1. Modern Atomic Theory Quantum Theory and the Electronic Structure of Atoms Chapter 11

2. Properties of Waves

3. The speed (u) of the wave = x

4. electromagnetic waves Electromagnetic radiation is the emission and transmission of energy in the form of electromagnetic waves. All electromagnetic radiation x  c

7. A photon has a frequency of 6.0 x 10 4 Hz. Convert this frequency into wavelength (nm). Does this frequency fall in the visible region?

8. Why all this info about light??? atomic emission spectrum of an element.

9. The emission spectrum of white light is continuous. Atomic emission spectra consist of relatively few lines and are discontinuous. Each line corresponds to a specific amount (quantum) of energy being emitted.

10. The emission spectra for each element is unique.

11. Classical physics does not explain the emission spectra of atoms. Energy (light) is emitted or absorbed in discrete units (quantum). E = h x Planck’s constant (h) h = 6.63 x 10 -34 J s

12. When copper is bombarded with high-energy electrons, X rays are emitted. Calculate the energy (in joules) associated with the photons if the wavelength of the X rays is 0.154 nm.

13. http://www.youtube.com/watch?v=oUolVZIuv18

14. Photoelectric Effect Light quanta are called photons. Light has a “dual nature” as it exhibits wave-particle behavior. In the photoelectric effect metals eject electrons when light shines on them.

15. Einstein used his particle theory of light to explain the photoelectric effect. He recognized there is a threshold value of energy below which this effect does not occur. Since E = h x v, if the frequency and therefore the energy of photons is too low, the photoelectric effect does not occur.

16. http://player.discoveryeducation.com/index.cfm?guidAssetId=B2E7CD0F-A754-4BA4-8D00-B0DE326F1038&blnFromSearch=1&productcode=USplayer.discoveryeducation.com/index.cfm?guidAssetId=B2E7CD0F-A754-4BA4-8D00-B0DE326F1038&blnFromSearch=1&productcode=US