Chemistry

General Chemistry 1

Matter and its properties
1. the particulate nature of matter
2. states of matter
a. the macroscopic
b. microscopic view
3. Physical and chemical properties
4. Extensive and intensive properties
5. Ways of classifying matter
a. pure substances and mixtures
b. elements and compounds
c. homogeneous and heterogeneous mixtures
6. Methods of separating mixtures into their
component substances

Measurements
1. Accuracy and precision
2. Significant figures in calculations
3. Density measurement 

Atoms, Molecules, and Ions
1. Dalton’s atomic theory
2. Basic laws of matter
3. Atomic structure
4. Subatomic particles (protons, electrons, neutrons)
5. Molecules and Ions
6. Chemical Formulas
7. Naming Compounds 

Stoichiometry
1. Atomic mass
2. Avogadro’s number
3. The mole concept
4. Percent composition and chemical formulas
5. Chemical reactions and chemical equations
6. Types of chemical reactions in aqueous solutions
7. Mass relationships in chemical reactions 

Electronic Structure of Atoms
1. Quantum mechanical description of the atom
2. Schrodinger’s model of the hydrogen atom and wave functions
3. Main energy levels, sublevels and orbitals
4. Quantum numbers
5. Electron Configuration
a. Aufbau Principle
b. Pauli Exclusion Principle
c. Hund’s Rule
d. Diamagnetism and Para magnetism
e. Orbital diagrams 

Electronic Structure and Periodicity
1. The Electron Configuration and the Periodic Table
2. Periodic Variation in Atomic Properties
a. Atomic Radius and effective nuclear charge; the shielding effect in many electron atoms
b. Ionic radius
c. Ionization energy
d. Electron affinity 

Chemical Bonding Ionic Bonds
1. The stability of noble gases
2. Forming ions
3. Ionic bonding
4. Ionic compounds
5. Formulas
6. Structure
7. Properties 

Covalent Bonds
1. Formation of covalent bonds
2. Formulas of molecular compounds
3. Lewis structure of molecules
4. Molecules of elements
5. Molecules of compounds
6. Structure and properties of molecular compounds
7. Strength of covalent bonds
8. Electronegativity and bond polarity
9. Geometry of molecules
10. Polarity of compounds 

Organic compounds
1. The carbon atom
2. Bonding patterns in hydrocarbons
3. Properties and reactivities of common functional
groups
4. Polymers
5. Biomolecules 

General Chemistry 2

Intermolecular Forces and Liquids and Solids
1. Kinetic molecular model of liquids and solids
2. Intermolecular Forces
3. Dipole-dipole forces
4. Ion-dipole forces
5. Dispersion forces
6. Hydrogen bonds
7. Properties of liquids and IMF
8. Surface Tension
9. Viscosity
10.Vapor pressure, boiling point
11. Molar heat of vaporization
12. Structure and Properties of Water
13. Types and properties of solids
14. Crystalline and amorphous solids
15. Types of Crystals – ionic, covalent, molecular,
metallic
16. Phase Changes - phase diagrams of water and
carbon dioxide 

Physical Properties of Solutions
1. Types of Solutions
2. Energy of solution formation
3. Concentration Units and comparison of
concentration units
a. percent by mass, by volume
b. mole fraction
c. molality
d. molarity
e. percent by volume, percent by mass, ppm
4. Solution stoichiometry
5. Factors affecting Solubility
6. Colligative Properties of Nonelectrolyte and
electrolyte solutions 

Thermochemistry
1. Energy Changes in Chemical Reactions: exothermic
and endothermic processes
2. First Law of Thermodynamics
3. Enthalpy of a Chemical Reaction - thermochemical "
equations
4. Calorimetry
5. Standard Enthalpy of Formation and Reaction Hess’ Law 

Chemical Kinetics
1. The Rate of a Reaction
2. Factors that influence reaction rate
3. The Rate Law and its components
4. Collision theory
5. Catalysis 

Chemical Thermodynamics
1. Spontaneous processes
2. Entropy
3. The Second Law of Thermodynamics
4. Gibbs Free Energy and Chemical Equilibrium 

Chemical Equilibrium
1. The equilibrium condition
2. Writing the reaction quotient/equilibrium constant expression
3. Predicting the direction of a reaction
4. Significance of the equilibrium constant
5. Le Chatelier’s Principle 

Acid-Base Equilibria and Salt Equilibria
1. Bronsted acids and bases
2. The acid-base properties of water
3. pH- a measure of acidity
4. Strength of acids and bases
5. Weak acids/weak bases and ionization constants
6. Relationship between the ionization constants of
acids and their conjugate bases
7. The Common Ion Effect
8. Buffer solutions
9. Solubility equilibria 

Electrochemistry
1. Redox reactions
2. Galvanic cells
3. Standard reduction potentials
4. Spontaneity of redox reactions
5. Batteries
6. Corrosion
7. Electrolysis