Curriculum Map 2012-2013 South Henry School Corporation Robinson, Michael / Chemistry I / Grade 10 (Tri jr/sr High School) Wednesday, November 20, 2013 Standards & Indicators Essential Questions Content Skills Assessment Activities / Strategies Differentiated Instruction Resources Matter and Change (Week 1, 4 Weeks) Science (2010), Grades 10-12 , Chemistry I The Nature of Science Develop explanatio ns based on reproducib le data and observatio ns gathered during laboratory investigat ions. Recognize that their explanatio ns must be based both on their data and other known informatio n from investigat ions of others. Clearly communicat e their ideas and results of investigat ions verbally and in written form using tables, graphs, diagrams and photograph s. Apply standard What is a chemical? Why classify things? What does it mean for something to change? How can you communicate with mathematics? Physical and Chemical Properties Physical and Chemical Changes Classification of Matter Density Significant Digits Metric Conversions Using Factor Label Distinguish between physical and chemical properties. Distinguish between physical and chemical changes. Propose scientific hypotheses Use models to explain different properties of solids, liquids, and gases. Classify matter as heterogeneous or homogeneous. Distinguish between heterogeneous mixtures, solutions, and pure substances. Distinguish between elements and compounds Discuss properties and techniques that can be used to determine whether matter is a mixture or a pure substance. Explain the difference between distillation and electrolysis. Distinguish between elements and Bell Work Other written assessments Each class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period. Physical and Chemical Lab Report Lab Assignment Lesson Plan Available in Links Day 1 Demonstrations of Physical and Chemical Changes and Properties Writing Observations Day 2 Physical and Chemical Lab (Day 1) Day 3 Complete Physical and Chemical Lab Day 4 Using Factor label to convert metric units Day 5 Factor Label Worksheet Non-metric conversions Day 6 Classification of Matter Factor Label Worksheet III Day 7 Classification of Matter Activity Day 8 Element and Compound Notes Day 9 Significant Digit Notes Conductivity Demonstration Assignment: p32: 12; p39: 31, 32; p41: 33, 34 Day 10 Poster board activity Day 11 Density Calculations Day 12 Density Lab Day 13 Lab Calculations Distillation and Electrolysis Day 14 Accuracy and Precision Oxygen in Air lab Day 15 Complete Lab Calculations Day 16 Review for Unit Test Day 17 Unit Test Syllabus: Matter and Math Unit Schedule Matter and Change Lesson Plans Differentiation by Content Varied supple mentar y materi als Some Resources Available on Moodle Site for Chemistry I H Factor Label Worksheet I (Metric) Factor Label Worksheet II (Non-metric) Factor Label Worksheet III (Squared and Cubed) Physical and Chemical Lab Activity Signficant Digits Notes Density Notes Elements and Compounds Notes Separation Techniques Notes Test Review Questions Test Review Worksheet
Transcript
Curriculum Map 2012-2013South Henry School CorporationRobinson, Michael / Chemistry I / Grade 10 (Tri jr/sr High School)Wednesday, November 20, 2013
Science (2010), Grades 10-12 , Chemistry IThe Nature of Science
Develop explanations based on reproducible data and observations gathered during laboratory investigations.
Recognize that their explanations must be based both on their data and other known information from investigations of others.
Clearly communicate their ideas and results of investigations verbally and in written form using tables, graphs, diagrams and photographs.
Apply standard techniques in laboratory investigations to measure physical quantities in appropriate units and convert quantities to other units as necessary.
Use
What is a chemical?Why classify things?What does it mean for something to change?How can you communicate with mathematics?
Physical and Chemical Properties
Physical and Chemical Changes
Classification of Matter
Density Significant Digits Metric
Conversions Using Factor Label
Distinguish between physical and chemical properties.
Distinguish between physical and chemical changes.
Propose scientific hypotheses
Use models to explain different properties of solids, liquids, and gases.
Classify matter as heterogeneous or homogeneous.
Distinguish between heterogeneous mixtures, solutions, and pure substances.
Distinguish between elements and compounds
Discuss properties and techniques that can be used to determine whether matter is a mixture or a pure substance.
Explain the difference between distillation and electrolysis.
Distinguish between elements and compounds on the submicroscopic level using the atomic model.
Contrast compounds and mixtures using the law of definite composition.
Define and distinguish between ions and molecules.
Define and distinguish between metals, nonmetals, and metalloids.
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.Physical and Chemical Lab ReportLab Assignment
Lesson Plan Available in Links Day 1 Demonstrations of Physical and Chemical Changes and Properties Writing ObservationsDay 2 Physical and Chemical Lab (Day 1)Day 3 Complete Physical and Chemical LabDay 4 Using Factor label to convert metric unitsDay 5 Factor Label Worksheet Non-metric conversionsDay 6 Classification of Matter Factor Label Worksheet IIIDay 7 Classification of Matter ActivityDay 8 Element and Compound NotesDay 9 Significant Digit Notes Conductivity Demonstration Assignment: p32: 12; p39: 31, 32; p41: 33, 34Day 10 Poster board activityDay 11 Density CalculationsDay 12 Density LabDay 13 Lab Calculations Distillation and ElectrolysisDay 14 Accuracy and Precision Oxygen in Air labDay 15 Complete Lab CalculationsDay 16 Review for Unit TestDay 17 Unit Test
Syllabus: Matter and Math Unit Schedule
Matter and Change Lesson Plans
Differentiation by Content
Varied supplementary materials
Some Resources Available on Moodle Site for Chemistry I H
analogies and models (mathematical and physical) to simplify and represent systems that are difficult to understand or directly experience due to their size, time scale or complexity. Recognize the limitations of analogies and models.
Standard 1: Properties and States of MatterDescribe the nature of physical and chemical properties and changes of matter.
C.1.1 Based on physical properties, differentiate between pure substances and mixtures.
C.1.2 Observe and describe chemical and physical properties of different types of matter and designate them as either extensive or intensive.
C.1.3 Recognize observable indicators of chemical changes.
C.1.4 Describe physical and chemical changes at the molecular
List the diatomic elements (hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, and iodine).
Recognize the meaning of kilo-, deci-, centi- and milli-
Apply factor label to converting metric units.
Write a conclusion summarizing laboratory exercises.
Use significant digits to represent answers to scientific calculations.
Calculate density by using problem solving strategies.
Compare and contrast states of matter at the molecular level.
C.1.7 Define density and distinguish among materials based on densities. Perform calculations involving density.
Atomic Theory(Week 5, 2 Weeks)
Science (2010), Grades 10-12 , Chemistry IStandard 2: Atomic Structure and the Periodic TableDescribe how the properties and arrangements of the subatomic particles contribute to the structures of atoms.
C.2.1 Describe how models of atomic structure changed over time based on available experimental evidence and understand the current model of atomic structure.
C.2.2 Describe how the subato
Why should we believe in atoms?What evidence exists that matter is electrical?What things can't be detected with human senses?Is radioactivity good or bad?
Atomic Models Protons,
Neutrons and Electrons
Atomic Number Atomic Mass Isotopes Radioactivity Alpha, Beta and
Gamma Radiation
Fission and Fusion
Half Life Calculations for Radioactive Decay
Evaluate the factors that influence the deflection of a charged particle.
Compare and contrast the atomic models of Dalton and Thomson.
Explain Millikan’s Oil Drop Experiment and its importance in the story of the atom.
Differentiate between atoms and ions.
Explain the experiment of Becquerel that led to the discovery of radioactivity. Know that Ernest Rutherford described the three types of radioactivity. Identify the characteristics of alpha, beta, and gamma radiation.
Analyze how Rutherford’s atomic model explains the results of his gold foil experiment. Discuss the alpha bombardment of
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Day 1 Atoms Notes IDay 2 Atoms Notes II Atom MathDay 3 Law of Definite Proportions LabDay 4 Nuclear Atom WorksheetDay 5 Bead Isotope ActivityDay 6 Proton, Neutron, Electron Quiz Average Atomic Mass WorksheetDay 7 Type of Radioactivity Notes Nuclear Equations WorksheetDay 8 Review WorksheetDay 9 Review ActivityDay 10 Unit Test
Syllabus Unit II Atoms
Atomic Theory Lesson Plans
Some Resources Available on Moodle Site for Chemistry I H
Atomic Scientists PowerPoint
Atom Notes
Atom Unit Review Worksheet
Counting Protons, Neutron and Electrons Review
Mathematics with Atoms Notes and Worksheet
Explaining the Difference Between Definite and Multiple Proportions
mic particles (i.e., protons, neutrons and electrons) contribute to the structure of an atom and recognize that the particles within the nucleus are held together against the electrical repulsion of the protons.
C.2.7 Compare and contrast nuclear reactions with chemical reactions.
C.2.8. Describe how fusion and fission processes transform elements present before the reaction into elements present after the reaction.
C.2.9 Understand that the radioactive
beryllium experiment of Irene Curie that led to Chadwick’s discovery of the neutron.
Identify the characteristics of subatomic particles.
Distinguish between atomic number and mass number. Define isotope and write isotopic symbols. Be able to calculate average atomic mass from mass spectrometer data.
Determine the number of protons, neutrons, and electrons in an isotope from its name or symbol.
Explain the differenece between nuclear fusion and fission.
Calculate the amount of material remaining after a certain number of half-lives have passed.
decay process is random for any given atom but that this property leads to a predictable and measurable exponential decay of a sample of radioactive material. Know how to calculate the initial amount, the fraction remaining or the half-life of a radioactive isotope when given two of the other three variables.
Describe how the structure of the periodic table reflects the numbers of electrons and protons and the configuration of electrons in an atom.
C.2.3 Determine the number of protons, neutrons, and electrons in
isotopes and in those isotopes that comprise a specific element. Relate these numbers to atomic number and mass number.
C.2.4 Calculate the average atomic mass of an element from isotopic abundance data.
Electrons and the Periodic Table(Week 7, 3 Weeks)
Science (2010), Grades 10-12 , Chemistry IDescribe how the structure of the periodic table reflects the numbers of electrons and protons and the configuration of electrons in an atom.
C.2.5 Write the electron configuration of an element and relate this to its position on the periodic table.
C.2.6 Use the periodic
What quantities may only have certain values?What is light?What is color?How can you know that something changes its energy?Does your family define you?
Bright Line Spectrum
Flame Tests Quantum Theory
of Atoms Electron
Configurations Periodic Table Valence
Electrons Atomic Radii Ionization
Energy
Describe properties of waves: amplitude, frequency, and wavelength.
Explain the relationship between energy and the frequency of light.
Compare and contrast different regions of the electromagnetic spectrum.
Explain how the bright-line spectrum of hydrogen demonstrates the quantized nature of energy.
Predict the position(s) of electrons in an atom, using the concepts of quantum numbers and orbitals.
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Day 1 Electromagnetic Spectrum NotesDay 2 Flame Tests; Bohr Model Notes Assignment: p121: 1-4; p124: 5bDay 3 Pencil Drop Activity Orbital Model NotesDay 4 Electron configuration notesDay 5 Electron Configuration Connect the Dots WorksheetDay 6 Cloud Model Worksheet Electron Configuration BingoDay 7 Electron Configurations from the Periodic Table p147: 79 a-h; 80Day 8 Concise Electron Configurations Periodic Table WorksheetDay 9 Electron Configuration Quiz Periodic Table Simulator ActivityDay 10 Periodicity Self Quiz Characteristics of Elements WorksheetDay 11 First Ionization Energy Notes
Some Resources Available on Moodle Site for Chemistry I H
Science (2010), Grades 10-12 , Chemistry IStandard 3: Bonding and Molecular StructureDescribe how the configuration of electrons within an atom determines its interactions with other atoms.
C.3.4 Write chemical formulas for ionic compounds given their names and vice versa.
Why should chemists agree on rules for naming compounds?
Why do elements only combine in certain ratios?
Binary Ionic Formulas
Binary Ionic Names
Ionic Compounds containing Polyatomic Ions
Stock System Binary Molecular
Formulas Binary Molecular
Names
Write the formulas for binary ionic compounds given the ions in the compound.
Write the names of binary ionic compounds given the ions present.
Write the formula for binary ionic compounds given the name of the compound.
Write the formulas and charges for ten polyatomic ions: nitrate, nitrite, sulfate, sulfite, carbonate, phosphate, acetate, hydroxide, cyanide, and ammonium.
Write the formula for ionic compounds containing polyatomic ions given the ions in the compound.
Write the names of ionic compounds containing polyatomic ions given the ions present.
Write the formulas for ionic compounds given the name of the compounds.
Write the name for molecular compounds in both the prefix systems.
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Day 1 Binary Ionic Compound Formula WritingDay 2 Binary Ionic Quiz Polyatomic Ions (formula writing)Day 3 Name to Formula Notes p226: 29-33; p236-237: 67, 74-78Day 4 Containing Polyatomic Ion Quiz Nomenclature WorksheetDay 5 Chemical Formula Crossword WorksheetDay 6 Binary Molecular Compound Notes Binary Molecular WorksheetDay 7 Chemical Formula Problems Crossword IIDay 8 Nomenclature BingoDay 9 Unit Test
Syllabus Unit IV: Chemical Formulas
Chemical Formulas Lesson Plans
Some Resources Available on Moodle Site for Chemistry I H
Chemistry IStandard 4: Reactions and StoichiometryUse balanced chemical equations and the mole concept to determine the quantities of reactants and products.
C.4.1 Predict products of simple reactions such as synthesis, decomposition, single replacement and double replacement.
C.4.2 Balance chemical equations using the law of conservation of mass and use them to describe chemical reactions.
C.4.5 Describe, classify and give examples of various kids of reactions-synthesis (i.e., combination), decomposition, single displacement,
chemical reaction?How can you know that a chemical reaction has taken place?
Chemical Equations
Endothermic and Exothermic Reactions
Types of Chemical Reactions
Predicting Products for Chemical Reactions
Ionic and Net Ionic Equations
Oxidation Numbers
Oxidation-Reduction (Redox) Reactions
chemical reactions by macroscopic observations.
Define energy and differentiate between kinetic and potential energy.
Explain the difference between endothermic and exothermic reactions.
Interpret the meaning of symbols in chemical equations.
Describe chemical reactions by writing balanced chemical equations.
Classify reactions as belonging to one of five general types: combustion, single replacement, double replacement, synthesis, and decomposition.
Predict the products of a reaction from the reactants.
Differentiate between decomposition reactions and dissociation.
Determine by using an activity series whether a single replacement reaction will occur.
Determine by using a table of solubility whether a combination of aqueous solutions will produce a precipitate.
Write ionic and net ionic equations for precipitation reactions.
Determine the
written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Day 1 Household Chemical LabDay 2 Balancing Chemical EquationsDay 3 Types of Chemical Reactions NotesDay 4 Parts 1, 2 and 3 of Types of Chemical Reactions LabDay 5 Review Observations for the Types of Chemical ReactionsDay 6 Combustion, Synthesis and Decomposition Notes Assignment: p289: 21-23; p305: 88Day 7 Page 1 of Single Replacement ActivityDay 8 Complete Procedures for Unknown Analysis 2 Single Replacement QuizDay 9 Predicting Double Replacment Notes 1-10 of Double Replacement WorksheetDay 10 Double Replacment Dissociation notes parts b and c of Double Replacement NotesDay 11 Complete Procedures for Precipitation ActivityDay 12 Complete Predicting Reactions worksheetDay 13 Ionic Equation Quiz Chemical Equation CrosswordDay 14 Review Worksheet and p307: 1-8Day 15 Unit TestDay 16 Oxidation Numbers p642: 4, 5; p643: 8, 9 p658: 44, 46, 47, 49Day 17 Metal and Voltage Lab Activity p658: 50, 51Day 18 Oxidation Number Quiz
C.4.6 Determine oxidation states and identify the substances gaining and losing electrons in redox reactions.
Standard 6: ThermochemistryRecognize that chemical reactions result in either the release or absorption of energy.
C.6.3 Classify chemical reactions and phase changes as exothermic or endothermic.
oxidation number for elements in the elemental state and in compounds.
Identify which elements have lost electrons and which have gained electrons.
The Mole(Week 16, 5 Weeks)
Science (2010), Grades 10-12 , Chemistry IStandard 4: Reactions and StoichiometryUse balanced chemical equations and the mole concept to determine the quantities of reactants and products.
C.4.3 Given
How can you count things as small as atoms?How can we know the ratio of elements in a compound?How could we find the mass of a single atom?
The Mole Avogadro's
Number Converting
Mass, Molecules and Moles
Molarity Percent
Composition Empirical
Formulas Molecular
Formulas
Define the term mole and describe how it is used in chemistry.
Explain and calculate molar mass.
Convert mass to moles and moles to mass.
Calculate equivalents among grams, moles, and number of particles.
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Day 1 Molar Mass NotesDay 2 Mole Conversion WorksheetDay 3 Whole Mole Activity Avogadro WorksheetDay 4 Molarity Notes and worksheetDay 5 Molarity Lab Activity p465: 15, 16; p466: 17Day 6 Molarity Quiz Percent Composition and Empirical Formula p331: 42, 43; p333: 46, 47Day 7 Empirical Formula LabDay 8 Empirical and Molecular
Some Resources Available on Moodle Site for Chemistry I H
mass of the sample, use the mole concept to determine the number of moles and number of atoms or molecules in samples of elements and compounds.
C.4.7 Perform calculations to determine the composition of a compound or mixture when given the formula.
Hydrates Define and solve problems for parts per million descriptions of solutions.
Calculate the amount of a compound in a given volume of solution, using the concept of molarity.
Explain how to prepare molar solutions.
Calculate percent composition by mass and use it to compare compounds.
Determine empirical formulas.
Determine molecular formulas.
Define and identify formulas for hydrates.
Calculate the formula for a hydrate with data of water and salt content.
Formula WorksheetDay 9 Empirical and Molecular Formula Quiz Review WorksheetDay 10 Calculation Review WorksheetDay 11 Unit TestDay 12 Hydrate Notes and AssignmentDay 13 Hydrate Lab Activity Hydrate Quiz
The Mole Lesson Plans
Syllabus: The Mole
Finals Semester 1(Week 19, 1 Week)
Stoichiometry(Week 21, 3 Weeks)
Science (2010), Grades 10-12 , Chemistry ICompare and contrast states of matter at the molecular level.
C.1.6 Explain and apply the law of conservation of mass as it
When do you need to calculate how much is something is used or made?How can you predict how much of a substance in made in a reaction?Why might the actual amount of something produced be different than the amount predicted?
Stoichiometry Calculations
Limiting Reagent
Percent Yield
Convert from moles of one species in a reaction to moles of another given balanced chemical equation.
Convert from mass of one species to mass of another given a balanced equation.
Calculate the percentage yield of a reaction given experimental
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Day 1 Stoichiometry Notes p379: 61-63Day 2 Stoichiometry Highway NotesDay 3 Stoichiometry labDay 4 Stoichiometry WorksheetDay 5 Stoichiometry Quiz Percent Yield p381: 84-86Day 6 Stoichiometry with Molarity Notes Stoichiometry with Molarity WorksheetDay 7 Stoichiometry with Molarity LabDay 8 Complete lab Molarity Worksheet II
Some Resources Available on Moodle Site for Chemistry I H
Standard 4: Reactions and StoichiometryUse balanced chemical equations and the mole concept to determine the quantities of reactants and products.
C.4.3 Given mass of the sample, use the mole concept to determine the number of moles and number of atoms or molecules in samples of elements and compounds.
C.4.4 Using a balanced chemical equation, calculate the quantities of reactants needed and products made in a chemical reaction that
data. Perform
stoichiometry calculations for reactions in aqueous solution given molarity and volume of a reactant.
Determine the theoretical yield of a reaction given experimental data.
Determine the limiting reagent for a reaction.
Day 9 Stoichiometry with Molarity Quiz Limiting Reagent NotesDay 10 Limiting Reagent AssignmentDay 11 Limiting Reagent Quiz Stoichiometry Review WorksheetDay 12 Review ActivityDay 13 Unit Test
Science (2010), Grades 10-12 , Chemistry IIdentify the factors that qualitatively affect solubility, reaction rates and dynamic equilibrium.
C.7.6 Write equilibrium expressions for reversible reactions.
Standard 8: Acids and BasesUse acid-base definitions to identify acids and bases when given their formulas and reactions.
C.8.1 Use Arrhenius and Brønsted-Lowry definitions to classify substances as acids or bases.
C.8.2 Describe the characteristic properties of acids and bases.
C.8.3 Compare and contrast the dissociation and
Where do you hear about acids and bases?What are some processes that are reversible?How can we know that a reaction is finished?
Arrhenius Acid-Base Theory
Bronsted-Lowry Acid-Base Theory
Titrations Equilibrium
Constants Strong Acid
Dissociation Weak Acid
Dissociation pH
Define the Arrhenius concept of an acid and base.
Define the Bronsted-Lowry concept of an acid and base.
Write an acid dissociation equation for a strong acid.
Write an acid dissociation equation for a weak acid.
Write an equilbrium expression for a reversible reaction.
Describe titration and calculate the concentration of an acid or base, using the results of titration.
Calculate the pH for strong acid and strong base solutions.
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Titration Lab Day 1: Standardization of NaOH Day 2: Molarity of VinegarTitration QuizAcid-Base Notes and AssignmentEquilibrium Expression Notes and AssignmentpH Notes and AssignmentpH Lab ActivityTest: Acids and Bases
Acid Base Lesson Plans
Some Resources Available on Moodle Site for Chemistry I H
For any aqueous solution, explain the meaning of the value indicated by the pH scale in terms of the hydrogen ion concentration.
C.8.4 Given the hydronium (H3O+) ion concentration in a solution, calculate the pH and vice versa. Explain the meaning of these values.
C.8.5 From acid-base titration data, calculate the concentration of an unknown solution.
Gases(Week 26, 3 Weeks)
Science (2010), Grades 10-12 , Chemistry IStandard 5: Behavior of GasesUsing the kinetic molecular theory, describe and explain the behavior of ideal gases.
C.5.1
How can you know that there's matter in a gas?Why don't gas particles stick together and accumulate at the bottom of a container?Why is knowing the volume of a gas meaningless in knowing the amount of
Pressure Pressure Units
(kPa, torr, atm) Boyles Law Charles Law Gay-Lussac's
Law Avogadro's Law Dalton's Law of
Partial Pressure Graham's Law of
Define pressure and distinguish between pressure and force.
Define atmospheric pressure and give the values for standard atmospheric pressure in kilopascals,
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer
Lesson Plan Available in Links Day 1 Pressure Demonstrations and Pressure Units p415: 69-71Day 2 Boyles ActivityDay 3 Kelvin Scale Charles Law and Combined law p430: 19-21; p448: 88 b,cDay 4 Ideal Gas law p437: 41-45Day 5 Changing Conditions and
Some Resources Available on Moodle Site for Chemistry I H
Use kinetic molecular theory to explain changes in gas volumes, pressure, moles and temperature.
Using the ideal gas equation of state PV = nRT, examine the relationship among the number of moles, volume, pressure and temperature for ideal gases.
C.5.2 Using the ideal gas equation of state PV = nRT, calculate the change in one variable when another variable is changed and the others are held constant.
C.5.3 Given the equation for a chemical reaction involving one or more gases as reactants, product
matter?
Diffusion Temperature Kelvin Standard
Temperature and Pressure
Molar Volume Gas
Stoichiometry Collecting a Gas
Over Water
atmospheres, and millimeters of mercury (torr).
Define Dalton’s law of Partial Pressure and use it to find the pressure of a gas collected over water.
Define and solve problems involving Boyles Law.
Explain the relationship between pressure and volume of a gas.
Define Charles Law and describe the relationship between volume and temperature.
Define absolute zero.
Convert from Celsius to Kelvin and vice versa.
Describe the relationships involved with the ideal gas law formula.
Solve problems involving the combined gas law.
Define diffusion. Solve problems
involving Graham’s Law of Diffusion.
Define molar volume and give its value for STP.
Use the molar volume value to solve stoichiometry calculations involving gaseous species.
at the beginning of the period.
Ideal WorksheetDay 6 Ideal Gas Constant LabDay 7 Gas Stoichiometry Notes and AssignmentDay 8 Mg in Acid LabDay 9 Gas Stoichiometry practice quizDay 10 Gas Stoichiometry Quiz Graham's law WorksheetDay 11 Kinetic Theory notes Graham's law LabDay 12 Graham's law Quiz Review WorksheetDay 13 Review ActivityDay 14 Review Activity IIDay 15 Unit Test
s or both, calculate the volumes of gas when assuming the reaction goes to completion and the ideal gas law holds.
Chemical Bonding(Week 29, 3 Weeks)
Science (2010), Grades 10-12 , Chemistry IDescribe how the structure of the periodic table reflects the numbers of electrons and protons and the configuration of electrons in an atom.
C.2.6 Use the periodic table and electron configuration to determine an element's number of valence electrons and its chemical and physical properties.
Standard 3: Bonding and Molecular StructureDescribe how the configuration of electrons within an atom determines its interactions with other atoms.
Why do atoms stick together?Why do some things stick together stronger than others?
Predict whether bonds are ionic, polar covalent, or nonpolar covalent using electronegativity values.
Determine the partial charge distribution of a polar covalent bond.
Apply the octet rule to write electron dot structures of simple molecules and polyatomic ions.
Identify limitations to the octet rule.
Predict the shapes of molecules.
Determine if a molecule is polar or nonpolar.
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Day 1 Bonding NotesDay 2 Ionic bonding dot diagrams Lewis Diagram NotesDay 3 Complete 9-42 of Dot Diagram NotesDay 4 Lewis Practice Quiz Octet Exception NotesDay 5 Lewis Quiz Electron Geometries 9-42 bDay 6 Molecular Geometry Notes 9-42 cDay 7 Molecular Modeling ActivityDay 8 Bond Angle NotesDay 9 Polarity Notes 9-52 dDay 10 Hybridization Notes 9-52 fDay 11 Bonding Assignment SheetDay 12 Practice QuizDay 13 Practice Quiz II; ReviewDay 14 Review ActivityDay 15 Unit Test
Chemical Bonding Lesson Plans
Syllabus: Bonding
Some Resources Available on Moodle Site for Chemistry I H
ionic, covalent network, metallic and polar and non-polar molecular crystals with respect to constituent particles, strength of bonds, melting and boiling points and conductivity; provide examples of each type.
Standard 4: Reactions and StoichiometryUse balanced chemical equations and the mole concept to determine the quantities of reactants and products.
C.4.1 Predict products of simple reactions such as synthesis, decomposition, single replacement and double replacement.
Balance chemical equations using the law of conservation of mass and use them to describe chemical reactions.
C.4.6 Determine oxidation states and identify the substances gaining and losing electrons in redox reactions.
Intermolecular Forces and Thermochemistry(Week 32, 3 Weeks)
Science (2010), Grades 10-12 , Chemistry ICompare and contrast states of matter at the molecular level.
C.1.5 Describe the characteristics of solids, liquids and gases and changes in state at the molecular level.
Standard 3: Bonding and Molecular StructureDescribe how the configuration of
Why are some things solid while others are liquid or gas?Why might a substance change from one substance into another?What happens when energy is added to a substance?
Intermolecular Forces
Solids, Liquids and Gases and Intermolecular Forces
Types of Solids Physical
Properties and Intermolecular Forces
Phase Diagrams Heating Curve Heat
Calculations
Classify solids as amorphous or crystalline.
Classify crystalline substances as metallic, ionic, molecular or macromolecular.
Explain how the three types of intermolecular forces arise.
Compare and contrast the physical properties of gases, liquids, and solids by comparing the strength of their intermolecular forces.
Predict which intermolecular forces will occur in a substance given its structure and composition.
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Day 1 Boiling Point of Ethanol and Water Activity Intermolecular Forces NotesDay 2 Surface Tension ActivityDay 3 Intermolecular Forces and Physical Properties NotesDay 4 Phase Diagram WorksheetDay 5 Intermolecular Forces WorksheetDay 6 Heat Calculation NotesDay 7 Specific Heat LabDay 8 Heating Curve NotesDay 9 Heating Curve Worksheet 1-5Day 10 Fuel Value LabDay 11 Heating Curve Quiz Review WorksheetDay 12 Review ActivityDay 13 Unit Test
Intermolecular Forces Lesson Plans
Syllabus: Intermolecular Forces and Heat
Some Resources Available on Moodle Site for Chemistry I H
electrons within an atom determines its interactions with other atoms.
C.3.1 Describe, compare and contrast the characteristics of the interactions between atoms in ionic and covalent compounds.
Describe the attractive forces among molecules and their effect on chemical and physical properties.
C.3.5 Compare and contrast ionic, covalent network, metallic and polar and non-polar molecular crystals with respect to constituent particles, strength of bonds, melting and boiling points and conductivity; provide examples of
Relate physical properties (rate of evaporation, vapor pressure, boiling point, melting point, volatility, critical temperature, heat of vaporization, and heat of fusion) to the strength of intermolecular forces.
Interpret a phase diagram
Interpret the features of a heating curve.
Solve calculations involving phase changes and temperature change for the amount of energy involved.
Explain the molecular basis for surface tension.
Explain how the structure of water accounts for its unusual properties.
specific heat, phase change constants (i.e., latent heat values) or both.
Solutions(Week 35, 2 Weeks)
Science (2010), Grades 10-12 , Chemistry IStandard 7: SolutionsDescribe the composition and characteristics of solutions.
C.7.1 Describe the composition and properties of types of solutions.
C.7.2 Explain how temperature, pressure and polarity of the solvent affect the solubility of a solute.
C.7.3 Describe the concentration of solutes in a solution in terms of molarity. Perform calculations using molarity, mass and
What happens when something dissolves?How can we describe how much of something has been dissolved in a solution?
Solubility Factors
Solute and Solvent
The dissolving process
Freezing and Boiling Points of Solutions
Distinguish solutions from other mixtures.
Describe the dissolving process.
Analyze the factors that affect solubility.
Relate changes in boiling and freezing temperature to the concentration of solute in a solution.
Bell WorkOther written assessmentsEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Lesson Plan Available in Links Day 1 Solutions Lab Parts I and IIDay 2 Solutions Lab Parts III and IVDay 3 Solutions NotesDay 4 Solubility Curve NotesDay 5 Chromatography ActivityDay 6 Solutions Review WorksheetDay 7 Review ActivityDay 8 Unit Test
Solutions Lesson Plans
Syllabus: Solutions
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Prepare a specific volume of a solution of a given molarity when provided with a known solute.
Chemical Kinetics and Equilibrium(Week 37, 1 Week)
Science (2010), Grades 10-12 , Chemistry IIdentify the factors that qualitatively affect solubility, reaction rates and dynamic equilibrium.
C.7.5 Explain how the rate of a reaction is qualitatively affected by changes in concentration, temperature, surface area and the use of a catalyst.
C.7.6 Write equilibrium expressions for reversible reactions.
Why might some reactions take a very long time?How can the rate of a chemical reaction be increased?What does it mean for a reaction to reach a dynamic equilibrium?
Factors affecting rate of reaction.
Collision Theory Dynamic
Equilibrium Equilibrium
Expressions
List factors that affect the rate of a chemical reaction.
Explain factors affecting reaction rates using collision theory.
Explain dynamic equilibrium
Write equilibrium expressions
Lesson Plan Available in Links Day 1 Chemical Kinetics NotesDay 2 Kinetics Lab Part IDay 3 Kinetics Lab Part IIDay 4 Chemical Equilibrium NotesDay 5 Review Equilibrium
Kinetics and Equilibrium Lesson Plans
Some Resources Available on Moodle Site for Chemistry I H
Week) Chemistry and BiochemistryDescribe the unique nature of carbon atoms’ ability to bond to one another and other elements, which forms countless carbon-based substances and macromolecules.
C.9.1 Use structural formulas to illustrate carbon atoms’ ability to bond covalently to one another to form many different substances.
C.9.2 Illustrate the variety of molecular types formed by the covalent bonding of carbon atoms and describe the typical properties of these molecular types.
Why is it important to study carbon compounds?
Functional Groups
Polymers
homologous series.
Draw structural formulas and name straight chain and cyclic hydrocarbons, using the IUPAC system.
Identify functional groups and describe how they affect the properties of the compounds in which they occur.
Describe the characteristics of polymers.
sEach class period begins with a question posted or otherwise displayed for students to answer at the beginning of the period.
Day 2 Naming Branched Hydrocarbons p705: 1-4Day 3 p714: 18, 19; p716: 21 a-c; Hydrocarbon WorksheetDay 4 p733: 61 a-c; 65 a, b; Functional Group Notes and WorksheetDay 5 PolymersDay 6 Organic Test/Worksheet
