1. Warm Up
Draw the Bohr Model for Aluminum and Neon.

2. Electrons in Atoms

3. Everything you ever wanted to know about where the electrons hang out!
Unit 2- Continued
Everything you ever wanted to know about where the electrons hang out!

4. Building on the Atomic Theory
What did Thompson determine?
(Think cathode ray tubes!)
What did Rutherford’s gold
foil experiment prove?

5. Section 1: Early 1900’s
Scientists started doing a lot of experiments looking at the absorption and emission of light by matter.
Found that there is a relationship between light and an atom’s electrons.

6. Light behaves as a wave
Transfer of energy

7. Draw the Wave!
Amplitude: height of the wave from the origin to the crest
Wavelength ( ) : the distance between the crests (m, cm, nm)
Frequency (v): number of waves to pass a given point per unit of time (waves/second = Hz)

8. Slinky Demo

9. An Important Relationship
The frequency and wavelength of all waves, including light, are inversely related.
As the wavelength of light increases, the frequency decreases.

10. Electromagnetic Radiation
Includes radio waves, radar, microwaves, visible light, infrared light, ultraviolet light, X-rays, and gamma rays

11. Wave Particle Duality http://www.youtube.com/watch?v=DfPeprQ7oGc
This is a cool video– way over their heads. I’m showing it anyway!

12. The Photon
Photon- a particle of electromagnetic radiation having no mass, carrying a quantum of energy.

13. Photoelectric Effect
Looks at the emission of electrons from a metal when light shines on the metal.
Light causes electrons to be ejected from the metal.

14. So, what happens when photons hit an atom and eject an electron?
The electron goes from the ground state to an excited state.
As the electron returns to the ground state, it gives off the energy that it gained- LIGHT

15. Energy Levels Energy levels are not evenly spaced Energy levels
become more closely
spaced the greater
the distance from the
nucleus

16. Another Cool Illustration

17. Color The energy given off has a certain wavelength.
Wavelength determines the colors that we see.

18. Flame Test Look at the color produced by the flame…
Determine the wavelength by comparing the color to those in the visible range on the Electromagnetic Spectrum.

19. Warm Up
You have two different samples… sample A. glows red and sample B. glows violet.
a. Draw what the waves might look like?
b. Which has the longer wavelength?
b. Which has the smaller frequency.

20. Atomic Spectra
White light is a combination of all the wavelengths in the visible range of the Electromagnetic Spectrum.

21. Spectral Tubes

22. Each element has a unique line-emission spectra
Atomic Line Spectrum

24. Interpretation of Atomic Spectra
The line spectrum is related to energy transitions in the atom.
Absorption = atom gaining energy
Emission = atom releasing energy
All samples of an element give the exact same pattern of lines.
Every atom of that element must have certain, identical energy states

25. Atomic Spectrum Activity

26. Using Atomic Spectral Data Bohr Model
Electrons orbit around a nucleus
Each orbit has a fixed energy and because of this cannot lose energy and fall into the nucleus
Energy Level of an electron is the region around the nucleus where the electron is likely to be moving

27. This helped explain the spectral lines
Absorption- the electron gains energy and moves to a higher energy level.
Emission- when the electron falls to a lower energy level.

28. Schrodinger Wave Equation
Developed an equation that treated electrons as waves and described the location of electrons.
Helped lay the foundation for modern quantum theory (atomic model).

29. The Quantum Model Finally– the truth (as we know it!)
Electrons can behave as both waves and particles.
Electrons can be considered waves with specific frequencies confined to the space around the nucleus.
Electrons can also be considered negatively charged particles.

30. Quantum Theory
Estimates the probability of finding an electron in a certain position
We denote the position of the electron as a “fuzzy” cloud
This volume of space where an electron is most likely to be found is called an orbital.
The atomic orbitals have distinct shapes

31. Work on Wave WS- 15 min
Go to shape ppt