AP Chemistry Flashcards: Galvanic Voltaic And Electrolytic Cells

What this deck covers

This deck focuses on Galvanic Voltaic And Electrolytic Cells, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

How to use these flashcards

Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: What is the role of inert electrodes like platinum?

Answer: To conduct electrons without participating in the reaction. Provide surface for electron transfer without reacting.

Flashcard 2: What occurs at the cathode in an electrolytic cell?

Answer: Reduction. Reduction still occurs at cathode regardless of cell type.

Flashcard 3: What is the primary function of an electrolytic cell?

Answer: To convert electrical energy into chemical energy. External power source drives non-spontaneous redox reactions.

Flashcard 4: State the function of a power source in an electrolytic cell.

Answer: To provide energy for non-spontaneous reactions. Overcomes negative cell potential of non-spontaneous reactions.

Flashcard 5: Find the cell potential given $E_{cathode} = 0.80$ V and $E_{anode} = 0.40$ V.

Answer: $0.40$ V. Using $E_{cell} = E_{cathode} - E_{anode} = 0.80 - 0.40$.

Flashcard 6: What is the purpose of an external circuit in a galvanic cell?

Answer: To allow electron flow. Completes circuit for electron movement between electrodes.

Flashcard 7: What occurs at the cathode in an electrolytic cell?

Answer: Reduction. Reduction still occurs at cathode regardless of cell type.

Flashcard 8: State the effect of temperature on cell potential.

Answer: Cell potential generally decreases with increasing temperature. Higher temperature typically reduces driving force for reaction.

Flashcard 9: Identify the charge of the anode in a galvanic cell.

Answer: Negative. Loses electrons during oxidation, creating electron excess.

Flashcard 10: What occurs at the cathode in a galvanic cell?

Answer: Reduction. Electrons are gained, making cathode the electron destination.

Flashcard 11: What is the role of the salt bridge in a galvanic cell?

Answer: To maintain electrical neutrality. Allows ion migration to balance charge as reactions proceed.

Flashcard 12: What happens to the mass of the anode in a galvanic cell during operation?

Answer: It decreases. Metal atoms leave electrode as oxidation occurs.

Flashcard 13: What is the primary function of a galvanic cell?

Answer: To convert chemical energy into electrical energy. Spontaneous redox reactions drive electron flow through external circuit.

Flashcard 14: Which metal acts as a reducing agent in a galvanic cell?

Answer: The metal at the anode. Undergoes oxidation, losing electrons to external circuit.

Flashcard 15: What is the standard cell potential $(E^\theta)$ for a galvanic cell?

Answer: Positive. Spontaneous reactions have positive cell potentials.

Flashcard 16: State the effect of temperature on cell potential.

Answer: Cell potential generally decreases with increasing temperature. Higher temperature typically reduces driving force for reaction.

Flashcard 17: What happens to the mass of the anode in a galvanic cell during operation?

Answer: It decreases. Metal atoms leave electrode as oxidation occurs.

Flashcard 18: What is the primary function of a galvanic cell?

Answer: To convert chemical energy into electrical energy. Spontaneous redox reactions drive electron flow through external circuit.

Flashcard 19: What occurs at the anode in a galvanic cell?

Answer: Oxidation. Electrons are lost, making anode the source of electrons.

Flashcard 20: State the relationship between Gibbs free energy and cell potential.

Answer: $\Delta G = -nFE_{cell}$. Links thermodynamic favorability to electrochemical potential.

Flashcard 21: What occurs at the cathode in a galvanic cell?

Answer: Reduction. Electrons are gained, making cathode the electron destination.

Flashcard 22: State the Nernst equation.

Answer: $E = E^\theta - \frac{RT}{nF} \ln Q$. Accounts for concentration effects on cell potential.

Flashcard 23: What occurs at the anode in an electrolytic cell?

Answer: Oxidation. Oxidation still occurs at anode regardless of cell type.

Flashcard 24: State the direction of electron flow in an electrolytic cell.

Answer: From cathode to anode. External power source forces electrons from cathode to anode.

Flashcard 25: What is the main difference between galvanic and electrolytic cells?

Answer: Galvanic cells are spontaneous; electrolytic cells are non-spontaneous. Spontaneity determines whether external power is needed.

Flashcard 26: What does a negative cell potential indicate?

Answer: The reaction is non-spontaneous. External energy required to drive the reaction forward.

Flashcard 27: State the effect of temperature on cell potential.

Answer: Cell potential generally decreases with increasing temperature. Higher temperature typically reduces driving force for reaction.

Flashcard 28: What is the standard cell potential $(E^\theta)$ for a galvanic cell?

Answer: Positive. Spontaneous reactions have positive cell potentials.

Flashcard 29: Which metal acts as a reducing agent in a galvanic cell?

Answer: The metal at the anode. Undergoes oxidation, losing electrons to external circuit.

Flashcard 30: What happens to the mass of the anode in a galvanic cell during operation?

Answer: It decreases. Metal atoms leave electrode as oxidation occurs.