Introduction to general Chemistry 2024-25

Exam Information

  • Course Name: Introduction to General Chemistry (345.240)

  • Languages: Offered in English and German.

Exam Details

  • Format: Written exam (90 minutes)

  • Language: Available in both German and English (identical exams for both languages)

  • Exam Dates:

    • Tuesday, November 12th, 2024

    • Thursday, December 13th, 2024

    • Friday, January 10th, 2025

  • Registration: Students must register (or unregister if needed) via KUSSS.

Bonus Points

  • Total Points in Exam: 48 points

  • Bonus Points:

    • Up to 2 bonus points can be earned by asking meaningful questions during the previous lectures (winter semester 2024/25).

    • Criteria for Bonus Points:

      • 2 Points: Ask questions in at least 10 out of 14 lectures (2/3 lectures).

      • 1 Point: Ask questions in at least 5 out of 14 lectures (1/3 lectures).

      • Meaningful Questions: Must relate specifically to the current lecture topic.

  • Submission Deadline: Questions must be submitted on the same day as the current lecture.

  • Anonymity: Questions submitted are not visible to other students.

Lecture Materials

  • Use of Slides: Slides are supplementary tools and do not replace lecture attendance. Additional explanations from lectures are necessary for a complete understanding.

  • Recommended Texts:

    • T.E. Brown, H.E. Lemay et al., Chemistry, The Central Science, Pearson

    • R. Lewis, W. Evans, Chemistry, Palgrave

    • P. Atkins, L. Jones, Chemical Principles, MacMillan

Course Content Overview

  1. General Introduction and Fundamentals

  2. Atoms and Elements

  3. The Periodic Table

  4. The Chemical Bond

  5. Properties of Gases, Liquids, and Solids

  6. Redox Reactions

  7. Chemical Equilibrium and Properties of Solutions

  8. Acids and Bases

  9. Short Introduction to Coordination Chemistry

  10. Complex/Coupled Equilibria

  11. Short Introduction to Thermochemistry and Chemical Thermodynamics

Key Definitions

Chemistry Definition

  • Chemistry is the scientific discipline examining elements and compounds composed of atoms, molecules, and ions, focusing on their composition, structure, properties, behavior, and reaction changes.

Chemical Reactions

  • Chemical Process: New substances with different properties are formed (e.g., Sodium and Chlorine form Sodium Chloride).

  • Physical Process: Substances retain their identity despite changes in state (e.g., Ice melting to Water).

Classical Chemistry Sub-divisions

  • Traditional fields include:

    • Organic Chemistry: Carbon-based chemistry.

    • Inorganic Chemistry: Non-carbon based chemistry.

    • Physical Chemistry: Underlying principles of chemistry.

    • Analytical Chemistry: Qualitative and quantitative composition analysis.

    • Biochemistry: Chemistry's role in biological systems.

Conceptual Framework

Three Levels of Chemistry

  • Macroscopic Level: Observable reactions (e.g., Magnesium reacting with oxygen).

  • Microscopic Level: Atomic interactions (e.g., ionic compound formation).

  • Symbolic Level: Chemical symbols and equations.

Matter Classification

  • Matter: Anything with mass and volume (e.g., water, iron).

  • Substance: Matter with distinct properties, consistent composition (e.g., water, gold).

  • Mixtures: Consist of multiple substances retaining individual properties.

    • Homogeneous Mixture: Uniform composition (e.g., salt water).

    • Heterogeneous Mixture: Non-uniform composition (e.g., rocks).

Physical and Chemical Properties

  • Physical Properties: Observable without changing identity (e.g., color, density).

  • Chemical Properties: Describes a substance's reactions (e.g., reactivity, acidity).

Measurement Units

Unit

Definition

Symbol

SI Base Unit

Mass

Kilogram

kg

kg

Length

Meter

m

m

Time

Second

s

s

Temperature

Kelvin

K

K

Amount

Mole

mol

mol

Electric Current

Ampere

A

A

Pressure

Newton per meter squared

N/m²

-

Chemical Reactions

Reaction Basics

  • Chemical reactions involve transformation of reactants into products with conservation of mass.

  • Balanced Reactions: Must have equal numbers of each type of atom on both sides of the equation.

    • Example: 2 H₂ + O₂ → 2 H₂O

Summary of Key Concepts and Principles

  • This outline includes significant terms, definitions, and laws relevant to general chemistry, setting a foundation for understanding future chemistry subjects.