Here are the reactions of metal oxides with acid:
1) Magnesium oxide + hydrochloric acid
MgO + 2HCl → MgCl2 + H2O
2) Sodium oxide + hydrochloric acid
Na2O + 2HCl → 2NaCl + H2O
3) Aluminium oxide + sulphuric acid
Al2O3 + 3H2SO4 → Al2(SO4)3 + 3H2O
The metal oxide acts as a base and neutralises the acid to form a salt and water.
2. 06/11/12
Elements
If a solid, liquid or gas is made up of only one type of
atom we say it is an element. For example, consider a
tripod made up of iron:
These atoms are
ALL iron – there’s
nothing else in here
3. 06/11/12
Compounds
Compounds are
different to
elements. They
contain different
atoms. Here are
some examples: Methane
Sodium
chloride (salt)
Glucose
5. Balancing equations
06/11/12
Consider the following reaction:
Sodium + water sodium hydroxide + hydrogen
Na
Na + O +
H H H
H H O
This equation doesn’t balance – there are 2 hydrogen
atoms on the left hand side (the “reactants” and 3 on
the right hand side (the “products”)
6. Balancing equations
06/11/12
We need to balance the equation:
Sodium + water sodium hydroxide + hydrogen
Na
O H
Na H H O
+ +
O Na H H
H H H
Na
O
Now the equation is balanced, and we can write it as:
2Na(s) + 2H2O(l) 2NaOH(aq) + H2(g)
7. Some examples
06/11/12
2 Mg + O2 2 MgO
Zn + 2 HCl ZnCl2 + H2
2 Fe + 3 Cl2 2 FeCl3
NaOH +
HCl NaCl + H 2O
CH4 + 2 O2 CO2 + 2H2O
Ca + 2 H2O Ca(OH)2 + H2
2 2
NaOH + H2SO4 Na2SO4 + H 2O
2 3 2 4
CH3OH + O2 CO2 + H 2O
8. Hazard signs to learn…
06/11/12
Acid Corrosive Toxic
h i
Harmful Irritant Oxidising
10. 06/11/12
The Earth’s Atmosphere
For the last 200 million years the atmosphere has remained roughly the
same – it contains 78% nitrogen, 21% oxygen, 1% noble gases and about
0.03% CO2
Carbon dioxide, water vapour Oxygen Nitrogen Noble gases
11. 06/11/12
Evolution of the Earth’s Atmosphere
Carbon Methane Ammonia Oxygen Nitrogen Others
dioxide
Present day
atmosphere contains
78% nitrogen, 21%
oxygen, 1% noble
gases and about
0.03% CO2
4 Billion years 3 Billion years 2 Billion years 1 Billion years Present day
12. 06/11/12
Evolution of the Earth’s Atmosphere
Volcanic activity
Some of the oxygen is
releases CO2, methane,
converted into ozone.
ammonia and water The ozone layer blocks
vapour into the out harmful ultra-violet
atmosphere. The water rays which allows for the
vapour condenses to development of new life.
form oceans.
4 Billion years 3 Billion years 2 Billion years 1 Billion years Present day
Green plants evolve which take in CO2 and give
out oxygen by photosynthesis, increasing the
amount of oxygen in the atmosphere. Carbon
from CO2 becomes locked up in sedimentary
rocks as carbonates and fossil fuels and is
dissolved into the sea. Methane and ammonia
react with the oxygen and nitrogen is
released.
13. 06/11/12
Carbon dioxide in the atmosphere
The amount of CO2 in the atmosphere is affected by 3 things:
1) Geological activity moves carbonate rocks deep into
the Earth and they release ______ _______ into the
atmosphere during volcanic activity.
2) Human activity - When fossil fuels are burned
the carbon contained in them reacts with _____
to form CO2. Furthermore, deforestation means
that less _____ are around to take in CO2.
3) Increased CO2 in the atmosphere causes a reaction
between it and _______. These reactions do not remove ALL
of the new CO2 so the greenhouse effect is still getting
_______!
Words – oxygen, seawater, carbon dioxide, worse, trees
15. What are rocks?
06/11/12
Rocks are made from a combination of minerals and can be
hard or soft depending on how the minerals are arranged.
Rocks can be
found here…
…and here…
…and here…
…and here
17. Sedimentary rocks
06/11/12
How sedimentary
rocks are formed:
1) Weathering
2) Transportation
3) Deposition
4) Burial
18. Metamorphic rocks
06/11/12
Quartzite
Slate
Marble (made from
chalk or limestone)
19. Metamorphic rocks
06/11/12
Metamorphic rocks are formed by the combined effect of
heat and pressure on other rocks:
Pressure from rocks above…
…and heat from magma nearby
21. Igneous Rock
06/11/12
Granite – a slow cooling
rock with big crystals
and rich in silica
Rhyolite – a fast cooling
rock with small crystals
and rich in silica
Gabbro – a slow cooling rock with
Basalt – a fast cooling rock with big crystals and rich in iron
small crystals and rich in iron
22. Igneous rocks
06/11/12
Igneous rocks
are formed
when lava or
magma cools
down and
solidifies
If the lava or magma cools
QUICKLY it has SMALL crystals
If the lava or magma cools
SLOWLY it has BIG crystals
23. Summary
06/11/12
Sedimentary, igneous or How they were formed Appearance
metamorphic?
Sedimentary Small pieces of sediment Usually soft, can contain
were ______ together by ________, easily eroded
salt and pressure from rocks
(e.g. sandstone, _______,
above
chalk)
Liquid rock (______ or lava) Contain ______, very hard,
Igneous
cooled down and turned back never contain fossils
into a ______
(e.g. basalt, _______)
Other rocks were acted on by Sometimes have tiny crystals,
Metamorphic heat and _______ over a long no fossils, always hard and
time sometimes arranged in
(e.g. ______, slate) _______
Words to use – layers, stuck, granite, marble, fossils, limestone,
crystals, pressure, magma, solid
24. 06/11/12
Conservation of mass in reactions
In any reaction the total mass of products is
the same as the total mass of the reactants
Example 1 – Magnesium oxide and hydrochloric acid
H Cl
Mg
O Cl H
Mg Cl O H
H Cl
1 x magnesium, 1 x oxygen, 2 x Also 1 x magnesium, 1 x oxygen, 2
hydrogen and 2 x chlorine atoms x hydrogen and 2 x chlorine atoms
Example 2 – Burning methane
H H O O
O O H H
C C
H O
H O O H O
H
25. Calcium Carbonate
06/11/12
Calcium carbonate is a common chemical in the Earth and we’ve
already come across it in a number of forms:
Limestone
Chalk
Marble (made from
chalk or limestone)
26. Limestone
06/11/12
View video of limestone being quarried
27. Limestone
06/11/12
Limestone is a __________ rock made up of
mainly calcium carbonate. It’s cheap and easy to
obtain. Some uses:
1) Building materials – limestone can be quarried
and cut into blocks to be used in _______.
However, it is badly affected by ____ ____.
2) Glass making – glass is made by mixing limestone
with _____ and soda:
Limestone + sand + soda glass
3) Cement making – limestone can be “roasted” in a rotary kiln
to produce dry cement. It’s then mixed with sand and gravel
to make _______.
Words – sand, building, sedimentary, concrete, acid rain
28. 06/11/12
Pros and Cons of quarrying limestone
Reasons why quarrying limestone Reasons why quarrying limestone
is a good idea is a bad idea
29. Limestone
06/11/12
Limestone has a number of uses when it undergoes chemical
reactions. There are two reactions to know:
1) Firstly, a THERMAL _________________ reaction is used
to break the calcium carbonate down into calcium ______ and
_______ __________:
HEAT
Calcium carbonate calcium oxide + carbon dioxide
2) _____ is then added to produce calcium __________:
WATER
Calcium oxide calcium hydroxide
Words – hydroxide, decomposition, carbon
dioxide, water, oxide
30. The “Limestone Cycle”
06/11/12
Calcium Carbonate
CO2
(limestone)
Step 4:
add CO2 Step 1:
heat
Calcium Hydroxide solution Calcium Oxide
Step 3: add Step 2:
more water add a little
and filter water
Calcium Hydroxide
31. 06/11/12
Uses of these Calcium compounds
Calcium carbonate (limestone), calcium oxide and calcium
hydroxide have a number of uses:
1) Neutralising acidic soil – calcium carbonate,
calcium hydroxide and calcium oxide are _______
and can be used to ________ soil acidity to help
______ growth.
2) Removing pollutants – calcium
carbonate can be used as a “_______”
to remove acidic gases from a coal-
fired power station’s waste products,
helping prevent ____ _____.
Words – acid rain, alkaline, plant, scrubber, neutralise
32. 06/11/12
Thermal decomposition of carbonates
Limestone undergoes thermal decomposition when heated.
The same happens to other carbonates. For example, consider
copper carbonate:
Copper carbonate
(green) turns into
copper oxide (black)
Limewater
Limewater goes
cloudy due to carbon
dioxide being made
Copper carbonate copper oxide + carbon dioxide
33. Topic 3 – Acids
06/11/12
Indigestion
Learning Objective: Be able to explain why stomach
acid is produced and how antacids are used to
neutralise the excess acid that causes indigestion.
Starter: Write down as many facts you know about
acids, alkalis and neutralisation.
35. Neutralisation reactions 06/11/12
When acids and alkalis react together they will NEUTRALISE
each other:
Sodium hydroxide Hydrochloric acid
Na OH H Cl
The sodium replaces the
hydrogen from HCl
Na Cl H 2O
Sodium chloride Water
36. Neutralisation experiment
06/11/12
In this experiment we mixed sodium hydroxide (an _____) and
hydrochloric acid together and they ________ each other.
The equation for this reaction is…
Sodium hydroxide + hydrochloric acid sodium chloride + water
A ____ was formed during the reaction, and we could have
separated this by __________ the solution. The salt that we
formed depended on the acid:
• Hydrochloric acid will make a CHLORIDE
• Nitric acid will make a _________
• Sulphuric acid will make a _________
Words – nitrate, neutralised, alkali, sulphate, salt, evaporating
37. Stomach Acid
06/11/12
Hydrochloric acid is used in the stomach to
help _______ and to kill ______. If we eat
too many “rich” foods our stomachs create
too much ____ – this is called ______. This
acid needs to be neutralised by taking
indigestion tablets. Indigestion tablets
contain substances such as _______ that
neutralise excess stomach acid.
Words – digestion, indigestion, acid, alkalis, bacteria
38. Topic 3 – Acids
06/11/12
Neutralisation
Learning Objective: Be able to explain how acids are
neutralised
Starter: Complete the following word equations:
Hydrochloric Acid + Sodium Hydroxide
Hydrochloric Acid + Calcium Carbonate
Sulphuric Acid + Aluminium Hydroxide
40. Neutralisation reactions
06/11/12
A neutralisation reaction occurs when an acid reacts with an alkali. An
alkali is a metal oxide or metal hydroxide dissolved in water.
ACID + ALKALI SALT + WATER
O Cl H
Na H Cl Na O H
H
Copy and complete the following reactions:
1) Sodium hydroxide + hydrochloric acid
2) Calcium hydroxide + hydrochloric acid
3) Sodium hydroxide + sulphuric acid
4) Magnesium hydroxide + sulphuric acid
41. Making salts
06/11/12
Whenever an acid and alkali neutralise each other we are left
with a salt, like a chloride or a sulphate. Complete the
following table:
Hydrochloric
Sulphuric acid Nitric acid
acid
Sodium Sodium
hydroxide chloride +
water
Potassium Potassium
hydroxide sulphate +
water
Calcium Calcium
hydroxide nitrate +
42. Using different bases
06/11/12
A metal oxide base:
Acid + metal oxide natural salt solution + water
heat
Suphuric acid + copper oxide copper sulphate + water
H2SO4(aq) + CuO(s) heat CuSO4(s) + H2O(l)
A metal carbonate base:
Acid + metal carbonate natural salt sol n + water + CO2
heat
Sulphuric acid + calcium carbonate calcium sulphate + water + CO 2
H2SO4(aq) + CaCO3(s) heat CaSO4(aq) + + H20(l) + CO2(g)
43. 06/11/12
Reactions of metals carbonates with acid
A metal carbonate is a compound containing a metal, carbon
and oxygen.
METAL CARBONATE + ACID SALT + CARBON DIOXIDE + WATER
Mg O H Cl O
Cl
Mg O
C C H H
O
O H Cl
Cl O
Copy and complete the following reactions:
1) Magnesium carbonate + hydrochloric acid
2) Calcium carbonate + hydrochloric acid
3) Sodium carbonate + sulphuric acid
44. 06/11/12
Reactions of metal oxides with acid
A metal oxide is a compound containing a metal and oxide. They are
sometimes called BASES. For example:
O
O Al
O Na O
Mg Na
Al
O
Magnesium oxide Sodium oxide Aluminium oxide
METAL OXIDE + ACID SALT + WATER
H Cl
Mg
O Cl H
Mg Cl O H
H Cl
Copy and complete the following reactions:
1) Magnesium oxide + hydrochloric acid
2) Calcium oxide + hydrochloric acid
3) Sodium oxide + sulphuric acid
47. Testing for Chlorine
06/11/12
Chlorine “bleaches” damp indicator paper. It is also a toxic gas
so don’t breathe it! This leads to problems when it comes to
large-scale manufacture of chlorine gas.
48. Topic 3 – Acids
06/11/12
The Importance of
Chlorine
Learning Objective: Be able to produce a mind map to
show how chlorine is produced, what chlorine is used
for and the potential problems with chlorine.
importance and the show what the uses
Starter: Complete the true and false statements
about chlorine.
50. Electrolysis of seawater
06/11/12
Seawater is a mixture of water and salt (sodium chloride)
and we can electrolyse it to produce chlorine and other
useful products:
Chlorine gas (Cl2) Hydrogen gas (H2)
Sodium
chloride
solution
(seawater)
NaCl(aq)
Sodium hydroxide
(NaOH(aq))
Positive Negative
electrode electrode
51. Uses of chlorine
06/11/12
Polyvinylchloride (PVC) is made up of lots of monomers of vinyl
chloride (chloroethene):
H Cl H Cl H H H H
C C C C C C C C
H H H H H H H H
Chloroethene Lots more Polyvinylchloride (PVC)
monomer Chloroethene
monomers
Chlorine is also used in the manufacture of bleach.
Sodium hydroxide is reacted with chlorine to form
sodium hypochlorite (bleach):
Cl2 + 2 NaOH → NaCl + NaClO + H2O
52. Topic 3 – Acids
06/11/12
Electrolysis of Water
Learning Objective: Be able to explain what are the
products from the electrolysis of water and how to
test for these gases.
Starter: How would you test for Hydrogen, Chlorine,
Carbon Dioxide and oxygen gas?? Write it down
54. Electrolysis of Water
06/11/12
Water is two atoms of hydrogen and one atom of
oxygen. It can be electrolysed to break it down: H O
H
Oxygen gas (O2) Hydrogen gas (H2)
Water
H 2O
Positive Negative
electrode electrode
56. 06/11/12
Topic 4 – Obtaining and Using Metals
Ores
Learning Objective: Be able to explain how metals are
extracted using the reactivity series
Starter: What is the reactivity series??
58. Reactivity series demonstration
• All metal elements have a different reactivity.
• Some such as sodium are very reactive even in air.
• Others such as gold are extremely unreactive.
• Watch the demonstration and think about which
elements are more reactive.
59. Finding an order?
• Can you place these elements a list of reactivity
with most reactive a the top and least at the
bottom?
Sodium
Sodium
Copper
Copper Zinc
Zinc
Magnesiu
Magnesiu
m
m
Gold
Gold Iron
Iron
60. Extracting Metals
06/11/12
Some definitions:
A METAL ORE is a mineral or mixture of
minerals from which it is “economically
viable” to extract some metal.
Most ores contain METAL OXIDES (e.g. rust = iron oxide).
To “extract” a metal from a metal oxide we need to REDUCE
the oxygen. This is called a REDUCTION reaction. To put it
simply:
Iron “Reduce” the oxygen
Iron Oxide
ore to make iron
61. How do we do it? 06/11/12
Potassium Metals ABOVE CARBON, because
Sodium of their high reactivity, are
extracted by ELECTROLYSIS,
Calcium
which is very expensive!
Magnesium
Metals BELOW CARBON are
Aluminium extracted by heating them with
Carbon carbon in a BLAST FURNACE.
This is a “displacement reaction”
Zinc
Iron
Tin Carbon Iron Oxide
Lead
Copper
These LOW REACTIVITY metals won’t
Silver need to be extracted because they are
Gold SO unreactive you’ll find them on their
own, not in a metal oxide
Platinum
62. Extracting metals
• A metal can be extracted from a compound by
reacting with an element higher up in the
reactivity series.
• So for example copper is more reactive than
silver.
• If we add copper metal to silver nitrate compound
we make silver metal.
• Draw a picture of this in your book.
63. Extracting iron
• Iron ore (haematite) is iron oxide.
• To make iron we need to remove the oxygen.
• This process is called REDUCTION
Copy down this equation
Iron oxide + carbon Iron + Carbon
Iron oxide + carbon Iron + Carbon
dioxide
dioxide
64. Extracting Iron from its ore
• Carbon can also be put into the reactivity series
and is higher (more reactive) than iron.
• This means iron can be extracted from its ore
using carbon.
65. Notes to copy and complete
Metals that are ______ reactive than carbon in the
reactivity series can be ___________ from their
oxides by _________ with ________.
Iron oxide is reduced in the _________ ________
to make iron.
[extracted, reduction, carbon, less, blast furnace]
66. What are Ores?
Most metals are too …………… to exist on their own in the ground.
Instead they exist combined with other elements (typically o………..
or sulphur) as ……………….. called ………….
A few metals are so ……………….. that they exist uncombined, as
……….metals e.g. gold, ………………..
Metal Name of ore Compound in ore
Words:
Aluminium Bauxite Aluminium oxide (Al2O3)
ores silver reactive
oxygen compounds unreactive pure
67. Displacement Reactions
1. Iron + Copper Sulphate Iron Sulphate + Copper
2. Copper + Silver Nitrate Copper Nitrate + Silver
3. Sodium + Zinc Carbonate Sodium Carbonate + Zinc
4. Potassium + Iron Oxide Potassium Oxide + Iron
5. Gold + Copper Carbonate Gold + Copper Carbonate
No reaction! Can you figure out why?
68. How do we extract metals from ores?
Watch this video clip:
http://jchemed.chem.wisc.edu/JCESoft/CCA/samples/cca7therm
It is called the thermite reaction.
The symbol equation is: Fe2O3 + Al Al2O3 + Fe
1. Copy out the symbol equation and write the word equation
underneath.
2. Why does this reaction happen?
3. Do you think that it’s a commercially viable way of extracting
iron from its ore? Explain your answer.
69. So how is it done?
Potassium
Sodium
Magnesium
The reactivity series of metals…
Aluminium
Zinc
Carbon can be used to extract some metals from
Iron
their ores e.g.
Copper
Copper oxide + Carbon Copper + Carbon dioxide
Silver
The copper oxide has lost oxygen. This is called a
Gold reduction reaction.
70. Potassium
Extracted from their ores by
Sodium electrolysis (using electricity)
Aluminium
Carbon
Zinc
Extracted from their ores by
Iron reduction by carbon
Copper
Silver No extraction necessary – found
Gold pure in the ground.
71. Extracting metals
06/11/12
1) What is an ore?
2) In what form are metals usually found in the Earth?
3) How do you get a metal out of a metal oxide?
4) What is this type of reaction called?
Type of metal Extraction process Examples
High reactivity (i.e anything
above carbon)
Middle reactivity (i.e.
anything below carbon)
Low reactivity
72. 06/11/12
Extracting Aluminium
Aluminium has to be extracted from its ore by electrolysis. This is
because aluminium is very ___________ and so it cannot be extracted
using ______. The amount of energy and _____ required to extract
aluminium and other metals is very high and so ________ is a much
better option.
Words – reactive, recycling, money, carbon
73. Copper, Aluminium and Titanium
06/11/12
Metal Uses and why Extraction Problems
method
Copper Electrical wires – Electrolysis Limited supply
good conductor
Gold Jewellery – None needed – Limited supply
attractive and its unreactive so and very
resistant to you find it in the expensive
corrosion Earth as gold
Aluminium and Planes – light and Complicated and Expensive and
titanium corrosion expensive difficult to
resistant extract
74. 06/11/12
Topic 4 – Obtaining and Using Metals
Oxidation and Reduction
Learning Objective: Be able to explain the terms
oxidation and reduction and relate it to equations
Starter: If reduction means removing
the oxygen what do you think oxidation
means??
77. Rusting
06/11/12
Rust is a hydrated form of
iron oxide. It is formed
when iron and/or steel
combines with oxygen and
water in an oxidation
reaction:
Iron + oxygen + water hydrated iron (III) oxide
78. Rusting
06/11/12
Task: To investigate what causes rusting
Tube 1 – Tube 2 – Tube 3 – Tube 4 –
drying boiled water + air water + air
agent water + salt
79. Rusting
06/11/12
Task: To investigate what causes rusting
No rust No rust Rust Lots of rust
Iron + oxygen + water hydrated iron oxide
80. Reducation and Oxidation
06/11/12
Some examples of reduction:
heat
Aluminium + iron oxide aluminium oxide + iron
2Al(s) + Fe2O3(s) heat Al2O3(s) + 2Fe(s)
heat
Lead oxide + carbon lead + carbon dioxide
2PbO(s) + C(s) heat 2Pb(s) + CO2(s)
An example of oxidation:
heat
Magnesium + oxygen magnesium oxide
Mg(s) + O2(s) heat 2MgO(s)
81. More on Redox Reactions
06/11/12
Basically, during a redox reaction electrons are either lost or
gained:
The Golden Rule: OILRIG
Oxidation Is Loss (of electrons)
Reduction Is Gain (of electrons)
For example:
Fe Fe2+ These reactions both involve the loss of
2Cl- Cl2 electrons – they are Oxidation reactions
Fe2+ Fe These reactions both involve the gain of
electrons – they are Reduction reactions
Cl2 2Cl-
82. C1.18 Reactions
.
Is the substance in red being oxidised or
reduced in the following reaction?
magnesium + oxygen → magnesium oxide
Oxidised
83. C1.18 Reactions
.
Is the substance in red being oxidised or
reduced in the following reaction?
lead oxide + carbon → lead + carbon dioxide
Reduced
84. C1.18 Reactions
Is the substance in red being oxidised or
reduced in the following reaction?
magnesium + hydrogen → magnesium + water
oxide
Reduced
85. C1.18 Reactions
Is the substance in red being oxidised or
reduced in the following reaction?
nickel + oxygen → nickel oxide
Oxidised
86. C1.18 Reactions
Is the substance in red being oxidised or
reduced in the following reaction?
4 Na + O2 → 2 Na2O
Oxidised
87. C1.18 Reactions
Is the substance in red being oxidised or
reduced in the following reaction?
Cr2O3 + 2 Al → 2 Cr + Al2O3
Reduced
88. 06/11/12
Topic 4 – Obtaining and Using Metals
Recycling Metals
Learning Objective: Be able to explain the importance
of recycling
Starter: Explain how recycled is carried out in
Newham
90. Recycling
06/11/12
Why recycle metals?
1) Less space will be needed for landfill sites
2) Recycled metals only need about 1/10th of the energy to
produce compared to producing new metals
3) Recycling saves on raw materials
4) Less excavation and mining costs
91. 06/11/12
Topic 4 – Obtaining and using metals
Properties of metals and Alloys
Learning Objective: Explain why certain metals are
used in relation to their properties.
Describe ways metal properties can be improved.
Starter: Sort out he properties of the metals on the
worksheet.
103. 06/11/12
Using impurities to strengthen Iron
In pure iron all
impurities are
removed. This
makes the iron soft:
Adding 1% impurities
makes the iron much
stronger:
104. Alloys
06/11/12
Steel is an “alloy” – i.e. a mixture of metals. Here are other
alloys:
Gold mixed with Aluminium mixed Aluminiun mixed
copper with magnesium with chromium
and copper
105. 06/11/12
Making steel
Strong Strength
Hardness
Amount of
Weak carbon
0.5% 1% 1.5% added (%)
Steel with a low Steel with a high Steel with chromium
carbon content is carbon content is and nickel is called
easily shaped strong but brittle stainless steel
106. Smart Alloys
06/11/12
A “smart alloy” is one that can “remember” its original state
after being bent or stretched.
These glasses are made from a “smart” material – if they are
bent they will return to their original shape. They could be
made from an alloy called “nitinol” (an alloy of nickel and
titanium) which can be bent but then returned to its original
shape simply by heating to its “transformation temperature”.
107. Gold alloys
06/11/12
Gold can be mixed with other metals to make alloys with
different properties. For example:
24-Carat gold 9-Carat gold
“Pure gold” – 99.99% of the atoms “9 carat gold” – around 9/24ths
in this bar are gold atoms (fineness of the atoms in these earrings
off 999.9). Pure and malleable but are gold atoms. Harder than
soft. pure gold but less malleable.
108. Materials in a Car
06/11/12
Copper wires Glass Nylon
windscreen seatbelts
Plastic trim
Steel body
Alloy wheels
109. Iron or aluminium?
06/11/12
Aluminium:
Does not corrode
Less dense so it’s lighter
Iron:
Cheaper than aluminium
Magnetic so easily recycled
Most cars are made from steel (an alloy of carbon)
From 2015 95% of a car will have to be made from recycled
material. What are the advantages of this?
110. 06/11/12
Topic 5 – Fuels
Crude Oil
Learning Objective: Explain how crude oil is formed
and its uses.
Starter: What elements are contained in
Hydrocarbons
112. Fuels
06/11/12
Fuels are substances that can be used to release useful
amounts of energy when they burn, e.g.
Wood Oil Gas Coal
These fuels are called “fossil fuels” and
are described as being “non-renewable”.
114. 06/11/12
Topic 5 – Fuels
Crude Oil fractions
Learning Objective:
Explain how hydrocarbon fractions are separated.
Starter: Write down three facts you remember form
last lesson
116. 06/11/12
Hydrocarbons and crude oil
Crude oil is a mixture of HYDROCARBONS
(compounds made up of carbon and hydrogen).
Some examples:
H H
Longer chains mean…
Increasing length
H C C H
H H
1. Less ability to flow
Ethane
2. Less flammable
H H H H
H C C C C H 3. Less volatile
H H H H
4. Higher boiling point
Butane
117. Distillation revision
06/11/12
This apparatus can be used to
separate water and ink
because they have different
_____ ______. The ______
will evaporate first, turn back
into a _______ in the
condenser and collect in the
_______. The ink remains in
the round flask, as long as the
_______ does not exceed
ink’s boiling point. This
method can be used to
separate crude oil.
Words – temperature, boiling points, water, beaker, liquid
118. .
06/11/12
Sort them into benefits and drawbacks of using oil
1 Accidents with oil wells or oil tankers can pollute the sea and
kill wildlife.
2 Cars that run on petrol are much more convenient than
battery-powered cars.
3 Burning fossil fuels produces carbon dioxide and other
polluting gases.
4 We can make lots of different chemicals out of the
substances in crude oil.
5 Crude oil will run out one day.
6 Bitumen is very useful for making roads.
7 We need oil to lubricate engines and other moving machines.
8 Petrol can cause explosions if it is not transported and stored
correctly.
119. Fractional distillation
06/11/12
Crude oil can be separated by fractional distillation. The oil is evaporated
and the hydrocarbon chains of different lengths condense at different
temperatures:
Fractions with
low boiling
points condense
at the top
Fractions with
high boiling
points condense
at the bottom
131. 06/11/12
Match up the names and uses
Fractions
Gases Fuel oil
Kerosene Petrol
Bitumen Diesel oil
Uses
Fuel for some cars Fuel for some cars
Making roads Cooking in homes
Fuel for large ships Fuel for aircraft
Heating homes Fuel for some trains
Fuel for some power
Making roofs waterproof
stations
133. 06/11/12
Topic 5 – Fuels
Combustion
Learning Objective:
•Able to explain what is produced when hydrocarbons
burn.
Starter: Draw a brainstorm to show everything you
remember about crude oil.
135. Burning Hydrocarbons
06/11/12
Burning hydrocarbons will produce water, carbon dioxide and
energy:
H H O O
O O H H
C C
H O
H O O H O
H
Methane + Oxygen Carbon + Water
dioxide
In this reaction the hydrocarbon is oxidised.
136. Testing for Carbon Dioxide
06/11/12
Gas
Limewater
Limewater turns
milky/cloudy
137. Burning Hydrocarbons
06/11/12
H H O O
O H
Lots of C
O
C
H
oxygen: H O
H O O H O
H
Methane + Oxygen Carbon + Water
dioxide
H O
H H O H
O O
C O
H C H H
Some H O
O
oxygen: H H C
O H O
H
C O
O O
H H H
H
Methane + Oxygen Carbon + Water
monoxide
H O
H H H
Little C O C
O O
oxygen: H
H
H H
Methane + Oxygen Carbon + Water
163. 06/11/12
Topic 5 – Fuels
Incomplete combustion and Acid Rain
Learning Objective:
Explain what happens if there is not enough oxygen
for burning.
Explain the consequences of Acid Rain
Starter: Write a balanced equation to show
combustion.
165. Incomplete Combustion
06/11/12
As well as producing carbon monoxide, incomplete combustion
can also produce soot:
H O
H H H
Little C O C
O O
oxygen: H
H
H H
Methane + Oxygen Carbon + Water
“Soot”
166. 06/11/12
Why Carbon Monoxide is Dangerous
Basically, carbon monoxide “sticks” to red blood cells instead
of oxygen, causing anybody inhaling it to essentially suffocate:
CO 1) Carbon Monoxide is breathed in
2) The molecule “sticks” to red blood
cells instead of oxygen
3) The red blood cells transport the
“carboxyhaemoglobin” molecule to
the rest of the body and the body’s
cells are starved of the oxygen
needed for respiration.
Carbon monoxide is odourless, colourless and
non-irritating so it’s very difficult to detect!
167. Burning Fossil Fuels
06/11/12
Burning fossil fuels like oil and coal causes pollution.
Oil contains carbon:
H H O O
O O H H
C C
H O
H O O H O
H
Carbon dioxide is a “greenhouse
gas” – it helps cause global warming
Coal contains carbon, sulfur and other particles:
sulfur + oxygen sulfur dioxide
Sulfur dioxide causes acid rain. Other particles can
cause “global dimming” – sunlight is absorbed by the
particles in the atmosphere.
176. Global Warming
06/11/12
Facts:
1) The 10 warmest years
of the last century
have all occurred
within the last 15
years
2) Sea level has risen by
between 12 and 24cm
in the last 100 years
3) Rainfall has risen by
1%
177. The Greenhouse Effect
06/11/12
We get heat
A lot of this heat is
from the sun:
_______ back into space.
However, most of it is kept inside the
Earth by a layer of gases that prevent
the heat escaping by _______ and
then re-radiating it back again.
This is called the _________ Effect. It has always been around, but is
currently being made worse due to:
1) Burning (releasing CO2)
2) __________ (removing trees that remove CO2)
3) Increased micro organism activity (from rotting ______)
4) Cattle and rice fields (they both produce _______)
These changes will cause GLOBAL WARMING and RISING SEA LEVELS
Words – methane, radiated, absorbing, deforestation, waste, greenhouse
179. 06/11/12
Reducing the amount of Carbon Dioxide
Scientists are trying to reduce the amount of carbon
dioxide in the atmosphere through a number of
possibilities:
1) “Iron seeding” – this is the process where iron is
intentionally put in seawater to help produce more
phytoplankton which then increases photosynthetic
activity, therefore reducing the amount of CO2 in the
atmosphere.
Aerial view of
phytoplankton
near Argentina
2) Converting CO2 into
hydrocarbons – carbon dioxide can
be converted into hydrocarbons and
then stored in the Earth by putting
it in such places as old oil fields or
coal beds.
180. Reducing Pollution from vehicles
06/11/12
A number of suggestions:
1) Buy a new, smaller, cleaner car
2) Buy a “hybrid” car
3) Convert your car to run on biodiesel
4) Make sure your car has a catalytic converter:
Carbon monoxide + oxygen carbon dioxide
Nitrogen monoxide + carbon monoxide nitrogen + carbon monoxide
5) Use the train or a bus!
181. 06/11/12
Topic 5 – Fuels
Biofuels and choosing fuels
Learning Objective:
•Explain the advantages and disadvantages of using
biofuels
•Explain how to choose the best fuel.
Starter: What do you know about biofuels
183. Ethanol as a biofuel
06/11/12
Ethanol is an important chemical. Many
countries are increasing the amount of
ethanol put into their petrol supplies: Ford Escape E85 –
runs on 85% ethanol
Ethanol is a “clean burning” energy source and produces little
or no greenhouse gases. How is it made?
The “renewable” way Sugar is produced from
standard crops like
Sugar ethanol + carbon dioxide sugar cane and corn
What’s the point?
When ethanol burns it only produces small amounts of carbon
dioxide. Making more cars run on ethanol means having less
cars that need petrol.
192. Choosing a biofuel
06/11/12
Does it create How much energy
pollution? does it release?
Biofuels Is it toxic?
How much does
it cost? How
much land is Does it take more CO2
needed?
to tranport it than it
takes in from the
How easy is it to atmosphere while
grow/make? growing?
193. Choosing a fuel
06/11/12
How easily does How much energy
it burn? does it release?
Which fuel should
Is it toxic?
you use?
How much smoke
does it produce? Is it easy to use,
store and transport?
194. Hydrogen Fuel Cells
06/11/12
Basically, a hydrogen fuel cell combines hydrogen and oxygen
to form water and release energy:
195. Hydrogen Fuel Cells
06/11/12
Advantages of fuel cells Advantages of petrol
Hydrogen fuel cells
vs Petrol
196. Energy from fuels
06/11/12
Copper
calorimeter Water
Spirit burner
Fuel