New AP Chemistry Cirriculum
What’s In
What’s Out
The 6 Big Ideas
1.
2.
3.
4.
5.
6.
Atomic Structure
Bonding and Properties
Reactions (including Electrochemistry)
Kinetics
Thermodynamics
Chemical Equilibrium
Big Idea 1
Atomic Structure
• The chemical elements are fundamental building
materials of matter, and all matter can be understood
in terms of arrangements of atoms. These atoms
retain their identity in chemical reactions
• Includes atomic theory, mole-mass calculations,
electronic configuration, periodicity
• Lab-wise: gravimetric analysis, titrations, Beer’s law
Big Idea 1 (Cont.)
Atomic Structure
Exclusions:
• Memorization of exceptions to Aufbau
principle, i.e., Cr and Cu, Mo and Ag
• Assignment of quantum numbers to electrons
What’s Out: Content
• Quantum Numbers
Big Idea 1 (Cont.)
Atomic Structure
New or emphasized:
• LO 1.5, 1.6, 1.7: Photoelectron Spectroscopy
• LO 1.7, 1.8: Coulomb’s Law – attractive force due to
opposite charges vs distance
• LO 1.13: Refining models
• LO 1.14: Mass spectrometry for isotopes
• LO 1.15: Vibration (IR) vs Electronic transition (UVVis)
Big Idea 2
Bonding and Properties
• Chemical and physical properties of materials can be
explained by the structure and the arrangement of atoms,
ions, or molecules and the forces between them
• Includes solids, liquids, gases, solutions, inter-particulate
forces, electronegativity, Lewis structures, VSEPR theory,
bonding, properties
• Lab-wise: LO 2.7, 2.10: separation techniques especially
chromatography and distillation; and LO 2.22: type of
bonding
Big Idea 2 (Cont.)
Bonding and Properties
Exclusions:
• Phase Diagram (prior knowledge)
• Colligative properties (prior knowledge)
• Molality, percent by mass and by volume (prior
knowledge)
• Weaker H-bonding with H not bonded to N, O, or F
• Specific types of crystal structures, e.g. ABC, ABA, etc.
Big Idea 2 (Cont.)
Bonding and Properties
Exclusions (Cont.):
• The use of formal charge to explain exception to octet rule
– but the use of formal charge calculation is still in
• Learning how to defend the Lewis model, e.g. with odd
number of electrons
• Hybridization beyond sp3
• Filling molecular orbital diagrams
• Specific varieties of crystal lattices for ionic compound
What’s Out: Content
• Hybridization beyond sp, sp2, and sp3
What’s Out: Content
• Phase Diagram
Big Idea 2 (Cont.)
Bonding and Properties
New or emphasized:
• LO 2.19, 2.21, 2.26: Macroscopic properties such as
viscosity, surface tension, capillary action, vapor pressure,
boiling point, volumes of mixing for liquids, hardness
• LO 2.14: Coulombic forces as IMFs in biological systems
and in hydrogen PE vs. nuclear distance
• LO 2.25, 2.26: Alloys
• LO 2.30: Semi-conductors using Si
Big Idea 3
Chemical Reactions
• Changes in matter involve the rearrangement and/or
reorganization of atoms and/or the transfer of electrons
• Equation writing, stoichiometric calculations, BronstedLowry acid-base theory, oxidation numbers, redox
reactions, energies involved, electrochemistry
• Lab-wise: LO 3.5, 3.6: synthesis and decomposition
reactions; LO 3.9: redox reactions; acid-base reactions
Big Idea 3 (Cont.)
Chemical Reactions
Exclusions:
• Lewis acid-base concepts (prior knowledge) but
complex ions and related solubility are included
• Language of reducing agent and oxidizing agent
• Labeling an electrode as positive or negative
• Calculations using the Nernst equation is excluded
but qualitative reasoning about effects of
concentration on cell potential is in
What’s Out: Content
• Lewis definition of acids and bases
Also no more 5 choice multiple choice, only 4 choices!
Big Idea 3 (Cont.)
Chemical Reactions
New or emphasized:
• LO 3.1: Pictorial representation at the particulate
level
• LO 3.10: Classify physical change, chemical change, or
ambiguous change based on macroscopic
observation and microscopic theory regarding
bonding and interactions of particles
• LO 3.11: Graphical depiction of energy diagrams
Big Idea 4
Kinetics
• Rates of chemical reactions are determined by
details of the molecular collisions
• Includes factors affecting reaction rates, rate
laws (both differential and integrated),
collision theory, reaction mechanism, catalysis
• Lab-wise: LO 4.1: Exploration of factors
affecting rate of reaction; Beer’s Law
Big Idea 4 (Cont.)
Kinetics
Exclusions:
• Arrhenius equation in calculations is out, but
conceptual aspects of the equation and
graphical interpretation are still in
• Collection of data pertaining to experimental
detection of a reaction intermediate
Big Idea 4 (Cont.)
Kinetics
New or emphasized:
• LO 4.7, 4.8: Catalysts function either by lowering
activation energy and keeping the same mechanism,
or by altering the mechanism by forming an
intermediate
• LO 4.9: Catalysis includes Acid-base catalysis, surface
catalysis, enzyme catalysis
Big Idea 5
Thermodynamics
• The laws of thermodynamics describe the essential
role of energy and explain and predict the direction
of changes in matter
• Includes kinetic theory, specific heat, heating curve,
calorimetry and enthalpy changes, intermolecular
forces, entropy, Gibb’s free energy, relation between
ΔG and K
• Lab-wise: LO 5.7: calorimetry
Big Idea 5 (Cont.)
Thermodynamics
Exclusions:
• None
New or emphasized:
• LO 5.1 Create or use graphical representations to connect the
dependence of potential energy to distance between atoms,
and factors such as bond order and polarity that influence the
interaction strength
• LO 5.2: Drawing of arrows to indicate particle velocities to
relate temperature and motion
Big Idea 5 (Cont.)
Thermodynamics
New or emphasized (Cont.):
• LO 5.3: Heat transfer to establish equilibrium
• LO 5.6: Heat and PV work in gas expansion and
contraction
• LO 5.9, 5.10, 5.11: IMF in small and large molecules,
polymers, enzymes, biological molecules
• LO 5.13, 5.14: The phrase “thermodynamically favored” in
place of “spontaneous”
Big Idea 5 (Cont.)
Thermodynamics
New or emphasized (Cont.):
• LO 5.15, 5.16, 5.17: External energy source or
coupling to make non-TF reactions occur, e.g.
electrochemistry, light requirement in
photosynthesis, ionization
Big Idea 6
Chemical Equilibrium
• Any bond or intermolecular attraction that can be
formed can be broken. These two processes are in a
dynamic competition, sensitive to initial conditions
and external perturbations
• Includes equilibrium, Le Chatelier’s principle, acidbase equilibria, pH, pOH, Kw, Ka, Kb, titration, buffers,
Ksp, ΔG and K
• Lab-wise: LO 6.13: acid-base titration; LO 6.18:
preparing a buffer
Big Idea 6 (Cont.)
Chemical Equilibrium
Exclusions:
• Numerical computation of concentrations of species
in titration of polyprotic acids
• Computing the change in pH resulting from addition
of acid or base to a buffer
• Production (derivation) of Henderson-Hasselbalch
equation from equilibrium constant expression
Big Idea 6 (Cont.)
Chemical Equilibrium
Exclusions (Cont.):
• Memorization of solubility rules beyond Na, K, NH4,
and nitrates salts
• Calculating solubility of salts as a function of pH
• Calculating solubility of salts in pH-sensitive solutions
Big Idea 6 (Cont.)
Chemical Equilibrium
New or emphasized:
• LO 6.11 Generate or use a particulate representation of
an acid (strong, weak, polyprotic) and a strong base to
explain the major species at equilibrium
• LO 6.24 Analyze the enthalpic and entropic changes
during dissolution of a salt, using particulate level
interactions and representations
• LO 6.25: “Exergonic/endergonic”distinction in biological
systems involving relationship of K and ΔG
Additional Content Deletion
• Organic Chemistry Nomenclature
• Nuclear Chemistry
• Complex Ion / Coordination Chemistry
Science Practices
• 7 Science Practices, p.185-189
• Enable students to establish lines of evidence
and to develop and refine testable
explanations and predictions
• Require students to think and conduct
scientific investigations like working scientists
Science Practices
The Student Can …
• SP1: Use representations and models to
communicate scientific phenomena and solve
scientific problems
• SP2: Use mathematics appropriately
• SP3: Engage in scientific questioning to extend
thinking or to guide investigations
• SP4: Plan and implement data collection strategies for
a scientific question
Science Practices
The Student Can …
• SP5: Perform data analysis and evaluation of
evidence
• SP6: Work with scientific explanation and theories
• SP7: Connect and relate knowledge across various
scales, concepts, and representations in and across
domains
Activity: Science Practices
• Example on Handbook p.7
• Answer questions on p.8 in your group
Science Practices
Not Emphasized in Textbooks
• 1.3: The student can refine representations and models of
natural or man-made phenomena and systems in the domain
• 1.4:The student can use representations and models to
analyze situations or solve problems qualitatively and
quantitatively
• 2.1:The student can justify the selection of a mathematical
routine to solve problems
• 3.1-3.3:The student can pose, refine, and evaluate scientific
questions
Science Practices
Not Emphasized in Textbooks
• 4.1:The student can justify the selection of the kind of data
needed to answer a particular scientific question
• 4.2:The student can design a plan for collecting data to answer
a particular scientific question
• 5.3:The student can evaluate the evidence provided by data
sets in relation to a particular scientific question
• 6.5:The student can evaluate alternative scientific explanations
• 7.1:The student can connect phenomena and models across
spatial and temporal scales
What’s Out: Content
• Nuclear reactions
• Flame Colors
What’s Out: Content
• Memorization of Conclusions
What’s Out: Question Type
What’s Out: Question Type
What’s Out: Content & Question Type
Correct statements about alpha particles include which of the
following?
I.
They have a mass number of 4 and a charge of +2.
II.
They are more penetrating than beta particles.
III.
They are helium nuclei.
(A) I only
(B) III only
(C)I and II
(D) I and III
(E) II and III