UEE Chemistry study plan

Balance redox and non-redox equations from word problems, then convert moles to mass, gas volume at STP, and solution concentration without a calculator shortcut sheet.

Solve limiting-reagent problems that require identifying the excess reactant and computing percent yield, working 15 multi-step items under timed conditions.

Compute pH, pOH, and percent dissociation for weak monoprotic acids from Ka values using the small-x approximation, and state when the approximation fails.

Build a one-page decision tree for stoichiometry setups (given unit to moles, mole ratio, target unit) and test it on 10 unfamiliar problems.

Write full and condensed electron configurations for cations and anions of the first four periods, including the Cr and Cu exceptions, and derive the block and group from each.

Rank isoelectronic species by radius and explain the trend using effective nuclear charge and shielding in writing.

Draw Lewis structures for 12 species containing expanded octets, formal charges, and resonance, then assign VSEPR geometry and bond angles to each.

Predict hybridization and molecular polarity for molecules with lone pairs on the central atom, and justify each prediction in one sentence.

Apply Le Chatelier's principle to predict shifts for changes in concentration, pressure, volume, and temperature, distinguishing temperature effects on K from concentration effects.

Calculate equilibrium concentrations from initial amounts and Kc for at least 8 systems, including cases requiring the quadratic formula.

Compute enthalpy changes using Hess's law and standard enthalpies of formation, and connect them to bond-breaking and bond-making energy bookkeeping.

Interpret a simple energy profile to identify activation energy, enthalpy of reaction, and the effect of a catalyst, and state which quantities change and which do not.

Solve combined gas law problems involving changing conditions and mixtures using partial pressures and mole fractions, keeping temperature in kelvin throughout.

Derive rate expressions from concentration-time data and determine reaction order by the initial-rate method for 6 data sets.

Use the integrated first-order rate law to compute half-life and remaining concentration, and distinguish first-order from zero- and second-order behavior from a graph.

Explain how temperature and catalysts affect rate constants and activation energy using the Arrhenius relationship qualitatively, without memorizing numerical constants.

Assign oxidation states across p-block and transition-metal species, then balance at least 6 redox equations in acidic and basic media by the half-reaction method.

Compute cell potential for galvanic cells from standard reduction potentials and predict spontaneity, clearly stating the sign convention used.

Describe periodic and group trends in the s- and p-block (ionization energy, oxide character, halide reactivity) and connect each trend to a specific reaction.

Summarize characteristic reactions and colors of common transition-metal ions and explain why they form colored complexes and show variable oxidation states.

Identify functional groups from condensed structural formulas and name at least 15 compounds using IUPAC rules, including branched chains and multiple functional groups.

Predict products of substitution, addition, elimination, oxidation, and esterification reactions, and distinguish primary, secondary, and tertiary reactivity patterns.

Explain isomerism types (chain, position, functional, geometric) and draw all isomers for two given molecular formulas.

Outline safe procedures for titration, filtration, distillation, and qualitative ion tests, and state the purpose of each piece of apparatus and one common error source per technique.

Re-solve 10 previously missed problems from weeks 1, 3, and 5 without notes, then compare answers to the original attempts and record what changed.

Complete two full-length timed practice sections mixing calculation-heavy domains, pacing at roughly one minute per question.

Explain buffer action and titration curve shape at the equivalence and half-equivalence points, and calculate buffer pH from the Henderson-Hasselbalch relationship.

Diagnose recurring error patterns (unit conversion, sign errors, approximation misuse) and write a correction rule for each.

Run three full-length timed mock exams under exam conditions and score each by domain to identify the weakest two areas.

Review only the weakest domains between mocks, using the week 7 error log rather than re-reading notes.

Recite from memory the key facts most prone to forgetting: electron configuration exceptions, VSEPR shapes, solubility and strong-acid lists, standard reduction conventions, and common functional group tests.

Finalize a one-page formula and constants sheet and confirm you can reproduce it from memory before exam day.