Ms. Villanueva
CP-1 Quantitative Chemistry Course Syllabus
Textbook: Chemistry, Expanded 4th Edition, Wilbraham, Staley & Matta, Addison-Wesley, 1997
Grade Determination: Grade: Tests (Tests and Labs/Lab Quizzes) = 65 %; Classwork (Homework, Activities, Regular
Quizzes and Participation) = 35 %;
First Semester
Chapter Topic
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I: Matter
1. Lab Safety
2. Matter Tree
3. Properties of Matter
4. States of Matter
5. Physical & Chemical Changes
6. Mixtures & Types of Mixtures
7. Elements & Compounds
8. Chemical Symbols
9. Chemical Reactions
10. Conservation of Mass/Matter (Mass vs. Weight)
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II. Scientific Measurement
1. The Scientific Method
2. Accuracy & Precision
3. Metric Units & Prefixes
4. Measuring Density & Specific Gravity
5. Measuring temperature and Conversions
6. Evaluating Measurements (% error)
7. Scientific Notation & Using a Scientific Calculator
8. Significant Figures in Measurements and Calculations
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III: Atomic Structure
1. Greek Philosophy (Democritus vs. Aristotle)
2. Atomic Models
3. Dalton (Dalton’s Theory)
4. Thomson (Plum Pudding Model)
5. Rutherford
6. Bohr (Bohr Model)
7. Quantum Mechanical
8. Sub-Atomic Particles
9. Lewis Dot Diagrams
10. Isotopes (Average Atomic Mass)
11. Light and Atomic Spectra
12. Wave Motion & Quantum Mechanics
13. Electron Configuration
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IV. Periodicity
1. Historical Development of the Periodic Table
a. Mendeleev
b. Mosely
2. The Modern Periodic Table
3. Periodic Trends
a. Atomic Size
b. Ionization
c. Ionic Size
d. Electronegativity
4. Revisiting Electron Configuration
Labs & Activities
Reactions & Observations
Mass & Volume
Isotopes of Pn
Relative Masses of Atoms
Periodic Table Cut & Paste
Flame Test
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CP-1 Quantitative Chemistry Course Syllabus
V. Chemical Names & Formulas
1. Atoms & Ions
2. Ionic Compounds
3. Laws of Definite & Multiple Proportions
4. Ionic Charges
5. Polyatomic Ions
6. Common & Systematic Names
7. Writing & Naming Formulas
VI. Types of Chemical Reactions
1. Writing Chemical Equations
2. Balancing Chemical Equations
3. Types of Reactions
a. Combination (Synthesis – Composition)
b. Decomposition
c. Single Replacement (Redox)
d. Double Replacement
e. Combustion
4. Predicting Products
5. Ionic Equations
VII. Problem Solving
1. Word Problems
2. Problem Solving Techniques
3. Conversion Factors
4. Dimensional Analysis
VIII. Chemical Quantities
1. Measuring Matter
2. The Mole (Avogadro’s Number)
3.Gram Formula Mass (Molar Mass)
4. Mass to Mole (Mole Map)
5. Volume to Mole
6. Particle to Mole
7. Percent Composition
8. Calculating Empirical & Molecular Formulas
IX. Stoichiometry
1.Interpreting Chemical Equations
2. Mole to Mole Calculations
3. Mass to Mass Calculations
4. Other Stoichiometric Calculations
5. Limiting Reagents
6. Percent Yield
Chemical Names & Formulas
Generation of Hydrogen &
Oxygen
Types of Reactions
Mole to Mole
How Much is Too Much?
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CP-1 Quantitative Chemistry Course Syllabus
Second Semester
Chapter Topic
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X. States of Matter
1. Kinetic Theory & Nature of Gases
2. Kinetic Energy & Kelvin Scale
3. Comparing Solids, Liquids & Gases
a. Liquids
b. Evaporation
c. Boiling Point
d. Solids
e. Sublimation & Deposition
4. Phase Diagrams
5. Plasma
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XI. Thermochemistry
1. Energy
2. Heat Capacity & Specific Heat
3. Exothermic & Endothermic Processes
4. Calorimetry
5. Thermochemical Equations
6. Heat & Changes of State
XII. Nuclear Chemistry
1. Nuclear Particles & Isotopes
2. Nuclear Equations
3. Fusion vs. Fission
4. Radioactive Decay & Half-Life
5. Radioisotope Uses
XIII. Behavior of Gases
1. Boyles Law
2. Charles’ Law
3. Gay-Lussac’s Law
4. Combined Gas Law
5. Ideal Gas Law
6. Dalton’s Law of Partial Pressure
IX. Covalent Bonds
1. The Nature of Covalent Bonding
2. Determining Bond Types
a. Single Bonds
b. Double & Triple Bonds
3. Forming Structural & Lewis Dot Diagrams
3. Polar Molecules - Bonding & Symmetry
4. Exceptions to the Octet Rule
5. VSEPR Theory
6. Isomers
7. Intermolecular Forces
8. Comparing Ionic & Covalent Substances
Labs
Melting Point of a Solid
Specific Heat of a Metal
Movie: The Dirty Bomb
Boyle’s Law
Reaction of a Metal with HCl
Ionic & Covalent Bonding Lab
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CP-1 Quantitative Chemistry Course Syllabus
X. Solutions
1. Water & Aqueous Solutions
a. The Water Molecule
b. Surface Properties of Water
c. Ice
d. Aqueous Solutions
e. Solvations
f. Suspensions & Colloids
2. Solution Formation
3. Solubility & Factors Affecting Solubility
4. Molarity
5. Dilutions
6. % Solutions
7. Colligative Properties
XI. Reaction Rates & Equilibrium
1. Reaction Rates
a. The Collision Theory
b. Factors Affecting Reaction Rates
2. Reversible Reactions
a. Equilibrium
b. Factors Affecting Equilibrium
3. Spontaneous Reactions
a. Heat, Entropy & Free Energy
4. Equilibrium Constants
XII. Electrochemistry
1. The Nature of Oxidation & Reduction
2. Electron Transfer
a. Determining What is Oxidized & What is Reduced
3. Writing Half Reactions
4. Using the Reactivity Series
5. Voltaic Cells
6. Electrolytic Cells
XIII. Acids & Bases
1. Properties of Acids & Bases
2. pH
3. Names & Formulas of Acids & Bases
4. Arrhenius Acids & Bases
5. Brønsted-Lowry Acids & Bases
6. Strengths of Acids & Bases
7. Calculating Disassociation Constants
8. Molarity, [H+], [OH-], pH, and pOH Relationships
XIV. Neutralization
1. Neutralization Reactions
2. Titration
a. Determining the Concentration of an Acid by Titration
3. Writing Half Reactions
4. Using the Reactivity Series
5. Voltaic Cells
6. Electrolytic Cells
Solubility of KNO3
Concentrations of Solutions
Decomposition of the
Hypochlorite Ion
Le Chatelier
Electrochemistry (RedOx)
Acid-Base Titration
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