Term | Definition |
Oxidation | Loss of electrons |
Reduction | Gain of electrons |
Oxidizing agent | Species that causes other species to be oxidized, or the species that is reduced |
Reducing agent | Species that causes the other species to be reduced, or the species that is oxidized |
Anode | The species in a galvanic cell that is oxidized |
Cathode | The species in a galvanic cell that is reduced |
In a galvanic cell, electrons flow from ___ to ___. | anode to cathode |
In a galvanic cell with a salt bridge, ___ ions flow to the anode and ___ ions flow to the cathode | negative ions (anions) to anode, positive ions (cations) to cathode |
In a galvanic cell with a porous disc, ___ ions flow to the anode. | negative ions (anions) |
A spontaneous reaction must have a ____ sign on the cell potential | positive |
The Faraday Constant | 96,485 C/mol e- |
The equation for finding the free energy of an electrochemical reaction | deltaG = - n * F * E where n is the number of moles of electrons transferred, F is the Faraday constant, and E is the total cell potential |
Order of steps when balancing a simple redox reaction | 1. Write half-reactions
2. Balance atoms
3. Balance charges by adding electrons
4. Multiply equations to have same number of electrons on either side
5. Cancel electrons
6. Add half-reactions together |
Order of steps when balancing a complex redox reaction in acidic solution | 1. Write half-reactions
2. Balance atoms
3. Balance oxygens by adding H2O
4. Balance hydrogens by adding H+
5. Balance charges by adding e-
6. Multiply equations to have same number of electrons on either side
7. Cancel e-
8. Add half-reactions |
Order of steps when balancing a complex redox reaction in basic solution | 1. Write half-rxns
2. Balance atoms
3. Balance Os by adding H2O and Hs by adding H+
5. Balance charges by adding e-
6. Multiply to have same # of e- on each side
7. Cancel e-
8. Add half-rxns
9. Add OH- to each side matching # of H+
10. Cancel H2O |