Lesson-4-Atomic-Mass-Empirical-Formula-and-Molecular-Formula

Atomic Mass Unit (amu)

A unit of mass used to express atomic and molecular masses, defined as one-twelfth the mass of a carbon-12 atom.

Isotope

Atoms of the same element that have different weights due to varying numbers of neutrons.

Molar Mass

The mass of one mole of a substance, reported in grams per mole, equal to its formula weight.

Empirical Formula

The formula of a compound that gives the smallest whole number ratio of atoms in the compound.

Molecular Formula

The true formula of a compound, showing the actual number of atoms of each element in one molecule.

Avogadro's Number

The number of units in one mole of any substance, approximately 6.022 × 10²³.

Percent Composition

The percent by mass of each element in a compound, calculated as (mass of element / molar mass of compound) x 100.

Relative Atomic Mass

The weighted average mass of an atom of an element, taking into account the relative abundances of its isotopes.

Formula Weight

The summation of the atomic weights of the atoms in a compound.

Average Atomic Mass

The average mass of an atom of an element compared to one-twelfth the mass of a carbon-12 atom.