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

Answer 1

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.