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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
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

Email Ms. Sarna

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