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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 124.1 nm? Given (h=6.62×10⁻³⁴ Js)

Asked in JEE Main 25th Jan 2nd Shift 2023 · Spectral series and wavelengths

Figure: Spectral series and wavelengths
Answer: (1) D

Step-by-step solution

E=(hc)/λ=(6.62×10⁻³⁴×3×10⁸)/(124.1×10⁻⁹)=1.6×10⁻¹⁸ J=10 eV

D goes from 0 eV to -10.0 eV: 10 eV.

Why the other options are wrong

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