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

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

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

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

Answer 2

Answer:

1.82 × 10⁻¹⁹ J

Explanation:

The Bohr model of the atom states that the energy required to transition between two energy levels is equal to the difference between the inverse squares of the energy levels multiplied by the Rydberg constant: