C6 Electrolysis Flashcards

1
Q

why can solid ionic compounds not conduct electricity?

A

the ions are locked in place and are not free to move

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2
Q

why can liquid or dissolved ionic compounds conduct electricity?

A

the forces of attraction between molecules are broken so the ions are free to move

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3
Q

what is an electrolyte?

A

a molten or dissolved ionic compound which can conduct electricity

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4
Q

what are the electrodes in electrolysis made from?

A

a conducting material e.g. graphite

or a metal

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5
Q

what is the negative electrode called?

A

the cathode

it is covered with electrons from the power pack

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6
Q

what is the positive electrode called?

A

the anode

it has a lack of electrons

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7
Q

what happens to positive ions in electrolysis?

A

they are attracted to the cathode.
they gain electrons and become atoms
this is a reduction reaction

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8
Q

what happens to negative ions in electrolysis?

A

they are attracted to the anode
they lose electrons to form atoms
this is an oxidation reaction

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9
Q

which metals are extracted with electrolysis?

A

ones more reactive than carbon

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10
Q

what is aluminium extracted from and how?

A

aluminium oxide

electrolysis

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11
Q

what is aluminium oxide mixed with during electrolysis and why?

A

cryolite

this lowers the melting point of aluminium oxide which reduced the amount of energy needed and saves money

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12
Q

what is the half equation for the electrolysis of aluminium oxide at the cathode?

A

Al3+ + 3e- –> Al

this is a reduction reaction

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13
Q

what is the half equation for the electrolysis of aluminium oxide at the anode?

A

2O2- –> 2O + 4e-
OR
2O2- - 4e- –> 2O
this is an oxidation reaction

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14
Q

why does the anode have to be replaced reguarly?

A

the oxygen molecules produced at the anode react with the graphite (carbon), forming CO2

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15
Q

why is electrolysis expensive?

A

melting the compound requires lots of energy

a lot of energy is required to produce the electric current

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16
Q

what do water molecules ionise to form?

A

hydrogen ions

hydroxide ions

17
Q

what is the rule for the reaction at the cathode?

A

hydrogen is produced at the cathode if the metal is more reactive than hydrogen

18
Q

what is usually made at the anode when electrolysis is being carried out on an aqueous solution?

A

oxygen

19
Q

what metal is often used as electrodes?

A

platinum

it is inert (unreactive) so will not react with the products of the electrolysis

20
Q

what is the half equation for the reaction at the anode in electrolysis with aqueous solutions?

A

4OH- –> O2 + 2H2O + 4e-
OR
4OH- - 4e- –> O2 + 2H2O

21
Q

what is the rule for what is produced at the anode in electrolysis of an aqueous solution?

A

if an aqueous solution contains halide ions, then the halogen will be produced at the anode

22
Q

what is the half equation when hydrogen is produced in electrolysis?

A

2H+ + 2e- –> H2

at the cathode

23
Q

what is the half equation when a halogen is produced? use chlorine as an example

A

2Cl- –> Cl2 + 2e-
OR
2Cl- - 2e- –> Cl2

24
Q

why must the electrodes not touch each other in electrolysis?

A

it would produce a short circuit

25
Q

how can you prove that a gas is chlorine?

A

hold a piece of damp blue litmus paper and it will become bleached

26
Q

what do you get discharged at each electrode when you carry our electrolysis on copper (II) chloride?

A

Copper at the cathode

Chlorine at the anode

27
Q

what is discharged in the electrolysis of sodium chloride?

A

anode - chlorine

cathode - hydrogen