AP Chemistry Unit 4 Vocabulary

A process in which atoms are rearranged as chemical bonds break and form, producing substances with different chemical identities.

A substance consumed or transformed during a chemical reaction, written on the left side of a chemical equation.

A substance formed by a chemical reaction, written on the right side of a chemical equation.

A symbolic representation of a chemical reaction showing reactants, products, and their relative stoichiometric amounts.

An equation with equal numbers of atoms of each element on both sides, consistent with conservation of matter.

A number placed before a chemical formula indicating the relative number of particles or moles involved in a balanced reaction.

A number indicating how many atoms of an element occur in a formula unit or molecule; changing it changes the chemical formula.

In a closed system, total mass remains constant during a chemical reaction because atoms are rearranged rather than created or destroyed.

An equation showing dissolved strong electrolytes as their constituent ions while retaining substances that do not dissociate completely in ionic form.

An equation showing only the species that participate in the chemical change, with spectator ions removed.

An ion that appears unchanged on both sides of a complete ionic equation and is omitted from the net ionic equation.

A substance that produces mobile ions when dissolved in water or melted, allowing the resulting solution or liquid to conduct electricity.

A substance that produces ions essentially completely in aqueous solution, such as a soluble ionic salt or strong acid.

A substance that produces relatively few ions in aqueous solution because ionization is incomplete, such as a weak acid.

A substance that dissolves without producing significant concentrations of ions and therefore contributes little to electrical conductivity.

A reaction in which dissolved species combine to form an insoluble solid.

An insoluble solid formed from substances initially present in solution.

A substance is dissolved in water; the notation alone does not establish whether the dissolved substance is ionized.

The substance is in the solid state.

The substance is in the liquid state.

The substance is in the gaseous state.

A change in physical form or state without changing the chemical identity of the substance.

A process that changes chemical identities through rearrangement of atoms and chemical bonds.

The quantitative study of relationships among reactants and products using the coefficients of balanced chemical equations.

The ratio of stoichiometric coefficients that relates amounts of two substances in a balanced chemical equation.

The reactant consumed first according to the reaction stoichiometry, determining the maximum amount of product that can form.

A reactant present in more than the stoichiometric amount required to consume the limiting reactant.

The maximum amount of product predicted from the limiting reactant, assuming complete reaction and no product losses.

The amount of product actually obtained in an experiment.

The actual yield divided by the theoretical yield, multiplied by 100%.

An analytical procedure in which a solution of known concentration reacts with an analyte to determine an unknown quantity, commonly concentration.

The solution delivered during a titration, usually from a buret, to react with the analyte.

The substance being analyzed, whose amount or concentration is being determined.

The point at which the added titrant and analyte have reacted in the exact stoichiometric ratio specified by the balanced equation.

The experimentally observed signal, such as an indicator color change, used to estimate the equivalence point.

A species that donates a proton, H+, to another species.

A species that accepts a proton, H+, from another species.

A reaction involving transfer of a proton from an acid to a base.

Two species that differ by exactly one proton, with the acid containing one more H+ than its conjugate base.

A chemical reaction involving electron transfer, reflected in changes in oxidation numbers.

Loss of electrons by a species, corresponding to an increase in oxidation number.

Gain of electrons by a species, corresponding to a decrease in oxidation number.

A species that causes another species to be oxidized by accepting electrons; the oxidizing agent is itself reduced.

A species that causes another species to be reduced by donating electrons; the reducing agent is itself oxidized.

A formal charge assigned to an atom using electron-accounting rules to track oxidation and reduction in chemical reactions.