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# Copper is an important mineral and element in our daily life. It is an important industrial metal due to its ductility, malleability, electrical conductivity and resistance towards corrosion.

# Copper used in electrical wiring must have a 99.99% purity. The purity of copper extracted by the process of melting is about 99.5%. Even a slight difference in copper purity will negatively impact its conductivity. To determine whether a copper metal is pure, one must conduct the purification of metals through electrolysis.

# The purification of copper by electrolysis is carried out with a piece of pure, thin copper as the cathode; impure copper as the anode; and an aqueous salt solution of copper, such as copper(II) nitrate, Cu(NO3)2 as electrolyte.

# Impure copper anode ionises to form copper(II) ions, Cu2+. Copper dissolves to become copper(II) ions, Cu2+ and impurities accumulate below the impure copper anode. The anode becomes thinner.
Cu(s) → Cu2+(aq) + 2e−

# At the pure copper cathode, copper(II) ions, Cu2+ are discharged to form copper atoms, Cu. Solid copper is deposited and the copper cathode becomes thicker.
Cu2+(aq) + 2e− → Cu(s)

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Electroplating of metals through electrolysis is done by:-
# making the object being electroplated as the cathode, the electroplating metal as the anode, and an aqueous solution containing the ions of the electroplating metal as the electrolyte

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Comparison Between Voltaic Cell and Electrolytic Cell

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Comparison Between Voltaic Cell and Electrolytic Cell

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Comparison Between Voltaic Cell and Electrolytic Cell

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Comparison Between Voltaic Cell and Electrolytic Cell

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Similarities
S1- Electrodes are dipped into the electrolyte
S2- Oxidation reactions at the anodes
S3- Reduction reactions at the cathodes
S4- Electrons flow from the anodes to the cathodes through the connecting wires

Differences

Voltaic cell:-
D1- Chemical energy to electrical energy
D2- Pairs of metals are of different types
D3- Negative terminal is anode and positive terminal is cathode
D4- Blue colour of copper(II) sulphate, CuSO4
solution becomes paler

Electrolytic cell:-
D1- Pairs of metals are the same type
D2- Electrical energy to chemical energy
D3- Blue colour of copper(II) sulphate, CuSO4 solution does not change
D4- Anode is connected to the positive terminal of the battery and cathode is connected to the battery’s negative terminal

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Factors that Affect the Electrolysis of an Aqueous Solution

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Factors that Affect the Electrolysis of an Aqueous Solution

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1. E0 Value

2. Concentration of solution

3. Type of electrode used
- anode
- cathode

Water also takes part in the electrolysis process.

The equation for water dissociation is as follows: H2O(l) ⇌ H+(aq) + OH−(aq)

During electrolysis, cations and hydrogen ions, H+ move to the cathode, while anions and hydroxide ions, OH− move to the anode.

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Conductors :-
# substance that conduct electricity in solid or molten state, but do not undergo chemical changes
# conduct electricity without undergoing decomposition
# can conduct electricity due to the presence of electrons that move freely
# electrical conductivity decreases as temperature increases
# exp: metals, graphite

Electrolyte :-
# substance that conduct electricity in molten state or aqueous solution, and undergo chemical changes
# conduct electricity and undergo decomposition into their constituent elements
# can conduct electricity due to the presence of ions that move freely
# electrical conductivity increases as temperature increases.
# exp: ionic compounds, acids, alkalis.

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Electrolysis is a process whereby compounds in the molten state or an aqueous solution decompose into their constituent elements by passing electricity through them.

Electrolytes are substances that can conduct electricity in either the molten state or aqueous solution and undergo chemical changes.

Non-electrolytes are substances that cannot conduct electricity in all states.

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Classifications