Galvanic cells

Definition

Galvanic cells, also known as voltaic cells, are electrochemical cells that convert chemical energy into electrical energy through spontaneous redox reactions. They consist of two half-cells connected by a salt bridge and an external circuit.

5 Must Know Facts For Your Next Test

1. In a galvanic cell, the anode is the electrode where oxidation occurs and is negatively charged.
2. The cathode is the electrode where reduction occurs and is positively charged in a galvanic cell.
3. Electrons flow from the anode to the cathode through an external circuit.
4. The salt bridge maintains ionic balance by allowing ions to move between the two half-cells without mixing the solutions directly.
5. Standard electrode potentials can be used to calculate the cell potential (voltage) of a galvanic cell.

Related terms

Oxidation:

A chemical reaction where a substance loses electrons, increasing its oxidation state.

Reduction:

A chemical reaction where a substance gains electrons, decreasing its oxidation state.

Electrode Potential:

$$E^0$$ values representing the tendency of a chemical species to be reduced, measured under standard conditions.