CHEM 101

 GENERAL CHEMISTRY 101 FOR ENGINEERS
Term Offered: Fall
Text(s): Required: Chemical Principles (4th edition) Steven S. Zumdahl; Study Guide and Selected Solutions Guide are recommended. CD-ROM (Saunders Interactive, Kotz & Vining) also recommended. Supplemental handouts provided on web-page:
Instructor(s): Professor Peter Davies, Room 200 LRSM, davies@lrsm.upenn.edu, 898-86703
Prerequisite(s):  
Grading:  
Course Home Page URL: http://www.seas.upenn.edu/~chem101/
Course Description: Basic concepts and principles of chemistry and their applications in chemistry and materials science and engineering. Understanding chemical reactions through atomic and molecular structure; so that students can solve chemical problems and can understand the principles involved in their solution. The course also includes an introduction to condensed matter and provides engineers with a number of examples of the application of the chemistry of materials to current issues in nanotechnology and materials science. The course is presented for students with high school chemistry and calculus.
Course Outline: 1. Terms and Concepts, Analysis of Matter: Review. (2 lectures; Chapters 1 & 2)
Basic terms and definitions; introduction to modern view of atomic structure; atomic and nuclear size; introduction to the periodic table; naming simple compounds.

2. Stoichiometry. (2 lectures, Chapter 3)
Atomic mass, exact and relative, isotopes, mass spectroscopy; compounds, molecules, definite proportions, the mole; molar mass, atomic %; empirical and molecular formulae; chemical equations, balancing chemical equations; stoichiometric calculations; limiting reactants

3. Types of Chemical Reactions (3 lectures, Chapter 4)
Solution chemistry, types of solutions, composition of solutions; Precipitation reactions; acid-base reactions; oxidation-reduction reactions, oxidation states, balancing, half-reaction method.

4. Gases; ideal gas laws; kinetic molecular theory (4 lectures, Chapter 5)
Pressure, units, temperature scales; Ideal gas law; Kinetic Molecular Theory of Gases; molecular velocity; Boltzmann distribution; effusion and diffusion; mean free path; real gases.

EXAM I

5. Quantum Mechanics and Atomic Theory; Periodicity. (7 lectures, Chapter 12)
Nature of Matter, quantized energy, dual nature of light; Bohr model, atomic spectrum of H; Quantum mechanics, electrons as waves, Schrodinger equation. Particle in a box; wave equation for the H atom, quantum numbers, orbital shapes and energies. Many electron atoms; Aufbau Principle, filling of the orbitals and the Periodic Table; Periodic trends in Atomic Properties, ionization energies, electron affinities, atomic size.

6. General Concepts of Chemical Bonding. (4 lectures; Chapter 13)
Bond types, properties of a chemical bond; Electronegativity, Ionic bonding, ionic size; Covalent bonding, Lewis structures, the octet rule, valence shell expansion, resonance structures, formal charge; Molecular shape and symmetry, VSEPR model.

EXAM II

7. Covalent Bonding: Orbitals. (4 lectures; Chapter 14)
Hybridization, sp3, sp2 and sp hybrids, sigma and pi bonds; Molecular Orbital Theory, simple diatomic molecules, bond order, paramagnetism of oxygen; heteronuclear diatomic molecules; multiple bonds; polyatomic molecules; conjugated pi bonds; HOMO-LUMO. Methane and benzene analogs for diamond and graphite.

8. Structure and Bonding in Solids and Liquids. (7 lectures, Chapter 16 and supplemental handouts)
Bonding and structure, the bond triangle; Inter- and intra-molecular bonding; Inter-molecular forces, London Dispersion forces, dipole-dipole interactions; hydrogen bonding; melting & boiling points; properties of liquids, surface tension, capillary forces. Solids, crystalline and amorphous; crystallinity, periodicity, unit cell, lattice parameter, space lattice types; Metallic bonding, close-packed structures, hcp and ccp packing, coordination number, density, bcc; Ionic bonding in the Solid State, lattice energy, ionic size, octahedral and tetrahedral interstices, radius ratio; NaCl, ZnS, CsCl, CaF2 structure types; Under-sized cations, dipoles in BaTiO3, ferroelectricity. Examples of "complex" inorganic structures: perovskite, high Tc superconductors, zeolites. Extended Covalent Bonding, framework structures, diamond structure, graphite. Formation of carbon nano-tubes. Conductivity of Metals, LCAO approach, crystal orbitals, band structure of metals; electronic properties of insulators and semi-conductors, simple band models.

EXAM III

9. Introduction to Organic Chemistry. (1 lecture, Chapter 22)

Main functional groups.

Assessment Tools:

1. Weekly Homework problems discussed in weekly recitation sections.
2. Three mid-term hour exams and one two-hour final exam.

 


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