**3. Characterization**

A scanning electron microscopy (JEOL-IT300 microscope equipped with an EDS detector, JEOL Ltd, Tokyo, Japan) was used to analyze the morphology and the microstructural features of MgAl-LDH, while the elemental analysis of the thin film was studied through energy dispersive electron microscopy (SEM-EDX) in planner mode. XRD patterns of the calcined and uncalcined LDH coated samples were recorded by X-ray diffraction (XRD) (X'Pert High Score diffractometer, Rigaku, Tokyo, Japan) at ambient conditions by using cobalt Kα (λ = 1.789 Å) emission source at 10 mA and 30 kV conditions. The step size of 0.005◦ was adjusted in the 2θ range of 5◦–110◦. The peak reflections at the (003) planes of layered double hydroxide were studied to measure the basal spacing and to define the full-width half maximum (FWHM) for the measurement of crystallite size (*D*), by using the Scherrer formula. The lattice parameters of Mg–Al layer double hydroxide were calculated by using Equation (1) [34], where *d* is the lattice spacing calculated by Braggs law.

$$\frac{1}{d^2} = \frac{4}{3} \left( h^2 + hk + \frac{k^2}{a^2} \right) + \frac{l^2}{c^2} \tag{1}$$

Fourier transformed infrared spectra (FTIR), Varian 4100 FTIR Excalibur Series instrument (Varian, Santa Clara, CA, USA), in the attenuated total reflectance (ATR) mode were recorded to analyze surface functional groups and the chemical bonding of the samples, in the range of 550–4000 cm<sup>−</sup><sup>1</sup> with a 4 cm<sup>−</sup><sup>1</sup> resolution and at 32 scans, by using a diamond crystal as Internal Reflective element (IRE). The electrochemical measurements were conducted (PAR Parstat 2273, Ametek, Berwyn, PA, USA) 0.1 M NaCl solution to understand the anti-corrosion properties performed at ambient conditions under Faraday cage to minimize the external noise on the system. A relatively diluted electrolyte (0.1 M) was employed in order to better highlight the differences between the investigated samples. A traditional three electrode setup was used, where the platinum mesh was used as a counter electrode while MgAl–LDH and Ag/AgCl/KCl (+210 mV vs. Standard Hydrogen Electrode (SHE)) were used as working and reference electrode respectively. The MgAl–LDH was exposed to the electrochemical solution for 30 min in 0.1 M NaCl solution before the measurement, for the system stabilization. The polarization curves were obtained with a sweep rate of 2 mV/s. The impedance measurements (EIS) were performed at the open circuit potential (OCP) over frequencies ranging from 100 kHz down to 10 mHz at a 5 mV (rms) amplitude.

#### **4. Results and Discussion**

#### *4.1. XRD Analysis*

Figure 2a,b shows the XRD pattern of MgAl–LDH thin film developed on the AA6082 at various temperature and crystallization time periods. The XRD pattern of the MgAl layer double hydroxide at 40 ◦C–24 h and at 60, 80, 100 ◦C for 12, 18, and 24 h crystallization time, demonstrated the characteristic peaks of layered double hydroxide structure, described in the literature [35], further the sharpness of the peaks suggested an ordered structure of LDH layers. It can be seen that synthesis temperature and crystallization time have an influential effect on characteristic peaks. The (003), (006), (009), (110), and (113) characteristics peaks of crystal planes are related to the MgAl–NO3 LDH film. The intensity and broadness of the reflection peaks vary with the increase of temperature and t also depend upon crystallization aging time. When the samples were synthesized at 60 ◦C and lower aging time (12 and 18 h), the pattern exhibited low intensity and a broader peak which describe their low crystallinity. At higher temperature range, for instance, 80 and 100 ◦C, the reflection peaks exhibited sharp and high intense narrow peaks which describe well the crystalline and ordered structure. The intense reflection peaks of (003) at low 2θ value exhibited an interlayer distance of ≈0.80 nm and the reflection peak could further be used to calculate the cell parameter "*c*" by the correlation "*c* = 3*d*003", while the *d*110 interlayer thickness was used to calculate the cell parameter "*a*" by the correlation "*a* = 2*d*110". The basal spacing of MgAl LDH slightly shifted to lower angle with the effect of enhanced temperature and crystallization aging time, indicating the strong intercalation of NO3 − ions. However due to the formation of carbonate anions, small absorption peaks of *d*003 at 40 ◦C–24h, 60 ◦C–18 h were also observed. Fourier transform-infrared spectroscopy (FT-IR) spectra further confirmed the presence of CO3 2− nions. The interlayer thickness, lattice constants of "*a*" and "*c*", and crystallite size for Mg–Al LDHs thin film on AA6082 are listed in Table 1.

**Figure 2.** The XRD spectra of Mg-Al layered double hydroxide (LDH) film samples developed on aluminum alloy AA6082 obtained at various reaction temperature and crystallization times.

#### *4.2. Fourier Transform Infrared Spectroscopy (FTIR)*

The selective samples, synthesized at various temperatures and crystallization times, were further investigated by FTIR analysis. FTIR spectra in attenuated total reflection mode were recorded, as shown in Figure 3. All the samples showed almost similar types of features. The broadbands displayed in the range of 3370–3427 cm<sup>−</sup><sup>1</sup> were assigned to OH group stretching and the absorption band around, 1627–1633 cm-1 was caused due to the flexural oscillation peaks of interlayer water molecules [36]. Moreover, the absorption peaks around 1350 cm<sup>−</sup><sup>1</sup> were assigned to the asymmetric stretching bond of intercalated NO3 − [37]. The small peak around 1520 cm<sup>−</sup><sup>1</sup> corresponded to the CO3 2− ions, which shows the presence of a small number of carbonate ions in the LDH phase. The bond at 655, 751, and

1202 cm<sup>−</sup><sup>1</sup> may be associated with Al–OH stretching [38]. The absorption peaks around 550–770 cm<sup>−</sup><sup>1</sup> correspond to the lattice vibration of metal–oxygen bonds (M–O) [39].


**Table 1.** Cell parameters and sizes of the coherent domains determined for the Mg−Al layered double hydroxide (LDH) precursor powders from X-ray diffraction.

**Figure 3.** ATR-FTIR spectra of Mg–Al LDH powder, scraped from as-prepared MgAl–LDH coated samples fabricated at different reaction temperatures.

#### *4.3. Scanning Electron Microscopy (SEM)*

As revealed from the SEM observations, shown in Figure 4, a compact and uniform interviewed LDH structure was obtained by the increase of reaction temperature and of aging time, moreover distinct surface morphological variations were also observed. Initially, the LDH granules started to originate and developed into distinct platelet structure with increase of reaction temperature and crystallization time, while on further increase of the temperature and aging time, the nano-sheets of the LDH structure fused to form a compact blade like LDH structure. For example at 80 ◦C temperature and 24 h aging time, a fully groomed curved shaped platelet morphology was obtained which fused on further increase in temperature and appeared as a compact needle-shaped structure. The atomic composition of LDH, calculated by energy disperse spectroscopy (EDS) plane scanning, is listed in Table 2. The EDS findings showed that the coated structure is mainly composed of Mg, Al, N, and oxygen. A small amount of carbon is also evident in the EDS study, caused by contamination from

air, which results in the formation of carbonate anions. The atomic ratio of Mg/Al varies with the effect of temperature and crystallization time. Table 2 showed that with a higher reaction temperature and crystallization time, a higher ratio of Mg/Al is obtained. The oxygen content also varied with the influence of temperature and time. The atomic ratio of Mg:Al lies in the range of 2.5:1–3.87:1, which provides a rough approximation of the MgAl LDH assembly. Note that the Mg:Al ratio increases with the duration of the treatment regardless of the temperature. The duration of the treatment seems therefore to affect the chemical composition of the LDHs which enrich with Mg during the long immersion time. The possible formation of MgAl LDH on the AA6082 surface may start with the dissolution of aluminum in the basic solution to release Al3+ ions (aluminum surface is partially dissolved on contact with the high pH solution and generated aluminum oxides) [40], which react with the water to form Al(OH)3 while the final step is related to the precipitation of Mg2+ and OH− on the surface of the Al(OH)3 surface to form the pre-MgAl LDH hydroxide mixture. The ammonium nitrate continuously hydrolyzed to form NO3− in the system, along with the release of ammonium ions which led to progressively keep the pH in the range of 10. Finally, the divalent Mg2+ ions in Mg(OH)2 were substituted by the trivalent Al3+ ions, which result in the coexistence of Al(OH)3 and Mg(OH)2 to form a stable hydrotalcite-like LDH structure. On the other hand, the hydroxyl ions present inside the galleries were exchanged by NO3− ions present in the solution and as the average atomic ratio of Mg to Al is approximately around three, as shown in Table 2 (EDS analysis), it can be concluded that the final film of Mg3Al(OH)2·*<sup>x</sup>*NO3·*y*H2O was formed on the substrate of AA6082 and formed stacking of LDH layers one above another to form the LBL configuration (Figure 1). The obtained EDS findings are in agreemen<sup>t</sup> with the XRD results.

**Figure 4.** SEM images of LDH films developed at various reaction temperatures and crystallization times.


**Table 2.** EDS study of atomic percentage at various reaction temperature and crystallization times.

The results from SEM (Figure 4) sugges<sup>t</sup> that the synthesis conditions promote the formation of uniform and quite ordered structures. As far as the appearance of the coatings is concerned, it seems that on increasing the treatment temperature from 60 to 100 ◦C, the LDHs layer becomes more and more compact and homogenous. Also the duration of the treatment plays a similar role: prolonged immersion in the solution promotes the formation of homogeneous LDHs structures in which the platelets are closely packed.

The effect on the film thickness of the synthesis parameters is reported in Figure 5, which shows also the cross-sectional image of MgAl LDH at 80 ◦C and 18 h (reported as an example). The results of the film thickness indicated that with the increase of reaction temperature and treatment time, the film thickness of coating increased. The film thickness increased from about 20.8–73.5 μm with the increase of the processing parameters. The high temperature and aging time in this study were shown to promote the growth rate of LDH formation, confirmed also by XRD and SEM analysis. It was observed that a rapid increase in film thickness was found for 100 ◦C temperature and 24 h treatment time. However, with the increase of thickness, the interface of substrate and coating become blurred and also caused an increase in defect density, which promoted loose interaction with the substrate. In fact, some pores were observed at the interface of coating and substrate with the increase of coating thickness. This fact is expected to negatively influence the corrosion protection ability of LDH.

**Figure 5.** MgAl LDH thickness of the film coated AA6082 estimated from the cross-sectional optical microscopic images as a function of reaction temperature and treatment time, (for representation, insight is the optical images of LDH at 80 ◦C and 18 h reaction conditions.).

#### *4.4. Electrochemical Study*

The as-prepared MgAl–LDH anticorrosion behavior was investigated through electrochemical studies. Figure 6 exhibits the potentiodynamic polarization curves of all the tested samples, while the corrosion current density and corrosion potential are listed in Table 3. With the increase of synthetic reaction temperature and crystallization time, the corrosion current density decreases, and also a significant increase in the film is observed. The reduction of both the anodic and cathodic currents suggests an increase in corrosion resistance. The polarization curves of MgAl LDH coating obtained from the specimens developed at 60 ◦C–24 h, 80 ◦C–18 h, 80 ◦C–24 h, 100 ◦C–18 h and 100 ◦C–24 h showed a noticeable decrease in corrosion of both anodic and cathodic current density compared to the bare AA6082. The significant reduction of the current densities suggests that the MgAl LDH thin films can help to decrease the corrosion rate of the substrate. All the developed films on AA6082 showed lower corrosion current density along with a shift of the corrosion potential to higher values compared to bare AA6082. As one can see, for almost all the investigated samples a rise in the corrosion potential was observed as the crystallization time increased. The MgAl LDH is believed to provide corrosion protection due to the following two mechanisms: (1) the barrier effect, as they are dielectric materials which protect the metal surface by avoiding interaction with the metal substrate; (2) by entrapping Cl− ions and releasing nitrates [41]. In the case of the polarization curves, it is likely that the main protection mechanism observed is the physical barrier effect provided by the LDH layer which promotes a decrease in the flow of current.

**Figure 6.** Polarization curves of bare AA6082 and the coated AA6082 in 0.1 M NaCl aqueous solution.


In order to further understand the corrosion resistance ability of MgAl LDH, EIS analysis was performed. Figures 7 and 8 show the impedance modulus and phase plots, respectively. At low frequency (about 0.01 Hz), higher impedance modulus values (|*Z*|0.01) are a rough estimation of the corrosion resistance properties [42]: It can be seen that the samples 100 ◦C–24 h and 100 ◦C–18 h exhibit the highest value of |*Z*|0.01 among the investigated samples. Furthermore, it is clear that |Z| values follow a general tendency of corrosion resistance, higher temperature, and crystallization time and exhibit greater propensity of corrosion resistance, according to the higher thickness of the LDH layers. These results are consistent with the results obtained from the potentiodynamic curves. The specimens fabricated at 100 ◦C–24 h showed comparatively a lower corrosion resistance than 100 ◦C–18 h, which may be due to their greater film thickness which causes more defects in the coating itself and/or pores at the interface with the substrate. The impedance results sugges<sup>t</sup> that the high temperature and aging time lead to an increase in corrosion resistance, which is probably due to increased crystallization of the layered double hydroxide and to a thickening of the layer as well. When the temperature conditions and aging time are moderate, the enhancement in terms of corrosion resistance is less pronounced. In addition, the |*Z*| values of the MgAl LDH film developed at different reaction conditions follow a general tendency: the higher the hydrothermal reaction temperature, the higher is the corresponding |*Z*| value obtained. The thickness of the film also plays a vital role in corrosion protection, and |*Z*| values vary with the increment in film thickness. The sample (100 ◦C–18 h) showed around 33 μm film thickness and also the highest corrosion resistance among all the processed samples.

**Figure 7.** EIS spectra (Bode plots of log(|*Z*|) vs. log(frequency) ) of bare AA6082 alloy and AA6082 alloy coated with LDH film at various reaction temperatures and crystallization times in 0.1 M NaCl solution.

**Figure 8.** EIS spectra (Phase angle vs. log(frequency)) of bare AA6082 alloy and AA6082 alloy coated with LDH film at various reaction temperatures and crystallization times in 0.1 M NaCl solution.

Figure 9 shows the evolution with an immersion time of the impedance modulus of the most representative samples among those investigated (data collected after 1, 3 and 7 days of immersion are reported). All the samples show a quite relevant decay of the protection properties during the 7 days of continuous immersion in the electrolyte. Regardless of the synthesis conditions, after one week of immersion, the low-frequency impedance is in the 105–106 Ω cm<sup>2</sup> range for all the investigated samples. This value is in any case remarkably higher than the | *Z*|0.01 value of the bare substrate at the beginning of the immersion in the electrolyte (| *Z*|0.01 ≈ 10<sup>4</sup> Ω cm2). The decrease in impedance observed for the investigated coatings is likely to rely on the presence of porosity and defect in the coating and at the metal/LDH layer interface. According to optical microscope observations of the LDH layer and LDH/metal interface, thicker coatings (i.e., with synthesis conditions which promote higher LDH growth rate) are more defective and porous. This would explain the evolution of the impedance spectra with time: at the beginning, the LDH layers act as a barrier against electrolyte permeation; as time elapses, the solution moves through the defects and pores thus reaching the metal/coating interface. The latter process promotes a decrease in impedance over all the frequency range since coating resistance is reduced and the Faradic process is promoted.

**Figure 9.** Bode plots of AA6082 samples, coated with MgAl–NO3 LDH thin film after immersion in 0.1 M NaCl: (**a**) 60 ◦C–24 h and 80 ◦C–18 h sample from 1 to 7 days immersion; (**b**) 80 ◦C–24 h and 100 ◦C–18 h 1 to 7 days immersion time.

The EIS spectra reported in Figure 9 were fitted in order to ge<sup>t</sup> some insight into the effect of the different parameters on the corrosion protection properties of the investigated coatings. According to Figure 8, all the samples show two relaxation processes, which are located in the middle–high or middle–low frequency range. Notice that the thickness, as well as the defectiveness, of the coatings strongly affect the electrochemical response of the diverse samples. For this reason, it is not surprising to observe dispersion of the relaxation processes in the investigated frequency range. According to the literature [43,44], the EIS response of the LDH covered samples can be analyzed employing a *R*s(CPELDH(*R*LDH(CPEdl *R*ct))) electrical equivalent circuit. In this circuit, *R*s stands for the resistance of the electrolyte. The relaxation process at the higher frequencies is fitted employing a resistance, *R*LDH, which indicates the pore resistance of the LDH layer and a constant phase element, CPELDH, which represents the dielectric properties of the layered double hydroxide coatings. The relaxation process at the lower frequencies is fitted employing a resistance, *R*ct, which is related to the superimposition of the contribution of the charge-transfer process and of the aluminum oxide and a constant phase element, CPEdl, which represents the double layer capacitance contribution, overlapped to that of the dielectric properties of the aluminum oxide. According to the mathematical representation of a CPE, (i.e. *Z*CPE = 1/( *Q*(ω*j*) α) the parameters *Q* and α were employed to describe the dielectric response of the electrodes. Table 4 shows the fitting results for the investigated samples. Notice that the parameters

αLDH and αdl are almost always far from unity. For this reason, it is not possible to attribute any precise physical meaning to the pre-exponential factors *Q*LDH and *Q*dl. As far as the *R*LDH and *R*ct parameters are concerned, one can observe a certain scattering during immersion time for the samples 60 ◦C–24 h and 80 ◦C–18 h, probably due to the porosity of the coatings and to the consequent localization of the corrosion attack promoted by chlorides. On the other hand, the samples 80 ◦C–24 h and 100 ◦C–18 h show a smoother decrease in the corrosion protection properties (described by *R*LDH and *R*ct) which indicates that the coatings are more compact (as suggested by the relatively high values of *R*LDH) and protective (as suggested by the relatively high values of *R*ct).


**Table 4.** Evolution with time of the fitting parameters *R*LDH, *Q*LDH, αLDH, *R*ct, *Q*dl, and αdl.

To better understand as to what extent the investigated LDH layers provide corrosion protection, the numerical values of *R*LDH and *R*ct obtained by fitting the experimental curves were compared with data from the literature. In Table 5, a comparison of the fitting parameters *R*LDH and *R*ct after about 1 day (or less) of immersion in a sodium chloride electrolyte is reported. The value of *R*LDH for the coatings developed in this study is remarkably higher compared to the data reported in the literature. However, one should consider that: (1) in this study the crystallization treatment was prolonged in order to obtain relatively thick coatings, while in the literature very often only a thin conversion layer of LDHs was investigated; (2) the electrolyte employed in this study is more dilute than 3.5 wt % NaCl (0.1 M ≈ 0.58 wt %): for this reason, higher resistance values are expected. Also the parameter *R*ct for the samples investigated in this study is one of the highest compared to other works reported in the literature (except the LDH reported in [43], which contains vanadates based on corrosion inhibitors). However, also in this case it has to be considered that the electrolyte employed is more dilute compared to the NaCl concentration employed in the studies reported in [44–46].

**Table 5.** Comparison with literature data referring to LDH conversion layers/coatings on aluminum alloys (n.p.: not provided).


The EIS results seem also to be in accordance with the visual observation of the immersed samples as shown in Figure 10: optical microscope photos were taken after the 7 days of immersion in 0.1 M NaCl solution. The bare aluminum sample was badly corroded after the immersion and was covered with a thick layer of corrosion products. Notice that cracks and blister are observed on the LDH layers, in accordance with the remarkable decrease in *R*LDH and *R*ct.

**Figure 10.** The specimens after 7 days of immersion in a solution of 0.1 M NaCl: (**a**) bare aluminum surface; (**b**) coated sample at 60 ◦C–24 h; (**c**) 80 ◦C–18 h; (**d**) 80 ◦C–24 h; and (**e**) 100 ◦C–18 h.

The surface morphologies of the MgAl–LDH after 7 days immersion in 0.1 M NaCl solution are shown in Figure 11. It can be seen that no serious collapse of platelet structure is observed after 7 days immersion and most of the structure remained almost intact and was shown to be similar to the as-prepared original structure (Figure 11a,b). However, due to the longtime contact, dissolution of some platelets of MgAl–LDH structure was observed at some points Strong Cl− signals in EDS analysis (inset of Figure 11b) were observed after contact with chloride solution, so we can say that the MgAl–LDH film exhibited anion exchange capability by absorbing Cl− while the XRD analysis also showed that the interlayer of the MgAl–LDH was able to retain Cl− inside the structure. The LDH film anion-exchange behavior on the aluminum alloy in the chloride solution can be generally expressed as follows [27]:

$$\text{LDH-NO}\_3^- + 2\text{Cl}^- \rightarrow \text{LDH-2Cl}^- + \text{NO}\_3^- \tag{2}$$

**Figure 11.** SEM images of (**a**) original MgAl LDH coating, 60 ◦C–24 h sample and (**b**) an immersed sample soaked in 0.1 M NaCl solution for 7 days (Insets are the corresponding EDS spectra).
