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

Explanation / Answer

E =hc/l

= 13.6(1/4^2 - 1/5^2)

= 0.0492 X 10 ^-18j

Energy will be released as the electron is coming from a state of higher energy to that of lower energy

hence

C, C. A photon of 4051 nm wavelength and 4.91x10-20 J energy was emitted

hence

= 13.6*

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