Question

n a simplified and example version of the solar system model (developed by Neils Bohr, a Danish chemist), an electron in an orbit of an atom has an energy of -50.3 J. If the atom absorbs a photon and the electron moves up to an orbit with the energy -18.5 J, what is the the energy of the photon of light that was absorbed?

Answer 1

Answer:

31.8 Joules is the the energy of the photon of light that was absorbed.

Explanation:

Initially the electron is present at energy level equal to -50.3 Joules and on absorbing an energy it jumps to energy level which has energy of -18.5 Joules.

$E_1=-50.3 J$ (Initial)

$E_2=-18.5 J$ (Final)

$\Delta E=E_2-E1$

$\Delta E = -18.5 J - (-50.3 J) = 31.8 J$

ΔE , here is also the energy of the photon absorbed by an electron before transition.

31.8 Joules is the the energy of the photon of light that was absorbed.