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(C) The Reactivity Series
of Metal and itsApplication
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Learning Objectives:
Compare the differences in the vigour of the reaction ofsome metals with oxygen.
Deduce the reactivity series of metal. Determine the positions of carbon and hydrogen in the
reactivity series of metal.
State what the reactivity series of metals are.
Describe the various applications of the change of
oxidation number in substances. Describe the existence of various types of ores in our
country.
Describe the extraction of iron and tin from their ores.
Explain the use of carbon as the main reducing agent inmetal extraction.
Describe the contribution of metal extraction industry tothe economy of our country
Use the reactivity series of metals to predict possiblereactions involving metals.
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Reactions of Metal with Oxygen
The more rapidly the metal burns in oxygen
and the brighter the flame produced, the
more reactive the metal is with oxygen.
It is used to build up the Reactive Series of
Metals
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The Reactivity Series of Metals
The RS is a series of metals
arranged in the order of howvigorously the metals react with
oxygen
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Experiment : To deduce the reactivity series of metals
Problem Statement:
How is the reactivity series of metals deduced from the reactionsof metals with oxygen?
Hypothesis:
The more reactive a metal, the more brightly and more rapidly themetal will burn in oxygen.
Variables:
MV: Type of metalRV : The intensity of the flame
FV : The amount of metal and potassium manganate(VII) used
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Apparatus Setup:
Apparatus:
Materials:
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Procedure:
1. Two spatula of potassium manganate(VII) crystals are placed
in a boiling tube.
2. A small quantity of glass wool is then placed inside the boiling
tube to prevent potassium manganate(VII) from spilling over.
3. A spatula of zinc powder is placed on a sheet of asbestos paper
and put inside the boiling tube.
4. The boiling tube is then clamped to a retort stand.
5. The zinc powder is heated strongly.
6. When the zinc powder has become very hot, potassium
manganate(VII) is heated strongly to produce oxygen gas.
7. The intensity of the flame or glow is recorded.
8. Steps 1 to 7 are repeated by replacing zinc powder with iron
powder, lead powder, copper powder and magnesium powder.
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Results:
Metal
Observation
Intensity of flame/glowColour of
hot oxide
Colour of
cold oxide
ZnBurns rapidly
Bright glowYellow White
FeBurns less rapidlyGlow less bright than burning
of Zn
Reddish-
brown
Reddish-
brown
PbBurns slowly
Faint glowBrown Yellow
Cu Faint glow Black Black
Mg
Burns very rapidly
Very bright white flame
produced
White White
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Conclusion
The reactivity of the five metals with oxygen
is as follows:
Mg > Zn > Fe > Pb > Cu
Reactivity decreases
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The Reactivity Series of Metals
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Apparatus Setup:
Apparatus:
Materials:
Carbonpowder
+ metal oxide
Asbestos
paper
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Procedure:
1. Two spatula of carbon powder are placed on a piece of
asbestos paper.
2. One spatula of zinc oxide is added to the carbon powder. The
zinc oxide and carbon powder are mixed uniformly.
3. The asbestos paper with its contents is placed on a wire gauze
over a tripod stand.
4. The mixture of zinc oxide and carbon is heated strongly for a
few seconds.
5. After this, the Bunsen flame is removed and the mixture
examined to determine whether it will continue to glow.
6. Steps 1 to 5 are repeated by replacing zinc oxide with
copper(II) oxide and aluminium oxide
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Results:
Mixture Observation
Reactivity of
Carbon
C + ZnOThe mixture glows brightly
A grey solid is formed
C is more
reactive than
Zn
C + CuO
The mixture burns with a bright
flame
A brown solid is obtain
C is more
reactive than
Cu
C + Al2O3 No changes
C is less
reactive than
Al
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Experiment : To determine the position of hydrogen in the RS
Apparatus:
Materials:
Figure 1
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Procedure:
1. Place one spatula of copper(II) oxide, CuO into a porcelaindish.
2. Place the porcelain dish into a combustion tube and clamp thetube horizontally.
3. Set up the apparatus as shown in Figure 1
4. Pass dry hydrogen gas through the combustion tube for a fewminutes to remove the air in the combustion tube.
5. Burn the excess hydrogen gas that flows out from the smallhole of the combustion tube.
6. Heat the copper(II) oxide, CuO in the combustion tubestrongly.
7. Observe any changes that occurs. Ensure that the hydrogen gas
is contineously flowing throughout this activity.8. Repeat steps 1 to 7 using zinc oxide, ZnO, lead(II) oxide, PbO
and iron(III) oxide, Fe2O3 respectively to replace copper(II)oxide, CuO
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Results:
Mixture Observation Inference
H2+ CuO
CuO burned brightly.
The black powder turned
brown.
Copper metal formed
H > reactive than Cu
H2 + ZnO No changes H< reactive than Zn
H2 + PbO
PbO burned brightly.
The yellow powder
became shiny grey
globules.
Lead metal formed
H > reactive than Cu
H2+ Fe2O3
Fe2O3burned brightly.
The brown powder
became shiny grey
globules.
Iron metal formed
H > reactive than Cu
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Conclusion
The position of H is between Zn and Fe in the
Reactivity Series:
Zn > H > Fe > Pb > Cu
Reactivity decreases
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Position of Carbon in RS
Carbon is between Aluminium and Zinc in
RS.
Carbon will reduce the oxide of metal X if
carbon is more reactive than metal X
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Position of Hydrogen in RS
Hydrogen is between zinc and iron in RS.
The position of hydrogen can be determined
by passing the hydrogen gas over hot metal
oxide
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Uses of RS in the Extraction of Metals
K
Na
Ca
Al
C
ZnFe
Sn
Pb
Cu
Hg
Ag
Au
Very Reactive Metal
- Their ores require strong reductionthrough electrolysis
Fairly Reactive Metal
- Their ores can be reduced by heating
strongly with carbon
Less Reactive Metal
- Their ores can be reduced by heating directly in the air
Least Reactive Metals
- They exist as uncombined element
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Why carbon?
It is cheap and widely available
Carbon dioxide gas produced during the
extraction process is non-poisonous
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Common Metals and their ores
Metal Ore
Main Mineral in
ore
Calcium Limestone CaCO3
Aluminium Bauxite Al2O3
IronHematite Fe2O3
Magnetite Fe3O4
Tin Cassiterite SnO2
Lead Galena PbS
Zinc Zinc blende (sphalerite) ZnS
copper Malachite CuCO3.Cu(OH)2
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Extraction of Iron1. Production of CO2
C + O2
CO2CaCO3CaO + CO2
2. Production of CO
C + CO22CO
3. Reduction of iron ore to iron
Fe2O3+ 3CO2Fe + 3CO2
Fe3O4+ 4CO3Fe + 4CO2Fe2O3+ 3C2Fe + 3CO
Fe3O4+ 2C3Fe + 2CO24. Removal of impurities
CaO + SiO2CaSiO3
limestone sand slag
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Extraction of Tin
Two main steps involved in the
extraction of tin are:
Concentration process
Reduction process
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Concentration process
1. Tin ores is concentrated by froth floatationmethod.
2. In this process, the tin ore is crushed to a finepowder and mixed with water and special oil
in a large tank.
3. The froth contains particles of concentratedtin ore.
4. The concentrated tin ore is then dried androasted to remove impurities such as carbon,sulphur and special oils.
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Reduction Process
1. The concentrated tin ore, SnO2is mixed with
coke and heated to a hightemperature(~1360C) in a furnace.
2. During heating, SnO2is reduced by carbon to
molten tin and carbon is oxidized to CO2andCO.
SnO2 + C Sn + CO2SnO2 + 2C Sn + 2CO
3. The CO produced can also reduced SnO2to tin.
SnO2 + 2CO Sn + 2CO2
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Practice C1. The oxide of metal X can be reduced by carbon but not hydrogen.
(a) identify the metal X(b) (i) write the equation for the reaction between the oxide of
metal X and aluminium powder.
(ii) identify the oxidizing and reducing agents in this reaction
2. (a) Give two reasons why carbon is chosen as the reducing agent in
the extraction of metals
(b) Chromium is extracted from chromium(III) oxide by heating a
mixture of aluminium powder and chromium(III) oxide strongly.
(i) write the equation for the reaction that occurs in this process.
(ii) what conclusion can be made regarding the reactivity of
chromium and aluminium.
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