Download C3 REVISION – CHAPTER 1 – The Periodic Table

C3 REVISION – CHAPTER 1 – The Periodic Table
How did Newlands arrange the
elements in his model of the
Periodic Table?
What was this layout of the
elements known as?
Why was it largely discredited?
What did Mendeleev do differently
to Newlands?
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Group 1: aka_____________________
Draw the electron structure of the first three elements
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Why is Mendeleev’s model of the
Periodic Table now accepted?
How can these elements be made stable in terms of electron shells?
How do they achieve this?
What charge ion do they therefore form?
What is different about the density and melting point of the group 1 metals?
What two products are formed when they react with water?
How are the elements in the
Periodic Table arranged now?
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Why could they not be arranged
like this when Mendeleev and
Newlands were working?
Name the following groups:
1.
Group 7: aka_____________________
Draw the electron structure of the first two elements
7.
0.
Which group(s) in the Periodic
Table contain only metals?
Which group(s) in the Periodic
Table contain only non-metals?
How can these elements be made stable in terms of electron shells?
How do they achieve this?
What charge ion do they therefore form?
What will a more reactive halogen do to an aqueous solution of another halogen salt?
Transition Metals
Compare the following properties of the transition metals with group 1 metals:
Patterns of Reactivity in Group 1 and Group 7
Describe how reactivity changes going down each group.
Melting point*:
Strength/Hardness:
Reactivity:
*which metal is the exception?
Transition metals can form ions with _____________ charges. They are
Group 1 ______________ down the group. Group 7 _____________down the group.
useful as _________ and form lots of different _____________ compounds.
Explain why reactivity changes going down each group.
C3 REVISION – CHAPTER 2 – Water
Hard Water
How can this experiment be used
to determine water hardness?
What is hardness in water caused by?
Water Quality
What should there not be lots of in drinking water?
How is water made suitable for drinking? (Main Stages)
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How do these substances come to
be in water?
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Two “types” of hard water
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Explain what happens during the following stages
•Filtration
Why does using hard water cost money?
•Sedimentation
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Explain How the Following Remove
‘Hardness’
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Sodium carbonate (washing soda)
What is the purpose of chlorination?
What are the benefits of chlorination?
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What is soap scum?
How is it formed?
What is the purpose of adding fluoride to drinking water?
Ion Exchange Column
What is limescale?
How is it formed?
List the benefits of using hard water
What are the drawbacks of adding fluoride to drinking water?
What is the purpose of water filters?
Boiling (temporary hard water only)
What is distillation of water?
Why is it not used to produce pure water?
C3 REVISION – CHAPTER 3 – Energy Change
What is the unit of energy?
What do we call reactions that release energy
to the surroundings? Give an example.
Use the bond energies from the table to calculate the overall
energy change in the Haber process.
N2(g) + 3H2(g)
What is the equation we use to
calculate energy released during
reactions?
Use the equation above to
calculate the energy required to
increase the temperature of
50cm3 of water from 21°C to 37°C
What do we call reactions that take in energy
from the surroundings? Give an example.
2NH3(g)
Bond
Bond Energy (kJ/mol)
N=N
945
H-H
436
N-H
391
Give a definition of a fuel.
What do we call the reaction when fuels react
with oxygen?
Draw an energy level diagram for an
exothermic reaction.
Is the Haber process endothermic or exothermic going
forward?
Draw a diagram of the apparatus
used to measure energy change in
What are the waste products from burning fossil fuels?
reactions.
What is the waste product from hydrogen fuel cells?
Draw an energy level diagram for an
endothermic reaction.
KEY WORDS:
Endothermic
Exothermic
Calorimeter
Reactants
Products
Bond Energy
Hydrogen Fuel Cells
ASSESSMENT:
C3 REVISION – CHAPTER 4 – Analysis & Quantitative Chemistry
TEST FOR POSITIVE IONS
State the flame colour produced by
the following ions in a flame test.
TEST FOR NEGATIVE IONS
Describe how you would test for a
CARBONATE (CO32- ion).
TITRATIONS
Describe the main steps in a general titration practical
including relevant equipment.
Lithium (Li+)____________________
Sodium (Na+)____________________
Potassium (K+)__________________
Calcium (Ca2+)____________________
Barium (Ba2+)_____________________
State the precipitate colour produced
by the following ions when they react
with OH- ions.
Copper II (Cu2+)__________________
Describe how you would test for the
following HALIDES
Chloride
Bromide
Iron II (Fe2+)__________________
Iron III (Fe3+)__________________
Iodide
Aluminium(Al3+)__________________
Magnesium(Mg2+)__________________
Calcium(Ca2+)__________________
Q. 25cm3 of 0.2M HCl reacts with 22.6cm3 of NaOH of an
unknown concentration: calculate the concentration of the
NaOH.
HCl(aq) + NaOH(aq)
NaCl(aq) + H2O(l)
Describe how you would test for the
presence of a SULPAHTE (SO42- ion)
How would you distinguish between
Aluminium, Magnesium and Calcium
hydroxides?
Aluminium
Magnesium
Calcium
Write out the equation to calculate the
number of moles of a substance in
solution.
KEY WORDS:
flame test, sulphate,
carbonate, halide,
barium chloride, end
point, neutralisation,
titration
ASSESSMENT:
C3 REVISION – CHAPTER 5 – Chemical Equlibrium & The Production of Ammonia
Explain what is meant when we say a reaction
is at equilibrium.
The Haber Process
N2(g) + 3H2(g)
2NH3(g) – 93kJ/mol
What can you say about energy in a reversible
reaction? [Think: exo and endothermic]
Draw a diagram to describe the main stages in
the Haber process.
Describe the anhydrous copper sulphate
reversible reaction (a diagram may help)
State and explain the effect of increasing
the pressure in the Haber process above.
Use your diagram above to explain how the
Haber process is made more efficient in terms
recycling unused reactants.
State and explain the effect of decreasing
the temperature in the Haber process above.
Describe how the Ammonia is separated from
the unused Nitrogen and Hydrogen.
What can anhydrous copper sulphate be used to
test for?
Describe the reaction conditions for the
Haber process above.
KEY WORDS:
Equilibrium, pressure,
forward reaction,
reverse reaction,
economy, reversible
reaction, catalyst
ASSESSMENT:
Why do we have to compromise with a lower
than expected pressure in the Haber process
C3 REVISION – CHAPTER 6 – Alcohols; Carboxylic Acids; Esters
Draw the structure of a simple alcohol,
name it and identify the functional
group.
Describe the properties of alcohols
Describe the properties of carboxylic acids
Carboxylic acids are ‘weak’ acids; explain what
is meant by a weak acid.
Give examples of the uses of alcohols
Draw the structure of a simple
Carboxylic Acid, name it and identify
the functional group.
Give examples of the uses of carboxylic acids
Describe the problems associated with alcohol
consumption in the UK.
Describe the properties of esters
Give examples of the uses of esters
Draw the structure of a simple Ester,
name it and identify the functional
group.
KEY WORDS:
Alcohol,
carboxylic acid,
ester, functional
group, solvent,
fuel, volatile
ASSESSMENT:
Describe how you would make an ester.