ORELA Chemistry (NT321) study plan

Map every topic in Subarea I (atomic structure, periodicity, bonding, molecular geometry, intermolecular forces) to a checklist and rate your confidence 1-5 on each item.

Derive electron configurations and orbital diagrams for neutral atoms and common ions through period 4, and explain anomalies such as Cr and Cu in your own words.

Predict periodic trends (atomic and ionic radius, ionization energy, electron affinity, electronegativity) and justify each prediction with effective nuclear charge and shielding.

Draw Lewis structures, assign formal charges, and identify resonance for at least 20 polyatomic ions and molecules.

Use VSEPR to assign geometry and bond angles and combine it with electronegativity to classify bond polarity and net dipole.

Classify intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding, ion-dipole) and rank boiling and melting points for given substances.

Relate molecular shape and polarity to solubility, vapor pressure, and surface tension in short written explanations.

Draw and interpret heating curves and phase diagrams, labeling triple point, critical point, and regions.

Apply gas laws (ideal, combined, Dalton partial pressures, Graham effusion) and the van der Waals equation to non-ideal cases.

Convert among concentration units (molarity, molality, mole fraction, mass percent) and explain when each is appropriate.

Balance redox equations in acidic and basic solution using half-reactions, and assign oxidation states in polyatomic ions.

Predict products and write net ionic equations for precipitation, acid-base, and gas-forming reactions.

Solve stoichiometry problems involving limiting reagents, percent yield, and solution stoichiometry with molarity.

Apply collision theory and factors affecting reaction rate, and interpret rate laws and reaction order from data.

Set up and solve equilibrium problems including ICE tables for Kc, Kp, and reaction quotient comparisons.

Calculate enthalpy changes using Hess's law, standard heats of formation, and calorimetry data.

Interpret entropy changes qualitatively and apply the second and third laws to predict spontaneity.

Compute Gibbs free energy from enthalpy and entropy at nonstandard temperatures and connect delta G to equilibrium constants.

Distinguish state functions from path functions and identify thermodynamic sign conventions in worked examples.

Sketch and interpret potential energy diagrams for exothermic and endothermic reactions with activation energy labeled.

Compare acid and base definitions (Arrhenius, Bronsted-Lowry, Lewis) and identify conjugate pairs in given reactions.

Calculate pH, pOH, and concentrations for strong and weak acids and bases, including polyprotic cases.

Describe buffer action quantitatively with the Henderson-Hasselbalch equation and predict pH shifts on adding strong acid or base.

Interpret titration curves for strong-strong, weak-strong, and polyprotic systems, identifying equivalence and half-equivalence points.

Apply Ksp to solubility and common-ion effect problems.

Balance nuclear equations for alpha, beta, positron, and gamma processes and identify transmutation products.

Distinguish fission from fusion and explain binding energy per nucleon trends.

Compute half-life problems and apply first-order kinetics to radioactive decay.

Classify organic compounds by functional group and predict simple reaction outcomes such as substitution, addition, and esterification.

Connect electrochemistry (galvanic versus electrolytic cells, cell potential, Nernst equation) to redox concepts from week 3.

Design a safe laboratory procedure for a given prompt, listing hazards, PPE, waste handling, and disposal steps.

Select appropriate glassware and instruments for measuring mass, volume, temperature, and pH, and justify precision choices.

Analyze error sources and classify them as random or systematic, then calculate percent error and propagation of uncertainty.

Interpret data tables and graphs (calibration curves, titration plots, spectra) to draw valid conclusions.

Explain proper use and limits of techniques such as titration, gravimetric analysis, distillation, and spectroscopy.

Re-rate every checklist item from week 1 and re-teach the three lowest-confidence items in each subarea.

Complete two full-length timed practice tests under exam conditions and record subarea-level accuracy for each.

Build a one-page formula and constants sheet from memory, then verify it against your notes.

Practice explaining reasoning aloud for calculation items to reduce careless errors and improve pacing.

Review the error logs from weeks 1-7 and confirm each recurring mistake has a corrective rule.