The diagram illustrates a simple cell. This simple cell was tested with different metals as electrodes, and the voltages were entered in the table.
If the voltage measured is positive, then metal 2 is more reactive than metal 1.
If the voltage measured is negative, then metal 1 is more reactive than metal 2.
The more reactive metal is oxidised.
The larger the gap in reactivity between the metals, the greater the voltmeter reading.
(a(i))[1]
Define oxidation in terms of electrons.
(a(ii))[1]
Write an ionic half-equation to show the oxidation of nickel.
(a(iii))[1]
What happens to the mass of the nickel electrode when the nickel is oxidised?
(b(i))[2]
Which metal in the table is the most reactive? Give a reason for your answer.
(b(ii))[1]
State which two different metals have the same reactivity.
(b(iii))[2]
Predict the voltage produced by a simple cell when beryllium is metal 1 and silver is metal 2.
(c)[2]
Describe how the simple cell in the diagram can be used to show that magnesium is more reactive than beryllium. Explain your answer.
Worked solution & mark scheme
This 10-mark question has a full step-by-step worked solution and mark scheme. One marking point: “Losing electrons” …