Download Light and Quantized Energy

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Light and Quantized Energy
Section 5.1
Read pages 136-145 in your textbook. Complete the guided notetaking questions. Also, it wouldn’t be a
bad idea for you to add any other notes that you think may be important as you read and try some extra
practice problems from this section to become more familiar with it.
Main Idea:
Scan Section 1 of your text. Use the checklist below as a guide.
• Read all section titles
• Read all boldfaced words
• Read all tables and graphs
• Look at all pictures and read the captions
Write three facts you discovered about light.
1.
2.
3.
Define each term from your text.
• Electromagnetic radiation
•
Wavelength
•
Frequency
•
Amplitude
•
Electromagnetic spectrum
•
Quantum
•
Planck’s constant
•
Photoelectric effect
•
Photon
•
Atomic emission spectrum
List the three reasons scientists found Rutherford’s nuclear atomic model to be fundamentally incomplete.
1.
2.
3.
Draw the wave diagram in Figure 3 (pg 138). Be sure to include all labels.
Explain the relationship shown by the figure you drew above. Use the following terms: wavelength,
frequency, amplitude, and speed.
Describe what white light is and what is produced when it goes through a prism.
Use diagram on page 139 to label the diagram below. Note, they are not exactly the same but do have all
the same info. You need to include everything except the wavelength and frequency numbers. Also,
since this diagram is not in color, either color or label the colors of the visible light spectrum (no indigo).
Explain the relationship between wavelength, frequency, and energy. Which of the visible colors has the
highest energy?
Why do you think that UV rays are so harmful to your skin? (not in the book)
Solve Read Example Problem 1 in your text. Do practice problems 1-4 on page 140. Answers to 1 and 3
are in the appendix.
Identify two facts the wave model of light failed to explain.
1.
2.
Describe Planck’s quantum concept by completing the following statement.
The quantum concept concludes that matter can gain or lose _____________ only in small, specific
amounts called _______________. A quantum is the minimum amount of energy that can be
________________ or _____________ by an atom.
Compare and contrast Einstein’s equation with Planck’s equation by completing the following
sentences.
Planck’s equation _________________, demonstrates mathematically that the energy of a quantum is
related to the _______________ of the emitted radiation. Einstein went further by explaining that, in
addition to its wavelike characteristics, a beam of light can be thought of as a stream of
________________ called ________________.
Contrast the continuous electromagnetic spectra and the atomic emission spectra.
Quantum Theory and the Atom
Section 5.2
Read pages 146-155 in your textbook and complete the guided notetaking questions.
Main Idea:
Use your text to define each term.
• Ground state
•
Quantum number
•
de Broglie equation
•
Heisenberg uncertainty principle
•
Quantum mechanical model of an atom
•
Atomic orbital
•
Principal energy level
•
Energy sublevel
Explain why different colors of light result from electron behavior in the atom.
Compare and Contrast the Bohr and quantum mechanical models of the atom.
Describe the impact of the de Broglie’s wave-particle duality and the Heisenberg uncertainty principle on
the current view of the electrons in atoms.
Explain the relationship between energy levels and sublevels.
Label Using Figure 17 on page 154, label the diagram below and describe the shapes of each orbital
(don’t worry about the shape of the f orbital). Be sure to include how many electrons can be held in each
orbital (table 2, page 155, may be helpful).