AP®︎ Chemistry: Topic 9.8 Flashcards

The study of redox reactions that convert chemical energy and electrical energy into each other.

A device in which separated half-reactions transfer electrons through a wire and ions through solution.

Separate oxidation and reduction equations that show electron loss and gain in a redox process.

Tabulated voltages for reduction half-reactions under standard conditions, used to calculate overall cell voltage.

Anode is where oxidation occurs; cathode is where reduction occurs in all electrochemical cells.

Electrons move through the wire from the anode to the cathode.

Solutions containing the ions involved in each electrode reaction, allowing charge transfer and reaction progress.

An external device connected to the circuit to measure the cell's potential difference or current.

The oxidation electrode loses mass, while the reduction electrode gains mass when solid metal is deposited.

Gas forms at an electrode when a half-reaction produces a gaseous product, often seen as bubbles.

Spontaneous cells generate electrical energy, while nonspontaneous cells require external electrical energy.

Overall voltage equals cathode reduction potential minus anode reduction potential; reversing changes sign only.

A tube of inert ions that maintains neutrality by sending anions to the anode and cations to the cathode.

Conductive surfaces where redox occurs; some are inert and only provide electron-transfer surfaces.

The flow of positive charge through a circuit, opposite the direction of electron flow.