Resources: 0.1 mol dm-3 magnesium sulfate solution, 0.1 mol dm-3 iron sulfate solution, 0.1 mol dm-3 copper sulfate solution, 0.1mol dm-3 zinc sulfate solution, 1cm magnesium ribbon, small iron nails or iron strips, copper strips, zinc strips, spotting tile and 4 pipettes.
Core Handout: An investigation sheet for the students to record their results as they investigate displacement reactions.
If necessary, use the completed unit on the periodic table to revise the arrangement of elements. Remind the students that the periodic table can be used to predict the behaviour of different elements in chemical reactions.
How can different metals be sorted? Students should discuss their ideas.
Using the presentation slides, show the students the periodic table to remind them about elements and how they are organised in the table.
Discuss how the metals can be compared by how vigorous their chemical reactions are. A short video is shown to students which shows the reactivity of 3 different metals in hydrochloric acid. This leads on to the introduction of the reactivity series and why elements are placed in these positions.
The students are then introduced to displacement reactions and then carry out their own investigation on the reactivity of four metals using displacement reactions.
Career Film: Take a tour around Rolls Royce SMR's Heritage Museum in Derby to find out about Mark Salisbury's job. Mark works as the Group Head of Regulatory Affairs for Rolls Royce SMR.
Expert Film: This is Mark Salisbury. Mark works as the Group Head of Regulatory Affairs for Rolls Royce SMR. Listen to Mark as he explains the reactivity series.
Determine the order of the reactivity series
Introduce the experiment and read through the method with the students to ensure that they are aware of the correct procedure.
After you have collected all your data, rank the metals from most reactive to least reactive, i.e. th e metal that had the most reactions → the metal that had the least reactions. Write the word equations and attempt the chemical equations for the reactions that have taken place.
Support: Give the students spotting tiles with the metals labelled and in the correct positions so that they only need to add solutions.
Challenge: Students use challenge task in handout to suggest and explain uses of metals in relation to their position on the reactivity series.
Using the students’ results, discuss the observations that they made and the order of reactivity. This can be extended into the challenge question where students can predict and write equations for displacement reactions based on their position in the reactivity series.
The reactivity series is a list that shows the most reactive metal to the least reactive metal. Metals can either be reactive or unreactive. However, a lot do fall in between the two. When something is unreactive, it means that partaking in chemical reactions is very difficult. When something is reactive. It means that partaking in chemical reactions is a lot easier. Chemical reactions make new substances so when a metal is reactive, it is more likely to do this.
The general reactivity series is as follows: potassium, sodium, calcium, magnesium, aluminium, zinc, iron, tin, lead, copper, silver, gold and platinum. Potassium is the most reactive and platinum is the least reactive. Potassium tends to react vigorously with water. Gold will not because it is super unreactive. Carbon fits in depending on its reactivity with metal oxides. It usually comes under aluminium. Carbon isn’t usually shown in the reactivity series because it is a non-metal. However, a lot of people include it because it allows us to understand what occurs in the extraction of iron.
The top five most reactive metals will react with oxygen and therefore burn in air. Metals from aluminium to copper will also react with oxygen in the air but form metal oxides. Aluminium does this the quickest and copper will do this the slowest. For example, aluminium will react with oxygen to form aluminium oxide. Aluminium and zinc do this quickly. Iron will react with oxygen to form iron oxide quite slowly at room temperature. This reaction can happen quicker if heat is applied. Tin, lead and copper react only when heated in air. Silver, gold and platinum do not react with oxygen.
The first four metals in the reactivity series react with water. Metals including magnesium to iron will react with steam not water. This also forms an oxide and hydrogen. These reactions are very much reversible. Again, the last five metals in the series do not react with either water or steam.
The first four metals in the reactivity series react with dilute sulphuric acid and dilute hydrochloric acid very vigorously. This reaction is dangerous, so care needs to be taken. A metal salt and hydrogen are formed as products of this reaction. Metals including magnesium to lead all react safely with the dilute acid. The reaction of zinc and sulphuric acid is used to make small amounts of hydrogen. This reaction is slow but can be increased by copper (||) sulphate. Any metal below hydrogen and including hydrogen, does not react with the dilute acid. These are just a few examples which show the properties of metals in the reactivity series.