Chemistry Units 4.1 - 4.5: Chemical Reactions and Stoichiometry

Vocabulary flashcards covering physical vs. chemical changes, types of chemical equations, particulate diagrams, dissolution, and stoichiometry fundamentals.

Physical change

A change in appearance, not chemical composition (examples include melting, shredding, boiling, and chopping).

Chemical change

A change in chemical composition where bonds are broken to form new bonds.

Signs of chemical change

Four indicators that a chemical change has occurred: production of heat/light, formation of gas (bubbles), formation of precipitate (solid), and color change.

Law of Conservation of Mass

A principle stating that there must be the same number of atoms of each element on both sides of a chemical reaction.

Balanced chemical equation (molecular equation)

A chemical equation in which all reactants and products are represented.

Complete ionic equation

A chemical equation in which all ions in an aqueous compound are represented, including ionic charges.

Net ionic equation

A chemical equation that includes only the species directly involved in the chemical reaction.

Particulate diagram

A visual representation showing atoms and states of matter.

Physical process

A process involving a change in intermolecular forces.

Chemical process

The breaking and/or formation of chemical bonds.

Dissolution (dissolving)

A process that is both physical and chemical: physical because it is reversible by evaporation, and chemical due to the breaking of ionic bonds.

Stoichiometry

Used to predict the amount of products produced or the amount of reactants required for a reaction to occur.

Limiting reactant

The reactant that runs out first during a chemical reaction.

Excess reactant

The reactant that is leftover after a chemical reaction is complete.

Theoretical yield

The amount of product predicted theoretically, assuming none is lost in the process.

Actual yield

The actual amount of product being produced.