Reactivity Series of Metals
Reactions of Metals
Effect of Heat on Metal Carbonates

Chemical Properties of Metals
◦ Metal reaction with cold water & steam
◦ Metal reaction with hydrochloric acid

Reaction of Metals: Displacement Reactions
◦ With aqueous ions of another metal
◦ With the oxide of another metal

Reaction of Metal Oxides
◦ With carbon
◦ With hydrogen

Effect of Heat on Metal Carbonates
◦ Thermal stability & reactivity
Reactivity Series of Metals
Recap:
Chemical Properties of Metals
Reaction with Water (Cold Water)
Metal + Cold Water  Metal Hydroxide + Hydrogen Gas
Eg. 2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g)
Which are some metals that react with cold water?
Recap:
Chemical Properties of Metals
Reaction with Water (Steam)
Metal + Steam  Metal Oxide + Hydrogen Gas
Eg. Mg(s) + H2O(g)  MgO(s) + H2(g)
Which metals only react with steam?
Recap:
Chemical Properties of Metals
Reaction with Hydrochloric Acid
Metal + Hydrochloric Acid  Salt + Hydrogen Gas
Eg. 2K(s) + 2HCl(l)  2KCl(aq) + H2(g)
The more vigorous the reaction
The higher it is in the reactivity series
The more reactive is the metal
Reaction of Metals
With the Aqueous Ions of Another Metal
• Displacement of metals from solution
• More reactive metals can displace less reactive
metals from their salt solutions.
• This can be used to find the position of metals in
the reactivity series.
Iron Nail in Copper(II) Sulphate Solution
Observations:
1.
2.
Reddish-brown solid forms on the surface of the
iron nail
Blue solution becomes pale green
Fe (s) +
Iron
CuSO4 (aq) 
Copper(II) Sulphate
Solution
FeSO4 (aq)
Iron(II) Sulphate
Solution
+
Cu (s)
Copper
Iron Nail in Copper(II) Sulphate Solution
Brown solid: Copper metal
Solution turns pale green


◦
◦
Copper has been removed from the solution.
Iron(II) sulphate solution is pale green in colour.
We say that…
Iron has displaced copper from the
copper(II) sulphate solution.
What will happen when
a piece of magnesium strip is immersed in
a solution of copper(II) sulphate?
Think!
Some Possible Observations
Deposit of the more reactive metal (from its
aqueous solution)
 Colour of the solution may change
 Heat may be given off

Displacement Reactions are Redox Reactions
The more reactive metal is oxidized
The less reactive metal is reduced
REDOX
reaction!
For example,
Chemical Equation:
Fe (s) + CuSO4 (aq)  FeSO4 (aq) + Cu (s)
Ionic Equation:
Fe (s) + Cu2+ (aq)  Fe2+ (aq) + Cu (s)
Displacement Reactions are Redox Reactions
A more reactive metal:
 readily gives up electrons in reactions
 has greater tendency to form positive ions
As a result…
A more reactive metal can displace
a less reactive metal,
from its solution or metallic oxide.
Reaction of Metals
With the Oxide of Another Metal

Displacement of metals from metallic oxides

A more reactive metal can reduce the oxide of a less
reactive metal.

For example: Thermit reaction
2Al (s) + Fe2O3 (s)  Al2O3 (s) + 2Fe (l)
Reaction of Metals
With the Oxide of Another Metal

Thermit Reaction
Iron(III) ions are reduced to become iron atoms
2Al (s) + Fe2O3 (s)  Al2O3 (s) + 2Fe (l)
Aluminium atoms are oxidized to become aluminium(III) ions

The more reactive the metal is, the more readily it
forms compounds.

Unreactive metals tend to stay umcombined.
Reaction of Metal Oxides With Carbon

Carbon can remove oxygen from the oxides of
metals that are not too high up in the Reactivity
Series.
The lower the position of a metal in the
Reactivity Series, the easier it is for carbon to
remove oxygen from the metal oxide.
Reaction of Metal Oxides With Carbon
metal oxide
reaction
potassium oxide
sodium oxide
calcium oxide
magnesium oxide
zinc oxide
iron(II) oxide
lead(II) oxide
copper(II) oxide
oxides are not reduced by carbon
silver oxide
oxide is reduced by heating
oxides are reduced by carbon
The Importance!
Reaction of Metal Oxides With Carbon

metals need to be extracted from their ores before
we can use them

metals below magnesium are often extracted from
their ores by reduction with carbon (WHY?)

metals above zinc cannot be extracted by reduction
with carbon bc they are stable (THEN WHAT?)
Reaction of Metal Oxides With Hydrogen

Hydrogen can remove oxygen from metallic oxides,
producing the metal and water(steam).
metal oxide + hydrogen  metal + steam
The lower the position of a metal in the
Reactivity Series, the easier it is for hydrogen
to remove oxygen from the metal oxide.
Reaction of Metal Oxides With Hydrogen
metal oxide
potassium oxide
sodium oxide
calcium oxide
magnesium oxide
zinc oxide
iron(II) oxide
lead(II) oxide
copper(II) oxide
silver oxide
reaction with hydrogen
heated metal oxides are not
reduced by hydrogen
heated metal oxides are reduced
by hydrogen
Effect of Heat on Metal Carbonates:
Thermal Stability & Reactivity

Most carbonates decompose when heated strongly
to produce a metal oxide and carbon dioxide gas.

The ease of decomposition depends on the position
of the metal in the reactivity series.
Recall the reactivity series.
Thermal Stability of Metal Carbonates
Metal Carbonate
Potassium Carbonate
Effect of Heat
Sodium Carbonate
Stable to heat
No visible reaction
Calcium Carbonate
Decomposes into metal oxide and carbon dioxide
Magnesium Carbonate
Metal 
Metal Oxide + Carbon Dioxide
Zinc Carbonate
Iron (III) Carbonate
Lead Carbonate
Copper(II) Carbonate
Silver Carbonate
Decomposes into silver and carbon dioxide
 Reactions with water & dilute acids:
More vigorous reaction
 Higher in the reactivity series
 The metal is more reactive
 Reaction with metal carbonates:
The more stable the metal carbonate is to
heat, the higher it is in the reactivity series.
Check this out!
http://www.chem.iastate.edu/group/Greenbowe/se
ctions/projectfolder/flashfiles/redox/home.html
Class Activity & Discussion
So, what have you learnt today?

Displacement Reaction
◦ They are redox reactions.
◦ A more reactive metal can displace a less reactive
metal, from its solution or metallic oxide.

Carbonates: Thermal stability & reactivity
The more stable the metal carbonate is to heat,
the higher it is in the reactivity series.