Honors Chemistry Final Review: Ionic and Covalent Compounds

Delocalized Electrons

Electrons that are free to move in metals

Oxidation Number

For a monatomic ion, is equal to the charge

Chemical Bond

The force that holds two atoms together

Polyatomic Ion

A charged particle containing more than one atom

Cation

A positively charged ion

Anion

A negatively charged ion

Electrolyte

An ionic compound whose aqueous solution conducts electricity

Salt

The name for most ionic compounds other than oxides

Electron Sea Model

Represents the way electrons exist in metals

Monatomic Ion

A charged particle containing only one atom

Lattice Energy

The energy needed to separate the ions of an ionic compound

Ionic Bond

The electrostatic force that holds oppositely charged particles together

Alloy

A mixture of elements that has metallic properties

Interstitial Alloy

A mixture formed when small atoms fill holes in a metallic crystal

Oxyanion

A polyatomic ion composed of an element bonded to at least one oxygen atom

Formula Unit

Shows the simplest ratio of ions in an ionic compound

Metallic Bond

The attraction of a metallic cation for delocalized electrons

A reaction in which a compound breaks down into two or more elements or new compounds

Decomposition reaction.

A number written in front of a chemical formula

Coefficient.

A solid produced during a chemical reaction in a solution

Precipitate.

A solution in which the solvent is water

Aqueous solution.

A statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a chemical reaction

Chemical equation.

An equation that shows all of the particles in solution as they actually exist

Complete ionic equation.

Substance dissolved in a solution

Solute.

An equation that includes only the particles that participate in the reaction

Net ionic equation.

An ion that is present but does not participate in a reaction

Spectator ion.

A reaction in which oxygen combines with a substance and releases heat and light energy

Combustion reaction.

A reaction in which the atoms of one element replace the atoms of another element in a compound

Single-replacement reaction.

A reaction involving the exchange of two elements

Double-replacement reaction.

The process by which the atoms of one or more substances are rearranged to form different substances

Chemical reaction.

A starting substance in a chemical reaction

Reactant.

A substance formed during a chemical reaction

Product.

A reaction in which two or more substances react to produce a single product

Synthesis reaction.

Avogadro's Number

6.02 × 10^23

Empirical Formula

Formula of a compound with the smallest whole-number mole ratio of the elements.

Molar Mass

Mass in grams of one mole of any pure substance.

Molecular Formula

Specifies the actual number of atoms of each element in one molecule of a compound.

Percent Composition

Percent by mass of each element in a compound.

actual yield

The amount of product actually produced by a chemical reaction.

mole ratio

A ratio between the number of moles of any two substances in a balanced chemical equation.

excess reactant

A reactant that has a portion remaining after the reaction has stopped.

theoretical yield

The maximum amount of product that can be produced from a given amount of reactant.

stoichiometry

The study of the quantitative relationships among the amounts of reactants used and the amounts of products formed by a chemical reaction.

percent yield

The ratio of the actual yield to the theoretical yield expressed as a percent.

Limiting Reactants

The reactant that is completely consumed in a chemical reaction, limiting the amount of product formed.

Excess Reactant Calculation

After the reaction, the amount of excess reactant left over can be calculated.

Gas Laws

Describes the relationships between pressure, volume, and temperature of gases.

Boyle's Law

At constant temperature, the pressure of a gas is inversely proportional to its volume.

Charles's Law

At constant pressure, the volume of a gas is directly proportional to its temperature in Kelvin.

Combined Gas Law

P1V1/T1 = P2V2/T2; relates pressure, volume, and temperature of a gas.