Asked by kayla
A hydrogen electron is elevated from level 1 to level 2. Another electron is elevated from level 2 to level 4. The transition requiring the greatest energy change is
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The 1 → 2 transition requires the greater energy.
Using En = −13.6 eV / n^2, the energy required is
- For 1 → 2: ΔE = E2 − E1 = −13.6(1/4 − 1) = 10.2 eV
- For 2 → 4: ΔE = E4 − E2 = −13.6(1/16 − 1/4) = 2.55 eV
So the 1→2 excitation needs 10.2 eV, which is larger than 2.55 eV.
Using En = −13.6 eV / n^2, the energy required is
- For 1 → 2: ΔE = E2 − E1 = −13.6(1/4 − 1) = 10.2 eV
- For 2 → 4: ΔE = E4 − E2 = −13.6(1/16 − 1/4) = 2.55 eV
So the 1→2 excitation needs 10.2 eV, which is larger than 2.55 eV.
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