Name: ______________________ Class: _________________ Date: _________
ID: A
Chemical Bonding - Practice Questions
Multiple Choice
Identify the choice that best completes the statement or answers the question.
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1. What is the name given to the electrons in the highest occupied energy level of an atom?
a. orbital electrons
c. anions
b. valence electrons
d. cations
2. How does calcium obey the octet rule when reacting to form compounds?
a. It gains electrons.
b. It gives up electrons.
c. It does not change its number of electrons.
d. Calcium does not obey the octet rule.
3. What is the charge on the strontium ion?
a. 2–
c. 1+
b. 1–
d. 2+
4. How many electrons does barium have to give up to achieve a noble-gas electron configuration?
a. 1
c. 3
b. 2
d. 4
5. What is the formula of the ion formed when potassium achieves noble-gas electron configuration?
a.
____
K
2+
b.
+
a.
Fe
c. K 1 −
2−
K
d. K
6. Which of the following ions has a pseudo-noble-gas electron configuration?
7.
____
8.
____
9.
____
10.
c. Cu +
2+
+
Mn
d. Ni
Which of the following elements does NOT form an ion with a charge of 1+?
a. fluorine
c. potassium
b. hydrogen
d. sodium
What is the charge on the cation in the ionic compound sodium sulfide?
a. 0
c. 2+
b. 1+
d. 3+
Which of the following occurs in an ionic bond?
a. Oppositely charged ions attract.
b. Two atoms share two electrons.
c. Two atoms share more than two electrons.
d. Like-charged ions attract.
What is the net charge of the ionic compound calcium fluoride?
a. 2–
c. 0
b. 1–
d. 1+
b.
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2+
1
Name: ______________________
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11. How many valence electrons are transferred from the nitrogen atom to potassium in the formation of
the compound potassium nitride?
a. 0
b. 1
12. How many valence electrons are transferred
compound calcium iodide?
a. 0
b. 1
13. What is the formula unit of sodium nitride?
a. NaN
b.
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Na 2 N
c. 2
d. 3
c. Na 3 N
d. NaN 3
Al 3 O
d. Al 2 O 3
Na 2 SO 4
d. Na 2 (SO 4 ) 2
17. What is the formula for potassium sulfide?
a. KS
b.
____
from the calcium atom to iodine in the formation of the
15. What is the name of the ionic compound formed from lithium and bromine?
a. lithium bromine
c. lithium bromium
b. lithium bromide
d. lithium bromate
16. What is the formula for sodium sulfate?
a. NaSO 4
c. Na(SO 4 ) 2
b.
____
c. 2
d. 3
14. What is the formula unit of aluminum oxide?
a. AlO
c. AlO 3
b.
____
ID: A
c. KS 2
K2 S
d. K 2 S2
18. Which of the following pairs of elements is most likely to form an ionic compound?
a. magnesium and fluorine
c. oxygen and chlorine
b. nitrogen and sulfur
d. sodium and aluminum
19. Which of these elements does not exist as a diatomic molecule?
a. Ne
c. H
b. F
d. I
20. How do atoms achieve noble-gas electron configurations in single covalent bonds?
a. One atom completely loses two electrons to the other atom in the bond.
b. Two atoms share two pairs of electrons.
c. Two atoms share two electrons.
d. Two atoms share one electron.
21. Why do atoms share electrons in covalent bonds?
a. to become ions and attract each other
b. to attain a noble-gas electron configuration
c. to become more polar
d. to increase their atomic numbers
2
Name: ______________________
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22. Which of the following elements can form diatomic molecules held together by triple covalent bonds?
a. carbon
c. fluorine
b. oxygen
d. nitrogen
23. Which of the following is the name given to the pairs of valence electrons that do not participate in
bonding in diatomic oxygen molecules?
a. unvalenced pair
c. inner pair
b. outer pair
d. unshared pair
24. Which of the following diatomic molecules is joined by a double covalent bond?
a. O 2
c. N 2
b.
____
ID: A
Cl 2
d. He 2
25. A molecule with a single covalent bond is ____.
a. CO 2
c. CO
b.
Cl 2
d. N 2
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26. Once formed, how are coordinate covalent bonds different from other covalent bonds?
a. They are stronger.
c. They are weaker.
b. They are more ionic in character.
d. There is no difference.
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27. When H + forms a bond with H 2 O to form the hydronium ion H 3 O + , this bond is called a coordinate
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28.
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29.
____
30.
____
31.
covalent bond because ____.
a. both bonding electrons come from the oxygen atom
b. it forms an especially strong bond
c. the electrons are equally shared
d. the oxygen no longer has eight valence electrons
Which of the following atoms acquires the most negative charge in a covalent bond with hydrogen?
a. C
c. O
b. Na
d. S
Which of the following covalent bonds is the most polar?
a. H—F
c. H—H
b. H—C
d. H—N
What causes hydrogen bonding?
a. attraction between ions
b. motion of electrons
c. sharing of electron pairs
d. bonding of a covalently bonded hydrogen atom with an unshared electron pair
Why is hydrogen bonding only possible with hydrogen?
a. Hydrogen’s nucleus is electron deficient when it bonds with an electronegative atom.
b. Hydrogen is the only atom that is the same size as an oxygen atom.
c. Hydrogen is the most electronegative element.
d. Hydrogen tends to form covalent bonds.
3
ID: A
Chemical Bonding - Practice Questions
Answer Section
MULTIPLE CHOICE
1. ANS:
OBJ:
2. ANS:
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3. ANS:
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4. ANS:
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18. ANS:
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20. ANS:
OBJ:
B
7.1.1
B
7.1.1
D
7.1.2
B
7.1.3
B
7.1.3
C
7.1.3
A
7.1.3
B
7.2.1
A
7.2.1
C
7.2.1
A
7.2.1
C
7.2.1
C
7.2.1
D
7.2.1
B
7.2.1
B
7.2.1
B
7.2.1
A
7.2.1
A
8.2.1
C
8.2.1
PTS:
STA:
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1
DIF: L1
Ch.1.c | Ch.2.a
1
DIF: L1
Ch.1.c | Ch.2.a
1
DIF: L1
Ch.1.c | Ch.2.g
1
DIF: L1
Ch.1.c | Ch.2.a | Ch.1.d
1
DIF: L1
Ch.3.a
1
DIF: L1
Ch.1.g
1
DIF: L1
Ch.1.g
1
DIF: L1
Ch.2.a
1
DIF: L1
Ch.2.a
1
DIF: L1
Ch.3.a
1
DIF: L2
Ch.2.a
1
DIF: L2
Ch.2.a
1
DIF: L2
Ch.3.a
1
DIF: L2
Ch.3.a
1
DIF: L2
Ch.2.a
1
DIF: L2
Ch.3.a
1
DIF: L2
Ch.3.a
1
DIF: L3
Ch.2.a
1
DIF: L1
Ch.2.a
1
DIF: L2
Ch.2.a
1
REF:
p. 187
REF:
p. 188
REF:
p. 190
REF:
p. 190
REF:
p. 190
REF:
p. 190
REF:
p. 190
REF:
p. 194
REF:
p. 194
REF:
p. 194
REF:
p. 194
REF:
p. 194
REF:
p. 195
REF:
p. 195
REF:
p. 192 | p. 195
REF:
p. 192 | p. 195
REF:
p. 192 | p. 195
REF:
p. 194
REF:
p. 217
REF:
p. 217
ID: A
21. ANS:
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28. ANS:
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29. ANS:
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30. ANS:
OBJ:
31. ANS:
OBJ:
B
8.2.1
D
8.2.1
D
8.2.2
A
8.2.3
B
8.2.1 | 8.2.4
D
8.2.4
A
8.2.4
C
8.4.1
A
8.4.1
D
8.4.3
A
8.4.1 | 8.4.3
PTS:
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1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
1
Ch.2.a
2
DIF:
L2
REF:
p. 217
DIF:
L2
REF:
p. 221
DIF:
L1
REF:
p. 218
DIF:
L2
REF:
p. 221
DIF:
L2
REF:
p. 222
DIF:
L2
REF:
p. 223
DIF:
L2
REF:
p. 225
DIF:
L2
REF:
p. 238 | p. 239
DIF:
L3
REF:
p. 238 | p. 239
DIF:
L2
REF:
p. 241
DIF:
L2
REF:
p. 241