AQA GCSE Chemistry (8462), Higher tier · Chemical changes › Reactivity of metals
Practise The reactivity series. 11 exam-style questions on this subtopic, at up to four difficulty levels, with full mark schemes and a progress tracker. Free, no account needed.
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Zinc reacts with dilute hydrochloric acid, but copper does not. Name the gas produced when zinc reacts with the acid.
hydrogen
Sample questions
Written for this site in the style of AQA exam questions. They are not taken from real past papers.
Question 1Easy3 marks
The reactivity series lists metals in order of reactivity.
(a) Which list shows these metals in order of decreasing reactivity (most reactive first)? Tick (✓) one box.[1]
potassium, zinc, iron, copper
copper, iron, zinc, potassium
zinc, potassium, copper, iron
iron, copper, potassium, zinc
(b) Zinc reacts with dilute hydrochloric acid, but copper does not. Name the gas produced when zinc reacts with the acid.[1]
(c) Explain, in terms of the ions that metals form, why zinc is more reactive than copper.[1]
Show the answer and mark scheme
(a)Answer: potassium, zinc, iron, copper
(b)Answer: hydrogen
hydrogen
(c)
zinc has a greater tendency than copper to form positive ions (to lose electrons)
Question 2Medium6 marks
When metals react with other substances the metal atoms form positive ions.
(a) Which metal forms positive ions most easily? Tick (✓) one box.[1]
Calcium
Copper
Iron
Zinc
(b) Explain why potassium is more reactive than magnesium. Use ideas about ions in your answer.[2]
(c) Describe what you would see when a small piece of calcium is added to cold water.[2]
(d) Hydrogen is often included in the reactivity series. Copper does not react with dilute acids. Should hydrogen be placed above or below copper in the reactivity series? Give a reason.[1]
Show the answer and mark scheme
(a)Answer: Calcium
(b)
potassium atoms lose electrons / form positive ions more easily than magnesium atoms
so potassium reacts more vigorously / faster (with water and acids)
(c)
fizzing / bubbles of gas
the calcium gets smaller / disappears
the solution turns cloudy / milky
(d)
above copper, because copper does not displace hydrogen from acids
Question 3Hard8 marks
A student wants to put four metals in order of reactivity: copper, iron, magnesium and zinc. The student has powdered samples of the metals, copper(II) sulfate solution and normal laboratory apparatus.
(a) Describe a method the student could use to put the metals in order of reactivity by measuring temperature changes. Include how the student should make it a fair test and how the results would show the order of reactivity.[6]
(b) Explain why the student should use powdered metals rather than lumps of metal.[2]
Show the answer and mark scheme
(a)
measure a fixed volume (e.g. 25 cm3) of copper(II) sulfate solution into a polystyrene cup (with a lid) using a measuring cylinder
measure the starting temperature of the solution with a thermometer
add a fixed mass (e.g. 1.0 g) of one metal powder (an excess) and stir
record the highest temperature reached and calculate the temperature rise
repeat with each metal using fresh copper(II) sulfate solution of the same concentration and volume, and the same particle size of metal
repeat each test and calculate a mean temperature rise
the greater the temperature rise, the more reactive the metal
copper produces no temperature change (no reaction), so it is the least reactive
Marked with levels of response: the full level descriptors are in the app.
(b)
powder has a larger surface area so reacts faster
so less energy is lost to the surroundings before the maximum temperature is reached / the reaction is complete