{
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    "id": "term:electrode-potential",
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    "label": "Electrode potential",
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      "id": "electrode-potential",
      "name": "Electrode potential",
      "section": "topic-electrochemistry",
      "definition": "The potential of an electrode relative to a reference, which for lithium-ion work is lithium metal in the same electrolyte, written as V vs Li/Li⁺. Graphite sits near 0.1 V and layered oxides near 3.7–4.3 V on this scale.",
      "unit": "V vs Li/Li⁺",
      "related": [
        "standard-potential",
        "cell-voltage",
        "reference-electrode",
        "half-reaction"
      ],
      "lesson": "labs/battery-materials-lab/#battery-materials-lab",
      "url": "https://lemonergy.com/learn/glossary/electrode-potential/",
      "mentions": [
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        "graphite",
        "electrolyte"
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      "id": "topic:topic-electrochemistry",
      "type": "Topic",
      "label": "Electrochemistry fundamentals",
      "properties": {
        "id": "topic-electrochemistry",
        "name": "Electrochemistry fundamentals",
        "lede": "The reactions and potentials that make a cell a battery.",
        "context": "Connect reaction sites and transport paths.",
        "example": "A circuit can predict terminal voltage while leaving electrode potentials and reaction kinetics unresolved.",
        "lesson_url": "https://lemonergy.com/learn/fundamentals/cell-anatomy/",
        "lesson_label": "Open cell anatomy"
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      "id": "term:standard-potential",
      "type": "Term",
      "label": "Standard electrode potential",
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        "id": "standard-potential",
        "name": "Standard electrode potential",
        "abbr": "E°",
        "section": "topic-electrochemistry",
        "definition": "An electrode’s potential under standard conditions, tabulated against the standard hydrogen electrode. Lithium’s −3.04 V is the most negative of any metal, which is why lithium cells have the highest voltages.",
        "unit": "V",
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          "electrode-potential",
          "nernst-equation",
          "cell-voltage"
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      "id": "term:cell-voltage",
      "type": "Term",
      "label": "Cell voltage",
      "properties": {
        "id": "cell-voltage",
        "name": "Cell voltage",
        "aka": [
          "electromotive force",
          "EMF"
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        "section": "topic-electrochemistry",
        "definition": "The difference between the positive and negative electrode potentials at equilibrium: for NMC against graphite about 3.7 V. It is set by the chemistry, and the difference in Gibbs free energy of the cell reaction per unit charge.",
        "formula": "E = E₊ − E₋ = −ΔG / nF",
        "unit": "V",
        "related": [
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          "gibbs-free-energy",
          "open-circuit-voltage",
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          "title": "Subtract equilibrium electrode potentials",
          "text": "If two illustrative electrode potentials are 4.0 V and 0.2 V versus the same reference, their equilibrium cell voltage is 3.8 V. Under load, resistance and polarization change the measured terminal voltage."
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      "properties": {
        "id": "reference-electrode",
        "name": "Reference electrode",
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        "definition": "An electrode of stable, known potential against which another is measured. In lithium-ion work it is a piece of lithium metal, which defines the Li/Li⁺ scale; outside it the standard hydrogen electrode is the primary reference.",
        "related": [
          "three-electrode-cell",
          "electrode-potential",
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      "label": "Half-reaction",
      "properties": {
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        "name": "Half-reaction",
        "aka": [
          "half-cell reaction"
        ],
        "section": "topic-electrochemistry",
        "definition": "The oxidation or reduction occurring at one electrode, written on its own with electrons shown explicitly. The cell reaction is the sum of its two half-reactions, and the cell voltage is the difference of their potentials.",
        "related": [
          "redox-reaction",
          "electrode-potential",
          "half-cell",
          "cell-voltage"
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        "lesson": "labs/battery-materials-lab/#bml-liion-mechanism",
        "url": "https://lemonergy.com/learn/glossary/half-reaction/",
        "mentions": [
          "electrode",
          "oxidation",
          "reduction"
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      "id": "term:electrode",
      "type": "Term",
      "label": "Electrode",
      "properties": {
        "id": "electrode",
        "name": "Electrode",
        "section": "topic-components",
        "definition": "A solid conductor where the cell’s reaction happens, in contact with the electrolyte. A lithium-ion cell has a negative electrode and a positive electrode, each a porous coating on a metal foil.",
        "related": [
          "negative-electrode",
          "positive-electrode",
          "porous-electrode",
          "current-collector"
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        "example": {
          "title": "Two transport paths",
          "text": "Electrons need connected solid paths to the collector; ions need electrolyte paths to reaction sites. More of one constituent displaces others at fixed volume."
        },
        "url": "https://lemonergy.com/learn/glossary/electrode/",
        "mentions": [
          "electrolyte",
          "coating"
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    {
      "id": "term:graphite",
      "type": "Term",
      "label": "Graphite",
      "properties": {
        "id": "graphite",
        "name": "Graphite",
        "section": "topic-components",
        "definition": "Layered carbon, the negative active material of nearly all lithium-ion cells. Lithium intercalates between its layers up to LiC₆, a theoretical 372 mAh/g, at a potential about 0.1 V above lithium metal.",
        "related": [
          "anode-active-material",
          "intercalation",
          "natural-graphite",
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          "lithium-plating"
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          "title": "Compare matching mass bases",
          "text": "A graphite value per gram of active material cannot be directly compared with a value including binder, additive and foil."
        },
        "url": "https://lemonergy.com/learn/glossary/graphite/",
        "mentions": [
          "milliampere-hour",
          "active-material"
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      "id": "term:electrolyte",
      "type": "Term",
      "label": "Electrolyte",
      "properties": {
        "id": "electrolyte",
        "name": "Electrolyte",
        "section": "topic-electrolytes",
        "definition": "The ion-conducting medium between the electrodes. In a liquid-electrolyte cell it fills the pores of both electrodes and the separator, so it is not a separate structural layer.",
        "related": [
          "lithium-salt",
          "carbonate-solvent",
          "electrolyte-additive",
          "ionic-conductivity",
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          "ionic-liquid-electrolyte"
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        "lesson": "fundamentals/cell-architecture/#electrolyte",
        "example": {
          "title": "Ions and electrons",
          "text": "Electrolyte carries ions between electrodes; the external circuit carries electrons. The two paths serve different roles."
        },
        "url": "https://lemonergy.com/learn/glossary/electrolyte/",
        "mentions": [
          "separator"
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      "id": "lesson:labs/battery-materials-lab/",
      "type": "Lesson",
      "label": "Battery materials lab",
      "properties": {
        "url": "https://lemonergy.com/learn/labs/battery-materials-lab/"
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    {
      "id": "reference:iupac-nernst",
      "type": "Reference",
      "label": "Nernst equation",
      "properties": {
        "title": "Nernst equation",
        "publisher": "IUPAC Gold Book",
        "url": "https://goldbook.iupac.org/terms/view/09068",
        "type": "Terminology reference",
        "scope": "Equilibrium potential as a function of activities; distinguishes activities from concentration approximations.",
        "year": 2025,
        "accessed": "2026-10-27"
      }
    }
  ]
}