Question detail
What happens to the reactivity of Group 2 metals as you move down the group?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Group 2, the alkaline earth metals
Question
- A. Reactivity decreases
- B. Reactivity remains constant
- C. Reactivity increases
- D. Reactivity fluctuates
Answer
Reactivity increases
Explanation
As you move down Group 2, the atomic radius increases, which means the outer electrons are further from the nucleus and experience less electrostatic attraction. This makes it easier for the metals to lose their outer electrons, thus increasing their reactivity.
Common mistake
Misunderstanding Reactivity Trends
Students often confuse the trend in reactivity down Group 2 with the trend in ionisation energy, thinking that as ionisation energy decreases, reactivity also decreases.
To clarify, remember that reactivity increases down Group 2 due to the decreasing ionisation energy, which makes it easier for the atoms to lose their outer electrons. The formula for first ionisation energy is related to the energy required to remove an electron from an atom. As you move down the group, the atomic radius increases, leading to a decrease in ionisation energy. Therefore, the substitution shows that larger atoms lose electrons more easily, resulting in increased reactivity. Thus, the conclusion is that reactivity increases down Group 2.
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