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Review

Spodumene: The Lithium Market, Resources and Processes

by
Colin Dessemond
1,
Francis Lajoie-Leroux
1,
Gervais Soucy
1,*,
Nicolas Laroche
2 and
Jean-François Magnan
2
1
Département de génie chimique et de génie biotechnologique, Université de Sherbrooke, Sherbrooke, QC J1K 2R1, Canada
2
Nemaska Lithium Inc., Quebec, QC G1K 3X2, Canada
*
Author to whom correspondence should be addressed.
Minerals 2019, 9(6), 334; https://doi.org/10.3390/min9060334
Submission received: 17 April 2019 / Revised: 16 May 2019 / Accepted: 24 May 2019 / Published: 29 May 2019
(This article belongs to the Special Issue Towards Sustainability in Extractive Metallurgy)
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Abstract

:
This literature review gives an overview of the lithium industry, including the lithium market, global resources, and processes of lithium compounds production. It focuses on the production of lithium compounds from spodumene minerals. Spodumene is one of the most critical minerals nowadays, due to its high lithium content and high rate of extraction. Lithium is one of the most sought-after metals, due to the ever-growing demand for lithium-ion batteries (LiBs). The data on lithium extraction from minerals is scattered through years of patents, journal articles, and proceedings; hence, requiring an in-depth review, including the comprehension of the spodumene phase system, the phase conversion processes, and the lithium extraction processes.

1. Introduction

Lithium is the third element of the periodic table. It is the lightest of all solid elements (d = 0.53 g∙cm−3 at 20 °C), has the highest specific heat capacity, the smallest ionic radius of all the alkali metals, and a high electrochemical potential [1]. Its two stable isotopes are 6Li and 7Li, with 7Li being the most abundant (92.5%) [2,3]. Several radioisotopes have been observed, such as 3Li, 4Li, 5Li, 8Li, 9Li, 10Li, 11Li, 12Li, 13Li [4], with 8Li and 9Li being the most stable, with a half-life of, respectively, 838 ms and 178 ms [5]. Lithium also contradicts the Big Bang Nucleosynthesis theory, which predicts the abundance of D, 3He, 4He, and 7Li in the universe [6,7,8], with observed rates three times lower than predicted. This contradiction has apparently been solved [9].
Lithium is one of the most critical metals in modern industry. Its usages range from pharmacy with lithium-based bipolar disorder treatment drugs to aeronautics with light aluminum/lithium alloys. The most important usage nowadays is Lithium-ion Batteries (LiBs). The lithium production was, until recently, dominated by the salt lake brines, because of their cheaper production cost. The ever-growing demand in lithium compounds led to the regaining of interest for another source, after the lithium price increased. This other source, lithium rich minerals, now account for 50% of the world’s lithium production [10]. Lithium minerals are numerous and include spodumene, eucryptite, petalite, bikitaite, etc. [11]. Lithium reserves estimations have significantly changed over the years, due to continuous exploration. Estimations have ranged from 16.7 Mt Li in minerals for a total of 43,6 Mt Li including the brines [12] to 14 Mt Li in minerals for a total of 62 Mt Li identified resources [13]. Among those minerals, spodumene LiAlSi2O6 is the most common and the most studied. It offers a theoretical Li2O content of 8 wt %, whereas raw minerals in nature typically offer 1 to 2 wt % Li2O with some notable exceptions such as Greenbushes, Australia which offers a high rate of 1,44 wt % Li (3.10 wt % Li2O) [14]. This review will offer an overview of the lithium market, the sources of lithium, and the production processes, and will then focus on the chemical system of the spodumene, of the conversion methods and finally the extraction methods.

2. Lithium Usage and Resources

2.1. Usage

Lithium usages are wide. They range from glass and ceramics to pharmacy (Figure 1). Glass and ceramics were the main usage of lithium up to 2005 [15]. Since this date, Lithium ion Batteries (LiBs) have taken over, since they play a major role in the development of the electronic and green industries.
Among those uses, LiBs show the highest growth rate and are expected to take an even bigger part in the lithium industry (Figure 2). The expected growth rate for lithium carbonate and lithium hydroxide is respectively 10% and 14.5% until 2025 [17], since they are two of the raw materials used for LiBs. In 2016, lithium carbonate prices were reported to range from 10,000 US$ to 16,000 US$ while lithium hydroxide prices were reported to range from 14,000 US$ to 20,000 US$ [18].
When it comes to ceramics, lithium is used in its mineral forms, such as spodumene, to give economic and environmental benefits by reducing the melting temperature. Concerning the LiBs, lithium is used to manufacture cathodes, anodes, and electrolytes alike. Lithium greases are used for their excellent temperature properties (they are stable at a high temperature and do not solidify at a low temperature). Lithium bromide solutions play an important role in air treatment, and lithium hydroxide is used as CO2 scrubbers in space shuttles and submarines.

2.2. Resources

The resources of lithium are primarily divided into three categories. The first are brines. They are, by far, the main source of lithium with more than 60% of the global identified reserves [12]. Among the brines, the salars, which are dried salt lakes, hold 78% of the lithium brine reserves. The second source, by amount of lithium available, is pegmatites. Recent estimations evaluate pegmatites as 23% to 30% of the lithium identified reserves [13]. Lithium-rich pegmatites, despite being one of the main sources of lithium worldwide, are very rare in comparison to pegmatites as a whole [20], forming less than 0.1% of the family.
The lithium minerals containing lithium inside those pegmatites are numerous and their lithium content varies greatly (Table 1).
The third source represents less than 3% of the global lithium resources. They are made of Sediment-Hosted Deposits. They are made of hectorite deposits and jadarite deposits. So far, two hectorite deposits are known, which are in McDermitt, United States and Sonora, Mexico. Only one jadarite deposit has been discovered in Jadar, Serbia. The main producers of lithium from minerals are Australia (40 kt Li), Chile (14.2 kt Li), China (6.8 kt Li), and Argentina (5.7 kt Li) for a global production of 69 kt Li. The biggest reserves (minerals only) are located in Chile (8 Mt Li), Australia (2.7 Mt Li), Argentina (2 Mt Li), and China (1 Mt Li). Other countries have a significant amount of identified reserves, which have yet to be categorized. An example of such a country is Canada, which has an identified reserve of 2 Mt Li [13]. The consumption of lithium by the electrical vehicle (EVs) industry is expected to reach 565 kt LCE (Lithium Carbonate Equivalent) or 106 kt Li by 2027 [21]. This would mean that minerals could provide the EVs industry for more than 130 years at maximum consumption (not accounting for the other lithium applications).

3. The Different Spodumene Phases

3.1. The Pegmatite Formation

Pegmatite is the name of a large family, which includes lithium aluminosilicates, among others. Pegmatites are divided between granitic and non-granitic pegmatites [22]. Spodumene is a granitic pegmatite [23,24,25]. Being very different in their nature, pegmatites forming a pluton are called a group.
Groups of pegmatite have a common granitic source, but differ from each other due to the nature of the source, depth, etc. [26,27]. In a perfect case, a group of pegmatite follows a regionally layered structure (Figure 3).
In the case of spodumene, a relation between its phases and other lithium aluminosilicates, such as eucryptite or petalite, exists in a quartz-saturated environment (Figure 4). This relationship between α- spodumene, β-spodumene and γ-spodumene (virgilite) shows that the crystallization of the minerals must have occurred under about 700 °C since β-spodumene does not occur naturally and virgilite is very rare and mostly found as inclusions [29].

3.2. The α, β, γ System

Spodumene is an aluminosilicate of lithium. It has been described for the first time in 1800 for an occurrence in Üto, Sweden [31]. Its name is derived from ancient Greek spodumenos, which means “burnt to ashes”, due to its grey ash-like color when grinded. Its color ranges from green to purple. Spodumene can produce two kinds of gems, hiddenite (green), and kunzite (purple) [32]. The mineral is mostly associated with quartz and albite, with sometimes traces of beryl [33]. Geologists only call it spodumene. However, in the lithium industry, the mined natural material is referred to as α-spodumene. Its chemical formula is LiAlSi2O6 and it has a monoclinic structure and a density of 3.184 g∙cm−3. Its aspect and X-Ray pattern are presented below (Figure 5 and Figure 6).
The second phase is called β-spodumene or spodumene-II. It is the most known phase of the system, due to its reactivity towards extraction. It is obtained after high temperature treatment of α-spodumene and is the base mineral of almost every lithium extraction processes. It has a tetragonal structure [34,35] and a density of 2.374 g∙cm−3. It has the particularity to be present in the Li2O–Al2O3–SiO2 ternary equilibrium system. Therefore, it is possible to synthesize it directly into this form following, for example, the LiAlO2 + Al6Si2O13 = 3Al2O3 + β-LiAlSi2O6 reaction [36].
The third phase is less known and has several different names. It is referred to as virgilite, γ-spodumene or spodumene-III [37,38]. It has a hexagonal structure and a density of 2.399 g∙cm−3. The formation of a pure γ-spodumene sample has not been reported yet. Given that γ-spodumene is never pure, the aspects and X-Ray patterns of β-spodumene and γ-spodumene are presented together below (Figure 7, Figure 8 and Figure 9). As seen on the X-Ray patterns, β-spodumene and γ-spodumene share the same angle for their main peak. Moreover, γ-spodumene’s peaks are fewer in number and lower in intensity, making it difficult to identify γ-spodumene in a sample.
The space groups and crystallographic data of the three phases are listed in the table below (Table 2 and Figure 9).
The thermodynamic data of the three phases have been measured and are listed below (Table 3).
When it comes to the Cp of the three phases, their relations to temperature have been calculated [40].
  • α-spodumene:
    C p ( T ) = 354.715 − 3375.72   T − 0.5   J . m o l − 1 . K − 1
  • β-spodumene and γ-spodumene:
    C p ( T ) = 362.8 − 0.003684   T − 3435.0   T − 0.5   J . m o l − 1 . K − 1
The phase transitions occur during the thermal treatment via a phenomenon called decrepitation. The latter is an expansion of the crystal lattice of the compound after reaching a determined temperature. The α-spodumene to β-spodumene transition occurs above 950 °C [42] and is endothermic [43]. The crystal lattice expands massively (27%) during the phase transition [44]. The γ-spodumene is known to appear before the β-spodumene [37] but is metastable and transitions to β-spodumene at higher temperatures.
The transitions existing within the spodumene system can be summarized as follows (Figure 10). Every single transition is irreversible.

3.3. General Flow Sheets

The lithium compounds production from minerals follows a simple succession of steps. Every raw mineral has to be grinded before being cleaned. A heat treatment is then applied before roasting. The process allows the recovery of lithium but not the production of technical lithium hydroxide of lithium carbonate. Another step, such as carbonation or electrodialysis is needed (Figure 11).
Concerning the lithium production from brines, the process revolves around concentrating the brines up to 6 wt% Li and removing the impurities one after the other (Figure 12). There has been research on the efficiency of lithium extraction, both ancient and novel. For example, fluorinated β-diketones have been investigated to separate lithium from sodium, potassium, rubidium, and caesium, due to their poor selectivity for lithium [46]. More recently, N-butyl pyridinium bis[(trifluoromethyl)sulfonyl]imide solution was found to have a high efficiency for lithium extraction from brines [47]. Other processes involving, for example, LiAl-layered double hydroxides as lithium-ion-selective capturing material, were proven to have lithium yields over 96% [48].

4. Production of Lithium from Spodumene

4.1. The Traditional Process

When it comes to the actual phase conversion of spodumene, the process has been known since the 1950s. The process has been patented [49] and, still nowadays, heavily dominates the lithium production industry. This process starts with the crushing of spodumene ore. The cause behind the grinding of the spodumene is an acceleration of the heat transfer between the surrounding atmosphere and the mineral. The crushed mineral is then heated in a furnace at, at least, 1000 °C for 30 min. It is stated that almost any kind of furnace will do for this part of the process. The thermal treatment will allow the α-spodumene to decrepitate into β-spodumene. However, nowhere in this process is it stated that γ-spodumene exists. Therefore, the data concerning the spodumene phase transitions is not complete. This process is stated to be exclusive to spodumene. The other lithium-bearing minerals being impossible to decrepitate using this method. It was the first process to efficiently extract lithium from spodumene (85% to 90% lithium yield at the time) and was scaled up shortly after [50]. The lithium extraction went from total digestion of minerals such as lepidolite (K(Li,Al)3(Si,Al)4O10(F,OH)2) or amblygonite ((Li,Na)AlPO4(F,OH)) followed by complex purification to selective extraction of lithium.
The process is based on the higher reactivity of β-spodumene towards sulphuric acid. The acid is brought into contact with the β-spodumene and heated at about 250 °C. It is reported that the temperature can go as low as 200 °C but cannot reach higher than 300 °C, temperature at which the sulphuric acid starts to decompose. The acid excess must be at least 30% to ensure the availability of the protons after reactions with impurities such as potassium or sodium. Depending on the grade of the ore, acid excess can go up to 140%. The reaction between the sulphuric acid and the spodumene is presented below.
2   L i A l S i 2 O 6   ( s ) +   H 2 S O 4   ( l )   → 2   H A l S i 2 O 6   ( s ) + L i 2 S O 4 ( s )
After reaction between the acid and the concentrate, the lithium sulphate is leached by water in which it dissolved while leaving the leached concentrate in its solid state. The lithium sulphate can thereafter be precipitated as is, or transformed into lithium chloride or lithium carbonate.
The authors of this patent have come to three statements, all of them being in favor of a diffusion mechanism allowing the protons to diffuse through the β-spodumene to allow the cationic exchange.
  • α-spodumene is almost completely resilient toward acid roasting contrary to β-spodumene
  • β-spodumene density is significantly lower than that of α-spodumene.
  • The structure of the leached β-spodumene is very similar to that of β-spodumene.
Hence, β-spodumene has a more open structure. This structure would allow the diffusion of ions through its matrix via a pseudo-Brownian movement. This statement was later confirmed by crystallographic studies [51] which confirmed that the structure of β-spodumene presents pseudo-zeolithic channels in which protons and lithium cations are free to move. The aluminosilicate portion of β-spodumene is in fact isostructural to keatite, which presents those channels. An important heat production is observed during the acid roasting around 175 °C. This exothermic reaction is linked to the formation of liquid lithium bisulfate (LiHSO4) as a reaction intermediate [52,53] since it has a melting point of around 170 °C.
This process was so efficient and easy to implement that it has been considered the one and only method of extracting lithium from spodumene in the lithium industry. From there, two major steps can be pointed out. The first one is the lithium extraction from β-spodumene and the second is the decrepitation of α-spodumene.

4.2. Other Processes of Extracting Lithium from Spodumene

The lithium extraction from β-spodumene has always been considered the critical step of the overhaul process and the one where major improvements on the lithium yield could be made. Therefore, this step has been heavily researched and still is nowadays. From the middle of the 20th century until the late 1960s, several processes concerning the extraction of lithium from spodumene have been patented. Those patents are listed below (Table 4). Only the processes involving H2SO4 (l), or a mixture of CaCO3 (s) + CaSO4 (s), have been commercially exploited, the others having been dismissed due to low lithium yield, high temperature or long duration.
Despite the domination of the traditional process [49], some research on alternative processes have been published (Table 5). None of those new processes has been commercially exploited, mainly because of the reticence of the companies to deviate from the long-established process.
A few things can be pointed out when it comes to the extraction of lithium from spodumene. First, γ-spodumene is ignored or even not reported in those studies, which means that its reactivity towards reagents is unknown. Therefore, its influence on the lithium yields is unknown. Second, there is no consistency concerning the granulometry of the samples used. Therefore, the influence of granulometry on the lithium yield cannot be evaluated. Those should not be underestimated because of the high cost related to communition [75] and the wasteful nature of communition [76]. Last, there is no consistency about the decrepitation temperature, while this temperature is known to have an effect on spodumene conversion and thus on lithium extraction.
When it comes to the impurities of spodumene and their influence on lithium extraction, research is scarce. However, it was pointed out that impurities were leached at rates independent of leaching conditions [77]. On the other hand, it was found out that quartz particles could protect β-spodumene particles from the sulphuric acid by coating them (Figure 13).

4.3. Conversion Processes of Spodumene

As stated in Section 3.2, the critical step of the process has always been considered to be the extraction step. Since the beginning of the selective extraction of lithium, decrepitation has been considered a minor step of the process where only minor improvements could be made. Hence, there is very little data on the behavior of spodumene with regards to the granulometry of the sample, the temperature of decrepitation, etc. There has been very little research on how to improve the decrepitation step of spodumene, many considering that the furnace heating in a rotary kiln is optimized. An equation describing the conversion of spodumene was derived from the Avrami equation [78] and is presented below.
1 −   ω = e x p ( − K t )
Where ω is the converted spodumene, K the rate of conversion and t the treatment time. This equation was developed from the Avrami equation and is considered an approximation of the phase transition, since the kinetic model only considers one molecule. The results presented by this study suggest that above 950 °C, the phase transition is almost instantaneous. The downside is that it does not consider the γ-spodumene. A compilation of spodumene studies shows that the decrepitation temperature differs greatly between the samples [79], with temperatures ranging from 950 to 1050 °C. Moreover, it was found that the temperature range suitable for the decrepitation becomes narrower with the increasing amount of impurities [80]. This was further later confirmed using the Delmon theory. According to this theory, the activation energy of the spodumene conversion is 296 kJ/mol ± 6 kJ/mol and is independent of the rate of impurities. This value fits the results found from the Avrami equation between 950 and 1050 °C. It was then concluded that the temperature of conversion was indeed influenced by the amount of impurities in the spodumene [43].
Despite the general consensus that the traditional method of decrepitating spodumene is the best, there has recently been some research about alternative methods to the rotary kiln. One still uses traditional heating but emphasizes on the grinding of the spodumene beforehand. It is stated that grinding cleaves the Li–O, Al–O, and Si–O–Si bonds from the tetrahedral site. It shows that the α-spodumene turns into γ-spodumene between 700 and 900 °C before transitioning into β-spodumene between 900 and 950 °C [81]. This would mean a decrease in the energy necessary to decrepitate the spodumene but does not consider the amount of energy needed to grind the material. One of the few alternative processes uses microwaves to decrepitate spodumene ore. This study found that the critical temperature for α-spodumene to start absorbing microwaves is about 634 °C. But it also states that the temperature is not uniform, with measures ranging from 650 to 1250 °C depending on the area of measurement. A significant amount of β-spodumene melts using this method, while the intermediate layer is composed of β-spodumene and γ-spodumene and the top layer is still in α-form [82]. Hybrid microwaving has also been studied using SiC susceptor tubes. It can allow the decrepitation to occur, despite a higher temperature of 1197 °C. The upside of this method is a shorter treatment time of only 170 s [37]. It also shows that γ-spodumene is formed if the temperature is not high enough and that this method also melts the concentrate. When it comes to the melting of the samples, it has been reported that the behavior of a spodumene sample differs greatly based on the impurities in the sample and their quantity [83], with melting temperatures ranging from 1000 to 1400 °C. For example, the melting point of the spodumene can go down as low as 930 °C if the sample is made of 50/50 α-spodumene/(Quartz–Albite–Microcline 10–20–20) [84].
If the decrepitation of the spodumene was studied, the effect of the phenomena on the size of the particle is not mentioned. It has been proven that decrepitation was able to grind coarse particles (size ranging from 2 mm to 2 cm) into micrometric particles suitable for acid roasting. This study shows that heating a coarse spodumene concentrate at 1050 °C for 30 min decrepitates the α-spodumene into β-spodumene and γ-spodumene with 65% of the initial mass becoming smaller than 180 µm and that some impurities were not affected by the thermal treatment, making them easy to remove from the converted concentrate. This study was realized without prior grinding or flotation of the mineral and found out that the lithium in the finer fraction was being extracted at a 99% yield using the traditional method [85], meaning that the need for grinding and flotation could be reduced, thus saving time and energy.
As can be seen above, when it comes to research about the decrepitation of the spodumene, γ-spodumene is taken into account in the recent studies while this is not the case with lithium extraction and older decrepitation studies. This shows that despite the disappearance of α-spodumene, the conversion of spodumene does not give only β-spodumene. It could mean that the limitations may not have originated only from the sulphuric acid behavior toward β-spodumene but also from the behavior of γ-spodumene itself.

5. Conclusions

Lithium is one of the most sought after metals in the modern industry. Spodumene is one of the most important sources of lithium in minerals. Many lithium companies use spodumene as their primary source and transform it into lithium using a process that was first introduced in 1950 and little improved over the years. As seen in this review, the literature concerning the thermal treatment is not complete. While finding new processes to decrepitate spodumene may not be necessary, it would be necessary to include γ-spodumene in every work to research its influence on the whole process. The granulometry of the samples and their grade should be mentioned since this seems to have great influence over the behavior of spodumene and ultimately on lithium yield. On the contrary, the process of extraction in itself has been heavily studied to try to give reasons for the limitations of the traditional process. Alternatives to the sulphuric acid process have been studied but little to none have been commercially exploited due to the reticence of the companies to deviate from a reliable and relatively efficient process.

Author Contributions

Writing—original draft preparation, C.D.; writing—review and editing, G.S., F.L.-L., N.L., J.F.-M.; supervision, G.S.

Funding

The research was funded by Fonds de recherche Nature et technologies, grant number 2015-MI-192454 and by Nemaska Lithium inc. with a mandatory portion of funding requested by the government funder.

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Diagram of lithium usages [16] (adapted with permission from Elsevier, Resources Policy; published by Elsevier, 2019).
Figure 1. Diagram of lithium usages [16] (adapted with permission from Elsevier, Resources Policy; published by Elsevier, 2019).
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Figure 2. Diagram of lithium usage proportions [19].
Figure 2. Diagram of lithium usage proportions [19].
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Figure 3. Chemical evolution through a lithium-rich pegmatite group with distance from the granitic source [28] (adapted with permission from the Mineralogical Association of Canada, Granitic Pegmatites in Science and Industry; published by the Mineralogical Association of Canada, 2019).
Figure 3. Chemical evolution through a lithium-rich pegmatite group with distance from the granitic source [28] (adapted with permission from the Mineralogical Association of Canada, Granitic Pegmatites in Science and Industry; published by the Mineralogical Association of Canada, 2019).
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Figure 4. Stability relations among eucryptite (LiAlSiO4), α-spodumene (LiAlSi2O6), petalite (LiAlSi4O10), β-spodumene (LiAlSi5O12) and virgilite (LiAlSi5O12), in the system LiAlSiO4–SiO2–H2O [30] (adapted with permission from the Mineralogical Society of America, American Mineralogist; published by the Mineralogical Society of America, 2019).
Figure 4. Stability relations among eucryptite (LiAlSiO4), α-spodumene (LiAlSi2O6), petalite (LiAlSi4O10), β-spodumene (LiAlSi5O12) and virgilite (LiAlSi5O12), in the system LiAlSiO4–SiO2–H2O [30] (adapted with permission from the Mineralogical Society of America, American Mineralogist; published by the Mineralogical Society of America, 2019).
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Figure 5. (a) Macroscopic (Optical), (b) Microscopic (SEM) aspects of a typical α-spodumene sample.
Figure 5. (a) Macroscopic (Optical), (b) Microscopic (SEM) aspects of a typical α-spodumene sample.
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Figure 6. X-Ray pattern of a typical α-spodumene sample, only the main peaks of α-spodumene are indicated.
Figure 6. X-Ray pattern of a typical α-spodumene sample, only the main peaks of α-spodumene are indicated.
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Figure 7. (a) Macroscopic (Optical), (b) Microscopic (SEM) aspects of a typical β-spodumene sample (red-brown particles).
Figure 7. (a) Macroscopic (Optical), (b) Microscopic (SEM) aspects of a typical β-spodumene sample (red-brown particles).
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Figure 8. X-Ray pattern of a typical β-spodumene and γ-spodumene sample.
Figure 8. X-Ray pattern of a typical β-spodumene and γ-spodumene sample.
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Figure 9. Crystal structures of spodumene. (a) α-spodumene, (b) β-spodumene, (c) γ-spodumene. Red: Oxygen. Yellow: Silicon. Blue: Aluminum. Green: Lithium. Note: The lattices images were obtained with the display module of the Jade2010TM software. At a macroscopic level, α-spodumene appears as a very hard rock. It is compact and difficult to cut or grind while β-spodumene appears as a dusty material with a low resistance to grinding. At a microscopic level, α-spodumene appears as a compact material made out of multiple layers stacked on top of each other while β-spodumene presents many cracks on its particles, which make its structure more random.
Figure 9. Crystal structures of spodumene. (a) α-spodumene, (b) β-spodumene, (c) γ-spodumene. Red: Oxygen. Yellow: Silicon. Blue: Aluminum. Green: Lithium. Note: The lattices images were obtained with the display module of the Jade2010TM software. At a macroscopic level, α-spodumene appears as a very hard rock. It is compact and difficult to cut or grind while β-spodumene appears as a dusty material with a low resistance to grinding. At a microscopic level, α-spodumene appears as a compact material made out of multiple layers stacked on top of each other while β-spodumene presents many cracks on its particles, which make its structure more random.
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Figure 10. Transitions occurring at high temperature (above 900 °C) in the spodumene system.
Figure 10. Transitions occurring at high temperature (above 900 °C) in the spodumene system.
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Figure 11. Flow sheets for the production of lithium compounds from mineral sources. Few steps, such as electrodialysis, have only been tested in feasibility studies [45] (adapted with permission from Elsevier Books, Lithium Process Chemistry; published by Elsevier, 2019).
Figure 11. Flow sheets for the production of lithium compounds from mineral sources. Few steps, such as electrodialysis, have only been tested in feasibility studies [45] (adapted with permission from Elsevier Books, Lithium Process Chemistry; published by Elsevier, 2019).
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Figure 12. Flow sheets for production of lithium compounds from brines.
Figure 12. Flow sheets for production of lithium compounds from brines.
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Figure 13. β-spodumene particles included within a quartz matrix. The big white and translucent particle is quartz and the smaller orange particles contained inside are mostly spodumene [77] (reproduced with permission from Elsevier, Minerals Engineering; published by Elsevier, 2019).
Figure 13. β-spodumene particles included within a quartz matrix. The big white and translucent particle is quartz and the smaller orange particles contained inside are mostly spodumene [77] (reproduced with permission from Elsevier, Minerals Engineering; published by Elsevier, 2019).
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Table
Table 1. Principal lithium-bearing minerals [11].
Table 1. Principal lithium-bearing minerals [11].
MineralFormulaTheoretical Li Content (%)
SpodumeneLiAlSi2O63.73
PetaliteLiAlSi4O102.27
EucryptiteLiAlSiO45.51
BikitaiteLiAlSi2O6.H2O3.40
LepidoliteKLi2AlSi3O10(OH,F)2~3.84
ZinnwalditeKLiFeAl2Si3O10(F,OH)21.59
Amblygonite(Li,Na)AlPO4(OH,F)4.73
MontebrasiteLiAl(PO4)(OH)1 to 4
LithiophyliteLiMnPO44.43
TriphyliteLiFePO44.40
HectoriteNa0,3(Mg,Li)3Si4O10(OH)2~1.93
JadariteLiNaAlSiB2O7(OH)2.85
ZabuyeliteLi2CO318.79
ElbaiteNa(Li1,5Al1,5)Al6Si6B3O27(OH)41.11
Table
Table 2. Crystallographic data of the different spodumene structures [34,38,39].
Table 2. Crystallographic data of the different spodumene structures [34,38,39].
FormStructureSpace Groupa (Å)b (Å)c (Å)Angles (°)Z
α-spodumeneMonoclinicC2/c9.458.395.215β = 1104
β-spodumeneTetragonalP432127.541-9.156-4
γ-spodumeneHexagonalP62225.217-5.464-1
Table
Table 3. Data of the different spodumene phases [40,41] (adapted with permission from Springer Nature, Contributions to Mineralogy and Petrology; published by Springer Nature, 2019).
Table 3. Data of the different spodumene phases [40,41] (adapted with permission from Springer Nature, Contributions to Mineralogy and Petrology; published by Springer Nature, 2019).
FormCp(298 K) (J∙K−1∙mol−1)H0i (kJ∙mol−1)S0i (J∙K−1∙mol−1)
α-spodumene158.93−3053.500129.412
β-spodumene162.77−3031.888155.376
γ-spodumene162.77−3032.128162.038
Table
Table 4. Patented processes of lithium extraction from spodumene [54].
Table 4. Patented processes of lithium extraction from spodumene [54].
Reagent(s)Size (µm)Yield (%)Decrepitation (°C)Temperature (°C)DurationReference
H2SO4 (l)<600901000250« Short »[49]
Ca(OH)2 (aq.)<100901100100–2052 h[55]
CaCO3 (s) + CaSO4 (s)<7585–90-During the decrepitation[56]
CaO (s)-84–100-700-[57]
CaCO3 (s) + CaCl2 (s) + SiO2 (s)<17590–95900–11001100–1200-[58]
(NH4)2SO4/NH4HSO4 (l)<175-1030150–370-[59]
KCl (s) + KCl·NaCl (s)<1501001050During the decrepitation[60]
NaCOOH + Na2CO3<30098–10010029030–90 min[61]
SO3 (g)<60097870335–45015 min[52]
NaOH/Na2CO3 (aq.) + CaO/Ca(OH)2 (aq.)--1010100–200-[62]
NaOH/Na2SiO3/2Na2O·B2O3/Na2S (aq.)<15093-70–1301–48 h[63]
Na2CO3 (s)-85–971000450–75010–120 min[64]
Cl2 (g) + CO (g)<449010401000-[65]
Table
Table 5. Published processes of lithium extraction from spodumene [54].
Table 5. Published processes of lithium extraction from spodumene [54].
Reagent(s)Size (µm)Yield (%)Decrepitation (°C)Temperature (°C)DurationReference
CaMg2Cl6·12H2O (s)<75871100During the decrepitation[66]
Mg(l)-10010501500-[67]
Bacteria (aq.)-<10No decrepitationRoom30 d[68]
Na2CO3 (aq.)-9410502251 h[69]
Na2CO3 (s)/H2O/H2O + NH4HCO3 (aq.)-<10-600 then room30 min then 4 h[70]
HF (aq)-9011007520 min[71]
Cl2 (g)<5099118010003 h[72]
CaCl2 (s)<509011809002 h[73]
Na2SO4 (aq)/NaOH or CaO (aq.)<75901100230-[74]

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Dessemond, C.; Lajoie-Leroux, F.; Soucy, G.; Laroche, N.; Magnan, J.-F. Spodumene: The Lithium Market, Resources and Processes. Minerals 2019, 9, 334. https://doi.org/10.3390/min9060334

AMA Style

Dessemond C, Lajoie-Leroux F, Soucy G, Laroche N, Magnan J-F. Spodumene: The Lithium Market, Resources and Processes. Minerals. 2019; 9(6):334. https://doi.org/10.3390/min9060334

Chicago/Turabian Style

Dessemond, Colin, Francis Lajoie-Leroux, Gervais Soucy, Nicolas Laroche, and Jean-François Magnan. 2019. "Spodumene: The Lithium Market, Resources and Processes" Minerals 9, no. 6: 334. https://doi.org/10.3390/min9060334

APA Style

Dessemond, C., Lajoie-Leroux, F., Soucy, G., Laroche, N., & Magnan, J. -F. (2019). Spodumene: The Lithium Market, Resources and Processes. Minerals, 9(6), 334. https://doi.org/10.3390/min9060334

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