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AP Chemistry
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General
Unit 1: Atomic Structure and Properties
1.1 Moles and Molar Mass
1.2 Mass Spectroscopy of Elements
1.3 Elemental Compositin of Pure Substances
1.4 Composition of Mixtures
1.5 Atomic Structure and Electron Configurations
1.6 Photoelectron Spectroscopy
1.7 Periodic Trends
1.8 Valence Electrons and Ionic Compounds
Unit 2: Molecular and Ionic Compound Structure and Properties
2.1 Types of Chemical Bonds
2.2 Intermolecular Force and Potential Energy
2.3 & 2.4 Structure of Ionic Solids & Alloys
2.5 Lewis Diagrams
2.6 Resonance and Formal Charge
2.7 VSEPR and Bond Hybridization
Unit 3: Intermolecular Forces and Properties
3.1 Intermolecular Forces
3.2 Properties of Solids
3.3 Solids, Liquids and Gases
3.4 Ideal Gas Law
3.5 Kinetic Molecular Theory
3.6 Deviation from Ideal Gas Law
3.7 Solutions and Mixtures
3.8 Representations of Solutions
3.9 Separation of Solutions and Mixtures Chromatography
3.10 Solubility
3.11 Spectroscopy and the Electromagnetic Spectrum
3.12 Photoelectric Effect
3.13 Beer-Lambert Law
Unit 4: Chemical Reactions
4.1 Introduction for 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 (Redox) Reactions
Unit 5: Kinetics
5.1 ReactionRates
5.2 Introduction to Rate Law
5.3 Concentration Changes over Time
5.4 Elementary Reactions
5.5 Collision Model
5.6 Reaction Energy Profile
5.7 Introduction to Reaction Mechanisms 1
5.8 ReactionMechanism and Rate Law
5.9 Steady-State Approximation
5.10 Multistep Reaction Energy Profile
5.11 Catalysis
Unit 6: Thermodynamics
6.1Endothermic and Exothermic 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 to Enthalpy of Reaction 4
6.7 Bond Enthalpies
6.8 Enthalpy of Formation
6.9 Hess’s Law
Unit 7: Equilibrium
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 CalculatingEquilibrium Concentrations
7.8 Representations of Equilibrium
7.9 Introduction to Le Châtelier’s Principle
7.10 Reaction Quotient and Le Châtelier’s Principle
7.11 Introduction to Solubility Equilibria
7.12 Common-Ion Effect
7.13 pH and Solubility
7.14 Free Energy of Dissolution
Unit 8: Acids and Bases
8.1 Introduction to Acids and Bases
8.2 pH and pOH of Strong Acids and Bases
8.3 Weak Acid and Base Equilibria
8.4 Acid-Base Reactions and Buffers
8.5 Acid-BaseTitrations
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
Unit 9: Applications of Thermodynamics
9.1 Introduction to Entropy
9.2 Absolute Entropy and Entropy Change
9.3 GibbsFreeEnergy and Thermodynamic Favorability
9.4 Thermodynamic and Kinetic Control
9.5 Free Energy and Equilibrium
9.6 Coupled Reactions
9.7 Galvanic (Voltaic) and Electrolytic Cells
9.8 Cell Potential and Free Energy
9.9 Cell Potential Under Nonstandard Conditions
9.10 Electrolysis and Faraday’s Law
LAB Practical
REVIEW
POST AP Test
Extras
Email Ms. Sarna
AP Chemistry
Home
About
Calendar
Resources
General
Unit 1: Atomic Structure and Properties
1.1 Moles and Molar Mass
1.2 Mass Spectroscopy of Elements
1.3 Elemental Compositin of Pure Substances
1.4 Composition of Mixtures
1.5 Atomic Structure and Electron Configurations
1.6 Photoelectron Spectroscopy
1.7 Periodic Trends
1.8 Valence Electrons and Ionic Compounds
Unit 2: Molecular and Ionic Compound Structure and Properties
2.1 Types of Chemical Bonds
2.2 Intermolecular Force and Potential Energy
2.3 & 2.4 Structure of Ionic Solids & Alloys
2.5 Lewis Diagrams
2.6 Resonance and Formal Charge
2.7 VSEPR and Bond Hybridization
Unit 3: Intermolecular Forces and Properties
3.1 Intermolecular Forces
3.2 Properties of Solids
3.3 Solids, Liquids and Gases
3.4 Ideal Gas Law
3.5 Kinetic Molecular Theory
3.6 Deviation from Ideal Gas Law
3.7 Solutions and Mixtures
3.8 Representations of Solutions
3.9 Separation of Solutions and Mixtures Chromatography
3.10 Solubility
3.11 Spectroscopy and the Electromagnetic Spectrum
3.12 Photoelectric Effect
3.13 Beer-Lambert Law
Unit 4: Chemical Reactions
4.1 Introduction for 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 (Redox) Reactions
Unit 5: Kinetics
5.1 ReactionRates
5.2 Introduction to Rate Law
5.3 Concentration Changes over Time
5.4 Elementary Reactions
5.5 Collision Model
5.6 Reaction Energy Profile
5.7 Introduction to Reaction Mechanisms 1
5.8 ReactionMechanism and Rate Law
5.9 Steady-State Approximation
5.10 Multistep Reaction Energy Profile
5.11 Catalysis
Unit 6: Thermodynamics
6.1Endothermic and Exothermic 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 to Enthalpy of Reaction 4
6.7 Bond Enthalpies
6.8 Enthalpy of Formation
6.9 Hess’s Law
Unit 7: Equilibrium
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 CalculatingEquilibrium Concentrations
7.8 Representations of Equilibrium
7.9 Introduction to Le Châtelier’s Principle
7.10 Reaction Quotient and Le Châtelier’s Principle
7.11 Introduction to Solubility Equilibria
7.12 Common-Ion Effect
7.13 pH and Solubility
7.14 Free Energy of Dissolution
Unit 8: Acids and Bases
8.1 Introduction to Acids and Bases
8.2 pH and pOH of Strong Acids and Bases
8.3 Weak Acid and Base Equilibria
8.4 Acid-Base Reactions and Buffers
8.5 Acid-BaseTitrations
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
Unit 9: Applications of Thermodynamics
9.1 Introduction to Entropy
9.2 Absolute Entropy and Entropy Change
9.3 GibbsFreeEnergy and Thermodynamic Favorability
9.4 Thermodynamic and Kinetic Control
9.5 Free Energy and Equilibrium
9.6 Coupled Reactions
9.7 Galvanic (Voltaic) and Electrolytic Cells
9.8 Cell Potential and Free Energy
9.9 Cell Potential Under Nonstandard Conditions
9.10 Electrolysis and Faraday’s Law
LAB Practical
REVIEW
POST AP Test
Extras
Email Ms. Sarna
More
Home
About
Calendar
Resources
General
Unit 1: Atomic Structure and Properties
1.1 Moles and Molar Mass
1.2 Mass Spectroscopy of Elements
1.3 Elemental Compositin of Pure Substances
1.4 Composition of Mixtures
1.5 Atomic Structure and Electron Configurations
1.6 Photoelectron Spectroscopy
1.7 Periodic Trends
1.8 Valence Electrons and Ionic Compounds
Unit 2: Molecular and Ionic Compound Structure and Properties
2.1 Types of Chemical Bonds
2.2 Intermolecular Force and Potential Energy
2.3 & 2.4 Structure of Ionic Solids & Alloys
2.5 Lewis Diagrams
2.6 Resonance and Formal Charge
2.7 VSEPR and Bond Hybridization
Unit 3: Intermolecular Forces and Properties
3.1 Intermolecular Forces
3.2 Properties of Solids
3.3 Solids, Liquids and Gases
3.4 Ideal Gas Law
3.5 Kinetic Molecular Theory
3.6 Deviation from Ideal Gas Law
3.7 Solutions and Mixtures
3.8 Representations of Solutions
3.9 Separation of Solutions and Mixtures Chromatography
3.10 Solubility
3.11 Spectroscopy and the Electromagnetic Spectrum
3.12 Photoelectric Effect
3.13 Beer-Lambert Law
Unit 4: Chemical Reactions
4.1 Introduction for 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 (Redox) Reactions
Unit 5: Kinetics
5.1 ReactionRates
5.2 Introduction to Rate Law
5.3 Concentration Changes over Time
5.4 Elementary Reactions
5.5 Collision Model
5.6 Reaction Energy Profile
5.7 Introduction to Reaction Mechanisms 1
5.8 ReactionMechanism and Rate Law
5.9 Steady-State Approximation
5.10 Multistep Reaction Energy Profile
5.11 Catalysis
Unit 6: Thermodynamics
6.1Endothermic and Exothermic 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 to Enthalpy of Reaction 4
6.7 Bond Enthalpies
6.8 Enthalpy of Formation
6.9 Hess’s Law
Unit 7: Equilibrium
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 CalculatingEquilibrium Concentrations
7.8 Representations of Equilibrium
7.9 Introduction to Le Châtelier’s Principle
7.10 Reaction Quotient and Le Châtelier’s Principle
7.11 Introduction to Solubility Equilibria
7.12 Common-Ion Effect
7.13 pH and Solubility
7.14 Free Energy of Dissolution
Unit 8: Acids and Bases
8.1 Introduction to Acids and Bases
8.2 pH and pOH of Strong Acids and Bases
8.3 Weak Acid and Base Equilibria
8.4 Acid-Base Reactions and Buffers
8.5 Acid-BaseTitrations
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
Unit 9: Applications of Thermodynamics
9.1 Introduction to Entropy
9.2 Absolute Entropy and Entropy Change
9.3 GibbsFreeEnergy and Thermodynamic Favorability
9.4 Thermodynamic and Kinetic Control
9.5 Free Energy and Equilibrium
9.6 Coupled Reactions
9.7 Galvanic (Voltaic) and Electrolytic Cells
9.8 Cell Potential and Free Energy
9.9 Cell Potential Under Nonstandard Conditions
9.10 Electrolysis and Faraday’s Law
LAB Practical
REVIEW
POST AP Test
Extras
Email Ms. Sarna
LAB Practical
TEST 4/17/2024
Study Resources
Experimental Procedures to Know
Lab Practical Notes
AP Chemistry Laboratory Review
LAB
Practical Review Due and test on
4/
17
/202
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