Basic Chemical Concepts and Tables

Steven L. Hoenig

• Publisher: CRC Press
• Year: 2019
• Print ISBN: 9780367230135
• eBook ISBN: 9781000721737
• Edition: 1
• Topic: Scienze fisiche
• Subtopic: Chimica analitica

Written as a quick reference to the many different concepts and ideas encountered in chemistry, Basic Chemical Concepts and Tables presents important subjects in a concise format that makes it a practical resource for any reader.

The author covers multiple subjects including general chemistry, inorganic chemistry, organic chemistry, and spectral analysis. Separate chapters offer physical constants and unit measurements commonly encountered and mathematical concepts needed when reviewing or working with basic chemistry concepts.

Other features include:

• 
  
  

• Tables that are useful as for the interpretation of ultra-violet (UV), infra-red (IR), nuclear magnetic resonance (NMR) and mass spectroscopy (MS) spectra.

• 
  
  

• Physical constants and unit measurements that are commonly encountered throughout the application of chemistry.

• 
  
  

• Sections devoted to the concept of isomers and polymer structures.

Graduate and undergraduate chemistry students, professionals, or instructors looking to refresh their understanding of a chemistry topic will find this ready reference indispensable in their daily work.

Written as a quick reference to the many different concepts and ideas encountered in chemistry, Basic Chemical Concepts and Tables presents important subjects in a concise format that makes it a practical resource for any reader.

The author covers multiple subjects including general chemistry, inorganic chemistry, organic chemistry, and spectral analysis. Separate chapters offer physical constants and unit measurements commonly encountered and mathematical concepts needed when reviewing or working with basic chemistry concepts.

Other features include:

• 
  
  

• Tables that are useful as for the interpretation of ultra-violet (UV), infra-red (IR), nuclear magnetic resonance (NMR) and mass spectroscopy (MS) spectra.

• 
  
  

• Physical constants and unit measurements that are commonly encountered throughout the application of chemistry.

• 
  
  

• Sections devoted to the concept of isomers and polymer structures.

Graduate and undergraduate chemistry students, professionals, or instructors looking to refresh their understanding of a chemistry topic will find this ready reference indispensable in their daily work.

General Chemistry1

1.1 Matter

1.2 Atomic Structure and the Periodic Table

1.3 Chemical Bonding

1.4 Gases

1.5 Solutions

1.6 Acids and Bases

1.7 Thermodynamics

1.8 Equilibria

1.9 Kinetics

1.10 Electrochemistry

1.1 MATTER

1.1.1 CLASSES OF MATTER

Matter can exist in different types of forms and can be classified into several distinct categories. Matter can exist either as:

A pure substance is a sample of matter that cannot be separated into simpler components without chemical change. Physical changes can alter the state of matter but not the chemical identity of a pure substance. Pure substances have fixed, characteristic elemental compositions and properties. There are two types of pure substances, elements and compounds. Elements are not chemically decomposable into other elements, and their properties do not vary. Compounds are elements combined chemically in law of definite proportions and their properties do not vary.

A compound is a material formed from elements chemically combined in definite proportions by mass. For example, water is formed from chemically bound hydrogen and oxygen. Any pure water sample contains 2g of hydrogen for every 16g of oxygen.

An element is a substance composed of atoms with identical atomic number. The older definition of element (an element is a pure substance that can’t be decomposed chemically) was made obsolete by the discovery of isotopes.

When one substance is mixed with another, two types of mixtures are formed – homogeneous and heterogeneous mixtures.

A homogeneous mixture is a sample of matter consisting of more than one pure substance with properties that do not vary within the sample. The components are uniformly mixed and have one phase. Can also be called a solution.

A heterogeneous mixture is a sample of matter consisting of more than one pure substance and more than one phase. Blood, protoplasm, milk, chocolate, smoke, and chicken soup are examples of heterogeneous mixtures. The components are not uniformly mixed and can have more than one phase.

1.1.2 PROPERTIES OF MATTER

Extensive property: A property that changes when the amount of matter in a sample changes. Examples are mass, volume, length, and charge.

Intensive property: A property that does not change when the amount of sample changes. Examples are density, pressure, temperature, color.

Chemical property: Measurement of a chemical property involves a chemical change. For example, determining the flammability of gasoline involves burning it, producing carbon dioxide and water.

Physical property: Measurement of a physical property may change the arrangement but not the structure of the molecules of a material. Examples of physical properties are density, color, boiling point, volume, temperature, and ma...

Table of contents

• Cover
• Half Title
• Title Page
• Copyright Page
• Dedication
• Table of Contents
• Preface
• Acknowledgments
• Chapter 1. General Chemistry
• Chapter 2. Inorganic Chemistry
• Chapter 3. Organic Chemistry
• Chapter 4. Nomenclature
• Chapter 5. Qualitative Chemical Analysis
• Chapter 6. Organic Spectroscopy Tables
• Chapter 7. Units and Measurements
• Chapter 8. Mathematical Concepts
• Appendix A
• Appendix B
• Bibliography
• Index