A list of topics and subtopics to study for CHEM 231 final exam
The most important topics; those which are emphasized or are vital for subsequent understanding are marked *.
Exam 1 Topics
Compounds, elements, mixtures (heterogeneous & homogeneous)
Names and symbols of elements*
Unit conversions; compound units*
Density problems
Atomic structure*
Electrons, protons, neutrons
Isotopes
Average atomic weights
Classic experiments: Rutherford, Millikan, etc.
Periodic table*
Names of groups
Other divisions: metals, main groups, transition elements
Ions: names and charges
Monatomic ions from periodic table
Polyatomic ions
Names and formulas*
Ionic compounds
Simple common covalent compounds and diatomic elements
Acids
Simple organic compounds (including structures)
Exam 2 Topics
Chemical equations*
Reactant, product, phase notation
Balancing
Empirical formulas; mass percents of elements
Formula weights*
Avogadro number and molar quantities
Stoichiometry*
Relating reaction masses
Limiting reactants
Solutions; solvents and solutes
Electrolytes: ions in aqueous solution*
Reaction types*
Oxidation-reduction; acid-base
Decomposition; combination
Solution reactions*
Double displacement type: Precipitation and acid-base (hydroxides, carbonates)*
Single displacement: Oxidation of metals by metal ions or acids*
Net ionic equations; spectator ions
Other reactions: Combustion, e.g.
Solution concentrations*
Units: Percent, molarity
Makingsolutions & diluting
Solution stoichiometry
Titrations
Exam 3 Topics
1st law of Thermodynamics
Work, heat, energy, enthalpy
Energy units: J, cal, eV, kJ/mole
Heat & temperature*
Heat capacity, specific heat & molar heat capacity
Reaction enthalpies*
Hess’s Law
Heat of formation & combustion
Using tabulated thermodynamic data
Thermochemical equations & stoichiometry
Energy conversions
Bond energies
Electromagnetic spectrum*
Wavelength, frequency, photon energy
Regions of spectrum & processes
Matter waves; uncertainty principle
Energy levels and wave functions for atoms and molecules*
Photon absorption and emission; calculate wavelengths
Electron states of hydrogen: shells, subshells, orbitals & quantum numbers
Electron structure of many-electron atoms*
Electron spin and Pauli principle
Electron configurations; relation to periodic table
Exam 4 Topics
Energies of electrons in atoms
Inner shell & valence electrons
Effective nuclear charge; shielding
Periodic trends of atomic properties
Size of atoms
Ionization energy & electron affinity
Electronegativity
Metallic nature of elements
Lattice energies & Born-Haber cycles
Lewis electron dot structures*
Atoms and atomic ions
Simple molecules; counting valence electrons
Octet rule
Formal charges & oxidation numbers
Violations of octet rule
Resonance structures
Reactions
Oxidation of metals (by acid, water, other metal ions, halogens)
Metal oxides as bases
Nonmetal oxides as acids
Activities of metals
Unit 5 Topics
Predicting geometry from Lewis structures*
Electron domains
Molecular geometries
Bond angles
Dipole moments
Hybridization
Double and triple bonds
Sigma and pi bonds
Delocalized pi orbitals
Gas laws*
Boyle’s, Charles’ , Avogadro’s Laws
Ideal gas law
Stoichiometry involving gases*
Kinetic theory of gases
Assumptions of the model
Explanations of gas behavior
Emphasized throughout
Estimating numerical answers*
Language of chemistry: translating words into chemical equations*
Unit analysis*