Reactivity Series (Cambridge (CIE) O Level Chemistry): Theory Questions

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.

i) Which two metals would not react with dilute hydrochloric acid?

[2]

ii) Which two unfamiliar metals (*) would react with cold water?

[2]

iii) What is the oxidation state of barium?

[1]

iv) Name an unfamiliar metal (*) whose oxide cannot be reduced by carbon.

[1]

v) Why should you be able to predict that metals such as iron and chromium have more than one oxidation state?

[1]

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.

i) The order was found to be:
manganese  - most reactive
zinc
tin
silver - least reactive

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

[3]

ii) Write the ionic equation for the reaction between tin atoms and silver(I) ions.

[2]

iii) The following is a redox reaction.

Mn + Sn²⁺ $\to$Mn²⁺ + Sn

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

[2]

iv) Explain why experiments of this type cannot be used to find the position of aluminium in the reactivity series.

[2]

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?

Magnesium ................

[1] 

Copper ................

[1] 

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

2X (s) + 2H₂O (l) → 2XOH (aq) + H₂ (g)

i) Describe the test you would use to show that the gas evolved is hydrogen.

[1]

ii) How could you show that the water contained a compound of the type XOH?

[2]

iii) In which group of the Periodic Table does metal X belong?

[1]

iv) The ore of X is its chloride. Suggest how metal X could be extracted from its chloride.

[2]

Tin is an element in Group IV.

The position of tin in the reactivity series is:

zinc

iron

tin

copper

For each of the following, decide if a reaction would occur. If there is a reaction, complete the equation, otherwise write ‘no reaction’.

Cu + Sn²⁺ → ..........................................

Fe + Sn²⁺ → ..........................................

Sn + Zn²⁺ → ..........................................

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

i) What is the product at the negative electrode (cathode)?

[1]

ii) Write the equation for the reaction at the positive electrode (anode).

[2]

iii) Name the acid formed in this electrolysis.

[1]

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:

magnesium, most reactive

zinc

lead

silver, least reactive

Complete the table, using Y to mean reacts and N to mean does not react.

Displacement reactions are redox reactions.

On the equation below, draw a ring around the reducing agent and an arrow to show the change which is oxidation.

Zn + Pb²⁺ → Zn²⁺ + Pb

Write the ionic equation for the reaction between zinc and aqueous silver ions.

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.

Metal A

Metal B

Metal C

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 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.

Give, as far as possible, the order of reactivity of these metals.

Write the least reactive first.

What additional experiment needs to be carried out to put all four metals in order of reactivity?

Write the ionic equation for the reaction between tin atoms and silver(I) ions.

Indicate on your equation the change which is oxidation.

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

i)

In the space at the top of the series, write an ionic equation that includes a more reactive metal.

[1]

ii)

Define oxidation in terms of electron transfer.

[1]

iii)

Explain why the positive ions are likely to be oxidising agents.

[1]

iv)

Which positive ion or ions can oxidise mercury metal, Hg?

[1]

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) $\to$ Pb (s) + Ni²⁺ (aq)

The ionic half-equations for this reaction are shown.

Ni (s) $\to$ Ni²⁺ (aq) + 2e^–

Pb²⁺ (aq) + 2e^– $\to$ 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.

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) $\to$ 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.