Chemistry Curriculum Map 2016-2017 Common Core Unit Name: Atomic Theory Unit Number: 1 Enduring 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 1.1.1 Analyze 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? ~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 1
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Chemistry Curriculum Map 2016-2017
Common Core Unit Name: Atomic Theory Unit Number: 1
Enduring 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
1.1.1 Analyze 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?
~2 days AtomAtomic TheoryIsotopeCathode Ray TubeOil-Drop ExperimentGold Foil ExperimentBeryllium-Wax ExperimentNucleusProtonNeutronElectronAtomic NumberMass NumberNuclear SymbolHyphen NotationAtomic Mass UnitRelative Atomic MassAverage Atomic Mass
1.1.2 Analyze 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?
~3 days Electromagnetic SpectrumLine SpectrumEmission SpectrumContinuous SpectrumBohr ModelElectron Cloud Model
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1.1.3 Explain 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?
~2 days Wave-Particle TheoryQuantaExcited StateGround StateQuantum TheoryPhotonWavelength FrequencyEnergyPlanck’s ConstantOrbitsOrbitals
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?
Suggested Resources by Unit Location of these resources
Atomic Theory NotesThomson’s CRT Experiments AnimationMillikan’s Oil Drop Experiment Animation Millikan’s Oil Drop Experiment Animation Rutherford’s Gold Foil Experiment AnimationRutherford’s Gold Foil Experiment AnimationIsotopes and Average Atomic Mass Practice WorksheetIsotopes and Atomic Mass SimulationPenny Isotope LabPenny Isotope Lab (Advanced)Electron Cloud Simulation ActivityObserving Spectral Lines Flame Test For Different Metals Animation Chem Alive! Field Trips CD – The Chemistry of FireworksFlame Test LabWebsite that summarizes development of atomic theory, including animationsWebsite with animation explaining electron configurationsElectron Configuration Practice WorksheetAtomic Theory Review
(Demonstration using gas discharge tubes and spectrophotometers)http://cwx.prenhall.com/petrucci/medialib/media_portfolio/text_images/039_FlameTestsMet.MOVChem 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
1.1.4 Explain 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?
~3 days RadiationNuclear decayAlpha radiationBeta radiationGamma radiationDecay equationsHalf-lifeFissionFusion
Suggested Resources by Unit Location of these resources
The Atomic Nucleus & Radioactivity NotesRutherford’s Experiment AnimationCloud Chamber LabChem Alive! Field Trips CD - Fusion and FissionNuclear Fission SimulationAtomic Nucleus and Radioactivity Practice WorksheetAtomic Nucleus and Radioactivity Review
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
1.3.1 Classify 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?
~1 day Periodic TablePeriodGroup/FamilyMetalMetalloidNonmetalTransition metal/element
1.3.2 Infer 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?
~2 days Atomic RadiusValence ElectronsIonic RadiusIonCationAnionIonization EnergyElectronegativityOctetElectron Affinity
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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 electronegativity difference between the atoms.
Standard Essential Questions Pacing Guideline
Key Academic Vocabulary
1.2.1 Compare (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?
3 days Covalent BondIonic BondMetallic BondOctetCationAnionFormula UnitMoleculeDiatomicSingle BondDouble BondTriple Bond
Suggested Resources by Unit Location of these resources
Bonding NotesFormation of NaCl MovieBond Formation in Hydrogen AnimationBonding Practice Worksheet WSProperties of Ionic & Covalent Compounds LabProperties of Ionic & Covalent Compounds Lab #2VSEPR Geometries WSMarshmallow Molecules ActivityMolecular Shapes SimulationOrganic Macromolecule Construction Activity (can be adapted to simpler molecules)Molecular Polarity SimulationDemonstration – Balloon/Static Electricity/Polarity of WaterDemonstration – Drops of Water on a Penny (H-bonding)Ink Chromatography LabPlant Pigment Chromatography LabTLC 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
1.2.4 Interpret 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?
3 days Monatomic ionsPolyatomic ionsNomenclatureCationAnionBinary compoundTernary compoundStock systemBinary acidOxyacid
2.2.2 Analyze the evidence of chemical What are some evidences that a chemical reaction has 1 day Precipitate9
Chemistry Curriculum Map 2016-2017
change. occurred?
What tests can you do to determine if oxygen, hydrogen, carbon dioxide or water have been produced in a chemical reaction?
Solubility rulesEndothermicExothermicDilution Burning splint testLime water testCobalt(II) chloride test
2.2.3 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).
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?
Suggested Resources by Unit Location of these resourcesChemical Nomenclature, Equations & Reactions NotesNomenclature Practice WorksheetBalancing Chemical Equations SimulationSynthesis of Aluminum Bromide VideoSynthesis of Sodium Chloride VideoSingle Replacement of Copper By Silver Ions VideoDemo – 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 WorksheetBalancing Equations Worksheet – Extra PracticeNomenclature, 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
2.2.4 Analyze 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?
8 days StoichiometryMole Avogadro’s numberMolar massAtomsMolecules Formula unitsMole ratioSTPSATPAvogadro’s lawStandard molar volumeLimiting reactantPercent yield Actual yieldTheoretical yield
2.2.5 Analyze quantitatively the How do you calculate the empirical and molecular formula 3 days Empirical formula
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composition of a substance (empirical formula, molecular formula, percent composition, and hydrates).
of a compound?
How do you determine the percentage composition by mass of a compound?
What is a hydrate?
Molecular formulaPercentage composition by massHydrate
Suggested Resources by Unit Location of these resources
Stoichiometry NotesStoichiometry Worksheet PacketThe Mole LabPercent Composition of Hydrates LabEmpirical Formula Lab (EF of Zinc Chloride)Limiting Reagent Lab (Vinegar & Baking Soda)Limiting Reactant / % Yield LabEmpirical Formula of a Hydrate SimulationReaction Stoichiometry Simulation
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
2.1.5 Explain 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
6 days Ideal gasReal gasStandard temperature and pressure (STP)Kinetic-molecular theory (KMT)Avogadro’s lawmm Hg / torrAtmospheresKilopascalsBoyle’s lawCharles’ lawGay-Lussac’s lawCombined gas lawIdeal Gas lawDalton’s law of partial PressuresBarometric pressure
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the total pressure and partial pressures of the other component gases in a mixture?
Water vapor pressure
Suggested Resources by Unit Location of these resources
Gases NotesGas Laws Problems Worksheet #1Gas Laws Problems Worksheet #2Water Vapor Pressure TableDemo – 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 DemonstrationsBoyle’s Law Microscale InvestigationDemo: Boyle’s Law With MarshmallowsGas Properties SimulationInvestigating Boyle’s Law Simulation/LabDetermining the Molar Mass of Butane LabAlka-Seltzer & The Ideal Gas Law LabGas Laws: Virtual Chemistry ExperimentKinetic-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
2.1.1 Explain 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?
1 day Kinetic energyPotential energyHeatTemperatureCelsiusKelvinJoulePhase changeChange of stateMeltingFreezing
Chm.2.1 Understand the relationship among pressure, temperature, volume, and phase. Phase diagrams communicate information about phases and phase changes of chemical species at various temperatures and pressures.
Chm.3.1 Understand the factors affecting rate of reaction and chemical equilibrium. When a system at equilibrium is subjected to a stress, the equilibrium will shift to minimize the stress on the system.
Standard Essential Questions Pacing Guideline
Key Academic Vocabulary
2.1.3 Interpret the data presented in phase diagrams.
(some overlap with and inclusion of:2.1.1 Explain the energetic nature of phase changes)
How do phase diagrams convey information about substances such as phase, phase changes, triple point and critical point?
~1 day Changes of stateVapor pressureMeltingBoilingVaporizationCondensationFreezingSublimationDepositionPhase diagramCritical pointTriple pointNormal melting pointNormal boiling point
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Supercritical fluid(Heating/Cooling curves)
3.1.2 Explain the conditions of a system at equilibrium.
What does it mean to say that a chemical reaction is at equilibrium?
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?
~1 day Physical equilibriumChemical equilibriumDynamic equilibriumReversibleEquilibrium constant (Kc)
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?
~1 day Le Chatelier’s PrincipleStress ShiftEntropy Catalyst
Suggested Resources by Unit Location of these resources
Equilibrium NotesChanges of State & Heating Curves AnimationStates of Matter SimulationPhase Changes: Virtual Chemistry ExperimentLe Chatelier’s Principle (Cobalt Ion Complex) VideoEquilibrium Problems PacketLe Chatelier’s Principle LabEquilibrium Lab (Spectroscopy)Equilibrium: Virtual Chemistry Experiments
Chm.3.2 Understand solutions and the solution process. The concentration and solubility of a solute dissolved in a solvent (a solution) can be determined quantitatively and graphically.
Standard Essential Questions Pacing Guideline
Key Academic Vocabulary
3.2.3 Infer the quantitative nature of a solution (molarity, dilution, and titration with a 1:1 molar ratio).
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?
1 day ConcentrationMolarityDilution
3.2.4 Summarize the properties of solutions.
What is a solution, and what are examples of each type of solution?
What is the difference between an electrolytic and a non-electrolytic solution?
What are colligative properties of solutions and what are examples of them?
2 days SolubleSoluteSolventSolutionHomogeneousAlloyAqueousElectrolyteNon-electrolyteMolalityColligative propertiesVapor pressure
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Vapor pressure reductionBoiling point elevationFreezing point reduction Osmotic pressure
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 curvesSaturatedUnsaturated(Henry’s Law)
3.2.6 Explain the solution process. Why does a particle ultimately dissolve or not dissolve?
For solutes that will dissolve, how does that process occur?
1 day Ion-dipole attractionsHeat (Enthalpy) of solutionEndothermicExothermic
Suggested Resources by Unit Location of these resources
Solutions NotesNaCl Electrolyte VideoSolutions Practice WorksheetMolar Enthalpy of Solution LabSalts & Solubility SimulationHenry’s Law SimulationMolarity SimulationVapor Pressure Reduction SimulationColligative Properties Simulation Ice Cream LabFreezing Point Depression Lab
Common Core Unit Name: Acids & Bases Unit Number: 11
Enduring Understanding:
Chm.3.2 Understand solutions and the solution process.
Acids and bases can be distinguished based on their properties, and their concentrations can be determined in reactions known as titrations.
Standard Essential Questions Pacing Guideline
Key Academic Vocabulary
3.1.4 Classify substances using the hydronium and hydroxide concentrations.
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?
3 days AcidBaseArrheniusBronstedHydroniumHydroxide(Conjugate acid)(Conjugate base)ConcentrationMolarityStrengthpHpOHExponentialIndicatorAmphoteric
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3.1.5 Summarize the properties of acids and bases.
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?
How does the strength of an acid or base affect its ability to conduct electricity?
1 day IndicatorLitmusPhenolphthaleinNeutralizationExothermicElectrolytes Alkali
3.1.6 Infer the quantitative nature of a solution (molarity, dilution, and titration with a 1:1 molar ratio).
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 ConcentrationMolarityDilutionTitrationStandard solutionTitrant EndpointEquivalence point Titration curve
Suggested Resources by Unit Location of these resources