Chemical Equations & Reactions

These flashcards cover key vocabulary terms related to chemical equations and reactions, providing definitions to aid in understanding and memorization.

Chemical Reaction

A process in which reactants undergo a transformation to form products.

Stoichiometric Coefficients

Numbers in front of chemical formulas in an equation that indicate the relative amounts of reactants and products.

Conservation of Matter

A principle stating that in a closed system, the total mass must remain constant; hence, chemical equations must be balanced.

Diatomic Molecules

Molecules consisting of exactly two atoms of the same element, such as O2 or H2.

Reactants

Substances that exist before a chemical reaction takes place.

Products

New substances formed as a result of a chemical reaction.

Balanced Equation

An equation in which the number of atoms of each element is the same on both sides.

Synthesis Reaction

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

Decomposition Reaction

A reaction in which a single compound breaks down into two or more simpler products.

Single-Replacement Reaction

A reaction where one element replaces another in a compound.

Double-Replacement Reaction

A reaction that involves the exchange of ions between two compounds.

Combustion Reaction

A reaction in which a hydrocarbon reacts with oxygen to produce carbon dioxide and water.

Complete Ionic Equation

An equation that shows all of the species present in a reaction, including ions.

Net Ionic Equation

An equation that shows only the particles that participate in the reaction, omitting spectator ions.

Spectator Ions

Ions that do not undergo a change during the reaction and are not included in the net ionic equation.

Solubility Rules

Guidelines used to determine whether a compound will dissolve in water.