Reactivity Series (Cambridge O Level Chemistry)

Give three differences in physical properties between the Group I metal, potassium, and the transition element, iron.

The following metals are in order of reactivity.

potassium
zinc
copper

For those metals which react with water or steam, name the products of the reaction, otherwise write ‘no reaction’.

      Potassium: 
      Zinc:
      Copper:

The reactivity series of metals given below contains both familiar and unfamiliar elements.
For most of the unfamiliar elements, which are marked *, their common oxidation states are given.

Choose metal(s) from the above list to answer the following questions.

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The reactivity series lists metals in order of reactivity.

To find out which is the more reactive metal, zinc or tin, the following experiment could be carried out.

This experiment could be carried out with other metals and the results are recorded in a table. Then the order of reactivity can be deduced.

Complete the table of results from which this order was determined.

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Mn + Sn²⁺ Mn²⁺ + Sn

Indicate on the equation the change which is oxidation. Give a reason for your choice.

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Potassium and calcium are very reactive metals at the top of the series. Because their ions have different charges, K⁺ and Ca²⁺, their compounds behave differently when heated.

Explain why the ions have different charges.

Some reactions of metals W, X, Y and Z are given below.

Arrange these metals in order of reactivity.

Which of these metals could be?

The equation for the reaction of X with cold water is given below.

2X (s) + 2H₂O (l) → XOH (aq) + H₂ (g)

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Tin is an element in Group IV.

The position of tin in the reactivity series is:

Aqueous tin(II) sulfate is electrolysed using carbon electrodes. This electrolysis is similar to that of aqueous copper(II) sulfate using carbon electrodes.

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Steel articles can be plated with tin or zinc to prevent rusting.

When the zinc layer is damaged exposing the underlying steel, it does not rust, but when the tin layer is broken the steel rusts. Explain.

One way of establishing a reactivity series is by displacement reactions.

A series of experiments was carried out using the metals lead, magnesium, zinc and silver.

Each metal was added in turn to aqueous solutions of the metal nitrates.

The order of reactivity was found to be:

Extended Only

Another way of determining the order of reactivity of metals is by measuring the voltage and polarity of simple cells. The polarity of a cell is shown by which metal is the positive electrode and which metal is the negative electrode. An example of a simple cell is shown below.

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Excess hydrochloric acid was added to powdered zinc. The hydrogen evolved was collected and its volume measured every 20 seconds. The experiments were repeated at the same temperature using the same number of moles of powdered magnesium and aluminium.

Identify metals A, B and C by choosing from zinc, magnesium and aluminium. Give a reason for each choice.

Extended Only

Using ‘moles’, explain why two of the metals form the same volume of hydrogen but the third metal forms a larger volume.

The reactions of a metal and the thermal stability of some of its compounds are determined by the position of the metal in the reactivity series.

To find the order of reactivity of the metals, cobalt, magnesium, silver and tin, the following experiments were carried out.

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A cell consists of two different metal electrodes in an electrolyte. Three possible cells are shown below.

In the following list of ionic equations, the metals are in order of reactivity.

The following diagram shows a simple cell.

Separate: Chemistry and Extended Only

Displacement reactions occur between metals and metal ions. Displacement reactions can be used to determine the order of reactivity of metals such as lead (Pb), nickel (Ni), and silver (Ag).

The ionic equation for a displacement reaction is shown.

Ni (s) + Pb²⁺ (aq) Pb (s) + Ni²⁺ (aq)

The ionic half-equations for this reaction are shown.

Ni (s) Ni²⁺ (aq) + 2e^–

Pb²⁺ (aq) + 2e^– Pb (s)

The ionic half-equations show that electrons are donated by nickel atoms and accepted by lead ions.

Identify the reducing agent in the displacement reaction. Give a reason for your answer.

reducing agent _________________________________________

reason_________________________________________________

Extended Only

What is the general term given to the type of reaction in which electrons are transferred from one species to another?

The ionic equation for another displacement reaction is shown.

Pb (s) + 2Ag⁺ (aq) 2Ag (s) + Pb²⁺ (aq)

Write the two ionic half-equations for this reaction.

Use the information in (a) and (c) to put the three metals lead, nickel and silver in order of reactivity.