Undoped and Eu3+ Doped Magnesium-Aluminium Layered Double Hydroxides: Peculiarities of Intercalation of Organic Anions and Investigation of Luminescence Properties

The Mg3/Al and Mg3/Al0.99Eu0.01 layered double hydroxides (LDHs) were fabricated using a sol-gel chemistry approach and intercalated with different anions through ion exchange procedure. The influence of the origin of organic anion (oxalate, laurate, malonate, succinate, tartrate, benzoate, 1,3,5-benzentricarboxylate (BTC), 4-methylbenzoate (MB), 4-dimethylaminobenzoate (DMB) and 4-biphenylacetonate (BPhAc)) on the evolution of the chemical composition of the inorganic-organic LDHs system has been investigated. The obtained results indicated that the type and arrangement of organic guests between layers of the LDHs influence Eu3+ luminescence in the synthesized different hybrid inorganic–organic matrixes. For the characterization of synthesis products X-ray diffraction (XRD) analysis, infrared (FTIR) spectroscopy, fluorescence spectroscopy (FLS), and scanning electron microscopy (SEM), were used.


A general chemical formula of layered double hydroxides (LDHs) is [M 2+
1−x M 3+ x (OH) 2 ] x+ (A y− ) x/y ·zH 2 O, here M 2+ and M 3+ are divalent and trivalent cations forming layered structure, respectively, and A y− is anion occupying interlayer space [1]. LDHs show hexagonal crystal structure that depends on different parameters of the intercalated species. Intercalation of different anions in LDH is a challenging topic because the anion-exchange could be performed mostly, when the introduced anion has higher affinity with the LDH layer than the host anion. Usually, the anions with small size and high charge density are used for such investigations. Nevertheless, the low-charge large organic anions could also be introduced to the LDH structure [2]. The possibility to substitute of monovalent anions in the Mg/Al LDH could be expressed by following order OH − > F − > Cl − > Br − > NO 3− . More selective are anions with higher charge CO 3 2− > SO 4 2− [3].
The anion-exchange selectivity is usually related to the guest orientation. Two orientations are observed for the organic anion within the gallery either vertical perpendicular to the layers or horizontal. Whether a vertical or horizontal orientation exists, depends upon the charge on the layers and the degree of hydration of the sample. Moreover, the water molecules stabilize the LDH structure via formation of a hydrogen bond [4][5][6]. The organic anions can create negative charge  4-dimethylaminobenzoate (DMB) and 4-biphenylacetonate (BPhAc) were synthesized using anion exchange technique. For this, 2 mmol of Mg 3 /Al or Mg 3 /Al 0.99 Eu 0.01 was immersed in the solution of disodium/sodium organic compounds with 1.5 molar excess amounts in comparison with LDHs. Next, the solution was stirred at room temperature for 24 h. After filtration and washing with deionized water and acetone, the synthesis product was dried at 40 • C for 12 h.

Characterization
X-ray diffraction analysis (XRD, Rigaku Mini Flex, Rigaku, The Woodlands, TX, USA) of synthesized compounds were performed with MiniFlex II diffractometer (Rigaku) using a primary beam Cu Kα radiation (λ = 1.541838 Å). The 2θ angle of the diffractometer was gradated from 8 to 80 • in steps of 0.02 • , with the measuring time of 0.4 s per step. Fourier-transform infrared spectroscopy (FT-IR) spectra were recorded using Bruker-Alpha FT-IR spectrometer (Bruker, Ettlingen, Germany) in the range of 4000-400 cm −1 . The luminescent properties were investigated using Edinburg Instruments FLS 980 spectrometer (Edinburgh Instruments, Kirkton Campus, UK). The surface morphological features were characterized using a scanning electron microscope (SEM, Hitachi, Tokyo, Japan) Hitachi SU-70. The particle and anion dimension sizes were calculated using the ImageJ and Avogadro programmes (Jolla, CA, USA). The amount of carbonate in the synthesized samples was calculated from the M II /M III atomic ratios, assuming that carbonate is the only charge balancing interlayer anion. The water content in the formula was determined from the results of TG analyses. The chemical composition was defined to be [Mg 0.75 Al 0.25 (OH) 2 ] (CO 3 ) 0.125 ·4H 2 O.

Results and Discussion
It is reported [3] that LDH containing not only nitrates or chlorides, but also CO 3 2− could be used for intercalation of other inorganic anions. Free CO 3 2− and the NO 3 − anions show similar symmetry, however, behave differently as interlayer anions in LDHs structure. The CO 3 2− is orientated parallel to the hydroxide layers. It can easily interact with hydroxyl groups of hydroxide layers by forming hydrogen bonds [25]. The NO 3 − has molecular plane tilted orientation, which makes disorder of the 3R rhombohedral symmetry [26] within a hexagonal unit cell of LDH crystal structure. Previously, the LDHs were obtained using the anion-exchanged method showing that values of basal spacing c increased significantly in comparison with starting carbonate containing LDH [11]. The parameter c depends on the size, charge and orientation of the intercalated species. In this work, the intercalated organic anions, such as short-long carbon chains (oxalate, laurate, malonate, succinate, tartrate) and benzoic (benzoate, 1,3,5-benzentricarboxylate, 4-methylbenzoate, 4-dimethylaminobenzoate and 4-biphenylacetonate) carboxyl acid groups could be arranged by anions size in the interlayer and by the charge to compensate the hydroxide layer. In the XRD patterns of the LDH phases obtained by the anion exchanged reactions the diffraction peaks were shifted to the lower values of 2θ angle proving that values of the basal spacing c increased. The positions of diffraction peaks (003) of LDHs intercalated with short-long chains (Mg 3 /Al-succinate, Mg 3 /Al-malonate, Mg 3 /Al-tartrate, Mg 3 /Al-laurate and Mg 3 /Al-oxalate (see Figure 1)) are shifted to smaller 2θ angle values. The similar shift was observed and for the LDHs modified with benzoic carboxylates (Figure 2). The determined values of the lattice parameters c (see Table 1) were monotonically increased from c = 23.613 Å for the Mg 3 /Al-CO 3 to c = 24.375 Å for the Mg 3 /Al-oxalate (in the case of short-long chains intercalation) and to c = 24.492 Å for the Mg 3 /Al 1 -4-biphenylacetonate (in the case of derivatives of aromatic hydrocarbons). These results led us to conclude that all anions studied have been successfully intercalated to the Mg 3 /Al LDHs structure.    The dimensions of anions (Table 2) show that the oxalate anion of intercalated LDH was the smallest by length (1.94 Å ) and having the highest height (5.01 Å ). Since the determined c parameter for the Mg3/Al-oxalate modified LDH is the largest between short-long chains intercalation, it can be deduced that the oxalate anion has specific vertical orientation in the LDHs (see Figure 3). In the case of aromatic hydrocarbons, the height of all anions is very similar. Therefore, the 4-biphenylacetonate which has a largest length (10.06 Å ) has horizontal orientation in the LDH structure ( Figure 3). The Mg3/Al-oxalate and the Mg3/Al-4-biphenylacetonate LDHs having similar basal spacings correspond to the intercalated LDHs with vertical and horizontal anion orientations in which they are grafting into the hydroxide layers. There are spherical energetic interferences between -CH3 groups of anions and M-OH hydroxide layers what cause difficult intercalation in the LDH structure. The formation of hydrogen bonds between water molecules in the layers, the hydroxide layers, the interlayer anions, and among the H2O molecules themselves is possible. The orientation of oxalate anion possibly is related to the formation of H2O molecules more compact structures with the two -COO − groups than with the hydrophobic ends of the monocarboxylate. Four oxalate -COO-groups are distributed perpendicular to the layers, with two O-atoms coordinated to different hydroxide layers. In the case of 4-biphenylacetonate, the -COO-groups are orientated differently, and the O-atoms of its -COO − groups that situated parallel to the layers can occupy M-OH sites along the H-H vectors, whereas those -COO-tend to occupy the centers of the M-OH triangles. The dimensions of anions (Table 2) show that the oxalate anion of intercalated LDH was the smallest by length (1.94 Å) and having the highest height (5.01 Å). Since the determined c parameter for the Mg 3 /Al-oxalate modified LDH is the largest between short-long chains intercalation, it can be deduced that the oxalate anion has specific vertical orientation in the LDHs (see Figure 3). In the case of aromatic hydrocarbons, the height of all anions is very similar. Therefore, the 4-biphenylacetonate which has a largest length (10.06 Å) has horizontal orientation in the LDH structure ( Figure 3). The Mg 3 /Al-oxalate and the Mg 3 /Al-4-biphenylacetonate LDHs having similar basal spacings correspond to the intercalated LDHs with vertical and horizontal anion orientations in which they are grafting into the hydroxide layers. There are spherical energetic interferences between -CH 3 groups of anions and M-OH hydroxide layers what cause difficult intercalation in the LDH structure. The formation of hydrogen bonds between water molecules in the layers, the hydroxide layers, the interlayer anions, and among the H 2 O molecules themselves is possible. The orientation of oxalate anion possibly is related to the formation of H 2 O molecules more compact structures with the two -COO − groups than with the hydrophobic ends of the monocarboxylate. Four oxalate -COO-groups are distributed perpendicular to the layers, with two O-atoms coordinated to different hydroxide layers. In the case of 4-biphenylacetonate, the -COO-groups are orientated differently, and the O-atoms of its -COO − groups that situated parallel to the layers can occupy M-OH sites along the H-H vectors, whereas those -COO-tend to occupy the centers of the M-OH triangles.     Europium substitution effects incorporating Eu 3+ at the Al 3+ positions in Mg3Al-organic anion LDHs have been investigated. According to [27], the Mg3/Al0.99Eu0.01 (with 1 mol% of Eu) have been prepared and intercalated with different organic anions. The XRD patterns (Figures 4 and 5) for the hybrid inorganic-organic Mg3/Al0.99Eu0.01 LDHs showed, that the position of the (003) diffraction line is relevant to the interlayer distance and depends on the size of the intercalated organic anion. Surprisingly, the shift of the diffraction lines in the XRD patterns of intercalated with different organic anions of Eu 3+ -substituted LDHs is less pronounced in comparison with the samples without europium. This might be due to the reason, that the electrostatic attraction between mixed-metal cations and anions is weaker influencing on the distance of interlayer. Europium substitution effects incorporating Eu 3+ at the Al 3+ positions in Mg 3 Al-organic anion LDHs have been investigated. According to [27], the Mg 3 /Al 0.99 Eu 0.01 (with 1 mol% of Eu) have been prepared and intercalated with different organic anions. The XRD patterns (Figures 4 and 5) for the hybrid inorganic-organic Mg 3 /Al 0.99 Eu 0.01 LDHs showed, that the position of the (003) diffraction line is relevant to the interlayer distance and depends on the size of the intercalated organic anion. Surprisingly, the shift of the diffraction lines in the XRD patterns of intercalated with different organic anions of Eu 3+ -substituted LDHs is less pronounced in comparison with the samples without europium. This might be due to the reason, that the electrostatic attraction between mixed-metal cations and anions is weaker influencing on the distance of interlayer. prepared and intercalated with different organic anions. The XRD patterns (Figures 4 and 5) for the hybrid inorganic-organic Mg3/Al0.99Eu0.01 LDHs showed, that the position of the (003) diffraction line is relevant to the interlayer distance and depends on the size of the intercalated organic anion. Surprisingly, the shift of the diffraction lines in the XRD patterns of intercalated with different organic anions of Eu 3+ -substituted LDHs is less pronounced in comparison with the samples without europium. This might be due to the reason, that the electrostatic attraction between mixed-metal cations and anions is weaker influencing on the distance of interlayer.  FT-IR spectra of Mg3/Al, Mg3/Al0.99Eu0.01 and hybrid inorganic-organic LDHs are shown in Figures 6 and 7. The spectra of all samples are almost identical with very little differences. The broad absorptions visible at 3500-3000 cm −1 are characteristic vibrations of (-OH) groups [11]. The most intensive absorption bands detectible at 1360 cm −1 could be assigned to the asymmetric vibrations of CO3 2− , which still exists in the interlayer of intercalated LDHs along with intercalated organic anions. The absorption bands in the range of 1570-1627 cm −1 are assigned to the of carbon-oxygen bonds of (-COO − ) group. The first absorption band is related to the asymmetric vibration of the carboxylate group (υas, COO − ) and the second is attributable to the symmetric vibration of the carboxylate group (υs, COO − ), demonstrating the coordination of carboxylates to Mg3/Al-benzoate (h), Mg3/Al-1,3,5benzentricarboxylate (i), Mg3/Al-4-methylbenzoate ( Figure 6) and Mg3/Al0.99Eu0.01-benzoate (g), Mg3/Al0.99Eu0.01-1,3,5-benzentricarboxylate (h) (Figure 7). The absorption bands visible at 2850-2937 cm −1 are due to the C-H stretching vibrations of methylene (-CH2-) of the organic compounds. Thus, the FT-IR results prove the formation of the inorganic-organic hybrids and interactions of the introduced organic species with the LDH layers. FT-IR spectra of Mg 3 /Al, Mg 3 /Al 0.99 Eu 0.01 and hybrid inorganic-organic LDHs are shown in Figures 6 and 7. The spectra of all samples are almost identical with very little differences. The broad absorptions visible at 3500-3000 cm −1 are characteristic vibrations of (-OH) groups [11]. The most intensive absorption bands detectible at 1360 cm −1 could be assigned to the asymmetric vibrations of CO 3 2− , which still exists in the interlayer of intercalated LDHs along with intercalated organic anions. The absorption bands in the range of 1570-1627 cm −1 are assigned to the of carbon-oxygen bonds of (-COO − ) group. The first absorption band is related to the asymmetric vibration of the carboxylate group (υ as , COO − ) and the second is attributable to the symmetric    Figure 8. The emission spectra of Mg3/Al0.99Eu0.01-organic anion LDHs show four main emission lines between 550 nm and 740 nm. All observed emission bands are due to 5 D0-7 FJ (J = 1, 2, 3, 4) transitions of Eu 3+ ions. According to the literature, the emissions are 5 D0→ 7 F1 (590 nm), 5 D0→ 7 F2 (613 nm), 5 D0→ 7 F3 (650 nm) and 5 D0→ 7 F4 (697 nm) transitions typical of Eu 3+ ion [28]. The Eu 3+ ions occupy a low-symmetry site, since the emission due to 5 D0→ 7 F2 transition is the strongest. Moreover, the results obtained indicate that the excitation energy to the Eu 3+ ion in most of the cases is transferring from the organic anion ligands increasing    Figure 8. The emission spectra of Mg3/Al0.99Eu0.01-organic anion LDHs show four main emission lines between 550 nm and 740 nm. All observed emission bands are due to 5 D0-7 FJ (J = 1, 2, 3, 4) transitions of Eu 3+ ions. According to the literature, the emissions are 5 D0→ 7 F1 (590 nm), 5 D0→ 7 F2 (613 nm), 5 D0→ 7 F3 (650 nm) and 5 D0→ 7 F4 (697 nm) transitions typical of Eu 3+ ion [28]. The Eu 3+ ions occupy a low-symmetry site, since the emission due to 5 D0→ 7 F2 transition is the strongest. Moreover, the results obtained indicate that the excitation energy to the Eu 3+ ion in most of the cases is transferring from the organic anion ligands increasing The emission spectra obtained at room temperature of Mg 3 /Al 0.99 Eu 0.01 and Mg 3 /Al 0.99 Eu 0.01 samples intercalated with benzoate, oxalate, laurate, malonate, succinate, tartrate, 1,3,5-benzentricarboxylate (BTC), 4-methylbenzoate (MB), 4-dimethylaminobenzoate (DMB) and 4-biphenylacetonate (BPhAc) anions (λ ex = 394 nm) are presented in Figure 8. The emission spectra of Mg 3 /Al 0.99 Eu 0.01 -organic anion LDHs show four main emission lines between 550 nm and 740 nm. All observed emission bands are due to 5 D 0 -7 F J (J = 1, 2, 3, 4) transitions of Eu 3+ ions. According to the literature, the emissions are 5 D 0 → 7 F 1 (590 nm), 5 D 0 → 7 F 2 (613 nm), 5 D 0 → 7 F 3 (650 nm) and 5 D 0 → 7 F 4 (697 nm) transitions typical of Eu 3+ ion [28]. The Eu 3+ ions occupy a low-symmetry site, since the emission due to 5 D 0 → 7 F 2 transition is the strongest. Moreover, the results obtained indicate that the excitation energy to the Eu 3+ ion in most of the cases is transferring from the organic anion ligands increasing the intensity of emission of the LDHs. Two mechanisms of intramolecular and intermolecular energy transfer between lanthanide ions and organic molecules have been suggested [29]. As was stated in [29], the intensity of emission of lanthanide distributed in host matrixes is affected by the energy matching degree between organic ligands and lanthanide ions. Evidently, when the energy matching degree is better, the energy transfer efficiency is higher and, consequently, the emission intensity of the compound is higher. The potency to absorb the UV radiation by interlayer organic anions and possible transfer this energy to the Eu 3+ center by the interaction between the carboxyl oxygen of the intercalated anions with the hydrogen of the M(OH) 6 octahedra via a hydrogen bond was suggested. The tartrate and benzoate having the strong basicity, showed higher ability to absorb the light [30]. Carbonate is a weaker base, thus transferring less energy to Eu 3+ ions. The aromatic ring in the benzene can also influence the levels of resonant energy of lanthanide ions. As we can see from emission spectra the Mg 3 /Al 0.99 Eu 0.01 -tartrate and Mg 3 /Al 0.99 Eu 0.01 -benzoate LDHs show the highest emission intensity to compare with LDHs containing other organic ligands. Carboxylate and carbonyl groups connected with aromatic ring usually decrease the intensity of emission. The energy matching degree in the benzoate and Eu(III) complex obviously should be enhanced influencing the intensity of emission [31]. Moreover, the bridge of methylene groups -CH 2 -can break up the conjugated π-electron system [18]. the intensity of emission of the LDHs. Two mechanisms of intramolecular and intermolecular energy transfer between lanthanide ions and organic molecules have been suggested [29]. As was stated in [29], the intensity of emission of lanthanide distributed in host matrixes is affected by the energy matching degree between organic ligands and lanthanide ions. Evidently, when the energy matching degree is better, the energy transfer efficiency is higher and, consequently, the emission intensity of the compound is higher. The potency to absorb the UV radiation by interlayer organic anions and possible transfer this energy to the Eu 3+ center by the interaction between the carboxyl oxygen of the intercalated anions with the hydrogen of the M(OH)6 octahedra via a hydrogen bond was suggested. The tartrate and benzoate having the strong basicity, showed higher ability to absorb the light [30].
Carbonate is a weaker base, thus transferring less energy to Eu 3+ ions. The aromatic ring in the benzene can also influence the levels of resonant energy of lanthanide ions. As we can see from emission spectra the Mg3/Al0.99Eu0.01-tartrate and Mg3/Al0.99Eu0.01-benzoate LDHs show the highest emission intensity to compare with LDHs containing other organic ligands. Carboxylate and carbonyl groups connected with aromatic ring usually decrease the intensity of emission. The energy matching degree in the benzoate and Eu(III) complex obviously should be enhanced influencing the intensity of emission [31]. Moreover, the bridge of methylene groups -CH2-can break up the conjugated πelectron system [18].  The SEM micrographs depicted in Figure 9 represent the microstructure of Mg3/Al-CO3 and Mg3/Al0.99Eu0.01-CO3 layered double hydroxides. As seen, the solids are composed of particles having plate form and size about of 200-400 nm. The representative SEM micrographs of LDHs intercalated with different organic anions are shown in Figure 10. The surface microstructure still represents the characteristic features of LDHs [32], however, the particle sizes increased considerably (500-600 nm). Finally, the SEM micrographs of the samples which showed the most intensive emission Mg3/Al0.99Eu0.01-tartrate and Mg3/Al0.99Eu0.01-benzoate are presented in Figure 11. Evidently, the surface microstructure of these two samples is almost identical. The hexagonally shaped particles with the size of ~450-500 nm have formed. The SEM micrographs depicted in Figure 9 represent the microstructure of Mg 3 /Al-CO 3 and Mg 3 /Al 0.99 Eu 0.01 -CO 3 layered double hydroxides. As seen, the solids are composed of particles having plate form and size about of 200-400 nm. The representative SEM micrographs of LDHs intercalated with different organic anions are shown in Figure 10. The surface microstructure still represents the characteristic features of LDHs [32], however, the particle sizes increased considerably (500-600 nm). Finally, the SEM micrographs of the samples which showed the most intensive emission Mg 3 /Al 0.99 Eu 0.01 -tartrate and Mg 3 /Al 0.99 Eu 0.01 -benzoate are presented in Figure 11. Evidently, the surface microstructure of these two samples is almost identical. The hexagonally shaped particles with the size of~450-500 nm have formed.

Conclusions
Mg 3 /Al-CO 3 and Mg 3 /Al 0.99 Eu 0.01 LDHs intercalated with benzoate, oxalate, laurate, malonate, succinate, tartrate, 1,3,5-benzentricarboxylate (BTC), 4-methylbenzoate (MB), 4-dimethylaminobenzoate (DMB) and 4-biphenylacetonate (BPhAc) were prepared by sol-gel processing. The XRD analysis results clearly showed that the positions of diffraction peaks (003) of LDHs intercalated with anions were shifted to smaller 2θ angle values. However, the shift of the diffraction lines in the XRD patterns of intercalated with different organic anions of Eu 3+ -substituted LDHs was less pronounced in comparison with the samples without europium. The FT-IR results demonstrated once again the formation of the inorganic-organic hybrids and interaction of the organic ions with the LDH layers. The obtained results let us to conclude that depending on the size of anions these species could have specific vertical or horizontal orientations in the LDH structure. The microstructure of Mg 3 /Al-CO 3 , Mg 3 /Al 0.99 Eu 0.01 -CO 3 and Mg 3 /Al 0.99 Eu 0.01 -organic anion was typical for LDH samples. The SEM images showed the formation of hexagonally shaped plate-like particles of LDHs of 200-600 nm in size with high degree of agglomeration. The room temperature luminescence of Mg 3 /Al 0.99 Eu 0.01 and Mg 3 /Al 0.99 Eu 0.01 samples intercalated with benzoate, oxalate, laurate, malonate, succinate, tartrate, 1,3,5-benzentricarboxylate (BTC), 4-methylbenzoate (MB), 4-dimethylaminobenzoate (DMB) and 4-biphenylacetonate (BPhAc) anions under excitation at 394 nm was investigated. In all spectra, the typical four emission bands due to transitions of 5 D 0 → 7 F 1 (590 nm), 5 D 0 → 7 F 2 (613 nm), 5 D 0 → 7 F 3 (650 nm) and 5 D 0 → 7 F 4 (697 nm) of Eu 3+ ion were determined. The Mg 3 /Al 0.99 Eu 0.01 -tartrate and Mg 3 /Al 0.99 Eu 0.01 -benzoate LDHs showed the highest emission intensity to compare with LDHs containing other organic ligands.