Electrolysis Flashcards

1
Q

What is electrolysis?

A

The splitting up of a compound using electricity

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2
Q

What is the half equation for the electrolysis of lead

A

Pb–>Pb 2+ +2e-

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3
Q

What is the equation for the formation pf bromine

A

2Br+2e- –> 2Br-

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4
Q

What state mus the compound be in for electrolysis

A

Liquid (aqueous solution) or molten

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5
Q

What is the cathode

A

The negative terminal, full of electrons

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6
Q

What is the anode

A

Positive terminal, lack of electrons

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7
Q

Why are the elements in the compounds attracted to the cathode or anode

A

Because opposites attract

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8
Q

What is oxidation

A

The loss of electrons

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9
Q

What is reduction

A

Gain of electrons

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10
Q

Where does oxidation occur

A

At the anode

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11
Q

Where does reduction occur

A

At the cathode

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12
Q

What is an aqueous solution

A

Something dissolved in water

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13
Q

What happens to water molecules during electrolysis

A

They also ionise, forming hydrogen ions (+) and hydroxide ions (-)

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14
Q

What is a reversible reaction

A

A reaction that can happen both ways

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15
Q

What happens at the anode during the electrolysis of NaCl dissolved in water

A

The chloride ions lose one electron each at the positive anode, pair up and become chloride gas (oxidation). The hydroxide ions get left behind in the solution

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16
Q

What is the half equation for chlorine at the anode

A

2Cl+ –> Cl(2) + 2e-

17
Q

What happens to sodium at the cathode

A

The sodium is more reactive than the hydrogen, meaning that hydrogen gas is released (H2). This means that sodium ions are left behind in the solution

18
Q

What is the half equation for what happens at the cathode during the electrolysis of NaCl

A

2H+ + 2e- –> H2

19
Q

What are the rules of electrolysis for positive ions

A

If the metal is less reactive then hydrogen, then it forms at the cathode, but if it is more reactive than hydrogen, then hydrogen gas is released at the cathode

20
Q

What are the rules pf electrolysis for negative ions

A

If halide (group 7) ions are present, they will be released at the anode. Next, is hydroxide ions,releasing oxygen at the anode. Half equation ( 4OH- –> 2H2O + O2 + 4e-). Any larger ions come next

21
Q

What is the overall equation for the electrolysis of aluminium oxide

A

2Al2 O3 (l) –> 4Al (l)+ 3O2 (g)

22
Q

Why are electrodes made from carbon graphite

A

Because they are solid, unreactive and good conductors

23
Q

What is the half equation for the aluminium in aluminium oxide

A

Al3+ (l) + 3e- –>Al (l) (reduction)

24
Q

What is the half equation for the oxygen in the aluminium oxide

A

2O2- (l) –> O2 (g) + 4e- (oxidation)

25
Q

What is phytomining

A

The extraction of copper using plants

26
Q

What is bioleaching

A

The extraction of copper using bacteria

27
Q

What is the word and symbol equation for the displacement reaction of adding scrap iron to the copper

A

Iron+ copper (II) sulfate –> iron (III) sulfate + copper

Fe (s) + Cu2+ (aq) –> Fe 2+ (aq) + Cu (s)

28
Q

Where are the pure and impure copper sheers placed during the reaction

A

The pure copper sheet is placed at the cathode, with the impure copper sheet placed at the anode

29
Q

What reaction happens at the cathode

A

Cu2+ (aq) + 2e- –> Cu (s)

30
Q

Why does the cathode strip get larger

A

Because solid copper is deposited there

31
Q

What reaction happens at the anode

A

Cu (s) –> Cu2+ (aq) + 2e-

32
Q

Why is there sludge at the anode

A

Because as the copper from the anode replaces the copper in the solution, other valuable materials below copper in the reactivity series are deposited at the bottom of the container