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An electrochemical cell consists of two half-cells, each containing an electrode immersed in an electrolyte solution. The half-cells are connected by a salt bridge, which allows ions to migrate between compartments while maintaining charge neutrality. An external wire enables electron flow between electrodes, completing the circuit and generating electric current through redox reactions.

A galvanic cell generates electricity spontaneously through a redox reaction without requiring an external power source. In contrast, an electrolytic cell requires an external current to drive a non-spontaneous reaction. Galvanic cells are used for power generation, while electrolytic cells are widely used in applications such as electroplating metals onto jewelry and industrial metal products.

In the Daniell cell, zinc oxidizes at the anode, releasing electrons: Zn → Zn²⁺ + 2e⁻. These electrons flow through the external wire to the copper cathode, where reduction occurs: Cu²⁺ + 2e⁻ → Cu. The overall reaction combines these half-reactions, generating the cell's electric current and driving the spontaneous redox process.

The salt bridge contains an electrolyte solution and maintains electrical neutrality by allowing ions—not electrons—to migrate between the two half-cell compartments. As electrons flow through the external wire from anode to cathode, ions traverse the salt bridge in the opposite direction, completing the electrical circuit and preventing charge accumulation in either half-cell.

Electrons flow from zinc to copper because the spontaneous redox reaction drives electron release at the zinc anode and electron acceptance at the copper cathode. In a galvanic cell, the anode is negative and the cathode is positive, creating an electrical potential difference that pushes electrons through the external circuit toward the positive cathode.

Half-reactions represent oxidation at the anode and reduction at the cathode as individual processes. When combined, they form the overall redox reaction responsible for current generation. In the Daniell cell, the oxidation half-reaction (Zn → Zn²⁺ + 2e⁻) and reduction half-reaction (Cu²⁺ + 2e⁻ → Cu) combine to produce the overall reaction: Zn + Cu²⁺ → Zn²⁺ + Cu.

The electromotive force (emf) is the open-circuit potential difference between the cell's terminals and reflects the driving force of the spontaneous reaction. A higher emf indicates a greater tendency for the redox reaction to proceed spontaneously, determining the cell's ability to generate electrical current. Understanding emf is essential for predicting cell behavior and applications of emf measurements in various electrochemical systems.