1. Physics and the Quantum Mechanical Model
Objectives
Describe the relationship between the wavelength and frequency of light.
I.D. the source of atomic emission spectra.
Explain how the frequencies of emitted light are related to changes in electron energies.
Distinguish between quantum mechanics and classical mechanics.

2. What are Electromagnetic Waves?
Electromagnetic waves are formed when an electric field (shown as red) couples with a magnetic field (shown as blue).
The magnetic and electric fields of an electromagnetic wave are perpendicular to each other and to the direction of the wave.

4. Properties of Waves
On your paper draw a horizontal line approximately 5 inches long.
Using the line as the midpoint draw two waves superimposed on each other. Both waves should have the same amplitude but different frequencies.
Draw another horizontal line and two waves with the same wavelength but different amplitudes.

5. Electromagnetic Spectrum

6. PRACTICE!

7. Atomic Spectra ATOMIC EMMISSION SPECTRUM
Light emitted atoms consists of a mixture of only specific frequencies.
Each specific frequency of visible light corresponds to a particular color.
When the light emitted by an atom passes through a prism it separates into discrete lines.

8. The lowest possible energy of the electron is the ground state. (n=1)
Absorbing energy moves it to the excited state (n=2,3,4, 5, 6, 7)
E = h x 
Planck's equation implies the higher the frequency of a radiation, the more energetic are its quanta.
E= quantum of Energy
= frequency
h= x J·s

9. Bohr’s Hydrogen Model and Atomic Spectra
Suppose an electron in its ground state (n=1) absorbs enough energy to jump to level 2. What type of radiation will it emit when it returns to the ground state?
Which series of lines can be observed in the emission spectrum of hydrogen?
Compare the energy of the Paschen and Balmer series.
What do you notice about the spacing of the energy levels from n=1 to n=7?

11. Science Trek
Melissa
Sergio
Professor Edwards