Download Ch 5 Set #3

Name: _________________________________________ Hr: ________ Date: _______
Ch 5 Set #3
1. What is the symbol for frequency? ______________________ unit? ___________________________
2. What is the symbol of the SI unit of frequency (not the name of the unit)? ____________________
3. What is the speed of light? _______________________________________________
4. What is Planck’s constant? _______________________________________________
5. Calculate the wavelength of a photon if the frequency is 3.4 x 104 Hz. Solve variable equation for appropriate variable, plug in
numbers, all units must cancel leaving desired unit.
6. Calculate the energy of the photon based on the info in question #6. Solve variable equation for appropriate variable, plug in
numbers, all units must cancel leaving desired unit.
7. Calculate the energy of a photon with a wavelength of 760 m. Solve variable equation(s) for appropriate variable, plug in numbers,
all units must cancel leaving desired unit.
8. Describe the relationships between the following as “inverse”, “direct”, or “no relationship”
Speed of light
Wavelength
Frequency
Energy
Speed of light
Planck’s constant
Wavelength
Frequency
Energy
Planck’s constant
9. There are eight main areas of the electromagnetic spectrum, and one of those eight areas contains 7 colors. Write the
electromagnetic spectrum in order of largest frequency to smallest frequency, and include the names of the 7 colors in proper
order in the appropriate category.
10. Draw a transverse wave and label the amplitude, wavelength, crest, trough, and frequency.
11. Which color has the longest wavelength? ________________ What is the wavelength? ______________________
12. Which color has the shortest wavelength? ________________ What is the wavelength? ______________________
13. Choose between the terms “high” or “low”
a. If an electron moves from a ______________________ energy level to a __________________ energy level, energy is
EMITTED as electromagnetic energy.
b. If an electron moves from a _______________________ energy level to a _________________ energy level, energy is
ABSORBED as electromagnetic energy.
Name: _________________________________________ Hr: ________ Date: _______
14. True or False: When an electron moves back down energy levels, it emits as much EM energy as it took to move up the energy
levels.
15. True or False: Electrons can only move up energy levels by absorbing light from the visible spectrum.
16. True or False: Electrons can only emit light from the visible portion of the EM spectrum when dropping energy levels.
17. True or False: Electrons will only move if it absorbs photons that are exactly the right amount of energy needed to get them to a
higher energy level.
18. How did Einstein use Planck’s theory to support the concept that EM waves can also act as particles? Name the concept.
19. Will infrared photons cause the strip to glow in the dark (class example)? UV photons? Why and what is the difference?
20. In figure 5.14, an atom of hydrogen is energized and produces light that has too little energy to be seen by the human eye. Which
energy level did the electron start from? __________________Name the series. _____________________
21. In figure 5.14, an atom of hydrogen is energized and produces light that can be seen by the human eye. Which energy level did
the electron start from? _________________________Name the series. ________________________
22. Explain the steps required for light to be produced by the metals in the flame tests (NOT lab procedures).
23. Did your eyes detect the “atomic emission spectra” for each tested metal in the flame test? Explain.
24. Picture two hydrogen atoms. The electron in the first hydrogen atom is in the n = 1 energy level. The electron in the second
hydrogen atom is in the n = 4 level.
a. Which atom has the ground state electron
c. In which atom is the electron farther from the
configuration?
nucleus?
b. Which atom can emit electromagnetic radiation?
d. In which atom does the electron have less energy?
25. For each of the configurations below, label as “ground state”, “excited state”, or “impossible configuration”.
b. 1s22s22p63s23p64s1
c. 1s22s22p63s23p7
a. 2s22p63s23p64s2
26. Draw a Bohr model of Hydrogen (such as F5.14) with three rings around the nucleus and one electron in the first ring.
a. Label the energy levels n =1, n = 2, n = 3…remember
the distance between n changes as n increases
b. Label the ground state.
c. Label an excited state.
d. Draw a straight arrow to show the direction an
electron moves when it absorbs energy.
e. Draw squiggly arrow to show the direction an electron
moves when it emits energy.