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 $124.1 nm$ ?
Given ( $h = 6.62 \times 10^{- 34} J s$ )

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 $124.1 nm$ ?

Given ( $h = 6.62 \times 10^{- 34} J s$ )

Aicharya · Accepted Answer

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

$∆ E = \frac{h c}{λ} = \frac{6.62 \times 10^{- 34} J s \times 3 \times 10^{8} m s^{- 1}}{1.6 \times 10^{- 19} J \times 124.1 nm} = \frac{1242 eV nm}{124.1 nm} = 10 eV$

Hence, option D is correct.

The energy levels of an atom is shown is figure. Which one of these transitions will result in the emission…

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