Chapter 8 and 9 test

Name: ________________________ Class: ___________________ Date: __________
ID: A
Chapter 8 and 9 Test
Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
____
____
____
____
____
1. What type of ions have names ending in -ide?
a. only cations
c. only metal ions
b. only anions
d. only gaseous ions
2. When Group 2A elements form ions, they ____.
a. lose two protons
c. lose two electrons
b. gain two protons
d. gain two electrons
3. When naming a transition metal ion that can have more than one common ionic charge, the numerical value
of the charge is indicated by a ____.
a. prefix
c. Roman numeral following the name
b. suffix
d. superscript after the name
4. Aluminum is a group 3A metal. Which ion does A1 typically form?
c. Al 5 −
a. Al 3 −
b. Al 3 +
d. Al 5 +
5. Which of the following compounds contains the Mn 3 + ion?
a. MnS
c. Mn 2 O 3
b.
____
____
____
d.
MnO
6. How are chemical formulas of binary ionic compounds generally written?
a. cation on left, anion on right
b. anion on left, cation on right
c. Roman numeral first, then anion, then cation
d. subscripts first, then ions
7. Which of the following formulas represents an ionic compound?
a. CS 2
c. N 2 O 4
b.
____
MnBr 2
BaI 2
d.
PCl 3
8. Which element, when combined with fluorine, would most likely form an ionic compound?
a. lithium
c. phosphorus
b. carbon
d. chlorine
9. Which of the following shows correctly an ion pair and the ionic compound the two ions form?
a.
Sn 4 + , N 3 − ; Sn 4 N 3
c.
Cr 3 + , I − ; CrI
b.
Cu 2 + , O 2 − ; Cu 2 O 2
d.
Fe 3 + , O 2 − ; Fe 2 O 3
____ 10. In which of the following is the name and formula given correctly?
a. sodium oxide, NaO
c. cobaltous chloride, CoCl 3
b.
barium nitride, BaN
d.
stannic fluoride, SnF 4
____ 11. Which of the following compounds contains the lead(II) ion?
a. PbO
c. Pb2O
b. PbCl4
d. Pb2S
1
Name: ________________________
ID: A
____ 12. Molecular compounds are usually ____.
a. composed of two or more transition elements
b. composed of positive and negative ions
c. composed of two or more nonmetallic elements
d. exceptions to the law of definite proportions
____ 13. Which of the following correctly shows a prefix used in naming binary molecular compounds with its
corresponding number?
a. deca-, 7
c. hexa-, 8
b. nona-, 9
d. octa-, 4
____ 14. Which of the following formulas represents a molecular compound?
a. ZnO
c. SO 2
b.
Xe
d.
BeF 2
____ 15. When naming acids, the prefix hydro- is used when the name of the acid anion ends in ____.
a. -ide
c. -ate
b. -ite
d. -ic
____ 16. Which of the following shows both the correct formula and correct name of an acid?
c. H 3 PO 4 , phosphoric acid
a. HClO 2 , chloric acid
b.
HNO 2 , hydronitrous acid
____ 17. What is the formula for sulfurous acid?
a. H 2 SO 4
b.
H 2 SO 3
d.
HI, iodic acid
c.
H 2 SO 2
d.
H2 S
____ 18. How are bases named?
a. like monatomic elements
c.
b. like polyatomic ions
d.
____ 19. Select the correct formula for sulfur hexafluoride.
c.
a. S 2 F 6
b.
F 6 SO 3
d.
like ionic compounds
like molecular compounds
F6 S2
SF 6
____ 20. Which of the following is the correct name for N 2 O 5 ?
a. nitrous oxide
b. dinitrogen pentoxide
____ 21. What is the correct name for Sn 3 (PO 4 ) 2 ?
c.
d.
nitrogen dioxide
nitrate oxide
a. tritin diphosphate
c. tin(III) phosphate
b. tin(II) phosphate
d. tin(IV) phosphate
____ 22. Which is a typical characteristic of an ionic compound?
a. Electron pairs are shared among atoms.
b. The ionic compound has a low solubility in water.
c. The ionic compound is described as a molecule.
d. The ionic compound has a high melting point.
____ 23. Which of these elements does not exist as a diatomic molecule?
a. Ne
c. H
b. F
d. I
2
Name: ________________________
ID: A
____ 24. 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.
____ 25. Which of the following diatomic molecules is joined by a double covalent bond?
c. N 2
a. O 2
d.
He 2
____ 26. A molecule with a single covalent bond is ____.
c.
a. CO 2
CO
b.
b.
Cl2
Cl 2
d.
N2
____ 27. According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as
possible?
a. pairs of valence electrons
c. mobile electrons
b. inner shell electrons
d. the electrons closest to the nuclei
____ 28. The shape of the methane (CH4) molecule is called ____.
a. tetrahedral
c. four-cornered
b. square
d. planar
____ 29. A bond formed between a silicon atom and an oxygen atom is likely to be ____.
a. ionic
c. polar covalent
b. coordinate covalent
d. nonpolar covalent
____ 30. Which of the following covalent bonds is the most polar?
a. H—F
c. H—H
b. H—C
d. H—N
Short Answer
31. Draw the Lewis Dot Diagram for H2O.
.
32. Draw the Lewis Dot Diagram for CF4.
.
33. Draw the Lewis Dot Diagram for N2O4.
.
3
Name: ________________________
ID: A
34. Draw two resonance structures for (CO3)-2.
.
4
ID: A
Chapter 8 and 9 Test
Answer Section
MULTIPLE CHOICE
1. ANS:
STO:
2. ANS:
STO:
3. ANS:
OBJ:
4. ANS:
STO:
5. ANS:
OBJ:
6. ANS:
STO:
7. ANS:
STO:
8. ANS:
OBJ:
9. ANS:
STO:
10. ANS:
OBJ:
11. ANS:
OBJ:
12. ANS:
STO:
13. ANS:
STO:
14. ANS:
STO:
15. ANS:
STO:
16. ANS:
STO:
17. ANS:
STO:
18. ANS:
STO:
19. ANS:
OBJ:
20. ANS:
OBJ:
B
C.1.33
C
C.1.7
C
9.1.1
B
C.1.33
C
9.2.1
A
C.1.6
B
C.1.6
A
9.2.1
D
C.1.6
D
9.2.1
A
9.2.1
C
C.1.36
B
C.1.36, C.1.6
C
C.1.36, C.1.6
A
C.1.8
C
C.1.8
B
C.1.8
C
C.1.8
D
9.3.2, 9.5.2
B
9.3.2, 9.5.3
DIF:
L1
REF: p. 254
OBJ: 9.1.1
DIF:
L1
REF: p. 254
OBJ: 9.1.1
DIF: L1
STO: C.1.6
DIF: L1
REF: p. 254, p. 255
DIF: L1
STO: C.1.7, C.1.6
DIF: L1
REF: p. 262, p. 263
REF: p. 261
OBJ: 9.2.1
DIF:
REF: p. 262
OBJ: 9.2.1
L2
REF: p. 253
OBJ: 9.1.1
DIF: L2
STO: C.1.36
DIF: L2
REF: p. 253, p. 254, p. 262
DIF:
STO:
DIF:
STO:
DIF:
L2
C.1.6
L2
C.1.6
L1
REF: p. 262, p. 263
REF: p. 268
OBJ: 9.3.1, 9.3.2
DIF:
L2
REF: p. 269
OBJ: 9.3.2
DIF:
L2
REF: p. 269
OBJ: 9.3.2
DIF:
L2
REF: p. 272
OBJ: 9.4.1
DIF:
L2
REF: p. 272
OBJ: 9.4.1
DIF:
L2
REF: p. 272
OBJ: 9.4.2
DIF:
L1
REF: p. 273
OBJ: 9.4.3
DIF:
STO:
DIF:
STO:
L2
C.1.8
L2
C.1.7
REF: p. 270, p. 278
REF: p. 262
OBJ: 9.2.1
REF: p. 262, p. 263
REF: p. 269, p. 277
1
ID: A
21. ANS:
OBJ:
22. ANS:
STO:
23. ANS:
STO:
24. ANS:
STO:
25. ANS:
STO:
26. ANS:
STO:
27. ANS:
STO:
28. ANS:
STO:
29. ANS:
OBJ:
30. ANS:
OBJ:
B
9.5.3
D
C.1.36
A
C.1.36
C
C.1.36
A
C.1.36
B
C.1.36
A
C.1.36
A
C.1.36
C
8.1.1, 8.4.1
A
8.4.1
DIF: L3
STO: C.1.7
DIF: L2
REF: p. 264, p. 277
REF: p. 244
OBJ: 8.1.1
DIF:
L1
REF: p. 217
OBJ: 8.2.1
DIF:
L2
REF: p. 217
OBJ: 8.2.1
DIF:
L2
REF: p. 221
OBJ: 8.2.3
DIF:
L2
REF: p. 222
OBJ: 8.2.1, 8.2.4
DIF:
L1
REF: p. 232
OBJ: 8.3.2
DIF:
L1
REF: p. 232
OBJ: 8.3.2
DIF:
STO:
DIF:
STO:
L2
C.1.36
L3
C.1.36
REF: p. 238, p. 239
REF: p. 238, p. 239
SHORT ANSWER
31. ANS:
See Drawing Key
32. ANS:
See drawing key
33. ANS:
See drawing key
34. ANS:
See drawing key
2