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Topic 3.22-3.31 Electrolytic processes

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Total cards: 15•Content version: v4•Public deck•Updated: 8/1/2026

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#1
Front (Question)

What are electrolytes?

Back (Answer)

Ionic compounds in the molten state or dissolved in water

#2
Front (Question)

Define electrolysis

Back (Answer)

A process in which electrical energy (from a direct current supply) decomposes electrolytes

#3
Front (Question)

Explain the movement of ions during electrolysis

Back (Answer)

Positively charged cations migrate to the negatively charged cathode. And Negatively charged anions migrate to the positively charged anode

#4
Front (Question)

What is oxidation?

Back (Answer)

Loss of electrons

#5
Front (Question)

Where does oxidation occur?

Back (Answer)

The Anode

#6
Front (Question)

What is reduction?

Back (Answer)

Gain of electrons

#7
Front (Question)

Where does reduction occur?

Back (Answer)

The cathode

#8
Front (Question)

Why can only ionic compounds be electrolysed?

Back (Answer)

Ionic compounds contain free-moving ions that can carry electrical current when molten or dissolved in solution, making electrolysis possible.

#9
Front (Question)

Explain the formation of the products in the electrolysis of copper sulfate solution, using copper electrodes, and how this electrolysis can be used to purify copper ​​ ​​​​ ​​​​ ​​ ​​​​ ​​ ​​ ​​​​ ​​ ​​ ​​​​ ​​​​

Back (Answer)

set​ ​up: ○ anode​ ​is​ ​made​ ​of​ ​impure​ ​copper​ ​(that​ ​you​ ​are​ ​purifying) ○ cathode​ ​is​ ​made​ ​of​ ​pure​ ​copper ○ the​ ​solution​ ​is​ ​copper​ ​sulfate ● what​ ​happens: ○ Cu2​+​​​ions​ ​from​​ the​​ anode​​ move​​ to​​ the​​ cathode,​​ where​​they​​ gain​​ electrons and​ ​are​ ​discharged​ ​as​ ​pure​ ​copper ○ impurities​ ​form​ ​as​ ​sludge​ ​below​ ​the​ ​anode ● the​ ​cathode​ ​will​ ​increase​ ​in​ ​mass​ ​as​ ​it​ ​gains​ ​pure​ ​copper,​ ​whilst​ ​the​ ​anode​ ​will lose​ ​mass​ ​as​ ​copper​ ​ions​ ​are​ ​lost​ ​(they​ ​replace​ ​the​ ​ones​ ​from​ ​the​ ​CuSO​4​​ ​solution that​ ​go​ ​to​ ​the​ ​cathode)​ ​and​ ​so​ ​are​ ​impurities

#10
Front (Question)

How can you predict where the products of electrolysis will go?

Back (Answer)

the​ ​+​ ​ions​ ​will​ ​go​ ​to​ ​the​ ​cathode ● the​ ​-​ ​ions​ ​will​ ​go​ ​to​ ​the​ ​anode

#11
Front (Question)

How do you form the half equation for an electrolysis?

Back (Answer)

negative​ ​electrode:​ ​X​+​​ ​->​ ​X, so X​+​​ ​+​ ​e-​ ​​ ​->​ ​X,​ ​electrons​ ​gained,​ ​so​ ​positive​ ​ions​ ​are​ ​reduced positive​ ​electrode:​ ​X​-​​ ​->​ ​X,​ ​so​ X​-​​ ​->​ ​e-​ ​​ ​+​ ​X,​ ​electrons​ ​are​ ​lost,​ ​so​ ​negative​ ​ions​ ​are​ ​oxidised

#12
Front (Question)

A student conducts an investigation to find out what is produced during the electrolysis of sodium sulfate. Describe how the student could carry out an investigation, and show (using ions) what is given off at each electrode.

Back (Answer)

Wearing safety glasses, add sodium sulfate solution to a beaker, and connect two inert electrodes (make sure they do not touch) to a power supply. Completely fill two small test tubes with sodium sulfate solution and position a test tube over each electrode, then turn on the power supply and observe what happens at each electrode. Any gases produced can be collected in the test tubes and tested (squeaky pop test - hydrogen, relight a glowing splint - oxygen). hydrogen gas will form at the negative electrode/cathode: 2H+(aq) + 2e- → H2(g) oxygen gas will form at the positive electrode/anode: 4OH-(aq) → 2H2O(l) + O2(g) + 4e-

#13
Front (Question)

What are the rules for production at the cathode from aqueous solutions?

Back (Answer)

• The metal will be produced at the cathode if it is less reactive than hydrogen and hydrogen will be produced if the metal is more reactive than it

#14
Front (Question)

What metals are less reactive than hydrogen?

Back (Answer)

Copper, silver, gold and platinum are less reactive than hydrogen

#15
Front (Question)

What are the rules for production at the anode for aqueous solutions?

Back (Answer)

• A halogen will be produced if the electrolyte contains a halide ion. Otherwise, oxygen is produced. (For non-aqueous solutions just the