Calculate the wavelength of the radiations emitted when an electron in a hydrogen atom undergoes a transition from $4^{t h}$ energy level to the $2^{n d}$ energy level. In which part of the electromagnetic spectrum does this line lie?

Infrared region

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Visible region

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microwave region

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radio wave region

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Solution

The correct option is B Visible region
Let,
wave number $= R_{H} [\frac{1}{(n_{1})^{2}} - \frac{1}{(n_{2})^{2}}]$
On substituting $n_{1} = 2, n_{2} = 4, R_{H} = 109678$ in equation,
wave number $= 109678 \times \frac{3}{16}$
Also, $λ = \frac{1}{w a v e n u m b e r}$
or $λ = 406 n m$
Hence, visible region is the answer

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What is the wavelength of light emitted when the electron in a hydrogen atom undergoes transition from an energy level with n = 4 to an energy level with n = 2?

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Calculate the wavelength of the radiations emitted when an electron in a hydrogen atom undergoes a transition from 4th energy level to the 2nd energy level. In which part of the electromagnetic spectrum does this line lie?

The correct option is B Visible regionLet,wave number =RH[1(n1)2−1(n2)2]On substituting n1=2,n2=4,RH=109678 in equation,wave number =109678×316Also, λ=1wavenumberor λ=406nmHence, visible region is the answer

Calculate the wavelength of the radiations emitted when an electron in a hydrogen atom undergoes a transition from $4^{t h}$ energy level to the $2^{n d}$ energy level. In which part of the electromagnetic spectrum does this line lie?