Galvanic Cells (3) Flashcards
1
Q
What are Galvanic Cells?
A
- A small scale portable device capable of generating electrical energy from redox reactions of chemicals contained within
- It is where the spontaneous reactions that produce electricity
2
Q
What are Galvanic Cells made up of?
A
- 2 Cells
- An oxidation half-cell + reduction half-cell
- 2 types of connection
- External metal wire where electrons flow
- Salt-bridge consisting of free ions to stabilise charge and complete circuit
3
Q
What is the purpose of a saltbridge and what does it consist of?
A
- Completes the circuit by allowing migration of ions to maintain cell neutrality
- Consists of a solution in which neither anion or cation will react with either half-cell
4
Q
Name the common types of salt bridges
A
- Sodium nitrate
- Potassium nitrate
- Ammonium nitrate
5
Q
What are the types of half cells?
A
- Metal half cells
- Solution half cells
- Gaseous half cells
6
Q
What’s so special about a hydrogen half-cell?
A
- It is a hydrogen gas bubbled over a platinum electrode
- Has a potential of 0 volts (in data booklet)
- Allowed other half cell potentials to be obtained by measuring cell potential when connected to hydrogen half cell
- Is known as ‘reference half cell’
7
Q
Oxidation occurs at the _____
A
Anode
8
Q
Reduction occurs at the _______
A
Cathode
9
Q
Anode is ________
A
Negative
10
Q
Cathode is ________
A
Positive
11
Q
Electrons flow _____ to _______
A
Anode to Cathode
12
Q
Positive ions in the salt bridge move to _______
A
Cathode
13
Q
NEgative ions in saltbridge move to the _____
A
Anode
14
Q
Build a galvanic cell between magnesium and copper. Include the diagram, overall equation w/ half cell potentials and label clearly.
A
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