10 questions · 110 marks · ≈ 2 hours
The diagram shows how particles are arranged in the three states of matter
Give the names of the changes of state labelled X, Y and Z. X Y Z
Water vapour condenses to form water. Give the equation for this change of state. Include the state symbols.
Describe how particles are arranged differently in solids and gases.
The box shows the names of some gases in the atmosphere.
argon · carbon dioxide · nitrogen · oxygen · water vapour
Choose gases from the box to answer these questions.
Identify the gas with a molecule that contains a triple bond.
Identify the gas in the atmosphere that exists as individual atoms.
Identify the gas needed for combustion reactions.
Explain how carbon dioxide can be formed from copper(II) carbonate.
A student uses this apparatus to calculate the percentage of oxygen in a sample of air. wet iron wool column of air water This is the student’s method.
Use the student’s results to calculate the percentage of oxygen in the sample of air. percentage = %
The percentage of oxygen in air is approximately 21%. Suggest an improvement to the method that would increase the accuracy of the student’s results.
This question is about atomic structure and the Periodic Table.
The diagram shows an atom of an element. X – + ++ – – – – + + Y W Z Use the diagram to answer these questions.
Which particle is a proton?
Choose your answer
W
X
Y
Z
Which particle has a relative charge of 0?
Choose your answer
W
X
Y
Z
Name the part of the atom labelled Z.
What is the group number of this element?
Choose your answer
2
3
5
11
What is the period number of this element?
Choose your answer
2
3
5
11
Give the chemical symbol of this element.
State what type of particle is formed when an atom loses its outer shell electrons.
The table shows the atomic number and the relative atomic mass (to 1 decimal place) of the elements in a period of the Periodic Table. Element Li Be B C N O F Ne Atomic number 3 4 5 6 7 8 9 10 Relative atomic mass 6.9 9.0 10.8 12.0 14.0 16.0 19.0 20.2
On the grid, add an appropriate scale to the y-axis, starting at 6.0
Plot the data on the grid. Do not join the points. Relative atomic mass 6.0 3 4 5 6 7 8 9 10 Atomic number
Identify the relationship between relative atomic mass and atomic number for the elements in this period.
This question is about ammonium chloride.
Draw a diagram to show the arrangement of the electrons in a chloride ion.
Two beakers are unlabelled. One beaker contains a solution of ammonium chloride and the other beaker contains a solution of ammonium sulfate. Describe tests that can be carried out to confirm that one beaker contains ammonium chloride and the other beaker contains ammonium sulfate.
A student draws a diagram to show the formation of solid ammonium chloride in a glass tube. cotton wool soaked cotton wool soaked in concentrated ammonium in concentrated ammonia solution chloride hydrochloric acid
Explain the mistake in the student’s diagram.
Complete the equation for the reaction in the glass tube by adding state symbols. NH₃ ( ) + HCl ( ) NH₄Cl ( )
This question is about displacement reactions. A student uses this method to investigate what happens when excess metal is added to a solution of copper(II) sulfate.
Give a reason why the student could not use copper(II) carbonate instead of copper(II) sulfate.
Explain why a polystyrene cup is used instead of a glass beaker.
Give two variables the student should control in the investigation. 1 2
The table shows the student’s results. Temperature increase in °C Mean temperature Metal increase in °C experiment 1 experiment 2 experiment 3 W 4.0 2.0 4.2 4.1 X 0.0 0.0 0.0 0.0 Y 6.1 6.3 6.0 Z 8.1 8.5 8.9 8.5
Calculate the mean temperature increase for metal Y. Give your answer to two significant figures. mean temperature increase = °C
Explain whether the anomalous result in experiment 2 could have been caused by stirring the mixture too quickly.
Explain the order of reactivity for metals W, X, Y and Z.
Explain why metal X could be silver.
Crude oil can be used to make useful products. Two of the processes used are shown.
Give the name of process 1.
Sketch a labelled diagram showing how the kerosene fraction is obtained from crude oil in process 1.
Give the two conditions needed for a reaction to occur in process 2. 1 2
Complete the equation for the reaction in process 2. C₁₄H₃₀ → +
Explain one use of octane as fuel.
Using displayed formulae, give the equation for the conversion of ethene into poly(ethene).
Give the term used to describe ethene in the polymerisation process.
A student uses this method to investigate the reaction between sodium hydroxide solution and dilute nitric acid. Step 1 pour 20 cm³ of dilute nitric acid into a 100 cm³ glass beaker Step 2 measure the temperature of the acid Step 3 add 5 cm³ of sodium hydroxide solution and stir the mixture Step 4 record the highest temperature reached The student repeats steps 3 and 4 until a total of 40 cm³ of sodium hydroxide solution has been added.
The graph shows the student’s results. Temperature change in C 0 5 10 15 20 25 30 35 40 Volume of sodium hydroxide solution in cm³
Determine the volume of sodium hydroxide solution at the point where the lines cross. volume = cm³
Determine the maximum temperature change reached during the investigation. maximum temperature change = °C
The student makes this statement about the shape of the graph. The first line on the graph shows that the temperature rises at a steady rate as more nitric acid is added and at 40 cm³, the acid has been neutralised by the sodium hydroxide. The student’s statement includes some mistakes and is incomplete.
Give two mistakes in the student’s statement. 1 2
Add another sentence to complete the student’s statement.
The student repeats the investigation. The student starts with 25 cm³ of dilute nitric acid at 19 °C. The student finds that 25 cm³ of sodium hydroxide solution is needed for complete neutralisation. The student calculates that the heat energy (Q) released is 3780 J. [for the solution, c = 4.2 J / g / °C] [mass for 1.0 cm³ of solution = 1.0 g]
Calculate the maximum temperature reached. maximum temperature = °C
The amount of dilute nitric acid used in the investigation was 0.079 mol. Calculate the value of ΔH, in kJ / mol, for the neutralisation reaction. Include a sign in your answer. ΔH = kJ / mol
This question is about ionic compounds.
The table shows the formulae of some ions. It also shows the formulae of some compounds containing these ions. Complete the table by giving the missing information. Ions Li+ Mg²⁺ Al³⁺ NO₃⁻ LiNO₃ Al(NO₃)₃ SO₄²⁻ MgSO₄ Al₂(SO₄)₃ PO₄³⁻ Li₃PO₄ Mg₃(PO₄)₂
Explain why magnesium oxide has a higher melting point than sodium chloride. Refer to structure and bonding in your answer.
This question is about propene and propane.
Complete the table by giving the missing information about propene. Displayed formula of propene Molecular formula of propene C₃H₆ Empirical formula of propene Relative formula mass of propene
Draw a dot-and-cross diagram for propane. Include only outer shell electrons.
Propene and propane react with bromine.
Which row shows the correct number of products for these reactions? Propene and bromine Propane and bromine
Choose your answer
1 1
1 2
2 1
2 2
Give the reaction condition needed for propane and bromine to react together.
A compound formed in the reaction between bromine water and an alkene has this percentage composition by mass. C = 25.9% H = 5.0% O = 11.5% Br = 57.6% Calculate the empirical formula of this compound. empirical formula =
Ethene and propene contain the same functional group.
State what is meant by the term functional group.
Draw an isomer of propene that does not have the same functional group.
This question is about aluminium sulfate. Aluminium reacts with sulfuric acid to form aluminium sulfate. This is the equation for the reaction. 2Al + 3H₂SO₄ → Al₂(SO₄)₃ + 3H₂
What is the total number of elements in the formula Al₂(SO₄)₃ ?
Choose your answer
3
5
14
17
A student uses this method to prepare some aluminium sulfate crystals. Step 1 add powdered aluminium to a beaker of dilute sulfuric acid and stir Step 2 keep stirring and adding powdered aluminium until it is in excess Step 3 filter the reaction mixture Step 4 heat the filtrate to evaporate some water and produce a saturated solution Step 5 allow the saturated solution to cool so that crystals form Step 6 filter to obtain the crystals and leave to dry
During step 3, the reaction mixture is filtered. Identify the substance that remains in the filter paper and the substances in the beaker after this filtration. filter paper beaker
State why the aluminium is added until it is in excess.
Explain why powdered aluminium is used.
The student adds 3.20 g of aluminium to 0.120 mol of dilute sulfuric acid.
Show that sulfuric acid is not in excess.
The student calculates the percentage yield of aluminium sulfate obtained from 0.120 mol of sulfuric acid as 113%. Calculate the mass, in grams, of aluminium sulfate produced if the yield is 113%. mass = g
Suggest a mistake the student made when carrying out the method that caused the percentage yield to be greater than 100%.