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General F004: Metals and redox reactions

  • Page ID
    63675
  • These questions focus on metals and their redox chemistry. You may wish to review the notes on this topic before taking the quiz.

    The following questions may be multiple answer or "fill in the blank". For multiple answer choose all answers which you think are most appropriate - though it may be that only one answer is correct. These questions are for self-testing only, and are not suitable for assignments or exams.

    1. Which of the following metals could be used to reduce lead(II) oxide to lead metal?

    Aluminium
    Copper
    Magnesium
    Silver
    Zinc

    2. Which of the following tests indicates that an oxidizing agent is present?

    litmus paper turns blue
    litmus paper turns red
    acidified potassium dichromate(VI) solution turns green
    alkaline potassium dichromate(VI) solution turns blue
    acidified potassium iodide solution turns brown

    3. Which of the following is/are true statements about the reaction of heated zinc with oxygen to produce zinc oxide?

    The zinc is oxidised.
    Oxygen is an oxidising agent.
    The zinc is reduced.
    There is a net flow of electrons from zinc to the oxygen
    There is a net flow of electrons from oxygen to zinc.

    4. Balance the following redox equation. Enter "1" if only one unit of the substance is needed - do not leave any number blank.

    Na + Al2O3Na2O + Al

    5. Balance the following redox equation. Enter "1" if only one unit of the substance is needed - do not leave any number blank.

    Mg(s) + CuSO4(aq) → MgSO4(aq) + Cu(s)

    6. Balance the following redox equation. Enter "1" if only one unit of the substance is needed - do not leave any number blank.

    Zn(s) + AgNO3(aq) → Zn(NO3)2(aq) + Ag(s)

    7. Balance the following redox equation. Enter "1" if only one unit of the substance is needed - do not leave any number blank, and do not use fractional numbers.

    Na(s) + H2O(l) → NaOH(aq) + H2(g)

    8. Indicate all the reactions where lead(IV) oxide is reduced.

    PbO2 + 4HF → PbF4 + 2H2O
    PbO2 + Cu → PbO + CuO
    PbO2 + 2H2 → Pb + 2H2O
    PbO2 + 2C → Pb + 2CO
    PbO2 + 2Mg → Pb + 2MgO

    9. Indicate all of the equations that represent redox reactions.

    2Mg + O2 → 2MgO
    MgO + 2HCl → MgCl2 + H2O
    PbO + H2 → Pb + 2H2O
    PbCl2 + 2Na2SO4 → PbSO4 + 2NaCl
    2AgNO3 + 2MgCl2 → 2AgCl + 2Mg(NO3)2

    Answers:

    1. A, C, E

    2. E

    3. A, B, D

    4. 6, 1, 3, 2

    5. 1, 1, 1, 1

    6. 1, 2, 1, 2

    7. 2, 2, 2, 2

    8. B, C, D, E

    9. A, C