IB SL Chemistry - Nomenclature

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Cards (34)

  • Ionic compounds: Metal is named normally; non-metal’s ending is changed to ide.
  • Ionic compounds: Name to formula: criss-cross ionic charges.
  • Ionic compounds: With multivalent metals, use roman numerals to indicate charge (for name).
  • Multivalent metals: (ous means lower charge, ic means higher charge).

    +1, +2: Copper, Mercury
    +2, +3: Cobalt, Chromium, Iron
    +2, +4: Manganese, Lead, Tin
  • Polyatomic ions: 2 or more atoms bonded together (exists as a single unit).
  • Polyatomic ions: Do not change ending to ide in an ionic compound.
  • Polyatomic ions: More than 1 unit = use brackets.
  • Base form of polyatomics: ATE.
  • Nitrate (NO3-).
  • Carbonate (CO32-).
  • Sulfate (SO42-).
  • Chlorate (ClO3-).
  • Phosphate (PO43-).
  • Iodate (IO3-).
  • Bromate (BrO3-).
  • Diatomic Gases: HOFBrINCl (Hydrogen, Oxygen, Fluorine, Bromine, Iodine, Nitrogen, Chlorine).
  • Acids: Include hydrogen.
  • Binary acids: hydrogen + non-metal.
  • Binary acids: hydrogen + non-metal.
  • Binary acids: Number of hydrogens depend on charge of non-metal.
  • Acid: When non-aqueous, name like a simple ionic compounds.
  • Acid: When aqueous, form is hydro_______ic acid.
  • Ternary acids/Oxyacids: hydrogen + polyatomic ion (with oxygen).
  • Ternary acids/Oxyacids: Naming depends on derivation of oxyanion (number of oxygens)
  • Bases: includes hydroxide (OH-).
  • Bases: Use brackets if there are multiple hydroxide units.
  • Hydrates: ionic compounds + water.
  • Hydrate formula: dot is put between compound and hydrate; number of hydrates goes before hydrate, rather than subscript.
  • Hydrate naming: hydrate with greek prefix is after the compound name.
  • Acid salts: When some oxygens in oxyacid are replaced by metal ions (metal + oxyanion/polyatomic).
  • Acid Salts: If one hydrogen is added to the polyatomic, add the word hydrogen and increase charge by +1.
  • Acid Salts: If two hydrogens are added to the polyatomic, add the word dihydrogen and increase charge by +2.
  • Peroxide: Do not reduce the two.
  • Peroxide: 1 more oxygen than normal binary oxide.