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Intercalation (chemistry)
Intercalation (chemistry)
Intercalation (chemistry)
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Intercalation is the reversible inclusion or insertion of a molecule (or ion) into layered materials with layered structures. Examples are found in graphite and transition metal dichalcogenides.[1][2]

Model of intercalation of potassium into graphite

Examples

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Graphite

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One famous intercalation host is graphite, which intercalates potassium as a guest.[3] Intercalation expands the van der Waals gap between sheets, which requires energy. Usually this energy is supplied by charge transfer between the guest and the host solid, i.e., redox. Two potassium graphite compounds are KC8 and KC24. Carbon fluorides (e.g., (CF)x and (C4F)) are prepared by reaction of fluorine with graphitic carbon. The color is greyish, white, or yellow. The bond between the carbon and fluorine atoms is covalent, thus fluorine is not intercalated.[clarification needed] Such materials have been considered as a cathode in various lithium batteries.

Diagram of intercalation of Li into a titanium disulfide cathode. One axis of the TiS2 crystal swells, and charge transfers from Li to Ti.

Treating graphite with strong acids in the presence of oxidizing agents causes the graphite to oxidise. Graphite bisulfate, [C24]+[HSO4]−, is prepared by this approach using sulfuric acid and a little nitric acid or chromic acid. The analogous graphite perchlorate can be made similarly by reaction with perchloric acid.[clarification needed]

Lithium-ion batteries

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One of the largest and most diverse uses of the intercalation process by the early 2020s is in lithium-ion electrochemical energy storage, in the batteries used in many handheld electronic devices, mobility devices, electric vehicles, and utility-scale battery electric storage stations.

By 2023, all commercial Li-ion cells use intercalation compounds as active materials, and most use them in both the cathode and anode within the battery physical structure.[4]

In 2012 three researchers, Goodenough, Yazami and Yoshino, received the 2012 IEEE Medal for Environmental and Safety Technologies for developing the intercalated lithium-ion battery and subsequently Goodenough, Whittingham, and Yoshino were awarded the 2019 Nobel Prize in Chemistry "for the development of lithium-ion batteries".[5]

Exfoliation

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An extreme case of intercalation is the complete separation of the layers of the material. This process is called exfoliation. Typically aggressive conditions are required involving highly polar solvents and aggressive reagents.[6] This process can be used to form nanosheets in many layered oxide structures like LiCoO2 and NMC, which are used in Li-ion battery cathode applications.[7]

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In biochemistry, intercalation is the insertion of molecules between the bases of DNA. This process is used as a method for analyzing DNA and it is also the basis of certain kinds of poisoning.

Clathrates are chemical substances consisting of a lattice that traps or contains molecules. Usually, clathrate compounds are polymeric and completely envelop the guest molecule. Inclusion compounds are often molecules, whereas clathrates are typically polymeric. Intercalation compounds are not 3-dimensional, unlike clathrate compounds.[8] According to IUPAC, clathrates are "Inclusion compounds in which the guest molecule is in a cage formed by the host molecule or by a lattice of host molecules."[9]

Stress caused by intercalation

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Intercalation of atoms into layered materials induces volumetric changes and lattice mismatch within the crystal structure. These changes generate localized tensile and compressive stresses. The magnitude of these stresses depends on factors such as the size of the intercalating species and the crystallographic structure of the host material.[10] In electrochemical systems, such as lithium-ion batteries, operating conditions—particularly the charge/discharge rate and temperature—also influence stress levels.[11]

Effects during battery operation

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During electrochemical cycling—the repeated charging and discharging of a battery—ions are intercalated and deintercalated from electrode materials, causing expansion and contraction of the layered structure. These volumetric fluctuations generate local stresses that can vary between cycles, leading to the buildup of residual stress.[12] Over time, this accumulation can result in mechanical fatigue and the formation of microcracks, especially at stress concentration sites.[13]

Such mechanical degradation contributes to capacity loss through several mechanisms:

  • Loss of electrical connectivity within the active material,[14]
  • Increased formation of the solid-electrolyte interphase (SEI), consuming electrolyte and active lithium,[15]
  • Enhanced susceptibility to further cracking and dendritic lithium growth.[16]

Collectively, these failure modes contribute to the progressive deterioration of battery performance and ultimately, failure.

Implications on battery design

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To mitigate intercalation-induced stress, electrode materials are selected based on their structural compatibility with the intercalating ion—most commonly lithium. Commercial lithium-ion electrodes, such as LiCoO2 or LiFePO4, are chosen in part for their relatively low intercalation-induced stress and structural stability, which contribute to longer cycle life.[17]

With the increasing interest in solid-state batteries, new challenges emerge. Solid electrolytes, unlike their liquid counterparts, can also accumulate mechanical stress as ions migrate through them. The volumetric changes in both the electrode and the solid electrolyte can lead to poor interfacial contact, impeding ion transport and potentially causing delamination at phase boundaries.[18]

Research

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Relevant to energy storage systems, the mechanical effects of ion intercalation, particularly volume expansion and the resulting stress accumulation, are central to the degradation mechanisms observed in many electrode materials.[10] Some electrode architectures can better accommodate these mechanical stresses. Nanostructured materials, including hollow particles, porous frameworks, and core–shell morphologies, can distribute mechanical loads more uniformly during cycling.[13] Flexible polymeric binders and conductive networks that are capable of self-healing or plastic deformation offer further potential to mitigate stress-induced damage.[16]

In solid-state batteries, the issue is even more pronounced due to the rigidity of inorganic solid electrolytes. Unlike liquid electrolytes, which can conform to morphological changes, solid electrolytes are more susceptible to cracking, void formation, and delamination at interfaces during cycling. These mechanical failures can impede ion transport and lead to cell failure.[18] Strategies to reduce stress in solid-state systems include the use of compliant interlayers, interface engineering, and electrolyte materials with improved mechanical toughness.[19]

See also

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Notes

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Intercalation (chemistry)

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In chemistry, intercalation refers to the reversible insertion of guest , such as atoms, ions, or molecules, into the layered or framework structure of a crystalline host material, preserving the host's structural integrity and often occurring at . This process, classified as a topotactic solid-state reaction, distinguishes intercalation compounds from inclusion or compounds by maintaining the host lattice while allowing ordered guest incorporation, sometimes exhibiting staging where guests form periodic layers. Intercalation typically involves charge transfer between the host and guest, weakening interlayer van der Waals or electrostatic interactions and enabling property modifications like enhanced conductivity or phase transitions. The phenomenon has roots dating back nearly a century, with early pioneering work by Ulrich Hofmann in the 1930s on intercalation compounds (GICs), though research peaked between 1970 and 1990 amid growing interest in layered materials. Intercalation compounds are categorized by dimensionality: one-dimensional (e.g., chains or tunnels in β-MnO₂ hosting Li), two-dimensional (e.g., layered structures like TiS₂ or V₂O₅ with Li insertion), and three-dimensional (e.g., frameworks such as Li₂Mn₂O₄). Notable examples include GICs, where alkali metals or insert between sheets; transition metal dichalcogenides (TMDs) like MoS₂ undergoing 2H to 1T phase shifts upon Li intercalation; and clays or serving as hosts for various guests. Intercalation's versatility stems from synthesis methods like direct , , or electrochemical processes, making it a cornerstone for tailoring material properties in applications ranging from to . In rechargeable batteries, such as lithium- systems, intercalation enables reversible shuttling in cathodes like LiCoO₂ or anodes like , underpinning high and cycle life. Beyond batteries, it facilitates the exfoliation and fabrication of two-dimensional materials like or TMD nanosheets for , , and sensors; enhances catalytic performance, as in Li-intercalated MoS₂ for with current densities up to 200 mA/cm²; and induces exotic properties like in Cu-intercalated Bi₂Se₃ at 3.8 K. These attributes position intercalation as a fundamental tool in modern , with ongoing research exploring sodium- and magnesium-based systems for technologies.

Fundamentals

Definition and Principles

Intercalation in chemistry refers to the reversible insertion of guest species, such as ions, molecules, or atoms, into the lattice of a host material, typically structures with layered or porous architectures, without causing substantial disruption to the host framework. This process allows the guest to occupy sites or interlayer spaces, forming intercalation compounds where the host retains its overall crystallinity and . Unlike adsorption, which confines interactions to the surface of the host, or inclusion compounds like clathrates that trap guests within rigid cage-like voids, intercalation involves into the bulk structure, enabling tunable modifications to the host's properties. The underlying principles of intercalation revolve around host-guest interactions that stabilize the inserted species while preserving reversibility. These interactions primarily include van der Waals forces between layers, electrostatic attractions for ionic guests, and occasionally covalent bonding or hydrogen bonding depending on the chemical nature of the host and guest. In layered hosts, the weak interlayer forces facilitate guest entry and exit, often driven by processes or effects, with the guest concentration determining the degree of lattice expansion. This reversibility distinguishes intercalation as a dynamic equilibrium, where guests can be extracted under appropriate conditions without permanent structural damage. Suitable host materials for intercalation exhibit structural , featuring interlayer spaces such as van der Waals gaps typically exceeding 3 to accommodate guest insertion without excessive strain. Common host classes include two-dimensional materials with weakly bound layers, where the gap size and layer rigidity dictate the feasibility and staging of intercalation—referring to ordered distributions of guest layers. The term "intercalation" was first used in 1951 to describe such compounds, particularly those involving , building on foundational research. Early studies trace back to and , when Rüdorff and Hofmann investigated the insertion of metals and acids into , proposing initial models for staged intercalation structures.

Thermodynamics and Kinetics

The thermodynamics of intercalation reactions in layered host materials is governed by the change, ΔG=ΔH−TΔS\Delta G = \Delta H - T \Delta S, which determines the energetic favorability of guest insertion between host layers. The term (ΔH\Delta H) arises primarily from host-guest bonding interactions, such as electrostatic or covalent forces, often resulting in exothermic contributions that stabilize the intercalated structure, while the term (ΔS\Delta S) reflects changes in configurational disorder due to layer expansion and guest mobility, typically providing a positive but smaller contribution at elevated temperatures. For instance, in multiphase layered systems, the local free energy density incorporates both enthalpic interactions (parameterized by regular solution models with interaction parameter Ωa\Omega_a, typically on the order of a few kBTk_B T) and entropic lattice gas contributions (kBT[c~ln⁡c~+(1−c~)ln⁡(1−c~)]k_B T [\tilde{c} \ln \tilde{c} + (1 - \tilde{c}) \ln (1 - \tilde{c})]), leading to ΔG<0\Delta G < 0 for spontaneous intercalation under suitable conditions. Stage formation further influences thermodynamic stability, where distinct phases emerge based on guest concentration: stage 1 represents full intercalation of every interlayer space, stage 2 involves alternating filled and empty layers, and higher stages feature more dilute guest distributions to minimize repulsive interactions between layers. These stages minimize the overall free energy by balancing host strain and guest-host attractions, with transitions driven by temperature and composition. Binary phase diagrams for guest-host systems, such as those derived from staging models, often depict intercalation compounds as line compounds (stoichiometric phases like stage n) or solid solutions (continuous concentration ranges), with phase boundaries reflecting coexistence regions where multiple stages are thermodynamically stable, as seen in temperature-dependent diagrams up to ~500 K for certain systems. Kinetically, intercalation proceeds via diffusion-controlled insertion of guests into interlayer spaces, with rates limited by activation energies typically ranging from 20 to 100 kJ/mol, encompassing barriers for desolvation, entry, and migration within the host lattice. Interlayer diffusion follows Fick's laws, where the flux J=−D∂c∂xJ = -D \frac{\partial c}{\partial x} yields diffusion coefficients D≈10−9D \approx 10^{-9} to 10−1210^{-12} m²/s, influenced by layer spacing and guest size; for example, in multiphase models, effective D0D_0 accounts for concentration-dependent mobility via chemical potential gradients. These low DD values highlight the sluggish nature of solid-state diffusion compared to solution-phase processes, often requiring elevated temperatures or electrochemical driving forces to achieve practical rates. In electrochemical intercalation, the process is potential-dependent, described by the Nernst equation E=E∘+RTnFln⁡aguestE = E^\circ + \frac{RT}{nF} \ln a_{\text{guest}}, where the equilibrium potential shifts with guest activity (aguesta_{\text{guest}}), linking thermodynamics to applied voltage and enabling control over ΔG\Delta G via Veq=EΘ−μeff/eV_{eq} = E^\Theta - \mu_{\text{eff}}/e. Overpotentials arise from kinetic limitations, including charge transfer and diffusion barriers, quantified through Butler-Volmer relations where excess voltage η\eta increases with current density, often adding 50-200 mV to drive non-equilibrium staging or phase transitions. Layered hosts facilitate these low-energy pathways due to their weak interlayer bonding, though detailed structural aspects are covered elsewhere.

Host Materials

Carbon-Based Hosts

Carbon-based materials serve as exemplary hosts for intercalation due to their layered or nanostructured architectures, which facilitate the reversible insertion of guest species between layers or within voids. Graphite, the archetypal carbon host, features a hexagonal lattice of sp²-hybridized carbon atoms arranged in AB-stacked layers, where adjacent layers are offset by one-sixth of the unit cell vector, resulting in a van der Waals interlayer distance of 3.35 Å. This weak interlayer bonding allows for significant expansion upon guest insertion, with interlayer spacings increasing to accommodate species up to approximately 10 Å, enabling the formation of stable intercalation compounds without disrupting the overall layered integrity. The intercalation capacity of graphite is notably high for alkali metals, achieving stage-1 compounds with stoichiometries up to C₆M (where M denotes an alkali metal such as Li or K), as seen in binary graphite intercalation compounds (GICs) like LiC₆ and KC₈. These structures exhibit ordered staging, where guest layers alternate with pristine graphene sheets, maximizing host utilization while minimizing strain. Ternary GICs further expand this capacity, incorporating solvents or co-intercalants, such as KC₈ compounded with ammonia or tetrahydrofuran, which stabilize the intercalate and enhance solubility in synthesis. Beyond graphite, other carbon allotropes offer distinct hosting capabilities, though with varying limitations. Graphene oxide (GO), with its oxidized functional groups (e.g., hydroxyl, epoxide), possesses an expanded interlayer spacing of about 7-10 Å, promoting intercalation of ions, dyes, or polymers that interact via hydrogen bonding or electrostatic forces. Carbon nanotubes (CNTs), particularly multi-walled variants, enable axial intercalation into open-ended structures or bundle interstices, allowing guest diffusion along the tube axis or between walls, though radial constraints limit loading compared to planar graphite. Fullerenes, such as C₆₀, exhibit restricted intercalation potential due to their closed, curved geometry, which precludes layered expansion and favors surface adsorption or doping over bulk insertion. Intercalated carbon hosts display enhanced functional properties, particularly in electron transport and thermal resilience. Donor-type GICs, formed with electron-rich guests like alkali metals, exhibit metallic behavior with electrical conductivities up to 10⁷ S/m, arising from charge transfer that populates the graphene π* bands and increases carrier density. Certain GICs, such as those with metal chlorides or alkali intercalates, maintain structural integrity and performance up to 600°C, benefiting from the robust sp² network that resists decomposition under thermal stress.

Inorganic Layered Hosts

Inorganic layered hosts represent a diverse class of materials beyond carbon-based structures, characterized by ionic and polar interlayer environments that enable tunable swelling and selective guest insertion. These hosts, including transition metal dichalcogenides, , and metal oxides/hydroxides, feature stacked layers held by weak electrostatic or van der Waals forces, allowing ions, molecules, or solvents to penetrate and expand the galleries. Their chemical versatility arises from surface charge and redox capabilities, facilitating applications in catalysis and ion exchange. Transition metal dichalcogenides (TMDs) such as MoS₂ and WS₂ adopt an MX₂ structure, where M denotes a transition metal (e.g., Mo, W) and X a chalcogen (S, Se, Te), forming trilayer sheets with intralayer covalent bonding and interlayer van der Waals interactions. The typical interlayer distance ranges from 6 to 7 Å, as seen in MoS₂ at approximately 6.15 Å, which accommodates guest species like alkali metals without significant structural collapse. Intercalation in TMDs often involves electron transfer, with redox-active sites at layer edges or defects promoting phase transitions, such as from semiconducting 2H to metallic 1T polymorphs in MoS₂ upon Li insertion. Clays and phyllosilicates, including and , serve as archetypal swelling hosts due to their aluminosilicate frameworks. features a 1:1 layer type, consisting of one tetrahedral silica sheet bonded to one octahedral alumina sheet; intercalation is challenging due to the limited available space (~2 Å), and often involves an initial expansion with DMSO, increasing the spacing to ~11 Å and enabling subsequent insertion of neutral polar molecules like alcohols or amines. In contrast, exhibits a 2:1 layer structure, with two tetrahedral sheets sandwiching an octahedral sheet, and its permanent negative charge from isomorphous substitution allows expansive swelling in aqueous environments, increasing basal spacing up to 20 Å upon hydration or organic cation exchange. This swelling behavior supports reversible guest insertion, such as water or alkylammonium ions, altering hydrophilicity for tailored interactions. Oxides and hydroxides provide additional platforms for selective intercalation, exemplified by layered double hydroxides (LDHs) and vanadium oxides. LDHs, with the general formula [M²⁺_{1-x}M³⁺x(OH)₂]^(x+)(A^{n-}){x/n}·mH₂O, feature brucite-like layers where divalent (e.g., Mg²⁺) and trivalent (e.g., Al³⁺) cations occupy octahedral sites, yielding positively charged host layers balanced by intercalated anions like carbonates; a representative example is Mg₂Al(OH)₆ with interlayer spacing around 7.8 Å, facilitating anion exchange for applications in sorption. Vanadium pentoxide (V₂O₅) forms orthorhombic layered structures with edge- and corner-sharing VO₅ square pyramids, exhibiting a pristine interlayer distance of about 4.4 Å that expands upon cation insertion, such as Li⁺ up to x=3 in Li_xV₂O₅ or Na⁺ increasing spacing to 4.8 Å, driven by reversible redox processes at vanadium sites. Unique behaviors in these hosts enhance their functionality, such as pillaring in clays with large polyoxometalate guests like Keggin ions (e.g., Al₁₃O₄(OH)₂₄(H₂O)₁₂^{7+}), which involves cation exchange into montmorillonite interlayers followed by calcination, yielding stable pillars that maintain expanded spacing (1.7-1.8 nm) and high surface areas up to 226 m²/g for catalytic use. In TMDs, redox-active sites enable coupled electron transfer during intercalation, as metal ions donate electrons to transition metal d-orbitals, stabilizing inserted phases and modulating electronic properties for enhanced charge storage. MXenes, two-dimensional transition metal carbides, nitrides, or carbonitrides with the formula M_{n+1}X_nT_x (where M is a transition metal, X is C and/or N, and T_x represents surface terminations), act as versatile hosts for intercalation. Their multilayered structure features interlayer distances of 1–2 nm, allowing reversible insertion of ions, molecules, or solvents, often with charge transfer that tunes electronic properties for applications in energy storage and sensors.

Intercalation Processes

Mechanisms of Guest Insertion

Intercalation of guest species into layered host materials typically proceeds via two primary insertion pathways: direct entry at the edges of the layers or diffusion through intrinsic defects within the structure. In the direct pathway, guests access the interlayer spaces by penetrating the exposed edges of the layered crystallites, which is favored for smaller ions and often initiates structural expansion from the periphery inward. This edge-entry mechanism is prevalent in pristine or low-defect hosts, where the basal planes remain largely impermeable, limiting initial insertion to peripheral sites before propagation occurs. Alternatively, diffusion through defects—such as vacancies, wrinkles, or dislocations—enables guests to enter via the top or basal surfaces, particularly in materials with natural imperfections that lower the energy barrier for penetration. These defect-mediated pathways become dominant in exfoliated or nanostructured hosts, allowing more uniform distribution but potentially introducing localized strain. In liquid-phase processes, solvation effects significantly influence insertion by stabilizing guest ions through coordination with solvent molecules, often leading to co-intercalation where both the ion and solvent enter the host together. For cations like Li⁺, the solvation shell reduces desolvation energy at the interface, facilitating faster diffusion and reversible insertion without forming a solid-electrolyte interphase, as the coordinated solvent acts as an electrostatic shield. This co-intercalation expands the interlayer spacing more substantially than bare ion insertion, enabling access to otherwise kinetically hindered sites, though the choice of solvent (e.g., ethers with strong coordination) is critical for maintaining stability. Guest species in intercalation encompass cations, anions, and neutral molecules, each interacting differently with the host lattice. Cations, such as Li⁺, typically require reductive conditions and often co-intercalate with solvents to mitigate charge repulsion from the host layers. Anions, like those in oxidative intercalation (e.g., in layered double hydroxides), enter via ion-exchange mechanisms, where they replace existing counterions and are stabilized by electrostatic attraction to positively charged layers. Neutral molecules, such as , intercalate through van der Waals or hydrogen-bonding interactions, acting as spacers that weakly perturb the electronic structure while expanding the gallery height. During partial filling, staging transitions govern the ordered distribution of guests, as described by the Daumas-Hérold model, where intercalate forms isolated islands within unoccupied galleries rather than uniform layers. This domain-based arrangement minimizes elastic strain energy and accommodates varying guest concentrations, leading to sequential stage formations (e.g., stage n to n-1) as filling progresses. Accompanying these transitions, the host layers undergo rippling or buckling to relieve in-plane stresses from guest insertion, resulting in transient distortions that facilitate further diffusion. Spectroscopic techniques provide direct evidence for these mechanisms, with in-situ X-ray diffraction (XRD) revealing real-time changes in interlayer spacing as guests insert, such as discrete shifts corresponding to staging plateaus. For instance, XRD patterns show progressive expansion of d-spacing from ~3.4 Å in pristine hosts to larger values upon intercalation, correlating with pathway activation. Complementarily, Raman spectroscopy detects shifts in vibrational modes, including guest-host interactions like new low-frequency peaks from interlayer modes or softening of in-plane vibrations due to charge transfer. These shifts, often downshifting by 10-20 cm⁻¹ for E₂g modes in transition metal dichalcogenides, confirm the degree of intercalation and local bonding changes.

Specific Examples in Graphite and Batteries

One prominent example of intercalation in graphite involves alkali metals, such as lithium, forming graphite intercalation compounds (GICs) like LiC₆, where lithium atoms occupy positions between the graphene layers, achieving a theoretical specific capacity of 372 mAh/g based on the formation of this fully lithiated stage-1 compound. During the intercalation process, the structure evolves through distinct staging sequences, starting from higher-stage compounds (e.g., stage 4, with intercalant layers separated by three empty graphene layers) and progressing to lower stages (stage 3, stage 2) as more lithium is inserted, culminating in stage 1 (LiC₆), where every interlayer is filled; this stepwise phase transition reflects the thermodynamic preference for ordered, periodic arrangements to minimize strain energy. Similar staging occurs with other alkali metals like potassium in KC₈ (stage 1) or sodium, though lithium's smaller ionic radius enables denser packing and higher capacity in practical applications. In lithium-ion batteries, graphite serves as the primary anode material, where Li⁺ ions intercalate during charging (inserting into the layered structure to form LiC₆) and deintercalate during discharge, enabling reversible storage without the safety risks of metallic lithium. The key electrochemical reaction at the anode is: \ceC6+Li++e−⇌LiC6\ce{C6 + Li+ + e- ⇌ LiC6} which occurs at a potential of approximately 0.1 V versus , corresponding to the coexistence of graphite and dilute lithiated phases before full stage-1 formation. Prior to significant intercalation, a solid electrolyte interphase (SEI) layer forms on the graphite surface through electrolyte decomposition at potentials around 0.8–1.5 V versus Li/Li⁺, creating a passivating film that permits Li⁺ transport while blocking electron flow and further solvent reduction, thus stabilizing the electrode for long-term cycling. On the cathode side, materials like LiCoO₂ exemplify intercalation by reversibly hosting Li⁺ ions between octahedral sites in its layered rock-salt structure, with deintercalation during charging (LiCoO₂ → Li_{1-x}CoO₂ + xLi⁺ + xe⁻) enabling high voltage operation up to 4 V versus Li/Li⁺. The integration of graphite anodes marked a pivotal historical milestone, with Sony commercializing the first lithium-ion battery in 1991 using petroleum coke-derived carbon (an early graphite precursor) paired with a LiCoO₂ cathode, achieving safe, high-energy-density performance that revolutionized portable electronics. This design overcame earlier limitations of lithium-metal anodes, such as dendrite formation, by leveraging reversible intercalation, though initial capacities were modest due to incomplete staging. Subsequent advancements have evolved toward silicon-graphite composite anodes, where silicon nanoparticles (offering ~3579 mAh/g theoretical capacity via alloying) are blended with graphite to boost overall energy density while mitigating silicon's volume expansion through graphite's structural buffering, enabling practical capacities exceeding 500 mAh/g in modern cells.

Applications

Energy Storage and Conversion

Intercalation reactions form the cornerstone of lithium-ion batteries (LIBs), where lithium ions reversibly insert into layered cathode materials such as LiCoO₂ and graphite anodes to achieve high energy densities typically ranging from 250 to 300 Wh kg⁻¹. This process enables a theoretical capacity of 372 mAh g⁻¹ for graphite via formation of LiC₆ stages, supporting practical cell voltages up to 4.2 V and volumetric densities around 600 Wh L⁻¹ in modern configurations. However, limitations such as potential lithium dendrite formation at high rates or low temperatures can compromise safety and cycle stability, necessitating optimized electrolytes and electrode designs. In supercapacitors, pseudocapacitive intercalation in transition metal oxides like MnO₂ and RuO₂ facilitates rapid charge storage through redox-mediated ion insertion, yielding specific capacitances exceeding 200 F g⁻¹ for MnO₂ and up to 1340 F g⁻¹ for nanostructured RuO₂ in aqueous electrolytes. For MnO₂, the reaction MnO₂ + xA⁺ + xe⁻ → AₓMnO₂ (where A⁺ is an alkali cation) supports fast kinetics with minimal structural change, enabling rate capabilities down to 20-second charge-discharge times while maintaining 490 F g⁻¹ at 50 mV s⁻¹ when hybridized with carbon supports. RuO₂ exhibits similar proton intercalation via RuOₓ(OH)ᵧ + dH⁺ + de⁻ → RuOₓ₋d(OH)ᵧ₊d, offering theoretical limits of 1450 F g⁻¹ over a 1 V window, though practical applications are constrained by cost. Sodium-ion batteries (SIBs) leverage intercalation into hard carbon anodes, which provide plateau capacities up to 300 mAh g⁻¹ at potentials below 0.1 V vs. Na/Na⁺ through a combination of layer intercalation and pore filling, contributing to cell energy densities around 150 Wh kg⁻¹. Optimal interlayer spacings of 0.36–0.40 nm enhance Na⁺ diffusion, with reported initial Coulombic efficiencies up to 94% and capacity retention of 99% over 100 cycles at low rates. In fuel cells, deposition of Pt nanoparticles onto graphene-derived supports improves catalyst stability and activity; for instance, PtCo on graphene-derived supports achieves mass activity retention of 55.7% after accelerated degradation tests and peak power densities of 1.04 W cm⁻² at 0.1 mg Pt cm⁻² loading. Key performance factors in intercalation-based devices include cycle life exceeding 1000 cycles, as demonstrated in LIB anodes with >90% retention and SIBs sustaining 162 mAh g⁻¹ after 1000 cycles at 0.05% loss per cycle. Rate capability is governed by lengths, where shorter paths in nanostructured hosts reduce barriers and enable high-rate operation, such as 5C discharges with 96% capacity retention in optimized layered oxides. This aligns with the reversible Li⁺ insertion in , which underpins efficient charge transport in LIBs without the irreversibility seen in conversion reactions. Beyond , intercalation enhances catalytic performance, as in Li-intercalated MoS₂ for the with current densities up to 200 mA/cm², and induces exotic properties like in Cu-intercalated Bi₂Se₃ at 3.8 K.

Nanomaterial Synthesis via Exfoliation

Intercalation plays a pivotal role in the synthesis of two-dimensional (2D) by facilitating the of layered host s into single- or few-layer sheets. In this process, guest species such as ions or molecules are inserted between the layers of a host , expanding the interlayer spacing and weakening the van der Waals interactions that hold the layers together. This intercalation-induced expansion creates internal stresses that, when combined with subsequent mechanical agitation, ultrasonication, or chemical shear, lead to the exfoliation of the bulk into nanoscale sheets. Yields of up to 90% single-layer nanosheets have been achieved through optimized intercalation strategies, particularly when using alkali metal-based intercalants like sodium naphthalenide, which enable efficient separation while preserving the structural integrity of the resulting 2D . Key methods for intercalation-driven exfoliation include chemical and electrochemical approaches, often applied to layered inorganic hosts such as and transition metal dichalcogenides (TMDs). The chemical route, exemplified by the , involves oxidizing with and to form , where oxygen-containing functional groups act as intercalants to disrupt interlayer bonding. This results in spontaneous or ultrasound-assisted exfoliation to graphene oxide (GO) sheets, with yields exceeding 70 wt% and over 90% consisting of single layers, typically 1-2 nm thick. Electrochemical methods, such as lithium-ion intercalation in bulk MoS₂, offer a faster alternative, completing in under 1 hour using a ; this process yields single-, bi-, and tri-layer MoS₂ nanosheets with average lateral dimensions of ~0.8 μm and monolayer thicknesses of approximately 0.65 nm. These techniques produce high-quality 2D products like (obtained via reduction of GO) and TMD nanosheets, which retain the electronic and optical properties of their bulk counterparts but exhibit enhanced surface areas. The exfoliated 2D nanomaterials find applications in electronic composites, where their large aspect ratios and tunable properties enable improved conductivity and mechanical reinforcement in devices like transistors and sensors. Recent post-2020 advances have focused on scalable liquid-phase exfoliation for —2D carbides and nitrides derived from —using intercalants like Li⁺ to enhance delamination efficiency during or after selective . For instance, Li⁺ intercalation increases interlayer spacing in Ti₃C₂Tₓ , facilitating high-yield dispersions (>80% few-layer nanosheets) via mild in aqueous media, which supports the fabrication of flexible films and coatings for . These developments emphasize environmentally benign solvents and continuous processing to bridge laboratory-scale synthesis with industrial production.

Structural and Mechanical Effects

Stress Generation and Material Deformation

During intercalation, the insertion of guest species into layered host materials induces significant changes, leading to mechanical stress and potential deformation. In , lithium intercalation results in a volume expansion of approximately 10% along the c-axis, primarily due to the increase in interlayer spacing from 3.35 in pristine graphite to about 3.70 in the fully lithiated LiC₆ stage. In dichalcogenides (TMDs), such as WTe₂, the process can produce anisotropic strains, with up to 5% in-plane expansion in one direction and 1% in the orthogonal direction upon minimal lithium insertion, reflecting the directional nature of guest accommodation within the van der Waals gaps. These expansions arise from the inherent mismatch between the size of the intercalating guests and the available interlayer space, which forces lattice dilation and generates internal pressures. The primary causes of stress include this geometric mismatch, where larger guests like alkali ions exceed the equilibrium interlayer dimensions, and abrupt phase transitions associated with staging phenomena. Staging refers to ordered configurations where guests occupy specific interlayer sites, leading to discrete volume jumps as the system transitions between stages (e.g., from stage 2 to stage 1 in ), which can amplify local strains by up to several percent. These transitions create heterogeneous strain fields, with regions of high guest concentration expanding more rapidly than surrounding areas, resulting in stress concentrations that promote deformation. In battery contexts, such deformations contribute to cracking and over cycles. The stresses generated are predominantly compressive during guest influx due to volumetric expansion, though tensile stresses can emerge at interfaces or during deintercalation as the lattice contracts. In constrained geometries, like particles, intercalation induces radial compressive stresses internally while surface regions experience tensile hoop stresses, potentially exceeding hundreds of MPa. For , the Griffith criterion governs crack propagation, where unstable growth occurs when the release rate surpasses the critical value for the material, often triggered by these stress gradients in layered hosts; the criterion posits that a crack advances if G≥2γG \geq 2\gamma, with GG as the strain release rate and γ\gamma the surface . Measurement of these effects relies on in-situ dilatometry, which tracks real-time dimensional changes in electrodes during cycling, revealing expansion strains as low as 0.1% with sub-micrometer resolution. Complementary finite element modeling simulates stress fields using the linear elastic relation σ=Eϵ\sigma = E \epsilon, where σ\sigma is , EE the , and ϵ\epsilon the strain tensor, allowing prediction of localized deformations from intercalation-induced volume shifts in complex microstructures. These techniques provide quantitative insights into how stresses evolve, aiding in the characterization of deformation without .

Design Implications and Future Directions

In battery design, intercalation-induced volume expansion in layered hosts like necessitates the incorporation of buffer layers, such as carbon coatings, to accommodate mechanical strain and prevent cracking during lithium insertion. These coatings enhance electrical conductivity and provide a compliant interface that mitigates degradation, thereby improving cycle life in -ion batteries. Similarly, three-dimensional (3D) architectures, including porous scaffolds and arrays, facilitate strain relief by distributing stress across a larger volume, reducing localized deformation in host materials like or oxides. However, without such measures, cracking from intercalation stresses leads to capacity fade. This degradation also poses safety risks, as mechanical failures can propagate cracks that trigger internal short circuits, potentially initiating through exothermic reactions. To address these challenges, mitigation strategies include engineering host materials, such as coated , which maintain stable intercalation while limiting expansion to around 10%. These modifications distribute lithium uptake, reducing stress concentrations and enhancing structural . Additionally, solid-state electrolytes offer a promising approach by providing mechanical robustness to counteract volume changes, with sulfide-based electrolytes demonstrating high capacity retention over hundreds of cycles in intercalation-based systems by suppressing unwanted reactions and accommodating expansion without liquid leakage. Looking to future directions, research in the has focused on stress-tolerant hosts like , two-dimensional carbides/nitrides that enable reversible intercalation with minimal deformation due to their accordion-like structure, achieving over 1000 cycles at high rates in solid-state configurations. AI-driven modeling is emerging as a tool for predicting deformation, using algorithms to simulate stress evolution in electrodes based on microstructural data, accelerating the design of resilient materials. As of October 2025, a theoretical formula has been developed to guide faster-charging batteries by linking lithium intercalation kinetics to mechanical properties, potentially reducing stress-induced degradation. Post-2020 advances in flexible batteries further highlight intercalation's role, with printed graphite-based anodes in bendable devices retaining high capacity after hundreds of bending cycles, paving the way for wearable electronics.

References

  1. https://www.sciencedirect.com/topics/chemical-engineering/intercalation-compound
  2. https://pubs.rsc.org/en/content/articlelanding/2014/dt/c4dt00203b
  3. https://www.nature.com/articles/s41699-021-00211-6
  4. https://advanced.onlinelibrary.wiley.com/doi/10.1002/adma.202312918
  5. https://www.researchgate.net/publication/313837637_Principle_of_intercalation
  6. https://pubs.rsc.org/en/content/articlehtml/2021/cs/d0cs00187b
  7. https://pubs.rsc.org/en/content/articlelanding/2019/cs/c9cs00162j
  8. https://www.osti.gov/servlets/purl/1986277
  9. https://www.researchgate.net/publication/262977402_Storylines_in_Intercalation_Chemistry
  10. https://www.nature.com/articles/s41467-017-01787-8
  11. https://link.aps.org/doi/10.1103/PhysRevLett.103.196401
  12. https://www.tandfonline.com/doi/abs/10.1080/00018738100101367
  13. https://pmc.ncbi.nlm.nih.gov/articles/PMC11258350/
  14. https://pubs.acs.org/doi/10.1021/acs.chemmater.5b00235
  15. https://www.sciencedirect.com/science/article/pii/S2405829725000224
  16. https://www.sciencedirect.com/science/article/abs/pii/0379677983900887
  17. https://jcp.edpsciences.org/articles/jcp/abs/1984/01/jcp198481p847/jcp198481p847.html
  18. https://pubs.acs.org/doi/10.1021/acs.jpcc.1c00327
  19. https://pubs.acs.org/doi/10.1021/jp5026762
  20. https://pubs.acs.org/doi/10.1021/jp301369u
  21. https://www.nature.com/articles/s41598-022-13509-2
  22. https://pubs.acs.org/doi/10.1021/acs.chemrev.8b00128
  23. https://www.tandfonline.com/doi/abs/10.1080/00018730110113644
  24. https://link.springer.com/article/10.1007/BF02723512
  25. https://pmc.ncbi.nlm.nih.gov/articles/PMC8469303/
  26. https://www.sciencedirect.com/science/article/abs/pii/S0379677919301353
  27. https://pubs.acs.org/doi/10.1021/acs.chemrev.5b00287
  28. https://www.nature.com/articles/s41598-023-31342-z
  29. https://www.sciencedirect.com/science/article/abs/pii/S157243520501010X
  30. https://www.sciencedirect.com/science/article/abs/pii/S0169131717304726
  31. https://pubs.rsc.org/en/content/articlelanding/2002/jm/b204076j
  32. https://pmc.ncbi.nlm.nih.gov/articles/PMC10746094/
  33. https://www.mdpi.com/2075-163X/11/11/1211
  34. https://pubs.acs.org/doi/10.1021/acsnano.1c04423
  35. https://doi.org/10.1016/j.pmatsci.2019.100631
  36. https://pubs.acs.org/doi/10.1021/acs.chemrev.4c00805
  37. https://www.nature.com/articles/s41467-021-23369-5
  38. https://pubs.rsc.org/en/content/articlehtml/2015/ta/c5ta05226b
  39. https://www.sciencedirect.com/science/article/abs/pii/S1388248118301656
  40. https://onlinelibrary.wiley.com/doi/full/10.1002/cey2.21
  41. https://www.sciencedirect.com/science/article/abs/pii/S001346861400810X
  42. https://pubs.acs.org/doi/10.1021/acs.jpclett.6b01886
  43. https://pubs.rsc.org/en/content/articlehtml/2020/se/d0se00175a
  44. https://www.sciencedirect.com/science/article/pii/S0008622316302676
  45. https://www.nature.com/articles/s41467-021-22662-7
  46. https://www.nature.com/articles/s41467-020-16259-9
  47. https://hal.science/hal-01171774/document
  48. https://www.sciencedirect.com/science/article/pii/S2666935824000326
  49. https://pubs.acs.org/doi/10.1021/acscatal.2c01753
  50. https://advanced.onlinelibrary.wiley.com/doi/10.1002/aenm.201802565
  51. https://www.sciencedirect.com/science/article/abs/pii/S240582972200068X
  52. https://www.nature.com/articles/ncomms3995
  53. https://pubs.rsc.org/en/content/articlehtml/2024/cs/d3cs00815k
  54. https://pubs.acs.org/doi/10.1021/acsomega.2c04099
  55. https://www.sciencedirect.com/science/article/abs/pii/S245226271830031X
  56. https://www.researchgate.net/figure/Comparison-between-Bulk-and-monolayer-MoS2_tbl2_350478259
  57. https://onlinelibrary.wiley.com/doi/full/10.1002/advs.202200296
  58. https://onlinelibrary.wiley.com/doi/full/10.1002/inf2.12516
  59. https://onlinelibrary.wiley.com/doi/10.1002/adma.202103633
  60. https://www.sciencedirect.com/science/article/pii/S0020740324005836
  61. https://www.sciencedirect.com/science/article/abs/pii/S0013468604004761
  62. https://www.science.org/doi/10.1126/sciadv.aav2820
  63. https://dspace.mit.edu/bitstream/handle/1721.1/80889/857792090-MIT.pdf?sequence=2&isAllowed=y
  64. https://advanced.onlinelibrary.wiley.com/doi/full/10.1002/admi.202100596
  65. https://iopscience.iop.org/article/10.1149/2.0122001JES
  66. https://www.nature.com/articles/s41578-020-00262-6
  67. https://news.mit.edu/2025/simple-formula-could-guide-design-faster-charging-longer-lasting-batteries-1002
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