Paper 1-style (Foundation)
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Paper 1-style practice paper: Foundation — question paper

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GCSE (9–1) · GCSE Chemistry (Foundation)

Paper 1-style practice paper

Foundation

Duration: 105 minutes
Total: 100 marks
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Class:
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Date:

READ THESE INSTRUCTIONS FIRST

  • Answer all questions.
  • Section A contains ten multiple-choice questions. Choose one answer, A, B, C or D, for each.
  • Section B contains structured questions. Write your answers in the spaces provided.
  • You may use a calculator. Values of relative formula mass (Mr) are given where needed.
  • The number of marks is given in brackets [ ] at the end of each question or part question.
  • The total mark for this paper is 100.

Original practice material written for the MOE GCSE Chemistry syllabus. It is not an official MOE or school examination paper. Foundation content of chapters 1–11: atomic structure and the periodic table, states of matter and separation, bonding, allotropes of carbon, formulae and conservation of mass, the mole, acids and salts, titration and concentration, reactivity and extraction, electrolysis, energy changes.

For Examiner’s Use
Section A/ 10
Section B/ 90
Total/ 100

Section A: Multiple-choice questions[10 marks]

Choose one answer for each question. Each question is worth 1 mark.

  1. 1

    The relative charge of a proton is

    1. A0
    2. B−1
    3. C+2
    4. D+1
    ( )
  2. 2

    The element with electronic structure 2,8,1 is

    1. Aoxygen
    2. Bsodium
    3. Cchlorine
    4. Dhelium
    ( )
  3. 3

    Which of these is a compound?

    1. AO₂
    2. BN₂
    3. CCO₂
    4. DAr
    ( )
  4. 4

    A typical property of ionic compounds is

    1. Alow melting point
    2. Bconduction as solids
    3. Chigh melting point
    4. Dsoftness
    ( )
  5. 5

    Which substance conducts electricity as a solid?

    1. Agraphite
    2. Bsodium chloride
    3. Cwater
    4. Dsulfur
    ( )
  6. 6

    The formula of calcium chloride is

    1. ACaCl
    2. BCaCl₂
    3. CCa₂Cl
    4. DCa₂Cl₃
    ( )
  7. 7

    The pH of a strong acid solution is closest to

    1. A7
    2. B10
    3. C1
    4. D14
    ( )
  8. 8

    During electrolysis of molten sodium chloride, the product at the cathode is

    1. Achlorine
    2. Bhydrogen
    3. Coxygen
    4. Dsodium
    ( )
  9. 9

    In an exothermic reaction, the temperature of the surroundings

    1. Arises
    2. Bfalls
    3. Cstays the same
    4. Ddoubles
    ( )
  10. 10

    The state symbol (s) shows a substance is

    1. Aa solution
    2. Ba solid
    3. Csoluble
    4. Dstable
    ( )

Section B: Structured questions[90 marks]

Answer all questions in the spaces provided.

  1. 11

    This question is about atoms.

    1. (a)

      A lithium atom has atomic number 3 and mass number 7. State the numbers of protons, neutrons and electrons in the atom.

      [3]
    2. (b)

      Explain why atoms have no overall charge.

      [1]
    3. (c)

      Write the electronic structure of a lithium atom.

      [1]
    4. (d)

      Describe what isotopes of an element have in common and how they differ.

      [2]
  2. 12

    This question is about Groups 1, 7 and 0 of the periodic table.

    1. (a)

      Write the balanced equation for sodium reacting with water.

      [2]
    2. (b)

      State how the reactivity of Group 1 metals changes down the group.

      [1]
    3. (c)

      Chlorine is bubbled into potassium bromide solution. Write the equation for the displacement reaction.

      [2]
    4. (d)

      Explain why the Group 0 gases are unreactive.

      [2]
    5. (e)

      State one typical property of transition metals.

      [1]
  3. 13

    This question is about mixtures and separation.

    1. (a)

      State what filtration separates.

      [1]
    2. (b)

      Describe how simple distillation works.

      [2]
    3. (c)

      In a chromatogram, dye P travels further than dye Q. State which dye is more attracted to the solvent.

      [1]
    4. (d)

      A spot moves 4.5 cm while the solvent front moves 6.0 cm. Calculate the Rf value.

      [2]
    5. (e)

      State what is meant by a formulation.

      [1]
  4. 14

    This question is about bonding.

    1. (a)

      Describe what happens when sodium reacts with chlorine to form sodium chloride.

      [3]
    2. (b)

      Explain why sodium chloride has a high melting point.

      [2]
    3. (c)

      State what a covalent bond is.

      [1]
    4. (d)

      Explain why metals conduct electricity.

      [2]
  5. 15

    This question is about the allotropes of carbon.

    1. (a)

      Explain why diamond is very hard and has a very high melting point.

      [3]
    2. (b)

      Explain why graphite conducts electricity but diamond does not.

      [3]
    3. (c)

      State one property of graphene and one use it is being developed for.

      [2]
  6. 16

    This question is about formulae and equations. (Mr: CaCO₃ = 100, CaO = 56, CO₂ = 44)

    1. (a)

      Balance the equation: Mg + O₂ → MgO.

      [2]
    2. (b)

      State the law this demonstrates about mass in reactions.

      [1]
    3. (c)

      Calculate the relative formula mass (Mr) of CaCO₃.

      [2]
    4. (d)

      100 g of calcium carbonate decomposes completely. Calculate the mass of carbon dioxide released.

      [3]
    5. (e)

      State what the state symbol (aq) means.

      [1]
    6. (f)

      Name the type of reaction in (d).

      [1]
  7. 17

    This question is about the mole. (Ar: Mg = 24, C = 12, O = 16)

    1. (a)

      Calculate the number of moles in 24 g of magnesium.

      [2]
    2. (b)

      Calculate the mass of 0.25 mol of carbon dioxide (Mr = 44).

      [2]
    3. (c)

      12 g of magnesium burns completely in oxygen to form magnesium oxide (Mr = 40). Calculate the mass of magnesium oxide formed.

      [4]
    4. (d)

      State the value of the Avogadro constant.

      [1]
    5. (e)

      Explain what one mole of a substance represents.

      [2]
  8. 18

    This question is about acids and salts.

    1. (a)

      Name the salt formed when hydrochloric acid neutralises sodium hydroxide.

      [1]
    2. (b)

      Write the balanced equation for this neutralisation.

      [2]
    3. (c)

      Describe how to make pure, dry crystals of copper sulfate from insoluble copper oxide and dilute sulfuric acid.

      [4]
    4. (d)

      State the pH of a dilute strong acid.

      [1]
    5. (e)

      State what is formed when an acid reacts with a carbonate.

      [1]
  9. 19

    This question is about titration and concentration.

    1. (a)

      Name the piece of apparatus used to add acid accurately during a titration.

      [1]
    2. (b)

      Name a suitable indicator for a titration and explain why universal indicator is not used.

      [2]
    3. (c)

      25 g of sodium hydroxide is dissolved in water to make 500 cm³ of solution. Calculate the concentration in g/dm³.

      [3]
    4. (d)

      State why titrations are repeated.

      [2]
    5. (e)

      State the reading precision expected from a burette.

      [2]
  10. 20

    This question is about reactivity, electrolysis and energy changes.

    1. (a)

      Metal P displaces metal Q from solution. Metal R displaces metal P. Place P, Q and R in order of reactivity, most reactive first.

      [2]
    2. (b)

      Write the balanced equation for the reduction of iron(III) oxide with carbon in the blast furnace.

      [2]
    3. (c)

      Name the products of electrolysis of molten sodium chloride at the cathode and anode.

      [2]
    4. (d)

      A reaction makes the temperature of the surroundings rise. State whether it is exothermic or endothermic and give one everyday example.

      [2]
    5. (e)

      Explain why electrolysis would not work if the sodium chloride were solid instead of molten.

      [2]
    6. (f)

      State the meaning of the term activation energy.

      [2]

— End of paper —