Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Atomic Theory
Unit Number: 1
Enduring Understanding:
1.1 – The properties of atoms and ions depend on the number and location of their protons, neutrons, and electrons, and the
changes that these subatomic particles undergo.
Standard
1.1.1
1.1.2
Analyze the structure of atoms,
isotopes, and ions.
Analyze an atom in terms of the
location of electrons.
Essential Questions

What are the relative charges and masses of protons,
neutrons, and electrons?

What do the numbers on the periodic table mean, and
how do they relate to the number of subatomic particles in
an isotope?

How do you calculate the average atomic mass of an
element?

How is the Bohr model of the hydrogen atom related to the
emission spectrum of hydrogen? (overlap with 1.1.3)

How are the electron configurations of atoms related to
the Bohr and electron cloud models of the atom?
Pacing
Guideline
Key Academic
Vocabulary
~2 days
Atom
Atomic Theory
Isotope
Cathode Ray Tube
Oil-Drop Experiment
Gold Foil Experiment
Beryllium-Wax
Experiment
Nucleus
Proton
Neutron
Electron
Atomic Number
Mass Number
Nuclear Symbol
Hyphen Notation
Atomic Mass Unit
Relative Atomic Mass
Average Atomic Mass
~3 days
Electromagnetic
Spectrum
Line Spectrum
Emission Spectrum
Continuous Spectrum
Bohr Model
Electron Cloud Model
1
Chemistry Common Core Curriculum Map 2012-2013
1.1.3
1.3.2
Explain the emission of
electromagnetic radiation in spectral
form in terms of the Bohr model.
Infer the atomic size, reactivity,
electronegativity, and ionization
energy of an element from its position
on the Periodic Table.

What happens when electrons in an atom gain energy and
release energy?

What is the relationship between frequency, wavelength,
and energy for a photon of electromagnetic radiation?

How is the Bohr model of the hydrogen atom related to the
emission spectrum of hydrogen? (overlap with 1.1.2)

Are electrons particles or waves?

How do you illustrate electron configurations of elements?

How is oxidation number related to the number of valence
electrons?
~2 days
Wave-Particle Theory
Quanta
Excited State
Ground State
Quantum Theory
Photon
Wavelength
Frequency
Energy
Planck’s Constant
Orbits
Orbitals
~2 days
Quantum Numbers
(Principal, Orbital,
Magnetic, Spin)
Shell
Subshell/Sublevel
Electron Configuration
Aufbau Principle
Hund’s Rule
Pauli Exclusion
Principle
Orbital Notation
Electron Configuration
Notation
Shorthand Electron
Configuration Notation
Electron (Lewis) Dot
Notation
Oxidation Number
Oxidation
Reduction
2
Chemistry Common Core Curriculum Map 2012-2013
Suggested Resources by Unit
Atomic Theory Notes
Thomson’s CRT Experiments Animation
Millikan’s Oil Drop Experiment Animation
Millikan’s Oil Drop Experiment Animation
Rutherford’s Gold Foil Experiment Animation
Rutherford’s Gold Foil Experiment Animation
Isotopes and Average Atomic Mass Practice Worksheet
Isotopes and Atomic Mass Simulation
Penny Isotope Lab
Penny Isotope Lab (Advanced)
Electron Cloud Simulation Activity
Observing Spectral Lines
Flame Test For Different Metals Animation
Chem Alive! Field Trips CD – The Chemistry of Fireworks
Flame Test Lab
Website that summarizes development of atomic theory,
including animations
Website with animation explaining electron configurations
Electron Configuration Practice Worksheet
Atomic Theory Review
Location of these resources
http://highered.mcgraw-hill.com/sites/0072512644/student_view0/chapter2/animations_center.html#
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/004_MILLIKANOIL.MOV
http://highered.mcgraw-hill.com/sites/0072512644/student_view0/chapter2/animations_center.html#
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/006_RUTHERFORD.MOV
http://highered.mcgraw-hill.com/sites/0072512644/student_view0/chapter2/animations_center.html#
http://phet.colorado.edu/en/simulation/isotopes-and-atomic-mass
(Demonstration using gas discharge tubes and spectrophotometers)
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/039_FlameTestsMet.MOV
Chem Alive! Field Trips CD
http://www.broadeducation.com/htmlDemos/AbsorbChem/HistoryAtom/page.htm
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/043_ElectronConfig.MOV
3
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: The Atomic Nucleus & Radioactivity
Unit Number: 2
Enduring Understanding:
1.1 – Radioactive isotopes have unstable nuclei that undergo predictable nuclear decay processes.
Standard
1.1.4
Explain the process of radioactive
decay using nuclear equations and
half-life.
Essential Questions

What are the differences between alpha, beta, and
gamma radiation?

What is nuclear decay, and how can it be described using
equations?

What is the half-life of a radioisotope?

What are the differences between nuclear fission and
fusion?
Suggested Resources by Unit
The Atomic Nucleus & Radioactivity Notes
Rutherford’s Experiment Animation
Cloud Chamber Lab
Chem Alive! Field Trips CD - Fusion and Fission
Nuclear Fission Simulation
Atomic Nucleus and Radioactivity Practice Worksheet
Atomic Nucleus and Radioactivity Review
Pacing
Guideline
~3 days
Key Academic
Vocabulary
Radiation
Nuclear decay
Alpha radiation
Beta radiation
Gamma radiation
Decay equations
Half-life
Fission
Fusion
Location of these resources
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/005_SEPARATION.MOV
http://phet.colorado.edu/en/simulation/nuclear-fission
4
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Periodicity
Unit Number: 3
Enduring Understanding:
1.3 – The physical and chemical properties of an element can be predicted based upon their location on the Periodic Table.
Standard
1.3.1
1.3.2
Classify the components of a
periodic table (period, group, metal,
metalloid, nonmetal, transition).
Infer the physical properties (atomic
radius, metallic and nonmetallic
characteristics) of an element based
on its position on the Periodic Table.
Essential Questions

Why are elements placed in a particular period or group
on the periodic table?

Which elements on the periodic table are: metals,
nonmetals, metalloids, representative (main group)
elements, transition elements, alkali metals, alkaline earth
metals, halogens, and noble gases?

How do you explain the trend for increasing radius of
atoms (or ions) on the periodic table?

How do you account for the metallic character of elements
classified as metals, and what is the trend for metallic
character among elements on the periodic table?

How do you explain the trend for ionization energy of
elements on the periodic table?

How do you explain the trend for electronegativity of
elements on the periodic table?
Pacing
Guideline
Key Academic
Vocabulary
~1 day
Periodic Table
Period
Group/Family
Metal
Metalloid
Nonmetal
Transition
metal/element
~2 days
Atomic Radius
Valence Electrons
Ionic Radius
Ion
Cation
Anion
Ionization Energy
Electronegativity
Octet
Electron Affinity
5
Chemistry Common Core Curriculum Map 2012-2013
Suggested Resources by Unit
Periodicity Notes
Sodium and Potassium Reactivity Movie
Demonstration: Sodium in Water (with Phenolphthalein)
Periodic Table Trends Animation
Atomic Radius Trend Animation
Ionization Energy Trend Animation
Ionization Energy Trend Animation
Electronegativity Trend Animation
Periodicity Problems Worksheet
Halide Ion Lab
Location of these resources
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/007_SODIUMANDPO.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/044_PeriodicProper.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/046_AtomicRadii.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/047_IonizationEner.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/048_PeriodicIoniza.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/052_Electronegativ.MOV
6
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Bonding
Unit Number: 4
Enduring Understanding:
1.2 – Elements form different types of bonds and attractions based on the nature of elements and the electronegativity
difference between the atoms.
Standard
1.2.1
1.2.2
Compare (qualitatively) the relative
strengths of ionic, covalent, and
metallic bonds.
Infer the type of bond and chemical
formula formed between atoms.
Essential Questions

What constitutes a metallic bond?

How are ions formed, and how are they related to the
number of valence electrons in an atom?

How are covalent bonds formed, and how do you draw the
Lewis structure of a molecule?

How can the electronegativity difference between two
atoms (or their positions on the periodic table) be used to
predict bond type?

How can the Lewis structure of a molecule be used to
predict its formula?
Pacing
Guideline
Key Academic
Vocabulary
3 days
Covalent Bond
Ionic Bond
Metallic Bond
Octet
Cation
Anion
Formula Unit
Molecule
Diatomic
Single Bond
Double Bond
Triple Bond
Octet Rule
Shared/Bonding Pair
Unshared/Non-bonding
Pair
Lewis Structures
Delocalized
Electron Sea
1 day
Non-Polar Covalent
Bond
Polar Covalent Bond
Ionic Character
Covalent Character
7
Chemistry Common Core Curriculum Map 2012-2013
1.2.3
1.2.5
Compare inter- and intra-particle
forces.
Compare the properties of ionic,
covalent, metallic, and network
compounds.

What are the differences between the intermolecular
forces?

What are the relative strengths of the intermolecular
forces compared to each other and to ionic, covalent and
metallic bonds?

How is bond length related to bond strength (bond
enthalpy)?

How do the different types of bonding determine the
properties of ionic, covalent and metallic compounds?

What is VSEPR Theory and how can it be used to predict
the shapes of covalent molecules?

What makes molecules polar or non-polar?

What are the differences between macromolecules and
network covalent solids?
1 day
Bond Length
Bond Enthalpy
Intermolecular Forces
Dipole-Dipole Forces
Hydrogen Bonding
van der Waals’ Forces
London Dispersion
Forces
Instantaneous Dipole
Induced Dipole
Ion-Dipole Attractions
3 days
Melting Point
Boiling Point
Brittle
Volatility
Electrical Conductivity
Thermal Conductivity
Malleability
Ductility
Luster
Electrolytic
Soluble
Insoluble
VSEPR Theory
Electron Pair Geometry
Molecular Geometry
Bond Angle
Linear
Trigonal Planar
Bent
Trigonal Pyramidal
Tetrahedral
Bond Polarity
Molecular Polarity
Dipole
Macromolecule
Network Covalent Solid
Polymers
Allotropes
8
Chemistry Common Core Curriculum Map 2012-2013
Suggested Resources by Unit
Bonding Notes
Formation of NaCl Movie
Bond Formation in Hydrogen Animation
Bonding Practice Worksheet WS
Properties of Ionic & Covalent Compounds Lab
Properties of Ionic & Covalent Compounds Lab #2
VSEPR Geometries WS
Marshmallow Molecules Activity
Molecular Shapes Simulation
Organic Macromolecule Construction Activity
(can be adapted to simpler molecules)
Molecular Polarity Simulation
Demonstration – Balloon/Static Electricity/Polarity of Water
Demonstration – Drops of Water on a Penny (H-bonding)
Ink Chromatography Lab
Plant Pigment Chromatography Lab
TLC Plant Pigment Chromatography Lab
Location of these resources
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/021_SODIUMCHLOR.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/038_H2BondForm.MOV
http://phet.colorado.edu/en/simulation/molecule-shapes
http://phet.colorado.edu/en/simulation/molecule-polarity
9
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Chemical Nomenclature, Equations & Reactions
Unit Number: 5
Enduring Understanding:
1.2 – Compounds are named based upon the type of bond they form.
2.2 – Chemical species undergo characteristic chemical changes, but mass is conserved in their reactions.
Standard
1.2.4
2.2.2
2.2.3
Interpret the name and formula of
compounds using IUPAC convention.
Analyze the evidence of chemical
change.
Analyze the law of conservation of
matter and how it applies to various
types of chemical equations
(synthesis, decomposition, single
replacement, double replacement,
and combustion).
Essential Questions

How do you write the names and formulas of covalent
compounds?

How do you write the names and formulas of ionic
compounds?

What are the names and formulas of some common
polyatomic ions and acids?

What are some evidences that a chemical reaction has
occurred?

What tests can you do to determine if oxygen, hydrogen,
carbon dioxide or water have been produced in a chemical
reaction?

How do you write and balance chemical equations?

What are the five types of chemical reactions?

How can the activity series be used to predict whether or
not a single replacement reaction will occur?
Pacing
Guideline
Key Academic
Vocabulary
3 days
Monatomic ions
Polyatomic ions
Nomenclature
Cation
Anion
Binary compound
Ternary compound
Stock system
Binary acid
Oxyacid
1 day
Precipitate
Solubility rules
Endothermic
Exothermic
Dilution
Burning splint test
Lime water test
Cobalt(II) chloride test
3 days
Reactants
Products
Balanced equation
Synthesis
Decomposition
Single replacement
10
Chemistry Common Core Curriculum Map 2012-2013

How can the solubility rules be used to predict precipitates
in a double replacement reaction?

How do you write and balance ionic and net ionic
equations for double replacement reactions?

What is produced when hydrocarbons and other
molecules containing C, H and O are combusted in
oxygen?
Suggested Resources by Unit
Chemical Nomenclature, Equations & Reactions Notes
Nomenclature Practice Worksheet
Balancing Chemical Equations Simulation
Synthesis of Aluminum Bromide Video
Synthesis of Sodium Chloride Video
Single Replacement of Copper By Silver Ions Video
Demo – Synthesis Reaction: CaO + H2O  Ca(OH)2
(in presence of phenolphthalein)
Demo – Decomposition Reaction: H2O2  H2O + O2
(in presence of MnO2 catalyst)
Demo – Single Replacement: Zn + HCl  ZnCl2 + H2
Demo – Single Replacement: Cu + AgNO3  Cu(NO3)2 + Ag
Demo – Double Replacement: Pb(NO3)2 + KI  PbI2 + KNO3
Demo – Combustion of Propane or Butane
(use CoCl2 paper to show water vapor is a product)
Demo – Splint tests to identify H2, O2, CO2
(use reactions above to generate H2, O2; CO2 from dry ice)
Demo – Lime water test (using CO2 from dry ice)
Balancing Equations & Reaction Types Practice Worksheet
Balancing Equations Worksheet – Extra Practice
Nomenclature, Equations, & Reactions Review Worksheet
Double replacement
Combustion
Activity series
Solubility rules
Acid-base
neutralization reaction
Ionic equation
Net ionic equation
Dissociation
Spectator ions
Hydrocarbons
Location of these resources
http://phet.colorado.edu/en/simulation/balancing-chemical-equations
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/012_FORMALUMBRO.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/021_SODIUMCHLOR.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/024_SILVERCRYSTA.MOV
11
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Stoichiometry
Unit Number: 6
Enduring Understanding:
2.2 – The composition of chemical species and the reactions they undergo can be described quantitatively.
Standard
2.2.4
2.2.5
Analyze the stoichiometric
relationships inherent in a chemical
reaction.
Analyze quantitatively the
composition of a substance
(empirical formula, molecular
formula, percent composition, and
hydrates).
Essential Questions

What are mole ratios and how are the related to the
coefficients in a balanced equation?

Given a balanced equation and the quantity of one
substance in a chemical reaction, how do you determine
the quantity of another substance in the reaction?

How do you calculate the empirical and molecular formula
of a compound?

How do you determine the percentage composition by
mass of a compound?

What is a hydrate?
Pacing
Guideline
Key Academic
Vocabulary
8 days
Stoichiometry
Mole
Avogadro’s number
Molar mass
Atoms
Molecules
Formula units
Mole ratio
STP
SATP
Avogadro’s law
Standard molar volume
Limiting reactant
Percent yield
Actual yield
Theoretical yield
3 days
Empirical formula
Molecular formula
Percentage
composition by mass
Hydrate
12
Chemistry Common Core Curriculum Map 2012-2013
Suggested Resources by Unit
Location of these resources
Stoichiometry Notes
Stoichiometry Worksheet Packet
The Mole Lab
Percent Composition of Hydrates Lab
Empirical Formula Lab (EF of Zinc Chloride)
Limiting Reagent Lab (Vinegar & Baking Soda)
Limiting Reactant / % Yield Lab
Empirical Formula of a Hydrate Simulation
Reaction Stoichiometry Simulation
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/working/empirical.swf
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/stoichiometry/stoic_excess_oxy.swf
13
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Gases
Unit Number: 7
Enduring Understanding:
2.1 – Ideal gases behave in predictable ways, and the relationships among pressure, volume, temperature, and quantity of
these gases can be described qualitatively and quantitatively.
Standard
2.1.5
Explain the relationships among
pressure, temperature, volume, and
quantity of gas, both qualitative and
quantitative.
Essential Questions

What are the characteristics of an ideal gas?

What are factors that affect the solubility of a gas?

How is gas volume related to the number of moles of gas?

How do you perform calculations involving gases using
information about pressure, volume, temperature, and
sometimes mass or moles?

How do you determine the partial pressure of a gas, given
the total pressure and partial pressures of the other
component gases in a mixture?
Pacing
Guideline
6 days
Key Academic
Vocabulary
Ideal gas
Real gas
Standard temperature
and pressure (STP)
Kinetic-molecular
theory (KMT)
Avogadro’s law
mm Hg / torr
Atmospheres
Kilopascals
Boyle’s law
Charles’ law
Gay-Lussac’s law
Combined gas law
Ideal Gas law
Dalton’s law of partial
Pressures
Barometric pressure
Water vapor pressure
14
Chemistry Common Core Curriculum Map 2012-2013
Suggested Resources by Unit
Gases Notes
Gas Laws Problems Worksheet #1
Gas Laws Problems Worksheet #2
Water Vapor Pressure Table
Demo – Fire Syringe (Combined Gas Law)
Demo – Collapsing Can (empty soda can crushed by
atmospheric pressure in ice water bath)
Demo – Cartesian Diver (Boyle’s Law)
Good Gas Laws Demonstrations
Boyle’s Law Microscale Investigation
Demo: Boyle’s Law With Marshmallows
Gas Properties Simulation
Investigating Boyle’s Law Simulation/Lab
Determining the Molar Mass of Butane Lab
Alka-Seltzer & The Ideal Gas Law Lab
Gas Laws: Virtual Chemistry Experiment
Kinetic-Molecular Theory: Virtual Chemistry Expt.
(Many Good Gas Law Simulations)
Location of these resources
http://www.arborsci.com/cool/chemistry-gas-laws-smorgasborg
http://phet.colorado.edu/en/simulation/gas-properties
http://content.blackgold.ca/ict/Division4/Science/Div.%204/Boyles%20Law/boyleslaw.htm
http://www.chm.davidson.edu/vce/GasLaws/index.html
http://www.chm.davidson.edu/vce/KineticMolecularTheory/index.html
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/gaslaw/
15
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Energetics & Kinetics
Unit Number: 8
Enduring Understanding:
2.1 – The energetic nature of substances undergoing phase changes can be described using phase diagrams.
2.2 – Molecules must collide in a specific manner in order for a reaction to occur.
3.1 – The rate of a chemical reaction is affected by factors including temperature, concentration, particle size and presence of a
catalyst.
Standard
2.1.1
Explain the energetic nature of phase
changes.
Essential Questions

How does the energy (both kinetic and potential) of the
particles of a substance change when heated, cooled, or
changing phase?

What is the difference between heat and temperature?
Pacing
Guideline
1 day
Key Academic
Vocabulary
Kinetic energy
Potential energy
Heat
Temperature
Celsius
Kelvin
Joule
Phase change
Change of state
Melting
Freezing
Evaporation
Boiling
Vaporization
Condensation
Sublimation
Deposition
Heating & cooling
curve
16
Chemistry Common Core Curriculum Map 2012-2013
2.1.2
2.1.4
2.2.1
Explain heating and cooling curves
(heat of fusion, heat of vaporization,
heat, melting point, and boiling
point).
Infer simple calorimetric calculations
based on the concepts of heat lost
equals heat gained and specific heat.
Explain the energy content of a
chemical reaction.

What is the specific heat capacity of a substance?

What are the heat of fusion and heat of vaporization of a
substance?

What information can you glean from the heating and
cooling curve of a substance?
Heat capacity
Specific heat capacity
Endothermic
Exothermic
Enthalpy of fusion
Enthalpy of
vaporization

How do you determine the enthalpy change in a
substance that is being heated, cooled or changing state?
(much overlap of
vocabulary with 2.1.1)

What is the difference between an endothermic and
exothermic process?

How is the law of conservation of energy obeyed in a
closed system?

How do you determine the enthalpy change for reactions
occurring in water (aqueous solutions)?

What conditions must be met in order for molecules to
react with each other?

What information about a reaction can you determine from
potential energy diagrams?
1 day
2-3 days
Law of conservation of
Energy
Closed system
Calorimetry
Calorimeter
Molar Enthalpy
1-2 days
Collision theory
Orientation
Collision geometry
Potential energy
diagram
Reactants
Products
Activated complex
Activation energy
Reverse activation
energy
Enthalpy change
17
Chemistry Common Core Curriculum Map 2012-2013
3.1.1
Explain the factors that affect the rate
of a reaction (temperature,
concentration, particle size and
presence of a catalyst).
Suggested Resources by Unit
Energetics & Kinetics Notes
Reaction Rates Simulation
Rate of Reaction Lab
Kinetics: Virtual Chemistry Experiments
Energetics Practice Problems Worksheet
Peanut Calorimetry Lab
Molar Enthalpy of Solution Lab
Enthalpy of Acids & Bases Neutralization Lab
Molar Enthalpy of Neutralization Lab
Changes of State & Heating Curves Animation
Enthalpy of Fusion of Ice Lab
Calorimetry: Virtual Chemistry Experiments
(Several Kinetics Simulations)
(Several Energetics/Thermodynamics Simulations)

What are the factors that affect the rate of a chemical
reaction?
1 day
Reaction rate
Surface area
Concentration
Pressure
Temperature
Catalyst
Location of these resources
http://phet.colorado.edu/en/simulation/reactions-and-rates
http://www.chm.davidson.edu/vce/Kinetics/index.html
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/031_ChangesState.MOV
http://www.chm.davidson.edu/vce/Calorimetry/index.html
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/kinetics2/
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/thermochem/
18
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Equilibrium
Unit Number: 9
Enduring Understanding:
2.1 – Phase diagrams communicate information about phases and phase changes of chemical species at various temperatures
and pressures.
3.1 – When a system at equilibrium is subjected to a stress, the equilibrium will shift to minimize the stress on the system.
Standard
2.1.3
Interpret the data presented in phase
diagrams.
Essential Questions
Pacing
Guideline

How do phase diagrams convey information about
substances such as phase, phase changes, triple point
and critical point?
~1 day
Changes of state
Vapor pressure
Melting
Boiling
Vaporization
Condensation
Freezing
Sublimation
Deposition
Phase diagram
Critical point
Triple point
Normal melting point
Normal boiling point
Supercritical fluid
(Heating/Cooling
curves)

What does it mean to say that a chemical reaction is at
equilibrium?
~1 day

How can the position of equilibrium (the extent to which a
reaction goes to completion) be quantified using an
expression that can be simplified to one number?
Physical equilibrium
Chemical equilibrium
Dynamic equilibrium
Reversible
Equilibrium constant
(Kc)
(some overlap with and inclusion of:
2.1.1 Explain the energetic nature of phase
changes)
3.1.2
Explain the conditions of a system at
equilibrium.
Key Academic
Vocabulary
19
Chemistry Common Core Curriculum Map 2012-2013
3.1.3
Infer the shift in equilibrium when a
stress is applied to a chemical
system (Le Chatelier’s Principle).

For a system at equilibrium, what happens when the
system is subjected to a stress?

How is a shift in the position of equilibrium for a system
related to the entropy of the system?
Suggested Resources by Unit
Equilibrium Notes
Changes of State & Heating Curves Animation
States of Matter Simulation
Phase Changes: Virtual Chemistry Experiment
Le Chatelier’s Principle (Cobalt Ion Complex) Video
Equilibrium Problems Packet
Le Chatelier’s Principle Lab
Equilibrium Lab (Spectroscopy)
Equilibrium: Virtual Chemistry Experiments
~1 day
Le Chatelier’s Principle
Stress
Shift
Entropy
Catalyst
Location of these resources
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/031_ChangesState.MOV
http://phet.colorado.edu/en/simulation/states-of-matter
http://www.chm.davidson.edu/vce/PhaseChanges/index.html
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/066_LeChateliersPr.MOV
http://www.chm.davidson.edu/vce/Equilibria/index.html
20
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Solutions
Unit Number: 10
Enduring Understanding:
3.2 – The concentration and solubility of a solute dissolved in a solvent (a solution) can be determined quantitatively and
graphically.
Standard
3.2.3
3.2.4
Infer the quantitative nature of a
solution (molarity, dilution, and
titration with a 1:1 molar ratio).
Summarize the properties of
solutions.
Essential Questions

How is a solution’s concentration (molarity) related to the
amount of solute and volume of solution?

How do you determine the volume or molarity of a solution
when it is diluted with the addition of water?

What is a solution, and what are examples of each type of
solution?

What is the difference between an electrolytic and a nonelectrolytic solution?

What are colligative properties of solutions and what are
examples of them?
Pacing
Guideline
Key Academic
Vocabulary
1 day
Concentration
Molarity
Dilution
2 days
Soluble
Solute
Solvent
Solution
Homogeneous
Alloy
Aqueous
Electrolyte
Non-electrolyte
Molality
Colligative properties
Vapor pressure
Vapor pressure
reduction
Boiling point elevation
Freezing point
reduction
Osmotic pressure
21
Chemistry Common Core Curriculum Map 2012-2013
3.2.5
Interpret solubility diagrams.

How can graphs be used to communicate information
about the solubility of a solute at various temperatures?
1 day
Solubility curves
Saturated
Unsaturated
(Henry’s Law)
3.2.6
Explain the solution process.

Why does a particle ultimately dissolve or not dissolve?
1 day

For solutes that will dissolve, how does that process
occur?
Ion-dipole attractions
Heat (Enthalpy) of
solution
Endothermic
Exothermic
Suggested Resources by Unit
Solutions Notes
NaCl Electrolyte Video
Solutions Practice Worksheet
Molar Enthalpy of Solution Lab
Salts & Solubility Simulation
Henry’s Law Simulation
Molarity Simulation
Vapor Pressure Reduction Simulation
Colligative Properties Simulation
Ice Cream Lab
Freezing Point Depression Lab
Location of these resources
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/015_ELECTANDNON.MOV
http://phet.colorado.edu/en/simulation/soluble-salts
http://wps.prenhall.com/wps/media/objects/1055/1080459/media/AACXBDW0.html
http://phet.colorado.edu/en/simulation/molarity
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/propOfSoln/vp3.html
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/propOfSoln/colligative.swf
22
Chemistry Common Core Curriculum Map 2012-2013
Common Core Unit Name: Acids & Bases
Unit Number: 11
Enduring Understanding:
3.2 – Acids and bases can be distinguished based on their properties, and their concentrations can be determined in reactions
known as titrations.
Standard
3.2.1
3.2.2
Classify substances using the
hydronium and hydroxide
concentrations.
Summarize the properties of acids
and bases.
Essential Questions

What are the characteristic chemical properties and
formulas (in terms of elements or functional groups) of
acids and bases?

What is the difference between strength and concentration
for acids and bases?

What pH values are considered acidic, basic, and neutral,
and how are these values related to the exponents in their
concentrations?

How can indicator color provide information about pH of
acid and base solutions?

How are pH, pOH, [H3O+], and [OH–] calculated?

What are the differences between acids and bases in
terms of taste, touch (feel), electrical conductivity
(electrolytic nature) and effect on indicator color, for
indicators such as phenolphthalein and litmus?

How does the reaction between an acid and a metal vary,
depending on the strength or concentration of an acid, and
the relative position of the metal in the activity series?
Pacing
Guideline
Key Academic
Vocabulary
3 days
Acid
Base
Arrhenius
Bronsted
Hydronium
Hydroxide
(Conjugate acid)
(Conjugate base)
Concentration
Molarity
Strength
pH
pOH
Exponential
Indicator
Amphoteric
1 day
Indicator
Litmus
Phenolphthalein
Neutralization
Exothermic
Electrolytes
Alkali
23
Chemistry Common Core Curriculum Map 2012-2013
3.2.3
Infer the quantitative nature of a
solution (molarity, dilution, and
titration with a 1:1 molar ratio).
Suggested Resources by Unit
Acids & Bases Notes
Acids and Bases Problems Packet
Demo – Common Acids & Bases w/ Indicators
(litmus, phenolphthalein, red cabbage, etc.)
Demo – React HCl + NaOH in calorimeter
Demo – React HCl + Zn
Demo – React HCl + Na2CO3 / NaHCO3
Acid-Base Solutions Simulation
pH Scale Simulation
Strong vs. Weak Acids & Bases Animation
Strong vs. Weak Acids & Bases Animation
Strong vs. Weak Acids & Bases Animation
Vinegar Titration Lab
Citric Acid (Soft Drink) Titration Lab
Polyprotic Acid (H3PO4) Titration
(Several Acid-Base Simulations)
Acid-Base Titration Simulation

Given the volumes of both reacting species and one of
their molarities, how can the molarity of an acid or base
solution be determined from a titration?

What information can be determined from the titration
curve of a strong acid with a strong base (or strong base
with strong acid)?
1 day
Concentration
Molarity
Dilution
Titration
Standard solution
Titrant
Endpoint
Equivalence point
Titration curve
Location of these resources
http://phet.colorado.edu/en/simulation/acid-base-solutions
http://phet.colorado.edu/en/simulation/ph-scale
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/017_AQUEOUSACIDS.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/016_STRONGWEAK.MOV
http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/018_AQUEOUSBASE.MOV
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/acidbasepH/
http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/stoichiometry/a_b_phtitr.swf
24