PERIODIC TABLE OF THE ELEMENTS
1A
1
H
8A
2
He
3
Li
2A
4
Be
3A
5
B
4A
6
C
5A
7
N
6A
8
O
7A
9
F
6.941
9.012
10.81
12.01
14.01
16.00
19.00
20.18
11
Na
12
Mg
13
Al
14
Si
15
P
16
S
17
Cl
18
Ar
1.008
22.99
24.31
3B
4B
5B
6B
7B
19
K
20
Ca
21
Sc
22
Ti
23
V
24
Cr
25
Mn
26
Fe
27
Co
39.10
40.08
44.96
47.88
50.94
52.00
54.94
55.85
37
Rb
38
Sr
39
Y
40
Zr
41
Nb
42
Mo
43
Tc
44
Ru
85.47
87.62
88.91
91.22
92.91
95.94
(98)
55
Cs
56
Ba
57
La
72
Hf
73
Ta
74
W
75
Re
2B
26.98
28.09
30.97
32.07
35.45
39.95
28
Ni
29
Cu
30
Zn
31
Ga
32
Ge
33
As
34
Se
35
Br
36
Kr
58.93
58.69
63.55
65.39
69.72
72.61
74.92
78.96
79.90
83.80
45
Rh
46
Pd
47
Ag
48
Cd
49
In
50
Sn
51
Sb
52
Te
53
I
54
Xe
101.1
102.9
106.4
107.9
112.4
114.8
118.7
121.8
127.6
126.9
131.3
76
Os
77
Ir
78
Pt
79
Au
80
Hg
81
Tl
82
Pb
83
Bi
84
Po
85
At
86
Rn
137.3
138.9
178.5
181.0
186.2
190.2
192.2
87
Fr
88
Ra
89
Ac
104
Unq
105 106 107
Unp Unh Uns
108
Uno
109
Une
(223)
226.0
227.0
(261)
(262)
(263)
(262)
(265)
(266)
58
Ce
59
Pr
60
Nd
61
Pm
62
Sm
63
Eu
140.1
140.9
144.2
(145)
150.4
90
Th
91
Pa
92
U
93
Np
94
Pu
231.0
amount in moles
ampere
atmosphere
atomic mass unit
Avogadro constant
Celsius temperature
coulomb
electromotive force
energy of activation
enthalpy
entropy
equilibrium constant
Faraday constant
238.0
237.0
(244)
10
Ne
1B
132.9
232.0
183.8
8B
4.003
195.1
197.0
200.6
204.4
207.2
209.0
(209)
64
Gd
65
Tb
66
Dy
67
Ho
68
Er
69
Tm
70
Yb
71
Lu
152.0
157.3
158.9
162.5
164.9
167.3
168.9
173.0
175.0
95
Am
96
Cm
97
Bk
98
Cf
99
Es
100
Fm
101 102
Md
No
103
Lr
(243)
(247)
(247)
(251)
ABBREVIATIONS AND SYMBOLS
n free energy
G molar mass
A frequency
ν mole
atm gas constant
R mole fraction
u gram
g Planck’s constant
NA hour
h pressure
J rate constant
°C joule
K reaction quotient
C kelvin
kPa second
E kilopascal
L speed of light
Ea liter
measure
of
pressure
mmHg
temperature, K
H
minute
min
time
S
molal
m
volt
K
molar
M
volume
F
(252)
(257)
(258)
(259)
(210)
(222)
(260)
CONSTANTS
M
mol
χ
h
P
k
Q
s
c
T
t
V
V
R = 8.314 J·mol–1·K–1
R = 0.0821 L·atm·mol–1·K–1
1 F = 96,500 C
1 F = 96,500 J·V–1
NA = 6.022 × 1023 mol–1
h = 6.626 × 10–34 J·s
c = 2.998 × 108 m·s–1
1 atm = 760 mmHg = 101.3 kPa
V (ideal gas) at STP = 22.4 L·mol–1
Part 1. Introductory Concepts
1. Which assumptions of Dalton’s atomic theory
had to be revised or discarded because of the
discovery of radioactivity?
5. What is the molar mass (in g mol–1) of
anhydrous iron(III) sulfate, to the nearest whole
number?
Atomic Molar Masses
Fe
55.8 g mol–1
O
16.0 g mol–1
S
32.1 g mol–1
Dalton’s Original Atomic Theory
1. The ultimate particles of matter are the
atoms of elements, which are indivisible
and indestructible.
2. All the atoms of a given element are alike
in all respects.
3. The atoms of different elements differ in
one or more properties.
4. Compounds are formed by combination of
different kinds of atoms.
(A)
(C)
l
3
(B)
(D)
2
4
2. The density of carbon tetrachloride is 1.60 g
mL–1. How many moles are there in a liter of the
pure CCl4?
Molar Mass
CCl4 154. g mol–1
(A)
(B)
10.4 mol
11.3 mol
(C)
(D)
23.7 mol
33.7 mol
3. If 1.0 g samples of each compound were
dehydrated, which sample would lose the greatest
mass of water?
LiCl.H2O
(A)
(B)
Molar Masses
60. g mol–1
MgSO4.H2O
138. g mol–1
FeSO4.H2O
170. g mol–1
SrC2O4.H2O
194. g mol–1
LiCl.H2O
MgSO4.H2O
(C)
(D)
FeSO4.H2O
(A)
(C)
(E)
NaCl
(B)
NH4NO3 (D)
NH4Cl
Na2SO4
(B)
(D)
152
336
6. Most nonmetals
(A) are relatively good reducing agents.
(B) form hydroxides that are basic or
amphoteric.
(C) form anions more readily than cations.
(D) are lustrous and highly conductive.
(E) have only 1, 2, or 3 electrons in the
outermost shell.
7. Which is most likely to be characteristic of an
atom showing metallic properties?
(A) a low atomic number
(B) a high ratio of protons to neutrons
(C) more than five valence electrons
(D) fewer than three valence electrons
8. The mass of a metal cylinder was determined on
an analytical balance and found to be 50.208 g.
The volume of the metal cylinder was measured
and determined to be 5.6 mL. The density of the
metal cylinder, expressed to the proper number of
significant digits, is
(A) 8.966 g mL–1
(B) 8.97 g mL–1
(C) 9 g mL–1
(D) 9.0 g mL–1
Part 2. Stoichiometry
9. When Pb(NO3)2 is heated in air, it decomposes to
a lead oxide. If 2.00 g Pb(NO3)2 produce 1.35 g of
the oxide, what is the formula of the oxide?
SrC2O4.H2O
Atomic Molar Masses
N
14. g mol–1
O
16. g mol–1
Pb
207. g mol–1
4. Which produces the greatest number of ions
when one mole dissolves in water?
(A)
C)
104
248
400
(A)
Pb2O3
(B)
PbO2
(C)
PbO
(D)
Pb3O4
10. What is the empirical formula for the
substance with this analysis:
Na
B
O
Molar Masses
10.8 g mol–1
23.0 g mol–1
16.0 g mol–1
(A) Na4BO4
(C) Na2B2O3
(B) Na3BO3
(D) NaB2O2
11. A hydrocarbon undergoes complete
combustion to give 0.44 g of CO2 and 0.27 g of
H2O. What is the simplest (empirical) formula of
the hydrocarbon?
Molar Masses
44.0 g mol–1
18.0 g mol–1
(A)
C44H27 (B)
CH4
(C)
C2H3
CH3
(D)
Atomic Molar Masses
Ag
108.! g mol–1
Cl
35.5 g mol–1
68.7%
91.3%
13. How many moles of Fe are needed to produce
10.0 mol of H2?
4H2O(g) + 3Fe(s) → Fe3O4(s) + 4H2(g)
7.50 mol
13.3 mol
(C)
(D)
1250 g
534 g
(B)
(D)
801 g
134 g
15. If 0.50 mol of Na3PO4 is mixed with 0.30 mol
of BaCl2, the maximum number of moles of barium
phosphate which can be formed is
(A)
(C)
0.10
0.30
(B)
(D)
0.15
0.50
Part 3. Atomic Structure
16. The number of neutrons in the nucleus of a
specific atom is equal to its
atomic mass.
mass number.
atomic number.
mass number minus the atomic number.
90
Calculate the percentage silver in the coin.
(A)
(B)
(A)
(C)
17. An atom of strontium–90 (38 Sr) contains
Ag+(aq) + Cl–(aq) → AgCl(s)
24.7% (B)
75.3% (D)
Atomic Molar Masses
Al
27.0 g mol–1
Cl
35.5 g mol–1
(A)
(B)
(C)
(D)
12. A 6.80 g coin was dissolved in nitric acid and
6.21 g of AgCl was precipitated by the addition of
excess sodium chloride,
(A)
(C)
Al2(SO4)3 + 3BaCl2 → 3BaSO4 + 2AlCl3
Elemental Analysis
54.0%
8.50%
37.5%
Atomic
B
Na
O
CO2
H2O
14. How many grams of aluminum chloride can one
obtain from 6.00 mol of barium chloride?
15.0 mol
30.0 mol
(A)
38 electrons, 38 protons, 52 neutrons.
(B)
38 electrons, 38 protons, 90 neutrons.
(C)
52 electrons, 52 protons, 38 neutrons.
(D)
52 electrons, 38 protons, 38 neutrons.
18. Which of these atoms has the greatest number
of neutrons in its nucleus?
(A)
56
25
Mn
(D)
57
27
Co
(B)
(E)
52
26
Fe
56
28 Ni
(C)
55
26
Fe
19. An atom has a valence shell electron
configuration of ns1. To which group of elements
in the periodic table does it belong?
(A) transition metals
(B) alkali metals
(C) alkaline earth metals
(D) rare earth metals
20. Which electron configuration is impossible?
(A) 1s22s22p63s2
(B)
(C)
1s22s22p62d2 (D)
1s22s22p63s23p6
1s22s22p53s1
21. The number of unpaired electrons in the
ground state of Mn0 is
(A)
(C)
one
five
(B)
(D)
three
seven
22. The maximum number of electrons that can
occupy an orbital labeled dxy is
(A)
(C)
l
3
(B)
(D)
2
4
23. The element X occurs naturally to the extent of
20.0% 12X and 80.0% 13X. The atomic mass of X is
nearest
(A) 12.2
(C) 12.8
(B) 12.5
(D) 13.0
24. Which electron transition is associated with the
largest emission of energy?
(A) n = 2 to n = 1
(B) n = 2 to n = 3
(C) n = 2 to n = 4
(D) n = 3 to n = 2
25. Which is an acceptable set of quantum
numbers for a 3d electron?
(A)
(B)
(C)
(D)
n
l
ml
ms
3
3
2
2
3
2
2
3
1
1
-1
2
+1/2
+1/2
-1/2
-1/2
Answers
1.
2.
3.
4.
5.
A
A
A
D
E
6. C
7. D
8. D
9. C
10. B
11.
12.
13.
14.
15.
D
B
A
C
A
16.
17.
18.
19.
20.
D
A
A
B
B
21.
22.
23.
24.
25.
C
B
C
A
B