The transition from n=5 to n=3 in hydrogen atom corresponds to the emission of a photon. The energy difference between the initial and final states is given by the Rydberg formula:
1/λ = R∞ (1/n1^2 - 1/n2^2)
where λ is the wavelength of the emitted photon, R∞ is the Rydberg constant, and n1 and n2 are the initial and final quantum numbers, respectively.
For this transition, n1 = 5 and n2 = 3. Substituting these values into the formula, we get:
1/λ = R∞ (1/5^2 - 1/3^2)
1/λ = R∞ (1/25 - 1/9)
1/λ = R∞ (16/225)
Solving for λ, we get:
λ = 225/(16 R∞)
At room temperature, R∞ = 1.097 x 10^7 m^-1. Substituting this value, we get:
λ = 225/(16 x 1.097 x 10^7)
λ = 1.213 x 10^-6 m
Therefore, the wavelength of the emitted radiation is 1.213 x 10^-6 m, which corresponds to the infrared region of the electromagnetic spectrum.
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=3
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