1.1
1.2
1.3
1.4
 Where did the gases in the early
atmosphere come from? (1)
 Name the two main gases in the
Earths early atmosphere (2)
 Explain why it’s difficult to be
precise about how gases in the
atmosphere have changed over
time
 Describe how the oceans were
formed (2)
1.5
 Describe three processes that
reduced the level of carbon
dioxide in the atmosphere (3)
1.6
 Explain how the level of oxygen in
the atmosphere increased (2)
a) Name the 3 main gases in the
atmosphere today and their
percentage abundance (3)
a) Describe how to measure the
amount of oxygen in the atmosphere
today (3)
1.8
1.7
1.7
1.9
 Volcanoes
 Carbon dioxide (1) and water
vapour (1)
 Limited information available from
different sources (1)/ open to
different interpretation (1).
 The Earth cooled to 100°C (1),
water vapour in the atmosphere
condensed to form oceans (1)
 Carbon dioxide dissolves in oceans.
(1) Locked up in sedimentary
rocks. (1)(as shells made using the
dissolved carbon dioxide in the
ocean) . Taken in by plants during
photosynthesis and locked up in
fossil fuels. (1)
 Plants evolved & produce oxygen (1)
during photosynthesis (1)
 Nitrogen 78% (1), oxygen 21% (1)
argon 1% (1)
a) Heat up iron wool (or copper) in a
boiling tube (1) connected to gas
syringe (1). Measure decrease in
volume of air in gas syringe (1).
b) Volume of gas in syringe decreases
as oxygen from air reacts with
metal (1) to form metal oxide (1)
b) I can explain why the experiment
to measure oxygen content works (2)
a) Explain how volcanoes can effect
a) Release carbon dioxide, this causes
the atmosphere (2)
global warming (1). Acidic gases
cause acid rain (1)
b) Identify and explain two ways
b) Burning fossil fuels- releases
humans are increasing the amount
carbon dioxide and causes global
of carbon dioxide in the
warming (1)
atmosphere (2)
Deforestation- cutting down trees
so less carbon dioxide is taken in
by photosynthesis (1)
2.1
2.2
2.3
2.4
2.5
2.6
2.6
2.7
2.9
2.8
a) Name an igneous rock (1)
b) Describe how igneous rocks are
formed (2)
c) Explain what affects the size of
crystals (2)
a) Granite / basalt/ (1)
b) Molten rock/ magma/ lava cools
Solidifies- forms a solid
c) Fast cooling (on outside of Earth)
causes small crystals and slow
cooling (inside Earths crust) cause
large crystal
 Name a sedimentary rock (1)
a) Limestone/ sandstone/ chalk (1)
 Describe how sedimentary rocks
b) Small bits of rock (sediment) sink
are formed (3)
the bottom of the sea (1)
compressed by more sediment
falling from above (1) over millions
of years (1)
c) Fossils (1) - due to compressed
 Explain how to recognise
organisms. Erodes easily (1) – due
sedimentary rocks (2)
to soft rounded grains.
 Name a metamorphic rock (1)
 Marble/ slate/ quartz (1)
a) Describe how metamorphic rocks
a) Heat(1) and pressure (1) caused
are formed (2)
when tectonic plates move
b) Describe how marble is formed (2) b) limestone (1) is heated and
compressed (1) by movements of
the Earths tectonic plates
a) Name the main chemical present in a) calcium carbonate
limestone, chalk and marble (1)
b) Describe some uses of limestone
b) Used in the formation of cement
that are commercially important (2)
(1)/ concrete (1)/ glass (1)
a) Recall one reason why people may a) More jobs (1)- more money for
be in favour of a limestone quarry
local people
in their community (1)
b) Dust pollution (1)/ noise pollution
b) I can identify reasons why people
(1) / destroys plant and animal
may not be in favour of a
habitats(1)/ spoils view (1)
limestone quarry in their
c) The main advantage is making more
community (2)
jobs and bringing money to the
c) I can evaluate both sides of an
local area.(1)
argument and give my opinion (3)
However the quarry will mean an
increase in level of dust & noise
pollution as well as spoiling the
view. (1) Over all I think…..give
reasons, use clues in given text.
2.10a a) What is meant by a thermal
decomposition reaction? (2)
b) Complete the word equations
below:
i) Calcium carbonate →
ii)
Sodium carbonate →
2.12
 Explain why some metal
carbonates decompose more
easily than others.(1)
2.11
Plan an experiment to find out which
metal carbonate decomposes the
fastest.
 Include equipment used (2)
 Independent variable (1)
 Dependent variable (1)
 Control variables (2)
2.13
a) Define an atom (1)
b) How can how you recognise
elements from diagrams and their
names? (2)
c) How can you recognise compounds
from diagrams and their names
a) Heat (1) is used to break down (1) a
chemical into several products
bi) Calcium
→ Calcium oxide +
carbonate
carbon dioxide
bii) Sodium
→ Sodium oxide +
carbonate
carbon dioxide
 The higher the metal is in the
reactivity series the longer it
takes for the metal carbonate to
decompose. (1) (For examplesodium carbonate takes longer to
decompose than copper carbonate)
 Boiling tube in a clamp stand with a
delivery tube going into a test tube
in a test tube rack. Bunsen burner
on a heat proof mat under the
boiling tube. (some of these = 1.
Most = 2)
 Independent variable- change the
metal carbonate (1)
 Dependent variable- measure time
for limewater to go cloudy (1)- this
measures how quickly carbon
dioxide gas is given off.
 Control variables- same mass of
metal carbonate in boiling tube.
/Same volume of limewater in test
tube. /Bunsen burner on same
flame Bunsen burner same height
below boiling tube.
(1 mark each, max 2 marks)
a) Smallest particle that makes up an
element (1)
b) Only made from one type of atom
(1), found in the periodic table (1) and
have one part names (1) eg oxygen
c) Contain atoms from different
elements (1) bonded together, (1)
have two part names, eg calcium oxide
2.13
2.14
2.15
2.16
2.17
2.18
di)
How many elements in the formula
CaCO3? (1)
Explain how to identify the
number of elements in a chemical
formula. (1)
di) 3 elements in CaCO3 as 3 capitals
Ca = Calcium C = carbon O = oxygen
dii)
dii) Count the number of CAPITAL
LETTERS. Element symbols either have
one CAPITAL letter, or one CAPITAL
letter followed by a lower case letter.
ei) How many atoms are there in CaCO3? ei) 5 (1 calcium + 1 carbon + 3 oxygen)
eii) Explain how to work out the number eii) If there is no number after a
of atoms in a chemical formula. (1)
CAPITAL or the lower case letter
following the CAPITAL there is only one
atom of this element. If there is a
number this means there is more than
one atom- equal to the number. Numbers
are always half way below the line.
f) Predict the mass of calcium oxide if
f) 100 – 44 = 56g (1)
100g of calcium carbonate are heated
Mass of reactant (calcium carbonate) =
and 44g of carbon dioxide is given off.
100g
Calcium carbonate →calcium oxide
Mass of products (calcium oxide + carbon
+ carbon dioxide
dioxide) must also equal 100g as mass
must be conserved.
100 = 44 + ?
a) Describe what happens when water is a) Heat is given off (1), a white crumbly
added to calcium oxide (2)
solid is formed.(1)
b) Name the product formed when
b) calcium hydroxide (1)
water is added to calcium oxide (1)
 Name solution formed when calcium
 Limewater (1)
hydroxide dissolves in water (1)
If you add 10g of copper chloride
20g of product (1)
solution to 10g of sodium hydroxide
Mass of reactants = Mass of products
what total mass of products will be
10 + 10 = 20g (1)
formed? (1) Explain how you know (1)
a) Alkalis (1) blue or purple with
a) What type of chemicals are calcium
universal indicator pH 8- 14
oxide, calcium hydroxide and calcium
carbonate (hint think pH scale) (1)
b) Calcium carbonate is an alkali(1)
b) Why is powdered calcium carbonate
neutralises acidic soil(1) crops grow
spread on some farmers fields? (3)
better
a) Name the main gas that causes acid rain a) Sulfur dioxide (1) or nitrogen oxides
b) Describe how this gas is produced (2)
b) Burning fossil fuels (1) (like petrol &
c) Explain how acidic gases can be removed
coal) containing sulphur impurities (1)
from waste gases from fossil fuel power
c) Pass acidic gases through containers
stations. (2)
of wet powdered calcium carbonate.
(1) Gases dissolve in water and are
neutralised by alkali. (1)