Chemistry Curriculum Map 2016-2017
Common Core Unit Name: Atomic Theory Unit Number: 1Enduring Understanding:
Chm.1.1 Analyze the structure of atoms and ions.
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 / Essential Questions / Pacing Guideline / Key Academic Vocabulary
1.1.1Analyze the structure of atoms, isotopes, and ions. /
- 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?
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
1.1.2Analyze an atom in terms of the location of electrons. /
- 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?
Line Spectrum
Emission Spectrum
Continuous Spectrum
Bohr Model
Electron Cloud Model
1.1.3Explain the emission of electromagnetic radiation in spectral form in terms of the Bohr model. /
- 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?
Quanta
Excited State
Ground State
Quantum Theory
Photon
Wavelength
Frequency
Energy
Planck’s Constant
Orbits
Orbitals
1.3.2 Infer the atomic size, reactivity,
electronegativity, and ionization
energy of an element from its position
on the Periodic Table. /
- How do you illustrate electron configurations of elements?
- How is oxidation number related to the number of valence electrons?
(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
Suggested Resources by Unit / Location of these resources
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 /
(Demonstration using gas discharge tubes and spectrophotometers)
Chem Alive! Field Trips CD
Common Core Unit Name: The Atomic Nucleus & Radioactivity Unit Number: 2
Enduring Understanding:
Chm.1.1 Analyze the structure of atoms and ions.
Radioactive isotopes have unstable nuclei that undergo predictable nuclear decay processes.
Standard / Essential Questions / Pacing Guideline / Key Academic Vocabulary
1.1.4Explain the process of radioactive decay using nuclear equations and half-life. /
- 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?
Nuclear decay
Alpha radiation
Beta radiation
Gamma radiation
Decay equations
Half-life
Fission
Fusion
Suggested Resources by Unit / Location of these resources
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 /
Common Core Unit Name: Periodicity Unit Number: 3
Enduring Understanding:
Chm.1.3 Understand the physical and chemical properties of atoms based on their position on the Periodic Table.
The physical and chemical properties of an element can be predicted based upon their location on the Periodic Table.
Standard / Essential Questions / Pacing Guideline / Key Academic Vocabulary
1.3.1Classify the components of a periodic table (period, group, metal, metalloid, nonmetal, transition). /
- 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?
Period
Group/Family
Metal
Metalloid
Nonmetal
Transition
metal/element
1.3.2Infer the physical properties (atomic radius, metallic and nonmetallic characteristics) of an element based on its position on the Periodic Table. /
- 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?
- Where are the atoms with the highest ionization energy located within a group on the periodic table? What is the period trend?
- How do you explain the trend for electronegativity of elements on the periodic table within a group and period?
- How does the size of a cation and anion compare to a neutral atom?
Valence Electrons
Ionic Radius
Ion
Cation
Anion
Ionization Energy
Electronegativity
Octet
Electron Affinity
Common Core Unit Name: Bonding Unit Number: 4
Enduring Understanding:
Chm.1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties
Elements form different types of bonds and attractions based on the nature of elements and the electronegativitydifference between the atoms.
Standard / Essential Questions / Pacing Guideline / Key Academic Vocabulary
1.2.1Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds. /
- 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?
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
1.2.2Infer the type of bond and chemical formula formed between atoms. /
- 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?
Bond
Polar Covalent Bond
Ionic Character
Covalent Character
1.2.3Compare inter- and intra-particle forces. /
- 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)?
Bond Enthalpy
Intermolecular Forces
Dipole-Dipole Forces
Hydrogen Bonding
van der Waals’ Forces
London Dispersion
Forces
Instantaneous Dipole
Induced Dipole
Ion-Dipole Attractions
1.2.5Compare the properties of ionic, covalent, metallic, and network compounds. /
- 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?
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
Suggested Resources by Unit / Location of these resources
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/StaticElectricity/Polarity of Water
Demonstration – Drops of Water on a Penny (H-bonding)
Ink Chromatography Lab
Plant Pigment Chromatography Lab
TLC Plant Pigment Chromatography Lab /
Common Core Unit Name: Chemical Nomenclature, Equations & Reactions Unit Number: 5
Enduring Understanding:
Chm.1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties
Compounds are named based upon the type of bond they form.
Chm.2.2 Analyze chemical reactions in terms of quantities, product formation, and energy.
Chemical species undergo characteristic chemical changes, but mass is conserved in their reactions.
Standard / Essential Questions / Pacing Guideline / Key Academic Vocabulary
1.2.4Interpret the name and formula of compounds using IUPAC convention. /
- 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?
Polyatomic ions
Nomenclature
Cation
Anion
Binary compound
Ternary compound
Stock system
Binary acid
Oxyacid
2.2.2Analyze the evidence of chemical change. /
- 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?
Solubility rules
Endothermic
Exothermic
Dilution
Burning splint test
Lime water test
Cobalt(II) chloride test
2.2.3Analyze the law of conservation of matter and how it applies to various types of chemical equations (synthesis, decomposition, single replacement, double replacement, and combustion). /
- How do you write and balance chemical equations?
- Why do chemical equations need to be balanced?
- 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?
- 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?
Products
Balanced equation
Synthesis
Decomposition
Single replacement
Double replacement
Combustion
Activity series
Solubility rules
Acid-base
neutralization reaction
Ionic equation
Net ionic equation
Dissociation
Spectator ions
Hydrocarbons
Suggested Resources by Unit / Location of these resources
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 SilverIons 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 /
Common Core Unit Name: Stoichiometry Unit Number: 6
Enduring Understanding:
Chm.2.2 Analyze chemical reactions in terms of quantities, product formation, and energy.
The composition of chemical species and the reactions they undergo can be described quantitatively.
Standard / Essential Questions / Pacing Guideline / Key Academic Vocabulary
2.2.4Analyze the stoichiometric relationships inherent in a chemical reaction. /
- 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?
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
2.2.5Analyze quantitatively the composition of a substance (empirical formula, molecular formula, percent composition, and hydrates). /
- 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?
Molecular formula
Percentage
composition by mass
Hydrate
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 /
Common Core Unit Name: Gases Unit Number: 7
Enduring Understanding:
Chm.2.1 Understand the relationship among pressure, temperature, volume, and phase.
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 / Essential Questions / Pacing Guideline / Key Academic Vocabulary
2.1.5Explain the relationships among pressure, temperature, volume, and quantity of gas, both qualitative and quantitative. /
- What are the characteristics of an ideal gas?
- How do ideal gases differ from real gases?
- How does KMT explain the behavior of gases?
- How do you determine what value of R to use when using the ideal gas law equation?
- 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?
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
Suggested Resources by Unit / Location of these resources
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) /
Common Core Unit Name: Energetics & Kinetics Unit Number: 8
Enduring Understanding:
Chm.2.1 Understand the relationship among pressure, temperature, volume, and phase.
The energetic nature of substances undergoing phase changes can be described using phase diagrams.
Chm.2.2 Analyze chemical reactions in terms of quantities, product formation, and energy.
Chemical species undergo characteristic chemical changes, but mass is conserved in their reactions.Molecules must collide in a specific manner in order for a reaction to occur.
Chm.3.1 Understand the factors affecting rate of reaction and chemical equilibrium.
The rate of a chemical reaction is affected by factors including temperature, concentration, particle size and presence of a catalyst.
Standard / Essential Questions / Pacing Guideline / Key Academic Vocabulary
2.1.1Explain the energetic nature of phase changes. /
- 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?
Potential energy
Heat
Temperature
Celsius
Kelvin
Joule
Phase change
Change of state
Melting
Freezing
Evaporation
Boiling
Vaporization
Condensation
Sublimation
Deposition
Heating & cooling
curve
2.1.2Explain heating and cooling curves (heat of fusion, heat of vaporization, heat, melting point, and boiling point). /
- 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?
- How do you determine the enthalpy change in a substance that is being heated, cooled or changing state?
- What is the difference between an endothermic and exothermic process?