C3.4

Question 1

Electrolyte

Answer 1

Solution that contains an ionic compound (where ions are free to move)

Question 2

What would you do if u had an insoluble substance for electrolysis?

Answer 2

Melt it into molten liquid to allow ions to be free to move

Question 3

Why are electrodes made of

Answer 3

They are solid conductors that are made from metal or carbon, or graphite

Question 4

Which side is which for the electrodes?

Answer 4

Anode on the right, cathode on the left

Question 5

Electrolysis

Answer 5

Splitting an ionic compound using electricity

Question 6

Where are cations attracted to and what happens?

Answer 6

Positive anode, they get discharged to become a neutral atom.

Question 7

Where are the anions attracted to and what happens?

Answer 7

The negative cathode, becomes discharged, forms layers of molten substance

Question 8

What happens at anode?

Answer 8

Oxidation, loss of electrons

Question 9

What happens at cathode?

Answer 9

Reduction, gain of electrons

Question 10

Where do electrons flow?

Answer 10

Electrons from cation pass to anode and then transported along wire to cathode using power of battery, and then passing the electrons to the anion to make a neutral ion.

Question 11

Why can some metals not be reduced?

Answer 11

Reducing metals to become a neutral atom only works if it’s less reactive than carbon. The more reactive metals need to do electrolysis

Question 12

Disadvantages of electrolysis

Answer 12

Expensive and requires a lot more energy

Question 13

How do you make solid metal aqueous for electrolysis?

Answer 13

Purify metal, melt it to make it molten. Dissolve in water
Equation : H2O (l) (two arrows) H+(aq) + OH- (aq)

Question 14

At negative cathode what’s the rule for the element that discharges first?

Answer 14

The ion of the least reactive element will be discharged.

Question 15

At the cathode, what’s happens is a very reactive metal is present and what is the equation?

Answer 15

H+ ions are discharged.
4H+ (aq) + 4e- -> 2H^2 + (g) (reduction)

Question 16

At the cathode, what happened if a low reactive metal is present and what’s the equation?

Answer 16

Metal is discharged.
4H+ (aq) + 4e- -> 2H^2 + (g) (reduction)

Question 17

At the positive anode, what’s the rule if halides are present?

Answer 17

Halide gets discharged.

Question 18

At the positive anode, what’s the rule if a hailed isn’t present?

Answer 18

Hydroxide always gets discharged.

Question 19

What’s the equation if hydroxide is discharged and what reaction is this?

Answer 19

4OH- (aq) -> 2H2O (l) + O2 (g) + 4e- (oxidation)

Question 20

What’s the coating in electroplating?

Answer 20

Anode

Question 21

What’s the object that’s being coated?

Answer 21

Cathode