ILTS Science: Chemistry (240) study plan

Build a one-page periodic-trend reference sheet that predicts atomic radius, ionization energy, electron affinity, and electronegativity for any main-group element, then self-quiz on 20 elements until you score 90% or better.

Draw Bohr and orbital diagrams for the first 20 elements and write the full and noble-gas electron configurations from memory, checking each against a periodic table.

Classify 25 bonds as ionic, polar covalent, or nonpolar covalent using electronegativity differences, and predict each compound's dominant intermolecular force.

Balance 20 equations of mixed types (synthesis, decomposition, combustion, single and double replacement) and identify the limiting reactant in 10 of them.

Compute molar mass, percent composition, and empirical-to-molecular formula conversions for 10 compounds without a calculator error.

Solve 15 stoichiometry problems spanning mass-mass, mass-volume at STP, and solution-molarity pathways, showing unit cancellation on every line.

Determine limiting reactant, theoretical yield, and percent yield for 8 reaction scenarios, including one where the excess reactant is given in moles.

Write complete ionic and net ionic equations for 12 precipitation and acid-base reactions, using a solubility-rules table you construct yourself.

Predict products and assign oxidation states for 10 redox reactions, then balance 5 of them by the half-reaction method in acidic solution.

Explain in writing (150-200 words) how a mole-map diagram generalizes every stoichiometry problem, and use it to solve 5 unfamiliar problems.

Calculate enthalpy change for 12 reactions using Hess's law, standard enthalpies of formation, and calorimetry data (q = mcΔT), tracking sign conventions.

Interpret and sketch potential-energy diagrams for exothermic and endothermic reactions, labeling activation energy, transition state, and ΔH.

Apply collision theory and the Arrhenius equation to explain how temperature, concentration, surface area, and catalysts change rate, and solve 6 rate-law problems from initial-rate data.

Determine reaction order and rate constant from a data table, then predict how doubling one reactant changes the rate.

Write equilibrium expressions and calculate Kc or Kp for 8 systems, then use Le Châtelier's principle to predict the shift for 10 stress scenarios.

Solve 10 equilibrium ICE-table problems, including one requiring the quadratic formula and one using the small-K approximation with a validity check.

Compute pH, pOH, [H+], and [OH-] for 15 strong and weak acid/base solutions, and verify each weak-acid answer with Ka.

Perform titration calculations for 8 scenarios, including identifying the equivalence point and selecting an appropriate indicator.

Explain the common-ion effect and buffer action, then calculate the pH of 5 buffer systems with the Henderson-Hasselbalch equation.

Distinguish Arrhenius, Brønsted-Lowry, and Lewis acid-base definitions with one original example each.

Calculate solution concentration in molarity, molality, mass percent, and mole fraction for 10 solutions, and convert between units.

Predict colligative property effects (boiling-point elevation, freezing-point depression, osmotic pressure) for 6 solutions, including one electrolyte with a van't Hoff factor.

Assign oxidation numbers, sketch and label a galvanic cell, and calculate E°cell and spontaneity (ΔG° = -nFE°cell) for 6 redox systems.

Identify functional groups and name 15 organic compounds using IUPAC rules, including 5 with stereocenters or cis/trans isomerism.

Describe the structure and function of carbohydrates, lipids, proteins, and nucleic acids, and connect one enzyme's kinetics to the rate concepts from Week 3.

Distinguish and give examples of alpha, beta, gamma, positron, and electron-capture decay, and complete 10 nuclear equations.

Solve 8 half-life problems and explain fission versus fusion with one real-world application of each.

Design a controlled experiment for a chemistry question, identifying independent, dependent, and controlled variables, a control group, and sources of error.

Evaluate a data set for accuracy and precision, calculate mean, percent error, and standard deviation, and interpret significant figures in 10 calculation chains.

Explain the scientific method, peer review, and the difference between hypothesis, theory, and law, using one chemistry example for each.

Create a lab-safety reference covering GHS hazard pictograms, SDS sections, PPE selection, and correct handling and disposal of acids, bases, and organic solvents.

Sequence the correct response to 5 lab emergencies (chemical splash, fire, spill, ingestion, glass cut) and identify the location and use of safety equipment.

Select appropriate techniques for measuring mass, volume, temperature, and pH, and explain when to use titration, filtration, distillation, or spectroscopy.

Draft a 20-minute lesson segment on one chemistry concept that includes a phenomenon hook, a model or demonstration, and a formative assessment.

Differentiate instruction for English learners and students with IEPs in a chemistry lab, listing three specific scaffolds.

Take two full-length timed practice exams under test conditions and log every missed item by domain and error type.

Re-teach your five weakest sub-topics from scratch on blank paper, then solve 5 new problems in each without notes.

Review your Week 1-7 deliverables and rewrite any sheet or summary that still contains an unresolved question.

Practice 10 constructed-response items, writing complete explanations with units, significant figures, and labeled reasoning.

Build a final one-page 'night before' sheet of constants, formulas, and trends, and confirm you can reconstruct it from memory.