Introduction to Electrochemistry Practice Flashcards

A set of vocabulary flashcards covering the fundamental concepts of electrochemistry, including redox definitions, cell types, and balancing methods.

Electrochemistry

The study of the relationship between electricity and chemical reactions.

Oxidation (Electronic definition)

A process in which electrons are lost by particles of a substance, resulting in an increase in oxidation numbers.

Reduction (Electronic definition)

A process in which electrons are gained by particles of a substance, resulting in a decrease in oxidation number.

Oxidation (Classical definition)

An increase in the oxygen content of particles of a substance.

Reduction (Classical definition)

A decrease in the oxygen content of particles of a substance.

Oxidation Number

A formal charge on atoms in chemical formulas of particles of substances calculated according to a set of rules, where neutral compounds equal $0$ and polyatomic ions equal the ion charge.

Redox Reaction

A chemical reaction that occurs through a simultaneous transfer of electrons from one species to another.

Oxidizing reagent (Oxidant)

A substance that gains electrons from another reagent during a reaction, thereby oxidizing it.

Reducing reagent (Reductant)

A substance that loses electrons to another reagent during a reaction, thereby reducing it.

Ionic Method

A method of balancing redox equations that focuses on balancing the individual oxidation and reduction half-reactions.

Oxidation State Method

A method of balancing redox equations that uses the change in oxidation numbers to ensure total electrons lost equals total electrons gained.

Electrochemical Cell

A system consisting of electrodes in contact with electrolytes that generates electrical energy from chemical reactions or uses supplied electrical energy to facilitate chemical reactions.

Voltaic (Galvanic) Cell

An electrochemical cell in which a spontaneous redox reaction generates electric current.

Electrolytic Cell

An electrochemical cell in which an electric current is used to cause a chemical change or drive a nonspontaneous reaction.

Anode

The electrode at which oxidation occurs; in a voltaic cell, it is the negative electrode.

Cathode

The electrode at which reduction occurs; in a voltaic cell, it is the positive electrode.

Salt Bridge

A tube consisting of electrolyte in a gel that allows the migration of ions to maintain charge balance while preventing the mixing of half-cell solutions.

Cell EMF (Electromotive Force)

The maximum potential difference between two electrodes, representing the maximum voltage produced by a voltaic cell, measured in Volts ($V$).

Standard Electrode Potential ($E^\circ$)

The electrode potential when solute concentrations are $1\,M$, gas pressures are $1\,atm$, and the temperature is at a specified value, usually $25^\circ C$.

Electrolysis

The process of producing a chemical change in an electrolytic cell by driving an electric current through it.

Down’s Cell

An electrolytic cell used to obtain sodium metal through the electrolysis of molten sodium chloride.