Why Are Alkali Metals So Reactive?
Part of Group 1: Alkali Metals · GCSE GCSE Chemistry revision
This deep dive covers Why Are Alkali Metals So Reactive? 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 3 of 13 in this topic. Use this deep dive to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 3 of 13
Practice
22 questions
Recall
20 flashcards
🔬 Why Are Alkali Metals So Reactive?
Every alkali metal has just ONE electron in its outer shell. That's the key to everything.
Think of it this way:
- A full outer shell is the most stable electron configuration (like noble gases)
- It takes far less energy to lose 1 electron than to gain 7
- So the atom is in a lower energy state after losing that electron
Why reactivity INCREASES down the group:
- Going down, atoms get bigger (more shells)
- Outer electron is further from the nucleus
- Less attraction = easier to lose = more reactive
Keep building this topic
Read this section alongside the surrounding pages in Group 1: Alkali Metals. That gives you the full topic sequence instead of a single isolated revision point.
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
22 questions on Group 1: Alkali Metals — practise free
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