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Problem Set 13: Wave-mechanical Model
Major Concepts
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Students learn the wave-mechanical model
Identify inadequacies on the Rutherford atomic model
Identify the new assumption in the Bohr model of the atom
Describe the energies and positions of electrons according to the quantum mechanical model
Describe how the shapes of orbitals at different sublevels vary
Describe the relationship between the wavelength and frequency of light
Explain how the frequencies of light are related to changes in electron energies
Distinguish between quantum mechanics and classical mechanics
Identify the cause of the atomic emission spectrum
Reading
Chapter 11.2, 11.3, 11.5, & 11.6
Using one paragraph per section, summarize the two sections you just read.
Reading Guide
Complete Reading Guide 13
Lab
Complete Lab 13
Lecture Notes
Print and read Lecture 13 from TheChemBook; Combine your notes from class with the
notes on TheChemBook. Use the Cornell Notes Strategy to review your notes each night (5
min.).
Vocabulary
Define each vocabulary word.
Electromagnetic radiation
(p. 324)
Frequency (p. 324)
Photons (p. 325)
Quantized (p. 329)
Wavelength (p. 324)
Wave mechanical model
(p. 331)
Questions and Problems
1. What is meant by electromagnetic radiation? Give examples.
2. What is a packet of electromagnetic energy called?
3. What is the relationship between wavelength of light and the energy of photons?
4. What is wrong with the Bohr model of the atom?
5. How does the wave mechanical model of the atom differ from Bohr’s model?
6. What does it mean to say that an atom is in an “excited state”?
7. Discuss briefly the difference between an orbit (as described by Bohr for hydrogen) and
an orbital (as described by the wave mechanical model).
Place your answers to problem set 13 in your 3-ring binder, Unit 1.