Question

A photon incident on a hydrogen atom causes the electron to make a transition from the n = 1 orbital to the n = 3 orbital. What is the wavelength of the photon, and what are the possible wavelengths of the emitted radiation when the electron returns to the n = 1 state?

Answer 1

For the first part, equate the energy difference between n=1 and n=3 levels to h*c/(wavelength). The wavelength of the photon required is obtained.


For the second part, there are 3 possible cases for electron transition from n=3 to n=1. The electron jumps from
(1) n=3 to n=2
(2) n=2 to n=1
(3) n=3 to n=1
In each of these cases, calculate the energy difference between the energy levels and equate it to the energy of the photon i.e. h*c/(wavelength). This should give you the possible wavelengths of the radiations.

Answer 2

ok thanks

Answer 3

what a bout this one
If an electron makes a transition from the n = 4 to the n = 1 Bohr orbital in a hydrogen atom, determine the wavelength of the light emitted and the recoil speed of the atom.

Answer 4

am interested in the recoil speed