1) Determine the wavelength of light emitted when an electron in a hydrogen atom makes a…
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Question “1) Determine the wavelength of light emitted when an electron in a hydrogen atom makes a…”
1) 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.
2) 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 =3
Answer
Answer (1) (2)
Rydberg equation can be used
R H = Rydberg Constant. 2.18
10 . -18.
n f = final level of energy
ni = initial energy level
Therefore,
1) Transition from n=6 – n=5
n f = 5.
n i = 6.
2.18 J [(1/62] – (1/52)] =.-2.66 *10-20 J (-ve Sign refers to energy released)
We know.
where h=6.626 10 -34Js and c=3
10 8 m/s
so,
(6.626
10-34 Js
3
108 m/s) / (2.66 * 10-20 J) = 7.47
10-6 m = 7472nm
2) Transition from n=2 – n=3
n f = 3.
n i = 2.
2.18 J *
10-18 J [(1)/22) – (1/32)] =3.03 * 10-19 J
(6.626
10-34 Js
3
108 m/s) / (3.03
10-19 J) = 6.56
10-7 m = 656nm
Conclusion
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