1. Which metal do you think would react with water in this way?
Reaction trends and predicting reactions
Quick Starter
Which metal do you think would react with water in this way?
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2. Which metal do you think would react with water in this way?
RReaction trends and predicting reactions
Quick Starter
Which metal do you think would react with water in this way?
Group 1
Hint X
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3. It reacts with water similarly to all Group 1 metals
Reaction trends and predicting reactions
Quick Starter
The metal is sodium
It reacts with water similarly to all Group 1 metals
Group 2 metals are less reactive
Transition metals don’t react with water very much at all
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4. LO
Learning questions:
How do we decide the order of reactivity in metals?
What affects how reactive a metal is?
Can I predict which metal will be more reactive based on their position in the periodic table?
Can I deduce the order of reactivity based on experimental results?
Keywords:
Reactivity, oxidation, electrons, trend, reactivity series, displacement reacction.

5. How can we compare the reactivity of metals?NK
How can we compare the reactivity of metals?
How can we tell if a metal is reacting? What can you look out for?
Colour change, temperature change, gas given off.
How could we compare the reactivity of different metals experimentally?
Keywords:
Reactivity, oxidation, electrons, trend, reactivity series, displacement reacction.

6. Comparing reactivity of metalsCM
Reactions of metals with water and acid.
Place a piece of one of the metals to a test tube and half fill the test tube with water. Note down any observations.
Repeat step 1 but with acid instead of water.
Repeat steps with all metals.
Equipment:
Test tubes, test tube rack, pipettes, sulphuric acid, metal samples
Keywords:
Reactivity, oxidation, electrons, trend, reactivity series, displacement reacction.

7. Comparing reactivity of metalsCM
Reactions of metals with water and acid.
Metal
Reaction with water
Reaction with acid
Zinc
Lead
Copper
magnesium
Calcium (teacher only)
Keywords:
Reactivity, oxidation, electrons, trend, reactivity series, displacement reacction.

8. Comparing reactivity of metalsCM
Rank the order of reactivity that you have noticed for the metals you have tested.
Try and find them all in the periodic table note down where they are found (which group, area if no group number)
How do they compare to the group 1 metals?
Why might there be a difference?
Keywords:
Reactivity, oxidation, electrons, trend, reactivity series, displacement reacction.

9. Displacement reactionsCM
Add the metals to the spotting tile as shown.
Cover with the solutions shown and record observations (colour change, bubbles etc)
Displacement reactions: a more reactive element displacing or taking place of a less reactive element in a compound
Is the order of reactivity the same as what you noticed before?

10. Reactivity explained
ATD
All metals are oxidised (lose electrons) to form positive charges when they form a compound.
The easier they do this the more reactive they are.
Why might some metals lose electrons easier?
(think back to group 1)
Thinks about what keeps electrons attached to an atom.
Less electrons in outer shell mean they will lose electrons easier. Then it relates to the size of the atom, larger, lower down the group = more reactive.
Keywords:
Electrons, trend, electronic structure, shielding, reactivity, atomic radius, attraction, nucleus

11. Reactivity series
What do you notice about where the most reactive elements are found in the periodic table?
Why do you think this is?
Think how many electrons they can lose from their outer shell.

12. How does reactivity affect metals?
If a metal is very reactive it is normally only found in a compound in the ground called an ore.
They have to be extracted to make them useful.
Unreactive metals are often found native, by themselves and not in a compound.
Iron ore
Gold

13. 1 a) What would you expect to see if zinc metal was placed in to copper sulphate solution?
(2 marks)
b) What are the products formed in this reaction? (2 marks)
2. When iron oxide is heated with aluminium powder, the following reaction takes place:
Aluminium + iron oxide → iron + aluminium oxide
When aluminium oxide is heated with iron no reaction takes place.
a) Which of the two metals is more reactive? (1 mark)
b) The formula for iron oxide is Fe2O3. The formula for aluminium oxide is Al2O3.
Write a balanced symbol equation to show the reaction between aluminium and iron oxide. (2 marks)
c) Window frames made from aluminium do not corrode as quickly as windows made form iron.
Explain this statement using the information above. (2 marks)