Question

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* =

5. Determine the wavelength of light emitted when an electron in a hydrogen atom makes a transition from an orbital in n = 6 to an orbital in n = 5.

Answer #1

**1)
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* (1/5^2 - 1/2^2)
lambda = 4.369*10^-7 m
lambda = 437 nm
Answer: 437 nm**

**2)
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/lambda = 1.097*10^7* (1/5^2 - 1/6^2)
lambda = 7.458*10^-6 m
lambda = 7458 nm
Answer: 7458 nm**

Determine the wavelength of the light absorbed when an electron
in a hydrogen atom makes a transition from an orbital in which n =
3 to an orbital in which n =6.
Answer in nm please. Thank you.

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...

Determine the frequency (Hz) and wavelength (nm) of light
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An electron in a hydrogen atom makes a transition from the n = 7
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1. a. A photon is absorbed by a hydrogen atom causing an
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b. After some time in the excited state, the electron falls from
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(1)
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