Download ISC 107 General Chemistry 2017

General Chemistry I (ISC107)
International Summer Campus 2017, Korea University
Instructor: Prof. Neil E. Schore
Email: [email protected]
Lecture texts:
Any textbook that covers the normal curriculum in General Chemistry is perfectly acceptable.
However, Iʼll refer mainly to
R.H. Petrucci, F.G. Herring. J.D. Madura, C. Bissonnette, “General Chemistry,” 10th edition,
Pearson, 2011.
Note: procure your textbook before you arrive. The Korea U. bookstore will not stock them.
Grading: Three 100-point examinations will cover the material approximately as shown below.
Exams:
Exam 1 – Monday, July 10 Units 1–5
Exam 2 – Monday, July 24 Units 6–10
Exam 3 – Wednesday, August 2 Units 11–13
Total
100 pts
100 pts
100 pts
300 pts
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
UNIT 2 – Chemical Compounds and Chemical Formulas
UNIT 3 – Chemical Reactions
UNIT 4 – Reactions in Aqueous Solutions
UNIT 5 – Gases
UNIT 6 – Electronic Structure of Atoms
UNIT 7 – Periodic Properties of Substances
UNIT 8 – The Fundamentals of Chemical Bonding
UNIT 9 – Chemical Bonding: The Quantum Model
UNIT 10 – Energy and the First Law of Thermodynamics
UNIT 11 – Liquids and Solids
UNIT 12 – Solutions and Their Properties
UNIT 13 – Chemical Equilibrium: The Extent of Chemical Reactions
Detailed list of Topics
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