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AQA GCSE Chemistry Revision > Reactions of metals > Flashcards

Reactions of metals Flashcards

1
Q

Recite the reactivity series from most to least reactive metal.

Include carbon and hydrogen for reference.

A
  • Potassium
  • Sodium
  • Lithium
  • Calcium
  • Magnesium
  • Carbon
  • Zinc
  • Iron
  • Hydrogen
  • Copper
  • Gold
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2
Q

State the general word equation for the reaction of a metal with water.

A

metal + water → metal hydroxide + hydrogen

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3
Q

sodium + water →

A

sodium hydroxide + hydrogen

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4
Q

State the general word equation for the reaction between a metal and an acid.

A

metal + acid → salt + hydrogen

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5
Q

Which salt is made when magnesium reacts with hydrochloric acid?

A

magnesium chloride

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6
Q

copper + sulfuric acid →

A

copper sulfate + hydrogen

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7
Q

State the general word equation for the reaction between a metal and oxygen.

A

metal + oxygen → metal oxide

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8
Q

magnesium + oxygen →

A

magnesium oxide

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9
Q

2Mg + O2 → 2MgO

Why is this reaction described as oxidation?

A

Because magnesium gains oxygen

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10
Q

2CuO(s) + C(s) → 2Cu(l) + CO2(g)

In this reaction, which element is oxidised?

A

Carbon

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11
Q

2CuO(s) + C(s) → 2Cu(l) + CO2(g)

In this reaction, which element is reduced?

A

Copper

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12
Q

What is reduction?

A

The loss of oxygen in a chemical reaction

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13
Q

Describe what happens in a displacement reaction.

A

A more reactive metal displaces a less reactive metal from its compound

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14
Q

Magnesium + copper sulfate → magnesium sulfate + copper

What kind of chemical reaction is this?

A

Displacement

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15
Q

iron + copper sulfate →

A

iron sulfate + copper

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16
Q

Why is there no reaction when copper is added to magnesium sulfate?

A

Because copper is less reactive than magnesium (so copper cannot displace magnesium)

17
Q

Mg(s) + CuSO4(aq) → MgSO4(aq) + Cu(s)

What is the half equation for the oxidation of magnesium?

A

Mg(s) → Mg2+(aq) + 2e-

18
Q

Mg(s) + CuSO4(aq) → MgSO4(aq) + Cu(s)

What is the half equation for the reduction of copper?

A

Cu2+(aq) + 2e- → Cu(s)

19
Q

What is oxidation in terms of electrons?

A

Oxidation is the loss of electrons

20
Q

What is reduction in terms of electrons?

A

Reduction is the gain of electrons

21
Q

What is a redox reaction?

A

When reduction and oxidation take place at the same time.

22
Q

What does OIL RIG stand for?

A

Oxidation

Is

Loss (of electrons)

Reduction

Is

Gain (of electrons)

23
Q

What is an ore?

A

A rock containing enough quantities of a mineral for extraction to be possible

24
Q

What is a disadvantage of using electrolysis to extract a metal?

A

Large amounts of electrical energy are needed, so electrolysis is expensive

25
Q

Which metals can be extracted using carbon?

A
  • Zinc
  • Iron
  • Copper
26
Q

Describe how copper is extracted from its ore using carbon.

A

Copper oxide is heated with carbon to form copper and carbon dioxide.

27
Q

Copper oxide + carbon → copper + carbon dioxide

Which element is oxidised and which element is reduced when copper is extracted using carbon?

A
  • Carbon is oxidised
  • Copper is reduced
28
Q

Iron(III) oxide is reduced to molten iron when it reacts with carbon.

What is the word equation for this reaction?

A

iron(III) oxide + carbon → iron + carbon monoxide

29
Q

Why must aluminium be extracted from its compound using electrolysis, not heating with carbon?

A

Because aluminium is more reactive than carbon (so carbon cannot displace aluminium from its compounds)

30
Q

Why is aluminium more expensive than iron?

A

Because of the large amounts of electrical energy used in the extraction process (electrolysis).

31
Q

What are two ways that aluminium oxide can be made into an electrolyte?

A
  • It is melted (very expensive)
  • Powdered aluminium oxide is dissolved in molten cryolite (less expensive)
32
Q

Why is the electrolysis of aluminium oxide so expensive?

A
  • Aluminium oxide has a very high melting point
  • A lot of energy is required to break its ionic bonds
33
Q

What is formed at the cathode during the electrolysis of aluminium oxide? How does this product form?

A

At the cathode, aluminium ions gain electrons and form aluminium atoms

34
Q

What is formed at the anode in the electrolysis of aluminium oxide? How is this product formed?

A

At the anode, oxide ions lose electrons and form oxygen gas

35
Q

Oxygen is produced at the anode in the electrolysis of aluminium chloride.

What is the half equation for the reaction at the anode?

A

2O2- → O2 + 4e-

36
Q

Aluminium is produced at the cathode in the electrolysis of aluminium oxide.

What is the half equation for this reaction?

A

Al3+ + 3e- → Al

AQA GCSE Chemistry Revision (13 decks)

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