O Levels/IGCSE Chemistry Lesson Plan 9.4

Section	Details
Objective	State the order of the reactivity series: potassium, sodium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold.
Activities	– Starter (5 mins): Show a list of common metals and ask: “Which of these do you think reacts the most vigorously?”- Main (25 mins): 1. Introduce the reactivity series in order of reactivity. 2. Explain how the position in the series reflects a metal’s tendency to form positive ions. 3. Discuss how non-metals like carbon and hydrogen are included for comparison. 4. Provide examples of applications, e.g., potassium and sodium in reactions, gold in jewelry due to its low reactivity.- Plenary (10 mins): Students memorize and arrange a scrambled list of the reactivity series in the correct order.
Resources	List of metals, periodic table, worksheets.
Time	40 minutes total: 5 mins (Starter) + 25 mins (Main) + 10 mins (Plenary).
Homework	Write a paragraph explaining why potassium is more reactive than iron, referencing the reactivity series.
Assessment	Worksheet: Arrange metals in the correct reactivity order and explain their positions.
Past Paper Practice	IGCSE Chemistry 0620/41/M/J/19 Q4(b) – Memorizing and applying the reactivity series.

Section	Details
Objective	Describe the relative reactivities of metals in terms of their tendency to form positive ions, through displacement reactions.
Activities	– Starter (5 mins): Show examples of displacement reactions and ask: “Why does one metal replace another in a reaction?”- Main (25 mins): 1. Define displacement reactions as reactions where a more reactive metal displaces a less reactive metal from its compound. 2. Demonstrate a few reactions, e.g., magnesium + copper sulfate → magnesium sulfate + copper. 3. Relate observations to the reactivity series. 4. Guide students in predicting the outcomes of displacement reactions.- Plenary (10 mins): Students complete a table of displacement reactions and their products.
Resources	Solutions of metal salts, metals, worksheets, periodic table.
Time	40 minutes total: 5 mins (Starter) + 25 mins (Main) + 10 mins (Plenary).
Homework	Write balanced equations for three displacement reactions based on given metal salt solutions.
Assessment	Worksheet: Predict the products of given displacement reactions and explain the observations.
Past Paper Practice	IGCSE Chemistry 0620/41/O/N/21 Q3(a) – Displacement reactions of metals.

Section	Details
Objective	Describe the reactions of metals with water, steam, and dilute acids, and explain these in terms of the reactivity series.
Activities	– Starter (5 mins): Show a video of metals reacting with water and acids and ask: “Why do some metals react more vigorously than others?”- Main (25 mins): 1. Discuss reactions of potassium, sodium, and calcium with cold water (producing hydrogen and hydroxides). 2. Explain how magnesium reacts with steam to form magnesium oxide and hydrogen. 3. Demonstrate or discuss reactions of metals like magnesium, zinc, iron, copper, silver, and gold with dilute HCl. 4. Relate the intensity of the reactions to the metal’s position in the reactivity series.- Plenary (10 mins): Students match metals to their expected reactions with water, steam, and acids.
Resources	Metal samples, water, dilute HCl, worksheets, reaction videos.
Time	40 minutes total: 5 mins (Starter) + 25 mins (Main) + 10 mins (Plenary).
Homework	Write balanced equations for the reactions of magnesium with steam and zinc with HCl.
Assessment	Worksheet: Predict and explain the reactions of given metals with water, steam, and acids.
Past Paper Practice	IGCSE Chemistry 0620/41/M/J/20 Q4(c) – Reactions of metals with water and acids.

Section	Details
Objective	Explain the apparent unreactivity of aluminium due to its oxide layer. Deduce an order of reactivity from experimental results.
Activities	– Starter (5 mins): Ask: “Why does aluminium, a relatively reactive metal, seem unreactive under normal conditions?”- Main (25 mins): 1. Explain how aluminium forms a thin oxide layer that prevents it from reacting easily. 2. Discuss how this property is advantageous (e.g., resistance to corrosion). 3. Guide students in analyzing experimental results (e.g., displacement, reaction intensity) to deduce the reactivity order of metals.- Plenary (10 mins): Students summarize why aluminium appears unreactive and analyze a set of experimental data to rank metals by reactivity.
Resources	Data tables of reactions, diagrams showing aluminium’s oxide layer, worksheets.
Time	40 minutes total: 5 mins (Starter) + 25 mins (Main) + 10 mins (Plenary).
Homework	Write a paragraph explaining why aluminium’s oxide layer is important in its applications.
Assessment	Worksheet: Deduce the reactivity order of metals from given experimental data.
Past Paper Practice	IGCSE Chemistry 0620/41/O/N/21 Q4(b) – Reactivity and aluminium oxide layer explanation.

Reactivity Series:
- Potassium > Sodium > Calcium > Magnesium > Aluminium > Carbon > Zinc > Iron > Hydrogen > Copper > Silver > Gold.
Displacement Reactions:
- More reactive metals displace less reactive metals from their compounds.
Reactions with Water and Acids:
- Potassium, sodium, and calcium react vigorously with water.
- Magnesium reacts with steam to produce oxide and hydrogen.
- Reactivity with acids decreases down the series.
Aluminium’s Oxide Layer:
- Forms a protective layer, making it appear unreactive under normal conditions.

Use demonstrations and videos to engage students and reinforce concepts safely.
Relate reactivity trends to practical applications (e.g., use of less reactive metals in jewelry).
Provide opportunities for students to analyze data and make predictions based on trends.