Name_______________________________
HW-9
Due Date____________ Period______ Score____/15
1. What is the speed of all forms of electromagnetic radiation? __________________________
2. List all forms of electromagnetic radiation according to increasing frequency:_________________________________
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3. List the colors of light in the visible spectrum according to increasing energy:__________________________________
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4. Which theory of light, the wave or particle theory, best explains the following phenomena?
a. the interference of light?_______________________ b. the photoelectric effect?______________________
c. The emission of electromagnetic radiation by an excited atom?________________________
5. Distinguish between the ground state and an excited state of an atom:_______________________________________
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6. According to Bohr’s model of the hydrogen atom, how is hydrogen’s emission spectrum produced?_______________
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7. Solve for the frequency of light whose wave length is 4.257 x 10-7 cm. (Show work and units)
Answer = ___________________________________
8-9.
a. What is the principle quantum number?_________________________________________________________
b. How is it symbolized?___________
c. What are shells?____________________________________________________________________________
d. What does n relate to the number of electrons allowed per main energy level?_________________________
10.
a. What information is given by the angular momentum quantum number?______________________________
b. What are sublevels, or subshells?______________________________________________________________
11.
a. What information is given by the magnetic quantum?_____________________________________________
b. What many orbital orientations are possible in each of the sublevels? s____
p____
d____
f____
12. a. What information is given by the spin quantum number?_______________________________________________
b. What are the possible values for this quantum number?_______________________________________________
13. a. Sketch the shape of an s orbital and a p orbital.
s=
p=
b. How does a 2s orbital differ from a 1s orbital?__________________________________________________________
c. How do a 2px and a 2py orbital differ?_________________________________________________________________
14-15. a. In your own words, state the Aufau principle.______________________________________________________
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b. State Hund’s rule:_________________________________________________________________________________
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c. State the Pauli exclusion principle_____________________________________________________________________
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d. What is the significance of the spin quantum number?____________________________________________________
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16. Determine the highest occupied energy level in the following elements.
He_____
Be______
Al______
Ca______
Sn_______
17. Write the orbital notation for the following elements:
F
Na
18-19. Write both the complete electron-configuration notation and the noble-gas notation for each of the elements:
a. Na
b. Sr
c. Cu
20-21. Identify each of the following atoms on the basis of its electron configuration:
_____a. 1s22s22p5
_____ c. [Ne] 3s23p5
_____b. [Ar] 4s1
_____ d. [Ar] 4s23d6
22. Draw a chart showing the electron orbital filling order.
23-24. Write the short-hand (noble gas) notation for the electron configurations of each of the following elements:
a. As
b. Pb
c. La
d. Lr
25. How do the electron configurations of chromium and copper contradict the Aufbau principle?___________________
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26-28. a. Write the electron configuration for phosphorus:
b. How many electrons are in each atom?
c. What is the atomic number of this element?
d. Write the orbital notation for this element:
e. How many unpaired electrons does an atom of phosphorus have?
f. What is its highest occupied energy level?
g. How many inner-shell electrons does the atom contain?
h. In which orbital(s) are these inner-shell electrons located?
______29. What is the maximum number of unpaired electrons that can be placed in a 3p sublevel?
a. 1
b. 2
c. 3 d. 4
30. (Refer to the “photoelectric effect” in you book [p.99]) When blue light shines on potassium metal in a photocell,
electrons are emitted. But when yellow light shines on the metal, no current is observed. Explain:
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