11 questions · 110 marks · ≈ 2 hours
The diagram shows the structure of an atom of an element
Give the name of particle Z.
Give the mass number of this atom.
Give the group number and period number for this element. group number period number
Give a reason why atoms of this element have no overall charge.
Identify this element.
Give the charge on an ion of this element.
This question is about iron and its compounds.
Name the substances needed for iron to rust. 1 2
A student uses this apparatus to react iron with dilute sulfuric acid and to collect the gas produced. hydrogen dilute sulfuric acid water iron
Name a metal that can safely react with dilute sulfuric acid to produce the same volume of hydrogen gas in a shorter time.
Give a test to show that the gas produced is hydrogen.
Which row gives the correct properties of iron(III) oxide? Nature of oxide Structure of oxide
Choose your answer
acidic giant ionic
basic simple molecular
acidic simple molecular
basic giant ionic
A student uses paper chromatography in an experiment to separate the dyes in four different food colourings, A, B, C and D. The diagram shows the appearance of the paper at the start and at the end of the experiment
Describe a method the student should use after putting a spot of each food colouring on the paper.
Describe the composition of food colouring A.
Food colouring D is a mixture of dyes. Suggest how the student could separate the dyes in food colouring D.
Calculate the Rf value of the most soluble dye on the chromatogram. Rf =
This question is about physical changes.
The table gives some physical processes. Complete the table by giving the name of the change for each process. Process Name of change water changes into ice solid iodine changes directly into a vapour sodium chloride crystals stirred in hot water
Explain why hot water evaporates more quickly than cold water.
A student is given a pure solid and an impure solid. Describe how the student can identify which solid is pure and which solid is impure by measuring a physical property.
This question is about gases.
The box lists the names of some gases. argon carbon dioxide ethene methane nitrogen sulfur dioxide The table gives some statements about gases. Complete the table by giving the correct gas from the box for each statement. Statement Gas a gas that is about 1% by volume of air a gas that is the product of the complete combustion of a hydrocarbon a gas that can be used to make a polymer a gas that occurs as diatomic molecules
A scientist analyses a sample of gases from the Moon. The sample is a mixture of the gases helium, hydrogen and neon. The scientist uses this apparatus to determine the percentage by volume of hydrogen in the mixture. gas syringe copper(II) oxide powder gas syringe mixture of gases electric heater from the Moon This is the scientist’s method.
Give a reason why helium and neon are unreactive.
Give a reason why the scientist allows the remaining gases to cool before recording the volume.
Give a reason why the scientist uses an electric heater rather than a Bunsen burner.
At the start of the experiment, the initial volume of gas in the apparatus is 157.0 cm³ At the end of the experiment, the final volume of gas is 106.7 cm³ Calculate the percentage by volume of hydrogen in the mixture of gases. Give your answer to one decimal place. percentage = %
Explain why the reaction between copper(II) oxide and hydrogen is a redox reaction.
This question is about ionic compounds.
The table gives the formulae of some positive ions, some negative ions, and some compounds containing these ions
Complete the table by giving the three missing formulae.
Give the name of the compound with the formula NH₄NO₃
Calculate the mass, in grams, of nitrogen in 100 g of NH₄NO₃ [for N Ar = 14] [for NH₄NO₃ Mr = 80] mass = g
Magnesium chloride (MgCl₂) is an ionic compound. The magnesium ions and chloride ions are held together by ionic bonding.
State the meaning of the term ionic bonding.
Magnesium chloride forms when magnesium reacts with chlorine. The diagram shows the arrangement of electrons in a magnesium atom and in a chlorine atom. magnesium atom chlorine atom Describe, in terms of electrons, what happens when magnesium chloride forms.
Describe a test to show that magnesium chloride contains chloride ions.
The table shows the student's results.
| Time in minutes | Volume of gas in cm3 |
|---|---|
| 0 | 0 |
| 1 | 16 |
| 2 | 18 |
| 3 | 30 |
| 4 | 36 |
| 5 | 40 |
| 6 | 40 |
| 7 | 40 |
| 8 | 40 |
Plot the student’s results on the grid.
Draw a curve of best fit, ignoring the anomalous result. Volume of gas in cm³ 1 2 3 4 5 6 7 8 Time in minutes
Suggest a mistake the student could have made to cause the anomalous result.
Draw a tangent to the curve at 4 minutes.
Use the tangent to determine the rate of reaction at 4 minutes. Include a unit in your answer. rate = unit =
Explain why the last four readings for the volume of gas are the same.
The table shows the displayed formulae of six organic compounds
Use the letters A to F to answer these questions. You may use each letter once, more than once, or not at all.
Give the letter of the compound that is not a hydrocarbon.
Give the letter of the compound that will decolourise bromine water.
Give the letter of the saturated compound with the empirical formula CH₂
Give the letter of the compound that has the same molecular formula as butane.
This equation represents a reaction that occurs during cracking. C₁₂H₂₆ → C₈H₁₈ + 2C₂H₄
Give the temperature and the catalyst needed for cracking. temperature catalyst
Explain why cracking is a useful process. Refer to the products of the reaction in your answer.
Complete the equation for the polymerisation of compound B.
This question is about copper and copper compounds.
A sample of copper contains two isotopes. • Cu with relative abundance 62.5% • Cu with relative abundance 37.5% Calculate the relative atomic mass (Ar) of copper in the sample. Ar =
Copper can be produced by reacting copper(II) sulfate solution with a metal, M. M is not the symbol for the metal. This is the equation for the reaction. M + CuSO₄ → MSO₄ + Cu
100.00 g of M produces 158.75 g of copper when reacted with an excess of copper(II) sulfate solution. Calculate the relative atomic mass (Ar ) of M. [for Cu Ar = 63.5] Ar =
Use the Periodic Table to identify M.
This is the ionic equation for the reaction between copper(II) sulfate and M. Cu²⁺ + M → Cu + M2+ Explain, in terms of electrons, which species is the reducing agent.
Copper can also be produced by reacting copper(II) oxide with carbon. This is the equation for the reaction. 2CuO + C → 2Cu + CO₂ A mixture of 10 000 mol of copper(II) oxide is heated with 70 kg of carbon. Show, by calculation, that carbon is in excess. [for C Ar = 12]
This question is about zinc sulfate.
Soluble salts such as zinc sulfate can be prepared by the reaction between a metal oxide and an acid. This is the word equation for the reaction. zinc oxide + sulfuric acid → zinc sulfate + water
State the name of this type of reaction.
State, in terms of protons, what happens in this reaction.
A student is given 50 cm³ of dilute sulfuric acid and some zinc carbonate powder. Describe a method the student should use to prepare dry crystals of hydrated zinc sulfate.
The student uses this apparatus to find the value of x in the formula ZnSO₄•xH₂O hydrated zinc sulfate heat When heated, the hydrated solid decomposes completely. This is the equation for the reaction. ZnSO₄•xH₂O → ZnSO₄ + xH₂O The table shows the student’s results. mass of empty tube in g 24.82 mass of tube + ZnSO₄•xH₂O in g 39.17 mass of tube + ZnSO₄ in g 32.87 Show that the value of x is 7. [for ZnSO₄ Mr = 161] [for H₂O Mr = 18]
Zinc sulfate solution reacts with ammonium hydroxide solution to form the insoluble solid, zinc hydroxide. This is the equation for the reaction. ZnSO₄(aq) + 2NH₄OH(aq) → Zn(OH)₂(s) + (NH₄)₂SO₄(aq)
A student reacts a solution containing 0.250 mol of ammonium hydroxide with an excess of zinc sulfate. The reaction produces 11.3 g of zinc hydroxide. Calculate the percentage yield of zinc hydroxide in this reaction. [for Zn(OH)₂ Mr = 99] percentage yield = %
The student repeats the experiment and correctly calculates a percentage yield of 107%. Suggest why this percentage yield is greater than 100%.
This question is about carbon. The table shows the structures of three different forms of carbon
Give the reason why these forms of carbon are elements.
Explain, in terms of its structure, why graphite can act as a lubricant.
Explain why diamond has a much higher boiling point than C₆₀ fullerene. Refer to structure and bonding in your answer.
Calculate the mass, in g, of one molecule of C₆₀ fullerene. Give your answer in standard form. [one mole contains 6.02 × 10²³ particles] [for C Ar = 12] mass = g