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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
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 Build Strong Content Knowledge
 Reason abstractly and quantitatively
 Use appropriate tools strategically
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Evaluate: Warm-Up
Explain: Emission Spectra Notes
Engage/Explore: Emission Spectra Lab
Elaborate: Star Spectra WS
Evaluate: Exit Ticket
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Write the abbreviated electron configurations
for the following:
 Au
 Br-
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What is wrong with this abbreviated
configuration for Cl?
 [He]2s22p63s23p5
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Today I will be able to:
 Explore how the photoelectric effect creates
atoms with unique atomic spectra
 Identify the anatomy of electromagnetic waves
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Finish Energy, Wavelength, Frequency
Calculations
Wear closed toe shoes Friday (B-day),
Monday (A-Day)
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Warm – Up
Emission Specta Notes
Emission Spectra Lab
Wavelength, Energy Frequency Calculations
Exit Ticket
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Electrons can be move as waves
When electrons release energy, release in the
form of light photons
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Study of the emission and absorption of light
by atoms and molecules

Wavelength (λ - lambda) – distance between
crests in a wave
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Frequency (v - nu) – number of complete
waves passing a point in a given amount of
time
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Amplitude - distance from wave origin to
peak or crest
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
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Photoelectric Effect
 Electrons are emitted from solids, liquids or gases
when they absorb energy from light.
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Color is seen if the electron falls back to
energy level (n) 2
 This is visible light
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The amount an e- fall determines the
frequency of EM radiation released (n = 1 =
UV; n = 3 infrared)
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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
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Emission Spectra of Hydrogen
1 nm = 1 x 10-9 m = “a billionth of a meter”
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Continuous
 All wavelengths of
visible light are seen
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Line (Emission) Spectra
 Only specific bands of
color are seen
1 nm = 1 x 10-9 m
Rotate from Station to Station to observe line spectrum of different
elements and complete the lab.
Complete the worksheet when you finish your lab.
c = λν
◦ C= 3.0 x 108 m/s (speed of light)
◦ λ = wavelength (meters)
◦ ν = frequency (Hertz or 1/seconds)
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Planck came up with the equation
E= hν
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E = Energy (Joules)
h = Planck’s Constant
 6.626 x 10-34 J*s
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ν = frequency (Hertz or 1/seconds)
Complete the practice at your desk. Ask Ms. Ose for help if you have
questions.
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What is happening to the electrons when we
see color on the emission spectrum?
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Revisit the Blue Electron Exam Study Guide
and Complete the boxes covered in class
today