Inorganic and Applied Chemistry

Arvostelut:
( 14 )
182 pages
Kieli:
 English
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Peter Dybdahl Hede has a M.Sc. and PhD degree in Chemical Engineering from the Technical University of Denmark and a Business Diploma (HD) in Finance from the Copenhagen Business School. Working as Customer Solutions Application Manager in a large biotech company Peters´ areas of expertise spans from

Søren Beier has a M.Sc. and PhD degree in Chemical Engineering from the Technical University of Denmark. Søren is working within enzyme recovery and formulation process development and production as Head of Production in a large biotech company. He is furthermore the owner and co

Atoms, chemical bonds and chemical compounds, chemical reaction kinetics, chemical equilibrium, acid and base theory, and electro chemistry - in an easy and nice way you will get an overview as well as an understaning of all these terms in this book. A large amount of graphics and examples will help you understand and learn. The book covers basic terms and theory corresponding to 1st year students, university level, within inorganic and applied chemistry; all in one book!

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 have knowledge about. This book can not replace existing educational textbooks about inorganic basic chemistry and general applied chemistry, but it gives a great supplement to the education. Many smaller assignments and examples including solutions are given in the book.

The book is divided into six main sections covering the introductory parts of the general chemical education at universities and chemical engineering schools. One of the aims of this book is to lighten the shift over 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 configuration
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
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 in ionic compounds
2.5 Summing up on chapter 2

3. Reactions kenetics
3.1 The chemical reaction
3.2 Rate of reaction
3.3 Rate expressions
3.4 Chemical kinetics and catalysts
3.5 Kinetics of radioactive decay
3.5.1 Half-life
3.6 Summing up on chapter 3

4. Equlibrium
4.1 Solubility equilibrium and 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
5.5.1 Buffer capacity
5.6 Titrations and pH curves
5.6.1 Titration of 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

7. Concluding remarks

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