Essentials of Chemistry

Atoms, chemical bonds and chemical compounds, chemical reaction kinetics, chemical equilibria, acid and base theory and electrochemistry – all of this is presented in a straightforward way helping students getting an overview and solid understanding of fundamental and applied chemistry. A large number of graphical illustrations and concrete examples help learning. The compendium covers basic concepts and theory corresponding to first years of university teaching in inorganic and general chemistry; all in one compendium!

This book is written primarily to engineering students in the fields of basic chemistry, environmental chemistry, food production, chemical and biochemical engineering who in the beginning of their university studies receive education in inorganic chemistry and applied chemistry in general.

The aim of this book is to explain and clarify important terms and concepts which the students are supposed to be familiar with. The book can not replace existing educational textbooks but it gives a great supplement to the education within chemistry. Many smaller assignments and examples including solutions are given in the book.

The book is divided into six chapters covering the introductory parts of the education within chemistry at universities and chemical engineering schools. One of the aims of this book is to lighten the shift from grammar school/high school/gymnasium to the university.

We alone are responsible for any misprints or errors and we will be grateful to receive any critics and suggestions for improvement.

Preface

1. Atoms
1.1 Atomic nucleus, electrons, and orbitals
1.1.1 Components of the atom
1.1.2 Electron movement and electromagnetic radiation
1.1.3 Bohr’s atomic model
1.1.4 Photons
1.1.5 Radioactive decay
1.1.6 Wave functions and orbitals
1.1.7 Orbital confi guration
1.2 Construction of the periodic table
1.2.1 Aufbau principle
1.2.2 Electron configuration
1.2.3 Categorization of the elements
1.2.4 Periodic tendencies
1.3 Summing up on chapter 1

2. Chemical compounds
2.1 Bonds and forces
2.1.1 Bond types (intramolecular forces)
2.1.2 Intermolecular forces
2.2 Covalent bonds
2.2.1 Energy considerations
2.2.2 Molecular orbital theory
2.2.3 Lewis structure
2.2.4 VSEPR theory
2.2.5 Orbital hybridization
2.3 Metallic bonds
2.3.1 Band theory
2.3.2 Lattice structures
2.4 Ionic bonds
2.4.1 Ionic character
2.4.2 Lattice structures for ionic compounds
2.4.3 Energy calculations for ionic compounds
2.5 Summing up on chapter 2

3. Reaction kinetics
3.1 Chemical reactions
3.2 Reaction rate
3.3 Rate expressions
3.4 Kinetics and catalysts
3.5 Kinetics of radioactive decay
3.6 Summing up on chapter 3

4. Chemical equilibrium
4.1 Solubility product
4.1.1 Relative solubility
4.1.2 Ion effects on solubility
4.2 Precipitation
4.2.1 Selective precipitation
4.3 Summing up on chapter 4

5. Acids and bases
5.1 About acids and bases
5.1.1 Acid strength
5.1.2 The pH-scale
5.1.3 The autoprotolysis of water
5.2 pH calculations
5.2.1 Calculation of pH in strong acid solutions
5.2.2 Calculation of pH in weak acid solutions
5.2.3 Calculation of pH in mixtures of weak acids
5.3 Polyprotic acids
5.4 Acid properties of salts
5.4 Ion effects on pH
5.5 Buffer
5.5.1 The Buffer equation
5.5.2 Buffer capacity
5.6 Titrations and pH curves
5.6.1 Titration of a polyprotic acids
5.6.2 Colour indicators for acid/base titration
5.7 Summing up on chapter 5

6. Electrochemistry
6.1 Oxidation and reduction
6.1.1 Level of oxidation
6.1.2 Methods for balancing redox reactions
6.2 Galvanic cells
6.2.2 Cell potentials
6.3 Standard reduction potentials
6.4 Concentration dependency of cell potentials
6.5 Batteries
6.6 Corrosion
6.7 Electrolysis
6.8 Summing up on chapter 6