Question

An electron in a hydrogen atom undergoes a transition from the n = 3 level to the n = 6 level. To accomplish this, energy, in the form of light, must be absorbed by the hydrogen atom. Calculate the energy of the light (in kJ/photon) associated with this transition.

Answer 1

Answer:$1.816\times 10^{-19} J$

Explanation:

Given

$E=\frac{hc}{\lambda }$

$E=2.18\times 10^{-18}(\frac{1}{n_1^2}-\frac{1}{n_2^2})$

where h=Planck constant

c=speed of light

$E=2.18\times 10^{-18}(\frac{1}{3^2}-\frac{1}{6^2})$

$E=2.18\times 10^{-18}\times \frac{1}{12}$

$E=1.816\times 10^{-19} J$