Electrolysis of Molten Compounds

1.

Multiple Choice

1 min

1 pt

What is the product formed at the cathode during the electrolysis of molten magnesium fluoride?

magnesium

hydrogen

fluorine

oxygen

2.

Multiple Choice

30 sec

1 pt

Explain why the electrolyte has to be a liquid.

So the ions can move

So the electrons can move

So that it doesn't get too hot

So the fish are ok

3.

Multiple Choice

30 sec

1 pt

What does the Cathode (-) do to ions?

Give electrons to the Positive ions to turn them back into atoms

Take electrons from the positive ions?

Turn ions back into atoms by removing electrons

Turn atoms into ions by adding electrons

4.

Multiple Choice

30 sec

1 pt

Describe oxidation in terms of electrons

oxidation is gain of electrons

oxidation is loss of electrons

5.

Multiple Choice

30 sec

1 pt

Describe reduction in terms of electrons

reduction is gain of electrons

reduction is loss of electrons

6.

Multiple Choice

30 sec

1 pt

Why can ionic compounds not conduct electricity when they are solid?

their electrons are not free to move

their ions are free to move

their ions are not free to move

their electrons are free to move

7.

Multiple Choice

30 sec

1 pt

What type of charge does a metal ion have?

+

-

8.

Multiple Choice

30 sec

1 pt

The electrode connected to the positive terminal of a battery is __________.

cathode

anode

9.

Multiple Choice

30 sec

1 pt

The negatively charged ions migrate toward the ________.

anode

cathode

10.

Multiple Choice

30 sec

1 pt

Which statement correctly describes the 2 electrodes?

The anode is negative and the cathode is positive

The anode and cathode are both positive

The anode is positive and the cathode is negative

The anode and cathode are both negative.

11.

Multiple Choice

30 sec

1 pt

Positive ions (cations) will move towards the cathode (-) where they will discharge by....

Breaking apart

Losing electrons

Clumping together.

Gaining electrons

12.

Multiple Choice

30 sec

1 pt

What is the equation to show what happens to chloride ions at the anode.

Cl^- --> Cl + e-

2Cl^- --> Cl₂ + 2e-

Cl₂ + 2e-2Cl^-

Cl₂ + 2e-_-->2Cl^-

13.

Multiple Choice

45 sec

1 pt

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

Al³⁺ - 3e^- --> Al

Al²⁺ + 3e^- --> Al

Al³⁺ + 3e^- --> Al

Al³⁺ --> Al + 3e^-

14.

Multiple Choice

30 sec

1 pt

Why ionic compounds can not conduct electricity when they are solid?

their electrons are not free to move

their ions are free to move

their ions are not free to move

their electrons are free to move

15.

Multiple Choice

30 sec

1 pt

What are the ions present in molten Al₂O₃?

Al²⁺ and O^3-

Al^2- and O³⁺

Al³⁺ and O^2-

Al^3- and O²⁺

16.

Multiple Choice

30 sec

1 pt

Oxidation is loss of electron. Where does oxidation take place during electrolysis.

At anode

In the solution

At cathode

In the circuit

17.

Multiple Choice

20 sec

1 pt

Electrolysis is .....

conduction of electricity by the ionic compound in solid state

conduction of electricity by ionic compound in molten and aqueous state

18.

Multiple Choice

20 sec

1 pt

What is electrolysis?

breaking down of a compound using a current

making a compound using a current

19.

Multiple Choice

45 sec

1 pt

Which statement correctly describes the 2 electrodes?

The anode is negative and the cathode is positive

The anode and cathode are both positive

The anode is positive and the cathode is negative

The anode and cathode are both negative.

20.

Multiple Choice

30 sec

1 pt

What happens at the positive electrode?

Positive non-metal ions are attracted

Positive metal ions are attracted

Negative non-metal ions are attracted

Negative metal ions are attracted

21.

Multiple Choice

30 sec

1 pt

Explain why the electrolyte has to be a liquid

So the ions can move

So the electrons can move

So that it doesn't get too hot

So the fish are ok

22.

Multiple Choice

30 sec

1 pt

What happens to the metal ions during electrolysis?

Nothing

Reduction; they gain electrons

Oxidation; they gain electrons

Reduction; they lose electrons

23.

Multiple Choice

30 sec

1 pt

Why can ionic compounds not conduct electricity when they are solid?

their electrons are not free to move

their ions are free to move

their ions are not free to move

their electrons are free to move

24.

Multiple Choice

30 sec

1 pt

Describe oxidation in terms of electrons

oxidation is gain of electrons

oxidation is loss of electrons

25.

Multiple Choice

30 sec

1 pt

What would the charges be on the ions that make up NaCl?

Na⁺ and Cl^-

Na^- and Cl⁺

Na^₊and Cl^_-

26.

Multiple Choice

20 sec

1 pt

What element is used to make up the electrodes?

oxygen

iron

carbon

magnesium

27.

Multiple Choice

20 sec

1 pt

Finish the statement...."Opposites..."

repel

attract

do nothing

28.

Multiple Choice

30 sec

1 pt

When NaCl solution is electrolysed what has forms at the anode?

Hydrogen

Oxygen

Chlorine

Sodium

29.

Multiple Choice

1 min

1 pt

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?

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

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

The ions in lead(II) bromide are acting as the mobile charge carriers when it is melted

There are no ions in solid lead(II) bromide

30.

Multiple Choice

30 sec

1 pt

Reduction occurs at the

anode

cathode

31.

Multiple Choice

30 sec

1 pt

What kind of Electrical Current does Electroysis require?

Direct

Indirect

Anternative

A alternating

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