An electon n in hydrogen atom jump from 5th shell to 3th shell calculate.1) a wave emitted.2) The series from which this wavelength belong.3) Region in which this wavelength fall.4) Frequency of this emitted light wavelength. 5) Energy of emitted light.
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Answers
Answer:
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Answer:
The energy transition will be equal to
1.55
⋅
10
−
19
J
.
So, you know your energy levels to be n = 5 and n = 3. Rydberg's equation will allow you calculate the wavelength of the photon emitted by the electron during this transition
1
λ
=
R
⋅
(
1
n
2
final
−
1
n
2
initial
)
, where
λ
- the wavelength of the emitted photon;
R
- Rydberg's constant -
1.0974
⋅
10
7
m
−
1
;
n
final
- the final energy level - in your case equal to 3;
n
initial
- the initial energy level - in your case equal to 5.
So, you've got all you need to solve for
λ
, so
1
λ
=
1.0974
⋅
10
7
m
−
1
⋅
(
1
3
2
−
1
5
2
)
1
λ
=
0.07804
⋅
10
7
m
−
1
⇒
λ
=
1.28
⋅
10
−
6
m
Since
E
=
h
c
λ
, to calculate for the energy of this transition you'll have to multiply Rydberg's equation by
h
⋅
c
, where
h
- Planck's constant -
6.626
⋅
10
−
34
J
⋅
s
c
- the speed of light -
299,792,458 m/s
So, the transition energy for your particular transition (which is part of the Paschen Series) is
E
=
6.626
⋅
10
−
34
J
⋅
s
⋅
299,792,458
m/s
1.28
⋅
10
−
6
m
E
=
1.55
⋅
10
−
19
J