Name:_________________________
Period:__
Date:___________
WS 5.1
Answer each of the questions below to show your achievement of the lesson objectives
Lesson Objective: Describe the relationships between speed, wavelength, and
frequency of light.
1. Light travels at a speed of ________ m/s
a. 2.998×105
b. 3×108
c. 3×106
d. 2.998×107
2. One of the following is not true of a wave
a. a wave with a short wavelength has a high frequency
b. frequency is usually measured in cycles/second
c. the amplitude is the width of the wave
d. c=λv
3. True or False: Electromagnetic radiation is a form of energy that exhibits wavelike
behavior.
4. True or False: The wavelengths of visible light are longer than those of infrared light.
5. Waves are characterized by their ________ motion.
6. A __________ is characterized as the distance between any two corresponding
points on adjacent waves.
7. Blue light in the visible spectrum has a frequency of approximately 630 THerz (1
THerz = 1012 cycles/sec). What is the wavelength of this light?
Lesson Objective: Understand the photoelectric effect and how it is related to the
wave-particle duality of light.
8. Light from a heated body is emitted
a. at all wavelengths
b. at only one or two wavelengths
c. at certain specific wavelengths
d. in no discernible pattern
9. A _______ is the minimum amount of energy that can be gained or lost by an
electron.
a. qualim
Name:_________________________
Period:__
Date:___________
b. quanta
c. quentum
d. quantum
10. True or False: A photon has the mass of one electron.
11. True or False: Einstein proposed that light could behave as a particle.
12. Light shined onto a _____ surface causes the ejection of _____ from that metal.
13. The _________ frequency needed to cause the ejection of electrons is referred to as
the _______ frequency.
14. What is the energy of a photon of light with a frequency of 690 THerz?
15. What is the frequency of a photon with a E of 3.51×10−19J?
Lesson Objective: Describe how changes in electron energies lead to atomic
emission spectra.
16. Energy levels of electrons in an atom are
a. equal
b. quantumized
c. continuous
d. quantized
17. There are _______ visible lines in the hydrogen atomic emission spectrum.
a. four
b. three
c. two
d. one
18. True or False: Electrons move to higher energy levels when they absorb energy.
19. True or False: Light emitted from electrons is composed of continuous wavelengths.
20. Light is emitted when electrons ________ to ________ energy levels.
21. White light viewed through a prism give a __________ spectrum.
22. Atomic emission spectra led a new ______ of the atom based on ______ _______.
Lesson Objective: Describe the Bohr model of the atom.
23. The Balmer series of hydrogen emission lines appear in the ______ region.
a. infrared
Name:_________________________
Period:__
Date:___________
b. visible
c. ultraviolet
d. far infrared
24. The Bohr model of the atom is sometimes referred to as the _______model.
a. orbital
b. quantum
c. planetary
d. solar system
25. The Lyman series has ______ different possible electron transitions.
a. seven
b. three
c. four
d. six
26. True or False: All the lines of the hydrogen emission spectrum appear in the visible
range.
27. True or False: The Bohr model of the atom only works for the hydrogen atom.
28. True or False: The Brackett series of hydrogen electron transitions drop electrons
from higher energy levels to energy level 4.
29. The series of emission lines from transitions of hydrogen electrons to energy level
three are called the _________ series.
30. The hydrogen emission lines indicate that the electrons were arranged into specific
_______ levels.
31. Low frequency light (red) is unable to cause ejection of electrons from the metal
surface. At or above the threshold frequency (green), electrons are ejected.
Incoming light that has the same intensity but a higher frequency (blue) causes the
ejection of the same number of electrons, but the ejected electrons move at a
greater speed.
32. Why would higher frequency light cause ejected electrons to move at a greater
speed?
33. Why are there more emission lines for helium than for hydrogen? Why is the
emission spectrum of iron so complex?
Name:_________________________
Period:__
Date:___________