I. Introduction
A. Safety rules and procedures
B. Scientific Method
C. Branches and careers in chemistry
D. Scientific Notation
E. Accuracy, precision, significant figures
F. Control vs. test and other types of experimentation
II. Measurement
A. System Internationale units (SI) vs. English units
B. Metric system and prefixes
C. Dimensional analysis conversions and technique
D. Percentage error calculations
E. Density, area, and volume calculations
F. Temperature scales and conversions
III. Matter
A. Mass vs. weight
B. Hetero- vs. Homogeneous matter
C. Extensive, intensive, physical and chemical properties
D. Phases of matter and changes in phase
E. Physical vs. chemical changes in matter
F. Elemental occurrences in nature, ores, minerals
G. Laws of conservation of matter/energy
H. Compounds vs. mixtures
IV. Energy
A. Definition, work, joules F. Heat vs. Temp., cal, kcal, Cal, kinetic theory of matter
B. Kinetic vs. potential, types of each G. Activation energy, calorimetry, specific heats
C. Endothermic vs. exothermic H. Specific heat calculations
D. Forms of energy, changes in form
*E. Electrostatic forces, current, voltage, resistance, insulators, conductors
V. Gases
A. Pressure defined, various units of pressure C. Standard temperature and pressure (STP)
B. Atmospheric pressure, barometer, manometer D. Boiling, melting, viscosity, changes in water
VI. The Gas Laws
A. Boyle’s Law (PV=k), Charles’ Law (V=kT), Gay-Lussac’s Law (P=kT), combined laws, (PV=kT) with calculations
B. Dalton’s Law of partial pressures E. Mole concept, molar volume and calculations
C. Graham’s Law of Diffusion F. Kinetic theory, Ideal gases, PV=nRT
D. Avogadro’s hypothesis and number
VII. Changes in Gases, Liquids and Solids
A. Mechanism of Evaporation
B. Vapor vs. Gas, volatility, vapor pressure
*C. Liquid-vapor equilibrium and pressure at equilibrium
D. What is Boiling?
E. Liquefaction, critical temperature and pressure
*F. Heats of vaporization, condensation, fusion, and crystallization
*G. Fractional distillation, hydration, cracking and related terms
VIII. Atomic Structure, History and Theory (Part 1)
A. Democritus, Lavoisier, Proust, Dalton, etc.
B. Atomos, conservation of matter experiments, laws of definite and multiple proportions
C. Dalton’s Modern Atomic Theory (1803) and its limitations
D. Crookes, Thomson, Millikan, Rutherford, Chadwick
E. Crookes tube, anode, cathode, cathode ray tubes
F. Charge-to-mass ratio of an electron - Oil Drop experiment
G. Discovery of the nucleus - Gold Foil experiment
H. Relative charges and masses of subatomic particles
I. Isotopes, avg. atomic masses, notation, important carbon and hydrogen isotopes
J. Atomic number vs. atomic mass
K. Waves and their characteristics (amplitude, wavelength, crest, trough, frequency, velocity, etc.)
L. The Electromagnetic Spectrum
M. c = λν, E = hν (or c = λf and E = hf)
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IX. Atomic Structure, History and Theory (Part 2)
A. Four branches of mechanics
B. Planck, Einstein, de Broglie, Heisenberg, Schroedinger, Bohr, Roentgen, Becquerel, Curie, Pauli, etc.
C. Wave particle duality of nature, exclusion principle, uncertainty principle, basic quantum theory, Hund’s Rule
D. Ground state energies, excited states, standing waves, nodes, *modes of vibration, spectroscopy
E. Four quantum numbers for each electron (principal, sublevel, orbital, spin)
F. Electron configurations, valence shell electrons
*G. Kernel concept, electron clouds, quantum mechanical probabilities, time-dependent psi
H. X-rays, transmutation, radioactivity (alpha, beta, gamma radiations), fission, fusion
I. Half-life calculations, nuclear equations, *rates of nuclear decay and causes thereof
X. Chemical Bonding (Part 1)
A. Chemical bonding, reactions and valence electrons
B. Noble gases and stable octets, octet rule and exceptions
C. Ionization energies, cations, anions
D. Electron dot diagrams, Lewis notation, configurations
E. Ionic bonding, crystal lattices, *42 crystal varieties
F. Covalent bonding, coordinate covalency, resonance
G. Metallic bonding, hydrogen bonding, Van der Waals forces, London forces
XI. Chemical Bonding (Part 2)
A. Electronegativity and the border number 1.7
B. Polar vs. non-polar compounds
C. Molecules and network solids, ionic crystals, *Bragg equation, *diamagnetism and paramagnetism
D. The VSEPR model, hybrid orbitals, *pi and sigma bonds, *bond order
E. Polyatomic ions, old vs. new names for cations
*F. Bond energies, bond angles, bond geometries
XII. The Periodic Table
A. Dobreiner, Newlands, Mendeleev et al
B. Periodicity and the Periodic Law
C. Periods, groups, families, trends and characteristics within them, compare and contrast
D. Ionic radii, cations vs. anions, electron affinity, atomic sizes
E. Metals, non-metals, metalloids
XIII. Chemical Formulas
A. Empirical formulas, molecular formulas, valences of ions, multivalent ions (old vs. new names)
B. Naming of compounds, prefixes, per-, hypo-, binary, ternary compounds
*C. Coordination compounds, ligands, metallic bonds, isomerism, etc.
XIV. Chemical Equations
A. Reactants vs. products
B. Balancing a chemical equation
C. Phases in chemical equations
D. Four types of chemical reactions
XV. Stoichiometry
A. The mole - Avogadro’s number
B. Molecular formula mass, formula weights
C. Percentage composition, empiricals F. Mass-mass & mass-volume problems
D. Determining formula from percentages G. Net ionic eqns, redox reactions, activity series
E. Limiting reagents, theoretical yields, spectator ions
XVI. Solutions
A. Characteristics of solutions, solutes, solvents
B. Types of solutions
C. What affects solubility, Henry’s Law, etc.
D. Factors affecting rate of solution
E. Solubility curves
F. Unsaturated, saturated, supersaturated
G. Dilute vs. concentrated
XVII. Expressing Solution Concentrations
A. Percentage by mass
B. Mass of solute per unit volume of solution
C. Parts per million, billion, trillion
D. Molarity and molality
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XVIII. Colligative Properties of Solutions
A. Electrolytes, non-electrolytes, vapor pressure, conductivity
B. Freezing point depression, boiling point elevation, *calculations of both
XIX. Chemical Kinetics
A. Reaction rates and effective collisions
B. Hetero- vs. homogeneous reactions
C. Catalysis
*D. Reaction mechanisms, rate-controlling steps
E. Potential energy diagrams w/activation energies w/ and w/o catalysts, activation complex
XX. Enthalpy and Entropy
A. Enthalpy and heat content
*B. Heats of formation vs. stability of a compound, Hess’ Law
C. *Entropy changes (DS), thermodynamic basics
*D. Gibbs Free Energy equation, spontaneity
XXI. Chemical Equilibrium
A. Reversible reactions
B. What is equilibrium?
C. Equilibrium constant (Keq) and the mass-action expression
D. Le Chatelier’s principle and its changes, the Haber Process
XXII. Solubility Products
A. Solubility product, Ksp, and its uses
B. Prediction of precipitation
XXIII. Acids, Bases and Salts
A. Ionization vs. dissociation, weak vs. strong acids and bases
*B. Definition of acids and bases (Arrhenius, Bronsted-Lowry, Lewis)
C. Ionization constants of acids and bases, Ka and Kb
D. Properties, consumer uses, and preparations of common acids and bases
E. Four types of salts, acid-base reactions w/gas formation
F. Ionization of water, Kw, and calculations
G. Definition and calculation of pH, pH + pOH = 14
H. Buffers, amphoterism, conjugates, titrations, indicators, neutralizations, hydrolysis, normality
XXIV. Electrochemistry
A. Redox revisited, voltaic cells, activity series potentials, half-reactions
B. Batteries, *Nernst equation, EMF, corrosion, *electrical work, fuel cells
XXV. Organic Chemistry
A. Structural formulas, isomers, saturated vs. unsaturated
B. Hydrocarbon chains and names
C. Benzene rings and related ideas
D. Alkanes, alkenes, alkynes, alcohols, aldehydes, ketones, ethers, esters, and organic esters
XXVI. Possible and Suggested Labs
A. Finding the Ratio of Moles of Reactants in a Chemical Reaction
B. Identification of Alum, KAl(SO4)2 • 12H2O
C. An Activity Series
D. Thermochemistry and Hess’ Law
E. Molecular Mass of a Volatile Liquid
F. Molecular Mass by Freezing Point Depression
G. Vapor Pressure and Enthalpy of Vaporization of Water
H. Analysis of a Commercial Bleach
I. Determination of the Hardness of Water
J. Study of the Kinetics of a Reaction
K. Determination of the Solubility Product of an Ionic Compound
L. Determination of the Equilibrium Constant for the Formation of FeSCN2+
M. Determination of the Dissociation Constants of Weak Acids
N. Determination of the Equivalent Mass and pKa of an Unknown Acid
O. Equilibrium and Le Chatelier’s Principle
P. Determination and Comparison of Solubility Curves
Q. Qualitative Analysis Using Paper Chromatography
R. Determination of Percentage Copper in an Alloy
S. Determination of the Formula of Various Hydrates
T. An Exploration Into Electrochemical Half-Cells
U. Laboratory Techniques for the Identification of Unknown Cations
V. The Preparation of Esters
XXVIII. Demonstrations
I will perform fifty to seventy-five demonstrations throughout the course of the school year chosen from my collection of over 500 that will supplement the student’s comprehension of chemical principles. Most of these are either too dangerous for the students to perform in groups or are subject to limitations in the chemical stockroom. |