Ionic Equations (for reactions in aqueous solution)
Strong and weak acids and bases
Solubility Rules
Metathesis reactions
    precipitation reactions (from solubility rules)
    neutralization reactions (formation of a weak electrolyte or a non-electrolyte)
    oxidation-reduction ("Redox") reactions (from Activity Series)
Driving force of a reaction
Oxidation
Reduction
Oxidizing Agent
Reducing Agent
Principle of Titration (determination of an unknown concentration)

Force and Work
Energy - Potential and kinetic
Energy units - joule and calorie
System and Surroundings
First Law of Thermodynamics (aka Law of Conservation of Energy)
Internal Energy of a System, E
E = q + w
Exothermic (q_system <0) and Endothermic (q_system > 0) Processes
E is a State Function, and is an Extensive property of the system
Enthalpy, H
H = q_P
H is a State Function, and is an Extensive property of the system
Enthalpies of Reaction
Calorimetry, calorimeter
Heat Capacity (specific heat of a substance, molar heat capacity of a substance, heat capacity of a calorimeter)
"Coffee cup" (constant pressure) calorimetry
Hess's Law (adding and subtracting equations; adding and subtracting DH's)
Standard enthalpy of Formation - definition and use
Standard States
Determination of DH's using Hess's Law
DH_reaction = Sum(DH_f's of products) - Sum(DH_f's of reactants)

Electromagnetic radiation - wavelength, frequency, amplitude
c = nl
Types of em radiation (from gamma rays to radio waves)
Quantum theory
Planck's constant, h
E = hn
Photoelectric effect and its explanation - photons
Atomic line spectra
    hydrogen spectrum - Balmer series
Bohr model for H atom
    quantized electron orbits
    ground and excited states
    quantum numbers, n
    Rydberg constant
    explanation of atomic spectrum of H
Waves as particles, particles as waves (de Broglie)
    l = h/mv
Uncertainty Principle (Heisenberg)
    position-momentum or frequency (energy)-time

Questions on the following topics, which were first presented in the lecture on wednesday, October 21, will count for no more (and maybe less) than 10% of the exam. This material will also be covered in the third exam.

wave mechanics/quantum mechanics
wave functions
orbitals, electron density distributions
other quantum numbers (l, m)
possible values of l and m
"meanings" of n, l, and m
s (l=0 and p (l=1) orbitals (names & shapes)
d (l=2) and f (l=3) orbitals (names only)

The following topics were not covered in wednesday's lecture and will appear in the third exam only.

relative energies of orbitals in many-electron atoms
effective nuclear charge and screening
Electron spin (quantum number s)
Pauli exclusion principle
Electron configurations and the Periodic Table