Formula Mass and Mole Concepts of Compounds

Molecular mass is the sum of atomic masses of all atoms in a chemical formula, measured in atomic mass units (amu). Molar mass is the mass of one mole of a compound, measured in grams per mole (g/mol). The numerical values are equal; for example, sucrose has a molecular mass of 342.3 amu and a molar mass of 342.3 g/mol.

Use the relationship that one mole of any compound contains 6.022 × 10²³ particles. First, divide the sample mass by the molar mass to find moles, then multiply by Avogadro's number. For example, 150 grams of sucrose (molar mass 342.3 g/mol) equals 2.63 × 10²³ molecules.

Both ionic and covalent formula masses are calculated by summing the average atomic masses of all atoms in the chemical formula. However, for ionic compounds, the formula does not represent a discrete molecule but rather the ratio of cations and anions. For covalent compounds like chloroform (CHCl₃), the formula represents a single molecule.

Mass percent composition shows the relative abundance of each element in a compound. It is calculated by dividing the total mass of an element in one mole of the compound by the total molar mass, then converting to a percentage. For sucrose, hydrogen comprises 6.4 mass percent of the compound.

The electron mass is negligibly small compared to atomic mass, so it is ignored in formula mass calculations. Although sodium cations are slightly lighter than sodium atoms and chloride anions are slightly heavier than chlorine atoms, these differences offset each other. Therefore, average atomic masses of neutral atoms are used for ionic compounds.

A chemical formula represents the smallest representative unit of a compound, which is either a molecule (for covalent compounds) or a formula unit (for ionic compounds). The formula shows the types and numbers of atoms or ions present. Adding the atomic masses of all atoms in the formula gives the molecular or formula mass.

Counting individual molecules by ordinary means is impractical because compounds contain enormous numbers of particles. The mole concept solves this by establishing that one mole of any compound contains exactly 6.022 × 10²³ particles. This allows chemists to relate measurable mass quantities to the number of molecules or particles present in a sample.