Question

# A. Determine the wavelength of the light absorbed when an electron in a hydrogen atom makes...

A. Determine the wavelength of the light absorbed when an electron in a hydrogen atom makes a transition from an orbital in which n=2 to an orbital in which n=7. Express the wavelength in nanometers to three significant figures.

B. An electron in the n=6 level of the hydrogen atom relaxes to a lower energy level, emitting light of λ=93.8nm. Find the principal level to which the electron relaxed. Express your answer as an integer.

Can you explain it in details? Where each number comes from

A)

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 = 1.097*10^7

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

1/lambda = - 1.097*10^7* (1/7^2 - 1/2^2)

lambda = 4.00*10^-7 m

lambda = 400 nm

B)

wavelength = 93.8 nm

wavelength = 9.38*10^-8 m

Here photon will be emitted

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

R is Rydberg constant. R = 1.097*10^7

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

1/9.38*10^-8 = 1.097*10^7*(1/nf^2 - 1/6^2)

(1/nf^2 - 1/6^2) = 0.9718

1/nf^2 = 0.9996

nf^2 = 1

nf = 1

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