1. What’s wrong with this picture?
Take out:
-Your lab notebook open to your warm up section
-Examining Emission Spectra & Getting Charged W.S.
-Grab your homework sheet! (Back Table)

2. Warm-up
How are atoms “excited” in the element tubes? What does it mean the atoms are “excited”?
In an emission spectra what color has the lowest energy?
RED

3. An Excited Electron  Emission
Energy
Photon of
light
emitted
Ground energy state
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 326

4. Review Homework- 6 minutes With a partner:
Discuss what the biggest difference between how the incandescent bulb works compared to the element tube?
Compare each others drawings for #3.
Were they the same? Different?
Why did you chose to draw it like that?
Left side partner: Explain #4 to right partner
Right partner: Explain #5 to left partner
Where are you (individually) on the LT? Record this on your HW sheet, then turn in

5. Why More Lines than Electrons?He Ne

6. Every atom is quantized!
Excited states!
Quantized – only certain values for energy levels are allowed
Every atom is quantized!
Ground State

7. An Excited Electron  Emission
Energy
Photon of
light
emitted
Ground energy state
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 326

8. Electron Ladders: Absorption
Electrons can only be at
specific energy levels,
NOT between levels.
The farther an electron falls,
the higher energy photon
it gives off
Ex: red= little fall
Ex: ultra violet= big fall!
Excited state
Ground state e- e-

9. Niels Bohr's Experiment
Bohr examined the emission spectra of Hydrogen and created a model of the atom based on his data
Thought electrons had restricted, circular orbits around the nucleus
Fit his hydrogen data perfectly!
Did not fit other atoms 

11. Why is this important?
Electrons in hydrogen atoms can only have specific energy levels since they can only give off certain colors
We can use the colors to hypothesize how electrons orbit each atom!
Ex: can use info to find out what stars are made of

12. Bohr and the Quantum Theory
When electrons fall they release Light Energy
Explains:
Empty spaces
Why electrons didn’t get “sucked” into the nucleus
Clip: Bohr’s Model of the Atom

13. Safety! Tie hair back! Goggles! Common sense! Awareness!
Help your buddy!

15. Flame Emission Spectra
Photographs of flame tests of burning wooden splints soaked in different salts.
methane gas
wooden splint
sodium ion
calcium ion
copper ion
strontium ion
Include link to web page

16. Fireworks

17. Homework: Finish Flame Lab Exit Task
What part of the atom is giving off the light, and how it is happening? (draw it using a bohr model!!)
Homework:
Finish Flame Lab