Introductory Chemistry: An Atoms First Approach https://www.mheducation.com/cover-images/Jpeg_400-high/1260148912.jpeg 2 9781260148916 From its very origin, Introductory Chemistry: An Atoms First Approach by Julia Burdge and Michelle Driessen 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 emphasized 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.
Introductory Chemistry: An Atoms First Approach

Introductory Chemistry: An Atoms First Approach

2nd Edition
By Julia Burdge and Michelle Driessen
ISBN10: 1260148912
ISBN13: 9781260148916
Copyright: 2020
Product Details +
09781260148916

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Program Details

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

About the Author

Julia Burdge

Dr. Julia Burdge did most of her undergraduate work at Iowa State University, completing her bachelor’s degree and Master’s 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 Master’s 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.

Michelle Driessen

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