The energy levels of an atom is shown is figure.
Which one of these transitions will result in the emission of a photon of wavelength $124 . 1nm$ ?
Given ( $h = 6 . 62 \times {10}^{– 34}Js$ )

Question

The energy levels of an atom is shown is figure. Which one of these transitions will result in the emission of a photon of wavelength 124 . 1nm ? Given ( h = 6 . 62 × 10 ^ – 34 Js )

Quantrex Academy · Accepted Answer

Correct answer: D. D

The change in energy is related to wavelength of photon emitted as:

$∆ E = \dfrac{hc}{\lambda} = \dfrac{6 . 62 \times {10}^{- 34}Js \times 3 \times {10}^{8}m{s}^{- 1}}{1 . 6 \times {10}^{- 19}J \times 124 . 1nm} = \dfrac{1242eVnm}{124 . 1nm} = 10eV$

Hence, option D is correct.

The energy levels of an atom is shown is figure. Which one of these...

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