An electron in the 3rd stationary state around a hydrogen atom has an energy value of -1.512 eV. What will the electron's energy be if the hydrogen atom absorbs a photon with a wavelength of 1090 nm?
E = -1.512 eV
Ephoton = hc/λ
The Attempt at a Solution
I'm unsure if my formula was the correct one to use...
E photon = hc/λ
= (6.63 x 10^-34 J*s)(3.00 x 10^8 m/s) / (1090 x 10^-9 m)
= 1.82477064 x 10^-19 J
= 1.140481651 eV
ΔE = Ef - Ei
Ef = ΔE + Ei
= (1.140481651 eV) + (-1.512 eV)
= -0.371518349 eV
The electron's energy will be about -0.3715 eV
I am really just unsure of my process and therefore my answer, so I would just like a second opinion. Thank you!