From its very origin, Introductory Chemistry: An Atoms First Approach has been developed and written using an atoms first approach specific to introductory chemistry. It is not a pared down version of a general chemistry text, but carefully crafted with the introductory chemistry student in mind. The ordering of topics facilitates the conceptual development of chemistry for the novice, rather than the historical development that has been used traditionally. Its language and style are student‐friendly and conversational and the importance and wonder of chemistry in everyday life are emphasised at every opportunity.
Continuing in the Burdge tradition, this text employs an outstanding art program, a consistent problem-solving approach, interesting applications woven throughout the chapters and a wide range of end-of-chapter problems.
By:
Julia Burdge,
Michelle Driessen
Imprint: McGraw-Hill Education
Country of Publication: United States
Edition: 2nd edition
Dimensions:
Height: 274mm,
Width: 216mm,
Spine: 20mm
Weight: 1.089kg
ISBN: 9781260565867
ISBN 10: 1260565866
Pages: 626
Publication Date: 29 January 2019
Audience:
College/higher education
,
Primary
Replaced By: 1266137076
Format: Paperback
Publisher's Status: Active
Chapter 1 Atoms and Elements 1.1 The Study of Chemistry 1.2 Atoms First 1.3 Subatomic Particles and the Nuclear Model of the Atom 1.4 Elements and the Periodic Table 1.5 Organization of the Periodic Table 1.6 Isotopes 1.7 Atomic Mass Chapter 2 Electrons and the Periodic Table 2.1 The Nature of Light 2.2 The Bohr Atom 2.3 Atomic Orbitals 2.4 Electron Configurations 2.5 Electron Configurations and the Periodic Table 2.6 Periodic Trends 2.7 Ions: The Loss and Gain of Electrons Chapter 3 Compounds and Chemical Bonds 3.1 Matter: Classification and Properties 3.2 Ionic Bonding and Binary Ionic Compounds 3.3 Naming Ions and Binary Ionic Compounds 3.4 Covalent Bonding and Molecules 3.5 Naming Binary Molecular Compounds 3.6 Covalent Bonding in Ionic Species: Polyatomic Ions 3.7 Acids 3.8 Substances in Review Chapter 4 How Chemists Use Numbers 4.1 Units of Measurement 4.2 Scientific Notation 4.3 Significant Figures 4.4 Unit Conversion 4.5 Success in Introductory Chemistry Class Chapter 5 The Mole and Chemical Formulas 5.1 Counting Atoms by Weighing 5.2 Counting Molecules by Weighing 5.3 Mass Percent Composition 5.4 Using Mass Percent Composition to Determine Empirical Formula 5.5 Using Empirical Formula and Molar Mass to Determine Molecular Formula Chapter 6 Molecular Shape 6.1 Drawing Simple Lewis Structures 6.2 Lewis Structures Continued 6.3 Resonance Structures 6.4 Molecular Shape 6.5 Electronegativity & Polarity 6.6 Intermolecular Forces Chapter 7 Solids, Liquids, and Phase Changes 7.1 General Properties of the Condensed Phases 7.2 Types of Solids 7.3 Physical Properties of Solids 7.4 Physical Properties of Liquids 7.5 Energy and Physical Changes Chapter 8 Gases 8.1 Properties of Gases 8.2 Pressure 8.3 The Gas Equations 8.4 The Gas Laws 8.5 Gas Mixtures Chapter 9 Physical Properties of Solutions 9.1 General Properties of Solutions 9.2 Aqueous Solubility 9.3 Solution Concentration 9.4 Solution Composition 9.5 Solution Preparation 9.6 Colligative Properties Chapter 10 Chemical Reactions and Chemical Equations 10.1 Recognizing Chemical Reactions 10.2 Representing Chemical Reactions with Chemical Equations 10.3 Balancing Chemical Equations 10.4 Types of Chemical Reactions 10.5 Chemical Reactions and Energy 10.6 Chemical Reactions in Review Chapter 11 Using Balanced Chemical Equations 11.1 Mole to Mole Conversions 11.2 Mass to Mass Conversions 11.3 Limitations on Reaction Yield 11.4 Aqueous Reactions 11.5 Gases in Chemical Reactions 11.6 Chemical Reactions and Heat Chapter 12 Acids and Bases 12.1 Properties of Acids and Bases 12.2 Definitions of Acids and Bases 12.3 Water as an Acid; Water as a Base 12.4 Strong Acids and Bases 12.5 pH and pOH Scales 12.6 Weak Acids and Bases 12.7 Acid-Base Titrations 12.8 Buffers Chapter 13 Equilibrium 13.1 Reaction Rates 13.2 Chemical Equilibrium 13.3 Equilibrium Constants 13.4 Factors that Affect Equilibrium Chapter 14 Organic Chemistry 14.1 Why Carbon is Different 14.2 Hydrocarbons 14.3 Isomers 14.4 Functional Groups 14.5 Alcohols and Ethers 14.6 Aldehydes & Ketones 14.7 Carboxylic Acids and Esters 14.8 Amines and Amides 14.9 Polymers Chapter 15 Biochemistry 15.1 Biologically Important Molecules 15.2 Lipids 15.3 Proteins 15.4 Carbohydrates 15.5 Nucleic Acids Chapter 16 Nuclear Chemistry 16.1 Radioactive Decay 16.2 Detection of Radiation and its Biological Effects 16.3 Dating using Radioactive Decay 16.4 Medical Applications of Radioactivity 16.5 Nuclear Fission and Nuclear Fusion Chapter 17 Electrochemistry 17.1 Balancing Oxidation-Reduction Reactions using the Half-Reaction Method 17.2 Batteries 17.3 Corrosion 17.4 Electrolysis
Dr. Julia Burdge did most of her undergraduate work at Iowa State University, completing her bachelors degree and Masters degree in inorganic chemistry at the University of South Florida in Tampa. She earned her Ph.D. in analytical chemistry at the University of Idaho. Her Masters and doctoral research involved the development of chemotherapeutic analogs of cisplatin and the development of instruments and methods for measuring ultra-trace concentrations of atmospheric sulfur compounds. Over the past 20 years, she has taught introductory and advanced courses in every division of the undergraduate chemistry curriculum, as well as interdisciplinary courses. She also developed and taught a new introductory chemistry course for pre-service science teachers, and initiated and served as a mentor in a future faculty development program for graduate students and post-doctoral associates. She is currently affiliated with the University of Idaho.
