The energy levels of an atom is shown in figure. Which one of these transitions will result in the emission of a photon of wavelength 124.1 nm? Given () [2023]

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Solution

Q.
The energy levels of an atom is shown in figure. Which one of these transitions will result in the emission of a photon of wavelength 124.1 nm Given ( $h = 6.62 \times 10^{- 34} Js$ ) [2023]

1 D

2 B

3 A

4 C

Ans.
(1)

$λ = \frac{h c}{Δ E}$

$Δ E_{A} = 2.2 eV$

$Δ E_{B} = 5.2 eV$

$Δ E_{C} = 3 eV$

$Δ E_{D} = 10 eV$

$λ_{A} = \frac{6.62 \times 10^{- 34} \times 3 \times 10^{8}}{2.2 \times 1.6 \times 10^{- 19}} = \frac{12.41 \times 10^{- 7}}{2.2} m = 564 nm$

$λ_{B} = \frac{1241}{5.2} nm = 238.65 nm$

$λ_{C} = \frac{1241}{3} nm = 413.66 nm$

$λ_{D} = \frac{1241}{10} nm = 124.1 nm$

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