Calculate the frequency of the radiation emitted when an electron jumps from n=3 in the Balmer series of hydrogen.

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Q. Calculate the frequency of the radiation emitted when an electron jumps from n=3 to n=2 in a hydrogen atom is:

Q. Calculate the wavelength of radiation emitted when electron in a hydrogen atom jumps from

n = \infty

n = 1

Q. Assertion: Emitted radiations lie in visible region when electrons jump from higher level to n = 2 in hydrogen.
Reason: Balmer series radiations belong to visible range in H-atoms.

The wavelength of radiation emitted is $λ_{0}$ when an electron in hydrogen atom jumps from 3rd to 2nd orbit. If in the hydrogen atom itself, the electron jumps from fifth orbit to second orbit, then the wavelength of emitted radiation will be:

Q. Using Bohr's postulates, derive the expression for the frequency of radiation emitted when an electron in a hydrogen atom undergoes transition from a higher energy state (quantum number

n_{i}

) to a lower state,

(n_{f})

.
When an electron in a hydrogen atom jumps from energy state

n_{i} = 4

n_{f} = 3, 2, 1,

identify the spectral series to which the emission lines belong.

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