Chemistry, 6E
By John E. McMurry s
Email: Richard@qwconsultancy.com
Table of Contents Chapter 1
Chemistry: Matter and Measurement
1
Chapter 2
Atoms, Molecules, and Ions
10
Chapter 3
Mass Relationships in Chemical Reactions
22
Chapter 4
Reactions in Aqueous Solution
32
Chapter 5
Periodicity and the Electronic Structure of Atoms
41
Chapter 6
Ionic Bonds and Some Main-Group Chemistry
50
Chapter 7
Covalent Bonds and Molecular Structure
59
Chapter 8
Thermochemistry: Chemical Energy
69
Chapter 9
Gases: Their Properties and Behavior
80
Chapter 10
Liquids, Solids, and Phase Changes
87
Chapter 11
Solutions and Their Properties
98
Chapter 12
Chemical Kinetics
107
Chapter 13
Chemical Equilibrium
120
Chapter 14
Aqueous Equilibria: Acids and Bases
129
Chapter 15
Applications of Aqueous Equilibria
139
Chapter 16
Thermodynamics:
152
Entropy, Free Energy, and Equilibrium Chapter 17
Electrochemistry
160
Chapter 18
Hydrogen, Oxygen, and Water
172
Chapter 19
The Main-Group Elements
183
Chapter 20
Transition Elements and Coordination Chemistry
199
Chapter 21
Metals and Solid-State Materials
212
Chapter 22
Nuclear Chemistry
222
Chapter 23
Organic and Biological Chemistry
229
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CHAPTER 1 CHEMISTRY: MATTER AND MEASUREMENT Chapter Learning Goals for Students Section 1.1
Describe the processes involved in the scientific method.
Section 1.2
Give the symbol and name of elements mentioned in this chapter.
Section 1.3
Given the properties of boron and aluminum, show how Mendeleev predicted the properties of eka-aluminum (gallium). Identify the group number and period to which an element belongs. Identify the regions of the periodic table.
Section 1.4
Identify properties as extensive or intensive and as chemical or physical. Identify the regions of the periodic table.
Section 1.5
List the seven basic SI units of measure, and give the numerical equivalent of the common metric prefixes used with these units. Express numbers in scientific notation (textbook Appendix A).
Section 1.6
Interconvert metric and English masses.
Section 1.7
Interconvert metric and English lengths.
Section 1.8
Interconvert Fahrenheit, Celsius, and Kelvin temperatures.
Section 1.9
Interconvert metric and English volumes.
Section 1.10
Calculate densities from measured masses and volumes. Use density to interconvert mass and volume.
Section 1.11
Define and perform calculations involving kinetic energy and potential energy. Relate changes in energy to changes in mass that occur in chemical reactions.
Section 1.12
Distinguish between accuracy and precision. Determine the number of significant digits in a measured quantity.
Section 1.13
State the result of a calculation involving measured quantities to the correct number of significant digits.
Section 1.14
Use dimensional analysis to solve metric-English conversion problems.
1
Chapter 1—Chemistry: Matter and Measurement
Lecture Outline Introduction 1.1. Approaching Chemistry: Experimentation1 A. Scientific Method – systematic approach to research 1. Experimentation 2. Hypothesis – interpretation explaining results of many experiments 3. Theory – consistent explanation of known observations; logical interpretations of experimental results 1.2. Chemistry and the Elements2 A. Element – fundamental substance that can’t be chemically changed or broken down into anything simpler 1. Chemical symbol –represents a specific element a. Capitalize first letter b. Lower case used for second letter if present B. Periodic table – tabular organization of all 114 elements 1.3. Elements and the Periodic Table3 A. Creation of the periodic table – ideal example of how scientific theory comes into being 1. Random observations 2. Organization of data in ways that make sense 3. Consistent hypothesis emerges a. Explains known facts b. Makes predictions about unknown phenomena B. Mendeleev’s hypothesis about organizing known chemical information – meets criteria for a good hypothesis 1. Listed the known elements by atomic weight 2. Grouped them together according to their chemical reactivity 3. Was able to predict the properties of unknown elements – eka–aluminum, eka–silicon C. Periodic table – grid of the elements arranged in 7 horizontal rows and 18 vertical columns 1. Periods – seven horizontal rows in the periodic table 2. Groups – 18 vertical columns in the periodic table a. Groups numbered 1A → 8A and 1B → 8B (or 1 →18) b. Actually have 32 groups – lanthanides (14 elements after lanthanum) and actinides (14 elements after actinium) not included in the group numbers c. Elements in a given group have similar chemical properties. D. The periodic table of the elements is the most important organizing principle of chemistry. 1. Regular progression in size of the seven periods – reflects a similar regularity in atomic structure 2. Main Group (or Representative) Elements – Groups 1A-8A; (two larger groups on the left and six larger groups on the right of the table) 3. Transition Metal Elements – Groups 1B-8B; (10 smaller groups in the middle of the table) 4. Inner Transition Metal (or Rare Earth) Elements (14 groups shown separately at the bottom of the table) 1.4. Some Chemical Properties of the Elements4 A. Property – any characteristic used to describe or identify matter 1. Physical properties – characteristics not involving chemical change of the sample 2. Chemical properties – properties that do change chemical makeup of the sample 3. Intensive properties – sample size-independent properties 1
Test Item File Questions: Multiple Choice 1-2; Short Answer 1 Test Item File Questions: Multiple Choice 3-7; Algorithmic 1-5; Short Answer 3-4 3 Test Item File Questions: Multiple Choice 8-19; 116-135; Algorithmic 6-10; Short Answer 5-7 4 Test Item File Questions: Multiple Choice 20-33; Algorithmic 11-16; Short Answer 8-10 2
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Chapter 1—Chemistry: Matter and Measurement 4. Extensive properties – sample size-dependent properties B. Elements within a group have similar chemical properties. 1. Group 1A – Alkali metals a. Lustrous, silvery metals b. React rapidly with water to form highly alkaline products 2. Group 2A – Alkaline earth metals a. Lustrous, silvery metals b. Less reactive than alkali metals 3. Group 7A – Halogens a. Corrosive, nonmetallic elements b. Salt formers 4. Group 8A – Noble gases: gases with low reactivity C. Three major classes of elements 1. Metals a. Largest category of elements b. Found on the left side of the periodic table (left of the heavy zigzag line) i. Solids (except mercury) ii. Malleable iii. Ductile – can be drawn into thin wires without breaking iv. Conduct heat and electricity 2. Nonmetals a. Relatively small number b. Found on the right side of the periodic table (right of the heavy zigzag line) i. Gases, liquids, or solids ii. Brightly colored iii. Brittle solids iv. Poor conductors of heat and electricity 3. Semimetals (metalloids) a. Elements adjacent to the zigzag boundary between metals and nonmetals b. Properties fall between metals and nonmetals i. Brittle ii. Poor conductors of heat and electricity 1.5. Experimentation and Measurement5 A. International System (SI) of Units – seven base units (and units derived from them) that suffice for all scientific measurements (textbook Table 1.3) B. Common prefixes used to modify SI units 1. giga (G); factor = 109 6 2. mega (M); factor = 10 3 3. kilo (k); factor = 10 –1 4. deci (d); factor = 10 –2 5. centi (c); factor = 10 –3 6. milli (m); factor = 10 –6 7. micro (μ); factor = 10 –9 8. nano (n); factor = 10 C. Scientific notation – exponential format for very large or very small numbers (textbook Appendix A) D. All measurements of physical quantities contain a 1. number. 2. unit label. 1.6. Mass and Its Measurement6 5 6
Test Item File Questions: Multiple Choice 34-46; Algorithmic 17-19; Short Answer 11-12 Test Item File Questions: Multiple Choice 47-54; Algorithmic 20-23; Short Answer 13 3