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

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10 Terms

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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.
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Isotope
Atoms of the same element that have different weights due to varying numbers of neutrons.
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Molar Mass
The mass of one mole of a substance, reported in grams per mole, equal to its formula weight.
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Empirical Formula
The formula of a compound that gives the smallest whole number ratio of atoms in the compound.
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Molecular Formula
The true formula of a compound, showing the actual number of atoms of each element in one molecule.
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Avogadro's Number
The number of units in one mole of any substance, approximately 6.022 × 10²³.
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Percent Composition
The percent by mass of each element in a compound, calculated as (mass of element / molar mass of compound) x 100.
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Relative Atomic Mass
The weighted average mass of an atom of an element, taking into account the relative abundances of its isotopes.
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Formula Weight
The summation of the atomic weights of the atoms in a compound.
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Average Atomic Mass
The average mass of an atom of an element compared to one-twelfth the mass of a carbon-12 atom.