Typical Reactions IGCSE CHEMISTRY Y11.pptx

Formulae, Equations and Amount of
Substance
Tuesday, December 19, 2023 1
Tuesday, December 19, 2023
Lesson 2
Topic: Typical Reactions
Formulae, Equations and Amount of Substance
Key Words
Displacement
Precipitation
Learning Intentions
1. Know and complete the general reactions
with acids.
2. Use the reactivity series to explain
displacement reactions.

Starter
Place the following words to create general word equations
Metal Salt Metal carbonate Water
Acid + Metal  __________ + Hydrogen
Acid+ ____________  Metal Salt + carbon dioxide + _______
Acid + Base Metal salt +_________
Complete the following word equations
Sulphuric acid + copper carbonate
Hydrochloric acid + Zinc
Nitric acid+ Sodium hydroxide 

© Boardworks Ltd 2004
1 of 20 © Boardworks Ltd 2005
3 of 32
magnesium
+ acid
hydrogen
burning
splint
Many metals react with acids.
When this happens the metal
fizzes as bubbles are produced.
What do the bubbles mean?
A gas is produced.
How can you test to find out if the gas produced is hydrogen?
Place a burning splint next to the mouth of test tube.
A ‘squeaky pop’ as the gas ignites shows that hydrogen
is the gas produced in this reaction.
Reaction of metals with acids

4 of 32
metal
nitrate
nitric acid
Reaction of metals with acids
When a metal reacts with an acid, the products are a salt
and hydrogen gas.
The salt produced depends on the metal and type of acid
involved in the reaction:
 When a metal reacts with hydrochloric acid, the
salt produced is a metal chloride.
 When a metal reacts with sulfuric acid, the salt
produced is a metal sulfate.
 When a metal reacts with nitric acid, the salt
produced is a metal nitrate.
metal hydrogen
sulfuric
acid
hydrochloric
acid
acid metal
sulfate
metal
chloride
salt

5 of 32
zinc
chloride
Complete the word equations
Complete the word equations for metals reacting with acid:
hydrogen
nitric
acid
magnesium
nitrate
magnesium ?
hydrogen
sulfuric
acid
iron iron
sulfate
?
hydrogen
hydrochloric
acid
zinc ?
hydrogen
sulfuric
acid
lead lead
sulfate
?
?

6 of 32
potassium
sodium
calcium
magnesium
aluminium
zinc
iron
lead
(hydrogen)
copper
silver
gold
increasing
reactivity
Reactivity of metals
Some metals react more vigorously with acids than others.
Metals can be listed in order of how reactive they are.
This list is called the reactivity series.
The more reactive the
metal, the more vigorous
the reaction.
A metal that is below
hydrogen will not react
with dilute acids.

7 of 32
When a metal carbonate reacts with an acid,
it fizzes giving off carbon dioxide gas.
Carbon dioxide can be tested for using the
limewater test.
When carbon dioxide gas is bubbled
through limewater, it turns the
limewater cloudy or milky white.
Reaction of metal carbonates with acids
Most metal carbonates are not very soluble
and so the reactions may be slow.

8 of 32
Reaction of metal carbonates with acids
When a metal carbonate reacts with an acid, the products
are a salt, carbon dioxide and water.
The salt produced depends on the metal carbonate and type
of acid involved in the reaction:
 When a metal carbonate reacts with hydrochloric acid,
the salt produced is a metal chloride.
 When a metal carbonate reacts with sulfuric acid,
the salt produced is a metal sulfate.
 When a metal carbonate reacts with nitric acid,
the salt produced is a metal nitrate.
metal
carbonate
carbon
dioxide water
nitric acid metal
nitrate
sulfuric
acid
hydrochloric
acid
acid metal
sulfate
metal
chloride
salt

9 of 32
carbon
dioxide
sodium
carbonate
carbon
dioxide
nitric
acid
sodium
nitrate water
Complete the word equation for each reaction between a
metal carbonates and an acid:
calcium
carbonate
carbon
dioxide
nitric
acid
calcium
nitrate water
? ?
?
metal
carbonate
carbon
dioxide
acid salt water
zinc
carbonate
zinc
sulfate water
sulfuric
acid ?
? ?

10 of 32
Using the products as a clue, what is the reaction between
a base (such as a metal oxide) and an acid called?
Reaction of metal oxides with acids
When a metal oxide reacts with an acid, the products are a
salt and water.
metal
oxide water
acid salt
A metal oxide is a type of chemical called a base.
Bases are chemicals that react with an acid to produce
a salt and water.
A base that is soluble in water is called an alkali.
neutralization

11 of 32
iron
chloride
Complete the word equation for each reaction between a
metal oxide and an acid:
nitric acid magnesium
nitrate
magnesium
oxide ?
water
sulfuric
acid
zinc oxide iron
sulfate
?
hydrochloric
acid
iron oxide ?
metal
oxide water
acid salt
water
water
?
?
?

12 of 32
Reaction of acids with metal oxide and metal hydroxides
So the general equation for the reaction of metal oxides or metal hydroxides with acid is:
Acid + metal oxide OR metal hydroxide → salt + water
Common Acids
 Hydrochloric acid HCl(aq)
 Sulfuric Acid H2SO4(aq)
 Nitric Acid HNO3(aq)
Metal Oxides and Hydroxides
 Sodium Hydroxide NaOH(aq)
 Zinc Oxide ZnO(s)
 Calcium Hydroxide Ca(OH)2(S)
 Magnesium Oxide MgO(S)
 Potassium Hydroxide KOH(aq)
 Copper Oxide CuO

Displacement reactions: metals
• These are reactions where two
metals are competing to be
combined with a non-metal.
• The more reactive metal wins the
competition and becomes part of
a compound.
• The less reactive metal is
displaced and so is present as
the metal at the end of the
reaction.
Potassium
sodium
calcium
magnesium
aluminium
zinc
iron
copper
silver
gold
Increasing
reactivity
A more reactive metal (higher in the reactivity series) will
displace a less reactive metal from its compound.

• Copper is quite low in the reactivity series.
• Several metals will displace it from its compounds.
magnesium copper
sulphate
solution
magnesium
sulphate solution
copper metal
Magnesium + Copper
sulphate
 Magnesium
sulphate
+ Copper
more
reactive
less
reactive
Magnesium wins the competition.
Copper is displaced.
K
Na
Ca
Mg
Al
Zn
Fe
Cu
Ag
Au

Here are some actual photos.
The colour changes from blue to red/black as
copper metal is displaced.
Magnesium + Copper
sulphate
 Magnesium
sulphate
+ Copper
more
reactive
less
reactive
Magnesium wins the
competition. Copper is displaced
photograph
at end of
reaction
photograph
at start of
reaction
K
Na
Ca
Mg
Al
Zn
Fe
Cu
Ag
Au

• Balanced Equation:
Mg (s) + CuSO4 (aq) → Cu (s) + MgSO4 (aq)
• Ionic Equation: (SO4 2- spectator ions)
• Mg (s) + Cu 2+ (aq) → Cu (s) + Mg 2+ (aq)

The thermit reaction takes place
between aluminium and iron oxide.
It is so exothermic that molten iron
is produced and the reaction is used
to repair broken railway tracks.
Aluminium + Iron
Oxide
 Aluminium
Oxide
+ Iron
more
reactive
less
reactive
Aluminium wins the competition.
Iron is displaced and melts at the
high temperatures produced.
K
Na
Ca
Mg
Al
Zn
Fe
Cu
Ag
Au
iron oxide +
aluminium
powder
magnesium
fuse

Here is a photo of the thermit reaction being
carried out in a laboratory.
iron oxide +
aluminium
powder
magnesium
fuse

• Fe2O3 + 2 Al → 2 Fe + Al2O3
Chemical Formula:
2Al (s) + Fe2O3 (s) → 2Fe (s) + Al2O3 (s)
Aluminum Powder + Iron Oxide Iron + Aluminum Oxide
Ionic Equation: 2Al 0 + 2Fe +3 + 3O -2 → 2 Fe 0 + 2Al +3 + 30 -2
Half Reactions: Oxidation: 2Al 0 + 6e → 2Al +3
Reduction: 2Fe +3 → 2Fe 0 + 6e

Predict which mixtures will result in a reaction.
Metal 
Solution
Iron Magnesium Zinc Copper
Iron
chloride
Magnesium
nitrate
Zinc nitrate
Copper
sulphate
Yes Yes No
No No No
No Yes No
Yes Yes Yes

Displacement reactions: halogens
• These are displacement
reactions where two
halogens are competing to
be combined with a metal.
• It is the more reactive
halogen that will win and
become part of a
compound.
• The less reactive halogen
remains (or becomes) the
element.
Increasing
reactivity
Fluorine
Chlorine
Bromine
Iodine
• We can often tell which halogen is present from the
colour of the solution.

For example, if chlorine solution is added to
sodium bromide.
sodium
bromide
solution
sodium chloride
solution
bromine
Chlorine + Sodium
Bromide
 Sodium
Chloride
+ Bromine
more
reactive
less
reactive
Chlorine wins the competition.
Bromine (red) is displaced.
F
Cl
Br
I
At
chlorine
solution

Chlorine +
When writing equations for halogen displacement
reactions you must remember that – when in the
form of the element – halogens exist in pairs.
For chlorine and sodium bromide:
+ bromine
sodium
chloride
Sodium
bromide
→
Cl2(aq) + 2NaBr(aq) → 2NaCl(aq) + Br2(aq)
F
Cl
Br
I
At
Cl More
reactive
Br Less
reactive
Solution goes
yellow/brown as
bromine is produced.

• If no reaction - not write “no reaction.”
• Where there is a reaction write the names of the
products and then write a chemical equation
underneath.
F
Cl
Br
I
At
1) iodine + sodium bromide solution →
2) bromine + sodium chloride solution →
3) chlorine + sodium iodide solution →
No reaction
No reaction
sodium chloride + iodine
Cl2(g) + 2NaI(aq) → 2NaCl(aq) + I2(aq)
Predict whether or not a chemical reaction will
occur.

• 1. chlorine + potassium bromide ==> potassium chloride + bromine
• Cl2(aq) + 2KBr(aq) ==> 2KCl(aq) + Br2(aq)
• Cl2(aq) + 2Br–(aq) ==> 2Cl–(aq) + Br2(aq)
• 2. chlorine + potassium iodide ==> potassium chloride + iodine
• Cl2(aq) + 2KI(aq) ==> 2KCl(aq) + I2(aq)
• Cl2(aq) + 2I–(aq) ==> 2Cl–(aq) + I2(aq)
• 3. bromine + potassium iodide ==> potassium bromide + iodine
• Br2(aq) + 2KI(aq) ==> 2KBr(aq) + I2(aq)
• Br2(aq) + 2I–(aq) ==> 2Br–(aq) + I2(aq)
• The halogen molecule is the electron acceptor (the oxidising agent) and is reduced by electron
gain to form a halide ion.
• The oxidation state of the halogen in the halogen molecule changes (reduces) from 0 to –1,
electron gain, reduction
• The halide ion is the electron donor (the reducing agent) and is oxidised by electron loss to
form a halogen molecule
• The oxidation state of the halogen in the halide ion changes (increases) from –1 to 0, electron
loss, oxidation

Typical Reactions IGCSE CHEMISTRY Y11.pptx

Recommended

Recommended

More Related Content

Similar to Typical Reactions IGCSE CHEMISTRY Y11.pptx

Similar to Typical Reactions IGCSE CHEMISTRY Y11.pptx (20)

Recently uploaded

Recently uploaded (20)

Typical Reactions IGCSE CHEMISTRY Y11.pptx