Things you are expected to know (items in italics are first-semester topics):
•
basic chemistry vocabulary/terminology (Look at the end of each chapter for Important Terms
given in bold)
•
intermolecular forces, lattice energy, phase transitions, relation of b.p. and m.p. to intermolecular
forces, phase diagrams, types of solids, unit cell calculations
•
types of solutions, solution concentrations (molarity, molality, %, mole fraction), solubility
curves, colligative properties, colloids, solubility curves for gases vs. curves for solids
•
kinetics, experimental determination of rate, determining the rate law using the initial rate
method, rate constants, elementary reactions, catalysis, reaction mechanisms, collision &
transition state theory, activation energy, concentration-time calculations, temperature and rate,
half-lives, graphical determinations of reaction order and rate constant, potential energy diagrams
•
chemical equilibrium, equilibrium constant, reaction quotient, LeChatlier’s Principle, predicting
reaction direction, calculating equilibrium concentrations, ICE tables
•
acid-base theories: Arrhenius and Bronsted-Lowry, acid-base strength and relation to molecular
structure, self-ionization of water, and pH , strong and weak acids and bases
•
acid & base ionization equlibria, polyprotic acids, salt solutions, common ion effect, buffers,
titration curves
•
solubility product constant, common ion effect, pH and solubility, precipitation calculations,
solubility rules, particularly for ions for which there are no exceptions to the rule
•
2
nd
& 3
rd
laws or thermodynamics, entropy and
∆
S, free energy and
∆
G, spontaneity, relation to
the equilibrium constant, work, state function, extensive property, enthalpy and
∆
H, Hess’s Law,
specific heat capacity
•
balancing redox reactions, voltaic and electrolytic cells, cell notation, emf, E
cell
, electrode
potentials, oxidation numbers (know your rules), oxidizing and reducing agents, strength of these
agents, applications of electrochemistry, electrolysis
•
fission, fusion, radioactivity, nuclear bombardment reactions, radioactive decay, half-lives, mass-
energy calculations, isotopes and nuclide symbols, mass numbers and atomic weights, subatomic
particles
•
chemical/physical change/properties, significant figures, SI units and prefixes
•
nomenclature – polyatomic ions and Greek prefixes, molecular compounds, ionic compounds,
acids, binary compounds, ion charge based on position in periodic table, diatomic elements
•
completing and balancing combustion and double replacement reactions, net ionic equations,
spectator ions, molecular equations, gas-producing reactions
•
basic stoichiometry – molar masses, molar ratios, limiting reactant, percent composition,
molarity, percentage yield, empirical and molecular formulas
•
gas laws: empirical, ideal, effusion, partial pressures, STP, kinetic-molecular theory, barometers
and manometers
•
energy, frequency, and wavelength, emission spectra, electron configurations, orbital diagrams,
quantum numbers (n, l, m
l
, m
s
)
•
periodic trends (atomic radii, ionization energies, electronegativities, ionic radii)
•
Lewis structures, resonance, formal charges, bond polarity, exceptions to octet rule, bond order
•
VSEPR model: hybridization, polarity of molecules, lone pairs, bonding pairs,
σ
and
π
bonds
•
g/cm
3
may be written as g·cm
-3
and
atmL
⋅
⋅
may be written as L
·
atm
·
mol
-1
·
K
-1
