General Chemistry I

Korea University

Course Description

  • Course Name

    General Chemistry I

  • Host University

    Korea University

  • Location

    Seoul, South Korea

  • Area of Study

    Chemistry

  • Language Level

    Taught In English

  • Course Level Recommendations

    Lower

    ISA offers course level recommendations in an effort to facilitate the determination of course levels by credential evaluators.We advice each institution to have their own credentials evaluator make the final decision regrading course levels.

    Hours & Credits

  • Credits

    3
  • Recommended U.S. Semester Credits
    3
  • Recommended U.S. Quarter Units
    4
  • Overview

    Topics:

    Topics and the tentative order they will be covered are listed below. Note that these are units, and they may not exactly correspond to the order of chapters in the Petrucci textbook.

    UNIT 1 – Atoms and Molecules

    The properties and classification of matter Atoms and atomic theory, Elements and the periodic table Laws: Conservation of Mass, Constant Composition, and Multiple Proportions Counting and weighing atoms and molecules, The mole

    UNIT 2 – Chemical Compounds and Chemical Formulas

    Types of compounds and formulas, Finding the molecular formula: composition, Oxidation states and oxidation numbers Inorganic compounds: names and structures; ions

    UNIT 3 – Chemical Reactions

    Chemical equations and stoichiometric calculations, Reactions in solution: the limiting reagent and yield of reaction.

    UNIT 4 – Reactions in Aqueous Solutions

    Precipitation reactions Acid-base reactions, Oxidation-reduction reactions, Stoichiometry of reactions in solution: titration.

    UNIT 5 – Gases

    The basics: P, V, T, and n Ideal gases: R, molar volume, density The gas laws: Boyleʼs, Charlesʼ, and Avogadroʼs Reactions in the gas phase, Gas mixtures: law of combining volumes; Daltonʼs law of partial pressures Kinetic model of gases

    UNIT 6 – Electronic Structure of Atoms

    The models of the atom Electromagnetic radiation and atomic spectra, The Bohr atom Wave/particle duality and quantum mechanics, Quantum numbers and electron orbitals, The hydrogen atom: n, l, and m Multielectron atoms; electron spin, The Aufbau principle, the Pauli exclusion principle, and Hundʼs rule Electronic configurations and the periodic table

    UNIT 7 – Periodic Properties of Substances

    The periods of the periodic table, Metals and nonmetals; electronic configurations and chemical properties, Sizes of atoms and ions Ionization energy and electron affinity, Consequences in chemical reactivity

    UNIT 8 – The Fundamentals of Chemical Bonding

    The Lewis model: depiction of Lewis structures, Electronegativity and covalent bonding: single, multiple, polar and nonpolar covalent bonds, Formal charge and oxidation number, The octet rule and its exceptions, Resonance Molecular shape and VSEPR

    UNIT 9 – Chemical Bonding: The Quantum Model

    The valence bond model: sigma and pi bonds, Atomic orbital hybridization, Molecular orbital theory; delocalization of electrons

    UNIT 10 – Energy and the First Law of Thermodynamics

    State functions: internal energy, Heat and work, Heats of reaction at constant volume and at constant pressure; enthalpy

    UNIT 11 – Liquids and Solids

    The three physical states and their interrelationships; phase diagrams, Changes of state, Intermolecular forces, Structures of solids

    UNIT 12 – Solutions and Their Properties

    Types of solutions, Specifying concentrations, Solubility of gases, Colligative properties: vapor pressure, bp, fp, and osmotic pressure

    UNIT 13 – Chemical Equilibrium: The Extent of Chemical Reactions

    The equilibrium state, The equilibrium constant; what does Keq actually tell us? Predicting the direction of net change Le Chatelierʼs principle Catalysts.

Course Disclaimer

Courses and course hours of instruction are subject to change.