Accelerated Chemistry 1 LECTURE TOPICS

I. Measurements of Matter

        A. SI Units – conversions in mass, volume, length, temperature, time

        B. Significant Figures - accuracy, precision, determination of, add/subtract, multiplication, division

        C. Equations - density, temperature scales

II. Atoms and Atomic Theory

        A. Element Names

        B. Basic Atomic Components - proton, neutron, electron, isotopes, mass#, atomic#, ionic charge; Rutherford, Thompson,
            Chadwick, Millikan

        C. Periodic Table - history, organization, Mendeleev, Moseley, diatomic elements, liquid elements, Family metals/non-metals,
            metalloids, representative, transition, inner-transition, Family names: alkali, alkaline earth, halogen, noble gas, noble metals

III. Chemical Compounds

        A. Nomenclature - ionic, covalent, binary & oxyacids, polyatomic ions, common names

IV. Introduction to Reactions and Balancing

        A. General Types of Reactions - Composition, Decomposition, Single and Double Displacement

        B. Specific examples - Neutralization, Combustion, Metals with acids, Redox, Precipitation, Born- Haber, Thermite, Acid/Base                 Synthesis

V. Stoichiometry

        A. Avogadro’s #, mole, Molar Mass

        B. Derivation of Empirical and Molecular Formulas

        C. Stoichiometry - mass A ® mole A ® mole B ® mass B

VI. Electronic Structure

        A. Spectrum, Wavelength, Frequency, Energy; c = ul ; E = hu = hc/l

        B. Basic Quantum Theory: emission spectra, photoelectric effect, Rydberg, Bohr, Schrodinger, Pauli Exclusion Principle, Heisenberg

        C. e- configuration; Aufbau Principle, 1/2 filled, ions

        D. Orbital diagram; Hund’s Rule, para/diamagnetic

VII. Periodic Table (trends)

        A. Zeff - periodic trends

        B. Size - periodic trends atomic radii, ionic radii

        C. Ionization - periodic trends, progressive ionizations, anomalies

        D. Electron Affinity - periodic trends, anomalies

        E. Electronegativity - periodic trends, ionic vs. covalent

VIII. Chemical Bonding

        A. Bonding - H2 model, orbital overlap, s , p , ionic, covalent, polar covalent

        B. Lewis Dot - atoms, ions, molecules - octet, non-octet, expanded octets, multiple bonds

        C. Geometry - VSEPR: AX, AX2, AX3, AX2E, AX4, AX3E, AX2E2, AX5, AX6, AX4E2, names of these geometries

        D. Polarity - molecular polar/non-polar

IX. Gases

        A. Behavior - Pressure, Kinetic Molecular Theory, speed, collision frequency, non ideal conditions

        B. Simple Gas Laws - Boyle, Charles, Gay-Lussac, Combined

        C. Ideal Gas Law; PV = nRT, FW = dRT/P

        D. Dalton’s Law of Partial Pressures - water vapor corrections

        E. Graham’s Law of Effusion - concept only

        F. Press/Temp and non-ideal conditions

        G. Volume Stoichiometry

X. Liquids, Solids, and Intermolecular Forces

        A. Intermolecular forces of attraction - induced dipole, dipole, H-bonding, ion

        B. Bonding in Solids - network covalent, ionic, metallic, molecular, amorphous

        C. Phase diagrams - solid, liq., gas, phase boundaries, triple pt., boiling and melting points, changing press & temp

XI. Solutions and their Physical Properties

        A. Types - g/g, g/l, g/s, l/l, l/s, s/s

        B. Expressions of concentration - molarity, molality, % w/w

        C. Properties of Solutions - Colligative properties: FP depression

XII. Thermochemistry

        A. Specific Heat; q = spH x m x D T

        B. Calorimetry; q = Cp x D T; -(heat lost) =  heat gained

        C. Phase changes; q = D H x mole

        D. Enthalpy

        E. Thermodynamic table; D Hf of elements, standard temperature, pressure, concentration, D Hrxn

        F. Hess’s Law, state function
 
XIII. Kinetics

        A. Grapical, slopes

        B. Order, Overall Order, Rate constant units, ratio method

        C. Integrated Rate Law - derivation of first order

        D. 1/2 Life - derivation of

        E. Factors affecting reaction rate: temperature, surface area, Catalysis

XIV. Equilibria

        A. Basic concepts

        B. Keq vs. Reaction Quotient

        C. Le Chatalier’s Principle

        D. Species table

XV. Acid/Base Equilibria

        A. Kw, Kw = [H+][OH- ] = 1.0 x 10-14; pH, pOH, pH = - log[H+], 14.00 = pH + pOH

        B. Theories - Arrhenius, Bronsted-Lowry, conjugate acids/bases

        C. Ka, Kb, [Ka][Kb] = Kw, pKa + pKb = 14.00, pH’s of weak acids and bases, approx. solution

        D. pH of salts; Buffers - preparation of, calculation of pH, Henderson-Hasselbach equation

XVI. Solubility

        A. Solubility Rules based on identity of anion

        B. Ksp & common ion effect

XVII. Spontaneous Change: Entropy & Gibb’s Free Energy

        A. Entropy: Disorder/Order, Spontaneity

        B. Temperature effects and signs of D H & D S (spontaneity: high temp/low temp/any temp/no temp, D G = D H - T(DS)

OPTIONAL TOPICS:

XVIII. Electrochemistry

        A. Basic Concepts - Redox

        B. 1/2 reactions - EMF’s, spontaneity,Galvanic (Voltaic), Electrolytic

        C. Nernst, Ecell = Eo - 0.0591/n [ln Q]

XIX. Nuclear chemistry

        A. Radioactivity, particles

        B. Naturally occuring radioactive isotopes

        C. Nuclear reactions and artifically induced radioactivity; Nuclear Stability, Rate of Decay, fission versus fusion

        D. Effects of radiation on matter; Application of radioisotopes

XX. Organic Chemistry

        A. Nomenclature of simple organic compounds: alkanes (C1-C8), ethene, acetylene, alcohols, ethers, esters, carboxylic acids,
            amines, aromatic, sugars

        B. Fundamental physical properties - MP,BP, water solubility

        C. Polymers - polyethylene, polyesters, nylon, polycarbonate, PVC, PS