Physics Department EXP. FIVE Kuwait University Course 127 The

Physics Department
Kuwait University
EXP. FIVE
Course 127
February, 2001
The Spectrum of Hydrogen
Objective
• To study the emission spectra of the Hydrogen gas.
• Visualize the spectral lines of the Balmer series using a spectrometer.
• Determine Plank’s constant, h.
Theory
If an electron at a certain energy level in an atom gains sufficient amount of energy, it
may jump to higher energy levels and the atom is said to be an excited atom. The atom
usually doesn’t last for long time in its excited state, but tends to return back to its
original state by emitting electromagnetic radiation, which is called photon (see Fig. 1).
Ei
photon
Ef
Figure 1: The emission of photon
If an electron in hydrogen atom, at energy level, Ei, makes a transition to a lower
energy level, Ef, it will emit a photon with energy, Eph, equals the difference between the
two energy levels, i.e.
Eph = Ei - Ef .
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(1)
The energy of the emitted photon is given as
Eph = hν,
(2)
where h is Plank’s constant, and ν is the frequency. Therefore,
hν = E i − E f .
(3)
The energy of an energy level, n, is given as
2π 2 k 2 me 4
En = −
,
h2n2
(4)
and the frequency, ν=c/λ, where c is the speed of light, and λ is the wavelength of the
photon. Therefore, substituting for ν, and En in Eq.(3) gives
h3 =
 1
1 

− 2 ⋅λ ,
2
n
ni 
 f
2π 2 k 2 me 4
c
(5)
where:
k is the electrostatic constant = 9 × 109 Nm2 c-2,
m is the electronic mass = 9 .11× 10-31 kg,
e is the electronic charge = 1.6 × 10-19 C,
c is the speed of light = 3 × 108 m/s,
h is the Plank's constant = 6.6256 × 10-34 Js,
nf is principle quantum number for the final energy level,
ni is principle quantum number for the initial energy level.
Therefore, if, for a specific transition, nf, and ni are known, Plank’s constant, h, can be
determined by measuring λ for the emitted photon,.
The wavelength, λ, is measured using a spectrometer (Fig. 2). It consists, mainly, of a
diffraction grating, collimator, and a telescope. The collimator directs the light waves
emerging through it’s slit, to the diffraction grating. The telescope, which is free to rotate
through various angles, gathers the light waves emerging from the grating and directs
them towards a magnifying lens at its end. The diffraction grating disperses (diffracts) the
polychromatic light waves at different angles.
The diffraction grating is a piece of glass with equally spaced parallel grooves being
ruled on one face. When a parallel beam of polychromatic light falls on one side of the
grating, each wavelength is dispersed through a specific angle θ, such that
nλ=d sinθ ,
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(6)
where n is order number, and d is the diffraction spacing constant.
Eye piece
Diffraction
grating
Light
sourc
Telescope
Collimator
Slit screw
Figure 2: The spectrometer
Eo (eV)
∝
5
-0.5
4
-0.8
3
-1.5
Paschen
Bracket
2
-3.4
Balmer
1
-13.6
Lyman
Figure 3: Probable transitions in the Hydrogen atom
Figure 3, shows the energy levels of hydrogen atom and the probable transitions for
the electron between the levels. For each energy level there is a series of spectral lines.
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For instance, all spectral lines produced by electron transitions from any level down to
level 1 are called Lyman series. As shown in Fig. 3, there are four series in the hydrogen
spectrum. They are Lyman, Balmer, Paschen, and Bracket series. In this experiment, the
Balmer series is going to be studied.
Equipment
• Spectrometer.
• Diffraction grating (300 lines/mm).
• mercury and hydrogen discharge tubes.
• power supply .
• piece of black cloth.
Procedure
Adjustments
1. Align the telescope with the collimator.
2. Assemble the diffraction grating in the holder.
3. Let the grating be at right angle to the collimator-telescope axis.
4. Place the mercury tube in the discharge socket, and put it in front of the collimator.
5. Cover the area between the collimator and the telescope with the black cloth.
6. Turn on the power to the discharge unit.
7. While looking through telescope, move the light source right and left till you see a
clear colored line.
8. Adjust the slit screw to narrow the line seen.
9. Rotate the telescope lens to adjust the plus sign.
10. Try to center the colored lined.
11. Record the value of the scale as your zero value (θzero).
Determination of d value
1. Rotate the telescope till you see the first appearance of the green line.
2. Read the angle value, θ’, and record in Table I.
3. Calculate the angle θ, corresponding to this line, and record in the table.
4. Given the wavelength of the green line of mercury λHgG = 5.46×10-7 m, determine d.
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5. Calculate d using the value written on the grating, and compare.
Hydrogen spectrum
1. Replace the mercury with the H2 tube. (use the cloth in holding, while power is off).
2. Measure the angles corresponding to the colors of the 1st order. Record in Table II.
3. Calculate the absolute angle values, and record in the table.
4. Calculate λ corresponding to each color line, and record in the table.
5. Using nf, and nI values given in the table, Calculate Plank’s constant, h.
6. Repeat steps 2-5 for the 2nd order. Record in Table III.
7. Calculate the average value for h for Tables II & III, then compare with the typical
value.
Table I
(θzero=
)
θ; ‘
λHgG (m)
θ
d (m)
dTheoritical (m)
5.46×10-7
Table II (1st order colors)
Color
nf
ni
Faint V.
2
6
Violet
2
5
Green
2
4
Red
2
3
θ; ‘
θ
λ (m)
h (J.s)
θ; ‘
θ
λ (m)
h (J.s)
Avg. h=
Table III (2nd order colors)
Color
nf
ni
Faint V.
2
6
Violet
2
5
Green
2
4
Red
2
3
Avg. h=
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Questions
1. How are the Hydrogen gas atoms excited?
2. What is the purpose of the diffraction grating?
3. What determines the maximum number of the order for a specific wavelength?
4. Is it possible to draw the energy level diagram for the second orbit and above, for the
Hydrogen, using your results? How?
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