FTCE Chemistry 6-12 study plan

Classify matter as pure substance, homogeneous mixture, or heterogeneous mixture and justify each classification with a particle-level description

Distinguish physical from chemical changes and write evidence-based justifications for ten given scenarios

Balance twenty skeletal equations, including combustion and redox, and label each as synthesis, decomposition, single replacement, double replacement, or combustion

Convert among moles, mass, particles, and gas volume at STP for twelve mixed problems

Name and write formulas for ionic and covalent compounds, including transition metals requiring Roman numerals and common polyatomic ions

Solve limiting reactant problems in which the excess reactant is identified and the leftover mass is calculated

Compute theoretical yield, actual yield, and percent yield for three multi-step reactions

Perform stoichiometric calculations involving solutions using molarity and dilution

Interpret and construct particle diagrams that represent conservation of mass before and after reaction

Explain the difference between empirical and molecular formulas and derive each from percent composition data

Draw Lewis structures for twenty species, applying formal charge and choosing the lowest-energy resonance form

Predict molecular geometry and bond angles from VSEPR for molecules with two through six electron domains, including lone-pair distortions

Determine hybridization and sigma/pi bonding for a set of molecules containing single, double, and triple bonds

Rank substances by lattice energy and by melting point using Coulomb's law reasoning about charge and ionic radius

Classify intermolecular forces in given substances and predict relative boiling points from them

Distinguish the three chemical bond types by electronegativity difference and predict bond polarity from periodic trends

Apply periodic trends in atomic radius, ionization energy, electron affinity, and electronegativity to explain anomalies such as the group 2 to 13 ionization energy drop

Design a controlled experiment that tests one variable affecting reaction rate, specifying independent, dependent, and controlled variables

Identify sources of random and systematic error in a described measurement and propose a specific correction

Apply significant figure and uncertainty rules when reporting calculated results

Apply the first law of thermodynamics to calculate internal energy change from heat and work for at least eight scenarios

Perform calorimetry calculations, including heat loss to a calorimeter and determination of specific heat or enthalpy of reaction

Interpret heating curves and phase diagrams to identify melting, boiling, and sublimation conditions and to calculate heat across phase changes

Distinguish endothermic from exothermic processes using enthalpy sign, potential energy diagrams, and bond energy accounting

Use Hess's law and standard enthalpies of formation to calculate reaction enthalpy

Predict the effect of changes in concentration, pressure, volume, and temperature on equilibrium position using Le Chatelier's principle

Write equilibrium constant expressions and calculate K or an equilibrium concentration from initial conditions

Solve acid-base problems involving strong and weak acids, pH, pOH, and Ka or Kb

Analyze titration curves to locate equivalence point and buffer region and select an appropriate indicator

Explain how a buffer resists pH change using conjugate acid-base reasoning

Explain how electrochemical cells convert between chemical and electrical energy and assign oxidation and reduction half-reactions

Compare galvanic and electrolytic cells and predict spontaneous direction from standard reduction potentials

Apply kinetics concepts, including rate laws, order, activation energy, and collision theory, to interpret given data

Evaluate the validity of a scientific claim by identifying the evidence, reasoning, and assumptions behind it

Interpret graphs of concentration, rate, and energy versus reaction coordinate and connect each feature to underlying theory

Take two full-length timed practice tests under exam conditions and record domain-by-domain accuracy

Diagnose the three weakest subskills from practice test data and re-teach each using worked examples

Reconstruct from memory the key equation sheet, including gas laws, stoichiometry, thermodynamics, equilibrium, and electrochemistry relationships

Explain aloud, in teacher-style language, three commonly misconceived concepts such as bond breaking being exothermic or equilibrium meaning equal concentrations

Build a final review sheet limited to one page per domain