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C2 independent study
task.
5
Settler: Why is helium used in
air balloons?
Challenge: What happens to
noble gases when you pass
electricity through them?
Choose your own tasks 
Answer all the questions and then get a lead learner
near you to check your answers with red pen.
C2.1 – Mendeleev and the periodic table
C2.2 – Ionic compounds
C2.3 – Covalent compounds
C2.4 – Groups in the periodic table
C2.5 – Rates of reaction
C2.6 – quantitative chemistry
C2.1 – Mendeleev and
the periodic table
1) What was special
about Mendeleev’s
periodic table.
2) What is the relationship
between proton number and
electron number
4) Describe the structure
of an atom
5) What is formed when
an atom loses or gains an
electron?
6) What does group
number tell us about an
atom?
8) What is an isotope?
9) 25% of chlorine is Cl-37
and 75% is Cl- 35. What is
the relative atomic mass
(Ar)
7) What does period
number tell us about an
atom?
3) How is neutron number
calculated?
C2.2 – Ionic bonding
1) Describe what ionic
bonding is.
2) Draw an ionic lattice
3) Draw the ionic bonding
in sodium chloride
4) Draw and explain the
ionic bonding in sodium
oxide.
5) List the flame tests
results for K+, Na+ Cu2+ and
Cu2+
6) Describe the test for
Cl – ions.
7) Describe the test for
sulfate ions.
8)Describe the test for
carbonate ions.
9) Describe the barium
meal test
C2.3 – Covalent
bonding
1) What is covalent
bonding?
2) Draw the covalent
bonding in hydrogen
chloride
4) Compare the properties
of ionic compounds to
covalent compounds
5) Give the uses of
diamond and link them to
its properties
6) Give the uses of
graphite and link them to
its properties
7) Compare the properties
of simple covalent
compounds to giant
covalent compounds
8) What does the term
‘delocalised electrons ‘
mean?
9) Why do giant covalent
substances have high
melting and boiling points?
3) Draw the covalent
bonding in carbon dioxide
C2.4 – Groups of the
periodic table
1) Describe the
reactions of Li and K
with water.
Give balanced symbol
equations
4) Explain what would
happen when chlorine is
added to potassium iodide.
Add balanced symbol
equations.
7) Why are noble gases
inert?
2) Explain the reactivity in
group 1
5) Describe the properties
and uses of transition
metals
8) Give the uses of helium and
argon and link them to their
properties.
3) Explain the reactivity
in group 7
What is displacement?
6) Draw metallic bonding.
9) Describe what happens to
atomic radius and nuclear
attraction as we go down each
group
C2.5 – Rates of
reaction
1) Explain how an
increase in temperature
affects rate of reaction?
2) Explain how an increase
in concentration affects
rate of reaction?
3) Explain how use of a
catalyst affects rate of
reaction?
4) Explain how surface
area affects rate of
reaction?
5) Describe what an
exothermic reaction is
with 2 examples.
6) Describe what an
endothermic reaction is
with 2 examples.
7) Draw an energy level
diagram for an exothermic
reaction
8) Draw an energy level
diagram for an exothermic
reaction
9) If the number of reactants
is doubled in a chemical
reaction, what will happen to
the amount of products?
C2.6 – Quantitative
chemistry
1) How are number of
moles calculated?
How many moles are
there in 238g of
potassium?
4) 1.35g of aluminium was heated in
oxygen until there was no further
gain in weight. The white oxide ash
formed weighed 2.55g. Deduce the
empirical formula of aluminium
oxide.
7) Describe what makes a
chemical reaction ‘good’.
2) What is the relative
formula mass of Mg(OH)2
5) Na2S(aq) + AgNO3(aq) →
Ag2S(s) + NaNO3(aq)
How many grams of Ag2S can
be produced from 7.88 grams
of AgNO3 and excess Na2S?
8) Describe why
percentage yield is never
100%?
3) What is the % of Cl in CaCl2
6) What is theoretical
yield?
9) The theoretical yield of
a reaction is 9.5g but the
actual yield was 4.7g.
What is the % yield?
Review
• Did going through
this type of task
help you?
• How?