Chapter summary
Periodicity and Metals, at a glance
Find patterns in the Periodic Table and use evidence to predict reactions.
O-Level 6092 (2026) / SEC G3 K324 (2027)
Quick revision
Revisit the essentials, then return to an explanation when you need it.
| Term | Definition to write |
|---|---|
| Group | A vertical column of the Periodic Table. Its elements have the same number of outer (valence) electrons. |
| Period | A horizontal row of the Periodic Table. Its elements have the same number of occupied electron shells. |
| Rusting | The corrosion of iron. It needs both oxygen and water, and forms hydrated iron(III) oxide. |
Pure only
| Term | Definition to write |
|---|---|
| Sacrificial protection | A more reactive metal, such as zinc or magnesium, is attached to iron. It loses electrons and corrodes instead of the iron. |
Groups share valence-electron patterns. Group 1 becomes more reactive down the group; group 17 becomes less reactive. Noble gases have full outer shells.
Metal order: K, Na, Ca, Mg, Zn, Fe, Pb, H, Cu, Ag. Use comparable experiments. Rusting needs oxygen and water; barriers remove contact with them.
Pure only
Pure: connect displacement to electron loss, compare oxide reduction and carbonate stability, and distinguish sacrificial protection from an intact barrier.
Quick recall
Why do elements in the same group have similar chemical properties?
Revisit an explanation
- Read position from electron arrangement
- Metal to non-metal across a period
- Group 1: lithium, sodium and potassium
- Group 17: identify displacement from the evidence
- Recognise noble gases and transition metals
- Build the metal reactivity series from experiments
- Use reactivity to explain extraction and heating
- Prevent rust by removing a condition or supplying protection