Question detail
Which of the following statements is true about the first ionisation energy of elements in the same group of the periodic table?
Try the question, check the answer, then read the explanation to understand the curriculum point.
At a glance
MCQ
Type
practice
Style
Topic
Atomic structure
Question
- A. It increases down the group
- B. It decreases down the group
- C. It remains the same down the group
- D. It varies randomly down the group
Answer
It decreases down the group
Explanation
In the same group of the periodic table, the first ionisation energy decreases down the group due to the increasing atomic radius and shielding effect, which makes it easier to remove the outermost electron.
Common mistake
Common Mistake in Writing Ionisation Equations
Students often forget to include the correct charge on the ion when writing equations for first and successive ionisation energies.
To fix this, remember that the first ionisation energy equation for an atom X should be written as: X(g) → X⁺(g) + e⁻. For successive ionisation energies, include the charge of the ion formed. For example, the second ionisation energy would be: X⁺(g) → X²⁺(g) + e⁻. Always ensure to indicate the state of the atom and the charge of the ions.
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