Year 10 - Science
The mole
Calculations involving masses
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This pupil-friendly study guide includes a unit summary, clear notes, common mistakes, and quick questions with answers.
Unit Summary
This unit covers writing chemical formulae, balancing equations, and using the conservation of mass. It includes calculating moles, empirical formulae, relative formula masses, and theoretical yields. Emphasis is on stoichiometry, concentration, gas volumes, and using standard form.
Lesson Summary
You will learn to describe what a mole is and its link with the Avogadro constant.
Key Notes
- Chemical amounts are measured in moles (mol).
- One mole of particles of a substance is defined as the Avogadro constant number of particles.
- The number of particles (atoms, ions, molecules etc.) in one mole of a substance is always the same.
- Use of Avogadro's number to calculate the number of particles of substance when number of moles is known and vice versa.
- The mass of one mole of a monatomic element is equal to the relative atomic mass of that element measured in grams.
Vocabulary To Learn
- mole: A mole of something is 6.02 × 10²³ of it. The mass of a mole of a substance is its relative mass expressed in grams.
- relative formula mass: The relative formula mass (RFM) of a substance is the sum of the relative atomic masses of all the atoms in a formula.
- Avogadro's constant: Avogadro's constant is the number of particles in one mole of a substance (6.02 × 10²³ mol⁻¹)
Common Mistakes To Avoid
- The number one mole represents can be difficult for pupils to grasp and appreciate.
3 Quick Questions (With Answers)
1. Explain the scientific idea in this lesson using two key points.
Chemical amounts are measured in moles (mol). One mole of particles of a substance is defined as the Avogadro constant number of particles.
2. Define this scientific word and use it in context. 'mole'
A mole of something is 6.02 × 10²³ of it. The mass of a mole of a substance is its relative mass expressed in grams. Include the word in a full scientific explanation, not as a single label.
3. Correct this common scientific misunderstanding.
Mistake: The number one mole represents can be difficult for pupils to grasp and appreciate. Correction: Show many real world examples of 6.02 × 10²³ examples of something - that many basketballs would form a planet the size of the Earth.
More Lessons In This Unit
- Balancing equations Study Guide
- Conservation of mass Study Guide
- Converting between mass and volume using moles Study Guide
- Converting between mass and volume using moles (RAM 1 d.p.) Study Guide
- Deducing an empirical formula experimentally Study Guide
- Deducing an empirical formula experimentally: using moles Study Guide
- Determining an equation experimentally: magnesium oxide Study Guide
- Determining an equation experimentally: magnesium oxide (RAM 1 d.p.) Study Guide
- Determining an equation experimentally: sodium hydrogencarbonate Study Guide
- Determining an equation experimentally: sodium hydrogencarbonate (RAM 1 d.p.) Study Guide
- Determining an equation from given values Study Guide
- Determining an equation from given values (RAM 1 d.p.) Study Guide
- Empirical formula calculations Study Guide
- Empirical formula calculations: using moles Study Guide
- Gas volumes Study Guide
- Gas volumes (RAM 1 d.p.) Study Guide
- Limiting reactants Study Guide
- Limiting reactants (RAM 1 d.p.) Study Guide
- Mass in a chemical reaction Study Guide
- Mass in a chemical reaction (RAM 1 d.p.) Study Guide
- Mass in a chemical reaction: using moles Study Guide
- Mass in a chemical reaction: using moles (RAM 1 d.p.) Study Guide
- Moles and masses Study Guide
- Moles and masses (RAM 1 d.p.) Study Guide
- Representations of a mole Study Guide
- Representations of a mole (RAM 1 d.p.) Study Guide
- The mole (RAM 1 d.p.) Study Guide
- Three types of chemical reaction Study Guide
- Uncertainties in measurements: chemistry Study Guide
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