Atomic Structure, Avogadro's Number, and Mole Conversions Vocabulary

Vocabulary flashcards reviewing core concepts, definitions, and conversions related to atomic structure, Avogadro's number, molar mass, and the mole.

Mole

The amount of a substance that contains the same number of particles as exactly $12\text{ g}$ of carbon-12, equal to $6.022 \times 10^{23}$ particles.

Avogadro's Number

$6.022 \times 10^{23}$ particles; the number of particles (such as atoms, molecules, or ions) that make up exactly one mole of a substance.

Amedeo Avogadro

The scientist whose work forms the basis for Avogadro's number ($6.022 \times 10^{23}$ particles per mole).

Molar Mass

The mass in grams of one mole of a substance ($x\text{ grams} = 1\text{ mole}$), where $x$ is the mass obtained from the periodic table.

Mole Highway

A conceptual diagram showing that conversions between the number of particles and mass must always route through moles first.

Atomic Mass Unit (amu)

A unit of mass used to express atomic weight, where the average mass of one single atom of carbon is $12.011\text{ amu}$, while one mole of carbon atoms weighs $12.011\text{ g}$.

Particles

Microscopic constituents of matter, specifically atoms, molecules, and ions, which are counted in chemistry using the mole.

Avogadro's Conversion Factors

The operational conversion ratios $\frac{6.022 \times 10^{23}\text{ atoms}}{1\text{ mol}}$ and $\frac{1\text{ mol}}{6.022 \times 10^{23}\text{ atoms}}$ used to convert between particle counts and moles.