Question

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 $1241\, nm$ ? Given $\left( h =6.62 \times 10^{-34} Js \right)$

• A. D
• B. B
• C. A
• D. $C$

Answer 1

Answer: (A)

D

Answer 2

The correct answer is (A) : D
λ=ΔEhc​
ΔEA​=2.2eV
ΔEB​=5.2eV
ΔEC​=3eV
ΔED​=10eV
λA​=2.2×1.6×10−196.62×10−34×3×108​
=2.212.41×10−7​m
=2.21241​nm=564nm
λB​=5.21241​nm=238.65nm
λC​=31241​nm=413.66nm
λD​=101241​=124.1nm