Question:
The ionisation energy of hydrogen atom is \(13.6\mathrm{eV}\). What will be the ionisation energy of He\(^+\)?
The ionisation energy of hydrogen atom is \(13.6\mathrm{eV}\). What will be the ionisation energy of He\(^+\)?
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Formula: \(E_n = -13.6 \times \frac{Z^2}{n^2}\) eV. Ionisation energy is \(|E_1|\).
Updated On: Apr 20, 2026
- \(13.6\mathrm{eV}\)
- \(54.4\mathrm{eV}\)
- \(122.4\mathrm{eV}\)
- Zero
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The Correct Option is B
Solution and Explanation
Step 1: Understanding the Concept:
For hydrogen-like species, Ionisation Energy (IE) \(\propto Z^2\).
Step 2: Detailed Explanation:
IE for H (Z=1) is 13.6 eV. For He\(^+\) (Z=2), IE = \(13.6 \times (2)^2 = 13.6 \times 4 = 54.4 \mathrm{eV}\).
Step 3: Final Answer:
54.4 eV
For hydrogen-like species, Ionisation Energy (IE) \(\propto Z^2\).
Step 2: Detailed Explanation:
IE for H (Z=1) is 13.6 eV. For He\(^+\) (Z=2), IE = \(13.6 \times (2)^2 = 13.6 \times 4 = 54.4 \mathrm{eV}\).
Step 3: Final Answer:
54.4 eV
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