AP Chemistry-MCQs and Free response -Exam Style Practice question and Answer

Multiple Choice Questions

MCQs

  • Time: 90 minutes 
  • 60 multiple – choice questions (core)
  • No marks deducted from incorrect answers
  • A four-function, scientific, or graphing calculator is allowed 
  • 50% weight

Free-Response Questions

  • Time: 105 minutes 
  • 4 Questions
  • No marks deducted from incorrect answers
  • A four-function, scientific, or graphing calculator is allowed 
  • 50% weight

Free-Response Questions(FRQs)

MCQs

  • Time: 90 minutes 
  • 60 multiple – choice questions (core)
  • No marks deducted from incorrect answers
  • A four-function, scientific, or graphing calculator is allowed 
  • 50% weight

Free-Response Questions

  • Time: 105 minutes 
  • 4 Questions
  • No marks deducted from incorrect answers
  • A four-function, scientific, or graphing calculator is allowed 
  • 50% weight

Unit 1: Atomic Structure and Properties

  • 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

Unit 2: Molecular and Ionic Compound Structure and Properties

  • 2.1 Types of Chemical Bonds
  • 2.2 Intramolecular 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

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 Reaction
  • 4.3 Representation 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: Kinematics

  • 5.1 Reaction Rate
  • 5.2 Introduction to Rate Law
  • 5.3 Concentration Change Over Time
  • 5.4 Elementary Reactions
  • 5.5 Collision Model
  • 5.6 Reaction Energy Profile
  • 5.7 Introduction to Reaction Mechanisms
  • 5.8 Reaction Mechanism and Rate Law
  • 5.9 Steady State Approximation
  • 5.10 Multisteps Reaction Energy profile
  • 5.11 Catalyst

Unit 6: Thermodynamics

  • 6.1 Endothermic 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
  • 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 Calculating Equilibrium 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-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

Unit 9: Applications of Thermodynamics

  • 9.1 Introduction to Entropy
  • 9.2 Absolute Entropy and Entropy Change
  • 9.3 Gibbs Free Energy 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

Course Content

The AP Chemistry Exam assesses student understanding of the science practices and learning objectives outlined in the course framework. The exam is 3 hours and 15 minutes long and includes 60 multiple-choice questions and 7 free-response questions. Starting with the 2022–23 school year (spring 2023 exam), a scientific or graphing calculator is recommended for use on both sections of the exam. Students are provided with the periodic table and a formula sheet that lists specific and relevant formulas for use on the exam

Units Exam Weighting
Unit 1: Atomic Structure and Properties 7–9%
Unit 2: Molecular and Ionic Compound Structure and Properties 7–9%
Unit 3: Intermolecular Forces and Properties 18–22%
Unit 4: Chemical Reactions 7–9%
Unit 5: Kinetics 7–9%
Unit 6: Thermodynamics 7–9%
Unit 7: Equilibrium 7–9%
Unit 8: Acids and Bases 11–15%
Unit 9: Applications of Thermodynamics 7–9%