Consider the electronic transition from n = 5 to n = 4 in a hydrogen atom, and s

Question

Consider the electronic transition from n = 5 to n = 4 in a hydrogen atom, and select the correct statement below.

A. A photon of 1823 nm wavelength and 1.09x10-19 J energy was emitted from the hydrogen atom during the electronic transition. B. A photon of 1823 nm wavelength and 1.09x10-19 J energy was absorbed by the hydrogen atom during the electronic transition. C. A photon of 4051 nm wavelength and 4.91x10-20 J energy was emitted from the hydrogen atom during the electronic transition. D. A photon of 4051 nm wavelength and 4.91x10-20 J energy was absorbed by the hydrogen atom during the electronic transition.

Explanation / Answer

Energy of hydrogen atom is given by

En = -13.6/n^2 eV where n is the orbital level

Now the difference is E5-E4 = -13.6(1/25-1/16) = 0.306 eV

but 1 eV = 1.6 *10^-19 J

=> energy = 1.6*0.306 * 10^-19 = 4.896 * 10^-20 J

and wavelength = hC/E = 6.625*10^-34 * 3 * 10^8/4.896*10^-20 J = 4051 nm

now since electron is coming from higher level to lower level energy is emitted

correct option is

C) photon of 4051nm wavelength and 4.90*10^-20 J energy was emitted

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