Below is the energy level diagram representing the transitions made by an electr

Question

Below is the energy level diagram representing the transitions made by an electron in a hydrogen atom which result in the observed lines of both the absorption and emission spectra.

4 different energy photons are represented (approximate wavelengths are given in parentheses): infrared (10-4 m) red ( 10-6 m) blue ( 107 m) ultraviolet (~ 10-8 m) ultraviolet ( 10-8 m) n=5 n=3 n=1 Match the transition (a - h) with the photon described (approximate wavelengths are given in parentheses.) (Please note: This is not a problem for which a calculator is required. Your knowledge of the Bohr model of the atom and the relative energies of transitions is all that is needed.) Red photon absorption ( 10 m) Blue photon emission (~ 107 m) Highest energy emission Lowest energy absorption 7

Explanation / Answer

Red photon absorption   = f

Blue photon emission = c

Highest energy emission = d

lowest energy absorption = e.

blue and red   are balmar series means transition happens at n= 2 only   either absorption or emission.as gap increases energy required or released will increase.

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