🧪 GCSE Chemistry Revision Newsletter - Moles (Higher Tier)

Part 1 - Keywords:

• Mole (mol)

• Avogadro Constant

• Relative Formula Mass (Mr)

• Particles

• Atoms

• Molecules

• Ions

• Chemical Amount

Part 2 - Key Facts:

• Chemical amounts are measured in moles (symbol = mol).

• One mole of a substance contains 6.02 × 10²³ particles (Avogadro constant).

• The mass of 1 mole of a substance (in grams) is numerically equal to its relative formula mass (Mr).

• This means:

  • 1 mole of carbon atoms (C) (Mr = 12) weighs 12 g and contains 6.02 × 10²³ atoms.

  • 1 mole of CO₂ molecules (Mr = 44) weighs 44 g and contains 6.02 × 10²³ molecules.

• The concept of the mole can apply to:

  • Atoms (e.g., Na atoms)

  • Molecules (e.g., H₂O molecules)

  • Ions (e.g., Na⁺ ions)

  • Electrons, formula units, and equations.

• This allows chemists to count particles in grams, not one by one!

Part 3 - Quick Quiz:

1️⃣ What is the value of the Avogadro constant?
2️⃣ How many atoms are in 1 mole of carbon (C)?
3️⃣ What is the relative formula mass (Mr) of CO₂?
4️⃣ What is the mass of 1 mole of CO₂?
5️⃣ What does the unit “mol” measure?

Part 4 - Answers:

1️⃣ 6.02 × 10²³ particles per mole.
2️⃣ 6.02 × 10²³ atoms.
3️⃣ 44 (12 + 16 + 16).
4️⃣ 44 g.
5️⃣ The amount of substance (number of particles).

Part 5 - Multiple Choice Questions:

1️⃣ The number of particles in one mole of a substance is called:
a) The Relative Atomic Mass
b) The Mass Number
c) The Avogadro Constant
d) The Formula Mass

2️⃣ How many molecules are there in 1 mole of water (H₂O)?
a) 6.02 × 10²³
b) 3.01 × 10²³
c) 1.00 × 10²³
d) 12.04 × 10²³

3️⃣ What is the mass of 1 mole of NaCl? (Na = 23, Cl = 35.5)
a) 35.5 g
b) 58.5 g
c) 23 g
d) 59.5 g

Part 6 - Multiple Choice Answers:

1️⃣ c) The Avogadro Constant
2️⃣ a) 6.02 × 10²³
3️⃣ b) 58.5 g (23 + 35.5 = 58.5)

Part 7 - Going Further:

Question:
Why do chemists use moles instead of counting particles directly?

Answer:
Because particles (atoms and molecules) are extremely small—it would be impossible to count them one by one. Using moles lets chemists easily measure amounts by weighing substances in grams, making calculations and reactions more practical.

Part 8 - Revision Tip:

✔️ Remember this formula:
Mass (g) = Moles × Mr
✔️ Practice calculating the mass of moles for different substances to boost your confidence!

💡 Fun fact:
1 mole of marshmallows (6.02 × 10²³) would cover the entire Earth in a layer thousands of miles deep! 🍬🌍

Part 9 - More Help:

Webpages

1. Moles - GCSE Chemistry Revision Notes
   Save My Exams
   This page provides comprehensive revision notes on the mole concept, including Avogadro's constant and calculations involving mass and moles.
2. Calculations Using Moles Questions and Revision
   MME Revise
   Offers detailed revision materials and practice questions on mole calculations, aiding in understanding and application of the concept.

YouTube Video

• GCSE Chemistry - The Mole (Higher Tier)
  YouTube
  This video explains the term 'mole', Avogadro's constant, and demonstrates example calculations relevant to GCSE Chemistry.

WANT 25% Off GCSE Science And Math Tuition OR Past Paper Revision Resources? Click this link - piacademy.co.uk and use this COUPON CODE - GCSE25.

Stay tuned for the next issue, where we’ll explore another key science concept! ⚗️🧪