Keywords: proton, neutron, electron, shells, negative, atomic number, mass number
C2 Topic 1 Atomic Structure and the Periodic Table
This topic looks at:
• The structure of the atom
• Subatomic particles and electron shells
• The periodic table
How can you use the following
numbers to give you the amount
of protons, neutrons and
electrons?
Electron Structure – Draw the electron
structure of:
Na
Draw the structure of an atom and label it’s subatomic particles giving their
mass and charge
Cl
On the periodic table – colour the metals and non metals separate colours and label the
following. Alkali metals, Halogens, Transition Metals, Halogens.
Al
What do the periods and groups tell you about the electron
structure?
Keywords: stable, full shell, positive, negative, transfer, molten, bonds
C2 Topic 2: Ionic Bonding
Using the structure of ionic compounds can you explain why
This topic looks at:
• Ionic Bonding, structure and properties
• Naming and formula of ionic compounds
• Precipitates
1) They have high boiling/melting points
Give Definitions for the following
ION
CATION
ANION
IONIC BONDING
2) They can conduct when molten but not when solid
Show the ionic bonding of NaCl (don’t forget your charges!)
Keywords: anion, cation, shells, current, ions,
Keywords (electrostatic forces, position, negative, ions, lattice)
Keywords: precipitate, insoluble, soluble, charges, balanced, solid,
C2 Topic 2: Ionic Bonding
Writing Ionic Formula Complete the table
This topic looks at:
• Ionic Bonding, structure and properties
• Naming and formula of ionic compounds
• Precipitates
Write the tests for the following ions
Carbonate CO32Sulfate SO42Chloride ClWrite the formula for
Metal Ions K+, Ca+, Cu2+, Na+
1.
Sodium chloride
2. Magnesium hydroxide
3. Potassium nitrate
4. Calcium carbonate
5. Copper nitrate
6. Aluminium oxide
Precipitates
7. Magnesium oxide
Using the following
8. Calcium hydroxide
table write the
precipitates in the
following reactions
1.
Give definitions for the following
Sodium hydroxide + barium chloride ___________________________
2. Silver nitrate + potassium chloride ___________________________
3. Barium chloride + sodium sulphate
___________________________
Precipitate
Soluble
Insoluble
Keywords: outer electron, nuclear attraction, electrons, nucleus, reactivity
C2 Topic 4: Groups in the Periodic Table
Halogen
This topic looks at:
• Alkali Metals
• Noble Gases
• Halogens
Draw the electronic structure of Fluorine, Chlorine and Bromine. Use this to
explain how the reactivity changes as you go down the group.
What do all the elements in Group 1 have in common?
What do all the elements in Group 7 have in common?
Alkali Metals
Draw the electronic structure of Lithium, sodium and potassium. Use this to
explain how the reactivity changes as you go down the group
Write word and symbol equations for the reaction of the alkali metals with
water
1.
Lithium
2. Sodium
3. Potassium
How could you test for the products formed?
Keywords: inert, delocalised electrons, conduct, unreactive, sea of electrons
C2 Topic 4: Groups in the Periodic Table
Noble gases
This topic looks at:
• Alkali Metals
• Noble Gases
• Halogens
What are the noble gases and what can they be used for?
Displacement Reactions of the Halogens
Write word and balanced symbol equations for the displacement reactions of
the halogens. How does this show you which is the most reactive?
1.
Potassium bromide + chlorine 
2. Potassium iodide + chloride 
What is Metallic bonding? Draw a diagram to explain your answer
3. Potassium iodide + bromine 
Transition Metals?
Will Aluminium be better at conducting that potassium? Why?
What are the transition metals?
Explain why:
1) Metals conduct electricity.
2)
Are Malleable
3) Have high melting points
Keywords: temperature, bond breaking, bond making
C2 Topic 5: Chemical Reactions
This topic looks at:
• Exothermic and endothermic reactions
• Factors that affect rates of reaction
Rates of Reaction. Using the particle model explain how the following affect the
rate of reaction. Make sure you include all the keywords
Concentration (3)
Surface Area (3)
What do you understand by
Endothermic reaction? (3)
Exothermic reaction?(3)
Temperature
(4)
Catalyst (3)
Energy Diagrams – Draw energy diagrams to represent exothermic and
endothermic reactions, Explain what is happening in each case using bond
breaking and formation
EXOTHERMIC
What is a catalyst and what can they be used for?
ENDOTHERMIC
Keywords: temperature, bond breaking, bond making
C2 Topic 5: Chemical Reactions
This topic looks at:
• Exothermic and endothermic reactions
• Factors that affect rates of reaction
Describe, in detail, how you would carry an experiment to measure the rates of
reaction between calcium carbonate and different concentrations of hydrochloric acid.
Explain how a catalytic convertor works.
Describe the benefits
What do you understand by activation energy?
How would you modify the experiment if you were to investigate the effects of
temperature?
Draw graphs to represent how a catalyst effects the activation energy of
energy. Explain what effects this has on the rate of reaction (4)
Explain what type of reaction the graph represents and why?
Keywords: Cabron-12, atomic mass, ratios,
C2 Topic 6: Quantitative Chemistry
Percentage mass
This topic looks at:
•RAM and RFM
•Empirical formula
•Calculating masses of reactants and products
How can you calculate the percentage mass of an element in a compound?
Calculate the percentage mass of oxygen in
What is the RAM of
What is the RFM of
1.
1.
Carbon
Water
2. Magensium
2. Carbon Dioxide
3. Pb
3. CaCO3
4. Potassium
4. Mg(OH)2
5. Neon
5. H2SO4
1. CO and 2. CO2
What is the empirical formula?
Work out the following empirical formulas below
1.Water, is a sample contains 0.6g of hydrogen and 4.8g of oxygen
How can you work out the yield?
What are the reasons for not achieving the expected yield?
2. Lithium carbonate, if a sample contains 2.8g of lithium and 2.4 g of carbon
and 9.6g of oxygen.
Keywords: Cabron-12, atomic mass, ratios,
C2 Topic 6: Quantitative Chemistry
Calculating Reactants and Products
This topic looks at:
•RAM and RFM
•Empirical formula
•Calculating masses of reactants and products
1. a. What is the theoretical yield that could be obtained from 256g of sulfur dioxide.
2SO2 + O2  2SO3
Name 3 products made in the petrochemical industry
1.
2.
3.
b. The actual yield of sulfur trioxide produced is 202g. Calculate the percentage yield.
Why is it expensive to dispose of waste products?
2. a. Iron is extracted from iron oxide by reducing with carbon
Fe2O3 + 3CO  2Fe + 3CO2
Using ideas about waste products explain why people
would object to a proposal to build a new factory to
manufacture plastics near to their home?
Calculate the theoretical yield of iron that could be obtained from 320 g of iron oxide.
b. The actual yield of iron produced is 89.6g. Calculate the percentage yield.