Chapter_7

Mole

A counting term that states a specific number of items; 1 mole = 6.02 × 10^23 items.

Avogadro's number

The number of particles in one mole, equal to 6.02 × 10^23.

Balanced chemical equation

A chemical equation where the number of atoms on the reactant and product sides is equal.

Molar mass

The mass of one mole of an element or compound, typically expressed in grams.

Combustion reaction

A chemical reaction in which a carbon-containing compound burns in oxygen to produce carbon dioxide and water.

Oxidation

Loss of electrons in a chemical reaction.

Reduction

Gain of electrons in a chemical reaction.

Exothermic reaction

A reaction that releases heat energy.

Endothermic reaction

A reaction that absorbs heat energy.

Law of Conservation of Mass

In a chemical reaction, matter cannot be created or destroyed; the total mass of reactants equals the total mass of products.

Chemical changes

Changes that result in the formation of new chemical substances.

Significant figures

Digits in a number that are meaningful in terms of accuracy and precision.

Conversion factor

A ratio used to convert between different units.

Reaction rate

The speed at which a chemical reaction occurs, dependent on factors like temperature and concentration.

Catalyst

A substance that increases the rate of a reaction by lowering the energy of activation without being consumed in the process.

Mole-mole factor

A ratio of the moles of two substances in a balanced chemical equation, used to convert between them.

Core Chemistry Skill

Essential techniques and knowledge required in chemistry, such as calculating molar mass or balancing equations.

Chemical equation

A representation of a chemical reaction using symbols and formulas.

Oxidation-Reduction Reactions

Reactions that involve the transfer of electrons between species.

Double replacement reaction

A reaction where two compounds exchange ions or bonds to form different compounds.

Single replacement reaction

A reaction in which one element replaces another element in a compound.

Decomposition reaction

A reaction where one compound breaks down into two or more simpler substances.

Combination reaction

A reaction where two or more substances combine to form a single product.

Miscible

Describes two liquids that can mix together in all proportions.

Buffer solution

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

Aqueous solution

A solution in which the solvent is water.

Spectator ions

Ions that exist in the same form on both sides of a chemical equation.

Hydrocarbon

Compounds composed entirely of hydrogen and carbon.

Saturation point

The point at which a solution can no longer dissolve additional solute.

Isomer

Compounds with the same molecular formula but different arrangements of atoms.

Stoichiometry

The calculation of reactants and products in chemical reactions.

Activation energy

The minimum energy required for a chemical reaction to occur.

Equilibrium

A state in which the forward and reverse reactions occur at the same rate, establishing a balance.

Titration

A technique used to determine the concentration of a solution by reacting it with a solution of known concentration.

Electrolyte

A substance that dissociates into ions in solution and can conduct electricity.

Precipitate

A solid that forms from a solution during a chemical reaction.

Dilution

The process of reducing the concentration of a solute in a solution, typically by adding more solvent.

pH scale

A scale used to measure the acidity or basicity of a solution, ranging from 0 (acidic) to 14 (basic).

Saponification

The process of making soap from fats or oils and an alkali.

Hydrolysis

A chemical reaction involving the breaking of a bond in a compound by the addition of water.