1.3.3 Voltaic Cell T/F

A chemical cell is an electrochemical cell that converts chemical energy into electrical energy.

Mg is oxidized to Mg²⁺ by losing two electrons.

Copper acts as the anode in a chemical cell using magnesium as an electrode.

Hydrogen gas bubbles form on the surface of the copper electrode.

Mg is more electropositive than Cu.

Mg²⁺ + 2e⁻ → Mg is a half-equation for oxidation.

In a chemical cell, anions move towards the anode.

Mg is more easily oxidized than Cu according to E° values.

Zn²⁺ is oxidized to Zn in the reaction with Cu²⁺.

In the Daniell cell, Zn acts as the anode and Cu as the cathode.

Cu²⁺ is reduced to Cu in the Daniell cell.

A more negative E° value indicates a lower ability to be oxidized.

The electrode where oxidation occurs is the cathode.

Zn²⁺ + 2e⁻ → Zn is a half-equation for reduction in the Daniell cell.

The Daniell cell uses a salt bridge to complete the circuit.