Chapter 4: Reactions in Aqueous Solutions

A set of vocabulary flashcards covering key concepts, terms, and definitions related to reactions in aqueous solutions.

Solution

A homogeneous mixture of two or more pure substances.

Solvent

The substance present in the greatest abundance in a solution.

Solute

All other substances in a solution apart from the solvent.

Polar Molecule

A molecule with an unequal charge distribution, having a partial negative charge on one end and partial positive charges on the other.

Dissociation

The process by which water pulls individual ions from ionic substances and solvates them.

Electrolyte

A substance that dissociates into ions when dissolved in water.

Nonelectrolyte

A substance that may dissolve in water but does not dissociate into ions.

Strong Electrolyte

A substance that completely dissociates into ions when dissolved in water.

Weak Electrolyte

A substance that only partially dissociates into ions when dissolved in water.

Acid (Arrhenius Definition)

A substance that increases the concentration of H+ ions in solution.

Base (Arrhenius Definition)

A substance that increases the concentration of OH- ions in solution.

Net Ionic Equation

An equation that shows only the species that undergo a chemical reaction, excluding spectator ions.

Precipitate

An insoluble solid formed from a reaction in solution.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Oxidation-Reduction Reaction (Redox)

A reaction where electrons are transferred from one atom or ion to another.

Oxidation Number

A number assigned to an element in a compound that reflects its loss or gain of electrons.

Solution

A homogeneous mixture of two or more pure substances.

Solvent

The substance present in the greatest abundance in a solution.

Solute

All other substances in a solution apart from the solvent.

Polar Molecule

A molecule with an unequal charge distribution, having a partial negative charge on one end and partial positive charges on the other.

Dissociation

The process by which water pulls individual ions from ionic substances and solvates them.

Electrolyte

A substance that dissociates into ions when dissolved in water.

Nonelectrolyte

A substance that may dissolve in water but does not dissociate into ions.

Strong Electrolyte

A substance that completely dissociates into ions when dissolved in water.

Weak Electrolyte

A substance that only partially dissociates into ions when dissolved in water.

Acid (Arrhenius Definition)

A substance that increases the concentration of H^+ ions in solution.

Base (Arrhenius Definition)

A substance that increases the concentration of OH^- ions in solution.

Net Ionic Equation

An equation that shows only the species that undergo a chemical reaction, excluding spectator ions.

Precipitate

An insoluble solid formed from a reaction in solution.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Oxidation-Reduction Reaction (Redox)

A reaction where electrons are transferred from one atom or ion to another.

Oxidation Number

A number assigned to an element in a compound that reflects its loss or gain of electrons.

Molarity

The concentration unit defined as the number of moles of solute per liter of solution.

Spectator Ions

Ions that are present in both the reactant and product sides of a reaction but do not participate in the chemical reaction itself.

Oxidizing Agent

The species that causes oxidation by accepting electrons, and is itself reduced.

Reducing Agent

The species that causes reduction by donating electrons, and is itself oxidized.

Precipitation Reaction

A reaction in which two soluble ionic compounds react to form an insoluble product (precipitate).

Solubility Rules

A set of guidelines used to predict whether an ionic compound will be soluble or insoluble in water.

Acid (Brønsted-Lowry Definition)

A proton (H^+) donor.

Base (Brønsted-Lowry Definition)

A proton (H^+) acceptor.