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Chapter 5: Galvanic Cells
This is a draft cheat sheet. It is a work in progress and is not finished yet.
Galvanic Cells
- Devices that spontaneously convert chemical energy into electrical energy via redox reactions |
- Galvanic Oxidation at the Anode is Negative |
- REDuction occurs at the CATthode (which is positive) |
- Discharges & is spontaneous |
⁻ve terminal anode |
⁺ve terminal cathode |
- 'S' shape formed on electrochemical series |
Galvanic Cell Components
- Half cells |
Purpose Of Salt Bridge |
- Anode |
- To keep each half cell neutral |
- Cathode |
- To complete the internal circuit |
- Voltmeter with connecting wires |
|
- Salt bridge |
- Solutions |
- Electrodes |
- Electron movement |
Electrolytes
Acidic |
Alkaline |
- H⁺ ions |
- OH⁻ ions |
|
|
Primary Vs Secondary Cells
Primary Cells |
Secondary Cells |
- Can't be recharged |
- Can be recharged |
- Products slowly move away from electrodes or are consumed by side reactions, preventing rechargability |
|
Electrolytic Cells
- The 'reverse' of galvanic cells |
- Non-spontaneous, recharges via an electrical current that is slightly higher in voltage than the cell |
⁺ve terminal anode (still undergoes oxidation) |
⁻ve terminal cathode (still undergoes reduction) |
Electrical → chemical energy via electrolysis |
'Z' shape on electrochemical series |
Battery Life Shortage Causes
- Detached products from electrode within cell |
- Unwanted side reactions due to other formed chemicals |
- Cell material (including electrodes) impurities |
- Corrosion |
- Failure of internal components |
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