Photocatalytic Degradation of 2,4,6-Trichlorophenol by MgO–MgFe 2 O 4 Derived from Layered Double Hydroxide Structures

: In recent years, the search for solutions for the treatment of water pollution by toxic compounds such as phenols and chlorophenols has been increasing. Phenols and their derivatives are widely used in the manufacture of pesticides, insecticides, paper, and wood preservers, among other things. Chlorophenols are partially biodegradable but not directly photodegradable by sunlight and are extremely toxic—especially 2,4,6-trichlorophenol, which is considered to be potentially carcinogenic. As a viable proposal to be applied in the treatment of water contaminated with 2,4,6-trichlorophenol, this paper presents an application study of the thermally activated Mg / Fe layered double hydroxides as photocatalysts for the mineralization of this contaminant. Activated Mg / Fe layered double hydroxides were characterized by X-ray di ﬀ raction, thermal analysis, N 2 physisorption, and scanning electron microscopy with X-ray dispersive energy. The results of the photocatalytic degradation of 2,4,6-trichlorophenol in aqueous solution showed good photocatalytic activity, with an e ﬃ ciency of degradation of up to 93% and mineralization of 82%; degradation values which are higher than that of TiO 2 -P25, which only reached 18% degradation. The degradation capacity is attributed to the structure of the MgO–MgFe 2 O 4 oxides derived from double laminate hydroxide Mg / Fe. A path of degradation based on a mechanism of superoxide and hollow radicals is proposed.


Introduction
Layered double hydroxides (LDH) or hydrotalcite-type compounds are a large class of natural and synthetic compounds of the anionic clay type [1,2]. These compounds are characterized by having a laminar structure with octahedral arrays of double metal hydroxides that generate a positive residual charge, which is neutralized by the presence of hydrated interlaminar anions [3][4][5]. Its structural formula is represented in a general way as [M(II) 1

X-Ray Diffraction (XRD)
The X-ray diffraction patterns of the LDH are shown in Figure 1a. The three patterns are similar in relation to the position of the signals, but it is observed that crystallinity increases when the Mg/Fe ratio increases, with a tendency of LDHM1F < LDHM2F < LDHM3F, which is associated with a greater crystallinity produced by the decrease of Fe 3+ within the brucite type network [Mg (OH) 2 ]. The characteristic signals are in the 2θ angles of 11.2 (003), 23.0 (006), 34.0 (012), 38.0 (015), 45 (018), 59.5 (110), and 61 (013), corresponding to the pyroaurite phase with the PDF card 25-0521 [2,37]. In Figure 1b, the X-ray diffraction pattern of the layered double hydroxides, calcined at 400 °C, is shown. The presence of the crystalline phase of periclase (MgO) can be observed by characteristic signals in the 2θ angles of 36.80 (111), 42.85 (200), and 62.23 (220) (JCPDS-4-0829), showing a tendency to increase the crystallinity with respect to the Mg/Fe ratio. In the case of the solid LDHM1F, it is observed that at 400 °C the periclase phase has been formed but with a lower crystallinity, which is attributed to the fact that at these temperatures phase changes have occurred, although a higher temperature is required to favor crystallization. For the LDHM2F and LDHM3F solids, a better definition of the peaks is observed, which is associated with a better crystallinity, attributed to the fact that-having a lower amount of Fe-the MgO is more rapidly segregated. The above is associated with the thermal profile described in the following section, in which, in addition to the crystalline phases of MgO, the spinel phase (MgFe2O4) is segregated, which at 400 °C is amorphous. It is not identifiable by XRD. Figure 2 shows the differential thermal and thermogravimetric analysis of laminar double hydroxides. In the curve of the DTA (Figure 2a), in all cases an endothermic reaction is observed centered at 145 °C and associated with the elimination of interlaminar water molecules, followed by endothermic reactions centered at 290 °C and 350 °C, due to the dehydroxylation of the sheets and decomposition of the interlaminar carbonate. It can be observed that in the case of solid LDHM1F, the evolution to periclase (MgO) and to amorphous spinel (MgFe2O4) occurs at 330 °C. In the case of the solid LDHM2F and LDHM3F, the same profile of thermal decomposition is observed; however, it has a stability up to 350 °C, which is attributed to the greater crystallinity that they present as this favors the activation of the catalyst. The reactions associated with the thermal decomposition of LDH are shown in Equations (1)- (3). Thermal reactions of the LDH can be represented as: In Figure 1b, the X-ray diffraction pattern of the layered double hydroxides, calcined at 400 • C, is shown. The presence of the crystalline phase of periclase (MgO) can be observed by characteristic signals in the 2θ angles of 36.80 (111), 42.85 (200), and 62.23 (220) (JCPDS-4-0829), showing a tendency to increase the crystallinity with respect to the Mg/Fe ratio. In the case of the solid LDHM1F, it is observed that at 400 • C the periclase phase has been formed but with a lower crystallinity, which is attributed to the fact that at these temperatures phase changes have occurred, although a higher temperature is required to favor crystallization. For the LDHM2F and LDHM3F solids, a better definition of the peaks is observed, which is associated with a better crystallinity, attributed to the fact that-having a lower amount of Fe-the MgO is more rapidly segregated. The above is associated with the thermal profile described in the following section, in which, in addition to the crystalline phases of MgO, the spinel phase (MgFe 2 O 4 ) is segregated, which at 400 • C is amorphous. It is not identifiable by XRD. Figure 2 shows the differential thermal and thermogravimetric analysis of laminar double hydroxides. In the curve of the DTA (Figure 2a), in all cases an endothermic reaction is observed centered at 145 • C and associated with the elimination of interlaminar water molecules, followed by endothermic reactions centered at 290 • C and 350 • C, due to the dehydroxylation of the sheets and decomposition of the interlaminar carbonate. It can be observed that in the case of solid LDHM1F, the evolution to periclase (MgO) and to amorphous spinel (MgFe 2 O 4 ) occurs at 330 • C. In the case of the solid LDHM2F and LDHM3F, the same profile of thermal decomposition is observed; however, it has a stability up to 350 • C, which is attributed to the greater crystallinity that they present as this favors the activation of the catalyst. The reactions associated with the thermal decomposition of LDH are shown in Equations (1)- (3). Thermal reactions of the LDH can be represented as: Figure 2b shows the weight loss profiles associated with the thermal decomposition of LDH, which are similar for all solids. In the first thermal decomposition reaction the solid LDHM1F reaches a weight loss of 21%, the solid LDHM2F a loss of 12.3%, and the solid LDHM3F a loss of 14.6%, which can be attributed to the desorption of water adsorbed on the porous surface of the solid and the water Catalysts 2019, 9, 454 4 of 20 occluded in the interlaminar space. The second weight loss is attributed to the partial dehydroxylation of the lamellar structure and the elimination of interlaminar carbonate ions; 16.86% for LDHM1F, 17.7% for LDHM2F, and 19.4% for LDHM3F. Finally, the final weight loss occurs when the solid is dehydroxylated completely, resulting in the collapse of the laminar structure with the subsequent segregation of the oxide phases, with losses of 7.72% for LDHM1F, 6.86% for LDHM2F, and of 9.69% for LDHM3F. The cumulative loss of transition from LDH precursors to the MgO and MgFe 2 O 4 oxides was 45.58%, 36.86%, and 43.69% for LDHM1F, LDHM2F, and LDHM3F, respectively.  Figure 2b shows the weight loss profiles associated with the thermal decomposition of LDH, which are similar for all solids. In the first thermal decomposition reaction the solid LDHM1F reaches a weight loss of 21%, the solid LDHM2F a loss of 12.3%, and the solid LDHM3F a loss of 14.6%, which can be attributed to the desorption of water adsorbed on the porous surface of the solid and the water occluded in the interlaminar space. The second weight loss is attributed to the partial dehydroxylation of the lamellar structure and the elimination of interlaminar carbonate ions; 16.86% for LDHM1F, 17.7% for LDHM2F, and 19.4% for LDHM3F. Finally, the final weight loss occurs when the solid is dehydroxylated completely, resulting in the collapse of the laminar structure with the subsequent segregation of the oxide phases, with losses of 7.72% for LDHM1F, 6.86% for LDHM2F, and of 9.69% for LDHM3F. The cumulative loss of transition from LDH precursors to the MgO and MgFe2O4 oxides was 45.58%, 36.86%, and 43.69% for LDHM1F, LDHM2F, and LDHM3F, respectively.

Fourier Transformed Infrared Spectrocopy (FTIR)
The FTIR spectra of the LDH calcined at 400 °C are shown in Figure 3. The signals are similar for all solids. They present a band centered on 3550 cm −1 that corresponds to the hydrogen bridge vibrations of the OH-OH2 and H2O-OH2 types of the hydroxyl and water molecules remaining. A signal at 1640 cm −1 corresponds to the H-OH vibration of the water. The band at 1360 cm −1 is attributed to the carbonate ions remaining in the structure. The bands in the range of 750 to 500 cm −1 are attributed to the metal-oxygen-metal stretch; specifically, the vibration frequency of 590 cm −1 is attributed to the Fe-OH bond, the band at 630 cm −1 corresponds to the vibration of O-Fe-O, and the band at 648 cm −1 to the Mg-OH vibration.

Fourier Transformed Infrared Spectrocopy (FTIR)
The FTIR spectra of the LDH calcined at 400 • C are shown in Figure 3. The signals are similar for all solids. They present a band centered on 3550 cm −1 that corresponds to the hydrogen bridge vibrations of the OH-OH 2 and H 2 O-OH 2 types of the hydroxyl and water molecules remaining. A signal at 1640 cm −1 corresponds to the H-OH vibration of the water. The band at 1360 cm −1 is attributed to the carbonate ions remaining in the structure. The bands in the range of 750 to 500 cm −1 are attributed to the metal-oxygen-metal stretch; specifically, the vibration frequency of 590 cm −1 is attributed to the Fe-OH bond, the band at 630 cm −1 corresponds to the vibration of O-Fe-O, and the band at 648 cm −1 to the Mg-OH vibration.  Figure 2b shows the weight loss profiles associated with the thermal decomposition of LDH, which are similar for all solids. In the first thermal decomposition reaction the solid LDHM1F reaches a weight loss of 21%, the solid LDHM2F a loss of 12.3%, and the solid LDHM3F a loss of 14.6%, which can be attributed to the desorption of water adsorbed on the porous surface of the solid and the water occluded in the interlaminar space. The second weight loss is attributed to the partial dehydroxylation of the lamellar structure and the elimination of interlaminar carbonate ions; 16.86% for LDHM1F, 17.7% for LDHM2F, and 19.4% for LDHM3F. Finally, the final weight loss occurs when the solid is dehydroxylated completely, resulting in the collapse of the laminar structure with the subsequent segregation of the oxide phases, with losses of 7.72% for LDHM1F, 6.86% for LDHM2F, and of 9.69% for LDHM3F. The cumulative loss of transition from LDH precursors to the MgO and MgFe2O4 oxides was 45.58%, 36.86%, and 43.69% for LDHM1F, LDHM2F, and LDHM3F, respectively.

Fourier Transformed Infrared Spectrocopy (FTIR)
The FTIR spectra of the LDH calcined at 400 °C are shown in Figure 3. The signals are similar for all solids. They present a band centered on 3550 cm −1 that corresponds to the hydrogen bridge vibrations of the OH-OH2 and H2O-OH2 types of the hydroxyl and water molecules remaining. A signal at 1640 cm −1 corresponds to the H-OH vibration of the water. The band at 1360 cm −1 is attributed to the carbonate ions remaining in the structure. The bands in the range of 750 to 500 cm −1 are attributed to the metal-oxygen-metal stretch; specifically, the vibration frequency of 590 cm −1 is attributed to the Fe-OH bond, the band at 630 cm −1 corresponds to the vibration of O-Fe-O, and the band at 648 cm −1 to the Mg-OH vibration. .

Textural Analysis
The N 2 adsorption-desorption isotherms of LDH calcined at 400 • C are shown in Figure 4, showing that for all cases, type IV isotherms corresponding to mesoporous materials are presented according to the IUPAC classification. The isotherms at high values of relative pressure (P/Po) did not show a horizontal tendency, which indicates that the nitrogen physisorption took place between the aggregates of particles that have a laminar morphology. Complementarily, the hysteresis cycles of the type H3 can be observed, which indicate the presence of pores of asymmetric size and asymmetrical shape.

Textural Analysis
The N2 adsorption-desorption isotherms of LDH calcined at 400 °C are shown in Figure 4, showing that for all cases, type IV isotherms corresponding to mesoporous materials are presented according to the IUPAC classification. The isotherms at high values of relative pressure (P/Po) did not show a horizontal tendency, which indicates that the nitrogen physisorption took place between the aggregates of particles that have a laminar morphology. Complementarily, the hysteresis cycles of the type H3 can be observed, which indicate the presence of pores of asymmetric size and asymmetrical shape.
.  Table 1 shows the values of the specific areas determined by the Brunauer-Emmett-Teller (BET) method for the physisorption isotherms of N2 of activated Mg/Fe layered double hydroxides, as well as the average pore diameter calculated by the Barrett, Joyner, and Halenda (BJH) method and the volume of the pores. It is observed that when the Mg/Fe ratio increases, there is a tendency to decrease the surface area, which is associated with the increase in the crystallinity of the solids and with the respective decrease in the pore size of the solids. The increase of area in the solids is because when the materials are calcined, the double structures collapse, and the pores of the tubular material expand (shape of the isotherm). The LDH with the highest specific area is the HTM1F-400 °C catalyst, which reaches specific areas close to 300 m 2 /g, which will favor the contact area of the photocatalyst with the pollutant.  Figure 5 shows the scanning microphotographs of activated layered double hydroxides. In the case of the solids LDHM2F-400 °C and LDHM3F-400 °C, crystals of heterogeneous size with numerous edges can be observed, in which the structure of stacked sheets can be seen, with crystallinity and very similar particle size, which will favor catalytic capacity for both solids. For the  Table 1 shows the values of the specific areas determined by the Brunauer-Emmett-Teller (BET) method for the physisorption isotherms of N 2 of activated Mg/Fe layered double hydroxides, as well as the average pore diameter calculated by the Barrett, Joyner, and Halenda (BJH) method and the volume of the pores. It is observed that when the Mg/Fe ratio increases, there is a tendency to decrease the surface area, which is associated with the increase in the crystallinity of the solids and with the respective decrease in the pore size of the solids. The increase of area in the solids is because when the materials are calcined, the double structures collapse, and the pores of the tubular material expand (shape of the isotherm). The LDH with the highest specific area is the HTM1F-400 • C catalyst, which reaches specific areas close to 300 m 2 /g, which will favor the contact area of the photocatalyst with the pollutant.  Figure 5 shows the scanning microphotographs of activated layered double hydroxides. In the case of the solids LDHM2F-400 • C and LDHM3F-400 • C, crystals of heterogeneous size with numerous edges can be observed, in which the structure of stacked sheets can be seen, with crystallinity and very similar particle size, which will favor catalytic capacity for both solids. For the solid LDHM1F-400 • C, The elemental composition of the surface of the activated LDH particles is shown in Figure 6, which contains the X-ray scattering energy spectra. As can be seen, the three solids have the same elements: Mg, Fe, and O, corresponding to the MgO and the spinel MgFe2O4, but with different elemental molar ratios. Only in the case of solid LDHM1F-400 °C is a small amount of Na present, which was trapped in the LDH network at the time of synthesis. Regarding the metal molar ratio of Mg/Fe on the surface, this was 1, 1.97, and 2.1 for LDHM1F-400 °C, LDHM2 F-400 °C, and LDHM3F-400 °C, respectively, which for the first two solids corresponds to the theoretical molar ratio, while for the third solid a significant decrease of the same is observed. The elemental composition of the surface of the activated LDH particles is shown in Figure 6, which contains the X-ray scattering energy spectra. As can be seen, the three solids have the same elements: Mg, Fe, and O, corresponding to the MgO and the spinel MgFe 2 O 4 , but with different elemental molar ratios. Only in the case of solid LDHM1F-400 • C is a small amount of Na present, which was trapped in the LDH network at the time of synthesis. Regarding the metal molar ratio of Mg/Fe on the surface, this was 1, 1.97, and 2.1 for LDHM1F-400 • C, LDHM2 F-400 • C, and LDHM3F-400 • C, respectively, which for the first two solids corresponds to the theoretical molar ratio, while for the third solid a significant decrease of the same is observed.
which contains the X-ray scattering energy spectra. As can be seen, the three solids have the same elements: Mg, Fe, and O, corresponding to the MgO and the spinel MgFe2O4, but with different elemental molar ratios. Only in the case of solid LDHM1F-400 °C is a small amount of Na present, which was trapped in the LDH network at the time of synthesis. Regarding the metal molar ratio of Mg/Fe on the surface, this was 1, 1.97, and 2.1 for LDHM1F-400 °C, LDHM2 F-400 °C, and LDHM3F-400 °C, respectively, which for the first two solids corresponds to the theoretical molar ratio, while for the third solid a significant decrease of the same is observed.

Diffuse Reflectance Spectroscopy (DRS)
The evaluation of the band gap energy (Eg) for activated LDH was calculated using the Kubelka-Munk equation [F(R) = (1−R) 2 /2R], where R is the converted reflectance (%) of the UV adsorption spectra, and these are reported in Figure 7. It can be observed that the values increase from 2.28 eV to 2.46 eV as a function of the Mg/Fe ratio, associated with the Fe 3+ content. These results show that the content of Fe 3+ in activated LDH materials modifies the semiconductor properties of solids due to a decrease in bandgap values by increasing the amount of Fe 3+ , reaching values lower than 3.20 eV, corresponding to TiO2-P25.

Diffuse Reflectance Spectroscopy (DRS)
The evaluation of the band gap energy (Eg) for activated LDH was calculated using the Kubelka-Munk equation [F(R) = (1−R) 2 /2R], where R is the converted reflectance (%) of the UV adsorption spectra, and these are reported in Figure 7. It can be observed that the values increase from 2.28 eV to 2.46 eV as a function of the Mg/Fe ratio, associated with the Fe 3+ content. These results show that the content of Fe 3+ in activated LDH materials modifies the semiconductor properties of solids due to a decrease in bandgap values by increasing the amount of Fe 3+ , reaching values lower than 3.20 eV, corresponding to TiO 2 -P25.

Diffuse Reflectance Spectroscopy (DRS)
The evaluation of the band gap energy (Eg) for activated LDH was calculated using the Kubelka-Munk equation [F(R) = (1−R) 2 /2R], where R is the converted reflectance (%) of the UV adsorption spectra, and these are reported in Figure 7. It can be observed that the values increase from 2.28 eV to 2.46 eV as a function of the Mg/Fe ratio, associated with the Fe 3+ content. These results show that the content of Fe 3+ in activated LDH materials modifies the semiconductor properties of solids due to a decrease in bandgap values by increasing the amount of Fe 3+ , reaching values lower than 3.20 eV, corresponding to TiO2-P25.    Figure 8 shows the ultraviolet-visible spectra of the degradation of a solution with a concentration of 80 parts per million (ppm), equivalent to 80 mg/L, of 2,4,6-trichlorophenol as a function of time, using activated LDH catalysts and TiO 2 at 400 • C as a reference control. The TiO 2 -P25 catalyst is used as a reference, since at the level of research and industrial application, it is used for the degradation of water polluting compounds due to its excellent stability, non-toxicity, being a semiconductor material with high photo-oxidation power, and low cost [19,36,38]. The 2,4,6-trichlorophenol spectra show three characteristic absorption bands, with the primary transition π→π * assigned to the aromatic group between 208 and 220 nm, the secondary transition π→π * at 243 nm due to the aromatic group, and the transition n→π * that is attributed to the C-Cl link located at 311 nm [33,39]. In the case of activated LDH (Figure 8a-c), it can be observed that as time passes, the intensity of the three bands decreases, which is associated with the degradation of the 2,4,6-trichlorophenol molecule, until the complete disappearance of the bands of the secondary transition π→π * at 243 nm occurs due to the aromatic group and the transition π→π * of the C-Cl bond, as well as the decrease until almost the disappearance of the primary transition n→π * assigned to the aromatic group at 240 min. In the case of the LDHM1F and LDHM2F catalysts, the decrease of the bands is very similar as a function of time, reaching degradation values higher than 90% at 90 min, while the LDHM3F catalyst at 90 min has only about 50% degradation, which is attributed to its band gap values of 2.34 and 2.47 eV. This is favored by the presence of Fe in the catalysts, requiring 240 min to reach values greater than 90% degradation of the entire organochlorine molecule. For TiO2 used as a reference In the case of the LDHM1F and LDHM2F catalysts, the decrease of the bands is very similar as a function of time, reaching degradation values higher than 90% at 90 min, while the LDHM3F catalyst at 90 min has only about 50% degradation, which is attributed to its band gap values of 2.34 and 2.47 eV. This is favored by the presence of Fe in the catalysts, requiring 240 min to reach values greater than 90% degradation of the entire organochlorine molecule. For TiO 2 used as a reference catalyst as a photocatalyst in the degradation of 2,4,6-trichlorophenol (Figure 8d), the intensity of the absorbance increases with the irradiation time, which is the opposite of the behavior of activated Mg/Fe LDH catalysts. The increase in the intensity of the signals is because the degradation of TiO 2 produces intermediates, which have higher absorptivity coefficients (This coefficient is proportional to the intensity in the absorbance), modifying the characteristic signals of 2,4,6-tetrachlorophenol at 245 and 310.5 nm. The intermediaries that are formed are mainly catechols, as well as benzoquinones and hydroxyquinones; all of them are compounds that preserve the aromatic ring increasing the signals between 200 and 225 nm. Figure 9 shows the graph of the relative degradation rate of 80 ppm of 2,4,6-trichlorophenol with different catalysts. It can be corroborated that the photocatalysts show a good degradation of 2,4,6-trichlorophenol at 90 min, reaching 93% for LDHM2F-400 • C, 92% for LDHM1F-400 • C, and 55% for LDHM3F-400 • C-values higher than the 18% degradation of TiO 2 -P25-400 • C. For the catalysts LDHM1F-400 • C and LDHM2F-400 • C, the degradation behavior as a function of time is very similar, only showing a small difference at the beginning of the degradation process, whereas the catalyst of Mg/Fe = 1 ratio at 15 min has degraded the pollutant more quickly, but at 30 min, both catalysts reach the same speed, which at 90 min is slightly higher for the ratio catalyst Mg/Fe = 2. and hydroxyquinones; all of them are compounds that preserve the aromatic ring increasing the signals between 200 and 225 nm. Figure 9 shows the graph of the relative degradation rate of 80 ppm of 2,4,6-trichlorophenol with different catalysts. It can be corroborated that the photocatalysts show a good degradation of 2,4,6trichlorophenol at 90 min, reaching 93% for LDHM2F-400 °C, 92% for LDHM1F-400 °C, and 55% for LDHM3F-400 °C-values higher than the 18% degradation of TiO2-P25-400 °C. For the catalysts LDHM1F-400 °C and LDHM2F-400 °C, the degradation behavior as a function of time is very similar, only showing a small difference at the beginning of the degradation process, whereas the catalyst of Mg/Fe = 1 ratio at 15 min has degraded the pollutant more quickly, but at 30 min, both catalysts reach the same speed, which at 90 min is slightly higher for the ratio catalyst Mg/Fe = 2. On the other hand, TiO2 shows zero activity during the first 15 min, and then the degradation of the pollutant begins at a low speed, which allows it to reach 14% degradation at 60 min after the degradation process has begun, and only 18% at 90 min, showing a decrease in rate. Figure 10 shows the adjustment of the kinetic model of the relative degradation rate of 80 ppm of 2,4,6-trichlorophenol with the different catalysts, which corresponds to a pseudo-first-order degradation behavior in all cases-corresponding to the kinetic model of Langmuir-Hinshelwood, which is used to describe many photocatalytic reactions where the rate follows the kinetics of the pseudo-first-order considering steady state conditions [38,40]. On the other hand, TiO 2 shows zero activity during the first 15 min, and then the degradation of the pollutant begins at a low speed, which allows it to reach 14% degradation at 60 min after the degradation process has begun, and only 18% at 90 min, showing a decrease in rate. Figure 10 shows the adjustment of the kinetic model of the relative degradation rate of 80 ppm of 2,4,6-trichlorophenol with the different catalysts, which corresponds to a pseudo-first-order degradation behavior in all cases-corresponding to the kinetic model of Langmuir-Hinshelwood, which is used to describe many photocatalytic reactions where the rate follows the kinetics of the pseudo-first-order considering steady state conditions [38,40]. Figure 10 shows the adjustment of the kinetic model of the relative degradation rate of 80 ppm of 2,4,6-trichlorophenol with the different catalysts, which corresponds to a pseudo-first-order degradation behavior in all cases-corresponding to the kinetic model of Langmuir-Hinshelwood, which is used to describe many photocatalytic reactions where the rate follows the kinetics of the pseudo-first-order considering steady state conditions [38,40]. As seen in the Figure 10, the velocity constantly increases when the Mg/Fe molar ratio decreases, which is attributed to the role that Fe 3+ plays in decreasing the bandgap value and allowing the photodegradation process to be carried out faster for the catalysts LDHM1F-400 • C and LDHM2F-400 • C, with the constant of apparent speed greater than 250 × 10 −4 min −1 and half-lives of 25 min. These are much higher than those of TiO 2 of 51 × 10 −4 min −1 , with average lifetimes of 136 min.

Mineralization Study
The analysis of organic carbon (TOC) is shown in Figure 11, where it can be seen that the degradation of 2,4,6-trichlorophenol reaches values close to 80% for the catalysts LDHM1F-400 • C and LDHM2F-400 • C, reaching a greater mineralization using the LDHM2F-400 • C catalyst at 120 min, with values of 82%, which are higher than those reached by LDHM3F-400 • C and TiO 2 -P25 of 61 and 29% at 120 min, respectively. As seen in the Figure 10, the velocity constantly increases when the Mg/Fe molar ratio decreases, which is attributed to the role that Fe 3+ plays in decreasing the bandgap value and allowing the photodegradation process to be carried out faster for the catalysts LDHM1F-400 °C and LDHM2F-400 °C, with the constant of apparent speed greater than 250 × 10 −4 min −1 and half-lives of 25 min. These are much higher than those of TiO2 of 51 × 10 −4 min −1 , with average lifetimes of 136 min.

Mineralization Study
The analysis of organic carbon (TOC) is shown in Figure 11, where it can be seen that the degradation of 2,4,6-trichlorophenol reaches values close to 80% for the catalysts LDHM1F-400 °C and LDHM2F-400 °C, reaching a greater mineralization using the LDHM2F-400 °C catalyst at 120 min, with values of 82%, which are higher than those reached by LDHM3F-400 °C and TiO2-P25 of 61 and 29% at 120 min, respectively.  Table 2 shows the values of the band gap, apparent speed constant, average flow time, percentage of degradation, and percentage of mineralization of the catalysts used in the degradation of 80 ppm of 2,4,6-trichlorophenol.   Table 2 shows the values of the band gap, apparent speed constant, average flow time, percentage of degradation, and percentage of mineralization of the catalysts used in the degradation of 80 ppm of 2,4,6-trichlorophenol. As can be seen, the LDHM1F and LDHM2 catalysts have very similar behaviors, however, the LDHM2F catalyst has a greater apparent speed constant, as well as a half-life of less than 25 min, 93% degradation and mineralization of 82%, which is why it can be considered as the catalyst with better photodegradation capacity for 2,4,6-trichlorophenol. This allowed LDHM2F-400 • C to be chosen to carry out studies on the possible mechanism of this photocatalytic reaction.

Detection of Hydroxyl Radicals (OH • )
In order to explore the mechanism of photocatalytic degradation, the possible formation of radicals was analyzed by fluorescence spectroscopy. For the detection of said radicals, coumarin was used as a molecule that captures the hydroxyl radicals, producing the hydroxyproduct 7-hydroxycoumarin [41], as shown in Figure 12. In order to explore the mechanism of photocatalytic degradation, the possible formation of radicals was analyzed by fluorescence spectroscopy. For the detection of said radicals, coumarin was used as a molecule that captures the hydroxyl radicals, producing the hydroxyproduct 7hydroxycoumarin [41], as shown in Figure 12 The fluorescence spectra obtained with hydroxycoumarin exhibit a characteristic band of emission between 400 and 600 nm. In the case of the activated LDHM2F catalyst, the intensity of the signal is low, which implies that there is little presence of OH • radicals associated with the scarce formation of these in 60 min of reaction. On the other hand, in the case of the reference catalyst TiO2-P25, an intense band associated with the production of hydroxycoumarin can be observed, due to the ability of the reference catalyst to produce hydroxyl radicals [42,43]. The above suggests that the activated LDHM2F catalyst does not favor the formation of OH • radicals.

Photocatalytic Evaluation of Superoxide Radicals ( 2 −• )
As observed in Equation (4), when a semiconductor material is irradiated with energy greater than or equal to that of its forbidden bandwidth, the electrons are photoexcited from the valence band to the conduction band, with the probability of migrating to the surface of the semiconductor and reacting with bubbled oxygen (Equation (5)) during the reaction to produce superoxide radicals, which, like the hydroxyl radicals, have great oxidizing power for degrading the organic compound [44].
Using this photocatalytic foundation as a model to determine the formation of superoxide radicals in the process, the UV-Vis spectra were obtained in the photodegradation of 2,4,6trichlorophenol. How the process develops in the presence of bubbled oxygen can be compared with The fluorescence spectra obtained with hydroxycoumarin exhibit a characteristic band of emission between 400 and 600 nm. In the case of the activated LDHM2F catalyst, the intensity of the signal is low, which implies that there is little presence of OH • radicals associated with the scarce formation of these in 60 min of reaction. On the other hand, in the case of the reference catalyst TiO 2 -P25, an intense band associated with the production of hydroxycoumarin can be observed, due to the ability of the reference catalyst to produce hydroxyl radicals [42,43]. The above suggests that the activated LDHM2F catalyst does not favor the formation of OH • radicals.

Photocatalytic Evaluation of Superoxide Radicals (O 2 −• )
As observed in Equation (4), when a semiconductor material is irradiated with energy greater than or equal to that of its forbidden bandwidth, the electrons are photoexcited from the valence band to the conduction band, with the probability of migrating to the surface of the semiconductor and reacting with bubbled oxygen (Equation (5)) during the reaction to produce superoxide radicals, which, like the hydroxyl radicals, have great oxidizing power for degrading the organic compound [44].
Using this photocatalytic foundation as a model to determine the formation of superoxide radicals in the process, the UV-Vis spectra were obtained in the photodegradation of 2,4,6-trichlorophenol. How the process develops in the presence of bubbled oxygen can be compared with a process with an absence of bubbling oxygen, where instead nitrogen gas is emitted, which is inert in the processes of photodegradation [45], as shown in Figure 13.
than or equal to that of its forbidden bandwidth, the electrons are photoexcited from the valence band to the conduction band, with the probability of migrating to the surface of the semiconductor and reacting with bubbled oxygen (Equation (5)) during the reaction to produce superoxide radicals, which, like the hydroxyl radicals, have great oxidizing power for degrading the organic compound [44].
Using this photocatalytic foundation as a model to determine the formation of superoxide radicals in the process, the UV-Vis spectra were obtained in the photodegradation of 2,4,6trichlorophenol. How the process develops in the presence of bubbled oxygen can be compared with a process with an absence of bubbling oxygen, where instead nitrogen gas is emitted, which is inert in the processes of photodegradation [45], as shown in Figure 13. As can be seen, in the presence of O 2 the catalyst shows a good degradation capacity of 2,4,6-trichlorophenol, achieving the elimination of the signals of the vibrations of the functional groups C-Cl and C-OH, as well as a decrease of the CC and CH vibrations of the aromatic ring at 240 min. On the other hand, in the presence of N 2 it is observed that the catalyst is active in the partial degradation of the 2,4,6-trichlorophenol molecule, showing an almost total decrease of the vibrations of the functional groups C-Cl and C-OH, but only a small decrease in the CC and CH vibrations of the aromatic ring at 240 min.
As seen in Figure 14, the photocatalytic activity decreases by about 35% for the elimination of the OH and Cl functional groups in the absence of bubbled oxygen, according to the values of the apparent kinetic constants. The above confirms that the generation of superoxide radicals is determinant for the elimination of the functional groups, as well as for the degradation of the aromatic ring for the complete photodegradation of 2,4,6-trichlorophenol. The partial degradation of the 2,4,6-trichlorophenol molecule in the absence of oxygen suggests the participation of photogenerated voids (h + ) in the catalyst. As can be seen, in the presence of O2 the catalyst shows a good degradation capacity of 2,4,6trichlorophenol, achieving the elimination of the signals of the vibrations of the functional groups C-Cl and C-OH, as well as a decrease of the CC and CH vibrations of the aromatic ring at 240 min. On the other hand, in the presence of N2 it is observed that the catalyst is active in the partial degradation of the 2,4,6-trichlorophenol molecule, showing an almost total decrease of the vibrations of the functional groups C-Cl and C-OH , but only a small decrease in the CC and CH vibrations of the aromatic ring at 240 min.
As seen in Figure 14, the photocatalytic activity decreases by about 35% for the elimination of the OH and Cl functional groups in the absence of bubbled oxygen, according to the values of the apparent kinetic constants. The above confirms that the generation of superoxide radicals is determinant for the elimination of the functional groups, as well as for the degradation of the aromatic ring for the complete photodegradation of 2,4,6-trichlorophenol. The partial degradation of the 2,4,6-trichlorophenol molecule in the absence of oxygen suggests the participation of photogenerated voids (h + ) in the catalyst.

Photocatalytic Evaluation of the Hole Trap (h + )
The evaluation of the photocatalytic activity by gauging holes was evaluated using a model molecule of ammonium oxalate as a sacrificial agent [46][47][48][49]. Figure 15 shows the UV-Vis absorption spectra of the photodegradation of 2,4,6-trichlorophenol in the presence of ammonium oxalate with

Photocatalytic Evaluation of the Hole Trap (h + )
The evaluation of the photocatalytic activity by gauging holes was evaluated using a model molecule of ammonium oxalate as a sacrificial agent [46][47][48][49]. Figure 15 shows the UV-Vis absorption spectra of the photodegradation of 2,4,6-trichlorophenol in the presence of ammonium oxalate with oxygen and nitrogen flow.

Photocatalytic Evaluation of the Hole Trap (h + )
The evaluation of the photocatalytic activity by gauging holes was evaluated using a model molecule of ammonium oxalate as a sacrificial agent [46][47][48][49]. Figure 15 shows the UV-Vis absorption spectra of the photodegradation of 2,4,6-trichlorophenol in the presence of ammonium oxalate with oxygen and nitrogen flow. According to the adsorption spectra, in the case of the photodegradation of 2,4,6-trichlorophenol in the presence of oxygen and ammonium oxalate, a reduction in the degradation of both the functional groups and the aromatic ring is observed. This confirms that the gaps that are formed in the LDHM2F-400 • C catalyst contribute in a significant way to the catalytic activity. On the other hand, in the case of the process of photodegradation in the absence of oxygen and in the presence of ammonium oxalate, it can be observed that the photodegradation process is completely modified, with the formation of a new band at the center at 275 nm. This is attributed to the formation of intermediaries which are identified by the signal of 2-chlorophenol, as well as a phase shift of the aromatic band attributed to the formation of phenol [27]. The above confirms that the catalytic activity of LDHM2F depends on the presence of voids, as well as the formation of superoxide radicals. Table 3 shows the comparison of the apparent kinetic constants, percentage of degradation, and percentage of mineralization of the evaluation of the active species involved in the photodegradation of 2,4,6-trichlorophenol. The catalytic activity related to the degradation of 2,4,6-trichlorophenol is decreased by more than 50% in the presence of ammonium oxalate and oxygen but is even more decreased in the absence of oxygen. As for mineralization, this is reduced by 77% in the absence of oxygen and in the presence of ammonium oxalate, which confirms that the degradation is partial, with the formation of intermediaries and not until mineralization has occurred. This behavior indicates that both the superoxide radicals and the holes (h + ) are the determinants, and both species contribute to the mechanism of photodegradation until the mineralization of 2,4,6-trichlorophenol using the LDHM2F-400 • C catalyst. The results in Table 3 show that the oxidation of 2,4,6-trichlorophenol occurs first in the holes (h + ) photogenerated in the double-layered hydroxides under reconstruction and subsequently the intermediates are removed by further oxidation with superoxide radicals or other oxygen oxidizing species.
2.13. Possible 2,4,6-Trichlorophenol Degradation Mechanisms Figure 16 shows a diagram of the proposed mechanism for the degradation of 2,4,6-trichlorophenol based on the properties of the catalysts and the different types of free radicals involved. As could be demonstrated in the fluorescence test for the detection of the generation of superoxide radicals, this is the main route involved in the degradation of the pollutant and, to a lesser extent, the holes. As observed in coumarin tests, photocatalysts do not favor the formation of hydroxyl radicals, so these free radicals do not contribute to the mechanism. Magnesium has a Pauling electronegativity of 1.31 eV and iron of 1.83 eV, so iron has a greater tendency to attract electrons to itself and transfer them to O 2 to generate the superoxide radical.  As proposed in the possible degradation routes, this occurs when the activated layered double hydroxides, which are in the form of simple and mixed oxides, meet the aqueous medium with oxygen, which when irradiated produce an excess of electrons in the conduction band and positive gaps in the valence band, as shown in Equation (6).

LDHMF-400 °C
On the other hand, electrons over the conduction band react with molecular oxygen, which acts as an electron acceptor to form superoxide radicals (Equation (7)).
The generated superoxide radicals can attack and oxidize 2,4,6-trichlorophenol (Equation (8)). As proposed in the possible degradation routes, this occurs when the activated layered double hydroxides, which are in the form of simple and mixed oxides, meet the aqueous medium with oxygen, which when irradiated produce an excess of electrons in the conduction band and positive gaps in the valence band, as shown in Equation (6).
On the other hand, electrons over the conduction band react with molecular oxygen, which acts as an electron acceptor to form superoxide radicals (Equation (7)).
The final LDHMF catalytic precursor is recovered thanks to the memory effect, a property characteristic of the laminar double hydroxide materials [50][51][52]. Said precursor can be reactivated for a second cycle as a catalyst for the degradation of 2,4,6-trichlorophenol.
The degradation to the mineralization takes place thanks to the presence of superoxide radicals accompanied by the holes until the disappearance of the total organic carbon [32,[53][54][55][56], implying a mechanism in which the superoxide radicals are carrying out the degradation of the aromatic ring simultaneously with the elimination of chlorine, since the formation of monochlorinated intermediates or phenols is not observed by the ultraviolet spectrum.
The catalyst with the highest photocatalytic activity is LDHM2F, whose pore volume value is higher compared to the LDHM1F-400 • C and LDHM3F-400 • C catalysts. This may indicate that there is enough separation between the laminar structures of the catalysts, promoting an improvement in the transfer of charges (e − and h + ) by decreasing the recombination and, therefore, increasing the photocatalytic activity.
In the analysis by SEM, it is observed that the particle size of the LDHM2F-400 • C catalysts is lower than that of LDHM1F-400 • C, which indicates that, by the synthesis method used, the nucleation is different with the addition of Fe to the LDH. Being smaller particles, a lower percentage of conglomerates is obtained, suggesting that Fe increases directly in the LDH by modifying its electronegativity in such a way that a better transfer of charges is obtained, and with this the photocatalytic activity increases.
The main advantages of the activated layered double hydroxides are that they are not toxic, they can regenerate for continuous use, and they can be synthesized in an easy way, and without needing to be doped. and subsequently coprecipitated at a pH of 11.5 with sodium hydroxide (NaOH) (Fermont, Lopez Mateos, Mexico). The coprecipitate was left and aged for 24 h, washed until it reached a pH of 9, and dried at 100 • C. The materials were identified as LDHM1F, LDHM2F, and LDHM3F, corresponding to the Mg/Fe = 1, 2, and 3 ratios.

Activation of Layered Double Hydroxides
The LDHs that were synthesized were thermally treated at 400 • C in an air atmosphere for 4 h for the formation of the mixed Mg/Fe oxides and were identified as LDHM1F-400 • C, LDHM2F-400 • C, and LDHM3F-400 • C.

Physicochemical Characterization of Catalytic Pre-Cursors and Catalysts
The materials were characterized by physicochemically fresh and calcined. To corroborate the present crystalline phase, X-ray diffraction was performed on a Siemens D500 powder diffractometer (University of Guanajuato, Guanajuato, Mexico) with CuKα radiation, a graphite crystal monochromator with a step of 2θ equal to 0.02 s −1 , and a counting time of 9 s per point. The thermal analyses were carried out in a TA Instruments Thermoanalyzer (University of Guanajuato, Guanajuato, Mexico) at a heating rate of 10 • C/min in an air atmosphere, at a speed of 100 mL/min and using α-alumina as a reference. The infrared spectra with Fourier transform were obtained in a Bruker model Tensor 27 Hyperion 7000 (University of Guanajuato, Guanajuato, Mexico) with a resolution of 4 cm −1 and 20 scans, from 400 to 4000 cm −1 , and the samples were prepared by dilution with KBr. The nitrogen adsorption-desorption isotherms were determined in TriStar Micromeritics equipment (University of Guanajuato, Guanajuato, Mexico), with the samples previously dried at 100 • C for 24 h, with a degassing at 150 • C, and a vacuum pressure of up to 0.5 mmHg. The BET model was used to obtain the specific area. Scanning electron microscopy analysis was performed on a Seizz 1550VP microscope with field emission, with Oxford EDS equipment (University of Guanajuato, Guanajuato, Mexico) with an opening of 30.0 µm and a width of 3.1 mm. The band gap energy of the photocatalysts was calculated from the ultraviolet absorption spectra coupled with an integrating sphere (diffuse reflectance) in a UV-Vis Recording S UV2401 Shimadzu instrument (University of Guanajuato, Guanajuato, Mexico), and using the Kubelka-Munk theory, which consists of plotting the energy of the photon against the square root of the Kubelka-Munk function multiplied by the energy of the photon and extrapolating the linear part with the abscissa axis.

Degradation of 2,4,6-Trichlorophenol
The photocatalytic degradation capacity of 2,4,6-trichlorophenol using activated LDH was determined under the following conditions: standard 200 ml solution at a concentration of 80 ppm of 2,4,6-trichlorophenol (Sigma-Aldrich, St. Louis, MO, USA), in a Batch reactor at a controlled temperature of 25 • C with constant magnetic stirring of 700 rpm, with a flow of air of 2 mL/s and a UV light irradiation of 254 nm, and an emission of 2.5 mW/cm 2 generated by a Pen-Ray UV lamp inserted in a tube of quartz. The photoactivity of all materials was determined by using 1 g/L of photocatalyst. To determine the adsorption phenomena effect, the suspension was stirred at 800 rpm under airflow in dark conditions for 1 h; after that, an aliquot was collected, and the reaction was started by turning on the UV lamp that was kept on for 240 min while stirring. Additionally, a sample of 2,4,6-trichlorophenol solution was subjected to photolysis in the absence of any catalyst to determine the effect of the radiation on the contaminant. In addition, for the comparison against a reference photocatalyst, commercial TiO 2 -P25 was used. In all cases, the process of degradation of 2,4,6-trichlorophenol was monitored using an aliquot sample of the reactor, with the subsequent quantification of this in a UV-Vis Cary 100 spectrophotometer (Metropolitan Autonomous University, Mexico City, Mexico) at a wavelength of 310.5 nm. The aliquots were collected at 15-minute intervals for 240 min, and in order to separate the solid catalyst from the aqueous solution, the aliquots were filtered using a nitrocellulose membrane with a pore size of 0.22 µm (Millipore Corporation, Burlington, Massachusetts, Estados Unidos). The amount of total organic carbon present in the irradiated solution was determined in a TOC-V-CSH/CSN Shimadzu 5000 TOC (Metropolitan Autonomous University, Mexico City, Mexico) to corroborate the degradation of the molecule until mineralization.

Detection of Hydroxyl and Superoxide Radicals and Study of the Hole Trap
A dilute aqueous solution (2 × 10 −3 M) of coumarin (Sigma-Aldrich, St. Louis, MO, USA) was prepared, in which 200 mL of solution and 200 mg of photocatalyst to be analyzed were poured into a Batch reactor. TiO 2 -P25 was used as the reference material. As above, the study was carried out in the absence of a photocatalyst (Photolysis) to observe the possible production of hydroxyl radicals with and without a photocatalyst. Once this was done, the solution was irradiated with UV light for 1 h with a Pen-Ray lamp (λ = 254 nm and I0 = 4.4 mWcm −2 ) under conditions of constant stirring, oxygen bubbling, and temperature (800 rpm, 1 mL/s, and 25 • C, respectively), extracting 3 mL aliquots at 10 min intervals. Finally, the fluorescence emission spectra in the irradiated solution were analyzed by photoluminescence in a Fluorescence spectroscopy Scinco FS-2 spectrometer (Metropolitan Autonomous University, Mexico City, Mexico), a wavelength of 320 nm, and the results obtained with the synthesized materials and photolysis were compared with those obtained using the reference solid TiO 2 -P25.

Photocatalytic Evaluation of Hole Capture with Ammonium Oxalate as a Sacrificial Agent
The photocatalytic reaction was monitored with the material with the highest photodegradation (HTM2F-400 • C) in the presence of ammonium oxalate (Sigma-Aldrich, St. Louis, MO, USA), and with oxygen and nitrogen flow. An aqueous solution of 246-TCF at 80 ppm was used, and 1 g/L of the photocatalyst with higher activity and a concentration of 0.004 M of ammonium oxalate were poured into a reactor. The solution was irradiated with UV light, maintaining the conditions of constant stirring, bubbling of nitrogen/oxygen, and temperature (800 rpm, 1 mL/s, and 25 • C, respectively), while extracting aliquots of 3 mL to be analyzed by UV-Vis spectroscopy.

Conclusions
The results of the present work show that layered double hydroxides of different Mg/Fe molar ratio can be synthesized by the coprecipitation method, which have a hydrotalcite crystalline structure, and which when calcined at 400 • C evolve to a crystalline phase of periclase and an amorphous phase of spinel, with Type IV isotherms characteristic of mesoporous materials and specific areas between 273.9 and 248.9 m 2 /g. Layered double hydroxides activated at 400 • C have Eg values ranging from 2.28 to 2.47, which are lower values than TiO 2 , so they have better semiconductor properties. These photocatalysts have good photocatalytic activity, with degradation efficiencies for 2,4,6-trichlorophenol of 93% LDHM2F-400 • C > 92% LDHM1F-400 • C > 55% LDHM3F-400 • C > 18% TiO 2 -P25-400 • C in less than 90 minutes. Therefore, it is concluded that the most active catalysts are LDHM2FI-400 • C and LDHM1F-400 • C, which present a greater amount of iron in the structure and which reach mineralization values of up to 82%. The degradation mechanism proposed for the photodegradation of 2,4,6-trichlorophenol considers that the degradation occurs first in the photogenerated holes in the layered double hydroxides under reconstruction and then the intermediates are removed by further oxidation with the superoxide radicals or other oxidizing species of oxygen. These photocatalysts obtained from Mg/Fe layered double hydroxides are promising for the photodegradation of recalcitrant chlorinated compounds.