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Electrolysis big review

Total questions: 45

Worksheet time: 27mins

Name
Class
Date
1.
What is electrolysis?
a)
breaking down of a compound using a current
b)
making a compound using a current
2.
What kind of Electrical Current does Electroysis require?
a)
Direct
b)
Indirect
c)
Anternative
d)
A alternating
3.
Which statement correctly describes the 2 electrodes?
a)
The anode is negative and the cathode is positive
b)
The anode and cathode are both positive
c)
The anode is positive and the cathode is negative
d)
The anode and cathode are both negative.
4.
What is the name given to the solution that is being electrolysed?
a)
Salt solution
b)
Electric solution
c)
Mineral solution
d)
Electrolyte
5.
Explain why the electrolyte has to be a liquid.
a)
So the ions can move
b)
So the electrons can move
c)
So that it doesn't get too hot
d)
So the fish are ok
6.
It is essetial that the electrolyte is a liquid so that...
a)
Charged ions can migrate towards the electrodes. 
b)
Charged ions can migrate towards the electrodes.
c)
The solution can move around.
d)
The current can flow through it.
7.
What happens at the positive electrode?
a)
Positive non-metal ions are attracted
b)
Positive metal ions are attracted
c)
Negative non-metal ions are attracted
d)
Negative metal ions are attracted
8.
When NaCl solution is electrolysed what has forms at the anode?
a)
Hydrogen
b)
Oxygen
c)
Chlorine
d)
Sodium
9.
Positive ions (cations) will move towards the cathode (-) where they will discharge by....
a)
Breaking apart
b)
Losing electrons
c)
Clumping together.
d)
Gaining electrons
10.
What does the Cathode (-) do to ions?
a)
Give electrons to the Positive ions to turn them back into atoms
b)
Take electrons from the positive ions?
c)
Turn ions back into atoms by removing electrons
d)
Turn atoms into ions by adding electrons
11.
What is the equation to show what happens to Cl ions at the anode.
a)
Cl- --> Cl + e-   
b)
2Cl- --> Cl2 + 2e-   
c)
Cl2 + 2e-   2Cl- 
d)
Cl2 + 2e-  -->  2Cl- 
12.

The diagram shows the electrolysis of lead(II) bromide using inert electrodes. Why does the bulb only light up when the lead(II) bromide is melted?

a)

Bromine atoms in lead(II) bromide are converted to ions when it is melted

b)

Electrons flow through the lead(II) bromide when it is melted

c)

The ions in lead(II) bromide are mobile charge carriers in the molten state.

d)

There are no ions in solid lead(II) bromide

13.

Anions get discharged by ________ electrons at the ___________

a)

gaining, cathode

b)

losing, anode

c)

gaining, anode

d)

losing, cathode

14.

What ions are present in molten aluminium oxide?

a)

Al3+, O2-, H+, OH-

b)

Al3+, O2-

c)

Al3+, OH-

15.
What happens at the positive electrode?
a)
Positive non-metal ions are attracted
b)
Positive metal ions are attracted
c)
Negative non-metal ions are attracted
d)
Negative metal ions are attracted
16.

___________ electrode is an inert electrode.

a)

Copper

b)

Iron

c)

Carbon

d)

Zinc

17.
What particle carries the charge in the wire?
a)
electron
b)
proton
c)
ion
d)
atom
18.
What particle carries the charge in the wire?
a)
electron
b)
proton
c)
ion
d)
atom
19.
What particle carries the charge in the electrolyte?
a)
electron
b)
proton
c)
ion
d)
atom
20.
What is an ore?
a)
a solid metal
b)
a rock cantaining a metal combined with other elements
c)
an element
d)
an object used to row a boat
21.
Which of these elements is unlikely to be found native?
a)
gold
b)
platinum
c)
aluminium
d)
silver
22.
What is the removal of oxygen from a substance called?
a)
reduction
b)
extraction
c)
electrolysis
d)
oxidation
23.
What is the addition of oxygen to a substance called?
a)
decomposition
b)
reduction
c)
oxidation
d)
extraction
24.
Which series is used to predict the reactions of metals with carbon and other elements?
a)
reactionary series
b)
reaction series
c)
redox series
d)
reactivity series
25.
How could you extract sodium from molten sodium chloride?
a)
reduction by carbon
b)
electrolysis
c)
decomposition
d)
oxidation
26.

What is the ore of aluminium called?

a)

Baxite

b)

Bauxite

c)

Cryolite

d)

Malachite

27.

The electrodes in electrolysis of aluminium are made of

a)

Steel

b)

Anodes

c)

Graphite

d)

Plastic

28.

What is the gas produced at the anode during the electrolysis of very dilute hydrochloric acid?

a)

water

b)

oxygen

c)

hydrogen

d)

chlorine

29.
What is the product formed at the anode during the electrolysis of concentrated copper(II) chloride?
a)
copper
b)
chlorine
c)
hydrogen
d)
oxygen
30.

Choose the half-equation that shows the discharge of aluminium ion.

a)

Al3+ - 3e- --> Al

b)

Al2+ + 3e- --> Al

c)

Al3+ + 3e- --> Al

d)

Al3+ --> Al + 3e-

31.

What is the half-equation for the discharge of hydroxide ions?

a)

2O2- --> O2 + 4e-

b)

OH- --> OH + e

c)

4OH- --> 2H2O + O2 + 4e-

d)

2H2O + O2 + 4e- --> 4OH-

32.

The picture shows electrolysis of copper(II) sulphate solution using graphite electrodes. Besides formation of brown solid on the cathode, what other observations can be made?

a)

The mass of graphite anode decreases.

b)

The blue colour solution becomes paler.

c)

Bubbles of gas form at the anode.

d)

The blue colour solution becomes darker.

33.
When NaCl solution is electrolysed what has forms at the anode?
a)
Hydrogen
b)
Oxygen
c)
Chlorine
d)
Sodium
34.
Molten lead(II) bromide is able to conduct electricity due to the presence of
a)
free atoms
b)
molten lead
c)
mobile ions
d)
bromine gas
35.

Which of the following requires the largest number of electrons for complete discharge during electrolysis?

a)

1 mol of Cu2+ ions

b)

2 mol of O2– ions

c)

3 mol of Na+ ions

d)

3 mol of Cl– ions

36.

Which of the following solutions would produce hydrogen gas at the cathode upon electrolysis?

1 Dilute nitric acid

2 Aqueous potassium hydroxide

3 Aqueous sodium chloride

a)

1 only

b)

1 and 2

c)

2 and 3

d)

All of the above

37.

Which ions are present in molten magnesium bromide?

a)

Mg+ and Br-

b)

Mg2+ and Br-

c)

Mg2+ and Br2-

d)

Mg2+ and Br2-

38.

What are the products when molten sodium oxide is electrolysed?

a)

Na2 and O2

b)

Na+ and O2-

c)

Na and O

d)

Na and O2

39.

Which process could happen at the cathode?

a)

Na+ + e- → Na

b)

2 O2- → O2 + 4 e-

40.

Which process could happen at the anode?

a)

Na+ + e- → Na

b)

2 O2- → O2 + 4 e-

41.

Which ions are present in sodium chloride solution?

a)

Na+ and Cl- only

b)

Na and Cl2

c)

Na+, Cl-, H+ and OH-

d)

Na, Cl2 and H2O

42.

Sodium is higher than lead in the reactivity series. If both sodium and lead cations were present in a solution, which would discharge at the cathode?

a)

Sodium

b)

Lead

43.

In sodium chloride solution, there are two cations present: Na+ and H+. Which will discharge at the cathode?

a)

Na+ to make Na metal

b)

H+ to make H2 gas

44.

In sodium chloride solution, there are two anions present: Cl- and OH-. Which will discharge at the anode?

a)

Cl- to make Cl2 gas

b)

OH- to make O2 gas

45.

What are the products when copper chloride solution is electrolysed?

a)

Cu and Cl2

b)

Cu and O2

c)

H2 and O2

d)

H2 and Cl2

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