Jonesville High School Chemistry One Overvie · Jonesville High School Chemistry One Overview: ......
Transcript of Jonesville High School Chemistry One Overvie · Jonesville High School Chemistry One Overview: ......
Jonesville High School
Chemistry One
Overview:
This one trimester course is designed to give students a solid foundation in the basic concepts of Chemistry in a manner which should prepare the
student to be a scientifically literate citizen. Chemistry I will also insure that the student is well equipped with the laboratory skills and scientific
practices in order for them to be successful in Chem II. This class covers many of the High School objectives described in the Michigan Merit
Curriculum for Chemistry (Michigan Department of Education, 2006) with a direct focus on The Next Generation Science Standards which our
department anticipates will be adopted by the state of Michigan. The document that describes these expectations can be obtained from the
Michigan Department of Education (www.mi.gov/mdoe). In addition, my goal is to guide students through common scientific practices with a series
of relevant laboratory activities and demonstrations which enrich the curriculum and further promote mastery of the concepts and lab experiences.
Units of Study
Unit Title: Length
1. Kinetic Molecular Theory & Solubility 2 weeks
○ Summative Assessment #1 = KMT, IMF & Solubility
2. Collision Theory and Properties of Matter 2 weeks
○ Summative Assessment #2 = Density, Collision Theory
3. Subatomic Particles and Nuclear Processes 2 weeks
○ Summative Assessment #3 = A review of Subatomic Particles and Nuclear Processes
4. Chemical Reactions and Conservation 2 weeks
○ Summative Assessment #4 = Atoms, ions, molecules and periodic trends
5. Conservation of Mass and Chemical Reactions 2.5 weeks
○ Summative Assessment #5 = Conservation of Mass & Chemical Reactions.
6. Properties of Acids and Bases 1.5 weeks
○ Summative Assessment #6 = Acid Base Reactions
Text: Scientific Journal Articles
Required course for 10-11 graders
10th Grade/Chemistry 1:
Unit One Title: Kinetic Molecular Theory and Solubility
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
MS-PS1-4: Develop a model that predicts and describes changes in particle motion, temperature, and state of a pure substance when thermal energy is added or removed. MS-PS1-2: Analyze and interpret data on the properties of substances before and after the substances interact to determine if a chemical reaction has occurred.
● Describe Chemistry.
● Describe Properties of matter.
● Develop a model that predicts and describes changes in particle motion as matter changes.
● Develop a model of changes in matter relate to changes in mass/volume.
● Identify physical changes within matter.
● Separate a mixture based on physical properties.
● Analyze a solubility curve.
● Describe freezing point depression and boiling point elevation
● Chemistry ● Matter ● Mass ● Volume ● Intermolecular
forces ● Temperature ● Phase Change ● Chemical
Change ● Bonds ● Kinetic Energy ● Solution/Mixture ● Physical
Property ● Solubility ● Unsaturated ● Saturated ● Supersaturated ● Solubility Curve ● Freezing Point
Depression ● Boiling Point
Elevation ● ACS -
Chemmatters salting the roads Journal Article.
● Steel Wool ● Ice ● Hot Plate ● Beaker ● Graduated
Cylinder ● Beaker Tongs ● H2O ● Computer ● Ammonia
Chloride; NH4Cl
● PASCO digital Thermometers
● Test Tubes ● Bunsen Burner ● Test Tube
Rack ● NaCl
FA - PHET - virtual kinetic molecular theory modeling activity. Students can develop a model that predicts and describes changes in particle motion, temp and state of a pure substance when thermal energy is added or removed.
SA - Lab - Modeling physical changes in matter. Students can develop a model that predicts and describes changes in particle motion, temp and state of a pure substance when thermal energy is added or removed.
FA - Separating a mixture. Students can describe properties of a mixture by separating one
based on physical properties.
FA - Graphical analysis of solubility curves. Students can plot and analyze a solubility curve.
FA - Lab - Creating a solubility curve. Students can collect data and analyze a solubility curve created in class to make predictions.
FA - Lab - Boiling Point Elevation. Students can describe boiling point elevation.
FA - Freezing Point depression Journal Analysis. Students can identify a real life application to freezing point depression.
SA - Unit #1 Test - Modeling KMT and IMF & Analysis of Solubility curve.
Text: Scientific Journal Articles
Required course for 10-11 graders
10th Grade/Chemistry 1:
Unit Two Title: Collision Theory and Properties of Matter
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
MS-PS1-5: Develop and use a model to describe how the total number of atoms does not change in a chemical reaction and thus mass is conserved. MS-PS1-2: Analyze and interpret data on the properties of substances before and after the substances interact to determine if a chemical reaction has occurred. HS-PS1-4 Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy. HS-PS1-5 Apply scientific principles and evidence to provide an explanation about the effects of changing the temperature or concentration of the reacting particles on the rate at which a reaction occurs.
● Describe how mass relates to volume in matter.
● Calculate density in lab.
● Make predictions based on data collected in lab (Density).
● Describe energy. ● Describe how energy
relates to the kinetic molecular theory.
● Describe how energy relates to temperature.
● Describe the perception of the transfer of energy.
● Describe Bond Energy
● Activation energy ● Analyze an energy
level diagram ● Describe the collision
theory. ● Describe how a
chemical reaction occurs between two molecules.
● Using the collision
● Matter ● Mass ● Volume ● Density ● Reactants ● Products ● Yield ● Molecule ● Bond ● Energy ● Temperature ● Endothermic ● Exothermic ● Bond Energy ● Activation
energy ● Energy Level
Diagram ● Collision
Theory ● Activation
energy ● Surface Area ● Concentration
● Computers ● Zn ● Cu ● Al ● Graduated
Cylinder ● H2O ● Scale ● PASCO
Thermometers ● Baking Soda ● Vinegar ● Magnesium ● 0.5 M HCl ● Graph Paper ● Stop Watches ● Scale ● Food Dye ● Mortar & Pestle ● Alka Seltzer ● PASCO
Thermometers ● Hot plate ● Solid H2O ● Graph Paper ● Vinegar ● Baking Soda
FA - Students can calculate density.
SA - Students can make an educated prediction about what a metal is based on measurements in mass and volume conducted in lab.
SA - Students can make predictions about matter based on density calculated in lab.
FA - Student can describe the difference between temperature and heat.
FA - Student can describe how energy is transferred from one substance to another.
FA - Student can observe a
theory, describe how temperature, concentration and surface area influence the rate of a chemical reaction.
chemical reaction and describe the difference between bond energy in reactants and products.
FA - Students can create and describe an energy level diagram.
FA - Students can create a model of and effective collision using the collision theory.
FA - Students can design a lab to investigate the influence of surface area , temperature and concentration on reaction rate.
FA - Students can create a graph to show show how S.A, Temp and Conc. influence reaction rate.
SA - Unit 2 Test: Collision Theory and Properties of Matter.
Text: Scientific Journal Articles
Required course for 10-11 graders
10th Grade/Chemistry 1:
Unit Three Title: Subatomic Particles and Nuclear Processes
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
HS-PS1-1 Develop models to describe the atomic composition of simple molecules and extended structures. HS-PS1-8 Develop models to illustrate the changes in the composition of the nucleus of the atom and the energy released during the processes of fission, fusion, and radioactive decay. HS-PS2-6 Communicate scientific and technical information about why the molecular-level structure is important in the functioning of designed materials.
● Identify Subatomic particles.
● Read and identify subatomic particles based off of atomic symbols.
● Construct a physical model to illustrate the substructures of an atom.
● Create a model showing how nuclear process occur, and write an essay about why the nuclear structure is important in the functioning of designed materials.
● Smallest bits of matter - NPR article.
● Periodic Table ● Atom ● Proton ● Neutron ● Electron ● Charge ● Mass ● Radius ● Nucleus ● Electron Cloud ● Fission ● Fusion ● Radiation ● Half Life ● Decay ● Alpha Decay ● Beta Decay ● Gamma
Radiation ● Nuclear Medicine ● Nuclear Energy ● Nuclear Weapons
● Computer ● Subatomic
particle modeling set
● Pennies (½ life modeling activity)
● Shoe boxes
FA - PHET - subatomic particles.
FA - Subatomic particles worksheet.
FA - PHET ½ Life FA - PHET alpha decay FA - PHET beta decay FA - Fission/Fusion FA - Gamma decay SA - Research project
in practical uses of nuclear chemistry in society.
SA - Unit 3 Test: Subatomic Particles and Nuclear Processes.
Text: Scientific Journal Articles
Required course for 10-11 graders
10th Grade/Chemistry 1:
Unit Four Title: Atoms, Ions, Molecules and Periodic Trends
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
MS-PS1-1 Develop models to describe the atomic composition of simple molecules and extended structures. HS-PS1-1 Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.
● Describe the composition of subatomic particles within a molecule.
● Identify Ionic, covalent and metallic bonds.
● Describe properties molecules based on bond type.
● Describe/create an alloy. ● Properly name atoms,
ions and molecules based on their bond type.
● Describe patterns in the periodic table.
● Use the periodic table to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms and trends in the periodic table.
● Describe reactivity. ● Make predictions about
reactivity based on trends in the periodic table.
● Atom ● Ion ● Molecule ● Bond ● Cation ● Anion ● Neutral Molecule ● Charge ● Mass number ● Proton ● Neutron ● Electron ● Valence Electron ● Metal ● Nonmetal ● Ionic Bond ● Covalent Bond ● Metallic Bond ● Alloy ● Lewis Dot
structure ● Ionization energy ● Electronegativity ● Atomic Radius ● Periodic Table ● Reactivity
● Index Cards ● Dot Stickers ● Markers ● Graph
paper ● Periodic
Tables ● Computer ● 0.5 M HCl ● Tin ● HCl ● Mg ● Ca ● Si ● H2O ● Test Tubes ● Test Tube
Rack ● Beakers ● Graduated
Cylinders. ● Periodic
Tables ● Computers ● Graph
Paper ● Journal
Articles
FA - Illustrating electron dot diagrams.
FA - Illustrating Ionic & Covalent bonds.
FA - Lab - Properties of ionic and covalent compounds.
FA - Metallic bonding - Alloy lab.
FA - Periodic Trends Worksheet.
FA - Using trends to describe bonding activity.
FA - Graphical Analysis of periodic trends.
FA - Lab - Using trends to describe properties in ionic and covalent compounds.
FA - Lab - Using periodic trends to describe reactivity.
SA - Unit 4 Test: Atoms, Ions, Molecules and periodic trends.
Text: Scientific Journal Articles
Required course for 10-11 graders
10th Grade/Chemistry 1:
Unit Five Title: Conservation of Mass and Chemical Reactions
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
MS-PS1-1 Develop and use a model to describe how the total number of atoms does not change in a chemical reaction and thus mass is conserved. HS-PS1-2 Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties. HS-PS1-7 Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction.
● Use mathematical representations to describe the law of conservation.
● I can describe how balancing chemical equations relates to the conservation of mass.
● Use periodic trends to describe/predict the outcome of chemical reactions.
● Identify different types of chemical reactions.
● Given a type of chemical reaction write a chemical reaction.
● Matter ● Mass ● Conservation ● Mole ● Molar Mass ● Coefficients ● Subscripts ● Balancing
Chemical Reactions
● Reactants ● Products ● Yield ● Coefficient ● Subscript ● Synthesis
Reaction ● Decomposition
Reaction ● Combustion
Reaction ● Double
Replacement Reaction
● Single Replacement
● Computers ● Vinegar ● Baking Soda ● Scale ● Graph Paper ● Magnesium ● Bunsen
Burner ● Crucible ● Computers ● Combustion
Demo apparatus
● Flour ● Candels ● Butane
Lighter ● Mg ● KI ● Dish soap ● HCl ● NaOH ● H2O2
FA - Students can convert mole conversions.
SA - Mole conversion quiz. FA - Students can balance
chemical reactions. SA - Balancing chemical
reactions quiz. FA - Students can collect and
organize/communicate data that supports the law of conservation.
FA - Student can make predictions using trends in the periodic table about how atoms will interact.
FA - Students can observe chemical reactions and identify the type of chemical reaction.
FA - Given material and the type of reaction involved, students can predict the products involved in a chemical reaction.
SA - Unit 5 Test: Conservation of Mass and Chemical
Reaction Reactions.
Text: Scientific Journal Articles
Required course for 10-11 graders
10th Grade/Chemistry 1:
Unit Six Title: Properties of Acid, Base Reactions
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
MS-PS1-1 Develop models to describe the atomic composition of simple molecules and extended structures. HS-PS2-6 Communicate scientific and technical information about why the molecular-level structure is important in the functioning of designed materials. HS-PS1-2 Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.
● Describe properties of acids and bases.
● Describe what an acid/base is under the Arrhenius model.
● Describe what an acid/base is under the Bronsted-Lowry Model.
● Describe what an indicator is and how it relates to pH.
● Identify conjugate acid/bases in acid/base reactions.
● Describe type of reaction that occurs in a acid/metal reaction.
● Describe type of reaction that occurs in a neutralization reaction.
● Acid ● Base ● pH ● Arrhenius
Model ● Bronsted-Lowry
Model ● Indicator ● Hydronium ion ● Hydroxide ion ● Neutralization
reaction ● Conjugate Acid ● Conjugate Base
● War heads ● Litmus paper ● Universal
Indicator ● 1M NaOH ● Vinegar ● Red Cabbage ● Various
Household acids/bases
● H2O ● 500 mL
Graduated cylinders
● 100 mL graduated cylinder
● Mortar and Pestle
● Test Tubes
FA - Conjugate acid/base worksheet.
FA - Dilution and [H3O+]
& [OH-]
FA - Red Cabbage indicator hydronium/hydroxide ion concentration lab.
FA - Neutralization lab. FA - Acid/Base reaction
lab. SA - Unit 6 Test:
Properties of acid, base reactions.
Jonesville High School
Chemistry Two
Overview:
This one trimester course is designed to elaborate on the concepts and laboratory skills built during chemistry one. Chemistry 2 is designed for
students to apply the concepts and practices established in chemistry one in a manner that creates a deep conceptual understanding and
appreciation of not only chemistry but science in general. My goal is that successful completion of chemistry 2 will provide students with a skill set
that will enable students to move forward in their education so they will be prepared to take a basic college chemistry class. While this class
covers many of the High School objectives described in the Michigan Merit Curriculum for Chemistry, (Michigan Department of Education, 2006)
an emphasis on The Next Generation Science Standards is the central focus of the curriculum design. The document that describes these
expectations can be obtained from the Michigan Department o Education (www.mi.gov/mdoe) as well as through the National Research Council
(www.nextgenscience.org.)
Units of Study
Unit Title: Length
1. Periodic Trends and Electron Configuration 1.5 weeks
2. Intramolecular, Intermolecular forces & Phase Diagrams 2.5 weeks
3. Chemical Kinetics and Equilibrium 1.5 weeks
4. Chemical Reactions and Conservation 3 weeks
5. Acid/Bases and Environmentalism 1.5 weeks
6. Energy in chemical reactions 2 weeks
Text: Scientific Journal Articles
Required course for 10-11 graders
11th Grade/Chemistry 2:
Unit One Title: Periodic Trends and Electron Configuration
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
HS-PS1-1 Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.
● Quantify subatomic particles based on atomic symbols.
● Quantify subatomic particles when mass number and charge changes.
● Describe the difference between mass number and average atomic mass.
● Describe how the percentage of each isotope contributes to average atomic mass number.
● Analyze trends and patterns within the periodic table.
● Make predictions based off of
● Periodic Table ● Proton ● Neutron ● Electron ● Mass number ● Charge ● Nucleus ● Ion ● Cation ● Anion ● Electron Cloud ● Isotope ● Average atomic
mass. ● Period ● Group ● Ionization
Energy ● Electronegativity ● Atomic Radius ● Reactivity ● Energy level ● Quantum
number ● Orbital
○ S ○ P ○ D ○ F
● Calcium ● Water ● Magnesium ● Tin ● 0.5 M HCl ● Test Tubes ● Test Tube
Rack ● Lima Beans ● Buckets ● Graph paper ● Electron
Configuration Bingo cards
● Plastic Bingo Markers
FA -Worksheet - Students can identify subatomic particles.
FA - Worksheet - Students can identify subatomic particles based off of atomic symbol when charge and mass number are manipulated.
FA - Lab - Students can identify how isotopes relate to average atomic mass.
FA - Lab - Students can write a lab report.
FA - Graphical Analysis - Students can create a graph analyzing trends and patterns
trends in the periodic table and collect data to support their predictions.
● Identify ground vs. excited state electron configuration.
● Relate electron configuration to charge.
● Electron Configuration
● Ground state electron configuration.
● Excited state electron configuration.
within the periodic table.
SA - Lab -Students can make predictions based off of trends in the periodic table and collect data to support their predictions.
FA - Activity - Students can describe how average atomic mass is calculated.
FA - Worksheet - Students can describe a 3D model of the electron cloud.
FA - Lab - Students can identify electron configuration in lab.
SA - Unit #1 Test: Periodic Trends and Electron Configuration
Text: Scientific Journal Articles
Required course for 10-11 graders
11th Grade/Chemistry 2:
Unit Two Title: Intramolecular, Intermolecular forces & Phase Diagrams
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
HS-PS1-1 Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties. HS-PS1-3 Plan and conduct an investigation to gather evidence to compare the structure of substances at the bulk scale to infer electrical forces between particles. HS-PS2-6 Communicate scientific and technical information about why the molecular-level structure is important in the functioning of designed materials. HS-ESS2-5 Plan and conduct an investigation of the properties of water and its effects on Earth materials and surface processes.
● Identify bond type.
● Use electronegativity to describe valence electron distribution in a chemical bond.
● Identify bond polarity.
● Identify molecular shape based off of molecular models.
● Use molecular geometry to describe VSEPR Theory.
● Use bond polarity and VSEPR to predict molecular polarity.
● Describe intermolecular forces.
● Identify and describe how intermolecular force relates to
● Chemical Bond ● Ionic ● Covalent ● Charge ● Electron ● Polar covalent ● Lewis Dot
Structure ● Valence
Electrons ● Nonpolar
covalent ● Electronegativity ● Polarity ● Bond Polarity ● VSEPR ● Molecular
Geometry ● Electron
Geometry ● Molecular
Polarity ● Intramolecular
Force ● Intermolecular
Force ● Kinetic
Molecular Theory
● Computers ● Molecular
Modeling blocks
● H2O ● Isopropyl
alcohol ● Ethyl alcohol ● Glycerol ● Xylenes ● NaCl ● Erlenmeyer
Flasks ● Plastic
Disposable Pipettes
● CO2 ● Buckets ● Pennies ● Wax Paper ● Pasco
Thermometers
● Graph paper
FA - Worksheet - Students can identify Bond Type (Polarity).
FA - Modeling Activity - Students can identify molecular shape based off of molecular models.
FA - PHET - Students can describe VSEPR Theory.
SA - VSEPR Theory Quiz.
FA - Worksheet - Student can identify and describe intermolecular forces.
FA - Labs - Student can identify and describe how intermolecular force relates to phase changes.
phase changes. ● Design a lab to
test IMF of an ion-dipole interaction in terms of strength of IMF.
● Describe how pressure and temperature relate to phase.
● Identify triple point within lab.
○ Solid ○ Liquid ○ Gas
● Surface Tension ● Evaporation ● Phase Change ● Temperature ● Pressure ● Phase Diagram ● Triple Point ● Critical Point
SA - Lab - Students can design a lab to test IMF of an ion-dipole interaction in terms of strength of IMF.
FA - Worksheet - Students can describe how pressure and temperature relate to phase.
FA - Lab - Students can identify triple point within lab.
SA - Unit #2 Test: Intra/Intermolecular forces & Phase Diagrams
Text: Scientific Journal Articles
Required course for 10-11 graders
11th Grade/Chemistry 2:
Unit Three Title: Chemical Kinetics and Equilibrium
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
HS-PS1-5 Apply scientific principles and evidence to provide an explanation about the effects of changing temperature or concentration of the reacting particles on the rate at which a reaction occurs. HS-PS1-6 Refine the design of a chemical system by specifying a change in conditions that would produce increased amounts of products at equilibrium.
● Identify factors that influence rate of reaction through data collection and analysis.
● Describe equilibrium.
● Describe equilibrium concentrations when reactants or products are favored.
● Analyze an equilibrium curve and identify when reaction has reached equilibrium.
● Describe Le Chateliers Principle.
● Design a chemical system and use Le Chatelier’s principle to describe how the reaction shifts.
● Surface Area ● Reactants ● Products ● Equilibrium ● Concentration ● Le Chateliers
Principle ● Equilibrium
Constant ● Pressure ● Temperature ● Stress
● Alka-Seltzer ● Ice ● Mortar &
Pestle ● CoCl2 ● AgNO3 ● 12 M HCl ● Ice ● Hot Plate ● Straws ● Graduated
Cylinders ● Respiration
and Le Chateliers Principle Article
● Fixing the nitrogen problem agriculture reading article.
SA - Lab Report - Students can I.D. factors that influence rate of reaction through data collection and analysis.
FA - Lab - Students can describe equilibrium.
FA - Lab - Students can describe equilibrium concentrations when reactants or products are favored.
FA - Worksheet - Students can analyze an equilibrium curve and identify when reaction has reached equilibrium.
FA - PHET - Students can describe Le Chateliers Principle.
FA - Lab Report - Students can
design a chemical system and use Le Chatelier’s principle to describe how the reaction shifts.
SA - Unit #3 Test: Chemical Kinetics and Equilibrium
Text: Scientific Journal Articles
Required course for 10-11 graders
11th Grade/Chemistry 2:
Unit Four Title: Chemical Reactions and Conservation of Mass
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
HS-PS1-2 Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties. HS-PS1-7 Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction. HS-ESS2-6 Develop a quantitative model to describe the cycling of carbon among the hydrosphere, atmosphere, geosphere, and biosphere
● Balance Chemical Reactions.
● Relate Balancing Chemical Reactions to the Law of Conservation.
● Describe how carbon cycles through our atmosphere.
● Relate the carbon cycle to the law of conservation.
● Count atoms. (mole conversions)
● Perform Stoichiometry calculations.
● Relate stoichiometry to the conservation of mass.
● Determine the limiting reactant.
● Determine percent yield.
● Design and carry out an
● Reactant ● Product ● Coefficient ● Subscript ● Mole ● Particle ● Stoichiometry ● Conversion ● Excess reactant ● Limiting reactant ● Percent Yield ● Law of
Conservation. ● Actual Yield ● Theoretical
Yield
● Aluminum ● Magnesium ● HCl ● Na2CO3 ● NaHCO3 ● Balloon ● CH3COOH ● H2SO4 ● Scale ● Calculators ● Crucibles
FA - Virtual Lab - Balancing Chemical Reactions.
FA - Mole Conversion Worksheet.
SA - Mole conversion Lab Practicum.
SA - Conservation of mass lab
FA - Law of conservation reading activity - Carbon Cycle.
FA - Mass → Mass
Stoichiometry
Worksheet.
FA - Mol → Mol Lab
FA - Mass → Mass
Lab
FA - Percent Yield Competition Lab
SA - NaHCO3 + HCl Independent Lab
SA - Unit #4 Test: Reaction Stoichiometry
Text: Scientific Journal Articles
Required course for 10-11 graders
11th Grade/Chemistry 2:
Unit Five Title: Acid/Bases and Environmentalism
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
HS-PS1-2 Construct and revise an
explanation for the outcome of a
simple chemical reaction based on
the outermost electron states of
atoms, trends in the periodic table,
and knowledge of the patterns of
chemical properties.
HS-ESS2-6 Develop a quantitative
model to describe the cycling of
carbon among the hydrosphere,
atmosphere, geosphere, and
biosphere.
HS-ESS3-6 Use a computational
representation to illustrate the
relationships among Earth systems
and how those relationships are
being modified due to human
activity.
HS-ESS3-1 Construct an
explanation based on evidence for
how the availability of natural
resources, occurrence of natural
hazards, and changes in climate
● Describe 3 models of Acid/Base Theory
● Identify acids and bases in chemical reactions based on proton movement.
● Describe the difference between an acid and a base.
● Describe a neutralization reaction.
● Describe how acid rain relates to the carbon cycle.
● Describe how ocean acidification relates to the carbon cycle.
● Describe how ocean acidification relates to the law of conservation.
● Describe proposed
● Acid ● Base ● Arrhenius ● Bronsted Lowry ● Lewis ● Propton ● Hydronium ● Hydroxide ● Neutralization ● Ocean
Acidification ● Acid Rain
● CaCO3 ● HCl ● CH3COOH ● Universal
Indicator ● Apple ● Petri Dish ● H2SO4 ● USGS Acid
Rain Reading Article
● Ocean Acidification Journal Article
● Internet
FA - Identifying Conjugate Acids/Bases Activity.
FA - Writing Neutralization Reactions WS
FA - Microscale Acid Rain Lab.
FA - Acid Rain USGS Article Reflection.
FA - Ocean Acidification Lab.
FA - Ocean Acidification Journal Article Reflection
FA - Addressing ecological issues in chemistry and investigating/designing solutions research paper.
SA - Unit #5 Test: Acid/Base Theory & Ocean Acidification
have influenced human activity.
HS-ETS1-1 Analyze a major global
challenge to specify qualitative and
quantitative criteria and constraints
for solutions that account for
societal needs and wants.
HS-ETS-1-3 Evaluate a solution to
a complex real-world problem
based on prioritized criteria and
trade-offs that account for a range
of constraints, including cost,
safety, reliability, and aesthetics as
well as possible social, cultural,
and environmental impacts.
solutions to environmental chemistry problems.
Text: Scientific Journal Articles
Required course for 10-11 graders
11th Grade/Chemistry 2:
Unit Six Title: Energy in Chemical Reactions
NGSS Standards: Learning Targets & “I can statements”:
(Performance Task)
Key Vocabulary and Case Studies:
Instructional Resources:
Suggested Assessment:
HS-PS1-4 Develop a model to
illustrate that the release or
absorption of energy from a
chemical reaction system depends
upon the changes in total bond
energy.
HS-PS3-1 Create a computational
model to calculate the change in
the energy of one component in a
system when the change in energy
of the other component(s) and
energy flows in and out of the
system are known.
HS-PS3-4 Plan and conduct an
investigation to provide evidence
that the transfer of thermal energy
when two components of different
temperature are combined within a
closed system results in a more
uniform energy distribution among
the components in the system
(second law of thermodynamics).
HS-PS3-3 Design, build, and refine
● Describe the difference between temperature and heat.
● Describe Bond Energy
● Describe endo and exothermic chemical reactions.
● Compare bond energy in reactants and products in a chemical reaction.
● Use bond energy to describe temperature change in chemical reactions.
● Describe how to measure energy change.
● Design/Make a calorimeter.
● Describe how to use a calorimeter.
● Calibrate a
● Heat ● Temperature ● Energy ● Endothermic
Chemical Reaction
● Exothermic Chemical Reaction
● Bond Energy ● Energy Level
Diagram ● Enthalpy ● Specific Heat ● Calorimeter ● Thermochemical
Equation ● MSDS
● Food Dye ● Hot plate ● PASCO
Thermometer ● Metal
Samples: ○ Al ○ Zn ○ Cu ○ Ni
● Styrofoam ● Styrofoam
cups. ● Beakers ● Graduated
cylinders ● Ionic
Compounds ● Material
Safety and Data Sheets
● Poster Board ● Matches ● Marshmallows ● Nuts ● Safety pins ● Cork ● Soda Can ● Ring stand ● Iron Ring ● Stir Rod
FA - Lab - Student can describe the difference between temperature and heat.
FA - Worksheet - Student can describe how energy is transferred from one substance to another.
FA - Lab - Student can observe a chemical reaction and describe the difference between bond energy in reactants and products.
FA - Lab - Students can create and describe an energy level diagram.
FA - Lab - Students can design and build a calorimeter.
a device that works within given
constraints to convert one form of
energy into another form of
energy.
calorimeter. ● Describe specific
heat. ● Calculate specific
heat of metals using a calorimeter.
● Calculate change in energy using a calorimeter
● Describe caloric value in terms of bond energy and joules.
FA - Lab - Students can calibrate a calorimeter.
FA - Students can describe specific heat.
FA - Worksheet & Lab - Students can calculate specific heat in lab.
FA - Lab - Students can relate food to bond energy and joules.
FA - Worksheet & Lab - Students can calculate caloric value per gram.
SA - Lab - Students can use understanding of thermochemistry to design and build a hand warmer.
SA - Unit #6 Test: Thermochemistry