Types of Chemical Reactions and Balancing Equations

These flashcards cover key concepts related to types of chemical reactions, equations, solubility rules, oxidation states, and redox reactions.

Single Replacement Reaction

A reaction where one element replaces another in a compound, e.g. A + BC -> B + AC.

Double Replacement Reaction

A reaction where two compounds exchange components, e.g. AB + CD -> AD + CB.

Synthesis Reaction

A reaction where two or more reactants combine to form a single product, e.g. A + B -> AB.

Decomposition Reaction

A reaction where a single compound breaks down into two or more products, e.g. AB -> A + B.

Neutralization Reaction

A reaction between an acid and a base resulting in water and a salt, e.g. H+ (aq) + OH- (aq) -> H2O (l).

Combustion Reaction

A reaction where a fuel combines with oxygen to produce carbon dioxide and water, e.g. HC + O2 -> CO2 + H2O.

Molecular Equation

An equation that shows the complete formulas of reactants and products without indicating dissociation in solution.

Complete Ionic Equation

An equation that shows all soluble ionic substances as dissociated ions.

Net Ionic Equation

An equation that shows only the species that actually change during the reaction.

Spectator Ions

Ions that do not participate in a reaction and remain unchanged in solution.

Solubility Rule

A guideline stating whether a substance is soluble or insoluble in water.

Oxidation Number

A value that represents the number of electrons lost or gained by an atom in a compound.

Reducing Agent

The element that loses electrons and is oxidized in a redox reaction.

Oxidizing Agent

The element that gains electrons and is reduced in a redox reaction.

Redox Reaction

A reaction in which one substance is oxidized (loses electrons) and another is reduced (gains electrons).

Activity Series

A list of metals arranged in order of decreasing reactivity; used to predict whether a single replacement reaction will occur.