{ "spore": "profile", "id": "lithium-metal", "spore_version": "0.2", "family": "lithium", "name": "Lithium metal", "abbreviation": "Li", "role": "anode", "category": "energy", "type": "lithium-metal", "summary": "Lithium metal is the lightest metal and, used as a battery anode, holds more charge per gram than any other anode material (3860 mAh/g). It is the anode in single-use (primary) lithium cells that have powered planetary probes, military radios and pacemakers, and it is the target anode for future high-energy rechargeable cells such as lithium-sulfur and solid-state batteries. Its problems are chemical: it reacts with water and air, grows needle-like dendrites when recharged, and melts at 180.5 C.\n", "best_for": "Highest charge per gram and lowest potential of any anode; primary cells that sit dormant for years before use.", "weakest_at": "Safe recharging (dendrites, short circuits, thermal runaway) and any contact with water or humid air.", "identity": { "formula": "Li", "cas": "7439-93-2", "designations": [], "source": "pubchem-lithium", "where": "Names and Identifiers > Other Identifiers > CAS" }, "tags": { "environments": [ "low-earth-orbit", "deep-space", "mars-surface", "launch", "lunar-night" ], "stresses": [ "extreme-cold", "total-radiation-dose", "vacuum-and-outgassing" ], "applications": [ "batteries", "rovers-and-surface-systems" ] }, "properties": [ { "benchmark": "theoretical_capacity", "value": 3860, "bound": "exact", "unit": "mAh/g", "scope": "material", "conditions": { "reaction": "Li to Li+, one electron per lithium atom", "electrode": "lithium metal anode" }, "method": "Value stated by the source (the source gives the number but shows no calculation)", "status": "calculated", "source": "liu-2016-ncomms", "where": "Introduction, paragraph 1", "source_detail": { "title": "Lithium-coated polymeric matrix as a minimum volume-change and dendrite-free lithium metal anode", "id": "doi:10.1038/ncomms10992", "url": "https://pmc.ncbi.nlm.nih.gov/articles/PMC4802050", "year": 2016, "kind": "paper", "license": "CC BY 4.0" } }, { "benchmark": "volumetric_capacity", "label": "Theoretical volumetric capacity", "value": 2061, "bound": "exact", "unit": "mAh/cm3", "scope": "material", "conditions": { "reaction": "Li to Li+", "electrode": "lithium metal anode" }, "method": "Calculation as stated by the source (3860 mAh/g times the density of lithium)", "status": "calculated", "note": "This source's abstract quotes a density of 0.59 g/cm3; this profile uses the 0.534 g/cm3 from PubChem. 3860 x 0.534 = 2061.", "source": "liu-2019-frontiers", "where": "Introduction, paragraph 1", "source_detail": { "title": "A Review of Carbon-Based Materials for Safe Lithium Metal Anodes", "id": "doi:10.3389/fchem.2019.00721", "url": "https://www.frontiersin.org/journals/chemistry/articles/10.3389/fchem.2019.00721/full", "year": 2019, "kind": "paper", "license": "CC BY 4.0" } }, { "benchmark": "density", "value": 0.534, "bound": "exact", "unit": "g/cm3", "scope": "material", "conditions": { "temperature": "25 C" }, "method": "Handbook value (HSDB entry reproduced in PubChem)", "status": "ground", "source": "pubchem-lithium", "where": "Chemical and Physical Properties > Experimental Properties > Density (HSDB)", "source_detail": { "title": "PubChem compound record, Lithium (CID 3028194), with HSDB, CAMEO, ICSC, ECHA C&L and ERG 2024 excerpts", "id": "PubChem CID 3028194", "url": "https://pubchem.ncbi.nlm.nih.gov/compound/3028194", "year": 2026, "kind": "database", "license": "public domain (NCBI); contributed data keep their own terms" } }, { "benchmark": "electrode_potential_she", "label": "Electrode potential versus standard hydrogen electrode", "value": -3.04, "bound": "exact", "unit": "V vs SHE", "scope": "material", "conditions": { "electrode": "lithium metal" }, "method": "Standard electrochemical potential as stated by the source", "status": "ground", "source": "liu-2016-ncomms", "where": "Introduction, paragraph 1", "source_detail": { "title": "Lithium-coated polymeric matrix as a minimum volume-change and dendrite-free lithium metal anode", "id": "doi:10.1038/ncomms10992", "url": "https://pmc.ncbi.nlm.nih.gov/articles/PMC4802050", "year": 2016, "kind": "paper", "license": "CC BY 4.0" } }, { "benchmark": "melting_point", "label": "Melting point", "value": 180.5, "bound": "exact", "unit": "C", "scope": "material", "conditions": { "pressure": "ambient" }, "method": "Handbook value", "status": "ground", "note": "PubChem lists 453.65 K (180.50 C) in the element record. Above this temperature lithium is liquid and ignites easily.", "source": "pubchem-element-lithium", "where": "Properties > Melting Point", "source_detail": { "title": "PubChem Periodic Table element record, Lithium", "id": "PubChem element 3", "url": "https://pubchem.ncbi.nlm.nih.gov/element/Lithium", "year": 2026, "kind": "database", "license": "public domain (NCBI)" } }, { "benchmark": "enthalpy_of_fusion", "label": "Enthalpy of fusion", "value": 432, "bound": "exact", "unit": "J/g", "scope": "material", "conditions": { "temperature": "at the melting point" }, "method": "Handbook value (HSDB entry reproduced in PubChem)", "status": "ground", "source": "pubchem-lithium", "where": "Chemical and Physical Properties > Experimental Properties > Melting Point (HSDB)", "source_detail": { "title": "PubChem compound record, Lithium (CID 3028194), with HSDB, CAMEO, ICSC, ECHA C&L and ERG 2024 excerpts", "id": "PubChem CID 3028194", "url": "https://pubchem.ncbi.nlm.nih.gov/compound/3028194", "year": 2026, "kind": "database", "license": "public domain (NCBI); contributed data keep their own terms" } }, { "benchmark": "electrical_resistivity", "label": "Electrical resistivity", "value": 9.446, "bound": "exact", "unit": "microohm cm", "scope": "material", "conditions": { "temperature": "20 C" }, "method": "Handbook value (HSDB entry reproduced in PubChem)", "status": "ground", "source": "pubchem-lithium", "where": "Chemical and Physical Properties > Experimental Properties > Other Experimental Properties (HSDB)", "source_detail": { "title": "PubChem compound record, Lithium (CID 3028194), with HSDB, CAMEO, ICSC, ECHA C&L and ERG 2024 excerpts", "id": "PubChem CID 3028194", "url": "https://pubchem.ncbi.nlm.nih.gov/compound/3028194", "year": 2026, "kind": "database", "license": "public domain (NCBI); contributed data keep their own terms" } }, { "benchmark": "electronic_conductivity", "value": 105865, "bound": "exact", "unit": "S/cm", "scope": "material", "conditions": { "temperature": "20 C" }, "method": "Reciprocal of the handbook resistivity of 9.446 microohm cm", "status": "calculated", "note": "Converted by the Space Mushroom editors, 1 / (9.446e-6 ohm cm). The source states resistivity only.", "source": "pubchem-lithium", "where": "Chemical and Physical Properties > Experimental Properties > Other Experimental Properties (HSDB)", "source_detail": { "title": "PubChem compound record, Lithium (CID 3028194), with HSDB, CAMEO, ICSC, ECHA C&L and ERG 2024 excerpts", "id": "PubChem CID 3028194", "url": "https://pubchem.ncbi.nlm.nih.gov/compound/3028194", "year": 2026, "kind": "database", "license": "public domain (NCBI); contributed data keep their own terms" } }, { "benchmark": "vapor_pressure", "label": "Vapor pressure", "value": 1, "bound": "exact", "unit": "hPa", "scope": "material", "conditions": { "temperature": "723 C" }, "method": "Supplier safety data sheet value", "status": "ground", "note": "The sheet gives 1 hPa (1 mmHg) at 723 C. It gives no vapor pressure near room temperature.", "source": "trace-sds-2025", "where": "Section 9, Physical and Chemical Properties", "source_detail": { "title": "Lithium Safety Data Sheet, Trace Sciences International", "id": "SDS Lithium (7 sections, CAS 7439-93-2, EC 231-102-5)", "url": "https://tracesciences.com/wp-content/uploads/2025/04/Lithium-SDS.pdf", "year": 2025, "kind": "datasheet", "license": "supplier document" } }, { "benchmark": "hardness_mohs", "label": "Mohs hardness", "value": 0.6, "bound": "exact", "unit": "Mohs", "scope": "material", "conditions": { "temperature": "room temperature, not stated by source" }, "method": "Handbook value (HSDB entry reproduced in PubChem)", "status": "ground", "note": "Soft enough to be cut with a knife; the source calls it the hardest of the alkali metals.", "source": "pubchem-lithium", "where": "Chemical and Physical Properties > Experimental Properties > Other Experimental Properties (HSDB)", "source_detail": { "title": "PubChem compound record, Lithium (CID 3028194), with HSDB, CAMEO, ICSC, ECHA C&L and ERG 2024 excerpts", "id": "PubChem CID 3028194", "url": "https://pubchem.ncbi.nlm.nih.gov/compound/3028194", "year": 2026, "kind": "database", "license": "public domain (NCBI); contributed data keep their own terms" } }, { "benchmark": "lithium_thickness_per_areal_capacity", "label": "Lithium thickness plated per mAh/cm2", "value": 4.85, "bound": "exact", "unit": "micrometre per mAh/cm2", "scope": "material", "conditions": { "basis": "bare lithium foil, fully dense" }, "method": "Thickness of lithium for 1 mAh/cm2, from the source's supplementary method", "status": "calculated", "note": "The source states \"for bare Li foil, 1 mAh cm-2 capacity represents about 4.85 um thickness of Li\". It also calls the relative volume change of hostless lithium \"virtually infinite\" (no percentage exists). The same figure follows from 1 mAh/cm2 divided by 2061 mAh/cm3.", "source": "liu-2016-ncomms", "where": "Results, \"Dendrite-free cycling with minimum volume change\" (text after Fig. 4)", "source_detail": { "title": "Lithium-coated polymeric matrix as a minimum volume-change and dendrite-free lithium metal anode", "id": "doi:10.1038/ncomms10992", "url": "https://pmc.ncbi.nlm.nih.gov/articles/PMC4802050", "year": 2016, "kind": "paper", "license": "CC BY 4.0" } }, { "benchmark": "thermal_runaway_onset", "label": "Self-heating onset (T1) in an anode-free lithium-metal pouch cell", "value": 61.5, "bound": "exact", "unit": "C", "scope": "cell", "conditions": { "cell": "NCM811 / copper anode-free pouch, 2 Ah", "state_of_charge": "100 %", "electrolyte": "1 M LiPF6 EC-DEC 1/1 by volume (LP40)", "test": "accelerating rate calorimetry, heat-wait-seek" }, "method": "Accelerating rate calorimetry (ARC)", "status": "ground", "note": "Lithium is deposited on the copper foil during charging, so this is a lithium-metal cell without a pre-built lithium foil. The temperature rate reached 10 C/min at 162.5 C (T2), maximum temperature 437.9 C (T3), peak rate about 13700 C/min.", "source": "psu-2026-jps", "where": "Section 2.2, Fig. 2a-c", "source_detail": { "title": "Impact of electrolyte and SEI passivity on thermal runaway: A comparative DSC and ARC analysis of anode-free lithium metal batteries", "id": "doi:10.1016/j.jpowsour.2026.239261", "url": "https://doi.org/10.1016/j.jpowsour.2026.239261", "year": 2026, "kind": "paper", "license": "all rights reserved (numbers cited only)" } }, { "benchmark": "thermal_runaway_trigger", "label": "Temperature where self-heating reached 10 C/min (T2) in the same cell", "value": 162.5, "bound": "exact", "unit": "C", "scope": "cell", "conditions": { "cell": "NCM811 / copper anode-free pouch, 2 Ah", "state_of_charge": "100 %", "electrolyte": "LP40" }, "method": "Accelerating rate calorimetry (ARC)", "status": "ground", "source": "psu-2026-jps", "where": "Section 2.2, Fig. 2a-c", "source_detail": { "title": "Impact of electrolyte and SEI passivity on thermal runaway: A comparative DSC and ARC analysis of anode-free lithium metal batteries", "id": "doi:10.1016/j.jpowsour.2026.239261", "url": "https://doi.org/10.1016/j.jpowsour.2026.239261", "year": 2026, "kind": "paper", "license": "all rights reserved (numbers cited only)" } }, { "benchmark": "li_electrolyte_exotherm_dsc", "label": "Lithium-electrolyte reaction peak, 1 charge cycle", "value": 180, "bound": "exact", "unit": "C", "scope": "material", "conditions": { "sample": "lithium deposited on copper foil with LP40 electrolyte", "cycles": 1, "charge_rate": "C/10", "test": "DSC" }, "method": "Differential scanning calorimetry", "status": "ground", "note": "The source says \"around 180 C\" and ties this peak to molten lithium reacting with the electrolyte.", "source": "psu-2026-jps", "where": "Section 2.3, Fig. 3a", "source_detail": { "title": "Impact of electrolyte and SEI passivity on thermal runaway: A comparative DSC and ARC analysis of anode-free lithium metal batteries", "id": "doi:10.1016/j.jpowsour.2026.239261", "url": "https://doi.org/10.1016/j.jpowsour.2026.239261", "year": 2026, "kind": "paper", "license": "all rights reserved (numbers cited only)" } }, { "benchmark": "li_electrolyte_exotherm_dsc", "label": "Lithium-electrolyte reaction peak, 20 charge cycles", "value": 140, "bound": "exact", "unit": "C", "scope": "material", "conditions": { "sample": "lithium deposited on copper foil with LP40 electrolyte", "cycles": 20, "charge_rate": "C/10", "test": "DSC" }, "method": "Differential scanning calorimetry", "status": "ground", "note": "The source says the lithium-electrolyte reaction occurs earlier, \"around 140 C\", after 20 cycles.", "source": "psu-2026-jps", "where": "Section 2.3, Fig. 3b", "source_detail": { "title": "Impact of electrolyte and SEI passivity on thermal runaway: A comparative DSC and ARC analysis of anode-free lithium metal batteries", "id": "doi:10.1016/j.jpowsour.2026.239261", "url": "https://doi.org/10.1016/j.jpowsour.2026.239261", "year": 2026, "kind": "paper", "license": "all rights reserved (numbers cited only)" } }, { "benchmark": "cycle_life", "label": "Cycles of a 350 Wh/kg Li/NMC622 pouch cell", "value": 350, "bound": "lower", "unit": "cycles", "scope": "cell", "conditions": { "cell": "lithium foil anode, NMC622 cathode, pouch format", "specific_energy": "350 Wh/kg", "enablers": "new electrolytes, thick cathode against thin lithium foil, applied cell-stack pressure" }, "method": "Cycling test reported by DOE Battery500 consortium", "status": "ground", "note": "The page says \"more than 350 cycles\". It does not give capacity-retention limit, rate or temperature, so it is not comparable with other cycle-life numbers.", "source": "doe-battery500-2020", "where": "Progress update, Figure 2 and text", "source_detail": { "title": "Battery500: Progress Update", "id": "US DOE, May 19, 2020", "url": "https://www.energy.gov/cmei/articles/battery500-progress-update", "year": 2020, "kind": "web", "license": "public domain (US Government work)" } }, { "benchmark": "cell_specific_energy", "label": "Cell specific energy, Li/SO2 D cell (Saft LO 26 SXC)", "value": 420, "bound": "exact", "unit": "Wh/kg", "scope": "cell", "conditions": { "temperature": "20 C", "current": "50 mA", "format": "D cell" }, "method": "JPL comparison table of commercial primary cells", "status": "ground", "source": "brandon-licfx-slides", "where": "Comparison of SOA vs. Advanced Cells table", "source_detail": { "title": "High Specific Energy Primary Batteries for NASA Missions (JPL one-page chart with cell comparison table)", "url": "https://smd-cms.nasa.gov/wp-content/uploads/2023/11/brandon-jpl-licfx-primary-batteries.pdf", "year": 2022, "kind": "report", "license": "public domain (NASA)" } }, { "benchmark": "cell_specific_energy", "label": "Cell specific energy, Li/SOCl2 D cell (Saft LSH 20)", "value": 421, "bound": "exact", "unit": "Wh/kg", "scope": "cell", "conditions": { "temperature": "20 C", "current": "50 mA", "format": "D cell" }, "method": "JPL comparison table of commercial primary cells", "status": "ground", "source": "brandon-licfx-slides", "where": "Comparison of SOA vs. Advanced Cells table", "source_detail": { "title": "High Specific Energy Primary Batteries for NASA Missions (JPL one-page chart with cell comparison table)", "url": "https://smd-cms.nasa.gov/wp-content/uploads/2023/11/brandon-jpl-licfx-primary-batteries.pdf", "year": 2022, "kind": "report", "license": "public domain (NASA)" } }, { "benchmark": "cell_specific_energy", "label": "Cell specific energy, Li/CFx D cell (Rayovac, Europa Lander development)", "value": 730, "bound": "exact", "unit": "Wh/kg", "scope": "cell", "conditions": { "temperature": "20 C", "current": "50 mA", "format": "D cell" }, "method": "JPL comparison table of primary cells", "status": "ground", "source": "brandon-licfx-slides", "where": "Comparison of SOA vs. Advanced Cells table", "source_detail": { "title": "High Specific Energy Primary Batteries for NASA Missions (JPL one-page chart with cell comparison table)", "url": "https://smd-cms.nasa.gov/wp-content/uploads/2023/11/brandon-jpl-licfx-primary-batteries.pdf", "year": 2022, "kind": "report", "license": "public domain (NASA)" } }, { "benchmark": "li_cfx_total_ionizing_dose", "label": "Total ionizing dose tolerated by Li/CFx primary cells", "value": 10, "bound": "lower", "unit": "Mrad", "scope": "cell", "conditions": { "cell": "Li/CFx D cells from Rayovac and EaglePicher", "testing": "radiation testing with Sandia National Laboratories" }, "method": "Radiation testing reported by JPL", "status": "ground", "note": "The abstract says \"high radiation tolerance up to 10 Mrad total ionizing doses\". The abstract does not state the capacity retained, the dose rate or the radiation source.", "source": "brandon-2022-abstract", "where": "Abstract, paragraph 2", "source_detail": { "title": "High Specific Energy Primary Batteries for NASA Missions (NASA SMD Tech Showcase abstract, E. J. Brandon, JPL)", "url": "https://science.nasa.gov/wp-content/uploads/2023/11/nasa-smd-tech-showcase-abstract-high-performance-primary-batteries-11-17-22.pdf", "year": 2022, "kind": "report", "license": "public domain (NASA)" } }, { "benchmark": "li_s_theoretical_specific_energy", "label": "Theoretical specific energy of a lithium-sulfur battery", "value": 2680, "bound": "exact", "unit": "Wh/kg", "scope": "cell", "conditions": { "anode": "lithium metal, 3860 mAh/g", "cathode": "sulfur, 1670 mAh/g" }, "method": "Value stated on a NASA slide (the slide gives the result without showing the working)", "status": "calculated", "source": "wu-2020-nasa", "where": "Slide \"Li/S - Potential High Energy Battery Chemistry\"", "source_detail": { "title": "Development of Solid-State Li/Sulfur-Selenium as Safe and High Capacity Battery (TMS 2020 invited presentation)", "id": "NTRS 20200001446", "url": "https://ntrs.nasa.gov/citations/20200001446", "year": 2020, "kind": "report", "license": "public domain (US Government work)" } } ], "corrosion": [ { "environment": "Liquid water", "headline": "Water reacts violently with lithium, giving off hydrogen and caustic lithium hydroxide, and usually ignites.", "effect": "Reacts violently, giving off hydrogen gas and a strong caustic solution (lithium hydroxide). Ignition usually occurs.", "rating": "severe", "conditions": { "form": "bulk metal; foil, ribbon and wire react relatively slowly on skin contact, powder reacts explosively" }, "source": "pubchem-lithium", "where": "Chemical and Physical Properties > Physical Description (CAMEO/USCG 1999); Stability and Reactivity > Hazardous Reactivities (HSDB)" }, { "environment": "Ambient room air (mass gain of bulk lithium)", "headline": "In room air lithium keeps taking up gas from the air.", "effect": "Lithium takes up gas from the air at several mg/h on a 1 cm2 surface at first, below 1 mg/h after one hour, about ten times slower after 24 h. A 9 mg sample had gained mass equal to complete conversion to lithium carbonate after 5 days.", "rating": "severe", "conditions": { "atmosphere": "ambient air", "surface": "about 1 cm2", "sample": "bulk lithium on a microbalance" }, "source": "hart-2016-pppl", "where": "Abstract" }, { "environment": "Room air at about 50 percent moisture (surface film growth)", "headline": "In humid air a surface film of oxides and carbonates grows at about 24 nm per minute.", "effect": "A surface layer of oxides and carbonates grows at roughly 24 nm per minute. Even after cleaning and polishing inside a glovebox, a layer a few tens of nanometres thick remains.", "rating": "severe", "conditions": { "atmosphere": "room air, about 50 % moisture", "method": "optical ellipsometry, real time" }, "source": "seo-2022-arxiv", "where": "Abstract" }, { "environment": "Dry synthetic air", "headline": "In dry air lithium still reacts, though about 30 times more slowly at first.", "effect": "The initial mass-gain rate is 30 times lower than in ambient air, but lithium still reacts. HSDB states lithium stays untarnished in dry air and does not react with oxygen at room temperature.", "rating": "moderate", "conditions": { "atmosphere": "dry synthetic air", "temperature": "room temperature" }, "source": "hart-2016-pppl", "where": "Abstract (30 times lower initial rate); PubChem HSDB excerpt for the untarnished statement" }, { "environment": "Dry air or oxygen when heated", "headline": "Heated to 100 °C or more in air or oxygen, lithium forms lithium oxide and can ignite.", "effect": "Forms lithium oxide (Li2O) when heated to 100 C or above. Clean lithium is spontaneously flammable in air if heated to 180 C. Finely divided metal may ignite in air at ambient temperature.", "rating": "severe", "conditions": { "temperature": "100 C and above; ignition at 180 C for clean surface" }, "source": "pubchem-lithium", "where": "Chemical and Physical Properties > Other Experimental Properties; Safety and Hazards > Fire Potential (HSDB)" }, { "environment": "Nitrogen gas at room temperature", "headline": "Whether lithium reacts with pure nitrogen at room temperature is disputed in the literature.", "effect": "The literature disagrees on whether lithium nitrides on contact with pure N2. In one X-ray photoelectron study no lithium nitride (Li3N) was detected at 10 mTorr or below; at 100 to 800 mTorr Li3N formed on the surface, and nitrogen stayed below 2 atomic percent because trace gases oxidize lithium first.", "rating": "low", "conditions": { "temperature": "room temperature", "pressure": "0.1 to 800 mTorr N2", "method": "ambient-pressure XPS" }, "source": "etxebarria-2025-jacs", "where": "Abstract" }, { "environment": "Nitrogen, oxygen, hydrogen or carbon dioxide at high temperature", "headline": "At high temperature lithium burns in air, oxygen, nitrogen, hydrogen and carbon dioxide.", "effect": "Lithium burns in air, oxygen, nitrogen, hydrogen and carbon dioxide. Reactions become extremely violent at higher temperatures, and molten lithium ignites more easily when oxides and nitrides are present on the surface.", "rating": "severe", "conditions": { "temperature": "molten lithium and above, no single temperature given" }, "source": "pubchem-lithium", "where": "Safety and Hazards > Stability and Reactivity > Reactivity Profile (CAMEO)" }, { "environment": "Argon glovebox", "headline": "An argon glovebox is the standard handling atmosphere, though a thin surface layer remains.", "effect": "Standard handling atmosphere (the SDS says store and handle under argon). A thin native layer of oxides and carbonates still exists on lithium prepared inside a glovebox.", "rating": "low", "conditions": { "atmosphere": "argon", "note": "layer a few tens of nm thick after chemical cleaning and mechanical polishing" }, "source": "seo-2022-arxiv", "where": "Abstract" }, { "environment": "Dry mineral oil", "headline": "Dry mineral oil is a recommended liquid for storing lithium if it is free of oxygen and water.", "effect": "Recommended liquid for storing lithium, if free of oxygen and water.", "rating": "low", "conditions": { "liquid": "mineral oil or other liquid free of oxygen or water" }, "source": "pubchem-lithium", "where": "Safety and Hazards > Handling and Storage > Storage Conditions (HSDB)" }, { "environment": "Carbonate liquid electrolyte, at room temperature", "headline": "Lithium reacts with carbonate electrolyte on contact and forms a surface film that cracks as the volume changes.", "effect": "Lithium reacts spontaneously with the solvent molecules and salt anions to form an insoluble surface layer (solid electrolyte interphase, SEI). Volume change cracks this layer, so fresh lithium is exposed and more electrolyte is consumed.", "rating": "moderate", "conditions": { "electrolyte": "carbonate-based liquid electrolyte", "temperature": "cell operating temperature, not stated" }, "source": "liu-2016-ncomms", "where": "Introduction, paragraph 2" }, { "environment": "Carbonate electrolyte (1 M LiPF6 in EC-DEC) when heated", "headline": "When heated, molten lithium reacts strongly with the electrolyte near 180 °C, and near 140 °C after 20 cycles.", "effect": "A strong exotherm from molten lithium reacting with the electrolyte appears near 180 C after 1 cycle and near 140 C after 20 cycles. A denser, inorganic-rich SEI from a localized high-concentration electrolyte pushed the reaction to a higher temperature.", "rating": "severe", "conditions": { "electrolyte": "1 M LiPF6 EC-DEC 1/1 (LP40)", "sample": "lithium deposited on copper", "test": "DSC", "heating": "see source" }, "source": "psu-2026-jps", "where": "Section 2.3, Fig. 3a-b" }, { "environment": "Copper current collector", "headline": "Copper is the most suitable current collector because it does not alloy with lithium.", "effect": "Copper is the most suitable current collector for lithium-metal anodes because it does not alloy with lithium at low potentials. Plain copper foil does not wet well with lithium (lithiophobic).", "rating": "low", "conditions": { "state": "in a cell, at lithium plating potentials" }, "source": "yang-2025-cu", "where": "Section 1, Introduction" }, { "environment": "Aluminium current collector", "headline": "Aluminium alloys with lithium at low potentials, so it is not used for lithium-metal anodes.", "effect": "Aluminium has a tendency to form alloys with lithium at low potentials, so it is not used for lithium-metal anodes.", "rating": "moderate", "conditions": { "state": "in a cell, at lithium plating potentials" }, "source": "yang-2025-cu", "where": "Section 1, Introduction" }, { "environment": "Molten lithium in contact with copper, zinc, tin or platinum", "headline": "Molten lithium dissolves copper, zinc and tin and reacts violently with platinum.", "effect": "Liquid lithium dissolves copper, zinc, tin and their alloys. Platinum and molten lithium react violently at 540 C plus or minus 20 C, forming an intermetallic compound.", "rating": "severe", "conditions": { "temperature": "above 180.5 C; platinum reaction at 540 C" }, "source": "pubchem-lithium", "where": "Chemical and Physical Properties > Melting Point (HSDB); Stability and Reactivity > Hazardous Reactivities and Incompatibilities (HSDB)" }, { "environment": "Carbon dioxide, halogenated extinguishers, sand, concrete, wood", "headline": "Burning lithium reacts with water, carbon dioxide, sand and concrete, and only dry Class D agents are suitable.", "effect": "Hot or burning lithium reacts with most extinguishing agents, including water, carbon dioxide and carbon tetrachloride, and reacts violently with concrete, wood, asphalt, sand and asbestos. Only dry Class D agents are suitable.", "rating": "severe", "conditions": { "state": "hot, molten or burning lithium" }, "source": "pubchem-lithium", "where": "Safety and Hazards > Hazards Identification > Fire Hazards (CAMEO); Fire Fighting (HSDB, ERG 2024 Guide 138)" }, { "environment": "Residual gases (H2O, CO, CO2) in a vacuum vessel", "headline": "Lithium reacts with residual gases in a vacuum vessel, though no rate is given.", "effect": "Elemental lithium reacts with these residual gases in a vacuum vessel. The paper gives no rate for vacuum conditions.", "rating": "unknown", "conditions": { "setting": "fusion-device vacuum vessel, as described in the abstract" }, "source": "hart-2016-pppl", "where": "Abstract" } ], "risks": { "hazards": [ { "text": "Classified Danger. In contact with water releases flammable gases which may ignite spontaneously (water-reactive, category 1; 100 % of ECHA notifications). Causes severe skin burns and eye damage (skin corrosion 1B; 100 %).", "ghs": [ "H260", "H314" ], "source": "pubchem-lithium", "where": "Safety and Hazards > GHS Classification (ECHA C&L, 549 reports from 7 notifications)" }, { "text": "Serious eye damage (eye damage category 1) is notified by 20.8 % of companies in ECHA C&L; the Trace Sciences SDS also lists it.", "ghs": [ "H318" ], "source": "pubchem-lithium", "where": "Safety and Hazards > GHS Classification (ECHA C&L)" }, { "text": "Transport class: UN1415, Division 4.3 (dangerous when wet), packing group I, label Dangerous When Wet.", "ghs": [], "source": "pubchem-lithium", "where": "Safety and Hazards > Hazards Identification > DOT Hazard Classification (49 CFR 172.101)" }, { "text": "Fire: molten lithium is easily ignited and difficult to extinguish. Burning lithium gives off strong alkali fumes. If lithium metal is heated to its melting point, spontaneous ignition is likely.", "ghs": [], "source": "pubchem-lithium", "where": "Safety and Hazards > Fire Hazards (CAMEO); Fire Potential (HSDB)" }, { "text": "Finely divided lithium may ignite spontaneously in air, and powder reacts explosively with water.", "ghs": [], "source": "pubchem-lithium", "where": "Safety and Hazards > Chemical Dangers (ICSC); Explosive Limits and Potential (HSDB)" }, { "text": "Corrosive to eyes, skin and respiratory tract; corrosive if swallowed; inhalation may cause lung oedema.", "ghs": [], "source": "pubchem-lithium", "where": "Safety and Hazards > Effects of Short Term Exposure (ICSC 0710)" } ], "failure_risks": [ { "mode": "Dendrite growth and internal short circuit", "trigger": "Uneven lithium deposition when a cell is recharged", "consequence": "Dendrites pierce the separator and short the cell; this can lead to thermal runaway.", "severity": "high", "source": "liu-2016-ncomms", "where": "Introduction, paragraph 2" }, { "mode": "Dendrite-driven thermal runaway in space-class cells", "trigger": "Dendrite growth during lithium plating and charge-discharge cycling", "consequence": "NASA Glenn states that dendrites can cause thermal runaway and short circuits and that reliable rechargeable lithium-metal use has not yet been achieved.", "severity": "high", "source": "wu-2019-nasa", "where": "Abstract" }, { "mode": "Thermal runaway of a charged lithium-metal pouch cell", "trigger": "Heating a fully charged anode-free NCM811/Cu cell in an adiabatic calorimeter", "consequence": "Self-heating from 61.5 C, 10 C/min at 162.5 C, a peak of 437.9 C and a rate near 13700 C/min. Cells at 0 % and 50 % charge stayed below 10 C/min. Severity rises with charge, charge rate and cycling.", "severity": "critical", "source": "psu-2026-jps", "where": "Section 2.2 and Section 2.3, Fig. 2-3" }, { "mode": "Melting of lithium and fast reaction with electrolyte", "trigger": "Cell temperature near 180 C (near 140 C after 20 cycles with the carbonate electrolyte tested)", "consequence": "Molten lithium reacts directly with the electrolyte and releases heat.", "severity": "high", "source": "psu-2026-jps", "where": "Section 2.3, Fig. 3a-b" }, { "mode": "Cracking of the SEI and loss of lithium", "trigger": "Repeated stripping and plating of hostless lithium (virtually infinite relative volume change)", "consequence": "Mechanical instability of the SEI, fresh lithium exposed to electrolyte, lower efficiency and shorter life.", "severity": "moderate", "source": "liu-2016-ncomms", "where": "Introduction, paragraph 2" }, { "mode": "Thick surface film from air exposure during cell building", "trigger": "Exposure to room air at about 50 % moisture (24 nm/min film growth)", "consequence": "The starting interface of a fabricated cell can differ from an ideal lithium/electrolyte contact.", "severity": "moderate", "source": "seo-2022-arxiv", "where": "Abstract" } ], "side_effects": [ { "text": "Dendrites pierce the separator and short-circuit the cell.", "affects": "Separator and cell", "source": "liu-2019-frontiers", "where": "The Formation Mechanism of Li Dendrites" }, { "text": "Molten or burning lithium reacts with concrete, wood, asphalt and sand, and dissolves copper, zinc and tin and their alloys.", "affects": "Fire surroundings, nearby metal parts", "source": "pubchem-lithium", "where": "Safety and Hazards > Fire Hazards (CAMEO); Melting Point (HSDB)" }, { "text": "Burning lithium produces strong alkali (corrosive) fumes; reaction with water leaves caustic lithium hydroxide.", "affects": "Nearby equipment, people, optics and surfaces exposed to the fumes", "source": "pubchem-lithium", "where": "Safety and Hazards > Hazards Identification > Fire Hazards (CAMEO)" }, { "text": "Lithium-CFx cells give off about 1 W of heat for every 1 W of electrical power delivered. This heat can keep a battery module warm, but it must be removed in a warm environment.", "affects": "Battery module thermal design", "source": "brandon-2022-abstract", "where": "Abstract" }, { "text": "A higher charge rate tends to form a more reactive lithium anode in anode-free lithium-metal cells.", "affects": "Cell safety margin", "source": "psu-2026-jps", "where": "Abstract" } ], "handling": [ { "text": "Store and handle under argon, keep the container tightly closed in a dry, well-ventilated place, and never let it contact water.", "source": "trace-sds-2025", "where": "Section 7.2" }, { "text": "Alternative storage: keep under mineral oil or another liquid free of oxygen or water; store cool and dry, separate from water.", "source": "pubchem-lithium", "where": "Safety and Hazards > Handling and Storage (HSDB, ICSC)" }, { "text": "Fire: use a Class D extinguisher or smother with dry sand, dry ground limestone or dry clay. Do not use water, foam or carbon dioxide.", "source": "trace-sds-2025", "where": "Section 5.2; PubChem ERG 2024 Guide 138 and HSDB" }, { "text": "Spill: isolate at least 25 m (75 ft) for solids; keep water away; cover with dry earth, dry sand or other non-combustible material.", "source": "pubchem-lithium", "where": "Safety and Hazards > Accidental Release Measures (ERG 2024 Guide 138)" }, { "text": "Shipping the metal: UN1415, class 4.3, packing group I.", "source": "trace-sds-2025", "where": "Section 14" }, { "text": "Shipping cells and batteries: in US rules, a lithium metal cell may contain no more than 1 g of lithium and a battery 2 g of lithium to use the small-cell exception (5 g and 25 g for highway or rail only); UN3090 is marked on such packages, and cells and batteries must pass UN Manual of Tests and Criteria section 38.3.", "source": "cfr-173-185", "where": "49 CFR 173.185 (a)(1), (c)(1)(ii), (c)(1)(iv), (c)(3)(i)" }, { "text": "Example of what a military lithium primary battery contains: the Saft BA 5590 B/U holds 24.0 g of lithium metal in a 1,000 g pack, with recommended maximum storage at +35 C.", "source": "saft-ba5590", "where": "Datasheet" }, { "text": "Personal protection: gloves, face shield, fire-retardant clothing; a German occupational limit (MAK) of 0.2 mg/m3 (inhalable fraction, as Li) is listed.", "source": "pubchem-lithium", "where": "Safety and Hazards > Exposure Control and Personal Protection (Haz-Map/DFG; HSDB)" } ], "mitigations": [ { "text": "Replace the flammable liquid electrolyte with a nonflammable solid electrolyte (garnet/ceramic or solid polymer nanocomposite) so lithium can cycle more safely. Low ionic conductivity and high interfacial impedance are the unsolved obstacles.", "source": "wu-2019-nasa", "where": "Abstract" }, { "text": "A nonflammable solid polymer composite electrolyte film tolerated current densities up to 15 mA/cm2 in lithium/lithium symmetric cells with low polarization, which indicates a stabilized lithium/polymer interface (lab result, not a flight cell).", "source": "wu-2020-nasa", "where": "Slides \"Solid Polymer Composite Electrolyte\"" }, { "text": "A localized high-concentration electrolyte forms a dense, LiF-rich SEI that postpones exotherms and lowers the maximum heating rate compared with the LP40 carbonate electrolyte.", "source": "psu-2026-jps", "where": "Highlights; Section 2.3" }, { "text": "Electrolyte additives that form a protective coating on the lithium were developed to improve cycle life and safety (NASA Tech Brief).", "source": "chen-2011-techbrief", "where": "Abstract" }, { "text": "Thin lithium foil against a thick cathode, new lithium-stable electrolytes, and applied stack pressure raised a lithium pouch cell from about 10 cycles to more than 350 cycles at 350 Wh/kg.", "source": "doe-battery500-2020", "where": "Progress update text" }, { "text": "Keep cells at a low state of charge when abuse is possible: 0 % and 50 % charged anode-free cells showed dT/dt below 10 C/min versus a violent runaway at 100 %.", "source": "psu-2026-jps", "where": "Section 2.2" }, { "text": "Pack-level protection in a fielded primary lithium battery: a fuse in each series group, a thermal fuse that opens on overheating, and a diode that blocks charging current.", "source": "saft-ba5590", "where": "Datasheet" } ] }, "uses": [ { "application": "batteries", "device": "Primary Li/SO2 battery of an atmospheric entry probe", "example": "Galileo probe to Jupiter: three battery modules with 39 D-size Li/SO2 cells, designed to keep capacity for over 50 months and then give 3 to 4 amperes for 48 minutes.", "source": "marcoux-1983", "where": "Abstract" }, { "application": "batteries", "device": "Primary Li/SO2 batteries of a lander", "example": "ESA Huygens probe: non-rechargeable lithium sulphur dioxide batteries that could stay inactive during the seven-year trip to Saturn and still had enough capacity for the Titan landing. JPL names Galileo and Huygens as heritage LiSO2 battery missions.", "source": "esa-2009-batteries", "where": "Page text" }, { "application": "rovers-and-surface-systems", "device": "Primary lithium-thionyl chloride battery of a Mars rover", "example": "Mars Pathfinder microrover: a 1996 JPL report covers requirements, cell design, battery design and test results for its Li-SOCl2 batteries.", "source": "staniewicz-1996", "where": "Abstract" }, { "application": "rovers-and-surface-systems", "device": "Primary lithium-thionyl chloride battery of a Mars penetrator probe", "example": "Deep Space 2 microprobes: a lithium-thionyl chloride primary battery of four D-size cells, two batteries wired in parallel, 600 milliamp-hours at -80 C according to the JPL page.", "source": "jpl-ds2-1999", "where": "Page text" }, { "application": "batteries", "device": "Primary Li/CFx batteries for launch-vehicle range safety and an orbital experiment", "example": "Space Shuttle solid rocket booster and external tank range-safety batteries and the orbital IECM contamination monitor used lithium carbon monofluoride batteries rated 18 ampere-hours with 13 cells per housing.", "source": "paschal-1980", "where": "Figures 1-38 and 1-43 text" }, { "application": "batteries", "device": "Primary Li/CFx battery modules for outer-planet probes and landers", "example": "JPL developed Li/CFx cells above 700 Wh/kg for the Europa Lander concept; applications named include atmospheric probes, Mars and ocean-world landers and lunar night survival. Technology readiness level 4 in 2022.", "source": "brandon-2022-abstract", "where": "Abstract" }, { "application": "batteries", "device": "Primary lithium-sulphur-chloride battery for a returnable microgravity capsule", "example": "ESA Foton M3 missions used lithium batteries (page wording: lithium-sulphuride chloride) to support microgravity experiments for more than 10 days before re-entry.", "source": "esa-2009-batteries", "where": "Page text" }, { "application": "batteries", "device": "Planned rechargeable lithium flight experiment", "example": "Lithium Battery Space Experiment (1995 Phase A study at JPL): intended as the first flight of a rechargeable lithium battery in space, to test lithium deposition and dissolution in microgravity. The paper describes the plan; this profile found no flight result.", "source": "mueller-1995", "where": "Abstract" }, { "application": "batteries", "device": "Solid-state lithium/sulfur-selenium cell under development", "example": "NASA Glenn work on a solid-state Li/S-Se battery for safe, high-capacity missions; NASA targets above 400 Wh/kg for spacesuit power and above 500 Wh/kg with more than 100 cycles for landers, rovers and habitats.", "source": "wu-2020-nasa", "where": "Slide \"NASA Demands Very High Specific Energy Batteries\"" }, { "application": "batteries", "device": "Military radio battery (Li/SO2)", "example": "Saft BA 5590 B/U 12 V/24 V pack for AN/PRC-104, -113, -117 and -119 radios and other military equipment, operating from -40 C to +71 C.", "source": "saft-ba5590", "where": "Datasheet, typical applications" }, { "application": "batteries", "device": "Implantable pacemaker cell (lithium/iodine)", "example": "Lithium-iodide batteries replaced mercury-zinc cells in pacemakers; the new cell had a life of 10 years compared with 2 years.", "source": "barold-2011", "where": "Pages 718-719" } ], "supply": [ { "subject": "Lithium", "abundance": "Estimated crustal abundance 2.0x10^1 mg/kg (about 20 parts per million) and oceanic abundance 1.8x10^-1 mg/L (PubChem). World reserves 37,000,000 t of lithium content; largest: Chile 9,200,000 t, Australia 8,400,000 t, China 4,600,000 t, Argentina 4,400,000 t, United States 4,400,000 t. Measured and indicated resources about 150 million tons (USGS, 2026). Estimated world end use: batteries 88 %, ceramics and glass 4 %, lubricating greases 2 %.", "producers": [ { "country": "Australia", "share_percent": 31.7, "year": 2025 }, { "country": "China", "share_percent": 21.4, "year": 2025 }, { "country": "Chile", "share_percent": 19.3, "year": 2025 }, { "country": "Zimbabwe", "share_percent": 9.7, "year": 2025 }, { "country": "Argentina", "share_percent": 7.9, "year": 2025 }, { "country": "Brazil", "share_percent": 4.1, "year": 2025 }, { "country": "Mali", "share_percent": 3.2, "year": 2025 }, { "country": "Canada", "share_percent": 1.9, "year": 2025 }, { "country": "Portugal", "share_percent": 0.1, "year": 2025 } ], "critical_lists": [ { "list": "USGS 2025 final list of critical minerals (60 minerals)", "listed": true }, { "list": "EU critical raw materials list (CRMA, 34 materials)", "listed": true }, { "list": "EU strategic raw materials list (CRMA), entry 'Lithium - battery grade'", "listed": true } ], "recycling": "USGS 2026: construction of lithium battery recycling plants continued throughout 2025, and automobile companies partnered with battery recyclers to supply battery materials. No recycled-share figure is given.", "substitutes": [ "Calcium, magnesium, mercury and zinc as anode material in primary batteries (USGS)", "Calcium and aluminum soaps for stearates in greases", "Sodic and potassic fluxes in ceramics and glass" ], "source": "usgs-mcs-2026", "where": "Critical lists: USGS final 2025 list (usgs.gov news item of Nov 14 2025, lithium named as used in rechargeable batteries) and EU JRC RMIS page rmis.jrc.ec.europa.eu/eu-critical-raw-materials (lithium on the 34-item critical list; 'Lithium - battery grade' on the 16-item strategic list). Lithium chapter, World Mine Production and Reserves table; Substitutes; Recycling. Shares computed by the editors from 2025 mine production (e) divided by the 290,000 t world total (which excludes U.S. production)." } ], "media": [ { "file": "/media/lithium/lithium-metal-1.jpg", "caption": "Purified lithium metal sealed in a glass ampoule under argon.", "shows": "Silvery lithium pieces, some with a dull crust, in a sealed glass ampoule. Lithium is stored under argon or under oil because it reacts with air and water.", "conditions": "Lithium purified by distillation under high vacuum, then sealed under argon (uploader's description); photo at room temperature", "alt": "A clear glass ampoule on a white surface holding shiny silver-grey chunks and flakes of lithium metal.", "credit": "AdvancedTinkering", "license": "CC BY-SA 4.0", "license_url": "https://creativecommons.org/licenses/by-sa/4.0/", "source_url": "https://commons.wikimedia.org/wiki/File:Purified_lithium_in_an_ampoule_under_argon.png" }, { "file": "/media/lithium/lithium-metal-2.jpg", "caption": "Scanning electron micrographs of cycled lithium electrodes; the bare lithium electrode (panels d and e) is covered in mossy dendrites.", "shows": "Figure 4 of Liu et al. 2016. Panels a-c: a lithium-coated polymer matrix after 10 cycles at 1, 3 and 5 mA/cm2 (the uniform fibres are the host matrix, not dendrites). Panels d-e: a bare lithium electrode after 10 cycles at 1 mA/cm2 with large amounts of mossy dendrites. Panels f-g: cross-sections of the matrix electrode before and after stripping.", "conditions": "SEM, top view; 10 stripping/plating cycles in EC/DEC electrolyte; scale bars 10 um (a-d), 5 um (e), 200 um (f-g)", "alt": "Seven grey scanning electron microscope images in a grid. Top row: fibrous matrix surfaces at three current densities. Bottom row: tangled mossy lithium dendrites on bare lithium, and two cross-sections of an electrode about 250 micrometres thick.", "credit": "Yayuan Liu, Dingchang Lin, Zheng Liang, Jie Zhao, Kai Yan and Yi Cui, Nature Communications 7:10992 (2016)", "license": "CC BY 4.0", "license_url": "https://creativecommons.org/licenses/by/4.0/", "source_url": "https://pmc.ncbi.nlm.nih.gov/articles/PMC4802050/" }, { "file": "/media/lithium/lithium-metal-3.jpg", "caption": "Lithium metal stored in paraffin oil.", "shows": "Cut pieces of lithium with bright metallic faces submerged in clear oil, the traditional way to keep lithium away from air and moisture.", "conditions": "Photograph, room temperature, lithium in paraffin oil (uploader's description)", "alt": "Several rectangular silver-grey pieces of lithium metal sitting in a glass jar filled with clear oil.", "credit": "Tomihahndorf (German Wikipedia)", "license": "Public domain", "license_url": "https://commons.wikimedia.org/wiki/File:Lithium_paraffin.jpg", "source_url": "https://commons.wikimedia.org/wiki/File:Lithium_paraffin.jpg" } ], "documents": [ { "title": "Lithium safety data sheet (Trace Sciences International)", "type": "sds", "url": "https://tracesciences.com/wp-content/uploads/2025/04/Lithium-SDS.pdf", "year": 2025 }, { "title": "PubChem: Lithium (CID 3028194), hazard and safety record", "type": "database", "url": "https://pubchem.ncbi.nlm.nih.gov/compound/3028194" }, { "title": "USGS Mineral Commodity Summaries 2026: Lithium", "type": "report", "url": "https://pubs.usgs.gov/periodicals/mcs2026/mcs2026-lithium.pdf", "year": 2026 }, { "title": "Lithium-coated polymeric matrix as a minimum volume-change and dendrite-free lithium metal anode (Nature Communications, open access)", "type": "paper", "url": "https://pmc.ncbi.nlm.nih.gov/articles/PMC4802050", "year": 2016 }, { "title": "NASA Glenn: Development of Solid-State Li/Sulfur-Selenium as Safe and High Capacity Battery", "type": "report", "url": "https://ntrs.nasa.gov/citations/20200001446", "year": 2020 }, { "title": "JPL: High Specific Energy Primary Batteries for NASA Missions", "type": "report", "url": "https://science.nasa.gov/wp-content/uploads/2023/11/nasa-smd-tech-showcase-abstract-high-performance-primary-batteries-11-17-22.pdf", "year": 2022 }, { "title": "NIST Atomic Weights and Isotopic Compositions for All Elements", "type": "database", "url": "https://physics.nist.gov/cgi-bin/Compositions/stand_alone.pl", "year": 2026 } ], "gaps": [ "Crystal system and space group of lithium: no source opened for this profile, so left out.", "Volume change on stripping and plating as a percentage: sources only say 'virtually infinite' (hostless anode); only the calculated 4.85 micrometres per mAh/cm2 is given.", "Practical (measured) reversible capacity of a lithium-metal anode and average voltage versus Li/Li+: no source read; lithium is the Li/Li+ reference by definition.", "Gas evolution from lithium metal in cells: no open source with numbers found (a preprint reports methane in ether electrolytes; not used).", "Corrosion of lithium by nickel, stainless steel and other current-collector metals, and by dry air at stated dew points: no sourced data found.", "Vacuum behaviour of lithium metal at room temperature (sublimation, outgassing): only a vapor pressure at 723 C was found; the PPPL paper mentions residual gases in a vacuum vessel but gives no vacuum rate.", "Rechargeable lithium-metal cell flight data: the 1995 Lithium Battery Space Experiment is a plan in the abstract; no result was found. No lithium-metal rechargeable cell flight record found.", "Radiation, cold and thermal-vacuum data exist only for primary cells (Li/CFx up to 10 Mrad; DS2 600 mAh at -80 C; Li/CFx batteries tested at 1e-6 torr); none for lithium-metal secondary cells.", "Lithium-iodine pacemaker cell and Li/SOCl2 cells: only abstracts and short pages opened; no cell-level performance numbers recorded.", "Recycled share of lithium supply and primary-source text of EU Regulation 2024/1252 Annexes: not read directly (EU lists confirmed through the JRC RMIS page)." ], "story": { "why": "Lithium metal is the lightest metal, and as a battery anode it holds more charge per gram than any other anode material, 3,860 mAh/g. It is the anode in single-use (primary) lithium cells that have powered planetary probes, military radios and pacemakers, and it is the target anode for future high-energy rechargeable cells such as lithium-sulfur and solid-state batteries. Its difficulties are chemical. It reacts with water and air, it grows needle-like dendrites when recharged, and it melts at 180.5 °C, which is within the range a failing cell can reach.", "uses": [ { "where": "Planetary probes", "line": "The Galileo probe to Jupiter carried three battery modules with 39 D-size lithium/sulfur dioxide cells, designed to keep their capacity for over 50 months and then deliver 3 to 4 amperes for 48 minutes. The Huygens probe used non-rechargeable lithium sulfur dioxide batteries that sat inactive during a seven-year trip to Saturn and still had enough capacity for the Titan landing." }, { "where": "Mars landers and penetrators", "line": "The Mars Pathfinder microrover used lithium-thionyl chloride batteries. The Deep Space 2 microprobes used a lithium-thionyl chloride primary battery of four D-size cells, rated at 600 mAh at -80 °C according to JPL." }, { "where": "Launch vehicles and orbital experiments", "line": "The Space Shuttle solid rocket booster and external tank range-safety batteries, and the orbital IECM contamination monitor, used lithium carbon monofluoride batteries rated 18 ampere-hours with 13 cells per housing. JPL has developed Li/CFx cells above 700 Wh/kg for the Europa Lander concept, at technology readiness level 4 in 2022." }, { "where": "Military radios and pacemakers", "line": "The Saft BA 5590 B/U lithium/sulfur dioxide pack powers radios and other military equipment from -40 °C to +71 °C. Lithium-iodine cells replaced mercury-zinc cells in pacemakers, with a life of 10 years against 2 years." }, { "where": "Rechargeable cells, still under development", "line": "NASA Glenn is working on a solid-state lithium/sulfur-selenium cell. NASA targets above 400 Wh/kg for spacesuit power and above 500 Wh/kg with more than 100 cycles for landers, rovers and habitats. A 1995 JPL study planned the first flight of a rechargeable lithium battery in space, and this profile found no flight result." } ], "can_do": [ { "label": "Capacity", "line": "The theoretical specific capacity of 3,860 mAh/g comes from the reaction of lithium to Li⁺ with one electron per atom. At a density of 0.534 g/cm³ this gives 2,061 mAh/cm³. The standard electrode potential is -3.04 V versus the standard hydrogen electrode, the lowest of any anode.", "scope": "material", "value": "3,860 mAh/g" }, { "label": "Energy in primary cells", "line": "In a JPL comparison of D-size primary cells at 20 °C and 50 mA, commercial lithium cells delivered 420 and 421 Wh/kg, and another primary cell type delivered 730 Wh/kg. The theoretical specific energy of a lithium-sulfur cell, from a NASA slide, is 2,680 Wh/kg.", "scope": "material", "value": "420 to 730 Wh/kg" }, { "label": "Melting", "line": "Lithium melts at 180.5 °C, and the heat of fusion is 432 J/g. Above this temperature it is liquid and ignites easily. In calorimetry of lithium deposited on copper with a carbonate electrolyte, a strong exotherm from molten lithium reacting with the electrolyte appeared near 180 °C after 1 cycle and near 140 °C after 20 cycles.", "scope": "material", "value": "180.5 °C" }, { "label": "A rechargeable cell", "line": "A lithium foil anode with an NMC622 cathode in a pouch cell reached more than 350 cycles at 350 Wh/kg in a DOE Battery500 test, up from about 10 cycles, using thin lithium against a thick cathode, new electrolytes and applied pressure. The page gives no retention limit, rate or temperature, so the figure is indicative only.", "scope": "material", "value": "More than 350 cycles" }, { "label": "Radiation", "line": "JPL reports high radiation tolerance for lithium/carbon monofluoride D cells up to total ionizing doses of 10 Mrad, tested with Sandia National Laboratories.", "scope": "material", "value": "Up to 10 Mrad" } ], "compare": "Lithium metal is not a cathode, so the table cannot compare it with LFP, NMC, LCO or NCA. It is the anode of the collection with the highest charge per gram, 3,860 mAh/g against 372 mAh/g for graphite and 175 mAh/g for lithium titanate, and the one that is hardest to use safely.", "compare_rows": [ { "label": "Density", "benchmark": "density", "scope": "material" }, { "label": "Melting point", "benchmark": "melting_point", "scope": "material" }, { "label": "Electrical resistivity", "benchmark": "electrical_resistivity", "scope": "material" } ], "handling": [], "good_for": [ "The highest charge per gram and the lowest potential of any anode.", "Primary cells that sit dormant for years before use, which is why they power probes, military radios and pacemakers." ], "watch_out": [ "Safe recharging is unsolved. Dendrites can pierce the separator and short the cell, which can lead to thermal runaway.", "It reacts violently with water and keeps reacting with air, so it must be handled under argon or mineral oil.", "It melts at 180.5 °C, and molten lithium reacts directly with the electrolyte and releases heat." ], "verdict": "Lithium metal is the highest-capacity anode and the most demanding one. It is proven in single-use cells and not yet in rechargeable ones.", "recipe": { "line": "Lithium metal is the pure element, Li, with one atom per formula unit. It is not a compound or alloy in this profile.", "parts": [ { "name": "Lithium", "symbol": "Li", "role": "The only element in the anode. NIST gives a range for natural abundance; 6.94 is the rounded value used in the LFP profile.", "atoms": 1, "atomic_weight": 6.94 } ] }, "risk_groups": [ { "title": "For people", "lead": "Lithium metal is classified Danger. It is water-reactive and corrosive.", "points": [ { "label": "Hazard classification", "line": "In contact with water it releases flammable gases that may ignite spontaneously (water-reactive category 1, in 100% of ECHA notifications). It causes severe skin burns and eye damage (skin corrosion 1B, in 100%). Serious eye damage category 1 is notified by 20.8% of companies." }, { "label": "Dust and powder", "line": "Finely divided lithium may ignite spontaneously in air, and the powder reacts explosively with water." }, { "label": "Corrosive effects", "line": "It is corrosive to the eyes, skin and respiratory tract, and corrosive if swallowed. Inhalation may cause lung oedema." }, { "label": "Fire", "line": "Molten lithium is easily ignited and difficult to extinguish. Burning lithium gives off strong alkali fumes, and spontaneous ignition is likely if the metal is heated to its melting point. Only dry Class D agents are suitable. Water, foam and carbon dioxide must not be used, and sand and concrete can also react." }, { "label": "Protection", "line": "The safety data sheet calls for gloves, a face shield and fire-retardant clothing. A German occupational limit of 0.2 mg/m³ (inhalable fraction, as Li) is listed." } ], "level": 4, "verdict": "Corrosive and water-reactive" }, { "title": "If a cell overheats", "lead": "These results come from laboratory tests, not from incidents in the field.", "points": [ { "label": "A charged lithium-metal cell", "line": "A fully charged 2 Ah NCM811/copper pouch cell, heated in an adiabatic calorimeter, began to heat itself at 61.5 °C and reached 10 °C/min at 162.5 °C. The peak was 437.9 °C, at a rate near 13,700 °C/min. Cells at 0% and 50% charge stayed below 10 °C/min. Severity rises with charge, charge rate and cycling." }, { "label": "Dendrites", "line": "Uneven lithium deposition when a cell is recharged forms dendrites that pierce the separator and short the cell. NASA Glenn states that this can lead to thermal runaway and that reliable rechargeable lithium-metal use has not yet been achieved." }, { "label": "Melting", "line": "Near 180 °C, or near 140 °C after 20 cycles with the carbonate electrolyte tested, molten lithium reacts directly with the electrolyte and releases heat." }, { "label": "Heat from the cell", "line": "Lithium-CFx cells give off about 1 W of heat for every 1 W of electrical power delivered. This heat can keep a battery module warm, but it must be removed in a warm environment." } ] }, { "title": "Handling and storage", "points": [ { "label": "Storage", "line": "Store and handle under argon in a tightly closed container in a dry, well-ventilated place. Mineral oil or another liquid free of oxygen and water is an alternative. Never let it contact water." }, { "label": "Spills", "line": "Isolate at least 25 m (75 ft) for solids, keep water away, and cover with dry earth, dry sand or another non-combustible material." }, { "label": "Shipping", "line": "The metal ships as UN1415, class 4.3, packing group I. Under US rules a cell may contain no more than 1 g of lithium and a battery 2 g to use the small-cell exception, and cells must pass UN Manual of Tests and Criteria section 38.3." }, { "label": "In cells", "line": "Pack-level protection in a fielded primary battery is a fuse in each series group, a thermal fuse that opens on overheating, and a diode that blocks charging current. Keeping cells at a low state of charge when abuse is possible greatly reduces the severity of runaway." }, { "label": "Safer designs", "line": "A nonflammable solid electrolyte lets lithium cycle more safely, although low ionic conductivity and high interfacial impedance are unsolved. A localized high-concentration electrolyte forms a dense, LiF-rich surface film that postpones exotherms." } ] } ] }, "updated": "2026-10-16", "review": { "status": "draft", "method": "assistant", "checked_values": 17, "unreachable": 4, "caveats": 2, "note": "Re-read by an AI assistant on 2026-10-16: 17 of 21 benchmark values match their cited source; 4 could not be opened; 0 did not match." }, "sources": { "usgs-mcs-2026": { "title": "Mineral Commodity Summaries 2026, Lithium (Brian W. Jaskula; contact Andrew A. 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