2.5: 5. ECHEM- Electrochemistry and RedOx Reactions
- Page ID
- 436101
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- Review concepts: Assign oxidation states to all atoms in a compound or element. Explain the difference between oxidation states and formal charges.
- Provide definitions for the following terms: oxidation state, oxidation, reduction, oxidizing agent, reducing agent, redox reaction, anode, and cathode.
- Identify the redox reactions from a given list of reactions and compare and contrast this type of reaction to other types of reactions, such as acid-base reactions, precipitations, etc.
- For a given redox reaction, decide which species is the reducing agent and explain why it is the reducing agent rather than some other species in the reaction.
- Write balanced redox reactions and determine the number of electrons transferred in a balanced chemical reaction.
- If any two given species are mixed, determine whether or not a spontaneous redox reaction will occur using tables of standard reduction potentials.
- Compare and contrast galvanic and electrolytic cells.
- For a given galvanic cell, identify (and define) the electrodes (anode and cathode), the positive (+) and negative (-) poles; the electrode where oxidation occurs, the electrode where reduction occurs, the "flow" of electrons through the external circuit, the flow of the ions through the solutions, and the salt bridge.
- If an electrode is changing size over the course of reaction, determine whether it is getting larger or smaller over time and explain why this is happening.
- Explain what the SHE half-cell is and how it is used to determine standard state reduction potentials for other species.
- Interpret cell diagrams to determine: 1) which species is the anode and which is the cathode and 2) the resulting voltage at that point in time.
- Calculate the standard cell potential from a table of reduction potentials and interpret the meaning of the sign of the calculated potential.
- Calculate the cell potential when the system is not at standard state conditions.
- Relate the cell potential when the system is in a state of equilibrium and calculate the value of the equilibrium constant from the standard state cell potential or vice-versa.
- Relate the cell potential to the change in free energy.
- Explain how a galvanic cell maintains overall electrical neutrality at all times.
- Explain what concentration cells are and how they are able to produce electrical energy, and calculate the cell potential for a concentration cell.
- Perform calculations involving Faradays’ equation for electrolysis; i.e. finding needed electrical current, time current needs to operate, mass of substance electrolyzed, or volume of gaseous substance produced by electrolysis at a given T and P.
- Create a list of real world applications or processes that involve redox reactions.