AP Chemistry Fall Final Review PDF

AP Chemistry Fall Final Review 1.​ Stoichiometry and Limiting Reagent Stoichiometry Ch. 3 2.​ Ch. 4 Aqueous Reactions a.​ Definition of electrolyte/nonelectrolyte b.​ Know the process of solvation (general interaction on how ionic compounds dissolve. solid breaks into...

AP Chemistry Fall Final Review 1.​ Stoichiometry and Limiting Reagent Stoichiometry Ch. 3 2.​ Ch. 4 Aqueous Reactions a.​ Definition of electrolyte/nonelectrolyte b.​ Know the process of solvation (general interaction on how ionic compounds dissolve. solid breaks into ions) c.​ Solubility Rules will be given to you. Using a solubility chart, be able to predict whether a precipitate will form based on reactions given. d.​ Know how to write Ionic and net ionic equations. Be able to determine spectator ions and know which spectator ions cancel. e.​ 4.3 Acids and Bases i)​ Know the definitions of acids and bases ii)​ Know the 6 strong acids. (Papa, can I buy new shoes?) (Chloric acid can be included, however then it will be 7 strong acids) iii)​ Know the products of a neutralization reaction. iv)​ Know the pH of acids, bases and water. v)​ Know the term amphoteric f.​ 4.4 Oxidation Reduction (This will be covered extensively during Spring Semester) i)​ Know definition of oxidation reduction. ii)​ Know how to calculate oxidation numbers iii)​ Identify what elements are oxidized and reduced in a reaction. iv)​ The activity series of metals will be given to you. Be able to determine if a REDOX reaction will occur based on activity series of metals. Sample problem 4.10 p. 145 g.​ 4.5 Concentration of Solution i)​ Know how to calculate molarity of a solution and calculate the molar calculation of ions in solution. P. 148 sample 4.12 p. 149 sample 4.13 ii)​ Titrations will NOT be on the Fall Final 3.​ Thermochemistry Ch. 5 a.​ 5.1 Kinetic and Potential Energy i)​ Know kinetic and potential energy ii)​ Know how to use electrostatic potential energy to describe the strength of ionic bonds. iii)​ Know the difference between system and surroundings. iv)​ Know what a joule and calorie is and how they are used. v)​ Know the definition of work and heat. st b.​ 1 Law of Thermodynamics i)​ Know internal energy ii)​ What is ΔE? iii)​ What does + E and –E mean? iv)​ Know how heat and work are related. P. 173 sample 5.2 v)​ Endo and exothermic processes vi)​ Know definition of state function c.​ 5.3 Enthalpy i)​ Know who to calculate pressure/volume work. P. 177 sample exercise 5.3 ii)​ Do practice Exercise 1 and 2 p. 178 d.​ 5.4 Enthalpies of Rxn i)​ See p. 180 sample exercise 5.5. e.​ 5.5 Calorimetry i)​ Know what specific heat and heat capacity are ii)​ Be able to calculate enthalpy for constant pressure and constant volume calorimetry. See pages 184 and 185 for sample problems. f.​ 5.6 Hess’s Law i)​ Know how to use Hess’s Law to calculate change in enthalpy. Sample Exercises p. 188 g.​ 5.7 Enthalpies of Formation i)​ Be able to calculate enthalpy of formation using Hess’s Law and by using standard enthalpies of formation chart. h.​ 5.8 will not be on the final. Ch. 6 Electronic Structure of Atoms a.​ 6.1 The Nature of Light: i)​ Know definition and properties of light. ii)​ Be able to calculate wavelength and frequency based on the speed of light. iii)​ Know the spectrum of light, which colors/rays have high energy versus low energy. b.​ 6.2 Quantized Energy and Photons i)​ Know what is meant by quantized energy levels ii)​ Be able to describe the photoelectric effect. iii)​ Calculate the energy of a photon. P. 218 sample problem 6.3 c.​ Line Spectra and the Bohr Model i)​ Be able to explain the Bohr Model ii)​ Be able to use the Rydberg equation to solve the energy of an electron in the hydrogen atom at specific principle energy levels. iii)​ Be able to calculate energy differences of the electron when it transitions from one energy level to another. d.​ 6.4 Wave Behavior of Matter i)​ e.​ 6.5 Quantum Mechanics and Atomic Orbitals i)​ Know electron density ii)​ Quantum numbers will NOT be on the final f.​ 6.6 Representative of Orbitals i)​ Know orbitals and shapes for s and p orbitals only. 6.7 Many-Electron Atoms i)​ Know the energies of each of the orbitals ii)​ Know Pauli Exclusion Principle g.​ 6.8- 6.9 Electron Configuration i)​ Know how to determine the electron configuration and condensed version of atoms ii)​ Know Hund’s Rule iii)​ Be able to diagram electron configuration using orbital diagrams. iv)​ You will NOT be tested on the exceptions of electron configuration by the transition metals. Ch. 7 Periodic Trends a.​ 7.1 i)​ Know Mendeleev, Meyers Moseley and Rutherford and their contributions to the periodic table b. 7.2 Effective Nuclear Charge ii)​ Know what effective nuclear charge is. Be able to use Coulombs law to explain attractive forces. Calculating Zeff will not be on the test. iii)​ Understand the Go Figure diagram on p. 261 iv)​ Slater’s Rule will not be on the test. v)​ Know trends of effective nuclear charge and be able to explain it. b.​ 7.3 Sizes of Atoms and Ions i)​ Know the trends of atomic radii for both atoms and ions. Be able to explain why these trends exist. ii)​ Know what isoelectronic means. c.​ 7.4 Ionization Energy i)​ Know the concepts of 1st and 2nd Ionization energy ii)​ Know trends and be able to explain the trend. d.​ 7.5 Electron Affinity i)​ Know the concept of electron affinity and the difference between electron affinity and ionization energy in both definition and in energy. e.​ 7.6-7.8 i) Know the general characteristics/trends for groups discussed in section 6-8 Ch. 8 Basic Concepts of Chemical Bonding a.​ 8.1 i)​ know how to draw lewis dot structures. b.​ 8.2 Ionic Bonding i)​ Be able to explain how ionic bonds form. ii)​ Know the definition of lattice energy. Be able to use Coulomb's Law to determine relative lattice energy of ionic compounds. c.​ 8.3 Covalent Bonds i)​ Know how covalent bonds are formed. Be able to draw Lewis dot structures for molecules. ii)​ Know how double and triple bonds exist in terms of hybridization. d.​ Bond Polarity and Electronegativity i)​ Know the concept of bond polarity. Be able to predict bond polarity based on position on the periodic table, using trends of electronegativity. ii)​ Know the difference between polar bonds and nonpolar bonds.  iii)​ Know how electronegativity affects bond polarity. If given a chart of electronegativity be able to determine if a bond is ionic, polar covalent or nonpolar covalent. iv)​ Know what a dipole is. Calculation of dipoles will not be on the test. e.​ 8.5 Lewis Dot Structures i)​ Be able to draw lewis dot structures. ii)​ Know how to calculate formal charge to determine the most likely structure. f.​ 8.6 Resonance Structures i)​ Know how to draw resonance structures. Know the structure for benzene as well. g.​ 8.7 Exceptions to the Octet Rule i)​ Know which atoms can violate the octet by having less than an octet or more than an octet. h.​ 8.8 Strengths and Lengths of Covalent Bonds i)​ Know how to calculate bond enthalpy ii)​ Know how bond length and bond strength are related. ​ Ch. 9 Molecular Geometry and Bonding Theories a.​ 9.1 Molecular Shapes i)​ Know the molecular shapes for molecules and their bond angles. b.​ 9.2 VSEPR i)​ Know what electron domain is and the difference between electron domain geometry and molecular geometry. Memorize the chart I gave you. Including the molecules with expanded octets. ii)​ Know the effects of nonbonding pairs of electrons on bond angles within a molecule. c.​ 9.3 Molecular Shape and Molecular Polarity i)​ Know how to determine the polarity of a molecule based on shape and dipole moments. Ch. 10 Gas Laws Know all the gas laws and how to use formulas to solve gas laws. Know how to solve problems using Dalton’s Law of partial pressure and mole fraction. Know the Kinetic Molecular Theory of Gases. Be able to use the Graham’s Law of Effusion. Know the difference between molecular effusion and diffusion. Be able to calculate Root-Mean Square. Know when gases do not behave ideally. END of Material for Jan 2025. Chapters 11-20 will be included in the Spring Semester  Spring Semester (Partial) Ch. 9 Molecular Geometry and Bonding Theories d.​ 9.1 Molecular Shapes ii)​ Know the molecular shapes for molecules and their bond angles. e.​ 9.2 VSEPR iii)​ Know what electron domain is and the difference between electron domain geometry and molecular geometry. Memorize the chart I gave you. Including the molecules with expanded octets. iv)​ Know the effects of nonbonding pairs of electrons on bond angles within a molecule. f.​ 9.3 Molecular Shape and Molecular Polarity ii)​ Know how to determine the polarity of a molecule based on shape and dipole moments. g.​ 9.4-9.5 i)​ know valence-bond theory and hybrid orbitals, sp, sp2 sp3. Know the shapes associated with hybrid orbitals. h.​ 9.6 Multiple Bonds i)​ Understand how unhybridized p orbitals form pi bonds. ii)​ Know what delocalized electrons are and how they are formed. i.​ 9.7 or 9.8 will not be on test with the exception of the definition of para and diamagnetism. Ch. 11 Liquids and Intermolecular Forces Know the atom arrangement of solids, liquids and gases. Know the 6 intermolecular forces and relative strengths. Be able to explain the graph on p. 449. Know how to determine which molecules would have the strongest IMF based on types of IMF present, polarity, and molecule complexity. Know definition of viscosity, capillary action and surface tension. Know the phase changes between each state of matter. Be able to read a phase diagram. Know what and where the triple points and critical point are. Know that the lines on a phase change diagram represent equilibrium between two phases. (except at the triple point where 3 phases are in equilibrium) Be able to explain the heating curve for water ( or another substance), see page 459 Figure 11.22 Know what vapor pressure is and enthalpy of vaporization. Know how atmospheric pressure and vapor pressure are related in terms of boiling. Ch 12. Solids and Modern Materials 12.1 Classification of Solids ​ Know the properties of a Metallic, Ionic, Molecular and Covalent Network solids. ​ Know the definition crystalline and amorphous solids. (Skip Unit Cells and Crystal Lattices, Filling the Unit Cell, Structures of Metallic Solids, Close Packing) Know what an alloy, interstitial, and substitutional alloys are ​ 12.4 Metallic Bonding:  Know how metals bond, understand what is meant by “sea of electrons” or “mobile electrons” Skip Molecular Orbital Orbitals ​ 12.5 Ionic Solids Know the definition and properties of an Ionic solid. Structures of Ionic Solids p. 498-501 will not be tested. ​ 12.6 Molecular Solids Know the definition and properties of Molecular Solids ​ 12.7 Covalent Network Solids Know definition and properties of Covalent Network solids. What are the two elements that form covalent network solids? What are the names of the network solids? How do they bond? What is the hybridization of the network solids? Semiconductors: know the definition and what p and n semiconductors are ​ 12.8 Polymers: know definition of polymer and be able to give at least 3 types of polymers. Ch. 13 Properties of Solutions 13.1 Solution Process Know what types of substances will mix to form a solution based on molecular structure. Know the enthalpy of solution ​ 13.2 Saturated Solutions and Solubility Know definitions of solubility, saturated solution, unsaturated solution, supersaturated solution, solute, solvent, solution ​ 13.3 Factors Affecting Solubility ​ ​ Know how structure, temperature and pressure affect the solubility of substances. Know the process of separating component of a solution by fractional crystalization, distillation, and chromatography ​ 13. 4 Expressing Solution Concentration ​ ​ Know how to calculate molarity, mass percent of a solution, and mol fraction ​ 13.5 and on will not be on the test.