Calculate the wavelength of light emitted when each of the following transactions occur in the hydrogen atom.what type of electromagnetic radiation is emitted in each transion n=5-n=4
The transition from n=5 to n=4 in a hydrogen atom results in the emission of a photon with a wavelength given by the Rydberg formula:
1/λ = R (1/4^2 - 1/5^2)
where R is the Rydberg constant (1.097 × 10^7 m^-1).
Plugging in the values, we get:
1/λ = 1.097 × 10^7 (1/16 - 1/25)
1/λ = 1.097 × 10^7 (0.0625 - 0.04)
1/λ = 1.097 × 10^7 (0.0225)
1/λ = 24713.5
λ = 4.05 × 10^-5 m
The electromagnetic radiation emitted in this transition is in the visible part of the spectrum, specifically in the red region, with a wavelength of 4.05 × 10^-5 m.