#### Question

The energy levels of an atom are as shown below. Which of them will result in the transition of a photon of wavelength 275 nm?

#### Solution

Energy transitions for A,B,C, and D are:

A = 2 eV

B = 4.5 eV

C = 2.5 eV

D = 8 eV

`E=(hC)/lamda`

Where,

*E *= Energy transition

λ = Wavelength

*h* = 6.63 × 10^{−34} Js

*C* = 3 × 10^{8} m/s

For B, we have

`lambda = (6.63 xx 10^-34 xx 3 xx 10^8)/(4.5 xx 1.6 xx 10^-19)`

`lambda = 275`nm

Thus, B will result in transition of a photon of wavelength of 275 nm.

Is there an error in this question or solution?

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The Energy Levels of an Atom Are as Shown Below. Which of Them Will Result in the Transition of a Photon of Wavelength 275 Nm? Concept: Energy Levels.

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