Electrochemistry: Glossary
Electrochemic Two half cells combined. Two electrodes are separated by an electrolyte.
al Cell The cells are used to measure the electrode potentials in reference to the
standard hydrogen electrode potential.
Important as electrode potentials cannot be measured directly so two half
cells must be combined.
Electrode A conductor through which electricity leaves and enters.
Electrolyte Medium which contains ions.
Electrochemic The list of electrode potentials in numerical form.
al Series
EMF The difference between the potential differences of the cathode and anode
in an electrochemical cell.
E cell E cell is a measure of how far from equilibrium the cell reaction lies. The
more positive the E cell the more likely the reaction is to occur.
Standard Has an electrode potential of 0V by definition. It is used to calculate the
Hydrogen electrode potentials of other cells.
Electrode
Standard When an electrode system is connected to the hydrogen electrode system,
Electrode and standard conditions apply the potential difference measured is called
Potential the standard electrode potential.
Salt Bridge Soaked with a solution of an inert strong electrolyte, e.g. a filter paper
soaked in KNO3. The salt ions flow through the bridge to complete the cell
and balance charges in solutions.
Must not react with the electrolyte.
Rechargeable Cells in which reversible reactions can occur with the
Cell
Non- Cell in which reacts are not reversible. Can only be used once.
rechargeable
Cell
Electrochemic Two half cells combined. Two electrodes are separated by an electrolyte.
al Cell The cells are used to measure the electrode potentials in reference to the
standard hydrogen electrode potential.
Important as electrode potentials cannot be measured directly so two half
cells must be combined.
Electrode A conductor through which electricity leaves and enters.
Electrolyte Medium which contains ions.
Electrochemic The list of electrode potentials in numerical form.
al Series
EMF The difference between the potential differences of the cathode and anode
in an electrochemical cell.
E cell E cell is a measure of how far from equilibrium the cell reaction lies. The
more positive the E cell the more likely the reaction is to occur.
Standard Has an electrode potential of 0V by definition. It is used to calculate the
Hydrogen electrode potentials of other cells.
Electrode
Standard When an electrode system is connected to the hydrogen electrode system,
Electrode and standard conditions apply the potential difference measured is called
Potential the standard electrode potential.
Salt Bridge Soaked with a solution of an inert strong electrolyte, e.g. a filter paper
soaked in KNO3. The salt ions flow through the bridge to complete the cell
and balance charges in solutions.
Must not react with the electrolyte.
Rechargeable Cells in which reversible reactions can occur with the
Cell
Non- Cell in which reacts are not reversible. Can only be used once.
rechargeable
Cell
