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Sum

The energy levels of an atom of a certain element are shown in the given figure. Which one of the transitions A, B, C, D or E will result in the emission of photons of electromagnetic radiation of wavelength 618.75 nm? Support your answer with mathematical calculations.

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#### Solution

The wavelength emitted λ = 618.75 nm

∴ Corresponding energy E = h `c/λ`

= `( 6.6 xx 10^-34 xx 3 xx 10^8 )/( 618.75 xx 10^-9 xx 1.6 xx 10^-19) e^V`

= `( 6.6 xx 3 )/( 618.75 xx 1.6 ) xx 100`

= 2eV

This corresponds to the transition D.

In which energy emitted is ΔE = - 1 - ( - 3 ) = 2eV

Concept: Electromagnetic Waves

Is there an error in this question or solution?

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