ExamView - naming review june 2.tst

Name: ________________________ Class: ___________________ Date: __________
ID: A
Naming
Matching
Match each item with the correct statement below.
a. monatomic ion
f.
b. acid
g.
c. base
h.
d. law of definite proportions
i.
e. law of multiple proportions
cation
binary compound
anion
polyatomic ion
____
1. consists of a single atom with a positive or negative charge
____
2. atom or group of atoms having a negative charge
____
3. atom or group of atoms having a positive charge
____
4. tightly-bound group of atoms that behaves as a unit and carries a net charge
____
5. compound composed of two different elements
____
6. produces a hydrogen ion when dissolved in water
____
7. produces a hydroxide ion when dissolved in water
____
8. In any chemical compound, the masses of elements are always in the same proportion by mass.
____
9. when two elements form more than one compound, the masses of one element that combine with the same
mass of the other element are in the ratio of small, whole numbers
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 10. What type of ions have names ending in -ide?
a. only cations
c.
b. only anions
d.
only metal ions
only gaseous ions
____ 11. When Group 2A elements form ions, they ____.
a. lose two protons
c.
b. gain two protons
d.
lose two electrons
gain two electrons
____ 12. What is the correct name for the N 3 − ion?
a. nitrate ion
b. nitrogen ion
nitride ion
nitrite ion
c.
d.
____ 13. 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
1
Name: ________________________
ID: A
____ 14. Aluminum is a group 3A metal. Which ion does A1 typically form?
c. Al 5 −
a. Al 3 −
b. Al 3 +
d. Al 5 +
____ 15. Which of the following correctly provides the name of the element, the symbol for the ion, and the name of
the ion?
a.
fluorine, F + , fluoride ion
c.
copper, Cu + , cuprous ion
b.
zinc, Zn 2 + , zincate ion
d.
sulfur, S 2 − , sulfurous ion
____ 16. The nonmetals in Groups 6A and 7A ____.
a. lose electrons when they form ions
b. have a numerical charge that is found by subtracting 8 from the group number
c. all have ions with a –1 charge
d. end in -ate
____ 17. What is the Stock name for chromic ion?
a. chromium(I) ion
b. chromium(II) ion
c.
d.
chromium(III) ion
chromium(IV) ion
c.
d.
Ca 2 +
mercurous ion
____ 18. Which of the following is NOT a cation?
a.
b.
iron(III) ion
sulfate
____ 19. In which of the following are the symbol and name for the ion given correctly?
a.
NH 4 + : ammonia; H + : hydride
c.
OH − : hydroxide; O 2 − : oxide
b.
C 2 H 3 O 2 − : acetate; C 2 O 4 − : oxalite
d.
PO 3 3 − : phosphate; PO 4 3 − : phosphite
____ 20. An -ate or -ite at the end of a compound name usually indicates that the compound contains ____.
a. fewer electrons than protons
c. only two elements
b. neutral molecules
d. a polyatomic anion
____ 21. Why are systematic names preferred over common names?
a. Common names do not provide information about the chemical composition of the
compound.
b. Common names are derived from the method used to obtain the compound.
c. Common names were assigned by the scientist who discovered the compound.
d. Common names are not very descriptive.
____ 22. Which of the following compounds contains the Mn 3 + ion?
a. MnS
c. Mn 2 O 3
b.
MnBr 2
d.
MnO
____ 23. 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
2
Name: ________________________
ID: A
____ 24. In which of the following are the formula of the ionic compound and the charge on the metal ion shown
correctly?
a.
UCl 5 , U +
c.
IrS 2 , Ir 2 +
b.
ThO 2 , Th 4 +
d.
NiO, Ni +
____ 25. Which of the following correctly represents an ion pair and the ionic compound the ions form?
a.
Ca 2 − , F − ; CaF 2
c.
Ba 2 + , O 2 − ; Ba 2 O 2
b.
Na + , Cl − ; NaCl 2
d.
Pb 4 + , O 2 − ; Pb 2 O 4
c.
d.
binary compound
polyatomic compound
____ 26. Sulfur hexafluoride is an example of a ____.
a. monatomic ion
b. polyatomic ion
____ 27. 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
____ 28. Binary molecular compounds are made of two ____.
a. metallic elements
c. polyatomic ions
b. nonmetallic elements
d. cations
____ 29. In naming a binary molecular compound, the number of atoms of each element present in the molecule is
indicated by ____.
a. Roman numerals
c. prefixes
b. superscripts
d. suffixes
____ 30. When dissolved in water, acids produce ____.
a. negative ions
c.
b. polyatomic ions
d.
hydrogen ions
oxide ions
____ 31. 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
____ 32. 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
d.
HI, iodic acid
c.
d.
sulfuric acid
sulfurous acid
____ 33. What is the name of H 2 SO 3 ?
a.
b.
hyposulfuric acid
hydrosulfuric acid
____ 34. When the name of an anion that is part of an acid ends in -ite, the acid name includes the suffix ____.
a. -ous
c. -ate
b. -ic
d. -ite
3
Name: ________________________
____ 35. What is the formula for sulfurous acid?
a. H 2 SO 4
ID: A
c.
H 2 SO 2
d.
H2 S
c.
HPO 2
d.
HPO 4
c.
HSO 2
H 2 SO 2
d.
H2 S
____ 38. How are bases named?
a. like monatomic elements
b. like polyatomic ions
c.
d.
like ionic compounds
like molecular compounds
b.
H 2 SO 3
____ 36. What is the formula for phosphoric acid?
a. H 2 PO 3
b.
H 3 PO 4
____ 37. What is the formula for hydrosulfuric acid?
a. H 2 S 2
b.
____ 39. In any chemical compound, the elements are always combined in the same proportion by ____.
a. charge
c. volume
b. mass
d. density
____ 40. What is the correct formula for barium chlorate?
a. Ba(ClO) 2
c.
b.
Ba(ClO 2 ) 2
d.
Ba(ClO 3 ) 2
BaCl 2
____ 41. What is the correct formula for calcium dihydrogen phosphate?
a. CaH 2 PO 4
c. Ca(H 2 PO 4 ) 2
b.
Ca 2 H 2 PO 4
d.
Ca(H 2 HPO 4 ) 2
____ 42. What does an -ite or -ate ending in a polyatomic ion mean?
a. Oxygen is in the formula.
c. Nitrogen is in the formula.
b. Sulfur is in the formula.
d. Bromine is in the formula.
____ 43. Which of the following is the correct name for N 2 O 5 ?
a.
b.
nitrous oxide
dinitrogen pentoxide
c.
d.
4
nitrogen dioxide
nitrate oxide
ID: A
Naming
Answer Section
MATCHING
1. ANS:
OBJ:
2. ANS:
OBJ:
3. ANS:
OBJ:
4. ANS:
OBJ:
5. ANS:
OBJ:
6. ANS:
OBJ:
7. ANS:
OBJ:
8. ANS:
OBJ:
9. ANS:
OBJ:
A
9.1.1
H
9.1.1
F
9.1.1
I
9.1.2
G
9.2.1
B
9.4.1
C
9.4.3
D
9.5.1
E
9.5.1
PTS: 1
DIF:
L1
REF: p. 253
PTS: 1
DIF:
L1
REF: p. 254
PTS: 1
DIF:
L1
REF: p. 253
PTS: 1
DIF:
L1
REF: p. 257
PTS: 1
DIF:
L1
REF: p. 261
PTS: 1
DIF:
L1
REF: p. 271
PTS: 1
DIF:
L1
REF: p. 273
PTS: 1
DIF:
L1
REF: p. 274
PTS: 1
DIF:
L1
REF: p. 274
PTS: 1
DIF:
L1
REF: p. 254
PTS: 1
DIF:
L1
REF: p. 254
PTS: 1
DIF:
L1
REF: p. 254
PTS: 1
DIF:
L1
REF: p. 254 | p. 255
PTS: 1
DIF:
L1
REF: p. 253
PTS: 1
DIF:
L2
REF: p. 254 | p. 255
PTS: 1
DIF:
L2
REF: p. 254
PTS: 1
DIF:
L2
REF: p. 255
PTS: 1
DIF:
L1
REF: p. 254 | p. 255 | p. 257
PTS: 1
DIF:
L2
REF: p. 254 | p. 257
MULTIPLE CHOICE
10. ANS:
OBJ:
11. ANS:
OBJ:
12. ANS:
OBJ:
13. ANS:
OBJ:
14. ANS:
OBJ:
15. ANS:
OBJ:
16. ANS:
OBJ:
17. ANS:
OBJ:
18. ANS:
OBJ:
19. ANS:
OBJ:
B
9.1.1
C
9.1.1
C
9.1.1
C
9.1.1
B
9.1.1
C
9.1.1
B
9.1.1
C
9.1.1
B
9.1.1 | 9.1.2
C
9.1.1 | 9.1.2
1
ID: A
20. ANS:
OBJ:
21. ANS:
OBJ:
22. ANS:
OBJ:
23. ANS:
OBJ:
24. ANS:
OBJ:
25. ANS:
OBJ:
26. ANS:
OBJ:
27. ANS:
OBJ:
28. ANS:
OBJ:
29. ANS:
OBJ:
30. ANS:
OBJ:
31. ANS:
OBJ:
32. ANS:
OBJ:
33. ANS:
OBJ:
34. ANS:
OBJ:
35. ANS:
OBJ:
36. ANS:
OBJ:
37. ANS:
OBJ:
38. ANS:
OBJ:
39. ANS:
OBJ:
40. ANS:
OBJ:
41. ANS:
OBJ:
42. ANS:
OBJ:
D
PTS:
9.1.2
A
PTS:
9.2.1
C
PTS:
9.2.1
D
PTS:
9.2.1
B
PTS:
9.2.1
A
PTS:
9.2.1
C
PTS:
9.3.1
C
PTS:
9.3.1 | 9.3.2
B
PTS:
9.3.2
C
PTS:
9.3.2
C
PTS:
9.4.1
A
PTS:
9.4.1
C
PTS:
9.4.1
D
PTS:
9.4.1
A
PTS:
9.4.1
B
PTS:
9.4.2
B
PTS:
9.4.2
D
PTS:
9.4.2
C
PTS:
9.4.3
B
PTS:
9.5.1
C
PTS:
9.2.2 | 9.2.3 | 9.5.2
C
PTS:
9.2.2 | 9.2.3 | 9.5.2
A
PTS:
9.1.3 | 9.5.3
1
DIF:
L2
REF: p. 257
1
DIF:
L1
REF: p. 260
1
DIF:
L1
REF: p. 262 | p. 263
1
DIF:
L2
REF: p. 262
1
DIF:
L2
REF: p. 262
1
DIF:
L2
REF: p. 262
1
DIF:
L2
REF: p. 268
1
DIF:
L1
REF: p. 268
1
DIF:
L1
REF: p. 268
1
DIF:
L1
REF: p. 269
1
DIF:
L1
REF: p. 271
1
DIF:
L2
REF: p. 272
1
DIF:
L2
REF: p. 272
1
DIF:
L2
REF: p. 272
1
DIF:
L2
REF: p. 272
1
DIF:
L2
REF: p. 272
1
DIF:
L2
REF: p. 272
1
DIF:
L3
REF: p. 272
1
DIF:
L1
REF: p. 273
1
DIF:
L1
REF: p. 274
1
DIF:
L3
REF: p. 257 | p. 264
1
DIF:
L3
REF: p. 257 | p. 264
1
DIF:
L1
REF: p. 257 | p. 278
2
ID: A
43. ANS: B
OBJ: 9.3.2 | 9.5.3
PTS: 1
DIF:
3
L2
REF: p. 269 | p. 277