MTTC Chemistry (018) study plan

Apply significant-figure, scientific-notation, and dimensional-analysis rules to multi-step density, volume, and concentration calculations, writing out every conversion factor.

Distinguish accuracy from precision and classify described laboratory errors as random or systematic, explaining the effect each has on a reported mean.

Design a controlled experiment by naming the independent, dependent, and controlled variables, plus one safety precaution and one waste-disposal step.

Interpret a data table or line graph to state the trend, flag outliers, and judge whether the stated conclusion is supported by the evidence.

Trace the sequence of atomic models from Dalton through the quantum-mechanical model and name the specific experimental evidence that forced each revision.

Assign the four quantum numbers to designated electrons and write ground-state electron configurations for neutral atoms and common ions, including the Cr and Cu exceptions.

Predict and justify periodic trends in atomic radius, ionization energy, electron affinity, and electronegativity using effective nuclear charge and shielding.

Classify a bond as ionic, polar covalent, or nonpolar covalent from electronegativity differences, then predict the formula of the resulting ionic compound from charges.

Draw Lewis structures for 15 species, assigning formal charges, showing resonance where required, and identifying the octet exceptions.

Predict electron-domain and molecular geometry, including bond-angle distortions from lone pairs, for species with two through six electron domains.

Determine the hybridization and the sigma/pi bonding framework of each atom in a given structure and explain how that framework constrains rotation.

Rank a set of substances by boiling point using the relative strength of London dispersion, dipole-dipole, and hydrogen-bonding forces.

Relate intermolecular forces to solubility, vapor pressure, surface tension, and viscosity, and predict which of two solvents will dissolve a given solute.

Convert among mass, moles, representative particles, and gas volume at standard conditions for pure substances and for mixtures of known composition.

Balance skeleton equations, including combustion and redox, and then solve limiting-reactant problems that require identifying the excess reagent and the amount left over.

Calculate theoretical yield, actual yield, and percent yield, and determine empirical and molecular formulas from percent composition or combustion analysis data.

Check every stoichiometry answer with a second method, either a mole-ratio road map or a before-change-after table, and reconcile any discrepancy.

Write complete and net ionic equations for precipitation, neutralization, and redox reactions, explicitly identifying spectator ions and balancing charge and mass.

Solve solution-stoichiometry problems involving molarity, dilution, and titration, including cases where the analyte is an impure solid sample.

Apply the ideal gas law and the combined gas law inside stoichiometric calculations for reactions run at nonstandard temperature and pressure.

Assign oxidation numbers and split a redox reaction into balanced half-reactions in both acidic and basic media.

Calculate enthalpy changes from calorimetry data, Hess's law, bond energies, and standard enthalpies of formation while keeping sign conventions and units consistent.

Determine the rate law and reaction order from initial-rate data and calculate activation energy from an Arrhenius plot or two-temperature data set.

Set up and solve ICE tables for Kc and Kp, including cases requiring the quadratic formula or the small-x approximation, and state when that approximation is valid.

Predict the direction of an equilibrium shift using Le Chatelier's principle for changes in concentration, pressure, volume, and temperature, and explain the effect on K.

Calculate pH, pOH, Ka, Kb, and buffer pH, and interpret a titration curve to locate the equivalence point and the buffer region.

Predict colligative property changes and the effect of temperature and intermolecular forces on solubility, then convert between molarity, molality, and mole fraction.

Identify functional groups, apply IUPAC naming to simple alkanes, alkenes, alcohols, and carboxylic acids, and classify reactions as substitution, addition, elimination, or condensation.

Describe the structure-function relationship of carbohydrates, lipids, proteins, and nucleic acids, and explain how enzymes lower activation energy and are affected by pH and temperature.

Complete two full-length timed practice tests under exam conditions and record both raw and scaled scores by domain.

Analyze every missed item by domain and error type to produce a ranked remediation list capped at ten items.

Re-teach the three weakest areas from a blank page, then verify each summary against notes and correct every gap found.

Rehearse the mole map, ICE setup, and Henderson-Hasselbalch equation for speed, timing each drill to confirm the target pace.