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Chemisty -GCSE Higher Tier > Electrolysis > Flashcards

Electrolysis Flashcards

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1
Q

What equipment is needed

A

Beaker, electrolyte, cathode and anode, battery, wire

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2
Q

What is an electrolyte

A

Liquid or solution that contains an ionic compound, the ions are free to move around.

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3
Q

Example of a soluble electrolyte

A

Copper Sulphate (CuSO4)

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4
Q

What is a soluble electrolyte

A

A compound dissolved in water

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5
Q

What is an insoluble electrolyte

A

A compound that needs to be melted to get a molten liquid so that the ions are free to move around

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6
Q

Example of an insolvable electrolyte

A

Lead Bromide (PbBr2)

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7
Q

What are electrodes

A

Solid consuctors

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8
Q

What are electrodes made out of

A

metal or graphite (carbon)

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9
Q

What is the positive electrode

A

The anode

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10
Q

The is the negative electrode

A

The cathode

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11
Q

What is the wire for

A

so the electrons can flow

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12
Q

what is the battery for

A

to drive the flow of electrons

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13
Q

what does electrolysis mean

A

‘splitting up with electricity’

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14
Q

what does electrolysis do

A

a current is passed through to electrolyte to separate the elements in a compound

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15
Q

What are negative ions attracted to

A

The positive anode

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16
Q

What are positive ions attracted to

A

the negative cathode

17
Q

What happens when ions reach an electrode

A

They are discharged meaning a charger ion becomes a neutral ion

18
Q

What happens when lead is discharged

A

It goes to the negative cathode and is discharged to form a layer of pure lead at the bottom of the beaker

19
Q

What happened when broke is discharged

A

the atoms pair up to form bromine gas which floats off

20
Q

What happens to the atoms at the anode

A

They are oxidised

21
Q

What happens to the atoms at the cathode

A

They are reduced

22
Q

What is oxidation

A

The ions at the anode lose electrons

23
Q

What is reduction

A

The ions at the cathode gain electrons

24
Q

How do the ions get reduced and oxidised

A

The electrons from the ions at the positive anode are transported along the wire to the cathode and are given to the ions at the negative cathode

25
Q

Why do the ions get reduced and oxidised

A

to discharge the ions so they are neutral are return to their original form as atoms

26
Q

Oxidisation half equation

A

2Br- —> Br2 + 2e-

27
Q

Reduction half equation

A

Pb2+ + 2e- —> Pb

28
Q

What side is the anode

A

Right

29
Q

What side is the cathode

A

Left

30
Q

Why do metal oxides need to be melted into a molten liquid

A

So that the ions can be free to move around

31
Q

What other ions do aqueous solutions contain

A

Positive Hydrogen and negative Hydroxide

32
Q

What is hydrogen attracted to

A

The negative cathode

33
Q

What is hydroxide attracted to

A

The positive anode

34
Q

If there is more than one ion at a cathode which will be discharged

A

The ion of the least reactive element

35
Q

What is the reactivity series

A

Potassium, Sodium, Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Tin, Lead, Hydrogen, Copper, Silver, Gold, Platinum

36
Q

What is a saying to remember the reactivity series

A

Pop Stars Can Make Absolute Crazy Zillions If Tiny Little Hungry Children Spend Generously Please

Chemisty -GCSE Higher Tier (2 decks)

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