplets.Figure 2
The formation and evolution model of salt spray droplets: (a) salt spray droplets adsorbed and spread on the surface; (b) the smaller salt spray droplets get together to form larger droplets; (c) part of the smaller or larger salt spray droplets deeply get together; (d) most part of the surface was covered with the larger salt spray droplets.Figure 3
The water contact angle at 0.5 h and 8h.Figure 4
Superficial morphology of Al–Li alloy at different salt spray time.


## 3.2. Mass vs. Time Behavior of Corrosion Product

Mass of corrosion product formed on 2060-T8 Al–Li alloy has been determined by XP 408 weighing balance. As shown in Figure5, the formation of corrosion product can be divided into three stages during salt spray corrosion. In the first stage (from 0.5 to 8 h), the mass of corrosion product increases with a highest slope; in the second stage (from 8 to 32 h), it increases slowly with a lowest slope; in the third stage (from 32 to 72 h), it increases faster than the second stage but slower than the first stage with a medium slope. As we all known, the 2060-T8 Al–Li alloy was covered with a thin layer of contact alumina passive film with Al and O atoms as the main compositions. After the compact alumina film is destroyed, active metal atoms of Al–Li alloys (i.e., Li, Mg) are directly contact with electrolyte solution containing aggressive ions (i.e., Cl-, Br-), which leads to active metal atoms dissolved and corrosion product formed on the alloys [41–43].Figure 5
Mass vs. time of corrosion product formed on 2060 Al–Li alloy after salt spray corrosion.


## 3.3. XRD Spectra of Corrosion Products

This passive behavior of Al–Li alloys is attributed to a duplex film, with an inner compact part composed of Al2O3.xH2O and an outer porous part composed of and Al2O3.xH2O [40, 44–49]. XRD spectra was conducted to identify the phase of corrosion product after salt spray corrosion at different time. The XRD patterns of 2060 Al–Li alloy at different time are shown in Figure 6. 2060-T8 Al–Li alloy contains a lot of precipitate phases (e.g., δ (Al3Li), θ(Al2Cu), T1(Al2CuLi) and S (Al2CuMg) phase), which is consistent with reported literature [1–9]. After salt spray corrosion, the diffraction peak of T1 and δ phase disappeared, which means that the first dissolution occurs at T1 or δ phase, as reported in the public literature [19–26]. There are no obvious diffraction peaks from 3 to 25°, which means the presence of amorphous microstructure formed on the surface of this alloy. We discovered that corrosion products mainly contained monoclinic Al2O3, aluminum hydroxide cubic Al(OH)3, and hexagonal AlOOH phases. Davo thought the pH increase permits the precipitation of a porous and open Al(OH)3 compounds, which is corresponding to the voluminous nonprotective aluminum oxides/hydroxides [18]. Bockris also discovered that it is of a porous outer layer, which consists predominantly of Al(OH)3 and (Al2O3), and an inner layer, which is a mixed crystal of (Al2O3) and AlOOH [48]. As the increasing of salt spray time, the phase angle of A12O3 shifts slightly to the left at 31.8°. There is a tensile stress in the A12O3 layer. As the salt spray time increases, the compact A12O3 passivity film becomes thinner, the morphologies changed from compact to porous, resulting in an increase in tensile stress. After 0.5 hour corrosion, no diffraction peak of A12O3 was found, we think that there is a crystal phase transition. The phase angle of A12O3 or AlOOH first shifts to the left, then to the right at 38.6°; at the same time, the peak intensity first increases and then decreases. We thought at the beginning that the tensile played a leading role. When the time exceeds 4 hours, compressive stress plays a major role. When the salt spray time was less than 4 hours, the AlOOH phase appeared and grew up with time increasing, and then changed into A12O3 or Al(OH)3 phase. Therefore, when the corrosion time exceeded 4 hours, diffraction peaks of Al(OH)3 were discovered and Al(OH)3 was formed on the surface of 2060-T8 Al–Li alloy, which is in accordance with the reported [18, 33, 40, 45–49].Figure 6
XRD patterns of 2060 Al–Li alloy at different time.


## 3.4. Morphology of Corrosion Products

Individual specimens were examined to determine the surface morphology of corrosion product formed on the 2060-T8 alloy at different salt spray corrosion time. As shown in Figure7, there was difference in the areas and distributions of corrosion products. After a shorter time, there were almost a few corrosion products formed on this alloy. After salt spray corrosion time over 24h, severe corrosion occurs, and parts of corrosion products peeled off from the surface of specimen. Spalling corrosion products accumulated on the surface of this alloy, and cracks in the form of mud-cracking were found on the surface of alloys. The oxidation film exposed to salt spray as a sacrificial anode to protect basic metal. The gelatinous Al(OH)3, which is pumped out by pits dries up eventually and cracks [25–28]. The corrosion products covered the cracks and pores so that the numbers of the cracks and pores seemed apparently smaller. Cheng et al. thought it may be a result of continuous dissolution of the metal elements on the alloy surface [1, 37]. Meanwhile, chloride anions migrate from surface electrolytes into corrosion product layer to keep electrical neutrality and lead to form second powdery aspect corrosion products on the top of corrosion cracks. Gharbi proposed a highly heterogeneous surface, with the evidence of surface mud or cracking feature, was induced by the dehydration of the hydroxide film or several precipitate particles on the surface [28]. Ma thought the distribution of surface cracks also depends on grain orientation [33, 34]. Local breakdown of some corrosion products leads to abrupt potential drops, which associated with an initiation of localized corrosion attack along the grain boundaries. Network cracking of corrosion products appears at part of specimen. It is believed that the cracks were introduced after water evaporation [30]. Subsequently, the corrosion products represented as dry mud grooves or cracking feature [18]. Cheng et al. thought it may be a result of continuous dissolution of the metal elements on the alloy surface [1, 37]. Meanwhile, chloride anions migrate from surface electrolytes into corrosion product layer to keep electrical neutrality and lead to form second powdery aspect corrosion products on the top of corrosion cracks. Gharbi proposed a highly heterogeneous surface, with the evidence of surface mud or cracking feature, was induced by the dehydration of the hydroxide film or several precipitate particles on the surface [28]. Ma et al. thought the distribution of surface cracks also depends on grain orientation [33, 34]. We obtained the three-dimensional (3D) images at 48h and 72h to reveal the surface of the localized corroded areas, as shown in Figure 8, which displayed that the time of salt spray droplet had an effect on depth of corrosion. We found that the time was shorter, the depth of pit cavity was less. As shown in Figure 9, we have performed the surface elemental distribution analysis on the surface of Al–Li alloy, we found that the surface elements were Mg,O, Cu, Cl, and Al, which showed the corrosion product formed on the surface.Figure 7
SEM images of corrosion product of 2060 Al–Li alloy after salt spray corrosion at different times: (a) 1, (b) 2, (c) 4, (d) 8, (e) 16, (f) 24, (g) 32, (h) 48, and (i) 72h.Figure 8
Image of three-dimensional (3D) profiles of sample surfaces.Figure 9
Element distribution map at 1 hour.


## 4. Formation Mechanism of Corrosion Product

The salt spray droplets dissolving a lot of chloride ions, which can adhere, spread out, and cover the most surface of 2060-T8 Al–Li alloy, as shown in Figure1. The chloride ions can migrate from the solution to the passivity film, break down the compact passivity film, resulting in active metal atoms directly exposed to chloride ions and the corrosion occurrence on the surface of this alloy. In the initial corrosion process, the pH value is lower, anodic reaction occurs due to the first dissolution of T1 or δ phase. The dissolution mechanism of this alloy in an acid condition is as follows [40–49]:(1)Liss⟶Li+aq+e−(2)H2O⟶H+aq+OH−aqwhere H+(aq) is the hydrogen ion in the aqueous solution, OH−(aq) represents the hydroxyl ion in the aqueous solution, and Li(ss) is the active element in the T1, T2, or δ phase.After the active Li element disappears, amounts of hydrogen ions are consumed and gas bubbles are generated, which makes the value of pH increases [4]. H2(g) is the gas due to the galvanic chemical reactivity.(3)H+aq+e−⟶H2g↑When the aluminum element in this alloy matrix begins to be dissolved, and transfers into solution, it causes the aluminum matrix to be corroded [40–50].(4)AI+ss⟶AI3+aq+3e−After the aluminum ions migrate into the solution, aluminum ions react with hydroxyl ion, in a short time, the content of hydroxyl ion in solution is lower, resulting in forming AlOH2+. The reaction is as follows:(5)AI3++OH−⟶AIOH2+The content of hydroxyl ion and the value of pH in solution increase with the time increasing, then AlOOH is formed, as shown in Figure3, and the reaction is(6)AI3++OH−⟶AIOOH+H+At the same time, the reaction is occurring:(7)AIOH2++Cl−⟶AlOHCl+(8)AlOHCl++Cl−⟶AlOHCl2When the value of pH exceeds 7, the Al(OH)3 phase can be formed, as shown in Figure 6:(9)AlOHCl++2OH−⟶AlOH3+Cl−(10)AlOHCl2+Cl−⟶AlCl3+OH−(11)AlCl3+3H2O⟶AlOH3+3HClThe Al(OH)3 phase may come from the AlOOH phase, and the reaction is(12)AlOOH+H2O⟶AlOH3The Al(OH)3 can decompose into Al2O3, and the reaction is as follows:(13)2AlOH3⟶Al2O3+3H2O


## 5. Conclusions

(1)
The corrosion product growth rate can be divided into three stages: in the first stage, it increased exponentially with time during the first 8 h; in the second stage, it increased linearly with a lower slope from 8 to 32 h; and, in the last stage, it changed linearly with a higher slope than the second stage from 32 to 72h.(2)
The main phases of corrosion products were Al2O3, Al(OH)3, and AlOOH phases. As the increasing of salt spray time, the phase angle of A12O3 shifts slightly to the left at 31.8°, and the phase angle of A12O3 first shifts to the left, then to the right at 38.6°.



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*Source: 8926780-2022-06-28.xml*