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Periodic Table of the Elements
Hydrogen
1
H
1
2
3
4
5
6
7
MAIN GROUP METALS
1.0079
1A
(1)
2A
(2)
Lithium
3
Beryllium
4
Li
TRANSITION METALS
Uranium
92
U
METALLOIDS
Be
6.941
9.0122
Sodium Magnesium
12
11
Na
Mg
3B
(3)
4B
(4)
5B
(5)
6B
(6)
7B
(7)
22.9898
24.3050
Potassium
19
Calcium
20
Scandium Titanium Vanadium Chromium Manganese
22
23
24
25
21
39.0983
40.078
44.9559
K
Ca
Rubidium Strontium
37
38
Rb
Sr
Sc
Yttrium
39
Ti
47.867
V
50.9415
Cr
51.9961
Mn
54.9380
Y
Zr
Nb
Hf
Ta
Tc
W
Re
132.9055
Francium
87
137.327 138.9055 178.49 180.9479 183.84
186.207
Radium Actinium Rutherfordium Dubnium Seaborgium Bohrium
105
107
104
106
88
89
Fr
Ra
88.9059
91.224 92.9064
Lanthanum Hafnium Tantalum
57
72
73
Mo
87.62
Barium
56
Ba
La
Ac
(223.02) (226.0254) (227.0278)
Note: Atomic masses are
2007 IUPAC values
(up to four decimal places).
Numbers in parentheses are
atomic masses or mass numbers
of the most stable isotope of
an element.
kotz_48288_00a_ EP2-3_SE.indd 2
Atomic weight
8B
(8)
(9)
(10)
1B
(11)
Iron
26
Cobalt
27
Nickel
28
Copper
29
55.845
58.9332
58.6934
63.546
Fe
Co
Ni
Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium
45
41
42
43
40
44
46
85.4678
Cesium
55
Cs
Symbol
238.0289
NONMETALS
Atomic number
Rf
(267)
Lanthanides
Actinides
Db
(268)
95.96
(97.907)
Tungsten Rhenium
75
74
Sg
(271)
Bh
(272)
Ru
101.07
Osmium
76
Os
Rh
Pd
Ir
Pt
Cu
Silver
47
Ag
102.9055 106.42 107.8682
Iridium Platinum
Gold
77
79
78
Au
190.23
192.22
195.084 196.9666
Hassium Meitnerium Darmstadtium Roentgenium
109
110
111
108
Hs
(270)
Mt
(276)
Ds
(281)
Rg
(280)
Cerium
58
Praseodymium Neodymium Promethium Samarium Europium Gadolinium
59
60
61
64
63
62
140.116
140.9076
Ce
Pr
Nd
144.242
Pm
(144.91)
Sm
150.36
Eu
151.964
Thorium Protactinium Uranium Neptunium Plutonium Americium
92
94
91
90
93
95
Th
Pa
U
Np
Pu
Am
Gd
157.25
Curium
96
Cm
232.0381 231.0359 238.0289 (237.0482) (244.664) (243.061) (247.07)
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8A
(18)
Helium
2
He
3A
(13)
4A
(14)
5A
(15)
6A
(16)
7A
(17)
4.0026
Boron
5
Carbon
6
Nitrogen
7
Oxygen
8
Fluorine
9
Neon
10
10.811
Aluminum
13
12.011
Silicon
14
14.0067 15.9994
Phosphorus Sulfur
15
16
18.9984
Chlorine
17
20.1797
Argon
18
2B
(12)
26.9815
28.0855
30.9738
32.066
35.4527
39.948
Zinc
30
Gallium
31
Germanium
32
Arsenic
33
Selenium
34
Bromine
35
Krypton
36
65.38
69.723
72.61
74.9216
78.96
79.904
83.80
Cadmium
48
Indium
49
Tin
50
Iodine
53
Xenon
54
112.411
Mercury
80
114.818
Thallium
81
118.710
Lead
82
200.59
204.3833
207.2
B
Zn
Cd
Hg
Copernicium
112
Cn
(285)
Al
Ga
In
Tl
C
Si
Ge
Sn
Pb
Tb
P
As
O
S
Se
Antimony Tellurium
51
52
Sb
121.760
Bismuth
83
Bi
Te
F
Cl
Br
I
127.60 126.9045
Polonium Astatine
84
85
Po
At
208.9804 (208.98) (209.99)
Ne
Ar
Kr
Xe
131.29
Radon
86
Rn
(222.02)
Ununtrium Ununquadium Ununpentium Ununhexium Ununseptium Ununoctium
113
114
115
116
117
118
Uut
Discovered
2004
Uuq
Discovered
1999
Terbium Dysprosium Holmium
66
67
65
158.9254
N
Dy
162.50
Ho
164.9303
Uup
Uuh
Uus
Uuo
Discovered
2004
Discovered
1999
Discovered
2010
Erbium
68
Thulium
69
Ytterbium Lutetium
71
70
167.26
168.9342
173.054 174.9668
Er
Tm
Yb
Discovered
2002
Lu
Standard Colors
for Atoms in
Molecular Models
carbon atoms
hydrogen atoms
oxygen atoms
Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium
97
100
102
98
99
101
103
nitrogen atoms
(247.07)
chlorine atoms
Bk
kotz_48288_00a_ EP2-3_SE.indd 3
Cf
Es
(251.08) (252.08)
Fm
Md
(257.10) (258.10)
No
Lr
(259.10) (262.11)
11/22/10 1:37 PM
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eighth edition
chemistry
& Chemical Reactivity
John C. Kotz
State University of New York
College at Oneonta
Paul M. Treichel
University of Wisconsin–Madison
John R. Townsend
West Chester University of Pennsylvania
Australia • Brazil • Japan • Korea • Mexico • Singapore • Spain • United Kingdom • United States
kotz_48288_00c_FM_i-xxxiii.indd 1
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Chemistry & Chemical Reactivity, Eighth Edition
John C. Kotz, Paul M. Treichel, John R. Townsend
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brief contents
18 Principles of Chemical Reactivity: Other Aspects of
Aqueous Equilibria 806
Part ONE The Basic Tools of Chemistry
1
Basic Concepts of Chemistry
Let’s Review: The Tools of Quantitative Chemistry
2
Atoms, Molecules, and Ions
3
Chemical Reactions
4
Stoichiometry: Quantitative Information about
Chemical Reactions 156
5
Principles of Chemical Reactivity:
Energy and Chemical Reactions 208
Interchapter: The Chemistry of Fuels and Energy
Resources 252
1
24
19 Principles of Chemical Reactivity: Entropy and Free
Energy 858
20 Principles of Chemical Reactivity: Electron Transfer
Reactions 894
50
110
The Structure of Atoms
7
The Structure of Atoms and Periodic Trends
21 The Chemistry of the Main Group Elements
22 The Chemistry of the Transition Elements
23 Nuclear Chemistry
960
1016
1058
Appendices
266
A
Using Logarithms and Solving Quadratic Equations
300
B
Some Important Physical Concepts
Interchapter: Milestones in the Development of
Chemistry and the Modern View of Atoms and
Molecules 334
C
Abbreviations and Useful Conversion Factors
D
Physical Constants
8
Bonding and Molecular Structure
E
A Brief Guide to Naming Organic Compounds
9
Bonding and Molecular Structure: Orbital
Hybridization and Molecular Orbitals 400
F
Values for the Ionization Energies and Electron
Attachment Enthalpies of the Elements A-18
G
Vapor Pressure of Water at Various Temperatures
H
Ionization Constants for Aqueous Weak Acids
at 25 °C A-20
I
Ionization Constants for Aqueous Weak Bases
at 25 °C A-22
J
Solubility Product Constants for Some Inorganic
Compounds at 25 °C A-23
K
Formation Constants for Some Complex Ions in
Aqueous Solution at 25 °C A-25
L
Selected Thermodynamic Values
10 Carbon: Not Just Another Element
344
438
Interchapter: The Chemistry of Life: Biochemistry
490
Part THREE States of Matter
11
Gases and Their Properties
508
12 Intermolecular Forces and Liquids
13 The Chemistry of Solids
548
582
14 Solutions and Their Behavior
616
Interchapter: The Chemistry of Modern
Materials 656
15 Chemical Kinetics: The Rates of Chemical
Reactions 668
720
17 Principles of Chemical Reactivity: The Chemistry of
Acids and Bases 756
kotz_48288_00c_FM_i-xxxiii.indd 3
A-2
A-6
A-9
A-13
A-15
A-19
A-26
M Standard Reduction Potentials in Aqueous Solution at
25°C A-32
Part FOUR The Control of Chemical
Reactions
16 Principles of Chemical Reactivity: Equilibria
946
Part FIVE The Chemistry of the Elements
and Their Compounds
Part TWO The Structure of Atoms
and Molecules
6
Interchapter: The Chemistry of the Environment
N
Answers to Chapter Opening Questions and Case
Study Questions A-36
O
Answers to Check Your Understanding Questions
P
Answers to Review & Check Questions
Q
Answers to Selected Interchapter Study
Questions A-72
R
Answers to Selected Study Questions
A-47
A-63
A-75
iii
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iv
contents
Preface
xvii
Part ONE The Basic Tools of Chemistry
1
Basic Concepts of Chemistry
Gold! 1
1.1
Chemistry and Its Methods 2
Hypotheses, Laws, and Theories 3
A Closer Look: Careers in Chemistry 4
Goals of Science 5
Dilemmas and Integrity in Science 5
3
Mathematics of Chemistry 33
Exponential or Scientific Notation 33
Significant Figures 35
4
Problem Solving by Dimensional Analysis 39
Case Study: Out of Gas! 40
5
Graphs and Graphing 41
6
Problem Solving and Chemical Arithmetic 42
1
1.2
Sustainability and Green Chemistry 5
A Closer Look: Principles of Green Chemistry 6
1.3
Classifying Matter 6
States of Matter and Kinetic-Molecular Theory 7
Matter at the Macroscopic and Particulate Levels 8
Pure Substances 8
Mixtures: Homogeneous and Heterogeneous 9
1.4
Elements 10
A Closer Look: Element Names and Symbols 11
1.5
Compounds 12
1.6
Physical Properties 13
Extensive and Intensive Properties 14
1.7
Physical and Chemical Changes 15
1.8
Energy: Some Basic Principles 16
Case Study: CO2 in the Oceans 17
Conservation of Energy 18
Study Questions 44
2
Atoms, Molecules, and Ions
The Periodic Table, the Central Icon of Chemistry 50
2.1
Atomic Structure—Protons, Electrons,
and Neutrons 51
2.2
Atomic Number and Atomic Mass 52
Atomic Number 52
Relative Atomic Mass and the Atomic Mass Unit 52
Mass Number 52
2.3
Isotopes 54
Isotope Abundance 54
Determining Atomic Mass and Isotope Abundance 54
2.4
Atomic Weight 55
Case Study: Using Isotopes: Ötzi, the Iceman of the
Alps 58
2.5
The Periodic Table 58
Developing the Periodic Table 58
A Closer Look: The Story of the Periodic Table 59
Features of the Periodic Table 61
A Brief Overview of the Periodic Table and the
Chemical Elements 62
Chapter Goals Revisited 19
Key Equation 19
Study Questions 20
50
Let’s Review: The Tools of Quantitative
Chemistry 24
2.6
Molecules, Compounds, and Formulas 66
Formulas 66
Molecular Models 68
Copper 24
2.7
1
Units of Measurement 25
Temperature Scales 25
Length, Volume, and Mass 27
A Closer Look: Energy and Food 29
Energy Units 29
Ionic Compounds: Formulas, Names, and Properties 69
Ions 69
Formulas of Ionic Compounds 73
Names of Ions 74
Properties of Ionic Compounds 76
2.8
Molecular Compounds: Formulas and Names 78
2
Making Measurements: Precision, Accuracy,
Experimental Error, and Standard Deviation 30
Experimental Error 31
Standard Deviation 32
2.9
Atoms, Molecules, and the Mole 80
Atoms and Molar Mass 80
A Closer Look: Amedeo Avogadro and His Number 81
Molecules, Compounds, and Molar Mass 82
iv
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2.10 Describing Compound Formulas 85
Percent Composition 85
Empirical and Molecular Formulas from Percent
Composition 87
Determining a Formula from Mass Data 89
Case Study: Mummies, Bangladesh, and the Formula of
Compound 606 92
Determining a Formula by Mass Spectrometry 92
A Closer Look: Mass Spectrometry, Molar Mass,
and Isotopes 93
2.11 Hydrated Compounds 94
Chapter Goals Revisited 96
Key Equations 97
Study Questions 98
3.9
Chapter Goals Revisited 147
Study Questions 148
Applying Chemical Principles: Superconductors 155
4
Stoichiometry: Quantitative Information
about Chemical Reactions 156
The Chemistry of Pyrotechnics 156
4.1
Mass Relationships in Chemical Reactions:
Stoichiometry 157
4.2
Reactions in Which One Reactant Is Present in Limited
Supply 161
A Stoichiometry Calculation with a Limiting
Reactant 161
4.3
Percent Yield 165
Applying Chemical Principles: Argon—An Amazing
Discovery 109
3
Chemical Reactions
Black Smokers and Volcanoes 110
3.1
Introduction to Chemical Equations 111
A Closer Look: Antoine Laurent Lavoisier, 1743–1794 112
3.2
Balancing Chemical Equations 114
3.3
Introduction to Chemical Equilibrium 116
3.4
Aqueous Solutions 119
Ions and Molecules in Aqueous Solutions 119
Solubility of Ionic Compounds in Water 122
3.5
Precipitation Reactions 123
Predicting the Outcome of a Precipitation
Reaction 124
Net Ionic Equations 126
3.6
110
Acids and Bases 128
Acids and Bases: The Arrhenius Definition 128
Acids and Bases: The Brønsted–Lowry Definition 130
A Closer Look: The Hydronium Ion—The H1 Ion
in Water 131
Reactions of Acids and Bases 132
A Closer Look: Sulfuric Acid 133
Oxides of Nonmetals and Metals 134
3.7
Gas-Forming Reactions 136
3.8
Oxidation–Reduction Reactions 137
Oxidation-Reduction Reactions and Electron
Transfer 138
Oxidation Numbers 139
A Closer Look: Are Oxidation Numbers “Real”? 140
Recognizing Oxidation–Reduction Reactions 141
kotz_48288_00c_FM_i-xxxiii.indd 5
Classifying Reactions in Aqueous Solution 144
Case Study: Killing Bacteria with Silver 144
4.4 Chemical Equations and Chemical Analysis 166
Quantitative Analysis of a Mixture 167
Case Study: Green Chemistry and Atom Economy 168
Determining the Formula of a Compound by
Combustion 169
4.5
Measuring Concentrations of Compounds
in Solution 173
Solution Concentration: Molarity 173
Preparing Solutions of Known Concentration 175
A Closer Look: Serial Dilutions 178
4.6 pH, a Concentration Scale for Acids and Bases 178
4.7
Stoichiometry of Reactions in Aqueous Solution 181
Solution Stoichiometry 181
Titration: A Method of Chemical Analysis 182
Standardizing an Acid or Base 184
Determining Molar Mass by Titration 185
Titrations Using Oxidation–Reduction Reactions 186
Case Study: How Much Salt Is There in Seawater? 187
4.8
Spectrophotometry 188
Case Study: Forensic Chemistry: Titrations and Food
Tampering 189
Transmittance, Absorbance, and the Beer–Lambert
Law 189
Spectrophotometric Analysis 191
Chapter Goals Revisited 193
Key Equations 194
Study Questions 195
Applying Chemical Principles: Antacids 207
Contents
v
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