12th Grade Chemistry

Students will compare and contrast early atomic models (Dalton, Thomson, Rutherford, Bohr) and their experimental evidence.

Students will explore the wave-particle duality of matter and light, and the four quantum numbers that describe electron states.

Exploration of wave particle duality and how electron configurations determine the chemical identity of elements.

Students will apply the Aufbau principle, Hund's rule, and Pauli exclusion principle to write electron configurations and draw orbital diagrams.

Analysis of how effective nuclear charge and electron shielding influence atomic radius, ionization energy, and electronegativity.

Students will investigate the energy changes associated with removing or adding electrons to atoms and their periodic trends.

Students will examine electronegativity as a measure of an atom's attraction for electrons in a bond and its relationship to metallic character.

Students will be introduced to the nucleus, isotopes, and the forces holding the nucleus together.

Students will study different types of radioactive decay (alpha, beta, gamma) and calculate half-life.

Students will investigate the processes of nuclear fission and fusion, their energy release, and applications.

Study of radioactive decay, fission, and fusion and their applications in energy and medicine.

Students will explore the formation of ionic bonds, properties of ionic compounds, and the concept of lattice energy.

Students will learn to draw Lewis structures for molecules and polyatomic ions, representing covalent bonds and lone pairs.

Students will investigate resonance structures and use formal charge to determine the most stable Lewis structure.

Using valence shell electron pair repulsion theory to predict the geometric arrangement of atoms in a molecule.

Students will explore the concept of orbital hybridization and differentiate between sigma and pi bonds.

Distinguishing between intramolecular bonds and the attractions between separate molecules.

Students will identify and compare dipole-dipole forces, hydrogen bonding, and London dispersion forces.

Examining the unique structures of metals and giant covalent networks like diamond and graphite.

Students will classify solids based on their bonding and predict their physical properties.

Bridging the gap between the microscopic world of atoms and the macroscopic world of grams.

Students will calculate molar mass and perform conversions between mass, moles, and number of particles.

Students will determine empirical and molecular formulas from percent composition or combustion analysis data.

Students will learn to balance chemical equations to satisfy the law of conservation of mass.

Using balanced equations to predict the amounts of products formed and reactants consumed.

Students will identify limiting reactants and calculate theoretical and percent yields for reactions.

Evaluating the efficiency of chemical processes in laboratory and industrial settings.

Students will define energy, heat, and work, and apply the first law of thermodynamics to chemical systems.

Measuring and calculating the heat flow in chemical systems.

Students will use Hess's Law and standard enthalpies of formation to calculate reaction enthalpies.

Students will define reaction rate and explore factors that influence it.

Investigating how molecular collisions lead to chemical change and how to manipulate reaction speed.

Students will explore multi-step reaction mechanisms and derive rate laws from experimental data.

Students will investigate the role of catalysts in lowering activation energy and speeding up reactions.

Predicting whether a reaction will occur naturally by looking at disorder and Gibbs free energy.

Students will use Gibbs free energy to predict the spontaneity of reactions under various conditions.

Understanding that chemical reactions can reach a state where forward and reverse rates are equal.

Students will write equilibrium constant expressions (Kc and Kp) and calculate their values.

Predicting how a system at equilibrium responds to external stresses like pressure or temperature changes.

Analyzing the limits of dissolution and the formation of solid precipitates in aqueous solutions.

Students will calculate and use the solubility product constant to predict precipitation.

Students will define solutions, solutes, and solvents, and explore different types of solutions.

Students will calculate and interconvert various concentration units (molarity, molality, percent by mass/volume).

Students will investigate how the presence of a solute affects the physical properties of a solvent.

Comparing the Arrhenius and Bronsted Lowry definitions of acids and bases.

Students will differentiate between strong and weak acids and bases and their ionization.

Using neutralization reactions to determine the unknown concentration of a solution.

Students will calculate and use acid and base ionization constants (Ka, Kb) for weak acids and bases.

Students will investigate the composition and function of buffer solutions.

Students will define oxidation and reduction and assign oxidation numbers.

Students will balance complex redox reactions using the half-reaction method.

Investigating the movement of electrons in oxidation reduction reactions and its application in batteries.

Students will construct galvanic cells and calculate standard cell potentials.

Students will explore electrolytic cells and their applications in electroplating and industrial processes.