AAC-Vorlesung-1.pdf

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Periodic Table of Elements

  • Noble gases:
      - He (Helium) - Atomic number: 2, Atomic weight: 4.0026
      - Ne (Neon) - Atomic number: 10, Atomic weight: 20.1797
      - Ar (Argon) - Atomic number: 18, Atomic weight: 39.948
      - Kr (Krypton) - Atomic number: 36, Atomic weight: 83.80
      - Xe (Xenon) - Atomic number: 54, Atomic weight: 131.293
      - Rn (Radon) - Atomic number: 86, Atomic weight: [222]

Schedule and Organizational Matters

Dates for Chemists and Biochemists

  • Final exam:
      - Date: Mon, 03.08.2026
      - Time: 9:00 - 12:00

  • Resit exam:
      - Date: Mon, 14.09.2026
      - Time: 9:00 - 12:00

Dates for Geoscientists

  • Final exam:
      - Date: Mon, 03.08.2026
      - Time: 9:00 - 12:00

  • Resit exam:
      - Date: Tue, 08.09.2026
      - Time: 9:00 - 12:00

Introduction to General and Inorganic Chemistry

Target Group

  • Intended for all listeners of natural science subjects such as Chemistry, Biochemistry, Physics, Geosciences, and Teaching Candidates.

Behavioral Rules

  • Be Proactive!: If arriving late, be as quiet as possible and take a seat at the edge.

  • Be Punctual!: Timeliness is expected.

  • Respect Others: No loud conversations with peers or instructors, no phone calls or internet surfing, and no loud music.

Lecture Levels

  • Lecture (V): Transmits comprehensive knowledge and theoretical foundations in chemistry.

  • Exercises (Ü): Typically accompanying lectures focused on applying theoretical knowledge to specific chemical examples to deepen understanding.

  • Practical Work (P): Aims at practical skill development, including experiment planning and execution with discussions on results.

Mathematical Knowledge Required

  • Basic operations in algebra.

  • Foundations of differential and integral calculus.

  • Basic knowledge of logarithmic calculations.

Contents Overview

  1. Introduction:
       - 1.1 Organizational Matters
       - 1.2 Literature
       - 1.3 Definition of Chemistry
       - 1.4 Importance of Chemistry to Humanity and Society
       - 1.5 History of Chemistry

  2. Elements, Compounds, Mixtures:
       - 2.1 Elements
       - 2.2 Pure Substances and Homogeneous/Heterogeneous Mixtures
          - 2.2.1 Definitions
          - 2.2.2 Separation Techniques

  3. Chemical Laws and Basic Concepts:
       - 3.1 Law of Conservation of Mass
       - 3.2 Law of Definite Proportions
       - 3.3 Law of Multiple Proportions
       - 3.4 Dalton's Atomic Hypothesis (1805)
       - 3.5 Atomic Mass, Molecular Mass, and the Concept of Mole

  4. Atomic Structure:
       - 4.1 Elementary Particles
       - 4.2 Mass Defect
       - 4.3 Nuclear Reactions

  5. Atomic Models:
       - 5.1 Hydrogen Spectra
       - 5.2 Bohr's Model of the Hydrogen Atom
       - 5.3 Wave Characteristics of Electrons
       - 5.4 Atomic Orbitals and Quantum Numbers
       - 5.5 Multi-Electron Atoms

  6. Periodic Properties of Elements:
       - 6.1 Moseley's Law
       - 6.2 Periodic Table of Elements (PSE)
       - 6.3 Trends in the Periodic Table of Elements

  7. Group 18: Noble Gases:
       - 7.1 Elements and Major Compounds
       - 7.2 Gas Laws

  8. Hydrogen:
       - 8.1 Occurrence and Isotopes
       - 8.2 Production
       - 8.3 Applications
       - 8.4 Physical and Chemical Properties
       - 8.5 Chemical Bonding
          - 8.5.1 Atomic Bonds and Lewis Structures
          - 8.5.2 Valence Bond Theory (VB Theory)
          - 8.5.3 Molecular Orbital Theory (MO Theory)

  9. Group 17, Halogens:
       - 9.1 Properties, Occurrence, Production, and Use
       - 9.2 Hydrogen Halides (HX)
       - 9.3 Reaction Kinetics
          - 9.3.1 Rate Laws
          - 9.3.2 Catalysis
       - 9.4 Chemical Equilibrium
       - 9.5 Electronegativity and Oxidation States
       - 9.6 Thermodynamics of Chemical Reactions
          - 9.6.1 Hess's Law
          - 9.6.2 Standard Enthalpy of Formation
          - 9.6.3 Gibbs-Helmholtz Equation
       - 9.7 Halogen Oxygen Compounds
       - 9.8 Interhalogen Compounds
       - 9.9 VSEPR Model

  10. Group 16, Chalcogens:
       - 10.1 Oxygen - Ozone
       - 10.2 Water
          - 10.2.1 Hydrogen Bonds
          - 10.2.2 Solutions, Water as a Solvent
          - 10.2.3 Solubility, Solubility Product
       - 10.3 Acids and Bases
          - 10.3.1 Acid-Base Theories
          - 10.3.2 pH-Level, Water's Ion Product
          - 10.3.3 Acidity Strength, pK_s Value
          - 10.3.4 Calculation of pH of Acids and Bases in Water
          - 10.3.5 Degree of Protonation α of Weak Acids (HA) - Ostwald's Dilution Law
          - 10.3.6 Proton Transfer in Salts
          - 10.3.7 Buffer Solutions
          - 10.3.8 Indicators, Acid-Base Titrations
       - 10.4 Hydrogen Peroxide (H₂O₂)
       - 10.5 Sulfur
       - 10.6 Hydrogen Sulfide, Metal Sulfides, Polysulfides
       - 10.7 Sulfur Oxides, SO₂, SO₃
       - 10.8 Oxoacids of Sulfur and their Salts
       - 10.9 Selenium and Tellurium
       - 10.10 Oxides of Se and Te

  11. Group 15, Pnictogens:
       - 11.1 Nitrogen
       - 11.2 NH Compounds
       - 11.3 Nitrogen Oxides
       - 11.4 Nitrous Acid; Nitric Acid
       - 11.5 Other N-Compounds
       - 11.6 Phosphorus
       - 11.7 Phosphine
       - 11.8 Phosphorus Oxides
       - 11.9 Oxygen Acids of Phosphorus
       - 11.10 Halogen Compounds of Phosphorus
       - 11.11 Arsenic, Antimony, and Bismuth

  12. Group 14, Carbon Group, Tetragens:
       - 12.1 Carbon
       - 12.2 Carbides
       - 12.3 Carbon Oxides
       - 12.4 Carbonic Acid, H₂CO₃, and Carbonates
       - 12.5 Nitrogen Compounds of Carbon
       - 12.6 Silicon
       - 12.7 Silicides, Silanes, and Silicon Halides
       - 12.8 Oxygen Compounds of Silicon
       - 12.9 Germanium, Tin, Lead

  13. Group 13, Earth Metals:
       - 13.1 Boron
       - 13.2 Diborane
       - 13.3 Oxygen Compounds of Boron
       - 13.4 Boron Halides and Nitrogen Compounds of Boron
       - 13.5 Metals
          - 13.5.1 Position in the Periodic Table and Properties
          - 13.5.2 Metal Structure
          - 13.5.3 Metal Bonding
       - 13.6 Salts
          - 13.6.1 Ionic Lattice
          - 13.6.2 A-B Structures
          - 13.6.3 A-B₂ Structures
       - 13.7 Aluminum, Gallium, Indium, Thallium

  14. Group 2, Alkaline Earth Metals:
       - 14.1 Occurrence, Production, and Use
       - 14.2 Selected Compounds

  15. Group 1, Alkali Metals:
       - 15.1 Occurrence, Properties, Production, and Use
       - 15.2 Selected Compounds

  16. Electrochemistry:
       - 16.1 Electrolysis and Galvanic Elements
       - 16.2 Standard Potential
       - 16.3 Nernst Equation
       - 16.4 Decomposition Voltage, Overvoltage
       - 16.5 Accumulators
       - 16.6 Local Elements/Corrosion

Conclusion

  • The lecture aims to provide a comprehensive foundation in General and Inorganic Chemistry for students. Topics covered stretch across historical perspectives, essential chemical concepts, and practical applications. Importantly, a strong grasp of these subjects will aid students in various scientific disciplines, affirming the interdisciplinary nature of chemistry as it intersects with numerous fields.