Unit 3 Chemistry: Equilibrium, Acids, and Redox Reactions

These flashcards cover key vocabulary and concepts from Unit 3 Chemistry, which includes topics on equilibrium, acids, and redox reactions.

Redox Reactions

A type of chemical reaction where the oxidation states of atoms are changed; it involves the transfer of electrons.

Oxidation

The loss of electrons from a chemical species.

Reduction

The gain of electrons by a chemical species.

Oxidation Number

A number that is assigned to an atom in a compound to represent the number of electrons that atom can gain, lose, or share.

OIL RIG

Mnemonic for Oxidation Is Loss and Reduction Is Gain.

Electrochemical Cell

A device that uses redox reactions to create electricity.

Half-Reaction

The equation that shows only the oxidation or reduction part of a redox reaction.

Standard Electrode Potential (SEP)

A measure of the tendency of a chemical species to be reduced, expressed in volts.

Dynamic Equilibrium

A state in which the forward and reverse reactions occur at the same rate, leading to constant concentrations of reactants and products.

Le Chatelier's Principle

If a system at equilibrium is subjected to change in concentration, pressure, or temperature, the system shifts to counteract the change.

Bronsted-Lowry Acid

A substance that donates protons (H+ ions) in a chemical reaction.

Amphiprotic Species

A substance that can both accept and donate protons.

Dissociation Constant (Ka)

An equilibrium constant that measures the strength of an acid in solution.

Equilibrium Constant (Kc)

A constant that indicates the ratio of concentrations of products to reactants at equilibrium.

Electrolysis

The process of driving a non-spontaneous redox reaction using an external electrical energy source.

Galvanic Cell

An electrochemical cell that generates electrical energy from spontaneous chemical reactions.

Buffer Solution

A solution that resists changes in pH when small amounts of acid or base are added.