I’m asking for curriculum planning. Rewrite each topic to have a title that encapsulate the content of each of the Topic Titles, Learning Objectives, Enduring Understandings, and Essential Knowledge statements. Rewritee each of UNITS 01-09 titles listed to have a title that is designed to encapsulate the content of each of the nine UNITS. Enduring understandings are the long-term takeaways related to the big ideas that leave a lasting impression on students. Learning objectives define what a student needs to be able to do with content knowledge in order to progress toward the enduring understandings. Essential knowledge statements describe the knowledge required to perform the learning objective. (Examples(not necessarily the content tested). Examples for You:
UNIT 01 - ATOMS, ELEMENTS & PERIODICITY
TOPIC 1A (LO 1.1): The Mole
TOPIC 1B (LO 1.2): Isotopes and Mass Spectrometry
TOPIC 1C (LO 1.3): Empirical & Molecular Formula
TOPIC 1D (LO 1.4): Pure & Impure
TOPIC 1E (LO 1.5): Atoms & Electronic Configuration
TOPIC 1F (LO 1.6): Photoelectron Spectroscopy
TOPIC 1G (LO 1.7): Periodicity
TOPIC 1H (LO 1.8): Formation of Ions
UNIT 02 - CHEMICAL BONDING I
TOPIC 2A (LO 2.1): Sliding Scale of Bond Type
TOPIC 2B (LO 2.2): Bond Length & Strength
TOPIC 2C (LO 2.3): The Ionic Lattice
TOPIC 2D (LO 2.4): Metallic Bonding & Alloys
TOPIC 2E (LO 2.5): Lewis Structures
TOPIC 2F (LO 2.6): Resonance & Formal Charge
TOPIC 2G (LO 2.7): VSEPR & Hybridization
UNIT 03 - CHEMICAL BONDING II & GASES
TOPIC 3A (LO 3.1): IMFs & Ion-dipole Forces
TOPIC 3B (LO 3.2): Types of Solids & Properties
TOPIC 3C (LO 3.3): States of Matter
TOPIC 3D (LO 3.4): Ideal Gases
TOPIC 3E (LO 3.5): Gases and Kinetic Molecular Theory
TOPIC 3F (LO 3.6): Deviations from Ideal Behavior
TOPIC 3G (LO 3.7): Solutions & Concentration
TOPIC 3H (LO 3.8): Particulate Diagrams of Solutions
TOPIC 3I (LO 3.9): Chromatography and Distillation
TOPIC 3J (LO 3.10): Solubility of Solutes in Solvents
TOPIC 3K (LO 3.11): Effect of Radiation on Matter
TOPIC 3L (LO 3.12): Photons
TOPIC 3M (LO 3.13): Beer’s Law
UNIT 04 - CHEMICAL REACTIONS
TOPIC 4A (LO 4.1): Chemical & Physical Change
TOPIC 4B (LO 4.2): Equations & Net Ionic Equations
TOPIC 4C (LO 4.3): Particulate Representations of Equations
TOPIC 4D (LO 4.4): Chemical & Physical Change in Terms of Bonds & Forces
TOPIC 4E (LO 4.5): Stoichiometry
TOPIC 4F (LO 4.6): Titrations I
TOPIC 4G (LO 4.7): Types of Chemical Reaction
TOPIC 4H (LO 4.8): Acid-Base Reactions
TOPIC 4I (LO 4.9): REDOX Reactions
UNIT 05 - CHEMICAL KINETICS
TOPIC 5A (LO 5.1): Factors Affecting Rates
TOPIC 5B (LO 5.2): Rate Laws
TOPIC 5C (LO 5.3): Rates, Graphs & Half-Life
TOPIC 5D (LO 5.4): Elementary Steps
TOPIC 5E (LO 5.5): Collision Theory
TOPIC 5F (LO 5.6): Energy Profiles I
TOPIC 5G (LO 5.7): Mechanisms
TOPIC 5H (LO 5.8): Mechanisms & Rate Law
TOPIC 5I (LO 5.9): Intermediates in Rate Determining Steps
TOPIC 5J (LO 5.10): Energy Profiles II
TOPIC 5K (LO 5.11): Catalysts
UNIT 06 - CHEMICAL THERMODYNAMICS I
TOPIC 6A (LO 6.1): Endothermic & Exothermic Reactions
TOPIC 6B (LO 6.2): Energy Diagrams
TOPIC 6C (LO 6.3): Heat
TOPIC 6D (LO 6.4): Calorimetry
TOPIC 6E (LO 6.5): Heating & Cooling Curves
TOPIC 6F (LO 6.6): Enthalpy
TOPIC 6G (LO 6.7): Bond Enthalpy
TOPIC 6H (LO 6.8): Enthalpy of Formation
TOPIC 6I (LO 6.9): Hess’s Law
UNIT 07 - CHEMICAL EQUILIBRIUM
TOPIC 7A (LO 7.1): Dynamic Equilibrium I
TOPIC 7B (LO 7.2): Dynamic Equilibrium II
TOPIC 7C (LO 7.3): Q & K
TOPIC 7D (LO 7.4): Kc & Kp
TOPIC 7E (LO 7.5): Large K & Small K
TOPIC 7F (LO 7.6): Mathematical Manipulation of Q & K
TOPIC 7G (LO 7.7): ICE Tables
TOPIC 7H (LO 7.8): Particulate Representation of Equilibrium
TOPIC 7I (LO 7.9): Le Châtelier’s Principle
TOPIC 7J (LO 7.10): Q versus K and Equilibrium Shifts
TOPIC 7K (LO 7.11): Ksp
TOPIC 7L (LO 7.12): Common Ion Effect
TOPIC 7M (LO 7.13): pH & Equilibrium Shifts
TOPIC 7N (LO 7.14): ∆G°, ∆H°, ∆S° and Solubility
UNIT 08 - ACIDS & BASES
TOPIC 8A (LO 8.1): pH, pOH & Kw
TOPIC 8B (LO 8.2): Strong Acids & Bases
TOPIC 8C (LO 8.3): Weak Acids & Bases, Ka & Kb
TOPIC 8D (LO 8.4): Neutralization, and Partial Neutralization to create a Buffer
TOPIC 8E (LO 8.5): Titrations II
TOPIC 8F (LO 8.6): Structure of Acids & Bases
TOPIC 8G (LO 8.7): pH of Buffers Relative to pKa
TOPIC 8H (LO 8.8): Introduction to Buffers
TOPIC 8I (LO 8.9): Henderson-Hasselbalch
TOPIC 8J (LO 8.10): Capacity of Buffers
UNIT 09 - CHEMICAL THERMODYNAMICS II & ELECTROCHEMISTRY
TOPIC 9A (LO 9.1): Entropy Introduction
TOPIC 9B (LO 9.2): Absolute Entropy & ∆S°
TOPIC 9C (LO 9.3): Gibb’s Free Energy & Thermodynamic Favorability
TOPIC 9D (LO 9.4): Kinetic Control
TOPIC 9E (LO 9.5): The Relationship between ∆G° and K
TOPIC 9F (LO 9.6): Coupling
TOPIC 9G (LO 9.7): Electrochemistry I
TOPIC 9H (LO 9.8): Electrochemistry II
TOPIC 9I (LO 9.9): Electrochemistry III,  Non-Standard Conditions
TOPIC 9J (LO 9.10): Quantitative Aspects of Electrolytic Cells)
Actual Content:
UNIT 1 Atomic Structure and Properties
TOPIC 1.1
Moles and
Molar Mass
Required Course Content
ENDURING UNDERSTANDING
SPQ-1
The mole allows different units to be compared.
LEARNING OBJECTIVE ESSENTIAL KNOWLEDGE
SPQ-1.A
Calculate quantities of a
substance or its relative
number of particles using
dimensional analysis and the
mole concept.
SPQ-1.A.1
One cannot count particles directly while
performing laboratory work. Thus, there must
be a connection between the masses of
substances reacting and the actual number of
particles undergoing chemical changes.
SPQ-1.A.2
Avogadro’s number (N = 6.022 × 1023 mol−1
A )
provides the connection between the number
of moles in a pure sample of a substance and
the number of constituent particles (or formula
units) of that substance.
SPQ-1.A.3
Expressing the mass of an individual atom
or molecule in atomic mass units (amu) is
useful because the average mass in amu of
one particle (atom or molecule) or formula
unit of a substance will always be numerically
equal to the molar mass of that substance
in grams. Thus, there is a quantitative
connection between the mass of a substance
and the number of particles that the
substance contains.
EQN: n = m/M
TOPIC 1.2
Mass Spectroscopy
of Elements
Required Course Content
ENDURING UNDERSTANDING
SPQ-1
The mole allows different units to be compared.
LEARNING OBJECTIVE ESSENTIAL KNOWLEDGE
SPQ-1.B
Explain the quantitative
relationship between the
mass spectrum of an element
and the masses of the
element’s isotopes.
SPQ-1.B.1
The mass spectrum of a sample containing a
single element can be used to determine the
identity of the isotopes of that element and the
relative abundance of each isotope in nature.
SPQ-1.B.2
The average atomic mass of an element can
be estimated from the weighted average of
the isotopic masses using the mass of each
isotope and its relative abundance.
X INTERPRETING MASS SPECTRA
Interpreting mass spectra of samples
containing multiple elements or peaks arising
from species other than singly charged
monatomic ions will not be assessed on
the AP Exam.
TOPIC 1.3
Elemental
Composition of
Pure Substances
Required Course Content
ENDURING UNDERSTANDING
SPQ-2
Chemical formulas identify substances by their unique combination of atoms.
LEARNING OBJECTIVE ESSENTIAL KNOWLEDGE
SPQ-2.A
Explain the quantitative
relationship between the
elemental composition by
mass and the empirical
formula of a pure substance.
SPQ-2.A.1
Some pure substances are composed of
individual molecules, while others consist
of atoms or ions held together in fixed
proportions as described by a formula unit.
SPQ-2.A.2
According to the law of definite proportions,
the ratio of the masses of the constituent
elements in any pure sample of that compound
is always the same.
SPQ-2.A.3
The chemical formula that lists the lowest
whole number ratio of atoms of the elements in
a compound is the empirical formula.
TOPIC 1.4
Composition
of Mixtures
Required Course Content
ENDURING UNDERSTANDING
SPQ-2
Chemical formulas identify substances by their unique combination of atoms.
LEARNING OBJECTIVE ESSENTIAL KNOWLEDGE
SPQ-2.B
Explain the quantitative
relationship between the
elemental composition by
mass and the composition of
substances in a mixture.
SPQ-2.B.1
While pure substances contain molecules or
formula units of a single type, mixtures contain
molecules or formula units of two or more
types, whose relative proportions can vary.
SPQ-2.B.2
Elemental analysis can be used to determine
the relative numbers of atoms in a substance
and to determine its purity.
TOPIC 1.5
Atomic Structure and
Electron Configuration
Required Course Content
ENDURING UNDERSTANDING
SAP-1
Atoms and molecules can be identified by their electron distribution and energy.
LEARNING OBJECTIVE ESSENTIAL KNOWLEDGE
SAP-1.A
Represent the electron
configuration of an element
or ions of an element using
the Aufbau principle.
SAP-1.A.1
The atom is composed of negatively charged
electrons and a positively charged nucleus that
is made of protons and neutrons.
SAP-1.A.2
Coulomb’s law is used to calculate the force
between two charged particles.
EQN: Fcoulombic ∝ q1
q2
r2
SAP-1.A.3
In atoms and ions, the electrons can be thought
of as being in “shells (energy levels)” and
“subshells (sublevels),” as described by the
electron configuration. Inner electrons are called
core electrons, and outer electrons are called
valence electrons. The electron configuration is
explained by quantum mechanics, as delineated
in the Aufbau principle and exemplified in the
periodic table of the elements.
X THE ASSIGNMENT OF QUANTUM NUMBERS
TO ELECTRONS IN SUBSHELLS OF AN
ATOM WILL NOT BE ASSESSED ON THE
AP EXAM.
Rationale: Assignment of quantum numbers
to electrons in specific subshells does not
increase students’ understanding of the
structure of the atom.
SAP-1.A.4
The relative energy required to remove an
electron from different subshells of an atom or
ion or from the same subshell in different atoms
or ions (ionization energy) can be estimated
through a qualitative application of Coulomb’s
law. This energy is related to the distance from
the nucleus and the effective (shield) charge of
the nucleus. 
TOPIC 1.6
Photoelectron
Spectroscopy
ENDURING UNDERSTANDING
SAP-1
Atoms and molecules can be identified by their electron distribution and energy.
LEARNING OBJECTIVE ESSENTIAL KNOWLEDGE
SAP-1.B
Explain the relationship
between the photoelectron
spectrum of an atom or
ion and:
a. The electron configuration
of the species.
b. The interactions
between the electrons
and the nucleus.
SAP-1.B.1
The energies of the electrons in a given
shell can be measured experimentally with
photoelectron spectroscopy (PES). The
position of each peak in the PES spectrum is
related to the energy required to remove an
electron from the corresponding subshell, and
the height of each peak is (ideally) proportional
to the number of electrons in that subshell.
TOPIC 1.7
Periodic Trends
Required Course Content
ENDURING UNDERSTANDING
SAP-2
The periodic table shows patterns in electronic structure and trends in
atomic properties.
LEARNING OBJECTIVE ESSENTIAL KNOWLEDGE
SAP-2.A
Explain the relationship
between trends in atomic
properties of elements and
electronic structure
and periodicity.
SAP-2.A.1
The organization of the periodic table is based
on the recurring properties of the elements and
explained by the pattern of electron configurations
and the presence of completely or partially filled
shells (and subshells) of electrons in atoms.
X WRITING THE ELECTRON CONFIGURATION
OF ELEMENTS THAT ARE EXCEPTIONS
TO THE AUFBAU PRINCIPLE WILL NOT BE
ASSESSED ON THE AP EXAM.
Rationale: The mere rote recall of the
exceptions does not match the goals of the
curriculum revision.
SAP-2.A.2
Trends in atomic properties within the
periodic table (periodicity) can be qualitatively
understood through the position of the element
in the periodic table, Coulomb’s law, the shell
model, and the concept of shielding/effective
nuclear charge. These properties include:
a. Ionization energy
b. Atomic and ionic radii
c. Electron affinity
d. Electronegativity.
SAP-2.A.3
The periodicity (in SAP-2.A.2) is useful to
predict /estimate values of properties in the
absence of data.
TOPIC 1.8
Valence Electrons and
Ionic Compounds
Required Course Content
ENDURING UNDERSTANDING
SAP-2
The periodic table shows patterns in electronic structure and trends in
atomic properties.
LEARNING OBJECTIVE ESSENTIAL KNOWLEDGE
SAP-2.B
Explain the relationship
between trends in the
reactivity of elements
and periodicity.
SAP-2.B.1
The likelihood that two elements will form
a chemical bond is determined by the
interactions between the valence electrons
and nuclei of elements.
SAP-2.B.2
Elements in the same column of the periodic
table tend to form analogous compounds.
SAP-2.B.3
Typical charges of atoms in ionic compounds
are governed by their location on the periodic
table and the number of valence electrons.