For this question consider the figure to the right shows an energy level diagram

Question

For this question consider the figure to the right shows an energy level diagram for a certain atom (not hydrogen). Several transitions are shown and are labeled by letters. a.) Which transition corresponds to the absorption of the photon with the longest wavelength? b.) Which transition corresponds to the absorption of the photon with the shortest wavelength? c.) Which transition corresponds to the absorption of a 413nm photon? d.) Which transition corresponds to the emission of a 248nm photon?

Explanation / Answer

emission is possible only when electron gets transformed from higher orbit to the lower one ie from outer to inner. And absorption is when electron gets switched from inner to outer.

So 4 to 2 and 2 to 1 transition leads to emission

and 1 to 3 and 2 to 3 and 3 to 4 leads to absoption

part A

the absorption of the photon with the longest wavelength =>

using the concept => Larger the energy difference between orbits, then larger the frequency and shorter the wavelength.

for longest wavelength that corresponds to absoption, energy difference must be smallest which is 3 to 4 transition.

part B

using the same concept

for shortest wavelength that corresponds to absoption, energy difference must be highest which is 1 to 3 transition.

part C

for 413 nm photon.... energy corresponding to this photon is E = hc / (413 x 10^-9 m) = 3eV

and this energy corresponds to 2 to 3 transition.

part d

for 248 nm photon.....energy corresponding to this photon is E = hc / (248 x 10^-9 m) = 5eV

and this energy corresponds to 4 to 2 transition.

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