AP CHEMISTRY TOPICS/LOs (FALL 2024 FORWARD)

TOPIC 1.1 The Mole

LO 1.1.A Calculate quantities of a substance or its relative number of particles using dimensional analysis and the mole concept

EK 1.1.A.1-3

TOPIC 1.2 Isotopes and Mass Spectrometry

LO 1.2.A Explain the quantitative relationship between the mass spectrum of an element and the masses of the element’s isotopes

EK 1.2.A.1-2

TOPIC 1.3 Empirical & Molecular Formula

LO 1.3.A Explain the quantitative relationship between the elemental composition by mass and the empirical formula of a pure substance

EK 1.3.A.1-3

TOPIC 1.4 Pure & Impure

LO 1.4.A Explain the quantitative relationship between the elemental composition by mass and the composition

EK 1.4.A.1-2

TOPIC 1.5 Atoms & Electronic Configuration

LO 1.5.A Represent the electron configuration of an element or ions of an element using the Aufbau principle

EK 1.5.A.1-4

TOPIC 1.6 Photoelectron Spectroscopy

LO 1.6.A Explain the relationship between the photoelectron spectrum of an atom or ion and:

i. The electron configuration of the species.

ii. The interactions between the electrons and the nucleus

EK 1.6.A.1

TOPIC 1.7 Periodicity

LO 1.7.A Explain the relationship between trends in atomic properties of elements and electronic structure and periodicity

EK 1.7.A.1-3

TOPIC 1.8 Formation of Ions

LO 1.8.A Explain the relationship between trends in the reactivity of elements

EK 1.8.A.1-3

TOPIC 2.1 Sliding Scale of Bond Type

LO 2.1.A Explain the relationship between the type of bonding and the properties of the elements participating in the bond

EK 2.1.A.1-5

TOPIC 2.2 Bond Length & Strength

LO 2.2.A Represent the relationship between potential energy and distance between atoms, based on factors that influence the interaction strength

EK 2.2.A.1-3

TOPIC 2.3 The Ionic Lattice

LO 2.3.A Represent an ionic solid with a particulate model that is consistent with Coulomb’s Law and the properties of the constituent ions

EK 2.3.A.1

TOPIC 2.4 Metallic Bonding & Alloys

LO 2.4.A Represent a metallic solid and/or alloy using a model to show essential characteristics of the structure and interactions

EK 2.4.A.1-3

TOPIC 2.5 Lewis Structures

LO 2.5.A Represent a molecule with a Lewis diagram

EK 2.5.A.1

TOPIC 2.6 Resonance & Formal Charge

LO 2.6.A Represent a molecule with a Lewis Diagram that accounts for resonance between equivalent structures of that uses formal charge to select between nonequivalent structures

EK 2.6.A.1-3

TOPIC 2.7 VSEPR & Hydridization

LO 2.7.A Based on the relationship between Lewis diagrams, VSEPR theory, bond orders, and bond polarities: a. Explain structural properties of molecules b. Explain electron properties of molecules

EK 2.7.A.1-4

TOPIC 3.1 IMFs & Ion-dipole Forces

LO 3.1.A Explain the relationship between the chemical structures of molecules and the relative strength of their intermolecular forces when:

i. The molecules are of the same chemical species.

ii. The molecules are of two different chemical species

EK 3.1.A.1-5

TOPIC 3.2 Types of Solids & Properties

LO 3.2.A Explain the relationship among the macroscopic properties of a substance, the particulate-level structure of the substance, and the interactions between these particles

EK 3.2.A.1-7

TOPIC 3.3 States of Matter

LO 3.3.A Represent the differences between solid, liquid and gas phases using a particulate-level model

EK 3.3.A.1-4

TOPIC 3.4 Ideal Gases

LO 3.4.A Explain the relationship between the macroscopic properties of a sample of gas or mixture of gases using the ideal gas law

EK 3.4.A.1-3

TOPIC 3.5 Gases & Kinetic Molecular Theory

LO 3.5.A Explain the relationship between the motion of particles and the macroscopic properties of gases with: a. The kinetic molecular theory (KMT). b. A particulate model. c. A graphical representation

EK 3.5.A.1-4

TOPIC 3.6 Deviations from Ideal Behavior

LO 3.6.A Explain the relationship among the non-ideal behaviors of gases, interparticle forces and/or volumes

EK 3.6.A.1

TOPIC 3.7 Solutions & Conentration

LO 3.7.A Calculate the number of solute particles, volume or molarity of solutions

EK 3.7.A.1-2

TOPIC 3.8 Particulate Diagrams of Solutions

LO 3.8.A Using particulate models for mixtures:

i. Represent interactions between components.

ii. Represent concentrations of components

EK 3.8.A.1

TOPIC 3.9 Chromatography and Distillation

LO 3.9.A Explain the results of a separation experiment based upon intermolecular interactions

EK 3.9.A.1

TOPIC 3.10 Solubility of Solutes in Solvents

LO 3.10.A Explain the relationship between the solubility of ionic and molecular compounds in aqueous and non-aqueous solvents, and the intermolecular interactions between particles

EK 3.10.A.1

TOPIC 3.11 Effect of Radiation on Matter

LO 3.11.A Explain the relationship between a region of the electromagnetic spectrum and the types of molecular or electronic transitions associated with that region

EK 3.11.A.1

TOPIC 3.12 Photons

LO 3.12.A Explain the properties of an absorbed or emitted photon in relationship to an electronic transition in an atom or molecule

EK 3.12.A.1-2

TOPIC 3.13 Beer’s Law

LO 3.13.A Explain the amount of light absorbed by a solution of molecules or ions in relationship to the concentration, path length, and molar absorptivity

EK 3.13.A.1-2

TOPIC 4.1 Chemical & Physical Change

LO 4.1.A Identify evidence of chemical and physical changes in matter

EK 4.1.A.1-2

TOPIC 4.2 Equations & Net Ionic Equations

LO 4.2.A Represent changes in matter with a balanced chemical or net ionic equation: a. For physical changes. b. For given information about the identity of the reactants and/or product. c. For ions in a given chemical reaction

EK 4.2.A.1-3

TOPIC 4.3 Particulate Representations of Equations

LO 4.3.A Represent a given chemical reaction of physical process with a consistent particulate model

EK 4.3.A.1

TOPIC 4.4 Chemical & Physical Change in Terms of Bonds & Forces

LO 4.4 Explain the relationship between the macroscopic characteristics and bond interactions for: a. Chemical processes b. Physical processes

EK 4.4.A.1-2

TOPIC 4.5 Stoichiometry

LO 4.5.A Explain changes in the amounts of reactants and products based on the balanced reaction equation for a chemical process

EK 4.5.A.1-3

TOPIC 4.6 Titrations I

LO 4.6.A Identify the equivalence point in a titration based on the amounts of the titrant and analyte, assuming the titration reaction goes to completion

EK 4.6.A.1

TOPIC 4.7 Types of Chemical Reaction

LO 4.7.A Identify a reaction as acid-base, oxidation-reduction, or precipitation

EK 4.7.A.1-5

TOPIC 4.8 Acid-Base Reactions

LO 4.8 Identify species as Brønsted-Lowry acids, bases, and/or conjugate acid-base pairs, based on proton-transfer involving those species

EK 4.8.A.1-3

TOPIC 4.9 REDOX Reactions

LO 4.9.A Represent a balanced REDOX reaction equation using half-reactions

EK 4.9.A.1

TOPIC 5.1 Factors Affecting Rates

LO 5.1.A Explain the relationship between the rate of a chemical reaction and experimental parameters

EK 5.1.A.1-3

TOPIC 5.2 Rate Laws

LO 5.2.A Represent experimental data with a consistent rate law expression

EK 5.2.A.1-5

TOPIC 5.3 Rates, Graphs & Half-Life

LO 5.3.A Identify the rate law expression of a chemical reaction using data that show how the concentrations of reaction species change over time

EK 5.3.A.1-6

TOPIC 5.4 Elementary Steps

LO 5.4.A Represent an elementary reaction as a rate law expression using stoichiometry

EK 5.4.A.1-2

TOPIC 5.5 Collision Theory

LO 5.5.A Explain the relationship between the rate of an elementary reaction and the frequency, energy, and orientation of molecular collisions

EK 5.5.A.1-3

TOPIC 5.6 Energy Profiles I

LO 5.6.A Represent the activation energy and overall energy change in an elementary reaction using a reaction energy profile

EK 5.6.A.1-4

TOPIC 5.7 Mechanisms

LO 5.7.A Identify the components of a reaction mechanism

EK 5.7.A.1-4

TOPIC 5.8 Mechanisms & Rate Law

LO 5.8.A Identify the rate law for a reaction from a mechanism in which the first step is rate limiting

EK 5.8.A.1

TOPIC 5.9 Intermediates in Rate Determining Steps

LO 5.9.A Identify the rate law for a reaction from a mechanism in which the first step is not rate limiting

EK 5.9.A.1

TOPIC 5.10 Energy Profiles II

LO 5.10.A Represent the activation energy and overall energy change in a multi-step reaction with a reaction energy profile

EK 5.10.A.1

TOPIC 5.11 Catalysts

LO 5.11.A Explain the relationship between the effect of a catalyst on a reaction and changes in the reaction mechanism

EK 5.11.A.1-5

TOPIC 6.1 Endothermic & Exothermic Reactions

LO 6.1.A Explain the relationship between experimental observations and energy changes associated with a chemical or physical transformation

EK 6.1.A.1-4

TOPIC 6.2 Energy Diagrams

LO 6.2.A Represent a chemical or physical transformation with an energy diagram

EK 6.2.A.1

TOPIC 6.3 Heat

LO 6.3.A Explain the relationship between the transfer of thermal energy and molecular collisions

EK 6.3.A.1-3

TOPIC 6.4 Calorimetry

LO 6.4.A Calculate the heat q absorbed or released by a system undergoing heating/ cooling based on the amount of the substance, the heat capacity, and the change in temperature

EK 6.4.A.1-7

TOPIC 6.5 Heating & Cooling Curves

LO 6.5.A Explain changes in the heat q absorbed or released by a system undergoing a phase transition based on the amount of the substance in moles and the molar enthalpy of the phase transition

EK 6.5.A.1-2

TOPIC 6.6 Enthalpy

LO 6.6.A Calculate the heat q absorbed or released by a system undergoing a chemical reaction in relationship to the amount of the reacting substance in moles and the molar enthalpy of reaction

EK 6.6.A.1-3

TOPIC 6.7 Bond Enthalpy

LO 6.7.A Calculate the enthalpy change of a reaction based on the average bond energies of bonds broken and formed in the reaction

EK 6.7.A.1-2

TOPIC 6.8 Enthalpy of Formation

LO 6.8.A Calculate the enthalpy change for a chemical or physical process based on the standard enthalpies of formation

EK 6.8.A.1

TOPIC 6.9 Hess’s Law

LO 6.9.A Represent a chemical or physical process as a sequence of steps

EK 6.9.A.1

LO 6.9.B Explain the relationship between the enthalpy of a chemical or physical process and the sum of the enthalpies of the individual steps

EK 6.9.B.1-2

TOPIC 7.1 Dynamic Equilibrium I

LO 7.1.A Explain the relationship between the occurrence of a reversible chemical or physical process, and the establishment of equilibrium, to experimental observations

EK 7.1.A.1-4

TOPIC 7.2 Dynamic Equilibrium II

LO 7.2.A Explain the relationship between the direction in which a reversible reaction proceeds and the relative rates of the forward and reverse reactions

EK 7.2.A.1

TOPIC 7.3 Q & K

LO 7.3.A Represent the reaction quotient Qc or Qp, for a reversible reaction, and the corresponding equilibrium expressions Kc = Qc or Kp = Qp

EK 7.3.A.1-2

TOPIC 7.4 Kc & Kp

LO 7.4.A Calculate Kc or Kp based on experimental observations of concentrations or pressures at equilibrium

EK 7.4.A.1

TOPIC 7.5 Large K & Small K

LO 7.5.A Explain the relationship between very large or very small values of K and the relative concentrations of chemical species at equilibrium

EK 7.5.A.1

TOPIC 7.6 Mathematical Manipulation of Q & K

LO 7.6.A Represent a multi-step process with an overall equilibrium expression, using the constituent K expressions for each individual reaction

EK 7.6.A.1-4

TOPIC 7.7 ICE Tables

LO 7.7.A Identify the concentrations or partial pressures of chemical species at equilibrium based on the initial conditions and the equilibrium constant

EK 7.7.A.1-2

TOPIC 7.8 Particulate Representation of Equilibrium

LO 7.8.A Represent a system undergoing a reversible reaction with a particulate model

EK 7.8.A.1

TOPIC 7.9 Le Châtelier’s Principle

LO 7.9.A Identify the response of a system at equilibrium to an external stress, using Le Châtelier’s principle

EK 7.12.A.1-2

TOPIC 7.10 Q versus K and Equilibrium Shifts

LO 7.9.A Explain the relationships between Q, K, and the direction in which a reversible reaction will proceed to reach equilibrium

EK 7.10.A.1-2

TOPIC 7.11 Ksp

LO 7.11.A Calculate the solubility of a salt based on the value of Ksp for the salt

EK 7.11.A.1-4

TOPIC 7.12 Common Ion Effect

LO 7.12.A Identify the solubility of a salt, and/or the value of Ksp for the salt, based on the concentration of a common ion already present in solution

EK 7.12.A.1

TOPIC 8.1 pH, pOH & Kw

LO 8.1.A Calculate the values of pH and pOH, based on Kw and the concentration of all species present in a neutral solution of water

EK 8.1.A.1-4

TOPIC 8.2 Strong Acids & Bases

LO 8.2.A Calculate pH and pOH based on concentrations of all species in a solution of a strong acid or a strong base

EK 8.2.A.1-2

TOPIC 8.3 Weak Acids & Bases, Ka & Kb

LO 8.3.A Explain the relationship among pH, pOH, and concentrations of all species in a solution of a monoprotic weak acid or weak base

EK 8.3.A.1-6

TOPIC 8.4 Neutralization, and Partial Neutralization to create a Buffer

LO 8.4.A Explain the relationship among the concentrations of major species in a mixture of weak and strong acids and bases

EK 8.4.A.1-4

TOPIC 8.5 Titrations II

LO 8.5.A Explain results from the titration of a mono- or polyprotic acid or base solution, in relation to the properties of the solution and its components

EK 8.5.A.1-5

TOPIC 8.6 Structure of Acids & Bases

LO 8.6.A Explain the relationship between the strength of an acid or base and the structure of the molecule or ion

EK 8.6.A.1

TOPIC 8.7 pH of Buffers Relative to pKa

LO 8.7.A Explain the relationship between the predominant form of a weak acid or base in solution at a given pH and the pKa of the conjugate acid or the pKb of the conjugate base

EK 8.7.A.1-3

TOPIC 8.8 Introduction to Buffers

LO 8.8.A Explain the relationship between the ability of a buffer to stabilize pH and the reactions that occur when an acid or a base is added to a buffered solution

EK 8.8.A.1

TOPIC 8.9 Henderson-Hasselbalch

LO 8.9.A Identify the pH of a buffer solution based on the identity and concentrations of the conjugate acid-base pair used to create the buffer

EK 8.9.A.1

TOPIC 8.10 Capacity of Buffers

LO 8.10.A Explain the relationship between the buffer capacity of a solution and the relative concentrations of the conjugate acid and conjugate base components of the solution

EK 8.10.A.1-2

TOPIC 8.11 pH & Equilibrium Shifts

LO 8.11.A Identify the qualitative effect of changes in pH on the solubility of a salt

EK 8.11.A.1

TOPIC 9.1 Entropy Introduction

9.1 Identify the sign and relative magnitude of the entropy change associated with chemical or physical processes

EK 9.1.A.1-2

TOPIC 9.2 Absolute Entropy & ∆S°

9.2 Calculate the entropy change for a chemical or physical process based on the absolute entropies of the species involved in the process

EK 9.2.A.1

TOPIC 9.3 Gibb’s Free Energy & Thermodynamic Favorability

9.3 Explain whether a physical or chemical process is thermodynamically favored based on an evaluation of ∆G°

EK 9.3.A.1-6

TOPIC 9.4 Kinetic Control

9.4 Explain, in terms of kinetics, why a thermodynamically favored reaction might not occur at a measurable rate

EK 9.4.A.1-2

TOPIC 9.5 The Relationship between ∆G° and K

9.5 Explain whether a process is thermodynamically favored using the relationships between K, ΔG°, and T

EK 9.5.A.1-4

TOPIC 9.6 ∆G°, ∆H°, ∆S° and Solubility

9.6 Explain the relationship between the solubility of a salt and changes in the enthalpy and entropy that occur in the dissolution process

EK 9.6.A.1-2

TOPIC 9.7 Coupling

9.7 Explain the relationship between external sources of energy or coupled reactions and their ability to drive thermodynamically unfavorable processes

EK 9.7.A.1-2

TOPIC 9.8 Electrochemistry I

9.8 Explain the relationship between the physical components of an electrochemical cell and the overall operational principles of the cell

EK 9.8.A.1-3

TOPIC 9.9 Electrochemistry II

9.9 Explain whether an electrochemical cell is thermodynamically favored, based on its standard cell potential and the constituent half-reactions within the cell

EK 9.9.A.1-3

TOPIC 9.10 Electrochemistry III,  Non-Standard Conditions

9.10 Explain the relationship between deviations from standard cell conditions and changes in the cell potential

EK 9.10.A.1-4

TOPIC 9.11 Quantitative Aspects of Electrolytic Cells

9.11 Calculate the amount of charge flow based on changes in the amounts of reactants and products in an electrochemical cell

EK 9.11.A.1