Evolution and stability of 2-mercaptobenzimidazole inhibitor film upon Al alloy 6061

Organic corrosion inhibitors have become competent alternatives to hazardous chrome conversion coatings due to their rapid adsorption over metal surfaces in corrosive environments. Literature suggests a wide range of organic corrosion inhibitors with high inhibition efficiency, barrier properties, and adsorption mechanisms. However, the long-term durability and protectiveness of an organic inhibitor film need to be understood with in-depth insights on its interaction with heterogenous alloy surfaces like AA6xxx, reduction of galvanic activities and time-resolved degradation due to ionic diffusion. The present article is focused on the time-resolved adsorption and degradation of 2-mercaptobenzimidazole (2-MBI)-induced inhibitor layer/film over AA6061 in 0.1 M NaCl solution. Electrochemical and surface analysis data indicate that the presence of 2-MBI drives the rapid formation of a 20–30 nm thick protective film comprised of constitutional elements of C, S, and N from 2-MBI upon the surface of AA6061 substrate. This film mitigated the corrosion cells associated with nano- and micro-sized Fe and Si-rich intermetallic particles (IMPs) in AA6061. XPS reveals two distinguished bonding states of S and N in the inhibitor film and chemical interactions between 2-MBI and the surface of AA6061. The protective film maintained 65% inhibiting efficiency after 1 day, which progressively degraded due to electrolyte ingress and eventually with a drop in inhibition efficiency down to 21% after 14 days. Inhibitor-induced film over AA6061 reduced the corrosion susceptibility of Fe, and Si-rich IMPs up to 1 day given the subsequent adsorption by S and N heteroatoms. However, this film became thick and defective after 1 day, which undermined its barrier properties against ingress of aggressive ions and facilitated water adsorption.


Introduction
Organic film-forming corrosion inhibitors are popular with coating technologies for their rapid adsorption over metal surfaces. Over the last decades, these have been extensively studied to protect heterogenous Al alloys as conventional chrome conversion coatings are hazardous to human health and the environment [1][2][3][4][5]. However, a limited number of studies reported the inhibitory efficiency of corrosion inhibitors on high-strength Al alloys 6xxx (AA6xxx) series [6][7][8][9][10][11], and the adsorption and durability of organic corrosion inhibitors in corroding environments need to be well understood. Comprehensive and in-depth investigation of film-forming organic inhibitors is required to understand film thickness, film chemistry, and the consequent barrier properties of an inhibitor film over an extended period [9,10]. It is critical to understand inhibitor interactions with an oxide layer and other available surface species, the breakdown mechanism of established inhibitor film and the role of ionic diffusion therein, and the changing coverage IMPs of inhibitors and the impact of such coverage on micro galvanic or nano galvanic couplings [12,13]. Systematic studies on the long-term behavior of such inhibitor systems in terms of film stability, durability, and breakdown should address existing knowledge gaps and develop sound systems with inhibitor layers promoting sustained inhibition efficiency.
AA6xxx possesses better corrosion resistance than their high-strength Al alloy counterparts, even given the presence of several IMPs within the Al matrix [14][15][16]. These IMPs are categorized as coarse constituent AlFeMnSi (α-phase), metastable or stable precipitates of Mg 2 Si (β-phase), pure Si particles, Al 5 Cu 2 Mg 8 Si 6 (Q-phase), Al 2 Cu (θ-phase), and Al 2 CuMg (S-phase), respectively. Most of these IMPs are either cathodic or anodic to the surrounding Al matrix and can initiate pitting in the adjacent matrix [17][18][19]. It has been reported that Mg 2 Si acts as an "anode" owing to the anodic corrosion potential to Al. Therefore, these IMPs preferentially dissolve with respect to the Al matrix in neutral and acidic NaCl solutions [15,[20][21][22]. In alkaline NaCl solutions (pH > 12), Mg 2 Si exhibits passivity and turns into "cathode", and Al matrix becomes anode [14]. Cathodic partial reactions could facilitate OH − (hydroxyl ion) generation and subsequent rise in pH [23,24]. Given the amphoteric nature of aluminium oxides, high pH values degrade oxide layers and thus expose bulk Al for further anodic dissolution. Therefore, Al matrix preferentially dissolves at the periphery of Mg 2 Si in AA6xxx. A good number of publications have confirmed that Mg 2 Si dissolves by preferential Mg dissolution, which leaves Si-rich remnant that is immune to further corrosion reactions [14,22,25,26]. Therefore, providing a barrier effect could be helpful to reduce the galvanic activity of IMPs where film-forming organic corrosion inhibitors could play a key role by rapidly adsorbing over IMPs in corrosive environments and mitigating the overall corrosion rate of AA6xxx. Limiting IMP activities by organic inhibitor adsorption has been minimally reported in the literature for AA6xxx [9,27].
The critical issues addressed in most inhibitor studies include reducing corrosion current density, enhanced polarization resistance, and the existence of non-ideally behaved capacitance of inhibitor films/layers [28][29][30][31][32][33]. The electrical parameters associated with an inhibitor-induced protective layer could provide a quantitative view of the corrosion resistive properties of an applied inhibitor. Alterations of these parameters in long durations tests (up to 14 days) could be crucial in understanding the surface reactions occurring on the substrate surface. The resistance offered by an inhibitor-derived layer could be represented by multiple resistive elements that are summed up to calculate the polarization resistance of the system, which is one of the indicators of long-term durability [34]. Therefore, time-resolved changes of polarization resistance coupled could provide critical information about the inhibitor coverage above the substrate surface and subsequent diffusion of aggressive ions through an inhibitor layer/coating. The constituent parameters of polarization resistance need to be discussed individually for a deeper understanding of the durability of corrosion inhibition. For instance, a barrier against charge transfer of a working electrode refers to the resistance of a metal-coating interface against ionic diffusion and desorption of water molecules [35,36]. Charge transfers resistance (R ct ) is one of the important parameters to look at during electrochemical analysis over the long-term, which has been minimally reported for AA6xxx [9,27]. Moreover, capacitive elements of an electrochemical system represent the homogeneity of its coverage over a substrate surface. It could be predicted to some extent by the ideality of respective quantified parameters [37]. Therefore, the deviation of capacitive elements from the behavior of an ideal capacitor with time needs to be taken into consideration during electrochemical analysis.
A large number of literatures on corrosion inhibition focused on the exposure of metal substrate directly to inhibited electrolyte and then measured electrochemical parameters at different periods [38][39][40][41]. In most of these studies, the working electrode was exposed to inhibited electrolyte, and electrochemical data were acquired at different time intervals to evaluate any inhibitor-induced layer's inhibition effect and barrier properties. However, the interactions of inhibitor molecule with working electrode could be different if it is exposed inhibitor-treated corrosive electrolyte without any external electrical connections, i.e. three cell electrode arrangements. Therefore, time-resolved growth monitoring could be more reliable if alloy substrate is exposed to inhibited electrolyte solution and then pulled out from that environment periodically, followed by electrochemical measurements using an electrolyte solution without inhibitor. Remarkably, this aspect has not been well reported in the open literature. Furthermore, the electrochemical properties of an inhibitor layer/coating critically depend on the adsorption criterion of inhibitor molecules, its influence on reducing the nano and micro galvanic activities around IMPs, and time-dependent change in the coating/layer thickness and composition.
Heterocyclic organic compounds have been numerously reported for corrosion mitigation of Cu, Au, and Fe alloys. The adsorption mechanisms have been explained by the interaction of electron-rich ligands with bulk metal [39,[42][43][44]. Azole-based heterocyclics, especially 2-MBI, have attracted corrosion researchers' interest due to their rapid film-forming behaviour over Cu-rich IMPs of aerospacegrade AA2024 alloy [45][46][47][48]. The growth and stability of 2-MBI film that forms over a metal or alloy substrate could vary as a function of the chemical nature of the electrolyte, interactions between inhibitor molecules with substrate oxide, and exposure time. Cu-free AA6xxx alloys constitute Fe, Si, and Mn-rich intermetallic phases. Therefore, the adsorption of 2-mercaptobenzimidazole (2-MBI) molecules could be investigated for any distinguishable change in bonding from the topmost inhibitor layer to the innermost metal-inhibitor layer interface. Previously, inhibitor adsorption mechanisms on AA6xxx alloys and the influence of IMPs have been explored with an exposure time ranging from 0 to 168 h. However, those studies were confined mainly to inorganic inhibitors [49,50]. In addition, limited studies have been conducted on organic inhibitors at shorter exposure times (less than 168 h) [9,27]. It is unclear about the growth of a barrier layer by 2-MBI in a corrosive environment. A deep understanding of the mechanisms of inhibitor film growth, stability, and breakdown is beneficial to develop and optimize inhibitor systems for extended use and enhanced durability [51]. Quantum chemical calculations postulate that 2-MBI inhibitor film could have a thickness of 0.75-1 nm when attached to a Cu substrate in a perpendicular orientation within a single layer [52]. However, in real-time conditions, adsorption of organic inhibitor molecules may result in a complex film over a metal substrate due to the presence of a metal oxide layer and electrolyte ions [48,53,54].
An inhibitor film could be a combination of available surface species like oxygen or ions from dissolved IMPs, metal matrix, electrolyte, etc. [12,13]. Available knowledge on 2-MBI inhibitor layer is insufficient to address some key factors when applied on AA6xxx [48,53,54]. These key factors could be the growth of a protective layer in the presence of 2-MBI molecules or barrier properties of that layer against diffusion of electrolyte. Additionally, desorption/adsorption of 2-MBI molecules calculated on relevant electrical parameters and the durability of inhibition due to degeneration of the protective layer could also be useful. Figure 1 hypothetically represents the film formation by an organic inhibitor molecule with a metal surface by interacting with heteroatoms and its breakdown at a longer exposure time. The left-hand side of the figure tentatively depicts the bond formation of an organic inhibitor molecule with a metal surface where the first interaction has been predicted through the bond formation by heteroatoms simultaneously with the metal or metal oxide. A second interaction could also be possible by the physical adsorption of inhibitor molecules, resulting in a complex multilayer film structure. Heterocyclic organic inhibitor molecules have different heteroatoms that could draw the benzene ring's electron clouds towards them and act as charge centers (X, Y & Z from Fig. 1). These charge centers then facilitate weak electrostatic interaction with the underlying metal or oxide, resulting in physical adsorption of inhibitor molecules through Vander walls force [55,56]. Subsequent chemical and physical adsorption of inhibitor molecules could result in a complex, multilayered structure over the substrate surface that may vary over time in bonding environments of heteroatoms [56][57][58][59][60]. This inhibitor film/layer could act as a barrier against charge transfer, i.e. higher polarization resistance, better hydrophobicity, etc. Mechanism of film formation and its structure could be predicted through the micro and nanoscopic surface analysis techniques with complementary electrochemical data. The structure of this film could be varied due to the chemical environment, charge density, and electrostatic interactions between an organic inhibitor molecule and substrate surface. This film/layer (right-hand side) could be porous and defective at longer exposure times due to breaking bonds with metal or oxide. It can be investigated through the quantitative analysis of electrochemical parameters. The available aggressive ions could penetrate this defective layer and accelerate further corrosion reactions at longer exposure times to corrosive electrolytes. In the case of a heterogeneous alloy surface, the formation of an inhibitor film/layer and its degradation with time could be critical due to inhomogeneous surface potential distribution across the surface. Therefore, the knowledge on the mechanism of inhibitor film formation over AA6061 and its durability in a corrosive electrolyte for a longer time could be valuable to current literature.
The present study aims to determine the durability and inhibition mechanism of 2-mercaptobenzimidazole (2-MBI) on AA6061 in 0.1 M NaCl at room temperature. A key component to investigate is the interaction of 2-MBI molecules with AA6061 surface in terms of protective layer formation in a corrosive environment and establishment of barrier properties of 2-MBI to any electrolyte diffusion, interaction with any oxide layer formed, and the durability of the protective film over an exposure period of 14 d. Changes in inhibitor performance with exposure time and the response heteroatoms of 2-MBI upon adsorption were investigated using a range of electrochemical and analytical techniques,

Substrate preparation
AA6061-T6 was used as substrate supplied by Calm Aluminum Pty., Melbourne. The nominal composition of the alloy provided by supplier includes Mn (0.10 wt%), Fe (0.20 wt%), Mg (0.80 wt%), Si (0.70 wt%), Cu (0.15%), Zn (0.02 wt%), Cr (0.07%), Ti (0.02%), Al (Balance). Two sets of samples were prepared for electrochemical and surface analysis, respectively. Samples used for electrochemical analysis were cut from the AA6061-T6 rods and then thoroughly cleaned and degreased with acetone, followed by rinsing in deionized water. Samples for surface analysis were ground with Si carbide papers down to 4000 grit, followed by diamond polishing up to 0.25 µm surface finish. Later samples were etched at 60 °C in 10% aqueous NaOH for 45 s, followed by 30 s in concentrated nitric acid at room temperature to remove any surface modifications originated from polishing [9]. All polished samples were cleaned in deionized water, dried, and stored in a desiccator for further use.

Static immersion and electrolyte solution preparation
2-mercaptobenzimidazole (C 7 H 6 N 2 S) (99%) was sourced from Sigma-Aldrich (Australia). NaCl solution (0.1 M) was used in this study, which was based on the fact that a large number of studies used 0.1 M of NaCl solution as corrosion media to examine the inhibitor behaviour with respect to Al and its alloys [61][62][63]. 2-MBI was added to the prepared NaCl solution to a 10 -3 M constant concentration for static immersion. 10 -3 M has been identified as the solubility limit of 2-MBI in NaCl solution. This is the rationale that this concentration was chosen as the optimal concentration for the present work [57,64,65]. To maximize the aqueous solubility of 2-MBI, it was dissolved in 10 ml water inside an ultrasonic bath. Followed by mixing drop by drop in saline solution to the desired concentration. Both sets of samples (electrochemical and surface analysis) were immersed in blank and inhibited NaCl solution and removed periodically from the immersion chambers at day 1, 7 and 14, respectively. This would allow time-resolved comparisons between the inhibitory effect of 2-MBI and blank NaCl solution on AA6061 samples. Then samples were rinsed with deionized water and dried in a nitrogen air flow. Electrochemical and surface characterizations were performed on immersed samples afterward. The samples immersed in inhibited saline solution are termed "inhibited" and their counterparts immersed in blank saline solution as "uninhibited" hereafter.

Electrochemical analysis
Electrochemical tests were conducted by Biologic potentiostat with a conventional three electrode arrangement. A Ag/AgCl electrode (with supersaturated KCl as electrolyte), a platinum mesh and AA6061 specimen were used as reference, counter, and working electrodes, respectively. The exposed area of the working electrode was 0.74 cm 2 (1 cm in diameter). Open circuit potential (OCP) was stabilized for 90 min prior to the electrochemical measurements.
Cathodic potentiodynamic polarization tests were carried out over the voltage range of − 0.7 to + 0.2 V vs OCP, and anodic potentiodynamic polarization tests were performed within a voltage range of + 0.7 to − 0.2 V vs OCP. The scan rate of 5 mV/s was employed on two different set of samples (different samples for cathodic and anodic scans). The chosen scan rate was faster than the usual for Tafel plots. However, this has been reported to be typical for 6xxx aluminum alloys [66,67].
Polarization resistance (R pol ) measurements were conducted by the cyclic polarization technique. Measurements were taken every 2.5 h up to 22 h. The test amplitude was ± 15 mV relative to the OCP with a scan rate of 0.167 mV s −1 .
Electrochemical impedance spectroscopy (EIS) was executed from a frequency range of 1 MHz to 10 mHz, employing 10 mV sinusoidal perturbation potential at OCP with 10 points per decade. EIS results were recorded every 3 h over 21 h. EC-Lab version V 11.27 was used for data fitting. All electrochemical measurements were performed at room temperature. All the electrochemical tests were triplicated to maintain the reproducibility of data. Uninhibited and inhibited samples were taken for cross-sectional and surface analysis studies after immersion to respective solutions.

pH measurements
pH measurements were made on static immersion solutions with AA6061 samples using a Toledo pH-meter at day 0, 1, 7, and 14 to observe and record the change in pH values with time.

Focus ion beam scanning electron microscopy & EDS (FIB-SEM EDS)
FIB-SEM images were taken at high magnifications (10 k to 850 k ×) using FIB milling by SCIOS FIB dual-beam SEM. The details of the technique have been reported in our previous article [16].

3
TEM lamellae were prepared from the inhibited AA6061 samples with FIB milling. A few selected zones were chosen randomly from the alloy surface, and Auto-TEM G2 mode was employed to prepare TEM-lamella. To protect surface layer present over the sample surface, 100 nm thick Pt layer was deposited over the selected areas by electron beam prior Auto-TEM procedure. The dimensions of TEM-lamella were set as 12 µm × 3 µm × 500 nm using a depth correction of 1.5 µm and a final thickness of 2 µm. Polishing of the lamellae was conducted with a Ga ion beam at 30 kV with 50 nA beam current, which was finally reduced up to 10 pA. Stan detector was used to acquire transmitted electrons through the samples and create high-angle annular dark-field images (HAADF) at higher magnification up to 3,500,000 times. After HAADF image acquisition, J cut lamella were welded to the micromanipulator of the FIB instrument and pulled out from the sample. Then the lamellae were welded to the Cu sample holder and stored in a vacuum for TEM/EDS analysis.

Transmission electron microscopy & EDS (TEM-EDS)
TEM was performed with a JEOL 2100F Transmission electron microscope operating at 200 kV, operated in STEM mode with a nominal probe size of 2 nm. The EDX detector was an Oxford Xmax n 80 T.

X-ray photoelectron spectroscopy (XPS) etching
Etching of the inhibited alloy surface were performed by XPS sputtering to reveal the bonding chemistry of different elements at coating-substrate interface. XPS was performed by Kratos AXIS Ultra XPS system (Kratos Analytical Ltd., UK). The spectrometer was equipped with a monochromatic Al Kα (E photon = 1486.7 eV) and an Ag Lα (E photon = 2984.2 eV) X-ray sources. Experimental details have been listed elsewhere [68].

OCP and potentiodynamic polarization scans (PDS)
OCP measurements are presented in Fig. 2a for uninhibited and inhibited conditions. Uninhibited condition seems to be associated with unstable OCP values with a large fluctuation in voltage. Instability in OCP values could be originated from the uneven distribution of local volta potential across the surface. In the case of uninhibited alloy surface, this could be resulted due to breakdown of the oxide layer, presence of localized cathodes and anodes, or generation of positive and negative ions due to cathodic and anodic partial reaction initiated at IMPs (cathode) and bulk Al (anode), respectively [69]. Inhibited saline solution has contributed to shifting the OCP to more positive values in comparison to blank saline solution. With the increment of exposure time, there was the shift of OCP to more negative values i.e. 7 and 14 days, and the instability of OCP is evident from 10 min to the rest of the exposure time. There is a shift of OCP from 0.73 to 0.66 V upon inhibitor addition at 1 day which further dropped down to 0.71 V and 0.73 V at 7 and 14 days, respectively. Corrosion rate of an electrochemical system can be obtained from the PDS curves. Cathodic and anodic polarizations provide the respective corrosion processes occurring in the cathodic and anodic regions of a working electrode [70]. Extrapolation of cathodic and anodic curves in the linear regions to the point of intersection provides both the corrosion potential (E corr ) and the corrosion current (i corr ).
Polarization curves for inhibited and uninhibited samples at 1 day, 7 day, and 14 day exposure are presented in Fig. 2b. The quantified parameters from Fig. 2b has been presented in Table 1. Cathodic shifts in the E corr values can be observed with the addition of the inhibitor for all three time periods (− 0.73 V to − 0.65 V, − 0.68 V and − 0.72 V at time t = 1, 7 and 14 days, respectively). These cathodic shifts suggest that the 2-MBI inhibitor acted as a cathodic inhibitor for the AA6061 system. An i corr value of 0.035 mA cm −2 was observed for uninhibited samples after 1 day. For inhibited conditions, i corr values decreased to 0.012 mA cm −2 after 1d and then increased after 7 day and 14 day with corresponding values of 0.022 mA cm −2 and 0.028 mA cm −2 , respectively. An inhibitor efficiency of 64.7% has been observed in the inhibited condition compared to the uninhibited condition after 1 day. Inhibition efficiency dropped further to 35.7% and 21.0% at 7 day and 14 day, respectively. The potential shift towards the cathodic direction in the case of inhibited samples with higher inhibition efficiencies than uninhibited ones implies the resistive properties of 2-MBI and extended coverage of cathodic areas of the working electrode. All these factors could have some influence on the decrease of charge transfer activities across the working electrode surface. Therefore, the possibility of oxygen interaction with the substrate surface is hindered by providing a barrier effect, thus reducing the current flow, i.e. i corr . Reduction of cathodic current in all inhibited exposure time indicates the reduction of cathodic activities due to the presence of inhibitor molecules. In the case uninhibited sample, E corr was − 0.73 V initially, shifted toward a positive value for inhibited condition at 1 day, and then decreased again for 7 and 14 day. i corr exhibits a similar trend to E corr , implying the formation and later breakdown of the passive layers. For the inhibited AA6061, a significantly positively shifted E corr of − 0.65 V was obtained, confirming an effective corrosion  protection by 2-MBI. The E corr gradually decreased over a long immersion time from 7 to 14 days, indicating the good stability of the 2-MBI-induced protection in a NaCl environment. Further analysis of the cathodic and anodic regions of the curves reveals a decrease in the cathodic Tafel slopes after 7 and 14 days exposure for inhibited samples. Likewise, a reduction in the voltage range of the anodic passive regions for inhibited samples can be observed after 1 day immersion. However, E corr values were shifted negatively in anodic regions from − 0.68 V (7 day) to − 0.72 V after 14 days in the inhibited sample. This could be due to the unstable corrosion products that temporarily shielded the anodic sites of the working electrode that shifted E corr by 0.07 V. The uninhibited sample showed a passive region in the anodic portion extending from -0.7 to − 0.56 V. Identical region was found to be absent in the inhibited sample for the same duration. These regions have slightly reappeared in 7 and 14 days inhibited samples from − 0.6 to − 0.55 V. This passive region could indicate repassivation of anodic sites by the corrosion products.

Electrochemical impedance spectroscopy (EIS)
Impedance responses of the uninhibited and the inhibited alloy surface in the form of Nyquist plots, after 1, 7 and 14 days are presented in Fig. 3a. The corresponding Nyquist response of the uninhibited sample has been provided inset of Fig. 3a because the impedance (Z) values were minimal compared to the inhibited ones. This will help the reader have a quantitative comparison between inhibited and uninhibited samples at longer exposure times.
A metal surface covered with a homogenous coating ideally shows a high impedance in accordance with a simplified Randle's cell. It will possess a single semicircle in the Nyquist plot i.e. a single time constant where the capacitance of the defect-free coating will merge with the inherent metal oxide layer [71]. In that case, the coating and the oxide layer cannot be distinguished by different capacitive elements. However, if the protective layer/coating on the metal surface becomes inhomogeneous and defective, there could be two or more-time constants associated with distinguished semicircles instead of one [72,73].
In an inhomogeneous or defective coating system, semicircles at higher frequency regions are supposed to be absent or depressed. The absence of higher frequency time constants is attributed to a defective coating system where corrosion was mostly occurring under charge transfer control processes [74]. In a porous and defective coating system, resistance associated with pores (R pore ) dictates the time constant at higher frequency regions i.e. high-frequency time constants. A coating system is assumed to be less defective at the initial stages of corrosion processes, showcasing a higher R pore i.e. a time constant in high-frequency regions [75]. With the advancement of time, pores could be generated in the coating structure that facilitates the movement of aggressive ions to the coating-metal interface. Then the Nyquist response results in depressed semicircles with low or medium frequency time constant as the pore resistance decreases. Eventually, it may cause the disappearance of the coating response in the high-frequency region, and the corrosion process could only be controlled by charge transfer processes [72,[75][76][77].
Nyquist plots displayed in Fig. 3a have shown that the AA6061 samples have a flawed or defective coating layer with a porous structure of inhibited and uninhibited conditions [76]. It has been presumed that AA6061 substrate, i.e. working electrode, is covered with inhibitor-oxide layer/ film. It could be comprised of two separate interfaces: metalcoating interface and coating-electrolyte interface. Thus, two semicircles in the Nyquist plots refer to two different responses of the working electrode. The high-frequency semicircle refers to the coating response which is associated with coating capacitance (Q oxide/inhibitor ) and pore resistance (R pore ). The low-frequency semicircle refers to corrosion processes, i.e. charge transfer resistance (R charge-transfer ) and double-layer capacitance (Q double layer ) [77]. The total resistance of the electrochemical systems in Fig. 3a can be described in terms of polarization resistance Rpol, a summation of all the resistive elements principally act in a faraday cage (R pol = R pore + R charge-tranfer + R solution ) [75].
Exposure of AA6061 to the inhibited 2-MBI electrolyte for 1 day, results in a significant rise in R pol (polarization resistance) as evidenced by the increased diameter of the semicircle compared to the uninhibited sample (inset of Fig. 3a). It underlines the excellent intrinsic inhibitive properties of 2-MBI, i.e. presence of a protective layer [78]. Uninhibited sample found to be associated with depressed semicircles in Nyquist plots, indicating large drop in R pol values. R pol value is roughly 22 times lower than those observed for inhibited samples at 1 day (Table 2). Uninhibited samples were observed with more depressed semicircles showcasing lower R pol values at 7 and 14 days. It confirms either the absence of a barrier layer or a defective oxide layer. Inhibited samples show a reduction in loop diameters with exposure time, which corresponds to a gradual decrease in R pol values at 7 days and 14 days inhibited sample.
Bode plots are presented in Fig. 3b for different exposure time durations. 2-MBI treated samples show improved low-frequency impedance modulus (lZl) for all exposure times compared to uninhibited ones. lZl gradually drops from ≈10 6 to ≈2.4 × 10 5 Ω for 1 day to 7 days exposure, respectively, for the inhibited conditions. Bode impedance modules further dropped marginally for 14 days inhibited sample to approx. 2.2 × 10 5 Ω. The same has been calculated as 1.2 × 10 5 Ω for uninhibited samples after 1 day. The medium frequency modulus is thought to be associated with the diffusion of different ions through the surface films over a metal substrate. Hence, θ max (medium frequency phase angle maximum) is considered one of the quantitative indicators of the barrier properties of a protective layer that has formed to the ingress of corrosive species [79]. Bode phase angle plots (Fig. 3b) show the (θ max ) for 2-MBI treated samples are typically around 77.5°, 75° and 74.9° for 1, 7, 14 days exposure periods, respectively (Fig. 3b). θ max for the uninhibited condition is found to be 74.8° for the same exposure period of 1 day, which is nearer to values observed for 7 and 14 days. θ max for the uninhibited condition were stable within a narrow frequency range (7 to 14 Hz). In contrast, it is nearly steady over a wider frequency range (3.5 to 950 Hz) for the inhibited samples immersed for 1 day. With the momentum of exposure time, a gradual leftward shift of the phase angle vs. frequency plots of the inhibited system with lower θ max values is evident from the Bode phase angle plots (Fig. 3b).
Time constants are indicators of different electrochemical processes occurring at the substrate surface with or without coating. An electrochemical system's middle and highfrequency time constants correspond to the electrochemical activities of any coating or coverage present over the substrate. The time constants in the low-frequency range correspond to electrochemical activity at the alloy surface, respectively [1]. In this study, both uninhibited and inhibited samples are thought to have mixed surface coverings produced from oxide layer and inhibitor-induced protective layer, respectively. Therefore, the electrical equivalent circuit (EEC) is fitted with two time constant (Fig. 1d), and Warburg resistance is introduced, to represent ionic diffusion through both the oxide layer and the inhibitor-induced layer [47]. All the circuit parameters are defined with the respective abbreviation in Fig. 3c, and the calculated values are presented in Table 2. The constant phase elements (CPE) were used in the EECs to describe the elements as non-ideal capacitors using parameters Q and η [80]. The inhibited system has an additional second time constant describing the electrochemical processes (corrosion) occurring at the aluminium substrate in terms of the pore resistance R pore (Fig. 3d). R pore is the resistance associated with ion-conducting paths that develops in a defective coating that stays on the metal side due to coating degradation [1]. The total value of R pol can be calculated from the summation of R charge-transfer , R pore, and R soultion . R pol values were 13 times higher for the inhibited conditions compared to the uninhibited conditions after 1 day. Figure 4 shows the polarization resistance (R pol ) of the AA6061 aluminum alloy for both uninhibited and inhibited conditions at different exposure times. Polarization resistance data with error bars have been presented in Fig.  S1 of the supplementary material. The main difference in the results is that the uninhibited system falls into range ≈ 3.0 × 10 4 to 1.7 × 10 4 Ω cm 2 . In contrast, the inhibited range is much higher, typically between ≈3.1 × 10 6 to 4.2 × 10 6 Ω cm 2 after 1 day immersion. For the inhibited system, the R pol values were observed to decrease at 7 days with a range of ≈ 3.1 × 10 5 to 2.5 × 10 5 Ω cm 2 and then further slightly dropped within the range of ≈ 2.6 × 10 5 to 2.0 × 10 5 Ω cm 2 after 14 days. Polarization resistance values from LPR and EIS equivalent circuit measurements are in accord with each other. Inhibited system display remarkably higher R pol values compared to the uninhibited system for the 1 day, although the drastic reductions was observed for the inhibited system at 7 days and 14 days. Higher R pol values attributed to the presence of barrier/coating layer over AA6061 in the presence of 2-MBI that gradually dropped with immersion time.

Linear polarization resistance (LPR)
R pol values can correspond to i corr values, therefore higher R pol indicates lower i corr values. It is suggested that lowering R pol , and hence higher i corr for the inhibited system with time, can indicate pores or defects in inhibitor-induced protective layer. These results revealed that inhibitor-induced coating/film provided an effective charge transfer barrier that has reduced over time. It is also evident from the drop of R charge-transfer values in the inhibited condition from 943,922 to 31,655 Ω cm 2 and 26,025 Ω cm 2 after 7 days and 14 days respectively ( Table 2). Diffusion of ions through inhomogeneous inhibitor-induced layer/coating could be one possible reason associated with this gradual drop of R pol [81]. Alterations of R pol values could provide valuable information about the long-term durability of an inhibitor-induced protective layer regarding barrier to oxygen reduction and hydrogen evolution reactions occurring on a metal surface. An identical methodology was reported by Hernadez-Alvarado et al. to study the film stability of a chromate-free corrosion inhibitor on steel for a duration of 140 days [82].
After 7 days, the inhibited sample displayed i corr value of 0.022 mA cm −2 compared with 0.012 mA cm −2 at 1 day, which further drops to 0.028 mA cm −2 after 14 days. These findings accord with the R pol findings as a reduction in R pol remain almost identical for both 7, and 14 days inhibited sample. Lower i corr values and the positive shifts of E corr in the cathodic portion suggest that the inhibitor has a dominant effect on the cathodic part of the polarization curve compared to the anodic part. It can be assumed that the cathodic sites could be obstructed to a greater extent by the inhibitor molecules than the anodic sites [83].

pH measurements
Changes in the pH values with exposure time for both uninhibited and inhibited conditions are presented in Fig. 5. The uninhibited system shows a higher pH value of 6.82 than 6.75 for the inhibited sample with the same exposure time of 1 day. Inhibited system displayed a moderate rise in pH values from 6.79 to 6.90 over the 7 to 14 days period of exposure.

FIB-SEM/EDS, TEM/EDS
A J cut TEM-lamella prepared from 1 day inhibited sample by FIB-SEM instrument is presented in Fig. 6a. A dark continuous layer is evident in the lamella beneath the Pt layer, which is thought to be the protective inhibitor layer that has acted as a barrier against corrosive degradation of AA6061 surface identified by electrochemical analysis. To gain more insights, high-angle annular dark-field image (HAADF) of the selected area (red dotted rectangle) from that lamella is taken using the Stan detector (Fig. 6b) of FIB instrument. The bright layer consists of several white crystals of aluminum oxide or hydroxides embedded in a grey sponge-like inhomogeneous layer. High-resolution TEM images of the same lamella are presented in Fig. 6c and d where the previous bright inhibitor layer has been identified as a continuous grey layer. The white spike-like constituents (blue arrows) are the IMPs distributed heterogeneously across the bulk Al. An EDS line scan of the inhibitor layer (marked by red rectangle) and the IMP beneath that layer (marked by the yellow rectangle) is shown in Fig. 6e and f, respectively. Two principal continents of the 2-MBI are evident from the EDS line scan, i.e. C and S, along with Al and O. Here, the Al signal's intensity is decreased, and the O signal remains stable over the analysis depth. C and S signals followed an identical signal ratio throughout the analysis depth. It could be attributed to the uniform distribution of inhibitor molecules throughout this layer and indicates the presence of inhibitor molecules (reacted or unreacted) over the aluminum oxide layer.
Among the different nano-sized IMPs identified beneath the inhibitor layer, one has been characterized by EDS line spectra nearest to the outermost surface (yellow dotted rectangle in Fig. 6d). The principal constituent of the IMP is found to be Fe, Si, Mn, and Al. This phase is thought to be the precipitates of β-Mg2Si or coarse constituent α-AlFeMnSi characteristic of Cu-free age hardenable AA6xxx alloys. Age hardenable AA6xxx consists of several types of IMPs, namely, coarse constituent α-AlFeMnSi, pure Si particles, and stable/metastable precipitates of β-phase (Mg 2 Si), Q-phase (Al 5 Cu 2 Mg 8 Si 6 ), θ-phase (Al 2 Cu), and S-phase (Al 2 CuMg) [84]. Fe containing particles could originate from impurities in 6xxx series Al alloys and its possible phases could be Al 15    matrix [85,86]. However, the identification of the exact composition of this IMP is beyond the scope of this article. Notably, there was no evidence of selective dissolution of Al in the boundary region. The subsequent enrichment of Si or Fe seemed to be absent in the identified IMP. Our recent study has revealed that AA6xxx exposed to blank 0.1 M NaCl solution has suffered selective dissolution of Al in Fe and Si-rich IMPs at boundary regions and consequent enrichment of nobler constituents [16]. Therefore, the barrier layer produced in the presence of 2-MBI after 1 day has provided adequate coverage to reduce the nano galvanic activity of nobler IMPs to Al matrix and stopped the dissolution of Al [87]. FIB-SEM image of the inhibited AA6061 specimens after 7 day's exposure is shown in Fig. 7a. The FIB milled cross-section of the same area (Fig. 7b) contains a thick film/layer (20-30 nm) over AA6061. This layer has been detected beneath the Pt deposited layer, and it was not uniform in nature. The composition of this bright layer has been confirmed through EDS map spectra. EDS map spectra of Fig. 7b have revealed that this layer consists of S, N, C, with trace amounts of O (Fig. 7c). Al was found to be absent in that thick layer. Beneath that layer, Si and Fe-rich intermetallic particles were unaffected from corrosion attack. The intactness of Fe and Si-rich IMPs has been assured beneath the thick inhibitor layer due to the absence of porous, sponge-like remnants around the IMPs, which are usually associated with the selective dissolution of Al or Mg due to micro galvanic coupling. King and co-workers have observed identical selective dissolution of Cu-rich nobler IMPs of AA2024 exposed to NaCl droplet [88]. Porous and sponge-like remnants were observed in anodic sites (AA2024 matrix) compared to the cathodic IMPs, which were nobler than the matrix. Dealloying of Al and Mg and consequent Cu enrichment were also reported. Figure 8 showcases the 2-MBI induced protective layer in 14 days inhibited sample. This layer seems thicker after 14 days immersion compared to 1 and 7 days. The continuity of this layer seemed to be reduced with time, corroborating the electrochemical analysis findings. The discontinuity of this layer may influence ionic transportation to the bulk alloy surface contributing to the reduction of barrier properties against charge transfer processes. However, the protectiveness of this layer against micro galvanic activity was found to be consistent after 14 days. The intactness of micronized Si and Fe-rich IMP beneath the discontinuous 2-MBI layer duly support this finding. The composition of the protective layer revealed the presence of S, C, and N, which is thought to be originated from the 2-MBI molecules. The increased thickness of the protective layer and the detection of additional N signals could result from physically absorbed 2-MBI molecules. However, the exact composition of this thickened layer is yet to be explored.

XPS etching
XPS wide survey spectra before sputtering has been presented in Fig. 9a. The at% of C found to be highest among the other elements that could be referring to pick up adventitious carbon from the environment in addition to inhibitor molecules. Besides C, S and N have been traced with excess O which could be originated from the oxide layer inherently present over Al surface. The comparative spectrums of inner most and outer most etched layers have been presented in Fig. S2 of supplementary material. Here, both Al 2 s and 2p spectra have been considered as they both indicate the identical bonding environments of Al, reducing the ambiguity originating from Al plasmons.
Sputtering with a gas cluster ion beam (GCIB), the change of Al 2p peak was significant after the first sputtering cycle (Fig. 2a in supplementary material). It shows two prominent peaks of binding energy, 75.64 eV and 72.73 eV for aluminum oxide and metal peaks. The outer most etched layer displays a narrow oxide and a metal peak that gets broader in the inner most layer (Fig. 9b, Ap 2 s). This finding is thought to be related to surface Al's activity increment with available surface elements, i.e. oxygen or 2-MBI, and probable formation of Al-2MBI complex. The latter stages of etching might indicate the partial removal of the Al-2MBI complex from the surface, producing more signals for the Al 2 O 3 and Al underneath the organic inhibitor layer. From the oxide metal peak ratio, the calculated oxide layer thickness was found to be approximately 3.3 nm. Oxide layer thickness has been calculated using the following equation reported elsewhere [89]. Here, d is the oxide thickness in angstrom. I m and I 0 , are the intensities (i.e. peak areas) of the metal and oxide photoelectron peaks, respectively. This layer could be the thickness of the Al-2MBI complex, which is much higher than the perpendicular length of 2-MBI in monolayer orientation. These results indicate having both chemisorbed and physio-absorbed 2-MBI molecules on AA6061.
The dominant C 1 s peak has been observed at 284.8 eV (Fig. 9c). It has been reported previously that 2-MBI solid chemical (powder), can be associated with three deconvoluted peaks referring to three different carbon environments. Here, the peak position at 284.8 eV (Fig. 9c) corresponds to the four carbon atoms in the benzene ring (not bonded to N) and the other two peaks at 286.51 eV 288.46 eV correspond to the C atoms bonded to S and N atoms, respectively. Studies have revealed that upon adsorption 2-MBI on the metal surface, no peak at 288.46 eV should be observed in the C 1 s spectra at all (Fig. 9c) [90][91][92]. The peak at 288 eV in the C 1 s spectrum corresponds to the carboxylic groups [90,[92][93][94]. 2-MBI powder with 99 wt% purity was employed in this study. However, it is possible that it also contained some other oxidized species containing carbon (impurities). Therefore, the peak at 288.46 eV most likely arises due to the presence of oxidized carbonaceous contaminants [12].
The gradual removal of the 2-MBI inhibitor layer by sputter beams shows the possibility of having two N environments (Fig. 9c). As this was not the case for the outermost layer (Fig. S2b of the supplementary material), it is more likely that these two peaks (399.87 eV and 401.02 eV) correspond to two different 2-MBI molecules bonding. Firstly, the topmost position involves the MBI-organometallic complex (401.02 eV), and secondly, 2-MBI molecules bonded with AA6061 substrate that are not engaged in organometallic complexes (399.87 eV) [95]. These two ways of 2-MBI bonding can already be detected simultaneously after sputtering, as seen in Fig. 9d.
A similar shift of the intensive feature is evident in Fig. 9b from the outermost layer to inner most layer, i.e. position for the S 2p spectra. The shift of S 2 s spectra has been presented in Fig. S2c of supplementary material to distinguish S peaks from Al peaks more precisely as S 2p spectra could coincide with Al plasmons. These shifts of the N 1 s and S 2 s support the claims of having two different types of 2-MBI bonding on the AA6061 surface. Moreover, the shape of the S 2p spectra in Fig. 9b matches the S 2p 3/2 and S 2p 1/2 peaks separated by 1.26 eV with an intensity ratio of 1:2 [13,90,96]. The main peak 1 for the 2-MBI solid chemical reported to be located at EB of 162.3 eV (Fig. 9b), which agrees with the position of 2-MBI reported previously [97]. The S 2p peak at 162.80 eV accords with the position for the thiol group, and. Since peaks at higher binding energies were not observed (166-172 eV) in the S 2p spectra, no S oxidation is thought to have occurred [96,[98][99][100]. For sulphonates (oxygenated S), a peak at binding energy more positive than 166 eV have been suggested in previous studies [101]. The change of the S 2 s spectrum in the innermost layer for the inhibited AA6061 suggests S-Al d(A) = 28 ln 1.4I 0 ∕I m + 1 .

3
bonding. Different authors have also reported that bonded thiols in the form of thiolate could be located at lower binding energies compared to unbound thiol molecules where the metal ions replace H from the S-H bond [13,90,102].
In this case, 2-MBI treated AA6061 showcased the features of the thiolate bond at binding energy 164.03 eV.

Formation of a protective inhibitor layer
Open circuit potential measurements (OCP) have predicted the presence of a protective layer that has masked the localized cathodes and anodes and shifted the potential to more positive values. This trend is typical for azole-based organic inhibitors that could minimize the localized cathodic and anodic activities [8,38,103,104]. This surface coverage results in a non-homogenous coating layer protecting the bulk against ionic diffusion [44]. The nature of unstable OCPs at longer immersion times could be associated with the nonuniform nature of the inhibitor coverage on AA6061. The Decline to more negative OCPs at 7 day and 14 day could be associated with thicker and porous inhibitor coverage that allows the diffusion of aggressive ions with time [105]. The presence of a protective layer has also been identified from the improved polarization resistance (R pol ) values observed from Nyquist and Bode plots for the inhibited conditions. Bode impedance plot reveals that low-frequency impedance modulus (/Z/) has increased for the inhibited condition compared to the uninhibited system, mainly attributed to improved corrosion protection through film formation [106]. The improved R pol values up to 1 day could be associated with rapid formation of a protective layer and consequent adsorption of inhibitor molecules to the substrate surface, which is also identified by polarization resistance values observed in Fig. 4. Prakashaiah et al. [107] observed identical findings for AA2024 with three thiosemicarzone derivatives in NaCl solution. They correlated the increased R pol values with the subsequent adsorption of inhibitor molecules to the substrate surface and desorption of water molecules. It is evident from EIS data that the corrosion inhibition provided by 2-MBI on AA6061 remain irreversible up to 1 day. Irreversibility of corrosion inhibition is one of the principle aspects corrosion resistance that is well established for AA2XXX series alloys with different azole derivatives like benzotriazole and 2-mercaptobenzothiazole in saline solutions, unlike AA6XXX [54]. 2-MBI induced inhibitor layer manifests moderate barrier against ionic diffusion in up to 1 day and then degrades gradually up to 14, which is evident from depressed semicircles of Nyquist plots. This could be attributed to the subsequent ingress of aggressive ions through the inhibitor layer that may produce a more porous and defective layer with the progression of time [108].

Structural evaluation of the inhibitor-induced layer from electrochemical measurements
The inhibited system manifested stable θ max values for a wide range of frequencies. Inhibited system was associated with stable θ max for a wide range of frequencies postulating slower diffusion tendency of ionic species through a protective coating [48]. The inhibited system predominantly shows a middle-frequency time constant over a wide frequency range. According to Recloux et al. [48], a time constant with a wide frequency spread could not be specific to either the inhibitive layer or oxide film. Instead, the medium or high-frequency relaxation process (widespread θ max values) could result from both the oxide and inhibitive layer impedance properties. These studies infer the presence of a complex corrosion protective layer that could be comprised of absorbed inhibitor molecules, an oxide layer, or available surface compounds that result in the improved R pol values. This symmetry suggests that there are possibly no overlapping time constants in this frequency range. Visser et al. have investigated AA2024 with different inhibitors up to 168 h and reported that asymmetric phase angle maxima could be due to the presence of two overlapping peaks [1]. It was suggested that this phenomenon referred to a discrete oxide layer beneath the inhibitor layer. Therefore, they have used individual time constants for those overlapping peaks. However, this may not be the case for this study as two well-defined time constants are visible with good symmetry (Fig. 3b). Consequently, the EEC (Fig. 3c) of the inhibited AA6061 is best fitted with two time constants referring to a thick protective layer as observed in the FIB-SEM cross sections. It is evident from Fig. 3b that after 1 day, the inhibited sample has a high-frequency time constant extended with a shoulder expanded from 1000 to 10,000 Hz. This highfrequency shoulder found to be absent in 7 and 14 day. This could be attributed to the gradual diffusion of aggressive ions through the thick inhibitor layer penetrating with time. Aggressive ions might have diffused to the oxide layer (protected beneath absorbed inhibitor molecules), reaching the alloy surface and facilitating its break down. In later stages, the oxide layer could be partially repaired by the inhibitor layer as the Warburg resistance values were higher at 7 day (Table 2) i.e. better resistance to ionic diffusion. Therefore, after 14 days, the substrate surface had a more complex mixed layer and high-frequency shoulder region of the phase angle curve found to be absent. The absence of a high-frequency shoulder region in the phase angle plot could be associated with low pore resistance. This later process also allows more water and aggressive ions to diffuse through to the surface, altering both R pore and R charge-transfer along with the capacitance of both layers. R pore values were found to decrease from 943,922 to 26,025 Ω cm 2 after 14 days inhibited sample ( Table 2), indicative of time-dependent transportation of aggressive ions thought the pores generated inside the coating structure. These findings postulate the porous nature of the inhibitor film after 14 days with a complex chemical composition comprised of oxides and inhibitor elements.

Influence of inhibitor layer on electrochemical parameters and its barrier properties
Nyquist plots have divulged the better R pol (R pol = R pore + R charge-tranfer + R solution ) values for the inhibited sample that could be associated with the emergence of 2-MBI induced protective layer or coexistent inhibitor-oxide mixed layer. The nyquist plot could consist of two semicircles in an inhomogeneous coating system. The semicircle at highfrequency is related to the coating response and the lowfrequency semicircle is related to corrosion processes [73]. The equivalent circuit diagram (EEC) presented in Fig. 3c suggests two related effects occurring on the AA6061 surface. Firstly, a coating builds up over AA6061, and secondly, the active metal surface is gradually covered by inhibitor molecules. The coating layer affects the resistive (R pore ) and a capacitive element (Q inhibitor-oxide ) which attributes to highfrequency responses of Nyquist plots in the inhibited conditions. Tweaking of R pore values ( Table 2) from 54.8 × 10 6 Ω cm 2 (uninhibited) to 72.1 × 10 6 Ω cm 2 (inhibited) confirms the barrier effect of inhibitor layer/film against water adsorption, charge transfer, ingress of aggressive ions. It is also indicative of surface coverage inhibitor molecules after 1 day. However, a drop in R pore values at 7 and 14 days immersed sample indicates gradual loss in protective nature of the inhibitor-induced film/layer due to either ingress of aggressive ions or adsorption of water molecules through the inhibitor-metal interface or both. Another aspect of protectiveness of an inhibitor-induced layer could be the surface coverage of the inhibitor molecules. This could help retract water molecules and counter-ions, declining the double-layer capacitance (Q dl ) and concurrently enhancing the charge transfer resistance. With the inhibitor addition, the available surface area for charge transfer activities decreases, and thus R charge-transfer increases at 1 day and then reduces drastically after 7 days (Table 2). Additionally, after 7 and 14 days the double-layer capacitance (Q dl ) has increased more than 10 times. The progressive rise in the (Q dl ) double-layer capacitance values at 7 and 14 days could indicate water adsorption over AA6061 [109,110]. R charge-transfer values are a useful indicator for the inhibitor performance that ultimately influence the overall corrosion rate. This could be illustrated by exchanging positive and negative charges during the electron-donation and back-donation from the substrate surface and subsequent substrate diffusion into the corrosive electrolyte. A Higher R charge-transfer value is associated with the resistive behavior of the metal, implying the effectiveness inhibitor against charge transfer processes. In addition to that, it could also be an area effect, i.e. the higher active surface area will provide higher R charge-transfer values. However, the decrease in R charge-transfer values after 1 day in the inhibited condition might have emerged because of the broadening pores on the inhibitor-induced protective layer that possibly decreased the inhibitor coverage over AA6061. The progressive drop of the Q dl (double-layer capacitance) in the inhibited sample could be attributed to the adsorption of 2-MBI and subsequent water displacement from AA6061 [109,110].
The higher R charge-transfer and lower Q dl values reveal the stabilizing effect of 2-MBI on the oxide layer on the AA6061 substrate. This behavior indicates the rapid formation of a protective layer on the substrate, followed by gradual densification of this layer with reduced porosity, overall increasing the oxide resistance while maintaining its thickness, as reflected by the FIB-SEM studies. Visser et al. [54] have reported such an identical stabilizing effect of 2-mercaptobenzothiazole on AA2024 substrate, which includes the coverage of Fe or Cu rich intermetallic particles and subsequent higher R pol values being reported. In comparison to uninhibited samples, R charge-transfer for 2-MBI treated samples increased by a factor of 1.5 times (Table 2). This implies that 2-MBI stabilizes the aluminium oxide up to 1 day, the time period where the highest R charge-transfer values were observed. A gradual reduction in the R charge-transfer can be observed upon exposure up to 14 d. Time-dependent desorption of the inhibitor molecules from the substrate surface, due to the presence of a porous and defective complex inhibitor layer, could be responsible for this phenomenon [9,27]. Shi et al. [105] reported time-dependent delamination of a protective inhibitor layer on AA2024. They observed intensive corrosion of AA2024 substrate due to degeneration of the cerium cinnamate inhibitor layer in saline solution after 13 days.
LPR and PDS results identified the barrier properties of the inhibitor complex layer and its stability for longer immersion times. For the inhibited system, a decrease in R pol values can be attributed to possible porosity within the complex protective layer that allows ingress of the electrolyte and contributes to enhanced i corr values. These findings also corroborate the EIS results as the R pol values calculated from EECs (Table 2) differentiate within a reasonable limit. Polarization resistance values evident for the 1d inhibited sample by LPR measurement was ≈3.1 × 10 6 to 4.2 × 10 6 Ω cm 2 which was calculated 7.2 × 10 6 Ω cm 2 from EEC ( Table 2). R pol values found to be almost identical for 7 days and 14 days inhibited samples by both EIS and LPR techniques. These findings support the argument that with increasing time, the inhibitor-induced layer developed pores and reduced its surface coverage that favors the charge transfer processes, i.e. higher i corr values. A gradual rise in current density from 0.012 to 0.028 mA cm −2 after 14 days is also supported by the explanation of the increase in charge transfer activities in the coating-substrate interface. Additionally, these findings agree with the PDS results as R pol significantly increased for inhibited conditions, compared with uninhibited conditions, that resulted in reduced current density.
The PDS curves showed lower i corr value for the inhibited system in 1 day immersed sample (Fig. 2b). This could be assigned to the emergence of a porous inhibitor film, offering a passable barrier to corrosion after 1 day immersion. Higher i corr values could be attributed to the filling up of porous cathodic sites with corrosion products, thus facilitating re-passivation processes and lowering the current density overall. Aballe et al. [111] have provided similar observations for AA5083 alloy in 3.5% NaCl solution. They reported substantial oxide film growth with immersion time that contributed to the re-passivation process. Rapid film formation in the inhibited system possibly contributed to the low i corr values, initially observed at 1 day. However, the likelihood of a time-dependent degradation of the inhibitorinduced film/layer resulted in lower i corr values at 14 days. The shift of Tafel curves to more negative E corr values in inhibited conditions with time indicates a predominant cathodic character of 2-MBI on AA6061.

Tentative correlation between pH and changes of electrochemical parameters
The steep rise of pH in the uninhibited system and moderate rise in inhibited condition could be attributed to the degree of dissolution of aluminum oxide layer/protective inhibitor layer due to micro galvanic coupling between the aluminum matrix and intermetallic particles [112]. It has been postulated in earlier studies that the cathodic partial reactions facilitate the oxygen reduction and hydrogen evolution reactions on the alloy surface. It could increase the solution pH and promote anodic dissolution of Al and Mg from different IMPs comprised of Cu or Fe. Hydroxyl ion (OH − ) generation enables a high pH environment that favors the dissolution of the aluminum oxide layer, gradually exposing the underneath alloy surface to the corrosive environment [23,24]. In this study, E corr values were found to be more positive for the inhibited conditions than uninhibited conditions. Pyun et al. [113] have suggested more negative E corr values for the uninhibited system than the inhibited system, referring to the loss of passivity of the AA6061 substrate. It could be related to thinning of the surface oxide layer by hydroxide ion (OH − ) attack (alkaline chemical dissolution) or to the absence of the primary oxide film [113]. In the current study, the presence of inhibitor molecules could have provided a barrier effect that delayed the onset of micro galvanic coupling, i.e. lowering the dissolution of the oxide layer and stabilizing it further. It may have delayed the charge transfer reaction at the electrolyte/oxide-inhibitor film interface or the Al 3+ ion transportation through the oxide film [114]. Furthermore, it can be appreciated in terms of LPR measurements, there is a fall in the R pol values in the inhibited system after 7 days, and it remains stable in between 7 and 14 days. This refers to the escalation of the dissolution activity of the system. This could result in unstable pH of the solution after 7 days and steeply displaced to more alkaline values at 14 days.

Coverage of Fe and Si-rich IMPs, protection of the bulk, and tentative mechanism of inhibition
Surface and electrochemical analysis results have postulated that in the inhibited sample, the protective film/layer over Fe and Si-rich IMPs supposedly prevented Al and Mg dealloying from these IMPs (Fig. 6c). It has been postulated that localized corrosion is usually initiated by a dealloying attack on IMPs but stabilizes (continuous corrosion) through nano galvanic interactions between regions rich in nobler metals and the IMPs. This phenomenon gradually promotes localized solution chemistry, diminishing the protective layer covering the nearby alloy matrix, leading to selective dissolution [115]. Adsorption of an organic inhibitor film could limit the activity of cathodically active nobler IMPs and restrain the anodic dissolution of active metals like Al and Mg [8,116]. Kharitonov et al. [49] have investigated inorganic Na 3 VO 4 (sodium orthovanadate) in saline solution on AA6063-T5 for 24 h. They have and postulated corrosion inhibition mechanism by rapid film formation over the local cathodic sites created by Mg-rich intermetallic that suppressed the dissolution of Mg and protected the bulk from pitting corrosion. The inhibition process started with the reduction reaction of NaVO 3 on the AA6063 surface. This reduction reaction helped form protective films of insoluble oxides and hydroxides over cathodic IMPs and slowed down anodic dissolution [117,118]. Similar but limited, studies for AAxxx alloys with organic inhibitors are available [9,27]. Uncorroded Si-rich IMPs in the subsurface region of AA6061 were identified beneath the protective inhibitor layer (Fig. 6b and d). The Fe and Si-containing IMPs concealed by the protective layer exhibit no significant indication of trenching, confirmed by the absence of selective dissolution of Al or Mg. The presence of weak Cl or O signals near the thick inhibitor layer further confirms that bulk Al was unaffected from anodic dissolution and cathodic reduction of O or Cl. The continuity of the inhibitor layer remains unchanged up to 7 days, with the identical chemical composition observed at 1 day. However, the inhibitor layer's continuity was reduced at 14 days, which confirms the time-dependent degradation 1 3 of protectiveness of 2-MBI and supports the findings of electrochemical data.
The thickness of the protective layer over AA6061 is much thicker (~ 3.3 nm from XPS etching) than the monolayer thickness of 2-MBI molecules and the thickness of the naturally occurring oxide layer of aluminum alloys [52,89]. In addition, the layer is comprised of atom species from 2-MBI inhibitor with traces of O. Therefore; this layer could be a complex of physically absorbed 2-MBI molecules or a complex layer formed through the interaction of inhibitor molecules with available surface oxygenated species. Moreover, instead of a mono layer, multiple layers of a complex inhibitor system have formed. The EDS results are consistent with the findings of EIS results regarding the presence of a thick protective/barrier layer that has delayed the ionic diffusion process and protected IMPs from corrosion attack [43]. In the latest study [119], 2-MBI film formed over Cu surface has been investigated by density functional theory, and insitu surface characterization was employed to strengthen the findings of molecular-level modeling. It has been proposed that 2-MBI could interact with oxide-covered Cu surface by S in the form of thione or thiolate, whereas N could interact in the form of pyrrole and pyridine. A multilayer film structure has been proposed where the first layer is chemically absorbed, followed by multiple layers of the Cu-MBI complex. Our results are slightly aligned with these findings as the XPS has revealed oxide and metal peaks of Al in the inhibitor-induced layer. The chemical shifts of the S and N environment from outermost to innermost layer also presumably corroborates the existence of the Al-2MBI complex in the coating-solution interface, which gets thicker and porous with time.
The changes of N 1 s and S 2p XPS spectra for the inhibited AA6061 confirms the chemisorption of 2-MBI molecules in the innermost layer. It could be rational to predict that N and S atoms have participated in the attachment of 2-MBI to the substrate surface. Based on previous articles, the tentative mechanism revealed from the XPS etching results could be expected. It was reported that S could be firmly adsorbed to the substrate surface (S-Al) and masked the bulk from corrosion [43]. It has been reported that 2-MBI in thione form could be adsorbed on Au surface in a solution having pH > 2 with an upward geometry [28]. However, the molecular orientation is beyond the scope of the current study as angle-resolved XPS has not been performed. Moreover, this arrangement is improbable for this study as N atoms (one or both) could be attached with AA6061 substrate. On the contrary, C atoms from the benzene ring were not observed to participate in the molecular attachment of 2-MBI with AA6061. Gas cluster ion beam sputtering associated with XPS measurements indicated two different 2-MBI molecules bonding in the surface layer, i.e. the topmost position contains 2-MBI molecules, i.e. physically absorbed ones. Later, the organometallic complexes have been thought to be formed via S and N interactions with Al.
The chemical interaction of an inhibitor molecule with a heterogeneous alloy surface and its durability in a corrosive electrolyte were the focus of this study, according to the thematic illustration of Fig. 1. Results have suggested that 2-MBI primarily interacted with AA6061 with S and N atoms in two different bonding environments to form a multilayer film, varying structurally from coating-solution interface to metal-coating interface. 2-MBI could simultaneously interact with metal or oxide layer and adsorb over AA6061 to enhance the protectiveness of the alloy surface up to 1 day against ionic diffusion, water adsorption, etc. The existence of this layer has masked the activity of IMPs to form localized corrosion cells and retarded the anodic dissolution of bulk Al. Adsorption of 2-MBI has resulted in higher polarization resistance. The highest contribution from film resistance (R pore ) is observed at 1 day and gradually drops further by supposedly breaking bonds between 2-MBI and the surface.
Consequently, after 7 and 14 days, this inhibitor film/layer became defective and thicker, allowing the transportation of aggressive ions through the porous structure to alloy surface, i.e. higher current density and low polarization resistance. The moderate rise in pH values indicates a possibility of a higher oxygen reduction rate at longer exposure times which may result in the quick breakdown of the oxide layer or any protective layer. However, the exact reasonings of timedependent degradation of the 2-MBI film are worth deeper in-situ experimental investigations.

Conclusions
This study elucidates the role of 2-MBI molecules in forming a protective layer over AA6061, identifying barrier properties of 2-MBI against electrolyte diffusion and the durability of inhibition over an exposure period of 14 days. EIS and LPR results indicated the emergence of a complex protective layer in the presence of the inhibitor, confirmed by the broad phase angle maxima at the middle-frequency range. This protective film/layer was stable up to 1 day, which became defective with a gradual drop in R charge-transfer and R pore values. A gradual reduction in inhibition efficiency from 64.7 to 21.0% after 14 days further confirms the ingress of electrolyte through the complex inhibitor layer. FIB-SEM and high-resolution TEM unveil the formation of a complex and multilayered structure of the protective film that consists of species associated with the inhibitor, i.e. S, N, and C, in addition to surface oxygen. It has covered the nobler IMPs (Fe & Si) and reduced the propensity of anodic dissolution of bulk Al. XPS etching results confirm the changes in bonding states of S to attach with Al and N have also been found in two different chemical environments. XPS results indicate the chemical and subsequent physical adsorption of 2-MBI molecules over AA6061, where the first interaction thought to be occurred by S and N from 2-MBI molecules. The latter could be a complex of Al-2MBI, or only the physically absorbed 2-MBI molecules coexisted with surface oxides. In summary, 2-MBI molecules formed a complex layer of ~ 3 nm over AA6061 substrate with the available surface oxygenated species that successfully protected the bulk from corrosion attack up to 1 d, beyond which this layer becomes more defective and less protective, over time due to diffusion of aggressive ions.