Inorganic Chemistry Summary 2024
University of Groningen
Lecturers: Dr. J. Klein and Prof. Dr. E. Otten
,Preface
This summary is based on lecture notes, slides and the book Inorganic Chemistry by Mark
Weller, Tina Overton, Jonathan Rourke & Fraser Armstrong (7th edition). The order of the
chapters is based on the order of the lectures given.
,Table of Content
Chapter 1: Atomic Structure 4
Chapter 2: Molecular structure and bonding 9
Chapter 4: Structure of solids 22
Chapter 5: Lewis Acids and Bases 28
Chapter 3: Molecular symmetry 35
Chapter 7: Coordination compounds 45
Chapter 20: d-metal complexes: electronic structure and properties 51
, Chapter 1: Atomic Structure
Ch1. Atomic Structure
● Quantum numbers and the atomic orbitals that are described by these quantum numbers, with
their (relative) energy.
● Explanation of the trends in the Periodic Table (ionisation energy, atomic/ionic radius,
electronegativity) based on electron configurations and penetration/shielding.
Figure 1: properties elements periodic table
Electron behaves like a particle and like waves.
Schrödinger equation: 𝐻 Ψ = 𝐸Ψ
2 2
𝐸Ψ =− ћ/2𝑚𝑒 𝑑 Ψ/𝑑𝑥 + 𝑉(𝑥) Ψ
V: Potential energy (PE), me: mass electron ћ = ℎ/2π
> Solution only exists for certain values of E.
→ quantization of energies that possess certain discrete
energies in an atom.
University of Groningen
Lecturers: Dr. J. Klein and Prof. Dr. E. Otten
,Preface
This summary is based on lecture notes, slides and the book Inorganic Chemistry by Mark
Weller, Tina Overton, Jonathan Rourke & Fraser Armstrong (7th edition). The order of the
chapters is based on the order of the lectures given.
,Table of Content
Chapter 1: Atomic Structure 4
Chapter 2: Molecular structure and bonding 9
Chapter 4: Structure of solids 22
Chapter 5: Lewis Acids and Bases 28
Chapter 3: Molecular symmetry 35
Chapter 7: Coordination compounds 45
Chapter 20: d-metal complexes: electronic structure and properties 51
, Chapter 1: Atomic Structure
Ch1. Atomic Structure
● Quantum numbers and the atomic orbitals that are described by these quantum numbers, with
their (relative) energy.
● Explanation of the trends in the Periodic Table (ionisation energy, atomic/ionic radius,
electronegativity) based on electron configurations and penetration/shielding.
Figure 1: properties elements periodic table
Electron behaves like a particle and like waves.
Schrödinger equation: 𝐻 Ψ = 𝐸Ψ
2 2
𝐸Ψ =− ћ/2𝑚𝑒 𝑑 Ψ/𝑑𝑥 + 𝑉(𝑥) Ψ
V: Potential energy (PE), me: mass electron ћ = ℎ/2π
> Solution only exists for certain values of E.
→ quantization of energies that possess certain discrete
energies in an atom.
