Related Experiment Video
Updated: Jul 9, 2025
12:28
Non-aqueous Electrode Processing and Construction of Lithium-ion Coin Cells
Published on: February 1, 2016
21.6K
Integrated Circular Economy Model System for Direct Lithium Extraction: From Minerals to Batteries Utilizing Aluminum
K Jayanthi1, Tej N Lamichhane1, Venkat Roy2
1Chemical Sciences Division, Oak Ridge National Laboratory, Oak Ridge, Tennessee 37831, United States.
ACS Applied Materials & Interfaces
|December 5, 2023
Summary
Amorphous aluminum hydroxide selectively extracts lithium ions with 86% efficiency. This sustainable method offers a circular economy model for lithium recovery, outperforming traditional processes.
Area of Science:
- Materials Science
- Chemical Engineering
- Environmental Science
Background:
- Aluminum hydroxide exists in four polymorphs: gibbsite, bayerite, nordstrandite, and doyleite.
- Amorphous aluminum hydroxide and crystalline polymorphs are explored for lithium extraction from sulfate solutions.
- Amorphous Al(OH)3 shows higher reactivity for Li+ ion extraction than crystalline forms.
Purpose of the Study:
- To investigate the energetics of aluminum hydroxide polymorphs using high-temperature oxide melt solution calorimetry.
- To evaluate amorphous aluminum hydroxide as a sorbent for selective lithium extraction.
- To assess the environmental and economic viability of this lithium extraction method.
Main Methods:
- High-temperature oxide melt solution calorimetry to determine enthalpic stability.
- Lithium extraction experiments using amorphous aluminum hydroxide.
- Acid-free delithiation and relithiation processes.
- Life cycle and operational cost analysis.
Main Results:
- Enthalpic stability order: gibbsite > bayerite > amorphous Al(OH)3.
- Amorphous Al(OH)3 spontaneously reacts with lithium, forming a stable layered double hydroxide phase.
- Achieved 86% lithium extraction efficiency with a maximum capacity of 37.86 mg·g-1.
- Demonstrated high selectivity and near-complete sorbent recoverability.
Conclusions:
- Amorphous aluminum hydroxide is a promising sorbent for selective lithium extraction from clay mineral leachate.
- The developed method offers a circular economy model for lithium recovery.
- This approach presents environmental advantages over conventional soda ash-based precipitation.
Keywords:
aluminum hydroxideamorphouscircular economydelithiationdirect lithium extractionlithiationrelithiationMore Related Videos
11:14Two-way Valorization of Blast Furnace Slag: Synthesis of Precipitated Calcium Carbonate and Zeolitic Heavy Metal Adsorbent
Published on: February 21, 2017
12.4K
11:25Identification and Quantification of Decomposition Mechanisms in Lithium-Ion Batteries; Input to Heat Flow Simulation for Modeling Thermal Runaway
Published on: March 7, 2022
4.6K
Related Concept Videos
01:19Acid Halides to Alcohols: LiAlH4 Reduction
2.8K
Acid halides are reduced to alcohols in the presence of a strong reducing agent like lithium aluminum hydride.
The mechanism proceeds in three steps. First, the nucleophilic hydride ion attacks the carbonyl carbon of the acid halide to form a tetrahedral intermediate. Next, the carbonyl group is re-formed, and the halide ion departs as a leaving group, generating an aldehyde. A second nucleophilic attack by the hydride yields an alkoxide ion, which, upon protonation, gives a primary alcohol as...
The mechanism proceeds in three steps. First, the nucleophilic hydride ion attacks the carbonyl carbon of the acid halide to form a tetrahedral intermediate. Next, the carbonyl group is re-formed, and the halide ion departs as a leaving group, generating an aldehyde. A second nucleophilic attack by the hydride yields an alkoxide ion, which, upon protonation, gives a primary alcohol as...
2.8K
00:56Extraction: Advanced Methods
450
Metal ions can be separated from one another by complexation with organic ligands–the chelating agent– to form uncharged chelates. Here, the chelating agent must contain hydrophobic groups and behave as a weak acid, losing a proton to bind with the metal. Since most organic ligands used in this process are insoluble or undergo oxidation in the aqueous phase, the chelating agent is initially added to the organic phase and extracted into the aqueous phase. The metal-ligand complex is...
450
01:17Esters to Alcohols: Hydride Reductions
3.5K
Esters are reduced to primary alcohols when treated with a strong reducing agent like lithium aluminum hydride. The reaction requires two equivalents of the reducing agent and proceeds via an aldehyde intermediate.
Lithium aluminum hydride is a source of hydride ions and functions as a nucleophile. The mechanism proceeds in three steps. Firstly, the nucleophilic hydride ion attacks the carbonyl carbon of the ester to form a tetrahedral intermediate. Subsequently, the carbonyl group re-forms,...
Lithium aluminum hydride is a source of hydride ions and functions as a nucleophile. The mechanism proceeds in three steps. Firstly, the nucleophilic hydride ion attacks the carbonyl carbon of the ester to form a tetrahedral intermediate. Subsequently, the carbonyl group re-forms,...
3.5K
01:24Preparation of Aldehydes and Ketones from Nitriles and Carboxylic Acids
3.5K
Although it is possible to reduce a carboxylic acid to an aldehyde, strong reducing agents, like lithium aluminum hydride (LAH), prohibit a controlled reduction, instead causing the generated aldehyde to instantly over-reduce to a primary alcohol.
Reducing carboxylic acid derivatives like acyl chlorides (RCOCl), esters (RCO2R′), and nitriles (RCN) using milder aluminum hydride agents like lithium tri-tert-butoxyaluminum hydride [LiAlH(O-t-Bu)3] and diisobutylaluminum hydride [DIBAL-H]...
Reducing carboxylic acid derivatives like acyl chlorides (RCOCl), esters (RCO2R′), and nitriles (RCN) using milder aluminum hydride agents like lithium tri-tert-butoxyaluminum hydride [LiAlH(O-t-Bu)3] and diisobutylaluminum hydride [DIBAL-H]...
3.5K
01:20Amides to Amines: LiAlH4 Reduction
4.8K
Amide reduction with strong reducing agents like lithium aluminum hydride proceeds through a nucleophilic acyl substitution to form amines. Primary, secondary, and tertiary amides yield primary, secondary, and tertiary amines, respectively.
Amide reduction requires two equivalents of the reducing agent, acting as a source of hydride ions. As shown in the figure, the reaction is initiated with a nucleophilic attack by the hydride ion at the carbonyl carbon to form a tetrahedral intermediate.
Amide reduction requires two equivalents of the reducing agent, acting as a source of hydride ions. As shown in the figure, the reaction is initiated with a nucleophilic attack by the hydride ion at the carbonyl carbon to form a tetrahedral intermediate.
4.8K