1. Activity 5: The Electronic Behavior of Atoms1

3. What do those colors mean???
ROY G BIV 3

4. The nature of Light 4

5. The electromagnetic spectrum
Wavelength decreases, frequency increases, Energy increases 5

6. Waves
The is the_____________ distance from the crest (top) of one wave to the crest of the next. 6

7. The _____________ of a wave is defined as how many cycles of a wave pass through a point per second The __________ the wavelength = the __________the frequency
Short wavelength
Long wavelength 7

8. Visible Region
As you move from _______ to Violet light, the wavelength of the waves____________.
An___________ the frequency of the wave and an increase in _____________ of the wave. 8

9. __________________ are associated with ____________.
What does this mean?
__________________ are associated with ____________.
_______ light has the least energy, while _________ light has the most energy. 9

11. Dan Flavin

13. Bohr’s “_____________ Model”
__________ are in fixed ________ levels around the ________
Energy levels get ______ together as they get ________ from the nucleus.
Think of a ladder that isn’t equally spaced + 13

14. How did Niels Bohr arrive at this model?
Flame Test Experiment 14

15. Bohr observed the flame colors through an instrument that ____________ the light into its component _________---just like a prism! 15

16. Spectroscope 16

17. ATOMIC EMISSION SPECTRUM
When the ______ colors are observed through a spectroscope, a pattern of_______
________ appears 17

18. ATOMIC EMISSION SPECTRUM
The bands of light are called
______________________________________
All elements have a __________
pattern of spectral lines that can be used to _________ the _____________.
This spectrum is ____________ to every _________________.

19. Why do we see this? ATOMIC EMISSION SPECTRUM
__________ can get “excited” and move from ________energy levels to ________energy levels by ______________energy.
When they ________________down to a ____________energy level the electron loses energy in the form of ___________.
ATOMIC EMISSION SPECTRUM

20. Atomic Emission Spectrum
Add energy

21. So… Electrons start off in the __________________________.
They absorb energy and move to the _________________________.
They then ________ this absorbed energy fall back down to the groundstate and _________ light!