Chemistry Chapter 13: Cells and Batteries

Solid conductors that allow electrons to flow in and out of a solution during a redox reaction.

The conducting solution that allows ions to move between the half-cells, maintaining neutrality.

A U-shaped tube filled with a salt solution that connects the two half-cells, preventing charge buildup.

The electrode where oxidation occurs, losing electrons and decreasing in mass.

The electrode where reduction occurs, gaining electrons and increasing in mass.

A process that uses a specific set of steps to design a spontaneous redox reaction and build a voltaic cell.

Describes a redox reaction that occurs spontaneously in a voltaic cell.

The standard half-reaction that involves the reduction of the oxidizing agent.

The standard half-reaction that involves the oxidation of the reducing agent.

An electrode made from a material that does not participate in the reaction but provides a surface for electron transfer.

A type of electrochemical cell that generates electrical energy from spontaneous chemical reactions.

An electrode that is made of a material that participates in the electrochemical reaction.

The flow of electrons from the anode to the cathode.

The movement of ions through the electrolyte solution to maintain charge balance.

A type of electrochemical cell where chemical energy is converted into electrical energy.

A type of chemical reaction involving the transfer of electrons between reactants.

The process by which metals react with substances in their environment, leading to deterioration.

A protective layer of zinc applied to iron to prevent corrosion.

The process by which a metal becomes the anode in a voltaic cell, sacrificing itself to protect another metal from corrosion.

A method of corrosion prevention where a sacrificial anode is attached to the object to be protected.

A method of corrosion prevention that involves coating the metal surface with a protective layer.

The process of applying a layer of metal over another metal to create a protective barrier.

A material that doesn't corrode easily and forms a protective oxide layer.

A chemical reaction involving the transfer of electrons from one substance to another.

The overpotential is the additional voltage required to overcome the activation energy barrier for a reaction to occur at an electrode. In other words, it's the extra 'push' needed to start the reaction.

In electrolysis of aqueous solutions, water can act as both an oxidizing agent (OA) and reducing agent (RA). The overpotential of water affects the overall reaction by making chlorine the strongest reducing agent.

The Chloride Anomaly: In electrolysis of aqueous sodium chloride solution, chlorine becomes the dominant reducing agent due to overpotential affecting water's reducing ability. This means chlorine is more likely to be reduced, even though sodium would be expected based on standard reduction potentials.

The Chloride Anomaly demonstrates that overpotential can significantly alter the outcome of electrolysis. Standard reduction potentials might not predict the actual reaction, as overpotential can change the strength of oxidizing and reducing agents.

The overpotential of water is approximately 0.6V, making it a weaker reducing agent in electrolysis. This allows chlorine to dominate as the strongest reducing agent in electrolysis of chloride solutions.

A cell that utilizes external electrical energy to drive a non-spontaneous redox reaction.

The minimum voltage required to initiate and sustain an electrolytic reaction.

The cell potential for the reverse reaction (electrolytic) is the opposite sign and magnitude of the spontaneous reaction (voltaic).

The negative cell potential indicates that the reaction is not spontaneous and requires external energy input to proceed.

The anode in an electrolytic cell is where oxidation occurs, unlike in a voltaic cell.

The cathode in an electrolytic cell is where reduction occurs, unlike in a voltaic cell.

The direction of electron flow in an electrolytic cell is opposite to the direction in a voltaic cell, moving from the external power source to the cathode.

In an electrolytic cell, the positive terminal of the external power source is connected to the anode, while the negative terminal is connected to the cathode.

The electrode where reduction occurs is called the cathode in both voltaic and electrolytic cells.