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(B) The Lyman series corresponds to transitions of electrons from higher energy levels to the ground state $(n_1 = 1)$.The least energetic photon in t

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$122$

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(B) The Lyman series corresponds to transitions of electrons from higher energy levels to the ground state $(n_1 = 1)$.The least energetic photon in the Lyman series corresponds to the transition from the first excited state $(n_2 = 2)$ to the ground state $(n_1 = 1)$.The energy difference for this transition is given as $\Delta E = 10.2 	ext{ eV}$.The relationship between energy and wavelength is given by $\lambda = \frac{hc}{\Delta E}$.Substituting the given values: $\lambda = \frac{1240 	ext{ eV-nm}}{10.2 	ext{ eV}}$.$\lambda \approx 121.57 	ext{ nm}$.Rounding to the nearest whole number, we get $\lambda \approx 122 	ext{ nm}$.

The wavelength of light for the least energetic photons emitted in the Lyman series of the hydrogen spectrum is nearly. [Take $hc = 1240 \text{ eV-nm}$, change in energy of the levels $= 10.2 \text{ eV}$] (in $\text{ nm}$)

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