Answer:
[tex]\Delta E=1.64*10^{-18}J[/tex]
Explanation:
The energy difference between the energy levels involved in the transition of the electron is directly proportional to the frequency of the emitted photon:
[tex]\Delta E=h\nu(1)[/tex]
Where h is the Planck constant. The photon's frequency is inversely proportional to its wavelegth:
[tex]\nu=\frac{c}{\lambda}(2)[/tex]
Here c is the speed of light. Replacing (2) in (1):
[tex]\Delta E=\frac{hc}{\lambda}\\\Delta E=\frac{(6.63*10^{-34}J\cdot s)(3*10^8\frac{m}{s})}{121.6*10^{-9}m}\\\Delta E=1.64*10^{-18}J[/tex]
