1. Spectral Lines
3.2

2. Spectral Line formation?
Electron has different energy levels: Floors in a building.
Lowest is called the Ground State.
Higher states are Excited States.

3. Changing Levels
If you add the RIGHT amount of energy to an atom, the electron will jump up energy floors.
If the electron drops down energy floors, the atom gives up the same amount energy.
From before, LIGHT IS ENERGY: E = hc/l

4. Kirchhoff’s Laws Light of all wavelengths shines on an atom.
Only light of an energy equal to the difference between “floors” will be absorbed and cause electrons to jump up in floors.
The rest of the light passes on by to our detector.
We see an absorption spectrum: light at all wavelengths minus those specific wavelengths.

5. Kirchhoff’s Laws Cont…
Excited electrons, don’t stay excited forever.
Drop back down to their ground floors.
Only light of the precise energy difference between floors is given off.
This light goes off in all directions.
From a second detector, we see these specific energy wavelengths: an emission spectrum.

6. Continuum, Absorption, Emission

8. Emission Lines
Every element has a DIFFERENT finger print.

9. Emission and Absorption spectra
The lines represent jumps or leaps from one energy level to another
Lines can be sharp or blurry
Blurry lines were later discovered to be a group of very close lines…some energy levels were very close in energy yet different
Later some of the blurry lines were found to respond to magnetic fields….implication is that orbits have 3-D orientation in space

10. Balmer equation 1/λ= RH (1/nf2 – 1/ni2)
Correctly predicts all the 4 lines for the hydrogen atom (only hydrogen)
λ= wavelength of light in metres
RH- Rydberg constant 1.10 x 107 m-1
nf= final energy level (once returned)
ni= initial energy level (once excited)

11. Blackbody radiation- Planck
First result after Bohr that was problematic for physicists
A blackbody is a solid object that is heated until it begins to glow (first red then blue then white hot) and then allowed to return to thermal equilibrium slowly
If the intensity or brightness of the different colours that is emitted is plotted a BELL shaped curve is seen…not what was expected!

12. Blackbody radiation

13. Interpretation
Higher energy (UV) has a higher peak, lower ernergy (IR) has a lower peak
According to classical physics, it should not be bell shaped but should be a exponential decay kind of curve. Starting high up on the left and going down and to the right like a hockey stick
That means that light emitted from a cooling object is like light, it is made up of chunks like light is made of particles called photons.
Einstein concurred and interpreted the results as meaning energy comes in quanta

14. Planck and Einstein E= hf = hc/λ Energy of the photon of light (J)
h= Planck’s constant 6.63 x Js
or 4.14 x eVs
c= speed of light (3.00 x 108 m/s)
λ= wavelength of light (m)

15. Photoelectric Effect Simulation

16. Explanation of Photoelectric Effect
In the photoelectric effect, electrons of metals are ejected when light shines on them
However, not all wavelengths of light will cause the photoelectric effect
Red light has no photoelectric effect on potassium
Yellow light causes this effect on potassium
Begin 3rd

17. Illustrations of Photoelectric Effect

18. Wavelength of light is critical

19. What does it mean?
Einstein interpreted the results and said that energy at the atomic level is in chunks. Only certain energies are allowed
The intensity of the light affects how many electrons jump but does not affect the speed of the electrons once they leave the surface
Frequency (and wavelength) are key. Threshold frequencies are observed for different materials
Minimum energy required to bump an electron off its orbit. If more is delivered, the electron leaves with a faster speed from the surface
Energy is quantized (quanta)
(Photoelectric effect like solar panel!)

20. Double slit experiment
Results indicated that light which was supposed to be a particle was behaving as a wave
Diffraction of the electrons through the double slit matches wave patterns.
Electron is not a particle but a smear. It’s location cannot be known for certain unless you measure it.
Einstein (God does not play dice)
Bohr (Do not tell God what to do)