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Introductory Chemistry - 1st Canadian Edition: Appendix A: Periodic Table of the Elements

Introductory Chemistry - 1st Canadian Edition
Appendix A: Periodic Table of the Elements
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table of contents
  1. Cover
  2. Title Page
  3. Copyright
  4. Table Of Contents
  5. Acknowledgments
  6. Dedication
  7. About BCcampus Open Education
  8. Chapter 1. What is Chemistry
    1. Some Basic Definitions
    2. Chemistry as a Science
  9. Chapter 2. Measurements
    1. Expressing Numbers
    2. Significant Figures
    3. Converting Units
    4. Other Units: Temperature and Density
    5. Expressing Units
    6. End-of-Chapter Material
  10. Chapter 3. Atoms, Molecules, and Ions
    1. Acids
    2. Ions and Ionic Compounds
    3. Masses of Atoms and Molecules
    4. Molecules and Chemical Nomenclature
    5. Atomic Theory
    6. End-of-Chapter Material
  11. Chapter 4. Chemical Reactions and Equations
    1. The Chemical Equation
    2. Types of Chemical Reactions: Single- and Double-Displacement Reactions
    3. Ionic Equations: A Closer Look
    4. Composition, Decomposition, and Combustion Reactions
    5. Oxidation-Reduction Reactions
    6. Neutralization Reactions
    7. End-of-Chapter Material
  12. Chapter 5. Stoichiometry and the Mole
    1. Stoichiometry
    2. The Mole
    3. Mole-Mass and Mass-Mass Calculations
    4. Limiting Reagents
    5. The Mole in Chemical Reactions
    6. Yields
    7. End-of-Chapter Material
  13. Chapter 6. Gases
    1. Pressure
    2. Gas Laws
    3. Other Gas Laws
    4. The Ideal Gas Law and Some Applications
    5. Gas Mixtures
    6. Kinetic Molecular Theory of Gases
    7. Molecular Effusion and Diffusion
    8. Real Gases
    9. End-of-Chapter Material
  14. Chapter 7. Energy and Chemistry
    1. Formation Reactions
    2. Energy
    3. Stoichiometry Calculations Using Enthalpy
    4. Enthalpy and Chemical Reactions
    5. Work and Heat
    6. Hess’s Law
    7. End-of-Chapter Material
  15. Chapter 8. Electronic Structure
    1. Light
    2. Quantum Numbers for Electrons
    3. Organization of Electrons in Atoms
    4. Electronic Structure and the Periodic Table
    5. Periodic Trends
    6. End-of-Chapter Material
  16. Chapter 9. Chemical Bonds
    1. Lewis Electron Dot Diagrams
    2. Electron Transfer: Ionic Bonds
    3. Covalent Bonds
    4. Other Aspects of Covalent Bonds
    5. Violations of the Octet Rule
    6. Molecular Shapes and Polarity
    7. Valence Bond Theory and Hybrid Orbitals
    8. Molecular Orbitals
    9. End-of-Chapter Material
  17. Chapter 10. Solids and Liquids
    1. Properties of Liquids
    2. Solids
    3. Phase Transitions: Melting, Boiling, and Subliming
    4. Intermolecular Forces
    5. End-of-Chapter Material
  18. Chapter 11. Solutions
    1. Colligative Properties of Solutions
    2. Concentrations as Conversion Factors
    3. Quantitative Units of Concentration
    4. Colligative Properties of Ionic Solutes
    5. Some Definitions
    6. Dilutions and Concentrations
    7. End-of-Chapter Material
  19. Chapter 12. Acids and Bases
    1. Acid-Base Titrations
    2. Strong and Weak Acids and Bases and Their Salts
    3. Brønsted-Lowry Acids and Bases
    4. Arrhenius Acids and Bases
    5. Autoionization of Water
    6. Buffers
    7. The pH Scale
    8. End-of-Chapter Material
  20. Chapter 13. Chemical Equilibrium
    1. Chemical Equilibrium
    2. The Equilibrium Constant
    3. Shifting Equilibria: Le Chatelier’s Principle
    4. Calculating Equilibrium Constant Values
    5. Some Special Types of Equilibria
    6. End-of-Chapter Material
  21. Chapter 14. Oxidation and Reduction
    1. Oxidation-Reduction Reactions
    2. Balancing Redox Reactions
    3. Applications of Redox Reactions: Voltaic Cells
    4. Electrolysis
    5. End-of-Chapter Material
  22. Chapter 15. Nuclear Chemistry
    1. Units of Radioactivity
    2. Uses of Radioactive Isotopes
    3. Half-Life
    4. Radioactivity
    5. Nuclear Energy
    6. End-of-Chapter Material
  23. Chapter 16. Organic Chemistry
    1. Hydrocarbons
    2. Branched Hydrocarbons
    3. Alkyl Halides and Alcohols
    4. Other Oxygen-Containing Functional Groups
    5. Other Functional Groups
    6. Polymers
    7. End-of-Chapter Material
  24. Chapter 17. Kinetics
    1. Factors that Affect the Rate of Reactions
    2. Reaction Rates
    3. Rate Laws
    4. Concentration–Time Relationships: Integrated Rate Laws
    5. Activation Energy and the Arrhenius Equation
    6. Reaction Mechanisms
    7. Catalysis
    8. End-of-Chapter Material
  25. Chapter 18. Chemical Thermodynamics
    1. Spontaneous Change
    2. Entropy and the Second Law of Thermodynamics
    3. Measuring Entropy and Entropy Changes
    4. Gibbs Free Energy
    5. Spontaneity: Free Energy and Temperature
    6. Free Energy under Nonstandard Conditions
    7. End-of-Chapter Material
  26. Appendix A: Periodic Table of the Elements
  27. Appendix B: Selected Acid Dissociation Constants at 25°C
  28. Appendix C: Solubility Constants for Compounds at 25°C
  29. Appendix D: Standard Thermodynamic Quantities for Chemical Substances at 25°C
  30. Appendix E: Standard Reduction Potentials by Value
  31. Glossary
  32. About the Authors
  33. Versioning History

1

Appendix A: Periodic Table of the Elements

David W. Ball

In this appendix, we present some data on the chemical elements. The periodic table, introduced in Chapter 3 “Atoms, Molecules, and Ions,” lists all the known chemical elements, arranged by atomic number (that is, the number of protons in the nucleus). The periodic table is arguably the best tool in all of science; no other branch of science can summarize its fundamental constituents in such a concise and useful way. Many of the physical and chemical properties of the elements are either known or understood based on their positions on the periodic table. Periodic tables are available with a variety of chemical and physical properties listed in each element’s box. What follows here is a more complex version of the periodic table than what was presented in the chapter “Atoms, Molecules, and Ions.” The internet is a great place to find periodic tables that contain additional information.

One item on most periodic tables is the atomic mass of each element. For many applications, only one or two decimal places are necessary for the atomic mass. However, some applications (especially nuclear chemistry; see Chapter 15 “Nuclear Chemistry”) require more decimal places. The atomic masses in Table A.1 “The Basics of the Elements of the Periodic Table” represent the number of decimal places recognized by the International Union of Pure and Applied Chemistry, the worldwide body that develops standards for chemistry. The atomic masses of some elements are known very precisely, to a large number of decimal places. The atomic masses of other elements, especially radioactive elements, are not known as precisely. Some elements, such as lithium, can have varying atomic masses depending on how their isotopes are isolated.

The web offers many interactive periodic table resources. For example, see PTable and the Accessible Syngenta Periodic Table of Elements.

First half of the periodic table of elements.Second half of the periodic table of elements.

Table A.1 The Basics of the Elements of the Periodic Table
NameAtomic SymbolAtomic NumberAtomic MassFootnotes
actinium*Ac89
aluminumAl1326.9815386(8)
americium*Am95
antimonySb51121.760(1)g
argonAr1839.948(1)g, r
arsenicAs3374.92160(2)
astatine*At85
bariumBa56137.327(7)
berkelium*Bk97
berylliumBe49.012182(3)
bismuthBi83208.98040(1)
bohrium*Bh107
boronB510.811(7)g, m, r
bromineBr3579.904(1)
cadmiumCd48112.411(8)g
caesium (cesium)Cs55132.9054519(2)
calciumCa2040.078(4)g
californium*Cf98
carbonC612.0107(8)g, r
ceriumCe58140.116(1)g
chlorineCl1735.453(2)g, m, r
chromiumCr2451.9961(6)
cobaltCo2758.933195(5)
copernicium*Cn112
copperCu2963.546(3)r
curium*Cm96
darmstadtium*Ds110
dubnium*Db105
dysprosiumDy66162.500(1)g
einsteinium*Es99
erbiumEr68167.259(3)g
europiumEu63151.964(1)g
fermium*Fm100
fluorineF918.9984032(5)
francium*Fr87
gadoliniumGd64157.25(3)g
galliumGa3169.723(1)
germaniumGe3272.64(1)
goldAu79196.966569(4)
hafniumHf72178.49(2)
hassium*Hs108
heliumHe24.002602(2)g, r
holmiumHo67164.93032(2)
hydrogenH11.00794(7)g, m, r
indiumIn49114.818(3)
iodineI53126.90447(3)
iridiumIr77192.217(3)
ironFe2655.845(2)
kryptonKr3683.798(2)g, m
lanthanumLa57138.90547(7)g
lawrencium*Lr103
leadPb82207.2(1)g, r
lithiumLi3[6.941(2)]†g, m, r
lutetiumLu71174.967(1)g
magnesiumMg1224.3050(6)
manganeseMn2554.938045(5)
meitnerium*Mt109
mendelevium*Md101
mercuryHg80200.59(2)
molybdenumMo4295.94(2)g
neodymiumNd60144.242(3)g
neonNe1020.1797(6)g, m
neptunium*Np93
nickelNi2858.6934(2)
niobiumNb4192.90638(2)
nitrogenN714.0067(2)g, r
nobelium*No102
osmiumOs76190.23(3)g
oxygenO815.9994(3)g, r
palladiumPd46106.42(1)g
phosphorusP1530.973762(2)
platinumPt78195.084(9)
plutonium*Pu94
polonium*Po84
potassiumK1939.0983(1)
praseodymiumPr59140.90765(2)
promethium*Pm61
protactinium*Pa91231.03588(2)
radium*Ra88
radon*Rn86
roentgenium*Rg111
rheniumRe75186.207(1)
rhodiumRh45102.90550(2)
rubidiumRb3785.4678(3)g
rutheniumRu44101.07(2)g
rutherfordium*Rf104
samariumSm62150.36(2)g
scandiumSc2144.955912(6)
seaborgium*Sg106
seleniumSe3478.96(3)r
siliconSi1428.0855(3)r
silverAg47107.8682(2)g
sodiumNa1122.98976928(2)
strontiumSr3887.62(1)g, r
sulfurS1632.065(5)g, r
tantalumTa73180.94788(2)
technetium*Tc43
telluriumTe52127.60(3)g
terbiumTb65158.92535(2)
thalliumTl81204.3833(2)
thorium*Th90232.03806(2)g
thuliumTm69168.93421(2)
tinSn50118.710(7)g
titaniumTi2247.867(1)
tungstenW74183.84(1)
ununhexium*Uuh116
ununoctium*Uuo118
ununpentium*Uup115
ununquadium*Uuq114
ununtrium*Uut113
uranium*U92238.02891(3)g, m
vanadiumV2350.9415(1)
xenonXe54131.293(6)g, m
ytterbiumYb70173.04(3)g
yttriumY3988.90585(2)
zincZn3065.409(4)
zirconiumZr4091.224(2)g
*Element has no stable nuclides. However, three such elements (Th, Pa, and U) have a characteristic terrestrial isotopic composition, and for these an atomic mass is tabulated.
†Commercially available Li materials have atomic weights that range between 6.939 and 6.996; if a more accurate value is required, it must be determined for the specific material.
g Geological specimens are known in which the element has an isotopic composition outside the limits for normal material. The difference between the atomic mass of the element in such specimens and that given in the table may exceed the stated uncertainty.
m Modified isotopic compositions may be found in commercially available material because it has been subjected to an undisclosed or inadvertent isotopic fractionation. Substantial deviations in the atomic mass of the element from that given in the table can occur.
r Range in isotopic composition of normal terrestrial material prevents a more precise Ar(E) being given; the tabulated Ar(E) value and uncertainty should be applicable to normal material.

Source: Adapted from Pure and Applied Chemistry 78, no. 11 (2005): 2051–66. © IUPAC (International Union of Pure and Applied Chemistry).

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Appendix B: Selected Acid Dissociation Constants at 25°C
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Copyright © 2014

                                by Jessie A. Key

            Introductory Chemistry - 1st Canadian Edition by Jessie A. Key is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License, except where otherwise noted.
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