Unit 3: Quantities in Chemical Reactions - Lesson 1: Introduction of the Mole

Vocabulary flashcards covering the concept of the mole, Avogadro's number, atomic mass, molar mass, and multi-step mass-particle conversions.

Mole

A chemical counting unit representing $6.02 \times 10^{23}$ units of a substance, used to quantify microscopic entities like atoms or molecules.

Avogadro's number ($N_A$)

The constant $6.02 \times 10^{23}$ (or $602,000,000,000,000,000,000,000$), representing the number of particles contained in one mole.

Amadeo Avogadro

The scientist in whose honor Avogadro's number is named, who discovered that gases at the same pressure and temperature contain the same number of molecules regardless of the gas type.

Molar Mass

The mass of one mole of a substance expressed in grams per mole ($\text{g/mol}$), which equals the numerical value of its average atomic mass.

Atomic Mass

The average mass of a specific element based on its naturally occurring isotopes, given in units ($\text{u}$).

Molar Mass of a Compound

The sum of the molar masses of all individual elements present in a chemical compound or molecule.

Moles to Particles Formula

The equation used to calculate the number of moles from a given count of particles: $\text{Number of moles} = \frac{\text{Number of particles}}{\text{Avogadro number}}$.

Moles to Mass Formula

The equation used to convert between mass and moles: $\text{number of moles} = \frac{\text{mass (g)}}{\text{molar mass (g per mole)}}$.

Mass to Particles Conversion Process

A two-part calculation process where mass must first be converted to moles using molar mass, and then moles are converted to the number of particles using Avogadro's number.