Stoichiometry-to measure the elements

Chemical formulas-symbolic representations that specify the elements present in a compound

Molecular compounds-composed of molecules=groups of two or more atoms

Ionic compounds-composed of a vast array of ions=electrically charged particles

Molecular formula-tells how many of each type of atom

Empirical formula-shows only the simplest ratio of atoms in a compound

Formula unit-the simplest ratio of atom in an ionic compound / the smallest division of an ionic compound

Simple cations-cations formed by simply removing one or more electrons from an atom

Simple anions-adding one or more electrons

Polyatomic ions-several atoms that act as a single ion

Molecular mass-the sum of the atomic masses of all the atoms in the formula of the compound

Avogadro’s number-6.022×10²³

Mole-the amount of a substance containing the same number of particles as exactly 12g of carbon-12

Molar mass-

Percent composition-the composistion of a compound given in percents by mass

Chemical equation-a symbolic representation of a chemical reaction

Reactants-on left

Products-on right

Law of conservation of mass-the sum of the masses of the products is always equal to the sum of the masses of the reactants

Limiting reactant-determines how much product can be formed

Mole ratio-a conversion factor that compares the amounts of any two substances involved in a chemical reaction