Exam tip; You DO NOT need to remember technical details
of the blast furnace
Prior Learning;
a) Understand what happens to carbonates when
they are heated
b) Know that an ore contain a metal mixed with rock
c) Know how to work safely in the laboratory
Keywords:
displacement, electrolysis, ore, native, reduce, coke,
reduced, cast iron
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Learning Objectives:
By the end of the lesson I can:
•Explain where metals are obtained from.
•Give examples of how metals are extracted from the Earth.
Metals that are less reactive than carbon can be extracted from their
oxides by reduction in carbon, for example iron oxide is reduced in the
blast furnace to make iron.
•Identify that metals less reactive than carbon can be
extracted by reducing their oxides.
•Explain that iron is extracted in a blast furnace.
•Consider and evaluate the social, economic and
environmental impacts of exploiting metal ores, of using
metals and of recycling metals.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
1. Ores contain enough metal
to make it economic to
extract the metal and this
changes3.over
time.
Most
metals are
found as compounds
that require chemical
reactions to extract the
metal.
2. No metals are naturally
found in the Earth as the
metal itself.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
http://video.google.co.uk/videoplay?docid=9009946453212399554&ei=dTz8
SrWYLte2-Aat-6TfCg&q=reactivity+series&hl=en#
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
The Reactivity Series
Metals are arranged in order of how reactive they
are. A more reactive metal will displace a less
reactive one from its compounds.
is this type of reaction
ForWhat
example,
zinc will displace copper from copper sulfate to
give zincGENERALLY
sulfate plus copper. called?
What is the word and symbol equation?
zinc(s) + copper sulfate(aq)
zinc sulfate(aq) + copper (s)
Zn(s) + CuSO4 (aq)
ZnSO4 (aq)
+ Cu (s)
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
The more vigorously an element forms
compounds the harder it will be to get back
that element from its compounds.
For example, magnesium gives out lots of
heat when it combines with oxygen.
This means we will have to put lots of energy
back to extract magnesium from magnesium
oxide and so it will be hard to extract.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
What about gold?
How would you extract it?
An ore containing the element Au
Would
this
The element Au
work?
Why?
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Potassium
Metals ABOVE CARBON, because
Sodium
of their high reactivity, are
extracted by ELECTROLYSIS
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Copper
Silver
Gold
Platinum
Metals BELOW CARBON are
extracted by heating them with
carbon in a BLAST FURNACE
These LOW REACTIVITY metals won’t
need to be extracted because they are
SO unreactive you’ll find them on their
own, not in a metal oxide. These are
panned for!
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
REDOX REACTION: Extracting copper from Malachite
Malachite is a mineral known as Copper
Carbonate ( CuCo3)
What
process is
When malachite
is heated
needed to
with Carbon,
extract copper?
it is reduced (oxygen is removed)How
to leave
could you
behind copper metal.
do it in the lab?
Copper Carbonate + Carbon Monoxide
Copper metal + Carbon dioxide
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Reduction by carbon
RESULTS TABLE
Method
1. Put on your eye protection.
2. Add a REACTION
spatula (1 cm3) ofOBSERVATIONS
the metal oxide and carbon to your boiling
tube (ratio 1:1)
3. ClampCopper
the boiling tube so that it is sloping. Make sure the tube is
clamped
close&at its open end.
oxide
4. Add a loosely fitting mineral wool plug to the open end of boiling tube.
Carbon
5. Light your Bunsen burner.
Iron
6. Heat the
tube using a hot flame. Direct the tip of the inner blue cone
onto the mixture and away from the plastic on the clamps!!!!
oxide &
7. Observe what happens. Write your observation in your results table.
Carbon
8. Stop heating
and allow the reaction mixture to cool.
AT THIS POINT WE WILL STOP AND CONTINUE IN PERIOD 5
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
…to remove oxygen from a metal oxide
Removal of
oxygen from
a compound
A list of elements
from most to
least reactive
A rock containing
enough metal to make it
economic to extract
…contain enough metal to make extraction economic
Unreactive
metals, found
as elements in
nature
Reduction
reactions are…
Metal ores are
rocks that…
native
Gold, platinum
& silver…
Reactivity series
reduction
ore
…native metals
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Prior Learning;
a) Understand what happens to carbonates when
they are heated
b) Know that an ore contain a metal mixed with rock
c) Know how to work safely in the laboratory
Keywords:
displacement, electrolysis, ore, native, reduce, coke,
reduced, cast iron
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Learning Objectives:
By the end of the lesson I can:
•Explain where metals are obtained from.
•Give examples of how metals are extracted from the Earth.
Metals that are less reactive than carbon can be extracted from their
oxides by reduction in carbon, for example iron oxide is reduced in the
blast furnace to make iron.
•Identify that metals less reactive than carbon can be
extracted by reducing their oxides.
•Explain that iron is extracted in a blast furnace.
•Consider and evaluate the social, economic and
environmental impacts of exploiting metal ores, of using
metals and of recycling metals.
EXT: Explain how electrolysis works and why it is not always used
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
…continuing on
1. Take an evaporating dish and add about
25 cm3 of sulfuric acid to it.
2. Take your (now cool) reaction mixture
and add it to the acid.
3. Observe what happens. Write your
observation in your results table.
4. Complete word and chemical equations
for your extraction.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Reactivity Series
Type of metal
High reactivity (i.e
anything above carbon)
Middle reactivity (i.e.
anything below carbon)
Extraction process
ELECTROLYSIS
BLAST FURNACE
(heating with
carbon to reduce
their oxides)
Low reactivity
PHYSICAL
EXTRACTION
Examples
Potassium, Sodium,
Calcium, Magnesium,
Aluminium
Zn, Fe, Sn, Pb, Cu
Silver, Gold,
Platinum
GCSE Core Chemistry
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of the blast furnace
Which substance is being oxidised? Reduced?
Iron oxide + carbon monoxide
iron + carbon dioxide
What are the molecular formulas?
& what do they mean?
CaCO3
Chemical: Calcium Carbonate
Fe2O3
Chemical: Iron (III) oxide
Common: Haematite
C
Chemical: Carbon
Common: Coke
Common: Limestone
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Blast furnace
Coke + oxygen gas (forms) carbon dioxide gas
Write the chemicalC reactions
+ O2 (forms)for
CO2the following
stages
in the
blast
furnace.
Carbon
dioxide
gas
+ coke
(forms) carbon monoxide gas
1. Hot air is blown
the blast
CO2 into
+ C (forms)
CO furnace
whichmonoxide
makesgas
the+ iron
coke
oxidise.
Carbon
(III)burn
oxide and
(forms)
iron metal
+ carbon dioxide
gas dioxide gas
2. At high temperatures,
carbon
Fe2Omore
(forms)and
2Fe is
+ 3CO
3 + 3COcoke
2
reacts with
reduced.
3. The resulting gas reacts with iron (III)
oxide causing it to reduce whilst the gas
oxidises in a ‘redox reaction’.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Iron Mining
Use you text (p41) and this video to
consider and evaluate the social,
economic and environmental impacts
of exploiting metal ores, of using
metals and of recycling metals.
http://www.youtube.com/watch?v=ruiydHeu
QSQ
(6 marks)
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Open-cast mining removes
ores using explosives. It
produces dust and can scar
the landscape. This disused
copper mine in Ajo, Arizona,
measures one mile wide.
Extracting metals causes
huge amounts of waste.
Copper production discards
99.5% of the extracted ore.
Harmful waste gases, including sulfur dioxide, carbon
dioxide and carbon monoxide, are produced by extraction.
Extraction, especially electrolysis, also uses lots of electricity.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
New mining techniques can decrease the effects of metal
extraction on the environment.
 Leaching uses less electricity than traditional
mining and does not produce waste gases.
Copper ores are treated with and dissolved in
dilute sulfuric acid, producing copper sulfate.
Electrolysis is then used to extract the copper.
Certain bacteria can also be used to dissolve
ores and form copper sulfate.
 Phytomining uses plants to absorb metals
from the soil. The process can be used to
clean contaminated land. Treating the plants
with certain chemicals increases their ability
to accumulate minerals in their cells.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Metals are easier to recycle than plastic and they retain
their original properties, such as conductivity and hardness.
 Recycling uses up to 95% less electricity
than producing metals from ores.
 Recycling costs less than extracting
metals and can be profitable.
 Recycling creates less waste and reduces
the number of sites that have to be mined.
One problem is that metallic materials in recycled objects are
often mixtures of different metals. This can mean that
obtaining pure metals from recycling is more expensive, as
it may use more electricity than extracting metals from ores.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Electrolysis is a process that uses electricity to
separate the elements in a compound. The word
electrolysis means ‘splitting with electricity’.
Electrolysis is expensive and so it is only
used to extract reactive metals that cannot
be extracted in other ways.
Aluminium is a reactive metal that is
found in the ore bauxite. It is combined
with oxygen as aluminium oxide.
Electrolysis is used to remove the
oxygen and extract aluminium, which
means that reduction takes place.
What is the word equation for the extraction of aluminium?
aluminium oxide
 aluminium
+
oxygen
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Copper is an excellent conductor and does
not corrode quickly. These properties make
it a good material for wiring and plumbing.
Only pure copper can be used for electric
wires. Even a very low level of impurities
will reduce copper’s conductivity.
Copper is not very reactive and
can occur native but it is rare to
find pure copper. Usually, it is found
combined with other elements,
such as in the ore malachite.
The copper extracted from compounds by reduction with
carbon is impure. Electrolysis can actually be used at this
stage to remove the impurities and obtain pure copper.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Impurities, iron ore (haematite), slag, coke,
reduced, road, limestone, oxidised, slag
A ……… furnace is used to reduce ………..
The solid raw materials are iron ore, ………..
and ………….
Coke is first …………. to carbon monoxide, and
this gas ………….. the iron ore. Limestone is
added to remove the …………. and makes
…………., which is used as ……. making
material and breezeblocks.
GCSE Core Chemistry
Exam tip; You DO NOT need to remember technical details
of the blast furnace
Learning Objectives:
By the end of the lesson I can:
•Explain where metals are obtained from.
•Give examples of how metals are extracted from the Earth.
Metals that are less reactive than carbon can be extracted from their
oxides by reduction in carbon, for example iron oxide is reduced in the
blast furnace to make iron.
•Identify that metals less reactive than carbon can be
extracted by reducing their oxides.
•Explain that iron is extracted in a blast furnace.
•Consider and evaluate the social, economic and
environmental impacts of exploiting metal ores, of using
metals and of recycling metals.
EXT: Explain how electrolysis works and why it is not always used
GCSE Core Chemistry