10 questions · 110 marks · ≈ 2 hours
The diagram represents an atom of an element.
Label the three subatomic particles on the diagram.
Use information from the diagram to complete the table for this element. mass number group number period number electronic configuration
Give the name of this element.
A small piece of lithium is added to a trough of water.
State two observations made when lithium reacts with water. 1 2
What are the products of the reaction?
Choose your answer
lithium hydroxide and hydrogen
lithium hydroxide and oxygen
lithium oxide and hydrogen
lithium oxide and oxygen
After the reaction is complete, a few drops of universal indicator are added to the solution in the trough.
Explain the colour and pH of the solution in the trough.
Give the formula of the ion responsible for this pH.
Lithium ions can be identified using a flame test. What flame colour indicates the presence of lithium ions?
Choose your answer
lilac
orange
red
yellow
A student uses paper chromatography to investigate the dyes in five different inks, V, W, X, Y and Z. The chromatogram shows the results of the investigation
Explain why the start line on the paper is drawn in pencil rather than in ink.
Explain which two inks contain the dye that is most soluble in the solvent.
Explain how the chromatogram shows that • W contains only one dye • V may contain more than one dye
Calculate the Rf value for the dye in W. Give your answer to two significant figures. Rf value =
Calcium phosphate is an ionic compound with the formula Ca₃(PO₄)₂
What is the total number of atoms in the formula Ca₃(PO₄)₂?
Choose your answer
8
11
13
19
What are the correct charges on the ions in calcium phosphate?
Choose your answer
Ca²⁺ and PO₄²⁻
Ca²⁺ and PO₄³⁻
Ca³⁺ and PO₄²⁻
Ca³⁺ and PO₄³⁻
Calculate the relative formula mass (Mr) of Ca₃(PO₄)₂ Mr of Ca₃(PO₄)₂ =
Calculate the percentage by mass of calcium in calcium phosphate. percentage = %
Calcium hydroxide can react with phosphoric acid to form calcium phosphate. Complete the equation for this reaction Ca(OH)₂ + H₃PO₄ → Ca₃(PO₄)₂ + H₂O
Butane (C₄H₁₀) is an alkane.
Explain why butane is a saturated hydrocarbon.
When butane burns completely in oxygen, carbon dioxide and water are produced. Give a chemical equation for this combustion reaction.
Incomplete combustion can occur when the oxygen supply is limited. One product of the incomplete combustion of butane is carbon monoxide. Give the name of another product of this incomplete combustion.
State why carbon monoxide is poisonous to humans.
C₄H₁₀ exists as two isomers.
State what is meant by the term isomers.
Draw the displayed formula of each isomer.
Explain why hexane (C₆H₁₄) has a higher boiling point than butane (C₄H₁₀).
When iron rusts, iron(III) oxide forms. State two conditions needed for iron to rust. 1 2
What is the name of the process used to coat iron with zinc?
Choose your answer
galvanisation
oxidation
reduction
sacrificial protection
What is the correct order of reactivity of these four metals? most reactive least reactive
Choose your answer
aluminium copper iron zinc
aluminium iron zinc copper
aluminium zinc iron copper
zinc aluminium iron copper
Describe a test to show that a solution contains Fe³⁺ ions. test result
A sample of iron(III) oxide reacts with excess carbon monoxide. This is the equation for the reaction. Fe₂O₃ + 3CO → 2Fe + 3CO₂
Explain why this is a redox reaction.
Calculate the minimum mass of iron(III) oxide needed to produce a theoretical yield of 28 g of iron. [for Fe₂O₃ Mr = 160] minimum mass of iron(III) oxide = g
The actual yield of iron from this sample is 21 g. Calculate the percentage yield of iron. percentage yield = %
A student does an experiment to determine the maximum temperature change when sulfuric acid reacts with sodium hydroxide.
Complete the chemical equation for this neutralisation reaction. Include the state symbols. 2NaOH(aq) + H₂SO₄(aq) → +
This is the student’s method. Step 1 add 50 cm³ of sodium hydroxide solution to a glass beaker Step 2 record the initial temperature of the sodium hydroxide solution Step 3 add 5 cm³ of dilute sulfuric acid to the beaker Step 4 stir the mixture and record the highest temperature reached The student repeats steps 3 and 4 until a total of 40 cm³ of acid has been added. Explain one way the student could improve the accuracy of the experiment.
The table shows the student’s results. Total volume of acid 0 5 10 15 20 25 30 35 40 in cm³ Temperature of mixture 21.0 22.3 23.8 24.4 26.5 28.0 28.5 28.2 27.9 in °C
Plot the results on the grid.
Draw a circle around the anomalous result.
Draw a straight line of best fit through the first six points, ignoring the anomalous result. Draw another straight line of best fit through the last three points. Make sure that the two lines cross. 30.0 Temperature in C 25.0 20.0 0.0 10.0 20.0 30.0 40.0 Volume of sulfuric acid in cm³
The point where the lines cross shows the volume of acid needed to exactly neutralise the alkali and the maximum temperature reached. Use your graph to determine these values. volume of acid = cm³ maximum temperature = °C
Explain what might have caused the anomalous result.
Diamond and graphite are two naturally‑occurring forms of carbon. They both have giant covalent structures
Explain, with reference to its bonding, why diamond has a high melting point.
Explain why graphite is soft and is a conductor of electricity. Refer to structure and bonding in your answer.
This question is about organic compounds.
Chloroethene (C₂H₃Cl) is a covalent molecule that is used to make poly(chloroethene). This is the displayed formula of chloroethene
Draw a dot‑and‑cross diagram of chloroethene. Show only the outer shell electrons.
Describe, in terms of electrostatic attraction, what is meant by a covalent bond.
Chloroethene is a monomer. Draw the displayed formula of the repeat unit of poly(chloroethene).
Poly(chloroethene) is non‑biodegradable. There are two main methods used to dispose of poly(chloroethene). Describe one problem caused by each method. 1 2
An organic compound contains this percentage composition by mass. C = 22.0% H = 4.6% Br = 73.4% Calculate the empirical formula of this compound. empirical formula =
Ethane and ethene undergo different types of reaction with bromine. Describe the differences between these two reactions.
A student uses this apparatus to investigate the energy content of different fuels
This is the student’s method. • pour some water into the copper can • record the mass of the spirit burner and fuel • measure the initial temperature of the water • place the spirit burner under the copper can and light the burner • stop heating the water when the temperature reaches 30°C • record the new mass of the spirit burner and fuel The student repeats the experiment with different fuels. Explain two variables the student should control to make this a valid test. 1 2
In one of the experiments, the student uses ethanol as the fuel. These are the student’s results for ethanol. initial mass of spirit burner and ethanol in g 38.52 final mass of spirit burner and ethanol in g 38.29 volume of water in cm³ 100 initial temperature of water in °C 18 final temperature of water in °C 30
Calculate the value of heat energy change (Q) in joules. [for water, c = 4.2 J/g/°C 1.0 cm³ of water has mass = 1.0 g] Q = J
Calculate the enthalpy change (ΔH) in kJ/mol. [for ethanol, Mr = 46] Include a sign in your answer. ΔH = kJ/mol