Chemistry
Mr. Reger
Review Guide – Ch. 11
Name ________________________
Date ______________ Period _____
1. Which of the following is not an example of electromagnetic radiation?
a. X-rays
b. Visible light
c. Sound waves
d. UV rays
e. All of the above are examples of electromagnetic radiation
2. Which of the following statements about atomic structure is incorrect?
a. electrons are located around the nucleus
b. when an electron moves to a higher energy level, it is farther from the nucleus
c. electrons move in circular orbits around the nucleus
d. none of the above are true
e. all of the above are true
3. The distance between two crests (or two troughs) in a wave is called the
a. frequency
b. wavelength
c. speed
d. amplitude
e. color
4. An orbital can be described as
a. a path followed by the electron
b. the direction in which the electron is moving
c. the wavelength of the electron
d. an area in space where the electron is likely to be found
e. none of the above
5. A photon with a longer wavelength will have
a. lower energy
b. higher energy
c. lower frequency
d. higher frequency
e. a and c
f. b and d
6. The fact that the emission spectrum of hydrogen consists of lines (rather than a continuous
spectrum) led scientists to what conclusion?
a. the energy of the hydrogen atom is quantized
b. every color of light can be emitted from an excited H atom
c. the Bohr model is incorrect
d. all of the above
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7. How many valence electrons are there in an atom of calcium?
a. 1
b. 2
c. 3
d. 4
e. 5
8. How many valence electrons are there in an atom of sulfur?
a. 2
b. 4
c. 5
d. 6
e. 8
9. How many unpaired electrons are there in an atom of Se?
a. 1
b. 2
c. 3
d. 4
e. 5
10. How many unpaired electrons are there in an atom of cobalt?
a. 1
b.2
c. 3
d. 4
e. 5
11. Which of the following orbitals is highest in energy?
a. 1s
b. 2s
c. 3s
d. 4s
e. 5s
12. Which of the following orbitals is highest in energy?
a. 5s
b. 5p
c. 5d
d. 5f
e. 5g
13. How many sublevels are there in the fourth energy level (n=4)?
a. 1
b. 2
c. 3
d. 4
e. 5
14. Which is NOT a valid orbital designation?
a. 6s
b. 3p
c. 4f
d. 2d
e. 1s
15. Which of the figures below represents a p orbital?
a.
b.
c.
d.
e.
16. Which of the figures below represents an s orbital?
a.
b.
c.
d.
e.
17. Write the complete electron configuration for magnesium.
18. Write the complete electron configuration for cadmium.
19. Write the complete electron configuration for arsenic (As).
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20. Write the complete orbital diagram for carbon.
21. How many unpaired electrons does a carbon atom have?
22. Write the complete orbital diagram for sulfur.
23. How many unpaired electrons does a sulfur atom have?
24. Write the complete orbital diagram for nickel.
25. How many unpaired electrons does a nickel atom have?
26. In terms of atomic size, which of the following is NOT true?
a. F < B < Li
b. I > Br > F
c. Na < Cs < Fr
d. Rb > Sr > Xe
e. C > Si > Ge
27. In terms of atomic size, which of the following is true?
a. Ca > Cr > K
b. Be < Ba < Ra
c. B < N < O
d. Ne > Ar > Kr
e. Fe < Ga < Br
28. In terms of ionization energy, which of the following is true?
a. Na > Mg > Al
b. Na < K < Rb
c. Ba < Ca < Be
d. Br < Se < As
e. F < O < N
29. Moving down the periodic table, does atomic size increase or decrease? Explain why.
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30. Moving across the periodic table (from left to right), does atomic size increase or decrease?
Explain why.
31. Moving down the periodic table, does ionization energy increase or decrease? Explain why.
32. Moving across the periodic table (from left to right), does ionization energy increase or
decrease? Explain why.
33. How many electrons can there be in one s orbital?
a. 1
b. 2
c. 3
d. 4
e. 5
34. How many electrons can there be in the 4d sublevel?
a. 2
b. 5
c. 6
d. 10
e. 14
35. Using the shorthand notation (with a noble gas core), write the electron configuration for
barium.
36. How many valence electrons does barium have?
37. How many unpaired electrons does barium have?
38. Using the shorthand notation (with a noble gas core), write the electron configuration for Sn.
39. How many unpaired electrons does tin have?
40. What was Erwin Schrodinger’s contribution to our understanding of the structure of the
atom?
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1. C
2. C
3. B
4. D
5. E
20.
6. A
7. B
8. D
9. B
10. C
11. E
12. E
13. D
14. D
15. C
↑↓
1s
↑↓ ↑_ ↑_ __
2s
2p
↑↓
1s
↑↓ ↑↓ ↑↓ ↑↓
2s
2p
↑↓ ↑↓ ↑_ ↑_
3s
3p
↑↓
1s
↑↓ ↑↓ ↑↓ ↑↓
2s
2p
↑↓ ↑↓ ↑↓ ↑↓
3s
3p
16. B
17. 1s2 2s22p6 3s2
18. 1s2 2s22p6 3s23p6 4s23d104p6 5s24d10
19. 1s2 2s22p6 3s23p6 4s23d104px14py14pz1
21. 2
22.
23. 2
24.
↑↓
4s
↑↓ ↑↓ ↑↓ ↑_ ↑_
3d
25. 2
26. E
27. B
28. C
29. Atomic size increases. Moving down the Periodic Table, additional electrons are added to a
new energy level. Since the higher energy levels are farther from the nucleus, the atomic radius
increases.
30. Atomic size decreases. Although additional electrons are being added, they are being added
to the same energy level and are therefore no farther from the nucleus. Since more protons are
being added as well, the positive charge in the nucleus is increasing and therefore pulls the
electrons closer to the nucleus.
31. Ionization energy decreases. The highest energy electron is farther from the nucleus and is
therefore easier (i.e., requires less energy) to remove.
32. Ionization energy increases. The highest energy electron is closer to the nucleus and is
therefore harder (i.e., requires more energy) to remove.
33. B
34. D
35. [Xe] 6s2
36. 2
37. 0
38. [Kr] 5s2 4d10 5px15py1
39. 2
40. He treated the electron as a wave and developed the idea of orbitals.
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