Quantitative Aspects: The Mole: Concept Map

≈ 30 min

Concept Map

Organise the vocabulary, quantities and relationships into a connected model.

This extension applies that lens specifically to Quantitative Aspects: The Mole.

Atoms are far too small and numerous to count one by one, so chemists count them in a big fixed bundle called the mole (mol).

One mole is $6{,}022 \times 10^{23}$ particles (Avogadro's number) — just as 'a dozen' always means 12.
The molar mass ( $M$ ) of a substance is the mass of one mole, in grams per mole ( $\text{g·mol}^{-1}$ ). You read it off the periodic table: carbon is $12\ \text{g·mol}^{-1}$ ; for a compound, add up the atoms — water $\text{H}_2\text{O}$ is $2(1) + 16 = 18\ \text{g·mol}^{-1}$ .

The key formula links number of moles ( $n$ ), mass ( $m$ ) and molar mass ( $M$ ):

n = \frac{m}{M}

Worked example: how many moles are in $36\ \text{g}$ of water? $n = \frac{36}{18} = 2\ \text{mol}$ .

Chemistry — Grade 10 — Concept Map: The molar mass of water is $18\ \text{g·mol}^{-1}$ . How many moles are in $54\ \text{g}$ of water?

Chemistry — Grade 10 — Concept Map: Carbon has a molar mass of $12\ \text{g·mol}^{-1}$ . What is the mass (in grams) of $2\ \text{mol}$ of carbon?

Chemistry — Grade 10 — Concept Map: Approximately how many particles are in one mole of any substance?

$1\,000$

$6{,}022 \times 10^{23}$

$100$

$12$

Name the original topic being extended by this concept map lesson.

Which statement is the best evidence-led starting point for Quantitative Aspects: The Mole: Concept Map?

Atoms are far too small and numerous to count one by one, so chemists count them in a big fixed bundle called the mole (mol). - One mole is $6{,}022 \times 10^{23}$ particles (Avogadro's number) — just as 'a dozen' always means 12. - The molar mass ( $M$ ) of a substance is the mass of one mole, in grams per mole ( $\text{g·mol}^{-1}$ ). You read it

Pure Substances and Mixtures

Elements and Compounds

A conclusion needs no observations, calculations or stated assumptions.