1. Waves & Bohr’s Theory
Chapter 7 §1-4

2. Waves Wavelength, λ, in meters (m)
The length of a wave from crest to crest or trough to trough.
Frequency, υ, in inverse seconds (s-1)
The number of waves that pass in a given amount of time.

3. Light’s Wave Characteristics

4. Light’s Wave Characteristics
Speed of light equation
c = speed of light, 3.00x108 m/s
λ = wavelength, in m
ν = frequency, in Hz or s–1

5. Light’s Wave Characteristics
What is the frequency of red light having a wavelength of 681 nm?
681 nm = 6.81x10–7 m
3.0x108 m/s = (6.81x10–7 m)(υ)
υ = 4.41x1014 s–1

6. Max Planck
Quantized

7. Planck’s Equation
n = integer other than zero, no unit, represents the energy level of the atom
h = Planck’s constant, 6.63x10–34 J•s
ν = frequency, in Hz or s–1
E = energy of a quantum – amount of energy to move an e– from its present energy to its next higher one

8. The Photoelectric Effect
Although the photoelectric effect was first discovered by Heinrich Hertz in 1887, Albert Einstein incorporated Planck’s ideas into the explanation of the photoelectric effect.

9. The Photoelectric Effect
Einstein stated that electrons could move within their atoms if a minimum amount of energy were reached.

10. Let’s Practice
The blue-green line of the hydrogen atom spectrum has a wavelength of 486 nm. What is the energy of a photon of this light?
486 nm = 4.86x10–7 m
3.0x108 m/s = (4.86x10–7 m) (υ)
υ = 6.17x1014 s–1
E = (1)(6.63x10–34 J•s)(6.17x1014 s–1)
E = 4.09x10–19 J

11. Bohr’s Line Spectra
Bohr noticed that elements emitted a line spectrum.

12. Bohr’s Line Spectra
He hypothesized that each line in the spectra were created when an electron fell from a higher energy level to a lower one within the atom.

13. Bohr’s Line Spectra
Here, the electron of the hydrogen atom is shown moving between the various energy levels.

14. Bohr’s Postulates Bohr felt the need to explain two main issues:
1st – If electrons are negative and protons are positive…..

15. Bohr’s Postulates Bohr felt the need to explain two main issues:
2nd – How are the line spectra being created?

16. Bohr’s Postulates Postulate #1:
Electrons only have specific energy values and energy levels.
= the energy of a particular e– energy level
= the Rydberg constant = 2.18x10–18 J
= integral value representing the energy level (principal quantum number

17. Bohr’s Postulates Postulate #2:
Electrons become excited by collisions of atoms or absorption of energy – think of anything colored… it absorbs light to later emit (reflect) other colors
Electrons can change energy only by going from one energy level to another – making a transition.

18. Bohr’s Postulates
Postulate #2:
The electron absorbing energy

19. Bohr’s Postulates Postulate #2:
When an electron falls from a higher energy level to a lower energy level, it emits a photon of light.

20. Bohr’s Postulates Postulate #2:
This energy of this photon can be found by:

21. Bohr’s Postulates Postulate #2:
Remember that the energy of a photon can be determined by:

22. Bohr’s Postulates
Postulate #2:
Which can be related to wavelength:

23. Bohr’s Postulates Postulate #2: Which leads to the Balmer equation:
This equation can calculate the wavelength of any electron falling to the 2nd energy level – emitting visible light.

24. Bohr’s Postulates Postulate #2:
By the end of Experiment #13, you should be able to identify the Balmer Series, along with the Paschen Series and the Lyman Series.

25. Let’s Practice
What is the wavelength of the light emitted when the electron in a hydrogen atom undergoes a transition from energy level n = 6 to level n = 3?

26. Let’s Practice
What is the wavelength of the light emitted when the electron in a hydrogen atom undergoes a transition from energy level n = 6 to level n = 3?
∆E = E3 – E6 =
υ = 2.74x1014 s–1
c = λυ → 3.0x108 m/s = λ (2.74x1014 s–1)
λ = 1.09x10–6 m = 1090 nm (Infrared)