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E-grāmata: Basic Chemistry Concepts and Exercises

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(Emeritus, Southeast Community College, Lincoln, Nebraska, USA)
  • Formāts: 468 pages
  • Izdošanas datums: 04-Oct-2010
  • Izdevniecība: CRC Press Inc
  • Valoda: eng
  • ISBN-13: 9781439896044
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Basic Chemistry Concepts and ExercisesPalielināt
  • Formāts: 468 pages
  • Izdošanas datums: 04-Oct-2010
  • Izdevniecība: CRC Press Inc
  • Valoda: eng
  • ISBN-13: 9781439896044
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Chemistry can be a daunting subject for the uninitiated, and all too often, introductory textbooks do little to make students feel at ease with the complex subject matter. Basic Chemistry Concepts and Exercises brings the wisdom of John Kenkels more than 35 years of teaching experience to communicate the fundamentals of chemistry in a practical, down-to-earth manner.

Using conversational language and logically assembled graphics, the book concisely introduces each topic without overwhelming students with unnecessary detail. Example problems and end-of-chapter questions emphasize repetition of concepts, preparing students to become adept at the basics before they progress to an advanced general chemistry course. Enhanced with visualization techniques such as the first chapters mythical microscope, the book clarifies challenging, abstract ideas and stimulates curiosity into what can otherwise be an overwhelming topic.

Topics discussed in this reader-friendly text include:











Properties and structure of matter Atoms, molecules, and compounds The Periodic Table Atomic weight, formula weights, and moles Gases and solutions Chemical equilibrium Acids, bases, and pH Organic chemicals

The appendix contains answers to the homework exercises so students can check their work and receive instant feedback as to whether they have adequately grasped the concepts before moving on to the next section. Designed to help students embrace chemistry not with trepidation, but with confidence, this solid preparatory text forms a firm foundation for more advanced chemistry training.
Preface to faculty xiii
Preface to Students xv
Acknowledgments xxii
Author xix
Chapter 1 Properties and Structure of Matter
1(26)
1.1 What Chemists Do
2(1)
1.2 Properties and Change
2(2)
1.3 Classification of Matter
4(5)
1.3.1 Introduction
4(1)
1.3.2 Elements and Compounds
5(3)
1.3.3 Homogeneous vs. Heterogeneous
8(1)
1.4 Structure and Composition of Material Substances
9(4)
1.4.1 Structure and Composition of Elements
9(1)
1.4.2 Structure and Composition of Compunds
10(3)
1.5 A Quick Look inside the Atom
13(2)
1.6 Number of Subatomic Particles
15(5)
1.6.1 Protons and Eloectrons
15(1)
1.6.2 Neutrons and Isotopes
16(2)
1.6.3 Atomic Weight
18(1)
1.6.4 Important Isotopes
19(1)
1.7 Homework Exercises
20(7)
Chapter 2 Significant Figures, the Metric System, and Dimensional Analysis
27(36)
2.1 Introduction
28(1)
2.2 Reading a Measuring Device
28(2)
2.3 Significant Figures
30(4)
2.3.1 Rounding
32(1)
2.3.2 Scientific Notation
33(1)
2.3.3 Rules for Significant Figures
34(1)
2.4 Dimensional Analysis
34(4)
2.5 Metric System
38(7)
2.5.1 Length
39(1)
2.5.2 Mass (Weight)
40(1)
2.5.3 Volume
40(2)
2.5.4 Examples of Conversion Problems
42(3)
2.6 Density
45(6)
2.6.1 Introduction
45(2)
2.6.2 Measuring the Density of Solids That Have Regular Dimensions
47(1)
2.6.3 Measuring the Density of Irregularly Shaped Solids
48(1)
2.6.4 Measuring the Density of Liquids
49(1)
2.6.5 Using Density as a Conversion Factor
49(2)
2.6.6 Density of Water
51(1)
2.7 Temperature
51(2)
2.7.1 Introduction
51(1)
2.7.2 Temperature Scales
52(1)
2.8 Homework Exercises
53(10)
Chapter 3 Names and Formulas of Compounds
63(24)
3.1 Subclassifications of Elements
64(2)
3.2 Formation of Ions
66(3)
3.3 Formulas of Ionic Compounds
69(4)
3.4 Naming Ionic Compounds
73(2)
3.5 Other Metal Ions
75(1)
3.6 Other Negative Ions
76(1)
3.7 Binary Covalent Compounds
77(1)
3.8 Identifying and Naming Acids
78(2)
3.9 Bases and Salts
80(1)
3.10 Homework Exercises
81(6)
Chapter 4 Atomic Structure
87(32)
4.1 Introduction
88(1)
4.2 History of Theories and Experiments
89(3)
4.3 Modern Theory of Light
92(5)
4.3.1 What Is Energy?
93(1)
4.3.2 What Is Light?
94(3)
4.4 Bohr Model
97(2)
4.4.1 Introduction
97(1)
4.4.2 Bohr Model and Light
98(1)
4.5 Schrodinger Model
99(5)
4.6 Orbital Diagrams
104(3)
4.7 Electron Configuration
107(6)
4.8 Homework Exercises
113(6)
Chapter 5 Periodic Table
119(20)
5.1 Introduction
120(1)
5.2 Mendeleev and Meyer
120(1)
5.3 Descriptive Chemistry of Selected Elements
121(7)
5.3.1 Alkali Metals
122(1)
5.3.2 Alkaline Earth Metals
123(1)
5.3.3 Halogens
124(1)
5.3.4 Hydrogen and Helium
125(1)
5.3.5 Carbon, Nitrogen, Oxygen, Phosphorus, and Sulfur
125(1)
5.3.6 Aluminum and Silicon
126(1)
5.3.7 Selected Top-Row Transition Elements: Chromium, Manganese, Iron, Cobalt, Nickel, Copper, and Zinc
127(1)
5.4 Periodicity and Trends: Atomic Size, Ionization Energy, and Electron Affinity
128(7)
5.4.1 Atomic Size
130(1)
5.4.2 Ionization Energy and Electron Affinity
131(4)
5.5 Homework Exercises
135(4)
Chapter 6 Molecular Structure
139(34)
6.1 Chemical Bonding
140(1)
6.2 Outermost Electrons
141(1)
6.3 Simple Ionic Compounds
142(1)
6.4 Simple Covalent Compounds: Slot Filling
143(3)
6.5 More Complicated Covalent Compounds
146(6)
6.6 Coordinate Covalent Bonds
152(1)
6.7 More Complicated Ionic Compounds
153(2)
6.8 Structure of Ionic Compounds
155(1)
6.9 Polar Bonds and Molecules
156(6)
6.9.1 Electronegativity and Bond Polarity
156(2)
6.9.2 Polarity of Molecules
158(1)
6.9.3 Water and the Hydrogen Bond
159(2)
6.9.4 Hydrates
161(1)
6.10 Valence-Shell Electron-Pair Repulsion Theory
162(3)
6.11 Molecular Orbitals
165(3)
6.12 Homework Exercises
168(5)
Chapter 7 Atomic Weight, Formula Weight, and Moles
173(18)
7.1 Introduction
174(1)
7.2 Atomic Weight Revisited
174(1)
7.3 Molecular Weight and Formula Weight
175(2)
7.4 Mole
177(2)
7.4.1 Atomic and Formula Weight: Number of Grams per Mole of an Element or a Compound
177(2)
7.4.2 Avogadro's Number: Number of Particles per Mole
179(1)
7.5 Percent Composition of Compounds
179(3)
7.5.1 Percent Composition from Formulas and Atomic and Formula Weights
180(2)
7.6 Derivation of Empirical Formulas
182(4)
7.6.1 Empirical Formulas from Percent Composition
183(2)
7.6.2 Empirical Formulas vs. Molecular Formulas
185(1)
7.7 Homework Exercises
186(5)
Chapter 8 Chemical Equations and Stoichiometry
191(22)
8.1 Introduction to Chemical Equations
192(1)
8.2 Balancing Chemical Equations
193(6)
8.2.1 Quantitative Information from Chemical Equations
193(1)
8.2.2 Law of Conservation of Mass
194(1)
8.2.3 Process of Balancing Equations
195(4)
8.3 Optional Symbols
199(2)
8.4 Calculations Based on Equations
201(4)
8.4.1 Mole-to-Mole Conversions
202(1)
8.4.2 Mole-to-Gram and Gram-to-Mole Conversions
203(1)
8.4.3 Gram-to-Gram Conversions
204(1)
8.5 Limiting Reactant
205(2)
8.6 Theoretical Yield, Actual Yield, and Percent Yield
207(1)
8.7 Homework Exercises
208(5)
Chapter 9 Gases and the Gas Laws
213(34)
9.1 Introduction
214(1)
9.2 Properties of Gases
214(4)
9.3 Kinetic-Molecular Theory of Gases
218(2)
9.4 Gas Pressure
220(4)
9.5 Boyle's Law
224(3)
9.6 Charles' Law
227(3)
9.7 Combined Gas Law
230(1)
9.8 Standard Temperature and Pressure
231(1)
9.9 Correction of a Gas Volume to STP
231(1)
9.10 Ideal Gas Law
232(2)
9.11 Avogadro's Law
234(1)
9.12 Dalton's Law
235(1)
9.13 Vapor Pressure
236(3)
9.14 Homework Exercises
239(8)
Chapter 10 Solutions
247(32)
10.1 Introduction
248(1)
10.2 Terminology
248(1)
10.3 Expressing Concentration
249(3)
10.3.1 Percent
250(1)
10.3.2 Molarity
251(1)
10.4 Preparing Solutions
252(8)
10.4.1 Dilution
252(4)
10.4.2 Liquid Solute and Volume Percent
256(1)
10.4.3 Solid Solute and Weight-to-Volume Percent
257(1)
10.4.4 Solid Solute and Molarity
258(1)
10.4.5 Summary of Calculations
259(1)
10.5 More Terminology
260(3)
10.6 Increasing Dissolution Rate
263(1)
10.6.1 Particle Size
263(1)
10.6.2 Agitation
264(1)
10.6.3 Temperature
264(1)
10.7 Mechanism of Dissolving
264(6)
10.7.1 Ionic Solutes in Water
264(2)
10.7.2 Molecular Solutes in Water
266(2)
10.7.3 Nonaqueous Solvents
268(2)
10.8 Homework Exercises
270(9)
Chapter 11 Chemical Equilibrium
279(24)
11.1 Introduction
280(2)
11.2 Chemical Equilibrium
282(1)
11.3 Important Examples of Chemical Equilibrium
283(1)
11.4 Equilibrium Constant
284(3)
11.5 Position of the Equilibrium
287(1)
11.6 Magnitude of the Equilibrium Constant
288(2)
11.7 Le Chatelier's Principle
290(1)
11.8 Effect of Concentration Change
291(2)
11.9 Effect of Temperature Change
293(1)
11.10 Effect of Pressure Change
294(2)
11.11 Effect of Catalysts
296(1)
11.12 Homework Exercises
296(7)
Chapter 12 Acids, Bases, and pH
303(26)
12.1 Introduction
304(1)
12.2 Formulas and Strengths of Acids and Bases
304(4)
12.3 General Properties of Acids and Bases
308(2)
12.4 Acidity Level: pH
310(8)
12.4.1 Water Ionization and the Ion Product Constant
310(1)
12.4.2 pH
311(1)
12.4.3 Logarithms
312(3)
12.4.4 Significant Figures Rule
315(1)
12.4.5 pOH
315(1)
12.4.6 Relationship between pH and pOH
316(1)
12.4.7 Calculations Summary
316(2)
12.5 Measurement of pH
318(1)
12.6 Theories of Acids and Bases
319(2)
12.6.1 Arrhenius Theory
319(1)
12.6.2 Bronsted-Lowry Theory
319(2)
12.7 Reactions Involving Acids and Bases
321(3)
12.7.1 Neutralization
321(1)
12.7.2 Reaction of Acids with Metals
322(1)
12.7.3 Reaction of Metal and Nonmetal Oxides with Water
323(1)
12.7.4 Reaction of Metal Oxides with Acids
324(1)
12.8 "Add Acid to Water" Rule
324(1)
12.9 Homework Exercises
324(5)
Chapter 13 Oxidation-Reduction Reactions
329(14)
13.1 Oxidation-Reduction Reactions
330(6)
13.2 Ion-Electron Method for Balancing Equations
336(2)
13.3 Homework Exercises
338(5)
Chapter 14 Organic Chemicals
343(40)
14.1 Introduction
344(1)
14.2 Chemistry of Carbon and Its Compounds
345(1)
14.3 Hybridization of Orbitals
345(1)
14.4 Geometry around Bonded Carbon Atoms
346(2)
14.5 Physical Properties
348(2)
14.6 Hydrocarbons
350(12)
14.6.1 Alkanes
351(1)
14.6.2 Isomers
352(4)
14.6.3 Alkenes
356(1)
14.6.4 Alkynes
357(1)
14.6.5 Ring Structures
358(4)
14.7 Organic Compounds Containing Oxygen
362(8)
14.7.1 Alcohols
363(1)
14.7.2 Ethers
364(1)
14.7.3 A ldehydes
365(1)
14.7.4 Ketones
366(1)
14.7.5 Carboxylic Acids
367(1)
14.7.6 Esters
368(2)
14.8 Summaries of Hydrocarbon and Oxygen Classifications
370(1)
14.9 Polymers
370(6)
14.9.1 Addition Polymers
371(5)
14.10 Homework Exercises
376(7)
Appendix: Answers to Homework Exercises 383(52)
Index 435
John Kenkel is a chemistry instructor at Southeast Community College (SCC) in Lincoln, Nebraska. Throughout his 33-year career at SCC, he has been directly involved in the education of chemistry-based laboratory technicians in a vocational program presently named Laboratory Science Technology. He has also been heavily involved in chemistry-based laboratory technician education on a national scale, having served on a number of American Chemical Society (ACS) committees, including the Committee on Technician Activities and the Coordinating Committee for the Voluntary Industry Standards project. Kenkel has been the Principal Investigator for a series of curriculum development project grants funded by the National Science Foundation's Advanced Technological Education Program, from which three of his seven books evolved.
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