A hydrogen atom absorbs energy and an electron is excited to the n = 2 shell. When the electron relaxes...

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A hydrogen atom absorbs energy and an electron is excited to the n = 2 shell. When the electron relaxes back to the ground state, n = 1, it emits light.
Calculate the change in energy of the electron from the excited state back to the ground state. Then, calculate the frequency of the light that was emitted.

SnapAndSolve AI · Accepted Answer

Change in Energy: The energy change when an electron transitions between two energy levels in a hydrogen atom is given by the formula:ΔE = -13.6 eV (1/nf2 - 1/ni2)For ni = 2 and nf = 1:ΔE = -13.6 eV (1/12 - 1/22)ΔE = -13.6 eV (1 - 1/4)ΔE = -13.6 eV (3/4)ΔE = -10.2 eVThe change in energy is 10.2 eV.Frequency of Light: The frequency of the emitted light can be calculated using the energy-frequency relation:E = hνWhere h is Planck's constant (4.135667696 × 10-15 eV·s).ν = ΔE / hν = 10.2 eV / 4.135667696 × 10-15 eV·sν ≈ 2.47 × 1015 HzThe frequency of the emitted light is approximately 2.47 × 1015 Hz.

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A hydrogen atom absorbs energy and an electron is excited to the n = 2 shell. When the electron relaxes...

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