Table 2.
Concepts related to electrochemistry which may form part of the 11–18 curriculum in high schools worldwide
| Concept | Illustration |
|---|---|
| Reactivity series | Simple list of the relative reactivity of metals (perhaps including carbon and hydrogen) |
| Metal displacement reactions | Use of a simple reactivity series of metals to predict displacement reactions, e.g. metal + metal salt |
| Redox in terms of electrons | OIL RIG definition |
| Half equations | Construction of simple half equations requiring balancing of atoms and electrons (not inclusion of H+/OH−/H2O) |
| Electrolysis of molten salts | Electrolysis of molten salts |
| Electrolysis of solutions | Electrolysis of soluble salts, e.g. sodium chloride |
| Faraday calculations | F = Le, where F is the Faraday constant, L is the Avogadro constant, and e is the charge on an electron (in terms of the number of coulombs it carries) |
| 2 different metals + electrolyte = voltage | Simple electrochemical cell set up with 2 different metals in an electrolyte producing a voltage |
| Fuel cells | A fuel cell as a device that generates electricity by a chemical reaction. Equations, advantages and disadvantages |
| Electrochemical series | Electrochemical series as a list of reduction equations together with their reduction potentials |
| Standard hydrogen electrode | The use of the Standard Hydrogen Electrode (S.H.E.) as a standard (E0 = 0.00 V), set up and conditions |
| Ecell calculations | E0cell = E0red − E0oxid and related variations |
| Nernst eqn | Relating the effective concentrations of the components of a cell reaction to the standard cell potential. Either in the general form for all temperatures or shortened form at 298 K |
| Context: extraction of metals | Extraction of metals relying on the relative reactivity of elements (e.g. reduction using carbon). Electrolysis of metals with higher reactivities |
| Context: electroplating | Use of electrolysis to electroplate materials, e.g. for decoration or for desirable properties |
| Context: pH probe | Understanding that a pH probe works by measuring the electrical potential produced by the solution and using the potential difference to determine the pH |
| Context: corrosion | Sacrificial protection as a method of preventing corrosion |
| Context: others | Alcosensors, electrochemistry for water treatment |