AP Chemistry Made Easy

Explore unit one concepts including moles, molar mass, mass spectroscopy, elemental composition, composition of mixtures, atomic structure for electron spectroscopy, periodic trends, valence electrons, and ionic compounds.

Explore atoms, ions, and isotopes within the periodic table and understand molar mass and moles. Apply Avogadro's number, dimensional analysis, and mass spectroscopy to find weighted atomic masses.

Explore pure substances, detailing covalent and ionic bonds, valence electrons, electronegativity, and octet stability, and distinguish homogeneous and heterogeneous mixtures with empirical and molecular formulas.

Explore how Mendeleev organized the periodic table into groups and periods. Learn about noble gases, halogens, alkali metals, alkaline earth metals, transition metals, and lanthanides and actinides.

Learn electron configuration and photoelectron spectroscopy by applying Coulomb's law to nucleus–electron attraction, explore energy levels and sublevels s, p, d, f, and apply Pauli exclusion and Hund's rule.

Explore types of chemical bonds, intermolecular forces, and the potential energy structures of ionic solids, metals, and alloys, with Lewis diagrams, resonance, and formal charge. Examine bond hybridization.

Explore how bond energy and bond length reflect bond order across ionic, covalent, polar covalent, and metallic bonds, using a potential energy graph. Explain roaming electrons and alloy formation.

Learn to build Lewis structures by counting valence electrons, constructing a skeleton, and forming bonds; evaluate bond order and formal charge, and consider polyatomic ions and resonance.

Explains valence electron pair repulsion shaping molecular geometry, from linear to trigonal planar and tetrahedral, and introduces electron geometry and s and p hybridization forming sigma and pi bonds.

Explore intermolecular forces, the phases of matter, kinetic molecular theory, and solutions and mixtures, then examine the photoelectric effect in ap chemistry.

The lecture compares nonpolar and polar molecules, introduces London dispersion forces, dipole-dipole forces, hydrogen bonding, and ion-dipole forces, and explains how stronger intermolecular forces raise melting and boiling points.

Explore solids, liquids, and gases with insights on ionic solids, metallic solids, covalent network solids, and covalent molecular solids, plus vapor pressure, boiling point, and the ideal gas law.

Explore electron spectroscopy: electrons absorb energy, emit photons, and reveal the electromagnetic spectrum; apply c = λ ν, E = h ν, and Beer-Lambert law for absorbance.

Explore ionic equations and representations of reactions, learn how reaction equations express chemical changes, examine physical and chemical changes, and identify the types of chemical reactions.

Explore chemical changes and physical changes, learn to balance equations under the law of conservation of mass, and apply stoichiometry and net ionic equations to predict precipitates and outcomes.

Explore limiting reactants and theoretical yield, and how percent yield compares to actual yield. See particle diagrams show excess reactants and precipitate formation in double-replacement reactions.

Explore titrations to determine unknown concentrations using a known titrant and indicator, reaching the equivalence point. Review acid-base, redox, and precipitation reactions, including definitions, oxidation numbers, and solubility rules.

Explore unit five concepts such as reaction rate, rate law introduction, elementary reactions, collision model, reaction mechanisms, the energy profile, and telesis.

Explore kinetics through the rate law and collision model, covering concentration, temperature, catalysts, and activation energy, and apply differential and integrated rate laws for zero, first, and second order.

Explore elementary reactions in AP chemistry made easy, identify the rate-determining step, and apply the steady-state approximation to derive the rate law using intermediates and catalysts.

Explore reaction profiles and energy graphs, identifying activation energy, reactants, and products, and compare single-step and multi-step pathways, including exothermic outcomes.

Examine how catalysts increase reaction rates by boosting effective collisions and lowering activation energy, while remaining unchanged and regenerating. Learn three catalysis types: binding, acid-base, and surface catalysis.

Explore endothermic and exothermic processes, heat transfer, and thermal equilibrium, including heat capacity and calorimeter energy during phase changes. Introduce enthalpy of reaction and formation and Hess's law.

Clarify how entropy, internal energy, and enthalpy interrelate through q, w, and PΔV, and differentiate endothermic and exothermic processes under constant pressure.

Apply Hess's law and heat of formation to compute reaction enthalpies, and use calorimetry and specific heat capacity to analyze phase changes, heat of fusion, and heat of vaporization.

Explore equilibrium concepts, calculate equilibrium constants and concentrations, review Le Chatelier's principle, examine solubility equilibria and solubility, and analyze the free energy of dissolution.

Explore dynamic equilibrium, comparing Q and the equilibrium constant, and learn how Ksp and molar solubility drive precipitation, solubility, and Le Chatelier’s principle in AP chemistry.

Explore the properties of acids and bases, including strong acids and bases, acid-base reactions, and buffers. Examine the molecular structure of acids and bases, and pH.

Explore acids and bases through the bronsted-lowry model, pH and h3o+ concepts, and the difference between strong and weak dissociation, including water and salts.

Explore acid-base equilibrium by examining Ka, Kb, and Kw, autoionization of water, pH and pOH, and the Henderson-Hasselbalch equation, including dilution effects and reaction shifts.

Explore how buffers resist pH changes, buffer zone, and learn buffer preparation by mixing a weak acid with its conjugate base or by half-neutralizing the acid with a strong base.

Explore entropy, Gibbs free energy, and thermodynamic favorability, and examine thermodynamic and kinetic controls, equilibrium, and electrochemical cells including galvanic, electrolyte, electrolysis, and Faraday's law.

Explore how entropy and Gibbs free energy govern spontaneity in chemical processes, showing how temperature, volume, and phase changes raise entropy, while Delta G and K determine equilibrium.

Compare galvanic and electrolytic cells, highlighting spontaneous redox energy versus external power, with electrons flowing to the cathode through an external circuit and the role of electrolytes and electrodes.