1a) In what region of the electromagnetic spectrum will the electron transitions

Question

1a) In what region of the electromagnetic spectrum will the electron transitions from a higher energy state to n1=3 appear for the hydrogen spectrum?
1b) Calculate the wavelength, in nm, for the nh = 4 to nl = 3 transition for the hydrogen atom. 1a) In what region of the electromagnetic spectrum will the electron transitions from a higher energy state to n1=3 appear for the hydrogen spectrum?
1b) Calculate the wavelength, in nm, for the nh = 4 to nl = 3 transition for the hydrogen atom.
1b) Calculate the wavelength, in nm, for the nh = 4 to nl = 3 transition for the hydrogen atom.

Explanation / Answer

1a)

Here photon will be captured and it will excite the atom

1/lambda = R* (1/nf^2 - 1/ni^2)

R is Rydberg constant. R = 1.097E7

1/lambda = - R* (1/nf^2 - 1/ni^2)

1/lambda = - 1.097E7* (1/3^2 - 1/1^2)

lambda = 1.032E-7 m

lambda = 103 nm

This falls in ultraviolet region as this is lyman series

Lyman series is the one where one of the state is n=1

1b)

Here photon will be emitted

1/lambda = R* (1/nf^2 - 1/ni^2)

R is Rydberg constant. R = 1.097E7

1/lambda = R* (1/nf^2 - 1/ni^2)

1/lambda = 1.097E7* (1/3^2 - 1/4^2)

lambda = 1.875E-6 m

lambda = 1875 nm

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