Unit 10.1.7: The reactivity series
E-assessement - B1: Periodic Table
- metals (and non-metals)
- transition metals
- Redox reactions
- reactivity series
- extraction of metals
- To understand that metals can be ordered in terms of reactivity based
on the empirical evidence gathered in this unit.
- To know that very reactive metals are good reducing agents and lose
Test mixtures of metals and metal ions to support prior emipical evidence.
Metals can be added to solutions while monitoring the temperature over
These could be test tube reactions using 10 ml of solution to a suitable
excess of metal.
Extension would be to prepare solutions of a known molarity (1M) using
their relative mass.
- Magnesium and iron(II) sulfate solution
- Magnesium and zinc sulfate solution
- Magnesium and copper sulfate solution
- Zinc and magnesium sulfate solution
- Zinc and iron(II) sulfate solution
- Zinc and nickel(II) sulfate solution
- Zinc and copper sulfate solution
- Iron and zinc sulfate solution
- Iron and copper sulfate solution
- Iron and nickel sulfate solution
- Copper and zinc sulfate solution
- Copper and iron(II) sulfate solution
- Copper and nickel sulfate solution
Data processing: Criteria C
The students could first be divided into groups to prepare enough stock
solution to supply the whole class.
- Magnesium sulfate
- Zinc sulfate
- Iron(II) sulfate
- Copper(II) sulfate
- Nickel(II) sulfate
10 ml of 1 mol dm-3 solution corresponds to 0.01 mol. All of the metals
are divalent, so an excess corresponds to > 0.01 mol of metal.
- Magnesium (Ar = 24) 0.01 mol = 0.24 g
- Zinc (Ar = 65) 0.015 mol = 0.65 g
- Iron (Ar = 56) 0.015 mol = 0.56 g
- Copper (Ar = 64) 0.015 mol = 0.64 g
All approximate values.