Learn about the fundamental concepts of chemistry including structure and states of matter, intermolecular forces, and reactions. You’ll do hands-on lab investigations and use chemical calculations to solve problems.

• Designing experiments and procedures to test a prediction or theory

• Creating graphs, diagrams, and models that represent chemical phenomena

• Explaining how the microscopic structure of a substance determines its chemical properties

• Balancing a chemical equation

• Making a scientific claim and supporting it with evidence

College Course Equivalent

• A one-year, introductory college general chemistry course

Recommended Prerequisites

• High school courses in chemistry and Algebra II

AP Credit Awarded by UH Mānoa by AP Exam Score

You’ll learn about the composition of atoms and ways scientists measure and categorize these molecular building blocks.

Topics may include:

• Moles and molar mass

• Mass spectroscopy of elements

• Elemental composition of pure substances

• Composition of mixtures

• Atomic structure and electron configuration

• Photoelectron spectroscopy

• Periodic trends

• Valence electrons and ionic compounds

On The Exam

7%–9% of exam score

You’ll discover the range of chemical bonds and how their structure can affect the properties of the molecules created

Topics may include:

• Types of chemical bonds

• Intramolecular force and potential energy

• Structure of ionic solids

• Structure of metals and alloys

• Lewis diagrams

• Resonance and formal charge

• VSEPR and bond hybridization

On The Exam

7%–9% of exam score

You’ll explore how atoms come together to create solids, liquids, and gases, and how subatomic forces govern the properties of everything around you

Topics may include:

• Intermolecular forces

• Solids, liquids, and gases

• Kinetic molecular theory

• Solutions and mixtures

• Photoelectric effect

On The Exam

18%–22% of exam score

You’ll learn how to differentiate physical and chemical processes, and how to measure and express chemical reactions via chemical equations

Topics may include:

• Introduction for reactions

• Net ionic equations

• Representations of reactions

• Physical and chemical changes

• Stoichiometry

• Types of chemical reactions

On The Exam

7%–9% of exam score

You’ll explore various methods to observe the changes that occur during a chemical reaction and the effects of a series of reactions.

Topics may include:

• Reaction rate

• Introduction to rate law

• Elementary reactions

• Collision model

• Introduction to reaction mechanisms

• Multistep reaction energy profile

• Catalysis

On The Exam

7%–9% of exam score

You’ll learn about energy changes in chemical reactions and how a transfer of energy can change a substance’s physical qualities

Topics may include:

• Endothermic and exothermic processes

• Heat transfer and thermal equilibrium

• Heat capacity and calorimetry

• Energy of phase changes

• Introduction to enthalpy of reaction

• Enthalpy of formation

• Hess’s law

On The Exam

7%–9% of exam score

You’ll chart how chemical reactions change over time, what causes substances to reach equilibrium, and how systems react when that equilibrium is disturbed

Topics may include:

• Introduction to equilibrium

• Calculating the equilibrium constant

• Calculating equilibrium concentrations

• Introduction to Le Châtelier’s principle

• Introduction to solubility equilibria

• pH and solubility

• Free energy of dissolution

On The Exam

7%–9% of exam score

You’ll learn more about pH, the qualities and properties of acids and bases, and how they interact in chemical reactions

Topics may include:

• Introduction to acids and bases

• pH and pOH of strong acids and bases

• Acid-base reactions and buffers

• Molecular structure of acids and bases

• pH and pKa

• Properties of buffers

On The Exam

11%–15% of exam score

You’ll be introduced to the concept of “thermodynamic favorability” for reactions, meaning how likely they are to occur given energy changes and environmental factors

Topics may include:

• Introduction to entropy

• Gibbs free energy and thermodynamic favorability

• Thermodynamic and kinetic control

• Free energy and equilibrium

• Galvanic (voltaic) and electrolyte cells

• Electrolysis and Faraday’s law

On The Exam

7%–9% of exam score