1. Describe the test for halide ions.
C3 topic 1 Qualitative chemistry
This topic looks at:
Water testing
Safe water
Ion identification
Safe limits
Fill in the colours of the solids formed by precipitation with NaOH.
How would you differentiate between the cations calcium and aluminium which both form the same colour precipitate?
Cation
Symbol
Effect of adding sodium hydroxide solution
Aluminium
Calcium
Copper (II)
Iron (II)
Iron (III)
Analysis can be quantitative or qualitative. State what these mean:
1. Quantitative =
2. Qualitative =
Describe how to do a flame test.
Write the colours you would expect to see in a flame test for these ions:
KeyWords: cations, anions, halides, quantitative, qualitative, flame tests, ammonium
Element
Symbol
Flame colour
Calcium
Sodium
Potassium
Copper
Equations
Write the balanced word and symbol equation for the reaction of sodium hydroxide and copper sulfate solutions.
2) Write the balanced word and symbol equations for the reaction between silver nitrate and sodium chloride.
Describe the test for halide ions.
Describe how to do a precipitation test to identify cations.

2. C3 topic 1 and 2 revision
This topic looks at:
Water testing
Safe water
Ion identification
Safe limits
What is the difference between hard and soft water?
What is soap wasted in hard water areas?
How would you test for ammonium ions?
Write the ionic equation for the reaction of silver nitrate with sodium chloride.
Explain how ion exchange columns soften hard water. Fill in the boxes on the right.
Keywords: ammonium, litmus, purity. Insoluble, soluble, hard, scum, precipitate, solute,
Describe and explain 2 uses of ion testing
How do calcium ions get into water?
Define these keywords: temporary hardness, ion exchange column, permanent hardness

3. C3 Topic 2 Quantitative analysis
This topic looks at:
Particles and moles
Preparing soluble salts
Titrations and calculations
6 mark question practice: Describe how you would make dry pure crystals of copper sulphate using a neutralisation reaction between an insoluble base and an acid. (5 step process, include the balanced symbol equation)
Number of moles of an element = mass of element in grams
relative atomic mass
Number of moles of a compound = mass of compound in grams
relative formula mass
Work out the number of moles in:
80g of calcium g of SO g of CaCO g of Ca(OH)2
Work out the mass of:
1. 1 mole of Cu atoms moles of MgCO moles of water
Top tip: make sure you convert to dm3
Keywords: relative atomic mass, Avogadro’s number, moles, relative formula mass
Concentration of a solution in mol dm-3 = number of moles of solute
volume of solution in dm3
Work out the concentration of these solutions:
6 moles of HCl in 3dm moles of NaOH in 250cm moles in 10cm3
Keywords for preparing soluble salts: base, salt, soluble, excess, filtrate, crystallise
Soluble salts are prepared from an a_____ and an i_________ reactant.
Excess of the reactant is added to make sure all of the a______ is u______ u_ .
The excess reactant can be removed by f________________________ .
The solution remaining is only s_____ and w______.
1000 cm3 in a dm3
Now use both the equations above to work out these:
A solution of H2SO4 has a concentration of 2 mol dm-3 .
How many moles of H2SO4 are in 1dm3 of solution?
What is the R.F.M of H2SO4 ?
What is the concentration of H2SO4 in g dm-3?
2. Copper sulphate CuSO4 is dissolved in water to make a 2 mol dm-3 concentration. Calculate the mass of copper sulphate dissolved in 500cm3 of the solution.

4. C3 Topic 2 Quantitative analysis
This topic looks at:
Particles and moles
Preparing soluble salts
Titrations and calculations
cm3
Burette
To prepare a soluble salt from a soluble base (= an alkali) and an acid, you have to use titration.
You usually put a fixed volume of alkali in the conical flask and titrate in a known concentration acid from a burette.
But you can also put a fixed volume of acid in the conical flask and titrate in a known concentration alklai from a burette.
Why do we use pipettes and burettes?
Why do we repeat the titration at least three times?
What should you do with the first result? Why?
Pipette
cm3
6 mark question: Describe how you could use titration to produce a pure sample of potassium nitrate KNO3
Keywords: titration, burette, pipette, indicator, phenolphthalein, litmus, clear end-point.
Keywords: hydrogen ions, hydroxide ions, neutralisation, alkali, acid, titre, evaporation.
Name two suitable indicators for use in titrations. State the colour changes in acid and alkali.
Why should you not use universal indicator in titrations?
State two uses of ammonium nitrate.

5. C3 Topic 2 Quantitative analysis
This topic looks at:
Particles and moles
Preparing soluble salts
Titrations and calculations
In a titration 20cm3 of a sodium hydroxide solution needed 30cm3 of 0.2 mol dm-3 hydrochloric acid to react completely. Work out the concentration of the sodium hydroxide solution.
2. In three titrations of 25cm3 of unknown concentration of sulfuric acid solution, 22.45, and cm3 of 0.1 mol dm-3 of sodium hydroxide were needed. What is the concentration of sulfuric acid solution?
H2SO4 + 2NaOH  Na2SO4 + 2H2O
Which triangle is used to calculate mole concentration from a given volume and number of moles?
Calculate the mole concentration of 345cm3 of NaCl.
Which triangle is used when converting mass concentration to mole concentration?
Calculate the mole concentration of 3.46g d/dm3 of sodium hydroxide.
SHOW YOUR WORKING
Keywords: hydrogen ions, hydroxide ions, neutralisation, alkali, acid, titre, evaporation.
Sort these soluble compounds into acids and alkalis (soluble bases):
Sodium hydroxide, citric acid, potassium hydroxide, ethanoic acid.
Write the word equation for a neutralisation reaction using two of these.

6. C3 topic 3 Electrolytic processes
This topic looks at:
Electrolysis
Electrolysis of salts
Uses of electrolysis
Write balanced half equations for the reaction at the anode or cathode for Na+ ions , Pb2+, Br- and Cl- ions.
What is an electrolyte?
In electrolysis two electrodes attached to a DC electricity supply are put into the electrolyte. Name the two types of ions and explain which electrode they will migrate towards and why.
Which products form in the electrolysis of sodium chloride solution (add ionic half equations)?
Create ionic half equations to show what forms at the electrodes:
Copper chloride solution
(ii) copper sulfate solution
(iii) Sodium sulfate solution
(iv) Molten lead bromide
Keywords: electrolytes, electrolysis, cations, cathode, anions, anode, reduction O I L R G
Describe the electrolysis of brine (sodium chloride in water)
Complete this to show what oxidation and reduction are.
Why are electrodes for electrolysis made of graphite, not metal?
In the electrolysis of copper sulfate solution, is copper reduced or oxidised?
More keywords: oxidation, discharged, corrosive, impure, refined, electroplating, corrosion

7. C3 topic 3 Electrolytic processes
This topic looks at:
Electrolysis
Electrolysis of sodium chloride
Uses of electrolysis
6 mark answer practice: Describe how you would electroplate a nickel medal with silver. Include two methods to make the layer of silver thicker.
Why does copper used for electrical wires need to be pure?
What is copper ore?
How is copper extracted from its ore?
How is copper purified (describe mass changes too)?
KeyWords: hydrogen fuelled, electroplated, galvanized, pure, resistance, dissociate
Explain how electroplating can be used to improve the appearance and the resistance to corrosion of metal objects.
Write the half equations for the anode and cathode reactions.
KeyWords: smelting, refined, anode, cathode, reduction, oxidation, sludge, increasing current, corrosion, cheaper, attractive

8. C3 topic 4 The Haber process
This topic looks at:
Fertilisers
The Haber process
Equilibria
6 mark practice: Over-use of fertiliser use can lead to excessive plant growth in rivers and lakes. Describe this process.
What do fertilisers contain and why?
Describe what is meant by a reversible process
Explain what is meant by an exothermic and an endothermic reaction
What is a dynamic equilibrium?
Keywords: fertilisers, manure, guano, ammonia, proteins, growth, Fritz Haber, reversible
Write the balanced symbol equation for the formation of ammonia.
6 mark practice: Explain the use of compromise conditions for the Haber process.
Equilibrium
Making changes to the concentration, pressure 
or temperature of a reaction can alter the position of the  equilibrium. The rule is that any change made to a reaction which is in equilibrium will result in the equilibrium position moving to minimise the change made (Le Chatelier's principle).
If you increase the temperature in a reaction where the forward process is exothermic, what will happen?
2. If you increase the pressure in this reaction, what will happen?
2SO2(g) + O2(g)   2SO3(g)
Advantages of artificial fertilisers
Disadvantages of artificial fertilisers

9. C3 topic 4 Gases, equilibria and ammonia
This topic looks at:
Molar volumes of gases
Fertilisers
The Haber process
moles = mass relative atomic mass
Calculating volumes of gases.
Write out the balanced symbol equation (if not given)
2. Work out the number of moles of the compound or element for which you are given the mass or the volume.
3. Use the balanced symbol equation to work out the number of moles of gas you are trying to find .
4. Calculate the volume of gas
e.g. How much hydrogen is needed to obtain 2.54g of copper by reducing copper oxide?
1, H2 + CuO  Cu + H2O
2. Moles = mass / molar mass
Moles = 2.54 / 63.5 = 0.04 moles
3. 1 mole of Cu needs 1 mole of H2
moles of H2 has a volume of:
0.04 x 24 = 0.96dm3
Describe how the particles in a gas can move.
Which triangle is used to calculate the number of moles in a gas?
moles =
mass
relative formula mass
KeyWords: mole, molar volume, Avogadro’s law, room temperature, atmospheric pressure
What is the volume of 3 moles of oxygen?
How many moles of helium are there in 120dm3 ?
Now try these:
The combustion of ethane is given by the equation: 2C2H6(g) + 7O2(g)4CO2(g) + 6H2O(l) What volume of carbon dioxide in cm3 is formed by burning 20g of ethane?
The combustion of methane is given by the equation: CH4(g) + 2O2(g)  CO2(g) + 2H2O(l) What volume of carbon dioxide in cm3 is formed on burning 710g of methane?
Mg(s) + 2HCl(aq)  MgCl2(aq) + H2(g) What volume of hydrogen gas, in dm3, is formed when 72g of magnesium dissolves in the acid?
What is the volume in dm3 of 0.85 g of a gas of molecular mass 17? 
2Na(s) + 2H2O(l)  2NaOH(aq) + H2(g) What mass of sodium in g will form 18 dm3 of hydrogen gas?
Define ‘molar volume of a gas’.
KeyWords: fertilisers, proteins, growth, nitrogenous, Haber process, reversible, eutrophication, algal bloom, decomposed, NH3

10. Naming organic compounds
C3 topic 5 Organic chemistry
This topic looks at:
Alcohol and the production of ethanol
Carboxylic acids and reactions of ethanoic acid
Esters
Soaps, fats and oils
Write word and symbol equations for the reactions of ethanoic acid with metals, bases, carbonates and indicators, a) b) c) d)
Ethanol can be produced by two different methods. These are: 1. 2.
What are the social issues associated with alcohol consumption and the effects of ethanol?
Write the names and structures of the first three carboxylic acids.
a) Methanoic acid
b) Ethanoic acid
c) Propanoic acid
KeyWords: ethanol, esters, hydroxyl, ethanoic acid, carboxylic acid,
Identification Key
Draw diagrams to show the functional groups in:
Alcohols
ii) Carboxylic acids
iii) Esters
Naming organic compounds
1 Carbon = meth
2 Carbon =
3 Carbon =
4 Carbon =
5 Carbon =
Uses of ethanoic acid
Fill in your own keywords:

11. C3 Organic chemistry
This topic looks at:
Alcohol and the production of ethanol
Carboxylic acids and reactions of ethanoic acid
Esters
Soaps, fats and oils
Show the reaction of alcohols with carboxylic acids to produce esters by drawing the structural formulae
Methanol + ethanoic acid 
Ethanol + propanoic acid 
c) Propanol + pentanoic acid 
What is a homologous series? Name examples and general formulae
Fats and oils are naturally occurring esters. What are the main differences between fats and oils?
Explain how liquid oils can be converted to solid fats
Keywords: hydrophilic, hydrophobic, recycling, plastics
Explain the uses of esters
Explain how soap anions remove dirt.
How are soaps created?