Chapter in Chemical Principles

1 - Matter and Measurement

• Review of factor-label method, conversion factors between units.
   

2 - Atoms, Molecules, and Ions

• Review nuclear nomenclature, average atomic mass.
• Operation of analytical balances and calibration of pipet lab (Sienko #2).
• Review Avogadro's Number, mole concept, molarity in solutions.
• Chemical nomenclature review, including complex ions.
• Exam
• Multiple Proportions Lab (Sienko#5)

3 - Mass Relations in Chemistry

• Percent composition from formula, empirical formula from percent composition, empirical formula from combustion analysis, molecular formulas.
• Writing balanced chemical equations, mass-mass stoichiometry.
• Limiting reactants, theoretical and actual yield.
• Exam
• Stoichiometry Lab (Sienko #9)

5 - Physical Behavior of Gases

• Gas Laws (Charles', Boyle's, Combined, Ideal).
• Charles' and Boyle's Law Lab (microchemistry).
• Stoichiometry with Gases, Dalton's Law of Partial Pressure.
• Real Gas Laws, Kinetic Theory.
• Exam
• Molar volume of oxygen lab (Sienko #11).

6 - The Electronic Structure of Atoms

• Quantum Theory principles - energy, frequency and wavelength relationships, Absorption/emission spectra, Bohr atom calculations.
• de Broglie wavelengths, Wave function, electron cloud probability, electron configurations and orbital diagrams, Quantum Numbers.

7 - Chemical Bonding

• Theory of chemical bonding, periodic properties, Lewis dot structures, bond polarity, bond energies.
• Molecular bonding theories (VSEPR, bond hybridization, molecular orbitals), geometries, bond angles, molecular polarities, molecular orbital configurations.
• Exam
• Spectrophotometer Lab.

9 - Liquids and Solids

• Clausius-Clapeyron Equation, phase diagrams.
• Solid Structure types (Ionic, molecular covalent, network covalent, metallic), Intermolecular Forces (dipole, hydrogen bonding, dispersion or London forces).
• Crystal Structure Lab (Sienko #15).
• Crystal structures (simple cubic, face-centered cubic, body-centered cubic).
• Exam

10 - Solutions

• Properties of solutions, mole fraction, molality, molarity, conversion between concentration units, dilution problems.
• Effects on solubility of temperature and pressure, Henry's Law, Raoult's Law, boiling point elevation, freezing point depression, osmotic pressure.
• Molar mass determination from colligative properties.
• Molecular weight from freezing point lowering lab.
• Exam 

11 - Rate of Reaction

• Definition of chemical rates, calculation of average rates, determination of rate law form experiment.
• Integrated rate laws, half-life, determination of rate order by graphical methods.  Reaction  coordinate diagrams, catalysis, relation between rate constant and temperature, rate laws from chemical mechanisms.
• Rate law determination (microchemistry).

12 - Gaseous Chemical Equilibrium

• Definition of equilibrium, equilibrium constant expression, prediction of direction of reaction.
• Equilibrium concentration given original concentration problems.
• LeChatlier's principle
• Exam

13 - Acids and Bases

• pH, pOH, [OH], and [H+] relationships, strong and weak acids/bases.
• Reactions of salts in water.
• Reactions of acids/bases in water  (proper ionic notation), acid/base titrations.
• Acid/Base titration curves, pH at endpoint, acid/base theories.
• Exam
• Titration of antacids lab (Sienko Special Project #XI)

20 - Acid-Base/Precipitation Equilibria

• Define Ka, Kb.  Determination of Ka from pH and % dissociation.
• Determination of [H+], pH for weak acid with/without quadratic formula, polyprotic acid analysis, introduce principles of buffers (what is buffer, how does it work, how is it made).
• Additional buffer problems, weak base ionization, Kw=KaKb, acid/base indicator principles.
• Rules for multiple equilibria using Ka, Kb, and Ksp, common ion effect, determination of pH in salt solutions.
• Solubility rules, writing balanced net ionic equations, precipitation titrations, problems with additive volumes.
• Ksp expressions, equilibria with precipitates, prediction of precipitate formation.
• Aqueous solubility calculations, common ion effect.
• Exam
• Qualitative analysis labs (Sienko #46, 52)
• Lab Exam

17 - Redox: Electrochemistry

• Rules for assigning oxidation numbers, oxidizing and reducing agents, balancing redox equations.
• Redox in net ionic form, redox titrations.
• Electrolytic cells, voltaic cells, quantitative electrolysis.
• Standard cell potentials (E), strength of oxidizing and reducing agents, Nernst equation and nonstandard conditions.

16 - Thermodynamics

• Define Enthalpy, Gibb's Free Energy, Entropy, find each for reaction from tables.  Gibbs-Hemholtz equation, relationships between Gdegrees and Keq, Gdegrees and Edegrees, Edegrees and Keq.
• Exam