1) Find the frequency of the spectral line for which the hydrogen
electron transits from the n=3 to the n= 2 energy level.
The energy at the n= 2 level is:
E(n=2) = - 13.6/ n2 =
- 13.6/ (2)2 =
- 13.6/4 (eV)
Now, 1 eV = 1.6 x 10-19 J so:
E(n=2) = - 13.6/4 (eV) = -(3.4) x 1.6 x
10-19 J =
-5.4 x 10-19 J
The n=
3 level has energy:
E(n=3) = - 13.6/ n2 =
- 13.6/ (3)2 =
- 1.51 (eV)
= -(1.51) x 1.6 x 10-19 J
= -2.4 x 10-19 J
Then the energy difference is:
E3 – E2 = [- 2.4 – (-5.4)] x 10-19 J
= 3.0 x 10 -19 J
From this, the wavelength of the photon emitted can be
found.
Since E = hf = h (c/ l): l = hc/
(E2 – E1)
l = (6.626069 x
10- 34 J-s)(3 x 10 8 m/s)/ 3.89 x 10-19 J
l = 1.21 x
10 -7 m
The frequency can then be found from:
f = (c/ l) = (3 x 10 8 m/s)
/ 1.21 x 10 -7 m = 2.47 x 10 15 Hz
(1) For the Balmer a line (called H-
alpha), we know:
E3 – E2 = - 13.6 eV ( 1/ 3 2 -
1/ 2 2 ) = 1.88 eV
a) From this information calculate the ratio
N2/ N1 for
T = 10 4 K
(
At the n=2 level the statistical weight is: g 1 = 2(2)2 = 8
b) Obtain the frequency of the spectral line for this
transition
Solutions:
(a) N2 / N1 = [g2 / g1] exp (- E2 – E1) / kT
From the table in the Dec. 5th post; g2 = 8 and g1 = 2
k = 8.6174 x 10 -5 eV/K
N2/ N1 = [8/ 2] exp (- E2 – E1) / kT
N2/ N1 = 4 exp (-1.88 eV)/ (8.61 x 10 -5 eV/K) (10 4 K)
N2/ N1 = 4(0.113) = 0.452
But 1 eV = 1.6 x
10 -19 J
Then: E3 – E2 = 1.88
( 1.6 x 10-19 J ) =
3.0 x 10 -19 J
From this, the wavelength of the photon emitted can be
found.
Since E = hf = h (c/ l): l = hc/
(E2 – E1)
l = (6.626069 x
10- 34 J-s)(3 x 10 8 m/s)/ 3.89 x 10-19 J
l = 1.21 x
10 -7 m
The frequency can then be found from:
f = (c/ l) = (3 x 10 8 m/s)
/ 1.21 x 10 -7 m = 2.47 x 10 15 Hz
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