MARC details
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08244cam a2200265 a 4500 |
| 001 - CONTROL NUMBER |
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724334 |
| 003 - CONTROL NUMBER IDENTIFIER |
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OSt |
| 005 - DATE AND TIME OF LATEST TRANSACTION |
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20231205165838.0 |
| 008 - FIXED-LENGTH DATA ELEMENTS--GENERAL INFORMATION |
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| fixed length control field |
980227s2000 maua 001 0 eng |
| 010 ## - LIBRARY OF CONGRESS CONTROL NUMBER |
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| LC control number |
98004528 |
| 020 ## - INTERNATIONAL STANDARD BOOK NUMBER |
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| International Standard Book Number |
9780697395979 |
| 020 ## - INTERNATIONAL STANDARD BOOK NUMBER |
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| International Standard Book Number |
0697395979 (acidfree paper) |
| 040 ## - CATALOGING SOURCE |
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| Original cataloging agency |
BUL |
| Transcribing agency |
BUL |
| Modifying agency |
BUL |
| Language of cataloging |
eng |
| Description conventions |
rda |
| 082 00 - DEWEY DECIMAL CLASSIFICATION NUMBER |
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| Classification number |
540 |
| Edition number |
21 |
| Item number |
SIL |
| 100 1# - MAIN ENTRY--PERSONAL NAME |
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| Personal name |
Silberberg, Martin S. |
| Fuller form of name |
(Martin Stuart) |
| 245 10 - TITLE STATEMENT |
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| Title |
Chemistry : |
| Remainder of title |
the molecular nature of matter and change / |
| Statement of responsibility, etc. |
Martin Silberberg ; consultants, Randy Duran . . . [et al.]. |
| 250 ## - EDITION STATEMENT |
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| Edition statement |
2nd edition. |
| 260 ## - PUBLICATION, DISTRIBUTION, ETC. |
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| Place of publication, distribution, etc. |
Boston : |
| Name of publisher, distributor, etc. |
McGraw-Hill, |
| Date of publication, distribution, etc. |
c2000. |
| 300 ## - PHYSICAL DESCRIPTION |
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| Extent |
xxxii, (various pagings) : |
| Other physical details |
ill. (some col.) ; |
| Dimensions |
28 cm. |
| 500 ## - GENERAL NOTE |
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| General note |
Contents;<br/><br/>Chapter 1. Keys to the study of chemistry<br/>1.1 Some fundamental definitions<br/>1.2 Chemical arts and the origins of modern chemistry<br/>1.3 The scientific approach: Developing a model<br/>1.4 Chemistry problem solving<br/>1.5 Measurement in scientific study<br/>etc.<br/><br/>Chapter 2. The components of matter<br/>2.1 Elements, compounds and mixtures: An atomic overview<br/>2.2 The observation that led to an atomic view of matter<br/>2.3 Dalton's Atomic theory<br/>2.4 The observations that led to the nuclear Atom model<br/>2.5 The Atomic theory today<br/>etc.<br/><br/>Chapter 3. Stoichiometry: Mole-mass-number relationships in chemical systems<br/>3.1 The mole<br/>3.2 Determining the formula of the unknown compound<br/>3.3 Writing and balancing chemical equations<br/>3.4 Calculating amounts of reactant and product<br/>3.5 Fundamentals of solution stoichiometry<br/><br/>Chapter 4. The major classes of chemical reactions<br/>4.1 The role of water as a solvent<br/>4.2 Writing equations for aqueous ionic reactions<br/>4.3 Precipitation reactions<br/>4.4 Acid-base reactions<br/>4.5 Oxidation-reduction ( redox) reactions<br/><br/>Chapter 5. Gases and the kinetic-molecular theory<br/>5.1 An overview of th physical states of matter<br/>5.2 Gas pressure and its measurement<br/>5.3 The gas laws and their experimental foundations<br/>5.4 Further applications of the ideal gas law<br/>5.5 The ideal gas law and reactions stoichiometry<br/>etc.<br/><br/>Chapter 6. Thermochemistry: Energy flow and chemical change<br/>6.1 Forms of energy and their interconversion<br/>6.2 Enthalpy: Heats of reaction and chemical change<br/>6.3 Calorimetry:Laboratory measurement of heats of reactions<br/>6.4 Stoichiometry of thermochemical equations<br/>6.5 Hess's law of heat summation<br/>etc.<br/><br/>Chapter 7. Quantum theory and atomic structure<br/>7.1 The nature of light<br/>7.2 Atomic spectra<br/>7.3 The wave-particle duality of matter and energy<br/>7.4 The quantum-mechanical model of the atom<br/><br/>Chapter 8. Electron configuration and chemical periodicity<br/>8.1 Development of the periodic table<br/>8.2 Characteristics of many-electron atoms<br/>8.3 The quantum-mechanical model and the periodic table<br/>8.4 Trends in some key periodic atomic properties<br/>8.5 The connection between atomic structure and chemical reactivity<br/><br/>Chapter 9. Models of chemical bonding<br/>9.1 Atomic properties and chemical bonds<br/>9.2 The ionic bonding model<br/>9.3 The covalent bonding model<br/>9.4 Between the extremes: Electronegativity and bond polarity<br/>9.5 An introduction to metallic bonding<br/><br/>Chapter 10. The shapes of molecules<br/>10.1 Depicting molecules and ions with Lewis structure<br/>10.2 Using Lewis structures and bond energies to calculate heats of reaction<br/>10.3 Valence-shell electron-pair repulsion (VSEPR) theory and molecular shape<br/>10.4 Molecular shape and molecular polarity<br/>etc.<br/><br/>Chapter 11. Theories of covalent bonding<br/>11.1 Valence bond (VB) theory and orbital hybridization<br/>11.2 The mode of orbital overlap and the types of covalent bonds<br/>11.3 Molecular orbital (MO) theory and electron delocalization<br/><br/>Chapter 12<br/><br/>Intermolecular forces:Liquids,solids and phase changes<br/>12.1 An overview of physical states and phase changes<br/>12.2 Quantitative aspects of phase changes<br/>12.3 Types of intermolecular forces<br/>12.4 Properties of the liquid state<br/>etc.<br/><br/>Chapter 13. The properties of mixtures: solutions and colloids<br/>13.1 Types of solutions: intermolecular forces and predicting solubility<br/>13.2 Energy changes in the solution process<br/>13.3 Solubility as an equilibrium process<br/>13.4 Quantitative ways of expressing concentration<br/>etc.<br/><br/>Chapter 14. Periodic patterns in the main- group elements:Bonding,structure, and reactivity<br/>14.1 Hydrogen, the simplest atom<br/>14.2 Trends across the periodic table: The period elements<br/>14.3 Group 1A (1): The alkali metals<br/>14.4 Group 1A (2):The alkaline earth metals<br/>etc.<br/><br/>Chapter 15. Organic compounds and the atomic properties of carbon<br/>15.1 The special nature of carbon and the characteristics of organic molecules<br/>15.2 The structures and classes of hydrocarbons<br/>15.3 Some important classes of organic reactions<br/>15.4 Properties and reactivities of common functional groups<br/><br/>Chapter 16. Kinetics: Rates and Mechanisms of Chemical Reactions <br/>16.1 Factors That Influence Reaction Rate <br/>16.2 Expressing the Reaction Rate <br/>16.3 The Rate Law and Its Components <br/>Tools of the Laboratory: Measuring Reaction Rates <br/>Determining the Initial Rate Reaction Order Terminology <br/>Determining Reaction Orders Determining the Rate Constant <br/>16.4 Integrated Rate Laws: Concentration Changes over Time Integrated Rate Laws for First-, Second-, and Zero-Order Reactions Determining the Reaction Order from the Integrated Rate Law Reaction Half-Life <br/>etc.<br/><br/>Chapter 17. Equilibrium: The Extent of Chemical Reactions <br/>17.1 The Dynamic Nature of the Equilibrium State <br/>17.2 The Reaction Quotient and the Equilibrium Constant <br/>Writing the Reaction Quotient <br/>Variations in the Form of the Reaction Quotient <br/>17.3 Expressing Equilibria with Pressure Terms: Relation Between Kc and Kp <br/>17.4 Reaction Direction: Comparing Q and K <br/><br/>etc.<br/><br/><br/>Chapter 18. Acid-Base Equilibria <br/>18.1 Acids and Bases in Water Release of H+ or OH- and the Classical Acid-Base Definition Variation in Acid Strength: The Acid-Dissociation Constant (Ka) Classifying the Relative Strengths of Acids and Bases <br/>18.2 Autoionization of Water and the pH Scale The Equilibrium Nature of Autoionization: The Ion-Product Constant for Water (Kw) Expressing the Hydronium Ion Concentration: The pH Scale 18.3 Proton Transfer and the Bronsted-Lowry Acid-Base Definition The Conjugate Acid-Base PairRelative Acid-Base Strength and the Net Direction of Reaction <br/>18.4 Solving Problems Involving Weak-Acid Equilibria Finding Ka Given a Concentration Finding Concentration Given Ka The Effect of Concentration on the Extent of Acid Dissociation The Behavior of Polyprotic Acids <br/>etc<br/><br/>Chapter 19. Ionic Equilibria in Aqueous Systems <br/>19.1 Equilibria of Acid-Base Buffer Systems <br/>How a Buffer Works: The Common-Ion Effect <br/>The Henderson-Hasselbalch Equation Buffer Capacity and Buffer Range <br/>Preparing a Buffer <br/>19.2 Acid-Base Titration Curves <br/>Monitoring pH with Acid-Base Indicators <br/>Strong Acid-Strong Base Titration Curves <br/>Weak Acid-Strong Base Titration Curves <br/>Weak Base-Strong Acid Titration Curves <br/>Titration Curves for Polyprotic Acids Amino Acids as Biological Polyprotic Acids <br/>19.3 Equilibria of Slightly Soluble Ionic Compounds <br/>The Ion-Product Expression (Qsp) and the Solubility-Product Constant (Ksp) <br/>Calculations Involving the Solubility-Product Constant <br/>The Effect of a Common Ion on Soubility <br/>The Effect of pH on Solubility Chemical Connections to Geology: Creation of a Limestone Cave Predicting the Formation of a Precipitate: Qsp vs. Ksp Chemical Connections to Environmental Science: The Acid-Rain Problem <br/>19.4 Equilibria Involving Complex Ions Formation of Complex Ions Complex Ions and the Solubility of Precipitates Complex Ions of Amphoteric Hydroxides <br/>etc.<br/><br/><br/>Chapter 20. Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions <br/><br/>Chapter 21. Eletrochemistry : Chemical Change and Electrical Work<br/><br/>Chapter 22.The Elements in Nature and Industry<br/><br/>Chapter 23. The Transition Elements and their Coordination Compounds <br/><br/>Chapter 24. Nuclear Reactions and their Applications <br/> |
| 504 ## - BIBLIOGRAPHY, ETC. NOTE |
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| Bibliography, etc. note |
Includes bibliographical references and index |
| 650 #0 - SUBJECT ADDED ENTRY--TOPICAL TERM |
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| Topical term or geographic name entry element |
Chemistry. |
| 942 ## - ADDED ENTRY ELEMENTS (KOHA) |
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| Source of classification or shelving scheme |
Dewey Decimal Classification |
| Koha item type |
Book Open Access |
| Edition |
2nd edition |
| Classification part |
540 |
| Item part |
1 |
| Call number prefix |
SIL |
| Call number suffix |
540 SIL |
