Honors Chemistry Final Exam 2011 Study Guide
General Concepts
atoms, molecules, ions, moles
chemical formulas, writing chemical formulas
percent error (as we calculated in lab)
density units and calculations
properties of metals and nonmetals
physical and chemical changes
density of a gas at STP (Avogadro’s hypothesis)
percent composition calculations
empirical and molecular formula calculations
oxidation state (valence numbers)
States of Matter
Heating curve - phase changes
Graham’s law of Effusion
sublimation (dry ice)
vapor pressure
intermolecular forces (effect of boiling point and freezing point)
combined gas law
ideal gas law
heat of fusion and vaporization
Atomic Structure, Bonding and Periodic Properties
electron configurations
nuclear fission and fusion
Dalton, Rutherford, Thompson, Bohr
quantum numbers
mass number and atomic number
average atomic mass (from atomic mass of isotopes)
electron energy for transitioning from higher energy level to ground state (i.e. n=3 to n=1)
electronegativity, ionization energy, atomic radius (periodic trends)
Londondispersion forces (as related to molecular size and melting point within a family)
molecular geometry (tetrahedral, Trigonal pyramidal, bent planar and linear shapes)
organic molecules (carboxylic acids, alcohols and the alkane series)
Equations and Stoichiometry
balancing equations
moles of gas as related to volume of a gas at STP or constant T and P
problem solving using mole-mole ratios and mass-mass quantities
calculations using molar concentrations (this appears often on the final exam) (find moles, grams, and volume)
synthesis, decomposition, double replacement, single replacement chemical reactions combustion of a hydrocarbon (can you write the chemical equation?)
Solutions, Solubility and Solution Reactions
Solubility graph
effects of temperature on solubility
saturated solutions, unsaturated solutions and supersaturated solutions
polar and nonpolar solvents
freezing point depression and boiling point elevation calculations
Acid/base theory – Arrhenius, Bronsted-Lowry
pH calculations
Electrolytes, weak and strong and nonelectrolytes
Ksp and solubility
Energy, Rates and Equilibrium
exothermic and endothermic reactions
changes in enthalpy (H) (heats of formation and Hess’s Law)
changes in entropy (S)
spontaneity and free energy (G)
effects of a catalyst on the activation energy and in the pathway of a chemical reaction
PE v reaction pathway graph for exo and endothermic reactions
Equilibrium and rate of forward and reverse reaction