AP-CHEM
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AP® Chemistry
AP Chemistry covers atomic structure, bonding, intermolecular forces, reaction mechanisms, and kinetics, preparing students for AP exam success and foundational college chemistry understanding and analytical problem-solving skills.
195
Minutes
67
Questions
3/5
Passing Score
$98
Exam Cost
Who Should Take This
High school juniors and seniors enrolled in AP Chemistry or equivalent introductory college chemistry courses should take this certification. They have solid grounding in periodic trends, nomenclature, and basic thermodynamics, and aim to validate their mastery for college credit or competitive academic programs.
What's Covered
1
All nine units of the AP Chemistry course framework (College Board, effective 2020-present): Unit 1 Atomic Structure and Properties
2
, Unit 2 Molecular and Ionic Compound Structure and Properties
3
, Unit 3 Intermolecular Forces and Properties
4
, Unit 4 Chemical Reactions
5
, Unit 5 Kinetics
6
, Unit 6 Thermodynamics
7
, Unit 7 Equilibrium
8
, Unit 8 Acids and Bases
9
, Unit 9 Applications of Thermodynamics
What's Included in AccelaStudy® AI
Adaptive Knowledge Graph
Practice Questions
Lesson Modules
Console Simulator Labs
Exam Tips & Strategy
20 Activity Formats
Course Outline
60 learning goals
1
Unit 1: Atomic Structure and Properties
2 topics
Atomic Models and Electron Configuration
- Describe the structure of the atom including protons, neutrons, and electrons, and use atomic number and mass number to determine the composition of isotopes.
- Write electron configurations for atoms and ions using the Aufbau principle, Hund's rule, and the Pauli exclusion principle, and relate configuration to position on the periodic table.
- Interpret photoelectron spectroscopy data to determine the electron configuration of an element and explain the relationship between peak height and the number of electrons in a subshell.
Periodic Trends
- Describe and explain periodic trends in atomic radius, ionization energy, electron affinity, and electronegativity in terms of effective nuclear charge and electron shielding.
- Analyze how electron configuration and periodic position determine the chemical properties and reactivity patterns of elements across periods and groups.
- Interpret mass spectrometry data to determine the isotopic composition and average atomic mass of an element, calculating weighted averages from relative abundance data.
2
Unit 2: Molecular and Ionic Compound Structure and Properties
2 topics
Chemical Bonding Models
- Distinguish between ionic, covalent, and metallic bonding based on the electronegativity differences and electron behavior of the atoms involved.
- Draw Lewis structures for molecules and polyatomic ions, including structures with multiple bonds and expanded octets, and assign formal charges to select the most favorable structure.
- Identify and draw resonance structures for molecules with delocalized electrons and explain how resonance affects bond length, bond energy, and molecular stability.
Molecular Geometry and Polarity
- Predict molecular geometry using VSEPR theory by determining the steric number and identifying the electron-pair and molecular geometries (linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral).
- Determine whether a molecule is polar or nonpolar by analyzing its molecular geometry and bond dipole vectors, explaining how symmetry affects the net dipole moment.
- Explain how ionic radius, lattice energy, and Coulomb's law relate to the properties and stability of ionic compounds, comparing ionic and covalent compound characteristics.
3
Unit 3: Intermolecular Forces and Properties
2 topics
Types of Intermolecular Forces
- Identify the types of intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding, ion-dipole) present between molecules based on their structure and polarity.
- Explain how the strength of intermolecular forces determines physical properties such as boiling point, melting point, vapor pressure, viscosity, and surface tension.
- Compare the physical properties of substances with different intermolecular forces and predict relative boiling points, solubilities, and vapor pressures based on molecular structure analysis.
Properties of Solids and Solutions
- Classify solids as ionic, molecular, covalent network, or metallic based on their bonding and intermolecular forces, and predict their relative melting points, hardness, and conductivity.
- Apply the principle of 'like dissolves like' to predict the solubility of substances in various solvents based on the intermolecular forces between solute and solvent molecules.
- Explain the principles behind separation techniques (chromatography, distillation, filtration) in terms of intermolecular force differences between components of a mixture.
- Construct explanations connecting molecular-level structure and intermolecular forces to macroscopic properties of materials, integrating concepts of bonding, geometry, and polarity.
4
Unit 4: Chemical Reactions
2 topics
Reaction Types and Stoichiometry
- Write and balance molecular equations, complete ionic equations, and net ionic equations for precipitation, acid-base, and oxidation-reduction reactions.
- Identify oxidation states of atoms in compounds and ions, determine which species are oxidized and reduced in a redox reaction, and identify the oxidizing and reducing agents.
- Perform stoichiometric calculations including mole-to-mole, mass-to-mass, and solution stoichiometry to determine quantities of reactants consumed or products formed.
Limiting Reagents and Yield
- Identify the limiting reagent in a reaction given the amounts of all reactants, and calculate the theoretical yield and percent yield of a product.
- Analyze experimental stoichiometry data to determine the empirical formula and molecular formula of an unknown compound from combustion analysis or gravimetric data.
5
Unit 5: Kinetics
2 topics
Reaction Rates and Rate Laws
- Define reaction rate and calculate average and instantaneous rates from concentration-time data or graphical representations.
- Determine the rate law (including rate constant and reaction order) from experimental initial rate data using the method of initial rates.
- Apply integrated rate laws for zero-order, first-order, and second-order reactions to calculate concentrations at given times and determine reaction order from graphical analysis of concentration-time data.
- Calculate the half-life of a reaction for each order and explain how half-life varies with initial concentration for zero-order, first-order, and second-order reactions.
Reaction Mechanisms and Temperature Effects
- Explain collision theory and the role of activation energy in determining reaction rates, interpreting energy diagrams for both single-step and multi-step reactions.
- Apply the Arrhenius equation to determine the activation energy from rate constant data at different temperatures and predict how temperature changes affect reaction rates.
- Evaluate proposed reaction mechanisms by verifying that elementary steps sum to the overall reaction, that the rate law derived from the rate-determining step matches experimental data, and that intermediates are accounted for.
- Explain how catalysts increase reaction rates by providing an alternative pathway with lower activation energy, distinguishing between homogeneous and heterogeneous catalysis.
6
Unit 6: Thermodynamics
1 topic
Enthalpy and Calorimetry
- Define enthalpy of reaction (delta H) and distinguish between exothermic and endothermic reactions using energy diagrams and sign conventions.
- Calculate enthalpy changes from calorimetry data using q = mc(delta T) for coffee-cup calorimetry experiments and interpret the results in terms of heat transfer between system and surroundings.
- Apply Hess's law to calculate the enthalpy of a target reaction by combining known thermochemical equations and their enthalpy values.
- Calculate enthalpy of reaction using standard enthalpies of formation and using bond enthalpies, comparing the accuracy and applicability of each approach.
7
Unit 7: Equilibrium
2 topics
Equilibrium Constants and Calculations
- Write equilibrium constant expressions (Kc and Kp) for reversible reactions and explain why pure solids and liquids are excluded from the expression.
- Calculate equilibrium concentrations using ICE tables given initial concentrations and the equilibrium constant, applying appropriate approximations when valid.
- Compare the reaction quotient Q to the equilibrium constant K to predict the direction a reaction will shift to reach equilibrium.
Le Chatelier's Principle and Solubility Equilibria
- Apply Le Chatelier's principle to predict how changes in concentration, pressure, volume, and temperature affect the position of equilibrium and the value of K.
- Write solubility product (Ksp) expressions for sparingly soluble salts, calculate molar solubility from Ksp values, and predict whether a precipitate will form using Q versus Ksp comparison.
- Explain the common ion effect and calculate how the addition of a common ion reduces the solubility of a sparingly soluble salt by shifting the dissolution equilibrium.
8
Unit 8: Acids and Bases
3 topics
Acid-Base Theory and pH
- Define acids and bases according to the Arrhenius, Bronsted-Lowry, and Lewis models and identify conjugate acid-base pairs in proton transfer reactions.
- Calculate pH, pOH, and hydrogen ion concentration for solutions of strong acids and strong bases, and explain the relationship pH + pOH = 14 at 25 degrees Celsius.
- Calculate the pH of weak acid and weak base solutions using Ka and Kb values, setting up and solving equilibrium expressions with ICE tables and appropriate approximations.
Buffers and Titrations
- Explain how buffer solutions resist changes in pH upon addition of small amounts of strong acid or base, and calculate the pH of a buffer using the Henderson-Hasselbalch equation.
- Describe the key features of titration curves for strong acid-strong base, weak acid-strong base, and strong acid-weak base titrations, identifying the equivalence point, half-equivalence point, and buffer regions.
- Calculate the pH at various points during an acid-base titration including before the titration begins, at the half-equivalence point, at the equivalence point, and beyond the equivalence point.
- Select an appropriate acid-base indicator for a titration based on its pKa relative to the pH at the equivalence point and explain the chemistry of indicator color changes.
- Design a buffer solution with a target pH by selecting an appropriate weak acid/conjugate base pair and calculating the required ratio and concentrations of components.
Polyprotic Acids and Acid-Base Properties of Salts
- Calculate the pH of polyprotic acid solutions by considering successive ionization constants and explaining why each subsequent Ka is smaller than the previous one.
- Predict whether a salt solution is acidic, basic, or neutral by analyzing the acid-base properties of the cation and anion and their relative Ka and Kb values.
9
Unit 9: Applications of Thermodynamics
2 topics
Entropy and Gibbs Free Energy
- Define entropy as a measure of the dispersal of matter and energy and predict the sign of the entropy change for physical and chemical processes based on changes in state, temperature, number of moles of gas, and mixing.
- Calculate the standard Gibbs free energy change using delta G = delta H minus T times delta S and determine whether a process is thermodynamically favorable under given conditions.
- Analyze the four combinations of enthalpy and entropy signs to predict temperature dependence of spontaneity and determine the crossover temperature where delta G changes sign.
- Explain the relationship between Gibbs free energy and the equilibrium constant using delta G = -RT ln(K) and predict how changes in temperature affect K and the position of equilibrium.
Electrochemistry
- Describe the components and operation of galvanic (voltaic) cells including anode, cathode, salt bridge, and external circuit, and calculate cell potential from standard reduction potentials.
- Describe the components and operation of electrolytic cells, explain the differences between galvanic and electrolytic cells, and apply Faraday's laws to calculate quantities in electrolysis.
- Apply the Nernst equation to calculate non-standard cell potentials and explain the relationship between cell potential, free energy, and the equilibrium constant.
- Construct integrated explanations connecting thermodynamic favorability, equilibrium position, and electrochemical cell behavior by synthesizing delta G, K, and E-cell relationships across chemical systems.
Scope
Included Topics
- All nine units of the AP Chemistry course framework (College Board, effective 2020-present): 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%).
- Atomic structure: atomic models, electron configurations using Aufbau principle, Hund's rule, and Pauli exclusion principle, periodic trends (atomic radius, ionization energy, electron affinity, electronegativity), photoelectron spectroscopy, mass spectrometry, and the relationship between electronic structure and chemical properties.
- Molecular and ionic compounds: Lewis structures, VSEPR theory and molecular geometry, bond polarity, formal charge, resonance structures, ionic versus covalent bonding, lattice energy concepts, and metallic bonding.
- Intermolecular forces: London dispersion forces, dipole-dipole interactions, hydrogen bonding, ion-dipole forces, and their effects on physical properties including boiling point, melting point, vapor pressure, viscosity, and surface tension. Chromatography, distillation, and separation techniques. Properties of solids (ionic, molecular, covalent network, metallic).
- Chemical reactions: net ionic equations, oxidation-reduction reactions, types of chemical reactions (precipitation, acid-base, redox), stoichiometry, limiting reagents, percent yield, and spectroscopy and analytical methods.
- Kinetics: reaction rates, rate laws, integrated rate laws (zero, first, second order), half-life, reaction mechanisms and rate-determining steps, collision theory, activation energy, and the Arrhenius equation.
- Thermodynamics: enthalpy of reaction, calorimetry, Hess's law, bond enthalpies, enthalpy of formation, and energy diagrams for endothermic and exothermic reactions.
- Equilibrium: equilibrium constants (Kc and Kp), reaction quotient Q, Le Chatelier's principle, ICE tables, solubility equilibria (Ksp), and the common ion effect.
- Acids and bases: Arrhenius, Bronsted-Lowry, and Lewis definitions, pH and pOH calculations, strong and weak acid/base equilibria (Ka and Kb), buffer solutions, Henderson-Hasselbalch equation, acid-base titrations, titration curves, and polyprotic acids.
- Applications of thermodynamics: entropy, Gibbs free energy, the relationship between delta G, delta H, and delta S, thermodynamic favorability, coupling reactions, electrochemistry (galvanic and electrolytic cells, cell potentials, Nernst equation), and the relationship between free energy and equilibrium constants.
- Exam-aligned laboratory skills including data collection, error analysis, graphical interpretation, and mathematical reasoning as tested in AP Chemistry free-response and multiple-choice questions.
Not Covered
- Organic chemistry reaction mechanisms, synthesis strategies, and spectroscopic identification of organic compounds beyond basic functional group recognition.
- Quantum mechanical wave functions, orbital theory beyond electron configuration, and advanced computational chemistry methods.
- Biochemistry, polymer chemistry, and materials science beyond the introductory scope of the AP Chemistry framework.
- Nuclear chemistry and radioactive decay beyond basic conceptual understanding.
- Industrial chemistry processes and chemical engineering applications beyond exam relevance.
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