1. Emission Spectra Lab

2. Common Core Connection
Today I will be able to:
Explore how the photoelectric effect creates atoms with unique atomic spectra
Identify the anatomy of electromagnetic waves
Informal assessment – monitoring student interactions and questions as they complete the lab
Formal assessment – analyzing student responses to the lab and exit ticket
Common Core Connection
Build Strong Content Knowledge
Reason abstractly and quantitatively
Use appropriate tools strategically

3. Lesson Sequence Evaluate: Warm-Up Explain: Emission Spectra Notes
Engage/Explore: Emission Spectra Lab
Elaborate: Star Spectra WS
Evaluate: Exit Ticket

4. Warm-Up
Write the abbreviated electron configurations for the following: Au
Br-
What is wrong with this abbreviated configuration for Cl?
[He]2s22p63s23p5
Take out the worksheet you completed for homework

5. Objective Today I will be able to:
Explore how the photoelectric effect creates atoms with unique atomic spectra
Identify the anatomy of electromagnetic waves
Explain the quantum model and photoelectric effect. [GT]
a. Describe the process that creates atomic spectra.
b. Explain the uniqueness of atomic spectra.
c. Provide examples of the common applications of atomic spectra, i.e. analysis of a mixture using atomic spectra.
d. Describe the relative energies of ultraviolet, visible, infrared, microwave, X-ray, radio, and TV waves. [GT]
e. Distinguish between absorption (excitation) and emission of energy. [GT]
f. Describe the properties of light. (i.e. wavelength, frequency and energy)
g. Calculate the wavelength, frequency and energy for a given electron transition. [GT]

6. Homework Finish Star Spectra WS Wear closed toe shoes Tuesday
STEM Fair Conclusion

7. Agenda Warm – Up Emission Specta Notes Emission Spectra Lab
Exit Ticket

8. Emission Spectra

9. According to the Quantum Model…
Electrons can be move as waves
When electrons release energy, release in the form of light photons

10. Spectroscopy
Study of the emission and absorption of light by atoms and molecules

11. Anatomy of a wave

12. Electromagnetic Spectrum

13. Electromagnetic Spectrum

14. Anatomy of a wave
Wavelength (λ - lambda) – distance between crests in a wave
Frequency (v - nu) – number of complete waves passing a point in a given amount of time
Amplitude - distance from wave origin to peak or crest

15. Bohr Model of Atom Electrons are found on specific energy levels
When electrons absorb energy, they more to a higher energy level
When electrons emit energy, they move to a lower energy level and release light energy

16. Absorption and Emission of Electrons

17. Absorption of Energy Photoelectric Effect
Electrons are emitted from solids, liquids or gases when they absorb energy from light.

18. Emitted Light
Color is seen if the electron falls back to energy level (n) 2
This is visible light
The amount an e- fall determines the frequency of EM radiation released (n = 1 = UV; n = 3 infrared)

19. Emitted Light
No two elements give off the same spectra of colors, because they vary in the number of protons and electrons
Emit their own unique line spectra
Can be used to identify elements

20. Line Spectra Emission Spectra of Hydrogen
1 nm = 1 x 10-9 m = “a billionth of a meter”

21. Continuous vs. Line spectra
All wavelengths of visible light are seen
Line (Emission) Spectra
Only specific bands of color are seen
1 nm = 1 x 10-9 m

22. Rotate from Station to Station to observe line spectrum of different elements and complete the lab.
Emission Spectrum Lab

23. Complete the worksheet when you finish your lab.
Star Spectra WS

24. Exit Ticket
What is happening to the electrons when we see color on the emission spectrum?