Battery

Definition

A battery is a device consisting of one or more electrochemical cells that convert stored chemical energy into electrical energy. It typically has a positive (cathode) and negative (anode) terminal.

5 Must Know Facts For Your Next Test

1. Batteries operate based on redox reactions, where oxidation occurs at the anode and reduction occurs at the cathode.
2. The standard notation for a galvanic cell (battery) includes the anode on the left and the cathode on the right, separated by two vertical lines representing the salt bridge.
3. $E^\circ_{cell}$, the standard cell potential, is calculated using $E^\circ_{cell} = E^\circ_{cathode} - E^\circ_{anode}$.
4. Primary batteries are non-rechargeable, while secondary batteries can be recharged multiple times.
5. Common types of batteries include alkaline, lead-acid, lithium-ion, and nickel-cadmium.

Review Questions

• What are the roles of the anode and cathode in a battery?
• How do you calculate the standard cell potential ($E^\circ_{cell}$) for a given battery?
• What is the main difference between primary and secondary batteries?

Related terms

Anode:

The electrode at which oxidation occurs in a battery.

Cathode:

The electrode at which reduction occurs in a battery.

$E^\circ_{cell}$: Standard cell potential; it quantifies the voltage difference between two half-cells under standard conditions.