The Periodic Table AND Physical & Transition Metal worksheet. (M3 & M5) OCR 2025
Chapter 7 - Periodicity
1) How is the periodic table arranged?
2) What are the four blocks of the periodic table and give a definition of each:
3) What is a first ionisation energy?
4) What are the three factors that affect first ionisation energy, stating whether they cause
an increase or decrease in ionisation energy:
5) Will the second successive ionisation energy be larger or smaller than the prior and
explain why:
6) Write an equation for the second ionisation of Iron stating whether it will be endothermic
or exothermic and why:
7)
a) Draw the general trend in first ionisation energies across the first period (Li - Ne):
b) Explain why this general pattern occurs:
c) Explain the two exceptions to this pattern:
d) Describe how this graph may change for element of period 3 rather than
elements of period 2:
8)
a) Draw the general trend in first ionisation energies down group 1 (Li - Cs):
b) Explain why this pattern occurs:
c) Describe how this graph may change for elements of group 6 rather than
elements of group 1:
9) The graph shows successive ionisation energies for an element. Which group of the
periodic table is this element in?
10) The first five successive ionisation energies of an element Y are shown below. What
Group is element Y from:
First Second Third Fourth Fifth
496 4563 6913 9544 13352
,The Periodic Table AND Physical & Transition Metal worksheet. (M3 & M5) OCR 2025
Chapter 8 - Reactivity Trends
1) What block of the periodic table is group 2 in?
2) Describe and explain the trend in reactivity down group 2.
3) Write two real life uses of group 2 compounds as bases.
4) Explain the trend in the alkalinity of the solution formed when group 2 oxides are added
to water.
5) What causes the boiling point to increase down the halogen group?
6) Explain the trend in reactivity down the Halogen group.
7) What colours form when these Halogens are dissolved in cyclohexane (a nonpolar
substance)?
a) Chlorine
b) Bromine
c) Iodine
8) Write the equation and state the colour change of the reaction between aqueous
bromide ions and aqueous chlorine.
9) When small amounts of chlorine are added to water, a disproportionation reaction
occurs.
a) Write an equation for this reaction.
b) Why is it a disproportionation reaction?
c) What real life use does this reaction have?
10) What reagents and observations show a positive test for a carbonate? Write an equation
for each step.
11) What reagent and observation shows a positive test for a sulfate? Write an ionic equation
for this reaction.
12) When testing for a halide
a) What are the reagents for a halide test?
b) Write the positive result for chloride
c) Write the positive result for bromide
d) Write the positive result for iodide
13) What is the correct sequence of tests for an anion, and state a reason for each.
14) How do you test for ammonium ions?
,The Periodic Table AND Physical & Transition Metal worksheet. (M3 & M5) OCR 2025
Chapter 9 - Enthalpy
1) What is enthalpy?
2) What is enthalpy change?
3) Outline the law of conservation of energy.
4) What is the difference between exothermic and endothermic?
5) What is activation energy? (+ a diagram to demonstrate change in enthalpy for both
endothermic and exothermic reactions):
6) What are the standard conditions?
7) Define with examples:
(i) Standard enthalpy change of reaction.
(ii) Standard enthalpy change of formation.
(iii) Standard enthalpy change of combustion.
(iv) Standard Enthalpy change of neutralisation.
8) What is the equation for enthalpy change, annotate it.
9) Outline a method to determine the enthalpy change of combustion.
10) Calculate the enthalpy change in kJ mol-1 when excess Mg is added to 100cm3 of 2.00
mol dm-3 CuSO4, the temperature rose from 20.0oC to 65.0oC.
The specific heat capacity of CuSO4(aq) is 4.18 J g-1 K-1.
11) This question looks at neutralisation reactions.
A student carries out an experiment to determine the enthalpy change for a
neutralisation reaction. The student measures out 35.0 cm3 of 2.40 mol dm–3 KOH and
35.0 cm3 of 1.20 mol dm–3 H2SO4. The temperature of each solution is 19.5 oC.
The student mixes the solutions. The KOH is all neutralised and the maximum
The temperature reached 36.0 °C.
Write the overall equation for the reaction that takes place.
Calculate the enthalpy change for the reaction between 1 mol KOH and 1 mol H2SO4.
Assume that the density of the mixture is 1.00 g cm–3 and that the specific heat
capacity for the solution is the same as for water.
12) How accurate are the experimental values?
13) What is a calorimeter?
14) How do cooling curves work?
15) What is an average bond enthalpy?
16) What are the limitations of average bond enthalpies?
17) Bond breaking is Exothermic [TRUE/FALSE].
18)
19) What is Hess’s Law?
20)Summarise Hess’s Law.
, The Periodic Table AND Physical & Transition Metal worksheet. (M3 & M5) OCR 2025
Chapter 10: Reaction Rates and Equilibrium
1) What does the ‘rate of a chemical reaction’ mean?
2) Describe this graph, and what is occurring:
3) What factors alter the rate of a chemical reaction?
4) Outline collision theory.
5) How does increasing the concentration affect the rate of reaction?
6) How does increasing the pressure of a gas affect the rate of reaction?
7) Name 2 methods for following the progress of a reaction.
8) Name 2 methods specific to reactions which produce a gas.
9) Describe an experimental method to deduce the rate of a reaction producing a gas.*
10) How can you edit this so you can use a mass balance?
11) What is a catalyst and its key features?
12) Draw enthalpy profile diagrams showing the change after the addition of a catalyst.
13) What is a homogeneous catalyst AND how does it work?
14) Detail 2 examples of homogeneous catalysts.
15) What is a heterogeneous catalyst AND how does it work?
16) Detail 4 examples of heterogeneous catalysts.
17) Deduce the sustainability and economic importance of catalysis.
18) What does the Boltzmann distribution show?
19) List the features, and label them on a drawn graph of boltzmann distribution.
20)How does it change with temperature + a line on your graph to show this?
21) How does it change with catalysts + a line on your graph to represent this?
22)What are reversible reactions?
23)Describe ‘Dynamic equilibrium’.
24)What is a ‘closed system’?
25)What does Le Chatelier’s principle state?
26)What is the effect of concentration on a reaction in equilibrium?
27)What is the effect of temperature on a reaction in equilibrium?
28)What is the effect of pressure on a reaction in equilibrium?
29)What is the effect of a catalyst on a reaction in equilibrium?
30)Using the Harber process as an example, describe how these factors may be controlled in
real life.
Chapter 7 - Periodicity
1) How is the periodic table arranged?
2) What are the four blocks of the periodic table and give a definition of each:
3) What is a first ionisation energy?
4) What are the three factors that affect first ionisation energy, stating whether they cause
an increase or decrease in ionisation energy:
5) Will the second successive ionisation energy be larger or smaller than the prior and
explain why:
6) Write an equation for the second ionisation of Iron stating whether it will be endothermic
or exothermic and why:
7)
a) Draw the general trend in first ionisation energies across the first period (Li - Ne):
b) Explain why this general pattern occurs:
c) Explain the two exceptions to this pattern:
d) Describe how this graph may change for element of period 3 rather than
elements of period 2:
8)
a) Draw the general trend in first ionisation energies down group 1 (Li - Cs):
b) Explain why this pattern occurs:
c) Describe how this graph may change for elements of group 6 rather than
elements of group 1:
9) The graph shows successive ionisation energies for an element. Which group of the
periodic table is this element in?
10) The first five successive ionisation energies of an element Y are shown below. What
Group is element Y from:
First Second Third Fourth Fifth
496 4563 6913 9544 13352
,The Periodic Table AND Physical & Transition Metal worksheet. (M3 & M5) OCR 2025
Chapter 8 - Reactivity Trends
1) What block of the periodic table is group 2 in?
2) Describe and explain the trend in reactivity down group 2.
3) Write two real life uses of group 2 compounds as bases.
4) Explain the trend in the alkalinity of the solution formed when group 2 oxides are added
to water.
5) What causes the boiling point to increase down the halogen group?
6) Explain the trend in reactivity down the Halogen group.
7) What colours form when these Halogens are dissolved in cyclohexane (a nonpolar
substance)?
a) Chlorine
b) Bromine
c) Iodine
8) Write the equation and state the colour change of the reaction between aqueous
bromide ions and aqueous chlorine.
9) When small amounts of chlorine are added to water, a disproportionation reaction
occurs.
a) Write an equation for this reaction.
b) Why is it a disproportionation reaction?
c) What real life use does this reaction have?
10) What reagents and observations show a positive test for a carbonate? Write an equation
for each step.
11) What reagent and observation shows a positive test for a sulfate? Write an ionic equation
for this reaction.
12) When testing for a halide
a) What are the reagents for a halide test?
b) Write the positive result for chloride
c) Write the positive result for bromide
d) Write the positive result for iodide
13) What is the correct sequence of tests for an anion, and state a reason for each.
14) How do you test for ammonium ions?
,The Periodic Table AND Physical & Transition Metal worksheet. (M3 & M5) OCR 2025
Chapter 9 - Enthalpy
1) What is enthalpy?
2) What is enthalpy change?
3) Outline the law of conservation of energy.
4) What is the difference between exothermic and endothermic?
5) What is activation energy? (+ a diagram to demonstrate change in enthalpy for both
endothermic and exothermic reactions):
6) What are the standard conditions?
7) Define with examples:
(i) Standard enthalpy change of reaction.
(ii) Standard enthalpy change of formation.
(iii) Standard enthalpy change of combustion.
(iv) Standard Enthalpy change of neutralisation.
8) What is the equation for enthalpy change, annotate it.
9) Outline a method to determine the enthalpy change of combustion.
10) Calculate the enthalpy change in kJ mol-1 when excess Mg is added to 100cm3 of 2.00
mol dm-3 CuSO4, the temperature rose from 20.0oC to 65.0oC.
The specific heat capacity of CuSO4(aq) is 4.18 J g-1 K-1.
11) This question looks at neutralisation reactions.
A student carries out an experiment to determine the enthalpy change for a
neutralisation reaction. The student measures out 35.0 cm3 of 2.40 mol dm–3 KOH and
35.0 cm3 of 1.20 mol dm–3 H2SO4. The temperature of each solution is 19.5 oC.
The student mixes the solutions. The KOH is all neutralised and the maximum
The temperature reached 36.0 °C.
Write the overall equation for the reaction that takes place.
Calculate the enthalpy change for the reaction between 1 mol KOH and 1 mol H2SO4.
Assume that the density of the mixture is 1.00 g cm–3 and that the specific heat
capacity for the solution is the same as for water.
12) How accurate are the experimental values?
13) What is a calorimeter?
14) How do cooling curves work?
15) What is an average bond enthalpy?
16) What are the limitations of average bond enthalpies?
17) Bond breaking is Exothermic [TRUE/FALSE].
18)
19) What is Hess’s Law?
20)Summarise Hess’s Law.
, The Periodic Table AND Physical & Transition Metal worksheet. (M3 & M5) OCR 2025
Chapter 10: Reaction Rates and Equilibrium
1) What does the ‘rate of a chemical reaction’ mean?
2) Describe this graph, and what is occurring:
3) What factors alter the rate of a chemical reaction?
4) Outline collision theory.
5) How does increasing the concentration affect the rate of reaction?
6) How does increasing the pressure of a gas affect the rate of reaction?
7) Name 2 methods for following the progress of a reaction.
8) Name 2 methods specific to reactions which produce a gas.
9) Describe an experimental method to deduce the rate of a reaction producing a gas.*
10) How can you edit this so you can use a mass balance?
11) What is a catalyst and its key features?
12) Draw enthalpy profile diagrams showing the change after the addition of a catalyst.
13) What is a homogeneous catalyst AND how does it work?
14) Detail 2 examples of homogeneous catalysts.
15) What is a heterogeneous catalyst AND how does it work?
16) Detail 4 examples of heterogeneous catalysts.
17) Deduce the sustainability and economic importance of catalysis.
18) What does the Boltzmann distribution show?
19) List the features, and label them on a drawn graph of boltzmann distribution.
20)How does it change with temperature + a line on your graph to show this?
21) How does it change with catalysts + a line on your graph to represent this?
22)What are reversible reactions?
23)Describe ‘Dynamic equilibrium’.
24)What is a ‘closed system’?
25)What does Le Chatelier’s principle state?
26)What is the effect of concentration on a reaction in equilibrium?
27)What is the effect of temperature on a reaction in equilibrium?
28)What is the effect of pressure on a reaction in equilibrium?
29)What is the effect of a catalyst on a reaction in equilibrium?
30)Using the Harber process as an example, describe how these factors may be controlled in
real life.
