AP Chemistry study plan

Derive rate laws from initial-rate data by comparing trials in which one reactant concentration changes while the others are held constant, then state each reactant's order and the overall order.

Distinguish zero-, first-, and second-order kinetics by testing which integrated plot (concentration vs. time, natural log vs. time, reciprocal vs. time) is linear, and compute half-life from the appropriate expression.

Apply the Arrhenius equation to calculate activation energy from two rate-constant/temperature pairs and to predict how a temperature increase or catalyst changes the rate constant.

Write electron configurations and interpret photoelectron spectra to justify periodic trends in atomic radius, first ionization energy, and electron affinity.

Calculate enthalpy changes from calorimetry data, Hess's law cycles, and standard enthalpies of formation, explicitly tracking sign conventions and limiting heat loss assumptions.

Differentiate state functions from path functions and explain why bond-enthalpy sums give only approximate reaction enthalpies.

Draw Lewis structures, assign formal charges, and predict electron-domain and molecular geometry with VSEPR for species having up to six electron domains.

Rank boiling points of related substances from intermolecular force analysis and connect each ranking to specific structural features such as polarity, hydrogen bonding, and molecular size.

Write equilibrium constant expressions in Kc and Kp form and manipulate them for reversed, multiplied, and summed reactions.

Construct ICE tables to solve for equilibrium concentrations and percent dissociation, including cases requiring the small-x approximation and cases where it fails.

Apply Le Châtelier's principle to predict the direction of shift from changes in concentration, volume or pressure, and temperature, distinguishing changes in Q from changes in K.

Solve solubility and common-ion problems with Ksp, and use the reaction quotient compared with K to determine the direction of net change.

Identify conjugate acid-base pairs and rank acid strength using Ka and pKa values together with structural factors such as bond polarity, oxyanion electronegativity, and resonance stabilization.

Calculate pH, pOH, and all species concentrations for strong and weak acids and bases, including polyprotic systems and salt solutions.

Analyze titration curves by locating equivalence and half-equivalence points, selecting appropriate indicators, and computing pH in every region of strong-strong and weak-strong titrations.

Explain buffer behavior quantitatively with the Henderson-Hasselbalch equation and predict the pH change caused by adding a strong acid or strong base.

Predict the sign and approximate magnitude of standard entropy change from particle count and phase changes, and calculate standard free energy change from enthalpy, entropy, and temperature.

Determine spontaneity and the crossover temperature by solving the free energy equation set equal to zero.

Convert among standard free energy change, equilibrium constant, and standard cell potential using the linking equations, and check each conversion for consistent units and significant figures.

Balance redox half-reactions in acidic and basic media, compute cell potentials for galvanic cells, and identify anode, cathode, and electron flow direction.

Apply the Nernst equation to nonstandard concentrations and use Faraday stoichiometry to calculate mass or charge in electrolysis.

Classify ionic, molecular, covalent-network, and metallic solids by melting point, hardness, and conductivity, and justify each property from the underlying structure.

Interpret phase diagrams and heating curves by labeling coexistence regions and calculating the energy transferred in each segment.

Apply gas laws and colligative properties to solution problems, including vapor-pressure lowering and boiling-point elevation.

Write balanced molecular, complete ionic, and net ionic equations for precipitation, acid-base, and redox reactions in aqueous solution.

Predict products and classify reaction types, including combustion and gas-forming reactions, directly from reactant formulas.

Reconstruct a one-page formula and constants sheet from memory, then verify every entry against the official reference table and mark gaps.

Complete two timed free-response sets under exam timing, writing every answer with explicit justification and unit-bearing calculations.

Re-derive from scratch, without notes, the five relationships missed most often across the first six weeks.

Audit the accumulated error logs and reattempt every previously missed item until each is answered correctly twice in a row.

Complete one full-length timed practice exam in a single sitting under exam conditions, including the seventy-five-minute multiple-choice section and the free-response section.

Classify every miss by domain and by error type: content gap, calculation slip, misread question, or pacing.

Rebuild the three weakest sub-topics with targeted drills and retest each one under time pressure.

Rehearse pacing strategy, allocating roughly ninety seconds per multiple-choice item and splitting free-response time by point value.