C3.4 Flashcards

1
Q

What is electrolysis?

A

The breaking down of an ionic compound using electricity.

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2
Q

What is the mnemonic for oxidation and reduction?

A

OIL RIG — Oxidation Is Loss, Reduction Is Gain (of electrons).

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2
Q

What happens at the cathode during electrolysis?

A

Positive ions (cations) move to the cathode and gain electrons (reduction).

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3
Q

What happens at the anode during electrolysis?

A

Negative ions (anions) move to the anode and lose electrons (oxidation).

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3
Q

What type of substance can be electrolyzed?

A

Ionic compounds when they are molten or dissolved in water (aqueous).

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4
Q

What forms at the cathode in electrolysis of molten ionic compounds?

A

Metals or hydrogen (if present).

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5
Q

What forms at the anode in electrolysis of molten ionic compounds?

A

Non-metals, such as halogens or oxygen.

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5
Q

When is hydrogen produced at the cathode in aqueous solutions?

A

When the metal in the solution is more reactive than hydrogen.

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6
Q

In electrolysis of aqueous solutions, what ions are present besides the ionic compound?

A

H⁺ (hydrogen) and OH⁻ (hydroxide) ions from water.

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7
Q

When is oxygen produced at the anode in aqueous solutions?

A

When there are no halide ions present.
OH⁻ ions are discharged to form O₂ gas.

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7
Q

What forms at the anode if halide ions (Cl⁻, Br⁻, I⁻) are present?

A

The corresponding halogen is produced.

Chloride (Cl⁻) → Chlorine (Cl₂)

Bromide (Br⁻) → Bromine (Br₂)

Iodide (I⁻) → Iodine (I₂)

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8
Q

What are inert electrodes?

A

Electrodes that do not react during electrolysis, such as graphite or platinum.

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9
Q

Why are non-inert electrodes used in some electrolysis reactions?

A

To allow purification or plating reactions where the electrode itself takes part.

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9
Q

What is formed at the cathode in the electrolysis of sodium chloride (NaCl) solution?

A

Hydrogen gas (H₂) because sodium is more reactive than hydrogen.

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10
Q

What is formed at the anode in the electrolysis of sodium chloride (NaCl) solution?

A

Chlorine gas (Cl₂) because of the presence of halide ions (Cl⁻).

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11
Q

What forms at the anode in the electrolysis of copper sulfate (CuSO₄) solution?

A

Oxygen gas (O₂) because sulfate ions (SO₄²⁻) are not halides.

11
Q

What forms at the cathode in the electrolysis of copper sulfate (CuSO₄) solution?

A

Copper metal (Cu) because it is less reactive than hydrogen.

12
Q

What is the equation for the reaction at the cathode when hydrogen is produced?

A

2H⁺ + 2e⁻ → H₂

13
Q

What is the equation for the reaction at the anode when oxygen is produced?

A

4OH⁻ → O₂ + 2H₂O + 4e⁻

14
Q

What is the purpose of electroplating?

A

To coat the surface of a metal object with another metal for appearance or protection.

15
Q

Why is electrolysis expensive?

A

It requires a lot of energy for electricity and to melt ionic compounds.

16
Q

In the purification of copper, what is used as the anode and cathode?

A

Anode: Impure copper (loses Cu²⁺ ions).

Cathode: Pure copper (gains Cu²⁺ ions).

17
Q

How do you identify the ions present in an electrolysis reaction?

A

Split the ionic compound into positive and negative ions.

Include H⁺ and OH⁻ if aqueous.

Positive ions → Cathode (Reduction)

Negative ions → Anode (Oxidation)

17
Q

What is the difference between molten and aqueous electrolysis?

A

Molten: Only ionic compound ions present.

Aqueous: Ions from water (H⁺ and OH⁻) also present.

18
Q

Why is cryolite used in the electrolysis of aluminium oxide?

A

It lowers the melting point of aluminium oxide, reducing energy costs.