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GCSE Chemistry > GCSE Topics 3 and 4 - Electrolysis and metal extraction > Flashcards

GCSE Topics 3 and 4 - Electrolysis and metal extraction Flashcards

1
Q

Metals that are found native

A

silver, gold and platinum

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2
Q

Metals that are extracted using reduction with carbon

A

zinc, iron, tin, lead, copper

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3
Q

Least reactive metal

A

platinum

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4
Q

Metals that are extracted using electrolysis

A

potassium, sodium, magnesium, calcium, aluminium

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5
Q

Positive electrode

A

Anode

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6
Q

Negative electrode

A

cathode

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7
Q

Symbol equation for aluminium oxide electrolysis

A

Al2O<span>3</span> ⇒ 2 Al + 1.5 O2

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8
Q

Symbol equation for water electrolysis

A

2 H2O (l) ⇒ 2 H2 (g) + O2 (g)

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9
Q

Symbol equation for brine electrolysis

A

2 NaCl (aq) + 2 H2O (l) ⇒ 2 NaOH (aq) + H2 (g) + Cl2 (g)

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10
Q

Symbol equation for the reduction of iron oxide

A

2 Fe2O3 (s) + 3 C (s) ⇒ 4 Fe (s) + 3 CO2 (g)

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11
Q

Anode product of brine electrolysis, name

A

chlorine

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12
Q

Cathode product of brine electrolysis, name

A

hydrogen

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13
Q

Anode product of water electrolysis, name

A

oxygen

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14
Q

Cathode product of water electrolysis, name

A

hydrogen

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15
Q

Anode product of aqueous copper sulfate electrolysis, name

A

oxygen

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16
Q

Cathode product of aqueous copper sulfate electrolysis, name

A

copper

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17
Q

Anode product of hydrochloric acid electrolysis, name

A

chlorine

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18
Q

Cathode product of hydrochloric acid electrolysis, name

A

hydrogen

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19
Q

Anode product of aluminium oxide electrolysis, name

A

oxygen

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20
Q

Cathode product of aluminium oxide electrolysis, name

A

aluminium

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21
Q

Anode product of aqueous copper chloride electrolysis, name

A

chlorine

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22
Q

Cathode product of aqueous copper chloride electrolysis, name

A

copper

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23
Q

Cathode half equation for water electrolysis

A

2 H+ (aq) + 2 e- ⇒ H2 (g)

24
Q

Anode half equation for water electrolysis

A

4 OH- (aq) ⇒ H2O (l) + O2 (g) + 4 e-

25
Q

Cathode half equation for aluminium oxide electrolysis

A

Al3+ + 3 e- ⇒ Al

26
Q

Anode half equation for aluminium oxide electrolysis

A

2 O2- ⇒ O2 + 4 e-

27
Q

Cathode half equation for aqueous copper sulfate electrolysis

A

Cu2+ (aq) + 2 e- ⇒ Cu (s)

28
Q

Anode half equation for aqueous copper sulfate electrolysis

A

4 OH- (aq) ⇒ H2O (l) + O2 (g) + 4 e-

29
Q

Cathode half equation for aqueous copper chloride electrolysis

A

Cu2+ (aq) + 2 e- ⇒ Cu (s)

30
Q

Anode half equation for aqueous copper chloride electrolysis

A

2 Cl- (aq) ⇒ Cl2 (g)

31
Q

Test for hydrogen gas and result

A

Squeeky pop test

Place a lit splint over a test tube. A positive result is a squeeky pop sound.

32
Q

Test for chlorine gas and result

A

Damp blue litmus paper

Place a piece of damp blue litmus paper over a test tube. It will turn red and then be bleached white.

The blue litmus turns red because chlorine reacts with water to produce hydrochloric acid.

33
Q

Test for oxygen gas and result

A

Glowing splint test

Place a glowing splint over a test tube. It relights in the presence of oxygen.

34
Q

Electrolysis definition

A

Decomposition of an electrolyte compound into its elements using electricity from direct current.

35
Q

Cathode product of aqueous sodium sulfate electrolysis, name

36
Q

Anode product of aqueous sodium sulfate electrolysis, name

37
Q

Cathode half equation for aqueous sodium sulfate electrolysis

A

2 H+ (aq) + 2 e- ⇒ H2 (g)

38
Q

Anode half equation for aqueous sodium sulfate electrolysis

A

4 OH- (aq) ⇒ H2O (l) + O2 (g) + 4 e-

39
Q

Cathode product of molten lead bromide electrolysis, name

40
Q

Anode product of molten lead bromide electrolysis, name

41
Q

Substance used to lower the temperature of aluminium oxide electrolysis

42
Q

Conditions for electrolysis of ionic compounds

A

Molten or aqueous

The ions are not free to move in the solid but are free to move in the molten compound or aqueous solution (NOT NOT delocalised electrons).

43
Q

Reduction, in terms of electrons

A

Gain of electrons

44
Q

Oxidation, in terms of electrons

A

Loss of electrons

45
Q

Reaction at the cathode

46
Q

Reaction at the anode

47
Q

Explanation for loss of mass of the anode in aluminium oxide electrolysis

A
  • The anode is made of graphite (carbon)
  • Oxygen gas is produced at the anode
  • Oxygen reacts with the electrode in a combustion reaction
  • Carbon dioxide gas is produced
  • Carbon dioxide escapes
48
Q

Explanation for gain of mass of the cathode in aqueous copper sulfate electrolysis

A
  • Aqueous copper sulfate contains Cu2+ ions
  • The copper ions are reduced
  • A layer of copper atoms are formed on the cathode
  • The half equation for the reaction is
  • Cu2+ (aq) + 2 e- ⇒ Cu (s)
49
Q

Phytomining

or

Phytoextraction

A
  • Extraction of a metal using plants
  • Plants grow on soil with a concentration of metal too low to make a profit from mining
  • Plants concentrate the metal in their sap
  • The plant is burned to leave ash, the energy produced from this may be used to generate electricity
  • The ash is dissolved in water, heated then filtered
  • Electrolysis is used. The metal is produced at the cathode.
50
Q

Explanation of metal reactivity

A
  • Metals are oxidised.
  • Metal atoms lose electrons to become cations.
  • The more reactive a metal is, the more easily oxidised it is.
  • Metals that are resistant to oxidation are less reactive
51
Q

The four ions present in aqueous sodium chloride (brine)

A

Na+ , Cl- , H+ , OH-

52
Q

The three ions present in hydrochloric acid

A

H+ , Cl- OH-

53
Q

The four ions present in aqueous copper chloride

A

H+ , Cu2+ , Cl- , OH-

54
Q

The four ions present in aqueous copper sulfate

A

H+ , OH- , SO42-

55
Q

Copper sulfate solution

56
Q

Diagram of aluminium oxide electrolysis

57
Q

Diagram of aqueous sodium chloride electrolysis

GCSE Chemistry (5 decks)

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