Chemistry AP

Atoms and the Electron

Summer + 2 wk

Scale, Proportion and Quantity

CR10. Empirical Formula of a Hydrate Lab (GI), Gravimetric Analysis of a Metal Carbonate Reaction Lab (GI).

CR5. Students represent common isotopes by graphing mass spec data based on average atomic mass. A sample element being bromine, which has two clear peaks (SP3).

• 1.1 Moles and Molar Mass 
• 1.2 Mass Spectroscopy of Elements
• 1.3 Elemental Composition of Pure Substances 
• 1.4 Composition of Mixtures 
• 1.5 Atomic Structure and Electron Configuration 
• 1.6 Photoelectron Spectroscopy 
• 1.7 Periodic Trends 
• 1.8 Valence Electrons and Ionic Compounds.

Bonding

4 wk

Structure and Properties

CR10. Chromatography Lab.

CR6. Students draw the Lewis structures of hexanes, water, and ethanol. In a written response, students have to explain the miscibility of hexanes and ethanol with water using intermolecular force (SP4). 

• 2.1 Types of Chemical Bonds
• 2.2 Intermolecular Force and Potential Energy 
• 2.3 Structure of Ionic Solids 
• 2.4 Structure of Metals and Alloys 
• 2.5 Lewis Diagrams 
• 2.6 Resonance and Formal Charge 
• 2.7 VSEPR and Bond Hybridization

Solids, Liquids, Gases

5 wk

Structure and Properties

CR10. Molar Mass of Butane Lab (GI), Solutions and Dilutions Lab, Spectrophotometer Lab (GI).

CR4. After learning about how pharmaceutical drugs are processed and made ready for the public, students develop a method to isolate and purify soluble solid product from a byproduct and the solvent. (SP2).

• 3.1 
• 3.2 
• 3.3 Solids, Liquids, and Gases
• 3.4 Ideal Gas Law
• 3.5 Kinetic Molecular Theory
• 3.6 Deviation from the Ideal Gas Law
• 3.7 Solutions and Mixtures 
• 3.8 Representation of solutions
• 3.9 Separation of Solutions and Mixtures Chromatography 
• 3.10 Solubility
• 3.13 Beer-Lambert Law

Aqueous Reactions

3 wk

Transformations

CR10. Identification of Precipitates (GI), Percent Hydrogen Peroxide Titration.

CR3. Students sketch representations of particulate matter (pure substances/mixtures) and how it changes through different types of chemical reactions. (SP1).

• 4.1 Introduction to Reactions
• 4.2 Net Ionic Equations
• 4.3 Representations of Reactions
• 4.4 Physical and Chemical Changes
• 4.5 Stoichiometry
• 4.6 Introduction to Titration
• 4.7 Types of Chemical Reactions
• 4.8 Introduction to Acid-Base Reactions
• 4.9 Oxidation-Reduction reactions

Kinetics

3 wk

Transformations and Energy

CR10. Rate Law of Fading Crystal Violet Lab

• 5.1 Reaction Rates
• 5.2 Introduction to Rate Law
• 5.3 Concentration Changes over Time
• 5.4 Elementary Reactions
• 5.6 Reaction Energy Profile
• 5.7 Introduction to Reaction Mechanisms
• 5.8 Reaction Mechanisms and Rate Law
• 5.9 Steady State Approximation
• 5.10 Multistep Reaction Energy Profile
• 5.11 Catalysis

Thermodynamics

4 wk

Energy

CR10. Calorimetry – 3 Parts, Hess’s Law, Hand Warmer Lab (GI), Heat of Formation of Magnesium Oxide.

• 6.1 Exothermic and Endothermic Processes
• 6.2 Energy Diagrams
• 6.3 Heat Transfer and Thermal Equilibrium
• 6.4 Heat Capacity and Calorimetry
• 6.5 Energy of Phase Changes
• 6.6 Introduction of Enthalpy of Reaction
• 6.7 Bond Enthalpies
• 6.8 Enthalpy of Formation
• 6.9 Hess’s Law
• 9.1 Introduction to Entropy
• 9.2 Absolute Entropy and Entropy Change
• 9.3 Gibbs Free Energy and Thermodynamic Favorability
• 9.4 Thermodynamics and Kinetic Control
• 9.5 Free Energy and Equilibrium
• 9.6 Coupled Reactions

Equilibrium

Transformations, Structure and Properties

CR10. FeSCN Equilibrium Lab.

CR8. Students will make a claim about how a given change will affect a chemical reaction at equilibrium; temperature, introduction of more starting material, removal of product, etc.  They argue how different changes will affect the  equilibrium of a system based on Le Chatelier’s principle (SP6).

• 7.1 Introduction to Equilibrium
• 7.2 Direction of Reversible Reactions
• 7.3 Reaction Quotient and Equilibrium Constant
• 7.4 Calculating the Equilibrium Constant
• 7.5 Magnitude of the Equilibrium Constant
• 7.6 Properties of the Equilibrium Constant
• 7.7 Calculating Equilibrium Concentrations
• 7.8 Representations of Equilibrium
• 7.9 Introduction to Le Chatelier's Principle
• 7.10 Reaction Quotient and Le Chatelier’s Principle
• 7.11 Introduction to Solubility Equilibrium
• 7.12 Common Ion Effect
• 7.13 pH and Solubility
• 7.14 Free Energy of Dissolution

Acids and Bases

Transformations, Structure and Properties

CR10. Strong and Weak Acid-Base Titration Lab, Buffer Lab.

CR7. Students are provided with the data from two titrations. They will be able to determine which is a strong acid and which is weak using the data. They will complete relevant calculations of strong and weak titration data (SP5).

• 8.1 Introduction to Acids and Bases
• 8.2 pH and pOH of Strong Acids and Bases
• 8.3 Weak Acid and Base Equilibrium
• 8.4 Acid-Base Reactions and Buffers
• 8.5 Acid-Base Titrations
• 8.6 Molecular Structure of Acids and Bases
• 8.7 pH and pKa
• 8.8 Properties of Buffers
• 8.9 Henderson-Hasselbalch Equation
• 8.10 Buffer Capacity

Electrolytic Cells

Transformations and Energy

CR10. Electrolysis Lab

CR9. Students read a current Chemical & Engineering News article on current battery technology. Students will then design a prototype of a galvanic cell and write an analysis of the chemical reactions that will occur in the cell. They will also discuss how their cell differs (and maybe improves upon) the research in the article. 

• 9.7 Galvanic and Electrolytic Cells
• 9.8 Cell Potential and Free Energy
• 9.9 Cell Potential Under Nonstandard Conditions
• 9.10 Electrolysis and Faraday’s Lab