Electrolysis Flashcards

(36 cards)

1
Q

How does electrolysis work?

A

Electrolysis is the decomposition of a compound into the elements that produce it. This only occurs in subsances that conduct electricity.

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2
Q

What is a positively charged ion called? And what is a negative one called?

A

Cation - positively charged ion
Anion - negatively charged ion

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3
Q

What is the electrode that attracts positively charged ions called?

A

Cathode

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4
Q

What is the charge of an anode?

A

Positive

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5
Q

What is the electrode that attracts negatively charged ions called?

A

anode

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6
Q

What is the charge of a Cathode?

A

Negative

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7
Q

What is the electode that attracts negative ions called?

A

anode

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8
Q

How does Cu²⁺ form copper in electrolysis?

(2 points)

A
  • When voltage is applied, the Cu²⁺ ions are attracted to the cathode.
  • When they touch the cathode, they gain two electrons to form the copper metal.
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9
Q

What happens at the cathode?

A

The metal forms

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10
Q

Explain Oxidation and Reduction in terms of electrolysis.

(HINT: OxidAtion, reduCtion)

A

Oxidation: electrons are lost. This happens at the anode.
Reduction: electrons are gained. This happens at the cathode.

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11
Q

What is an aqueous solution?

A

A solution where the solvent is water.

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12
Q

What happens at the cathode in the electrolysis of an aqueous solution?

A

H⁺ (hydrogen) is produced if the metal is more reactive/higher up on the reactivity series than hydrogen.
The metal ions will form if it is less reactive/further down in the reactivity series than hydrogen.

(e.g, copper)

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13
Q

What happens at the anode in the electrolysis of an aqueous solution?

A

If there are Halide ions present, the respective halides will form.

If there are no halides, oxygen (NOT HYDROXIDE) will form.

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14
Q

What are the half equations for the electrolysis of lead bromide (PbBr₂)?

A

anode, oxidation:
Pb⁺² + 2e⁻ → Pb
cathode, reduction:
2Br⁻ → Br₂ + 2e⁻

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15
Q

Is the electron a product or a reactant in the half equation or a non metal? And why?

A

Product. It has an overall negative charge and needs to loose electrons to become stable.

If the electron is a product the substance is gaining electrons.

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16
Q

Is the electron a product or reactant in the half equasion for a metal?

A

Reactant. It has an overall positive charge and needs to gain electrons to become stable.

If the electron is a reactant the substance is loosing electrons.

17
Q

What two ions form when water is involved in electrolysis? And what electrode are they attracted to?

A

Hydrogen ions: Cathode.
Hydroxide ions: Anode.

18
Q

What is the BALANCED half equation for when oxygen forms at the anode?

A

4OH⁻ → O₂ + 2H₂O + 4e⁻

19
Q

Electrolysis can be used to extract copper from a solution of copper (II) sulfate. Suggest how oxygen is also produced.

A

Oxygen is produced through discharge of hydroxide ions from the water.

20
Q

State two reasons why we use graphite electrodes in the electrolysis of ionic compounds.

A
  • good conductors of electricity
  • inert/unreactive
21
Q

In the extraction of aluminium from aluminium oxide by electrolysis the positive electrode is made of carbon and needs to be regularly replaced. Explain why.

A

The oxygen may react with the carbon anode to form carbon dioxide.

22
Q

How can we test for Hydrogen?

(2 marker)

A
  • squeaky pop test (1 mark)
  • a lighted splint is exposed to the hydrogen. If it makes a squeaky pop then hydrogen is present in thr solution (1 mark)
23
Q

How can we test for oxygen?

(2 marker)

A
  • relight test (1 mark)
  • a lighted splint is exposed to the solution. If oxygen is present then the splint will reignite. (1 mark)
24
Q

Why is the remaining electrolyte an alkali solution after electrolysis has occured in an aqueous solution?

A

There are excess OH- ions (which are alkali)

25
Write the balanced equation for when Hydrogen is discharged/formed in electrolysis.
2H⁺ + 2e⁻ -> H₂
26
What is electroplation and why is it sometimes used in electrolysis?
- Electroplation is when a layer of a metal is put on a different metal. - This is done to improve the physical appearance of the metal - It can also be used to prevent corrosion of the electrodes
27
How can we test for chlorine at the anode? | (2 marker)
Litmus paper test (1 mark) Dampen the litmus paper with water. Expose the litmus paper to chlorine. The paper will be bleached if chlorine is present. (1 mark)
28
How do we know if Bromine has formed at the anode?
A brown gas will form due to the high temperatures reached in the process.
29
Reduction is - Oxidation is -
Reduction is - the gain of electrons Oxidation is - the loss of electrons
30
What are the two elements in brass?
Copper and Zinc
31
What happens at the negative electrode? What happens at the positive electrode? Identify in terms of reduction or oxidation
Reduction occurs at the negative electrode Oxidation occurs positive electrode
32
Why is magnesium extracted using electrolysis instead of carbon?
Magnesium is more reactive than carbon, and therfore carbon cannot be used to extract it.
33
Why is extracting metals through electrolysis so expensive?
Lots of energy is required to... - heat the solution - produce the elecric current
34
What is the first step to undergo electrolysis when extracting aluminum?
The aluminum should be mixed with cryolite, so as to reduce the melting point.
35
When extracting aluminum with electrolysis, the anodes are replaced often. Why is this?
The oxygen molecules (from aluminum oxide) react with the carbon anode to produce carbon dioxide.
36
Recite the steps of the electrolysis practical.
- Pour 50cm³ of the molten/aqueous solution into a beaker - Place a petri dish over the beaker. It should have 2 holes, each of which are for either electrode - Insert the carbon-graphite elecrodes through the holes in the petri dish. - Ensure the electodes do not touch. (it would produce a short-circuit) - Attach crocodile leads to the rods and plug them into a low-voltage power supply and select 4 Volts