1. Principles of Chemistry Revision – PARTICLES
Draw a representation of the particles in a solid, liquid and gas. Name the transitions
KEY WORDS:
Particle
Kinetic theory
Solid
Liquid
Gas
Attraction
Complete the table to compare AND explain the properties
Solid
Liquid
Gas
Define diffusion. Give an
example
How do
particles
move?
Attraction
between
particles
Arrangement
of particles
Shape
Compressibility
1
2. Principles of Chemistry Revision – Atomic Structure
Draw the symbol for sodium
include its atomic mass and atomic
number (what do they tell us?)
What are the charges and masses of
electrons, protons and neutrons?
Where are electrons and neutrons and protons
found in an atom?
What is an electron ‘shell’?
How many electrons can be
found in each ‘shell’?
Draw the electronic configuration for sodium, oxygen
and argon
How many atoms of which elements are there in: C2H5OH ?
What is an alloy? Give two examples and how they are useful
Define Isotope:
Give an example:
KEY WORDS:
Electron
Proton
Neutron
Shell
Electronic Configuration
Orbit
What is a radioactive
isotope?
3
3. Principles of Chemistry Revision – CHEMICAL BONDING 1
Describe how sodium and chlorine bond;
Use a dot cross diagram to show
how sodium and chlorine bond
Describe the structure of metals and metallic
bonding
List the properties of metals
Complete the table to show and explain the properties of ionic compounds
Property
Ionic quality
Explanation
Hardness
Melting/boili
ng point
Solubility
Conductivity
Malleability
KEY WORDS:
Electron
Proton
Neutron
Shell
Electronic Configuration
Covalent/Ionic/Metallic
4
4. Principles of Chemistry Revision – CHEMICAL BONDING 2
Make a diagram to explain how a giant lattice is formed for an ionic structure
Diamonds and Graphite are both made of carbon. Make a table of their differences
KEY WORDS:
Electron
Sharing
Inter molecular
Covalent/Ionic/
Metallic
Attraction
5
5. Principles of Chemistry Revision – STOICHIOMETRY
What is Ar?
What is a mole?
What is Mr?
What equation links mole with mass?
What is the Mr of C2H5OH?
What equation links mole with concentration
of solution?
What is Avogadro’s number?
Write the formula of:
Magnesium oxide:
What is percentage yield and what is the
equation to calculate it?
H2 + O2  H2O
N2 + H2  NH3
S8 + O2  SO3
N2 + O2  N2O
HgO  Hg + O2
CO2 + H2O  C6H12O6 + O2
Zn + HCl  ZnCl2 + H2
SiCl4 + H2O  H4SiO4 + HCl
Na + H2O  NaOH + H2
H3PO4  H4P2O7 + H2O
C10H16 + Cl2  C + HCl
Calculate what volume of hydrogen gas is formed at RTP when
5.7g of magnesium is added to excess sulfuric acid..
Sodium chloride:
Potassium phosphide:
Balance these equations:
Calculate the empirical formula for a
compound containing:
Na 0.167 g, C 0.0435 g, O 0.174 g
KEY WORDS:
Calcium fluoride:
Reversible
Haber Process
Relative Atomic Mass
Relative Formula Mass
Isotope
Moles
6
6. Physical Chemistry Revision – ELECTROLYSIS 1
What is electrolysis?
What does OILRIG stand for?
What do we call the substance that is
broken down during electrolysis
Describe the movement of ions and electrons at
each electrode when potassium iodide is
electrolysed
How is the electrolysis of used to purify
copper? [Draw a diagram to help]
What is the positive electrode called?
What is the negative electrode called?
Label a diagram showing the electrolysis
of Lead (II) bromide
What happens when a solution containing
potassium iodide is electrolysed?
What 3 products are made when we electrolyse
brine? Give a use for each?
KEY WORDS:
What ions are formed?
Electrolysis
Cathode
Anode
Oxidation
Reduction
7
7. Physical Chemistry Revision – ELECTROLYSIS 2 & REDOX
What is electroplating and what is it used for?
Oxidation can be defined in two ways, they
are:
What is a reducing agent?
What is an oxidising agent?
Reduction can be defined in two ways, they
are:
Describe the process used to extract aluminium
from its ore. Give the conditions. Include
equations. A diagram could be useful.
Write the symbol equation for the
displacement of copper from copper(II)
oxide by zinc.
What are oxidation states?
How are they shown in chemical names, give an
example?
Rewrite this as an ionic equation
What do changes in oxidation state represent?
Give 3 uses of aluminium and the properties
that make it useful
Rewrite this as two half equations
KEY WORDS:
Redox
Electron
Oxidation
Reduction
Agent
Ion
8
8. Physical Chemistry Revision– ENERGY & REACTIONS 1
What are exothermic reactions?
Define Enthalpy change (its symbol?)
Give an example and explain why it is
exothermic?
Define activation energy
What are bond energy values? Why are they
average values?
What are bond energy values? Why are they
average values?
What are endothermic reactions?
Draw fully labelled energy profile diagrams for
exo and endo thermic reactions.
Explain how to calculate bond energy for a
reaction:
Give an example and explain why it is
endothermic
KEY WORDS:
Collision Theory
Catalyst
Activation Energy
Rate of Reaction
Concentration
Temperature
Bond Energy values (J/mol)
H−H
F-F
H−F
O−H
C−H
432
154
565
467
413
Cl−Cl 239
C−O 358
C=C 614
C≡O 1072
C=O 745
C−C 347
C=O 799
C−Cl 339
O=O 495
9
9. Physical Chemistry Revision – ENERGY CALCULATIONS 2
We calculated the energy used when burning fuels using the following calculation:
Energy released = mass of water X
specific heat
X
rise in
heated
capacity of water
temperature
This is sometimes written as:
Use the bond energy values on the previous page to calculate
the enthalpy change for each of these reactions:
1. H2(g) + F2(g) → 2HF(g)
𝑄 = 𝑚𝑐∆𝑇
We also need to know the amount of energy released per gram or per mole to
compare the efficiency of the fuels:
1𝑔
Energy released per gram (kJ/g) = energy released X
2.
CH4(g) + 2O2(g) → CO2(g) + 2H2O (g)
3.
CO(g) + 2H2(g) → CH3OH(l)
4.
2H2(g) + O2(g) → 2H2O(g)
5.
2H2O(g) → 2H2(g) + O2(g)
𝑐ℎ𝑎𝑛𝑔𝑒 𝑖𝑛 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑓𝑢𝑒𝑙
Energy released per mole (kJ/mol) = energy released X
𝑅𝐴𝑀 𝑜𝑓 𝑓𝑢𝑒𝑙
𝑐ℎ𝑎𝑛𝑔𝑒 𝑖𝑛 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑓𝑢𝑒𝑙
Use these equations to show which fuel is more efficient:
0.2 g of fuel A heats 50g of water from 16°C to 41°C
0.46 g of fuel B heats 50g of water from 21°C to 57°C
0.13 g of fuel C heats 35ml of water from 21°C to 46°C
KEY WORDS:
Energy release
Activation
Energy
energy
transfer
Catalyst
Solutions
Bond breaking
Exothermic
Bond making
Endothermic
Bond energy
10
10. Physical Chemistry Revision – RATES OF REACTION
What do we mean by ‘rate of
reaction’?
Explain the effect of concentration on the
rate of reaction
Explain the effect of temperature on the rate of
reaction [think about: kinetic energy & number of
collisions]
What 4 factors affect the rate
of a reaction?
What must happen for a reaction
to occur?
Draw diagrams to represent it?
Draw diagrams to represent it:
What is the smallest amount of
energy that must be overcome for
a reaction to occur?
How does surface area affect
rate of reaction?
Low concn
High concn
What do catalysts do?
Low temp
High temp
KEY WORDS:
Give two examples of catalysed reactions
Collision Theory
Catalyst
Activation Energy
Rate of Reaction
Concentration
Temperature
11
11. Physical Chemistry Revision – REVERSIBLE REACTIONS
What is a reversible reaction?
What is the symbol for a reversible
reaction?
What can you say about energy in a reversible
reaction? [Think: exo and endothermic]
What happens to the equilibrium when the
concentration of products is increased? Why?
What is a dynamic equilibrium?
If the forward reaction of an equilibrium is
exothermic and the temperature of the system
is increased, what would happen to the
equilibrium why?
What is the Haber process?
State Le Chatelier’s principle
What are the raw materials?
For the Haber process, what would happen to
the equilibrium if the pressure was reduced
why?
What is the reaction equation?
KEY WORDS:
What conditions are required?
Collision Theory
Catalyst
Activation Energy
Rate of Reaction
Concentration
Temperature
How does a catalyst affect the equilibrium?
Why?
12
12. Physical Chemistry Revision – ACIDS, ALKALIS & SALTS
What is a base?
Write a general equation for an acid reacting
with a metal and two examples:
What is produced when an acid and an alkali react?
What type of reaction is this called?
What is an alkali?
How can this reaction be simplified using just the ions
involved?
What ions make something alkali?
Define Acid:
Write a general equation for an acid reacting
with a base and two examples:
What ions make something acidic?
What is a precipitation reaction?
How can we make ammonium hydroxide?
What is the pH scale?
What happens when we add nitric acid to it?
Describe 2 uses for acids and alkalis in the ‘real world’
KEY WORDS:
Acid
Base
Alkali
pH scale
Indicator
Precipitate
13
13. Inorganic Chemistry Revision – THE PERIODIC TABLE
State how each of these scientists aided in
the development of the modern periodic table:
Newland:
Describe how the modern periodic
table is arranged:
Mendeleev:
What are rows called in the P. table?
Create a key for the colours displayed on the periodic table above:
What are columns called?
Group 1 – the alkali metals:
Describe the properties:
Give some group 1 compounds and their uses
Describe their reactions with air
Describe their reactions with water
Describe Group 1 reactions with chlorine
KEY WORDS:
Reactivity
Reactive metals
Non-metals
Melting point
Boiling point
Alkali metals
14. Inorganic Chemistry Revision – THE PERIODIC TABLE
Group 7 – the Halogens
Describe the properties:
Describe their reactions with
Metals
Give some group 1 compounds and their uses:
Describe their reactions with water
Write ionic
equations for the
halogen displacement
reactions
Describe what the halogen displacement reactions are and why
they occur:
KEY WORDS:
Transition metals
Describe the properties:
Noble gases – group 8/0
Describe the properties and electron structure:
What is unique about trans metals oxidation states and
how does this affect them?
Give some uses of noble gases:
Reactivity
Reactive metals
Non-metals
Melting point
Boiling point
Halogens
Nobel gases
16
15. Inorganic Chemistry Revision – METALS
Put these metals in their order of reactivity
Carbon, Calcium, aluminium, Magnesium, potassium, lead, gold, Copper, Iron, zinc,
silver, sodium
Write a general equation and two examples for each below:
Heating metal nitrate
Complete the displacement equation below and then make your own :
Copper Oxide + Carbon
 _______________ + _______________

Heating metal carbonate


What is an ore?
How is steel made? Include equations
Heating metal hydroxides
How is iron extracted? Include equations
Give 2 uses of:
Aluminium
Copper
Draw a diagram to show metallic bonding
KEY WORDS:
DISPLACEMENT
ORE
BLAST FURNACE
ALLOY
Steel
Metallic bonding
17
16. Inorganic Chemistry Revision – SULFUR AND CARBONATES
Describe the steps of the contact process. Include equations. You could use a
diagram.
Write equations to show how sulfuric acid reacts with
alkalis, bases, carbonates and glucose:
Describe some uses of:
Quicklime
Limestone
Slaked lime
What is sulfuric acid used for?
What are the conditions for
industrial thermal decomposition of
limestone
KEY WORDS:
DISPLACEMENT
ORE
BLAST FURNACE
ALLOY
Steel
Metallic bonding
18
17. Inorganic Chemistry Revision – AIR & WATER
What are the layers of the Earth?
What is the chemical test for water?
Sketch the water cycle
Complete the table to show the
atmosphere of Earth today
Gas
%
How is water cleaned for drinking?
Others (inc. Argon)
Describe the Nitrogen cycle
How are humans disrupting/
effecting the nitrogen cycle?
What is the carbon cycle? Briefly
describe the steps
What are NPK fertilisers?
What are the three key processes of the C cycle?
Give the equations
KEY WORDS:
ATMOSPHERE
CARBON CYCLE
Nitrates
Nitrifying bacteria
Decomposers
Precipitation
19
18. Inorganic Chemistry Revision – POLLUTION
Complete the table to show the source of pollutants in the air
Pollutant
Sketch a diagram to show global warming
Source
Carbon monoxide
Sulfur dioxide
Nitrogen oxides
Lead compounds
Describe how acid rain forms.
Include equations.
Describe some techniques used to
reduce pollutants in the air
What are CFCs? Why are they
important to pollution chemistry?
Describe methods used to prevent rusting.
KEY WORDS:
ATMOSPHERE
CARBON CYCLE
Nitrates
Nitrifying bacteria
Decomposers
Precipitation
20
19. Organic Chemistry Revision – CRUDE OIL & FUELS
Name the process by which we separate crude
oil into useful components:
What are fossil fuels?
Give the name of 8 fractions of crude oil and their uses
Fraction
Use
Num. of C
What property does this process rely on?
How does it work?
What are hydrocarbons?
Write a general equation for combustion and incomplete combustion
Describe how these properties change further up the
fractionating column:
Boiling point
Molecule size
Viscosity
What does ‘cracking’ mean?
Ease of burning
Smokiness of flame
Strength of intermolecular forces
Why is cracking important?
KEY WORDS:
Write an equation with an example of a cracking reaction
ALKANE
ALKENE
SATURATED
FRACTIONAL DISTILLATION
COMBUSTION
21
20. Organic Chemistry Revision – ALKANES AND ALKENES
What does it mean if a molecule is
saturated or unsaturated?
What is a homologous series?
Describe the, use, procedure and outcome of the bromine test
Complete the table to summarise alkanes and alkenes:
ALKANES
Saturated or
unsaturated
ALKENES
Define Isomer
Define Structural isomerism
Reactivity
General formula
Uses
Draw and name 2 isomers of C6H14
Name the first 5
Draw an example
KEY WORDS:
CRACKING
POLYMERISATION
PLASTIC
POLYMER
MONOMER
FERMENTATION
BIODEGRADABLE
22
21. Organic Chemistry Revision – ORGANIC CHEMISTRY
Alcohols:
What is the functional group and general
formula?
Carboxylic acids:
What is the functional group and general
formula?
Draw 2 structural isomers of butanol
Draw and name the structure of the first 3
members:
Esters:
Describe how esters are made:
Give two uses of esters:
Draw and name three esters
Briefly state the some of the uses of alcohol:
Describe how carb, acids are made, include an
equation:
Describe the conditions and procedure of
producing ethanol by
Fermentation:
Describe the reaction of carboxylic acid with
carbonates:
Briefly describe the issues of using ethanol as a fuel
Hydration:
KEY WORDS:
Alcohol
Functional
group
Homologous
series
Carboxylic acid
Esters
Combustion
Oxidation
Ethanol
23
22. Organic Chemistry Revision – POLYMERS
Define monomer and polymer
What is ‘condensation polymerisation’?
List 3 problems with plastics:
Draw an amide link and state what it is formed
from:
Give examples of two naturally
occurring polymers and their
monomers:
Draw an ester link and state what it is formed
from:
Describe and explain how addition polymers form. You could use a diagram
How are biodegradable plastics made?
What are the problems with them?
KEY WORDS:
CRACKING
POLYMERISATION
PLASTIC
POLYMER
MONOMER
FERMENTATION
BIODEGRADABLE
24
23. Principles of Chemistry Revision – EXPERIMENTAL TECHNIQUES
What is the range of a
measuring implement?
What is the function of paper
chromatography?
What is the interval?
Describe the steps involved in paper
chromatography:
What instrument and
unit do you use to
measure:
Describe the steps used to purify a solid. You could use a labelled
diagram.
Describe the steps used to purify an impure liquid. You could use a
labelled diagram.
Time:
Mass:
What is a Retention Factor and how do you
calculate it?
Temperature:
Volume of liquids:
What is the simplest test of purity?
KEY WORDS:
Desalination
Distillation
Soluble
Solvent
Chromatogram
2
24. Physical Chemistry Revision – ANALYSIS AND SYNTHESIS
Fill in the table to show your understanding
of flame tests:
Fill in the flow chart to show your understanding of positive ion tests:
Metal ion
Colour of precipitate
Further tests required
Metal ion
Copper Cu2+
Lithium (Li+)
Reddish-brown
Sodium (Na+)
Iron Fe2+
Lilac
Magnesium Mg2+
Insoluble in excess NaOH, red flame test
Aluminium Al3+
Flame colour
White
Describe how to carryout a titration:
Red
Barium (Ba2+)
Fill in the table to show your understanding of negative ion
tests:
Anion
Test
Observation
CO2 gas produced
Colour precipitate:
Chloride 
Bromide 
Iodide 
Halide
State the different types of chemical
analysis that can be carried out:
Sulphate
KEY WORDS:
Flame test
Sodium
hydroxide
Carbonates
Halides
Sulphates
Titration
White precipitate
End point
Concentration
Chemical analysis
Equilibrium
Pressure
Energy
Haber process
14