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Physics - Modern Physics Question with Solution | TestHub

PhysicsModern PhysicsAtomic structureEasy2 minQB

PhysicsEasysingle choice

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 ( $h = 6.62 \times 1 0^{-34} J s$ )

Options:

Answer:

Solution:

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

$Δ E = \frac{h c}{λ} = \frac{6.62 \times 1 0 ^{- 34} J s \times 3 \times 1 0 ^{8} m s ^{- 1}}{1.6 \times 1 0 ^{- 19} J \times 124.1 nm} = \frac{1242 e Vnm}{124.1 nm} = 10 e V$

Hence, option D is correct.

Stream:JEESubject:PhysicsTopic:Modern PhysicsSubtopic:Atomic structure

⏱ 2mℹ️ Source: QB

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