ABSTRACT

The synthesis of a novel Li⁺ /Mg²⁺ /Al³⁺ containing layered double hydroxide (LDH) by using a hydrothermal synthesis route is represented in this work. The autoclaves were heated up to 100˚C, 120˚C, 140˚C and 160˚C for 10 h and 48 h with a water to solid ratio (W/S) of 15:1. The physicochemical properties of the synthesized LDHs were investigated by X-ray powder diffraction (PXRD), fourier transform infrared spectroscopy (FTIR), thermo gravimetric and differential thermal analysis (TG-DTA), inductively coupled plasma optical emission spectroscopy (ICP-OES) and scanning electron microscopy (SEM). The formation of a solid solution phase depends strongly on the composition of the reactants and the synthesis temperature. Using an exact stoichiometric ratio of Li⁺/Mg²⁺/Al³⁺ resulted in the synthesis of amorphous phases without producing plenty of crystalline amounts of the expected solid solutions while using higher temperatures than 140˚C resulted in a formation of AlO(OH). To avoid the formation of an Al containing amorphous phase or an AlO(OH) crystalline phase, the stoichiometric ratio of Li⁺ was changed. The results show solid solutions with the formula [Li_0+xMg_2−2xAl_1+x(OH)₆] [Cl·mH₂O] with X ≥ 0.9. The lattice parameters and chemical compositions for solid solutions with different compositions were determined and the pure solid solution with the highest amount of Mg (x = 0.9) is [Li_0.9Mg_0.2Al_1.9(OH)₆] [Cl∙0.50H₂O] with the lattice parameters a = 5.1004(4) Å, c = 15.3512(1) Å, V = 345.844(9) ų. For X < 0.9 two separate phases, a Mg²⁺ and a Li⁺ dominated solid solution, are coexistent.

Keywords:

Lithium LDH, Magnesium LDH, Solid Solution, X-Ray Powder Diffraction

1. Introduction

Layered double hydroxides (LDHs) consist of alternate positively charged mixed metal hydroxide layers and negative charged interlayer anions. The stoichiometry of these materials can be formulated as [M^z+_1−xM³⁺_x(OH)₂]^p+[(Aⁿ⁻)_p/n·mH₂O] with z = 2, M = bi- and trivalent metallic elements, A = organic or inorganic anions and m = amount of interlayer H₂O depending on the temperature, relative humidity and hydration level [1] . A special case is M^z+ = Li⁺(z = 1) and M³⁺ = Al³⁺. The ratio between Li and Al is always 1:2 [2] while the ratio between M^z+ and M³⁺ (z = 2) can vary strongly [3] depending on which M²⁺ ion or synthesis parameters are used. These layered materials are able to intercalate negatively charged and neutral molecules or exchange the interlayer anion with organic [4] [5] [6] [7] [8] or inorganic [3] [9] anions of different sizes or charges. The [M^z+_1−xM³⁺_x(OH)₂]^p+ main layer remains stable and is not capable of ion exchange once it is formed.

Two well-known and described LDHs are [LiAl₂(OH)₆] [Cl∙mH₂O] [2] [9] [10] and [Mg₂Al(OH)₆] [Cl∙mH₂O] [11]. Both compounds are generally synthesized by a direct reaction of a LiXor MgX₂(X = Cl⁻, OH⁻, NO₃⁻, etc) with Al(OH)₃[2/4]or by a hydrothermal reaction with higher temperatures and pressures [1] .

The structure of Al(OH)₃is built up of double layered sheets of hexagonally packed O atoms. Two thirds of the octahedral holes are occupied by Al atoms. Using LiX as the reaction partner leads to the formation of [LiAl₂(OH)₆] [X·mH₂O] with Li⁺ cations entering the vacancies in the aluminum hydroxide layers and A entering the interlayer space [1] [9] . The structure of the resulting Li-LDH depends directly on the structure of the used aluminium hydroxide. Syntheses using gibbsite as starting material leads to Li-LDHs with hexagonal symmetry, while reactions with bayerite or nordstrandite produce LDHs with rhombohedra symmetry [1] [10] [12] . In the brucite-like structure of [Mg₂Al(OH)₆][X·mH₂O], Mg²⁺ is octahedrally coordinated to six OH⁻ anions. These octahedrons share edges and form thereby a layer. Substituting Mg²⁺ with a trivalent ion like Al³⁺ leads to a positive charge which can be compensate by interlayer anions [11] . [Mg₂Al(OH)₆][X·mH₂O] can also be rhombohedra or hexagonal [13] [14] . The pure [Mg₂Al(OH)₆] [X·mH₂O] phase produced within this work was hexagonal (P6/m).

Almost all publications concerning the interlayer anion exchange or the synthesis and physicochemical properties use a combination of M^z+ (z = 1 or 2) + M³⁺ in the main layer with a variation of two different elements [3] [5] [15] - [20] . The aim of this research is to invent a novel solid solution by adding a Me²⁺ cation (Mg²⁺) into the structure of a Li-LDH. The distance between Li⁺ and O²⁻ ions in a [LiAl₂(OH)₆] [Cl·mH₂O] LDH is 2.129Å and between Al³⁺ and O²⁻ 1.926Å [2] . In a [Mg₂Al(OH)₆][Cl·mH₂O] LDH, Mg²⁺ and Al³⁺ ions occupy the same positions with the same distance of 2.013Åbetween the cations and O²⁻ [21] . Comparing both structures and the bonding distances, it should be possible for Mg²⁺ ions to occupy the Al³⁺ and the Li⁺ position in the solid solution.

2. Experimental

2.1. Reagents

The starting materials for this work were LiCl (ROTH, purity ≥ 99%), MgCl₂・6H₂O (AppliChem ≥ 99%), AlCl₃・6H₂O (Serva ≥ 98%) and NaOH (Fluka ≥ 97%). XRD investigations and loss of ignition (LOI) were done with all chemicals to exclude contaminations and determine the amount of crystal water.

2.2. Measurements

APAN anlytical X’PERT³ Powder diffractometer with Pixcel detector and a Cu radiation (45 kV/40 mA) was used for the X-ray powder diffraction (XRD). The samples were prepared with back loading procedure and recorded from 5˚ - 70˚2θ with a step width of 0.017˚2θ and a irradiation time per step of 19.685 s. Thermogravimetric analysis and differential thermal analysis (TGA/DTA) for the dried samples (relative humidity (RH) 35%) were done simultaneously by the 320U from Seiko Instruments under nitrogen flow and a 2.5 K/min heating rate between 25˚C - 1000˚C. Fourier transform infrared spectra (FTIR) were recorded by an IFS 55 Equinox FTIR spectrometer from Bruker (400 - 4000 cm⁻¹). The scanning electron microscope (SEM) pictures were taken by a JOEL 640 SEM and the chemical compositions of the samples were proven by a Horiba Ultima2 inductively coupled plasma optical emission spectroscopy (ICP-OES).

2.3. Synthesis

All mixtures of the initial components were prepared in a glove box with nitrogen atmosphere to avoid carbonatization. The synthesis were carried out in 35 ml PTFE-lined stainless-stealautoclaves [1] by adding solutions of LiCl, MgCl₂∙6H₂O and AlCl₃·6H₂Owith a W/S of 15: 1(a total of 1 g salts with 15 ml deionized/ decarbonized water) and 5M NaOH until an alkaline pH (8.5) was reached and heating it up 10 h and 48 h. A series of experiments with different temperatures, synthesis times and pH were carried out to achieve the best result for a pure solid solution. The synthesis temperature was varied between 100˚C, 120˚C, 140˚C and 160˚C and two different synthesis times (10 h and 48 h) and pH (8.5/9.5) were tested. To synthesize pure [Mg₂Al(OH)₆][Cl·mH₂O] an exact ratio of 2 mol Mg²⁺: 1 mol Al³⁺was chosen andthe pure [LiAl₂(OH)₆][Cl·mH₂O] was prepared by adding the Li⁺ and Al³⁺ salts in an exact 1 mol : 2 mol ratio. While the Mg containing LDH was prepared without problems, the Li LDH showed a high proportion of an amorphous phase. ICP-OES investigations stated that only 20% of Li⁺ was incorporated in the LDH structure leaving 80% of Li⁺ in the solution and the so remaining excess of Al³⁺ as an amorphous phase. A five times higher concentration of Li⁺ [10] , as required by stoichiometry for the preparation of the pure [LiAl₂(OH)₆][Cl·mH₂O] LDH, was necessary to compensate the 80 % lack of Li⁺ in the solid state.

After the synthesis of pure [Mg₂Al(OH)₆][Cl·mH₂O], the amount of Li⁺ was increased and the amount of Mg²⁺ was reduced in 10 mol% (X = 0.1) steps until 100 mol% Li ([LiAl₂(OH)₆][Cl·mH₂O]) was reached. The products were filtered, washed with 30 ml deionized water and dried (RH 35%) until a constant mass was reached.

The mineralogical phases were determined by X-ray powder diffraction, the chemical compositions of the products by ICP-OES using the filtrate and the synthesis products dissolved in HNO₃ [11] [16] .

3. Results and Discussion

3.1. Stoichiometric Composition

First experiments were carried out at 100˚C, pH 8.5, 10 h synthesis time and a W/S ratio of 15:1. Using an exact stoichiometric ratio of Li⁺/Mg²⁺/Al³⁺ resulted in the synthesis of a high proportion of an amorphous phase with a small amount of a crystalline solid solution. After drying at 80˚C, XRD analysis showed a recrystallized Al(OH)₃ phase next to the LDH main phase.

Investigations of the filtered solutions and the dissolved products with ICP-OES stated that, independent from the Mg reactant amount, 99% - 100% of Mg²⁺ but only 20% of Li⁺ were build-in into a LDH phase. The other 80% of Li⁺ remained in the solution. Due to the stoichiometric reactant ratio the leftover Li⁺ ions in the solution are leading to leftover Al³⁺. These Al³⁺ ions formed Al(OH)₃ in the basic environment. Using higher temperatures (up to 160˚C) or synthesis times (48 h) showed no positive effect for the crystallization of a pure LDH phase. Increasing pH from 8.5 to 9.5 resulted in a slightly higher amount of a crystalline phase.

3.2. Composition with Increased Li⁺ Content

After a five times increasement of the stoichiometric amount of Li⁺ (equal to the pure Li-LDH synthesis), with a resulting ratio of Li: Mg: Al = 5: 1: 1, a pure crystalline LDH phase could be achieved. ICP-OES studies stated that >99% of Mg²⁺ and Al³⁺ and the needed 20 % of the five times higher Li⁺ concentration were build-in into the crystalline phase.

3.2.1. PXRD Analysis

By increasing X from 0 to 1 in 0.1 mol steps in [Li_0+xMg_2−2xAl_1+x(OH)₆][Cl∙mH₂O], the amount of Mg²⁺is decreased and replaced by Al³⁺ and Li⁺. This leads to a change of the lattice parameter a and the cell volume. Comparing the ion radii of Mg²⁺ (0.65 Å) with Li⁺ (0.60 Å) and Al³⁺ (0.50 Å) it is to be expected that the lattice parameter a starts to decrease with higher Li⁺/Al³⁺content [7] . A dependent change in the lattice parameter c or the basal reflections (00l) is not visible. By means of the (110)/(112) and (300)/(302) peaks, it is easily possible to distinguish the two different phases [Mg₂Al(OH)₆][Cl·mH₂O] (P6/m) and [LiAl₂(OH)₆][Cl·mH₂O] (P6₃/m). Starting with X = 0 (pure [Mg₂Al(OH)₆][Cl·mH₂O] phase) a separation in two phases is visible between X = 0.1 and X = 0.8 (Figure 1 and Figure 2). The ˚2Θ positions of the 110/112peaks at X = 0.1 - 0.8 show a peak shift to higher ˚2Θ angles in relation to the pure [Mg₂Al(OH)₆][Cl·mH₂O]

phase (Figure 2 and Figure 3) which is also visible in the lattice parameter (Table 1). This shift increases with higher Li⁺ reactant amounts, which indicates Mg dominated solid solutions with different Li⁺/Mg²⁺ ratios.

While the (110)/(112) peaks are completely erased for X = 0.9, the (300)/(302) peaks shifted and the solid solution hasa different lattice parameter compared to [LiAl₂(OH)₆][Cl·mH₂O] at X = 1 [2] (Figure 2 and Figure 3, Table 1). The lattice parameter a is closeto the calculated ideal position of a solid solution. Between X = 0.1 - 0.8 the (300)/(302) peaks have nearly the same position which is shifted to lower ˚2Θ angles and the lattice parameter are also nearly constant. This indicates a stable Li dominated solid solution with a defined amount of

Mg²⁺ independent from the Mg²⁺ reactant amount. The miscibility gap for X = 0.1 - 0.8 was observed at all tested synthesis temperatures (100˚C - 160˚C) and times (10 h/48 h).

To synthesize pure solid solution phases, test series between X = 0.9 and X = 1 (in 0.02 mol steps) were conducted. XRD results show a single mineral phase with h0l peak shifts (Figure 4 and Figure 5). This peak shifts follow nearly the

calculated shifts for the solid solutions (Figure 6). These experiments were also done at four different temperatures (100˚C, 120˚C, 140˚C, 160˚C). Although there is a shift difference depending on the temperature (Figure 6), no phase separation was observed for all investigated solid solutions (Figure 5).

The optimal results for a pure solid solution phase were achieved at 120˚C/10 h synthesis time/pH 9.5 and W/S ratio 15:1 (Figure 6/Table 2). The measured lattice parameters a differ only slightly from the calculated and the lattice parameters c are nearly constant (Table 2).

The products were fitted by Pawley fit and the space group was determined as P6₃/m for all pure solid solutions up to X = 0.9. Investigations of the lattice parameter a show a straight increase from ~5.08Å (X = 0) [8] to ~5.10Å (X = 0.1) as calculated (Figure 6/Table 2).

3.2.2. ICP-OES Analysis

To determine the chemical formula, all products were completely dissolved insuprapur 65% nitric acid and investigated with ICP-OES [11] [16] . The results were used to calculatethe LDH formulas (Table 4). These calculations also stated a maximum content of an amorphous phase of <1%. Recrystallization tests showed no Al containing phases. Synthesis temperatures higher than 140˚C led to a destabilization of the LDH phase and the formation of AlO(OH) (Figure 7). The test series with 160˚C were repeated several times producing always AlO(OH) next to the LDH. Calculations showed an Al containing amorphous phase and crystalline AlO(OH) proportion of 10 % to 90 % (Table 3). The resulting lack of Al³⁺ in the solid solution leads to LDH phases with a higher Mg/Al ratio than 2:1 and therefore to the formation of a LDH with higher Mg²⁺ amounts next to the AlO(OH) phase (Figure 6(d)).

3.2.3. Thermal Analysis

The amount of interlayer water was determined by TG/DTA for [LiAl₂(OH)₆] [Cl·0.50H₂O], [Mg₂Al(OH)₆][Cl·0.55H₂O]and all pure solid solutions (Table 4). An example for the Li-LDH, Mg-LDH and the solid solution with the highest Mg²⁺ amount [Li_0.9Mg_0.2Al_1.90(OH)₆][Cl·0.51H₂O] is shown in Figure 8. Comparing the solid solution with the pure Li- and Mg-LDH, there is a high similarity in mass loss and exothermal reaction. The mass loss at 75˚C - 100˚C is caused by the removal of intercalated interlayer water [2] [6] . With 4.5% for the pure Li-LDH, 4.2% for the solid solution and 4.7% for the pure Mg-LDH it corresponds with the loss of 0.50 to 0.55 water per formula unit of the LDHs. While the differential thermal analysis of the pure Li- and Mg-LDH show a single endothermic reaction at 275˚C - 325˚C, the solid solution shows two (260˚C and 320˚C). At this temperature, the LDH starts to dehydroxylate which results in the destruction of the metal hydroxide main layer [2] [6] [7] [11] . Combining Li⁺ and Mg²⁺ with Al³⁺ in the main layer leads to a two-step dehydroxylation.

3.2.4. FTIR Spectroscopy

To prove purity of the products, all samples were investigated by FTIR spectroscopy (Figure 9). Although there are 10 mol% Mg²⁺ in the solid solution, there is only a slight difference to a pure [LiAl₂(OH)₆][Cl·0.51H₂O] FTIR spectrum visible. All three spectra show the typical H₂O/OH⁻ absorption at ~3500 cm⁻¹ and 1630 cm⁻¹ [5] [18] [22] and only the spectra of [Li_0.9Mg_0.2Al_1.90(OH)₆] [Cl・0.50H₂O] and [Mg₂Al(OH)₆][Cl・0.55H₂O] show an insignificant amount of carbonatization with the absorption at 1380 cm⁻¹ [5] [18] [23] . The absorption of Al (980/720/520 cm⁻¹) related groups is very good visible for the pure Li-LDH but not as distinct for the solid solution [11] [24] . Mg related absorptions at 415 cm⁻¹ are only visible in the pure Mg-LDH (Table 5). The amount of Mg²⁺ is high enough to influence the absorption spectra but not to show a clear Mg related absorption.

3.2.5. SEM Analysis

SEM pictures (Figure 10) show flat, (pseudo-) hexagonal particles with different sizes, starting at 2 - 3 µm until nearly nanosize. These particles form cluster in the size of 200 - 600 µm.

3.2.6. Structure of the Solid Solution

Based on the assumption that Mg²⁺ ions can occupy the positions of Li⁺ and Al³⁺ because of the fitting bonding length [2] [21] , the ion radii [7] and the determined hexagonal P6₃/m space group, the structure of the pure phased solid solution should be identical with the Li-LDH (Figure 11). This is also indicated by the chemical composition with the formula [Li_0.9Mg_0.2Al_1.90(OH)₆][Cl・0.50H₂O]. If Mg²⁺ ions could not enter one of the two octahedral positions, there would be two possibilities: they would exchange with Li⁺ ions only, which would reduce the amount of Li⁺ in the solid solution while the amount of Al³⁺ would not change, or they would exchange only with Al³⁺ ions with the opposite result. The results of this work show, that in fact Mg²⁺ has to be statistically distributed with 5 mol% on the Li⁺ and 5 mol% on the Al³⁺ position to provide the measured chemical formula.

4. Conclusion

It is possible to synthesise a pure [Li_0+xMg_2−2xAl_1+x(OH)₆][Cl·mH₂O] solid solution using autoclaves with temperatures of 100˚C, 120˚C and 140˚C with a maxi- mum amount of 10 mol% Mg²⁺ (X = 0.9). Using more Mg²⁺ in the reactant leads to a parallel formation of an Mg²⁺ dominated and a Li⁺ dominated solid solution. Optimal results for a pure solid solution can be achieved at 120˚C, pH 9.5, W/S15: 1, 10 h synthesis time. Changing the temperature to 160˚C provides the formation of an AlO(OH) phase. The pure solid solution with the highest Mg content is [Li_0.9Mg_0.2Al_1.9(OH)₆][Cl·0.50H₂O].

Cite this paper

Niksch, A. Pöllmann, H. (2017) Synthesis and Characterization of a [Li_0+xMg_2−2xAl_1+x(OH)₆][Cl∙mH₂O] Solid So- lution with X = 0 - 1 at Different Temperatures. Natural Resources, 8, 445-459. https://doi.org/10.4236/nr.2017.86029

References