| I. Structure of Matter (20%) |
A. Atomic theory and atomic structure
1.Atomic masses; determination by chemical and physical means .Atomic number and mass number; isotopes
2. Electron energy levels: atomic spectra, quantum numbers, atomic orbitals
3. Periodic relationships including, for example, atomic radii, ionization energies, electron affinities, oxidation states
B. Chemical bonding :
1. Binding forces :a. Types: ionic, covalent, metallic, hydrogen bonding, van der Waals (including London dispersion forces)
2. Molecular models :a. Lewis structures and VSEPR : Geometry of molecules and ions, structural isomerism of simple organic molecules and coordination complexes
b. Valence bond: hybridization of orbitals, resonance, sigma and pi bonds
c. Nuclear chemistry: nuclear equations, half-lives, and radioactivity; chemical applications |
| Ii. States of Matter (20%) |
A. Gases :
1. Laws of ideal gases , Equation of state for an ideal gas ,. Partial pressures
2. Kinetic molecular theory :Interpretation of ideal gas laws on the basis of this theory
Avogadro's hypothesis and the mole concept ,Dependence of kinetic energy of molecules on temperature, Deviations from ideal gas laws
B. Liquids and solids
1. Liquids and solids from the kinetic-molecular viewpoint
2. Phase diagrams of one-component systems, Changes of state, including critical points and triple points
3. Structure of solids; lattice energies
C. Solutions
1. Liquids and solids from the kinetic-molecular viewpoint
2. Methods of expressing concentration (use of normalities is not tested)
3. Raoult's law and colligative properties (nonvolatile solutes); osmosis , Nonideal behavior (qualitative aspects) |
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| III. Reactions (35-40%) |
A. Reaction types
1. Acid-base reactions; concepts of Arrhenius, Brønsted-Lowry, and Lewis; coordination complexes; amphoterism
2. Precipitation reactions
3. Oxidation-reduction reactions:a. Oxidation number , The role of the electron in oxidation-reduction
4. Electrochemistry: electrolytic and galvanic cells; Faraday's laws; standard half-cell potentials; Nernst equation; prediction of the direction of redox reactions
B. Stoichiometry
1. Balancing of equations, including those for redox reactions,Ionic and molecular species present in chemical systems: net ionic equations .
2. Mass and volume relations with emphasis on the mole concept, including empirical formulas and limiting reactants
C. Equilibrium
1. Concept of dynamic equilibrium, physical and chemical; Le Chatelier's principle; equilibrium constants
2. Quantitative treatment:a. Equilibrium constants for gaseous reactions: K p , K
3. Equilibrium constants for reactions in solution :(1) Constants for acids and bases; pK; pH ,(2) Solubility product constants and their application to precipitation and the dissolution of slightly soluble compounds ,(3) Common ion effect; buffers; hydrolysis
D. Kinetics
1. Concept of rate of reaction ,. Use of experimental data and graphical analysis to determine reactant order, rate constants, and reaction rate laws
2. Effect of temperature change on rates,Energy of activation; the role of catalysts
3. The relationship between the rate-determining step and a mechanism
E. Thermodynamics
1. First law: State functions ,change in enthalpy; heat of formation; heat of reaction; Hess's law; heats of vaporization and fusion; calorimetry
2. Second law: entropy; free energy of formation; free energy of reaction; dependence of change in free energy on enthalpy and entropy changes
3. Relationship of change in free energy to equilibrium constants and electrode Potentials |
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| IV. Descriptive Chemistry (10-15%) |
1. Chemical reactivity and products of chemical reactions
2. Relationships in the periodic table: horizontal, vertical, and diagonal with examples from alkali metals, alkaline earth metals, halogens, and the first series of transition elements
3. Introduction to organic chemistry: hydrocarbons and functional groups (structure, nomenclature, chemical properties)
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| IV. Descriptive Chemistry (10-15%) |
making observations of chemical reactions and substances
recording data
calculating and interpreting results based on the quantitative data obtained
communicating effectively the results of experimental work
Chemical Calculations
1. Percentage composition
2. Empirical and molecular formulas from experimental data
3. Molar masses from gas density, freezing-point, and boiling-point measurements
4. Gas laws, including the ideal gas law, Dalton's law, and Graham's law
5. Stoichiometric relations using the concept of the mole; titration calculations
6. Mole fractions; molar and molal solutions
7. Faraday's laws of electrolysis
8. Equilibrium constants and their applications, including their use for simultaneous equilibria
9. Standard electrode potentials and their use; Nernst equation
10. Thermodynamic and thermochemical calculations
11. Kinetics calculations
Attention should be given to significant figures, precision of measured values, and the use of logarithmic and exponential relationships. |
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