{
  "node": {
    "id": "term:high-concentration-electrolyte",
    "type": "Term",
    "label": "High-concentration electrolyte",
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      "id": "high-concentration-electrolyte",
      "name": "High-concentration electrolyte",
      "abbr": "HCE",
      "aka": [
        "superconcentrated electrolyte",
        "localised high-concentration electrolyte",
        "LHCE",
        "water-in-salt electrolyte"
      ],
      "section": "topic-electrolytes",
      "definition": "An electrolyte with so much salt, often 3–5 mol/L instead of the usual 1, that nearly every solvent molecule is bound to a lithium ion. Anions then decompose first and build a robust inorganic interphase, and oxidation stability rises. Viscosity and cost are high, so localised versions dilute it with a non-solvating fluorinated ether that keeps the clustered solvation structure.",
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        "lithium-salt",
        "solvation",
        "fluorinated-electrolyte",
        "lifsi",
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        "acetonitrile-electrolyte"
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        "oxidation"
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      "label": "Electrolytes and separators",
      "properties": {
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        "name": "Electrolytes and separators",
        "lede": "What sits between the electrodes: liquid, gel and solid electrolytes, their salts, solvents and additives, and the separator that keeps the electrodes apart.",
        "context": "Connect transport with electronic isolation.",
        "example": "Greater liquid uptake may improve wetting while changing mechanical behavior. Several properties define separator performance.",
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      "id": "term:lithium-salt",
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      "label": "Lithium salt",
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        "definition": "The dissolved salt that supplies the mobile lithium ions in a liquid electrolyte, almost always lithium hexafluorophosphate, LiPF₆, at about one mole per litre. It reacts with traces of water to form hydrofluoric acid, which is why cells are filled in a dry room.",
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        "definition": "A lithium ion in a liquid electrolyte travels wrapped in a shell of solvent molecules and must shed it, at an energy cost, before entering graphite. Desolvation is a large part of charge-transfer resistance, especially in the cold.",
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      "id": "term:fluorinated-electrolyte",
      "type": "Term",
      "label": "Fluorinated electrolyte",
      "properties": {
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        "name": "Fluorinated electrolyte",
        "aka": [
          "fluorinated solvent",
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        "definition": "An electrolyte whose solvents largely carry fluorine — fluorinated carbonates such as FEC, or fluorinated ethers used as diluents. Fluorine draws electron density from the solvent, raising its oxidation stability towards 5 V, and its reduction leaves a lithium-fluoride-rich SEI. That suits high-voltage cathodes and lithium metal, at higher cost and with PFAS concerns.",
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          "oxidation",
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      "id": "term:lifsi",
      "type": "Term",
      "label": "Lithium bis(fluorosulfonyl)imide",
      "properties": {
        "id": "lifsi",
        "name": "Lithium bis(fluorosulfonyl)imide",
        "abbr": "LiFSI",
        "section": "topic-electrolytes",
        "definition": "A salt with higher conductivity and far better thermal and moisture stability than LiPF₆, increasingly blended with it or used in fast-charge and lithium-metal electrolytes. Its drawback is corrosion of aluminium at high voltage unless LiPF₆ is also present.",
        "related": [
          "lipf6",
          "lithium-salt",
          "litfsi",
          "fast-charging"
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        "mentions": []
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    {
      "id": "term:aqueous-battery",
      "type": "Term",
      "label": "Aqueous battery",
      "properties": {
        "id": "aqueous-battery",
        "name": "Aqueous battery",
        "aka": [
          "water-based battery",
          "aqueous electrolyte battery"
        ],
        "section": "topic-other-chemistries",
        "definition": "Any battery whose electrolyte is water-based, from lead–acid and nickel–metal hydride to aqueous zinc-ion and sodium-ion designs. Water is cheap, non-flammable and highly conductive, but it splits at 1.23 V in theory and around 2 V in practice, which caps cell voltage and energy density.",
        "related": [
          "lead-acid",
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        "mentions": [
          "electrolyte",
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          "cell-voltage"
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    },
    {
      "id": "term:acetonitrile-electrolyte",
      "type": "Term",
      "label": "Acetonitrile electrolyte",
      "properties": {
        "id": "acetonitrile-electrolyte",
        "name": "Acetonitrile electrolyte",
        "abbr": "AN",
        "aka": [
          "acetonitrile",
          "CH₃CN",
          "nitrile electrolyte"
        ],
        "section": "topic-electrolytes",
        "definition": "An electrolyte based on acetonitrile, CH₃CN, a solvent of very low viscosity and high polarity that gives excellent ionic conductivity. It is standard in supercapacitors, but in lithium-ion cells it is reduced on graphite unless the salt is superconcentrated, an approach shown to allow very fast charging. It is flammable and toxic.",
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        "url": "https://lemonergy.com/learn/glossary/acetonitrile-electrolyte/",
        "mentions": [
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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.",
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        "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": "term:oxidation",
      "type": "Term",
      "label": "Oxidation",
      "properties": {
        "id": "oxidation",
        "name": "Oxidation",
        "section": "topic-electrochemistry",
        "definition": "Loss of electrons by a species. On discharge the negative electrode is oxidised as lithium leaves it as Li⁺, which is why that electrode is called the anode.",
        "related": [
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