Name:__________________________ Period:____ Date:____________
WS 5.2
Answer each of the questions below to show your achievement of the lesson objectives
Lesson Objective: Understand the de Broglie wave equation and how it illustrates the wave nature of the electron.
1. The de Broglie wave equation showed that the wavelength of any moving object is equal to a. b. c. d.
2. One of the following statements will not be true if quantum mechanics are used in explanations of particle behavior a. sub-atomic particles display quantum behavior b. wave-particle duality must exist c. some quantum behavior can be observed visually d. discrete energy levels must be shown
3. True or False: The Bohr model of the electron clearly explained why atomic energy states were quantized.
4. True or False: Electrons can only exist in an atom at specific energies.
5. Acceptance of the _____ nature of the electron allowed a new way of understanding how electrons functioned.
6. The Heisenberg Uncertainty Principal states that the _______ and __________ of a particle cannot be determined simultaneously.
7. In an eight-ball pool game, the cue ball can travel 5m/sec. If the cue ball has a mass of 160 g, what is the wavelength it demonstrates?
Lesson Objective: Explain the difference between quantum mechanics and classical mechanics.
8. All of the following statements about classical mechanics are true except one. a. all objects move with wavelike motion b. objects gain or lose energy in any amount c. the materials demonstrate wave-particle duality d. size and mass of objects obscures any quantum effects

Name:__________________________ Period:____ Date:____________
9. The Heisenberg Uncertainty Principle states a. velocity and position can both be determined at the same time b. a beam of light can interfere with the path and speed of an electron c. photons do not affect the position of an electron d. the velocity of a car cannot accurately be measured by a radar beam
10. True or False: Particles described by quantum theory can only lose or gain energy in discrete units.
11. True or False: The Heisenberg Uncertainty Principle says that we can never measure the position and velocity of the moon accurately.
12. Particles whose motions are better described by quantum mechanics can only gain or lose energy in discrete units called _________.
13. The study of motion in large objects is called _______ _________ .
Lesson Objective: Understand how the Heisenberg uncertainty principle and
Sc hrödinger's wave equation led to the idea of atomic orbitals.
14. Which of the following statements about the Schrödinger wave equation is not true? a. the quantum mechanical model of the electron comes from this equation b. this equation supports the Bohr model of electron orbits c. solutions to this equation are called wave functions d. quantization of electron energies is required to solve the equation
15. An electron cloud a. represents a 50% probability of finding an electron b. has uniform density c. can be called an orbital d. can only show where the electron is not located
16. True or False: An orbital represents a three-dimensional area of space.
17. True or False: Electrons travel around the nucleus in circular orbits.
18. The electron cloud represents an area of space where there is a _____% probability of finding an electron.
19. The ___________ wave equation accurately described the behavior of the electron in a hydrogen atom.

Name:__________________________ Period:____ Date:____________
Lesson Objective: Know the four quantum numbers and how they are related to the arrangement of electrons in an atom.
20. Each electron can be described by ___________ quantum numbers. a. 4 b. 3 c. 2 d. 1
21. The quantum numbers describe all the characteristics of an electron except a. velocity b. magnetic spin c. energy level d. orbital shape
22. True or False: The principal quantum number describes the magnetic spin of an electron.
23. True or False: The magnetic quantum number describes the orientation of an orbital.
24. Each orbital can hold a maximum of ____ electrons.
25. The possible values for the spin quantum number are ___ and ____ .
Lesson Objective: Describe the interrelationships between principal energy level, sublevel, orbital and electron spin and how they relate to the number of electrons of an atom.
26. One of the following is not an allowable sublevel for n = 3 a. p b. d c. f d. s
27. For n = 2, the number of orbitals per principal energy level is a. 3 b. 6 c. 1 d. 2

Name:__________________________ Period:____
28. True or False: The p orbitals are dumbbell-shaped.
29. True or False: All s orbitals have complex shapes.
30. The following image represents a _____ orbital.
Date:____________
31.
32. The total number of allowable orbitals for n = 4 is ________.
33. The Heisenberg Uncertainty Principle states that it is impossible to determine simultaneously both the position and the velocity of a particle. The detection of an electron, for example, would be made by way of its interaction with photons of light.
Since photons and electrons have nearly the same energy, any attempt to locate an electron with a photon will knock the electron off course, resulting in uncertainty about where the electron is headed.
34. A running back collides with a defensive tackle and is knocked down. Explain how the Heisenberg Uncertainty Principle applies to this situation.
35. Do a unit analysis of the de Broglie equation to show how an increase in mass affects the wavelength of the moving object.