1. Chapter 11 “The Electromagnetic Spectrum”

2. Physics and the Quantum Mechanical Model
OBJECTIVES:
Describe the relationship between the wavelength and frequency of light.

3. Physics and the Quantum Mechanical Model
OBJECTIVES:
Identify the source of atomic emission spectra.

4. Physics and the Quantum Mechanical Model
OBJECTIVES:
Explain how the frequencies of emitted light are related to changes in electron energies.

5. Physics and the Quantum Mechanical Model
OBJECTIVES:
Distinguish between quantum mechanics and classical mechanics.

6. Electromagnetic Spectrum

7. Electromagnetic Spectrum
Electromagnetic radiation has a dual behavior.
It has properties of a particle called a photon and as a wave traveling at the speed of light.
Characterized by a wavelength and frequency.

8. Light
The study of light led to the development of the quantum mechanical model.
Light is a kind of electromagnetic radiation.
Electromagnetic radiation includes many types: gamma rays, x-rays, radio waves…
Speed of light = x 108 m/s, and is abbreviated “c”
All electromagnetic radiation travels at this same rate when measured in a vacuum

9. - Page 139
“R O Y G B I V”
Frequency Increases
Wavelength Longer

10. Parts of a wave
Crest
Wavelength - λ
Amplitude
Origin
Trough

11. Wavelength and Frequency
Are inversely related
As one goes up the other goes down.
Different frequencies of light are different colors of light.
There is a wide variety of frequencies
The whole range is called a spectrum

12. Low Energy High Energy Radiowaves Microwaves Infrared . Ultra-violet
X-Rays
GammaRays
Low Frequency
High Frequency
Long Wavelength
Short Wavelength
Visible Light

13. Long
Wavelength =
Low Frequency
Low ENERGY
Short
Wavelength =
High Frequency
High ENERGY

14. Atomic Spectra
White light is made up of all the colors of the visible spectrum.
Passing it through a prism separates it.
Continuous spectra (rainbow)
(frequency: red is low, violet is high)

15. The Nature of Energy
Another mystery involved the emission spectra observed from energy emitted by atoms and molecules.

16. If the light is not white
By heating a gas with electricity we can get it to give off colors.
Passing this light through a prism does something different.

17. Atomic Spectrum Each element gives off its own characteristic colors.
Can be used to identify the atom.
This is how we know what stars are made of.

18. The Nature of Energy
One does not observe a continuous spectrum, as one gets from a white light source.
Only a line spectrum of discrete wavelengths is observed.

19. Emission/line spectra
only certain frequencies are emitted proportional to the amount of energy released
Unique to each element, like fingerprints!
Very useful for identifying elements

20. Absorption spectra
opposite of emission; certain frequencies are absorbed proportional to the amount of energy gained (each is unique)

21. After Planck’s Quantum Theory, Einstein concluded that energy is proportional to frequency in the: Photoelectric Effect
“the ejection of an electron from a metal when exposed to light (above yellow) by photons”
ex. photoelectric cell
light → electricity (calculators, TV, movie soundtracks, security systems, automatic doors)

22. So, what is light?
Light is a particle - it comes in chunks or particles called Photons.
Light is a wave - we can measure its wavelength and frequency so it behaves as a wave

23. Wave-Particle Duality
J.J. Thomson won the Nobel prize for describing the electron as a particle.
His son, George Thomson won the Nobel prize for describing the wave-like nature of the electron.
The electron is a particle!
The electron is an energy wave!

24. The physics of the very small
Quantum mechanics explains how very small particles behave
Quantum mechanics is an explanation for subatomic particles and atoms as waves
Classical mechanics describes the motions of bodies much larger than atoms

25. Heisenberg Uncertainty Principle
“One cannot simultaneously determine both the position and momentum of an electron.”
You can find out where the electron is, but not where it is going.
OR…
You can find out where the electron is going, but not where it is!
Werner Heisenberg

26. It is more obvious with the very small objects
To measure where a electron is, we use light.
But the light energy moves the electron
And hitting the electron changes the frequency of the light.

27. After Before Photon wavelength changes Photon Moving Electron
Electron velocity changes

28. Schrodinger’s Wave Equation
Equation for the probability of a single electron being found along a single axis (x-axis)
Erwin Schrodinger
Erwin Schrodinger

29. The Quantum Mechanical Model
Has energy levels for electrons.
Orbits are not circular.
It can only tell us the probability of finding an electron a certain distance from the nucleus.

30. The Quantum Mechanical Model
The atom is found inside a blurry “electron cloud”
An area where there is a chance of finding an electron.
Think of fan blades

31. The End