C101 FINAL EXAM REVIEW QUESTIONS
revised 12/2011
Questions 1 – 71 are more or less in the order the material was covered in the course. These questions
come from Chapters 1 – 7 of your textbook. At the end of this document you will find a group of 29
questions that are over the “new material” from Chapters 8 and 9. Don’t “study” the review questions,
but rather use the review questions to gauge how prepared you are for the final exam and to get a feel for
the kinds of questions you will be asked on the final exam. The answer key and a sample cover sheet are
the last two pages of this document.
1.
Which of the following are halogens?
a.
b.
c.
2.
have identical electron configurations.
have the same charge.
have identical mass numbers, A.
have the same number of protons, but different numbers of neutrons.
reside in the same period in the periodic table.
1 electron.
2 electrons.
6 electrons.
d.
e.
10 electrons.
18 electrons.
calcium.
zirconium.
silicon.
d.
e.
magnesium.
carbon.
arsenic
germanium
boron
d.
e.
technetium
antimony
The atomic weight listed for an element on the periodic table is
a.
b.
c.
d.
e.
8.
thalium
nickel
Which of the following is not a metalloid?
a.
b.
c.
7.
d.
e.
The element from group 2 and period 4 is
a.
b.
c.
6.
vanadium
fluorine
rhodium
A single orbital may, at most, contain
a.
b.
c.
5.
Na, Li, K, Cs
Co, Mn, Fe, Pd
Isoelectronic refers to species that
a.
b.
c.
d.
e.
4.
d.
e.
Which of the following elements is misspelled?
a.
b.
c.
3.
O, S, P
He, Ar, Ne, Rn
Cl, Br, I, F
the same as its mass number
the sum of the protons and neutrons
the mass in amu of the most stable isotope
the mass in grams of the most abundant isotope
an average of the weights of naturally-occurring isotopes.
If a 250. g gold bar (specific heat: 0.031 cal/g·°C) absorbs 300. cal, how much will its temperature increase?
a.
b.
c.
110°C
1.0°C
270°C
d.
e.
39°C
27°C
9.
Suppose 500. cal is absorbed by each of the following metals. Which has the greatest temperature increase?
gold:
brass:
copper:
stainless steel:
a.
b.
c.
10.
131
b.
122
d.
e.
20 g/cm3
24 g/cm3
131
I
Sn
d.
179
Hf
e.
177
Hf
Xe
an odd number of electrons.
an even number of electrons.
the largest possible charge on an ion.
d.
e.
equal numbers of electrons and protons.
noble gas configurations.
d.
e.
Al2+
Al3+
The most stable aluminum ion is
Al2–
Al1–
Al1+
Which of the following denotes an excited state of an uncharged carbon atom?
a.
b.
c.
15.
stainless steel
all have the same temperature change
The electron configurations that permit maximum stability are those with
a.
b.
c.
14.
8 g/cm3
12 g/cm3
16 g/cm3
a.
a.
b.
c.
13.
d.
e.
Which of the following contains 78 neutrons?
c.
12.
gold
brass
copper
A student measured the mass of 5 mL of a liquid to be 120.0 g. What is the density of the liquid (with
proper attention to the number of significant figures)?
a.
b.
c.
11.
100 g, with specific heat = 0.031 cal/g·°C
100 g, with specific heat = 0.089 cal/g·°C
200 g, with specific heat = 0.091 cal/g·°C
300 g, with specific heat = 0.122 cal/g·°C
1s22s22p4
1s22s22p6
1s22s22p23s2
d.
e.
1s22s22p63s1
1s22s23s2
Which neutral element has the following electron configuration:
[Ne]3s23p4
a.
b.
c.
16.
d.
e.
O
P
Arrange the following electromagnetic radiation in order of increasing energy.
a.
b.
c.
17.
S
Al
B
blue light
microwaves
infrared
yellow light
I
II
III
IV
I < II < III < IV
III < IV < I < II
II < III < IV < I
d.
e.
III < I < IV < II
IV < I < III < II
d.
e.
krypton
radon
Ba2+ is isoelectronic with:
a.
b.
c.
radium
argon
xenon
18.
Phosphorus forms the stable monatomic ion:
a.
b.
c.
19.
MgCN
Mg2CN
Mg(CN)2
d.
e.
Mg(CN)3
Mg3(CN)2
Cr2NO3
Cr2(NO3)2
Cr(NO3)2
d.
e.
CrNO3
Cr3(NO3)2
CaPO4
Ca(PO4)2
Ca2(PO4)2
d.
e.
Ca2(PO4)3
Ca3(PO4)2
AlNO2
Al3(NO2)2
Al2(NO2)2
d.
e.
€
Al2(NO2)3
Al(NO2)3
€
3
5
6
d.
e.
7
8
3
5
10
d.
e.
18
24
Carbon dioxide contains two double bonds, each from carbon to an oxygen atom. The shape of carbon
dioxide is best described by the term
a.
b.
c.
28.
Cs
O
The total number of valence electrons involved in the bonding and structure of BCl3 is
a.
b.
c.
27.
d.
e.
The total number of valence electrons involved in the bonding and structure of NH3 is
a.
b.
c.
26.
S
C
F
The ionic compound formed from Al 3+ and NO1–
2 has the formula:
a.
b.
c.
25.
Sr2–
Sr1+
The ionic compound formed from calcium ion and the phosphate ion has the formula:
a.
b.
c.
24.
d.
e.
Chromium (II) nitrate has the formula:
a.
b.
c.
23.
Sr3+
Sr3–
Sr2+
Magnesium cyanide has the formula:
a.
b.
c.
22.
P2–
P1+
Which of the following is the most electronegative element?
a.
b.
c.
21.
d.
e.
Strontium forms the stable monatomic ion:
a.
b.
c.
20.
P3+
P3–
P2+
bent.
linear.
T-shaped.
d.
e.
tetrahedral.
trigonal planar.
d.
e.
Br2
none of the above
Which of the following contains a single bond?
a.
b.
c.
P2
N2
CO
29.
Which of the following molecules has exactly one lone pair of electrons?
a.
b.
c.
30.
F–F
N–O
NO4
NO3
NO5
d.
e.
N 2O 3
N 2O 4
tetrahedral
trigonal planar
trigonal bipyramidal
d.
e.
triangular pyramidal
square planar
NH5 exists and uses nitrogen 2s and 2p orbitals for bonding.
NH5 exists and uses nitrogen 2s, 2p, and 3s orbitals for bonding.
NH5 exists and uses nitrogen 2s, 2p, and 3d orbitals for bonding.
NH5 does not exist since there are no 2d orbitals.
NH5 does not exist since there are no 3d orbitals.
90°
105°
109°
d.
e.
120°
180°
Al2SO4
Al2(SO4)3
Al(SO3)3
d.
e.
Al3(SO4)2
AlSO3
What is the oxidation number of bromine in the perbromate ion, BrO1–
4 ?
a.
b.
c.
38.
d.
e.
What is the formula of the salt formed when aluminum hydroxide is neutralized with sulfuric acid?
a.
b.
c.
37.
C–O
N≡N
O–Cl
What is the H-C-H angle in methane, CH4?
a.
b.
c.
36.
Cs2O
CS2
Comment on the existence and structure of NH5.
a.
b.
c.
d.
e.
35.
d.
e.
What term best describes the shape of CH2O (formaldehyde)? Hint: Carbon is the central atom.
a.
b.
c.
34.
CaCl2
NaCl
NaF
What is the formula of dinitrogen tetraoxide?
a.
b.
c.
33.
BF3
PH3
Which of the following bonds is most polar?
a.
b.
c.
32.
d.
e.
Which of the following is best described as a covalently bonded molecule?
a.
b.
c.
31.
CS2
Cl2
CO2
+1
+3
+4
d.
e.
+5
+7
€
What is the oxidation number of carbon in sodium carbonate?
a.
b.
c.
+1
+3
+4
d.
e.
+5
+8
39.
Which of the following describes an endothermic reaction?
a.
b.
c.
40.
d.
e.
ΔH = +200 kcal and ΔS = 0
both b and d above
ΔS > 0
ΔS < 0
ΔH > 0
d.
e.
ΔH < 0
ΔG < 0
alters the heat of a chemical reaction.
increases the free energy of a reaction.
increases the entropy change in a chemical reaction.
reduces the activation energy of a chemical reaction.
does all of the above.
Le Châtelier’s Principle states
a.
b.
c.
d.
e.
44.
ΔH = –100 kcal
ΔH = +100 kcal
ΔH = 0
A catalyst
a.
b.
c.
d.
e.
43.
ΔH < 0 and heat is absorbed
ΔH = 0 and heat is released
The “spontaneity criterion” for chemical reactions is given by:
a.
b.
c.
42.
d.
e.
Which of the following is an example of an exothermic reaction?
a.
b.
c.
41.
ΔH > 0 and heat is released
ΔH < 0 and heat is released
ΔH > 0 and heat is absorbed
when stress is applied to a system in equilibrium, the equilibrium shifts to relieve the stress.
that the forward reaction is the same as the reverse reaction in a chemical equilibrium.
that the entropy of the universe is increasing.
that the entropy of the universe is decreasing.
that, when an exothermic reaction is heated, the forward reaction rate will increase.
In the compound magnesium permanganate, Mg(MnO4)2, what is the oxidation number of manganese?
a.
b.
c.
+8
+7
+5
d.
e.
+3
+1
Use the balanced reaction below for the next two problems.
2AuCl 3 + 3Sn → 3SnCl 2 + 2Au
45.
If 10 mol of gold (III) chloride are used with excess tin, how many mol of tin (II) chloride are produced?
a.
b.
c.
46.
d.
e.
15
30
If 30 mol of tin metal are used, how many moles of gold are produced?
a.
b.
c.
47.
3
6
12
2
15
20
d.
e.
25
60
In the reaction,
2 N2(g) + 5 O2(g) → 2 N2O5(g)
if 3.0 moles of nitrogen gas are reacted with excess oxygen, what mass of dinitrogen pentoxide is produced?
a.
b.
c.
108 g
216 g
320 g
d.
e.
810 g
1.3 kg
48.
How many molecules are there in 3.00 moles of C6H6?
a.
b.
c.
49.
1.0
3.0
1.20 × 1024
d.
e.
1.81 × 1024
6.02 × 1023
What is the equilibrium expression for the following reaction?
2 NO (g) + 2 CO (g)  N2 (g) + 2 CO2 (g) + heat
a.
K=
[NO]2 [CO]2
[N2 ]2 [CO2 ]2
d.
K=
[ N2 ][CO2 ]2
[NO]2 [CO]2
b.
K=
[2N2 ][2CO2 ]2
[2NO]2 [CO]2
e.
K=
2[NO]2[CO]2
[N2 ] + [CO2 ]2
€
c.
K=
€
€
Find the activation energy for reactants forming products.
∆G, kcal
50.
[N2 ]2 [CO2 ]2
[NO]2 [CO]2
€
16
€
15
14
13
12
11
10
9
8
7
6
5
4
3
2
1
reaction progress →
a.
b.
c.
51.
54.
5.5 kcal
16 kcal
4 kcal
–6.5 kcal
+6.5 kcal
d.
e.
10.5 kcal
12 kcal
d.
e.
4 moles
5 moles
How many moles are 72 g of water?
a.
b.
c.
53.
d.
e.
Use the diagram in the previous question to determine ΔG for the backward reaction.
a.
b.
c.
52.
10.5 kcal
4.0 kcal
12. kcal
1 mole
2 moles
3 moles
Iron corrodes to iron (III) oxide in the presence of excess oxygen gas. Which of the following is the correct
balanced equation for this oxidation?
a.
Fe + O 2 → Fe2 O 3
d.
4Fe + 2O 2 → 2Fe 2 O 3
b.
2Fe + 3O 2 → Fe2 O 3
e.
4Fe + 3O 2 → 2Fe 2 O 3
c.
2Fe + O 2 → Fe2 O 3
If all the gases below are in a flask together, which gas has the highest average speed?
a.
b.
c.
Xe
C 2H 2
CCl4
d.
e.
NH3
H 2S
55.
A balloon occupying 12 L at 1 atm occupies what volume in the upper atmosphere at a pressure of 0.50
atm? Assume the temperature remains constant.
a.
b.
c.
56.
its surprisingly high boiling point.
all of the above
water
CH3CH2CH2CH2CH2OH
CH3CH2CH2CH2CH2CH2CH2CH2Br
d.
e.
both a and b
both b and c
methane
carbon dioxide
hydrogen chloride
d.
e.
carbon disulfide
propane, C3H8
100 torr
200 torr
273 torr
d.
e.
760 torr
1000 torr
boiling point will be lowered
freezing point will be lowered
freezing point will be elevated
d.
e.
both a and b
both a and c
H2··· HCl
H2··· CS2
HCl··· CS2
d.
e.
CS2··· CS2
HCl··· HCl
If you wanted to form 10 L of the product, N2O4(g), exactly how many liters of nitrogen and oxygen would
be required in the following reaction?
N2(g) + 2O2(g) → N2O4(g)
a.
b.
c.
d.
e.
64.
d.
e.
A flask contains the gases H2, HCl, and CS2. Between which molecules is the dipole-dipole force greatest?
a.
b.
c.
63.
temperature independence of vapor pressure.
its surprisingly low specific heat.
its low heat of vaporization.
Adding a non-volatile solute to a solvent will likely result in which of the following?
a.
b.
c.
62.
2L
1L
How many torr are equivalent to 1 atm of pressure?
a.
b.
c.
61.
d.
e.
Which of the following gases likely has significant dipole-dipole intermolecular forces?
a.
b.
c.
60.
12 L
6L
3L
Which of the following would be a good solvent for CCl4?
a.
b.
c.
59.
12 L
24 L
The existence of hydrogen bonding between water molecules is responsible for
a.
b.
c.
58.
d.
e.
A balloon occupies 3 L at 1 atm at 300 K. What is its volume at 2 atm and 600 K?
a.
b.
c.
57.
0.75 L
1.5 L
6.0 L
2.5 L nitrogen and 5 L oxygen
5 L nitrogen and 5 L oxygen
5 L nitrogen and 10 L oxygen
3.3 L nitrogen and 6.7 L oxygen
10 L nitrogen and 20 L oxygen
If 1.0 L of 0.33 M NaF solution were evaporated to dryness, how many g of NaF salt would we have?
a.
b.
c.
3g
14 g
51 g
d.
e.
39 g
42 g
65.
If a 2 L flask contains a gas at a pressure of 4 atm at 100 K, about how much gas must be in the flask?
a.
b.
c.
66.
d.
e.
4 moles
5 moles
A flask contains 0.75 L of helium and 0.25 L of neon at 2.0 atm. What is the partial pressure of helium?
a.
b.
c.
67.
1 mole
2 moles
3 moles
0.5 atm
0.75 atm
1.0 atm
d.
e.
The enthalpy change is 43.2 kcal for the reaction:
1.5 atm
2.0 atm
N2 + O2 → 2 NO
Formation of 90.0 g of NO gas will result in ______ being ______ .
68.
69.
a.
21.6 kcal; released
b.
64.8 kcal; released
c.
43.2 kcal; absorbed
d.
64.8 kcal; absorbed
e.
130. kcal; absorbed
What is the concentration if a 50.0 L sample of river water contains 250 microliters of dioxin?
a.
5.0 %
b.
0.05 %
c.
0.50 ppm
d.
5.0 ppm
e.
500 ppm
Suppose 200 mL of a solution contains 50. g of sucrose. What is its w/v %?
a.
b.
c.
70.
d.
e.
50% (w/v)
75% (w/v)
The addition of a soluble, non-volatile solute, such as KI, to water
a.
b.
c.
71.
10% (w/v)
20% (w/v)
25% (w/v)
lowers its boiling point.
raises its freezing point.
decreases its conductivity.
d.
e.
increases its vapor pressure.
decreases its vapor pressure.
The melting point of acetone is –95°C. How much heat is needed to melt 12.2 g of acetone at –95°C?
Heat of fusion is 23.4 cal/g
Heat of vaporization is 124.7 cal/g
q = mCΔT
a.
285 cal
d.
0.888 kcal
b.
603 cal
e.
27.1 kcal
c.
1520 cal
Cacetone = 0.52 cal/g°C
The following problems cover concepts from Chapter 8 (N1 - N15) and Chapter 9 (N16 – N29).
N1.
Which of the following are strong acids?
a.
b.
c.
N2.
d.
e.
NH3
CH3COOH
a buffer
strong acid
strong base
d.
e.
water
all of the above
water
CH3COO–the hydronium ion
d.
e.
OH–
H+
d.
e.
10
none of the above
d.
e.
> 14
10–10
Which of the following corresponds to the pH of an acid?
a.
b.
c.
N6.
HCl
NH4+
H2SO4
What is the conjugate base of CH3COOH?
a.
b.
c.
N5.
nitric acid
all of the above
Which of the following is always a consequence of a neutralization reaction?
a.
b.
c.
N4.
d.
e.
Which is an example of a Brønsted-Lowry base?
a.
b.
c.
N3.
sulfuric acid
hydrochloric acid
hydrobromic acid
12
7
2
If [H+] = 10–2 M, what is the pH?
a.
b.
c.
<1
2
4
N7.
If [H+] = 2.5 × 10–5 M, what is its pH? You will need a calculator.
________________
N8.
The sum of the pH and the pOH is:
a.
b.
c.
N9.
0
14
10–7
d.
e.
10–14
7
The following weak acids are in order of decreasing strength:
HNO2 > CH3COOH > HCN
weak
weakest
Arrange their conjugate bases in order of increasing basicity.
a.
b.
c.
N10.
NO2– < CN– < CH3COO–
NO2– < CH3COO– < CN–
CN– < NO2– < CH3COO–
d.
e.
CN– < CH3COO– < NO2–
CH3COO– < CN– < NO2–
Buffers have which of the following properties?
a.
b.
c.
d.
e.
Combinations of a weak acid and its conjugate base that resists changes in pH
Show, with color changes, the relative pH of two solutions
Solutions formed from combination of a strong acid and a strong base
Solutions with such high pH that they are unaffected by addition of acids
Solutions where the Ka is very sensitive to small changes in H+ or OH– concentrations
N11.
What is [H+] in a 0.5 M H2SO4 solution?
a.
b.
c.
N12.
ozone emission
both a and b
d.
e.
100 mL
125 mL
salt formed from mixing a strong acid and a weak base
salt formed from mixing a weak acid and a strong base
salt formed from mixing a strong acid and a strong base
both a and b
both b and c
HCl
HCN
NaOH
7
9
10
19
d.
e.
H2PO4–
NH3
d.
e.
19
none of the above
d.
e.
24
none of the above
d.
e.
78
8
F?
€
2+
How many protons are in 42
?
20 Ca
a.
b.
c.
N18.
25 mL
50 mL
75 mL
How many neutrons are in
a.
b.
c.
N17.
d.
e.
Which can behave both as a Brønsted-Lowry acid and as a Brønsted-Lowry base?
a.
b.
c.
N16.
sulfur dioxide emission
NOx emission
CO emission
Which of the following salts yields a basic solution when added to water?
a.
b.
c.
d.
e.
N15.
1M
2M
About how many mL of 0.30 M NaOH are required to completely neutralize 50 mL of 0.75 M HCl?
a.
b.
c.
N14.
d.
e.
Acid rain is formed from
a.
b.
c.
N13.
0.1 M
0.2 M
0.5 M
18
20
22
How many neutrons are in
a.
b.
c.
133
54
79
133
Xe ?
€
What is the product of each of the following decay paths?
Nuclide
Nuclear emission
N19.
131
53
I
β–
N20.
18
F
β+
N21.
222
Rn
α
N22.
131I
a.
b.
c.
Product
has a half-life of 8 days. If you start with a 120 g sample of 131I, how much remains after 32 days?
240 g
60 g
30 g
d.
e.
15 g
7.5 g
N23.
What is X in this reaction?
2
1
N24.
a.
4
2
b.
0
+1
β
c.
0
–1
β
b.
c.
b.
c.
b.
c.
2 neutrons
e.
2 protons
d.
e.
214
85 At
218
85 As
214
81 Tl
214
82 Pb
218
84 Po
d.
e.
214
81 Rn
214
82 Tl
microwaves < red light < yellow light < gamma rays
microwaves < gamma rays < red light < yellow light
microwaves < yellow light < red light < gamma rays
yellow light < red light < microwaves < gamma rays
gamma rays < microwaves < red light < yellow light
235
92 U
?
238
90 U
238
92 U
235
94 U
d.
both a and b
e.
both b and c
d.
e.
anti-proton
anti-neutron
A proton is converted into a neutron. What is emitted?
a.
b.
c.
N29.
214
81 Tl
210
81 Tl
214
81 Bi
Which of the following is an isotope of
a.
N28.
d.
Arrange the following in order of increasing energy: gamma rays, microwaves, red light, yellow light
a.
b.
c.
d.
e.
N27.
α
Rn (222) decays with the following emissions: α, α, and then β+. What nuclide do you now have?
a.
N26.
3
If 214Bi decays with emission of an alpha particle, what results?
a.
N25.
3
H+ 1H→ 2 He + X
electron
positron
α particle
Transmutation refers to the
a.
b.
c.
d.
e.
conversion of one element to another.
effect of ionizing radiation on body tissues.
fragmentation of heavy nuclei.
separation of different isotopes of the same element.
conversion of matter into energy.
C101 Final Exam Review Answers
1c
31a
61b
New Material
2d
32e
62e
N1e
3a
33b
63e
N2d
4b
34d
64b
N3d
5a
35c
65a
N4b
6d
36b
66d
N5c
7e
37e
67d
N6b
8d
38c
68d
N7
9a
39c
69c
N8b
10d
40a
70e
N9b
11a
41e
71a
N10a
12e
42d
N11d
13e
43a
N12e
14e
44b
N13e
15a
45d
N14b
16c
46c
N15d
17c
47c
N16c
18b
48d
N17b
19c
49d
N18c
20c
50d
N19
131
54
21c
51c
N20
18
8
22c
52d
N21
218
84
23e
53e
N22e
24e
54d
N23d
25e
55e
N24b
26e
56c
N25a
27b
57d
N26a
28d
58e
N27b
29e
59c
N28b
30e
60d
N29a
pH = 4.6
Xe
O
Po
Typical Cover Sheet
Name ____________________
C101 FINAL EXAM
1. Print and code your name (last name, space, first name) on your answer sheet in the “last name” block. Print and code the
form of your exam in the first box under “course.” Print and code the last 5 digits of your ID number in the first 5 spots in
the “ID number” block. Please code carefully and check your coding.
2. Print your name in the space provided on the exam booklet.
3. Choose the best answer for each question. Using a #2 pencil, fill in the corresponding balloon on the scoring sheet.
4. Return the answer sheet AND Final Examination Booklet to your instructor when finished.
ΔG = ΔH – TΔS
PV = nRT
P1V1/T1 = P2V2/T2
[H+][OH–] = 10–14
pH = –log[H+]
pH + pOH = 14
K = °C + 273
q = mCΔT
R = 0.0821 L· atm/mol· K
NA = 6.023 × 1023
1 mile = 5280 ft
1 amu = 1.6606 × 10–24 g
1 inch = 2.54 cm
mass of proton: 1.6726 × 10–24 g
1 atm = 760 mm Hg = 760 torr
mass of electron: 9.1094 × 10–28 g
1 mL = 1 cm3
mass of neutron: 1.6749 × 10–24 g
1 cal = 4.184 J
1 mole of an ideal gas at STP occupies 22.4 liters
H
C
N
O
F
2.1
2.5
3.0
3.5
4.0
Electronegativities
K
0.8
Ca
1.0
Cl
3.0
Br
2.8
I
2.5
Periodic Table of the Elements
s-block
1
1A
1
2
H
1.008
2A
3
4
d-block transition metals
p-block
18
8A
2
He
13
3A
5
14
4A
6
15
5A
7
16
6A
8
17
7A
9
4.003
10
Li
Be
B
C
N
O
F
Ne
6.941
9.012
10.811
12.011
14.007
15.999
18.998
20.180
11
12
13
14
15
16
17
18
Na
Mg
22.990
24.305
19
20
3
3B
21
4
4B
22
5
5B
23
6
6B
24
7
7B
25
K
Ca
Sc
Ti
V
Cr
39.098
40.078
44.956
47.867
50.942
37
38
39
40
41
Rb
Sr
Y
Zr
85.468
87.62
88.906
55
56
57
Cs
Ba
La
132.905 137.328 138.905
10
26
9
8B
27
12
2B
30
Al
Si
P
S
Cl
Ar
26.981
28.086
30.974
32.065
35.453
39.948
28
11
1B
29
31
32
33
34
35
Mn
Fe
36
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
51.996
54.938
42
43
55.845
58.933
58.693
63.546
65.409
69.723
72.61
74.922
78.96
79.904
83.798
44
45
46
47
48
49
50
51
52
53
Nb
Mo
54
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
91.224
92.906
72
73
95.94
[98]
101.07
102.906
106.42
74
75
76
77
78
79
80
81
82
83
84
Hf
85
86
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
178.49
180.948
183.84
186.207
190.23
200.59
204.383
207.2
208.980
[209]
[210]
[222]
104
105
106
107
108
87
88
89
Fr
Ra
Ac
Rf
Db
Sg
Bh
[223]
[226]
[227]
[261]
[262]
[266]
[264]
58
59
60
61
62
Ce
Pr
Nd
Lanthanide
series
Actinide
series
140.116 140.908 144.242
Pm Sm
8
192.217 195.084 196.967
109
110
111
Hs
Mt
Ds
Rg
[277]
[268]
[271]
[272]
f-block transition metals
63
64
65
66
Eu
Gd
[145]
150.36
151.964
157.25
90
91
92
93
94
95
96
Th
Pa
U
Np
Pu
[237]
[244]
232.038 231.036 238.029
107.868 112.411 114.818 118.710 121.760
Am Cm
[243]
[247]
127.60
126.904 131.293
Copyright © 2007 by Keith S. Anliker
www.chem.iupui.edu/~anliker
67
68
69
70
71
Tb
Dy
Ho
Er
Tm
Yb
Lu
173.04
174.967
97
98
99
100
101
102
103
Bk
Cf
Es
Fm
Md
No
Lr
[247]
[251]
[252]
[257]
[258]
[259]
[262]
158.925 162.500 164.930 167.259 168.934