🎯 Common Question Types:
- Write the equation for an alkali metal reacting with water (2 marks)
- Describe observations when sodium/potassium is added to water (3 marks)
- Explain why reactivity increases going down Group 1 (3 marks)
- Compare properties of alkali metals with transition metals (4 marks)
📝 Key Command Words:
- Describe: State what you would see — fizzing, floating, melting, flame colour
- Explain: Link to outer electrons — distance from nucleus, shielding
- Write: Give word or symbol equation (remember to balance)
- Predict: Use the trend to forecast behaviour of rubidium or caesium
⚠️ Common Mistakes to Avoid:
- Saying reactivity decreases down Group 1 — it INCREASES
- Forgetting the products are hydroxide AND hydrogen (not just one)
- Not balancing the equation (2Na + 2H₂O → 2NaOH + H₂)
- Describing alkali metals as hard or dense — they are soft and low density
This exam tips covers Exam Tips — Alkali Metals within Group 1: Alkali Metals for GCSE Chemistry. Revise Group 1: Alkali Metals in Atomic Structure for GCSE Chemistry with 22 exam-style questions and 20 flashcards. This topic appears less often, but it can still be a useful differentiator on mixed-topic papers. It is section 11 of 13 in this topic. Treat this as a marking guide for what examiners are looking for, not just a fact list.
Practice questions for Group 1: Alkali Metals
How many electrons do alkali metals have in their outermost shell?
Explain why potassium is more reactive than sodium when it reacts with water.
Quick recall flashcards
More reactive: Li or K?
Potassium (further down = more reactive)
Equation: sodium + water →
2Na + 2H₂O → 2NaOH + H₂