Metals: Properties, Reactions & Extraction in Chemistry
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KS3 Chemistry
Metals
1 Forces and Motion
3 Waves
5 Solid Liquids Gases
6 Magnetism
7 Radioactivity
8 Astrophysics
Topics….
Lesson 1:Metals
Lesson 2:Metal Properties
Lesson 3:Metal and Non-metal Oxides
Lesson 4:Metals and Water
Lesson 5:Metals and Acid
Lesson 6:Displacement Reactions
Lesson 7/8:Test and Review
Lesson 9:Metals Extraction
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Revision Videos…
Metals Useful Information
Element of Death..... (Quick Review)
Questions
1.
Describe the idea of the
term “element”
2.
Where was the
polonium detected?
3.
How much polonium is
required in your body
to kill you.
4.
Suggest a reason why
some elements kill and
others are good for the
body?
(5mins)
On the 1st of November 2006, ex-Russian spy
Alexander Litvinenko met
friends for lunch in
London. He spent the night being sick. Days later his
hair fell out. His liver started to fail. By the end of the
month,
Litvinenko was dead.
Detectives suspected
murder.
Scientists detected polonium in
Litvinenko’s urine.
Polonium is radioactive. Just 0.000 000 000 007 g
of
it is enough to kill.
Polonium is a silver-grey solid at room temperature
which Marie and Pierre Curie discovered it in 1898.
Polonium is an
element.
Each element is made of its
own type of
atom
, which is unique to that element.
You can’t split an element into anything simpler. Each
element has its own symbol – the symbol for
polonium is Po. And every
element
has its own
properties.
Outstan
ding
Lesson 1: Metals
I
know
that
metals
conduct electricity whilst
non-metals
don’t AND some non-metals
have
low melting
points
++ I can
explain why
graphite is an exception to the
rule and is a non-metal that
conducts electricity
.
+
explain
how
atoms can
gain
or
lose
electrons to become
ions
, metal =
positive
(cation), non-metal =
negative
(anion)
+++ I can
explain
the concept of a
delocalised electron
Key Ideas….
Metals mostly conduct electricity
and have high melting points.
Lesson 1: Metals
Task 1: What is an electrical
current?
1) Explain
what an electric current
is.
2) What happens inside a metal
when it conducts.
Task 2: Formation of Ions
1)
Use the
diagrams
you have been given to
explain
how Li
2
O forms.
2)
Explain
how NaCl is formed and include a proper equation to explain the
electron movement?
Task 3: Formation of Ions
1)
Name
5 key properties of graphite.
2)
Explain
one
Physical
and one
electrical
property in detail.
Metals and Non-Metals – on a slant!
Non-metals have a diagonal line
which is confusing
This version has most of the elements and
clearly is a lot larger and the
transition
metals
show up as a much
bigger group
.
When the
lamp
is on, millions of electrons
pass through it every second. The electric
current through the lamp is due to
electrons passing through it. Each electron
carries a
tiny negative charge
. The rate of
flow of electrical charge is called the
current
. The filament of the torch lamp is a
fine metal wire.
Metals
conduct electricity because they
contain conduction (or sea of
delocalised
)
electrons. These
electrons
move about
freely
inside the metal. They are not
confined to a single atom as they would be
in an insulator such as plastic. When the
torch is switched on, the cell pushes
electrons
through the
filament
.
Insulators
can’t conduct electricity because all the
electrons are held in atoms.
What is an “Electric Current”
TASK:
1.
explain
what an electric
current is.
2.
What happens inside a metal
when it
conducts
.
https://youtu.be/Xe-SwR7iRyI
- No sound (shows Li
2
O)
https://youtu.be/PCZtnbxtXqE
– NaCl formation - 3mins
Formation of Ions – Ionic Bonding – Stealing!
Ions can be formed when a
metal reacts
with a non-metal
.
Atoms form ions in
order to gain an
full outer shell
i.e.
Lithium Oxide
to form an
ionic bond
.
Metal atoms
lose electrons to
get/achieve a full outer shell
.
Ionic bonds
form when the charges
between the
metal cation
and
non-metal
anion
are
equal
and
opposite
.
This means that 2 x Li
+
cations will
balance
with one O
−2
anions
.
This makes the formula for
lithium
oxide Li
2
O
•
Graphite is black,
shiny
and
opaque
.
•
Graphite is
insoluble
in water.
•
It has a
high melting point.
•
It is a
good conductor
of electricity. Each
carbon atom is bonded into its layer with
three strong covalent bonds. This leaves
each atom with a
spare electron
, which
together form a
delocalised 'sea'
of
electrons loosely bonding the layers
together. These
delocalised
electrons can
all move along together.
•
Graphite contains
layers
of carbon atoms. It
is used in
pencil leads
because the layers
easily slide onto the paper, leaving a black
mark. It is a component of many
lubricants
,
for example bicycle chain oil.
Graphite as a Conductor
Task…
•
Name 5 key properties of
graphite.
•
Explain one Physical and
one electrical property.
Why does solid Iodine Sublime… Low Melting Point (Challenge!)
Iodine molecules I
2
have strong bonds between the
atoms but
weak intermolecular forces
. They are called
van der Waals
forces and rely on
transient dipoles
.
Some electrons move to one side of the molecule
creating a +/- dipole. However, when you heat iodine
is quickly
sublimes
and does not have a liquid phase.
Sublimation
is the
endothermic
transition of a
substance directly from the solid to the gas phase
without passing through the intermediate liquid
phase.
Task…
Write a title and introduction
to your practical for how you
will investigate the
conductivity of materials.
Then
draw
your table (or use
the one given) and conduct
your investigation with a
partner recording your results.
Write a clear conclusion.
Apparatus
(for testing)
•
6V cells
•
Leads
•
Lamp
•
Croc Clips
Conductivity of Materials Practical
Task….
Write a clear title in your book
Write an introduction and
draw out the circuit you will
use to test each material
Create your own table to test
each of the materials and tick
or cross
Task…
Write a title and introduction
to your practical for how you
will investigate the
conductivity of materials.
Then
draw
your table (or use
the one given) and conduct
your investigation with a
partner recording your results.
Write a clear conclusion.
Apparatus
(for testing)
•
6V cells
•
Leads
•
Lamp
•
Croc Clips
Conductivity of Materials Practical
Task….
Write a clear title in your book
Write an introduction and
draw out the circuit you will
use to test each material
Create your own table to test
each of the materials and tick
or cross
Outstan
ding
Lesson 2: Metal Properties
I know several
basic
properties
that metals have
++ I can
explain
why a reaction
with aluminium is limited AND
what an
alloy
is.
+
describe
how metals may
be suited to a role and why
+++ I can
Key Ideas….
Know and explain some key
metallic
properties
Element of Beauty.....
Questions
1.
Give two properties of
platinum that are
typical of
most metals
?
2.
Give two properties of
platinum that explain why
it makes
good jewellery
?
3.
Suggest why platinum
might be used in the
manufacture of
hard disks
and
catalytic converters
?
(5mins)
Platinum is a silvery-white
element
. It’s not
poisonous. It’s a metal, so it conducts
electricity
well. Platinum does not react with most other
chemicals. It does not react with
dilute acids
. The
symbol for
platinum is Pt.
Platinum jewelry is
shiny
and popular. South
Americans probably made the first platinum
jewellery – including nose rings and
pendants – around 2000 years ago.
Now, computer hard disks store information in
layers of platinum and cobalt which is another
metal (symbol Co). Platinum in
catalytic
converters
reduces pollution from cars.
Platinum can form other compounds which have
various applications in photography, zinc etchings,
indelible ink,
plating
, mirrors, porcelain coloring
Metal Uses
Jewellery
should be; shiny, hard,
malleable and not react with water or air
easily. Good choice are;
gold, silver,
platinum
Electrical Wires
need to be ductile, a
good conductor of electricity, don’t react
with water or air. So copper or
aluminium choices. Copper is a better
conductor than aluminium.
Saucepans
have to be; good conductors
of heat, not react with water be
malleable, strong. Copper, aluminium or
stainless steel are all good choices.
Planes are often made from
low density,
Malleable, strong, nonreactive
aluminium.
Aluminium
does not react
with water or air because it forms a
protective coating
on its surface
Examples of Alloys
Examples of Alloys
H
2
0
Making Magnesium hydroxide…
A very clean magnesium ribbon has a mild
reaction with cold water, given below.
Mg
(s)
+ H
2
O
(g)
→ Mg(OH)
2(s)
+ H
2(g)
After several minutes,
hydrogen gas bubbles
form on its surface, and the coil of
magnesium
ribbon
usually floats to the surface. However,
the reaction is short-lived because the
magnesium hydroxide
formed is almost
insoluble
in water and MgO
forms a barrier
on
the
magnesium
preventing further reaction.
As a general rule, if a metal reacts with cold
water, a
metal hydroxide
is produced.
If it reacts with steam, the
metal oxide
is
formed.
Mg
H
2(
g
)
Common Examples of Alloys…
An
alloy
is a uniform mixture. It is made up of
two or more chemical elements of which at
least one is a metal.
An
alloy
has properties different from the
metals it is made of it may be
tougher
, more
resistant to
corrosion
or
lighter
.
Most
alloys
are made by melting the metals,
mixing them while they are liquid to form a
solution, then leaving them to cool and turn
solid again.
Some alloys have the original metal atoms
“
substituted
”
but some may have them added
“
interstitial”
to the structure OR it can be a
mixture of both ideas.
Duralumin
(aluminium, copper,
magnesium and manganese)
Stainless steel
(iron, carbon and
chromium), steel (iron and carbon)
Bronze
(copper and tin), brass
(copper and zinc)
Pewter
(tin, copper and antimony)
Task..
Draw your own diagram to show how
the metals combine, make a note to explain
the ideas.
Lesson 2: Metal Properties….
Alloys
An
alloy
is a uniform mixture. It is
made up of two or more chemical
elements of which at least one is a
metal. An alloy has properties different
from the metals it is made of. Most
alloys are made by melting the metals,
mixing them while they are liquid to
form a solution, then leaving them to
cool and turn solid again.
There are some common
alloys
:
Brass
is made of 35% zinc and 65%
copper and is used for musical
instruments, jewellery , taps and
decorative hardware.
Stainless steel
is made of 18%
chromium , 80.6% iron , 1% nickel and
0.4% carbon and is used for tableware
, cookware and surgical tools.
Steel
is made of 99% iron and 1%
carbon and is used for tools, car
bodies, machinery, girders and rails .
Steel is used in buildings.
Bronze
is made of 87.5% copper and
12.5% tin and is used for boat
hardware, screws and grill work.
Solder
is a mixture of lead and tin used
to join other metals together.
1)
a)
What is the alloy of zinc and copper called?
b)
What is the difference between steel and stainless
steel?
c)
Organise the information provided into a table with
three columns.
2) Solder is an alloy of tin and lead only.
The melting
point of solder depends on the percentages of tin and
lead mixed together
a)
What percentages of tin and lead are present in
the solder with the lowest melting point?
b)
Solder is also used in electronic circuit boards
apart from its low melting point, what other
property of solder makes it suitable for use in
electronic circuit boards?
3) The Falkirk Wheel is made of steel which is an alloy
a.
What is meant by the term alloy?
b.
The table gives information on the hardness of
some steel alloys. Predict the hardness of the
steel alloy containing 0.6% carbon.
4) Titanium can be mixed with other metals to make a
substance that is strong and lightweight.
Medical instruments can be made from a mixture of
metals containing
76% titanium, 4% zirconium and the
rest is other metals. Label your pie chart with this
information
5) Make an
informative
poster A4 on Alloys and their
uses. Include ideas from the internet and images if
possible.
Outstan
ding
Lesson 3: Metal and Non-metal Oxides
I know
that metals and non-
metals react with oxygen to make
oxides
++ I can
explain
in detail
environmental
problems associated with some oxides –
acid rain
and
rusting
+
describe
that metals make alkaline
oxides and non-metals make acidic
oxides and give examples
+++ I can explain how acid rain and sulfuric acid
is formed in a two stage reaction
Key Ideas….
How do we form oxides and what do
they do?
Mini Review Test
1)
Write the symbol for…. (6 marks)
a)
Aluminium
b)
Potassium
c)
Carbon
d)
Calcium
e)
Sodium
f)
Lithium
2) Which of these are metallic properties (4 marks)
a)
Shiny
b)
Brittle
c)
Insulator
d)
Conductor of heat and electricity
e)
Malleable
f)
Dull
g)
Solid at room temperature
3) Name the following compounds:
•
NaF
•
CuS
•
LiNO
3
4) Name the elements in… CuSO
4
.5H
2
O
Total:
17
Answers…
1)
•
Al
•
K
•
C
•
Ca
•
Na
•
Li
2) a, d, e, g
3
•
Sodium Fluoride
•
Copper Sulphide
•
Lithium Nitrate
4) Copper, Sulphur,
Oxygen, Hydrogen
SA
Making Magnesium Oxide – Pupil Experiment
Example Method
1)
Glasses on, hair and tie back, blazer off.
2)
Setup a
Bunsen burner
and
mat
and connect to
the gas supply. Ensure the
airhole
is closed.
3)
Have a
beaker
of
water
or a
watch glass
ready
next to your Bunsen burner.
4)
Heat the
magnesium ribbon
until it starts to ignite
LOOK AWAY
to prevent it burning your retina.
5)
Take the
white oxidised powder
and stir into the
water or watch glass to check pH
6)
Add a few drop of UI and check the pH against a
scale.
Conclusion…
Decide
what colour the dissolved MgO is on the
periodic table?
Review the chemical equations below and check
they are balanced…
2Mg + O
2
2MgO
MgO + H
2
O
Mg(OH)
2
MgO + H
2
O
Mg
2+
+ 2OH
-
Metals or Non-Metals & Oxygen
Many metals and non-metals react with
oxygen in the air when they are heated to
produce
metal oxides
and
non-metal oxides
.
Steel wool burns brightly to form Fe
2
O
3
We place some
sulfur
on a
deflagrating spoon
and heat. Then we put the sulfur into a glass
jar with oxygen gas to react and form sulfur
dioxide gas. If we add water to the jar we can
form sulfuric acid (acid rain) and test for
acidity.
S(s) + O
2
(g)
SO
2
(g)
https://youtu.be/K
DaNg7OjMdQ
Task…
1.
Watch the video
2.
Copy the table into your
book
3.
Discuss how these reactions
may effect the rain?
Making Magnesium Oxide – iGCSE Extension Method
https://youtu.be/OuFqtxZJRvM
1) Find the mass
of a crucible
2) Find the mass of a
crucible + Mg ribbon
3) Heat the ribbon
4) Lift the lid
to allow O
2
to
mix and react
FLASH DANGER
5) Add water to dissolve the
MgO and freeing Nitrogen (
if it
has reacted to form ammonia
NH
3
)
to get pure MgO
6) Heat until you have
dried the pure white MgO
and H
2
O has evaporated
7) Allow to cool in the
crucible
8) Weigh your new product
taking into account the
original readings
Acid Rain -
Sulfur dioxide and carbon monoxide
Lichens
can be used as biological indicators of sulfur dioxide pollution. They grow in
exposed places such as rocks or tree bark, which means they easily absorb water and
nutrients to grow there. Rainwater contains just enough nutrients to keep them alive.
Air pollutants dissolved in rainwater, especially sulfur dioxide, can damage lichens and
prevent them from growing. This makes lichens natural indicators of air pollution. For
example:
•
bushy lichens need really clean air
•
leafy lichens can survive a small amount of air pollution
•
crusty lichens can survive in more polluted air
In places where no lichens are growing it is often a sign that the air is heavily polluted
with sulfur dioxide. Trees and limestone buildings are also damaged by acid rain.
Carbon monoxide
, CO, is produced when fuels burn in a
limited amount of air. It is a colourless, odourless and
tasteless gas. Carbon monoxide passes into the
red blood
cells
after breathing it in. It binds more strongly
to
haemoglobin
than oxygen does, so the blood will be
able to carry less oxygen than it should. This can cause
tiredness, unconsciousness and even death.
Fossil fuels naturally contain sulfur compounds. These
produce
sulfur dioxide
, a gas with a sharp, choking smell,
when the fuel is burned. When sulfur dioxide dissolves in
water droplets in clouds, it makes the rain more acidic than
normal. This is called
acid rain
.
Acid rain
damages the waxy layer on the leaves of trees.
This makes it more difficult for trees to absorb the minerals
they need for healthy growth and they may die. Acid rain
also makes rivers and lakes too acidic for some aquatic life
to survive.
Task…
Read the article discuss with a partner the
key issues surrounding acid rain
Greenhouse Effect (Review)
Some gases in the Earth's atmosphere absorb
infrared
radiation
. These gases are called
greenhouse gases
and
they keep our planet warm.
Carbon dioxide
is a
greenhouse gas. Even though it is only 0.04% of the
atmosphere, carbon dioxide is the key.
Other greenhouse gases are
water vapour
, and also
methane
. Even though methane is only present in tiny
amounts, it is a very efficient absorber of infrared.
The
greenhouse effect
is a natural process that keeps
the Earth’s atmosphere warm. This has been essential to
the evolution of life as we know it.
Since the
Industrial Revolution
, humans have been
releasing greenhouse gases into the atmosphere faster
than natural processes can remove them. For example,
burning
fossil fuels
releases carbon dioxide.
The extra carbon dioxide increases the greenhouse
effect, which makes the planet warmer than it would be
naturally. The increase in global temperature this causes
is called
global warming
.
Global warming
is beginning to trigger big changes in the
environment. The average temperature of the
atmosphere and oceans is increasing slightly every
decade, and this is already causing polar ice caps to melt
and sea levels to rise.
1.
The Sun’s rays enter the Earth’s atmosphere.
2.
Energy is absorbed by the Earth’s surface and re-emitted at
longer
wavelengths
, such as infrared radiation (heat).
3.
Some emitted heat passes through the atmosphere into space.
4.
Some heat is absorbed by carbon dioxide, a greenhouse gas. Heat is re-
emitted in all directions and some becomes trapped within the Earth’s
atmosphere. The Earth becomes hotter as a result.
Task…
Read
the article on global warming and
highlight
any
key ideas
“Rusting” - Oxidation
https://youtu.be/q0CAfXV-YdY
Iron
is a good example of “
rusting
” or
oxidation
. The metal
will slowly break down by a simple reaction on the
surface
which then eventually breaks away to leave
fresh iron
and
process starts again.
Iron + oxygen + water
Hydrated Iron (III) Oxide
We can also stop this process by removing any of the
reactants
from the situation. When we say that the iron is
oxidised
we mean electrons are removed to make a +3 ion.
Task…
Make your own notes on the idea of
rusting as a chemical concept.
(Removal of
electrons)
(addition of
electrons)
Rusting Demonstration
4 jars were setup with iron nails
so they could “rust”
We then waited for 3 days to see
the results
Then we shook the jars to see
how that would change the
outcomes.
Which one is rusts more and
why?
Why did the boiled water make
no difference?
https://youtu.be/V-0wocipCcI
3mins
Outstan
ding
Lesson 4: Metals and Water
I
know
that different
metals have different
reactivity in group 1
++ I can
explain
how some
metals will react with steam
+
describe
how
metals
react with water to make
metal hydroxide solutions
and hydrogen
+++ I can write some equations to explain the
reactions of metals and water
Key Ideas….
What happens when you mix a metal
and water from Group 1
Reactivity of Metals
The reactivity series will need
to be learned for GCSE.
Group
1 metals
feature in this series.
Each metal has a similar
reaction with water.
The
metal
reacts with
water
to
form
hydroxides
which are
soluble in water or
alkaline
in
nature. We can test for the
presence using litmus paper or
indicator solution. The
reaction is also
exothermic
and gives off heat.
They also emit
hydrogen gas
which is flammable.
Group 1 Metal + Water → Metallic Hydroxide + Hydrogen
2Na
(s)
+ 2H
2
O
(l)
→ 2NaOH
(aq)
+ H
2
(g)
Task..
Explain
this idea and
write
down the
equations (check
that they they
balance
)
Li, Na, K -
https://youtu.be/Tzl4kGneIp
Y
Rb, Cs -
https://youtu.be/-
p2kpZRWxM8
Group 1 Metals
The pattern for group 1 metals is simple and the reasoning is that
there is
one electron
in the outer shell which is
easily lost
to another
atom.
As you get further down the periodic table the atoms get larger
(
Francium
) and the electron is less tightly held (or
shielded
from the
charge in the nucleus). Hence it reacts more easily.
Tasks:
Make a note of use for
each metal shown in the
table.
Can you comment on why
the reactivity changes?
Can you predict and
balance a reaction of
Rb
with water
2Na
(s)
+ 2H
2
O
(l)
→ 2NaOH
(aq)
+ H
2
(g)
Elements of Life.....
Potassium
is vital to life. It keeps your heart,
kidneys and nerves working. A shortage of
potassium
makes people weak, confused and
depressed, and can even cause
heart attacks
.
No one eats pure
potassium
– the element catches
fire when it touches water. Instead, we eat
compounds
that contain
potassium
.
Eating too much ordinary table salt (
sodium
chloride
) is harmful to health. So some people eat
‘salt substitutes’, which are a mixture of
potassium
chloride
and
sodium chloride
. Foods like raisins,
peanuts
and bananas are rich in
potassium
compounds
.
Tasks:
Discuss with a partner
why Potassium is
important in our bodies?
Outstan
ding
Lesson 5: Metals and Acids
I know what MASH
stands for!
++ I can
explain
what products are
produced and the pattern
+
complete a practical which
shows a reactivity series for
metal + acid (MAZIT)
+++ I can write
word
and symbol equations for
reaction of metals with acids.
Key Ideas….
MASH & MAZIT?
Exam Review Question /3
1.
Copper is a metal.
At room temperature
copper is a strong solid. Give
two
other
properties of copper that show it is a
metal. (2)
2.
When copper metal is heated it reacts
with a gas in air
What is the chemical name of the
product
formed when copper reacts with
a gas in
air? (1)
Answers…
1)
•
it conducts electricity or
heat
•
ductile/ malleable
•
high melting/ boiling point
•
it is shiny / sonorous
•
it forms basic oxides’
2)
CuO – Copper Oxide
MASH ??
MASH
is a really easy way to remember
how acids and metals react.
They all have the same generic
reactants and products…
Metal + Acid → Salt + Hydrogen
magnesium + sulfuric acid →
magnesium sulfate + hydrogen
Mg(s) + H₂SO₄(aq) → MgSO₄(aq) + H₂(g)
Iron + sulfuric acid → iron sulfate +
hydrogen
Fe(s) + H₂SO₄(aq) → FeSO₄(aq) + H₂(g)
Task…
1.
Write
out and
explain both
check
they are balanced.
2.
Make a
note
of what
MASH
means
and how it works.
3.
Explain
how the acid changes the
salt
Practical....
You have been given the following
equipment and need to design an
experiment to test this out...
1.
A test tube and test tube rack.
2.
Measuring cylinder
3.
Some samples of metal:
•
Iron (Fe)
•
Zinc (Zn)
•
Magnesium (Mg)
•
Lead (Pb)
4.
Hydrochloric Acid 16 cm
3
(dilute)
5.
Wooden Split & bunsen (need to
light it)
A student has a
hypothesis
.....
“I think that different metals will react more or less strongly with hydrochloric acid”
Make sure you
clearly
show the
following in your work....
1.
Title/Hypothesis (copied)
2.
Equipment List
3.
Diagram (use a ruler)
4.
Method of steps to make a
“fair test”
5.
Results Table with obs
6.
Analysis (what you conclude)
Extra Help/ Hints..
If you get stuck ask to see the extra
sheets for a quick look
Extra Help...
Reacting Acids with Metals...
“I think that the different metals will react
more or less strongly with hydrochloric acid”
Method
1.
I will setup .......
Analysis
I think that ........
Diagram:
Extra Special Help...
Reacting Acids with Metals...
“I think that the different metals will react
more or less strongly with hydrochloric acid”
Method
1.
I will setup a small sample of each metal
in turn with the 4cm
3
of acid.
2.
I will place my finger over the end of the
tube to collect any gas and observe the
fizzing reactions
3.
When the fizzing slows down I will light a
split and “pop” the gas.
Analysis
…….
Extra Special Help...
Reacting Acids with Metals...
“I think that the different metals will react
more or less strongly with hydrochloric acid”
Method
1.
I will setup a small sample of each metal
in turn with the 4cm
3
of acid.
2.
I will place my finger over the end of the
tube to collect any gas and observe the
fizzing reactions.
3.
When the fizzing slows down I will light a
splint and “pop” the gas.
Analysis
I think that the gas given off (hydrogen)
shows which is the most reactive metal which
in this case is clearly magnesium as there was
the most………………..
Review Questions Metals and Acids
Answers…
1.
Use the same amount of acid in each test tube, use
pieces of metal that are the same mass or size (or any
other sensible suggestions).
2.
The acid and metal mixture effervesces or exothermic
3.
Magnesium, zinc, iron, lead.
(MAZIT)
4.
Hydrogen, squeaky pop test, with a lit splint.
1.
How can you make his
experiment a fair test?
2.
Give one sign showing that
chemical reactions are going on?
3.
What is the reactivity order,
starting with the most vigorous?
4.
What is the gas given off and
how do you test of it?
MAZIT
M
A
Z
I
T
MAZIT
is a really easy and simple way to
remember some of the reactivity series.
Start with “M”
Magnesium
as most reactive
down to “T”
Tin
the Least.
Task…
Make a note of this idea “MAZIT”
Metals and Acids – Review 3 mins
Task…
Watch this expanded group
of metals and see how this
compares to your sheet.
https://youtu.be/Na_6j9y9ke8
M
A
Z
I
T
MAZINTL???
Task…
If you are now happy with MAZIT then why not try out….
MAZINTL!
Police
Sergeant
Charlie
MAZINTL
Caught
Me
Stealing
Gold
Plate
Outstanding
Lesson 6: Displacement Reactions
I
know
the reactivity series
++ I can
explain several
example
reactions and give
evidence
for why
they occur and how they are useful.
+
I can
use
the reactivity
series to predict whether a
reaction
will occur.
+++ I can write displacement word equations
which are
balanced
Key Ideas….
How do these reactions work and how
is it linked to the reactivity series?
What is a displacement reaction?
A
displacement
involves a
metal
and the
compound
of a
different
metal
.
A
more reactive metal
will
displace
or
push
out a less
reactive metal
from its
compound in a
displacement
reaction. The least
reactive metal
is left on its own
after the reaction. It is no longer
chemically bonded
to any other elements. It is
now a
pure element
.
So
anything higher
on the series i.e. Lithium will be able to split up any lower
elements which are in a compound.
The image shows an example for
how
magnesium
can displace
copper
which then falls out of solution as a
precipitate
.
We can see the change of
colour
in
the
solution
as a 2
nd
piece of
evidence for the change in this case
but there may be
no visible change
.
What is a displacement reaction?
Magnesium
is more reactive than
copper
. When a piece of
magnesium
is dipped into
blue copper sulfate
solution, a
displacement reaction occurs.
This is the word equation:
magnesium + copper sulfate → copper +
magnesium sulfate
This is the symbol equation:
Mg
(s) +
Cu
SO₄(aq) →
Cu
(s) +
Mg
SO₄(aq)
This reaction cannot happen in reverse. Copper
cannot
displace magnesium from a compound because copper is
less reactive than magnesium.
Mg
(s) +
Cu
SO₄(aq) →
Cu
(s) +
Mg
SO₄(aq)
Mg
(s) +
Cu
SO₄(aq) →
Cu
(s) +
Mg
SO₄(aq)
Thermite Reaction
The
blast furnace
is used to produce iron on a large
scale. Sometimes, it is necessary to produce a small
amount of iron more quickly, for example if
railway
workers
need to produce molten metal to fix a broken
rail.
The
thermite reaction
uses aluminium powder
and
iron(III) oxide
. When ignited, the mixture reacts
vigorously because of the
large difference
in
reactivity
between
aluminium
and
iron
. The
heat
produced in the
reaction melts the iron produced.
iron(III) oxide + aluminium → iron + aluminium oxide
Fe
2
O
3
(s) + 2Al(s) → 2Fe(l) + Al
2
O
3
(s)
In this reaction,
iron oxide
loses
oxygen
to form
iron
so
the iron(III) oxide is
reduced
. The
Aluminium
is more
reactive that Iron and so steals the
oxygen
.
https://youtu.be/5uxsFglz2ig
- Thermite Welding of Train Tracks (3mins 48)
Task…
Write a short
note of how this works
Task…
Work out which metal is the most reactive and
which is the least by logical deductions…
Lesson 6: Displacement Reactions (Competition Reactions)
Task 1:
Task 2:
Task 1 My Deductions:
Task 2 My Deductions:
Task…
Work out which metal is the most reactive and
which is the least by logical deductions…
Lesson 6: Displacement Reactions (Competition Reactions)
Task 1:
Task 2:
Task 1 My Deductions:
Task 2 My Deductions:
Task 1: Using competition reactions to investigate reactivity
A
reactivity series
can be produced by carrying
out several competition reactions. A metal is
mixed with a metal oxide and heated to see if a
reaction takes place.
Different combinations
of metal and metal
oxide are tested. The table shows the results of
one of these investigations.
Answers….
Metal B
is the most reactive - it reacts
with both A oxide and C oxide.
Metal C
is the least reactive - it does
not win the competition reaction with
either A oxide or B oxide.
The order of
reactivity
of these metals
is therefore
B > A > C
.
Task…
Work out which metal is the most
reactive and which is the least by logical
deductions…
Task 2: Using competition reactions to investigate reactivity
Answers….
•
magnesium could displace lead and iron,
•
iron could only displace lead
•
lead could not displace magnesium or iron.
The order of reactivity is
magnesium > iron > lead
Task…
Work out which metal is the
most reactive and which is the
least by logical deductions…
Task 1
Use the reactivity series to predict the following
reactions, write each one out….
1. copper oxide + magnesium
2. lead nitrate + tin
3. lead chloride + iron
4. copper sulphate + calcium
5. aluminium + silver chloride
6. iron oxide + carbon
Task 2
Look at this list of reactions. Use your reactivity
series to predict which reactions will take place.
Complete the reactions that will take place, put a
cross by the ones that will not. (having written them
out)
1. aluminium + zinc oxide
2. sodium chloride + aluminium
3. zinc sulphate + copper
4. calcium chloride + iron
5. magnesium + silver nitrate
Reactions Practice…
Answers
Task 1
1 magnesium oxide + copper
2 tin nitrate + lead
3 iron chloride + lead
4 calcium sulphate + copper
5 aluminium chloride + silver
6 iron + carbon dioxide
Task 2
1. aluminium + zinc oxide zinc +
aluminium oxide
2. sodium chloride + aluminium x
3. zinc sulphate + copper x
4. calcium chloride + iron x
5. magnesium + silver nitrate silver nitrate
+ magnesium
Remember:
a metal element
higher in the table will displace
(pinch) the nonmetal element(s)
(e. g. oxygen) or their salts (e.g.
sulphate), from a metal lower in
the reactivity series. These are
displacement reactions
KS3 Chemistry
Atoms, Elements and
Compounds
1 Forces and Motion
3 Waves
5 Solid Liquids Gases
6 Magnetism
7 Radioactivity
8 Astrophysics
Review
5.1 Elements & compounds quiz
Which substance is a compound?
(a) Carbon dioxide
(b) Silver
(c) Oxygen
(a) Carbon dioxide
5.1 Elements & compounds quiz
Match the names to the symbols:
Carbon
Calcium
Oxygen
Ca
O
C
5.1 Elements & compounds quiz
Match the names to the symbols:
Hydrogen
He
H
Iron
Fe
Helium
I
Iodine
About 1000 years ago, Al-Biruni of Persia studied gemstones.
He used this apparatus to measure their densities.
5.6 Genuine gem?
Which gem?
Outstanding
Lesson 9: Metal Extraction
I
know
metals can displace
others in reactions.
++ I can
explain several
example
reactions and give
evidence
for why
they occur and how they are useful.
+
I can
use
the reactivity
series to
predict
whether a
metal can be extracted
+++ I can write displacement word equations
which are
balanced
Key Ideas….
How do these reactions work and how
is it linked to the reactivity series?
Iron Extraction
6mins
Aluminium Extraction
6mins
Copper Extraction
6mins
Summary of Extraction
This table shows how they are usually extracted from ores due to the reactivity.
Metal Extraction – Worksheet 1
Metals and Water
When a
metal
reacts with water, a
metal
hydroxide
and
hydrogen
are formed. For example,
sodium
reacts rapidly with
cold
water.
In general, the more reactive the metal, the more rapid the
reaction is
;
Sodium + water → sodium hydroxide + hydrogen
2Na(s) + 2H
2
O(l) → 2NaOH(aq) + H
2
(g)
Metals and Dilute Acids
When a metal reacts with a dilute
acid
, a
salt
and
hydrogen
are formed. For
example, magnesium reacts rapidly with dilute hydrochloric acid:
Magnesium + hydrochloric acid → magnesium chloride + hydrogen
Mg(s) + 2HCl(aq) → MgCl
2
(aq) + H
2
(g)
The more reactive the metal, the more rapid the reaction is. But, a metal below
hydrogen in the reactivity series will not react with dilute acids.
Ores
Unreactive metals
such as gold are
often found in the Earth's
crust
as an
element
. However, most metals are
found combined with other elements to
form
compounds
. Most metals are
extracted from
ore
found in the Earth's
crust. An
ore
is a rock that contains
enough of a
metal
or a
metal
compound
to make extracting the
metal worthwhile.
A
l
t
h
o
u
g
h
a
n
u
n
r
e
a
c
t
i
v
e
m
e
t
a
l
i
s
f
o
u
n
d
a
s
t
h
e
m
e
t
a
l
i
t
s
e
l
f
,
c
h
e
m
i
c
a
l
r
e
a
c
t
i
o
n
s
a
r
e
o
f
t
e
n
n
e
e
d
e
d
t
o
r
e
m
o
v
e
o
t
h
e
r
e
l
e
m
e
n
t
s
t
h
a
t
m
i
g
h
t
c
o
n
t
a
m
i
n
a
t
e
i
t
.
A
n
e
x
a
m
p
l
e
f
o
r
t
h
i
s
w
o
u
l
d
b
e
g
o
l
d
.
(
t
o
p
i
m
a
g
e
)
o
r
B
a
u
x
i
t
e
w
h
i
c
h
i
s
a
r
e
d
c
o
l
o
u
r
e
d
r
o
c
k
A
l
(
O
H
)
3
Questions…
1.
Explain
in your own
words
the trend for
metals
how they react with
water
?
2.
Do the same for
Acids
+
Metals?
3.
Explain
the dif
ference between an ore and an element?
4.
Describ
e
verbally
to another student in your own words / diagrams how iron and
aluminium are extracted from their ores using the reactivity series using the
printed resources
.
Iron(III) oxide
is reduced to molten iron when it reacts
with carbon. One of the products is carbon monoxide:
iron(III) oxide + carbon → iron + carbon monoxide
Fe
2
O
3
(s) + 3C(s) → 2Fe(l) + 3CO(g)
This method of extraction works because carbon is
more reactive than iron, so it can
displace
iron from
iron compounds.
Extracting a metal by heating with
carbon
is cheaper
than using
electrolysis
.
Metal Extraction – Information Sheet
Metal Extraction – Worksheet 2
Questions…
1.
Use the information above to draw a poster to show both the reactions with reactants, products and
methods clearly shown and annotated with labels.
2.
What do
the (s) (l) (g) mean for each equation?
3.
What product is given off for both reactions?
4.
Comment
on how mining and processing of copper ores can effect the environment and atmosphere?
5.
Why must the copper oxide and c
harcoal (carbon) be ground up finely?
6.
How
do we see that CO2 is escaping the surface of the powder when heated?
7.
How might you extract any carbon and Copper oxide from the Copper at the end of the process. Draw a
diagram to show your ideas.
8.
What do you think the term “Thermal Composition” mean?
(Hint… Reaction 1)
9.
How does the reactivity series apply to this process?
(Hint… Reaction 2)
Metal Extraction – Worksheet 2
-
Answers
2.
Solid, Liquid and Gas
3.
CO
2
gas
4.
The reactions will release CO2 and that might accelerate global warming. Also any industrial
processes might also leave waste products which could enter an ecosystem and effect
animals and plants in that area or contaminate drinking water.
5.
The increased surface area makes the reaction happen more quickly and also uses up more
reactant to produce more prod
ucts.
6.
Little puffs in the powder can be seen as they CO2 escapes with high Kinetic Energy store.
7.
Potentially a small sieve system, water to wash away the lighter chemicals, some solvent to
make the powder more soluble (then filter)
8.
When you heat a carbonate the CO
2
will separate.
9.
When you react two compounds or elements which have a difference on the reactivity series
one will bond more easily and take a molecule such as oxygen or element away from another
bond.
What is a displacement reaction?
When
metals
react with other
substances, the
metal
atoms
lose
electrons
to
form positive
ions
.
The
reactivity series
of metals is a
chart showing metals in order of
decreasing
reactivity
. In general,
the more
reactive
a metal is:
•
the more vigorous its
reactions are
•
the more easily it loses
electrons in reactions to form
positive ions (cations)
The table summarises some reactions of
metals in the reactivity series.
Hydrogen and carbon are shown for
comparison.
Reactions of metals with water
When a
metal
reacts with water, a
metal
hydroxide
and
hydrogen
are formed.
For example,
sodium
reacts rapidly with
cold
water.
In general, the more reactive the metal, the
more rapid the reaction is.
Sodium + water → sodium hydroxide + hydrogen
2Na(s) + 2H
2
O(l) → 2NaOH(aq) + H
2
(g)
Reactions of metals with dilute acids
When a metal reacts with a dilute
acid
, a
salt
and
hydrogen
are formed. For
example, magnesium reacts rapidly with dilute hydrochloric acid:
Magnesium + hydrochloric acid → magnesium chloride + hydrogen
Mg(s) + 2HCl(aq) → MgCl
2
(aq) + H
2
(g)
The more reactive the metal, the more rapid the reaction is. But, a metal below
hydrogen in the reactivity series will not react with dilute acids.
Ores v Metals
Unreactive metals
such as gold are often found
in the Earth's
crust
as an
element
. However,
most metals are found combined with other
elements to form
compounds
.
Most metals are extracted from
ore
found in
the Earth's crust. An
ore
is a rock that contains
enough of a
metal
or a
metal compound
to
make extracting the metal worthwhile.
A
l
t
h
o
u
g
h
a
n
u
n
r
e
a
c
t
i
v
e
m
e
t
a
l
i
s
f
o
u
n
d
a
s
t
h
e
m
e
t
a
l
i
t
s
e
l
f
,
c
h
e
m
i
c
a
l
r
e
a
c
t
i
o
n
s
a
r
e
o
f
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e
n
n
e
e
d
e
d
t
o
r
e
m
o
v
e
o
t
h
e
r
e
l
e
m
e
n
t
s
t
h
a
t
m
i
g
h
t
c
o
n
t
a
m
i
n
a
t
e
i
t
.
A
n
e
x
a
m
p
l
e
f
o
r
t
h
i
s
w
o
u
l
d
b
e
g
o
l
d
.
(
t
o
p
i
m
a
g
e
)
o
r
B
a
u
x
i
t
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w
h
i
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i
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d
c
o
l
o
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e
d
r
o
c
k
A
l
(
O
H
)
3
Extracting Iron (Blast Furnace)
Iron(III) oxide is reduced to molten
iron when it reacts with carbon.
One of the products is carbon
monoxide:
iron(III) oxide + carbon → iron +
carbon monoxide
Fe
2
O
3
(s) + 3C(s) → 2Fe(l) + 3CO(g)
This method of extraction works
because carbon is more reactive
than iron, so it can
displace
iron
from iron compounds.
Extracting a metal by heating with
carbon
is cheaper than using
electrolysis
.
iron(III) oxide + carbon → iron + carbon monoxide
Fe
2
O
3
(s) + 3C(s) → 2Fe(l) + 3CO(g)
Extracting Aluminium
Aluminium is more
reactive
than
carbon so it must be extracted from
its
compounds
using
electrolysis
which is an expensive process
.
Aluminium oxide is
insoluble
in
water, so it must be molten to act as
an electrolyte. However,
the
melting point
of
aluminium
oxide
is high.
A lot of
energy
must be transferred to break its strong
ionic bonds
, and this is
expensive. To reduce costs,
powdered aluminium oxide
is dissolved in
molten
cryolite
. (
a mineral consisting of a fluoride of sodium and aluminium).
This
compound melts at a
lower temperature
than
aluminium oxide
, reducing costs.
However, significant amounts of energy are required to melt the
cryolite
.
The diagram shows an electrolysis cell used to extract aluminium.
Both
electrodes
are made of
graphite
, a form of carbon with a high melting point
and which conducts electricity.
Extraction Methods
The
extraction
method used depends upon the metal's
position in the
reactivity series
. In principle, any metal
could be extracted from its compounds using
electrolysis
.
However, large amounts of
electrical energy
are needed
to do this, so electrolysis is expensive. If a metal is
less reactive
than
carbon
, it can be extracted from its
compounds by heating with carbon.
Copper
is an
example of this.
Copper
mostly occurs as
sulfide ores
,
which are heated in air to convert them to copper(II)
oxide.
Molten copper
can be produced from copper oxide
by heating with carbon:
Copper oxide + carbon → copper + carbon dioxide
2CuO(s) + C(s) → 2Cu(l) + CO
2
(g)
Copper oxide is
reduced
(addition of electrons) as carbon
is
oxidised
(removal of electrons)
so this is an example of
a
redox
reaction and a metal is produced at the end
.
Using the Reactivity Series
CuCO
3(s)
Heating
Heating
Copper oxide + carbon → copper + carbon dioxide
2CuO(s) + C(s) → 2Cu(l) + CO
2
(g)
Using the Reactivity Series
Explore the fascinating world of metals through lessons on their properties, reactions with water and acids, displacement reactions, extraction processes, and more. Delve into key terms, such as ions and reactivity series, while discovering how metals interact with various substances. Engage with revision videos demonstrating practical experiments and learn about the deadly element Polonium in a real-life case. Enhance your knowledge of metals with useful information and test your understanding with thought-provoking questions.
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Presentation Transcript
Topics. Lesson 1: Metals Lesson 2: Metal Properties Lesson 3: Metal and Non-metal Oxides Lesson 4: Metals and Water Lesson 5: Metals and Acid Lesson 6: Displacement Reactions Lesson 7/8: Test and Review Lesson 9: Metals Extraction KS3 Chemistry Metals 1 Forces and Motion 3 Waves 5 Solid Liquids Gases 6 Magnetism 7 Radioactivity 8 Astrophysics Animated Science 2022
Revision Videos Lesson Metals - Title /Link https://youtu.be/Xe-SwR7iRyI - No sound (shows Li2O) 30s 1 https://youtu.be/PCZtnbxtXqE NaCl formation - 3mins 2 https://youtu.be/T0acKc_GD70 - Alloys https://youtu.be/OuFqtxZJRvM Mg and O2 reaction to form MgO using crucible method https://youtu.be/naCFC8oZ_V0 - Simple burning Mg in air to get MgO https://youtu.be/KDaNg7OjMdQ - Sulfur burns in O2 to form SO2 and acid rain 3 https://youtu.be/nWdK1L7GXys - Burning Steel wool (5mins first half) https://youtu.be/V-0wocipCcI - Bottles and Nail to Show Rusting https://youtu.be/q0CAfXV-YdY - Rusting or Corrosion https://youtu.be/hEtjIHNh1Dk - Copper and Oxygen https://youtu.be/-xVgs60LmXg An experiment demonstrating the reaction of sodium, potassium, zinc, aluminium and iron (nail, steel wool and filings) with oxygen (5 mins) https://youtu.be/J-3lLPTuSG0 - Burning Metals in Air https://youtu.be/-p2kpZRWxM8 - Rubidium and Caesium in water (Seriously Fun!) 4 5 https://youtu.be/Na_6j9y9ke8 - Metals and Acids reactivity series 3mins 6 https://youtu.be/5uxsFglz2ig - Thermite Welding of Train Tracks (3mins 48) Animated Science 2022
Metals Useful Information Key Term Definition Ion Atom that has lost or gained an electron Reactivity Series Non- Metal a positively charged ion, i.e. one that would be attracted to the cathode in electrolysis. Property Metal Cation Potassium State at 25 C Sodium Solid usually S/L/G a negatively charged ion, i.e. one that would be attracted to the anode in electrolysis. Anion Reacts with Water Lithium MP High Low When an electron is free to roam inside a metal (or conductor) this carries the electrical current. Barium delocalised Elec or Thermal Conductivity Good Conductors Insulator Strontium Mixture of metal atoms (randomly) that have unique properties to the original metals i.e. stronger, low corrosion Calcium alloy Shiny (if polished) Magnesium Appearance Dull Reactivity series How we can order materials into how they react with water, acids or oxygen. Aluminium MAZIT! Density High Low Carbon MASH Metal + Acid Salt + Hydrogen Strength Hard / Strong Brittle Zinc alloy Mixture of two metals to improve the properties With Acids Chromium Oxidation With bases Oxidation / Rusting When metals react with oxygen and the metal is oxidised so electrons are removed and an oxide is made. Reacts with Acids Iron Malleability / Ductile deflagrating spoon A small long spoon that we put chemicals on to heat and test in a gas. Yes No Cadmium Cobalt Effervesces When a reaction gives off bubbles like Hydrogen gas. Nickel Tin Lead Hydrogen Antimony Bismuth Copper Unreactive Mercury Silver Gold Animated Science Platinum 2022
Element of Death..... (Quick Review) Questions On the 1st of November 2006, ex-Russian spy Alexander Litvinenko met friends for lunch in London. He spent the night being sick. Days later his hair fell out. His liver started to fail. By the end of the month, Litvinenko was dead. Detectives suspected murder. 1. Describe the idea of the term element 2. Where was the polonium detected? 3. How much polonium is required in your body to kill you. Scientists detected polonium in Litvinenko s urine. Polonium is radioactive. Just 0.000 000 000 007 g of it is enough to kill. 4. Suggest a reason why some elements kill and others are good for the body? (5mins) Polonium is a silver-grey solid at room temperature which Marie and Pierre Curie discovered it in 1898. Polonium is an element. Each element is made of its own type of atom, which is unique to that element. You can t split an element into anything simpler. Each element has its own symbol the symbol for polonium is Po. And every element has its own properties. Animated Science 2022
Mr D Powell 2022 Animated Science 2022 Lesson 1: Metals Key Ideas . Metals mostly conduct electricity and have high melting points. I know that metals conduct electricity whilst non-metalsdon t AND some non-metals have low melting points D/E + explain how atoms can gain or lose electrons to become ions, metal = positive (cation), non-metal = negative (anion) C ++ I can explain why graphite is an exception to the rule and is a non-metal that conducts electricity. B +++ I can explain the concept of a delocalised electron Animated Science 2022
Lesson 1: Metals Conductivity Material Task 1: What is an electrical current? Good Some Zero Copper 1) Explain what an electric current is. Nickel Aluminium 2) What happens inside a metal when it conducts. Tin Iron (large nail) Task 2: Formation of Ions Zinc Sulphur 1) Use the diagrams you have been given to explain how Li2O forms. Carbon 2) Explain how NaCl is formed and include a proper equation to explain the electron movement? Plastic (ruler) Card Task 3: Formation of Ions Rubber (tubing) Glass (beaker) 1) Name 5 key properties of graphite. 2) Explain one Physical and one electrical property in detail. Animated Science 2022
Metals and Non-Metals on a slant! Non-metals have a diagonal line which is confusing This version has most of the elements and clearly is a lot larger and the transition metals show up as a much bigger group. Animated Science 2022
What is an Electric Current When the lamp is on, millions of electrons pass through it every second. The electric current through the lamp is due to electrons passing through it. Each electron carries a tiny negative charge. The rate of flow of electrical charge is called the current. The filament of the torch lamp is a fine metal wire. Metals conduct electricity because they contain conduction (or sea of delocalised) electrons. These electrons move about freely inside the metal. They are not confined to a single atom as they would be in an insulator such as plastic. When the torch is switched on, the cell pushes electrons through the filament. Insulators can t conduct electricity because all the electrons are held in atoms. TASK: 1. explain what an electric current is. What happens inside a metal when it conducts. 2. Animated Science 2022
Formation of Ions Ionic Bonding Stealing! Ions can be formed when a metal reacts with a non-metal. Atoms form ions in order to gain an full outer shell i.e. Lithium Oxide to form an ionic bond. Metal atoms lose electrons to get/achieve a full outer shell. Ionic bonds form when the charges between the metal cation and non-metal anion are equal and opposite. This means that 2 x Li+cations will balance with one O 2anions. This makes the formula for lithium oxide Li2O https://youtu.be/Xe-SwR7iRyI - No sound (shows Li2O) https://youtu.be/PCZtnbxtXqE NaCl formation - 3mins Animated Science 2022
Graphite as a Conductor Graphite is black, shiny and opaque. Graphite is insoluble in water. It has a high melting point. It is a good conductor of electricity. Each carbon atom is bonded into its layer with three strong covalent bonds. This leaves each atom with a spare electron, which together form a delocalised 'sea' of electrons loosely bonding the layers together. These delocalised electrons can all move along together. Task Name 5 key properties of graphite. Graphite contains layers of carbon atoms. It is used in pencil leads because the layers easily slide onto the paper, leaving a black mark. It is a component of many lubricants, for example bicycle chain oil. Explain one Physical and one electrical property. Animated Science 2022
Why does solid Iodine Sublime Low Melting Point (Challenge!) Iodine molecules I2have strong bonds between the atoms but weak intermolecular forces. They are called van der Waals forces and rely on transient dipoles. Some electrons move to one side of the molecule creating a +/- dipole. However, when you heat iodine is quickly sublimes and does not have a liquid phase. Sublimation is the endothermic transition of a substance directly from the solid to the gas phase without passing through the intermediate liquid phase. Animated Science 2022
Conductivity of Materials Practical Conductivity Task . Good Material Some Zero Task Write a clear title in your book Copper Write a title and introduction to your practical for how you will investigate the conductivity of materials. Nickel Write an introduction and draw out the circuit you will use to test each material Aluminium Tin Iron Create your own table to test each of the materials and tick or cross Then draw your table (or use the one given) and conduct your investigation with a partner recording your results. (large nail) Zinc Sulphur Carbon Plastic (ruler) Card Write a clear conclusion. Apparatus (for testing) 6V cells Leads Lamp Croc Clips Rubber (tubing) Glass (beaker) Animated Science 2022
Conductivity of Materials Practical Conductivity Task . Good Material Some Zero Task Write a clear title in your book Copper Write a title and introduction to your practical for how you will investigate the conductivity of materials. Nickel Write an introduction and draw out the circuit you will use to test each material Aluminium Tin Iron Create your own table to test each of the materials and tick or cross Then draw your table (or use the one given) and conduct your investigation with a partner recording your results. (large nail) Zinc Sulphur Carbon Plastic (ruler) Card Write a clear conclusion. Apparatus (for testing) 6V cells Leads Lamp Croc Clips Rubber (tubing) Glass (beaker) Animated Science 2022
Mr D Powell 2022 Animated Science 2022 Lesson 2: Metal Properties Key Ideas . Know and explain some key metallic properties I know several basic properties that metals have D/E MgO(s) + describe how metals may be suited to a role and why C H20 ++ I can explain why a reaction with aluminium is limited AND what an alloy is. Mg B +++ I can Animated Science 2022
Element of Beauty..... Questions Platinum is a silvery-white element. It s not poisonous. It s a metal, so it conducts electricity well. Platinum does not react with most other chemicals. It does not react with dilute acids. The symbol for platinum is Pt. 1. Give two properties of platinum that are typical of most metals? 2. Give two properties of platinum that explain why it makes good jewellery? Platinum jewelry is shiny and popular. South Americans probably made the first platinum jewellery including nose rings and pendants around 2000 years ago. 3. Suggest why platinum might be used in the manufacture of hard disks and catalytic converters? Now, computer hard disks store information in layers of platinum and cobalt which is another metal (symbol Co). Platinum in catalytic converters reduces pollution from cars. (5mins) Platinum can form other compounds which have various applications in photography, zinc etchings, indelible ink, plating, mirrors, porcelain coloring Animated Science 2022
Metal Uses Jewellery should be; shiny, hard, malleable and not react with water or air easily. Good choice are; gold, silver, platinum Electrical Wires need to be ductile, a good conductor of electricity, don t react with water or air. So copper or aluminium choices. Copper is a better conductor than aluminium. Saucepans have to be; good conductors of heat, not react with water be malleable, strong. Copper, aluminium or stainless steel are all good choices. Planes are often made from low density, Malleable, strong, nonreactive aluminium. Aluminium does not react with water or air because it forms a protective coating on its surface Animated Science 2022
Examples of Alloys Animated Science 2022
Examples of Alloys Animated Science 2022
Making Magnesium hydroxide A very clean magnesium ribbon has a mild reaction with cold water, given below. H20 Mg Mg(s) + H2O(g) Mg(OH)2(s) + H2(g) After several minutes, hydrogen gas bubbles form on its surface, and the coil of magnesium ribbon usually floats to the surface. However, the reaction is short-lived because the magnesium hydroxide formed is almost insoluble in water and MgO forms a barrier on the magnesium preventing further reaction. H2(g) Mg(OH)2(s) H20 As a general rule, if a metal reacts with cold water, a metal hydroxide is produced. Mg If it reacts with steam, the metal oxide is formed. Animated Science 2022
Common Examples of Alloys An alloy is a uniform mixture. It is made up of two or more chemical elements of which at least one is a metal. An alloy has properties different from the metals it is made of it may be tougher, more resistant to corrosion or lighter. Most alloys are made by melting the metals, mixing them while they are liquid to form a solution, then leaving them to cool and turn solid again. Duralumin (aluminium, copper, magnesium and manganese) Some alloys have the original metal atoms substituted but some may have them added interstitial to the structure OR it can be a mixture of both ideas. Stainless steel (iron, carbon and chromium), steel (iron and carbon) Bronze (copper and tin), brass (copper and zinc) Task.. Draw your own diagram to show how the metals combine, make a note to explain the ideas. Pewter (tin, copper and antimony) Animated Science 2022
Lesson 2: Metal Properties. Alloys 1) a) What is the alloy of zinc and copper called? b) What is the difference between steel and stainless steel? c) Organise the information provided into a table with three columns. MP of solder oC % of tin An alloy is a uniform mixture. It is made up of two or more chemical elements of which at least one is a metal. An alloy has properties different from the metals it is made of. Most alloys are made by melting the metals, mixing them while they are liquid to form a solution, then leaving them to cool and turn solid again. 25 270 45 225 65 180 85 205 2) Solder is an alloy of tin and lead only.The melting point of solder depends on the percentages of tin and lead mixed together Carbon present in steel alloy% 0.1 0.2 0.3 0.4 0.5 0.6 a) What percentages of tin and lead are present in the solder with the lowest melting point? Solder is also used in electronic circuit boards apart from its low melting point, what other property of solder makes it suitable for use in electronic circuit boards? There are some common alloys: Hardness/ Units b) Brass is made of 35% zinc and 65% copper and is used for musical instruments, jewellery , taps and decorative hardware. 123 157 190 220 260 3) The Falkirk Wheel is made of steel which is an alloy Stainless steel is made of 18% chromium , 80.6% iron , 1% nickel and 0.4% carbon and is used for tableware , cookware and surgical tools. a. b. What is meant by the term alloy? The table gives information on the hardness of some steel alloys. Predict the hardness of the steel alloy containing 0.6% carbon. Steel is made of 99% iron and 1% carbon and is used for tools, car bodies, machinery, girders and rails . Steel is used in buildings. 4) Titanium can be mixed with other metals to make a substance that is strong and lightweight. Medical instruments can be made from a mixture of metals containing 76% titanium, 4% zirconium and the rest is other metals. Label your pie chart with this information Bronze is made of 87.5% copper and 12.5% tin and is used for boat hardware, screws and grill work. 5) Make an informative poster A4 on Alloys and their uses. Include ideas from the internet and images if possible. Solder is a mixture of lead and tin used to join other metals together. Animated Science 2022
Mr D Powell 2022 Animated Science 2022 Lesson 3: Metal and Non-metal Oxides Key Ideas . How do we form oxides and what do they do? I know that metals and non- metals react with oxygen to make oxides D/E + describe that metals make alkaline oxides and non-metals make acidic oxides and give examples C ++ I can explain in detailenvironmental problems associated with some oxides acid rain and rusting B +++ I can explain how acid rain and sulfuric acid is formed in a two stage reaction Animated Science 2022
Mini Review Test Answers 1) Al K C Ca Na Li 1) Write the symbol for . (6 marks) a) Aluminium b) Potassium c) Carbon d) Calcium e) Sodium f) Lithium 2) Which of these are metallic properties (4 marks) a) Shiny b) Brittle c) Insulator d) Conductor of heat and electricity e) Malleable f) Dull g) Solid at room temperature 2) a, d, e, g 3 Sodium Fluoride Copper Sulphide Lithium Nitrate 4) Copper, Sulphur, Oxygen, Hydrogen 3) Name the following compounds: NaF CuS LiNO3 SA Total: 17 4) Name the elements in CuSO4.5H2O Animated Science 2022
Making Magnesium Oxide Pupil Experiment Example Method 1) Glasses on, hair and tie back, blazer off. 2) Setup a Bunsen burner and mat and connect to the gas supply. Ensure the airhole is closed. 3) Have a beaker of water or a watch glass ready next to your Bunsen burner. 4) Heat the magnesium ribbon until it starts to ignite LOOK AWAY to prevent it burning your retina. 5) Take the white oxidised powder and stir into the water or watch glass to check pH 6) Add a few drop of UI and check the pH against a scale. Conclusion Decide what colour the dissolved MgO is on the periodic table? Review the chemical equations below and check they are balanced 2Mg + O2 2MgO MgO + H2O Mg(OH)2 MgO + H2O Mg2+ + 2OH- Animated Science 2022
Metals or Non-Metals & Oxygen Task 1. 2. Watch the video Copy the table into your book Discuss how these reactions may effect the rain? Many metals and non-metals react with oxygen in the air when they are heated to produce metal oxides and non-metal oxides. Steel wool burns brightly to form Fe2O3 3. We place some sulfur on a deflagrating spoon and heat. Then we put the sulfur into a glass jar with oxygen gas to react and form sulfur dioxide gas. If we add water to the jar we can form sulfuric acid (acid rain) and test for acidity. S(s) + O2(g) https://youtu.be/K DaNg7OjMdQ SO2(g) Element Type Reaction type Oxide Nature Highly exothermic - magnesium burns with bright white flame Magnesium oxide, MgO - solid white powder Magnesium Metal Basic exothermic - carbon glows orange when heated strongly Carbon dioxide, CO2- colourless gas with no odour Carbon Non-metal Acidic Sulfur dioxide, SO2- colourless gas with choking smell Sulfur Non-metal Burns slowly with a blue flame Acidic Animated Science 2022
https://youtu.be/OuFqtxZJRvM Making Magnesium Oxide iGCSE Extension Method 1) Find the mass of a crucible 5) Add water to dissolve the MgO and freeing Nitrogen (if it has reacted to form ammonia NH3) to get pure MgO 2) Find the mass of a crucible + Mg ribbon 6) Heat until you have dried the pure white MgO and H2O has evaporated 3) Heat the ribbon 7) Allow to cool in the crucible FLASH DANGER 8) Weigh your new product taking into account the original readings 4) Lift the lid to allow O2 to mix and react Animated Science 2022
Acid Rain - Sulfur dioxide and carbon monoxide Carbon monoxide, CO, is produced when fuels burn in a limited amount of air. It is a colourless, odourless and tasteless gas. Carbon monoxide passes into the red blood cells after breathing it in. It binds more strongly to haemoglobin than oxygen does, so the blood will be able to carry less oxygen than it should. This can cause tiredness, unconsciousness and even death. Fossil fuels naturally contain sulfur compounds. These produce sulfur dioxide, a gas with a sharp, choking smell, when the fuel is burned. When sulfur dioxide dissolves in water droplets in clouds, it makes the rain more acidic than normal. This is called acid rain. Acid rain damages the waxy layer on the leaves of trees. This makes it more difficult for trees to absorb the minerals they need for healthy growth and they may die. Acid rain also makes rivers and lakes too acidic for some aquatic life to survive. Lichens can be used as biological indicators of sulfur dioxide pollution. They grow in exposed places such as rocks or tree bark, which means they easily absorb water and nutrients to grow there. Rainwater contains just enough nutrients to keep them alive. Air pollutants dissolved in rainwater, especially sulfur dioxide, can damage lichens and prevent them from growing. This makes lichens natural indicators of air pollution. For example: bushy lichens need really clean air leafy lichens can survive a small amount of air pollution crusty lichens can survive in more polluted air In places where no lichens are growing it is often a sign that the air is heavily polluted with sulfur dioxide. Trees and limestone buildings are also damaged by acid rain. Task Read the article discuss with a partner the key issues surrounding acid rain Animated Science 2022
Greenhouse Effect (Review) CFC s Carbon Dioxide Methane Nitrous Oxide Haloalkanes Some gases in the Earth's atmosphere absorb infrared radiation. These gases are called greenhouse gases and they keep our planet warm. Carbon dioxide is a greenhouse gas. Even though it is only 0.04% of the atmosphere, carbon dioxide is the key. Refrigerators / Aircon Cattle Oil Gasoline Aerosols Fertiliser Coal Agriculture Other greenhouse gases are water vapour, and also methane. Even though methane is only present in tiny amounts, it is a very efficient absorber of infrared. The greenhouse effect is a natural process that keeps the Earth s atmosphere warm. This has been essential to the evolution of life as we know it. Since the Industrial Revolution, humans have been releasing greenhouse gases into the atmosphere faster than natural processes can remove them. For example, burningfossil fuels releases carbon dioxide. The extra carbon dioxide increases the greenhouse effect, which makes the planet warmer than it would be naturally. The increase in global temperature this causes is called global warming. Global warming is beginning to trigger big changes in the environment. The average temperature of the atmosphere and oceans is increasing slightly every decade, and this is already causing polar ice caps to melt and sea levels to rise. 1. The Sun s rays enter the Earth s atmosphere. 2. Energy is absorbed by the Earth s surface and re-emitted at longer wavelengths, such as infrared radiation (heat). 3. Some emitted heat passes through the atmosphere into space. Task Read the article on global warming and highlight any key ideas 4. Some heat is absorbed by carbon dioxide, a greenhouse gas. Heat is re- emitted in all directions and some becomes trapped within the Earth s atmosphere. The Earth becomes hotter as a result.
Rusting - Oxidation Ironis a good example of rusting or oxidation. The metal will slowly break down by a simple reaction on the surface which then eventually breaks away to leave fresh iron and process starts again. https://youtu.be/q0CAfXV-YdY Iron + oxygen + water Hydrated Iron (III) Oxide We can also stop this process by removing any of the reactants from the situation. When we say that the iron is oxidised we mean electrons are removed to make a +3 ion. (Removal of electrons) (addition of electrons) Task Make your own notes on the idea of rusting as a chemical concept. Animated Science 2022
Rusting Demonstration 4 jars were setup with iron nails so they could rust We then waited for 3 days to see the results Then we shook the jars to see how that would change the outcomes. Which one is rusts more and why? Why did the boiled water make no difference? https://youtu.be/V-0wocipCcI 3mins Animated Science 2022
Mr D Powell 2022 Animated Science 2022 Lesson 4: Metals and Water Key Ideas . What happens when you mix a metal and water from Group 1 I know that different metals have different reactivity in group 1 D/E + describe how metals react with water to make metal hydroxide solutions and hydrogen C ++ I can explain how some metals will react with steam B +++ I can write some equations to explain the reactions of metals and water Animated Science 2022
Reactivity of Metals Task.. Explain this idea and write down the equations (check that they they balance) Reactivity Series Potassium The reactivity series will need to be learned for GCSE. Group 1 metals feature in this series. Each metal has a similar reaction with water. Sodium Reacts with Water Lithium Barium Strontium Calcium Magnesium Aluminium The metal reacts with water to form hydroxides which are soluble in water or alkaline in nature. We can test for the presence using litmus paper or indicator solution. The reaction is also exothermic and gives off heat. Carbon Zinc Chromium Reacts with Acids Iron Cadmium Cobalt Nickel Tin Lead Li, Na, K - https://youtu.be/Tzl4kGneIp Y Hydrogen Antimony Bismuth They also emit hydrogen gas which is flammable. Copper Rb, Cs - https://youtu.be/- p2kpZRWxM8 Unreactive Mercury Silver Gold Group 1 Metal + Water Metallic Hydroxide + Hydrogen 2Na (s) + 2H2O (l) 2NaOH (aq) + H2 (g) Platinum Animated Science 2022
Group 1 Metals The pattern for group 1 metals is simple and the reasoning is that there is one electron in the outer shell which is easily lost to another atom. As you get further down the periodic table the atoms get larger (Francium) and the electron is less tightly held (or shielded from the charge in the nucleus). Hence it reacts more easily. Tasks: 2Na (s) + 2H2O (l) 2NaOH (aq) + H2 (g) Make a note of use for each metal shown in the table. Metal Use Increasing Reactivity Lithium batteries Sodium part of table salt Can you comment on why the reactivity changes? Potassium found in nerve cells melts at 400C / thin film battery Rubidium Can you predict and balance a reaction of Rb with water liquid at room temp/ trigger for a bomb Caesium Francium radioactive Animated Science 2022
Elements of Life..... Tasks: Potassium is vital to life. It keeps your heart, kidneys and nerves working. A shortage of potassium makes people weak, confused and depressed, and can even cause heart attacks. Discuss with a partner why Potassium is important in our bodies? No one eats pure potassium the element catches fire when it touches water. Instead, we eat compounds that contain potassium. Eating too much ordinary table salt (sodium chloride) is harmful to health. So some people eat salt substitutes , which are a mixture of potassium chloride and sodium chloride. Foods like raisins, peanuts and bananas are rich in potassium compounds. Animated Science 2022
Mr D Powell 2022 Animated Science 2022 Lesson 5: Metals and Acids Key Ideas . MASH & MAZIT? I know what MASH stands for! D/E + complete a practical which shows a reactivity series for metal + acid (MAZIT) C ++ I can explain what products are produced and the pattern B +++ I can write word and symbol equations for reaction of metals with acids. Animated Science 2022
Exam Review Question /3 Answers 1. Copper is a metal. At room temperature copper is a strong solid. Give two other properties of copper that show it is a metal. (2) 1) it conducts electricity or heat 2. When copper metal is heated it reacts with a gas in air ductile/ malleable high melting/ boiling point it is shiny / sonorous it forms basic oxides 2) What is the chemical name of the product formed when copper reacts with a gas in air? (1) CuO Copper Oxide Animated Science 2022
MASH ?? Task 1. Write out and explain both check they are balanced. Make a note of what MASH means and how it works. Explain how the acid changes the salt MASH is a really easy way to remember how acids and metals react. 2. 3. They all have the same generic reactants and products Metal Acid Salt name Magnesium chloride Magnesium nitrate Magnesium sulfate Metal + Acid Salt + Hydrogen Hydrochloric acid Magnesium magnesium + sulfuric acid magnesium sulfate + hydrogen Magnesium Nitric acid Magnesium Sulfuric acid Mg(s) + H SO (aq) MgSO (aq) + H (g) Hydrochloric acid Nitric acid Sulfuric acid Hydrochloric acid Nitric acid Sulfuric acid Zinc Zinc chloride Iron + sulfuric acid iron sulfate + hydrogen Zinc Zinc Zinc nitrate Zinc sulfate Iron Iron chloride Fe(s) + H SO (aq) FeSO (aq) + H (g) Iron Iron Iron nitrate Animated Science Iron sulfate 2022
Practical.... A student has a hypothesis..... I think that different metals will react more or less strongly with hydrochloric acid You have been given the following equipment and need to design an experiment to test this out... Make sure you clearly show the following in your work.... 1. 2. 3. 4. Title/Hypothesis (copied) Equipment List Diagram (use a ruler) Method of steps to make a fair test Results Table with obs Analysis (what you conclude) 1. A test tube and test tube rack. 2. Measuring cylinder 3. Some samples of metal: Iron (Fe) Zinc (Zn) Magnesium (Mg) Lead (Pb) 5. 6. Extra Help/ Hints.. If you get stuck ask to see the extra sheets for a quick look Hydrochloric Acid 16 cm3 (dilute) Wooden Split & bunsen (need to light it) 4. 5. Animated Science 2022
Extra Help... Diagram: Reacting Acids with Metals... I think that the different metals will react more or less strongly with hydrochloric acid Method 1. I will setup ....... Effervescen ce Metal Iron (Fe) Analysis Zinc (Zn) I think that ........ Magnesium (Mg) Copper (Cu) Animated Science 2022
Extra Special Help... Reacting Acids with Metals... I think that the different metals will react more or less strongly with hydrochloric acid Method 1. I will setup a small sample of each metal in turn with the 4cm3 of acid. I will place my finger over the end of the tube to collect any gas and observe the fizzing reactions When the fizzing slows down I will light a split and pop the gas. 2. Metal Effervescence 3. Iron (Fe) Zinc (Zn) Analysis Magnesium (Mg) . Lead (Pb) Animated Science 2022
Extra Special Help... Reacting Acids with Metals... I think that the different metals will react more or less strongly with hydrochloric acid Method 1. I will setup a small sample of each metal in turn with the 4cm3 of acid. I will place my finger over the end of the tube to collect any gas and observe the fizzing reactions. When the fizzing slows down I will light a splint and pop the gas. 2. Metal Effervescence 3. 3rd Iron (Fe) 2nd Zinc (Zn) Analysis Magnesium (Mg) 1st Most I think that the gas given off (hydrogen) shows which is the most reactive metal which in this case is clearly magnesium as there was the most .. 4th Least Lead (Pb) Animated Science 2022
Review Questions Metals and Acids Reactivity Series Potassium Sodium 1. How can you make his experiment a fair test? Reacts with Water Lithium Barium Strontium Calcium 2. Give one sign showing that chemical reactions are going on? Magnesium Aluminium Carbon 3. What is the reactivity order, starting with the most vigorous? Zinc Chromium Reacts with Acids Iron Cadmium 4. What is the gas given off and how do you test of it? Cobalt Nickel Tin Lead Answers 1. Use the same amount of acid in each test tube, use pieces of metal that are the same mass or size (or any other sensible suggestions). 2. The acid and metal mixture effervesces or exothermic 3. Magnesium, zinc, iron, lead. (MAZIT) 4. Hydrogen, squeaky pop test, with a lit splint. Hydrogen Antimony Bismuth Copper Unreactive Mercury Silver Gold Platinum Animated Science 2022
MAZIT Reactivity Series Potassium MAZIT is a really easy and simple way to remember some of the reactivity series. Sodium Reacts with Water Lithium Barium Strontium Start with M Magnesium as most reactive down to T Tin the Least. M Calcium Magnesium Aluminium A Carbon Zinc Chromium Reacts with Acids Iron Z Cadmium Cobalt Nickel I Tin Lead Hydrogen T Antimony Bismuth Copper Unreactive Mercury Silver Gold Task Make a note of this idea MAZIT Platinum Animated Science 2022
Metals and Acids Review 3 mins Reactivity Series Potassium Task Sodium Reacts with Water Lithium Barium Watch this expanded group of metals and see how this compares to your sheet. Strontium M Calcium Magnesium Aluminium A Carbon https://youtu.be/Na_6j9y9ke8 Zinc Chromium Reacts with Acids Iron Z Cadmium Cobalt Nickel I Tin Lead Hydrogen T Antimony Bismuth Copper Unreactive Mercury Silver Gold Platinum Animated Science 2022
MAZINTL??? Reactivity Series Potassium Task Sodium Reacts with Water Lithium Barium If you are now happy with MAZIT then why not try out . Strontium Calcium MAZINTL! Magnesium Aluminium Carbon Police Sergeant Charlie Zinc Chromium Reacts with Acids Iron Cadmium Cobalt Nickel MAZINTL Tin Lead Hydrogen Antimony Caught Me Stealing Gold Plate Bismuth Copper Unreactive Mercury Silver Gold Platinum Animated Science 2022
Mr D Powell 2022 Animated Science 2022 Lesson 6: Displacement Reactions Key Ideas . How do these reactions work and how is it linked to the reactivity series? I know the reactivity series D/E + I can use the reactivity series to predict whether a reaction will occur. C ++ I can explain several example reactions and give evidence for why they occur and how they are useful. B +++ I can write displacement word equations which are balanced Animated Science 2022
What is a displacement reaction? A displacement involves a metal and the compound of a differentmetal. A more reactive metal will displace or push out a less reactive metal from its compound in a displacement reaction. The least reactive metal is left on its own after the reaction. It is no longer chemically bonded to any other elements. It is now a pure element. So anything higher on the series i.e. Lithium will be able to split up any lower elements which are in a compound. The image shows an example for how magnesium can displace copper which then falls out of solution as a precipitate. We can see the change of colour in the solution as a 2 evidence for the change in this case but there may be no visible change. nd piece of Animated Science 2022
What is a displacement reaction? Magnesium is more reactive than copper. When a piece of magnesium is dipped into blue copper sulfate solution, a displacement reaction occurs. This is the word equation: magnesium + copper sulfate copper + magnesium sulfate This is the symbol equation: Mg(s) + CuSO (aq) Cu(s) + MgSO (aq) This reaction cannot happen in reverse. Copper cannot displace magnesium from a compound because copper is less reactive than magnesium. Animated Science 2022
Mg(s) + CuSO(aq) Cu(s) + MgSO(aq) Mg(s) + CuSO (aq) Cu(s) + MgSO (aq) Animated Science 2022
https://youtu.be/5uxsFglz2ig - Thermite Welding of Train Tracks (3mins 48) Thermite Reaction The blast furnace is used to produce iron on a large scale. Sometimes, it is necessary to produce a small amount of iron more quickly, for example if railway workers need to produce molten metal to fix a broken rail. The thermite reaction uses aluminium powder and iron(III) oxide. When ignited, the mixture reacts vigorously because of the large difference in reactivity between aluminium and iron. The heat produced in the reaction melts the iron produced. iron(III) oxide + aluminium iron + aluminium oxide Fe2O3(s) + 2Al(s) 2Fe(l) + Al2O3(s) In this reaction, iron oxide loses oxygen to form iron so the iron(III) oxide is reduced. The Aluminium is more reactive that Iron and so steals the oxygen. Task Write a short note of how this works Animated Science 2022
